# Adsorption and Photocatalytic Decomposition of theβ-Blocker Metoprolol in Aqueous Titanium Dioxide Suspensions: Kinetics, Intermediates, and Degradation Pathways

Authors: Violette Romero; Pilar Marco; Jaime Giménez; Santiago Esplugas
Journal: International Journal of Photoenergy
 (2013)

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## Abstract

This study reports the photocatalytic degradation of theβ-blocker metoprolol (MET) using TiO2 suspended as catalyst. A series of photoexperiments were carried out by a UV lamp, emitting in the 250–400 nm range, providing information about the absorption of radiation in the photoreactor wall. The influence of the radiation wavelength on the MET photooxidation rate was investigated using a filter cutting out wavelengths shorter than 280 nm. Effects of photolysis and adsorption at different initial pH were studied to evaluate noncatalytic degradation for this pharmaceutical. MET adsorption onto titania was fitted to two-parameter Langmuir isotherm. From adsorption results it appears that the photocatalytic degradation can  occur mainly on the surface of TiO2. MET removed by photocatalysis was 100% conditions within 300 min, while only 26% was achieved by photolysis at the same time. TiO2 photocatalysis degradation of MET in the first stage of the reaction followed approximately a pseudo-first-order model. The major reaction intermediates were identified by LC/MS analysis such as 3-(propan-2-ylamino)propane-1,2-diol or 3-aminoprop-1-en-2-ol. Based on the identified intermediates, a photocatalytic degradation pathway was proposed, including the cleavage of side chain and the hydroxylation addition to the parent compounds.


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## Body

## 1. Introduction

The presence of pharmaceutical drugs and endocrine disruptors in surface, ground, and drinking waters is a growing environmental concern [1–9]. This pollution is caused by emission from production sites, direct disposal of surplus drugs in households, excretion after drug administration to humans and animals, wastewater from fish and other animal farms, and industry [3, 10, 11].  Some of these drugs, as β-blockers, have been detected in the order of ng L−1 to μg L−1 in the water [3–9, 12]. As an example, metoprolol tartrate salt (MET), which is usually prescribed as antihypertensive or antiarrhythmic, has been quantified up to 2 μg L−1 in sewage treatment plant (STP) effluents and to 240 ng L−1 in rivers [13]. Metoprolol and atenolol together account for more than 80% of total β-blockers consumption in Europe [6]. During the last years, metoprolol usage increased by a factor of 4, probably due to a change in human behavior [6]. Although full ecotoxicity data are not available [13, 14], it has been shown that they can adversely affect aquatic organisms, even at low concentration [2].  Due to its widespread occurrence and potential impact, MET must be removed from treated water before discharge or reuse.Several treatments for the removal of these compounds have been reported in the literature, including membrane filtration [15], activated carbon adsorption [16], and reverse osmosis [17, 18]. However, the conventional water treatment processes are relatively inefficient in treating these compounds [4, 19]. These pharmaceuticals can undergo abiotic degradation (hydrolysis, photolysis) [13] and most of them are photoactive because their structural compositions consist of aromatic rings, heteroatoms, and other functional groups that can absorb solar radiation [20].  Thus, sunlight induced photochemical treatments should be considered as an alternative to traditional treatment. Several researches have demonstrated that MET shows slow direct phototransformation and/or hydrolysis [13, 21, 22]. In this context, advanced oxidation processes (AOPs) appear as a good alternative for its degradation due to their versatility and ability to increase biodegradability [23, 24]. Among the different advanced oxidation processes, heterogenous photocatalysis has been a potential alternative for the degradation of hazardous pollutants. Oxidation of organic compounds by means of TiO2 was achieved by hydroxyl radical generation through the e-/h+ pair generated when the semiconductor is exposed to UV radiation [11, 14].The main objective of this investigation is to undertake a study on the heterogeneous photocatalytic degradation and mineralization of MET in aqueous suspensions with TiO2. In addition, the contribution of the degradation of MET by direct photolysis and the adsorption of the metoprolol onto TiO2 were studied. In this way, the effect of different initial pH values on the photodegradation rate and the adsorption isotherms of metoprolol in TiO2 suspensions were determined. The contribution of direct photolysis in photocatalysis was also examined in detail by using different wavelengths and glass type photoreactors. Additionally, an attempt has been completed to estimate the kinetic parameters and to identify the main intermediates formed during the photocatalytic degradation of MET.


## 2. Materials and Methods

### 2.1. Chemicals and Reagents

Metoprolol tartrate (MET) salt was purchased from Sigma Aldrich Chemical Co. (Spain) and used as received (1-[4-(2 methoxyethyl)phenoxy]-3-(propan-2-ylamino)propan-2-ol tartrate (2:1), CAS no 56392-17-7, (C15H25NO3)2 C4H6O6, MW 684.81). Solutions of 50 mg L−1 of MET were prepared using deionized water to assure accurate measurements of concentrations, to follow the TOC, to secure identification of intermediates, and to make predictions about possible mechanisms of photocatalysis. For pH adjustment, 0.1 mol L−1 sulphuric acid or 0.1 mol L−1 sodium hydroxide was used. All chemicals were HPLC grade, and they were used without further purification. Titanium dioxide (TiO2) Degussa P-25 (commercial catalyst ~70% anatase, ~30% rutile, surface area 50 ± 5.0 m2 g−1, and 300 μm particle size [25]) was used as received. This TiO2 is a photochemical stable material [6, 26, 27].


### 2.2. Analytical Instruments

The target compounds concentrations were monitored by a high-performance liquid chromatograph (HPLC) from Waters using aSEA18 5 μm 15 × 0.46 Teknokroma column and Waters 996 photodiode array detector using Empower Pro software 2002 Water Co. The mobile phase was composed by water and acetonitrile (20 : 80), injected with a flow-rate of 0.85 mL min−1, and detected at maximum metoprolol (221.9 nm). Total organic carbon (TOC) was measured in a Shimadzu TOC-V CNS. pH was measured by a Crison GLP 22 instrument. UV-VIS spectra of MET (Figure 1) were obtained for 10 mg L−1 aqueous solution on a PerkinElmer UV/vis Lambda 20 (200–400 nm range) spectrophotometer.Figure 1
Absorbance spectrum of MET for aqueous concentration of 10 mg L−1 (left axis) and lamp spectrum (right axis), where f(λ) represents the spectral distribution of the lamp.


### 2.3. Experimental Procedure

Photodegradation experiments were conducted in a Solarbox (CO.FO.MEGRA, Milan, Italy) and equipped with a Xenon lamp (Phillips XOP, 1000W) and a tubular-horizontal photoreactor (0.084L illuminated volume) located at the axis of a parabolic mirror in the bottom of the Solarbox. The photon flux inside the photoreactor was evaluated by o-nitrobenzaldehyde actinometry [28, 29], being 2.68 μEinstein s−1. A stirred reservoir tank (1.0 L) was filled with the pharmaceutical-TiO2 (suspended) aqueous solution. The solution was continuously pumped (peristaltic pump Ecoline VC-280 II, Ismatec) to the equipment and recirculated to the reservoir tank with a flow of 0.65 L min−1. In order to keep the solution at 25°C, the jacket temperature of the stirred tank was controlled with an ultrathermostat bath (Haake K10). Samples were taken every 30 minutes during 300 minutes and quickly analyzed. Before HPLC analysis, samples were filtered through 0.20 μm PVDF membrane to separate TiO2. All the experiments were duplicated and the results presented were the mean values.According to the literature [13], metoprolol stability in aqueous solution was previously verified, by storing 50 mg L−1 during 3 days in the dark at room temperature, and no degradation was observed.MET adsorption of TiO2 was also measured. Thus, MET solution (0 to 50 mg L−1) was prepared with TiO2 in suspension (0.4 g L−1) and placed into 25 mL hermetic closed flasks, adjusting the pH with NaOH solution (0.1 mol L−1). The conical flasks were shaken at a constant speed of 100 rpm and at room temperature (25 ± 0.5°C). Samples were taken every 24 h, assuming that adsorption equilibrium was reached.For the identification of byproducts, the final sample mixture, at 300 minutes, was analyzed by electrospray ionization/mass spectrometry using a PerSeptive, TOF Mariner Jascoo AS-2050 plus IS mass spectrometer into them/z range of 50–1000. The experiments were carried out in replicate.


## 2.1. Chemicals and Reagents

Metoprolol tartrate (MET) salt was purchased from Sigma Aldrich Chemical Co. (Spain) and used as received (1-[4-(2 methoxyethyl)phenoxy]-3-(propan-2-ylamino)propan-2-ol tartrate (2:1), CAS no 56392-17-7, (C15H25NO3)2 C4H6O6, MW 684.81). Solutions of 50 mg L−1 of MET were prepared using deionized water to assure accurate measurements of concentrations, to follow the TOC, to secure identification of intermediates, and to make predictions about possible mechanisms of photocatalysis. For pH adjustment, 0.1 mol L−1 sulphuric acid or 0.1 mol L−1 sodium hydroxide was used. All chemicals were HPLC grade, and they were used without further purification. Titanium dioxide (TiO2) Degussa P-25 (commercial catalyst ~70% anatase, ~30% rutile, surface area 50 ± 5.0 m2 g−1, and 300 μm particle size [25]) was used as received. This TiO2 is a photochemical stable material [6, 26, 27].


## 2.2. Analytical Instruments

The target compounds concentrations were monitored by a high-performance liquid chromatograph (HPLC) from Waters using aSEA18 5 μm 15 × 0.46 Teknokroma column and Waters 996 photodiode array detector using Empower Pro software 2002 Water Co. The mobile phase was composed by water and acetonitrile (20 : 80), injected with a flow-rate of 0.85 mL min−1, and detected at maximum metoprolol (221.9 nm). Total organic carbon (TOC) was measured in a Shimadzu TOC-V CNS. pH was measured by a Crison GLP 22 instrument. UV-VIS spectra of MET (Figure 1) were obtained for 10 mg L−1 aqueous solution on a PerkinElmer UV/vis Lambda 20 (200–400 nm range) spectrophotometer.Figure 1
Absorbance spectrum of MET for aqueous concentration of 10 mg L−1 (left axis) and lamp spectrum (right axis), where f(λ) represents the spectral distribution of the lamp.


## 2.3. Experimental Procedure

Photodegradation experiments were conducted in a Solarbox (CO.FO.MEGRA, Milan, Italy) and equipped with a Xenon lamp (Phillips XOP, 1000W) and a tubular-horizontal photoreactor (0.084L illuminated volume) located at the axis of a parabolic mirror in the bottom of the Solarbox. The photon flux inside the photoreactor was evaluated by o-nitrobenzaldehyde actinometry [28, 29], being 2.68 μEinstein s−1. A stirred reservoir tank (1.0 L) was filled with the pharmaceutical-TiO2 (suspended) aqueous solution. The solution was continuously pumped (peristaltic pump Ecoline VC-280 II, Ismatec) to the equipment and recirculated to the reservoir tank with a flow of 0.65 L min−1. In order to keep the solution at 25°C, the jacket temperature of the stirred tank was controlled with an ultrathermostat bath (Haake K10). Samples were taken every 30 minutes during 300 minutes and quickly analyzed. Before HPLC analysis, samples were filtered through 0.20 μm PVDF membrane to separate TiO2. All the experiments were duplicated and the results presented were the mean values.According to the literature [13], metoprolol stability in aqueous solution was previously verified, by storing 50 mg L−1 during 3 days in the dark at room temperature, and no degradation was observed.MET adsorption of TiO2 was also measured. Thus, MET solution (0 to 50 mg L−1) was prepared with TiO2 in suspension (0.4 g L−1) and placed into 25 mL hermetic closed flasks, adjusting the pH with NaOH solution (0.1 mol L−1). The conical flasks were shaken at a constant speed of 100 rpm and at room temperature (25 ± 0.5°C). Samples were taken every 24 h, assuming that adsorption equilibrium was reached.For the identification of byproducts, the final sample mixture, at 300 minutes, was analyzed by electrospray ionization/mass spectrometry using a PerSeptive, TOF Mariner Jascoo AS-2050 plus IS mass spectrometer into them/z range of 50–1000. The experiments were carried out in replicate.


## 3. Results and Discussion

### 3.1. Effect of UV Radiation Photolysis on Metoprolol Degradation

When studying photocatalysis, it is very important to be able to separate the influence of photolysis, since it is expected to tackle the degradation of the substances mainly induced by the action of the catalyst. For this purpose, a series of experiments was done with UV illumination, and without catalyst to highlight the metoprolol ability to absorb the radiation reaching the system.Figure2 shows the results obtained after applying simulated sunlight. As observed, MET is not fast enough to be photodegraded in water by direct photolysis [30]; only 26% of MET in 300 minutes was degraded under simulated UV. Moreover, it shows that direct photolysis was not able to produce MET mineralization at the experimental conditions tested. This behavior can be explained because the MET absorption spectrum overlaps only slightly the spectrum of the incoming radiation (Figure 1).Figure 2
MET photodegradation removal (○) and TOC/TOCo (●) under simulated UV.The UV-VIS absorbance was used to calculate the molar absorption coefficient (ε) of the metoprolol at a wavelength of 221.9 nm (Figure 1), assuming that Beer-Lambert’s law is followed:
(1)A=-log(T)=ε×l×C,
where A is the absorbance (measured directly by the spectrophotometer), T is the transmittance, ε is the molar absorption coefficient, l is the distance that the light travels through the material, and C is the concentration of pollutant. The molar absorption coefficient (ε) was 281 L mol−1 cm−1; this value is very similar to other reported values [12, 13]. This low value explains the MET stability in direct photolysis conditions. Nevertheless, different studies [12, 13, 31] show a high photoability of some β-blockers, for example, propranolol, nadolol, and alprenolol. The rapid photodegradation of these compounds was supported by a high molecular absorption coefficient (ε > 800 L mol−1 cm−1). This confirmed the hypothesis that photoinitiated reactions contribute to the degradation of naphthalene backbone (i.e., propranolol) [32], whereas the metoprolol, having a benzoic skeleton, is not sensitive to direct photolysis when dissolved in deionized water [33].The efficiency of the photochemical transformation process depends on many factors such as the irradiation setups, the characteristics of the light source, the water matrix used, the initial concentration, and the pH of the solutions [31]. Tests were carried out using different photoreactors, a borosilicate Duran, and quartz glass reactor, cutting out wavelengths shorter than 290 and 320 nm, respectively. Other experiments have been done with and without glass filter for restricting transmissions of light below 280 nm.In this study, the effect of borosilicate Duran and quartz glass material reactor has been investigated under UV radiation. It was observed that MET removal was 25% and 28% and the TOC reduction was 3.60% and 1.62%, for reactors made with borosilicate Duran and quartz, respectively. Thus, although the mineralization was not significant, there is a small photodegradation of MET for the two tested reactors, after 300 minutes of reaction. Moreover, the effect of a filter glass cutting out wavelengths shorter than 280 nm has been investigated. As a result, only 19% of MET in 300 minutes has been removed with the glass filter; however, MET removal of 25% can be achieved without filter glass. TOC conversion was 6.37% and 3.60% with and without filter, correspondingly after 300 minutes, thus confirming that the mineralization is very low in both cases.Summarizing, UV irradiation in the absence of TiO2 achieved an MET degradation lower than 30% after 300 minutes of irradiation, confirming that the direct photolysis is not fast enough to be considered as an adequate technology.


### 3.2. The Role of the Adsorption on the Photocatalytic Degradation

Since the adsorption can play an important role in the evolution of the photodegradation, adsorption experiments at constant temperature (25 ± 0.5°C) were carried out. The adsorption capacity of MET,qe (mg g−1), was calculated from the difference in MET concentration in the aqueous phase before and after adsorption at different initial MET concentrations (0, 6.2, 12.5, 25, 37.5, and 50 mg L−1). The variation in adsorption of MET onto TiO2 was studied at two pHs: 9 and free pH (pH≈5.8). Figure 3 presents the obtained results and indicates that the amount adsorbed increases when pH does it.Figure 3
Effect of pH on adsorption of MET over TiO2 at 25°C, pH 9 (●), and free pH (○).The increase in the adsorption of metoprolol with increasing pH can be elucidated by considering the surface charge of the adsorbent material (pHpzc ~ 6.5) [13, 34]. That is, titanium dioxide surface is positively charged in acid media pH (pH ≤ 7) whereas it is negatively charged under alkaline conditions (pH ≥ 7) [29, 35]. Also, metoprolol can be transformed to MET anion in the basic pH (pH ~ 10) since the pKa value of metoprolol is 9.7 [36]. Under free pH conditions, close to the point zero charge of TiO2 (6.5) [30], MET is positively charged. A low adsorption was observed due to no electrostatic attraction between the surface charge and MET. A highest adsorption between MET and TiO2 would be observed at pH 9, because the negative charges of the surface of the catalyst attract the protonated MET form. In addition the photocatalytic degradation would be expected on the surface of the catalysis.Two-parameter isotherm models (Langmuir, Freundlich, Temkin, and Dubinin-Radushkevich) and three-parameter isotherm models (Redlich-Peterson and Langmuir-Freundlich) were tested in the fitting of the adsorption data of MET onto titanium dioxide [37, 38].K
a, KF, KT, KRP, and KL are the Langmuir, Freundlich, Temkin, Redlich-Peterson and Langmuir-Freundlich adsorption equilibrium constants (L mol−1), respectively; aR and aLF are also  the Redlich-Peterson and Langmuir-Freundlcih constants (L mol−1), respectively; Ce and qe are the equilibrium concentration (mol L−1) and the adsorption capacity (mol g−1), respectively; qD is the Dubinin-Radushkevich saturation capacity (mol g−1). The parameter qm represents the maximum monolayer adsorption capacity (mol g−1) and 1/n the adsorption intensity, which provides an indication of favorability and capacity of the adsorbent/adsorbate system. The parameter b is related to the adsorption heat; BD gives the mean adsorption free energy ED (kJ mol−1). The parameters β and nLF are the Redlich-Peterson and Langmuir-Freundlich exponents which lie between 0 and 1 [39]. And R2 is the corresponding sum of squares error obtained in the fitting experimental data of each model.From Table1, it was observed that the best fitting were obtained for Langmuir isotherm (R2 = 0.987 and 0.998 for free pH and pH 9, respectively). Thus, these models represent the equilibrium adsorption of MET on TiO2 particles in the range of concentration studied. Accordingly, the adsorption mechanism may be interpreted as a monolayer coverage of the catalyst surface.Table 1
Isotherm parameters for MET adsorption onto TiO2 obtained by linear method at 25°C.
Two-parameter model
Parameters
pH
Free
9
Langmuirqe=qmKaCe1+KaCe
q
m (mol g−1)
0.0014
0.0250
K
L (L mol−1)
0.0930
0.0817
R
2
0.987
0.998
Freundlichqe=KFCe1/n
1
/
n
0.244
0.670
K
F (L mol−1)
0.00042
0.00129
R
2
0.105
0.147
Temkinqe=RTbln(KT+Ce)
R
T
/
b
0.00024
0.00508
K
T  (L mol−1)
2.718
0.962
R
2
0.604
0.982
Dubinin-Radushkevichqe=qDexp(-Bd[RTln(1+1Ce)])
q
D (mol g−1)
0.0013
0.0233
B
D
×
10
-
3 (mol2 kJ−2)
1.533
1.532
R
2
0.835
0.778
Three-parameter model
Redlich-Petersonqe=KRPCe1+aRCeβ
K
RP (L mol−1)
0.00011
0.10
a
R(L mol−1)
0.051
18.040
β
0.999
0.679
R
2
0.826
0.789
Langmuir-Freundlichqe=KLFCenLF1+(aLFCe)nLF
K
LF (L mol−1)
0.000205
0.00809
a
LF (L mol−1)
0.134
0.310
n
LF
0.779
0.92
R
2
0.211
0.734For free pH MET adsorption (qm) was lower than for pH 9, 0.0014 mol g−1, and 0.0250 mol g−1, respectively. In these cases, the adsorption does not play an important role in the photocatalytic process. The MET percentage removal in dark conditions was 0.1% and 11% for free pH and pH 9. These low adsorption values and MET percentage removals suggest that the most possible way of degradation could be reached by migration of •OH radicals to the bulk of the suspension.


### 3.3. Degradation of MET by Photocatalytic Process

The photocatalytic degradation of MET solution (50 mg L−1) was carried out during 300 minutes, in the presence of 0.4 g L−1 of TiO2 under UV-VIS light at room temperature. It is know that, in heterogeneous photocatalysis, the rate of degradation is not always proportional to the catalyst load [40]. An optimal point exists where TiO2 loaded shows a maximum degradation rate. Previous studies carried out in our research group reported that the optimum catalyst concentration was 0.4 g L−1 [41]. Over this value, scattering can appear, and therefore increase in degradation rate does not occur.Firstly, the solution mixture was stirred for 24 hours without irradiation in order to get the equilibrium of MET adsorption.Figure4 depicts the photocatalytic degradation of MET at free pH and pH 9.   Maximum conversions are achieved at 240 and 300 minutes for pH 9 and free pH, respectively. An important remark is that the initial removal rate for free pH and pH 9 experiments is different, being higher at pH 9.  The effect of pH on the conversion is a complex issue related to the ionization states of the catalyst surface and the substrate, as well as the rate of formation of radicals and other reactive species in the reaction mixture [42]. These effects can be assessed since the action of the holes is favored at acidic conditions, while hydroxyl radicals become the dominant species at neutral and alkaline conditions [42].Figure 4
MET and TOC removal (%) versus time (min) at free pH and pH 9 in photocatalytic experiments.As known, photocatalysis occurs through the energy adsorption by the catalyst (light between 200 and 400 nm for TiO2). Under excited condition, the valance band-electron is transferred to the conduction band forming the hole-electron pair (h+/e-) (2). The hydroxyl radicals are formed by cleavage of adsorbed molecules of water [43]:
(2)TiO2+hγ⟶TiO2*(h+e-)(3)h++H2O⟶∙OH+H+
If organic compounds are absorbed on the surface of the catalyst, the •OH nonselective attack promotes the cleavage of compounds bounds. The higher MET degradation and the low MET adsorption on catalyst at a pH 9 suggest that the •OH attack in the bulk of solution can be responsible for the MET degradation [40, 44].The values of TOC during the photocatalytic degradation of MET, at two different pHs, are given in Figure4. The TOC increases with time, indicating the increasing mineralization of the initial organic structures.


### 3.4. Kinetics of MET Degradation

The Langmuir-Hinshelwood (L-H) model is usually used to describe the kinetics of photocatalytic degradation of organic pollutants [12, 13, 30, 31, 41, 45], being the kinetic equation expressed as
(4)r=-dCdt=Kads·kH-L·C1+Kads·C,
where r is the degradation rate,  C is the reactant concentration,  t  is the time, kH-L is the rate constant, and Kad is the adsorption equilibrium constant.This model assumes that adsorption is a rapid equilibrium process and that the rate-determining step of the reaction involves the species present in a monolayer at the solid–liquid interface. Furthermore if the adsorption of MET onto the surface of the photocatalysts is very low,Kads·C can be neglected in the denominator simplifying the equation to a pseudo-first-order equation as given by [46]
(5)r=-dCdt=Kads·kH-L·C=k·C.
The integrated form of the above equation is represented by
(6)ln(CoC)=kapp·t,
where C0 is the initial pollutant concentration and kapp is the apparent pseudo-first-order reaction rate constant.The half-life was calculated with the following expression:(7)t1/2=ln2k.
The values of t1/2 in Table 2 verify that the direct photolysis under simulated light was very low. The low photodegradation of MET was also supported by a low molar absorption coefficient (281 L mol−1 cm−1) measured at 221.9 nm wavelength. However, an important increasing difference is observed in the MET degradation when TiO2 is present. Also, when photocatalytic process is applied, results in TOC conversion (63%) are notoriously improved, for initial concentration of 50 mg L−1 of MET and 0.4 g L−1 of catalyst.Table 2
Kinetics of metoprolol UV-C photodegradation under different conditions.
Glass material reactor
Glass filterλ≥280 nm
pH
t
1
/
2 (h)
Photolysis
Borosilicate
with
5.8
±
1
16.5
±
0.5
without
5.8
±
1
11.6
±
0.6
Quartz
without
5.8
±
1
10.5
±
0.5
Photocatalysis
Borosilicate
without
5.8
±
1
0.81
±
0.4
without
9.0
±
1
0.58
±
0.3If both processes are compared, photocatalytic process is always much faster than the photolytic degradation of MET. Therefore, the interest of using photocatalysis in the treatment of this type of pollutant is obvious.


### 3.5. Intermediates during Reaction

The major by-products formed during 6 hours of photocatalytic treatment of MET were identified (Figure5). The study was carried out using HPLC/MS in positive electrospray model. The degradation intermediates for MET are shown in Table 3.Table 3
Intermediates proposed for the photocatalytic degradation of MET.
Detected compound (DP)
Ret. time(min)
m
/
z (Da)
Molecular formula
Proposed structure
Metoprolol
3.24
268
C15H25NO3
1
2.59
74
C4H11N
2
3.24
76
C3H9NO
3
2.59
92
C3H9NO2
4
2.59
102
C5H11NO
5
2.59
116
C6H13NO
6
3.24
118
C6H15NO
7
2.59
120
C5H125NO2
8
2.59
134
C6H15NO2
9
3.23
161
C11H12O
10
3.23
193
C12H16O2
11
3.24
208
C12H17NO2
12
3.03
220
C13H17NO2
13
3.03
226
C12H19NO3
14
4.71
238
C13H19NO3
15
3.23
240
C13H21NO3
16
3.98
300
C15H25NO5
17
3.98
316
C13H25NO6
18
3.23
332
C13H19NO7Figure 5
MS spectrum of major oxidation products of metoprolol.The metoprolol has a molecular weight [M + H+] = 268. Three intermediates corresponding to the binding of •OH radicals in the aromatic ring were detected atm/z 300, 316, and 332, di-(DP (Detected Compound) 16), tri-(DP 17), and tetrahydroxy (DP 18) DPs, respectively. After breaking the C–C bond in the aliphatic part of the MET molecule, amino-diol (DP 8) was identified as one of the dominant intermediates with m/z = 134.  Different fragments of the ethanolamine side were also identified (DP 1, DP 2, DP 3, DP 4, DP 5, DP 6, and DP 7), probably due to the loss of the hydroxyl group and the loss of isopropyl moiety.PD 15 can be formed probably by reactions which involve attack on the ether side chain followed by elimination. On the other hand, the oxidation of alcohols to aldehydes can be explained by the formation of DP 14 withm/z=238 [47].  The hydrogen abstraction and the water elimination of DP 14 probably generate a carbonyl, followed by an intermolecular electron transfer; it generates a double bond and the consequent formation of DP 12.Oxidative attack on the dimethylamine moiety results in a DP 13 withm/z=226. Following this, the hydrogen abstraction and elimination of water of DP 13 generate a carbonyl which followed by intermolecular electron transference, generates a double bond and forming DP 11. The DP 11 can generate DP 10 corresponding to a loss of ammonia after the hydrogen abstraction. The intermediate 9 could be formed by the loss of methanol combined with the attack of •OH on the C atom next to the ether oxygen in the aliphatic part of DP 10.A simplified fragmentation pathway of metoprolol degradation is shown in Figure6.Figure 6
Proposed pathways for the degradation of MET.


## 3.1. Effect of UV Radiation Photolysis on Metoprolol Degradation

When studying photocatalysis, it is very important to be able to separate the influence of photolysis, since it is expected to tackle the degradation of the substances mainly induced by the action of the catalyst. For this purpose, a series of experiments was done with UV illumination, and without catalyst to highlight the metoprolol ability to absorb the radiation reaching the system.Figure2 shows the results obtained after applying simulated sunlight. As observed, MET is not fast enough to be photodegraded in water by direct photolysis [30]; only 26% of MET in 300 minutes was degraded under simulated UV. Moreover, it shows that direct photolysis was not able to produce MET mineralization at the experimental conditions tested. This behavior can be explained because the MET absorption spectrum overlaps only slightly the spectrum of the incoming radiation (Figure 1).Figure 2
MET photodegradation removal (○) and TOC/TOCo (●) under simulated UV.The UV-VIS absorbance was used to calculate the molar absorption coefficient (ε) of the metoprolol at a wavelength of 221.9 nm (Figure 1), assuming that Beer-Lambert’s law is followed:
(1)A=-log(T)=ε×l×C,
where A is the absorbance (measured directly by the spectrophotometer), T is the transmittance, ε is the molar absorption coefficient, l is the distance that the light travels through the material, and C is the concentration of pollutant. The molar absorption coefficient (ε) was 281 L mol−1 cm−1; this value is very similar to other reported values [12, 13]. This low value explains the MET stability in direct photolysis conditions. Nevertheless, different studies [12, 13, 31] show a high photoability of some β-blockers, for example, propranolol, nadolol, and alprenolol. The rapid photodegradation of these compounds was supported by a high molecular absorption coefficient (ε > 800 L mol−1 cm−1). This confirmed the hypothesis that photoinitiated reactions contribute to the degradation of naphthalene backbone (i.e., propranolol) [32], whereas the metoprolol, having a benzoic skeleton, is not sensitive to direct photolysis when dissolved in deionized water [33].The efficiency of the photochemical transformation process depends on many factors such as the irradiation setups, the characteristics of the light source, the water matrix used, the initial concentration, and the pH of the solutions [31]. Tests were carried out using different photoreactors, a borosilicate Duran, and quartz glass reactor, cutting out wavelengths shorter than 290 and 320 nm, respectively. Other experiments have been done with and without glass filter for restricting transmissions of light below 280 nm.In this study, the effect of borosilicate Duran and quartz glass material reactor has been investigated under UV radiation. It was observed that MET removal was 25% and 28% and the TOC reduction was 3.60% and 1.62%, for reactors made with borosilicate Duran and quartz, respectively. Thus, although the mineralization was not significant, there is a small photodegradation of MET for the two tested reactors, after 300 minutes of reaction. Moreover, the effect of a filter glass cutting out wavelengths shorter than 280 nm has been investigated. As a result, only 19% of MET in 300 minutes has been removed with the glass filter; however, MET removal of 25% can be achieved without filter glass. TOC conversion was 6.37% and 3.60% with and without filter, correspondingly after 300 minutes, thus confirming that the mineralization is very low in both cases.Summarizing, UV irradiation in the absence of TiO2 achieved an MET degradation lower than 30% after 300 minutes of irradiation, confirming that the direct photolysis is not fast enough to be considered as an adequate technology.


## 3.2. The Role of the Adsorption on the Photocatalytic Degradation

Since the adsorption can play an important role in the evolution of the photodegradation, adsorption experiments at constant temperature (25 ± 0.5°C) were carried out. The adsorption capacity of MET,qe (mg g−1), was calculated from the difference in MET concentration in the aqueous phase before and after adsorption at different initial MET concentrations (0, 6.2, 12.5, 25, 37.5, and 50 mg L−1). The variation in adsorption of MET onto TiO2 was studied at two pHs: 9 and free pH (pH≈5.8). Figure 3 presents the obtained results and indicates that the amount adsorbed increases when pH does it.Figure 3
Effect of pH on adsorption of MET over TiO2 at 25°C, pH 9 (●), and free pH (○).The increase in the adsorption of metoprolol with increasing pH can be elucidated by considering the surface charge of the adsorbent material (pHpzc ~ 6.5) [13, 34]. That is, titanium dioxide surface is positively charged in acid media pH (pH ≤ 7) whereas it is negatively charged under alkaline conditions (pH ≥ 7) [29, 35]. Also, metoprolol can be transformed to MET anion in the basic pH (pH ~ 10) since the pKa value of metoprolol is 9.7 [36]. Under free pH conditions, close to the point zero charge of TiO2 (6.5) [30], MET is positively charged. A low adsorption was observed due to no electrostatic attraction between the surface charge and MET. A highest adsorption between MET and TiO2 would be observed at pH 9, because the negative charges of the surface of the catalyst attract the protonated MET form. In addition the photocatalytic degradation would be expected on the surface of the catalysis.Two-parameter isotherm models (Langmuir, Freundlich, Temkin, and Dubinin-Radushkevich) and three-parameter isotherm models (Redlich-Peterson and Langmuir-Freundlich) were tested in the fitting of the adsorption data of MET onto titanium dioxide [37, 38].K
a, KF, KT, KRP, and KL are the Langmuir, Freundlich, Temkin, Redlich-Peterson and Langmuir-Freundlich adsorption equilibrium constants (L mol−1), respectively; aR and aLF are also  the Redlich-Peterson and Langmuir-Freundlcih constants (L mol−1), respectively; Ce and qe are the equilibrium concentration (mol L−1) and the adsorption capacity (mol g−1), respectively; qD is the Dubinin-Radushkevich saturation capacity (mol g−1). The parameter qm represents the maximum monolayer adsorption capacity (mol g−1) and 1/n the adsorption intensity, which provides an indication of favorability and capacity of the adsorbent/adsorbate system. The parameter b is related to the adsorption heat; BD gives the mean adsorption free energy ED (kJ mol−1). The parameters β and nLF are the Redlich-Peterson and Langmuir-Freundlich exponents which lie between 0 and 1 [39]. And R2 is the corresponding sum of squares error obtained in the fitting experimental data of each model.From Table1, it was observed that the best fitting were obtained for Langmuir isotherm (R2 = 0.987 and 0.998 for free pH and pH 9, respectively). Thus, these models represent the equilibrium adsorption of MET on TiO2 particles in the range of concentration studied. Accordingly, the adsorption mechanism may be interpreted as a monolayer coverage of the catalyst surface.Table 1
Isotherm parameters for MET adsorption onto TiO2 obtained by linear method at 25°C.
Two-parameter model
Parameters
pH
Free
9
Langmuirqe=qmKaCe1+KaCe
q
m (mol g−1)
0.0014
0.0250
K
L (L mol−1)
0.0930
0.0817
R
2
0.987
0.998
Freundlichqe=KFCe1/n
1
/
n
0.244
0.670
K
F (L mol−1)
0.00042
0.00129
R
2
0.105
0.147
Temkinqe=RTbln(KT+Ce)
R
T
/
b
0.00024
0.00508
K
T  (L mol−1)
2.718
0.962
R
2
0.604
0.982
Dubinin-Radushkevichqe=qDexp(-Bd[RTln(1+1Ce)])
q
D (mol g−1)
0.0013
0.0233
B
D
×
10
-
3 (mol2 kJ−2)
1.533
1.532
R
2
0.835
0.778
Three-parameter model
Redlich-Petersonqe=KRPCe1+aRCeβ
K
RP (L mol−1)
0.00011
0.10
a
R(L mol−1)
0.051
18.040
β
0.999
0.679
R
2
0.826
0.789
Langmuir-Freundlichqe=KLFCenLF1+(aLFCe)nLF
K
LF (L mol−1)
0.000205
0.00809
a
LF (L mol−1)
0.134
0.310
n
LF
0.779
0.92
R
2
0.211
0.734For free pH MET adsorption (qm) was lower than for pH 9, 0.0014 mol g−1, and 0.0250 mol g−1, respectively. In these cases, the adsorption does not play an important role in the photocatalytic process. The MET percentage removal in dark conditions was 0.1% and 11% for free pH and pH 9. These low adsorption values and MET percentage removals suggest that the most possible way of degradation could be reached by migration of •OH radicals to the bulk of the suspension.


## 3.3. Degradation of MET by Photocatalytic Process

The photocatalytic degradation of MET solution (50 mg L−1) was carried out during 300 minutes, in the presence of 0.4 g L−1 of TiO2 under UV-VIS light at room temperature. It is know that, in heterogeneous photocatalysis, the rate of degradation is not always proportional to the catalyst load [40]. An optimal point exists where TiO2 loaded shows a maximum degradation rate. Previous studies carried out in our research group reported that the optimum catalyst concentration was 0.4 g L−1 [41]. Over this value, scattering can appear, and therefore increase in degradation rate does not occur.Firstly, the solution mixture was stirred for 24 hours without irradiation in order to get the equilibrium of MET adsorption.Figure4 depicts the photocatalytic degradation of MET at free pH and pH 9.   Maximum conversions are achieved at 240 and 300 minutes for pH 9 and free pH, respectively. An important remark is that the initial removal rate for free pH and pH 9 experiments is different, being higher at pH 9.  The effect of pH on the conversion is a complex issue related to the ionization states of the catalyst surface and the substrate, as well as the rate of formation of radicals and other reactive species in the reaction mixture [42]. These effects can be assessed since the action of the holes is favored at acidic conditions, while hydroxyl radicals become the dominant species at neutral and alkaline conditions [42].Figure 4
MET and TOC removal (%) versus time (min) at free pH and pH 9 in photocatalytic experiments.As known, photocatalysis occurs through the energy adsorption by the catalyst (light between 200 and 400 nm for TiO2). Under excited condition, the valance band-electron is transferred to the conduction band forming the hole-electron pair (h+/e-) (2). The hydroxyl radicals are formed by cleavage of adsorbed molecules of water [43]:
(2)TiO2+hγ⟶TiO2*(h+e-)(3)h++H2O⟶∙OH+H+
If organic compounds are absorbed on the surface of the catalyst, the •OH nonselective attack promotes the cleavage of compounds bounds. The higher MET degradation and the low MET adsorption on catalyst at a pH 9 suggest that the •OH attack in the bulk of solution can be responsible for the MET degradation [40, 44].The values of TOC during the photocatalytic degradation of MET, at two different pHs, are given in Figure4. The TOC increases with time, indicating the increasing mineralization of the initial organic structures.


## 3.4. Kinetics of MET Degradation

The Langmuir-Hinshelwood (L-H) model is usually used to describe the kinetics of photocatalytic degradation of organic pollutants [12, 13, 30, 31, 41, 45], being the kinetic equation expressed as
(4)r=-dCdt=Kads·kH-L·C1+Kads·C,
where r is the degradation rate,  C is the reactant concentration,  t  is the time, kH-L is the rate constant, and Kad is the adsorption equilibrium constant.This model assumes that adsorption is a rapid equilibrium process and that the rate-determining step of the reaction involves the species present in a monolayer at the solid–liquid interface. Furthermore if the adsorption of MET onto the surface of the photocatalysts is very low,Kads·C can be neglected in the denominator simplifying the equation to a pseudo-first-order equation as given by [46]
(5)r=-dCdt=Kads·kH-L·C=k·C.
The integrated form of the above equation is represented by
(6)ln(CoC)=kapp·t,
where C0 is the initial pollutant concentration and kapp is the apparent pseudo-first-order reaction rate constant.The half-life was calculated with the following expression:(7)t1/2=ln2k.
The values of t1/2 in Table 2 verify that the direct photolysis under simulated light was very low. The low photodegradation of MET was also supported by a low molar absorption coefficient (281 L mol−1 cm−1) measured at 221.9 nm wavelength. However, an important increasing difference is observed in the MET degradation when TiO2 is present. Also, when photocatalytic process is applied, results in TOC conversion (63%) are notoriously improved, for initial concentration of 50 mg L−1 of MET and 0.4 g L−1 of catalyst.Table 2
Kinetics of metoprolol UV-C photodegradation under different conditions.
Glass material reactor
Glass filterλ≥280 nm
pH
t
1
/
2 (h)
Photolysis
Borosilicate
with
5.8
±
1
16.5
±
0.5
without
5.8
±
1
11.6
±
0.6
Quartz
without
5.8
±
1
10.5
±
0.5
Photocatalysis
Borosilicate
without
5.8
±
1
0.81
±
0.4
without
9.0
±
1
0.58
±
0.3If both processes are compared, photocatalytic process is always much faster than the photolytic degradation of MET. Therefore, the interest of using photocatalysis in the treatment of this type of pollutant is obvious.


## 3.5. Intermediates during Reaction

The major by-products formed during 6 hours of photocatalytic treatment of MET were identified (Figure5). The study was carried out using HPLC/MS in positive electrospray model. The degradation intermediates for MET are shown in Table 3.Table 3
Intermediates proposed for the photocatalytic degradation of MET.
Detected compound (DP)
Ret. time(min)
m
/
z (Da)
Molecular formula
Proposed structure
Metoprolol
3.24
268
C15H25NO3
1
2.59
74
C4H11N
2
3.24
76
C3H9NO
3
2.59
92
C3H9NO2
4
2.59
102
C5H11NO
5
2.59
116
C6H13NO
6
3.24
118
C6H15NO
7
2.59
120
C5H125NO2
8
2.59
134
C6H15NO2
9
3.23
161
C11H12O
10
3.23
193
C12H16O2
11
3.24
208
C12H17NO2
12
3.03
220
C13H17NO2
13
3.03
226
C12H19NO3
14
4.71
238
C13H19NO3
15
3.23
240
C13H21NO3
16
3.98
300
C15H25NO5
17
3.98
316
C13H25NO6
18
3.23
332
C13H19NO7Figure 5
MS spectrum of major oxidation products of metoprolol.The metoprolol has a molecular weight [M + H+] = 268. Three intermediates corresponding to the binding of •OH radicals in the aromatic ring were detected atm/z 300, 316, and 332, di-(DP (Detected Compound) 16), tri-(DP 17), and tetrahydroxy (DP 18) DPs, respectively. After breaking the C–C bond in the aliphatic part of the MET molecule, amino-diol (DP 8) was identified as one of the dominant intermediates with m/z = 134.  Different fragments of the ethanolamine side were also identified (DP 1, DP 2, DP 3, DP 4, DP 5, DP 6, and DP 7), probably due to the loss of the hydroxyl group and the loss of isopropyl moiety.PD 15 can be formed probably by reactions which involve attack on the ether side chain followed by elimination. On the other hand, the oxidation of alcohols to aldehydes can be explained by the formation of DP 14 withm/z=238 [47].  The hydrogen abstraction and the water elimination of DP 14 probably generate a carbonyl, followed by an intermolecular electron transfer; it generates a double bond and the consequent formation of DP 12.Oxidative attack on the dimethylamine moiety results in a DP 13 withm/z=226. Following this, the hydrogen abstraction and elimination of water of DP 13 generate a carbonyl which followed by intermolecular electron transference, generates a double bond and forming DP 11. The DP 11 can generate DP 10 corresponding to a loss of ammonia after the hydrogen abstraction. The intermediate 9 could be formed by the loss of methanol combined with the attack of •OH on the C atom next to the ether oxygen in the aliphatic part of DP 10.A simplified fragmentation pathway of metoprolol degradation is shown in Figure6.Figure 6
Proposed pathways for the degradation of MET.


## 4. Conclusions

Langmuir isotherm fits very well the experimental data, which indicates that the adsorption of the MET onto TiO2 is by monolayer coverage of the catalyst surface. The results confirmed that the degradation of MET is not able to undergo by direct photolysis due to its lower absorption coefficient. In contrast, the addition of TiO2 photocatalyst significantly increases its degradation rate and, after 240 min of irradiation, MET was totally eliminated for pH 9.  The experimental data indicates that TiO2 photocatalysis allows a fast and efficient removal of metoprolol, transforming substrate into by-products that are more difficult to be degraded by photocatalysis, as evidenced by the level of mineralization achieved (63%). Disappearance of MET by photocatalysis follows Langmuir-Hinshelwood model that can be simplified as a pseudo-first-order equation, as usually found in heterogenous photocatalysis at low concentration. Photocatalytic degradation rate of MET depends on pH, occurring the faster degradation at pH 9. At last, based on the identified degradation intermediates at 6-hour reaction time, a photocatalytic degradation pathway of metoprolol was proposed. The main pathways involved in the photocatalytic degradation process include hydroxilation of the aromatic ring, shortening of methoxyl contained in the lateral chain, and cleavage of or addition of •OH to the amine lateral chain.



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*Source: 138918-2013-12-22.xml*