# Removal of Zinc from Aqueous Solutions by Magnetite Silica Core-Shell Nanoparticles

Authors: Masoomeh Emadi; Esmaeil Shams; Mohammad Kazem Amini
Journal: Journal of Chemistry
 (2013)

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## Abstract

Magnetite silica core-shell nanoparticles (Fe3O4-SiO2) were synthesized and evaluated as a nanoadsorbent for removing Zn(II) from aqueous solutions. The core-shell nanoparticles were prepared by combining coprecipitation and sol-gel methods. Nanoparticles were characterized by X-ray diffraction, transmission electron microscopy (TEM), and FT-IR. The magnetization values of nanoparticles were measured with vibrating sample magnetometer (VSM). The adsorption of Zn(II) ions was examined by batch equilibrium technique. The effects of pH, initial Zn(II) concentration, and contact time on the efficiency of Zn(II) removal were studied. The equilibrium data, analyzed by using Langmuir and Freundlich isotherm models, showed better agreement with the former model. Using the Langmuir isotherm model, maximum capacity of the nanoadsorbent for Zn(II) was found to be 119 mg g−1 at room temperature. Kinetic studies were conducted and the resulting data were analyzed using first- and second-order equations; pseudo-second-order kinetic equation was found to provide the best correlation. The adsorption and sedimentation times were very low. The nanoadsorbent can be easily separated from aqueous solution by a magnet. Repeated adsorption acid regeneration cycles were performed to examine the stability and reusability of the nanoadsorbent. The result of this study proved high stability and reusability of Fe3O4-SiO2 as an adsorbent for Zn(II) ions.


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## Body

## 1. Introduction

Water pollution due to toxic heavy metals remains a serious environmental and public problem [1]. Among heavy metals, zinc is frequently used in the production of steel, alkaline batteries, and anticorrosive paintings. High concentrations of Zn(II) have been observed in wastewaters from pharmaceutical, galvanizing, paint, pigment, insecticide, and cosmetic industries. It has also been reported that zinc ion occurs in the leachate of landfills at high concentrations [2, 3]. Low concentration of zinc is necessary for the growth of living systems, but it can easily form large aggregates, which may become harmful to health once beyond the permissible limits [3]. Thus, the removal of zinc like other heavy metals from aqueous solutions is a critical challenge for environmental researchers.Various processes and methods such as precipitation, electrochemical treatment, chemical oxidation reduction, membrane separation, solvent extraction, and ion exchange have been employed to remove metal pollutants from aqueous solutions [4]. However, most of these methods suffer from low removal efficiency, especially when large volumes of dilute heavy metal solutions are present [5]. Adsorption is one of the most effective and economic techniques for removing heavy metal ions from aqueous solutions. The efficiency of adsorption relies on the capability of the adsorbent to concentrate or adsorb metal ions from solution onto its surfaces and the rate of removing ions from the solution. Different adsorbents such as activated carbon [6], zeolites [7, 8], resins [9, 10], biosorbents [4, 11], hydrogel, and magnetic hydrogel [12, 13] have been used for the removal of heavy metal ions by adsorption. Despite the availability of a number of adsorbents for the removal of low concentrations of heavy metal ions from aqueous solutions, there is still a need for the development of new adsorbent with superior adsorption capacity, facile adsorption-desorption kinetics, high stability, and easiness of operation.Recently, nanometer-sized materials have been used for wastewater treatment [14–16]. These materials possess a series of unique physical and chemical properties. These materials have large surface area and are easily dispersed in aqueous solutions. In addition, a large number of their atoms are surface atoms which are unsaturated and have high adsorption capacities to many metal ions [15, 17]. However, from a practical point of view, there is a major drawback to the application of such nanomaterials for treating wastewater. Because the treatment of wastewater is usually conducted in a suspension of the nanostructures, an additional separation step is required to remove the nanomaterials from a large volume of solution, resulting in increased expenses [18].Nanometer-sized iron oxide-based materials with superparamagnetic characteristic are very effective as adsorbents for heavy metal ions removal. Superparamagnetic particles adhered to the target can be removed very quickly from a matrix using a magnetic field, but they do not retain their magnetic properties when the field is removed [19]. This system also has several advantages compared with conventional and other nanoadsorbents in that the process does not generate secondary waste and the materials involved can be recycled and facilely used on an industrial scale. Furthermore, the magnetic particles can be tailored to fix and separate metal species in water, wastes, or slurries [20, 21]. In recent years, different magnetic nanoparticles (MNPs) have been synthesized and used as sorbents for removal or preconcentration of heavy metal ions [14, 22–28]. Unmodified magnetic Fe2O3 and Cu(II) ion imprinted Fe3O4 nanoparticles were employed as adsorbents for the removal of Cr(VI) [22] and Cu(II) [23], respectively, from wastewater. Capturing of As(III) and As(VI) by magnetite (Fe3O4) nanoparticles modified with oleic acid have been reported [24]. Undecanoic acid-modified Fe3O4 nanoparticles have been reported to be efficient for removal of Cd(II) [25]. Attachment of chitosan [26], humic acid [27], α-ketoglutaric acid-modified chitosan [14], and dimercaptosuccinic acid [19] on Fe3O4 nanoparticles resulted in magnetic sorbent materials effective for the removal of heavy metal ions from water. However, it should be pointed out that uncoated magnetic nanoparticles are highly susceptible to oxidation when exposed to atmosphere and also susceptible to leaching under acidic conditions [23, 29]. In addition, due to the hydrophobic interactions between the sub-nm size particles, iron oxide MNPs tend to aggregate to micron size clusters. In the presence of an external magnetic field, further magnetization of these aggregates can occur increasing their aggregation [29]. The aggregation of MNPs may alter their magnetic properties and their adsorption efficiency. Therefore, stabilization of iron oxide MNPs by coating their surface is an important issue. Organic polymers, silica, metals (e.g., gold), and organic dyes have been used as stabilizing agents for iron oxide MNPs [29]. Silica coating has attractive properties including: biocompatibility [29], high adsorption capacity, acid-base properties, insolubility in most solvents, and chemical and thermal stability [30]. Being hydrophilic in nature, silica-coated core-shell MNPs can be easily dispersed in aqueous solutions. Furthermore, since SiO2 is stable under acidic conditions, iron oxide-SiO2 MNPs can be used as adsorbent in acidic solutions. The surface of silica is dominated by hydroxyl or silanol groups. Silanol groups participate in adsorption as well as chemical modification of the silica surface. At pHs greater than its isoelectric point (>2) silica exhibits ion exchange capabilities via these weakly acidic silanol groups [31]. In addition, silica can be grafted with a variety of functional groups, leading to considerable enhancement of their surface properties. In spite of their good characteristics, the use of silica-coated core-shell MNPs in heavy metal removal is quite rare [32, 33].The versatile application of several types of silica as adsorbent for heavy metal ions removal [34, 35] motivated us to synthesize Fe3O4-SiO2 for this purpose. Magnetite nanoparticles were synthesized by coprecipitation method and their surface covered with silica shell using sol-gel technique in alkaline solution. The nanoparticles were characterized and tested as adsorbent for Zn(II) removal from aqueous solutions. The important factors affecting the adsorption efficiency such as solution pH, contact time, and initial Zn(II) concentration were investigated. The best kinetic and isotherm models were found from experimental data.


## 2. Materials and Methods

### 2.1. Synthesis of Fe3O4-SiO2 Nanoparticles

Chemical coprecipitation as a simple but effective method for preparation of hydrophilic nanoparticles [36] was used for the preparation of magnetite nanoparticles by a little modification of the methodology already described in the literature [37]. According to this method, 3.5 g FeCl2·4H2O and 8.0 g FeCl3·6H2O with molar ratio 1 : 2 were dissolved in 38 mL of deoxygenated 0.4 M HCl solution. The resulting solution was rapidly added to 375 mL of deoxygenated 0.7 M ammonia solution under argon flow. After sonication for 30 minutes, the magnetite nanoparticles were separated with a permanent magnet and washed twice with pure ethanol. The synthesized MNPs were suspended in 150 mL deionized water for use in the next steps.Classical Stöber method [38] (base-catalyzed hydrolysis and condensation of tetraethoxysilane (TEOS)) was used for coating magnetite nanoparticles with a silica shell. Typically, 20 mL of magnetite suspended in water was added to 200 mL 2-propanol and sonicated at room temperature for 15 min under argon flow. Then 20 mL water and 10 mL NH3 (28%, Merck) were added, respectively, and after 15 min 1.3 mL of TEOS (99%, Aldrich) was introduced into the suspension and the mixture was again sonicated for 1 h. Fe3O4-SiO2 nanoparticles was centrifuged at 3000 rpm for 10 minutes, the solvent was discarded and nanoparticles were washed two times with water and ethanol, respectively, and dried in vacuum oven at room temperature.


### 2.2. Characterization of Fe3O4-SiO2

The synthesized MNPs were characterized using X-ray diffraction (XRD) (Bruker D8 Advance, with Ni-filtered Cu-Kα source of 1.5406 Å), transmission electron microscopy (TEM) (Phillips-CM10 operating at 100 kV with a Cu grid), and FT-IR (Jasco model 6300). Vibrating sample magnetometer (VSM) (PAR EG&G 4500) was used to determine magnetization value of the MNPs. EDX spectra were recorded by Energy-dispersive X-ray spectroscopy (EDX) (Philips XL 30).


### 2.3. Batch Removal Experiments

Adsorption of Zn(II) was carried out by batch technique at room temperature. The isotherm studies were performed by mixing 10 mg adsorbent (dry) with 10 mL of a solution containing Zn(NO3)2 at known concentration into a 20 mL polypropylene tube and insert it in the ultrasonic bath. After reaching adsorption equilibrium, MNPs were separated from the aqueous solution using a 1.2 T neodymium iron boron magnet. Then metal analysis of the solutions was performed by atomic absorption spectrophotometry (AAS) (Shimadzu AA-670). The equilibrium concentration of the adsorbed Zn(II), qe (in mg g−1), was calculated according to (1):
(1)qe=(Co-Ce)VM,
where Co and Ce (in mg L−1) are the initial and equilibrium concentrations of Zn(II) in solution, respectively, V (in L) is the total volume of the solution, and M (in g) is the adsorbent mass.The effect of pH on the adsorption of Zn(II) by the MNPs was studied in the range of 2.0–8.0. The pH was adjusted by adding appropriate amounts of 0.1 M hydrochloric acid or 0.1 M sodium hydroxide.Kinetic studies were performed under similar conditions used for isotherm studies and at pH 6.0 which was the optimum pH for Zn(II) removal. In these studies aliquots of the supernatant were withdrawn for Zn(II) analysis at different periods of time.


### 2.4. Desorption, Reusability, and Stability Studies

To study the regeneration efficiency of the adsorbent, the adsorption step was performed batchwise as described previously, and then nanoadsorbents were separated magnetically and added to 1.0 mL of the desorbing solution. The mixture was placed in ultrasonic bath for 15 min at room temperature. To evaluate desorption efficiency, MNPs were separated magnetically and the concentration of Zn(II) in the desorbing solution was determined using AAS. The reusability of the adsorbent was studied by repeating the adsorption-desorption cycles consecutively.Stability of Fe3O4-SiO2 nanoparticles under harsh acidic conditions was examined by dispersing 20 mg of the nanoparticles in 10.0 mL 2.0 M HCl and stirring for 12 h. The iron concentration in leachate was measured by AAS.


## 2.1. Synthesis of Fe3O4-SiO2 Nanoparticles

Chemical coprecipitation as a simple but effective method for preparation of hydrophilic nanoparticles [36] was used for the preparation of magnetite nanoparticles by a little modification of the methodology already described in the literature [37]. According to this method, 3.5 g FeCl2·4H2O and 8.0 g FeCl3·6H2O with molar ratio 1 : 2 were dissolved in 38 mL of deoxygenated 0.4 M HCl solution. The resulting solution was rapidly added to 375 mL of deoxygenated 0.7 M ammonia solution under argon flow. After sonication for 30 minutes, the magnetite nanoparticles were separated with a permanent magnet and washed twice with pure ethanol. The synthesized MNPs were suspended in 150 mL deionized water for use in the next steps.Classical Stöber method [38] (base-catalyzed hydrolysis and condensation of tetraethoxysilane (TEOS)) was used for coating magnetite nanoparticles with a silica shell. Typically, 20 mL of magnetite suspended in water was added to 200 mL 2-propanol and sonicated at room temperature for 15 min under argon flow. Then 20 mL water and 10 mL NH3 (28%, Merck) were added, respectively, and after 15 min 1.3 mL of TEOS (99%, Aldrich) was introduced into the suspension and the mixture was again sonicated for 1 h. Fe3O4-SiO2 nanoparticles was centrifuged at 3000 rpm for 10 minutes, the solvent was discarded and nanoparticles were washed two times with water and ethanol, respectively, and dried in vacuum oven at room temperature.


## 2.2. Characterization of Fe3O4-SiO2

The synthesized MNPs were characterized using X-ray diffraction (XRD) (Bruker D8 Advance, with Ni-filtered Cu-Kα source of 1.5406 Å), transmission electron microscopy (TEM) (Phillips-CM10 operating at 100 kV with a Cu grid), and FT-IR (Jasco model 6300). Vibrating sample magnetometer (VSM) (PAR EG&G 4500) was used to determine magnetization value of the MNPs. EDX spectra were recorded by Energy-dispersive X-ray spectroscopy (EDX) (Philips XL 30).


## 2.3. Batch Removal Experiments

Adsorption of Zn(II) was carried out by batch technique at room temperature. The isotherm studies were performed by mixing 10 mg adsorbent (dry) with 10 mL of a solution containing Zn(NO3)2 at known concentration into a 20 mL polypropylene tube and insert it in the ultrasonic bath. After reaching adsorption equilibrium, MNPs were separated from the aqueous solution using a 1.2 T neodymium iron boron magnet. Then metal analysis of the solutions was performed by atomic absorption spectrophotometry (AAS) (Shimadzu AA-670). The equilibrium concentration of the adsorbed Zn(II), qe (in mg g−1), was calculated according to (1):
(1)qe=(Co-Ce)VM,
where Co and Ce (in mg L−1) are the initial and equilibrium concentrations of Zn(II) in solution, respectively, V (in L) is the total volume of the solution, and M (in g) is the adsorbent mass.The effect of pH on the adsorption of Zn(II) by the MNPs was studied in the range of 2.0–8.0. The pH was adjusted by adding appropriate amounts of 0.1 M hydrochloric acid or 0.1 M sodium hydroxide.Kinetic studies were performed under similar conditions used for isotherm studies and at pH 6.0 which was the optimum pH for Zn(II) removal. In these studies aliquots of the supernatant were withdrawn for Zn(II) analysis at different periods of time.


## 2.4. Desorption, Reusability, and Stability Studies

To study the regeneration efficiency of the adsorbent, the adsorption step was performed batchwise as described previously, and then nanoadsorbents were separated magnetically and added to 1.0 mL of the desorbing solution. The mixture was placed in ultrasonic bath for 15 min at room temperature. To evaluate desorption efficiency, MNPs were separated magnetically and the concentration of Zn(II) in the desorbing solution was determined using AAS. The reusability of the adsorbent was studied by repeating the adsorption-desorption cycles consecutively.Stability of Fe3O4-SiO2 nanoparticles under harsh acidic conditions was examined by dispersing 20 mg of the nanoparticles in 10.0 mL 2.0 M HCl and stirring for 12 h. The iron concentration in leachate was measured by AAS.


## 3. Results and Discussion

### 3.1. Nanoadsorbent Characterization

Powder X-ray diffraction (XRD) patterns were used to identify the crystalline structure of magnetite and Fe3O4-SiO2. XRD peaks with 2θ at 30.4°, 35.6°, 43.3°, 57.3°, and 62.8° (Figure 1(a)) show good consistency with the reported data and can be indexed to pure phase of Fe3O4 structure. The average crystallite size of the Fe3O4 nanoparticles calculated from Scherrer’s equation was 11 nm. Figure 1(b) shows that the XRD pattern of the Fe3O4-SiO2 nanoparticles is very similar to that of the uncoated Fe3O4 nanoparticles. This indicates the stability of the crystalline phase of Fe3O4 nanoparticles after silica coating. It also indicates that the silica coating is in amorphous form.X-ray patterns of (a) Fe3O4 and (b) Fe3O4-SiO2.
(a)
(b)The background corrected FT-IR spectra of MNPs are presented in Figure2. The absorption bands around 580–610 and 410–440 cm−1 in the IR spectra of both Fe3O4 and Fe3O4-SiO2 nanoparticles (Figures 2(a) and 2(b)) correspond to Fe–O bonds, and are attributed to the formation of the ferrite phase. In addition, the final product obtained from the coprecipitation was dense, black and magnetic implying the presence of magnetite as the main phase. Comparison of the FT-IR patterns shows a pronounced change in the 1300–700 cm−1 region, indicating the presence of the silica coating. The peaks at 970 and 1088 cm−1 correspond to symmetric stretching of Si–O and Si–O–Si, respectively [39], and The broad band around 3400 cm−1 can be assigned to O–H stretching vibrations.FT-IR of (a) uncoated and (b) silica-coated magnetite nanoparticles.
(a)
(b)Figure3(a) shows the TEM image of the MNPs. The mean diameter determined from the TEM image is about 20 nm, which agrees approximately with the value calculated from the Scherrer formula for the strongest diffraction peak in the X-ray diffraction patterns. As shown in the TEM image, despite their hydrophilicity, the magnetite particles tend to aggregate. This is due to the ultrasmall size and the requirement to decrease their interface energy [36]. Therefore, the crystallite size evaluated from X-ray diffraction is smaller than the nanoparticles size estimated from TEM. Silica phases can be seen in Figure 3(b) which shows the TEM image of Fe3O4-SiO2. The average size of nanoparticles in Figure 3(b) (30 nm) is larger than that of Figure 3(a) (20 nm) indicating that the silica shell thickness is in the nanometer range.TEM images of (a) bare magnetite and (b) silica-coated magnetite.
(a)
(b)The EDX spectrum of silica-coated nanoparticles is shown in Figure4. Atomic weight ratio of O : Si : Fe was 37.423 : 27.086 : 35.491, which indicates the magnetite nanoparticles are successfully coated by silica.Figure 4
EDX spectrum of silica-coated magnetite nanoparticles.Magnetic measurements of the pure and the silica coated Fe3O4 nanoparticles were carried out using a VSM. The saturation magnetic moments of pure Fe3O4 and Fe3O4-SiO2 nanoparticles were 65.5 and 31.5 emu g−1, respectively (Figure 5). The smallest saturation magnetization value for Fe3O4-SiO2 nanoparticles can be explained by considering the diamagnetic contribution of the silica shells surrounding the Fe3O4 nanoparticles [40]. In addition, both Fe3O4 and Fe3O4-SiO2 nanoparticles showed superparamagnetic property at room temperature. These magnetic properties are critical in the applications of MNPs in separation. An efficient magnetic separation is allowed when the MNPs undergo strong magnetization, however, when the applied magnetic field is removed, redispersion of the MNPs will take place rapidly.Figure 5
VSM of (…) magnetite and (- -) silica-coated magnetite nanoparticles.


### 3.2. Metal Removal Experiments

#### 3.2.1. Chemical Affinity as a Function of pH

It is well documented that solution pH is an important parameter affecting the sorption of heavy metal ions. Therefore, the dependence of Zn(II) uptake on pH was studied at a constant Zn(II) concentration (10 mg L−1) using 10 mg of the nanoadsorbent. As shown in Figure 6, Zn(II) adsorption increase with increasing pH in the range of 2.0–5.0 and is approximately independent of pH in the range of 5.0–8.0. Thus, pH 6.0 was adopted for further studies. The dependence of metal sorption on pH is related to both the surface functional groups of the adsorbent and the metal ion chemistry in solution [41]. The hydrolysis of Zn2+ has been investigated at different pHs and various pressures by several authors [42–46]. It has been shown that in the pH range 2.0–9.0 the system is quite simple, containing Zn2+ and ZnOH+ ions but at higher pHs Zn(OH)2 may precipitate [45]. Lower adsorption percentage of Zn(II) on the nanoparticles at highly acidic conditions (pH ≤ 2) is probably due to the presence of high concentration of H+ ions on the adsorbent surface competing with Zn(II) for adsorption sites. With an increase in the solution pH (3.0–8.0), the silanol groups become deprotonated and, consequently, the removal efficiency is increased.Figure 6
Effect of solution pH on the adsorption of Zn(II) onto Fe3O4-SiO2 nanoparticles adsorbent. Conditions: 10.0 mL of 10.0 mg L−1 Zn(II) solution and 10.0 mg of adsorbent.


#### 3.2.2. Effect of Contact Time and the Metal Sorption Kinetics

One of the most important parameters that significantly describe the adsorbent characteristics is sorption time. Sorption kinetics was studied to determine the time required for the adsorption to reach the equilibrium. Figure7(a) shows a plot of Zn(II) adsorption versus contact time. The plot clearly shows three distinct regions. In the initial 5 minutes, the adsorption of Zn(II) is very rapid so that more than 90% of Zn(II) ions are adsorbed during this period. However, in the interval between 5 to 20 min, the adsorption kinetics slow down and gradually tends to level off. At times greater than 20 min the adsorption reaches its maximum value and becomes independent of contact time, illustrating that adsorption equilibrium is achieved. The fast step of the Zn(II) adsorption may occur on the particle surface due to an immediate interaction between Zn(II) ions and the active –SiOH groups on the surface of the Fe3O4-SiO2 nanoparticles. Although the equilibrium was achieved after 20 min, a contact time of 1 h was selected for further works to be confident of the equilibrium establishment.Figure 7
Effect of contact time on the adsorption of Zn(II) onto the Fe3O4-SiO2 nanoparticles at room temperature and pH 6.0 (a), and the corresponding plots of pseudo-first-order (b) and pseudo-second-order (c) kinetic models. Conditions are the same as Figure 5.The pseudo-first-order and pseudo-second-order kinetic equations were chosen to fit the obtained adsorption kinetics data and to estimate the rate constant of the adsorption phenomenon.The pseudo-first-order rate equation is generally expressed as:(2)log⁡⁡(qe-qt)=log⁡⁡qe-k1t2.303,
where qe and qt are the amount of species adsorbed per unit mass of adsorbent (mg g−1) at equilibrium and at any time t, respectively and k1 is the rate constant of pseudo-first-order adsorption (min−1).The pseudo-second-order rate equation is given as follows:(3)tqt=1k2qe2+tqe,
where k2 is the rate constant of pseudo-second-order sorption (g mg−1 min−1).Figures7(b) and 6(c) show the results of this study, presented as plots of log(qe-qt) and t/qt versus t from zero to 20 minutes. As shown in these figures, the adsorption of Zn(II) onto Fe3O4-SiO2 nanoparticles is more appropriately described by a pseudo-second-order kinetic model since its correlation coefficient (0.999) is greater than that of the pseudo-first-order model (0.886) and also the difference between the theoretical qe (10 mg g−1) and experimental qe (9.9 mg g−1) is smaller than the values calculated based on the pseudo-first-order kinetic model (3 mg g−1). The rate constant of the pseudo-second-order adsorption of Zn(II) onto Fe3O4-SiO2 nanoparticles, k2, was found to be 0.37 g mg−1min−1.


#### 3.2.3. Effect of Initial Zn(II) Concentration and Metal Sorption Isotherms

To find maximum capacity of the adsorbent which is very important for the design of adsorption systems, the equilibrium adsorption isotherms were constructed. The adsorption isotherm of Zn(II) ions by the MNPs at constant pH 6.0 is shown in Figure8(a). Based on the kinetic studies, a period of 1 h was selected as the contact time to ensure that equilibrium is reached. The equilibrium data were analyzed according to the linear form of the Langmuir sorption isotherm as:
(4)ceqe=1KLqmax⁡+1qmax⁡ce,
where qe is the adsorption capacity (mg g−1) based on the dry weight of nanoadsorbent, Ce is the equilibrium concentration of metal ion (mg L−1) in solution, qmax is the maximum adsorption capacity (mg g−1) of metal that can be adsorbed in a monolayer, and KL is the Langmuir adsorption equilibrium constant (L mg−1) that is related to the energy of adsorption. The Langmuir plot is represented in Figure 8(b). The parameters of this model, calculated from Figure 8(b), are given in Table 1. A good agreement between the model and the experimental data suggests that the sorbed Zn(II) ions form a monolayer on the adsorbent surface.Table 1
Isotherm models for Zn(II) sorption onto magnetic nanoparticles.
Mathematical model
Equation
Correlation coefficient
q
m (mg g-1) or 1/n
K
L (L mg-1) or KF (L mg-1)
Langmuir
c
e
/
q
e
=
0.059
+
0.008
c
e
0.997
125.0
0.1356
Freundlich
log
q
e
=
1.117
+
0.663
log
c
e
0.975
0.663
13.09Figure 8
Adsorption of Zn(II) ions the Fe3O4-SiO2 nanoparticles at pH 6.0 and room temperature as a function of initial Zn(II) concentration (a), and the corresponding Langmuir (b) and Freundlich (c) isotherm plots.The Freundlich model, which assumes that different sites with several adsorption energies are involved, was also tested to describe the sorption data. The linear representation of the Freundlich adsorption equation is(5)log⁡⁡⁡qe=log⁡⁡KF+1nlog⁡⁡Ce,
where KF is the energy term and n is an exponent term related to the strength of the adsorption. The Freundlich plot is shown in Figure 8(c) and the KF and 1/n parameters with the corresponding determination coefficient, R2, are presented in Table 1.Table1 shows that the adsorption behavior of Zn(II) ions onto the magnetic nanoparticles is best described by the Langmuir isotherm model because this model yields a higher determination coefficient and a smaller difference between theoretical qmax (119 mg g−1) and experimental qe (101 mg g−1).


#### 3.2.4. Desorption and Reusability Studies

Restoring the adsorption capacity of exhausted adsorbents is an important factor in practical application. Therefore, the reusability of the Fe3O4-SiO2 was tested. To investigate the possibility of restoring the adsorption capacity, at first desorption experiments were conducted under batch experimental conditions. The suppressed adsorption of Zn(II) ions on Fe3O4-SiO2 nanoparticles at low pHs (Figure 6) implies that the adsorbent could be regenerated by acid treatment. Among the various examined acids including acetic acid, hydrochloric acid, sulfuric acid and nitric acid (all at 0.1 M concentration), hydrochloric acid showed the best regenerating results. The effect of HCl concentration on the regeneration efficiency was also studied and it was observed that the desorption efficiency increases with increasing the acid concentration up to 1.0 M and then remained constant. Therefore, 1.0 M hydrochloric acid was used as the optimum for all subsequent experiments. The stability of Fe3O4-SiO2 nanoparticles under acidic conditions was also examined by measuring the extent of Fe leached into the solution per gram of the adsorbent after contacting it for 12 h with 1.0 M hydrochloric acid. The Fe leaching of less than 3 wt.% confirmed the stability of the adsorbent under acidic conditions, which be related to the effect of silica coating.The reusability of the adsorbent for zinc ion adsorption was tested by repeating the adsorption-desorption cycle several times using the same adsorbent. The result of this study showed that the adsorbent retained about 93% of its initial sorption efficiency after 7 cycles. This property allows multiple uses of adsorbents for at least 7 times.


## 3.1. Nanoadsorbent Characterization

Powder X-ray diffraction (XRD) patterns were used to identify the crystalline structure of magnetite and Fe3O4-SiO2. XRD peaks with 2θ at 30.4°, 35.6°, 43.3°, 57.3°, and 62.8° (Figure 1(a)) show good consistency with the reported data and can be indexed to pure phase of Fe3O4 structure. The average crystallite size of the Fe3O4 nanoparticles calculated from Scherrer’s equation was 11 nm. Figure 1(b) shows that the XRD pattern of the Fe3O4-SiO2 nanoparticles is very similar to that of the uncoated Fe3O4 nanoparticles. This indicates the stability of the crystalline phase of Fe3O4 nanoparticles after silica coating. It also indicates that the silica coating is in amorphous form.X-ray patterns of (a) Fe3O4 and (b) Fe3O4-SiO2.
(a)
(b)The background corrected FT-IR spectra of MNPs are presented in Figure2. The absorption bands around 580–610 and 410–440 cm−1 in the IR spectra of both Fe3O4 and Fe3O4-SiO2 nanoparticles (Figures 2(a) and 2(b)) correspond to Fe–O bonds, and are attributed to the formation of the ferrite phase. In addition, the final product obtained from the coprecipitation was dense, black and magnetic implying the presence of magnetite as the main phase. Comparison of the FT-IR patterns shows a pronounced change in the 1300–700 cm−1 region, indicating the presence of the silica coating. The peaks at 970 and 1088 cm−1 correspond to symmetric stretching of Si–O and Si–O–Si, respectively [39], and The broad band around 3400 cm−1 can be assigned to O–H stretching vibrations.FT-IR of (a) uncoated and (b) silica-coated magnetite nanoparticles.
(a)
(b)Figure3(a) shows the TEM image of the MNPs. The mean diameter determined from the TEM image is about 20 nm, which agrees approximately with the value calculated from the Scherrer formula for the strongest diffraction peak in the X-ray diffraction patterns. As shown in the TEM image, despite their hydrophilicity, the magnetite particles tend to aggregate. This is due to the ultrasmall size and the requirement to decrease their interface energy [36]. Therefore, the crystallite size evaluated from X-ray diffraction is smaller than the nanoparticles size estimated from TEM. Silica phases can be seen in Figure 3(b) which shows the TEM image of Fe3O4-SiO2. The average size of nanoparticles in Figure 3(b) (30 nm) is larger than that of Figure 3(a) (20 nm) indicating that the silica shell thickness is in the nanometer range.TEM images of (a) bare magnetite and (b) silica-coated magnetite.
(a)
(b)The EDX spectrum of silica-coated nanoparticles is shown in Figure4. Atomic weight ratio of O : Si : Fe was 37.423 : 27.086 : 35.491, which indicates the magnetite nanoparticles are successfully coated by silica.Figure 4
EDX spectrum of silica-coated magnetite nanoparticles.Magnetic measurements of the pure and the silica coated Fe3O4 nanoparticles were carried out using a VSM. The saturation magnetic moments of pure Fe3O4 and Fe3O4-SiO2 nanoparticles were 65.5 and 31.5 emu g−1, respectively (Figure 5). The smallest saturation magnetization value for Fe3O4-SiO2 nanoparticles can be explained by considering the diamagnetic contribution of the silica shells surrounding the Fe3O4 nanoparticles [40]. In addition, both Fe3O4 and Fe3O4-SiO2 nanoparticles showed superparamagnetic property at room temperature. These magnetic properties are critical in the applications of MNPs in separation. An efficient magnetic separation is allowed when the MNPs undergo strong magnetization, however, when the applied magnetic field is removed, redispersion of the MNPs will take place rapidly.Figure 5
VSM of (…) magnetite and (- -) silica-coated magnetite nanoparticles.


## 3.2. Metal Removal Experiments

### 3.2.1. Chemical Affinity as a Function of pH

It is well documented that solution pH is an important parameter affecting the sorption of heavy metal ions. Therefore, the dependence of Zn(II) uptake on pH was studied at a constant Zn(II) concentration (10 mg L−1) using 10 mg of the nanoadsorbent. As shown in Figure 6, Zn(II) adsorption increase with increasing pH in the range of 2.0–5.0 and is approximately independent of pH in the range of 5.0–8.0. Thus, pH 6.0 was adopted for further studies. The dependence of metal sorption on pH is related to both the surface functional groups of the adsorbent and the metal ion chemistry in solution [41]. The hydrolysis of Zn2+ has been investigated at different pHs and various pressures by several authors [42–46]. It has been shown that in the pH range 2.0–9.0 the system is quite simple, containing Zn2+ and ZnOH+ ions but at higher pHs Zn(OH)2 may precipitate [45]. Lower adsorption percentage of Zn(II) on the nanoparticles at highly acidic conditions (pH ≤ 2) is probably due to the presence of high concentration of H+ ions on the adsorbent surface competing with Zn(II) for adsorption sites. With an increase in the solution pH (3.0–8.0), the silanol groups become deprotonated and, consequently, the removal efficiency is increased.Figure 6
Effect of solution pH on the adsorption of Zn(II) onto Fe3O4-SiO2 nanoparticles adsorbent. Conditions: 10.0 mL of 10.0 mg L−1 Zn(II) solution and 10.0 mg of adsorbent.


### 3.2.2. Effect of Contact Time and the Metal Sorption Kinetics

One of the most important parameters that significantly describe the adsorbent characteristics is sorption time. Sorption kinetics was studied to determine the time required for the adsorption to reach the equilibrium. Figure7(a) shows a plot of Zn(II) adsorption versus contact time. The plot clearly shows three distinct regions. In the initial 5 minutes, the adsorption of Zn(II) is very rapid so that more than 90% of Zn(II) ions are adsorbed during this period. However, in the interval between 5 to 20 min, the adsorption kinetics slow down and gradually tends to level off. At times greater than 20 min the adsorption reaches its maximum value and becomes independent of contact time, illustrating that adsorption equilibrium is achieved. The fast step of the Zn(II) adsorption may occur on the particle surface due to an immediate interaction between Zn(II) ions and the active –SiOH groups on the surface of the Fe3O4-SiO2 nanoparticles. Although the equilibrium was achieved after 20 min, a contact time of 1 h was selected for further works to be confident of the equilibrium establishment.Figure 7
Effect of contact time on the adsorption of Zn(II) onto the Fe3O4-SiO2 nanoparticles at room temperature and pH 6.0 (a), and the corresponding plots of pseudo-first-order (b) and pseudo-second-order (c) kinetic models. Conditions are the same as Figure 5.The pseudo-first-order and pseudo-second-order kinetic equations were chosen to fit the obtained adsorption kinetics data and to estimate the rate constant of the adsorption phenomenon.The pseudo-first-order rate equation is generally expressed as:(2)log⁡⁡(qe-qt)=log⁡⁡qe-k1t2.303,
where qe and qt are the amount of species adsorbed per unit mass of adsorbent (mg g−1) at equilibrium and at any time t, respectively and k1 is the rate constant of pseudo-first-order adsorption (min−1).The pseudo-second-order rate equation is given as follows:(3)tqt=1k2qe2+tqe,
where k2 is the rate constant of pseudo-second-order sorption (g mg−1 min−1).Figures7(b) and 6(c) show the results of this study, presented as plots of log(qe-qt) and t/qt versus t from zero to 20 minutes. As shown in these figures, the adsorption of Zn(II) onto Fe3O4-SiO2 nanoparticles is more appropriately described by a pseudo-second-order kinetic model since its correlation coefficient (0.999) is greater than that of the pseudo-first-order model (0.886) and also the difference between the theoretical qe (10 mg g−1) and experimental qe (9.9 mg g−1) is smaller than the values calculated based on the pseudo-first-order kinetic model (3 mg g−1). The rate constant of the pseudo-second-order adsorption of Zn(II) onto Fe3O4-SiO2 nanoparticles, k2, was found to be 0.37 g mg−1min−1.


### 3.2.3. Effect of Initial Zn(II) Concentration and Metal Sorption Isotherms

To find maximum capacity of the adsorbent which is very important for the design of adsorption systems, the equilibrium adsorption isotherms were constructed. The adsorption isotherm of Zn(II) ions by the MNPs at constant pH 6.0 is shown in Figure8(a). Based on the kinetic studies, a period of 1 h was selected as the contact time to ensure that equilibrium is reached. The equilibrium data were analyzed according to the linear form of the Langmuir sorption isotherm as:
(4)ceqe=1KLqmax⁡+1qmax⁡ce,
where qe is the adsorption capacity (mg g−1) based on the dry weight of nanoadsorbent, Ce is the equilibrium concentration of metal ion (mg L−1) in solution, qmax is the maximum adsorption capacity (mg g−1) of metal that can be adsorbed in a monolayer, and KL is the Langmuir adsorption equilibrium constant (L mg−1) that is related to the energy of adsorption. The Langmuir plot is represented in Figure 8(b). The parameters of this model, calculated from Figure 8(b), are given in Table 1. A good agreement between the model and the experimental data suggests that the sorbed Zn(II) ions form a monolayer on the adsorbent surface.Table 1
Isotherm models for Zn(II) sorption onto magnetic nanoparticles.
Mathematical model
Equation
Correlation coefficient
q
m (mg g-1) or 1/n
K
L (L mg-1) or KF (L mg-1)
Langmuir
c
e
/
q
e
=
0.059
+
0.008
c
e
0.997
125.0
0.1356
Freundlich
log
q
e
=
1.117
+
0.663
log
c
e
0.975
0.663
13.09Figure 8
Adsorption of Zn(II) ions the Fe3O4-SiO2 nanoparticles at pH 6.0 and room temperature as a function of initial Zn(II) concentration (a), and the corresponding Langmuir (b) and Freundlich (c) isotherm plots.The Freundlich model, which assumes that different sites with several adsorption energies are involved, was also tested to describe the sorption data. The linear representation of the Freundlich adsorption equation is(5)log⁡⁡⁡qe=log⁡⁡KF+1nlog⁡⁡Ce,
where KF is the energy term and n is an exponent term related to the strength of the adsorption. The Freundlich plot is shown in Figure 8(c) and the KF and 1/n parameters with the corresponding determination coefficient, R2, are presented in Table 1.Table1 shows that the adsorption behavior of Zn(II) ions onto the magnetic nanoparticles is best described by the Langmuir isotherm model because this model yields a higher determination coefficient and a smaller difference between theoretical qmax (119 mg g−1) and experimental qe (101 mg g−1).


### 3.2.4. Desorption and Reusability Studies

Restoring the adsorption capacity of exhausted adsorbents is an important factor in practical application. Therefore, the reusability of the Fe3O4-SiO2 was tested. To investigate the possibility of restoring the adsorption capacity, at first desorption experiments were conducted under batch experimental conditions. The suppressed adsorption of Zn(II) ions on Fe3O4-SiO2 nanoparticles at low pHs (Figure 6) implies that the adsorbent could be regenerated by acid treatment. Among the various examined acids including acetic acid, hydrochloric acid, sulfuric acid and nitric acid (all at 0.1 M concentration), hydrochloric acid showed the best regenerating results. The effect of HCl concentration on the regeneration efficiency was also studied and it was observed that the desorption efficiency increases with increasing the acid concentration up to 1.0 M and then remained constant. Therefore, 1.0 M hydrochloric acid was used as the optimum for all subsequent experiments. The stability of Fe3O4-SiO2 nanoparticles under acidic conditions was also examined by measuring the extent of Fe leached into the solution per gram of the adsorbent after contacting it for 12 h with 1.0 M hydrochloric acid. The Fe leaching of less than 3 wt.% confirmed the stability of the adsorbent under acidic conditions, which be related to the effect of silica coating.The reusability of the adsorbent for zinc ion adsorption was tested by repeating the adsorption-desorption cycle several times using the same adsorbent. The result of this study showed that the adsorbent retained about 93% of its initial sorption efficiency after 7 cycles. This property allows multiple uses of adsorbents for at least 7 times.


## 3.2.1. Chemical Affinity as a Function of pH

It is well documented that solution pH is an important parameter affecting the sorption of heavy metal ions. Therefore, the dependence of Zn(II) uptake on pH was studied at a constant Zn(II) concentration (10 mg L−1) using 10 mg of the nanoadsorbent. As shown in Figure 6, Zn(II) adsorption increase with increasing pH in the range of 2.0–5.0 and is approximately independent of pH in the range of 5.0–8.0. Thus, pH 6.0 was adopted for further studies. The dependence of metal sorption on pH is related to both the surface functional groups of the adsorbent and the metal ion chemistry in solution [41]. The hydrolysis of Zn2+ has been investigated at different pHs and various pressures by several authors [42–46]. It has been shown that in the pH range 2.0–9.0 the system is quite simple, containing Zn2+ and ZnOH+ ions but at higher pHs Zn(OH)2 may precipitate [45]. Lower adsorption percentage of Zn(II) on the nanoparticles at highly acidic conditions (pH ≤ 2) is probably due to the presence of high concentration of H+ ions on the adsorbent surface competing with Zn(II) for adsorption sites. With an increase in the solution pH (3.0–8.0), the silanol groups become deprotonated and, consequently, the removal efficiency is increased.Figure 6
Effect of solution pH on the adsorption of Zn(II) onto Fe3O4-SiO2 nanoparticles adsorbent. Conditions: 10.0 mL of 10.0 mg L−1 Zn(II) solution and 10.0 mg of adsorbent.


## 3.2.2. Effect of Contact Time and the Metal Sorption Kinetics

One of the most important parameters that significantly describe the adsorbent characteristics is sorption time. Sorption kinetics was studied to determine the time required for the adsorption to reach the equilibrium. Figure7(a) shows a plot of Zn(II) adsorption versus contact time. The plot clearly shows three distinct regions. In the initial 5 minutes, the adsorption of Zn(II) is very rapid so that more than 90% of Zn(II) ions are adsorbed during this period. However, in the interval between 5 to 20 min, the adsorption kinetics slow down and gradually tends to level off. At times greater than 20 min the adsorption reaches its maximum value and becomes independent of contact time, illustrating that adsorption equilibrium is achieved. The fast step of the Zn(II) adsorption may occur on the particle surface due to an immediate interaction between Zn(II) ions and the active –SiOH groups on the surface of the Fe3O4-SiO2 nanoparticles. Although the equilibrium was achieved after 20 min, a contact time of 1 h was selected for further works to be confident of the equilibrium establishment.Figure 7
Effect of contact time on the adsorption of Zn(II) onto the Fe3O4-SiO2 nanoparticles at room temperature and pH 6.0 (a), and the corresponding plots of pseudo-first-order (b) and pseudo-second-order (c) kinetic models. Conditions are the same as Figure 5.The pseudo-first-order and pseudo-second-order kinetic equations were chosen to fit the obtained adsorption kinetics data and to estimate the rate constant of the adsorption phenomenon.The pseudo-first-order rate equation is generally expressed as:(2)log⁡⁡(qe-qt)=log⁡⁡qe-k1t2.303,
where qe and qt are the amount of species adsorbed per unit mass of adsorbent (mg g−1) at equilibrium and at any time t, respectively and k1 is the rate constant of pseudo-first-order adsorption (min−1).The pseudo-second-order rate equation is given as follows:(3)tqt=1k2qe2+tqe,
where k2 is the rate constant of pseudo-second-order sorption (g mg−1 min−1).Figures7(b) and 6(c) show the results of this study, presented as plots of log(qe-qt) and t/qt versus t from zero to 20 minutes. As shown in these figures, the adsorption of Zn(II) onto Fe3O4-SiO2 nanoparticles is more appropriately described by a pseudo-second-order kinetic model since its correlation coefficient (0.999) is greater than that of the pseudo-first-order model (0.886) and also the difference between the theoretical qe (10 mg g−1) and experimental qe (9.9 mg g−1) is smaller than the values calculated based on the pseudo-first-order kinetic model (3 mg g−1). The rate constant of the pseudo-second-order adsorption of Zn(II) onto Fe3O4-SiO2 nanoparticles, k2, was found to be 0.37 g mg−1min−1.


## 3.2.3. Effect of Initial Zn(II) Concentration and Metal Sorption Isotherms

To find maximum capacity of the adsorbent which is very important for the design of adsorption systems, the equilibrium adsorption isotherms were constructed. The adsorption isotherm of Zn(II) ions by the MNPs at constant pH 6.0 is shown in Figure8(a). Based on the kinetic studies, a period of 1 h was selected as the contact time to ensure that equilibrium is reached. The equilibrium data were analyzed according to the linear form of the Langmuir sorption isotherm as:
(4)ceqe=1KLqmax⁡+1qmax⁡ce,
where qe is the adsorption capacity (mg g−1) based on the dry weight of nanoadsorbent, Ce is the equilibrium concentration of metal ion (mg L−1) in solution, qmax is the maximum adsorption capacity (mg g−1) of metal that can be adsorbed in a monolayer, and KL is the Langmuir adsorption equilibrium constant (L mg−1) that is related to the energy of adsorption. The Langmuir plot is represented in Figure 8(b). The parameters of this model, calculated from Figure 8(b), are given in Table 1. A good agreement between the model and the experimental data suggests that the sorbed Zn(II) ions form a monolayer on the adsorbent surface.Table 1
Isotherm models for Zn(II) sorption onto magnetic nanoparticles.
Mathematical model
Equation
Correlation coefficient
q
m (mg g-1) or 1/n
K
L (L mg-1) or KF (L mg-1)
Langmuir
c
e
/
q
e
=
0.059
+
0.008
c
e
0.997
125.0
0.1356
Freundlich
log
q
e
=
1.117
+
0.663
log
c
e
0.975
0.663
13.09Figure 8
Adsorption of Zn(II) ions the Fe3O4-SiO2 nanoparticles at pH 6.0 and room temperature as a function of initial Zn(II) concentration (a), and the corresponding Langmuir (b) and Freundlich (c) isotherm plots.The Freundlich model, which assumes that different sites with several adsorption energies are involved, was also tested to describe the sorption data. The linear representation of the Freundlich adsorption equation is(5)log⁡⁡⁡qe=log⁡⁡KF+1nlog⁡⁡Ce,
where KF is the energy term and n is an exponent term related to the strength of the adsorption. The Freundlich plot is shown in Figure 8(c) and the KF and 1/n parameters with the corresponding determination coefficient, R2, are presented in Table 1.Table1 shows that the adsorption behavior of Zn(II) ions onto the magnetic nanoparticles is best described by the Langmuir isotherm model because this model yields a higher determination coefficient and a smaller difference between theoretical qmax (119 mg g−1) and experimental qe (101 mg g−1).


## 3.2.4. Desorption and Reusability Studies

Restoring the adsorption capacity of exhausted adsorbents is an important factor in practical application. Therefore, the reusability of the Fe3O4-SiO2 was tested. To investigate the possibility of restoring the adsorption capacity, at first desorption experiments were conducted under batch experimental conditions. The suppressed adsorption of Zn(II) ions on Fe3O4-SiO2 nanoparticles at low pHs (Figure 6) implies that the adsorbent could be regenerated by acid treatment. Among the various examined acids including acetic acid, hydrochloric acid, sulfuric acid and nitric acid (all at 0.1 M concentration), hydrochloric acid showed the best regenerating results. The effect of HCl concentration on the regeneration efficiency was also studied and it was observed that the desorption efficiency increases with increasing the acid concentration up to 1.0 M and then remained constant. Therefore, 1.0 M hydrochloric acid was used as the optimum for all subsequent experiments. The stability of Fe3O4-SiO2 nanoparticles under acidic conditions was also examined by measuring the extent of Fe leached into the solution per gram of the adsorbent after contacting it for 12 h with 1.0 M hydrochloric acid. The Fe leaching of less than 3 wt.% confirmed the stability of the adsorbent under acidic conditions, which be related to the effect of silica coating.The reusability of the adsorbent for zinc ion adsorption was tested by repeating the adsorption-desorption cycle several times using the same adsorbent. The result of this study showed that the adsorbent retained about 93% of its initial sorption efficiency after 7 cycles. This property allows multiple uses of adsorbents for at least 7 times.


## 4. Conclusions

The present study demonstrates that Fe3O4-SiO2 nanoparticles are promising adsorbents for efficient removal of Zn(II) from aqueous solutions (see Table 2). The efficiency of adsorption was highly dependent on the initial concentration of Zn(II), pH, adsorbent dosage, and contact time. Langmuir and Freundlich isotherm models were employed to describe the Zn(II) adsorption. It was found that the adsorption behavior of Zn(II) ions onto the MNPs is best described by the Langmuir isotherm model. Zn(II) showed fast sorption kinetics following pseudo-second-order model. The equilibrium for Zn(II) adsorption onto the Fe3O4-SiO2 nanoparticles reached only after 20 minutes. The adsorbent can be easily and effectively regenerated by using 1.0 M HCl as the regenerating solution. Further, due to protection by inert silica layer, leaching of Fe3O4 during the adsorption and regeneration processes is negligible, hence the adsorbent can be used for multiple sorption-desorption steps. The adsorbent could be easily separated from the sorbing and regeneration solutions in short times (1.0 min) by using a magnet. The proposed adsorbent offers attractive properties compared to the previous ones such as high adsorption capacity (119 mg g−1), short equilibration (20 min) and sedimentation (1 min) times, and high stability. In conclusion, the above system can be a potential candidate for the practical removal of Zn(II) from aqueous solutions.Table 2
Important parameters of several adsorption systems for removal of Zn(II) from aqueous solutions.
Adsorbent
Maximum adsorption capacity (mg g-1)
Equilibrium time (min)
Reusability
Reference
Alternanthera philoxeroides biomass
18.57
60
Not reported
[39]
Native Lentinus edodes pellets
37.7
Inactive Lentinus edodes pellets
63.3
120
Not reported
[45]
Lewatit MonoPlus M 600
80.64
Lewatit MonoPlus MP 500
18.01
Lewatit MonoPlus MP 64
24.44
20
Retained about 95% of its initial efficiency after 10 cycles
[9]
Amberlite IRA 402
31.94
Hybrid precursor of silicon and carbon
28.76
30
Not reported
[46]
Sulfuric acid-treated rice husk (dry sorbent)
18.94
Sulfuric acid-treated rice husk (wet sorbent)
19.38
120
Not reported
[47]
Lemon peel
27.86
Lemon peel cellulose (LPC)
112.36
600
Not reported
[48]
Surface-modified LPC (LPCACS)
222.22
Amidoximated polyacrylonitrile/organobentonite composite
65.40
90–180
Retained about 85% of its initial efficiency after 4 cycles
[49]
Magnetic hydroxyapatite nanoparticles
140.6
576
Desorption efficiency in first cycle 67%
[50]
Magnetic nanoparticles coated with silica
119
20
Retained about 93% of its initial efficiency after 7 cycles
This work



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*Source: 787682-2012-07-10.xml*