Study of the Adsorption of Arsenic (III and V) by Magnetite Nanoparticles Synthetized via AACVD

Abstract

Globally, water pollution is mainly caused by the presence of heavy metals and metalloids such as arsenic. The majority of the techniques employed in the removal are of low efficiency and high cost. Therefore, in this work it is presented the adsorption processes of arsenic (As III and V) ions employing magnetite nanoparticles (MNPs) synthesized by the aerosol assisted chemical vapor deposition (AACVD) process. The adsorption efficiency was determined at different times and concentrations. The remaining As concentration in the solutions was analyzed by atomic absorption spectroscopy. The adsorbed As ions on the surface of the NMPs was analyzed by high resolution transmission electron microscopy. The results showed an overall removal efficiency of 87% for As⁺³ and 98% for As⁺⁵, in a contact time of 15 minutes. Results suggested the use of NMPs as a promising alternative in the removal of As ions in water.

Keywords:
AACVD; MNPs; adsorption isotherms; physisorption process

1. Introduction

Heavy metals such as lead¹, mercury¹, cadmium², chromium³, nickel⁴ and arsenic metalloid⁵, are found naturally in the earth's crust; eventually these heavy metals can become contaminants in the air, surface water, groundwater, soil and other aquatic environments. In recent decades, the aquatic environment has been exposed to a large contamination mainly caused by the continuous discharges of pollutants containing heavy metals produced from anthropogenic sources². When these metals reach the food chain, generate a high health risk for the living beings and humanity, because they can accumulate in living tissues causing various disorders and diseases as skin diseases, kidney cancer and even incomplete embryonic development during pregnancy^6,7. Thus, for this reason, most of the health agencies in the world have decided to reduce the maximum concentration of these toxic ions established in the international norms.In the case of arsenic, it is present in large quantities of groundwater and effluents worldwide, with an allowed maximum limit⁸ of 0.01 mg L^-1. In natural water bodies, As is found as hydrogen arsenate (H₃AsO₄) and arsenic acid (H₃AsO₃), which at oxidizing or reducing conditions produce As⁺⁵ and As⁺³ ions, respectively⁹. From these ions, As⁺³ is more toxic. The mobility and bioavailability of these ions largely depend on the adsorption/desorption process of As within the soil and the pH conditions in groundwater^10,11. The treatment techniques include methodologies such as oxidation, precipitation and co-precipitation^12,13, inverse osmosis¹⁴, and ion exchange¹⁵. These techniques employ solid adsorbents particles for immobilizing the As ions such as alumina, mineral oxides, active carbon, polymer resins and zeolites¹⁶. Additionally, when both As ions are presented in the water fluent, the removal process becomes more complex, since As⁺³ must be first oxidized into As⁺⁵. Clearly, this increases the overall cost for decontamination of water. Thus, there is a growing interest in the development of low cost methodologies for water treatment, especially for As ions. Consequently, in recent years several adsorbents based on nanometric-scale oxides have been synthesized and tested (TiO₂, Fe₂O₃, Fe₃O₄)^17-21. Among these oxides, iron oxides have been widely employed due to its high efficiency caused by the strong affinity between the As and Fe at mild conditions of room temperature and pH^22,23. Therefore, in this work were studied the equilibrium and kinetics of the adsorption process of arsenic ions on magnetite hollow nanoparticles (MNPs). The equilibrium study will provide relevant information related with the affinity between the adsorbate and adsorbent. The kinetics study will contribute with data associated with the time and concentration required to perform the removal process²⁴. The experimental data was fitted with different kinetic models in order to set if the process was driven by physisorption or chemisorption. Additionally, several thermodynamic parameters such as the adsorption energy and Gibbs free energy were calculated.

2. Experimental procedure

2.1. Synthesis and MNPs characterization

The MNPs were synthesized by the AACVD technique, details of the technique have been previously reported elsewhere^25-27. Briefly, AACVD consists of an ultrasonic nebulizer, where the precursor solution is converted into a fine aerosol. The aerosol is transported into de furnace by the carrying gas. Once inside the furnace, the precursor solution contained in the aerosol is decomposed by effect of the thermal energy into the oxide, forming in it a fine powder on the walls of the tubular furnace. The precursor solution was a dilution of Fe (II) chloride in methanol (99.9%), at a concentration of 0.05 mol L^-1. The aerosol was carried by a mixture of Ar-air flow, (relation of 0.250:0.004 L min^-1, respectively). Synthesis temperature was fixed at 723 K. A collection flask was placed on super magnets with the function of attracting and collecting the MNPs obtained.

The microstructure of the pure MNPs and the MNPs-As was analyzed in two field emission microscopes, a scanning electron microscope (SEM) JEOL JSM-7401F and in a high resolution transmission electron microscope (HRTEM) JEOL JEM-2200FS. The elemental analysis was carried out by energy dispersive x-ray spectroscopy (EDS) attached to the column of the microscope. The EDS employed was an Inca from Oxford Instruments. Sample preparation consisted in dispersing the MNPs in ethanol and mixing under sonic conditions by 5 minutes. One drop of the solution was deposited on a Holey-Carbon Cu grid. Excess of ethanol was removed by drying under a visible light lamp. Prior to the introduction in the column the Cu-grid was cleaned with Plasma by 10 seconds.

MNPs-As were prepared as follows: first a solution of 500 ppm of arsenic in 100 ml of tridistilled water was prepared. Subsequently, 10 mg of MNPs were added to the solution and placed in ultrasonic agitation for 10 minutes. Once the time was elapsed, the solution was subjected to centrifugation at 5000 rpm by 15 minutes. Then the solution was decanted and separated from the collected MNPs-As. For the SEM analysis, the particles were dispersed in methanol by ultrasound for 1 minute, then three drops of the solution were deposited on a silicon substrate with an approximate area of 0.5 cm², and the substrate was allowed to dry. In this case, an elemental mapping for arsenic detection was performed on the MNPs-As. The specific surface area of MNPs was analyzed by the BET method before and after the contact with the arsenic to determine the amount of specific surface area being occupied by the ions of arsenic after the adsorption process.

2.2. Arsenic removal test

The arsenic ions precursors (99% purity, JT Baker) used in the preparation of solutions were sodium arsenite (NaAsO₂) and sodium arsenate dibasic heptahydrate (Na₂HAsO₄ ^.7H₂O), for the As⁺³ and As⁺⁵, respectively. Two dilute solutions for each ion were prepared as: As⁺³ 0.152 and 0.164 mg L^-1, and As⁺⁵ 0.033 and 0.066 mg L^-1. To each of the dilute solutions were added 10 mg of MNPs and then left in contact under ultrasonic agitation. The contact times were 1, 5, 10, 15 and 30 minutes. After elapsed this time, in order to separating the MNPs from the liquid, the solutions were centrifuged at 5000 RPM by 10 minutes. Each clear solution was analyzed by atomic absorption spectroscopy (AAS, Avanta Sigma, GBC Scientific Equipment Ltd.) for determining the As and Fe content. The removal efficiency was calculated with equation (1), where C₀ is the initial As concentration in the solution prior to the contact test, and C_f is the As concentration determined from the AAS characterization:

(1) $\mathit{Removal}\mathit{efficiency}\left(\%\right)=\left[\left({\mathit{C}}_0-{\mathit{C}}_{\mathit{f}}\right)/{\mathit{C}}_0\right]\times 100$

2.3. Equilibrium study

2.3.1. Adsorption capacity

The adsorption capacity (q_e) was calculated from a mass balance according to equation (2), where C_o was the initial As concentration in the solution (mg L^-1), C_e the As concentration in the equilibrium (mg L^-1), V the volume of the solution (L) and M the mass of the MNPs (g).

(2) ${\mathit{q}}_{\mathit{e}}=\left[\mathit{V}*\left({\mathit{C}}_0-{\mathit{C}}_{\mathit{e}}\right)\right]/M$

2.3.2. Adsorption isotherms

The equilibrium adsorption isotherms provide useful information about the interactions between the adsorbate and the adsorbent. From this type of curves it was possible to determine the thermodynamic parameters and the maximum adsorption capacity. Several fitting models were tested (Langmuir²⁸, Freundlich²⁹ and Dubinin³⁰) in order to find the best adjustment between the experimental data and the theoretical behavior. The models and the corresponding parameters are depicted in Table 1.

Table 1
Models and parameters employed for fitting the adsorption isotherms in the equilibrium.

Isotherm	General Equation	Linearized equation	Parameters	Description
Langmuir	${\mathit{q}}_{\mathit{e}}=\frac{{\mathit{Q}}_0{\mathit{K}}_{\mathit{L}}{\mathit{C}}_{\mathit{e}}}{{\mathit{C}}_{\mathit{e}}{\mathit{K}}_{\mathit{L}}+1}$	$\frac{{\mathit{C}}_{\mathit{e}}}{{\mathit{q}}_{\mathit{e}}}=\frac{{\mathit{C}}_{\mathit{e}}}{{\mathit{Q}}_0}+\frac{1}{{\mathit{K}}_{\mathit{L}}{\mathit{Q}}_0}$	Q0	Maximum adsorption capacity
			KL	Constant Langmuir (Adsorption energy)
			Ce	Equilibrium concentration of the As
			qe	Equilibrium adsorption capacity of adsorbent
Freundlich	${\mathit{q}}_{\mathit{e}}={\mathit{Q}}_0\mathit{C}_{\mathit{e}}{}^{\frac{1}{{\mathit{K}}_{\mathit{F}}}}$	$\ln \left({\mathit{q}}_{\mathit{e}}\right)=\ln \left({\mathit{Q}}_0\right)+\frac{1}{{\mathit{K}}_{\mathit{F}}}\ln \left({\mathit{C}}_{\mathit{e}}\right)$	Q0	Maximum adsorption capacity
			KF	Constant Freundlich (Adsorption energy)
			Ce	Equilibrium concentration of the solution
Dubinin			Q0	Maximum adsorption capacity
			KD	Free energy of the adsorption per molecule
	${\mathit{q}}_{\mathit{e}}={\mathit{Q}}_0{\mathit{e}}^{\mathit{k}{\epsilon }^2}$	$\ln \left({\mathit{q}}_{\mathit{e}}\right)=\ln \left({\mathit{Q}}_0\right)-{\mathit{K}}_{\mathit{D}}{\epsilon }^2$	qe	Equilibrium adsorption capacity of adsorbent
		$\epsilon =\mathit{RT}\ln \left(1+\frac{1}{{\mathit{C}}_{\mathit{e}}}\right)$	R	Universal gas constant
			Ɛ	Polanyi potential
			T	Ambient Temperature

2.4. Adsorption process thermodynamics

2.4.1. Adsorption energy

The adsorption free energy (E) was determined to according to equation (3) and it represents the energy change required for transferring one mole of As ions from the solution onto the surface of the solid. If E is lower than 20 kJ mol^-1 the adsorption process is called physisorption, if it is between 20-40 kJ mol^-1 the process is known as ionic exchange, and when E is larger than 40 kJ mol^-1 it is a chemisorption process. The Gibbs free energy (ΔG) indicates the energy required to displace the adsorbate onto the surface of the adsorbent³¹ and was calculated according to equation (4).

(3) $\mathit{E}=\frac{1}{\sqrt{2{\mathit{K}}_{\mathit{D}}}}$

(4) $\Delta \mathit{G}=\mathit{RT}\mathit{Ln}\frac{1}{{\mathit{K}}_{\mathit{L}}}$

where K_D is the Dubinin constant, K_L is Langmuir constant, R is the universal gas constant (8.314 J mol^-1 K^-1) and T is absolute temperature.

3. Results and discussion

3.1. Microstructure of the MNPS

Figure 1 (a-b) shows SEM micrographs of the MNPs synthesized by the AACVD method.

Figure 1
SEM images showing a) the morphology of the MNPs before arsenic adsorption process. b) Morphology of MNPs after the arsenic adsorption process.

We can see particles with spherical morphology, each sphere is composed of crystallites, these particles tend to agglomerate, due to its size it is nanostructured. Two effects are observed when the size is reduced to nanostructured scale: a) a significant increase in surface area relative; b) a significant number of atoms on the surface increase. These effects increase the chemical reactivity of the surface of nanoparticles; this chemical reactivity and other properties depend on many factors: size, shape, chemical composition, electronic structure, surface structure, defects, diffusion, surface energy of the nanocrystals, interactions with atoms that are near and its chemical environment. The atoms on the surface of the nanoparticles are unstable, have a higher energy level and forces that are attracted by the atoms located inside the mass are very weak⁵³. Therefore, by reducing the size at the nanoscale, the forces of Van der Waals attraction and its magnetic nature^25-27 of the nanostructures, increase and the spheres tend to attract each other and to form agglomerates. Most of the spherical particles consisted of crystallites with nanometric size, which formed the surface of the hollow sphere. The average particle size of the spherical particle was 300 ± 78 nm. Once analyzed, the MNPs were added to the arsenic solution and the results obtained by SEM show any change in the morphology of the nanoparticles (It is called nanoparticle because the sphere is formed of crystallites with size average of 20 nm, this means that the requirement of having at least 100 nm in size in one dimension is fulfilled, therefore, it can be mentioned as nanoparticle) after the adsorption of arsenic (Figure 1b). Figure 2 (a-b) shows a micrograph obtained by HRTEM of a single MNP and the corresponding elemental mapping determined by EDS . In Figure 2b the white dots forming the image of the particle indicated the presence of arsenic. It was observed a homogeneous distribution of the As adsorbed on the MNPs. With this, the adsorption of As by the MNPs was confirmed. However, the As was preferentially adsorbed on the crust of the particle rather than in the bulk. Figure 3 shows the EDS analysis performed on several of the MNPs. As expected, the quantification of the elements showed the presence of a high concentration of Fe and O, originated from the MNPs. The C, Si and Cu detected were originated from the elements conforming the support where the MNPs were deposited. The relatively low concentration of As was evidently produced by the adsorption of the ions on the surface of MNPs. Figure 4 shows the micrograph obtained by HRTEM and the corresponding line scan of elementes (Fe, O and As) determiend by EDS. With the line scans it was possible to determine the overall As distribution on the surface of a single MNP. These results suggested that most of the crystals forming the MNP contributed in the adsorption process, attraping several As ions^32,33.

Figure 2
HRTEM image from a single MNP and Elemental mapping of a single MNPs. The scattered white dots indicate the distribution of the As ions on the MNPs.

Figure 3
EDS analyses from the MNPs synthesized by the AACVD method, after the contact tests with As ions (As⁺³ y As⁺⁵⁾.

Figure 4
Scanning line by HRTEM, indicates the elemental distribution of As, O and Fe in MNPs.

3.2. Surface area measurements

The surface area calculated for MNPs before and after the adsorption process was 92 and 84 m²/g respectively. The difference between these two measurements (8.7%) indicated that this value was the surface area occupied by arsenic. It is evident that the adsorption capacity depends largely on the specific surface area of the adsorbent and the affinity between the adsorbate and adsorbent. Altough the adsorbed As covered only a 8.7% of the surface of the particles, there still a large surface area where As ions may be adsorbed. This indicates the existence of free active sites for adsorbing more As ions i.e. in a continuos adsorption process.

3.3. Effect of contact time and solution concentration

Figure 5 shows the plots of the removal efficiency against the contact time of As ions (As⁺⁵ and As⁺³) solutions at the different concentration. The curves showed a similar adsorption behavior. At early stages of the contact time, there was a high adsorption rate of As on the MNPs, which was caused by the large amount of available sites for As adsorption³⁴. As the contact time elapsed, the active sites are being saturated with more As ions; this was observed as the decrease in the adsorption rate until the adsorption equilibrium is reached³⁵. For the systems studied in this work, the equilibrum was attached after 15 minutes of contact time. These results were similar to those previously reported by Naushad et al.^2,36 who found that the rate of adsorption was higher in the early stages of the removal process and then tend to decrease when the process reached the state of equilibrium. Table 2 shows the calculated removal efficiency (%) of As ions. As observed, for As⁺⁵ ions after 10 minutes of contact time it was reached an efficiency of 95%, while As⁺³ ions after 15 minutes of contact time reached only 87%. These efficiency values were of importance since at these levels it was fulfilled the maximun concentration of As in water allowed in the international health standards. After 30 minutes of contact time As⁺⁵ ions were fully removed from the solution, while As⁺³ ions were removed only at 90%. Clearly, these suggested differences in the adsorption mechanism between the As⁺⁵ and As⁺³ ions. Commonly, prior to the removal of As⁺³ ions, these must be oxidized into As⁺⁵. However, in the adsorption experiments performed in this work, As⁺³ ions were removed from water at a relative high efficiency without any previous treatment.

Figure 5
The removal efficiency of the As ions at different contact time.

Table 2
Results of the removal of As ions (As⁺³ y As⁺⁵) from water. The initial concentration of As in the solution is indicated in square brackets.

Time (min)	As+5 removal (%) [0.036 mg L-1]	As+5 removal (%) [0.066 mg L-1]	As+3 removal (%) [0.152 mg L-1]	As+3 removal (%) [0.164 mg L-1]
1	64	70	49	54
5	89	91	62	68
10	94	95	73	78
15	96	98	85	87
30	100	100	88	90

The mechanism of adsorption of As ions on FeOH was previoulsy reported by Xu et al.³⁷, Westeroff et al.³⁸ and Eby³⁹, and it was depicted in Figure 6. Results showed that only 10 mg of MNPs were enough to reach those removal eficiencies. The advantages of employing this type of MNPs are the low contact time required to achieve a high removal efficiency^40,41 and the prevention in the generation of residual sludge, which reduce the overall cost of the water treatment process.

Figure 6
Proposed mechanism of arsenic adsorption process by MNPs^37-39

3.4. Adsorption isotherms

Adsorption isotherms were constructed in order to show the adsorption capacity of the MNPs in the equilibrium. Table 3 shows the experimental conditions and the results of the calculated adsorption capacity (q_e). As observed in Table 3, the adsorption capacity increased with the initial concentration of the As solution; this was observed for both of the As ions tested. This behavior was explained in terms of the high mass transfer velocity produced by the larger amount of adsorbate available in the more concentrated solution^3,42,43. Table 4 shows a summary of the results reported in literature of the adsorption capacities obtained with different types of adsorbents^44-46. As can be infered, the adsorption capacity of the adsorbatent depends on the initial concentration of the adsorbeate, and in consequence the saturation point or equilibrium may be shifted in any direction. The experimental data describing the interactons solute-adsorbate was calculated from the fitting of the different models. Table 5 shows the results of the linnear regresion according to the Langmuir model. The monolayer content level (Q₀) represents the mass of ions adsorbed on the MNPs and forming a single monolayer of As ions^47-36. Since in every case, the q_e values is larger than the Q₀, then it was suggested the formation of several layers adsorbed on the initial monolayer. This is a typical performance observed in physisorption processes. The calculated Lagmuir constant (K_L) can be interpred as the enthalpy of adsorption, showed negative values. This suggested the exothermal nature of the process and indicated that the surface of the MNPs was energetically favorable to react with the As ions. Table 6 shows the results of the Freundlich model. According to Mandal S. et al.^48,49, at higher K_F value will be higher the adsorption capacity of the adsorbent. Additionally, a K_F value higher than the unit indicates the spontaneous nature of the process ⁵⁰. In terms of the adsorption capacity, these results agreed with those calculated by the Langmuir model. However, for all the adsorption ishoterms, the regression coeficient (R²) was more reliable for the Freundlich model than for the Langmuir model. Table 7 shows the results obtained after applying the Dubinin model. The regression coefficent was similar to those calculated by the Freundlich model, and the Q₀ value was lower than the q_e value, confirming the formation of several adsorbed layers of As ions during the adsorption process ².

Table 3
Experimental conditions employed in the contact adsorption tests for calculating the adsorption capacity.

	C0 (mg L-1)	V (L) Solution	MNPs (mg)	qe (mg g-1)
As+5	0.036	0.1	0.01	0.355
As+5	0.066	0.1	0.01	0.63
As+3	0.152	0.1	0.01	1.33
As+3	0.164	0.1	0.01	1.38

Table 4
Adsorption capacities of different types adsorbents, with different amounts of adsorbate and adsorbent.

Adsorbent	Initial concentration of adsorbate	Adsorption capacity (mg g-1)	Amount ofAdsorbent utilized
Nickel/nickel boride nanoparticles coated resin 4	100 ppm	23.4 As+3	0.1 g
		17.8 As+5	0.4 g
Fe7S8 nanoparticles5	300 ppb	14.3 As+3	0.01g
		31.3 As+5
Iron oxide Green nanoparticles44	600 ppm	3.77 As+5	2.5 g
MOF-808 nanoparticles45	5 ppm	24.83 As+5	0.01 g
TiO2 nanoparticles46	0.1 ppm	3.1 As+5	0.2 gr
Magnetite nanoparticles (this work)	0.066 ppm	0.63 As+5	0.01 g
	0.134 ppm	1.38 As+3

Table 5
Results from the Langmuir model for the adsorption of As ions (As⁺³ y As⁺⁵) on the MNPs.

	As+5		As+3
	Concentration 0.036 mg L-1	Concentration 0.066 mg L-1	Concentration 0.152 mg L-1	Concentration 0.164 mg L-1
Adsorption capacity of a monolayer Q0 (mg g-1)	0.338	0.623	1.052	1.219
Langmuir constant KL (L mg-1)	-37	-23	-2.4	-1.9
Adsorption capacity qe (mg g-1)	0.35	0.63	1.33	1.38
Regression coefficient R2	0.85	0.91	0.97	0.95

Table 6
Results from the Freundlich model for the adsorption of As ions (As⁺³ y As⁺⁵) on the MNPs.

	As+5		As+3
	Concentration 0.036 mg L-1	Concentration 0.066 mg L-1	Concentration 0.152 mg L-1	Concentration 0.164 mg L-1
Adsorption capacity of a monolayer Q0 (mg g-1)	0.28	0.54	0.610	0.77
Freundlich constant KF (L mg-1)	-32	-36	-5	-6.3
Adsorption capacity qe (mg g-1)	0.35	0.63	1.33	1.38
Regression coefficient R2	0.97	0.96	0.98	0.99

Table 7
Results from the Dubinin model for the adsorption of As ions (As⁺³ y As⁺⁵) on the MNPs.

	As+5		As+3
	Concentration 0.036 mg L-1	Concentration 0.066 mg L-1	Concentration 0.152 mg L-1	Concentration 0.164 mg L-1
Adsorption capacity of a monolayer Q0 (mg g-1)	0.278	0.528	0.439	0.606
Dubinin constant KD (L mg-1)	0.0013	0.0012	0.011	0.0086
Adsorption capacity qe (mg g-1)	0.35	0.63	1.33	1.38
Regression coefficient R2	0.96	0.97	0.99	0.99

3.5. Determination of adsorption energy and Gibbs free energy

Tables 8 and 9 show the results of the adsorption free energy and Gibbs free energy, calculated from the Dubinin and Langmuir constants, respectively. The results indicated that the energy required to transfer one mole of As ions from the solution onto the surface of the adsorbate (MNPs) was very close to 20 kJ mol^-1 for the As⁺⁵ and 7.6 kJ mol^-1 for the As⁺³. These values corroborated that the interactions among the adsorbate and the adsorbent were of the physical type, i.e. physisorption process^51,52. The calculated Gibbs free energy for the both. As ions presented a negative value, indicating the spontaneous nature of the process. Furthermore, as the concentration of the solution decreased, the calculated value of the energies (E and ΔG) was more negative, indicating that the physisorption process was more favorable. These results were similar to those reported by Naushad et al.⁵². Furthermore, when the concentration of the adsorbate in the solution decreased, the calculated value for the energies (E and ΔG) also decreases, indicating that the physisorption process was more favorable.

Table 8
Adsorption free energy for As ions (As⁺⁵ y As⁺³) at different experimental conditions, calculate from the Dubinin model

As ion	Concentration (mg L-1)	Dubinin Constant (mol2 kJ-2)	Adsorption free Energy (kJ mol-1)
As+5	0.036	0.0013	19
As+5	0.066	0.0012	20
As+3	0.152	0.0011	6.7
As+3	0.164	0.0086	7.6

Table 9
Gibbs free energy for As ions (As⁺⁵ y As⁺³) at different experimental conditions, calculate from the Langmuir model

As ion	Concentration (mg L-1)	Langmuir Constant (mol2 kJ-2)	Adsorption free energy (kJ mol-1)
As+5	0.036	37	-8.8
As+5	0.066	23	-7.6
As+3	0.152	2.4	-2.14
As+3	0.164	1.9	-1.57

4. Conclusions

The study presented herein showed that the hollow magnetic nanoparticles (MNPs) can be employed as a promising material in the removal of As ions (As⁺⁵ and As⁺³) from water. The adsorption experiments showed that As ions could be removed with a high efficiency (90%) in a relatively short time (15 minutes). From the high resolution electron microscopy images, it was observed that the As ions were adsorbed and well distributed on the surface of the MNPs. Several physical models were employed to fit the experimental data and the results indicated the formation of several layers of As ions on the MNPs. The calculated adsorption free energy and Gibbs free energy indicated that the adsorption process was conducted by physisorption (E < 20 kJ mol^-1) and spontaneously (ΔG < 0). From the three models fitted (Langmuir, Freundlich and Dubinin), Langmuir showed the lower regression coefficients, but the three models agreed very well in predicting the adsorption capacity.

5. Acknowledgements

Authors thank to S. Miranda, A. Benavidez, P. Peregrino, C. Ornelas, O. Esquivel-Pereyra, A. Heiras-Trevizo, G. Romero-Rubio for the technical assistance provided during the realization of this work. This work was partially supported by a grant from CONACYT PDCPN2014-01 Project 248289.

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Publication Dates

• Publication in this collection
  08 Dec 2016
• Date of issue
  Dec 2016

History

• Received
  04 Nov 2015
• Reviewed
  05 Oct 2016
• Accepted
  21 Nov 2016