Selective Cu(II) Adsorption from Aqueous Solutions Including Cu(II), Co(II), and Ni(II) by Modified Acrylic Acid Grafted PET Film

Rahman, Nazia; Sato, Nobuhiro; Yoshioka, Satoru; Sugiyama, Masaaki; Okabe, Hirotaka; Hara, Kazuhiro

doi:https://doi.org/10.1155/2013/536314

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Research Article | Open Access

Volume 2013 | Article ID 536314 | https://doi.org/10.1155/2013/536314

Selective Cu(II) Adsorption from Aqueous Solutions Including Cu(II), Co(II), and Ni(II) by Modified Acrylic Acid Grafted PET Film

Nazia Rahman,¹Nobuhiro Sato,²Satoru Yoshioka,¹Masaaki Sugiyama,²Hirotaka Okabe,¹and Kazuhiro Hara¹

Academic Editor: S. Ifuku, W. S. Chow, M. Sanopoulou, X. Colin

Received12 Jun 2013

Accepted05 Jul 2013

Published29 Jul 2013

Abstract

Acrylic acid (AAc) grafted polyethylene terephthalate (PET) films were prepared by γ irradiation. The graft films showed little metal ion adsorption due to compact structure of the graft chains as shown by the scanning electron microscopy (SEM) images which restricted the access of metal ions to the functional groups. Therefore, the graft films were modified with KOH treatment for expansion of the graft chains to facilitate the access of metal ions to the functional groups. The modified films were used to study the selective Cu²⁺ adsorption from aqueous solution containing Cu²⁺, Co²⁺, and Ni²⁺. Langmuir and Freundlich isotherm models were used for interpretation of selective equilibrium adsorption data and Langmuir model showed better fitting with experimental data. Again pseudo-first-order and pseudo-second-order equations were used for interpretation of selective kinetic adsorption data and pseudo-second-order equation showed better prediction of experimental data. The adsorbent film showed high selectivity towards Cu²⁺ in presence of Cu²⁺, Co²⁺, and Ni²⁺ in the pH range of 1.5 to 4.5. Desorption and reuse of the adsorbent film were also studied which indicated that the film can be used repeatedly for selective Cu²⁺ sorption from aqueous solution.

1. Introduction

In recent years, heavy metals have received much public attention as potential hazards for human life and health ignited by the well-known environmental destruction cases: Minamata disease (organic mercury poisoning) and itai-itai disease (cadmium poisoning) and the stricter environmental regulations on the discharge of heavy metals make it necessary to develop efficient and low cost technologies for their removal [1]. About heavy metal pollution it should be also realized that to prevent heavy metal poisoning, immediate detoxification of heavy-metal wastewater through appropriate treatment is essential. Because, unlike many organic pollutants, heavy metals are not decomposed by microbiological activity, rather heavy metals can be enriched by organisms and the type of bonding can be converted to more poisonous metal-organic complexes and the polluted areas can become widened by diffusion in the environment. But the conventional methods for removal of hazardous metal ions from wastewater such as precipitation, ion exchange, activated carbon adsorption, and electrolytic method have limitations like high cost, low removal rate or difficulty for regeneration, and reuse. Therefore, many researches focused on the study of alternative low-cost-effective adsorbents from sawdust [2], sporopollenin [3, 4], chitosan [5], peat [6], cellulose [7], and clay mineral [8].

One of the new developments in the field of heavy metal adsorption is the use of functional monomer grafted synthetic polymers as adsorbent. Attracting with the excellent chemical and thermal stability and mechanical properties of PET, adsorbents prepared by grafting of various monomers on PET fibers [9–17] and films [18] have been investigated for the adsorption of hazardous heavy metal ion from water which demonstrated good potential of PET-based adsorbents in heavy metal removal. However, most of the previous studies on PET-based adsorbents focused on metal ion adsorption from single metal solution while less results appeared in the literature on metal ion adsorption from multimetal solution which is important for separation of one metal ion from wastewater containing other metal ions. Therefore, we are interested in selective metal ion adsorption from multi metal solution. In the present work, we prepared AAc grafted PET films by irradiation. The graft films showed little metal ion adsorption due to compact structure of the graft chains. Therefore, the graft films were modified with KOH treatment for expansion of the graft chains to increase the metal ion adsorption. The modified films were used to study the potential of selective Cu²⁺ adsorption from aqueous solution containing Cu²⁺, Co²⁺, and Ni²⁺ focusing with the four main objectives: characterization of modified AAc grafted PET films by FTIR and SEM, studying the equilibrium adsorption isotherm of selective Cu²⁺ adsorption from ternary metal solutions of Cu²⁺, Co²⁺, and Ni²⁺ and use of Langmuir and Freundlich isotherm models for interpretation of equilibrium adsorption data, studying the kinetic of selective Cu²⁺ adsorption from ternary metal solutions of Cu²⁺, Co²⁺, and Ni²⁺ and use of pseudo-first-order and pseudo-second-order equations for interpretation of adsorption kinetic data, and studying the desorption of metal ions from the film and reuse of the film.

2. Experimental

2.1. Materials and Reagents

Commercial PET films (Teijin DuPont films, G2) of thickness 50 μm were kindly provided by Teijin Co., Ltd. These films were cut into small pieces (3.5 × 1.5 cm²), washed with acetone, and dried in vacuum oven before use. AAc and FeCl₃ were procured from Sigma-Aldrich. KOH was supplied by Wako pure chemical industries Ltd. Cobalt(II) chloride, nickel(II) chloride, and copper(II) chloride (anhydrous, Chameleon reagent), and cobalt, nickel and copper standard solutions (Fluka) were used as a source of the adsorbate and for the calibration of metal ion concentrations, respectively.

2.2. Instrument and Apparatus

The PET films were analyzed by a Fourier transform infrared (FTIR) spectrophotometer, Jasco FTIR 620 in the wavenumber range 400–4000 cm⁻¹ to investigate the chemical and/or physical interactions. Scanning electron microscopy (SEM) image observations of the carbon coated PET films were performed using Zeiss Ultra-55 SEM operated at 7–10 keV. The metal-ion concentrations in the solutions were analyzed by an inductively coupled plasma mass spectrometer, Agilent7700 Series ICP-MS.

2.3. Grafting of AAc onto the PET Films by Gamma Radiation

The dry PET films weighing were taken into glass bottles containing different concentrations (20–40 wt%) of AAc aqueous solutions. FeCl₃ at a constant concentration (1 wt%) was added to the AAc solutions to minimize homopolymer formation. The contents of the glass bottles were then irradiated with different doses (20–100 kGy) of rays with a dose rate of 1.0 kGy/h in air (-ray irradiation of the PET films was carried out at the ⁶⁰Co -ray irradiation facility of Research Reactor Institute, Kyoto University). The obtained grafted films were washed in distilled water at 60°C for 24 h to remove the homopolymers. Then the films were dried in a vacuum oven at 60°C for 24 h and were weighed . The graft yield was determined by the percent increase in the weight as follows.

Graft yield

2.4. KOH Treatment of the AAc Grafted Film

The AAc grafted films with 40% graft yield (obtained at 40% AAc concentration and 100 kGy dose) were modified by treatment with 2.5% KOH for 2 min at 25°C.

2.5. Metal Ion Adsorption by the Modified AAc Grafted PET Film

The modified AAc grafted films of 60 mg were soaked into the 10 mL aqueous solutions including of Cu(II), Ni(II), and Co(II) at a definite metal ion concentration and pH for 60 min at room temperature (25°C). pH of the solutions was adjusted using HCl and NaOH solution. Metal loaded films were washed and dried. The metal-ion concentrations of the solutions were analyzed by ICP-MS.

2.6. Determination of Metal Ion Uptake Capacity

The metal ion uptake capacity of the film was calculated as follows: where is the adsorption amount (mg/g), the weight of the film (g), the volume of solution (L), and and are the concentrations (mg/L) of metal ion before and after adsorption, respectively.

2.7. Desorption of Metal Ions

The desorption of Cu(II), Ni(II), and Co(II) ions from the adsorbent films was carried out by the treatment with 2 M aqueous solution of HCl for 30 min. The percent of desorption was calculated using the following equation.

3. Results and Discussion

3.1. Preparation and Characterization of the Adsorbent Film

Grafting of AAc onto PET films was carried out by irradiation. AAc grafting on PET film might have followed a free radical mechanism where at first primary free radical is formed on PET backbone initiated by ray which then reacts with monomer to form graft growing chain and finally the graft copolymer is formed by a termination reaction [19]. The prepared AAc grafted films (G-40%) were modified by treatment with KOH which increased the metal ion adsorption capacity of the films largely, almost 10 times than the AAc grafted films. The adsorption capacity of Cu²⁺, Co²⁺, and Ni²⁺ ions obtained in the present study together with that reported in previous studies are presented in Table 1. The modified AAc grafted PET film after adsorption of Cu²⁺, Co²⁺, and Ni²⁺ ions are shown in Figure 1.

To understand the change of the PET film after AAc grafting and KOH treatment, the IR spectra of the films were determined. IR spectrum of the PET film (Figure 2(a)) represented the peaks characteristic for poly(ethylene terephthalate) chemical structure (absorption peak for OH stretching at 3430 cm⁻¹, aromatic C–H stretching at 3054 cm⁻¹, aliphatic C–H stretching at 2969 and 2907 cm⁻¹, C=O stretching vibration at 1684 cm⁻¹, and bands associated with the aromatic ring at 1614, 1578, and 1505 cm⁻¹). IR spectrum of the AAc grafted PET film showed new peaks for carboxyl –OH groups around 2300–3700 cm⁻¹ which was absent in IR spectrum of pristine PET film (Figure 2(a)). The –OH peaks near 2580 and 2900 cm⁻¹ indicate the existence of strong hydrogen bonding between –COOH groups in the AAc grafted PET film [20, 21]. After KOH treatment the −OH peak near 2580 cm⁻¹ disappeared (Figure 2(a)) indicating the reduction of hydrogen bonding between the –COOH groups and formation of some –COO⁻K⁺ groups which is confirmed by the appearance of new peak near 1560 cm⁻¹ assigned for carboxylate ion (Figure 2(b)) [22]. Therefore it can be said that AAc grafted PET film can show little adsorption of metal ion due to the presence of hydrogen bonded –COOH groups, but after KOH treatment, the films showed greater metal ion adsorption due to the reduction of hydrogen bonding between –COOH groups and the presence of some ionized –COO⁻K⁺ groups. The conversion percentage of –COOH groups to –COO⁻K⁺ groups can be calculated from the IR spectra by the following equation: where , , and represent the total area under the IR peaks from 2300–3700 cm⁻¹ (the region where carboxyl –OH peaks appeared) for pristine PET, AAc grafted PET, and KOH treated AAc grafted PET, respectively. The conversion percentage calculated is 28%.

(a)

(b)

The reason behind increase of metal ion adsorption after KOH treatment can be better understood from the SEM image. SEM micrographs of pristine PET film, AAc grafted PET film, and modified AAc grafted PET film are shown in Figure 3. The effect of KOH treatment is not only conversion of some extent of –COOH group to –COOK group, but rather the more significant effect is the structural change of the graft film surface after introduction of some –COOK group. Before KOH treatment, the graft chains showed a compact structure in SEM image (Figure 3(b)) which is due to the attraction between the graft chains because of hydrogen bonding (Figure 3(b1)). At this condition many of the functional groups (–COOH) were inaccessible to the metal ions. After KOH treatment, graft chains showed an expanded structure in SEM image (Figure 3(c)) which is due to the repulsion of graft chains by the electrostatic force of some ionic –COO⁻ groups. (Figure 3(c1)). At this condition the initial functional groups (–COOH) of the graft films became easily accessible to the metal ions besides the new functional groups (–COOK). The average surface roughness () calculated from the SEM image of pristine PET, AAc grafted PET, and KOH treated AAc graft PET film is 9.6, 10.8, and 20.7 pixel, respectively (roughness is calculated by using an image processing program, imageJ). Large increase of surface roughness after KOH treatment provides further proof of the rearrangement of the graft chains from compact structure to expanded structure which facilitated the metal ion adsorption.

(a)

(b)

(c)

3.2. Selective Cu(II) Ion Adsorption by the Adsorbent Film

The modified graft film adsorbed 55.6, 9.0, and 7.8 mg/g of Cu(II), Ni(II), and Co(II), respectively, from a ternary solutions of Cu(II), Ni(II), and Co(II) under the same initial concentrations of 2000 mg/L of each metal ion at pH 4. The selectivity of an adsorbent is often measured from the distribution coefficient (). The term refers to the affinity of an adsorbent for a particular ion in presence of interfering ions. can be calculated by (5) [23] as where is the distribution coefficient (mL/g), and 　(mg mL⁻¹) are the initial and equilibrium concentrations of a metal species, respectively, (mL) is the volume of the testing solution, and (g) is the amount of adsorbent.

Now, the selectivity coefficient, (dimensionless), for a specific metal ion in the presence of competitor ions can be expressed by (6) as where is the value of the targeted metal (Cu(II) ions in this case), and is the value of the other metal in the mixed metal solutions (Ni(II) or Co(II) ions in this case). The selectivity coefficient for binding of Cu(II) over Ni(II) and Co(II) calculated (at initial concentrations of 2000 mg/L and pH 4) for modified AAc grafted PET film is and , respectively. The selectivity sequence for the modified graft film (Cu(II) > Ni(II) > Co(II)) followed the Irving-Williams series, which refers to the relative stabilities of complexes formed by the transition metal ions with ligands [24]. The high selectivity for Cu(II) can be explained in terms of the Pearson’s concept of hard and soft acids and bases. According to the concept, the carboxylate groups can be considered as soft bases, and on the other hand Cu²⁺ can be considered as a soft acid, while Ni²⁺ and Co²⁺ are relatively hard acids [25]. Generally, hard acids coordinate better with hard bases and soft acids with soft bases. Therefore, a strong interaction between Cu²⁺ and carboxylate group bearing adsorbent films is expected.

3.3. Equilibrium Adsorption Isotherm of Selective Cu(II) Ion Adsorption

An adsorption isotherm which represents the relationship between the amount of metal ions adsorbed by the adsorbent and the metal ions concentration remaining in solution is commonly used to study the adsorption process. Adsorption isotherms for competitive adsorption of Cu(II), Ni(II), and Co(II) under the same initial concentrations are shown in Figure 4. In case of Cu(II), the adsorption capacity increased with the increase of equilibrium concentration while for Ni(II) and Co(II), the adsorption capacity reached maximum for equilibrium concentration of 167 and 172 mg/L, respectively, and thereafter decreased with increase of equilibrium concentration. This might be due to the high affinity of the adsorbent for Cu(II) than Ni(II) and Co(II) (Section 3.2), for which with increase of Cu(II) ion concentration with respect to the available adsorption sites, the adsorption of Ni(II) and Co(II) decreased.

For interpretation of the selective Cu(II) adsorption data, the Langmuir [26] and Freundlich [27] isotherm models were used. The linear form of the Langmuir isotherm is presented by where is the equilibrium concentration (mg L⁻¹), the monolayer saturation adsorption capacity of adsorbent (mg g⁻¹), is the equilibrium adsorption capacity, and is Langmuir adsorption constant (Lmg⁻¹). The plot of / versus shown in Figure 5 was drawn from the experimental data given in Figure 4. The relationship between / and is linear indicating that the adsorption behavior follows the Langmuir adsorption isotherm. The , , and correlation coefficients () values are presented in Table 2.

The Freundlich isotherm is described by the following equation: where is the equilibrium concentration (mg L⁻¹), is the equilibrium adsorption capacity, the sorption capacity (mg g⁻¹), and is an empirical parameter. The plot of log versus log shown in Figure 6 was drawn from the experimental data given in Figure 4. The , , and correlation coefficients () values are presented in Table 2.

The linear plots show that the two studied models, the Langmuir equation and Freundlich equation, can give prediction of experimental data. The Langmuir model assumes monolayer adsorption of adsorbate on a structurally homogeneous adsorbent where all adsorption sites are identical. On the other hand, the Freundlich model is not restricted to homogeneous system or monolayer adsorption; it can also describe heterogeneous system and multilayer adsorption. Therefore, fitting of experimental data with Langmuir model suggests that a monolayer adsorption of ions on the adsorbent is appropriate to describe the selective Cu(II) adsorption on the modified AAc grafted PET. This also suggests that the adsorption was mainly chemical adsorption and the adsorption sites are identical to the metal ions; in other words surface heterogeneity of apparently heterogeneous surface of the modified AAc grafted PET is not significant in respect of adsorption phenomenon. Similar conclusion has been drawn when the adsorption of metal ions on the rough surface of meranti sawdust followed the Langmuir adsorption isotherm model [28].

3.4. Adsorption Kinetic of Selective Cu(II) Ion Adsorption

Figure 7 shows the kinetics of competitive adsorption of Cu(II), Ni(II), and Co(II) under the same initial concentrations of metal ions by modified AAc grafted PET films. It was observed that the adsorption of Cu(II) ions increased with increasing soaking time while adsorption of Ni(II) and Co(II) reached maximum after 10 min and after that decreased with increasing soaking time. This can be explained as the adsorbent Ni(II) and adsorbent Co(II) complexes are less stable than adsorbent Cu(II) complex (Section 3.2); therefore, with increase of soaking time more stable complexes replace less stable complexes.

The pseudo-first-order and pseudo-second order kinetic models were applied to fit the selective Cu(II) adsorption by the modified AAc grafted PET films. The pseudo-first-order and pseudo-second-order equations [29, 30], are expressed as: where and are the amount of ions adsorbed (mg g⁻¹) at any time and equilibrium time, respectively, is the rate constant (min⁻¹) of first-order adsorption, and (g min⁻¹mg⁻¹) is the rate constant of second-order adsorption. The pseudo-first-order rate constants could be determined experimentally by plotting log) against as shown in Figure 8. The experimental and theoretical value, first-order rate constant, and the correlation coefficients () are given in Table 3. It can be seen from the results that the experimental value and the value calculated from first-order kinetic model are not in agreement with each other. Pseudo-second-order rate constants could be determined experimentally by plotting against as shown in Figure 9. All the second-order kinetic parameters for selective Cu(II) adsorption are given in Table 3. It can be seen that the experimental and the value calculated from second-order kinetic model are in accordance with each other. Therefore, the pseudo-second-order equation can be used to interpret selective Cu(II) adsorption on the modified AAc grafted PET. Pseudo-second-order model fit with the experimental kinetic data indicate that intraparticle diffusion process was the rate-limiting step of the adsorption [31] and it also proves that the chelating interaction plays the major role in the adsorption process [32].

3.5. Effect of pH on Selective Cu(II) Ion Adsorption

Effect of pH on competitive adsorption of Cu(II), Ni(II), and Co(II) by the modified graft films at initial concentration 500 mg/L is shown in Figure 10. It can be seen that the adsorbent is highly selective towards Cu(II) in the pH range 1.5 to 4.5. At low pH, the carboxylate ions are more protonated and therefore adsorption of all metal ions was low. With increase of pH from 1.5 to 4.5, adsorption of all metal ions increased and in the pH range the adsorbent showed selectivity towards Cu(II) due to its the high affinity towards Cu(II). But increase of pH after 4.5 caused precipitation of Cu(OH)₂.

3.6. Desorption and Reuse of the Adsorbent

After adsorption of metal ion on the modified AAc grafted PET, the adsorbents were regenerated using 2 M hydrochloric acid. Desorption took place rapidly and the equilibrium achieved within 10–20 min. The desorption ratio was 99%. During desorption, the hydrogen ions in the solution were exchanged with the metal ions on the sorption sites. The regenerated film (–COOH form) was treated with KOH solution (to convert to –COO⁻K⁺ form) before being reused in subsequent cycles. Because we found that this –COOH form showed much lower metal adsorption than –COO⁻K⁺ form which may be due to the formation of hydrogen bonding again. The sorption capacity of the film for Cu(II) from aqueous solution of Cu(II), Co(II) and Ni(II) in five successive cycles is shown in Figure 11. For the 2nd cycle the sorption capacity decreased which may be due to the loss of physically adsorbed homopolymer of AAc which might have washed out in acid and base solutions [33]. However, the sorption capacity did not change that much in subsequent cycles indicating that the film can be used repeatedly for Cu(II) adsorption.

4. Conclusion

The KOH treated AAc graft PET films containing carboxylate groups can form more stable complex with Cu²⁺ than Co²⁺ or Ni²⁺ and therefore can show selective Cu²⁺ adsorption from aqueous solution containing Cu²⁺, Co²⁺, and Ni²⁺ with a selectivity coefficient of 7 and 8 for binding of Cu²⁺ over Ni²⁺ and Co²⁺, respectively, at pH 4 and initial concentration 2000 mg/L. Langmuir isotherm model and pseudo-second-order equation can be used for interpretation of selective equilibrium and kinetic adsorption data, respectively. The adsorbent film can be used repeatedly for Cu²⁺ sorption from aqueous solution of Cu²⁺, Co²⁺, and Ni²⁺.

Acknowledgment

This work was supported by JSPS KAKENHI Grant number 24360398.

References

J. Ui, Ed., Industrial Pollution in Japan (the Japanese Experience Series), United Nations University Press, Tokyo, Japan, 1992, http://www.unu.edu/unupress/unupbooks/uu35ie/uu35ie00.htm.
M. Šćiban, M. Klašnja, and B. Škrbić, “Modified softwood sawdust as adsorbent of heavy metal ions from water,” Journal of Hazardous Materials, vol. 136, no. 2, pp. 266–271, 2006.
View at: Publisher Site | Google Scholar
N. Ünlü and M. Ersoz, “Adsorption characteristics of heavy metal ions onto a low cost biopolymeric sorbent from aqueous solutions,” Journal of Hazardous Materials, vol. 136, no. 2, pp. 272–280, 2006.
View at: Publisher Site | Google Scholar
M. Arslan, Z. Temoçin, and M. Yiǧitoǧlu, “Removal of cadmium (II) from aqueous solutions using sporopollenin,” Fresenius Environmental Bulletin, vol. 13, no. 7, pp. 616–619, 2004.
View at: Google Scholar
R. Schmuhl, H. M. Krieg, and K. Keizer, “Adsorption of Cu(II) and Cr(VI) ions by chitosan: kinetics and equilibrium studies,” Water SA, vol. 27, no. 1, pp. 1–7, 2001.
View at: Google Scholar
Y. S. Ho, J. C. Y. Ng, and G. McKay, “Removal of lead(II) from effluents by sorption on peat using second-order kinetics,” Separation Science and Technology, vol. 36, no. 2, pp. 241–261, 2001.
View at: Publisher Site | Google Scholar
S. R. Shukla and V. D. Sakhardande, “Column studies on metal ion removal by dyed cellulosic materials,” Journal of Applied Polymer Science, vol. 44, no. 5, pp. 903–910, 1992.
View at: Publisher Site | Google Scholar
Y. S. Al-Degs, M. I. El-Barghouthi, A. A. Issa, M. A. Khraisheh, and G. M. Walker, “Sorption of Zn(II), Pb(II), and Co(II) using natural sorbents: equilibrium and kinetic studies,” Water Research, vol. 40, no. 14, pp. 2645–2658, 2006.
View at: Publisher Site | Google Scholar
R. Coşkun and C. Soykan, “Lead(II) adsorption from aqueous solution by poly(ethylene terephthalate)-g-acrylamide fibers,” Journal of Polymer Research, vol. 13, no. 1, pp. 1–8, 2006.
View at: Publisher Site | Google Scholar
H. Băg, A. R. Türker, R. Coşkun, M. Saçak, and M. Yigitoglu, “Determination of zinc, cadmium, cobalt and nickel by flame atomic absorption spectrometry after preconcentration by poly(ethylene terephthalate) fibers grafted with methacrylic acid,” Spectrochimica Acta B, vol. 55, no. 7, pp. 1101–1108, 2000.
View at: Google Scholar
O. Bozkaya, M. Yiǧitoǧlu, and M. Arslan, “Investigation on selective adsorption of Hg(II) ions using 4-vinyl pyridine grafted poly(ethylene terephthalate) fiber,” Journal of Applied Polymer Science, vol. 124, no. 2, pp. 1256–1264, 2012.
View at: Publisher Site | Google Scholar
R. Coşkun, C. Soykan, and M. Saçak, “Adsorption of copper(II), nickel(II) and cobalt(II) ions from aqueous solution by methacrylic acid/acrylamide monomer mixture grafted poly(ethylene terephthalate) fiber,” Separation and Purification Technology, vol. 49, no. 2, pp. 107–114, 2006.
View at: Publisher Site | Google Scholar
R. Coşkun, C. Soykan, and M. Saçak, “Removal of some heavy metal ions from aqueous solution by adsorption using poly(ethylene terephthalate)-g-itaconic acid/acrylamide fiber,” Reactive and Functional Polymers, vol. 66, no. 6, pp. 599–608, 2006.
View at: Publisher Site | Google Scholar
M. Arslan, “Preparation and use of amine-functionalized glycidyl methacrylate-g-poly(ethylene terephthalate) fibers for removal of chromium(VI) from aqueous solution,” Fibers and Polymers, vol. 11, no. 3, pp. 325–330, 2010.
View at: Publisher Site | Google Scholar
M. Yiǧitoǧlu and M. Arslan, “Adsorption of hexavalent chromium from aqueous solutions using 4-vinyl pyridine grafted poly(ethylene terephthalate) fibers,” Polymer Bulletin, vol. 55, no. 4, pp. 259–268, 2005.
View at: Publisher Site | Google Scholar
M. Yiǧitoǧlu and M. Arslan, “Selective removal of Cr(VI) ions from aqueous solutions including Cr(VI), Cu(II) and Cd(II) ions by 4-vinly pyridine/2-hydroxyethylmethacrylate monomer mixture grafted poly(ethylene terephthalate) fiber,” Journal of Hazardous Materials, vol. 166, no. 1, pp. 435–444, 2009.
View at: Publisher Site | Google Scholar
M. Karakişla, “The adsorption of Cu(II) ion from aqueous solution upon acrylic acid grafted poly(ethylene terephthalate) fibers,” Journal of Applied Polymer Science, vol. 87, no. 8, pp. 1216–1220, 2002.
View at: Publisher Site | Google Scholar
H. H. Abdel-Razik and E. Kenawy, “Synthesis, characterization, and amidoximation of diaminomaleodinitrile- functionalized polyethylene terephthalate grafts for collecting heavy metals from wastewater,” Journal of Applied Polymer Science, vol. 125, no. 2, pp. 1136–1145, 2012.
View at: Publisher Site | Google Scholar
X. Ping, M. Wang, and X. Ge, “Radiation induced graft copolymerization of n-butyl acrylate onto poly(ethylene terephthalate) (PET) films and thermal properties of the obtained graft copolymer,” Radiation Physics and Chemistry, vol. 80, no. 5, pp. 632–637, 2011.
View at: Publisher Site | Google Scholar
J. J. Max and C. Chapados, “Infrared spectroscopy of aqueous carboxylic scids: comparison between different scids and their salts,” Journal of Physical Chemistry A, vol. 108, no. 16, pp. 3324–3337, 2004.
View at: Publisher Site | Google Scholar
T. Kobayashi, H. Ying Wang, and N. Fujii, “Molecular imprint membranes of polyacrylonitrile copolymers with different acrylic acid segments,” Analytica Chimica Acta, vol. 365, no. 1–3, pp. 81–88, 1998.
View at: Publisher Site | Google Scholar
W. J. MacKnight, L. W. McKenna, B. E. Read, and R. S. Stein, “Properties of ethylene-melhacrylic acid copolymers and their sodium salts: infrared studies,” Journal of Physical Chemistry, vol. 72, no. 4, pp. 1122–1126, 1968.
View at: Google Scholar
H. Yan, J. Dai, Z. Yang, H. Yang, and R. Cheng, “Enhanced and selective adsorption of copper(II) ions on surface carboxymethylated chitosan hydrogel beads,” Chemical Engineering Journal, vol. 174, no. 2-3, pp. 586–594, 2011.
View at: Publisher Site | Google Scholar
H. Irving and R. J. P. Williams, “The stability of transition-metal complexes,” Journal of the Chemical Society, pp. 3192–3210, 1953.
View at: Google Scholar
B. L. Rivas, L. N. Schiappacasse, U. E. Pereira, and I. Moreno-Villoslada, “Interactions of polyelectrolytes bearing carboxylate and/or sulfonate groups with Cu(II) and Ni(II),” Polymer, vol. 45, no. 6, pp. 1771–1775, 2004.
View at: Publisher Site | Google Scholar
I. Langmuir, “The adsorption of gases on plane surfaces of glass, mica and platinum,” The Journal of the American Chemical Society, vol. 40, no. 9, pp. 1361–1403, 1918.
View at: Google Scholar
H. M. F. Freundlich, “Über die adsorption in lösungen,” Zeitschrift Für Physikalische Chemie A, vol. 57, pp. 385–470, 1906.
View at: Google Scholar
M. Rafatullah, O. Sulaiman, R. Hashim, and A. Ahmad, “Adsorption of copper (II), chromium (III), nickel (II) and lead (II) ions from aqueous solutions by meranti sawdust,” Journal of Hazardous Materials, vol. 170, no. 2-3, pp. 969–977, 2009.
View at: Publisher Site | Google Scholar
Y. S. Ho, “Review of second-order models for adsorption systems,” Journal of Hazardous Materials, vol. 136, no. 3, pp. 681–689, 2006.
View at: Publisher Site | Google Scholar
C. Namasivayam and D. J. S. E. Arası, “Removal of congo red from wastewater by adsorption onto waste red mud,” Chemosphere, vol. 34, no. 2, pp. 401–417, 1997.
View at: Publisher Site | Google Scholar
S. Rengaraj, J. Yeon, Y. Kim, Y. Jung, Y. Ha, and W. Kim, “Adsorption characteristics of Cu(II) onto ion exchange resins 252H and 1500H: kinetics, isotherms and error analysis,” Journal of Hazardous Materials, vol. 143, no. 1-2, pp. 469–477, 2007.
View at: Publisher Site | Google Scholar
Y. Li, Q. Y. Yue, and B. Y. Gao, “Adsorption kinetics and desorption of Cu(II) and Zn(II) from aqueous solution onto humic acid,” Journal of Hazardous Materials, vol. 178, no. 1–3, pp. 455–461, 2010.
View at: Publisher Site | Google Scholar
S. Deng and Y. P. Ting, “Fungal biomass with grafted poly(acrylic acid) for enhancement of Cu(II) and Cd(II) biosorption,” Langmuir, vol. 21, no. 13, pp. 5940–5948, 2005.
View at: Publisher Site | Google Scholar

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Copyright © 2013 Nazia Rahman et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

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