Applied Water Science

, Volume 3, Issue 1, pp 263–270 | Cite as

Heterogeneous Fenton process using steel industry wastes for methyl orange degradation

  • Mohamed E. M. AliEmail author
  • Tarek A. Gad-Allah
  • Mohamed I. Badawy
Open Access
Original Article


Steel industry wastes (iron-containing waste) could be used as a Fenton-catalyst for the decolorization of methyl orange dye. Various reaction conditions were investigated including catalyst concentration, hydrogen peroxide concentration and pH value. The obtained results indicated that the dye degradation rate increases with increasing catalyst and hydrogen peroxide (H2O2) concentrations and with decreasing pH value. Over 98 % decolorization of the dye was achieved within 30 min at optimum reaction conditions; 200 mg/L catalyst and 34 mM H2O2 concentrations at pH 2 for 20 mg/L initial dye concentration. Reaction kinetics was also carried out to determine the order of reaction in both catalyst and H2O2 concentrations. Stability and reusability of Iron-containing waste were investigated. The iron-containing waste as catalyst can be reused several times with nearly same efficiency of Fenton-like oxidation of MO.


Steel waste Fenton-like reaction Methyl orange Decolorization 


Textile dyeing process produced large amounts of wastewater that are discharged into the environment. These effluents usually contain several classes of toxic dyes that exhibit low biodegradability and/or increased toxicity. Thus, effluents not only deteriorate the receiving waters, but also pose significant threat to the aquatic life because of the oxygen deficiency and formation of some toxic products by hydrolysis of dyes in the wastewater. Most of textile dyes are designed to produce long-lasting colors and are resistant to mild oxidation conditions. Therefore, stronger oxidation process is needed to degrade these structures (Dukkanc et al. 2010). For that purpose, advanced oxidation technologies (AOTs) were extensively investigated. These processes rely on the generation of extremely active OH radicals, which are identified as strong and non-selective oxidants of almost all organic compounds (Li et al. 2006). As one of AOTs, Fenton-like (Heterogeneous Fenton) process was used to generate the powerful hydroxyl radicals from H2O2 in the presence of iron as Fe2+ or Fe3+, to decompose many organic compounds including dyes (Dukkanc et al. 2010).

In case of Heterogeneous Fenton reaction, soluble Fe2+ catalyst is replaced by Fe-containing solids. This kind of Fenton reaction has been proved to be also effective in the treatment of industrial wastewater containing non-biodegradable organic pollutants. Furthermore, this process has numerous advantages over classical homogenous Fenton catalysis; e.g. no iron sludge is generated and easy separation of the catalyst from the treated stream (Bautista et al. 2008; Garrido-Ramirez et al. 2010). Various heterogeneous Fenton-like catalysts such as Fe2O3 (Feng et al. 2004), S-doped Fe2O3 (Guo et al. 2010) and Fe3O4 (Zhang et al. 2008) were used for wastewater treatment. Unfortunately, a lot of these catalysts do not exhibit favorable catalytic activity at neutral pH and the working pH values are usually around 3. Therefore, acidifying the wastewater or inputting external energy into the reaction system is a frequently used method to enhance their activity (Muthukumari et al. 2009; Cruz-González et al. 2010; Li et al. 2010). So it is worth to use low cost catalyst to reduce the overall cost of the treatment process while keeping reasonable efficiency.

In this study, the waste produced from steel industry was used as a catalyst in heterogeneous Fenton oxidation process. Steel is manufactured by the chemical reduction of iron ore, using an integrated steel manufacturing process or a direct reduction process. In the conventional integrated steel manufacturing process, the iron from the blast furnace is converted to steel in a basic oxygen furnace (BOF). Steel can also be made in an electric arc furnace (EAF) from scrap steel and, in some cases, from direct reduced iron. Three major waste streams are generated during steel manufacturing, air emissions, wastewater and solid waste. The solid waste from the conventional process, including furnace slag and collected dust, is generated at an average rate ranging from 300 kg/t of steel manufactured to 500 kg/t. This waste is rich in iron and can be used as a catalyst in heterogeneous Fenton process for wastewater treatment. The use of iron-containing waste in the treatment of wastewater will hopefully reduce the cost of wastewater treatment.

This work focuses on the use of iron-containing waste instead of iron salts as a catalyst in heterogeneous Fenton process using methyl orange as a model compound for dye wastewater. The effect of different reaction conditions (e.g. pH value, catalyst dose, hydrogen peroxide concentration and initial dye concentration) on degradation of dye was assessed along with catalyst reusability.



All chemicals used in this study were of analytical grade and were used without further purification. Iron-containing waste was kindly supplied by Egyptian Company for Iron and Steel and was used after sieving to fine powder. H2O2 (30 %, v/v) and methyl orange (C14H14N3NaO3S; Fig. 1) were purchased from Fluka Company (Germany). Double distilled water was used for the preparation of dye solutions.
Fig. 1

Chemical structure of methyl orange dye

Analysis and procedure

XRD pattern of iron-containing waste (catalyst) was recorded on Bruker diffractometer equipped with graphite monochromatized Cu-Kα radiation (Germany). Amount of leached iron was determined with the aid of atomic absorption spectrometer (Varian, Spectra AA 220). All experiments were conducted in conical flask (250 mL) placed on orbital shaker (Stuart scientific, UK) with 200 rpm rotation speed and under dark circumstance. The reaction suspension containing specified concentrations of both MO dye and steel waste was prepared, and its initial pH was adjusted by diluted H2SO4. The experiments were initiated by adding the desired amount of H2O2 to the reaction mixture. Five milliliter samples were collected at pre-determined time intervals during the reaction, and then NaOH was immediately added to the sample as reaction inhibitor because at first, H2O2 is not stable in alkaline solution and second, the formation of ferric hydroxide complexes leads to a reduction of ·OH radical (Ji et al. 2011). Samples were allowed to settle for short time before measuring absorbance at λmax of methyl orange by UV–Visible spectrophotometer (Jasco V530, Japan).

Results and discussion

XRD characterization of steel industry waste

Iron-containing waste used in this study contains about 90 % of iron as detected by atomic absorption spectrometer. Figure 2 shows XRD pattern of steel industry waste. The diffraction peaks match well with magnetite (Fe3O4) (PDF#72-2303), hematite (Fe2O3) (PDF#871165) and wuestite (Fe0.925O) (PDF#89-0689). The major phase was magnetite (Fe3O4) which provides magnetic property to this waste leading to easy electromagnetic separation from the treated wastewater.
Fig. 2

XRD pattern of steel industry waste; (filled triangle) magnetite, (closed circle) hematite and (open circle) Wüstite phases

Heterogeneous Fenton catalytic activity of steel industry waste

To assess the catalytic activity of iron-containing waste as a catalyst for the degradation of MO via heterogeneous Fenton process, experiments were conducted under different reaction conditions; (1) H2O2 only, (2) catalyst only, and (3) catalyst and H2O2. Figure 3 shows the decolorization rate of 40 mg/L of MO as a function of time at the pre-mentioned conditions. Low and negligible decolorization rate was observed under condition (1) due to the limited oxidation ability of H2O2 compared to hydroxyl radical. While, using steel industry waste led to decolorization efficiency of 21 % after 2 h because of adsorption capability of the catalyst. However, with simultaneous presence of catalyst and H2O2, decolorization efficiency was very close to 98 % within 2 h revealing that iron-containing waste exhibited an excellent catalytic activity and could react with H2O2 to generate more radicals.
Fig. 3

Efficiency of MO decolorization using (1) H2O2, (2) 200 mg/L Iron-containing waste, (3) 200 mg/L catalyst and H2O2 (heterogeneous Fenton process), and (4) 1.9 mg/L Fe3+ and H2O2 (Homogeneous Fenton process). Reaction conditions: 40 mg/L MO, 30 mM H2O2, and pH 4

To exclude the possibility of homogeneous Fenton reaction by the leached iron, the concentration of leached iron was measured using atomic absorption spectrometer and was found to be 0.15 mg/L. Then, homogeneous Fenton process was carried out using the same concentration of iron that was leached out from the catalyst. Under the same operating conditions, the decolorization efficiency of homogeneous Fenton process after 2 h was only 8 % which was much less than that in case of heterogeneous system using iron-containing waste. Therefore, the catalytic activity has been primarily attributed to the steel industry waste catalyst and not to the dissolved iron ions.

A plausible mechanism of Fenton-like reaction using iron-containing waste as a catalyst is illustrated in Eqs. 13. Steel industry waste contains Wüstite (Fe0.925O) which could participate in Fenton reaction according to Eq. 1. The co-presence of both Fe3O4 and Fe2O3 oxides (Fig. 2) may enhance Fenton process by catalyst regeneration through a series of reactions involving hydroperoxyl radicals (HO2·) intermediate (Eqs. 2, 3) and hence, more hydroxyl radicals are generated in the system.
$$ {\text{Fe}}^{2 + } + {\text{H}}_{2} {\text{O}}_{2} \to {\text{Fe}}^{3 + } + \cdot {\text{OH}} + {\text{OH}}^{ - } $$
$$ {\text{Fe}}^{3 + } + {\text{H}}_{2} {\text{O}}_{2} \to {\text{Fe}}^{2 + } + {\text{HO}}_{2}^{ \cdot } + {\text{H}}^{ + } $$
$$ {\text{Fe}}^{3 + } + {\text{HO}}_{2}^{ \cdot } \to {\text{Fe}}^{2 + } + {\text{O}}_{2} + {\text{H}}^{ + } $$

Effect of pH

pH of wastewater has an important effect on heterogeneous Fenton process because pH controls the catalytic activity in the course of affecting the oxidant, the substrate, the dominant iron species, and the stability of hydrogen peroxide (Xu and Wang 2011). Thus, the effect of pH on the MO decolorization by iron-containing waste was investigated at pH range from 2 to 5 (Fig. 4). The results showed that the decolorization rate decreased with the reduction in pH value which is in agreement with classical Fenton process. The complete decolorization of MO was achieved within 60 min at pH 2. While at pH 5, only 55 % decolorization efficiency was gained at same reaction time. These results are also consistent with the previously reported data for the oxidative decolorization of Acid Red 1 solutions by Fe–zeolite Y type catalyst (Hassan and Hameed 2011).
Fig. 4

Effect of pH on decolorization rate of MO; Reaction conditions: 200 mg/L catalyst, 24 mM of H2O2 and 40 mg/L MO

Effect of initial dye concentration

To study the effect of initial dye concentration on the decolorization efficiency, the experiments were carried out using different initial concentration of MO ranging from 10 to 80 mg/L while keeping other conditions invariable. The results are depicted in Fig. 5. The higher the initial dye concentration, the longer the time needed for MO degradation. For instance, the MO concentration was below the detectable level after 30 min for 10, 20 and 40 mg/L initial dye concentrations, whereas 60 and 80 mg/L initial dye concentrations needed 120 min for 99 and 97 % degradation efficiencies, respectively. This phenomenon might be due to the fact that the number of dye molecules is increased but number of OH· is still constant. On the other hand, with the increase in initial concentration of the dye, more dye molecules were adsorbed onto the surface of catalyst (Zhang et al. 2009). Thereby, the generation of ·OH radicals on the surface catalyst is reduced since the active sites were occupied by dye ions.
Fig. 5

Effect of initial dye concentration on decolorization of MO dye; Reaction conditions: 200 mg/L catalyst, 40 mM H2O2 and at pH 2

Effect of catalyst and hydrogen peroxide concentrations

Both the iron-containing waste and hydrogen peroxide concentrations have a significant effect on the rate of heterogeneous Fenton process as production of hydroxyl radicals depends mainly on these two factors according to Eq. 1. The influence of hydrogen peroxide concentration on decolorization rate of MO dye at different catalyst doses by heterogeneous Fenton process is illustrated in Fig. 6. In general, efficiency of heterogeneous Fenton degradation of MO dye increased, when both catalyst and hydrogen peroxide doses increased to some extent due to production of additional hydroxyl radicals.
Fig. 6

Effect of hydrogen peroxide and Catalyst concentrations on degradation rate of MO; a 50, b 100, c 200 and d 250 mg/L catalyst concentrations; Reaction conditions: pH 2 and 20 mg/L MO

The decolorization efficiency of MO increased when hydrogen peroxide concentration increased from 12 to 48 mM. However, further addition of H2O2 to the reaction retarded the color removal. This could be due to that hydrogen peroxide not being selectively converted to hydroxyl radicals but instead autodecomposed to water and oxygen and/or, once radicals have been generated, they are exhausted through scavenging reaction mechanisms by hydrogen peroxide itself to form hydroperoxyl radicals (Eq. 6) with a lower oxidizing power (Hassan and Hameed 2011); the latter can also scavenge hydroxyl radicals according to Eq. 7, (Liao et al. 2009).
$$ {\text{H}}_{2} {\text{O}}_{2} + \cdot {\text{OH}} \to {\text{H}}_{2} {\text{O}} + {\text{HOO}} \cdot $$
$$ {\text{HOO}} \cdot + \cdot {\text{OH}} \to {\text{H}}_{2} {\text{O}} + {\text{O}}_{2} $$
Decolorization rate was also found to increase with the increase in catalyst (iron-containing waste) concentration till reaching maximum value and then slightly decreased upon further addition of the catalyst (Fig. 6). Same phenomenon has been reported by Liao et al. (2009). The inhibition effect of iron species is considered as the reason for this decrease because the scavenging of hydroxyl radicals or other radicals occurs when presenting excessive metal species, which can be expressed by the following equations (Lam et al. 2005; Ramirez et al. 2007; Romero et al. 2009).
$$ {\text{Fe}}^{2 + } + \cdot {\text{OH}} \to {\text{Fe}}^{3 + } + {\text{OH}}^{ - } $$
$$ {\text{Fe}}^{2 + } + \cdot {\text{OOH}} \to {\text{Fe}}^{3 + } + {\text{OOH}}^{ - } $$

Thus, it could be concluded that the optimum catalyst and hydrogen peroxide concentrations for degradation MO dye are 200 mg/L and 24 mM, respectively.

Kinetics of dye decolorization by heterogeneous Fenton reaction

From engineering point of view, it is useful to find out rate equation that fits the experimental data. So, the kinetics of heterogeneous Fenton reaction was studied extensively. The change in the MO concentration with time was described by zero-, half-, and first- and second-order kinetics (Fig. 7) according to Eqs. 10, 11, 12 and 13, respectively, where \( C_{{{\text{MO}}_{t} }} \) is the MO concentration at time t, \( C_{{{\text{MO}}_{0} }} \) is the initial MO concentration and t is time; k0, k0.5, k1, and k2 are the rate constants of the zero-, half-, first- and second-order kinetics, respectively.
$$ C_{t} = C_{0} - k_{0} t,\quad t_{1/2} = \frac{{C_{0} }}{{2k_{0} }} $$
$$ \sqrt {C_{t} } = \sqrt {C_{0} } - \frac{{k_{0.5} }}{2}t,\quad t_{1/2} = \frac{{0.59\sqrt {C_{0} } }}{{k_{0.5} }} $$
$$ \ln C_{t} = \ln C_{0} - k_{1} t,\quad t_{1/2} = \frac{\ln 2}{{k_{1} }} $$
$$ \frac{1}{{C_{t} }} = \frac{1}{{C_{0} }} + k_{2} t,\quad t_{1/2} = \frac{1}{{C_{0} k_{2} }} $$
Fig. 7

Reaction kinetics of MO degradation using different initial dye Concentration: a zero-order, b half-order, c first-order, d second-order reaction kinetics

Table 1 represents the calculated reaction rate constants, half-life time and linear correlation coefficient (R2). At all concentrations of MO, the heterogeneous Fenton degradation of MO is more pronounced in the case of first-order kinetics compared with other orders because reaction rate constant decreases with the increase in initial dye concentration which is consistent with observed data. Also, comparing t1/2 values deduced from Fig. 5 and from Eqs. 10 and 11 confirms that removal of MO via heterogeneous Fenton reaction can be described well by first-order kinetics.
Table 1

Rate constants obtained from linear regression analysis of dye removal using different kinetic models

C0 (ppm)

Zero-oder kinetics

Half-oder kinetics

First-oder kinetics

Second-oder kinetics

k0 (ppm min−1)

t1/2 (min)

R 2

k0.5 (ppm0.5 min−1)

t1/2 (min)

R 2

k (min−1)

t1/2 (min)

R 2

k2 (ppm−1 min−1)

t1/2 (min)

R 2













































It was previously shown that the rate of heterogeneous Fenton oxidation of MO depends mainly on catalyst dose and hydrogen peroxide concentration. Hence, the rate of MO degradation equation can be expressed as in Eq. 15.
$$ - \frac{{{\text{d}}C_{\text{Dye}} }}{{{\text{d}}t}} = kC_{\text{Dye}}^{1} C_{\text{Fe}}^{m} C_{{{\text{H}}_{2} {\text{O}}_{2} }}^{n} $$
where Cdye, CFe, and \( C_{{{\text{H}}_{2} {\text{O}}_{2} }} \) are the concentrations of MO, catalyst and H2O2, respectively, l, m and n are order of reaction in MO, catalyst and H2O2, respectively and k is the rate constant. In order to calculate order of reaction in catalyst and H2O2, it was assumed that the apparent rate constant (calculated from pseudo first order kinetics of decolorization process, Fig. 6) is directly proportional to concentration of both catalyst and hydrogen peroxide; and hence:
$$ k^{ * } = kC_{\text{Fe}}^{m} C_{{{\text{H}}_{2} {\text{O}}_{2} }}^{n} $$
$$ \ln k^{ * } = \ln kC_{{{\text{H}}_{2} {\text{O}}_{2} }}^{n} + m\ln C_{\text{Fe}} $$
$$ \ln k^{ * } = k^{ * * } + m\ln C_{\text{Fe}} ,\quad k^{ * * } = \ln kC_{{{\text{H}}_{2} {\text{O}}_{2} }}^{n} $$
where k* is the apparent rate constant of pseudo-first-order kinetics, k is the actual rate constant.
Figure 8 represents the change in k* as a function in catalyst dose at 20 mg/L of dye concentration. The slope of straight lines represents order of reaction in catalyst concentration (m) which was found to be 1.12 and intercept represents k**. The order of reaction in hydrogen peroxide concentration (n) can be determined by plotting the intercepts (k**) in Fig. 8 against ln H2O2 concentration (Fig. 9). The calculated reaction orders in H2O2 concentration was 0.426. Finally, it can be concluded that the rate equation that describe decolorization of MO dye using steel industry waste is:
$$ - \frac{{{\text{d}}C_{\text{MO}} }}{{{\text{d}}t}} = kC_{\text{MO}} C_{\text{Fe}}^{1.12} C_{{{\text{H}}_{2} {\text{O}}_{2} }}^{0.426} $$
Fig. 8

Change in rate constant with catalyst concentration at different H2O2 concentrations; Reaction conditions: pH 2 and 20 mg/L MO

Fig. 9

Change in k** with different H2O2 concentration

Stability and reusability of iron-containing waste

To assess the stability of iron-containing waste as catalyst in heterogeneous Fenton reaction, samples were analyzed to determine the concentration of dissolved iron ions. The amount of leached iron from waste was 0.15 mg/L after 120 min at pH 2. This result supports that heterogeneous Fenton reaction using steel industry waste was carried out efficiently without iron leaching and this also may support the reuse of this catalyst for several times with same efficiency. After MO decolorization, used waste (catalyst) was separated from solution by magnetic separation and reused for several consecutive MO decolorization processes. As illustrated in Fig. 10, the activity decreased gradually during successive runs. However, the removal rate was rather comparable for all the runs at longer reaction times. 96 % decolorization of MO was still achieved within 45 min and after catalyst being used for 5 cycles.
Fig. 10

Reusability and stability of catalyst


In this study, iron-containing waste was used as a heterogeneous Fenton-catalyst. The iron-containing waste had a high catalytic activity toward the degradation of MO dye in the presence of H2O2 and in acidic pH range. 200 mg/L of waste could catalyze 24 mM H2O2 to achieve 99 % of decolorization efficiency of solution containing 20 mg/L of MO dye in just 30 min at pH 2. Different kinetic models were investigated to determine the exact rate equation that fits the experimental data. First-order kinetics was found to be the best rate equation. Order of reaction in hydrogen peroxide concentration was 0.426, while order of reaction in catalyst concentration was 1.12, respectively. This indicates that rate or reaction was more dependent on catalyst concentration rather than hydrogen peroxide concentration. Results also showed that the catalyst have a good stability and reusability. This study may provide useful information for the use of low cost materials as catalysts in heterogeneous Fenton process catalysts for degradation of organic pollutants.


  1. Bautista P, Mohedano AF, Casas JA, Zazo JA, Rodriguez JJ (2008) An overview of the application of Fenton oxidation to industrial wastewaters treatment. J Chem Technol Biotechnol 83:1323–1338CrossRefGoogle Scholar
  2. Cruz-González K, Torres-López O, García-León A, Guzmán-Mar JL, Reyes LH, Hernández-Ramírez A, Peralta-Hernández JM (2010) Determination of optimum operating parameters for Acid Yellow 36 decolorization by electro-Fenton process using BDD cathode. Chem Eng J 160:199–206CrossRefGoogle Scholar
  3. Dukkanc M, Gunduz G, Yýlmaz S, Prihodko RV (2010) Heterogeneous Fenton-like degradation of Rhodamine 6G in water using CuFeZSM-5 zeolite catalyst prepared by hydrothermal synthesis. J Hazard Mater 181:343–350CrossRefGoogle Scholar
  4. Feng JY, Hu XJ, Yue PL (2004) Discoloration and mineralization of Orange II using different heterogeneous catalysts containing Fe: a comparative study. Environ Sci Technol 38:5773–5778CrossRefGoogle Scholar
  5. Garrido-Ramirez EG, Theng BKG, Mora ML (2010) Clays and oxide minerals as catalysts and nanocatalysts in Fenton-like reactions—a review. Appl Clay Sci 47:182–192CrossRefGoogle Scholar
  6. Guo LQ, Chen F, Fan XQ, Cai WD, Zhang JL (2010) S-doped Fe2O3 as a highly active heterogeneous Fenton-like catalyst towards the degradation of Acid Orange 7 and phenol. Appl Catal B Environ 96:162–168CrossRefGoogle Scholar
  7. Hassan H, Hameed BH (2011) Oxidative decolorization of Acid Red 1 solutions by Fe–zeolite Y type catalyst. Desalin 276:45–52CrossRefGoogle Scholar
  8. Ji F, Li C, Zhang J, Deng L (2011) Efficient decolorization of dye pollutants with LiFe (WO4)2 as a reusable heterogeneous Fenton-like catalyst. Desalin 269:284–290CrossRefGoogle Scholar
  9. Lam SW, Chiang K, Lim TM, Amal R, Low GKC (2005) The role of ferric ion in the photochemical and photocatalytic oxidation of resorcinol. J Catal 234:292–299CrossRefGoogle Scholar
  10. Li YM, Lu YQ, Zhu XL (2006) Photo-Fenton discoloration of the azo dye X-3B over pillared bentonites containing iron. J Hazard Mater B132:196–201CrossRefGoogle Scholar
  11. Li HL, Lei HY, Yu Q, Li Z, Feng X, Yang BJ (2010) Effect of low frequency ultrasonic irradiation on the sonoelectro-Fenton degradation of cationic red X-GRL. Chem Eng J 160:417–422CrossRefGoogle Scholar
  12. Liao Q, Sun J, Gao L (2009) Degradation of phenol by heterogeneous Fenton reaction using multi-walled carbon nanotube supported Fe2O3 catalysts. Colloids Surf A Physicochem Eng Asp 345:95–100CrossRefGoogle Scholar
  13. Muthukumari B, Selvam K, Muthuvel I, Swaminathan M (2009) Photoassisted hetero-Fenton mineralization of azo dyes by Fe-(II)–Al2O3 catalyst. Chem Eng J 153:9–15CrossRefGoogle Scholar
  14. Ramirez JH, Maldonado-Hodar FJ, Perez-Cadenas AF, Moreno-Castilla C, Costa CA, Madeira LM (2007) Azo-dye Orange II degradation by heterogeneous Fenton like reaction using carbon-Fe catalysts. Appl Catal B Environ 75:312–323CrossRefGoogle Scholar
  15. Romero A, Santos A, Vicente F (2009) Chemical oxidation of 2,4-dimethylphenol in soil by heterogeneous Fenton process. J Hazard Mater 162:785–790CrossRefGoogle Scholar
  16. Xu L, Wang J (2011) A heterogeneous Fenton-like system with nanoparticulate zero-valent iron for removal of 4-chloro-3-methyl phenol. J Hazard Mater 186:256–264CrossRefGoogle Scholar
  17. Zhang JB, Zhuang J, Gao LZ, Zhang Y, Hu N, Feng J, Yang DL, Zhu JD, Yan XY (2008) Decomposing phenol by the hidden talent of ferromagnetic nanoparticles. Chemosphere 73:1524–1528CrossRefGoogle Scholar
  18. Zhang H, Fu H, Zhang DB (2009) Degradation of C.I. Acid Orange 7 by ultrasound enhanced heterogeneous Fenton-like process. J Hazard Mater 172:654–660CrossRefGoogle Scholar

Copyright information

© The Author(s) 2013

This article is published under license to BioMed Central Ltd.Open AccessThis article is distributed under the terms of the Creative Commons Attribution License which permits any use, distribution, and reproduction in any medium, provided the original author(s) and the source are credited.

Authors and Affiliations

  • Mohamed E. M. Ali
    • 1
    Email author
  • Tarek A. Gad-Allah
    • 1
  • Mohamed I. Badawy
    • 1
  1. 1.Water Pollution Research DepartmentNational Research CentreCairoEgypt

Personalised recommendations