# Study on the Adsorption Mechanism of Graphene Oxide by Calcareous Sand in South China Sea

Authors: Beifeng Lv; Wenjie Yu; Jiale Luo; Biao Qian; Mulugeta Belete Asefa; Na Li
Journal: Adsorption Science & Technology
 (2021)

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## Abstract

To remove graphene oxide from wastewater, we used batch experiments with calcareous sand to recover GO. The adsorption properties and mechanisms of GO by calcareous sand were investigated by different characterization techniques. In this paper, the relationship between the coagulation of GO on calcareous sand and pH, calcareous sand content, GO initial concentration, and temperature was studied. The results show that calcareous sand can effectively adsorb GO from aqueous solution, the interaction of GO with calcareous sand achieved interaction equilibrium in 5 h, and the adsorption of GO by calcareous sand strongly depends on pH. The isotherm data fitted to a Langmuir equation. A possible mechanism can be expressed from FT-IR, XRD, Raman spectra, SEM, EDS, TEM, AFM, and XPS results. The test results indicate that calcareous sand is a potentially recoverable GO material.


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## Body

## 1. Introduction

In recent years, GO (graphene oxide) has gained unprecedented development due to its special structure and excellent physical and chemical properties [1, 2]. As one of the most excellent derivatives of graphene, GO has a layered structure with the epoxy group and hydroxyl group on its surface [3, 4]. With the widespread production and use of GO, GO will inevitably be discharged into the environment as a pollutant during production, transportation, use, and disposal. However, GO has been found to be toxic. Under certain conditions, it can cause harm to the human skin [5], lungs [6], and cells [7]. Therefore, in order to prevent GO from flowing into the natural ecosystem, it is necessary to study how to remove GO. At present, the main way to remove GO is to use adsorptive agent to adsorb GO; for this purpose, various chemical, physical, and biological methods were used for wastewater treatment which includes filtration, advanced oxidation, flocculation and coagulation, catalysis, photo and chemical degradation, and adsorption. Due to low cost and easy operation, adsorption is the most appropriate and reasonable choice for the removal of organic pollutants and inorganic heavy metal ions from wastewater [8, 9]. In existing studies, the main adsorbent for adsorbing GO is LDH. Although it shows a high adsorption capacity for GO, its production process is complex [10, 11], and the adsorption efficiency is still to be further improved by the maturity of the technology. Calcareous sand is an accumulation of carbonate material fragments, usually from shell fragments and bone fragments of marine organisms, the calcium carbonate content exceeds 50% and is widely distributed in the South China Sea, the Red Sea, the western continental platform of Australia, and the Bass Strait, covering about 40% of the land-sea interface [12, 13]. In recent years, calcareous soil has entered the field of adsorption of heavy metal ions [14, 15]. The adsorption of Cd, Cu, Fe, Mn, Ni, Zn, and other heavy metal ions on calcareous soil is superior [16, 17]. Among them, the adsorption effect of calcareous soil on zinc is particularly prominent, so that plants on the calcareous soil are generally deficient in zinc [18, 19], and as a result, the yield of crops on calcareous soils is greatly reduced. On the other hand, the general lack of zinc on crops will also cause the human body that depends on the grain-based diet to obtain the necessary zinc. Zinc is an indispensable trace element for the human body. Lack of zinc in the human body can cause a series of health problems, such as impaired body development, immune system, and brain function [20, 21]. At the same time, many studies have shown that the adsorption process of heavy metal ions by calcareous soil is a spontaneous endothermic process, and the adsorption capacity will increase with the increase of temperature [19, 22]. The description of the above study shows that calcareous soil has good adsorption capacity. However, the interaction between GO and calcareous sand has not been extensively studied systematically, calcareous sand is rich in calcium ions which can cause GO to solidify and thus adsorb to calcareous sand, and that the absorption of toxic GO from excess calcareous sand in the ocean, which could leak into the natural world, could not only make proper.In this work, using calcareous sand from the South China Sea to explore its adsorption effect on GO under different pH, calcareous sand content, GO concentration, and temperature conditions. The interaction between GO and calcareous sand and its role in GO removal have been conducted. The main objectives of this work contain the following aspects: (1) study the effects of pH, calcareous sand content, GO concentration, and temperature on the removal of GO by calcareous sand. (2) Fit the adsorption isotherm and thermodynamics of calcareous sand to remove GO. (3) Characterize the interaction of GO with calcareous sand by using spectroscopic and morphologic (FT-IR, Raman spectra, XPS, EDS, XRD, SEM, TEM, AFM) analyses and elucidate its role in GO removal. The work is expected to provide the fundamental experimental data of calcareous sand in South China Sea used to eliminate carbon nanomaterials from aqueous solutions.


## 2. Experimental Section

### 2.1. Materials

The GO aqueous solution was obtained from Suzhou Tanfeng Technology Co., Ltd. The graphene oxide was a high-purity single-layer graphene oxide freeze-dried by an improved Hummer method. The calcareous sand is collected from the reefs of the South China Sea, white, size below 2 mm. The minimum and maximumv pore ratios (emin and emax) are 1.37 and 1.85, respectively. Chemical analysis of calcareous contains 92.70% calcium, 3.94% magnesium, 1.82% strontium, 0.64% sodium, 0.54% phosphorus, 0.39% sulfur, and 0.27% aluminum.


### 2.2. Characterization

Using CuKα radiation, the crystal structure of the absorber was checked by X-ray diffractometer (XRD, Empyrean). The functional groups were identified by Fourier transform infrared spectroscopy (FTIR, NEXUS), and the scanning range was 400-4000 cm-1. Raman spectra are detected by Laser Confocal Micro-Raman Spectroscopy form Horiba Jobin Yvon (Raman Lab RAM HR800), and the exciter is 532 nm.The surface morphology was observed on with scanning electron microscope (SEM, JSM-6360LV), atomic force microscope (AFM, SPA400), and transmission electron microscope (JEOL JEM-1011). Energy dispersive X-ray spectroscopy (EDS) was performed on (OXFORD) X-act to detect the change of elements. Thermo ESCALAB 250 uses a focused monochromatic Al Ka X-ray source (hm=1486.6eV) for X-ray photoelectron spectroscopy (XPS) analysis. The zeta potential value was obtained by Zetasizer (ZS90) from Malvern Instruments.


### 2.3. Methods

The effect of certain factors, such as GO initial concentration 60 mg/L a, calcareous sand content 50 mg, temperature 30-50°C, and effects of pH, contact time, calcareous sand content, and GO initial concentrations on GO removal, was studied. Perform bath experiments in duplicate and use average data to evaluate adsorption performance.At the wavelength of 221 nm, the absorbance after adsorption is obtained by UV-Vis spectrophotometer. The calculation formula is as follows: (Eqs. (1)-(3)) [9].
(1)R=C0−CeC0×100%,(2)qe=C0−Ce×Vm,(3)Kd=qeCe,where C0 (mg·L−1) is the initial GO concentration of simulated solution, Ce (mg/L) is the concentrations at equilibrium, R% is the adsorption rate of GO by calcareous sand, qe (mg/g) is the adsorption capacity of GO by calcareous sand, m (g) is the content of calcareous sand, V (L) is the GO solution volume, Kd is the distribution coefficient.The fitting formula of the adsorption isotherm (Langmuir, Freundlich and Temkin) model is as follows (Eqs. (4)–(6)) [23]:
(4)1qe=1qm+1KL×qm×1Ce,(5)lnqe=lnKF+1n×lnCe,(6)qe=KT×lnf+KT×lnCe,where KL is the adsorption equilibrium constant of Langmuir, KF is the adsorption equilibrium constant of Freundlich, and KT is the adsorption equilibrium constant of Temkin.


## 2.1. Materials

The GO aqueous solution was obtained from Suzhou Tanfeng Technology Co., Ltd. The graphene oxide was a high-purity single-layer graphene oxide freeze-dried by an improved Hummer method. The calcareous sand is collected from the reefs of the South China Sea, white, size below 2 mm. The minimum and maximumv pore ratios (emin and emax) are 1.37 and 1.85, respectively. Chemical analysis of calcareous contains 92.70% calcium, 3.94% magnesium, 1.82% strontium, 0.64% sodium, 0.54% phosphorus, 0.39% sulfur, and 0.27% aluminum.


## 2.2. Characterization

Using CuKα radiation, the crystal structure of the absorber was checked by X-ray diffractometer (XRD, Empyrean). The functional groups were identified by Fourier transform infrared spectroscopy (FTIR, NEXUS), and the scanning range was 400-4000 cm-1. Raman spectra are detected by Laser Confocal Micro-Raman Spectroscopy form Horiba Jobin Yvon (Raman Lab RAM HR800), and the exciter is 532 nm.The surface morphology was observed on with scanning electron microscope (SEM, JSM-6360LV), atomic force microscope (AFM, SPA400), and transmission electron microscope (JEOL JEM-1011). Energy dispersive X-ray spectroscopy (EDS) was performed on (OXFORD) X-act to detect the change of elements. Thermo ESCALAB 250 uses a focused monochromatic Al Ka X-ray source (hm=1486.6eV) for X-ray photoelectron spectroscopy (XPS) analysis. The zeta potential value was obtained by Zetasizer (ZS90) from Malvern Instruments.


## 2.3. Methods

The effect of certain factors, such as GO initial concentration 60 mg/L a, calcareous sand content 50 mg, temperature 30-50°C, and effects of pH, contact time, calcareous sand content, and GO initial concentrations on GO removal, was studied. Perform bath experiments in duplicate and use average data to evaluate adsorption performance.At the wavelength of 221 nm, the absorbance after adsorption is obtained by UV-Vis spectrophotometer. The calculation formula is as follows: (Eqs. (1)-(3)) [9].
(1)R=C0−CeC0×100%,(2)qe=C0−Ce×Vm,(3)Kd=qeCe,where C0 (mg·L−1) is the initial GO concentration of simulated solution, Ce (mg/L) is the concentrations at equilibrium, R% is the adsorption rate of GO by calcareous sand, qe (mg/g) is the adsorption capacity of GO by calcareous sand, m (g) is the content of calcareous sand, V (L) is the GO solution volume, Kd is the distribution coefficient.The fitting formula of the adsorption isotherm (Langmuir, Freundlich and Temkin) model is as follows (Eqs. (4)–(6)) [23]:
(4)1qe=1qm+1KL×qm×1Ce,(5)lnqe=lnKF+1n×lnCe,(6)qe=KT×lnf+KT×lnCe,where KL is the adsorption equilibrium constant of Langmuir, KF is the adsorption equilibrium constant of Freundlich, and KT is the adsorption equilibrium constant of Temkin.


## 3. Results and Discussion

### 3.1. Adsorption Property

#### 3.1.1. Effect of Time

To investigate the effect of contact time on GO condensation on calcareous sand, separate adsorption processes were performed using calcareous sand content (50 mg) after different contact times (see Figure1). The adsorption curves clearly show that the deposition/coagulation of GO on calcareous sand increases rapidly over a short period of time, reaches equilibrium after 5 h, and then remains stable.Figure 1
Effect of the contact time on GO adsorption on calcareous sand.The GO removal rate increased from 20% to 92% within an increase in contact time from 0 to 5 hours, and theqe increases from 23 mg/g to 110 mg/g; Kd is also an increase from 0.5 to 22. At the initial contact time, the Ca2+ on the calcareous sand may play an important role in the adsorption of GO [24, 25], and the interaction between GO and calcareous sand is easy and rapid, thereby reducing the concentration of GO in the aqueous solution.


#### 3.1.2. Effect of pH

pH has a great influence on adsorption [26, 27]. The pH of the solution has a significant effect on the surface properties of the adsorbent [9], and qe, R, and Kd of GO on calcareous sand as a function of pH are shown in Figure 2(a). The zeta potential values of GO and calcareous sand/GO are also measured at different pH values, as shown in Figure 2(b). As shown in Figure 2(a), all the adsorption capacity, removal rate, and distribution coefficient of GO increase with increasing pH at pH<6 and then decreasing quickly with pH increasing at pH>6. The maximum adsorption capacity, removal rate, and distribution coefficient of GO by calcareous sand are 54.9 mg/g, 91.5%, and 10.8, respectively. Slightly higher than the adsorption capacity of GO with iron tailings (53.9 mg/g) [28], it can be seen from the zeta potential diagram that the zeta values of GO and calcareous sand/GO are both negative values, both of which are electrostatic repulsion; so, the adsorption that occurs in this process may be chemical adsorption, that is, in the oxygen-containing functional groups on the surface of GO and the hydrogen bonding and Lewis acid-base interaction in calcareous sand [29], the hydroxyl group on the surface of calcareous sand can be regarded as Lewis base, and the delocalized π electron on the surface of GO can be regarded as Lewis acid.Figure 2
Adsorption of GO on calcareous (a) effect of pH. (b) Zeta potentials of GO and calcareous sand/GO. (c) Effect of calcareous sand content. (d) GO initial concentration.
(a)(b)(c)(d)As shown in Figure2(b), when the pH is less than 5, the potential difference between GO and calcareous sand becomes smaller, indicating that the electrostatic repulsion between the two is decreasing, indicating that the hydrogen bond and Lewis acid-base interaction between GO and calcareous sand are relatively increasing. For the increase in adsorption capacity, however, when the pH is greater than 5, the potential difference gradually becomes larger; that is, the electrostatic repulsion between GO and calcareous sand is greater than the hydrogen bond and the Lewis acid-base effect, making the adsorption capacity weaker.


#### 3.1.3. Effect of Calcareous Sand Content

Figure2(c) presents the influence of m on the qe, R, and Kd of the GO adsorption. The result will provide an opportunity to expect less adsorbent consumption or higher adsorption efficiency. With the calcareous sand content increasing from 30 mg to 70 mg, removal rate and distribution coefficient of GO increase gradually, tending to 94% and 12.8, respectively. This is because as the content of calcareous sand increases, the Ca in calcareous sands also increases. However, the adsorption capacity of GO decreased. The adsorption capacity of calcareous sand for GO decreased. This is because increasing the content of calcareous sand under the premise of maintaining the GO concentration of 60 mg/L, resulting in a decrease in the adsorption capacity of calcareous sand per unit. This shows that we need to reasonably choose high removal rate (low residue) or high adsorption capacity (low adsorbent consumption) according to the actual application. [30]. In this study, 70 mg of calcareous sand was taken as an example for follow-up experiments.


#### 3.1.4. Effect of GO Initial Concentration

The removal of GO on calcareous sand was studied with differentC0 of 80, 100, 120, 140, and 160 mg/L, respectively. Figure 2(d) shows that the R is influenced by GO initial concentrations. It can be seen from Figure 2(d) that as the initial concentration of GO increases, the adsorption capacity of calcareous sand on GO increases, and the maximum can reach 103 mg/g, but the removal rate and distribution coefficient reach 100 gm/L at the initial concentration of GO; it began to decline afterwards, which may be due to the fact that calcareous sand has not yet reached saturation at a lower initial GO concentration, and the limited available calcareous sand quickly saturates at a higher initial GO concentration. [31]. Therefore, the initial GO concentration of 100 mg/L is the saturation point of calcareous sand adsorption.


### 3.2. Adsorption Isotherm and Thermodynamic Study

#### 3.2.1. Adsorption Isotherm

Figure3 shows the adsorption isotherm of go on calcareous sand. The fitting results of Langmuir model, Freundlich model, and Temkin model are shown in Table 1. It can be seen that with the increase of temperature, the adsorption capacity of calcareous sand on go gradually increases, and the maximum adsorption capacity calculated from different isotherms increases with the increase of temperature, indicating that the increase of temperature helps to improve the maximum adsorption capacity. It can be seen from Table 1 that the data show that for the adsorption of go on calcareous sand, the relevant parameters fitted by Langmuir model are higher; that is, Langmuir model is more suitable for the process. Therefore, we speculate that the adsorption of go on calcareous sand is mainly monolayer adsorption, and there is no lateral effect or steric hindrance between the adsorbed molecules and adjacent points, and the combination of GO and calcareous sand surface is driven by physical force and all positions equivalent in energy and the same affinity to GO [32, 33]. The Temkin model can also be fitted linearly to evaluate adsorption systems with heterogeneous surfaces. The correlation coefficient is as high as 0.96, indicating that the change of adsorption heat with adsorption capacity is not exponential, but linear energy [34, 35]. This may be due to the strong chemical bond interaction between GO and calcareous sand adsorbent.Figure 3
(a) Adsorption isotherms of GO on calcareous sand atT=303K, 313 K, and 323 K. Equilibrium adsorption isotherms fitted by (b) Langmuir model, (c) Freundlich model, and (d) Temkin model.
(a)(b)(c)(d)Table 1
Adsorption isotherm models parameters.
Model parametersLangmuirFreundlichTemkinqmKLR21/nKFR2KT (L/mg)fR2(mg/g)(L/mg)T/K303357.140.000.930.7016.490.9654.040.480.96313250.000.070.970.6323.490.9349.110.760.96323149.250.360.960.4645.730.9236.412.80.96


#### 3.2.2. Adsorption Thermodynamic

The temperature is a significant parameter for the adsorption process [36]. Figure 4 shows the effect of temperature on the removal of GO by calcareous sand. Obviously, the removal of GO by calcareous sand was more favorable at higher temperature. The thermodynamic parameters of the adsorption process, i.e., the values of standard Gibbs free energy (ΔG°), standard enthalpy (ΔH°), and standard entropy (ΔS°), are calculated by the following formulas (Eqs. (7) and (8)) [24]:
(7)lnKd=−△H°R×1T+△S°R,(8)lnKd=−△H°R×1T+△S°R,where T is the Kelvin absolute temperature, and R is the ideal gas constant, usually 8.314 J/(mol·K)). ΔH° can reflect whether the adsorption process is endothermic or exothermic, ΔS° represents whether the adsorption is entropy increase or entropy decrease, and ΔG° reflects whether the adsorption is spontaneous. The thermodynamic parameters are summarized in Table 2, ΔG° is a negative value, indicating that the adsorption reaction of GO on calcareous sand is a spontaneous process; ΔH° is a positive value, indicating that the adsorption of GO on calcareous sand is an endothermic process. The positive value may be due to the formation of new chemical bonds during the adsorption process, resulting in changes in the original structure [37, 38]. Thermodynamic studies show that the adsorption of GO on calcareous sand is a spontaneous endothermic reaction.Figure 4
Linear relationship between lnKd and 1/T (K−1) adsorbed by GO on calcareous sand.Table 2
Adsorption thermodynamic parameters.
AdsorbateC0ΔH°ΔS°ΔG° (kJ/Mol)(mg/L)(kJ/Mol)(kJ/Mol)303 K313 K323 KCalcareous sand8053.050.19-5.24-7.16-9.0910048.710.18-5.36-7.14-8.9312030.580.12-5.56-6.75-7.9414036.640.14-5.28-6.66-8.0516033.480.13-4.67-5.93-7.19


## 3.1. Adsorption Property

### 3.1.1. Effect of Time

To investigate the effect of contact time on GO condensation on calcareous sand, separate adsorption processes were performed using calcareous sand content (50 mg) after different contact times (see Figure1). The adsorption curves clearly show that the deposition/coagulation of GO on calcareous sand increases rapidly over a short period of time, reaches equilibrium after 5 h, and then remains stable.Figure 1
Effect of the contact time on GO adsorption on calcareous sand.The GO removal rate increased from 20% to 92% within an increase in contact time from 0 to 5 hours, and theqe increases from 23 mg/g to 110 mg/g; Kd is also an increase from 0.5 to 22. At the initial contact time, the Ca2+ on the calcareous sand may play an important role in the adsorption of GO [24, 25], and the interaction between GO and calcareous sand is easy and rapid, thereby reducing the concentration of GO in the aqueous solution.


### 3.1.2. Effect of pH

pH has a great influence on adsorption [26, 27]. The pH of the solution has a significant effect on the surface properties of the adsorbent [9], and qe, R, and Kd of GO on calcareous sand as a function of pH are shown in Figure 2(a). The zeta potential values of GO and calcareous sand/GO are also measured at different pH values, as shown in Figure 2(b). As shown in Figure 2(a), all the adsorption capacity, removal rate, and distribution coefficient of GO increase with increasing pH at pH<6 and then decreasing quickly with pH increasing at pH>6. The maximum adsorption capacity, removal rate, and distribution coefficient of GO by calcareous sand are 54.9 mg/g, 91.5%, and 10.8, respectively. Slightly higher than the adsorption capacity of GO with iron tailings (53.9 mg/g) [28], it can be seen from the zeta potential diagram that the zeta values of GO and calcareous sand/GO are both negative values, both of which are electrostatic repulsion; so, the adsorption that occurs in this process may be chemical adsorption, that is, in the oxygen-containing functional groups on the surface of GO and the hydrogen bonding and Lewis acid-base interaction in calcareous sand [29], the hydroxyl group on the surface of calcareous sand can be regarded as Lewis base, and the delocalized π electron on the surface of GO can be regarded as Lewis acid.Figure 2
Adsorption of GO on calcareous (a) effect of pH. (b) Zeta potentials of GO and calcareous sand/GO. (c) Effect of calcareous sand content. (d) GO initial concentration.
(a)(b)(c)(d)As shown in Figure2(b), when the pH is less than 5, the potential difference between GO and calcareous sand becomes smaller, indicating that the electrostatic repulsion between the two is decreasing, indicating that the hydrogen bond and Lewis acid-base interaction between GO and calcareous sand are relatively increasing. For the increase in adsorption capacity, however, when the pH is greater than 5, the potential difference gradually becomes larger; that is, the electrostatic repulsion between GO and calcareous sand is greater than the hydrogen bond and the Lewis acid-base effect, making the adsorption capacity weaker.


### 3.1.3. Effect of Calcareous Sand Content

Figure2(c) presents the influence of m on the qe, R, and Kd of the GO adsorption. The result will provide an opportunity to expect less adsorbent consumption or higher adsorption efficiency. With the calcareous sand content increasing from 30 mg to 70 mg, removal rate and distribution coefficient of GO increase gradually, tending to 94% and 12.8, respectively. This is because as the content of calcareous sand increases, the Ca in calcareous sands also increases. However, the adsorption capacity of GO decreased. The adsorption capacity of calcareous sand for GO decreased. This is because increasing the content of calcareous sand under the premise of maintaining the GO concentration of 60 mg/L, resulting in a decrease in the adsorption capacity of calcareous sand per unit. This shows that we need to reasonably choose high removal rate (low residue) or high adsorption capacity (low adsorbent consumption) according to the actual application. [30]. In this study, 70 mg of calcareous sand was taken as an example for follow-up experiments.


### 3.1.4. Effect of GO Initial Concentration

The removal of GO on calcareous sand was studied with differentC0 of 80, 100, 120, 140, and 160 mg/L, respectively. Figure 2(d) shows that the R is influenced by GO initial concentrations. It can be seen from Figure 2(d) that as the initial concentration of GO increases, the adsorption capacity of calcareous sand on GO increases, and the maximum can reach 103 mg/g, but the removal rate and distribution coefficient reach 100 gm/L at the initial concentration of GO; it began to decline afterwards, which may be due to the fact that calcareous sand has not yet reached saturation at a lower initial GO concentration, and the limited available calcareous sand quickly saturates at a higher initial GO concentration. [31]. Therefore, the initial GO concentration of 100 mg/L is the saturation point of calcareous sand adsorption.


## 3.1.1. Effect of Time

To investigate the effect of contact time on GO condensation on calcareous sand, separate adsorption processes were performed using calcareous sand content (50 mg) after different contact times (see Figure1). The adsorption curves clearly show that the deposition/coagulation of GO on calcareous sand increases rapidly over a short period of time, reaches equilibrium after 5 h, and then remains stable.Figure 1
Effect of the contact time on GO adsorption on calcareous sand.The GO removal rate increased from 20% to 92% within an increase in contact time from 0 to 5 hours, and theqe increases from 23 mg/g to 110 mg/g; Kd is also an increase from 0.5 to 22. At the initial contact time, the Ca2+ on the calcareous sand may play an important role in the adsorption of GO [24, 25], and the interaction between GO and calcareous sand is easy and rapid, thereby reducing the concentration of GO in the aqueous solution.


## 3.1.2. Effect of pH

pH has a great influence on adsorption [26, 27]. The pH of the solution has a significant effect on the surface properties of the adsorbent [9], and qe, R, and Kd of GO on calcareous sand as a function of pH are shown in Figure 2(a). The zeta potential values of GO and calcareous sand/GO are also measured at different pH values, as shown in Figure 2(b). As shown in Figure 2(a), all the adsorption capacity, removal rate, and distribution coefficient of GO increase with increasing pH at pH<6 and then decreasing quickly with pH increasing at pH>6. The maximum adsorption capacity, removal rate, and distribution coefficient of GO by calcareous sand are 54.9 mg/g, 91.5%, and 10.8, respectively. Slightly higher than the adsorption capacity of GO with iron tailings (53.9 mg/g) [28], it can be seen from the zeta potential diagram that the zeta values of GO and calcareous sand/GO are both negative values, both of which are electrostatic repulsion; so, the adsorption that occurs in this process may be chemical adsorption, that is, in the oxygen-containing functional groups on the surface of GO and the hydrogen bonding and Lewis acid-base interaction in calcareous sand [29], the hydroxyl group on the surface of calcareous sand can be regarded as Lewis base, and the delocalized π electron on the surface of GO can be regarded as Lewis acid.Figure 2
Adsorption of GO on calcareous (a) effect of pH. (b) Zeta potentials of GO and calcareous sand/GO. (c) Effect of calcareous sand content. (d) GO initial concentration.
(a)(b)(c)(d)As shown in Figure2(b), when the pH is less than 5, the potential difference between GO and calcareous sand becomes smaller, indicating that the electrostatic repulsion between the two is decreasing, indicating that the hydrogen bond and Lewis acid-base interaction between GO and calcareous sand are relatively increasing. For the increase in adsorption capacity, however, when the pH is greater than 5, the potential difference gradually becomes larger; that is, the electrostatic repulsion between GO and calcareous sand is greater than the hydrogen bond and the Lewis acid-base effect, making the adsorption capacity weaker.


## 3.1.3. Effect of Calcareous Sand Content

Figure2(c) presents the influence of m on the qe, R, and Kd of the GO adsorption. The result will provide an opportunity to expect less adsorbent consumption or higher adsorption efficiency. With the calcareous sand content increasing from 30 mg to 70 mg, removal rate and distribution coefficient of GO increase gradually, tending to 94% and 12.8, respectively. This is because as the content of calcareous sand increases, the Ca in calcareous sands also increases. However, the adsorption capacity of GO decreased. The adsorption capacity of calcareous sand for GO decreased. This is because increasing the content of calcareous sand under the premise of maintaining the GO concentration of 60 mg/L, resulting in a decrease in the adsorption capacity of calcareous sand per unit. This shows that we need to reasonably choose high removal rate (low residue) or high adsorption capacity (low adsorbent consumption) according to the actual application. [30]. In this study, 70 mg of calcareous sand was taken as an example for follow-up experiments.


## 3.1.4. Effect of GO Initial Concentration

The removal of GO on calcareous sand was studied with differentC0 of 80, 100, 120, 140, and 160 mg/L, respectively. Figure 2(d) shows that the R is influenced by GO initial concentrations. It can be seen from Figure 2(d) that as the initial concentration of GO increases, the adsorption capacity of calcareous sand on GO increases, and the maximum can reach 103 mg/g, but the removal rate and distribution coefficient reach 100 gm/L at the initial concentration of GO; it began to decline afterwards, which may be due to the fact that calcareous sand has not yet reached saturation at a lower initial GO concentration, and the limited available calcareous sand quickly saturates at a higher initial GO concentration. [31]. Therefore, the initial GO concentration of 100 mg/L is the saturation point of calcareous sand adsorption.


## 3.2. Adsorption Isotherm and Thermodynamic Study

### 3.2.1. Adsorption Isotherm

Figure3 shows the adsorption isotherm of go on calcareous sand. The fitting results of Langmuir model, Freundlich model, and Temkin model are shown in Table 1. It can be seen that with the increase of temperature, the adsorption capacity of calcareous sand on go gradually increases, and the maximum adsorption capacity calculated from different isotherms increases with the increase of temperature, indicating that the increase of temperature helps to improve the maximum adsorption capacity. It can be seen from Table 1 that the data show that for the adsorption of go on calcareous sand, the relevant parameters fitted by Langmuir model are higher; that is, Langmuir model is more suitable for the process. Therefore, we speculate that the adsorption of go on calcareous sand is mainly monolayer adsorption, and there is no lateral effect or steric hindrance between the adsorbed molecules and adjacent points, and the combination of GO and calcareous sand surface is driven by physical force and all positions equivalent in energy and the same affinity to GO [32, 33]. The Temkin model can also be fitted linearly to evaluate adsorption systems with heterogeneous surfaces. The correlation coefficient is as high as 0.96, indicating that the change of adsorption heat with adsorption capacity is not exponential, but linear energy [34, 35]. This may be due to the strong chemical bond interaction between GO and calcareous sand adsorbent.Figure 3
(a) Adsorption isotherms of GO on calcareous sand atT=303K, 313 K, and 323 K. Equilibrium adsorption isotherms fitted by (b) Langmuir model, (c) Freundlich model, and (d) Temkin model.
(a)(b)(c)(d)Table 1
Adsorption isotherm models parameters.
Model parametersLangmuirFreundlichTemkinqmKLR21/nKFR2KT (L/mg)fR2(mg/g)(L/mg)T/K303357.140.000.930.7016.490.9654.040.480.96313250.000.070.970.6323.490.9349.110.760.96323149.250.360.960.4645.730.9236.412.80.96


### 3.2.2. Adsorption Thermodynamic

The temperature is a significant parameter for the adsorption process [36]. Figure 4 shows the effect of temperature on the removal of GO by calcareous sand. Obviously, the removal of GO by calcareous sand was more favorable at higher temperature. The thermodynamic parameters of the adsorption process, i.e., the values of standard Gibbs free energy (ΔG°), standard enthalpy (ΔH°), and standard entropy (ΔS°), are calculated by the following formulas (Eqs. (7) and (8)) [24]:
(7)lnKd=−△H°R×1T+△S°R,(8)lnKd=−△H°R×1T+△S°R,where T is the Kelvin absolute temperature, and R is the ideal gas constant, usually 8.314 J/(mol·K)). ΔH° can reflect whether the adsorption process is endothermic or exothermic, ΔS° represents whether the adsorption is entropy increase or entropy decrease, and ΔG° reflects whether the adsorption is spontaneous. The thermodynamic parameters are summarized in Table 2, ΔG° is a negative value, indicating that the adsorption reaction of GO on calcareous sand is a spontaneous process; ΔH° is a positive value, indicating that the adsorption of GO on calcareous sand is an endothermic process. The positive value may be due to the formation of new chemical bonds during the adsorption process, resulting in changes in the original structure [37, 38]. Thermodynamic studies show that the adsorption of GO on calcareous sand is a spontaneous endothermic reaction.Figure 4
Linear relationship between lnKd and 1/T (K−1) adsorbed by GO on calcareous sand.Table 2
Adsorption thermodynamic parameters.
AdsorbateC0ΔH°ΔS°ΔG° (kJ/Mol)(mg/L)(kJ/Mol)(kJ/Mol)303 K313 K323 KCalcareous sand8053.050.19-5.24-7.16-9.0910048.710.18-5.36-7.14-8.9312030.580.12-5.56-6.75-7.9414036.640.14-5.28-6.66-8.0516033.480.13-4.67-5.93-7.19


## 3.2.1. Adsorption Isotherm

Figure3 shows the adsorption isotherm of go on calcareous sand. The fitting results of Langmuir model, Freundlich model, and Temkin model are shown in Table 1. It can be seen that with the increase of temperature, the adsorption capacity of calcareous sand on go gradually increases, and the maximum adsorption capacity calculated from different isotherms increases with the increase of temperature, indicating that the increase of temperature helps to improve the maximum adsorption capacity. It can be seen from Table 1 that the data show that for the adsorption of go on calcareous sand, the relevant parameters fitted by Langmuir model are higher; that is, Langmuir model is more suitable for the process. Therefore, we speculate that the adsorption of go on calcareous sand is mainly monolayer adsorption, and there is no lateral effect or steric hindrance between the adsorbed molecules and adjacent points, and the combination of GO and calcareous sand surface is driven by physical force and all positions equivalent in energy and the same affinity to GO [32, 33]. The Temkin model can also be fitted linearly to evaluate adsorption systems with heterogeneous surfaces. The correlation coefficient is as high as 0.96, indicating that the change of adsorption heat with adsorption capacity is not exponential, but linear energy [34, 35]. This may be due to the strong chemical bond interaction between GO and calcareous sand adsorbent.Figure 3
(a) Adsorption isotherms of GO on calcareous sand atT=303K, 313 K, and 323 K. Equilibrium adsorption isotherms fitted by (b) Langmuir model, (c) Freundlich model, and (d) Temkin model.
(a)(b)(c)(d)Table 1
Adsorption isotherm models parameters.
Model parametersLangmuirFreundlichTemkinqmKLR21/nKFR2KT (L/mg)fR2(mg/g)(L/mg)T/K303357.140.000.930.7016.490.9654.040.480.96313250.000.070.970.6323.490.9349.110.760.96323149.250.360.960.4645.730.9236.412.80.96


## 3.2.2. Adsorption Thermodynamic

The temperature is a significant parameter for the adsorption process [36]. Figure 4 shows the effect of temperature on the removal of GO by calcareous sand. Obviously, the removal of GO by calcareous sand was more favorable at higher temperature. The thermodynamic parameters of the adsorption process, i.e., the values of standard Gibbs free energy (ΔG°), standard enthalpy (ΔH°), and standard entropy (ΔS°), are calculated by the following formulas (Eqs. (7) and (8)) [24]:
(7)lnKd=−△H°R×1T+△S°R,(8)lnKd=−△H°R×1T+△S°R,where T is the Kelvin absolute temperature, and R is the ideal gas constant, usually 8.314 J/(mol·K)). ΔH° can reflect whether the adsorption process is endothermic or exothermic, ΔS° represents whether the adsorption is entropy increase or entropy decrease, and ΔG° reflects whether the adsorption is spontaneous. The thermodynamic parameters are summarized in Table 2, ΔG° is a negative value, indicating that the adsorption reaction of GO on calcareous sand is a spontaneous process; ΔH° is a positive value, indicating that the adsorption of GO on calcareous sand is an endothermic process. The positive value may be due to the formation of new chemical bonds during the adsorption process, resulting in changes in the original structure [37, 38]. Thermodynamic studies show that the adsorption of GO on calcareous sand is a spontaneous endothermic reaction.Figure 4
Linear relationship between lnKd and 1/T (K−1) adsorbed by GO on calcareous sand.Table 2
Adsorption thermodynamic parameters.
AdsorbateC0ΔH°ΔS°ΔG° (kJ/Mol)(mg/L)(kJ/Mol)(kJ/Mol)303 K313 K323 KCalcareous sand8053.050.19-5.24-7.16-9.0910048.710.18-5.36-7.14-8.9312030.580.12-5.56-6.75-7.9414036.640.14-5.28-6.66-8.0516033.480.13-4.67-5.93-7.19


## 4. Adsorption Mechanism

The mechanism of GO adsorption on calcareous sand was discussed from the FT-IR, XRD, Raman spectrum, SEM, TEM, AFM, and XPS analysis. The FT-IR spectra can effectively analyze the characterization of surface functional groups of GO adsorbed on calcareous sand [11]. As shown in Figure 5(a), the bands at approximately 3413 cm-1 are caused by the stretching vibrations of lattice water and -OH groups and 1612 cm-1 assigned to the H-O-H stretching and bending vibrations, respectively [39]. Comparing the spectra of GO, calcareous sand, and calcareous sand/GO after adsorption, the spectra of calcareous sand/GO are closer to those of calcareous sand, and the functional group does not change much, indicating that the surface of the adsorbed material is more covered by calcareous sand.Figure 5
FT-IR spectra of GO, calcareous sand, and calcareous sand/GO (a); XRD patterns of GO, calcareous sand, and calcareous sand/GO (b); and Raman spectra of GO and calcareous sand/GO (c).
(a)(b)(c)The obtained XRD patterns have overwhelming support for estimating the structure of the adsorbent before and after adsorption [40]. The XRD patterns of GO, calcareous sand, and calcareous sand/GO are shown in Figure 5(b). From Figure 5(b), we can see that the typical peaks of calcareous sand/GO after adsorption are basically the same as those of calcareous sand before adsorption, which indicates that the structure of calcareous sand will not be destroyed after GO adsorption [41], and it is also consistent with the FT-IR test results. Most of the material obtained after calcareous sand adsorbs GO that is calcareous sand or calcareous sand adheres to GO.Raman spectroscopy is used to study the degree of order on the surface of adsorption composites [42, 43]. Figure 5(c) shows the Raman spectrum of calcareous sand/GO obtained by the adsorption of GO and calcareous sand. There are two distinct characteristic peaks of GO at 1350 cm-1 and 1580 cm-1 [44, 45], which are consistent with the D band and G band reported in the literature. The D band originates from the stretching vibration of the sp3 carbon atom, causing defects and misalignment, while the G band originates from the stretching vibration of the sp2 carbon atom, which corresponds to the first-order scattering of the E2g mode [46]. The peak position of calcareous sand has shifted after the adsorption of GO, and after the adsorption occurs, the relative intensity ratio (ID/IG) increased significantly and disorderly increased. This conclusion is also consistent with the FT-IR and XRD test results.The morphologies and structure of adsorption materials are shown in Figure6. The surface morphology of GO was studied by TEM and SEM, and the images are shown in Figures 6(a) and 6(d). The SEM and TEM images of GO show a characteristic two-dimensional structure with many wrinkles, which is the typical morphology of GO reported in many preliminary works [47]. It can be seen from Figure 6(b) that calcareous sand is needle-like and plate-like crystal grains, with many cavities on its surface and inside [48, 49]; so, it is conducive to its adsorption of GO. Observe the SEM figure (Figure 6(c)) of the substance obtained after the calcareous sand adsorbs GO, and the surface becomes flat, indicating that the calcareous sand with many holes on the surface is filled by GO after the adsorption. Meanwhile, it can be seen from Figures 6(d) and 6(e) that the surface morphology of GO changed obviously after adsorption, and a lot of black substances were attached to the surface; so, it can be inferred that calcareous sand has adsorbed GO. In order to further verify that calcareous sand adsorbs GO and the two are fused with each other, the chemical composition of the material before and after adsorption is analyzed by EDS test; the test results are shown in Figures 6(f)–6(h). The result of EDS shows that the content of C and O elements on calcareous sand increases, indicating that GO is in calcareous sand.Figure 6
SEM images of GO (a), calcareous sand (b), and calcareous sand/GO (c). TEM images of GO (d) and calcareous sand/GO (e), EDS images of GO (f), calcareous sand (g) and calcareous sand/GO (h).
(a)(b)(c)(d)(e)(f)(g)(h)AFM analysis provides an effective method for characterizing the microstructure [50]. Figure 7 shows the AFM images of GO and calcareous sand/GO. The AFM micrograph and height profile of the synthesized GO are shown in Figure 7(a). it is found that the thickness of GO is about 0.5 nm, and the thickness of the calcareous sand/GO after adsorption is close to 12 nm, indicating that the thickness of the adsorbed material increases after adsorption, which is consistent with the results in SEM and TEM images. However, the surface of calcareous sand has become smoother. This may be because the GO has adsorbed and gathered to a point. This can also be verified from the height distribution map. The height distribution of GO is more concentrated around 7 nm, while the calcareous sand/GO is less concentrated around 12 nm.Figure 7
AFM image of GO (a) and calcareous sand/GO (b).
(a)(b)XPS was used to further analyze the GO adsorption mechanism of calcareous sand. As shown in Figure8(a), the peaks for N 1 s, C 1 s, and O 1 s are all observed for GO before and after adsorption. It can be observed that the strength of C 1 s peak enhances after GO coagulation, indicating the strong adsorption of GO on calcareous sand [26]. The high deconvolution of C 1 s spectrum before and GO adsorption is shown in Figure 8(b) and observes that the C 1 s spectrum before GO is adsorbed; it can be deconvoluted into three components at 284.7, 287.0, and 288.5 eV [51–53], which are assigned to C-C, C-O, and O-C=O groups, respectively. However, after GO is adsorbed by calcareous sand, the area for the peak assigned to O-C=O increases, and the peak position of O-C=O changes from 288.5 eV to 290.0 eV. The change of the area and position of O-C=O shows that the interaction of GO with calcareous sand is conducted by O-C=O in the adsorption process [54]. It can be seen from the above analysis that GO can be effectively removed by adsorbing go on the surface of calcareous sand.Figure 8
XPS spectra (a). The high C 1 s deconvolution (b).
(a)(b)


## 5. Conclusion

The interaction between GO and calcareous sand was systematically studied by adsorbing GO on calcareous sand. The interaction between GO and calcareous sand was studied by the combination of adsorption test and micromorphology characterization. The results show that the contact time, pH content, and initial concentration of GO will affect the adsorption process of GO adsorbed by calcareous sand. The adsorption capacity of GO by calcareous sand first increases and then decreases with the increase of pH and decreases with the increase of calcareous sand content, but increases with the increase of initial concentration of GO. Through microscopic characterization, it was found that after calcareous sand adsorbed GO, GO attached to the surface of calcareous sand, and the adsorption process was accompanied by the change of functional groups. The results show that GO is easy to interact with calcareous sand, thus affecting its environmental behavior.At the same time, calcareous sand is widely used as a construction material [55], and it is therefore foreseeable that the addition of calcareous sand as a construction material in the construction of GO contaminated sites could also adsorb GO from contaminated sites to avoid GO harming human health through the water cycle, indicating that the adsorption potential of calcareous sand for GO is very high.



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*Source: 2227570-2021-11-23.xml*