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Article

Core-shell Fe3O4@zeolite NaA as an Adsorbent for Cu2+

by
Jun Cao
1,
Peng Wang
2,
Jie Shen
1 and
Qi Sun
1,*
1
College of Materials and Metallurgy, Guizhou University, Guiyang 550025, China
2
Wuhan National Laboratory for Optoelectronics, School of Optical and Electronic Information, Huazhong University of Science and Technology 1037 Luoyu Road, Wuhan 430074, China
*
Author to whom correspondence should be addressed.
Materials 2020, 13(21), 5047; https://doi.org/10.3390/ma13215047
Submission received: 7 October 2020 / Revised: 30 October 2020 / Accepted: 3 November 2020 / Published: 10 November 2020
(This article belongs to the Section Advanced Composites)
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Versions Notes

Abstract

:
Here, using Fe3O4@SiO2 as a precursor, a novel core-shell structure magnetic Cu2+ adsorbent (Fe3O4@zeolite NaA) was successfully prepared. Several methods, namely X-ray diffraction (XRD), Fourier transform infrared spectrometer (FTIR), Transmission electron microscope (TEM), Brunauer Emmett Teller (BET) and vibrating sample magnetometry (VSM) were used to characterize the adsorbent. A batch experiment was conducted to study the Cu2+ adsorption capacity of Fe3O4@zeolite NaA at different pH values, contact time, initial Cu2+ concentration and adsorbent does. It is found that the saturated adsorption capacity of Fe3O4@zeolite NaA on Cu2+ is 86.54 mg/g. The adsorption isotherm analysis shows that the adsorption process of Fe3O4@zeolite NaA to Cu2+ is more consistent with the Langmuir model, suggesting that it is a monolayer adsorption. Adsorption kinetics study found that the adsorption process of Fe3O4@zeolite NaA to Cu2+ follows the pseudo-second kinetics model, which means that the combination of Fe3O4@zeolite NaA and Cu2+ is the chemical chelating reaction. Thermodynamic analysis shows that the adsorption process of Fe3O4@zeolite NaA to Cu2+ is endothermic, with increasing entropy and spontaneous in nature. The above results show that Fe3O4@zeolite NaA is a promising Cu2+ adsorbent.

Graphical Abstract

1. Introduction

Cu2+ is a bioaccumulative heavy metal pollutant resistant to degradation [1,2]. In recent years, due to the rapid development of industry, heavy metal ions represented by Cu2+ have been discharged into water bodies and can be biomagnified through the food chain, which poses a huge threat to human health and the ecological environment [3]. According to reports, when the Cu2+ concentration in the adult body exceeds 2 mg/L, it can cause various diseases, such as gastrointestinal discomfort, kidney, liver damage and even cancer [4,5]. Therefore, removing Cu2+ from sewage has great significance [6]. In the past years, a large number of methods have been used to remove Cu2+ from sewage, including extraction, chemical precipitation, and filtration [7,8,9]. Compared with these technologies, the adsorption method has obvious advantages of low cost, simple operation and high efficiency [10] and some adsorbents have been successfully developed for the adsorption of Cu2+ [11].
Zeolite NaA is a microporous crystalline aluminosilicate with a pore size of about 0.4 nm. Its frame structure consists of [SiO4]4− and [AlO4]5− tetrahedrons connected by a common oxygen atom. [12]. This special structure makes the zeolite NaA have large surface area and strong selective adsorption capacity [13]. At present, a large number of reports confirm the possibility of using zeolite NaA as an adsorbent [14,15,16]. However, the absorbed zeolite NaA is difficult to be separate from the liquid phase, which is due to its powder morphology. To solve this problem, one method is to synthesize magnetic zeolite NaA. Li et al. [17] successfully prepared a NaA magnetic zeolite in 2013. They found that under the action of an external magnetic field, the NaA magnetic zeolite can be easily separated from the liquid phase, showing excellent separation performance. However, most of the magnetic Fe3O4 nanoparticles in magnetic zeolite NaA are distributed on the surface of the zeolite NaA, which causes part of the zeolite NaA surface that can be used for adsorption being occupied by magnetic Fe3O4 nanoparticles, thus exerting an adverse effect on the adsorption performance of magnetic zeolite NaA [18]. Many new material properties will appear in materials with nanoscale dimensions, such as excellent optical, electrical, magnetic, thermal and mechanical properties. In recent years, the emergence of core-shell nanomaterials represented by Fe3O4@SiO2 has attracted widespread attention and has been applied to control oral insulin delivery, curcumin release, microwave absorption, photocatalytic activity and other fields [19,20,21,22,23]. It is well known that SiO2 in Fe3O4@SiO2 can be used as a silicon source to generate zeolite NaA. Moreover, when Fe3O4@SiO2 is used as a precursor for further reactions, the Fe3O4 contained in Fe3O4@SiO2 can provide products with excellent magnetic properties. The core-shell Fe3O4@zeolite NaA may be formed, which Fe3O4@SiO2 is used as the precursor and after adding the corresponding quality aluminum and alkali. Because the reaction to form zeolite NaA is carried out on the surface of Fe3O4@SiO2, the magnetic Fe3O4 nanoparticles in Fe3O4@zeolite NaA are encapsulated by zeolite NaA. In short, this novel structure retains the excellent magnetic separation performance of traditional magnetic zeolite NaA and avoids magnetic Fe3O4 nanoparticles attaching on the zeolite NaA surface, thereby solving the problem with traditional magnetic zeolite NaA as mentioned above.
In this work, a novel core-shell adsorbent Fe3O4@zeolite NaA was successfully prepared. The fabrication process of Fe3O4@zeolite NaA is shown in Scheme 1. XRD, FTIR, TEM, BET and VSM were used to characterize Fe3O4@zeolite NaA. In addition, the effect of various experimental parameters of Cu2+ adsorption from aqueous including pH of the solution, contact time, initial concentration and adsorbent mass, as well as adsorption kinetics, isotherm models and thermodynamics was discussed.

2. Experimental

2.1. Raw Materials

(NH3·H2O, 25%, AR), FeCl3·6H2O (AR), FeCl2·4H2O (AR), NaOH (AR), and TEOS (99.99%) were purchased from Sinopharm Chemical Reagent Co Ltd (Beijing, China). NaAlO2 (AR) was purchased from Shanghai Macklin Biochemical Co. Ltd (Shanghai, China). NaSiO3·9H2O (AR) was purchased from Aladdin Reagent (Shanghai, China) Co. Ltd. The deionized water was made by the laboratory.

2.2. Preparation of Samples

The magnetic Fe3O4 nanoparticles were prepared by a coprecipitation method. In brief, 27.03 g of FeCl3·6H2O and 9.94 g of FeCl2·4H2O (a molar ratio of 2:1) were dissolved into deionized water and mechanically stirred under a nitrogen atmosphere at 90 °C. After that, 5 mL of NH3·H2O was added dropwise into the mixture solution. The formed precipitates were collected, washed with deionized water and vacuum dried at 60 °C for 8 h.
The Fe3O4@SiO2 nanoparticles were synthesized by a modified method [24]. Magnetic Fe3O4 nanoparticles (20 mg) were uniformly dispersed into 20 mL ethanol under ultrasonication. Two mL of TEOS(Si(OC2H5)4) and 2 mL of NH3·H2O were then added under mechanical agitation to form a homogenous mixture. After that, 1:4 (V/V) deionized/ethanol solution was added dropwise under stirring within 4 h. The obtained particles were magnetically separated using a permanent magnet and washed by ethanol for several times. The samples were vacuum dried overnight at 60 °C.
The process of preparing Fe3O4@zeolite NaA is described below. The content of SiO2 in the prepared Fe3O4@SiO2 was determined by XRF analysis (Table S1). Fe3O4@SiO2 (20 mg) was uniformly dispersed into 2 mol/L sodium hydroxide solution under ultrasonication. 14.121 mg of NaAlO2 was added to the mixed solution (Si/Al ratio = 1). The reactant in the mixed solution to fully dispersed under ultrasonication. Transfer the mixed solution to the reactor and react at 110 °C for 10 h. The obtained sample was magnetically separated using a permanent magnet and washed by deionized water for several times. The sample was dried overnight at 80 °C.
The process of preparing magnetic zeolite NaA was as follows: 2 g of magnetic Fe3O4 nanoparticles, 14.21 g of NaSiO3·9H2O and 4.0985 g of NaAlO2 (1:1of Si/Al ratio) were mixed in 2 mol/L NaOH solution. The mixture was stirred vigorously for 2 h at 60 °C. The reactants were transferred to the reactor and crystallized for 9 h at 90 °C. The obtained sample was washed repeatedly with deionized water and dried under vacuum at 60 °C for 6 h.

2.3. Characterization

X-ray diffraction (XRDpatterns were recorded on a PRO XRD diffractometer (X’Pert, Holland) equipped with a Cu Kα radiation source operating at 40 kV and 100 mA. X Ray Fluorescence (XRF) were analysed on a Axios spectrometer (PANalytical, Holland). Vibrating sample magnetometry (VSM) tests were performed on a PPMS DynaCool magnetometer (Quantum Design, America). Fourier transform infrared spectra (FTIR) were obtained by the KBr wafer technique using a Ft-5dx infrared spectrometer (America) in the 4000–400 cm−1 region. The N2 adsorption isotherms of the samples were measured using N2 at 77 K using a 3H-2000PS4 analyzer (China). The samples were degassed at 300 °C for 5 h before the measurement (BET). The microstructure was analyzed by transmission electron microscope (TEM, Tecnai F30, Philips FEI, Holland). The structural feature and crystallinity of the samples were analyzed by an AXS D8-Focus system (Bruker Berlin, Germany). The degree of crystallinity was estimated by taking the ratio of summation of peak height of the peaks appearing at 2θ = 7.2°, 10.3°, 12.6°, 16.2°, 21.8°, 24.0°, 27.2°, 29.9° and 34.2° of the test sample to the summation of peak height of the same peaks in the commercial zeolite 4A, the crystallinity was calculated by Equation (1) [25]:
% Crystallinity = ( ∑   peak   height   of   sample ∑   peak   height   of   commerical   zeolite ) × 100 %

2.4. Preparation of Heavy Metal Solutions

Prepared a standard Cu2+ stock solution (500 mg/L) by dissolving Cu(SO4)2·5H2O in a beaker. The solution was then diluted to the desired concentration using deionized water (see the Supporting Information S1 for detailed operational steps).

2.5. Adsorption Experiments

In this paper, the adsorption capacities of Fe3O4@zeolite NaA and magnetic zeolite NaA for Cu2+ were studied. The influence of pH, contact time, adsorbent mass and Cu2+ initial concentration were optimized by varying one factor while keeping others constant. Equations (S1) and (S2) were used to calculate the adsorption content of Cu2+ and the removal rate of Cu2+ by adsorbent (see the details in Supporting Information S2). Adsorption kinetics, adsorption isotherm and thermodynamic have been studied (see the details in Supporting Information S2).

3. Results and Discussion

3.1. Characterization of Samples

The XRD patterns of magnetic Fe3O4 nanoparticle, Fe3O4@SiO2, Fe3O4@zeolite NaA and magnetic zeolite NaA are shown in Figure 1. The characteristic peaks are at 2θ = 18.3°, 30.1°, 35.5°, 43.1°, 53.5°, 57.1° and 62.6° (Figure 1a), which is characteristic of the (111), (220), (311), (400), (422), (511) and (440) crystal planes of Fe3O4 (JCPDS 88-0315), respectively, and it is in agreement with the previously reported article [26]. Compared with magnetic Fe3O4 nanoparticles, the XRD pattern of Fe3O4@SiO2 not only contains the characteristic magnetic Fe3O4 nanoparticle peaks, but also a slightly wider peak at 2θ = 20°–30° (Figure 1b), which corresponds to a coating of amorphous SiO2 [27]. In Figure 1c, the XRD pattern of Fe3O4@zeolite NaA has characteristic peaks of magnetic Fe3O4 nanoparticle and zeolite NaA. The characteristic peaks at 2θ = 35.5°, 43.1° and 62.6° are attributed to magnetic Fe3O4 nanoparticle, and at 2θ = 7.2°, 10.3°, 12.5°, 16.1°, 21.7°, 24.0°, 27.2°, 29.9° and 34.2° peaks, which are the main characteristic diffraction peaks of NaA zeolite (JCPDS 00-039-0222) and correspond to the (200), (220), (222), (420),(600), (622), (642), (644) and (664) crystal planes of NaA zeolite, respectively [28]. Except for the characteristic peaks of magnetic Fe3O4 nanoparticle and zeolite NaA, no other characteristic peaks are observed. This result indicates that no new substances are formed during the synthesis of Fe3O4@zeolite NaA. The XRD pattern of magnetic zeolite NaA (Figure 1d) shows similar characteristic peaks to Fe3O4@zeolite NaA.
By XRD analysis, no difference between magnetic zeolite NaA and Fe3O4@zeolite NaA can be found, so more work must be done to confirm the superiority of Fe3O4@zeolite NaA. Figure 2 shows the crystallinity of magnetic zeolite NaA and Fe3O4@zeolite NaA. It can be seen that the crystallinity of Fe3O4@zeolite NaA (92.7%) is higher than that of magnetic zeolite NaA, which means that the presence of magnetic Fe3O4 nanoparticle in Fe3O4@zeolite NaA has a smaller effect on the formation of zeolite NaA.
Figure 3 shows the FTIR spectra of magnetic Fe3O4 nanoparticle, Fe3O4@SiO2, Fe3O4@zeolite NaA and magnetic zeolite NaA. In the spectra of magnetic Fe3O4 nanoparticle and Fe3O4@SiO2 (Figure 3a,b), the peaks at approximately 620 cm−1, 1680 cm−1 and 3440 cm−1 correspond to Fe–O stretching vibrations [29], H–O–H bending vibrations [30] and O–H stretching vibrations [31]. In addition, in the FTIR spectrum of Fe3O4@SiO2, the peak at about 1100 cm−1 corresponds to the stretching vibration of the Si–O bond [32], proves that the sample contains SiO2. The FTIR spectra of Fe3O4@zeolite NaA and magnetic zeolite NaA are shown in Figure 3c,d.
It can be clearly seen that both Fe3O4@zeolite NaA and magnetic zeolite NaA have characteristic bands at 470 cm−1, 563 cm−1, 1005 cm−1, 1680 cm−1 and 3440 cm−1, respectively. Except for these peaks, no other peaks appear in the FTIR spectrum of Fe3O4@zeolite NaA and magnetic zeolite NaA. The peak at 470 cm−1 [33] is related to the internal bond vibration of the TO4 (T = Si or Al) tetrahedron in the zeolite structure. Compared with Fe3O4@SiO2, the peaks corresponding to Fe–O stretching vibrations and stretching vibration of the Si–O bond are shifted to 563 cm−1 and 1005 cm−1, respectively. The characteristic bands at 1680 cm−1 and 3440 cm−1 correspond to the H–O–H bending vibrations and O–H stretching vibrations, respectively. The FTIR spectrum can show that Fe3O4@zeolite NaA and magnetic zeolite NaA contain similar functional groups.
In order to determine the microstructure and morphology of the sample, transmission electron microscopy (TEM) is effectively used for microscopic inspection. Figure 4a shows that the well-dispersed Fe3O4@SiO2 nanoparticles are spherical and the surface is relatively smooth. Among them, the black center part is a magnetic core composed of multiple magnetic Fe3O4 nanoparticles. The diameter of a single magnetic Fe3O4 nanoparticle is about 15 nm, and the thickness of the SiO2 coating layer is about 13 nm. This information can be obtained from Figure 4b. In addition, the lattice fringes of the sample can be easily seen from Figure 4c. The measured lattice spacing of 0.253 nm and 0.297 nm correspond to the (311) and (220) crystal planes of Fe3O4, respectively. The different color areas shown in Figure 4d represent the distribution of Fe, O and Si in the real structure of Fe3O4@SiO2, respectively. The Fe3O4 core and the SiO2 shell can be clearly distinguished, which directly proves the successful preparation of the core-shell morphology Fe3O4@SiO2. In Figure 4e, we can clearly see that Fe3O4@zeolite NaA presents a cubic morphology, and the shell formed by zeolite NaA wraps the core formed by Fe3O4. Compared with magnetic zeolite NaA (Figure S1), due to there is no magnetic Fe3O4 nanoparticle attached to the surface, it can be seen that the surface of Fe3O4@zeolite NaA is smoother. The high-resolution TEM image of Fe3O4@zeolite NaA in Figure 4f shows clear lattice spacing of 0.870 nm, 1.231 nm and 0.253 nm, corresponding to the (220) and (200) crystal planes of zeolite NaA and (311) crystal plane of Fe3O4, respectively. The TEM results further proved that Fe3O4@zeolite NaA with core-shell structure was successfully prepared.
The specific surface area and pore structure are two important characteristics of adsorbent. The specific surface area and pore structure of magnetic zeolite NaA and Fe3O4@zeolite NaA were studied by measuring nitrogen adsorption-desorption isotherms. The results are shown in Figure 5.
The nitrogen adsorption-desorption isotherms of both magnetic zeolite NaA and Fe3O4@zeolite NaA belong to the typical type IV isotherm [34]. Among them, the nitrogen adsorption-desorption isotherm of Fe3O4@zeolite NaA has an evident H3 hysteresis loop [35] at a relative pressure ranging from 0.5–0.9, indicating that Fe3O4@zeolite NaA contains a certain number of mesopores [36], and magnetic zeolite NaA has almost no hysteresis loop in the nitrogen adsorption-desorption isotherm. The specific surface area, average pore diameter and pore volume of the samples are shown in Table 1. The specific surface areas of magnetic zeolite NaA and Fe3O4@zeolite NaA are calculated using BET technique, which are 2.7310 m2/g and 26.8461 m2/g, respectively. It is obvious that the specific surface area of Fe3O4@zeolite NaA is much higher than that of magnetic zeolite NaA. In this study, the smaller specific surface area of magnetic zeolite NaA may be attributed to its surface being occupied by magnetic Fe3O4 nanoparticles [37], which reduces the exposed area for adsorption. Correspondingly, a large specific surface area will contain a larger number of adsorption sites [38], which will increase the possibility of adsorbed substances being removed. Figure 5b,c clearly show that magnetic zeolite NaA and Fe3O4@zeolite NaA have a wide pore size distribution. The pore volumes of magnetic zeolite NaA and Fe3O4@zeolite NaA are calculated using the BJH method, which are 0.017872 cm3/g and 0.136697 cm3/g, respectively. Obviously, the pore volume of Fe3O4@zeolite NaA is much higher than that of magnetic zeolite NaA, which means that Fe3O4@zeolite NaA has better adsorption performance [39]. The average pore diameter of Fe3O4@zeolite NaA is smaller than magnetic zeolite NaA, it may be related to the increase in the number of micropores in Fe3O4@zeolite NaA [40]. The results of nitrogen adsorption-desorption isotherms show that the specific surface area and pore volume of Fe3O4@zeolite NaA are much higher than that of magnetic zeolite NaA.
Figure 6 shows magnetization curves of magnetic Fe3O4 nanoparticle, Fe3O4@SiO2 and Fe3O4@zeolite NaA. No hysteresis effect was observed on the three samples, indicating that the prepared samples are all superparamagnetic [41]. Once the external magnetic field is withdrawn, there is no residual magnetism on the samples. It is found that the saturation magnetization value of the magnetic Fe3O4 nanoparticle is 54.79 emu/g. After being coated with SiO2, the saturation magnetization value of Fe3O4@SiO2 decreases to 19.95 emu/g, indicating that SiO2 has been successfully coated on the surface of the magnetic Fe3O4 nanoparticle. The saturation magnetization of Fe3O4@zeolite NaA is 5.38 emu/g, which is sufficient to ensure that Fe3O4@zeolite NaA can be separated quickly under an external magnetic field, as shown in Figure S2. Based on these results, it is proved that the Fe3O4@zeolite NaA prepared in this study has superparamagnetism and can be quickly separated from the liquid under the action of an external magnetic field.

3.2. Optimization of Adsorption Parameters

3.2.1. Effect of pH

The influence of various pH values (1–5) on the adsorption of Cu2+ by the adsorbents (2 g/L) is shown in Figure 7. We can clearly see that the adsorption capacity of Fe3O4@zeolite NaA on Cu2+ was enhanced when the pH increased from 1 to 4, and reaches the maximum adsorption capacity of 86.54 mg/g at pH = 4. As the pH ranged from 4.0 to 5.0, the adsorption capacity of Fe3O4@zeolite NaA on Cu2+ decreased significantly. When pH = 1, the low pH environment could lead to more H3O+ in the Cu2+ solution. These H3O+ ions compete with Cu2+ for active sites on the Fe3O4@zeolite NaA surface, which affects adsorption capacity of Cu2+ by Fe3O4@zeolite NaA. As the pH continues to increase, the amount of H3O+ continues to decrease. When pH = 2, Cu2+ began to become the main ion in the solution. Therefore, the adsorption capacity of Fe3O4@zeolite NaA on Cu2+ has experienced a substantial increase in the range of pH value is 2–4. With the increase in value of pH, the OH- concentration of the solution has gradually increased and after combining with Cu2+, Cu(OH)2 begins to precipitate [42,43]. Therefore, excessive pH is not conducive to the adsorption of Cu2+ by Fe3O4@zeolite NaA. Under the influence of different pH values, the adsorption trend of magnetic zeolite NaA on Cu2+ is similar to that of Fe3O4@zeolite NaA, and reaches the maximum adsorption capacity of 32.12 mg/g at pH = 4. The result shows that at different pH, Fe3O4@zeolite NaA has a higher adsorption capacity for Cu2+ than magnetic zeolite NaA. Subsequent batch adsorption experiments are carried out under the condition of pH = 4. (Adsorption condition: Adsorbent dose is 0.1 g; Cu2+ solution volume is 50 mL; Initial Cu2+ concentration is 200 mg/L; Temperature is 298.15 K; Contact time is 24 min).

3.2.2. Effect of Adsorbent Does on Cu2+ Adsorption

As shown in Figure 8, regardless of the adsorbent used in this study (magnetic zeolite NaA or Fe3O4@zeolite NaA), the adsorption capacity of Cu2+ increased as the adsorbent mass increases from 0.06 g to 0.1 g, and then remained almost unchanged from 0.1 g to 0.14 g. It can be found that the maximum adsorption capacity of Cu2+ was found to be 86.54 mg/g for Fe3O4@zeolite NaA and 32.12 mg/g for magnetic zeolite NaA, indicating that the adsorption capacity of Fe3O4@zeolite NaA is 2.7 times that of magnetic zeolite NaA. In the subsequent adsorption experiment, the does of the adsorbent is set to 0.1 g. (adsorption condition: pH = 4; Cu2+ solution volume is 50 mL; Initial Cu2+ concentration is 200 mg/L−1; Temperature is 298.15 K; Contact time is 24 min)

3.2.3. Effect of Contact Time on Cu2+ Adsorption

At different concentrations of Cu2+, the effect of contact time on the removal of Cu2+ by magnetic zeolite NaA and Fe3O4@zeolite NaA can be seen from Figure 9a,b, respectively.
It can be seen from the figure that when the contact time is from 1 min to 10 min, the adsorption amount of Cu2+ by magnetic zeolite NaA and Fe3O4@zeolite NaA increases greatly with the increase of contact time. When the contact time is from 10 min to 24 min, the adsorption amount of Cu2+ by magnetic zeolite NaA and Fe3O4@zeolite NaA still keeps increasing which the adsorption amount of Cu2+ by Fe3O4@zeolite NaA still keeps increasing greatly. When the contact time is more than the 24 min, which the adsorption capacity of magnetic zeolite NaA and Fe3O4@zeolite NaA on Cu2+ remained basically unchanged. It shows that the adsorption of Cu2+ by the adsorbent (magnetic zeolite NaA or Fe3O4@zeolite NaA) reaches the adsorption equilibrium at 24 min. The prepared Fe3O4@zeolite NaA is also compared with other adsorbents of Cu2+ reported in literature [44,45]. It is found that the equilibrium adsorption time of Fe3O4@zeolite NaA in this study is shorter and more suitable for practical applications. Similarly, as the concentration of Cu2+ increases, the amount of Cu2+ adsorbed by the adsorbent will also increase. The adsorption equilibrium is reached which the Cu2+ concentration reaches 200 mg/L. When Cu2+ concentration is 25 mg/L to 200 mg/L, the saturated adsorption capacity of Fe3O4@zeolite NaA on Cu2+ is 12.42, 23.66, 37.28, 49.36, 62.12, 67.36 and 86.54 mg/g, respectively. The saturated adsorption capacity of magnetic zeolite NaA for Cu2+ is 11.16, 18.66, 24.12, 27.02, 29.72, 31.16 and 32.12 mg/g, respectively. It can be seen that Fe3O4@zeolite NaA has higher adsorption capacity for Cu2+. In the subsequent adsorption experiment, the contact time of the adsorbent is set to 24 min. (Adsorption condition: Adsorbent dose is 0.1 g; Cu2+ solution volume is 50 mL; pH = 4; Temperature is 298.15 K)

3.2.4. Effect of Initial Concentration

Figure 10 shows the effect of different initial concentrations on the adsorption performance of the adsorbents (2 g·L−1) for Cu2+. Figure 10a shows that with increase of the initial concentration, the adsorption of Cu2+ on magnetic zeolite NaA gradually increases. When the initial concentration reaches a certain value (200 mg/L−1), the adsorption capacity of magnetic zeolite NaA on Cu2+ reaches saturation (32.12 mg/g). It can be seen from the change curve of Remove% that when the initial concentration over 100 mg/L−1, the Remove% value of Cu2+ by magnetic zeolite NaA starts to be lower than 55%. When the initial concentration reaches 200 mg/L, the magnetic zeolite NaA Remove% value of Cu2+ is only 32.12%. The above results indicate that magnetic zeolite NaA cannot be used as a Cu2+ adsorbent in practical applications. Figure 10b shows that the adsorption capacity of Fe3O4@zeolite NaA on Cu2+ increases with the increase of the initial concentration, and reaches the Cu2+ adsorption equilibrium when the initial concentration is 200 mg/L (the adsorption capacity is 86.54 mg/g), indicating that all adsorption sites of Fe3O4@zeolite NaA have been occupied by Cu2+ [46]. The change curve of Remove% of Fe3O4@zeolite NaA vs.(versus) Cu2+ shows that as the initial concentration continues to increase, the overall trend of Remove% value is downward, but the decline is small. When the initial concentration is 200 mg/L, it can still maintain 86.54%. The Remove% of Cu2+ shows that Fe3O4@zeolite NaA can be used as an effective adsorbent to remove Cu2+ in sewage. The initial concentration value of the subsequent adsorption experiments are all select as 200 mg/L. (Adsorption condition: Adsorbent dose is 0.1 g; Cu2+ solution volume is 50 mL; pH = 4; temperature is 298.15 K; contact time is 24 min).

3.3. Adsorption Isotherm

The adsorption isotherm can be used to study the binding mechanism of the adsorbents and Cu2+ which through the equilibrium adsorption capacity of the adsorbents to Cu2+ for different initial concentrations. The experimental data of adsorbent adsorption of Cu2+ at different initial concentrations were linearly fitted to Freundlich, Tempkin and Langmuir models, the conditions under which the pH value of 4, the adsorbent dose of 0.1 g, the Cu2+ solution volume of 50 mL, the contact time of 24 min and the temperature of 298.15 K. The fitting parameters of Freundlich, Tempkin and Langmuir adsorption isotherms are shown in Table 2. In Figure 11, we can clearly see that Langmuir model provides a better description of the adsorption process of magnetic zeolite NaA than Freundlich and Tempkin model. Table 2. shows that the Langmuir model of magnetic zeolite NaA has a higher R2 (0.99890) than the Freundlich model (0.93447) and Tempkin model (0.96782), which directly proves the above point. Combining the analysis in Figure 11 and Table 2, we found that the R2 value of the Freundlich model (0.61082) and Tempkin model(0.73113) of Fe3O4@zeolite NaA is smaller than Langmuir model (0.99734), which means that the Langmuir model can better describe the effect of Fe3O4 @zeolite NaA on Cu2+ adsorption behavior under different initial concentrations. It shows that the process of Fe3O4@zeolite NaA adsorption of Cu2+ is monolayer adsorption [47], the adsorption sites are uniformly distributed on the surface of Fe3O4@zeolite NaA [48]. The maximum adsorption capacity (Qmax) of Fe3O4@zeolite NaA for Cu2+ calculated by the Langmuir model is 86.58 mg/g, which is very similar to the actual amount of Qmax (86.54 mg/g). The maximum adsorption capacity (Qmax) of Fe3O4@zeolite NaA on Cu2+ is compared with other adsorbents (including magnetic zeolite NaA). The relevant results are summarized in Table 3, which proves the Fe3O4@zeolite NaA has excellent adsorption performance for Cu2+. As the RL value lies between 0 and 1, it shows that the adsorption of Fe3O4@zeolite NaA to Cu2+ is spontaneous [49].

3.4. Adsorption Kinetics

In order to further study the adsorption mechanism of magnetic zeolite NaA and Fe3O4@zeolite NaA for Cu2+. The adsorption kinetics of Cu2+ adsorption on magnetic zeolite NaA and Fe3O4@zeolite NaA were used for this research, which by the conditions of pH = 4, room temperature(298.15 K), initial concentration of 200 mg/L, adsorbent dose of 0.1 g, Cu2+ solution volume of 50 mL and different contact time. Two types of kinetics models are generally used and compared, namely the pseudo-first order and pseudo-second. The results and related parameters are shown in Figure 12 and Table 4, respectively. The results in Figure 12 and Table 4 show that the adsorption of Cu2+ on magnetic zeolite NaA and Fe3O4@zeolite NaA more followed the pseudo-second-order kinetic model (R2 = 0.99702, 0.99305), compared to the pseudo-first-order kinetic model (R2 = 0.89008, 0.84336), which implies that the adsorption process of Cu2+ by magnetic zeolite NaA and Fe3O4@zeolite NaA is of chemisorption mechanism [54].
In addition, the equilibrium adsorption capacity (Qe = 34.282, 95.147) of magnetic zeolite NaA and Fe3O4@zeolite NaA calculated by using the pseudo-second-order kinetic model is closer to the experimental data (Qe = 32.12, 86.54). The pseudo-second order rate parameters (K2) were higher for the magnetic zeolite NaA compared to those of the Fe3O4@zeolite NaA, which means magnetic zeolite NaA has a faster adsorption rate.

3.5. Adsorption Thermodynamics

The adsorption capacity of Cu2+ by magnetic zeolite NaA and Fe3O4@zeolite NaA at different temperatures was studied (Figure 13a). Adsorption thermodynamics of Cu2+ onto magnetic zeolite NaA and Fe3O4@zeolite NaA are studied, which under the conditions of initial concentration value of 200 mg/L, pH of 4, contact time of 24 min, adsorbent dose of 0.1 g, Cu2+ solution volume of 50 mL and temperature of 288.15 K, 298.15 K, 308.15 K and 318.15 K, respectively (Figure 13b).The relevant adsorption thermodynamic parameters are shown in Table 5. We found that the adsorption capcity of Cu2+ by magnetic zeolite NaA and Fe3O4@zeolite NaA increased with the increase of temperature (Figure 13a), which means that high temperature caused the increase of Cu2+ mobility [55]. However, the improvement of adsorption capacity is very small, which shows that different temperatures have little effect on the capacity of magnetic zeolite NaA and Fe3O4@zeolite NaA to adsorb Cu2+. The above results indicate that the magnetic zeolite NaA and Fe3O4@zeolite NaA at room temperature basically have the saturated adsorption capacity for Cu2+. It can be seen from Table 5 that the ΔGo values of magnetic zeolite NaA and Fe3O4@zeolite NaA are both negative, and decrease with the increase of temperature, indicating that the adsorption process of magnetic zeolite NaA and Fe3O4@zeolite NaA to Cu2+ is spontaneous [56]. The values of ΔHo are 8.05 and 9.64 KJ·mol−1, respectively, and both are between 20.9–418.4 KJ·mol−1, which proves once again that the adsorption of Cu2+ by magnetic zeolite NaA and Fe3O4@zeolite NaA is chemical adsorption and the adsorption is an endothermic process. [57]. The positive values of ΔS0 indicate that the adsorption of Cu2+ by magnetic zeolite NaA and Fe3O4@zeolite NaA is moving in the direction of increasing the chaos of the system [58,59,60].

4. Conclusions

A novel magnetic Cu2+ adsorbent Fe3O4@zeolite NaA was successfully prepared. XRD, FTIR, and TEM analyses showed that Fe3O4@zeolite NaA has good crystallinity and presents a typical core-shell structure. BET technical analysis showed that the specific surface area of Fe3O4@zeolite NaA reached 26.846 m2·g−1. VSM analysis shows that the saturation magnetization of Fe3O4@zeolite NaA is 5.38 emu/g, which means that it has the ability to quickly separate from the liquid phase under the action of an external magnetic field. The ability of Fe3O4@zeolite NaA to adsorb Cu2+ was tested, and it was found that the time to reach adsorption equilibrium was only 24 min. Under certain conditions (Adsorbent dose is 0.1 g; Cu2+ solution volume is 50 mL; Initial Cu2+ concentration is 200 mg/L−1; Temperature is 298.15 K; contact time is 24 min; pH = 4), Fe3O4@zeolite NaA has an adsorption capacity of 86.54 mg/g for Cu2+, and the Remove% value has reached 86.54%. The process of Fe3O4@zeolite NaA adsorption to Cu2+ has been studied by isotherm, kinetics and thermodyna. Adsorption data fit better with the Langmuir isotherm, suggesting that the adsorption is a monolayer adsorption. Kinetics study indicates that the adsorption follows the pseudo-second-order model, suggesting that is the chemical interaction between Cu2+ and adsorbent. The values of separation constant (0 < RL <1) indicate that the adsorption for Cu2+ is a favorable process. Thermodynamic studies have shown that the adsorption of Fe3O4@zeolite NaA on Cu2+ is a spontaneous process with endothermic and entropy increase. In a word, Fe3O4@zeolite NaA is suitable as a Cu2+ adsorbent.

Supplementary Materials

The following are available online at https://www.mdpi.com/1996-1944/13/21/5047/s1, Figure S1: TEM image of magnetic zeolite NaA, Figure S2: Separation ability test of Fe3O4@zeolite NaA, Table S1: XRF analyze of Fe3O4@SiO2 (w %).

Author Contributions

Conceptualization, P.W.; methodology, J.S.; writing—original draft preparation, J.C.; writing—review and editing, Q.S.; funding acquisition, Q.S. All authors have read and agreed to the published version of the manuscript.

Funding

This research was funded by the Guizhou Science and Technology Plan Project [(2017) No. 7247].

Conflicts of Interest

The authors declare no conflict of interest.

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Materials 13 05047 sch001 550
Scheme 1. Fabrication process of Fe3O4@zeolite NaA.
Scheme 1. Fabrication process of Fe3O4@zeolite NaA.
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Materials 13 05047 g001 550
Figure 1. XRD patterns of (a) Fe3O4, (b) Fe3O4@SiO2, (c) Fe3O4@zeolite NaA and (d) Magnetic zeolite NaA.
Figure 1. XRD patterns of (a) Fe3O4, (b) Fe3O4@SiO2, (c) Fe3O4@zeolite NaA and (d) Magnetic zeolite NaA.
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Materials 13 05047 g002 550
Figure 2. The crystallinity degree of Fe3O4@zeolite NaA and magnetic zeolite NaA.
Figure 2. The crystallinity degree of Fe3O4@zeolite NaA and magnetic zeolite NaA.
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Materials 13 05047 g003 550
Figure 3. FTIR patterns of (a) Fe3O4, (b) Fe3O4@SiO2, (c) Fe3O4@zeolite NaA and (d) Magnetic zeolite NaA.
Figure 3. FTIR patterns of (a) Fe3O4, (b) Fe3O4@SiO2, (c) Fe3O4@zeolite NaA and (d) Magnetic zeolite NaA.
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Materials 13 05047 g004 550
Figure 4. (a) and (b) TEM images of the Fe3O4@SiO2 (c) HRTEM images of Fe3O4@SiO2 (d) Element mapping of the Fe3O4@SiO2 based on Fe, O and Si (e) TEM image of the Fe3O4@zeolite NaA (f) HRTEM image of Fe3O4@zeolite NaA.
Figure 4. (a) and (b) TEM images of the Fe3O4@SiO2 (c) HRTEM images of Fe3O4@SiO2 (d) Element mapping of the Fe3O4@SiO2 based on Fe, O and Si (e) TEM image of the Fe3O4@zeolite NaA (f) HRTEM image of Fe3O4@zeolite NaA.
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Materials 13 05047 g005 550
Figure 5. (a) N2 adsorption-desorption isotherms of Fe3O4@zeolite NaA and magnetic zeolite NaA (b,c) Pore size distributions of magnetic zeolite NaA and Fe3O4@zeolite NaA.
Figure 5. (a) N2 adsorption-desorption isotherms of Fe3O4@zeolite NaA and magnetic zeolite NaA (b,c) Pore size distributions of magnetic zeolite NaA and Fe3O4@zeolite NaA.
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Figure 6. Magnetic hysteresis curves of (a) Fe3O4, (b) Fe3O4@SiO2 and (c) Fe3O4@zeolite NaA.
Figure 6. Magnetic hysteresis curves of (a) Fe3O4, (b) Fe3O4@SiO2 and (c) Fe3O4@zeolite NaA.
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Figure 7. Effect of pH on the adsorption of Cu2+ onto magnetic zeolite NaA and Fe3O4@zeolite NaA.
Figure 7. Effect of pH on the adsorption of Cu2+ onto magnetic zeolite NaA and Fe3O4@zeolite NaA.
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Figure 8. Effect of adsorbent mass on the adsorption of Cu2+ by magnetic zeolite NaA and Fe3O4@zeolite NaA.
Figure 8. Effect of adsorbent mass on the adsorption of Cu2+ by magnetic zeolite NaA and Fe3O4@zeolite NaA.
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Figure 9. Effect of contact time on the uptake of Cu2+ by magnetic zeolite NaA (a) and Fe3O4@zeolite NaA (b).
Figure 9. Effect of contact time on the uptake of Cu2+ by magnetic zeolite NaA (a) and Fe3O4@zeolite NaA (b).
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Figure 10. Effect of initial concentration on the adsorption of Cu2+ by magnetic zeolite NaA (a) and Fe3O4@zeolite NaA (b).
Figure 10. Effect of initial concentration on the adsorption of Cu2+ by magnetic zeolite NaA (a) and Fe3O4@zeolite NaA (b).
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Figure 11. Freundlich model (a), Langmuir model (b) and Tempkin model (c) fittings for Cu2+ adsorption onto magnetic zeolite NaA and Fe3O4@zeolite NaA.
Figure 11. Freundlich model (a), Langmuir model (b) and Tempkin model (c) fittings for Cu2+ adsorption onto magnetic zeolite NaA and Fe3O4@zeolite NaA.
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Figure 12. Pseudo-first order model (a) and pseudo-second order model (b) fittings for Cu2+ adsorption onto magnetic zeolite NaA and Fe3O4@zeolite NaA.
Figure 12. Pseudo-first order model (a) and pseudo-second order model (b) fittings for Cu2+ adsorption onto magnetic zeolite NaA and Fe3O4@zeolite NaA.
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Figure 13. (a) Effect of temperature on adsorption of Cu2+ by magnetic zeolite NaA and Fe3O4@zeolite NaA (b).
Figure 13. (a) Effect of temperature on adsorption of Cu2+ by magnetic zeolite NaA and Fe3O4@zeolite NaA (b).
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Table
Table 1. Textual properties of magnetic zeolite NaA and Fe3O4@zeolite NaA.
Table 1. Textual properties of magnetic zeolite NaA and Fe3O4@zeolite NaA.
SampleBET Surfac Area
(m2·g−1)		Pore Volume
(cm3·g−1)		Average Pore Size
(nm)
Magnetic zeolite NaA2.7310.01787231.7899
Fe3O4@zeolite NaA26.8460.13669720.5846
Table
Table 2. Isotherm constants for adsorption by magnetic zeolite NaA and Fe3O4@zeolite NaA.
Table 2. Isotherm constants for adsorption by magnetic zeolite NaA and Fe3O4@zeolite NaA.
ModelsParameterMagnetic zeolite NaAFe3O4@zeolite NaA
R20.934470.61082
Freundichn4.14064.5773
KF (mg/g)9.909434.6927
R20.998900.99734
LangmuirQmax (mg/g)33.8986.58
KL (L/mg)0.108350.53177
R20.967820.73113
TempkinB15.072169.8778
Kt (L/mg)3.8574367.35653
Table
Table 3. Comparison of different adsorbents for Cu2+ adsorption.
Table 3. Comparison of different adsorbents for Cu2+ adsorption.
AdsorbentQm (mg/g)Ref.
Sewage sludge AC7.73[47]
Wheat shell10.84[50]
Lignocellulosic waste N-CDs26.95[51]
Mg2Al-LS-LD71.4[52]
Sulfonated MWCNT36.8[53]
Magnetic zeolite NaA32.12This study
Fe3O4@zeolite NaA86.54This study
Table
Table 4. Kinetics constants for adsorption by magnetic zeolite NaA and Fe3O4@zeolite NaA.
Table 4. Kinetics constants for adsorption by magnetic zeolite NaA and Fe3O4@zeolite NaA.
ModelsParameterMagnetic Zeolite NaAFe3O4@zeolite NaA
K1 (min−1)0.0990.07775
Pseudo-first-orderQe (mg/g)13.89841.698
R20.890080.84336
K2 (min−1)0.009690.00224
Pseudo-second-orderQe (mg/g)34.28295.147
R20.997020.99305
Table
Table 5. Thermodynamic parameters for Cu2+ adsorption on magnetic zeolite NaA and Fe3O4@zeolite NaA.
Table 5. Thermodynamic parameters for Cu2+ adsorption on magnetic zeolite NaA and Fe3O4@zeolite NaA.
SampleΔHoΔSoΔGo(KJ·mol−1)
(KJ·mol−1)[J·(K·mol)−1]288.15 K298.15 K308.15 K318.15 K
Magnetic zeolite NaA8.0514.86−4.27−4.42−4.57−4.72
Fe3O4@zeolite NaA9.6442.38−12.19−12.63−13.05−13.47
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Cao, J.; Wang, P.; Shen, J.; Sun, Q. Core-shell Fe3O4@zeolite NaA as an Adsorbent for Cu2+. Materials 2020, 13, 5047. https://doi.org/10.3390/ma13215047

AMA Style

Cao J, Wang P, Shen J, Sun Q. Core-shell Fe3O4@zeolite NaA as an Adsorbent for Cu2+. Materials. 2020; 13(21):5047. https://doi.org/10.3390/ma13215047

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Cao, Jun, Peng Wang, Jie Shen, and Qi Sun. 2020. "Core-shell Fe3O4@zeolite NaA as an Adsorbent for Cu2+" Materials 13, no. 21: 5047. https://doi.org/10.3390/ma13215047

APA Style

Cao, J., Wang, P., Shen, J., & Sun, Q. (2020). Core-shell Fe3O4@zeolite NaA as an Adsorbent for Cu2+. Materials, 13(21), 5047. https://doi.org/10.3390/ma13215047

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