Synthesis and Application of Novel Magnetic Ion-Imprinted Polymers for Selective Solid Phase Extraction of Cadmium (II)

Ion-imprinted polymers (IIPs) have received much attention in the fields of separation and purification. Nevertheless, selectivity of IIPs for trace target ions in complicated matrix remains a challenge. In this work, a cadmium magnetic ion-imprinted polymer (MIIP) was synthesized via surface imprinting, using methacrylic acid and acrylamide as dual functional monomers, vinyltrimethoxysilane as ligand, Fe3O4@SiO2 as support, azodiisobutyronitrile as initiator, and ethylene glycol dimethacrylate as crosslinker. The MIIP was characterized by transmission electron microscopy, infrared spectroscopy, thermal gravimetric analysis, and a vibrating sample magnetometer. The maximum adsorption capacities of the MIIP and magnetic non-imprinted polymer for Cd(II) were 46.8 and 14.7 mg·g−1, respectively. The selectivity factors of Pb(II), Cu(II), and Ni(II) were 3.17, 2.97, and 2.57, respectively, which were greater than 1. The adsorption behavior of Cd(II) followed the Freundlich isotherm and a pseudo second order model. The MIIP was successfully used for the selective extraction and determination of trace Cd(II) in representative rice samples. The limit of detection and recovery of the method was 0.05 µg·L−1 and 80–103%, respectively, with a relative standard deviation less than 4.8%. This study shows that MIIP provides an attractive strategy for heavy metal detection.


Introduction
Cadmium is one of the most toxic heavy metals and causes serious harm to human health via the food chain [1,2]. The International Agency for Research on Cancer classified cadmium as a human carcinogen [3]. Therefore, developing reliable methods for the removal and determination of cadmium in food is important. A wide range of analytical techniques to evaluate cadmium(II) in the spiked or real samples have been reported in recent years, including atomic absorption spectrometry (AAS) [4], inductively coupled plasma mass spectrometry (ICP-MS) [5], electrochemical sensor [6]. Among them, atomic absorption spectrometry has been popular because of its simplicity, easy operation, and low cost [7]. However, its low sensitivity in trace analysis of complex systems largely limits its applications because of the matrix interferences [8]. Therefore, a suitable separation and preconcentration step such as solid-phase extraction is necessary for concentrating the target analytes from real samples [9].
Ion imprinting is a process in which co-polymerization has been performed between functional and cross-linking monomers in the presence of a target ion (the imprint ion) [10]. Extraction of the template molecules leaves a predetermined arrangement of ligands and a tailored binding pocket [11]. Now, ion-imprinted polymers (IIPs) are becoming promising solid-phase extraction (SPE) sorbents and have gained much attention because of their outstanding advantages such as high selectivity, large adsorption capacity, and good reusability [12,13]. Ghorbani et al. [14] successfully synthesized Pd(II) ion-imprinted polymers for selective extraction and determination in food and environmental samples. A Ni(II) ion-imprinted polymer prepared by Saraji et al. [15] was employed as a sorbent in a solid-phase extraction column to preconcentrate trace nickel with satisfactory results. However, complicated post-processing, such as filtration and centrifugation, are required when applying these ion-imprinted polymers [16]. If ion-imprinted polymer materials are chemically grafted onto Fe 3 O 4 nanoparticles, which have unique magnetic properties and high surface area, easy separation and selective extraction can be achieved with the application of an external magnetic field. Previously published papers have shown a successful combination of ion-imprinted polymers and Fe 3 O 4 , and superior performance from magnetic imprinted polymers was reported compared with that of imprinted polymers without magnetic nanoparticles attached [17][18][19].
Despite the emerged interests in magnetic ion imprinting techniques, single functional monomers are widely and generally used for preparing imprinted polymers and thereby result in low selectivity. Thus, it has become quite imperative to develop new functional monomers and/or utilize dual/multiple functional monomers for improving the selective recognition capabilities and adsorption capacities of IIPs [20]. In the present work, a novel magnetic ion-imprinted polymer (MIIP) for Cd(II) was synthesized using dual functional monomers of MAA and acrylamide (AM) by surface imprinting. In addition, the characterization, kinetics, isotherm model of Cd(II) adsorption process, selectivity, and application of this new magnetic sorbent are discussed in this study.

Reagents and Chemicals
Cd, Pb, Cu, and Ni reference solutions were supplied by Shanghai Macklin Biochemical Co., Ltd. (Shanghai, China), with a minimum 99% purity. All other reagents and chemicals including FeCl 3 ·6H 2 O, FeCl 2 ·4H 2 O, PEG200, CdCl 2 ·5/2H 2 O, tetraethyl orthosilicate, vinyltrimethoxysilane, hexadecyl trimethyl ammonium bromide, methacrylic acid, acrylamide, ethylene glycol, dimethacrylate, and azodiisobutyronitrile were in analytical grade and purchased from Aladdin Industrial Corporation (Shanghai, China). Cd standard solution (100 mg·L −1 ) was prepared by diluting a reference solution in 2% nitric acid solution. All of the solutions were stored in the fridge (4 • C) and allowed to reach ambient temperature prior to use. The water used was ultrapure (18.3 MΩ·cm resistivity).

Characterization
An AA800 graphite furnace atomic absorption spectrometer (Perkin Elmer, Shelton, CT, USA) was used to determine the concentration of metal ions (Cd, Ni, Cu, and Pb) in aqueous solution. The instrumental parameters were those recommended by the manufacturer. Hollow cathode lamps were used as the radiation sources. The wavelengths selected were 228.8, 232.0, 324.8, and 283.3 nm for Cd, Ni, Cu, and Pb, respectively. A 780 digital pH Meter (Metrohm, Herisau, Switzerland), equipped with a combined Ag/AgCl glass electrode was used for the pH adjustments at room temperature. Fourier transform infrared (FT-IR) spectra (4000-500 cm −1 ) were recorded using a Vertex 70 spectrometer (Bruker, Ettlingen, Germany) with KBr pellets and a resolution of 0.4 cm −1 . Transmission electron microscope (TEM) images were acquired on a JEM-2100F instrument (JEOL, Peabody, MA, USA). Thermal gravimetric analysis (TGA) was performed on a TG209 F1 Libra instrument (Netzsch, Hanau, Germany) under argon atmosphere at a heating rate of 10 • C/min. Magnetic characteristics of Fe 3

Preparation of Vinyl-Functionalized Fe 3 O 4 Nanoparticles
Fe 3 O 4 nanoparticles were synthesized by the method of titration hydrolysis with minor modification [21]. Briefly, 0.02 mol FeCl 3 ·6H 2 O and 0.012 mol FeCl 2 ·4H 2 O were dissolved in 100 mL of deionized water under a nitrogen atmosphere. This solution was subsequently heated to 80 • C by a magnetic stirrer, followed by the addition of 15 mL of NH 3 ·H 2 O (32% solution) and 2 mL of PEG200 sequentially. The resultant Fe 3 O 4 nanoparticles were separated by a magnet, washed three times with ethanol and ultrapure water, and dried in a vacuum oven at 60 • C overnight.
Vinyl modified Fe 3 O 4 nanoparticles were performed as previously reported [22,23]. Fe 3 O 4 nanoparticles (0.5 g), 50 mL of anhydrous ethanol and 10 mL of NH 3 ·H 2 O were suspended in 100 mL of deionized water, and 2 mL of tetraethyl orthosilicate was added to the mixture dropwise. The Fe 3 O 4 @SiO 2 was obtained under stirring at room temperature after 6 h. The Fe 3 O 4 @SiO 2 was dispersed in 100 mL of the mixture of water and ethanol (1:5, v/v). Ammonia water (10 mL) containing 2 g of hexadecyl trimethyl ammonium bromide, 4 mL of tetraethyl orthosilicate, and 3.7 mL of vinyltrimethoxysilane were added into the above mixture under vigorous stirring. After reaction at ambient temperature for 6 h, the resultant products were refluxed in acetone solution at 80 • C for 24 h to remove the hexadecyl trimethyl ammonium bromide.

Preparation of Magnetic Cadmium Ion-imprinted Polymer
The preparation of magnetic cadmium ion-imprinted polymer is schematically shown in Figure 1. Briefly, 0.5 mmol of CdCl 2 ·5/2H 2 O, 1.5 mmol of methacrylic acid, and 0.5 mmol of acrylamide were dispersed into a mixture solution of acetonitrile (40 mL) and water (10 mL) under stirring at room temperature for 90 min. Then 0.5 g of vinyl-modified Fe 3 O 4 @SiO 2 , 1.98 g of ethylene glycol dimethacrylate and 0.15 g of azodiisobutyronitrile were added consecutively. The polymerization reaction was performed at 85 • C with 10 h of stirring to obtain particles with a highly crosslinked structure. The product was separated with an external magnetic force, washed with ethanol, and oven-dried at 65 • C for 6 h. The template was removed by 2.0 M of HCl. For comparison, magnetic non-imprinted polymer (MNIP) was also prepared using an identical procedure in the absence of the template (cadmium ions).

Preparation of Vinyl-Functionalized Fe3O4 Nanoparticles
Fe3O4 nanoparticles were synthesized by the method of titration hydrolysis with minor modification [21]. Briefly, 0.02 mol FeCl3·6H2O and 0.012 mol FeCl2·4H2O were dissolved in 100 mL of deionized water under a nitrogen atmosphere. This solution was subsequently heated to 80 °C by a magnetic stirrer, followed by the addition of 15 mL of NH3·H2O (32% solution) and 2 mL of PEG200 sequentially. The resultant Fe3O4 nanoparticles were separated by a magnet, washed three times with ethanol and ultrapure water, and dried in a vacuum oven at 60 °C overnight.
Vinyl modified Fe3O4 nanoparticles were performed as previously reported [22,23]. Fe3O4 nanoparticles (0.5 g), 50 mL of anhydrous ethanol and 10 mL of NH3·H2O were suspended in 100 mL of deionized water, and 2 mL of tetraethyl orthosilicate was added to the mixture dropwise. The Fe3O4@SiO2 was obtained under stirring at room temperature after 6 h. The Fe3O4@SiO2 was dispersed in 100 mL of the mixture of water and ethanol (1:5, v/v). Ammonia water (10 mL) containing 2 g of hexadecyl trimethyl ammonium bromide, 4 mL of tetraethyl orthosilicate, and 3.7 mL of vinyltrimethoxysilane were added into the above mixture under vigorous stirring. After reaction at ambient temperature for 6 h, the resultant products were refluxed in acetone solution at 80 °C for 24 h to remove the hexadecyl trimethyl ammonium bromide.

Preparation of Magnetic Cadmium Ion-imprinted Polymer
The preparation of magnetic cadmium ion-imprinted polymer is schematically shown in Figure  1. Briefly, 0.5 mmol of CdCl2·5/2H2O, 1.5 mmol of methacrylic acid, and 0.5 mmol of acrylamide were dispersed into a mixture solution of acetonitrile (40 mL) and water (10 mL) under stirring at room temperature for 90 min. Then 0.5 g of vinyl-modified Fe3O4@SiO2, 1.98 g of ethylene glycol dimethacrylate and 0.15 g of azodiisobutyronitrile were added consecutively. The polymerization reaction was performed at 85 °C with 10 h of stirring to obtain particles with a highly crosslinked structure. The product was separated with an external magnetic force, washed with ethanol, and oven-dried at 65 °C for 6 h. The template was removed by 2.0 M of HCl. For comparison, magnetic non-imprinted polymer (MNIP) was also prepared using an identical procedure in the absence of the template (cadmium ions).

Adsorption Experiments
The adsorption of Cd(II) from aqueous solutions was investigated in batch experiments. The effect of pH on the adsorption capacity of the MIIP sorbents was studied with 20 mL of 70 µg·mL −1 Cd(II) solutions in the pH range 1.0-6.3. The pH of the suspensions was changed using 0.1 M HCl or 0.1 M NH3·H2O. The static adsorption rates were studied with 20 mL of 70 µg·mL −1 Cd (II) solutions at pH 6.0 from 5 to 70 min. To measure the maximum adsorption capacity of MIIP and MNIP, the  solutions at pH 6.0 from 5 to 70 min. To measure the maximum adsorption capacity of MIIP and MNIP, the obtained MIIP (20 mg) and MNIP (20 mg) were added with 20 mL Cd(II) solutions containing different initial concentrations (30-80 µg·mL −1 ) at a constant temperature of 25 • C for 35 min. After complete adsorption, the adsorbent was collected with an external magnetic force, and the supernatant was introduced into the graphite furnace atomic absorption spectrometer for determining Cd(II) concentration. To assess the reusability of MIIP, 20 mg MIIP was added into cadmium standard aqueous solution (70 µg·mL −1 ) for a multiple adsorption-elution-adsorption process under the same conditions. The amount of Cd(II) bound by the polymer was calculated by the following equation:

Adsorption Experiments
where Q represents the amount of Cd(II) adsorbed (mg·g −1 ), C 0 and C e are the initial and equilibrium concentration (µg·mL −1 ) of Cd(II), respectively, V is the volume of cadmium standard solution (mL), and W is the mass of sorbent (g). All the tests were performed in triplicate.
To investigate the mechanism of the adsorption process, the Freundlich and Langmuir models were applied to fit the adsorption data. The Freundlich and Langmuir adsorption isothermal equations are as follows [24,25]: where Q e is the equilibrium adsorption capacity (mg·g −1 ), C e is the equilibrium concentration, K f and n are the Freundlich constants related to the adsorption capacity and intensity, respectively, Q max represents the maximum adsorption capacity, and K b is the Langmuir constant representing the affinity between the solute and adsorbent. To further understand the mechanism of the adsorption process, two different kinetic models (Laguerre pseudo-first-order and pseudo-second-order kinetic models) were used to fit the kinetic data. The two kinetic models for the adsorption of solid/liquid system are as follows [26,27]: where F equals to Q t /Q e , Q t and Q e are the adsorption capacities of Cd(II) at time t and at equilibrium, respectively, and k a and k b are the first order and second order rate constants, respectively. The selective adsorption experiments of Pb(II), Cu(II), and Ni(II) ions with respect to Cd(II) ions were conducted using MIIP or MNIP sorbents. Briefly, 20 mg of MIIP and MNIP sorbents were added to 20 mL of a binary mixture containing 20 mg·mL −1 Cd(II)/Pb(II), Cd(II)/Cu(II), or Cd(II)/Ni(II) at pH 6.0 for 35 min. The imprinting factor (α) and selectivity factor (β) for Cd(II) ions relative to competing ions were calculated from the following equations: where Q A and Q B represent adsorption capacities of metal ions onto MIIP and MNIP, respectively, and α 1 and α 2 are imprinting factors of Cd(II) and other ions.

Real Sample Pretreatment
To evaluate the practicability of MIIP for Cd(II) extraction from real samples with different matrices, rice 1 (Hunan, China), rice 2 (Heilongjiang, China), and rice 3 (Shandong, China) were selected. Because there were trace Cd(II) in the three rice samples, 0.5, 1, and 2 ng·mL −1 Cd(II) standard solutions were also spiked in the above rice samples.
The three spiked rice samples were subjected to acid digestion according to the previously published method [28]. Afterwards, 20 mL of digested solution was transferred into a 50 mL conical flask to form a dark cloudy suspension. Then, MIIP sorbent (30 mg) was added into the sample solution after adjusting the pH to neutral. Extraction was achieved by shaking the sample solution for 35 min. The sorbent was separated by a magnet, and the solution became clear. The sorbent was eluted with 2 M HCl. After 8 h, the supernatant was obtained, and the concentration of Cd(II) ion was determined by graphite furnace atomic absorption spectrometry.

Characterization
The infrared spectra of  The three spiked rice samples were subjected to acid digestion according to the previously published method [28]. Afterwards, 20 mL of digested solution was transferred into a 50 mL conical flask to form a dark cloudy suspension. Then, MIIP sorbent (30 mg) was added into the sample solution after adjusting the pH to neutral. Extraction was achieved by shaking the sample solution for 35 min. The sorbent was separated by a magnet, and the solution became clear. The sorbent was eluted with 2 M HCl. After 8 h, the supernatant was obtained, and the concentration of Cd(II) ion was determined by graphite furnace atomic absorption spectrometry.

Characterization
The infrared spectra of Fe3O4, Fe3O4@SiO2, Fe3O4@SiO2-C=C, and MIIP are displayed in Figure 2. The adsorption peak at 589 cm −1 observed in all samples can be assigned to Fe-O stretching vibrations, which indicated the presence of Fe3O4. These peaks intensity diminished as ion-imprinted polymer was layered onto Fe3O4 [29]. The peaks of Fe3O4@SiO2 at 1100, 953, and 801 cm −1 corresponded to the Si-O-Si, Si-O-H, and Si-O stretching, respectively, and indicated that the silica was modified onto the surface of Fe3O4 successfully. The peaks at 1603, 3063, and 3026 cm −1 coming from C=C stretching suggested that the vinyl groups were grafted onto the surface of Fe3O4@SiO2. The peak of MIIP at 1732 cm −1 was the characteristic group frequencies of the C=O stretching vibration, and the appearance of the stretching vibrations at 1263 cm −1 belonging to C-N-H indicated that methacrylic acid and acrylamide were both involved in the imprinted polymerization. Appropriate MIIP shell thickness enables easy access for the target ions and leads to higher adsorption capacity [30]. Figure 3 showed the morphology and microstructure of the Fe3O4 and MIIP. Magnetic Fe3O4 particles were spherical and uniform in size, with an average diameter of 20 nm. After polymerization, the Fe3O4 particles were coated with a thick layer, and the surface was rough and irregular. The diameter of MIIP was larger compared with that of Fe3O4 and the thickness of the MIIP was about 100 nm. The TEM micrograph observations confirmed that the imprinted layer was successfully immobilized on the surface of Fe3O4 particles. Appropriate MIIP shell thickness enables easy access for the target ions and leads to higher adsorption capacity [30]. The magnetic hysteresis loops of Fe3O4 and MIIP are illustrated in Figure 4. The two loops showed similar shapes and coercive force, which indicated that both of them were superparamagnetic in nature. The saturation magnetization of Fe3O4 was 55.6 emu·g −1 . In comparison, the MIIP showed a lower saturation magnetization, which was 4.88 emu·g −1 , suggesting the formation of the polymer layer on the surface of Fe3O4@SiO2. Therefore, the magnetic separation of MIIP can be achieved with an external magnetic force.
The thermogravimetric curves of MIIP and Fe3O4@SiO2 have been established from room temperature (25 °C) to 800 °C. As shown in Figure 5, Fe3O4@SiO2 exhibited weight loss of less than 16% during the whole process. MIIP had a slight weight loss of about 5% up to 300 °C, which might be assigned to the physical evaporation of H2O. The other loss (about 80%) of mass of MIIP occurred between 300 and 600 °C, and was attributed to the thermal decomposition of the organic component in the MIIP. The above results indicate that there is a thin imprinted layer on the surface of Fe3O4, which is in agreement with the observations from TEM and magnetism analysis. It also demonstrates that the sorbent prepared in this study has a good thermal stability, so it can be used in a wide temperature range.
.  The thermogravimetric curves of MIIP and Fe 3 O 4 @SiO 2 have been established from room temperature (25 • C) to 800 • C. As shown in Figure 5, Fe 3 O 4 @SiO 2 exhibited weight loss of less than 16% during the whole process. MIIP had a slight weight loss of about 5% up to 300 • C, which might be assigned to the physical evaporation of H 2 O. The other loss (about 80%) of mass of MIIP occurred between 300 and 600 • C, and was attributed to the thermal decomposition of the organic component in the MIIP. The above results indicate that there is a thin imprinted layer on the surface of Fe 3 O 4 , which is in agreement with the observations from TEM and magnetism analysis. It also demonstrates that the sorbent prepared in this study has a good thermal stability, so it can be used in a wide temperature range.  The magnetic hysteresis loops of Fe3O4 and MIIP are illustrated in Figure 4. The two loops showed similar shapes and coercive force, which indicated that both of them were superparamagnetic in nature. The saturation magnetization of Fe3O4 was 55.6 emu·g −1 . In comparison, the MIIP showed a lower saturation magnetization, which was 4.88 emu·g −1 , suggesting the formation of the polymer layer on the surface of Fe3O4@SiO2. Therefore, the magnetic separation of MIIP can be achieved with an external magnetic force.
The thermogravimetric curves of MIIP and Fe3O4@SiO2 have been established from room temperature (25 °C) to 800 °C. As shown in Figure 5, Fe3O4@SiO2 exhibited weight loss of less than 16% during the whole process. MIIP had a slight weight loss of about 5% up to 300 °C, which might be assigned to the physical evaporation of H2O. The other loss (about 80%) of mass of MIIP occurred between 300 and 600 °C, and was attributed to the thermal decomposition of the organic component in the MIIP. The above results indicate that there is a thin imprinted layer on the surface of Fe3O4, which is in agreement with the observations from TEM and magnetism analysis. It also demonstrates that the sorbent prepared in this study has a good thermal stability, so it can be used in a wide temperature range. .

Adsorption Capacity
Adsorption capacity is an important indicator for the evaluation of the sorbent. Figure 6 showed the effect of the initial concentration of Cd(II) ion on the adsorption capacity. The adsorption amount of MIIP and MNIP increased with the increase of cadmium ion solution concentration within 30-80

Adsorption Capacity
Adsorption capacity is an important indicator for the evaluation of the sorbent. Figure 6 showed the effect of the initial concentration of Cd(II) ion on the adsorption capacity. The adsorption amount of MIIP and MNIP increased with the increase of cadmium ion solution concentration within 30-80 µg·mL −1. The adsorption capacity of MIIP was higher than that of the MNIP under the same experimental concentration, suggesting that Cd(II)-MIIP had imprinted sites because of template ions added during synthesis. The maximum static adsorption capacities of the MIIP and MNIP for Cd(II) ion were 46.80 and 14.70 mg·g −1 , respectively. The fitting results for the Langmuir and Freundlich isotherms are shown in Figure 7. Compared with the Langmuir model, the Freundlich model was more suitable because of the value of the correlation coefficients (R 2 ), which suggests that the adsorption of Cd(II) ion onto the MIIP was a multilayer adsorption, and the adsorption occurred on a heterogeneous surface with different active sites.

Adsorption Capacity
Adsorption capacity is an important indicator for the evaluation of the sorbent. Figure 6 showed the effect of the initial concentration of Cd(II) ion on the adsorption capacity. The adsorption amount of MIIP and MNIP increased with the increase of cadmium ion solution concentration within 30-80 µg·mL −1. The adsorption capacity of MIIP was higher than that of the MNIP under the same experimental concentration, suggesting that Cd(II)-MIIP had imprinted sites because of template ions added during synthesis. The maximum static adsorption capacities of the MIIP and MNIP for Cd(II) ion were 46.80 and 14.70 mg·g −1 , respectively. The fitting results for the Langmuir and Freundlich isotherms are shown in Figure 7. Compared with the Langmuir model, the Freundlich model was more suitable because of the value of the correlation coefficients (R 2 ), which suggests that the adsorption of Cd(II) ion onto the MIIP was a multilayer adsorption, and the adsorption occurred on a heterogeneous surface with different active sites.

Adsorption Kinetics
The effect of contact time on the adsorption capacity of Cd(II) ion on the MIIP in aqueous solution at pH 5.0 at room temperature is presented in Figure 8. The amount of Cd ion uptake increased rapidly with the increase of contact time during the first 5 min. From 5 to 35 min, the adsorption amount increased slowly, and a plateau was reached with equilibrium. These results show that there were a large number of specific binding sites on the sorbent surface, which were available for the adsorption of Cd(II) at the early stage. Gradually, the specific binding sites were completely occupied. Furthermore, the adsorption kinetic curve of MNIP was similar to that of MIIP except that the saturated adsorption amount was lower. This difference in capacity was because the cavities left in the MIIP were complementary in size and shape to the template ion, whereas there were no imprinted sites in the MNIP.

Adsorption Kinetics
The effect of contact time on the adsorption capacity of Cd(II) ion on the MIIP in aqueous solution at pH 5.0 at room temperature is presented in Figure 8. The amount of Cd ion uptake increased rapidly with the increase of contact time during the first 5 min. From 5 to 35 min, the adsorption amount increased slowly, and a plateau was reached with equilibrium. These results show that there were a large number of specific binding sites on the sorbent surface, which were available for the adsorption of Cd(II) at the early stage. Gradually, the specific binding sites were completely occupied. Furthermore, the adsorption kinetic curve of MNIP was similar to that of MIIP except that the saturated Polymers 2017, 9, 360 8 of 12 adsorption amount was lower. This difference in capacity was because the cavities left in the MIIP were complementary in size and shape to the template ion, whereas there were no imprinted sites in the MNIP.
The effect of contact time on the adsorption capacity of Cd(II) ion on the MIIP in aqueous solution at pH 5.0 at room temperature is presented in Figure 8. The amount of Cd ion uptake increased rapidly with the increase of contact time during the first 5 min. From 5 to 35 min, the adsorption amount increased slowly, and a plateau was reached with equilibrium. These results show that there were a large number of specific binding sites on the sorbent surface, which were available for the adsorption of Cd(II) at the early stage. Gradually, the specific binding sites were completely occupied. Furthermore, the adsorption kinetic curve of MNIP was similar to that of MIIP except that the saturated adsorption amount was lower. This difference in capacity was because the cavities left in the MIIP were complementary in size and shape to the template ion, whereas there were no imprinted sites in the MNIP. The corresponding linear regression correlation coefficients, R 2 , were calculated from the linear plots of Equations (4) and (5) and are shown in Figure 9. The Lagergren pseudo-first-order kinetic model showed an R 2 average of 0.951. However, the pseudo-second-order model showed a higher R 2 value (more than 0.99). In addition, the calculated Qe values also agreed with the experimental data in the case of pseudo-second-order kinetics. The above results indicated that the pseudo-secondorder kinetic model was more suitable to predict the adsorption process of Cd(II) onto MIIP. The corresponding linear regression correlation coefficients, R 2 , were calculated from the linear plots of Equations (4) and (5) and are shown in Figure 9. The Lagergren pseudo-first-order kinetic model showed an R 2 average of 0.951. However, the pseudo-second-order model showed a higher R 2 value (more than 0.99). In addition, the calculated Q e values also agreed with the experimental data in the case of pseudo-second-order kinetics. The above results indicated that the pseudo-second-order kinetic model was more suitable to predict the adsorption process of Cd(II) onto MIIP.

Selectivity Adsorption
Pb(II), Cu(II), and Ni(II) ions were used as competitive metal ions because of their similar charge and ionic radius with Cd(II). Table 1 showed that the imprinting factors of Cd(II), Pb(II), Cu(II), and Ni(II) were 3.42, 1.08, 1.15, and 1.33, respectively. The selectivity factors of Pb(II), Cu(II), and Ni(II) were 3.17, 2.97, and 2.57, respectively. Figure 10 showed that MIIP exhibited a higher selectivity toward Cd(II) than other ions despite their similar size and charge in solution. Therefore, the high affinity, because of using template ions during imprinting, enabled the MIIP sorbent to extract Cd(II) selectively in the presence of other metal ions.

Selectivity Adsorption
Pb(II), Cu(II), and Ni(II) ions were used as competitive metal ions because of their similar charge and ionic radius with Cd(II). Table 1 showed that the imprinting factors of Cd(II), Pb(II), Cu(II), and Ni(II) were 3.42, 1.08, 1.15, and 1.33, respectively. The selectivity factors of Pb(II), Cu(II), and Ni(II) were 3.17, 2.97, and 2.57, respectively. Figure 10 showed that MIIP exhibited a higher selectivity toward Cd(II) than other ions despite their similar size and charge in solution. Therefore, the high affinity, because of using template ions during imprinting, enabled the MIIP sorbent to extract Cd(II) selectively in the presence of other metal ions.

Selectivity Adsorption
Pb(II), Cu(II), and Ni(II) ions were used as competitive metal ions because of their similar charge and ionic radius with Cd(II). Table 1 showed that the imprinting factors of Cd(II), Pb(II), Cu(II), and Ni(II) were 3.42, 1.08, 1.15, and 1.33, respectively. The selectivity factors of Pb(II), Cu(II), and Ni(II) were 3.17, 2.97, and 2.57, respectively. Figure 10 showed that MIIP exhibited a higher selectivity toward Cd(II) than other ions despite their similar size and charge in solution. Therefore, the high affinity, because of using template ions during imprinting, enabled the MIIP sorbent to extract Cd(II) selectively in the presence of other metal ions.

Effect of Sample pH
pH is one of the most important parameters for the adsorption performance of MIIP. The influence of different pH values in the range of 1.0-6.3 on the adsorption capacity of MIIP was studied, and the results are presented in Figure 11a. The results showed that the adsorption capacity increased quickly with the increase of pH value from 1.0 to 4.0, and then remained constant in the pH range of 4.0-6.3. Because the positive charge on the surface of MIIP protonates binding sites, the affinity between MIIP and Cd(II) was weakened at low pH values, and a decrease in adsorption capacity was observed [26]. Thus, the optimum pH was 6.0.

Reusability
The reusability and stability of MIIP were studied by eluting and reusing the same sorbent, and the adsorption results are presented in Figure 11b. As shown in Figure 11b, during the six adsorption-desorption cycles, there was no significant decrease in the adsorption capacity for Cd (II), and the recovery was higher than 90%. The above results indicated that MIIP showed a stable regeneration adsorption efficiency and can be used repeatedly.

Effect of Sample pH
pH is one of the most important parameters for the adsorption performance of MIIP. The influence of different pH values in the range of 1.0-6.3 on the adsorption capacity of MIIP was studied, and the results are presented in Figure 11a. The results showed that the adsorption capacity increased quickly with the increase of pH value from 1.0 to 4.0, and then remained constant in the pH range of 4.0-6.3. Because the positive charge on the surface of MIIP protonates binding sites, the affinity between MIIP and Cd(II) was weakened at low pH values, and a decrease in adsorption capacity was observed [26]. Thus, the optimum pH was 6.0.

Reusability
The reusability and stability of MIIP were studied by eluting and reusing the same sorbent, and the adsorption results are presented in Figure 11b. As shown in Figure 11b, during the six adsorptiondesorption cycles, there was no significant decrease in the adsorption capacity for Cd (II), and the recovery was higher than 90%. The above results indicated that MIIP showed a stable regeneration adsorption efficiency and can be used repeatedly.

Analytical Performance of the Method
As shown in Table 2, the recoveries of Cd(II) ions from the real and spiked samples varied in the range of 80%-103%, and the relative standard deviation was less than 4.8%. The limit of detection, defined as CLOD = 3 Sb/m, where Sb is the standard deviation of seven replicate blank signals and m is the slope of the linear section of calibration curve after preconcentration for a sample volume of 50 mL, was 0.05 µg·L −1 . In comparison with other reported Cd((II) IIPs for SPE extraction (Table 3), the

Analytical Performance of the Method
As shown in Table 2, the recoveries of Cd(II) ions from the real and spiked samples varied in the range of 80-103%, and the relative standard deviation was less than 4.8%. The limit of detection, defined as C LOD = 3 S b /m, where S b is the standard deviation of seven replicate blank signals and m is the slope of the linear section of calibration curve after preconcentration for a sample volume of 50 mL, was 0.05 µg·L −1 . In comparison with other reported Cd((II) IIPs for SPE extraction (Table 3), the proposed method shows comparable results in terms of analytical performance. The results support that the synthesized MIIP is a selective and reliable sorbent suitable for preconcentration and determination of Cd(II) ions at trace levels in real samples.