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The Effect of Dissolved Ligands upon the Sorption of Cu(II) by Ca-Montmorillonite

Published online by Cambridge University Press:  28 February 2024

Markus Stadler  and
Paul W. Schindler
Markus Stadler*
Affiliation:
Institute for Inorganic Chemistry, University of Berne, Freiestrasse-3, 3012-Berne, Switzerland
Paul W. Schindler
Affiliation:
Institute for Inorganic Chemistry, University of Berne, Freiestrasse-3, 3012-Berne, Switzerland
*
1Author to whom correspondence should be addressed.
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Abstract

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The effect of three organic ligands on the adsorption of Cu on Ca-montmorillonite was studied. The results indicate that these effects include three different processes:

  1. 1) Enhanced uptake of positively charged Cu-ligand complexes by ion-exchange.

  2. 2) Formation of ternary surface complexes involving surface aluminol groups.

  3. 3) Inhibited uptake due to competition between the surface ligands and the dissolved ligands for dissolved copper.

Ethylenediamine promotes Cu uptake by ion-exchange at low pH but tends to suppress adsorption at aluminol groups by ligand competition at high pH. The same mechanisms are operative for β-alanine; however, the uptake of Cu(β-ala)+ by ion-exchange is not promoted by the attached ligand. The influence of malonate includes both ligand competition and formation of ternary complexes. A quantitative interpretation based on the surface complexation model using the least-square programs FITEQL (Westall, 1982) and GRFIT (Ludwig, 1992) is presented. The obtained equilibrium constants are listed in Tables 2b and 3.

Keywords

Adsorptionβ-alanineCopperEthylenediamineMalonic acidModelingMontmorillonite
Type
Research Article
Information
Clays and Clay Minerals , Volume 41 , Issue 6 , December 1993 , pp. 680 - 692
Copyright
Copyright © 1993, The Clay Minerals Society

References

Benson, L. V., 1982 A tabulation and evaluation of ion exchange data on smectites Environ. Geol. 4 23 10.1007/BF02380496.CrossRefGoogle Scholar
Bjerrum, N., 1948 Bull. Soc. Chim. Beiges 57 432 10.1002/bscb.19480571003.CrossRefGoogle Scholar
Bodenheimer, W., Heller, L., Kirson, B. and Yariv, S., 1962 Organo-metallic clay complexes, part II Clay Miner. Bull. 5 145 10.1180/claymin.1962.005.28.09.CrossRefGoogle Scholar
Bodenheimer, W., Kirson, B. and Yariv, S., 1963 Organo-metallic clay complexes, part I Israel J. Chem. 1 69 10.1002/ijch.196300016.CrossRefGoogle Scholar
Bodenheimer, W., Heller, L. and Yariv, S., 1966 Organometallic clay complexes, part VII: Thermal analysis of montmorillonite-diamine and glycol complexes Clay Miner. 6 167 10.1180/claymin.1966.006.3.04.CrossRefGoogle Scholar
Cloos, P. and Laura, R. D., 1972 Adsorption of ethylenedi-amine (EDA) on montmorillonite saturated with different cations—II. Hydrogen- and ethylenediammonium-montmorillonite protonation and hydrogen bonding Clays & Clay Minerals 20 259 10.1346/CCMN.1972.0200503.CrossRefGoogle Scholar
Fletcher, P. and Sposito, G., 1989 The chemical modeling of clay/electrolyte interactions for montmorillonite Clay Miner. 24 375 10.1180/claymin.1989.024.2.14.CrossRefGoogle Scholar
Ludwig, Charles 1992() GRIFT, a Program for Solving Speciation Problems, Evaluation of Equilibrium Constants, Concentrations and Other Physical Parameters: Internal Report, University of Berne, Switzerland.Google Scholar
Maes, A., Peigneur, P. and Cremers, A., 1978 Stability of metal uncharged ligand complexes in ion exchangers. Part 2. The copper+ethylenediamine complex in montmorillonite and sulphonic acid resin J. Chem. Soc. Faraday Trans. I 74 182 10.1039/f19787400182.CrossRefGoogle Scholar
Martell, A. E. and Smith, R. M., 1976 Critical Stability Constants New York and London Plenum Press.Google Scholar
Shaviv, A. and Mattigod, S. V., 1985 Cation exchange equilibria in soils expressed as cation-ligand complex formation Soil Sci. Soc. Am. J. 49 569 10.2136/sssaj1985.03615995004900030007x.CrossRefGoogle Scholar
Siffert, B. and Espinasse, P., 1980 Adsorption of organic diacids and sodium polyacrylate onto montmorillonite Clays & Clay Minerals 28 381 10.1346/CCMN.1980.0280508.CrossRefGoogle Scholar
Sillèn, L. G. and Martell, A. E., 1964 Stability Constants of Metal-Ion Complexes, Section I: Inorganic Ligands London The Chemical Society.Google Scholar
Schindler, P. W., (1990) Co-adsorption of metal ions and organic ligands: Formation of ternary surface complexes: in Mineral-Water Interface Geochemistry, Vol. 23, Hochella, M. F., and White, A. F., eds., Mineralogical Society of America, p. 281.CrossRefGoogle Scholar
Schindler, P. W., and Stumm, W., (1987) The surface chemistry of oxides, hydroxides, and oxide minerals: in Aquatic Surface Chemistry, Stumm, W., ed., Wiley Interscience, p. 83.Google Scholar
Stadler, M. and Schindler, P. W., 1993 Modelling of H+ and Cu2+ adsorption on Ca-montmorillonite Clays & Clay Minerals 41 288 10.1346/CCMN.1993.0410303.CrossRefGoogle Scholar
Tsunashima, A. and Hayashi, H., 1984 Adsorption of some amino acids by Ca-, Co-, and Cu-montmorillonite Rep. Res. Inst. Underground Resources, Min. Coll., Akita Univ. 49 53.Google Scholar
Velghe, F., Schoonheydt, R. A. and Uytterhoeven, J. B., 1977 Spectroscopic characterization and thermal stability of cop-per(II) ethylenediamine complexes on solid surfaces. 2. Montmorillonite J. Phys. Chem. 81 1187 10.1021/j100527a013.CrossRefGoogle Scholar
Westall, J. C., 1982 A Program for the Determination of Chemical Equilibrium Constants from Experimental Data: User’s Guide vs. 1.2 Oregon Oregon State University Corvallis.Google Scholar