EPA 600-2-81-062
CHEMICAL SPECIATION OF
FLUE GAS DESULFURIZATION SLUDGE
CONSTITUENTS '
SCS ENGINEERS
STEARNS, CONRAb AND SCHMIDT
CONSULTING ENGINEERS, INC.
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FINAL REPORT
CHEMICAL SPECIATION OF
FLUE GAS DESULFURIZATION SLUDGE
CONSTITUENTS -
Phase I
Contract No. 68-03-2471
Prepared by:
Jasenka Vuceta, Ph.D.
John P. Woodyard, P.E.
SCS Engineers
4014 Long Beach Boulevard
Long Beach, California 90807
James C. S. Lu, Ph.D.
Cal Science Research, Inc.
7261 Murdy Circle
Huntington Beach, California 92647
Prepared for:
Solid and Hazardous Waste Research Division
Municipal Environmental Research Laboratory
U.S. Environmental Protection Agency
Cincinnati, Ohio 45268
Donald E. Sanning, Project Officer
January 1981
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ABSTRACT
This project addresses the problem of flue gas desulfuriza-
tion (FGD) sludge disposal to land. Specifically, the chemical
species of FGD sludge constituents are thermodynamically modeled
using the equilibrium constant approach, in an attempt to predict
the constituent concentrations in fresh and aged FGD wastewater
and sludge. This method involves solving the stoichiometric
equations of various chemical species, which are subject to con-
straints imposed by the equilibrium constants as well as mass
balance and charge balance relations. Diagrams, such as Eh-pH
plots, ion-ratio plots, concentrations pH figures, and species
distribution figures, are then used to display the stability
field and speciation results.
The thermodynamic model used in this study was verified for
suitability and accuracy by the analytical results of various FGD
sludge samples taken from the Kansas City Power and Light La
Cygne Power Station. The model is also operated over a wide
range of operational and chemical changes to determine their im-
pacts on the concentration and speciation of various solid and
soluble species. The impacts of (1) changes in pH and ionic
strength; (2) addition of lime, silicates, hydrogen sulfide, and
phosphates to the sludge; (3) variation of chloride, sulfate, and
borate levels; (4) addition of magnesium to the sorbent; and (5)
sulfite oxidation, are all estimated using the model.
The report was submitted in fulfillment of Contract No. 68-
03-2471 by SCS Engineers, Long Beach, California. The work was
completed January 27, 1981.
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CONTENTS
Page
Disclaimer i
Foreword i i
Abstract iii
Figures ; v i
Tab! es xi i
Acknowl edgements xi v
1. Introduction ;' 1
Description of Problem 1
FGD Waste Characteristics 2
Available Thermodynamic Models 7
Project Objectives 10
2. Principles and Methodologies for Investigations
into Chemical Speciation of FGD Sludge 12
The Stability Field of Constituent Species 12
The Speciation Model 15
3. Stability Field of Solid Species in FGD Sludge 23
Common Solid Species and Thermodynamic Data....23
Results of Stability Field Analysis 40
4. Soluble Chemical Species in Fresh FGD Wastewater....67
Constituent Speciation: Low Ionic Strength....94
Constituent Speciation: High Ionic
Strength 100
5. Constituent Speciation in Aged FGD Sludge 106
Constituent Speciation: Low Ionic
Strength 106
Constituent Speciation: High Ionic
Strength 134
6. Thermodynamic Model Verification 160
Comparison of Modeling Results with
Analytical Data 161
Evaluation of Model in Relation to Scientific
Considerations 184
7. Effects of Operational (Chemical) Changes on
FGD Sludge Chemical Species 186
Effects on pH on Speciation 186
Effects of Ionic Strength on Speciation 188
Effects of Chloride Concentration on the
Solubilities of Metals 188
Effects of Sulfate Concentration on the
Solubilities of Metals 198
Effects of Borate Concentration on the
Solubilities of Metals 204
i v
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CONTENTS (continued)
Effects of Lime Addition to FGD Sludge and
Wastewater 204
Effects of Silicate Addition to FGD SIudge... .211
Effects of Hydrogen Sulfide Addition to
FGO Sludge 222
Effects of Phosphate Addition to FGD
Sludge 225
Effects of Magnesium Addition to the FGD
Sorbent 227
Effects of Sulfite Oxidation 235
8. Summary of Findings 259
Intro duction 259
Methodology of Species Analyses 260
Speciation of Solid and Soluble Chemical
Species 260
Model Verification 267
Effects of FGD System and Sludge Variables
on Chemical Speciation 271
9. Conclusions and Recommendations 283
References 297
Appendices
A. Stability Constants of Soluble Metal Species 301
B. Chemical Analyses of Fresh and Aged FGD Sludge
Samples 307
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FIGURES
Number
1 Stability fiel
2 Stability fiel
3 Stability fiel
4 Stability fiel
5 Stability fiel
6 Stability fiel
7 Stability fiel
8 Stability fiel
9 Stability fiel
10 Stability fiel
11 Stability fiel
12 Stability fiel
13 Stability fiel
14 Stability fiel
15 Stability fiel
16 Speciation of
17 Speciation of
18 Speciation of
19 Speciation of
20 Speciation of
21 Speciation of
22 Speciation of
23 Speciation of
24 Speciation of
25 Speciation of
26 Speciation of
27 Speciation of
28 Speciation of
29 Speciation of
30 Speciation of
31 Speciation of
32 Speciation of
33 Speciation of
34 Speciation of
35 Speciation of
36 Speciation of
37 Speciation of
38 Speciation of
39 Primary distri
40 Speciation of
41 Primary distri
42 Speciation of
43 Primary distri
d of Al in FGD sludge 41
d of Sb in FGD sludge ...44
d of As in FGD wastes 45
d of Cd in'FDG sludge 46
d of Ca in FGD sludge 48
d of Cr in FGD waste 50
d of Cu in FGD sludge 51
d of Fe in FGD waste" 52
d of Pb in FGD sludge 54
d of Hg in FGD waste 58
d of Mn in FGD waste 59
d of Ni in FGD sludge 61
d of Se in FGD waste 62
d of S in FGD waste ....64
d of Zn in FGD sludge 65
Ca in raw FGD wastewater 72
Mg in raw FGD wastewater 73
K in raw FGD wastewater 74
Na in raw FGD wastewater 75
Cd in raw FGD wastewater 76
Cr in raw FGD wastewater 77
Cu in raw FGD wastewater .....78
Fe in raw FGD wastewater 79
Hg in raw FGD wastewater 80
Pb in raw FGD wastewater 81
Zn in raw FGD wastewater 82
Ca in raw FGD wastewater 83
Mg in raw FGD wastewater 84
K in raw FGD wastewater 85
Na in raw FGD wastewater 86
Cd in raw FGD wastewater 87
Cr in raw FGD wastewater 88
Cu(II) in raw wastewater 89
Fe in raw FGD wastewater 90
Hg in raw FGD wastewater 91
Pb in raw FGD wastewater 92
Zn in raw FGD wastewater 93
soluble Ca in aged FGD wastes 109
bution of Ca in aged FGD wastes...... 110
soluble Mg in aged FGD wastes Ill
bution of Mg in aged FGD wastes 112
soluble K in aged FGD wastes 113
bution of K in aged FGD wastes 114
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FIGURES (continued)
Number
44 Speciation of
45 Primary distri
46 Speciation of
47 Primary distri
48 Speciation of
49 Primary di stri
50 Speciation of
51 Primary distri
52 Speciation of
53 Primary distri
wastes
54 Speciation of
55 Primary distri
56 Speciation of
57 Primary distri
58 Speciation of
59 Primary distri
60 Speciation of
61 Primary distri
62 Speciation of
63 Primary distri
64 Speciation of
65 Primary distri
66 Speciation of
67 Primary distri
68 Speciation of
69 Primary distri
70 Speciation of
71 Primary distri
72 Speciation of
73 Primary distri
74 Speciation of
wastes
75 Primary distri
76 Speciation of
77 Primary distri
78 Speciation of
79 Primary distri
80 Speciation of
81 Primary distri
82 Total soluble
FGD wastes.
83 Total soluble
wastes
84 Total soluble
FGD wastes..
85 Total soluble
FGD wastes..
Page
soluble Na in aged FGD wastes 115
bution of Na in aged FGD wastes 116
soluble Cd in aged FGD wastes 117
bution of Cd in aged FGD wastes 118
soluble Cr in aged FGD wastewater.,..119
bution of Cr in aged FGD wastes 120
soluble Cu in aged FGD wastes 121
bution of Cu in aged FGD wastes 122
Fe(III) in aged FGD wastes 123
bution of Fe(III) in aged FGD
124
soluble Hg(II) in aged FGD waste 125
bution of Hg in FGD wastes 126
soluble Pb in aged FGD wastes 127
bution of Pb in aged FGD wastes 128
soluble Zn in aged FGD wastes 129
bution of Zn in aged FGD wastes 130
soluble Ca in aged FGD wastes 135
bution of Ca in aged FGD wastes 136
soluble Mg in aged FGD wastes 137
bution of Mg in aged FGD wastes 138
soluble K in aged FGD wastes 139
bution of K in aged FGD wastes 140
soluble Na in aged FGD wastes 141
bution of Na in aged FGD wastes 142
soluble Cd in aged FGD wastes ..143
bution of Cd in aged FGD wastes 144
soluble Cr in aged FGD wastes 145
bution of Cr in aged FGD wastes 146
soluble Cu in aged FGD wastes 147
bution of Cu in aged FGD wastes 148
soluble Fe(III) in aged FGD
149
bution of Fe(III) in FGD wastes 150
soluble Hg(II) in aged FGD wastes.... 151
bution of Hg in FGD wastes 152
soluble Pb in aged FGD wastes 153
bution of Pb in aged FGD wastes 154
soluble Zn in aged FGD wastes 155
bution of Zn in aged FGD wastes 156
A! (Ill) concentration in La Cygne
166
As concentration in La Cygne FGD
B(III) concentration in La Cygne
Cd(II) concentration in La Cygne
167
168
169
VI 1
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FIGURES (continued)
Number Page
86 Total soluble Ca concentration in La Cygne FGD
wastes 170
87 Total soluble Cr(III) concentration in La Cygne
FGD wastes 171
88 Total soluble Co(II) concentration in La Cygne
FGD wastes 172
89 Total soluble F(I) concentration in La Cygne FGD
wastes 173
90 Total soluble Fe(III) concentration in La Cygne
FGD wastes : 174
91 Total soluble Pb(II) concentration in La Cygne
FGD wastes 175
92 Total soluble Mg(II) concentration in La Cygne
FGD wastes .' 176
93 Total soluble Mn(II) concentration in La Cygne
FGD wastes 177
94 Total soluble Hg concentration in La Cygne FGD
wastes 178
95 Total soluble K(I) concentration in La Cygne FGD
wastes 179
96 Total soluble Se concentrations in La Cygne FGD
wastes 180
97 Total soluble Na(I) concentration in La Cygne FGD
wastes 181
98 Total soluble Zn(II) concentration in La Cygne
FGD wastes 182
99 Effects of ionic strength on the speciation of
sol uble Ca 189
100 Effects of ionic strength on the speciation of
soluble Cd(I I) 190
101 Effects of chloride concentration on soluble Cd
concentration 191
102 Effects of chloride concentration on soluble Cu
concentration 192
103 Effects of chloride concentration on soluble Pb
concentration 193
104 Effects of chloride concentration on soluble Hg
concentration 194
105 Effects of chloride concentration on soluble Zn
concentration 195
106 Effects of total sulfate concentration on soluble
Ca concentration 200
107 Effects of total sulfate concentration on soluble
Mg concentration 201
108 Effects of total sulfate concentration on soluble
K concentration 202
109 Effects of total sulfate concentration on soluble
Na concentration 203
vi 11
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FIGURES (continued)
Number
110 Effects of borate concentration on soluble Cu
concentration 205
111 Effects of borate concentration on soluble Pb
concentration 206
112 Effects of lime addition on the concentrations of
free ligands 208
113 Effects of lime addition on the total soluble
concentrations of major ions 209
114 Effects of lime addition on the total soluble
concentrations of minor ions 210
115 Effects of silicate addition on Al in FGD
waste water 212
116 Effects of silicate addition on Zn in FGD
waste water ;" 213
117 Effects of silicate addition on Ca in FGD
waste water 214
118 Effects of silicate addition on magnesium in FGD
waste water 215
119 Effects of silicate addition on K in FGD
waste water 216
120 Effects of silicate addition on Na in FGD
wastewater ..217
121 Effects of silicate addition on Cd in FGD
wastewater 218
122 Effects of silicate addition on Cr in FGD
wastewater 219
123 Effects of silicate addition on Cu in FGD
wastewater 220
124 Effects of silicate addition on Pb in FGD
wastewater 221
125 Effects of sulfide addition on the total soluble
levels of metals in the raw FGD waste 223
126 Effects of sulfide addition on the distribution
of sulfide species in the FGD waste 224
127 Effects of phosphate concentration on the total
soluble concentrations of metals 226
128 Effects of phosphate concentration on the total
soluble concentrations of metals 228
129 Effects of Mg addition on the distribution of
soluble Mg complexes 229
130 Effects of Mg addition on the speciation of Ca 230
131 Effects of Mg addition on the speciation of Cd 231
132 Effects of Mg addition on the speciation of
Cr(III) 232
133 Effects of Mg addition on the speciation of Cu 233
134 Effects of Mg addition on the speciation of Zn 234
135 Effects of sulfite oxidation on the concentrations
of sulfite complexes 236
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FIGURES (continued)
Number Page
136 Effects of sulfite oxidation on the primary
distribution of S03= species 237
137 Effects of sulfite oxidation on the speciation
of Ca 238
138 Effects of sulfite oxidation on the primary
distribution of Ca species 239
139 Effects of sulfite oxidation on the speciation
of Mg 240
140 Effects of sulfite oxidation on the primary
distribution of Mg species 241
141 Effects of sulfite oxidation on the speciation
Of K 242
142 Effects of sulfite oxidation on the primary
distribution of K species .' 243
143 Effects of sulfite oxidation on the speciation
of Na 244
144 Effects of sulfite oxidation on the primary
distribution of Na species 245
145 Effects of sulfite oxidation on the speciation
of Cd 246
146 Effects of sulfite oxidation on the primary
distribution of Cd species 247
147 Effects of sulfite oxidation on the speciation
of Cr 248
148 Effects of sulfite oxidation on the primary
distribution of Cr species 249
149 Effects of sulfite oxidation on the speciation
of Cu 250
150 Effects of sulfite oxidation on the primary
distribution of Cu species 251
151 Effects of sulfite oxidation on the speciation
of Fe 252
152 Effects of sulfite oxidation on the primary
distribution of Fe species 253
153 Effects of sulfite oxidation on the speciation
of Pb 254
154 Effects of sulfite oxidation on the primary
distribution of Pb species , 255
155 Effects of sulfite oxidation on the speciation
of Zn 256
156 Effects of sulfite oxidation on the primary
distribution of Zn species 257
157 Range of aluminum concentrations in aged FGD
sludge leachates by thermodynamic model
calculation 286
158 Range of arsenic concentrations in aged FGD
sludge leachates by thermodynamic model
calculation... 287
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FIGURES (continued)
Number
159
160
161
162
163
164
165
166
167
Range of
siudge
calcul
Range of
siudge
cal cul
Range of
siudge
calcul
Range of
si udge
calcul
Range of
siudge
calcul
Range of
si udge
cal cul
Range of
siudge
cal cul
Range of
siudge
calcul
Range of
leacha
cadmium concentrations in aged FGD
leachates by thermodynamic model
ation 288
boron concentrations in aged FGD
leachates by thermodynamic model
ation 259
cobalt concentrations in aged FGD
leachates by thermodynamic model
ation 290
copper concentrations in aged FGD
leachates by thermodynamic model
ation 291
iron concentrations in aged FGD
leachates by thermodynamic model
ation 292
manganese concentrations in aged FGD
leachates by thermodynamic model
ation 293
potassium concentrations in aged FGD
leachates by thermodynamic model
ation 294
sodium concentrations in aged FGD
leachates by thermodynamic model
ation 295
zinc concentrations in aged FGD sludge
tes by thermodynamic model calculation ... .296
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TABLES
Number Page
1 Major Composition of Sludge from Operating
S02 Scrubbers 3
2 Concentrations of Trace Elements in FGD
SI udges 4
3 Concentration of Constituents in FGD Scrubber
Liquors ;' 5
4 Common Solid Species of Metals in Nature 24
5 Important Solubility Products of Metals
(in pKsp) 33
6 Possible Chemical Species Existing in FGD
Wastes 68
7 Distributions of Chemical Species in Low-
Ionic-Strength Fresh FGD Wastewater (at
pH 7) 95
8 Distribution of Chemical Species in High-
.Ionic-Strength Fresh FGD Wastewater 101
9 Total Levels of Constituents in Aged FGD
Systems Used for Computation 107
10 Analytical Results of FGD Samples from KCP&L
La Cygne Power Station 162
11 Total Concentrations of Constituents in La
Cygne FGD System 165
12 Comparisons of the Analytical Results of FGD
Wastewater to the Results Predicted by
Computer Model 183
13 General Models Used for Speciation
Calculation 261
14 Predominant Species of Soluble Constituents
in Fresh FGD Wastewater 264
xi i
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TABLES (continued)
Number Page
15 Predominant Species of Constituents in Aged
FGD Sludge 268
16 Validity of the Thermodynamic Model for the
Prediction of FGD Sludge Speciation 272
17 Effects of Chemical Changes on the Speciation
of Constituents in FGD Sludge 273
18 Effects of Addition of'Chemical Compounds
on the Speciation of FGD Sludge
Constituents 278
XI 1 1
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ACKNOWLEDGEMENTS
This document is the product of a detailed thermodynamic
modeling of FGD sludge constituents, intended as a predictive
tool for estimating the environmental impact of FGD sludge dis-
posal to land. The competent guidance and assistance of Mr.
Donald E. Sanning, Project Officer, Municipal Environmental
-Research Laboratory (MERL), of U.S. EPA, Cincinnati, Ohio, on
this highly complex and technically advanced project are grate-
fully acknowledged. The assistance o.f Mr. Michael C. Osborne,
IERL/RTP, as a technical reviewer is al so... greatly appreciated.
SCS project participants were Curtis J. Schmidt, Project
Director; John P. Woodyard, Project Manager; and Dr. Jasenka
Vuceta, Project Scientist; Dr. James C. S. Lu, Cal Science
Research, Inc., served as the SCS project scientist on the spe-
ciation modeling and draft report preparation until 1978, and
thereafter served as a technical consultant to SCS.
xi v
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SECTION 1
INTRODUCTION
DESCRIPTION OF PROBLEM
The removaT of sulfur oxides .from power plant exhaust
gases to meet air quality standards (flue gas desulfurization,'
or FGD) is usually accomplished by wet scrubbing. These scrub-
ber systems are classified by the type of sorbent employed:
lime, limestone, or sodium salts (double alkali). Lime and
limestone sorbents are both effective and inexpensive relative
to other FGD alternatives , and as a result are currently the
most popular types of sorbents. These sorbents are also non-
regenerable; the sorbents are removed from the system after a
certain contact period. Because the ultimate disposal of the
spent sorbent sludges is usually accomplished on land, by pond-
ing or landfilling, a potential for detrimental environmental
effects exists from groundwater or surface water contamination
near the disposal site.
An important consideration when-assessing the potential
environmental impact of FGD sludge disposal is the chemical
forms of major and minor constituents in the sludge and leachate.
The mobility or attenuation of these impurities as they pass
through underlying soils depends upon their chemical forms
and is not necessarily a function of total concentration.
This is particularly true for metals, which may be transported
in soluble or particulate form. Conventional chemical
analysis only provides information on the total concentration,
not on the speciation of the elements present.
The only feasible means of obtaining species information in
a complex system (such as FGD sludge) lies in thermodynamic
modeling. This approach is not entirely successful when complex
organic materials exist along with inorganic materials. However,
FGD sludge may be an ideal subject for this approach because the
material is dominated by well-defined crystal phases and contains
no significant organic materials.
A wide variety of elements exist in FGD sludge, as either
dominant or trace species. The equations governing interactions
between all the species and phases present can be solved on a
computer, where it is also possible to explore the effects of
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various FGD operating changes on sludge chemistry without con-
ducting expensive field testing.
The scrubber operating mode may create nonequi1ibriurn con-
ditions, which manifest themselves in the growth rate of the
crystals during sludge formation. The crystal nucleation and
growth rate is controlled by operating parameters such as liquid
flow rates, sulfur dioxide removal efficiencies, hold tank
design, and point of reagent addition. Impurities absorbed on
the surfaces may be buried in the crystals. Whether these non-
equilibrium impurities buried in the crystal phases will achieve
equilibrium in a reasonable time during storage depends upon
solid state diffusion kinetics.
Even without fully accounting for the above effects, a thermo
dynamic model will show the migration trends of the constituents.
If the soluble level of trace metals in the FGD wastewater is
below the equilibrium level, it can be predicted that the con-
stituents will be released from the solid phase(s). Conversely,
when the analyzed soluble level exceeds the equilibrium level,
the dissolved forms will decrease in concentration with age. A
combined liquid and solid phase thermodynamic model could there-
fore serve as a useful prediction of both chemical species and
their concentrations in FGD sludge leachate.
FGD WASTE CHARACTERISTICS
The application of large-scale wet scrubbing technology for
FGD is gaining favor in the United States. The most popular of
the wet FGD systems are the lime/limestone processes. More than
half of the systems currently being considered or implemented
are of this variety. By the early 1980's these systems may
account for over 20,000 megawatts of generating capacity.
The physical and chemical properties of the wastes from wet
FGD processes are influenced by many interrelated factors, such
as fuel type and composition; boiler type, design and operation;
fly ash and bottom ash removal systems and their relation to
sludge generation; FGD system type, design, and operation; and
FGD reagent and input water quality. Because of the numerous
variables involved, the composition and quantity of FGD wastes
can vary over extremely wide ranges (Ref. 1). The general con-
centration ranges of constituents in FGD sludges and leachates
are listed in Tables 1 to 3.
Table 1 shows that the by-products on nonregenerable FGD
systems are typically composed of four major solid constituents:
calcium sulfate dihydrate (CaS04.2^0), calcium sulfite hemi-
hydrate (CaSOa .1/2H20), calcium carbonate (CaCOa), and fly ash.
The solid phase of FGD sludge also contains significant amounts
of magnesium, barium, iron, sodium, and potassium. There is
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TABLE 1. MAJOR COMPOSITION OF SLUDGE FROM OPERATING S02 SCRUBBERS1
Sludge composition (dry basis), wt percent
Fac 1 1 1 ty
Lawrence
Hawthorn 3
Hawthorn 4
Will County 1
Stock Island
La Cygne
Choi la
Paddy's Run 6
Mohave 2
Shawnee 1
Shawnee 2
Phillips
Parma
Scholz 1A
Utah
Col strip
Scrubber Sorbent
Limestone
Limestone
Limestone
Limestone
Limestone
Limestone
Limestone
L1me
Limestone
Limestone
Lime
Lime
Dual alkali
Dual alkali
Dual alkali
Lime/ alkaline ash
CaS03-l/2H?0
10
20
17
50
20
40
15
94
2
19-23
50
13
. 14
65-90
0.2
0.5
CaS04'2H?0
40
25
23
15
5
15
20
2
95
15-32
6
19
72
5-25
82
5-20
CaC03
5
5
15
20
74
30
0
0
0
4-14
3
0.2
8
2-10
11
0
Fly Ash Comments
45
50
45
15
1 Oil fired
15
65 14% CaS203-6H20
4
3
20-43
41
60 9.8$ CaS3010
7
0
9
40-70 5-30% MgS04
* Reference 2, 3.
t By-products on nonregenerable FGD systems are typically composed of four major solid constituents.
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TABLE 2. CONCENTRATIONS OF TRACE ELEMENTS IN FGD SLUDGES'
El ement
Arsenic
Beryl 1 i urn
Cadmium
Chromium
Copper
Lead
Manganese
Mercury
Nickel
Selenium
Zinc
Concentration
Ranges (ppm)
3.4
0.62
0.7
3.5
1.5
1.0
11 •
0.02
6.7
<0.2
9.8
- 63
- 11
- 350
- 34
- 47
- 55
- 120
- 6.0
- 27
- 19
- 118
Median
Concentration
(ppm)
33
3.2
4.0
16
14
14
63
1
17
7
57
Number of
Observations
9
8
9
8
9
9
5
9
5
9
5
Range of Trace
Elements Measured
in Coal (ppm)
3-60
0.08 - 20
-
2.5 - 100
1 - 100
3-35
-
0.01 - 30
-
0.5 - 30
0.9 - 600
* Reference 5.
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TABLE 3. CONCENTRATION OF CONSTITUENTS IN FGD SCRUBBER LIQUORS'
Constituents
Alumi num
Antimony
Arsenic
Beryl 1ium
Boron
Cadmium
Calci urn
Chromium (total )
Cobalt
Copper
Iron
Lead
Magnesium
Manganese
Mercury
Molybdenum
Nickel
Potassium
Seleni urn
Si 1 icon
Silver
Sodi urn
Range of Constituent Concentrations at
Potential Discharge Points
mg/1 (Except pH)
0.03 - 0.3
0.09 - 2.3
<0.004 - 0.3
<0.002 - 0.14
8.0 - 46
0.004 - 0.11
520 - 3,000
0.01 - 0.5
0.10 - 0.7
<0.002 - 0.2
0.02 - 8.1
0.01 - 0.4
3.0 - 2,750
0.09 - 2.5
0.0004 - 0.07
0.91 - 6.3
0.05 - 1.5
5.9 - 32
<0.001 - 2.2
0.2 - 3.3
0.005 - 0.6
14 - 2,400
M
10-5.95_1Q-4.95
io-6-13-io-4-72
-7.27
-10
-5.40
<10-6.65_10-4.81
10
-3.13.10-2.37
io-7-44-io-6-01
10-l-89.iQ-l.12
io-6-72-io-5-02
io-5-77-io-4-92
<10-7.50_1Q-5.50
10-6.45_10-3.84
10-7.32_10-5.71
10-3.91.10-0.95
10-5.79.10-4.34
10-8.70.10-6.46
io-4-71-io-4-18
10-3 .82_10-3 .09
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TABLE 3 (continued)
Range of Constituent Concentrations at
Potential Discharge Points
Constituents mg/1 (Except pH) M
Tin 3.1 - 3.5 iQ-4'58-io'4'53
Vanadium <0.001 - 0.67 <10"7*71-10-4*88
Zinc 0.01 - 0.35 10'6 '82-10'5 '21
Carbonate 41 - 150 lO-3-39-lQ-2-82
(as
Chloride 420 - 4,800 10"1-93-10"°'87
Fluoride 0.07 - 10 io~5'43-10~3*28
Sulfite 0.8 - 3,500 10"5•°°-10-1-36
Sulfate 720 - 10,000 10'2'12-10"0*98
Phosphate 0.03 - 0.41 10-6.50_1Q-5.36
pH 3.04 - 10.7 10"3*04-10"10-7
Ionic strength 0.05 - 0.80
* Reference 4.
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also a wide variety of trace metals contained in the solid phase
as shown in Table 2. These solid constituents in raw FGD sludges
can originate in the fly ash, sorbent, or makeup water.
The liquid phase of FGD wastes is important due to its
potential as leachate. As can be seen in Table 3, the FGD
liquors typically contain high soluble levels of sulfate, sul-
fite, calcium, magnesium, sodium, potassium, chloride, carbonate,
and also various trace chemical species. The concentrations of
these constituents range from trace amounts (e.g., trace metals)
to as high as 10,000 ppm (e.g., sulfate). However, these con-
stituents are usually in a nonequi1ibriurn condition. In fact,
most of the major chemical species are oversaturated. After a
certain time period, the effects of precipitation, dissolution,
redox reaction, complexation, or adsorption could affect the
redistribution of the chemical species. Chemical analysis data
is usually available only for fresh FGD sludge. Concentration
data for constituents in aged FGD sludge are less available.
FGO processes employ inorganic reagents and caustic solu-
tions, and are subject to high temperature exhaust gases. These
factors do not create an environment conducive to biological
activity. The organic species in the FGD wastes therefore exist
at nondetectable levels, which will increase the accuracy of
any inorganic equilibrium model.
AVAILABLE THERMODYNAMIC MODELS
Comparing the sludge equilibrium chemical composition
derived from a thermodynamic model with that of the actual solid-
aqueous system can provide a clearer understanding of the chem-
ical behavior of the system. An FGD process can be represented
by an array of chemical reactions, including the transfer of mass
from reactant species (either solid or soluble species) to other
species in the system. Due to the oversaturation of the species
in most FGD systems and the high reactivity between the consti-
tuents in flue gas and in scrubber liquor, the components in the
scrubber are commonly in a state of nonequi1ibrium or partial
equilibrium during the scrubbing process. The partial equili-
brium may occur among species in the liquid phase, due to the
relatively high rate of complexation reactions. However, the
equilibrium between the solid phase and soluble phase (in FGD
liquor) may not be reached so quickly due to kinetic constraints
(Ref. 6, 7, 8).
Many techniques can be used for constructing and interpret-
ing a chemical thermodynamic model for the calculation of the
equilibrium condition of a complex system. The first step in
the equilibrium calculations is to identify the components and
phases in the system. The next step is to identify the maximum
number of unknown activities with the number of independent
-------
relationships that describe the system, such as the equilibrium
constant for each reaction, sto\chiometrie conditions, and elec-
troneutrality conditions in the solution phase. With the phase-
composition requirements identified and with adequate thermo-
dynamic data (free energies, equilibrium constants) available,
chemical equilibrium in the closed system is then assumed. The
composition variables (activities, partial pressures, mole frac-
tions) of the system are then computed.
The actual calculation of chemical equilibrium may be per-
formed using the following methods:
• The equilibrium constant approach (or K approach)
• The Gibbs free energy of reaction and reaction quotient
approach (or AG and Q approach)
• The total Gibbs function minimization approach (or G and
£ approach)
,"-
• The mass transfer approach (or M approach)
• The nongeneralized approach.
In the equilibrium constant approach, stoichiometric equa-
tions involving all possible chemical speci es are set up and
solved subject to constraints imposed by the equilibrium con-
stants, mass balance and charge balance relations. This method
was pioneered by Brinkley (Ref. 9, 10) and further developed by
Feldman, et al. (Ref. 11), Morel and Morgan (Ref. 12) and Crerar
(Ref. 13).
In the Gibbs free energy and reaction quotient approach, the
free energy for each reaction, AG, is computed from
AG = G° + RT In Q (1)
or
AG = RT In | (2)
subject to the stoichiometric constraints. At equilibrium,
AG = 0 and the composition is then the equilibrium composition
(Ref. 6).
In the total Gibbs function minimization approach, the
optimization techniques are used to minimize the total Gibbs free
energy function. This method, again, is subject to mass and
charge balance constraints. This method was first proposed by
White, et al. (Ref. 14), then modified and extended by many
researchers, including Naphtali (Ref. 15) and Karpov and Kazmin
(Ref. 16).
8
-------
The concentrations of these two species at varying pH levels are
shown in Figure 18. Note that the soluble levels are relatively
unchanged throughout the entire pH range.
Sodium
The results of the speciation of sodium in fresh FGD waste-
water at I = 0.05 is presented in Figure 19. The distribution of
soluble species for sodium is quite similar to that of potassium,
with the exception of the presence of NaCO^.
Cadmium
Figure 20 displays the speciation of cadmium in fresh FGD
wastewater at I = 0.05. Cadmium can form strong sol-uble com-
plexes with Cl" and SOf. At high pH levels (pH >8) the Cd-C03
species will also become significant. When the pH is below 8,
the relative concentrations of soluble cadmium species in FGD
wastewaters are as follows:
Cd2+ > Cd-Cl complexes (mainly CdCl+) > CdS04(aq)
Cd-C03 complexes (mainly CdKC03+) > Cd-OH complexes
(mai nly CdOH ).
When the pH is above 8, the concentrations of the Cd-C03
complex (primarily CdC03(aq) and Cd-OH complexes (primarily
Cd(OH)2(aq)) increase significantly; free metal ion, Cd^*, and
CdSQ4(aq) concentrations show a corresponding decrease.
Chromium
Figure 21 shows that the Cr-OH complexes (including CrOH +,
Cr(OH)j, and Cr(OH)5 are the predominant soluble chromium species
in fresh FGO wastewater when the pH is greater than 4. The
speciation calculation shows that CrOH2+ is predominant (50 to 79
percent of the total soluble chromium) between pH levels of 4 and
5. Between pH levels of 5 and 7, Cr(OH)£ will predominate (50 to
90 percent). At a pH greater than 7, the Cr(OH)4 species can
account for almost all soluble chromium. This is consistent with
the stability field calculation in Section 3 (see Figure 6).
Aside from the OH" complexes, free Cr is the next most
common species when the pH is below 4. Other complexes such as
CrS04, CrHPOj, Cr-Cl complexes (mainly CrCl2+), and Cr-F
complexes (mainly CrF2+) can also exist in the FGD wastewater at
very low concentrations.
-------
The mass transfer approach was developed by Helgeson (Ref.
17-19). Differential equations providing for simultaneous
dissolution of multiple reactant minerals, precipitation of
mineral assemblages, variable activity of HgO, oxidation reduc-
tion reactions, binary solid solution, and changes in activity
coefficients in both open and closed systems are incorporated
in a grand matrix equation for describing mass transfer. Com-
puter and thermodynamic data permit mass transfer calculations
to be carried out for a complex system under a variation of
temperature and pressure.
The nongeneralized approach entails specific, as opposed to
generalized, calculations. Here, a set of equations describing
a given system is reduced to one or more equations amenable to
simple numerical solution. Typical examples are Butler (Ref.
20), Helgeson (Ref. 21), Stumm and Morgan (Ref. 6), Crerar and
Anderson (Ref. 22), and Lu (Ref. 23).
PROJECT OBJECTIVES
^
As discussed previously, constituents in FGD wastes (both
sludges and leachates) can exist in various chemical forms with
substantial differences in mobility and pollution potential.
However, documentation of constituent speciation in FGD wastes
is still lacking. A thermodynamic model that can be used to
characterize the distributions, migration trends, stability
fields, concentration levels, and environmental effects of the
constituents is therefore desirable.
In this study, a thermodynamic equilibrium model suitable
for evaluating the chemical speciation of FGD waste constituents
is evaluated. The Eh-pH plot and ion-ratio methods are also
used to construct the stability field of the species.
In order to perform the stability field and speciation cal-
culation, collection, and evaluation of existing FGD waste data
and thermodynamic data was necessary. The FGD waste data in-
cludes concentrations of various constituents in solid and solu-
tion phases. The thermodynamic data including available informa-
tion on liquid phase interactions between all species present in
the FGD wastes, together with the information on possible solid
species, interactions between the soluble species and solid sur-
faces, as well as the solid-solution effects.
After stability field and speciation models were constructed,
verification of the calculated results with actual chemical
analyses was performed. It is impossible to verify the models
directly by chemical analysis data since both the distribu-
tion of solid and soluble species of a constituent in the FGD
system cannot be determined experimentally. However, the models
can be verified by the migration trends of the constituents as
well as the ultimate concentration levels in the aged FGD wastes.
10
-------
The models were then used to determine the effects of vari-
ous changes in the FGD system or sludge treatment system on the
concentration and chemical form of the impurities of interest.
Eleven specific investigations were conducted:
• Effects of pH on speciation
• Effects of ionic strength on speciation
• Effects of chloride concentrations on the solubilities
of metals
• Effects of sulfate concentrations on the solubilities
of metals
• Effects of borate concentrations on the solubilities of
metals
• Effects of lime addition on FGD was.ies
• Effects of silicate addition on FGD wastes
• Effects of hydrogen sulfide addition on FGD wastes
• Effects of phosphate addition on FGD wastes
• Effects of magnesium addition on FGD sorbent
• Effects of sulfite oxidation.
11
-------
-------
SECTION 2
PRINCIPLES AND METHODOLOGIES FOR
INVESTIGATIONS INTO CHEMICAL SPECIATION OF FGD SLUDGE
THE STABILITY FIELD OF CONSTITUENT SPECIES
Two principal graphical treatments have been used to
describe the stability relationships of the distribution of the
various soluble and insoluble forms of.constituents in the
aqueous solution: Eh-pH plots and the ion-ratio method (Ref. 6,
23). The Eh-pH stability field diagram shows the simultaneous
effect of protons and electrons on the equilibria under various
Eh and pH conditions, and can thus indicate which species pre-
dominate under any given condition of Eh and pH. This method is
useful for constituents such as iron, manganese, mercury,
arsenic, and selenium, which appear in nature in different oxi-
dation states. However, for other constituents with only one
oxidation state, the Eh-pH approach becomes unsuitable. In the
latter case, the ion-ratio method can be used. The ion-ratio
method shows the most stable solid phase by comparing the relevant
reaction constants and ion ratios. Details are given in the
following pages.
Eh-pH Stability Diagrams
The Eh-pH stability diagram of a specific constituent can
be constructed using mass laws and concentration conditions for
that constituent. The general procedures are as follows:
• Identify all the species present in the system
• Identify all the possible reactions among the species
in the system
• Set up the mass equations by relating the stability
constants and the molar concentrations of the possible
reactions
• Plot the resulting equations on a graph with Eh and pH
axes
12
-------
The following is an example of the calculated stability
field for selenium in the FGD system using the Eh-pH approach.
Possible species of selenium include:
Solid - Se°
Soluble - H2Se03, HSeO^, HSeO^, SeO2" , SeO2"
The associated equilibrium conditions are as follows:
Se° + 3H0 d^" HSe03 + 5H+ + 4e~ K = 10"52'3 (3)
Se° + 3H20 ^" Seo|~ + 6H+ + 4e" K = 10~58'8 (4)
Se° + 3H20 — H2Se03 + 4H + + 4e~ K = 10"49'8 (5)
HSeO" — Se02~ + H+ K = 10"5'53 (6)
H2Se03 ^H^ HSeO^ + H+ K = 10"2'55 (7)
• HSeO^ + H20 ^=^ Se02"+ 3H+ + 2e~ K = 10"36'1 (8)
Se02"+ H20 ^^ Se02"+ 2H+ + 2e~ K = 10"29'5 (9)
The concentration condition is as follows:
[Se,.] = 1.4 x 10~ M (total selenium concentration)
The resulting mass equations corresponding to Equations 3
through 9 are as follows:
Redox Couple Equation (at 1=0, T=25°C)
Se° - HSeO^ 5 pH + 0.24 Eh = 47.5 (10)
6 pH + 0.24 Eh = 54.5 (11)
Se° - H2Se03 4 pH + 0.24 Eh = 44.9 (12)
HSe03 - SeO2" pH = 6.53 (13)
H2Se03 - HSe03 pH = 2.55 (14)
HSe03 - SeO2" 3 pH + 0.12 Eh = 36.1 (15)
SeO2"- SeO2" 2 pH + 0.12 Eh = 29.6 (16)
Equations 10 through 16 can then be plotted on the Eh-pH diagram,
as shown in Figure 13 (see Section 3).
13
-------
Due to the wide variety of constituents in the FGD system,
the construction of Eh-pH* diagrams first requires that the
speciation model identify the important soluble species. In the
construction of the Eh-pH diagram for mercury, for example, the
HgClg (aq) complex may become one of the predominant species.
Therefore, for FGD systems, mercury should be considered in an
Hg-H20-Cl system instead of an Hg-H20 system.
Ion-Ratio Method
The ion-ratio method can be used to identify the most
abundant or the most stable solid of a constituent by comparing
all the concentrations of anions which comprise the possible
solid species of that constituent. For example, if comparing
two solid compounds of metal M, Mm.Xn and MpYq, the reactions are
MmXn(s) = m M + z + n X~r (17)
MpYq(s) = p M+Z + q Y;S (18)
where m, n, p, q, z , r, and s are positive integers and,
M,. = free metal ion with + z valence
X"r = free anion with -r valence
Y~s = free anion with -s valence
The mass equations become
(20)
where y is the activity coefficient.
The free metal ion concentrations, controlled by solids
MmXn and MpYq, can be solved by equations 19 and 20, respectively,
as shown below:
(K
,M+z, _ _ ^ * m n
' "
(K )P
-
14
-------
From equations 21 and 22, the ratio of the free metal ion
concentrations can be calculated as follows:
I
(23)
f
the solid MpYq will
is MYq is more
If the result of equation 23 is >1 , then
become the solubility controlling sol.id; that s p
stable than MmXn. If the result is <1 , the situation will be
reversed. Therefore, the right-hand side of equation 23 can
exist under three conditions:
[Y
[X
"fSl
VI
q/
n/
p
m
(y
(Y
X
Y
f
r
r
s
^n/m
)q/p
(Ksp,
(KSP,
M/)1
M X ^
/P
/m.
(24)
The value of
if the conditions
stant value is R,
the right-hand side of equation 24 is constant
of the system are known. Assuming this con-
then
[x-r]n/m
> R
(25)
means MY is more stable than MX. If
[X-r]n/m
(26)
this means MmXn is more stable than MpYq. If more than two solid
compounds of a constituent can exist in the system, then the com-
parison should be made among all the possible ion ratios of the
anions to obtain the corresponding R values. In this way, the most
stable solid will be identified and the remainder screened out.
THE SPECIATION MODEL
Soluble cations (such as trace metals) in a complex system
will not exist as a bare ion (i.e., free ion) alone. These
cations will instead combine with molecules or anions containing
free paris of electrons (bases) in the solution phase. This
phenomenon is called complex formation or coordination.
In general, the metal cation (i.e., central atom) will be
surrounded by the anions or molecules;, these surrounding species
15
-------
are called ligands. The nearest neighbor atoms to the central
atom constitute the first or inner coordination sphere, and the
number of atoms in this first coordination sphere is the coordi-
nation number of the central atom. Complexes with coordination
numbers from two to nine are known, but most exhibit two-, four-,
of six-fold coordination. Complexes with different coordination
numbers will exhibit different properties even when they have
the same metal cation. Therefore, it is important to know the
species (coordination number and metal cation) of a complex in
order to evaluate its mobility. In a complex system, the thermo-
dynamic model approach is the only way to obtain this information.
Case 1: No Solids Present
In a system where there is no solid present or no migration
of constituents between solid and liquid phases, equilibrium
among soluble species is easily reached. The relative distribu-
tion of all soluble species can be characterized by one of the
five methods described previously. In this study, the equilib-
rium constant approach will be used.
The actual mathematical equilibrium model solves a series
of simultaneous equations which describes the interactions among
components of the system. For any given metal M(i) and ligand
L(j), these equations can be expressed as follows:
[M(DmUj)n! • B(i,j)nm fH(1)f]- (L(J)fIn ' lSiii_ItIll(27)
k 1 h
[M(i)T] = [M(i)f] +1 E _E m [M(i )mL( j )nl (28)
k 1 g
[L(j)T] = [L(j)J + E E E n [M(i) L(j)J (29)
I T i i .: _ i m M
where :
[M(i)T] = total soluble metal concentration of ith metal
(in mol es/1 i ter )
[L(j)-r] = total soluble ligand concentration of jth ligand
(in mol es/1 i ter )
[M(i)f] _ free concentration of ith metal
[L(j)] = free concentration of jth ligand
i = metal species
j - ligand species
16
-------
[M(i)mL(j)nl = concentration of complex M(i) L(j)
k = maximum number of metals M(i) coordinating ligands
L(j)
1 = maximum number of ligands L(j) coordinating metals
M(1)
g = total number of metals
h = total number of ligands
(i.j)_m = overall formation constant of complexes
nm M(1)mL(J)n. and
y = thermodynamic activity coefficient of species x.
/\
(In general, multi-salt ligands are negligible and therefore are
omitted in the above equations.)
In order to solve the above three equations, data are needed
for overall formation constants, activity coefficients and total
concentrations of metals and ligands in the system. In an FGD
system, the major metal species considered are calcium, magne-
sium, potassium, sodium, iron, manganese, copper, cadmium, zinc,
nickel, mercury, lead, cobalt, silver, chromium, aluminum,
beryllium, tin, and hydrogen. The major ligands are carbonate
(COs-), sulfate (S0| }, chloride (Cl~), fluoride (F~), phosphate
(P0|-j, silicate (SiO?"), borate (8(08)4), sulfite (S0§-),
hydroxide (OH~), molybdate (MoO§- ) , arsenate (AsO$-), bivanadate
(HVOJ-), and selenite (SeO|").
The overall formation constants used in this study are com-
piled from the work of Sillen and Martell (Ref. 24, 25), Ringbom
(Ref. 26), and Garrels and Christ (Ref. 27). Individual activity
coefficients for the soluble species are calculated from the
Davies modification of the Debye-H'uckel expression by using
A = 0.52 (Ref. 28):
log T7 = 0.51 z2 (— -- 0.31), (30)
2 1 + /I
where :
z = valence of the soluble species, and
I = ionic strength of the solution.
A computer is necessary for solving equations 27, 28, and
29 simultaneously, as the expanded equations number in the
hundreds. The resultant nonlinear equations are solved by
17
-------
Newton-Raphson iteration. A detailed description of the computer
model is contained in Morel and Morgan (Ref. 12) and McDuff and
Morel (Ref. 29).
Case 2: Solid and Gas are Present
If a system contains liquid, solid, and gas phases, the
distribution of a constituent is also affected by the solubility
products and Henry's constants of its constituent species. For
metals under equilibrium conditions, the concentration levels of
various soluble species are controlled by the solubilities of
the solids. For volatile constituents, both solid and gas spe-
cies can control the soluble levels of these constituents in the
solution phase.
If there is only one solid species, MpXq, for a given metal
M, then the free metal ion concentration can be regulated at the
following level under the equilibrium condition:
[Mf] =1 n „ * MJ (3D
where:
[Xf] = concentration of free anion (in moles/liter)
K = solubility product of solid M X .
sp J p q
This free metal ion can react further with ligands in the
system and form complex species. The concentration of the metal
complex can be solved as follows:
m
v
[L(1)f]n . Y"YL(i) (32)
By combining equations 31 and 32, the total soluble concen-
tration of the metal can thus be solved as shown below:
[MT] I [M ] + Z t Z m [ML(j)n] = [M.] +
1 r m = i n = l j = l m n f
k 1 h m n
mB(i)nm[Mf]m [L(j)f3n . J (33)
J.I nm f f ^M L(j)
18
-------
In order to solve equation 33, the data on solubility
products, ligand species and concentrations, overall formation
"constants (3(i)nm), and activity coefficients are needed. If
the solubility controlling solids of each ligand are known, the
same procedure (equations 31, 32, and 33) also can be used to
solve for the free ligand concentrations. If the total concen-
trations of ligands are known, then solving for the free ligand
concentrations should follow the same procedures as mentioned
in the previous section (using the simultaneous solution of
equations 27 through 29).
The solids occurring in nature are seldom pure solid phases,
i.e., more than one solid species controls the solubility of a
constituent. Isomorphous replacement by a foreign component in
the crystalline lattice is an important factor by which the con-
centration of the constituent may -be decreased. This phenomenon
is called the solid-solution effect.
To characterize the sol id-sol ution' effect on the solubility
of a given metal, M, consider a heterogeneous system where solid
MuXy(s) as solute become dissolved in another solid MpYq as the
solvent. The reaction may be characterized by the equilibrium
uMpYq(s) +pvX'r =PMuXv(s) +uqY'S (34)
The equilibrium constant for equation 34 (the distribution con-
stant D) corresponds to the quotient of the solubility product
constants of M Y (s) and MuXy(s)
Ypu[Mf]puypvx[xf]pv _ K
fX ' •
{36)
(37)
The activity ratio of the solids may be replaced by the mole
fractions multiplied by activity coefficients:
(38)
fMpYq (39)
19
-------
where :
NM x
I> = _ "_v _ (40)
_ __
M Y N + N
PI \Xv MpYq
The total amount of M in the system will become
k 1 h c d
[MT] - [M,] + Z Z E m[M'L(j)n] + E I u [M X (s)]
1 f m = i n = i j = i m n u = i v = l u v
a b ' (42)
+ Z Z p[MY(s)],
p-1 q-1 P q
where [MuXv(s)] and [MpYg(s)] are the molar concentration of
solids based on the solution volume. Limits a, b, c, and d
represent the maximum numbers of metals or ligands in the solids
In equation 42, [Mf] should be solved simultaneously using
equations 35 and 36. If there are more than two solids of M
involved, [Mf] should be calculated by solving all the mass
equations (similar to equations 35 and 36) simultaneously. The
same procedures can be used to solve for [L(i)f] if L(i) is con-
trolled by more than one solid species. If a gas phase is in-
volved, the same type of equations also can be derived by substi-
tuting solubility products for Henry's constants.
Therefore, in order to characterize a system which includes
solid, gas, and liquid phases, the following general equations
should be solved simultaneously:
m r n
[M(i)mLU)n] - B(i,j)nm[M(i)f]-[L(j)f]n ' MillkUl. (43)
(44)
20
-------
v U • v V
YM(i) YL(j)
p, q=1 MdJpLU),,- (46)
2 2 2 RM(n ,(i) - 1 (47)
1=1 u-1 v = l "^'u'-tJJv
k 1 h
[M(1)T] = [M(1)f] + I 2 Z m[M(i)mL(j)J
1 r m = i n = i j = i m n
h a b
+ £ Z Z p[M(1) L(j) J
j-1 p=l q=l P q
h c d
E n[M(1) L(j) ] (48)
m n
k ] §
• tLU)^rJ + I- *••» • ,m- »„ , n.
gab
2 2 2 q[M(i)L(j)J
1=1 p = l q = l P ^
Z Z Z [M(1)uL(j)v] (49)
where:
[M(i)mL(j)n] = concentration of complex M(1)_L(j)_ (in
mn i/i»j.\ in n
moles/11ter )
[M(i)J = free metal ion concentration of ith metal
(in moles/liter)
[L(j)^j = free concentration of jth ligand (in
moles/1i ter)
[M(i)-r] = total concentration of ith metal in the
system (in moles/liter)
21
-------
RM(T)pL(j)q
and
RMMv 1/M = mole fraction of solid or gas species for
^^u u;v metal or ligand solids
i = metal species
' j = ligand species
g = total number of metals
h = total number of ligands
k = maximum number of metals M(i) coordinating
1 i g a n d s L ( j )
1 = maximum number of ligands L(j) coordinating
metals M(i)
a,b,c, and d = positive integer showing maximum number of
the composition of metals or ligands in the
solids or gases
8 ( i > J ) = overall formation constant of complex
Y = thermodynamic activity coefficient of soluble
x species x, and
f = thermodynamic activity coefficient of solid
(or gas) species x (in this study, assume
x - 1 ) .
K = solubility products or Henry's constants.
In order to solve the above equations simultaneously, the
information on metal and ligand species, overall formation con-
stants, solubility products (or Henry's constants), and activity
coefficients must be known.
The computer model used in this study follows the simul-
taneous solution methodology used by Morel and Morgan (Ref. 12)
and McOuff and Morel (Ref. 29) with some minor modifications.
The major metals and ligands present in FGD sludge were noted
previously. The overall formation constants, solubility pro-
ducts, and Henry's constants were compiled from the literature
(Ref. 24-27). The activity coefficients for soluble species
are followed by Davies modification of the Debye-Huckel expres-
sion.
22
-------
-------
SECTION 3
STABILITY FIELD OF SOLID SPECIES
IN FGD SLUDGE
COMMON SOLID SPECIES AND THERMODYNAMIC DATA
Knowledge of the solid specie's in FGD sludge is important to
evaluate both the migration trends and levels of contaminants.
The solid species in the raw FGD wastes originate mainly in
fly ash, undissolved sorbent, bottom ash, and new precipitates.
Due to the nonequi 1 i bri urn conditions of the''raw FGD wastes, the
original solid species in the FGD system may be gradually trans-
formed to another species and subsequently affect contaminant
mobility as the wastes are aging. Stability field analyses can
be used to derive these transformation trends. In order to per-
form these stability field analyses, information on common solid
species and their thermodynamic data are required.
The common solid species of metals in nature are compiled in
Table 4. This table follows the information compiled by Lu
(Ref. 23). Additional information in this table is from Wedepohl
(Ref. 30), Energlyn and Brealey (Ref. 31), Garrels and Christ
(Ref. 27), Garrels (Ref. 32), Latimer (Ref. 33, Stumm and Morgan
(Ref. 6), Krauskopf (Ref. 34), Leckie and James (Ref. 7), and
Weber and Posselt (Ref. 35). The important solubility products
of these metallic solids are compiled in Table 5. These data
are mainly from Latimer (Ref. 33), Sillen and Martell (Ref. 24,
25), and Ringbom (Ref. 8) .
In the stability field analyses performed in this study, the
solids considered are limited to simple metallic solids. This is
because simple solids are usually more active than complex
solids. Such active solids may persist in metastable equilibrium
with the solution and may convert ("age") slowly into inactive
forms (Ref. 6). As can be seem from Tables 4 and 5, most of the
simple metallic solids in the FGD system are oxides, hydroxides,
carbonates, sulfites, sulfates, phosphates, and simple silicates.
Due to the slow nucleation rates and dissolution rates of the
complex solids (especially complex silicates), it is not likely
that they will play important roles in the regulation of soluble
species; they will therefore be omitted in the stability field
analysis.
23
-------
TABLE 4. COMMON SOLID SPECIES OF METALS IN NATURE'
Aluminum
Oxides:
Hydroxides:
Phosphates:
Silicates:
Antimony
Native:
Oxides:
Hydroxides:
Simple
Sulfides:
Compl ex
Sulfides:
Arsenic
Native:
Oxides:
Compl ex
Oxides:
Simple
Sulfides:
Complex
Sulfides:
Hal ides:
A1203 (corundum)
A1(OH)3 (gibbsite)
A1P04, A1(H2P04)(OH)2
AloSioOc (kaolinite), NaAlSioOp (albite)
£ £ 3 O O
CaAl2Si208 (anorthite), KAl3Si3010(OH)2(K-mica)
KAlSi3Og (K-feldspar), NaQ<33Al2<33Si3 67°lo(°H
(Na-montmorillonite)
Can o7Al/i c7Si7 -n09n(OH)/, (Ca-montmorillonite)
u»oo t• o/ / »oo cu H1
Sb°
Sb(OH)3, Sb(OH)3Cl2
(cervanite)
AgSbS2, Ag3SbS3 (pyrargyrite) , Cu^
2PbS ' Sb2S3 (jamesonite), 3Cu2S *
3(PbCu2)S . Sb2S3 (bournonite)
(tetrabedrite)
(famatinite)
As°
As203, Ca3(As04)2
Ag3As03, Ag3As04, Ca3(As04)2
As2S3, As2S5, As4S3, AsS (realgar)
FeAsS (mispickel), CoAsS (cobaltite), Ag3AsS3 (proustite)
Cu3AsS4 (enargite), AgAsS2
AsBr3, AsI3
24
-------
TABLE 4 (continued)
Beryl 1i urn
Oxides:
Complex
Oxides:
Hydroxides:
Simple
Sulfides:
Sulfates:
Hal ides:
Silicates:
Other:
Cadmi urn
Oxides:
Hydroxides:
Carbonates:
Sulfides:
BeO (bromellite)
BeO . Al70o (chrysoberyl)
Cm O
Be(OH)2 amorphous, cc-Be(OH)2> p-Be(OH)2, BeO
BeS
Be(OH)
BeCl2, BeBr2, BeI2, Na2BeCl4, K
3BeO ' A1203 • 6Si02 (beryl), (Zn,Fe)2(Fe2S)Be(Si04)3
(helvite)
NaCaBeF(Si03)2 (leucophane), Be2Fe(YO)2(Si04)2
(gadolinite)
Be(V03)2, BeMo04
CdO (monteporrite)
Cd(OH)2
CdC03 (otavite)
CdS (greenockite)
Calcium
Hydroxides:
Carbonates:
Simple
Sulfides:
Sulfates:
Phosphates:
Ca(OH)2
CaC03 (calcite), CaC03 (aragonite), CaMg(C03)2 (dolomite)
CaS (oldhamite)
CaS04, CaS03, CaS04 • 2H20, CaS03 * 1/2H20
Ca2P207, CaHP04, Ca3(P04)2, CaH2(P04)2, Ca5OH(P04)3
25
-------
TABLE 4 (continued)
NaCaFBe(Si03)2 (leucophane),
(laumontite)
CaSi03 (wollastonite), CaO * MgO * 2Si02 (diopside)
CalQMg2Al4(Si207)2(Si04)5(OH)4 (idocrase)
CaAl2Si2Og (anorthite), CaQf33Al433020(OH)4
( Ca-montmori 1 1 oni t e)
CaF2> CaBr2, CaI2
Silicates:
Hal ides:
Chromi um
Oxides:
Hydroxides:
4H20
FeO ' C
Cr(OH)3
(chromite), PbCr04 (crocoisite) ,
Cobalt
Oxides:
Hydroxides:
Carbonates:
Simple
Sulfides:
Compl ex
Sulfides:
Sulfates:
Phosphates:
Silicates:
Copper
Native:
Oxides:
Hydroxides:
Carbonates:
Simple
Sulfides:
CoO, Co203, Co304
Co(OH)3, Co(OH)2
CoC03 (spherocobaltite)
CoS, Co(HS)2
CoAsS
Co(S04)2 ' H20, Co(OH)li5(S04)0>25
C03(P04)2, CoHP04
Co2Si04
Cu°
Cu20 (cuprite), CuO (tenorite)
CuCl2 ' 3Cu(OH)2 (ataramite), Cu(OH)2
Cu2(OH)2C03 (malachite), Cu3(OH)2(C03)2 (azurite)
Cu2S (chalcocite), CuS (covellite)
26
-------
TABLE 4 (continued)
Complex
Sulfides:
Sulfates:
Silicates:
Iron
Oxides:
Hydroxides:
Carbonates:
Sulfides:
Sulfates:
Phosphates:
Silicates:
Lead
Native:
Oxides:
Hydroxides:
Carbonates:
Sulfides:
Sulfate:
Hal ides:
(chalcopyrite), Cu^FeS4 (bornite)
> (enargite), (Cu,Fe)12Sb4S13 (tetrahedrite)
Cu4(OH)gS04 (brochantite), CuS04 * 5H20 (chalcanthite)
CuSi03 • nH20 (chrysocolla), CuO ' Si02 * H20 (dioptase)
Fe203 (hematite), FeOOH (geothite), Fe304 (magnetite)
FeOOH * nH20 (limonite)
Fe(OH)3, Fe3(OH)8 (ferrosofferric hydroxide)
FeC03 (siderite)
FeS2 (pyrite), Fe^_xS (pyrrhotite), FeS (machinawite)
Fe3S4 (greigite)
KFe3(OH)6(S04)4 (jarosite)
FeP04
FeSi03 (glauconite), (Fe(II), Fe(III), Mg,Al)
(Si,Al)07>3_5(OH)4_1 (chamosite)
Pb°
PbO (massicot), Pb02 (plattnerite), Pb304 (minimum)
PbCr04 (crocoite), PbMo04 (wulfenite)
Pb(OH)2
PbC03 (cerussite), Pb3(OH)2(C03)2 (hydrocerussite)
PbS (galena)
PbS04 (anglesite)
3Pb3As208 ' Pbd2 (mimetite), 3Pb3V208 * PbCl2
(vanadinite)
27
-------
TABLE 4 (continued)
Magnesium
Oxides:
Hydroxides:
Carbonates:
Simple
Sulfides:
Sulfates:
Phosphates:
Hal ides:
Silicates:
Manganese
Simple
Oxides:
Compl ex
Oxides:
Hydroxides:
Carbonates:
Sulfides:
Silicates:
MgO (periclase), Mg7Cl2B1603g (boracite)
MgAl204 (spinel)
Mg(OH)2 (brucite)
MgCa(C03)2 (dolomite), MgC03 (magnesite), MgC03
(nesquehonite)
3MgC03 ' Mg(OH)2 ' 3H20 (hydromagnesite)
MgS
MgS04
MgNH4(P04), Mg3(P04)2, MgNH4(P04)(H20)6, MgK(P04
MgHP04(H20)3
MgF2, KMgCl3(H20)3, MgCl2(H20)6, MgCl2
MgSi03 (clinoenstatite), Mg2Si04 (forsterite)
Mg3Si401Q(OH)2 • nH20 (vermicul ite) , Mg3Si401Q(OH)2 (talc)
Mn02 (pyrolusite), Mn304 (hausmannite) , MnOOH or Mn03
(manganite)
Mn0^i2 to Mn02 (nonstoichiometric oxides)
(Mn,Si)203 (braunite), Mn304 * Fe304 (vrendenburgite)
(Mn,Fe)203 (bixbyrite), (Mn(II)Fe)(Mn(III)Fe)204
(jacobsite)
BaMn(II)Mn(IV)8Ol6(OH)4 (psilomelane)
Mn(OH)2 (pyrochroite), Mn(OH)3
MnC0 (rhodochrosite)
03 (rhodochrosite)
MnS (alabandite)
MnS (alabandite)
MnSi03 (rhodonite), Mn3Al2(Si04)3 (spessartite)
28
-------
TABLE 4 (continued)
Mercury
Native:
Oxides:
Hydroxides:
Sulfides:
Sulfates:
Halides:
Molybdenum
Oxides:
Simple
Sulfides:
Phosphates:
Hg°
HgO, HgSb^Oy (livingstonite)
Hg(OH)2
HgS (cinnabar)
HgS04 ' 2HgO
HgCl2, Hg2OCl, Hg4OCl2, Hg2Cl2 (calomel)
Mo03 (molybdine), Mo02, H2Mo04, PbMo04 (mulfenite)
MoS2 (molybdenite), MoS3, MoS4
Mo(P03)6
Nickel
Oxides:
Hydroxides:
Carbonates:
Sulfides:
Sulfates:
Silicates:
Ni02, Ni203, Ni304, Ni304, Ni3As20Q • 8H20 (annabergite)
Ni(OH)2
NiC03, NiC03 ' 2Ni(OH)2 • 4H20 (emerald nickel)
NiS (millerite)
NiS04 • 7H20 (nickel vitroil)
(Ni,Mn)3Si205(OH)4 (garnierite), Nepouite (nickelferrous
chlorite)
Potassium
Complex
Oxides:
Phosphates:
Halides:
Silicates:
K2(U02)2(V04)2(V04)2 ' 3H20 (carnotite)
K3P04(Mo03)n, K3P04(W03)12
K2SiF6
(alunite), KAl3(AlSi301Q)(OH)2 (muscovite)
KAlSi308 (orthoclase), K(Mg,Fe)3(AlSi301Q)(OH)2 (biotite)
-------
TABLE 4 (continued)
Seleni urn
Native:
Oxide:
Sulfides:
Se°
Se02
SeS
Silicon
Oxides:
Hal ides:
Silver
Native:
Oxides:
Complex
Oxides:
Hydroxides:
Carbonates:
6H20
Si02 (quartz), Si02 (amorphous), A^SiOg (kaolinite)
NaAlSi3Og (a! bite), 3BeO . A1203 . 6Si02 (beryl),
(ZnFe)2 • (Fe2S)Be(Si04)3 (helvite)
NaCaBeF(Si07)9 (leucophane), Na~AUSioOin ' 2H90
0 £ C
-------
TABLE 4 (continued)
Simple
Sulfides:
Complex
Sulfides:
Sul fates:
Phosphates:
Hal ides:
Sodi urn
Oxides:
Sulfates:
Hal ides:
Silicates:
Tin
Native:
Oxides:
Hydroxides:
Sulfides:
Phosphates:
Vanadium
Oxides:
Hydroxides:
Sulfides:
Ag2S
Ag3AsS3, Ag3SbS3, AgAsS2, AgSbS2
Ag2S04, Ag2S03
Ag3P04, AgP03, AgP20?
AgCl, AgBr, Agl, Ag(NH3)2Br
Na2V04, Na20 • 2CaO • 2B203 * IOH20 (kramite)
NaCaB5Og • 8H20 (ulexite), Na20 ' 2B203 • 5H20
NaHS04
Na2STF6
NaAlSi3Og (albite), Na-montmorillonite, NaCaBeF(Si03)2
(leucophane)
Na2Al2Si301Q • 2H20 (natrolite), Na20 • A1203 • 4Si02
(jadeite)
NaCa2(Mg,Fe,Al)5(Si,Al)8022(OH)2 (hornblende)
Sn°
Sn02, SnO, Sn2As2
Sn(OH)2,.Sn(OH)4
SnS, SnS2, Sn2S3,
SnHP04, Sn3(P04)2
* FeS ' SnS2 (stannine)
V2°5> V2°3> V2°2' V02'
K2(U02)2(V04)2 ' 3H20 (carnotite), (PbCl)Pb4(V04)3
(randinite)
V(OH)2, V(OH)3, VO(OH)2
V2S5
31
-------
TABLE 4 (continued)
Zi nc
Oxides: ZnO (zincite)
Hydroxides: Zn(OH)2
Carbonates: ZnCO^ (smithsonite)
Sulfides: ZnS (sphalerite)
Sulfates: ZnS04 • 7H20 (goslarite)
Silicates: ZnSi03> 2ZnO . Si02 (willemite), Zn2Si04 * nH20 (calamine)
Zn4(OH)2Si207 • H20 (hemimorphite)
* Main Ref. 6, 23, 27, 30, 31, 32, 33, 34, 35, and 36.
32
-------
TABLE 5. IMPORTANT SOLUBILITY PRODUCTS OF METALS* (IN pKsp)
OJ
CO
Hatal Oxide
Al(lll) 34
(filbbstte)
Sb(lll) 41.f1
Oe(ll) 26.flt
(UeO)
54.lt
(hydroxide Carbonate Sulflde Sulfite Siilfate Chloride Phosphate Silicate
31.7
70.5
20.0
(Amorphous)
21.1
( Y-Bfi(OII),)
21.5 • *
-0.4fit
-6.25
-1.71 -26.4
21
(A1PO.)
-------
TABLE 5 (continued)
co
Hutal Oxide Hydroxide Carbonate Sulflde Sulflte Sulfate Chloride Phosphate
Ca(ll) -4.6* 5.26 a.32 2.94 6.5. 4.6 6.25
(Calcite) (CallPO.)
fl.22 6.08 (CaSO.? 9, *
(Araqonlte) (CaSO,- ?ll nS If* ten \ \
1 c 1 T ** slip"! I ^4 at • "A 1 o I
(Dolomite) Iifl20) 1.14
(Call2 •
(PO.),)
6.4
(Cal!P04-
40.92
S6.6
:(Ca&OII
120.66
(Cajfl(P04)fi
Cr(lll) 31.0 •
Co(ll) 04.3* 14.2 (blue) 12.84 21. 3M U.7* -'-32 34.7
14.0 (pink 26.6(a) (Co(OH) (Co3
1S.7 (S?«k. (S0.)'& tf**W
*fled) A OC» 6.'7
Silicate
3.7
(CaSI03)
62.3*
(Anor-
thlte)
585.2*
(Ca-
Hontiiui-
rlllonlte)
-------
TABLE 5 (continued)
CO
en
Hetal Oxide
Mm)
Cu(ll) 20.35
fe(ll)
Mill) fiO.lt
(Fe203)
Pb(ll) 15.35t
(PbO)
•Hfl(l 1)
Hydroxide
40.5
18.59
15.3
39.3
16.09
la.a*
|Pb3(0»)2
(co3)2)
9.2
(active)
11.6
(Qruclte)
Carbonate
9.63
(CuC03)
33.16
(on)2)
10.2
13.1
4.9
(Magneslte)
S.4
(Nesquehon-^
JteJ
16.7*
JHgCJ
Sulflde Sulflte Sulfate Chloride Phosphate Silicate
35.2 37.7
J6-9 33.3 18. 9t
18.2 2S.a
2fi.fi 7.78 4.79 43.5
1 ? fi^
(PbllPO.)
4
-2.41 -2.85 -4.27 4.44f 28.4
2 3 42
Oi2o)6) 12. et
4.00t
-------
TABLE 5 (continued)
U>
en
total Oxide
Ma(ll) 0.92t
»U(!)
(Mil) 25. 7t
111(11)
MI)
(
Se
Aa(0 7.7)
Hydroxide Carbonate Sulflde Sulflte Sulfate Chloride Phosphate
12.72 9.30 12.9 " . 22
( Crystal -
Ine)
15.7
(Precipi-
tated)
23.7 16.05 45.0 6.13 17.68 12.4
26.4 52.2 13.8
(Metacl-
nnabar)
53.6
(Cinna-
bar)'
14.7 6.9 18.5 -2.91
(fresh) (x) (HISO.)
17.2 24.0 1.46
(aged) (fl)
25.7 " (HIS04-
6II..O)
t
-4.11 -11.02 -4.53 1.72 -0.93
11.1 49.2 13.02 4. B 9.75i. 15.84
Silicate
13. 2t
76. 4t
(K-Feldspar)
123. iit
(K-HIca)
-------
TABLE 5 (continued)
CJ
Ham 0*1, Id Mydroxldo Carbonate Sulflda Sulflta Sulfata Chloride Phosphite
Ha(l)
6.5 -1.55
(HJISO^)
Silicate
40.6*
(All.lte)
294
(Na-Hont-
morllloiilte)
Sn(ll) 1.76f 20. 1 26.0
V(ll) 15.4
V(lll) 34.4
MID
i
'
5.60 10.70 25.15 36.7
Amorphous) (Snhale-
6.95 rite)
Amorphous , 2 2. BO
tged) (Uurz-
S.92 fte)
21. 031
(Cryst. 22.65
aged) (Precl-
pita ted)
-------
TABLE 5 (continued)
Values in pKsp at I = 0, T = 256C; main Ref. 8, 24, 25. 33.
3*
O., • 3I!20 (S.GIbbslte) - A.1 * 3011"
•iAl2SI206(OH)4 (S.Kaollnlte) t 2M«20 - Al3* t I^S104 * 3011"
NaAlSI3Ott (S.AlbHa or Ha - Feldspar) * 7H20 * II* • Al3* + Na* * 3»4S104 - 30ir
CaAl2S12Ofl (S.Anoythlte or Cj-Feldspar) * ailgO - 2A13* t 2II4$|0. + OOH" + Ca2*
i - 3*
l'iKAlSI3Oa (S.K-Feldspar or Orthoclasa) t 12II20 • l^Al * lijK + 4«sM4S10. +'60ll"
KAI3SI3°|02 (S.K-Nlci'or Muscovite)* lflll.,0 • 3A13* * K* * 3H4S104 f 10 011"
lonlte).* 3011,0 « 7A13 + .11ILSIO. * 220H" t Ha*
3C*0.33A11.67SI7 33°2o!OII)4 (S,Ca-Hont«or111onlte) + 60II20 - HA13* + 22ILSIO. * 440H" t Ca2*
i,Sb?033(OH)2(C03)2(s) « 3Pb2* f 2011" • 2Cfl"
PbO(s) + II20 - Pb2* * 2011"
PbllPo4(s) - Pb2* t llPflJ"
HaNH4(P04)(s) - Hg2* + NIlJ * PoJ"
HgMII4(P04)(ll20)ti(s) - Hg2* + NIlJ * PO3" i 6II20
HgllP04(H20)3(s) * Hg2* + IIP04" + 3II20
HgCl2(H20)fi (S.blschoflte) - Hg2* + Cl" + 6ILO
-------
TABLE 5 (continued)
CO
U3
KMflCl3(H2OJ3 (S.CinulHU) - K* * Ma2* + Cl~ +
Hn02(s) t 2|l* - Mn2* * M>2 * »20
HnSI03(s) t H20 - Mn2* + 2011" * S102(s)
»flfl(s) * H?0 » Hfl2* +2011"
• »a2 * 2a'.E° - -0.789
Sa° + 60H" • Saol"1* ailfl i 4a", £° - 0.366
SnO(s) * 211* »
ZnStO}(s) + H20 - Z« * 2011" t
As° + 3»20 - II3AS03 + 3llf f 3«"
-------
RESULTS OF STABILITY FIELD ANALYSIS
The stability field of solids can be described as either
(1) a function of Eh and pH or (2) a function of associated ions
and corresponding activity coefficients. Results are reported
in Eh-pH diagrams or ionic ratio (in log scale) and ionic
strength diagrams. Only the stability field diagrams of alumi-
num, antimony, arsenic, cadmium, calcium, chromium, copper, iron,
lead, mercury, manganese, nickel, selenium, sulfur, and zinc
will be evaluated.
Due to the wide variety of FGD wastes, the data used here
to construct the ion-ratio diagram was chosen from both the
minimum and maximum levels of contaminants in order to cover all
possible conditions (see Table 3). Owing to the complexity of
the calculation and graphing procedures in the Eh-pH diagram,
only median levels of the constituents were used. Results of the
stability field analyses are discussed below.
Aluminum
The stability field of aluminum in the FGD wastes is shown
in Figure 1. There are three possible solid forms of aluminum (Al )
that can exist in the FGD wastes: Al 203. 3^0 (s ), AlPO^s) and
Al(H2P04J(OH)2(s L. Figure 1 shows that if the equilibrium ratio
of fQH~}3 to [PO4] of the FGD wastewater is greater than about
10"'4, the Al203-3H20(s) solid is more stable than JJie AlP04(s)
solid. However, if (OH"}3 /[PO4"] is less than 10" , the
AlP04(s) species becomes more stable than Al203 . 3H20(s ) species.
From the diagram, it can also be seen that the effect of
ionic strength on the stability field of aluminum is usually
minor. Between species Al303.3H20(s) and AlP04(s), the boundary
effects of the ionic ratio upon the ionic strength (0.05 to 0.8
for FGD systems) vary only from 1Q-"13 to 10-14-2. For
Al203 . 3H20(s) and Al(H2P04)(OH)2(s), this variation is from
10-3-50 to 10-3-64 and for Al(H2P04)(OH)2(s) and A1P04(S) it is
from TO'9-5 to 10-10 -5.
In order to illustrate the use of the ion-ratio diagram,
consider the following example: Assume a sample of FGD waste-
water has the following characteristics:
I = 0.6
pH = 8
PT = 10" ' M (total phosphate concentration)
and the dissociations constants of phosphate species at I = 0
and T - 25QC are:
K1 = 10-2.2, K2 = 10-7-°, and KS = IQ'12-0.
40
-------
cr
UJ
4
0
-4
-8
-16
-20
-24
-28
-32
-36
-40
sAl2033H2Os
(s)/
(A)
i i i i i i
I
z
o
i
-3-
O
Q_
CM
Ol
O
UJ
4
3;
2
1
0
-1
-2
-3
-4
-5
-6
0 0.2 0.4 0.6 0.8 1.0 1.2 U
-7,
(B)
;A1(H2P04)(OH)2
I i i i i i
0 0.2 0.4 0.6 0.8 1.0 1.2 1.4
T2
814
4
• •*
o
a.
CM
CM
I
3=
O
MI .4
J-
O
a.
as
o
-8
-12
-16
-20
-24
-28
A1(H2P04)(OH)2
^(01
//
V
(s)/
(C)
0 0.2 0.4 0.6 0.8 1.0 1.2 1.4
Figure 1. Stability field of Al in FGD sludge
41
-------
From equation 30, the activity of the soluble species can
be solved:
Valence y
0 1
1 0.74
2 0.3
3 0.066
Therefore:
1 .22 21 24
-7J x 10 - lO"^'1 = — ^ — 5 - (50)
0 7d 7 n fi fi ] [H
Ki = 1± x 10-7-0 = 1Q-6.6 = - 1^
0*3 V T 1*1 — I £ • U TT ••» IrUyl
. 3 X I 0 ,-.-11.3 4
n ncg =10 =
» \ •/ i- /
[HP04 ]
Assume:
PT = [H3P04] + [H2P04~] - [HP04~] + [P04~] (53)
From equations 5 to 53 and the given pH value, the free con-
centrations of the phosphate species can be determined. These
equilibrium results are:
[H2P04] = 10"6'9 M (54)
[P0?~] = 10"8'8 M (55)
Therefore :
[P043'] TO
1Q-9.2 (56)
42
-------
By using this value and also Figure 1(A), it can be found that
Al203-3H20(s) is more stable than AlP04(s). And following the
determination of the ionic ratio:
(OH"}2 = (IP"6)2 = 10-5.1, (57)
[H2PQ-] TO'6'9
it can be seen that the more stable solid falls in the stability
field of Al(H2P04)(OH)2(s) (see Figure 1(B)). It can be con-
cluded from the above that Al(H2P04)(OH)2(s) will become the most
stable solid. If there are any other phosphate solids present
in this given condition, they will gradually transform to
Al(H2P04) (OH)2(s ) . Therefore, if the soluble aluminum level is
very high in the FGD wastewater in this condition, it can be
predicted that the soluble aluminum level will gradually be
controlled by the solid Al(H2P04 ) (OH)2(s) .
Antimony
,f
The stability field for antimony (Sb) solids is given in
Figure 2. The main solid species for antimony in nature are
oxide and hydroxide-chloride species. However, under most FGO
system conditions, the only possible stable solid species of
antimony is Sb(OH ) 30!2(s ) . The stability field of this solid
is very narrow and is controlled mainly by the chloride concen-
tration (see Figure 2 ) .
Arsenic
The stability diagram for arsenic (As) is given in Figure 3.
Native element As (s) is the only solid considered in this cal-
culation. Since there are three valances involved in the trans-
formation of arsenic, the Eh-pH plot was used for the stability
field analysis. The total arsenic concentration chosen for the
calculation is 2 X 10~6M.
Results show that in the FGO system the As°(s) species can
exist under_reducing conditions. In a strong oxidizing environ-
ment, H2As04 is the most stable species in the low pH region
(<7) and HAs042- will become the most stable species in the
high pH region. In a moderate oxidizing environment,_HsAs03(aq)
will be dominant at a pH of less than about 9. H2As03 also
has a small predominant field in the high pH levels (see Figure
3).
Ca dmi urn
There are two possible solid stability fields for cadmium
(Cd) in the FGD system: Cd(OH)2(s) and CdC03(s) (see Figure 4).
43
-------
34
30-
2.8-
2.6-
2-4-
2,2
20
18
-------
en
+ 1 .0
+0.5
LU
-0.5
-1 .0
2H+ + 2e-
pH
8 10 12 14
Figure 3. Stability field of As in FGD wastes at [AsT] =2 x 10~6M.
-------
urn
en
o
s_
-Q
0 0.1 -0.2 0.3 0.4 0.5 0.6~6~.7 0.8 0.9 1.0 1.1 1.2
Figure 4. Stability field of Cd in FOG sludge.
46
-------
The boundary between these two solids under equilibrium condi-
tions lies in the range of the following ionic ratio, depending
on the ionic strengths:
{OH?} = 0.18 to 0.23 (58)
[CO*']
-2 2-
If the chemical equilibrium ionic ratio of (OH } /[CO, ] of
a FGD system exceeds this range, then the hydroxide solid,
Cd(OH)2(s), will become the predominant solid. Otherwise, the
carbonate solid, CdC03(s), will predominate.
Figure 4 shows that CdCOs(s) has a larger possible stability
field than that of Cd(OH)2(s) in an FGD system. CdC03(s) can
predominate in the 10-7.2 to 0.2 {.OH-}2/[CO^"] ratio range. The
same ratio for the stability field of Cd(OH)2(s) on^y ranges from
10-1.5 to 0.2. Due to the high levels of carbonate (from the
flue gas) in the FGD sludge liquid phase, CdC03(s) is more likely
to be present in most FGD systems. Therefore, the solubility of
cadmium in the FGD wastes is more likely controlled by the carbo-
nate concentration and the solubility product of CdCOs(s).
Calci urn
Calcium (Ca) solids which can exist in the FGD system are
hydroxide, carbonate, sulfite, sulfate, phosphate, fluoride and
silicate. However, stability field calculations show that only
carbonate, sulfite or sulfate solids of calcium predominate.
The comparison of these three solids is given in Figure 5. The
boundaries for these solids exist at the following equilibrium
ionic ratios:
[C°3 ] _ ln-3.72 (59)
2- ~
[SO ]
= 102'44 (60)
[CQ2-]
cso2"] , 28
|— = 10"' -28 (61)
[SOp
Results show that CaC03(s) has a relatively smaller stability
field than that of CaS04 . 2H£0(s) and CaSOs . 1/2H20(s) (see
Figure 5). This is due to the extremely high levels of sulfate
or sulfite ions in the FGD liquid phase. Results also show that
ionic strength is not a very significant factor in the distribu-
tion of calcium solids.
47
-------
0 0.2 0.4 0.6 0.8
0 0.2 0.4 0.6 0.8 1.0
0!
-1
-2
-3
I "4
•r- '
^ -5
•f"
•f™
lr -6
en
o
(C)
J I
Q 0.2 0.4 0.6 0.8 1.0
Figure 5. Stability field of Ca in FGD sludge.
48
-------
In most FGD systems, the speciation of calcium solids
appears to be governed by the stability constants of CaS04. 2H20(s)
and CaSOs.1/2H20(s) as well as the relative concentration of
sulfate and sulfite ions. Due to the tremendous amount of Ca
and S in the FGD wastewater, the Ca-S-H20 system also may affect
the redox conditions of the entire FGD system. Therefore, the
stability field of calcium and the relative levels of sulfate and
sulfite ions can become one of the most important factors in deter-
mining the characteristics of FGD wastes.
Chromi urn
The stability field of chromium (III) (Cr) in FGC wastes can
be examined in Figure 6. Chromium can exist as a stable hydroxide
solid (Cr(OH)3(s)) in the FGD waste system. However, at the
median concentration of soluble chromium (10-5-30^) (Table 3),
the predominant species are hydroxide complexes. As shown in
Figure 6, at low pH levels (pH 5), the.Cr(OH)2+ species is the
most predominant. More Cr3+ ions can coordinate with available
hydroxide ligands when the pH levels increase. This shift of
predominant species to Cr(OH)2 occurs in the pH range of 5 to 7,
and to Cr(OH)4 at pH values higher than 7.
Copper
Among the copper (Cu) solids (oxide, hydroxide, carbonate,
phosphate, sulfate, etc.), Cu(OH)2(s) and Cu2C03(OH)z(s) are the
most common in FGD sludge. The stability field of these two '
solids is shown in Figure 7. The boundary between these two
solids under equilibrium conditions ranges from 10-14.30 to
10-14.55 for [CO§-]1/2{OH-}.
As can be seen from the diagram, the soluble concentrations
of copper in the FGD liquors are largely regulated by both
hydroxide and carbonate concentrations. Higher hydroxide or
carbonate concentrations tend to lower the concentration of
soluble copper species. At neutral or slightly alkaline condi-
tions Cu2C03(OH)2(s) is less soluble than Cu(OH)2(s). Since
higher soluble carbonate concentrations favor the formation of
Cu2C03(OH)2(s) (see Figure 7), the soluble carbonate levels in
the FGD systems may control copper mobility.
Iron
The stability field of iron (Fe) in FGD sludge is shown in
Figure 8. At a pH of less than about 7, and under reducing and
moderately oxidizing conditions, the ferrous ion (Fe2+) will
become the predominant species. At a pH of less than 5, and
under strong oxidizing conditions, the FeS03+ species may pre-
dominate. Under all other conditions, iron will exist primarily
in the solid phase.
49
-------
en
o
-20
--15
14
Figure 6. Stability field of Cr in FGD waste. (Activity of
soluble Cr = 10"5-3°M (i = 0, T = 25°O)
-------
0 0.1 0.2 0.3"0.4 0.5 0.6 0.7 0.8 0.9 1.0 1.1 1.2
Figure 7. Stability field of Cu in FGD sludge.
51
-------
CJ1
ro
Fe(OH)2 (s) -
12
-10
--15
14
Figure 8. Stability field of Fe in FGD waste. (CT = 10~3M; [S03"]T = 10~1'66M;
PT = 10~5-64; activity of soluble Fe = 10~4-UM (l = 0, T = 25°C,
sulfide not Included))
-------
The three most common iron solids in FGD sludge are
Fe(OHJ3(s), FeC03(s), and Fe(OH)2(s). Among these three solids,
FeC03(s) and Fe(OH)2(s) can only exist in relatively small
regions of the stability field. As shown in Figure 8, Fe(OH)3(s)
is probably the most important sink for iron in the FGD sludge
system. Since Fe(OH)3(s) has a very low solubility, it is ex-
pected that soluble iron will gradually be reduced to trace
levels as the sludge ages.
Lead
Fourteen lead solids were considered for the FGD sludge
system: PbO(s), PbCOs, Pb02(s), Pb°(s), PbsfOH)2(COs)2(s),
Pb(OH)2(s), PbSOs, PbS(s), PbS04(s)f PbCl2(s), Pb3(P04)2(s) ,
PbHP04(s), PbF2(s), and PbMo04(s). Among these solids only
Pb(OH)2(s), PbC03(s), Pbs(OH)2(COs)2(s), and PbMo04(s) show a
stability field in FGD sludge. The ion-ratios (R's) for these
four solids under equilibrium conditions are as follows:
Pb(OH)2(s)-PbC03(s):
LQ.H"}2 : R = YCQ2- Ksp,Pb(OH)2 = 1Q-2.99 1Q-3.54
[COp] ———2 * •£ (62)
(YOH ) ^sp,PbC03
(see Figure 9(A))
Pb3(OH)2(C03)2(s)-PbC03(s):
(OH'}2/3 : R - YC03~ . KSP,Pb3(OH)2(C03)2
» io-5-7 . io-5-88
(see Fi gure 9(B))
Pb(OH)2(s)-Pb3(OH)2(C03)2:
{OH'}4/3 : R = (YOH")2/3 (YCO§-)2/3 ^ Ksp,Pb(OH)2
[CO|-]2/3 (YQH")2 Ksp,Pb3(OH)2(C03)2
102'71 ^ lO2'34
(see Figure 9(C))
= 102'71 ^ lO2'34 (64)
53
-------
-20
(B)
L\ v \ \ v \ V V V V. \ \ r
>b3(OH)2(C03)2(sK
z_
PttCO, (s)
0 0.2 0.4 0.6 0.8 1.0 0 0.2 0.4 0.6 0.8 1.0
m
\
CM
I
r— 1
ir
m
o
ro
o>
o
0
-3
-6j-
-9
3
•£ -12
_a
•r-
r -15
[Pb(OH)
(C)
;Pb3(OH)2(CO,),(sH
//
J I I I
0 0.2 0.4 0.6 0.8 1.0
Figure 9. Stability field of Pb in FGD sludge.
54
-------
-4
8
o
o
01
o
£ -2.
3
CT
-4
(F)
W/////
b(OH)2(s)
J I
0 0.2 0.4 0.6 0.8
PH
1.0
Figure 9 (continued)
55
-------
PbMo04(s)-PbC03(s):
n i» (ui /^ rtirt
(65)
[Mo02~]
[CO^"]
: R = YC02'
YMo02'
Ksp,PbMo04
Ksp,PbC03
10-o.io
(see Figure 9(D))
PbMo04(s)-Pb(OH)2(C)3)2(s):
[MoO2'] . R a
{OH-}2/3[C02-]2/3 - YMo02-
Ksp,PbMo04 = 1Q5.80 1Q5.25 (66)
Ksp,Pb3(OH)2(CO)3)2
(see Figure 9(E))
PbMo04(s)-Pb(OH)2(s):
= Y-2 sP.PbMoQ = 3'09 2'5
R = (YOH-) . .4 = TO' . 10
2' K
(OH'} YMo0' sp,Pb(OH)2
(see Fi gure 9 ( F) )
67)
A comparison among Pb(OH)2(s), PbC03(s), and Pbs( OH ) 2 ( COs) 2 ( s )
solids reveals that Pb(OH)2(s) has a relatively small stability
field in FGD sludge. In particular, when Pb3 ( OH ) 2 ( CDs) 2 ( s ) is
present, Pb(OH)2(s) will not exist in FGD sludge.
PbMg04(s) solid is stable at low pH levels in the FGD system
when MoO^'concentrations are high (Figures 9(D) and 9(E)). This
solid species may in fact control the soluble lead levels in low
pH FGD wastes .
Mercury
The mercury (Hg) stability field includes the eight signi-
ficant solids species and the six significant soluble species
shown below (chosen from the results of the speciation calcula-
tion) :
Solids: Hg°(M, HgCl2(s), HgO(s), HgS04(s), Hg(OH)2(s),
(s), Hg2OCl(s), and Hg4OCl(s).
56
-------
Soluble: HgClgUq), HgCl?, Hg(OH)?(aq), HgCl (OH ) (aq ) ,
HgCl42-, and Hg2 + . *
Although mercury can exist as 0, +1, and +2 oxidation states
in nature, the +1 oxidation state is quite unstable (Ref. 33) and
is therefore excluded from the calculations. The results show
that only three mercury species can predominate in FGD systems:
Hg°U), HgCl2(aq), and Hg(OH)2(aq) (Figure 10). HgCl2(aq) will
predominate when both the redox potential of the FGD system is
above +300 mv and the pH is below 9. Hg(OH)2(aq) will pre-
dominate at levels of similar high pH and redox potential (see
Figure 10). The balance of the commonly encountered Eh-pH
levels are contained in the stability field of Hg°(M. This
region provides moderately oxidizing or reducing conditions.
Since most FGD sludges are moderately oxidizing or reducing,
the majority of the mercury contained in FGD sludge will exist
as Hg°(&). This is favorable for the control of mercury con-
tamination from FGD leachates.
Manganese
It has been reported that the most common manganese (Mn)
compounds are those in the +2, +3, and +4 oxidation states
(Ref. 33). The +3 oxidation state of manganese compounds is
relatively unstable, unless stabilized by very strong complexing
agents in the aqueous environment (Ref. 6). The +6 oxidation
state of manganese can exist in a highly oxidizing and alkaline
environment (Ref. 33). The primary species of manganese used
for the stability field calculation include the oxide, hydroxide,
and carbonate solids, as well as soluble complexes of chloride,
hydroxide, sulfate and manganous ions (Mn^+). As suggested by
Mandel (Ref. 37), manganese can exist in different oxide solids,
such as MnO(s), Mn02(s)» Mn203(s), and Mn304(s). Ponnamperuma, et
al. (Ref. 38), noted that more than 150 nonstoichiometric oxides
of manganese ranging from MnOi.2(s) to Mn02(s) have been identi-
fied in nature. In view of these complicated phenomena, coupled
with the lack of reliable thermodynamic data, the construction of
a manganese stability field is a difficult task.
In this study, the solid species used follow those employed
by Stumm and Morgan (Ref. 6) and Bricker (Ref. 39): MnC03(s),
Mn(OH)2(s), Mn304(s), MnOOH(s), and Mn02(s). The significant
soluble species used in constructing the stability diagram are
taken mainly from the results of the speciation model. These
species are: Mn2 + , HMnO^, MnO^2', Mn(OH)5, MnOH+, MnS04(aq),
and MnCl+. The manganese stability diagram is presented in
Figure 11. It can be seen from the diagram that Mn2+ is the
predominant species at low pH levels (pH less than about 7).
The MnC03(s) species can exist in FGD sludge at a pH of about
7 to 11 and at a reducing to moderately oxidizing redox poten-
tial. Mn(OH)2(s) solid can exist when the pH is greater than
57
-------
en
00
1.4
1 .2
1.0
0.8
0.6
. 0.4
0.2
0
-0.2
-0.4
-0.6
-0.8
0
HgU)
pH
8
10
12
20
15
10
O)
CL
0
-5
-10
-15
14
Figure 10. Stability field of Hg in FGD waste. (Cl = 10~1'13M; activity of
soluble Hg = 10~6-70M (j = 0, T = 25°C, HgT = 10""5-78M))
-------
in
ID
1.4
1.2
1.0
0.8
0.6
: 0.4
x
1 0.2
0
-0.2
-0.4
-0.6
-0.8
H
20
15
10
0)
o.
0
-5
-10
-15
PH
8
10
12
14
Figure 11. Stability field of Mn in FGO waste. (CT = 10~3M; activity of soluble
Mn = 10~4>62M (I = 0, T = 25°C))
-------
11, which is outside normal FGD conditions. Mn304(s), MnOOH(s),
and Mn02(s) also have stability fields in the FGD sludge at
higher redox potentials (see Figure 11).
Since conditions usually change toward higher redox poten-
tial and higher pH levels as FGD sludges age, it can be specu-
lated that the predominant species of manganese will transform
as follows during the aging process:
Mn2+ -* MnC03(s) -* Mn304(s) + MnOOH(s) + M02(s)
This transformation trend indicates that the soluble manganese
concentration will be gradually reduced in the FGD leachates
with time.
Nickel
When constructing the stability field for nickel (Ni), the
major solids of concern are Ni(OH)2 (s, fresh), Ni(OH)2 (s, aged),
NiC03(s), NiS04(s), Ni$04-6H20(s), N1S(«x) ,' and NiS(y)- Only
Ni(OH)2(s, aged) and NiC03(s) have a stability field in FGD
sludge. The boundary between these two solid species exists at
the following ion-ratios (Figure 12):
, YC03" . KSP.NJ(OH)2, aged 10.30 in-10.85
rt = —._ — _ = i u i u
(YOH~r Nsp,NiC03
The Ni(QHJ2(s,aged) species will predominate when the ratio
of {OH~}2/[CQi~] is higher than the above R values. Otherwise,
the NiC03(s) species will be the most stable solid in the FGD
siudge .
Selenium
Like arsenic, only one solid species is considered for
selenium (Se): native selenium (Se°(s)). The transformation
of sel.enium also involves a valence change, so the Eh-pH plot is
used. A selenium concentration of 1.4 X 10"^ M was chosen.
The stability field of selenium is presented in Figure 13.
Results show that the predominant species of selenium in FGD
sludge are Se°(s), SeO^~, HSe03~, and SeO$ . Among these four
species, the former three are the most likely to exist in FGD
sludge. Se°(s) is the most stable selenium species in moderately
oxidizing or reducing environments. However, if conditions be-
come more oxidizing, HSeQ3~ will predominate at low pH levels
(less than about pH 6.5) and SeOy will predominate at high pH
levels. As FGD wastes age, conditions usually change toward
higher redox potentials and higher pH levels. Therefore, it
60
-------
CM
ii ro
o
2
0
-2
-4
-8
-10
-12
-14
-18
-20
-22
-24
-26
-28
-30
-32
-34
-36
J I
0 0.1 0.2 0.3 0.40.5 0.6 0.7 0.8 0.9 1.0 1.1 1.2
Figure 12. Stability field of Ni in FGD sludge.
61
-------
6
pH
10 12 14
Figure 13. Stability field of Se in FGD waste
at [SeT] = 1.4 x 1(T5M.
62
-------
would appear that selenium would exist as SeQ(s) in the raw
FGD wastes, and transform with time to SeO^' and HSeO^. There-
fore, the aging of FGD sludge will probably increase the sele-
nium levels in the associated leachate.
Sulfur
The important sulfur (S) species in FGD sludge include the
following:
Solids: CaS04.2H20(s), CaSOs . 1/2H20(s ), S°(s), and
BaS04(s).
3 - 2 +
Soluble: SO? , HS04, S03 » HS03> CaS04(aq), and FeS03 .
Among the listed species, CaS04.2H20(s ) , CaSOs. 1/2H20(s),
and S°(s) are the predominant species in FGD sludge. The
stability fields of these three species are,shown in Figure 14.
The resulting boundaries among these species are as follows:
Redox couple Equation (at I = 0,T = 25°C)
CaS04.2H20(s)-CaS03..1/2H20(s) pH + 16.95 Eh =-0.93 (69)
CaS04.2H20(s)-S°(s) pH + 12.71 Eh = 4.18 (70)
CaS03.l/2 H20(s)-S°(s) pH + 11.30 Eh = 5.89 (71)
It can be seen in Figure 14 that the CaS04.2H20(s) species
predominates in FGD sludges at any pH value if redox potential is
positive. The figure also shows that elemental sulfur (S°(s))
may exist as the major sulfur species in strong reducing environ-
ments. The sulfide species may not be significant in strong
reducing environment due to the extremely low organic contents
of the FGD sludges. CaSOs.1/2H20(s ) is thermodynamical1y un-
stable and will gradually convert to CaS04 . 2H20(s) .
Zi nc
The primary oxidation state of zinc (Zn) in the aqueous
environment is +2 (Ref. 33). Since the transformation of zinc
species occurs without electron transfer, the ion-ratio method is
used for the evaluation of the zinc stability field. Zinc solids
which are stable in FGD sludge may include hydroxide, carbonate,
silicate, and phosphate. The solids used in the stability calcu-
lation are Zn(OH)2 (s, amorphous), Zn(OH)2 (s, amorphous aged),
ZnC03(s), Zn3(P04)2(s), and ZnSi03(s). Among these solids,
Zn(OHJ2(s, amorphous aged), ZnC03(s) and ZnSi03(s) are the pos-
sible predominant solids. As shown in Figure 15, the boundary
63
-------
cr>
PH
Figure 14. Stability field of S in FGD waste. ([ST] = 10~°-001M,
[Ca2+] = 10~1'35M (I = 0, T = 25°CM
-------
a\
en
-2
-4
-6
-8
\\\\\\\\\\\\\\
Wn(OH)2 (sK\\N
\\\\\\\\\\\
1.0 1.2 1.4
Figure 15. Stability field of Zn in FGD sludge.
-------
between Zn(OH)2(s) and ZnCOats) is at the {OH~} /[C0§~] ratio
of 10-5.17 to IQ'5.72. P0r ZnSfOaLsJ and ZnCOs(s), the boundary
field is a ratio of 1Q-10-25 to IQ-10-80. Zn(OH)2(s) is rela-
tively unstable when ZnSiO-(s) is present in F6D sludge.
66
-------
SECTION 4
SOLUBLE CHEMICAL SPECIES IN FRESH
FGD WASTEWATER
The speciation of soluble constituents in FGD wastewater
can be modeled as demonstrated in Section 2. The models, which
described interactions among solid- and soluble species, are
inherently complex and subject to inaccuracy if all significant
species are not considered.
When modeling speciation in fresh FGD wastewater, however,
two simplifying assumptions can be made: (1) the equilibrium
conditions among the soluble species can easily be reached, and
(2) the rates of nucleation and dissolution of the solid species
are very low. The thermodynamic modeling of fresh FGD wastewater
can therefore be performed as if no solid species were present.
The speciation in this study was performed in such a manner.
Modeling accuracy was 'assured through the incorporation of
all significant species. Included in the model were 20 important
metals, 13 important ligands, and 155 possible complexes. These
species are listed in Table 6; the corresponding formation
constants are listed in Appendix A.
Because the composition of fresh FGD wastewater varies sub-
stantially, the speciation modeling was performed only for the
extremes of the expected range (shown in Table 3). The minimum
concentration of species in FGD wastewater at the scrubber dis-
charge point occurs at an ionic strength (I) of about 0.05. The
maximum ionic strength can-reach I = 0.80, which is higher than
the seawater condition (I = 0.67). It is expected that all other
possible distributions of species would fall within this range.
The following discussion presents the modeling results for
species concentrations in the low and high ionic strength cases,
respectively. In each case, the results were prepared in graphi-
cal form (Figures 16-37). The concentrations of each group of
complexes are plotted against pH values. With the exception of
free ions, each curve on the graph represents the summation of
the concentrations of similar ligand complexes. For example, the
"Cl~" curve in the speciation diagram of cadmium (see Figure 20),
represents [CdCl ] + [CdCl2(aq)] + [CdCl3~] + [CdCl42-] + [CdClg ]
67
-------
TABLE 6. POSSIBLE CHEMICAL SPECIES EXISTING IN FGD WASTES
Constituent
Aluminum
Beryllium
Cadmium
Calcium
Chromium
Cobalt
Chemical Species
uiicniiv*ai upci-icJ
Solid Soluble
AlP04(s), Al2(Si03)2(OH)2(s), A1S04+, AHSO^-, AlF2+, A1F2+,
AlAs04(s), Al(OH)'3(s), AlF3(aq), A1F4", A1F52-, AlFg3",
Al(H2P04)(OH)2(s), A10H2*, A1(OH)4-
Al203'3H20(s)
Be3(P04)2(s), Be(OH)2(s)
A10H2
BeS04(aq), Be(S04)22",
. Be(S04)34-,BeCl+, BeF+
CdC03(s), Cd3(As04)2(s),
CdSe03(s), Cd(OH)2(s)
BeF,
BeF3", BeOH+
BeF^(aq), BeF3", BeOH
CdC03(aq), CdHC03+, CdS04(aq),
CdCl+, CdCl2(aq), CdCl3",
CdCl42',CdOHCl{aq), CdF"1",
CdF2(aq), CdF^, CdP04",
Cd(S03)22-, CdOH+; Cd{OH)2(aq),
Cd(OH)3-, Cd(OH)42-, Cd2OH3+,
Cd4(OH)44+
t • t
CaC03(s), CaS04-2H20(s), CaC03(aq), CaHC03+, CaS04(aq),
CaF2(s), Ca(P04)3(OH)(s), CaF+, CaHP04(aq), CaOH+
Ca4(P04)3H(s), CaHP04(s),
CaSi03(s), CaS03-l/2H20(s),
CaMo04(s), Ca3(As04)2(s),
/^ »r* — f\ ( _ \ /^-/rtii\ ^_\
^^v *i 9 °"3v n;5W4 '21
CaSe03(s), Ca(OH)2(s)
CrAs04(s), Cr(OH)3(s)
CoC03(s), Co3(As04)2(s),
CoSe03(s), Co(OH)2(s)
CrS04+, CrCl2+, CrCl^, CrF2+,
CrF2+, CrF3(aq), CrHP04+,
CrOH2+, Cr(OH)2+, Cr(OH)4~
CoC03(aq), CoHC03+, CoS04(aq),
CoCl+, CoCl2(aq), CoHP04(aq),
CoOH+, Co(OH)2(aq), Co(OH)3~
68
-------
TABLE 6 (continued)
Constituent
Copper
Hydrogen
Iron
Lead
Chemical
Species
Solid
CuC03(OH)2(s), Cu3(P04)2(s),
Cu3(As04)2(s), CuSe03(s),
Cu(OH)2(s), CuC03(s)
FeP04(s), FeAs04(s), FeSe03(s)
Fe(OH)3(s), FeC03(s),
Fe(OH)2(s)
PbC03(s), Pb3(C03)2(OH)2(s),
PbF2(s), PbHP04(s),
Pb3(P04)2(s), Pb5(P04)3(OH)(s),
Pb2Si03(OH)2(s), PbMo04(s),
Pb3(As04)2(s), PbSe03(s),
Pb(OH)2(s), PbO(s), Pb02(s),
PbS03(s), PbS04(s),
PbCl2(s)
Soluble
CuC03(aq), Cu(C03)22', CuHC03+,
CuOHC03~, CuS04(aq), CuCl+,
CuCl2(aq), CuCl3", CuCl42",
CuOHCl(aa), CuF+, CuHP04(aq),
CuH2P04+, CuB(OH)4+,
Cu(B(OH)4)2(aq), CuOH+,
Cu(QH)2(aq), Cu(OH)3~,
Cu(OH)42-,Cu2(OH)22+
HC03", H2C03(aq), HS04', HF(aq),
HP042-, H2P04-, H3P04(aq),
HSi03~, H2Si03(aq), HB(OH)4(aq),
HS03~, HMo04", HAs042',
H2As04", H2V04~, HSe03",
FeS04+, Fe(S04)2-, FeCl2+,
FeCl2+, FeCl3(aq), FeF2+, F
FeF3+, FeHP04+, FeHSi032+,
FeB(OH)42+, Fe{B(OH)4)2+,
FeS03+, FeOH2+, Fe(OH)2+,
Fe(OH)4', Fe2(OH)24+
PbCo3(aq), Pb(C03)22', PbHC03+,
Pb(HC03)2(aq), PbS04(aq), PbCl+,
PbCl2(aq), PbCl3~, PbCl42~,
PbOHCl(aq), PbB(OH)4+,
Pb(B(OH)4)2(aq), PbOH+,
Pb(OH)2(aq), P8(OH)3-, Pb°(s),
Pb2(OH)3+, Pb3(OH)4+, Pb6(OH)84+
69
-------
TABLE 6 (continued)
Constituent
Chemical Species
Nickel
Potassium
Sodium
Silver
Tin
Solid
Soluble
Magnesium MgC03(s), MgF2(s), Mg3(P04)2(s), MgC03, MgHCO-j"1", MgS04(aq), MgF*.
Mg3 (As04)2(s), MgSe03(s), MgHP04(aq), MgOH+
Mg(OH)2(s)
Manganese MnC03(s), MnSi03(s),
Mn3(As04)2(s), MnSe03(s),
Mn(OH)2(s), Mn304(s)
Mercury Hg(OH)2(s),
MnOOH(aq), Mn02(aq), MnHC03+,
MnS04°, MnCl+, MnCl2°, MnCl3-,
MnHP04°, MnOH+, Mn(OH)3~
HgC03(aq)-, HgHC03+, HgS04(aq),
Hg(S04)22-, HgCl"1", HgCl2(aq),
2-
HgCl2-, HgOHCl(aq),
HgF+, HgOH+, Hg(OH)2(aq),
NiC03(s), Ni3(As04)2(s),
NiSe03(s), N1(OH)2(s)
Hg(OH)2(aq), Hg(OH)3-, Hg2OH3+;
Hg3(OH)33+
NiC03(aq), NiHCO/, NiS04(aq),
NiCl + , NiCl2(aq), NiF+,
NiHP04(aq), NiOH+
KSO/,'
', NaS04
Ag2C03(s), Ag2S04(s), AgCl(s), AgS04", AgCl(aq), AgCl2",
Ag3P04(s), Ag2Mo04(s),
Ag3As04(s), Ag2Se03(s),
AgOH(s), Ag°(s)
Sn(OH)2(s) SnFr, SnF0(aq), SnF,~. SnOHn
2- . rl 3-
Ag(S03)3~, AgOH(aq),
Ag{OH)2~
SnF+, SnF?(aq), SnFo
£. %J
70
-------
TABLE 6 (continued)
Constituent Chemical Species
Solid Soluble
Zinc ZnC03(s), Zn3(P04)2(s), ZnC03(aq), ZnHC03+, ZnS04(aq),
ZnSi03(s), Zn3(As04)2(s), ZnCl+, ZnCl2(aq), ZnCl3",
ZnSe03(s), Zn(OH)2(s) ZnOHCl(aq), ZnCl42", ZnF+,
ZnHP04(aq), ZnOH+, Zn(OH)3"'
Zn(OH)42-, Zn(OH)2(aq), Zn2OH3J
* Represents those included in the Thermodynamic Model.
71
-------
-6
11
Figure 16. Speciation of Ca in raw FGD wastewater
at I = 0.05, [CaT] = 10"1'89M.
72
-------
-1Q2
en
o
11
Figure 17.
Speciation of Mg in raw FGD wastewater
at I = 0.05, [MgT] = 10"3'91M.
73
-------
2-
Free-K"
so;
102
i.o
o.
a.
10'
10
10
-6
7
pH
11
Figure 18.
Speciation of K in raw FGu wastewater
at I = 0.05, [KT] = 10~382M.
74
-------
-102
~ 6-
7
pH
11
Figure 19. Speciation of Na in raw FGD wastewater
at I = 0.05, [NaT] = 10~3<21M.
75
-------
-10-10
-10-15
-in-20
11
Figure 20.
Speciation of Cd in raw FGD wastewater
at I = 0.05, [CdT] = 10-7.44M.
76
-------
1Q-20
11
Figure 21. Speciation of Cr in raw FGD wastewater
at I = 0.05, [CrT] = 10
-6.72
M.
77
-------
5 io
3
O
CD
O
15
20
25
/ree
B(OH)
7
PH
1.0
-O
Q.
Q.
XQ-10
10-15
1Q-20
11
Figure 22. Speciation of Cu in raw FGD wastewater
at I = 0.05, [CuT] = 10
-7.50
M.
78
-------
ID'20
11
Figure 23. Speciation of Fe in raw FGD wastewater
at I = 0.05, [FeT] = 10
-6.45
M.
79
-------
-25
11
Figure 24. Speciation of Hg in raw FGD wastewater
at I = 0.05, [HgT] = 1.0"8'7M.
80
-------
_a
a_
en
o
-4
11
Figure 25. Speciation of Pb in raw FGD wastewater
at I = 0.05, [PbT] = 10
-7.32
M.
81
-------
Ol:
o
-1 n~8
11
Figure 26. Speciation of Zn in raw FGD wastewater
at I = 0.05, [ZnT] = 10
-6.82
M.
82
-------
11
Figure 27. Speciation of Ca in raw FGD wastewater
at I = 0.8, [CaT] = 10
-1 .12
M.
83
-------
Figure 28. Speciation of Mg in raw FGD wastewater
at I = 0.8, [MgT] = 10"Q-95M.
84
-------
0
§ 2
1 — 1
1— «
a. 4
o
6
8
i i i i i
Free K+
so;
—
—
till!
3 5 7 9 11
10.6
10*
102
1.0
ID'2
10-*
pH
CL
a.
Figure 29. Speciation of K in raw FGD wastewater
at I = 0.8, [KT] = 10~3-09M.
85
-------
01
o
-6
11
Figure 30. Speciation of Na in raw FGD wastewater
at I = 0.8, [NaT] = lO-Q-^M.
86
-------
O)
o
1 12-
J3
Q.
Q.
-6
11
Figure 31.
Speciation of Cd in raw FGD wastewater
at i = 0.8, [CdT] = lQ-6-01M.
87
-------
s-
O
at
o
B 15 -
25 -
7
pH
-ID'20
11
"Figure 32.
Speciation of Cr in raw FGD wastewater
at i = 0.8, [CrT] = 10-5-02M.
88
-------
11
Figure 33.
Speciation of Cu(II) in raw wastewater
at i = 0.8, [CuT] = 10~5-5M.
89
-------
cu
u.
01
o
4 =
-10'
-10-6
11
Figure 34. Speciation of Fe in raw FGD wastewater
at I = 0.8, [FeT] = 10~3-84M.
90
-------
5 14-
en
CT
O
26-
11
Figure 35. Speciation of Hg in raw FGD wastewater
at i = 0.8, [HgT] = 10'6-47M.
91
-------
-10'
Figure 36.
Speciation of Pb in raw FGD wastewater
at I » 0.8, [PbT] = lO-5-71M.
92
-------
11
Figure 37.
Speciation of Zn in raw FGD wastewater
at I = 0.8, [ZnT] = 10"5-67M.
93
-------
From these diagrams, it can be seen that the major ions
exist mainly as free ions. However, trace metals are complexed
considerably in fresh FGD wastewater.
CONSTITUENT SPECIATION: LOW IONIC STRENGTH
In this section, the speciat ion of four major ions, Ca, Mg,
K, and Na~, and eleven minor ions, Cd, Cr, Cu, Fe, Hg, Pb, Zn,
As, B, F, and Se will be discussed. The discussion will also
cover the possible soluble complexes with the following important
ligands: Cl", OH", S042~, C032-, B(OH)4, SOs2', F~, P043',
S2032", Mo042', As043~, HV042', and 5eQ^~ - Tne major species
and their percentage of the total concentrations for the consti-
tuents studied are listed in Table 7.
Calcium
The speciation of calcium in fresh FGD wastewater at low
ionic strength (I = 0.05) is shown in Figure 16. This figure
shows that the most significant soluble calcium species in this
condition is the free calcium ion. This ion alone can account
for from 78.4 percent (at pH 11) to 83.6 percent (at pH 3) of
the total soluble calcium in fresh FGD wastewater. The second
significant species is CaS04(aq), which may account for 16.4
percent to 16.5 percent of the total calcium concentration. The
calcium-carbonate and calcium-hydroxide complexes are significant
only in the high pH region. At pH 11, for example, CaC03(aq)
and CaHC03+(aq) constitute about 2 percent of the total soluble
calcium content. At lower pH levels, the carbonate complex
concentration becomes negligible. Other less significant spec'ies
(e.g., fluoride and phosphate complexes) may also exist. Other
ligands considered (Cl~, B(OH)4, S032~), cannot form stable com-
plexes with calcium.
Magnesi urn
The speciation of magnesium in fresh FGD wastewater at
I = 0.05 is presented in Figure 17. The relative importance of
ligands in magnesium complexation is similar to that of calcium.
The majority of soluble magnesium also exists as a free ion,
ranging from 59.0 percent (at pH 11) to 80.2 percent (at pH 3).
MgS04(aq) is the second important soluble species of magnesium,
and can range from 15.7 percent (at pH 11) to 19.8 percent (at
pH 3). The relatively minor concentrations of other magnesium
complexes are shown in Figure 17.
Potassium
Thermodynamic calculations show that there are only two
significant soluble species for potassium in FGD wastewaters:
free K+, 'and KS04 (97.2 percent and 2.8 percent, respectively).
94
-------
TABLE 7. DISTRIBUTIONS OF CHEMICAL
SPECIES IN LOW-IONIC-STRENGTH FRESH
FGD WASTEWATER (AT pH 7}
Major Ions Ma
Calcium Ca
CaS04(a
2 +
Magnesium Mg
MgS04(a
Potassium K
KS04
Sodium N a
NaS04
Minor Ions
Cadmium Cd
CdS04(a
CdCl,+
'
+ CdC
Chromium CrOH
Copper Cu
Cud/
+ CuC
CuB(OH)
Iron (III) FeOH2+
FeB(OH)
Mercury HgCl+ +
+
HgOH+ +
jor Species
q)
q)
q)
+ CdC1?(aq) + CdCl "
7 - ?-
i + r H r i
+ Cr(OH)2 + Cr(OH)~
+ Cud 9(aq) + Cud ,"
2- J
14 + CuOHCl (aq)
4+ + Cu(B(OH)4)2(aq)
+ Fe(OH)2 + Fe(OH)"
T4 +
+ Fe2(OH)2
4+ + Fe(B(OH)4)2
HgCl p (aq ) + HgCl Z
\J
HcGl|" + HgOHCl (aq)
Hg(OH),(aq) + Hg(OH):
Perce
82.
17.
79.
20.
97.
2.
98.
1 .
48.
10.
40.
1 00
1 .
0.
97.
99.
0.
99.
0.
ntage
8
2
2
7
2
8
8
2
6
1
9
1
9
9
6
3
5
5
95
-------
TABLE 7 (continued)
Minor Ions
Lead
Zinc
Arsenic
Boron
Fluorine
Selenium
Major Species
Pb2*
2 j.
PbCO,(aq) + Pb(CO,)9 + PbHCO,
3 32 3
+ Pb(HC03)2(aq)
PbS04(aq)
PbCl1++ PbCl2(aq) -i- PbCl3
+ PbCl2' + PbOHCl (aq)
PbB(OH)4+ + Pb(B(OH)4)2(aq)
PbOH+ + Pb(OH)2(aq) + ?b(OH)3
7 4-
lnd +
ZnS04(aq )
ZnCl+ + ZnCl2(acl) + ZnC13
+ ZnOHCl (aq) + ZnCl2"
HAs042" + H2AsO'
B(OH)'
HB(OH)4(aq)
F"
CaF +
BeF+ + BeF2 (aq ) -f- BeF3
SnF + SnF, (aq ) + SnFZ
-------
Copper
2-
Copper can form complex species with B(OH)4, OH , Cl , C03 »
SO?, POg", and F" ligands. However, at low pH levels (pH 5),
these complexes account for only 29 to 45 percent of the total
soluble copper; free Cu2 is the predominant species here. When
the pH is greater than 5, B(OH)4 can account for 24 percent to
99.9 percent of the total soluble copper (depending on pH).
At pH 7, the relative distribution of copper in fresh FGD
wastewater was shown in Table 7. At this pH level, the Cu2+-
B(OH)4 complexes comprise about 97.7 percent of the total soluble
copper. The two borate complexes, CuB(OH)4 and Cu(B(OH)4)2 (aq )
exist at approximately equal concentrations at pH 7. When the pH
is higher than 7, Cu(B(OH)4)2(aq) will predominate (see Figure 22)
Iron
The calculated concentrations of soluble iron(III) species
are presented in Figure 23. As is the case'with chromium,
hydroxide complexes are the most important soluble species for
Fe(III). Their existence can account for 27 to almost 100 percent
of the total soluble Fe(III), depending on pH. Other species
such as free Fe3+, FeSO|, and Fe-B(OH)4 complexes (mainly
FeB(OH)2."1") may become significant at a pH below 4.
Mercury
The speciation of mercury in fresh FGD wastewater is pre-
sented in Figure 24. Results of thermodynamic calculations show
that when the pH is less than about 8.5, Hg2+-C1~ complexes
(primarily HgCl2(aq)) are the predominant soluble mercury species.
These species can account for 50 to almost 100 percent of the
total soluble mercury. When the pH exceeds 8.5, Hg-OH complexes
(primarily Hg(OH)2(aq) become the principal soluble mercury
species. Other soluble mercury species, such as Hg-C03 com-2+
plexes (including HgCOs(aq) and HgHCO^), free metal ions, Hg
Hg-S04 complexes (including HgS03(aq) and Hg(S04)2,-), and
H g F + will also exist in low concentrations.
Lead
The distribution of soluble lead species is shown in Figure
25. Soluble lead speciation shows two distinct trends: concen-
trations of free metal ions, Pb2+, Pb-S04 complexes, and Pb-Cl
complexes decrease when pH increases; concentrations of P b - 8 (0 H ) 4
complexes, Pb-OH complexes, and P b - C 0 3 complexes increase when
pH increases. The division occurs at about pH 7. As can be seen
in the diagram, free Pb2+ is the dominant lead species below pH
7. When the pH is higher than 7, borate complexes dominate;
Pb(B(OH)4)2(aq) is the most important species under this condition
The relative distribution of the primary species at pH 7 is
97
-------
listed in Table 7. Examination of this table shows almost all
the possible lead-ligand complexes to comprise at least two per-
cent of the total soluble lead. This distribution phenomenon is
quite different from the other elements studied.
Zinc
Thermo dynamic calculations showing that zinc forms predomi-
nantly hydroxide complexes (primarily Zn(OH)2(aq)) in fresh FGD
wastewaters when the pH is higher than 8.5. In this pH region,
carbonate, sulfate, chloride, fluoride, and phosphate complexes
also may be formed but in trace amounts only (see Figure 26).
When the pH is below 8.5, free zinc ion is the predominant spe-
cies and accounts for 50 to 75 percent of the total soluble zinc
(depending on the pH level). In this pH region, ZnS04(aq) and
Zn-Cl complexes can account for about 15 percent and 10 percent,
respectively, of the total soluble zinc. Other zinc Complexes
occur at insignificant levels.
Arsenic, Boron, Fluorine, and Selenium
Arsenic (As), boron (B), fluorine (F), and selenium (Se) in
FGD wastewater exist as ligands. Among these four elements,
boron (existing as borate, B(OH)4") and fluorine (existing as
fluoride, F") serve as important ligands for certain trace metals,
B(OH)4 for Cu and Pb, and F" for Sn. Arsenic and selenium exist
either alone as free ligands, or in association with hydrogen
i ons .
Although borate forms predominant complexes with certain
trace metals, the relatively low metal concentrations and high
borate concentrations will force the majority of borate ions to
exist either as free ions (B(OH)4) or as HB(OH)4(aq). The fluoride
species, however, will complex with a variety of metals under
different pH levels. The following calculated results show the
complexing trends of soluble fluoride species in low ionic
strength in fresh FGD wastewater:
Distribution
(% of available
pH Species
3 Sn
Al
F"
HF
F+
F2 +
(aq)
fluoride)
94.5
2.4
1 .7
1 .2
98
-------
Distribution
(% of available
pH Species
5 SnF +
F"
A1F2 + + A1F*
5 CaF +
BeF +
7 F"
CaF +
SnF +
BeF +
9 F"
CaF +
11 F"
CaF +
fluo
52
24
20
1
0
91
5
2
0
94
5
94
5
ride)
.2
.6
.8
.4
.7
.4
.4
.1
.8
.2
.5
.6
.2
In the low ionic strength, fresh FGD wastewater, arsenic
exists primarily as HAs042', H2As04~ and AsOs^". These three
species comprise almost 100 percent of the total soluble arsenic
The calculated distribution of these three species is as follows
Distribution
.of available
pH Species
5 H2As04"
HAsO,2"
4
2_
7 HAs04
H AsO"
arsenic)
97.7
2.3
66.9
33.1
99
-------
Distribution
(% of available
pH Species
9 HAs042"
H2AsO-
As043'
11 HAs042"
As043'
arse
99
0
0
67
32
ni c )
.0
.5
.5
.1
.9
Two_seleniurn species predominate in fresh FGD wastewater:
free SeO^, and either HSeO;j or SeO^. The relative distribution
of these species is shown below:
Distribution
(% of available
Speci es seleni urn
H2Se03(aq)
SeO?"
3
5 HSeO:
3
7 HSe03
SeO2-
H2Se03(aq)
9 Se°|"
HSe03
11 Se°3~
72
26
0
99
93
6
0
86
13
99
.4
.9
.7
.9
.3
.1
.6
.6
.3
.8
CONSTITUENT SPECIATION: HIGH IONIC STRENGTH
The relative distribution of the important soluble species
in high it>nic strength (I = 0.80), fresh FGD wastewater is given
in Table 3. In general, the relative distribution of the species
100
-------
TABLE 8. DISTRIBUTION OF CHEMICAL
SPECIES IN HIGH-IONIC-STRENGTH FRESH
FGD WASTEWATER
Major Ions Major Species
Calcium Ca
CaS04(aq)
2 +
Magnesium M g
MgS04(aq)
Potassium K
KSO"
Sodium Na
NaS04
Minor Ions
2 +
Cadmium Cd
CdS04(aq)
CdCl* + CdCl«(aq) + CdCl" +
2- ? J
CdCl 7 + CdClc
4_ 5
Cd(SO-)2-
O tm
Chromium CrOH2+ + Cr(OH)2 + Cr(OH)4
Copper CuB(OH)4 + Cu ( B ( OH )4)£ (aq )
Iron(III) ' FeOH2+ + Fe(OH)2 + Fe(OH)4
^c /nu^4+
+Fe2(OH)2
FeB(OH)2+ + Fe(B(OH)4)2
FeS03
Mercury HgCl+ + HgCl2(aq) + HgCl^
+ HgCl2" + HgOHCl (aq)
Lead Pb2+
PbC03(aq) + Pb(CO,), + PbHCot
PbS04(aq) J ^ J
PbCl+ + PbCU(aq) + PbCI"
o • »J
+ PbCl4 + PbOHCl (aq)
Percentage
70.7
29.3
65.6
34.2
89.8
10.2
95.7
4.3
5.6
2.3
33.5
58.5
99.9
99.4
83.4
9.2
7.4
100
1 .9
0.5
2.0
4.9
101
-------
TABLE 8 (continued)
Minor Ions Major Species
Lead PbB(OH)J + Pb (B (OH )4)2 (aq )
Major Ions
Arsenic HAsO2" + HgAsOj
Boron B(OH)]J
HB(OH)4(aq)
FeB(OH)2+
Fluorine F~
CaF +
MgF+
A1F2+ + A1F* + AlF,(aq) + Al F~
t >2 ^
+ A1F2" + A1F^~
3 0
BeF+ + BeF2(aq) + BeF^
SnF+ + SnF2(aq) + SnF^
Selenium SeO^
HSeOl + H9SeO,(aq)
Percentage
90
100
1
97
0
40
6
43
3
4
0
10
89
.6
.4
.8
.6
.9
.3
.5
.8
.7
.8
.3
.7
102
-------
of major ions in both high and low ionic strength cases is quite
similar. However, due to the tremendous increase in ligand con-
centrations, the relative distribution of trace metal species in
high ionic strength wastewater can differ significantly from the
low ionic., strength distribution. The important calculated results
for some selected elements are discussed below.
Major Ions
The major cations which exist in high ionic strength fresh
FGD wastewater are calcium, magnesium, potassium, and sodium.
The speciation of these four elements is displayed in Figures
27 through 30. Comparing the results of the high ionic strength
and low ionic strength calculations (i.e., comparing Figures 27-
30 with Figures 16-19), it can be found that all the soluble
species of these four elements display similar concentration vs.
pH patterns. The concentrations of calcium, magnesium, potas-
sium, and sodium in the, high ionic strength case are about 6,
920, 5,and 170 times higher, respectively, than those calculated
for the low ionic strength case. The high ionic strength ligand
concentrations are from 4 to 4,380 times higher (see Table 3).
The increase in concentration of both the metals and ligands
leads to an associated increase in the concentrations of soluble
complexes (refer to Equation 27, Section 2). Therefore, the
relative distribution of species shifts toward major ion com-
plexes and away from free ions. This phenomenon can be observed
by comparing the results shown in Table 8 to those in Table 7.
For example, in the low ionic strength case, the ratio of Ca2+
to CaS04(aq) is 82.8 to 17.2. In the high ionic strength
case, the ratio becomes 70.7 to 29.3. Although the concentra-
tions of soluble complexes is higher in high ionic strength
fresh FGD wastewater, the majority of major ion soluble species
still exist as free metal ions. This is because major ions, in
general, have relatively low formation constants for complex
species. The lack of variety of possible complex species (as
can be seen in Appendix A) also limits the complexation trend.
Minor Ions
Eleven minor ions were considered in the high ionic strength
case: cadmium, chromium, copper, iron, mercury, lead, zinc,
arsenic, boron, fluorine, and selenium. The total soluble, con-
centrations of these elements are listed in Table 3, The models
used for calculation are equations 27-30, described in Section 2.
The total soluble levels of the above mentioned elements were
found to be from 6 to 2,200 times higher than in the low ionic
103
-------
strength case. The following table summarizes the approximate
ranges of concentration differences for each element:
Concentration ratio
of e-lements (high
ionic strength to
low ionic strength) Elements
1-10 B
10-50 Cd, Cr, Pb, Zn
50-100 As, Cu
100-1,000 - Fe, Hg, F
1,000 Se
The thermodynamic calculations show that the relative dis-
tribution of soluble species for cadmium, copper, iron, lead,
zinc, and fluorine are significantly different from the low ionic
strength results (comparing Figures 20-26 with Figures 31-37, and
Table 7 with Table 8). The distribution patterns of soluble
species for chromium, mercury, arsenic, selenium, and boron, how-
ever, are similar to those of Case I results.
Figure 31 shows that the Ca-Cl complexes (primarily CdCl )
and the Cd(S03)2~ complex may become the predominant species of
cadmium in the high ionic strength case. The free metal ion, Cd2
and Cd-COs complexes (which are among the predominant species in
the low ionic strength case) are less significant in relation to
total soluble cadmium.
The speciation of chromium in the high ionic strength case
is shown in Figure 32. By comparing this diagram with Figure 21,
it can be seen that the relative distribution of soluble chromium
species is quite similar in both high and low ionic strength
cases. The predominant species of chromium at pH greater than
4 are the Cr-OH complexes. For pH lower than 4, Cr3+ is the
predominant chromium species.
In the+high ionic strength case, Cu-Cl complexes (pri-
marily CuCl ), are the predominate copper species when the waste-
water pH is lesspthan 5 (Figure 33). At corresponding pH levels,
however, free Cu + is the predominant species for low ionic
strength wastewater (Figure 22). When the pH is higher than 5,
Cu-B(OH)4 complexes are the major species for both high and
low ionic strength wastewaters.
Figure 34 indicates that the predominant species of soluble
Fe(III) can shift with increasing ionic strength from hydroxide
complexes (Figure 23) to sulfite complex (FeS03+) in the low pH
104
-------
regions (pH 6.5). This is due to both the high sulfite level in
high ionic strength FGD wastewater, and the relatively high for-
mation constant of PeSOs* species.
The -speciation pattern of mercury in the fresh high ionic
strength wastewater is quite similar to that of the low ionic
strength wastewater (see Figures 24 and 35). The only signifi-
cant difference between these two cases is that the region of
Hg-Cl predominance can be extended from pH 8 to about pH 10.
This phenomenon is due primarily to the increase in HgOHCl(aq )
concentration at high p H .
When the pH exceeds 6, the predominant species for lead in
high ionic strength wastewater is the Pb-B(OH)4 complex
(Figure 36). The same complex predominates in the low ionic
strength case at a pH higher than 7 (Figure 25). However, in the
high ionic strength acidic region, the predominant species for
soluble lead will be Pb-Cl complexes (mainly PbCl+) rather
than freePb2"1" ion.
In high ionic strength wastewater, as in the low ionic
strength case, free Zn2* is still the predominant soluble zinc
species when the pH is lower than 8. However, the second most
predominant species changes from ZnS04(aq) to Zn-Cl complexes
(primarily ZnCl+) (Figure 37). A similar situation exists at
high pH levels (pH 9), where Zn-OH complexes (primarily
Zn(OH)2(aq) are the predominant species, followed in importance
by Zn-Cl complexes (primarily (ZnOHCl(aq)). Between pH 8 and 9,
the Zn-Cl complexes may become the predominant species. There-
fore, chloride concentration will also play an important role
in the speciation of zinc in FGD wastewater.
For the speciation of arsenic, selenium, and boron, very
little change results from a variation in the ligand concentra-
tions (see Tables 7 and 8). The major factor affecting the dis-
tribution of species for these elements is the pH value of the
wastewater. For fluoride, the percent distribution of free
fluoride will be reduced due to the formation of significant
complexes with Ca2 + , Mg^*, A13+, and Sn^+. This can be seen by
comparing Tables 7 and 8.
105
-------
-------
SECTION 5
CONSTITUENT SPECIATION IN AGED FGD SLUDGE
The speciation of constituents in aged FGD wastes was also
evaluated for both low and high ionic strength conditions. It
was assumed that the equilibrium condition among all the soluble
and solid species in the aged FGD wastes had been reached. The
concentrations of constituents used for the speciation computa-
tion are compiled in Table 9. These data are derived from
Ref. 1, 5, and 36. Only the median levels of constituents
in FGD sludge were used for the computation. The models used
for calculation are discussed in Section 1. The results are dis-
cussed in the following sections.
CONSTITUENT SPECIATION: LOW IONIC STRENGTH
In the low ionic strength speciation computation, twenty
important metals and thirteen important ligands in FGD sludge were
included. The total concentrations of constituents selected for
use are the lowest levels present in FGD sludge. Calculated re-
sults can be viewed as the least deleterious situation in terms
of leachate quality. Results of the speciation calculation for
selected constituents in FGD sludge at low ionic strength
(I = 0.05) are presented in Figures 38 through 59.
Results show that in the aged FGD wastes, the total soluble
levels and species of constituents can be greatly affected by
the solid phases. It can also be seen that the distribution of
species is pH-dependent.
Calci urn
The speciation diagram of calcium (Figure 38) shows that the
most predominant soluble calcium species in the aged, low ionic
strength FGD wastewater is the free Ca2+ ion. Ca-S04 complex
is the second predominant soluble species for calcium; however,
its concentration becomes significant only at high pH levels
(pH 9).
It is evident from comparing Figures 16 and 38, that the
levels of_ soluble calcium species will increase with aged in FGD
wastes for low pH levels (pH 9). This is especially true for
the free Ca2+ ion.
106
-------
TABLE 9. TOTAL LEVELS OF CONSTITUENTS IN AGED
F6D SYSTEMS USED FOR COMPUTATION
Total Concentrations in FGD Wastes
(Aqueous and Solid Phases)
Constituent
Ca
Mg
K
Na
Fe
Mn
Cu
Cd
Zn
Mi
Hg
Pb
Co
Ag
Cr
Al
Be
Sn
Ba
CO,
I = 0.05 (M)
100.19
10-3.91
10-1-89
1Q-1.36
10-0-57
10-3.46
10-4.18
1Q-4.97
10-3.58
1Q-4.06
10-5.83
10-4.69
10-2.87 •
10-4.56
10-4-03
1Q-5.95
10-3.97
1Q-3 .06
10-2.76
10-0.20
I = 0.8 (M)
100.21
10-0.95
10-1-87
1Q-0.83
10-0.57
10-3.41
ID-*-"
10-4.97
10-3.57
10-3.95
10-5.74
1Q-4.65
10-2.86
10-4.48
10-3.99
10-4.95
10-3.91
10-3.06
10-2-76
10-0.20
S04 ID'0-45 10-0-35
107
-------
TABLE 9 (continued)
Total Concentrations in FGD Wastes
(Aqueous and Solid Phases)
Constituent
Cl
F
P04
ST03
B(OH)4
S°3
Mo04
As04
HV04
Se03
I = 0.05 (M)
1Q-1.93
ID'2'2
1Q-6.50
10-5.15
1Q-2.57
10-0.24
1Q-3.95
1Q-3.88
10-3-45
10-4.58
I = 0.8 (M)
10-0.87
10-2.17
1Q-5.36
10-3-93
10-2.21
1Q-0.21
1Q-3.80
1Q-3.87
10-3.43
10-4.27
108
-------
ITJ
O
o>
O
3 _
12
15, —
pH
- 10'
_ 1.0
-•10
-3
CL
O.
10
-6
_ 10
-8
_ 10
-11
11
Figure 38.
Speciation of soluble Ca in aged FGD wastes
at I = 0.05, original [CaT] = 10°-19M.
109
-------
100 =
»* 80-
-------
en
as
8 _
12 _
16
20 -
pH
q 10'
_ i.o
10
-4
Q.
CL
- 10
-8
10
-12
. 10
-16
11
Figure 40. Speciation of soluble Mg in aged FGD wastes
at I = 0.05, original [MgT] = 10'3-91M.
Ill
-------
100
Mg(OH)2(aq)
80
60
40
C
o
-Q
S_
I/I
•!•"•
Q
20
Free Mg (aq)
7
PH
11
Figure 41. Primary distribution of Mg in aged FGD wastes
at I = 0.05, original [MgT] = 10
-3.91
M.
112
-------
Free K
10*
1.0
^ 6
en
o
£
Q.
Q.
10
-2
10
10'
io-<
12L
7
PH
11
Figure 42. Speciation of soluble K in aged FGD wastes
at I = 0.05, original [KT] = 10~1'89M.
113
-------
100
80
60
o
c
o
•r-
4->
3
5-
1/1
•r"
O
40
20
Free K1
7
pH
11
Figure 43. Primary distribution of K in aged FGD wastes
at I = 0.05, original [KT] = 10
-1 .89
M.
114
-------
0
o
I
4 _
8 _
12 _
16
20 _
PH
Q.
Q.
-12
_ 10
-16
.11
Figure 44. Speciation of soluble Na in aged FGD wastes
at I = 0.05, original [NaT] = 10"1-36M.
115
-------
100
80
60
c
o
•£ 40
-------
01
o
16 _
20 _
- 10'
I 10
-1
.a
a.
a.
- 10
-5-
. 10
-9
- 10
-13
24 L_l
7
PH
11
Figure 46. Speciation of soluble Cd in aged FGD wastes
at I = 0.05, original [CdT] = 10"4<97M.
117
-------
100
80 -
60 -
•o
O
M-
O
40 -
Free Cd++(aq)
PH
Figure 47. Primary distribution of Cd in aged FGO wastes
at I = 0.05, original [CdT] = 10~4'97M.
118
-------
Figure 48. Speciation of soluble Cr in aged FGD wastewater
at I = 0.05, original [CrT] = 10
-4.03
M.
119
-------
100
Cr(OH)7 (aq)
7
pH
11
Figure 49. Primary distribution of Cr in aged FGD wastes
at I = 0.05, original [CrT] = 10
-4.03
M.
120
-------
CD
O
-23
10
-28
11
Figure 50.
Speciation of soluble Cu in aged ™DgWastes
I = 0.05, original [CuT] = 10" ' M.
at
121
-------
100
*« 80
3
O
o
c
o
•^*
4->
3
J3
S_
4J
01
*^-
O
60
40
20
Cu,CO^(OH)
7
pH
n
Figure 51. Primary distribution of Cu in aqed FGD wastes
at i = 0.05, original [CuT] = 10
-4.18
M.
122
-------
o
-24
Figure 52. Speciation of Fe(III) in aged FGD wastes
at I = 0.05, original [FeT] = 10
-0.57
M.
123
-------
FeSOt (aq)
10,0
7
pH
11
Figure 53. Primary distribution of Fe(III) in aged FGD wastes
at I = 0.05, original [FeT] = 10"°'57M.
124
-------
-12
-16
CL
O.
-10-20
-24
11
Figure 54. Specfation of soluble Hg(II) in aged FGD wastes
at I = 0.05, original [HgT] = 10"5<83M.
125
-------
100
7
pH
11
Figure 55. Primary distribution of Hg in FGD wastes
at I = 0.05, original [HgT] = 10"5'83M.
126
-------
Pb2+ - C0= (aq)
(aq)
100
*« 80
n
Figure 56. Speciation of soluble Pb in aged FGD wastes
at I = 0.05, original [PbT] = 10"4'69M.
127
-------
2+
PIT - COf (aq)
100
Pb* - B(OH)4 (aq)
80
60
.a
a.
c
o
.a
•i—
5-
40 D
20
PH
(a
-------
o
I
Figure 58.
Speciation of soluble Zn in aged FGD wastes
at I = 0.05, original [ZnT] = 10~3-58M.
129
-------
100
ZnSo4 (aq)
20-
n
Figure 59. Primary distribution of Zn in aged FGD wastes
at I = 0.05, original [ZnT] = 10
-3.58
M.
130
-------
As shown in Figure 39, the major calcium solids at low pH
levels are CaS04.2H20(s) and CaSOs.1/2H20(s). These two solids
have relatively higfi solubilities compared to that of CaC03(s).
Therefore, the increase in total soluble calcium levels at low
pH is apparently caused by the lack of low solubility calcium
solids. At a high pH, the calcium concentrations in the aged
FGD wastes are substantially reduced (Figure 33). This is
caused by a reduction in the free calcium ion through the forma-
tion of CaCO^s) (Figure 39). Since the aging of FGD wastes
usually results in a higher pH, it is therefore expected that
the soluble calcium levels will gradually decrease as FGD wastes
are aging.
Magnesi urn
Figures 40 and 41 show the speciation results of magnesium
in the aged FGD wastes. It can be seen that the free magnesium
ion is the most predominant soluble species at a pH below 10.
The magnesium-sulfate complex will become significant when the
pH is between 8 and 10. The levels of free magnesium ion and
magnesium-sulfate complexes will decrease at a pH higher than
about 10, while the Mg(OH)2(s) solid will begin to form and
reduce the soluble magnesium concentration by two orders of
magnitude from its original level.
Comparing fresh and aged FGD wastes at 1=0.05, it appears
that the concentrations of soluble magnesium species are altered
by the aging effect. More free magnesium ion forms in aged
wastes than in fresh wastes when the pH is less than 8. At a pH
between 8 and 10, an increase in the magnesium-sulfate complex
concentration occurs (see both Figures 40 and 41). The distribu-
tion diagram (Figure 41) shows that the increase is associated
with the loss of free Mg^ + ion.
Potassi urn
Figures 42 and 43 show that the free K ion is the predomi-
nant species of soluble potassium in the aged low ionic strength
FGD wastes. This species comprises almost 100 percent of the
soluble potassium when the pH is below 7. At higher pH (pH 7),
small amounts of K2S04(aq) can be formed (about 10 percent, as can
be seen from Figure 43. No new potassium solid will be formed
during the aging of the FGD wastes due to the slow nucleation of
the complex potassium solids and the high solubility of the
simple potassium solids.
Sodium
In general, the distribution of soluble sodium in aged FGD
wastes at. 1=0.05 is quite similar to that of potassium. If the
sodium sp'eciation in aged (Figures 44 and 45) and fresh (Figure
19) FGD sludge are compared, the distribution of N
131
-------
appears to increase as the wastes age. As with potassium, how-
ever, no new sodium solid can be formed during aging due to the
slow nucleation of the complex sodium solids and the high solu-
bility of the simple sodium solids.
Cadmiurn
The thermodynamic model shows that at low pH levels (pH<-6),
the+majority of the cadmium species exists as soluble free
Cd2 and CdCl+ (Figure 46 and 47). As the pH increases, cadmium
is removed from solution through the precipitation of CdC03(s).
Due to the formation of this solid, cadmium levels in aged FGD
wastewater can be reduced to as low as 1 ppb (see Figure 46).
As the pH rises above 10.7, the soluble cadmium concentration
increases, again owing to the formation of the more soluble
Cd(OH)2(s).
Comparing the fresh and aged FGD wastes, the predominance
of soluble Cd-S04 complex appears to decrea.se with age at low.pH
levels. The relative predominance of this complex in the soluble
phase increases when CdC03(s) is formed at high pH, which also
reduces the concentrations of both the free Cd2+ and Cd-Cl
complexes. In fresh FGD wastes (see Figure 20) the cadmium-
carbonate complexes will become the predominant soluble species
at a pH of 9 to 11; in the aged FGD wastes, the levels of cad-
mium-carbonate complexes in the same pH range are lower than those
of the free cadmium ion, cadmium-chloride, and cadmium-sulfate
complexes .
Chromium
The calculated results for the speciation of chromium are
given in Figures 48 and 49. By comparing Figure 48 to the specia-
tion results of chromium in fresh FGD wastes (Figure 21), it is
found that the predominant soluble species of chromium (free
Cr3+ for pH less than about 4, and Cr-OH complexes for pH
greater than 4) are similar in both cases. However, the concen-
tration of soluble chromium in aged wastes decreases (see Figure
48) when conditions favor Cr(OH)3(s) formation (see Figure 49).
The Cr(OH)3(s) can account for as much as 80 percent of the total
chromium in the aged FGD sludge. Neutral pH levels favor the
formation of this solid (pH of 5.5 to 9 appears to be the optimum
range).
Copper
Thermodynamic calculations indicate that at 1=0,05, the
predominant soluble species of copper in aged FGD wastes are free
copper ion at pH less than 4.8, and copper-borate complexes
mainly CujB (OH )at)z ( aci) » at higher pH . Copper-chloride, copper-
hydroxide, or copper-carbonate complexes are the next most
132
-------
important soluble species under pH levels as shown in Figure 50.
Almost 100 percent of the total available copperexists as
Cu2C03(QH)2(s) precipitate, however (see Figure 51). Due to the
formation of this solid, the soluble copper concentration can be
reduced to extremely low levels. Therefore, the aging of FGD
wastes should control copper migration into the aqueous environ-
ment.
Iron
The speciation of Fe(III) is shown in Figures 52 and 53.
Under the studied condition, it was found that most of the iron
in FGD sludge will precipitate out as Fe(OH)j(s) (see Figure 53).
Soluble iron (as FeS03+) may exist in a significant concentration
at low pH levels (pH 5). Although Fe-OH complexes are the
predominant soluble species when the pH is greater than 5, their
concentrations are typically less than 1 ppb. Since the aging
process increases both the pH and Eh va-lues, the removal of iron
from the FGD wastewaters is favored.
Mercury
The speciation of mercury in the aged FGD wastes is repre-
sented in Figures 54 and 55. Note that when the pH is less than
about 8.5, the predominant soluble species are Hg-Cl complexes
(primarily HgCl2(*q)). At higher pH, Hg-OH complexes (primarily
Hg(OH)2(aq) will predominate in the soluble phase. However, due
to the formation of Hg°(£) in aged FGD sludge, most of the mercury
in the sludge will precipitate out of the FGD wastewater. This
mechanism can regulate the total soluble mercury down to trace
levels (less than 10-4 ppb, as can be seen in Figure 54). There-
fore, the aging process will also remove mercury from the FGD
1eachates .
Lead
Under the aged, low ionic strength condition, lead can form
very strong complexes with the B(OH)4 ion in the pH range of
6.8 to 8.4. Between pH 8.4 and 11, Pb-C03 complexes are the
principal soluble species (see Figure 56).
The thermodynamic model also shows that under conditions of
low pH, PbMoO^s) can be formed. This solid will account for
about 90 percent of the total lead in the sludge (Figure 57).
Through the formation of PbMoO/^s), the soluble lead concentra-
tion can be reduced to about 10 ppb (Figure 56). At a high pH,
PbC03(s) is more stable than PbMoO^s). The soluble lead concen-
tration can therefore be reduced even further The soluble lead
concentration in this pH region from pH 7 to 11 is between 10 ppb
and 0.1 pj>b. Aging would appear to favor the removal of lead
from soluti on .
133
-------
Z i n c
Free zinc ion is the major species in-aged FGD waste at pH
levels of less than 8.3 (Figures 58 and 59). When pH is above
8.0, most, of the zinc precipitates as hydroxide and silicate
solids. When the pH is higher than 9.3, the hydroxide solid is
still the predominant species, but major soluble species are con-
verted to zinc-hydroxide complexes.
In the low pH region (pH 8), due to the lack of stable zinc
soTids in the aged FGD sludge, the soluble zinc levels may in-
crease in relation to those of the fresh FGD sludge (see Figure
26). Therefore, if the pH level of aged FGD' sludge is less than
about 8, the aging process will tend to release zinc into solu-
ti on .
CONSTITUENT SPECIATIQN: HIGH IONIC STRENGTH
Speciation of constituents in the aged FGD wastes of high
ionic strength (1=0.8) was also evaluated for 20 metals and 13
ligands (155 complexes and 71 possible solids in all). Results
of thermodynamic calculations are given in Figures 60 to 81.
Calcium
The distribution pattern and the final total soluble concen-
trations of calcium in aged FGD waste at 1=0.8, is quite similar
to that at 1=0.05 (see Figures 38, 39, 60, and 61). The principal
difference between these two cases is that the high ionic strengh
FGD sludge will possess more calcium solids (compare Figures 39
and 61) .
In comparing the speciat ion calculation results for fresh
and aged FGD wastes (Figures 60 and 27), the total soluble
calcium in aged FGD wastes appears to be higher than that in
fresh FGD wastes when the pH is below 8. When the pH is higher
than 8, the situation is reversed. Therefore, the aging process
can cause the release of calcium into solution if the pH remains
below about 8; when the pH is higher than 8, the soluble calcium
will gradually be removed from solution.
Magnes i urn
In general, the distribution of magnesium species at 1=0.8
is similar to the distribution at 1=0.05 (see Figures 40, 41, 62
and 63). Some differences can still be found. For example, in
the high ionic strength case, the hydroxide solid (Mg(OH)2(s))
can be formed from high pH levels down to about pH 8. The same
solid for the low ionic strength (1=0.05) case can only be formed
above pH JO. The relative percentage of Mg-S04 complex is
smaller i~h the high ionic strength case. The existence of
134
-------
11
Figure 60. Speciation of soluble Ca in aged FGD wastes
at I = 0.8, original [CaT] = 10°'21M.
135
-------
100
80 _
60
o
H-
O
-M
ZJ
•*->
LO
40 .,
20 r
11
pH
Figure 61. Primary distribution of Ca in aged FGD wastes
at I = 0.8, original [CaT] = 10
0.21
M.
136
-------
o>
o
Q.
a.
-2
-4
-icr6
11
Figure 62. Speciation of soluble Mg in aged FGD wastes
at I = 0.8, original [MgT] = 10"°-95M.
137
-------
100
en
O
C
o
I/J
•r"
Q
20-
Figure 63.
Primary distribution of Mg in aged FGD wastes
at I = 0.8, original [MgT] = 10"°-95M.
138
-------
2 =
en
o
8 _
10
12
Free K
pH
10
10'
1.0
10
-2
o.
0.
10
-4
10
-6
11
Figure 64. Speciation of soluble K in aged FGD wastes
at I = 0.8, original [KT] = 10"1'87M.
139
-------
100
80
60
40
o
o
s_
-u
en
20
Free K
11
pH
Figure 65.
Primary distribution of K in aged FGD wastes
at I = 0.8, original [KT] = 10~1-87M.
140
-------
18
S
o.
Q.
-12
Figure 66. Speciation of soluble Na in aged FGD wastes
at I = 0.8, original [NaT] = 10
"°'83
M.
141
-------
100,
80 _
60
C
O
40
20
(aq)
Free Na (aq)
11
pH
Figure 67. Primary distribution of Na in aged FGD wastes
at I = 0.8, original [NaT] = 10"°-83M.
142
-------
•o
o
Ol
o
11
Figure 68. Speciation of soluble Cd in aged FGO wastes
at I = 0.8, original [CdT] = 10
~4'97
M.
143
-------
100
80
60
o
o
4->
-Q
I 40
t/>
Q
20
Free Cd++(aq)
CdCl+ (aq)
CdC03 (s)
7
pH
-=*-Cd(OH),(s)
n
Figure 69. Primary distribution of Cd in aged FGD wastes
at I = 0.8, original [CdT] = 10
~4<97
M.
144
-------
i.
o
o>
o
18
_ 10'
-12
11
PH'
Figure 70. Speciation of soluble Cr in aged FGD wastes
at I = 0.8, original [CrT] = 10
-3.99
M.
145
-------
CrCl++ (aq)
100
80
60 _
o
o
3
-Q
S_
-u
40 _
20 _
Cr(OH}2 + Cr(OH)4 (aq)
0.
Q.
11
PH
Figure 71. Primary distribution of Cr in aged FGD wastes
at I = 0.8, original [CrT] = 10
-3.99
M.
146
-------
3
O
Ol
O
5 _
10 __
15
20 _
25
30
7
pH
,-3
,-8
- 10
-13
-Q
Q-
O.
- 10
-18
_ 10
-23
- 10
-28
11
Figure 72. Speciation of soluble Cu in aged FGD wastes
at I = 0.8, original [CuT] = 10~4<16M.
147
-------
100
80
60
•Cu-.CO.(OH).
. C, O i
40
c
o
3
.Q
V)
a
PH
11
Figure 73. Primary distribution of Cu in aged FGD wastes
at I = 0.8, original [CuT] = 10~4-16M.
148
-------
6 -
12 -
zr is -
.
-------
FeSO* (aq)
100
80
60
tu
u.
c
o
S_
•M
40
20 25
11
PH
Figure 75. Primary distribution of Fe(III) in FGD wastes
at I = 0.8, original [Fe(III)T] - 10"°-57M.
150
-------
12
O)
O
16
20
' 28
32 _
36
PH
-24
11
Figure 76. Speciation of soluble Hg(II) in aged FGD wastes
at I = 0.8, original [HgT] = 10"5'74M.
151
-------
100
80
60
4-
o
s_
4->
cn
O
11
PH
Figure 77. Primary distribution of Hg in FGD wastes
at I « 0.8, original [HgT] = 10
152
-5.74
M.
-------
cn
o
11
Figure 78. Speciation of soluble Pb in aged FGD wastes
at I = 0.8, original [PbT] = 10
-4.65
M.
153
-------
PbB(OH)! + Pb(B(OH)j: (aq)
100
11
Figure 79. Primary distribution of Pb in aged FGD wastes
at I = 0.8, original [PbT] = 10
-4.65
M.
154
-------
11
Figure 80. Speclation of soluble Zn in aged FGD wastes
at I = 0.8, original [ZnT] = 10
-3.57
M.
155
-------
Zn(OH)° (aq)
100
ZnCl+ (aq) >
Figure 81. Primary distribution of Zn in aged FGD wastes
at I = 0.8, original [ZnT] = 10
-3.57
M.
156
-------
hydroxide complexes (mainly Mg(OH)2(aq) also become insignifi-
cant in the high ionic strength case.
Due to the formation of hydroxide solids at high pH levels
(pH 9), the available soluble magnesium decreases as the wastes
are aging. The concentration of soluble magnesium decreases A
only slightly with age at pH 9, but decreases by a factor of 10
at pH 11 (see Fi gure 62) .
Potassi urn
The distribution of potassium in aged FGD wastes at 1=0.8 is
also similar to that at 1=0.05. But due to the tremendous
increase of the soluble sulfate concentration, the concentration
of K-S04 complex is relatively higher in the high ionic strength
case. This can be seen by comparing Figures 42 and 43 with
Figures 64 and 65.
As mentioned previously, no significant simple potassium
solid can be formed in the sludge, so the migration of potassium
between solid and liquid phases is negligible. Potassium does
exist as complex solids in nature (see Table 4), but with ex-
tremely low nucleation and dissolution rates. Therefore, the
complex solids of potassium will not play an important role for
regulating the soluble potassium levels.
Sodi urn
The calculated speciation of sodium in aged FGD wastes at
1=0.8, is shown in Figures 66 and 67. The pattern of sodium
speciation is similar between low and high ionic strength wastes
(compare Figures 44 and 45 to Figures 66 and 67). The only dif-
ference between these two conditions is the concentration level.
Like potassium, there is no significant simple sodium solid
that can regulate the soluble sodium levels in the FGD sludge.
Due to kinetic constraints, the complex sodium solid will not
play an important role in the transformation of sodium species.
Therefore, the sodium concentration in both solid and solution
phases of FGD systems will remain at a constant • 1 eve! .
Cadmi urn
The relative concentrations and percentage distributions of
cadmium species in the aged FGD wastes at 1=0.8, are shown in
Figures 68 and 69. In the high ionic strength case, the cadmium-
chloride complexes (mainly CdCl2(acl) will become the dominant
soluble species. Free cadmium ion is the second dominant soluble
species; this species is the most common species in the low ionic
strength case (1=0.05) .
157
-------
The results also show that cadmium solids are readily formed
in aged FGO waste at a pH greater than 7. Two cadmium solids
have a stability field in this FGD waste condition: CdCOsCs)
and Cd(OH)2(s). The former solid is predominant in the pH range
from 7 to TO.8. Above pH 10.8, the hydroxide solid can account
for more than 40 percent of the total solid cadmium.
Comparing Figures 31 and 68, soluble cadmium concentrations
appear to be lower in the aged wastes than in the fresh wastes
in the pH range of 7.8 to 10.2 This pH range is in the stability
field of CdC03(s) .
Chromi urn
The results of the chromium speciation calculation are
shown in Figures 70 and 71. Since" the amount of soluble chromium
is only slightly different between low and high ionic strength
cases (Table 9), the speciation patterns of chromium are very
similar in both cases (see also Figures 48 and 49.)
In comparing the fresh FGD sludge (Figure 32) to the aged
sludge (Figures 70 and 71), it appears that chromium is removed
from solution during the aging process.
Copper
The thermodynamic model shows that under the conditions
studied, the predominant species of copper are the copper-chlo-
ride complexes (mainly C u C1 2 (a q )) at pH less than 4.8, and the
copper-borate complexes (mainly Cu(B(OH)4)2(aq)) when the pH is
between 4.8 and 11 (see Figures 72 and 73).
Results also show that copper is readily removed from solu-
tion when Cu2C03(OH)2(s) is formed under aging conditions. This
will decrease the soluble copper concentration to trace levels
when FGD wastes are aging.
Iron
There is little difference in the total iron concentration
in FGD sludge between high and low ionic strength conditions.
Therefore, the distribution pattern of iron is similar in both
cases (Figures 52 and 53 versus Figures 74 and 75). Since the
high ionic strength sludge has higher ligand concentrations,
however, the percentage of FeSOs"1" in the FGD sludge appears to
be higher in the high ionic strength case.
Mercury
Since in both high and low ionic strength cases the mercury
concentration is controlled by Hg°(O, the distribution patterns
are very similar (Figures 54 and 55 versus Figures 76 and 77).
Almost 100 percent of the mercury exists in the solid phase.
158
-------
As described previously, the Hg-Cl complexes dominate the
soluble levels in the low pH region (less than about 9). Due
to the high chloride concentration in the high ionic strength
case, the soluble mercury is higher in the high ionic strengh
FGD sludge than in the low ionic strength FGD sludge.
Lead
Comparing the aged FGD wastes of low (1=0.05) and high
(1=0.8) ionic strengths, the most important soluble lead species
at low pH (pH 6.8) will change from free lead ion, Pb2+, to the
lead-chloride complexes, Pb-Cl, when ionic strength increases.
At high pH, the predominant lead species are the lead-borate com-
plexes, Pb-B(OH)4, in the high ionic strength case. Results
also show that in the high ionic strength case, 60 to 90 percent
of the lead can be precipitated as1 PbMo04(s) in the low pH region.
At high pH (
-------
SECTION 6
THERMODYNAMIC MODEL VERIFICATION
In order to verify the suitability and accuracy of the ther-
modynamic model used in this study, two complementary verifica-
tion procedures were employed:
• Comparison of modeling results with analytical data
• Evaluation of the model itself in relation to certain
scientific considerations.
The comparison of model results with analytical data is
limited by the current state of analytical procedures. In recent
years, considerable advances in chemical .speciation have been
made (Ref. 40-45). No sound analytical scheme exists, however,
that can accurately define all chemical species which exist in a
given natural system. The difficulty is due both to typical
system complexity and to the low concentrations of metal species
in nature. Therefore, verification of the model using analytical
data was limited to (1) comparing total liquid phase concentra-
tions with the total concentrations predicted by the model; and
(2) comparison of the solid transformation data to the predicted
distribution of stable solids.
Evaluation of the model according to certain scientific con-
siderations provides a general check on model behavior. If a
certain variation of input parameters is performed, its pertur-
bation of the model system can be checked for reasonableness
against expected trends or results. For example, consider the
case in which the model predicts that, for element X, one percen-
of the total liquid phase concentration of X exists as the chem-
ical species Mmln. This cannot be verified by total chemical
analysis. However, by increasing the concentration of ligand L
to abnormally high levels, the predicted change in MmLn concen-
tration can be compared to scientific fact.
160
-------
COMPARISON OF MODELING RESULTS WITH ANALYTICAL DATA
As mentioned previously, evaluation of the model using
analytical data can be approached in two ways:
• Comparison of the total soluble concentrations of con-
stituents in stabilized leachates to the total soluble
concentrations of constituents, as predicted by the model
• Comparison of the solid transformation data to the
distribution of stable solids as predicted by the model.
Due to the lack of solid transformation data in the published
literature, only the first method of comparison will be discussed
A comparison of the total soluble constituent concentrations
with the results of thermodynamic calculation requires analytical
data for aged F6D wastes. Unfortunately, almost all available
data is for relatively fresh FGD wastes, such as scrubber liquor,
discharged slurries, or sludge lagoon supernatant. Data for
aged sludge (such as interstitial water from the bottom of the
sludge lagoons) is still lacking. Because of this, chemical
analysis of raw and aged FGD samples was performed.
The La Cygne Power Station (Kansas City Power and Light) was
chosen as a location from which necessary samples could best be
obtained. The La Cygne FGD system has been on line for several
years without a flue gas bypass, and the limestone and coal used
by the plant are mined on the site. The FGD chemistry was there-
fore expected to approach "steady state" conditions with respect
to sludge composition. Four types of FGD siudge/wastewater
samples were obtained for analysis:
• Fresh FGD wastewater samples from the scrubber
• Fresh FGD sludge solids samples from the FGD scrubber
• Aged FGD wastewater samples from the far end (away from
the discharge point), of the second-stage sludge lagoon
• Aged FGD sludge samples from the far end (the oldest
deposition of lime sludge) of the second-stage sludge
lagoon, 180 to 270 cm below the surface of the disposed
siudge sol ids .
The sludge samples were further divided into pore water samples
and solid sludge samples. The details of sample collection,
shipment, preparation, and analytical methods are presented in
Appendix B. The results of the analysis of these samples are
presented in Table 10.
161
-------
TABLE 10. ANALYTICAL RESULTS OF FGD SAMPLES FROM
KCP&L LA CYGNE POWER STATION
Constituent
Al
Sb
As
Be
Cd
Ca
Cr
Co
Cu
Fe
Pb
Mg
Mn
Hg
Mo
Ni
K
Se
Na
V
Zn
Alk. (as CaC03)
F~
S032"
so42-
Eh (mv)
P04-P
NO^-N
FW
0.48
0.086
0.66
0.005
0.045
850
0.001
0.049
Nil
1.0
Nil
170
2.52
Nil
3.0
0.40
83
0.250
73
0.19
0.71
198
707
13.6
19
675
27
0.2
4.8
SW
0.43
0.034
0.24
0.002
0.045
663
0.002
0.038
Nil
0.55
Nil
88
2.10
Nil
2.1
0.38
46
0.235
55
0.26
1.31
44
605
9.6
17
1650
130
0.1
1.4
Type of
FSP
0.30
0.066
0.20
0.003
0.010
810
0.001
0.022
Nil
0.1
Nil
174
0.55
Nil
4.7
0.23
74
0.475
73
0.16
0.06
188
760
9.4
50
925
77
0.1
2.3
Sampl e
SSP
0.20
0.038
0.12
0.001
0.010
410
0.002
0.010
Nil
0.04
Nil
7.0
0.15
Nil
5.8
0.02
82
0.425
75
0.21
0.06
60
708
5.5
93
625
94
0.06
1.5
FSS
833
13.9
32.6
0.69
51.4
3.45xl05
42.7
12.9
57
15,220
382
1,810
306
0.28
207
69.0
5,340
53.4
1,180
42.2
591
—
1,120
185
sss
856
8.24
26.7
0.34
56.7
3.18X105
26.6
11.7
54
18,990
340
2,330
303
0.23
203
70.2
4,940
48.3
1,310
35.6
534
—
1,093
154
162
-------
TABLE 10 (continued)
Type of Sample
Constituent FW SW FSP
Si 68 30 30
B 38.4 20 33
TOC Nil Nil Nil
TDS 3,700 3,980 3,920 4,
pH 6.54 7.14 7.65
CaS04-2H20(g/kg) -
CaS03'l/2H20
(g/kg)
CaC03(g/kg)
SSP
6.5
18.4
Nil
160
9.30
—
—
FSS ' SSS
— _ __
85 61
—
—
—
452 384
295 73.4
371 515
* FW = Fresh wastewater.
SW = Stabilized wastewater.
FSP = Pore water from 20 days aged fresh
SSP = Pore water from stabilized sludge
FSS = Fresh sludge solid.
sludge.
(about 5
years old).
SSS = Stabilized sludge solid (about 5 years old).
Units: Unless specified; for water sample
sample, the unit is mg/kg.
, the uni
t i s mg/1 ; for sol i d
163
-------
The analytical results of the total amount of constituents
in the La Cygne Plant raw FGD wastes (see Table 11) were entered
into the computer model. The total soluble concentrations of
constituents in the FGD wastes in aged condition were then pre-
dicted by-the model at different pH levels, and compared to the
field data. The results are shown in Figures 82 through 98.
In these figures, the analytical results are represented by
the numbers 0, 1, 2, and 3. Symbol 0 represents the input data
(total levels of constituents in the fresh FGD waste). Symbol 1
represents the analytical results for the soluble constituents
in the fresh wastewater (0-day data). Symbol 2 represents the
analytical results for the soluble constituents in the "rela-
tively" fresh sludge pore water (fresh sludge was aged in the
laboratory for 20 days before the pore water was analyzed). The
analytical results for the soluble constituents in the fully
aged sludge are represented by Symbol 3. According to the La
Cygne Plant engineers, the aged sludge had been in the sludge
lagoon for about five (5) years. Therefore, it was assumed that
the aged pore water data represents potential (stabilized)
leachate conditions in the FGD sludge lagoon.
The evaluation of model results in relation to the analytical
data can be performed using the migration trends of the consti-
tuents represented by Symbols 1, 2, and 3. If the soluble con-
centrations indicated by the three data points approach the
concentrations predicted by the model, then the model can be
deemed an accurate prediction of aging phenomena. The results
of the evaluation for the 18 selected elements are summarized in
Table 12.
It was found that the analytical results for aluminum,
arsenic, cadmium, boron, cobalt, copper, iron, manganese, mercury,
potassium, selenium, sodium, and zinc are all either very close
to or approach the concentration levels predicted by the model.
Therefore, it can be concluded that the model serves as a valid
predictor for the final (stabilized) concentration or migration
trends of the various species of the above-mentioned elements in
the FGD wastes. For some other elements (calcium, chromium,
fluoride, lead, and magnesium), prediction techniques were not
as successful. For calcium, the total soluble concentrations
predicted by the model are much lower than the analytical results.
The low levels predicted by the model are due primarily to the
formation of calcite, as well as the high levels of free carbon-
ate and sulfate (CO?,- and SOi", respectively) in regions of high
pH. For chromium, the high levels of hydroxide complexes cal-
culated by the model lead to the high soluble levels of chromium
in the aqueous phase. For lead, the formation of Pb-COs complexes
predicted by the model is the primary reason for the discrepancy.
For fluoride, the solid phases assumed for the calculation are
apparently not suitable. It was also found by this evaluation
that the solid phases assumed for magnesium are too soluble.
164
-------
TABLE 11. TOTAL CONCENTRATIONS OF CONSTITUENTS IN
LA CYGNE FGD SYSTEM
Constituent
Ca
Mg
K
Na
Fe
Mn
Cu
Cd
Zn
Ni
Hg
Pb
Co
Cr
Al
Be
co32-
so42~
CT
F"
P043~
sio32-
B(OH)4
so32-
Mo042~
As043-
HV042-
Se032-
Total Concentrations in
FGD Wastes (Fresh Wastewater
and Fresh Sludge) (M)
10-0.387
10-1.53
10-2.67
10-2.50
10-1.09
10-2.77
10-3.57
10-3.86
10-2.57
10-3.44
10-6.38
10-3.26
10-4.17
1Q-3.61
10-2.03
10-4.63
1Q0.048
1Q-0.096
10-1.70
1Q-1.73
10-2-75
10-2.61
10-2.23
10-0-16
10-3.04
10-3.85
10-3.59
10-3.68
Ionic Strength 0.1
165
-------
200
160
Q.
Q.
120
HI
_J
in
D
_J
a
ul
80
0 (252 ppm)
;Model
7X10
6 X 10
-4
-4
5 X 10
4 X
-4
3 X 10
2 X 10
1 X 10
-3
-3
-3
1 (0.48 ppm) V 2 (0.30 ppm) 3 (0.20 ppm)
I /Si— — ^^ 1 — ^^^— ^. _ ^^__^ __ ]___ /gy ____ _j
3
10
Figure 82.
Total soluble Al(III) concentration in La Cygne FGD
wastes (see text for explanation).
166
-------
200
160 -
120 -
.a
a.
Q.
Lu
_J
CD
a
0 (lO.S.ppm)
(200 ppb)
2.7 X 10
-6
2,13 XTQ"6
l.o X 1 0
-6
1.1 X 10"
5.3 X 10
-7
pH
Figure 83.
Total soluble As concentration in La Cygne FGD
wastes (see text for explanation).
167
-------
Q.
Q.
CD
LU
_!
03
75
60
45
30
15
0 (63.6 ppm)
1 (38.4 ppm)
2 (33
Model
6.9 X 10
-3
5.6 X 10
4,2 X 10
-3
2.8 X 10
-3
(18.4 ppm)
-1.4 X 10
-3
10
pH
Figure 84.
Total soluble B(III) concentration in La Cygne FGD
wastes (see text for explanation).
168
-------
Q.
Q.
UJ
_i
CD
_!
a
en
H-
O
2 (10 PPBX
1 (45 PPB)
5 -
-2.2X10
-4
- 1.78X 10
-4
- 1.37 X 10
-4
- 8.9 X 10"5
- 4.4X10
-5
Figure 85.
Total soluble Cd(II) concentration in La Cygne FGD
wastes (see text for explanation).
169
-------
-5 x 10-3
1 (850 ppm) 2 (810 ppm) 3. (410 ppm)
-0.5 x 10~3
1Q
Figure 86.
Total soluble Ca concentration in La Cygne FGD
wastes (see text for expl anat-i on).
170
-------
S
CL
Q.
CJ
UJ
_1
03
3
_J
O
if)
Q
I-
18
12
0 (12.8 ppm)
2 (0.001 ppm)
1 (0.001 ppm
3 (0.002 ppm)
2.9 X 10
-4
2.3 X 10
-4
1.7 X 10
-4
1.15 X 10
-4
5.8 X 10"5
8
10
pH
Figure 87.
Total soluble Cr(III) concentration in La Cygne FGD
wastes (see text for explanation).
171
-------
5 -
4 c
S
Q.
Q.
3 -
o
C_3
UJ
_l
CO
3
-1
a
en
H
a
i-
2 -
2 (0.022 ppm) -
- 1 X 10
-4
- 7 X 10
-5
1 X 10
-5
3 (0.01 ppm)
^•^^^^•mJ
9 10
Figure 88.
Total soluble Co(II) concentration in La Cygne FGD
wastes (see text for explanation).
172
-------
150 -
120
Q.
Q.
90
60
m
_i
CD
3
-1
a
30
0 (354 ppm)
-7.9 X 10
-3
2 (9.4 ppm)
6.3 X 10
-3
4.7 X 10
-3
3.15 X 10
-3
1-..53 X 10
-3
1 (13.6 ppm)
3 (5.5 ppm)
10
pH
Figure 89.
Total soluble F(I) concentration in La Cygne FGD
wastes (see text for explanation).
173
-------
1860
0 (4540 ppm)
1550 -
1240
CD
a.
a.
1 (1 ppm)
930
0>
u_
UJ
a
en
O
I-
620
310 -
3.3 X 10
-5
2.77 X 10
-5
2.22 X 10
-5
T.,66 X 10
-5
Y.ll X 10
-5
5.55 X 10
-6
3 (0.04 ppm)
10
Figure 90.
Total soluble Fe(III) concentration in La Cygne FGD
wastes (see text for explanation).
174
-------
2400
2000 -
1600
1200
O.
HI
J
-------
1,000
800
CL
Q.
600
400
111
_i
CD
a
en
f-
a
200
0 (708 ppm)
Model
1 (170 ppm) 2 (174 ppm)
pH
4.1 X 10
-2
3.2 X 10
2.9 X 10
-2
-2
2,05 X 10
-2
1.2 X 10
-2
4.1 X 10"3
(7 ppm)
10
Fiqure 92.
Total soluble Mg(II) concentration in La Cygne FGD
wastes (see text for explanation).
176
-------
100
80
CL
Q.
IU
_!
CD
3
_J
a
i-
a
i-
60
40
20
0 (.93.4 ppm)
2 (0.55 ppm)
1 (2.52 p-pm)
iModel
3
PH
1 .8 X 10"3
1.45 X 10
-3
1.1 X 10
-3
7.3 X 10
-4
3.6 X 10
-4
3 (0.15 ppm)
10
Figure 93.
Total soluble Mn(II) concentration in La Cygne FGD
wastes (see text for explanation).
177
-------
10
-4
10
-6
10
-14
CL
a.
10
-8
10
-16
-------
100
1 (83 ppm)
Model
3 (823pm)
ao
_ Model
2 (74 ppm)
0
Q.
Q.
60
LU
_J
CD
-I
O
H-
O
20
2 X 10
-3
1 X 10
-3
1 X 10
-4
10
PH
Figure 95.
Total soluble K(I) concentration in La Cygne FGD
wastes (see text for explanation).
179
-------
-27
Figure 96.
Total soluble Se concentrations in La Cygne FGD
wastes (see text for explanation).
180
-------
100 -
30
1 (73 ppm) 2 (73 ppm) 3 (75 PP"0
Q.
O.
60
IT3
111
_J
IB
O
I-
a
40
20
4 X 10
-3
3 X 10
-3
2 X 10
-3
1 x 10
-3
10
PH
Figure 97. Total soluble Na(I) concentration in La Cygne FGD
wastes (see text for explanation).
181
-------
0 (176 ppm)
pH
- 3.05 X 10
2 (0.06 ppm)
3 (0.06 ppm)
-3
2.45 X 1 0
,-3
1.33 X 10"
.^2 X 10
-3
6.1 X 10
-4
10
Figure 98.
Total soluble Zn(II) concentration in La Cygne FGD
wastes (see text for explanation).
182
-------
TABLE 12. COMPARISONS OF THE ANALYTICAL RESULTS OF FGD
WASTEWATER TO THE RESULTS PREDICTED BY COMPUTER MODEL
Constituent
Al
As
Cd
B
Ca
Cr
Co
Cu
F
Fe
Pb
Mg
Mn
Hg
K
Se
Na
Zn
(1)
(Fresh Leachate,
pH = 6.5)
0.48
0.66
0.045
38.4
850
0.001
0.049
Nil
13.6
1.0
Nil
170
2.52
Nil
83
0.25
73
0.71
Constituent
(ppm - unless
(2)
(20-Day -Aged
Leachate,
pH = 7.7)
0.30
0.20
0.010
33.0
810
0.001
0.022
Nil
9.4
0.1
Nil
174
0.55
Nil
74
0.48
73
0.06
Concentration
otherwise noted)
(3)
(5-Year-Aged
Leachate,
pH = 9.3)
0.20
0.12
0.010
18.4
410
0.002
0.010
Nil
5.5
0.04
Nil
7
0.15
Nil
82
0.43
75
0.06
Model
(Equilibrium
Condition,
pH = 9.3)
0.14
0.0002
0.011
17.5
20
12.8
0.003
4.4xlO"13t
79
0.012
1.9
645
0.156
5xlO-9t
83
3.22#
73
0.073
* Refer to Figures 82 through 95.
t ppb.
# pH = 9.15, Se = 0.43 ppm.
pH = 9.3, Se = 3.22 ppm.
183
-------
Many solid phases (such as dolomite, magnesite, nesquehonite,
and other sulfate and phosphate species) have been tried for the
calculation of the soluble magnesium in the FGD system, but none
gave results consistent with the experimental data. Additional
study is necessary to improve prediction accuracy for these
elements .
EVALUATION OF MODEL IN RELATION TO SCIENTIFIC CONSIDERATIONS
The evaluation of the thermodynamic model in relation to
scientific considerations was performed during the phase and
speciation calculations (Sections 2-5), as well as during the
calculation of the effects of chemical changes on the chemical
species (see Section 7). In general, the model results follow
the expected behavior patterns. The following are some examples
which were used to test the acceptability of the model.
Effects of pH and Eh on the System
The pH of a chemical system can influence the direction of
the alternation process (precipitation, dissolution, redox reac-
tion, and sorption), and will affect the speciation of almost all
the constituents in the system. Theoretically, low pH conditions
tend to dissolve more solids of oxide, hydroxide, carbonate,
silicate, sulfate, and thus increase the concentrations of free
soluble metal ions. High pH levels tend to precipitate more
solids, decrease the free metal ions, and enhance the formation
of metal-hydroxide complexes in the system. High pH levels can
also increase the concentrations of metal-1igands, if such
ligands have a tendency to complex more in the high pH region
(e.g., C0|", SO?', POJ-, etc.).
The results of thermodynamic calculations show that the
constituents of the above-mentioned solids have higher free
metal concentrations in the low pH region, and form more solids
in the high pH region (refer to Figures 60-81). The predicted
levels of metallic hydroxide, and of carbonate, sulfate,
and phosphate complexes, also represent tremendous increases in
the high pH region (if the decrease of the free metal ions is
taken i nto account) .
The Eh (redox potential) of a chemical system will affect
the valence and chemical forms of many constituents in the system.
Owing to the redox change, the solubility of some solids, as well
as the transformation of solids, wiTl be affected. An increase
in Eh usually results in a transfer of reduced solids to either
higher oxidation state solids (e.g., CaSOa-1/2H20(s) transforms to
CaC04-2H20(s); MnC03(s) transforms to MnOOH(s), or to other Mn
oxides), or more elemental solids will be dissolved (e.g., As°(s),
Hg°(M, and Se°(s)). These transformations can affect the solu-
bility of affected solids.
184
-------
The results derived from the model usually follow the trends
mentioned above. For example, as the La Cygne FGD wastes age,
the redox potential increases (Table 10). This change should
result in a significant increase in soluble mercury and selenium
levels in the system (Figures 94 and 96), which agrees with the
model results .
Effects of Ligand Concentrations on the Levels of Metallic Com-
p 1 ex e s
It is known that ligand concentration can affect the soluble
level of metallic complexes. Based on previous related studies
(Ref. 6-8, 23-25, 27), it is known that the chloride ligand is
important to the solubility of cadmium, copper, lead, and zinc.
In accounting for soluble copper and lead levels, the borate
ligand may also become significant'. The hydroxide ligand is
important to the dissolution of three-valence metals (e.g.,
Fe and Cr). The results calculated by the model (see Sections
4 and 5) do follow these general trends. A more detailed discus-
sion of the effects of ligands on the soluble levels of metals
is presented in Section 7.
185
-------
SECTION 7
EFFECTS OF OPERATIONAL (CHEMICAL)
CHANGES ON FGD SLUDGE CHEMICAL SPECIES
The principal goals of FGD sludge disposal are to minimize
the concentration of toxic constituents in the liquid phase
(leachate), and/or to allow such impurities to exist only in a
chemical form which is nontoxic and/or readily adsorbed by soils.
In order to assess the potential of contaminant species modifi-
cation to achieve these goals, the model was operated over a
wide range of conditions to determine the impact of various
operating changes on the various chemical species. In this
study, the effects of 11 operational (chemical) changes were
studied. The results are discussed in the following pages.
EFFECTS OF pH ON SPECIATION
As was discussed previously, change in pH level in any
chemical system can influence the direction of the alteration
process and the speciat ion of almost all the constituents in
both solution and solid phases. In this study, the effects of
pH on the speciation of constituents in the FGD sludges have
been quantitatively estimated in Eh-pH and ion-ratio diagrams
(Figures 1 through 15) and in the primary distribution diagrams
(Figures 39 through 81). The effects of pH on the speciation
of constituents in the FGD wastewaters (leachates) can be viewed
in the resultant speciation diagrams (Figures 16 through 37 and
38 through 80). The effects of pH on soluble constituents can
also be seen in Figures 82 through 98.
Effects on Solid Species
The results of thermodynamic calculations show that the pH
level can have a significant effect on the stability field of
FGD sludge constituents. Figures 3, 10, and 13 indicate that
the decrease of pH values favor the formation of elemental As°(s),
Hg°U), and Se°(s). However, for constituents which can form
hydroxide or carbonate solids such as iron (Figure 8) and man-
ganese (Figure 11), an increase in pH levels instead favors
solids formation .
186
-------
The ion-ratio diagrams shown in Section 3 also indicate the
significance of pH on the stability field of other consti-
tuents in the FGD sludges. In general, high pH levels favor the
formation of oxide or hydroxide solids instead of carbonate,
phosphate or other solids in FGD sludge. For example, higher pH
levels favor the formation of Al203 • 3H20(s), Cd(OH)2(s),
Cu(OH)2(s), Pb(OH)2(s), Ni(OH)2 and Zn(OH)2(s) over
Al(H2P04)(OH)2(s), CdC03(s), Cu2C03(OH)2(s}, PbC03(s), NiC03(s)
and ZnC03(s), respectively (see Figures 1, 4, 7, 9, 12, and 15).
The effects of pH on relative distribution of primary
solids for some selected constituents in the FGD sludges also
can be seen in Figures 39 to 81. These results show that the
most significant effect of pH on calcium solids is in the forma-
tion of CaC03(s) in high pH sludges. This phenomenon indicates
that, theoretically, the soluble calcium concentration in FGD
sludge liquid phase decreases at high pH due to the formation of
CaC03(s). For magnesium, modeling results indicate that high pH
levels favor the formation of Mg(OH)2(s). The pH effect on the
relative distribution of the two most important cadmium solids
(CdCOaU) and Cd(OH)2(s) can be seen in Figures 47 and 69. It
was found that Cd(OH)2(s) may become the predominant solid in
FGD sludges only in the very high pH region (pH >10.8). In
actual practice, few FGD systems will have such a high pH. For
chromium, the data show that Cr(OH)3(s) is the important species
only in the neutral pH region, that is, pH 6 to 9 (Figures 49 and
71 .
The effects of pH on copper, iron, and mercury is not as
obvious due to the tremendous amount of Cu2C03(OH)2(s ) ,
Fe(OH)3(s), and Hg (£) in the system (Figures 51, 53, 55, 73,
75, and 77). The most significant effect of pH on the solid
distribution of lead is that at a pH below 9, PbMo04(s) will
become the predominant species. However, high pH levels (pH 9)
favor the formation of PbC03(s). For zinc, the pH level can also
affect the relative distribution of ZnC03(s), Zn(OH)2(s), and
ZnSi03(s) in the FGD sludges. High pH levels favor the formation
of Zn(OH)2(s). When pH decreases, ZnSi03(s) will gradually re-
place Zn(OH)2(s) (Figures 59 and 81).
Effects on Soluble Species
The effects of pH on the soluble species were discussed pre-
viously in Sections 4 and 5. In general, most species of major
ions will be significantly affected by a pH change. Unaffected
species include free Ca2+, Mg2 , K+, and Na+, and their sulfate
complexes.
Typical examples of the pH effects on the total soluble
constituent levels were discussed in Section 6. In general, a
high pH will reduce the number and concentration of soluble
187
-------
species. However, due to the complexation effect in the high
pH region, the total soluble levels for some species may increase
again. Examples are the total soluble levels of chromium (Figure
87), fluoride (Figure 89), lead (Figure 91), mercury (Figure 94),
and selenium (Figure 96).
EFFECTS OF IONIC STRENGTH ON SPECIATION
The ionic strength will affect the solubility constants on
various reactions in the chemical systems. Through this effect,
the concentrations and relative distributions of species may be
altered. However, the calculated results show that the effects
of ionic strength on FGD systems are relatively small compared
to effects such as pH changes or ligands concentration changes.
The quantitative effects of ionic strength on the stability
field of constituents have been discussed using ion-ratio dia-
grams in Section 3. The influence on the stability field of
solid phase by ionic strength is usually less than a order of
magnitude from I = 0 to I = 1.0 (see Figures 1, 2, 4, 5, 7, 9,
12, and 15). In FGD systems (I = 0.05 to 0.8), the maximum
ionic strength variation will expand or reduce the stability
field of solids by a factor of no more than four.
The effect of ionic strength variation on the speciation
of soluble constituents is also small. Among the constituents
studied, only the relative distribution of cadmium between its
free metal ion, Cd2+, and its chloro complexes, Cd-Cl, can be
altered by a change in ionic strength (Figure 100). Other solu-
ble species, such as sulfate complexes (a typical example is
given in Figure 99), may also be affected by as much as one order
of magnitude. However, these effects will not significantly
change the relative distribution of various soluble species.
EFFECTS OF CHLORIDE CONCENTRATION ON THE SOLUBILITIES OF METALS
The speciation calculations show that chloride complexes
may be the predominant soluble species for cadmium, copper, lead,
mercury, and zinc. For example, when the chloride concentration
is higher than 400 ppm (Figure 101), the Cd-Cl complexes may
become the predominant species for cadmium. In general, if the
chloride concentration is known, the total soluble levels of
chloride-complexing metals can usually be predicted if no other
ligands dominate the system.
The results of related calculations are shown in Figures 101
through 105. In this study, the assumed chloride concentrations
ranged from 50 to 6,000 ppm. Other parameters used for calcula-
tion were based on analysis of the La Cygne FGD wastewater.
188
-------
10*
Free Ca++
so;
10'
CO:
1.0
a.
a.
ea
o
o
6-
OH-'
10"
poi
io-*
10
10
-6
12
I I I I 1 1 \ I
0.050.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8
Ionic Strength (I)
Figure 99.
Effects of ionic strength on the speciation of
soluble Ca.
189
-------
S 9
en
o
12
15
18
CV
Free Cd"
SOI
co:
I I
10:
1.0
a.
a.
1Q
-6
10
-9
io-12
.05 0.1 0.2 0,3 0,4 0-5 0.6 0.7 0:8
Ionic Strength (I)
Figure 100.
Effects of ionic strength on the speciation of
soluble Cd(II) .
190
-------
cr>
O
= 6,000 ppm
1" = 4,000 ppm
•C1~ = 400 ppm
1" = 3,000 ppm
Cl" = 2,000 ppm
CL
Q.
-6
31Q-8
Figure 101.
Effects of chloride concentration on soluble Cd
concentration.
191
-------
3
O
12
1.6
20
24
•Cl~ = 1,000 ppm
-CT = 2,000 ppm
= 3,000 ppm
CT = 4,000 ppm
CT, - 5,000 ppm
CT » 6,000 ppm
10'
1.0
10'
£
Q.
10
-a
10
-12
10
-16
Figure 102.
Effects of chloride concentration on soluble Cu
concentration.
192
-------
.a
a.
en
o
2-
10
12
-Cl" = 6,000 ppm.
r-Cl" = 5,000 ppm
CT = 4,000 ppm
-Cl" = 3,000 ppm
CT = 2,000 ppm
*-^
10'
1.0
Q.
a.
10
-2
10-'
10
-6
11
io-8
pH
Figure 103.
Effects of chloride concentration on soluble Pb
concentration.
193
-------
15
17
19
en
en
o
21
23
25
27
I—Cl" = 6,000 ppm
-C1~ = 5,000 ppm
7
pH
10
-8
10
-10
10
-O
Q.
-12 <=•
10
-14
10
-16
10
-18
11
Figure 104.
Effects of chloride concentration on soluble Ho
concentration.
194
-------
cn
o
8
10
12
Cl" = 3,000 ppm
Cl" = 6,000 ppm
—Cl" = 5,000 ppm
-Cl" = 4,000 ppm
Cl" = 2,000 ppm
1" = 1,000 ppm
10'
1.0 I.
Q.
10'
10~a
10-12
11
Figure 105.
Effects of chloride concentration on soluble Zn
concentration.
195
-------
Effect on Cadmium
It was found that a variation of chloride concentrations
from 50 to 6,000 ppm can lead to about a two order of magnitude
concentration change for cadmium in FGD wastewaters for any
given pH . As shown in Figures 46 and 68, in any FGD sludge free
Cd^ + is the only species which can exist at a higher concentration
than that of the Cd-Cl complexes when the pH is less than 8.7.
When the pH exceeds 8.7, species such as cadmi um-sul fa te , sulfite,
or hydroxide complexes may exist in higher concentrations than
that of Cd-Cl complexes depending on the ligand concentrations
and pH 1 eve! s .
Therefore, in order to predict cadmium species concentra-
tions in the aged FGD wastewater, the following equations are
used :
pH <8.7
[CdT] = [Cd2+] + [Cd-Cl complexes] - (73)
pH > 8. 7
[Cdy] = [Cd-Cl complexes] + [Cd-S04 complex]
+ [Cd-S03 complex] + [Cd-OH complexes] (74)
Generic equations 73 and 74 can be approximated by the following
two equations:
pH <8.7
[CdT] *> [Cd2+] + [CdCl+]
, [Cd2+] + 102-2[Cd2+] [Cl~] (75)
pH >8.7
[Cd?] = [Cd2+] + [CdCl+] + [CdOHCl(aq)] + [CdS04(aq)]
+ [Cd(S03)2~] + [CdOH+]
* [Cd2+] + 102<2[Cd2+] [Cl~] + 107>3[Cd2 + ] [OH'] [Cl"]
+ 102'3[Cd2+] [S024~] + 105'4[Cd2 + ] [SO2"]
+ 104[Cd2 + ] [OH"] (76)
The value of free cadmium ion concentration, [Cd +], can be
solved usjng Equation 31 (Section 2) with the aid of the ion-
ratio or Eh-pH methods to identify the predominant solid species.
196
-------
If the Cd-Cl complexes are the most important (predominant)
species for soluble cadmium, then Figure 101 can be employed
for quick estimation of the total soluble cadmium concentration
i n aged FGD siudge .
Effect on Copper
Figure 80 indicates that the studied range of chloride con-
centrations can cause a one order of magnitude variation in
concentrations of Cu-Cl complexes, As shown in Figures 50
and 72, free Cu2 + ion is the only species whose concentration
can exceed the concentration of the Cu-Cl complexes at low pH
(pH 4.7). From Figure 102, it can also be seen that this phe-
nomenon occurs when the chloride concentration reaches about
2,000 ppm in the FGD wastewater. At a pH higher than about 4.7,
the Cu-B(OH)4 complexes will usually dominate Cu-Cl complex
'formati on .
The same type of equations used previously for the predic-
tion of the total soluble cadmium concentration also can be used
for copper:
pH < 4.7
[CuT] = [Cu2 + ] + [CuCl+] + [CuOHCl(aq)]
~ [Cu2+] + 101 -6[Cu2*] [Cl~] + 109'1 [Cu2 + ] [OH"] [Cl~] (77)
pH > 4.7
[CuT] * [CuB(OH)J] + [Cu(B(OH)4)2(aq)]
1 , 1
(78)
From the above discussion, it appears that Figure 102 is a valid
predictor of the total soluble copper concentration in aged FGO
wastewater when (1) pH is less than 4.7, and (2) the chloride
concentration is sufficiently high.
Effect on Lead
The speciation diagrams (Figures 56 and 78 in Section 5)
indicate that the Pb-Cl complexes may become the predominant
soluble lead species at pH 7 only when chloride is present at a
high concentration. (Figure 103 shows this level to be a minimum
of 1,500 ppm.) When the pH is higher than 7, the Pb-Cl com-
plexes are insignificant. Therefore, the same types of predic-
tion equations are applicable:
pH < 7
[Pbf] * [Pb2+] + [PbCl+]
= [Pb2 + ] + lO1'7^2*] [CT] (79)
197
-------
The model verification indicates that at high pH levels the
calculated value for total soluble lead may be higher than the
analytical value. Therefore, it is recommended that the thermo-
dynamic model not be used for lead when the pH is higher than
about 7.
Effect on Mercury
When the pH is less than about 9, the Hg-Cl complexes
alone can account for all soluble mercury. The effect of the
soluble chloride level on the soluble mercury level is shown in
Figure 104. When the chloride concentration is increased from
50 to 6,000 ppm, the overall soluble mercury concentration will
vary by more than four orders of magnitude in the FGD wastewater.
Figure 104, which can be used to e.stimate the total soluble
mercury concentration in FGD wastewater when pH is less than
about 9, suggests that this estimation is usually unnecessary due
to the low concentration.
Effect on Zi nc
The effect of soluble chloride on soluble zinc levels is
presented graphically in Figure 105. When chloride concentration
is increased from 50 to 6,000 ppm, the concentration of soluble
zinc increases about two orders of magnitude. The results of
the speciat ion calculation (Figures 58 and 80) show that Zn-Cl
complexes may become the predominant soluble zinc species (1)
when pH 9, and (2) when the soluble chloride concentration is
higher than about 3,000 ppm. Conversely, when the pH is less
than about 9 and if soluble chloride concentration is below
3,000 ppm, the free metal ion, Zn2+, can account for all soluble
zinc. However, if soluble chloride concentration is higher
than 3,000 ppm in the same pH region, the total soluble zinc in
the aged FGD sludge will depend on the chloride levels. There-
fore, Figure 105 can be used to predict soluble zinc levels with-
in the above mentioned pH range.
The following equation can be used for the estimation of
total soluble zinc in the aged FGD wastewater at low pH:
pH < 9
[ZnT] ~ [Zn2 + ] + 101-4[Zn2 + ] [CT] (80)
EFFECTS OF SULFATE CONCENTRATION ON THE SOLUBILITIES OF METALS
The speciation study thus far has shown that sulfate com-
plexes may become significant at high pH levels for major ions
(Ca^"1", Mg^ + , K+, and Na + ) and several minor ions such as zinc.
Only the effects of sulfate concentration on major ions will be
198
-------
discussed here, however, due to the less important role of sul-
fate in the speciation of minor ions. Figures 106 to 109 show
the overall sulfate effect.
In this study, the soluble sulfate concentration was varied
from 100 up to 40,000 ppm. This variation will result in an in-
crease of four orders of magnitude in the concentration of solu-
ble calcium-sulfate complexes (Figure 106). Since free Ca^+'
ion and CaSQ^Uq) are the main soluble species for calcium in
FGD wastewater, the total soluble level of calcium can thus be
approximated as:
[CaT3 * [Ca2+] + 1O2 ' 3 [Ca2+] [SO2'] (81)
Figure 106 indicates that the sulfate concentration will not
play an important role in the chemical behavior of calcium in the
FGD wastewater when the pH is less than about 5. When the pH is
higher than 5, the Ca-S04 complex, (CaS04(aq), may become
the predominant soluble calcium species in FGD wastewater if
S04<-5,000 ppm.. As discussed in Section 6, 'the actual distribu-
tion of calcium solids in aged FGD wastewater cannot be accu-
rately estimated by the model. Therefore, it is suggested that
Equation 81 receive additional study.
Effect on Magnesium
Figure 107 shows that soluble magnesium levels, (MgS04(aq)),
can vary by almost six orders of magnitude for an increase in
soluble sulfate levels from 100 to 40,000 ppm. When the soluble
sulfate concentration is raised to as high as 3,000 to 5,000 ppm
(depending on the pH 1 evel ), the level of MgSO^aq) may exceed
the level of free Mg2+. The following equation best describes
the predicted magnesium levels:
[MgT] * [Mg2 + ] + 1O2 '4 [Mg2 + ] [S0°] (82)
In this case, [Mg2+] should be calculated from the solubility
controlling solids of magnesium. As was the case with calcium,
the actual solid phases of magensium in aged FGD wastes cannot
accurately be estimated. Figure 107 is therefore not suggested
for the prediction of soluble magnesium levels. It is expected
that Equation 82, however, will still be valid for FGD wastewater.
Effects on Potassium and Sodium
The effects of soluble sulfate on the soluble level of
potassium and sodium are shown in Figures 108 and 109. Although
soluble sulfate levels can affect the formation of potassium or
sodium sulfate complexes, the significance of+these complex
species i.s far below that of the free ions (K and Na + ). Even
when the soluble sulfate level is as high as 40,000 ppm (FGD
sludge usually has soluble sulfate less than 10,000 ppm), the
199
-------
-in*
o
I
40,000 ppm
= 20,000 ppm
= 10,000 ppm
s.
Q.
a.
-6
11
Figure 106.
Effects of total sulfate concentration on soluble
Ca concentration.
200
-------
Free
en
o
10
12
SOJ = 20,000 ppm
2 + SOJ = 40,000 ppm
,, w, www ppm
50= = 10,000 ppm
SO;; = 100 ppm
7
PH
10'
Q.
Q-
10'
1.0
10
-2
10"
11
Figure 107.
Effects of total sulfate concentration on soluble
Mg concentration.
201
-------
- in*
= 40,000 ppm
-S0= = 20,000 ppm
SO? = 10,000 ppm
S07 = 5,000 ppm
= 100 ppm
0.
a.
-6
11
Figure 108.
Effects of total sulfate concentration on soluble
K concentration.
202
-------
SOl = 1,500 ppm
01
o
a
10
12
504 = 5,000 ppm
SOf = 10,000 ppm
S0= = 20,000 ppm
SOT = 100 ppm
10*
10'
1.0
£ .
Q.
O.
10
-2
10-'
10
-6
11
pH
Figure 109.
Effects of total sulfate concentration on soluble
Ma concentration.
203
-------
free Ion concentrations of potassium and sodium still predomi-
nate.
EFFECTS OF BORATE CONCENTRATION ON THE SOLUBILITIES OF METALS
The speciation study has shown that total soluble copper
and lead concentrations can be greatly affected by borate con-
centration of FGD wastewater. These effects are summarized in
Figures 110 and 111.
As discussed previously (refer to Equation 78), the
Cu-B(OH)4 complex may account for almost 100 percent of the
total soluble copper in the FGD wastewater when the pH is
higher than about 4.7. In this study, the soluble borate levels
were varied from 5 ppm to 200 ppm to observe the effects on
copper. Figure 110 shows that a borate concentration increase
of this magnitude results in a 2,000-fold increase in the
copper-borate concentration.
For lead, an increase from 5 ppm to 200 ppm in borate
concentration may produce a 10,000-fold increase in soluble
Pb-B(OH)4 (see Figure 111).
Although it is still impossible to verify the presence of
various soluble lead species in the FGD wastewater, it can be
shown on a theoretical basis that Pb-B(OH)4 complexes can
account for a major portion of the total soluble lead concen-
tration. The Pb-C03 and Pb-OH complexes are the only species
which may compete with Pb-B(OH)4 levels when the pH is higher
than about 7. If the theoretical evaluation is correct, the
soluble lead level can be approximated by the following equation
for pH higher than 7 (when pH 7, Equation 79 is followed):
pH > 7
[PbT] * 105'2[Pb2+] [B(OH)'] + 1011 -1 [Pb2 + ] [B(OH)^]3
+ 107<4[Pb2+] [CO'] + 1010<8[Pb2+][CO^]2
+ 105-3[Pb2+][OH~] + 1010>9[Pb2+] [OH~]2 (83)
EFFECTS OF LIME ADDITION TO FGD SLUDGE AND WASTEWATER
The addition of lime and fly ash to FGD sludge has been
employed as a fixative process, primarily to enhance physical
properties (permeability, load-bearing strength) through a
pozzolanic reaction. However, if lime addition achieves no
reductionof the total soluble levels or any toxic complexes of
the constituents, or if soluble trace metals constituents
204
-------
3
O
CT
O
7
PH
Q.
Q.
11
Figure 110.
Effects of borate concentration on soluble Cu
concentration.
205
-------
£ 9
12
15
18
B(OH); 40 ppm
B(OH)~ 80 ppm
B(OH)4 . 120 ppm-
pH
10
1.0
10
-3
a.
a.
1Q
-6
10
-9
io-12
11
Figure 111.
Effects of borate concentration on soluole Pb
concentration.
206
-------
increase in concentration, there will be little environmental
advantage of disposing the sludge with lime addition. Therefore,
it would be useful to determine how various kinds of lime addi-
tions affect the concentrations of constituents in the sludge
liquid phase. Specifically, if lime addition does have benefi-
cial effects, it may be possible to determine how to achieve the
optimum lime dosage in order to obtain the minimum concentra-
tions of constituents in the liquid phase.
In this study, the Kansas City Power and Light La Cygne
Plant FGD waste was used for the evaluation. The amount of
lime addition used for the study ranged from 0 to 10,000 ppm
(as Ca(OH)2). Figures 112 through 114 show selected results.
As illustrated in Figure 112, the concentrations of free CO?",
P0$~, SiO|", and OH" can be increased significantly by lime addi-
tion. Free SO^'is reduced slightly when lime is added. Other
ligands, such as SOJ", Cl", F~, B(OH)I, MoO|% AsOr', and HVO?',
are only slightly, if at all, affected. It is expected that,
without any decrease in free metal ion concentrations, the in-
crease in ligand levels will lead to the increase in related
metal-ligand complex ing.
Figure 113 displays the results of lime addition on the
total soluble concentrations of major ions. As can be seen from
this diagram, only the total soluble calcium levels may be
affected by the lime addition. The total calcium concentration
can be increased dramatically by an added 100 ppm of lime. When
the dosage of lime is increased from 100 ppm to 10,000 ppm, total
soluble calcium will increase steadily from about 200 ppm to 400
ppm.
Most of the minor ions are affected by lime addition.
Although lime addition is usually accompanied by a pH increase,
the total soluble concentrations of minor ions rather than show-
ing a decreasing trend, usually increase in the FGD sludge liquid
phase. This is due to the formation of the strong metallic
complexes of hydroxide or carbonate. As shown in Figure 114,
total soluble cadmium can be increased from 0.01 ppb to 1.45 ppb
if the lime addition exceeds 1,500 ppm. Total soluble Fe(III)
also will increase to the level of 22 ppb from its original
level of 0.012 ppb for a similar lime dosage. Total soluble
manganese is reduced from its original level of 156 ppb to about
20 ppb as the dosage of lime is increased from 0 to about 500 ppm
(as Ca(OH)2). When the dosage exceeds 500 ppm, total soluble
manganese can reach concentrations as high as 36.5 ppb. Lime
addition also may increase the total soluble levels of Cu(II) b.y
a factor of 10. These levels, however, are still in the trace
level range (<0.001 ppb).
From,, the above discussion, it can be seen that thermodyna-
mically, the lime addition has a beneficial effect only for
manganese. The liquid phase concentrations of many other soluble
207
-------
en
o
10
12
-Free C03 Free SO!
Free OH'
Free P0~
4
Free SiO:
0 1. 2 345678 91011
Lime Addition (in 1000 ppm as Ca(OH)2)
Figure 112.
Effects of lime addition on the concentrations of
free 1i gands .
208
-------
1200
£
Q.
Q.
c
o
O
800
600
400
200
0 L
Mg(II)
0 1 2
6 7 8 9 10
Lime Addition (in 1000 ppm as Ca(OH) )
Figure 113.
Effects of lime addition on the total soluble
concentrations of major ions.
209
-------
-Q
a.
a.
•P
03
S-
+J
C
-------
constituents, such as Ca, Fe, Cd, will increase significantly
when extra lime is added to the FGD waste, thereby increasing
the potential for leaching of these constituents from the sludge
disposal site. This phenomenon, however, needs additional field
study to verify.
EFFECTS OF SILICATE ADDITION TO FGD SLUDGE
As was the case with lime, the addition of silicate com-
pounds has been employed for the fixation of FGD sludge. How
the concentration of metals and other ions in their various forms
change as a function of silicate additive concentration was
examined in this study. This examination was divided into two
sections: (1) to evaluate the overall effects of the silicate
addition, and (2) to identify the silicate level where the sili-
cate addition may become significant. The results are given in
Figures 115 through 124.
In this study, the effects of silicate addition were ob-
served from 10-5M to 10°M (0.28 to 28,000 mg/1 as Si) of total
silicate concentrations in the FGD system. The results of thermo-
dynamic calculations show that silicate addition may have a sig-
nificant effect on the levels of soluble aluminum (Figure 115)
and zinc (Figure 116). However, soluble levels of other elements
studied (Figures 117 through 124) were not shown to vary with the
silicate addition.
It can be observed in Figure 115 that the level of soluble
aluminum species is greatly reduced in the aged FGD sludge
liquor when the total silicate level is higher than 1 0 ~ 2 M (280
mg/1 as Si). When silicate levels increase from 10~2M to IQ-^M
(280 mg/1 to 2,800 mg/1 as Si), the total soluble aluminum con-
centration (about 2.7 ppm) can be reduced by about four orders
of magnitude. As silicate levels are further increased ( 10~'M),
however, the total soluble aluminum level will remain unchanged.
Therefore, if silicate is added for the control of aluminum
solubility, the optimum levels of silicate in the FGD system
are about lO-^M to 10~^M, depending on the final aluminum levels
desired.
Zinc exhibits behavior similar to that of aluminum when
silicate is added to the FGD sludge (Figure 116). The total zinc
levels will not be affected by silicate until the silicate level
reaches as high as 10'2M (280 mg/1 as Si). Between 10-2M and
IQ-IM of silicate, the total soluble zinc level can be reduced
4,000-fold. The same optimum levels of silicate addition for
aluminum are suggested for zinc in order to control soluble zinc
in the FGD sludge leachate. With the exception of aluminum and
zinc, other elements studied (Figures 117 through 124 will not
be affected significantly by silicate addition).
211
-------
~ 8
- 12
o
I
16
20
4321
Total Soluble Silicate Concentration
-log [SiT] (M)
Figure 115.
Effects of silicate addition on Al in FGD
wa stewater.
212
-------
3-
C0=
12
15
18
so-
Free Zn2+
Cl
PO:
J_
4321
Total Soluble Silicate Concentrate
-log [SiT] (M)
Figure 116.
Effects of silicate addition on Zn in FGD
wastewater.
213
-------
«3
CJ
CD
O
so;
OH"
003 Free Ca2+
PO:
10
12
4 3-2 1
Total Soluble Silicate Concentration
-log [SiT] (M)
Figure 117.
Effects of silicate addition on Ca in FGD
wastewater.
214
-------
10
12
so=
Free Mg2+
CO-
OH'
PO:
J I
4321
Total Soluble Silicate Concentration
-log [SiT] (M)
Figure 118
Effects of silicate addition on magnesium in F6D
wastewater.
215
-------
en
o
SOf
Free K+
Total Soluble Silicate Concentration
-log [SiT] (M)
Figure 119. Effects of silicate addition on K in FGD wastewater
216
-------
1-
4-
Free ;Na
COf
so;
4321
Total Soluble Silicate Concentration
-log [S1T] (M)
Figure 120.
Effects of silicate addition on Na in FGD
wastewater.
217
-------
u
3
_ 6
s:
r— i
t— i
•o Q
0
1 — 1
CD
0
1
12
15
18
soi
cof
CT ^"^
OH"
F~
~ PO|
I i I i
4321
Total Soluble Silicate Concentration
-log [SiT] (M)
Figure 121.
Effects of silicate addition on Cd in FGO
wastewater.
218
-------
u
3
s:
^ 6
i— «
i— i
H-«
l__l
9
o
t
12
15
18
~" OH"
F"
POZ
S04
_ Free Cr3+
Cl"
i i i i
4321
Total Soluble Silicate Concentration
-log [SiT] (M)
Figure 122.
Effects of silicate addition on Cr in FGD
wastewater.
219
-------
en
0
15
18
Free Cu
2+
*
OH
12
PO
4
4321
Total Soluble Silicate Concentration
-log [SiT] (M)
Figure 123. Effects of silicate addition on Cu in FGD
wastewater.
220
-------
Ol
O
Free Pb'
10
B(OH)'
CO!"
3
so;
OH;
CT
12
54321
Total Soluble Silicate Concentration
-log [SiT] (M)
Figure 124. Effects of silicate addition on Pb in FGD
wastewater.
221
-------
EFFECTS OF HYDROGEN SULFIDE ADDITION TO FGD SLUDGE
Sulfide is known to be an extremely effective scavenger for
removing certain trace metals from the aqueous solution. Since
hydrogen sulfide may be available at some power plants, the
effects of sulfide addition to FGD wastes were investigated.
For modeling purposes, the total sulfide concentration was
varied from 10-7-51M to 10-3.20M (0.001 ppm to 20 ppra). The
results of calculation show that the distributions of copper,
lead, cadmium, zinc, mercury, silver, and cobalt species in the
FGD waste are significantly affected by sulfide addition. The
effect of sulfide addition on other constituents is negligible.
As shown in Figure 125, the total soluble concentrations of
both lead and copper can be reduced to trace levels by adding
as little as 0.001 ppm (10-7.5lM) of sulfide to the FGD sludge.
The total soluble levels of these two elements will be further
reduced when sulfide addition is increased.^ The effect of sul-
fide addition on the total soluble cadmium concentration also
displays similar behavior (Cd concentration decreases as sulfide
addition increases). The total soluble cadmium concentration
will not, however, reach trace levels until the sulfide concen-
tration exceeds about 0.2 ppm. The reduction achieved in total
soluble zinc concentration is negligible if sulfide addition is
less than 0.1 ppm. When the total added sulfide exceeds 0.5
ppm, the soluble zinc can also be reduced to trace levels. The
reduction in levels of soluble heavy metals is due to the for-
mation of insoluble metallic sulfide compounds such as CuS(s),
PbS(s), CdS(s), and ZnS(s). Figure 126 displays the distribu-
tion of metallic sulfides in FGD waste as a function of the sul-
fide concentration. At low total sulfide levels (e.g., less
than 0.001 ppm), sulfide addition will favor the formation of
Ag2S(s) and CuS(s). After sufficient soluble silver and copper
are removed from solution, the remaining soluble sulfide can then
react with other soluble metals. The order of metallic sulfide
formation with increasing sulfide levels is as follows: AggSfs) •
CuS(s) - PbS(s) - CdS(s) - ZnS(s) - CoS(s). This sequence can
be seen in Figure 126.
Although the trace heavy metals can be removed efficiently
by sulfide addition, this treatment may not be desirable for two
reasons. First, excess hydrogen sulfide itself is an undesirable
contaminant in wastewater (leachate). Second, the FGD sludge
lagoon is an open pond, where oxygen can gradually diffuse into
the FGD waste and oxidize the metallic sulfide solids. Diffusion
and oxidation will eventually convert the sulfide solids into the
original predominant solids, and again release the soluble metal
species.
222
-------
c
o
•r-
C
-------
0)
•T—
u
(U
Q.
-------
EFFECTS OF PHOSPHATE ADDITION TO FGD SLUDGE
In this study La Cygne Plant data are used for evaluation,
total phosphate concentrations in the FGD sludge ranged from
10-5 to 10-lM (0.31 to 3,100 mg/1 as P). Among the metals
studied, it was found that only the total levels of magnesium,
calcium, and cadmium can be significantly affected by phosphate
addition. Soluble magnesium is reduced by a factor of 2.5 as
the phosphate level is increased from 10-5 to lO^M (Figure 127)
This change is due primarily to the formation of Mg3(P04)2(s)
solid in the FGD sludge. According to the calculation, the
level of Mg3(P04)2(s) solid in the sludge is increased at the
following ratios:
Total phosphate (M) % of Mq formed
in the FGD system as Mg3(PQ4)2(s)
10"5 * 0
10-4 = 0
10-3 5
10-2 31.9
10-1 55.5
Due to the formation of Mg3(P0*)2(s), the concentration
Mg2+ ion is significantly reduced. This change also le<
of free
leads to
a decrease in the concentration of all soluble magnesium com-
plexes (except the Mg-P04 complexes, which shows an increase
in concentration with the increase of phosphate addition.
The total soluble calcium can also be reduced slightly as
the total phosphate level exceeds about lO'^M (310 mg/1 as P)
(Figure 127). In a manner similar to magnesium, this reduction
is due to the formation of calcium phosphate solids in the FGD
sludge. Three Ca-P04 solids may be formed in the FGD sludge:
Cas(P04)30H(s ) , Ca4 ( P04 ) 3H (s ) , and CaHP04(s). The following
table shows the effect of phosphate variation on Ca-P04 solids
formati on :
Total phosphate (M) % of Ca formed
in the FGD system^ as phosphate sol
10
10
10
system^ as phosphate solids
'*
,
,
"
10"'
= 0
* 0
* 0
1
36
.5
.2
Because of the Ca-P04 solids formation, the amount of CaF2(s)
solid will decrease slightly (about 0.1 in terms of the total
calcium l£vel in the sludge). This effect will lead to an in-
crease in the soluble fluoride level of about 23 percent for a
IO*IM addition of phosphate to the sludge.
225
-------
E
Q.
a.
c
o
s=
-------
The formation of calcium phosphate solids also causes a
decrease in the amount of CaSCs*!/2H20(s) in the FGD sludge.
Due to this change, the free S03" concentration is increased
substantially (about 50 percent above its original level). This
change leads to a significant increase in Cd(S03)i~ complexes,
and in so doing increases the total soluble cadmium concentration
by a factor of 2 above its original level (see Figure 128).
EFFECTS OF MAGNESIUM ADDITION TO THE FGD SORBENT
The use of high magnesium scrubbing reagents could become
widespread (Ref. 1). This study used the model to identify the
effects of various concentrations of magnesium additives on the
FGD sludge liquid phase. In this study, the magnesium concen-
tration in the FGD sorbent was var.ied from 10~4 to 1OM (2.4 ppm
to 0.24 percent as Mg) to observe the effects on the speciation
of metals. Results for some selected elements are shown in
Figures 129 through 134.
Figure 129 shows that an increase in magnesium concentration
in the FGD sorbent will also increase the levels of all soluble
species of magnesium, This formation of strong magnesium com-
plexes in the FGD sorbent is due to th« increase of soluble free
Mg2+ ion. This phenomenon leads to the decrease of available
free ligands such as S0^~, F~, P0|", and CO^" • Therefore, the
concentrations of the complexes formed by tne above ligands
with other metals are usually reduced (see Figures 130 to 134).
The effects of magnesium addition on the speciation of
calcium in the FGD system is shown in Figure 130. As can be
seen from the diagram, the concentrations of'Ca-S04, Ca-F,
and Ca-P04 complexes are greatly reduced in the FGD sorbent
when the total magnesium concentration in the system exceeds
IQ-^M (2,430 ppm as Mg). The Ca-C03 complexes appear to be un-
affected when magnesium is added to the system. The most impor-
tant species for calcium in the system is free Ca^* ion, which
will not be affected by the addition of magnesium. Therefore,
magnesium addition will not alter the total soluble level of
calcium in the system.
Similar phenomena also hold true for sodium and potassium.
When magnesium is added to the system, the concentrations of
sulfate complexes with sodium or potassium are decreased, but
total soluble levels of potassium and sodium remain unchanged.
For minor ions, the effects of magnesium addition are also
confined to concentration changes of the S0|~, F~, and PQ^com-
plexes (Figures 131 through 134). In general, if these com-
plexes comprise the predominant soluble species for a minor
element, *then magnesium addition may affect the total soluble
levels of that element. Otherwise, the effects are confined
227
-------
300
250-
200-
o.
o.
c
o
-------
en
o
10-3 1Q-2 10'1
Total Mg(II) Concentration
10'
Figure 129.
Effects of Mg addition on the distribution of
soluble Mg complexes.
229
-------
CD
o
Free !Ca2+
S04
OH'
10
12
10-3 io~2 1Q-1 10°
Total Mg(II) Concentration (M)
Figure 130. Effects of Mg addition on the speciation of Ca
230
-------
•a
o
en
o
4 _
8
12
16
20
24
so;
co:
OH-
503
POJ
,-4
,-3 1n-2
CT
Free Cd2+
,-1
10"* 10~J lO"" 10 ' 10°
Total Mg(Il) Concentration (M)
10
Figure 131. Effects of Mg addition on the speciation of Cd,
231
-------
en
o
12
15
18
J I
10° 10
Total Mg(II) Concentration (M)
Figure 132.
Effects of Mg addition on the speciation of
Cr(III).
232
-------
3-
12
Free Cu
2 +
B(OH)
Cl
CO
15
18
PCT
10~3 10~2 10-1 10° 10
Total Mg(II) Concentration (M)
Figure 133. Effects of Mg addition on the speciation of Cu
233
-------
01
O
.10
12
10
-4
otr
soi
POf
,-3
Free Zn
21-
Cl
-1 °
10 ' 10
Total Mg\(II) Concentration (M)
Figure 134. Effects of Mg addition on the speciation of Zn.
234
-------
only to elements forming the above-mentioned complexes. It is
expected that the total soluble levels of most minor elements
studied will not be altered by magnesium addition. The principal
exception is chromium, which may form strong Cr(III)-F complexes
(primarily Crp2+) in the low pH region.
EFFECTS OF SULFITE OXIDATION
As discussed previously, the aging of the FGD wastes usually
results in an increase of redox potential and pH. During this
aging process, it is expected that the sulfite species will
gradually be oxidized to sulfate. Since both sulfite and sulfate
species are major components in FGD sludge, the oxidation of sul-
fite may cause changes in other constituents. In this study, the
possible effects of sulfite oxidat.ion on some selected elements
were examined. The results are presented in Figures 135 through
156.
In this discussion, total sulfite was assumed to be oxidized
from an original concentration of 10-0.16^ to a concentration of
10-4-16^ y^g effects on other constituents at the La Cygne
Plant were used for the calculation. Only the results of two
typical pH values (pH = 6.5 and 9.0) are discussed here.
Figure 135 and 136 show the effects of sulfite oxidation on
various sulfite species. Due to the decrease of total sulfite
concentrations in the system, various sulfite complexes are also
decreased. As can be seen from Figure 135, the decrease of HSOo
or free $03 species approximately follow the rate of sulfite
oxidation. However, tne concentration trends of metallic sulfite
complexes are different from that of total sulfite concentration.
For example, total sulfite oxidation to 10~^ of its original
level will result in a factor of 10"7 decrease in the Cd-S03
complex concentration. Figure 136 indicates that sulfite oxi-
dation will cause a tremendous decrease in the level of
CaS03'l/2H20(s) solid in the FGD sludge. For La Cygne Plant FGD
wastes, if the total sulfite level is oxidized to one-tenth of
its original level (perhaps by aeration), the CaS03 • 1 /2\\2§( s )
solid will disappear as shown in Figure 136.
Sulfite oxidation has only a minor effect on the speciation
of soluble calcium (see Figure 137). It may cause a tremendous
change, however, in the level of calcium solids in the FGD
sludge (see Figure 138). The calculations show that the
CaSOs'l/SHgOU j solid will be transformed to CaS04 '2H20(s) during
sulfite oxidation when the pH equals 6.5 and to CaC03(s) when
the pH equals 9 .0 .
The magnesium species will not be affected significantly
during su*lfite oxidation (Figures 139 and 140). For potassium
and sodium (Figures 141-144) sulfite oxidation causes an increase
235
-------
pH = 6.5
pH = 9.0
ro
co
a\
x
01
Q.
E
o
o
ii n 6
o
en
o
12
15
JQ
-0.16
Figure 135. Effects of sulfite oxidation on the concentrations of sulfite complexes.
-------
ro
100
80-
£ 60 -
Q
40-
20
0
10"
\
>
\
\
-
ft
s
V
1
— >
\
- 0
T
r—
|CM
%ro
0
CO
(
0.
IO
_3
—
1
y
pH =6.5
1 1 1
Free SO^ (aq)
v.
v^
HSOg (aq)
—
—
I
\
\
\
\
\\ . i
100
80
c
o
•r—
JD
T 60
10
•t—
O
40
20
n
pH = 9.0
"\ '
^-HSO^ (aq)
_ _
Free S0| (aq)
\
\
L
\
\
( J\
to
N \
r-^Kj \
o1 \
CO \
to \ \
°i m
I ll\ .
6 10~1>16 10~2'16 10~3'16 10~4'16 10~°'16 10"1'16 10~2-16 10~3-16 10"4
[so|T]
Figure 136. Effects of sulfite oxidation on the primary distribution of S03= species.
-------
ro
CO
0
o
en
O
12
15
pH =6.5
I 1 1
Free Ca2+
OH
1 i i
0
CO
O
CD
O
8
12
16
pH = 9.0
—i r
so:
Free Ca2+
OH-
j-0.16 jQ-1.16 jQ-2.16 jQ-3.16 jQ-4.16
20
n-0. 1 6
1 I i
10"1'16 10~2-16 10~3-16 10~4-16
Figure 137. Effects of sulfite oxidation on the speciation of Ca.
-------
100
c
o
-Q
•r—
J-
ro
40
PH =6.5
oi
04
o"
///////// /, /////// / /
S
Z Z Z Z Z Z Z Z Z / Z Z Z Z Z Z Z Z Z
Z_///// S ////// _S //////
^z/zZZ///////z// //Z/ Z
Z////////ZZZZZZ. ZZ/
20
S///Z/////S////Z//
/////////////////S///
/////////////////// /-?
S/////////S/S/////.
S////////////////S//S
s/////////////////
s/ZZZ//Z Z////////Z/Z//
//z/z///////s z/z z/z/z *
ZZZ
///////////////•?
ZZZZZZ Z/Z Z//Z Z Z/ZZZZ
z z/ z zzzz z _z/~z/ z z z z/ _z~z/.
Z Z Z Z Z Z Z Z Z Z Z Z / / Z Z Z Z Z Z Z A
_z z z_zs z z z z z z z / z z z z z z z z
Z Z Z Z Z Z Z Z Z Z Z Z / / Z Z Z / Z Z / Z
100
CaF2(s)-
pH = 9.0
\\ \ \ \ \ N\ V\ \ \ "V A \~\' V \ \ \ \ T7^. ~\ \ \ \\ \
s~
•*->
I/I
i-O. 16
16
1Q
-2.16
1-4.16
CSO=T]
Figure 138. Effects of sulfite oxidation on the primary distribution of Ca species.
-------
0
pH '= 6.5
1 1
so
cn
o
' q
y
12
Free Mg+2
OH
15
10
1 I
0
cn
2!
cn
O
12
-0.16
15
pH = 9 . 0
n i r
so
Free Mg+2
OH
i i
.16 JQ-2.16 jQ-3.16 jQ-4.16 1Q-0.16 1Q-1.16 j Q-2 .1 6 j Q-3.1 6 10~4.16
[SO=T]
[so=T]
Figure 139. Effects of sulfite oxidation on the speciation of Mg.
-------
ro
100
pH =6.5
80
c.
o
£ 60
S-
o
40
20
0
1 I
Free Mg
2+
MgSO°(aq)
1 I i
100
pH = 9.0
Free Mg
80
c
o
•I—
$-
to
Q
60
40
20
MgSO°(aq)
10
-o.i6
10-2-16 10~3'16 10~4'16
0
i i
10~2-16 10~3-16 10~4-16
[so=T]
Figure 140. Effects of sulfite oxidation on the primary distribution of Mg species.
-------
ro
0
pH =6.5
pH = 9.0
3 -
6~
o>
o
9 _
12-
15
1 1 1
50=
Free K+
— •—
- -
l l i
u
3
s:
i — i
t— i
•* 6
i i
en
o
I
9
12
15
l 1 1
^_ Free K+
""™ —
-
l i i
10
-0.16
-3. 16
~ l ' J 6 ~2 -1 6 "3'1 6
Figure 141. Effects of sulfite oxidation on the speciation of K.
-------
100
80
c
0
•r—
£ 60
i/>
a
ro
£ 40
20
0
pH '= 6.5
1 1 I
Free K+
_^^
— -
KSO; (aq)
_ —
1 I I
100
80
c.
0
I 60
to
•r-
Q
40
20
0
pH = 9.0
i 1 I
Free K*
~/^
_
KSO- (aq)
_ _
I I i
1Q
-0.16
10-2.16 iQ-3.16 jo"4-16
[SO=T]
Figure 142. Effects of sulfite oxidation on the primary distribution of K species.
-------
ro
pH = 6.5
Cl
Free Na+
en
O
COf
12
15
I i
1Q
-0.16
.16 1Q
-3.16
0
12
15
pH = 9.0
1
SOZ
Free
j i i
0~2 -1 6
~3A 6
Figure 143. Effects of sulfite oxidation on the speciation of Na.
-------
ro
100
80
c
o
60
40
20
0
pH = 6.5
1 I
Free Na
NaSQ-(aq)
4
1 1 1
100
80
c
o
60
40
20
10
-0.16
JQ-2.16 jQ-3.16 lfl-4.16
0
pH = 9.0
i i r
Free Na
NaSO-(aq)
I i i
10-2.16 1Q-3.16 10-4.16
[SO|T]
Figure 144. Effects of sulfite oxidation on the primary distribution of Na species.
-------
ro
-p.
cr.
0
O
o
I
12
pH = 6.5
I I
P04
I I
0
pH = 9.0
^ 8
•a
01
o
12
16
15
iQ-0.16 jQ-1.16 jQ-2.16 jQ-3.16 jQ-4.16
20
^3
^so^
C0|
C1
OH"
Free
i i
jQ
[SO=T]
-0.16 jQ-1.16 }Q-2.16 jg-3.16
[SO=T]
Figure 145. Effects of sulfite oxidation on the speciation of Cd.
-------
ro
100
pH '= 6.5
c
o
•f—
-M
a
.a
•r—
s-
4->
in
•r—
Q
-0.16 -1.16 -2.16
100
80
c
•o
J_
4J
CO
•i—
Q
60
40
20
0
pH = 9.0
(s)
-4.16 jQ-0.16 1Q-1.16 jQ-2.16 jQ-3.16
Figure 146. Effects of sulfite oxidation on the primary distribution of Cd species.
-------
ro
oo
o
en
o
12
15
pH = 6.5
1 I T
OH
Free Cr
3f
Cl
I i i
\~0.16 in—1• 1 6 -I rt~ 2 • 1 6 -i r\~~ 3 . 1 6 i.
0
pH = 9.0
8
o
en
O
12
16
20
i 1 i
OH
Free Cr
I i i
10
-2.16
1-^.16
[SO=T]
Figure 147. Effects of sulfite oxidation on the speciation of Cr.
-------
ro
45>
V£)
100
CrF
pH = 6.5
80
C
O
£ 60
40
20
0
Cr(OH)3 (s
100
Cr(OH)t> + Cr(OH)^ (aq)
CrAsO, (s)
j i I
80
c
o
I 60
40-
20
0
pH = 9.0
Cr(OHy;(aq)
j i i
JQ
-0.16
jQ-0.16 jQ-1.16 jQ-2.16 jg-3.16 jQ-4.16
Figure 148. Effects of sulfite oxidation on the primary distribution of Cr species.
-------
pH =6.5
pH = 9.0
u
5
2?
^ 10
i — i
»— i
i_j
cr>
ro o
£ ' 15
20
25
1 1 1
B(OH)-
soi
rree LU
n'—^
C03
F -^ PQ.L
1 li
u
6
i
1 — 1
5 12
o
1 — 1
en
o
18
24
•\f\
\ \ \
B(OH)-
nn~— S0/"~v PA—
UH -^ J"4 ^ C03
\ \ cr
: \— .-i —. - — . .-.
Free Cu+?-/
c-
r\r\ -~
rl)4
1 1 1
j-0.16 jQ-1.16 jQ-2.16 jQ-3.16 jQ-4.16
CSO=T]
1Q
-3.16 iA-^.16
[so;T]
Figure 149. Effects of sulfite oxidation on the speciation of Cu.
-------
ro
en
100
80
c
o
60
40
20
0
pH = 6.5
Cu2C03(OH)2(s)
c
o
•I—
4J
n
JD
*f"
J-
4->
CO
•I—
Q
pH = 9.0
1UU
80
60
40
20
0
(
;i
2
C
)
>(
C
H
);
,
'<
1
-
-
-
jQ-0.16 jQ-1.16 jQ-2.16 jQ-3.16 jQ-4.16 jQ-0.16 jQ-1.16 jQ-2.16 jQ-3.16 jQ-4.16
Figure 150. Effects of sulfite oxidation on the primary distribution of Cu species.
-------
pH =6.5
pH = 9.0
0
4
sT
• — i
~ a
i— i
>— <
v
u_
1 — 1
en
01 T 12
ro lit
16
20
10"
1 1 1
— ^2i^_ OH
^"---^
^~\B(OH)7 —*
F """ --^
P04
Free Fe3^
Cl~
— 4 —
SiOl -/
I i i
0.16 jQ-1.16 jQ-2.16 jQ-3.16 j
0
\
5
S
r~I 1 n
' — ID
i — i
t— 4
»— t
*oT
U-
1 — 1
en
Q
7 15
20
25
0-4.i6 1Q-(
1 1 1
OH~
(OH)^
S0= ^^^^>^^
F Si 03
pol
Free Fe+3
Cl"
i i i
). 16 1Q-1.16 jQ-2.16 10-3.16 1Q-4
[so=T]
Figure 151. Effects of sulfite oxidation on the speciation of Fe
-------
100
80
c
o
•r—
-»->
£ 60
S-
-M
to
•r-
Q
&«
ro
a 40
20
0
pH = 6.5
~*
-
_
1
I
Fe(
|
OH)3
I
(s)
1
1
"
-
^_
100
80
c
o
•r—
-M
3
^3
t 60
4->
1O
•r—
Q
^
40
20
0
pH = 9.0
-
I
Fe(
1
3H)3
1
(s)
\
I
-
10
-0.16
lfl
-3.16
1Q
-0.16
1Q
-2.16
Figure 152. Effects of sulflte oxidation on the primary distribution of Fe species.
-------
pH =6.5
pH = 9.0
in
u
3
2:
i — i
i — i
>—>
^ 6
a.
en
o
1
q
12
15
1 1 1
S0=
Free Pb2 + — ,
B(OH)4 \
C 1 rn=
3
OH"
1 i i
u
3
z:
i — i
i — i
i— i
JD 6
a.
i_i
en
o
i
12
15
I I 1
col
B(OH)-
~
so^
OH-
Cl
i o 4-
iFree Pb2
I i i
10
-o.i6
10~3'16 10~4'16
10-2.16 10~3.16
[SOIT]
Figure 153. Effects of sulflte oxidation on the speciation of Pb.
-------
ro
en
en
c
o
s_
+J
I/)
•I—
a
-1.16 -2.16 -3.16
100
pH = 9.0
80
c
o
•I—
4->
3
.£»
•r-
f-
-«->
I/I
•r~
C3
Jr«
60
40
20
0
10~u-
jQ-0.16 jQ-1.16 jQ-2.16 jQ-3.16 jQ-4.16
[SO=T]
Figure 154. Effects of sulfite oxidation on the primary distribution of Pb species
-------
0
pH =6.5
1 1
0
pH = 9.0
1 T
Free In
2+
ro
cn
C
M
cn
O
OH'
so
OH
c.
M
CT>
O
Free Zn2+
Cl
12
12
15
I i
j-0.16 jQ-1.16 jQ-2.16 jQ-3.16 iQ-4.]
151
r>-0. 1 6
10~ul6 lO"2-16 1Q-3-16 10~4'16
Figure 155. Effects of sulfite oxidation on the speclation of Zn.
-------
ro
tn
100
pH =6.5
80
c
o
60
O
40
20
0
Free Zn
2
-ZnCl(aq)
ZnSO.(aq)
I I
10
-0.16
1Q
-3.16
100
80
c
o
jQ
•i—
i-
60
40
20
0
pH = 9.0
10-1.16 10-2.16 jQ-3,16
[so;T]
Figure 156. Effects of sulfite oxidation on the primary distribution of Zn species.
-------
in the concentration of sulfate complexes and the decrease of
free ions.
2_
Due to the oxidation of sulfite, the Cd(S03)2 species will
be transformed gradually into the CdS04(aq) species. As can be
seen in Figures 145 and 146, a tenfold decrease in total sulfite
concentration will completely transform the Cd(S03)£~ species to
CdS04(aq). The sulfite oxidation, however, will not affect the
cadmium solid phase significantly.
Iron is similar in behavior+to cadmium as sulfite oxida-
tion tends to transform the FeS03 complex to Fe(S04)2 complex.
The solid phase of iron, however, again remains unchanged
(Figures 151 and 152).
Other minor elements studied,' such as chromium, copper,
lead, and zinc, appear to be unaffected by sulfite oxidation
(Figures 147-150 and 153-156). This is because of the absence
of a sulfite complex, as well as the constant oxidation states
for these elements in the FGD sludges. Although the concen-
trations of sulfate complexes of these elements show an increase
during sulfite oxidation, the changes are only minor.
258
-------
-------
SECTION 8
SUMMARY OF FINDINGS
INTRODUCTION
A conventional environmental .impact assessment of flue gas
desul furization (FGD) sludge disposal would include chemical
analysis and identification of the total concentrations of con-
stituents in the sludge and its leachate. However, public health
effects of FGD waste disposal depend on whi.ch chemical forms or
species of the constituents are released to surrounding waters,
and not necessarily on their total concentration.
The only feasible means of obtaining contaminant species
information in FGD sludge lies in thermodynamic modeling. A
thermodynamic model can also be used to predict the migration
trends of the constituents when the FGD wastes age; to estimate
the final concentrations of constituents in the FGD leachate
(aged wastewater), without conducting expensive field monitoring;
and to predict the effects of operational and chemical changes
i n the FGD wastes .
Many available techniques can be used to construct and
interpret a chemical thermodynamic model. In this study, the
equilibrium constant approach is employed. This method involves
solving the stoichiometric equations of various chemical species,
which are subject to constraints imposed by the equilibrium con-
stants as well as mass balance and charge balance relations.
Diagrams, such as Eh-pH plots, ion-ratio plots, concentration
pH figures, and species distriubtion figures, are then used to
display the stability field and speciation results.
The thermodynamic model used in this study was verified for
suitability and accuracy by the analytical results of various FGD
sludge samples taken from the Kansas City Power and Light La
Cygne Power Station. The model is also operated over a wide
range of operational and chemical changes to theoretically deter-
mine their impacts on the concentration and speciation of various
solid and soluble species. The impacts of (1) changes in pH and
ionic strength; (2) addition of lime, silicates, hydrogen sulfide,
and phospiiates to the sludge; (3) variation of chloride, sulfate,
and borate levels; (4) addition of magnesium to the sorbent; and
(5) sulfite oxidation, were all estimated using the model.
259
-------
METHODOLOGY OF SPECIES ANALYSES
Two principal graphical treatments, Eh-pH plots and the ion-
ratio method, are used to describe the stability fields of con-
stituents in F6D sludge. The Eh-pH plot is employed for con-
stituents with different redox species, such as iron, manganese,
mercury, arsenic, and selenium. The ion-ratio method is used
for constituents with only one redox state, or for reactions
involving no electron transfer.
The speciation model is constructed by the equilibrium con-
stant approach. The actual mathematical equilibrium model in-
volves a series of simultaneous equations which describe the
various interactions among components of the system. Seven
general equations are involved, as shown in Table 13. In order
to solve these equations simultaneously, the information on
metal and ligand species, overall formation constants, solubility
products (and/or Henry's constants), and activity coefficients
must be compiled from the literature. A computer solution is
necessary, as the expanded equations number in the hundreds.
The resultant nonlinear equations are solved by Newton-Raphson
iteration .
Because the chemical composition of FGD sludge can vary over
an' extremely wide range, this study focused on speciation at the
lowest levels (ionic strength (I) = 0.05) and the highest levels
(I = 0.8). All possible distributions of species are expected
to be within this range.
SPECIATION OF SOLID AND SOLUBLE CHEMICAL SPECIES
Fresh FGD Sludge
The thermodynamic modeling of the fresh FGD wastewater sys-
tem can be performed as if no solid were formed or dissolved,
because (1) the equilibrium conditions among soluble species
can easily be reached, and (2) the rates of nucleation and disso-
lution of the solid species are very low. The predominant solu-
ble species, based upon thermodynamic calculation, are summarized
in Table 14. This table shows that the major ions (i.e., cal-
cium, magnesium, potassium, and sodium) and the manganese species
exist as free ions, in the fresh FGD wastewaters .
Other trace metals, however, can be complexed considerably
in the same wastewaters. As shown in Table 14, chloride corn-
pi exes may under certain conditions become the predominant
species for cadmium, copper, lead, mercury, and zinc; borate
complexes may become the predominant species for copper and lead;
sulfite complexes may become the predominant species for cadmium
and iron; and hydroxide complexes may become the predominant
species for mercury, zinc, and the trivalent metals, such as
260
-------
TABLE 13. GENERAL MODELS USED FOR
SPECIATION CALCULATION
B(1.J)nm[M(1)f][L(J)f]
nm f f
m n
M(i)mL(j)n
KM(i)L(j) ' RM(i) L(j) ' fM(1) L(j)
[H(Df] = - E - g - _ - p__g - B - a
M(1) ' L(j) - [L(j)f]q
w T U V
YM(i) ' L(j) ' [M(i)f]V
h a b
j'l P=I S-l R«(')pUj)q = 1
g c d
Z Z z RM(i) L(j) = ]
k 1 h
[M(i)T] = [M(1)f] + 2 Z _Z m[M(1)mL(j)n]
h a b
h c d
+222 n[M(i) L(j) ]
j-1 u=1 v=l m n
k 1 g
[L(j)T] = [L(j)f] + I I Z n[M(i)L(j)n]
1 T m = 1 n = 1 j = 1 m n
gab
+ 2 Z Z [M(i)L(j)J
1=1 p=1 q=] P q
g c d
+ 2 Z Z [M(i) L(o) 1
261
-------
TABLE 13 (Continued)
where:
[M(i) L(j) ] = concentration of complex M(i) L(j) (in
n moles/liter) m n
[M(i)-] = free metal ion concentration of ith metal
(in moles/liter)
[L(j),] = free 'concentration of jth ligand (in
moles/1i ter )
[M(i)j] = total concentration of ith metal in the
system (in moles/liter)
RM(DpL(j)q
and
RM/.N ./ • \ = mole fraction of solid or gas species for
u ^'v metal or ligand solids
i = metal species
j = ligand speci es
g = total number of metals
h = total number of ligands
k = maximum number of metals (M(i) coordinating
ligands L(j)
1 = maximum number of ligands L(j) coordinating
metal M(1)
a,b,c, and d = positive integer showing maximum number
of metals or ligands in the solids or gases
6(i.j) = overall formation constant of complex
Y = thermodynamic activity coefficient of soluble
x species x.
262
-------
TABLE 13 (Continued)
f = thermodynamic activity coefficient of solid
(or gas) species x (in this study, assume
f * 1 ).
x '
K = solubility products or Henry's constants.
263
-------
TABLE 14. PREDOMINANT SPECIES OF SOLUBLE CONSTITUENTS IN FRESH FGD WASTEWATER
ro
cr>
Ionic
Constituent Strength
Predominant Species
Al
As
Cd
Ca
Cr
Co
0.05
0.8
0.05
0.8
0.05
0.8
0.05
0.8
0.05
0.8
0.05
0.8
pH = 5
A1F2*(34).A1(OH)2*(20),
A1F2+(17)
AlF2+(55)
H2As04'(98)
H2As04~(95)
Cd2+(50)CdC03(aq)(40)
CdCl+(66)
Ca2+{83)
Ca2+(71)
Cr(OH)2+(79)
CrOH2+(65)
Co2+(69)
Co2+(40),CoS04(aq)(26)
pH = 7
A1(OH)4-(100)
A1F2+(38),A1F3(31)
HAs042~(68)
HAs042'(78)
Cd2+(49),CdCl+(40)
Cd(S03)22-(59)
Ca2+(89)
Ca2+(71)
Cr(OH)2+(85)
Cr(OH)2+(81)
Co2+(68)
Co2"l'(40),CoS04(aq)(26)
pH = 9
A1(OH)4-(100)
A1(OH)4-(100)
HAs042"(100)
HAs042'(97)
CdC03(35),Cd2+(21),
CdClOH2+(20)
Cd(S03)22"(65)
Ca2+(81)
Ca2+(71)
Cr(OH)4-(100)
Cr(OH)4-(100)
CoC03(aq)(44),Co2+(26)
CoC03(aq)(28),Co2+(25),
CoCl+(20)
-------
TABLE 14 (continued)
Ionic
Constituent Strength
Predominant Species
ro
CTl
en
Cu
Fe
Pb
Mg
Mn
0.05
0.8
0.05
0.8
0.05
0.8
0.05
0.8
0.05
0.8
0.05
0.8
pH » 5
Cu2+{54)
CuB(OH)4+(35),CuCl+(26)
F~(25),SnF+(52)
CaF+(40),F~(38)
Fe(OH)2+(83)
FeS03+(97)
Pb2+(55)
PbCl+(33),
PbS04(22),Pb2+(21)
Mg2*(79)
Mg2+(66)
Mn2+(79)
Mn2+(55)
pH = 7
Cu(B(OH)4)2(aq)(51)
Cu(B(OH)4)2(aq)(83)
F~(40),MgF+(44)
Fe(OH)2+(100)
Fe(OH)2*{84)
Pb(B(OH)4)2(aq)(45),
Pb2+(19)
Pb(B(OH)4)2(aq)(87)
Mg2+(79)
Mg2+(66)
Mn2+(78)
Mn2+(55)
pH = 9
Cu(B(OH)4)2(aq)(97),
Cu(B(OH)4)2(aq)
Cu(B(OH)4)2(aq)(100)
F~(93)
MgF+(47),F"(45)
Fe(OH)4-(93)
Fe(OH)2+(93)
Pb'(B(OH)4)2(aq)(95),
Pb(B(OH)4)2(aq)
Pb(B(OH)4)2(aq)(100)
Mg2+(65)
Mn2+(76)
Mn2+(54)
-------
TABLE 14 (continued)
Ionic
Constituent Strength
Predominant Species
en
cr>
Hg
Se
Na
Zn
0.05
0.8
0.05
0.8
0.05
0.8
0.05
0.8
0.05
0.8
pH = 5
HgCl2(aq)(87)
HgCl3-(47),HgCl42-(26)
HgCl2(aq)(27)
K+(97)
K+(89)
HSe03~(97)
HSeOo~(97)
O
Na+(95)
Na+(95)
Zn2+(74)
Zn2+(47),ZnCl+(34)
pH = 7
HgCl2(aq)(62)
HgCl3-(46),
K+(97)
K+(89)
Se032-(74)
Se032-(74)
Na+(95)
Na+(95)
Zn2+{74)
Zn2+(43),ZnCl+(33)
pH = 9
Hg(OH)2(aq)(65)
HgC10H(aq)(52)
K+(98)
K+(89)
Se032"(99)
Se032~(99)
Na+(97)
Na+(95)
Zn(OH)2(aq)(68)
Zn(OH)2(aq)(42),
ZnC10H(aq)(26)
Note: Values in the parentheses indicate the percent of the total concentration.
* If one species accounts for less than 50 percent of the total concentration, then more than one species
will appear.
-------
chromium and iron. In the fresh FGD wastewater, arsenic and
selenium exist primarily as arsenate and selenite species. The
predominance of a given species can be affected significantly
by the pH level of the wastewater. The ionic strength (or,
more specifically, the soluble levels of the related ligands)
also plays an important role in the speciation of most consti-
tuents .
Aged FGD Sludge
The speciation of constituents in the solid and soluble
phases of aged FGD sludge was computed with the assumption that
the equilibrium condition among all the soluble and solid species
had been reached. Due to the long contact period, it is generally
quite possible that equilibrium conditions between solid and
liquid phases can be reached in the aged FGD wastes. The cal-
culated results are summarized in Table 15.
Results show that sulfur dioxide removed from the flue gas
reacts to form CaS04-2H2
-------
TABLE 15. PREDOMINANT SPECIES OF CONSTITUENTS IN AGED FGD SLUDGE
ro
crv
00
Ionic
Constituent Strength
A1 0.05
0.8
As 0.05
0.8
Cd 0 05
0.8
Ca 0.05
0.8
Cr 0.05
O.B
Predominant
pH -.5
A1(H2P04)(OH)2(s)
Al(H2P04MOII)2(s)
As°(s)
As°(s)
CdC03(s)
CdC03(sJ
CaS03.l/2H20(s),
CaS04.2H20(s)
CaS03.H20(s),
CaS04.2H20(s)
Cr(OH)3(s)
Cr(OH)3(s)
Solid Species
pll » 7
Al(M2P04)(OII)2(s)
Al(H2P04)(OH)2(s)
As°(s)
As°(s)
CdC03(s)
CdC03(s)
CaS03.l/2H20(s),
CaS04.2H20(s)
CaS03.H20(s),
CaS04.2H20(s)
0{OH)3(s)
Cr
HAs042-{8.82)
HAs042-(10.91)
Cd(S03)22-(7.72)
CdC10H(aq)(6.07)
Ca2*(2.19)
Ca2t(2.0)
Cr(OH)4-(4.03)
Cr(OH)4'(3.99)
-------
TABLE 15 (continued)
ro
Predominant Solid Species Predominant Soluble Sf
Constituent
Cu
Fe
Pb
Mg
Mil
"9
Ionic
Strength
0.05
0.8
0.05
0.8
0.05
0.8
0.05
0.8
0.05
0.8
0.05
0.8
pH - 5
Cu2C03(OH)2(s)
Cu2C03(OI()2(s)
Fe(OH)3(s)
Fe(OH)3(s)
PbMo04(s)
PbMo04(s)
— t
— t
— t
— t
Hg°(l)
Hg°(l)
pH * 7
Cu2C03(OH)2(s)
Cu2C03(OI1)2(s)
Fe(OH)3(s)
Fe(OH)3(s)
PbHo04(s)
PbMo04(s)
--t
— t
1
— t
Hg°(l)
Hg°(l)
pll = 9
Cu2C03(OH)2(s)
Cu2C03(OH)2(s)
Fe(OH)3(s)
Fe(OH)3(s)
PbMo04(s)
PbMo04(s),
PbC03(s)
Hg(OH)2(s)
Mg(OH)2(s)
HnC03(s)
Mn(OH)?(s),
MnC03(s)
Hg°(l)
Hg°(l)
pH = 5
CuB(OH)/(15.38)
(16.78)*
CuB(OH)/(14.99)
(16.09)
Fe(OH)2*(7.16)
FeS03+(6.98)
Pb2+(5.80)
PbCl+(5.67)
Mg2+(3.91)
Mg2+(0.95)
Mn2+(3.49)
Mn2+(3.56)
HgCl2(aq)(22.1)
HgCU-(19.9)
pH » 7
Cu(B(Olt).)7(aq)
(16.9) * '
Cu(B(OH).)7(aq)
(16.4) * *
Fe(OH)2+(9.16)
Fe(OH)2+(9.12)
PbB(OH)/(5.82)
PbB(OH)4*(5.44)
Mg2+(3.92)
Mg2+(0.95)
Mn2*(3.49)
Mn2*(3.56)
HflCl2(aq)(20.4)
HgCl3-(18.2)
)ec1es
pH = 9
Cu(B(OH)4)2(aq)
Cu(B(OH)4)2(aq)
Fe(OH)4-(10.07)
Fe(OII)4-(8.96)
Pb(B(OH)4)3-(7.14)
Pb(B(OH)4)3-(5.55)
Mg2t(4.16)
Mg2*(1.13)
MnS04(aq)(4.10)
Mn2+(4.33)
Hg(OH)2(aq)(17.9)
HgC10H(aq)(17.0)
-------
TABLE 15 (continued)
ro
•~-j
o
Ionic
Constituent Strength
K 0.05
o.a
Se 0.05
0.8
Na 0.05
0.8
Zn 0.05
0.8
Predominant
pH = 5
— t
— t
Se°
-------
Evaluation of the model in relation to analytical data, was
performed by comparing the known soluble concentrations of con-
stituents in aged FGD wastes to those predicted by the model.
As summarized in Table 16, the calculated results for aluminum,
arsenic, boron, cadmium, cobalt, copper, iron, manganese, mercury,
potassium, selenium, sodium, and zinc, either approach or are
very close to the concentration levels experienced in the field.
For other elements (specifically calcium, chromium, fluoride,
lead, and magnesium), the model was not as effective. The low
levels of calcium predicted by the model are due primarily to
the interaction of calcite with the Ca-C03 and Ca-S03
complexes in the model. The high levels of chromium and lead
calculated by the model are due to the inclusion of hydroxide
and carbonate complexes in the model. For fluoride and magnesium,
the discrepancy may be caused by certain unsuitable solids in-
cluded in the model. The discrepancies also may be due to (1)
errors in the stability constants and activity coefficients;
(2) the effects of other mechanisms, such as adsorption by hydrox-
ide solids or clay minerals; and (3) the effects of kinetic con-
straints.
An evaluation of the thermodynamic model was also performed
according to scientific considerations. In general, the model
results behave in accordance with basic chemical and thermody-
namic principles, including the effects of changing pH, Eh, and
ligand levels.
EFFECTS OF FGD SYSTEM AND SLUDGE VARIABLES ON CHEMICAL SPECIATION
For the purpose of selecting a sludge treatment or disposal
procedure, it is useful to observe the possible beneficial or
adverse effects of operational or chemical changes in an FGD sys-
tem on sludge speciation. The chemical changes studied here
include those of pH, ionic strength, chloride concentration,
borate concentration, sulfate concentration, and sulfite oxida-
tion. Table 17 summarizes the qualitative results. The opera-
tional changes studied were limited to the addition of lime,
silicates, hydrogen sulfide, phosphates, and magnesium to the
FGD system. The results are summarized in Table 18.
A change in pH can influence the direction of the alteration
processes (dissolution, precipitation, adsorption, or complexa-
tion), in any chemical system. In general, a pH increase in the
FGD sludge system tends to dissolve more elemental constituents,
such as As°(s), Hg°(£), and Se°(s), and to transform some of the
carbonate, phosphate, or other solids into hydroxide solids, thus
affecting the concentration of soluble constituents. A pH change
may also affect the ligand concentrations, and thereby change the
concentration of soluble constituents.
271
-------
TABLE 16. VALIDITY OF THE THERMODYNAMIC MODEL FOR THE
PREDICTION OF FGD SLUDGE SPECIATION
Constituent
Al
As
B
Cd
Ca
Cr
Co
Cu
F
Fe
Pb
Mg
Mn
Hg
K
Se
Na
Zn
Validity of
Model Reason for Discrepancy
Excellent
Good
Excellent
Excellent
Not applicable Form strong CaCOgfs) when pH >7
Not applicable Form strong Cr-OH complexes
Good
Excellent
Not applicable Solubility-controlling solid unknown
Good
Not applicable Form strong Pb-C03 and Pb-OH
compl exes
Not applicable Solubility-controlling solid unknown
Excellent
Excellent
Good
Good
Good
Excellent
* Based on comparison of modeling results with Kansas City Power and Light
FGD sludge analysis.
t "Excellent" means that the migration trends of the constituent follow those
predicted by the model, and measured levels in the aged leachate are within
30 percent of those estimated by the model; "Good" means that both estimated
and calculated levels of constituents show the same migration trends when
FGD waste ages.
272
-------
TABLE 17. EFFECTS OF CHEMICAL CHANGES ON THE SPECIATION OF
CONSTITUENTS IN FGD SLUDGE
Constituent
Al
ro
>-j
CO
As
Cd
Solid: High pH levels
favor the formation of
A1203'3H20(S), low pH
levels favor the for-
mation of A1(II,PO.)
(OH)2(s) f *
Soluble: When pH Is
higher than about 6,
the predominant
species will change
from A1F2 to A1J -OH"
complexes
High pH levels tend to
dissolve As°(s) and
form arsenate species
Solid: When pH Is
higher than 10.5,
CdC03(s) may grad-
ually transform to
Cd(OH)2(s)
Soluble: High pH
level can lower the
total Cd level
Ionic Strength
Negligible (when re-
lated llgand concen-
trations are unchanged)
Chloride
Concentration
Negligible
Borate
Concentration
Negligible
Negligible
The relative distri-
bution of Cdz+ and
Cd-Cl complexes can
be altered by Ionic
strength changes
Negligible
Negligible
Sulfate
Concentration
Negligible
Negligible
Can greatly affect Negligible Cd-SO. complex
the total soluble
Cd levels when chlo-
ride Is higher than
certain levels
may become predom-
inant when Cl",
SO
or OH"
complexes are not
significant
Sul f 1 te
Oxidation
Negligible
Negligible
Negligible, if the
redox potential Is
not controlled by
sul fate/sul flte species
Will reduce Cd(S03)o2"
and Increase CdSO^ faq)
levels. However,
effects on total solu-
ble Cd and Cd solids
are negligible
-------
TABLE 17 (continued)
Cons t1 tuent pll
Ca Solid: CaC03(s) may
Ionic Strength
Negligible
Chloride
Concentration
Negligible
Borate
Concentration
Negligible
Sul fate
Concentration
When pH >5, and the
Sul flte
Oxidation
Will convert the sul-
ro
greatly Increase In the
sludge when pH >7
Soluble: When pll >7,
the total Ca and Ca^
are reduced signifi-
cantly
Cr Solid: Cr(OH)3(s) is Negligible
significant when pll
ranges from 6 to 9
Soluble: When pll 1s
higher than about 4,
the predominant species
will change from Cr^
to Cr-OH complexes
Cu Solid: Negligible Negligible
Soluble: When pll
>4.8, the predominant
species will change
from Ctr to Cu-
BfOII)^ complexes
Fe Solid: Negligible Negligible
Soluble: High pll
levels (pH >8.5) tend
to Increase Fe-OH"
complexes, but reduce
the total Fe levels
Negligible
When pH <4.7.
Cu-Cl com-
plexes may become
predominant when
the chloride
level Is higher
than 2,000 ppm
Negligible
Negligible
sulfate level Is
higher than about
5,000 ppm. the CaS04
(aq) species may
become predominant
Negligible
fite solid into sul fate
or carbonate solids.
However, will have very
little effect on
soluble Ca
Negligible
When the bor-
ate level in-
creases from
5 ppm to 200
ppm, the solu-
ble lead level
can be Increased
about 2.000
Negligible
Negligible
Negligible
Negligible
Will transform FeS03*
to Fe(SO)2", but the
solid phase will remain
unchanged
-------
TABLE 17 (continued)
Constituent pll Ionic Strength
Pb Solid: When pit <9, Negligible
PbMo04(s) is predomi-
nant; otherwise, PbC03(s)
is predominant
Soluble: At high pH
levels, Pb-CO, may
Increase the total Pb
levels
Chloride
Concentration
When ptl >7, Pb-
Cl complexes may
become predominant
when the chloride
level is higher
than 1,500 ppm
Borate Sulfate
Concentration Concentration
When the bor- Negligible
ate level In-
creases from
5 ppm to 200
ppm, the solu-
ble lead level
can be Increased
about 10,000
times
Sulfite
Oxidation
Negligible
ro
-•j
01
Mg Solid: High pH levels Negligible
(pH >9) favor the for-
mation of Mg(OH)2(s)
Soluble: When pH Is
increased, the MgSO
-------
TABLE 17 (continued)
Chloride Borate Sulfate Sulfite
Constituent pH Ionic Strength Concentration Concentration Concentration Oxidation
llg Low pll levels favor the Negligible When the chloride Negligible Negligible
If the redox poten-
IV)
^4
CT>
Se
Na
formation of Hg°(l) In
the sludge. High pH
levels tend to Increase
the soluble levels of
HgCl,, HgCl3-,
Hg(OH)2(aq), and
HgClOHtaq)
Slightly reduces the K* Negligible
levels when pll Is
Increased
High pll levels tend to Negligible
dissolve Se°(s) and
form selenate species
Will slightly reduce Negligible
the Na levels when
pll Increases
level varies from
50 to 6,000 ppm, the
total soluble Hg can
be Increased for
more than four orders
of magnitude
Negligible
Negligible
Negligible
Negligible
Negligible
Negligible
Can affect the
KoS04(aq) level.
Will not, however,
affect the total
soluble level of K
Negligible
Can affect the
Na~S04(aq) level.
Will not, however,
affect the total
soluble level of Na
ttal Is controlled
by sulfate/sulflte
species, sulflte oxi-
dation can Increase
the soluble Mg level
Will Increase the
K2S04(aq) level
and reduce the K*
level. But will not
have a significant
effect on total
soluble K
If the redox potential
Is controlled by sul-
fate/sulflte species,
sulflte oxidation can
increase the soluble
Se level
Will Increase the
NapS04(aq) level and
reduce the Na level.
But will not have a
significant effect on
total soluble Na
-------
TABLE 17 (continued)
Constituent pll
Zn Solid: High pH levels
Ionic Strength
Negligible
Chloride
Concentration
When pH <9, the
Cor ate
Concentration
Negligible
Sulfate
Concentration
ZnSO.(aq) may
Sulflte
Oxidation
Negligible
favor the formation of
Zn(OH)2(s). When pll
decreases, ZnS10->(s)
will replace Zn(OH)2(s)
Soluble: Will reduce
total levels when pH
Increases
total soluble Zn
exists predomi-
nantly as ZnCl* if
the chloride level
Ishlgher than
3.000 ppni
become predominant
at a pH around 9
when Cl- and Oil'
complexes are not
significant
ro
-------
TABLE 18. EFFECTS OF ADDITION OF CHEMICAL COMPOUNDS ON THE
SPECIATION OF FGD SLUDGE CONSTITUENTS
Addition of
Constituent Lime
A1 Effect on total soluble
Addition of
Silicates
The soluble Al level can
Addition of
Hydrogen Sulflde
Negligible
Addition of
Phosphates
Effect on total soluble
Addition of
Magnesium
Will not affect the total
ro
>~j
oo
Al Is negligible
As Lime addition can cause
more Ba3(AsS04)2(s) to
form, so reduce the
total soluble As
slightly
Cd When the lime dosage is
higher than 1,500 ppm,
soluble Cd can be
Increased from 0.01 ppb
to 1.45 ppb
Ca When the dosage of lime
is from 100 to 10,000
ppm, the total soluble
Ca will Increase from
200 ppm to 400 ppm
Cr Lime addition tends to
Increase the total
soluble Cr due to
hydroxide complexes
formation
be greatly reduced when
silicate addition Is
higher than 280 ppm as
Si
Negligible
Negligible
Negligible
Negligible
Negligible
Cd can be reduced to
trace levels when sul-
flde addition is higher
than 0.2 ppm
Negligible
Negligible
Al Is negligible
Negligible
When phosphate addition
Is higher than 310 ppm
(as P), the soluble Cd
can be Increased about
2 times
If phosphate addition is
higher than 310 ppm
(as P), soluble Ca can
be reduced slightly
Negligible
soluble Al
Will not affect the total
soluble As
Will not affect the total
soluble Cd
Magnesium addition may
decrease the Ca-S04
and Ca-F complexes, but
will not change the total
soluble Ca
May affect the total solu-
ble Cr through the CrF*+
reduction
-------
TABLE 18 (continued)
ro
Addition of Addition of
Constituent Lime Silicates
Cu Lime addition tends to Negligible
Increase soluble Cu, but
will not raise the
soluble Cu above the
detectable level
Fe When the lime dosage Is Negligible
higher than 1,500 ppm,
the soluble Fe level will
be Increased from 0.012
ppb to 22 ppb
Pb Lime addition tends to Negligible
Increase the total sol-
uble Pb due to carbon-
ate complex formation
Mg Lime addition will only Negligible'
affect the total soluble
Mg slightly but will
significantly transform
Mg-COj complexes
Mn Lime addition tends to Negligible
reduce the soluble Mn
to the 20-36 ppb range
Mg Lime addition tends to Negligible
Increase the total sol-
uble Kg slightly due
to an Increase In pll
Addition of
Hydrogen Sulf1de
Cu can be reduced to
trace levels by adding
as little as 0.001 ppm
of sulflde
Negligible
Pb can be reduced to
trace levels by adding
as little as 0.001 ppm
of sulflde
Negligible
Addition of
Phosphates
Negligible
llg can be reduced to
trace levels by adding
as little as 0.001 ppm
of sulfide
Negligible
Negligible
Negligible
Soluble Mg will be
reduced about 2.5
times as the phos-
phate level Is
Increased from 0.3
to 3,100 ppm (as P)
Negligible
Negligible
Addition of
Magnesium
Will not affect the total
soluble Cu
Will not affect the total
soluble Fe
Will not affect the total
soluble Pb
Mill cause the increase of
soluble Mg
Will not affect the total
soluble Mn
Will not affect the total
soluble llg
-------
TABLE 18 (continued)
Constituent
Addition of
Lime
Addition of
Silicates
ro
oo
o
Se
Na
Zn
Negligible
Lime addition will In-
crease the total soluble
Se due to an increase
In pH
Negligible
Lime addition may
Increase the total
soluble Zn to ppm
1 evel s
Negligible
Negligible
Negligible
The soluble Zn level
Is reduced when sili-
cate addition exceeds
280 ppm as SI
Addition of
Hydrogen Sulfide
Addition of
Phosphates
Negligible
Negligible
Negligible
Zn will be reduced to
trace levels when sul-
fide addition is higher
than 0.5 ppm
Negligible
Negligible
Negligible
Neglfglble
Addition of
Magnesium
Magnesium addition may
decrease the KoS04(aq)
level, but will not affect
the total soluble K
Will not affect the total
soluble Se
Magnesium addition may
decrease the Na2SO.(aq)
level, but will not affect
the total soluble Na
Will not affect the total
soluble Zn
-------
The overall effects of pH on the total constituent concen-
tration depend on the solubility constants of the new solids
formed, the new ligand concentrations, and the formation con-
stants of the complexes. For example, a high pH level can in-
crease total soluble mercury and selenium, and yet decrease most
of the other bivalent trace metals. For trivalent metals such
as chromium and iron, the minimum soluble constituent concen-
trations occur in the neutral pH region.
Although a change in ionic strength in the FGD sludge can
affect the stability constants, its effect on the soluble levels
of constituents, or on the stability fields of various solids,
are usually negligible if their related ligand levels are un-
changed. The soluble chloride concentration of the FGD waste is
a very important factor in determining the total soluble level
of cadmium, copper, lead, mercury, and zinc. Variations in borate
concentration have an impact primarily on total soluble copper
and lead concentrations. The soluble sulfate concentration may
affect the total soluble calcium, magnesium, cadmium, and zinc
concentrations. In general, if the total soluble levels of the
above-mentioned ligands (e.g., chloride, borate, and sulfate)
are known, the total soluble metal concentrations in the aged FGD
leachates can be approximated without extensive computation.
With regard to operational changes, sulfite oxidation may
reduce the concentration of sulfite complexes and increase the
concentration of sulfate complexes, but will have very little
impact on the total soluble concentration of most metals. The
most significant effect of sulfite oxidation is the transforma-
tion of CaSOs-l/2H20(s ) to CaS04 .2H2d(s) or CaC03(s), depending on
pH levels. This transformation may affect the soluble levels of
arsenic, mercury, and selenium if the redox potential is con-
trolled by sulfate/sulfite species.
The addition of lime to the FGD sludge has been employed in
pozzolanic fixation processes for the purpose of improving the
engineering properties of the dewatered sludge. However, the
model shows that lime addition may have an adverse effect on
constituent solubility. The addition of lime to FGD wastes may
reduce the total soluble levels of certain constituents such as
arsenic and manganese. However,the total soluble levels of most
other trace toxic metals, such as cadmium, chromium, copper,
lead, mercury, selenium, and zinc, increase in aged FGD sludge
following lime addition. This may actually increase the poten-
tial for environmental damage, should the concentration increase
outweight the dilution factor decrease which results from per-
meability reduction.
The addition of silicates may reduce the total soluble alumi-
num and zjnc concentrations, but other elements studied are vir-
tual 1y unaffected.
281
-------
Phosphate addition will only reduce two soluble major ions
(calcium and magnesium) while increasing the soluble cadmium
level. Phosphate itself is also a water pollutant, so the addi-
tion of phosphates is not recommended for the treatment of FGD
wastewater.
Hydrogen sulfide addition may reduce the soluble concentra-
tions of trace metals substantially, as shown in Table 18. This
operational change, however, may not be desirable for an FGD
system for two reasons: (1) hydrogen sulfide itself is a pollu-
tant, and (2) the diffusion of oxygen into the sludge, followed
by the oxidation process, will eventually return the soluble
metals to their original concentration.
Magnesium has been shown to improve the efficiency of wet
FGD systems; the use of high magnesium reagents could therefore
become commonplace. The model shows that, in general, the mag-
nesium addition will not significantly affect the total soluble
levels of most constituents.
282
-------
SECTION 9
CONCLUSIONS AND RECOMMENDATIONS
1. Thermodynamic modeling of chemical speciation in FGD
sludge has shown that sludge constituents can exist in a wide
variety of chemical forms or species. The predominance and con-
centration of any particular chemical species are influenced by
chemical factors such as pH, Eh, ionic strength, and total con-
centrations of ligands and metals in the system. Although the
FGO chemical systems are extremely complex, .the speciation of
their elemental constituents can be quantified by calculation
with reasonable accuracy.
2. The thermodynamic approach indicates that, in most FGD
systems (ionic strength (I) of 0.05 to 0.8, and pH of 3 to 11),
the major solid species for metals are usually sulfates, sulfites,
carbonates, and hydroxides. Silicate, phosphate, elemental
metal, and molybdate solids may also become the predominant
solid species under certain conditions. Based on the pH, Eh,
and various related ligand conditions, the predominant solid
species of most elemental constituents in the FGD system can be
derived. The solids which will predominate for the sludge con-
stituents of concern are as follows:
Aluminum - Al 203 • 3H20 ( s ), AlPO^s) and Al ( H2P04 ) ( OH )2 ( s )
Antimony - Sb(OH)3d2 (s)
Arsenic - As°(s)
Cadmium - CdCOaU) and Cd(OH)2(s)
Calcium - CaS04 • 2H20(s), CaSOs • 1/2H20(s ) , and CaCOsls)
Chromium - Cr(OH)3(s)
Copper - Cu2C03(OHJ2(s) and Cu(OH)2(s)
Iron - Fe(OH)3(s) and FeC03(s)
Lead - PbC03(s), Pb(OH)2(s), Pb3 (OH ) 2(COs ) (s ) , and PbMo04'(s)
Mercury - Hg°(£)
Manganese - MnOOH(s), MnC03(s), Mn(OH)2(s), Mn304(s) and Mn02(s)
Nickel - NiCO^(s) and Ni(OH)2(s)
Selenium -Se°(s)
Zinc - ZnSi03(s), ZnC03(s), and Zn(OH)2(s)
3. The results of thermodynamics calculations also show that
the relative distribution of various soluble species in fresh and
aged FGD sludges are quite similar. Stated another way, although
the aging process may reduce or increase the total soluble
283
-------
concentration of constituents, the primary soluble species
(specieswhich predominate, or whose concentration may become
significant in the leachate) is common to both conditions. For
each constituent, only a few species may become predominant for
a given FGD condition. These soluh.le. species are as follows:
Calcium - Ca ; Ca-S04 complexes
Magnesium - Mg2*; Mg-SO^ complexes
Potassi urn - + K
Sodium-Na2+
Cadmium - Cd ; Cd-Cl complexes; Cd-CO., complexes;
Cd-S03 complexes; Cd-S04 complexes
Chromium - Cr3 + ; Cr-OH complexes
Copper - Cu'+; Cu-B(OH)4 complexes; Cu-Cl complexes
Iron - Fe-OH complexes; Fe-S03 complexes
Mercury -2Hg-Cl complexes; Hg-OH complexes
Lead - Pb ; Pb-B(OH)4 complexes; Pb-Cl complexes;
Pb-C03 complexes
Zinc - Zn2 + ; Zn-Cl complexes; Zn-OH complexes
4. Knowledge of the relative distribution of constituent
species "in the FGD system is useful for (1) the evaluation of
general toxicity, and (2) predicting the migration of the con-
stituent in the environment. Although it was impossible to
consider all the possible FGD conditions in this study, the cal-
culated results for the boundary conditions (ionic strength of
0.05 and 0.8) do provide a range of the possible species concen-
trations. Most FGD sludges are expected to fall within these
boundary conditions. The boundary results can be viewed in
Figures 1 through 81, in the main text of this report.
After the primary solid and the soluble species are identi-
fied by the methods of this study, the total soluble constituent
concentrations in the aged sludge can be calculated without the
aid of a computer, The concentrations of free ions can be
approximated by solving the mass equation(s) of primary solid(s)
solubilities. The concentrations of soluble primary species can
then be solved by the mass equations which, including the free
soluble ions and the complex formation constraints, are described
in Section 2. The summation of the primary soluble species for
each constituent, will provide its estimated total level in the
sludge liquid phase. Equations 73 through 83 are examples of
this type of calculation.
5. When assessing the potential impacts of FGD sludge
leachate on groundwater, examination of data from aged FGD
wastes is most appropriate. Most in situ FGD sludges have a low
permeability (10-4 to 10-10 cm/sec) (Ref. 1, 46) which provides
months to years of contact time between leachate and sludge.
During this period, various chemical species in the FGD sludge
(either fn the solid or soluble phases) would gradually approach
equilibrium. Unfortunately, there is a lack of documented
284
-------
information relating to the chemical species present in aged
FGD waste, due to the similar lack of long-term FGD operations.
Therefore, the thermodynamic model can be useful for predicting
both the concentrations of various species, and the total solu-
ble concentrations of constituents in aged FGD sludge. The
background required for the calculation need include no more than
the total levels of the constituents in the fresh FGD waste. This
thermodynamic approach could provide a considerable cost saving
over the traditional field survey.
6. The thermodynamic model discussed here can also be used
to predict solid or soluble species changes, and changes in the
levels of total soluble constituents caused by operational or
chemical factors. Examples of these sensitivity calculations
are presented in Section 7, and are summarized in Section 8.
The soluble constituent concentrations at the boundary conditions
(ionic strength of 0.05 and 0.8) are displayed in Figures 157
through 167. The shaded areas indicate the ranges of possible
total constituent concentrations in the aged FGD wastes. These
values may be used for rough estimation of the total soluble
constituents in various aged FGD leachates. Only those elements
for which the model projections agree with the analytical results,
are shown.
7. The thermodynamic model employed in this study was found
to be inaccurate when predicting the speciation of calcium,
chromium, fluoride, lead, and magnesium. The disparity may have
been caused by several factors, including adsorption fay various
solids or the kinetic constraints of the reactions. The specia-
tion of other constituents, such as aluminum, arsenic, cadmium,
boron, cobalt, copper, iron, manganese, mercury, potassium,
selenium, sodium, and zinc, showed very close correlation with
the analytical results. More study is therefore suggested to
(1) verify the model against different types of FGD wastes, or
(2) include more of the controlling factors in the model.
285
-------
300
250
.a
O.
a.
200
.a
3
^ '1501
100
11
Figure 157.
Range of aluminum concentrations in aged FGD
sludge leachates by thermodynamic model calcu-
lation.
286
-------
12,000,
_ 10,000
.a
CL
CL.
8,000
-------
1200
11
Figure 159.
Range of cadmium
sludge leachates
1 a t i o n .
concentrations in aged FGD
by thermodynamic model calcu-
288
-------
E
Q.
O.
CO
-------
£
Q.
a.
o
o
a>
3
O
to
o
Figure 161.
Range of cobalt concentrations in aged FGD
sludge leachates by thermodynamic model calcu-
lation.
290
-------
10
10-12
11
Figure 162.
Range of copper concentrations in aged FGD
sludge leachates by thermodynamic model calcu-
lation.
291
-------
J3
Q.
a.
-------
E
O.
Q.
C
s
O)
O
C/1
-------
60
50-
£
n.
CL
O)
.Q
40
30
2.0
10
I = 0.8
I = 0.05
11
PH
Figure 165.
Range of potassium concentrations
sludge leachates by therraodynamic
1 at ion.
in aged FGD
model cal cu^
294
-------
3000
2500-
2000^
OJ
15006
ITS
-M
O
.10006
500
11
Figure 166.
Range of sodium concentrations in aged FGD
sludge leachates by thermodynamic model calcu
1 a t i o n .
295
-------
24000
20000-
O.
Q.
£=
M
-------
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Prentice-Hall, Englewood Cliffs, New Jersey, 1964.
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Micronutrients in Agriculture, ed. by J.J. Mortvedt,
P .M ^. Giordano, and W.L. Lindsay. Soil Sci . Soc. Amer.,
Inc., Madison, Wisconsin, 1972. pp. 7-40.
299
-------
35. Weber, W.J., Jr. and H.S. Posselt. Equilibrium Models and
Precipitation Reactions for Cadmium (II).. In: Aqueous-
Environmental Chemistry of Metals, ed. by A.J. Rubin, Ann
Arbor Sci. Pub., Ann Arbor, Michigan, 1974.
36. Radian Corporation. The Environmental Effects of Trace
Elements in the Pond Disposal of Ash and Flue Gas Desul-
furization Sludge. Prepared for -Electric Power Research
Institute, Research Project 202, Palo Alto, California, 1975
37. Mandel, L.N. Transformation of Iron and Manganese in Water-
Logged Soils. Soil Science, 91(2 ) : 121-126 , 1961.
38. Ponnamperuma, F.N., T.A. Loy, and E.M. Tianco. Redox
Equilibrian in Flooded Soils r II. The Manganese Oxide
Systems. Soil Science, 1 08( 1 ) -.48-57, 1969.
39. Bricker, 0. Some Stability Relations in the System
Mn-02-H20 at 25°C and One Atmosphere Total Pressure.
Amer. Mineral. 50:1296-1354, 1965.
40. Florence, T.M. and G.E. Batley. Determination of the
Chemical Forms of Trace Metals in Natural Waters, with
Special Reference to Copper, Lead, Cadmium and Zinc.
Talanta, 24:151-158, 1977.
41. Smith, R.G., Jr. Evaluation of Combined Applications of
Ul trafi 1 tration and Complexation Capacity Techniques to
Natural Waters. Anal. Chem. 48:74-76, 1976.
42. Florence, T.M. and G.E. Batley. Trace Metals Species in
Seawater - I. Removal of Trace Metals from Seawater by
a Chelating Resin. Talanta, 23:179-186, 1976.
43. Chan, Y.K. and K.L. Chan. Determination of Labile and
Strongly Bound Metals in Lake Water. Water Res., 8:383-388,
1974.
44. Karger, B.L., L.R. Snyder, and C. Horvath. An Introduction
to Separation Science. Wiley, New- York, 1973.
45. Batley, G.E. and T.M. Florence. Determination of the
Chemical Forms of Dissolved Cadmium, Lead and Copper in
Seawater. Marine Chem., 4:347-363, 1976.
46. Radian Corporation. Evaluation of the Physical Stability
and Leachability of Flue Gas Cleaning Wastes. Electric
Power Research Institute, November 1977.
300
-------
APPENDIX A. STABILITY CONSTANTS OF SOLUBLE METAL SPECIES
OJ
o
Species Ligand
A13+ S04=
F"
OH"
Ba24" OH
Be21" S042"
Cl~
F"
OH"
Cd2+ C032"
so42~
Cl"
F"
Br"
I"
po43-
N03-
OH"
OH"
fa2+ rn
l» a LU o
so42"
F"
on 3-
Log p^
3.2
6.9
9.5
1.2
1.9
1.6
5.6
7.7
5.4
2.3
2.2
1.1
2.1
2.4
3.9
0.7
4
3.0
2.3
1.1
Log
4
13
18
3
9
2
1
2
3
7
11
p9 Log Pi Log ft, Log p^ Log pfi Log K
.8
.0 16.9 19.5 20.8 20.5
.5 27.0
.0 2.0
.7 12.7
-
tCdOM**)
! tCdr*]tCl"3[H*]
-, n 1 ' 1 r [CdClOHl.qU
*/ ^ • J. J. * D ~~ 9+ • IT
.5 2.2
.9 3.2 3.7
.5 5.2 6. 1
CCdjOM3*)
.6 8.7 8.5 [cdz*)zto»n
4 4
[Cd } [OH* I
, ft [C»COjH
(c«lP04)H(>al)
K
12. 2
-6.7
54.6
23.1
11.6
1/1 £
-------
APPENDIX A (continued)
o
ro
Species Li
Co2+ CO
SO
Cl
Br
PO
OH
Cu2+ CO
SO
n
U 1
F"
Br
I"
PO
PO
B(
OH
Cr3+ SO
Cl
F~
Br
PO
OH
gand
3
4
™"
-
4
—
0
J
4
-
-
4
4
2-
2-
3-
2-
2-
3-
3-
OH)4~
4
"•
-
4
~
2-
3-
Log
5.
2.
1.
0.
4.
6.
2.
i
A .
1.
1.
9.
7.
6.
2.
0.
4.
-1.
-10.
Pi
4
5
4
6
8
7
3
f.
\J
3
1
7
1
1
7
8
5
9
7
Log
1
9
9
2
C.
-0
9
12
i f\
10
1
9
19
P9 Log (3., Log (3A Log (3^ Log pfi Log K
UoCO,H*J
9
[C.^JtCo'-UH*]
lCDro4HU«))
(Co!*HPoJ"KH*l
.7
.7 10.8
CCuCOjH ]
. 9 ![CuZ*]tCOj-]tH*l
' (CuCOjIOH)'2)
tC^^JICflj^HOH-]2
0 1 0 1 A (CuClOM(.q)!
tCu JlCl JlOH J
.3 -1.8 -4.0
.5
{CuCO.NItl)))
tt«z*][ro43-KH*J
ItuPO^Hj'1]
ttMZ*]tMj*][M']*
.4
7-irrt 1£"1
15.2 16.1 [CU!*]ZCOH-JZ
.9
.1 11.3
[CrFOtH*]
[tr4*J[l>oJ-}tH*)
.2 18.2
K
12.3
15.0
12.5
-13.0
-4 9
~ • -*
16.0
21.3
n-i
. 7
21.5
-------
APPENDIX A (continued)
Species Ligand Log pt Log ^ Log {3q Log p
H+ C032-
so42-
F"
s2-
P043~
P0«
" -
P04
sio2(OH)22-
o B(OH)4-
CO o
so32-
Mo042"
As043"
HVOd2"
2
SeOo
1+ 9
Fe3+ S04^
CT
F~
Br~
I
po43-
^in-/nu\.2-
10.2
2.2
3.0
14.0
12.5
13.1
9.1
7.3
4.3
11.8
8.2
8.5
4.1 5.6
1.4 2.1 1.3
5.6 10.2 12.9
0.7 0.5
3.5 2.4
4 Log P5 Log pg Log K K
[Hzco3i.,n
[M*)2!^-) 16.5
(HgMxin
H.4!1?*-*! 21.2
, [«,»»,-)
:tM*]lc»oJ-i 19.9
{[H.ro.ito)]
T * O 1 O
fH 1 fPO 1
1 fH2slo?10H1?i oo 7
[H AtO "3
tH^tMOp 18.8
[H itO,l.q))
« J
CM )'[s«0j ] 1 1 . t
ffeP04M*)
[FeS*UfoJ*]tH'*] 20 . 7
2 ? 1 0 C
-------
APPENDIX A (continued)
Species
Fe2 +
Pb2 +
Mg2 +
Li gand
B(OH)4-
OH~
so42~
CT
P043~
OH"
co32~
co32=
so42-
Cl~
Br~
I-
B(OH)4~
OH"
All""
OH
OH~
co32-
so42-
F~
P043"
OH"
Log (3j
8.9
11.8
2.3
0.9
21.6
5.4
7.4
2.7
1.7
1.9
1.8
5.2
6.3
-7.7
3.2
2.4
1.8
Log p2 Log p3 Log p4 Log P5 Log p6 Log K
15.8
21.8 28.8 tF.VtoH-]2
23.9
24.8
(PbCO.H ]
3
10.8 [pbz*uco*-UM']
CFbtCOjIjHjItq)]
[Pbz*)iCcoi']ztM*3
CPbC10H(iaH
t.u C.O t.U tPb KC) HOH")
3.2 3.8 3.9
3.6 4.2 4.4
11.1
10.9 13.0 tPbX'J
-17.1 -28.1 CPb**]*{OH']
CPbjIOMlJ*]
CPb*^]JCflM"]4
CPbjIOHlJ*)
CM9'CO~H*]
fMa^^K COz"lfH*3
CN9iP04)H(tq|]
CM.'*][P044-KH*]
[HgOH']
CMjZ*)tOH']
K
25.1
13.2
25.4
-6.6
7.7
O f\ 1
30. 1
68.4
11.6
15.1
3.8
-------
APPENDIX A (continued)
Species Ligand
O i f\
Mn^+ C03^
so42"
Cl"
Br"
po43-
OH~
O _L O
Hg C^3
so42~
O i
£ Hgz+ Cl~
F-
Br"
I"
S2-
OH~
OH"
O 4- O
Ni2+ C032-
so42-
CT
F~
Br"
po43-
OH"
Log Pj Log P2 Log p3 Log p4 Log p5 Log pg Log K
(HnCO.H*!
J
tHr.Z*]tCof"HH*]
2.3
1.1 1.1 0.6
0.9 0.8
[Mol>04N(<4>}
tHn'*KP04J-HH*]
3.9 9.8
IMjCOjH*]
2.4 3.5
(HgClOHliqH
7f\ -\ \ c\ 1 i~ 1 1 r fl .
.2 14.0 15.1 15.4 tHdz*Kcri[M*)
1.6
9.6 18.1 20.5 24.0
13.4 24.6 28.4 30.3
IHsSjHjUql)
54 . 2 tH,z*]£iz-)
-------
APPENDIX A (continued)
CO
o
en
Species
K +
Ag+
Na +
Sn2 +
Zn2+
L1 gand
F~
so42"
CT
F~
Br~
I"
s2-
so32-
OH~
so4-
F~
Br~
OH"
so4-
H
ci -
F~
Br~
OH~
Log Pj
1.1
1.1
3.1
0.4
4.3
14.0
5.6
2.0
0.7
6.9
1.1
10.8
2.3
1.4
1.3
0.9
4.5
Log p2 Log P3 Log p,, Log P5
4.9 4.9 5.1
7.3 8.0 8.7
13.9
17.3
7.9
4.0
9.7 10.2
1.7 1.4
1.7 0.8 1.2
0.9 0.3 0
11.1 13.6 14.8
Log P6 Log K K
: [AgSHI.nl]
[A,*HS-HH*] 14.0
...^Ll^ 19.0
ClnClOMtial]
tz»z*ncruoiri -7.0
; [InPO.Hllq)]
-t r~ JT.
ClOjOH3*] c
[I«^*]Z[OM-]
-------
APPENDIX B
CHEMICAL ANALYSIS OF FRESH AND
AGED FGD SLUDGE SAMPLES
In order to verify the thermodynamic model used In this
study, chemical analysis of fresh and aged FGD wastes were per-
formed. This section describes the sampling procedures and
analytical methods used.
SAMPLING PROCEDURE
Samples of FGD sludges and wastewaters were collected on
October 18-19, 1977, at the Kansas City Power and Light La Cygne
Power Station. The following is a description of the methods used
to collect, prepare, preserve, and transport the samples taken.
Sample Container Preparation
The sample containers (1- and 4-liter capacities), caps, and
filtration syringes used were made of polypropylene material.
This equipment was soaked in a solution of 5-percent nitric acid.
The containers, cap, and syringes remained in the acid solution
for 24 hours. Upon completion of the acid soak, the containers,
caps, and syringes were immediately rinsed three times each with
doubly distilled deionized water. Upon vigorous shaking off of
excess water, the caps were placed on the containers and stored.
The syringes were shaken of excess water and then wrapped in para-
film to prevent contamination.
Sample Col 1ecti on
Approximately 125 ml of sludge were drawn from the sludge
effluent lines of each of the eight scrubbers. The eight 125-ml
aliquots of sludge were then placed into a 1-liter polypropylene
bottle and allowed to settle for 4 hours. Upon settling, a 150-ml
aliquot of the supernatant was then drawn from and filtered
through a 0.45- m Millipore filter. Two 75-ml portions of the
filtrate were then placed in a separate 600-ml polypropylene
bottle. The sample container identified for metal determination
was then acidified with ultra-pure nitric acid to a pH of 1.
Both sample containers were then refrigerated at 5°C until the
next sampling addition. The final volume of each subset sample
was 600 ml .
307
-------
Fresh Wastewater--
The composite sample was taken six times during a 24-hour
period over two consecutive days. The sample consisted of two
subset samples (refer to Table 81). The subset sample identified
as 2876-KAN-RW-l was designated for metal analysis only; sample
2876-KAN-RW-2 was used for all other analyses.
Fresh Sludge--
The fresh sludge composite sample was taken at the same time
intervals and fashion as the fresh effluent. A 2.5-liter aliquot
was taken from each of the sludge effluent lines and placed in a
20-liter polypropylene container. Upon settling (4 hours), the
supernatant was discarded and approximately 500 ml of settled
sludge was transferred to a 4-liter polypropylene container. The
sludge composite sample was then refrigerated (4°C). Part of the
sludge sample was aged for 20 days' for the study of the aging
effects on the FGD sludge.
Stabilized Wastewater--
The stabilized wastewater composite was sampled from the
sludge lagoon. The samples were taken in an .area of quiescence
near the point to reentry to the power plant. Samples were
taken once daily with a 600-ml aliquot, which was filtered
(0.45 m) and split into two 300-ml subset samples. The sample
marked 2876-KAN-SW-l was then acidified with ultra-pure nitric
acid to a pH of 1. Both subset samples were refrigerated (4°C).
Stabilized Sludge--
The stabilized sludge was also taken from the sludge lagoon.
The plant engineer identified the areas of oldest deposition of
lime sludge (about 5 years old). These areas had formed sills
and were easily accessible.
A casing was needed to take samples from 180 to 270 cm below
the surface of the sill. The casing was fabricated from eight-
inch diameter PVC pipe. The original 360-cm casing was cut into
two 180 cm sections and filled with a connector.
Once the casing was in place, the sample of stabilized
sludge was augered from a depth of 180 to 270 cm and placed in a
4-liter container. The auger bucket was teflon-coated to prevent
metal contamination.
Sample Shipment
All samples described above were placed in metal ice chests.
Ample amounts of ice were included to ensure that the sample
remained at 4°C. The sample was airfreighted from Kansas City to
Los Angeles and delivered to the DSC Department of Environmental
Engineering within 10 hours.
308
-------
TABLE B-l . FGD SLUDGE SAMPLE IDENTIFICATION SCHEME
Label SampleDescription
2876-KAN-RS Fresh sludge from scrubber mixing
tank (all parameters)
2876-KAN-SS Stabilized sludge from lagoon
(all parameters)
2876-KAN-RW-l Fresh wastewater - from scrubber
mixing tank, filtered, fixed
(acidi fied)(metals )
2876-KAN-RW-2 Fresh wastewater - from scrubber
mixing tank, filtered - not
fixed (all other parameters)
2876-KAN-SW-l Stabilized wastewater - from
lagoon, filtered, fixed (metals)
2876-KAN-SW-2 Stabilized wastewater - from
lagoon, filtered, not fixed
(all other parameters)
ANALYTICAL METHODS
Below is a discussion of the analytical procedures imple-
mented in the parameter determination on the samples of wastewater
and sludge taken at the La Cygne station.
General Parameters
The determination of pH, nitrogen compounds, alkalinity,
chloride, fluoride, redox potential, and total dissolved solids
follows the standard methods described in Ref. 1. The procedures
and instruments used are as follows:
• pH Potentiometry (Orion 801A)
• NH3-N Brucine Method (Perkin-Elmer 124,
light path 10 cm, 410 nm)
• Alkalinity Potentiometric titration
(Orion 801A)
• Chloride Mercuric nitrate method
309
-------
• Redox potential Potentiometry (Pt electrode,
Orion 810A)
• Total dissolved Gravimetry
solids
• Boron Curcumin method
• Silica Molybdosi1icate
The determination of phosphorus was accomplished using the
modified Ascorbic Method. The procedures of the method are out-
1ined as follows:
(a) Measure 1 ml of slurry sample and put in teflon beaker
(if filtrate sample, use 50-100 ml).
(b) Digest the sample at water boiler temperature using
HF (1 ml) and HC104 (2 ml) with teflon cover.
(c) After solution is clear, remove the cover and heat to
dryness .
(d) Cool, add 2 ml of H?®? and heat to dryness again.
(e) Add 20 ml of H20 and 5 ml of ION H2S04.
(f) Filter the sample through the glass fiber and dilute
to 100 ml .
(g) Take 40 ml of sample and add 3 ml of 1.6 percent
ammonium molybdate and 4 ml of mixed reagent. (Mixed
reagent = 50 ml of tartrate + 50 ml of 10 percent
ascorbic acid). (If dilution is required, the reagents
to sample ratio should be kept constant. An appropriate
amount of ION H2S04 should be used to keep the final pH
value constant).
(h) Measure the sample by spectrophotometer at 717 nm.
The measurement of orthosphate on filtrates was performed as
above without the digestion procedures.
A refractometer (American Optical Corp. Goldberg T/C, Model
10419), was used for the measurement of salinity. The dry weight
data of the total slurry samples were analyzed on both volume
and wei ght basi s .
310
-------
A titrimetric method is used for dissolved sulfide deter-
mination. Total acid-soluble sulfide was determined by stripping
and titrimetric processes:
(a) Measure 5 ml ZnAc and 95 ml distilled water into each
of two absorption flasks. Connect the two absorption
flasks with a 1-liter reaction flask and purge the
system with N~ gas for 5 minutes.
(b) Transfer 10 - 50 ml slurry sample into the reaction
flask and add distilled water to 500 ml, then mix
completely.
(c) Acidify the sample with 10 ml cone. H2S04 and replace
the prepared 2-hole stopper tightly. Pass N£ through
the sample for approximately one hour.
(d) Add 10 ml of iodine solution and 2.5 ml cone. HC1 to
each of the absorption flasks, sha-ke and mix thoroughly
(e) Transfer contents of both flasks to a 500 ml flask and
back-titrate with 0.025N sodium thiosulfate titrant,
using starch solution as indicator.
The analysis of FGD sludge for carbonate sulfite and sulfate
followed the Palmrose Method as described below:
(a) Obtaining and preparing sample
(1) Using a 2-1/2 ml syringe, exactly 2 ml of sludge
sample are drawn. Care must be taken here, for if
excess sample is taken and if the excess is dis-
carded by drawing the plunger back to 2 ml, the
solids may partially settle and what remains is
no longer representative.
(2) The sample is then injected into a beaker contain-
ing 60 to 75 ml of demineralized water. The
diluted sample is redrawn into the syringe several
times to completely wash or purge the sample.
(b) CaS03 Titration
(1) Add 5 ml of starch - KI solution to the sample.
(2) Estimate the expected CaC03 concentration. Deter-
mine the volume of H2S04 needed to neutralize the
CaCOs. Add 5 ml to that volume and add the sum
to the sample and record the volume added.
(3) Titrate the sample with potassium iodate (KIOs).
Do not stir the sample until a blue color starts
311
-------
to appear. Titrate until one drop produces an
intense blue color. Premature stirring would
aggravate the S02 stripping problem. Note the
volume of KI03 used.
(c) Excess Acid Titration
(1) To bring the sample back from the deep blue to a
clear color, add a couple drops of sodium thio-
sulfate. If more than a few drops are required
to effect the color change, the KI03 end point
was exceeded and the entire process should be
started over.
(2) A few drops (3 to 5) of methyl purple indicator
are added to the sample. This will turn the solu-
tion blue.
(3) Titrate the sample to a greenish yellow end point
with 1/8 normal NaOH. Recorci the volume of
hydroxide titrated. If the ml of NaOH is less
than 5 ml or greater than 10 ml, the entire
analysis should be redone by adjusting the amount
of H2S04 added in step (b)(2).
(d) Calculations
If this procedure is followed exactly and all reagents
are of the specified normality, the composition is calculated
as follows:
gm CaC03/l = 3.125 x (ml H2S04 - ml NaOH)
gm CaS03'l/2H20 - 4.025 x ml KI03
The concentration of CaS04-2H20 was calcualted by subtract-
ing the amount of calcium in CaCOs and CaS03-^H20 from that of
total calcium concentration in sludge.
Metals
Sludge samples used in the determination of metals (except
mercury) in the lime slurry sludge, were digested by concen-
trated hydrofluoric acid (HF), nitric acid (HNOs), and perchloric
acid (HC103) to clear the solution at 175°C in a teflon beaker
(with teflon cover). Atomic absorption spectrophotometers
(Perkin Elmer's 3058 and 4-60) were used in the analyses of metals
Both flame and heated graphite atomizers (HGA 2100) were employed
in total sample analysis. The choice of an atomizer is dependent
on the suitable linear range (concentration) of the element which
is being determined. The following table was the guide used in
choosing the atomizer:
312
-------
Optimum Working Range
Fl ame
atomizer (mg/£)
0
0
0
0
0
0
0
0
10
0
0
1
0
5
2
0
.03
.1
.2
.02
.002
.05
.2
.3
.1
.3
.002
.05
1
2
- 20
2
0
2
- 10
- 10
- 300
- 10
-' 10
- 20
0
- 100
- 100
2
.02
.02
Heated graphite
atomizer (pg)*
20 -
10 -
20 -
1 -
50 -
3 -
50 -
30 -
500 -
10 -
200 -
50 -
50 -
1000 -
400 -
1 -
2000
2500
1000
40
1000
100
2000
1000
7000
500
5000
1500
1000
80000
20000
70
£1ement
Na
K
Ca
Mg
As
Cd
Cu
Fe
Hg
Mn
Ni
Pb
Se
Ti
V
Zn
*Based on interrupt flow of argon gas
The fresh and stabilized wastewater needed no further diges-
tion since the sample had been filtered (0 .4 5 y m) and fixed pH = l)
in the field. Analysis of the metals (except mercury) was
accomplished by direct injection into the HGA furnace.
Mercury determination was accomplished by flameless atomic
adsorption cold vapor method. Samples (raw and stabilize lime
slurry sludges) for total mercury analysis were digested in
teflon bombs (Parr No. 4745). The procedures are as follows:
(a) Weight triplicate 0.1 - Ig of sample and place in
bottom of a teflon acid digestion bomb.
(b) Carefully add 10 ml cone. HNOs, 3 ml 48% HF and 1 g
KMn04 and close the digestion bomb tightly.
(c) Place the digestion bomb into an oven (or hot plate)
and adjust the temperature to 70°C.
(d) Digest the sample until solution is clear.
(e) Determinations were accomplished by flameless atomic
adsorption cold vapor method.
313
-------
The pore water samples were withdrawn from various sludge
samples (fresh, 20-day-old, and stabilized) by the centrifugation
method at 5,000 g and 30 minutes of centrifugation . After centri-
fugation, the supernatants were filtered through a 0.45 m Milli-
pore filter, and were immediately acidified to pH around 1 to
preserve the sample. The procedures used for the analysis of
pore water samples are the same as those used for the analysis
of fresh and stabilized wastewaters, as described previously.
314
-------
APPENDIX B
REFERENCES
APHA, AWWA, WPCF. Standard Methods for the Examination of
Water and Wastewater, 14th ed., Washington, D.C. 1975.
315
------- |