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Dissolution experiments of Na- and Ca-montmorillonite in groundwater simulants under anaerobic conditions

Published online by Cambridge University Press:  09 July 2018

E. Myllykylä ,
M. Tanhua-Tyrkkö ,
A. Bouchet  and
M. Tiljander
E. Myllykylä*
Affiliation:
VTT Technical Research Centre of Finland. P.O.Box 1000, FI-02044 VTT, Finland
M. Tanhua-Tyrkkö
Affiliation:
VTT Technical Research Centre of Finland. P.O.Box 1000, FI-02044 VTT, Finland
A. Bouchet
Affiliation:
Etudes Recherches Matériaux ERM, Centre Régional d'Innovation du Biopôle, 4 rue Carol Heitz, 86000 Poitiers, France
M. Tiljander
Affiliation:
Geological Survey of Finland, P.O. Box 96, FI-02151 Espoo, Finland
*
*E-mail: [email protected]
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Abstract

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The effects of simulant groundwater composition, pH and temperature on the dissolution and alteration of Na- and Ca-montmorillonite have been studied. Prior to the experiments, Wyoming type Na-montmorillonite, Swy-2, was purified to decrease the amount of accessory minerals. For Ca-montmorillonite experiments, the interlayer cation Na+ of purified Swy-2 was exchanged with Ca2+. The batch experiments were conducted with the purified montmorillonites in simulated fresh and saline waters at 25°C and 60°C under anaerobic conditions in an Ar atmosphere. The concentrations of Si, Al, Fe and Mg were analysed from ultra-filtered solution samples with High Resolution Inductively Coupled Plasma Mass Spectrometry (HR-ICP-MS) as a function of dissolution time. The pH evolution was also measured. The solid smectite phases were analysed with X-ray Diffraction (XRD) and Scanning Electron Microscopy (SEM). XRD analyses indicated that the nature of the smectite mineral did not change over 140 days. However, the experimental conditions, more or less, modified the structure (e.g. the layer stacking of montmorilllonite; the partial dissolution of the smectite), which cannot be detected by XRD but was evidenced by chemical data, and can be considered as a possible contributor to the stacking faults of the montmorillonite. The log rates (mol g–1 s–1), based on the dissolved amount of Si, varied between –10.64 and –12.13 depending on the experimental conditions.

Keywords

dissolutionmontmorillonitegroundwateranaerobic conditionsbentonite bufferalteration
Type
Research Article
Information
Clay Minerals , Volume 48 , Issue 2 , May 2013 , pp. 295 - 308
Creative Commons
Creative Common License - CCCreative Common License - BY
Copyright © The Mineralogical Society of Great Britain and Ireland 2013 This is an Open Access article, distributed under the terms of the Creative Commons Attribution license. (http://creativecommons.org/licenses/by/4.0/), which permits unrestricted re-use, distribution, and reproduction in any medium, provided the original work is properly cited.
Copyright
Copyright © The Mineralogical Society of Great Britain and Ireland 2013

References

Ammann, L. (2003) Cation Exchange and Adsorption on Clays and Clay Minerals. Dr. rer. nat. dissertation submitted to Faculty of Mathematics and Natural Sciences, Chistian-Albrechts-Universität.Google Scholar
Amram, K. & Ganor, J. (2005) The combined effect of pH and temperature on smectite dissolution rate under acidic conditions. Geochimica et Cosmochimica Acta, 69, 2535–2546.10.1016/j.gca.2004.10.001CrossRefGoogle Scholar
Baeyens, B. & Bradbury, M.H. (1995) A quantitative mechanistic description of Ni, Zn and Ca sorption on Na-montmorillonite. Part I: Physico-chemical characterization and titration measurements. PSI Bericht No. 95-10 and Nagra NTB 95-04, 64.Google Scholar
Bauer, A. & Berger, G. (1998) Kaolinite and smectite dissolution rate in high molar KOH solutions at 35 and 80°C. Applied Geochemistry, 13, 905–916.Google Scholar
Brady, P.V. & Walther, J.V. (1990) Kinetics of quartz dissolution at low temperatures, Chemical Geology, 82, 253–264.10.1016/0009-2541(90)90084-KGoogle Scholar
Brantley, S.L., Kubicki, J.D. & White, A.F. (2008) Kinetics of Water-Rock Interaction. Springer, New York.10.1007/978-0-387-73563-4Google Scholar
Brindley, G.W. (1980) Order-disorder in clay mineral structures. Pp. 125–195 in: Crystal Structures of Clay Minerals and their X-ray Identification (G.W. Brindley & G. Brown, editors). Monograph no. 5, Mineralogical Society, London.Google Scholar
Chipera, S.J. & Bish, D.L. (2001) Baseline studies of the Clay Minerals Society source clays: powder X-ray diffraction analyses. Clays and Clay Minerals, 49, 398–409.10.1346/CCMN.2001.0490507Google Scholar
Golubev, S.V., Bauer, A. & Pokrovsky, O.S. (2006) Effect of pH and organic ligands on the kinetics of smectite dissolution at 25°C. Geochimica et Cosmochimica Acta, 70, 4436–4451.10.1016/j.gca.2006.06.1557Google Scholar
Knauss, K.G. & Wolery, T.J. (1987) The dissolution of quartz as a function of pH and time at 70°C. Geochimica et Cosmochimica Acta, 52, 43–53.Google Scholar
Lasaga, A.C. (1998) Kinetic Theory in the Earth Sciences. Princeton Series in Geochemistry, Princeton University Press, Princeton.Google Scholar
Malmström, M., Banwart, S., Lewenhagen, J., Duro, L. & Bruno, J. (1996) The dissolution of biotite and chlorite at 25°C in the near-neutral pH region. Journal of Contaminant Hydrology, 21, 201–213.10.1016/0169-7722(95)00047-XCrossRefGoogle Scholar
Marty, N.C., Cama, J., Sato, T., Chino, D., Villiéras, F., Razafitianamaharavo, A., Brendlé, J., Giffaut, E., Soler, J. M., Gaucher, E.C. & Tournassat, C. (2011) Dissolution kinetics of synthetic Na-smectite. An integrated experimental approach, Geochimica et Cosmochimica Acta, 75, 5849–5864.Google Scholar
Moore, D.M. & Hower, A. (1986) Ordered interstratification of dehydrated and hydrated Na-smectite. Clays and Clay Minerals, 34, 379–384.10.1346/CCMN.1986.0340404Google Scholar
Moore, D.M. & Reynolds, R.C. (1989) X-ray Diffraction and the Identification and Analysis of Clay Minerals. Oxford University Press, New York, 332 pp.Google Scholar
Myllykylä, E., Tanhua-Tyrkkö, M. & Bouchet, A. (2011) Alteration and dissolution of Na-montmorillonite in simulated groundwaters. Materials Research Society Symposium Proceedings, 1475, 329–334. Materials Research Society, Buenos Aires, Argentina, 2–7 October 2011.Google Scholar
Rassineux, F, Griffault, L., Meunier, A., Berger, G., Petit, S., Vieillard, P., Zellagui, R., & Munoz, M. (2001) Expandability-layer stacking relationship during experimental alteration of a Wyoming bentonite in pH 13.5 solutions at 35 and 60°C. Clay Minerals, 35, 197–210.Google Scholar
Reynolds, R.C. (1980) Interstratified clay minerals. Pp. 249–303 in: Crystal Structures of Clay Minerals and their X-ray Identification (G.W. Brindley & G. Brown, editors). Monograph 5, Mineralogical Society, London.CrossRefGoogle Scholar
Reynolds, R.C. (1985) Description of program NEWMOD© for the calculation of the one-dimensional X-ray diffraction patterns of mixed-layered clays. Manuel d’utilisation (R.C Reynolds, editor). 8 Brook Road, Hanover, New Hampsire, 03755.Google Scholar
Rozalen, M.L., Huertas, F.J., Brady, P.V., Cama, J., Carcía-Palma, S. & Linares, J. (2008) Experimental study of the effect of pH on the kinetics of montmorillonite dissolution at 25°C. Geochimica et Cosmoschimica Acta, 72, 4224–4253.10.1016/j.gca.2008.05.065Google Scholar
Rozalen, M., Huertas, F.J. & Brady, P.V. (2009) Experimental study of the effect of pH and temperature on the kinetics of montmorillonite dissolution. Geochimica et Cosmochimica Acta, 73, 3752–3766.10.1016/j.gca.2009.03.026Google Scholar
Tournassat, C., Greneche, J-M., Tisserand, D. & Charlet, L. (2004) The titration of clay minerals: I. Discontinuous back-titration technique combined with CEC measurements. Journal of Colloid and Interface Science, 273, 224–223.10.1016/j.jcis.2003.11.021Google Scholar
Wolery, T.J. (1992) EQ3NR, A computer program for geochemical aqueous speciation – solubility calculations: theoretical manual, user's guide, and related documentation (Version 7). Lawrence Livermore National Laboratory, Livermore, CA.Google Scholar
Zysset, M. & Schindler, P.W. (1996) The proton promoted dissolution kinetics of K-montmorillonite. Geochimica et Cosmochimica Acta, 60, 921–931.10.1016/0016-7037(95)00451-3Google Scholar