Thermodynamics and kinetics of adsorption of Cu(II) from aqueous solutions onto a new cation exchanger derived from tamarind fruit shell
Introduction
Removal of toxic pollutants from water and wastewater is becoming an important process with the increase of industrial activities. Various heavy metal ions are discharged into water streams from large industrial sectors. Pb, Hg, Cr, Cd, Cu, Zn, and Ni are the most frequently found heavy metals in industrial wastewaters. Copper and its compounds are widely used in many industries and there are many potential sources of copper pollution. Copper contamination in water streams occurs mainly from metal cleaning and plating bath, fertilizer, refineries, paper and pulp, and wood preservatives [1]. The continued intake of copper by human beings leads to necrotic changes in the liver and kidney, mucosal irritation, wide spread capillary damage, depression, gastrointestinal irritation, and lung cancer [2]. According to Safe Drinking Water Act the permissible limit of copper in drinking water is 1.3 mg · dm−3 [3].
Adsorption is a promising technique for the removal of heavy metals from aqueous environments especially when adsorbents are derived from lignocellulosic materials [4]. Most of the lignocellulosic agricultural waste biosorbents used in sorption process are having low cost, non-hazardous, inexhaustible, highly selective for metal ions and organics and can be easily disposed by incineration. Agricultural waste products as a whole exceed 3.2 · 108 tonnes/year. A number of biomaterials including saw dust [5], olive stone waste [6], grape stalk waste [7] and tea industry waste [8] are being used as sorbents for the removal of metal ions from aqueous solutions.
Since the adsorption process is influenced by the diffusion of metal ions and the surface interaction mechanism, the presence of surface functional groups on the adsorbent plays a major role in adsorption process [9]. The adsorption capacity of these biosorbents can be enhanced by graft polymerization followed by functionalisation. Through various chemical reactions surface functional groups effective for the adsorption process can be grafted onto the biomass [10].Tamarind fruit shell or hull (TFS) is an easily available agricultural waste material. In the present work, a new cation-exchanger (TFS-CE) having carboxylate functional group at the chain end is prepared by graft copolymerization of hydroxyethylmethacrylate (HEMA) onto TFS in the presence of N,N′-methylenebisacrylamide (MBA) and it is utilized for the removal of Cu(II) ions from aqueous solutions.
Section snippets
Preparation of TFS-CE
Scheme 1 represents the general procedure adopted for the preparation of TFS-CE. Fifty grams of TFS powder was suspended in 75 cm3 distilled water containing 0.346 M MBA, 0.134 M potassium persulfate (K2S2O8) and 0.05 M sodium thiosulphate (Na2S2O3) in a glass reactor. In order to remove the dissolved oxygen, nitrogen was purged for 10 min. HEMA (3.21 M) was added into the reaction mixture and stirred vigorously at T = 343 K for 2 h. The product probably containing cross-linked homopolymer (PHEMA)
Effect of pH on Cu(II) adsorption
The pH influences the metal chemistry in solution or the protonation or deprotonation of the adsorbent. The pH dependence of equilibrium adsorption data of Cu(II) ions in solution is shown in figure 1. From the figure it may be observed that amount of Cu(II) adsorbed increases with increase in pH and reaches maximum 4.96 mg · g−1 (99.2%) and 12.24 mg · g−1(97.9%) for an initial concentration of 10 mg · dm−3 and 25 mg · dm−3, respectively, at pH 6.0. The removal of Cu(II) can be written as follows:
Summary
This preliminary study concerning the adsorption capacity of TFS-CE indicated great potential for the removal of Cu(II) from aqueous solutions. The optimum pH for maximum adsorption of Cu(II) was found to be at pH 6.0. The kinetics of adsorption follows pseudo-second-order model and the rate constant increases with increase in temperature indicating endothermic nature of adsorption. The values of Ea, ΔH#, ΔS#, and ΔG# were calculated using the Arrhenius and Eyring equations to predict the
Acknowledgements
The authors are grateful to the Professor and Head, Department of Chemistry, University of Kerala, Trivandrum for providing laboratory facilities for this work.
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