# Preparation and Characterization of Biochar Derived from Agricultural By-Products for Dye Removal

Authors: Phuong Thu Le; Huyen Thuong Bui; Duy Ngoc Le; Thi Hue Nguyen; Le Anh Pham; Hong Nam Nguyen; Quoc Son Nguyen; Thu Phuong Nguyen; Ngọc Trinh Bich; Thi Thuy Duong; Marine Herrmann; Sylvain Ouillon; Thi Phuong Quynh Le
Journal: Adsorption Science & Technology
 (2021)

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## Abstract

In this study, biochar was derived from the agricultural by-products coconut coir (BC1) and rice husk (BC2) activated with NaOH 25%. This material was characterized through analytical methods such as SEM images, XRD, FTIR, and Raman. Analysis results indicated that the carbon structure carbon is amorphous and with many graphene layers. A high specific surface area was detected with 364.22 m2.g-1 for BC1 and 329.71 m2.g-1 for BC2 with many meso and micropores when analyzed by N2 and CO2 adsorption. The material also showed anionic and cationic dye adsorption capacity for textile wastewater following both Langmuir and Freundlich models where BC2 had better max adsorption capacity compared to BC1, 6.519 mg.g-1 for MO and 8.612 mg.g-1 for MB.


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## Body

## 1. Introduction

Textile is one of the largest industries in the globe. Vietnam was ranked 8th in exporting textile and dye products in 2018 according to the WTO, which provided over 1.6 million employments [1]. However, this industry emits huge amounts of wastewater that need to be treated. Many solutions such as biological treatments [2, 3], electrocoagulation [4–6], membrane bioreactors [7–9], or photochemical methods [10] have been developed. [11] combined a coagulation-flocculation treatment with alkali-activated carbon made from sand with a TAN efficiency of 70%. Compared to other methodologies, many studies have confirmed that adsorption methods with activated carbon from agricultural by-products are highly effective when treating textile dyeing wastewater.Various studies have shown that agricultural by-products such as straw, rice husks, corn cobs, or coir have a high potential for adsorption of pollutants, especially pesticides and dyes in wastewater [12, 13]. The superiority of these types of material lies in the fact that it is inexpensive or even free, is available in abundance, especially in countries with strong agricultural economies like Vietnam, and is easily biodegradable in the environment. Vietnam is classified among the top five rice-producing countries in the world with an output of 38 million tons.year-1 (GSO, 2009), equivalent to 38 million tons of straw and 6-7 million tons of rice husks. Common agricultural by-products from rice production straw, rice husk ash, and rice hulls [14] have all be shown to be beneficial in removing pesticides [14–16] and dyes [17–19]. Rice husk-derived biochar has also been studied and applied to remove contaminants from polluted water with an adsorption capacity of 123.03 mg.g-1 for glyphosate [20] and 9.73 mg.g-1 for the methylene blue [21].In addition to rice, Vietnam is also known as one of the ten largest manufacturers of coconut-related products in the world with an output of around 1.5 million tons in 2017, the second-largest producer of coir in the world with 36,000 tons in 2017 (FAO,2018). The primary by-product of coconut is coconut shell which has a high adsorption capacity and is hence widely used in biofilter systems for the purpose of pesticides removal [22–24]. Other studies have proven its usefulness in textile wastewater treatments [25–27]. Results all showed that biochar has a high ability to remove pollutants in general. The vast majority of agricultural by-products are lignocellulose materials composed largely of polysaccharides (cellulose and hemicelluloses) and lignins with a chemical composition of hydroxyl and carboxyl groups [28]. Interactions between these functional groups and pesticides are also expected to be the primary mechanism for adsorption of agricultural by-products [29]. Agricultural by-products have received much attention from scientists as a source for biochar [30]. For a long time, combining biochar with the right measurement of soil has been used to increase the water holding capacity as well as soil nutrients and crop yield [31]. Furthermore, recent studies have demonstrated the high efficiency and feasibility of biochar-soil blending at laboratory and field scales for the purpose of preventing glyphosate-containing pesticides in soil from leaking into natural water sources [32–35]. However, De Gisi et al. [36] showed that there is a lack of data concerning the characteristics of the new by-products studied such as their average particle size or specific surface area.With the abundance of input materials as well as the necessity to recycle such a valuable agricultural waste, biochar derived from rice husk and coconut coir is expected to be the answer to the demand for an economically and environmentally friendly material that has effective pollutants adsorption ability for application in surface water treatment.In this study, biochar was prepared in the laboratory from agricultural by-products in Vietnam such as coconut coir (named BC1) and rice husks (named BC2) by a pyrolysis method to investigate its potential in water pollution treatment. To be more specific, this research is designed to test the adsorbability of the biochar towards two different dyes, i.e., methylene blue—a cationic dye, and methyl orange—an anionic dye.


## 2. Chemicals and Methodology

### 2.1. Chemicals

Methylene blue trihydrate (MB, C16H18ClN3S.3H2O, ≥98.5%)—a cationic dye and methyl orange (MO, C14H14N3NaO3S, ≥98.5%)—an anionic dye represent both types of separate functional group and were purchased from Xilong Chemical Co., Ltd. (China). We used sodium chloride (NaCl, ≥99.5%) and sodium hydroxide (NaOH, ≥99.5%) from Merck (Germany), and hydrochloric acid (HCl, 35.0-37.0%) and nitric acid (HNO3, 65%) from Daejung chemicals and metals (Korea).


### 2.2. Methodology

#### 2.2.1. Biochar Production

Rice husk was collected from Bac Ninh province, Northern Vietnam, and thoroughly sieved to keep only the 5 mm diameter husk for use. Coconut fiber was collected from Hoai Duc district, Hanoi city, cut into small pieces, and sieved into coir less than 2 mm and more than 1 mm in diameter.Rice husk and coconut coir were carefully washed three times with tap water and twice with distilled water to remove impurities. After that, the coir and the husk were dried at 105°C in the oven for 5 hours until they were completely dried. The husk (or coir) was then placed in a stainless steel pot and covered on the surface with commercial charcoal to prevent the formation of ash and coke during carbonization. Next, the pot was sealed and put into the Nabertherm furnace (Germany) under limited oxygen conditions. The material heating program used is shown in the diagram in Figure1. At the end of the carbonization, the biochars’ weight, density, and mass loss (%) were calculated (Table 1).Figure 1
Biochar production process diagram.Table 1
Density and weight loss of each material before and after carbonization.
MaterialDensity before carbonization (g.mL-1)Density after carbonization (g.mL-1)Weight loss (%)Coir/biochar 10.13090.104460Husk/biochar 20.22590.130957Biochar after carbonization is activated by NaOH 25%: biochar’s specific surface area, ion-exchange capacity, and the number of oxygen-containing functional groups all raise after it is treated with NaOH [37, 38]. It can simultaneously be used as an effective, inexpensive, and ecologically acceptable activator [39]. A mixture of 18 g biochar and 300 mL of NaOH 25% solution were thus added into a Duran bottle of 500 mL, and the mixture was shaken at 250 rpm in an IKA KS 4000i incubator shaker for 4 hours at room temperature. The material was then filtered out and washed with distilled water (with a conductivity less than 18 megaohms), dried naturally at room temperature, and stored in a brown bottle.


#### 2.2.2. Characterization of Biochars

A temperature-induced mass loss of 0.7 g each raw material (rice husk and coconut shell) was determined by thermogravimetric analysis and differential gravimetric analysis (TGA/DTG) using a CIRAD-designed Macro-TGA from 25°C to 800°C at a heating rate of 5°C.min-1 under air. Every 5 seconds, mass loss data and temperature changes were recorded by the MTG software and analyzed on the Origin software. The functional groups and characterizing covalent bonding information of the different biochars after the pyrolysis were analyzed by FT-IR spectrometer (Thermo scientific iS50). Information on the crystal structure, phase, orientation, and molecular interactions of the biochars after fabrication were studied on the Equinox 5000-XRD Spectrometreler and the Raman spectrometer NRS-5100 from JASCO Corporation, Japan. The surface morphology and porous structure were observed by a scanning electron microscope (SEM, Hitachi S-4800). This instrument is also integrated with Energy Dispersive X-ray Spectroscopy for the analysis of the surface elemental composition of materials.N2 and CO2 adsorption isotherms of samples processed under vacuum conditions at 300°C were analyzed. The measurement was performed by a Belsorp minill MicrotracBEL device at -196°C (for N2 sorption) and 25°C (for CO2 sorption), pressure 1 bar. The Belsorp software (BEL master TM) was used to analyze the porosity properties of carbon materials. Application of N2 adsorption isotherm by the BET equation and graph data allowed calculation of the specific surface area, total pore volume, and micrometer-sized pore distribution. The CO2 adsorption isotherm by the Dubinin-Astakhov (DA) method was used to determine the pore volume of the sample.To determine pHpzc, two different solutions of sodium chloride (NaCl) were prepared at 10-2 M and 5×10−2M with purged deionized water (CO2–free) and adjusted with pure hydrochloric acid (HCl) and pelleted sodium hydroxide (NaOH) to different pH values, i.e. 2, 4, 6, 8, 10, and 12. Then, each biochar was added into separated bottles at a ratio of 5 g of biochar to 1 L of pH–adjusted sodium chloride solution of 70 mL total. The bottles were secured in the incubator shaker for 24 hours. After shaking, the pH value was recorded in order to sketch an initial and final pH diagram.


#### 2.2.3. Adsorbability of Biochars

MB and MO dyes were used to study the adsorption capacity of the biochar prepared at room temperature. These experiments were carried out in a 70 mL solution containing a 10 mg.L-1 dye solution and a 5 mg.L-1 biochar in a 100 mL Duran bottle. The initial pH was chosen based on the BC pHpzc data adjusted by using a solution of H2SO4 and NaOH. A mixing series was set up, and the solution was shaken in the incubator shaker IKA KS 4000i at 250 rpm. All experiments were carried out at room temperature. Each sample was collected after 2 hours. The adsorbents were centrifuged in Hermle centrifuge Z 366 K at 4500 rpm for 20 minutes, separated by Whatman cellulose acetate paper with a pore size of 0.45 μm, and dried at 105°C for 2 hours. The concentration changes of the dye solutions were measured by Shimadzu UV–1800 UV–Vis spectrometer.


#### 2.2.4. Determination of MB and MO Concentrations by UV-Vis Spectrophotometry

For the study of MB removal efficiency, the absorbance of the samples at maximum wavelengthλmax=664nm was measured. Calibration curves for MB were prepared with 7 different standard concentrations ranging from 0 mg.L-1 to 12 mg.L-1. Since the color of MO is pH-dependent, the absorbance of the solution was measured at λmax=507nm for pH=2, and at λmax=464nm for both pH=12, the natural pH value of the solution.TheH removal efficiency (%) can be calculated based on the dye concentration:(1)H=C0−CtC0×100,whereC0 and Ct are the dye concentrations at initial time and time t, respectively.According to Lamber Beer’s law:Abs=εbC, the dye concentration C is directly proportional to the absorbance since the molar attenuation coefficient ε and the path length b (size of cuvette) remain constant. Therefore, the H removal efficiency (%) can be calculated based on the absorbance of the solution:(2)H=Abs0−AbstAbs0×100,whereAbs0 and Abst are the absorbances measured at initial time and time t, respectively.Batch adsorption experiments for MB and MO removal were conducted in triplicates. In this study, the pH value of the research samples was determined by Hana instrument HI98197 portable multiparameter meter according to TCVN 6492 : 2011, ISO 10523 : 2008.


## 2.1. Chemicals

Methylene blue trihydrate (MB, C16H18ClN3S.3H2O, ≥98.5%)—a cationic dye and methyl orange (MO, C14H14N3NaO3S, ≥98.5%)—an anionic dye represent both types of separate functional group and were purchased from Xilong Chemical Co., Ltd. (China). We used sodium chloride (NaCl, ≥99.5%) and sodium hydroxide (NaOH, ≥99.5%) from Merck (Germany), and hydrochloric acid (HCl, 35.0-37.0%) and nitric acid (HNO3, 65%) from Daejung chemicals and metals (Korea).


## 2.2. Methodology

### 2.2.1. Biochar Production

Rice husk was collected from Bac Ninh province, Northern Vietnam, and thoroughly sieved to keep only the 5 mm diameter husk for use. Coconut fiber was collected from Hoai Duc district, Hanoi city, cut into small pieces, and sieved into coir less than 2 mm and more than 1 mm in diameter.Rice husk and coconut coir were carefully washed three times with tap water and twice with distilled water to remove impurities. After that, the coir and the husk were dried at 105°C in the oven for 5 hours until they were completely dried. The husk (or coir) was then placed in a stainless steel pot and covered on the surface with commercial charcoal to prevent the formation of ash and coke during carbonization. Next, the pot was sealed and put into the Nabertherm furnace (Germany) under limited oxygen conditions. The material heating program used is shown in the diagram in Figure1. At the end of the carbonization, the biochars’ weight, density, and mass loss (%) were calculated (Table 1).Figure 1
Biochar production process diagram.Table 1
Density and weight loss of each material before and after carbonization.
MaterialDensity before carbonization (g.mL-1)Density after carbonization (g.mL-1)Weight loss (%)Coir/biochar 10.13090.104460Husk/biochar 20.22590.130957Biochar after carbonization is activated by NaOH 25%: biochar’s specific surface area, ion-exchange capacity, and the number of oxygen-containing functional groups all raise after it is treated with NaOH [37, 38]. It can simultaneously be used as an effective, inexpensive, and ecologically acceptable activator [39]. A mixture of 18 g biochar and 300 mL of NaOH 25% solution were thus added into a Duran bottle of 500 mL, and the mixture was shaken at 250 rpm in an IKA KS 4000i incubator shaker for 4 hours at room temperature. The material was then filtered out and washed with distilled water (with a conductivity less than 18 megaohms), dried naturally at room temperature, and stored in a brown bottle.


### 2.2.2. Characterization of Biochars

A temperature-induced mass loss of 0.7 g each raw material (rice husk and coconut shell) was determined by thermogravimetric analysis and differential gravimetric analysis (TGA/DTG) using a CIRAD-designed Macro-TGA from 25°C to 800°C at a heating rate of 5°C.min-1 under air. Every 5 seconds, mass loss data and temperature changes were recorded by the MTG software and analyzed on the Origin software. The functional groups and characterizing covalent bonding information of the different biochars after the pyrolysis were analyzed by FT-IR spectrometer (Thermo scientific iS50). Information on the crystal structure, phase, orientation, and molecular interactions of the biochars after fabrication were studied on the Equinox 5000-XRD Spectrometreler and the Raman spectrometer NRS-5100 from JASCO Corporation, Japan. The surface morphology and porous structure were observed by a scanning electron microscope (SEM, Hitachi S-4800). This instrument is also integrated with Energy Dispersive X-ray Spectroscopy for the analysis of the surface elemental composition of materials.N2 and CO2 adsorption isotherms of samples processed under vacuum conditions at 300°C were analyzed. The measurement was performed by a Belsorp minill MicrotracBEL device at -196°C (for N2 sorption) and 25°C (for CO2 sorption), pressure 1 bar. The Belsorp software (BEL master TM) was used to analyze the porosity properties of carbon materials. Application of N2 adsorption isotherm by the BET equation and graph data allowed calculation of the specific surface area, total pore volume, and micrometer-sized pore distribution. The CO2 adsorption isotherm by the Dubinin-Astakhov (DA) method was used to determine the pore volume of the sample.To determine pHpzc, two different solutions of sodium chloride (NaCl) were prepared at 10-2 M and 5×10−2M with purged deionized water (CO2–free) and adjusted with pure hydrochloric acid (HCl) and pelleted sodium hydroxide (NaOH) to different pH values, i.e. 2, 4, 6, 8, 10, and 12. Then, each biochar was added into separated bottles at a ratio of 5 g of biochar to 1 L of pH–adjusted sodium chloride solution of 70 mL total. The bottles were secured in the incubator shaker for 24 hours. After shaking, the pH value was recorded in order to sketch an initial and final pH diagram.


### 2.2.3. Adsorbability of Biochars

MB and MO dyes were used to study the adsorption capacity of the biochar prepared at room temperature. These experiments were carried out in a 70 mL solution containing a 10 mg.L-1 dye solution and a 5 mg.L-1 biochar in a 100 mL Duran bottle. The initial pH was chosen based on the BC pHpzc data adjusted by using a solution of H2SO4 and NaOH. A mixing series was set up, and the solution was shaken in the incubator shaker IKA KS 4000i at 250 rpm. All experiments were carried out at room temperature. Each sample was collected after 2 hours. The adsorbents were centrifuged in Hermle centrifuge Z 366 K at 4500 rpm for 20 minutes, separated by Whatman cellulose acetate paper with a pore size of 0.45 μm, and dried at 105°C for 2 hours. The concentration changes of the dye solutions were measured by Shimadzu UV–1800 UV–Vis spectrometer.


### 2.2.4. Determination of MB and MO Concentrations by UV-Vis Spectrophotometry

For the study of MB removal efficiency, the absorbance of the samples at maximum wavelengthλmax=664nm was measured. Calibration curves for MB were prepared with 7 different standard concentrations ranging from 0 mg.L-1 to 12 mg.L-1. Since the color of MO is pH-dependent, the absorbance of the solution was measured at λmax=507nm for pH=2, and at λmax=464nm for both pH=12, the natural pH value of the solution.TheH removal efficiency (%) can be calculated based on the dye concentration:(1)H=C0−CtC0×100,whereC0 and Ct are the dye concentrations at initial time and time t, respectively.According to Lamber Beer’s law:Abs=εbC, the dye concentration C is directly proportional to the absorbance since the molar attenuation coefficient ε and the path length b (size of cuvette) remain constant. Therefore, the H removal efficiency (%) can be calculated based on the absorbance of the solution:(2)H=Abs0−AbstAbs0×100,whereAbs0 and Abst are the absorbances measured at initial time and time t, respectively.Batch adsorption experiments for MB and MO removal were conducted in triplicates. In this study, the pH value of the research samples was determined by Hana instrument HI98197 portable multiparameter meter according to TCVN 6492 : 2011, ISO 10523 : 2008.


## 2.2.1. Biochar Production

Rice husk was collected from Bac Ninh province, Northern Vietnam, and thoroughly sieved to keep only the 5 mm diameter husk for use. Coconut fiber was collected from Hoai Duc district, Hanoi city, cut into small pieces, and sieved into coir less than 2 mm and more than 1 mm in diameter.Rice husk and coconut coir were carefully washed three times with tap water and twice with distilled water to remove impurities. After that, the coir and the husk were dried at 105°C in the oven for 5 hours until they were completely dried. The husk (or coir) was then placed in a stainless steel pot and covered on the surface with commercial charcoal to prevent the formation of ash and coke during carbonization. Next, the pot was sealed and put into the Nabertherm furnace (Germany) under limited oxygen conditions. The material heating program used is shown in the diagram in Figure1. At the end of the carbonization, the biochars’ weight, density, and mass loss (%) were calculated (Table 1).Figure 1
Biochar production process diagram.Table 1
Density and weight loss of each material before and after carbonization.
MaterialDensity before carbonization (g.mL-1)Density after carbonization (g.mL-1)Weight loss (%)Coir/biochar 10.13090.104460Husk/biochar 20.22590.130957Biochar after carbonization is activated by NaOH 25%: biochar’s specific surface area, ion-exchange capacity, and the number of oxygen-containing functional groups all raise after it is treated with NaOH [37, 38]. It can simultaneously be used as an effective, inexpensive, and ecologically acceptable activator [39]. A mixture of 18 g biochar and 300 mL of NaOH 25% solution were thus added into a Duran bottle of 500 mL, and the mixture was shaken at 250 rpm in an IKA KS 4000i incubator shaker for 4 hours at room temperature. The material was then filtered out and washed with distilled water (with a conductivity less than 18 megaohms), dried naturally at room temperature, and stored in a brown bottle.


## 2.2.2. Characterization of Biochars

A temperature-induced mass loss of 0.7 g each raw material (rice husk and coconut shell) was determined by thermogravimetric analysis and differential gravimetric analysis (TGA/DTG) using a CIRAD-designed Macro-TGA from 25°C to 800°C at a heating rate of 5°C.min-1 under air. Every 5 seconds, mass loss data and temperature changes were recorded by the MTG software and analyzed on the Origin software. The functional groups and characterizing covalent bonding information of the different biochars after the pyrolysis were analyzed by FT-IR spectrometer (Thermo scientific iS50). Information on the crystal structure, phase, orientation, and molecular interactions of the biochars after fabrication were studied on the Equinox 5000-XRD Spectrometreler and the Raman spectrometer NRS-5100 from JASCO Corporation, Japan. The surface morphology and porous structure were observed by a scanning electron microscope (SEM, Hitachi S-4800). This instrument is also integrated with Energy Dispersive X-ray Spectroscopy for the analysis of the surface elemental composition of materials.N2 and CO2 adsorption isotherms of samples processed under vacuum conditions at 300°C were analyzed. The measurement was performed by a Belsorp minill MicrotracBEL device at -196°C (for N2 sorption) and 25°C (for CO2 sorption), pressure 1 bar. The Belsorp software (BEL master TM) was used to analyze the porosity properties of carbon materials. Application of N2 adsorption isotherm by the BET equation and graph data allowed calculation of the specific surface area, total pore volume, and micrometer-sized pore distribution. The CO2 adsorption isotherm by the Dubinin-Astakhov (DA) method was used to determine the pore volume of the sample.To determine pHpzc, two different solutions of sodium chloride (NaCl) were prepared at 10-2 M and 5×10−2M with purged deionized water (CO2–free) and adjusted with pure hydrochloric acid (HCl) and pelleted sodium hydroxide (NaOH) to different pH values, i.e. 2, 4, 6, 8, 10, and 12. Then, each biochar was added into separated bottles at a ratio of 5 g of biochar to 1 L of pH–adjusted sodium chloride solution of 70 mL total. The bottles were secured in the incubator shaker for 24 hours. After shaking, the pH value was recorded in order to sketch an initial and final pH diagram.


## 2.2.3. Adsorbability of Biochars

MB and MO dyes were used to study the adsorption capacity of the biochar prepared at room temperature. These experiments were carried out in a 70 mL solution containing a 10 mg.L-1 dye solution and a 5 mg.L-1 biochar in a 100 mL Duran bottle. The initial pH was chosen based on the BC pHpzc data adjusted by using a solution of H2SO4 and NaOH. A mixing series was set up, and the solution was shaken in the incubator shaker IKA KS 4000i at 250 rpm. All experiments were carried out at room temperature. Each sample was collected after 2 hours. The adsorbents were centrifuged in Hermle centrifuge Z 366 K at 4500 rpm for 20 minutes, separated by Whatman cellulose acetate paper with a pore size of 0.45 μm, and dried at 105°C for 2 hours. The concentration changes of the dye solutions were measured by Shimadzu UV–1800 UV–Vis spectrometer.


## 2.2.4. Determination of MB and MO Concentrations by UV-Vis Spectrophotometry

For the study of MB removal efficiency, the absorbance of the samples at maximum wavelengthλmax=664nm was measured. Calibration curves for MB were prepared with 7 different standard concentrations ranging from 0 mg.L-1 to 12 mg.L-1. Since the color of MO is pH-dependent, the absorbance of the solution was measured at λmax=507nm for pH=2, and at λmax=464nm for both pH=12, the natural pH value of the solution.TheH removal efficiency (%) can be calculated based on the dye concentration:(1)H=C0−CtC0×100,whereC0 and Ct are the dye concentrations at initial time and time t, respectively.According to Lamber Beer’s law:Abs=εbC, the dye concentration C is directly proportional to the absorbance since the molar attenuation coefficient ε and the path length b (size of cuvette) remain constant. Therefore, the H removal efficiency (%) can be calculated based on the absorbance of the solution:(2)H=Abs0−AbstAbs0×100,whereAbs0 and Abst are the absorbances measured at initial time and time t, respectively.Batch adsorption experiments for MB and MO removal were conducted in triplicates. In this study, the pH value of the research samples was determined by Hana instrument HI98197 portable multiparameter meter according to TCVN 6492 : 2011, ISO 10523 : 2008.


## 3. Results and Discussion

### 3.1. TGA/DTG and Biochar Density

The biochar carbonization process was set up based on the result of TGA/DTG analysis, shown in Figure2.Figure 2
DTG/TGA diagram of coir (a) and rice husk (b).
(a)(b)The TGA/DTG diagram shows the mass loss curves of both materials (coir and husk) as a function of temperature at the heating rate of 5°C.min-1. The materials were dried before carbonization, so in the temperature range from 100°C to 250°C, the mass does not change much, indicating the absence of free water molecules in the materials. The biggest mass loss occurs at 250–300°C, with a loss greater than 60% and 40% for coir and husk, respectively, suggesting that water and bounds organic compounds have been decomposed. In the temperature range of 300°C-450°C, the pyrolysis process continues at a slower rate, with the final yield reaching about 5% for coir and 25% for husk. Both TGA/DTG diagrams of coir and husk indicate that the mass yield hardly changes at temperatures above 450°C, which suggests that only ash remains.These results show that although the DTG/TG curve of husk is a little different from that of coir, they are very similar at the first order, which justifies that the same calcination process was used for both materials (Figure1).Before and after the carbonization process, each mass and volume of each material were measured to calculate the initial and final density (before/after carbonization). The density of each material is recorded in Table1.There is no common pattern for the variation of density of the two materials before and after the carbonization process. For coconut coir (biochar 1 or BC1) and husk (biochar 2 or BC2), the density decreases by 20% and almost 50%, respectively. This is due to the fact that during calcination, water and organic compounds bound in the structure of the material were lost in gases and water vapor. However, the shape of the coconut coir (BC1) and the husk (BC2) was not altered much after the carbonization process, especially for the husk (which retained the shape of rice grains). Therefore, the density of both materials decreased slightly.As can be seen clearly from Table1, the actual mass loss after the carbonization of coir and husk was only 60% and 57%, respectively, much lower than when doing the TGA/DTG analysis (respectively, 95% and 75%, Figure 2). This can be explained by the formation of ash during TGA/DTG analysis, while during calcination, ashes were significantly reduced by covering the surface material with coal in the calcination process.


### 3.2. Point of Zero Charge (PZC)

The pH of the solution (methylene blue and methyl orange) has a great influence on the adsorption capacity of the adsorbent on the adsorbate [40]. In order to optimize this capacity, the point of zero charge (PZC) should be analyzed and used. When pH values are below the PZC of an adsorbent, anions are attracted to its surface; cations experience the same effect when pH values exceed the PZC [41]. Therefore, several experiments were carefully carried out to determine the PZC value for three types of biochar made from coir of two different sizes and from husk. The results on PZC are shown in Figures 3(a) and 3(b).Figure 3
PZC of BC1 (a) and PZC of BC2 (b) in a buffer solution containing, respectively, 0.05 M and 0.01 M NaCl.
(a)(b)A buffer solution was used for the determination of PZC: a solution of NaCl with NaOH or HCl provided a buffer to stabilize and ensure the desired pH values so that the PZC result was correct.For initial pH values of 2 and 12, the final pH values were almost identical to the initial values. Differences were only observed for initial pH values of 4, 6, and 10, where the final pH values remained stable around 9. This indicated that biochar 1 has an estimated PZC value atpH=9, at which the biochar surface reaches electrically neutral state. In addition, according to the PZC theory, at pH values above the PZC value, the materials are negatively charged, and vice versa for pH values below the PZC.For biochar 2, the initial–final pH curve is also similar to that of biochar 1; however, the PZC obtained for biochar 2 was lower than that of the biochar 1, atpH=8.


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

All FTIR spectra of the obtained biochars were collected in the midinfrared from 4000 cm-1 to 390 cm-1 and are shown in Figure 4.Figure 4
FTIR analysis on the biochar.The two spectra showed similarities, in the single bond region, a wideband showing up at 3500 cm-1 attributed to the O–H stretching mode of hydroxyl groups, and in the double bond region. At about 1650 cm-1, the adsorption band was attributed to C=O stretching. For the spectrum of biochar 2, the greatest bands were observed at 1050 cm-1, which was in the fingerprint region, and it was attributed to the C–O stretching. In the wavenumber range of 900 cm-1 to 400 cm-1, the spectrum was quite complex and hard to observe. However, in particular, when observing the spectrum of biochar 2, some peaks could be clearly seen at 1087, 800, and 460 cm-1, which were attributed to the carbon-silicon group (C–Si) (Pankaj [42, 43]). This carbon-silicon group is often found on the husk surface and is not found in coir. The spectra of biochar 1 did not show many differences. Besides the two spectral bands observed at 3500 cm-1 and 1650 cm-1, the fingerprint region was also complex and hard to assign.


### 3.4. X-Ray Diffraction Spectroscopy (XRD) Results

The diffraction diagram of the biochars is presented in Figure5. Two wide peaks range at 2θ=22.5° and 2θ=43° and the absence of peak showing the formation of the crystal phase indicates that the BCs were amorphous carbon. In addition, the diagrams revealed the presence of graphene structure in all biochar samples. The formation of graphene structures can occur during the pyrolysis of materials derived from agricultural by-products [44]. This result is similar to the conclusions of BC diffraction studies from [44]. The diagram also showed that graphene is the only crystal structure that appears in the BCs. In other words, no crystal structure of other metals could be found on the BC samples. Many studies have also shown that silica compounds in rice husk can form crystals when the temperature reaches 800°C.Figure 5
Diffraction diagram of biochars 1 and 2.


### 3.5. Raman Spectrum

The carbon structure of biochar was also determined using Raman spectroscopy, complementing the results obtained from XRD (Figure6).Figure 6
Raman spectrum of difference BCs.Raman spectroscopy showed two main peaks at D band (1361 cm–1) and G band (1591 cm–1), corresponding to the graphene layer edge and an ideal lattice carbon, respectively [45]. Both peaks showed the presence of carbon atoms (sp2) in an aromatic compound that corresponds to the amorphous form of the benzene ring [46, 47]. Despite being different raw materials, the two biochars derived from rice husk and coir had the same shape spectrum, proving that the formation of biochar structure by pyrolisis from different agricultural by-products is the same. This result was also confirmed by the X-ray diffraction method of biochar. Biochar after pyrolysis has an amorphous form with several layers of graphene to create the porous structure of the material.


### 3.6. Surface Morphology of Biochars

Surface morphology and porous structure are important features in the adsorption process. In particular, for biochar, solids are obtained from the pyrolysis of rice husks and coir in an anaerobic environment (lack of oxygen and high pressure). The surface morphology, as well as the main surface elemental composition, was investigated by scanning electron microscopy (SEM) (Figures7 and 8) and energy dispersive X-ray emission (EDX).Figure 7
SEM images of BC1.Figure 8
SEM images of BC2.Generally, all BCs had porous meso and micropore structures with different shapes and sizes. SEM image observation of both BC types also showed the structure of the graphene layers formed along with the field structure of BC. These results also correspond to the results of [44].The SEM image of rice husk biochar (BC2) showed that it remained intact in its structure (fiber shape) of the original husk, and the pores were fairly uniform. After being broken in half, the cross-section image of BC2 revealed a series of pores with a capillary structure on the BC2 wall, about 5 to 10μm in diameter. Besides, although the mesopore structure was uneven, the micropore size was quite uniform with a diameter of approximately 50 nm.In contrast, the results for BC1 yielded a greater variety of pore sizes. Specifically, the surface morphology of biochar from coconut coir showed many pores of fairly nonuniform size with a large structure.The average percentage values of surface elemental composition in biochars, corresponding to the SEM micrographs analysis positions and dispersive spectrum are presented in Figure9 and Table 2.Figure 9
Energy dispersive spectrum corresponding to a SEM image analysis position of BC1 (a) and BC2 (b).
(a)(b)Table 2
Average mass percentage of surface elemental composition in biochar.
ComponentsBC1BC2C K (%)82.9340.27O K (%)16.7644.92Mg K (%)0.310.00Si K (%)0.0014.81Total100.00100.00The obtained results showed that the main component of all BCs was carbon, which confirmed the decomposition of cellulose, lignin, and organic matters contained in agricultural by-products at high-temperature 500-600°C. Besides, they revealed a significant content of oxygen. Combined with the results of the FTIR analysis, the oxygen content in the BCs was confirmed to come from the functional groups -COO- and -OH existing on the surface of BCs. Specifically, Si content included in the BC2 structure was consistent with the results of the FTIR analysis, indicating the bond between silicon and carbon (Si-C). However, the contents of C, O, and Si are unevenly distributed at different locations of the BCs.


### 3.7. Specific Surface Area and Pore Volume

The N2 adsorption-desorption isotherms (Figure 10) were used to determine the porosity of the BCs. The specific surface area and pore volume are significant parameters that have a strong link with the adsorption ability of the material. Micropores (diameter<2nm) and mesopores (between 2 and 50 nm) actively participate in the sorption capacity of biochar, while larger pores usually have a much smaller effect [48].Figure 10
BET-plot (a) and adsorption/desorption isotherm (b) of BC1 and BC2 in N2.
(a)(b)The BC2 had a higher microporosity compared to that of the BC1, as shown by the higher position of the corresponding isotherm and the larger slope at relative pressuresp/po above 0.1. The N2 adsorption-desorption isotherm of the BC1 exhibited type I isotherms in the IUPAC classification [49], which indicated that the microporous structure was dominant in the BC1. Meanwhile, the BC2’s isotherms exhibited type IV with a large range for the hysteresis loop. This can be explained by the capillary condensation phenomenon, whereby a gas in a pore condenses into a liquid phase at a pressure p<po of the bulk liquid [49]. This result strongly suggests that in the case of BC2, besides micropores, mesopores were also present.Table3 shows the results of total surface area (SBET) and total pore volume (VBET), estimated by the BET method, and micropore volume (VMicro) and mesopore volume (VMeso), estimated by the t-plot and BJH methods, respectively.Table 3
Parameters of specific surface area and pore of biochar.
SampleSBET (m2.g-1)VBET (cm3.g-1)Vmeso (cm3.g-1)VMicro (BET) (cm3.g-1)VMicro (DA) (cm3.g-1)BC1329.70.170.030.140.21BC2364.20.260.140.150.26TheSBET of BC2 was higher than that of BC1 (364.2 m2.g-1 vs. 329.7 m2.g-1). Similarly, the pore volume of BC2 was 0.26 cm3.g-1 compared to 0.17 cm3.g-1 for BC1. Compared to other biomass chars produced under similar carbonization conditions, such as fern char [50] or cashew nutshell char [51], BCs produced in this study achieved higher porosity levels. The VMicro (estimated by BET technique) of BC1 and BC2 is similar. However, the large size of the N2 molecules prevents them from entering the ultra-micropores, i.e., pores with diameters less than 1 nm. Therefore, CO2 adsorption/desorption was performed to fully reflect the microporous structures of these BCs (Figure 11).Figure 11
DA-plot (a) and adsorption/desorption isotherm (b) of BC1 and BC2 in CO2.
(a)(b)The adsorption/desorption isotherm plot of CO2 of BC2 is above that of BC1, indicating a higher micropore volume. Moreover, both isotherms showed hysteresis at low-pressure. This indicates that the CO2 molecules were in a metastable state, and the gas was not readily released at the level corresponding to the value of thermodynamic equilibrium at pressure decrease [52]. In other words, both BCs exhibited heterogeneous surface properties with bottleneck shapes at the micropore entrance. This pore shape is known to be favorable for long particule capture.TheVMicro (estimated by DA method) reached 0.26 cm3.g-1 for BC2 and 0.21 cm3.g-1 for BC1. The smaller kinetic diameter of CO2 (0.3 nm) compared to N2 (0.36 nm) gave a much higher VMicro calculated by the DA method than by the t-plot method. This indicates that the microporous structures were better developed in rice husk biochar than in coir biochar.


### 3.8. Biochar Adsorbability

#### 3.8.1. General Evaluation of BC1 Adsorbability with Methylene Blue (MB)

Evaluation of the effect of pH on biochar 1 adsorbability of methylene blue was first performed. Experiments were carried out to evaluate the effect of varying pH values of dye solution on the ability of biochar to adsorb methylene blue ions. The results are shown in Figure12.Figure 12
Evaluation of the effect of pH on biochar 1 (5 g.L-1) adsorbability of methylene blue ions.The effect of pH on methylene blue adsorption was not significant for biochar 1 as there was little difference between the three efficiency lines. AtpH=2, the adsorbability of BC1 was however slightly weaker than at other pH values for the first hours of the time series, which accurately reflects the point of zero charge principle. The difference between the efficiency lines of BC1 was more distinct for the efficiency lines at pH=2 and at other pH values. The efficiency reached 66% at pH 2 and 87% at both pH 6 and pH 12 after 30 minutes of adsorption. When the adsorption time was increased to 1 hour, the adsorption efficiency showed similar differences, 87% at pH 2 and 94% at the other two pH values. It was found that dye adsorption increases with pH, with a maximum adsorption at pH 6. This could be due to the fact that the surface of the adsorbent becomes negative at higher pH values, favoring the adsorption of positively charged MB cationic dye via electrostatic attraction. Moreover, there is a slight reduction in adsorption at pH 12 due to the repulsion of adsorbent surface and the existence of a partial negative charge (Cl-) on MB [42].


#### 3.8.2. Evaluation of the Effect of Biochar Dosage on Adsorbability with Methylene Blue

The effect of varying biochar concentration on the adsorption of dye ions on the biochar surface was studied with methylene blue. The results are given in Figure13.Figure 13
Evaluation of the effect of biochar 1 dosage on adsorbability.As expected, the higher the biochar concentration, the better the adsorbability. However, the differences are not really significant. Based on these results, a catalyst concentration of 5 g.L-1 was selected for further studies.


#### 3.8.3. Evaluation of the Effect of pH on Biochar Adsorbability with Methyl Orange

The laboratory–synthesized biochar BC1 was studied for its ability to remove not only methylene blue but also methyl orange, an anionic dye. The results are shown in Figure14.Figure 14
Evaluation of the effect of pH on biochar 1 (5 g.L-1) adsorbability of methyl orange.At pH 2, it took less than an hour to reach 80% efficiency, and after 5 hours, biochar 1 had removed over 96% of the MO in the solution. In contrast, the efficiency of dye removal at pH 6 and 12 was approximately half that at pH 2, 49%, and 47%, respectively. At pH 6 and pH 12, the surface was, respectively, neutral and positively charged; therefore; adsorption efficiency is much lower.In addition to the electrostatic interaction following the PZC principle, many functional groups exist on the biochar surface and bind to methylene blue or methyl orange, thus, facilitating the adsorption on the biochar surface. When the pH of the solution was decreased significantly, the positive surface charge of the BC increased and, consequently, the adsorption of methyl orange anions on the BC surface increased significantly. On the contrary, when the pH of the solution was increased, the adsorption of methyl orange on BC1 decreased due to the repulsive force between the adsorbent and the negatively charged adsorbate. However, the adsorption of methylene blue at high pH was enhanced due to the strong electrostatic interaction between the cationic groups of MB molecule and the negatively charged BC surface. Therefore, this could be the main mechanism of the adsorption. The results showed that the highest adsorption efficiency of BC was obtained at basic pH values for MB and at acidic pH for MO.In consequence, the influence of the two different biochars on dye adsorbability was investigated at pH 6 for MB and at pH 2 for MO (Figure15).Figure 15
Effect of two different biochars on adsorbability of dyes molecules.Figure15 clearly demonstrates that the adsorption of BC2 was superior to that of BC1 under the same conditions with a peak efficiency of nearly 100%. This difference is also partly due to the physical characteristics of the adsorbent. BC2 is derived from the rice husk with a much higher number of pores than BC1 which is coconut coir. It has both meso and micropores, so the total BET and total porous volume of BC2 are larger than BC1, 364.22m2.g−1>329.71m2.g−1 and 0.26m2.g−1>0.17m2.g−1.Moreover, biochar 2 has a relatively high microporous and mesoporous area, 0.15 cm3.g1 and 0. 14 cm3.g-1 compared to 0.14 cm3.g-1 and 0.03 cm3.g-1 for biochar 1, respectively. Apart from those factors, these two types of biochar had similar surface functional groups, and the only difference was the silicon components found in BC2.The MB adsorption efficiency of BC1 was close to 94%, much higher than that of MO (about 82%) after 1 hour of the reaction. BC2 also showed a similar trend with the adsorption efficiency slightly higher for MB than for MO, about 100% and 96%, respectively. Both materials had better electronic interactions with MB than with MO. This suggested that the adsorption capacity of both biochars was more efficient for MB than for MO. Considering the physicochemical properties of the adsorbent surface, although MO (1.31×0.55×0.18nm) has a smaller molecular size than MB (1.26×0.77×0.65nm), which means that MO molecules were able to enter the pores and being retained in more micro and mesopores; however, MB ions were more selectively adsorbed.This result is consistent with the study of Phuong et al. [53] who obtained an average surface area including micropore and mesopore of rice husk–derived biochar of 118 m2.g-1. Since the volume of mesopore was quite small and most of the pore volume was micropore, MB ions took longer to be adsorbed into the BCA pores, so the adsorbability rate was slowed down. In our study, the dye adsorption rate of BC1 was slower than that of BC2 because BC2 had a larger BET volume and much larger pore volume, as mentioned above. Both dyes can be completely adsorbed.


#### 3.8.4. Isothermal Adsorption

The results of the physicochemical characteristics analysis showed that BC2 had a higher adsorption capacity than BC1 due to its larger surface area and pore volume, a larger number of surface functional groups, and a lower pH of PZC. Therefore, the adsorption isotherm of MB and MO adsorption was also evaluated through two popular adsorption models, Langmuir and Freundlich isotherm models. Figure16 shows the isotherm of MB and MO adsorption on BC1 material according to Langmuir and Freundlich models.Figure 16
Langmuir (a) and Freundlich (b) adsorption isotherm model fittings for the adsorption of MB and MO on BC1 and BC2 at 25°C.
(a)(b)The parameters of Langmuir and Freundlich adsorption isotherms were calculated from the slope values and the vertical cut and are presented in Table4.Table 4
The adsorption isotherm of MO and MB adsorbed on BC2 and BC2 materials according to Langmuir and Freundlich models.
ModelParametersMBMOBC1BC2BC1BC2Langmuir isotherm parametersR20.9220.9940.9910.969qmax (mg.g-1)6.4188.6123.0806.519B (L.mg-1)0.6932.4451.6311.153Freundlich isotherm parametersR20.9920.3650.6720.988KF[(mg.g-1) (L.mg-1)]n2.0674.8341.8012.536n2.1293.9782.6942.268Langmuir and Freundlich adsorption isotherms are two chemisorption models in which Langmuir is a monolayer adsorption process while Freundlich describes a multilayer adsorption capacity of the material.The results demonstrated that the adsorption capacity of BC2 followed both Langmuir and Freundlich models with MO adsorbent. The regression coefficientsR2 were both high (0.97 and 0.99 for Langmuir and Freundlich, respectively), revealing that the adsorption process follows both models. In contrast, with the MB adsorbent, the adsorption isotherm followed the Langmuir model with a regression coefficient of 0.99. For BC1 adsorption, MO followed the Langmuir model with R2 of 0.99 and MB followed Freundlich with the same R2 value. Overall, in this study, the dye removal efficiency of BC2 was higher than that of BC1, both following the Langmuir and Freundlich isotherm models.Remind that the Freundlich model suggests multilayer physisorption on the surface of the material with different adsorption energy levels whereas the Langmuir model proposes monolayer chemisorption by the donor-acceptor interaction based on electrophilic addition [54, 55]. This was because the charge-rich carbonized surface created bonds with protonated amino groups in the acidic medium. In addition, H-H and H-O bonding between the carbon-silicon group on the surface of biochar with the phenolic group of dye molecules could also be able to occur [56].Rodriguez also indicated that the mechanism of dye adsorption on biochars may be classified into two types of interactions: nonelectrostatic and electrostatic. Adsorption is affected by the pH of the solution as well as the pHPZC. Therefore, at pH<pHpzc, the surface of the biochar is positively charged, promoting anionic species adsorption, and negatively charged at pH>pHpzc, favoring cationic species adsorption [57]. Furthermore, all biochar samples had pHpzc values of 8 and 9 for BC1 and BC2, respectively, higher than the pH values of MB (6.0) and MO (2) solutions. Biochar has a positive charge, MB is a cation dye that has a positive charge when dissolved in water, and MO is an anion dye that becomes negatively charged when dissolved in water. The adsorption mechanism is therefore dominated by the dispersion interaction between the dissociated electrons on the surface of the activated carbon and the free electrons of the dye molecule contained in the aromatic ring [58].TheRL separation factor values for dye adsorption on the particular adsorbent were all positive and less than unity in all cases, suggesting extremely favorable adsorption under all circumstances. This is furthermore consistent with the results for the 1/nF values, which were less than unity, suggesting that the dye is preferentially absorbed by biochar.In terms of the maximum adsorption capacity of a material, BC2 adsorbs both dyes well and better than BC1 with aqmax value of 8.612 mg.g-1 and 6.519 mg.g-1 for MB and MO, respectively. These values are was quite low compared to that of various adsorbents, such as bamboo-activated carbon [59], pea shells [60], modified clay-ball [61], and activated biochar derived from wakame [62]. However, biochars prepared with a particle size of 1-2 mm for coir and 5 mm for rice husk are more ecologically friendly and economically effective compared to other adsorbents. First, the granular nature of the adsorbent is useful since it can be easily separated after filtration and sedimentation without creating sludge. Second, in terms of recycling, using an agricultural by-product allows waste to be a valued resource to reduce environmental risks [12].


## 3.1. TGA/DTG and Biochar Density

The biochar carbonization process was set up based on the result of TGA/DTG analysis, shown in Figure2.Figure 2
DTG/TGA diagram of coir (a) and rice husk (b).
(a)(b)The TGA/DTG diagram shows the mass loss curves of both materials (coir and husk) as a function of temperature at the heating rate of 5°C.min-1. The materials were dried before carbonization, so in the temperature range from 100°C to 250°C, the mass does not change much, indicating the absence of free water molecules in the materials. The biggest mass loss occurs at 250–300°C, with a loss greater than 60% and 40% for coir and husk, respectively, suggesting that water and bounds organic compounds have been decomposed. In the temperature range of 300°C-450°C, the pyrolysis process continues at a slower rate, with the final yield reaching about 5% for coir and 25% for husk. Both TGA/DTG diagrams of coir and husk indicate that the mass yield hardly changes at temperatures above 450°C, which suggests that only ash remains.These results show that although the DTG/TG curve of husk is a little different from that of coir, they are very similar at the first order, which justifies that the same calcination process was used for both materials (Figure1).Before and after the carbonization process, each mass and volume of each material were measured to calculate the initial and final density (before/after carbonization). The density of each material is recorded in Table1.There is no common pattern for the variation of density of the two materials before and after the carbonization process. For coconut coir (biochar 1 or BC1) and husk (biochar 2 or BC2), the density decreases by 20% and almost 50%, respectively. This is due to the fact that during calcination, water and organic compounds bound in the structure of the material were lost in gases and water vapor. However, the shape of the coconut coir (BC1) and the husk (BC2) was not altered much after the carbonization process, especially for the husk (which retained the shape of rice grains). Therefore, the density of both materials decreased slightly.As can be seen clearly from Table1, the actual mass loss after the carbonization of coir and husk was only 60% and 57%, respectively, much lower than when doing the TGA/DTG analysis (respectively, 95% and 75%, Figure 2). This can be explained by the formation of ash during TGA/DTG analysis, while during calcination, ashes were significantly reduced by covering the surface material with coal in the calcination process.


## 3.2. Point of Zero Charge (PZC)

The pH of the solution (methylene blue and methyl orange) has a great influence on the adsorption capacity of the adsorbent on the adsorbate [40]. In order to optimize this capacity, the point of zero charge (PZC) should be analyzed and used. When pH values are below the PZC of an adsorbent, anions are attracted to its surface; cations experience the same effect when pH values exceed the PZC [41]. Therefore, several experiments were carefully carried out to determine the PZC value for three types of biochar made from coir of two different sizes and from husk. The results on PZC are shown in Figures 3(a) and 3(b).Figure 3
PZC of BC1 (a) and PZC of BC2 (b) in a buffer solution containing, respectively, 0.05 M and 0.01 M NaCl.
(a)(b)A buffer solution was used for the determination of PZC: a solution of NaCl with NaOH or HCl provided a buffer to stabilize and ensure the desired pH values so that the PZC result was correct.For initial pH values of 2 and 12, the final pH values were almost identical to the initial values. Differences were only observed for initial pH values of 4, 6, and 10, where the final pH values remained stable around 9. This indicated that biochar 1 has an estimated PZC value atpH=9, at which the biochar surface reaches electrically neutral state. In addition, according to the PZC theory, at pH values above the PZC value, the materials are negatively charged, and vice versa for pH values below the PZC.For biochar 2, the initial–final pH curve is also similar to that of biochar 1; however, the PZC obtained for biochar 2 was lower than that of the biochar 1, atpH=8.


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

All FTIR spectra of the obtained biochars were collected in the midinfrared from 4000 cm-1 to 390 cm-1 and are shown in Figure 4.Figure 4
FTIR analysis on the biochar.The two spectra showed similarities, in the single bond region, a wideband showing up at 3500 cm-1 attributed to the O–H stretching mode of hydroxyl groups, and in the double bond region. At about 1650 cm-1, the adsorption band was attributed to C=O stretching. For the spectrum of biochar 2, the greatest bands were observed at 1050 cm-1, which was in the fingerprint region, and it was attributed to the C–O stretching. In the wavenumber range of 900 cm-1 to 400 cm-1, the spectrum was quite complex and hard to observe. However, in particular, when observing the spectrum of biochar 2, some peaks could be clearly seen at 1087, 800, and 460 cm-1, which were attributed to the carbon-silicon group (C–Si) (Pankaj [42, 43]). This carbon-silicon group is often found on the husk surface and is not found in coir. The spectra of biochar 1 did not show many differences. Besides the two spectral bands observed at 3500 cm-1 and 1650 cm-1, the fingerprint region was also complex and hard to assign.


## 3.4. X-Ray Diffraction Spectroscopy (XRD) Results

The diffraction diagram of the biochars is presented in Figure5. Two wide peaks range at 2θ=22.5° and 2θ=43° and the absence of peak showing the formation of the crystal phase indicates that the BCs were amorphous carbon. In addition, the diagrams revealed the presence of graphene structure in all biochar samples. The formation of graphene structures can occur during the pyrolysis of materials derived from agricultural by-products [44]. This result is similar to the conclusions of BC diffraction studies from [44]. The diagram also showed that graphene is the only crystal structure that appears in the BCs. In other words, no crystal structure of other metals could be found on the BC samples. Many studies have also shown that silica compounds in rice husk can form crystals when the temperature reaches 800°C.Figure 5
Diffraction diagram of biochars 1 and 2.


## 3.5. Raman Spectrum

The carbon structure of biochar was also determined using Raman spectroscopy, complementing the results obtained from XRD (Figure6).Figure 6
Raman spectrum of difference BCs.Raman spectroscopy showed two main peaks at D band (1361 cm–1) and G band (1591 cm–1), corresponding to the graphene layer edge and an ideal lattice carbon, respectively [45]. Both peaks showed the presence of carbon atoms (sp2) in an aromatic compound that corresponds to the amorphous form of the benzene ring [46, 47]. Despite being different raw materials, the two biochars derived from rice husk and coir had the same shape spectrum, proving that the formation of biochar structure by pyrolisis from different agricultural by-products is the same. This result was also confirmed by the X-ray diffraction method of biochar. Biochar after pyrolysis has an amorphous form with several layers of graphene to create the porous structure of the material.


## 3.6. Surface Morphology of Biochars

Surface morphology and porous structure are important features in the adsorption process. In particular, for biochar, solids are obtained from the pyrolysis of rice husks and coir in an anaerobic environment (lack of oxygen and high pressure). The surface morphology, as well as the main surface elemental composition, was investigated by scanning electron microscopy (SEM) (Figures7 and 8) and energy dispersive X-ray emission (EDX).Figure 7
SEM images of BC1.Figure 8
SEM images of BC2.Generally, all BCs had porous meso and micropore structures with different shapes and sizes. SEM image observation of both BC types also showed the structure of the graphene layers formed along with the field structure of BC. These results also correspond to the results of [44].The SEM image of rice husk biochar (BC2) showed that it remained intact in its structure (fiber shape) of the original husk, and the pores were fairly uniform. After being broken in half, the cross-section image of BC2 revealed a series of pores with a capillary structure on the BC2 wall, about 5 to 10μm in diameter. Besides, although the mesopore structure was uneven, the micropore size was quite uniform with a diameter of approximately 50 nm.In contrast, the results for BC1 yielded a greater variety of pore sizes. Specifically, the surface morphology of biochar from coconut coir showed many pores of fairly nonuniform size with a large structure.The average percentage values of surface elemental composition in biochars, corresponding to the SEM micrographs analysis positions and dispersive spectrum are presented in Figure9 and Table 2.Figure 9
Energy dispersive spectrum corresponding to a SEM image analysis position of BC1 (a) and BC2 (b).
(a)(b)Table 2
Average mass percentage of surface elemental composition in biochar.
ComponentsBC1BC2C K (%)82.9340.27O K (%)16.7644.92Mg K (%)0.310.00Si K (%)0.0014.81Total100.00100.00The obtained results showed that the main component of all BCs was carbon, which confirmed the decomposition of cellulose, lignin, and organic matters contained in agricultural by-products at high-temperature 500-600°C. Besides, they revealed a significant content of oxygen. Combined with the results of the FTIR analysis, the oxygen content in the BCs was confirmed to come from the functional groups -COO- and -OH existing on the surface of BCs. Specifically, Si content included in the BC2 structure was consistent with the results of the FTIR analysis, indicating the bond between silicon and carbon (Si-C). However, the contents of C, O, and Si are unevenly distributed at different locations of the BCs.


## 3.7. Specific Surface Area and Pore Volume

The N2 adsorption-desorption isotherms (Figure 10) were used to determine the porosity of the BCs. The specific surface area and pore volume are significant parameters that have a strong link with the adsorption ability of the material. Micropores (diameter<2nm) and mesopores (between 2 and 50 nm) actively participate in the sorption capacity of biochar, while larger pores usually have a much smaller effect [48].Figure 10
BET-plot (a) and adsorption/desorption isotherm (b) of BC1 and BC2 in N2.
(a)(b)The BC2 had a higher microporosity compared to that of the BC1, as shown by the higher position of the corresponding isotherm and the larger slope at relative pressuresp/po above 0.1. The N2 adsorption-desorption isotherm of the BC1 exhibited type I isotherms in the IUPAC classification [49], which indicated that the microporous structure was dominant in the BC1. Meanwhile, the BC2’s isotherms exhibited type IV with a large range for the hysteresis loop. This can be explained by the capillary condensation phenomenon, whereby a gas in a pore condenses into a liquid phase at a pressure p<po of the bulk liquid [49]. This result strongly suggests that in the case of BC2, besides micropores, mesopores were also present.Table3 shows the results of total surface area (SBET) and total pore volume (VBET), estimated by the BET method, and micropore volume (VMicro) and mesopore volume (VMeso), estimated by the t-plot and BJH methods, respectively.Table 3
Parameters of specific surface area and pore of biochar.
SampleSBET (m2.g-1)VBET (cm3.g-1)Vmeso (cm3.g-1)VMicro (BET) (cm3.g-1)VMicro (DA) (cm3.g-1)BC1329.70.170.030.140.21BC2364.20.260.140.150.26TheSBET of BC2 was higher than that of BC1 (364.2 m2.g-1 vs. 329.7 m2.g-1). Similarly, the pore volume of BC2 was 0.26 cm3.g-1 compared to 0.17 cm3.g-1 for BC1. Compared to other biomass chars produced under similar carbonization conditions, such as fern char [50] or cashew nutshell char [51], BCs produced in this study achieved higher porosity levels. The VMicro (estimated by BET technique) of BC1 and BC2 is similar. However, the large size of the N2 molecules prevents them from entering the ultra-micropores, i.e., pores with diameters less than 1 nm. Therefore, CO2 adsorption/desorption was performed to fully reflect the microporous structures of these BCs (Figure 11).Figure 11
DA-plot (a) and adsorption/desorption isotherm (b) of BC1 and BC2 in CO2.
(a)(b)The adsorption/desorption isotherm plot of CO2 of BC2 is above that of BC1, indicating a higher micropore volume. Moreover, both isotherms showed hysteresis at low-pressure. This indicates that the CO2 molecules were in a metastable state, and the gas was not readily released at the level corresponding to the value of thermodynamic equilibrium at pressure decrease [52]. In other words, both BCs exhibited heterogeneous surface properties with bottleneck shapes at the micropore entrance. This pore shape is known to be favorable for long particule capture.TheVMicro (estimated by DA method) reached 0.26 cm3.g-1 for BC2 and 0.21 cm3.g-1 for BC1. The smaller kinetic diameter of CO2 (0.3 nm) compared to N2 (0.36 nm) gave a much higher VMicro calculated by the DA method than by the t-plot method. This indicates that the microporous structures were better developed in rice husk biochar than in coir biochar.


## 3.8. Biochar Adsorbability

### 3.8.1. General Evaluation of BC1 Adsorbability with Methylene Blue (MB)

Evaluation of the effect of pH on biochar 1 adsorbability of methylene blue was first performed. Experiments were carried out to evaluate the effect of varying pH values of dye solution on the ability of biochar to adsorb methylene blue ions. The results are shown in Figure12.Figure 12
Evaluation of the effect of pH on biochar 1 (5 g.L-1) adsorbability of methylene blue ions.The effect of pH on methylene blue adsorption was not significant for biochar 1 as there was little difference between the three efficiency lines. AtpH=2, the adsorbability of BC1 was however slightly weaker than at other pH values for the first hours of the time series, which accurately reflects the point of zero charge principle. The difference between the efficiency lines of BC1 was more distinct for the efficiency lines at pH=2 and at other pH values. The efficiency reached 66% at pH 2 and 87% at both pH 6 and pH 12 after 30 minutes of adsorption. When the adsorption time was increased to 1 hour, the adsorption efficiency showed similar differences, 87% at pH 2 and 94% at the other two pH values. It was found that dye adsorption increases with pH, with a maximum adsorption at pH 6. This could be due to the fact that the surface of the adsorbent becomes negative at higher pH values, favoring the adsorption of positively charged MB cationic dye via electrostatic attraction. Moreover, there is a slight reduction in adsorption at pH 12 due to the repulsion of adsorbent surface and the existence of a partial negative charge (Cl-) on MB [42].


### 3.8.2. Evaluation of the Effect of Biochar Dosage on Adsorbability with Methylene Blue

The effect of varying biochar concentration on the adsorption of dye ions on the biochar surface was studied with methylene blue. The results are given in Figure13.Figure 13
Evaluation of the effect of biochar 1 dosage on adsorbability.As expected, the higher the biochar concentration, the better the adsorbability. However, the differences are not really significant. Based on these results, a catalyst concentration of 5 g.L-1 was selected for further studies.


### 3.8.3. Evaluation of the Effect of pH on Biochar Adsorbability with Methyl Orange

The laboratory–synthesized biochar BC1 was studied for its ability to remove not only methylene blue but also methyl orange, an anionic dye. The results are shown in Figure14.Figure 14
Evaluation of the effect of pH on biochar 1 (5 g.L-1) adsorbability of methyl orange.At pH 2, it took less than an hour to reach 80% efficiency, and after 5 hours, biochar 1 had removed over 96% of the MO in the solution. In contrast, the efficiency of dye removal at pH 6 and 12 was approximately half that at pH 2, 49%, and 47%, respectively. At pH 6 and pH 12, the surface was, respectively, neutral and positively charged; therefore; adsorption efficiency is much lower.In addition to the electrostatic interaction following the PZC principle, many functional groups exist on the biochar surface and bind to methylene blue or methyl orange, thus, facilitating the adsorption on the biochar surface. When the pH of the solution was decreased significantly, the positive surface charge of the BC increased and, consequently, the adsorption of methyl orange anions on the BC surface increased significantly. On the contrary, when the pH of the solution was increased, the adsorption of methyl orange on BC1 decreased due to the repulsive force between the adsorbent and the negatively charged adsorbate. However, the adsorption of methylene blue at high pH was enhanced due to the strong electrostatic interaction between the cationic groups of MB molecule and the negatively charged BC surface. Therefore, this could be the main mechanism of the adsorption. The results showed that the highest adsorption efficiency of BC was obtained at basic pH values for MB and at acidic pH for MO.In consequence, the influence of the two different biochars on dye adsorbability was investigated at pH 6 for MB and at pH 2 for MO (Figure15).Figure 15
Effect of two different biochars on adsorbability of dyes molecules.Figure15 clearly demonstrates that the adsorption of BC2 was superior to that of BC1 under the same conditions with a peak efficiency of nearly 100%. This difference is also partly due to the physical characteristics of the adsorbent. BC2 is derived from the rice husk with a much higher number of pores than BC1 which is coconut coir. It has both meso and micropores, so the total BET and total porous volume of BC2 are larger than BC1, 364.22m2.g−1>329.71m2.g−1 and 0.26m2.g−1>0.17m2.g−1.Moreover, biochar 2 has a relatively high microporous and mesoporous area, 0.15 cm3.g1 and 0. 14 cm3.g-1 compared to 0.14 cm3.g-1 and 0.03 cm3.g-1 for biochar 1, respectively. Apart from those factors, these two types of biochar had similar surface functional groups, and the only difference was the silicon components found in BC2.The MB adsorption efficiency of BC1 was close to 94%, much higher than that of MO (about 82%) after 1 hour of the reaction. BC2 also showed a similar trend with the adsorption efficiency slightly higher for MB than for MO, about 100% and 96%, respectively. Both materials had better electronic interactions with MB than with MO. This suggested that the adsorption capacity of both biochars was more efficient for MB than for MO. Considering the physicochemical properties of the adsorbent surface, although MO (1.31×0.55×0.18nm) has a smaller molecular size than MB (1.26×0.77×0.65nm), which means that MO molecules were able to enter the pores and being retained in more micro and mesopores; however, MB ions were more selectively adsorbed.This result is consistent with the study of Phuong et al. [53] who obtained an average surface area including micropore and mesopore of rice husk–derived biochar of 118 m2.g-1. Since the volume of mesopore was quite small and most of the pore volume was micropore, MB ions took longer to be adsorbed into the BCA pores, so the adsorbability rate was slowed down. In our study, the dye adsorption rate of BC1 was slower than that of BC2 because BC2 had a larger BET volume and much larger pore volume, as mentioned above. Both dyes can be completely adsorbed.


### 3.8.4. Isothermal Adsorption

The results of the physicochemical characteristics analysis showed that BC2 had a higher adsorption capacity than BC1 due to its larger surface area and pore volume, a larger number of surface functional groups, and a lower pH of PZC. Therefore, the adsorption isotherm of MB and MO adsorption was also evaluated through two popular adsorption models, Langmuir and Freundlich isotherm models. Figure16 shows the isotherm of MB and MO adsorption on BC1 material according to Langmuir and Freundlich models.Figure 16
Langmuir (a) and Freundlich (b) adsorption isotherm model fittings for the adsorption of MB and MO on BC1 and BC2 at 25°C.
(a)(b)The parameters of Langmuir and Freundlich adsorption isotherms were calculated from the slope values and the vertical cut and are presented in Table4.Table 4
The adsorption isotherm of MO and MB adsorbed on BC2 and BC2 materials according to Langmuir and Freundlich models.
ModelParametersMBMOBC1BC2BC1BC2Langmuir isotherm parametersR20.9220.9940.9910.969qmax (mg.g-1)6.4188.6123.0806.519B (L.mg-1)0.6932.4451.6311.153Freundlich isotherm parametersR20.9920.3650.6720.988KF[(mg.g-1) (L.mg-1)]n2.0674.8341.8012.536n2.1293.9782.6942.268Langmuir and Freundlich adsorption isotherms are two chemisorption models in which Langmuir is a monolayer adsorption process while Freundlich describes a multilayer adsorption capacity of the material.The results demonstrated that the adsorption capacity of BC2 followed both Langmuir and Freundlich models with MO adsorbent. The regression coefficientsR2 were both high (0.97 and 0.99 for Langmuir and Freundlich, respectively), revealing that the adsorption process follows both models. In contrast, with the MB adsorbent, the adsorption isotherm followed the Langmuir model with a regression coefficient of 0.99. For BC1 adsorption, MO followed the Langmuir model with R2 of 0.99 and MB followed Freundlich with the same R2 value. Overall, in this study, the dye removal efficiency of BC2 was higher than that of BC1, both following the Langmuir and Freundlich isotherm models.Remind that the Freundlich model suggests multilayer physisorption on the surface of the material with different adsorption energy levels whereas the Langmuir model proposes monolayer chemisorption by the donor-acceptor interaction based on electrophilic addition [54, 55]. This was because the charge-rich carbonized surface created bonds with protonated amino groups in the acidic medium. In addition, H-H and H-O bonding between the carbon-silicon group on the surface of biochar with the phenolic group of dye molecules could also be able to occur [56].Rodriguez also indicated that the mechanism of dye adsorption on biochars may be classified into two types of interactions: nonelectrostatic and electrostatic. Adsorption is affected by the pH of the solution as well as the pHPZC. Therefore, at pH<pHpzc, the surface of the biochar is positively charged, promoting anionic species adsorption, and negatively charged at pH>pHpzc, favoring cationic species adsorption [57]. Furthermore, all biochar samples had pHpzc values of 8 and 9 for BC1 and BC2, respectively, higher than the pH values of MB (6.0) and MO (2) solutions. Biochar has a positive charge, MB is a cation dye that has a positive charge when dissolved in water, and MO is an anion dye that becomes negatively charged when dissolved in water. The adsorption mechanism is therefore dominated by the dispersion interaction between the dissociated electrons on the surface of the activated carbon and the free electrons of the dye molecule contained in the aromatic ring [58].TheRL separation factor values for dye adsorption on the particular adsorbent were all positive and less than unity in all cases, suggesting extremely favorable adsorption under all circumstances. This is furthermore consistent with the results for the 1/nF values, which were less than unity, suggesting that the dye is preferentially absorbed by biochar.In terms of the maximum adsorption capacity of a material, BC2 adsorbs both dyes well and better than BC1 with aqmax value of 8.612 mg.g-1 and 6.519 mg.g-1 for MB and MO, respectively. These values are was quite low compared to that of various adsorbents, such as bamboo-activated carbon [59], pea shells [60], modified clay-ball [61], and activated biochar derived from wakame [62]. However, biochars prepared with a particle size of 1-2 mm for coir and 5 mm for rice husk are more ecologically friendly and economically effective compared to other adsorbents. First, the granular nature of the adsorbent is useful since it can be easily separated after filtration and sedimentation without creating sludge. Second, in terms of recycling, using an agricultural by-product allows waste to be a valued resource to reduce environmental risks [12].


## 3.8.1. General Evaluation of BC1 Adsorbability with Methylene Blue (MB)

Evaluation of the effect of pH on biochar 1 adsorbability of methylene blue was first performed. Experiments were carried out to evaluate the effect of varying pH values of dye solution on the ability of biochar to adsorb methylene blue ions. The results are shown in Figure12.Figure 12
Evaluation of the effect of pH on biochar 1 (5 g.L-1) adsorbability of methylene blue ions.The effect of pH on methylene blue adsorption was not significant for biochar 1 as there was little difference between the three efficiency lines. AtpH=2, the adsorbability of BC1 was however slightly weaker than at other pH values for the first hours of the time series, which accurately reflects the point of zero charge principle. The difference between the efficiency lines of BC1 was more distinct for the efficiency lines at pH=2 and at other pH values. The efficiency reached 66% at pH 2 and 87% at both pH 6 and pH 12 after 30 minutes of adsorption. When the adsorption time was increased to 1 hour, the adsorption efficiency showed similar differences, 87% at pH 2 and 94% at the other two pH values. It was found that dye adsorption increases with pH, with a maximum adsorption at pH 6. This could be due to the fact that the surface of the adsorbent becomes negative at higher pH values, favoring the adsorption of positively charged MB cationic dye via electrostatic attraction. Moreover, there is a slight reduction in adsorption at pH 12 due to the repulsion of adsorbent surface and the existence of a partial negative charge (Cl-) on MB [42].


## 3.8.2. Evaluation of the Effect of Biochar Dosage on Adsorbability with Methylene Blue

The effect of varying biochar concentration on the adsorption of dye ions on the biochar surface was studied with methylene blue. The results are given in Figure13.Figure 13
Evaluation of the effect of biochar 1 dosage on adsorbability.As expected, the higher the biochar concentration, the better the adsorbability. However, the differences are not really significant. Based on these results, a catalyst concentration of 5 g.L-1 was selected for further studies.


## 3.8.3. Evaluation of the Effect of pH on Biochar Adsorbability with Methyl Orange

The laboratory–synthesized biochar BC1 was studied for its ability to remove not only methylene blue but also methyl orange, an anionic dye. The results are shown in Figure14.Figure 14
Evaluation of the effect of pH on biochar 1 (5 g.L-1) adsorbability of methyl orange.At pH 2, it took less than an hour to reach 80% efficiency, and after 5 hours, biochar 1 had removed over 96% of the MO in the solution. In contrast, the efficiency of dye removal at pH 6 and 12 was approximately half that at pH 2, 49%, and 47%, respectively. At pH 6 and pH 12, the surface was, respectively, neutral and positively charged; therefore; adsorption efficiency is much lower.In addition to the electrostatic interaction following the PZC principle, many functional groups exist on the biochar surface and bind to methylene blue or methyl orange, thus, facilitating the adsorption on the biochar surface. When the pH of the solution was decreased significantly, the positive surface charge of the BC increased and, consequently, the adsorption of methyl orange anions on the BC surface increased significantly. On the contrary, when the pH of the solution was increased, the adsorption of methyl orange on BC1 decreased due to the repulsive force between the adsorbent and the negatively charged adsorbate. However, the adsorption of methylene blue at high pH was enhanced due to the strong electrostatic interaction between the cationic groups of MB molecule and the negatively charged BC surface. Therefore, this could be the main mechanism of the adsorption. The results showed that the highest adsorption efficiency of BC was obtained at basic pH values for MB and at acidic pH for MO.In consequence, the influence of the two different biochars on dye adsorbability was investigated at pH 6 for MB and at pH 2 for MO (Figure15).Figure 15
Effect of two different biochars on adsorbability of dyes molecules.Figure15 clearly demonstrates that the adsorption of BC2 was superior to that of BC1 under the same conditions with a peak efficiency of nearly 100%. This difference is also partly due to the physical characteristics of the adsorbent. BC2 is derived from the rice husk with a much higher number of pores than BC1 which is coconut coir. It has both meso and micropores, so the total BET and total porous volume of BC2 are larger than BC1, 364.22m2.g−1>329.71m2.g−1 and 0.26m2.g−1>0.17m2.g−1.Moreover, biochar 2 has a relatively high microporous and mesoporous area, 0.15 cm3.g1 and 0. 14 cm3.g-1 compared to 0.14 cm3.g-1 and 0.03 cm3.g-1 for biochar 1, respectively. Apart from those factors, these two types of biochar had similar surface functional groups, and the only difference was the silicon components found in BC2.The MB adsorption efficiency of BC1 was close to 94%, much higher than that of MO (about 82%) after 1 hour of the reaction. BC2 also showed a similar trend with the adsorption efficiency slightly higher for MB than for MO, about 100% and 96%, respectively. Both materials had better electronic interactions with MB than with MO. This suggested that the adsorption capacity of both biochars was more efficient for MB than for MO. Considering the physicochemical properties of the adsorbent surface, although MO (1.31×0.55×0.18nm) has a smaller molecular size than MB (1.26×0.77×0.65nm), which means that MO molecules were able to enter the pores and being retained in more micro and mesopores; however, MB ions were more selectively adsorbed.This result is consistent with the study of Phuong et al. [53] who obtained an average surface area including micropore and mesopore of rice husk–derived biochar of 118 m2.g-1. Since the volume of mesopore was quite small and most of the pore volume was micropore, MB ions took longer to be adsorbed into the BCA pores, so the adsorbability rate was slowed down. In our study, the dye adsorption rate of BC1 was slower than that of BC2 because BC2 had a larger BET volume and much larger pore volume, as mentioned above. Both dyes can be completely adsorbed.


## 3.8.4. Isothermal Adsorption

The results of the physicochemical characteristics analysis showed that BC2 had a higher adsorption capacity than BC1 due to its larger surface area and pore volume, a larger number of surface functional groups, and a lower pH of PZC. Therefore, the adsorption isotherm of MB and MO adsorption was also evaluated through two popular adsorption models, Langmuir and Freundlich isotherm models. Figure16 shows the isotherm of MB and MO adsorption on BC1 material according to Langmuir and Freundlich models.Figure 16
Langmuir (a) and Freundlich (b) adsorption isotherm model fittings for the adsorption of MB and MO on BC1 and BC2 at 25°C.
(a)(b)The parameters of Langmuir and Freundlich adsorption isotherms were calculated from the slope values and the vertical cut and are presented in Table4.Table 4
The adsorption isotherm of MO and MB adsorbed on BC2 and BC2 materials according to Langmuir and Freundlich models.
ModelParametersMBMOBC1BC2BC1BC2Langmuir isotherm parametersR20.9220.9940.9910.969qmax (mg.g-1)6.4188.6123.0806.519B (L.mg-1)0.6932.4451.6311.153Freundlich isotherm parametersR20.9920.3650.6720.988KF[(mg.g-1) (L.mg-1)]n2.0674.8341.8012.536n2.1293.9782.6942.268Langmuir and Freundlich adsorption isotherms are two chemisorption models in which Langmuir is a monolayer adsorption process while Freundlich describes a multilayer adsorption capacity of the material.The results demonstrated that the adsorption capacity of BC2 followed both Langmuir and Freundlich models with MO adsorbent. The regression coefficientsR2 were both high (0.97 and 0.99 for Langmuir and Freundlich, respectively), revealing that the adsorption process follows both models. In contrast, with the MB adsorbent, the adsorption isotherm followed the Langmuir model with a regression coefficient of 0.99. For BC1 adsorption, MO followed the Langmuir model with R2 of 0.99 and MB followed Freundlich with the same R2 value. Overall, in this study, the dye removal efficiency of BC2 was higher than that of BC1, both following the Langmuir and Freundlich isotherm models.Remind that the Freundlich model suggests multilayer physisorption on the surface of the material with different adsorption energy levels whereas the Langmuir model proposes monolayer chemisorption by the donor-acceptor interaction based on electrophilic addition [54, 55]. This was because the charge-rich carbonized surface created bonds with protonated amino groups in the acidic medium. In addition, H-H and H-O bonding between the carbon-silicon group on the surface of biochar with the phenolic group of dye molecules could also be able to occur [56].Rodriguez also indicated that the mechanism of dye adsorption on biochars may be classified into two types of interactions: nonelectrostatic and electrostatic. Adsorption is affected by the pH of the solution as well as the pHPZC. Therefore, at pH<pHpzc, the surface of the biochar is positively charged, promoting anionic species adsorption, and negatively charged at pH>pHpzc, favoring cationic species adsorption [57]. Furthermore, all biochar samples had pHpzc values of 8 and 9 for BC1 and BC2, respectively, higher than the pH values of MB (6.0) and MO (2) solutions. Biochar has a positive charge, MB is a cation dye that has a positive charge when dissolved in water, and MO is an anion dye that becomes negatively charged when dissolved in water. The adsorption mechanism is therefore dominated by the dispersion interaction between the dissociated electrons on the surface of the activated carbon and the free electrons of the dye molecule contained in the aromatic ring [58].TheRL separation factor values for dye adsorption on the particular adsorbent were all positive and less than unity in all cases, suggesting extremely favorable adsorption under all circumstances. This is furthermore consistent with the results for the 1/nF values, which were less than unity, suggesting that the dye is preferentially absorbed by biochar.In terms of the maximum adsorption capacity of a material, BC2 adsorbs both dyes well and better than BC1 with aqmax value of 8.612 mg.g-1 and 6.519 mg.g-1 for MB and MO, respectively. These values are was quite low compared to that of various adsorbents, such as bamboo-activated carbon [59], pea shells [60], modified clay-ball [61], and activated biochar derived from wakame [62]. However, biochars prepared with a particle size of 1-2 mm for coir and 5 mm for rice husk are more ecologically friendly and economically effective compared to other adsorbents. First, the granular nature of the adsorbent is useful since it can be easily separated after filtration and sedimentation without creating sludge. Second, in terms of recycling, using an agricultural by-product allows waste to be a valued resource to reduce environmental risks [12].


## 4. Conclusions

Biochars derived from agricultural by-products including coconut coir and rice husk were successfully produced in large quantity, homogenized following the calcination process, and then activated byH 25%. The biochars had a high specific surface area of 364.22 m2.g-1 and 329.71 m2.g-1 for rice husk and coconut coir biochars, respectively. All biochars had micro and mesopore structures but with different amounts. SEM images as well as XRD and Raman analysis of different biochars also showed various graphene layers with an amorphous structure. These results suggest that the biochar obtained in this study could have a high adsorbability for small to large molecules. Indeed, both biochar BC1 and BC2 showed good adsorption ability for MB and MO. In addition, BC2 had a better performance in dye adsorption than BC1.The results of adsorption isotherm experiments indicated BC2 material followed Langmuir and Freundlich isotherms when adsorbing MO with a maximal adsorption volume of 6.519 mg.g-1. In the case of MB adsorption, BC2 only followed the Langmuir isotherm with a maximal adsorption volume of 8.612 mg.g-1. On the contrary, BC1 adsorbed MB following the Freundlich isotherm while its MO adsorption followed the Langmuir isotherm. In general, the agricultural by-products can be reused after treatment as adsorbers for persistent organic pollutants, including those found in wastewater from the textile industry.



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*Source: 9161904-2021-11-11.xml*