Magnetic chitosan nanoparticles for removal of Cr(VI) from aqueous solution

Magnetic chitosan nanoparticles for removal of Cr(VI) from aqueous solution Nguyen Ngoc Thinh a , Pham Thi Bich Hanh b , Le Thi Thanh Ha a , Le Ngoc Anh c , Tran Vinh Hoang a , Vu Dinh Hoang a , Le Hai Dang d , Nguyen Van Khoi b , Tran Dai Lam e, ⁎ a School of Chemical Engineering, Hanoi University of Science and Technology, 1, Dai Co Viet Road, Hanoi, Viet Nam b Institute of Chemistry, Vietnam Academy of Science and Technology, 18, Hoang Quoc Viet Road, Hanoi, Viet Nam c Institute of Marine Geology and Geophysics, Vietnam Academy of Science and Technology, 18, Hoang Quoc Viet Road, Hanoi, Viet Nam d Hanoi National University of Education,136 Xuan Thuy, Hanoi, Viet Nam e Institute of Materials Science, Vietnam Academy of Science and Technology, 18, Hoang Quoc Viet Road, Hanoi, Viet Nam abstractarticle info Article history: Received 28 April 2012 Received in revised form 29 August 2012 Accepted 3 December 2012 Available online 9 December 2012 Keywords: Fe 3 O 4 Magnetic chitosan nanoparticles Adsorption isotherm Cr(VI) A simple method was introduced to prepare magnetic chitosan nanoparticles by co-precipitation via epichlorohydrin cross-linking reaction. The average size of magnetic chitosan nanoparticles is estimated at ca. 30 nm. It was found that the adsorption of Cr(VI) was highly pH-dependent and its kinetics follows the pseudo-second-order model. Maximum adsorption capacity (at pH 3, room temperature) was calculated as 55.80 mg·g −1 , according to Langmuir isotherm model. The nanoparticles were thoroughly characterized before and after Cr(VI) adsorption. From this result, it can be suggested that magnetic chitosan nanoparticles could serve as a promising adsorbent for Cr(VI) in wastewater treatment technology. © 2012 Elsevier B.V. All rights reserved. 1. Introduction Contamination of water by toxic heavy metals through the dis- charge of industrial wastewater is a worldwide environmental prob- lem. Rapid industrialization has seriously contributed to the release of toxic heavy metals to water streams. Among the various heavy metals, chromium (Cr) is one of the most toxic pollutants generated by the electroplating, leather tanning, metal finishing, steel fabrica- tion, textile industries and chromate preparation. The most common oxidation states of Cr in nature are Cr(III) and Cr(VI). Chromium(VI) is more hazardous than Cr(III) as it can diffuse as CrO 4 2− or HCrO 4 − through cell membranes and o xidize biological molecules [1].Awide range of physical and chemical processes are available for the removal of chromium from wastewater such as filtratio n [2], electrochemical precipitation [3], adsorption [4,5],electrodeposition[6] and membrane sys- tems or ion exchange process [7–9]. Among these methods, adsorption is one of the most econo mically favorable while being t echnically easy [10–12] . Chitosan has excellent propert ies for the adsorption of heavy metal ions, principally due to the presence of amino groups (–NH 2 )in the polymer matrix, which interact with metal ions in solution by ion exchange and complexation reactions [13–15 ]. Most of the chitosan-based adsorbents are sub micron to micron-sized and need large internal poros- ities to ensure adequate surface area for adsorption. However, the diffusion limitation within the particles leads to the decrease in the adsorption rate and a vailable capacity. C ompared to t he traditional micron-sized supports used in separation process, nano-sized adsorben ts display better performance due to high specific surface area and the ab- sence of internal diffusion resistance. The nano-adsorbents cannot be sep- arated easily from aqueous solution by filtration or centrifugation [16]. The application of magnetic adsorbent technology to solve environmental problems has received considerable attention in recent years [16–18]. In this paper, magnetic chitosan nanoparticles were prepared, characterized and applied for the removal of Cr(VI) in the water solution. Af- terwards, thermodynamic and kinetic aspects of the adsorption process were considered. The improved magnetic and high adsorption uptake properties are two main features of the synthesized nanoparticles that can be advantageously used in water treatment. 2. Experimental 2.1. Chemicals FeCl 3 ·6H 2 O, FeSO 4 ·7H 2 O, K 2 Cr 2 O 7 ,CH 3 COOH, NaOH and NH 3 were of analytical grade. Chitosan (MW=400,000, DA=70%) was purchased from Nha Trang Aquatic Institute (Vietnam) and re-characterized by viscometry and IR measureme nts at our laboratory [18]. Double distilled water was used in the preparation of all solutions. 2.2. Preparation of magnetic chitosan nanoparticles Magnetic chitosa n nanoparticles were prepared by co-precipitation method [18–20], with several modifications. Experiments were carried Materials Science and Engineering C 33 (2013) 1214–1218 ⁎ Corresponding author. Tel.: +84 4 37564129; fax: +84 438360705. E-mail address: tdlam@vast.ac.vn (T.D. Lam). 0928-4931/$ – see front matter © 2012 Elsevier B.V. All rights reserved. http://dx.doi.org/10.1016/j.msec.2012.12.013 Contents lists available at SciVerse ScienceDirect Materials Science and Engineering C journal homepage: www.elsevier.com/locate/msec out in inert gas (N 2 ). Fe 3 O 4 nanoparticles were synthesized by co-precipitation of ferric and ferrous salts. The am ount 6.4795 g of FeCl 3 ·6H 2 O and 3.3339 g of FeSO 4 ·7H 2 O were dissolved into 150 mL of deoxygenated distilled water. After stirring for 30 min, chemical precipitation was achieved at 30 °C under vigorous stirring by adding 20 mL of NH 3 ·H 2 O solution (28%, v/v). During the reaction process, pH was maintained at about 10. The reaction system was kept at 70 °C for 1h.1gchitosanflake was dissolved in a 150 mL CH 3 COOH solution 2% (w/v). The chitosan solution was then dropped into the obtained magnetic fluid in t he flask through a dropper. Afterwards, 2 mL of pure e pichlorohydrin was added into reaction flask and stirred at 85 °C for 3 h, before the flask was cooled down to room temperature. The precipitate was washed with distilled water to remove all existing in the e ffluents. Silver nitrate (AgNO 3 ) was used to detect residue of Cl − . The precipitate was then washed with ethanol and dried at 50 °C, in the vacuum oven. 2.3. Adsorption experiments The sorption experiments were performed by batch method. Sam- ples of 0.1 g of magnetic chitosan nanoparticles were equilibrated with 50 mL of solution containing various amount of Cr(VI). The pH value of solutions was adjusted by using diluted solution of NaOH and HCl. The temperature of the solutions (25 °C, 35 °C, 45 °C) was controlled with the thermostatic bath. The adsorbed amount of Cr(VI) per unit weight of magn etic ch itosan n anoparticle s, q t (mg·g −1 ), was calculated from the mass balance equation as: q t ¼ C 0 −C t ðÞ⋅V m ð1Þ where C 0 and C t (mg/L) are the initial Cr(VI) concentration and the Cr(VI) concentrations at any time t,respectively;V (L)isthevolumeofthe Cr(VI) solution; and m (g)isthemassofthemagneticchitosan nanoparticles. Samples o f t he Cr(VI) solution were collected at pre- determined time intervals and analyzed using a UV–Vis Spectrophotom- eter (model UV-PC1600, Shimadzu), at λ max =540 nm, according to the 1,5-diphenyl-carbazide method [21]. All measuremen ts were conducted triplicate. 2.4. Characterization methods X-ray diffraction (XRD) patterns were obtained at room temperature by D8 Advance, Bruker ASX, using CuKα radiation (λ=1.5406 Å) Fig. 1. Camera pictures (a, b); FE-SEM images (c, d) and TEM images (e, f) of magnetic chitosan nanoparticles. 1215N.N. Thinh et al. / Materials Science and Engineering C 33 (2013) 1214–1218 in the range of 2θ=10°–60°, and a scanning rate of 0.02°·s −1 . Mor- phology of magnetic chitosan nanoparticles was analyzed by Field Emission Hitachi S-4500 Scanning Electron Microscope (FE-SEM) and Transmission Electron Microscope (TEM, JEOL, Voltage: 80 kV). Absor- bance measurements were carried out using Shimadzu UV-PC1600 spectrophotometer in the range of 400–800 nm. The magnetic properties were measured with home-made vibrat- ing sample magnetometer (VSM) and evaluated in terms of saturation magnetization and coercivity. Chemical composition of samples was determined by JEOL Scanning Electron Microscope and Energy Dispersive Spectroscopy (SEM/EDS) JSM-5410 Spectrometer. 3. Results and discussion 3.1. Characterization of magnetic chitosan nanoparticles TEM and SEM micrograph of magnetic chitosan particles provides information on their size and morphology. It can be observed from Fig. 1 that the magnetic particles have a spherical shape with a diameter of about 30 nm. XRD pattern of magnetic chitosan nanoparticles shows six charac- teristic peaks for Fe 3 O 4 corresponding to (220), (311), (400), (422), (511) and (440) (JCPDS file, PDF No. 65-3107) (Fig. 2). Quite w eak diffraction lines of composite indicated that Fe 3 O 4 particles have been coat- ed by amorphous chitosan, which did not affect the phase and structure of Fe 3 O 4 . Particle size of magnetic chitosan nanoparticles can be estimated approximately as 30 nm, via line broadening in the pattern, using Debye–Scherrer equation (d=kλ/βcos θ). Typical magnetization loops were recorded by VSM and shown on Fig. S1 (supporting information). From the plot of magnetization vs. magnetic field and its enlargement near the origin, the saturation magnetization, remanence magnetization, coercivity and squareness could be calculated. Because of no remanence and coercivity, it can be suggested that the beads are superparamagnetic. It can also be observed from this figure that magnetization moment of Fe 3 O 4 nanoparticles decreases very little after chitosan surface coating, meaning that chitosan does not affect magnetic properties of these magnetic chitosan nanoparticles. Therefore, maintaining such a hi gh saturation magne tiza- tion value (M s )aftercoatingthesenanoparticlesisadvantageousand susceptible to the external magnetic field for magnetic separation. 3.2. Effect of initial pH on the adsorption process It is well known that some metals are preferentially adsorbed in acidic media while chitosan can dissolve under this acidic condition. In this regard, the chemical modification of chitosan by using crosslinkingreac- tion offers an important pathway for producing chemically more stable chitosan derivatives, extending the potential applications of this bio- polymer. In our study, the crosslinking approach with epichlorohydrin to block/crosslink via hydroxyl (OH) group is expected to improve chemical stability, mechanical resistance and adsorption/desorption properties, c ompared to that with g lutaraldehyde (to blo ck amino (NH 2 ) group respectively), when keeping reactive amino groups intact for complexing reaction with heavy metal ions [14,16,19]. Next, selecting an optimum pH is very important for the adsorption process, since pH affects not only the surface charge of adsorbent, but also the degree of ionization and the speciation of the adsorbate during the reaction. The effect of pH on the adsorption process was investigated over the range from 2 to 6. As indicated in Fig. 3, the maximum capacity of Cr(VI) absorption occurred at pH of 3. The ex- planation would be addressed as the pH of the aqueous solution affects to stability of chromium speciation and the surface charge of the adsorbent. At pH 1, the chromium ions exists in the form of H 2 CrO 4 , while in the pH range of 1–6, different forms of chromium such asCr 2 O 7 2− ,HCrO 4 − ,andCr 3 O 10 2− coexist while HCrO 4 − predominates. As the pH increases, those form shifts to Cr 2 O 4 2− and Cr 2 O 7 2− [11].Cr(VI) exists predominantly a s HCrO 4 − in aqueous solution below pH 4 and the amino groups (–NH 2 ) of magnetic chitosan nanoparticles would be in protonated cationic form (–NH 3 + ) to a higher extent in acidic solution. This results in the stronger attraction for negatively charged ions. Electrostatic interaction between the sorbent and HCrO 4 − ions also con- tributes to the high chromium removal. However, at the pH lower than 3, decrease in uptake capacity is observed as the predomination of H 2 CrO 4 and the stro ng competition for adsorption sites betw een H 2 CrO 4 and protons. The decreasing of the adsorption capacity at higher pH values may be explained by the dual competition of CrO 4 2− and OH − for adsorption [11]. Thus, pH 3 was selected as the optimum pH value for the following adsorption experiment. 3.3. Adsorption isotherms Equilibrium experimental data were successfully fitted to the Langmuir isotherm whose equation can be expressed as q ¼ q m ⋅K L ⋅C e 1 þ K L ⋅C e ð2Þ where q m (mg·g −1 ) is the maximum sorption capacity (corresponding to complete monolayer coverage), C e is the equilibrium concentration in the solution (mg/L), q e is the equilibrium Cr(VI) concentration in 20 30 40 50 60 70 (440) (511) (422) (400) (311) (220) Intensity 2θ Fig. 2. XRD pattern of magnetic chitosan nanoparticles. 23456 50 55 60 65 70 75 80 85 R(%) pH Fig. 3. The influence of initial pH value on the adsorption of the Cr(VI) on magnetic chitosan nanoparticles. 1216 N.N. Thinh et al. / Materials Science and Engineering C 33 (2013) 1214–1218 the sorbent (mg·g −1 ), and K L is the sorption affinity constant related to the binding energy of sorption (L·mg −1 ). The experimental data (Table 1) fitted well with Langmuir model (R 2 >0.99), confirming that the adsorption process is monolayer adsorption. The results of adsorption studies by Langmuir model, indicating improved Cr(VI) uptake properties of magnetic chitosan nanoparticles (55.80 mg·g −1 ,pH3, room temperature, compared to the other adsorben ts (Table 2)), probably relates to the smaller loss of amine groups of chitosan, involved in the cross-linking reaction wh en using epic hlorohydrin as a cross-linker. Cr(VI) removal by adsorbent as a function of contact time with different initial concentrations (40, 80 and 180 mg·L −1 ) of Cr(VI) is shown in Fig. 4, where the adsorption rate of metal uptake was quite slow and the maximum uptake was observed within 100 min. 3.4. Thermodynamic and kinetic studies In this section, thermodynamic and kinetic aspects of the adsorption process will be considered. The experimental data obtained at different temperatures were used in calculating the thermodynamic parameters such as Gibbs free energy (ΔG), enthalpy (ΔH) and entro- py (ΔS) according to the following equations: ΔG ¼ ΔH−T Â ΔS ð3Þ lnK ¼ ln q e =C e ðÞ¼−ΔH=RT þ ΔS=R: ð4Þ Where K is the equilibrium constant, obtained from Langmuir isotherms at different temperature and R is the universal gas constant. ΔH and ΔS were obtained from the slope and intercept of the plot log (q e /C e ) vs. 1/T (Fig. 5), namely: ΔH ¼ −0:6853 kJ⋅mol −1  and ΔS ¼ −115:7366 J⋅mol −1 ⋅K −1  : Table 1 Adsorption equilibrium constants obtained from Langmuir isotherm in the adsorption of Cr(VI) onto magnetic chitosan nanoparticles (volume: 50 mL; absorbent dose: 0.1 g; initial concentrations: 60, 80 and 180 mg·L −1 ; pH value: 3.0; temperature: 298,308, 318 K). Temperature (K) q max (mg·g −1 ) K L R 2 298 55.80 0.366 0.993 308 46.71 0.119 0.997 318 43.29 0.138 0.994 Table 2 Comparison of adsorption capacities of Cr(VI) with other adsorbents. Adsorbents Adsorption capacity (mg·g −1 ) pH Ref. Tires activated carbon 58.50 2.0 [23] Rubberwood activated carbon 44.05 2.0 [3] Coconut shell activated carbon 20.00 2.0 [24] Hazelnut shell activated carbon 17.70 2.0 [25] Beech sawdust 16.10 1.0 [26] Sugarcane bagasse 13.40 2.0 [27] Coconut shell charcoal 10.88 4.0 [28] Coconut tree sawdust 3.60 3.0 [29] Chitosan 22.09 3.0 [30] Non-cross linked chitosan 78.00 5 [31] Cross linked chitosan 50.00 5 [31] Magnetic chitosan nanoparticles (this study) 55.80 3 0 50 100 150 200 250 300 350 400 10 15 20 25 30 35 40 45 50 55 60 65 70 q(mg/g) t(min) 40mg/L 80mg/L 180mg/L Fig. 4. Effect of contact time on Cr(VI) adsorption (volume: 50 mL; absorbent dose: 0.1 g; initial concentrations: 40, 80 and 180 mg·L −1 ; pH value: 3.0; temperature: 298 K). 3.20 3.22 3.24 3.26 3.28 3.30 3.32 3.34 3.36 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 y=-13.92069+4.38115x,R=0.99017 Ln(q e /C e ) 1/T*10 -3 (1/K) C=80 mg/L Fig. 5. Thermodynamic plot of ln (q e /C e ) vs. 1/T. Table 3 Thermodynamic data of Cr(VI) adsorption process. T (K) ΔG (kJ·mol −1 ) ΔH (kJ·mol −1 ) ΔS (J·mol −1 ·K −1 ) 298 −35.164 −0.6853 −115.7366 303 −35.742 307 −36.205 312 −36.784 -50 0 50 100 150 200 250 300 350 -7 -6 -5 -4 -3 -2 -1 0 1 2 3 4 t(min) 40mg/L 80mg/L 180mg/L ln(q e -q t ) Fig. 6. Kinet ic pseudo-first order sorption kinetics of Cr(VI) (volume: 50 mL; abso rbent dose: 0.1 g; initial concentrations: 40, 80 and 180 mg·L −1 ;pHvalue:3.0;temperature:298K). 1217N.N. Thinh et al. / Materials Science and Engineering C 33 (2013) 1214–1218 The negative value of ΔGobtainedfromEq.(3) reflects a spontaneous (favorable) adsorption process of Cr(VI) (Table 3), while the negative value of ΔH indicates that the a dsorption reaction i s exoth ermic and the adsorption of Cr(VI) is more effective at lower temperatures. Kinetically, in order to understand the behavior of the adsorbent and to examine the controlling mechanism of the adsorption process, the pseudo-first-order an d the pseudo-second-order were applied to the experimental data (Figs. 6 and 7). The pseudo-first-order rate expression of Lagergren is given as: ln(q e − q t )=ln(q e )− k 1 ⋅ t where q e and q t are the amountsofCr(VI)(mg·g − 1 ) adsorbed on the adsorbent at equilibrium and at time t, respectively and k 1 is the rate constant of first-order adsorption (min −1 ). The slopes and intercepts of plots of ln(q e −q t )vs.t were used to determine the first-o rder rate constant k 1 . The pseudo- second-order kinetic model is expressed as: t q t ¼ 1 k 2 ⋅q e 2 þ 1 q e Â t where k 2 (g·mg − 1 ·min −1 ) i s the rate constant of seco nd order a dsorption. The slopes and intercepts of plots of t/qt vs. t were used to calculate the second-order rate constant k 2 and q e [22]. A dsorption rate constants were summarized in Ta ble 4. The values of regression coefficient for pseudo-second-order model were close to 1 for all initial Cr(VI) concentrations. The calculated values q e,cal were very close to obtained q e,exp values. Hence, the adsorption of Cr(VI) on to magnetic chitosan na no- particles could obey the pseudo-second-order kinetic model. 4. Conclusion In this work, cross-linked with epichlorohydrin magnetic chitosan nanoparticles were prepared and characterized. The Cr(VI) adsorption behavior on the prepared ma gnetic c hitosan nanoparti cles has been studied under various conditions of different solution pH values and adsorption contact times. Optimal adsorption conditions of Cr(VI) were found at pH 3, and contact time of 100 min, with maximum adsorption capacity of 55.80 mg·g − 1 . Th e Langmuir model was found to fit well with the experimental data (correlation coefficient R 2 >0.99), indicating the occurrence of monolayer adsorption proce ss. Ther- modynamically, the adso rpti on of Cr(VI) is spontaneous (in term of ΔG) and exotherm ic (in term of ΔH) process. Kinetically, the ads orption of Cr(VI) onto magnetic chitosan nanopa rticles obeyed the pseudo-second-order model. Compared to the other adsorbents, magnetic chitosan nanoparticles shows greatly improved uptake properties of Cr(VI), probably due to high concentr ation of remaining active sites on the surface of magnetic chitosan nanoparticles. The improved magnetic and ad sorption uptake properties are two main features o f the synthesized nanopart icles that can be advantageously used in water treatment. Acknowledgments Funding of this work was provided by Vietnam Ministry of Science and Technology (grant 08/2011/HÐ-NÐT). Appendix A. Supplementary data Supplementary data to this article can be found online at http:// dx.doi.org/10.1016/j.msec.2012.12.013. References [1] P.G. Krishna, J.M. Gladis, U. Rambabu, T.P. Rao, G.R.K. Naidu, Talanta 63 (2004) 541–546. [2] C. 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Table 4 Comparison of the first-order and second-order adsorption rate constants, calculated q e,cal and experimental q e,exp values for different initial Cr(VI) concentrations. C 0 (mg·L −1 ) q e,exp (mg/g) First-order kinetic model Second-order kinetic model k 1 (min −1 ) q e,cal (mg·g −1 )R 2 k 2 (g·mg −1 ·min −1 ) q e,cal (mg·g −1 )R 2 40 19.42 0.029 5.59 0.946 8.38×10 −3 19.94 0.994 80 37.05 0.030 25.43 0.876 2.08×10 −3 38.46 0.992 180 53.8 0.025 22.04 0.956 2.16×10 −3 55.55 0.996 1218 N.N. Thinh et al. / Materials Science and Engineering C 33 (2013) 1214–1218 . 0.1 g of magnetic chitosan nanoparticles were equilibrated with 50 mL of solution containing various amount of Cr(VI). The pH value of solutions was adjusted by using diluted solution of NaOH. Magnetic chitosan nanoparticles for removal of Cr(VI) from aqueous solution Nguyen Ngoc Thinh a , Pham Thi Bich Hanh b , Le Thi Thanh. Cr(VI) concentrations at any time t,respectively;V (L)isthevolumeofthe Cr(VI) solution; and m (g)isthemassofthemagneticchitosan nanoparticles. Samples o f t he Cr(VI) solution were collected at pre- determined time

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