Removal of Heavy and Transition Metal Ions from Water Samples by Using Polymeric Chelating Resin

Shah et al. Int. J. Res. Chem. Environ. Vol.3 Issue 1 January 2013(163170) International Journal of Research in Chemistry and Environment Vol. 3 Issue 1 January 2013(163170) ISSN 22489649 Research Paper Removal of Heavy and Transition Metal Ions from Water Samples by Using Polymeric Chelating Resin *Shah Pathik M., Srinivasulu B., Shit Subhas C. Central Institute of Plastics Engineering & Technology, Vatva, Ahmedabad, (Gujarat), INDIA (Received 21 st September 2012, Accepted 20 th November 2012) Available online at: www.ijrce.org Abstract: A polymeric chelating resin was synthesized from Salicylic acidformaldehyde copolymerized with mcresol (SFC) in NaOH media. The polymeric structure was confirmed by Elemental analysis, FTIR and 1 HNMR spectra. The resin was highly stable in acidic and alkaline solutions and has been studied as a chelating sorbent for heavy metal ions [Pb(II) and Cd(II)] and transition metal ions [Ni(II) and Cu(II)]. Polymeric resin shows higher exchange capacity for Ni(II). The effect of concentration of electrolytes (Tartaric acid) on distribution coefficient (K d ) for metal ions has been investigated. The quantitative separation was achieved on the column of the chelating resin include Cu(II)Pb(II). The polymeric resin was utilized for column operation for separation of metal ions from industrial waste water. The developed procedure was also tested for the removal of Cd(II) and Pb(II) from natural water of Purna River nearby Navsari, Gujarat, India. Keyword: Chelating Resin, Heavy Metal, Quantitative Separation. Waste Water Treatment. Introduction The environmental contamination with heavy metals may create acute or chronic toxicity problems, which should be avoided whenever possible. Indeed, although heavy metals could be found naturally in soils, sediments, water and even in living organisms, anthropogenic releases can increase its concentration to unacceptable levels. The electroplating industries are examples of processes that may create serious problems, since their wastewaters may contain large number of heavy metals, including chromium, copper, nickel, zinc, manganese and lead. The specific contaminant addressed in this work was nickel and copper. Nickel was selected mainly due to its high concentration in electroplating effluents, significant commercial value and also based on health concerns. Lead may be regarded as a very toxic nonessential metal for microorganisms and plants. Adverse effects of lead on plants may be observed during germination processes, growth of roots, stems and leaves as well as throughout plant physiological processes such as photosynthesis, water relations and mineral nutrition. Copper is in general a transition metal of concern because of its toxicity to aquatic life. For instance, although normal growth of most plants occurs at 5 20 mg/l, they may suffer from copper deficit at concentrations below 5 mg /L or from Cu(II) toxicity at concentrations over 20 mg / L [1]. Babula et al. stressed that Cu(II) may be essential as constituent of pigments and enzymes but it becomes toxic at high concentration because of disrupting enzyme functions, replacing essential metals in pigments or producing reactive oxygen species [2]. Intended for removal and recovery of valuable metals, ion exchange has been recognized as a promising alternative technique to traditional methods of precipitation coupled with filtration. The chelating resins were commonly employed as ionexchange materials, once their ligands can selectively bind to certain metallic ions through ionic and coordinating interactions [3]. Recent studies have shown that these resins could be used for selective removal and recovery of chromium and copper. A method of separation and preconcentration for the determination of Zn, Cu, and Mn in natural water was described and real samples were studied by Farshid Ahmadi [4]. This method was based on the adsorption of Mn 2+, Cu 2+ and Zn 2+ onto 3((1HIndol3yl) (3 nitrophenol) methyl)1h indole (INMI) that is loaded onto Triton X100coated polyvinyl chloride. A new resin was synthesized with polymerization of thioureaformaldehyde. This resin was used to preconcentration of Ni(II) ions in 163

the Kan River (Tehran, Iran) [5]. It has a potential for enrichment of trace amounts of Ni(II) from large sample volumes. The aim of this article is to study the ability of polymeric chelating resin that contains hydroxyl and carboxylic acid groups as active sites. The resin was characterized by different instrumental technique. The optimum condition for the efficient sorption of metal ions [Ni(II), Cu(II),Pb(II) and Cd(II)] on polymeric resin was determined. The effect of electrolyte like tartaric acid on distribution coefficient (K d ) was investigated. The quantitative separation of Cu(II)Pb(II) was achieved on the columns of the chelating resin. The resin was used for removal of metal ions from industrial waste water [Cu(II) and Ni(II)]. The chelating resin has also been studied for recovery of Pb(II) and Cd(II) from Purna river water. Material and Methods Reagents and Solutions: Analytical reagent (AR) grade chemicals were used. Stock solutions of metal ions were prepared by dissolving appropriate amounts of metal acetate in deionized water, acidified with 5 ml of acetic acid. The working solutions of metal ions were obtained by dilution of the stock solutions with double distilled water. The solutions were adjusted to various phs using acetate buffer. The water samples from the Purna River (Navsari, Gujarat, India) was collected, acidified with 2% HNO 3 immediately, filtered and stored in the glass bottles. All solutions were standardized by the literature methods [6]. Resin Synthesis: Fine powder of salicylic acid (0.1 mole) was dissolved in 30 ml of 2 M NaOH and taken in 250 ml three necked round bottom flask. Formaldehyde (0.3 mole) and solution of mcresol (0.1 mole in 2M NaOH) was added to above solution from addition funnel dropwise at the flow rate of 2 ml/min simultaneously with constant stirring at room temperature. Then mixture was refluxed on a water bath with constant stirring at 85 ± 5 o C for 45 60 minute until a viscous solution was obtained with the formation of a jelly mass of redbrown color resin [7]. This jelly mass then dried in open to become soft solid mass. It was ground to small pieces. The resin was cured in an oven at 80 o C for 8 hour. The resin particle was washed with NaOH and DMF and finally with hot distilled water till the complete removal of monomer impurities was achieved. The yield of this resin was found to be 7580 %. The solubility tests of the resin were performed at room temperature with intermittent shaking. It was found almost insoluble in all common organic solvents like acetone, ethanol, benzene, DMF, Carbon tetrachloride, chloroform etc. and all acids and alkalies of higher strengths. The dried resin sample (SFC) was sieved to uniform particle size of 2050 mesh size. Dry resin sample was examined for Elemental and Spectral (FTIR, 1 HNMR) analysis. The resin sample was equilibrated with 2M HCI solution for 24 hours to convert it in H + form and washed 164 Shah et al. Int. J. Res. Chem. Environ. Vol.3 Issue 1 January 2013(163170) with deionized water till it was freed from chloride by testing with silver nitrate solution. The H + form of resin was used for further studies. It was necessary to evaluate ion exchange processes in terms of resin properties such as % Moisture Content, Void Volume Fraction, Sorption capacity for sodium ion and other heavy metal ions [8]. Instrumental Analysis: A Flame Atomic Absorption Spectrophotometer (AAS) (Electronic Corporation of India Ltd, Hyderabad, India, Model 4129) with an airacetylene flame (air and acetylene flow rates: 10 L/min and 2.0 L/min, respectively) was used for Atomic Absorption Spectrometric measurements. The wavelength (nm) used for monitoring Ni, Cu, Cd and Pb are 232.0, 324.8, 228.8 and 217.0 respectively. The Elemental Analysis was carried out on Elemental Analyser (Carlo Erba, model 1160). FTIR Spectra of the synthesized resin sample have been scanned in KBr pallets on FTIR Spectrophotometer (Shimadzu model8201pc). The 1 HNMR spectra was taken in DMSO d 6 solvent on BrukerDPX200 Spectrometer at 200 MHz with a sweep time of 10 min at room temperature. The internal reference used was Tetra methyl silane (TMS). A mechanical shaker equipped with incubator (Hindustan Scientific, New Delhi, India) with a speed of 200 strokes per min was used for equilibration of metal ions with chelating resin. Effect of ph on Exchange Capacity: To study the effect of ph on the metal ion uptake, it was necessary to buffer the resin and then solutions were used. Different sets of accurately weighed (0.250 g) dry resin were equilibrated with buffer solution (3.5 ph To 6.5 ph) in different glass stopper bottles for 6 h, so that resin attained desired ph value (3.5 ph To 6.5 ph). After 6 h, buffer solutions were decanted and 50 ml of 0.05M metal ion solutions of varying ph from 3.56.5 were added. Metal ion solutions were equilibrated at room temperature for 24 h with intermittent shaking. Maintain its ph by adding acid or base. After 24 h, solutions were filtered with 0.02 µm membrane filter to separate the resin and solution. From the filtrate unabsorbed metal ions were estimated by EDTA method. Exchange Capacity was determine by following equation: q e ( Co W Ce) V Where Co and Ce are the initial and equilibrium concentration of metal ions in aqueous phase respectively and V is volume of metal ion solution in ml and W is weight of resin in gram. Effect of Electrolytes Concentration on Distribution Coefficient (K d ) of Metal Ions: The dry resin sample (0.250 g) was suspended in electrolyte solution like Tartaric acid (50 ml) of different known concentrations (0.1M and 0.3 M). Tartaric acid is powerful organic chelating agent as it contains greater number of lone pair

Shah et al. Int. J. Res. Chem. Environ. Vol.3 Issue 1 January 2013(163170) of electron which helps for chelation. The ph of the suspension was adjusted to the desired value (3.0 ph to 6.0 ph) and the resin was equilibrated for 6 h. To the suspension, 2.0 ml of (5.0 mg/ml) solution of the metal ion under study was added. The ph was again adjusted to desired ph value (3.0 ph to 6.0 ph). The mixture was further equilibrated for 24 hours and then filtered. The solid was washed with water. The filtrate and washings were combined and examined for the metal ion concentration. K d { Wt.(in mg) of metal ions taken up by 1g of { Wt.( in mg) of metal ions resin } present in 1mL of resin } Metal ions Separation from Synthetic water sample: The chelating resin in H + form was equilibrated at optimized ph based on K d values and packed into a chromatographic column to form a bed of 17 cm height and 0.4 cm diameter. The superior selectivity towards multivalent cations exhibited by chelating resin has been demonstrated in column experiments by using K d value. An ideal situation would be such that one K d value is ten times greater than the K d value for other ion, while the other approaches zero. The first eluting fraction of tartaric acid carries one metal ion, which has a smaller K d value. The second metal ion can be eluted by changing the tartaric acid concentration to a level that has a lowest K d value for second metal ion. Mixtures of metal ions (10 mg of each per 20 ml) at optimized ph based on K d were passed through the column at a flow rate of 0.5 ml/min. The chelated metal ions were eluted using tartaric acid. During elution, a flow rate of 0.5 ml/min was maintained. Industrial Wastewater Treatment: The combined wastewater sample to be studied was collected from electroplating unit situated at Valsad, M/s Excell Shine Private Limited. It has four major sections: (1) Electro less nickel plating section (2) Copper plating section (3) Chrome plating section (4) Other pretreating section. Chromatographic column separation was performed for the random sample collected. The characteristic of electroplating industries wastewater is shown in Table 1. 25ml of this industrial effluent was taken for the separation of its major content Cu(II) and Ni(II) by SFC resin. Recovery of Heavy Metal Ions from Purna River Water: 20 liter of Purna River water sample from Navsari city was collected in polythene container. Several water samples were analyzed to contain Cd(II) (0.01 to 0.17 ppm) and Pb(II) (0.01 to 0.4 ppm), which is higher than the Indian Standard Desirable Limits. It exhibits higher concentration of these metal ions at Jalalpor and Weircum Causeway. This may be due to industrial effluent of sewage waste in the river water. A one liter water sample was recycled through the resin columns for the preconcentration of these metal ions at a flow rate of 1 ml/min. Results and Discussion PhysicoChemical Properties: Water content of resin is the ability of resin to hold the moisture. The moisture content of a resin furnishes a measure of its water loading capacity or its swelling capacity. Moisture content depends on many factors such as, on the composition of the resin matrix, the degree of crosslinking or the nature of the active groups and the ionic form of resins. When resin sample was heated up to 100 o C, initially they lose some weight, soon weight is regained after exposing it in the air for 24 h. This indicates that resin sample contain percentage of moisture. The percentage of moisture content of synthesized resin was 10.2. The value were calculated in hydrogen ion form and water associated with 1.0 g of dry resin. It has been observed that this resin has low range of percentage moisture content compared to the commercial resins. The amount of cross linking in the bead has an impact on the moisture content of the bead and the moisture content in turn has an impact on the selectivity. A bead with high moisture content has a high porosity and the active groups are spaced further apart from each other. True density of synthesized resin was 1.19 g/cm 3. The true density of commercial resins generally lies between 1.1g/cm 3 to 1.7 g/cm 3. To avoid the floating of resin particles, true density must be more than one. Floating of resin particles is undesirable in chromatographic study, as it hampers formation of compact column. Optimum density and uniform particle size gives perfect column packing and performance of the column. The measurement of column density or apparent density was necessary because commercially it was sold on volume basis and packed on weight basis. Apparent density of synthesized resin was 0.74, which is comparable to the density of commercial resins. It may be because of charge in polymeric matrix, different functional group and the method of synthesis. The apparent density parameter gives an idea of probable length of the packed column for an ideal column chromatography study. The value of void volume fraction of resin was 0.37. The appreciable values of void volume fraction help the diffusion of the exchangeable ion on the resin and hence increase the rate of exchange of ions. Minimum essential void volume provides better diffusion of exchangeable ions and thus feasibility of column operation. The sodium exchange capacity of SFC resin was 7.2 mmol /g. 165

Shah et al. Int. J. Res. Chem. Environ. Vol.3 Issue 1 January 2013(163170) S. No. Parameters ( in ppm) Table 1 The characteristic of electroplating industries wastewater General composite sample analysis in South Gujarat region Average combined wastewater from M/s Excell Shine Private Ltd. 1 Copper [as Cu(II) ] 100300 348 2 Nickel [as Ni(II) ] 100450 300 3 Iron [as Fe(II) ] 15.0 4 Sulphate [as SO 2 4 ] 5500 5 Nitrate [as NO 1 3 ] 30 6 Chromium[as Cr +6 ] 0.550 90 Table 2 Elemental Analysis %C %H %N Calculated 64.68 4.68 Nil Founded 65.02 4.70 Nil Table 3 FTIR spectrum data of SFC resin Vibrational Mode Reported wave number (cm 1 ) Observed wave number (cm 1 ) υ(oh) of phenolic and carboxylic group 3100 3500 3369 υ(ch) of methylene group 28503000 2919 υ(c=o) of aromatic acid group 16301820 1703 δ (CH) of ArCH 3. 15001350 1375 υ (CO) of phenol. 10001250 1212 Tetrasubstituted benzene ring. 558 900 772 CH 3 HO O OH + HCHO + HO Condensation in 2M NaOH CH. 3 CH 2. OH HO HO O Scheme1 Synthesis of SFC resin n 166

Shah et al. Int. J. Res. Chem. Environ. Vol.3 Issue 1 January 2013(163170) Instrumental Analysis: The result of the Elemental Analysis was in good agreement with calculated values of %C, %H and %N, which is shown in Table2. The data of FTIR of SFC copolymer resin is presented in Table3. FTIR of SFC resin shows peak at 2929 cm 1, which indicates presence of methylene polymeric linkage between monomers. The values of Elemental Analysis and FTIR confirm the proposed structures of the resin presented in Scheme1. The polymeric structure was also confirmed by 1 HNMR. The peak observed at 11.4 ppm was due to the H of carboxylic acid group (ArCOOH).The peak observed at 3.4 ppm was due to the 2H of methylene group of polymeric linkage (ArCH 2 Ar) [9]. Here the peak observed at 6.5 ppm to 8.4 ppm was due to the H of benzene ring. The sharp singlet peak at 4.5 ppm was due to the H of phenolic OH group. The sharp singlet peak was also observed at 2.2 ppm was due to the H of ArCH 3. This is shown in Figure1. Effect of ph on Exchange Capacity: From Figure 2, it reveals that, the maximum exchange capacity for Ni(II) and Cd(II) was at ph 6.0. For Cu (II), it was at ph 5.5 and for Pb (II) was at ph 4.5. The selectivity order for metal ions is Pb (II) < Cd (II) < Cu (II) < Ni (II). A polymeric chelating resin, poly (2thiozylmethacrylamide codivinylbenzene co 2acrylamido 2methyl 1 propanesulfonic acid) also gives this type of selectivity order for metal ions [10]. The chelating resin containing nitrosocatechol [11] show different results. The maximum exchange capacity for Cd(II) was at 4.0 ph and for Pb(II) it was at 6.0 ph. The SFC resin show low exchange capacity for heavy metals as compared to other metal ions under study. The transition elements Cd (II) and Pb (II) of 4d series metal ions show less capacity. It is because of having greater hydrated ion radius than 3d series transition metal ions [Cu (II) and Ni (II)] under study. This will results in electrostatic attraction between the metal and coordinating group, lower the complex stability and hence lower the capacity [7]. Figure 1: 1 HNMR of SFC 167 Figure 2: Effect of ph on SFC resin. The polymer surface chemistry as well as the solution chemistry of these metal ions was ph dependent. The amount of absorbed metal ions depends on the species stability in solution phase and on the adsorbent s absorbing properties. Changes in ph were known to affect the adsorbent s surface charge and the adsorbent s degree of ionization and speciation [12]. The results SFC resin show that the uptake of metal ions was increased with increase in ph up to a certain value and thereafter it decreased. From the nature of the trend observed indicates that the cation exchange behavior of this resin was similar to acidic cation exchangers. As in acidic ion exchanger, the exchange capacity was ph dependent. The exchange capacity of resin for different metal ions varies due to different tendency of chelate formation at different ph. This can be related to the difference in ion stability of metal complexes formed with resin. An increase in ph increases the negatively charged nature of the sorbent surface. This leads to an increase in the electrostatic attraction between positively charged metal ions and negatively charged sorbent and results in increase in the

% Metal Elution Shah et al. Int. J. Res. Chem. Environ. Vol.3 Issue 1 January 2013(163170) uptake of metal ions. The decrease in the removal of metal ions at lower ph is due to the higher concentration of H + ions present in the reaction mixture which compete with the metal ions for the sorption sites on the sorbent surface. Meanwhile the observed decrease in sorption at higher ph was due to the formation of insoluble hydroxy complexes of the metal ions. SFC chelating resin was more effective than complexing agent like N, Nbis (carboxymethyl) glutamic acid because they were difficult to reuse [13]. Effect of Electrolytes Concentration on Distribution Coefficient (K d ) of Metal Ions: The distribution coefficient (K d ) of metal ions was function of concentration of different electrolyte solution. The distribution coefficient was determined by the batch equilibrium method. Electrolytes of different concentration at optimum ph were used as equilibrium media for different systems of metal ions. During exchange of metal ions in the presence of electrolyte solution the difference in the distribution coefficient values was caused by the competition between metal ions and counter ions from electrolyte solution for the available exchange sites. To study the effect of electrolyte concentration on distribution coefficients of Ni(II), Cu(II), Cd(II) and Pb(II) ion, 0.1 to 0.3 M solutions of tartaric acid, was used. The result is given in Table 4. Metal ion Table 4 K d values of metal ions on SFC resin Tartaric acid Conc. (M) Ni(II) 0.1 0.3 Cu(II) 0.1 0.3 Cd(II) 0.1 0.3 Pb(II) 0.1 0.3 K d values at different ph 3.0 3.5 4.0 5.0 6.0 245 480 225 55 3 302 145 6 72 25 106 170 45 43 72 121 177 14 72 105 190 22 300 42 70 3 45 The metal ion exchange takes place due to the chelation with the carboxylic and phenolic group in the resin whereas the electrolyte used just gets absorbed in the resin. The electrolyte exclusion was more efficient with counter ions of low valency and coions of high valency. The synthesized SFC resin exhibit lower values for Pb(II). This may be explained on the basis of stability constant or difference in energy of the complexes according to Irving and Williams [14]. The value of distribution ratio for given concentration of electrolytes at optimum ph depends upon the nature and the stability of a chelate formation for particular metal ion. To achieve more clean separation of heavy metal ions in short time with practical elution volume, maximum (K d ) value difference was selected for optimized conditions of chromatography [15]. 168 Metal ions Separation from Synthetic water sample: Separation of Cu (II) from Pb(II) was performed, at initial ph 4.0 by selective elution of Cu(II) with 0.3 M tartaric acid solution and Pb(II) with 0.1 M tartaric acid solution at ph 3.0, which is shown in Figure 3. The elution percentage of Cu(II) and Pb(II) was found to be 70% and 85% respectively. A comparative result was found by polymeric chelating gel resin [poly (MelamineformaldehydeNTA)] which was used for removal of Cu(II) from synthetic water sample [16]. Purolite C100 [17] was applying for quantitative separation of Pb(II) from a synthetic binary mixtures using ammonium acetate as eluting agent. This eluting agent shows good elute for Pb(II) but fails to elute the other cations while for SFC resin, tartaric acid was more effective eluting agent for Pb(II) as well as Cd(II). 40 35 30 25 20 15 10 5 0 Cu(II) 0.3M,4.0 ph Pb(II) 0.1M,3.0 ph 0 10 20 30 40 50 60 ml of Eluate Figure 3: Separation of Cu(II) and Pb(II) on SFC resin. Figure 4: Separation of Cu(II) from Ni(II) of industrial effluent on SFC resin

Shah et al. Int. J. Res. Chem. Environ. Vol.3 Issue 1 January 2013(163170) Industrial wastewater treatment: Cu(II) was eluted by 0.3M tartaric acid at ph3.0 and Ni(II) eluted by 0.3M tartaric acid at ph6.0, which is shown in Figure 4. No cross contamination was observed during the separation. The recovery of Cu(II) and Ni(II) was 68 % and 55 % respectively. The lower recovery may be due to existence of co ions. Modified Duolite XAD761 [18] resin show higher recovery of Ni(II) from synthetic mixture in presence of co ions. Recovery for Heavy Metal Ions from Purna River Water: To verify the applicability of the present chelating resin using preconcentration of trace metal ions like Cd(II) and Pb(II) from river water sample, the extraction and elution of metal ions was studied. The metal ion concentration of Cd(II) and Pb(II), in river water and after preconcentration was determined by Atomic Absorption Spectroscopy. The recovery of heavy metal ion from column was carried out using 2M HCl solution. The recovery of Cd(II) and Pb(II) ions was 82.47 % and 80.11 %. The results indicate that the extraction and elution of Cd(II) and Pb(II) was little affected by the coexistence of salt matrices. A chelating resin of polystyrene divinylbenzene resin functionalized by 1(2pyridylazo) 2 naphtol (PSDVBPAN) shows higher recovery of Cd(II) from river water samples collected from Citarum River, West Java, Indonesia.[19] Conclusion The condensation polymeric resin SFC was prepared from salicylic acid and mcresol with formaldehyde in alkaline medium. The hydrogen form of the prepared resin showed a good adsorption affinity towards various heavy and transition metal ions. The uptake capacity of metal ions by the resin was carried out by the batch equilibrium technique. The uptake capacities of metal ions by the copolymer resin were ph dependent. The maximum adsorption capacity of the resin followed the order Pb(II) < Cd(II) < Cu(II) < Ni(II). This order was related to the stability of complex formation between carboxylic acid and phenolic active sites and metal ions. The resin was describe by, (i) relative better uptake values of the resin towards metal ions, (ii) easy separation from the electrolyte medium. (iii) Higher stability in acidic and basic media and easy of regeneration with higher efficiency up to 90%. All of the above characteristics make this resin promising in the field of drinking water as well as wastewater treatment. References 1. He Z. L, Yang X. E, and Stoffella P. J. Trace elements in agro ecosystems and impacts on the environment. J. Trace Elem. Med. Biol. 19(23), 125140 (2005) 2. Babula P., Adam V., Opatrilova R., Zehnalek J., Havel L., and Kizek R. Uncommon heavy metals, metalloids and their plant toxicity: a review, Environ. Chem. Letter. 6(4),189213 (2008) 3. Popat, K.M., Anand. P.S. and Dasare. B.D. Calcium ion uptake by porous condensate aminocarboxylic type ionexchanger based on copolymer of mphenylene diglycine dihydrochloride paraformaldehyde, Journal of Polymer Materials.8, 279282 (1991) 4. Farshid A., Khodabakhsh N., Ebrahim N., and Azadeh K. PVC Coated with an Indole Derivative Loaded Triton X100: a New Sorbent for Cu, Zn and Mn Ions. The Arabian Journal for Science and Engineering. 36(1), 4756 (2011) 5. Homayon A. P., Amir A.M.S., Mehrnaz B., and Elham M. Determination and preconcentration of nickel in water with flame atomic absorption spectrometry by thiourea formaldehyde as chelating resin, The Arabian Journal for Science and Engineering, 35(2A),149160 (2010) 6. Vogel S. Textbook of Qualitative Chemical Analysis. 6 th edition Cambridge University Press, Cambridge (2009) 7. Shah P. M., Shah B. A. and Shah A. V. Selective Sorption of Heavy Metal Ions from Aqueous Solutions Using mcresol Based Chelating Resin and Its Analytical Applications. Iran. J. Chem. Chem. Eng. 29(2), 4958 (2010) 8. Kunin R. Ion Exchange Resin. Wiley London (1958) 9. Shah B. A., Shah A. V. and Patel N. B. A Benign Approach of Microwave Assisted Synthesis of Co polymeric Resin with Improved Thermal, Spectral and Ionexchange Properties. Iranian Polymer Journal. 17(1), 317 (2008) 10. Turan S., Tokalıoğlu Ş., Şahan A. and Soykan C. Synthesis, characterization and application of a chelating resin for solid phase extraction of some trace metal ions from water, sediment and tea sample. Reactive and Functional Polymers. 72(10), 722728 (2012) 11. Pandey S.S and Thakker N.V. Synthesis characterization and applications of new chelating resin containing nitrosocatechol. Journal of Scientific and Industrial Research. 63,682688 (2004) 12. Shah P. M., Shah B. A. and Shah A. V. Metal Ions Uptake By Chelating Resin Derived From O Substituted Benzoic Acid And Its Synthesis, Characterization And Properties. Macromolecular Symposia. 274(1), 8190 (2008) 13. Dorota K. The effect of the novel complexing agent in removal of heavy metal ions 169

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