# Performance and Mechanism of UV/Immobilized Cu-TiO2 System to Degradation Histidine

Authors: Cheng Liu; Jie Wang; Wei Chen; Zhehao Sun; Zhen Cao
Journal: Journal of Nanomaterials
 (2016)

---

## Abstract

More and more attention is paid to dissolved organic nitrogen (DON) and some specific categories of amino acids are considered to be the direct precursors of nitrogenous disinfection byproducts (N-DBPs). Histidine was chosen to study the efficiency and mechanism of amino acid in UV/Cu-TiO2 system. Moreover, the influences of pH, organics, and inorganic ion on the photocatalytic efficiency were also investigated. The results show that the degradation rate of DON in the UV/Cu-TiO2 system was about 50% after 60 min, and it was much lower than that of histidine (72%), which indicated that a part of degraded histidine was oxidized to other N-containing organics. The optimal pH value was 7.0 for the photodegradation of histidine, and the presence of organic compound and inorganic ion would decrease the degradation performance to some extent. After 6 h irradiation, histidine was totally degraded into N
H
4
+, and in the following 2 h, N
H
4
+ was oxidized to N
O
3
- firstly and then N
O
3
- was reduced to N2 and overflowed from water, which should be attributed to the doping of Cu in the TiO2 and provided a way to totally degrade the DON from the water.


---

## Body

## 1. Introduction

Total dissolved nitrogen (TDN) is presented as dissolved inorganic nitrogen (DIN) (the sum ofN
O
3
-, N
O
2
-, and N
H
4
+ species) and dissolved organic nitrogen (DON) in natural waters. It is a subclass of Natural Organic Matters (NOM) in fresh water, accounting for a portion of 1–5% by weight [1, 2]. In brief, DON is the org-N structure of dissolved organic matters (DOM) [3]. Input of DON to natural waters is largely a result of autochthonous biological process, including extracellular exudate yielded by phytoplankton, N2 fixation, bacterial respiration, viral cell-lysis, and sloppy feeding by zooplankton and faecal pellet decay. Additionally, external sources of DON arise from sewage and industrial effluents, terrestrial run-off, and atmospheric deposition [4–6]. This nitrogen fraction includes not only a large spectrum of natural compounds like free and hydrolysable amino acids, chlorophyll, and amino sugars but also synthetic compounds like pesticides (e.g., atrazine) [7]. Dissolved organic nitrogen (DON) is currently drawing more and more attention in drinking water treatment for its potential to form nitrogenous disinfection byproducts (N-DBPs) [7, 8], which are far more carcinogenic or mutagenic than some of the regulated DBPs [9–11]. As to the dissolved organic matters, amino acids are mainly present as combined amino acids and constitute a small proportion (7.2 ± 4.3%) of the total DON [2]. However, some special categories of amino acids were considered as the main precursor of N-DBPs according to former studies [12–15] and some other DON matters may change to amino acids during the water treatment. Therefore, experiments conducted with typical amino acid model compound will be useful to better understand the reactivity of the amine functional group during the process of photocatalytic degradation. In this study, histidine was chosen as the target compound because of its relative higher concentration in raw water and higher potential to form N-DBPs [16, 17]. Currently, studies about DON are mainly focusing on its analytical measurement, structural composition, occurrence, and potential in N-DBPs formation [18–21]. Photocatalytic oxidation using TiO2 is widely used in water treatment due to its availability, nontoxicity, cheapness, and relatively chemical stability. Additionally, the photocatalytic oxidation process can be carried out under wide conditions and leads to complete mineralization [12]. Konstantinou and Albanis reported the wide use of heterogeneous photocatalysis with TiO2 (TiO2/UV) to effectively degrade NOM from water [13]. However, limited results on its degradation performance for the amino acids by TiO2 are available. In addition, UV only occupies a small fraction of sunlight, which means an inefficient utilization of solar light by TiO2. All of the above limit the wide application of TiO2. Cu-doped TiO2 were selected in this paper, which has been reported to be attributed to increase in visible light adsorption and lengthening of the photogenerated electron-hole pair recombination time [22, 23]. In previous researches [24, 25], Cu-TiO2 catalyst participated in the reaction in suspended state, which may cause the low recovery rate. Therefore, in this paper, Cu-TiO2 was immobilized on fiber glass net.Therefore, the main purpose of this research was to investigate the degradation performance and mechanism of typical amino acids by UV/Cu-TiO2 system; the proper load of copper ion on the TiO2 was optimized to enhance the degradation efficiency. Additionally, the effects of pH value, organic compounds, and inorganic ions on photocatalytic efficiency will also be discussed.


## 2. Methods

### 2.1. Materials

Histidine was purchased from J & K Scientific Ltd. (Beijing, China), and other reagents were obtained from Sinopharm Chemical Reagent Co. (Shanghai, China). All the chemicals used were at least of analytical grade.Blank TiO2 and Cu-doped TiO2 were prepared by referring to the reported sol-gel method [9]. TiO2 was prepared by a conventional sol-gel method using butyl titanate (TBT) (80 mL) in ethanol (320 mL) as a precursor. The hydrolysis solution of TBT solution was achieved by adding double distilled water (DDW) of 8 mL. Sol-gel synthesis in acidic solution was performed by substituting DDW of 8 mL by 2.5 mL nitric acid/water (volume ratio = 1 : 4). In addition, Cu-doped TiO2 were obtained by dissolving the corresponding amount of copper precursor, Cu(NO3)2, into the initial ethanol or acid/ethanol solution. The resulting sol was obtained after 24 hours under room temperature. Glass fiber nets selected in this study were 15 cm × 30 cm and were full of holes (15 mm × 15 mm). The holes are in favor of the attachment of Cu-TiO2 particles to glass fiber nets. Glass fiber nets were impregnated with the sol for 5 min and dried under room temperature and finally calcined at 500°C for 2 h. After repeating for 3-4 times, Cu-TiO2 photocatalysts supported on glass fiber nets were obtained, and the weight of Cu-TiO2 adhering to one piece of glass fiber net is 1.0 g. According to our previous work [10], when copper loading was 1.0%, Cu-TiO2 showed the best photocatalytic performance for DON degradation. Therefore, the photocatalyst used in the following experiments was Cu-TiO2 (1.0%).


### 2.2. Analytical Methods

In this paper, the characteristics of blank TiO2 and Cu-TiO2 were examined by X-ray diffraction (XRD), diffuse reflectance ultraviolet-visible spectroscopic (DR-UV-Vis) analysis, and X-ray photoelectron spectroscopy (XPS). DR-UV-Vis was conducted on a Lambda 950 spectrometer with the wavelength ranges of 175–3300 nm. The X-ray diffraction measurement was performed with a Bruker D8 diffractometer using Cu Kα radiation (λ = 1.542 Å) at 40 kV, 30 mA over the 2θ range 10–70°. The samples were coated with a layer of platinum-palladium prior to scanning at 100 K magnification. XPS spectra were obtained on a VG Scientific ESCA-Lab220i-XL hemispherical electron analyzer, which worked at a pressure <3 × 10−9 Torr, with a dual X-ray source working with K Br at 300 W.N
O
3
-, N
O
2
-, and N
H
4
+ were measured by Monitoring and Analysis Methods of Water and Wastewater 4th [26]. Total dissolved nitrogen (TDN) was measured using a TOC analyzer (Multi N/C 2100, Germany). DON was determined from the difference between measured TDN and sum of measured DIN species using the following: (1)
D
O
N
m
g
/
L
=
T
D
N
-
N
H
3
-
N
+
N
O
2
-
N
+
N
O
3
-
N
.Amino acids were analyzed by HPLC with 6-aminoquinolyl-N-hydroxysuccinimidyl (AQC) derivatization [27]. Briefly, the reaction between AQC and amino acids (and ammonia also) leads to the formation of fluorescent complexes separated on AccQ.Tag Waters (3.9 mm ∗ 150 mm, C18) HPLC column and detected at excitation and emission wavelengths of 240 and 395 nm, respectively. The HPLC system consisted of a Waters TM 600 gradient pump, a Merck AS-4000 autosampler, a column heater, and a 474 Waters TM fluorescence detector.The isoionic point of Cu-TiO2 was measured by the following method. The homogeneous solution was obtained by dissolving Cu-TiO2 powder into pure water and ultrasonic dispersion for 15 min. The pH value of the solutions was adjusted by 0.1 M HCl and 0.1 M NaOH, and the zeta potential of the solution under different pH value was measured by Nano-Z Zeta Potential analyzer. When the zeta potential of the solution was zero, the pH value was the isoionic point of Cu-TiO2.


### 2.3. Experiments

Standard jar-tests were used to study the photodegradation efficiency and mechanism of amino acids. A high pressure Hg lamp (30 W) supplied by Applied Photophysics was used, which showed the main emission line at 365 nm, and UV365 intensity was 1970 μw/cm2. For the UV/Cu-TiO2 oxidation experiments, raw water was obtained by dissolving certain histidine in pure water, and the concentration of histidine was 30 mg/L. One piece of glass fiber net loading Cu-TiO2 was fixed on the inner wall of beakers and immersed in 1000 mL water sample. In the meantime, a contrast test was performed with blank TiO2. The pH value of the solutions was adjusted by 0.1 M HCl and 0.1 M NaOH. The solutions were put outside simultaneously under UV irradiation for 1 h and continuously stirred during the reaction. Water samples were taken every 10 minutes, and the samples were filtered through 0.45 μm cellulose acetate membrane filters and placed in sample vials. The photocatalytic reactor was shown in Figure 1.Figure 1
Schematic of the photocatalytic reactor.All experiments were performed in three replicates. Statistical analysis was performed using SPSS 19.0 software (IBM Corporation, USA). The values are expressed as mean ± standard deviation (SD) and all data were checked for normality. Comparisons between control and treated groups were made by statistical analysis of variance. The value ofp < 0.05 represents significant difference.


## 2.1. Materials

Histidine was purchased from J & K Scientific Ltd. (Beijing, China), and other reagents were obtained from Sinopharm Chemical Reagent Co. (Shanghai, China). All the chemicals used were at least of analytical grade.Blank TiO2 and Cu-doped TiO2 were prepared by referring to the reported sol-gel method [9]. TiO2 was prepared by a conventional sol-gel method using butyl titanate (TBT) (80 mL) in ethanol (320 mL) as a precursor. The hydrolysis solution of TBT solution was achieved by adding double distilled water (DDW) of 8 mL. Sol-gel synthesis in acidic solution was performed by substituting DDW of 8 mL by 2.5 mL nitric acid/water (volume ratio = 1 : 4). In addition, Cu-doped TiO2 were obtained by dissolving the corresponding amount of copper precursor, Cu(NO3)2, into the initial ethanol or acid/ethanol solution. The resulting sol was obtained after 24 hours under room temperature. Glass fiber nets selected in this study were 15 cm × 30 cm and were full of holes (15 mm × 15 mm). The holes are in favor of the attachment of Cu-TiO2 particles to glass fiber nets. Glass fiber nets were impregnated with the sol for 5 min and dried under room temperature and finally calcined at 500°C for 2 h. After repeating for 3-4 times, Cu-TiO2 photocatalysts supported on glass fiber nets were obtained, and the weight of Cu-TiO2 adhering to one piece of glass fiber net is 1.0 g. According to our previous work [10], when copper loading was 1.0%, Cu-TiO2 showed the best photocatalytic performance for DON degradation. Therefore, the photocatalyst used in the following experiments was Cu-TiO2 (1.0%).


## 2.2. Analytical Methods

In this paper, the characteristics of blank TiO2 and Cu-TiO2 were examined by X-ray diffraction (XRD), diffuse reflectance ultraviolet-visible spectroscopic (DR-UV-Vis) analysis, and X-ray photoelectron spectroscopy (XPS). DR-UV-Vis was conducted on a Lambda 950 spectrometer with the wavelength ranges of 175–3300 nm. The X-ray diffraction measurement was performed with a Bruker D8 diffractometer using Cu Kα radiation (λ = 1.542 Å) at 40 kV, 30 mA over the 2θ range 10–70°. The samples were coated with a layer of platinum-palladium prior to scanning at 100 K magnification. XPS spectra were obtained on a VG Scientific ESCA-Lab220i-XL hemispherical electron analyzer, which worked at a pressure <3 × 10−9 Torr, with a dual X-ray source working with K Br at 300 W.N
O
3
-, N
O
2
-, and N
H
4
+ were measured by Monitoring and Analysis Methods of Water and Wastewater 4th [26]. Total dissolved nitrogen (TDN) was measured using a TOC analyzer (Multi N/C 2100, Germany). DON was determined from the difference between measured TDN and sum of measured DIN species using the following: (1)
D
O
N
m
g
/
L
=
T
D
N
-
N
H
3
-
N
+
N
O
2
-
N
+
N
O
3
-
N
.Amino acids were analyzed by HPLC with 6-aminoquinolyl-N-hydroxysuccinimidyl (AQC) derivatization [27]. Briefly, the reaction between AQC and amino acids (and ammonia also) leads to the formation of fluorescent complexes separated on AccQ.Tag Waters (3.9 mm ∗ 150 mm, C18) HPLC column and detected at excitation and emission wavelengths of 240 and 395 nm, respectively. The HPLC system consisted of a Waters TM 600 gradient pump, a Merck AS-4000 autosampler, a column heater, and a 474 Waters TM fluorescence detector.The isoionic point of Cu-TiO2 was measured by the following method. The homogeneous solution was obtained by dissolving Cu-TiO2 powder into pure water and ultrasonic dispersion for 15 min. The pH value of the solutions was adjusted by 0.1 M HCl and 0.1 M NaOH, and the zeta potential of the solution under different pH value was measured by Nano-Z Zeta Potential analyzer. When the zeta potential of the solution was zero, the pH value was the isoionic point of Cu-TiO2.


## 2.3. Experiments

Standard jar-tests were used to study the photodegradation efficiency and mechanism of amino acids. A high pressure Hg lamp (30 W) supplied by Applied Photophysics was used, which showed the main emission line at 365 nm, and UV365 intensity was 1970 μw/cm2. For the UV/Cu-TiO2 oxidation experiments, raw water was obtained by dissolving certain histidine in pure water, and the concentration of histidine was 30 mg/L. One piece of glass fiber net loading Cu-TiO2 was fixed on the inner wall of beakers and immersed in 1000 mL water sample. In the meantime, a contrast test was performed with blank TiO2. The pH value of the solutions was adjusted by 0.1 M HCl and 0.1 M NaOH. The solutions were put outside simultaneously under UV irradiation for 1 h and continuously stirred during the reaction. Water samples were taken every 10 minutes, and the samples were filtered through 0.45 μm cellulose acetate membrane filters and placed in sample vials. The photocatalytic reactor was shown in Figure 1.Figure 1
Schematic of the photocatalytic reactor.All experiments were performed in three replicates. Statistical analysis was performed using SPSS 19.0 software (IBM Corporation, USA). The values are expressed as mean ± standard deviation (SD) and all data were checked for normality. Comparisons between control and treated groups were made by statistical analysis of variance. The value ofp < 0.05 represents significant difference.


## 3. Results and Discussion

### 3.1. Characterization of Cu-Doped TiO2

#### 3.1.1. XRD Analysis

Figure2 shows the XRD patterns of blank and Cu-doped TiO2 photocatalysts. Peaks at 25°, 38°, 48°, and 54° were corresponding to TiO2 anatase phase, which was the most reactive form of TiO2 [28]. Characteristic peaks indicated that the doped copper ions were not detected. This phenomenon may be due to the fact that ionic radius of Cu2+ is 0.72 Å, which is close to the ionic radius of Ti4+ (0.68 Å). Therefore, Cu2+ was incorporated in the crystalline of TiO2 and replaced Ti4+ to form the lattice imperfection [29].Figure 2
XRD diffractograms for blank TiO2 and Cu-TiO2 photocatalysts.


#### 3.1.2. DR-UV-Vis Analysis

The DR-UV-Vis spectra of Cu-doped TiO2 and blank TiO2 are shown in Figure 3. The spectra of TiO2 show an absorption peak at 350 nm in the UV region. When doped with 1.0% copper onto TiO2, considerable shift of the peak towards the visible range at around 400–800 nm occurred (red shift). It has been reported that the band at 210–270 nm would indicate the O2-(2p)→Cu2+(3d) ligand to metal charge transfer transition, where the copper ions occupy isolated sites over the support. A band at 350 nm would indicate the formation of (Cu-O-Cu)2+ clusters in a highly dispersed state. The broad band between 400 nm and 600 nm is attributed to the presence of Cu1+ clusters in partially reduced CuO matrix as well as (Cu-O-Cu)2+ clusters. The absorption band at 600–800 nm indicates the crystalline and bulk CuO in octahedral symmetry [25]. The incorporation of copper ion caused a red shift and increased the absorption band to the visible or even near-infrared range and this promoted the photocatalytic activity. The optimal doping of copper ion is 1.0%.Figure 3
Diffuse reflectance spectra for blank TiO2 and Cu-doped TiO2 (1.0%).


#### 3.1.3. XPS Analysis

Figure4 shows the XPS spectra corresponding to elements on the surface of thin film. There are five kinds of elements (Ti, O, C, Si, and Cu) on the surface of thin film. The presence of Si was due to the fact that the ingredient of the film is SiO2. The binding energy of T
i
2
p
3
/
2 peak at around 457 eV and T
i
2
p
1
/
2 peak at around 464 eV indicated that Ti was tetravalent. The binding energy of Cu 2p3/2 peak at around 933 eV together with the characteristic shake-up feature at a binding energy of 942 eV is indicative of Cu2+ species, while slightly lower binding energy (932 eV) and the absence of shake-up are characteristic of Cu1+ [27, 28]. Our results point out that the copper species are mainly present as Cu1+ and Cu2+.Figure 4
XPS spectra of Cu-TiO2 photocatalysts (1%).
(a)
(b)
(c)


### 3.2. Photocatalytic Activity

#### 3.2.1. Degradation Effects of DON and Histidine

As seen from Figure5(a), both doped and undoped systems could degrade histidine effectively, while the degradation through the Cu-TiO2 adsorption or photodegradation by UV separately was negligible. Moreover, according to the reported research by Castaño et al. [30], lixiviation was neglectful compared to the removal effect of histidine. Thus, the reaction product between UV and TiO2 may be responsible for the degradation performance. It is well known that TiO2 under the ultraviolet radiation could produce electron-hole pairs on its surface; then the electron-hole pairs react with the water, including org-N rich matters. However, Cu-TiO2 achieved better performance than blank TiO2, and it may be due to the fact that the recombination of excited electrons and holes in undoped system was relatively high, but in doped system the recombination of photogenerated carriers was suppressed effectively [10, 31]. Besides, the incorporation of copper ion caused a red shift and increased the absorption band to the visible or even near-infrared range and this promoted the photocatalytic activity (Figure 3). Figure 5(b) shows similar results for the degradation of DON. As seen from Figures 5(a) and 5(b), in the same reaction condition, the degradation rate of DON was significantly lower than that of histidine (50% versus 72%). This could be explained by the fact that amino acids can not be mineralized completely and be transformed to other org-N matters, which also can be detected by DON. Seen from the degradation rate of DON, only a small part of DON was directly oxidized to inorganic ion.Figure 5
Degradation of DON and amino acids by doped and undoped system (Cu-TiO2: 1%; pH = 7.0; UV365 intensity: 1970 μw/cm2).
(a)
(b)


### 3.3. Influence of Water Parameters on the Photocatalysis

#### 3.3.1. Effect of pH

In raw water, pH value changes with the climate and the growth of plankton (especially algae and aquatic plants), while pH value affects not only the electriferous state of the surface of TiO2, but also the ionization degree of target compound in reaction system. Therefore, it is necessary to figure out the influence of pH value on the photocatalytic efficiency and the corresponding experimental results were shown in Figure 8.It can be seen from Figure6 that DON degradation rate increased first and then decreased with the increase of pH value. The degradation rate of DON was up to 50% when pH value is 7. In this study, the point of zero charge of TiO2 is 6.5, and the isoionic point of histidine is 7.59 [32]. We may discover that both the catalysts and histidine are negatively charged when pH value of solution is higher than 7.59. On the contrary, both catalysts are positively charged when pH value of solution is lower than 6.5. When pH value is in the range of 6.5 and 7.59, the catalysts are negatively charged and histidine is positively charged, which enhances the chance of the collision between TiO2 and histidine.Figure 6
Effect of pH value on the photocatalytic system (Cu-TiO2: 1%; UV365 intensity: 1970 μw/cm2).


#### 3.3.2. Effect of Organic Compound and Inorganic Ions

There are large quantity of natural organic materials (NOM) and inorganic ion in raw water, and their presence will affect the degradation efficiency of target compound. So it is essential to investigate the effect of organics and inorganic ion on the photocatalytic system. Due to the measurement method of DON, the organic compound chosen as the representative should not contain N element, so isopropanol was selected. Cl− was chosen as the typical inorganic ion. The results are shown in Figure 9.It can be seen from Figure7 that the degradation efficiency of DON decreased with the increases of isopropanol and Cl− concentration. It may be due to the fact that organics and Cl− consume OH-radicals in the water [33]. Besides, there is competitive adsorption between Cl− and target compound.Figure 7
(a) Effect of isopropanol on the degradation efficiency (Cu-TiO2: 1%; pH = 7.0; UV365 intensity: 1970 μw/cm2). (b) Effect of Cl− on the degradation efficiency (Cu-TiO2: 1%; pH = 7.0; UV365 intensity: 1970 μw/cm2).
(a)
(b)Figure 8
Changes of TN,N
O
3
-, and N
H
4
+ in the DON degradation in the UV/Cu-TiO2 system (Cu-TiO2: 1%; pH = 7.0; UV365 intensity: 1970 μw/cm2).Figure 9
Variation of the main categories of nitrogen in the pure histidine in the UV/Cu-TiO2 system (Cu-TiO2: 1%; pH = 7.0; UV365 intensity: 1970 μw/cm2).


### 3.4. Proposed Mechanism

To confirm the oxidation extent of DON in water, the concentrations of total dissolved nitrogen (TDN), ammonium nitrogen (N
H
4
+), nitrate nitrogen (N
O
3
-), and nitrite nitrogen (N
O
2
-) were determined in the different reaction time. The results are shown in Figure 10.Figure 10
The photocatalytic degradation mechanism of DON.Seen from Figure8, the main categories of nitrogen showed different variation tendency. The concentrations of TDN, N
O
3
-, and DON decreased, while the concentration of N
H
4
+ kept increasing. No N
O
2
- was detected during the whole oxidation process. The decrease of TDN means the production and overflow of N2 during the oxidation process, which may be caused by the photocatalyzed reduction of N
O
3
-. For the lowered concentration values of the TDN and N
O
3
- were nearly the same. In addition, the increase of N
H
4
+ may be due to the oxidation of DON. However, the transformation mechanism for the pure histidine by the photocatalyzed oxidation was not clear for the presence of nitrate in the histidine used in the experiment. Granular activated carbon (GAC) adsorption method was used to degrade the nitrate in the water sample before the oxidation process until nitrate was not detected. After absorption, the DON concentration was still about 1.45 mg/L after the adsorption for its poor degradation by the GAC’s adsorption approach. Besides, reaction time was extended to about 8 h until DON was totally degraded into inorganic nitrogen and the transformation occurred between the inorganic nitrogen ions; the results are shown in Figure 9.Seen from Figure9, the histidine was totally degraded into N
H
4
+ and the concentration of TDN kept consistent in the first 6 h reaction time, which indicated that the main reaction in this phase was to oxidize the histidine into N
H
4
+. In the following 2 h, concentration of N
H
4
+ decreased, while the concentration of N
O
3
- increased. In addition, the concentration of TDN decreased. The above results demonstrated that N
H
4
+ was oxidized to N
O
3
- firstly and then N
O
3
- was reduced to N2 and overflowed from water. Compared with results shown in Figure 9, we may conclude that the reaction between the categories of nitrogen in the water may have some sequence in the oxidation process of histidine. The oxidation of histidine had the priority to other reactions; then the further oxidation of N
H
4
+ to N
O
3
- and the following reduction of N
O
3
- to N2 happened. What needs to be noted in the reaction process was the formation of N2 and the decrease of TDN’s concentration, which was not found in the oxidation of UV/immobilized TiO2 system [6]. The reason may lie in the doping of copper ion. According to former studies, the doping of copper ion could not only improve the oxidation ability to certain compounds in water [34] but also enhance the reduction efficiency of nitrate to N2 and the degradation performance of TN through the way of photocatalyzed reaction [35]. The formation of N2 may lead to the total degradation of nitrogen from water and had special important significance for the water sources which had been in serious eutrophication. The enhanced conversion rate from the nitrate to N2 may be explained as follows: the bandgap energies of the Cu-TiO2 and blank TiO2 were calculated based on DR-UV-Vis spectra (Figure 3) analysis according to our former study [9], and bandgap energy of blank TiO2 was 3.15 eV, while Cu-TiO2 was 2.95 eV. We may find that the copper doping causes the decrease of bandgap energy because of the dispersion of metal and metal nanoparticles diffusion in the TiO2 matrix. Electron can be easily excited from the defect state to the conduction band of TiO2 by photon. Based on the results above and reported mechanism [36–38], a possible photocatalytic oxidation approach was proposed in Figure 10.


## 3.1. Characterization of Cu-Doped TiO2

### 3.1.1. XRD Analysis

Figure2 shows the XRD patterns of blank and Cu-doped TiO2 photocatalysts. Peaks at 25°, 38°, 48°, and 54° were corresponding to TiO2 anatase phase, which was the most reactive form of TiO2 [28]. Characteristic peaks indicated that the doped copper ions were not detected. This phenomenon may be due to the fact that ionic radius of Cu2+ is 0.72 Å, which is close to the ionic radius of Ti4+ (0.68 Å). Therefore, Cu2+ was incorporated in the crystalline of TiO2 and replaced Ti4+ to form the lattice imperfection [29].Figure 2
XRD diffractograms for blank TiO2 and Cu-TiO2 photocatalysts.


### 3.1.2. DR-UV-Vis Analysis

The DR-UV-Vis spectra of Cu-doped TiO2 and blank TiO2 are shown in Figure 3. The spectra of TiO2 show an absorption peak at 350 nm in the UV region. When doped with 1.0% copper onto TiO2, considerable shift of the peak towards the visible range at around 400–800 nm occurred (red shift). It has been reported that the band at 210–270 nm would indicate the O2-(2p)→Cu2+(3d) ligand to metal charge transfer transition, where the copper ions occupy isolated sites over the support. A band at 350 nm would indicate the formation of (Cu-O-Cu)2+ clusters in a highly dispersed state. The broad band between 400 nm and 600 nm is attributed to the presence of Cu1+ clusters in partially reduced CuO matrix as well as (Cu-O-Cu)2+ clusters. The absorption band at 600–800 nm indicates the crystalline and bulk CuO in octahedral symmetry [25]. The incorporation of copper ion caused a red shift and increased the absorption band to the visible or even near-infrared range and this promoted the photocatalytic activity. The optimal doping of copper ion is 1.0%.Figure 3
Diffuse reflectance spectra for blank TiO2 and Cu-doped TiO2 (1.0%).


### 3.1.3. XPS Analysis

Figure4 shows the XPS spectra corresponding to elements on the surface of thin film. There are five kinds of elements (Ti, O, C, Si, and Cu) on the surface of thin film. The presence of Si was due to the fact that the ingredient of the film is SiO2. The binding energy of T
i
2
p
3
/
2 peak at around 457 eV and T
i
2
p
1
/
2 peak at around 464 eV indicated that Ti was tetravalent. The binding energy of Cu 2p3/2 peak at around 933 eV together with the characteristic shake-up feature at a binding energy of 942 eV is indicative of Cu2+ species, while slightly lower binding energy (932 eV) and the absence of shake-up are characteristic of Cu1+ [27, 28]. Our results point out that the copper species are mainly present as Cu1+ and Cu2+.Figure 4
XPS spectra of Cu-TiO2 photocatalysts (1%).
(a)
(b)
(c)


## 3.1.1. XRD Analysis

Figure2 shows the XRD patterns of blank and Cu-doped TiO2 photocatalysts. Peaks at 25°, 38°, 48°, and 54° were corresponding to TiO2 anatase phase, which was the most reactive form of TiO2 [28]. Characteristic peaks indicated that the doped copper ions were not detected. This phenomenon may be due to the fact that ionic radius of Cu2+ is 0.72 Å, which is close to the ionic radius of Ti4+ (0.68 Å). Therefore, Cu2+ was incorporated in the crystalline of TiO2 and replaced Ti4+ to form the lattice imperfection [29].Figure 2
XRD diffractograms for blank TiO2 and Cu-TiO2 photocatalysts.


## 3.1.2. DR-UV-Vis Analysis

The DR-UV-Vis spectra of Cu-doped TiO2 and blank TiO2 are shown in Figure 3. The spectra of TiO2 show an absorption peak at 350 nm in the UV region. When doped with 1.0% copper onto TiO2, considerable shift of the peak towards the visible range at around 400–800 nm occurred (red shift). It has been reported that the band at 210–270 nm would indicate the O2-(2p)→Cu2+(3d) ligand to metal charge transfer transition, where the copper ions occupy isolated sites over the support. A band at 350 nm would indicate the formation of (Cu-O-Cu)2+ clusters in a highly dispersed state. The broad band between 400 nm and 600 nm is attributed to the presence of Cu1+ clusters in partially reduced CuO matrix as well as (Cu-O-Cu)2+ clusters. The absorption band at 600–800 nm indicates the crystalline and bulk CuO in octahedral symmetry [25]. The incorporation of copper ion caused a red shift and increased the absorption band to the visible or even near-infrared range and this promoted the photocatalytic activity. The optimal doping of copper ion is 1.0%.Figure 3
Diffuse reflectance spectra for blank TiO2 and Cu-doped TiO2 (1.0%).


## 3.1.3. XPS Analysis

Figure4 shows the XPS spectra corresponding to elements on the surface of thin film. There are five kinds of elements (Ti, O, C, Si, and Cu) on the surface of thin film. The presence of Si was due to the fact that the ingredient of the film is SiO2. The binding energy of T
i
2
p
3
/
2 peak at around 457 eV and T
i
2
p
1
/
2 peak at around 464 eV indicated that Ti was tetravalent. The binding energy of Cu 2p3/2 peak at around 933 eV together with the characteristic shake-up feature at a binding energy of 942 eV is indicative of Cu2+ species, while slightly lower binding energy (932 eV) and the absence of shake-up are characteristic of Cu1+ [27, 28]. Our results point out that the copper species are mainly present as Cu1+ and Cu2+.Figure 4
XPS spectra of Cu-TiO2 photocatalysts (1%).
(a)
(b)
(c)


## 3.2. Photocatalytic Activity

### 3.2.1. Degradation Effects of DON and Histidine

As seen from Figure5(a), both doped and undoped systems could degrade histidine effectively, while the degradation through the Cu-TiO2 adsorption or photodegradation by UV separately was negligible. Moreover, according to the reported research by Castaño et al. [30], lixiviation was neglectful compared to the removal effect of histidine. Thus, the reaction product between UV and TiO2 may be responsible for the degradation performance. It is well known that TiO2 under the ultraviolet radiation could produce electron-hole pairs on its surface; then the electron-hole pairs react with the water, including org-N rich matters. However, Cu-TiO2 achieved better performance than blank TiO2, and it may be due to the fact that the recombination of excited electrons and holes in undoped system was relatively high, but in doped system the recombination of photogenerated carriers was suppressed effectively [10, 31]. Besides, the incorporation of copper ion caused a red shift and increased the absorption band to the visible or even near-infrared range and this promoted the photocatalytic activity (Figure 3). Figure 5(b) shows similar results for the degradation of DON. As seen from Figures 5(a) and 5(b), in the same reaction condition, the degradation rate of DON was significantly lower than that of histidine (50% versus 72%). This could be explained by the fact that amino acids can not be mineralized completely and be transformed to other org-N matters, which also can be detected by DON. Seen from the degradation rate of DON, only a small part of DON was directly oxidized to inorganic ion.Figure 5
Degradation of DON and amino acids by doped and undoped system (Cu-TiO2: 1%; pH = 7.0; UV365 intensity: 1970 μw/cm2).
(a)
(b)


## 3.2.1. Degradation Effects of DON and Histidine

As seen from Figure5(a), both doped and undoped systems could degrade histidine effectively, while the degradation through the Cu-TiO2 adsorption or photodegradation by UV separately was negligible. Moreover, according to the reported research by Castaño et al. [30], lixiviation was neglectful compared to the removal effect of histidine. Thus, the reaction product between UV and TiO2 may be responsible for the degradation performance. It is well known that TiO2 under the ultraviolet radiation could produce electron-hole pairs on its surface; then the electron-hole pairs react with the water, including org-N rich matters. However, Cu-TiO2 achieved better performance than blank TiO2, and it may be due to the fact that the recombination of excited electrons and holes in undoped system was relatively high, but in doped system the recombination of photogenerated carriers was suppressed effectively [10, 31]. Besides, the incorporation of copper ion caused a red shift and increased the absorption band to the visible or even near-infrared range and this promoted the photocatalytic activity (Figure 3). Figure 5(b) shows similar results for the degradation of DON. As seen from Figures 5(a) and 5(b), in the same reaction condition, the degradation rate of DON was significantly lower than that of histidine (50% versus 72%). This could be explained by the fact that amino acids can not be mineralized completely and be transformed to other org-N matters, which also can be detected by DON. Seen from the degradation rate of DON, only a small part of DON was directly oxidized to inorganic ion.Figure 5
Degradation of DON and amino acids by doped and undoped system (Cu-TiO2: 1%; pH = 7.0; UV365 intensity: 1970 μw/cm2).
(a)
(b)


## 3.3. Influence of Water Parameters on the Photocatalysis

### 3.3.1. Effect of pH

In raw water, pH value changes with the climate and the growth of plankton (especially algae and aquatic plants), while pH value affects not only the electriferous state of the surface of TiO2, but also the ionization degree of target compound in reaction system. Therefore, it is necessary to figure out the influence of pH value on the photocatalytic efficiency and the corresponding experimental results were shown in Figure 8.It can be seen from Figure6 that DON degradation rate increased first and then decreased with the increase of pH value. The degradation rate of DON was up to 50% when pH value is 7. In this study, the point of zero charge of TiO2 is 6.5, and the isoionic point of histidine is 7.59 [32]. We may discover that both the catalysts and histidine are negatively charged when pH value of solution is higher than 7.59. On the contrary, both catalysts are positively charged when pH value of solution is lower than 6.5. When pH value is in the range of 6.5 and 7.59, the catalysts are negatively charged and histidine is positively charged, which enhances the chance of the collision between TiO2 and histidine.Figure 6
Effect of pH value on the photocatalytic system (Cu-TiO2: 1%; UV365 intensity: 1970 μw/cm2).


### 3.3.2. Effect of Organic Compound and Inorganic Ions

There are large quantity of natural organic materials (NOM) and inorganic ion in raw water, and their presence will affect the degradation efficiency of target compound. So it is essential to investigate the effect of organics and inorganic ion on the photocatalytic system. Due to the measurement method of DON, the organic compound chosen as the representative should not contain N element, so isopropanol was selected. Cl− was chosen as the typical inorganic ion. The results are shown in Figure 9.It can be seen from Figure7 that the degradation efficiency of DON decreased with the increases of isopropanol and Cl− concentration. It may be due to the fact that organics and Cl− consume OH-radicals in the water [33]. Besides, there is competitive adsorption between Cl− and target compound.Figure 7
(a) Effect of isopropanol on the degradation efficiency (Cu-TiO2: 1%; pH = 7.0; UV365 intensity: 1970 μw/cm2). (b) Effect of Cl− on the degradation efficiency (Cu-TiO2: 1%; pH = 7.0; UV365 intensity: 1970 μw/cm2).
(a)
(b)Figure 8
Changes of TN,N
O
3
-, and N
H
4
+ in the DON degradation in the UV/Cu-TiO2 system (Cu-TiO2: 1%; pH = 7.0; UV365 intensity: 1970 μw/cm2).Figure 9
Variation of the main categories of nitrogen in the pure histidine in the UV/Cu-TiO2 system (Cu-TiO2: 1%; pH = 7.0; UV365 intensity: 1970 μw/cm2).


## 3.3.1. Effect of pH

In raw water, pH value changes with the climate and the growth of plankton (especially algae and aquatic plants), while pH value affects not only the electriferous state of the surface of TiO2, but also the ionization degree of target compound in reaction system. Therefore, it is necessary to figure out the influence of pH value on the photocatalytic efficiency and the corresponding experimental results were shown in Figure 8.It can be seen from Figure6 that DON degradation rate increased first and then decreased with the increase of pH value. The degradation rate of DON was up to 50% when pH value is 7. In this study, the point of zero charge of TiO2 is 6.5, and the isoionic point of histidine is 7.59 [32]. We may discover that both the catalysts and histidine are negatively charged when pH value of solution is higher than 7.59. On the contrary, both catalysts are positively charged when pH value of solution is lower than 6.5. When pH value is in the range of 6.5 and 7.59, the catalysts are negatively charged and histidine is positively charged, which enhances the chance of the collision between TiO2 and histidine.Figure 6
Effect of pH value on the photocatalytic system (Cu-TiO2: 1%; UV365 intensity: 1970 μw/cm2).


## 3.3.2. Effect of Organic Compound and Inorganic Ions

There are large quantity of natural organic materials (NOM) and inorganic ion in raw water, and their presence will affect the degradation efficiency of target compound. So it is essential to investigate the effect of organics and inorganic ion on the photocatalytic system. Due to the measurement method of DON, the organic compound chosen as the representative should not contain N element, so isopropanol was selected. Cl− was chosen as the typical inorganic ion. The results are shown in Figure 9.It can be seen from Figure7 that the degradation efficiency of DON decreased with the increases of isopropanol and Cl− concentration. It may be due to the fact that organics and Cl− consume OH-radicals in the water [33]. Besides, there is competitive adsorption between Cl− and target compound.Figure 7
(a) Effect of isopropanol on the degradation efficiency (Cu-TiO2: 1%; pH = 7.0; UV365 intensity: 1970 μw/cm2). (b) Effect of Cl− on the degradation efficiency (Cu-TiO2: 1%; pH = 7.0; UV365 intensity: 1970 μw/cm2).
(a)
(b)Figure 8
Changes of TN,N
O
3
-, and N
H
4
+ in the DON degradation in the UV/Cu-TiO2 system (Cu-TiO2: 1%; pH = 7.0; UV365 intensity: 1970 μw/cm2).Figure 9
Variation of the main categories of nitrogen in the pure histidine in the UV/Cu-TiO2 system (Cu-TiO2: 1%; pH = 7.0; UV365 intensity: 1970 μw/cm2).


## 3.4. Proposed Mechanism

To confirm the oxidation extent of DON in water, the concentrations of total dissolved nitrogen (TDN), ammonium nitrogen (N
H
4
+), nitrate nitrogen (N
O
3
-), and nitrite nitrogen (N
O
2
-) were determined in the different reaction time. The results are shown in Figure 10.Figure 10
The photocatalytic degradation mechanism of DON.Seen from Figure8, the main categories of nitrogen showed different variation tendency. The concentrations of TDN, N
O
3
-, and DON decreased, while the concentration of N
H
4
+ kept increasing. No N
O
2
- was detected during the whole oxidation process. The decrease of TDN means the production and overflow of N2 during the oxidation process, which may be caused by the photocatalyzed reduction of N
O
3
-. For the lowered concentration values of the TDN and N
O
3
- were nearly the same. In addition, the increase of N
H
4
+ may be due to the oxidation of DON. However, the transformation mechanism for the pure histidine by the photocatalyzed oxidation was not clear for the presence of nitrate in the histidine used in the experiment. Granular activated carbon (GAC) adsorption method was used to degrade the nitrate in the water sample before the oxidation process until nitrate was not detected. After absorption, the DON concentration was still about 1.45 mg/L after the adsorption for its poor degradation by the GAC’s adsorption approach. Besides, reaction time was extended to about 8 h until DON was totally degraded into inorganic nitrogen and the transformation occurred between the inorganic nitrogen ions; the results are shown in Figure 9.Seen from Figure9, the histidine was totally degraded into N
H
4
+ and the concentration of TDN kept consistent in the first 6 h reaction time, which indicated that the main reaction in this phase was to oxidize the histidine into N
H
4
+. In the following 2 h, concentration of N
H
4
+ decreased, while the concentration of N
O
3
- increased. In addition, the concentration of TDN decreased. The above results demonstrated that N
H
4
+ was oxidized to N
O
3
- firstly and then N
O
3
- was reduced to N2 and overflowed from water. Compared with results shown in Figure 9, we may conclude that the reaction between the categories of nitrogen in the water may have some sequence in the oxidation process of histidine. The oxidation of histidine had the priority to other reactions; then the further oxidation of N
H
4
+ to N
O
3
- and the following reduction of N
O
3
- to N2 happened. What needs to be noted in the reaction process was the formation of N2 and the decrease of TDN’s concentration, which was not found in the oxidation of UV/immobilized TiO2 system [6]. The reason may lie in the doping of copper ion. According to former studies, the doping of copper ion could not only improve the oxidation ability to certain compounds in water [34] but also enhance the reduction efficiency of nitrate to N2 and the degradation performance of TN through the way of photocatalyzed reaction [35]. The formation of N2 may lead to the total degradation of nitrogen from water and had special important significance for the water sources which had been in serious eutrophication. The enhanced conversion rate from the nitrate to N2 may be explained as follows: the bandgap energies of the Cu-TiO2 and blank TiO2 were calculated based on DR-UV-Vis spectra (Figure 3) analysis according to our former study [9], and bandgap energy of blank TiO2 was 3.15 eV, while Cu-TiO2 was 2.95 eV. We may find that the copper doping causes the decrease of bandgap energy because of the dispersion of metal and metal nanoparticles diffusion in the TiO2 matrix. Electron can be easily excited from the defect state to the conduction band of TiO2 by photon. Based on the results above and reported mechanism [36–38], a possible photocatalytic oxidation approach was proposed in Figure 10.


## 4. Conclusions

Surface properties and photocatalytic activity of blank and Cu-doped TiO2 were investigated. The XRD patterns show that Cu-TiO2 is in anatase phase, which is the most reactive form of TiO2. SEM images imply that the size of Cu-TiO2 particles is small and homogeneous. DR-UV-Vis analysis shows that the incorporation of copper ion caused a red shift and increased the absorption band to the visible or even near-infrared range and this promoted the photocatalytic activity.UV/Cu-TiO2 system has a good performance in degrading histidine, and the concentration of DON and histidine was examined. The results show that the degradation rate of histidine is 72% after 60 min, which is much higher than that of DON (50%). Besides, histidine is totally degraded into N
H
4
+ in the first 6 h; in the following 2 h, N
H
4
+ was oxidized to N
O
3
- firstly and then N
O
3
- was reduced to N2 and overflowed from water. Thus, the photocatalytic system (UV/Cu-TiO2) has a tremendous potential in solving the environmental problem caused by DON. The optimal pH value is 7.0, and the presence of isopropanol and Cl− decreases the degradation efficiency.



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*Source: 8946019-2016-07-25.xml*