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Article

Preparation of Biochar with Developed Mesoporous Structure from Poplar Leaf Activated by KHCO3 and Its Efficient Adsorption of Oxytetracycline Hydrochloride

by
Zhenhua Wei
,
Chao Hou
,
Zhishuo Gao
,
Luolin Wang
,
Chuansheng Yang
,
Yudong Li
,
Kun Liu
* and
Yongbin Sun
*
Institute of Optical Functional Materials for Biomedical Imaging, School of Chemistry and Pharmaceutical Engineering, Shandong First Medical University & Shandong Academy of Medical Sciences, Taian 271016, China
*
Authors to whom correspondence should be addressed.
Molecules 2023, 28(7), 3188; https://doi.org/10.3390/molecules28073188
Submission received: 16 March 2023 / Revised: 1 April 2023 / Accepted: 1 April 2023 / Published: 3 April 2023
(This article belongs to the Special Issue Chemical Functionalization of Two-Dimensional Materials)
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Abstract

:
The effective removal of oxytetracycline hydrochloride (OTC) from the water environment is of great importance. Adsorption as a simple, stable, and cost-effective technology is regarded as an important method for removing OTC. Herein, a low-cost biochar with a developed mesoporous structure was synthesized via pyrolysis of poplar leaf with potassium bicarbonate (KHCO3) as the activator. KHCO3 can endow biochar with abundant mesopores, but excessive KHCO3 cannot continuously promote the formation of mesoporous structures. In comparison with all of the prepared biochars, PKC-4 (biochar with a poplar leaf to KHCO3 mass ratio of 5:4) shows the highest adsorption performance for OTC as it has the largest surface area and richest mesoporous structure. The pseudo-second-order kinetic model and the Freundlich equilibrium model are more consistent with the experimental data, which implies that the adsorption process is multi-mechanism and multi-layered. In addition, the maximum adsorption capacities of biochar are slightly affected by pH changes, different metal ions, and different water matrices. Moreover, the biochar can be regenerated by pyrolysis, and its adsorption capacity only decreases by approximately 6% after four cycles. The adsorption of biochar for OTC is mainly controlled by pore filling, though electrostatic interactions, hydrogen bonding, and π-π interaction are also involved. This study realizes biomass waste recycling and highlights the potential of poplar leaf-based biochar for the adsorption of antibiotics.

Graphical Abstract

1. Introduction

Oxytetracycline hydrochloride (OTC) is an effective broad-spectrum antibacterial agent, which plays an important role in animal husbandry and disease therapy [1]. However, approximately 70% of OTC is dispersed into the natural environment as feces and urine are excreted [2]. It has been demonstrated that the chronic exposure of zebrafish to OTC at a concentration of 0.42 g·L−1 will reduce its nonspecific immune response [3], and concentrations of 4 g·L−1 OTC can cause genotoxic damage to zebrafish [4]. The extensive use of OTC brings convenience to human life; however, its residues in the water environment lead to microbial death and antibiotic resistance gene transmission, which induce a threat to ecological and public health safety [5]. Moreover, OTC may cause endocrine disorders, cancer, and other diseases through the accumulation of food chain, which could seriously affect human health [6]. Therefore, it is of great importance to develop effective technologies to remove OTC from the water environment.
Presently, there are various technologies to remove antibiotics from the water environment [7], including biodegradation [8], chemical oxidation [9], membrane separation [10], photocatalytic degradation [11], adsorption [12], etc. Among these, the adsorption technology is simple, efficient, stable, and relatively economic [13]. More importantly, the adsorption process does not introduce secondary pollutants, and is considered to be one of the most effective methods for removing antibiotics in water [14,15]. Adsorbents are the key to adsorption technology [16,17,18,19,20]. In the past decades, researchers have developed a variety of adsorbents, including metal oxides [21], molecular sieves [22], MOFs [23], carbon nanotubes [24], MXenes [25], etc. Recently, biochar has been widely used to remove antibiotics from the environment due to its porous structure and low cost [26,27,28]. However, biochar obtained from the direct pyrolysis of biomass usually has a low specific surface area, undeveloped pore structure, and few adsorption sites, resulting in its poor adsorption performance [29,30]. In order to optimize the adsorption performance of biochar, activating agents are usually added during the synthesizing process. The most commonly used activators, such as KOH [31], H3PO4 [32], ZnCl2 [33], and FeCl3 [34], can effectively create pores in biochar, but they are strongly corrosive and cause serious pollution to the environment. Furthermore, the biochar synthesized with the above activators possesses a relatively large specific surface area, but lacks a mesoporous structure, which is not conducive to the improvement of adsorption rate or the adsorption of antibiotics with relatively large molecular sizes [35,36,37]. Therefore, it is more appropriate to choose an activator with less pollution and a greater mesoporous forming ability. Herein, we chose KHCO3 as the activator, as it can meet the two above-mentioned advantages. First, K2CO3 produced by KHCO3 during pyrolysis can react with the biomass to form microporous and mesoporous structures in the biochar. Second, CO2 gas produced by KHCO3 erodes the biomass and endows the biochar with more mesopores [38,39,40].
The biomass used to synthesize biochar are varied. Here, we choose poplar leaf as the raw material, which is widely distributed in China, Europe, West Asia, and North Africa, and has a huge annual output. The biochar is prepared from poplar leaf activated by KHCO3 using an oxygen-limited pyrolysis method. We studied the effect of the KHCO3 addition on the specific surface area and pore distribution of the biochar. In addition, the adsorption capability and adsorption mechanism of biochar to OTC was analyzed. Finally, we studied the adsorption performance of biochar on OTC in natural water matrices and its regeneration performance, which highlights the potential application of poplar leaf-based biochar in the remediation of antibiotic pollution.

2. Results and Discussion

2.1. Preparation and Characterizations of Biochars

The biochars were prepared using poplar leaves as raw materials and KHCO3 as the activator using an oxygen-limited pyrolysis method (Scheme 1). The yield of biochar (PKC-0) without activation is 21.3 wt%, which is the highest among all of the samples. With the increase of the KHCO3 addition, the yields decline continuously (Table S1, Supplementary Materials). This implies that KHCO3 and its decomposition products react with the biomass and etch some biochar, resulting in a lower yield.
The morphology of biochars was observed by scanning electron microscopy (SEM), as shown in Figure 1; the biochar PKC-0 inherited the structure of the poplar leaf and presented a smooth and compact surface. After adding KHCO3, the biochars became small pieces and presented many pores, indicating KHCO3 has a significant pore-forming effect on biochar. With the increase of the KHCO3 addition, the biochars became increasingly fragmented, implying that the etching effect of KHCO3 on biochar is more and more obvious, which is consistent with the declining trend of biochar yields.
Raman spectra were performed to analyze the graphitization degree of these biochars. As shown in Figure 2, all patterns display two distinct peaks, which can be assigned to D-band (around 1340 cm−1) and G-band (around 1590 cm−1), corresponding to amorphous carbon and graphitic carbon in biochars, respectively [41]. The intensity ratio (IG/ID) of G-band to D-band was used to reflect the graphitization degree of biochars [42]. As shown in Table S2 (Supplementary Materials), with the increase of the KHCO3 addition, the IG/ID ratios decrease from 0.993 to 0.850, indicating that KHCO3 destroys the biochar matrix and reduces its graphitization degree.
X-ray photoelectron spectra (XPS) were performed to analyze the composition and the state of the elements of these biochars. The full spectra (Figure S1, Supplementary Materials) show that biochars are mainly composed of carbon, nitrogen, and oxygen elements. As shown in Table S3 (Supplementary Materials), with the increase of the KHCO3 addition, the carbon elemental atomic percentage keeps decreasing, while the oxygen elemental atomic percentage keeps rising, indicating that KHCO3 can oxidize carbon atoms and produce oxygen-containing groups. To understand the detailed bonding configuration of the oxygen element, high-resolution O1s spectra were recorded (Figure S2, Supplementary Materials). The splitting O1s peaks of biochars at 530.4, 531.7, and 532.8 eV are attributed to the lattice oxygen (C=O) [43], carboxyl oxygen (−COOH), and hydroxy oxygen (−OH) [44,45], respectively. Among them, the proportion of carboxyl oxygen and hydroxyl oxygen is more than 90%, which may promote the adsorption performance of biochars.
In order to clarify the differences of pore structures between different biochars, the specific surface areas and pore size distributions were analyzed using nitrogen adsorption and desorption technology. As shown in Figure 3a, the nitrogen adsorption capacity of PKC-0 is very weak, indicating that its specific surface area is small, and its pore structure is not developed. Meanwhile, the nitrogen adsorption capacity of PKC-1 is much higher, indicating that KHCO3 plays a significant role in activating biochars. In the P/P0 range of less than 0.1, the nitrogen adsorption capacities of all biochars are relatively high, indicating that micropores are present in all biochars [46]. In addition, all biochars exhibit a type IV curve with hysteresis loops in the P/P0 range of 0.40–1.0, indicating the presence of mesopores [47].
The BET method and the BJH method were used to calculate the total specific surface area and the mesoporous specific surface area of biochars, respectively. The detailed calculation method is provided in the supplementary information, and the results are shown in Table 1. With the increase of the KHCO3 addition, both the total specific surface area and the mesoporous specific surface area increased initially, then stabilized, and finally decreased slightly, which implies that KHCO3 can effectively make pores in biochars, but excessive KHCO3 will cause the pore structure of biochars to collapse and reduce their specific surface areas. It should be noted that the total specific surface area of PKC-3 is close to that of PKC-2, but its mesoporous specific surface area is much higher than that of PKC-2. This change also applies to pore volume and average pore size. These results indicate that mesopores are probably formed by KHCO3 corrosion micropores. For the biochars activated by KHCO3, the ratios of mesoporous specific surface area to total specific surface area (Smeso/Stotal) initially increased from 16% to approximately 65%, and then stabilized, which implies that excessive KHCO3 does not help the formation of the mesoporous structure. Figure 3b displays the pore size distributions of biochars calculated using the BJH method through nitrogen desorption isothermal curves. It shows that the pore sizes are all concentrated around 3.8 nm, further indicating the good mesopore-forming effect of KHCO3. All these characteristics demonstrate that KHCO3 can create both micropores and mesopores in biochars, thus significantly increasing their specific surface areas.
The interaction of KHCO3 with biochar can be divided into three steps. First, at 100–200 °C, KHCO3 decomposes to generate K2CO3 and CO2, which moderately erode the poplar leaf. Second, at 200–700 °C, the poplar leaf decomposes constantly, and K2CO3 is reduced to metallic potassium by carbon, which is etched into CO to create pores (K2CO3 + 2C → 2K + 3CO). Third, at 800 °C, K2CO3 decomposes slowly to generate K2O and CO2 (K2CO3 → K2O + CO2), which might etch carbon (CO2 + C → 2CO) to generate more pores and enlarge the existing pores.

2.2. Adsorption Kinetics

To evaluate the adsorption kinetics of biochars, the initial OTC concentration was fixed at 200 ppm, and the adsorption time was limited to 1–180 min. As shown in Figure 4, OTC is rapidly adsorbed by biochars at the initial stage of the adsorption process. As the adsorption proceeds, OTC continues to occupy the adsorption site, resulting in a decrease in the adsorption rate and finally reaching the adsorption equilibrium. It is worth noting that within 20 min, the adsorption capacities of PKC-3 and PKC-5 reached more than 80% of their maximum adsorption capacities, and PKC-4 reached more than 95% of its maximum adsorption capacity, which indicates that the adsorption rate of these biochars is very high. This is probably due to the presence of abundant mesopores in these biochars, which is beneficial to the diffusion of OTC and its interaction with adsorption sites in biochars [48,49,50]. Comparatively, within 20 min, the adsorption capacity of PKC-2 was only approximately 57% of its maximum adsorption capacity, which indicates that the adsorption rate of PKC-2 is much lower, even though its specific surface area is close to the above three biochars. This is probably due to its underdeveloped mesoporous structure, which hinders the diffusion of OTC. In addition, with the increase of the KHCO3 addition, the maximum adsorption capacities of biochars for OTC initially increased, and then decreased slightly. This change trend is the same as that of the total specific surface area of biochars, indicating that the total specific surface area may be an important factor for determining adsorption capacities.
To better understand the adsorption kinetics of these biochars, a pseudo-first-order model and a pseudo-second-order model were used to analyze the kinetic data—the fitted curves are displayed in Figure S3 (Supplementary Materials) and the related parameters are displayed in Table 2. For all biochars, the correlation coefficient R2 of the pseudo-second-order model was higher than that of the pseudo-first-order model, indicating that the pseudo-second-order model provides a better fit to the kinetic data. These results imply that the adsorption interaction of OTC with biochars involves both physical adsorption and chemical adsorption [51]. Compared with all biochars, PKC-4 shows the highest adsorption performance; its maximum adsorption capacity of 543 mg/g was calculated from the pseudo-second-order model, which is higher than that reported in most of the literature (Table S4, Supplementary Materials), confirming that PKC-4 is highly effective for the adsorption of OTC.
Furthermore, an intra-particle diffusion model was used to study the role of diffusion in adsorption. As shown in Figure S4 (Supplementary Materials), these data can be mapped along three straight lines with different slopes and intercepts, indicating that the adsorption process can be divided into three stages. Stage I was the fastest step, which can be associated with surface diffusion. At stage I, there were abundant unoccupied adsorption sites on the surface of biochars, and the mass transfer resistance through the surface film was low, resulting in a high adsorption rate. At stage II, the surface adsorption sites were occupied, and adsorbate molecules faced higher mass transfer resistance to traverse the mesopores of biochars, resulting in a lower adsorption rate. At stage III, the adsorption rate was further reduced, reflecting the saturation of biochars without future adsorption. In addition, the intercepts of all lines were not equal to zero, indicating that the adsorption rate was controlled by film diffusion and intra-particle diffusion [52]. With the increase of the KHCO3 addition, the intercepts generally increase, indicating that the influence of the boundary layer on adsorption is more and more obvious.

2.3. Adsorption Isotherms

To evaluate the adsorption isotherms of biochars, the initial OTC concentration was fixed at 25 ppm, 50 ppm, 100 ppm, 150 ppm, and 200 ppm, respectively, and the adsorption time was fixed at 180 min. As shown in Figure 5, with the increase of the initial concentration of OTC, the equilibrium adsorption capacities of biochars and the equilibrium concentrations of OTC in the solution also increase.
To better understand the adsorption isotherms of biochars, the Langmuir model and the Freundlich model were used to analyze the equilibrium data—the fitted curves are displayed in Figure S5 (Supplementary Materials) (Langmuir model) and Figure S6 (Supplementary Materials) (Freundlich model), and the related parameters are displayed in Table 3. The correlation coefficient R2 of the Freundlich model was higher than that of the Langmuir model except for PKC-2 adsorption, indicating that the Freundlich model provides a better fit to the equilibrium data except for PKC-2 adsorption. The closer fit of the Freundlich model implies that the adsorption of OTC on biochars is mainly multi-layer adsorption [53]. In general, the factor 1/n is used to predict the adsorption difficulty. As shown in Table 3, the values of 1/n in all biochars are between 0 and 1, suggesting that the adsorption of biochars for OTC is favorable [54]. Furthermore, these biochars possess a mesoporous structure, and the proportion of mesoporous specific surface area of some biochars exceeds 64%, resulting in the accumulation of adsorbed molecules and ensuring the possibility of multi-layer adsorption. Comparatively, the Langmuir model provided a better fit to the equilibrium data for PKC-2 adsorption, indicating that the leading part of OTC adsorption is monolayer adsorption. As previously described, PKC-2 is rich in microporous structures, and the proportion of mesoporous specific surface area of PKC-2 is only 31%, which is not conducive to the accumulation of adsorbed molecules, making it difficult to achieve multi-layer adsorption.

2.4. Effects of Solution pH and Metal Ions

Solution pH is considered to be an important factor in the adsorption process, which affects the speciation of the pollutant and the surface charge of the adsorbent. To evaluate the impact of the solution pH, PKC-4 was selected as the adsorbent, and the initial OTC concentration was fixed at 200 ppm. As shown in Figure 6a, with the increase of the solution pH, the adsorption capacity decreased gradually, but the overall change was small, indicating that the effect of the solution pH was small. When the pH was lower, PKC-4 was electrically neutral, no obvious electrostatic repulsion between OTC and PKC-4 is observed. As the solution pH increases, the oxygen-containing functional groups (such as carboxyl group and hydroxyl group) on the surface of PKC-4 may be deprotonated, resulting in a negative surface charge of PKC-4. At the same time, OTC exists in the form of a negative charge, and the electrostatic repulsion between PKC-4 and OTC leads to the reduction of adsorption capacity. In addition, high pH value weakens the hydrogen bonding between PKC-4 and OTC, further reducing the adsorption capacity. It is noteworthy that the adsorption capacities are all around 500 mg/g in the range of 3–11 pH, indicating that PKC-4 can maintain high adsorption performance at different pH values.
The effect of metal cations in solution on adsorption equilibrium was also analyzed. For comparison, the concentration of metal cations was fixed at 100 ppm. As shown in Figure 6b, the presence of Na+ increased adsorption capacity, which may be because Na+ enhances the hydrophobic interaction between PKC-4 and OTC through salting out. K+ reduced adsorption capacity, possibly because it occupies the adsorption site of PKC-4. Compared with K+, Cu2+ had a more obvious effect on reducing adsorption capacity, which may be due to its high charge occupying more adsorption sites of PKC-4. Ca2+ and Mg2+ had little effect on adsorption capacity, which may be attributed to two aspects. On the one hand, they may occupy the adsorption sites of PKC-4 and reduce adsorption capacity; on the other hand, they may play a bridging role between OTC and the surface groups of PKC-4, increasing adsorption capacity [55]. Notably, Fe3+ reduced adsorption capacity by almost half. The reason may be that excessive positive charges occupy a large number of adsorption sites of PKC-4.
In addition, we analyzed the adsorption performance of PKC-4 in campus lake water and city water. As shown in Figure S7 (Supplementary Materials), compared to deionized water, the adsorption capacity of PKC-4 in campus lake water and city water decreased by 7.6% and 12.8%, respectively, indicating that PKC-4 has good potential in practical application.

2.5. Reusability

Recycling performance is an important factor in practical application. Here, biochar PKC-4 was regenerated by pyrolysis at 800 °C for 2 h under nitrogen flow, and then directly used for the next adsorption. As shown in Figure S8 (Supplementary Materials), after four cycles, adsorption capacity only decreased by approximately 6%, indicating that PKC-4 is highly stable in the adsorption process.

2.6. Possible Adsorption Mechanism

Various interactions participate in the adsorption of OTC by biochar. First, pore-filling is considered to be the main factor determining OTC adsorption. The correlation between the total specific surface area, pore volume, and the adsorption capacity of PKC-4 is shown in Figure S9 (Supplementary Materials). Both parameters display a good linear correlation with adsorption capacity, indicating that the pore structure has a very significant effect on adsorption. In addition, the nitrogen adsorption and desorption analysis shows that the total specific surface area and pore volume of PKC-4 are significantly reduced after use (Figure S10 and Table S5, Supplementary Materials), demonstrating that pore-filling is an important factor determining OTC adsorption [52]. It is noted that the ratio Smeso/Stotal of PKC-4 after use increases from 64.4% to 96.8%, and the corresponding average pore size increases from 2.95 nm to 3.61 nm, indicating that both micropores and mesopores participate in the adsorption of OTC.
Second, the electrostatic interaction plays an important role in the adsorption of OTC by biochar. OTC exhibits different charges under different pH conditions, and the adsorption capacity of PKC-4 varies with the change of the solution pH. Furthermore, the capacity declines sharply in the presence of Cu2+ and Fe3+, demonstrating that the electrostatic interaction is one of the adsorption mechanisms.
Third, functional groups on biochar surfaces also promote the adsorption of OTC by biochar. XPS spectra confirm the existence of oxygen-containing functional groups in these biochars, which can generate H-bonds, and that OTC has hydroxyl and amino groups, which could also form H-bonds. Fourier transform infrared (FTIR) spectra show that the tensile vibration of O–H bond at 3627 cm−1 and the stretching vibration of C=O bond at 1640 cm−1 of PKC-4, shift to 3622 cm−1 and 1644 cm−1, respectively, after OTC adsorption (Figure S11, Supplementary Materials). This is due to the deprotonation of carboxyl and hydroxyl groups in the adsorption process, indicating that the H-bonds play an important role in the adsorption process.
Finally, the adsorption of OTC by biochar can also be explained based on the π-π interaction. Raman spectra confirm the existence of graphitic carbon in these biochars, which can act as electron donors for their aromatic rings. These biochars can form a π-π electron-donor-acceptor (EDA) interaction with OTC for its electron-deficient polar aromatic rings.

3. Materials and Methods

3.1. Materials and Reagents

Poplar leaves were collected in the campus of Shandong First Medical University and Shandong Academy of Medical Sciences. Potassium bicarbonate, hydrochloric acid, sulphuric acid, sodium hydroxide, sodium chloride, potassium carbonate, calcium chloride, magnesium sulfate, copper nitrate, and iron nitrate were purchased from Sinopharm Chemical Reagent Co., Ltd. (Beijing, China). Nitrogen was purchased from Taian Yingchun Gas Co., Ltd. (Taian, China). Oxytetracycline hydrochloride was purchased from Beijing InnoChem Science and Technology Co., Ltd. (Beijing, China). All purchased reagents were used without further purification.

3.2. Preparation of Biochar

Poplar leaves were cleaned, dried, smashed to pieces, and stored in a dry atmosphere. A total of 5 g of smashed poplar leaf was mixed carefully with KHCO3 (the weight 1~5 g), and then the mixtures were placed in a tubular furnace and pyrolyzed at 800 °C for 2 h under nitrogen flow at a heating rate of 10 °C per minute. The samples were collected after cooling to room temperature, and washed with 2 M hydrochloric acid for 4 h at room temperature to remove inorganic salts. After filtration, washing, and drying, the biochar was obtained, which was denoted as PKC-n, where n represents the weight of KHCO3 added in the synthesis process.

3.3. General Procedure for the Adsorption of Oxytetracycline Hydrochloride

A total of 10 mg of biochar was added into 30 mL of OTC solution with a certain concentration, then placed into a table concentrator operating at a speed of 150 r/min at 25 °C. After adsorption for a period of time, some of the aqueous mixture was collected, and then diluted to 3 mL and filtered with 0.22 μm membrane. Its absorbance at 275 nm was analyzed using a UV-visible spectrophotometer. Each dataset was repeated three times. The adsorption capacity of biochar to OTC was calculated using the following equation:
q = A 0 − A t × c 0 × V m
where q (mg/g)—adsorption amount of OTC at time t; A0—absorbance of initial aqueous mixture; At—absorbance of aqueous mixture at time t; c0 (mg/L)—initial OTC concentration; V (L)—volume of OTC solution; and m (g)—mass of biochar.

3.4. Analysis of Adsorption Kinetics and Isotherms

The adsorption kinetics were fitted with a pseudo-first-order model (Equation (2)), a pseudo-second-order model (Equation (3)) and an intra-particle diffusion model (Equation (4)), respectively:
q = q e 1 − e − k 1 t
q = q e k 2 t 2 1 + q e k 2 t
q = k p t 1 / 2 + b
where q (mg/g)—adsorption amount of OTC at time t; qe (mg/g)—equilibrium adsorption amount of OTC; k1—adsorption constant of pseudo-first-order model; k2—adsorption constant of pseudo-second-order model; and kp—adsorption constant of intra-particle diffusion model.
The adsorption isotherms were fitted with the Langmuir model (Equation (5)) and the Freundlich model (Equation (6)):
c e q e = 1 q m K L + c e q m
ln q e = ln K F + 1 n ln c e
where qe (mg/g)—equilibrium adsorption amount of OTC; ce (mg/g)—equilibrium OTC concentration; qm (mg/g)—the maximum adsorption amount of OTC; KL—the Langmuir constant; KF—the Freundlich affinity coefficient; and n—the Freundlich exponential coefficient.

3.5. Characterizations

The morphology of biochar was observed by JSM-7610F SEM (Jeol, Tokyo, Japan). Nitrogen adsorption and desorption isotherms were analyzed at 77 K using a Jingweigaobo JW-BK100C analyzer (Beijing, China), and the samples were degassed at 200 °C for 4 h before measurements. The absorbance of the aqueous mixture was analyzed using a UV-1800 UV-Vis spectrophotometer (Shimadzu, Kyoto, Japan). FTIR spectra were performed on an IRPRestige-21 infrared spectrometer. Raman spectra were recorded using a renishaw inVia Raman spectrometer with an Ar laser (532 nm) as the excitation source. XPS were obtained from a ULVAC-PHI PHI5000 VersaprobeIII instrument (ULVAC-PHI, Chigasaki, Japan) with Al Kα radiation.

4. Conclusions

In this study, we prepared low-cost biochars through pyrolysis with poplar leaves as the raw material and KHCO3 as the activator. Characterizations indicate that KHCO3 can create abundant mesopores in biochars by etching micropores, but excessive KHCO3 cannot continuously promote the formation of a mesoporous structure. When used for adsorption of OTC, PKC-4 exhibits the best adsorption performance due to its large surface area and rich mesoporous structure. Model analysis shows that the pseudo-second-order model and the Freundlich model can best describe the adsorption kinetics and isotherms. In addition, PKC-4 displays high OTC adsorption capacity in a wide pH range, different metal ions, and different water matrices. Moreover, the biochar can be regenerated easily, and its adsorption capacity decreases little after four cycles. The adsorption mechanism is mainly pore-filling, though electrostatic interaction, hydrogen bond, and π-π interaction are also involved. This study realizes biomass waste recycling and highlights the potential of poplar leaf-based biochar for the adsorption of antibiotics.

Supplementary Materials

The following supporting information can be downloaded at: https://www.mdpi.com/article/10.3390/molecules28073188/s1, Calculation method for specific surface area and pore diameter. Figure S1: XPS full spectra of biochars prepared from poplar leaves with KHCO3 as activator; Figure S2: high-resolution O1s XPS spectra of biochars; Figure S3: (a) pseudo-first-order kinetic model (solid line) and (b) pseudo-second-order kinetic model (solid line) for the adsorption capacities of biochars at different times; Figure S4: linear intra-particle diffusion fittings for OTC on biochars; Figure S5: Langmuir model (solid line) for the equilibrium adsorption capacities of biochars at different initial OTC concentration; Figure S6: Freundlich model (solid line) for the equilibrium adsorption capacities of biochars at different initial OTC concentration; Figure S7: adsorption capacity of PKC-4 on OTC in different water matrices; Figure S8: cyclic adsorption performance of PKC-4 for OTC; Figure S9: correlation between the total specific surface area, pore volume and the adsorption capacity of PKC-4; Figure S10: nitrogen adsorption-desorption isotherms of Fresh PKC-4 and used PKC-4; Figure S11: FTIR spectra of fresh PKC-4 and used PKC-4; Table S1: yields of the biochars prepared from poplar leaves with KHCO3 as activator; Table S2: the IG/ID ratios of biochars; Table S3: the elemental atomic percentage of biochars analyzed by XPS; Table S4: a comparison between the adsorption performance over PKC-4 and other samples for the adsorption of OTC. Table S5: specific surface areas and porosity characteristics of fresh PKC-4 and used PKC-4. References [44,56,57,58,59,60,61,62,63] are cited in the supplementary materials.

Author Contributions

Biochar synthesis, Z.G. and L.W.; adsorption of OTC, C.Y. and Y.L.; SEM analysis and Raman analysis, C.H.; FTIR spectra and XPS spectra, K.L.; nitrogen adsorption and desorption isotherms analysis, Z.W.; data analysis, Z.W. and Y.S.; writing-original draft preparation, Z.W.; writing—review and editing, K.L. and Y.S.; project administration, K.L. and Y.S.; funding acquisition, C.H. All authors have read and agreed to the published version of the manuscript.

Funding

This research was funded by the Shandong Medical and Health Science and Technology Development Plan Project (202102020612), the Academic Promotion Programme of Shandong First Medical University (2019QL008) and the Incubation Program of Youth Innovation of Shandong Province.

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

Data is contained within the article or Supplementary Material.

Acknowledgments

We thank Shandong First Medical University and Shiyanjia Lab (http://www.shiyanjia.com (accessed on 22 February 2023)) for help in instrumental analysis.

Conflicts of Interest

The authors declare no conflict of interest.

Samples Availability

Samples of the compounds are not available from the authors.

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Molecules 28 03188 sch001 550
Scheme 1. Schematic representation of the biochar synthesis from poplar leaf with KHCO3 as activator.
Scheme 1. Schematic representation of the biochar synthesis from poplar leaf with KHCO3 as activator.
Molecules 28 03188 sch001
Molecules 28 03188 g001 550
Figure 1. SEM images of biochars prepared from poplar leaves with KHCO3 as activator (×5000).
Figure 1. SEM images of biochars prepared from poplar leaves with KHCO3 as activator (×5000).
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Molecules 28 03188 g002 550
Figure 2. Raman spectra of biochars.
Figure 2. Raman spectra of biochars.
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Molecules 28 03188 g003 550
Figure 3. (a) Nitrogen adsorption−desorption isotherms and (b) pore size distributions of biochars.
Figure 3. (a) Nitrogen adsorption−desorption isotherms and (b) pore size distributions of biochars.
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Molecules 28 03188 g004 550
Figure 4. Time-dependent adsorption capacities over different biochars.
Figure 4. Time-dependent adsorption capacities over different biochars.
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Molecules 28 03188 g005 550
Figure 5. The equilibrium adsorption capacities of biochars at different initial OTC concentrations.
Figure 5. The equilibrium adsorption capacities of biochars at different initial OTC concentrations.
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Molecules 28 03188 g006 550
Figure 6. The influence of (a) different initial solution pH and (b) different types of ions on the adsorption of OTC by PKC-4.
Figure 6. The influence of (a) different initial solution pH and (b) different types of ions on the adsorption of OTC by PKC-4.
Molecules 28 03188 g006
Table
Table 1. Specific surface areas and porosity characteristics of biochars.
Table 1. Specific surface areas and porosity characteristics of biochars.
BiocharTotal Specific Surface Area (m2/g)Mesoporous Specific Surface Area (m2/g)Smeso/StotalPore Volume (cm3/g)Average Pore Size (nm)
PKC-036.234.093.9%0.06957.68
PKC-1913.3145.716.0%0.59662.49
PKC-21543.1478.431.0%0.96192.61
PKC-31686.11100.265.3%1.24262.92
PKC-41769.71140.064.4%1.29452.95
PKC-51684.01091.164.8%1.27983.04
Table
Table 2. Adsorption kinetic parameters of pseudo-first-order model and pseudo-second-order model for OTC adsorption on biochars.
Table 2. Adsorption kinetic parameters of pseudo-first-order model and pseudo-second-order model for OTC adsorption on biochars.
BiocharPseudo-First-Order ModelPseudo-Second-Order Model
qe (mg/g)k1 min−1R2qe (mg/g)k2 (mg·g−1·min−1)R2
PKC-051.5 ± 2.30.30697 ± 0.083970.826854.3 ± 1.830.00855 ± 0.002250.9215
PKC-1127.8 ± 4.60.56475 ± 0.134960.8629133.6 ± 3.430.00612 ± 0.001380.9425
PKC-2393.6 ± 18.10.06058 ± 0.012150.9137438.4 ± 17.680.00020 ± 0.000040.9617
PKC-3509.3 ± 14.30.20737 ± 0.033540.9405538.4 ± 8.770.00060 ± 0.000070.9849
PKC-4524.3 ± 6.80.56311 ± 0.048370.9816543.0 ± 2.130.00165 ± 0.000060.9986
PKC-5501.9 ± 14.20.45826 ± 0.083380.9190524.0 ± 8.580.00132 ± 0.000180.9777
Table
Table 3. Adsorption isotherm parameters of Langmuir model and Freundlich model for OTC adsorption on biochars.
Table 3. Adsorption isotherm parameters of Langmuir model and Freundlich model for OTC adsorption on biochars.
BiocharLangmuir ModelFreundlich Model
qm (mg/g)kL (L/mg)R2KF (mg/g (L/mg)1/n)1/nR2
PKC-059.5 ± 16.10.00648 ± 0.0004290.83830.94 ± 0.390.6886 ± 0.09340.9476
PKC-1141.0 ± 17.70.02159 ± 0.00310.956013.84 ± 2.060.4083 ± 0.03600.9772
PKC-2324.7 ± 16.30.08284 ± 0.015480.992652.52 ± 7.740.3915 ± 0.04450.9627
PKC-31514.7 ± 852.10.02025 ± 0.006450.623033.38 ± 8.110.8679 ± 0.10340.9592
PKC-41850.5 ± 737.10.01909 ± 0.0051130.731736.79 ± 5.150.8958 ± 0.06410.9848
PKC-51819.8 ± 822.70.01692 ± 0.0049940.692133.04 ± 4.930.8880 ± 0.06480.9843
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Wei, Z.; Hou, C.; Gao, Z.; Wang, L.; Yang, C.; Li, Y.; Liu, K.; Sun, Y. Preparation of Biochar with Developed Mesoporous Structure from Poplar Leaf Activated by KHCO3 and Its Efficient Adsorption of Oxytetracycline Hydrochloride. Molecules 2023, 28, 3188. https://doi.org/10.3390/molecules28073188

AMA Style

Wei Z, Hou C, Gao Z, Wang L, Yang C, Li Y, Liu K, Sun Y. Preparation of Biochar with Developed Mesoporous Structure from Poplar Leaf Activated by KHCO3 and Its Efficient Adsorption of Oxytetracycline Hydrochloride. Molecules. 2023; 28(7):3188. https://doi.org/10.3390/molecules28073188

Chicago/Turabian Style

Wei, Zhenhua, Chao Hou, Zhishuo Gao, Luolin Wang, Chuansheng Yang, Yudong Li, Kun Liu, and Yongbin Sun. 2023. "Preparation of Biochar with Developed Mesoporous Structure from Poplar Leaf Activated by KHCO3 and Its Efficient Adsorption of Oxytetracycline Hydrochloride" Molecules 28, no. 7: 3188. https://doi.org/10.3390/molecules28073188

APA Style

Wei, Z., Hou, C., Gao, Z., Wang, L., Yang, C., Li, Y., Liu, K., & Sun, Y. (2023). Preparation of Biochar with Developed Mesoporous Structure from Poplar Leaf Activated by KHCO3 and Its Efficient Adsorption of Oxytetracycline Hydrochloride. Molecules, 28(7), 3188. https://doi.org/10.3390/molecules28073188

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