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This article was downloaded by: [York University Libraries] On: 22 November 2014, At: 02:00 Publisher: Taylor & Francis Informa Ltd Registered in England and Wales Registered Number: 1072954 Registered office: Mortimer House, 37-41 Mortimer Street, London W1T 3JH, UK Journal of Environmental Science and Health, Part B: Pesticides, Food Contaminants, and Agricultural Wastes Publication details, including instructions for authors and subscription information: http://www.tandfonline.com/loi/lesb20 Comparison of Fenton and Photo-Fenton Processes for Livestock Wastewater Treatment JAE-HONG PARK a , IL-HYOUNG CHO b & SOON-WOONG CHANG c a Research Institute for Environmental Technology and Sustainable Development, Korea University , Seoul, Korea b New Town Development Division , Gyeonggi Innovation Corporation , Suwon, Korea c Department of Environmental Engineering , Kyonggi University , Suwon, Korea Published online: 18 Aug 2006. To cite this article: JAE-HONG PARK , IL-HYOUNG CHO & SOON-WOONG CHANG (2006) Comparison of Fenton and Photo-Fenton Processes for Livestock Wastewater Treatment, Journal of Environmental Science and Health, Part B: Pesticides, Food Contaminants, and Agricultural Wastes, 41:2, 109-120 To link to this article: http://dx.doi.org/10.1080/03601230500364740 PLEASE SCROLL DOWN FOR ARTICLE Taylor & Francis makes every effort to ensure the accuracy of all the information (the “Content”) contained in the publications on our platform. However, Taylor & Francis, our agents, and our licensors make no representations or warranties whatsoever as to the accuracy, completeness, or suitability for any purpose of the Content. Any opinions and views expressed in this publication are the opinions and views of the authors, and are not the views of or endorsed by Taylor & Francis. The accuracy of the Content should not be relied upon and should be independently verified with primary sources of information. 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ISSN: 0360-1234 (Print); 1532-4109 (Online) DOI: 10.1080/03601230500364740 Comparison of Fenton and Photo-Fenton Processes for Livestock Wastewater Treatment Jae-Hong Park,1 Il-Hyoung Cho,2 and Soon-Woong Chang3 1Research Institute for Environmental Technology and Sustainable Development, Korea University, Seoul, Korea 2New Town Development Division, Gyeonggi Innovation Corporation, Suwon, Korea 3Department of Environmental Engineering, Kyonggi University, Suwon, Korea In this study, the photochemical degradation of livestock wastewater was carried out by the Fenton and Photo-Fenton processes. The effects of pH, reaction time, the mo- lar ratio of Fe2+/H2O2, and the Fe2+ dose were studied. The optimal conditions for the Fenton and Photo-Fenton processes were found to be at a pH of 4 and 5, an Fe2+ dose of 0.066 M and 0.01 M, a concentration of hydrogen peroxide of 0.2 M and 0.1 M, and a molar ratio (Fe2+/H2O2) of 0.33 and 0.1, respectively. The optimal reaction times in the Fenton and Photo-Fenton processes were 60 min and 80 min, respectively. Under the optimal conditions of the Fenton and Photo-Fenton processes, the chemical oxygen demand (COD), color, and fecal coliform removal efficiencies were approximately 70–79, 70–85 and 96.0–99.4%, respectively. Key Words: Livestock wastewater; Fenton process; Photo-Fenton process. INTRODUCTION In general, wastewaters derived from livestock farms, including cattle, swine, and poultry farms, are highly concentrated in organic matter and nutrients (i.e., nitrogen and phosphorus). Therefore, although the quantity of livestock wastewater is small compared with that of municipal and industrial wastewa- ter, its concentration of pollutants is 50–150 times higher than that of municipal wastewater in Korea.[1] In Korea, livestock wastewater is either treated separately or combined with municipal wastewater and night soil. However, the treatment capacities Received August 17, 2004. Address correspondence to Jae-Hong Park, Research Institute for Environmental Technology and Sustainable Development, Korea University, Seoul, Korea; E-mail: jhong@korea.ac.kr 109 D ow nl oa de d by [ Y or k U ni ve rs ity L ib ra ri es ] at 0 2: 00 2 2 N ov em be r 20 14 110 Park, Cho, and Chang of these methods are insufficient to deal with all of the livestock wastewater that is generated. Therefore, it is believed that the excess is discharged untreated into soil, farmland, and watersheds. However, the inappropriate disposal of livestock wastewater may pose environmental problems such as the accumula- tion of pollutants in soil and the pollution of ground and surface water due to the leaching and runoff of pollutants. For this reason, livestock wastewater is considered to be one of the main sources of water pollution in Korea. The problem posed by the inappropriate disposal of livestock wastewater is not limited to Korea but is also a problem faced by countries all over the world. For example, in a pollutant source survey conducted in 1998 in the USA,[2] it was shown that about 60% of river water pollution and about 45% of lake wa- ter pollution were caused by agriculture sources. Concentrated animal feeding operations (CAFOs) were considered to be the main source of such pollution. The high concentration and industrial typology of livestock farms, which are often not connected with land cultivation, lead to the excessive generation of animal wastes, at a level which is frequently higher than their recycling potential on land as a fertilizer. Livestock farms located in both sewered and nonsewered areas generate an intermittent type of wastewater discharge with a high organic content that should be removed in such a way as to en- sure compliance with effluent limitations. From a technological standpoint, biological treatment processes appear to constitute the only viable alterna- tive for the handling of these wastewaters. However, many studies have re- vealed that biologically treated effluents may contain nonbiodegradable or- ganic fractions, consisting of chemicals that either were initially present in the wastewater or were microbially generated during the biological processes.[3−5] These residual or inert fractions are of great import in meeting the discharge standards. Therefore, advanced methods of wastewater treatment based on chemical oxidation, which generate powerful oxidants (hydroxyl radicals), are gain- ing importance. They allow these nonbiodegradable and/or inert organic compounds to be oxidized by free radicals and bring about their complete mineralization to water and carbon dioxide. The classical Fenton oxidation reaction and photoassisted Fenton oxidation reaction, usually referred to as Photo-Fenton oxidation, are two such methods which offer the possibility of producing hydroxyl radicals. Recently, several studies on the degradation of nonbiodegradable, toxic, and hazardous substances were carried out using the Fenton and Photo-Fenton reactions.[6−10] However, few studieshave been carried out on the treatment of real livestock wastewater using these methods. The purpose of this study was to evaluate the use of the Fenton and Photo-Fenton reactions for the treatment of livestock wastewater using a lab-scale reactor. The effect of adding hydrogen peroxide and a ferrous salt, and the influence of the pH value on the degradation of organic pollutants, color, and fecal coliform were investigated. The feasibility D ow nl oa de d by [ Y or k U ni ve rs ity L ib ra ri es ] at 0 2: 00 2 2 N ov em be r 20 14 Comparison of Fenton and Photo-Fenton Processes 111 of the real-scale application of the Fenton and Photo-Fenton processes at the farm level was also evaluated. MATERIALS AND METHODS Chemical Reagents The pH was controlled with an accuracy of ±0.02 by adding either sodium hydroxide (reagent grade, Duksan) or sulfuric acid (reagent grade, Duksan). Ferrous sulfate heptahydrate (FeSO4·7H2O, 99.5%) obtained from Duksan, hydrogen peroxide (H2O2, 30%, wt) from Merck, and ferric chloride (FeCl3, 97%) from Samchon were used. Preparation of the Livestock Wastewater The livestock wastewater, which was pretreated by coagulation with 3000 mgL−1 FeCl3,was obtained from a livestock wastewater treatment plant lo- cated in Kyonggi province in Korea. The characteristics of the settled livestock wastewater used in this experiment were as follows: COD 5320 mgL−1, fecal coliform 3.5 × 1010 number/100 mL, and color 0.3215 abs. Experimental Procedures A 2 L beaker equipped with a glass bar with a diameter of 10 mm acting as a baffle was used as the Fenton reactor. The reactor was first filled with 1 L of livestock wastewater and the pH was adjusted with concentrated H2SO4 and/or NaOH. The second step was the addition of ferrous sulfate (analytical grade, heptahydrate). The third step was the addition of hydrogen peroxide (reagent grade, 30%) and the reaction was started. The concentration of hydrogen peroxide was measured using the iodometric method.[11] After the reaction was finished, the pH was adjusted to 8.5, and then the liquid was transferred to a graduated cylinder and allowed to precipitate for 3 h. After the precipitation was completed, the upper 30% portion of the liquid was separated from the precipitate, and the COD, color, and fecal coliform were measured. A schematic diagram of the Photo-Fenton experimental setup used in this study is shown in Figure 1. It consists of an irradiation source and a photoreac- tor. All of the experiments were carried out in a continuous flow through eight cylindrical quartz columns (each having a diameter of 10 mm and a length of 700 mm) with recirculation of the solution. The light source was provided by 40 W UV lamps (Sankyo Denki Co., Ltd., 1200 mm in length, 32 mm in diam- eter), mounted on standard fluorescent tube holders. The column was exposed to a luminous source composed of eight UV lamps with a maximum emission at 254 nm. The total UV intensity was controlled by turning on different numbers D ow nl oa de d by [ Y or k U ni ve rs ity L ib ra ri es ] at 0 2: 00 2 2 N ov em be r 20 14 112 Park, Cho, and Chang Figure 1: Schematic diagram of the Photo-Fenton reactor. of UV lights, and the maximum intensity was 4.325 mWcm−2 (with all eight UV lights on). The effective volume of the photoreactor (550 mm (width) × 640 mm (length) × 110 mm (height)) was 1.88 L. The bottom of the photoreactor was wrapped in aluminum to reflect any illumination toward the column. For the Photo-Fenton experiment, the livestock wastewater (5 L) was con- tained in a 10 L Pyrex glass vessel and was stirred. The livestock wastewater circulated through the eight modules of the Photo-Fenton reactor (Fig. 1) at a flow rate of 1 L min−1. The eight modules were connected in series, and the livestock wastewater flowed directly from one to the other and finally to the reservoir tank. The temperature of the livestock wastewater was maintained at 25 – 27◦C during the reaction. The H2O2 dosage was determined based on the stoichiometric ratio with respect to the COD, and ferrous salt was also added at a molar ratio of H2O2 to Fe(II). For the analysis, a 50 mL aliquot was taken at various intervals. After the reaction was finished, the pH was adjusted to 8.5, and then the liquid was transferred to a graduated cylinder and allowed to precipitate for 3 h. After the precipitation was completed, the upper 50% portion of the liquid was separated from the precipitate, and then the COD, color, and fecal coliform were measured. Analytical Methods The UV intensity was measured with a radiometer (VLX-3W Radiometer 9811-50, Cole Parmer lnstrument Co.) at 254 nm. The pH was measured by means of an Orion pH meter, model 525A. The concentration of hydrogen per- oxide was measured using the iodometric method.[11] The decolorization of the livestock wastewater was monitored using a UV-Vis spectrometer (Shimadzu UV-1201, absorption at λmax, 355 nm). The potassium dichromate closed reflux D ow nl oa de d by [ Y or k U ni ve rs ity L ib ra ri es ] at 0 2: 00 2 2 N ov em be r 20 14 Comparison of Fenton and Photo-Fenton Processes 113 colorimetric method was used to measure the COD.[12] The fecal coliform was measured using the standard method.[12] RESULTS AND DISCUSSION The Effect of pH The pH value has a decisive effect on the oxidation potential of OH radicals because of the reciprocal relation between the oxidation potential and the pH value (Eo = 2.8 V and E14 = 1.95 V).[6] Furthermore, the concentration of inor- ganic carbon and the hydrolytic speciation of the Fe(III) species were strongly affected by the pH value.[6] Therefore, the pH is an important parameter in the Fenton and Photo-Fenton processes. Figure 2 illustrates the effect of the pH on the COD removal efficiency in the Fenton and Photo-Fenton processes. The experiments have been carried out at pH range from 2 to 9, and detailed experimental conditions in the Fenton and Photo-Fenton processes were: [Fe2+] of 0.1 M and 0.01 M, [H2O2] of 0.1 M, reaction time of 1 h and 4 h, and UV254 intensity of 4.325 mWcm−2, respectively. The pH values of 4 and 5 were found to be the optimum pH values for the Fenton and Photo-Fenton processes, respectively. However, the COD removal efficiency was hardly influenced by the pH below pH 3, due to the hydroxyl radical scavenging effects of H+ at low pH. Also, the COD removal efficiency rapidly decreased with increasing pH in the range of 5–9. Our results are in good agreement with those of previous reports.[13−15] Hydrogen peroxide was most stable in the range of pH 3–4, but the decom- position rate rapidly increased with increasing pH above pH 5.[13] When the pH of the reaction was higher than 5, the COD removal efficiency rapidly decreased with increasing pH, not only due to the decomposition of hydrogen peroxide,[14] but also because of the deactivation of the ferrous catalyst due to the formation of ferric hydroxy complexes.[15] Figure 2: Effect of pH on COD removal. D ow nl oa de d by [ Y or k U ni ve rs ity L ib ra ri es ] at 0 2: 00 2 2 N ov em be r 20 14 114 Park, Cho, and Chang The Effect of Fe2+ and H2O2 Addition of an excess of H2O2 did not improve the maximum degradation in either the Fenton or Photo-Fenton process. This may be due to the autode- composition of H2O2 to oxygen and water and the recombination of OH radicals (OH·) as follows: 2 H2O2 −→ 2 H2O + O2 (1) OH· + H2O2 −→ H2O + HO2· (2) Since the OH radicals react with H2O2, the H2O2 itself contributes to the OH· scavenging capacity.[16] Therefore, H2O2 should be added at the optimal concentration to achieve the best degradation. Also, the higher addition of Fe(II) results in a brown turbidity that hinders the absorption of the UV light required for photolysis and causes the recombi- nation of OH radicals. In the case, Fe(II) reacts with OH radicals, acting as a scavenger.[17] OH· +Fe2+ −→ OH− + Fe3+ (3) It is desirable that the ratio of H2O2 to Fe(II) should be as small as possible, so that the above recombination reaction can be avoided and the production of sludge resulting from the iron complex is also reduced. To determine the optimal ratio of Fe2+/H2O2 in the Fenton process, experi- ments were carried out at 10 different molar ratios from 0.1 to 5. The detailed experimental conditions were: a pH of 4, a reaction time of 1 h, and [Fe2+] of 0.05 M. Figure 3 shows that the COD removal efficiency was distinctly increased by decreasing the dosage of hydrogen peroxide. However, the COD removal efficiency decreased with decreasing dosage of hydrogen peroxide when the Fe2+:H2O2 ratio was less than 0.33. From these results, it was determined that the optimal ratio of Fe2+/H2O2 for COD removal was 0.33. Figure 4 illustrates the COD degradation process as a function of H2O2 at the optimal Fe2+/H2O2 molar ratio. The investigation was conducted at a dosage Figure 3: Variation of COD removal with molar ratio in Fenton oxidation. D ow nl oa de d by [ Y or k U ni ve rs ity L ib ra ri es ] at 0 2: 00 2 2 N ov em be r 20 14 Comparison of Fenton and Photo-Fenton Processes 115 Figure 4: Variation of COD removal with H2O2 dosage in Fenton oxidation. of H2O2 ranging from 0.01 to 0.45 M, and detailed experimental conditions were: a pH of 4, a reaction time of 1 h, and Fe2+/H2O2 ratio of 0.33. The COD removal efficiency was increased by increasing the dosage of H2O2 in the range of 0– 0.2 M. However, it hardly changed above an H2O2 dosage of 0.2 M. Therefore, the optimal dosage of H2O2 for COD removal was considered to be 0.2 M. In the Photo-Fenton process, the presence of hydrogen peroxide can increase the efficiency of COD removal. Being an electron acceptor, hydrogen peroxide reacts with conduction band electrons [Eq. (4)] to generate hydroxyl radicals, which are required for the photomineralization of organic pollutants. When hydrogen peroxide absorbs UV light with a wavelength <300 nm, one H2O2 molecule is converted to two OH radicals, as shown in Eq. (5).[18] H2O2 + e− −→ OH· + OH− (4) H2O2 + hv −→ 2OH· (5) However, if the H2O2 concentration is too high, the COD removal efficiency does not improve the maximum degradation because of the autodecomposition of H2O2 and the recombination of OH radicals (OH·), as indicated in Eq. (2). To determine the optimal Fe(II) dosage in the Photo-Fenton process, ex- periments were conducted at five different dosages from 0.025 to 0.05 M. The detailed experimental conditions were: a pH of 5, UV254 intensity of 4.325 mW- cm−2, and [H2O2] of 0.1 M. Figure 5 shows the effect of Fe(II) dosage on the COD removal efficiency. The optimal Fe(II), dosage for COD removal was found to be 0.01 M. COD removal efficiencies of 70 to 74% were achieved at higher concentrations of Fe(II), and only about 30 to 36% of the COD was eliminated at lower concentrations of Fe(II), whereas 83% of the COD was eliminated at the optimal Fe(II) dosage at the reaction time of 2 h. Figure 6 shows the effects of the dosage of H2O2 on the COD removal effi- ciency in the case of the Photo-Fenton process. The investigation was carried out at H2O2 dosages ranging from 0.01 to 0.2 M, and detailed experimental conditions were: a pH of 5, UV254 intensity of 4.325 mWcm−2, and [Fe2+] of D ow nl oa de d by [ Y or k U ni ve rs ity L ib ra ri es ] at 0 2: 00 2 2 N ov em be r 20 14 116 Park, Cho, and Chang Figure 5: Effect of Fe2+ dosage on COD removal in Photo-Fenton oxidation. 0.01 M. As expected, the COD removal efficiency was increased by increasing the concentration of H2O2. The optimum H2O2 dosage was found to be 0.1 M. The Effect of Fe(II) on the Color Removal Efficiency In order to determine the effects of Fe(II) on the color removal efficiency, ex- periments were conducted at various Fe(II) dosages under the optimal operating conditions of the Fenton and Photo-Fenton processes. As shown in Figure 7, the Figure 6: Effect of H2O2 dosage on COD removal in Photo-Fenton oxidation. D ow nl oa de d by [ Y or k U ni ve rs ity L ib ra ri es ] at 0 2: 00 2 2 N ov em be r 20 14 Comparison of Fenton and Photo-Fenton Processes 117 Figure 7: Variation of color removal with Fe2+ dosage. color removal efficiency rapidly increased with increasing Fe(II) dosage in the range of 0 – 0.07 M and 0 – 0.006 M in the case of the Fenton and Photo-Fenton processes, respectively. However, in the Fenton process, the color removal effi- ciency was not influenced by the Fe(II) dosage at dosages above 0.07 M. This could be explained by the fact that the addition of a large amount of Fe(II) resulted in a brown turbidity that hindered the absorption of the UV light. Even with no addition of Fe(II) in the Photo-Fenton process, the color re- moval was 25%. This reduction may be due to the photolysis of H2O2 when hydrogen peroxide absorbs the UV light at a wavelength <300 nm (Eq. 5) and the direct photolysis of the organic pollutants. Because the lamp used in this study emits in the UV-C range, the photolysis of H2O2 takes place simultane- ously during the reaction. Due to their direct photolysis, the organic pollutant molecules may enter an excited state in which they can be partly oxidized by the oxygen present in the solution. The Sludge Production Figure 8 shows the sludge production as a function of the Fe2+ dosage under the optimal conditions of the Fenton and Photo-Fenton processes, re- spectively. The sludge production increased rapidly with increasing Fe(II) dosage. As shown in Figure 8, the sludge productions were 36 mL/100 mL and 7.5 mL/100 mL, respectively. Figure 8: Production of sludge with Fe2+ dosage. D ow nl oa de d by [ Y or k U ni ve rs ity L ib ra ri es ] at 0 2: 00 2 2 N ov em be r 20 14 118 Park, Cho, and Chang Figure 9: Variation of fecal coliform removal with reaction time at the optimal conditions. The Fecal Coliform Removal Efficiency Figure 9 shows the fecal coliform removal efficiency under the optimal conditions in the Fenton and Photo-Fenton processes, respectively. The fecal coliform removal efficiency increased rapidly with increasing reaction time. However, in comparing the results of the Photo-Fenton and Fenton oxidation reactions (Fig. 9) it is evident that the Photo-Fenton reaction results in greater and faster reduction of fecal coliform than the Fenton reaction. CONCLUSION Based on the present study of the treatment of livestock wastewater by the Fenton and Photo-Fenton processes, the following conclusions can be drawn. The Fenton oxidation rate is influenced by many factors, such as the pH value, molar ratio of Fe2+/H2O2, and the amounts of hydrogen peroxide and ferrous salt. The optimum conditions for degradation were found to be: a pH of 4, a reaction time of 60 min, a molar ratio of Fe2+/H2O2 of 0.33, a hydrogen peroxide concentration of 0.2 M, and a ferrous salt concentration of 0.066 M. Under the optimal conditions of the Fenton process, the COD, color, and fecal coliform removal efficiencies were about 70, 85, and 96.0%, respectively, and the sludge production was 36 mL from 100 mL of solution. The optimum conditions for degradation in the case of the Photo-Fenton ox- idation were: a pH of 5, a reaction time of 80 min, a ferrous salt concentration of 0.01 M, and a hydrogen peroxide concentration of 0.1 M. Under the optimal conditions of the Photo-Fenton process, the COD, color, and fecal coliform re- moval efficiencies were about 79, 70, and 99.4%, respectively, and the sludge production was 7.5 mL from 100 mL of solution. Based on the results presented in this study, the Photo-Fenton process shows a lower color removal efficiency compared with the Fenton process, but it has a higher COD and fecal coliform removal efficiency under the optimum conditions. Also, the Photo-Fenton process was associated with lower sludge productioncompared with the Fenton process. D ow nl oa de d by [ Y or k U ni ve rs ity L ib ra ri es ] at 0 2: 00 2 2 N ov em be r 20 14 Comparison of Fenton and Photo-Fenton Processes 119 The study of the Fenton and Photo-Fenton processes for livestock wastew- ater treatment is important for developing a new approach to the treatment of highly concentrated livestock wastewater. Based on the results of our study, it can be concluded that the Fenton and Photo-Fenton processes represent good alternative treatment methods for livestock wastewater, provided that the amount of suspended solids is not too high. When the solid concentration is very high, the penetration of light into the Photo-Fenton reactor is impeded. In general, livestock wastewater is treated using conventional biological treatment methods, which do not allow for the effective removal of the COD and color. Based on our results, we suggest that the combined use of the Fenton/Photo-Fenton process with biological treatment would provide a promis- ing alternative to the existing methods because it would take advantage of the best aspects of both methods. REFERENCES 1. Choi, Y.S.; Hong, S.W.; Kim, S.J.; Chung, I.H. Development of a biological process for livestock wastewater treatment using a technique for predominant outgrowth of Bacillus species. Water Sci. Technol. 2002, 45(12), 71–78. 2. U.S. EPA. Feedlot Industry Sector Profile Revised Draft Report. U.S. EPA: Washington, DC, 1998. 3. Chudoba, J. Quantitative estimation in COD of refractory organic compounds pro- duced by activated sludge microorganisms. Water Res. 1985, 19(1), 37–43. 4. Artan, N.; Orhon, D. The effects of reactor hydraulics on the performance of activated sludge systems. II-The formation of microbial products. Water Res. 1989, 23(12), 1519– 1525. 5. Orhon, D.; Artan, N.; Cimtit, Y. The concept of soluble residual product formation in the modeling of activated sludge. Water Sci. Technol. 1989, 21, 339. 6. Kim, S.M.; Geissen, S.U; Vogelpohl, A. Landfill leachate treatment by a photoas- sisted fenton reaction. Water Sci. Technol. 1997, 35(4), 239–248. 7. Bauer, R.; Waldner, G.; Fallmann, H.; Hanger, S.; Klare, M.; Krutzler, T. The photo- fenton reaction and the TiO2/UV process for wastewater treatment–novel developments. Catalysis Today 1999, 53, 131–144. 8. Engwall, M.A.; Pignatello, J.J.; Grasso, D. Degradation and detoxification of the wood preservatives creosote and pentachlorophenol in water by the photofenton reaction. Water Res. 1999, 33(5), 1151–1158. 9. Kang, Y.W.; Hwang, K.Y. Effects of reaction conditions on the oxidation efficiency in the Fenton process. Water Res. 2000, 34(10), 2786–2790. 10. Oh, D.; Jun, S.; Park, S.; Yoon, T. Effects of reaction conditions on wastewater treatment efficiency in Fenton oxidation. J. Korean Soc. Environ. Eng. 1994, 16, 51–59. 11. Jeffery, G.H.; Bassett, J.; Mendham, J.; Denny, R.C. In Vogel’s Textbook of Quanti- tative Chemical Analysis; Longman Scientific and Technical: UK, 1989. 12. Franson, M.A.H.; Eaton, A.D.; Clesceri, L.S.; Greenberg, A.E. Standard Methods for the Examination of Water and Wastewater, 20th Ed.; APHA,AWWA, WEF: Washington, DC, USA, 1998. D ow nl oa de d by [ Y or k U ni ve rs ity L ib ra ri es ] at 0 2: 00 2 2 N ov em be r 20 14 120 Park, Cho, and Chang 13. Meeker, R.E. Stabilization of hydrogen peroxide. US Pat. 3,208,606, 1965. 14. Feurstein, W. Model experiments for the oxidation of aromatic compounds by hy- drogen peroxide in wastewater treatment. Vom vasser 1981, 56, 35–54. 15. Bigda, R.J. Consider Fenton’s chemistry for wastewater treatment. Chem. Eng. Prog. 1995, 91, 62–66. 16. Buxton, G V.; Greenstock, C.L.; Helman, W.P.; Ross, A.B. Critical review of rate constants for reaction of hydrated electrons, hydrogen atoms and hydroxyl radicals in aqueous solution. J. Phys. Chem. Ref. Dat. 1988, 17, 513–886. 17. Walling, C. Fenton’s reagent revisited. Acc. Chem. Res. 1975, 8, 125–131. 18. Jacob, N.; Balakrishnam, I.; Reddy, M.P. Characterization of the hydroxyl radical in some photochemical reactions. J. Phys. Chem. 1977, 81, 17–22. D ow nl oa de d by [ Y or k U ni ve rs ity L ib ra ri es ] at 0 2: 00 2 2 N ov em be r 20 14
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