International Journal of Photoenergy

International Journal of Photoenergy / 2013 / Article

Research Article | Open Access

Volume 2013 |Article ID 578191 | 11 pages |

The Comparison of Photocatalytic Degradation and Decolorization Processes of Dyeing Effluents

Academic Editor: Leonardo Palmisano
Received18 Sep 2012
Revised13 Dec 2012
Accepted19 Dec 2012
Published20 Feb 2013


Treatment of dye effluents resulting from the industrial scale dyeing of cotton, polyacrylic fibres, leather, and flax fabrics by photocatalytic methods was investigated. Photocatalytic processes were initiated by UV-a light ( 366 nm) and were conducted in the presence of TiO2, TiO2/FeCl3, or FeCl3 as photocatalysts. It was found that the photocatalytic process carried out with TiO2 and TiO2/FeCl3 was the most effective method for decolorization of textile dyeing effluents and degradation of dyes, except for effluents containing very high concentrations of stable azo dyes. During the photocatalytic degradation of anionic dyes, a mixture of TiO2/FeCl3 was more effective, while in the case of cationic dyes, more suitable seems to be TiO2 alone.

1. Introduction

The textile industry is recognized as one of a major polluting industry which generates large quantities of wastewater [1]. It is estimated that the annual market for dyes is more than tonnes per year, and about 10%–15% of the world dye production is lost during the dyeing process and released into the environment [2, 3]. The conventional, biological methods widely used in recent years for the treatment of textile effluent containing synthetic stable dyes can often be ineffective [4]. As a result, colored textile effluents containing mixtures of heavy metals, auxiliaries, and recalcitrant materials can be released into the environment. This and the presence of suspended solids and sediments can negatively affect the aquatic life due to the toxicity of these compounds, a depletion of transparency and dissolved oxygen in water [5]. High level of decolorization of dyeing wastewater is achieved using various physicochemical methods, for example, microfiltration, precipitation, coagulation, flocculation, or different sorption techniques commonly with activated carbon [6]. Unfortunately, these methods only lead to the separation of dyes and to their physical transfer in the environment, for example, from water or wastewater to another storage place (e.g., to sludge dumps) but not to their degradation [2, 7]. Therefore, in recent years, special attention has been focused on the studies concerning the use of advanced oxidation processes (AOPs) that base on the production of highly reactive oxygen species including hydroxyl radicals (). AOPs can be an alternative for the treatment of wastewater or effluent containing hardly biodegradable organic compounds because they may lead to the formation of low-molecular-weight carboxylic acids or to complete degradation of pollutants to CO2 and H2O [810].

The photocatalytic process can be carried out under heterogeneous, for example, TiO2 [11, 12] conditions, as follows: and/or homogeneous conditions, for example, Fe3+ salts [13, 14] as follows:

The properties of as a photocatalyst are commonly known and well described in the literature [11, 15]. There have been numerous studies on the removal of organic pollutants including dyes from wastewater on the photoirradiated TiO2 surface [1619]. The photocatalytic degradation of pollutants in the presence of Fe(III) salts has been also presented in the literature [2022], but there are only few papers describing photocatalytic properties of TiO2/FeCl3 mixture [2325]. It was found that a combination of Fe3+ ions and TiO2 in suspension showed a positive synergistic effect accelerating the photodegradation of organic pollutants [24, 25]. However, none of these papers related to the degradation of azo dyes in real wastewaters.

Most of the experiments were conducted in artificial systems with the use of aqueous solutions (often distilled water) that do not mimic the conditions like in real wastewater. Meanwhile, real dyes effluents commonly contain unused dyes, inorganic ions, and other organic substances that can significantly slow down the photocatalytic degradation efficiency of contaminants. So far, there are some papers and reports concerning treatment of real dye wastewater using photocatalytic processes [2629], but they demand more profound investigations. The main objective of the study was to compare the efficiency of photodegradation and decolorization processes carried out in the presence of TiO2 and FeCl3 as well as in the mixture of TiO2/FeCl3 during the treatment of raw real effluents including azodyes. We intended to test four types of wastewaters from large textile factory, industrial tannery, and two from small manufacturies.

2. Experimental

2.1. Characteristics of the Used Effluents

The used raw effluents (without dilution and pretreatment) were obtained from the industrial scale dyeing of cotton (WCot), polyacrylic fibers (WPac), leathers (WLeat), and flax fabrics (WFlax). They contained auxiliary substances used during the dyeing process and also, in the case of WLeat, municipal wastes and tannins. Physical and chemical characteristics of effluents are presented in Table 1. A criterion for choice of wastewater was the presence of azo dyes resistant to biological degradation. The analyzed wastes differed due to the type of used technology and the type of dyed materials. Dyes contained in wastewaters were stable and did not undergo biodegradation during the storage by a period of 28 days in room temperature. To remove sulfides wastes, were intensively aerated for 30 min, before commencement of the experiments.

Effluent from dyeing process of Dyeing technology Abbreviation in text Azo dyes in effluents Other substances in effluents pH COD (mg ) Max of absorbance ( ) in raw effluents Comments
C.I. nameChemical character

Polyacrylic fibresContinuous processWPacBasic Yellow 28
Basic Red 22
Basic Blue 41
Basic Black
Thickener (Prisulon),
Auxiliary agents (Roksol PAN 3K),
Glutaric acids
4.4 ± 0.114400.262 (340 nm)
0.159 (430 nm)
0.166 (540 nm)
0.199 (610 nm)
Biologically stablea

Acid Red 88Anionic
LeatherBatch processWLeatAcid Blue 193Anionic<10% of tannery wastes7.0 ± 0.14600.365 (510 nm)
0.075 (620 nm)
Biologically unstablec
Other dyesbAnionic

Flax fabricBatch processWFlaxUnknownAnionicUnknown6.9 ± 0.19100.965 (350 nm)dBiologically stablea

Cotton fabricBatch processWCotDirect Black 22AnionicUnknown8.2 ± 0.2893040.05 (480 nm)Biologically stablea

aThe biological stability of dyeing effluent was estimated based on changes in their appearance (changes in UV-VIS spectrum, precipitation of sediments) and their digestion during the storage period of 28 days (at 20°C under anaerobic conditions).
bOnly in trace amounts.
cEffluents were digested during short-time storage (about few hours) but their absorbance at 510 nm did not undergo significant changes.
dAbsorption band without any clear maximum.
2.2. Characteristics of Photocatalysts

Titanium (IV) dioxide powder (TiO2) used as the photocatalyst was obtained from Riedel de Haën (anatase 100%, a mean BET surface area of 9–11 m2 g−1, residues on filter >40 μm after dispersion in water <0.02%, ) [30]. During preliminary studies, it was found that during decolorization of cationic dyes solutions this catalyst was more effective than TiO2-P25. Moreover, its mixture with FeCl3 was more effective during decolorization of anionic dyes in distilled water than that with TiO2-P25 [23].

The iron (III) chloride (FeCl3·6H2O) and all other chemicals used for analysis were purchased from POCH (Poland) and were of analytical grade. Freshly prepared FeCl3 stock solution in distilled water (1.0 mol L−1) or solid TiO2 (2.5 g L−1) or a mixture of TiO2 (2.5 g L−1) and FeCl3 (1.0 mol L−1) was added to 100 mL of effluents. The concentrations of TiO2 and FeCl3 were established as optimal, based on preliminary published experiments [23] and according to the unpublished data. The used amount of FeCl3 solution was determined experimentally in such manner that after its addition to effluent, the pH of sample was about 3 (Table 2).

(mmol L−1)
(g L−1)
pHaConcentration of Fe(III) in irradiated effluenta  
(mmol L−1)




aAt the beginning of UV-a irradiation, bno data.
2.3. Irradiation

Before irradiation, the samples with TiO2 were stirred magnetically for 20 min in the dark to ensure the complete equilibrium between adsorption/desorption processes of organic compounds on the photocatalyst surface.

In all experiments, five open glass crystallizers (volume: 500 mL, the exposed surface: 102 cm2) containing 100 mL of effluent with catalysts were irradiated by four UV-a lamps (Philips TL-40 W/05 at 366 nm) in order to ensure the steady-state illumination of the entire surface of crystallizers. The intensity of UV-a and VIS radiation measured by the Quantum-foto radiometer DO9721 (Delta OHM) was 5.35 and 12.0 W m−2, respectively. The scheme of the test stand is shown in Figure 1.

During the whole experiment, all samples were intensively stirred at a constant speed and had a free contact with atmospheric air but were not aerated additionally. During irradiation, the concentration of dissolved oxygen in the samples was >80%. The initial temperature of samples was °C. The pH and concentration of oxygen dissolved in irradiated samples were measured by multimeter HD22569.2 (Delta OHM).

2.4. The Analysis

After the appropriate irradiation time (0–300 min), samples were centrifuged for 30 min at 4000 rpm at room temperature (MPW-360 centrifuge, Poland). The UV-VIS spectra of the irradiated effluents in the range from 200 to 800 nm were recorded by spectrophotometer (Secoman S-750) in 1 cm quartz cuvettes. The concentrations of dyes in samples were determined using HPLC method (HPLC D-7000 Merck, detector UV VIS Hitachi-L 7400, column: Supelcosil LC-18.5 μm, 250 mm × 4.6 mm, mobile phase: 10 mM K2HPO4 at pH 9.0/CH3CN, in the ratio 95 : 5 for WLeat, WFlax, and WCot and 20 mM acetic buffer at pH 4.8/CH3CN, in the ratio 6 : 4 for WPac, resp.). Before HPLC analysis, water-insoluble sediments containing Fe(III) compounds with components of effluents were dissolved after adding the concentrated HCl (to ) or NaOH (to ). The chemical oxygen demand (COD) was estimated by titration method (US EPA 410.1-3) [31]. Additionally, dyes degradation in effluents was determined spectrophotometrically based on the decrease of peaks on characteristic wavelengths at (Table 3). The analysis of the intermediate products was not performed because it was not the main aim of this study.

Dyes degradation after Reduction of color
Effluent (nm) Photocatalytic system 60 min of irradiationIn the photocatalytic process In the physical  processes  
Y (%)
Total decolorization of effluents at COD removal after 300 min
after 60 min of irradiation  Total (%)of irradiation (%)  
X (%) (min−1) Z (%) (min−1)

FeCl3~0~02 ~0−606−593
340TiO2370.008 ± 0.002260.006 ± 0.002328
TiO2/FeCl3100.002 ± 0.001780.024 ± 0.003−3471
430TiO2580.014 ± 0.003360.008 ± 0.002440
WPacTiO2/FeCl3170.003 ± 0.002490.010 ± 0.002−7611 ~0.14.9a
540TiO2860.030 ± 0.005570.014 ± 0.002 3 58
TiO2/FeCl3400.008 ± 0.002220.004 ± 0.001−717
610TiO2n.d.n.d.830.030 ± 0.004484
TiO2/FeCl3n.d.n.d.350.006 ± 0.0021142

510TiO224 (63)c0.004 ± 0.002110.002 ± 0.0001424
WLeatTiO2/FeCl3~30 (100)c0.005 ± 0.001110.002 ± 0.0019595 ~0.40.15a
620TiO2n.d.n.d.210.003 ± 0.0011836

WFlax350dTiO210e0.001 ± 0.001220.003 ± 0.002~022−40
TiO2/FeCl335 ÷ 42e0.008 ± 0.002500.011 ± 0.0033366−33

FeCl3~0 ~0~0c~09696c~0
WCot480TiO2~0 ~05c~0~05c11
TiO2/FeCl3~0 ~05c~09796c7

aIn the presence of FeCl3, TiO2, and TiO2/FeCl3, respectively, bno data, cafter 300 min of UV-a iradiation, dabsorption band without clear maximum, ebased on the peak area measurement at 480 nm using HPLC method.
2.5. Results Elaboration

The degree of degradation for particular dyes () was calculated based on the results obtained from HPLC method according to the following equation: where is the peak area corresponding to the undecomposed dye after the irradiation of wastewater, and is the peak area corresponding to the dye before the irradiation.

Its means that any transformation of dye occurring as a result of the irradiation in the presence of a photocatalyst was considered as its degradation. In this sense, the dye degradation does not mean its mineralization. In the case of azo dyes, their degradation will mean their decomposition to lower and simpler organic compounds by breaking of azo bonds.

The reaction rate constant for dyes photodegradation was determined as for the pseudo first-order reaction, that is, as the slope of the following linear dependency:

Reduction of color in the physical process only () was calculated based on the absorbance of raw, centrifuged effluents () and the absorbance of the same effluents but after addition of the catalyst (TiO2 and/or FeCl3) and after centrifugation () as follows: In these cases, the photocatalyst-containing samples were not exposed to irradiation; that is, the photocatalytic processes did not proceed in them but only adsorption, coagulation, flocculation, and precipitation. In some samples, the addition of FeCl3 resulted in an increased intensity of color in effluents, so the value was negative.

Reduction of color in the photocatalytic process only () was determined based on the absorbance of centrifuged effluents with catalysts (TiO2 and/or FeCl3) () and the absorbance of the same effluents but after their irradiation with these catalysts () as follows: In these cases, the reason of effluents decoloration may be the photocatalytic process only.

The rate constant for dyes photodecolorization () was determined as the slope of the following linear function:

Total decolorization of effluents (Total) was calculated using the following formula:

COD removal () was determined based on the following equation: where was determined in raw effluents and COD300 was determined in the same effluents but after 300 min of UV-a irradiation in the presence of TiO2 and/or FeCl3.

3. Results and Discussion

3.1. Effect of FeCl3

The high photocatalytic activity of Fe(III) salts in model solutions is related to their partial hydrolysis products, namely, Fe(OH)2+ ions, that show the maximum photocatalytic activity in the [13]. The addition of FeCl3 to effluent samples caused precipitation of water-insoluble matter (with the exception of WPac), and almost total their decolorization (Table 3). However, the UV-a irradiation for 60 min did not cause significant changes in UV-Vis spectra and in HPLC chromatograms for any of the analyzed samples. Additionally, after a prolonged irradiation time to 300 min, no significant changes in chromatograms and in COD values were observed.

After the dissolution of water insoluble Fe-organic complexes, chromatograms of samples (before and after UV irradiation) remained practically unchanged. This observation indicates that during UV-a irradiation of effluents with Fe(III) salt only, dyes did not undergo the photocatalytic degradation. The use of FeCl3 and probably also other Fe(III) salts as a catalyst in the photocatalytic treatment process of dye effluents is completely ineffective (after 60 min of irradiation the photodegradation efficiency was in the range of 0%). Therefore, under model conditions, model Fe(OH)2+ ions can have photocatalytic activity at pH 3, but in real wastewater samples, for example, in dye effluents, they may act as a coagulant only.

3.2. Effect of TiO2

After centrifugation of nonirradiated samples with TiO2, no significant changes in UV-VIS spectra (Figure 2) and HPLC chromatograms were observed. Simultaneously, in all effluent samples the photocatalyst was coagulated only in a negligible level.

As can be seen from the UV-VIS spectra shown in Figure 2(a), after UV-a irradiation of samples containing cationic dyes (WPac) with TiO2 for 60 min, the effluent underwent high decolorization resulting in a completely colorless effluent. The disappearance of the absorption bands ( at 340, 430, 520, and 610 nm) suggests that the chromophore groups, responsible for color, progressively break down during UV-a irradiation. Therefore, in the case of cationic dyes, the effluent decolorization was almost exclusively the result of the photocatalytic process and only in a small degree due to physical processes such as precipitation, coagulation, or sorption. The degradation efficiency of cationic dyes was in the range of 37%–86%, but the COD removal was low even after 300 min of irradiation and was only 14% (Table 3).

The decolorization (a decrease in absorbance) was also observed in WLeat and WFlax effluents containing anionic dyes (Figures 2(b) and 2(c)). After irradiation of samples in the presence of TiO2, a decrease of absorbance at 510 and 620 nm for WLeat and a decrease of a continuous band (without any distinct maximum) for WFlax were observed. In the case of effluent resulting from dyeing of leather (WLeat), decolorization was the result of both the photodegradation and the physical processes. The maximum degradation degree of one of the dyes, namely, Acid Red 88, was 63% after 300 min of UV-a irradiation (Table 3).

On the other hand, WFlax effluents irradiated for 60 min with TiO2 exhibited lower dyes degradation, in the range of 10%. The UV-a irradiation for 300 min caused a decrease in COD value about 40% in WLeat effluents and, on the contrary, an increase in COD value of 40% in WFlax (Table 3).

As shown in Figure 2(d), in effluents from cotton dyeing processes (WCot), decolorization and changes in HPLC chromatograms practically were not observed. The degradation degree of dye was <5% even after 300 min UV-a irradiation. In these samples, the degradation efficiency was very low probably because of less transmission of UV-a light through the black effluents. Additionally, WCot samples containing high concentration of dye (Direct Black 22) had the highest COD, over 8900 mg O2 L−1. Therefore, after 300 min of irradiation, the COD removal was about 11% (Table 3).

The photodegradation of compounds during/in heterogeneous photocatalysis depends among other factors on the chemical properties of substrates and their adsorption ability onto the photocatalyst surface [11]. In accordance to heterogeneous catalysis theory (Langmuir- Himselwood model), the increase in adsorption of dyes causes the increase in the photocatalytic degradation rate. Additionally, TiO2 shows an amphoteric character and its photocatalytic activity depends also on the pH of samples. In the case of the investigated TiO2 (pure anatase), the determined pH value of the point of zero charge () was 3.00. In the used dyes effluents, the pHs were always higher than and therefore TiO2 surface should be negatively charged as follows: This fact may explain the higher adsorption and higher photodegradation ability of cationic dyes (in WPac effluents) and lower adsorption of anionic dyes (WCot and WFlax) onto the TiO2 surface under the studied conditions. However, it does not simply explain high degradation of anionic dyes in WLeat effluents. The adsorption process onto TiO2 surface under UV-irradiation conditions is complex and some differences in an adsorption capacity of particles may occur. Probably, a higher removal of COD in WLeat can be attributed to the adsorption of increased amounts of undissociated particles (e.g., anionic dyes with organic or inorganic ions) on the TiO2 surface. Additionally, the organic compounds in WLeat, that is, dyes, surfactant agents, and auxiliaries, were rather photo labile and they were easily transformed to less stable organics (byproducts).

3.3. Effect of TiO2/FeCl3

As shown in Figure 3, the addition of TiO2/FeCl3 mixture to nonirradiated effluents caused a significant coagulation and decolorization of all samples. Therefore, in these processes, Fe salts could play a role of coagulant. However, UV-a irradiation of such samples resulted in their decolorization (Figure 3, Table 3) and this may indicate its role as a photosensitizer.

It was found that the photocatalytic degradation in effluent containing cationic dyes (WPac) was less effective in the mixture of TiO2/FeCl3 than in the presence of TiO2 alone (Table 3). After 60 min of UV-a irradiation, the degradation efficiency of dyes was in the range 10%–40%. Simultaneously, WPac underwent the effective decolorization which can be explained only as the dyes photodegradation (Figure 3(a)). This process was not inhibited by strong coagulation of photocatalysts and by auxiliary substances, contained in these samples. After the addition of TiO2/FeCl3 but before UV-a irradiation, absorbance in WPac effluent at  nm was significantly higher due to the presence of dissolved Fe(III) compounds (dashed line). The data concerning COD removal indicate that the efficiency of WPac mineralization after 300 min of UV-a irradiation reached only 9%.

On the contrary, effluents containing anionic dyes (WLeat and WFlax) underwent the photocatalytic degradation more effectively in the presence of TiO2/FeCl3 than in TiO2 alone (Table 3). Upon UV-a irradiation, there were continuous decreases in absorbance all along the spectra meaning the fragmentation of organic structures and the photocatalytic degradation of dyes (Figures 3(b) and 3(c)). As shown in Table 2, the complete removal of Acid Red 88 from WLeat was the result of both direct precipitation and/or adsorption on the photocatalyst surface and photodegradation process. The degradation efficiency of this dye was high and reached even 100% after 300 min of UV-a irradiation (Table 3). The decolorization of WFlax was caused to a greater extent by the photocatalytic process than coagulation and/or precipitation (Figure 3(c)). The dyes degradation was in the range 35%–42% after 60 min of UV-a irradiation. Removal of COD in WLeat in the presence of TiO2/FeCl3 was 15% and was lower than in the presence of TiO2 alone. On the other hand, similarly as during irradiation of WFlax with TiO2 alone, after 300 min of UV-a irradiation with TiO2/FeCl3 there was not a decrease of COD value but its increase.

In our opinion, an increase in COD removal upon UV-a irradiation of WFlax with TiO2 and TiO2/FeCl3 is only provisional. This effect can be explained by an increase in the concentration of smaller organics molecules formed during the photocatalytic oxidation of dyes and suspended solids. Most of the decomposable compounds are removed in the initial time of this process and the remained part of organic pollutants, for example, lower molecular weight carboxylic acids, aldehydes, and ketones, can be less removable. These byproducts may not be completely mineralized by K2Cr2O7 because they are quite resistant and their chemical oxidation can be the rate-limiting step in oxidation processes. Therefore, they require more severe oxidation conditions or a longer time for their conversion. On the other hand, the COD values enable only qualitative rather than quantitative assessment of the mineralization process [32].

After the addition of TiO2/FeCl3 to WCot, the decolorization was found to be almost 100% resulting in a completely colorless effluent (Figure 3(d)). However, the removal of Direct Black 22 was the result of its precipitation only and not the photocatalytic process. The efficiency of photocatalytic degradation of this dye after 300 min of UV-a irradiation was <5% (Table 3).

Furthermore, the organic load of WCot effluent irradiated with TiO2/FeCl3 did not change significantly; the COD removal remained low at a value of about 7%. Taking into account the high chemical stability of dye (Direct Black 22) in WCot as well as its high concentration in effluent, the photocatalytic degradation of WCot in the presence of TiO2 and TiO2/FeCl3 is not an effective method.

An estimation of the efficiency of the studied photocatalytic systems (TiO2 and TiO2/FeCl3) used during the photocatalytic degradation of real effluents also depends on the chemical properties of dyes and on the possibility of formation of coordination compounds with Fe3+ ions.

In the case of effluents containing cationic dyes (WPac), the addition of Fe(III) salt was unfavorable because the efficiency of photodegradation of these dyes and COD removal were lower than that in the presence of TiO2 only. The explanation of this result can be the change of charge of TiO2 particles (in the presence of Fe3+ ions) that limits the possibility of sorption of the positively charged particles of cationic dyes.

In the case of effluents containing anionic dyes (WLeat and WFlax), the presence of Fe3+ ions had a beneficial effect on the efficiency of photocatalytic degradation of these compounds. The possible explanations may be a formation of photoactive complexes between dyes particles and Fe3+ ions that absorb UV-a irradiation much better than individual molecules of dyes or an adsorption of complexes of dyes with Fe3+ ions on the photocatalyst surface.

The investigated dyes effluents containing also other pollutants, such as fatty acids, sugars, and amino acids which may also be substrates for the photodegradation and can therefore compete with the dyes. Additionally, they may contain inorganic mobile anions, such as , ,    , , and , which may significantly affect the distribution of hydroxyl radicals in the following process:

As a result, these anions at high concentrations can decrease the photodegradation that simultaneously occurs between HO radicals and dyes molecules.

From the viewpoint of COD removal, TiO2 alone was a much more effective photocatalyst than TiO2/FeCl3. The increase in COD value in WFlax effluent probably was connected with the presence of a very persistent substance(s) that did not undergo the oxidation during the COD determination. On the other hand, the photocatalytic process leads to degradation of these substances and the obtained products are much less chemically resistant. In this aspect, the observed phenomenon is not negative. In our publication [33], we have reported, similar to other authors [34], that the complete photocatalytic degradation of contaminants during the treatment of effluents is still not economically feasible due to high operating costs. Therefore, the reduction of time of photocatalytic process only to the time necessary to initial degradation of nonbiodegradable substances (e.g., azo dyes) towards the most readily biodegradable intermediates is the most reasonable. It is obvious that one single treatment step cannot remove all pollutants contained in dyes effluents. The optimal solution is the combination of different treatment processes, for example, the photocatalytic degradation using sunlight as the source of UV light with a biological process. It may significantly decrease the overall cost of the dye effluents treatment. Additionally, the photocatalytic pre-treatment of dyeing effluents can lead to improvement of their biodegradability, for example, initial toxicity induced by photodegradation of textile antraquinone dye to Vibria fisheri progressively decreased during the course of process [35]. In this way, a significant decrease in the overall cost of the treatment of dyes effluents is expected mainly through the combination of several AOPs, for example, the photocatalytic degradation as a pretreatment method with biological processes [36]. An increase of biodegradability of these effluents would facilitate their subsequent biological treatment and an effective removal of undesirable and/or recalcitrant pollutants making the complete mineralization unnecessary.

4. The Mechanism of Wastewater Decolorization Processes

The experiments confirmed that TiO2 caused decolorization of wastewater mainly due to photocatalytic process. However, the decolorization of WLeat could be a result of dyes sorption onto TiO2 surface (Table 3).

As previously described, FeCl3 alone could not be the cause of decolorization of wastewater during the photocatalytic process. On the other hand, the addition of FeCl3 accelerated undoubtedly the photocatalytic degradation of anionic dyes. According to Měšťánková et al., this effect was mainly the result of the synergism of photochemical activity between TiO2 and FeCl3 [24]. However, the results of experiments showing that FeCl3 alone did not exhibit the photochemical activity in wastewater and it decreased the photodegradation rate of cationic dyes may indicate other possible mechanism. It should be noted that even more important is the above described process of intensification of sorption of dyes coordinated with FeCl3 onto TiO2 surface [23]. The other reason could be the fact that the addition of FeCl3 and simultaneously decrease of pH cause agglomeration of suspensions in wastewaters and also increase in stability and photoavailability of the TiO2 used [30].

5. Conclusions

Dyeing effluents irradiated in the presence of FeCl3 alone were decolorized, but azo dyes almost completely did not undergo degradation. On the country, the photocatalytic process carried out with TiO2 and TiO2/FeCl3 as photocatalysts was the effective method of decolorization and dyes photodegradation in the investigated effluents (except samples containing high concentration of very stable azo dye). During the photocatalytic degradation of anionic dyes, a mixture of TiO2/FeCl3 was more effective while in the case of cationic dyes, more suitable seems to be TiO2 alone.


This work was supported by the Medical University of Silesia (Grant no. KNW-1-043/P/2/0).


  1. R. G. Saratale, G. D. Saratale, J. S. Chang, and S. P. Govindwar, “Decolorization and biodegradation of reactive dyes and dye wastewater by a developed bacterial consortium,” Biodegradation, vol. 21, no. 6, pp. 999–1015, 2010. View at: Publisher Site | Google Scholar
  2. T. Robinson, G. McMullan, R. Marchant, and P. Nigam, “Remediation of dyes in textile effluent: a critical review on current treatment technologies with a proposed alternative,” Bioresource Technology, vol. 77, no. 3, pp. 247–255, 2001. View at: Publisher Site | Google Scholar
  3. J. C. Garcia, J. L. Oliveira, A. E. C. Silva, C. C. Oliveira, J. Nozaki, and N. E. de Souza, “Comparative study of the degradation of real textile effluents by photocatalytic reactions involving UV/TiO2/H2O2 and UV/Fe2+/H2O2 systems,” Journal of Hazardous Materials, vol. 147, no. 1-2, pp. 105–110, 2007. View at: Publisher Site | Google Scholar
  4. I. M. C. Gonçalves, A. Gomes, R. Brás, M. I. A. Ferra, M. T. P. Amorim, and R. S. Porter, “Biological treatment of effluent containing textile dyes,” Coloration Technology, vol. 116, pp. 393–397, 2000. View at: Publisher Site | Google Scholar
  5. M. Asgher, H. N. Bhatti, S. A. H. Shah, M. J. Asad, and R. L. Legge, “Decolorization potential of mixed microbial consortia for reactive and disperse textile dyestuffs,” Biodegradation, vol. 18, no. 3, pp. 311–316, 2007. View at: Publisher Site | Google Scholar
  6. B. H. Hameed, A. L. Ahmad, and K. N. A. Latiff, “Adsorption of basic dye (methylene blue) onto activated carbon prepared from rattan sawdust,” Dyes and Pigments, vol. 75, no. 1, pp. 143–149, 2007. View at: Publisher Site | Google Scholar
  7. H. Selcuk, “Decolorization and detoxification of textile wastewater by ozonation and coagulation processes,” Dyes and Pigments, vol. 64, no. 3, pp. 217–222, 2005. View at: Publisher Site | Google Scholar
  8. A. S. Stasinakis, “Use of selected advanced oxidation processes (AOPs) for wastewater treatment—a mini review,” Global NEST Journal, vol. 10, pp. 376–385, 2008. View at: Google Scholar
  9. R. Aplin and T. D. Waite, “Comparison of three advanced oxidation processes for degradation of textile dyes,” Water Science and Technology, vol. 42, no. 5-6, pp. 345–354, 2000. View at: Google Scholar
  10. I. Arslan-Alaton, G. Tureli, and T. Olmez-Hanci, “Treatment of azo dye production wastewaters using Photo-Fenton-like advanced oxidation processes: optimization by response surface methodology,” Journal of Photochemistry and Photobiology A, vol. 202, no. 2-3, pp. 142–153, 2009. View at: Publisher Site | Google Scholar
  11. J. M. Herrmann, “Heterogeneous photocatalysis: state of the art and present applications,” Topics in Catalysis, vol. 34, no. 1–4, pp. 49–65, 2005. View at: Publisher Site | Google Scholar
  12. I. K. Konstantinou and T. A. Albanis, “TiO2-assisted photocatalytic degradation of azo dyes in aqueous solution: kinetic and mechanistic investigations: a review,” Applied Catalysis B, vol. 49, no. 1, pp. 1–14, 2004. View at: Publisher Site | Google Scholar
  13. W. Feng and D. Nansheng, “Photochemistry of hydrolytic iron (III) species and photoinduced degradation of organic compounds. A minireview,” Chemosphere, vol. 41, no. 8, pp. 1137–1147, 2000. View at: Publisher Site | Google Scholar
  14. I. P. Pozdnyakov, Y. A. Sosedova, V. F. Plyusnin et al., “Photodegradation of organic pollutants in aqueous solutions caused by (OH)aq2+ photolysis: evidence of OH radical formation,” International Journal of Photoenergy, vol. 6, no. 2, pp. 89–93, 2004. View at: Google Scholar
  15. U. I. Gaya and A. H. Abdullah, “Heterogeneous photocatalytic degradation of organic contaminants over titanium dioxide: a review of fundamentals, progress and problems,” Journal of Photochemistry and Photobiology C, vol. 9, no. 1, pp. 1–12, 2008. View at: Publisher Site | Google Scholar
  16. O. K. Dalrymple, D. H. Yeh, and M. A. Trotz, “Removing pharmaceuticals and endocrine-disrupting compounds from wastewater by photocatalysis,” Journal of Chemical Technology and Biotechnology, vol. 82, no. 2, pp. 121–134, 2007. View at: Publisher Site | Google Scholar
  17. R. Rajeswari and S. Kanmani, “A study on degradation of pesticide wastewater by TiO2 photocatalysis,” Journal of Scientific and Industrial Research, vol. 68, no. 12, pp. 1063–1067, 2009. View at: Google Scholar
  18. Z. F. Guo, R. X. Ma, and G. J. Li, “Degradation of phenol by nanomaterial TiO2 in wastewater,” Chemical Engineering Journal, vol. 119, pp. 55–59, 2006. View at: Publisher Site | Google Scholar
  19. C. Jia, Y. Wang, C. Zhang, and Q. Qin, “UV-TiO2 photocatalytic degradation of landfill leachate,” Water, Air, and Soil Pollution, vol. 217, no. 1–4, pp. 375–385, 2011. View at: Publisher Site | Google Scholar
  20. V. Sarria, M. Deront, P. Péringer, and C. Pulgarin, “Degradation of a biorecalcitrant dye precursor present in industrial wastewaters by a new integrated iron(III) photoassisted-biological treatment,” Applied Catalysis B, vol. 40, no. 3, pp. 231–246, 2003. View at: Publisher Site | Google Scholar
  21. L. Poulain, G. Mailhot, P. Wong-Wah-Chung, and M. Bolte, “Photodegradation of chlortoluron sensitised by iron(III) aquacomplexes,” Journal of Photochemistry and Photobiology A, vol. 159, no. 1, pp. 81–88, 2003. View at: Publisher Site | Google Scholar
  22. C. Catastini, S. Rafqah, G. Mailhot, and M. Sarakha, “Degradation of amitrole by excitation of iron(III) aquacomplexes in aqueous solutions,” Journal of Photochemistry and Photobiology A, vol. 162, no. 1, pp. 97–103, 2004. View at: Publisher Site | Google Scholar
  23. W. Baran, A. Makowski, and W. Wardas, “The influence of FeCl3 on the photocatalytic degradation of dissolved azo dyes in aqueous TiO2 suspensions,” Chemosphere, vol. 53, no. 1, pp. 87–95, 2003. View at: Publisher Site | Google Scholar
  24. H. Měšťánková, J. Krýsa, J. Jirkovský, G. Mailhot, and M. Bolte, “The influence of Fe(III) speciation on supported TiO2 efficiency: example of monuron photocatalytic degradation,” Applied Catalysis B, vol. 58, pp. 185–191, 2005. View at: Publisher Site | Google Scholar
  25. J. Zhang, D. Fu, Q. Peng, L. Deng, and X. Yang, “Fe3+-assisted photocatalytic oxidation of sulfamethazine in TiO2 suspended solution,” Fresenius Environmental Bulletin, vol. 20, no. 4, pp. 1051–1056, 2011. View at: Google Scholar
  26. I. A. Alaton, I. A. Balcioglu, and D. W. Bahnemann, “Advanced oxidation of a reactive dyebath effluent: Comparison of O3, H2O2/UV-C and TiO2/UV-A processes,” Water Research, vol. 36, no. 5, pp. 1143–1154, 2002. View at: Publisher Site | Google Scholar
  27. P. A. Pekakis, N. P. Xekoukoulotakis, and D. Mantzavinos, “Treatment of textile dyehouse wastewater by TiO2 photocatalysis,” Water Research, vol. 40, no. 6, pp. 1276–1286, 2006. View at: Publisher Site | Google Scholar
  28. C. C. Liu, Y. H. Hsieh, P. F. Lai, C. H. Li, and C. L. Kao, “Photodegradation treatment of azo dye wastewater by UV/TiO2 process,” Dyes and Pigments, vol. 68, no. 2-3, pp. 191–195, 2006. View at: Publisher Site | Google Scholar
  29. J. C. Garcia, J. I. Simionato, A. E. C. Silva, J. Nozaki, and N. E. de Souza, “Solar photocatalytic degradation of real textile effluents by associated titanium dioxide and hydrogen peroxide,” Solar Energy, vol. 83, no. 3, pp. 316–322, 2009. View at: Publisher Site | Google Scholar
  30. W. Baran, E. Adamek, and A. Makowski, “The influence of selected parameters on the photocatalytic degradation of azo-dyes in the presence of TiO2 aqueous suspension,” Chemical Engineering Journal, vol. 145, no. 2, pp. 242–248, 2008. View at: Publisher Site | Google Scholar
  31. “Methods for Chemical Analysis of Water and Wastes, Chemical Oxygen Demand, Titrimetric Methods 410.1-3,” US EPA United States Environmental Protection Agency, Office of Research and Development, Washington, DC, USA, EPA/600/4-79/020, pp. 443–451, March 1983, View at: Google Scholar
  32. W. Baran, A. Makowski, and W. Wardas, “Changes in COD values in aqueous solutions of the selected azo dyes during the photocatalytic degradation process,” in Micropollution in the Human Environment, vol. 51, pp. 215–221, Częstochowa University of Technology Publishing House, Częstochowa, Poland, 2003. View at: Google Scholar
  33. W. Baran, J. Sochacka, and W. Wardas, “Toxicity and biodegradability of sulfonamides and products of their photocatalytic degradation in aqueous solutions,” Chemosphere, vol. 65, no. 8, pp. 1295–1299, 2006. View at: Publisher Site | Google Scholar
  34. E. Bizani, K. Fytianos, I. Poulios, and V. Tsiridis, “Photocatalytic decolorization and degradation of dye solutions and wastewaters in the presence of titanium dioxide,” Journal of Hazardous Materials, vol. 136, no. 1, pp. 85–94, 2006. View at: Publisher Site | Google Scholar
  35. C. Lizama, J. Freer, J. Baeza, and H. D. Mansilla, “Optimized photodegradation of reactive blue 19 on TiO2 and ZnO suspensions,” Catalysis Today, vol. 76, no. 2–4, pp. 235–246, 2002. View at: Publisher Site | Google Scholar
  36. D. Mantzavinos and E. Psillakis, “Enhancement of biodegradability of industrial wastewaters by chemical oxidation pre-treatment,” Journal of Chemical Technology and Biotechnology, vol. 79, no. 5, pp. 431–454, 2004. View at: Publisher Site | Google Scholar

Copyright © 2013 Ewa Adamek et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

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