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Quinoline Sorption on Na-Montmorillonite: Contributions of the Protonated and Neutral Species

Published online by Cambridge University Press:  02 April 2024

Calvin C. Ainsworth ,
John M. Zachara  and
Ron L. Schmidt
Calvin C. Ainsworth
Affiliation:
Battelle, Pacific Northwest Laboratories, P.O. Box 999, Richland, Washington 99352
John M. Zachara
Affiliation:
Battelle, Pacific Northwest Laboratories, P.O. Box 999, Richland, Washington 99352
Ron L. Schmidt
Affiliation:
Battelle, Pacific Northwest Laboratories, P.O. Box 999, Richland, Washington 99352
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Abstract

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Dilute aqueous solutions of quinoline were contacted with Na-montmorillonite to elucidate the sorption process of the neutral and protonated species. Sorption occurs via a combination of ion exchange and molecular adsorption and yields S-type isotherms. Exchange between the quinolinium ion (QH+) and Na can be described by means of Vanselow selectivity coefficients and a thermodynamic exchange constant (Kex). Due to the apparent adsorption of the neutral species at high mole fractions (x) of the solid phase, the thermodynamic standard state was defined as 0.5 mole fraction. The selectivity at pH ~4.95 of the QH+ species over Na (at XQH+ = 0.5) was determined to be Kv = 340. At pH ≥ 5.5 surface mole fractions of 0.5 could not be obtained without adsorption of the neutral species. This study suggests that at dilute solution concentrations quinoline is sorbed preferentially as the cation even at pHs ≫ pKa. A critical surface-solution concentration is apparently necessary for adsorption of the neutral species.

Keywords

AdsorptionCation exchangeMontmorilloniteQuinolineVanselow selectivity
Type
Research Article
Information
Clays and Clay Minerals , Volume 35 , Issue 2 , April 1987 , pp. 121 - 128
Copyright
Copyright © 1987, The Clay Minerals Society

References

Literature Cited

Babcock, K. L. and Duckart, E. C., 1980 The standard state for exchangeable cations Soil Sci. 130 64 – 67.CrossRefGoogle Scholar
Babcock, K. L. and Schulz, R. K., 1970 Isotopic and conventional determination of exchangeable sodium percentage of soil in relation to plant growth Soil Sci. 109 19 – 22.CrossRefGoogle Scholar
Bailey, G. W., White, J. L. and Rothberg, T., 1968 Adsorption of organic herbicides by montmorillonite: Role of pH and chemical character of adsorbate Soil Sci. Soc. Amer. Proc. 32 222 – 234.CrossRefGoogle Scholar
Bums, I. G., Hayes, M. H. G. and Stacey, M., 1973 Some physicochemical interactions of paraquat with soil organic materials and model compounds Weed Res. 13 79 – 90.Google Scholar
Chander, S., Fuerstenau, D. W., Stigter, D., Ottewill, R. H., Rochester, C. H. and Smith, A. L., 1983 On hemimicelle formation at oxide/water interfaces Adsorption from Solution New York Academic Press 197 – 210.CrossRefGoogle Scholar
Cowen, C. T. and White, D., 1958 The mechanisms of exchange reactions between sodium montmorillonite and various n-primary aliphatic amine salts Trans. Faraday Soc. 54 691 – 697.CrossRefGoogle Scholar
Dixon, J. B., Moore, D. E., Agnihotri, N. P. and Lewis, D. E. Jr., 1970 Exchange of diquat2+ in soil clays, Vermiculite, and smectite Soil Sci. Soc. Amer. Proc. 34 805 – 808.CrossRefGoogle Scholar
Doehler, R. W., Young, W. A. and Swineford, A., 1961 Some conditions affecting the adsorption of quinoline by clay minerals in aqueous suspensions Clays and Clay Minerals, Proc. 9th Natl. Conf, West Lafayette, Indiana, 1960 New York Pergamon Press 468 – 483.Google Scholar
Duckart, E. C. and Babcock, K. L., 1984 Thermodynamics of cation exchange using Babcock’s standard state Soil Sci. 138 1 – 7.CrossRefGoogle Scholar
Gilmour, J. T. and Coleman, N. T., 1971 s-Triazine adsorption studies: Ca-H-humic acid Soil Sci. Soc. Amer. Proc. 35 256 – 259.CrossRefGoogle Scholar
Grim, R. E., Allaway, W. H. and Cuthbert, F. L., 1947 Reaction of different clay minerals with some organic cations J. Amer. Chem. Soc. 30 137 – 142.Google Scholar
Hayes, M. H. B. Pick, M. E. and Toms, B. A., 1978 The influence of organocation structure on the adsorption of mono- and of bipridinium cations by expanding lattice clay minerals. I. Adsorption by Na+-montmorillonite J. Colloid Interface Sci. 65 254 – 265.CrossRefGoogle Scholar
Helmy, A. K., De Bussetti, S. G. and Ferreiro, E. A., 1983 Adsorption of quinoline from aqueous solutions by some clays and oxides Clays & Clay Minerals 31 29 – 36.CrossRefGoogle Scholar
Karickhoff, S. W. and Bailey, G. W., 1976 Protonation of organic bases in clay-water systems Clays & Clay Minerals 24 170 – 176.CrossRefGoogle Scholar
Lailach, G. E., Thompson, T. D. and Brindley, G. W., 1968 Absorption of pyrimidines, purines, and nucleosides by Li-, Na-, Mg-, and Ca-montmorillonite (clay-organic studies XII) Clays & Clay Minerals 16 285 – 293.CrossRefGoogle Scholar
Lailach, G. E., Thompson, T. D. and Brindley, G. W., 1968 Absorption of pyrimidines, purines, and nucleosides by Co-, Ni-, Cu-, and Fe(III)-montmorillonite (clayorganic studies XIII) Clays & Clay Minerals 16 295 – 301.CrossRefGoogle Scholar
Moreale, A. and Van Bladel, R., 1976 Influence of soil properties on adsorption of pesticide-derived aniline and p-chloroaniline J. Soil Sci. 27 48 – 57.CrossRefGoogle Scholar
Mortland, M. M., 1970 Clay-organic complexes and interactions Adv. Agron. 22 75 – 117.CrossRefGoogle Scholar
Peigneur, R., Maes, A. and Cremers, A., 1975 Heterogeneity of charge distribution in montmorillonite as inferred from cobalt adsorption Clays & Clay Minerals 23 71 – 75.CrossRefGoogle Scholar
Perrin, D. D., Dempsey, B. and Serjeant, E. P., 1981 pKa Predictionfor Organic Acids and Bases New York Chapman and Hall.CrossRefGoogle Scholar
Philen, O. D. Jr. Weed, S. B. and Weber, J. B., 1970 Estimation of surface charge density of mica and Vermiculite by competitive adsorption of diquat2+ vs. paraquat2+ Soil Sci. Soc. Amer. Proc. 34 527 – 531.CrossRefGoogle Scholar
Sposito, G., 1981 The Thermodynamics of Soil Solutions New York Oxford University Press.Google Scholar
Sposito, G., 1984 The Surface Chemistry of Soils New York Oxford University Press.Google Scholar
Sposito, G., Holtzclaw, K. M., Johnston, C. T. and LeVesque-Madore, C. S., 1981 Thermodynamics of sodium-copper exchange on Wyoming bentonite at 298°K Soil Sci. Soc. Amer. J. 45 1079 – 1084.CrossRefGoogle Scholar
Theng, B. K. G., 1974 The Chemistry of Clay-Organic Reactions New York Wiley 221 – 319.Google Scholar
Theng, B. K. G. Greenland, D. J. and Quirk, J. P., 1967 Adsorption of alkylammonium cations by montmorillonite Clay Miner. 7 1 – 17.CrossRefGoogle Scholar
Thompson, T. D. and Brindley, G. W., 1969 Adsorption of pyrimidines, purines and nucleosides by Na-, Mg-, and Cu(II)-illite (clay-organic studies XVI) Amer. Miner. 54 858 – 868.Google Scholar
Vansant, E. F. and Uytterhoeven, J. B., 1972 Clays & Clay Minerals 20 Thermodynamicsofexchangeofn-alkylammoniumionsonNamontmorillonite 47 – 54.CrossRefGoogle Scholar
White, D. and Cowen, C. T., 1960 Aromatic amine derivatives of montmorillonite Brit. Ceram. Soc. 59 16 – 21.Google Scholar
Weed, S. B. and Weber, J. B., 1969 The effect of cation exchange capacity on the retention of diquat2+ and paraquat2+ by three-layer type clay minerals. I. Adsorption and release Soil Sci. Soc. Amer. Proc. 33 379 – 385.CrossRefGoogle Scholar
Zachara, J. M., Ainsworth, C. C., Felice, L. J. and Resch, C. T., 1986 Quinoline sorption to subsurface materials: Role of pH and retention of the organic cation Environ. Sci. Technol. 20 620 – 627.CrossRefGoogle ScholarPubMed
Zierath, D. L., Hassett, J. J., Banwart, W. L., Wood, S. G. and Means, J. C., 1980 Sorption of benzidine by sediments and soils Soil Sci. 129 277 – 281.CrossRefGoogle Scholar