Hostname: page-component-586b7cd67f-2brh9 Total loading time: 0 Render date: 2024-11-30T18:39:22.284Z Has data issue: false hasContentIssue false

The effect of an Fe(II)-silicate on selected properties of a montmorillonitic clay

Published online by Cambridge University Press:  09 July 2018

D. W. Oscarson
Affiliation:
Atomic Energy of Canada Limited, Whiteshell Nuclear Research Establishment, Pinawa, Manitoba ROE 1LO Canada
R. B. Heimann
Affiliation:
Atomic Energy of Canada Limited, Whiteshell Nuclear Research Establishment, Pinawa, Manitoba ROE 1LO Canada

Abstract

A montmorillonite clay and an X-ray amorphous Fe(II)-silicate were suspended in a synthetic groundwater solution under oxic and anoxic conditions at 23 and 70°C for 200 days. The clay samples were then analysed for total Fe, Fe(II), dithionite- and oxalate-extractable Fe (Fed and Feo), cation exchange capacity (CEC), and examined by X-ray diffraction (XRD) and diffuse reflectance spectrometry (DRS). The total iron content and Fe(II)/Fe(III) ratio of the clay increased with an increase in temperature and both were greater under anoxic than oxic conditions, as were the amounts of Fed and Feo. The CEC of the clay was lower in the presence of the Fe-silicate, suggesting that Fe-hydroxide had precipitated at the edges of the clay blocking some cation-exchange sites. No changes in the clay were detected by XRD or DRS after contact with the Fe-silicate, nor was there any evidence for Fe-hydroxide material in the interlayer region of the clay. However, it is shown that the amount and nature of iron associated with clay can be significantly altered and certain properties of the clay, such as CEC, can be affected when the clay is in contact with Fe(II)-containing materials.

Type
Research Article
Copyright
Copyright © The Mineralogical Society of Great Britain and Ireland 1988

Access options

Get access to the full version of this content by using one of the access options below. (Log in options will check for institutional or personal access. Content may require purchase if you do not have access.)

References

Alperovitch, N., Shainberg, I., Keren, R., Singer, M.J. (1985) Effect of clay mineralogy and aluminum and iron oxides on the hydraulic conductivity of clay-sand mixtures. Clays Clay Miner. 33, 443–450.CrossRefGoogle Scholar
Ames, L., McGarrah, J.E., Walker, B.A. Salter, P.F. (1983) Uranium and radium sorption on amorphous ferric oxyhydroxide. Chem. Geol. 40, 135–148.Google Scholar
Arden, T.V. (1950) The solubility products of ferrous and ferrosic hydroxides. J. Chem. Soc. 882885.CrossRefGoogle Scholar
Blackmore, A.V. (1973) Aggregation of clay by the products of iron (III) hydrolysis. Aust. J. Soil Res. 11,7582.Google Scholar
Brown, G. Brindley, G. W. (1984) X-ray diffraction procedures for clay mineral identification. Pp. 305360 in: Crystal Structures of Clay Minerals and their X-ray Identification (Brindley, G.W. Brown, G., editors). Mineralogical Society, London.Google Scholar
Carstea, D.D. (1968) Formation of hydroxy-Al and -Fe interlayers in montmorillonite and vermiculite: influence of particle size and temperature. Clays Clay Miner. 16, 231–238.Google Scholar
Carstea, D.D., Harward, M.E. Knox, E.G. (1970) Comparison of iron and aluminium hydroxy interlayers in montmorillonite and vermiculite: I. Formation. Soil Sci. Soc. Am. Proc. 34, 517–521.Google Scholar
Clark, J.S. Nichol, W.E. (1968) Reactions of iron hydrous oxide with Wyoming bentonite. Can. J. Soil Sci. 48, 173–183.Google Scholar
Davies, C.W. (1962) Ion Association. Butterworths, London.Google Scholar
El-Rayah, H.M.E. & Rowell, D.L. (1973) The influence of iron and the permeability of a Na-soil. J. Soii ScL 24, 137–144.Google Scholar
El-Swaify, S.A. & Emerson, W.W. (1975) Changes in the physical properties of soil clays due to precipitated aluminum and iron hydroxides: I. Swelling and aggregate stability after drying. Soil Sci. Soc. Am. Proc. 39, 1056-1063.CrossRefGoogle Scholar
Fournier, R.O. Potter, R.W. (1982) An equation correlating the solubility of quartz in water from 25 ° to 900 °C at pressures up to 10 000 bars. Geochim. Cosmochim. Acta 46, 1969–1973.Google Scholar
Frape, S.K., Fritz, P. & McNutt, R.N. (1984) Water-rock interaction and chemistry of groundwaters from the Canadian Shield. Geochim. Cosmochim. Acta 48, 1617–1627.Google Scholar
Grim, R.E. (1968) Clay Mineralogy, 2nd ed., McGraw-Hill, New York.Google Scholar
Hancox, W.T. (1986) Progress in the Canadian nuclear fuel waste management program. Proc. 2nd Int. Conf. Radioactive Waste Management, Winnipeg, Manitoba, 19.Google Scholar
Hillebrand, W.F., Lundell, G.E.F., Bright, H. A. Hoffman, J.I. (1953) Applied Inorganic Analysis 2nd ed., John Wiley Sons, New York.Google Scholar
Jackson, M.L. (1975) Soil Chemical Analysis–Advanced Course 2nd ed. Published by the author, University of Wisconsin, Madison, Wisconsin,Google Scholar
Jenne, E.A. (1968) Controls on Mn, Fe, Co, Ni, Cu, and Zn concentrations in soils and water: the significant role of hydrous Mn and Fe oxides. Am. Chem. Soc., Adv. Chem. Ser. 73, 337–387.Google Scholar
Kinthr, E.B. Diamond, S. (1956) A new method for preparation and treatment of oriented-aggregate specimens of soil clays for X-ray diffraction analysis. Soil Sci. 81, 111–120.Google Scholar
Lewis, D.G. Schwertmann, U. (1979) The influence of aluminum on the formation of iron oxides. IV. The influence of (Al), (OH), and temperature. Clays Clay Miner. 27, 195–200.Google Scholar
Lindsay, W.L. (1979) Chemical Equilibrium in Soils. John Wiley, New York.Google Scholar
Marshall, W.L. (1980) Amorphous silica solubilities–III. Activity coefficient relations and predictions of solubility behaviour in salt solutions, 0-350 °C. Geochim. Cosmochim. Acta 44, 925–931.CrossRefGoogle Scholar
McKeague, J.A. Day, J.H. (1966) Dithionite- and oxalate-extractable Fe and A1 as aids in differentiating various classes of soils. Can. J. Soil Set 46, 13–22.Google Scholar
Oscarson, D.W. Miller, H.G. (1988) A method for preventing the rehydration of heated smectites during X- ray diffraction analysis. Atomic Energy of Canada Limited Technical Record TR-446.Google Scholar
Ponnamperuma, F.N., Tianco, E.M. & Loy, T. (1967) Redox equilibria in flooded soils: I. The iron hydroxide systems. Soil Sci. 103, 374–382.Google Scholar
Quigley, R.M. (1984) Quantitative mineralogy and preliminary pore-water chemistry of candidate buffer and backfill materials for a nuclear fuel waste disposal vault. Atomic Energy of Canada LImited Report AECL-7827Google Scholar
Rich, C.I. (1968) Hydroxy interlayers in expansible layer silicates. Clays Clay Miner. 16, 15–30.CrossRefGoogle Scholar
Roberson, H.E. & Lahann, R.W. (1981) Smectite to illite conversion rates : effects of solution chemistry. Clays Clay Miner. 29, 129–135.CrossRefGoogle Scholar
Schwertmann, U. Taylor, R.M. (1977) Iron oxides. Pp. 145180 in: Minerals in Soil Environments. (Dixon, J.B. Weed, S.B., editors). Soil Science Society of America, Madison, Wisconsin.Google Scholar
Srodon, J. (1980) Precise identification of illite/smectite interstratifications by X-ray powder diffraction, days Clay Miner. 28, 401–411.Google Scholar
Stucki, J.W. (1981) The quantitative assay of minerals for Fe2+ and Fe3+ using 1,10-phenanthroline. II. A photochemical method. Soil Sci. Soc. Am. J. 45, 638–641.Google Scholar
Thomas, G.W. (1982) Exchangeable Cations. Pp. 159165 in: Methods of Soil Analysis, Part 2, Chemical and Microbiological Properties 2nd ed., American Society of Agronomy, Inc., Madison, Wisconsin.Google Scholar