# Eco-Friendly Adsorbent from Waste of Mint: Application for the Removal of Hexavalent Chromium

Authors: Fatima Khammour; Fatouma Mohamed Abdoul-Latif; Ayoub Ainane; Jalludin Mohamed; Tarik Ainane
Journal: Journal of Chemistry
 (2021)

---

## Abstract

A serious environmental disaster is looming on the horizon due to the indiscriminate release of heavy metals into the soil and wastewater from human industrial practices. In this study, waste mint (WM) was used to remove chromium(VI) from aqueous solution using batch experiments. The adsorbent material (WM) was characterized using scanning electron microscopy coupled with energy dispersive analysis of X-ray spectroscopy (SEM-EDS), Fourier transform infrared spectroscopy (FTIR), differential scanning calorimetry (DSC), and thermal gravimetric analysis (TGA). The adsorption parameters optimized were as follows: pH solution (2–11), initial concentration of Cr(VI) (10–50 mg/L), adsorbent dose (0.1–10 g/L), and temperature conditions (298 K, 308 K, and 318 K). The experimental data fitted well to the fractional power kinetic model (0.97≤R2≤ 0.99) and Langmuir isotherm (R2 = 0.984) with a maximum adsorption capacity Qmax = 172.41 mg/g. The thermodynamic parameters for Cr(VI) sorption were also calculated, confirming that the adsorption process was spontaneous and accompanied by an exothermic adsorption (−4.83 ≤ ΔG ≤ −3.22 kJ/mol and ΔH = −28.93 kJ/mol). The Cr(VI) removal percentage was within the range of 41–98%, and the highest removal was noted at pH = 2. The results of the present study suggest that WM is a potential low-cost adsorbent for the removal of chromium(VI) from aqueous solutions.


---

## Body

## 1. Introduction

The growing demand for adsorbents used in environmental protection processes has made their price more expensive, prompting further research for the manufacture of new, less expensive absorbent materials from plant waste. From its discovery, mint is used as a medicinal and aromatic plant. In Morocco, mint cultivation is practiced everywhere, on small plots almost at the level of all farms, so spearmint is available throughout the year, and the yield is 4 to 6 tonnes of dry matter per hectare and per cut [1]. Different household waste treatment channels aim to recover waste, including in agriculture and breeding and particularly in environmental applications, especially in wastewater treatment. The presence of heavy metals in the environment is a major concern due to their toxicity to many life forms on the planet. Unlike organic pollutants, which are mostly biologically degradable, heavy metals do not degrade into harmless end-products [2]. The metals of greatest concern are Cr, Mn, Fe, Zn, and Cd, which are widely distributed in the materials that make up the Earth's surface. Among these heavy metals, chromium is found in higher concentrations in wastes from electroplating, paints, dyes, leather tanning, paper mills, and many other industries [3, 4]. Chromium VI is classified as certain carcinogenic to humans but only during exposure by inhalation (Arab et al., 2014). In humans, the associated cancer is that of the lungs. Some data also assume an increase in nasal and sinus cancers, and chronic exposure to chromium VI via drinking water causes gastrointestinal (mouth ulcerations, diarrhea, abdominal pain, dyspepsia, and vomiting) and haematological (anemia and leukocytosis) effects and immature neutrophils [5]. For workers exposed to chromium via air, the main effects observed relate to the respiratory system (irritation of the nasal mucosa, asthma, cough, shortness of breath, and wheezing) and the development of allergies to chromium. These effects have been confirmed in animals [6]. This metal is extremely toxic; therefore, exposure to high concentration of chromium can cause an epigastric pain, nausea, vomiting, severe diarrhea, and hemorrhage [7]. The maximum level of chromium in drinking water must not exceed 0.05 mg/L [8]. To remove heavy metal ions dissolved in wastewater, several techniques such as solvent extraction, ion exchange, membrane process, electrodialysis, precipitation, phytoextraction, ultrafiltration, reverse osmosis, and adsorption have been tested [9]. With the exception of adsorption, those methods are not economically viable and have some disadvantages, such as incomplete removal of metals, high cost of reagents, and energy requirements, and also, it can product a toxic sludge or other wastes requiring further disposal or treatment [10]. Adsorption is generally the most preferred method for the removal of heavy metal ions due to its high efficiency, easy handling, availability of different adsorbents, and cost-effectiveness [11]. Many investigations have been carried out on the effective removal of heavy metals from solution using natural adsorbents derived from household wastes [12–16]. The purpose of this study is therefore to investigate the possible use of mint waste, a household waste, for the removal of chromium ions from aqueous solution.


## 2. Materials and Methods

### 2.1. Reagents

The entire reagents used in this work were of high grade. Stock solutions of the chromium metal ions were prepared by dissolving K2Cr2O7 in bidistilled water. All the aqueous solutions were prepared using bidistilled water which was chrome free.


### 2.2. Preparation of Adsorbent

The waste mint (Mentha spicata) was collected from the discharge of the cafeteria in Hassan II University (Casablanca, Morocco). The collected materials were washed several times with boiled water and finally with distilled water to remove any adhering dirt. The washed materials were then dried in the oven at 60°C for 72 h. The dried biomass was then ground and sieved to obtain the particle size in the range of 250–500 μm. No other chemical or physical treatments were applied to the support. Finally, the resulting product was stored in an air-tight container for further use.


### 2.3. Characterization of Adsorbent

Scanning electron microscope coupled to energy dispersive analysis of X-ray spectroscopy (SEM-EDS, JSM-5800; JEOL CO., Tokyo, Japan) was used in order to determine the surface morphology and the elementary compositions of the adsorbent (WM).Fourier transform infrared (FTIR) spectrum of the sample was recorded by the Fourier transform infrared spectrophotometer (FTIR, BRUKER VERTEX 70, Billerica, USA), ranged from 4000 to 400 cm−1 at a resolution of 4 cm−1, from which the functional groups of the adsorbent were determined.The thermal analysis: differential scanning calorimetry (DSC) and thermal gravimetric analysis (TGA) of the adsorbent, was done using thermal analyzer (Linseis Stapt-1600, Germany), and the temperature range was from 0 to 1000°C at a heating rate of 10°C/min.


### 2.4. Apparatus and Instruments for Adsorption

Every equipment used was soaked in concentrated HNO3 for 12 h and then washed initially with tap water and then with distilled water. Then, the equipment was dried in a hot air oven. A digital pH meter (W&W) was used for all pH measurements. A high-precision electrical balance was used for weighing. All absorbance measurements were carried out with a spectrophotometer (Shidmadzu Model UV-1601, Kyoto, Japan) equipped with 1 cm quartz cells.


### 2.5. Analysis of Chromium(VI) Ions

The residual concentration of Cr(VI) ions in the effluent has been determined using diphenyl carbazide as a complexing agent: one milliliter of diphenyl carbazide solution (0.2% (w/v)) prepared in 95% acetone and 1 mL of 1/5 H2SO4 solution was added to the sample (1 mL) containing less than 100 mg/L of Cr(VI). The absorbance of the purple-colored solution was read at 540 nm after 10 min [17].


### 2.6. Batch Sorption Experiments

Adsorption studies were carried out using the batch technique to obtain rate and equilibrium data. The effects of various parameters on the rate of adsorption process were studied by varying initial pH solution (2–11), initial chromium ion concentration (C0: 10–50 mg/L), adsorbent mass (W: 0.1–10 g/L), and temperature of adsorption (T: 298–318 K).The experiments were performed in a thermal shaker using 250 mL beakers containing 100 mL of different chromium(VI) concentrations. Continuous mixing was provided during the experimental period with a constant agitation speed for better mass transfer to obtain a high interfacial area of contact. The remaining concentration of chromium in each sample (after the adsorption test) was determined by using a spectrophotometer after filtering the adsorbent with Whatman filter paper to make it WM free. The pH of the solution was adjusted to the required value by adding either dilute H2SO4 or NaOH solutions. The Cr(VI) concentration retained in the adsorbent phase was calculated according to the following equation[18]:(1)q=C0−CeW,where C0 and Ce are the initial and equilibrium concentrations (mg/L) of Cr(VI) solution, respectively, and W is the weight of the adsorbent (g/L).The percentage removal of dye was calculated as follows:(2)removal percentage=C0−CeC0×100.To increase the accuracy of the data, each experiment was repeated 3 times, and the average value was reported.


### 2.7. Kinetic, Isotherm, and Thermodynamic Studies and Modeling

Fractional power, pseudo-first order, pseudo-second order, Elovich, and intraparticle diffusion rate equations have been used in order to model the kinetics of chromium(VI) adsorption [19, 20].To investigate the interaction between the amount absorbed and the chromium concentration at equilibrium, we used the theoretical models described in [21, 22].Thermodynamic parameters, including the Gibbs-free energy (∆G°), enthalpy (∆H°), and entropy (∆S°), are the actual indicators for practical application of an adsorption process. According to the values of these parameters, the processes that occur spontaneously can be determined. The thermodynamic parameters were determined using the following equations [23]:(3)ΔG°=ΔH°−TΔS°,(4)K=QeCe,(5)LnK=ΔS°R−ΔH°R.T,where K, Qe, Ce, R, and T are the equilibrium constant, the amount of the metal adsorbed at equilibrium (mol/L), the equilibrium concentration of metal (mol/L), the gas constant (8.314 J/mol.K), and the absolute temperature (Kelvin), respectively. By plotting a graph of ln K versus 1/T, the values ∆H° and ∆S° can be estimated from the slopes and intercepts.Figure 1
Preprocessing of adsorbent and adsorption process.


### 2.8. Preprocessing of Adsorbent and Adsorption Process

The experimental procedures are shown in Figure1.


## 2.1. Reagents

The entire reagents used in this work were of high grade. Stock solutions of the chromium metal ions were prepared by dissolving K2Cr2O7 in bidistilled water. All the aqueous solutions were prepared using bidistilled water which was chrome free.


## 2.2. Preparation of Adsorbent

The waste mint (Mentha spicata) was collected from the discharge of the cafeteria in Hassan II University (Casablanca, Morocco). The collected materials were washed several times with boiled water and finally with distilled water to remove any adhering dirt. The washed materials were then dried in the oven at 60°C for 72 h. The dried biomass was then ground and sieved to obtain the particle size in the range of 250–500 μm. No other chemical or physical treatments were applied to the support. Finally, the resulting product was stored in an air-tight container for further use.


## 2.3. Characterization of Adsorbent

Scanning electron microscope coupled to energy dispersive analysis of X-ray spectroscopy (SEM-EDS, JSM-5800; JEOL CO., Tokyo, Japan) was used in order to determine the surface morphology and the elementary compositions of the adsorbent (WM).Fourier transform infrared (FTIR) spectrum of the sample was recorded by the Fourier transform infrared spectrophotometer (FTIR, BRUKER VERTEX 70, Billerica, USA), ranged from 4000 to 400 cm−1 at a resolution of 4 cm−1, from which the functional groups of the adsorbent were determined.The thermal analysis: differential scanning calorimetry (DSC) and thermal gravimetric analysis (TGA) of the adsorbent, was done using thermal analyzer (Linseis Stapt-1600, Germany), and the temperature range was from 0 to 1000°C at a heating rate of 10°C/min.


## 2.4. Apparatus and Instruments for Adsorption

Every equipment used was soaked in concentrated HNO3 for 12 h and then washed initially with tap water and then with distilled water. Then, the equipment was dried in a hot air oven. A digital pH meter (W&W) was used for all pH measurements. A high-precision electrical balance was used for weighing. All absorbance measurements were carried out with a spectrophotometer (Shidmadzu Model UV-1601, Kyoto, Japan) equipped with 1 cm quartz cells.


## 2.5. Analysis of Chromium(VI) Ions

The residual concentration of Cr(VI) ions in the effluent has been determined using diphenyl carbazide as a complexing agent: one milliliter of diphenyl carbazide solution (0.2% (w/v)) prepared in 95% acetone and 1 mL of 1/5 H2SO4 solution was added to the sample (1 mL) containing less than 100 mg/L of Cr(VI). The absorbance of the purple-colored solution was read at 540 nm after 10 min [17].


## 2.6. Batch Sorption Experiments

Adsorption studies were carried out using the batch technique to obtain rate and equilibrium data. The effects of various parameters on the rate of adsorption process were studied by varying initial pH solution (2–11), initial chromium ion concentration (C0: 10–50 mg/L), adsorbent mass (W: 0.1–10 g/L), and temperature of adsorption (T: 298–318 K).The experiments were performed in a thermal shaker using 250 mL beakers containing 100 mL of different chromium(VI) concentrations. Continuous mixing was provided during the experimental period with a constant agitation speed for better mass transfer to obtain a high interfacial area of contact. The remaining concentration of chromium in each sample (after the adsorption test) was determined by using a spectrophotometer after filtering the adsorbent with Whatman filter paper to make it WM free. The pH of the solution was adjusted to the required value by adding either dilute H2SO4 or NaOH solutions. The Cr(VI) concentration retained in the adsorbent phase was calculated according to the following equation[18]:(1)q=C0−CeW,where C0 and Ce are the initial and equilibrium concentrations (mg/L) of Cr(VI) solution, respectively, and W is the weight of the adsorbent (g/L).The percentage removal of dye was calculated as follows:(2)removal percentage=C0−CeC0×100.To increase the accuracy of the data, each experiment was repeated 3 times, and the average value was reported.


## 2.7. Kinetic, Isotherm, and Thermodynamic Studies and Modeling

Fractional power, pseudo-first order, pseudo-second order, Elovich, and intraparticle diffusion rate equations have been used in order to model the kinetics of chromium(VI) adsorption [19, 20].To investigate the interaction between the amount absorbed and the chromium concentration at equilibrium, we used the theoretical models described in [21, 22].Thermodynamic parameters, including the Gibbs-free energy (∆G°), enthalpy (∆H°), and entropy (∆S°), are the actual indicators for practical application of an adsorption process. According to the values of these parameters, the processes that occur spontaneously can be determined. The thermodynamic parameters were determined using the following equations [23]:(3)ΔG°=ΔH°−TΔS°,(4)K=QeCe,(5)LnK=ΔS°R−ΔH°R.T,where K, Qe, Ce, R, and T are the equilibrium constant, the amount of the metal adsorbed at equilibrium (mol/L), the equilibrium concentration of metal (mol/L), the gas constant (8.314 J/mol.K), and the absolute temperature (Kelvin), respectively. By plotting a graph of ln K versus 1/T, the values ∆H° and ∆S° can be estimated from the slopes and intercepts.Figure 1
Preprocessing of adsorbent and adsorption process.


## 2.8. Preprocessing of Adsorbent and Adsorption Process

The experimental procedures are shown in Figure1.


## 3. Results and Discussion

### 3.1. Characterization of the Adsorbent

#### 3.1.1. SEM-EDS Studies

The scanning electron microscope (SEM) images shown in Figure2 revealed the morphological nature of the piece of waste mint (0.5 cm × 0.5 cm) at the resolution of 50 μm (Figure 2(a)) and 10 μm (Figure 2(b)).Figure 2
SEM images of the WM adsorbent: (a) 50μm; (b) 10 μm.The results obtained show, on the one hand, an irregular and porous structure and, on the other hand, a heterogeneity of the pores shapes over the whole surface of the WM. This result encourages the evaluation of this waste as an adsorbent in the treatment of chromium-polluted water. Furthermore, the microanalysis by energy dispersive analysis of X-ray spectroscopy (EDX) of this surface gives a chemical composition as functions of mass percentages as it listed in Table1.Table 1
Percent for major atomic composition determined by EDX.
CompositionCONOther elementsPercentage content (%)66.3321.844.636.2The results show a high percentage of carbon (C) and oxygen (O), which is consistent with the organic nature of the support.


#### 3.1.2. FTIR Spectroscopy

Figure3 illustrates the FTIR spectrum of MM. The broad band in the region around 3425 cm−1 is attributed to the surface hydroxyl groups of the bonded carboxylic acid. The O-H stretching vibrations occurred within a broad range of frequencies indicating the presence of free hydroxyl groups and bonded O-H bands of carboxylic acid. The asymmetric C-H stretching of the methyl surface groups usually present on the lignin structure is observed at 2920 cm−1. The characteristic peaks of C-O group in the carboxylic and alcoholic groups were found at 1050 and 1033 cm−1. The ionisation of the carboxylic acid and hydroxyl functional groups present in the structure of the adsorbent can be obtained by deprotonation, which allows it to interact easily with metals, and can therefore constitute the main adsorption sites for the removal of Cr(VI) ions from solutions. The -OH, -NH, carbonyl, and carboxylic groups have been reported as very important sorption sites for metal ions [24, 25].Figure 3
FTIR spectra of WM.


#### 3.1.3. TGA and DSC Studies

The DSC and TGA result curves are shown in Figures4 and 5. The thermal changes in the WM can be observed during heating. The DSC curve shows a peak of endothermic transformation at 136.17°C, which explains the evaporation of water molecules and also the fusion of the organic molecules that have remained in the waste mint. These results, after the thermal transformation, were confirmed by the TGA curve which gives a water loss of the WM of 7.8% (86.4% decomposable before 200°C), in addition to the 5.9% related to the residues of the WM left during heating to 1000°C. Based on these results, we can suggest that the WM material can be used for adsorption experiments at temperatures below 100°C, as no thermal changes will be detected in this range.Figure 4
TGA for WM.Figure 5
DSC for WM.


### 3.2. Effect of Various Adsorption Parameters

#### 3.2.1. Effect of Solution pH

The pH effect on the adsorption process was investigated by undertaking the batch adsorption technique at different hydrogen ion concentrations while maintaining the other parameters constant atT = 298 K, t = 120 min, m = 2 g/L, and Ci = 50 mg/L Cr(VI). The pH of the adsorption medium was varied between 2 and 11, and the adsorbent (WM) gave the highest performance of 76% at the pH = 2 (Figure 6). The maximum performance was obtained at pH = 2, and hence, all the other experiments were carried at this pH value. In aqueous solutions, Cr(VI) exists in several stable forms such as CrO42−, HCrO4−, and Cr2O72− [26]. In the range of maximum adsorption pH, the dominant species was reported to be HCrO4−. The chemical nature of the functional groups in waste mint (WM) can be modified by changes in the pH of the adsorption medium and subsequently increasing the sorption capacity of the metals in the adsorbents [27].Figure 6
Effect of pH on the adsorption of Cr(VI) ions from aqueous solution using WM adsorbent atT = 298 K, time = 120 min, adsorbent dose W = 2 g/L, and [Cr(VI)] = 50 mg/L.There was reported competition for the same sorption sites with metal ions by hydrogen ions at low pH values, and it is therefore suggested that the sites of adsorption on the surface of the WM are taken up by hydrogen ions (H+), making the surface positively charged. Then, the negatively charged ions HCrO4− will approach and spontaneously access the binding sites on the adsorbent in order to pick up the more important metal ions due to the electrical attraction with the positive sites generated by the H+ [28].


#### 3.2.2. Effect of Cr(VI) Initial Concentration

The performance effectiveness of WM has been studied at different initial concentrations of hexavalent chromium of 10, 20, 30, 40, and 50 mg/L (Figure7), while keeping other parameters constant. The adsorption efficiency decreases with increasing concentration of Cr(VI) ions, and it is noted that the removal percentage has a maximum value of 90% for the initial chromium concentration of 10 mg/L. The explanation of this phenomenon is that when the concentration of Cr(VI) is high enough, the surface of the adsorbent is occupied and the efficiency starts to decrease, and therefore, the molecules desorb from the adsorbent surface.Figure 7
Effect of Cr(VI) concentration on the adsorption rate from aqueous solution using WM adsorbent atT = 298 (K), pH = 2, time = 120 min, and adsorbent dose W = 2 g/L.


#### 3.2.3. Effect of Adsorbent Dosage

Figure8 shows that the percentage removal of hexavalent chromium from the MW increased from 11% to 98% as the adsorbent dosage increased from 0.1 to 10 g/L. This is attributed to the increase in adsorption area and the availability of more adsorption sites.Figure 8
Effect of adsorbent dose on Cr(VI) ions removal from aqueous solution using WM adsorbent atT = 298 (K), pH = 2, time = 120 min, and [Cr(VI)] = 50 mg/L.


#### 3.2.4. Effect of Temperature

The temperature effect on the removal of Cr(VI) ions by MW was studied at three temperatures: 298 K, 308 K, and 318 K, as shown in Figure9. The maximum adsorption capacity was obtained at 298 K for a pH of 2 (74.9%). The adsorption capacity decreased with increasing temperature, suggesting that the adsorption process was exothermic.Figure 9
Effect of temperature on the adsorption of Cr(VI) from aqueous solution using WM adsorbent at pH = 2, time = 120 min, adsorbent doseW = 2 g/L, and [Cr(VI)] = 50 mg/L.


### 3.3. Adsorption Kinetics

In order to define the adsorption kinetics of Cr(VI) by the WM adsorbent, the kinetic parameters of the adsorption process were studied for contact times varying from 0 to 120 min by controlling the concentration of Cr(VI) held in the filtrate. Figure10 shows the adsorption kinetics curves for different initial concentrations of Cr(VI): 10, 20, 30, 40, and 50 mg/L.Figure 10
Kinetics adsorption of Cr(VI) from aqueous solution using WM adsorbent at pH = 2, time = 120 min, and adsorbent doseW = 2 g/L.All kinetic parameters of Cr(VI) adsorption by WM are determined from the linear form of the model equations described in [19, 20].The linear representations are shown in Figures11–14, respectively.Figure 11
Linearity of the pseudo-first-order model.Figure 12
Linearity of the pseudo-second-order model.Figure 13
Linearity of Elovich model.Figure 14
Linearity of intraparticle diffusion model.To find the best fit kinetic model, the correlation coefficients (R2) of the different models were compared and are grouped in Table 2. However, R2 correlation coefficients showed that the fractional power model fits better to the experimental data (0.97 ≤ R2 ≤ 0.99) than the other models (R2 is in the range of 0.24–0.99).Table 2
Adsorption kinetic model parameters at pH 2 for Cr(VI) removal.
ModelParametersC0 = 10 mg/LC0 = 20 mg/LC0 = 30 mg/LC0 = 40 mg/LC0 = 50 mg/LFractional powerLinear expressiony = 0.217x + 0.560y = 0.264x + 0.984y = 0.289x + 1.233y = 0.280x + 1.509y = 0.276x + 1.592R20.970.980.970.990.97kp1.7502.6753.4314.5224.913Υ0.2170.2640.2890.2800.276Pseudo-first-orderLinear expressiony = −0.035x + 1.398y = −0.030x + 1.994y = −0.025x + 2.335y = −0.023x + 2.634y = −0.025x + 2.739R20.930.970.920.950.93k1P (min−1)0.0250.0230.0250.0300.035qe.1P (mg.g−1)15.47113.92910.3297.3444.047Pseudo-second-orderLinear expressiony = 1.940x + 0.195y = 1.321x + 0.099y = 1.025x + 0.068y = 0.745x + 0.055y = 0.672x + 0.052R20.950.980.960.940.91k2P (g.mg−1.min−1)0.1000.0740.0660.0730.077qe.2P (mg.g−1)5.12810.10114.70518.18119.230ElovichLinear expressiony = 0.866x + 0.772y = 1.908x + 0,228y = 2.942x – 0.603y = 3.715x – 0.66y = 3.947x – 0.603R20.960.990.970.970.95αE (mg.g−1.min−1)2.1112.1502.3963.1103.387βE (g.mg−1)1.1540.5240.3390.2690.253Intraparticle diffusionLinear expressiony = 0.253x + 2.248y = 0.552x + 3.521y = 0.853x + 4.458y = 1.101x + 5.558y = 1.176x + 5.948R20.960.960.950.990.98kD (mg.g−1.min−1/2)0.2530.5520.8531.1011.176CD (mg.g−1)2.2483.5214.4585.5585.948


### 3.4. Adsorption Isotherms Studies

The isotherms study of Cr(VI) adsorption by the MW was carried out for 2 hours, with an initial Cr(VI) C0 concentration of 50 mg/L and a pH = 2, for different masses of the MW (W = 0.1, 0.5, 1, and 2 g/L). The variation of the adsorption capacity Qe is related with the equilibrium concentration Ce. Several models were applied to describe the experimental data for the adsorption isotherms. The Freundlich and Langmuir models are the most frequently used. In the present work, four models were used and described in [21, 22]. All parameters of the isotherms were determined from the linear relation (Figures 15–18) according to the equations of the models described in [21, 22].Figure 15
Linearity of Freundlich model.Figure 16
Linearity of Langmuir model.Figure 17
Linearity ofD-R model.Figure 18
Linearity of Temkin model.The best-fit isotherms models were determined by calculating the determination coefficients (R2). Parameter values at pH = 2 for the maximum Cr (VI) adsorption by MW are reported in Table 3. From the values of the correlation coefficients, it can be concluded that the Langmuir model was best fitted to the experimental results of Cr(VI) adsorption by WM.Table 3
Adsorption isotherms models parameter at pH 2 for Cr(VI) adsorption by WM.
ModelModel parametersValues of parametersFreundlichLinear expressiony = 0.824+0.856R20.97KF (L/g)2.354nF0.824LangmuirLinear expressiony = 0.593x+0.005R20.98KL (L/g)0.009qm.L (mg/g)172.410RL0.999D-RLinear expressiony = −175.960x + 3.915R20.87E (J/mol)186.770qm,DR (mg/g)50.180TemkinLinear expressiony = 27.690x-53.113R20.92KT (L/g)0.146BT (J/mol)27.690The essential characteristic parameter of the Langmuir isotherm can be expressed in terms of a dimensionless constant separation factor or also known as the equilibrium parameterRL [29]:(6)RL=11+KL⋅C0,where KL (L/mg) is the Langmuir constant and C0 (mg/L) is the initial concentration. RL = 1 represents linear adsorption, while RL = 0 stands for the irreversible adsorption process. RL < 1 is for favorable adsorption, while RL > 1 represents unfavorable adsorption. In this work, the value of RL was found to be 0.999, suggesting that the equilibrium parameter was less than 1 but near to 1, which means a favorable linear adsorption. This means that the equilibrium isotherms can be well described by the Langmuir model (Figure 19), and the adsorption process takes place as a monolayer (ML) on a surface with a finite number of identical sites, which are distributed homogeneously over the surface of the adsorbent [30].Figure 19
Modeling of the isotherm adsorption by Langmuir model.


### 3.5. Thermodynamics Studies

The thermodynamic parameters of an adsorption process are necessary to decide whether the process is spontaneous or not. Experimental data obtained at different temperatures were used to calculate thermodynamic parameters such as Gibbs-free energy change (ΔG°), enthalpy change (ΔH°), and entropy change (ΔS°). The Gibbs-free energy changes in the sorption reaction are given by equations (3)–(5), where K = KL is the equilibrium constant, which can be obtained from the Langmuir isotherm at different temperatures. ΔH° and ΔS° were obtained from the slope and intercept of the plot of ln KL vs. 1/T (Figure 20). The calculated results are reported in Table 4.Figure 20
FTIR spectra of WM before and after adsorption.Table 4
Thermodynamic parameters of adsorption of Cr(VI) on the WM.
ΔH° (KJ/mol)ΔS° (KJ/K.mol)ΔG° (KJ/mol)298 K308 K318 K-28.93−0.081−4.83−4.02−3.22The negative values of ΔG° confirm the feasibility of the process and the spontaneous nature of adsorption. The standard enthalpy and entropy changes in adsorption determined from Figure 20 were −28.93 kJ/mol and −0.081 kJ/k.mol, respectively, with a correlation coefficient of 0.96. The value of ΔH° is negative, indicating that the adsorption reaction is exothermic. The negative value of ΔS° reflects a decrease in the randomness at the solid/solution interface during the adsorption process [31].


### 3.6. Mechanism of Adsorption by FTIR

The FTIR spectra before and after the adsorption of Cr(VI) by WM are shown in Figure19. For the spectrum obtained after the adsorption of hexavalent chromium, there is a remarkable change in the intensities of the infrared bands without any change in position. The characterization by infrared spectroscopy also made it possible to confirm the results obtained by other methods of investigation. The structural properties of the adsorbent determine the effect of the degree of impregnation on the pore type distribution and the pore structure of the adsorbent. It has been determined that vigorous stimulation promotes pore formation at this level [32].


### 3.7. Comparison of Cr(VI) Adsorption Capacity of Different Adsorbents

The adsorption capacity of the different Cr(VI) adsorbents previously studied in the bibliography was compared with the current results, as shown in Table5. It can be observed that the maximum adsorption capacity (Qmax), at pH = 2, is higher (172 mg/g for the WM) than the most recently reported adsorbents. This result indicates that the waste mint applied in this study is a better alternative to other low-cost adsorbents. However, higher adsorption capacities of 250 and 278 mg/g were reported for modified rice husk and mosambi (Citrus limetta) peel at the same pH, respectively.Table 5
Comparison of adsorption capacities of WM with other adsorbents for Cr(VI).
No.AdsorbentQmax (mg/g)pHRef.1Modified rice husk2782[33]2Mosambi (Citrus limetta) peel2502[34]3Modified groundnut shell1312[35]4Chrysophyllum albidum (Sapotaceae) seed shells84.313[36]5Treated waste newspaper59.883[37].6Guar gum–nano-zinc oxide55.567[38]7Rice husk carbon47.612[39]8Eucalyptus bark452[40]9Wool41.152[41]10Olive cake33.442[42]11Chitosan-coated fly ash33.275[43]12Modified seaweed (Bifurcaria bifurcata)29.295.8[18]13Plantain waste16.1[44]14Saw dust15.822[45]15Almond10.612[46]16Banana (Musa Lacatan) waste102[47]17Tea (Camellia sinensis) waste7.292[42]18Pine needles7.082[48]19Peels of pea (Pisum sativum) pod4.332[49]20Waste of mint (Mentha spicata)1722This work


## 3.1. Characterization of the Adsorbent

### 3.1.1. SEM-EDS Studies

The scanning electron microscope (SEM) images shown in Figure2 revealed the morphological nature of the piece of waste mint (0.5 cm × 0.5 cm) at the resolution of 50 μm (Figure 2(a)) and 10 μm (Figure 2(b)).Figure 2
SEM images of the WM adsorbent: (a) 50μm; (b) 10 μm.The results obtained show, on the one hand, an irregular and porous structure and, on the other hand, a heterogeneity of the pores shapes over the whole surface of the WM. This result encourages the evaluation of this waste as an adsorbent in the treatment of chromium-polluted water. Furthermore, the microanalysis by energy dispersive analysis of X-ray spectroscopy (EDX) of this surface gives a chemical composition as functions of mass percentages as it listed in Table1.Table 1
Percent for major atomic composition determined by EDX.
CompositionCONOther elementsPercentage content (%)66.3321.844.636.2The results show a high percentage of carbon (C) and oxygen (O), which is consistent with the organic nature of the support.


### 3.1.2. FTIR Spectroscopy

Figure3 illustrates the FTIR spectrum of MM. The broad band in the region around 3425 cm−1 is attributed to the surface hydroxyl groups of the bonded carboxylic acid. The O-H stretching vibrations occurred within a broad range of frequencies indicating the presence of free hydroxyl groups and bonded O-H bands of carboxylic acid. The asymmetric C-H stretching of the methyl surface groups usually present on the lignin structure is observed at 2920 cm−1. The characteristic peaks of C-O group in the carboxylic and alcoholic groups were found at 1050 and 1033 cm−1. The ionisation of the carboxylic acid and hydroxyl functional groups present in the structure of the adsorbent can be obtained by deprotonation, which allows it to interact easily with metals, and can therefore constitute the main adsorption sites for the removal of Cr(VI) ions from solutions. The -OH, -NH, carbonyl, and carboxylic groups have been reported as very important sorption sites for metal ions [24, 25].Figure 3
FTIR spectra of WM.


### 3.1.3. TGA and DSC Studies

The DSC and TGA result curves are shown in Figures4 and 5. The thermal changes in the WM can be observed during heating. The DSC curve shows a peak of endothermic transformation at 136.17°C, which explains the evaporation of water molecules and also the fusion of the organic molecules that have remained in the waste mint. These results, after the thermal transformation, were confirmed by the TGA curve which gives a water loss of the WM of 7.8% (86.4% decomposable before 200°C), in addition to the 5.9% related to the residues of the WM left during heating to 1000°C. Based on these results, we can suggest that the WM material can be used for adsorption experiments at temperatures below 100°C, as no thermal changes will be detected in this range.Figure 4
TGA for WM.Figure 5
DSC for WM.


## 3.1.1. SEM-EDS Studies

The scanning electron microscope (SEM) images shown in Figure2 revealed the morphological nature of the piece of waste mint (0.5 cm × 0.5 cm) at the resolution of 50 μm (Figure 2(a)) and 10 μm (Figure 2(b)).Figure 2
SEM images of the WM adsorbent: (a) 50μm; (b) 10 μm.The results obtained show, on the one hand, an irregular and porous structure and, on the other hand, a heterogeneity of the pores shapes over the whole surface of the WM. This result encourages the evaluation of this waste as an adsorbent in the treatment of chromium-polluted water. Furthermore, the microanalysis by energy dispersive analysis of X-ray spectroscopy (EDX) of this surface gives a chemical composition as functions of mass percentages as it listed in Table1.Table 1
Percent for major atomic composition determined by EDX.
CompositionCONOther elementsPercentage content (%)66.3321.844.636.2The results show a high percentage of carbon (C) and oxygen (O), which is consistent with the organic nature of the support.


## 3.1.2. FTIR Spectroscopy

Figure3 illustrates the FTIR spectrum of MM. The broad band in the region around 3425 cm−1 is attributed to the surface hydroxyl groups of the bonded carboxylic acid. The O-H stretching vibrations occurred within a broad range of frequencies indicating the presence of free hydroxyl groups and bonded O-H bands of carboxylic acid. The asymmetric C-H stretching of the methyl surface groups usually present on the lignin structure is observed at 2920 cm−1. The characteristic peaks of C-O group in the carboxylic and alcoholic groups were found at 1050 and 1033 cm−1. The ionisation of the carboxylic acid and hydroxyl functional groups present in the structure of the adsorbent can be obtained by deprotonation, which allows it to interact easily with metals, and can therefore constitute the main adsorption sites for the removal of Cr(VI) ions from solutions. The -OH, -NH, carbonyl, and carboxylic groups have been reported as very important sorption sites for metal ions [24, 25].Figure 3
FTIR spectra of WM.


## 3.1.3. TGA and DSC Studies

The DSC and TGA result curves are shown in Figures4 and 5. The thermal changes in the WM can be observed during heating. The DSC curve shows a peak of endothermic transformation at 136.17°C, which explains the evaporation of water molecules and also the fusion of the organic molecules that have remained in the waste mint. These results, after the thermal transformation, were confirmed by the TGA curve which gives a water loss of the WM of 7.8% (86.4% decomposable before 200°C), in addition to the 5.9% related to the residues of the WM left during heating to 1000°C. Based on these results, we can suggest that the WM material can be used for adsorption experiments at temperatures below 100°C, as no thermal changes will be detected in this range.Figure 4
TGA for WM.Figure 5
DSC for WM.


## 3.2. Effect of Various Adsorption Parameters

### 3.2.1. Effect of Solution pH

The pH effect on the adsorption process was investigated by undertaking the batch adsorption technique at different hydrogen ion concentrations while maintaining the other parameters constant atT = 298 K, t = 120 min, m = 2 g/L, and Ci = 50 mg/L Cr(VI). The pH of the adsorption medium was varied between 2 and 11, and the adsorbent (WM) gave the highest performance of 76% at the pH = 2 (Figure 6). The maximum performance was obtained at pH = 2, and hence, all the other experiments were carried at this pH value. In aqueous solutions, Cr(VI) exists in several stable forms such as CrO42−, HCrO4−, and Cr2O72− [26]. In the range of maximum adsorption pH, the dominant species was reported to be HCrO4−. The chemical nature of the functional groups in waste mint (WM) can be modified by changes in the pH of the adsorption medium and subsequently increasing the sorption capacity of the metals in the adsorbents [27].Figure 6
Effect of pH on the adsorption of Cr(VI) ions from aqueous solution using WM adsorbent atT = 298 K, time = 120 min, adsorbent dose W = 2 g/L, and [Cr(VI)] = 50 mg/L.There was reported competition for the same sorption sites with metal ions by hydrogen ions at low pH values, and it is therefore suggested that the sites of adsorption on the surface of the WM are taken up by hydrogen ions (H+), making the surface positively charged. Then, the negatively charged ions HCrO4− will approach and spontaneously access the binding sites on the adsorbent in order to pick up the more important metal ions due to the electrical attraction with the positive sites generated by the H+ [28].


### 3.2.2. Effect of Cr(VI) Initial Concentration

The performance effectiveness of WM has been studied at different initial concentrations of hexavalent chromium of 10, 20, 30, 40, and 50 mg/L (Figure7), while keeping other parameters constant. The adsorption efficiency decreases with increasing concentration of Cr(VI) ions, and it is noted that the removal percentage has a maximum value of 90% for the initial chromium concentration of 10 mg/L. The explanation of this phenomenon is that when the concentration of Cr(VI) is high enough, the surface of the adsorbent is occupied and the efficiency starts to decrease, and therefore, the molecules desorb from the adsorbent surface.Figure 7
Effect of Cr(VI) concentration on the adsorption rate from aqueous solution using WM adsorbent atT = 298 (K), pH = 2, time = 120 min, and adsorbent dose W = 2 g/L.


### 3.2.3. Effect of Adsorbent Dosage

Figure8 shows that the percentage removal of hexavalent chromium from the MW increased from 11% to 98% as the adsorbent dosage increased from 0.1 to 10 g/L. This is attributed to the increase in adsorption area and the availability of more adsorption sites.Figure 8
Effect of adsorbent dose on Cr(VI) ions removal from aqueous solution using WM adsorbent atT = 298 (K), pH = 2, time = 120 min, and [Cr(VI)] = 50 mg/L.


### 3.2.4. Effect of Temperature

The temperature effect on the removal of Cr(VI) ions by MW was studied at three temperatures: 298 K, 308 K, and 318 K, as shown in Figure9. The maximum adsorption capacity was obtained at 298 K for a pH of 2 (74.9%). The adsorption capacity decreased with increasing temperature, suggesting that the adsorption process was exothermic.Figure 9
Effect of temperature on the adsorption of Cr(VI) from aqueous solution using WM adsorbent at pH = 2, time = 120 min, adsorbent doseW = 2 g/L, and [Cr(VI)] = 50 mg/L.


## 3.2.1. Effect of Solution pH

The pH effect on the adsorption process was investigated by undertaking the batch adsorption technique at different hydrogen ion concentrations while maintaining the other parameters constant atT = 298 K, t = 120 min, m = 2 g/L, and Ci = 50 mg/L Cr(VI). The pH of the adsorption medium was varied between 2 and 11, and the adsorbent (WM) gave the highest performance of 76% at the pH = 2 (Figure 6). The maximum performance was obtained at pH = 2, and hence, all the other experiments were carried at this pH value. In aqueous solutions, Cr(VI) exists in several stable forms such as CrO42−, HCrO4−, and Cr2O72− [26]. In the range of maximum adsorption pH, the dominant species was reported to be HCrO4−. The chemical nature of the functional groups in waste mint (WM) can be modified by changes in the pH of the adsorption medium and subsequently increasing the sorption capacity of the metals in the adsorbents [27].Figure 6
Effect of pH on the adsorption of Cr(VI) ions from aqueous solution using WM adsorbent atT = 298 K, time = 120 min, adsorbent dose W = 2 g/L, and [Cr(VI)] = 50 mg/L.There was reported competition for the same sorption sites with metal ions by hydrogen ions at low pH values, and it is therefore suggested that the sites of adsorption on the surface of the WM are taken up by hydrogen ions (H+), making the surface positively charged. Then, the negatively charged ions HCrO4− will approach and spontaneously access the binding sites on the adsorbent in order to pick up the more important metal ions due to the electrical attraction with the positive sites generated by the H+ [28].


## 3.2.2. Effect of Cr(VI) Initial Concentration

The performance effectiveness of WM has been studied at different initial concentrations of hexavalent chromium of 10, 20, 30, 40, and 50 mg/L (Figure7), while keeping other parameters constant. The adsorption efficiency decreases with increasing concentration of Cr(VI) ions, and it is noted that the removal percentage has a maximum value of 90% for the initial chromium concentration of 10 mg/L. The explanation of this phenomenon is that when the concentration of Cr(VI) is high enough, the surface of the adsorbent is occupied and the efficiency starts to decrease, and therefore, the molecules desorb from the adsorbent surface.Figure 7
Effect of Cr(VI) concentration on the adsorption rate from aqueous solution using WM adsorbent atT = 298 (K), pH = 2, time = 120 min, and adsorbent dose W = 2 g/L.


## 3.2.3. Effect of Adsorbent Dosage

Figure8 shows that the percentage removal of hexavalent chromium from the MW increased from 11% to 98% as the adsorbent dosage increased from 0.1 to 10 g/L. This is attributed to the increase in adsorption area and the availability of more adsorption sites.Figure 8
Effect of adsorbent dose on Cr(VI) ions removal from aqueous solution using WM adsorbent atT = 298 (K), pH = 2, time = 120 min, and [Cr(VI)] = 50 mg/L.


## 3.2.4. Effect of Temperature

The temperature effect on the removal of Cr(VI) ions by MW was studied at three temperatures: 298 K, 308 K, and 318 K, as shown in Figure9. The maximum adsorption capacity was obtained at 298 K for a pH of 2 (74.9%). The adsorption capacity decreased with increasing temperature, suggesting that the adsorption process was exothermic.Figure 9
Effect of temperature on the adsorption of Cr(VI) from aqueous solution using WM adsorbent at pH = 2, time = 120 min, adsorbent doseW = 2 g/L, and [Cr(VI)] = 50 mg/L.


## 3.3. Adsorption Kinetics

In order to define the adsorption kinetics of Cr(VI) by the WM adsorbent, the kinetic parameters of the adsorption process were studied for contact times varying from 0 to 120 min by controlling the concentration of Cr(VI) held in the filtrate. Figure10 shows the adsorption kinetics curves for different initial concentrations of Cr(VI): 10, 20, 30, 40, and 50 mg/L.Figure 10
Kinetics adsorption of Cr(VI) from aqueous solution using WM adsorbent at pH = 2, time = 120 min, and adsorbent doseW = 2 g/L.All kinetic parameters of Cr(VI) adsorption by WM are determined from the linear form of the model equations described in [19, 20].The linear representations are shown in Figures11–14, respectively.Figure 11
Linearity of the pseudo-first-order model.Figure 12
Linearity of the pseudo-second-order model.Figure 13
Linearity of Elovich model.Figure 14
Linearity of intraparticle diffusion model.To find the best fit kinetic model, the correlation coefficients (R2) of the different models were compared and are grouped in Table 2. However, R2 correlation coefficients showed that the fractional power model fits better to the experimental data (0.97 ≤ R2 ≤ 0.99) than the other models (R2 is in the range of 0.24–0.99).Table 2
Adsorption kinetic model parameters at pH 2 for Cr(VI) removal.
ModelParametersC0 = 10 mg/LC0 = 20 mg/LC0 = 30 mg/LC0 = 40 mg/LC0 = 50 mg/LFractional powerLinear expressiony = 0.217x + 0.560y = 0.264x + 0.984y = 0.289x + 1.233y = 0.280x + 1.509y = 0.276x + 1.592R20.970.980.970.990.97kp1.7502.6753.4314.5224.913Υ0.2170.2640.2890.2800.276Pseudo-first-orderLinear expressiony = −0.035x + 1.398y = −0.030x + 1.994y = −0.025x + 2.335y = −0.023x + 2.634y = −0.025x + 2.739R20.930.970.920.950.93k1P (min−1)0.0250.0230.0250.0300.035qe.1P (mg.g−1)15.47113.92910.3297.3444.047Pseudo-second-orderLinear expressiony = 1.940x + 0.195y = 1.321x + 0.099y = 1.025x + 0.068y = 0.745x + 0.055y = 0.672x + 0.052R20.950.980.960.940.91k2P (g.mg−1.min−1)0.1000.0740.0660.0730.077qe.2P (mg.g−1)5.12810.10114.70518.18119.230ElovichLinear expressiony = 0.866x + 0.772y = 1.908x + 0,228y = 2.942x – 0.603y = 3.715x – 0.66y = 3.947x – 0.603R20.960.990.970.970.95αE (mg.g−1.min−1)2.1112.1502.3963.1103.387βE (g.mg−1)1.1540.5240.3390.2690.253Intraparticle diffusionLinear expressiony = 0.253x + 2.248y = 0.552x + 3.521y = 0.853x + 4.458y = 1.101x + 5.558y = 1.176x + 5.948R20.960.960.950.990.98kD (mg.g−1.min−1/2)0.2530.5520.8531.1011.176CD (mg.g−1)2.2483.5214.4585.5585.948


## 3.4. Adsorption Isotherms Studies

The isotherms study of Cr(VI) adsorption by the MW was carried out for 2 hours, with an initial Cr(VI) C0 concentration of 50 mg/L and a pH = 2, for different masses of the MW (W = 0.1, 0.5, 1, and 2 g/L). The variation of the adsorption capacity Qe is related with the equilibrium concentration Ce. Several models were applied to describe the experimental data for the adsorption isotherms. The Freundlich and Langmuir models are the most frequently used. In the present work, four models were used and described in [21, 22]. All parameters of the isotherms were determined from the linear relation (Figures 15–18) according to the equations of the models described in [21, 22].Figure 15
Linearity of Freundlich model.Figure 16
Linearity of Langmuir model.Figure 17
Linearity ofD-R model.Figure 18
Linearity of Temkin model.The best-fit isotherms models were determined by calculating the determination coefficients (R2). Parameter values at pH = 2 for the maximum Cr (VI) adsorption by MW are reported in Table 3. From the values of the correlation coefficients, it can be concluded that the Langmuir model was best fitted to the experimental results of Cr(VI) adsorption by WM.Table 3
Adsorption isotherms models parameter at pH 2 for Cr(VI) adsorption by WM.
ModelModel parametersValues of parametersFreundlichLinear expressiony = 0.824+0.856R20.97KF (L/g)2.354nF0.824LangmuirLinear expressiony = 0.593x+0.005R20.98KL (L/g)0.009qm.L (mg/g)172.410RL0.999D-RLinear expressiony = −175.960x + 3.915R20.87E (J/mol)186.770qm,DR (mg/g)50.180TemkinLinear expressiony = 27.690x-53.113R20.92KT (L/g)0.146BT (J/mol)27.690The essential characteristic parameter of the Langmuir isotherm can be expressed in terms of a dimensionless constant separation factor or also known as the equilibrium parameterRL [29]:(6)RL=11+KL⋅C0,where KL (L/mg) is the Langmuir constant and C0 (mg/L) is the initial concentration. RL = 1 represents linear adsorption, while RL = 0 stands for the irreversible adsorption process. RL < 1 is for favorable adsorption, while RL > 1 represents unfavorable adsorption. In this work, the value of RL was found to be 0.999, suggesting that the equilibrium parameter was less than 1 but near to 1, which means a favorable linear adsorption. This means that the equilibrium isotherms can be well described by the Langmuir model (Figure 19), and the adsorption process takes place as a monolayer (ML) on a surface with a finite number of identical sites, which are distributed homogeneously over the surface of the adsorbent [30].Figure 19
Modeling of the isotherm adsorption by Langmuir model.


## 3.5. Thermodynamics Studies

The thermodynamic parameters of an adsorption process are necessary to decide whether the process is spontaneous or not. Experimental data obtained at different temperatures were used to calculate thermodynamic parameters such as Gibbs-free energy change (ΔG°), enthalpy change (ΔH°), and entropy change (ΔS°). The Gibbs-free energy changes in the sorption reaction are given by equations (3)–(5), where K = KL is the equilibrium constant, which can be obtained from the Langmuir isotherm at different temperatures. ΔH° and ΔS° were obtained from the slope and intercept of the plot of ln KL vs. 1/T (Figure 20). The calculated results are reported in Table 4.Figure 20
FTIR spectra of WM before and after adsorption.Table 4
Thermodynamic parameters of adsorption of Cr(VI) on the WM.
ΔH° (KJ/mol)ΔS° (KJ/K.mol)ΔG° (KJ/mol)298 K308 K318 K-28.93−0.081−4.83−4.02−3.22The negative values of ΔG° confirm the feasibility of the process and the spontaneous nature of adsorption. The standard enthalpy and entropy changes in adsorption determined from Figure 20 were −28.93 kJ/mol and −0.081 kJ/k.mol, respectively, with a correlation coefficient of 0.96. The value of ΔH° is negative, indicating that the adsorption reaction is exothermic. The negative value of ΔS° reflects a decrease in the randomness at the solid/solution interface during the adsorption process [31].


## 3.6. Mechanism of Adsorption by FTIR

The FTIR spectra before and after the adsorption of Cr(VI) by WM are shown in Figure19. For the spectrum obtained after the adsorption of hexavalent chromium, there is a remarkable change in the intensities of the infrared bands without any change in position. The characterization by infrared spectroscopy also made it possible to confirm the results obtained by other methods of investigation. The structural properties of the adsorbent determine the effect of the degree of impregnation on the pore type distribution and the pore structure of the adsorbent. It has been determined that vigorous stimulation promotes pore formation at this level [32].


## 3.7. Comparison of Cr(VI) Adsorption Capacity of Different Adsorbents

The adsorption capacity of the different Cr(VI) adsorbents previously studied in the bibliography was compared with the current results, as shown in Table5. It can be observed that the maximum adsorption capacity (Qmax), at pH = 2, is higher (172 mg/g for the WM) than the most recently reported adsorbents. This result indicates that the waste mint applied in this study is a better alternative to other low-cost adsorbents. However, higher adsorption capacities of 250 and 278 mg/g were reported for modified rice husk and mosambi (Citrus limetta) peel at the same pH, respectively.Table 5
Comparison of adsorption capacities of WM with other adsorbents for Cr(VI).
No.AdsorbentQmax (mg/g)pHRef.1Modified rice husk2782[33]2Mosambi (Citrus limetta) peel2502[34]3Modified groundnut shell1312[35]4Chrysophyllum albidum (Sapotaceae) seed shells84.313[36]5Treated waste newspaper59.883[37].6Guar gum–nano-zinc oxide55.567[38]7Rice husk carbon47.612[39]8Eucalyptus bark452[40]9Wool41.152[41]10Olive cake33.442[42]11Chitosan-coated fly ash33.275[43]12Modified seaweed (Bifurcaria bifurcata)29.295.8[18]13Plantain waste16.1[44]14Saw dust15.822[45]15Almond10.612[46]16Banana (Musa Lacatan) waste102[47]17Tea (Camellia sinensis) waste7.292[42]18Pine needles7.082[48]19Peels of pea (Pisum sativum) pod4.332[49]20Waste of mint (Mentha spicata)1722This work


## 4. Conclusion

Removal of Cr(VI) from wastewater is possible using several abundantly available low-cost adsorbents. The present investigation showed that the WM is an effective adsorbent for the removal of chromium(VI) from aqueous solutions. The WM was characterized using SEM, FTIR, TGA, and DSC analysis. The effects of pH, initial concentration of Cr(VI), and adsorbent dose and temperature, on adsorption were investigated. The adsorption decreased with increasing pH, initial concentration of Cr(VI), and temperature, while it increased with increasing adsorbent dose. The kinetic data followed the fractional power kinetic model. The isotherm data were analyzed by Freundlich, Langmuir,D–R, and Temkin isotherms, and the data fitted the Langmuir model better than the other models. The maximum monolayer coverage adsorption capacity from the Langmuir isotherm model was 172 mg/g. The thermodynamics parameters were calculated: the negative values of ΔG˚ indicate the spontaneous nature of the adsorption process, and the negative values of ΔH˚ indicate the exothermic nature of the adsorption. Finally, the FTIR results suggested that the adsorption of Cr(VI) on the WM was mechanical entrapment.



---

*Source: 8848964-2021-04-22.xml*