**1. Introduction**

Water pollution due to petroleum compounds such as MTBE is one of the main problems in water resources [1,2]. MTBE is classified as an oxygenated compound added to gasoline to restore combustion [3]. MTBE has expanded as an octane booster and antiknocking agent in the past two decades due to its low cost and easy usage, transition, and distribution. MTBE, (CH3)3COCH3, is a volatile, colorless, and flammable liquid, and it is soluble in water (48 g/L at 25 ◦C). However, it causes environmental and health effects (IARC), such as nervous system reactions, dizziness, distraction, nausea, and forgetfulness [4,5]. Moreover, it has a low-threshold taste and odor (40 and 15 µg/L, respectively) [6]. The maximum contaminant level of MTBE in drinking water has been determined to be

Derakhshan, Z.; Abbasi, F.; Samaei, M.R.; Baghapour, M.A.; Hoseini, M.; Lima, E.C.; Bilal, M. The Effect of Arsenic on the Photocatalytic Removal of Methyl Tet Butyl Ether (MTBE) Using Fe2O3/MgO Catalyst, Modeling, and Process Optimization.

**Citation:** Mehdizadeh, A.;

doi.org/10.3390/catal12080927 Academic Editor: John Vakros

*Catalysts* **2022**, *12*, 927. https://

Received: 29 June 2022 Accepted: 18 August 2022 Published: 22 August 2022

**Publisher's Note:** MDPI stays neutral with regard to jurisdictional claims in published maps and institutional affiliations.

**Copyright:** © 2022 by the authors. Licensee MDPI, Basel, Switzerland. This article is an open access article distributed under the terms and conditions of the Creative Commons Attribution (CC BY) license (https:// creativecommons.org/licenses/by/ 4.0/).

20–40 µg/L by the USEPA. MTBE enters groundwater in various ways, such as leakage from road accidents, underground storage tanks (USTs), and pipelines [7,8].

The effective removal of MTBE from water is essential. Many attempts have been made over the past decades to eliminate MTBE from groundwater. However, MTBE removal using conventional water treatment processes is difficult due to its high solubility, low tendency to the soil, resistance to degradation, the presence of ether bands, and its resistant carbon chain [9–13]. The most commonly used processes for MTBE removal are adsorption using activated carbon, air stripping, and advanced oxidation processes (AOPs). According to previous studies, AOPs, especially photocatalytic oxidation, are the most effective for MTBE decomposition [14–18]. AOPs can remove MTBE effectively, but their efficiency depends on the water-quality characteristics and the level of other contaminants, such as metals [19–21], because the oxidation of metals during AOPs might decrease the efficiency of MTBE removal.

Arsenic is a highly toxic metalloid, and its presence in water is a global problem. Elevated concentrations of arsenic have been detected in some parts of the world, including Bangladesh; India; some South American countries, such as Argentina; and some areas of Kurdistan and Hashtrood in Iran [22]. Arsenic leaches into water from natural and anthropogenic sources, including biological activities, volcanic releases, and human activities, such as the use of pesticides and minerals. Therefore, investigating the removal efficiency of organic matter in arsenic-contaminated water is essential. As(III), oxidized to As(V) during photocatalytic oxidation [23], can be considered a competitor for the removal of organic matter (such as MTBE). One suggested solution is a combination process with a high oxidation capacity, such as the photocatalytic process. The initial energy obtained from the photo resource and the activation energy is decreased using catalysts in the photocatalytic process.

In this study, Fe2O3/MgO was used as a catalyst because it is a porous structure with a high capacity for adsorbing organic matter [24,25] and generating free radicals [26]. Moreover, its band gap is 5.4–5.45 ev, so the electron in the band layer excites the current layer [24]. Therefore, its photocatalytic effect is performed when it is exposed to UV radiation. In other words, MgO doped with a metal oxide improves photocatalytic activity [27,28]. So, the removal efficiency of organic dye using Fe2O3-doped MgO is estimated to be above 92% after five regenerations [29] therefore, the combination of MgO and Fe2O<sup>3</sup> can improve the removal efficiency of organic matter, such as MTBE, which is used for the first time in this study. In an earlier study, the photocatalytic process was used for MTBE removal [30], but there was less attention paid to the effect of metal, especially arsenic, on the MTBE's removal efficiency. For example, Zhang et al. (2018) reported that nickel decreased the adsorption capacity of MTBE using ZSM-5 zeolite [6]. However, for the first time, this study focuses on the decreasing trend in the photocatalytic oxidation of MTBE using Fe2O3/MgO due to arsenic.

Arsenic, as a semimetal, can participate in electron-hole processes in aqueous solutions so that it turns into arsenic with an oxidation number of five during the redox reaction. Since the photocatalytic process is a suitable method for mineralizing organic compounds such as MTBE, the released radicals ultimately cause water treatment. Therefore, the paths for both arsenic deposition and photocatalytic reactions are the same, which greatly increases the possibility of interference. Numerous studies have examined the effect of some metals on interference in the photocatalytic process, including the formation, recombination, and formation rate of radicals. However, these effects have been less investigated when considering semimetals, especially arsenic. Due to the existence of a variety of arsenic concentrations in the water resources of Iran and other regions of the world; the high potential of semiconductors for active participation in electron transfer processes; and the strong tendency for arsenic to change its oxidation number and phase from soluble to insoluble forms in aqueous solutions exposed to the photocatalytic process, the present study aims to model and determine the interference effect on a laboratory scale for the first time in order to consider the type and amount of interference effect in the treatment

of water resources using the photocatalytic process on a real scale and optimize the parameters accordingly. from soluble to insoluble forms in aqueous solutions exposed to the photocatalytic process, the present study aims to model and determine the interference effect on a laboratory

processes; and the strong tendency for arsenic to change its oxidation number and phase

*Catalysts* **2022**, *12*, x FOR PEER REVIEW 3 of 14

Arsenic is a toxic metalloid detected in some water supplies, such as in Iran. Concerning the oxidation potential of arsenic in an aqueous solution, it is expected that its interference in the photocatalytic removal of organic matter includes MTBE. Regarding the significant concern about MTBE, the high concentrations of arsenic that have been reported in some areas of Iran, and its interference effect on the mineralization and degradation of MTBE, as well as the lack of documents, imply the effect of metals on the removal efficiency of organic matter. Therefore, this study aims to investigate the effect of arsenic on the photocatalytic oxidation process of MTBE using Fe2O3/MgO as a catalyst. Moreover, the interactions between the effective factors and the optimization of the process were determined by the response surface methodology (RSM) method. scale for the first time in order to consider the type and amount of interference effect in the treatment of water resources using the photocatalytic process on a real scale and optimize the parameters accordingly. Arsenic is a toxic metalloid detected in some water supplies, such as in Iran. Concerning the oxidation potential of arsenic in an aqueous solution, it is expected that its interference in the photocatalytic removal of organic matter includes MTBE. Regarding the significant concern about MTBE, the high concentrations of arsenic that have been reported in some areas of Iran, and its interference effect on the mineralization and degradation of MTBE, as well as the lack of documents, imply the effect of metals on the removal efficiency of organic matter. Therefore, this study aims to investigate the effect of

#### **2. Results** arsenic on the photocatalytic oxidation process of MTBE using Fe2O3/MgO as a catalyst.

#### *2.1. Specification of the Catalyst* Moreover, the interactions between the effective factors and the optimization of the pro-

#### 2.1.1. SEM–EDX Analysis cess were determined by the response surface methodology (RSM) method.

SEM determined the microstructure and morphology of the catalyst, and its images are shown in Figure 1. **2. Results** 

The synthesized catalyst has a uniform and aggregated structure, making separation from the liquid effluent easier after the photocatalytic process [31]. In addition, it has good dispersion, and the sample has a diameter of approximately 2 µm. In Figure 1b, the elements' quantitative levels in the nanocatalyst were determined using EDX, confirming the presence of the elements MgO (45.06%) and Fe2O<sup>3</sup> (33.06%) in the synthesized catalyst. *2.1. Specification of the Catalyst*  2.1.1. SEM–EDX Analysis SEM determined the microstructure and morphology of the catalyst, and its images are shown in Figure 1.

**Figure 1.** *Cont.*

**Figure 1. Figure 1.**  SEM ( SEM ( **a**) and EDX ( **a**) and EDX ( **b**) images for the nanocatalyst. **b**) images for the nanocatalyst.

## 2.1.2. XRD Analysis

**2. Results** 

*2.1. Specification of the Catalyst* 

2.1.1. SEM**–**EDX Analysis

are shown in Figure 1.

The XRD analysis (10–80◦ 2θ) of the nanocatalyst is shown in Figure A1. The average crystal size of the sample was calculated using the Scherrer equation: (d = Kλ/(*β* cos *θ*)) The strong and sharp peaks in Figure A1 suggest that the nanocatalyst has a crystalline structure. The values for Fe2O<sup>3</sup> and MgO were 91.1 and 27.9 nm, respectively. As shown in the figure, the diffraction peaks of both Fe2O<sup>3</sup> and MgO could be observed. The blue peaks are associated with Fe2O3, and the red peaks are related to MgO. This nanocatalyst had two peaks at 33.06◦ and 36.5◦ that can be associated with Fe2O<sup>3</sup> and MgO, respectively. According to Figure A1, the peaks related to Fe2O<sup>3</sup> are wholly covered over by MgO's peaks, indicating the high precision of the sol–gel process.

removal efficiency of organic matter. Therefore, this study aims to investigate the effect of arsenic on the photocatalytic oxidation process of MTBE using Fe2O3/MgO as a catalyst. Moreover, the interactions between the effective factors and the optimization of the

SEM determined the microstructure and morphology of the catalyst, and its images

process were determined by the response surface methodology (RSM) method.

## *2.2. Photocatalytic Removal of MTBE*

The interactions between independent and dependent variables while removing MTBE were investigated in DE7.

The effect of the Fe2O3/MgO nanocatalyst dosage, pH, and initial MTBE concentrations on the photocatalytic removal efficiency and optimization of these variables was investigated by Factorial Experimental Design. The MTBE's lowest, highest, and average removal efficiencies were 61%, 90.90% and 73%, respectively. The ANOVA results for the proposed model for the photocatalytic removal of MTBE based on the experiment's results and the effect of the parameters are presented in Table 1. The F-value and *p*-value for MTBE were 835.92 and >0.0001, respectively. Thus, the *p*-value of the investigated parameters (*p* ≤ 0.05) shows that the concentration of MTBE and the concentration of catalyst are effective parameters for the photocatalytic oxidation of MTBE (Table 1).

In the model, the F-value also shows that the defined parameters in the models have significant effects, and the effect of the initial MTBE concentration was more pronounced than other parameters. However, only a 0.01% chance of the occurrence of the F-value was due to noise. The effects of the significant parameters based on the suggested model are presented in Equation (1) and Figure A2, which are used for predicting the photocatalytic oxidation values of MTBE.

$$\text{MTBE} = 18.70 + 11.32^\text{a} - 0.89 \text{C} + 1.03 \text{BC} - 1.43 \text{DE} - 1.38 \text{B}^2 \tag{1}$$

The MTBE residual was increased based on the model equation, increasing the MTBE (A) concentration and decreasing the catalyst (C). Furthermore, the factors for interactions, such as concentration of arsenic × concentration of catalyst, which had a positive effect and the effect of pH × time, which had a negative effect on the response, and the response affected the quadratic of the arsenic concentration. Based on any of the coefficients, the effect of the catalyst was higher than other parameters.


**Table 1.** ANOVA results for the Response Surface Quadratic Model (MTBE).

Moreover, the perturbation plot of independent variables on the photocatalytic oxidation of MTBE is shown in Figure A2.

According to Figure A2, the most influential factor was MTBE concentration. Moreover, the effect of arsenic concentration on the MTBE photocatalytic process was insignificant.

The proportion of predicted values of the photocatalytic oxidation efficiency of As(III) in the model and the actual values obtained from the experiments are shown in Figure 2.

The determination coefficient for the actual and predicted values of residual MTBE was acceptable (R<sup>2</sup> = 0.9693). The difference between the adjusted determination coefficient (Adj R<sup>2</sup> ) and the predicted determination coefficient (Pred R<sup>2</sup> ) should not be more than 0.2 [32]. Based on the results, this difference was 0.0498, indicating the model's adequacy. Furthermore, R<sup>2</sup> 0.97 for MTBE shows that the model can explain about 97 data variations. The calculated lack of fit in these models is 2.74, which is not significant; therefore, the disordered data do not affect the model.

The Simultaneous Effect of the Concentration of Fe2O3/MgO and Initial MTBE

The efficiency of MTBE removal at various initial concentrations of MTBE and the Fe2O3/MgO catalyst is shown in Figure 3.

**Figure 2.** Predicted versus actual experimental results for residual MTBE. **Figure 2.** Predicted versus actual experimental results for residual MTBE.

**Figure 3.** Contour and 3D Plots of the interactive effect of catalyst dosage (g/L) and MTBE (mg/L). concentrations increased costs. **Figure 3.** Contour and 3D Plots of the interactive effect of catalyst dosage (g/L) and MTBE (mg/L).

According to Figure 3, 1**–**2.5 g/L of catalyst can slightly increase MTBE's removal efficiency, while a catalyst concentration of more than 4 g/L had a negative effect. This is

amount of free radicals that improved the degradation of MTBE. However, a further increase in the catalyst dosage caused the reduction in active sites on the surface of Fe2O3/MgO. Therefore, the removal efficiency of MTBE was decreased [33,34]. Concerning this result, the best concentration of nanoparticles was 1.54 g/L, but the higher

According to Figure 3, 1–2.5 g/L of catalyst can slightly increase MTBE's removal efficiency, while a catalyst concentration of more than 4 g/L had a negative effect. This is because the number of photons and adsorbed molecules in a high catalyst level also increases. This reaction increased the particle density in the brightness range and the amount of free radicals that improved the degradation of MTBE. However, a further increase in the catalyst dosage caused the reduction in active sites on the surface of Fe2O3/MgO. Therefore, the removal efficiency of MTBE was decreased [33,34]. Concerning this result, the best concentration of nanoparticles was 1.54 g/L, but the higher concentrations increased costs.

#### **3. Materials and Methods**

#### *3.1. Materials*

All the analytical-grade chemical materials, including MTBE, sodium arsenite (NaAsO2), magnesium oxide (MgO), hematite (Fe2O3), sodium hydroxide (NaOH), hydrochloric acid (HCL), citric acid (C6H8O7), acetone (C3H6O), hexane (C6H14), and ethanol (C2H6O), were purchased from Sigma Aldrich Company (St. Louis, MI, USA). NaOH and HCl were used for adjusting the pH. The double-distilled water (18 MΩ cm) was applied to prepare the solutions. A UV lamp (11W) was used for the light supply. A powder X-ray diffractometer (XRD) (Philips PW 1800, Round Rock, TX, USA) was used to determine the gel structure. Scanning electron microscopy (SEM) (Carl-Zeiss-Promenade, Jena, Germany) measurement (HV: 20.0 kV) was used to envisage the nanoparticles' surface morphology.

#### *3.2. Preparation of the Catalyst*

In a typical process, highly active MgO nanoparticles were prepared via a simple sol–gel method. First, the MgO nanoparticles were dissolved in ethanol at 60 ◦C for 5 h, and citric acid was added slowly to form the gelling solution by stirring. When the solution was completely dispersed, the compound was concentrated at 65 ◦C to form a wet gel. The wet gel was then dried at 110 ◦C for 12 h. Finally, the above-obtained product was calcinated at 550 ◦C with a heating rate of 4 ◦C min−<sup>1</sup> for 4 h. The Fe2O<sup>3</sup> solution was synthesized by the sol–gel method. This solution was joined to make the final coating with the MgO gel to obtain the final product of Fe2O3/MgO [30].

#### *3.3. Stability and Reusability of the Catalyst*

To examine the stability of the catalyst, 1 g/L of the catalyst was placed in the simulated conditions of the experiments, and then, the concentrations of iron and magnesium remaining in the solution were measured after 0–50 min as described in Table 2.


**Table 2.** Concentration of iron and magnesium remaining in the solution after 0–50 min.

The leakage rate of both magnesium and iron in the aqueous solution was less than 5% during the laboratory conditions, which was statistically confirmed.

After performing the photocatalytic process, the studied reactor was placed in the magnetic field to investigate the secondary application of the catalyst in laboratory conditions during the study period, the efficiency of which was favorable. After drying the catalyst at 70 ◦C, the collected catalyst was weighed on a scale, and the weight difference was estimated to be less than 15%. Moreover, the catalyst was photographed after the photocatalytic process, which did not differ significantly from the initial images. Thus, it can be said that the MTBE mineralization and removal operations were carried out under suitable conditions.

## *3.4. Sample Preparation*

This study used a high-purity MTBE solution (99.9%). An arsenite stock solution (1000 mg/L) was prepared by dissolving potassium arsenite (KAsO2) in distilled water (acid-distilled twice) with HCl (with a final concentration of 2.5%). The samples were stored in a refrigerator at 4 ◦C after preparation. NaOH and HCL were used to adjust the reaction mixture's pH.

#### *3.5. Chemical Reactor and Optimization*

The photocatalytic removal of MTBE was carried out in a laboratory-scale batch slurry reactor. The reactor comprised transparent Plexiglas with dimensions (length, width, and height) of 20 × 10 × 14 cm and 1 L effective volume. A UV lamp (11 W) was submerged in the solution to provide UV radiation for the reactor. First, the reactor was tightly closed and stirred completely. Then, the reactor was fixed and made in the two-seated form. The temperature of the reactor was controlled at 25–30 ◦C. Then, the solution was centrifuged (at 4000 rpm for 30 min) to separate the nanocatalyst.

The design of the experiments was performed based on a partial factorial method. Table 3 lists the values and variables used in the design of the experiments.

**Table 3.** Natural and coded levels of independent variables based on the central composite design.


The values of the natural and coded independent variables were designed based on the central composite design (CCD). The order of each experiment was selected randomly by Design Expert 7 (DE7) software based on past studies and observed values in Iran's groundwaters. To more closely look at the effect of each variable on the process, one of the values of MTBE, the catalyst or arsenic, is considered zero in the DE7. Finally, 50 experiments were designed as Factorial Designs.

#### *3.6. MTBE Extraction Method*

MTBE was extracted using the dispersive liquid–liquid microextraction (DLLME) method. DLLME is a simple, fast, and sensitive method for extracting organic compounds from aqueous solutions [35]. First, 10 mL of the sample was added to a glass tube with a conical bottom centrifuge tube. The acetonitrile (1 mL) and hexane (0.2 mL) were used as dispersing and extraction solutions, respectively. Next, the mixture solution was centrifuged at 5000 rpm for 2 min. After this stage, hexane droplets were separated, removed with a 10 µL Hamilton syringe, and injected into the GC.

#### *3.7. Data Analysis*

Data analysis was performed using the RSREG method in DE7. The regression coefficients of the empirical data were generalized as a quadratic polynomial model [36]. This model is as follows in Equation (2):

$$Y = \beta\_0 + \sum\_{i=1}^{3} \beta\_i X\_i + \sum\_{i=1}^{3} \beta\_{ii} X\_{i^2} + \sum\_{i<1=1}^{3} \beta\_{ij} X\_i X\_j \tag{2}$$

*Y* = the amount of MTBE, *β*<sup>0</sup> = interactive regression coefficients, *β<sup>i</sup>* = linear regression coefficients, *βii* = quadratic regression coefficients, *βij* = interactive regression coefficients, and *X<sup>i</sup>* and *X<sup>j</sup>* = dependent variables

ANOVA was used to determine the significance of the model and independent variables and determine the values of R<sup>2</sup> , R<sup>2</sup> adjusted, and R<sup>2</sup> predicted. The *p*-value and lack of fit in the variance analysis table, the normal curves, and the predicted values versus the real values were used to check the model's desirability and data. The statistically significant level of the *p*-value was 0.05 [37]. The lack of fit value should not be meaningful (meaning any distorted data in the model). The contours and three-dimensional charts were plotted to analyze the removal rate of MTBE and the interactions of independent variables. Finally, the RSM-obtained optimal conditions for removing MTBE and arsenic were obtained using predicted equations.

#### **4. Conclusions**

Although the photocatalytic process is a suitable method for treating MTBE in an aqueous solution, the presence of some contaminants can be a limiting factor for efficient removal. Arsenic is a metalloid that oxides during the photocatalytic process and competes with MTBE for oxidation. In general, it can be concluded that the method used in this study is more suitable for lower concentrations of MTBE. Although less attention was paid to the effect of As on water treatment, this study showed that the presence of arsenic in water could limit the efficiency of removal of MTBE. Since there is arsenic in some water resources and MTBE leaching, pretreatment for the removal of arsenic is essential. The photocatalytic process is more cost-effective than other methods used to remove organic compounds, such as air stripping, GAC, incineration, and ozonation. This process generally destroys organic pollutants at an ambient temperature and pressure without any need for direct oxygen injection. However, this treatment method is applicable in conditions that are optimal in economic, environmental, and operational terms. The presence of some inhibitory and disruptive factors, such as arsenic, in the water environment could reduce the process efficiency. Therefore, it could be argued that arsenic separation and removal before the photocatalytic process is one of the best options for decreasing this inhibitory effect, which reduces downstream treatment costs.

In this study, the inhibitory effect of arsenic on the photocatalytic oxidation process of MTBE using Fe2O3/MgO was investigated. The Fe2O3/MgO nanocatalyst was successfully synthesized based on the SEM, EDX, and XRD analyses. The results showed that MTBE was removed successfully by photocatalytic oxidation and the best model was the quadratic model (*p* < 0.0001, F = 45.84, R<sup>2</sup> = 0.9693, R<sup>2</sup> adjusted = 0.9482, and R<sup>2</sup> predicted = 0.8984). According to the quadratic model and ANOVA analysis, the most effective factors were the initial concentration of MTBE and the catalyst dosage. The process optimization expressed that the efficiency of the MTBE oxidation process was improved by increasing both the catalyst dosage and time and decreasing MTBE and the pH. The predicted and experimental removal efficiencies were 90.90% and 88.73%, respectively, under the optimal conditions (initial concentration of MTBE = 37.5 mg/L, pH = 5,Catalyst = 1.54 g/L, and Time = 21.41 min). Although the process successfully removed MTBE, arsenic was introduced as an inhibitor factor. So, the highest inhibitory effect related to the initial arsenic is 0.5 mg/L. Concerning these results, the pretreatment of arsenic from water resources and more details about the inhibitory effect of arsenic on the photocatalytic removal of MTBE, such as the formation of hole-electrons, is essential. Moreover, further studies are suggested to determine the effect of other heavy metals and metalloids on organic matter removal efficiency.

**Author Contributions:** Conceptualization, A.M. and M.R.S.; methodology, F.A.; software, M.A.B. and A.M.; validation, M.H.; investigation, Z.D.; resources, E.C.L.; writing—review and editing, M.B. and E.C.L. All authors have read and agreed to the published version of the manuscript.

**Funding:** This research received no external funding.

1

**Data Availability Statement:** The data presented in this study are available on request from the corresponding author.

**Acknowledgments:** This article was extracted from a thesis written by Akbar Mehdizadeh (proposal No. 14140), which Shiraz University of Medical Sciences financially supported.

**Conflicts of Interest:** The authors declare no conflict of interest.

**Appendix A**

**Figure A1.** XRD patterns of Fe2O<sup>3</sup> and MgO.

**Figure A2.** The perturbation Plot of independent variables in the photocatalytic oxidation of MTBE. **Figure A2.** The perturbation Plot of independent variables in the photocatalytic oxidation of MTBE.

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