# Binding of Cd(II) by Amorphous Aluminum Hydroxide-Organophosphorus Coprecipitates: From Macroscopic to Microscopic Investigation

Authors: Lei Lu; Feng Xu; Wenkai Rao; Ning Nie; Huihui Du
Journal: Adsorption Science & Technology
 (2021)

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## Abstract

The mobility of Cd(II) in soils, sediments, and aquatic systems is strongly dependent on adsorption behaviors occurring at the mineral-water interface, and this process may be influenced by the presence of organic phosphorus (OP). In this study, we investigate Cd(II) adsorption onto amorphous aluminum hydroxide (AAH), both in the presence and absence of OP, represented by the widely abundant myo-inositol hexakisphosphate (IHP). Isothermal adsorption experiment coupled with attenuated total reflection Fourier transform infrared (ATR-FTIR) and1H solid-state NMR spectra were employed. Physiochemical characterization shows that IHP can increase the surface negative charge and the number of surface sites. Isothermal results show that high IHP loading enhances Cd(II) adsorption while no obvious increase is observed at low IHP loading. The overall effect of IHP on Cd(II) sorption depends on the extent of two positive processes, i.e., (1) IHP can form ternary complexes with adsorbed Cd(II) on AAH and (2) IHP can increase the negative surface charge of AAH, and a negative process, i.e., AAH competes with Cd(II) for AAH surface sites. ATR-FTIR results confirm the possible formation of three structurally distinct ternary complexes, i.e., the AAH-IHP-Cd, AAH-Cd-IHP, and AAH-Cd-IHP-Cd. The analysis of 1H solid-state NMR demonstrates that IHP only increases the number of surface OH groups rather than changes their chemical environment and speciation. Cd does not bind to the AAH surface but mainly binds with the OH groups of IHP. All findings of this work suggest that the presence of high dose of OP promotes the retention of Cd(II) in soils, thereby decreasing their bioavailability to biota.


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## Body

## 1. Introduction

Heavy metals released from industrial and agricultural activities accumulate in soil, resulting in the degradation of soil quality [1, 2]. Sorption, desorption, and precipitation reactions of heavy metals onto soil components, i.e., metal (hydr)oxides and organic constituents, determine their mobility, migration, and bioavailability, which remarkably affects crop safety [3–6]. Both iron and aluminum (hydr)oxides are widely present in soils and sediments, especially in tropical and subtropical soils with variable charges [7]. Poorly crystalline Fe/Al (hydr)oxides provide abundant active sorption sites for toxic heavy metals through precipitation [8, 9] and complexation [10]. As such, they can be a substantial sink for heavy metal pollutants, thereby governing their biogeochemical cycles in contaminated environment.In soils, the presence of anionic compounds can enhance or suppress the surface interaction of heavy metals on Fe/Al (hydr)oxides [11, 12]. Phosphate is an ubiquitous reactive ligand in the environment, showing high reactivity to soil minerals [13, 14]. A large number of studies have shown that phosphate can significantly affect heavy metals adsorption onto mineral phases [15–17]. This can occur as the result of the following: (a) electrostatic interaction [18], (b) ternary surface complexion [19], (c) competition with heavy metals for surface adsorption sites [11, 20], and (d) formation of metal-phosphate surface precipitation [21]. Ren et al. [22] showed an enhanced adsorption of Cu(II) with coexisting phosphate on γ-Al2O3 at pH 5.5, which is attributed to the formation of ternary surface complexes (phosphate as bridging molecule). Recent research by Hinkle et al. [19] suggested that the synergistic adsorption behavior of phosphate and Fe(II) is probably due to electrostatic interactions and the ternary complexation formation on Fe oxide surfaces. An earlier study by Li et al. [20] found that phosphate treatment suppresses the maximum adsorption of Cd/Cu on hematite, owing to the decreased inner-sphere adsorption sites with coexisting phosphate. Singh et al. [21] also observed the formation of surface ternary complexes of goethite-phosphate-U, and U(VI)-phosphate precipitation occurred when U(VI) concentration was up to ~100 μM. As mentioned above, most studies have focused on the influences of inorganic phosphate on toxic metals binding to Fe/Al (hydr)oxide, but relatively few studies have explored the effects of organic phosphorus.Organic phosphorus (OP) accounts for 50~80% of total P in soils, among which myo-inositol hexakisphosphate (IHP) is the most abundant one that is involved in many biogeochemical processes [23, 24]. It is well documented that IHP can strongly interact with metal (hydr)oxides, such as Al (hydr)oxide [25–27], Fe (hydr)oxide [28, 29], and metal nanoparticles [30, 31]. The coexisting IHP can significantly promote Cd(II) sorption on gibbsite and kaolinite below pH 8 [32, 33]. ATR-FTIR spectroscopy results have confirmed two structurally distinct ternary surface complexes in ternary system of IHP, Cd(II), and hematite [23]. Yan et al. [34] investigated the adsorption of Zn(II) and IHP on γ-Al2O3 surfaces and showed that the presorption of IHP restrains the formation of Zn−Al layered double hydroxide (LDH) precipitates. The above results have shown that the presence of IHP can remarkably affect the interaction between heavy metals and minerals. Despite this, very limited studies have investigated the reactivity of minerals-IHP coprecipitates, especially their sorption behavior towards heavy metals.Amorphous Al hydroxide (AAH), serving as the most active Al (hydr)oxides in soils, exhibits a great number of reactive functional groups and high specific surface area [26, 27]. The adsorption processes of Cd(II) or IHP on AAH have been systematically studied before [26, 35], while the binding mechanisms of Cd(II) on AAH-IHP coprecipitates are still poorly understood. The spectroscopy technology, i.e., Fourier transform infrared spectroscopy (ATR-FTIR) and solid-state 1H nuclear magnetic resonance spectroscopy (1H NMR), can provide molecular-scale information for the binding characteristics of heavy metals on mineral surface and allow for the direct identification of their surface species. In the present study, we synthetized AAH-IHP coprecipitates with two different P loadings. We characterized the AAH-IHP coprecipitates in terms of mineralogy, crystallinity, surface functional groups, and surface charge. We combined batch sorption, ATR-FTIR spectroscopy, and solid-state 1H NMR spectroscopy to explore the binding mechanisms of Cd(II) in the composite system. Our finding is helpful to understand the interaction of trace elements with Al-organophosphorus coprecipitates in Al-rich soils and sediments.


## 2. Materials and Methods

### 2.1. Synthesis of Pure AAH and AAH-IHP Coprecipitates

Myo-inositol hexakisphosphate (C6H18O24P6, IHP) was produced from Sigma-Aldrich (Shanghai, China). Amorphous Al hydroxide (AAH) was prepared according to the method reported previously [26], by adding 0.5 M NaOH to a 0.167 M AlCl3 solution at pH ~6.0. Two kinds of AAH-IHP coprecipitates were synthesized by mixing 0.05 M aluminum nitrate with 1 mM or 10 mM of IHP under vigorous stirring. After 15 min, the pH of the suspensions was adjusted to 7.3 and then left for 20 min to obtain two different AAH-IHP coprecipitates, named as AAH-IHP_low and AAH-IHP_high, respectively. The suspensions were centrifuged at 4500 × g for 20 min, and the resulting supernatants with unadsorbed IHP were removed. Both the pure AAH and AAH–IHP coprecipitates were washed three times with deionized water and dialyzed for 2 days in the dark. The freshly synthesized AAH and AAH–IHP coprecipitates were employed for batch Cd(II) sorption experiments, and a proportion of the freeze-dried precipitates were used for TEM, XRD, ATR-FTIR, and zeta (ζ) potential measurements.


### 2.2. Cd(II) Adsorption Experimental Designs

Cd(II) stock solution was prepared at 1000 mg/L by dissolving Cd(NO3)2·4H2O in deionized water. Potassium nitrate (KNO3) was prepared at 0.1 M as the background electrolyte. Prior to the sorption experiment, the adsorbents were first dispersed with electrolyte (0.1 M KNO3) and purged with N2 to remove CO2. Sorption experiments were performed in a series of 50 mL centrifuge tubes at room temperature (~25°C). In each tube, sorption samples contained 0.1 g/L of sorbents (AAH or AAH-IHP coprecipitates), 0~40 mg/L Cd, and background electrolyte. The sorption suspensions were immediately shaken for 24 hours at pH 6.5 and then centrifuged at 4500 × g for 10 minutes. The supernatants were filtered through 0.22 μm membrane filters and acidified with 1% HNO3 for measurement of Cd(II) using ICP-OES (PerkinElmer Optima 8300). The residual solids were freeze-dried for selected analyses of ATR-FTIR and 1H solid-state NMR. All the measurements were performed in three replicates, and sample blanks were conducted throughout the whole processes. The Langmuir isotherm (Eq. (1)) was used to model the results [36]:
(1)Qe=QmKCe1+KCe,where Qe (mg/g) and Qm (mg/g) refer to the equilibrium adsorption capacity and maximum adsorption capacity, respectively. K (L/mg) represents the Langmuir constant, and Ce (mg/L) is the equilibrium concentration after adsorption.


### 2.3. Characterization of Pure AAH and AAH-IHP Coprecipitates with or without Adsorbed Cd(II)

The morphology of pure AAH and AAH-IHP coprecipitates was recorded using a transmission electron microscopy (TEM, FEI Tecnai G2 F20, US) after fixing them with 2.5% glutaraldehyde. The mineral identity was analyzed on a Bruker D8 Advance diffractometer (XRD, Shimadzu XRD-6100) equipped with a Cu Kα radiation (λ=1.5406 nm). Diffractograms were collected from 1° to 85° with a 10 s acquisition time and a step size of 0.02°. The surface charge property was determined by a zeta potential analyzer (Zetaplus90, Brookhaven). Prior to zeta potential collection, the freshly samples (0.1 g/L) were dispersed in 0.1 M KNO3 at pH 6.5. ATR-FTIR was performed on a PerkinElmer FT-IR spectrometer equipped with an advanced 6 reflection ATR units (Specac Ltd. London, U.K.). Each spectrum was recorded in the range extending from 800 cm–1 to 2600 cm–1 at a resolution of 4 cm–1. Solid-state 1H NMR spectra were recorded on a 600 MHz Bruker spectrometer (11.74 T) equipped with a high-speed MAS probe. 1H MAS-NMR spectra were measured with an excitation π/2 pulse of width 6 μs and a 20 s relaxation delay. Trimethylsilane solution was employed as the external standard to calibrate the chemical shift. The experimental error was ±0.1 ppm for the shift.


## 2.1. Synthesis of Pure AAH and AAH-IHP Coprecipitates

Myo-inositol hexakisphosphate (C6H18O24P6, IHP) was produced from Sigma-Aldrich (Shanghai, China). Amorphous Al hydroxide (AAH) was prepared according to the method reported previously [26], by adding 0.5 M NaOH to a 0.167 M AlCl3 solution at pH ~6.0. Two kinds of AAH-IHP coprecipitates were synthesized by mixing 0.05 M aluminum nitrate with 1 mM or 10 mM of IHP under vigorous stirring. After 15 min, the pH of the suspensions was adjusted to 7.3 and then left for 20 min to obtain two different AAH-IHP coprecipitates, named as AAH-IHP_low and AAH-IHP_high, respectively. The suspensions were centrifuged at 4500 × g for 20 min, and the resulting supernatants with unadsorbed IHP were removed. Both the pure AAH and AAH–IHP coprecipitates were washed three times with deionized water and dialyzed for 2 days in the dark. The freshly synthesized AAH and AAH–IHP coprecipitates were employed for batch Cd(II) sorption experiments, and a proportion of the freeze-dried precipitates were used for TEM, XRD, ATR-FTIR, and zeta (ζ) potential measurements.


## 2.2. Cd(II) Adsorption Experimental Designs

Cd(II) stock solution was prepared at 1000 mg/L by dissolving Cd(NO3)2·4H2O in deionized water. Potassium nitrate (KNO3) was prepared at 0.1 M as the background electrolyte. Prior to the sorption experiment, the adsorbents were first dispersed with electrolyte (0.1 M KNO3) and purged with N2 to remove CO2. Sorption experiments were performed in a series of 50 mL centrifuge tubes at room temperature (~25°C). In each tube, sorption samples contained 0.1 g/L of sorbents (AAH or AAH-IHP coprecipitates), 0~40 mg/L Cd, and background electrolyte. The sorption suspensions were immediately shaken for 24 hours at pH 6.5 and then centrifuged at 4500 × g for 10 minutes. The supernatants were filtered through 0.22 μm membrane filters and acidified with 1% HNO3 for measurement of Cd(II) using ICP-OES (PerkinElmer Optima 8300). The residual solids were freeze-dried for selected analyses of ATR-FTIR and 1H solid-state NMR. All the measurements were performed in three replicates, and sample blanks were conducted throughout the whole processes. The Langmuir isotherm (Eq. (1)) was used to model the results [36]:
(1)Qe=QmKCe1+KCe,where Qe (mg/g) and Qm (mg/g) refer to the equilibrium adsorption capacity and maximum adsorption capacity, respectively. K (L/mg) represents the Langmuir constant, and Ce (mg/L) is the equilibrium concentration after adsorption.


## 2.3. Characterization of Pure AAH and AAH-IHP Coprecipitates with or without Adsorbed Cd(II)

The morphology of pure AAH and AAH-IHP coprecipitates was recorded using a transmission electron microscopy (TEM, FEI Tecnai G2 F20, US) after fixing them with 2.5% glutaraldehyde. The mineral identity was analyzed on a Bruker D8 Advance diffractometer (XRD, Shimadzu XRD-6100) equipped with a Cu Kα radiation (λ=1.5406 nm). Diffractograms were collected from 1° to 85° with a 10 s acquisition time and a step size of 0.02°. The surface charge property was determined by a zeta potential analyzer (Zetaplus90, Brookhaven). Prior to zeta potential collection, the freshly samples (0.1 g/L) were dispersed in 0.1 M KNO3 at pH 6.5. ATR-FTIR was performed on a PerkinElmer FT-IR spectrometer equipped with an advanced 6 reflection ATR units (Specac Ltd. London, U.K.). Each spectrum was recorded in the range extending from 800 cm–1 to 2600 cm–1 at a resolution of 4 cm–1. Solid-state 1H NMR spectra were recorded on a 600 MHz Bruker spectrometer (11.74 T) equipped with a high-speed MAS probe. 1H MAS-NMR spectra were measured with an excitation π/2 pulse of width 6 μs and a 20 s relaxation delay. Trimethylsilane solution was employed as the external standard to calibrate the chemical shift. The experimental error was ±0.1 ppm for the shift.


## 3. Result

### 3.1. Physiochemical Characteristics of AAH-IHP Coprecipitates

The results of TEM and XRD are presented in Figure1. According to the TEM images, both pure AAH and AAH-IHP coprecipitates show networks of coalesced aggregates, which are composed of amorphous and nanosized particles. This finding indicates the formation of poorly crystalline Al hydroxide [7]. No significant differences are observed between pure AAH and AAH-IHP coprecipitates. The XRD pattern of pure AAH exhibits three broad peaks at ~0.42, 0.22, and 0.14 nm, which agrees with those of amorphous Al hydroxide [26]. By comparison, AAH-IHP coprecipitates show slightly reduced crystallinity according to the decreased peak intensity at 0.22 and 0.14 nm. The possible explanation is that the frequent reactions between AAH and IHP molecules prevent cross-linking and lead to the reduced size of coherent scattering domains [37]. Combined results of TEM and XRD analyses demonstrate that IHP can slightly alter the surface structure of AAH, which agrees with other organo–AAH composites reported previously [7, 26].Figure 1
(a–c) TEM, (d) XRD, and (e) ATR-FTIR spectra of pure AAH and AAH-IHP coprecipitates (AAH-IHP_low and AAH-IHP_high).
(a)(b)(c)(d)(e)ATR-FTIR spectra are regarded as an efficient technique to identify IR vibrations of the OP molecules and to characterize the interaction between OP and minerals by changing these vibrations [23, 34]. The ATR-FTIR spectra (800~2600 cm–1) of IHP interacted with AAH are given in Figure 1(e). The absorbance band at ~2427 cm–1 is assigned to the Al-OH vibration. The bands at ~1065 and 1176 cm–1 correspond to the symmetric and asymmetric stretching vibration of P–O [25], while the bands at ~932 and 883 cm–1 are assigned to the P-OH vibration. The characteristic peak of C–C in IHP molecule locates at ~1724 cm–1. In general, in the range of 800~1200 cm–1 and ~1724 cm–1, most characteristic bands for IHP molecules are observed in high IHP-reacted samples. With the increase of initial IHP loading, the original absorbance band at ~946 cm–1 gradually disappears, which accords with the results of Yan et al. [26]. The increased IHP loading decreases the absorbance band at ~2427 cm–1, which may result from inner-sphere surface complex formation between AAH and IHP [38]. The intensity of the absorbance bands at ~1065 and 1176 cm–1 is enhanced as IHP loading increases, and the spectrum of AAH-IHP_high shows the presence of characteristic peaks of C–C (~1724 cm–1) and P–OH (~932 and 883 cm–1) vibrations of IHP molecule. These results indicate that high OP loading plays a key role in changing the mineral surface property, and thus affecting their environmental reactivity.Zeta potentials of AAH and AAH-IHP coprecipitates are presented in Table1. Our results show that the IHP loading decreases the zeta potentials of AAH from 3.85 to –2.56 mV, which agrees with other mineral systems reported previously [23, 27, 39]. However, the low IHP loading only reduces the amount of surface positive change. When the IHP concentration further increases, the surface adsorption sites become increasingly negatively charged, which are favorable to attract cations such as Cd2+ onto mineral surfaces.Table 1
Zeta potentials of pure AAH and AAH-IHP coprecipitates (AAH-IHP_low and AAH-IHP_high) at pH 6.5.
MaterialsmVAAH3.85 (0.08)AAH-IHP_low1.54 (0.06)AAH-IHP_high–2.56 (0.11)


### 3.2. Isothermal Adsorption

Cd(II) adsorption isotherms at pH 6.5 are displayed in Figure2. The goodness (R>0.97, Table 2) of fits in Table 2 signifies that Langmuir model can adequately simulate Cd(II) adsorption onto pure AAH and AAH-IHP coprecipitates. The maximum Cd adsorption capacity for AAH, AAH-IHP_low, and AAH-IHP_high are 106.97, 107.63, and 204.71 mg/g, respectively. AAH-IHP_high exhibits the highest adsorption capacity. In addition, the binding affinities (K, Table 2) for Cd(II) adsorption on three samples are close to each other, which signifies that high IHP increases the number of adsorption sites rather than changes the affinity between Cd(II) and AAH. There is no obvious differences between pure AAH and AAH-IHP_low, which implies that low-dose OP treatment nearly exerts no impact on Cd(II) immobilization on Al (hydr)oxides.Figure 2
Adsorption isotherms of Cd(II) on pure AAH and AAH-IHP coprecipitates (AAH-IHP_low and AAH-IHP_high) at pH 6.5.Table 2
Isotherm parameters for Cd(II) adsorption on pure AAH and AAH-IHP coprecipitates (AAH-IHP_low and AAH-IHP_high) at pH 6.5.
Langmuir modelAdsorbentsQm (mg/g)K (L/mg)R2AAH106.970.050.97AAH-IHP_low107.630.060.99AAH-IHP_high204.710.040.99Note:Qm is the maximum adsorption capacity, and K represents the Langmuir constant.


### 3.3. ATR-FTIR Spectroscopy

The ATR-FTIR spectra (800~2600 cm–1) of AAH and AAH-IHP coprecipitates before and after adsorbing Cd(II) at pH 6.5 are presented in Figure 3. The characteristic peak of AAH at ~2427 cm–1 (Al-OH vibration) decreases after adsorbing Cd(II). Exceptionally, the spectra of AAH with adsorbed Cd show no obvious differences compared to the Cd-free spectrum. When AAH is coprecipitated with IHP, the spectrum intensity of P–OH vibration at ~883 and 932 cm–1 is reduced, and a new absorbance band at 1038 cm–1 appears, which is associated with the P–O–Cd symmetric stretching vibration [23]. This finding suggests that the adsorbed Cd(II) replaces hydrogen of the OH groups on the surface of pure AAH and AAH-IHP_high. However, the peak intensity of Al–OH vibration (~2427 cm–1) with or without adsorbed Cd(II) in AAH-IHP_high shows no apparent differences. This observation suggests that Cd(II) is mainly binding to the IHP molecules instead of AAH in the composites. Moreover, it is interesting that the characteristic peaks of P–O (~1176 cm–1) and C–C (~1724 cm–1) vibrations in AAH-IHP_high with adsorbed Cd(II) are enhanced. Possible explanation is because a part of IHP is desorbed from AAH-IHP coprecipitates in background electrolyte, and some of the free Cd ions occupy the adsorption sites of desorbed IHP on AAH, thus promoting the binding of desorbed IHP with the newly adsorbed Cd on the surface [23, 27].Figure 3
ATR-FTIR spectra of pure AAH and AAH-IHP coprecipitates (AAH-IHP_low and AAH-IHP_high) with or without adsorbed Cd.


### 3.4.1H Solid-State NMR Spectroscopy

In order to gain a deeper insight into fundamental binding mechanisms of OP interacted with AAH and their effects on binding of Cd(II), the1H NMR spectra of pure AAH and AAH-IHP_high with and without adsorbed Cd(II) were analyzed and the results are given in Figure 4. The 1H NMR spectra of pure AAH exhibit a main peak at δH−1=4.7 ppm, with two shoulders around 0.8 and 3.3 ppm, respectively. The 1H NMR peak at 4.7 ppm corresponds to the physically adsorbed water, and those at δH−1=0.8 and 3.3 ppm are assigned to the OH groups in AAH or IHP molecule [40]. When IHP is coprecipitated with AAH, the peak intensity at δH−1=0.8 and 3.3 increases and no new peak occurs. This result indicates that the chemical environment and speciation of OH groups in IHP molecule is very similar to that in AAH, and high IHP loading increases the number of OH groups. On the other hand, the presence of adsorbed Cd(II) decreases those characteristic peaks of OH groups at δH−1=0.8 and 3.3 ppm in all samples, corresponding to the reduced spectrum intensity at ~883, 932, and 2427 cm–1 observed in Figure 3. This finding demonstrates that Cd(II) binds to pure AAH and AAH-IHP coprecipitates by surface complexation with OH groups.Figure 4
The1H NMR spectra of pure AAH and AAH-IHP coprecipitates (AAH-IHP_low and AAH-IHP_high) with or without adsorbed Cd.


## 3.1. Physiochemical Characteristics of AAH-IHP Coprecipitates

The results of TEM and XRD are presented in Figure1. According to the TEM images, both pure AAH and AAH-IHP coprecipitates show networks of coalesced aggregates, which are composed of amorphous and nanosized particles. This finding indicates the formation of poorly crystalline Al hydroxide [7]. No significant differences are observed between pure AAH and AAH-IHP coprecipitates. The XRD pattern of pure AAH exhibits three broad peaks at ~0.42, 0.22, and 0.14 nm, which agrees with those of amorphous Al hydroxide [26]. By comparison, AAH-IHP coprecipitates show slightly reduced crystallinity according to the decreased peak intensity at 0.22 and 0.14 nm. The possible explanation is that the frequent reactions between AAH and IHP molecules prevent cross-linking and lead to the reduced size of coherent scattering domains [37]. Combined results of TEM and XRD analyses demonstrate that IHP can slightly alter the surface structure of AAH, which agrees with other organo–AAH composites reported previously [7, 26].Figure 1
(a–c) TEM, (d) XRD, and (e) ATR-FTIR spectra of pure AAH and AAH-IHP coprecipitates (AAH-IHP_low and AAH-IHP_high).
(a)(b)(c)(d)(e)ATR-FTIR spectra are regarded as an efficient technique to identify IR vibrations of the OP molecules and to characterize the interaction between OP and minerals by changing these vibrations [23, 34]. The ATR-FTIR spectra (800~2600 cm–1) of IHP interacted with AAH are given in Figure 1(e). The absorbance band at ~2427 cm–1 is assigned to the Al-OH vibration. The bands at ~1065 and 1176 cm–1 correspond to the symmetric and asymmetric stretching vibration of P–O [25], while the bands at ~932 and 883 cm–1 are assigned to the P-OH vibration. The characteristic peak of C–C in IHP molecule locates at ~1724 cm–1. In general, in the range of 800~1200 cm–1 and ~1724 cm–1, most characteristic bands for IHP molecules are observed in high IHP-reacted samples. With the increase of initial IHP loading, the original absorbance band at ~946 cm–1 gradually disappears, which accords with the results of Yan et al. [26]. The increased IHP loading decreases the absorbance band at ~2427 cm–1, which may result from inner-sphere surface complex formation between AAH and IHP [38]. The intensity of the absorbance bands at ~1065 and 1176 cm–1 is enhanced as IHP loading increases, and the spectrum of AAH-IHP_high shows the presence of characteristic peaks of C–C (~1724 cm–1) and P–OH (~932 and 883 cm–1) vibrations of IHP molecule. These results indicate that high OP loading plays a key role in changing the mineral surface property, and thus affecting their environmental reactivity.Zeta potentials of AAH and AAH-IHP coprecipitates are presented in Table1. Our results show that the IHP loading decreases the zeta potentials of AAH from 3.85 to –2.56 mV, which agrees with other mineral systems reported previously [23, 27, 39]. However, the low IHP loading only reduces the amount of surface positive change. When the IHP concentration further increases, the surface adsorption sites become increasingly negatively charged, which are favorable to attract cations such as Cd2+ onto mineral surfaces.Table 1
Zeta potentials of pure AAH and AAH-IHP coprecipitates (AAH-IHP_low and AAH-IHP_high) at pH 6.5.
MaterialsmVAAH3.85 (0.08)AAH-IHP_low1.54 (0.06)AAH-IHP_high–2.56 (0.11)


## 3.2. Isothermal Adsorption

Cd(II) adsorption isotherms at pH 6.5 are displayed in Figure2. The goodness (R>0.97, Table 2) of fits in Table 2 signifies that Langmuir model can adequately simulate Cd(II) adsorption onto pure AAH and AAH-IHP coprecipitates. The maximum Cd adsorption capacity for AAH, AAH-IHP_low, and AAH-IHP_high are 106.97, 107.63, and 204.71 mg/g, respectively. AAH-IHP_high exhibits the highest adsorption capacity. In addition, the binding affinities (K, Table 2) for Cd(II) adsorption on three samples are close to each other, which signifies that high IHP increases the number of adsorption sites rather than changes the affinity between Cd(II) and AAH. There is no obvious differences between pure AAH and AAH-IHP_low, which implies that low-dose OP treatment nearly exerts no impact on Cd(II) immobilization on Al (hydr)oxides.Figure 2
Adsorption isotherms of Cd(II) on pure AAH and AAH-IHP coprecipitates (AAH-IHP_low and AAH-IHP_high) at pH 6.5.Table 2
Isotherm parameters for Cd(II) adsorption on pure AAH and AAH-IHP coprecipitates (AAH-IHP_low and AAH-IHP_high) at pH 6.5.
Langmuir modelAdsorbentsQm (mg/g)K (L/mg)R2AAH106.970.050.97AAH-IHP_low107.630.060.99AAH-IHP_high204.710.040.99Note:Qm is the maximum adsorption capacity, and K represents the Langmuir constant.


## 3.3. ATR-FTIR Spectroscopy

The ATR-FTIR spectra (800~2600 cm–1) of AAH and AAH-IHP coprecipitates before and after adsorbing Cd(II) at pH 6.5 are presented in Figure 3. The characteristic peak of AAH at ~2427 cm–1 (Al-OH vibration) decreases after adsorbing Cd(II). Exceptionally, the spectra of AAH with adsorbed Cd show no obvious differences compared to the Cd-free spectrum. When AAH is coprecipitated with IHP, the spectrum intensity of P–OH vibration at ~883 and 932 cm–1 is reduced, and a new absorbance band at 1038 cm–1 appears, which is associated with the P–O–Cd symmetric stretching vibration [23]. This finding suggests that the adsorbed Cd(II) replaces hydrogen of the OH groups on the surface of pure AAH and AAH-IHP_high. However, the peak intensity of Al–OH vibration (~2427 cm–1) with or without adsorbed Cd(II) in AAH-IHP_high shows no apparent differences. This observation suggests that Cd(II) is mainly binding to the IHP molecules instead of AAH in the composites. Moreover, it is interesting that the characteristic peaks of P–O (~1176 cm–1) and C–C (~1724 cm–1) vibrations in AAH-IHP_high with adsorbed Cd(II) are enhanced. Possible explanation is because a part of IHP is desorbed from AAH-IHP coprecipitates in background electrolyte, and some of the free Cd ions occupy the adsorption sites of desorbed IHP on AAH, thus promoting the binding of desorbed IHP with the newly adsorbed Cd on the surface [23, 27].Figure 3
ATR-FTIR spectra of pure AAH and AAH-IHP coprecipitates (AAH-IHP_low and AAH-IHP_high) with or without adsorbed Cd.


## 3.4.1H Solid-State NMR Spectroscopy

In order to gain a deeper insight into fundamental binding mechanisms of OP interacted with AAH and their effects on binding of Cd(II), the1H NMR spectra of pure AAH and AAH-IHP_high with and without adsorbed Cd(II) were analyzed and the results are given in Figure 4. The 1H NMR spectra of pure AAH exhibit a main peak at δH−1=4.7 ppm, with two shoulders around 0.8 and 3.3 ppm, respectively. The 1H NMR peak at 4.7 ppm corresponds to the physically adsorbed water, and those at δH−1=0.8 and 3.3 ppm are assigned to the OH groups in AAH or IHP molecule [40]. When IHP is coprecipitated with AAH, the peak intensity at δH−1=0.8 and 3.3 increases and no new peak occurs. This result indicates that the chemical environment and speciation of OH groups in IHP molecule is very similar to that in AAH, and high IHP loading increases the number of OH groups. On the other hand, the presence of adsorbed Cd(II) decreases those characteristic peaks of OH groups at δH−1=0.8 and 3.3 ppm in all samples, corresponding to the reduced spectrum intensity at ~883, 932, and 2427 cm–1 observed in Figure 3. This finding demonstrates that Cd(II) binds to pure AAH and AAH-IHP coprecipitates by surface complexation with OH groups.Figure 4
The1H NMR spectra of pure AAH and AAH-IHP coprecipitates (AAH-IHP_low and AAH-IHP_high) with or without adsorbed Cd.


## 4. Discussion

Sorption onto mineral surfaces plays a key role in the mobility, speciation, and bioavailability of heavy metals, thus controlling their eventual fate in soils [41, 42]. The omnipresence of organic phosphorus (OP) can strongly interact with mineral phases, resulting in a change of the surface charge and reactive surface adsorption sites, and therefore the interaction of mineral surface with many toxic metals [27, 34]. This research represents a scenario in which Cd(II) occurs in natural environments where Al (hydr)oxides are associated with OP. The isotherm adsorption results indicate that high IHP loading promotes Cd(II) adsorption onto AAH through increasing the adsorption sites, while no obvious increase is observed with low P loading (Figure 2, Table 2). Li et al. [8] demonstrated that Zn(II) adsorption on γ-Al2O3 in the presence of glyphosate (GPS) is directly bonded with the carboxyl group of GPS and may form Zn−Al LDH precipitates. Li et al. [20] revealed that phosphate decreases the inner-sphere adsorption sites, thus reducing Cd(II) and Cu(II) adsorption on hematite. Collins et al. [11] indicated that the enhancement of Cd(II) adsorption onto goethite with coexisting phosphate and sulphate is solely by electrostatic interaction. Therefore, from these results, it could be concluded that the OP in the form of IHP may play several different roles in the ternary systems: (1) IHP molecules are bound to AAH with phosphate groups through the formation of inner-sphere surface complexes [25, 38], which increases the amount of reactive OH groups (Figure 4), and thus, the adsorption sites are enhanced; (2) at low concentration of IHP loading, the positive charge is reduced (Table 1), but meanwhile, IHP may compete with Cd for the AAH adsorption sites [20, 43, 44]; (3) when at high IHP loading, the AAH surfaces become more negatively charged, which enhances electrostatic interaction between the minerals and free Cd(II), and the adsorbed Cd(II) is mainly bound to the OH groups in IHP molecule instead of the mineral surface [8, 23].OP not only affects the number of adsorption sites, but also changes the metal species on the mineral surface. Yan et al. [26] revealed that IHP surface complex is formed on AAH when the reaction time is below 6 h; afterwards, the complexes are rapidly transformed to surface precipitates. Sun et al. [43] showed that less than 12% of Cd-Al LDH precipitates is emerged when Cd(II) is interacted with γ-Al2O3 in 18 h at 25°C. Recent researches confirmed that the preadsorbed OP hinders the formation of Zn−Al LDH precipitates on γ-Al2O3 [8, 34]. Therefore, in our experiment, we speculate that very few Cd−Al LDH precipitates are formed due to the limited reaction time (~35 min), and ternary surface complex is the main mechanism. To the best of our knowledge, ternary surface complexes can be further classified in general into the following: (1) a type A in which the adsorbed metal ions are near the mineral surface (i.e., S–M–L, where S, M, and L represent mineral surface, metal ions, and ligand, respectively) [8]; (2) a type B in which the adsorbed ligand is near the surface (i.e., S–L–M) [17]; or (3) a type C in which both the metal ion and ligand are near the surface (i.e., S–M–L–S) [16, 18]. It is well known that bivalent metal ions can coordinate with two phosphate groups of IHP molecules [45]. Meanwhile, our ATR-FTIR results show that the adsorbed Cd(II) reduces the characteristic peak of Al–OH vibration at 2427 cm–1 while no corresponding reduction is observed in AAH-IHP complexes. These results suggest that the free Cd(II) possibly associates with phosphate groups of AAH-IHP, which results in the formation of type A ternary surface complexes (AAH-IHP-Cd). In addition, our ATR-FTIR results show that the addition of Cd further promotes the readsorption of desorbed IHP in high IHP treatment, in agreement with the studies reported previously [23, 27]. This may be attributed to that a small proportion of Cd(II) is adsorbed by AAH, and the desorbed IHP further binds with the newly adsorbed Cd(II) due to the increased electrostatic attraction. With this in mind, there may appear type B and C complexes (AAH-Cd-IHP and AAH-Cd-IHP-Cd) in our ternary systems. Due to the formation of the above ternary surface complexes, the coexistence of OP may exert an great impact on the mobility of Cd(II) in Al minerals and Al-rich soil. Anthropogenic activities lead to the accumulation of both OP and Cd(II) in soil systems [46]. High OP loading enhances the adsorption on Al (hydr)oxides, therefore decreasing the availability of Cd(II) to plants. However, low OP loading results in no remarkable promoting effect on adsorption. This provides a new role of OP, that is to say, high OP accumulation in soils would to some extent reduce the environmental risk of Cd(II) and thus the exposure to biota. On the other hand, our study proposes an ideal for the remediation of heavy metal contaminated soils, that is, to use mineral-organic phosphorus composite to reduce the bioavailability of heavy metals as well as increasing essential phosphorus element for biological growth. Lastly, our study shows progress in the using of ATR-FTIR and NMR to investigate the molecular binding mechanism of heavy metals to mineral-organo composite, and this approach has the potential for wide application in the area of environmental science, where adsorption process is involved.


## 5. Conclusions

The results of this study show that OP facilitates Cd(II) adsorption onto Al hydroxides at high-dose IHP loading (204.71 mg/g), but nearly exhibits no effect at low IHP loading (107.63 mg/g). ATR-FTIR results show that the adsorbed Cd may have a slight promoting effect on IHP sorption to AAH in high IHP treatment. IHP interacts intensively with Al hydroxides by increasing the amount of reactive OH groups instead of changing the chemical environment and speciation of OH groups. IHP promotes Cd adsorption through surface complexation via binding with OH groups, and several structurally distinct ternary complexes are possibly formed. These findings indicate that coexisting OP at high concentration lowers Cd mobility in Al (hydr)oxides or Al-rich soils, and thus the risk to crop safety and human health.



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*Source: 9943663-2021-04-28.xml*