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Article

Hydrothermal Enhanced Nanoscale Zero-Valent Iron Activated Peroxydisulfate Oxidation of Chloramphenicol in Aqueous Solutions: Fe-Speciation Analysis and Modeling Optimization

by
Lie Yang
1,2,*,
Hong Li
1,
Jianming Xue
2,3,
Liuyang He
1,
Yongfei Ma
1,
Li Wu
1,* and
Zulin Zhang
1,4,*
1
Hubei Key Laboratory of Mineral Resources Processing and Environment, School of Resources and Environmental Engineering, Wuhan University of Technology, Wuhan 430070, China
2
Scion, Christchurch 8440, P.O. Box 29237, New Zealand
3
College of Biology and the Environment, Nanjing Forestry University, Nanjing 210037, China
4
The James Hutton Institute, Craigiebuckler, Aberdeen ABI5 8QH, UK
*
Authors to whom correspondence should be addressed.
Water 2020, 12(1), 131; https://doi.org/10.3390/w12010131
Submission received: 26 November 2019 / Revised: 21 December 2019 / Accepted: 28 December 2019 / Published: 31 December 2019
(This article belongs to the Special Issue Advanced Oxidation Processes (AOPs) for Urban Wastewater Treatment and Re-use)
Browse Figures
Versions Notes

Abstract

:
The efficiencies of the nanoscale zero-valent iron (nZVI) and hydrothermal and nZVI-heat activation of peroxydisulfate (PS) were studied for the decomposition of chloramphenicol (CAP) in aqueous solutions. The nZVI heat combined with activation of PS provided a significant synergistic effect. A central composite design (CCD) with response surface methodology (RSM) was employed to explore the influences of single parameter and interactions of selected variables (initial pH, PS concentration, nZVI and temperature) on degradation rates with the purpose of condition optimization. A quadratic model was established based on the experimental results with excellent correlation coefficients of 0.9908 and 0.9823 for R2 and R2adj. The optimized experimental condition for 97.12% CAP removal was predicted with the quadratic model as 15 mg/L, 0.5 mmol/L, 7.08 and 70 °C for nZVI dosage, PS, initial pH, and temperature, respectively. This study demonstrated the effectiveness of RSM for the modeling and prediction of CAP removal processes. In the optimal condition, Fe2O3 and Fe3O4 were the predominant solid products after reactions based on X-ray photoelectron spectroscopy (XPS) and X-ray diffraction (XRD) analysis, which could also act as the activators along with the reaction. Overall, it could be concluded that hydrothermal enhanced nZVI activation of PS was a promising and efficient choice for CAP degradation.

1. Introduction

Since the 1950s chloramphenicol (CAP) has acted as a widely applied broad-spectrum antibiotic with excellent antibacterial properties [1,2,3]. Approximately 16% to 38% of CAP potentially leaves organisms as a form of parent compound through feces or urine before being discharged into sewage [4]. It was reported that CAP was not effectively removed by traditional wastewater plants and largely reached surface waters, causing notable ecological risks [5,6]. CAP concentrations of up to 28.36 ng·L−1 have been found in urban water supplies of Shanghai, China [7]. The concentrations of CAP in raw wastewater and biologically treated wastewater were reported as 38.84 ± 44.74 mg·L−1 and 21.24 ± 15.74 mg·L−1, respectively [8]. Its negative effects, such as bone marrow suppression and aplastic anemia cannot be ignored, [9], as they pose a notable threat to human health [10]. Thus, novel techniques are urgently needed for efficient CAP removal.
There have been some techniques applied for CAP removal from aqueous solution, such as adsorption [11,12,13,14,15], nano materials [16,17,18,19], electrochemistry [20,21], and advanced oxidation processes [8]. Among them, persulfate (PS) has, in recent years, attracted great attention as an alternative to H2O2 for advanced oxidation processes due to its high redox potential (2.5 V–3.1 V) and longer lifetime than •OH [22,23,24]. Moreover, PS has the advantage of convenient storage and delivery in the form of solid particles due to its stability in the inactive state [22] and its longevity. It is also non-selective for degradation of a variety of contaminants [25]. There are a series of available methods for PS activation [25]. It is worth mentioning that nanoscale zero-valent iron (nZVI) activation has attracted increasing attention due to its combined effects of Fe0, Fe2+, Fe3+, FeOOH, and Fe3O4 [26]. Furthermore, nZVI has been verified to be capable for decomposing organic pollutants through the reaction with dissolved oxygen to generate •OH, O2•, and HO2• [27,28]. Thus, nZVI-activated PS oxidation could act as a potential choice for CAP removal. As for reaction rate improvement, reaction temperature is a crucial operational variable for aqueous viscosity [29] and mass transfer coefficients [30]. As the temperature increases, heat energy can also act as a persulfate activator to increase the SO4−• radicals [31]. Hydrothermal enhanced degradation of CAP using nZVI-activated PS oxidation was investigated in this study. Response surface methodology (RSM), a widely used optimized tool [32,33,34], was used to assess the selected operational variables based on a proposed quadratic model. The main aims of this study were to: (1) investigate the synergistic effects of a heat/nZVI combined activation of PS on CAP removal and (2) optimize the operational conditions of CAP degradation based on a proposed quadratic model.

2. Material and Methods

2.1. Materials

Chloramphenicol (analytical grade, 99.2%) was bought from Dr. Ehrenstorfer GmbH. Sodium persulfate (Na2S2O8, ≥98%) was obtained from Sinopharm Chemical Reagents Co., Ltd. (Shanghai, China). nZVI (≥99.9%, 50 nm) was purchased from Hubei Institute of Material Protection. All reagents were of analytical grade and all the solution were prepared with Milli-Q ultrapure water. The physicochemical characteristics and molecular details of CAP are demonstrated in Table 1 [6].

2.2. Experimental Setup and Analysis Method

A wide range of CAP concentrations were applied in the other studies, which included 110 mg/L [17], 10 mg/L [21], 20 mg/L [21], and 9.69 mg/L [35]. In this work, all trials were implemented in glass reaction tanks (250 mL) containing 100 mL of CAP solution and the initial concentration was 1 mg/L to simulate a low CAP concentration in wastewater. Before adding PS and nZVI, the reactor with CAP solution was heated in water-bath (HH-4, Changzhou Aohua Instrument Co., Ltd., Changzhou, China) for about 5 min to reach the required temperature (40–80 °C). The solution was continuously stirred with a mechanical stirrer equipped with Teflon stirring blades (DJ1C-40, Jintandadi, Changzhou, China) during the reaction period. A 4 cm diameter blade was placed in the middle of each vessel. The stirring speed was maintained at 250 rpm/min and an entire reaction lasted for 20 min. The solution pH was adjusted using 0.1 mol/L H2SO4 or NaOH solution. At selected time points, 1 mL solution was taken out for further determination and an equal volume of methanol was added into the sample immediately to inhibit CAP oxidation during the determination process. The mixture was filtered through 0.22 μm membrane (Jinteng Ltd., Tianjin, China) and prepared for further LC-MS/MS analysis. The CAP concentrations in the reaction system was determined with Q-SightTM 210 LX50 HPLC (PerkinElmer) coupled to a Triple Quad Mass Spectrometer with electrospray ionization (ESI). A Phenomenex Kinetic C18 100A column (Size 100 × 4.6 mm; particle size 2.6 μm) and negative ESI mode was used for CAP determination. The column temperature was set as 35 °C, and the injection volume was set as 2 μL each time. The mobile phase comprised acetonitrile and water (volume ratio 6:4) and the flow rate was maintained at 0.6 mL/min. The crystalline structure analysis of mixed powder after reactions was conducted with D8 X-ray diffraction (XRD) spectra (Bruker, Germany). Jade 5.0 software was used to determine the crystalline structure of nZVI surface after reactions. In addition, X-ray photoelectron spectroscopy (XPS) analysis of mixed powder was performed using KRATOS Axis Ultra (Kratos Analytical, Manchester, United Kingdom) and analyzed with XPS peak 41 software (Raymund Kwok, HongKong, China).

2.3. Experimental Details

As a widely used method, RSM gives guidance for variable optimization within minimal trial runs by model prediction [36]. In this research, four independent variables were selected and analyzed for the maximal CAP removal from aqueous solution. With a view to exploring the effects of relevant operating variables (initial pH, nZVI dosage, PS concentration, and temperature) on CAP decomposition, the selected vital factors affecting CAP removal rate and the optimal level of interaction were set by central composite design (CCD). For each factor, five levels (+2, +1, 0, −1, and −2) were applied (Table 2) [33]. Thus a four-factor of five-level CCD design with 30 runs was employed, and the five coded levels of each variable were designated as −2, −1, 0, +1, and +2 (Table 3). A software named Design-Expert 8.0.6 (State-Ease, Minneapolis, AL, USA) was used to design, analyze, and optimize the experimental model [33]. All experimental data were analyzed by the least-squares regression method to predict the process response and to estimate the coefficients according to a second-order equation [33]. In order to determine the accuracy and adequacy of the prediction model, the appropriate graph of the “actual vs. predicted” values and the graph of the model response and residual application were presented, respectively. The accuracy of proposed equation was examined using the analysis of variance (ANOVA). Model coefficients calculated by multiple regression analysis of experimental data were analyzed to assess whether a given term had a significant effect (p ≤ 0.05). These effects were outlined based on a fitting quadratic equation. Eventually, the optimized operating condition was calculated and provided to maximize CAP removal.

3. Results and Discussion

3.1. The Synergistic Effect of nZVI-Heat Activated PS Degradation of CAP

With a view to exploring the synergistic effects, CAP degradation was conducted under various treatments (nZVI, PS, nZVI-PS, heat-PS, and nZVI-heat-PS) with initial CAP concentration of 1 mg/L and with 20 min of reaction time. Different CAP degradation efficiencies were obtained in the various processes as demonstrated in Figure 1. The CAP removal efficiencies for nZVI alone and PS alone were only 11.57% and 10.13%, respectively. As for PS activation processes, 22.60%, 42.86%, and 70.89% were obtained in nZVI-PS, heat-PS, and nZVI-heat-PS processes, respectively. The pseudo-first-order kinetic model (Equation (1)) has been widely used to describe the removal of conventional and emerging organic contaminants [18]. The combined degradation of CAP presented an enhanced degradation rate constant (5.76 × 10−2 min−1) compared with the individual activation processes of 1.18 × 10−2 min−1 and 2.86 × 10−2 min−1 for nZVI and heat activation, respectively. There is an equation for the calculation of synergistic influences (Equation (2)) [37]. Synergy index values greater than 1.0 indicated a positive synergistic effect of the combined process [36]. In this research, the combined activated PS degradation of CAP showed a synergistic index of 1.43, indicating an excellent performance of nZVI-heat activation. The phenomenon could be ascribed to a series of complicated reactions including radical effects and non-radical effects. The results evidently verified that the nZVI-heat combined activation of PS oxidation is an alternative solution for CAP removal from aqueous solution.
ln(Ct/C0) = −kobs × t
Synergy index = k(nZVI + heat + PS)/(k(nZVI + PS) + k(heat + PS))

3.2. Model Analysis

The obtained results were fitted with the proposed model. The multiple regression analysis was applied in RSM and the detailed outcomes of regression analysis of the model for CAP removal were summarized (Table 4). Additionally, the significance of linear, interactive, and quadratic terms could be expressed by p-values [33,36]. When p-values < 0.05 (95%), the terms could be considered to be significant. Based on the results, it was observed that the obtained coefficients of all the first-order terms (X1, X2, X3, and X4), two interaction terms (X1X4 and X3X4) and three quadratic coefficients (X12, X32, and X42) were significant (p < 0.05, 95%). The other insignificant term coefficients (p > 0.05, 95%) could be removed from the model due to their insignificant influence on CAP degradation efficiency. As a result, the model was presented in Equation (3) to simulate the CAP degradation efficiency using nZVI + heat + PS processes.
Y = 75.47 + 1.69 X1 + 4.53 X2 − 12.18 X3 + 19.93 X4 − 2.84X1X4 + 10.74 X3X4 + 1.62 X12 − 2.73 X32 − 4.87 X42
Y represents the efficiency of CAP degradation. X1, X2, X3, and X4 represent the terms of nZVI (mg), PS concentration (mM), initial pH, and temperature (°C), respectively. Generally, positive coefficients (>0) indicate favorable effects on degradation efficiency, whereas negative coefficients (<0) indicate unfavorable effects on degradation efficiency [36,38]. Based on data diagnostics, two representative graphs were obtained to verify the accuracy of proposed model. As demonstrated in Figure 2a, the points showed a good linearity and fit well with the normal distribution. According to Figure 2b, it was obvious that the predicted model could predict the degradation efficiency accurately. Thus, the established equation is creditable for the simulation of CAP degradation in the control condition.
The detailed statistical information of the established model was analyzed and summarized in Table 5. The crucial parameters (F, P, CV, R2, and R2adj etc.) were assessed for the validity and accuracy of the proposed model [39,40,41,42]. It was observed that Fisher’s F-value of 115.86 was much higher than 2.3928 (Fcritical,0.05,9,20), implying the significance of the proposed model [33,36]. Additionally, the extremely low probability value (<0.0001) could also confirm the significance of the proposed model. Also, the lack-of-fit (LOF) (F-value 0.0004 < 4.7725) and the adequate precision ratio (AP 35.224 > 4) could confirm the insignificant shortage and sufficient adequacy for the model [33,36]. It was reported that low coefficient of variance (CV) (<10%) meant satisfactory repeatability of experiments [36]. The CV of this study was 4.55% (<10%) and met the mentioned requirement. The R2 (0.9908) and adjusted R2 (0.9823) indicated the model′s satisfactory adequacy for the prediction of CAP removal.

3.3. Interactive Effects of Operational Parameters

The 3D response surface and 2D contour plots, frequently being applied in other studies [32,33], were provided to demonstrate the interactive influences of selected variables (Figure 3). As shown in Table 5, two interaction term coefficients (X1X4 and X3X4) were significant (p < 0.05, 95%), implying that the interactive effects of relevant operational parameters (nZVI and temperature and pH and temperature) were crucial for CAP degradation.
Figure 3a,b show nZVI and temperature impacts on the CAP removal efficiency with 3D and 2D methods, respectively. It was clear that the CAP removal rate was mainly dependent on reaction temperature. With the temperature increasing, the CAP degradation efficiency kept increasing in the selected range. Similar phenomena have been frequently observed especially for thermal activation decomposition of organics [43,44,45,46]. The O–O bond breakage is reasonably enhanced with temperature increase and more SO4•− could be generated via Equation (4) [45]. In addition, reaction temperature is a crucial variable for aqueous viscosity [29] and the mass transfer coefficient [30]. It has been frequently reported that increasing temperature has a positive effect on pollutant degradation [30,31,47,48]. As for nZVI dosage, the CAP removal efficiency was slightly enhanced by increasing nZVI dosage from 15 mg/L to 25 mg/L at 50 °C. On the one hand, nZVI could react with S2O82− to generate Fe2+, which could further activate S2O82− to produce SO4•− (Equations (5) and (6)) [49,50,51]. When Fe2+ accumulates in the solution, it could consume SO4•− via Equation (7) [52]. On the other hand, nZVI could react with dissolved oxygen to generate hydrogen peroxide (H2O2) as an intermediate product and •OH formation would be found [17,19,27]. When nZVI dosage increases, Fe3+ could be reduced to Fe2+ due to the reaction with excessive nZVI via Equation (10) [26]. Then heterogeneous Fe0 activation would be gradually replaced by homogeneous Fe2+ activation along with the reaction process [26,53]. Therefore, the degradation enhancement could be ascribed to the greater Fe2+ formation and the larger contact area between S2O82− and nZVI. It is worth mentioning that the CAP degradation efficiency showed a higher value with a low range of nZVI dosage at 70 °C as demonstrated in Figure 3a,b. The phenomenon was probably attributed to the scavenging effect of Fe2+ on SO4•− via Equation (7). At a high temperature, the mass transfer is accelerated and more Fe2+ is generated with a certain dose of nZVI. It was reported that increasing the Fe2+ concentration beyond a value over 300 μM would accelerate consumption of SO4•− [54]. As a result, appropriate nZVI dosage is vital for the CAP degradation efficiency.
S2O82− + heat→2SO4•−
S2O82− + Fe0→Fe2+ + 2SO42−
S2O82− + Fe2+→Fe3+ + SO42− + SO4•−
SO4•− + Fe2+→Fe3+ + SO42−
Fe0 + O2 + 2H+→H2O2 + Fe2+
H2O2 + Fe2+→Fe3+ + •OH + OH−
2Fe3+ + Fe0→3Fe2+
SO4•− + OH−→SO42− + HO•
Figure 3c,d show pH and temperature impact on the CAP removal efficiency with 3D and 2D methods, respectively. The thermal enhancement has been discussed above. The acidic pH was more favorable than neutral and alkaline pH for CAP removal efficiency at 50 °C, which was evidently due to the enhancement of Equation (8). Increasing Fe2+ could promote the activation of PS (Equation (6)). The amount of soluble Fe2+ decreased at pH > 4.0 due to the formation of Fe2+ complexes which hindered the further activation of PS [55]. SO4•− are rapidly consumed by hydroxyl ions other than CAP and converted to HO• at basic conditions, as shown in Equation (11) [6]. On the whole, acidic pH could promote the CAP degradation based on the increasing Fe2+ activation. When the temperature reached 70 °C, higher removal efficiency was observed in the pH range of 5.5–7.5 according to Figure 3d. Under the circumstance, thermal activation was believed to be the predominant role in the degradation process. The pH range of 5.5–7.5 was favorable for the maintenance of appropriate Fe2+ concentrations due to Fe2+ shortage in alkaline pH and the radical scavenging effect of excessive Fe2+ in acidic pH [56].

3.4. Fe-Speciation Analysis

To reveal the Fe-containing species of mixed powder after reaction, XPS was employed to analyze the Fe species under the optimal condition (Figure 4). Based on the binding energies of peaks, it could be inferred that Fe2O3 and Fe3O4 were the predominant components in mixed powder. The binding energy of Fe 2p1/2 of Fe2O3 was reported to be 724.6 eV [57,58], indicating that Peak A was the spectra of Fe2O3. Peak B located in the binding energy of 718.3 eV, which could be considered as the satellite peak for Fe 2p1/2 [57,58]. Peak C was 713.4 eV, which was believed to be Fe3O4 according to previous studies [58,59]. Based on the binding energy and cover ratio, Peak D could be inferred as Fe3O4, which is consistent with the existing studies [59,60]. In addition, Peaks E and F being located in 711.2 eV and 709.8 eV could be considered as Fe3O4 and Fe2O3, respectively [58,61]. Overall, Fe2O3 and Fe3O4 were the predominant components in mixed powder.
Furthermore, the XRD patterns of the crystalline structure on nZVI surface before and after reactions are demonstrated in Figure 5. Sharp reflection peaks at 44.87° and 65.24° could be indexed as the planes of Fe0 (PDF#65-4899). Thus, the nZVI sample before reactions was of high purity in iron content. Even after reactions, excess Fe0 was observed in the system. In addition to Fe0, the XRD patterns of Fe3O4 (PDF#65-3107) and Fe2O3 (PDF#39-1346) fit well with the crystalline structure after reactions. It is worth mentioning that the planes of Fe3O4 (PDF#65-3107) and Fe2O3 (PDF#39-1346) showed high similarity in major reflection peaks, probably because stoichiometric Fe3O4 could also be expressed to FeO·Fe2O3 with the Fe2+:Fe3+ ratio of 1:2 [57]. The XRD results were in line with those of XPS analysis.
Since the optimal pH was in the range of 5.5–7.5, the precipitation of Fe3+ ions occurred whenever the pH > 4.0 [56] and FeOOH and Fe3O4 may be produced via a series of reactions Equations (12)–(14) [26]. Meanwhile Fe2+(s) in magnetite contributed to persulfate activation by donating electrons [26,62]. Furthermore, FeOOH was believed to react with Fe0 to generate Fe3O4 due to no FeOOH being found in this study. Meanwhile, it has been demonstrated that Fe(OH)3 can produce the mixture of FeOOH and α-Fe2O3 at the range of 40–80 °C (Equation (15)) [63,64]. FeOOH could be converted to Fe2O3 due to poor chemical stability (Equation (16)) [63]. Fe3O4 and Fe2O3 were both reported in previous persulfate activation investigations [65,66], thus, it could be induced that Fe3O4 and Fe2O3 gradually become the persulfate activators. Fe3O4 and Fe2O3 on the surface of nZVI slacken the release of Fe2+ from nZVI, eliminating the scavenging effects of Fe2+ on sulfate radicals. After the treatment, there might be Fe3+ or Fe2+ in the treated effluent. Therefore, alkaline pH is necessary for the treated effluent to remove Fe3+ and Fe2+ by precipitation formation.
Fe3+ + 3OH−→Fe(OH)3(s)
Fe2+ + 2H2O↔FeOOH(s) + 3H+
8FeOOH(s) + Fe0→3Fe3O4(s) + 4H2O
2Fe(OH)3(s)→α − Fe2O3 + 3H2O
2α − FeOOH(s)+→α − Fe2O3 + H2O

3.5. Optimization of Removal Process

Optimization treatment was carried out by numerical technique built in Design Expert 8.0.6 [33]. The optimum values of parameters required to obtain the highest CAP removal were obtained. The goals for the parameters (initial pH, nZVI dosage, temperature, and PS concentration) were set as “in range”, while Y was set as “maximize”. And then the equation (Equation (3)) was employed as a predicting tool to calculate and provide the optimal conditions. The optimum solution was selected based on economic considerations and availability and cost of reagents and energy [36]. Based on these principles, the model provided the optimal variable values of 15 mg/L, 0.5 mmol/L, 7.08, and 70 °C for nZVI dosage, PS, initial pH, and temperature, respectively, with 97.12% of degradation efficiency. Eventually, an extra experiment was performed under the mentioned variables for accuracy confirmation. An excellent decomposition efficiency (average removal of 98.32% with triplicate) was observed, which was in proximity to the predicted efficiency. The main concern of the process is the need for relatively high temperature (70 °C) because of the cost of treating large volumes of wastewater. More real conditions need to be considered in future work to evaluate the operational cost.

4. Conclusions

In this study, Design Expert 8.0 was employed to optimize the operational variables for CAP removal in a “heat + nZVI + PS” system. The combined activated PS degradation of CAP showed a synergistic index of 1.43, indicating an excellent performance of nZVI-heat activation. A 4-factor, 5-level CCD design based on RSM was carried out for the experiments. A quadratic model with high correlation coefficients (R2adj = 0.9823) was established to predict the CAP degradation efficiency. The influences of selected variables (initial pH, PS concentration, nZVI, and temperature) and their interactions were assessed and summarized using ANOVA. Subsequently, the optimized experimental conditions for CAP removal in this study were predicted by the quadratic model of 15 mg/L, 0.5 mmol/L, 7.08, and 70 °C for nZVI dosage, PS, initial pH, and temperature, respectively, for 97.12% of CAP removal. Under the optimum conditions, average removal of 98.32% with triplicate was achieved, which was in proximity to the predicted efficiency. In addition, Fe-speciation analysis was conducted to reveal the actual composition of mixed powders of Fe2O3 and Fe3O4 after reactions, which could also act as the activators along with the reaction. Overall, it could be concluded that the nZVI-heat activation of PS was an efficient technique for CAP degradation.

Author Contributions

Writing—original draft, L.Y.; investigation, H.L.; writing—review and editing, resources, J.X.; investigation, L.H.; data curation, Y.M.; supervision, L.W.; writing—review and editing, project administration, Z.Z. All authors have read and agreed to the published version of the manuscript.

Funding

This work was financially supported by the Changjiang River Scientific Research Institute (CRSRI) Open Research Program (Program SN: CKWV2019771/KY), National Natural Science Foundation of China (No. 51878523, No. U1703120, and No. 51508430), the Recruitment Program of Global Experts (Young Professionals), the Fundamental Research Funds for the Central Universities (WUT:193108003, 2019IVA032) and the Scottish Government′s Rural and Environment Science and Analytical Service Division (RESAS).

Conflicts of Interest

The authors declare no conflict of interest.

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Water 12 00131 g001 550
Figure 1. Degradation efficiencies of CAP under different processes. Experimental conditions: initial CAP concentration C0 = 1 mg/L, pH = 7.0, nZVI 20 mg/L, temperature 60 °C, PS concentration = 0.4 mM, and the solution volume 100 mL.
Figure 1. Degradation efficiencies of CAP under different processes. Experimental conditions: initial CAP concentration C0 = 1 mg/L, pH = 7.0, nZVI 20 mg/L, temperature 60 °C, PS concentration = 0.4 mM, and the solution volume 100 mL.
Water 12 00131 g001
Water 12 00131 g002 550
Figure 2. (a) Normal plot of the internally studentized residuals and (b) actual values versus predicted data for CAP removal.
Figure 2. (a) Normal plot of the internally studentized residuals and (b) actual values versus predicted data for CAP removal.
Water 12 00131 g002
Water 12 00131 g003 550
Figure 3. The 3D response surface and 2D contour plots of the effects of the interaction on the CAP degradation efficiency (%). (a) 3D graph of temperature and nZVI, (b) 2D graph of temperature and nZVI, (c) 3D graph of temperature and initial pH, and (d) 2D graph of temperature and nZVI.
Figure 3. The 3D response surface and 2D contour plots of the effects of the interaction on the CAP degradation efficiency (%). (a) 3D graph of temperature and nZVI, (b) 2D graph of temperature and nZVI, (c) 3D graph of temperature and initial pH, and (d) 2D graph of temperature and nZVI.
Water 12 00131 g003
Water 12 00131 g004 550
Figure 4. The X-ray photoelectron spectroscopy (XPS) spectrum of nZVI surface after reactions.
Figure 4. The X-ray photoelectron spectroscopy (XPS) spectrum of nZVI surface after reactions.
Water 12 00131 g004
Water 12 00131 g005 550
Figure 5. X-ray diffraction (XRD) spectra of solid powders before and after reactions.
Figure 5. X-ray diffraction (XRD) spectra of solid powders before and after reactions.
Water 12 00131 g005
Table
Table 1. Physicochemical properties of chloramphenicol (CAP) [6].
Table 1. Physicochemical properties of chloramphenicol (CAP) [6].
ParameterCharacter
FormulaC11H12Cl2N2O5
Molecular weight323.13
Solubility (mg/L), 25 °C2500
Log Kow1.14
pKa9.5
CAS number56-75-7
Molecular structure Water 12 00131 i001
Table
Table 2. Experimental arrangements based on central composite design (CCD).
Table 2. Experimental arrangements based on central composite design (CCD).
FactorsSymbolsLevel of Factors
−2−1012
Nanoscale zero-valent iron (nZVI) (mg/L)X11015202530
Peroxydisulfate (PS) concentration (mM)X20.20.30.40.50.6
Initial pHX3357911
Temperature (°C)X44050607080
Table
Table 3. The 4-factor CCD matrix and the actual values for CAP removal.
Table 3. The 4-factor CCD matrix and the actual values for CAP removal.
Run NumberFactorsDegradation Efficiency (%)
X1X2X3X4ObservedPredicted
1250.555080.7281.82
2200.478093.0795.84
3200.436090.6288.90
4200.676084.7682.45
5150.355060.9362.96
6150.395017.4218.36
7150.597094.9594.64
8150.595024.4527.15
9250.557096.2595.02
10250.597093.5490.88
11200.4116037.5240.16
12250.397080.1179.40
13100.476082.8378.58
14150.397086.6284.89
15200.476076.4275.47
16150.357086.7686.53
17200.474017.9716.12
18200.476074.8075.47
19200.476075.6175.47
20250.357089.0385.70
21200.476075.7075.47
22200.276061.1264.35
23300.476080.1685.33
24150.555069.1669.58
25250.355073.4673.48
26250.395028.5924.22
27200.476075.5175.47
28250.595034.7934.73
29200.476074.7775.47
30150.557090.3894.12
Table
Table 4. Significant terms from regression analysis of the proposed model.
Table 4. Significant terms from regression analysis of the proposed model.
TermCoefficient EstimateStandard Errorp-Value
Intercept75.471.31<0.0001
X11.690.650.0208
X24.530.65<0.0001
X3−12.180.65<0.0001
X419.930.65<0.0001
X1X4−2.840.800.0029
X3X410.740.80<0.0001
X121.620.610.0181
X32−2.730.610.0004
X42−4.870.61<0.0001
Table
Table 5. Details of the proposed model for the CAP removal.
Table 5. Details of the proposed model for the CAP removal.
TermSquaresdfSquareValueProbability > F
Model16,615.92141186.85115.86<0.0001
X168.28168.286.660.0208
X2491.411491.4147.97<0.0001
X33562.8913562.89347.80<0.0001
X49532.9219532.92930.57<0.0001
X1X22.9812.980.290.5978
X1X321.72121.722.120.1660
X1X4128.711128.7112.560.0029
X2X34.6914.690.460.5091
X2X40.9410.940.0920.7660
X3X41845.1311845.13180.11<0.0001
X1272.15172.157.040.0181
X227.3317.330.720.4110
X32205.081205.0820.020.0004
X42651.021651.0263.55<0.0001
Residual153.661510.24
Lack of Fit151.751015.1739.610.0004
Pure Error1.9250.38
Corrected Total16,769.5829
R20.9908
Adjusted R20.9823
Adequate Precision35.224
C.V.%4.55

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Yang, L.; Li, H.; Xue, J.; He, L.; Ma, Y.; Wu, L.; Zhang, Z. Hydrothermal Enhanced Nanoscale Zero-Valent Iron Activated Peroxydisulfate Oxidation of Chloramphenicol in Aqueous Solutions: Fe-Speciation Analysis and Modeling Optimization. Water 2020, 12, 131. https://doi.org/10.3390/w12010131

AMA Style

Yang L, Li H, Xue J, He L, Ma Y, Wu L, Zhang Z. Hydrothermal Enhanced Nanoscale Zero-Valent Iron Activated Peroxydisulfate Oxidation of Chloramphenicol in Aqueous Solutions: Fe-Speciation Analysis and Modeling Optimization. Water. 2020; 12(1):131. https://doi.org/10.3390/w12010131

Chicago/Turabian Style

Yang, Lie, Hong Li, Jianming Xue, Liuyang He, Yongfei Ma, Li Wu, and Zulin Zhang. 2020. "Hydrothermal Enhanced Nanoscale Zero-Valent Iron Activated Peroxydisulfate Oxidation of Chloramphenicol in Aqueous Solutions: Fe-Speciation Analysis and Modeling Optimization" Water 12, no. 1: 131. https://doi.org/10.3390/w12010131

APA Style

Yang, L., Li, H., Xue, J., He, L., Ma, Y., Wu, L., & Zhang, Z. (2020). Hydrothermal Enhanced Nanoscale Zero-Valent Iron Activated Peroxydisulfate Oxidation of Chloramphenicol in Aqueous Solutions: Fe-Speciation Analysis and Modeling Optimization. Water, 12(1), 131. https://doi.org/10.3390/w12010131

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