# Removal of the Hazardous Congo Red Dye through Degradation under Visible Light Photocatalyzed by C,N Co-Doped TiO2 Prepared from Chicken Egg White

Authors: Nurul H. Aprilita; Della Amalia; Endang T. Wahyuni
Journal: The Scientific World Journal
 (2022)

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## Abstract

The C,N co-doped TiO2 photocatalyst was prepared by interacting the chicken egg white having various weights (1, 2, and 4 g) with 1 g of TiO2 in an autoclave through the hydrothermal process at 150°C. The C,N co-doped TiO2 photocatalysts were characterized using Fourier transform infrared (FTIR), X-ray diffraction (XRD), specular reflectance UV/visible (SRUV/Vis), and transmission electron microscope (TEM) instruments. The photocatalytic activity of the co-doped TiO2 was evaluated by monitoring the photo-decolorization of Congo red dye under visible light through a batch experiment. The characterization results assigned that the C and N atoms from the chicken egg white have been successfully co-doped into TiO2 through interstitial and substitutional combination, which could notably narrow their band gap energy entering into the visible region. In line with the gap narrowing, the co-doping C,N into TiO2 could remarkably improve the photocatalytic activity under visible light in the dye photo-decolorization. The enhancement of the photocatalyst activity of TiO2-C,N was controlled by the weight of the egg white introduced, and 2 g of the egg white resulted in the highest activity. Further, the best dye photo-decolorization, which was about 98%, of 10 mg/L Congo red dye in 100 mL of the solution under visible irradiation could be reached by applying TiO2-C,N prepared from 2 g of the egg white, within 45 min, at pH 7, and 50 mg of the photocatalyst mass.


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## Body

## 1. Introduction

Titania (TiO2) is a photocatalyst with several excellent properties such as strong oxidative power, high chemical stability, low cost, and nontoxic [1–26], which has been widely used for the degradation of various toxic chemicals in light irradiation [2, 11, 18, 12–21, 25, 26]. TiO2 with the wide band gap energy (Eg), that is, 3.2 eV (for anatase type), however, has limited application since it can only be activated by UV light [1–3, 6, 8–10, 12] occupying a very small fraction (4–5%) in the solar spectrum [2, 6, 9, 10, 13, 14]. The other recognized weakness of TiO2 is the fast recombination of the electron-hole pair, which results in the low photocatalysis efficiency [6, 9, 10, 12, 13]. The application of TiO2 under cheap and abundant visible light and under solar light is beneficial that has to be afforded. In addition, the retardation of the electron-hole pair recombination in TiO2 is very essential, to get high photocatalysis efficiency.An intensive effort has been directed to narrow the gap in the semiconductor structure of TiO2, that is by doping mono-nonmetallic elements including N [1, 3–10], S [2, 15], and C [12, 16], as well as double nonmetallic dopants, such as C-S [17], N-S [18, 19], N-P [14, 20], and C-N [13, 21–25]. All of the authors have found that the doping could noticeably enhance the visible light absorption and corresponding photocatalytic activity. In addition, some of them [4, 10, 14–17, 24] reported that the doping could not only broader the light absorption spectrum into the visible region to make it visible light active, but also promoted the separation of the hole-electron pair, which slowed down the recombination and so enhanced the efficiency of the photocatalysis process. The doping approach offers solutions for the two drawbacks of TiO2. Furthermore, compared with single-doped TiO2 photocatalysts, the doped TiO2 with two or more elements showed higher enhancement photocatalytic activity due to the beneficial synergy effect from the multi-dopants [14, 18, 21–24, 26].Among the two dopant combinations, the double dopants of C-N are believed to be of high interest because it possesses both enhanced visible light absorption and separation efficiency of electron-hole pairs, which can contribute remarkably to improving photocatalytic activity [13, 21–25]. Many studies have focused on the preparation of C,N-doped TiO2, which frequently introduced two sources for the respective double dopants such as CCl4 and polyaniline [15], nitric acid and nonionic surfactant [22], and nitrate acid and acetylacetone [24]. Using a single source including diaminopyridine [13], polyaniline [21], and tetramethylammonium hydroxide [23] has gained a satisfactory result in constructing C,N co-doped TiO2. In comparison with the multisources, the single source has resulted in the more active co-doped TiO2 [18] due to the lesser residual of the dopant source left that impurified the TiO2 surface. In addition, the use of the single source of dopant is believed to be more practice and lower cost compared with the multisources [13, 18, 21, 23].Many works have been addressed in the introducing single source for C,N dopants [13, 21, 23]; however, to the best of our knowledge, very limited study relates to protein in the chicken egg as the single source for multi-dopants on TiO2 [26]. A study [27] presented that the main components of the fresh chicken egg white are water (88.80%w), protein (10.60%w), carbohydrates (0.80%w), lipid (0.10%w), and very low sulfur (0.16%w). It is implied that large N and C atoms can be found in the egg white, allowing the egg white to be a potential single source for C and N multi-dopants.Under the circumstance, in this study, the utilization of fresh chicken egg white as a single source of double dopants of C,N by hydrothermal method is addressed. We realize that a study on the co-doping TiO2 with C and N elements with a single source has been intensively conducted, but the use of the fresh chicken egg white is relatively new. A similar study has been reported [26], but this study dealt with the use of the expired chicken egg white as a single source for C,N,S triple dopants, and the co-doping was conducted by sol-gel method. The C,N,S co-doped TiO2 prepared was examined for rhodamine-B dye photodegradation.In the current research, hydrothermal for co-doped TiO2 preparation is selected because this method involves high temperature, which was 124–200oC within 10–24 h [6], which meets with the temperature needed for decomposition of the compounds in the egg white. The egg white decomposition may result in the smaller compounds, which enable them to incorporate facilely in the TiO2 crystal lattice [2, 26].The activity of the double co-doped photocatalyst in this work is investigated for Congo red (CR) dye removal from aqueous media. Congo red dyes, having a structure as seen in Figure1, are selected as a pollutant probe due to their widely used for coloring cotton and other wearable materials [28–30]. The contamination of water by low levels of dye is noticeable, unpleasant, and hazardous for people’s health and environment [30]. Consequently, the removal of the CR dye from wastewater is urgent to be conducted before reaching the environment. A favorite method for removing dyes is photodegradation, whether by undoped [30] and the doped TiO2 photocatalyst [28, 29], due to the effective destruction by forming harmless smaller molecules. To the best of our knowledge, no references regarding photodegradation of Congo red by TiO2 co-doped with C-N atoms from a single source of chicken egg white can be traced. Under the circumstance, in this study, the photodegradation of Congo red over the co-doped TiO2 under visible light is addressed. To obtain a condition giving maximum dye photodegradation, the photocatalyst dose, contact time, and solution pH are optimized.Figure 1
Chemical structure of Congo red dye.


## 2. Materials and Methods

### 2.1. Material

TiO2 P25, Congo red dye, HCl, and NaOH in the analytical grade were purchased from Merck Company and were used without any purification. Chicken eggs were collected from a public market in Yogyakarta, Indonesia.


### 2.2. Preparation of the Doped-TiO2 by Hydrothermal

In a typical process, 1 g of TiO2 suspended in water was mixed with chicken egg white with various weights (1, 2, and 4 g) accompanied by constant stirring at 500 rpm for 2 h. The mixture then was transferred into an autoclave to be heated in the oven at 180°C for 4 h. Afterward, the photocatalyst was collected, dried at 100°C for 2 h, and calcined at 500°C for 2 h. The samples obtained were coded as TiO2-C,N (1 : 1), TiO2-C,N (1 : 2), and TiO2-C,N (1 : 4) following the weight ratio of TiO2 powder to the egg white.


### 2.3. Characterization of the Co-Doped Photocatalysts

Characterizations of the undoped and co-doped TiO2 samples were conducted by several instruments, as explained below. The Fourier transform infrared (FTIR) spectra of the samples were recorded on a Shimadzu Prestige 21 FTIR spectrophotometer using the KBr pellet technique in the range of 4000–400 cm−1 to detect the functional group changes. PharmaSpec UV-1799 specular reflectance UV-visible (SRUV-visible) spectrophotometer was used to determine the Eg. A Shimadzu 6000X XRD powder diffractometer using Cu-Kα radiation with 40 KV of the potential and 30 mA of the current was operated for crystallinity detection. The surface morphology of the co-doped TiO2 samples was observed by transmission electron microscope (TEM), which was taken on a JEOL JEM-2010 electron microscope operated at an accelerated voltage of 200 kV.


### 2.4. Photo-Decolorization of Dye Over TiO2-C,N

The dye photo-decolorization was conducted through a batch experiment in a set of closed apparatus (Figure2) equipped with wolfram (visible light source) and/or deuterium lamp (UV light source) with TL-D intensity @20 W, 2000 lm/m2. A mixture of 100 mL of a solution containing 10 mg/L Congo red and 10 mg of the TiO2 powder was exposed under visible light for 45 min along with the constant rate of stirring. The solution from the photo-decolorization separated by filtration was analyzed by a UV-visible spectrophotometer at 510 nm of the wavelength to observe its absorbance. The absorbance observed then was interpolated into the respective standard curve, to get the dye concentration left in the solution. The dye photo-decolorization presented in % was calculated by following formula:(1)%photo−decolorization=C0−C1C0⋅100%,where Co is initial amount of Congo red (mg) and Cl is the amount of Congo red undegraded or left in the solution (mg).Figure 2
A set of apparatus used for photo-process, composed of (a) melamine box, (b) UV or visible lamps, (c) magnetic stirrer plate, (d) beaker glass, (e) magnetic stirrer bar, and (f) sample solution.The same procedure was duplicated for serial processes using TiO2-C,N (1 : 1), TiO2-C,N (1 : 2), and TiO2-C,N (1 : 4), as well as with various photocatalyst mass (10, 30, 50, 70, and 100 mg), variation of the irradiation time (5, 15, 30, 45, 60, 75, 90, and 120 min), and pH alteration (2, 4, 6, 8, and 10).


## 2.1. Material

TiO2 P25, Congo red dye, HCl, and NaOH in the analytical grade were purchased from Merck Company and were used without any purification. Chicken eggs were collected from a public market in Yogyakarta, Indonesia.


## 2.2. Preparation of the Doped-TiO2 by Hydrothermal

In a typical process, 1 g of TiO2 suspended in water was mixed with chicken egg white with various weights (1, 2, and 4 g) accompanied by constant stirring at 500 rpm for 2 h. The mixture then was transferred into an autoclave to be heated in the oven at 180°C for 4 h. Afterward, the photocatalyst was collected, dried at 100°C for 2 h, and calcined at 500°C for 2 h. The samples obtained were coded as TiO2-C,N (1 : 1), TiO2-C,N (1 : 2), and TiO2-C,N (1 : 4) following the weight ratio of TiO2 powder to the egg white.


## 2.3. Characterization of the Co-Doped Photocatalysts

Characterizations of the undoped and co-doped TiO2 samples were conducted by several instruments, as explained below. The Fourier transform infrared (FTIR) spectra of the samples were recorded on a Shimadzu Prestige 21 FTIR spectrophotometer using the KBr pellet technique in the range of 4000–400 cm−1 to detect the functional group changes. PharmaSpec UV-1799 specular reflectance UV-visible (SRUV-visible) spectrophotometer was used to determine the Eg. A Shimadzu 6000X XRD powder diffractometer using Cu-Kα radiation with 40 KV of the potential and 30 mA of the current was operated for crystallinity detection. The surface morphology of the co-doped TiO2 samples was observed by transmission electron microscope (TEM), which was taken on a JEOL JEM-2010 electron microscope operated at an accelerated voltage of 200 kV.


## 2.4. Photo-Decolorization of Dye Over TiO2-C,N

The dye photo-decolorization was conducted through a batch experiment in a set of closed apparatus (Figure2) equipped with wolfram (visible light source) and/or deuterium lamp (UV light source) with TL-D intensity @20 W, 2000 lm/m2. A mixture of 100 mL of a solution containing 10 mg/L Congo red and 10 mg of the TiO2 powder was exposed under visible light for 45 min along with the constant rate of stirring. The solution from the photo-decolorization separated by filtration was analyzed by a UV-visible spectrophotometer at 510 nm of the wavelength to observe its absorbance. The absorbance observed then was interpolated into the respective standard curve, to get the dye concentration left in the solution. The dye photo-decolorization presented in % was calculated by following formula:(1)%photo−decolorization=C0−C1C0⋅100%,where Co is initial amount of Congo red (mg) and Cl is the amount of Congo red undegraded or left in the solution (mg).Figure 2
A set of apparatus used for photo-process, composed of (a) melamine box, (b) UV or visible lamps, (c) magnetic stirrer plate, (d) beaker glass, (e) magnetic stirrer bar, and (f) sample solution.The same procedure was duplicated for serial processes using TiO2-C,N (1 : 1), TiO2-C,N (1 : 2), and TiO2-C,N (1 : 4), as well as with various photocatalyst mass (10, 30, 50, 70, and 100 mg), variation of the irradiation time (5, 15, 30, 45, 60, 75, 90, and 120 min), and pH alteration (2, 4, 6, 8, and 10).


## 3. Results and Discussion

### 3.1. Characterization Data

#### 3.1.1. FTIR Data

Figure3 displays the FTIR spectra of the chicken egg white, TiO2, and all of the TiO2-C,N photocatalysts. The spectra of the chicken egg white (Figure 3(a)) present several absorption peaks located at 3448, 1651, 1543, 1234, and 1072 cm−1 that were attributed to O-H and/or N-H stretching vibration, the bending vibration of O-H bond, and/or C=O bonds from amide I in protein, the N-H bond of amide II in protein, the bond of C-N from amide III in protein, and the C-O bond vibration, respectively [31]. The several characteristic peaks suggest the presence of protein as the main component in the chicken egg white.Figure 3
FTIR spectra of (a) chicken egg white, (b) TiO2, (c) TiO2-C,N (1 : 1), (d) TiO2-C,N (1 : 2), and (e) TiO2-C,N (1 : 4).In the FTIR spectra of TiO2 (Figure 3(b)), the characteristic peaks are seen at 800 and 650 cm−1 that were attributed to Ti-O-Ti and O-Ti-O bond vibrations of the TiO2 lattice [1, 3, 15]. In addition, the broad absorbance peak located at 3400 cm−1 and the sharp peak at 1640 cm−1 are also observed, which were assigned to O-H stretching and bending vibrations, respectively, of water adsorbed on the surface of TiO2 [2, 8, 12, 13].For the case of all co-doped TiO2-C,N samples, similar peaks to that of TiO2, with some additional new absorbance peaks, are observable. The new weak peak appears at 1527 cm−1 that could be ascribed to the N-H bond, as also found in the chicken egg white [31]. This peak suggests the presence of the residual of undecomposed protein from the egg. Another peak located at 1380 cm−1 indicated the presence of -NO3 absorbed [6] and/or -CO from -COO- of the amino acid group [31]. The peak corresponding to 1249 cm−1 was characteristic absorption of C-O bond [16] and/or of N-Ti bond [6]. The characteristic absorption spectrum of N-Ti bond is also seen at 1126 cm−1 [16]. The absorbance peak appearing at 1041 cm−1 was linked to the presence of Ti-C [16] and/or Ni-Ti [9]. The intensities of the presented peaks are seen to increase when the egg weights applied were enlarged. The appearance of the Ti-C and Ti-N bonds in the co-doped TiO2 suggests that C and N species have been incorporated into the TiO2 lattice, which may be through the substitutional of O atoms from TiO2 by C and N dopant atoms [3, 6]. The lasts are very weak peaks at 2901, 2862, 2368, and 2337 cm−1 that are observable in all samples. According to Lin [2], the weak peaks at 2368 cm−1 can be attributed to CO2 gas adsorbed on the TiO2 samples; meanwhile, the rest peaks were most possible from organic compounds polluting the KBr as pelleting material [2, 10].


#### 3.1.2. XRD Data

The XRD patterns of C,N-doped TiO2 prepared with different quantities of chicken egg white, along with the un-co-doped TiO2, are demonstrated in Figure 4. All samples present diffraction peaks at 25.091, 37.651, 48.021, 53.891, 55.071, 62.381, 68.701, 70.041, and 75.001 of the 2θ, which are well fitted with those of the standard anatase phase of TiO2 recorded by JCPDS card number of 01-071-1167 [1, 4, 13].Figure 4
XRD patterns of (a) TiO2, (b) TiO2-C,N (1 : 1), (c) TiO2-C,N (1 : 2), and (d) TiO2-C,N (1 : 4).The characteristic pattern of TiO2 crystal is noticeable in the XRD patterns of all TiO2-C,N samples, with no detectable dopant-related peaks. The figure also informs that the co-doping C,N into TiO2 leads to a decrease in the diffraction peak intensities, and the decrease is proportional to the weight of the egg white as the C,N dopant source. The decrease in the intensities implied a reduction in the crystallinity of TiO2 due to the partial structural distortion [10, 15]. It is also exhibited that the larger structural distortion of TiO2 occurred as the enhancement of the egg white weight since more C and N have been dopped. The distortion of the crystal could provide evidence that C and N from the white egg were successfully doped via substitutional mechanism [1, 3, 4, 6, 13].


#### 3.1.3. UV/Visible Reflectance Data

The UV/visible reflectance spectra of the co-doped photocatalysts are presented in Figure5. Based on data in Figure 5, using the Tauc plot, the respective Eg values were obtained as illustrated in Figure 6. The absorption edge wavelengths and Eg values are displayed in Table 1. From Figure 5 and Table 1, it is apparent that the co-doping C and N atoms into TiO2 have remarkably shifted the light absorption into the visible region. The shift was created by narrowing the gap in the TiO2 semiconductor structure [4, 6, 13, 15, 18, 19], due to the double atoms incorporated in the lattice of TiO2 crystal [6]. Furthermore, the decrease in Eg, as seen in Figure 6 and Table 1, was found to be more effective when the amount of the dopant source was enlarged since more amount of C and N dopants could occupy the gap. However, with the largest mass of the chicken egg white, a decrease in the band energy was less effective. This opposite trend can be caused by the agglomeration of the organic material from the chicken egg white, which constrains to insert into the lattice crystal of TiO2. The same trend was also reported previously [4, 13, 15, 18, 19]. The significant decrease in the Eg values provides evidence of the interstitial C and N co-doped mechanisms [3, 6, 10].Figure 5
SRUV spectra of (a) TiO2, (b) TiO2-C,N (1 : 1), (c) TiO2-C,N (1 : 2), and (d) TiO2-C,N (1 : 4).Figure 6
Tauc plot result of (a) TiO2, (b) TiO2-C,N (1 : 1), (c) TiO2-C,N (1 : 2), and (d) TiO2-C,N (1 : 4).Table 1
Effect of doping on the band gap energy of TiO2.
SampleTiO2TiO2-C,N (1 : 1)TiO2-C,N (1 : 2)TiO2-C,N (1 : 4)The absorption wavelength (nm)387415450430The band gap energy (eV)3.253.042.692.88


#### 3.1.4. The TEM Data

The TEM images of undoped and the co-doped TiO2 samples are displayed in Figure 7. It is seen that TiO2 particles have a spherical shape of various sizes. In the TiO2-C,N samples, the spherical shapes are seen as darker due to the C,N co-doped into TiO2 lattice. A similar image has also been obtained [24]. The large agglomerates coating the TiO2-C,N surface are observed when a very large weight (4 g) of the egg white was introduced. With the very large amount of the egg white, the protein in the egg white may be incompletely decomposed, resulting in the large organic compound. The large compounds forming agglomerate [2] blocked the TiO2 surface. These TEM images imply the occurrence of the co-doping C and N from the chicken egg white to the TiO2 crystal [25].Figure 7
TEM images of (a) TiO2, (b) TiO2-C,N (1 : 1), (c) TiO2-C,N (1 : 2), and (d) TiO2-C,N (1 : 4).
(a)(b)(c)(d)


### 3.2. Photocatalytic Activity of the Doped TiO2-C,N

#### 3.2.1. The Effect of Co-Doping on the TiO2-C,N Photocatalytic Activity

The activity of the co-doped photocatalyst represented by TiO2-C,N (1 : 2) was evaluated through Congo red photo-decolorization. The effect of the co-doping on the activity of TiO2-C,N under UV and visible light exposure is presented in Figure 8.Figure 8
Dye photo-decolorization results, in the presence of (a) TiO2 + visible, (b) TiO2 + UV, (c) TiO2-C,N (1 : 2) + visible, and (d) TiO2-C,N (1 : 2) + UV (Congo red dye concentration = 10 mg L−1, solution volume = 100 mL, photocatalyst mass = 50 mg, reaction time = 45 min, and pH = 7).Figure8(c) reveals, as expected, that the co-doping has improved the photo-activity of TiO2-C,N in the dye photo-decolorization under visible light irradiation, in comparison with the un-co-doped one (Figure 8(a)). Under visible light irradiation, the dye photo-decolorization over undoped TiO2 was around 57% and the dye photo-decolorization with TiO2-C,N increased up to 91%. The photocatalyst of TiO2-C,N (1 : 2) with Eg as high as 2.67 eV that is equal to the energy of visible light allowed it to strongly absorb the visible light, which could generate an adequate number of OH radicals represented by equation (2) until equation (5) [2]. The radicals played a very important role in the dye decolorization since the radicals can act as strong oxidation agent [11], which was able to destroy the Congo red effectively into smaller molecules such as CO2, H2O, and NO3- [28, 30]. In contrast, the bare TiO2 with Eg of 3.25 eV (Figure 8(a)), which is higher than the energy of the visible light, was constrained to release electrons from the valence band under visible stimulation [2, 3], and so only a few numbers of OH radicals could be provided. Accordingly, the higher effectiveness of the dye photo-decolorization of co-doped TiO2 over un-co-doped TiO2 resulted. A similar trend has been reported by many studies [4, 13, 15, 18].(2)TiO2+light⟶TiO2e−+h+,(3)h++H2O⟶OH+H+,(4)TiOH+h+⟶Ti⋅OH,(5)h++O2⟶O2.The dye photo-decolorization process under UV light over TiO2-C,N (1 : 2) (Figure 8(d)) is much more effective than over the bare TiO2 (Figure 8(b)). It is clear that the co-doping also enhanced the TiO2 activity under UV light, as also found by others [4, 10, 13, 15–17]. The enhancement should be promoted by inhibiting the electron-hole recombination since the dopants can act as a separation center [4, 10, 13, 15–17].


#### 3.2.2. The Influence of the Dopant Loaded in TiO2

The influence of the egg weight introduced into TiO2 towards the activity of the co-doped TiO2 in the dye decolorization is displayed in Figure 9. Concerning the C,N-doped samples, an increase in the activity is observed for all samples compared with the corresponding pure TiO2 materials. Further, it is seen that the increase in the egg weight resulted in higher dye decolorization, but larger egg weight than 2 g caused opposite photo-decolorization result. Many studies have also found a similar trend [4]. The mass of the egg white should be proportional to the amount of C, N co-doped into TiO2. The photocatalyst with the increasing amount of the dopants, having lower Eg, was able to absorb visible light more effectively. This condition provided more number of radicals, which further resulted in the higher dye photo-decolorization.Figure 9
Dye photo-decolorization efficiency under visible process over TiO2-C,N prepared from the egg white with (a) 1 g, (b) 2 g, and (c) 4 g into 1 g TiO2 (Congo red dye concentration = 10 mg L−1, solution volume = 100 mL, photocatalyst mass = 50 mg, reaction time = 45 min, and pH = 7).The heaviest weight of the egg white, implying the largest dopant content, should result in the highest effective photo-decolorization, but the contrary result was observed. In this typical co-doped TiO2, the agglomerate of the organic residual covered the TiO2 surface, as demonstrated by TEM images, which limited the contact of TiO2-C,N (1 : 2) with the light, diminishing OH radical formation. In addition, the covered surface of TiO2 also inhibited the OH radical on the TiO2 surface to contact with the dye. These situations constrained the dye photo-decolorization.From Figures8 and 9, it is notable that the photo-decolorization is enhanced sharply as the length of the irradiation time up to 30 mins, then the slight increase is notified within 35 to 45 mins, but with a longer time than 45 mins, the photo-decolorization is not influenced by time. Similar data have also been reported by others [2]. The extension time could enhance the light penetration to reach the TiO2 surface, which resulted in a larger number of OH radicals, and so that a greater collision frequency occurred between the OH radicals and the dye [2]. These conditions were conducive to dye photo-decolorization. After reaching the maximum formation of the OH radicals and so the photo-decolorization, TiO2-C,N may be saturated that suffered from the formation of the OH radicals, so that the photo-decolorization insignificantly changed or almost constant [2, 10].


#### 3.2.3. The Influence of the Photocatalyst Mass and Solution pH

The photo-decolorization resulting from the process with various photocatalyst mass and pH alteration is displayed in Figure10. In the figure, more effective photo-decolorization could be reached with the enlargement of the photocatalyst mass, but with the higher mass than the optimum level, the photo-decolorization was found to be detrimental. With increasing photocatalyst mass, more OH radicals were provided, hence improving the dye photo-decolorization. In contrast, a very large mass caused more turbid solution, which screened the light penetration, and so the photo-decolorization was retarded [14, 10].Figure 10
Influence of pH on the photo-decolorization, with the photocatalyst mass of (a) 10 mg, (b) 30 mg, (c) 50 mg, and (d) 100 mg in 100 mL of the dye solution (Congo red dye concentration = 10 mg L−1, solution volume = 100 mL, egg white mass = 2 g, and reaction time = 45 min).It is also observable that the photo-decolorization significantly improved when the pH was elevated and reached the maximum level at pH 7. The opposite trend appears at pH higher than 7. At low pH, the surface of TiO2 was protonated by H+ to form positively charged surface [14, 10] and Congo red also existed as cationic form [20, 21]. The same charges refused the interaction between TiO2 surface and Congo red dye molecules, which led to the photo-decolorization being very less effective. It is important to note that most OH radicals are associated with TiO2 surface and for proceeding with the photo-decolorization, and Congo red has to be adsorbed on the surface of the photocatalyst to interact with the OH radicals [12, 19]. Increasing pH can gradually reduce the protonation of both photocatalyst [12] and Congo red molecules [20] to form neutral molecules. The increase in the number of neutral molecules is beneficial to mutually interact, which promoted more effective photo-decolorization. In the solution with higher pH (basic condition), both the surface of TiO2 and the Congo red tended to be negatively charged [12, 20]. Consequently, the interaction between Congo red and the TiO2 photocatalyst was constrained, causing the photo-decolorization declined as shown in Figure 10.


## 3.1. Characterization Data

### 3.1.1. FTIR Data

Figure3 displays the FTIR spectra of the chicken egg white, TiO2, and all of the TiO2-C,N photocatalysts. The spectra of the chicken egg white (Figure 3(a)) present several absorption peaks located at 3448, 1651, 1543, 1234, and 1072 cm−1 that were attributed to O-H and/or N-H stretching vibration, the bending vibration of O-H bond, and/or C=O bonds from amide I in protein, the N-H bond of amide II in protein, the bond of C-N from amide III in protein, and the C-O bond vibration, respectively [31]. The several characteristic peaks suggest the presence of protein as the main component in the chicken egg white.Figure 3
FTIR spectra of (a) chicken egg white, (b) TiO2, (c) TiO2-C,N (1 : 1), (d) TiO2-C,N (1 : 2), and (e) TiO2-C,N (1 : 4).In the FTIR spectra of TiO2 (Figure 3(b)), the characteristic peaks are seen at 800 and 650 cm−1 that were attributed to Ti-O-Ti and O-Ti-O bond vibrations of the TiO2 lattice [1, 3, 15]. In addition, the broad absorbance peak located at 3400 cm−1 and the sharp peak at 1640 cm−1 are also observed, which were assigned to O-H stretching and bending vibrations, respectively, of water adsorbed on the surface of TiO2 [2, 8, 12, 13].For the case of all co-doped TiO2-C,N samples, similar peaks to that of TiO2, with some additional new absorbance peaks, are observable. The new weak peak appears at 1527 cm−1 that could be ascribed to the N-H bond, as also found in the chicken egg white [31]. This peak suggests the presence of the residual of undecomposed protein from the egg. Another peak located at 1380 cm−1 indicated the presence of -NO3 absorbed [6] and/or -CO from -COO- of the amino acid group [31]. The peak corresponding to 1249 cm−1 was characteristic absorption of C-O bond [16] and/or of N-Ti bond [6]. The characteristic absorption spectrum of N-Ti bond is also seen at 1126 cm−1 [16]. The absorbance peak appearing at 1041 cm−1 was linked to the presence of Ti-C [16] and/or Ni-Ti [9]. The intensities of the presented peaks are seen to increase when the egg weights applied were enlarged. The appearance of the Ti-C and Ti-N bonds in the co-doped TiO2 suggests that C and N species have been incorporated into the TiO2 lattice, which may be through the substitutional of O atoms from TiO2 by C and N dopant atoms [3, 6]. The lasts are very weak peaks at 2901, 2862, 2368, and 2337 cm−1 that are observable in all samples. According to Lin [2], the weak peaks at 2368 cm−1 can be attributed to CO2 gas adsorbed on the TiO2 samples; meanwhile, the rest peaks were most possible from organic compounds polluting the KBr as pelleting material [2, 10].


### 3.1.2. XRD Data

The XRD patterns of C,N-doped TiO2 prepared with different quantities of chicken egg white, along with the un-co-doped TiO2, are demonstrated in Figure 4. All samples present diffraction peaks at 25.091, 37.651, 48.021, 53.891, 55.071, 62.381, 68.701, 70.041, and 75.001 of the 2θ, which are well fitted with those of the standard anatase phase of TiO2 recorded by JCPDS card number of 01-071-1167 [1, 4, 13].Figure 4
XRD patterns of (a) TiO2, (b) TiO2-C,N (1 : 1), (c) TiO2-C,N (1 : 2), and (d) TiO2-C,N (1 : 4).The characteristic pattern of TiO2 crystal is noticeable in the XRD patterns of all TiO2-C,N samples, with no detectable dopant-related peaks. The figure also informs that the co-doping C,N into TiO2 leads to a decrease in the diffraction peak intensities, and the decrease is proportional to the weight of the egg white as the C,N dopant source. The decrease in the intensities implied a reduction in the crystallinity of TiO2 due to the partial structural distortion [10, 15]. It is also exhibited that the larger structural distortion of TiO2 occurred as the enhancement of the egg white weight since more C and N have been dopped. The distortion of the crystal could provide evidence that C and N from the white egg were successfully doped via substitutional mechanism [1, 3, 4, 6, 13].


### 3.1.3. UV/Visible Reflectance Data

The UV/visible reflectance spectra of the co-doped photocatalysts are presented in Figure5. Based on data in Figure 5, using the Tauc plot, the respective Eg values were obtained as illustrated in Figure 6. The absorption edge wavelengths and Eg values are displayed in Table 1. From Figure 5 and Table 1, it is apparent that the co-doping C and N atoms into TiO2 have remarkably shifted the light absorption into the visible region. The shift was created by narrowing the gap in the TiO2 semiconductor structure [4, 6, 13, 15, 18, 19], due to the double atoms incorporated in the lattice of TiO2 crystal [6]. Furthermore, the decrease in Eg, as seen in Figure 6 and Table 1, was found to be more effective when the amount of the dopant source was enlarged since more amount of C and N dopants could occupy the gap. However, with the largest mass of the chicken egg white, a decrease in the band energy was less effective. This opposite trend can be caused by the agglomeration of the organic material from the chicken egg white, which constrains to insert into the lattice crystal of TiO2. The same trend was also reported previously [4, 13, 15, 18, 19]. The significant decrease in the Eg values provides evidence of the interstitial C and N co-doped mechanisms [3, 6, 10].Figure 5
SRUV spectra of (a) TiO2, (b) TiO2-C,N (1 : 1), (c) TiO2-C,N (1 : 2), and (d) TiO2-C,N (1 : 4).Figure 6
Tauc plot result of (a) TiO2, (b) TiO2-C,N (1 : 1), (c) TiO2-C,N (1 : 2), and (d) TiO2-C,N (1 : 4).Table 1
Effect of doping on the band gap energy of TiO2.
SampleTiO2TiO2-C,N (1 : 1)TiO2-C,N (1 : 2)TiO2-C,N (1 : 4)The absorption wavelength (nm)387415450430The band gap energy (eV)3.253.042.692.88


### 3.1.4. The TEM Data

The TEM images of undoped and the co-doped TiO2 samples are displayed in Figure 7. It is seen that TiO2 particles have a spherical shape of various sizes. In the TiO2-C,N samples, the spherical shapes are seen as darker due to the C,N co-doped into TiO2 lattice. A similar image has also been obtained [24]. The large agglomerates coating the TiO2-C,N surface are observed when a very large weight (4 g) of the egg white was introduced. With the very large amount of the egg white, the protein in the egg white may be incompletely decomposed, resulting in the large organic compound. The large compounds forming agglomerate [2] blocked the TiO2 surface. These TEM images imply the occurrence of the co-doping C and N from the chicken egg white to the TiO2 crystal [25].Figure 7
TEM images of (a) TiO2, (b) TiO2-C,N (1 : 1), (c) TiO2-C,N (1 : 2), and (d) TiO2-C,N (1 : 4).
(a)(b)(c)(d)


## 3.1.1. FTIR Data

Figure3 displays the FTIR spectra of the chicken egg white, TiO2, and all of the TiO2-C,N photocatalysts. The spectra of the chicken egg white (Figure 3(a)) present several absorption peaks located at 3448, 1651, 1543, 1234, and 1072 cm−1 that were attributed to O-H and/or N-H stretching vibration, the bending vibration of O-H bond, and/or C=O bonds from amide I in protein, the N-H bond of amide II in protein, the bond of C-N from amide III in protein, and the C-O bond vibration, respectively [31]. The several characteristic peaks suggest the presence of protein as the main component in the chicken egg white.Figure 3
FTIR spectra of (a) chicken egg white, (b) TiO2, (c) TiO2-C,N (1 : 1), (d) TiO2-C,N (1 : 2), and (e) TiO2-C,N (1 : 4).In the FTIR spectra of TiO2 (Figure 3(b)), the characteristic peaks are seen at 800 and 650 cm−1 that were attributed to Ti-O-Ti and O-Ti-O bond vibrations of the TiO2 lattice [1, 3, 15]. In addition, the broad absorbance peak located at 3400 cm−1 and the sharp peak at 1640 cm−1 are also observed, which were assigned to O-H stretching and bending vibrations, respectively, of water adsorbed on the surface of TiO2 [2, 8, 12, 13].For the case of all co-doped TiO2-C,N samples, similar peaks to that of TiO2, with some additional new absorbance peaks, are observable. The new weak peak appears at 1527 cm−1 that could be ascribed to the N-H bond, as also found in the chicken egg white [31]. This peak suggests the presence of the residual of undecomposed protein from the egg. Another peak located at 1380 cm−1 indicated the presence of -NO3 absorbed [6] and/or -CO from -COO- of the amino acid group [31]. The peak corresponding to 1249 cm−1 was characteristic absorption of C-O bond [16] and/or of N-Ti bond [6]. The characteristic absorption spectrum of N-Ti bond is also seen at 1126 cm−1 [16]. The absorbance peak appearing at 1041 cm−1 was linked to the presence of Ti-C [16] and/or Ni-Ti [9]. The intensities of the presented peaks are seen to increase when the egg weights applied were enlarged. The appearance of the Ti-C and Ti-N bonds in the co-doped TiO2 suggests that C and N species have been incorporated into the TiO2 lattice, which may be through the substitutional of O atoms from TiO2 by C and N dopant atoms [3, 6]. The lasts are very weak peaks at 2901, 2862, 2368, and 2337 cm−1 that are observable in all samples. According to Lin [2], the weak peaks at 2368 cm−1 can be attributed to CO2 gas adsorbed on the TiO2 samples; meanwhile, the rest peaks were most possible from organic compounds polluting the KBr as pelleting material [2, 10].


## 3.1.2. XRD Data

The XRD patterns of C,N-doped TiO2 prepared with different quantities of chicken egg white, along with the un-co-doped TiO2, are demonstrated in Figure 4. All samples present diffraction peaks at 25.091, 37.651, 48.021, 53.891, 55.071, 62.381, 68.701, 70.041, and 75.001 of the 2θ, which are well fitted with those of the standard anatase phase of TiO2 recorded by JCPDS card number of 01-071-1167 [1, 4, 13].Figure 4
XRD patterns of (a) TiO2, (b) TiO2-C,N (1 : 1), (c) TiO2-C,N (1 : 2), and (d) TiO2-C,N (1 : 4).The characteristic pattern of TiO2 crystal is noticeable in the XRD patterns of all TiO2-C,N samples, with no detectable dopant-related peaks. The figure also informs that the co-doping C,N into TiO2 leads to a decrease in the diffraction peak intensities, and the decrease is proportional to the weight of the egg white as the C,N dopant source. The decrease in the intensities implied a reduction in the crystallinity of TiO2 due to the partial structural distortion [10, 15]. It is also exhibited that the larger structural distortion of TiO2 occurred as the enhancement of the egg white weight since more C and N have been dopped. The distortion of the crystal could provide evidence that C and N from the white egg were successfully doped via substitutional mechanism [1, 3, 4, 6, 13].


## 3.1.3. UV/Visible Reflectance Data

The UV/visible reflectance spectra of the co-doped photocatalysts are presented in Figure5. Based on data in Figure 5, using the Tauc plot, the respective Eg values were obtained as illustrated in Figure 6. The absorption edge wavelengths and Eg values are displayed in Table 1. From Figure 5 and Table 1, it is apparent that the co-doping C and N atoms into TiO2 have remarkably shifted the light absorption into the visible region. The shift was created by narrowing the gap in the TiO2 semiconductor structure [4, 6, 13, 15, 18, 19], due to the double atoms incorporated in the lattice of TiO2 crystal [6]. Furthermore, the decrease in Eg, as seen in Figure 6 and Table 1, was found to be more effective when the amount of the dopant source was enlarged since more amount of C and N dopants could occupy the gap. However, with the largest mass of the chicken egg white, a decrease in the band energy was less effective. This opposite trend can be caused by the agglomeration of the organic material from the chicken egg white, which constrains to insert into the lattice crystal of TiO2. The same trend was also reported previously [4, 13, 15, 18, 19]. The significant decrease in the Eg values provides evidence of the interstitial C and N co-doped mechanisms [3, 6, 10].Figure 5
SRUV spectra of (a) TiO2, (b) TiO2-C,N (1 : 1), (c) TiO2-C,N (1 : 2), and (d) TiO2-C,N (1 : 4).Figure 6
Tauc plot result of (a) TiO2, (b) TiO2-C,N (1 : 1), (c) TiO2-C,N (1 : 2), and (d) TiO2-C,N (1 : 4).Table 1
Effect of doping on the band gap energy of TiO2.
SampleTiO2TiO2-C,N (1 : 1)TiO2-C,N (1 : 2)TiO2-C,N (1 : 4)The absorption wavelength (nm)387415450430The band gap energy (eV)3.253.042.692.88


## 3.1.4. The TEM Data

The TEM images of undoped and the co-doped TiO2 samples are displayed in Figure 7. It is seen that TiO2 particles have a spherical shape of various sizes. In the TiO2-C,N samples, the spherical shapes are seen as darker due to the C,N co-doped into TiO2 lattice. A similar image has also been obtained [24]. The large agglomerates coating the TiO2-C,N surface are observed when a very large weight (4 g) of the egg white was introduced. With the very large amount of the egg white, the protein in the egg white may be incompletely decomposed, resulting in the large organic compound. The large compounds forming agglomerate [2] blocked the TiO2 surface. These TEM images imply the occurrence of the co-doping C and N from the chicken egg white to the TiO2 crystal [25].Figure 7
TEM images of (a) TiO2, (b) TiO2-C,N (1 : 1), (c) TiO2-C,N (1 : 2), and (d) TiO2-C,N (1 : 4).
(a)(b)(c)(d)


## 3.2. Photocatalytic Activity of the Doped TiO2-C,N

### 3.2.1. The Effect of Co-Doping on the TiO2-C,N Photocatalytic Activity

The activity of the co-doped photocatalyst represented by TiO2-C,N (1 : 2) was evaluated through Congo red photo-decolorization. The effect of the co-doping on the activity of TiO2-C,N under UV and visible light exposure is presented in Figure 8.Figure 8
Dye photo-decolorization results, in the presence of (a) TiO2 + visible, (b) TiO2 + UV, (c) TiO2-C,N (1 : 2) + visible, and (d) TiO2-C,N (1 : 2) + UV (Congo red dye concentration = 10 mg L−1, solution volume = 100 mL, photocatalyst mass = 50 mg, reaction time = 45 min, and pH = 7).Figure8(c) reveals, as expected, that the co-doping has improved the photo-activity of TiO2-C,N in the dye photo-decolorization under visible light irradiation, in comparison with the un-co-doped one (Figure 8(a)). Under visible light irradiation, the dye photo-decolorization over undoped TiO2 was around 57% and the dye photo-decolorization with TiO2-C,N increased up to 91%. The photocatalyst of TiO2-C,N (1 : 2) with Eg as high as 2.67 eV that is equal to the energy of visible light allowed it to strongly absorb the visible light, which could generate an adequate number of OH radicals represented by equation (2) until equation (5) [2]. The radicals played a very important role in the dye decolorization since the radicals can act as strong oxidation agent [11], which was able to destroy the Congo red effectively into smaller molecules such as CO2, H2O, and NO3- [28, 30]. In contrast, the bare TiO2 with Eg of 3.25 eV (Figure 8(a)), which is higher than the energy of the visible light, was constrained to release electrons from the valence band under visible stimulation [2, 3], and so only a few numbers of OH radicals could be provided. Accordingly, the higher effectiveness of the dye photo-decolorization of co-doped TiO2 over un-co-doped TiO2 resulted. A similar trend has been reported by many studies [4, 13, 15, 18].(2)TiO2+light⟶TiO2e−+h+,(3)h++H2O⟶OH+H+,(4)TiOH+h+⟶Ti⋅OH,(5)h++O2⟶O2.The dye photo-decolorization process under UV light over TiO2-C,N (1 : 2) (Figure 8(d)) is much more effective than over the bare TiO2 (Figure 8(b)). It is clear that the co-doping also enhanced the TiO2 activity under UV light, as also found by others [4, 10, 13, 15–17]. The enhancement should be promoted by inhibiting the electron-hole recombination since the dopants can act as a separation center [4, 10, 13, 15–17].


### 3.2.2. The Influence of the Dopant Loaded in TiO2

The influence of the egg weight introduced into TiO2 towards the activity of the co-doped TiO2 in the dye decolorization is displayed in Figure 9. Concerning the C,N-doped samples, an increase in the activity is observed for all samples compared with the corresponding pure TiO2 materials. Further, it is seen that the increase in the egg weight resulted in higher dye decolorization, but larger egg weight than 2 g caused opposite photo-decolorization result. Many studies have also found a similar trend [4]. The mass of the egg white should be proportional to the amount of C, N co-doped into TiO2. The photocatalyst with the increasing amount of the dopants, having lower Eg, was able to absorb visible light more effectively. This condition provided more number of radicals, which further resulted in the higher dye photo-decolorization.Figure 9
Dye photo-decolorization efficiency under visible process over TiO2-C,N prepared from the egg white with (a) 1 g, (b) 2 g, and (c) 4 g into 1 g TiO2 (Congo red dye concentration = 10 mg L−1, solution volume = 100 mL, photocatalyst mass = 50 mg, reaction time = 45 min, and pH = 7).The heaviest weight of the egg white, implying the largest dopant content, should result in the highest effective photo-decolorization, but the contrary result was observed. In this typical co-doped TiO2, the agglomerate of the organic residual covered the TiO2 surface, as demonstrated by TEM images, which limited the contact of TiO2-C,N (1 : 2) with the light, diminishing OH radical formation. In addition, the covered surface of TiO2 also inhibited the OH radical on the TiO2 surface to contact with the dye. These situations constrained the dye photo-decolorization.From Figures8 and 9, it is notable that the photo-decolorization is enhanced sharply as the length of the irradiation time up to 30 mins, then the slight increase is notified within 35 to 45 mins, but with a longer time than 45 mins, the photo-decolorization is not influenced by time. Similar data have also been reported by others [2]. The extension time could enhance the light penetration to reach the TiO2 surface, which resulted in a larger number of OH radicals, and so that a greater collision frequency occurred between the OH radicals and the dye [2]. These conditions were conducive to dye photo-decolorization. After reaching the maximum formation of the OH radicals and so the photo-decolorization, TiO2-C,N may be saturated that suffered from the formation of the OH radicals, so that the photo-decolorization insignificantly changed or almost constant [2, 10].


### 3.2.3. The Influence of the Photocatalyst Mass and Solution pH

The photo-decolorization resulting from the process with various photocatalyst mass and pH alteration is displayed in Figure10. In the figure, more effective photo-decolorization could be reached with the enlargement of the photocatalyst mass, but with the higher mass than the optimum level, the photo-decolorization was found to be detrimental. With increasing photocatalyst mass, more OH radicals were provided, hence improving the dye photo-decolorization. In contrast, a very large mass caused more turbid solution, which screened the light penetration, and so the photo-decolorization was retarded [14, 10].Figure 10
Influence of pH on the photo-decolorization, with the photocatalyst mass of (a) 10 mg, (b) 30 mg, (c) 50 mg, and (d) 100 mg in 100 mL of the dye solution (Congo red dye concentration = 10 mg L−1, solution volume = 100 mL, egg white mass = 2 g, and reaction time = 45 min).It is also observable that the photo-decolorization significantly improved when the pH was elevated and reached the maximum level at pH 7. The opposite trend appears at pH higher than 7. At low pH, the surface of TiO2 was protonated by H+ to form positively charged surface [14, 10] and Congo red also existed as cationic form [20, 21]. The same charges refused the interaction between TiO2 surface and Congo red dye molecules, which led to the photo-decolorization being very less effective. It is important to note that most OH radicals are associated with TiO2 surface and for proceeding with the photo-decolorization, and Congo red has to be adsorbed on the surface of the photocatalyst to interact with the OH radicals [12, 19]. Increasing pH can gradually reduce the protonation of both photocatalyst [12] and Congo red molecules [20] to form neutral molecules. The increase in the number of neutral molecules is beneficial to mutually interact, which promoted more effective photo-decolorization. In the solution with higher pH (basic condition), both the surface of TiO2 and the Congo red tended to be negatively charged [12, 20]. Consequently, the interaction between Congo red and the TiO2 photocatalyst was constrained, causing the photo-decolorization declined as shown in Figure 10.


## 3.2.1. The Effect of Co-Doping on the TiO2-C,N Photocatalytic Activity

The activity of the co-doped photocatalyst represented by TiO2-C,N (1 : 2) was evaluated through Congo red photo-decolorization. The effect of the co-doping on the activity of TiO2-C,N under UV and visible light exposure is presented in Figure 8.Figure 8
Dye photo-decolorization results, in the presence of (a) TiO2 + visible, (b) TiO2 + UV, (c) TiO2-C,N (1 : 2) + visible, and (d) TiO2-C,N (1 : 2) + UV (Congo red dye concentration = 10 mg L−1, solution volume = 100 mL, photocatalyst mass = 50 mg, reaction time = 45 min, and pH = 7).Figure8(c) reveals, as expected, that the co-doping has improved the photo-activity of TiO2-C,N in the dye photo-decolorization under visible light irradiation, in comparison with the un-co-doped one (Figure 8(a)). Under visible light irradiation, the dye photo-decolorization over undoped TiO2 was around 57% and the dye photo-decolorization with TiO2-C,N increased up to 91%. The photocatalyst of TiO2-C,N (1 : 2) with Eg as high as 2.67 eV that is equal to the energy of visible light allowed it to strongly absorb the visible light, which could generate an adequate number of OH radicals represented by equation (2) until equation (5) [2]. The radicals played a very important role in the dye decolorization since the radicals can act as strong oxidation agent [11], which was able to destroy the Congo red effectively into smaller molecules such as CO2, H2O, and NO3- [28, 30]. In contrast, the bare TiO2 with Eg of 3.25 eV (Figure 8(a)), which is higher than the energy of the visible light, was constrained to release electrons from the valence band under visible stimulation [2, 3], and so only a few numbers of OH radicals could be provided. Accordingly, the higher effectiveness of the dye photo-decolorization of co-doped TiO2 over un-co-doped TiO2 resulted. A similar trend has been reported by many studies [4, 13, 15, 18].(2)TiO2+light⟶TiO2e−+h+,(3)h++H2O⟶OH+H+,(4)TiOH+h+⟶Ti⋅OH,(5)h++O2⟶O2.The dye photo-decolorization process under UV light over TiO2-C,N (1 : 2) (Figure 8(d)) is much more effective than over the bare TiO2 (Figure 8(b)). It is clear that the co-doping also enhanced the TiO2 activity under UV light, as also found by others [4, 10, 13, 15–17]. The enhancement should be promoted by inhibiting the electron-hole recombination since the dopants can act as a separation center [4, 10, 13, 15–17].


## 3.2.2. The Influence of the Dopant Loaded in TiO2

The influence of the egg weight introduced into TiO2 towards the activity of the co-doped TiO2 in the dye decolorization is displayed in Figure 9. Concerning the C,N-doped samples, an increase in the activity is observed for all samples compared with the corresponding pure TiO2 materials. Further, it is seen that the increase in the egg weight resulted in higher dye decolorization, but larger egg weight than 2 g caused opposite photo-decolorization result. Many studies have also found a similar trend [4]. The mass of the egg white should be proportional to the amount of C, N co-doped into TiO2. The photocatalyst with the increasing amount of the dopants, having lower Eg, was able to absorb visible light more effectively. This condition provided more number of radicals, which further resulted in the higher dye photo-decolorization.Figure 9
Dye photo-decolorization efficiency under visible process over TiO2-C,N prepared from the egg white with (a) 1 g, (b) 2 g, and (c) 4 g into 1 g TiO2 (Congo red dye concentration = 10 mg L−1, solution volume = 100 mL, photocatalyst mass = 50 mg, reaction time = 45 min, and pH = 7).The heaviest weight of the egg white, implying the largest dopant content, should result in the highest effective photo-decolorization, but the contrary result was observed. In this typical co-doped TiO2, the agglomerate of the organic residual covered the TiO2 surface, as demonstrated by TEM images, which limited the contact of TiO2-C,N (1 : 2) with the light, diminishing OH radical formation. In addition, the covered surface of TiO2 also inhibited the OH radical on the TiO2 surface to contact with the dye. These situations constrained the dye photo-decolorization.From Figures8 and 9, it is notable that the photo-decolorization is enhanced sharply as the length of the irradiation time up to 30 mins, then the slight increase is notified within 35 to 45 mins, but with a longer time than 45 mins, the photo-decolorization is not influenced by time. Similar data have also been reported by others [2]. The extension time could enhance the light penetration to reach the TiO2 surface, which resulted in a larger number of OH radicals, and so that a greater collision frequency occurred between the OH radicals and the dye [2]. These conditions were conducive to dye photo-decolorization. After reaching the maximum formation of the OH radicals and so the photo-decolorization, TiO2-C,N may be saturated that suffered from the formation of the OH radicals, so that the photo-decolorization insignificantly changed or almost constant [2, 10].


## 3.2.3. The Influence of the Photocatalyst Mass and Solution pH

The photo-decolorization resulting from the process with various photocatalyst mass and pH alteration is displayed in Figure10. In the figure, more effective photo-decolorization could be reached with the enlargement of the photocatalyst mass, but with the higher mass than the optimum level, the photo-decolorization was found to be detrimental. With increasing photocatalyst mass, more OH radicals were provided, hence improving the dye photo-decolorization. In contrast, a very large mass caused more turbid solution, which screened the light penetration, and so the photo-decolorization was retarded [14, 10].Figure 10
Influence of pH on the photo-decolorization, with the photocatalyst mass of (a) 10 mg, (b) 30 mg, (c) 50 mg, and (d) 100 mg in 100 mL of the dye solution (Congo red dye concentration = 10 mg L−1, solution volume = 100 mL, egg white mass = 2 g, and reaction time = 45 min).It is also observable that the photo-decolorization significantly improved when the pH was elevated and reached the maximum level at pH 7. The opposite trend appears at pH higher than 7. At low pH, the surface of TiO2 was protonated by H+ to form positively charged surface [14, 10] and Congo red also existed as cationic form [20, 21]. The same charges refused the interaction between TiO2 surface and Congo red dye molecules, which led to the photo-decolorization being very less effective. It is important to note that most OH radicals are associated with TiO2 surface and for proceeding with the photo-decolorization, and Congo red has to be adsorbed on the surface of the photocatalyst to interact with the OH radicals [12, 19]. Increasing pH can gradually reduce the protonation of both photocatalyst [12] and Congo red molecules [20] to form neutral molecules. The increase in the number of neutral molecules is beneficial to mutually interact, which promoted more effective photo-decolorization. In the solution with higher pH (basic condition), both the surface of TiO2 and the Congo red tended to be negatively charged [12, 20]. Consequently, the interaction between Congo red and the TiO2 photocatalyst was constrained, causing the photo-decolorization declined as shown in Figure 10.


## 4. Conclusions

It can be concluded that chicken egg white as a single source can be used for co-doped C,N into TiO2 that has successfully decreased the Eg and shifted the absorption into the visible region. The decrease in Eg was influenced by the amount of the chicken egg, and the highest decrease in Eg (into 2.69 eV from 3.25 eV) was demonstrated by the photocatalyst of TiO2-C,N prepared from 2 g of the chicken egg white for 1 g of TiO2. Further, the doped TiO2-C,N exhibited stronger activity in the photo-decolorization of Congo red dye under visible irradiation than the undoped photocatalyst did. The highest dye photo-decolorization in 100 mL of the solution with 10 mg/L of the concentration could be reached using TiO2-C,N (1 : 2) photocatalyst with 50 mg of the mass, for 45 min and at pH 7, which was about 98%.



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*Source: 2613841-2022-04-15.xml*