Effect of CeO2-Reinforcement on Pb Absorption by Coconut Coir-Derived Magnetic Biochar

Magnetic separable biochar holds great promise for the treatment of Pb2+-contaminated wastewater. However, the absorption effect of unmodified magnetic biochar is poor. Considering this gap in knowledge, CeO2-doped magnetic coconut coir biochar (Ce-MCB) and magnetic coconut coir biochar (MCB) for Pb2+ absorption were prepared by the impregnation method, and the efficiency of Ce-MCB for Pb2+ absorption was evaluated in comparison with MCB. Conducting the absorption experiments, the study provided theoretical support for the exploration of the absorption mechanism. The quantitative analysis exposed that the enhanced absorption capacity of Ce-MCB was attributed to the increase in oxygen-containing functional groups and mineral precipitation. The Langmuir and Freundlich isotherm model showed that Ce-MCB is a suitable adsorbent for Pb2+. The absorption characteristics of Ce-MCB was fit well with the pseudo-second-order (PSO) and Langmuir models, which revealed that the absorption of Pb2+ in water was monolayer chemisorption with a maximum theoretical adsorption capacity of 140.83 mg·g−1. The adsorption capacity of Ce-MCB for Pb(II) was sustained above 70% after four cycles. In addition, the saturation magnetization intensity of Ce-MCB was 7.15 emu·g−1, which was sufficient to separate out from the solution. Overall, Ce-MCB has wide application prospects in terms of biomass resources recycling and environmental conservation.


Introduction
The widespread occurrence of pollution in surface water and groundwater, especially toxic elements, due to human activities may be exceptionally detrimental to the ecosystem [1]. Heavy metals are persistent in the environment and accumulate in organisms through the food chain, negatively impacting the growth of plants and animals. Pb 2+ is one of the toxic and harmful pollutants present in industrial wastewater [2]. Over the last two centuries, Pb 2+ has been widely used in production and daily life such as those from battery production, electroplating, mining, metal smelting, and the use of irrigation, which has proliferated the spread of lead into the environment [3]. Pb can enter the human body mainly through drinking water and food, which creates severe toxicity to human organs. High concentrations of Pb cause adverse effects such as anemia, kidney dysfunction, and gastric cancer [4,5]. The Agency for Toxic Substances and Disease Registry (IARC) identified Pb 2+ as one of the most hazardous elements [6].
Biochar as a carbon-rich material is considered a cost-effective and environmentally friendly adsorbent, and has received more concern because of its simple preparation, wide range of sources, low price, and strong effect. It has sufficient selectivity and applicability in removing toxic heavy metal ions from various water environments. [17]. Coconut coir is a typical abundant and inexpensive agricultural waste, which is still mainly used for the production of low value-added products, with only a small amount for biochar production. More than 420,000 tons coconuts are produced annually in China, and the production of coconut skin can reach 250 million pieces [18]. In the current study, Li et al. [19] reported that coconut-coir-derived biochar can provide binding sites for Pb 2+ . However, the ability of pristine biochar to remove heavy metals is not impressive, and it is difficult to separate from aqueous solution. In general, biochar magnetically treated by means of Fe 2+ /Fe 3+ solution or natural hematite can be easily separated from the solution by external magnets, but magnetic biochar without modification has poor adsorption performance [20]. As magnetic biochar has a low adsorption capacity, it was modified to expand the absorption capacity of the biochar while retaining the magnetic properties.
There are few studies that have reported the use of cerium-nitrate-modified magnetic biochar for Pb 2+ removal in aqueous environments. Previous research has shown that the absorbents have been modified by loading transition metal oxides and alkaline earth mental oxides on the surface of biochar [21,22]. CeO 2 is one of the most industrially useful rare earth metal oxides with low toxicity, and its pure metal has a high emission threshold to the environment, which makes the absorbent less toxic [23,24]. CeO 2 nanoparticles, as a new absorption material, have great potential in heavy metal removal. In Malinee's study, samaria-doped ceria nanopowder had a high removal capacity at low Pb 2+ concentrations, but was confined by the aggregation of nanoparticles. In addition, the theoretical maximum absorption capacity of the adsorbent is 23 mg·g −1 [25]. Market-Borayo reported the efficiency of Pb 2+ absorption by CeO 2 nanoparticles, while the results were comparable in a previous study [15]. Recillas et al. [26] synthesized CeO 2 nanocrystal precipitates, where they showed strong absorption capacities of Pb 2+ up to 189 mg·g −1 . Nevertheless, CeO 2 nanocrystal precipitates presented a high phytotoxicity, which undoubtedly poses a great threat to aqueous organisms and human health. In order to fully utilize the excellent adsorption performance of CeO 2 , its high toxicity disadvantage needs to be overcome as a priority. In this study, we propose the stabilization of CeO 2 on magnetic carbon materials by high-temperature calcination to make it easy to separate.
In the study, the synthesis of magnetic biochar doped with CeO 2 (noted as Ce-MCB) via a simple impregnation method is reported to improve the adsorption performance of Pb 2+ . The physicochemical properties (surface morphology, pore structure, chemical composition, magnetic properties, etc.) of magnetic biochar (MCB) and CeO 2 -doped magnetic biochar (Ce-MCB) were explored. Moreover, the effects of time dependence, pH, and Pb 2+ concentration on the absorption capacity of two magnetic biochars were also analyzed. The corresponding models of isotherms and kinetics were further developed to describe the adsorption process. In terms of the adsorption mechanism, XPS, XRD, and FTIR analyses were performed on the biochar before and after adsorption to qualitatively explore the adsorption mechanism, and the adsorption rate of each component was quantified by the acid washing method. The experimental procedure is shown in Scheme 1.

Morphology Characteristics
In order to understand the surface characteristics and elemental composition of Ce-MCB, a systematic characterization of the as-prepared magnetic adsorbent was performed. Additionally, to investigate the effect of Ce addition on the adsorption performance, MCB was also prepared and tested for physicochemical properties.
The morphology and composition of MCB and Ce-MCB were carried out by SEM. As can be seen from Figure 1a-d, Ce-MCB had a richer pore structure compared to MCB. Meanwhile, Ce-MCB also exhibited a rougher surface, which affords a vast range of available surface-active sites. These differences suggest that the added Ce(NO3)3, which can act as a chemical activator during pyrolysis at high temperatures, lead to a significant change in the textural properties of the biochar [27]. In addition, the presence of Fe on MCB and the presence of Ce and Fe on Ce-MCB were detected by the SEM-EDX test, which indicates the successful preparation of the adsorbents (Figure 1e,f).

Morphology Characteristics
In order to understand the surface characteristics and elemental composition of Ce-MCB, a systematic characterization of the as-prepared magnetic adsorbent was performed. Additionally, to investigate the effect of Ce addition on the adsorption performance, MCB was also prepared and tested for physicochemical properties.
The morphology and composition of MCB and Ce-MCB were carried out by SEM. As can be seen from Figure 1a-d, Ce-MCB had a richer pore structure compared to MCB. Meanwhile, Ce-MCB also exhibited a rougher surface, which affords a vast range of available surface-active sites. These differences suggest that the added Ce(NO 3 ) 3 , which can act as a chemical activator during pyrolysis at high temperatures, lead to a significant change in the textural properties of the biochar [27]. In addition, the presence of Fe on MCB and the presence of Ce and Fe on Ce-MCB were detected by the SEM-EDX test, which indicates the successful preparation of the adsorbents (Figure 1e,f).
The specific surface area (SSA) and pore size distribution of biochar were analyzed and the results are shown in Figure 2 and Table 1. As seen from Figure 2a, the N 2 adsorption isotherms of both samples belonged to the type IV mode with a clear hysteresis loop according to the International Union of Pure and Applied Chemistry (IUPAC) classification, which indicates the presence of mesoporous structures in them [28][29][30]. The curve of MCB was open, which is attributed to the difficulty of completely desorbing the gas from pores of MCB after adsorption due to the complex of the pore structure for biochar and the tendency to produce elastic or ink-bottle-like pores [31,32]. The BET surface area of Ce-MCB was 246.32 m 2 ·g −1 , which was higher than that of MCB (234.35 m 2 ·g −1 ). As shown in the BJH pore size distribution curve (Figure 2b), a large abundance of microporous and mesoporous structures were present in the prepared adsorbents. Notably, the quantity of Ce-MCB mesopores was significantly increased compared to MCB, especially in the size range of 2.5-5 nm, which suggests that the incorporation of cerium oxide had a certain activating effect on the development of pore structure in biochar [33,34]. As can be seen from Figure 1a-d, Ce-MCB had a richer pore structure compared to MCB. Meanwhile, Ce-MCB also exhibited a rougher surface, which affords a vast range of available surface-active sites. These differences suggest that the added Ce(NO3)3, which can act as a chemical activator during pyrolysis at high temperatures, lead to a significant change in the textural properties of the biochar [27]. In addition, the presence of Fe on MCB and the presence of Ce and Fe on Ce-MCB were detected by the SEM-EDX test, which indicates the successful preparation of the adsorbents (Figure 1e,f).  The specific surface area (SSA) and pore size distribution of biochar were analyzed and the results are shown in Figure 2 and Table 1. As seen from Figure 2a, the N2 adsorption isotherms of both samples belonged to the type IV mode with a clear hysteresis loop according to the International Union of Pure and Applied Chemistry (IUPAC) classification, which indicates the presence of mesoporous structures in them [28][29][30]. The curve of MCB was open, which is attributed to the difficulty of completely desorbing the gas from pores of MCB after adsorption due to the complex of the pore structure for biochar and the tendency to produce elastic or ink-bottle-like pores [31,32]. The BET surface area of Ce-MCB was 246.32 m 2 ·g −1 , which was higher than that of MCB (234.35 m 2 ·g −1 ). As shown in the BJH pore size distribution curve (Figure 2b), a large abundance of microporous and mesoporous structures were present in the prepared adsorbents. Notably, the quantity of Ce-MCB mesopores was significantly increased compared to MCB, especially in the size range of 2.5-5 nm, which suggests that the incorporation of cerium oxide had a certain activating effect on the development of pore structure in biochar [33,34].  The specific surface area (SSA) and pore size distribution of biochar were analyzed and the results are shown in Figure 2 and Table 1. As seen from Figure 2a, the N2 adsorption isotherms of both samples belonged to the type IV mode with a clear hysteresis loop according to the International Union of Pure and Applied Chemistry (IUPAC) classification, which indicates the presence of mesoporous structures in them [28][29][30]. The curve of MCB was open, which is attributed to the difficulty of completely desorbing the gas from pores of MCB after adsorption due to the complex of the pore structure for biochar and the tendency to produce elastic or ink-bottle-like pores [31,32]. The BET surface area of Ce-MCB was 246.32 m 2 ·g −1 , which was higher than that of MCB (234.35 m 2 ·g −1 ). As shown in the BJH pore size distribution curve (Figure 2b), a large abundance of microporous and mesoporous structures were present in the prepared adsorbents. Notably, the quantity of Ce-MCB mesopores was significantly increased compared to MCB, especially in the size range of 2.5-5 nm, which suggests that the incorporation of cerium oxide had a certain activating effect on the development of pore structure in biochar [33,34].  The G and D bands measured by RS were widely used to evaluate the microstructure of biochar. The G peak (1580-1600 cm −1 ) was generated by the in-plane tangential vibration of sp2 carbon atoms, while the D peak (1340-1357 cm −1 ) was produced by the The G and D bands measured by RS were widely used to evaluate the microstructure of biochar. The G peak (1580-1600 cm −1 ) was generated by the in-plane tangential vibration of sp2 carbon atoms, while the D peak (1340-1357 cm −1 ) was produced by the oscillation of disordered carbon materials [35,36]. The defect degree of biochar can be indicated by the I D /I G value in the Raman spectrum, and the higher the I D /I G ratio of the sample, the greater the degree of defect on the surface [37]. From the results in Figure 3, the I D /I G value of Ce-MCB (0.875) was larger than that of MCB (0.851), which demonstrated that Ce-MCB possessed higher activity with more abundant defects and functional groups [38]. The increased degree of defects in the biochar modified with Ce(NO 3 ) 3 may be related to the destruction of the original graphitized structure by the doped CeO 2 and NO 3 − . In addition, the attaching metal oxides on the surface of biochar could also act as the active sites of the adsorbent, thus promoting the reaction efficiency [36].
Int. J. Mol. Sci. 2023, 24, x FOR PEER REVIEW 5 oscillation of disordered carbon materials [35,36]. The defect degree of biochar ca indicated by the ID/IG value in the Raman spectrum, and the higher the ID/IG ratio o sample, the greater the degree of defect on the surface [37]. From the results in Figu the ID/IG value of Ce-MCB (0.875) was larger than that of MCB (0.851), which dem strated that Ce-MCB possessed higher activity with more abundant defects and f tional groups [38]. The increased degree of defects in the biochar modified with Ce(N may be related to the destruction of the original graphitized structure by the doped C and NO3 − . In addition, the attaching metal oxides on the surface of biochar could also as the active sites of the adsorbent, thus promoting the reaction efficiency [36]. The zeta potential is a technique for measuring the surface charge of materials b on the fact that the number of surface charges of biochar varies with the pH value o solution [39]. When the pH was lower than the point of zero charge (pHpzc), the surfa the material was positively charged, which was unfavorable for the absorption of due to the electrostatic repulsion. With increasing pH, the carboxylic acid groups hydroxyl groups were deprotonated. Under the condition that the pH was greater pHpzc, the surface of the biochar was negatively charged, which enhanced the electros attraction [40]. As shown in Figure 4, the point of zero charge of MCB was 2.72, while of Ce-MCB was increased to 3.94. The zeta potential ranged from 18.3 to −37.5 mV MCB and from 10.2 to −31.1 mV for Ce-MCB over the pH range of 2-10. It is thus both biochar surfaces were negatively charged over a wide pH range and that the potential of Ce-MCB was slightly higher than that of MCB. The above result is in cordance with P et al. that Ce-MCB provides more positive charge as compared to M which could be attributed to the greater formation of metal oxide [41].   The zeta potential is a technique for measuring the surface charge of materials based on the fact that the number of surface charges of biochar varies with the pH value of the solution [39]. When the pH was lower than the point of zero charge (pH pzc ), the surface of the material was positively charged, which was unfavorable for the absorption of Pb 2+ , due to the electrostatic repulsion. With increasing pH, the carboxylic acid groups and hydroxyl groups were deprotonated. Under the condition that the pH was greater than pH pzc , the surface of the biochar was negatively charged, which enhanced the electrostatic attraction [40]. As shown in Figure 4, the point of zero charge of MCB was 2.72, while that of Ce-MCB was increased to 3.94. The zeta potential ranged from 18.3 to −37.5 mV for MCB and from 10.2 to −31.1 mV for Ce-MCB over the pH range of 2-10. It is thus that both biochar surfaces were negatively charged over a wide pH range and that the zeta potential of Ce-MCB was slightly higher than that of MCB. The above result is in accordance with P et al. that Ce-MCB provides more positive charge as compared to MCB, which could be attributed to the greater formation of metal oxide [41]. oscillation of disordered carbon materials [35,36]. The defect degree of biochar can be indicated by the ID/IG value in the Raman spectrum, and the higher the ID/IG ratio of the sample, the greater the degree of defect on the surface [37]. From the results in Figure 3, the ID/IG value of Ce-MCB (0.875) was larger than that of MCB (0.851), which demonstrated that Ce-MCB possessed higher activity with more abundant defects and functional groups [38]. The increased degree of defects in the biochar modified with Ce(NO3)3 may be related to the destruction of the original graphitized structure by the doped CeO2 and NO3 − . In addition, the attaching metal oxides on the surface of biochar could also act as the active sites of the adsorbent, thus promoting the reaction efficiency [36]. The zeta potential is a technique for measuring the surface charge of materials based on the fact that the number of surface charges of biochar varies with the pH value of the solution [39]. When the pH was lower than the point of zero charge (pHpzc), the surface of the material was positively charged, which was unfavorable for the absorption of Pb 2+ , due to the electrostatic repulsion. With increasing pH, the carboxylic acid groups and hydroxyl groups were deprotonated. Under the condition that the pH was greater than pHpzc, the surface of the biochar was negatively charged, which enhanced the electrostatic attraction [40]. As shown in Figure 4, the point of zero charge of MCB was 2.72, while that of Ce-MCB was increased to 3.94. The zeta potential ranged from 18.3 to −37.5 mV for MCB and from 10.2 to −31.1 mV for Ce-MCB over the pH range of 2-10. It is thus that both biochar surfaces were negatively charged over a wide pH range and that the zeta potential of Ce-MCB was slightly higher than that of MCB. The above result is in accordance with P et al. that Ce-MCB provides more positive charge as compared to MCB, which could be attributed to the greater formation of metal oxide [41].   Previous studies have shown a positive correlation between hydrophilic and contact angle for biochar [42]. Biochar had wettability and was capable of absorbing water rapidly as well [43]. The hydrophilic properties of biochar were expressed by measuring the contact angle, as shown in Figure 5. The contact angle of the MCB was 8 • , indicating that it was a hydrophilic material. In contrast, Ce-MCB had a contact angle of 0 • and was a superhydrophilic material. The results showed that the hydrophilicity of Ce-MCB was higher than that of MCB, which is associated with the preferential orientation of the polar oxygencontaining groups (e.g., hydroxyl groups) enriched on the surface of Ce-MCB toward water [44]. The FTIR test results also prove the presence of these polar groups. Remarkably, the cerium oxide loaded on the Ce-MCB surface was inherently hydrophilic [45]. Previous studies have shown a positive correlation between hydrophilic and contact angle for biochar [42]. Biochar had wettability and was capable of absorbing water rapidly as well [43]. The hydrophilic properties of biochar were expressed by measuring the contact angle, as shown in Figure 5. The contact angle of the MCB was 8°, indicating that it was a hydrophilic material. In contrast, Ce-MCB had a contact angle of 0° and was a superhydrophilic material. The results showed that the hydrophilicity of Ce-MCB was higher than that of MCB, which is associated with the preferential orientation of the polar oxygen-containing groups (e.g., hydroxyl groups) enriched on the surface of Ce-MCB toward water [44]. The FTIR test results also prove the presence of these polar groups. Remarkably, the cerium oxide loaded on the Ce-MCB surface was inherently hydrophilic [45]. FTIR measurements were performed on MCB and Ce-MCB to characterize the functional groups present on the adsorbent surface, which were essential for the absorption process of metal ions. As shown in Figure 6, several peaks were observed in the spectra at about 3440, 1610, 1350, and 1070 cm −1 . The bands at about 3440 cm −1 and 1350 cm −1 indicated -OH asymmetric stretching vibration. In the aqueous environment, Ce 3+ can be used as active sites for the dissociation of H2O to form -OH [46]. The bands of 1610 cm −1 could be attributable to C=O (COO − ) stretching and bending vibrations [47]. The 1070 cm −1 band corresponded to the vibration of C-O. The peaks of carboxyl and hydroxyl groups were greatly enhanced after Ce(NO3)3 modification, which facilitates the absorption of heavy metals. The FTIR analysis results were in agreement with RS as well as contact angle results. The hysteresis loops of MCB and Ce-MCB were represented as magnetic properties. Figure 7 shows that the saturation magnetization of MCB and Ce-MCB were found to be 11.054 emu·g −1 and 7.149 emu·g −1 , respectively. Although the saturation magnetization FTIR measurements were performed on MCB and Ce-MCB to characterize the functional groups present on the adsorbent surface, which were essential for the absorption process of metal ions. As shown in Figure 6, several peaks were observed in the spectra at about 3440, 1610, 1350, and 1070 cm −1 . The bands at about 3440 cm −1 and 1350 cm −1 indicated -OH asymmetric stretching vibration. In the aqueous environment, Ce 3+ can be used as active sites for the dissociation of H 2 O to form -OH [46]. The bands of 1610 cm −1 could be attributable to C=O (COO − ) stretching and bending vibrations [47]. The 1070 cm −1 band corresponded to the vibration of C-O. The peaks of carboxyl and hydroxyl groups were greatly enhanced after Ce(NO 3 ) 3 modification, which facilitates the absorption of heavy metals. The FTIR analysis results were in agreement with RS as well as contact angle results.
Previous studies have shown a positive correlation between hydrophilic a tact angle for biochar [42]. Biochar had wettability and was capable of absorbin rapidly as well [43]. The hydrophilic properties of biochar were expressed by me the contact angle, as shown in Figure 5. The contact angle of the MCB was 8°, in that it was a hydrophilic material. In contrast, Ce-MCB had a contact angle of 0° a a superhydrophilic material. The results showed that the hydrophilicity of Ce-M higher than that of MCB, which is associated with the preferential orientation of lar oxygen-containing groups (e.g., hydroxyl groups) enriched on the surface of C toward water [44]. The FTIR test results also prove the presence of these polar Remarkably, the cerium oxide loaded on the Ce-MCB surface was inherently philic [45]. FTIR measurements were performed on MCB and Ce-MCB to characte functional groups present on the adsorbent surface, which were essential for the tion process of metal ions. As shown in Figure 6, several peaks were observed spectra at about 3440, 1610, 1350, and 1070 cm −1 . The bands at about 3440 cm −1 a cm −1 indicated -OH asymmetric stretching vibration. In the aqueous environme can be used as active sites for the dissociation of H2O to form -OH [46]. The b 1610 cm −1 could be attributable to C=O (COO − ) stretching and bending vibratio The 1070 cm −1 band corresponded to the vibration of C-O. The peaks of carbo hydroxyl groups were greatly enhanced after Ce(NO3)3 modification, which fa the absorption of heavy metals. The FTIR analysis results were in agreement wi well as contact angle results. The hysteresis loops of MCB and Ce-MCB were represented as magnetic pro Figure 7 shows that the saturation magnetization of MCB and Ce-MCB were fou 11.054 emu·g −1 and 7.149 emu·g −1 , respectively. Although the saturation magne The hysteresis loops of MCB and Ce-MCB were represented as magnetic properties. Figure 7 shows that the saturation magnetization of MCB and Ce-MCB were found to be 11.054 emu·g −1 and 7.149 emu·g −1 , respectively. Although the saturation magnetization intensity of the Ce-MCB was lower than that of MCB, it is sufficient to support an external magnet to magnetically separate it from the solution. The introduction of CeO 2 decreased the saturation magnetization intensity of biochar. This might be attributed to the oxidation of Ce(NO 3 ) 3 , causing the oxidation of iron in the biochar, which can be inferred from the XPS results. The magnetic properties of the biochar remained almost unchanged after absorption of Pb 2+ , indicating that the magnetic properties of the adsorbent were stable.
Int. J. Mol. Sci. 2023, 24, x FOR PEER REVIEW intensity of the Ce-MCB was lower than that of MCB, it is sufficient to support nal magnet to magnetically separate it from the solution. The introduction of C creased the saturation magnetization intensity of biochar. This might be attribut oxidation of Ce(NO3)3, causing the oxidation of iron in the biochar, which can be from the XPS results. The magnetic properties of the biochar remained almost un after absorption of Pb 2+ , indicating that the magnetic properties of the adsorbe stable.       In the Fe 2p spectrum, there were two asymmetric peaks at 711.38 eV and 725.18 eV attributed to Fe 2p1/2 and Fe 2p3/2, respectively [54]. Compared with MCB, Ce-MCB had a higher proportion of Fe 3+ on its surface. The result is consistent with the VSM findings. The Ce oxidation state on the Ce-MCB surface was further studied and the Ce3d5/2 and Ce3d3/2 spectra are shown in Figure 9i. The spectra were deconvoluted into 10 peaks, where v0, v2, u0, and u2 (peaks marked in blue) corresponded to Ce 3+ and the rest (peaks marked in red) corresponded to Ce 4+ [55,56].

Effect of Solution pH
The absorption capacity of biochar for heavy metals varies substantially with pH because the presence of Pb 2+ is influenced by the pH of the solution. Considering that Pb 2+ generates precipitation, Pb 2+ begins to precipitate to a pH of solution greater than 5.8 [57]. At solution pH values greater than 6, the Pb 2+ in solution is readily converted to hydroxide complexes, including but not limited to Pb(OH) 2+ , Pb(OH)2, Pb2(OH) 3+ , and Pb3(OH)2 4+ [58]. When the pH of the solution is around 7, the Pb 2+ almost completely In the Fe 2p spectrum, there were two asymmetric peaks at 711.38 eV and 725.18 eV attributed to Fe 2p1/2 and Fe 2p3/2, respectively [54]. Compared with MCB, Ce-MCB had a higher proportion of Fe 3+ on its surface. The result is consistent with the VSM findings. The Ce oxidation state on the Ce-MCB surface was further studied and the Ce3d 5/2 and Ce3d 3/2 spectra are shown in Figure 9i. The spectra were deconvoluted into 10 peaks, where v 0 , v 2 , u 0 , and u 2 (peaks marked in blue) corresponded to Ce 3+ and the rest (peaks marked in red) corresponded to Ce 4+ [55,56].

Effect of Solution pH
The absorption capacity of biochar for heavy metals varies substantially with pH because the presence of Pb 2+ is influenced by the pH of the solution. Considering that Pb 2+ generates precipitation, Pb 2+ begins to precipitate to a pH of solution greater than 5.8 [57]. At solution pH values greater than 6, the Pb 2+ in solution is readily converted to hydroxide complexes, including but not limited to Pb(OH) 2+ , Pb(OH) 2 , Pb 2 (OH) 3+ , and Pb 3 (OH) 2 4+ [58]. When the pH of the solution is around 7, the Pb 2+ almost completely converts to Pb(OH) 2 (s) [59]. Therefore, the initial pH of the solution was adjusted betweeñ 2 and~6. Figure 10 reveals that the pH of the initial solution significantly influenced the absorption of Pb 2+ by magnetic biochar. For both biochars, the absorption capacity of Pb 2+ increased markedly when the pH increased from 2 to 5. This may be due to the decrease in the concentration of H + ions in the solution and the deprotonation of surface groups, which favored the interaction of biochar with Pb 2+ [60]. However, between pH 5 and 6, a slight decrease in absorption capacity was observed. The variation might be explained by the presence of Pb 2+ existing in the form of Pb(OH) − , which could precipitate and become the main factor affecting the Pb 2+ removal. Compared with MCB, the absorption capacity of Ce-MCB was more significantly affected by pH. The result may be explained by the fact that the part of the Ce-MCB surface that played a dominant role in absorption was dissolved in the acidic solution, resulting in a significant decrease in the absorption capacity of Ce-MCB. When the pH increased to 5, the absorption capacity of Pb 2+ of biochar was highest. Therefore, the subsequent experiments were performed at an optimal solution initial pH of 5.

Absorption Kinetics
To evaluate absorption kinetics, the effects of contact time on the absorption of Pb 2+ by MCB and Ce-MCB are illustrated in Figure 11. The parameters of the fitting results for PFO (pseudo-first-order) and PSO (pseudo-second-order) are shown in Table 2. Although the R 2 value for the PSO (R 2 = 0.9680, 0.9985) was better than that of the PFO (R 2 = 0.9429, 0.9928), the PSO also fit the experimental data well. The absorption of Pb 2+ increased rapidly in the first 200 min and slowed in 200-500 min. After 500 min, the absorption process of the adsorbents reached dynamic equilibrium. The results revealed that chemisorption might be dominated and physical absorption might supplement the absorption process of Pb 2+ on biochar, and the theoretical maximum absorption values

Absorption Kinetics
To evaluate absorption kinetics, the effects of contact time on the absorption of Pb 2+ by MCB and Ce-MCB are illustrated in Figure 11. The parameters of the fitting results for PFO (pseudo-first-order) and PSO (pseudo-second-order) are shown in Table 2. Although the R 2 value for the PSO (R 2 = 0.9680, 0.9985) was better than that of the PFO (R 2 = 0.9429, 0.9928), the PSO also fit the experimental data well. The absorption of Pb 2+ increased rapidly in the first 200 min and slowed in 200-500 min. After 500 min, the absorption process of the adsorbents reached dynamic equilibrium. The results revealed that chemisorption might be dominated and physical absorption might supplement the absorption process of Pb 2+ on biochar, and the theoretical maximum absorption values were closer to the values of the actual absorption experiment. 0.9429, 0.9928), the PSO also fit the experimental data well. The absorption of Pb 2+ increased rapidly in the first 200 min and slowed in 200-500 min. After 500 min, the absorption process of the adsorbents reached dynamic equilibrium. The results revealed that chemisorption might be dominated and physical absorption might supplement the absorption process of Pb 2+ on biochar, and the theoretical maximum absorption values were closer to the values of the actual absorption experiment.  Figure 11. Pseudo-second-order and pseudo-first-order model of biochar to Pb 2+.
To further explore the potential absorption mechanisms of Ce-MCB and MCB, the Elovich and intra-particle diffusion models were also used to formulate the absorption kinetics, and the results are shown in Figures 12 and 13. As shown in Table 3, the intraparticle diffusion model with R 2 > 0.89 characterizes the adsorption process in stages. The Elovich model with R 2 > 0.95 (Table 4) also appropriately depicted the absorption process, accounting that the absorption of Pb 2+ on Ce-MCB was a complex process that might have  To further explore the potential absorption mechanisms of Ce-MCB and MCB, the Elovich and intra-particle diffusion models were also used to formulate the absorption kinetics, and the results are shown in Figures 12 and 13. As shown in Table 3, the intraparticle diffusion model with R 2 > 0.89 characterizes the adsorption process in stages. The Elovich model with R 2 > 0.95 (Table 4) also appropriately depicted the absorption process, accounting that the absorption of Pb 2+ on Ce-MCB was a complex process that might have a linear dependence over a wide time range. Based on the studies of former users, the intra-particle diffusion model was divided into three stages [61][62][63]. In the first stage, Pb 2+ diffused rapidly on the adsorbent surface and the absorption process occurred on the external surface. With time, the second phase began, the absorption sites were occupied, and the absorption rate gradually decreased until equilibrium. The fitted graphs for three stages deviated from the origin, indicating that chemisorption had an effect on the absorption rate. a linear dependence over a wide time range. Based on the studies of former users, the intra-particle diffusion model was divided into three stages [61][62][63]. In the first stage, Pb 2+ diffused rapidly on the adsorbent surface and the absorption process occurred on the external surface. With time, the second phase began, the absorption sites were occupied, and the absorption rate gradually decreased until equilibrium. The fitted graphs for three stages deviated from the origin, indicating that chemisorption had an effect on the absorption rate.

Absorption Isotherms
The Langmuir isotherm equation postulates that the surface of the biochar is homogeneous with the same affinities and that reaction takes place in a monolayer absorption pattern [64]. The Freundlich equation describes the multilayer sorption that occurs on heterogeneous surfaces, in which the availability of absorption sites has different absorption forces [65]. The Langmuir and Freundlich parameters for the absorption of Pb 2+ are listed in Table 5. The higher correlation coefficient values of the Langmuir model compared to the Freundlich model indicated that the Langmuir model was more suitable for describing the absorption process. As can be seen from Figure 14, the theoretical maximum absorption capacities of MCB and Ce-MCB were 29.61 mg·g −1 and 140.83 mg·g −1 , respectively. The absorption process was attributed to single-molecular-layer absorption and the active sites of biochar were relatively uniformly distributed. In addition, the separation factor (R L ) allowed for assessing the favorability of the absorption, which is defined by: R L = 1/(1 + K L C 0 ). The value of this parameter indicates the basic characteristics of the absorption process, which is irreversible (R L = 0), favorable (0 < R L < 1), linear (R L = 1), or unfavorable (R L > 1) [25]. In this study, the value of R L was calculated to be between 0.0079 and 0.023, which confirmed that the absorption process was easy to carry out. The result might be explained by the fact that the high initial concentration of the solution provides the mass transfer driving force for the absorption process. characteristics of the absorption process, which is irreversible (RL = 0), favorable 1), linear (RL = 1), or unfavorable (RL > 1) [25]. In this study, the value of RL was ca to be between 0.0079 and 0.023, which confirmed that the absorption process wa carry out. The result might be explained by the fact that the high initial concentr the solution provides the mass transfer driving force for the absorption process. ) C e (mg·L −1 ) Figure 14. Absorption isotherm of Pb 2+ adsorbed on biochars.

Reusability Studies
The absorption efficiencies of MCB and Ce-MCB for Pb 2+ after four cycles vestigated ( Figure 15). The results demonstrated that after the fourth cycle, the tion of Ce-MCB and MCB decreased from 114.74 mg·g −1 to 82.63 mg·g −1 and 27.0 to 17.47 mg·g −1 , respectively. These reductions in absorption capacity were mainl the partial loss of minerals from the adsorbent surface during the desorption pro

Reusability Studies
The absorption efficiencies of MCB and Ce-MCB for Pb 2+ after four cycles were investigated ( Figure 15). The results demonstrated that after the fourth cycle, the absorption of Ce-MCB and MCB decreased from 114.74 mg·g −1 to 82.63 mg·g −1 and 27.01 mg·g −1 to 17.47 mg·g −1 , respectively. These reductions in absorption capacity were mainly due to the partial loss of minerals from the adsorbent surface during the desorption process.

Effect of Coexisting Alkali Metal Ions
There are common metal cations (Na + , K + , and Mg 2+ ) in industrial wastewater might interfere with the removal of Pb 2+ [66]. The effects of alkali metal ions (K + , N Ca 2+ ) and strength on Pb 2+ absorption by Ce-MCB were investigated. As displ Figure 16, the presence of K + and Na + had little effect on the sorption capacity of Pb may be ascribed to the low charge density of K + and Na + , which did not compe Pb 2+ for absorption sites [67]. However, the absorption capacity of Ce-MCB for P 2+ 2+ Figure 15. Regeneration of Pb 2+ absorption on magnetic biochars.

Effect of Coexisting Alkali Metal Ions
There are common metal cations (Na + , K + , and Mg 2+ ) in industrial wastewater, which might interfere with the removal of Pb 2+ [66]. The effects of alkali metal ions (K + , Na + , and Ca 2+ ) and strength on Pb 2+ absorption by Ce-MCB were investigated. As displayed in Figure 16, the presence of K + and Na + had little effect on the sorption capacity of Pb 2+ . This may be ascribed to the low charge density of K + and Na + , which did not compete with Pb 2+ for absorption sites [67]. However, the absorption capacity of Ce-MCB for Pb 2+ was significantly affected by Ca 2+ , while in 5 mM, we can conclude that Ca 2+ had a stronger inhibitory effect on the absorption process of Pb 2+ compared to K + and Na + . On the one hand, the absorption of Pb 2+ decreased by more than 10%, and the presence of Ca 2+ formed a competitive absorption with Pb 2+ , occupying part of the absorption site of Pb 2+ . On the other hand, the presence of Ca 2+ led to the aggregation of CeO 2 nanoparticles [68], resulting in the compression of the electric double layer and the formation of a dense structure, which reduces the effective available area for biochar absorption and decreases the active sites.
There are common metal cations (Na + , K + , and Mg 2+ ) in industrial wastewat might interfere with the removal of Pb 2+ [66]. The effects of alkali metal ions (K + , Ca 2+ ) and strength on Pb 2+ absorption by Ce-MCB were investigated. As disp Figure 16, the presence of K + and Na + had little effect on the sorption capacity of may be ascribed to the low charge density of K + and Na + , which did not comp Pb 2+ for absorption sites [67]. However, the absorption capacity of Ce-MCB for significantly affected by Ca 2+ , while in 5 mM, we can conclude that Ca 2+ had a inhibitory effect on the absorption process of Pb 2+ compared to K + and Na + . On hand, the absorption of Pb 2+ decreased by more than 10%, and the presenc formed a competitive absorption with Pb 2+ , occupying part of the absorption sit On the other hand, the presence of Ca 2+ led to the aggregation of CeO2 nanopart resulting in the compression of the electric double layer and the formation o structure, which reduces the effective available area for biochar absorption and d the active sites.  Table 6 shows the maximum absorption capacity (Qm) of Ce-MCB for Pb 2 parison with those gained in other investigations. Despite the different expe conditions used, the comparison of Qm values was useful because the absorption was the criterion that provided the performance of Ce-MCB relative to other m Among the listed materials, the Ce-MCB showed excellent performance based removal efficiency.  Table 6 shows the maximum absorption capacity (Q m ) of Ce-MCB for Pb 2+ in comparison with those gained in other investigations. Despite the different experimental conditions used, the comparison of Q m values was useful because the absorption capacity was the criterion that provided the performance of Ce-MCB relative to other materials. Among the listed materials, the Ce-MCB showed excellent performance based on Pb 2+ removal efficiency.

FTIR Analysis
The hydroxyl and carboxyl functional group on the surface perform an essential role in the Pb absorption process. In the FTIR spectra of biochar after absorption (see Figure 17), the peak of Ce-MCB biochar at 3440 cm −1 (-OH bending vibration) was significantly attenuated. In addition, the peak at 1382 cm −1 (O-H bending vibration) shifted mildly to 1375 cm −1 . These changes indicated that -OH was involved in the absorption process of Pb 2+ and formed a monodentate complex on the biochar surface [75,76].The absorption peak located at 1610 cm −1 was weakened, indicating that the carboxyl group was also involved in the absorption of Pb 2+ . MCB-Pb showed a similar variation to Ce-MCB-Pb.

FTIR Analysis
The hydroxyl and carboxyl functional group on the surface perform an essen in the Pb absorption process. In the FTIR spectra of biochar after absorption (see 17), the peak of Ce-MCB biochar at 3440 cm −1 (-OH bending vibration) was signi attenuated. In addition, the peak at 1382 cm −1 (O-H bending vibration) shifted m 1375 cm −1 . These changes indicated that -OH was involved in the absorption pro Pb 2+ and formed a monodentate complex on the biochar surface [75,76].The abs peak located at 1610 cm −1 was weakened, indicating that the carboxyl group w involved in the absorption of Pb 2+ . MCB-Pb showed a similar variation to Ce-MCB

XRD Analysis
The XRD analysis of MCB and Ce-MCB after Pb 2+ absorption is shown in Fig  After the absorption of Pb 2+ , new diffraction peaks were observed on the surface char. The emerging peaks corresponded to the diffraction peaks of PbC Pb3(CO3)2(OH)2, showing the chemical reactions that occurred during the absorp Pb 2+ and the formation of PbCO3 and Pb3(CO3)2(OH)2 crystals. Therefore, it could termined that the precipitation formed on the surface of biochar was one of the nisms of Pb 2+ removal, which may be caused by the co-precipitation reaction b Pb 2+ and minerals (such as CO3 2-and HCO3 − ) [77].

XRD Analysis
The XRD analysis of MCB and Ce-MCB after Pb 2+ absorption is shown in Figure 18. After the absorption of Pb 2+ , new diffraction peaks were observed on the surface of biochar. The emerging peaks corresponded to the diffraction peaks of PbCO 3 and Pb 3 (CO 3 ) 2 (OH) 2 , showing the chemical reactions that occurred during the absorption of Pb 2+ and the formation of PbCO 3 and Pb 3 (CO 3 ) 2 (OH) 2 crystals. Therefore, it could be determined that the precipitation formed on the surface of biochar was one of the mechanisms of Pb 2+ removal, which may be caused by the co-precipitation reaction between Pb 2+ and minerals (such as CO 3 2− and HCO 3 − ) [77].

XPS Analysis
XPS was also used to analyze the absorption mechanism. XPS surveys of after absorption are presented in Figure 19. The binding energies and ratios of th peaks in the O1s spectra changed significantly. After absorption of Pb 2+ , the Carea ratio of Ce-MCB decreased from 77.52% to 55.23%, suggesting that π-π on

XPS Analysis
XPS was also used to analyze the absorption mechanism. XPS surveys of biochar after absorption are presented in Figure 19. The binding energies and ratios of the three peaks in the O1s spectra changed significantly. After absorption of Pb 2+ , the C-C peak area ratio of Ce-MCB decreased from 77.52% to 55.23%, suggesting that π-π on the adsorbent surface had cation-π interaction with Pb 2+ [78].

XPS Analysis
XPS was also used to analyze the absorption mechanism. XPS surveys of biochar after absorption are presented in Figure 19. The binding energies and ratios of the three peaks in the O1s spectra changed significantly. After absorption of Pb 2+ , the C-C peak area ratio of Ce-MCB decreased from 77.52% to 55.23%, suggesting that π-π on the adsorbent surface had cation-π interaction with Pb 2+ [78].

Relative Distributions of Absorption Mechanisms
The removal of Pb 2+ was ascribed to three fractions: Q m , Q π , and Q f . Compared with MCB, the Q m and Q f values of Ce-MCB increased significantly, while the values of Q π remained almost unchanged. As shown in Figure 20, the value of the oxygen functional groups contribution increased from 1.24 mg·g −1 to 10.37 mg·g −1 . The increase in Q f was due to the Ce(NO 3 ) 3 treatment, which introduced more oxygen-containing functional groups and enhanced the absorption properties of the functional groups. Due to the high adsorption capacity of minerals to heavy metals, the increase in the proportion of minerals caused by the loading of CeO 2 on the surface of biochar is also an important reason for the improvement of adsorption capacity. Compared with MCB, the Q m value of Ce-MCB was increased by 80.899 mg·g −1 . However, the Q π values of MCB and Ce-MCB were almost similar, indicating that the CeO 2 -doped was free of a significant effect on Q π [79]. groups and enhanced the absorption properties of the functional groups. Due to t adsorption capacity of minerals to heavy metals, the increase in the proportion of als caused by the loading of CeO2 on the surface of biochar is also an important rea the improvement of adsorption capacity. Compared with MCB, the Qm value of C was increased by 80.899 mg·g −1 . However, the Qπ values of MCB and Ce-MCB w most similar, indicating that the CeO2-doped was free of a significant effect on Qπ

Preparation of Magnetic Biochar
The coconut skin fiber was purchased from an orchard site in Haikou, province. The ingredients were washed with deionized water to remove the imp and subsequently dried in an oven at 105 °C to a constant weight. After crushi powder and passing through a 20-mesh sieve, the coconut coir was stored in a zip lock bag in the laboratory.
Coconut skin fiber (CS) of 11.22 g and Fe(NO3)3·9H2O of 4.04 g were mixed w mL of ethanol in a magnetic stirrer for 24 h. For Ce(NO3)3/Fe(NO3)3 co-modificat coconut skin of 11.22 g was mixed with 4.04 g of Fe(NO3)3·9H2O and 4.3 Ce(NO3)3·6H2O and stirred for 24 h. The suspensions were mixed in ultrasound for and then dried in oven at 65 °C. The Fe(NO3)3-loaded CS (MCS Ce(NO3)3/Fe(NO3)3-loaded CS (Ce-MCS) were dried and packed in a crucible, wh placed in a tube furnace and calcined to 600 °C with a ramp of 10 °C min −1 and flowing N2 for 2 h. The obtained biochar was named as MCB and Ce-MCB.

Characterization of the Biochars
Scanning electron microscopy (SEM, Hitachi Limited SU-70, Tokyo, Japa used to be examined the appearance and morphology of biochar samples. The

Preparation of Magnetic Biochar
The coconut skin fiber was purchased from an orchard site in Haikou, Hainan province. The ingredients were washed with deionized water to remove the impurities, and subsequently dried in an oven at 105 • C to a constant weight. After crushing into powder and passing through a 20-mesh sieve, the coconut coir was stored in a plastic zip lock bag in the laboratory.
Coconut skin fiber (CS) of 11.22 g and Fe(NO 3 ) 3 ·9H 2 O of 4.04 g were mixed with 100 mL of ethanol in a magnetic stirrer for 24 h. For Ce(NO 3 ) 3 /Fe(NO 3 ) 3 co-modification, the coconut skin of 11.22 g was mixed with 4.04 g of Fe(NO 3 ) 3 ·9H 2 O and 4.34 g of Ce(NO 3 ) 3 ·6H 2 O and stirred for 24 h. The suspensions were mixed in ultrasound for 1 hour and then dried in oven at 65 • C. The Fe(NO 3 ) 3 -loaded CS (MCS) and Ce(NO 3 ) 3 /Fe(NO 3 ) 3loaded CS (Ce-MCS) were dried and packed in a crucible, which was placed in a tube furnace and calcined to 600 • C with a ramp of 10 • C min −1 and under flowing N 2 for 2 h. The obtained biochar was named as MCB and Ce-MCB.

Characterization of the Biochars
Scanning electron microscopy (SEM, Hitachi Limited SU-70, Tokyo, Japan) was used to be examined the appearance and morphology of biochar samples. The specific surface areas (SSAs), total pore volume (V t ), and porosity were measured by an N 2 absorption and desorption analyzer (Quantachrome, QI3, Boynton Beach, FL, USA) at 77 K. The surface organic functional groups were characterized using Fourier transform infrared spectroscopy (FTIR, Thermo Fisher Nicolet iS50, Waltham, MA, USA). Raman spectroscopy (Raman, HORIBA Jobin Yvon LabRAM HR800, Montpellier, French) recorded the degree of defects and graphitization. X-ray diffraction (XRD, PANalytical X'Pert Pro MPD, Heracles Almelo, The Netherlands) was used to characterize the crystalline structure of biochar. The surface composition and chemical valence of biochar was analyzed by X-ray photoelectron spectroscopy (XPS, Scientific Thermo Fisher K-Alpha, Waltham, MA, USA). Hydrophilic properties were calculated using the contact angle gauges. The zeta potential of biochar was determined using the laser particle sizer (Zeta, Malvern nano ZS & Mastersizer, Malvern, UK). A vibrating sample magnetometer (VSM, Lake Shore Lake Shore 7404, Westerville, OH, USA) was used to detect the magnetization of biochar.

Absorption Experiment
The Pb(NO 3 ) 3 of 1.598 g was dissolved in deionized water to configure a solution with a concentration of 1 g L −1 . The solution was diluted with ultrapure water to the required concentration and the initial pH (LICHEN pH-100, Changsha, China) of the solution was controlled at 5 by 1 M NaOH and 1 M HCl. The experimental conditions were adjusted to 5 ± 0.2 and the ion concentration was 200 mg·L −1 (the absorption amount was close to saturation at the ion concentration of 200 mg·L −1 ).
Absorption kinetics of Pb 2+ onto 0.3 g of biochar were placed in conical flasks containing 300 mL of aqueous solution. In a typical reaction, the flask was shaken in a water bath shaker with a fixed speed of 200 rpm. At predetermined time intervals, 2 mL of solution was collected and its residual Pb 2+ concentration was detected by ICP-OES.
Absorption isotherms of Pb 2+ onto 10 mg of biochar were added to the centrifugal tubes with 10 mL of Pb 2+ solution where the concentration was from 0 to 1000 mg L −1 . The tubes were shaken at 200 rpm in a water bath shaker for 48 h. After the absorption equilibrium, all samples were filtered, and the heavy metal concentrations were determined by the same method.
To investigate the reusability of magnetic biochar in a real environment, the regeneration was conducted. In each cycle, the Pb 2+ adsorbed MCB or Ce-MCB was magnetically separated from the absorption mixture and then transferred to another conical flask containing 300 mL of CH 3 COONa aqueous (1 mol·L −1 for a 2 h desorption). The desorption-absorption experiment was repeated for 4 cycles.
Investigating the influence of pH value on absorption behavior, 10 mL Pb 2+ (200 mg L −1 ) solutions were added in centrifugal tubes. The initial pH of the solution was adjusted to 2.0-6.0 by droplets of 0.1 M HCl and 0.1 M NaOH. In the test for the effect of co-existing alkali metal ions, the solution with different concentrations of K + /Na + /Ca 2+ was added to the Pb 2+ (200 mg L −1 ). An amount of 10 mg of biochar was added to the solution and the tubes were shaken at 200 rpm for 48 h. The Pb 2+ concentration in all samples was detected by ICP-OES.

Model Fitting
The biochar equilibrium absorption amount q t (mg g −1 ) of Pb 2+ was calculated by Equation (1): where C 0 (mg L −1 ) represents the initial concentration of Pb 2+ ; C t (mg L −1 ) is the concentration of Pb 2+ in the solution at time t (h); V (mL) is the volume of absorption solution; M (mg) is the mass of biochar; q t (mg g −1 ) is the Pb 2+ -adsorbed amount at a time t (min).
To explain the details of absorption kinetics, the pseudo-first-order kinetic model (PFO), pseudo-second-order kinetic model (PSO), Elovich model, and intra-particle diffusion model were used to describe the absorption kinetics, and the results of the fits are shown below [51,80].
PFO : q t = q e 1 − e −k 1 t PSO : q t = k 2 q 2 e t 1 + k 2 q e t Elovich : q t = 1 β ln(αβ) + 1 β lnt (4) Intra − particle diffusion : q t = k id t 1/2 (5) where k 1 is the absorption rate constant of PFO; k 2 represents the equilibrium rate constant of PSO; q e (mg g −1 ) is the Pb 2+ adsorbed amount at equilibrium; α is the initial absorption rate constant; β is the desorption rate constant; k id (mg·g −1 ·min −1/2 ) is the intra-particle diffusion rate constant. The models of Langmuir and Freundlich were used to describe the absorption isotherm [81]: Langmuir : q e = Q 0 K L C e 1 + K L C e Freundlich : q e = K F C 1/n e where K F and K L represent the absorption rate constants of the Langmuir and Freundlich equations, respectively; Q 0 is the Langmuir static theoretical absorption capacity; C e is the concentration of equilibrium adsorbent in the aqueous phases; n is the isothermal constant of the Freundlich isotherm curvature.

Quantitative Analysis of the Different Absorption Mechanisms
The absorption mechanism of Pb 2+ was composed of three parts: surface complexation of functional groups (Q f ), mineral precipitation (Q m ), and coordination of metal-π-electron (Pb 2+ -π) interaction (Q π ).
The biochar was acid-washed and demineralized for removal, at which point there was no change in the functional groups on the surface of the biochar. The reduced absorption capacity during the de-ashed biochar was the contribution of the minerals. The mechanism of absorption following de-ashed biochar includes oxygen functional groups and π interaction. During the contribution of oxygen functional groups, hydroxyl and carboxyl groups released H + into solution by the reaction. Therefore, the pH of the solution was measured before and after absorption of demineralized biochar, the amount of H + released was calculated, and, accordingly, the amount of Pb 2+ adsorbed by the functional group complexation (Q f ) was calculated. The remainder of de-ashed biochar was considered to be π-electron interaction (Q π ), as shown in Equation (9). [57] Q m = Q e − Q a (8) where Q a is the absorption capacity of biochar after HCl washing, Q m is the absorption by mineral precipitation, Q e is the total absorption, Q π is the absorption by π-electron interaction, and Q f is the absorption by complexation of oxygen-containing functional groups.

Conclusions
The combination of magnetic coconut coir biochar and CeO 2 has proven to be a valuable option for creating high-capacity and reusable adsorbents. FTIR, XRD, and XPS analysis demonstrated that Ce(NO 3 ) 3 modification greatly increased the content of the inorganic mineral fraction and oxygen-containing functional groups of the biochar, which provided more active sites for the adsorption of Pb 2+ . The VSM results showed that the Ce-MCB had sufficient magnetic properties to readily achieve magnetic separation. The modified adsorbent displayed enhanced adsorption capacity for Pb 2+ with a maximum theoretical adsorption capacity of 140.83 mg·g −1 , which was 4.8 times higher than that of MCB. Ce-MCB exhibited good reusability characteristics in sequential cycling experiments, maintaining a high adsorption capacity after four cycles still. Additionally, a comprehensive characterization of the Ce-MCB after Pb adsorption revealed that the primary absorption mechanism of Ce-MCB was the acidic oxygen-containing functional group complexation (Q m = 98.11 mg·g −1 ), π-electron interaction (Q π = 6.26 mg·g −1 ), and inorganic precipitation (Q f = 10.37 mg·g −1 ). These results demonstrate the outstanding performance of Ce-MCB in biomass recycling for environmental remediation.