# Activated Carbon from the Peelings of Cassava Tubers (Manihot esculenta) for the Removal of Nickel(II) Ions from Aqueous Solution

Authors: Brice Armel Ajouafeu Alongamo; Lydie Dodo Ajifack; Julius Numbonui Ghogomu; Ndi Julius Nsami; Joseph Mbadcam Ketcha
Journal: Journal of Chemistry
 (2021)

---

## Abstract

Activated carbons were obtained from the peelings of cassava tubers (Manihot esculenta) by chemical activation using potassium hydroxide and phosphoric acid at impregnation ratios of 2 : 1 and 1 : 1, respectively, at 400°C for batch adsorption of nickel(II) ions from aqueous solution. Characterization of activated carbon samples was achieved via proximate analysis, Fourier-transform infrared spectroscopy, pH of zero-point charge, Boehm method, elemental analysis, scanning electron microscopy, and iodine number determination for each adsorbent. The effects of pH, contact time, initial adsorbate concentration, and adsorbent dose were studied at 27°C in order to optimize the conditions for maximum adsorption. Equilibrium was attained after 40 minutes of contact of both materials with activating solutions. Maximum adsorption capacities of 41.15 mg/g for ACPH, 47.39 mg/g for ACPA, 35.34 mg/g for NIC, and 34.48 mg/g for RM, respectively, were obtained at pH = 4. Equilibrium data showed that the Langmuir model best described the adsorption process with R2 closed to unity, indicative of monolayer adsorption on a homogeneous surface. Kinetic studies showed that the adsorption process is controlled by the pseudo-second-order model. These results show that activated carbon prepared from cassava peelings constitutes an effective low-cost material for the treatment of wastewater containing nickel(II) ions.


---

## Body

## 1. Introduction

Pollution by heavy metals is a global health and environmental concern [1]. Nickel is a nonbiodegradable and toxic heavy metal, which is ubiquitous in wastewater bodies in various proportions [2]. The main origin of nickel pollution in water is from industrial processes such as galvanization, smelting mining, dyeing operation, battery manufacturing, and metal finishing [3]. Trace amounts of nickel are beneficial to human life as enzyme activators. Above permissible concentrations (toxic limits) of nickel of 0.1 mg/m3 (World Health Organization (WHO)) [4], different types of diseases may be contracted such as lung cancer, renal edema, dermatitis, and gastrointestinal disorder. Conventional methods for nickel(II) removal from wastewater include chemical oxidation or reduction, chemical precipitation, ion exchange, membrane separation, filtration, electrochemical treatment, and adsorption [5]. These techniques which are economically expensive suffer from incomplete metal removal, generation of toxic sludge, and other disposable waste products [6]. Adsorption techniques using organic, inorganic, natural, synthetic, activated, or modified adsorbents are the most widely employed procedures in wastewater treatment and constitute low-cost alternatives. From the literature survey, potential low-cost adsorbents (activated or not) for heavy metal removal include the following: Rice Husk [4], sugarcane bagasse pith [7], coconut husk, date stones, teak tree bark [8], palm fruit seeds [9], exhausted olive cake, coconut leaves, ion exchange resins [10], industrial wastes [11], fruit wastes, sugar industry wastes, seafood-processing wastes, wood-type materials, petroleum wastes, and fertilizer wastes [12]. Activated carbon is obtained via either physical or chemical activation procedures and is characterized by a large surface area, high adsorption capacity, high yields, porous structure, selective adsorption, and high purity [13]. During the chemical activation process, reagents such as inorganic salts (ZnCl2, FeCl3, KHCO3, NaCl, MgCl2, Na2CO3 CaCl2, and K2CO3), acids (HNO3, H2SO4, and H3PO4), or soluble bases (NaOH, KOH) are often used [14]. These chemical agents favor the dehydration of materials and allow for the development of micropores [15]. The objective of this study was to evaluate the performance of activated carbons obtained by chemical activation with KOH and H3PO4 of the peelings of cassava tubers (Manihot esculenta) for the removal of nickel(II) from aqueous solution.


## 2. Materials and Methods

### 2.1. Collection and Pretreatment of Raw Materials

In order to valorize low-cost local materials like activated carbon, the Forastero variety of cassava tuber peelings (Manihot esculenta) was used as a precursor because of its abundance in the subregion. Cassava tuber peelings were acquired in great quantity from a local factory in Santchou village situated in the West Region of Cameroon which is involved in the processing of cassava-based foodstuff. They were transported to the laboratory after undergoing thorough washing and cleaning under tap and distilled water for the removal of residual soil and other impurities. In the laboratory, they were stripped of their outer thin skin with a plastic brush, chopped into smaller pieces, and air dried for two weeks after which they were crushed in a mill and finally sieved to have the coarse grain fraction with average particle size of 2 mm (with increased surface area for activation). The dried peelings underwent coarse crushing in order to obtain homogeneous materials (precursors). After sieving through standard steel sieves, only fractions with diameters of less than 400 µm were retained (Figure 1).Figure 1
Step-by-step illustration of AC preparation from the peelings of cassava tubers.


### 2.2. Production of Activated Carbon

In this study, all chemicals used for activation purposes were of analytical grade. Test samples were prepared in two ways: the first part involved the chemical activation process involving phosphoric acid (H3PO4, from Fischer Scientific International at 85% purity) and potassium hydroxide (KOH, from Fischer Scientific International at 87.90% purity) as activation agents. This method consisted of mixing the precursor material with either 10% weight of KOH (activated carbon, potassium hydroxide (ACPH)) or 10% weight of H3PO4 (activated carbon, phosphoric acid (ACPA)) before carbonization. 10.0 g of material samples was impregnated with solutions of activating agent (KOH and H3PO4) in a desired weight ratio of material to the activating agent of 2 : 1, 1 : 1, and 1 : 2, respectively. The impregnated samples were then placed in an oven at 110°C for 24 hours. In the second part, samples were prepared in the same manner but without impregnation or activation. Both the treated and untreated samples were later carbonized for one hour in a Carbolite furnace (Heraeus) in the absence of air (oxygen). Initially, the furnace was heated to temperatures of 300, 400, and 500°C, respectively, at a heating rate of 10°C min−1 for 1 hour (activation time). The variation of these activation and calcination parameters is summarized in Table S1 of supplementary materials. The carbonized samples were then allowed to cool to ambient temperature. ACPA samples after washing abundantly with distilled water were treated with lead nitrate (0.1 M) (from BDH Chemicals Ltd. at 98% purity) in order to ensure the complete elimination of traces of phosphate ions. ACPH samples on their part were then leached with a solution of hydrochloric acid (HCl 0.1 M (from Prolabo at 36% purity)) for 2 hours and abundantly washed with distilled water until the pH of the resulting samples ranged between 6 and 7. Silver nitrate (from Alfa Aesar at 99.9% purity) test was conducted to check for complete elimination of the chloride ions introduced [14]. The resultant activated carbon samples (ACPH, ACPA) and the nonimpregnated carbon (NIC) along with precursors (raw material (RM)) were then oven-dried at 110°C for a period of 24 hours, ground, and then sieved to obtain particles with diameters less than 100 µm. The preparation steps are as indicated in Figure 1.


### 2.3. Proximate Analysis

Proximate analysis is a series of tests used for the determination of the composition of available macronutrients (moisture content, volatile matter, ash content, and fixed carbon content) in the cassava tuber peelings when samples were heated and treated under specific conditions.


#### 2.3.1. Moisture Content

The moisture content of the material samples was determined according to the procedure established by the American Society for Testing and Materials (ASTMD 2867-99) [16] in which 1.0 g of dried material was weighed in a cleaned crucible and was oven-dried at 110°C for 3 hours. After drying, samples were then cooled at room temperature in a desiccator and reweighed in order to determine their moisture contents according to the following equation:(1)moisture content%=loss in weight in dryingginitial sample weightg×100.


#### 2.3.2. Ash Content

The ash content of the material samples was determined via the ASTMD 2867-94 standard method [16] in which 1.0 g of dry sample was weighed inside a crucible, oven-dried at 105°C, and later introduced into a Carbolite furnace (Heraeus) that was then heated to 600°C at a heating rate of 10°C min−1 for 1 hour. The carbonized sample was then allowed to cool to ambient temperature. The samples were then removed from the furnace and stored in a desiccator. The sample was then reweighed, and the ash content was obtained from the difference in weight according to the following equation:(2)ash content%=weight of ashgoven dry weightg×100.


#### 2.3.3. Volatile Matter

Volatile matter of the material samples was determined via the ASTMD 2867-99 standard method [16] in which 1.0 g of dry sample is weighed inside a crucible and oven-dried at 105°C and then heated to 600°C for 1 hour in a Carbolite furnace (Heraeus) at a heating rate of 10°C min−1. The carbonized sample was then allowed to cool to ambient temperature and later was removed from the furnace and stored in a desiccator. The sample was then reweighed, and the volatile matter was calculated from the difference in weight according to the following equation:(3)volatile matter%=weight of volatile componentgoven−dry weightg×100.The fixed carbon content was obtained by subtracting the percentage of moisture, ash, and volatile matter content of the materials from a hundred percent according to(4)fixed carbon%=100−moisture%−ash content%−volatile matter%.


### 2.4. Iodine Number (IN)

The iodine number (IN) is a relative indicator of porosity in activated carbon. The iodine number was measured according to the procedure established by the American Society for Testing and Materials (ASTM D2866-94) [17]. It is the number of milligrams of iodine adsorbed by 1.0 g of carbon when the iodine concentration of the filtrate is 0.02 N. The iodine number is accepted as a fundamental parameter used to characterize activated carbon performance. Iodine number was employed in this study as a test for microporosity via volumetric analysis. This fundamental ability test for activated carbon determines its microporosity to ≤2 nm.


#### 2.4.1. Standardization of Iodine Solution

10 mL of 0.02 N iodine solutions (from Merck at 99.95% purity) was measured and put into a conical flask, and 2-3 drops of a starch solution were added to it. The pale-yellow color of the iodine solution turned blue and was titrated against a 0.005 N sodium thiosulphate solution (from Fischer Scientific International at 99.8%) until the mixture became colorless.


#### 2.4.2. Determination of Iodine Number

0.1 g of activated carbon was weighed (mAC) and carefully introduced into a dry screw cap conical flask. 30 mL of 0.02 N iodine solutions was then added. The flask was magnetically stirred for 3 hours, and the content was filtered into a dry conical flask. Then, 10 mL of the filtrate was titrated against sodium thiosulphate solution (5 × 10−3 M) (Na2S2O3 from Acros organics at 99% purity) using starch as indicator until a clear solution was observed according to equation (5). The volume delivered by the burette was then noted (Vn). The iodine number for the sample was then calculated according to equation (6):(5)2Na2S2O3aq+I2⟶Na2S4O6aq+2NaIaq(6)iodine number=25.4×30−VnmAC,where mAC (g) is the mass of the activated carbon and Vn (mL) is the volume of the sodium thiosulphate solution at the equivalence point.


## 2.1. Collection and Pretreatment of Raw Materials

In order to valorize low-cost local materials like activated carbon, the Forastero variety of cassava tuber peelings (Manihot esculenta) was used as a precursor because of its abundance in the subregion. Cassava tuber peelings were acquired in great quantity from a local factory in Santchou village situated in the West Region of Cameroon which is involved in the processing of cassava-based foodstuff. They were transported to the laboratory after undergoing thorough washing and cleaning under tap and distilled water for the removal of residual soil and other impurities. In the laboratory, they were stripped of their outer thin skin with a plastic brush, chopped into smaller pieces, and air dried for two weeks after which they were crushed in a mill and finally sieved to have the coarse grain fraction with average particle size of 2 mm (with increased surface area for activation). The dried peelings underwent coarse crushing in order to obtain homogeneous materials (precursors). After sieving through standard steel sieves, only fractions with diameters of less than 400 µm were retained (Figure 1).Figure 1
Step-by-step illustration of AC preparation from the peelings of cassava tubers.


## 2.2. Production of Activated Carbon

In this study, all chemicals used for activation purposes were of analytical grade. Test samples were prepared in two ways: the first part involved the chemical activation process involving phosphoric acid (H3PO4, from Fischer Scientific International at 85% purity) and potassium hydroxide (KOH, from Fischer Scientific International at 87.90% purity) as activation agents. This method consisted of mixing the precursor material with either 10% weight of KOH (activated carbon, potassium hydroxide (ACPH)) or 10% weight of H3PO4 (activated carbon, phosphoric acid (ACPA)) before carbonization. 10.0 g of material samples was impregnated with solutions of activating agent (KOH and H3PO4) in a desired weight ratio of material to the activating agent of 2 : 1, 1 : 1, and 1 : 2, respectively. The impregnated samples were then placed in an oven at 110°C for 24 hours. In the second part, samples were prepared in the same manner but without impregnation or activation. Both the treated and untreated samples were later carbonized for one hour in a Carbolite furnace (Heraeus) in the absence of air (oxygen). Initially, the furnace was heated to temperatures of 300, 400, and 500°C, respectively, at a heating rate of 10°C min−1 for 1 hour (activation time). The variation of these activation and calcination parameters is summarized in Table S1 of supplementary materials. The carbonized samples were then allowed to cool to ambient temperature. ACPA samples after washing abundantly with distilled water were treated with lead nitrate (0.1 M) (from BDH Chemicals Ltd. at 98% purity) in order to ensure the complete elimination of traces of phosphate ions. ACPH samples on their part were then leached with a solution of hydrochloric acid (HCl 0.1 M (from Prolabo at 36% purity)) for 2 hours and abundantly washed with distilled water until the pH of the resulting samples ranged between 6 and 7. Silver nitrate (from Alfa Aesar at 99.9% purity) test was conducted to check for complete elimination of the chloride ions introduced [14]. The resultant activated carbon samples (ACPH, ACPA) and the nonimpregnated carbon (NIC) along with precursors (raw material (RM)) were then oven-dried at 110°C for a period of 24 hours, ground, and then sieved to obtain particles with diameters less than 100 µm. The preparation steps are as indicated in Figure 1.


## 2.3. Proximate Analysis

Proximate analysis is a series of tests used for the determination of the composition of available macronutrients (moisture content, volatile matter, ash content, and fixed carbon content) in the cassava tuber peelings when samples were heated and treated under specific conditions.


### 2.3.1. Moisture Content

The moisture content of the material samples was determined according to the procedure established by the American Society for Testing and Materials (ASTMD 2867-99) [16] in which 1.0 g of dried material was weighed in a cleaned crucible and was oven-dried at 110°C for 3 hours. After drying, samples were then cooled at room temperature in a desiccator and reweighed in order to determine their moisture contents according to the following equation:(1)moisture content%=loss in weight in dryingginitial sample weightg×100.


### 2.3.2. Ash Content

The ash content of the material samples was determined via the ASTMD 2867-94 standard method [16] in which 1.0 g of dry sample was weighed inside a crucible, oven-dried at 105°C, and later introduced into a Carbolite furnace (Heraeus) that was then heated to 600°C at a heating rate of 10°C min−1 for 1 hour. The carbonized sample was then allowed to cool to ambient temperature. The samples were then removed from the furnace and stored in a desiccator. The sample was then reweighed, and the ash content was obtained from the difference in weight according to the following equation:(2)ash content%=weight of ashgoven dry weightg×100.


### 2.3.3. Volatile Matter

Volatile matter of the material samples was determined via the ASTMD 2867-99 standard method [16] in which 1.0 g of dry sample is weighed inside a crucible and oven-dried at 105°C and then heated to 600°C for 1 hour in a Carbolite furnace (Heraeus) at a heating rate of 10°C min−1. The carbonized sample was then allowed to cool to ambient temperature and later was removed from the furnace and stored in a desiccator. The sample was then reweighed, and the volatile matter was calculated from the difference in weight according to the following equation:(3)volatile matter%=weight of volatile componentgoven−dry weightg×100.The fixed carbon content was obtained by subtracting the percentage of moisture, ash, and volatile matter content of the materials from a hundred percent according to(4)fixed carbon%=100−moisture%−ash content%−volatile matter%.


## 2.3.1. Moisture Content

The moisture content of the material samples was determined according to the procedure established by the American Society for Testing and Materials (ASTMD 2867-99) [16] in which 1.0 g of dried material was weighed in a cleaned crucible and was oven-dried at 110°C for 3 hours. After drying, samples were then cooled at room temperature in a desiccator and reweighed in order to determine their moisture contents according to the following equation:(1)moisture content%=loss in weight in dryingginitial sample weightg×100.


## 2.3.2. Ash Content

The ash content of the material samples was determined via the ASTMD 2867-94 standard method [16] in which 1.0 g of dry sample was weighed inside a crucible, oven-dried at 105°C, and later introduced into a Carbolite furnace (Heraeus) that was then heated to 600°C at a heating rate of 10°C min−1 for 1 hour. The carbonized sample was then allowed to cool to ambient temperature. The samples were then removed from the furnace and stored in a desiccator. The sample was then reweighed, and the ash content was obtained from the difference in weight according to the following equation:(2)ash content%=weight of ashgoven dry weightg×100.


## 2.3.3. Volatile Matter

Volatile matter of the material samples was determined via the ASTMD 2867-99 standard method [16] in which 1.0 g of dry sample is weighed inside a crucible and oven-dried at 105°C and then heated to 600°C for 1 hour in a Carbolite furnace (Heraeus) at a heating rate of 10°C min−1. The carbonized sample was then allowed to cool to ambient temperature and later was removed from the furnace and stored in a desiccator. The sample was then reweighed, and the volatile matter was calculated from the difference in weight according to the following equation:(3)volatile matter%=weight of volatile componentgoven−dry weightg×100.The fixed carbon content was obtained by subtracting the percentage of moisture, ash, and volatile matter content of the materials from a hundred percent according to(4)fixed carbon%=100−moisture%−ash content%−volatile matter%.


## 2.4. Iodine Number (IN)

The iodine number (IN) is a relative indicator of porosity in activated carbon. The iodine number was measured according to the procedure established by the American Society for Testing and Materials (ASTM D2866-94) [17]. It is the number of milligrams of iodine adsorbed by 1.0 g of carbon when the iodine concentration of the filtrate is 0.02 N. The iodine number is accepted as a fundamental parameter used to characterize activated carbon performance. Iodine number was employed in this study as a test for microporosity via volumetric analysis. This fundamental ability test for activated carbon determines its microporosity to ≤2 nm.


### 2.4.1. Standardization of Iodine Solution

10 mL of 0.02 N iodine solutions (from Merck at 99.95% purity) was measured and put into a conical flask, and 2-3 drops of a starch solution were added to it. The pale-yellow color of the iodine solution turned blue and was titrated against a 0.005 N sodium thiosulphate solution (from Fischer Scientific International at 99.8%) until the mixture became colorless.


### 2.4.2. Determination of Iodine Number

0.1 g of activated carbon was weighed (mAC) and carefully introduced into a dry screw cap conical flask. 30 mL of 0.02 N iodine solutions was then added. The flask was magnetically stirred for 3 hours, and the content was filtered into a dry conical flask. Then, 10 mL of the filtrate was titrated against sodium thiosulphate solution (5 × 10−3 M) (Na2S2O3 from Acros organics at 99% purity) using starch as indicator until a clear solution was observed according to equation (5). The volume delivered by the burette was then noted (Vn). The iodine number for the sample was then calculated according to equation (6):(5)2Na2S2O3aq+I2⟶Na2S4O6aq+2NaIaq(6)iodine number=25.4×30−VnmAC,where mAC (g) is the mass of the activated carbon and Vn (mL) is the volume of the sodium thiosulphate solution at the equivalence point.


## 2.4.1. Standardization of Iodine Solution

10 mL of 0.02 N iodine solutions (from Merck at 99.95% purity) was measured and put into a conical flask, and 2-3 drops of a starch solution were added to it. The pale-yellow color of the iodine solution turned blue and was titrated against a 0.005 N sodium thiosulphate solution (from Fischer Scientific International at 99.8%) until the mixture became colorless.


## 2.4.2. Determination of Iodine Number

0.1 g of activated carbon was weighed (mAC) and carefully introduced into a dry screw cap conical flask. 30 mL of 0.02 N iodine solutions was then added. The flask was magnetically stirred for 3 hours, and the content was filtered into a dry conical flask. Then, 10 mL of the filtrate was titrated against sodium thiosulphate solution (5 × 10−3 M) (Na2S2O3 from Acros organics at 99% purity) using starch as indicator until a clear solution was observed according to equation (5). The volume delivered by the burette was then noted (Vn). The iodine number for the sample was then calculated according to equation (6):(5)2Na2S2O3aq+I2⟶Na2S4O6aq+2NaIaq(6)iodine number=25.4×30−VnmAC,where mAC (g) is the mass of the activated carbon and Vn (mL) is the volume of the sodium thiosulphate solution at the equivalence point.


## 3. Characterization of Adsorbents

### 3.1. Determination of Oxygen Containing Functional Groups

The determination of the total surface acidity and basicity of the activated carbons was carried out via the Boehm method [18, 19]. Acidic surface functions (carboxylic, lactonic, phenolic) were determined by adding 40 mL decimolar solution of NaHCO3 (from Fischer Scientific International at 99.7%), Na2CO3 (from Fischer Scientific International at 99.8% purity), and NaOH (from Fischer Scientific International at 99.5%) into different reactors, each of which previously contained 0.1 g of activated carbon sample. Titration of the excess base was done by using a decimolar solution of HCl after stirring for 48 hours. In the determination of basic functions, 0.1 g of activated carbon was added to 40 mL of a decimolar solution of HCl. After stirring for 48 hours, the excess acid was titrated with a decimolar solution of NaOH.


### 3.2. Determination of pH at Zero-Point Charge (pHzpc)

The pH at a zero-point charge (pHzpc) corresponds to a pH at which the surface charge of activated carbon is neutral. pHzpc of the activated carbon samples was estimated according to the standard procedure [20, 21]. 40.0 mL of a decimolar solution of NaCl (from Fischer Scientific International at 99.5%) was introduced into reactors each containing 0.1 g of activated carbon to be analyzed. The pH of each solution was then adjusted by the addition of decimolar solutions of NaOH or HCl (by varying values of pH between 2 and 12). pHzpc was determined by the intersection of the representative curves pH (final) = f (pH (initial)) and the first bisector curve. Stirring was maintained at 27°C for 48 hours with the aid of a multiagitator system (Edmund BühlerGmbH) and at 150 rpm. The contents of the reactors were then filtered with Whatman filter paper N°4 after which the pH of the final solutions was measured.


### 3.3. Analysis by Fourier-Transform-IR Spectrophotometer (FTIR)

Surface functional groups of adsorbents and their transformation after activation were analyzed using an infrared spectrophotometer (Brüker alpha-p spectrometer) with ethanol (from Fischer Scientific International at 98%) as a solvent with a resolution of 4 cm−1 within the interval 400–4000 cm−1.


### 3.4. Scanning Electron Microscopy (SEM) Analysis

Surface morphology and adsorbent porosity of activated carbon samples were examined by a scanning electron microscope (SEM′ PHILIPS XL30 S-FEG) equipped with a spectrometer having a cathode luminescence detector. These were achieved by the juxtaposition of SEM images of precursor samples (RM) with those of the activated carbon (ACPH, ACPA, and NIC). Only the precursor and the activated carbon samples with high iodine numbers were chosen for SEM analysis.


### 3.5. Elemental Analysis

Elemental composition (C, H, N, S, and O) of ACPH, ACPA, NIC, and RM at 400°C was obtained using an elemental analyzer (Thermo Scientific FLASH 2000).


## 3.1. Determination of Oxygen Containing Functional Groups

The determination of the total surface acidity and basicity of the activated carbons was carried out via the Boehm method [18, 19]. Acidic surface functions (carboxylic, lactonic, phenolic) were determined by adding 40 mL decimolar solution of NaHCO3 (from Fischer Scientific International at 99.7%), Na2CO3 (from Fischer Scientific International at 99.8% purity), and NaOH (from Fischer Scientific International at 99.5%) into different reactors, each of which previously contained 0.1 g of activated carbon sample. Titration of the excess base was done by using a decimolar solution of HCl after stirring for 48 hours. In the determination of basic functions, 0.1 g of activated carbon was added to 40 mL of a decimolar solution of HCl. After stirring for 48 hours, the excess acid was titrated with a decimolar solution of NaOH.


## 3.2. Determination of pH at Zero-Point Charge (pHzpc)

The pH at a zero-point charge (pHzpc) corresponds to a pH at which the surface charge of activated carbon is neutral. pHzpc of the activated carbon samples was estimated according to the standard procedure [20, 21]. 40.0 mL of a decimolar solution of NaCl (from Fischer Scientific International at 99.5%) was introduced into reactors each containing 0.1 g of activated carbon to be analyzed. The pH of each solution was then adjusted by the addition of decimolar solutions of NaOH or HCl (by varying values of pH between 2 and 12). pHzpc was determined by the intersection of the representative curves pH (final) = f (pH (initial)) and the first bisector curve. Stirring was maintained at 27°C for 48 hours with the aid of a multiagitator system (Edmund BühlerGmbH) and at 150 rpm. The contents of the reactors were then filtered with Whatman filter paper N°4 after which the pH of the final solutions was measured.


## 3.3. Analysis by Fourier-Transform-IR Spectrophotometer (FTIR)

Surface functional groups of adsorbents and their transformation after activation were analyzed using an infrared spectrophotometer (Brüker alpha-p spectrometer) with ethanol (from Fischer Scientific International at 98%) as a solvent with a resolution of 4 cm−1 within the interval 400–4000 cm−1.


## 3.4. Scanning Electron Microscopy (SEM) Analysis

Surface morphology and adsorbent porosity of activated carbon samples were examined by a scanning electron microscope (SEM′ PHILIPS XL30 S-FEG) equipped with a spectrometer having a cathode luminescence detector. These were achieved by the juxtaposition of SEM images of precursor samples (RM) with those of the activated carbon (ACPH, ACPA, and NIC). Only the precursor and the activated carbon samples with high iodine numbers were chosen for SEM analysis.


## 3.5. Elemental Analysis

Elemental composition (C, H, N, S, and O) of ACPH, ACPA, NIC, and RM at 400°C was obtained using an elemental analyzer (Thermo Scientific FLASH 2000).


## 4. Equilibrium Studies via Batch Adsorption

### 4.1. Preparation and Determination of Nickel(II) Ions

A standard 2000 mg/L mother solution of nickel(II) was prepared by dissolving 2.1 g of AR grade nickel chloride hexahydrate (NiCl2.6H2O) of molar mass (M = 237.71 g/mol at 98.6% purity from Fischer Scientific International) inside a 250 mL volumetric flask. 5 mL of a 1% HNO3 (from Merck at 65% purity) was immediately added to it. Then, the contents were made up to the mark with distilled water and homogenized for 1 hour. Successive dilution of the mother solution gave rise to the working solutions.


### 4.2. Analysis of Nickel(II)

Nickel(II) was estimated spectrophotometrically using dimethylglyoxime (DMG, from Fischer Scientific International) solution [22]. Different working solutions containing less than 300 mg/L of nickel(II) were prepared by dilution. To each given nickel filtrate was added with 2 mL of 4% w/v potassium persulphate (K2S2O8, from Prolabo at 100% purity) and allowed to react for 10 minutes. Then, 4 mL of ammonia (4 M) (from Fischer Scientific International at 87% purity) and 0.5 mL of DMG (10% w/v) were also added. The absorbance of the mixture was measured after 30 minutes using a UV-visible spectrophotometer (JENWAY) at 465 nm.


### 4.3. Equilibrium Studies Using Batch Method

Kinetic and equilibrium studies of nickel(II) adsorption were carried out in a thermostatic batch reactor maintained at 27°C. In each measurement, 0.1 g of adsorbent was introduced into a 20 mL beaker containing nickel(II) solution which previously underwent pH adjustment by addition of 0.1 N solution of HCl or NaOH. The effect of the adsorbent dose was carried out at pH 4 with an initial metal ion concentration of 240 mg/L and varying the adsorbent dose from 0.1 g to 0.6 g. The effect of pH on the adsorption of nickel(II) ions was investigated by varying the pH of the equilibrium solution from 2 to 8 (using Hannah Instruments). In kinetic studies, the different mixtures were stirred within a time interval between 5 and 60 minutes for equilibrium time determination. After filtration of trial solutions with Whatman filter paper No. 4, the residual nickel(II) ion concentration in each sample was determined by UV-visible spectrophotometer (JENWAY) at 465 nm wavelength. The sorption capacity of samples at equilibrium (Qe) and the percentage removal (%R) are given by (7) and (8).(7)Qe=C0−CfVm,(8)%R=C0−Cf×100C0,where v is the volume of nickel, m is the sample mass, and C0 and Cf are the initial and final concentrations of nickel, respectively.


### 4.4. Nonlinear Regression Analysis

In this study, nonlinear regression was applied using the Microsoft Excel Solver function and using Origin Pro 9, 64 bit for fitting the curve. The best fit for experimental data was determined from the regression coefficient (R2) and residual root mean square error (RMSE). More detailed definitions of the error functions and statistical comparison values are presented in Table 1.Table 1
Error functions and their equations.
Error functionAbbreviationFormulaEquation numberReferencesResidual root mean square errorRMSE1/n−2∑i=1NQe,exp−Qe,cal2(9)[23]Coefficient of regressionR2∑i=1NQe,cal−Qeexp2/∑i=1NQe,cal−Qeexp2+Qe,cal−Qeexp2(10)[24]


## 4.1. Preparation and Determination of Nickel(II) Ions

A standard 2000 mg/L mother solution of nickel(II) was prepared by dissolving 2.1 g of AR grade nickel chloride hexahydrate (NiCl2.6H2O) of molar mass (M = 237.71 g/mol at 98.6% purity from Fischer Scientific International) inside a 250 mL volumetric flask. 5 mL of a 1% HNO3 (from Merck at 65% purity) was immediately added to it. Then, the contents were made up to the mark with distilled water and homogenized for 1 hour. Successive dilution of the mother solution gave rise to the working solutions.


## 4.2. Analysis of Nickel(II)

Nickel(II) was estimated spectrophotometrically using dimethylglyoxime (DMG, from Fischer Scientific International) solution [22]. Different working solutions containing less than 300 mg/L of nickel(II) were prepared by dilution. To each given nickel filtrate was added with 2 mL of 4% w/v potassium persulphate (K2S2O8, from Prolabo at 100% purity) and allowed to react for 10 minutes. Then, 4 mL of ammonia (4 M) (from Fischer Scientific International at 87% purity) and 0.5 mL of DMG (10% w/v) were also added. The absorbance of the mixture was measured after 30 minutes using a UV-visible spectrophotometer (JENWAY) at 465 nm.


## 4.3. Equilibrium Studies Using Batch Method

Kinetic and equilibrium studies of nickel(II) adsorption were carried out in a thermostatic batch reactor maintained at 27°C. In each measurement, 0.1 g of adsorbent was introduced into a 20 mL beaker containing nickel(II) solution which previously underwent pH adjustment by addition of 0.1 N solution of HCl or NaOH. The effect of the adsorbent dose was carried out at pH 4 with an initial metal ion concentration of 240 mg/L and varying the adsorbent dose from 0.1 g to 0.6 g. The effect of pH on the adsorption of nickel(II) ions was investigated by varying the pH of the equilibrium solution from 2 to 8 (using Hannah Instruments). In kinetic studies, the different mixtures were stirred within a time interval between 5 and 60 minutes for equilibrium time determination. After filtration of trial solutions with Whatman filter paper No. 4, the residual nickel(II) ion concentration in each sample was determined by UV-visible spectrophotometer (JENWAY) at 465 nm wavelength. The sorption capacity of samples at equilibrium (Qe) and the percentage removal (%R) are given by (7) and (8).(7)Qe=C0−CfVm,(8)%R=C0−Cf×100C0,where v is the volume of nickel, m is the sample mass, and C0 and Cf are the initial and final concentrations of nickel, respectively.


## 4.4. Nonlinear Regression Analysis

In this study, nonlinear regression was applied using the Microsoft Excel Solver function and using Origin Pro 9, 64 bit for fitting the curve. The best fit for experimental data was determined from the regression coefficient (R2) and residual root mean square error (RMSE). More detailed definitions of the error functions and statistical comparison values are presented in Table 1.Table 1
Error functions and their equations.
Error functionAbbreviationFormulaEquation numberReferencesResidual root mean square errorRMSE1/n−2∑i=1NQe,exp−Qe,cal2(9)[23]Coefficient of regressionR2∑i=1NQe,cal−Qeexp2/∑i=1NQe,cal−Qeexp2+Qe,cal−Qeexp2(10)[24]


## 5. Results and Discussion

### 5.1. Proximate Analysis

The results of the proximate analysis for the determination of macronutrients of cassava peelings are presented in Figure2 which shows 1% moisture content, 8% ash content, 13% volatile matter, and 78% of fixed carbon. It can be seen here that the materials are good precursors for the production of activated carbon [16].Figure 2
The proximate analysis giving the composition of the peelings of cassava tubers.


### 5.2. Elemental Analyses

The results of the elemental composition of investigated precursors and activated carbons carbonized at 400°C are given in Table2. Results show higher proportions of carbon and oxygen in the precursor (RM) than of hydrogen and nitrogen, confirming the organic and acidic nature of the materials. We also observe a considerable reduction in oxygen content and a slight increase in nitrogen content after the activation/calcination process, thus confirming the acidic nature of the precursor and the acid-base nature of the different carbon materials. The activated carbons obtained are very rich in acid-base surface functions. Carbon content increases as one passes from precursor to the different activated carbons prepared (ACPH, ACPA, and NIC). This means that calcination/carbonization of precursor facilitates the liberation of volatile entities such as hydrogen [25].Table 2
Elemental composition (%) of ACPH, ACPA, NIC, and RM.
Sample%N%C%H%OACPH2.6968.902.7626.13ACPA2.6464.522.1130.73NIC2.6966.602.4828.23RM1.2340.575.9952.21


### 5.3. Effect of Calcination Temperature on the Iodine Number

Figure3 shows that as temperature increased from 300°C to 400°C, the iodine number increased as well for ACPA, ACPH, and NIC samples. The main reason for this increase is the development of micropores on the adsorbent surface, thus increasing their adsorption capacity [26]. But beyond 400°C, the iodine number decreased as a result of the destruction of formed micropores and consequently a sharp decrease in their adsorption capacity [26]. It can be observed from these results that iodine number reached its maximum value at 400°C for ACPA, ACPH, and NIC with optimal iodine numbers of 523.46, 618.64, and 492.17 mg/g, respectively, indicative of microporous activated carbon according to ASTMD 2866-94 norms [17].Figure 3
Effect of calcination temperature on the iodine number.


### 5.4. Characterization of Adsorbents

#### 5.4.1. Determination of Oxygen Containing Functional Groups

Boehm titration was used to determine oxygenated surface groups [19]. Table 3 shows results of quantitative surface chemical analysis (amount of acidic and basic functional groups on ACPH, ACPA, NIC, and RM). These results show that the three activated carbon samples contain more basic than acidic (carboxylic and phenolic groups) functions. On the contrary, precursor samples showed more acidic (carboxylic and phenolic groups) than basic due to a decrease in the number of lactonic functions. This observation is in conformity with the pHPZC values which are proportional to the acidic and basic functions.Table 3
Surface functional groups of precursors and activated carbon from peelings of cassava tubers.
MaterialsCarboxylic (meq g−1)Phenolic (meq g−1)Lactonic (meq g−1)Total acid (meq g−1)Total basic (meq g−1)ACPH1.231.750.002.983.18ACPA2.650.110.002.763.17NIC1.341.360.002.703.17RM2.491.560.004.053.07


#### 5.4.2. Determination of pH at Zero-Point Charge (pHzpc)

pHzpc values indicate the acidic or basic character of samples and their net surface charges. Knowledge of pHzpc helps to predict the type of interactions that take place during the adsorption process. The pHzpc obtained for each activated carbon and for the peelings of cassava tubers (Figure4) is coherent with the quantification of the surface functional groups obtained via the Boehm method. According to Figure 4, the values of the pHzpc obtained are 8.0, 7.8, 7.3, and 6.3 for ACPH, ACPA, NIC, and RM adsorbents, respectively. Hence, in these experiments and for pH < pHzpc, samples will have their surfaces positively charged while those for which pH > pHzpc will have their surfaces negatively charged.Figure 4
Determination of pHzpc of different adsorbents.


#### 5.4.3. Fourier-Transform Infrared Spectroscopy (FTIR)

The results of FTIR analysis for the peelings of cassava tuber samples are depicted in Figure5. After activation of the peelings of cassava tubers powder, a comparison of the different spectra of the products obtained with that of the biomass was made in order to measure the effects of activation and the modification brought to the surface of the raw material. Figure 5 illustrates these different spectra. The superimposed FTIR spectra of the activated carbons (ACPH, ACPA, NIC, and RM) with the peelings of cassava tubers are shown in Figure 5. Table 4 summarizes the wavenumbers and assignments of the main bands observed in Figure 5.Figure 5
FT-IR spectra of the peelings of cassava tubers and their activated carbon.Table 4
Wavenumbers and attributions of the principal bands in the FTIR spectra of peelings of cassava tubers and activated carbons (ACPH, ACPA, NIC, and RM).
Wavenumber (cm−1)Functional groups and chromophoresACPHACPANICRM3400–3200O-H stretching vibration, characteristic peak of carboxyls, phenols, alcohols, or water absorbed∗∗∗∗3000–2800C-H aliphatic stretching vibration of aromatic methoxyl groups or in methyl and methylene side chains∗1720.35C=O stretching vibration of the carbonyl group in ketones, aldehydes, lactones, or the carboxyls groups∗1628.14C=C stretching variation in aromatic rings enhanced by polar functional groups∗∗∗∗1008.11C-O stretching vibration in carboxylic acids, alcohol, phenol, ether or the P=O bond in phosphate esters, or still O-C bond in P-O-C linkage and P=OOH [27]∗900–400=C-H bending vibrations of the aromatic polynuclear systems∗From the above results obtained from spectral analysis of the activated carbons (ACPH, ACPA, and (NIC), we observe a broad absorption band centered around 3284.84 cm−1 corresponding to O-H bond stretching characteristic of phenol, alcohol, or water. We note that this broadband decreases in intensity during the calcination. This is due to the fact that the surface of the material is degraded during the calcination process and thereby causing the departure of the C, H, and O atoms in the form of gases (CO2, CH4, and CO) and the disappearance of the water molecules [28]. This is further justified by the fact that phosphoric acid and potassium hydroxide being dehydrating agents would react with the raw material, and this will cause the departure of water molecules contained at the surface. We also note the disappearance of the band of asymmetrical (C-H) stretching vibration at 2925.80 cm−1 for the three activated carbons (ACPH, ACPA, and NIC). This indicates that activation significantly destroys part of the aliphatic and aromatic C-H bond [29]. The bands located around 1628.14 cm−1 are attributed to the aromatic carbon–carbon double bonds (C=C). After activation, a significant reduction in absorption peak was observed for a series of complex bands around 1008.11 cm−1 for the precursor, which includes C-O stretching vibration in carboxylic acids, alcohol, phenol, ether, or the P=O bond in phosphate esters, or still O-C bond in P-O-C linkage and P=OOH [27]. From 900 to 400 cm−1, there are bands characteristic of aromatic rings.


#### 5.4.4. Scanning Electron Microscopy (SEM)

SEM micrographs of the precursor (Figure6(a)), the untreated activated carbons (Figure 6(b)), the treated activated carbons by H3PO4 (Figure 6(c)), and KOH (Figure 6(d)), respectively, are presented in Figure 6. We notice here that the precursor (a) has a surface with no visible pores before carbonization. After carbonization of precursor (Figures 6(b)–6(d)), we observe porous structures and rough textures of the surface. These pores resulted from the evaporation of the chemical reagent (H3PO4 and KOH) during carbonization, leaving the space previously occupied by the reagents.Figure 6
Morphology of samples: (a) precursor-RM, (b) NIC, (c) ACPA, and (d) ACPH.
(a)(b)(c)(d)


## 5.1. Proximate Analysis

The results of the proximate analysis for the determination of macronutrients of cassava peelings are presented in Figure2 which shows 1% moisture content, 8% ash content, 13% volatile matter, and 78% of fixed carbon. It can be seen here that the materials are good precursors for the production of activated carbon [16].Figure 2
The proximate analysis giving the composition of the peelings of cassava tubers.


## 5.2. Elemental Analyses

The results of the elemental composition of investigated precursors and activated carbons carbonized at 400°C are given in Table2. Results show higher proportions of carbon and oxygen in the precursor (RM) than of hydrogen and nitrogen, confirming the organic and acidic nature of the materials. We also observe a considerable reduction in oxygen content and a slight increase in nitrogen content after the activation/calcination process, thus confirming the acidic nature of the precursor and the acid-base nature of the different carbon materials. The activated carbons obtained are very rich in acid-base surface functions. Carbon content increases as one passes from precursor to the different activated carbons prepared (ACPH, ACPA, and NIC). This means that calcination/carbonization of precursor facilitates the liberation of volatile entities such as hydrogen [25].Table 2
Elemental composition (%) of ACPH, ACPA, NIC, and RM.
Sample%N%C%H%OACPH2.6968.902.7626.13ACPA2.6464.522.1130.73NIC2.6966.602.4828.23RM1.2340.575.9952.21


## 5.3. Effect of Calcination Temperature on the Iodine Number

Figure3 shows that as temperature increased from 300°C to 400°C, the iodine number increased as well for ACPA, ACPH, and NIC samples. The main reason for this increase is the development of micropores on the adsorbent surface, thus increasing their adsorption capacity [26]. But beyond 400°C, the iodine number decreased as a result of the destruction of formed micropores and consequently a sharp decrease in their adsorption capacity [26]. It can be observed from these results that iodine number reached its maximum value at 400°C for ACPA, ACPH, and NIC with optimal iodine numbers of 523.46, 618.64, and 492.17 mg/g, respectively, indicative of microporous activated carbon according to ASTMD 2866-94 norms [17].Figure 3
Effect of calcination temperature on the iodine number.


## 5.4. Characterization of Adsorbents

### 5.4.1. Determination of Oxygen Containing Functional Groups

Boehm titration was used to determine oxygenated surface groups [19]. Table 3 shows results of quantitative surface chemical analysis (amount of acidic and basic functional groups on ACPH, ACPA, NIC, and RM). These results show that the three activated carbon samples contain more basic than acidic (carboxylic and phenolic groups) functions. On the contrary, precursor samples showed more acidic (carboxylic and phenolic groups) than basic due to a decrease in the number of lactonic functions. This observation is in conformity with the pHPZC values which are proportional to the acidic and basic functions.Table 3
Surface functional groups of precursors and activated carbon from peelings of cassava tubers.
MaterialsCarboxylic (meq g−1)Phenolic (meq g−1)Lactonic (meq g−1)Total acid (meq g−1)Total basic (meq g−1)ACPH1.231.750.002.983.18ACPA2.650.110.002.763.17NIC1.341.360.002.703.17RM2.491.560.004.053.07


### 5.4.2. Determination of pH at Zero-Point Charge (pHzpc)

pHzpc values indicate the acidic or basic character of samples and their net surface charges. Knowledge of pHzpc helps to predict the type of interactions that take place during the adsorption process. The pHzpc obtained for each activated carbon and for the peelings of cassava tubers (Figure4) is coherent with the quantification of the surface functional groups obtained via the Boehm method. According to Figure 4, the values of the pHzpc obtained are 8.0, 7.8, 7.3, and 6.3 for ACPH, ACPA, NIC, and RM adsorbents, respectively. Hence, in these experiments and for pH < pHzpc, samples will have their surfaces positively charged while those for which pH > pHzpc will have their surfaces negatively charged.Figure 4
Determination of pHzpc of different adsorbents.


### 5.4.3. Fourier-Transform Infrared Spectroscopy (FTIR)

The results of FTIR analysis for the peelings of cassava tuber samples are depicted in Figure5. After activation of the peelings of cassava tubers powder, a comparison of the different spectra of the products obtained with that of the biomass was made in order to measure the effects of activation and the modification brought to the surface of the raw material. Figure 5 illustrates these different spectra. The superimposed FTIR spectra of the activated carbons (ACPH, ACPA, NIC, and RM) with the peelings of cassava tubers are shown in Figure 5. Table 4 summarizes the wavenumbers and assignments of the main bands observed in Figure 5.Figure 5
FT-IR spectra of the peelings of cassava tubers and their activated carbon.Table 4
Wavenumbers and attributions of the principal bands in the FTIR spectra of peelings of cassava tubers and activated carbons (ACPH, ACPA, NIC, and RM).
Wavenumber (cm−1)Functional groups and chromophoresACPHACPANICRM3400–3200O-H stretching vibration, characteristic peak of carboxyls, phenols, alcohols, or water absorbed∗∗∗∗3000–2800C-H aliphatic stretching vibration of aromatic methoxyl groups or in methyl and methylene side chains∗1720.35C=O stretching vibration of the carbonyl group in ketones, aldehydes, lactones, or the carboxyls groups∗1628.14C=C stretching variation in aromatic rings enhanced by polar functional groups∗∗∗∗1008.11C-O stretching vibration in carboxylic acids, alcohol, phenol, ether or the P=O bond in phosphate esters, or still O-C bond in P-O-C linkage and P=OOH [27]∗900–400=C-H bending vibrations of the aromatic polynuclear systems∗From the above results obtained from spectral analysis of the activated carbons (ACPH, ACPA, and (NIC), we observe a broad absorption band centered around 3284.84 cm−1 corresponding to O-H bond stretching characteristic of phenol, alcohol, or water. We note that this broadband decreases in intensity during the calcination. This is due to the fact that the surface of the material is degraded during the calcination process and thereby causing the departure of the C, H, and O atoms in the form of gases (CO2, CH4, and CO) and the disappearance of the water molecules [28]. This is further justified by the fact that phosphoric acid and potassium hydroxide being dehydrating agents would react with the raw material, and this will cause the departure of water molecules contained at the surface. We also note the disappearance of the band of asymmetrical (C-H) stretching vibration at 2925.80 cm−1 for the three activated carbons (ACPH, ACPA, and NIC). This indicates that activation significantly destroys part of the aliphatic and aromatic C-H bond [29]. The bands located around 1628.14 cm−1 are attributed to the aromatic carbon–carbon double bonds (C=C). After activation, a significant reduction in absorption peak was observed for a series of complex bands around 1008.11 cm−1 for the precursor, which includes C-O stretching vibration in carboxylic acids, alcohol, phenol, ether, or the P=O bond in phosphate esters, or still O-C bond in P-O-C linkage and P=OOH [27]. From 900 to 400 cm−1, there are bands characteristic of aromatic rings.


### 5.4.4. Scanning Electron Microscopy (SEM)

SEM micrographs of the precursor (Figure6(a)), the untreated activated carbons (Figure 6(b)), the treated activated carbons by H3PO4 (Figure 6(c)), and KOH (Figure 6(d)), respectively, are presented in Figure 6. We notice here that the precursor (a) has a surface with no visible pores before carbonization. After carbonization of precursor (Figures 6(b)–6(d)), we observe porous structures and rough textures of the surface. These pores resulted from the evaporation of the chemical reagent (H3PO4 and KOH) during carbonization, leaving the space previously occupied by the reagents.Figure 6
Morphology of samples: (a) precursor-RM, (b) NIC, (c) ACPA, and (d) ACPH.
(a)(b)(c)(d)


## 5.4.1. Determination of Oxygen Containing Functional Groups

Boehm titration was used to determine oxygenated surface groups [19]. Table 3 shows results of quantitative surface chemical analysis (amount of acidic and basic functional groups on ACPH, ACPA, NIC, and RM). These results show that the three activated carbon samples contain more basic than acidic (carboxylic and phenolic groups) functions. On the contrary, precursor samples showed more acidic (carboxylic and phenolic groups) than basic due to a decrease in the number of lactonic functions. This observation is in conformity with the pHPZC values which are proportional to the acidic and basic functions.Table 3
Surface functional groups of precursors and activated carbon from peelings of cassava tubers.
MaterialsCarboxylic (meq g−1)Phenolic (meq g−1)Lactonic (meq g−1)Total acid (meq g−1)Total basic (meq g−1)ACPH1.231.750.002.983.18ACPA2.650.110.002.763.17NIC1.341.360.002.703.17RM2.491.560.004.053.07


## 5.4.2. Determination of pH at Zero-Point Charge (pHzpc)

pHzpc values indicate the acidic or basic character of samples and their net surface charges. Knowledge of pHzpc helps to predict the type of interactions that take place during the adsorption process. The pHzpc obtained for each activated carbon and for the peelings of cassava tubers (Figure4) is coherent with the quantification of the surface functional groups obtained via the Boehm method. According to Figure 4, the values of the pHzpc obtained are 8.0, 7.8, 7.3, and 6.3 for ACPH, ACPA, NIC, and RM adsorbents, respectively. Hence, in these experiments and for pH < pHzpc, samples will have their surfaces positively charged while those for which pH > pHzpc will have their surfaces negatively charged.Figure 4
Determination of pHzpc of different adsorbents.


## 5.4.3. Fourier-Transform Infrared Spectroscopy (FTIR)

The results of FTIR analysis for the peelings of cassava tuber samples are depicted in Figure5. After activation of the peelings of cassava tubers powder, a comparison of the different spectra of the products obtained with that of the biomass was made in order to measure the effects of activation and the modification brought to the surface of the raw material. Figure 5 illustrates these different spectra. The superimposed FTIR spectra of the activated carbons (ACPH, ACPA, NIC, and RM) with the peelings of cassava tubers are shown in Figure 5. Table 4 summarizes the wavenumbers and assignments of the main bands observed in Figure 5.Figure 5
FT-IR spectra of the peelings of cassava tubers and their activated carbon.Table 4
Wavenumbers and attributions of the principal bands in the FTIR spectra of peelings of cassava tubers and activated carbons (ACPH, ACPA, NIC, and RM).
Wavenumber (cm−1)Functional groups and chromophoresACPHACPANICRM3400–3200O-H stretching vibration, characteristic peak of carboxyls, phenols, alcohols, or water absorbed∗∗∗∗3000–2800C-H aliphatic stretching vibration of aromatic methoxyl groups or in methyl and methylene side chains∗1720.35C=O stretching vibration of the carbonyl group in ketones, aldehydes, lactones, or the carboxyls groups∗1628.14C=C stretching variation in aromatic rings enhanced by polar functional groups∗∗∗∗1008.11C-O stretching vibration in carboxylic acids, alcohol, phenol, ether or the P=O bond in phosphate esters, or still O-C bond in P-O-C linkage and P=OOH [27]∗900–400=C-H bending vibrations of the aromatic polynuclear systems∗From the above results obtained from spectral analysis of the activated carbons (ACPH, ACPA, and (NIC), we observe a broad absorption band centered around 3284.84 cm−1 corresponding to O-H bond stretching characteristic of phenol, alcohol, or water. We note that this broadband decreases in intensity during the calcination. This is due to the fact that the surface of the material is degraded during the calcination process and thereby causing the departure of the C, H, and O atoms in the form of gases (CO2, CH4, and CO) and the disappearance of the water molecules [28]. This is further justified by the fact that phosphoric acid and potassium hydroxide being dehydrating agents would react with the raw material, and this will cause the departure of water molecules contained at the surface. We also note the disappearance of the band of asymmetrical (C-H) stretching vibration at 2925.80 cm−1 for the three activated carbons (ACPH, ACPA, and NIC). This indicates that activation significantly destroys part of the aliphatic and aromatic C-H bond [29]. The bands located around 1628.14 cm−1 are attributed to the aromatic carbon–carbon double bonds (C=C). After activation, a significant reduction in absorption peak was observed for a series of complex bands around 1008.11 cm−1 for the precursor, which includes C-O stretching vibration in carboxylic acids, alcohol, phenol, ether, or the P=O bond in phosphate esters, or still O-C bond in P-O-C linkage and P=OOH [27]. From 900 to 400 cm−1, there are bands characteristic of aromatic rings.


## 5.4.4. Scanning Electron Microscopy (SEM)

SEM micrographs of the precursor (Figure6(a)), the untreated activated carbons (Figure 6(b)), the treated activated carbons by H3PO4 (Figure 6(c)), and KOH (Figure 6(d)), respectively, are presented in Figure 6. We notice here that the precursor (a) has a surface with no visible pores before carbonization. After carbonization of precursor (Figures 6(b)–6(d)), we observe porous structures and rough textures of the surface. These pores resulted from the evaporation of the chemical reagent (H3PO4 and KOH) during carbonization, leaving the space previously occupied by the reagents.Figure 6
Morphology of samples: (a) precursor-RM, (b) NIC, (c) ACPA, and (d) ACPH.
(a)(b)(c)(d)


## 6. Adsorption Studies

### 6.1. Effect of Contact Time

In order to determine the effect of contact time on the extent of adsorption, 0.1 g of the adsorbent was stirred with a 20 mL solution of nickel(II) ions of initial concentration of 200 mg/L for a time interval of 5–60 minutes for ACPH, ACPA, NIC, and RM. The experimental results obtained for the adsorption of nickel(II) ions during various contact times are illustrated in Figure7. From the results, it can be observed that the adsorbed quantity of nickel(II) ions increased rapidly and attained maximum values at 51.81 mg/g for ACPH, 50.86 mg/g for ACPA, 47.74 mg/g for NIC, and 41.41 mg/g for RM after an equilibrium time of 40 minutes for the four samples. This can be explained by the fact that initially there are available free adsorption sites on the surface of the adsorbents for adsorption. Beyond this stage, one observes the progressive surface saturation of various materials studied. This saturation is due to the total occupation of the active sites at the surface of the adsorbents [18]. Results show a higher adsorption capacity of prepared activated carbon samples compared to the raw material.Figure 7
Effect of contact time on nickel(II) adsorption for ACPH, ACPA, NIC, and RM (volume = 20 mL, Co=200 mg/L, pH = 4, adsorbent dose = 0.1 g, stirring rate 150 rpm).


### 6.2. Effect of the Initial pH

Figure8 represents the effect of the initial pH of the solution on the adsorption of nickel(II) ions onto ACPH, ACPA, NIC, and RM using 200 mg/L initial nickel(II) concentration and 0.1 g of adsorbent. pH was varied between 2 and 8 within 40 minutes of contact time. Results show that adsorbed quantities of the nickel(II) ions increase gradually until maximum removal is attained at pH = 4 (51.81 mg/g for ACPH, 51.86 mg/g for ACPA, 48.85 mg/g for NIC, and 27.93 mg/g for RM) and decrease thereafter. At lower pH values, nickel(II) removal is inhibited because of the competition between hydrogen and nickel(II) ions for sorption sites [30]. The decrease in the adsorbed quantity beyond pH = 4 is due to the formation of a nickel hydroxide precipitate (Ni(OH)2) in agreement with the work of [7].Figure 8
Effect of pH on nickel(II) adsorption for ACPH, ACPA, NIC, and RM (volume = 20 mL, teq = 40 min, Co=200 mg/L, adsorbent dose = 0.1 g, stirring rate 150 rpm).The mechanism of the adsorption of Ni(II) ions from the aqueous solution by the activated carbons has been explained in terms of the surface chemistry of the carbons and the pH of the solution. In aqueous solutions, Ni(II) may exist as Ni2+, Ni(OH)+, Ni(OH)−4, and Ni(OH)2 (as a precipitate): the acidic carbon-oxygen surface group on ionization produce H+ and the negatively charged surface sites. However, the presence of nickel ions in the solution and the concentration of the negative site or the negative charge on the carbon surface are determined by the pH of the solution [7, 31].At a low pH value (pH below pHzpc), the carbon surface has a positive charge because of low ionization of the surface groups and excessive protonation of the surface and creates repulsive interactions with the nickel cations leading to low adsorption. But at higher pH values (pH > pHzpc), the adsorption of Ni(II) increases as a result of a high degree of ionization of the surface acidic groups and the dominance of nickel cation in the solution phase that enhances the attractive interactions. At very high pH values, the dominant nickel ions in the solution are anionic complexes that produce repulsive interactions and decrease the adsorption [7, 31].


### 6.3. Effect of Adsorbent Dose

The influence of the adsorbent dose on the removal of nickel(II) ions from an aqueous solution was studied by varying its concentration from 0.1 to 0.6 g. Figure9 represents the influence of adsorbent dose on the adsorption of nickel(II) ions onto ACPH, ACPA, NIC, and RM using 200 mg/L initial nickel(II) concentration at pH = 4 for a contact time of 40 minutes. The adsorbed quantity decreased with increasing adsorbent masses. This is due to the fact that an increase in adsorbent dose leads to an agglomeration of particles which prevent the nickel(II) ions to approach the sites of adsorption and consequently a reduction in the quantity adsorbed per unit mass of adsorbent [32]. This can still be explained by the fact that during the process of adsorption, certain adsorption sites remain unsaturated [18].Figure 9
Effect of adsorbent mass on nickel(II) adsorption for ACPH, ACPA, NIC, and RM (v = 20 mL, t = 40 min, Co=200 mg/L, pH = 4, stirring velocity 150 rpm).


### 6.4. Effect of the Initial Concentration of Nickel(II)

Studies were performed with initial nickel(II) concentrations ranging from 110 to 210 mg/L. 0.1 g of adsorbent and pH = 4 was used for the adsorption experiments. The experimental results of the effect of the initial nickel(II) concentration on the adsorption capacity are presented in Figure10. It is obvious from this figure that nickel(II) adsorption increases with an increase in initial nickel(II) concentration because an increase in the initial concentration of nickel(II) ions brings about an increase in mass transfer from the aqueous phase to the solid phase. This can still be explained by the increasing driving force of the metal ions toward the active sites on the adsorbents [33].Figure 10
Effect of initial concentration on nickel(II) adsorption for ACPH, ACPA, NIC, and RM (v = 20 mL, t = 40 min, pH = 4, adsorbent dose = 0.1 g, stirring velocity 150 rpm).


## 6.1. Effect of Contact Time

In order to determine the effect of contact time on the extent of adsorption, 0.1 g of the adsorbent was stirred with a 20 mL solution of nickel(II) ions of initial concentration of 200 mg/L for a time interval of 5–60 minutes for ACPH, ACPA, NIC, and RM. The experimental results obtained for the adsorption of nickel(II) ions during various contact times are illustrated in Figure7. From the results, it can be observed that the adsorbed quantity of nickel(II) ions increased rapidly and attained maximum values at 51.81 mg/g for ACPH, 50.86 mg/g for ACPA, 47.74 mg/g for NIC, and 41.41 mg/g for RM after an equilibrium time of 40 minutes for the four samples. This can be explained by the fact that initially there are available free adsorption sites on the surface of the adsorbents for adsorption. Beyond this stage, one observes the progressive surface saturation of various materials studied. This saturation is due to the total occupation of the active sites at the surface of the adsorbents [18]. Results show a higher adsorption capacity of prepared activated carbon samples compared to the raw material.Figure 7
Effect of contact time on nickel(II) adsorption for ACPH, ACPA, NIC, and RM (volume = 20 mL, Co=200 mg/L, pH = 4, adsorbent dose = 0.1 g, stirring rate 150 rpm).


## 6.2. Effect of the Initial pH

Figure8 represents the effect of the initial pH of the solution on the adsorption of nickel(II) ions onto ACPH, ACPA, NIC, and RM using 200 mg/L initial nickel(II) concentration and 0.1 g of adsorbent. pH was varied between 2 and 8 within 40 minutes of contact time. Results show that adsorbed quantities of the nickel(II) ions increase gradually until maximum removal is attained at pH = 4 (51.81 mg/g for ACPH, 51.86 mg/g for ACPA, 48.85 mg/g for NIC, and 27.93 mg/g for RM) and decrease thereafter. At lower pH values, nickel(II) removal is inhibited because of the competition between hydrogen and nickel(II) ions for sorption sites [30]. The decrease in the adsorbed quantity beyond pH = 4 is due to the formation of a nickel hydroxide precipitate (Ni(OH)2) in agreement with the work of [7].Figure 8
Effect of pH on nickel(II) adsorption for ACPH, ACPA, NIC, and RM (volume = 20 mL, teq = 40 min, Co=200 mg/L, adsorbent dose = 0.1 g, stirring rate 150 rpm).The mechanism of the adsorption of Ni(II) ions from the aqueous solution by the activated carbons has been explained in terms of the surface chemistry of the carbons and the pH of the solution. In aqueous solutions, Ni(II) may exist as Ni2+, Ni(OH)+, Ni(OH)−4, and Ni(OH)2 (as a precipitate): the acidic carbon-oxygen surface group on ionization produce H+ and the negatively charged surface sites. However, the presence of nickel ions in the solution and the concentration of the negative site or the negative charge on the carbon surface are determined by the pH of the solution [7, 31].At a low pH value (pH below pHzpc), the carbon surface has a positive charge because of low ionization of the surface groups and excessive protonation of the surface and creates repulsive interactions with the nickel cations leading to low adsorption. But at higher pH values (pH > pHzpc), the adsorption of Ni(II) increases as a result of a high degree of ionization of the surface acidic groups and the dominance of nickel cation in the solution phase that enhances the attractive interactions. At very high pH values, the dominant nickel ions in the solution are anionic complexes that produce repulsive interactions and decrease the adsorption [7, 31].


## 6.3. Effect of Adsorbent Dose

The influence of the adsorbent dose on the removal of nickel(II) ions from an aqueous solution was studied by varying its concentration from 0.1 to 0.6 g. Figure9 represents the influence of adsorbent dose on the adsorption of nickel(II) ions onto ACPH, ACPA, NIC, and RM using 200 mg/L initial nickel(II) concentration at pH = 4 for a contact time of 40 minutes. The adsorbed quantity decreased with increasing adsorbent masses. This is due to the fact that an increase in adsorbent dose leads to an agglomeration of particles which prevent the nickel(II) ions to approach the sites of adsorption and consequently a reduction in the quantity adsorbed per unit mass of adsorbent [32]. This can still be explained by the fact that during the process of adsorption, certain adsorption sites remain unsaturated [18].Figure 9
Effect of adsorbent mass on nickel(II) adsorption for ACPH, ACPA, NIC, and RM (v = 20 mL, t = 40 min, Co=200 mg/L, pH = 4, stirring velocity 150 rpm).


## 6.4. Effect of the Initial Concentration of Nickel(II)

Studies were performed with initial nickel(II) concentrations ranging from 110 to 210 mg/L. 0.1 g of adsorbent and pH = 4 was used for the adsorption experiments. The experimental results of the effect of the initial nickel(II) concentration on the adsorption capacity are presented in Figure10. It is obvious from this figure that nickel(II) adsorption increases with an increase in initial nickel(II) concentration because an increase in the initial concentration of nickel(II) ions brings about an increase in mass transfer from the aqueous phase to the solid phase. This can still be explained by the increasing driving force of the metal ions toward the active sites on the adsorbents [33].Figure 10
Effect of initial concentration on nickel(II) adsorption for ACPH, ACPA, NIC, and RM (v = 20 mL, t = 40 min, pH = 4, adsorbent dose = 0.1 g, stirring velocity 150 rpm).


## 7. Adsorption Isotherms

Adsorbate distribution between liquid and solid phases, solute-solution interaction, and knowledge of the adsorption capacity of adsorbent are described by isotherm models such as Langmuir, Freundlich, and Temkin models [34].


### 7.1. Langmuir Adsorption Isotherm

The Langmuir model assumes that metal ion uptake occurs on a homogeneous surface by monolayer adsorption without any interaction between adsorbed ions, uniform energies of adsorption are involved, and there is no transmigration of adsorbate in the plane of the surface [35]. The linearized Langmuir isotherm equation is expressed as(9)CeQe=1KLQm+CeQm,where KL is the Langmuir adsorption constant (L/mg) which is related to the maximum sorption capacity and the adsorption energy, Ce is the equilibrium concentration (mg/L), Qe is the quantity adsorbed per gram of adsorbent at equilibrium (mg/g), and Qm (mg/g) is an indicator of monolayer adsorption capacity. The efficiency of the Langmuir adsorption process is further assessed by (12):(10)RL=11+KLCo,where RL is a dimensionless constant referred to as separation factor, KL is the Langmuir constant related to the adsorption energy, and Co is the initial solute concentration (mg/L). If RL > 1, adsorption is said to be unfavorable, RL = 1 for linear adsorption, 0 < RL < 1 for favorable adsorption, and RL = 0 for irreversible adsorption [36].


### 7.2. Freundlich Adsorption Isotherm

The Freundlich model assumes that the uptake of metal ions occurs on a heterogeneous surface by monolayer adsorption [37]. The linearized relation (11) is given as follows:(11)LogQe=LogKF+1nLogCe,where Qe is the quantity of the solute adsorbed at equilibrium (adsorption density: mg of adsorbate per g of adsorbent). Ce is the concentration of adsorbate at equilibrium, 1/n (mg/L) is the adsorption intensity or the heterogeneity factor, and KF is the Freundlich constant related to the adsorption energy (mol2/kJ2). The last two constants are dependent on temperature and the nature of sorbent and sorbate.


### 7.3. Temkin Adsorption Isotherm

It is expressed by the following linear relationship between the amount adsorbedQe, and concentration of the solution at equilibrium Ce [38].(12)Qe=BTlnKT+lnCe,where KT (L/g) is the Temkin isotherm constant (equilibrium binding constant), BTJ/mol is a constant related to the heat of sorption, R is the gas constant (8.314 × 10−3 kJ/mol.K), and T is the absolute temperature (K). This model takes into account the heterogeneity of the surface [38]. In order to find the most appropriate model for the nickel(II) adsorption, the data was fitted to each isotherm model.Table5 presents the calculated parameters of the different models from which we can be seen that only the Langmuir isotherm model (R2 = 0.995, 0.982, 0.966, and 0.947 for ACPH, ACPA, NIC, and RM, respectively) best fits the experimental data. Adsorption of nickel(II) ions at 27°C according to the Langmuir model was found to be equal to 41.15, 47.39, 35.34, and 34.48 mg/g for ACPH, ACPA, NIC, and RM samples, respectively. The shape of the Langmuir isotherm was characterized by the dimensionless constant or separation term (RL). In this investigation, the equilibrium parameter was found to be in the range 0 < RL < 1 as shown in Table 5. This indicates that the sorption process was very favorable and that the adsorbent employed exhibits good adsorption potentials. From the Freundlich model, the values of the constants 1/n are lower than unity for all four materials and proved that adsorption is favorable in all cases studied. These values show that the activated carbon ACPA presents a better affinity for the nickel(II) ions compared to the three other materials. The Temkin model provided various heats of adsorption brought into play at the time of the various interactions. Taking into account the results presented in Table 5, one notes that these values of heats of adsorption (∆Q) of the four materials ACPH, ACPA, NIC, and RM are positive (∆Q > 0). This means that the adsorption process is exothermic (physical adsorption). The values of Temkin constants AT and BT as well as the correlation coefficients are listed in Table 5. Isotherms for Langmuir, Freundlich, and Temkin models are found in supplementary materials (Figures S1–S3, respectively).Table 5
Results of adsorption parameters for the different isotherm models.
ModelsConstantsACPHACPANICRMLangmuir isothermR20.9950.9820.9660.947Qmax (mg/g)41.1547.3935.3434.48KL (L/mg)1.7480.0950.0670.053RL0.0030.0500.0700.086RMSE5.9071.4121.6541.917Freundlich isothermR20.6320.9880.9330.8911/n0.1420.3830.2930.297K (L/g)27.569.6458.5607.414RMSE3.9640.6421.2421.838Temkin isothermR20.7070.9690.9030.853KT (L/g)3.4310.9430.9810.876∆Q (KJ/mol)22.6511.8612.5912.62RMSE38.6934.7029.2927.92


## 7.1. Langmuir Adsorption Isotherm

The Langmuir model assumes that metal ion uptake occurs on a homogeneous surface by monolayer adsorption without any interaction between adsorbed ions, uniform energies of adsorption are involved, and there is no transmigration of adsorbate in the plane of the surface [35]. The linearized Langmuir isotherm equation is expressed as(9)CeQe=1KLQm+CeQm,where KL is the Langmuir adsorption constant (L/mg) which is related to the maximum sorption capacity and the adsorption energy, Ce is the equilibrium concentration (mg/L), Qe is the quantity adsorbed per gram of adsorbent at equilibrium (mg/g), and Qm (mg/g) is an indicator of monolayer adsorption capacity. The efficiency of the Langmuir adsorption process is further assessed by (12):(10)RL=11+KLCo,where RL is a dimensionless constant referred to as separation factor, KL is the Langmuir constant related to the adsorption energy, and Co is the initial solute concentration (mg/L). If RL > 1, adsorption is said to be unfavorable, RL = 1 for linear adsorption, 0 < RL < 1 for favorable adsorption, and RL = 0 for irreversible adsorption [36].


## 7.2. Freundlich Adsorption Isotherm

The Freundlich model assumes that the uptake of metal ions occurs on a heterogeneous surface by monolayer adsorption [37]. The linearized relation (11) is given as follows:(11)LogQe=LogKF+1nLogCe,where Qe is the quantity of the solute adsorbed at equilibrium (adsorption density: mg of adsorbate per g of adsorbent). Ce is the concentration of adsorbate at equilibrium, 1/n (mg/L) is the adsorption intensity or the heterogeneity factor, and KF is the Freundlich constant related to the adsorption energy (mol2/kJ2). The last two constants are dependent on temperature and the nature of sorbent and sorbate.


## 7.3. Temkin Adsorption Isotherm

It is expressed by the following linear relationship between the amount adsorbedQe, and concentration of the solution at equilibrium Ce [38].(12)Qe=BTlnKT+lnCe,where KT (L/g) is the Temkin isotherm constant (equilibrium binding constant), BTJ/mol is a constant related to the heat of sorption, R is the gas constant (8.314 × 10−3 kJ/mol.K), and T is the absolute temperature (K). This model takes into account the heterogeneity of the surface [38]. In order to find the most appropriate model for the nickel(II) adsorption, the data was fitted to each isotherm model.Table5 presents the calculated parameters of the different models from which we can be seen that only the Langmuir isotherm model (R2 = 0.995, 0.982, 0.966, and 0.947 for ACPH, ACPA, NIC, and RM, respectively) best fits the experimental data. Adsorption of nickel(II) ions at 27°C according to the Langmuir model was found to be equal to 41.15, 47.39, 35.34, and 34.48 mg/g for ACPH, ACPA, NIC, and RM samples, respectively. The shape of the Langmuir isotherm was characterized by the dimensionless constant or separation term (RL). In this investigation, the equilibrium parameter was found to be in the range 0 < RL < 1 as shown in Table 5. This indicates that the sorption process was very favorable and that the adsorbent employed exhibits good adsorption potentials. From the Freundlich model, the values of the constants 1/n are lower than unity for all four materials and proved that adsorption is favorable in all cases studied. These values show that the activated carbon ACPA presents a better affinity for the nickel(II) ions compared to the three other materials. The Temkin model provided various heats of adsorption brought into play at the time of the various interactions. Taking into account the results presented in Table 5, one notes that these values of heats of adsorption (∆Q) of the four materials ACPH, ACPA, NIC, and RM are positive (∆Q > 0). This means that the adsorption process is exothermic (physical adsorption). The values of Temkin constants AT and BT as well as the correlation coefficients are listed in Table 5. Isotherms for Langmuir, Freundlich, and Temkin models are found in supplementary materials (Figures S1–S3, respectively).Table 5
Results of adsorption parameters for the different isotherm models.
ModelsConstantsACPHACPANICRMLangmuir isothermR20.9950.9820.9660.947Qmax (mg/g)41.1547.3935.3434.48KL (L/mg)1.7480.0950.0670.053RL0.0030.0500.0700.086RMSE5.9071.4121.6541.917Freundlich isothermR20.6320.9880.9330.8911/n0.1420.3830.2930.297K (L/g)27.569.6458.5607.414RMSE3.9640.6421.2421.838Temkin isothermR20.7070.9690.9030.853KT (L/g)3.4310.9430.9810.876∆Q (KJ/mol)22.6511.8612.5912.62RMSE38.6934.7029.2927.92


## 8. Kinetics of Adsorption Process

Four kinetic models have been studied in describing the adsorption phenomenon of nickel(II) ions onto the four material samples studied herein: pseudo-first-order, pseudo-second-order, Elovich, and intraparticle diffusion models.


### 8.1. Pseudo-First-Order Model

Kinetic parameters for the adsorption process were studied for contact times ranging between 5 and 60 minutes by monitoring the quantity of nickel(II)) adsorbed as a function of time. The data were then regressed against the Lagergren equation (13), which represents a first-order kinetic equation [39].(13)LnQe−Qt=LnQe−Ktt,where k1 is the pseudo-first-order rate constant (min−1); Qe and Qt are the adsorption capacities at equilibrium and at a given time t and are expressed in (mg/g).


### 8.2. Pseudo-Second-Order Model

The linearized pseudo-second-order chemisorption kinetic model, equation (14) [40], has been appropriately utilized in experiments involving the adsorption of organics and heavy metals on activated carbon.(14)tQt=1K2Qe2+tQe,where K2 is the pseudo-second-order rate constant (mg.g−1.min−1).


### 8.3. Elovich Model

The linearized Elovich equation is generally expressed as(15)Qt=1βlnαβ+1βlnt,where α is the initial sorption rate (mg/g min) and β is the desorption rate constant (g/mg) during any one experiment. These constants will be obtained from the relation qt=flnt [41].


### 8.4. Intraparticle Diffusion Model

The rate constants of intraparticle diffusion (Kid) at different nickel(II) ion concentrations were determined using the following linearized equation:(16)qt=Kidt1/2+C,where qt is the amount of nickel(II) sorbed at time t. Kid is the intraparticle diffusion constant (mg.g−1.min−1/2). When intraparticle diffusion plays a significant role in controlling the kinetics of the sorption process, straight-line plots through the origin are obtained and their slopes give the rate constant, kid.The results of kinetic studies (Table6) indicate that the adsorption process follows the second-order rate equation for the four adsorbents with correlation coefficient R2 = 0.999 for ACPH, ACPA, NIC, and RM. This implies that chemisorption is the limiting step of the process [41]. By comparison, the values of Qe determined from this model, which stand as 52.63 mg/g for ACPH, 51.81 mg/g for ACPA, 50.00 mg/g for NIC, and 42.37 mg/g for RM, are very close to their experimental analogs. This confirms once more that ACPH and ACPA performed better in nickel(II) uptake compared to the two others. Initial rates show that the kinetics of adsorption of the pollutant is faster on the surface of ACPH than to ACPA, NIC, and RM. The half-life of the pseudo-second-order reaction shows that adsorption kinetics of the nickel(II) ions is faster on the surface of the NIC compared to the other materials (ACPH, ACPA, and RM).Table 6
Results of adsorption parameters for the different kinetic models.
ModelConstantsACPHACPANICRMPseudo-first-orderR20.9780.9850.9170.897K1 (min−1)0.0550.0620.0500.073Qe (mg/g)6.4598.04913.6216.11RMSE53.8950.7741.0229.23Pseudo-second-orderR20.9990.9990.9990.999h (mg/g. min)57.0648.9919.7017.11t1/2 (min)0.9211.0582.5352.475K2 (g/mg.min)0.0210.0180.0080.010Qe (mg/g)52.6351.8150.0042.37RMSE1.2421.2421.3801.175Intraparticle diffusionR20.9960.9720.9740.996Kid1 (min−1)1.0051.8573.6273.970C1 (mg/g)44.8840.4627.9219.81RMSE0.4842.3534.9316.063R20.6460.6270.6790.094Kid2 (min−1)0.4760.5091.4500.291C2 (mg/g)48.3647.0936.9638.32RMSE1.4181.9852.3195.652ElovichR20.9700.9770.9710.934β (g/mg)0.4750.3730.1980.197α (mg/g min)1.99×1099.24×1061.30×1033.28×102RMSE0.2940.3190.6831.057Results obtained from intraparticle diffusion model (obtained viaQt = f (t1/2)) are graphs with two linear portions each (Figure 11) indicative of an adsorption process taking place in two steps for all four adsorbents. The first portion is characterized by rapid or fast diffusion of nickel(II) from the external surface toward the macropores of the adsorbents also known as macroporous diffusion [42]. This portion is also characterized by higher diffusion constants, Kdi1. The second portion corresponds to very slow diffusion with slow constant values of Kdi2 showing saturation of macropores by nickel ions. This step is called internal diffusion because diffusion takes place in the micropores [43]. It is obvious here that intraparticle diffusion model does not govern the adsorption process since the curves do not pass through the origin. Figures of the pseudo-first-order, pseudo-second-order, and Elovich models are found in supplementary materials (Figures S4–S6, respectively). The values of all the model parameters and the correlation coefficients are presented in Table 6.Figure 11
Intraparticle diffusion model for the adsorption of nickel(II) ions onto prepared activated carbon (ACPH, ACPA, and NIC) and raw material, RM.Our results on the adsorption capacity of studied activated samples have been compared with some results from the literature [22, 30, 44, 45] (see Table 7). We observe that activated carbons prepared from cassava tuber peelings (this study) offer better adsorption capacities for Ni(II) ions (adsorbate) and thereby constitute low-cost biomass for the depollution of nickel ions in an aqueous solution.Table 7
Comparison of adsorption capacity (Ni2+ ions) of activated carbons (adsorbents).
AdsorbentsAdsorption capacity (mg/g)ReferencesMosambi fruit peelings29.41[22]Cajanus cajan L. Millsp seed shell activated carbons29.60[30]Activated carbon from artichoke49.02[43]Modified holly sawdust22.47[45]Activated carbon from peelings of cassava tubers46.53Present study


## 8.1. Pseudo-First-Order Model

Kinetic parameters for the adsorption process were studied for contact times ranging between 5 and 60 minutes by monitoring the quantity of nickel(II)) adsorbed as a function of time. The data were then regressed against the Lagergren equation (13), which represents a first-order kinetic equation [39].(13)LnQe−Qt=LnQe−Ktt,where k1 is the pseudo-first-order rate constant (min−1); Qe and Qt are the adsorption capacities at equilibrium and at a given time t and are expressed in (mg/g).


## 8.2. Pseudo-Second-Order Model

The linearized pseudo-second-order chemisorption kinetic model, equation (14) [40], has been appropriately utilized in experiments involving the adsorption of organics and heavy metals on activated carbon.(14)tQt=1K2Qe2+tQe,where K2 is the pseudo-second-order rate constant (mg.g−1.min−1).


## 8.3. Elovich Model

The linearized Elovich equation is generally expressed as(15)Qt=1βlnαβ+1βlnt,where α is the initial sorption rate (mg/g min) and β is the desorption rate constant (g/mg) during any one experiment. These constants will be obtained from the relation qt=flnt [41].


## 8.4. Intraparticle Diffusion Model

The rate constants of intraparticle diffusion (Kid) at different nickel(II) ion concentrations were determined using the following linearized equation:(16)qt=Kidt1/2+C,where qt is the amount of nickel(II) sorbed at time t. Kid is the intraparticle diffusion constant (mg.g−1.min−1/2). When intraparticle diffusion plays a significant role in controlling the kinetics of the sorption process, straight-line plots through the origin are obtained and their slopes give the rate constant, kid.The results of kinetic studies (Table6) indicate that the adsorption process follows the second-order rate equation for the four adsorbents with correlation coefficient R2 = 0.999 for ACPH, ACPA, NIC, and RM. This implies that chemisorption is the limiting step of the process [41]. By comparison, the values of Qe determined from this model, which stand as 52.63 mg/g for ACPH, 51.81 mg/g for ACPA, 50.00 mg/g for NIC, and 42.37 mg/g for RM, are very close to their experimental analogs. This confirms once more that ACPH and ACPA performed better in nickel(II) uptake compared to the two others. Initial rates show that the kinetics of adsorption of the pollutant is faster on the surface of ACPH than to ACPA, NIC, and RM. The half-life of the pseudo-second-order reaction shows that adsorption kinetics of the nickel(II) ions is faster on the surface of the NIC compared to the other materials (ACPH, ACPA, and RM).Table 6
Results of adsorption parameters for the different kinetic models.
ModelConstantsACPHACPANICRMPseudo-first-orderR20.9780.9850.9170.897K1 (min−1)0.0550.0620.0500.073Qe (mg/g)6.4598.04913.6216.11RMSE53.8950.7741.0229.23Pseudo-second-orderR20.9990.9990.9990.999h (mg/g. min)57.0648.9919.7017.11t1/2 (min)0.9211.0582.5352.475K2 (g/mg.min)0.0210.0180.0080.010Qe (mg/g)52.6351.8150.0042.37RMSE1.2421.2421.3801.175Intraparticle diffusionR20.9960.9720.9740.996Kid1 (min−1)1.0051.8573.6273.970C1 (mg/g)44.8840.4627.9219.81RMSE0.4842.3534.9316.063R20.6460.6270.6790.094Kid2 (min−1)0.4760.5091.4500.291C2 (mg/g)48.3647.0936.9638.32RMSE1.4181.9852.3195.652ElovichR20.9700.9770.9710.934β (g/mg)0.4750.3730.1980.197α (mg/g min)1.99×1099.24×1061.30×1033.28×102RMSE0.2940.3190.6831.057Results obtained from intraparticle diffusion model (obtained viaQt = f (t1/2)) are graphs with two linear portions each (Figure 11) indicative of an adsorption process taking place in two steps for all four adsorbents. The first portion is characterized by rapid or fast diffusion of nickel(II) from the external surface toward the macropores of the adsorbents also known as macroporous diffusion [42]. This portion is also characterized by higher diffusion constants, Kdi1. The second portion corresponds to very slow diffusion with slow constant values of Kdi2 showing saturation of macropores by nickel ions. This step is called internal diffusion because diffusion takes place in the micropores [43]. It is obvious here that intraparticle diffusion model does not govern the adsorption process since the curves do not pass through the origin. Figures of the pseudo-first-order, pseudo-second-order, and Elovich models are found in supplementary materials (Figures S4–S6, respectively). The values of all the model parameters and the correlation coefficients are presented in Table 6.Figure 11
Intraparticle diffusion model for the adsorption of nickel(II) ions onto prepared activated carbon (ACPH, ACPA, and NIC) and raw material, RM.Our results on the adsorption capacity of studied activated samples have been compared with some results from the literature [22, 30, 44, 45] (see Table 7). We observe that activated carbons prepared from cassava tuber peelings (this study) offer better adsorption capacities for Ni(II) ions (adsorbate) and thereby constitute low-cost biomass for the depollution of nickel ions in an aqueous solution.Table 7
Comparison of adsorption capacity (Ni2+ ions) of activated carbons (adsorbents).
AdsorbentsAdsorption capacity (mg/g)ReferencesMosambi fruit peelings29.41[22]Cajanus cajan L. Millsp seed shell activated carbons29.60[30]Activated carbon from artichoke49.02[43]Modified holly sawdust22.47[45]Activated carbon from peelings of cassava tubers46.53Present study


## 9. Conclusion

This work aimed at the removal of nickel(II) ions from an aqueous solution by batch adsorption experiments onto activated carbon from the peelings of cassava tubers (ACPH, ACPA, and NIC). Best values of iodine indices were obtained at 400°C (pyrolysis temperature) for materials obtained via impregnation ratios of 2 : 1 and 1 : 1 for ACPH and ACPA, respectively. The functional groups on the surface of the adsorbents were characterized by chemical analysis of activated samples by the Boehm method and FTIR analysis. Elemental analysis of three activated carbon samples (ACPH, ACPA, and NIC) revealed a higher carbon content for activated materials compared to the precursors. SEM imaging techniques showed microporous structures. Equilibrium studies showed that the Langmuir model best described the adsorption process with the best correlation coefficient close to unity, therefore implying monolayer adsorption on a homogeneous surface. Kinetic study of nickel(II) adsorption showed that the process is controlled by the pseudo-second-order model with correlation coefficientR2 = 0.999 for ACPH, ACPA, NIC, and RM, respectively. This work has portrayed that activated carbons from cassava peelings can serve as effective low-cost agricultural materials for the treatment of water contaminated by nickel(II) ions.



---

*Source: 5545110-2021-08-02.xml*