# Novel Electrochemical Treatment of Spent Caustic from the Hydrocarbon Industry Using Ti/BDD

Authors: Alejandro Medel; Erika Méndez; José L. Hernández-López; José A. Ramírez; Jesús Cárdenas; Roberto F. Frausto; Luis A. Godínez; Erika Bustos; Yunny Meas
Journal: International Journal of Photoenergy
 (2015)

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## Abstract

During the crude oil refining process, NaOH solutions are used to remove H2S, H2Saq, and sulfur compounds from different hydrocarbon streams. The residues obtained are called “spent caustics.” These residues can be mixed with those obtained in other processes, adding to its chemical composition naphthenic acids and phenolic compounds, resulting in one of the most dangerous industrial residues. In this study, the use of electrochemical technology (ET), using BDD with Ti as substrate (Ti/BDD), is evaluated in electrolysis of spent caustic mixtures, obtained through individual samples from different refineries. In this way, the Ti/BDD’s capability of carrying out the electrochemical destruction of spent caustics in an acidic medium is evaluated having as key process a chemical pretreatment phase. The potential production of •OHs, as the main reactive oxygen species electrogenerated over Ti/BDD surface, was evaluated in HCl and H2SO4 through fluorescence spectroscopy, demonstrating the reaction medium’s influence on its production. The results show that the hydrocarbon industry spent caustics can be mineralized to CO2 and water, driving the use of ET and of the Ti/BDD to solve a real problem, whose potential and negative impact on the environment and on human health is and has been the environmental agencies’ main focus.


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## Body

## 1. Introduction

The aqueous residues produced by the hydrocarbon industry, which involve the use of sodium hydroxide (NaOH) to remove hydrogen sulfide (H2S), sulfhydric acid (H2Saq), and sulfur compounds, found in different fractions of crude oil, are known as spent caustics. The process of producing said residues begins when an aqueous solution of NaOH is mixed with a fraction of oil. Although the oil itself can contain sulfur, the process is commonly carried out after the oil fraction is distilled, due to its contact with air, allowing the formation of H2S, which is very corrosive and difficult to remove. If the H2S is formed, the NaOH reacts with it to form sodium sulfide, which is water soluble. The spent caustics are also obtained from different and specific processes, whereby they are classified as sulfidic spent caustics (removal of H2S and mercaptans from hydrocarbons), naphthenics (removal of naphthenic acids from kerosene and diesel), and cresylic spent caustics (removal of organic acids, phenols, cresols, and xylenols). In the case of naphthenics and cresylics, the NaOH reacts with the naphthenic acids, leading to the formation of sodium naphthenates and phenolates, respectively. Accordingly and depending on the quantity and type of products processed, a refinery can generate spent caustics with multiple characteristics containing sulfide (S2−, 1–4 wt%), mercaptans (0.1–4 wt%), phenols (0–2,000 mg L−1), total organic carbon (TOC, 6,000–20,000 mg L−1), chemical oxygen demand (COD, 20,000–60,000 mg L−1), biochemical oxygen demand (BOD, 5,000–15,000 mg L−1), and potentially toxic elements (PTEs) such as Cu, Ni, Cd, Pb, and Cr, among others [1], which require unconventional handling and treatment due to their highly toxic nature and unpleasant odor (the mercaptans can be detected in ppb). In the specific case of spent caustics produced from olefins plants, large amounts of S2− (14,000–21,000 mg L−1), pH values of 13.5 to 13.7, and emulsified hydrocarbons have also been reported [2]. With regard to the phenolic content, depending on the refining process, it can reach up to 30,600 mg L−1 [3]. The potential danger of the spent caustics can be understood considering the fact that, by not having technology for its treatmentin situ, the different types of spent caustics can be combined, resulting in the production of highly toxic mixtures. On the other hand, when the spent caustics are not treated immediately, these are temporarily stored or confined by authorized companies, with their transport and storage being a latent threat due to the possibility of spillage, which has already been recorded in history with a highly negative impact on human health. A concentration of phenol ranging from 5 to 25 mg L−1 is as toxic for aquatic life as it is for humans [4, 5]. For this reason, the maximum limits allowed of phenol residues found in industrial discharges vary between 0.5 and 1.0 mg L−1 [5]. In the case of potable drinking water, the European Union (EU), in its 80/778/EC Directive, assigned a maximum limit allowed of <0.0005 mg L−1 for phenol in all of its forms [4], given that the consumption of water containing these compounds can induce cancer or death [6]. At the same time, the elevated danger of this contaminant for aquatic life has marked phenol and some phenolic compounds as priority contaminants, in agreement with the criteria of the Environmental Protection Agency (EPA) of the United States [4, 5]. In a conventional manner, the treatment of spent caustics from refineries has been carried out in three steps: (1) wet air oxidation (WAO), (2) acid neutralization (AN), and (3) biological oxidation (BO). On occasions, step (2) can be followed by steam stripping. After AN, stripping removes residual H2S and mercaptans. The liquid effluent obtained has high BOD and COD concentrations because the major portion of the organic constituents is unaffected by the stripping process. Although WAO can treat spent caustic to lower than 1,000 mg L−1 COD in 60 min at 475 K and 28 bar, the process is very expensive, and due to severe reaction conditions, safety is a major concern [2]. At the same time, though the elimination of contaminants in steps (1) and (2) can lead to the obtainment of wastewater easily treatable by BO, this depends strictly on the level of conversion and removal of the contaminants found. For example, if the sulfur content is high and the concentration of phenols is low, the BO (use of bacteria from the genusThiobacillus) is possible. Contrarily, the process can be deactivated when the concentration of phenol is high. It has been reported that effluents containing phenol with a concentration of >3000 mg L−1 cannot be treated through BO [4]. Taking this problem into account, different processes have been applied and evaluated for the treatment of effluents from refineries, leaving aside the treatment of the spent caustics. It is important to mention that the physicochemical nature and composition of the spent caustics is not comparable to wastewater produced as part of the extraction processes of crude oil (water produced) or the wastewater produced in other processes. In spent caustics the content of phenolic compounds can reach a value of 30,600 mg L−1 [3], while in water produced or any other kind of wastewater this value can oscillate between 20 and 200 mg L−1 [7–9]. In the case of wastewaters from refineries, the chemical coagulation using polyaluminium chloride [10], chemical precipitation [11], integrated processes (coagulation-flocculation and flotation) [12], and electrocoagulation (EC) has been reported to remove the high content of the organic material found [13]. At the same time and considering the importance of the phenolic content, as well as the content of commonly found fats and oils [14], the EC has also been evaluated, using NaCl, reaching removal percentages of 91% [15] and 94.5% [16] for synthetic and real samples, respectively. In other studies, the combination of electroflotation (EF) and EC and integrated processes (EC-adsorption-BO) have also been proposed [17, 18]. Although, in spent caustics, the EC has been tested for the removal of sulfides and organic material [1], it is important to highlight that the nature of this process is not destructive, allowing the transference of the pollutants from one phase to another with the subsequent disposal problem. On the other hand and considering the technical difficulties in treating aqueous wastes containing phenol or phenolic compounds through WAO, BO or EC, alternative processes of a destructive nature such as the chemical advanced oxidation processes (AOPs, in the presence or absence of sunlight or assisted light), like the use of hydrogen peroxide (H2O2), ozone (O3), photocatalysis, Fenton process, and the ozonation in alkaline medium, have been amply tested in the treatment of phenols and phenolic compounds. However, the majority of these studies have only been carried out on synthetic samples. In real samples from refineries, applying these processes, only a few studies have been reported [19]. Considering the importance implied in the treatment of real samples, in the last years (2000–2014), different isolated studies have been reported on the treatment of spent caustics using the Fenton process. In this sense, samples containing a COD of 20,160 mg L−1 and a total of phenols of 1,800 mg L−1 have been successfully treated obtaining removal efficiencies of 90% for COD and 99% for total phenols at a pH of 4 [20]. At the same time, when comparing this process using assisted light (photo-Fenton) in the treatment of sulfidic spent caustics, a greater efficiency was reached with a removal of COD and sulfide up to 97% and 100%, respectively [21]. Applying both processes and despite the excellent results, in practice, the percentage of total destruction of the organic content is strictly dependent on the physicochemical composition of the sample to be treated. An elevated organic charge consumes a large amount of H2O2. Also, because of a high concentration of H2S (up to 20 g L−1), its reaction with ferric ion causes a loss of iron catalyst activity [2]. At the same time, it is necessary to emphasize that the chemical AOPs do not possess the ability to destroy the reaction byproducts. Contrarily, one of the most efficient processes and with the potential to carry out the destruction of any contaminant, including phenol and phenolic compounds, is electrochemical oxidation (EO). Said technology bases its efficiency on the nature of the material used as anode [22]. In this sense, two types of anodic materials are known: (i) active anodes (Au, Ni, stainless steel (SS), Pt, IrO2, Ti/RuO2, and analogous combinations) and, (ii) inactive anodes (Ti/PbO2, Ti/SnO2-Sb, and analogous combinations), which are materials with a low or high production of •OH radicals (•OHs), respectively. The •OHs can destroy any toxic pollutant to CO2 and water, due to its high oxidation potential (2.8 V vs. ENH). For this reason the use of inactive anodes is preferred. Here, it is important to mention that Au, Ni, SS, Pt, and analogous combinations are included, due to their similar active or inactive behavior. These materials are not included in the original reference. Although, in the literature, there are numerous studies related to the EO of phenol in synthetic samples [22–53], only a few studies have been reported applying this technology in the treatment of samples from refineries and, as far as we know, there are no reported studies on the treatment of spent caustics. It is also important to consider that both types of aqueous residues represent a highly complex matrix, whose chemical composition can favor or diminish the process efficiency. According to this, using a titanium (Ti) electrode, coated with titanium oxide and ruthenium oxide (RuO2), efficiencies of phenol degradation in 99.7% and 94.5% and oxidation percentages of COD in 88.9% and 70.1% were obtained for synthetic and real samples (petroleum refinery wastewater), respectively [54]. In other studies using Ti/TiO2-RuO2-IrO2 for phenol degradation in wastewater samples from refineries, removal percentages of 74.75% and 48% for COD and TOC, respectively, were obtained, even when using high quantities of chloride ions [7]. At the same time, the use of Ti/RuO2-TiO2-SnO2 has also been evaluated in the hydrocarbon industry effluents, obtaining low percentages of phenol degradation around 20–47% [55]. Ruling out the use of active electrodes and mixtures of these [56], a very important option is the use of Ti/SnO2-Sb and Ti/PbO2, which possess a high production of •OHs; however, the application of these materials continues to be restricted due to structural problems and to the possible release of Pb ions [57–59]. As an alternative anodic material, the boron doped diamond (BDD) has been amply evaluated and accepted due to its unusual properties such as a high corrosion resistance, a low adsorption of organic compounds, generation of oxidizing species (O3, H2O2, and •OH) [60], and an elevated overpotential for the reaction of oxygen evolution, ηO2 [61]. The BDD efficiency is based on its high production of •OHs, which are produced through the water oxidation process (1), leading to the complete mineralization of pollutants to CO2 and water (2), with high current efficiencies [62]. This process is known as electrochemical incineration [22]: (1)H2O⟶OH•+H++e-(2)R+MOH•⟶M+mCO2+nH2O+H++e-It is important to emphasize that different studies on the oxidation of phenol and phenolic compounds in synthetic samples, using BDD, have been presented from 2000 to 2014 [63–86], demonstrating the capability of the use of BDD for the destruction of these pollutants. When comparing the use of Ti/BDD with Ti/SnO2-Sb [87, 88] and PbO2 [89], it was found that the BDD electrode is much better for the destruction of phenol. Although the application of BDD in real samples has been weakly explored, when comparing the BDD with the electro-Fenton process for the treatment of wastewaters from refineries, it has been confirmed that even though the electro-Fenton process can induce a greater phenol degradation in comparison with the BDD electrode, the greater efficiency of degradation of the reaction byproducts (in terms of COD and TOC) occurs with BDD [9, 90]. At the same time, other important studies applying the BDD for the treatment of water produced and typical wastewater from refineries have demonstrated the great efficiency of BDD [91–93]. Said studies and those previously presented not only highlight the effectiveness of the use of the electrochemical technology using BDD but also represent a platform which impulses the use of the BDD, whose scaling potential must be examined in order to advance strategically in solving real problems. According to the above, and based on an extensive review of specialized literature from 1980 to 2014 (use of national and international databases), the object of the present study is to demonstrate the technical feasibility of the use of the Ti/BDD in the electrochemical treatment of spent caustics mixtures, one of the most toxic residues at an industrial level, whose potential and negative impact on the environment and human health is and has been the main focus of environmental agencies.


## 2. Experimental Details

### 2.1. Chemicals

Sulfuric acid (H2SO4), hydrochloric acid (HCl), NaOH, and phenol (C6H5OH) were obtained from J. T. Baker. K2HPO4, KH2PO4, NH4OH, potassium ferricyanide (K3Fe(CN)6), and 4-aminoantipyrine (C11H13N3O) for analysis of phenol in all of its forms were obtained from Aldrich. Coumarin was obtained from Aldrich. The luminescent marine bacteriaVibrio fischeri(Photobacterium phosphoreum) for toxicity analysis was provided by SDI.


### 2.2. Instruments

Analysis of phenol in all of its forms was carried out through visible ultraviolet spectroscopy (UV-Vis), using a Lambda XLS+ spectrophotometer. COD and TOC were evaluated using a Hach model DR/200 reactor/Uv-Vis spectrophotometer DR/2010 and Shimadzu Model TOC-VCSN equipment, respectively. COD was obtained using HACH products. Toxicity analysis was done using a DeltaTox kit, provided by SDI. Electrolysis using ultraviolet light (λ=254 nm) was done by using a Philips mercury lamp with 11 W. Orion Star A215 equipment was used for pH/ORP/conductivity measurements. The electrolysis experiments in galvanostatic mode were performed using Tektronix PWS4323 equipment. The PTEs analyses were performed using a Perkin Elmer Optima 3300 DV model and an Analyst 200/MHS-15 Perkin Elmer. The first equipment was used for the inductively coupled plasma (ICP) analysis and the second for the Hg analyses by hydride generation. The morphology and element analysis of the different electrodes evaluated during the selection of the best anodic material were obtained using a scanning electron microscope (JEOL JMS-6060LV) equipped with an energy dispersive spectrometer (EDS). Crystal structure analysis using X-ray diffraction (XRD) was carried out in a Rigaku Minifles, using Cu Kα radiation, with a 30 kV operation voltage and 15 mA of current, at a velocity of 2°/min. Cyclic voltammetry (CV) was carried out with an Autolab PGSTAT 30. The •OHs analysis was performed by fluorescence spectroscopy using the equipment HORIBA Jobin MOD Fluorolog 3–22 with double monochromator.


### 2.3. Characterization of the Spent Caustics

#### 2.3.1. Sample Preparation

A total of 10 samples (20 L each) of spent caustic were obtained from different refineries and stored at room temperature. From these samples, a composite sample was prepared by combining 1 L of each individual sample. The sample obtained (called mixture) is shown in Figure1(a). This process was carried out using safety equipment (Figure 1(b)) and working under an exhaust hood, which was attached to a gas scrubber containing NaOH (Figure 1(c)).Figure 1
Handling and control of (a) spent caustics mixture, (b) safety equipment, and (c) specialized infrastructure.
(a)
(b)
(c)Before taking each sample, the container was stirred vigorously and the sample was taken immediately. The mixture obtained was also stirred vigorously and stored under refrigeration (4°C) until its analysis.


#### 2.3.2. Physicochemical Analysis

Before carrying out any analysis, the container of the mixture of spent caustics was stirred vigorously. The PTEs analysis was done by using inductively coupled plasma atomic emission spectroscopy (ICP-AES), with the exception of Hg, which was analyzed by hydride generation atomic absorption spectroscopy (HGAAS). The analysis was done prior to digestion of the samples. The concentration of anions present was done through ion chromatography according to the EPA method 300.1 (EPA, 1997). This analysis was performed using a high resolution liquid chromatograph Dionex ICS-2500 HPLC/IC fitted with a Dionex IonPac AS14A column and coupled to a conductivity detector (ED50A). The mobile phase was Na2CO3/NaHCO3 (1 mL min−1). The equipment was calibrated using prepared solutions from the 7-Anion Standard of Dionex and the quality of the results was evaluated from the analysis of the certified standard of Inorganic Ventures IC-FAS-1A. The determination of volatile and semivolatile organic compounds (CIDETEQ and Intertek laboratories) in qualitative form was done through gas chromatography mass spectrometry (GC-MS) in accordance with the EPA 5030/EPA 8260C-2006 and EPA 3510/EPA 8270D-2007 procedures. Other physicochemical analyses were done under standard procedures. It is important to highlight that, during the entire process of preparation and analysis of the samples, a strict security protocol was followed, from the use of a personalized infrastructure and safety equipment such as gas masks, nitrile, and neoprene gloves, to that of a special suit.


### 2.4. Electrochemical Treatment

#### 2.4.1. Selection of the Anode

Morphological, structural, and electrochemical analysis of the different materials evaluated (Ti/IrO2-Ta2O5, Ti/SnO2-Sb, and Ti/BDD) by SEM-EDS, XRD, and CV were done over the same area (2.185 cm2). Ti/IrO2-Ta2O5 and Ti/SnO2-Sb electrodes were synthesized by the thermal deposition method using a special formulation. Polycrystalline boron ((B)=1300 ppm) doped diamond film (Ti/BDD) of 3 μm thickness, provided by Adamant Technologies, was synthesized by hot filament chemical vapor deposition (HF-CVD). The electroactivity of each material was evaluated by CV using a three-electrode cell (60 mL capacity, with a reaction volume of 50 mL). Ti/IrO2-Ta2O5, Ti/SnO2-Sb, and Ti/BDD electrodes (2.185 cm2) were used as anodes, a rod of Ti was used as cathode, and a mercury sulfate electrode (Hg/Hg2SO4/K2SO4 (SAT), E°=0.640 V vs. SHE) was the reference electrode. The temperature was maintained at 298 K and the voltammetric profiles for each electrode were obtained applying a scan rate of 100 mV s−1 using 0.5 M H2SO4 as the supporting electrolyte. Before each analysis, the system was deoxygenated using N2 gas. In this analysis the Ti/BDD was previously activated (to eliminate C-sp2 impurities) developing a special methodology [94]. Ti/IrO2-Ta2O5 and Ti/SnO2-Sb were activated by cycling each electrode (50 cycles, 100 mV s−1 in 0.5 M H2SO4) to stabilize the surface and eliminate impurities.


#### 2.4.2. Selection of the Reaction Medium

Three aspects were taken into account: (i) the pH effect on the chemical state of phenol, (ii) the pH effect on the electrochemical response of the previously selected electrode, and (iii) the pH effect on the production of•OHs. In the first point, analysis by UV-Vis spectroscopy to different pH values was performed with the goal of identifying possible chemical changes on the phenol structure. In this analysis, a synthetic sample was used. The second point was evaluated by the use of CV analyzing two types of acids, HCl and H2SO4 (0.5 M), under the same conditions mentioned above. The last point was evaluated through electrolysis experiments, which were performed applying an anodic potential pulse (2.3 V vs. Hg/Hg2SO4, polarization time of 10 min, use of a Pt mesh as counter electrode, 298 K). This last analysis was performed through the use of fluorescence spectroscopy using coumarin (3 × 10−5M) as a probe compound to give way to the formation of the 7-hydroxycoumarin with a wavelength of maximum excitation and emission of 332 nm and 500 nm, respectively (λex=332 nm, λem=500 nm). During electrolysis, samples of 10 μL were withdrawn every minute and immediately analyzed. The equipment and the cell used for detection of the 7-hydroxycoumarin are shown in Figure 2(a).Figure 2
Experimental system for (a) hydroxyl radicals’ analysis by fluorescence spectroscopy, where (a1)–(a4) are the steps for analysis of 7-hydroxycoumarin, and (b) electrolysis in galvanostatic mode of spent caustics mixture using Ti/BDD: (b1) heat exchanger, (b2) rectifier, and (b3) electrochemical cell.
(a)
(b)


#### 2.4.3. Electrolysis of the Spent Caustic

The electrochemical destruction process of the mixture of spent caustics was done in galvanostatic mode, using the experimental system shown in Figure2(b). In this process, a cell with a single compartment and a capacity of 120 mL (reaction volume of 100 mL, 8 rpm, 298 K and Ti/Pt (3 cm2 as counter electrode)) was used. The area of the anode (prior selection) was 3 cm2. Electrolysis with UV light (λ=254 nm) was done under the same conditions indicated above. In each experiment, representative samples were taken at different reaction times (tr), and the degradation of aromatic compounds (phenol and phenolic compounds) and reaction intermediates was done through TOC and COD analysis.The removal percentages were calculated according to the following formula (3), where Co is the initial concentration (mg L−1) and Cf is the final concentration (mg L−1) [90]: (3)%removal=Co-CfCo*100.The phenol analysis was done using a standard procedure [95], while the toxicity tests were done using a standard method using a lyophilized bacteria,Vibrio Fischeri (Photobacterium phosphoreum), of a luminescent nature, where the reduction of light is proportional to the degree of toxicity.


## 2.1. Chemicals

Sulfuric acid (H2SO4), hydrochloric acid (HCl), NaOH, and phenol (C6H5OH) were obtained from J. T. Baker. K2HPO4, KH2PO4, NH4OH, potassium ferricyanide (K3Fe(CN)6), and 4-aminoantipyrine (C11H13N3O) for analysis of phenol in all of its forms were obtained from Aldrich. Coumarin was obtained from Aldrich. The luminescent marine bacteriaVibrio fischeri(Photobacterium phosphoreum) for toxicity analysis was provided by SDI.


## 2.2. Instruments

Analysis of phenol in all of its forms was carried out through visible ultraviolet spectroscopy (UV-Vis), using a Lambda XLS+ spectrophotometer. COD and TOC were evaluated using a Hach model DR/200 reactor/Uv-Vis spectrophotometer DR/2010 and Shimadzu Model TOC-VCSN equipment, respectively. COD was obtained using HACH products. Toxicity analysis was done using a DeltaTox kit, provided by SDI. Electrolysis using ultraviolet light (λ=254 nm) was done by using a Philips mercury lamp with 11 W. Orion Star A215 equipment was used for pH/ORP/conductivity measurements. The electrolysis experiments in galvanostatic mode were performed using Tektronix PWS4323 equipment. The PTEs analyses were performed using a Perkin Elmer Optima 3300 DV model and an Analyst 200/MHS-15 Perkin Elmer. The first equipment was used for the inductively coupled plasma (ICP) analysis and the second for the Hg analyses by hydride generation. The morphology and element analysis of the different electrodes evaluated during the selection of the best anodic material were obtained using a scanning electron microscope (JEOL JMS-6060LV) equipped with an energy dispersive spectrometer (EDS). Crystal structure analysis using X-ray diffraction (XRD) was carried out in a Rigaku Minifles, using Cu Kα radiation, with a 30 kV operation voltage and 15 mA of current, at a velocity of 2°/min. Cyclic voltammetry (CV) was carried out with an Autolab PGSTAT 30. The •OHs analysis was performed by fluorescence spectroscopy using the equipment HORIBA Jobin MOD Fluorolog 3–22 with double monochromator.


## 2.3. Characterization of the Spent Caustics

### 2.3.1. Sample Preparation

A total of 10 samples (20 L each) of spent caustic were obtained from different refineries and stored at room temperature. From these samples, a composite sample was prepared by combining 1 L of each individual sample. The sample obtained (called mixture) is shown in Figure1(a). This process was carried out using safety equipment (Figure 1(b)) and working under an exhaust hood, which was attached to a gas scrubber containing NaOH (Figure 1(c)).Figure 1
Handling and control of (a) spent caustics mixture, (b) safety equipment, and (c) specialized infrastructure.
(a)
(b)
(c)Before taking each sample, the container was stirred vigorously and the sample was taken immediately. The mixture obtained was also stirred vigorously and stored under refrigeration (4°C) until its analysis.


### 2.3.2. Physicochemical Analysis

Before carrying out any analysis, the container of the mixture of spent caustics was stirred vigorously. The PTEs analysis was done by using inductively coupled plasma atomic emission spectroscopy (ICP-AES), with the exception of Hg, which was analyzed by hydride generation atomic absorption spectroscopy (HGAAS). The analysis was done prior to digestion of the samples. The concentration of anions present was done through ion chromatography according to the EPA method 300.1 (EPA, 1997). This analysis was performed using a high resolution liquid chromatograph Dionex ICS-2500 HPLC/IC fitted with a Dionex IonPac AS14A column and coupled to a conductivity detector (ED50A). The mobile phase was Na2CO3/NaHCO3 (1 mL min−1). The equipment was calibrated using prepared solutions from the 7-Anion Standard of Dionex and the quality of the results was evaluated from the analysis of the certified standard of Inorganic Ventures IC-FAS-1A. The determination of volatile and semivolatile organic compounds (CIDETEQ and Intertek laboratories) in qualitative form was done through gas chromatography mass spectrometry (GC-MS) in accordance with the EPA 5030/EPA 8260C-2006 and EPA 3510/EPA 8270D-2007 procedures. Other physicochemical analyses were done under standard procedures. It is important to highlight that, during the entire process of preparation and analysis of the samples, a strict security protocol was followed, from the use of a personalized infrastructure and safety equipment such as gas masks, nitrile, and neoprene gloves, to that of a special suit.


## 2.3.1. Sample Preparation

A total of 10 samples (20 L each) of spent caustic were obtained from different refineries and stored at room temperature. From these samples, a composite sample was prepared by combining 1 L of each individual sample. The sample obtained (called mixture) is shown in Figure1(a). This process was carried out using safety equipment (Figure 1(b)) and working under an exhaust hood, which was attached to a gas scrubber containing NaOH (Figure 1(c)).Figure 1
Handling and control of (a) spent caustics mixture, (b) safety equipment, and (c) specialized infrastructure.
(a)
(b)
(c)Before taking each sample, the container was stirred vigorously and the sample was taken immediately. The mixture obtained was also stirred vigorously and stored under refrigeration (4°C) until its analysis.


## 2.3.2. Physicochemical Analysis

Before carrying out any analysis, the container of the mixture of spent caustics was stirred vigorously. The PTEs analysis was done by using inductively coupled plasma atomic emission spectroscopy (ICP-AES), with the exception of Hg, which was analyzed by hydride generation atomic absorption spectroscopy (HGAAS). The analysis was done prior to digestion of the samples. The concentration of anions present was done through ion chromatography according to the EPA method 300.1 (EPA, 1997). This analysis was performed using a high resolution liquid chromatograph Dionex ICS-2500 HPLC/IC fitted with a Dionex IonPac AS14A column and coupled to a conductivity detector (ED50A). The mobile phase was Na2CO3/NaHCO3 (1 mL min−1). The equipment was calibrated using prepared solutions from the 7-Anion Standard of Dionex and the quality of the results was evaluated from the analysis of the certified standard of Inorganic Ventures IC-FAS-1A. The determination of volatile and semivolatile organic compounds (CIDETEQ and Intertek laboratories) in qualitative form was done through gas chromatography mass spectrometry (GC-MS) in accordance with the EPA 5030/EPA 8260C-2006 and EPA 3510/EPA 8270D-2007 procedures. Other physicochemical analyses were done under standard procedures. It is important to highlight that, during the entire process of preparation and analysis of the samples, a strict security protocol was followed, from the use of a personalized infrastructure and safety equipment such as gas masks, nitrile, and neoprene gloves, to that of a special suit.


## 2.4. Electrochemical Treatment

### 2.4.1. Selection of the Anode

Morphological, structural, and electrochemical analysis of the different materials evaluated (Ti/IrO2-Ta2O5, Ti/SnO2-Sb, and Ti/BDD) by SEM-EDS, XRD, and CV were done over the same area (2.185 cm2). Ti/IrO2-Ta2O5 and Ti/SnO2-Sb electrodes were synthesized by the thermal deposition method using a special formulation. Polycrystalline boron ((B)=1300 ppm) doped diamond film (Ti/BDD) of 3 μm thickness, provided by Adamant Technologies, was synthesized by hot filament chemical vapor deposition (HF-CVD). The electroactivity of each material was evaluated by CV using a three-electrode cell (60 mL capacity, with a reaction volume of 50 mL). Ti/IrO2-Ta2O5, Ti/SnO2-Sb, and Ti/BDD electrodes (2.185 cm2) were used as anodes, a rod of Ti was used as cathode, and a mercury sulfate electrode (Hg/Hg2SO4/K2SO4 (SAT), E°=0.640 V vs. SHE) was the reference electrode. The temperature was maintained at 298 K and the voltammetric profiles for each electrode were obtained applying a scan rate of 100 mV s−1 using 0.5 M H2SO4 as the supporting electrolyte. Before each analysis, the system was deoxygenated using N2 gas. In this analysis the Ti/BDD was previously activated (to eliminate C-sp2 impurities) developing a special methodology [94]. Ti/IrO2-Ta2O5 and Ti/SnO2-Sb were activated by cycling each electrode (50 cycles, 100 mV s−1 in 0.5 M H2SO4) to stabilize the surface and eliminate impurities.


### 2.4.2. Selection of the Reaction Medium

Three aspects were taken into account: (i) the pH effect on the chemical state of phenol, (ii) the pH effect on the electrochemical response of the previously selected electrode, and (iii) the pH effect on the production of•OHs. In the first point, analysis by UV-Vis spectroscopy to different pH values was performed with the goal of identifying possible chemical changes on the phenol structure. In this analysis, a synthetic sample was used. The second point was evaluated by the use of CV analyzing two types of acids, HCl and H2SO4 (0.5 M), under the same conditions mentioned above. The last point was evaluated through electrolysis experiments, which were performed applying an anodic potential pulse (2.3 V vs. Hg/Hg2SO4, polarization time of 10 min, use of a Pt mesh as counter electrode, 298 K). This last analysis was performed through the use of fluorescence spectroscopy using coumarin (3 × 10−5M) as a probe compound to give way to the formation of the 7-hydroxycoumarin with a wavelength of maximum excitation and emission of 332 nm and 500 nm, respectively (λex=332 nm, λem=500 nm). During electrolysis, samples of 10 μL were withdrawn every minute and immediately analyzed. The equipment and the cell used for detection of the 7-hydroxycoumarin are shown in Figure 2(a).Figure 2
Experimental system for (a) hydroxyl radicals’ analysis by fluorescence spectroscopy, where (a1)–(a4) are the steps for analysis of 7-hydroxycoumarin, and (b) electrolysis in galvanostatic mode of spent caustics mixture using Ti/BDD: (b1) heat exchanger, (b2) rectifier, and (b3) electrochemical cell.
(a)
(b)


### 2.4.3. Electrolysis of the Spent Caustic

The electrochemical destruction process of the mixture of spent caustics was done in galvanostatic mode, using the experimental system shown in Figure2(b). In this process, a cell with a single compartment and a capacity of 120 mL (reaction volume of 100 mL, 8 rpm, 298 K and Ti/Pt (3 cm2 as counter electrode)) was used. The area of the anode (prior selection) was 3 cm2. Electrolysis with UV light (λ=254 nm) was done under the same conditions indicated above. In each experiment, representative samples were taken at different reaction times (tr), and the degradation of aromatic compounds (phenol and phenolic compounds) and reaction intermediates was done through TOC and COD analysis.The removal percentages were calculated according to the following formula (3), where Co is the initial concentration (mg L−1) and Cf is the final concentration (mg L−1) [90]: (3)%removal=Co-CfCo*100.The phenol analysis was done using a standard procedure [95], while the toxicity tests were done using a standard method using a lyophilized bacteria,Vibrio Fischeri (Photobacterium phosphoreum), of a luminescent nature, where the reduction of light is proportional to the degree of toxicity.


## 2.4.1. Selection of the Anode

Morphological, structural, and electrochemical analysis of the different materials evaluated (Ti/IrO2-Ta2O5, Ti/SnO2-Sb, and Ti/BDD) by SEM-EDS, XRD, and CV were done over the same area (2.185 cm2). Ti/IrO2-Ta2O5 and Ti/SnO2-Sb electrodes were synthesized by the thermal deposition method using a special formulation. Polycrystalline boron ((B)=1300 ppm) doped diamond film (Ti/BDD) of 3 μm thickness, provided by Adamant Technologies, was synthesized by hot filament chemical vapor deposition (HF-CVD). The electroactivity of each material was evaluated by CV using a three-electrode cell (60 mL capacity, with a reaction volume of 50 mL). Ti/IrO2-Ta2O5, Ti/SnO2-Sb, and Ti/BDD electrodes (2.185 cm2) were used as anodes, a rod of Ti was used as cathode, and a mercury sulfate electrode (Hg/Hg2SO4/K2SO4 (SAT), E°=0.640 V vs. SHE) was the reference electrode. The temperature was maintained at 298 K and the voltammetric profiles for each electrode were obtained applying a scan rate of 100 mV s−1 using 0.5 M H2SO4 as the supporting electrolyte. Before each analysis, the system was deoxygenated using N2 gas. In this analysis the Ti/BDD was previously activated (to eliminate C-sp2 impurities) developing a special methodology [94]. Ti/IrO2-Ta2O5 and Ti/SnO2-Sb were activated by cycling each electrode (50 cycles, 100 mV s−1 in 0.5 M H2SO4) to stabilize the surface and eliminate impurities.


## 2.4.2. Selection of the Reaction Medium

Three aspects were taken into account: (i) the pH effect on the chemical state of phenol, (ii) the pH effect on the electrochemical response of the previously selected electrode, and (iii) the pH effect on the production of•OHs. In the first point, analysis by UV-Vis spectroscopy to different pH values was performed with the goal of identifying possible chemical changes on the phenol structure. In this analysis, a synthetic sample was used. The second point was evaluated by the use of CV analyzing two types of acids, HCl and H2SO4 (0.5 M), under the same conditions mentioned above. The last point was evaluated through electrolysis experiments, which were performed applying an anodic potential pulse (2.3 V vs. Hg/Hg2SO4, polarization time of 10 min, use of a Pt mesh as counter electrode, 298 K). This last analysis was performed through the use of fluorescence spectroscopy using coumarin (3 × 10−5M) as a probe compound to give way to the formation of the 7-hydroxycoumarin with a wavelength of maximum excitation and emission of 332 nm and 500 nm, respectively (λex=332 nm, λem=500 nm). During electrolysis, samples of 10 μL were withdrawn every minute and immediately analyzed. The equipment and the cell used for detection of the 7-hydroxycoumarin are shown in Figure 2(a).Figure 2
Experimental system for (a) hydroxyl radicals’ analysis by fluorescence spectroscopy, where (a1)–(a4) are the steps for analysis of 7-hydroxycoumarin, and (b) electrolysis in galvanostatic mode of spent caustics mixture using Ti/BDD: (b1) heat exchanger, (b2) rectifier, and (b3) electrochemical cell.
(a)
(b)


## 2.4.3. Electrolysis of the Spent Caustic

The electrochemical destruction process of the mixture of spent caustics was done in galvanostatic mode, using the experimental system shown in Figure2(b). In this process, a cell with a single compartment and a capacity of 120 mL (reaction volume of 100 mL, 8 rpm, 298 K and Ti/Pt (3 cm2 as counter electrode)) was used. The area of the anode (prior selection) was 3 cm2. Electrolysis with UV light (λ=254 nm) was done under the same conditions indicated above. In each experiment, representative samples were taken at different reaction times (tr), and the degradation of aromatic compounds (phenol and phenolic compounds) and reaction intermediates was done through TOC and COD analysis.The removal percentages were calculated according to the following formula (3), where Co is the initial concentration (mg L−1) and Cf is the final concentration (mg L−1) [90]: (3)%removal=Co-CfCo*100.The phenol analysis was done using a standard procedure [95], while the toxicity tests were done using a standard method using a lyophilized bacteria,Vibrio Fischeri (Photobacterium phosphoreum), of a luminescent nature, where the reduction of light is proportional to the degree of toxicity.


## 3. Results

### 3.1. Characterization of the Spent Caustics

#### 3.1.1. Physicochemical Analysis

Table1 shows the results obtained in the physicochemical characterization of the sample corresponding to the mixture of spent caustics (mixture of 10 samples). Comparatively, it shows the analysis of a simple sample, corresponding to the sample of greater toxicity (preliminary evaluation of the phenolic content), including the reported values in the literature for spent caustics as well as for wastewater from refineries [1, 3, 7, 9, 13, 16–19, 96–98].Table 1
Physicochemical analysis of spent caustics.
Parameter
Value
Value reference
Simple sample
Mixture
Spent caustic
Typical refinery wastewater
Total phenol (mg L−1)
7,270.89
11,041.74
30,600 [3]
13 [16], 172.50 [18], 3.17 [17], 192.90 [9], 141 [7], 113 [19], 23 [96]
Oil and grease (mg L−1)
239.70
3,399.70
—
85 [97], 1.96 [17], 12.70 [19], 15 [98]
BOD5 (mg L−1)
6,930
7,811
—
323 [97], 40.25 [16], 570 [3]
COD (mg O2 L−1)
72,065
98,750–102,842.50
72,450 [1], 320,100 [3]
3,150 [97], 100 [16], 4,450 [18], 2,323 [13], 257 [17], 590 [9], 602 [7], 935 [19], 2,746 [98], 1,220 [96]
BOD5/COD
0.09
0.07
—
0.60 [19]
Sulfides (mg L−1)
<37.29
<37.29
34,517 [1], 48,500 [3]
19 [19]
Ammonia (mg L−1)
—
—
—
13.10 [19]
Cyanides (mg L−1)
<0.25
<0.25
—
—
pH
13.02
13.50
12.97 [1], 13 [3]
8 [16], 8.60 [18], 8.05 [13], 7.60 [17], 9.20 [7], 8.10 [19], 7.59 [98], 10 [96]
TOC (mg L−1)
—
20,137.50
53,900 [3]
370 [19], 1,500 [96]
Hydrocarbons (mg L−1)
—
—
—
11.72 [17], 0.02 [19]
Conductivity (mS cm−1)
129.20
208.44
126.70 [1]
6 [18], 13.06 [13], 15.63 [7], 1.73 [7], 0.06 [98]
Alkalinity, CaCO3 (mg L−1)
52,266.35
—
15,500 [3]
3,990 [96]
Total dissolved solid (mg L−1)
—
169,680
—
5,000 [18], 7,990 [13], 1,333 [7], 4,380 [98]
Settleable solids(mg L−1)
—
40
—
—
Total suspended solids(mg L−1)
—
3,940
—
22.80 [16], 35 [18], 100 [13], 1,000 [96]
Toxicity (%)
100
100
—
—
F− (mg L−1)
50
135
—
—
Cl− (mg L−1)
86
54,900
37,900 [3]
63 [97], 112 [7], 200,000 [96]
Br− (mg L−1)
12
<0.30
—
—
NO
3
- (mg L−1)
11
<0.25
—
—
P
O
4
3
- (mg L−1)
381
<0.30
4,600 [3]
—
SO
4
2
- (mg L−1)
608
1,882
20,300 [3]
1,054.50 [13], 212 [7], 1,650 [96]
ORP (mV)
−334.20
—
—
—
Turbidity (NTU)
—
—
—
6.10 [16], 37 [17], 37 [19]The analysis of the mixture showed a phenolic content of 11,041.74 mg L−1, while the simple sample showed a content of 7,270.89 mg L−1. The difference between both samples clearly demonstrates the environmental problem that commonly appears in the hydrocarbon industry. That is to say, residues of low or high toxicity are mixed with each other, resulting in a residue of greater toxicity. Here, the phenol concentration, organic load, and dissolved solids are not comparable with any other residue, including wastewater from different refining processes [90]. The phenol concentration in the samples analyzed suggest that this residue cannot be treated by BO (a concentration >3,000 mg L−1 leads to the complete deactivation of the microorganisms). This is confirmed by the result obtained in the toxicity tests (100% toxic) and through the analysis of the BOD5/COD = 0.09 and 0.07 for the simple sample and the sample corresponding to the mixture, respectively. On the other hand, the elevated alkalinity (52,266.35 mg L−1) and an elevated pH (13–13.5) reflect the reducing nature of these residues, which should be considered in the treatment to be chosen. Many of the contaminants can be fixed at an alkaline pH and be liberated under oxidizing conditions. The reactivity analysis for sulphides and cyanides showed values below the detection limit (<37.29 and <0.25 mg L−1, resp.). Based on the results obtained in this phase of characterization, the samples evaluated were classified as cresylic spent caustics.


#### 3.1.2. Ion Analysis

The analysis of anions, done through ion chromatography, in the case of the simple sample, showed a low content of chlorides (Cl−) and sulfates (SO4-2) with values of 86 and 608 mg L−1, respectively, with their concentration being much higher in the mixture, with values of 54,900 and 1,882 mg L−1, respectively. It is necessary to mention that in this case the presence of chlorides is very important. The chlorides, while they can give rise to the presence of compounds of greater toxicity, can also exert a synergic effect during an EO process, giving way to the formation of different oxidizing species [99, 100].


#### 3.1.3. Analysis of Volatile and Semivolatile Organic Compounds

An analysis through GC-MS, corresponding to the mixture of spent caustics, was carried out to determine the different phenolic compounds (reflected in the analysis of phenol in all of its forms, Table1). Different compounds were considered, of which 43 were for volatile and 62 for semivolatile analysis. The results showed only the presence of 2,4-dimethylphenol, phenol, m-methylphenol, p-methylphenol, and o-methylphenol, all highly toxic compounds. Figure 3 shows the representative chemical structures of each compound identified.Figure 3
Chemical structure of the main phenolic compounds identified by GC-MS in the spent caustics mixture: (a) 2,4-dimethylphenol, (b) phenol, (c) m-methylphenol, (d) p-methylphenol, and (e) o-methylphenol.
(a)
(b)
(c)
(d)
(e)At the same time, a PTEs analysis through ICP was carried out, taking into account that the physicochemical composition of the mixture of spent caustics includes PTEs and possible catalyst traces used in the different processes of hydrocarbon refining. The selection of each PTE was based on an extensive bibliography review. Table2 shows the main PTEs identified in the mixture sample. In this analysis, a high amount of Na+ and Fe with values of 19,148 mg L−1 and 1,323 mg L−1, respectively, was identified. The presence of Na+ confirms the caustic nature of the sample, while the presence of Fe, though it is not an especially toxic element, is commonly controlled by the effect of turbidity caused by the precipitation of oxides and hydroxides. The analysis of Fe was done taking into account its catalytic activity on H2O2, to give way for the •OH through the Fenton reaction [90]. Due to this, the presence of Fe could be used to accelerate the mineralization process and decrease the residence times during the EO process.Table 2
Analysis of PTEs in spent caustics mixture.
MLA (mg L−1) in rivers
PTE (mg L−1)
Agricultural irrigation (A)
Public-urban (B)
Protection of aquatic life (C)
p.d
p.m
p.d
p.m
p.d
p.m
Al
15.46
—
—
—
—
—
—
As
<0.098
0.2
0.4
0.1
0.2
0.1
0.2
Cd
<0.114
0.2
0.4
0.1
0.2
0.1
0.2
Co
2.42
—
—
—
—
—
—
Cu*
6.89
4.0
6.0
4.0
6.0
4.0
6.0
Cr*
1.95
1.0
1.5
0.5
1.0
0.5
1.0
Fe
1,323
—
—
—
—
—
—
Mn
7.23
—
—
—
—
—
—
Ca
148.87
—
—
—
—
—
—
Mg
34
—
—
—
—
—
—
Na
19,148
—
—
—
—
—
—
Hg*
0.07
0.01
0.02
0.005
0.01
0.005
0.01
Ni*
6.75
2
4
2
4
2
4
Pb*
1.23
0.5
1
0.2
0.4
0.2
0.4
Zn
4.68
10
20
10
10
20
10
V
0.24
—
—
—
—
—
—
MLA = maximum limits allowed; p.d = per day; p.m = per month.
*Values that exceed the established MLA under Mexican Regulation.On the other hand, PTEs like As and Cd remained under the detection limit (<0.098 and <0.114 mg L−1, resp.), while Cu, Cr, Hg, Ni, and Pb exceeded the maximum limits allowed under the Mexican Regulation [101]. It is important to highlight the elevated toxicity of said elements and, specially, that of the Hg [102, 103] and Pb, which have the ability to enter into the food chains and to concentrate in organisms (magnification process). Considering these analyses, the elevated toxicity of the spent caustics is confirmed, thus justifying the need to direct efforts towards their treatment and/or destruction.


### 3.2. Electrochemical Treatment

#### 3.2.1. Selection of the Anode

Morphology, elemental composition, crystal structure, and electrochemical analysis. The results corresponding to these analyses are shown in Figure4. The morphology of metal oxide coatings (Ti/IrO2-Ta2O5 and Ti/SnO2-Sb) (Figures 4(a) and 4(b), resp.) showed smaller cracks in comparison with Ti/BDD (Figure 4(c)). The latter showed a compact structure, demonstrating the quality of the coating and the adherence of the diamond to the titanium substrate. In parallel, X-ray dot-mapping was used to analyze the distribution of coating elements.Figure 4
SEM analysis. (a) Ti/IrO2-Ta2O5. (b) Ti/SnO2-Sb. (c) Ti/BDD, applying 15 kV with its respective micrographies and X-ray dot-mapping analysis, identifying: (a1) Ir, (a2) Ta, (b1) Sn, (c1) B, and (c2) C. (d) Cyclic voltammetry analysis for (d1) Ti/IrO2-Ta2O5, (d2) Ti/SnO2-Sb, and (d3) Ti/BDD in 0.5 M H2SO4.This analysis showed a uniform distribution of Ir (a1), Ta (a2), Sn (b1), B (c1), and C (c2). However, the Sb, in the case of Ti/SnO2-Sb, was not detected. The absence of Sb was probably due to the additive ratio in the coating solution. To verify its presence, an XRD analysis was done demonstrating the presence of SnO2, Sb2O3, and Sb2O5. For this specific reason, pretreatment of this electrode was performed before the cyclic voltammetric analysis. At the same time, for both materials (Ti/IrO2-Ta2O5 and Ti/SnO2-Sb), the wt% of each element was obtained by EDS. In this analysis, the presence of additional elements such as O, Ti, and Si was detected. The results of these analyses (XRD and EDS) have been omitted due to the formulation used. In the case of Ti/BDD, an exhaustive characterization was performed in other studies [94]. The electrochemical characterization of each electrode by CV is shown in Figure 4(d). It shows a comparative analysis of Ti/IrO2-Ta2O5 (d1), Ti/SnO2-Sb (d2), and Ti/BDD (d3), in 0.5 M H2SO4. This graph shows that Ti/BDD has the highest potential window in comparison to Ti/IrO2-Ta2O5 and Ti/SnO2-Sb. An elevated ηO2 is important taking into account that the oxidation reaction of the organic compounds during the EO occurs in parallel to the evolution of O2. Using a material with a high ηO2, the oxidation reaction is favored over the evolution of O2, resulting in high current efficiencies. Based on this, it was decided that Ti/BDD was the best material to use in the electrochemical treatment of spent caustic.


#### 3.2.2. Selection of the Reaction Medium

To carry out the electrochemical destruction of the spent caustics using Ti/BDD, the selection of the reaction medium was done taking into account the following approaches: (i) the pH effect on the chemical state of phenol, (ii) the pH effect on the Ti/BDD’s electrochemical response, and (iii) the pH effect on•OHs production. According to the first approach, in an extremely alkaline environment (pH 13–13.5, Table 1), the phenol is chemically transformed into sodium phenolates [90]. Although the electronic state of phenol in an alkaline medium has been shown to be favorable for an EO process using electrodes with a low ηO2 [28], this does not occur using BDD, where the most degradation efficiency is obtained using an acidic medium [90]. Frequently, in literature, different types of acids have been reported for the EO of phenol, such as HClO4 [63, 104] and HNO3 [105]; however, for a possible industrial application, the costs of said acids must be considered. For this reason and considering that during the ion analysis a high quantity of chlorides (54,900 mg L−1) and sulfates (1,882 mg L−1) was identified as part of the chemical composition of the spent caustics mixture, HCl and H2SO4 were selected as possible acids to carry out the pH adjustment (13, 13.5 to 1). Initially, the acidification process was evaluated using a synthetic sample in order to rule out any chemical change that occurred on the phenol molecule during the acidification process and to avoid an overestimation of the subsequent results. In said analysis, a solution of 0.05 M NaOH containing phenol 30 mg L−1 (TOC) was adjusted to different pH values in an interval of 12–1, using 0.5 M HCl and H2SO4. The changes that occurred during the acidification process were evaluated through UV-Vis spectroscopy. Figure 5 shows the different UV-Vis absorption spectrums obtained during the adjustment of the pH using H2SO4 (Figure 5(a)) and HCl (Figure 5(b)). It is clearly observed that the chemical conversion of sodium phenolates to phenol (λ=270 nm) is obtained with both types of acids at a pH of 9, reaching the maximum conversion efficiency at a pH of 7.Figure 5
UV-Vis analysis of the pH effect on the chemical state of phenol, using 30 mg L−1 of TOC in (a) 0.05 M NaOH/H2SO4 (pH 12–1), (b) 0.05 M NaOH/HCl (pH 12–1), and (c) ORP analysis under the same conditions to 298 K.
(a)
(b)
(c)There were no additional and significant chemical changes observed. In parallel to this measurement, an analysis of the redox potential (ORP) was carried out at 298 K. The result of this analysis is shown in Figure5(c). The values obtained clearly show that an acidic pH favors highly oxidizing conditions, which is of high importance considering that, albeit, an acidic environment does not alter the chemical structure of phenol, the contaminants associated with the spent caustics can be liberated, whereby, a specialized infrastructure and safety equipment are necessary. Using H2SO4, a slight increase in the ORP was observed in comparison with HCl, which is logical considering a greater number of protons. To evaluate the second approach (effect of the pH on the electrochemical response of the Ti/BDD), different voltammograms were obtained through the adjustment of 0.05 M NaOH with 0.5 H2SO4 and HCl in a pH range of 12–1 (data not shown). It was observed that when the pH values descended to acidic, the ηO2 increased considerably [106]. When comparing the window of potential of H2SO4 with that of HCl (pH 1) (Figure 6(a)), a difference in overpotential of 0.5 V was obtained. Considering these results and according to the third approach (pH effect on •OHs production), an analysis of the generation of the •OHs was carried out in both reaction mediums (pH 1). Figure 6(b) shows the influence of the reaction medium on the production of •OHs. It is clearly observed that the production of •OHs is greater in NaOH/H2SO4 (pH 1).Figure 6
Electrochemical characterization of Ti/BDD by cyclic voltammetric analysis using (a1) 0.05 M NaOH/HCl (pH 1) and (a2) 0.05 M NaOH/H2SO4 (pH 1). (b) •OHs analysis by fluorescence spectroscopy using (b1) 0.05 M NaOH/HCl (pH 1) and (b2) 0.05 M NaOH/H2SO4 (pH 1). (c) Selection of the current density using synthetic solutions of phenol (30 mg L−1 of TOC) in 0.05 NaOH/H2SO4 (pH 1).
(a)
(b)
(c)This result is of great importance considering that, with the use of a BDD electrode, the formation of any oxidizing species produced in parallel to the oxidation of organic compounds is strictly dependent on the formation of the•OHs. Based on this result, H2SO4 was selected to carry out the acidification process.


#### 3.2.3. Electrolysis Using Ti/BDD

Before performing the degradation experiments, a preliminary analysis using a synthetic solution with a phenol concentration of 30 mg L−1 of TOC was carried out in NaOH/H2SO4 (pH 1) with the goal of identifying the current to be applied. The currents evaluated were 0.24, 0.48, 0.72, 0.96, 1.20, and 1.44 A, for a 2-hour period, under constant stirring. Ti/BDD (3 cm2) was used as anode and Ti/Pt (3 cm2) was used as counter-electrode. It was observed that the middle point of the removal was reached at 0.96 A (j=0.32 A cm−2), as shown in Figure 6(c). After having identified the current to be applied and before carrying out electrolysis of the spent caustics mixture, a preliminary electrolysis was performed using a simple sample (Table 1). The conditions of electrolysis were j=0.32 A cm−2, pH 1 (adjustment with H2SO4). In this analysis, the effect of ultraviolet light was considered for the purpose of favoring the synergic effect on the production of the •OH. It has been reported that, in the presence of chlorides, the use of ultraviolet light (λ=254 nm) can lead to the production of the •OH, according to the reaction (4):(4)HOCl+hν⟶OH•+Cl•Figure7 shows the degradation profiles (TOC and COD) obtained in the different analyses done in the presence and absence of UV light (λ=254 nm).Figure 7
Evaluation of the use of UV light (λ=254 nm). Removal of COD and TOC in spent caustic corresponding to the simple sample using Ti/BDD, applying 0.96 A (j=0.32 A cm−2), under constant stirring, pH 1 (adjustment with H2SO4) and tr=12 h. Images of (a) in the absence of UV light, (b) in the presence of UV light (λ=254 nm), and (c) photolysis.The results obtained in electrolysis in the absence of light were more satisfactory than those obtained in its presence (λ=254 nm). The results obtained can be attributed to the type of sample analyzed. A real sample is not comparable to a synthetic sample. Here, it is inferred that, due to the high content of organic material, oxidation processes, different from those that occurred in the interface or by the action of the oxidants themselves, are not significant. When analyzing the effect of UV light (λ=254 nm), without applying a current (photolysis), no significant change was observed.Figure8 shows the analysis of images obtained during the different electrolysis carried out.Figure 8
Images of electrolysis of spent caustic corresponding to the simple sample. (a) In the absence of UV light. (b) In the presence of UV light (λ=254 nm). (c) Photolysis, using Ti/BDD, applying 0.96 A (j=0.32 A cm−2), under constant stirring, pH 1 (adjustment with H2SO4) and tr=12 h.
(a)
(b)
(c)The initial image (tr=0 h) corresponds to the simple sample submitted to a special pretreatment before electrolysis (acidification to pH 1 using H2SO4). A dark brown color in the first stages of the phenol electrolysis is related to the formation of byproducts such as benzoquinone and hydroquinone, known as an active redox couple in equilibrium in an aqueous solution [51]. The color degradation in each experiment was gradual. When comparing each image (tr=8 h), it is clearly observed that, in electrolysis carried out in the absence of light (Figure 8(a)), the sample turned completely crystalline, indicating a high level of destruction of the organic content. Contrarily, in electrolysis in the presence of light (λ=254 nm) (Figure 8(b)) and in photolysis experiments (Figure 8(c)), the opposite process was observed. In the presence of light (λ=254 nm), the degradation time to obtain a visually crystalline sample was greater (tr=12 h). Based on these results, the use of UV light (λ=254 nm) was discarded. On the other hand and considering the results obtained, the possible passivation of Ti/BDD as an important point was also evaluated. In this analysis, the •OHs production was performed in function of the interfacial potential or current applied. The result (data not shown) indicates that these species only are generated in the zone corresponding to the decomposition of the medium, whereby, if the domains of the potential or current applied are not the correct ones, the electrode can be completely passivated. The image analysis of this test is shown in Figure 9. As can be observed (Figure 9(a)), when working with a current, where the production of the •OHs does not occur, a thick layer of organic compounds is deposited, causing the deactivation of the electrode.Figure 9
Electrochemical treatment of spent caustics mixture. (a) Applying a current where the•OHs are not generated. (b) Applying a current where the •OHs are generated. (c) Electrolyzed sample (without pretreatment). (d) Sample obtained after the electrochemical treatment with Ti/BDD applying 0.96 A (j=0.32 A cm−2), under constant stirring, pH 1 (adjustment with H2SO4) and tr=15 h.
(a)
(b)
(c)
(d)Contrarily, when the current is applied, inducing a greater interfacial potential by which•OHs are electrogenerated, the Ti/BDD electrode can be operated successfully (Figure 9(b)). Finally and according to the previous studies, the electrolysis of the mixture (100 mL) of spent caustics was carried out (pH 1/H2SO4, j=0.32 A cm−2). The results obtained in this analysis are shown in Table 3. The results obtained were similar to those from electrolysis of the simple sample.Table 3
Electrochemical treatment of spent caustics (mixture) using Ti/BDD.
Sample
COD(mg L−1)
COD removal (%)
Total removal efficiency, WT-ET (%)
TOC(mg L−1)
TOC removal (%)
Total removal efficiency, WT-ET (%)
Without treatment (WT)
98,750
0
—
20,137.5
0
0
Chemical treatment (CT)*
24,533
75.15
—
15,700
22.03
—
Electrochemical treatment (ET)
2,333
90.40
96.63
2,322
85.21
88.46
*Acidification to pH 1 using H2SO4.The analysis of the image of the sample corresponding to the mixture of spent caustics before and after the electrochemical treatment with Ti/BDD (tr=15 h) is shown in Figures 9(c) and 9(d), respectively. Complementary analyses of toxicity and phenol in all of its forms showed that the sample electrochemically treated is not toxic, presenting a low phenol content (<3 ppm), with this value being the minimum standard discharge limit for refinery effluents [107].


## 3.1. Characterization of the Spent Caustics

### 3.1.1. Physicochemical Analysis

Table1 shows the results obtained in the physicochemical characterization of the sample corresponding to the mixture of spent caustics (mixture of 10 samples). Comparatively, it shows the analysis of a simple sample, corresponding to the sample of greater toxicity (preliminary evaluation of the phenolic content), including the reported values in the literature for spent caustics as well as for wastewater from refineries [1, 3, 7, 9, 13, 16–19, 96–98].Table 1
Physicochemical analysis of spent caustics.
Parameter
Value
Value reference
Simple sample
Mixture
Spent caustic
Typical refinery wastewater
Total phenol (mg L−1)
7,270.89
11,041.74
30,600 [3]
13 [16], 172.50 [18], 3.17 [17], 192.90 [9], 141 [7], 113 [19], 23 [96]
Oil and grease (mg L−1)
239.70
3,399.70
—
85 [97], 1.96 [17], 12.70 [19], 15 [98]
BOD5 (mg L−1)
6,930
7,811
—
323 [97], 40.25 [16], 570 [3]
COD (mg O2 L−1)
72,065
98,750–102,842.50
72,450 [1], 320,100 [3]
3,150 [97], 100 [16], 4,450 [18], 2,323 [13], 257 [17], 590 [9], 602 [7], 935 [19], 2,746 [98], 1,220 [96]
BOD5/COD
0.09
0.07
—
0.60 [19]
Sulfides (mg L−1)
<37.29
<37.29
34,517 [1], 48,500 [3]
19 [19]
Ammonia (mg L−1)
—
—
—
13.10 [19]
Cyanides (mg L−1)
<0.25
<0.25
—
—
pH
13.02
13.50
12.97 [1], 13 [3]
8 [16], 8.60 [18], 8.05 [13], 7.60 [17], 9.20 [7], 8.10 [19], 7.59 [98], 10 [96]
TOC (mg L−1)
—
20,137.50
53,900 [3]
370 [19], 1,500 [96]
Hydrocarbons (mg L−1)
—
—
—
11.72 [17], 0.02 [19]
Conductivity (mS cm−1)
129.20
208.44
126.70 [1]
6 [18], 13.06 [13], 15.63 [7], 1.73 [7], 0.06 [98]
Alkalinity, CaCO3 (mg L−1)
52,266.35
—
15,500 [3]
3,990 [96]
Total dissolved solid (mg L−1)
—
169,680
—
5,000 [18], 7,990 [13], 1,333 [7], 4,380 [98]
Settleable solids(mg L−1)
—
40
—
—
Total suspended solids(mg L−1)
—
3,940
—
22.80 [16], 35 [18], 100 [13], 1,000 [96]
Toxicity (%)
100
100
—
—
F− (mg L−1)
50
135
—
—
Cl− (mg L−1)
86
54,900
37,900 [3]
63 [97], 112 [7], 200,000 [96]
Br− (mg L−1)
12
<0.30
—
—
NO
3
- (mg L−1)
11
<0.25
—
—
P
O
4
3
- (mg L−1)
381
<0.30
4,600 [3]
—
SO
4
2
- (mg L−1)
608
1,882
20,300 [3]
1,054.50 [13], 212 [7], 1,650 [96]
ORP (mV)
−334.20
—
—
—
Turbidity (NTU)
—
—
—
6.10 [16], 37 [17], 37 [19]The analysis of the mixture showed a phenolic content of 11,041.74 mg L−1, while the simple sample showed a content of 7,270.89 mg L−1. The difference between both samples clearly demonstrates the environmental problem that commonly appears in the hydrocarbon industry. That is to say, residues of low or high toxicity are mixed with each other, resulting in a residue of greater toxicity. Here, the phenol concentration, organic load, and dissolved solids are not comparable with any other residue, including wastewater from different refining processes [90]. The phenol concentration in the samples analyzed suggest that this residue cannot be treated by BO (a concentration >3,000 mg L−1 leads to the complete deactivation of the microorganisms). This is confirmed by the result obtained in the toxicity tests (100% toxic) and through the analysis of the BOD5/COD = 0.09 and 0.07 for the simple sample and the sample corresponding to the mixture, respectively. On the other hand, the elevated alkalinity (52,266.35 mg L−1) and an elevated pH (13–13.5) reflect the reducing nature of these residues, which should be considered in the treatment to be chosen. Many of the contaminants can be fixed at an alkaline pH and be liberated under oxidizing conditions. The reactivity analysis for sulphides and cyanides showed values below the detection limit (<37.29 and <0.25 mg L−1, resp.). Based on the results obtained in this phase of characterization, the samples evaluated were classified as cresylic spent caustics.


### 3.1.2. Ion Analysis

The analysis of anions, done through ion chromatography, in the case of the simple sample, showed a low content of chlorides (Cl−) and sulfates (SO4-2) with values of 86 and 608 mg L−1, respectively, with their concentration being much higher in the mixture, with values of 54,900 and 1,882 mg L−1, respectively. It is necessary to mention that in this case the presence of chlorides is very important. The chlorides, while they can give rise to the presence of compounds of greater toxicity, can also exert a synergic effect during an EO process, giving way to the formation of different oxidizing species [99, 100].


### 3.1.3. Analysis of Volatile and Semivolatile Organic Compounds

An analysis through GC-MS, corresponding to the mixture of spent caustics, was carried out to determine the different phenolic compounds (reflected in the analysis of phenol in all of its forms, Table1). Different compounds were considered, of which 43 were for volatile and 62 for semivolatile analysis. The results showed only the presence of 2,4-dimethylphenol, phenol, m-methylphenol, p-methylphenol, and o-methylphenol, all highly toxic compounds. Figure 3 shows the representative chemical structures of each compound identified.Figure 3
Chemical structure of the main phenolic compounds identified by GC-MS in the spent caustics mixture: (a) 2,4-dimethylphenol, (b) phenol, (c) m-methylphenol, (d) p-methylphenol, and (e) o-methylphenol.
(a)
(b)
(c)
(d)
(e)At the same time, a PTEs analysis through ICP was carried out, taking into account that the physicochemical composition of the mixture of spent caustics includes PTEs and possible catalyst traces used in the different processes of hydrocarbon refining. The selection of each PTE was based on an extensive bibliography review. Table2 shows the main PTEs identified in the mixture sample. In this analysis, a high amount of Na+ and Fe with values of 19,148 mg L−1 and 1,323 mg L−1, respectively, was identified. The presence of Na+ confirms the caustic nature of the sample, while the presence of Fe, though it is not an especially toxic element, is commonly controlled by the effect of turbidity caused by the precipitation of oxides and hydroxides. The analysis of Fe was done taking into account its catalytic activity on H2O2, to give way for the •OH through the Fenton reaction [90]. Due to this, the presence of Fe could be used to accelerate the mineralization process and decrease the residence times during the EO process.Table 2
Analysis of PTEs in spent caustics mixture.
MLA (mg L−1) in rivers
PTE (mg L−1)
Agricultural irrigation (A)
Public-urban (B)
Protection of aquatic life (C)
p.d
p.m
p.d
p.m
p.d
p.m
Al
15.46
—
—
—
—
—
—
As
<0.098
0.2
0.4
0.1
0.2
0.1
0.2
Cd
<0.114
0.2
0.4
0.1
0.2
0.1
0.2
Co
2.42
—
—
—
—
—
—
Cu*
6.89
4.0
6.0
4.0
6.0
4.0
6.0
Cr*
1.95
1.0
1.5
0.5
1.0
0.5
1.0
Fe
1,323
—
—
—
—
—
—
Mn
7.23
—
—
—
—
—
—
Ca
148.87
—
—
—
—
—
—
Mg
34
—
—
—
—
—
—
Na
19,148
—
—
—
—
—
—
Hg*
0.07
0.01
0.02
0.005
0.01
0.005
0.01
Ni*
6.75
2
4
2
4
2
4
Pb*
1.23
0.5
1
0.2
0.4
0.2
0.4
Zn
4.68
10
20
10
10
20
10
V
0.24
—
—
—
—
—
—
MLA = maximum limits allowed; p.d = per day; p.m = per month.
*Values that exceed the established MLA under Mexican Regulation.On the other hand, PTEs like As and Cd remained under the detection limit (<0.098 and <0.114 mg L−1, resp.), while Cu, Cr, Hg, Ni, and Pb exceeded the maximum limits allowed under the Mexican Regulation [101]. It is important to highlight the elevated toxicity of said elements and, specially, that of the Hg [102, 103] and Pb, which have the ability to enter into the food chains and to concentrate in organisms (magnification process). Considering these analyses, the elevated toxicity of the spent caustics is confirmed, thus justifying the need to direct efforts towards their treatment and/or destruction.


## 3.1.1. Physicochemical Analysis

Table1 shows the results obtained in the physicochemical characterization of the sample corresponding to the mixture of spent caustics (mixture of 10 samples). Comparatively, it shows the analysis of a simple sample, corresponding to the sample of greater toxicity (preliminary evaluation of the phenolic content), including the reported values in the literature for spent caustics as well as for wastewater from refineries [1, 3, 7, 9, 13, 16–19, 96–98].Table 1
Physicochemical analysis of spent caustics.
Parameter
Value
Value reference
Simple sample
Mixture
Spent caustic
Typical refinery wastewater
Total phenol (mg L−1)
7,270.89
11,041.74
30,600 [3]
13 [16], 172.50 [18], 3.17 [17], 192.90 [9], 141 [7], 113 [19], 23 [96]
Oil and grease (mg L−1)
239.70
3,399.70
—
85 [97], 1.96 [17], 12.70 [19], 15 [98]
BOD5 (mg L−1)
6,930
7,811
—
323 [97], 40.25 [16], 570 [3]
COD (mg O2 L−1)
72,065
98,750–102,842.50
72,450 [1], 320,100 [3]
3,150 [97], 100 [16], 4,450 [18], 2,323 [13], 257 [17], 590 [9], 602 [7], 935 [19], 2,746 [98], 1,220 [96]
BOD5/COD
0.09
0.07
—
0.60 [19]
Sulfides (mg L−1)
<37.29
<37.29
34,517 [1], 48,500 [3]
19 [19]
Ammonia (mg L−1)
—
—
—
13.10 [19]
Cyanides (mg L−1)
<0.25
<0.25
—
—
pH
13.02
13.50
12.97 [1], 13 [3]
8 [16], 8.60 [18], 8.05 [13], 7.60 [17], 9.20 [7], 8.10 [19], 7.59 [98], 10 [96]
TOC (mg L−1)
—
20,137.50
53,900 [3]
370 [19], 1,500 [96]
Hydrocarbons (mg L−1)
—
—
—
11.72 [17], 0.02 [19]
Conductivity (mS cm−1)
129.20
208.44
126.70 [1]
6 [18], 13.06 [13], 15.63 [7], 1.73 [7], 0.06 [98]
Alkalinity, CaCO3 (mg L−1)
52,266.35
—
15,500 [3]
3,990 [96]
Total dissolved solid (mg L−1)
—
169,680
—
5,000 [18], 7,990 [13], 1,333 [7], 4,380 [98]
Settleable solids(mg L−1)
—
40
—
—
Total suspended solids(mg L−1)
—
3,940
—
22.80 [16], 35 [18], 100 [13], 1,000 [96]
Toxicity (%)
100
100
—
—
F− (mg L−1)
50
135
—
—
Cl− (mg L−1)
86
54,900
37,900 [3]
63 [97], 112 [7], 200,000 [96]
Br− (mg L−1)
12
<0.30
—
—
NO
3
- (mg L−1)
11
<0.25
—
—
P
O
4
3
- (mg L−1)
381
<0.30
4,600 [3]
—
SO
4
2
- (mg L−1)
608
1,882
20,300 [3]
1,054.50 [13], 212 [7], 1,650 [96]
ORP (mV)
−334.20
—
—
—
Turbidity (NTU)
—
—
—
6.10 [16], 37 [17], 37 [19]The analysis of the mixture showed a phenolic content of 11,041.74 mg L−1, while the simple sample showed a content of 7,270.89 mg L−1. The difference between both samples clearly demonstrates the environmental problem that commonly appears in the hydrocarbon industry. That is to say, residues of low or high toxicity are mixed with each other, resulting in a residue of greater toxicity. Here, the phenol concentration, organic load, and dissolved solids are not comparable with any other residue, including wastewater from different refining processes [90]. The phenol concentration in the samples analyzed suggest that this residue cannot be treated by BO (a concentration >3,000 mg L−1 leads to the complete deactivation of the microorganisms). This is confirmed by the result obtained in the toxicity tests (100% toxic) and through the analysis of the BOD5/COD = 0.09 and 0.07 for the simple sample and the sample corresponding to the mixture, respectively. On the other hand, the elevated alkalinity (52,266.35 mg L−1) and an elevated pH (13–13.5) reflect the reducing nature of these residues, which should be considered in the treatment to be chosen. Many of the contaminants can be fixed at an alkaline pH and be liberated under oxidizing conditions. The reactivity analysis for sulphides and cyanides showed values below the detection limit (<37.29 and <0.25 mg L−1, resp.). Based on the results obtained in this phase of characterization, the samples evaluated were classified as cresylic spent caustics.


## 3.1.2. Ion Analysis

The analysis of anions, done through ion chromatography, in the case of the simple sample, showed a low content of chlorides (Cl−) and sulfates (SO4-2) with values of 86 and 608 mg L−1, respectively, with their concentration being much higher in the mixture, with values of 54,900 and 1,882 mg L−1, respectively. It is necessary to mention that in this case the presence of chlorides is very important. The chlorides, while they can give rise to the presence of compounds of greater toxicity, can also exert a synergic effect during an EO process, giving way to the formation of different oxidizing species [99, 100].


## 3.1.3. Analysis of Volatile and Semivolatile Organic Compounds

An analysis through GC-MS, corresponding to the mixture of spent caustics, was carried out to determine the different phenolic compounds (reflected in the analysis of phenol in all of its forms, Table1). Different compounds were considered, of which 43 were for volatile and 62 for semivolatile analysis. The results showed only the presence of 2,4-dimethylphenol, phenol, m-methylphenol, p-methylphenol, and o-methylphenol, all highly toxic compounds. Figure 3 shows the representative chemical structures of each compound identified.Figure 3
Chemical structure of the main phenolic compounds identified by GC-MS in the spent caustics mixture: (a) 2,4-dimethylphenol, (b) phenol, (c) m-methylphenol, (d) p-methylphenol, and (e) o-methylphenol.
(a)
(b)
(c)
(d)
(e)At the same time, a PTEs analysis through ICP was carried out, taking into account that the physicochemical composition of the mixture of spent caustics includes PTEs and possible catalyst traces used in the different processes of hydrocarbon refining. The selection of each PTE was based on an extensive bibliography review. Table2 shows the main PTEs identified in the mixture sample. In this analysis, a high amount of Na+ and Fe with values of 19,148 mg L−1 and 1,323 mg L−1, respectively, was identified. The presence of Na+ confirms the caustic nature of the sample, while the presence of Fe, though it is not an especially toxic element, is commonly controlled by the effect of turbidity caused by the precipitation of oxides and hydroxides. The analysis of Fe was done taking into account its catalytic activity on H2O2, to give way for the •OH through the Fenton reaction [90]. Due to this, the presence of Fe could be used to accelerate the mineralization process and decrease the residence times during the EO process.Table 2
Analysis of PTEs in spent caustics mixture.
MLA (mg L−1) in rivers
PTE (mg L−1)
Agricultural irrigation (A)
Public-urban (B)
Protection of aquatic life (C)
p.d
p.m
p.d
p.m
p.d
p.m
Al
15.46
—
—
—
—
—
—
As
<0.098
0.2
0.4
0.1
0.2
0.1
0.2
Cd
<0.114
0.2
0.4
0.1
0.2
0.1
0.2
Co
2.42
—
—
—
—
—
—
Cu*
6.89
4.0
6.0
4.0
6.0
4.0
6.0
Cr*
1.95
1.0
1.5
0.5
1.0
0.5
1.0
Fe
1,323
—
—
—
—
—
—
Mn
7.23
—
—
—
—
—
—
Ca
148.87
—
—
—
—
—
—
Mg
34
—
—
—
—
—
—
Na
19,148
—
—
—
—
—
—
Hg*
0.07
0.01
0.02
0.005
0.01
0.005
0.01
Ni*
6.75
2
4
2
4
2
4
Pb*
1.23
0.5
1
0.2
0.4
0.2
0.4
Zn
4.68
10
20
10
10
20
10
V
0.24
—
—
—
—
—
—
MLA = maximum limits allowed; p.d = per day; p.m = per month.
*Values that exceed the established MLA under Mexican Regulation.On the other hand, PTEs like As and Cd remained under the detection limit (<0.098 and <0.114 mg L−1, resp.), while Cu, Cr, Hg, Ni, and Pb exceeded the maximum limits allowed under the Mexican Regulation [101]. It is important to highlight the elevated toxicity of said elements and, specially, that of the Hg [102, 103] and Pb, which have the ability to enter into the food chains and to concentrate in organisms (magnification process). Considering these analyses, the elevated toxicity of the spent caustics is confirmed, thus justifying the need to direct efforts towards their treatment and/or destruction.


## 3.2. Electrochemical Treatment

### 3.2.1. Selection of the Anode

Morphology, elemental composition, crystal structure, and electrochemical analysis. The results corresponding to these analyses are shown in Figure4. The morphology of metal oxide coatings (Ti/IrO2-Ta2O5 and Ti/SnO2-Sb) (Figures 4(a) and 4(b), resp.) showed smaller cracks in comparison with Ti/BDD (Figure 4(c)). The latter showed a compact structure, demonstrating the quality of the coating and the adherence of the diamond to the titanium substrate. In parallel, X-ray dot-mapping was used to analyze the distribution of coating elements.Figure 4
SEM analysis. (a) Ti/IrO2-Ta2O5. (b) Ti/SnO2-Sb. (c) Ti/BDD, applying 15 kV with its respective micrographies and X-ray dot-mapping analysis, identifying: (a1) Ir, (a2) Ta, (b1) Sn, (c1) B, and (c2) C. (d) Cyclic voltammetry analysis for (d1) Ti/IrO2-Ta2O5, (d2) Ti/SnO2-Sb, and (d3) Ti/BDD in 0.5 M H2SO4.This analysis showed a uniform distribution of Ir (a1), Ta (a2), Sn (b1), B (c1), and C (c2). However, the Sb, in the case of Ti/SnO2-Sb, was not detected. The absence of Sb was probably due to the additive ratio in the coating solution. To verify its presence, an XRD analysis was done demonstrating the presence of SnO2, Sb2O3, and Sb2O5. For this specific reason, pretreatment of this electrode was performed before the cyclic voltammetric analysis. At the same time, for both materials (Ti/IrO2-Ta2O5 and Ti/SnO2-Sb), the wt% of each element was obtained by EDS. In this analysis, the presence of additional elements such as O, Ti, and Si was detected. The results of these analyses (XRD and EDS) have been omitted due to the formulation used. In the case of Ti/BDD, an exhaustive characterization was performed in other studies [94]. The electrochemical characterization of each electrode by CV is shown in Figure 4(d). It shows a comparative analysis of Ti/IrO2-Ta2O5 (d1), Ti/SnO2-Sb (d2), and Ti/BDD (d3), in 0.5 M H2SO4. This graph shows that Ti/BDD has the highest potential window in comparison to Ti/IrO2-Ta2O5 and Ti/SnO2-Sb. An elevated ηO2 is important taking into account that the oxidation reaction of the organic compounds during the EO occurs in parallel to the evolution of O2. Using a material with a high ηO2, the oxidation reaction is favored over the evolution of O2, resulting in high current efficiencies. Based on this, it was decided that Ti/BDD was the best material to use in the electrochemical treatment of spent caustic.


### 3.2.2. Selection of the Reaction Medium

To carry out the electrochemical destruction of the spent caustics using Ti/BDD, the selection of the reaction medium was done taking into account the following approaches: (i) the pH effect on the chemical state of phenol, (ii) the pH effect on the Ti/BDD’s electrochemical response, and (iii) the pH effect on•OHs production. According to the first approach, in an extremely alkaline environment (pH 13–13.5, Table 1), the phenol is chemically transformed into sodium phenolates [90]. Although the electronic state of phenol in an alkaline medium has been shown to be favorable for an EO process using electrodes with a low ηO2 [28], this does not occur using BDD, where the most degradation efficiency is obtained using an acidic medium [90]. Frequently, in literature, different types of acids have been reported for the EO of phenol, such as HClO4 [63, 104] and HNO3 [105]; however, for a possible industrial application, the costs of said acids must be considered. For this reason and considering that during the ion analysis a high quantity of chlorides (54,900 mg L−1) and sulfates (1,882 mg L−1) was identified as part of the chemical composition of the spent caustics mixture, HCl and H2SO4 were selected as possible acids to carry out the pH adjustment (13, 13.5 to 1). Initially, the acidification process was evaluated using a synthetic sample in order to rule out any chemical change that occurred on the phenol molecule during the acidification process and to avoid an overestimation of the subsequent results. In said analysis, a solution of 0.05 M NaOH containing phenol 30 mg L−1 (TOC) was adjusted to different pH values in an interval of 12–1, using 0.5 M HCl and H2SO4. The changes that occurred during the acidification process were evaluated through UV-Vis spectroscopy. Figure 5 shows the different UV-Vis absorption spectrums obtained during the adjustment of the pH using H2SO4 (Figure 5(a)) and HCl (Figure 5(b)). It is clearly observed that the chemical conversion of sodium phenolates to phenol (λ=270 nm) is obtained with both types of acids at a pH of 9, reaching the maximum conversion efficiency at a pH of 7.Figure 5
UV-Vis analysis of the pH effect on the chemical state of phenol, using 30 mg L−1 of TOC in (a) 0.05 M NaOH/H2SO4 (pH 12–1), (b) 0.05 M NaOH/HCl (pH 12–1), and (c) ORP analysis under the same conditions to 298 K.
(a)
(b)
(c)There were no additional and significant chemical changes observed. In parallel to this measurement, an analysis of the redox potential (ORP) was carried out at 298 K. The result of this analysis is shown in Figure5(c). The values obtained clearly show that an acidic pH favors highly oxidizing conditions, which is of high importance considering that, albeit, an acidic environment does not alter the chemical structure of phenol, the contaminants associated with the spent caustics can be liberated, whereby, a specialized infrastructure and safety equipment are necessary. Using H2SO4, a slight increase in the ORP was observed in comparison with HCl, which is logical considering a greater number of protons. To evaluate the second approach (effect of the pH on the electrochemical response of the Ti/BDD), different voltammograms were obtained through the adjustment of 0.05 M NaOH with 0.5 H2SO4 and HCl in a pH range of 12–1 (data not shown). It was observed that when the pH values descended to acidic, the ηO2 increased considerably [106]. When comparing the window of potential of H2SO4 with that of HCl (pH 1) (Figure 6(a)), a difference in overpotential of 0.5 V was obtained. Considering these results and according to the third approach (pH effect on •OHs production), an analysis of the generation of the •OHs was carried out in both reaction mediums (pH 1). Figure 6(b) shows the influence of the reaction medium on the production of •OHs. It is clearly observed that the production of •OHs is greater in NaOH/H2SO4 (pH 1).Figure 6
Electrochemical characterization of Ti/BDD by cyclic voltammetric analysis using (a1) 0.05 M NaOH/HCl (pH 1) and (a2) 0.05 M NaOH/H2SO4 (pH 1). (b) •OHs analysis by fluorescence spectroscopy using (b1) 0.05 M NaOH/HCl (pH 1) and (b2) 0.05 M NaOH/H2SO4 (pH 1). (c) Selection of the current density using synthetic solutions of phenol (30 mg L−1 of TOC) in 0.05 NaOH/H2SO4 (pH 1).
(a)
(b)
(c)This result is of great importance considering that, with the use of a BDD electrode, the formation of any oxidizing species produced in parallel to the oxidation of organic compounds is strictly dependent on the formation of the•OHs. Based on this result, H2SO4 was selected to carry out the acidification process.


### 3.2.3. Electrolysis Using Ti/BDD

Before performing the degradation experiments, a preliminary analysis using a synthetic solution with a phenol concentration of 30 mg L−1 of TOC was carried out in NaOH/H2SO4 (pH 1) with the goal of identifying the current to be applied. The currents evaluated were 0.24, 0.48, 0.72, 0.96, 1.20, and 1.44 A, for a 2-hour period, under constant stirring. Ti/BDD (3 cm2) was used as anode and Ti/Pt (3 cm2) was used as counter-electrode. It was observed that the middle point of the removal was reached at 0.96 A (j=0.32 A cm−2), as shown in Figure 6(c). After having identified the current to be applied and before carrying out electrolysis of the spent caustics mixture, a preliminary electrolysis was performed using a simple sample (Table 1). The conditions of electrolysis were j=0.32 A cm−2, pH 1 (adjustment with H2SO4). In this analysis, the effect of ultraviolet light was considered for the purpose of favoring the synergic effect on the production of the •OH. It has been reported that, in the presence of chlorides, the use of ultraviolet light (λ=254 nm) can lead to the production of the •OH, according to the reaction (4):(4)HOCl+hν⟶OH•+Cl•Figure7 shows the degradation profiles (TOC and COD) obtained in the different analyses done in the presence and absence of UV light (λ=254 nm).Figure 7
Evaluation of the use of UV light (λ=254 nm). Removal of COD and TOC in spent caustic corresponding to the simple sample using Ti/BDD, applying 0.96 A (j=0.32 A cm−2), under constant stirring, pH 1 (adjustment with H2SO4) and tr=12 h. Images of (a) in the absence of UV light, (b) in the presence of UV light (λ=254 nm), and (c) photolysis.The results obtained in electrolysis in the absence of light were more satisfactory than those obtained in its presence (λ=254 nm). The results obtained can be attributed to the type of sample analyzed. A real sample is not comparable to a synthetic sample. Here, it is inferred that, due to the high content of organic material, oxidation processes, different from those that occurred in the interface or by the action of the oxidants themselves, are not significant. When analyzing the effect of UV light (λ=254 nm), without applying a current (photolysis), no significant change was observed.Figure8 shows the analysis of images obtained during the different electrolysis carried out.Figure 8
Images of electrolysis of spent caustic corresponding to the simple sample. (a) In the absence of UV light. (b) In the presence of UV light (λ=254 nm). (c) Photolysis, using Ti/BDD, applying 0.96 A (j=0.32 A cm−2), under constant stirring, pH 1 (adjustment with H2SO4) and tr=12 h.
(a)
(b)
(c)The initial image (tr=0 h) corresponds to the simple sample submitted to a special pretreatment before electrolysis (acidification to pH 1 using H2SO4). A dark brown color in the first stages of the phenol electrolysis is related to the formation of byproducts such as benzoquinone and hydroquinone, known as an active redox couple in equilibrium in an aqueous solution [51]. The color degradation in each experiment was gradual. When comparing each image (tr=8 h), it is clearly observed that, in electrolysis carried out in the absence of light (Figure 8(a)), the sample turned completely crystalline, indicating a high level of destruction of the organic content. Contrarily, in electrolysis in the presence of light (λ=254 nm) (Figure 8(b)) and in photolysis experiments (Figure 8(c)), the opposite process was observed. In the presence of light (λ=254 nm), the degradation time to obtain a visually crystalline sample was greater (tr=12 h). Based on these results, the use of UV light (λ=254 nm) was discarded. On the other hand and considering the results obtained, the possible passivation of Ti/BDD as an important point was also evaluated. In this analysis, the •OHs production was performed in function of the interfacial potential or current applied. The result (data not shown) indicates that these species only are generated in the zone corresponding to the decomposition of the medium, whereby, if the domains of the potential or current applied are not the correct ones, the electrode can be completely passivated. The image analysis of this test is shown in Figure 9. As can be observed (Figure 9(a)), when working with a current, where the production of the •OHs does not occur, a thick layer of organic compounds is deposited, causing the deactivation of the electrode.Figure 9
Electrochemical treatment of spent caustics mixture. (a) Applying a current where the•OHs are not generated. (b) Applying a current where the •OHs are generated. (c) Electrolyzed sample (without pretreatment). (d) Sample obtained after the electrochemical treatment with Ti/BDD applying 0.96 A (j=0.32 A cm−2), under constant stirring, pH 1 (adjustment with H2SO4) and tr=15 h.
(a)
(b)
(c)
(d)Contrarily, when the current is applied, inducing a greater interfacial potential by which•OHs are electrogenerated, the Ti/BDD electrode can be operated successfully (Figure 9(b)). Finally and according to the previous studies, the electrolysis of the mixture (100 mL) of spent caustics was carried out (pH 1/H2SO4, j=0.32 A cm−2). The results obtained in this analysis are shown in Table 3. The results obtained were similar to those from electrolysis of the simple sample.Table 3
Electrochemical treatment of spent caustics (mixture) using Ti/BDD.
Sample
COD(mg L−1)
COD removal (%)
Total removal efficiency, WT-ET (%)
TOC(mg L−1)
TOC removal (%)
Total removal efficiency, WT-ET (%)
Without treatment (WT)
98,750
0
—
20,137.5
0
0
Chemical treatment (CT)*
24,533
75.15
—
15,700
22.03
—
Electrochemical treatment (ET)
2,333
90.40
96.63
2,322
85.21
88.46
*Acidification to pH 1 using H2SO4.The analysis of the image of the sample corresponding to the mixture of spent caustics before and after the electrochemical treatment with Ti/BDD (tr=15 h) is shown in Figures 9(c) and 9(d), respectively. Complementary analyses of toxicity and phenol in all of its forms showed that the sample electrochemically treated is not toxic, presenting a low phenol content (<3 ppm), with this value being the minimum standard discharge limit for refinery effluents [107].


## 3.2.1. Selection of the Anode

Morphology, elemental composition, crystal structure, and electrochemical analysis. The results corresponding to these analyses are shown in Figure4. The morphology of metal oxide coatings (Ti/IrO2-Ta2O5 and Ti/SnO2-Sb) (Figures 4(a) and 4(b), resp.) showed smaller cracks in comparison with Ti/BDD (Figure 4(c)). The latter showed a compact structure, demonstrating the quality of the coating and the adherence of the diamond to the titanium substrate. In parallel, X-ray dot-mapping was used to analyze the distribution of coating elements.Figure 4
SEM analysis. (a) Ti/IrO2-Ta2O5. (b) Ti/SnO2-Sb. (c) Ti/BDD, applying 15 kV with its respective micrographies and X-ray dot-mapping analysis, identifying: (a1) Ir, (a2) Ta, (b1) Sn, (c1) B, and (c2) C. (d) Cyclic voltammetry analysis for (d1) Ti/IrO2-Ta2O5, (d2) Ti/SnO2-Sb, and (d3) Ti/BDD in 0.5 M H2SO4.This analysis showed a uniform distribution of Ir (a1), Ta (a2), Sn (b1), B (c1), and C (c2). However, the Sb, in the case of Ti/SnO2-Sb, was not detected. The absence of Sb was probably due to the additive ratio in the coating solution. To verify its presence, an XRD analysis was done demonstrating the presence of SnO2, Sb2O3, and Sb2O5. For this specific reason, pretreatment of this electrode was performed before the cyclic voltammetric analysis. At the same time, for both materials (Ti/IrO2-Ta2O5 and Ti/SnO2-Sb), the wt% of each element was obtained by EDS. In this analysis, the presence of additional elements such as O, Ti, and Si was detected. The results of these analyses (XRD and EDS) have been omitted due to the formulation used. In the case of Ti/BDD, an exhaustive characterization was performed in other studies [94]. The electrochemical characterization of each electrode by CV is shown in Figure 4(d). It shows a comparative analysis of Ti/IrO2-Ta2O5 (d1), Ti/SnO2-Sb (d2), and Ti/BDD (d3), in 0.5 M H2SO4. This graph shows that Ti/BDD has the highest potential window in comparison to Ti/IrO2-Ta2O5 and Ti/SnO2-Sb. An elevated ηO2 is important taking into account that the oxidation reaction of the organic compounds during the EO occurs in parallel to the evolution of O2. Using a material with a high ηO2, the oxidation reaction is favored over the evolution of O2, resulting in high current efficiencies. Based on this, it was decided that Ti/BDD was the best material to use in the electrochemical treatment of spent caustic.


## 3.2.2. Selection of the Reaction Medium

To carry out the electrochemical destruction of the spent caustics using Ti/BDD, the selection of the reaction medium was done taking into account the following approaches: (i) the pH effect on the chemical state of phenol, (ii) the pH effect on the Ti/BDD’s electrochemical response, and (iii) the pH effect on•OHs production. According to the first approach, in an extremely alkaline environment (pH 13–13.5, Table 1), the phenol is chemically transformed into sodium phenolates [90]. Although the electronic state of phenol in an alkaline medium has been shown to be favorable for an EO process using electrodes with a low ηO2 [28], this does not occur using BDD, where the most degradation efficiency is obtained using an acidic medium [90]. Frequently, in literature, different types of acids have been reported for the EO of phenol, such as HClO4 [63, 104] and HNO3 [105]; however, for a possible industrial application, the costs of said acids must be considered. For this reason and considering that during the ion analysis a high quantity of chlorides (54,900 mg L−1) and sulfates (1,882 mg L−1) was identified as part of the chemical composition of the spent caustics mixture, HCl and H2SO4 were selected as possible acids to carry out the pH adjustment (13, 13.5 to 1). Initially, the acidification process was evaluated using a synthetic sample in order to rule out any chemical change that occurred on the phenol molecule during the acidification process and to avoid an overestimation of the subsequent results. In said analysis, a solution of 0.05 M NaOH containing phenol 30 mg L−1 (TOC) was adjusted to different pH values in an interval of 12–1, using 0.5 M HCl and H2SO4. The changes that occurred during the acidification process were evaluated through UV-Vis spectroscopy. Figure 5 shows the different UV-Vis absorption spectrums obtained during the adjustment of the pH using H2SO4 (Figure 5(a)) and HCl (Figure 5(b)). It is clearly observed that the chemical conversion of sodium phenolates to phenol (λ=270 nm) is obtained with both types of acids at a pH of 9, reaching the maximum conversion efficiency at a pH of 7.Figure 5
UV-Vis analysis of the pH effect on the chemical state of phenol, using 30 mg L−1 of TOC in (a) 0.05 M NaOH/H2SO4 (pH 12–1), (b) 0.05 M NaOH/HCl (pH 12–1), and (c) ORP analysis under the same conditions to 298 K.
(a)
(b)
(c)There were no additional and significant chemical changes observed. In parallel to this measurement, an analysis of the redox potential (ORP) was carried out at 298 K. The result of this analysis is shown in Figure5(c). The values obtained clearly show that an acidic pH favors highly oxidizing conditions, which is of high importance considering that, albeit, an acidic environment does not alter the chemical structure of phenol, the contaminants associated with the spent caustics can be liberated, whereby, a specialized infrastructure and safety equipment are necessary. Using H2SO4, a slight increase in the ORP was observed in comparison with HCl, which is logical considering a greater number of protons. To evaluate the second approach (effect of the pH on the electrochemical response of the Ti/BDD), different voltammograms were obtained through the adjustment of 0.05 M NaOH with 0.5 H2SO4 and HCl in a pH range of 12–1 (data not shown). It was observed that when the pH values descended to acidic, the ηO2 increased considerably [106]. When comparing the window of potential of H2SO4 with that of HCl (pH 1) (Figure 6(a)), a difference in overpotential of 0.5 V was obtained. Considering these results and according to the third approach (pH effect on •OHs production), an analysis of the generation of the •OHs was carried out in both reaction mediums (pH 1). Figure 6(b) shows the influence of the reaction medium on the production of •OHs. It is clearly observed that the production of •OHs is greater in NaOH/H2SO4 (pH 1).Figure 6
Electrochemical characterization of Ti/BDD by cyclic voltammetric analysis using (a1) 0.05 M NaOH/HCl (pH 1) and (a2) 0.05 M NaOH/H2SO4 (pH 1). (b) •OHs analysis by fluorescence spectroscopy using (b1) 0.05 M NaOH/HCl (pH 1) and (b2) 0.05 M NaOH/H2SO4 (pH 1). (c) Selection of the current density using synthetic solutions of phenol (30 mg L−1 of TOC) in 0.05 NaOH/H2SO4 (pH 1).
(a)
(b)
(c)This result is of great importance considering that, with the use of a BDD electrode, the formation of any oxidizing species produced in parallel to the oxidation of organic compounds is strictly dependent on the formation of the•OHs. Based on this result, H2SO4 was selected to carry out the acidification process.


## 3.2.3. Electrolysis Using Ti/BDD

Before performing the degradation experiments, a preliminary analysis using a synthetic solution with a phenol concentration of 30 mg L−1 of TOC was carried out in NaOH/H2SO4 (pH 1) with the goal of identifying the current to be applied. The currents evaluated were 0.24, 0.48, 0.72, 0.96, 1.20, and 1.44 A, for a 2-hour period, under constant stirring. Ti/BDD (3 cm2) was used as anode and Ti/Pt (3 cm2) was used as counter-electrode. It was observed that the middle point of the removal was reached at 0.96 A (j=0.32 A cm−2), as shown in Figure 6(c). After having identified the current to be applied and before carrying out electrolysis of the spent caustics mixture, a preliminary electrolysis was performed using a simple sample (Table 1). The conditions of electrolysis were j=0.32 A cm−2, pH 1 (adjustment with H2SO4). In this analysis, the effect of ultraviolet light was considered for the purpose of favoring the synergic effect on the production of the •OH. It has been reported that, in the presence of chlorides, the use of ultraviolet light (λ=254 nm) can lead to the production of the •OH, according to the reaction (4):(4)HOCl+hν⟶OH•+Cl•Figure7 shows the degradation profiles (TOC and COD) obtained in the different analyses done in the presence and absence of UV light (λ=254 nm).Figure 7
Evaluation of the use of UV light (λ=254 nm). Removal of COD and TOC in spent caustic corresponding to the simple sample using Ti/BDD, applying 0.96 A (j=0.32 A cm−2), under constant stirring, pH 1 (adjustment with H2SO4) and tr=12 h. Images of (a) in the absence of UV light, (b) in the presence of UV light (λ=254 nm), and (c) photolysis.The results obtained in electrolysis in the absence of light were more satisfactory than those obtained in its presence (λ=254 nm). The results obtained can be attributed to the type of sample analyzed. A real sample is not comparable to a synthetic sample. Here, it is inferred that, due to the high content of organic material, oxidation processes, different from those that occurred in the interface or by the action of the oxidants themselves, are not significant. When analyzing the effect of UV light (λ=254 nm), without applying a current (photolysis), no significant change was observed.Figure8 shows the analysis of images obtained during the different electrolysis carried out.Figure 8
Images of electrolysis of spent caustic corresponding to the simple sample. (a) In the absence of UV light. (b) In the presence of UV light (λ=254 nm). (c) Photolysis, using Ti/BDD, applying 0.96 A (j=0.32 A cm−2), under constant stirring, pH 1 (adjustment with H2SO4) and tr=12 h.
(a)
(b)
(c)The initial image (tr=0 h) corresponds to the simple sample submitted to a special pretreatment before electrolysis (acidification to pH 1 using H2SO4). A dark brown color in the first stages of the phenol electrolysis is related to the formation of byproducts such as benzoquinone and hydroquinone, known as an active redox couple in equilibrium in an aqueous solution [51]. The color degradation in each experiment was gradual. When comparing each image (tr=8 h), it is clearly observed that, in electrolysis carried out in the absence of light (Figure 8(a)), the sample turned completely crystalline, indicating a high level of destruction of the organic content. Contrarily, in electrolysis in the presence of light (λ=254 nm) (Figure 8(b)) and in photolysis experiments (Figure 8(c)), the opposite process was observed. In the presence of light (λ=254 nm), the degradation time to obtain a visually crystalline sample was greater (tr=12 h). Based on these results, the use of UV light (λ=254 nm) was discarded. On the other hand and considering the results obtained, the possible passivation of Ti/BDD as an important point was also evaluated. In this analysis, the •OHs production was performed in function of the interfacial potential or current applied. The result (data not shown) indicates that these species only are generated in the zone corresponding to the decomposition of the medium, whereby, if the domains of the potential or current applied are not the correct ones, the electrode can be completely passivated. The image analysis of this test is shown in Figure 9. As can be observed (Figure 9(a)), when working with a current, where the production of the •OHs does not occur, a thick layer of organic compounds is deposited, causing the deactivation of the electrode.Figure 9
Electrochemical treatment of spent caustics mixture. (a) Applying a current where the•OHs are not generated. (b) Applying a current where the •OHs are generated. (c) Electrolyzed sample (without pretreatment). (d) Sample obtained after the electrochemical treatment with Ti/BDD applying 0.96 A (j=0.32 A cm−2), under constant stirring, pH 1 (adjustment with H2SO4) and tr=15 h.
(a)
(b)
(c)
(d)Contrarily, when the current is applied, inducing a greater interfacial potential by which•OHs are electrogenerated, the Ti/BDD electrode can be operated successfully (Figure 9(b)). Finally and according to the previous studies, the electrolysis of the mixture (100 mL) of spent caustics was carried out (pH 1/H2SO4, j=0.32 A cm−2). The results obtained in this analysis are shown in Table 3. The results obtained were similar to those from electrolysis of the simple sample.Table 3
Electrochemical treatment of spent caustics (mixture) using Ti/BDD.
Sample
COD(mg L−1)
COD removal (%)
Total removal efficiency, WT-ET (%)
TOC(mg L−1)
TOC removal (%)
Total removal efficiency, WT-ET (%)
Without treatment (WT)
98,750
0
—
20,137.5
0
0
Chemical treatment (CT)*
24,533
75.15
—
15,700
22.03
—
Electrochemical treatment (ET)
2,333
90.40
96.63
2,322
85.21
88.46
*Acidification to pH 1 using H2SO4.The analysis of the image of the sample corresponding to the mixture of spent caustics before and after the electrochemical treatment with Ti/BDD (tr=15 h) is shown in Figures 9(c) and 9(d), respectively. Complementary analyses of toxicity and phenol in all of its forms showed that the sample electrochemically treated is not toxic, presenting a low phenol content (<3 ppm), with this value being the minimum standard discharge limit for refinery effluents [107].


## 4. Conclusions

A greater production of the•OH was obtained by using H2SO4 as a reaction medium. The degradation of spent caustics in an acidic medium (H2SO4, pH 1) using Ti/BDD in simple samples proceeded at 100%, while for the mixture, percentages of destruction of 90.40% and 85.21% for COD and TOC, respectively, were obtained. The use of UV light (λ=254 nm) did not show an improvement of the process. Further studies are necessary to improve the efficiencies obtained.



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*Source: 829136-2015-08-25.xml*