Materials

Methods

Adsorption Experiments

Adsorption of glyphosate on Zn₂Al-LDO was investigated in batch experiments in triplicate. Standard glyphosate solutions with initial concentrations of 10, 20, 40, 60, 80, 100, 120, 150, 200, 250, and 300 μg mL⁻¹ were prepared by diluting the 500 μg mL⁻¹ glyphosate stock solution with an appropriate amount of Milli-Q water. Then 25 mg of Zn₂Al-LDO was added to 50 mL of the respective glyphosate solutions in a series of 100 mL Erlenmeyer flasks The mixtures were stirred at 150 rpm. To determine the effect of temperature on adsorption, experiments were performed at 25, 35, and 45°C. After stirring, the solid was separated from the mixture by filtration. Residual glyphosate was determined in the filtrates by the optimized Ruhemann colorimetric method (Reference Hottes, Bauerfeldt, Herbst, Castro and da Silva San GilHottes et al., 2021). The adsorption capacity and adsorption percent of glyphosate on Zn₂Al-LDO were calculated using Eqs. 1 and 2, respectively:

(1) $q_e=\frac{\left(C_o,-,C_e\right).V}{m}$

(2) $R\left(\%\right)=\frac{(C_o-C_e)}{C_o}\times 100$

where, C _o and C _e represent the initial and equilibrium concentrations of glyphosate, respectively (μg mL⁻¹); V denotes the volume of glyphosate solution used (mL); and m represents the mass of the LDO adsorbent (μg) (Reference Rosset, Weidlich, Perez-Lopez and AmaralRosset et al., 2020). All adsorption experiments were performed at least three times to achieve data accuracy and reproducibility. Adsorption isotherm models were applied to describe the fraction of adsorbate that was partitioned between liquid and solid phases at equilibrium. In this study, Langmuir, Freundlich, and Temkin models were adopted to evaluate the adsorption behavior of glyphosate by Zn₂Al-LDO. Non-linear and linearized equations were used to make appropriate adjustments. For the sake of clarity, non-linear equations (Reference Tan and HameedTan & Hameed, 2017) are given as Langmuir (Eq. 3), Freundlich (Eq. 4), and Temkin (Eq. 5).

(3) $Q_e=\frac{Q_{\max }{K}_L{C}_e}{1+K_L{C}_e}$

(4) $q_e=K_F{C}_e^{1/n}$

(5) $q_e=\frac{RT}{b}\ln \left(a_T{C}_e\right)$

where, Q _max (μg mg⁻¹) is the maximum adsorption capacity associated with a monolayer formed over a solid surface, K_L is the equilibrium or Langmuir constant, C _e (µg.mL⁻¹) is the equilibrium concentration, q _e (μg mg⁻¹) is the amount of solute adsorbed at equilibrium, K_F is the Freundlich constant, 1/n is a constant related to site heterogeneity, a_T is the Temkin constant, b is a constant related to the heat of adsorption, T is temperature, and R is the universal gas constant (Reference FreundlichFreundlich, 1907; Reference LangmuirLangmuir, 1918; Reference Tan and HameedTan & Hameed, 2017). For comparison purposes, the experimental adsorption data were also fitted using linearized equations related to the Langmuir, Freundlich, and Temkin models. These equations are presented in the supplementary material. In addition, the equilibrium data were submitted to χ² (chi-square) analysis according to Eq. 6 (Reference Zhang, Gao, Zhao, Lei, Yuan, He, Gao and DengZhang et al., 2019).

(6) $\chi 2=\sum {\left({qe}_{\exp },-,{qe}_{\mathrm{cal}}\right)}^2/{qe}_{\exp }$

The kinetics of glyphosate adsorption by the Zn₂Al-LDO was studied using the adsorption capacity obtained from isotherm experiments. The glyphosate adsorption rate after various contact times was measured over the time range 5–200 min, with an initial glyphosate concentration of 300 μg mL⁻¹. The procedure was conducted as detailed in the adsorption isotherms, except that the temperature was controlled at 25 ± 1°C. To understand the glyphosate adsorption mechanism, experimental data were fitted to different kinetics models, corresponding to the pseudo-first order model (Eq. 7), pseudo-second order model (Eq. 8), and the Weber-Morris intraparticle diffusion model (Eq. 9):

(7) $q_t=q_e\left(1,-,e^{-k_{1}t}\right)$

(8) $q_t=\left(q_e^2,k_2,t\right)/\left(1,+,q_e,k_2,t\right)$

(9) $q_t=K_{\mathrm{iff}}{t}^{1/2}+C$

where, k₁ is the pseudo-first order constant, k₂ is the pseudo-second order constant, K_iff is the intraparticle diffusion rate constant, C is a constant, Q _e is the maximum amount of glyphosate adsorbed (μg Mg⁻¹), and Q _t is the amount adsorbed (μg mg⁻¹) at time t (min) (Reference Tan and HameedTan & Hameed, 2017).

Thermodynamic Parameters

The thermodynamic study was performed by reproducing the adsorption isotherm experiments with glyphosate solutions also at 35ºC and 45°C. The change in free energy of glyphosate adsorption (ΔG°), change in entropy of adsorption (ΔS°), and change in enthalpy of adsorption (ΔH°) were calculated using Eqs. 10, 11, and 12, respectively (Reference Tan and HameedTan & Hameed, 2017).

(10) $\Delta G^{\circ }=-RT\mathrm{lnK}$

(11) $\Delta G^{\circ }=\Delta H^{\circ }-T\Delta S^{\circ }$

(12) $\mathrm{lnK}=\frac{\Delta S^{\circ }}{R}-\frac{\Delta H^{\circ }}{RT}$

Characterization of Solids Before and After Glyphosate Adsorption

The Zn²⁺ and Al³⁺ contents obtained from the atomic absorption analysis were 29% and 15%, respectively, indicating an experimental Zn/Al ratio of 1.96. This value suggests that the experimental data were in agreement with the nominal mass data used in the experiment. Based on the percentages of cations, the following formula for the solid is proposed: [Zn_0.67Al_0.33(OH₂)]^0.33(CO₃)_0.165. Three mass-loss peaks were revealed by the thermograms obtained in an oxidizing atmosphere at 80°C, 170°C, and 230°C (Fig. 1) Such peaks between 25°C and 200°C are well known to indicate the loss of water molecules present in the extrinsic and intrinsic domains of the LDH structure. The peak recorded at 230°C suggests the beginning of the breakdown process of the lamellar structure and also the loss of carbonate present in the interlayer region. A wide and low-intensity peak was also observed in the region of 500°C, attributed to the decarbonation process of LDH (Reference Montanari, Sisani, Nocchetti, Vivani, Herrera, Ramis, Busca and CostantinoMontanari et al., 2010).

Fig. 1

TGA-DTG curves for Zn₂Al-LDH

The powder XRD patterns for Zn₂Al-LDH, Zn₂Al-LDO, and Zn₂Al-LDO-gly (Fig. 2) were obtained to compare the structures of Zn₂Al-LDH and Zn₂Al-LDO and to map possible changes due to glyphosate adsorption (comparing Zn₂Al-LDO and Zn₂Al-LDO-gly). The positions of the main diffraction peaks of Zn₂Al-LDH (d ₀₀₃ = 0.75 nm) observed in the XRD pattern (Fig. 2) were in agreement with those predicted in the literature for LDH of the Zn-Al system containing carbonate anions in the interstices (Reference Aisawa, Kudo, Hoshi, Takahashi, Hirahara, Umetsu and NaritaAisawa et al., 2004). The profile of the diffraction peaks also indicated the high crystallinity of the solid, as well as its structural organization. The crystallite size obtained using the Scherrer equation and the reflection peak (003) was 0.34 nm. A similar value (0.33 nm) was observed by Reference Aisawa, Kudo, Hoshi, Takahashi, Hirahara, Umetsu and NaritaAisawa et al. (2004) while studying the intercalation of amino acids by LDH of the Zn-Al system. Calcination at 450°C led to the collapse of the precursor structure, so observing the presence of reflection peaks (003) and (006) in the XRD patterns, characteristic of LDH, was no longer possible because of the presence of extended peaks typical of ZnO. The diffraction peaks observed in the solid after calcination are in agreement with those present in the literature for LDH of the Zn-Al-CO₃ system calcined at temperatures between 450 and 500°C (Reference Hu, Yan, Hu, Feng and ZhouHu et al., 2018; Reference Montanari, Sisani, Nocchetti, Vivani, Herrera, Ramis, Busca and CostantinoMontanari et al., 2010). After rehydration in aqueous solution, the typical ZnO diffraction peaks disappeared (Fig. 2), accompanied by the formation of peaks with patterns identical to that of the precursor, indicating the solid reversibility and structure regeneration (OH/LDH). However, the basal spacing of ~0.75 obtained after regeneration suggested that glyphosate intercalation was not the main process in the reconstruction. A broadening of the diffraction peaks was observed, suggesting that during the reconstruction step, multiple anions may have been intercalated, such as OH^– to CO₃ ^2– (Reference Aisawa, Kudo, Hoshi, Takahashi, Hirahara, Umetsu and NaritaAisawa et al., 2004; Reference Montanari, Sisani, Nocchetti, Vivani, Herrera, Ramis, Busca and CostantinoMontanari et al., 2010; Reference Rosset, Weidlich, Perez-Lopez and AmaralRosset et al., 2020). Thus, glyphosate may have been superficially adsorbed to the solid and also on the sides of the layer.

Fig. 2

XRD pattern of calcined, non-calcined, and reconstructed solids in glyphosate solution

The FTIR/ATR spectrum of non-adsorbed glyphosate (Fig. S1, Supplementary Material) revealed absorption bands at 3384, 1633/1581, and 1373 cm⁻¹. Bands in he region of 779–557 cm⁻¹ in the Zn₂Al-LDH FTIR spectrum (Fig. 3) correspond to the vibrational modes of the O–H bonds of the LDH structure and interstitial and adsorbed water, O-H-O bending, C-O stretching of carbonate, and structural M-O-M and O-M-O stretching, respectively (Reference Hu, Yan, Hu, Feng and ZhouHu et al., 2018; Reference Jiang, Hua, Han, Yang, Lu and WangJiang et al., 2009).

Fig. 3

FTIR/ATR spectra of calcined, non-calcined, and reconstructed solids in glyphosate solution

After calcination, complete disappearance of the band at 3384 cm⁻¹ and drastic reduction of the 1350 cm⁻¹ band, referring to the carbonate, were observed, indicating that these anions may still have been present in small amounts in Zn₂Al-LDO (Fig. 3) even after calcination of the precursor. Concerning Zn₂Al-LDO-gly (Fig. 3), the interaction of glyphosate with the layer was confirmed by the presence of absorption bands at 1573 cm⁻¹, corresponding to vibrational modes of the COO⁻ bond, and at 1065 cm⁻¹ and 967 cm⁻¹, corresponding to the vibrational modes of the P–O bond of the phosphonate group. According to the literature, when glyphosate is not adsorbed, C = O stretching can be observed in the form of two absorption maxima at 1730 and 1713 cm⁻¹ (Reference Li, Wang, Yang, Evans, Forano and DuanLi et al., 2005; Reference Meng, Zhang, Evans and DuanMeng et al., 2005). Concerning Zn₂Al-LDO-gly, the interaction of glyphosate with the layer was confirmed by the presence of absorption bands at 1573 cm⁻¹, corresponding to vibrational modes of the COO⁻group, and at 1065 cm⁻¹ and 967 cm⁻¹, corresponding to the vibrational modes of the phosphonate groupFurthermore, vibrational modes referring to P–O bonds of free glyphosate split into five bands with peaks at 1269, 1170, 1065, 1075, and 912 cm⁻¹. But after interaction with the solid surface, these bands were reduced to two or three modes, as also noted in the present study. Reference Li, Wang, Yang, Evans, Forano and DuanLi et al. (2005) and Reference Meng, Zhang, Evans and DuanMeng et al. (2005) suggested that the band at 1360 cm⁻¹ contains contributions from the vibrational modes of the C–O bonds of carbonate adsorbed from the environment during the experiments and also from the complementary vibrational modes of the C = O bond of the carboxylate portion of glyphosate, previously recorded at 1424 cm^–1 in its non-adsorbed form.

The porosity and surface area of the Zn ₂ Al-LDH and Zn₂Al-LDO samples were evaluated using the nitrogen desorption-adsorption method (Fig. 4a, b and Table 1). For both samples, type IV adsorption isotherms with type H3 hysteresis were observed, suggesting a mesoporous structure. The solids mostly had a pore size distribution between 2 and 10 nm. After calcination, a significant increase in the surface area of the adsorbent was observed, from 77.01 m² G⁻¹ in Zn₂Al-LDH to 102 m² g⁻¹ in Zn₂Al-LDO. The surface areas, obtained for both solids synthesized in the present study, were greater than those reported previously in the literature: 16.6 m² G⁻¹ for Zn-Al-LDH and 55.9 m² G⁻¹ for Zn-Al-LD (Reference Hu, Yan, Hu, Feng and ZhouHu et al., 2018), indicating that the method in the present work led to the formation of materials with greater adsorptive potential. According to the literature, the substantial increase in the area of the calcined solid compared to the non-calcined solid may be related to the loss of water and interstitial carbonate molecules, as well as changes in porosity. The heat treatment induced the formation of a larger number of pores in the region from 2 to 10 nm in the calcined solid (Fig. 4b).

Fig. 4

a Nitrogen adsorption isotherms and b pore-size distribution (BJH)

Table 1

Specific surface area (S _BET), pore radius (r _p), and pore volume (V _p) of the Zn₂Al-LDH and Zn₂Al-LDO samples. Data fitting based on the BET and BJH methods (desorption branch) (Reference SingSing, 1982)

For a better understanding of the glyphosate/Zn₂Al-LDO interaction mechanism, ¹³C and ³¹P SSMR experiments were performed. Experimental and simulated spectra, obtained for free glyphosate and adsorbed/interleaved glyphosate (Figs. S2 and S3), revealed only one peak in free glyphosate, with a chemical shift δ_P-31 = 18 ppm. After adsorption on the solid Zn₂Al-LDO, signals with isotropic chemical shifts equal to δ_P-31 = 23 to 14 ppm were present. According to Reference Li, Feng, Yan, Sparks and PhillipsLi et al. (2013), the signal at δ_P-31 = 12 ppm suggests a chemical environment in which phosphorus is complexed with aluminum sites (Al-O-P) in the solid layers. The broadened signal which shifted to greater frequency at δ_P-31 = 24 ppm suggests a chemical environment where the phosphonate moiety is associated with the solid surface by electrostatic interactions. As pointed out by Reference Li, Zhang, Evans, Forano and DuanLi et al., (2004, Reference Li, Feng, Yan, Sparks and Phillips2013), when investigating the adsorption of phosphate by various minerals, the broadening of NMR signals is related to stronger dipolar interactions between molecules as well as interactions with the solid surface, decreasing their mobility, in addition to being influenced by the formation of hydrogen bonds with neighboring molecules or with surrounding water molecules.

In the ³¹C-CPMAS spectrum, signal were observed at δ_C-13 = 169 ppm (carboxylate) and a doublet at 48 and 46 ppm. After adsorption, the signal at δ_C-13 = 169 ppm split into three signals at δ_C-13 = 180, 171, and 172 ppm. These displacements may be explained by the participation of carboxylate groups in a network of hydrogen bonds and/or non-bonded bridge interactions on the solid surface, as well as possible electrostatic interactions and complexation by the carboxyl with lamellar zinc atoms (C-O-Zn) (Reference Li, Feng, Yan, Sparks and PhillipsLi et al., 2013).

Adsorption of Glyphosate as a Function of pH

The surface charge and the adsorbate–adsorbent interactions are influenced directly by the pH of the aqueous solution (Reference Zubair, Daud, Mckay, Shehzad and Al-HarthiZubair et al., 2017). Glyphosate solutions are naturally acidic and, thus, can promote the leaching of Al³⁺ and Mg²⁺ cations due to the attack on the octahedral sheets, promoting deterioration of the solids and reducing their efficiency as adsorbents (Reference Rosset, Weidlich, Edith and HidalgoRosset et al., 2019, Reference Rosset, Weidlich, Perez-Lopez and Amaral2020). Glyphosate has different anionic forms depending on the pH of the medium, which is also important for its interaction with the solid matrix. According to Reference Peixoto, Bauerfeldt, Herbst, Pereira and da SilvaPeixoto et al. (2015), in aqueous solutions with pH values ≈10, the anionic forms gly²⁻ and gly³⁻ are observed, with trivalent anions being in greater proportion. These theoretical data were later confirmed experimentally by Reference Liu, Dong, Yu, Li, Wu, Tan and LuoLiu et al. (2016). Furthermore, Reference Li, Wang, Yang, Evans, Forano and DuanLi et al. (2005) observed good efficiency of glyphosate adsorption by both LDH and LDO, occurring at pH values ≥ 9 and < 11 and decreasing dramatically at pH > 11, thus suggesting that the glyphosate–solid interaction is highly unstable. Recent studies have indicated that good glyphosate adsorption can be achieved by LDH-type materials at pH values close to 10. Reference Cardoso and ValimCardoso and Valim (2006) reported that the adsorption of acidic pesticides on LDO-type solids was satisfactorily efficient at pH close to 9. Because a higher anionic charge density may contribute to greater adsorption potential due to greater chemical interaction and the distribution of glyphosate ionic species as a function of the pH, experiments in the present study were conducted at pH ≈ 10. A relevant aspect is that aqueous suspensions containing LDO and low concentrations of glyphosate will reach pH values close to the working pH, requiring the addition of minimal amounts of a basic solution to adjust the pH to 10. Buffer solutions were avoided because they might introduce unwanted anions into the reaction medium, leading to possible competition for the adsorption sites.

Equilibrium Study

Experimental adsorption curves of glyphosate by solid Zn2Al-LDO at different temperatures were fitted to non-linear (Fig. 5) and linear equations (Fig. S4, and Fig. 6) according to the Langmuir, Freundlich, and Temkin models. Regression parameters from non-linear and linear fits are shown in Table 2.

Fig. 5

a Experimental adsorption isotherms at 25, 35, and 45°C. Fitting of the Langmuir, Freundlich, and Temkin non-linear models b 25°C, c 35°C, and d 45°C

Fig. 6

Experimental kinetics curves of glyphosate adsorption on Zn₂Al LDO: a pseudo-first order kinetics model; b pseudo-second order kinetics model; and c Weber-Morris intraparticle diffusion model

Table 2

Adsorption parameters obtained from various linearized equations for glyphosate adsorbed on Zn₂Al-LDO: Langmuir (K_L, Langmuir constant; Q _max, maximum adsorption capacity); Freundlich (K_f, Freundlich constant); and Temkin (A and B, Temkin parameters)

The analysis of the adsorption isotherms (Fig. 5a) suggests H-type isotherms, according to the Giles classification, and strong interaction between the adsorbent and adsorbate, which can occur mainly by electrostatic interactions in view of the nature of the species (Reference Giles and SmithGiles & Smith, 1974). However, other forms of interactions must also be considered, such as hydrogen bonds and complexation, as already mentioned. According to the literature, an H-type isotherm is considered a special case of an L-type isotherm, where the initial section of the curve is vertical (Reference Abdellaoui, Pavlovic, Bouhent, Benhamou and BarrigaAbdellaoui et al., 2017; Reference Aisawa, Kudo, Hoshi, Takahashi, Hirahara, Umetsu and NaritaAisawa et al., 2004; Reference Giles and SmithGiles & Smith, 1974; Reference Rosset, Weidlich, Edith and HidalgoRosset et al., 2019, Reference Rosset, Weidlich, Perez-Lopez and Amaral2020). The correlation coefficients clearly indicated that the Langmuir model best fits the adsorption isotherms (Fig. 5b, d). Through this analysis, obtaining information about the nature of the adsorptive process was possible. The analysis of data (Table 2) indicates that the K_L values obtained by the linear and non-linear equations increased when the adsorption temperature changed from 25 to 45°C, reflecting an increasing adsorption capacity of the solid. This process is endothermic and can be explained by ion exchange with the medium. The greater adsorption efficiency was attributed to better dispersion of the adsorbent in the medium and exposure of adsorption sites.

Kinetics Study

The contact time of glyphosate with Zn₂Al-LDO was 200 min, for a glyphosate concentration of 300 μg mL⁻¹, with adsorbent dosage of 0.5 mg mL⁻¹, and pH equal to 10 (± 0.3). The amount of glyphosate adsorbed on LDO as a function of time (Fig. 6a) suggests that the removal of glyphosate from the aqueous solution increased dramatically in the first 50 min, when it reached its maximum, and then remained constant and in an equilibrium state until at least 200 min. The different steps of the adsorption curve as a function of time were affected by the concentration of the adsorbate in the medium. The high initial concentration of glyphosate favored a process of rapid mass transfer from the liquid phase to the surface or pores of the solid, which explains the steep slope of the curve in the initial period. As the adsorbate concentration decreases, the mass transfer rate tended to decrease until the equilibrium state was achieved and a dynamic adsorption-desorption process was established.

Reference Peng, Tang and ZhouPeng et al. (2021) investigated glyphosate adsorption on Ca_-Al-LDO and reported a fast rate of adsorption in the first 80 min. They obtained an adsorption rate of 40 μg of glyphosate per mg of adsorbent during 50 min. In the present study, for the same time interval, a greater adsorption rate of 190 μg mg⁻¹ was attained over a period of 50 min. The greater adsorption rate of the analyte to the solid phase observed in the present study when compared to that of Reference Peng, Tang and ZhouPeng et al. (2021) can be explained by the large difference in the surface area of the materials used, which were 14.37 m² g⁻¹ of the solid Ca_-AL-LDO versus 102.30 m² g⁻¹ of the solid Zn₂Al-LDO in the current study.

Reference Khenifi, Derriche, Mousty, Prévot and ForanoKhenifi et al. (2010) studied the adsorption of glyphosate on NiAlNO₃-LDH and observed a rapid mass transfer of the adsorbate to the surface, with ~180 μg of solution being removed from the glyphosate solution/mg of adsorbent in an average time of 30 min. In the present study, in the same period the diffusion process led to the adsorption of only 160 μg of glyphosate per mg of solid adsorbent. However, the higher diffusion rate observed by Reference Khenifi, Derriche, Mousty, Prévot and ForanoKhenifi et al. (2010) can be explained by the use of a greater adsorbent load in their experiments (1 mg mL⁻¹) compared to the mass used in the present study (0.5 mg mL⁻¹). Unlike the current observations and those previously reported, Reference Li, Wang, Yang, Evans, Forano and DuanLi et al. (2005) verified that the step with the greatest percentage of glyphosate adsorption by the solid they studied (MgAlNO₃-LDH) took place over an average time of 150 min, reaching a state of equilibrium after that period.

To obtain information about the mechanism of glyphosate adsorption on Zn₂Al-LDO, the experimental adsorption as a function of time was fitted to the non-linear pseudo-first order and pseudo-second order models and to the Weber-Morris intraparticle diffusion model (Fig. 6b, c and Table 3).

Table 3

Kinetics parameters and intraparticle diffusion parameters for adsorption of glyphosate by Zn₂Al-LDO: calculated adsorption capacity (Q _e,_cal, μg mg^–1); pseudo-first order rate constant (K₁, min⁻¹); pseudo-second order rate constant (K₂, mg μg^–1 min⁻¹); diffusion constant (K_diff, μg mg^–1 min^–1/2); and intraparticle diffusion parameter, C

The best fit was obtained with the pseudo-second order model (Fig. 6b and Table 3). This result indicates that the decisive step in the adsorption rate of glyphosate on Zn₂Al-LDO passed through a chemisorption process, i.e. distinct chemical interactions occurred that led to structural variations in the solid formed by the adsorbate–adsorbent adduct. This conclusion was corroborated by the explicit changes in the FTIR-ATR and SSNMR spectra of ¹³C and ³¹P, indicating that glyphosate was bound chemically to the solid. Moreover, the Weber-Morris intraparticle diffusion model was used (Fig. 6c) and the multilinearity observed in the graph referring to the diffusion adjustment indicated that the adsorptive process occurred at least in one of the steps being controlled by the formation of the intrafilm.

Also noted was a reduction in the value of the diffusion constant from step 1 to step 2. This effect indicates that the diffusion of glyphosate decreased from the liquid phase to the surface of the adsorbent due to the reduction of its concentration in solution and suggests that the system was moving toward a state of equilibrium. A non-zero value of C indicates that the line does not pass through the origin. This behavior may be due to the difference in the mass-transfer rate variation at the beginning and end of the adsorptive process. These data indicate further that an external diffusion process rather than pore diffusion is the rate-limiting step.

Thermodynamic Study

The thermodynamic parameters such as Gibbs free energy, enthalpy, and entropy were estimated from equilibrium data obtained from isotherm experiments at 25, 35, and 45°C, as reported in Table 4. The equilibrium experiments performed at these temperatures showed an increase in the amount of glyphosate adsorbed with increasing temperature, indicating the endothermic nature of the adsorption. The negative ΔG value indicates that the nature of the adsorption was spontaneous and that the affinity of the glyphosate/LDO increased with increasing temperature. The increase in glyphosate adsorption was accompanied by an increase in medium disorder, indicating that the process depends on surface anion exchange. The positive enthalpy value also confirmed that the adsorption process was strictly dependent on entropy (Reference Extremera, Pavlovic, Pérez and BarrigaExtremera et al., 2012; Reference Marangoni, Ramos and WypychMarangoni et al., 2009).

Table 4

Thermodynamics parameters for glyphosate adsorption by Zn₂Al-LDO: ΔG°, standard free energy of adsorption; ΔH°, standard enthalpy of adsorption; ΔS°, standard entropy of adsorption

Anionic Competition

The effects of anionic competition of the glyphosate in the presence of Cl–, NO₃, HPO₄ ^2–, CO₃ ^2–, and SO₄ ^2– anions using the Zn₂Al-LDO adsorbent have not been published previously, but are presented here in order to quantify any adsorption inhibition which might be caused by the competing anions. The results (Fig. 7) indicated that the gradual increase in the concentration of all anions induced a reduction in the adsorption of glyphosate anions, as their equilibrium concentration tended to increase in the medium. However, the extent of inhibition of glyphosate adsorption was not equivalent in all cases. According to Reference Abdellaoui, Pavlovic, Bouhent, Benhamou and BarrigaAbdellaoui et al. (2017), anions that present adequate symmetry and high charge-radius ratio can stabilize the LDH structure during the reconstruction process. Moreover, anions with greater charge density, such as sulfate, hydrogen phosphate, and carbonate, inhibited glyphosate adsorption on LDO more efficiently than nitrate and chloride anions. The trend observed was that, among the anions with higher charge density, the competitive effect varied and greater glyphosate adsorption inhibition was promoted by carbonate, hydrogen phosphate, and sulfate anions.

Fig. 7

Influence of the concentration of the various anions on the adsorption of glyphosate

According to Reference Constantino and PinnavaiaConstantino and Pinnavaia (1995) and Reference Abdellaoui, Pavlovic, Bouhent, Benhamou and BarrigaAbdellaoui et al. (2017), this variation can be attributed to the greater symmetry observed in the carbonate anions which, when added to the charge, provides greater efficiency in the stabilization of the lamellae in the case of intercalation. Sulfate and hydrogen phosphate, although less symmetrical than carbonate, induce greater inhibition of adsorption due to their high charge and smaller size compared to glyphosate. A study investigating the effect of anionic competition involving the anions mentioned above in relation to amaranth dye indicated that anions with greater charge density and symmetry, such as carbonate, sulfate, and phosphate, were responsible for promoting greater inhibition of adsorbate adsorption (Reference Abdellaoui, Pavlovic, Bouhent, Benhamou and BarrigaAbdellaoui et al., 2017).