# Doxycycline Degradation by the Oxidative Fenton Process

Authors: Alexandre A. Borghi; Milena F. Silva; Saleh Al Arni; Attilio Converti; Mauri S. A. Palma
Journal: Journal of Chemistry
 (2015)

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## Abstract

Doxycycline is a broad-spectrum tetracycline occurring in domestic, industrial, and rural effluents, whose main drawback is the increasing emergence of resistant bacteria. This antibiotic could be degraded by the so-called Fenton process, consisting in the oxidation of organic pollutants by oxygen peroxide (H2O2) in the presence of Fe2+. Experiments were performed according to an experimental Rotational Central Composite Design to investigate the influence of temperature (0–40.0°C), H2O2 concentration (100–900 mg/L), and Fe2+ concentration (5–120 mg/L) on residual doxycycline and total organic carbon concentrations. Whereas the final residual doxycycline concentration ranged from 0 to 55.8 mg/L, the oxidation process proved unable to reduce the total organic carbon by more than 30%. The best operating conditions were concentrations of H2O2 and Fe2+ of 611 and 25 mg/L, respectively, and temperature of 35.0°C, but the analysis of variance revealed that only the first variable exerted a statistically significant effect on the residual doxycycline concentration. These results suggest possible application of this process in the treatment of doxycycline-containing effluents and may be used as starting basis to treat tetracycline-contaminated effluents.


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## Body

## 1. Introduction

The major source of environmental contamination by drugs is municipal wastewater, either treated or not. However, additional important contributions are given by the effluents of chemical and pharmaceutical industries, the improper disposal of expired drugs, the rural effluents, and the presence of antibiotics in animal manure used to fertilize the soil [1]. World consumption of antibiotics has increased dramatically in the last decade, thus contributing to their release into the environment, either as being in their original form or as metabolites. Most ingested antibiotics are not fully metabolized by humans and animals; therefore, about 25 to 75% of them leave the organism in unaltered form [2–4]. Bacterial resistance is actually now as a major concern, as there are strains resistant to almost all currently known antibiotics [5].Tetracyclines are the third most consumed family of antibiotics, but, owing to their widespread use, a growing number of bacteria resistant to them have been detected [6–8]. They are considered safe antibiotics with a lot of favorable properties such as broad spectrum of antibacterial activity, low toxicity, and low cost [9]. However, there are side health effects, among which the most common are nausea, vomiting, and diarrhea; in addition, patients who take insulin must have special monitoring, since tetracyclines may increase its persistence in the body [10]. Besides their use in humans, tetracyclines are used in animal therapy to treat infections and promote growth [9].Doxycycline is a tetracycline with broad spectrum of action, which is used, in both human and veterinary medicine, against a wide range of Gram-positive and Gram-negative bacteria. Because of its widespread use, its concentration can reach 6.7μg/L in wastewaters and 1.5 mg/kg in domestic sewage sludge [1]; therefore, it becomes of paramount importance to set up efficient and inexpensive techniques to treat these effluents, given the increase in bacterial resistance to this antibiotic.Several processes have been proposed for the treatment of doxycycline-containing effluents, among which there are charcoal adsorption, UV photolysis, ozonation [4], UV/H2O2 photolysis [11], oxidation with H2O2 in the presence of Cu2+ as a catalyst [12], photocatalysis [13], γ-radiolysis, and electron pulse radiolysis of water [9]. A possible alternative to these expensive processes could be the so-called Fenton process that basically consists of the generation of hydroxyl radicals, via dissociation of hydrogen peroxide in aqueous solution catalyzed by the oxidation of the ferrous ion to the ferric one. Indeed, hydroxyl radicals are extremely reactive and nonselective and are widely used to pretreat wastewaters. The main advantages of the Fenton process are its low cost and the formation of nontoxic substances (H2O and O2) by H2O2-induced decomposition, whereas the main drawback is the production of ferric hydroxide sludge.The present work aims to study doxycycline degradation by the Fenton process and to optimize the experimental conditions of temperature, initial concentration of hydrogen peroxide, and initial concentration of ferrous ion in order to minimize the residual concentrations of doxycycline and total organic carbon at the end of the process.


## 2. Materials and Methods

### 2.1. Chemicals

Sulfuric acid (98%), hydrogen peroxide (29%), sodium hydroxide, and ferrous sulfate heptahydrate, potassium iodide, anhydrous sodium sulfite, sodium molybdate, sodium nitrate, methanol, acetic acid, and sodium acetate were purchased from Synth (Diadema, São Paulo, Brazil) and doxycycline hydrochloride was purchased from Calbiochem (San Diego, CA, USA). All the chemical compounds, except the solutions, were of high purity grade reagents.


### 2.2. Experimental Set-Up

A schematic diagram of the experimental set-up used for doxycycline degradation tests is illustrated in Figure1.Figure 1
Schematic diagram of the experimental set-up used for doxycycline oxidation tests by the Fenton process. A = beaker containing 100 mg/L doxycycline hydrochloride solution; B = thermostatic bath (0–100°C); C = mechanical stirrer; D = thermocouple; E = pH meter.A beaker (A) containing an aqueous solution of 100 mg/L doxycycline hydrochloride was immersed in a thermostatic bath (B), model TE 184 (Tecnal, São Paulo, SP, Brazil), for temperature regulation between 0 and 100°C. It was equipped with a mechanical stirrer (C), model RZR 2021 (Heidolph, Schwabach, Germany), a thermocouple (D), model Gulterm 200 (Gulton, São Paulo, SP, Brazil), and a pH meter (E), model 10 MB (Marte, São Paulo, SP, Brazil). Dosages and samplings were done using 0–20, 20–200, and 100–1000μL micropipettes (Finnpipette, Vantaa, Finland) and an analytical balance, model AL 500 (Marte).


### 2.3. Experimental Design

Doxycycline oxidation tests were performed according to a Rotational Central Composite Design (RCCD) [14, 15], whose results in terms of residual doxycycline (CDox,R) and total organic carbon (TOC) concentrations at the end of the process are listed in Table 1.Table 1
Experimental conditions of tests of doxycycline degradation carried out according to the experimental RCCD, coded and uncoded values of the independent variables, and results of residual doxycycline (CDox,R) and total organic carbon (TOC) concentrations at the end of the Fenton process.
Test
X
1
X
2
X
3
C
Fe
2
+ (mg/L)
C
H
2
O
2 (mg/L)
T (°C)
C
Dox
,
R (mg/L)
TOC (mg/L)
1
−1
−1
−1
28.3
262
8.1
28.6
38.4
2
+1
−1
−1
96.7
262
8.1
5.8
45.8
3
−1
+1
−1
28.3
738
8.1
18.5
45.0
4
+1
+1
−1
96.7
738
8.1
4.3
41.7
5
−1
−1
+1
28.3
262
31.9
13.6
41.9
6
+1
−1
+1
96.7
262
31.9
2.6
40.7
7
−1
+1
+1
28.3
738
31.9
7.8
36.0
8
+1
+1
+1
96.7
738
31.9
3.0
40.6
9
−1.68
0
0
5.0
500
20.0
4.4
47.4
10
+1.68
0
0
120.0
500
20.0
3.3
45.3
11
0
−1.68
0
62.5
100
20.0
55.8
46.6
12
0
+1.68
0
62.5
900
20.0
4.7
38.8
13
0
0
−1.68
62.5
500
0.0
21.4
40.7
14
0
0
+1.68
62.5
500
40.0
2.6
40.4
15
0
0
0
62.5
500
20.0
0.0
40.4
16
0
0
0
62.5
500
20.0
0.2
45.6
17
0
0
0
62.5
500
20.0
2.0
45.2
18
0
0
0
62.5
500
20.0
0.0
41.2
19
0
0
0
62.5
500
20.0
0.0
39.2
20
0
0
0
62.5
500
20.0
0.4
38.5
Mean results at the central point
0.43
41.7
Standard deviation at the central point
0.52
3.0
Variation coefficient at the central point
1.21
0.073
C
Fe
2
+ = initial concentration of ferrous ion; CH2O2 = initial concentration of hydrogen peroxide; T = temperature; X1 = coded values of CFe2+;  X2 = coded values of CH2O2;  X3 = coded values of T.


### 2.4. Experimental Procedure

Two hundred mL of 100 mg/L doxycycline hydrochloride solution was transferred to a beaker wrapped in aluminum foil in order to protect it from ambient light, which was then put in a bath thermostated at the selected temperature (0, 8.0, 20.0, 32.0, or 40.0°C) and mechanically stirred at 250 rpm. Once the desired temperature had been reached, ferrous sulfate and hydrogen peroxide solutions were added to the medium up to the achievement of the desired concentrations ofFe2+ (5.0, 28.3, 62.5, 96.7, and 120 mg/L) and H2O2 (100, 262, 500, 738, and 900 mg/L). Every test started with H2O2 addition, whereupon a timer was activated and aliquots of the medium were collected at selected times for analyses.


### 2.5. Chemical Analyses

#### 2.5.1. Determination of Doxycycline Concentration

Since Fe2+ and H2O2 are well known to interfere with the spectrophotometric determination of doxycycline, it was necessary to treat the samples with an aqueous inhibiting solution consisting of 1.0 M potassium iodide, 1.0 M sodium sulfite, and 0.1 M sodium hydroxide as described by Mota et al. [16]. For this purpose, after addition of 1.0 mL of sample to a test tube containing 1.0 mL of this inhibiting solution, the resulting solution was mixed and filtered through cellulose acetate filters with 0.45 μm pore diameter, model N-11106-25 (Sartorius, Göttingen, Germany). A 1.0 mL aliquot of the filtrate was then transferred into a 5.0 mL volumetric flask containing 1.0 mL of 0.005 M Na2MoO4, 0.5 mL of 1.0 M NaNO3, and 0.5 mL of 0.01 M acetate buffer, the pH was adjusted to 5.0, and distilled water was added up to a final volume of 5.0 mL. After mixing, the absorbance of this solution was read at a wavelength of 390 nm using a UV-Vis spectrophotometer, model 600 S (Femto, São Paulo, SP, Brazil). To determine the residual concentration of doxycycline in samples after treatment with the Fenton process, we used doxycycline hydrochloride solutions with known concentrations as standards.


#### 2.5.2. Determination of Total Organic Carbon

To prepare samples for TOC concentration determination, 3.5 mL of the above inhibiting solution was added to 3.5 mL of sample, and the resulting mixture was filtered through cellulose acetate filters. H2SO4 1 : 5 was then added to the filtrate up to a pH value in the range between 2.0 and 3.0, and TOC concentration was finally determined by a TOC-5000A equipment (Shimadzu, Tokyo, Japan).


#### 2.5.3. Identification of Doxycycline Degradation Products

Samples of the reaction medium from the Fenton process carried out under the best conditions identified through the RCCD (CFe2+=25 mg/L, CH2O2=611 mg/L, and T=35.0°C) were collected after 10, 30, 60, 90, 120, and 300 min and submitted to LCMS-IT-TOF analysis to identify doxycycline degradation products. Thirty μL of 0.1 M NaOH was added to 2.0 mL aliquots of the reaction medium to precipitate Fe3+ and neutralize residual H2O2. The resulting solution was then filtered through cellulose acetate filters with 0.45 μm pore diameter, and the pH adjusted to 1.5 with H2SO4 1 : 5.Analyses were made at 40°C under isocratic conditions by a liquid chromatograph, model Prominence UFLC (Shimadzu, Tokyo, Japan), coupled with a mass spectrometer LCMS-IT-TOF, and equipped with a column, model Shim-pack XR-ODS (2.0 × 50 mm, 2μm). The mobile phase was a mixture of 50% methanol and 50% acetic acid (0.1% v/v) aqueous solutions. The mobile phase flow rate was 0.2 mL/min, the injected sample volume 1.0 μL, and the run time 5 min. In the chromatograms, only peaks with height at least three times higher than the noise level were ascribed to degradation products.


## 2.1. Chemicals

Sulfuric acid (98%), hydrogen peroxide (29%), sodium hydroxide, and ferrous sulfate heptahydrate, potassium iodide, anhydrous sodium sulfite, sodium molybdate, sodium nitrate, methanol, acetic acid, and sodium acetate were purchased from Synth (Diadema, São Paulo, Brazil) and doxycycline hydrochloride was purchased from Calbiochem (San Diego, CA, USA). All the chemical compounds, except the solutions, were of high purity grade reagents.


## 2.2. Experimental Set-Up

A schematic diagram of the experimental set-up used for doxycycline degradation tests is illustrated in Figure1.Figure 1
Schematic diagram of the experimental set-up used for doxycycline oxidation tests by the Fenton process. A = beaker containing 100 mg/L doxycycline hydrochloride solution; B = thermostatic bath (0–100°C); C = mechanical stirrer; D = thermocouple; E = pH meter.A beaker (A) containing an aqueous solution of 100 mg/L doxycycline hydrochloride was immersed in a thermostatic bath (B), model TE 184 (Tecnal, São Paulo, SP, Brazil), for temperature regulation between 0 and 100°C. It was equipped with a mechanical stirrer (C), model RZR 2021 (Heidolph, Schwabach, Germany), a thermocouple (D), model Gulterm 200 (Gulton, São Paulo, SP, Brazil), and a pH meter (E), model 10 MB (Marte, São Paulo, SP, Brazil). Dosages and samplings were done using 0–20, 20–200, and 100–1000μL micropipettes (Finnpipette, Vantaa, Finland) and an analytical balance, model AL 500 (Marte).


## 2.3. Experimental Design

Doxycycline oxidation tests were performed according to a Rotational Central Composite Design (RCCD) [14, 15], whose results in terms of residual doxycycline (CDox,R) and total organic carbon (TOC) concentrations at the end of the process are listed in Table 1.Table 1
Experimental conditions of tests of doxycycline degradation carried out according to the experimental RCCD, coded and uncoded values of the independent variables, and results of residual doxycycline (CDox,R) and total organic carbon (TOC) concentrations at the end of the Fenton process.
Test
X
1
X
2
X
3
C
Fe
2
+ (mg/L)
C
H
2
O
2 (mg/L)
T (°C)
C
Dox
,
R (mg/L)
TOC (mg/L)
1
−1
−1
−1
28.3
262
8.1
28.6
38.4
2
+1
−1
−1
96.7
262
8.1
5.8
45.8
3
−1
+1
−1
28.3
738
8.1
18.5
45.0
4
+1
+1
−1
96.7
738
8.1
4.3
41.7
5
−1
−1
+1
28.3
262
31.9
13.6
41.9
6
+1
−1
+1
96.7
262
31.9
2.6
40.7
7
−1
+1
+1
28.3
738
31.9
7.8
36.0
8
+1
+1
+1
96.7
738
31.9
3.0
40.6
9
−1.68
0
0
5.0
500
20.0
4.4
47.4
10
+1.68
0
0
120.0
500
20.0
3.3
45.3
11
0
−1.68
0
62.5
100
20.0
55.8
46.6
12
0
+1.68
0
62.5
900
20.0
4.7
38.8
13
0
0
−1.68
62.5
500
0.0
21.4
40.7
14
0
0
+1.68
62.5
500
40.0
2.6
40.4
15
0
0
0
62.5
500
20.0
0.0
40.4
16
0
0
0
62.5
500
20.0
0.2
45.6
17
0
0
0
62.5
500
20.0
2.0
45.2
18
0
0
0
62.5
500
20.0
0.0
41.2
19
0
0
0
62.5
500
20.0
0.0
39.2
20
0
0
0
62.5
500
20.0
0.4
38.5
Mean results at the central point
0.43
41.7
Standard deviation at the central point
0.52
3.0
Variation coefficient at the central point
1.21
0.073
C
Fe
2
+ = initial concentration of ferrous ion; CH2O2 = initial concentration of hydrogen peroxide; T = temperature; X1 = coded values of CFe2+;  X2 = coded values of CH2O2;  X3 = coded values of T.


## 2.4. Experimental Procedure

Two hundred mL of 100 mg/L doxycycline hydrochloride solution was transferred to a beaker wrapped in aluminum foil in order to protect it from ambient light, which was then put in a bath thermostated at the selected temperature (0, 8.0, 20.0, 32.0, or 40.0°C) and mechanically stirred at 250 rpm. Once the desired temperature had been reached, ferrous sulfate and hydrogen peroxide solutions were added to the medium up to the achievement of the desired concentrations ofFe2+ (5.0, 28.3, 62.5, 96.7, and 120 mg/L) and H2O2 (100, 262, 500, 738, and 900 mg/L). Every test started with H2O2 addition, whereupon a timer was activated and aliquots of the medium were collected at selected times for analyses.


## 2.5. Chemical Analyses

### 2.5.1. Determination of Doxycycline Concentration

Since Fe2+ and H2O2 are well known to interfere with the spectrophotometric determination of doxycycline, it was necessary to treat the samples with an aqueous inhibiting solution consisting of 1.0 M potassium iodide, 1.0 M sodium sulfite, and 0.1 M sodium hydroxide as described by Mota et al. [16]. For this purpose, after addition of 1.0 mL of sample to a test tube containing 1.0 mL of this inhibiting solution, the resulting solution was mixed and filtered through cellulose acetate filters with 0.45 μm pore diameter, model N-11106-25 (Sartorius, Göttingen, Germany). A 1.0 mL aliquot of the filtrate was then transferred into a 5.0 mL volumetric flask containing 1.0 mL of 0.005 M Na2MoO4, 0.5 mL of 1.0 M NaNO3, and 0.5 mL of 0.01 M acetate buffer, the pH was adjusted to 5.0, and distilled water was added up to a final volume of 5.0 mL. After mixing, the absorbance of this solution was read at a wavelength of 390 nm using a UV-Vis spectrophotometer, model 600 S (Femto, São Paulo, SP, Brazil). To determine the residual concentration of doxycycline in samples after treatment with the Fenton process, we used doxycycline hydrochloride solutions with known concentrations as standards.


### 2.5.2. Determination of Total Organic Carbon

To prepare samples for TOC concentration determination, 3.5 mL of the above inhibiting solution was added to 3.5 mL of sample, and the resulting mixture was filtered through cellulose acetate filters. H2SO4 1 : 5 was then added to the filtrate up to a pH value in the range between 2.0 and 3.0, and TOC concentration was finally determined by a TOC-5000A equipment (Shimadzu, Tokyo, Japan).


### 2.5.3. Identification of Doxycycline Degradation Products

Samples of the reaction medium from the Fenton process carried out under the best conditions identified through the RCCD (CFe2+=25 mg/L, CH2O2=611 mg/L, and T=35.0°C) were collected after 10, 30, 60, 90, 120, and 300 min and submitted to LCMS-IT-TOF analysis to identify doxycycline degradation products. Thirty μL of 0.1 M NaOH was added to 2.0 mL aliquots of the reaction medium to precipitate Fe3+ and neutralize residual H2O2. The resulting solution was then filtered through cellulose acetate filters with 0.45 μm pore diameter, and the pH adjusted to 1.5 with H2SO4 1 : 5.Analyses were made at 40°C under isocratic conditions by a liquid chromatograph, model Prominence UFLC (Shimadzu, Tokyo, Japan), coupled with a mass spectrometer LCMS-IT-TOF, and equipped with a column, model Shim-pack XR-ODS (2.0 × 50 mm, 2μm). The mobile phase was a mixture of 50% methanol and 50% acetic acid (0.1% v/v) aqueous solutions. The mobile phase flow rate was 0.2 mL/min, the injected sample volume 1.0 μL, and the run time 5 min. In the chromatograms, only peaks with height at least three times higher than the noise level were ascribed to degradation products.


## 2.5.1. Determination of Doxycycline Concentration

Since Fe2+ and H2O2 are well known to interfere with the spectrophotometric determination of doxycycline, it was necessary to treat the samples with an aqueous inhibiting solution consisting of 1.0 M potassium iodide, 1.0 M sodium sulfite, and 0.1 M sodium hydroxide as described by Mota et al. [16]. For this purpose, after addition of 1.0 mL of sample to a test tube containing 1.0 mL of this inhibiting solution, the resulting solution was mixed and filtered through cellulose acetate filters with 0.45 μm pore diameter, model N-11106-25 (Sartorius, Göttingen, Germany). A 1.0 mL aliquot of the filtrate was then transferred into a 5.0 mL volumetric flask containing 1.0 mL of 0.005 M Na2MoO4, 0.5 mL of 1.0 M NaNO3, and 0.5 mL of 0.01 M acetate buffer, the pH was adjusted to 5.0, and distilled water was added up to a final volume of 5.0 mL. After mixing, the absorbance of this solution was read at a wavelength of 390 nm using a UV-Vis spectrophotometer, model 600 S (Femto, São Paulo, SP, Brazil). To determine the residual concentration of doxycycline in samples after treatment with the Fenton process, we used doxycycline hydrochloride solutions with known concentrations as standards.


## 2.5.2. Determination of Total Organic Carbon

To prepare samples for TOC concentration determination, 3.5 mL of the above inhibiting solution was added to 3.5 mL of sample, and the resulting mixture was filtered through cellulose acetate filters. H2SO4 1 : 5 was then added to the filtrate up to a pH value in the range between 2.0 and 3.0, and TOC concentration was finally determined by a TOC-5000A equipment (Shimadzu, Tokyo, Japan).


## 2.5.3. Identification of Doxycycline Degradation Products

Samples of the reaction medium from the Fenton process carried out under the best conditions identified through the RCCD (CFe2+=25 mg/L, CH2O2=611 mg/L, and T=35.0°C) were collected after 10, 30, 60, 90, 120, and 300 min and submitted to LCMS-IT-TOF analysis to identify doxycycline degradation products. Thirty μL of 0.1 M NaOH was added to 2.0 mL aliquots of the reaction medium to precipitate Fe3+ and neutralize residual H2O2. The resulting solution was then filtered through cellulose acetate filters with 0.45 μm pore diameter, and the pH adjusted to 1.5 with H2SO4 1 : 5.Analyses were made at 40°C under isocratic conditions by a liquid chromatograph, model Prominence UFLC (Shimadzu, Tokyo, Japan), coupled with a mass spectrometer LCMS-IT-TOF, and equipped with a column, model Shim-pack XR-ODS (2.0 × 50 mm, 2μm). The mobile phase was a mixture of 50% methanol and 50% acetic acid (0.1% v/v) aqueous solutions. The mobile phase flow rate was 0.2 mL/min, the injected sample volume 1.0 μL, and the run time 5 min. In the chromatograms, only peaks with height at least three times higher than the noise level were ascribed to degradation products.


## 3. Results and Discussion

Table1 lists the results of doxycycline oxidation tests performed according to a Rotational Central Composite Design (RCCD) in which the concentration of ferrous ion (CFe2+), concentration of hydrogen peroxide (CH2O2), and temperature (T) were selected as the independent variables, while the residual concentrations of doxycycline (CDox,R) and total organic carbon (TOC) were the responses. Although one can see a large variation in the residual doxycycline concentration (0≤CDox,R≤55.8 mg/L), incidentally the lowest values (0≤CDox,R≤2 mg/L) were obtained just at the central point (CH2O2=500 mg/L, CFe2+=62.5 mg/L, and T=20.0°C), suggesting significant influence of the operating conditions on such a response.To investigate these effects in greater detail, the experimental results of both responses were worked out using the Statistica software, version 12 (StatSoft, Tulsa, OK, USA), which showed that onlyCH2O2 had a statistically significant effect (P<0.05) on CDox,R, while TOC reduction at the end of tests did not exceed 30% and was not significantly influenced by any of the independent variables. The best operating conditions to minimize CDox,R (CFe2+=25 mg/L, CH2O2=611 mg/L, and T=35.0°C) were then identified by equating to zero the partial derivatives of the software-generated surface equation
(1)CDox,R=0.625-3.995X1+0.015X12-7.536X2+9.341X22-4.540X3+2.875X32+1.844X1X2+2.676X1X3+0.783X2X3
using the coded values of the three independent variables, namely, CFe2+(X1), CH2O2(X2), and T(X3), that is, finding the function minimum [17]. Such operational conditions were then assumed as the starting point to perform a parametric study, whose results are shown in Figures 2–4 for both responses.Influence of temperature (T) on residual concentrations of (a) doxycycline (CDox,R) and (b) total organic carbon (TOC) at the end of the Fenton process.
(a)
(b)Influence of initial hydrogen peroxide concentration (CH2O2) on residual concentrations of (a) doxycycline (CDox,R) and (b) total organic carbon (TOC) at the end of the Fenton process.
(a)
(b)Influence of initial concentration of ferrous ion (CFe2+) on final concentrations of (a) doxycycline (CDox,R) and (b) total organic carbon (TOC) at the end of the Fenton process.
(a)
(b)The obtained results allowed estimating forCDox,R the regression coefficients listed in Table 2, while those of the related analysis of variance (ANOVA) are presented in Table 3.Table 2
Results of linear (L) and quadratic (Q) regression analyses applied to residual doxycycline concentration data collected at the end of the Fenton process under different operating conditions.
Regression coefficient
Standard error
t
P value
95% Lower confidence limit
95% Upper confidence limit
Mean
0.625
3.688
0.169
0.868
−7.59
8.85
X
1 (L)
−3.995
2.448
−1.635
0.132
−9.46
1.45
X
1 (Q)
−0.015
2.386
−0.005
0.995
−5.33
5.30
X
2 (L)
−7.536
2.448
−3.078
0.011
−12.99
−2.08
X
2 (Q)
9.341
2.386
3.914
0.002
4.02
14.66
X
3 (L)
−4.540
2.448
−1.849
0.094
−9.98
0.93
X
3 (Q)
2.875
2.386
1.204
0.256
−2.44
8.19
X
1
X
2
1.844
3.198
0.578
0.575
−5.28
8.98
X
1
X
3
2.676
3.198
0.828
0.426
−4.48
9.78
X
2
X
3
0.783
3.198
0.242
0.813
−6.35
7.90
L = linear regression; Q = quadratic regression;t = Student’s t-test; X1 = codified values of CFe2+; X2 = codified values of CH2O2;  X3 = codified values of T.Table 3
(a) Results of the analysis of variance applied to residual doxycycline concentration data collected at the end of the Fenton process under different operating conditions. (b) Results obtained by the quadratic model.
(a)
Sum of squares
Degrees of freedom
Mean square
F-calc.
P value
X
1 (L)
218.87
1
218.868
2.68
0.133
X
1 (Q)
0.003
1
0.002
0.00
0.998
X
2 (L)
775.21
1
775.219
9.50
0.012
X
2 (Q)
1253.19
1
1253.195
15.36
0.003
X
3 (L)
279.76
1
279.760
3.43
0.094
X
3 (Q)
118.65
1
118.652
1.46
0.255
X
1
X
2
27.38
1
27.380
0.33
0.575
X
1
X
3
56.18
1
56.180
0.69
0.426
X
2
X
3
4.805
1
4.805
0.06
0.813
(b)
Variation source
Sum of squares
Degrees of freedom
Mean square
F-calc.
P value
Regression
2688.80
9
298.756
3.65
0.0279
Residues
817.95
10
81.795
Lack of fit
814.87
5
162.975
265.14
0.000005
Pure error
3.07
5
0.615
Total
3506.75
19
% explained variation (R2)
76.675
TabledF 9; 10; 0.05
3.02
L = linear regression; Q = quadratic regression;X1 = coded values of CFe2+; X2 = coded values of CH2O2; X3 = coded values of T.Only the linear and quadratic regression coefficients forX2 were statistically significant (P<0.05), which means that only the initial concentration of H2O2 exerted a significant influence on the residual doxycycline concentration in samples collected at the end of the Fenton process.The experimental results shown in Figures2–4 confirm those of ANOVA. In particular, temperature did not statistically significantly influence the performance of the Fenton process in terms either of CDox,R or of TOC (Figure 2). It is likely that doxycycline was completely degraded into compounds able to react with molybdate in the same way as the antibiotic, thus interfering with the spectrophotometric analysis.Instead,CDox,R was strongly influenced by CH2O2 (Figure 3(a)), thereby suggesting that low values of this variable did not lead to the formation of hydroxyl radicals in concentration enough to degrade either doxycycline or its degradation products. On the other hand, as expected, the residual concentration of TOC (Figure 3(b)) was found to be independent of CH2O2, owing to the sensitivity of the analytical methodology to any organic compound finally present in the medium, that is, not only to doxycycline but also to its oxidation products. Finally, the initial concentration of Fe2+ had a dual effect on CDox,R, in that for CFe2+<20 mg/L an increase in this variable led to a remarkable decrease in CDox,R, while no significant influence was detected beyond this threshold value (Figure 4(a)). Since the same behavior was also observed for TOC (Figure 4(b)), it is likely that, at low CFe2+ values, the formation of hydroxyl radicals, as in the first case, was insufficient to promote the degradation of both the antibiotic and its oxidation products.Because of TOC insensitivity to the selected independent variables, to shed light on the phenomena responsible for doxycycline degradation by the Fenton process, samples collected at different times during the test carried out under the best operating conditions (CFe2+=25 mg/L, CH2O2=611 mg/L, and T=35.0°C) were analyzed by LCMS-IT-TOF, whose mean results in terms of molar masses of doxycycline degradation products are summarized in Table 4, while Figure 5 illustrates the most significant chromatograms.Table 4
Molar masses of the main doxycycline degradation products identified by LCMS-IT-TOF at different sampling times during tests carried out under the best operating conditions identified by the RCCD (CFe2+ = 25 mg/L, CH2O2 = 611 mg/L, and T = 35.0°C). (A) Doxycycline, (B–E) main doxycycline degradation products.
Retention time(s)
Sampling time (s)
30
60
180
300
600
Molar mass (g/mol)
41
104 (B)
104 (B)
104 (B)
104 (B)
115
164
154 (D)
164
186
186
186
164
186
240
240
240
184
240
268
268
269
244
268
306
350
350
268
350
350
—
—
306
—
382
—
—
350
—
432
—
54
142
142
142
142
142
164
164
262
262
164
262
262
382
306
262
382
306
444 (A)
382
306
444 (A)
382
502 (E)
444 (A)
382
—
444 (A)
—
502 (E)
404
—
—
—
—
502 (E)
72
—
74
—
—
—
—
262
—
—
—
—
339
—
—
—
—
399 (C)
—
—
—LCMS-IT-TOF results of doxycycline samples submitted to the Fenton process (a) for 60 s, retention time of 41 s, (b) for 180 s, retention time of 54 s. Operating conditions of the Fenton process:CFe2+=25 mg/L, CH2O2=611 mg/L, and T=35.0°C. A, B, D, and E: doxycycline degradation products with MM=444, 104, 154, and 502 g/mol, respectively.
(a)
(b)Based on these results, it is evident that doxycycline, which has an empirical formula of C22H24N2O8 and a molar mass (MM) of 444 g/mol (Figure 6, A), was completely degraded by the Fenton process within only 10 min, that is, already at the beginning of the process, mainly leading to products with less MM (104–399 g/mol) and even one with higher MM (502 g/mol) (E) (Table 4). One can believe that initially formed degradation products suffered an attack by the hydroxyl radical that caused the formation of unstable compounds able to react with other molecules present in the medium, hence allowing the formation of more stable compounds, while maintaining a high TOC level. These results suggest that the hydroxyl radical was capable of promoting either the loss of atoms and functional groups located at doxycycline molecules periphery or the breakdown of aromatic rings.Figure 6
Molecular structures of doxycycline (A) and its degradation products with molar mass of 104 g/mol (B), 399 g/mol (C), and 154 g/mol (D) [9, 11, 13]. (E) Molecular structure of doxycycline degradation product with molar mass of 502 g/mol.According to these results, we sought to identify the main degradation products by comparison with structures proposed by other authors [9, 11, 13] (Figure 6, B–D). In particular, Yuan et al. [11], who investigated the products of doxycycline photolysis by UV and UV/H2O2, identified the same MM=104 g/mol compound detected in this work as propanedioic acid (Figure 6, B), which was the likely result of the breakdown of rings of the drug molecule. The same authors also found a product with MM=186 g/mol, like that detected in our work, but did not suggest any molecular structure for it.Jeong et al. [9], who analyzed doxycycline degradation products formed by the action of hydroxyl radicals generated by the electron pulse radiolysis of water, reported the presence, among others, of a compound with MM=399 g/mol and suggested for it the molecular structure shown in Figure 6, C. On the other hand, Maroga Mboula et al. [13], using the heterogeneous photocatalysis with TiO2, identified, among the degradation products of tetracycline, which differs from doxycycline only for the presence of an additional OH, a compound with MM=154 g/mol, for which they suggested two possible molecular structures (Figure 6, D). Finally, based on the results of search in the database of ChemSpider (Royal Society of Chemistry, Cambridge, UK), we are able to propose for the product with the highest MM (502 g/mol), detected in samples withdrawn from the medium after 3, 5, and 10 min, the structure E illustrated in Figure 6, which could be explained by (a) replacement of the amino group with a carboxymethyl group, (b) attack of a hydroxyl group to the α ring, and (c) formation of a cycle adjacent to the δ ring of doxycycline.


## 4. Conclusions

In this work, dealing with doxycycline degradation by the Fenton process, the optimal conditions of initial concentrations of ferrous ion(CFe2+) and hydrogen peroxide (CH2O2) and of temperature (T), able to minimize the residual doxycycline (CDox,R) and total organic carbon (TOC) concentrations, were identified through a Rotational Central Composite Design.A parametric analysis highlighted that the above three variables exerted different effects onCDox,R, but the analysis of variance showed that CH2O2 was the only one that statistically significantly influenced it. The best experimental conditions able to minimize both residual doxycycline (1.1 mg/L) and TOC (32.8 mg/L) concentrations were CFe2+=25 mg/L, CH2O2=611 mg/L, and T=35.0°C. The TOC results showed that the organic load was not significantly reduced, which indicates that the Fenton process led to the formation of doxycycline oxidation products sensitive to the TOC analytical methodology.A LCMS-IT-TOF investigation allowed identifying the main degradation products of doxycycline oxidation, which were mainly constituted by low molar mass products (104–399 g/mol) as well as a product with higher molar mass (502 g/mol) than doxycycline.



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*Source: 492030-2015-02-24.xml*