Hostname: page-component-78c5997874-dh8gc Total loading time: 0 Render date: 2024-11-05T08:30:57.788Z Has data issue: false hasContentIssue false

Adsorption of Cr(VI) and As(V) on Chitosan-Montmorillonite: Selectivity and pH Dependence

Published online by Cambridge University Press:  01 January 2024

Jong-Hyok An
Affiliation:
Institute of Soil Science, Leibniz University of Hannover, Herrenhäuser Str. 2, D-30419 Hannover, Germany
Stefan Dultz*
Affiliation:
Institute of Soil Science, Leibniz University of Hannover, Herrenhäuser Str. 2, D-30419 Hannover, Germany
*
* E-mail address of corresponding author: [email protected]
Rights & Permissions [Opens in a new window]

Abstract

Core share and HTML view are not available for this content. However, as you have access to this content, a full PDF is available via the ‘Save PDF’ action button.

Montmorillonite modified with the cationic biopolymer, chitosan, has, in weak acidic solutions, protonated amine groups which act as anion-adsorption sites. Due to the specific surroundings of the adsorption sites and diffusion paths in the interlayer of chitosan-montmorillonite, preferential adsorption of certain anions is likely. In the present study, the adsorption properties for the inorganic anions Cr(VI) and As(V) were determined, taking into account solution pH and competitive adsorption in the presence of Cl and SO42−${\rm{SO}}_4^{2 - }$. Chitosan-montmorillonite was prepared by adding an amount of chitosan equivalent to 500% of the cation exchange capacity (CEC) at pH 5 and 75°C. The resulting anion exchange capacity was ∼0.34 molc/kg. The adsorption properties for As(V) and Cr(VI) were determined with the batch technique at pH 3 to 9. Adsorption isotherms were fitted to the Langmuir and Dubinin-Radushkevich equations and judged quantitatively by the correlation coefficient. To describe the competitive adsorption, the selectivity (S) was determined by the ratio of amounts of anions A and B adsorbed (qA/qB) in a binary system. The ionic species adsorbed, i.e. either Cr(VI) or As(V), depended on the pH, as did the degree of protonation of the amine groups, and this played a decisive role in the amount of anions adsorbed. The maximum amount of Cr(VI) adsorbed was 180 mmol/kg at pH 3.5, whereas for As(V) it was 120 mmol/kg at pH 4.0 to 5.0. The adsorption process of Cr(VI) and As(V) fit well to the Langmuir isotherm. By increasing the concentration of the competitive anion, Cl, in solution, the amount of Cr(VI) and As(V) adsorbed remained almostconstant, whereas SO42−${\rm{SO}}_4^{2 - }$ had a more pronounced competitive effect. At concentration ratios of 0.5 and 1 for SO42−${\rm{SO}}_4^{2 - }$ to Cr(VI) and As(V), respectively, the sorption capacity decreased by 10 and 25%, respectively. The sequence of the selectivity was: Cr(VI)>SO42−>As(V)>Cl−${\rm{Cr}}\left( {{\rm{VI}}} \right) > {\rm{SO}}_4^{2 - } > {\rm{As}}\left( {\rm{V}} \right) > {\rm{C}}{{\rm{l}}^ - }$. Chitosan-montmorillonite showed a high selectivity for Cr(VI), which adsorbed chemically. Despite the lower affinity for As(V) and physical adsorption, the adsorption capacity was relatively high.

Type
Article
Copyright
Copyright © The Clay Minerals Society 2009

References

An, J.-H. and Dultz, S., 2007 Adsorption of tannic acid on chitosan-montmorillonite as a function of pH and surface charge properties Applied Clay Science 36 256264 10.1016/j.clay.2006.11.001.CrossRefGoogle Scholar
An, J.-H. and Dultz, S., 2007 Polycation adsorption on montmorillonite: pH and T as decisive factors for the kinetics and mode of chitosan adsorption Clay Minerals 42 329340 10.1180/claymin.2007.042.3.06.CrossRefGoogle Scholar
Beall, G.W., 2003 The use of organo-clays in water treatment Applied Clay Science 24 1120 10.1016/j.clay.2003.07.006.CrossRefGoogle Scholar
Bhakat, P.B. Gupta, A.K. Ayoob, S. and Kundu, S., 2006 Investigation on arsenic (V) removal by modified calcined bauxite Colloids and Surfaces A 281 237245 10.1016/j.colsurfa.2006.02.045.CrossRefGoogle Scholar
Böckenhoff, K. and Fischer, W.R., 2001 Determination of electrokinetic charge with a particle-charge detector, and its relation to the total charge Fresenius Journal of Analytical Chemistry 371 670674 10.1007/s002160100897.CrossRefGoogle Scholar
Bors, J. Dultz, S. and Riebe, B., 2000 Organophilic bentonites as adsorbents for radionuclides I. Adsorption of ionic fission products Applied Clay Science 16 113 10.1016/S0169-1317(99)00041-1.CrossRefGoogle Scholar
Chakraborty, S. Wolthers, M. Chatterjee, D. and Charlet, L., 2007 Adsorption of arsenite and arsenate onto muscovite and biotite mica Journal of Colloid and Interface Science 309 392401 10.1016/j.jcis.2006.10.014.CrossRefGoogle ScholarPubMed
Chang, M.Y. and 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 1825 10.1016/j.jcis.2004.05.029.CrossRefGoogle ScholarPubMed
Darder, M. Colilla, M. and Ruiz-Hitzky, E., 2003 Biopolymer-clay nanocomposites based on chitosan intercalated in montmorillonite Chemistry of Materials 15 37743780 10.1021/cm0343047.CrossRefGoogle Scholar
David, K. Patricia, P. and Bomumil, V., 1998 Removal of trivalent and hexavalent chromium by seaweed biosorbent Environmental Science & Technology 32 26932698 10.1021/es971073u.Google Scholar
Gecol, H. Ergican, E. and Miakatsindila, P., 2005 Biosorbent for tungsten species removal from water: Effects of co-occurring inorganic species Journal of Colloid and Interface Science 292 344353 10.1016/j.jcis.2005.06.016.CrossRefGoogle ScholarPubMed
Inglezakis, V.J. Loizidou, M.D. and Grigoropoulou, H.P., 2003 Ion exchange of Pb2+, Cu2+, Fe3+, and Cr3+ on natural clinoptilolite: selectivity determination and influence of acidity on metal uptake Journal of Colloid and Interface Science 261 4954 10.1016/S0021-9797(02)00244-8.CrossRefGoogle ScholarPubMed
Karahan, S. and Yurdakoç, M., 2006 Removal of boron from aqueous solution by clays and modified clays Journal of Colloid and Interface Science 293 3642 10.1016/j.jcis.2005.06.048.CrossRefGoogle Scholar
Krishna, B.S. Murty, D.S.R. and Jai Prakash, B.S., 2001 Surfactant-modified clay as adsorbent for chromate Applied Clay Science 20 6571 10.1016/S0169-1317(01)00039-4.CrossRefGoogle Scholar
Kundu, S. and Gupta, A.K., 2007 Adsorption characteristics of As (III) from aqueous solution on iron oxide coated cement(IOCC) Journal of Hazardous Materials 142 97104 10.1016/j.jhazmat.2006.07.059.CrossRefGoogle ScholarPubMed
Li, Y.H. Willms, C.A. and Kniola, K., 2003 Removal of anionic contaminants using surfactant-modified palygorskite and sepiolite Clays and Clay Minerals 51 445451 10.1346/CCMN.2003.0510411.CrossRefGoogle Scholar
Li, Z.H. and Bowman, R.S., 1998 Sorption of chromate and PCE by surfactant-modified clay minerals Environmental Engineering Science 15 237245 10.1089/ees.1998.15.237.CrossRefGoogle Scholar
Li, Z. and Zou, Y., 1999 A comparison of chromate analyses by AA, UV—Vis spectrophotometric, and HPLC methods Advances in Environmental Research 3 125131.Google Scholar
Lin, T.F. Liu, C.C. and Hsieh, W.H., 2006 Adsorption kinetics and equilibrium of arsenic onto an iron-based adsorbentand an ion exchange resin Water Science & Technology: Water Supply 6 201207.Google Scholar
Lv, L. Hou, M.P. Su, F. and Zhao, X.S., 2005 Competitive adsorption of Pb2+, Cu2+ and Cd2+ ions on microporous titanosilicate ETS-10 Journal of Colloid and Interface Science 287 178184 10.1016/j.jcis.2005.01.073.CrossRefGoogle ScholarPubMed
Manning, B.A. and Goldberg, S., 1996 Modeling arsenate competitive adsorption on kaolinite, montmorillonite and illite Clays and Clay Minerals 44 5 10.1346/CCMN.1996.0440504 609–623.CrossRefGoogle Scholar
Masscheleyn, P.H. Delaune, R.D. Jr. and Patrick, W.H., 1991 Effect of redox potential and pH on arsenic speciation and solubility in a contaminated soil Environmental Science & Technology 25 14141419 10.1021/es00020a008.CrossRefGoogle Scholar
Meleshyn, A. and Bunnenberg, C., 2006 Interlayer expansion and mechanisms of anion sorption of Na-montmorillonite modified by cetylpyridinium chloride: A Monte Carlo study Journal of Physical Chemistry B 110 22712277 10.1021/jp056178v.CrossRefGoogle ScholarPubMed
Mortland, M.M. Shaobai, S. and Boyd, S.A., 1986 Clay-organic complexes as adsorbents for phenol and chlorophenols Clays and Clay Minerals 34 581585 10.1346/CCMN.1986.0340512.CrossRefGoogle Scholar
Payne, K.B. and Abdel-Fattah, T.M., 2005 Adsorption of arsenate and arsenite by iron-treated activated carbon and zeolites: Effects of pH, temperature, and ionic strength Journal of Environmental Science and Health, Part A Toxic/Hazardous Substances and Environmental Engineering 40 723749 10.1081/ESE-200048254.Google ScholarPubMed
Saeed, M.M., 2003 Adsorption profile and thermodynamic parameters of the preconcentration of Eu(III) on 2-thenoyl-trifluoroacetone loaded polyurethane(PUR) foam Journal of Radioanalytical and Nuclear Chemistry 256 7380 10.1023/A:1023300109423.CrossRefGoogle Scholar
Seki, H. Suzuki, A. and Maruyama, H., 2005 Biosorption of chromium(VI) and arsenic(V) onto methylated yeast biomass Journal of Colloid and Interface Science 281 261266 10.1016/j.jcis.2004.08.167.CrossRefGoogle ScholarPubMed
Zachara, J.M. Cowan, C.E. Schmidt, R.L. and Ainsworth, C.C., 1988 Chromate adsorption by kaolinite Clays and Clay Minerals 36 317326 10.1346/CCMN.1988.0360405.CrossRefGoogle Scholar