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Modeling Arsenate Competitive Adsorption on Kaolinite, Montmorillonite and Illite

Published online by Cambridge University Press:  28 February 2024

Bruce A. Manning  and
S. Goldberg
Bruce A. Manning
Affiliation:
USDA-ARS, U.S. Salinity Laboratory, 450 West Big Springs Road, Riverside, California 92507
S. Goldberg
Affiliation:
USDA-ARS, U.S. Salinity Laboratory, 450 West Big Springs Road, Riverside, California 92507
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Abstract

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The adsorption of arsenate (As(V)) on kaolinite, montmorillonite and illite was investigated at varying pH and competing anion concentration while holding As(V) concentration (6.7 × 10−7M), clay suspension density (2.5 g L−1) and ionic strength (0.1 M NaCl) constant. The effects of 2 concentrations of phosphate (P) or molybdate (Mo) (6.7 × 10−7 and 6.7 × 10−6M) on As(V) adsorption envelopes (adsorption vs. pH) gave evidence for direct competitive adsorption (in the case of As(V) + P) and possibly site-specific non-competitive adsorption (As(V) + Mo). Distinct As(V) adsorption maxima occurred at approximately pH 5.0 for kaolinite, 6.0 for montmorillonite and 6.5 for illite, and ranged from 0.15 to 0.22 mmol As(V) kg−1. When both As(V) and P were present at equimolar concentrations (6.7 × 10−7M), As(V) adsorption decreased slightly, whereas As(V) adsorption substantially decreased in binary As(V)/P systems when the P concentration was 6.7 × 10−6M, which was 10 times greater than As(V). The presence of Mo at equimolar (6.7 × 10−7 M) and 10 times greater (6.7 × 10−6M) concentrations than As(V) caused only slight decreases in As(V) adsorption because the Mo adsorption maximum occurred at pH < 4. The constant capacitance surface complexation model was applied to As(V) and P adsorption data and was used to predict As(V) adsorption at varying P concentrations. The model gave reasonable descriptions of As(V) adsorption on the 3 clay minerals at varying pH and in the presence of a competing oxyanion (P), indicating that surface complexation modeling may be useful in predicting As(V) adsorption in soils.

Keywords

Arsenate competitive adsorptionIlliteKaoliniteMontmorillonite
Type
Research Article
Information
Clays and Clay Minerals , Volume 44 , Issue 5 , October 1996 , pp. 609 - 623
Copyright
Copyright © 1996, The Clay Minerals Society

References

Anderson, M.A. and Malotky, D.T.. 1979. The adsorption of protolyzable anions on hydrous oxides at the isoelectric pH. J Coll Interface Sci 72: 413–427.CrossRefGoogle Scholar
Barrow, N.J.. 1992. The effect of time on the competition between anions for sorption. J Soil Sci 43: 421–428.CrossRefGoogle Scholar
Bleam, W.F., Pfeffer, P.E., Goldberg, S., Taylor, R.W. and Dudley, R.. 1991. A 31P solid-state nuclear magnetic resonance study of phosphate adsorption at the boehmite/aqueous solution interface. Langmuir 7: 1702–1712.CrossRefGoogle Scholar
Chen, Y.S.R., Butler, J.N. and Stumm, W.. 1973a. Adsorption of phosphate on alumina and kaolinite from dilute aqueous solutions. J Coll Interface Sci 43: 421–436.CrossRefGoogle Scholar
Chen, Y.S.R., Butler, J.N. and Stumm, W.. 1973b. Kinetic study of phosphate reaction with aluminum oxide and kaolinite. Environ Sci Technol 7: 327–332.CrossRefGoogle Scholar
Davis, J.A. and Kent, D.B.. 1990. Surface complexation modeling in aqueous geochemistry. Rev Mineral 23: 177–260.Google Scholar
Edzwald, J.K., Toensing, D.C. and Leung, M.C.Y.. 1976. Phosphate adsorption reactions with clay minerals. Environ Sci Technol 10: 485–490.CrossRefGoogle Scholar
Ferguson, J.F. and Gavis, J.. 1972. A review of the arsenic cycle in natural waters. Water Res 6: 1259–1274.CrossRefGoogle Scholar
Frost, R.R. and Griffin, R.A.. 1977. Effect of pH on adsorption of arsenic and selenium from landfill leachate by clay minerals. Soil Sci Soc Am J 41: 53–57.CrossRefGoogle Scholar
Glaubig, R.A. and Goldberg, S.. 1988. Determination of inorganic arsenic (III) and arsenic (III plus V) using automated hydride-generation atomic-absorption spectrometry. Soil Sci Soc Am J 52: 536–537.CrossRefGoogle Scholar
Goldberg, S.. 1986. Chemical modeling of arsenate adsorption on aluminum and iron oxide minerals. Soil Sci Soc Am J 50: 1154–1157.CrossRefGoogle Scholar
Goldberg, S. and Glaubig, R.A.. 1988. Anion sorption on a calcareous, montmorillonitic soil-arsenic. Soil Sci Soc Am J 52: 1297–1300.CrossRefGoogle Scholar
Herbelin, A.L. and Westall, J.C.. 1994. FITEQL: A computer program for the determination of chemical equilibrium constants from experimental data. Rep. 94–01, Oregon State University, Corvallis.Google Scholar
Hingston, F.J., Posner, A.M. and Quirk, J.P.. 1971. Competitive adsorption of negatively charged ligands on oxide surfaces. Discuss Faraday Soc 52: 334–342.CrossRefGoogle Scholar
Hingston, F.J., Posner, A.M. and Quirk, J.P.. 1972. Anion adsorption by goethite and gibbsite. I. The role of the proton in determining adsorption envelopes. J Soil Sci 23: 177–192.CrossRefGoogle Scholar
Hsia, T.H., Lo, S.L., Lin, C.F. and Lee, D.Y.. 1994. Characterization of arsenate adsorption on hydrous iron oxide using chemical and physical methods. Colloids Surf A: Physicochemical and Engineering Aspects 85: 1–7.CrossRefGoogle Scholar
Huang, P.M.. 1975. Retention of arsenic by hydroxy-aluminum on surfaces of micaceous mineral colloids. Soil Sci Soc Am Proc 39: 271–274.CrossRefGoogle Scholar
Jacobs, L.W., Syers, J.K. and Kenney, D.R.. 1970. Arsenic sorption by soils. Soil Sci Soc Am Proc 34: 750–754.CrossRefGoogle Scholar
Keren, R. and Talpaz, H.. 1984. Boron adsorption by montmorillonite as affected by particle size. Soil Sci Soc Am J 48: 555–559.CrossRefGoogle Scholar
Livesey, N.T. and Huang, P.M.. 1981. Adsorption of arsenate by soils and its relation to selected chemical properties and anions. Soil Sci 131: 88–94.CrossRefGoogle Scholar
Lumsdon, D.G., Fraser, A.R., Russell, J.D. and Livesey, N.T.. 1984. New infrared band assignments for the arsenate ion adsorbed on synthetic goethite. J Soil Sci 35: 381–386.CrossRefGoogle Scholar
Manning, B.A. and Goldberg, S.. 1996. Modeling competitive adsorption of arsenate with phosphate and molybdate on oxide minerals. Soil Sci Soc Am J 60: 121–131.CrossRefGoogle Scholar
Masscheleyn, P.H., Delaune, R.D. and Patrick, W.H. Jr. 1991a. Effect of redox potential and pH on arsenic speciation and solubility in a contaminated soil. Environ Sci Technol 25: 1414–1419.CrossRefGoogle Scholar
Masscheleyn, P.H., Delaune, R.D. and Patrick, W.H. Jr. 1991b. Arsenic and selenium chemistry as affected by sediment redox potential and pH. J Environ Qual 20: 522–527.CrossRefGoogle Scholar
Michaels, A.S. and Bolger, J.C.. 1964. Particle interactions in aqueous kaolinite suspensions. Ind Eng Chem Fundam 3: 14–20.CrossRefGoogle Scholar
Motta, M.M. and Miranda, C.F.. 1989. Molybdate adsorption on kaolinite, montmorillonite, and illite: Constant capacitance modeling. Soil Sci Soc Am J 53: 380–385.CrossRefGoogle Scholar
Muljadi, D., Posner, A.M. and Quirk, J.P.. 1966. The mechanism of phosphate adsorption on kaolinite, gibbsite and pseudoboehmite. I. The isotherms and the effect of pH on adsorption. J Soil Sci 17: 212–229.CrossRefGoogle Scholar
Perrott, K.W., Langdon, A.G. and Wilson, A.T.. 1974. Sorption of phosphate by aluminum and iron(III)-hydroxy species on mica surfaces. Geoderma 12: 223–231.CrossRefGoogle Scholar
Rand, B. and Melton, J.E.. 1975. Isoelectric point of the edge surface of kaolinite. Nature 257: 214–216.CrossRefGoogle Scholar
Roy, W.R., Hassett, J.J. and Griffin, R.A.. 1986. Competitive coefficients for the adsorption of arsenate, molybdate, and phosphate mixtures by soils. Soil Sci Soc Am J 50: 1176–1182.CrossRefGoogle Scholar
Sadiq, M., Zaida, T.H. and Mian, A.A.. 1983. Environmental behavior of arsenic in soils: Theoretical. Water Air Soil Pollut 20: 369–377.CrossRefGoogle Scholar
Schindler, P.W. and Gamsjäger, H.. 1972. Acid-base reactions of the TiO2 (anatase)-water interface and the point of zero charge of TiO2 suspensions. Kolloid Z Z Polym 250: 759–763.CrossRefGoogle Scholar
Stumm, W., Hohl, H. and Dalang, F.. 1976. Interactions of metal ions with hydrous oxide surfaces. Croat Chem Acta 48: 491–504.Google Scholar
Stumm, W., Huang, C.P. and Jenkins, S.R.. 1970. Specific chemical interaction affecting the stability of dispersed systems. Croat Chem Acta 42: 223–245.Google Scholar
Stumm, W., Kummert, R. and Sigg, L.. 1980. A ligand exchange model for the adsorption of inorganic and organic ligands at hydrous oxide interfaces. Croat Chem Acta 53: 291–312.Google Scholar
Swartzen-Allen, L.S. and Matijevic, E.. 1974. Surface and colloid chemistry of clays. Chem Rev 74: 385–400.CrossRefGoogle Scholar
Waychunas, G.A., Rea, B.A., Fuller, C.C. and Davis, J.A.. 1993. Surface chemistry of ferrihydrite: Part 1. EXAFS studies of the geometry of coprecipitated and adsorbed arsenate. Geo-chim Cosmochim Acta 57: 2251–2269.CrossRefGoogle Scholar
Westall, J.C. and Hohl, H.. 1980. A comparison of electrostatic models for the oxide/solution interface. Adv Coll Interface Sci 12: 265–294.CrossRefGoogle Scholar
Wieland, E. and Stumm, W.. 1992. Dissolution kinetics of kaolinite in acidic aqueous solutions at 25°C. Geochim Cosmochim Acta 56: 3339–3355.CrossRefGoogle Scholar
Xu, H., Allard, B. and Grimvall, A.. 1988. Influence of pH and organic substance on the adsorption of As(V) on geologic materials. Water Air Soil Pollut 40: 293–305.CrossRefGoogle Scholar
Zachara, J.M., Cowan, C.E., Schmidt, R.L. and Ainsworth, C.C.. 1988. Chromate adsorption by kaolinite. Clays Clay Miner 36: 317–326.CrossRefGoogle Scholar