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Clays and Clay Minerals

, Volume 8, Issue 1, pp 102–114 | Cite as

Water Vapor Sorption on Kaolinite: Entropy of Adsorption

  • R. Torrence Martin
Article

Abstract

Water vapor adsorption isotherms at five temperatures between 0 and 40°C were obtained on Li and Na kaolinite. By a careful experimental technique, the error in the determination of weight of water adsorbed was reduced to + 0.01 mg/g and that of equilibrium vapor pressure was reduced to ± 0.0002 mm Hg. The data were used to calculate the integral and differential entropy of the adsorbed water phase.

The differential entropy of adsorption (the partial molar entropy of water in the sorbate phase minus the molar entropy of normal liquid water) has large positive values at low surface coverage. As more water is adsorbed, the differential entropy drops to a negative value approximately equal to that of a two-dimensional liquid which is about the same as the entropy for hypothetical ice at this temperature and pressure. The water can hardly be treated as “ice” because the large negative entropy persists over a very small p/p0 range and occurs at a p/p0 such that the surface is only about 70 percent covered. The integral entropy of adsorption (the molar entropy of water in the sorbate phase minus the molar entropy of normal liquid water) has positive values on both Li and Na kaolinite throughout the p/p0 range investigated; p/p0 = 0 to p/p0 = 0.5. These entropy data indicate that the water molecules in the adsorbed phase on Li or Na kaolinite possess greater randomness than the water molecules in normal liquid water from the dry clay up to at least p/p0 =0.5. The difference between integral and differential entropies is explained as a “configurational entropy“ that changes with the amount of the adsorbed phase.

A hypothesis to explain the entropy data is proposed in which one builds inward from normal liquid water to the solid surface rather than the more conventional mechanisms which build outward from the solid surface. In this way the entropy data can be explained in terms of what happens to the structure of normal liquid water when different sized ions or nonpolar molecules, or both, are added. Literature data for the low density and dielectric coefficient of the sorbed phase plus the large amounts of -unfrozen water still present at — 5°C are frequently used as evidence for the quasi-solid structure of the sorbed phase. A consideration of the water molecules in the sorbed phase as more random than normal liquid water is an equally plausible explanation. Nuclear magnetic resonance and magnetic susceptibility data which cannot be explained by an increase in water structure are in complete agreement with the entropy data and the proposed new working hypothesis. It is concluded that not only the present entropy data but also all literature data (known to the author) concerning the sorbed phase can be satisfactorily explained if one considers the water molecules in the sorbed phase as being more random, less structured, than normal liquid water.

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References

  1. Anderson, D. M. and Low, P. F. (1958) The density of water adsorbed by lithium-, sodium—, and potassium-bentonite: Soil Sci. Soc. Amer. Proc., v. 22, pp. 99–103.CrossRefGoogle Scholar
  2. Buswell, A. M. and Rodebush, W. H. (1956) Water: Scientific American, v. 194, pp. 77–89.Google Scholar
  3. Frank, H. S. and Wen, W. Y. (1957) Structural aspects of ion-solvent interaction in aqueous solutions: A suggested picture of water structure: Disc. Faraday Soc., no. 24, pp. 133–140.CrossRefGoogle Scholar
  4. Goates, Rex and Bennett, S. J. (1957) Thermodynamic properties of water adsorbed on soil minerals: II, Kaolinite: Soil Sci., v. 83, pp. 325–330.CrossRefGoogle Scholar
  5. Grim, R. E. (1953) Clay Mineralogy: McGraw Hill Company, Inc., New York, 384 pp.CrossRefGoogle Scholar
  6. Hemwall, J. B. and Low, P. F. (1956) The hydrostatic repulsive force in clay swelling: Soil Sci., v. 82, pp. 135–145.CrossRefGoogle Scholar
  7. Hendricks, S. B. and Jefferson, M. E. (1938) Structures of kaolin and talc-pyrophyllite hydrates and their bearing on water sorption of the clays: Amer. Min., v. 23, pp. 863–875.Google Scholar
  8. Hill, T. L. (1950) Statistical mechanics of adsorption, IX. Adsorption thermodynamics and solution thermodynamics: J. Chem. Phys., v. 18, pp. 246–256.CrossRefGoogle Scholar
  9. Jurinak, J. J. and Volman, D. H. (1958) Thermodynamics of ethylene dibromide vapor adsorption by Ca-montmorillonite and Ca-kaolinite: Soil Sci., v. 86, pp. 6–12.CrossRefGoogle Scholar
  10. Keenan, A. G., Mooney, R. W. and Wood, L.A. (1951) The relation between exchangeable ions and water adsorption on kaolinite: J. Phys. Colloid Chem., v. 55, pp. 1462–1474.Google Scholar
  11. MacDougall, F. H. (1948) Thermodynamics and Chemistry: John Wiley and Sons, Inc., New York, 3rd ed.Google Scholar
  12. Martin, R. T. (1958) Water vapor sorption on lithium kaolinite: in Clays and Clay Minerals: Natl. Acad. Sci.—Natl. Res. Council, pub. 566, pp. 23–38.Google Scholar
  13. Martin, R. T. (1959) Water-vapor sorption on kaolinite: Hysteresis: in Clays and Clay Minerals, Proc. 6th Conf., Pergamon Press, N.Y., pp. 259–278.Google Scholar
  14. Mathieson, A. McL. and Walker, G. F. (1954) Crystal structure of magnesium vermiculite: Amer. Min., v. 39, pp. 231–255.Google Scholar
  15. Milligan, W. O. and Whitehurst, H. B. (1952) Magnetic properties of adsorbed vapors: J. Phys. Chem., v. 56, pp. 1073–1077.CrossRefGoogle Scholar
  16. Mooney, R. W., Keenan, A. G. and Wood, L. A. (1952) Adsorption of water vapor by montmorillonite, II. Effect of exchangeable ions and lattice swelling as measured by x-ray diffraction: J. Amer. Chem. Soc., v. 74, pp. 1371–1374.CrossRefGoogle Scholar
  17. Norton, F. H. and Hodgdon, F. B. (1932) Some notes on the nature of clay: J. Amer. Ceram. Soc., v. 15, pp. 191–205.CrossRefGoogle Scholar
  18. Norton, F. H. and Johnson, A. L. (1944) Fundamental study of clay: V, Nature of water film in plastic clay: J. Amer. Ceram. Soc, v. 26, pp. 77–80.Google Scholar
  19. Pickett, A. G. and Lemcoe, M. M. (1957) Research studies of methods for increasing soil trafficability: A report by Southwest Research Institute under contract to C.R.Z.G., A.F.C.R.C., Hanseom Field, Bedford, Mass.Google Scholar

Copyright information

© The Clay Minerals Society 1959

Authors and Affiliations

  • R. Torrence Martin
    • 1
  1. 1.Soil Engineering DivisionMassachusetts Institute of TechnologyCambridgeUSA

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