# Thermodynamic Studies of the Arsenic Adsorption on Iron Species Generated by Electrocoagulation

Authors: J. R. Parga; V. Vazquez; H. Moreno
Journal: Journal of Metallurgy
 (2009)

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## Abstract

Protection of global environment and sustainable sources of clean water are a necessity for human survival. The wide use of heavy metals by modern industries has generated heavy metals containing wastes and by-products. Specifically, large quantities of arsenic compounds are being discharged into the environment. The full potential of Electrocoagulation (EC) with air injection as an alternative wastewater treatment technique to remove arsenic from water showed more than 99 percent of removal without adding any chemicals. This study has been carried out to determine the feasibility of arsenic adsorption on iron species by EC process using the Langmuir's Isotherm. Thermodynamic parameters such asΔH°, ΔS°, and ΔG° were calculated. It was found that the adsorption process is exothermic and spontaneous. Some experiments were conducted to determine the optimum operating conditions such as current density, pH, and residence time. Also in this study, X-Ray Diffraction, Scanning Electron Microscopy, Mössbauer Spectroscopy, and Fourier Transform infrared spectroscopy were used to characterize the EC solid products that revealed the expected crystalline iron oxides (lepidocrocite, magnetite, gohetite, and iron oxide).


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## Body

## 1. Introduction

Arsenic contaminants are generated from various industries such as steel making, electroplating, leather tanning, and industrial operations that involve the processing of ferrous and nonferrous metals. Some other metal wastes associated with these activities include nickel, lead, cadmium, and mercury. Arsenic contaminated natural waters, including surface water and ground water, are a significant problem as some of these compounds are known to be toxic, mutagenic, and carcinogenic. The deleterious health effects associated with ingestion of arsenic require that its concentrations should be kept below 10.0 ppb in potable water supplies. The metals existing in wastewater are usually removed by precipitation. Other treatments used include coagulation, flocculation, ion exchange, solvent extraction, cementation, adsorption, evaporation, filtration and   electrochemical, biological, and membrane processes [1]. Seventy percent of electroplating facilities use some form of precipitation treatment [2]. Three types of precipitation treatments in these industries, hydroxide, carbonate, and sulfide precipitation [1], take considerable time and require an extensive setup. Each step takes place in a separate tank, and the entire treatment may require several pH adjustments as well as the addition of acid coagulant, lime, and caustic or polymeric flocculants. In addition, the process generates large volumes of sludge/waste, which requires disposal. Hydroxide precipitation is the most commonly used precipitation method due to its relative simplicity, low cost, and automatic pH control [3]. However, most heavy metal hydroxides have similar solubilities; so the most effective pH must be determined prior to treatment when multiple metals are present at high concentrations (e.g., in metal finishing). Furthermore, it may not be possible to remove all metals simultaneously merely by hydroxide precipitation [4].Arsenic is conventionally removed by chemical techniques such as treatment with lime, aluminum coagulation, iron coagulation, and chemical oxidation. Other processes used with varying degrees of success include adsorption onto activated carbon, reverse osmosis, nanofiltration, and ion exchange resins [5]. These conventional processes generate a considerable quantity of secondary pollutants such as solid sludge, which also pose serious environmental problems.The Langmuir isotherm was used to obtain the thermodynamic parameters such as free energy, enthalpy, and entropy. Evaluation of these parameters (ΔG°=-34 kJ/mol, ∆H°=-29 kJ/mol and ∆S°=-0.0181 kJ/molK°) indicates the spontaneous and exothermic nature of the adsorption of arsenic particles on the iron species.


## 2. Remediation Technique

Arsenic removal in the conventional techniques is performed by oxidation of soluble As (Section3) to less soluble As (Section 4) followed by separation of As (Section 5). Techniques like coagulation-precipitation, adsorption, ion exchange, reverse osmosis, electro dialysis, and so forth take advantage of any of the physicochemical properties. The conversion of As (Section 3) to As (Section 5) is done by using some oxidizing agents like chlorine, potassium permanganate, and so forth. Addition of chemicals in the oxidation step increases the cost of these techniques [6, 7]. These physicochemical techniques can be classified as shown in Table 1.Table 1
Comparison of conventional processes for as removal [12, 13].
TechnologiesAdvantagesDisadvantages% RemovalOxidation/precipitationAir oxidationRelatively simple, low-cost but slow processMainly removes arsenic (V) and accelerate the oxidation process80%In situ arsenic removalAlso oxidizes other inorganic and organic constituents in waterChemical oxidationRelatively simple and fast processEfficient control of the pH and oxidation step is needed90%Oxidizes other impurities and kills microbesMinimum residual massCoagulation/coprecipitationAlum coagulationRelatively low capital cost and simple in operationProduces toxic sludges90%Durable powder chemicals are availableLow removal of arsenicEffective over a wider range of pHPreoxidation may be requiredIron coagulationCommon chemicals are availableMedium removal of As (III)94.5%More efficient than alum coagulation on weigh basisSedimentation and filtration neededLime softeningMost common, chemicals are available commerciallyReadjustment of pH is required91%Sorption techniquesActivated aluminaRelatively well known and commercially availableNeeds replacement after 4 to 5 regeneration88%Iron-coated sandExpected to be cheapYet to be standardized93%No regeneration is requiredProduces toxic solid wasteRemove both As (III) and As (V)Ion exchange resinWell-defined medium and capacityHigh cost87%The process is less dependent on pH of waterRequires high tech operation and maintenanceExclusive ion specific resin to remove arsenicRegeneration creates a sludge disposal problemAs (III) is difficult to removeLife of resinsMembrane techniquesNanofiltrationWell-defined and high removal efficiencyVery high capital cost95%PreconditioningHigh water rejectionReverse osmosisNo toxic solid waste is producedHigh tech operation and maintenance96%ElectrodialysisCapable of removing  other contaminantsToxic wastewater produced95%


## 3. Electrocoagulation Characteristics

Electrocoagulation has been known as an electrochemical phenomenon since the last century. It has been employed previously for treating many types of wastewater with varying degrees of success. However, most studies have focused on the efficiency of waste removal without exploring the fundamental mechanisms involved in EC [8]. This electrochemical method of waste removal requires smaller quantities of salt addition to increase the conductivity of the solution and the maintenance and operation of the EC cells are relatively simple. Since 1970, this technology has become increasingly popular around the world for treatment of industrial wastewater containing heavy metals [9]. Electrocoagulation processes offer significant potential for removing soluble ionic species from solution, particularly heavy metals [10]. EC operating conditions are highly dependent on the chemistry of the aqueous medium, especially conductivity and pH. Other important characteristics such as particle size, type of electrodes, retention time between plates, plate spacing, and chemical constituent concentrations dictate the operating parameters of the process [11]. The EC process operates on the principle that the cations produced electrolytically from iron and/or aluminum anodes enhance the coagulation of contaminants from an aqueous medium. The sacrificial metal anodes are used to continuously produce polyvalent metal cations in the vicinity of the anode. These cations facilitate coagulation by neutralizing the negatively charged particles that are carried toward the anodes by electrophoretic motion.A schematic representation of the EC process is shown in Figure1. As mentioned above, the gas bubbles produced by the electrolysis carry the pollutant to the top of the solution where it is concentrated, collected, and removed. The removal mechanisms in EC may involve oxidation, reduction, decomposition, deposition, coagulation, absorption, adsorption, precipitation, and flotation [14].Figure 1
An illustration of the EC mechanism (arrows indicate the migration of electrolysis gasH2).EC overall reactions are(1)Fe+6H2O→Fe(H2O)4(OH)2(s)+H2(g)↑(2)Fe+6H2O→Fe(H2O)3(OH)3(s)+112H2(g)↑In the appropriate conditions, iron (II) and iron (III) hydroxides combine in the following proportion to generate Green Rust:(3)xFe(OH)3(aq)+(6-X)Fe(OH)2(aq)→xFe(OH)3*(6-X)Fe(OH)2(s)


### 3.1. Green Rust (GR)

EC can be considered as an accelerated corrosion process. GR is recognized as an important intermediate phase in corrosion ofFe0 (Figure 2).Figure 2
Green rust generated with EC.GRs are layered Fe(II)-Fe(III) hydroxides having a pyroaurite-type structure consisting of alternating positively charged hydroxide layers and hydrated anion layers. Some of the Fe(II) of the octahedral sheets ofFe(OH)2 is replaced by Fe(III). This results in positive layers of charge that are balanced by the inclusion of anions between the layers [15]. Its exact nature depends on the interlayer anion. Various forms have been synthesized and studied. Results of many studies have shown that GRs conform to a general chemical composition and stoichiometry, that can be represented with the general formula: [Fe(6-x)IIFexIII(OH)12]x+[(A)x/n·yH2O]x-, where x ranges from 0.9 to 4.2, A is an n-valent anion (typically CO32-, Cl-, or SO42-, and y denotes the varying amounts of interlayer water (typically y ranges from 2 to 4 for most GRs [16].GRs, unlike most iron oxides in whatever form, have an internal surface area; so these minerals have both large specific surface areas and reactivity. The amphoteric surface hydroxyl groups lead to both sorption of heavy metals (cations) as well as organic anions, for example, linear alkyl benzene sulfonates and inorganic anions, for example, silicate, arsenate, and selenate. Furthermore, polar noncharged compounds are sorbed into the interlayer. Cations as Cu(II), Ni(II), Zn(II), Cd(II), Co(II), and Mg(II) may isomorphically substitute for Fe(II) during GR formation (co precipitation). For example, nickelous-ferric GR rusts, the end products obtained by substitution of Fe(II) ions by Ni(II) ions, have been demonstrated [17–20]. This incorporation of cationic inorganic contaminants into the structures of GR could provide an effective means of sequestering contaminants in the subsurface.


## 3.1. Green Rust (GR)

EC can be considered as an accelerated corrosion process. GR is recognized as an important intermediate phase in corrosion ofFe0 (Figure 2).Figure 2
Green rust generated with EC.GRs are layered Fe(II)-Fe(III) hydroxides having a pyroaurite-type structure consisting of alternating positively charged hydroxide layers and hydrated anion layers. Some of the Fe(II) of the octahedral sheets ofFe(OH)2 is replaced by Fe(III). This results in positive layers of charge that are balanced by the inclusion of anions between the layers [15]. Its exact nature depends on the interlayer anion. Various forms have been synthesized and studied. Results of many studies have shown that GRs conform to a general chemical composition and stoichiometry, that can be represented with the general formula: [Fe(6-x)IIFexIII(OH)12]x+[(A)x/n·yH2O]x-, where x ranges from 0.9 to 4.2, A is an n-valent anion (typically CO32-, Cl-, or SO42-, and y denotes the varying amounts of interlayer water (typically y ranges from 2 to 4 for most GRs [16].GRs, unlike most iron oxides in whatever form, have an internal surface area; so these minerals have both large specific surface areas and reactivity. The amphoteric surface hydroxyl groups lead to both sorption of heavy metals (cations) as well as organic anions, for example, linear alkyl benzene sulfonates and inorganic anions, for example, silicate, arsenate, and selenate. Furthermore, polar noncharged compounds are sorbed into the interlayer. Cations as Cu(II), Ni(II), Zn(II), Cd(II), Co(II), and Mg(II) may isomorphically substitute for Fe(II) during GR formation (co precipitation). For example, nickelous-ferric GR rusts, the end products obtained by substitution of Fe(II) ions by Ni(II) ions, have been demonstrated [17–20]. This incorporation of cationic inorganic contaminants into the structures of GR could provide an effective means of sequestering contaminants in the subsurface.


## 4. Experimental Details

For the adsorption tests a beaker size reactor (400 mL) was used, and it was equipped with two carbon steel electrodes (6 cm by 3 cm) separated 5 mm. A universal AC/DC adaptor was used as a power source. pH values were registered with a VWR scientific 8005 pH meter.To determine the adsorption of arsenic on iron species electrolytic solutions were prepared with sodium arsenateNa2HAsO4 (reagent grade with a purity of 97% made by Monterrey chemical products) and deionized water with a conductivity of 0.95 μS (Aldrich Chemical Co. 99.5+%, A.C.S. reagent, Lot number DI02350AI). Arsenic concentrations in the prepared solutions were 1, 2, 5, 7, 13, 20, and 30 mg/L.Conductivity was adjusted by adding one gram of NaCl per liter of water (Fisher, 99.8% A.C.S. Certified, Lot number 995007). Solution and solids were separated by filtration through cellulose filter paper. The sludge from the EC was dried either in an oven or under vacuum at room temperature.


## 5. Adsorption Results

### 5.1. Calculus of Arsenic Moles Adsorbed on Iron Species

The amount of arsenic at equilibriumqe(mg/g) on iron species was calculed from the following equation:(4)N=v*(C0-CeW),
where  C0and Ce (mg/L) are the liquid phase concentrations of arsenic at initial and equilibrium, respectively, v is the volume of the solution, and W is the mass of adsorbent used (g) (in this case the Fe dissolved from EC) (Table 2).Table 2
Conditions for arsenic adsorption tests.
SamplesInitial concentration (mg/L)Initial temperature(C°)Initial pHIntensity current (amperes)Voltage (volts)Time (min)11202.860.498.5522203.020.5212535202.900.4410547203.050.4112.85513202.900.4810.75620203.020.510.255730204.170.756.685The metal amount that dissolves or deposits depends on the quantity of electricity that passes across the electrolytic solution and the residence time in the EC cell.A simple relation between the current density and the quantity of substance dissolved (g ofMfor cm2) stems from Faraday’s law [21, 22]:(5)W=(D*t*M)n*F,
where W is the amount of the electrode dissolved (grcm-2), D the current density (Acm-2), t the time (seconds), M the relative molar mass of the electrode, n the number of electrons in the redox reaction, and F Faraday’s constant (96500 coulombs).The number of arsenic moles adsorbed on iron species is calculated by (4). Results (Table 3) show that arsenic adsorption increases as the arsenic concentration in the solution increases [23].Table 3
Arsenic moles adsorbed on iron species (N).
SampleC0As (mmol/L)CeAs (mmol/L)W (grs)N (mmol/gr)10.0133470.00020.0284350.16182720.0266950.00060.0336580.27065530.0667370.00090.0255340.90199440.0934320.00200.0237931.34498150.1735180.00490.0278552.11822360.2669510.01260.0290163.06714770.4004270.01680.0435233.084857


### 5.2. Langmuir’s Isotherm

The Langmuir equation is given in the following equation:(6)N=(NmaxKLCe1+KLCe),
where N is the solid phase adsorbate concentration in equilibrium (mg/g), Nmax the maximum adsorption capacity corresponding to complete monolayer coverage on the surface (mg/g), Ce the concentration of adsorbate at equilibrium (mg/L), and KL the Langmuir constant (L/mg). Equation (6) can be rearranged  to a linear form:(7)CeN=1NmaxKL+CeNmax.It was observed that the equilibrium adsorption data followed Langmuir’s model. Langmuir’s isotherm (Figure3) shows the arsenic adsorption capacity on iron species [24, 25]. Constants can be evaluated from the intercepts and the slopes of the linear plots of Ce/N versus Ce.Langmuir isotherm for arsenic adsorption on iron species.
(a)(b)Table4 shows the results of linear regression. The value of Nmax indicates the maximum adsorption capacity corresponding to complete monolayer coverage on the iron surface. The value of KL is the Langmuir adsorption constant [26].Table 4
Linear regression results for arsenic adsorption.
R20.9665Nmax(mmolAs)/gFe)4.242681KL (L/mmol)181.30


### 5.3. Covered Fraction of Arsenic on Iron Species

Equationθ=N/Nmax calculates the covered fraction (θ) with the obtained results for N and Nmax. In Table 5 it can observed that the covered fraction θ approaches 1 when N concentration increases.Table 5
Covered fractionθ for arsenic.
N(mmol/gr)Nmax (mmol/gr)θ0.1618274.24260.0380.2706554.24260.0640.9019944.24260.2131.3449814.24260.3172.1182234.24260.4993.0671474.24260.7223.084854.24260.727


## 5.1. Calculus of Arsenic Moles Adsorbed on Iron Species

The amount of arsenic at equilibriumqe(mg/g) on iron species was calculed from the following equation:(4)N=v*(C0-CeW),
where  C0and Ce (mg/L) are the liquid phase concentrations of arsenic at initial and equilibrium, respectively, v is the volume of the solution, and W is the mass of adsorbent used (g) (in this case the Fe dissolved from EC) (Table 2).Table 2
Conditions for arsenic adsorption tests.
SamplesInitial concentration (mg/L)Initial temperature(C°)Initial pHIntensity current (amperes)Voltage (volts)Time (min)11202.860.498.5522203.020.5212535202.900.4410547203.050.4112.85513202.900.4810.75620203.020.510.255730204.170.756.685The metal amount that dissolves or deposits depends on the quantity of electricity that passes across the electrolytic solution and the residence time in the EC cell.A simple relation between the current density and the quantity of substance dissolved (g ofMfor cm2) stems from Faraday’s law [21, 22]:(5)W=(D*t*M)n*F,
where W is the amount of the electrode dissolved (grcm-2), D the current density (Acm-2), t the time (seconds), M the relative molar mass of the electrode, n the number of electrons in the redox reaction, and F Faraday’s constant (96500 coulombs).The number of arsenic moles adsorbed on iron species is calculated by (4). Results (Table 3) show that arsenic adsorption increases as the arsenic concentration in the solution increases [23].Table 3
Arsenic moles adsorbed on iron species (N).
SampleC0As (mmol/L)CeAs (mmol/L)W (grs)N (mmol/gr)10.0133470.00020.0284350.16182720.0266950.00060.0336580.27065530.0667370.00090.0255340.90199440.0934320.00200.0237931.34498150.1735180.00490.0278552.11822360.2669510.01260.0290163.06714770.4004270.01680.0435233.084857


## 5.2. Langmuir’s Isotherm

The Langmuir equation is given in the following equation:(6)N=(NmaxKLCe1+KLCe),
where N is the solid phase adsorbate concentration in equilibrium (mg/g), Nmax the maximum adsorption capacity corresponding to complete monolayer coverage on the surface (mg/g), Ce the concentration of adsorbate at equilibrium (mg/L), and KL the Langmuir constant (L/mg). Equation (6) can be rearranged  to a linear form:(7)CeN=1NmaxKL+CeNmax.It was observed that the equilibrium adsorption data followed Langmuir’s model. Langmuir’s isotherm (Figure3) shows the arsenic adsorption capacity on iron species [24, 25]. Constants can be evaluated from the intercepts and the slopes of the linear plots of Ce/N versus Ce.Langmuir isotherm for arsenic adsorption on iron species.
(a)(b)Table4 shows the results of linear regression. The value of Nmax indicates the maximum adsorption capacity corresponding to complete monolayer coverage on the iron surface. The value of KL is the Langmuir adsorption constant [26].Table 4
Linear regression results for arsenic adsorption.
R20.9665Nmax(mmolAs)/gFe)4.242681KL (L/mmol)181.30


## 5.3. Covered Fraction of Arsenic on Iron Species

Equationθ=N/Nmax calculates the covered fraction (θ) with the obtained results for N and Nmax. In Table 5 it can observed that the covered fraction θ approaches 1 when N concentration increases.Table 5
Covered fractionθ for arsenic.
N(mmol/gr)Nmax (mmol/gr)θ0.1618274.24260.0380.2706554.24260.0640.9019944.24260.2131.3449814.24260.3172.1182234.24260.4993.0671474.24260.7223.084854.24260.727


## 6. Thermodynamic Studies

The thermodynamic parameters such as change in standard free energy (ΔG∘), enthalpy (ΔH∘), and entropy (ΔS∘) were determined using the following equations:(8)ln(1b)=ΔG°RT,ln(b)=b0-(ΔH∘RT),ΔG∘ads=ΔH∘ads-TΔS∘ads,
where R is the gas constant, (Jmol-1K-1°) is the absolute temperature, b is Langmuir’s constant which is related to the energy of adsorption, and b0 is a constant.Table6 shows a negative value of ΔG∘, indicating that arsenic adsorption on iron species by EC is a spontaneous process. The negative value of ΔH∘ indicates an exothermic process and suggests physisorption according to the value for the liberated heat between −20 and −40 KJ/mol. The negative value of ΔS∘ suggests that there is not a significant change in the internal structure of the adsorbent during the adsorption of As [25, 26].Table 6
Thermodynamic Parameters for arsenic adsorption.
ΔHads(kJ/mol)ΔGads(KJ/mol)ΔSads(KJ/molK°)−34.6885−29.3929−0.01814


## 7. Product Characterization

It is difficult to differentiate between iron oxide and oxyhydroxide species using only a single analytical technique. In this study, Powder X-ray Diffraction (XRD), Scanning Electron Microscope (SEM), and Transmission Mössbauer Spectroscopy (TMS) were used to characterize the solid products formed from carbon steel electrodes during EC.


### 7.1. X-Ray Diffraction

Diffractogram was obtained with a Philips X'Pert MPD system operating withCuKα radiation source filtered with a graphite monochromator (λ = 1.5406 Å). The spectrum scan rate was set at 0.02 degrees per second. For arsenic a diffractogram was obtained with a Bruker-AXS D4 Endeavor diffractometer operating with CuKα radiation source filtered with a graphite monochromator (λ = 1.5406 Å). The samples were ground to a fine powder in isopropyl alcohol (Sigma-Aldrich) and loaded into a sample holder. The XRD scans were recorded from 20 to 70 degrees 2θ with 0.020° step-width, and with 10 seconds counting time for every step-width. Experiments were run at 40 kV and 40 mA. Figure 4 shows the diffractogram of EC solid product sample obtained from a 2 ppm of arsenic solution at pH 7. The identified species were lepidocrocite and iron arsenate in crystalline form.Figure 4
XRD of the EC solid products that shows iron impregnated with Arsenic.


### 7.2. Scanning Electron Microscopy (SEM) and Energy Dispersive Analysis of X-rays (EDAX)

Figure5 shows SEM and EDAX images of As on iron oxide/oxyhydroxide particles, respectively. These SEM and EDAX results show that the surfaces of these iron oxide/oxyhydroxide particles were coated with a layer of As and species.SEM and EDAX images of by-products generated from the arsenic contaminated water samples.
(a)(b)


### 7.3. Transmission Mössbauer Spectroscopy for Arsenic

Figure7 shows the spectrum obtained from the EC solid product from 2 ppm arsenic solution pH = 7.0. Mössbauer Spectra for each sample was obtained on a ± 15 mm/s velocity scale, which allows observation of wide magnetic hyperfine spectra expected from iron oxide compounds. The spectrum consists of a doublet magnetic spectrum, which is probably due to fine particles of iron oxides (nonstoichiometric magnetite) or iron hydroxides (Goethite, etc., see Figure 6).Figure 6
Mössbauer spectrum with arsenic at pH=7, indicating the presence of magnetite.Figure 7
FT-IR spectrum of iron electrode by-product.From the analysis of these techniques the in-situ generated small fine particles of iron- oxide/oxyhydroxides in the EC process are nonstoichiometric magnetite, goethite and iron hydroxide oxide. A recent study [18] shows that EC can be combined with magnetic seeding to produce a magnetic aggregate that can be efficiently separated by High-Gradient Magnetic Separation (HGMS) in-line with the EC reactor.


### 7.4. Fourier Transform Infrared Spectroscopy

FT-IR analyses were carried out by Thermonicolate FTIR spectrometer and OMNIC software using potassium bromide pellets (sample: KBr = 1: 50). The spectra were usually recorded in the range of 4000–400cm-1 with 2 cm-1 resolution. 64 scans were collected for each specimen. Figure 7 shows the FT-IR spectrum of the by-product. Infrared analysis of iron electrode by-product showed OH stretching at 3738 and 3447 cm-1, hydroxyl bending and γ′(OH) water bending vibration, or overtones of hydroxyl bending around 1637 cm-1 [19, 20]. Bands for lepidocrocite phase showed up at 1120, 1023, and 745 cm-1 [21]. Magnetite (Fe3O4 or Fe3-xO4) band at 575 cm-1and Fe-O vibration band is seen at 469 cm-1 [21, 22]. For details of FT-IR analysis see Table 7. XRD analyses also confirmed the presence of these species detected by FT-IR.Table 7
FT-IR vibrations and their corresponding wavenumbers and region for the bands observed for the EC-by product.
Electrode materialType of vibrationsVibration wavenumbers (cm-1)Vibration range (cm-1)IronOH stretching37383689–378734473550–3000Hydroxyl bending16371572–1813γ′(OH) water bending16371572–1813Overtones of hydroxyl bending16371572–1813Magnetite (Fe3O4 or Fe3-xO4)575526–840Fe-O469416–510Lepidocrocite11201090–12451023923–1057745730–90


## 7.1. X-Ray Diffraction

Diffractogram was obtained with a Philips X'Pert MPD system operating withCuKα radiation source filtered with a graphite monochromator (λ = 1.5406 Å). The spectrum scan rate was set at 0.02 degrees per second. For arsenic a diffractogram was obtained with a Bruker-AXS D4 Endeavor diffractometer operating with CuKα radiation source filtered with a graphite monochromator (λ = 1.5406 Å). The samples were ground to a fine powder in isopropyl alcohol (Sigma-Aldrich) and loaded into a sample holder. The XRD scans were recorded from 20 to 70 degrees 2θ with 0.020° step-width, and with 10 seconds counting time for every step-width. Experiments were run at 40 kV and 40 mA. Figure 4 shows the diffractogram of EC solid product sample obtained from a 2 ppm of arsenic solution at pH 7. The identified species were lepidocrocite and iron arsenate in crystalline form.Figure 4
XRD of the EC solid products that shows iron impregnated with Arsenic.


## 7.2. Scanning Electron Microscopy (SEM) and Energy Dispersive Analysis of X-rays (EDAX)

Figure5 shows SEM and EDAX images of As on iron oxide/oxyhydroxide particles, respectively. These SEM and EDAX results show that the surfaces of these iron oxide/oxyhydroxide particles were coated with a layer of As and species.SEM and EDAX images of by-products generated from the arsenic contaminated water samples.
(a)(b)


## 7.3. Transmission Mössbauer Spectroscopy for Arsenic

Figure7 shows the spectrum obtained from the EC solid product from 2 ppm arsenic solution pH = 7.0. Mössbauer Spectra for each sample was obtained on a ± 15 mm/s velocity scale, which allows observation of wide magnetic hyperfine spectra expected from iron oxide compounds. The spectrum consists of a doublet magnetic spectrum, which is probably due to fine particles of iron oxides (nonstoichiometric magnetite) or iron hydroxides (Goethite, etc., see Figure 6).Figure 6
Mössbauer spectrum with arsenic at pH=7, indicating the presence of magnetite.Figure 7
FT-IR spectrum of iron electrode by-product.From the analysis of these techniques the in-situ generated small fine particles of iron- oxide/oxyhydroxides in the EC process are nonstoichiometric magnetite, goethite and iron hydroxide oxide. A recent study [18] shows that EC can be combined with magnetic seeding to produce a magnetic aggregate that can be efficiently separated by High-Gradient Magnetic Separation (HGMS) in-line with the EC reactor.


## 7.4. Fourier Transform Infrared Spectroscopy

FT-IR analyses were carried out by Thermonicolate FTIR spectrometer and OMNIC software using potassium bromide pellets (sample: KBr = 1: 50). The spectra were usually recorded in the range of 4000–400cm-1 with 2 cm-1 resolution. 64 scans were collected for each specimen. Figure 7 shows the FT-IR spectrum of the by-product. Infrared analysis of iron electrode by-product showed OH stretching at 3738 and 3447 cm-1, hydroxyl bending and γ′(OH) water bending vibration, or overtones of hydroxyl bending around 1637 cm-1 [19, 20]. Bands for lepidocrocite phase showed up at 1120, 1023, and 745 cm-1 [21]. Magnetite (Fe3O4 or Fe3-xO4) band at 575 cm-1and Fe-O vibration band is seen at 469 cm-1 [21, 22]. For details of FT-IR analysis see Table 7. XRD analyses also confirmed the presence of these species detected by FT-IR.Table 7
FT-IR vibrations and their corresponding wavenumbers and region for the bands observed for the EC-by product.
Electrode materialType of vibrationsVibration wavenumbers (cm-1)Vibration range (cm-1)IronOH stretching37383689–378734473550–3000Hydroxyl bending16371572–1813γ′(OH) water bending16371572–1813Overtones of hydroxyl bending16371572–1813Magnetite (Fe3O4 or Fe3-xO4)575526–840Fe-O469416–510Lepidocrocite11201090–12451023923–1057745730–90


## 8. Conclusions

The results of this study indicate that arsenic can be successfully adsorbed on iron species by electrocoagulation process. Based on Langmuir’s isotherm analysis, the adsorption capacity was determined to be 4.24 mmol/gr for arsenic. The negative values ofΔG∘ obtained indicated that the arsenic adsorption on iron species by EC is a spontaneous process. The negative values of ΔH∘ represent an exothermic process and suggest a physisorption behavior. The negative values of ΔS∘ suggest that a significant change does not happen in the internal structure of the adsorbent during the adsorption of As. The X-ray diffraction, Scanning Electronic Microscopy, Transmission Mössbauer, and Fourier Transform Infrared Spectroscopy techniques demonstrate that the formed species are of magnetic type, like lepidocrocite which adsorbed the arsenic particles on his surface due to the electrostatic attraction between both metals. The 99% arsenic removal in the experimental EC reactor is usually completed within 60 seconds (data is not shown here) or less for most experiments with current efficiency of 100%. EC with the air injection technique built in a robust pilot system is a very promising technology for removal of toxic and heavy metals where adjustment of pH is not required during the EC process.



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