Design and Synthesis of a Biochar-Supported Nano Manganese Dioxide Composite for Antibiotics Removal From Aqueous Solution

Introduction

Antibiotics are widely used for preventing bacterial infections in humans and animals (Luo et al., 2011; Hong et al., 2013). Since the discovery of antibiotics, their global production and use have been increasing rapidly, causing some concern (Kasprzyk-Hordern et al., 2009). Antibiotics have different half-lives in the environment, and some of them have high persistence; therefore, they have been polluting the environment at an alarming rate (Petrie et al., 2015; Carvalho and Santos, 2016). Residues have been frequently detected in surface water and groundwater worldwide (Homem and Santos, 2011; Yu et al., 2016). Notably, long-term exposure to antibiotic residues at relatively low concentrations can induce antibiotic resistance genes (Ahmed et al., 2015; Huang et al., 2015; Hou et al., 2016; Sharma et al., 2016). Due to the exposure to sublethal concentrations of antibiotic residues, drug-resistant strains of pathogens have become the dominant strains, which have rapidly developed and inherited antibiotic resistance genes. Therefore, antibiotics are ineffective against the pathogens with the corresponding antibiotic resistance genes, rendering their infections in humans difficult to cure (Drury et al., 2013; Frieri et al., 2017; Medernach and Logan, 2018). The World Health Organization studied the exact size of the world’s bacterial resistance status in 2014 and reported that the resistance of common bacteria to antibiotics has reached alarming levels, and in several countries, the main groups of antibiotics have failed to benefit half of the patients (Organization, 2014). In addition, antibiotics may adversely affect human health by interfering with endocrines (Huang et al., 2018). Therefore, aqueous solution containing antibiotics must be effectively treated before being discharged into the environment. Tetracyclines have become one of the most consumed antibiotics in the world at low prices and broad-spectrum antibacterial properties (Zhang et al., 2018). The tetracycline residue in original wastewater of pharmaceutical factories was reported in extremely high levels (844–1077 mg⋅L^–1), while that in treated wastewater still ranged from several to dozens of mg⋅L^–1 (Li et al., 2008; Zhang et al., 2018). Therefore, two typical tetracyclines, namely tetracycline hydrochloride (TC) and doxycycline (DC), were selected as target pollutants.

The main methods of removing antibiotics from water are biodegradation (Zhang et al., 2017), hydrolysis (Sarmah et al., 2006), photodegradation (Lu et al., 2018), and adsorption (Zeng et al., 2018; Liu et al., 2019). Among them, the adsorption method, which is the most efficient, economical, and environmentally friendly, has been widely used in the treatment of aqueous solution containing antibiotics. Finding an effective adsorbent is the key to expanding the application of this technology to antibiotic aqueous solution treatment. Biochar seems to be a promising adsorption material in pollutant treatment technologies, owing to its porous structure, complex surface, abundance of raw material, and economic benefits (Tan et al., 2015, 2016b; Liang et al., 2017; Zhang et al., 2019b). However, there is room to further improve the adsorption capacity of original biochar (Cai et al., 2018, 2019; Zhang et al., 2019a).

Nanoparticles of manganese oxide have been widely reported as an effective adsorbent (Song et al., 2014). Nano-scale MnO_x particles have a high specific surface area owing to their superior polycrystalline structure, as well as high adsorption performance (Wang et al., 2010; Xiao et al., 2010). However, nano-sized MnO_x particles easily agglomerate, thus limiting their practical application as adsorbents (Tyson et al., 2011; Li et al., 2017). In this study, a simple, low-cost method of loading MnO_x nanoparticles onto biochar was developed for preparing a new biochar composite that can be used to adsorb antibiotics in aqueous solution. This method not only solves the agglomeration problem, but also improves the effectiveness of the nano-metal oxide MnO_x in aiding biochar for better pollutant removal.

The main objectives of this study included: (1) Preparation of a biochar-supported manganese dioxide composite; (2) Characterization of the prepared composite using scanning electron microscopy (SEM), Fourier transform infrared spectroscopy (FTIR), X-ray diffraction (XRD), and X-ray photoelectron spectroscopy (XPS); (3) Removal of TC and DC using the prepared composite under different experimental conditions; (4) Evaluation of the isotherms and kinetic laws of the adsorption process.

Materials and Methods

Material Preparation

Preparation of Biochar

Rice husk, which is a common agricultural waste, was used as the biomass raw material in the preparation of biochar. The rice husk collected from the farm was rinsed with ultrapure water and air dried. Subsequently, it was completely dried in an oven at 60°C and grounded to a powder form. The rice husk powder was placed in a quartz boat and then heated in a quartz tube furnace (SK-1200°C, Tianjin Zhonghuan Experimental Furnace Co., Ltd., Tianjin, China). Both ends of the quartz tube were sealed, and the hose was connected. N₂ was passed through the furnace chamber at a flow rate of 400 mL⋅min^–1 from one end, and an inert atmosphere was maintained during the pyrolysis process. The volatile products generated during the pyrolysis of biomass were collected from the other end. The temperature was programmed to increase to 500°C at a rate of 7°C min^–1 and was maintained at the peak temperature for 2 h, which was the optimal preparation condition in preliminary study (Wu et al., 2016). Finally, the chamber was cooled to room temperature (25 ± 1°C) to obtain rice husk biochar.

Synthesis of Biochar-Supported Nano Manganese Dioxide Composite

A 4 mmol⋅L^–1 manganese chloride solution was prepared and then purified under N₂ (100 mL⋅min^–1) for 20 min to remove dissolved oxygen. One gram of the above-mentioned chaff biochar was added to 30 mL of a manganese chloride solution and stirred under N₂ atmosphere (100 mL⋅min^–1) for 1 h to form a biochar–Mn²⁺ mixture. This mixture was added dropwise to 20 mL of a solution containing potassium permanganate and sodium hydroxide while stirring at 250 r⋅min^–1 using a magnetic stirrer. The stirring was continued for 20 min to ensure a complete reaction. After aging for 24 h at room temperature (25 ± 1°C), the mixture was washed several times with ultrapure water until the pH was neutral. Finally, it was completely dried in an oven at 80°C. After grinding, it was made to pass through a 100-mesh sieve to obtain a biochar-supported nano manganese dioxide composite (BC/MnO₂).

Characterization Methods

The microstructure and morphology of the composites were studied using a QUANTA 250 FE-SEM (FEI, United States). XRD patterns were acquired using a Bruker D8-Advance X-ray diffractometer (Bruker, Germany). The surface elements were determined using an ESCALAB 250Xi X-ray photoelectron spectrometer (Thermo Fisher Scientific, United States). A Fourier transform infrared spectrometer was used (NICOLET 5700; Thermo Nicolet Corporation, United States). The thermogravimetric (TG) curve of the material was measured in N₂ atmosphere by varying the temperature from room temperature (25 ± 1°C) to 1000°C (flux rate: 100 mL⋅min^–1; heating rate: 10°C⋅min^–1) using an SDT Q600 thermal analyzer (TA, United States). The Brunner–Emmet–Teller (BET) specific surface area of the material was measured using a Micromeritics 3Flex analyzer (Micromeritics Instrument Corporation, United States).

Adsorption Experiments

Effect of Adsorbent Dose on Adsorption

Various amounts of BC/MnO₂ (10, 20, 40, 80, 100, and 150 mg) were added to 25 mL of 5 mg⋅L^–1 TC and DC solutions (pH = 6.0). The resulting mixture was sealed using a plastic wrap and rotated in a constant-temperature shaker at a speed of 170 r⋅min^–1. The reaction temperature was set to 25°C, and the mixture was shaken for 24 h. Finally, a sample was taken for measurement.

Effect of pH on Adsorption

TC and DC solutions (both the concentrations were 5 mg⋅L^–1) with a pH value ranging from 2.0 to 10.0 were prepared. Subsequently, 0.1 g of BC/MnO₂ was added to 25 mL of the above solution. The mixture was sealed using a plastic wrap and rotated in the constant-temperature shaker at a speed of 170 r⋅min^–1. The reaction temperature was set to 25°C, and the mixture was shaken for 24 h. Finally, a sample was taken for measurement.

Effect of Initial Antibiotics Concentration and Adsorption Temperature

TC and DC solutions were prepared at a concentration ranging from 5 to 100 mg⋅L^–1 (pH = 6.0). At reaction temperatures of 25, 35, and 45°C, 0.1 g of BC/MnO₂ was taken and added to 25 mL of the above solutions. The mixture was then sealed using a plastic wrap and rotated in the constant-temperature shaker at a speed of 170 r⋅min^–1. The mixture was shaken for 24 h and sampled for measurement.

Effect of Reaction Time on Adsorption

The kinetic test interval was from 0 to 1440 min. BC/MnO₂ (0.1 g) was added to 25 mL of TC and DC solutions with a concentration of 50 mg⋅L^–1, with pH = 6.0. The mixture was sealed using a plastic wrap, and the reaction temperature was set to 25°C. It was then shaken in the constant temperature shaker at a speed of 170 r⋅min^–1. Samples were taken for measurement at the corresponding time.

Detection Method

The residual antibiotics concentration in the solution was determined by UV spectrophotometry (Ma et al., 2018). The solutions were separated and filtered, and the residual concentration of TC and DC in the liquid was detected by UV spectrophotometer (UV-2550, Shimadzu, Japan) at 357 nm (Jing et al., 2014) and 346 nm (Xiong et al., 2019), respectively.

Results and Discussion

Characterization

Table 1 lists the physical and chemical characteristics of BC/MnO₂. The elemental analysis shows that compared with the original biochar, manganese appears on the surface of BC/MnO₂ owing to the introduction of MnO₂, and the carbon content of the biochar is decreased, whereas the oxygen content is increased. Compared with the original biochar (0.006 cm³⋅g^–1), BC/MnO₂ (0.24 cm³⋅g^–1) has a significantly larger total pore volume. In addition, the specific surface area of the biochar is increased from 6.67 to 64.32 m²⋅g^–1, indicating an improvement in its pore structure.

TABLE 1

Table 1. Characteristics of BC/MnO₂.

The N₂ adsorption–desorption isotherm and pore size distribution of BC/MnO₂ were measured at 77.3 K. Figure 1 shows the results. According to the IUPAC classification, the shape of the isotherm is IV, indicating that BC/MnO₂ has a flat slit, wedge structure (Saiah et al., 2009). The pore size distribution of BC/MnO₂ is mainly in the range of 0–50 nm, and the average pore size is 13.10 nm. The increased specific surface area and total pore volume were beneficial for improving the adsorption performance of BC/MnO₂.

FIGURE 1

Figure 1. (A) Nitrogen adsorption–desorption isotherms, and (B) pore size distribution of BC/MnO₂.

Figure 2 shows the SEM morphologies of BC/MnO₂. BC/MnO₂ exhibits an irregular surface with micropores of different shapes and sizes, and a large number of particles are uniformly precipitated on the surface of biochar, indicating the successful coating of the MnO₂ nanoparticles on the biochar surface. The TEM image (Figure 3) shows that MnO₂ is successfully loaded on the biochar and that MnO₂ nano-flakes are embedded in the biochar matrix.

FIGURE 2

Figure 2. SEM images of BC/MnO₂ under different magnification: (a,b) 10000×, (c,d) 40000×, and (e,f) 160000×.

FIGURE 3

Figure 3. TEM images of BC/MnO₂ under different magnification: (a) 0.2 μm, (b) 100 nm, (c) 50 nm, and (d) 20 nm.

Figure 4A shows the XRD pattern of BC/MnO₂. The characteristic peak of BC/MnO₂ at 2θ = 30.082° indicates the presence of MnO₂ on the biochar surface. Figure 4B shows the TG analysis results. The weight loss of approximately 10% in the temperature range of 30–120°C is mainly due to the dehydration process (Shete et al., 2015). When the temperature gradually increases from 120 to 500°C, the weight loss of the biochar decreases by only approximately 20%. The weight loss at 800°C is approximately 30%. This shows that BC/MnO₂ has higher thermal stability than the original biochar.

FIGURE 4

Figure 4. (A) XRD spectrum of BC/MnO₂, (B) TG curves of BC/MnO₂.

The chemical composition of the BC/MnO₂ surface was further studied by conducting an XPS analysis (Figure 5). The characteristic Mn2p peak (Figure 5A) can be divided into three peaks by Gaussian fitting. The peak position of Mn⁴⁺ can be observed at 644.04 eV (Yin et al., 2015). The peaks at 642.05 and 653.78 eV belong to Mn2p_3/2 and Mn2p_1/2, respectively, with an energy interval of 11.73 eV, which is consistent with the results reported for MnO₂ (Xie et al., 2017; Li et al., 2018). The characteristic peaks of the XPS spectrum of O1s (Figure 5B) are 533.20, 531.55, 530.54, and 529.56 eV, indicating the presence of C-O, C = O, O-H, and Mn–O, respectively (Yu et al., 2007; Han et al., 2013; Zhang et al., 2014; Bose and Biju, 2015). These functional groups can serve as binding sites for the adsorption of antibiotics. The above results once again demonstrate the successful loading of the MnO₂ nanoparticles on the surface of biochar.

FIGURE 5

Figure 5. XPS spectra of BC/MnO₂: (A) Mn2p and (B) O1s.

Comparison of the Performance of Pristine Biochar and BC/MnO₂

The adsorption ability of pristine biochar and BC/MnO₂ for TC and DC were compared at initial antibiotic concentrations range from 5 to 100 mg⋅L^–1. As can be seen from Figure 6, after the coating of MnO₂, the adsorption ability of BC/MnO₂ for both TC and DC were significantly higher than that of pristine biochar. These results suggested that the loading of MnO₂ was an effective way to improve the adsorption ability of biochar for TC and DC. The increased specific surface area and total pore volume, and the loading of MnO₂ served as bonding sites might be account for the enhanced adsorption performance of BC/MnO₂.

FIGURE 6

Figure 6. The adsorption ability of biochar and BC/MnO₂ for TC and DC.

Effect of Adsorbent Dose

Figure 7 shows the effect of BC/MnO₂ dose on the adsorption of TC and DC. With the increase in the BC/MnO₂ dose, the relative adsorption amounts of TC and DC gradually decrease. This is mainly because an excessive dose leads to excess adsorption sites and reduces the adsorbent utilization rate (Wu et al., 2014). With the increase in the adsorbent dose, the removal rates of TC and DC increase, mainly because of the increase in the number of adsorption sites. However, there was no significant difference between the adsorption ability of BC/MnO₂ for TC and DC, with slightly higher performance for DC. Similar results could be found in the later adsorption experiments.

FIGURE 7

Figure 7. Effect of adsorbent (BC/MnO₂) dose on adsorption efficiency: (A) tetracycline hydrochloride, (B) doxycycline.

As can be seen from Figure 7, when the dose of BC/MnO₂ is 0.1 g, the effect of the composite material on antibiotic contaminants is very obvious, in which the removal rate of doxycycline reaches 90%, and the removal rate of tetracycline hydrochloride is nearly 95%. This is conducive to the comparative observation of experimental effects. Therefore, according to the concentration of antibiotic contaminants and the results of preliminary experiments, we chose 0.1 g as the dose of adsorbent in other parts of the experiment.

Effect of pH

Figure 8 shows the effect of initial pH on the adsorption of TC and DC by BC/MnO₂. According to the result obtained by Figure 8B, the zero-potential point of BC/MnO₂ is around 3.2. At low pH, TC and DC mainly exist in cationic form, and the surface of the biochar composite is positively charged (Figure 8B). Therefore, under this condition, electrostatic repulsion may occur between them. Similarly, at high pH, anionic antibiotics are repelled by the negatively charged biochar surface (Figure 8B), inhibiting TC and DC adsorption (Wang et al., 2016). However, the removal rate did not change significantly across the tested pH range, suggesting that the electrostatic interactions were not the main mechanism whereby biochar composites adsorb TC and DC. Other forces may have formed between the antibiotics and the carboxyl or hydroxyl groups on the surface of the new biochar composite, including π-π interaction and hydrogen bonding (Zheng et al., 2013; Zeng et al., 2019; Ye et al., 2020). In addition, part of TC and DC could be adsorbed by MnO₂ particles on biochar surface (Mahamallik et al., 2015). Overall, the effect of pH on the adsorption of TC and DC by the new biochar composite is not significant.

FIGURE 8

Figure 8. (A) Effect of solution pH on the adsorption of TC and DC by BC/MnO₂; (B) the zeta potential of BC/MnO₂ at different pH.

Adsorption Isotherms

The Langmuir, Freundlich and Temkin models were used to study the adsorption equilibrium isotherms and fit the experimental data. The adsorption models are expressed as follows (Zhang et al., 2019a):

$$\frac{C_{\text{e}}}{q_{\text{e}}}=\frac{C_{\text{e}}}{q_{\max }}+\frac{1}{q_{\max }{K}_{\text{L}}}(1)$$

Here, q_e is the adsorption amount (mg⋅g^–1); C_e is the concentration at the end of the adsorption reaction (mg⋅L^–1); q_max is the maximum adsorption amount (mg⋅g^–1); and K_L is the Langmuir constant related to adsorption (L⋅mg^–1), which is used to indicate whether the adsorption equilibrium is favorable (0 < K_L < 1) or unfavorable (K_L > 1).

$$\ln q_{\text{e}}=\ln K_{\text{F}}+\frac{1}{n}\ln C_{\text{e}}(2)$$

Here, q_e is the adsorption amount (mg⋅g^–1); C_e is the concentration at the end of the adsorption reaction (mg⋅L^–1); K_F is the Freundlich constant (L⋅mg^–1) representing the adsorption capacity; and n is the Freundlich constant representing the adsorption strength.

$$q_{\text{e}}=B_{\text{T}}\ln K_{\text{T}}+B_{\text{T}}\ln C_{\text{e}}(3)$$

Here, q_e is the adsorption amount (mg⋅g^–1), C_e is the concentration at the end of the adsorption reaction (mg⋅L^–1). B_T = RT/b_T and b_T (J⋅mol^–1) is the Temkin constant, R is the universal gas constant (8.314 J⋅mol^–1⋅K^–1) and T is the temperature (K); K_T (L⋅mg^–1) is the maximum binding energy constant.

In the Langmuir model, it is assumed that a single molecular layer is formed when adsorption occurs and that the adsorbed molecules do not interact. Figure 9 shows the relationship between C_e/q_e and C_e. Table 2 lists the values of the related parameters. Temkin isotherm is based on an assumption that the indirect interactions are existed between adsorbate molecules, and the heat of adsorption of molecules will decrease linearly with surface coverage (Zhang et al., 2019a).

FIGURE 9

Figure 9. Equilibrium isotherms for tetracycline hydrochloride and doxycycline adsorbed by BC/MnO₂ at different temperatures: (A) Langmuir model for TC; (B) Freundlich model for TC; (C) Temkin model for TC; (D) Langmuir model for DC; (E) Freundlich model for DC; and (F) Temkin model for DC.

TABLE 2

Table 2. Model parameters and the corresponding correlation coefficients of isotherm models.

At the three temperatures studied, the adsorption data show a poor correlation with the Langmuir and Temkin model, whereas they show a strong correlation with the Freundlich model, indicating that the adsorption of TC and DC by BC/MnO₂ better conforms to the Freundlich adsorption model (Wu et al., 2014). The Freundlich adsorption model is an empirical equation where it is assumed that adsorption occurs on a heterogeneous surface and that the adsorption capacity is related to the equilibrium concentration (Cui et al., 2015). In Table 2, the values of 1/n are less than 1, indicating that TC and DC easily get adsorbed by BC/MnO₂ at these temperatures.

Thermodynamic analysis was further applied to study thee adsorption process and mechanisms. The Gibbs free energy ΔG°, enthalpy ΔH°, entropy ΔS° were calculated using the following equations (Tan et al., 2016a):

$$\mathrm{\Delta }{G}^0=-RT{K}^0(4)$$

$$\ln k^0=-\frac{\mathrm{\Delta }{H}^0}{RT}+\frac{\mathrm{\Delta }{S}^0}{R}(5)$$

Here, R is the gas constant 8.314 J⋅mol^–1⋅K^–1, T (K) is the adsorption temperature; K⁰ could be calculated by plotting ln(q_e/c_e) versus c_e and extrapolating c_e to zero.

The calculated thermodynamic data of ΔG°, ΔH°, and ΔS° are given in Table 3. The negative value of ΔG° at three temperatures indicated the feasibility and spontaneous reaction of TC and DC adsorption onto BC/MnO₂. In addition, the ΔG° values of TC and DC decreased from −2.80 to −4.25 kJ⋅mol^–1 and from −3.33 to −4.25 kJ⋅mol^–1 with the increase of temperature, respectively, indicating that higher temperature was more favorable for adsorption. The positive ΔH° value indicated the endothermic property of the adsorption process. The positive value of ΔS° might be due to the increase of randomness of solid and solution interface in the process of adsorption (Tan et al., 2016a).

TABLE 3

Table 3. Thermodynamic parameters for TC and DC adsorption by BC/MnO₂.

Adsorption Kinetics

To determine the adsorption equilibrium time of BC/MnO₂ for TC and DC and to study the kinetics of the adsorption process, the effect of time on the adsorption of TC and DC by BC/MnO₂ was analyzed. Two conventional kinetic models were used to analyze the results: a pseudo-first-order kinetic model and a pseudo-second-order kinetic model. Intra-particle diffusion model was further applied to determine the diffusion mechanisms and the rate controlling procedures.

The pseudo-first-level model is expressed as:

$$\ln (q_{\text{e}}-q_{\text{t}})=\ln q_{\text{e}}-k_{1}t(6)$$

The pseudo-secondary model is expressed as:

$$\frac{t}{q_{\text{t}}}=\frac{1}{k_2{q}_{\text{e}}^2}+\frac{t}{q_{\text{e}}}(7)$$

Here, q_e is the removal amount at equilibrium (mg⋅g^–1); q_t is the removal amount at a given time t (mg⋅g^–1); k₁ is the adsorption rate constant of the pseudo-first-order model (min^–1); and k₂ is the adsorption rate constant of the pseudo-second-order model (g⋅mg^–1⋅min^–1).

The intra-particle diffusion model is expressed as Zeng et al. (2018):

$$q_{\text{t}}=k_{\text{id}}{\text{t}}^{1/2}+c_{\text{i}}(8)$$

Here, q_t (mg⋅g^–1) is the removal amount at time t, k_id is the intra-particle diffusion rate constant (mg⋅g^–1⋅min^–1/2), and c_i is the intercept related to the thickness of the boundary layer.

Figure 10 shows the results of the adsorption kinetics study. Table 4 lists the parameter values. The adsorption process reached equilibrium after 420 min. Compared with the pseudo-first-order kinetic model, the adsorption data better fit the pseudo-second-order kinetic model (R² = 0.999) (Turki et al., 2015). The pseudo-second-order kinetic model fitting results indicate that the process controlling the adsorption of TC and DC may be chemisorption (Tan et al., 2015). As shown in Figure 10 and Table 5, three linear portions were existed in the plots of q_t against t^1/2, suggesting that multiple steps including intra-particle diffusion and film diffusion were involved in the adsorption process.

FIGURE 10

Figure 10. Kinetics of the adsorption process of TC and DC by BC/MnO₂: (A) Change in TC adsorption amount with time; (B) Change in DC adsorption amount with time; (C) TC adsorption modeled using the pseudo-first-order equation; (D) DC adsorption modeled using the pseudo-first-order equation; (E) TC adsorption modeled using the pseudo-second-order equation; (F) DC adsorption modeled using the pseudo-second-order equation; (G) TC adsorption modeled using Intraparticle diffusion equation; and (H) DC adsorption modeled using Intraparticle diffusion equation.

TABLE 4

Table 4. Model parameters and corresponding correlation coefficients of kinetics models.

TABLE 5

Table 5. Intra-particle diffusion parameters for the adsorption of TC and DC by BC/MnO₂.

Regeneration of BC/MnO₂

To investigate the regeneration ability of BC/MnO₂, several cycles of adsorption-desorption experiments were performed. The TC and DC loaded BC/MnO₂ was desorbed using ethanol. The adsorption performance of TC and DC by BC/MnO₂ after different adsorption cycles are shown in Figure 11. The results indicated that the adsorption capacity of BC/MnO₂ decreased gradually with the increase of cycles. After five adsorption/desorption cycles, the adsorption amount of TC and DC onto the regenerated BC/MnO₂ still remained higher than the pristine biochar, indicating that BC/MnO₂ could be regenerated.

FIGURE 11

Figure 11. The adsorption performance of TC and DC by BC/MnO₂ after different adsorption cycles.

Conclusion

In this study, a biochar-supported nano manganese dioxide composite was prepared by loading manganese dioxide nanoparticles on biochar, with rice husk as the raw material. Compared with the original biochar, MnO₂ nanoparticles appeared on the surface of BC/MnO₂, the carbon content decreased, and the oxygen content increased. BC/MnO₂ exhibited significantly larger total pore volume and specific surface area, and the pore structure of the biochar was improved. The comparative study about the adsorption ability of pristine biochar and BC/MnO₂ suggested that the loading of MnO₂ was an effective way to improve the adsorption ability of biochar for TC and DC. The effects of pH on the adsorption of TC and DC by BC/MnO₂ were found to be insignificant. With an increase in the adsorbent dose, the removal rates of TC and DC increased, and the removal ability of BC/MnO₂ for TC was slightly higher than that for DC. Therefore, BC/MnO₂ may be an efficient material for TC and DC removal from aqueous solution. Further research about its efficiency for other antibiotics removal and deeper mechanisms should be studied.

Data Availability Statement

The datasets generated for this study are available on request to the corresponding author.

Author Contributions

JL and XC contributed conception and design of the study. YL and YG organized the database. HW, ShaL, SimL, YY, and SijL performed the statistical analysis. All authors contributed to manuscript revision, read and approved the submitted version.

Funding

This study was financially supported by the National Natural Science Foundation of China (Grant No. 51909283) and the Natural Science Foundation of Hunan Province, China (Grant No. 2018JJ3096).

Conflict of Interest

The authors declare that the research was conducted in the absence of any commercial or financial relationships that could be construed as a potential conflict of interest.

Abbreviations

BC/MnO2, Biochar-supported manganese dioxide composite; BET, Brunner–Emmet–Teller; DC, Doxycycline; FTIR, Fourier transform infrared spectroscopy; SEM, Scanning electron microscopy; TC, Tetracycline hydrochloride; TG, Thermogravimetric; XPS, X-ray photoelectron spectroscopy.

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