Hostname: page-component-848d4c4894-sjtt6 Total loading time: 0 Render date: 2024-06-22T23:58:12.408Z Has data issue: false hasContentIssue false

Textural properties of synthetic clay-ferrihydrite associations

Published online by Cambridge University Press:  09 July 2018

R. Celis
Affiliation:
Instituto de Recursos Naturales y Agrobiología de Sevilla, CSIC, PO Box 1052, E-41080 SevilIa, Spain
J. Cornejo
Affiliation:
Instituto de Recursos Naturales y Agrobiología de Sevilla, CSIC, PO Box 1052, E-41080 SevilIa, Spain
M. C. Hermosin
Affiliation:
Instituto de Recursos Naturales y Agrobiología de Sevilla, CSIC, PO Box 1052, E-41080 SevilIa, Spain

Abstract

Kaolinite-ferrihydrite and montmorillonite-ferrihydrite associations were prepared following a procedure based on the Russell method for the synthesis of ferrihydrite and the texture of the clay-ferrihydrite complexes was studied using different techniques. The textural properties of kaolinite were little affected by the Fe association, showing only a slight increase in the specific surface area measured by nitrogen adsorption and a decrease in the largest pores (>10 µm), as measured by mercury porosimetry. In contrast, the nitrogen specific surface area of the montmorillonite complexes was much higher than that of the clay without Fe and the pore structure depended on the amounts of Fe in the complexes. Application of the fractal approach to nitrogen adsorption data indicated that the surface roughness (microporosity) was greater for the complexes prepared from diluted Fe(III) solutions, in agreement with the information obtained from classical interpretation of the adsorption isotherms (shape of the isotherms and t-plots).

Type
Research Article
Copyright
Copyright © The Mineralogical Society of Great Britain and Ireland 1998

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

Arias, M., Barral, M.T. & Díaz-Fierros, F. (1995) Effects of iron and aluminium oxides on the colloidal and surface properties of kaolin. Clays Clay Miner. 43, 406416.Google Scholar
Avnir, D. & Jaroniec, M. (1989) An isotherm equation for adsorption on fractal surfaces of heterogeneous porous materials. Langmuir, 5, 1431–1433.Google Scholar
Aylmore, L.A.G. & Quirk, J.P. (1967) The micropore size distribution of clay mineral systems. Soil Sci. 18, 117.Google Scholar
Aylmore, L.A.G., Sills, I.D. & Quirk, J.P. (1970) Surface area of homoionic illite and montmorillonite clay minerals as measured by the sorption of nitrogen and carbon dioxide. Clays Clay Miner. 18, 91–96.Google Scholar
Barnhisel, R.I. & Bertsch, P.M. (1989) Chlorites and hydroxyinterlayered vermiculite and smectites. Pp. 729–788 in: Minerals in Soil Environments (Dixon, J.B. & Weed, S.S., editors) SSSA, Madison, WI.Google Scholar
Brooks, C.S. (1955) Nitrogen adsorption experiments on several clay minerals. Soil Sci. 79, 331-347.Google Scholar
Brunauer, S., Deming, L.S., Deming, W.S. & Teller, E. (1940) On a theory of the van der Waals adsorption of gases. J. Am. Chem. Soc. 62, 17231732.Google Scholar
Brunauer, S., Emmett, P.H. & Teller, E. (1938) Adsorption of gases in multimolecular layers. J. Am. Chem. Soc. 60, 309319.Google Scholar
Celis, R., Cornejo, J. & Hermosín, M.C. (1996) Surface fractal dimensions of synthetic clay-hydrous iron oxide associations from nitrogen adsorption isotherms and mercury porosimetry. Clay Miner. 31, 355363.Google Scholar
Fusi, P., Arfaioli, P., Calamai, L. & Bosetto, M. (1993) Interactions of two acetanilide herbicides with clay surfaces modified with Fe(IlI) oxyhydroxides and hexadecyltrimethyl ammonium. Chemosphere, 27, 764771.Google Scholar
Greene, R.S.B. (1975) Clay particle assemblage and their interaction with stabilizing agents. PhD thesis, Univ. Western Australia.Google Scholar
Greene-Kelly, R. (1964) The specific surface areas of montmorillonite. Clay Miner. Bull. 5, 392400.Google Scholar
Gregg, S.J. & Sing, K.S.W. (1982) Adsorption, Surface Area and Porosity. 2nd ed. Academic Press. London.Google Scholar
Halsey, G.D. (1948) Physical adsorption on non-uniform surfaces. J. Chem. Phys. 16, 931937.CrossRefGoogle Scholar
IUPAC (1985) Reporting physisorption data for gas/solid systems ith special refernce to the determination of surface area and porosity. Pure Appl. Chem. 57, 603619.Google Scholar
Lefebvre, Y., Lacelle, S. & Jolicoeur, C. (1992) Surface fractal dimensions of some industrial minerals from gas-phase adsorption isotherms. J. Mater. Res. 7, 18881891.CrossRefGoogle Scholar
Lippens, B.C. & de Boer LH. (1965) Studies on pore systems in catalysts. V. The t-method. J. Catal. 4, 319323.CrossRefGoogle Scholar
Mandelbrot, B. (1982) The Fractal Geometry of Nature. Freeman, San Francisco.Google Scholar
McKeague, J.A. & Day, J.H. (1966) Dithionite- and oxalate-extratable Fe and AI as aids in differentiating various classes of soils. Can. J. Soil Sci. 46, 13–22.Google Scholar
Murray, R.S. & Quirk, J.P. (1990) Surface area of clays. Langmuir, 6, 122–124.Google Scholar
Oades, J.M. (1984) Interactions of polycations of aluminum and iron with clays. Clays Clay Miner. 32, 4957.Google Scholar
Quirk, J.P. & Aylmore, L.A.G. (1971) Domains and quasi-crystalline regions in clay systems. Soil Sci. Soc. Am. Proc. 35, 652654.CrossRefGoogle Scholar
Rengasamy, P. & Oades, J.M. (1977a) Interaction of monomeric and polymeric species of metal ions with clay surfaces. I. Adsorption of iron (III) species. Aust. J. Soil Res. 15, 221233.Google Scholar
Rengasamy, P. & Oades, J.M. (1977b) Interaction of monomeric and polymeric species of metal ions with clay surfaces. II. Changes in surface properties of clays after addition of iron (III). Aust. J. Soil Res. 15, 235242.Google Scholar
Rutherford, D.W., Chiou, C.T. & Eberl, D.D. (1997) Effects of exchanged cation on the microporosity of montmorillonite. Clays Clay Miner. 45, 534–543.Google Scholar
Russell, J.D. (1979) Infrared spectroscopy of ferrihydrite: evidence for the presence of structural hydroxyl groups. Clay Miner. 14, 109–114.Google Scholar
Schwertmann, U. (1979) The influence of aluminum on iron oxides: 5. Clay minerats as sources of aluminum. Soil Sci. 128, 195200.CrossRefGoogle Scholar
Schwertmann, U. (1988) Goethite and hematite formation in the presence of clay minerals and gibbsite at 25°C. Soil Sci. Soc. Am. J. 52, 288291.Google Scholar
Sing, K.S.W. (1967) Assesment of microporosity. Chem. lnd. 20, 829830.Google Scholar
Srasra, E., Bergaya, F., Van Damme, H. & Ariguib, N.K. (1989) Surface properties of an activated bentonitedecolorisation of rape-seed oils. Appl. Clay Sci. 4, 411421.Google Scholar
Thomas, J. Jr. & Bohor, B.F. (1968) Surface area of montmoriltonite from the dynamic sorption of nitrogen and carbon dioxide. Clays Clay Miner. 16, 8391.Google Scholar
Van Damme, H. & Ben Ohoud, M. (1990) From flow to fracture and fragmentation in colloidal media. 2. Local order and fragmentation geometry. Pp. 105 – 116 in: Disorder and Fracture (Charmet, J.C. et al., editors) Plenum Press, New York.Google Scholar
Varadachari, C., Mondal, A.J. & Ghosh, K. (1991) Some aspects of clay-humus complexation: effect of exchangeable cations and lattice charge. Soil Sci. 151, 220227.CrossRefGoogle Scholar
Washburn, E.W. (1921) Note on a method of determining the distribution of pore sizes in a porous material. Proc. Nat. Acad Sci. U.S.A. 7, 115116.Google Scholar
Yin, Y. (1991) Adsorption isotherm on fractally porous materials. Langmuir, 7, 216–217.CrossRefGoogle Scholar