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Polycation adsorption on montmorillonite: pH and T as decisive factors for the kinetics and mode of chitosan adsorption

Published online by Cambridge University Press:  09 July 2018

J.-H. An  and
S. Dultz
J.-H. An*
Affiliation:
Institute of Soil Science, Leibniz University of Hannover, Herrenhäuser Str. 2, D-30419 Hannover, Germany
S. Dultz
Affiliation:
Institute of Soil Science, Leibniz University of Hannover, Herrenhäuser Str. 2, D-30419 Hannover, Germany
*
*E-mail: [email protected]
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Abstract

Adsorption of the polycation chitosan on montmorillonite was studied at different pH values from 4.5 to 6.5 and at temperatures of 25, 50 and 75ºC. The amount of chitosan adsorbed increased with temperature, indicating that temperature is a decisive factor. At pH 5.0 and 25ºC the amount adsorbed was 1.18 molc kg–1, whereas it was 1.5 times higher (1.79 molc kg–1) at 75ºC. The uptake of chitosan increased significantly at higher pH. This can be attributed to the decrease in the degree of protonation. Surface charge and X-ray diffraction measurements indicate that most of the chitosan is adsorbed in the interlayer, where mono- and bilayer structures are formed.

The kinetics of chitosan adsorption also depend on temperature and pH. At ⩾ 50ºC, the adsorption mechanism of chitosan on montmorillonite is closest to the intraparticle diffusion model, whereas at lower temperature (25ºC) the adsorption process is closer to the pseudo-second order model. The pH of the solution affects the protonation degree of chitosan and the mode of adsorption on montmorillonite, but not the adsorption rate.

For chitosan-montmorillonite prepared at pH 5.0 and 75ºC, the effective anion exchange capacity (AEC) was found to be 80% (0.36 molc kg–1) of the calculated value. The relatively large AEC and the location of most of the anion exchange sites in the interlayer make chitosan-montmorillonite an interesting prospect as an adsorbent for water-purification procedures.

Keywords

organo-clay mineralchitosanmontmorilloniteadsorption kinetics}anion exchange capacity
Type
Research Article
Information
Clay Minerals , Volume 42 , Issue 3 , September 2007 , pp. 329 - 339
Copyright
Copyright © The Mineralogical Society of Great Britain and Ireland 2007

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References

An, J.-H. & Dultz, S. (2007) Adsorption of tannic acid on chitosan-montmorillonite as a function of pH and surface charge properties. Applied Clay Science, 36, 256–264.CrossRefGoogle Scholar
Beall, G.W. (2003) The use of organo-clays in water treatment. Applied Clay Science, 24, 11–20.Google Scholar
Böckenhoff, K. & Fischer, W.R. (2001) Determination of electrokinetic charge with a particle-charge detector, and its relationship to the total charge. Journal of Analytical Chemistry, 371, 670–674.Google Scholar
Bors, J., Dultz, S. & Riebe, B. (2000) Organophilic bentonites as adsorbents for radionuclides I. Adsorption of ionic fission products. Applied Clay Science, 16, 1–13.Google Scholar
Breen, C. (1999) The characterisation and use of polycation-exchanged bentonites. Applied Clay Science, 15, 187–219.Google Scholar
Chang, M.Y. & Juang, R.S. (2004) Adsorption of tannic acid, humic acid and dyes from water using the composite of chitosan and activated clay. Journal of Colloid and Interface Science, 278, 18–25.Google Scholar
Dambies, L., Guimon, C., Yiacoumi, S. & Guibal, E. (2001) Characterization of metal ion interactions with chitosan by X-ray photoelectron spectroscopy. Colloids and Surfaces A: Physicochemical and Engineering Aspects, 177, 203–214.Google Scholar
Darder, M., Colilla, M. & Ruiz-Hitzky, E. (2003) Biopolymer-clay nanocomposites based on chitosan intercalated in montmorillonite. Chemistry of Materials, 15, 3774–3780.Google Scholar
Denoyel, R., Durand, G., Nafuma, F. & Audebert, R. (1990) Adsorption of cationic polyelectrolytes onto montmorillonite and silica: Microcalorimetric study of their conformation. Journal of Colloid and Interface Science, 139, 281–290.Google Scholar
Döppers, L.-M., Breen, C. & Sammon, C. (2004) Diffusion of water and acetone into poly(vinyl alcohol)-clay nanocomposites using ATR-FTIR. Vibrational Spectroscopy, 35, 27–32.Google Scholar
Gecol, H., Ergican, E. & Miakatsindila, P. (2005) Biosorbent for tungsten species removal from water: Effects of co-occurring inorganic species. Journal of Colloid and Interface Science, 292, 344–353.Google Scholar
Ho, Y.S. & McKay, G. (1999) Comparative sorption kinetic studies of dyes and aromatic compound onto fly ash. Journal of Environmental Science and Health, A34, 1179–1204.Google Scholar
Ho, Y.S. & McKay, G. (2000) The kinetics of sorption of divalent metal ions onto sphagnum moss peat. Water Research, 34, 735–742.Google Scholar
Li, Z. & Bowman, R.S. (1998) Sorption of chromate and PCE by surfactant —modified clay minerals. Environmental Engineering Science, 15, 237–245.Google Scholar
Li, Y.Y., Chen, X.G., Yu, L.M., Wang, S.X., Sun, G.Z. & Zhou, H.Y. (2006) Aggregation of hydrophobically modified chitosan in solution and at the air-water interface. Journal of Applied Polymer Science, 102, 1968–1973.Google Scholar
Mortland, M.M., Shaobai, S. & Boyd, S.A. (1986) Clay-organic complexes as adsorbents for phenol and chlorophenols. Clays and Clay Minerals, 34, 581–585.Google Scholar
Müller, R.H. (1996) Zetapotential und Partikelladung in der Laborpraxis. Wissenschaftliche Verlagsgesellschaft, 254 pp.Google Scholar
Petit-Agnely, F. & Iliopoulos, I. (1999) Aggregation mechanism of amphiphilic associating polymers studied by 19F and 13C nuclear magnetic resonance. Journal of Physical Chemistry B, 103, 4803–4808.Google Scholar
Philippova, O.E., Volkov, E.V., Sitnikova, N.L. & Khokhlov, A.R. (2001) Two types of hydrophobic aggregates in aqueous solutions of chitosan and its hydrophobic derivative. Biomacromolecules, 2, 483–490.Google Scholar
Vinod, V.P. & Anirudhan, T.S. (2001) Sorption of tannic acid on zirconium pillared clay. Journal of Chemical Technology and Biotechnology, 77, 92–101.Google Scholar
Wu, F.C., Tseng, R.L. & Juang, R.S. (2000) Kinetic modeling of liquid-phase adsorption of reactive and metal ions on chitosan. Water Research, 35, 613–618.Google Scholar
Wu, F.C., Tseng, R.L. & Juang, R.S. (2001) Enhanced abilities of highly swollen chitosan beads for color removal and tyrosinase immobilization. Journal of Hazardous Materials, B81, 167–177.Google Scholar