Open Access

Photocatalytic degradation of Metronidazole with illuminated TiO2 nanoparticles

  • Mahdi Farzadkia1,
  • Edris Bazrafshan2,
  • Ali Esrafili1,
  • Jae-Kyu Yang3 and
  • Mehdi Shirzad-Siboni1Email author
Journal of Environmental Health Science and Engineering201513:35

DOI: 10.1186/s40201-015-0194-y

Received: 15 September 2014

Accepted: 15 April 2015

Published: 21 April 2015


Metronidazole (MNZ) is a brand of nitroimidazole antibiotic, which is generally used in clinical applications and extensively used for the treatment of infectious diseases caused by anaerobic bacteria and protozoans. The aim of this investigation was to degrade MNZ with illuminated TiO2 nanoparticles at different catalyst dosage, contact time, pH, initial MNZ concentration and lamp intensity. Maximum removal of MNZ was observed at near neutral pH. Removal efficiency was decreased by increasing dosage and initial MNZ concentration. The reaction rate constant (k obs ) was decreased from 0.0513 to 0.0072 min−1 and the value of electrical energy per order (EEo) was increased from 93.57 to 666.67 (kWh/m3) with increasing initial MNZ concentration from 40 to 120 mg/L, respectively. The biodegradability estimated from the BOD5/COD ratio was increased from 0 to 0.098. The photocatalyst demonstrated proper photocatalytic activity even after five successive cycles. Finally, UV/TiO2 is identified as a promising technique for the removal of antibiotic with high efficiency in a relatively short reaction time.


Titanium dioxide Metronidazole Photocatalysis Kinetics


Recently, several different types of emerging contaminants in water systems are known as new environmental hazards those need to be treated with suitable methods [1]. As various pharmaceutical compounds have been used since the 1950s due to rapid population growth and development of medical science, several pharmaceutical compounds have been found in surface water, ground water and effluents from wastewater treatment plants. Metronidazole (2-methyl-5-nitroimidazole-1-ethanol) has been widely used to treat infections caused by anaerobic bacteria, bacteroides and protozoa [2-4]. Residual concentrations of metronidazole (MNZ) in surface waters and wastewater are 1 ~ 10 ng/L [5,6]. As MNZ is non-biodegradable and highly soluble in water, it can be accumulated in the aquatic environment [7,8]. Elimination of MNZ from water system is an important issue considering its toxicity, potential mutagenicity and carcinogenity [7,8]. In order to remove MNZ, many techniques such as adsorption [9,10], reduction with nanoscale zero-valent iron particles [11], biological methods [12,13], ozonation technology [14], photolysis [15], Fenton and photo-Fenton processes [16], heterogeneous photocatalysis [15,17,18] and electro-Fenton process with a Ce/SnO2–Sb coated titanium anode [1] have been applied.

Adsorption is widely used method for the treatment of wastewater containing toxic organic compounds. However, it just transfer contaminants from water to a solid phase without any degradation [9,10,19,20]. Biological method is also known as one of the suggested techniques. However this method generally requires long periods for treatment [12,21]. Oxidation is a promising process but sometimes it is regarded as a limited process due to the formation of intermediates with higher toxicity than the parent compound [5,8,22]. Therefore near complete mineralization of MNZ is the most relevant option. For this purpose, advanced oxidation process (AOP) is regarded as a promising option to treat wastewater containing MNZ due to a complete mineralization of parent material as well as lack of selectivity [7,23]. Generally AOPs involve generation of hydroxyl radicals through UV/photocatalyst, UV/H2O2 and UV/O3 processes [24-26]. Among these methods, photocatalytic reaction using TiO2/UV can treat non-biodegradable organic compounds to biodegradable species [23,24,27]. Considering characteristics of the AOP, it can be used as pre- or post-treatment process in wastewater treatment because of its installation easiness in conventional wastewater treatment facilities [23,24,27].

Therefore, in the present work, P-25 TiO2 was selected as a catalyst in the photocatalytic removal of MNZ. Effects of several operational parameters including pH, TiO2 dosage and MNZ concentration on photocatalytic degradation of MNZ were investigated. Kinetic parameters for the photocatalytic degradation were obtained by application of the Langmuir–Hinshelwood (L–H) model. Finally, electrical energy per order (EEo) was obtained to evaluate cost-efficiency of the processes used in this research.

Material and methods


Analytical grade of MNZ (C6H9N3O3; 99% chemical reagent) was purchased from Merck (Darmesdat, Germany) and its physical and chemical characteristics are summarized in Table 1. Potassium dihydrogen phosphate (KH2PO4) and acetonitrile (99.7%, HPLC grade) were purchased from Merck. P-25 TiO2 (80/20 mixture of anatase and rutile) was obtained from Degussa Corp. It has approximately spherical shape and has greater than 99.5% purity. The specific surface area of the TiO2 particles was 50 ± 15 m2/g according to Evonik-Industrial Co. The average size of the TiO2 particles was 21 nm. The antibiotic aqueous solution was prepared by dissolving 1 g of MNZ in 1 L distilled water. The antibiotic aqueous solution was prepared weekly and stored at 4°C. Initial COD and BOD5/COD ratio of 1000 mg/L MNZ was 126 mg/L and approximately 0, respectively.
Table 1

Physical and chemical properties of MNZ


Metronidazole antibiotic (MNZ)

Molecular structure

Molecular formula


Molecular weight (g/mol)


Water solubility (g/L)




Melting point (°C)


KH (mol/dm3.atm)

5.92 × 107

Vp (Pa)

4.07 × 10−7

Figure 1a and b shows X-ray diffraction (XRD) and Fourier transform infrared spectroscopy (FT-IR) image of TiO2, respectively. The main peaks at 2θ values of 25.367, 37.909, 38.667, 48.158, 54.051, 55.204, 62.817 and 68.976 were correspond to the (101), (004), (112), (200), (105), (211), (204) and (116) planes of P-25 TiO2 (JCPDS card no. 36–1451). FT-IR analysis of TiO2 was performed in the range of 400–4000 1/cm (Figure 1b). The absorption bands at 438 1/cm and 620 1/cm was attributed to the Eg and A2g mode, respectively. The pHZPC of TiO2 nanocatalyst was determined adopting the previously reported method.
Figure 1

Characteristics of titanium dioxide: (a) XRD pattern (b) FT-IR pattern.

Experimental set-up

The experimental reactor used for the photocatalytic degradation of MNZ is shown in Figure 2. The total volume of the reactor was 2 L with working volume of 1 L. The solution in the reactor was constantly stirred via a magnetic stirrer (170 rpm). A 125 W medium-pressure UVC lamp emitting maximum wavelength at 247.3 nm and a low-pressure UV lamp with irradiation intensity 8 W were applied as light sources. The light intensity of the UVC lamp was equal to 1020 μw/cm2 measured by a Spectroline model DRC-100X digital radiometer combined with a DIX-365 radiation sensor (ShokofanTosee, Company, Iran).
Figure 2

A schematic diagram of the experimental reactor.

Experimental procedure and analysis

In batch experiments, a selected dosage of TiO2 (0.5-3 g/L) was added in 1000 mL of MNZ solution with a certain concentration (40–120 mg/L) at different solution pH ranging from 3 to 11. Initial pH of the solution was adjusted by adding NaOH and HCl (0.1 mol/L) and measured by pH meter (Metron, Switzerland). All runs were performed under ambient conditions for 3 h. During the experiments, the solution in the photoreactor was constantly stirred and kept at constant temperature (25 ± 1°C). The MNZ solutions loaded with TiO2 were equilibrated in the dark for 30 min. After the equilibration period, the UV-lamp was switched on and 10 mL of the solution was taken at distinct time intervals. The aqueous samples were centrifuged (Sigma-301, Germany) at 4000 revolution per minute (rpm) for 10 min to eliminate TiO2 and then measured concentration of residual MNZ. The concentration of residual MNZ was determined by high performance liquid chromatography (HPLC, Waters, USA) equipped with a UV detector at 348 nm. A Diamonsil (R) C18 column (5 μm, 250 mm long × 4.6 mm ID) was used. The data were recorded by a chemistation software. The mobile phase was composed of a mixture of acetonitrile and distilled water (30/70, v/v). The flow speed was set at 1.0 mL/min and 20 μL injections were used [4]. COD was determined by COD reactor model AR851 (HACH, USA) and biodegradability was measured by five-day biochemical oxygen demand (BOD5) according to the Standard Methods [28]. A typical HPLC chromatogram of MNZ is shown in Figure 3.
Figure 3

A typical HPLC chromatogram of Metronidazole.

The removal efficiency (%) is calculated by Eq. (1).
$$ \mathrm{Removal}\ \mathrm{efficiency}\ \left(\%\right) = \frac{{\mathrm{C}}_0\hbox{-} \mathrm{C}}{{\mathrm{C}}_0}\times 100 $$
where C0 and C are the concentrations of MNZ at initial and at time t (mg/L), respectively.

All experiments were repeated three times and the average values with error percents were reported.

Results and discussion

Effect of TiO2 dosage

Effect of TiO2 dosage on the photocatalytic degradation of MNZ (80 mg/L) was investigated at pH 7. As shown in Figure 4, degradation efficiency of MNZ was increased from 64.28 to 97.61% by increasing irradiation time from 30 to 180 min at 0.5 g/L TiO2. A greater degradation efficiency of MZN was observed over the entire reaction time at low TiO2 dosage. This phenomena can be explained by the increased blockage of the incident UV light with increasing photocatalyst dosage [18,29]. Since the photocatalytic degradation of MNZ was not much increased over the 0.5 g/L of TiO2, further experiments were performed with 0.5 g/L TiO2. Similar results have been reported by other researchers [23,24,27].
Figure 4

The effect of catalyst dosage on the photocatalytic degradation of MNZ and COD removal (pH = 7, MNZ =80 mg/L, BOD5/COD ~ 0, COD = 126 mg/L).

Biodegradability of MNZ was evaluated in this work. To measure the biodegradability, BOD5 and COD values were measured before and after UV irradiation and the ratio of BOD5/COD was used as a biodegradability indicator. After 3 h reaction time, removal efficiency of COD was above 97.6% at all catalyst dosages and the ratio of BOD5/COD increased from 0 to 0.098 as the dosage increased from 0.5 to 3 g/L. This result indicates that MNZ can be changed to more biodegradable products.

Effect of pH

Effect of pH on the photocatalytic degradation of MNZ (80 mg/L) was investigated at constant TiO2 dosage (0.5 g/L) by varying the initial pH of solution. Figure 5 shows that the greatest degradation efficiency was obtained at neutral pH over the entire reaction time. MNZ degradation after 180 min in pH 3, 7 and 11 was 98.2, 99.48 and 97.3%, respectively. Also, COD removal after 180 min in pH 3, 7 and 11 was 97.61, 98.02 and 96.82%, respectively. This trend can be explained by the variation of charges on MNZ as well as on the surface of TiO2 at different solution pH. The pHzpc of TiO2 is determined as 6.52 and pKa value of MNZ is 2.55. Therefore, at acidic pH, both TiO2 and MNZ are positively charged, causing negative effect for the adsorption of MNZ on the surface of TiO2. At neutral pH, no repulsive forces between the TiO2 and MNZ might be developed. At basic pH, both TiO2 and MNZ have negative charges, causing negative effect for the adsorption of MNZ on the surface of TiO2. In this study, even though a distinct removal efficiency of MNZ was not observed at different solution pH, the most effective degradation of MNZ was observed at pH 7. Thus further experiments were performed at neutral pH [4,15,18].
Figure 5

The effect of initial pH on the photocatalytic degradation of MNZ and COD removal (dosage = 0.5 g/L, MNZ =80 mg/L, BOD5/COD ~ 0, COD = 126 mg/L).

Effect of initial MNZ concentration

Photocatalytic degradation of MNZ by TiO2 was studied by varying the initial MNZ concentration at pH 7 and dosage equal to 0.5 g/L. Figure 6 shows that photocatalytic degradation efficiency decreased as the initial MNZ concentration increased. The presumed reason is that more surface of the TiO2 surface may be occupied by MNZ as the initial MNZ concentration increased. In addition, more degradation intermediates can be accumulated on the TiO2 surface, causing a negative effect in the utilization of hydroxyl radicals or positive holes in the valence band of the TiO2 surface. Moreover, once the concentration of the MNZ increases, more absorption of UV light by MNZ molecules, known as inner filtration effect, can occur. This effect causes decrease of photons reaching to the TiO2 surface [4]. Similar results have been reported by other researchers [15,18,23].
Figure 6

The effect of initial MNZ concentration on the photocatalytic degradation of MNZ (dosage = 0.5 g/L, pH = 7, BOD5/COD ~ 0, COD = 126 mg/L).

Kinetic study and electrical energy determination

In order to obtain kinetic information, experimental result in Figure 6 was fitted with a pseudo-first-order equation as expressed in Eq. (2).
$$ \ln \left[{\left(\mathrm{M}\mathrm{N}\mathrm{Z}\right)}_0/{\left(\mathrm{M}\mathrm{N}\mathrm{Z}\right)}_{\mathrm{t}}\right]={\mathrm{k}}_1\mathrm{t} $$
To calculate the rate constant from the plot ln[C0/C] versus t, only initial data points were considered. Figure 7 shows the plot of ln[C0/C] versus t for the degradation of MNZ. The first-order rate constants of photocatalytic process (kobs (1/min)) at different initial concentrations of MNZ are summarized in Table 2. The relationship between the initial photocatalytic degradation rate (r) and the initial concentration of organic substrate for a heterogeneous photocatalytic process can be described by Langmuir–Hinshelwood (L-H) model (Eqs. 3 and 4) [30,31]:
Figure 7

First-order kinetic model for the photocatalytic degradation of MNZ (dosage = 0.5 g/L, pH = 7, BOD5/COD ~ 0, COD = 126 mg/L).

Table 2

Pseudo-first order kinetic parameters and E Eo values for the photocatalytic degradation of MNZ at different initial MNZ concentrations (catalyst dose = 0.5 g/L and pH =7)

E Eo (kWh/m 3 )

R 2

1/k obs (min)

k obs (1/min)

[MNZ] 0 (mg/L)
















$$ \mathrm{r}=\frac{{\mathrm{k}}_{\mathrm{c}}{\mathrm{K}}_{\mathrm{MNZ}}\ \left[\mathrm{M}\mathrm{N}\mathrm{Z}\right]}{1+{\mathrm{K}}_{\mathrm{MNZ}}{\left[\mathrm{M}\mathrm{N}\mathrm{Z}\right]}_0}={\mathrm{k}}_{\mathrm{obs}}\left[\mathrm{M}\mathrm{N}\mathrm{Z}\right] $$
$$ \frac{1}{{\mathrm{k}}_{\mathrm{obs}}}=\frac{1}{{\mathrm{k}}_{\mathrm{c}}\ {\mathrm{K}}_{\mathrm{MNZ}}}+\frac{{\left[\mathrm{M}\mathrm{N}\mathrm{Z}\right]}_0}{{\mathrm{k}}_{\mathrm{c}}} $$
where [MNZ]0 is the initial concentration of the antibiotic in mg/L, kc (mg/L/min) is the kinetic rate constant of surface reaction and KMNZ (L/mg) is the Langmuir adsorption constant. The values of KMNZ and kc were obtained as 0.0285 L/mg and 0.67 mg/L/min, respectively. This L–H kinetic model has been used by several authors to analyze heterogeneous photocatalytic reactions [30,31].
For the case of photocatalytic reaction, electrical energy is very important factor for the real application and evaluation for the electrical energy should be provided. Thus, in this work, electrical energy was evaluated by calculating electrical energy per order (EEO). It is defined as the number of kWh of electrical energy required to reduce concentration of a pollutant by 1 order of magnitude (90%) in 1 m3 of contaminated water. The EEO (kWh/m3) can be calculated from the following equation:
$$ {E}_{EO}=\frac{\mathrm{p}\times \mathrm{t}\times 1000}{\mathrm{V}\times 60\times \log \left({\mathrm{C}}_1/{\mathrm{C}}_{\mathrm{f}}\right)} $$
$$ {E}_{EO}=\frac{38.4 \times \mathrm{P}}{{\mathrm{V} \times \mathrm{k}}_{obs}} $$
where P is the rated power (kW) of the AOP system, t is the irradiation time (min), k obs is the pseudo-first order rate constant (1/min), V is the volume (L) of the wastewater in the reactor, Ci and Cf is the initial and final MNZ concentrations, respectively. The EEO value for UV-alone and UV/TiO2 processes are reported in Table 3. EEO value for UV/TiO2 process was lower than UV-alone process.
Table 3

The E Eo values for the removal of MNZ ([MNZ] 0 = 80 mg/L, catalyst dose = 0.5 g/L and pH =7)


E Eo (kWh/m 3 )

UV 8 W-alone




UV 8 W/TiO2


UV 125 W/TiO2


Comparison of different MNZ removal processes and reusability test

MNZ removal by TiO2-alone, UV 8 W-alone, UV 125 W-alone, UV 8 W/TiO2 and UV 125 W/TiO2 processes are shown in Figure 8. Removal efficiency of MNZ through adsorption process (TiO2-alone) was low. Overall removal efficiency of MNZ by TiO2-alone, UV 8 W-alone, UV 125 W-alone and UV 8 W/TiO2 process was 9.63%, 24.52, 42.32% and 53.53%, respectively. But 99.48% of MNZ was removed with UV 125 W/TiO2. These experiments demonstrate that both UV light and TiO2 are necessary for the effective degradation of MNZ.
Figure 8

The contribution of each process involved in the photocatalytic degradation of MNZ (dosage = 0.5 g/L, pH = 7, MNZ = 80 mg/L, BOD5/COD ~ 0, COD = 126 mg/L).

Based on the above experiments and analysis, mechanism of the photocatalysis could be proposed as following:

An electron excites from the valence band to the conduction band of TiO2, generating electron–hole pair, with UV light (λ < 390 nm) (Eq. 7) [24,27]:
$$ \mathrm{T}\mathrm{i}\mathrm{O}2 + \mathrm{h}\upupsilon\ \to \mathrm{T}\mathrm{i}\mathrm{O}2\left({\mathrm{e}}_{\mathrm{CB}}^{\hbox{-} }+{\mathrm{h}}_{\mathrm{VB}}^{+}\right) $$
Then, the generated electron–hole pairs can participate in the reactions with electron acceptors like O2 and donors like H2O or OH to generate highly reactive radical species particularly hydroxyl radicals (E0 = +3.06 V), which can oxidize organic contaminants and their degradation intermediates unselectively. Furthermore, positive holes can oxidize pollutants directly, too (Eqs. 811) [24,27]. Also Homem and Santos [32] reviewed degradation and removal methods of antibiotics from aqueous matrices and suggested removal mechanisms.
$$ {\mathrm{h}}_{\mathrm{VB}}^{+}+\mathrm{M}\mathrm{N}\mathrm{Z}\ \to \mathrm{intermediates}\ \mathrm{or}\ \mathrm{products} $$
$$ {\mathrm{h}}_{\mathrm{VB}}^{+}+{\mathrm{H}}_2\mathrm{O}\ \to {\mathrm{H}}^{+}+\cdotp \cdot \mathrm{O}\mathrm{H} $$
$$ {\mathrm{h}}_{\mathrm{VB}}^{+} + {\mathrm{OH}}^{-}\to \cdotp \cdotp \cdot \mathrm{O}\mathrm{H} $$
$$ \cdotp \cdot \mathrm{O}\mathrm{H}+\mathrm{M}\mathrm{N}\mathrm{Z}\to \kern0.5em \mathrm{intermediates}\kern0.5em \mathrm{or}\kern0.5em \mathrm{products} $$
The reusability of a photocatalyst is an important factor for real application. Hence, five consecutive photocatalytic experiments were performed by UV/TiO2 process. As can be seen in Figure 9, quite similar photocatalytic activity was maintained over five consecutive runs. Photocatalytic degradation of MNZ with illuminated TiO2 was compared with other reported data. Removal efficiency and reaction rate constant were compared and summarized in Table 4.
Figure 9

Reusability test of UV/TiO2 for the photocatalytic degradation of MNZ over five consecutive runs (dosage = 0.5 g/L, pH = 7, MNZ =80 mg/L, BOD5/COD ~ 0, COD = 126 mg/L).

Table 4

Comparison of photocatalytic degradation of MNZ



Catalyst dosage (g/L)

[MNZ ] 0 (mg/L)

Lamp (W)

Time (min)

Removal efficiency (%)

k obs (min −1 )










































Lp Mp

5 5

6 12

0.005616 0.02304


UV/Niobate K6Nb10.8O30

















Present study


From the application of TiO2 for the photocatalytic degradation of MNZ in aqueous solutions, a maximum removal of MNZ was observed at neutral pH. Removal efficiency was decreased by increasing TiO2 dosage and initial MNZ concentration. Electrical energy per order was increased and reaction rate constant was decreased with increasing initial MNZ concentration. Photocatalytic activity was maintained even after five consecutive runs. Finally, UV/TiO2 is identified as a promising technique for the removal of MNZ with high efficiency in a relatively short reaction time.



The authors thank the Iran and Zahedan Universities of Medical Sciences, Iran for all of the support provided. Also, authors would like to thank Mr. Bonyani for the HPLC analysis in the laboratory of nutrition department.

Authors’ Affiliations

Department of Environmental Health Engineering, School of public Health, Iran University of Medical Sciences
Health Promotion Research Center, Zahedan University of Medical Sciences
Divisions of General Education, Kwangwoon University


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