UNDERSTANDING VARIATION IN PARTITION COEFFICIENT, Kd ...

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Landa, E. R., A. H. Le, R. L. Luck, and P. J. Yeich. 1995. “Sorption and Coprecipitation of Trace Concentrations of Thorium with Various Minerals Under Conditions Simulating an Acid Uranium Mill Effluent Environment.” Inorganica Chimica Acta, 229:247-252. Langmuir, D. 1978. “Uranium Solution-mineral Equilibria at Low Temperatures with Applications to Sedimentary Ore Deposits.” Geochimica et Cosmochimica Acta, 42:547-569. Langmuir, D., and J. S. Herman. 1980. “The Mobility of Thorium in Natural Waters at Low Temperatures.” Geochimica et Cosmochimica Acta, 44:1753-1766. Leckie, J. O., M. M. Benjamin, K. Hayes, G. Kaufman, and S. Altman. 1980. Adsorption/Coprecipitation of Trace Elements from Water With Iron Oxyhydroxides. EPRI-RP-910, Electric Power Research Institute, Palo Alto, California. Lefevre, R., M. Sardin, and D. Schweich. 1993. “Migration of Strontium in Clayey and Calcareous Sandy Soil: Precipitation and Ion Exchange.” Journal of Contaminant Hydrology, 13:215-229. Lemire, R. J., and P. R. Tremaine. 1980. “Uranium and Plutonium Equilibria in Aqueous Solutions to 200EC.” Journal of Chemical Engineering Data, 25:361-370. Levi-Minzi, R., G. F. Soldatini, and R. Riffaldi. 1976. “Cadmium Adsorption by Soils.” Journal of Soil Science, 27:10-15. Levy, R., and C. W. Francis. 1976. “Adsorption and Desorption of Cadmium by Synthetic and Natural Organo-Clay Complexes.” Geoderma, 18:193-205. Lindenmeier, C. W., R. J. Serne, J. L. Conca, A. T. Owen, and M. I. Wood. 1995. Solid Waste Leach Characteristics and Contaminant-Sediment Interactions Volume 2: Contaminant Transport Under Unsaturated Moisture Contents. PNL-10722, Pacific Northwest Laboratory, Richland, Washington. Lindsay, W. L. 1979. Chemical Equilibria in Soils. J. Wiley and Sons, New York, New York. MacNaughton, M. G. 1977. “Adsorption of Chromium(VI) at the Oxide-Water Interface.” In Biological Implications of Metals in the Environment, H. Drucker and R. F. Wildung (eds.), pp. 244-253, CONF-750929, National Technical Information Service, Springfield, Virginia. Mattigod, S. V., and A. L. Page. 1983. “Assessment of Metal Pollution in Soils.” In Applied Environmental Geochemistry, I. Thornton (ed.), pp. 355-394, Academic Press, New York, New York. 6.12
Mattigod, S. V., A. L. Page, and I. Thornton. 1986. “Identification of Some Trace Metal Minerals in a Mine-Waste Contaminated Soil.” Soil Science Society of America Journal, 50:254-258. McBride, M. B. 1980. “Chemisorption of Cd 2+ on Calcite Surfaces.” Soil Science Society of America Journal, 44:26-28. McBride, M. B., L. D. Tyler, and D. A. Hovde. 1981. “Cadmium Adsorption by Soils and Uptake by Plants as Affected by Soil Chemical Properties.” Soil Science Society of America Journal, 45:739-744. McHenry, J. R. 1954. Adsorption and Retention of Cesium by Soils of the Hanford Project. HW-S1011, Westinghouse Hanford Company, Richland, Washington. McHenry, J. R. 1958. “ Ion Exchange Properties of Strontium in a Calcareous Soil.” Soil Science Society of America Proceedings, 22:514-518. McKinley, J. P., J. M. Zachara, S. C. Smith, and G. D. Turner. 1995. “The Influence of Uranyl Hydrolysis and Multiple Site-Binding Reactions on Adsorption of U(VI) to Montmorillonite.” Clays and Clay Minerals, 43(5):586-598. McLean, J. E., and B. E. Bledsoe. 1992. Behavior of Metals in Soils. EPA/540/S-92/018, U.S. Environmental Protection Agency, Ada, Oklahoma. Meybeck, M. 1982. “Carbon, Nitrogen, and Phosphorous Transport by World Rivers.” American Journal of Science, 282:401-450. Morris, D. E., C. J. Chisholm-Brause, M. E. Barr, S. D. Conradson, and P. G. Eller. 1994. 2+ “Optical Spectroscopic Studies of the Sorption of UO2 Species on a Reference Smectite.” Geochimica et Cosmochimica Acta, 58:3613-3623. Nakashima, S., J. R. Disnar, A. Perruchot, and J. Trichet. 1984. “Experimental Study of Mechanisms of Fixation and Reduction of Uranium by Sedimentary Organic Matter Under Diagenetic or Hydrothermal Conditions.” Geochimica et Cosmochimica Acta, 48:2321-2329. Nakayama, E., T. Kumamoto, S. Tsurubo, and T. Fujinaga. 1981. “Chemical Speciation of Chromium in Sea Water. Part 2. Effects of Manganese Oxides and Reducible Organic Materials on the Redox Processes of Chromium.” Analytica Chimica Acta, 130:401-404. Nash, K., S. Fried, A. M. Freidman, and J. C. Sullivan. 1981. “Redox Behavior, Complexing, and Adsorption of Hexavalent Actinides by Humic Acid and Selected Clays.” Environmental Science and Technology, 15:834-837. 6.13
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United States Office of Air and Rad
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NOTICE The following two-volume rep
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This publication is the result of a
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TO COMMENT ON THIS GUIDE OR PROVIDE
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CONTENTS NOTICE ...................
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Concentrations Extractable Iron Con
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Appendix A - Acronyms and Abbreviat
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Figure E.1. Variation of K d for Cr
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Table 5.16. Uranium(VI) aqueous spe
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Table H.3. Simple and multiple regr
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1.0 Introduction The objective of t
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discussed. The geochemical modeling
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2.0 The K d Model The simplest and
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track many more parameters and some
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of interest. The retardation factor
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(e.g., soil). An increasing body of
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complexation constants for the cont
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the soil column. Additionally, the
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Element Table 5.2. Concentrations o
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5.2.3 Aqueous Speciation Cadmium fo
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5.2.4 Dissolution/Precipitation/Cop
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cadmium, indicating that cadmium an
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5.2.6.2.2 Limits of K d Values with
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5.3.4 Dissolution/Precipitation/Cop
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organic chelates (e.g., EDTA). Init
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(tarapacaite) in chromium sludge fr
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K d). Soils containing Mn oxides ox
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Table 5.7. Estimated range of Kd va
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most common valence state of lead e
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Table 5.8. Lead aqueous species inc
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Under reducing conditions, galena (
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C Adsorption of lead increases with
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(Choppin, 1983). Plutonium hydrolyt
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Table 5.10. Plutonium aqueous speci
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5.6.5 Sorption/Desorption Plutonium
Page 75 and 76: content in the system. Additionally
Page 77 and 78: 5.6.6.2.2 Limits of K d Values with
Page 79 and 80: 5.7.4 Dissolution/Precipitation/Cop
Page 81 and 82: much greater concentrations. Thus,
Page 83 and 84: exchanged which they attributed to
Page 85 and 86: up tables was based in part on thei
Page 87 and 88: organic complexes likely predominat
Page 89 and 90: Thorium undergoes hydrolysis in aqu
Page 91 and 92: The distribution of thorium aqueous
Page 93 and 94: from about 10 -8.5 mol/l (0.0007 mg
Page 95 and 96: Based on the assumptions and limita
Page 97 and 98: 5.10 Tritium Geochemistry And K d V
Page 99 and 100: uranium. Uranium(VI) species domina
Page 101 and 102: gives 0.1 to 10 µg/l as the range
Page 103 and 104: mineral in reducing ore zones (Fron
Page 105 and 106: Percent Distribution 100 80 60 40 2
Page 107 and 108: 5.11.6 Partition Coefficient, K d ,
Page 109 and 110: No attempt was made to statisticall
Page 111 and 112: Table 5.18. Selected chemical and t
Page 113 and 114: Another objective of this report is
Page 115 and 116: 6.0 REFERENCES Adriano, D. C. 1992.
Page 117 and 118: Bensen, D. W. 1960. Review of Soil
Page 119 and 120: Metals by Geomedia. Variables, Mech
Page 121 and 122: EPA (U.S. Environmental Protection
Page 123 and 124: Griffin, R. A., A. K. Au, and R. R.
Page 125: + Keeney-Kennicutt, W. L., and J. W
Page 129 and 130: Oscarson, D. W., and H. B. Hume. 19
Page 131 and 132: Relyea, J. F. and D. A. Brown. 1978
Page 133 and 134: Schultz, R. K., R. Overstreet, and
Page 135 and 136: Szalay, A. 1964. “Cation Exchange
Page 137 and 138: Yariv, S., and H. Cross. 1979. Geoc
Page 139 and 140: APPENDIX A Acronyms, Abbreviations,
Page 141 and 142: PC Personal computers operating und
Page 143 and 144: A.3.0 List of Symbols and Notation
Page 145 and 146: APPENDIX B Definitions
Page 147 and 148: Clay Content - particle size fracti
Page 149 and 150: Polynuclear Species - an aqueous sp
Page 151 and 152: C.1.0 Background Appendix C Partiti
Page 153 and 154: Cadmium K d Table C.2. Correlation
Page 155 and 156: C.3.0 Data Set for Soils Table C.4
Page 157 and 158: Cd K d (ml/g) Clay Cont. (wt%) pH C
Page 167 and 168: D.1.0 Background Appendix D Partiti
Page 169 and 170: A second data set (see Section D.4)
Page 171 and 172: Table D.3. Correlation coefficients
Page 173 and 174: By transposing the CEC and cesium K
Page 175 and 176: Table D.6. Cesium K d values measur
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eported in Table D.8 are described
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a 1 b 1 Range of Solution Cs Concen
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Figure D.4. Generalized cesium Freu
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Table D.10. Estimated range of K d
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D.3.0 K d Data Set for Soils and Pu
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Cesium Kd (ml/g) Clay (wt.% ) Mica
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Cesium K d (ml/g) Clay (wt%) Mica (
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Bruggenwert, M. G. M., and A. Kamph
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Shiao, S. Y., P. Rafferty, R. E. Me
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E.1.0 Background Appendix E Partiti
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chromium-reductive soils may stem f
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E.2.0 Approach The approach used to
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Table E.3. Estimated range of K d v
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Table E.4. Data from Rai et al. (19
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E.4.0 References Davis, J. A. and J
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APPENDIX F Partition Coefficients F
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(CEC) of the soils. Such an anomaly
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Table F.1. Summary of K d values fo
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Figure F.2. Variation of K d as a f
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F.4.0 References Abd-Elfattah, A.,
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APPENDIX G Partition Coefficients F
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A number of investigators have exam
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pH value, which is typical of the m
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These significant reductions in ads
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This is typically accomplished by t
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The scatterplots are typically disp
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Table G.2. Regression models for pl
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G.4.0 References Barney, G. S. 1984
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Nelson, D. M., R. P. Larson, and W.
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APPENDIX H Partition Coefficients F
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1.6 ml/g for a measurement made on
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Figure H.1. Relation between stront
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Figure H.2. Relation between stront
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H.2.4 Approach Figure H.4. Relation
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A second look-up table (Table H.5)
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Sr K d (ml/g) Clay Content (%) pH C
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Sr K d (ml/g) Clay Content (%) pH C
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Sr K d (ml/g) Clay Conten t (%) pH
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Konishi, M., K. Yamamoto, T. Yanagi
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APPENDIX I Partition Coefficients F
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descriptive statistics of the thori
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Figure I.1. Linear regression betwe
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The look-up table (Table I.5) for t
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Thorium K d (ml/g) pH Clay (wt.%) C
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Rai, D., A. R. Felmy, D. A. Moore,
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J.1.0 Background Appendix J Partiti
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J.2.2 Uranium K d Studies on Soils
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Washington. The studies included an
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and then decreases with increasing
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Kd (ml/g) 100,000 10,000 1,000 100
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papers. Warnecke et al. (1984) indi
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Anderson et al. (1982) summarize an
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McKinley and Scholtis (1993) compar
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In a similar comparison of sorption
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J.3.1 K d Values as a Function ff p
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discussed, and one would have to ma
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al., 1992; and others). These refer
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· Manskaya et al. (1956) studied a
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concentrations of humic acid, there
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pH U Kd (ml/g) Clay Cont. (wt.%) CE
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J.6.0 References Ames, L. L., J. E.
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Erikson, R. L., C. J. Hostetler, R.
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R. C. Ewing. Materials Research Soc
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Sheppard, M. I., and D. H. Thibault
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Yamamoto, T., E. Yunoki, M. Yamakaw
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