# Well-Dispersed Nanoscale Zero-Valent Iron Supported in Macroporous Silica Foams: Synthesis, Characterization, and Performance in Cr(VI) Removal

Authors: Chaoxia Zhao; Jie Yang; Yihan Wang; Bo Jiang
Journal: Journal of Materials
 (2017)

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## Abstract

Well-dispersed nanoscale zero-valent iron (NZVI) supported inside the pores of macroporous silica foams (MOSF) composites (Mx-NZVI) has been prepared as the Cr(VI) adsorbent by simply impregnating the MOSF matrix with ferric chloride, followed by the chemical reduction with NaHB4 in aqueous solution at ambient atmosphere. Through the support of MOSF, the reactivity and stability of NZVI are greatly improved. Transmission electron microscopy (TEM) results show that NZVI particles are spatially well-dispersed with a typical core-shell structure and supported inside MOSF matrix. The N2 adsorption-desorption isotherms demonstrate that the Mx-NZVI composites can maintain the macroporous structure of MOSF and exhibit a considerable high surface area (503 m2·g−1). X-ray photoelectron spectroscopy (XPS) and powder X-ray diffraction (XRD) measurements confirm the core-shell structure of iron nanoparticles composed of a metallic Fe0 core and an Fe(II)/Fe(III) species shell. Batch experiments reveal that the removal efficiency of Cr(VI) can reach 100% when the solution contains 15.0 mg·L−1 of Cr(VI) at room temperature. In addition, the solution pH and the composites dosage can affect the removal efficiency of Cr(VI). The Langmuir isotherm is applicable to describe the removal process. The kinetic studies demonstrate that the removal of Cr(VI) is consistent with pseudo-second-order kinetic model.


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## Body

## 1. Introduction

Water pollution caused by heavy metal ions, such as Ni(II), Cr(VI), Mo(VI), and Pb(II) in groundwater, is one of the most serious environmental problems. Among the toxic metal oxyanions, chromium is widely distributed and exists in the waste coming from paint industry, metal finishing, textile dyeing, electroplating, and leather tanning [1]. Chromium mainly exists as trivalent [Cr(III)] and hexavalent [Cr(VI)] form in the natural environment. Because of the low solubility, mobility, and the weak ability to oxidize other species, the toxicity of Cr(III) is much lower than Cr(VI) [2]. In contrast, Cr(VI) demonstrates the higher toxicity, which can produce mutagenic, teratogenic, and carcinogenic effects in biological systems by reacting with nucleic acids and other cellular components [3]. Due to high toxicity of Cr(VI), applying efficient methods to remove Cr(VI) from waste water is of great importance.So far, various kinds of methods have been developed to reduce the harmful effects of Cr(VI), such as chemical extraction [4], reduction-precipitation [5], ion exchange [6], bioleaching process [7, 8], and biosorption [9, 10]. Among these methods, adsorption holds the significant position due to its high removal efficiency, low energy demand, and less chemical investment [11–13]. In the past years, researchers have applied various adsorbents to remove Cr(VI) from waste water, such as activated carbons [14], zeolites [15, 16], clays [17], and nanomagnetic particles [18]. However, these adsorbents have many defects including low porosity, low surface area, and lack of functional groups [19], which is of great importance for an efficient adsorbent. Hence adsorbents with high porosity, large surface area, and high functionality need to be developed for efficient removal of Cr(VI).Nanoscale zero-valent iron (NZVI) has been extensively applied to treat various contaminants in aqueous solution because of its low cost and strong reducing activity [20–24]. Also, NZVI has demonstrated the excellent ability to remove Cr(VI) from waste water through the mechanism of reduction, adsorption, or coprecipitation. However, some serious drawbacks associated with the practical application of NZVI need considering. The severe aggregation of iron nanoparticles during preparation and storage as well as the agglomeration into micrometer particles after the reaction with Cr(VI) may cause the dramatic deterioration in the reactivity [20, 25]. To conquer these issues, dispersing NZVI in supporting materials, such as activated carbon, polymers, clay minerals, and molecular sieves based on silica, is a promise solution. Because silica-based molecular sieves have a porous structure giving a large surface area and uniform pore sizes, which are of great importance for a good adsorbent, it has been greatly used as the potential support for the fabrication of efficient adsorbent. To date, for the fabrication of NZVI based adsorbents for Cr(VI) removal, porous silica such as SBA-15 [26–29] and MCM-41 [30–32] and silica fumes [33, 34] has been used as the matrix to support NZVI particles in order to minimize the aggregation and increase the reactivity of NZVI. However, this porous silica has relative small pores below 10 nm. Whether larger pore size can promote the reactivity of NZVI is still unknown. What is more, NZVI in these composites is supported on the external surfaces of the supports rather than going into pores [26, 27, 30, 33], which causes the underutilization of pores of the porous materials. Zero-valent iron nanoparticles inside the pores of ordered mesoporous silica have been successfully reported by other researchers [28, 29, 31, 34, 35], but a hydrogen reduction process under a harsh and dangerous condition including explosive hydrogen and higher temperatures or a complicated “two solvents” reduction technique using toxic cyclohexane as solvent is in demand. Therefore, it is necessary to develop a facile method to disperse nanoscale zero-valent iron nanoparticles homogeneously inside the pores of the porous matrix under mild, safe, and green condition.In this work, macroporous siliceous foams (MOSF) [36] with large pores of around 100 nm and high pore volumes were chosen as the support material to load ZVI nanoparticles for the preparation of efficient adsorbent for Cr(VI) removal. Nonionic block copolymers are used as the supramolecular template to synthesize MOSF materials via a facile supra-assembly approach. Appropriately modified MOSF can be applied in bioapplications, phosphate and arsenic adsorption [37–40]. In this paper, we have synthesized MOSF-supported nanoscale zero-valent iron composites (Mx-NZVI) simply by the direct reduction of Fe3+ ions in MOSF with NaBH4 at normal pressures and temperatures, where water was used as a green solvent. The final materials were tested for their applicability in the remediation of Cr(VI). The main objectives of this work are (1) to synthesize nanoscale zero-valent iron supported inside MOSF composites (Mx-NZVI) with different NZVI contents; (2) to characterize Mx-NZVI composites with TEM, SEM, XRD, XPS, nitrogen isotherms analysis, magnetization measurements, and so on; (3) to evaluate Cr(VI) adsorption performance of Mx-NZVI composites; (4) to study the possible mechanism for the removal of Cr(VI) using Mx-NZVI composites.


## 2. Materials and Methods

### 2.1. Materials

The following reagents were used as purchased without further purification: EO20PO70EO20 (denoted as P123, where EO is poly(ethylene oxide) and PO is poly(propylene oxide)) was purchased from Sigma-Aldrich. Tetramethyl orthosilicate (TMOS) was purchased from Energy Chemical (Shanghai, China). Other chemicals were purchased from Kelong Chemical Reagents Factory (Chengdu, China).


### 2.2. Synthesis of MOSF

MOSF was synthesized at 35°C in a pH = 5.0 buffer solution with P123 as the template according to the method reported previously [36]. Briefly, at 35°C, P123 (1 g) and Na2SO4 (1.7 g, 0.40 M) were dissolved in pH = 5.0 NaAc–HAc (Ac = acetate) buffer solution (30 g) (Ct = 0.04 M, where Ct = CNaAc + CHAc) to form a homogeneous solution under stirring. To this solution mixture, TMOS (1.52 g) was added under stirring. After 5 minutes, the stirring was stopped. The resultant mixture was kept in a static condition for 24 h and then hydrothermally treated at 100°C for another 24 h. The white precipitates were filtered, repeatedly washed with water to remove the inorganic salts, and then dried at room temperature. The final MOSF products were obtained by calcination at 550°C for 5 h at heating steps of 2°C·min−1.


### 2.3. Preparation of MOSF-Supported Nanoscale Zero-Valent Iron Composites (Mx-NZVI)

MOSF-supported nanoscale zero-valent iron was synthesized according to a protocol reported by Petala [30]. Briefly, MOSF (0.2 g) was dispersed in absolute ethanol (5 g), followed by the addition of a 10 wt% ethanolic solution (0.5, 1.0, and 1.5 g) containing FeCl3·6H2O. The mixture was heated at 45°C to evaporate the solvent, and then the obtained powder was dispersed in 5 mL of absolute ethanol again. The reducing agent was prepared by dissolving NaBH4 (0.56, 0.112, and 0.168 g) in 50 mL of deionized water and was added drop-wise to the MOSF-Fe3+ solution while swirling by hand. The mixture was filtered and washed with water once and absolute ethanol three times and then dried in vacuum oven overnight. The weight percentage of iron in the final product was calculated to be 4.31, 8.30, and 12.8 wt% according to the results of AAS (see Characterization), denoted Ma-NZVI, Mb-NZVI, and Mc-NZVI, respectively.


### 2.4. Characterization

The 2θ X-ray powder diffraction data (XRD) were collected with a DX-1000 CSC diffraction instrument at 40 kV and 25 mA. The scanning scope and scanning speed were in the 2θ range from 5 to 80°, in steps of 3° per min. Scanning electron microscopy (SEM) images of Mx-NZVI were taken using a Navo NanoSEM 450 field-emission scanning electron microscope operated at 5 KV. X-ray photoelectron spectroscopy (XPS) measurements were performed with an AXIS UltraDLD (KRATOS). The linear background was subtracted from all spectra. N2 adsorption-desorption isotherms were measured on a Quantachrome NOVA 1000e surface area analyzer after degassing the samples at 180°C for 6 hours. The pore volume was calculated from the adsorption isotherms using BJH (Barrett–Joyner–Halenda) method. To determine the actual iron content loaded on the samples, the composites were extracted by diluted hydrofluoric acid and nitric acid. Obtained solution was analyzed by Atomic Absorption Spectroscopy (AAS) using SpectrAA 220FS. Magnetization (M) measurements were performed on a superconducting quantum interference device (SQUID) magnetometer (MPMS VSM). Magnetic hysteresis loops were characterized at temperature of 300 K in external applied magnetic fields (B) ranging from −7 to +7 T.


### 2.5. Batch Experiments for the Reduction of Cr(VI)

Cr(VI) adsorption isotherms were acquired through batch experiments. K2Cr2O7 was selected as the source of Cr(VI). 0.03 g of Mx-NZVI was added to 30 mL of K2Cr2O7 water solution (concentration of Cr(VI): 3, 6, 9, 12, 15 mg·L−1) followed by shaking (200 rpm) at 25°C for 24 h. The initial pH of the suspension was adjusted to 2 by 0.1 M HCl or NaOH solution. To explore the effect of coexisting cations on Cr(VI) removal, 100 mg·L−1 of each cations was added to 15 mg·L−1 of Cr(VI) solution without adjusting pH, respectively. After shaking, the suspension was filtered through a 0.45 μm membrane filter. The Cr(VI) concentration of the solution was then determined by using the 1,5-diphenylcarbazide method [41].All adsorption isotherm data were fitted with Langmuir isotherm model and Freundlich isotherm mode. The mathematical description of Langmuir isotherm model is given below [42]:(1)qeq=bQmaxCeq1+bCeq,where qeq is the adsorption capacity at equilibrium (mg·g−1), Ceq is residual metal ion concentration at equilibrium (mg·L−1), Qmax (mg·g−1) is the maximum adsorption amount of metal ion per gram of adsorbent, and b is a constant related to the energy or net enthalpy of adsorption (L·mg−1).The Freundlich isotherm explains the adsorption on a heterogeneous surface with uniform energy. This equation has the following form as(2)qe=KCe1/n,where K and n are the Freundlich constants, which are related to adsorption capacity and strength, respectively.The adsorption kinetic experiments were performed by adding a given mass of Mx-NZVI to 50 mL of K2Cr2O7 solution with the concentration of 15 mg·L−1 followed by shaking (200 rpm) at 25°C for 24 h. The initial pH of the suspension was adjusted to 2, 5, and 8. During the reaction, at different periods, aliquots of the under study suspension were taken at certain time intervals. After filtration, the Cr(VI) concentration was analyzed. The contact time (t) was calculated after the addition of adsorbent into the solution.In order to investigate the mechanism of absorption and potential rate controlling step, the pseudo-first-order and the pseudo-second-order kinetic model were used to fit experimental data. The Lagergren first-order equation is generally expressed as(3)dcdt=-KobsC;after integration of (3) with the boundary conditions as follows, t=0, C=C0, and, at t=t, C=C, the integrated form is given as (4)ln⁡CC0=-Kobst,where C0 and C express Cr(VI) concentration in the solution at time 0 and t and kobs is the rate constant of the pseudo-first-order reaction (min−1). The values of were linearly correlated with t. The straight-line plots of against t should give a linear relationship, from which rate constants (Kobs) can be determined from the slope and intercept of the plot.The pseudo-second-order kinetic rate equation is expressed as(5)dqtdt=kqeq-qt2,where qeq is the sorption capacity at equilibrium (mg·g−1), qt is the amount adsorbed at a contact time t (mg·g−1), and k is the rate constant (g·mg−1·min−1). k and qeq were calculated from the slope and intercept of the plots of t/qt versus t according to equation:(6)tqt=1kqeq2+tqeq.


## 2.1. Materials

The following reagents were used as purchased without further purification: EO20PO70EO20 (denoted as P123, where EO is poly(ethylene oxide) and PO is poly(propylene oxide)) was purchased from Sigma-Aldrich. Tetramethyl orthosilicate (TMOS) was purchased from Energy Chemical (Shanghai, China). Other chemicals were purchased from Kelong Chemical Reagents Factory (Chengdu, China).


## 2.2. Synthesis of MOSF

MOSF was synthesized at 35°C in a pH = 5.0 buffer solution with P123 as the template according to the method reported previously [36]. Briefly, at 35°C, P123 (1 g) and Na2SO4 (1.7 g, 0.40 M) were dissolved in pH = 5.0 NaAc–HAc (Ac = acetate) buffer solution (30 g) (Ct = 0.04 M, where Ct = CNaAc + CHAc) to form a homogeneous solution under stirring. To this solution mixture, TMOS (1.52 g) was added under stirring. After 5 minutes, the stirring was stopped. The resultant mixture was kept in a static condition for 24 h and then hydrothermally treated at 100°C for another 24 h. The white precipitates were filtered, repeatedly washed with water to remove the inorganic salts, and then dried at room temperature. The final MOSF products were obtained by calcination at 550°C for 5 h at heating steps of 2°C·min−1.


## 2.3. Preparation of MOSF-Supported Nanoscale Zero-Valent Iron Composites (Mx-NZVI)

MOSF-supported nanoscale zero-valent iron was synthesized according to a protocol reported by Petala [30]. Briefly, MOSF (0.2 g) was dispersed in absolute ethanol (5 g), followed by the addition of a 10 wt% ethanolic solution (0.5, 1.0, and 1.5 g) containing FeCl3·6H2O. The mixture was heated at 45°C to evaporate the solvent, and then the obtained powder was dispersed in 5 mL of absolute ethanol again. The reducing agent was prepared by dissolving NaBH4 (0.56, 0.112, and 0.168 g) in 50 mL of deionized water and was added drop-wise to the MOSF-Fe3+ solution while swirling by hand. The mixture was filtered and washed with water once and absolute ethanol three times and then dried in vacuum oven overnight. The weight percentage of iron in the final product was calculated to be 4.31, 8.30, and 12.8 wt% according to the results of AAS (see Characterization), denoted Ma-NZVI, Mb-NZVI, and Mc-NZVI, respectively.


## 2.4. Characterization

The 2θ X-ray powder diffraction data (XRD) were collected with a DX-1000 CSC diffraction instrument at 40 kV and 25 mA. The scanning scope and scanning speed were in the 2θ range from 5 to 80°, in steps of 3° per min. Scanning electron microscopy (SEM) images of Mx-NZVI were taken using a Navo NanoSEM 450 field-emission scanning electron microscope operated at 5 KV. X-ray photoelectron spectroscopy (XPS) measurements were performed with an AXIS UltraDLD (KRATOS). The linear background was subtracted from all spectra. N2 adsorption-desorption isotherms were measured on a Quantachrome NOVA 1000e surface area analyzer after degassing the samples at 180°C for 6 hours. The pore volume was calculated from the adsorption isotherms using BJH (Barrett–Joyner–Halenda) method. To determine the actual iron content loaded on the samples, the composites were extracted by diluted hydrofluoric acid and nitric acid. Obtained solution was analyzed by Atomic Absorption Spectroscopy (AAS) using SpectrAA 220FS. Magnetization (M) measurements were performed on a superconducting quantum interference device (SQUID) magnetometer (MPMS VSM). Magnetic hysteresis loops were characterized at temperature of 300 K in external applied magnetic fields (B) ranging from −7 to +7 T.


## 2.5. Batch Experiments for the Reduction of Cr(VI)

Cr(VI) adsorption isotherms were acquired through batch experiments. K2Cr2O7 was selected as the source of Cr(VI). 0.03 g of Mx-NZVI was added to 30 mL of K2Cr2O7 water solution (concentration of Cr(VI): 3, 6, 9, 12, 15 mg·L−1) followed by shaking (200 rpm) at 25°C for 24 h. The initial pH of the suspension was adjusted to 2 by 0.1 M HCl or NaOH solution. To explore the effect of coexisting cations on Cr(VI) removal, 100 mg·L−1 of each cations was added to 15 mg·L−1 of Cr(VI) solution without adjusting pH, respectively. After shaking, the suspension was filtered through a 0.45 μm membrane filter. The Cr(VI) concentration of the solution was then determined by using the 1,5-diphenylcarbazide method [41].All adsorption isotherm data were fitted with Langmuir isotherm model and Freundlich isotherm mode. The mathematical description of Langmuir isotherm model is given below [42]:(1)qeq=bQmaxCeq1+bCeq,where qeq is the adsorption capacity at equilibrium (mg·g−1), Ceq is residual metal ion concentration at equilibrium (mg·L−1), Qmax (mg·g−1) is the maximum adsorption amount of metal ion per gram of adsorbent, and b is a constant related to the energy or net enthalpy of adsorption (L·mg−1).The Freundlich isotherm explains the adsorption on a heterogeneous surface with uniform energy. This equation has the following form as(2)qe=KCe1/n,where K and n are the Freundlich constants, which are related to adsorption capacity and strength, respectively.The adsorption kinetic experiments were performed by adding a given mass of Mx-NZVI to 50 mL of K2Cr2O7 solution with the concentration of 15 mg·L−1 followed by shaking (200 rpm) at 25°C for 24 h. The initial pH of the suspension was adjusted to 2, 5, and 8. During the reaction, at different periods, aliquots of the under study suspension were taken at certain time intervals. After filtration, the Cr(VI) concentration was analyzed. The contact time (t) was calculated after the addition of adsorbent into the solution.In order to investigate the mechanism of absorption and potential rate controlling step, the pseudo-first-order and the pseudo-second-order kinetic model were used to fit experimental data. The Lagergren first-order equation is generally expressed as(3)dcdt=-KobsC;after integration of (3) with the boundary conditions as follows, t=0, C=C0, and, at t=t, C=C, the integrated form is given as (4)ln⁡CC0=-Kobst,where C0 and C express Cr(VI) concentration in the solution at time 0 and t and kobs is the rate constant of the pseudo-first-order reaction (min−1). The values of were linearly correlated with t. The straight-line plots of against t should give a linear relationship, from which rate constants (Kobs) can be determined from the slope and intercept of the plot.The pseudo-second-order kinetic rate equation is expressed as(5)dqtdt=kqeq-qt2,where qeq is the sorption capacity at equilibrium (mg·g−1), qt is the amount adsorbed at a contact time t (mg·g−1), and k is the rate constant (g·mg−1·min−1). k and qeq were calculated from the slope and intercept of the plots of t/qt versus t according to equation:(6)tqt=1kqeq2+tqeq.


## 3. Results and Discussion

Figure1 shows the wide-angle X-ray diffraction (XRD) patterns of Mx-NZVI (x=a, b, and c, where the weight percentage of iron is 4.31, 8.30, and 12.8%, resp.; see Materials and Methods). Mx-NZVI composites with different iron loading amount have the similar diffraction patterns. The characteristic peak at 2θ≈22° in the XRD patterns of samples indicates the presence of amorphous silica [39]. The peak intensity of amorphous silica weakens with increased loading amount of Fe0. Another peak at 2θ≈44.9° can be indexed to the diffraction of Fe0 with the space group of Im⁡3-m (JCPDS Card number 06–0696), indicating the presence of Fe0 in the MOSF matrix. The broad diffraction peak of Fe0 also demonstrates the small particle size of NZVI loaded in MOSF. Other diffractions due to the existence of iron oxides such as magnetite, γ-Fe2O3, or hematite are not observed in the XRD patterns of Mx-NZVI, which manifests iron predominantly in the Fe0 state.Figure 1
The wide-angle X-ray diffraction patterns of Mx-NZVI composites.From nitrogen sorption analysis, the BET surface areas, the pore sizes, and the total pore volumes of pristine MOSF and Mx-NZVI composites can be obtained. As shown in Figure S1, all samples show typical type II isotherms with relatively large hysteresis loops (see Figure S1 in Supplementary Material available online athttps://doi.org/10.1155/2017/3094606). Besides, the capillary condensation occurs at relatively pressure P/P0 higher than 0.9. Both can demonstrate the macroporous structure of MOSF and Mx-NZVI. The structural parameters of MOSF and Mx-NZVI are summarized in Table S1. The surface area and total pore volume of MOSF are 503 m2·g−1 and 1.81 cm3·g−1, respectively. With the increase of iron loading amount from 4.31% to 12.8%, the surface area decreases from 379 to 311 m2·g−1, and the pore volume reduces from 1.56 to 1.28 cm3·g−1. Although after the loading of iron in MOSF, the pore size drops slightly from 124 nm (MOSF) to 117 nm (Mc-NZVI), Mx-NZVI materials still maintain the macroporous structure. Such marcoporous structure with large pore size and high pore volume may benefit the fast diffusion and transportation of Cr(VI) ions during adsorption process.The surface morphologies and structures of MOSF and Mx-NZVI were investigated by scanning electron microscope (SEM), as seen in Figure2. SEM images of MOSF and Mx-NZVI clearly show uniform hexagonally arrayed columns in large scale. Few aggregated ZVI nanoscale particles can be observed on the surface of MOSF, which indicates most of the NZVI are loaded inside the pores of MOSF. Furthermore, TEM characterization demonstrates similar results to those of SEM. As displayed in Figure 3(a), pristine MOSF exhibits the foam-like structure packed by polyhedral units following a surface minimization principle [43]. The typical TEM images of Mc-NZVI at a low and a higher magnification are shown in Figures 3(b) and 3(c). Macropores of Mc-NZVI with the diameter of ~100 nm can be clearly observed, indicating that the foam-like structure of MOSF can be well maintained after the loading of NZVI particles in MOSF. Besides, the homogeneous distribution of NZVI particles in MOSF (dark dots with a high contrast in Figures 3(b) and 3(c)) without aggregation can be clearly seen through the whole sample. NZVI particles supported in MOSF have the elliptical shape with the size distribution of 20–120 nm according to the size distribution histogram of NZVI particles counted in Figure 3(b) (Supporting Information, Figure S2). Inset of Figure 3(c) shows TEM image of NZVI nanoparticles inside MOSF with higher resolution. NZVI nanoparticles possess a typical core-shell structure, in which the shell thickness is less than 10 nm, similar to the previous observations. The core is mainly made up of Fe0 and the shell could result from the inevitable oxidation of zero-valent iron [22, 44, 45]. Figure 3(d) is a typical high resolution TEM image of NZVI particles supported by MOSF, where the (200) lattice fringes of Fe0 can be clearly observed in the NZVI. TEM observation confirms that, with the supporting of MOSF matrix, the aggregation degree of NZVI particles can be minimized. Mx-NZVI composites with lower NZVI loading amount, namely, Ma-NZVI and Mb-NZVI, were also characterized by TEM (Supporting Information, Figure S3). Due to the lower content of iron, the number of ZVI nanoparticles supported in MOSF is less compared with Mc-NZVI. Elemental maps of Mc-NZVI elucidate the homogeneous distribution of zero-valent iron nanoparticles in MOSF (Figure 4). Fe, Si, and O elements are found uniformly distributed and well correlated with the shape of the sample area.Figure 2
SEM images of MOSF (a), Ma-NZVI (b), Mb-NZVI (c), and Mc-NZVI(d), respectively.
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(d)Figure 3
TEM images of MOSF (a) and Mc-NZVI at a low magnification (b). (c) and inset of (c) are TEM images of Mc-NZVI at higher magnification. (d) is the HRTEM image of ZVI nanoparticles.
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(d)Figure 4
DF-STEM image (a) and the corresponding Si (b), O (c), and Fe (d) elemental maps of Mc-NZVI.
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(d)To further confirm the successful loading of homogeneously dispersed NZVI particles in MOSF, XPS analysis was carried out. The survey spectrum of Mc-NZVI (Figure5(a)) reveals the existence of Fe, O, Si, and C, in good agreement with the results of elemental maps. In Fe 2p (Figure 5(b)), a photoelectron peak appears at 707 eV, indicating the presence of Fe0 inside MOSF. It is noteworthy that two photoelectron peaks are located at 711.7 eV and 725.4 eV, which can be assigned to the Fe 2p3/2 and Fe 2p1/2 for Fe(II) and Fe(III) species [22]. Such results are conflicting with the XRD results. From XRD analysis, the presence of Fe(II)/Fe(III) species inside MOSF cannot be detected, while, according to XPS results, Fe(II)/Fe(III) species and Fe0 are both found in MOSF. Such conflict may be due to the amorphous nature of Fe(II)/Fe(III) species acting as shells around the NZVI, or because of the small amount that cannot be detected by XRD. Because the XPS analysis could only detect the photoelectrons from the outer surface with the thickness of 10 nm, it is supposed that the thickness of the shell of Fe(II)/Fe(III) species around the ZVI nanoparticles could be less than 10 nm considering the appearance of Fe0 signal in the Fe 2p spectrum [46]. According to the results of TEM, XRD, and XPS, it can be concluded that NZVI nanoparticles inside the pores of MOSF have a core-shell structure, where the core is composed of NZVI and the shell is Fe(II)/Fe(III) species with the shell thickness of less than 10 nm. The similar results are found in the XPS analysis for Ma-NZVI and Mb-NZVI (Supporting Information, Figure S4(a-b)).Figure 5
XPS spectra of the Mc-NZVI: (a) the survey scan and (b) Fe 2p.
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(b)Magnetization measurements were taken to reveal the physical properties of Mx-NZVI samples. Figure6 shows the hysteresis loops of Mx-NZVI composites recorded at 300 K. All samples show ferromagnetic or ferrimagnetic characteristics, corresponding to the metallic Fe0 or iron oxide phases. Saturation magnetization (Ms) at 20 KOe is ~3.77 and 11.81 to 17.70 emu/g for Ma-NZVI, Mb-NZVI, and Mc-NZVI, which comes as a consequence of the hybrid-microstructured nature with the introduction of iron species. The hysteresis loops of Mb-NZVI and Mc-NZVI display coercivity (Hc) of about 0.275 and 0.278 kOe, which are higher than that of the Ma-NZVI (about 0.062 kOe), indicating the difference in the shell thickness of iron oxide and crystal size of iron core [46]. The magnetization with applied field shows smooth change in the hysteresis loops, suggesting that iron core and iron oxide shell were in intimate contact and exchange coupled [47].Figure 6
Hysteresis loops of Mx-NZVI composites recorded at 300 K.The maximum adsorption capacities of the Mx-NZVI composites on hexavalent chromium removal were estimated by conducting a series of batch experiments. The Cr(VI) adsorption isotherms and the fitting results are demonstrated in Table S2. The adsorption data are slightly better fitted to Langmuir isotherm model (Figure7(a)) than Freundlich isotherm model (Supporting Information, Figure S5a) because the coefficient (R2) for Langmuir isotherm model is higher. Such correlation results indicate the adsorption process of Cr(VI) occurs on the homogeneous surface of Mx-NZVI materials [40]. It is observed that the adsorption capacities of Mx-NZVI composites can be improved with increased iron loading amount. The maximum Cr(VI) adsorption capacities of Ma-NZVI, Mb-NZVI, and Mc-NZVI are calculated to be 5.415, 7.658, and 12.665 mg·g−1, respectively.Figure 7
(a) Cr(VI) adsorption isotherms of Mx-NZVI composites; (b) adsorption kinetics of Mx-NZVI composites. (c) Adsorption kinetics of Mc-NZVI with different dosage. (d) Adsorption kinetics of Mc-NZVI at different initial pH. (e) Cr(VI) uptake of Mc-NZVI as a function of pH. (f) The effect of coexisting cations on Cr(VI) adsorption capacity of Mc-NZVI. The initial Cr(VI) concentration is 15 mg⋅L−1.
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(f)Figures7(b) and 7(c) display the Cr(VI) adsorption kinetics of Mx-NZVI composites, and the kinetic parameters are summarized in Table S3. All the experimental data can be fitted to the pseudo-second-order kinetic model with a high correlation coefficient over 0.98 (Supporting Information, Figure S5(b–d)), suggesting that the sorption of Cr(VI) by Mx-NZVI is mainly through chemisorption [48]. In addition, the pseudo-first-order model was also used to interpret the experimental data, but the fitting result was not very good as pseudo-second-order model (Supporting Information, Figure S6). It is noted that, in all kinetic experiments, a rapid removal rate of Cr(VI) is displayed during initial 3 h, which hints that most of the adsorption sites exist on the surface of the adsorbent and are easily accessible by the Cr(VI) species [49]. Then, the removal rate slightly declines in the later adsorption stage. The rate declination can be explained as below. During the adsorption process, first Cr(VI) species in aqueous solution move to Mx-NZVI. Then, physical/chemical adsorption of Cr(VI) occurs on the surface of Mx-NZVI material. Finally, Fe0 is oxidized to Fe(III) and Cr(VI) is reduced by Fe0 to Cr(III), and precipitation of Cr(III) forms on the surface of Mx-NZVI [50]. The rate declination is caused by the formation of chromium oxide precipitates or Fe(III)–Cr(III) hydroxides, which may exist as a thin layer on the surface of Mx-NZVI. The presence of thin layer prevents the electron transferring from NZVI to Cr(VI) and thus accordingly eliminates the following reduction of Cr(VI) to Cr(III) [44].When the dosage of Mx-NZVI is 3 g·L−1 and the initial concentration of Cr(VI) is 15 mg·L−1, the equilibrium can be reached after 500–700 min (Figure 7(b)). After 24 h adsorption, 48.28% of Cr(VI) can be removed by Ma-NZVI, while nearly 100% of Cr(VI) can be eliminated using Mc-NZVI. According to the rate constant which is related to removal rate of Cr(VI), Mc-NZVI with the highest rate constant of 0.0115 g·mg·min−1 exhibits the fastest Cr(VI) removal rate from water among three samples.The effect of Mc-NZVI dosage (1.0 to 3.0 g L−1) on the adsorption kinetics of Cr(VI) with the initial concentration of 15.0 mg·L−1 was investigated. As exhibited in Figure 7(c), the Cr(VI) removal efficiency increases significantly from 45.04% to nearly 100% as the dosage of Mc-NZVI grows from 1 g·L−1 to 3 g·L−1 in 24 h. This phenomenon is attributed to the increase of the active sites on the surface of Mc-NZVI [51]. In addition, the adsorption rate of Cr(VI) is also enhanced with the increase of Mc-NZVI dosage. With the dosage changing from 1 to 3 g·L−1, the rate constants are 0.00304, 0.00381, and 0.01115 (g·mg·min−1), respectively. Apparently, the high dosage of Mc-NZVI is beneficial for the fast adsorption rate due to increment of active sites.The dependence of the Cr(VI) removal efficiency on pH was investigated by adjusting the solution pH to 2, 5, and 8. The initial Cr(VI) concentration is 15 mg·L−1 and the Mc-NZVI dosage is 3.0 g·L−1. As shown in Figure 7(d), the Cr(VI) removal efficiency decreases significantly with the increase of initial pH. Only 21.16% of Cr(VI) is adsorbed at pH 8.0 after 24 h, while 100% of Cr(VI) can be removed within 24 h at pH 2.0. What is more, adsorption capacity of Mc-NZVI at other higher pH has also been studied (Figure 7(e)). Removal efficiency was 100% at pH 2 and 3. When the pH was higher than 3, a sharp decrease can be clearly seen in the removal efficiency. Clearly, the acidity of the Cr(VI) solution has a major influence on the removal efficiency of Cr(VI), which can be explained by following points. On one hand, the reduction of Cr(VI) by Fe0 would produce hydroxyl ions. Under low pH condition, hydroxyl ions can be consumed by H+, leading to the much easier reaction between Cr(VI) and Fe0. This process can be clearly expressed by the following equations (7)–(9):(7)Fe0+2H+⟶Fe2++H2↑(8)HCrO4-+3Fe2++7H+⟶3Fe3++Cr3++4H2O(9)2HCrO4-+3Fe0+14H+⟶3Fe3++Cr3++8H2OOn the other hand, pH has an impact on the surface charge of Mc-NZVI and Cr(VI) species. In the pH range of 2–8, the predominant species of Cr(VI) is negatively chargedHCrO4-/CrO42- [52]. The lower initial pH of the solution can result in the surface of Mc-NZVI with more positive charge. Hence, in pH of 2, the electrostatic interaction between Cr(VI) species and Mc-NZVI is much stronger compared with that in pH of 11. Accordingly, the Cr(VI) adsorption capacity of Mc-NZVI decreases with the increase of pH [53]. What is more, the solubility of Fe(III)–Cr(III) coprecipitation existing as a thin layer around NZVI is very low when the pH of solution is comparatively high [54], providing resistance for the subsequent redox adsorption of Cr(VI) [30]. These explain why a lower pH environment benefits the Cr(VI) removal in aqueous solution.The effect of common cations (Na+, K+, Mg2+, and Ca2+) in ground water was also investigated without adjusting pH. As shown in Figure 7(f), with the absence of coexisting cations, the removal efficiency was only 30.56%. With the addition of K+, the removal efficiency can be enhanced to 53.84%. The removal efficiency can be as high as 100% in the presence of Na+, Mg2+, and Ca2+. Obviously, the presence of cations can greatly improve the removal of Cr(VI) by Mc-NZVI composites, indicating the applicability of Mx-NZVI composites in the removal of Cr(VI) in ground water.To provide direct evidence to our explanation for possible adsorption and reduction mechanism of Cr(VI) with Mx-NZVI, the XPS analysis was carried out for Mc-NZVI after absorbing Cr(VI) (15 mg·L−1) at initial pH 2 and 25°C in a powder mode. The survey spectrum (Figure 8(a)) confirms coexistence of Fe, O, Si, Cr, and adventitious C. Figure 8(b) shows the high resolution XPS spectra of Fe 2p of Mc-NZVI after Cr(VI) removal. The Fe species in the form of Fe0 cannot be detected because the NZVI particles are covered with the oxide layer and/or Fe(III)–Cr(III) coprecipitation, which hinder the reaction process. The XPS scan of the Cr 2p region is shown in Figure 8(c) with Cr 2p1/2 and Cr 2p3/2 lining at 586.0 and 576.7 eV for Cr(III), respectively. It can be confirmed that Cr(VI) is reduced to Cr(III) by NZVI particles on the surface of the sample. The peak positions of Cr 2p1/2 and Cr 2p3/2 for Cr(VI) are comparatively higher located at 587.9 and 579.0 eV [22, 28, 55]. According to the quantitative curve fitting to the individual peak areas of Cr 2p peaks, about 70% of the chromium species has been reductive transformation into Cr(III) on the surface of Mx-NZVI. After the reduction of Fe0, Cr(III) and Fe(III) form a thin layer of Fe(III)–Cr(III) hydroxides on the outer surface of ZVI nanoparticles. Aforementioned date imply that the adsorption of Cr(VI) is based on both chemisorption and chemical reduction processes, and chemical reduction played a main role.Figure 8
XPS spectra of the Cr(VI)-adsorbed Mc-NZVI. (a) is the survey, (b) is Fe 2p, and (c) is Cr 2p spectra of Cr(VI)-adsorbed Mc-NZVI.
(a)
(b)
(c)In light of the aforementioned results, we hypothesize that the removal of Cr(VI) by Mx-NZVI composites may go through the reduction or/and precipitation processes. When Cr(VI) species in the solution diffuse into the pores of Mx-NZVI and are absorbed on the surfaces of the NZVIs, Cr(VI) is reduced to Cr(III) by NZVI inside the macropores [28, 52]. Such reduction process could proceed via direct or indirect pathway as shown in Figure 9. The direct pathway can be described by the reduction of Cr(VI) to Cr(III) due to the electron transfer from Fe0 core, coupled with direct oxidation of Fe0 to Fe(III). Meanwhile, another indirect pathway presents the reduction reaction between Cr(VI) and Fe(II) [22, 50]. These active Fe(II) species derive from the electron transfer of Fe0 species, expressed by the following equations:(10)Fe-2e⟶Fe2+(11)Fe+2Fe3+⟶3Fe2+In the precipitation process, (CrxFe1–x)(OH)3 or CrxFe1–xOOH precipitates could form through the reaction of Cr (III) and Fe (III). Such precipitates are coated on the surface of NZVI as a passive layer [50], causing the gradual increase in the resistance of electron transform from Fe0 to Cr(VI). As a result, Cr(VI) species retain on Fe(III)/Cr(III) hydroxide layer on the surface of Mx-NZVI rather than being reduced to Cr(III) [55].Figure 9
Schematic illustration of Cr(VI) removal mechanism by Mx-NZVI composites.


## 4. Conclusion

In this study, well-dispersed nanoscale zero-valent iron supported in macroporous silica foams composites as the efficient Cr(VI) adsorbents has been fabricated and characterized. Through the support of MOSF matrix with large surface area and high pore volume, the reactivity and stability of Mx-NZVI composites were improved due to the prevention of aggregation of NZVI. NZVI nanoparticles inside MOSF showed a typical core-shell architecture, in which the core mainly consisted of Fe0 and the thin shell (less than 10 nm) is largely made of Fe(II)/Fe(III) species. Mx-NZVI composites with macroporous structure and homogeneously dispersed NZVI particles in nanoscale range (20–120 nm) exhibited the good Cr(VI) adsorption performance. Batch experiments showed the composites were efficient adsorbents for the fast removal of Cr(VI) from aqueous solution. The kinetic data were well fitted to pseudo-second-order kinetic model, implying a chemisorption process. The adsorption capacities increased as the Mc-NZVI dosage and NZVI loading amount increased and fell as pH increased. It was also observed that the adsorption of Cr(VI) was fitted well on the Langmuir isotherm equilibrium. However, further experiments are still needed to investigate the remove process in real waste water and for other contaminants.



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*Source: 3094606-2017-09-10.xml*