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Free Energy of Formation of Beidellite from Apparent Solubility Measurements

Published online by Cambridge University Press:  01 July 2024

U. K. Misra
Affiliation:
Department of Agronomy, University of Missouri, Columbia, MO 65201, U.S.A.
W. J. Upchurch*
Affiliation:
Department of Agronomy, University of Missouri, Columbia, MO 65201, U.S.A.
*
Research Associate and Associate Professor of Agronomy, respectively.
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Abstract

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The structural formula for K and Mg saturated beidellite was calculated from the total elemental analysis of the < 0.2 μm clay fraction of the B2t horizon of a Mexico soil. The free energies of formation (ΔGfo) of K-beidellite and Mg-beidellite as determined from their apparent solubilities were -2491.3 and -2484.0 ± 3.2 kcal per mole, respectively. The free energies of formation correspond to a clay mineral structure calculated on the basis of a 24 oxygen cell.

Type
Research Article
Copyright
Copyright © 1976 The Clay Minerals Society

Footnotes

*

Contribution from the Missouri Agr. Exp. Sta., Journal Series Number 7087.

References

Garrels, R. M. (1957) Some free energy values from geologic relations: Am. Miner. 48, 897910.Google Scholar
Garrels, R. M. and Christ, C. L. (1965) Solutions, Minerals, and Equilibria: Harper & Row, New York.Google Scholar
Greene-Kelly, R. (1953) Identification of montmorillonoids: J. Soil Sci. 4, 233237.CrossRefGoogle Scholar
Helgeson, H. C. (1969) Thermodynamics of hydrothermal systems at elevated temperatures and pressures: Am. J. Sci. 267, 725804.CrossRefGoogle Scholar
Helgeson, H. C., Brown, T. R. and Leeper, R. H. (1969) Handbook of Theoretical Activity Diagrams Depicting Chemical Equilibria in Geological Systems Involving an Aqueous Phase at 1 atm. and 0–300°C: Freeman, Cooper & Co., San Francisco.Google Scholar
Hem, J. D., Roberson, C. E., Linde, C. J. and Polzer, W. L. (1973) Chemical interaction of aluminum and aqueous silica at 25°C: U.S. Geol. Survey Water-Supply Paper 1827-E.Google Scholar
Huang, W. H. and Keller, W. D. (1971) Dissolution of clay minerals in dilute organic acids at room temperature: Am. Miner. 56, 10821095.Google Scholar
Huang, W. H. and Keller, W. D. (1973) Gibbs free energies of formation calculated from dissolution data using specific mineral analyses—III: Clay Minerals: Am. Miner. 58, 10231028.Google Scholar
Iler, R. K. (1955) Colloid Chemistry of Silica and Silicates: Cornell University Press, Ithaca, New York.CrossRefGoogle Scholar
Olson, R. V. (1965) Iron: Methods of Soil Analyses, Part II. Am. Soc. Agronomy, Madison, Wisconsin.Google Scholar
Jackson, M. L. (1956) Soil Chemical Analysis—Advanced Course: Publ. by the author, Dept. of Soils, Univ. of Wis., Madison 6, Wis.Google Scholar
Kittrick, J. A. (1966) Free energy of formation of kaolinite from solubility measurements: Am. Miner. 51, 14571466.Google Scholar
Kittrick, J. A. (1970) Precipitation of kaolinite at 25°C and 1 atm: Clays & Clay Minerals 18, 261268.CrossRefGoogle Scholar
Kittrick, J. A. (1971a) Stability of Montmorillonites; Soil Sci. Soc. Am. Proc. 35, 140145.CrossRefGoogle Scholar
Kittrick, J. A. (1971b) Montmorillonite equilibria and weather environment: Soil Sci. Soc. Am. Proc. 35, 815820.CrossRefGoogle Scholar
Kittrick, J. A. (1971c) Stability of montmorillonites—II: Aberdeen montmorillonites: Soil Sci. Soc. Am. Proc. 35, 820823.CrossRefGoogle Scholar
Langmuir, D. (1969) The Gibbs free energies of substances in the system Fe–O2–H2O–H2–CO2 at 25°C: U.S. Geol. Surv. Prof. Paper 650-B, pp 180183.Google Scholar
Marshall, C. E. (1949) The Colloid Chemistry of the Silicate Minerals: Academic, New York.Google Scholar
Marshall, C. E., Chowdhury, M. Y. and Upchurch, W. J. (1973) Lysimetric and chemical investigations of pedological changes—II: Equilibration of profile samples with aqueous solutions: Soil Sci. 116, 336358.CrossRefGoogle Scholar
Misra, U. K., Blanchar, R. W. and Upchurch, W. J. (1974) Aluminum content of soil extracts as function of pH and ionic strength: Soil Sci. Soc. Am. Proc. 38, 897902.CrossRefGoogle Scholar
Pickett, E. E. and Koirtyohann, S. R. (1969) The nitrous oxide-acetylene flame in emission analysis—III: Aluminum, gallium, indium, thallium, germanium and tin: Spectrochim. Acta. 24B, 325333.CrossRefGoogle Scholar
Plumb, R. C. and Swaine, J. W. Jr. (1964) Oxide coated electrodes—II: Aluminum in alkaline solution and the nature of the aluminate ion: J. phys. Chem. 68, 20572064.CrossRefGoogle Scholar
Pruden, G. and King, H. G. C. (1969) A scheme of semi-micro analysis for the major elements in clay minerals based on modifications to conventional methods of silicate analysis: Clay Miner. 8, 113.CrossRefGoogle Scholar
Raupach, M. (1963) Solubility of simple aluminum compounds expected in soils—I: Hydroxides and oxyhydroxides: Aust. J. Soil Res. 1, 2835.CrossRefGoogle Scholar
Reesman, A. L. and Keller, W. D. (1967) Chemical composition of illite: J. sedim. Petrol. 37, 592596.Google Scholar
Reesman, A. L. and Keller, W. D. (1968) Aqueous solubility studies of high-alumina and clay minerals: Am. Miner. 35, 929941.Google Scholar
Richburg, J. S. and Adams, F. (1970) Solubility and hydrolysis of aluminum in soil solutions and saturated-paste extracts: Soil Sci. Soc. Am. Proc. 34, 728734.CrossRefGoogle Scholar
Robie, R. A. and Waldbaum, D. R. (1968) Thermodynamic properties of minerals and related substances: Geol. Survey Bull., 1952.Google Scholar
Smith, R. W. and Hem, J. D. (1972) Effect of aging on aluminum hydroxide complexes in dilute aqueous solutions: U.S. Geol. Survey Water-Supply Paper 1827–D.Google Scholar
Stumm, W. and Morgan, James J. (1970) Oxidation and reduction: In Aquatic Chemistry, pp. 350371. Wiley-Interscience, N.Y.Google Scholar
Truesdell, A. H. and Jones, B. F. (1973) WATEQ, A computer program for calculating chemical equilibria of natural waters: NTIS, U.S. Dept. Commerce, Springfield, Va. 22151.Google Scholar
Whittig, L. D. (1965) X-ray diffraction technique for mineralogical identification and mineralogical composition: Methods of Soil Analysis, Part I (edited by Black, C. A.) Amer. Soc. of Agronomy, Madison, WI.Google Scholar