Youning Chen,
Wei Zhao and
Juncai Zhang
College of Chemistry and Chemical Engineering, Xianyang Normal College, Xianyang 712000, China. E-mail: cyn5363@163.com
First published on 16th January 2017
The study focused on the preparation of a chelating resin with pyridine ring as the functional group. The 4VP monomer was directly grafted on the surface of CMPS resin via SI-ATRP, and the performance of adsorption of resin for Cr(VI), Pb(II), Cr(III), Zn(II), and Cd(II) was determined. With the extension of ATRP time and increase of 4VP consumption, the 4VP grafting rate was linearly increased, indicating an increase in the density of the pyridine ring on the resin surface. Adsorption experiments indicated that the adsorption capacity of the resin for the metal ions considerably improved when compared with that of those reported in literature, whereas the desorption rate and reusability were equivalent to those of the conventional resins. When the pH value was greater than 5.0, Pb(II), Cr(III), Zn(II), and Cd(II) ions could be adsorbed; however, when the pH value was less than 3.0, Cr(VI) could be selectively adsorbed. These results are indicative of a potential application of the resin in the treatment of heavy metal wastewater. Therefore, adoption of one-step SI-ATRP is one of the effective methods for preparing a chelating resin with high capacity via the selection of an appropriate functional monomer.
From the perspective of monomer structures, vinyl pyridine contains –N, which has one unused electron pair that is not involved in the conjugated system on the ring; therefore, the vinyl pyridine modified resin has advantages and specific functions as compared to those of the styrene resin.13–15 The carbon atoms and nitrogen atoms on the pyridine ring are bonded via sp2 hybrid orbitals. Each atom in the ring contains 1 p orbital, and each p orbital contributes 1 electron for a total of 6 p electrons; thus, an annular enclosed conjugated system is formed that conforms to the Huckel's rule (4n + 2) of aromaticity. One sp2 hybrid orbital can also be found on the nitrogen atom, occupied by one lone pair of electrons, which is not involved in bonding and can therefore bind with the protons; therefore, pyridine is alkaline and also acts as a good ligand, which can bind or react with multiple metal ions to form complexes. 4-Vinylpyridine block copolymer is a very important type of polymer that can manifest an excellent performance due to the presence of nitrogen atoms on the pyridine ring; therefore, they can form self-assembly supramolecular structures16 and are capable of coordinating with metal ions.17,18 As reported in some previous studies, the 4-vinylpyridine-grafted polyethylene terephthalate fiber can effectively remove Cr(VI), Cu(II), and Cd(II) from a solution,19 and the 4-vinylpyridine-modified polyethyleneglycol dimethacrylate and glycol dimethacrylate microspheres exhibit a good adsorption performance for Pb(II), Cd(II), Cr(III), and Cu(II).20
Benzyl chloride is an effective initiator in the ATRP reactions and chloromethylated polystyrene contains benzyl chloride initiation sites. In this study, based on 4-vinylpyridine (4VP) as the functional monomer, a novel type of poly-4-vinylpyridine chelating polymeric adsorbent (P4VP-g-PS) was prepared using the SI-ATRP method to directly modify 4VP on the CMPS resin surface. The synthetic resin obtained using the abovementioned resin to adsorb Cr(VI), Pb(II), Cr(III), Zn(II), and Cd(II) has been characterized with a relatively high adsorption volume and can be repeatedly used, providing a feasible idea and method for the preparation of novel polymeric adsorbent.
TENSOR type 27 Fourier transform infrared spectrometer (Bruker, Germany), Rario type II elemental analyser (Elementar, Germany), novAA400 atomic absorption spectrometer (Analytik Jena AG, Germany), KYKY-2800B scanning electron microscope (KYKY Technology Co., Ltd., Beijing), and K-Alpha X-ray electron spectrometer (Termo Fisher, USA); Micromeritics ASAP 2010 (Georgia USA).
(2) Removal of copper ion: the products were washed using acetone followed by stirring in 10% EDTA (EDTA/ethanol volume ratio: 1:
1) for 24 hours. Then, they were filtered and washed with water and finally with ethanol. They were dried under vacuum at 35 °C.
The polymerization time and monomer dosage were used to control the degree of grafting (GD) of 4-vinylpyridine in CMPS and GD can be calculated using the following equation:
GD (%) = (Wa − Wb)/Wb × 100% | (1) |
Adsorption isotherm test: the pH value of the Cr(VI) stock solution was adjusted to 3.0, whereas the pH value of the Pb(II), Cr(III), Zn(II), and Cd(II) stock solutions was adjusted to 5.0. The solutions were then diluted using NaAc–HAc buffer solution to obtain the solutions at different concentrations (from 0.5 mmol L−1 to 8.0 mmol L−1). 0.1 g of resin was added to 100 mL of the abovementioned solutions. The beaker was placed onto a constant temperature oscillator and oscillated at a rate of 200 rpm at a constant temperature for 12 hours. Curves were plotted for Qe versus Ce to determine the Cr(VI), Pb(II), Cr(III), Zn(II), and Cd(II) adsorption isotherms.
Adsorption kinetic test: the initial concentration of Cr(VI), Pb(II), Cr(III), Zn(II), and Cd(II) solutions was 5 mmol L−1, the pH value of the Cr(VI) solution was 3.0, and the pH value of Pb(II), Cr(III), Zn(II), and Cd(II) solutions was 5.0; the pH value was not adjusted during the adsorption process. 1 mL of solution was extracted at regular intervals; atomic absorption spectrometry (AAS) was used to determine the concentration of metal ions in the solution and the adsorption volume of the resin was calculated. A dynamical parameter curve was plotted for adsorptive capacity (Q) versus adsorption time (T).
During the study of the effects of pH on the adsorptive capacity, the HAc–NaAc buffer solution was used to prepare the Cr(VI), Pb(II), Cr(III), Zn(II), and Cd(II) stock solutions at different pH values at an initial concentration of 5 mmol L−1.
After the adsorption was completed, 0.2 μm membrane filtration was performed to separate the resin and atomic absorption spectroscopy (AAS) was used to determine the concentration of the residual metal ions in the filtrate. Finally, the adsorptive capacity (Q) was calculated as follows:
![]() | (2) |
Degree of desorption (%) = mass of the desorbed metal ions/mass of the adsorbed metal ions × 100% | (3) |
To further determine the reusability of the resin, 10 consecutive adsorption–desorption cycles were conducted.
As is shown in Fig. 2, within 10 hours, the grafting degree of 4-vinylpyridine linearly increased with the increase in the polymerization time, indicating that the thickness of P4VP on the resin surface linearly increased. After 10 hours, the degree of grafting reached 75%. However, with the prolonged polymerization time, the growth rate gradually became slow due to the following reasons: with the progress of the reaction, the concentration of the monomer 4VP significantly decreased, the high rate of 4VP at the beginning was somewhat controlled, and double-base coupling and double-base disproportionation termination were the dominant reactions. As is shown in Fig. 3, the degree of grafting linearly increased with the increase in the monomer dosage. The abovementioned analysis indicates that the polymerization of 4-vinylpyridine on the material surface belongs to the active controllable polymerization, showing that on controlling the polymerization time and monomer dosage, the grafting amount of 4-vinylpyridine can be controlled.
The relationship between the grafting degree and adsorptive capacity was investigated. Fig. 2 and 3 present the volume of Cr(VI), Pb(II), Cr(III), Zn(II), and Cd(II) adsorbed by the P4VP resin at different ATRP time intervals and at different 4VP dosages. As is shown in Fig. 2, within 10 hours, with the prolonging of the ATRP reaction time, the adsorptive capacity linearly increased, presenting a direct proportion with the grafting amount of 4-vinylpyridine on the resin surface. After 10 hours, the rising tendency of the adsorptive capacity becomes slow probably due to the following reasons: with the prolonging in the polymerization time, the surface and interiors of the resin were covered with relatively long P4VP polymer brushes; however, the volume of the resin surface holes was limited, such that when the polymers obstruct the holes, the ATRP reaction will stop. As is shown in Fig. 3, when the 4VP dosage is within 10 mL, the adsorptive capacity linearly increases with the monomer dosage and is in a direct proportion with the amount of 4VP grafted on the resin surface. When the volume exceeds 10 mL, the rising tendency of the adsorptive capacity becomes slow probably due to the following reasons: with the increase in the monomer dosage, the density of 4VP on the resin surface increases, resulting in varying degrees of obstruction in the holes on the resin surface and preventing the reactions from proceeding further. Thus, the abovementioned analyses indicate that it is appropriate to control the ATRP reaction time and 4VP dosage within 10 h and 10 mL, respectively.
The infrared spectra are shown in Fig. 4. In Fig. 4(a), the absorption peaks at 759 and 698 cm−1 represent the stretching vibrations of C–Cl in –CH2Cl. After surface modification, when compared with Fig. 4(a), obvious changes in these two characteristic absorption peaks were observed (Fig. 4(b)). In Fig. 4(b), the CN absorption peaks on the pyridine ring appeared near 1605 cm−1, 1597 cm−1, 1557 cm−1, and 1415 cm−1 are the stretching vibration peaks of the pyridine ring, indicating that pyridine groups have been successfully grafted on the surface of the chloromethylated polystyrene resin.
Analysis of the XPS spectra (Fig. 5), showed the modification in the resin structure. There was no N absorption peak in the unmodified CMPS resin; after the SI-ATRP reaction, an N1s absorption peak appeared at 399.8 eV in the spectrum of the P4VP-g-PS resin, indicating that pyridine rings were successfully grafted on the resin surface. XPS analysis also indicated the content of the elements on the resin surface, as shown in Table 1.
Sample | Elemental content/% | ||
---|---|---|---|
C | Cl | N | |
CMPS | 81.4 | 8.12 | 0 |
PS-P4VP(ATRP1h) | 88.55 | 3.16 | 4.57 |
PS-P4VP(ATRP3h) | 67.92 | 6.15 | 5.06 |
PS-P4VP(ATRP5h) | 72.09 | 5.41 | 5.23 |
PS-P4VP(ATRP8h) | 75.02 | 2.03 | 5.36 |
PS-P4VP(ATRP10h) | 74.02 | 3.05 | 5.48 |
PS-P4VP(ATRP16h) | 77.84 | 4.83 | 5.51 |
PS-P4VP(ATRP20h) | 85.81 | 3.19 | 6.46 |
As shown in Table 1, the N content on the surface of P4VP-g-PS resin increases with the increase in the polymerization time. This further verified that the degree of grafting would increase with the increase in the polymerization time.
Peak splitting was further performed for the C1s peak to obtain the detailed information about the changes in the components of the resin surface (Fig. 6).
For CMPS, the C1s peak was split into two peaks at 284.3 and 286.2 eV (Fig. 6(A)), which correspond to C–C and C–C1, respectively. For P4VP-g-PS, the C1s peak was split into three peaks at 284.13 eV, 285.6 eV, and 286.92 eV (Fig. 6(B)), which correspond to C–C, C–N, and C–Cl bonds, respectively, again indicating that the pyridine ring was successfully grafted on the resin surface.
The differences in surface topography of the resin before and after the modification were studied by scanning electron microscopy. Fig. 7 displays the SEM images of the CMPS resin and P4VP-g-PS resin, indicating that obvious changes have occurred in the surface topography of the modified resin. A comparison with the non-modified CMPS resin indicates that the surface of P4VP-g-PS resin became smooth. The probable reasons are as follows: after the use of ATPR technology to graft the 4VP monomer on the CMPS resin surface, the surface is covered with high-density polymer molecular brushes, partially obstructing the original resin holes and therefore making the modified resin surface smooth.
Langmuir and Freundlich adsorption isotherm models were used to explain the experimental data for adsorption. According to the Langmuir model, adsorption of metal ions happened on monomolecular layers with even surfaces, whereas according to the Freundlich model, adsorption of metal ions happened on heterogeneous surfaces. Langmuir adsorption isotherm models are shown in formula (4):
![]() | (4) |
b = (KC − 1) × M/ρ | (5) |
A plot of Ce/Qe versus Ce can generate a straight line with slope of 1/Q0 and intercept of 1/Q0b. Analysis of the experimental data obtained from the Langmuir adsorption isotherm model revealed that Ce/Qe had a linear relationship with Ce and indicated that the adsorption behavior conforms to the Langmuir adsorption isotherm model. The values of b, Q0, and linearly dependent coefficient are shown in Table 2.
Metal ions | Langmuir parameters | Freundlich parameters | |||||
---|---|---|---|---|---|---|---|
Q0 (mmol g−1) | b | KC | RL2 | KF | RF2 | ||
Cd(II) | 1.136 | 1.062 | 60 | 0.98705 | 1.114 | 0.6262 | 0.97244 |
Zn(II) | 2.108 | 1.164 | 65.67 | 0.99284 | 0.649 | 0.6192 | 0.9702 |
Cr(III) | 2.086 | 1.781 | 99.94 | 0.99564 | 1.797 | 0.7999 | 0.94258 |
Pb(II) | 3.11 | 1.823 | 102.28 | 0.9953 | 0.719 | 0.6393 | 0.9569 |
Cr(VI) | 4.695 | 1.284 | 72.33 | 0.98682 | 2.322 | 0.7601 | 0.97896 |
The Freundlich adsorption isotherm model is shown in formula (6):
![]() | (6) |
The value of the linearly dependent coefficient R2 verified that the Langmuir model was a better fit for the experimental data than the Freundlich model; therefore, the adsorption process can be described using the Langmuir model, indicating that the adsorption of resin on heavy metal ions belong to the monomolecular layer adsorption.
As shown in Table 2, the maximum adsorptive capacity of P4VP-g-PS resin for Cr(VI), Pb(II), Cr(III), Zn(II), and Cd(II) was 4.56 mmol g−1, 2.83 mmol g−1, 1.94 mmol g−1, 1.76 mmol g−1, and 1.01 mmol g−1, respectively. The comparison with other reagents is shown in Table 3 and shows that the amount of Cr(VI), Pb(II), Cr(III), Zn(II), and Cd(II) adsorbed by the P4VP-g-PS resin is far higher than those of the other adsorbents. ATRP reaction increases the density of the pyridine ring on the surface of P4VP-g-PS resin, such that the resin has a relatively high adsorptive capacity. This indicates that the adoption of ATRP technology to graft the functional monomer on the resin surface is an effective method to prepare a high-capacity chelating resin.
Adsorbents | Adsorption capacities (mmol g−1) | Reference | ||||
---|---|---|---|---|---|---|
Cr(VI) | Pb(II) | Cr(III) | Zn(II) | Cd(II) | ||
4-Vinyl pyridine/2-hydroxyethylmethacrylate, monomer mixture grafted poly(ethylene terephthalate) fiber | 1.56 | — | — | — | 0.20 | 21 |
Amino-functionalized magnetic cellulose nanocomposite | 3.28 | — | — | — | 22 | |
GA–APTES–glass beads | 0.223 | 0.048 | — | — | — | 23 |
Novel Fe3O4 magnetic nanoparticles (MNPs) modified with 3-aminopropyltriethoxysilane, (APS) and copolymers of acrylic acid (AA) and crotonic acid (CA) | — | 0.37 | — | 0.61 | 0.29 | 24 |
poly(glycidyl methacrylate-co-ethylene dimethacrylate) monolith functionalized with ethylenediamine | — | 0.537 | 3.633 | — | — | 25 |
Sugar beet pulp | — | 0.35 | — | 0.27 | 0.42 | 26 |
Salicylic acid type chelate adsorbent | — | 0.42 | — | 0.48 | 0.98 | 27 |
P4VP-g-PS resins | 4.56 | 2.83 | 1.94 | 1.76 | 1.01 | This work |
Fig. 9 presents a plot of the amount of adsorbed metal ions at equilibrium state versus pH, indicating that changes in the pH value have great effects on the amount of Cr(VI), Pb(II), Cr(III), Zn(II), and Cd(II) adsorbed by the resin. In the case of a pH value of 3.0, the adsorptive capacity for Cr(VI) was the strongest, whereas in the case of a pH value of 5.0, the adsorption capacity for Pb(II), Cr(III), Zn(II), and Cd(II) reached a peak value. The reason behind this phenomenon is the formation of ions and chelating functionality at different pH environments:
![]() | ||
Fig. 9 Effect of pH on the adsorption of P4VP-g-PS resin for Cr(VI), Pb(II), Cr(III), Zn(II), and Cd(II) (initial concentration: 6 mmol L−1; 25 °C; adsorbent dose: 0.1 g). |
(1) When the pH value was relatively low, the N atom on the pyridine ring is easy to be protonated and loaded with positive charges; thus, the adsorptive capacity for Pb(II), Cr(III), Zn(II), and Cd(II) is relatively poor. A very high concentration of H+ at the interface had electrostatic repulsion effects on the positively charged Pb(II), Cr(III), Zn(II), and Cd(II) ions, thereby preventing their approach to the resin surface. A low pH value meant a more obvious protonation effect; a smaller number of nitrogen atoms that experience chelation will be unfavorable to the reaction with the metal ions and will decrease the adsorption performance. In the case of a pH value of 5.0, the N atom on the pyridine ring is electroneutral, but it contains a lone electron pair, which can adsorb Pb(II), Cr(III), Zn(II), and Cd(II) ions, as shown in Fig. 10.
(2) The stability curve of Cr(VI)28,29 showed that the main form of Cr(VI) in the solution is HCrO4−, CrO42−, Cr2O72−, and other oxygen-containing anions. In the case of a relatively low pH value, HCrO4− is the main species, whereas CrO42− is the main form at a pH greater than 7.0. In the case of a pH value of 3.0, the N atom on the pyridine is protonated and positively charged, and the protonated groups can attract the anions including Cr(VI) through the electrostatic interactions. In the case of an increase in the pH value, the protonated groups relatively decrease and the adsorption of Cr(VI) through electrostatic interactions is not important anymore, as shown in Fig. 11.
The abovementioned analysis indicate that the optimum pH value for the selective separation of Cr(VI) from Pb(II), Cr(III), Zn(II), and Cd(II) was 3.0.
A thermodynamic study was employed to better explain the reaction process, and some thermodynamic studies, such as Gibbs free energy (ΔG), enthalpy change (ΔH), and entropy change (ΔS), can be obtained through the calculation via the following formulas (7) and (8):
ΔG = −RT![]() ![]() | (7) |
ΔG = ΔH − TΔS | (8) |
The van't Hoff equation can be deduced through the formulas (7) and (8) as follows:
ln![]() | (9) |
The results of the analysis of data presented in Fig. 12 using formulas (7) to (9) are shown in Table 4.
Metal ions | ΔH (kJ mol−1) | ΔS (J mol−1 K−1) | ΔG (kJ mol−1) | ||
---|---|---|---|---|---|
25 °C | 35 °C | 45 °C | |||
Cd(II) | 5.594 | 52.8 | −10.14 | −10.65 | −11.23 |
Zn(II) | 2.384 | 42.8 | −10.37 | −10.79 | −11.24 |
Cr(III) | 5.576 | 57 | −11.41 | −11.98 | −12.55 |
Pb(II) | 10.433 | 73.5 | −11.47 | −12.19 | −12.97 |
Cr(VI) | 7.508 | 60.8 | −10.61 | −11.21 | −11.84 |
As shown in the analysis of the thermodynamic data in Table 4, ΔG is a negative value, indicating that the adsorption process of P4VP-g-PS resin on the metal ions is spontaneous; with the increase in temperature, ΔG value slightly decreases, indicating that the adsorptive capacity will somewhat increase at a relatively high temperature. ΔH and ΔS were positive, indicating that the adsorption process of P4VP-g-PS resin on metal ions was a heat-absorbing and entropy-driven spontaneous process.
As shown in Fig. 13, the adsorption rate was relatively rapid at the beginning, and then it gradually flattened out. The time taken by the five kinds of metal ions to reach the adsorption equilibrium is within 120 min. During metal ion adsorption by porous adsorbents, metal ions must first reach the boundary, then diffuse to the resin surface and enter the porous structures of the resin to bind with the chelation sites. Therefore, a relatively long contact time is required during the adsorption process.
The adsorption mechanism of resin can be predicted through the adsorption kinetic study. The ion exchange process was very rapid and mainly controlled through the diffusion rate. Chelation was activated very slowly and was often dependent on the particle diffusion mechanism of a quasi-secondary reaction.
The kinetic equation of a quasi-secondary reaction is given as follows:
![]() | (10) |
Formula (10) is used for the curve fitting of the adsorption kinetic data; plotting of t/Qt against t generated a straight line. The linearly dependent coefficient of the straight line was greater than 0.998, indicating that adsorption of resin for Cr(VI), Pb(II), Cr(III), Zn(II), and Cd(II) conformed to a quasi-secondary kinetic model and further proved that the P4VP-g-PS resin adsorbed the metal ions via chelation effects. Through the intercept and the slope of the straight line, the reaction rate constant of Cr(VI), Pb(II), Cr(III), Zn(II), and Cd(II) were obtained to be 0.689, 0.703, 0.375, 0.230, and 0.194 g mmol−1 h−1.
Under normal circumstances, electrostatic interactions, surface complexation, and ion exchange are often considered as the main adsorption mechanisms. As previously reported, the pyridine ring functional groups on the resin surface can effectively adsorb Cr(VI)30 in a solution. Therefore, the interaction between the P4VP-g-PS resin and metal ions mainly depends on the pyridine rings on the resin surface. In a multicomponent system, P4VP-g-PS presents a relatively high affinity for Cr(VI) and the existence of Zn(II) and Cd(II) in the solution has few effects on the adsorption of Cr(VI) by P4VP-g-PS resin. In the binary solutions of Cr(VI)–Zn(II), Cr(VI)–Cd(II), Cr(VI)–Cr(III), and Cr(VI)–Pb(II) and the quinary Cr(VI)–Pb(II)–Cr(III)–Zn(II)–Cd(II) systems, the adsorption selectivity for Cr(VI) was as high as 98%. In the case of a pH value of 3.0, P4VP-g-PS resin highly selectively adsorbs Cr(VI) in the secondary or quinary solution. Therefore, in the solution containing Pb(II), Cr(VI), Cr(III), Zn(II), and C(II), P4VP-g-PS resin quantitatively and selectively adsorbed Cr(VI) via controlling the pH value of solution.
To investigate the regeneration performance of the resin, the metal ions were adsorbed and desorbed using the same method over ten cycles, and the experimental results are shown in Table 5.
Cycle | Adsorption capacities (mmol g−1) | ||||
---|---|---|---|---|---|
Cd(II) | Zn(II) | Cr(III) | Pb(II) | Cr(VI) | |
1 | 1.01 | 1.76 | 1.94 | 2.83 | 4.56 |
2 | 1.00 | 1.76 | 1.93 | 2.82 | 4.56 |
3 | 1.00 | 1.74 | 1.93 | 2.82 | 4.56 |
4 | 0.97 | 1.75 | 1.92 | 2.81 | 4.54 |
5 | 0.98 | 1.74 | 1.92 | 2.80 | 4.53 |
6 | 0.95 | 1.73 | 1.90 | 2.83 | 4.55 |
7 | 0.97 | 1.75 | 1.91 | 2.82 | 4.52 |
8 | 0.96 | 1.74 | 1.92 | 2.79 | 4.53 |
9 | 0.99 | 1.73 | 1.91 | 2.78 | 4.54 |
10 | 0.95 | 1.72 | 1.91 | 2.79 | 4.52 |
As shown in Table 5, after 10 adsorption–desorption cycles, the adsorptive capacity for Cr(VI) decreased by only 0.88%, whereas that for Pb(II), Cr(III), Zn(II), and Cd(II) decreased by 1.41%, 1.55%, 2.27%, and 5.94%, respectively. This fully demonstrated that P4VP-g-PS resin has excellent performance for repeated use.
The maximal adsorptive capacities of 4-vinylpyridine resin for Cr(VI), Pb(II), Cr(III), Zn(II), and Cd(II) were 4.56 mmol g−1, 2.83 mmol g−1, 1.94 mmol g−1, 1.76 mmol g−1, and 1.01 mmol g−1, respectively. When the pH value was greater than 5.0, the resin can adsorb Pb(II), Cr(III), Zn(II), and Cd(II) ions; when the pH value was less than 3.0, the resin can selectively adsorb Cr(VI). The method has a good metal ion desorption rate and good performance for repeated use, without obvious change in the adsorptive capacity. Therefore, 4-vinylpyridine resin had potential prospects of application during the processing of heavy metal wastewater.
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