# The Comparison of Photocatalytic Degradation and Decolorization Processes of Dyeing Effluents

Authors: Ewa Adamek; Wojciech Baran; Justyna Ziemiańska; Andrzej Sobczak
Journal: International Journal of Photoenergy
 (2013)

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## Abstract

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 (λmax 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.


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## Body

## 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 7×105 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 (HO•). 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 [8–10].The photocatalytic process can be carried out under heterogeneous, for example, TiO2 [11, 12] conditions, as follows:
(1)TiO2(aq)+hν→TiO2(hVB+,eCB-)(aq)(2)TiO2(hVB+,eCB-)(aq)+O2→HO•+O2•-+H+
and/or homogeneous conditions, for example, Fe3+ salts [13, 14] as follows:
(3)Fe3+(aq)+hν→Fe2+(aq)+HO•+H+The properties ofTiO2 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 [16–19]. The photocatalytic degradation of pollutants in the presence of Fe(III) salts has been also presented in the literature [20–22], but there are only few papers describing photocatalytic properties of TiO2/FeCl3 mixture [23–25]. 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 [26–29], 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 Table1. 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.Table 1
The characteristics of the investigated dye effluents.
Effluent from dyeing process of
Dyeing technology
Abbreviation in text
Azo dyes in effluents
Other substances in effluents
pH
COD (mgO21)
Max of absorbance (λmax) in raw effluents
Comments
C.I. name
Chemical character
Polyacrylic fibres
Continuous process
WPac
Basic Yellow 28Basic Red 22Basic Blue 41Basic Black
CationicCationicCationicCationic
Thickener (Prisulon),Auxiliary agents (Roksol PAN 3K),Glutaric acids
4.4 ± 0.1
1440
0.262 (340 nm)0.159 (430 nm)0.166 (540 nm)0.199 (610 nm)
Biologically stablea
Acid Red 88
Anionic
Leather
Batch process
WLeat
Acid Blue 193
Anionic
<10% of tannery wastes
7.0 ± 0.1
460
0.365 (510 nm)0.075 (620 nm)
Biologically unstablec
Other dyesb
Anionic
Flax fabric
Batch process
WFlax
Unknown
Anionic
Unknown
6.9 ± 0.1
910
0.965 (350 nm)d
Biologically stablea
Cotton fabric
Batch process
WCot
Direct Black 22
Anionic
Unknown
8.2 ± 0.2
8930
40.05 (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 λ 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%,  pHpzc=3.00±0.05) [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).Table 2
The concentrations of reagents used and experimental conditions.
Effluent
FeCl3  (mmol L−1)
TiO2  (g L−1)
pHa
Concentration of Fe(III) in irradiated effluenta  (mmol L−1)
1.0
—
3.3
n.d.b
WPac
—
2.5
4.4
—
1.0
2.5
3.6
n.d.b
—
—
3.1
0.02
WLeat
—
2.5
7.0
—
1.5
2.5
3.4
0.04
1.5
—
3.2
0.30
WFlax
—
2.5
6.3
—
1.5
2.5
3.2
0.30
13
—
3.0
2.80
WCot
—
2.5
8.8
—
13
2.5
2.8
1.82
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 λmax 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.Figure 1
The scheme of test stand.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 was20±2°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-18.5μm, 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 pH<1) or NaOH (to pH≈13). 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 λmax (Table 3). The analysis of the intermediate products was not performed because it was not the main aim of this study.Table 3
The results of the treatment of dye effluents.
Dyes degradation after
Reduction of color
Effluent
λ
max (nm)
Photocatalytic system
60 min of irradiation
In the photocatalytic process
In the physical  processesY (%)
Total decolorization of effluents atλmax
COD removal after 300 min
after 60 min of irradiation
Total (%)
of irradiationRCOD (%)
X (%)
k
X (min−1)
Z (%)
k
Z (min−1)
FeCl3
~0
~0
2
~0
−606
−593
340
TiO2
37
0.008 ± 0.002
26
0.006 ± 0.002
3
28
TiO2/FeCl3
10
0.002 ± 0.001
78
0.024 ± 0.003
−347
1
FeCl3
~0
~0
~0
~0
−147
−155
430
TiO2
58
0.014 ± 0.003
36
0.008 ± 0.002
4
40
WPac
TiO2/FeCl3
17
0.003 ± 0.002
49
0.010 ± 0.002
−76
11
~0.14.9a
FeCl3
~0
~0
~0
~0
−17
−20
540
TiO2
86
0.030 ± 0.005
57
0.014 ± 0.002
3
58
TiO2/FeCl3
40
0.008 ± 0.002
22
0.004 ± 0.001
−7
17
FeCl3
n.d.b
n.d.
3
~0
4
7
610
TiO2
n.d.
n.d.
83
0.030 ± 0.004
4
84
TiO2/FeCl3
n.d.
n.d.
35
0.006 ± 0.002
11
42
FeCl3
~0
~0
~0
~0
95
95
510
TiO2
24 (63)c
0.004 ± 0.002
11
0.002 ± 0.000
14
24
WLeat
TiO2/FeCl3
~30 (100)c
0.005 ± 0.001
11
0.002 ± 0.001
95
95
~0.40.15a
FeCl3
n.d.
n.d.
~0
~0
100
100
620
TiO2
n.d.
n.d.
21
0.003 ± 0.001
18
36
TiO2/FeCl3
n.d.
n.d.
100
—
96
100
FeCl3
~0e
~0
10
<0.001
50
53
~0
WFlax
350d
TiO2
10e
0.001 ± 0.001
22
0.003 ± 0.002
~0
22
−40
TiO2/FeCl3
35 ÷ 42e
0.008 ± 0.002
50
0.011 ± 0.003
33
66
−33
FeCl3
~0(0)c
~0
~0c
~0
96
96c
~0
WCot
480
TiO2
~0(5)c
~0
5c
~0
~0
5c
11
TiO2/FeCl3
~0(5)c
~0
5c
~0
97
96c
7
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 (Xi) was calculated based on the results obtained from HPLC method according to the following equation:
(4)Xi=100·(1-SiSo),
where  Si  is the peak area corresponding to the ​​undecomposed dye after the irradiation of wastewater, and So  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(kXi) was determined as for the pseudo first-order reaction, that is, as the slope of the following linear dependency:(5)lnSoSi=f(t).Reduction of color in the physical process only (Y) was calculated based on the absorbance of raw, centrifuged effluents (Ao) and the absorbance of the same effluents but after addition of the catalyst (TiO2 and/or FeCl3) and after centrifugation (AY) as follows:
(6)Y=100·(1-AYAo).
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 Y value was negative.Reduction of color in the photocatalytic process only (Z) was determined based on the absorbance of centrifuged effluents with catalysts (TiO2 and/or FeCl3) (AY) and the absorbance of the same effluents but after their irradiation with these catalysts (Az) as follows:
(7)Z=100·(1-AZAY).
In these cases, the reason of effluents decoloration may be the photocatalytic process only.The rate constant for dyes photodecolorization (kZi) was determined as the slope of the following linear function:
(8)lnAYAZ=f(t).Total decolorization of effluents (Total) was calculated using the following formula:(9)Total=100·(1-AzAo).COD removal (RCOD) was determined based on the following equation:
(10)RCOD=100·(1-COD300CODo),
where CODo 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.


## 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 Table1. 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.Table 1
The characteristics of the investigated dye effluents.
Effluent from dyeing process of
Dyeing technology
Abbreviation in text
Azo dyes in effluents
Other substances in effluents
pH
COD (mgO21)
Max of absorbance (λmax) in raw effluents
Comments
C.I. name
Chemical character
Polyacrylic fibres
Continuous process
WPac
Basic Yellow 28Basic Red 22Basic Blue 41Basic Black
CationicCationicCationicCationic
Thickener (Prisulon),Auxiliary agents (Roksol PAN 3K),Glutaric acids
4.4 ± 0.1
1440
0.262 (340 nm)0.159 (430 nm)0.166 (540 nm)0.199 (610 nm)
Biologically stablea
Acid Red 88
Anionic
Leather
Batch process
WLeat
Acid Blue 193
Anionic
<10% of tannery wastes
7.0 ± 0.1
460
0.365 (510 nm)0.075 (620 nm)
Biologically unstablec
Other dyesb
Anionic
Flax fabric
Batch process
WFlax
Unknown
Anionic
Unknown
6.9 ± 0.1
910
0.965 (350 nm)d
Biologically stablea
Cotton fabric
Batch process
WCot
Direct Black 22
Anionic
Unknown
8.2 ± 0.2
8930
40.05 (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 λ 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%,  pHpzc=3.00±0.05) [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).Table 2
The concentrations of reagents used and experimental conditions.
Effluent
FeCl3  (mmol L−1)
TiO2  (g L−1)
pHa
Concentration of Fe(III) in irradiated effluenta  (mmol L−1)
1.0
—
3.3
n.d.b
WPac
—
2.5
4.4
—
1.0
2.5
3.6
n.d.b
—
—
3.1
0.02
WLeat
—
2.5
7.0
—
1.5
2.5
3.4
0.04
1.5
—
3.2
0.30
WFlax
—
2.5
6.3
—
1.5
2.5
3.2
0.30
13
—
3.0
2.80
WCot
—
2.5
8.8
—
13
2.5
2.8
1.82
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 λmax 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.Figure 1
The scheme of test stand.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 was20±2°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-18.5μm, 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 pH<1) or NaOH (to pH≈13). 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 λmax (Table 3). The analysis of the intermediate products was not performed because it was not the main aim of this study.Table 3
The results of the treatment of dye effluents.
Dyes degradation after
Reduction of color
Effluent
λ
max (nm)
Photocatalytic system
60 min of irradiation
In the photocatalytic process
In the physical  processesY (%)
Total decolorization of effluents atλmax
COD removal after 300 min
after 60 min of irradiation
Total (%)
of irradiationRCOD (%)
X (%)
k
X (min−1)
Z (%)
k
Z (min−1)
FeCl3
~0
~0
2
~0
−606
−593
340
TiO2
37
0.008 ± 0.002
26
0.006 ± 0.002
3
28
TiO2/FeCl3
10
0.002 ± 0.001
78
0.024 ± 0.003
−347
1
FeCl3
~0
~0
~0
~0
−147
−155
430
TiO2
58
0.014 ± 0.003
36
0.008 ± 0.002
4
40
WPac
TiO2/FeCl3
17
0.003 ± 0.002
49
0.010 ± 0.002
−76
11
~0.14.9a
FeCl3
~0
~0
~0
~0
−17
−20
540
TiO2
86
0.030 ± 0.005
57
0.014 ± 0.002
3
58
TiO2/FeCl3
40
0.008 ± 0.002
22
0.004 ± 0.001
−7
17
FeCl3
n.d.b
n.d.
3
~0
4
7
610
TiO2
n.d.
n.d.
83
0.030 ± 0.004
4
84
TiO2/FeCl3
n.d.
n.d.
35
0.006 ± 0.002
11
42
FeCl3
~0
~0
~0
~0
95
95
510
TiO2
24 (63)c
0.004 ± 0.002
11
0.002 ± 0.000
14
24
WLeat
TiO2/FeCl3
~30 (100)c
0.005 ± 0.001
11
0.002 ± 0.001
95
95
~0.40.15a
FeCl3
n.d.
n.d.
~0
~0
100
100
620
TiO2
n.d.
n.d.
21
0.003 ± 0.001
18
36
TiO2/FeCl3
n.d.
n.d.
100
—
96
100
FeCl3
~0e
~0
10
<0.001
50
53
~0
WFlax
350d
TiO2
10e
0.001 ± 0.001
22
0.003 ± 0.002
~0
22
−40
TiO2/FeCl3
35 ÷ 42e
0.008 ± 0.002
50
0.011 ± 0.003
33
66
−33
FeCl3
~0(0)c
~0
~0c
~0
96
96c
~0
WCot
480
TiO2
~0(5)c
~0
5c
~0
~0
5c
11
TiO2/FeCl3
~0(5)c
~0
5c
~0
97
96c
7
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 (Xi) was calculated based on the results obtained from HPLC method according to the following equation:
(4)Xi=100·(1-SiSo),
where  Si  is the peak area corresponding to the ​​undecomposed dye after the irradiation of wastewater, and So  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(kXi) was determined as for the pseudo first-order reaction, that is, as the slope of the following linear dependency:(5)lnSoSi=f(t).Reduction of color in the physical process only (Y) was calculated based on the absorbance of raw, centrifuged effluents (Ao) and the absorbance of the same effluents but after addition of the catalyst (TiO2 and/or FeCl3) and after centrifugation (AY) as follows:
(6)Y=100·(1-AYAo).
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 Y value was negative.Reduction of color in the photocatalytic process only (Z) was determined based on the absorbance of centrifuged effluents with catalysts (TiO2 and/or FeCl3) (AY) and the absorbance of the same effluents but after their irradiation with these catalysts (Az) as follows:
(7)Z=100·(1-AZAY).
In these cases, the reason of effluents decoloration may be the photocatalytic process only.The rate constant for dyes photodecolorization (kZi) was determined as the slope of the following linear function:
(8)lnAYAZ=f(t).Total decolorization of effluents (Total) was calculated using the following formula:(9)Total=100·(1-AzAo).COD removal (RCOD) was determined based on the following equation:
(10)RCOD=100·(1-COD300CODo),
where CODo 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 pH≈3 [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.Absorption and decolorization spectra of WPac (a), WLeat (b), WFlax (c), and WCot (d). Solid line (red): initial spectrum of effluent,Ao; dotted line (blue): effluent with TiO2, without UV-a irradiation, AY; solid line (blue): effluent with TiO2, after UV-a irradiation, AZ; (●) total decolorization of effluent with TiO2 (2.5 g L−1) and after UV-a irradiation; (◯) decolorization of effluent as a result of the photocatalytic process in the presence of TiO2 (2.5 g L−1) and after UV-a irradiation.
(a)
(b)
(c)
(d)As can be seen from the UV-VIS spectra shown in Figure2(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 (λmax 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 (Figures2(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 Figure2(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 (pHpzc) was 3.00. In the used dyes effluents, the pHs were always higher than pHpzc and therefore TiO2 surface should be negatively charged as follows:
(11)Ti–OH2+⟺pH<pHpzcTi–OH⟺pH>pHpzcTiO-
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 Figure3, 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.Absorption and decolorization spectra of WPac (a), WLeat (b), WFlax (c), and WCot (d). Solid line (red): initial spectrum of effluent,Ao; dotted line (blue): effluent with TiO2 and FeCl3 but without UV-a irradiation, AY; solid line (blue): effluent with TiO2, FeCl3and after UV-a irradiation, AZ; (●) total decolorization of effluent with TiO2 (2.5 g L−1) and FeCl3 (1.0 mmol L−1) and after UV-a irradiation; (◯) decolorization of effluent as a result of the photocatalytic process in the presence of TiO2 (2.5 g L−1), FeCl3 (1.0 mmol L−1), and after UV-a irradiation.
(a)
(b)
(c)
(d)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 λ<500 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 asCl-, CO32-,    SO4-2, PO43-, and NO3-, which may significantly affect the distribution of hydroxyl radicals in the following process:
(12)XOn-+HO•→XO•(n-1)-+OH-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.


## 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 pH≈3 [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.Absorption and decolorization spectra of WPac (a), WLeat (b), WFlax (c), and WCot (d). Solid line (red): initial spectrum of effluent,Ao; dotted line (blue): effluent with TiO2, without UV-a irradiation, AY; solid line (blue): effluent with TiO2, after UV-a irradiation, AZ; (●) total decolorization of effluent with TiO2 (2.5 g L−1) and after UV-a irradiation; (◯) decolorization of effluent as a result of the photocatalytic process in the presence of TiO2 (2.5 g L−1) and after UV-a irradiation.
(a)
(b)
(c)
(d)As can be seen from the UV-VIS spectra shown in Figure2(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 (λmax 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 (Figures2(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 Figure2(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 (pHpzc) was 3.00. In the used dyes effluents, the pHs were always higher than pHpzc and therefore TiO2 surface should be negatively charged as follows:
(11)Ti–OH2+⟺pH<pHpzcTi–OH⟺pH>pHpzcTiO-
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 Figure3, 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.Absorption and decolorization spectra of WPac (a), WLeat (b), WFlax (c), and WCot (d). Solid line (red): initial spectrum of effluent,Ao; dotted line (blue): effluent with TiO2 and FeCl3 but without UV-a irradiation, AY; solid line (blue): effluent with TiO2, FeCl3and after UV-a irradiation, AZ; (●) total decolorization of effluent with TiO2 (2.5 g L−1) and FeCl3 (1.0 mmol L−1) and after UV-a irradiation; (◯) decolorization of effluent as a result of the photocatalytic process in the presence of TiO2 (2.5 g L−1), FeCl3 (1.0 mmol L−1), and after UV-a irradiation.
(a)
(b)
(c)
(d)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 λ<500 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 asCl-, CO32-,    SO4-2, PO43-, and NO3-, which may significantly affect the distribution of hydroxyl radicals in the following process:
(12)XOn-+HO•→XO•(n-1)-+OH-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.



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*Source: 578191-2013-02-20.xml*