Archina Buthiyappan,
Abdul Aziz Abdul Raman* and
Wan Mohd Ashri Wan Daud
Department of Chemical Engineering, Faculty of Engineering, University of Malaya, 50603 Kuala Lumpur, Malaysia. E-mail: azizraman@um.edu.my; Fax: +60 3 79675319; Tel: +60 3 79675300
First published on 1st March 2016
The batik industry is operated as a cottage industry due to variation in the designs and demand of batik. Batik is considered an art. However, the batik industry consumes a large volume of water and produces a large amount of wastewater that contains grease, resin, surfactants, wax, suspended solids and dyes. Hence, this industry requires treatment systems, which are inexpensive, simple, safe to operate, energy efficient, do not require skilled workers and do not produce secondary pollutants. In this regard, AOPs characterized by the production of highly reactive radicals, which are able to degrade most of the recalcitrant organic pollutants, have been found to fulfil the requirement. The Fenton process is one of the low-cost, low-footprint, simple and less complicated AOPs that can be used to treat effluent that has a high COD. At the optimal conditions (room temperature, undiluted contaminants), 81.4% COD, 70.5% TOC and 99.6% color removal were obtained within an hour by the Fenton process. The samples were analyzed using FTIR, GC-MS and HPLC, which confirmed the superiority of the Fenton process. The GC/MS analysis revealed that the Fenton process successfully removed 71% of organic compounds. Sludge characterization by SEM and particle size distribution showed that the Fenton generated sludge achieved suitable disposal qualities.
Among the treatment techniques that have been investigated to reduce the organic contaminants to a safe and acceptable state, Advanced Oxidation Processes (AOPs) have the potential to treat wastewater contaminated with toxic and biorefractory organic compounds. Fenton oxidations, photocatalysis, UV/H2O2, sonolysis and ozonation are the most commonly used AOPs techniques.7–16 In this context, Fenton oxidation has been proposed as a promising alternative technology for the batik wastewater treatment at room temperature and pressure, particularly for the degradation of non-biodegradable and toxic components to H2O, CO2 and inorganics.17–20 Fenton system is effective in degrading various recalcitrant compounds by using highly oxidative hydroxyl radicals and rapid oxidation kinetics with a cheap and easily maintained operating system.16,21–23 It should be noted that very limited studies have been conducted on the Fenton reaction using real wastewater. Torrades and García-Montaño (2014) are among the few researchers who have conducted such studies. They have investigated the use of Fenton reagent and UV-irradiation for treating real dye wastewater from a Spanish textile manufacturer in one of their studies at laboratory scale and reported that 120 min of treatment resulted in a 62.9% and 76.3% reduction in the chemical oxygen demand after the Fenton and photo-Fenton treatments, respectively at the optimum conditions.19
In the present study, the efficiency of the Fenton system to treat real batik wastewater was investigated. In the Fenton oxidation process, pollutants removal highly depends on the initial pH of wastewater, dosage of H2O2 and Fe2+, and initial concentration of pollutants. It should be noted that most of the available studies only focus on the decolourization efficiency, not the mineralization or degradation efficiencies to represent the effectiveness of the Fenton process. In this work, we focused on both the degradation and mineralization efficiencies. We also evaluated the characteristics of Fenton's sludge since it is the main limitation of practical application of the Fenton process. Besides, intermediate study was also conducted before and after the treatment by using FTIR, GC/MS and HPLC. to check the superiority of the Fenton process. Each operating parameter was evaluated by using Central Composite Design (CCD), a commonly used form of Response Surface Methodology (RSM). Then, the model developed for the textile wastewater was further validated using the other types of real wastewater with low, medium and high COD values. The results showed that the Fenton oxidation process could successfully treat the batik wastewater. This work does not only open up a new avenue for the application of the Fenton process in treating the batik wastewater, but also gives information on the by-products that can possibly be formed as a result of excessive chemicals.
Parameters | Mean value ± standard deviation |
---|---|
COD (mg l−1) | 1600–1900 ± 15 mg l−1 |
TOC (mg l−1) | 170 ± 15 mg l−1 |
Color (ADMI) | 1500 ± 50 |
pH | 12.5 ± 2 |
Appearance | Dark blue |
In this study, DOE was used to predict the values of COD, TOC and color removals. Response Surface Methodology (RSM) has recently been used to study the effects of several independent variables on COD removal efficiency.25–31 RSM, in comparison to the other modeling techniques, offers several advantages such as less experiments, clearly interprets the operating parameters, high cost efficiency and provides detailed information on the interaction between the parameters and responses.10,32,33
In this context, Central Composite Design (CCD) was employed to design and optimize the experiments for the Fenton oxidation process. The mass ratios of H2O2:
COD and H2O2
:
Fe2+, initial pH and retention time were chosen as the independent variables while COD, TOC, color removal percentages were the response variables. All the response variables are represented by a second-order polynomial equation that correlates response surfaces for evaluating the experimental results. The second-order polynomial equation (quadratic equation) is as follows:
![]() | (1) |
![]() | (2) |
A Total Organic Carbon (TOC) analyser (Shimadzu, Japan) was used to measure the TOC concentration in the solutions. The analysis was conducted to assess the extent the organic components were decomposed into CO2. The mineralization of the samples was analysed using the combustion/non-dispersive infrared gas analysis method. The TOC removal efficiency was calculated as:
![]() | (3) |
The color was measured after filtration using a UV-Spectrophotometer (Spectroquant Pharo 300, Merck, Germany) in ADMI unit. The decolorization efficiency of the treated sample was calculated as follows:
![]() | (4) |
The gas chromatography/mass spectrometry (GC-MS) analyses were performed using Agilent Technologies 6890 gas chromatograph, equipped with an HP-5MS column (30 m × 0.25 mm i.d. × 0.25 mm), coupled to an MSD 5973 selective mass detector (Agilent Technologies). A split–splitless injector was used under the following conditions: an injection volume of 5 μl and an injector temperature of 250 °C. The program temperature was 4 min at 105 °C, 25 °C min−1 to 180 °C, 5 °C min−1 to 230 °C, and 30 °C min−1 to 260 °C. The analyses were performed using the electron impact ionization (EI) mode at 70 eV. The spectrometer detector was run in a full-scan mode from 50 to 500 amu. The temperature of the MS interface and the ionization source was fixed at 280 °C and 250 °C, respectively. The decomposition of intermediates were determined by high performance liquid chromatography (HPLC) using Agilent Technology 1200 series. C18 column (4.6 mm × 250 mm × 5 μm) at 20 °C was used as the separation column. The eluent used was 60% acetonitrile/40% water (v/v); the injection volumes were 10 ml, and the eluent flow rate was 1 ml min−1. The detection wavelength was set at 254 nm.
The unique characteristics of the treated and untreated samples were presented by the Fourier transform infrared (FTIR) spectrum of the solution and recorded using FTIR (Perkin Elmer Spectrum One FTIR Spectrometer). In the present study, the attenuated total reflection (ATR) technique in the mid infrared region (MIR) of 4000–400 cm−1 was used for the characterization and assessment. In this work, surface morphology and composition of the sludge were analyzed using the 122 Phenom ProX SEM. The surface area method was used to calculate the percentage composition of the sludge generated. Particle size distribution (PSD) of the treated effluent with sludge (non-filtered sample) was measured by Malvern Mastersizer 2000, which works on the principle of laser detraction. Malvern Mastersizer can measure particles in the size range of 0.02 μm to 2000 μm. The process was fully automated and the results were based on the standard operating procedures provided by the manufacturer to eliminate user-to-user variability.
It is known that pH is one of the most important factors in the Fenton oxidation process.36 Various optimized pH values are observed in a few previous studies and some synthetic dyes are found to be efficient in both the basic and neutral conditions.37 Nevertheless, most of the studies have reported that Fenton process is ideal in acidic conditions.38 It has been reported that pH of the reaction is highly dependent on the property of the pollutants. Since this research focused on real textile effluents that comprise various components, the pH of the solution was varied from very acidic to basic conditions (initial pH values of 2 to 9).
The main aim of the study was to reduce the treatment cost by reducing energy consumption. All the experiments were conducted at room temperature (298 K). Oxidation and coagulation can take place simultaneously in the Fenton process and this is the major advantage. The mixing speed of the system also affects the solubility of iron salts and the reaction rate. In order to identify the best mixing speed, preliminary experiments were conducted in the range of 50–300 rpm. The COD removal efficiency was observed to increase with the mixing speed till 250 rpm, and no significant changes were observed at 300 rpm. Therefore, 250 rpm was selected as the optimized mixing speed and made constant during the course of the treatment process.
Since real textile effluent was used, initial chemical oxygen demand ([COD]i) was selected instead of concentrations. The value of [COD]i was varied between 1600–1900 mg l−1 and dependent on the samples collected from the batik industry.
Four operating factors were selected as the control factors to study the degradation efficiency of textile effluents: mass ratios of H2O2:
COD and H2O2
:
Fe2+, initial pH of the solution and retention time of the reaction. A total of 30 experiments was carried out in this analysis in accordance with the model indicated by the CCD. The selected range of the operating parameters and level of the independent variables are given in Table 2. The selected design required experiments outside the experimental range to allow the prediction of the response functions outside the selected range. The COD, TOC and color removal percentages were chosen as the response variables because they could provide necessary information for evaluating the analytical performance.
Independent variable | Units | Coded levels | ||||
---|---|---|---|---|---|---|
−2 | −1 | 0 | +1 | +2 |
Independent variable | Units | Actual levels | ||||
---|---|---|---|---|---|---|
H2O2![]() ![]() |
w/w | 4.5 | 1 | 6.5 | 12 | 17.5 |
H2O2![]() ![]() |
w/w | 4.5 | 2 | 8.5 | 15 | 21.5 |
pH | — | 1.5 | 2 | 5.5 | 9 | 12.5 |
Retention time | min | 0 | 30 | 60 | 90 | 120 |
The responses based on the experimental runs on color, COD and TOC removal percentages proposed by CCD are given in the Table 3. The results presented in the table are the duplicates of the experimental results at each operating condition proposed by CCD. Based on the results obtained from the experimental runs, the second-order polynomial equation was used to correlate the experimental results with the response functions. Polynomial models are commonly used to describe the behavior of the complex systems due to their good interpolation ability and simplicity of the parameter estimation.
Run | Block | Independent variable | Responses (%) | |||||
---|---|---|---|---|---|---|---|---|
H2O2![]() ![]() |
H2O2![]() ![]() |
pH | RT (min) | COD | TOC | CR | ||
1 | Block 1 | 12 | 2 | 9 | 90 | 71.5 | 53.5 | 98 |
2 | Block 1 | 1 | 2 | 9 | 30 | 57.2 | 49.2 | 78 |
3 | Block 1 | 1 | 2 | 2 | 90 | 52.7 | 50.3 | 77 |
4 | Block 1 | 6.5 | 8.5 | 5.5 | 60 | 76.1 | 64.1 | 96 |
5 | Block 1 | 6.5 | 8.5 | 5.5 | 60 | 75.4 | 65.8 | 96 |
6 | Block 1 | 12 | 15 | 2 | 90 | 50.4 | 35.8 | 85 |
7 | Block 1 | 1 | 15 | 9 | 90 | 60.1 | 45.1 | 84 |
8 | Block 1 | 1 | 15 | 2 | 30 | 62.4 | 52.4 | 86 |
9 | Block 1 | 12 | 15 | 9 | 30 | 52.7 | 36.2 | 88 |
10 | Block 1 | 12 | 2 | 2 | 30 | 74.2 | 61 | 90 |
11 | Block 2 | 12 | 2 | 9 | 30 | 70.8 | 55.8 | 96 |
12 | Block 2 | 1 | 15 | 9 | 30 | 60.4 | 52 | 83 |
13 | Block 2 | 12 | 2 | 2 | 90 | 73.2 | 62.1 | 83 |
14 | Block 2 | 1 | 15 | 2 | 90 | 62.3 | 50.1 | 90 |
15 | Block 2 | 1 | 2 | 9 | 90 | 61.6 | 48.2 | 79 |
16 | Block 2 | 1 | 2 | 2 | 30 | 56.3 | 48.4 | 75 |
17 | Block 2 | 12 | 15 | 9 | 90 | 49.5 | 28.7 | 90 |
18 | Block 2 | 6.5 | 8.5 | 5.5 | 60 | 76.4 | 63.9 | 97 |
19 | Block 2 | 12 | 15 | 2 | 30 | 54.5 | 37.1 | 87 |
20 | Block 2 | 6.5 | 8.5 | 5.5 | 60 | 74.3 | 65.2 | 98 |
21 | Block 3 | 6.5 | 8.5 | 5.5 | 120 | 62.2 | 38.2 | 95 |
22 | Block 3 | 6.5 | 8.5 | 12.5 | 60 | 35.3 | 22.3 | 80 |
23 | Block 3 | 17.5 | 8.5 | 5.5 | 60 | 76.8 | 60.3 | 95 |
24 | Block 3 | 6.5 | 21.5 | 5.5 | 60 | 62.6 | 48.3 | 88 |
25 | Block 3 | 6.5 | −4.5 | 5.5 | 60 | 78.3 | 68.2 | 85 |
26 | Block 3 | 6.5 | 8.5 | 5.5 | 60 | 74.6 | 61.9 | 96 |
27 | Block 3 | 6.5 | 8.5 | −1.5 | 60 | 41.5 | 33.1 | 73 |
28 | Block 3 | −4.5 | 8.5 | 5.5 | 60 | 70.2 | 62.8 | 86 |
29 | Block 3 | 6.5 | 8.5 | 5.5 | 0 | 56.2 | 39.2 | 95 |
30 | Block 3 | 6.5 | 8.5 | 5.5 | 60 | 74.3 | 62.9 | 96 |
Based on the experimental results, the final quadratic equation of the response in term of coded factors is presented in eqn (5)–(7), as shown in Table 4. The negative and positive values of the coefficients represent the antagonistic and synergistic effect of each model term on the response respectively. Positive effect means that the COD removal efficiency increases with factors while negative effect indicates that the response decreases when the factor level increases. The equations correlate the response variables as a function of the operating factors and a bad equation will result in poor lack-of-fit and violation of the analysis of variance (ANOVA) assumptions. The ANOVA results of the quadratic polynomial models for the Fenton oxidation treatment for the color, COD and TOC models are shown in ESI as Table S1.† The equation clearly shows that all the four operating parameters had positive effects on the COD, TOC and color removal percentages within the investigated range.
Responses | Proposed quadratic model | Eqn |
---|---|---|
COD% | =28.07 + 1.92 (H2O2![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() |
(5) |
TOC% | =11.80 + 1.50 (H2O2![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() |
(6) |
Color% | =63.30 + 1.55 (H2O2![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() ![]() |
(7) |
Consequently, all the three polynomial equations gave a good visualization of the effects of the significant factors and their effects on the response.
The fit of the model was evaluated by ANOVA. The result revealed the effects of the model that were statistically significant for a confidence level of 95% (p-value < 0.05). The p value represents the occurrence probability of F due to noise; the smaller the value of p, the more significant the corresponding parameter is. Values of Prob > F less than 0.05 indicate that the model is significant and values greater than 0.01 imply that the model is insignificant. The results of the ANOVA analysis, showed that all the models had a p value less than 0.0001, indicating that the models were significant to describe the color, COD and TOC removal efficiencies.
Furthermore, the validity of the models was determined by the values of lack-of-fit. The ‘lack-of-fit’ for both models was not significant relative to the pure error and this confirmed the good predictability of the model. However, the “Lack-of-Fit F-value” of 29.41 implied that the Lack-of-Fit was significant and the model was not fit for color removal%. This was not surprising since the color abatement occurred within 2–5 minutes under all experimental conditions. Therefore, it was quite difficult to model color removal using the same time interval for COD and TOC removals because near-complete decolorization could be achieved at this reaction time.
Besides, the ANOVA analysis showed that the F values for the COD, TOC and color removal models were 128.3, 143 and 29.2 respectively, indicating that the models were highly significant. There was only 0.015 chance that the ‘model F value’ could occur due to noise. In addition, the quality of fit of the polynomial models was expressed by the value of correlation coefficient (R2). The models were found to be adequate to fit all the experimental data with R2, adjusted R2, and predicted R2 of 99.3, 98.5, and 94.8% for COD removal; 99.3, 98.7, 95.3% for TOC removal; and 96.9, 93.6 and 77.7% for color removal. The R2 value of the response variables, in descending order were COD > TOC > color removal. All the obtained predicted R2 values were in reasonable agreement with the adjusted R2, except for the color removal. This indicated the good predictability of the models for both COD and TOC removal%. It was difficult to model color removal based on the same retention time fixed for COD and TOC removals because decolorization happened within minutes. The good agreement between the experimental and predicted values for COD, TOC and color removal%, as illustrated in ESI as Fig. S1† revealed the accuracy of the model.
Besides, the adequate precision ratios of 39.12, 40.9 and 16.4 derived from the COD, TOC and color removal% indicated that there were adequate signals for all response variables. The perturbation graph obtained based on the experimental result could be used to explain that all the four investigated operating factors had a tremendous effect on the degradation efficiency. Fig. S2 (ESI†) shows the perturbation graph of COD, TOC and color removals. The plot was obtained for initial pH of 5.5, H2O2:
COD = 6.5, H2O2
:
Fe2+ = 8.5 and RT of 60 min. The steepiness of the plot indicates the sensitivity of the response to the factors. The plot depicted that the COD, TOC and color removal efficiencies were very sensitive to the mass ratio of H2O2
:
COD, followed by initial pH, mass ratio of H2O2
:
Fe2+ and retention time. In conclusion, based on the ANOVA analysis, the model was well explained and it could be used to navigate the design space in terms of COD and TOC removal% efficiencies.
Color removal during the Fenton process may result from destruction of dyestuffs by hydroxyl radicals formed during the Fenton reaction or from coagulation by Fe3+. It was observed that decolorization was very efficient through the Fenton oxidation process with the removal efficiency between 73% and 98%. Rapid decolorization (within 5 minutes) was observed in most of the experimental runs right after the Fenton reagent was added to the wastewater. The dark blue wastewater turned pale yellow and colourless after the filtration process. The pale yellow color might be caused by the intermediates that destroyed the azo groups found in the wastewater. Although almost a complete color removal was observed, the low COD and TOC removal percentages showed that it was difficult to destroy aromatic compounds or other functional groups contributing to the recalcitrant nature of the wastewater.
Fig. 3 shows the 3D and 2D response surface plots representing the color removal percentage as a function of the ratio of H2O2:
COD and H2O2
:
Fe2+, H2O2
:
COD and pH, and H2O2
:
Fe2+ and pH. The plots showed that color removal increased with increased ratio of H2O2
:
COD and decreased ratio of H2O2
:
Fe2+. However, further increase in the ratio of H2O2
:
COD and H2O2
:
Fe2+ beyond the optimum region resulted in decreased color removal efficiency. Since excessive hydroxyl radicals in the system will be converted to hydroxyl ions and cause the precipitation of Fe3+ ions, the amount of Fe2+ was reduced, leading to decreased colour removal, as seen in eqn (8)–(10).38 This result was supported by Benatti and others (2006)29 who reported that the color removal efficiency of chemical laboratory wastewater was inversely proportional to the ratio of H2O2
:
Fe2+.
H2O2 → HO˙ + ˙OH | (8) |
Fe2+ + HO˙ → Fe3+ + OH− | (9) |
[Fe3+][OH−] → Fe(OH)3 | (10) |
Moreover, at constant retention time and ratio of H2O2:
Fe2+, increase in color removal was observed with increased ratio of H2O2
:
COD and initial pH of the solution. The plots showed that the optimum pH for color removal (96.6%) was pH 6, beyond which, there was decreased decolourization. The wastewater pH is very important as its controls the generation of hydroxyl radicals and concentration of iron salts. The results supported the fact that decomposition of hydrogen peroxide rapidly increases at pH above 6.5. The results showed that the color removal efficiency was significantly higher in weak acidic conditions compared to weak alkaline solutions. The oxidation rate of the Fenton oxidation process was decreased at pH higher than 6, which could be due to the precipitation of Fe3+ to ferric hydro complexes. The formed ferric hydroxide could decompose the available H2O2 into oxygen and water and this consequently decreased the oxidation rate due to low concentration of hydroxyl radicals. Besides, the formed [Fe(II)(H2O)6]2+ reacted slowly with H2O2 than with [Fe(II)(OH)(H2O)5]2+ and this caused less generation of hydroxyl radicals.42 Moreover, low decolorization percentage was reported at very low pH due to the hydroxyl radical scavenging effects of H+ ion.43,44 These findings were consistent with the results reported by other researchers.42,45–47
Besides, increasing the ratio of H2O2:
Fe2+ and initial pH of the solution at constant ratio of H2O2
:
COD increased the color removal efficiency. However, a decrease in the efficiency was observed above the optimal value of both the H2O2
:
Fe2+ and initial pH. This was because at constant H2O2
:
COD ratio, increase in the ratio of H2O2
:
Fe2+ contributed to the reduction in the concentration of Fe2+. The color removal rate was restarted there was insufficient Fe2+ to react with H2O2 to generate hydroxyl radicals in the system. It should also be noted that the authors observed immediate color change of the wastewater samples and formation of small flocs at pH higher than 5 with the addition of ferrous salt alone. This clearly showed that coagulation took place.
H2O2 + HO˙ → H2O + HO˙2, k = 2.7 × 107 M−1 s−1 | (11) |
HO˙2 + HO˙ → H2O + O2, k = 1.0 × 1010 M−1 s−1 | (12) |
HO˙ + HO˙ → H2O2, k = 4.2 × 109 M−1 s−1 | (13) |
Therefore, it is important to optimize the dosage of H2O2 to generate a sufficient amount of hydroxyl radicals. In this context, the minimum and maximum ratios of H2O2:
COD were chosen based on the previous studies reported in the literature and preliminary experiments were also conducted to identify the suitable range to avoid excessive usage of oxidants. The initial COD of wastewater was chosen as one of the parameters as it plays an important role in selecting the optimum concentration of H2O2 and Fe2+. Real textile wastewater with initial [COD]i of 1610 mg l−1 was used and it was kept constant throughout the Fenton oxidation process. Based on the second-order polynomial equation, it could be concluded that the key factor that contributed to the reduction of COD and TOC was the initial ratio of H2O2
:
COD.
Fig. 4 shows the response surface analysis and contour between the mass ratios of H2O2:
COD and H2O2
:
Fe2+ on the COD and TOC removal efficiencies. Removal of COD increased with an increase in the mass ratio of H2O2
:
COD. At the fixed COD value of 1610 mg l−1 and mass ratio of H2O2
:
Fe2+ of 2, the final COD removal efficiency increased from 71.7% to 85% at a retention time of 60 min when the mass ratio of H2O2
:
COD increased from 1 to 15. The increase in the removal efficiency was due to the increase in the hydroxyl radical concentration as a result of the addition of H2O2.49 However, at a fixed mass ratio of H2O2
:
COD, an increase in the mass ratio of H2O2
:
Fe2+ from 2 to 18 reduced the COD removal efficiency from 85% to 57.6%. It was because there was an insufficient amount of ferrous salts that was available in the system. Increasing the mass ratio of H2O2
:
Fe2+ at fixed COD and H2O2 dosage reduced the amount of Fe2+ to be catalysed by hydrogen peroxide to produce hydroxyl radicals (eqn (14)). This result was similar to the findings presented by Gulkaya and others (2006).50 This was agreeable since the developed polynomial model also showed that both ratios exhibited a negative interaction.
Fe2+ + ˙OH → Fe3+ + OH− | (14) |
![]() | ||
Fig. 4 Contour for percent COD and TOC removal as a function of mass ratios of H2O2![]() ![]() ![]() ![]() |
The highest COD reduction of 85% was obtained at H2O2:
COD = 11 and H2O2
:
Fe2+ = 2 at a center value of initial pH and retention time. On the other hand, a decrease in the efficiency was observed when the ratio of H2O2
:
Fe2+ was less than 2 and H2O2
:
COD was above 12 (refer to Table 3). Moreover, unfavourable effect in the COD removal was observed when higher concentration of H2O2 was used. Self-scavenging of HO radicals caused by excessive amount of H2O2 contributed to this condition.34,41 This means that insufficient or excess H2O2 and Fe2+ reduced the efficiency of hydroxyl radicals to oxidize the contaminants. Zhang and others (2007) also reported that the removal efficiency of organic materials in the leachate wastewater decreased with increased Fenton reagent dosage beyond an optimal value.51 Therefore, it is suggested to keep the ratio lower than 11 and lower H2O2 concentration is also more economically viable compared to higher H2O2 concentration. The TOC removal percentage showed the similar trend as the COD removal efficiency with the highest mineralization of 70% observed at H2O2
:
COD = 10. The TOC removal efficiency was found to decrease when the ratio increased, as shown in Fig. 4. It should be noted that the concentration of H2O2 required to complete the degradation varied with the initial COD of the samples.
Moreover, the interaction effect between the initial pH and mass ratio of H2O2:
COD and H2O2
:
Fe2+ at a fixed retention time of 60 min was also evaluated in this study. It was observed that there were significant changes in the removal efficiency when we used different initial pH values (2, 5.5, 9 and 12). Fig. 5 shows that the removal efficiency decreased from 85% to 76.1% and 53.1% when the initial pH was changed to 9 and 12, respectively from 5.5. A further reduction in the removal efficiency (79.1%) was observed when the initial pH of 2 was used in the system, as shown in Fig. 5. This showed that there was a strong interaction between the dosage of the Fenton reagent and the initial pH of the pollutant. The following section discusses the effects of initial pH and mass ratios of H2O2
:
COD and H2O2
:
Fe2+ on COD and TOC removal efficiencies.
Fig. 6 shows the semi spherical response surface that explains the effects of initial pH of the solution on the COD and TOC removal percentages. The graph shows that the mineralization and degradation efficiencies increased with the initial pH of the solution from 2–5 but the efficiency decreased slightly above pH 6. The maximum COD and TOC removals were determined to be 76.1% and 64.6%, respectively. The removal efficiency was reportedly decreased to 67.1% and 55% when the pH was increased above 7 at a mass ratio of H2O2:
Fe2+ = 8.5, as illustrated in Fig. 6. At the optimum condition, H2O2 was converted rapidly to hydroxyl free radicals that could non-selectively decompose these pollutants in the batik wastewater.
![]() | ||
Fig. 6 Response surface and contour for COD and TOC removal percentages as a function of H2O2![]() ![]() |
Moreover, an increase in the ratio of H2O2:
Fe2+ from 2–15 at the lowest initial pH of 2 and fixed mass ratios of H2O2
:
COD = 6.5 caused a steady reduction in the removal efficiency of COD from 80.4 to 61.5%, as shown in Fig. 7. This may be due to the scavenging of hydroxyl caused by ferrous ion (eqn (8)).57 Moreover, increasing the mass ratios of H2O2
:
Fe2+ above 15 caused a drastic change in the removal efficiency, whereby only 56% and 42.8% removals were achieved at the mass ratio of H2O2
:
Fe2+ of 20 and 30, respectively. It was proven that the dosage of Fe2+ and H2O2 had a strong interaction with the initial pH of the solution. In conclusion, the result showed that the oxidation was more active in acidic conditions while alkaline conditions favoured the coagulation process.
Fig. 8 shows the interaction between the mass ratio of H2O2:
Fe2+ and retention time for the COD and TOC removals at the fixed mass ratios of H2O2
:
COD = 6.5 and initial pH of 5.5. It was observed that the degradation efficiency increased with the mass ratio of H2O2
:
Fe2+ and retention time. The maximum COD (77.9%) and TOC (67.3%) removals were achieved at pH 5.5, mass ratio of H2O2
:
COD = 6.5, H2O2
:
Fe2+ = 2 between 48–54 minutes. When the oxidation time and ratio of H2O2
:
Fe2+ increased beyond the optimal point, the COD and TOC removals were reduced to 67.1% and 55% respectively. A drop in the removal efficiency might be caused by longer treatment time that contributed to the formation of toxic intermediates or scavenging caused by excessive hydroxyl radicals and iron salts. The result indicated that there should be an optimised oxidation time.
![]() | ||
Fig. 8 Response surface and contour for percent COD and TOC removal as a function of H2O2![]() ![]() |
In addition, the interactions between the retention time and mass ratios of H2O2:
Fe2+ and H2O2
:
COD were also evaluated in this study. When the H2O2
:
COD mass ratio was increased from 12 to 24 and 36, a drastic decrease in the COD removal was observed, as shown in Fig. 9. This indicated that longer retention time and excessive hydroxyl in the system might caused the formation of intermediates, which increased the toxicity level of the wastewater.
Res. | COD (mg l−1) | H2O2![]() ![]() |
H2O2![]() ![]() |
pH | RT | H2O2 (ml) | Fe2+ (ml) | Pred. | Exp. |
---|---|---|---|---|---|---|---|---|---|
a Desirability = 1, CR = color removal. | |||||||||
CR | 1610 | 10.18 | 4.74 | 4.77 | 63.4 | 49.2 | 17.16 | 96.6 | 99.6 |
COD | 1610 | 10.18 | 4.74 | 4.77 | 63.4 | 49.2 | 17.16 | 80.1 | 81.4 |
TOC | 1610 | 10.18 | 4.74 | 4.77 | 63.4 | 49.2 | 17.16 | 68.2 | 70.5 |
Zero order reaction:
![]() | (15) |
First order reaction:
![]() | (16) |
Second order reaction:
![]() | (17) |
By integrating eqn (15)–(17), the following equations can be obtained (eqn (18)–(20)):
ct = c0 − k0t | (18) |
ct = c0e−k1t | (19) |
![]() | (20) |
The regression analysis based on the zero-, first- and second-order reaction kinetics for the COD removal from the batik wastewater using the Fenton oxidation process, which was conducted at the optimized conditions. The results are shown in Fig. 10. It was found that that the regression coefficients, R2 of the second-order reaction kinetics (Fig. 10(c)) was 0.9748, which was obviously much higher than that based on the zero-order (R2 = 0.8583) and the first-order (R2 = 0.9601) reaction kinetics. Comparing the regression coefficients obtained by the graphical representation, we concluded that the first-order reaction kinetics fit the reaction best. The first-order rate constant k1 = 0.0252 s−1 was calculated from the slope. The result obtained from this study was consistent with the work from Nitoi and others (2013).58
An understanding of the surface chemistry can be acquired through conducting Fourier transform infrared spectroscopy (FTIR). FTIR spectroscopy is widely used to characterize and analyze the general functional groups present in wastewater. In the present study, the comparison of the FTIR spectrum of the untreated and treated batik wastewater clearly indicated the mineralization of wastewater by the Fenton oxidation process. Fig. 11 shows the FTIR spectrum of the untreated batik wastewater and treated wastewater by the Fenton oxidation process at the optimized experimental conditions as followed: mass ratio of H2O2:
COD = 10.18, and H2O2
:
Fe2+ = 4.74, initial pH 4.77 and retention time = 63.4 min.
Fig. 11 shows the comparison of the spectrum before and after the treatment. A decrease in the number of peaks was observed. Therefore, it can be concluded that the Fenton process successfully mineralized most of the organic compounds present in the wastewater. It was clear from the FTIR spectrum that the peaks at the wavelengths of 3317 cm−1 and 1637 cm−1 were observed with a reduction in their intensity in the spectrum of the Fenton treated wastewater. A strong and broad peak located at 3317 cm−1 can be associated with the presence of hydroxyl groups. It was believed that the band that occurred at 1637 cm−1 was caused by the aromatic CC bonds, which were polarized by the oxygen atoms bond near one of the C atom. This might be due to the incorporation of oxygen groups into the carbonaceous phase caused by the attacks by hydroxyl radicals.
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Fig. 14 Chromatogram for organic in batik wastewater (a) before and (b) after Fenton treatment (S = siloxanes, A = alkanes, AH = aromatic hydrocarbon alkane, ES = ester, CA = carboxylic acid). |
COD (mg l−1) | H2O2![]() ![]() |
H2O2![]() ![]() |
pH | RT | Predicted | Experimental | |||||
---|---|---|---|---|---|---|---|---|---|---|---|
CR | COD | TOC | CR | COD | TOC | ||||||
Steel industry | 326 | 10.18 | 4.74 | 4.77 | 63.4 | 96.6 | 80.1 | 68.2 | 100 | 67.5 | 50.2 |
POME | 34![]() |
10.19 | 4.75 | 4.77 | 63.4 | 96.6 | 80.1 | 68.2 | 99.4 | 98.9 | 72.5 |
Leachate | 5040 | 10.20 | 4.76 | 4.77 | 63.4 | 96.6 | 80.1 | 68.2 | 99.5 | 92.7 | 71.6 |
Footnote |
† Electronic supplementary information (ESI) available. See DOI: 10.1039/c5ra26775g |
This journal is © The Royal Society of Chemistry 2016 |