Adsorption Behaviour and Kinetics of Zearalenone on Hydroxyl-Fe-Al-Intercalated Montmorillonite

Pristine montmorillonite (Mont) was used as raw materials to prepare hydroxyl-Fe-pillared Mont, hydroxyl-Al-pillared Mont, and hydroxyl-Fe-Al-pillared Mont composites. By varying the OH/Fe and Fe/Al molar ratios during the preparation of the pillared Mont, the adsorption capacity of zearalenone (ZEA) and the kinetics were elucidated. .e characterization of X-ray diffraction (XRD) and Fourier transform infrared (FT-IR) spectroscopy reveals the adsorption mechanism of pristine and modified Mont. .e results indicated that the ZEA adsorption capacity is Mont (0.05mg/g)<< 1.5OH/Fe-Mont (0.28mg/g) <<OH/Al-Mont (0.51mg/g)< 0.5Fe/Al-Mont (0.56mg/g) in the condition of pH� 8 and 37°C, in which both 0.5Fe/Al-Mont and OH/Al-Mont reached maximum adsorption capacity and 1.5OH/Fe-Mont attained 5 times the capacity of Mont. Adsorption isotherm studies revealed that Freundlich adsorption isotherms best represented the experimental data. .e kinetic data for ZEA adsorption revealed that the Mont adsorption capacity for ZEA equilibrates in 1 hour and is best described using the pseudosecond-order rate equation..e XRD analysis indicated that the amplification of Fe-dominant pillared Mont interlayer spacing is the main reason for the observed increases in the adsorption capacity of ZEA, while Al-dominant pillared Mont has a relatively stable Keggin structure; therefore, interlayer spacing is not the primary mechanism for changes in the adsorption capacity of both OH/Al-Mont and Al-dominant pillared Mont. An FT-IR analysis demonstrated that cationic exchange was the dominant mechanism that allowed ZEA and hydroxyl-Al ions to enter theMont interlayers, while this cationic exchangemechanismwas not the dominant mechanism used by hydroxyl-Fe entering the Mont layers.


Introduction
Mycotoxins are toxic and harmful metabolites produced by fungus or mould in suitable conditions and mainly consist of aflatoxin, zearalenone, ochratoxin, and fumagillin [1][2][3][4][5][6]. According to a report released by the United Nations Food and Agriculture Organization, approximately 25% of crops globally are contaminated by mycotoxins, resulting in major economic losses [4]. In China, this contamination is in excess of 60-70%, especially in the southern and eastern regions [7]. erefore, resolving mycotoxin contamination of foodstuffs is a global challenge [8].
Zearalenone (ZEA) is one of the most prevalent mycotoxins in contaminated grain and is produced as a secondary metabolite by a variety of fungi within the Fusarium genus [9,10]. ZEA is a toxin that exhibits behaviour similar to oestrogen, which readily and irreversibly binds to intrauterine oestrogen receptors. is binding results in significant harm to the reproductive physiology of livestock, which calls for immediate mitigation strategies [11][12][13]. Currently, the removal of mycotoxins through both physical and chemical means destroys the nutritional contents in food, whereas biological treatments are time-consuming. erefore, simple adsorption is considered to be the most effective method [14][15][16].
Montmorillonite (Mont), the main mineral component of bentonite, possesses a high ion exchange capacity due to the intrinsically layered structure of this mineral in which high-valence cations within voids are readily replaced with low-valence ions [17]. To date, most research has focused on the removal of ZEA through the use of organic cationmodified Mont, despite its environmental risks of organic cations. In contrast, there has been no report on the adsorption characteristics and mechanism of ZEA removal using inorganic hydroxyl-Fe-Al-composite-pillared Mont [11,18,19]. e present study focused on the use of Mont, hydroxyl-Fe-modified Mont (OH/Fe-Mont), hydroxyl-Al-modified Mont (OH/Al-Mont), and hydroxyl-Fe-Al compoundmodified Mont (Fe/Al-Mont) in the in vitro adsorption of ZEA, and the capacity of and applicable model for adsorption to both Mont and inorganically modified Mont were investigated. e effects of pH, time, temperature, and ZEA initial concentration on the adsorption of ZEA were characterized by X-ray diffraction (XRD), Fourier transform infrared (FT-IR) spectroscopy, and other methods.

Experimental Materials.
High purity ZEA standards and Mont were obtained from Sigma-Aldrich, USA; the ion exchange capacity (CEC) of Mont is 24.6 mmol/100 g; the molecular formula of ZEA is C 18 H 22 O 5 , with a molecular weight of 318.36, pK a1 of 7.62, and a log K ow of 3.66 [17]. All of the other reagents were purum or chromatography grade. A ZEA stock solution (250 mg/L) was prepared with a mixture of acetonitrile/methanol (1 : 1) and stored in the dark at −20°C; deionized water (18 MΩ·cm) was used in all experiments.

Adsorbent Characterization.
Powder X-ray diffraction (XRD) was performed to investigate the crystal structure of the samples on a Rigaku MiniFlex 600 X-ray diffractometer with Ni-filtered Cu Kα irradiation (α �1.5406Å). And data were recorded at a scan rate of 0.8 sec/step in the range from 5°to 20°. Fourier transform infrared (FT-IR) spectra of the samples were recorded on a ermo Scientific Nicolet iS10 spectrometer by using KBr pellets. e scanning electron microscope (SEM) images were taken through a SUPRA 55 instrument (Zeiss Sigma). Specific surface area analysis (BET) is the use of N2 low-temperature adsorption and desorption to determine the specific surface area, pore volume, and pore size distribution of the sample; the sample is prebaked at 90°C and then degassed at 150°C for 4 hours for analysis. X-ray photoelectron spectroscopy (XPS) is the use of X-ray photoelectron spectroscopy to qualitatively analyze the element types of substances (instrument performance parameters: aluminum target (photoelectron energy hv � 1486.6 eV), energy resolution 0.6 eV, and spatial resolution <3 um), collect the full scan spectrum of 2-1202 eV of the sample, and collect the narrow scan spectrum of the relevant orbits of each element. ermal analysis research (TG-DSC) is to use the thermal analysis system-synchronous thermal analyzer to study the phase transition and reaction enthalpy of the sample and to determine its characteristic parameters. e test method is to put the sample in still air, set the program heating rate to 10°C/min, and measure the temperature range from room temperature to 1000°C.

ZEA Adsorption
Test. 0.100 g of Mont and modified Mont adsorbent was used; the solution volume was 20.0 mL; samples were wrapped in aluminium foil to prevent exposure to light and placed in a temperature-controlled oscillator set to 170 rpm. e samples were then centrifuged at 4000 rpm for 5 minutes, and the amount of ZEA remaining in solution was analysed via HPLC (Agilent 1260 HPLC). e ZEA calibration curve was established using 9 standards with a linear correlation coefficient of r 2 > 0.999. e equilibrium adsorption experiments were conducted with a fixed oscillator time of 24 hours and a temperature of 37°C. In the adsorption isotherm studies, 20 mL of ZEA solution at various concentrations (0.1, 0.25, 0.5, 1, 2.5, and 5 mg/L) was added to different adsorbents at 25°C. e effects of solution pH (2,4,6,8,10) at 25°C and temperature (15,25,35,45, 55°C) on the adsorption characteristics were investigated with various adsorbents. Adsorption kinetics studies were conducted by first adding various adsorbents to 20 mL of ZEA (5 mg/L, pH 8, 25°C), and then aliquots were taken after centrifugation at time intervals of 0.25, 0.5, 0.75, 1, 2, 4, 8, 12, and 24 hours to determine the ZEA concentration.

SEM Analysis.
e SEM images of the original montmorillonite and pillared montmorillonite before and after adsorbing ZEA are shown in Figure 1. It can be seen that the pore structure of montmorillonite changes to a certain extent after adsorption. Among them, K10-Mont adsorbs ZEA, the larger pores are more blocked, the mesopores are less, and the surface fine particles are increased. e pores of 1.5 OH/Fe-Mont samples are filled with a certain amount of flocs, the pore size becomes smaller, and the flocs on the clay surface decrease after adsorption, and the macropore density decreases. e smaller floc particles on the surface are reduced, thereby making the surface of montmorillonite smoother. After adsorption of ZEA on 0.5 Fe/Al-Mont samples, the density of the larger pore diameter decreases, the macropores are blocked, and the spherical particles on the surface increase, indicating that the ZEA molecules enter the mineral interlayer domain.

BET Analysis.
It can be seen from Table 1 that the specific surface area of OH/Fe-Mont is greater than K10-Mont, but the total pore volume and pore size are less than K10-Mont. e specific surface area of OH/Al-Mont and hydroxyl-aluminum-doped hydroxyiron-aluminum pillared montmorillonite (Fe/Al≤0.5) is less than K10-Mont, and the total pore volume and pore size are also less than K10-Mont. e maximum BET specific surface area of 1.5OH/Fe-Mont reaches 271.9 m 2 /g and the pore volume reaches 0.347 cm 3 /g, but the pore size is smaller at 5.11 nm. Figure 2 shows the isotherms of nitrogen adsorption and desorption of hydroxyiron-pillared montmorillonite and the isotherms of nitrogen adsorption and desorption of hydroxyiron-aluminum-pillared montmorillonite, respectively. It can be seen from Figure 2 that the adsorption isotherms of pillared montmorillonite are relatively close in shape, similar to the type II adsorption isotherms in the BDDT classification, and are typical of porous media adsorption. When the relative pressure is between 0.05 and 0.45, the adsorption amount increases gently, indicating that the pore size of montmorillonite is continuously distributed. When the relative pressure is greater than 0.45, the amount of adsorption increases rapidly, and the adsorption isotherm warps, which is caused by capillary condensation in the larger pores [23].
Desorption branch of the low-temperature nitrogen adsorption isotherm of the sample is processed, and the pore volume distribution result of the obtained sample is shown in Figure 3. e most probable pore diameters of K10-Mont and OH/Fe-Mont are all around 3.6 nm, and both belong to the mesopore range (mesopores). e pore volume of OH/ Fe-Mont is improved compared to K10-Mont, but it is not obvious, and the maximum pore volume can be increased by 50% (1.5OH/Fe-Mont), so this study believes that the pillaring agent OH/Fe effect is to increase the number of mesopores, which has a significant effect on the increase in pore volume. e OH/Al-Mont's most achievable pore diameter is 3.609 nm, and its most achievable pore volume is 0.0264 cm 3 /g. Compared with K10-Mont, the most achievable pore volume is significantly improved. After the OH/Fe pillaring agent is added to the OH/Al pillaring agent, when the Fe/Al molar ratio is 0.5, the most permissible pore volume is 0.0222 cm 3 /g. Figure 4 is a TG-DSC chart of K10-Mont, OH/Fe-Mont, Fe/Al-Mont, and OH/Al-Mont. ese four samples have similar TG curves. When the temperature of K10-Mont reaches 60°C, a large endothermic valley begins to appear on the DSC curve, and the thermogravimetric curve drops rapidly in this interval. Because the K10-Mont absorbs heat, a large amount of attached water and interlayer water escape. When the temperature reaches above 600°C, a broad endothermic valley appears on the DSC curve. When the temperature is around 650°C, the K10-Mont dehydroxylation endotherm will produce an endothermic valley. When the temperature continues to rise above 800°C, the montmorillonite lattice will be destroyed, showing an amorphous body, and there will also be absorption hot valley. ere is no obvious temperature division between these two processes, which will cause the endothermic valleys to overlap, so a wide endothermic valley is formed. When montmorillonite is introduced into hydroxyiron and hydroxyaluminum pillaring agent, the thermal stability is enhanced, and the thermal stability of hydroxyiron pillared montmorillonite is better than that of hydroxyl-aluminum pillared montmorillonite.

XPS Analysis.
e XPS spectrum of the original montmorillonite and pillared montmorillonite before and after the adsorption of ZEA is shown in Figure 5, and the partial element spectrum is shown in Figures 6 and 7. It can be seen from the full spectrum of the three montmorillonites (K10-Mont, 1.5OH/Fe-Mont, 0.5Fe/Al-Mont) that the Fe signal of the original montmorillonite K10-Mont is very weak. After aluminum struts, the signal of Fe characteristic peak is obviously enhanced, indicating that the Fe content near the surface increases. After the adsorption of ZEA, the Fe content decreased again, indicating that after ZEA was adsorbed to the pillared montmorillonite, Fe was replaced, which is consistent with the XRD and FTIR results. To further study the adsorption mechanism of iron and ironaluminum pillared montmorillonite, the characteristic elements of the two pillared montmorillonite were analysed in detail. Figure 6 shows the changes of the binding energies of O1s, Al 2p, Si 2p, and Fe 2p before and after adsorption of ZEA by hydroxyiron pillared montmorillonite. It can be seen from Figure 7(a) that after the adsorption of ZEA, Fe is replaced by ion exchange, the content decreases sharply, and the binding energy rises from 712.23 eV to 712.74 eV. erefore, Fe participates in the adsorption of ZEA as a lost electron. Figure 7 shows the inner layer of oxygen 1s electrons (O1s), the inner layer of aluminum 2p electrons (Al2p), the inner layer of silicon 2p electrons (Si2p), and iron XPS spectrum of layer 2p electrons (Fe2p). It can be seen from   Journal of Nanotechnology hydroxyiron-pillared montmorillonite contributed greatly to the negative charge movement on the surface of montmorillonite during the adsorption process, while the ironhydroxyaluminum pillared montmorillonite contributed the most to iron. Most of the iron in the former is removed from montmorillonite, while the latter has limited O1s contribution. e difference in adsorption mechanism leads to a difference in the amount of ZEA adsorption.

XRD Analysis.
Both the XRD patterns and interlayer distances d(001) of OH/Fe-Mont, OH/Al-Mont, and Fe/Al-Mont are shown in Figure 8. It can be observed from the XRD patterns that while modified and unmodified Mont exhibit similar characteristic XRD peaks, characteristics of coexposed (001) facets peak such as the 2θ, peak full width at half maximum, and diffraction peak intensity changed significantly. is result indicates that the hydroxyl pillar modification process significantly altered the overall structure of Mont, resulting in a significant change in the d(001) of both OH/Fe-Mont and Fe/Al-Mont.
As illustrated in Figure 8(a), the d(001) of Mont is 1.19 nm, whereas the adsorbent 0.6 OH/Fe-Mont exhibited a maximum d(001) of 1.62 nm.
is increase in interlayer distance was observed to occur in two stages: the d(001) increased gradually when the OH/Fe molar ratio was less than 0.8; however, once the OH/Fe molar ratio exceeded 0.8, the d(001) was observed to increase rapidly until it reached a maximum of 1.62 nm at an OH/Fe molar ratio of 1.5. is result indicates that the primary hydrolysate of Fe ions had partially intercalated into the Mont particle layer, resulting in an increase in interlayer distance. When the OH/Fe molar ratio was increased to 2, the d(001) was observed to decrease to 1.54 nm. A rise in pH due to a large OH/Fe molar ratio in solution led to the precipitation of Fe hydroxide, which covered much of the Mont surface and rendered the pillared structure ineffective. For all of the samples, none of the XRD patterns exhibited any pillared structures with a d(001) of 2.5 nm ± 0.4 nm, which has been reported in various publications.
is observation agrees with the perspective of Diekman et al. [24], who hypothesized that unlike Al cations, which can form stable, consistent-sized structures (Keggin structure) after hydrolysis, the hydrolysates of Fe cations vary in size and consistency, rendering the formation of pillared structures difficult. Figure 8(b) indicates that X-ray diffraction patterns basic of hydroxyl-Fe-Al-pillared remained consistent with hydroxyl-Al-pillared montmorillonite when Fe/Al ≤ 0.05, the d(001) value of Fe/Al-Mont slightly are higher than the hydroxyl-Al free hydroxyl. is is due to the ion radius of Fe 3+ (0.064 nm) > Al 3+ (0.051 nm), causing d(001) slightly larger, but the d(001) remained consistent at approximately 1.74 nm ± 0.1 nm, which does not agree with the range of 2.3 nm ± 0.1 nm reported in the literature [25].
is discrepancy may be attributed to inconsistencies in the pillar structure resulting from differences in experimental conditions. e d(001) was observed to decrease from 1.70 to 1.55 nm when the Fe/Al ≥ 0.10, which indicates that the interlayer spacing no longer exhibits the Keggin structure.
is observation can be attributed to the fact that the addition of Fe destroys the OH/Al-Mont structure, forming a composite material that consists of polymeric Fe 3+ structures. is structural change is reflected in the change in interlayer spacing, and with an increasing rate of Fe, the pillared Mont structure becomes dominated by OH/Fe, thus reducing the interlayer spacing.

FT-IR Analysis.
e FTIR spectra and analysis results of Mont, 1.5OH/Fe-Mont, OH/Al-Mont, and 0.5Fe/Al-Mont before and after ZEA adsorption are depicted in Figure 9. Figure 9 indicates that hydroxyl-Fe-Al-pillared Mont exhibited a vibration peak at 1384 cm −1 prior to ZEA adsorption, which suggests the presence of NO − 3 ions despite repeated centrifugation/washing cycles. With the increase of the content of the iron in the montmorillonite, the needed charge to balance the positive is also increased, which means that the number of NO − 3 entering the montmorillonite was increased. e NO − 3 concentration in the solution of after the column is lower than that of before the column (37.2 mg/l), which is verified by the NO − 3 ion as counter-ions to the positively charged Fe hydrolysate polymers that were located outside of the Mont interlayers. is result shows that much of the iron hydrolysate polymer did not enter the Mont interlayer through ion exchange. e presence of NO − 3 ions thus bestows an anionic exchange functionality upon  hydroxyl-pillared Mont, allowing anions to enter Mont to give rise to new functionalities. Research by Akin and Zeng has also confirmed this conclusion [25,26]. e vibrational peak at 1384 cm −1 in OH/Al-Mont was comparatively weak, which indicates that only a small amount of NO − 3 ion is present. is result occurs mainly because hydroxyl-Al ions enter the Mont spacing through ion exchange, and NO − 3 ions escaped the Mont interlayers during this process [24]. e same 1384 cm −1 absorption peak was observed to weaken significantly and even disappear after the ZEA adsorption assays, which suggests that NO − 3 ions escaped the Mont interlayers by exchanging with the relevant ion of ZEA, confirming that ion exchange is the dominant mechanism of ZEA adsorption onto Mont adsorbents [27]. Figure 10 presents the equilibrium adsorption capacities of pristine Mont and modified Mont with differing OH/Fe and Fe/Al molar ratios assayed after 24 hours of adsorption. It can be observed from this analysis that pristine Mont (with an OH/Fe molar ratio of 0) exhibited an equilibrium adsorption capacity of 0.05 mg/g, whereas the adsorption capacity of OH/Fe-Mont increased with increasing OH/Fe molar ratios up to <1.5, reaching a maximum ZEA adsorption capacity of 0.28 mg/g when the OH/Fe molar ratio was at 1.5. At this molar ratio, there was a 5-fold increase in the adsorption capacity compared to pristine Mont. At OH/ Fe molar ratios >1.5, the adsorption capacity was observed to decline. e equilibrium adsorption capacity of hydroxyl-Al-pillared Mont (i.e., Fe/Al molar ratio of 0) was measured to be 0.51 mg/g, whereas the adsorption capacity of Fe/Al-Mont increased with increasing Fe/Al molar ratios up to <0.5, reaching a maximum of 0.56 mg/g at a Fe/Al molar ratio of 0.5. is value is a 10-fold increase in the adsorption capacity compared to pristine Mont and is only slightly higher than hydroxyl-modified Al-pillared Mont [28].

Effects of OH/Fe, OH/Al, and Fe/Al Molar Ratios.
Changes in the d(001) of pillared Mont as measured using XRD can be used to explain the impact of the OH/ Fe molar ratio on the ZEA adsorption capacity. e adsorption capacity was observed to correlate with the d(001) of Mont: the maximum observed ZEA adsorption capacity coincided with the maximum d(001) value at an OH/Fe molar ratio of 1.5. is demonstrates that the OH/ Fe pillar modification of Mont significantly improves the ZEA adsorption characteristics, up to a 5-fold increase in adsorption capacity. As indicated in Figure 4, compared with the adsorption to OH/Fe-Mont, a different trend in the characteristics of ZEA adsorption to Fe/Al-Mont is observed, which is likely due to a complex mechanism associated with a composite-pillared structure that warrants further investigation. From the same Figure 4, it can also be observed that when the molar ratios of both OH/Fe and Fe/Al are less than 1.   Journal of Nanotechnology adsorption. At higher ZEA concentrations, the competition for adsorption sites on the adsorbents increases significantly, thereby increasing adsorption. According to Figure 11, the ZEA adsorption capacities are ranked as follows, regardless of the ZEA initial concentration: is result indicates that the ZEA adsorption capacity of Mont increased significantly after modification; therefore, the hydrolysed Fe, hydrolysed Al, and hydrolysed Fe/Al pillar modification of Mont significantly increased the ZEA adsorption capacity. e experimental data obtained were modelled using a Langmuir adsorption isotherm (1) and a Freundlich adsorption isotherm [31]: In the above equation, q e is the equilibrium adsorption capacity (mg/g), C e is the equilibrium concentration (mg/L), q max is the maximum adsorption capacity (mg/g), K L is the Langmuir adsorption coefficient (L/mg), and K F is the Freundlich adsorption coefficient (mg 1−1/n ·L 1/n ·g −1 ). e parameters used in both Langmuir and Freundlich isotherms are summarized in Table 2. It can be inferred from Table 2 that the Freundlich model (r 2 ≥ 0.95) is a better fit than the Langmuir model (r 2 < 0.05) for Mont, 1.5OH/Fe-Mont, OH/Al-Mont, and 1.5Fe/Al-Mont regarding the ZEA adsorption. e Langmuir model is a description of a particle monolayer adsorption with identical adsorption sites, and every adsorption process is completely independent. From Table 1, it is apparent that the Langmuir adsorption model is not representative of both pristine Mont and modified Mont, which indicates that the ZEA adsorption process is complex in multimolecular layer adsorption.
is result agrees with recent research, which also suggests that ZEA undergoes multilayer adsorption in which both the surface and interlayer spacing of the Mont are available adsorption sites. As a result, ZEA may adsorb onto the surface of adsorbent materials through surface complexation reactions or through spatial interpolation layer adsorption, which agrees with the current data and suggests that the Freundlich model is a better reflection of the ZEA adsorption processes on the surface of Mont. In the Freundlich model, the ease of adsorption is described by the parameter 1/n, where a value <1 or close to 1 indicates high adsorption probability. is also explains   that modified Mont can be used as an effective adsorbent to remove ZEA [32][33][34].

Effects of pH and Temperature.
e effect of pH on the ZEA adsorption capacity is illustrated in Figure 12, which shows that between the pH range of 2-8, the adsorption capacity increases with increasing pH value, and the capacity of modified Mont is significantly greater than pristine Mont. e correlation between pH value and adsorption capacity is represented in two stages: when pH < 8, the adsorption capacity increases with increasing pH value; when pH > 8, the adsorption capacity decreases with increasing pH. is observation can be attributed to the fact that ZEA possesses a chemical structure (   O   O   O OH HO ) similar to phenol and is considered a weak acid. Because pK a1 of ZEA is 7.62, under conditions where pH < 7.62, the ZEA molecules are positively charged; therefore, under low pH conditions, the number of excess H + ions in solution reduces the number of available adsorption sites within the interlayer spacing of Mont, thus reducing the overall adsorption of ZEA [35,36]. With increasing pH, the number of available adsorption sites increases up to a maximum pH of 8. With further increases in pH, the presence of hydroxide in solution begins to break down the polymer adsorption characteristics, thereby reducing the overall adsorption capacity of Mont.
e effect of solution temperature on the ZEA adsorption capacity of Mont is depicted in Figure 13. Initially, the ZEA adsorption capacity increases with increasing temperature and peaks at a temperature of 35°C, after which the adsorption capacity decreases with further increases in temperature. is result can be attributed to the increase in reactivity of the unsaturated active sites in Mont with increasing temperature within the range of 15°C to 35°C, which is conducive to the formation of a bond with ZEA. In contrast, at temperatures above 35°C, excess heat can cause bond breakage, leading to lower adsorption. Because the pH  Wave number (cm -1 ) Figure 9: FT-IR spectra before and after ZEA adsorption (+ZEA represents adsorption) on hydroxyl-Fe-Al-pillared Mont. value in livestock is in the range of 6.5-7.5, and the body temperature is 37-42°C, the use of Mont as an adsorbent in vivo can be considered because the optimum performance parameters of Mont lie within this range [33][34][35][36][37]. Figure 14 displays the ZEA adsorption capacity of Mont as a function of time. It can be observed that, at any point in time, the adsorption capacities of the adsorbents are consistently ranked as follows: Mont << 1.5OH/Fe-Mont << OH/Al-Mont < 0.5Fe/Al-Mont. e relationship between the adsorption quantity and time can be described using a kinetic model, and it was found that a pseudo-second-order kinetic model best fits the experimental data ( Figure 14). is model has been widely used in the solution adsorption of ZEA and other pollutants [38,39].

Conclusions
(1) e XRD analysis revealed that the interlayer spacing d(001) of hydrolysed Fe-pillared Mont increases gradually with increasing OH/Fe molar ratios, up to a ratio of ≤1.5, while the d(001) decreases with increasing Fe/Al molar ratios in hydrolysedFe/Al-composite-pillared Mont. e amplification of Fe-dominant pillared Mont interlayer spacing is the main reason for the observed increases in the adsorption capacity of ZEA. However, aluminium pillared Monts possess a relatively stable Keggin structure in which the adsorption capacity is not dictated by interlayer spacing. e FT-IR analysis clearly indicated that the mechanism in which ZEA and Al ions enter Mont is predominantly due to cationic exchange, whereas the migration of hydrolysed Fe into the interlayer spacing of Mont is not governed by ion exchange.
(2) e difference in the ZEA adsorption capacities between hydrolysed Fe and Al compared to a composite-pillared structure can be ranked as follows: Mont (0.05 mg/g) << 1.5OH/Fe-Mont (0.28 mg/g) << OH/Al-Mont (0.51 mg/g) < 0.5Fe/ Al-Mont (0.56 mg/g); both 0.5Fe/Al-Mont and OH/ Al-Mont possess the greatest adsorption capacity, which is approximately an order of magnitude greater than pristine Mont. Hydroxyl Fe Mont with a molar ratio of 1.5 (1.5OH/Fe-Mont) exhibited a 5fold increase in adsorption capacity compared to pristine Mont.
(3) Adsorption isotherm studies confirmed that the Freundlich adsorption model well represents (r 2 > 0.95) the ZEA adsorption of Mont. In the model, the parameter 1/n < 1 gave a value between 0.8 and 1, which indicates that ZEA is readily adsorbed. (4) e ZEA adsorption capacity increases with increasing pH at pH values ≤8. At pH > 8, the adsorption capacity decreases with further increases in pH. e optimum performance temperature was found to be within a biological range of approximately 35°C. (5) ZEA adsorption onto Mont was found to equilibrate within an hour. Kinetic studies and parameters demonstrated that the adsorption process can be described using pseudo-second-order kinetics (correlation coefficient R 2 > 0.99). e equilibrium adsorption capacity q e of the various adsorbents was found to be Mont (0.02 mg·g −1 ) << 1.5OH/Fe-Mont (0.18 mg·g −1 ) < OH/Al-Mont (0.25 mg·g −1 ) << 0.5Fe/ Al-Mont (0.41 mg·g −1 ). e mechanisms of interaction between pristine Mont and ZEA and between hydroxyl-Fe-Al-pillared Mont and ZEA were elucidated in this study, which can be used to improve the removal efficacy of mycotoxins. e use of hydroxyl-pillared Mont in the in vivo removal of ZEA from  animal gastrointestinal tracts warrants further investigation. Hydroxyl-iron, hydroxyl-aluminum, and hydroxyl-aluminum-iron are supported on montmorillonite and have a large amount of positive charge on the surface. e ZEA molecule has two phenolic hydroxyl groups, which can be regarded as weakly acidic molecules. When the pH is 8, ZEA dissociates to a greater extent. e anions formed by ZEA dissociation can chemisorb with the positive charge on the side of montmorillonite. e increase in pH makes the competitive adsorption of hydrogen ions and ZEA weaker, so the amount of ZEA adsorbed by the adsorbent gradually increases.

Data Availability
e data used to support the findings of this study are included within the article.

Conflicts of Interest
e authors declare that there are no conflicts of interest regarding the publication of this paper.