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Abstract

The Fe₃O₄/Talc nanocomposite was synthesized by the coprecipitation-ultrasonication method. The reaction was carried out under a inert gas environment. The nanoparticles were characterized by X-ray diffraction (XRD), field-emission scanning electron microscopy (FESEM), fourier-transform infrared spectroscopy (FT-IR) and vibrating sample magnetometry techniques (VSM), the surface area of the nanoparticles was determined to be 77.92 m²/g by Brunauer-Emmett-Teller method (BET). The kinetic data showed that the adsorption process fitted with the pseudo-second order model. Batch experiments were carried out to determine the adsorption kinetics and mechanisms of Cr(VI) by Fe₃O₄/Talc nanocomposite. The adsorption process was found to be highly pH-dependent, which made the material selectively adsorb these metals from aqueous solution. The isotherms of adsorption were also studied using Langmuir and Freundlich equations in linear forms. It is found that the Langmuir equation showed better linear correlation with the experimental data than the Freundlich. The thermodynamics of Cr(VI) adsorption onto the Fe₃O₄/Talc nanocomposite indicated that the adsorption was exothermic. The reusability study has proven that Fe₃O₄/Talc nanocomposite can be employed as a low-cost and easy to separate.

Keywords

hexavalent chromium kinetics thermodynamics

Introduction

Chromium used for many applications in different industries, including alloy fabrication, corrosion protection of metals, paint, textile, tanning, electroplating (Sueker, 1964). Chromium discharged from these industries has caused serious pollution in the water environment. Chromium has five oxidation states (from +2 to +6) but three of them (Cr(0), Cr(III), Cr(VI)) are used commercially and present in the environment. The oxidation state of chromium affects its toxicity and mobility in aquatic media. In the aquatic environment, Chromium is found in predominantly two forms, trivalent chromium (Chromium (III) or Cr³⁺) which is nontoxic, less mobile and has a tendency to absorb to clays, sediments, organic matter, and hexavalent chromium, which is toxic, more mobile (Wilbur et al., 2000). According to WHO guidelines, the concentration of chromium in drinking water should not exceed 0.05 mg/l. IARC has classified chromium (VI) as carcinogenic (Group 1) and chromium (III) as noncarcinogen (Group 3) (WHO, 2003). There are many methods that used generally to remove chromium and other heavy metal from water (Mahmoodi et al., 2019; Mostafavi et al., 2019), such as adsorption (Chávez-Guajardo et al., 2015; Deveci and Kar, 2013), filtration (Gherasim et al., 2011; Jayalakshmi et al., 2012), precipitation [(Golbaz et al., 2014), ion exchang (Alvarado et al., 2013; Kalantari et al., 2014), electrochemical treatment (Malkoc et al., 2006). In recent years, nanotechnology is a practical approach in treating wastewaters, too. Among all these possible methods, those with cost-effective, environment-friendly and no further pollutant features are the favorites (Lofrano et al., 2017). The solid wastes could be used the development of new adsorbents, low – cost from biogenic sources (Badruddoza et al., 2013); waste materials from industry (Bhatnagar et al., 2011); locally available agricultural waste (Ligate and Mdoe, 2015). This adsorbent materials are capable of capturing heavy metal ions form aqueous solution. Such as nano Talc doped Fe₃O₄ materials, are many methods to produce the nano Fe₃O₄ materials such as coprecipitation (Jahanbakhsh et al., 2017; Wei et al., 2012), solvothermal reduction (Sun and Zeng, 2002; Vuong et al., 2015), polyol (Laurent et al., 2008), copolymer gels (Qi et al., 2011), electrochemical (Jouyandeh et al., 2019a; Jouyandeh et al., 2019b)),…. Maryam Jouyandeh (Jouyandeh et al., 2019c) et al. have electrochemically synthesized Zn_xFe_3-xO₄ magnetic nanoparticles to apply in curing epoxy. Now, to stabilize liquid particles, increase the dispersity and increase the specific surface area, scientists use Talc [Mg₃Si₄O₁₀(OH)₂ coatings on the surface of Fe₃O₄ particles. Talc has a platy structure that consists of three layers, including a magnesium hydroxide layer sandwiched between two silicate layers. Adjacent layers are connected by weak van der Waals forces. The surface of talc powder has a large number of Mg-O, OH, Si-O-Si and O-Si-O bonds that will cooperate or complex with heavy metal ions in water or soil to immobilize them on the surface of talc powder (Wang et al., 2018). Talc has been studied as an adsorbent for heavy metals in both forms: unmodified and modified talc. M.E. Ossman et al. used talc powder as an adsorbent for removing Cr(VI) from water. The results showed that the adsorption fitted well with the Freundlich model, optimization conditions include pH = 4, a contact time of 70 minutes to reach equilibrium (Ossman et al., 2014). Recently, some studies have been done on Fe₃O₄/Talc nanomaterial. Kamyar Shameli et al. (Kalantari et al., 2013) prepared Fe₃O₄ nanoparticles in talc as substrate using an environmentally friendly process. Fe₃O₄ MNPs have a mean size of 1.95–2.59 nm on the talc layers. K. Kalantari et al. (Kalantari et al., 2014) prepared Fe₃O₄/talc nanocomposites and used them as adsorbents for removing Cu(II), Ni(II), Pb(II) ions in the aqueous system. In optimal conditions, removal time of 120 s, removal efficiency for Cu(II), Ni(II), Pb(II) are 72.15%, 50.23%, 91.35%, respectively. The adsorption kinetics comply with the pseudo-second order kinetic equation and the Langmuir isotherm fitted well with data of the adsorption process. Shalini Rajput et al. (Rajput et al., 2016) synthesized Fe₃O₄ nanoparticles and used them for aqueous Cr(VI) and Pb(II) removal. Sorption data abided by pseudo-second order kinetics. The adsorptions of Cr(VI) and Pb(II) are in good agreement with the Sips and Langmuir models, respectively. The maximum adsorption capacities were 34.87 mg/g for Cr(VI) ions and 53.11 mg/g for Pb²⁺ ions at 45°C.

In Ultrasonic-assisted synthetic (Sonochemical synthesis) method, chemical reactions are facility due to the application of powerful ultrasound radiation (20 kHz–10 MHz). Sonochemistry generates small, hot bubbles that can archieve high temperature (5000–25,000 K), pressure of more than 1000 atmospheres and rate of cooling/heating that can exceed 10⁻¹¹ K/s. These can break chemical bonds or produces chemical and physical effects that can be used for the production or modification of nanostructured materials (Qiao et al., 2011). Untrasonic-assisted reaction produced the smaller size, purer and more dispersible nanomaterials (Jiang et al., 2012) .

In this work, The Fe₃O₄/Talc nanocomposites were synthesized on the surface of talc layers in aqueous solution using Ferric chloride hexahydrate (FeCl₃.6H₂O), frerrous chloride tetrahydrate (FeCl₂.4H₂O), NH₄OH as the iron precursor and reduction agent and Talcum powder substrate (Mg₃Si₄O₁₀(OH)₂). Talcum powder (30–50 µm) for preparing the nanocomposite was supplied by Talcum powder Phu Tho-Viet Nam. The adsorption isotherm, kinetic of Cr(VI) ion onto Fe₃O₄/Talc nanocomposite produced from Talc (Phu Tho – Viet Nam) were studied.

Materials and methods

Materials

Ferric chloride hexahydrate (FeCl₃.6H₂O), ferrous chloride tetrahydrate (FeCl₂.4H₂O) and potassium dichromate (K₂Cr₂O₇) was purchased from Merck. The Talc – VietNam (particle size ≤50 μm; density 2.4 g/cm³; main components include: SiO₂: 56.8%; MgO: 31.5%; Fe₂O₃: 3.5%). NH₄OH were obtained from Macklin-China, India. A stock solution of 1000 mgl⁻¹ Cr(VI) ions was made by dissolving 2.8289 g of K₂Cr₂O₇ in distilled water. The working solutions of desired concentrations were made by suitable dilution of the stock solution with distilled water. Deionized water was used for the preparation of all aqueous solutions.

Synthesis of Fe₃O₄/Talc nanocomposite

The material is synthesized by the coprecipitation-ultrasonication method on the talc layers in an inert atmosphere, with the 1:2 ratio of Fe²⁺/Fe³⁺. The Fe₃O₄/Talc nanocomposite was prepared by mixing FeCl₃.6H₂O and FeCl₂.4H₂O with a ratio of 2:1 into 100 ml of distilled water. Adding Talc to the solution and vigorously stirring by a magnetic stirrer for 120 minutes. The sonication of the reaction mixture was then performed by an ultrasonic probe (Sonics & materials – VCX500; 500 w, 20 kHz), 20 mL of 25–28% NH₃ solution was dropped gradually.

These procedures resulted in the formation of black precipitates of Fe₃O₄/Talc nanoparticles that was washed with distilled water several times until it reached the neutral pH, followed by washing twice with ethanol before dried in an oven at a temperature of 343 K. Figure 1 describes preparation process of the nanocomposite.

Figure 1.

The procedure for preparation of Fe₃O₄/Talc nanocomposite.

The structure of materials was characterized by X-ray diffraction patterns of the solid powders on a P’Pret Pro – PANalytical X-ray diffractometer at 1,8kW (40 mA/45 KV) using Cu Kα (λ=1.5406 Å) radiation. FTIR spectra of the solid samples were recorded by KBr pellet method using a Bruker FTIR spectrometer. FESEM measurements were carried out using a Hitachi S-4800, EMAX operating at 20 keV. The minimal amount of solid sample was dispersed in ethanol and small drops were placed on an aluminium grid. The grid was dried from 1–2 h in a vacuum over at 40°C prior to the FESEM studies. Magnetic measurements of the solid samples were performed at room temperature (25°C) using a Magnet B-10 Vibrating sample magnetometer (VSM).

Nitrogen adsorption-desorption isotherms were performed at 77 K in Tristar 3000-Micromeritics equipment, USA, using the static adsorption procedure. Samples were degassed at 80°C and 10⁻⁶Torr for minimum 12 h prior to analysis. BET surface areas were calculated from the linear part of BET plot according to IUPAC recommendation, pore size distributions of the samples were calculated via the conventional BJD model.

Batch adsorption procedure

Hexavalent chromium (Cr(VI)) adsorption was evaluated by the batch method, which permits to determinate of influence of parameters on the adsorption process easily. The batch adsorption experiments were carried out to investigate the influence of major affecting parameters like adsorbent dosage, pH, contact time, initial hexavalent chromium concentration and temperature on the amount of adsorption capacity. In the batch method, a fixed quantity of Fe₃O₄/Talc nanocomposite is mixed continuously with a specific volume of Cr(VI) solution and constantly shakened at 303 ± 1 K, until the equilibrium was reached. The contents in the flask were shaken in incubator Orbital shaker (OXYOS) at 120 r.min⁻¹. After shaking, the solutions were filtered through a Whatman No. 42 filter paper. The filtrate was collected in polyethylene tubes and diluted before analysis. During the study, the adsorbent dosage varied from 0.5 to 6.0 g.l⁻¹, pH from 4.0 to 9.0, the initial Cr(VI) concentration from 10 to 30 mg.l⁻¹, the temperature from 293 to 313 K and the contact time from 0 to 120 min. The pH of Cr(VI) solution was adjusted using either 0.1 N HCl or 0.1 N NaOH solutions to the required value.

For adsorption isotherms, a series of 100-ml flask glass were filled with 50 mL Cr(VI) solution of varying concentrations (10–30 mg.l⁻¹), maintained at the desired temperature and pH. After the amount of Fe₃O₄/Talc nanocomposite used for Cr(VI) solutions was 2.0 g.l⁻¹. The optimum uptake time 60 min the concentrations of chromium ion was calculated by taking the difference in their initial and final concentrations. In each experiment constant shaking of the solution was performed by using a shaker. All the experiments were repeated three times and average values were reported. The standard deviation was found to be ±2.0%.

Thermodynamic studies of Cr(VI) adsorption onto the Fe₃O₄/Talc nanocomposite were also carried out at three temperatures (297, 303 and 313 K). Kinetic studies of adsorption by Fe₃O₄/Talc nanocomposite were also carried out at four initial chromium concentrations from 10 to 25 mg.l⁻¹ at 303 K where in the extent of adsorption was analyzed at regular time intervals.

Analysis of Cr(VI) ions

The concentration of Cr(VI) ions in the sample was determined by UV visible spectrophotometer with GENESYS 10S UV-Vis using 1,5-Diphenylcarbazide in acidic solution (H₃PO₄). The absorbance of the purple colored complex was measured at 540 nm wavelength (Clesceri et al., 1998).

Adsorption capacity of Fe₃O₄/Talc nanocomposite was calculated by the formula (Ngah and Fatinathan, 2010):

q = \frac{(C_{o} - C_{t}) . V}{m}

(1)

Where, q is the amount of Cr(VI) ion adsorbed per unit mass of adsorbent (mg.g⁻¹), V is the volume of solution (l); m is the mass of adsorbent (g); C₀, C_t are Cr(VI) concentrations in the initial solution and at time t respectively (mg.l⁻¹).

The Cr(VI) ion removed by adsorbent was calculated by the formula:

% R = \frac{C_{0} - C_{e}}{C_{0}} \times 100

(2)

R is the percentage of Cr(VI) adsorbed by Fe₃O₄/Talc nanocomposite and C_e is Cr(VI) equilibrium concentrations (mg.l⁻¹).

Results and discussion

Characterization of Fe₃O₄/Talc nanocomposite

The resulted brown-black precipitate can be attracted by a permanent magnet (Figure 1) that proved the formation of Fe₃O₄ crystals onto Talc. Characterization of the material reveals X-ray, FESEM-EDX, BET, FT-IR and VSM measurements. The X-ray patterns (a) and FT-IR (b) of synthesized material are shown in Figure 2.

Figure 2.

X-ray patterns (a) and FT-IR (b) of Talc and Fe₃O₄/Talc nanocomposite.

Figure 2(a) depicts the powder X-ray diffraction (XRD) patterns of the Talc substrates and Fe₃O₄/Talc nanocomposite samples. The position and relative intensity of all diffraction peaks in both XRD patterns are fully matched. The peaks related to talc are observed at 2θ = 34.41^°, 36.10^°, 40.53^°, 42.69^°, 48.61^°, 54.52^°, 60.46^°, 66.48^°, 70.04^° and 72.39^°.

The Fe₃O₄/Talc nanocomposite samples, all diffraction peaks were in agreement with the standard card of Fe₃O₄ (00–072-2303). It is worth noting that the main peak (311) of Fe₃O₄/Talc nanocomposite samples is clearly the characteristic peak of magnetite (Daou et al., 2006). However, all the peak positions at 18.2 (111), 35.4 (311), 57.2 (511) and 62.6 (440) are consistent with the standard X-ray data for the magnetite phase of the Fe₃O₄/Talc nanocomposite. The change in the d spacing of Talc after interaction with Fe₃O₄ nanoparticles is negligible and these signify that the nanoparticles are on the external surface of the Talc (Kalantari et al., 2013). Figure 2 showed that, the original d-spacing (ds) of Talc at 2θ 9.35 degrees was 0.95 nm, which gradually decreased to 0.91 nm at 2θ 9.50 degrees by the formation of Fe₃O₄ nanoparticles on the surface of Talc layers.

Figure 2(b) shows the FT-IR spectra of Talc substrate and Fe₃O₄/Talc nanocomposite samples. There are three obvious peaks at 3633, 3429–34,271,630 cm⁻¹ and 450–669 cm⁻¹ in the spectrum of Talc and the synthesized nanoparticles. The peaks basically represent the vibrations of Mg₃-OH, O-H stretching, H-O-H bending and Mg-O, Si-O-Mg, Si-O, respectively (Kalantari et al., 2013; Li et al., 2015). However, the peak areas of Mg-O bonds (451 cm⁻¹), Si-O-Mg bonds (529 cm⁻¹) and Si-O (669 cm⁻¹) were all decreased in the spectrum of Fe₃O₄/Talc nanocomposite. It is because the ordering and bonding effects were influenced in the layer structure, since some of the Mg-O bonds were broken with radiant energy from the microwave synthesis system, making the binding force weaken in the interlayer. Finally, the Mg⁺ and Si-O⁻ were exhibited [Li S-F et al., 2015]. The peak at 580 cm⁻¹ in the spectrum of Fe₃O₄/Talc nanocomposite was attributed to Fe-O stretch vibrations of nano Fe₃O₄ (Willis et al., 2005), confirming the nature of the iron oxide nanoparticles. These FT-IR and X-ray results imply that the nanoparticles were synthesis successful.

The surface properties, porosity or pore size is one of the factors to evaluate the adsorption capacity of the material. Figure 3 is the FESEM image, BET and VMS of Fe₃O₄/Talc nanocomposite.

Figure 3.

(a) FESEM images of the Talc and Fe₃O₄/Talc nanocomposite; (b) Nitrogen adsorption - desorption isotherms of Fe₃O₄/Talc nanocomposite; (c) M-H curves for Fe₃O₄/Talc nanocomposite.

Figure 3(a) showed the Talc surface material has particle sizes in the range of 30–50 µm, cubic particles are less uniform and have smooth surface. Nanocomposite materials at different magnifications, had distribution of Fe₃O₄ nanoparticles with dimensions less than 30 nm. Then, the synthetic nanocomposite material will give a larger surface area than the base material, which will be shown through the measurement of specific surface area by BET.

Figure 3(b) showed the Fe₃O₄/Talc nanocomposite samples which give adsorption-desorption isotherm of the intermediate form between III and IV with the appearance of H3 hysteresis loop, rod-shaped and letter-shaped according to IUPAC classification (Thommes et al., 2015). This allows the prediction that synthetic nanocomposite materials contain both macropores and mesopores, in which mesopores are more numerous. The pore size distribution obtained from the BJH analysis, the BJH curve shows narrow and intensity peaks in the pore size distribution curve. The hole size distribution curve shows that appear in a range 1 to 150 nm. The specific surface area of talc surface material is 3.45 m².g⁻¹ which is much smaller than that of the nanocomposite material, which reaches 77.92 m².g⁻¹. In particular, macropore area of the nanocomposite S_macro = S_BET – S_BJH,ads – S_micro = 8.27 m².g⁻¹; the pore diameter averages 11.8 nm. A similar types of Fe₃O₄ nanocomposite were also reported by some other workers (Chávez-Guajardo et al., 2015; Cui et al., 2015).

The magnetic properties of materials are assessed by the method of vibrating-sample magnetometry. The results of saturation magnetization of Fe₃O₄/Talc nanocomposite was 38.06 emu.g⁻¹, this indicates that the survey sample is superparamagnetic, the iron oxide particles are distributed with nano size on the soluble surface. Therefore, the material is convenient to separate from the aqueous solution after adsorption with the help of external magnetic fields (Lv et al., 2014).

Adsorption studies

Effect of pH: One of the most influential factors on Cr(VI) removal is the pH of the solution, which influences on the properties of the adsorption process. In this experiment, the initial of Cr(VI) was 10 and 20 mg.l⁻¹; the initial pH values of the adsorption solution were adjusted in the range of 4 to 9; the contact time was 60 min. The amount of Cr(VI) adsorbed depends on the distribution of Cr₂O₇²⁻, HCrO₄⁻ and CrO₄²⁻ which are controlled by pH of the solution. In acidic medium, Cr(VI) exists in the form of oxyanions such as HCrO₄⁻ (pK_a 0.8), Cr₂O₇²⁻ (pK_a 1.52), CrO₄²⁻ (pK_a 6.5). The lowering of pH causes the surface of the adsorbent to be protonated to a higher extent, a strong attraction exists between these oxyanions of Cr(VI) and the positively charged surface of the adsorbent (Dubey and Gopal, 2007; Gupta et al., 2010). Hence, the uptake increases with increasing pH from 4.0 to 6.0 of the solution. At high pH, there will be abundance of negatively charged hydroxyl ions in aqueous solution, causing hindrance between negatively charged ions Cr₂O₇²⁻, CrO₄²⁻,… and negatively charged adsorbent, resulting in a decrease of adsorption (Dubey and Gopal, 2007; Gupta et al., 2010). However, the survey process was carried out from pH = 4 to pH = 9 because, at points of pH less than 4, the dissolution of Fe₃O₄ nanoparticles occurs (Iram et al., 2010). Figure 4 describes the effect of pH on the adsorption of Cr(VI) on the Fe₃O₄/Talc nanocomposite at 303 K. Figure 4 showed equilibrium chromium sorption which was suitable by acidic of 4.0–5.5.

Figure 4.

Effect of pH (adsorbent dosage = 0.1 g/100 ml; [Cr(VI)] = 10 and 20 mg/l; t = 60 min; agitation 120 rpm).

Effect of contact time: Figure 5 shows the comparative data of the effect of contact time on the extent of adsorption of Cr(VI) on the Fe₃O₄/Talc nanocomposite at 10, 15, 20 and 25 mg.l⁻¹ initial chromium concentration at pH 5.0 and temperature 303 K. It has been observed that the metal adsorption rate is high at the beginning and then increases slowly till saturation levels were completely reached at the equilibration point of 60 minutes. In the study, the data were further used to successfully evaluate the kinetics of the adsorption process.

Figure 5.

Effect of contact time (adsorbent dosage = 0.1 g/10 ml; pH = 5.0; agitation 120 rpm).

Effect of sorbent dosage: In this study, to determine the effect of adsorbent dosage, different amounts from 0.05 to 5 g.l⁻¹ of adsorbent were suspended in 50 ml chromium solution and at pH 5.0, 303 K. The effects of adsorbent dosage on the amount of Cr(VI) adsorbed and extent of removal Cr(VI) for the adsorbent are shown in Figure 6. Figure 6 showed that, the extent of Cr(VI) removal was be 24% for 0.5 g.l⁻¹ of adsorbent and 68% for 2 g.l⁻¹ of adsorbent. However, it has been observed that there was only a slow change in the extent of Cr(VI) adsorption for Fe₃O₄/Talc nanocomposite, when the adsorbent dose was over 2 g.l⁻¹. At a low dose, all types of sites are entirely exposed and the adsorption on the surface is saturated faster, showing a higher capacity adsorption value. At a higher adsorbent dose, the availability of higher energy sites decreases with a larger fraction of lower energy sites occupied, resulting in a lower capacity adsorption value. Thus, all the experiment was selected 2 g.l⁻¹ as sorbent dosage.

Figure 6.

Effect of adsorbent dosage ([Cr(VI)] = 10 mg/l; t = 60 min; agitation 120 rpm, pH = 5.0, T = 303 K).

Effect of Cr(VI) concentration: In this study, to determine the effect of Cr(VI) concentration, different initial of Cr(VI) from 10 to 30 g.l⁻¹ of solution adsorption at pH 5.0 and temperature 303 K. The effects of Cr(VI) concentration on the amount of Cr(VI) adsorbed and extent of removal Cr(VI) for the adsorbent are shown in Figure 7.

Figure 7.

Effect of Cr(VI) concentration (t = 60 min; agitation 120 rpm, pH = 5.0, T = 303 K).

Figure 7 showed that, the q_e increases from 4.45 to 7.17 mg.g⁻¹ and removal efficiency decreases from 89.13 to 47.86%, respectively Cr(VI) initial concentration increases from 10 to 30 mg.l⁻¹. When, higher initial concentrations, the active sites of prepared adsorbent would be surrounded with more Cr(VI) ions in the solution, the equilibrium adsorption capacity of Fe₃O₄/Talc nanocomposite increases with the increase of the Cr(VI) ion concentration which enhances the adsorption process. In addition, the removal percentage decreases by the increase in metal initial concentration. At low initial concentrations, the ratio of initial number of chromium ions to the accessible active sites of adsorbent is low; therefore, the removal efficiency of Cr(VI) is higher and at higher concentrations, further residual Cr(VI) ions remain in the aqueous solution (Radnia et al., 2012; Aydın et al., 2008).

Adsorption isotherm modeling

To understand the adsorption mechanism and surface characteristics of the Fe₃O₄/Talc nanocomposite, the mathematical models developed by Langmuir and Freundlich have been applied to the data. The linear equations of Langmuir and Freundlich isotherm models can be described as equation (3) (Ossman et al., 2014).

\frac{C_{e}}{q_{e}} = \frac{1}{q_{\max .} K_{L}} + \frac{C_{e}}{q_{\max}}

(3)where C_e is the concentration of Cr (VI) ion (mg/L) at equilibrium, q_max is the monolayer capacity of the adsorbent (mg/g) and K_L is the Langmuir sorption constant (L/mg). The plot of C_e/q_e versus C_e was given as a straight line (Figure 8) and the values of q_max and K_L can be calculated from the slope and intercept of the plot.

\log q_{e} = \log K_{F} + \frac{1}{n} \log C_{e}

(4)

Where C_e is the equilibrium concentration (mg/L), K_F is a roughly indicator of the adsorption capacity and n is an empirical parameter. The plot of the log q_e versus log C_e gives a straight line (Figure 8) and K_F and n values are calculated from the intercept and slope of this straight line.

Figure 8.

Langmuir isotherm and Fruendlich isotherm (adsorbent dosage = 0.1 g/100 ml; pH 5.0; t = 60 min; agitation 120 rpm).

The related values of parameters and constants for these isotherms are presented in Table 1. The values of regression coefficient obtained from these models were used as the fitting criteria to find out these isotherms.

Table 1.

Langmuir and Freudlich isotherm constants for the adsorption of Cr(VI) on Fe₃O₄/Talc nanocomposit at different temperatures and pH 5.0.

Temperature (K)	Langmuir isotherm				Freundlich isotherm
Temperature (K)	R²	K_L	q_max	R_L	R²	K_F	n
293 K	0.9958	0.81	7.17	0.10–0.25	0.9933	1.99	6.05
303 K	0.9907	0.30	7.47	0.04–0.11	0.9782	4.39	5.93
313 K	0.9740	0.05	35.84	0.33–0.67	0.9902	3.77	1.28

Table 1 showed both plots depiced the linearized form of the isotherms at all temperatures and extremely high correlation coefficients (R² = 0.97 to 0.99), thus indicating both monolayer and heterogeneous surface conditions. Also, from the Langmuir adsorption constant q_e, the adsorption capacity of Cr(VI) on Fe₃O₄/Talc nanocomposite was observed as 7.17, 7.47 to 35.84 mg.g⁻¹ with the rise in temperature from 293, 303 to 313 K, respectively. This result also showed that the value of R_L, and the separation factor fell in the range of 0 to 1 which clearly showed that the adsorption process is favorable. Freundlich constant also varied from 1 to 10 which again proved that the adsorption is favorable. At pH = 5, the existence of Cr(VI) in solution was HCrO₄⁻ (Dubey and Gopal, 2007; Gupta et al., 2010). So, the formation and mechanism for the adsorption of Cr(VI) onto Fe₃O₄/Talc nanocomposite was described at Figure 9.

Figure 9.

Illustration of the prepared Fe₃O₄/Talc nanocomposite and mechanism for the adsorption of Cr(VI) onto Fe₃O₄/Talc nanocomposite.

Table 2 compares maxium adsorption capacities and rate of removal obtained in this study with some other values reported in the article The adsorption capacity for Cr(VI) using Fe₃O₄/Talc nanocomposite, a low-cost adsorbent from the ferilizer industry. The adsorption capacity for Cr(VI) of Fe₃O₄/Talc nanocomposite is of the same order of magnitude has been found using similar adsorbents.

Table 2.

Removal rate/adsorption capacity of heavy metal ions onto various adsorbents.

Adsorbent	Optimum pH	Adsorbate removal rate/maximum adsorption capacity	References
Ag-groundnut husk carbon	3.0	96.6 % initial Cr(VI) concentration 100 mg.l⁻¹; 11.4 mg.g⁻¹	(Dubey and Gopal, 2007)
Groundnut husk carbon	3.0	89.7 % initial Cr(VI) concentration 100 mg.l⁻¹; 11.4 mg.g⁻¹	(Dubey and Gopal, 2007)
Carbon slurry	2.0	65.0 % initial Cr(VI) concentration 100 mg.l⁻¹; 15.24 mg.g⁻¹	(Gupta et al., 2010)
Waste pomace of olive oil factory (WPOOF)	2.0	30.37% initial Cr(VI) concentration 200 mg.l⁻¹; 12.15 mg.g⁻¹	(Malkoc et al., 2006)
Nanoscale zero-valen iron (nZVI)/Fe₃O₄-graphene (nZVI@MG)	3.0	83.8 % (nZVI@MG); 18.0 % (nZVI); 21.6 % (Fe₃O₄ NPs); 23.7 % (Graphene) initial Cr(VI) concentration 100 mg.l⁻¹; 101.0 mg.g⁻¹ (nZVI@MG)	(Lv et al., 2014)
Nanoscale zero-valen iron (nZVI)/Fe₃O₄-graphene (nZVI@MG)	8.0	66.2 mg.g⁻¹ (nZVI@MG)	(Lv et al., 2014)
Talc powder	4.0	77.0 % initial Cr(VI) concentration 3000 mg.l⁻¹26.5 mg.g⁻¹ (318 K)	(Ossman et al., 2014)
ZnO/Talc nanocomposie	5.0	92.87 % initial Cr(VI) concentration 100 mg.l⁻¹48.3 mg.g⁻¹	(Sani et al., 2016)
Fe₃O₄/Talc nanocomposie	Neutral	72.15 % initial Cu²⁺ concentration 100 mg.l⁻¹; 21.05 mg.g⁻¹ (298 K) 50.23 % initial Ni²⁺ concentration 92 mg.l⁻¹; 33.33 mg.g⁻¹ (298 K) 91.35 % initial Pb²⁺ concentration 270 mg.l⁻¹; 74.62 mg.g⁻¹ (298 K)	(Kalantari et al., 2014)

Adsorption kinetics

Kinetics of the adsorption process is studied based on the pseudo-first-order adsorption kinetics equation (B1) in linear form:

\ln (q_{e} - q_{t}) = \ln (q_{e}) - k_{1} . t

(5)where: k₁ (min⁻¹) is the rate constant of the pseudo-first-order adsorption kinetics process; q_e, q_t (mg/g) are the adsorption capacities at the equilibrium time and time t. The pseudo-second-order adsorption kinetics equation in linear form:

\frac{t}{q_{t}} = \frac{t}{q_{e}} + \frac{1}{k_{2} \cdot q_{e}^{2}}

(6)

Where: k₂ (mg/g.min) is the rate constant of the adsorption kinetics process (Ho, 1995; Yuh-Shan, 2004). Intraparticle diffusion kinetic equation:

\ln (q_{t}) = \ln (k_{D}) + 0.5 . \ln (t)

(7)where: k_D (mg/g.(min)^0.5) is the diffusion coefficient (Ge and Li, 2011). Elovich equation:

q_{t} = \frac{1}{β} l n (α β) + \frac{1}{β} l n (t)

(8)where: α and β are constants of Elovich – type equation (Thajeel, 2013). The adsorption rate constant k₁, k₂, k_D, α, β for Cr(VI) was calculated from the slope of the linear plot of ln(q_e – q_t) versus time, plot between t/q_t against t, and plot of ln(q_t) versus ln(t), plot between q_t against ln(t) as shown in Figure 10. The kinetic rate constants obtained form pseudo-first- and -second-order, diffusion kinetic, elovich equations are given in Table 3.

Figure 10.

The kinetic models of adsorption of Cr(VI) ion on the Fe₃O₄/Talc nanocomposite (adsorbent dosage = 0.1 g/100 ml; pH 5.0; T = 303 K; agitation 120 rpm).

Table 3.

Kinetic parameters for the removal of Cr(VI) onto Fe₃O₄/Talc nanocomposite.

Co (ppm)	Pseudo 1st order				Pseudo 2st order
Co (ppm)	Equation	R²	k₁	Equation	R²	q_e	k₂
10	y = −0.045x + 0.2258	0.9645	0.045	y = 0.2098x + 0.6027	0.9998	4.7664	0.0730
15	y = −0.0162x + 0.3588	0.9309	0.0162	y = 0.1854x + 0.4481	0.9998	5.3937	0.0767
20	y = −0.0204x + 0.2564	0.9133	0.0204	y = 0.1627x + 0.3348	0.9995	6.1463	0.0790
25	y = −0.0964x + 0.9165	0.9625	0.0964	y = 0.1447x + 0.3087	0.9996	6.9108	0.0678
	Intraparticle diffusion model				Elovich model
Co (ppm)	Equation	R²	k_D	Equation	R²	α	β
10	y = 0.116x + 1.0573	0.9004	2.8785	y = 0.4758x + 2.6649	0.9153	128.78	2.1017
15	y = 0.0881x + 1.2939	0.9716	3.6470	y = 0.0881x + 1.2939	0.9716	210541.3	11.3507
20	y = 0.0756x + 1.48	0.9552	4.3929	y = 0.4218x + 4.2522	0.9561	10075.45	2.3708
25	y = 0.0885x + 1.549	0.9177	4.7068	y = 0.5486x + 4.5037	0.9193	2016.37	1.8228

Table 3 showed the values of correlation coefficient R² for the Pseudo-second-order adsorption model which is relatively high (R² > 0.999), furthermore, the values of the k constant are almost unchanged, which indicates that the speed constant does not depend on concentration. This proves that the adsorption process depends on the number of adsorption centers on the surface and the adsorbate is the Cr(VI) ion.

Thermodynamic study

In this study, the thermodynamics of adsorption of Cr(VI) onto Fe₃O₄/Talc nanocomposite, thermodynamic constants such as: enthalpy change ΔH^o, free energy change ΔG^o and entropy change ΔS can be related to the Langmuir isotherm constant by the following equations (Gupta et al., 2004).

{Δ G}^{o} = - RT \ln (K_{L})

(9)

\ln (K_{L}) = \frac{{Δ S}^{o}}{R} - \frac{{Δ H}^{o}}{R . T}

(10)

Thus, a plot of ln(K_L) versus 1/T should be a straight line. ΔH^o and ΔS^o values could be obtained from the slope and intercept of this plot. The values of these parameters are given in Table 4. Figure 11 show thermodynamic data of adsorption of Cr(VI) onto Fe₃O₄/Talc nanocomposite.

Table 4.

Thermodynamic parameters for the adsorption of Cr(VI) on Fe₃O₄/Talc nanocomposite at different temperatures.

Temperature (K)	${Δ G}^{o} (kJ / mol)$	${Δ S}^{o} (kJ / mol . K$ )	${Δ H}^{o} (kJ / mol)$ ^a
293	0.478
303	3.033	–0.362	–105.804
313	7.796

^aMeasured between 293 K and 303 K.

Figure 11.

Thermodynamic analysis (adsorbent dosage = 0.1 g/100 ml; pH 5.0; t = 60 minutes; agitation 120 rpm).

Table 4 showed that the values of ${Δ H}^{o} (- 105.804 k J / mol)$ is negative. And it also indicate that the adsorption is the process of chemical adsorption and the process is exothermic. The negative values of ${Δ S}^{o} (- 0.362 k J / mol)$ indicate that there is a decrease in the degree of freedom of the adsorbed. The positive ${Δ G}^{o}$ value corresponds, showed that the instability activation complex of the adsorption reaction is increased with increasing temperature (Zhang et al., 2012).

Conclusion

The Fe₃O₄/Talc nanocomposite was synthesized with the Talcum powder Phu Tho – Viet Nam by the coprecipitation-ultrasonication method. X-ray, FTIR, FESEM, BET and VSM analyses were performed for characterizing the synthesized nanocomposite. The surface area of the nanoparticles was determined to be 77.92 m².g⁻¹ with an average diameter of 11.8 nm and the saturation magnetization of 38.06 emu.g⁻¹. The peak positions at 18.2 (111), 35.4 (311), 57.2 (511) and 62.6 (440) are consistent with the standard X-ray data for the magnetite phase of the Fe₃O₄/Talc nanocomposite. The original d-spacing (ds) of talc at 2θ 9.35 degrees was 0.95 nm, and 0.91 nm at 2θ 9.50 degrees by the formation of Fe₃O₄ nanoparticles on the surface of Talc layers. The peak at 580 cm⁻¹ in the spectrum of Fe₃O₄/Talc nanocomposite was attributed to Fe-O stretch vibrations, confirming the nature of the iron oxide nanoparticles. These FT-IR and X-ray results imply that the nanoparticles were synthesis successful.

The batch studies experimental results indicate that the Fe₃O₄/Talc nanocomposite is an effective adsorbent of Cr(VI) ion from the aqueous solution. The adsorption equilibrium data fitted very well to the Langmuir and Freundlich adsorption isotherm models. The kinetic data showed that the adsorption process followed the pseudo-second order kinetic model. The maximum adsorption capacities of 35.84 mg/g occurred at pH 5.0 and 313 K, with adsortion dosage is 2 g.l⁻¹. The adsorption is the process of chemical and exothermic. These results permit us to conclude that Fe₃O₄/Talc nanocomposite is a promising low-cost adsorbent for Cr(VI) removal from wastewater and can be applied in a magnetically-assisted water treatment technology.

Footnotes

Declaration of Conflicting Interests

The author(s) declared no potential conflicts of interest with respect to the research, authorship, and/or publication of this article.

Funding

The author(s) received no financial support for the research, authorship, and/or publication of this article.

ORCID iDs

Nguyen Thi Huong

Nguyen Ngoc Son

Cong Tien Dung

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Synthesis Fe 3 O 4 /Talc nanocomposite by coprecipition-ultrasonication method and advances in hexavalent chromium removal from aqueous solution

Abstract

Keywords

Introduction

Materials and methods

Materials

Synthesis of Fe3O4/Talc nanocomposite

Batch adsorption procedure

Analysis of Cr(VI) ions

Results and discussion

Characterization of Fe3O4/Talc nanocomposite

Adsorption studies

Adsorption isotherm modeling

Adsorption kinetics

Thermodynamic study

Conclusion

Footnotes

Declaration of Conflicting Interests

Funding

ORCID iDs

References

Synthesis of Fe₃O₄/Talc nanocomposite

Characterization of Fe₃O₄/Talc nanocomposite