# Snail Shells Adsorbent for Copper Removal from Aqueous Solutions and the Production of Valuable Compounds

Authors: Redouane Ouafi; Meryem Asri; Anass Omor; Mustapha Taleb; Zakia Rais
Journal: Journal of Chemistry
 (2021)

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## Abstract

This research explored the efficiency of snail shells powder (SSP) for Cu(II) removal from aqueous solutions and the production of valuable compounds from the residual product. To confirm its chemical and mineral components, the material was characterized by different instrumental techniques. The effects of experimental parameters such as the pH of the solution, the effect of SSP dose, particle size, and initial concentration of Cu(II) on the removal process were studied. The removal of Cu(II) was reasonably fast to be completed within a time frame of 90 min. The kinetics following the pseudo-second-order model (R2 = 0.979) were better compared to the pseudo-first-order model (R2 = 0.896). The increase in pH values leads to an increase in the amount of Cu(II) adsorbed. Afterward, the adsorption capacity reaches stability at pH near 7. The maximum Cu(II) removal occurred with a mass of 8 g·L−1 and a particle size of 300 μm. This particle size presents approximately 44.5% of SSP particles, which is the largest proportion of the sample as shown by particle size analysis. The adsorption isotherm was well described by Langmuir and Freundlich equations. The thermodynamic parameters values showed that the Cu(II) adsorption was a spontaneous and exothermic process. Furthermore, with the presence of CaCO3, the precipitation of Cu(II) in the form of posnjakite occurred with a high Cu(II) removal rate close to 99%. The residual SSP was used for the production of valuable compounds through the thermal decomposition process at various temperatures.


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## Body

## 1. Introduction

Their persistence against chemical and biological decomposition and their great environmental mobility characterize heavy metals. They exhibit an extreme bioaccumulation tendency in the food chain, thus exposing human and environmental health to slow but certain poisoning [1]. Heavy metals such as cobalt (Co), copper (Cu), chromium (Cr), iron (Fe), magnesium (Mg), manganese (Mn), molybdenum (Mo), nickel (Ni), selenium (Se), and zinc (Zn) are essential nutrients [2]. They are involved in very low concentrations in various biochemical and physiological functions necessary to maintain the metabolism of the human body, plants, and animals [3]. However, at high concentrations, these micronutrients can cause various effects on human health, including cardiovascular disease, developmental abnormalities, nervous system damage, neurological disorders, diabetes, reduced growth, hematological and immunological disorders, various types of cancer, and, in extreme cases, death [4, 5].Cu enzymes are involved in several metabolic processes, such as the use of oxygen during cell respiration and energy utilization. They also participate in the production of essential compounds such as the diverse proteins of the skeleton's connective tissues and blood vessels. The adult human body was estimated to contain from 50 to 120 mg of Cu [2]. Cu is one of the most valuable and commonly used metals in many industrial applications, such as metal surface treatment, electroplating, and foundries [6, 7]. It is a toxic metal even at low concentrations and is generally found at high concentrations in wastewater. Therefore, Cu-contaminated wastewater must be treated before being discharged into the environment. New easy-to-implement technologies deserve special attention. Indeed, adsorption using low-cost natural material to remove heavy metals from wastewater has proven its worth as a promising alternative to traditional physicochemical methods. These available and inexpensive materials can be involved in an effective and economically attractive remediation process [8]. In recent decades, a growing interest in low-cost adsorbents has been observed. Due to their many advantages, they have been extensively used for heavy metals and removal of other pollutants [9, 10]. Therefore, various materials have been investigated as adsorbents to remove different types of pollutants from aqueous solutions [11–13]. These materials include chitosan [14, 15], bentonite [16], almond shell [17], pistachio wood [18], Ballota biomass [19], chicken eggshell [20], and oyster shell [21].In common with the incessant search for cheaper, feasible, and effective products for removal of heavy metals and environmental restoration, the ability of the snail shells for Cu(II) removal from contaminated aqueous solutions was explored in the present research. Snail shells are an abundant, inexpensive, and natural waste. Snails are appreciated as gastronomic food in several countries including Morocco. They provide an easily harvested source of protein for local communities, discarding the shells as waste [22]. Using these shells as an adsorbent turns waste material into a potentially useful resource. The characterization of the product was carried out by using scanning electron microscope (SEM), energy dispersive X-ray spectroscopy (EDX), Fourier transform infrared spectroscopy (FTIR), the point of zero charge (pHpzc), and X-ray diffraction analysis (DRX). The influence of pH of solutions, SSP dose, particle size, and initial Cu(II) concentration on the Cu(II) removal efficiency by SSP was studied through the batch method. The kinetic studies and mechanism adsorption between Cu(II) and SSP were discussed. The isotherm models and thermodynamic parameters were investigated. The production of valuable products in a single simple operation was also examined.


## 2. Materials and Methods

### 2.1. Adsorbent Material Preparation

The snail shells were collected from ambulant merchants in Fez, Morocco. They were washed several times with tap water and then oven-dried at 80°C for 2 hours. The shells were crushed in an agate mortar; impurities such as the flesh were removed. They were finally washed several times with distilled water and dried in an oven at 100°C for 12 hours. The above-dried shells were grounded to a fine powder. The resulting SSP was sieved through a range of sieves. The different resulting powders were collected and used for experimental purposes.


### 2.2. Aqueous Metal Ions Solutions Preparation

The solutions of Cu(II) were prepared by dissolving 3.927 g of CuSO4.5H2O in deionized water (Barnstead EASYpure II) to achieve a concentration of 1000 mg·L−1. Experimental solutions of the desired concentrations of metal ions were prepared by diluting the stock solution in deionized water. The pH of the solutions was adjusted using 0.1 N HCl and 0.1 N NaOH to achieve a pH value ranging from 2 to 8; measurements were performed using a Hanna pH-meter model HI 2221. All reagents were AR-grade reagents obtained from Sigma-Aldrich Chemical Company.


### 2.3. Physicochemical Characterization

#### 2.3.1. Fourier Transform Infrared Spectroscopy

Fourier transform infrared spectroscopy (FTIR) analysis was recorded using a Bruker FTIR spectrophotometer model Vertex 70 (Germany) in the range of 400–4000 cm−1, using ATR mode; 16 scans were accumulated at a resolution of 4 cm−1.


#### 2.3.2. Scanning Electron Microscopy

Morphological and elemental composition analyses were carried out using a JEOL JSM IT500HR (Japan) scanning electron microscope equipped with an energy dispersive X-ray spectroscopy (EDX) operated under high vacuum mode, a landing voltage (HV) of 10–12 kV, and a working distance (WD) of 10.5 mm.


#### 2.3.3. X-Ray Diffraction Analysis

X-ray diffraction (XRD) analysis was obtained using a Panalytical X'Pert Pro X-ray diffractometer (Netherlands) equipped with a Cu-Kα monochromatic source (1.54 Å), operating at a voltage of 40 kV and a filament current of 40 mA. The diffraction pattern was recorded from 10° to 90° (2θ) with continuous scanning at a step size of 0.017 (2θ) and a scan step time of 45.08 s.


#### 2.3.4. Thermogravimetric Analysis

Thermogravimetric Analysis (TGA) and Differential Thermal Analysis (DTA) of the SSP were performed using a SHIMADZU DTG-60H (Japan) instrument under air atmosphere, with a heating rate of 20°C/min from 27 to 1000°C. The sample mass introduced was 27.40 mg.


#### 2.3.5. Particle Size Analysis

The particle size analysis was conducted using an AS 200 RETSCH analytical sieving machine (Germany) through a series of sieves in accordance with ISO3310-1. A sample of 200 g of SSP was removed and sieved for 40 minutes at an amplitude of 1.8 mm; the resulting refusal is collected and weighed.


#### 2.3.6. Specific Surface Area

The specific surface area (SBET) was measured using a Gemini VII 2390t surface area analyzer, Micromeritics Instruments Corp. (United States). The values SBET of SPP were determined from the N2 adsorption isotherms by applying the Brunauer–Emmett–Teller (BET) equation at a relative pressure range of 0.05–0.30 and an average area per molecule of N2 in a completed monolayer (σm) of 0.1620 nm2.


#### 2.3.7. Point of Zero Charge

The point of zero charge (pHpzc) is an important feature that determines the pH at which the surface of the adsorbent has net electrical neutrality. At this value, the acidic or basic functional groups no longer contribute to the pH of the solution. The adsorption of the cations will be more favorable at pH higher than pHpzc. The pHpzc of SSP was determined by the solid addition method in our previous study [23].


### 2.4. Batch Adsorption Experiments

The experiments in batch modes were carried out by bringing into contact in 100 mL flasks a determined quantity of adsorbents, with 50 mL of a synthetic solution of the metal ion at the desired concentration. The flasks were stirred in a shaker incubator (Cleaver Scientific Ltd.) at a constant speed and temperature of 25°C. After sufficient contact time, allowing the adsorption to reach equilibrium, the solutions were collected and the supernatant was separated by centrifugation at 4000 rpm for 5 min using Hettich Universal 320 centrifuge. Afterward, the Cu(II) concentration in the supernatant was determined using inductively coupled plasma-atomic emission spectroscopy (ICP-AES), model Activa from Horiba Jobin-Yvon (French). The solid residue collected was dried at atmospheric conditions for phase identification. The amount of heavy metal ions sequestratedqe (mg·g−1) was calculated by the following expression [24, 25]:(1)qe=C0−CeVm.The Cu(II) elimination rateR (%) was defined by(2)R%=C0−CeC0×100,where C0 is the initial metal ion concentration in the solution (mg·L−1), Ce is the residual metal ion concentration measured at equilibrium (mg·L−1), m is the mass of adsorbents introduced in solution (g), and V is the volume of the Cu(II) solution (L).


### 2.5. Kinetic Study

The kinetic study was carried out by using a method similar to batch adsorption experiments. After specified time intervals, the solutions of the flasks were collected and the supernatant was separated by centrifugation. The amount of metal ions adsorbed at timet, qt (mg·g−1), was calculated from the following expression:(3)qt=C0−CtVm,where C0 and Ct are the initial metal ion concentration and concentration at a defined time (mg·L−1), V is the solution volume (L), and m is the mass of the adsorbent (g).In this study, pseudo-first-order model (PFO) [26], pseudo-second-order model (PSO) [27], and Elovich [28] were employed to analyze the adsorption kinetics of Cu(II) by SSP.The PFO equation can be expressed in the following linear form:(4)lnqe−qt=lnqe−k1t.The PSO equation can be expressed in the following linear form:(5)tqt=1k2qe2+1qet,where qt is the amount of adsorbate adsorbed at time t (mg·g−1) calculated using equation (3), qe is the equilibrium adsorption capacity (mg·g−1), k1 is the pseudo-first-order rate constant (min−1), k2 (g·mg−1·min−1) is the pseudo-second-order rate constant, and t is the contact time (min).The plot of ln (qe − qt) versus t gives a straight line for the pseudo-first adsorption kinetics, which allows the determination of k1 from the slope and qe from the y-intercept. For the pseudo-second-order adsorption kinetics, qe and k2 can be determined from the intercept of the linearized plot of t/qt versus t.The Elovich equation can be expressed mathematically as follows:(6)qt=1βlnt+1βlnαβ,where α is the initial rate constant (mg·g−1·min−1) and β (mg·g−1) is the desorption constant at time t. The parameters α and β can be calculated from the slope (1/β) and intercept (1/β)ln(α β) of the linear plot of qt versus ln(t) with β = 1/slope and α = exp(intercept × β)/β.


### 2.6. Effects of Experimental Parameters on Cu(II) Removal

#### 2.6.1. Effect of pH

The effect of pH on the adsorption process was examined maintaining the described batch adsorption experiments and varying the pH of the solution from 2 to 8. The initial Cu(II) concentration was 100 mg·L−1 and the mass of the adsorbent was 0.4 g. The mixture was shaken for 90 min at an agitation speed equal to 200 rpm and a temperature equal to 25°C.


#### 2.6.2. Effect of Adsorbent Dose

The effect of adsorbent dose was determined by maintaining the described batch adsorption experiments and varying the amount of SSP from 0.05 to 1.2 mg. The initial Cu(II) concentration was 100 mg·L−1 and pH was 4.7. The mixture was shaken for 90 min at an agitation speed equal to 200 rpm and a temperature equal to 25°C.


#### 2.6.3. Effect of Particle Size

The effect of particle size of SSP was examined through different particle sizes from 50 to 800μm. The initial Cu(II) concentration was 100 mg·L−1 and the mass of the adsorbent was 0.4 g. The mixture was shaken for 90 min at an agitation speed equal to 200 rpm, a temperature equal to 25°C, and a pH equal to 4.7.


#### 2.6.4. Effect of Initial Metal Concentration

The effect of metal concentration on Cu(II) elimination rate was examined by varying the Cu(II) concentration from 50 to 500 mg·L−1. The adsorbent mass was 0.4 g and the particle size was 300 μm. The mixture was shaken for 90 min at an agitation speed equal 200 rpm, a temperature equal to 25°C, and a pH equal to 4.7.


### 2.7. Equilibrium Isotherm

Langmuir [29] and Freundlich [30] models were used to investigate and describe adsorption removal processes. The models were used to describe the distribution of metal ions between liquid and solid phases. The nonlinear method was used to calculate the parameters of the isotherms using the original form of the equation [31]. The isotherms models were fitted through Levenberg-Marquardt algorithm using OriginPro software.


### 2.8. Thermodynamic Study

The thermodynamic parameters were investigated at 298, 313, 323, and 333 K. The standard free energy change (∆Gº), standard enthalpy change (∆Hº), and standard entropy change (∆Sº) were calculated according to the following equations [24]:(7)ΔG°=−RTlnKc,ΔG°=ΔH°−TΔS°,lnKc=−ΔH°R1T+ΔS°R,where R is the universal gas constant (8.3144 J·mol−1·K−1), T is the absolute temperature in Kelvin (K), and Kc is the equilibrium constant.According to previous works, the equilibrium constantKc must be dimensionless and could be derived from the Langmuir constant using the following equation [32–34]:(8)Kc=63.54×55.5×1000×KL,where 55.5 (mol·L−1) is the number of moles of pure water per litre, 63.54 (g·mol−1) is the molecular weight of Cu, 1000 (g·L−1) is the value of the water density, and KL is the Langmuir constant (L·mg−1).


### 2.9. Thermal Treatment of the Residual Product

The residual product obtained after the Cu(II) removal by SSP was used as a precursor to produce mixed oxide. A simple one-step thermal decomposition method was used. For this purpose, 20 g of the residual product was calcined at 700, 900, and 1000°C for 120 min under an air atmosphere. The thermal treatment was performed with a Nabertherm P330 muffle furnace.


## 2.1. Adsorbent Material Preparation

The snail shells were collected from ambulant merchants in Fez, Morocco. They were washed several times with tap water and then oven-dried at 80°C for 2 hours. The shells were crushed in an agate mortar; impurities such as the flesh were removed. They were finally washed several times with distilled water and dried in an oven at 100°C for 12 hours. The above-dried shells were grounded to a fine powder. The resulting SSP was sieved through a range of sieves. The different resulting powders were collected and used for experimental purposes.


## 2.2. Aqueous Metal Ions Solutions Preparation

The solutions of Cu(II) were prepared by dissolving 3.927 g of CuSO4.5H2O in deionized water (Barnstead EASYpure II) to achieve a concentration of 1000 mg·L−1. Experimental solutions of the desired concentrations of metal ions were prepared by diluting the stock solution in deionized water. The pH of the solutions was adjusted using 0.1 N HCl and 0.1 N NaOH to achieve a pH value ranging from 2 to 8; measurements were performed using a Hanna pH-meter model HI 2221. All reagents were AR-grade reagents obtained from Sigma-Aldrich Chemical Company.


## 2.3. Physicochemical Characterization

### 2.3.1. Fourier Transform Infrared Spectroscopy

Fourier transform infrared spectroscopy (FTIR) analysis was recorded using a Bruker FTIR spectrophotometer model Vertex 70 (Germany) in the range of 400–4000 cm−1, using ATR mode; 16 scans were accumulated at a resolution of 4 cm−1.


### 2.3.2. Scanning Electron Microscopy

Morphological and elemental composition analyses were carried out using a JEOL JSM IT500HR (Japan) scanning electron microscope equipped with an energy dispersive X-ray spectroscopy (EDX) operated under high vacuum mode, a landing voltage (HV) of 10–12 kV, and a working distance (WD) of 10.5 mm.


### 2.3.3. X-Ray Diffraction Analysis

X-ray diffraction (XRD) analysis was obtained using a Panalytical X'Pert Pro X-ray diffractometer (Netherlands) equipped with a Cu-Kα monochromatic source (1.54 Å), operating at a voltage of 40 kV and a filament current of 40 mA. The diffraction pattern was recorded from 10° to 90° (2θ) with continuous scanning at a step size of 0.017 (2θ) and a scan step time of 45.08 s.


### 2.3.4. Thermogravimetric Analysis

Thermogravimetric Analysis (TGA) and Differential Thermal Analysis (DTA) of the SSP were performed using a SHIMADZU DTG-60H (Japan) instrument under air atmosphere, with a heating rate of 20°C/min from 27 to 1000°C. The sample mass introduced was 27.40 mg.


### 2.3.5. Particle Size Analysis

The particle size analysis was conducted using an AS 200 RETSCH analytical sieving machine (Germany) through a series of sieves in accordance with ISO3310-1. A sample of 200 g of SSP was removed and sieved for 40 minutes at an amplitude of 1.8 mm; the resulting refusal is collected and weighed.


### 2.3.6. Specific Surface Area

The specific surface area (SBET) was measured using a Gemini VII 2390t surface area analyzer, Micromeritics Instruments Corp. (United States). The values SBET of SPP were determined from the N2 adsorption isotherms by applying the Brunauer–Emmett–Teller (BET) equation at a relative pressure range of 0.05–0.30 and an average area per molecule of N2 in a completed monolayer (σm) of 0.1620 nm2.


### 2.3.7. Point of Zero Charge

The point of zero charge (pHpzc) is an important feature that determines the pH at which the surface of the adsorbent has net electrical neutrality. At this value, the acidic or basic functional groups no longer contribute to the pH of the solution. The adsorption of the cations will be more favorable at pH higher than pHpzc. The pHpzc of SSP was determined by the solid addition method in our previous study [23].


## 2.3.1. Fourier Transform Infrared Spectroscopy

Fourier transform infrared spectroscopy (FTIR) analysis was recorded using a Bruker FTIR spectrophotometer model Vertex 70 (Germany) in the range of 400–4000 cm−1, using ATR mode; 16 scans were accumulated at a resolution of 4 cm−1.


## 2.3.2. Scanning Electron Microscopy

Morphological and elemental composition analyses were carried out using a JEOL JSM IT500HR (Japan) scanning electron microscope equipped with an energy dispersive X-ray spectroscopy (EDX) operated under high vacuum mode, a landing voltage (HV) of 10–12 kV, and a working distance (WD) of 10.5 mm.


## 2.3.3. X-Ray Diffraction Analysis

X-ray diffraction (XRD) analysis was obtained using a Panalytical X'Pert Pro X-ray diffractometer (Netherlands) equipped with a Cu-Kα monochromatic source (1.54 Å), operating at a voltage of 40 kV and a filament current of 40 mA. The diffraction pattern was recorded from 10° to 90° (2θ) with continuous scanning at a step size of 0.017 (2θ) and a scan step time of 45.08 s.


## 2.3.4. Thermogravimetric Analysis

Thermogravimetric Analysis (TGA) and Differential Thermal Analysis (DTA) of the SSP were performed using a SHIMADZU DTG-60H (Japan) instrument under air atmosphere, with a heating rate of 20°C/min from 27 to 1000°C. The sample mass introduced was 27.40 mg.


## 2.3.5. Particle Size Analysis

The particle size analysis was conducted using an AS 200 RETSCH analytical sieving machine (Germany) through a series of sieves in accordance with ISO3310-1. A sample of 200 g of SSP was removed and sieved for 40 minutes at an amplitude of 1.8 mm; the resulting refusal is collected and weighed.


## 2.3.6. Specific Surface Area

The specific surface area (SBET) was measured using a Gemini VII 2390t surface area analyzer, Micromeritics Instruments Corp. (United States). The values SBET of SPP were determined from the N2 adsorption isotherms by applying the Brunauer–Emmett–Teller (BET) equation at a relative pressure range of 0.05–0.30 and an average area per molecule of N2 in a completed monolayer (σm) of 0.1620 nm2.


## 2.3.7. Point of Zero Charge

The point of zero charge (pHpzc) is an important feature that determines the pH at which the surface of the adsorbent has net electrical neutrality. At this value, the acidic or basic functional groups no longer contribute to the pH of the solution. The adsorption of the cations will be more favorable at pH higher than pHpzc. The pHpzc of SSP was determined by the solid addition method in our previous study [23].


## 2.4. Batch Adsorption Experiments

The experiments in batch modes were carried out by bringing into contact in 100 mL flasks a determined quantity of adsorbents, with 50 mL of a synthetic solution of the metal ion at the desired concentration. The flasks were stirred in a shaker incubator (Cleaver Scientific Ltd.) at a constant speed and temperature of 25°C. After sufficient contact time, allowing the adsorption to reach equilibrium, the solutions were collected and the supernatant was separated by centrifugation at 4000 rpm for 5 min using Hettich Universal 320 centrifuge. Afterward, the Cu(II) concentration in the supernatant was determined using inductively coupled plasma-atomic emission spectroscopy (ICP-AES), model Activa from Horiba Jobin-Yvon (French). The solid residue collected was dried at atmospheric conditions for phase identification. The amount of heavy metal ions sequestratedqe (mg·g−1) was calculated by the following expression [24, 25]:(1)qe=C0−CeVm.The Cu(II) elimination rateR (%) was defined by(2)R%=C0−CeC0×100,where C0 is the initial metal ion concentration in the solution (mg·L−1), Ce is the residual metal ion concentration measured at equilibrium (mg·L−1), m is the mass of adsorbents introduced in solution (g), and V is the volume of the Cu(II) solution (L).


## 2.5. Kinetic Study

The kinetic study was carried out by using a method similar to batch adsorption experiments. After specified time intervals, the solutions of the flasks were collected and the supernatant was separated by centrifugation. The amount of metal ions adsorbed at timet, qt (mg·g−1), was calculated from the following expression:(3)qt=C0−CtVm,where C0 and Ct are the initial metal ion concentration and concentration at a defined time (mg·L−1), V is the solution volume (L), and m is the mass of the adsorbent (g).In this study, pseudo-first-order model (PFO) [26], pseudo-second-order model (PSO) [27], and Elovich [28] were employed to analyze the adsorption kinetics of Cu(II) by SSP.The PFO equation can be expressed in the following linear form:(4)lnqe−qt=lnqe−k1t.The PSO equation can be expressed in the following linear form:(5)tqt=1k2qe2+1qet,where qt is the amount of adsorbate adsorbed at time t (mg·g−1) calculated using equation (3), qe is the equilibrium adsorption capacity (mg·g−1), k1 is the pseudo-first-order rate constant (min−1), k2 (g·mg−1·min−1) is the pseudo-second-order rate constant, and t is the contact time (min).The plot of ln (qe − qt) versus t gives a straight line for the pseudo-first adsorption kinetics, which allows the determination of k1 from the slope and qe from the y-intercept. For the pseudo-second-order adsorption kinetics, qe and k2 can be determined from the intercept of the linearized plot of t/qt versus t.The Elovich equation can be expressed mathematically as follows:(6)qt=1βlnt+1βlnαβ,where α is the initial rate constant (mg·g−1·min−1) and β (mg·g−1) is the desorption constant at time t. The parameters α and β can be calculated from the slope (1/β) and intercept (1/β)ln(α β) of the linear plot of qt versus ln(t) with β = 1/slope and α = exp(intercept × β)/β.


## 2.6. Effects of Experimental Parameters on Cu(II) Removal

### 2.6.1. Effect of pH

The effect of pH on the adsorption process was examined maintaining the described batch adsorption experiments and varying the pH of the solution from 2 to 8. The initial Cu(II) concentration was 100 mg·L−1 and the mass of the adsorbent was 0.4 g. The mixture was shaken for 90 min at an agitation speed equal to 200 rpm and a temperature equal to 25°C.


### 2.6.2. Effect of Adsorbent Dose

The effect of adsorbent dose was determined by maintaining the described batch adsorption experiments and varying the amount of SSP from 0.05 to 1.2 mg. The initial Cu(II) concentration was 100 mg·L−1 and pH was 4.7. The mixture was shaken for 90 min at an agitation speed equal to 200 rpm and a temperature equal to 25°C.


### 2.6.3. Effect of Particle Size

The effect of particle size of SSP was examined through different particle sizes from 50 to 800μm. The initial Cu(II) concentration was 100 mg·L−1 and the mass of the adsorbent was 0.4 g. The mixture was shaken for 90 min at an agitation speed equal to 200 rpm, a temperature equal to 25°C, and a pH equal to 4.7.


### 2.6.4. Effect of Initial Metal Concentration

The effect of metal concentration on Cu(II) elimination rate was examined by varying the Cu(II) concentration from 50 to 500 mg·L−1. The adsorbent mass was 0.4 g and the particle size was 300 μm. The mixture was shaken for 90 min at an agitation speed equal 200 rpm, a temperature equal to 25°C, and a pH equal to 4.7.


## 2.6.1. Effect of pH

The effect of pH on the adsorption process was examined maintaining the described batch adsorption experiments and varying the pH of the solution from 2 to 8. The initial Cu(II) concentration was 100 mg·L−1 and the mass of the adsorbent was 0.4 g. The mixture was shaken for 90 min at an agitation speed equal to 200 rpm and a temperature equal to 25°C.


## 2.6.2. Effect of Adsorbent Dose

The effect of adsorbent dose was determined by maintaining the described batch adsorption experiments and varying the amount of SSP from 0.05 to 1.2 mg. The initial Cu(II) concentration was 100 mg·L−1 and pH was 4.7. The mixture was shaken for 90 min at an agitation speed equal to 200 rpm and a temperature equal to 25°C.


## 2.6.3. Effect of Particle Size

The effect of particle size of SSP was examined through different particle sizes from 50 to 800μm. The initial Cu(II) concentration was 100 mg·L−1 and the mass of the adsorbent was 0.4 g. The mixture was shaken for 90 min at an agitation speed equal to 200 rpm, a temperature equal to 25°C, and a pH equal to 4.7.


## 2.6.4. Effect of Initial Metal Concentration

The effect of metal concentration on Cu(II) elimination rate was examined by varying the Cu(II) concentration from 50 to 500 mg·L−1. The adsorbent mass was 0.4 g and the particle size was 300 μm. The mixture was shaken for 90 min at an agitation speed equal 200 rpm, a temperature equal to 25°C, and a pH equal to 4.7.


## 2.7. Equilibrium Isotherm

Langmuir [29] and Freundlich [30] models were used to investigate and describe adsorption removal processes. The models were used to describe the distribution of metal ions between liquid and solid phases. The nonlinear method was used to calculate the parameters of the isotherms using the original form of the equation [31]. The isotherms models were fitted through Levenberg-Marquardt algorithm using OriginPro software.


## 2.8. Thermodynamic Study

The thermodynamic parameters were investigated at 298, 313, 323, and 333 K. The standard free energy change (∆Gº), standard enthalpy change (∆Hº), and standard entropy change (∆Sº) were calculated according to the following equations [24]:(7)ΔG°=−RTlnKc,ΔG°=ΔH°−TΔS°,lnKc=−ΔH°R1T+ΔS°R,where R is the universal gas constant (8.3144 J·mol−1·K−1), T is the absolute temperature in Kelvin (K), and Kc is the equilibrium constant.According to previous works, the equilibrium constantKc must be dimensionless and could be derived from the Langmuir constant using the following equation [32–34]:(8)Kc=63.54×55.5×1000×KL,where 55.5 (mol·L−1) is the number of moles of pure water per litre, 63.54 (g·mol−1) is the molecular weight of Cu, 1000 (g·L−1) is the value of the water density, and KL is the Langmuir constant (L·mg−1).


## 2.9. Thermal Treatment of the Residual Product

The residual product obtained after the Cu(II) removal by SSP was used as a precursor to produce mixed oxide. A simple one-step thermal decomposition method was used. For this purpose, 20 g of the residual product was calcined at 700, 900, and 1000°C for 120 min under an air atmosphere. The thermal treatment was performed with a Nabertherm P330 muffle furnace.


## 3. Results and Discussion

### 3.1. SEM Analysis

The surface morphologies of SSP before and after the Cu(II) treatment are shown in Figure1. The SEM images in Figure 1(a) indicate that the surface of SSP consists of condensed agglomerates made up of small particles. Furthermore, the SSP exhibits heterogeneous surface morphology. These results are in accordance with those found in previous studies [24, 35, 36].Figure 1
Images of SSP visualized by SEM: (a) raw SSP; (b) Cu(II) loaded SSP. EDX spectral data: (c) raw SSP; (d) Cu(II) loaded SSP.
(a)(b)(c)(d)Clear differences in raw SSP and Cu(II) loaded SSP surface morphology can be observed from the SEM images. Indeed, the SEM images in Figure1(b) show the emergence of secondary solids on the surface in the form of thin platelets. These aggregates indicate that surface precipitation may occur during the reaction, leading to the presence of structures whose morphology was matching on the study observed from the synthesized posnjakite particles [37, 38]. These observations were further strengthened by the EDX results. As indicated in Figure 1(c), the elemental compositions of raw SSP are carbon (C), oxygen (O), and calcium (Ca). The existence of Cu on the Cu(II) loaded SSP surface is shown evidently in Figure 1(d). This result shows the accumulation of Cu on the surface of SPP.SBET of the SSP determined using the BET method was 0.72 m2·g−1. The SSP was classified as a nonporous material in accordance with IUPAC classification [39]. In this case, the adsorption ability of the SSP is presumably not impacted by SBET. Several researchers found that the CaCO3-rich adsorbent has a low SBET value. Lertwattanaruk et al. [40] reported that the surface area of a ground short-necked clam, green mussel, and cockle shell powder was determined as being 0.82, 0.61, and 0.82 m2·g−1, respectively. Van et al. [41] reported a specific surface area of 1.45 m2·g−1 for biogenic freshwater mussel shells. Also, Lim and Aris [42] found a specific surface area of 0.21 m2·g−1 for dead calcareous skeletons.


### 3.2. FTIR Analysis

The infrared spectra of raw SSP (Figure2(a)) indicated the presence of the characteristic functional groups of the carbonate ions (CO32-), identified by the absorption bonds of 1447.40 cm−1, 1082.62 cm−1, 854.19 cm−1, and 712.33 cm−1. The double peak at 699.60 cm−1 and 712.33 cm−1 and the peak at 1082.62 cm−1 are characteristic of the aragonite structure. A FTIR spectral detailed analysis of raw SSP was carried out in our previous study [23]. Those results are consistent with previous research [43, 44].Figure 2
Characterization of raw SSP and Cu(II) loaded SSP: (a) FTIR spectrum; (b) X-ray patterns.
(a)(b)The infrared spectra of SSP after reaction revealed a decrease in the relative intensities of most of the absorption bands of CaCO3, especially those located at 1447.40 cm−1, 854.19 cm−1, 712.33 cm−1, and 699.60 cm−1. In addition, new bands appeared at 1116.68 cm−1, 800.38 cm−1, 603.66 cm−1, 516.87 cm−1, and 435.87 cm−1. A shift of the absorption bands located at 1447.40 and 854.19 cm−1 was observed. Those modifications of the FTIR spectrum may be due to the presence of posnjakite as a new phase in accordance with the results obtained from XRD patterns. Alternatively, the shift of the absorption bands may be evidence of a binding between Cu and SSP. These results are consistent with previous studies [24, 37, 45].


### 3.3. XRD Analysis

The crystalline structure of the SSP can be observed by analyzing the results of XRD shown in Figure2(b). The main diffraction peaks are identified in the range of 2θ = 25°–55°. The most representative peaks with their miller indices are located at 26.23° [111], 27.22° [102], 33.14° [201], 36.17° [020], 37.90° [211], 45.88° [122], 48.42° [220], and 52.47° [311]. These peaks are assigned to the aragonite crystal form of calcium carbonate (CaCO3) as deduced by comparison with the data file COD reference code 96-901-5426. The characterizing of SSP powder was performed with the HighScore Plus software. There are three characteristic crystal phases of CaCO3, namely, aragonite, calcite, and vaterite [43]. CaCO3 that constitutes the snail shells can have two mineralogical forms, calcite and/or aragonite. The calcite crystallizes in the rhomboidal system and aragonite in the orthorhombic system [24].The XRD pattern of Cu(II) loaded SSP showed the emergence of a new phase assigned to the posnjakite [Cu4(SO4) (OH)6,H2O] as deduced from the comparison with the data file ICDD reference code 00-020-0364. The most representative peaks are located at 12.73°, 25.69°, 31.12°, 33.13°, 34.28°, 37.27°, 38.60°, 44.88°, 48.43°, 56.83°, and 60.12°. Posnjakite is a monoclinic hydrated copper hydroxyl sulfate belonging to the same group as wroewolfeite and langite [45–47]. CaCO3 dissolved in solution combines with copper ions to produce a precipitate as a new component. The formation of posnjakite is similar to the phenomenon reported by Zhang et al. [38] and Chen et al. [48].


### 3.4. Kinetic Studies

The effect of contact time was studied to determine the contact time required for SSP to reach the equilibrium with the Cu(II) (Figure3(a)). The Cu(II) adsorption capacity increased with the contact time until it reached a maximum value of 12.2 mg·g−1 at 90 min and remained constant over time. The removal rate was close to 99% reducing the concentration of residual copper in the solution to less than 0.5 mg·L−1 to reach a level lower than the permissible limit of Cu(II) in the drinking water [49].Figure 3
Kinetics of Cu(II) removal by SSP: (a) effect of time; (b) Elovich model; (c) pseudo-first-order model; (d) pseudo-second-order model (pH: 4.7; Cu(II) concentration: 100 mg·L−1; dose: 8 g·L−1; agitation speed: 200 rpm; particle size: 300 μm; temperature: 25°C).
(a)(b)(c)(d)A contact time of 90 min was long enough to nearly complete the reaction between Cu(II) and SPP. This contact time was assumed appropriate for subsequent experiments, in which case the equilibrium could be reached.The faster Cu (II) removal rate within the first 30 min could be attributed to the large number of active sites on the SSP which are accessible for adsorption. Subsequently, the slower elimination rate in the second step may be explained by the steric hindrance induced by the precipitation and diffusion of metals to the surface of the SSP, which reduces the amount of the available sorption sites.Due to the weak acidity of copper sulfate, the initial pH of the solution was 4.7. The introduction of SSP increased this pH to 8.7. The increase in solution pH was assigned to the consumption of weak acidity from copper sulfate by CaCO3, which is the SSP's main constituent.The kinetic parameters in equation (4) and (5) could be derived from the slopes and intercepts of the fitted curves shown in Figures 3(c) and 3(d). The rate constants, expected metal uptake, and correlation coefficients are given in Table 1. Regarding the pseudo-first-order model, the correlation coefficient obtained is low, R2 = 0.896, and the predicted metal uptake is much higher than the experimental one. For the pseudo-second-order model, the correlation coefficient obtained was R2 = 0.979 and the predicted metal uptake with this model was 14.075 mg·g−1, which is much nearer to the experimental value of 12.193 mg·g−1. The correlation coefficient obtained for Elovich model was R2 = 0.879. These findings indicate that the adsorption process of Cu(II) by SSP is based on the pseudo-second-order model. This model has been commonly used to describe chemisorption involving valence forces through the sharing or exchange of electrons as covalent forces and ion exchange between the adsorbent and adsorbent. These results are in accordance with previous findings [15, 19, 50].Table 1
Parameters and correlation coefficients obtained from the analysis of adsorption kinetics by pseudo-first-order model, pseudo-second-order model, and Elovich equation.
Kinetic modelParameterPseudo-first-orderk1 (min−1)qe,cal (mg·g−1)qe,exp (mg·g−1)R2Radj20.06615.06412.1930.8960.884Pseudo-second-orderk2 (g·mg−1·min−1)qe,cal (mg·g−1)qe,exp (mg·g−1)R2Radj20.00414.07512.1930.9790.977Elovichβ (mg·g−1)α (mg·g−1·min−1)R2Radj20.3171.6050.8790.868


### 3.5. Effects of Experimental Parameters

#### 3.5.1. Effect of pH of the Solution

The amount of removal of the metal ions as a function of pH is depicted in Figure4(a). It has been observed that, under highly acidic conditions with a pH value of 2, the amount of adsorbed metals was very low, while the adsorption capacity increased with increasing pH values until a pH value of 7 was reached. Afterward, the adsorption capacity remained constant in the pH range between 7 and 10, reaching almost 99%. These findings corroborate with previous research [21].Figure 4
Effect of different experimental parameters on Cu(II) adsorption by SSP: (a) pH; (b) initial Cu(II) concentration; (c) particle size; (d) adsorbent dose.
(a)(b)(c)(d)The lower removal efficiency at a low pH is apparently due to an increase of hydrogen ions’ concentration in the solution. This may be attributed to the competition between Cu(II) and hydrogen ions for the same active sites on the SSP surface. Furthermore, as the pH increases, the hydrogen ion concentration in the solution decreases and the amounts ofHCO3− and CO32− anions available for reaction increase, leading to enhanced Cu(II) adsorption by the SSP surface. For pH > 7, the copper removal was mainly dominated by precipitation of the hydroxide ions or metal oxides that occur at alkaline pH. These results are consistent with previous research [21, 51].An experiment was carried out in a 50 mL solution without Cu(II) having 0.4 g of SSP at 25°C for a contact time of 90 min. The introduction of SSP increased the pH of the solution from 4.7 to 8.75. This may be explained by the increase of the amount of OH− by the release of the ionic base such as CO32− and HCO3− (equations (9)–(11)).(9)CaCO3↔Ca2++CO32−(10)CO32−+H2O↔HCO3−+OH−(11)HCO3−+H2O↔H2CO3+OH−The hydrolysis reaction of SSP leads also to the production of the following chemical species: Ca2+, CaOH+, and CaHCO3+ (equations (12)–(14)) [41, 52, 53]:(12)HCO3−+H+↔H2O+CO2(13)Ca2++HCO3−↔CaHCO3+(14)Ca2++OH−↔CaOH+According to the results of our previous works, the pHpzc of SSP was found to be 7.97 [23]. Therefore, at solution pH lower than 7.97, the surface of SSP is predominated by positive charges and could interact with negative species, while at pH higher than 7.97, the surface of the SSP is predominated by negative charges and could interact with positive metal species.According to pHpzc and considering the hydrolysis reaction of calcite of SSP, it seems that cationic species such as Ca2+, CaHCO3+, and CaOH+ overcome for pH < 7.97 and hence offer a positive charge to the SSP surface. At pH > 7.97, the negative species such as CO32- and HCO3- prevail. The effect of pH can be explained by the ion-exchange adsorption mechanism that occurs on the SSP surface, in which carbonate groups play an important role. The increase of calcium concentrations in the solution after Cu(II) adsorption resulted from the dissolution of CaCO3.The substitution process of Cu2+ with Ca2+ defined as ion exchange may be responsible for copper uptake in the solution. The same result has been reported in other studies using different heavy metals [41, 42, 54, 55]. The binding due to cation exchange between Cu2+ and Ca2+ can be presented as follows:(15)CaCO3+Cu2+⟶CuCO3+Ca2+(16)CaCO3+Cu2++CO32−⟶Ca,CuCO3


#### 3.5.2. Effect of Particle Size

The particle size distribution of SSP obtained through the particle size analysis is presented in Table2. Approximately 44.5% of SSP particles presented size of 300 µm, which represents the largest proportion of the sample (89 g). The particle size distribution curve obtained through the sieve analysis is available in our previous studies [23].Table 2
Particle size distribution of SSP.
Size (µm)Mass (g)Percentage mass (%)>80042213008944.5200178.51002010<503115.5Moreover, the effect of particle size on the percent of Cu(II) removal is presented in Figure4(c). Experimental results showed that the effect of particle size on the removal percentage was insignificant. Nonetheless, the particle size of more than 300 μm was found to yield the highest removal percentage of Cu(II). Therefore, a particle size of 300 μm was selected for this experimental study to decrease the future cost of material preparation.


#### 3.5.3. Effect of SSP Dose

The Cu(II) removal efficiency was significantly influenced by the amount of SSP as evident from Figure4(d). The removal efficiency of Cu(II) was increased with increasing SSP concentration. The maximum removal of Cu(II) from the aqueous solutions occurred with 8 g·L−1 of SSP and remained almost unchanged thereafter. This observation was mainly due to the saturation of the active sites in SSP and the establishment of the adsorption equilibrium. Indeed, the increase in the mass of SSP could provide enough adsorption sites for the metal ions and also increase the contact between the Cu(II) and the adsorbent. Several researchers have reported similar results [24, 56].


#### 3.5.4. Effect of Initial Concentrations on Cu(II) Removal

Figure4(b) shows the effect of initial concentration on Cu(II) uptake by SSP. The material shows a high elimination rate close to 99% with an initial Cu(II) concentration of 100 mg·L−1. This percentage decreases as the Cu(II) concentration further increases. Meanwhile, at a used concentration of 2000 mg·L−1, the elimination rate was found to be nearly 69%. The removal efficiency declined clearly at higher concentrations. However, a good Cu(II) removal efficiency was observed when the metal ions concentrations were less than 500 mg·L−1. As the percentage adsorbed decreased with increasing initial concentration, the equilibrium adsorption capacity increased, indicating increasing occupation of available binding sites. These findings are in agreement with previous studies [21].


### 3.6. Equilibrium Isotherms

Both the Langmuir and Freundlich models were used to describe adsorption isotherms. The nonlinear expression of the Langmuir isotherm model is given as(17)qe=qmaxKLCe1+KLCe,where Ce is the equilibrium Cu(II) concentration (mg·L−1), qe is the amount of Cu(II) adsorbed at equilibrium (mg·g−1), qmax is the maximum saturated monolayer adsorption capacity (mg·g−1), and KL is the Langmuir constant (L·mg−1) related to the energy of adsorption which quantitatively reflects the affinity of binding sites. The Langmuir model can be expressed in terms of a constant known as separation factor or equilibrium parameter (RL) given by the following equation [57]:(18)RL=11+KLC0,where KL is the Langmuir equilibrium constant (L·mg−1) and C0 is the initial Cu(II) concentration (mg·L−1). It has been recognized that, for favorable isotherm shapes, RL must be between 0 and 1 [58].The nonlinear expression of the Freundlich isotherm model is given as [30](19)qe=KFCe1/n,where KF (mg·g−1) (L·mg−1)1/n and n (dimensionless) are Freundlich isotherm constants, Ce (mg·L−1) is the Cu(II) concentration at equilibrium, and qe (mg·g−1) is the amount of Cu(II) adsorbed at equilibrium.The representations of Langmuir and Freundlich isotherms of Cu(II) adsorption at 25°C are given in Figure5(a). Their parameters are listed in Table 3. The values of R2 and Radj2 were high for both models. The Langmuir isotherm assumes a completely homogeneous surface, while the Freundlich isotherm is suitable for highly heterogeneous surfaces. The RL results were found to be between 0 and 1. Therefore, the adsorption of the Cu(II) by SSP was favorable. The calculated qmax was found to be 905.08 mg·g−1, which is greater than that found for Anadara inaequivalvis mollusk shells, qmax = 384.6 mg·g−1 [24].Figure 5
Cu(II) adsorption by SSP: (a) isotherm fitting of Langmuir and Freundlich; (b) plot of lnKc versus 1/T.
(a)(b)Table 3
Isotherms parameters of Cu(II) adsorption by SSP.
ModelParameterValueLangmuirqmax (mg·g−1)905.08KL (L·mg−1)1.16E − 04Radj20.99RL0.994–0.812R20.99FreundlichKF (mg·g−1) (L·mg−1)1/n0.22Radj20.99n1.14R20.99


### 3.7. Thermodynamic Study

The values of ΔH° and ΔS° can be obtained through the Van’t Hoff plots in Figure 5(b). The thermodynamic parameters for adsorption of Cu(II) by SSP are listed in Table 4. The negative values of ΔG° indicated that the adsorption phenomenon occurred favorably and spontaneously. The negative values of ΔH° suggested the exothermic nature of the process. Thus, the total energy absorbed in bonds breaking is lower than the total energy released in bonds making, causing the release of extra energy in the form of heat during the adsorptive process [33, 59]. The positive values of ΔS° suggested a rise in the randomness and disorder at the solid/solution interface during the adsorption of Cu(II).Table 4
Thermodynamic parameters for the adsorption of Cu(II) by SSP.
T (K)ΔG0 (kJ·mol−1)ΔH0 (kJ·mol−1)ΔS0 (J·mol−1·K−1)298.15−14.91−10.3115.28313.15−15.05323.15−15.17333.15−15.48


### 3.8. Mechanism of Copper Removal by SSP

While hydroxide complexes are always present in water, individual anions or combinations of them can bind to Cu(II) to form complexes. Cu(II) will form complexes with common anions, including OH−, HCO3-, CO32-, and SO42-. The common precipitates are malachite [Cu2(CO3) (OH)2] [60, 61], langite [Cu4(SO4) (OH)6,2H2O] [47], and posnjakite [Cu4(SO4) (OH)6,H2O] [38, 45].Both XRD and microstructure results demonstrate the manifestation of a new phase of copper sulfate, probably posnjakite [Cu4(SO4) (OH)6,H2O]. The possible precipitation reaction produced by the SSP may be represented by the following formula [38]:(20)4Cu2++4SO42−+4CaCO3+5H2O⟶Cu4SO4OH6⋅H2O↓+3SO42−+4Ca2++2HCO3−+2CO2↑The removal of Cu(II) can be predicted as a mixture of two effects. Firstly, the rough surface of SSP gives solid contact, resulting in chemisorption of metal ions through ion-exchange mechanism at low concentrations ((15) and (16). Secondly, the presence of dissolved CaCO3 leads to the increase of pH, which causes metal precipitation (see formula (20)). Figure 6 gives a schematic description of the mechanism of Cu(II) fixation by SSP. Adsorption and precipitation involve characteristic reactions of Cu(II) with CaCO3 surfaces, with precipitation dominating at high concentrations of metal. Moreover, the final pH after Cu(II) removal stayed in the neutral range, allowing direct discharge of the water without further adjustment. Indeed, typically tolerable discharges into surface watercourses are limited to a pH range of 6 to 9. Water discharge outside these limits is harmful to the environment [62, 63].Figure 6
Schematic diagram of Cu(II) fixation by chemical precipitation and ion-exchange mechanism.


### 3.9. Use of the Residual SSP for the Production of Valuable Compounds

Calcination is a thermal decomposition process that requires substantial energy consumption. Nevertheless, it showed the extreme importance to deal with complex waste. Indeed, it allows in a one-step process the formation of a reusable component or a waste generally more stable than the original one.The residual product after the Cu(II) removal by SSP is mainly composed of CaCO3 and posnjakite. It can be used as a precursor to synthesize mixed oxide, which is composed of copper (II) oxide (CuO), calcium oxide (CaO), and calcium copper oxide (Ca2CuO3). Figure 7(a) illustrates the preparation process of the mixed solid oxides. As shown in Figure 7(c), CaCO3 was obtained as the main phase in the calcined residual SSP at a temperature of 700°C, while CuO and CaO were obtained as a minor phase.Figure 7
(a) Calcination of Cu(II) loaded SSP. (b) Thermogravimetric Analysis (TGA) and derivative thermogravimetry (DTG) profiles of SSP. (c) XRD patterns comparison for raw SSP, Cu(II) loaded SSP, and Cu(II) loaded SSP calcined at 700, 900, and 1000°C along with their data file reference (COD: Crystallography Open Database, ICDD: International Centre for Diffraction Data).
(a)(b)(c)The reaction pathway of the thermal decomposition of posnjakite to CuO included the thermal dehydration and desulfurization processes. It can be expressed by the following reaction [64]:(21)Cu4SO4OH6⋅H2O⟶700°C4CuO+4H2O+SO2+12O2By increasing temperature to 900°C, the diffraction peaks corresponding to Ca2CuO3 appear as reported elsewhere [65]. Residual SSP calcined at 900°C was a mixed solid oxide consisting of CaO as the main phase and Ca2CuO3 as the minor phase.The TGA measurements of SSP reveal that the major weight loss (40.18%) occurs in the temperature range of 668 to 870°C (Figure7(b)). It may be attributed to the endothermic decomposition of CaCO3 to calcium oxide (CaO) and carbon dioxide (CO2). It can be expressed by the following reaction:(22)CaCO3s↔CaOs+CO2gThe proposed method is chemical-free and efficient in terms of time. Moreover, it allows the valorization of the residual SSP. The mixed oxide obtained can be applied in different areas. Indeed, CuO nanoparticle is employed in a broad variety of practical applications such as catalysis for biodiesel production, gas sensors, thermoelectric materials, batteries, and ceramic pigments [66–68]. Furthermore, copper nanoparticles exhibit extraordinary performance as antibacterial and antimicrobial agents [69, 70]. CaO is extensively used in water and sewage treatment, in Portland cement production, in soil stabilization, and in biomedicine [71–73]. Mixed metal oxides have been widely used for various applications such as pigments in coatings and catalysts for transesterification of triglyceride [74, 75].The increasing costs and the environmental considerations associated with the use of commercial adsorbents have led to the development of alternative low-cost adsorbents derived from renewable resources. The use of natural materials for heavy metals removal is a new, economic, efficient, and eco-friendly alternative over conventional treatment methods. The SSP used in this research is an available and inexpensive material that can be used to support both the goals of water purification and resource recovery. Table5 presents the comparison of adsorption capacities of various adsorbents for Cu(II).Table 5
Comparison of Cu(II) adsorption studies using various adsorbents.
AdsorbentAdsorption capacity (mg·g−1)ReferenceSSP905.08This studyMollusk shells384.6[24]Raw corn silk15.35[76]Bentonite56.95[77]Apricot stones5.90[78]Maple sawdust9.19[79]Pine cones powder9.08[80]


## 3.1. SEM Analysis

The surface morphologies of SSP before and after the Cu(II) treatment are shown in Figure1. The SEM images in Figure 1(a) indicate that the surface of SSP consists of condensed agglomerates made up of small particles. Furthermore, the SSP exhibits heterogeneous surface morphology. These results are in accordance with those found in previous studies [24, 35, 36].Figure 1
Images of SSP visualized by SEM: (a) raw SSP; (b) Cu(II) loaded SSP. EDX spectral data: (c) raw SSP; (d) Cu(II) loaded SSP.
(a)(b)(c)(d)Clear differences in raw SSP and Cu(II) loaded SSP surface morphology can be observed from the SEM images. Indeed, the SEM images in Figure1(b) show the emergence of secondary solids on the surface in the form of thin platelets. These aggregates indicate that surface precipitation may occur during the reaction, leading to the presence of structures whose morphology was matching on the study observed from the synthesized posnjakite particles [37, 38]. These observations were further strengthened by the EDX results. As indicated in Figure 1(c), the elemental compositions of raw SSP are carbon (C), oxygen (O), and calcium (Ca). The existence of Cu on the Cu(II) loaded SSP surface is shown evidently in Figure 1(d). This result shows the accumulation of Cu on the surface of SPP.SBET of the SSP determined using the BET method was 0.72 m2·g−1. The SSP was classified as a nonporous material in accordance with IUPAC classification [39]. In this case, the adsorption ability of the SSP is presumably not impacted by SBET. Several researchers found that the CaCO3-rich adsorbent has a low SBET value. Lertwattanaruk et al. [40] reported that the surface area of a ground short-necked clam, green mussel, and cockle shell powder was determined as being 0.82, 0.61, and 0.82 m2·g−1, respectively. Van et al. [41] reported a specific surface area of 1.45 m2·g−1 for biogenic freshwater mussel shells. Also, Lim and Aris [42] found a specific surface area of 0.21 m2·g−1 for dead calcareous skeletons.


## 3.2. FTIR Analysis

The infrared spectra of raw SSP (Figure2(a)) indicated the presence of the characteristic functional groups of the carbonate ions (CO32-), identified by the absorption bonds of 1447.40 cm−1, 1082.62 cm−1, 854.19 cm−1, and 712.33 cm−1. The double peak at 699.60 cm−1 and 712.33 cm−1 and the peak at 1082.62 cm−1 are characteristic of the aragonite structure. A FTIR spectral detailed analysis of raw SSP was carried out in our previous study [23]. Those results are consistent with previous research [43, 44].Figure 2
Characterization of raw SSP and Cu(II) loaded SSP: (a) FTIR spectrum; (b) X-ray patterns.
(a)(b)The infrared spectra of SSP after reaction revealed a decrease in the relative intensities of most of the absorption bands of CaCO3, especially those located at 1447.40 cm−1, 854.19 cm−1, 712.33 cm−1, and 699.60 cm−1. In addition, new bands appeared at 1116.68 cm−1, 800.38 cm−1, 603.66 cm−1, 516.87 cm−1, and 435.87 cm−1. A shift of the absorption bands located at 1447.40 and 854.19 cm−1 was observed. Those modifications of the FTIR spectrum may be due to the presence of posnjakite as a new phase in accordance with the results obtained from XRD patterns. Alternatively, the shift of the absorption bands may be evidence of a binding between Cu and SSP. These results are consistent with previous studies [24, 37, 45].


## 3.3. XRD Analysis

The crystalline structure of the SSP can be observed by analyzing the results of XRD shown in Figure2(b). The main diffraction peaks are identified in the range of 2θ = 25°–55°. The most representative peaks with their miller indices are located at 26.23° [111], 27.22° [102], 33.14° [201], 36.17° [020], 37.90° [211], 45.88° [122], 48.42° [220], and 52.47° [311]. These peaks are assigned to the aragonite crystal form of calcium carbonate (CaCO3) as deduced by comparison with the data file COD reference code 96-901-5426. The characterizing of SSP powder was performed with the HighScore Plus software. There are three characteristic crystal phases of CaCO3, namely, aragonite, calcite, and vaterite [43]. CaCO3 that constitutes the snail shells can have two mineralogical forms, calcite and/or aragonite. The calcite crystallizes in the rhomboidal system and aragonite in the orthorhombic system [24].The XRD pattern of Cu(II) loaded SSP showed the emergence of a new phase assigned to the posnjakite [Cu4(SO4) (OH)6,H2O] as deduced from the comparison with the data file ICDD reference code 00-020-0364. The most representative peaks are located at 12.73°, 25.69°, 31.12°, 33.13°, 34.28°, 37.27°, 38.60°, 44.88°, 48.43°, 56.83°, and 60.12°. Posnjakite is a monoclinic hydrated copper hydroxyl sulfate belonging to the same group as wroewolfeite and langite [45–47]. CaCO3 dissolved in solution combines with copper ions to produce a precipitate as a new component. The formation of posnjakite is similar to the phenomenon reported by Zhang et al. [38] and Chen et al. [48].


## 3.4. Kinetic Studies

The effect of contact time was studied to determine the contact time required for SSP to reach the equilibrium with the Cu(II) (Figure3(a)). The Cu(II) adsorption capacity increased with the contact time until it reached a maximum value of 12.2 mg·g−1 at 90 min and remained constant over time. The removal rate was close to 99% reducing the concentration of residual copper in the solution to less than 0.5 mg·L−1 to reach a level lower than the permissible limit of Cu(II) in the drinking water [49].Figure 3
Kinetics of Cu(II) removal by SSP: (a) effect of time; (b) Elovich model; (c) pseudo-first-order model; (d) pseudo-second-order model (pH: 4.7; Cu(II) concentration: 100 mg·L−1; dose: 8 g·L−1; agitation speed: 200 rpm; particle size: 300 μm; temperature: 25°C).
(a)(b)(c)(d)A contact time of 90 min was long enough to nearly complete the reaction between Cu(II) and SPP. This contact time was assumed appropriate for subsequent experiments, in which case the equilibrium could be reached.The faster Cu (II) removal rate within the first 30 min could be attributed to the large number of active sites on the SSP which are accessible for adsorption. Subsequently, the slower elimination rate in the second step may be explained by the steric hindrance induced by the precipitation and diffusion of metals to the surface of the SSP, which reduces the amount of the available sorption sites.Due to the weak acidity of copper sulfate, the initial pH of the solution was 4.7. The introduction of SSP increased this pH to 8.7. The increase in solution pH was assigned to the consumption of weak acidity from copper sulfate by CaCO3, which is the SSP's main constituent.The kinetic parameters in equation (4) and (5) could be derived from the slopes and intercepts of the fitted curves shown in Figures 3(c) and 3(d). The rate constants, expected metal uptake, and correlation coefficients are given in Table 1. Regarding the pseudo-first-order model, the correlation coefficient obtained is low, R2 = 0.896, and the predicted metal uptake is much higher than the experimental one. For the pseudo-second-order model, the correlation coefficient obtained was R2 = 0.979 and the predicted metal uptake with this model was 14.075 mg·g−1, which is much nearer to the experimental value of 12.193 mg·g−1. The correlation coefficient obtained for Elovich model was R2 = 0.879. These findings indicate that the adsorption process of Cu(II) by SSP is based on the pseudo-second-order model. This model has been commonly used to describe chemisorption involving valence forces through the sharing or exchange of electrons as covalent forces and ion exchange between the adsorbent and adsorbent. These results are in accordance with previous findings [15, 19, 50].Table 1
Parameters and correlation coefficients obtained from the analysis of adsorption kinetics by pseudo-first-order model, pseudo-second-order model, and Elovich equation.
Kinetic modelParameterPseudo-first-orderk1 (min−1)qe,cal (mg·g−1)qe,exp (mg·g−1)R2Radj20.06615.06412.1930.8960.884Pseudo-second-orderk2 (g·mg−1·min−1)qe,cal (mg·g−1)qe,exp (mg·g−1)R2Radj20.00414.07512.1930.9790.977Elovichβ (mg·g−1)α (mg·g−1·min−1)R2Radj20.3171.6050.8790.868


## 3.5. Effects of Experimental Parameters

### 3.5.1. Effect of pH of the Solution

The amount of removal of the metal ions as a function of pH is depicted in Figure4(a). It has been observed that, under highly acidic conditions with a pH value of 2, the amount of adsorbed metals was very low, while the adsorption capacity increased with increasing pH values until a pH value of 7 was reached. Afterward, the adsorption capacity remained constant in the pH range between 7 and 10, reaching almost 99%. These findings corroborate with previous research [21].Figure 4
Effect of different experimental parameters on Cu(II) adsorption by SSP: (a) pH; (b) initial Cu(II) concentration; (c) particle size; (d) adsorbent dose.
(a)(b)(c)(d)The lower removal efficiency at a low pH is apparently due to an increase of hydrogen ions’ concentration in the solution. This may be attributed to the competition between Cu(II) and hydrogen ions for the same active sites on the SSP surface. Furthermore, as the pH increases, the hydrogen ion concentration in the solution decreases and the amounts ofHCO3− and CO32− anions available for reaction increase, leading to enhanced Cu(II) adsorption by the SSP surface. For pH > 7, the copper removal was mainly dominated by precipitation of the hydroxide ions or metal oxides that occur at alkaline pH. These results are consistent with previous research [21, 51].An experiment was carried out in a 50 mL solution without Cu(II) having 0.4 g of SSP at 25°C for a contact time of 90 min. The introduction of SSP increased the pH of the solution from 4.7 to 8.75. This may be explained by the increase of the amount of OH− by the release of the ionic base such as CO32− and HCO3− (equations (9)–(11)).(9)CaCO3↔Ca2++CO32−(10)CO32−+H2O↔HCO3−+OH−(11)HCO3−+H2O↔H2CO3+OH−The hydrolysis reaction of SSP leads also to the production of the following chemical species: Ca2+, CaOH+, and CaHCO3+ (equations (12)–(14)) [41, 52, 53]:(12)HCO3−+H+↔H2O+CO2(13)Ca2++HCO3−↔CaHCO3+(14)Ca2++OH−↔CaOH+According to the results of our previous works, the pHpzc of SSP was found to be 7.97 [23]. Therefore, at solution pH lower than 7.97, the surface of SSP is predominated by positive charges and could interact with negative species, while at pH higher than 7.97, the surface of the SSP is predominated by negative charges and could interact with positive metal species.According to pHpzc and considering the hydrolysis reaction of calcite of SSP, it seems that cationic species such as Ca2+, CaHCO3+, and CaOH+ overcome for pH < 7.97 and hence offer a positive charge to the SSP surface. At pH > 7.97, the negative species such as CO32- and HCO3- prevail. The effect of pH can be explained by the ion-exchange adsorption mechanism that occurs on the SSP surface, in which carbonate groups play an important role. The increase of calcium concentrations in the solution after Cu(II) adsorption resulted from the dissolution of CaCO3.The substitution process of Cu2+ with Ca2+ defined as ion exchange may be responsible for copper uptake in the solution. The same result has been reported in other studies using different heavy metals [41, 42, 54, 55]. The binding due to cation exchange between Cu2+ and Ca2+ can be presented as follows:(15)CaCO3+Cu2+⟶CuCO3+Ca2+(16)CaCO3+Cu2++CO32−⟶Ca,CuCO3


### 3.5.2. Effect of Particle Size

The particle size distribution of SSP obtained through the particle size analysis is presented in Table2. Approximately 44.5% of SSP particles presented size of 300 µm, which represents the largest proportion of the sample (89 g). The particle size distribution curve obtained through the sieve analysis is available in our previous studies [23].Table 2
Particle size distribution of SSP.
Size (µm)Mass (g)Percentage mass (%)>80042213008944.5200178.51002010<503115.5Moreover, the effect of particle size on the percent of Cu(II) removal is presented in Figure4(c). Experimental results showed that the effect of particle size on the removal percentage was insignificant. Nonetheless, the particle size of more than 300 μm was found to yield the highest removal percentage of Cu(II). Therefore, a particle size of 300 μm was selected for this experimental study to decrease the future cost of material preparation.


### 3.5.3. Effect of SSP Dose

The Cu(II) removal efficiency was significantly influenced by the amount of SSP as evident from Figure4(d). The removal efficiency of Cu(II) was increased with increasing SSP concentration. The maximum removal of Cu(II) from the aqueous solutions occurred with 8 g·L−1 of SSP and remained almost unchanged thereafter. This observation was mainly due to the saturation of the active sites in SSP and the establishment of the adsorption equilibrium. Indeed, the increase in the mass of SSP could provide enough adsorption sites for the metal ions and also increase the contact between the Cu(II) and the adsorbent. Several researchers have reported similar results [24, 56].


### 3.5.4. Effect of Initial Concentrations on Cu(II) Removal

Figure4(b) shows the effect of initial concentration on Cu(II) uptake by SSP. The material shows a high elimination rate close to 99% with an initial Cu(II) concentration of 100 mg·L−1. This percentage decreases as the Cu(II) concentration further increases. Meanwhile, at a used concentration of 2000 mg·L−1, the elimination rate was found to be nearly 69%. The removal efficiency declined clearly at higher concentrations. However, a good Cu(II) removal efficiency was observed when the metal ions concentrations were less than 500 mg·L−1. As the percentage adsorbed decreased with increasing initial concentration, the equilibrium adsorption capacity increased, indicating increasing occupation of available binding sites. These findings are in agreement with previous studies [21].


## 3.5.1. Effect of pH of the Solution

The amount of removal of the metal ions as a function of pH is depicted in Figure4(a). It has been observed that, under highly acidic conditions with a pH value of 2, the amount of adsorbed metals was very low, while the adsorption capacity increased with increasing pH values until a pH value of 7 was reached. Afterward, the adsorption capacity remained constant in the pH range between 7 and 10, reaching almost 99%. These findings corroborate with previous research [21].Figure 4
Effect of different experimental parameters on Cu(II) adsorption by SSP: (a) pH; (b) initial Cu(II) concentration; (c) particle size; (d) adsorbent dose.
(a)(b)(c)(d)The lower removal efficiency at a low pH is apparently due to an increase of hydrogen ions’ concentration in the solution. This may be attributed to the competition between Cu(II) and hydrogen ions for the same active sites on the SSP surface. Furthermore, as the pH increases, the hydrogen ion concentration in the solution decreases and the amounts ofHCO3− and CO32− anions available for reaction increase, leading to enhanced Cu(II) adsorption by the SSP surface. For pH > 7, the copper removal was mainly dominated by precipitation of the hydroxide ions or metal oxides that occur at alkaline pH. These results are consistent with previous research [21, 51].An experiment was carried out in a 50 mL solution without Cu(II) having 0.4 g of SSP at 25°C for a contact time of 90 min. The introduction of SSP increased the pH of the solution from 4.7 to 8.75. This may be explained by the increase of the amount of OH− by the release of the ionic base such as CO32− and HCO3− (equations (9)–(11)).(9)CaCO3↔Ca2++CO32−(10)CO32−+H2O↔HCO3−+OH−(11)HCO3−+H2O↔H2CO3+OH−The hydrolysis reaction of SSP leads also to the production of the following chemical species: Ca2+, CaOH+, and CaHCO3+ (equations (12)–(14)) [41, 52, 53]:(12)HCO3−+H+↔H2O+CO2(13)Ca2++HCO3−↔CaHCO3+(14)Ca2++OH−↔CaOH+According to the results of our previous works, the pHpzc of SSP was found to be 7.97 [23]. Therefore, at solution pH lower than 7.97, the surface of SSP is predominated by positive charges and could interact with negative species, while at pH higher than 7.97, the surface of the SSP is predominated by negative charges and could interact with positive metal species.According to pHpzc and considering the hydrolysis reaction of calcite of SSP, it seems that cationic species such as Ca2+, CaHCO3+, and CaOH+ overcome for pH < 7.97 and hence offer a positive charge to the SSP surface. At pH > 7.97, the negative species such as CO32- and HCO3- prevail. The effect of pH can be explained by the ion-exchange adsorption mechanism that occurs on the SSP surface, in which carbonate groups play an important role. The increase of calcium concentrations in the solution after Cu(II) adsorption resulted from the dissolution of CaCO3.The substitution process of Cu2+ with Ca2+ defined as ion exchange may be responsible for copper uptake in the solution. The same result has been reported in other studies using different heavy metals [41, 42, 54, 55]. The binding due to cation exchange between Cu2+ and Ca2+ can be presented as follows:(15)CaCO3+Cu2+⟶CuCO3+Ca2+(16)CaCO3+Cu2++CO32−⟶Ca,CuCO3


## 3.5.2. Effect of Particle Size

The particle size distribution of SSP obtained through the particle size analysis is presented in Table2. Approximately 44.5% of SSP particles presented size of 300 µm, which represents the largest proportion of the sample (89 g). The particle size distribution curve obtained through the sieve analysis is available in our previous studies [23].Table 2
Particle size distribution of SSP.
Size (µm)Mass (g)Percentage mass (%)>80042213008944.5200178.51002010<503115.5Moreover, the effect of particle size on the percent of Cu(II) removal is presented in Figure4(c). Experimental results showed that the effect of particle size on the removal percentage was insignificant. Nonetheless, the particle size of more than 300 μm was found to yield the highest removal percentage of Cu(II). Therefore, a particle size of 300 μm was selected for this experimental study to decrease the future cost of material preparation.


## 3.5.3. Effect of SSP Dose

The Cu(II) removal efficiency was significantly influenced by the amount of SSP as evident from Figure4(d). The removal efficiency of Cu(II) was increased with increasing SSP concentration. The maximum removal of Cu(II) from the aqueous solutions occurred with 8 g·L−1 of SSP and remained almost unchanged thereafter. This observation was mainly due to the saturation of the active sites in SSP and the establishment of the adsorption equilibrium. Indeed, the increase in the mass of SSP could provide enough adsorption sites for the metal ions and also increase the contact between the Cu(II) and the adsorbent. Several researchers have reported similar results [24, 56].


## 3.5.4. Effect of Initial Concentrations on Cu(II) Removal

Figure4(b) shows the effect of initial concentration on Cu(II) uptake by SSP. The material shows a high elimination rate close to 99% with an initial Cu(II) concentration of 100 mg·L−1. This percentage decreases as the Cu(II) concentration further increases. Meanwhile, at a used concentration of 2000 mg·L−1, the elimination rate was found to be nearly 69%. The removal efficiency declined clearly at higher concentrations. However, a good Cu(II) removal efficiency was observed when the metal ions concentrations were less than 500 mg·L−1. As the percentage adsorbed decreased with increasing initial concentration, the equilibrium adsorption capacity increased, indicating increasing occupation of available binding sites. These findings are in agreement with previous studies [21].


## 3.6. Equilibrium Isotherms

Both the Langmuir and Freundlich models were used to describe adsorption isotherms. The nonlinear expression of the Langmuir isotherm model is given as(17)qe=qmaxKLCe1+KLCe,where Ce is the equilibrium Cu(II) concentration (mg·L−1), qe is the amount of Cu(II) adsorbed at equilibrium (mg·g−1), qmax is the maximum saturated monolayer adsorption capacity (mg·g−1), and KL is the Langmuir constant (L·mg−1) related to the energy of adsorption which quantitatively reflects the affinity of binding sites. The Langmuir model can be expressed in terms of a constant known as separation factor or equilibrium parameter (RL) given by the following equation [57]:(18)RL=11+KLC0,where KL is the Langmuir equilibrium constant (L·mg−1) and C0 is the initial Cu(II) concentration (mg·L−1). It has been recognized that, for favorable isotherm shapes, RL must be between 0 and 1 [58].The nonlinear expression of the Freundlich isotherm model is given as [30](19)qe=KFCe1/n,where KF (mg·g−1) (L·mg−1)1/n and n (dimensionless) are Freundlich isotherm constants, Ce (mg·L−1) is the Cu(II) concentration at equilibrium, and qe (mg·g−1) is the amount of Cu(II) adsorbed at equilibrium.The representations of Langmuir and Freundlich isotherms of Cu(II) adsorption at 25°C are given in Figure5(a). Their parameters are listed in Table 3. The values of R2 and Radj2 were high for both models. The Langmuir isotherm assumes a completely homogeneous surface, while the Freundlich isotherm is suitable for highly heterogeneous surfaces. The RL results were found to be between 0 and 1. Therefore, the adsorption of the Cu(II) by SSP was favorable. The calculated qmax was found to be 905.08 mg·g−1, which is greater than that found for Anadara inaequivalvis mollusk shells, qmax = 384.6 mg·g−1 [24].Figure 5
Cu(II) adsorption by SSP: (a) isotherm fitting of Langmuir and Freundlich; (b) plot of lnKc versus 1/T.
(a)(b)Table 3
Isotherms parameters of Cu(II) adsorption by SSP.
ModelParameterValueLangmuirqmax (mg·g−1)905.08KL (L·mg−1)1.16E − 04Radj20.99RL0.994–0.812R20.99FreundlichKF (mg·g−1) (L·mg−1)1/n0.22Radj20.99n1.14R20.99


## 3.7. Thermodynamic Study

The values of ΔH° and ΔS° can be obtained through the Van’t Hoff plots in Figure 5(b). The thermodynamic parameters for adsorption of Cu(II) by SSP are listed in Table 4. The negative values of ΔG° indicated that the adsorption phenomenon occurred favorably and spontaneously. The negative values of ΔH° suggested the exothermic nature of the process. Thus, the total energy absorbed in bonds breaking is lower than the total energy released in bonds making, causing the release of extra energy in the form of heat during the adsorptive process [33, 59]. The positive values of ΔS° suggested a rise in the randomness and disorder at the solid/solution interface during the adsorption of Cu(II).Table 4
Thermodynamic parameters for the adsorption of Cu(II) by SSP.
T (K)ΔG0 (kJ·mol−1)ΔH0 (kJ·mol−1)ΔS0 (J·mol−1·K−1)298.15−14.91−10.3115.28313.15−15.05323.15−15.17333.15−15.48


## 3.8. Mechanism of Copper Removal by SSP

While hydroxide complexes are always present in water, individual anions or combinations of them can bind to Cu(II) to form complexes. Cu(II) will form complexes with common anions, including OH−, HCO3-, CO32-, and SO42-. The common precipitates are malachite [Cu2(CO3) (OH)2] [60, 61], langite [Cu4(SO4) (OH)6,2H2O] [47], and posnjakite [Cu4(SO4) (OH)6,H2O] [38, 45].Both XRD and microstructure results demonstrate the manifestation of a new phase of copper sulfate, probably posnjakite [Cu4(SO4) (OH)6,H2O]. The possible precipitation reaction produced by the SSP may be represented by the following formula [38]:(20)4Cu2++4SO42−+4CaCO3+5H2O⟶Cu4SO4OH6⋅H2O↓+3SO42−+4Ca2++2HCO3−+2CO2↑The removal of Cu(II) can be predicted as a mixture of two effects. Firstly, the rough surface of SSP gives solid contact, resulting in chemisorption of metal ions through ion-exchange mechanism at low concentrations ((15) and (16). Secondly, the presence of dissolved CaCO3 leads to the increase of pH, which causes metal precipitation (see formula (20)). Figure 6 gives a schematic description of the mechanism of Cu(II) fixation by SSP. Adsorption and precipitation involve characteristic reactions of Cu(II) with CaCO3 surfaces, with precipitation dominating at high concentrations of metal. Moreover, the final pH after Cu(II) removal stayed in the neutral range, allowing direct discharge of the water without further adjustment. Indeed, typically tolerable discharges into surface watercourses are limited to a pH range of 6 to 9. Water discharge outside these limits is harmful to the environment [62, 63].Figure 6
Schematic diagram of Cu(II) fixation by chemical precipitation and ion-exchange mechanism.


## 3.9. Use of the Residual SSP for the Production of Valuable Compounds

Calcination is a thermal decomposition process that requires substantial energy consumption. Nevertheless, it showed the extreme importance to deal with complex waste. Indeed, it allows in a one-step process the formation of a reusable component or a waste generally more stable than the original one.The residual product after the Cu(II) removal by SSP is mainly composed of CaCO3 and posnjakite. It can be used as a precursor to synthesize mixed oxide, which is composed of copper (II) oxide (CuO), calcium oxide (CaO), and calcium copper oxide (Ca2CuO3). Figure 7(a) illustrates the preparation process of the mixed solid oxides. As shown in Figure 7(c), CaCO3 was obtained as the main phase in the calcined residual SSP at a temperature of 700°C, while CuO and CaO were obtained as a minor phase.Figure 7
(a) Calcination of Cu(II) loaded SSP. (b) Thermogravimetric Analysis (TGA) and derivative thermogravimetry (DTG) profiles of SSP. (c) XRD patterns comparison for raw SSP, Cu(II) loaded SSP, and Cu(II) loaded SSP calcined at 700, 900, and 1000°C along with their data file reference (COD: Crystallography Open Database, ICDD: International Centre for Diffraction Data).
(a)(b)(c)The reaction pathway of the thermal decomposition of posnjakite to CuO included the thermal dehydration and desulfurization processes. It can be expressed by the following reaction [64]:(21)Cu4SO4OH6⋅H2O⟶700°C4CuO+4H2O+SO2+12O2By increasing temperature to 900°C, the diffraction peaks corresponding to Ca2CuO3 appear as reported elsewhere [65]. Residual SSP calcined at 900°C was a mixed solid oxide consisting of CaO as the main phase and Ca2CuO3 as the minor phase.The TGA measurements of SSP reveal that the major weight loss (40.18%) occurs in the temperature range of 668 to 870°C (Figure7(b)). It may be attributed to the endothermic decomposition of CaCO3 to calcium oxide (CaO) and carbon dioxide (CO2). It can be expressed by the following reaction:(22)CaCO3s↔CaOs+CO2gThe proposed method is chemical-free and efficient in terms of time. Moreover, it allows the valorization of the residual SSP. The mixed oxide obtained can be applied in different areas. Indeed, CuO nanoparticle is employed in a broad variety of practical applications such as catalysis for biodiesel production, gas sensors, thermoelectric materials, batteries, and ceramic pigments [66–68]. Furthermore, copper nanoparticles exhibit extraordinary performance as antibacterial and antimicrobial agents [69, 70]. CaO is extensively used in water and sewage treatment, in Portland cement production, in soil stabilization, and in biomedicine [71–73]. Mixed metal oxides have been widely used for various applications such as pigments in coatings and catalysts for transesterification of triglyceride [74, 75].The increasing costs and the environmental considerations associated with the use of commercial adsorbents have led to the development of alternative low-cost adsorbents derived from renewable resources. The use of natural materials for heavy metals removal is a new, economic, efficient, and eco-friendly alternative over conventional treatment methods. The SSP used in this research is an available and inexpensive material that can be used to support both the goals of water purification and resource recovery. Table5 presents the comparison of adsorption capacities of various adsorbents for Cu(II).Table 5
Comparison of Cu(II) adsorption studies using various adsorbents.
AdsorbentAdsorption capacity (mg·g−1)ReferenceSSP905.08This studyMollusk shells384.6[24]Raw corn silk15.35[76]Bentonite56.95[77]Apricot stones5.90[78]Maple sawdust9.19[79]Pine cones powder9.08[80]


## 4. Conclusion

The present research investigated the efficiency of SSP for Cu(II) removal from contaminated aqueous solutions and the production of valuable compounds from the residual product. The removal of Cu(II) was reasonably fast to be completed within a time frame of 90 min. The kinetics of adsorption following the pseudo-second-order model (R2 = 0.979) were better compared to the pseudo-first-order model (R2 = 0.896). The amount of Cu(II) adsorbed increases with increasing pH value until a pH of 7 was reached. The maximum Cu(II) removal occurred with a mass of SSP equal to 8 g·L−1 and a particle size of 300 μm. This particle size presents approximately 44.5% of SSP particles, which is the largest proportion of the sample as shown by particle size analysis. The adsorption process obeyed the Freundlich and the Langmuir adsorption isotherms. The thermodynamic analysis indicated that the Cu(II) adsorption by SSP was a spontaneous and exothermic process. The adsorption mechanism on the SSP surface is considered to be ion exchange and precipitation as posnjakite. SSP exhibits an excellent ability to remove Cu(II). The Cu(II) removal rate could reach almost 99% for a concentration of 100 mg·L−1. After Cu(II) removal, the final pH was in the neutral range, which allowed direct water discharge without further adjustment. Calcite form of CaCO3 was obtained as the main phase in the residual SSP at a temperature of 700°C, while CuO and CaO were obtained as a minor phase. CaO as the main phase and Ca2CuO3 as the minor phase were obtained in the residual SSP calcined at 900°C. The proposed method is efficient in terms of time and does not require chemical compounds or expensive raw materials. It is expected that this simple approach can be used as an inexpensive and convenient method for the removal of Cu(II) from aqueous solutions and the production of mixed oxide.



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*Source: 9537680-2021-09-23.xml*