Anionic Dye Removal Using a Date Palm Seed-Derived Activated Carbon/Chitosan Polymer Microbead Biocomposite

The discharge of textile wastewater into aquatic streams is considered a major challenge due to its effect on the water ecosystem. Direct blue 78 (DB78) dye has a complex structure. Therefore, it is difficult to separate it from industrial wastewater. In this study, carbon obtained from the pyrolysis of mixed palm seeds under different temperatures (400 °C and 1000 °C) was activated by a thermochemical method by using microwave radiation and an HCl solution in order to improve its adsorption characteristics. The generated activated carbon was used to synthesize a novel activated carbon/chitosan microbead (ACMB) for dye removal from textile wastewater. The obtained activated carbon (AC) was characterized by a physicochemical analysis that included, namely, particle size, zeta potential, SEM, EDX, and FTIR analyses. A series of batch experiments were conducted in terms of the ACMB dose, contact time, pH, and activated carbon/chitosan ratios in synthetic microbeads for enhancing the adsorption capacity. A remarkable improvement in the surface roughness was observed using SEM analysis. The particle surface was transformed from a slick surface with a minor-pore structure to a rough surface with major-pore structure. The zeta potential analysis indicated a higher improvement in the carbon surface charge, from −35 mv (before activation) to +20 mv (after activation). The adsorption tests showed that the dye-removal efficiency increased with the increasing adsorbent concentration. The maximum removal efficiencies were 97.8% and 98.4% using 3 and 4 g/L of AC400°C MB-0.3:1 and AC1000°C MB-0.3:1, respectively, with initial dye concentrations of 40 mg/L under acidic conditions (pH = 4–5), and an optimal mixing time of 50 min. The equilibrium studies for AC400°C MB-0.3:1 and AC1000°C MB-0.3:1 showed that the equilibrium data best fitted to the Langmuir isothermal model with R2 = 0.99. These results reveal that activated carbon/chitosan microbeads are an effective adsorbent for the removal of direct blue 78 dye and provide a new platform for dye removal.


Introduction
Water is considered the most effective and central substance in human life. Due to its major applications in various industries, water is exposed to several pollutants and can therefore be contaminated. In recent years, water pollution has become a major threat to water ecology, and thus the extraction of pollutants from industrial wastewater before discharging into water streams is essential [1]. Industrial wastewater mostly contains organic Two carbon samples, obtained from the pyrolysis of mixed date palm seeds (DPS) under temperatures of 400 °C and 1000 °C, were used in this study [31]. The carbon samples were placed into 400 mL distilled water. The solution was stirred 4 h with a mixing speed of 200 RPM at 30 °C. Samples were washed, filtered using a Whatman filter paper, and left to dry at 110 °C for 12 h using a thermal dryer. In order to activate the carbon, the samples were subjected to a microwave-chemical-activation process. These samples were activated by immersing 15 g of carbon into 250 mL of an HCl solution, with a concentration of 7% wt/wt, and then the solution was placed into a domestic microwave (frequency: 2.45 GHz; power: 600 W) for a contact time of 6 min. At the end of the activation process, the mixture was filtrated using a Whatman filter paper, washed using distilled water, and left to dry at 110 °C for 24 h. Physical and chemical analyses were conducted to characterize the activated carbon.

Chitosan and Dye
Chitosan is an amino-based polymer that is synthesized in vast amounts by the Ndeacetylation of chitin. The characteristics of the chitosan used in this study are a white powder with a molecular weight range from 140 to 220 kDa, a degree of deacetylation (DAC) = 81.2%, viscosity = 36,000 cps, and a density of 0.15 g/mL. The chemical structure of chitosan is shown in Figure 1a.
The direct blue 78 (DB78) dye had a relative molecular mass of 1059.95, a maximum wavelength of λmax = 604 nm, and solubility up to 10 g/L at 25 °C. The direct blue 78 was selected for adsorption tests as it is widely used in the textile industry. The chemical structure of direct blue 78 is shown in Figure 1b.

Preparation of Activated Carbon/Chitosan Microbeads (ACMB)
Activated carbon/chitosan microbeads (ACMB) with different ratios of activated carbon to chitosan were synthesized. In ACmMB-z, m and z refer to the pyrolysis temperatures for carbon extraction (400 °C and 1000 °C) and the ratio of AC to chitosan, respectively. The adsorption studies were conducted using polymer-based composite materials with different mixing ratios: ACmMB-0.1:1, ACmMB-0.2:1, ACmMB-0.3:1, ACmMB-0.4:1, and ACmMB-0.5:1. In AC400°C MB-0.3:1, the chitosan solution was prepared under magnetic stirring for 3 h by dissolving 1.5 g (1.5 wt.%) of chitosan powder in diluted acetic acid to The direct blue 78 (DB78) dye had a relative molecular mass of 1059.95, a maximum wavelength of λ max = 604 nm, and solubility up to 10 g/L at 25 • C. The direct blue 78 was selected for adsorption tests as it is widely used in the textile industry. The chemical structure of direct blue 78 is shown in Figure 1b.

Preparation of Activated Carbon/Chitosan Microbeads (ACMB)
Activated carbon/chitosan microbeads (ACMB) with different ratios of activated carbon to chitosan were synthesized. In AC m MB-z, m and z refer to the pyrolysis temperatures for carbon extraction (400 • C and 1000 • C) and the ratio of AC to chitosan, respectively. The adsorption studies were conducted using polymer-based composite materials with different mixing ratios: AC m MB-0.1:1, AC m MB-0.2:1, AC m MB-0.3:1, AC m MB-0.4:1, and AC m MB-0.5:1. In AC 400 • C MB-0.3:1, the chitosan solution was prepared under magnetic stirring for 3 h by dissolving 1.5 g (1.5 wt.%) of chitosan powder in diluted acetic acid to form 100 mL of chitosan hydrogel. A total of 450 mg from activated carbon (pyrolysis temperature: 400 • C), representing 0.45 wt.%, was added to the formed hydrogel (45 mg of AC was added to 10 mL of chitosan hydrogel under magnetic stirring for 4 h and a temperature of 60 • C). The final prepared gel was dropped into a 0.7 M NaOH solution (contact time: 3 h) using a micropipette to form the beads. The formed beads were then washed using distilled water. Finally, the beads were oven-dried at 60 • C. The preparation process is illustrated in Figure 2.
form 100 mL of chitosan hydrogel. A total of 450 mg from activated carbon (pyrolysis temperature: 400 °C), representing 0.45 wt.%, was added to the formed hydrogel (45 mg of AC was added to 10 mL of chitosan hydrogel under magnetic stirring for 4 h and a temperature of 60 °C). The final prepared gel was dropped into a 0.7 M NaOH solution (contact time: 3 h) using a micropipette to form the beads. The formed beads were then washed using distilled water. Finally, the beads were oven-dried at 60 °C. The preparation process is illustrated in Figure 2.

Adsorption Studies
This study was conducted using the batch adsorption system (lab scale) on singlecomponent synthetic wastewater. The activated carbon/chitosan microbead dose used in this study was 0.5-6.5 g. Synthetic wastewater with an initial concentration of 40 mg/L was mixed with ACMB at 200 RPM for the contact time (0-100) minimum at room temperature (25 ± 2 °C). The spectrophotometrically analysis was applied to determine the removal efficiency by measuring the dye concentration before and after the adsorption process at λmax = 600 nm for DB78, as given in Equation (1): Equilibrium loading can be determined by using Equation (2): where Co and C are the initial and equilibrium concentrations of pollutant, respectively; V is the volume of solution (L); and m is the quantity of adsorbent (g).

Characterization of Materials
The activated carbon suspension was diluted in water and sonicated for 30 min in an ultrasonic bath at 4% (w/v). Model USC-1400 is one of a kind (40 kHz of ultrasound frequency). The Malvern 3000 Zetasizer NanoZS (Malvern Instruments, Malvern, UK) was used to measure the average particle size of produced activated carbon at 400 °C and 1000 °C. It measures the diffusion of particles moving under Brownian motion, and it translates the data to size and size distribution using dynamic light scattering. It is also used in laser doppler microelectrophoresis to provide an electric field to a dispersion of particles, which then move at a rate proportional to their zeta potential. The Smoluchowski algorithm was used to determine the particle size. Prior to adsorption studies, the samples were degasified at 200 °C for 4 h, and then the surface area was measured in the presence of N2 adsorption at −195.65 °C using surface-area analyzers (Autosorb-l-C-8, Quantachrome,

Adsorption Studies
This study was conducted using the batch adsorption system (lab scale) on singlecomponent synthetic wastewater. The activated carbon/chitosan microbead dose used in this study was 0.5-6.5 g. Synthetic wastewater with an initial concentration of 40 mg/L was mixed with ACMB at 200 RPM for the contact time (0-100) minimum at room temperature (25 ± 2 • C). The spectrophotometrically analysis was applied to determine the removal efficiency by measuring the dye concentration before and after the adsorption process at λ max = 600 nm for DB78, as given in Equation (1): Equilibrium loading can be determined by using Equation (2): where C O and C are the initial and equilibrium concentrations of pollutant, respectively; V is the volume of solution (L); and m is the quantity of adsorbent (g).

Characterization of Materials
The activated carbon suspension was diluted in water and sonicated for 30 min in an ultrasonic bath at 4% (w/v). Model USC-1400 is one of a kind (40 kHz of ultrasound frequency). The Malvern 3000 Zetasizer NanoZS (Malvern Instruments, Malvern, UK) was used to measure the average particle size of produced activated carbon at 400 • C and 1000 • C. It measures the diffusion of particles moving under Brownian motion, and it translates the data to size and size distribution using dynamic light scattering. It is also used in laser doppler microelectrophoresis to provide an electric field to a dispersion of particles, which then move at a rate proportional to their zeta potential. The Smoluchowski algorithm was used to determine the particle size. Prior to adsorption studies, the samples were degasified at 200 • C for 4 h, and then the surface area was measured in the presence of N 2 adsorption at −195.65 • C using surface-area analyzers (Autosorb-l-C-8, Quantachrome, Boynton Beach, FL, USA). By applying the BET (Brunauer-Emmett-Teller) equation to the adsorption data, the BET surface area for the sample was determined.
FTIR studies for all samples were conducted using a VERTEX 80v vacuum FTIR Spectrometer, Bruker corporation, Germany. The surface morphology and porous microstructure of samples were investigated by SEM analysis (TESCAN MIRA-High Resolution scanning electron microscope, Tescan Essence company, Brno, Czech Republic).
Surface morphology and elemental analysis were performed using field-emission scanning electron microscopy (TESCAN MIRA-High Resolution scanning electron microscope, Tescan Essence company, Brno, Czech Republic) coupled with an energy-dispersive X-ray (EDX) (Oxford instrument nano analysis detector, UK).
The colorimetric analysis was carried out in this study using a LAMOTTE smart spectrophotometer v3 2000-01-MN, Washington Ave. Chestertown, MD, USA.

Characterization of Adsorbents
The adsorbent samples were characterized by using a zeta sizer to measure the particle size. The zeta potential was used to measure the carbon particles' net surface charge, and BET analysis was conducted to determine the surface area. The surface morphology was investigated by using SEM analysis. The elemental analysis was studied by using EDX analysis. The chemical function groups were determined by using FTIR analysis.

Zeta Sizer Analysis
Due to its major effect and great influence on the adsorption process, the particle size distribution of activated carbon was investigated. Figure 3 shows that 96.5% of the AC 400 (activated carbon from a pyrolysis temperature of 400 • C) had average particle sizes less than 1.6 µm. For the AC 1000 • C (activated carbon from a pyrolysis temperature of 1000 • C), 97.5% of the particle sizes were less than 1.2 µm. It was reported that there is an inverse relationship between the particle size and the adsorption capacity. The smaller the particle size, the higher the available surface area, which leads to a maximum adsorption capacity [32].
adsorption data, the BET surface area for the sample was determined.
FTIR studies for all samples were conducted using a VERTEX 80v vacuum FTIR Spectrometer, Bruker corporation, Germany. The surface morphology and porous microstructure of samples were investigated by SEM analysis (TESCAN MIRA-High Resolution scanning electron microscope, Tescan Essence company, Brno, Czech Republic).
Surface morphology and elemental analysis were performed using field-emission scanning electron microscopy (TESCAN MIRA-High Resolution scanning electron microscope, Tescan Essence company, Brno, Czech Republic) coupled with an energy-dispersive X-ray (EDX) (Oxford instrument nano analysis detector, UK) The colorimetric analysis was carried out in this study using a LAMOTTE smart spectrophotometer v3 2000-01-MN, Washington Ave. Chestertown, MD, USA.

Characterization of Adsorbents
The adsorbent samples were characterized by using a zeta sizer to measure the particle size. The zeta potential was used to measure the carbon particles' net surface charge, and BET analysis was conducted to determine the surface area. The surface morphology was investigated by using SEM analysis. The elemental analysis was studied by using EDX analysis. The chemical function groups were determined by using FTIR analysis.

Zeta Sizer Analysis
Due to its major effect and great influence on the adsorption process, the particle size distribution of activated carbon was investigated. Figure 3 shows that 96.5% of the AC400 (activated carbon from a pyrolysis temperature of 400 °C) had average particle sizes less than 1.6 µm. For the AC1000 o C (activated carbon from a pyrolysis temperature of 1000 °C), 97.5% of the particle sizes were less than 1.2 µm. It was reported that there is an inverse relationship between the particle size and the adsorption capacity. The smaller the particle size, the higher the available surface area, which leads to a maximum adsorption capacity [32].

Zeta Potential Analysis
It was observed from the zeta potential analysis that the activation process using the HCl solution and microwave radiation has a remarkable effect on the surface charge of

Zeta Potential Analysis
It was observed from the zeta potential analysis that the activation process using the HCl solution and microwave radiation has a remarkable effect on the surface charge of carbon particles. As illustrated in Figure 4a,b, carbon produced at high temperatures (1000 • C) has very hydrophobic behavior. However, due to the dehydration and deoxygenation of the palm seeds, it has reduced amounts of H-and O-containing functional groups. Surface groups can act as electron donors or acceptors, resulting in the creation of coexisting zones with a variety of characteristics that range from acidic to basic and from hydrophilic to hydrophobic. As a result, the ion-exchange capacity of carbon particles may be reduced. Biochar generated at lower temperatures (400 • C) has a more varied organic character due to the presence of aliphatic and cellulose-type structures. As a result, biochar's structure looks to have less surface-functional-group content as the temperature increases. The surface charges of carbon particles were +5 mv and −35 mv, respectively, for carbon at 400 • C and 1000 • C. Figure 4a,b shows that the activation of carbon particles using acidic solution led to an increase in the positive charge to +30 mv and +20 mv for AC 400 • C and AC 1000 • C , respectively. This improvement in the surface charge is attributed to the accumulation of hydrogen ions (H + ) on the activated carbon particle surface after the thermochemical modification process using microwave radiation and the HCl solution (chemical agent). °C) has very hydrophobic behavior. However, due to the dehydration and deoxygenation of the palm seeds, it has reduced amounts of H-and O-containing functional groups. Surface groups can act as electron donors or acceptors, resulting in the creation of coexisting zones with a variety of characteristics that range from acidic to basic and from hydrophilic to hydrophobic. As a result, the ion-exchange capacity of carbon particles may be reduced. Biochar generated at lower temperatures (400 °C) has a more varied organic character due to the presence of aliphatic and cellulose-type structures. As a result, biochar's structure looks to have less surface-functional-group content as the temperature increases. The surface charges of carbon particles were +5 mv and −35 mv, respectively, for carbon at 400 °C and 1000 °C. Figure 4a,b shows that the activation of carbon particles using acidic solution led to an increase in the positive charge to +30 mv and +20 mv for AC400°C and AC1000°C, respectively. This improvement in the surface charge is attributed to the accumulation of hydrogen ions (H + ) on the activated carbon particle surface after the thermochemical modification process using microwave radiation and the HCl solution (chemical agent).

Energy-Dispersive X-ray (EDX) Analysis
In order to determine the carbon content and presence of different elements in the two types of activated carbon samples (AC400°C and AC1000°C), the energy-dispersive X-ray

Energy-Dispersive X-ray (EDX) Analysis
In order to determine the carbon content and presence of different elements in the two types of activated carbon samples (AC 400 • C and AC 1000 • C ), the energy-dispersive X-ray (EDX) analysis was conducted. Figure 5a shows peaks at~0.2, 1.2, 2, and 3.5 KeV. These peaks are attributed to carbon (C), magnesium (Mg), phosphorus (P), and potassium (K), respectively. The elemental analysis for the AC 400 • C sample indicated the presence of high carbon content (86.7%). For the AC 1000 • C , peaks are observed at 0.2 and 3.5 KeV. These peaks are attributed to carbon (C) and potassium (K), respectively. Furthermore, the elemental analysis for the AC 1000 • C sample indicated the presence of a higher carbon content (97.4%) than the carbon contents for the AC 400 • C . These results are in good agreement with the reported data, as changes in the structure and physicochemical characteristics of biochar are significantly associated with the pyrolysis temperature. The temperature of pyrolysis has a significant impact on the physicochemical characteristics of biochar (e.g., surface area, pH, and functional groups). The surface area, carbonized fractions, pH, and volatile matter increased as the pyrolysis temperature increased, whereas the cation-exchange capacity and content of the surface functional groups decreased.
(EDX) analysis was conducted. Figure 5a shows peaks at ~0.2, 1.2, 2, and 3.5 KeV. These peaks are attributed to carbon (C), magnesium (Mg), phosphorus (P), and potassium (K), respectively. The elemental analysis for the AC400°C sample indicated the presence of high carbon content (86.7%). For the AC1000°C, peaks are observed at 0.2 and 3.5 KeV. These peaks are attributed to carbon (C) and potassium (K), respectively. Furthermore, the elemental analysis for the AC1000°C sample indicated the presence of a higher carbon content (97.4%) than the carbon contents for the AC400°C. These results are in good agreement with the reported data, as changes in the structure and physicochemical characteristics of biochar are significantly associated with the pyrolysis temperature. The temperature of pyrolysis has a significant impact on the physicochemical characteristics of biochar (e.g., surface area, pH, and functional groups). The surface area, carbonized fractions, pH, and volatile matter increased as the pyrolysis temperature increased, whereas the cation-exchange capacity and content of the surface functional groups decreased.

Scanning Electron Microscopy (SEM) Analysis
An SEM analysis was conducted to study the impact of the thermochemical activation process using the HCl solution and microwave radiation on the carbon surface morphology and the pore's structure. Figure 6a,c shows that the carbon obtained from the pyrolysis of date palm seeds (DPS) under temperatures of 400 °C and 1000 °C had a smooth and slick surface with a restricted pore structure. The two carbon samples had macropore diameters that ranged from 0.71-0.82 µm to 2.13:2.7 µm for carbon at 400 °C and 1000 °C, respectively. After the activation process, the carbon particles had a noticeable variation, as is shown in Figure 6b,d. The surface converted from a slick surface to an eroded rough surface, with a remarkable improvement in the porous structure. As a result of this major change in the surface morphology, the two activated carbon samples showed larger pore diameters. The pore size increased from 5.2 to 5.94 µm and from 3.70 to 4.71

Scanning Electron Microscopy (SEM) Analysis
An SEM analysis was conducted to study the impact of the thermochemical activation process using the HCl solution and microwave radiation on the carbon surface morphology and the pore's structure. Figure 6a,c shows that the carbon obtained from the pyrolysis of date palm seeds (DPS) under temperatures of 400 • C and 1000 • C had a smooth and slick surface with a restricted pore structure. The two carbon samples had macropore diameters that ranged from 0.71-0.82 µm to 2.13:2.7 µm for carbon at 400 • C and 1000 • C, respectively. After the activation process, the carbon particles had a noticeable variation, as is shown in Figure 6b,d. The surface converted from a slick surface to an eroded rough surface, with a remarkable improvement in the porous structure. As a result of this major change in the surface morphology, the two activated carbon samples showed larger pore diameters. The pore size increased from 5.2 to 5.94 µm and from 3.70 to 4.71 µm at 400 • C and 1000 • C, respectively. This large improvement in the carbon physical characteristics can be attributed to the direct interaction between the microwave radiation and the particles inside the pressed compact material in the presence of HCl as a chemical agent. Figure 6e shows the distribution of the carbon particles (AC 1000 • C ) in the chitosan matrix. The activated carbon was found to be capable of dispersing effectively in chitosan, and forming composite beads with no agglomerations. µm at 400 °C and 1000 °C, respectively. This large improvement in the carbon physical characteristics can be attributed to the direct interaction between the microwave radiation and the particles inside the pressed compact material in the presence of HCl as a chemical agent. Figure 6e shows the distribution of the carbon particles (AC1000°C) in the chitosan matrix. The activated carbon was found to be capable of dispersing effectively in chitosan, and forming composite beads with no agglomerations.

FTIR Analysis
In order to classify the main infrared (IR) bands of organics and determine the adsorption mechanism (physisorption or chemosorption), pure and loaded activated carbon/chitosan microbeads (AC400°C MB-0.3:1 and AC1000°C MB-0.3:1) were investigated by FTIR analysis. Figure 7a,b shows that the bands at 3338 cm −1 and 3299 refer to the bending stretch of the NH2 group. The peaks observed at 1641 cm −1 and 1639.3 can be attributed to the axial deformation of C=O of the acetamide group, which was assigned to the acetylated part of chitosan. The bands at 1406 cm −1 and 1035 cm −1 are assigned to the angular deformation of C-H of the CH3 group and to C-O binding and stretching, respectively. These results are close to those recorded for activated carbon/chitosan composites investigated elsewhere [33]. By comparing the two spectra (before and after adsorption), it was noticed that there was no change in the peaks. This means that no chemical bonds were formed within the adsorption process. The change in the peak intensity can be attributed to the electrostatic interaction between the anionic dye molecules and H + ions that accumulated on the activated carbon surface and -NH2 groups on the surface of the chitosan.

FTIR Analysis
In order to classify the main infrared (IR) bands of organics and determine the adsorption mechanism (physisorption or chemosorption), pure and loaded activated carbon/chitosan microbeads (AC 400 • C MB-0.3:1 and AC 1000 • C MB-0.3:1) were investigated by FTIR analysis. Figure 7a,b shows that the bands at 3338 cm −1 and 3299 refer to the bending stretch of the NH 2 group. The peaks observed at 1641 cm −1 and 1639.3 can be attributed to the axial deformation of C=O of the acetamide group, which was assigned to the acetylated part of chitosan. The bands at 1406 cm −1 and 1035 cm −1 are assigned to the angular deformation of C-H of the CH 3 group and to C-O binding and stretching, respectively. These results are close to those recorded for activated carbon/chitosan composites investigated elsewhere [33]. By comparing the two spectra (before and after adsorption), it was noticed that there was no change in the peaks. This means that no chemical bonds were formed within the adsorption process. The change in the peak intensity can be attributed to the electrostatic interaction between the anionic dye molecules and H + ions that accumulated on the activated carbon surface and -NH 2 groups on the surface of the chitosan.
3.1.6. Surface Area As shown in Figure 8, the BET surface area analysis was conducted in order to investigate the effect of the thermochemical activation process on the adsorption characteristics of carbon particles, such as the surface area and pore volume. The analysis showed that there was a higher improvement in the surface area and pore volume for carbon particles. For carbon at 400 • C, the BET surface area and pore volume increased from 32.5 m 2 /g and 0.023 cm 3 /g (before activation) to 99.9 m 2 /g and 0.037 cm 3 /g (after activation), respectively. Furthermore, for carbon at 1000 • C, the BET surface area and pore volume increased from 33.1 m 2 /g and 0.025 cm 3 /g (before activation) to 138 m 2 /g and 0.045 cm 3 /g (after activation), respectively. The results shown in Table 1 indicate that the applied activation process using the HCl solution and microwave radiation gas had a major effect on the BET surface area and pore volume for carbon particles. 3.1.6. Surface Area As shown in Figure 8, the BET surface area analysis was conducted in order to investigate the effect of the thermochemical activation process on the adsorption characteristics of carbon particles, such as the surface area and pore volume. The analysis showed that there was a higher improvement in the surface area and pore volume for carbon particles. For carbon at 400 °C, the BET surface area and pore volume increased from 32.5 m 2 /g and 0.023 cm 3 /g (before activation) to 99.9 m 2 /g and 0.037 cm 3 /g (after activation), respectively. Furthermore, for carbon at 1000 °C, the BET surface area and pore volume increased from 33.1 m 2 /g and 0.025 cm 3 /g (before activation) to 138 m 2 /g and 0.045 cm 3 /g (after activation), respectively. The results shown in Table 1 indicate that the applied activation process using the HCl solution and microwave radiation gas had a major effect on the BET surface

Effect of Microbead Dose on DB78-Dye-Removal Efficiency
The doses of activated carbon/chitosan microbeads were varied in order to inv gate their effects on the efficiency of the direct blue 78 dye removal. It was found th increasing the microbead dosage (increasing the active adsorption sites), the equilib loading decreases and the removal efficiency increases until reaching the maximum ciency, and then approximately reaches a fixed value. The experiments were condu

Effect of Microbead Dose on DB78-Dye-Removal Efficiency
The doses of activated carbon/chitosan microbeads were varied in order to investigate their effects on the efficiency of the direct blue 78 dye removal. It was found that by increasing the microbead dosage (increasing the active adsorption sites), the equilibrium loading decreases and the removal efficiency increases until reaching the maximum efficiency, and then approximately reaches a fixed value. The experiments were conducted by varying the doses of AC 400 • C MB-0.3:1 and AC 1000 • C MB-0.3:1 from 0.5 to 6.5 g/L. The adsorption process was conducted at initial concentrations of DB78-dye synthetic solutions of 40 mg/L at an ambient temperature of 20 • C, a pH of 4-5, a stirring speed of 200 RPM, and a contact time of 40 min. Figure 9 demonstrates the influence of the activated carbon/chitosan microbeads on both the dye-removal efficiency (%) and the equilibrium loading (mg/g). For AC 400 • C MB-0.3:1, the removal efficiency (97.8%) and equilibrium loading (13.1 mg/g) were obtained by using a AC 400 • C MB-0.3:1 dose of 3 g/L for the solution with an initial concentration of 40 mg/L. The maximum equilibrium loading was reached at 31.5 mg/g. It was obtained by using a AC 400 • C MB-0.3:1 dose of 0.5 g/L. 0.3:1, the removal efficiency (97.8%) and equilibrium loading (13.1 mg/g) were obtain by using a AC400°C MB-0.3:1 dose of 3 g/L for the solution with an initial concentration 40 mg/L. The maximum equilibrium loading was reached at 31.5 mg/g. It was obtain by using a AC400°C MB-0.3:1 dose of 0.5 g/L.
Furthermore, for the AC1000°C MB-0.3:1 experimental analysis, the removal efficien (98.4%) and equilibrium loading (9.85 mg/g) were obtained by using a AC1000°C MB-0 dose of 4 g/L for the solution with an initial concentration of 40 mg/L. The maximum eq librium loading reached was 32.2 mg/g. It was obtained by using a AC1000°C MB-0.3:1 d of 0.5 g/L. It is worth noting that higher q values and lower Ceq values indicate that th is less dye in the solution and better adsorption.

Effect of pH on DB78-Dye-Removal Efficiency
The effect of the initial pH of the dye solution was experimentally investigated un a pH range of from 2 to 9. The results are shown in Figure 10  Furthermore, for the AC 1000 • C MB-0.3:1 experimental analysis, the removal efficiency (98.4%) and equilibrium loading (9.85 mg/g) were obtained by using a AC 1000 • C MB-0.3:1 dose of 4 g/L for the solution with an initial concentration of 40 mg/L. The maximum equilibrium loading reached was 32.2 mg/g. It was obtained by using a AC 1000 • C MB-0.3:1 dose of 0.5 g/L. It is worth noting that higher q values and lower C eq values indicate that there is less dye in the solution and better adsorption.

Effect of pH on DB78-Dye-Removal Efficiency
The effect of the initial pH of the dye solution was experimentally investigated under a pH range of from 2 to 9. The results are shown in Figure 10 In addition, the swelling of chitosan powder into chitosan beads in the presence of acidic conditions will protonate the amine groups (NH 2 ) into NH 3 + . This process will improve the electrostatic interaction between chitosan particles and dye ions, and enhance the activated carbon/chitosan microbead ability for anionic-dye removal. and improved their surface positive charge. This improvement in the surface charg creases the ability of activated carbon particles to attract the anionic molecules of d blue 78 dye.
In addition, the swelling of chitosan powder into chitosan beads in the presen acidic conditions will protonate the amine groups (NH2) into NH3 + . This process wil prove the electrostatic interaction between chitosan particles and dye ions, and enh the activated carbon/chitosan microbead ability for anionic-dye removal.    Figure 11 shows the influence of the contact time on the dye-removal efficiency and equilibrium loading. It was experimentally observed that the percentage of dye removal increases with the increase in the contact time. At a specific time, the microbead reached its maximum loading capacity (equilibrium loading q e ). At contact time (50 min) and the AC 1000 • C MB-0.3:1 dose (3 g/L), the equilibrium concentration decreased to 1.1 mg/L, with a dye-removal efficiency of 97%, and an optimum loading capacity of 9.7 mg/g for an initial dye concentration of 40 mg/L. These experiments were conducted under the following conditions: a temperature of 20 • C and a rate of mixing of 200 RPM. To study the composition of the microbead production on the DB78-dye-removal ficiency, different ratios of AC and chitosan were applied (e.g., ACMB -0.1:1, ACMB-0.2 ACMB-0.3:1, ACMB-0.4:1, and ACMB-0.5:1). The initial dye concentration was 40 mg the pH range was 4:5, the contact time was 40 min, the microbead dose was 3 g/L, and t

Effect of Activated Carbon/Chitosan Ratio on DB78 Dye Removal
To study the composition of the microbead production on the DB78-dye-removal efficiency, different ratios of AC and chitosan were applied (e.g., ACMB -0.1:1, ACMB-0.2:1, ACMB-0.3:1, ACMB-0.4:1, and ACMB-0.5:1). The initial dye concentration was 40 mg/L, the pH range was 4:5, the contact time was 40 min, the microbead dose was 3 g/L, and the stirrer speed was 200 RPM. The experimental results show that the dye-removal efficiency increases with the increase in the activated carbon loading up to 0.3:1. No significant improvement in the dye removal was found at higher activated carbon loads, as is shown in Figure 12. This can be attributed to a blockage of the internal porosities of chitosan by the incorporation of higher activated carbon loadings. Figure 13 shows the DB78 dye solution and dye removal using AC 400 • C MB-0.3:1 and AC 1000 • C MB-0.3:1. It was observed that there was a slight improvement in the efficiency of the dye removal using AC 1000 • C compared with AC 400 • C . This result is in a good agreement with the EDX analysis, as a higher carbon content (97.4%) was found in the activated carbon produced at 1000 • C.

Effect of Contact Time
The influence of the contact time on the dye removal percentage and adsorbent load ing was studied. The percentage of dye removed increased with the increase in the mixin time until the maximum removal efficiency was reached, as is illustrated in Figure 14. Th

Effect of Contact Time
The influence of the contact time on the dye removal percentage and adsorbent loading was studied. The percentage of dye removed increased with the increase in the mixing time until the maximum removal efficiency was reached, as is illustrated in Figure 14. The

Effect of Contact Time
The influence of the contact time on the dye removal percentage and adsorbent loading was studied. The percentage of dye removed increased with the increase in the mixing time until the maximum removal efficiency was reached, as is illustrated in Figure 14. The adsorbent achieved its maximum loading capacity at this point (equilibrium loading q e ). For a dye concentration of 40 mg/L of solution, a contact time of 50 min, and a 3 g/L adsorbent dose of AC 1000 • C MB-0.3:1, the dye-removal efficiency was 99%, and the optimal loading capacity was 10 mg/g. When comparing AC 1000 • C MB-0.3:1 with AC 400 • C MB-3:1, a slight improvement in the dye removal was observed. This could be due to the AC 1000 • C MB-3's increased carbon content.  Figure 15 shows the adsorption isothermal curve. It indicates the amount of adsorbate (DB78 dye) by the activated carbon/chitosan microbead (AC400°C MB-0.3:1 and AC1000°C MB-0.3:1) qeq against the adsorbate concentration in the liquid state (Ceq). The initial concentration was 40 mg/L. These results are essential considerations in the design of adsorption systems. Moreover, the form of the equilibrium curve helps to describe other phenomena that are linked with the adsorption mechanism. The equilibrium curves are identified under four main classes according to the primary slope and subgroups that are described for each class based on the upper-part shapes and slope changes: (a) S curves, or vertical-orientation isotherms; (b) L curves, or normal or "Langmuir" isotherms; (c) H curves, or high-affinity isotherms; and (d) C curves, or constant-partition isotherms [34].

Adsorption Isotherm
The initial shape of the equilibrium curve (L shape) in Figure 15 follows the basic premise that the higher the solute concentration, the greater the adsorption capacity, until the number of the adsorption site clearance is limited, and competition occurs between the solute molecules for the available sites. This isotherm type indicates that the adsorption occurs due to relatively weak forces, such as "van der Waals forces". Several isothermal models (equations) are available, and the two important isotherms are selected in this study, which are, namely, the Freundlich and Langmuir isotherms.  Figure 15 shows the adsorption isothermal curve. It indicates the amount of adsorbate (DB78 dye) by the activated carbon/chitosan microbead (AC 400 • C MB-0.3:1 and AC 1000 • C MB-0.3:1) q eq against the adsorbate concentration in the liquid state (C eq ). The initial concentration was 40 mg/L. These results are essential considerations in the design of adsorption systems. Moreover, the form of the equilibrium curve helps to describe other phenomena that are linked with the adsorption mechanism. The equilibrium curves are identified under four main classes according to the primary slope and subgroups that are described for each class based on the upper-part shapes and slope changes: (a) S curves, or vertical-orientation isotherms; (b) L curves, or normal or "Langmuir" isotherms; (c) H curves, or high-affinity isotherms; and (d) C curves, or constant-partition isotherms [34].

Adsorption Isotherm
The initial shape of the equilibrium curve (L shape) in Figure 15 follows the basic premise that the higher the solute concentration, the greater the adsorption capacity, until the number of the adsorption site clearance is limited, and competition occurs between the solute molecules for the available sites. This isotherm type indicates that the adsorption occurs due to relatively weak forces, such as "van der Waals forces". Several isothermal models (equations) are available, and the two important isotherms are selected in this study, which are, namely, the Freundlich and Langmuir isotherms. The Freundlich isotherm refers to the adsorption on a heterogeneous surface, and the adsorbed mass increased exponentially with an increase in the concentration [35]. This isotherm explains the equilibrium on heterogeneous surfaces and, hence, the capacity is not a presumed monolayer. In the liquid phase, this isotherm is given by Equation (3): where kF is the Freundlich fixed value (kF unit = mg/g, where nF is the Freundlich exponent). This isotherm focused on integrating the role of the adsorbent (adsorbate-surface interactions). Figure 16 shows the application of equilibrium data according to the Freundlich isotherm. For AC400°C MB-0.3:1, the Freundlich constant (kf) value was 11.86, and the heterogeneity factor (1/nf) value was 0.36 for the solution with an initial concentration of 40 mg/L. For AC1000°C MB-0.3:1, the Freundlich constant (kf) value was 11.13 mg/L, and the heterogeneity factor (1/nf) value was 0.37 for an initial concentration 40 mg/L. The Freundlich equation's (nf) parameter was used to subjectively test the adsorption intensity, revealing the adsorbent's affinity for the dye removal, and suggesting good adsorption when it had values greater than 1. The Freundlich isotherm refers to the adsorption on a heterogeneous surface, and the adsorbed mass increased exponentially with an increase in the concentration [35]. This isotherm explains the equilibrium on heterogeneous surfaces and, hence, the capacity is not a presumed monolayer. In the liquid phase, this isotherm is given by Equation (3): where k f is the Freundlich fixed value (k f unit = mg/g, where n f is the Freundlich exponent). This isotherm focused on integrating the role of the adsorbent (adsorbate-surface interactions). Figure 16 shows the application of equilibrium data according to the Freundlich isotherm. For AC 400 • C MB-0.3:1, the Freundlich constant (k f ) value was 11.86, and the heterogeneity factor (1/n f ) value was 0.36 for the solution with an initial concentration of 40 mg/L. For AC 1000 • C MB-0.3:1, the Freundlich constant (k f ) value was 11.13 mg/L, and the heterogeneity factor (1/n f ) value was 0.37 for an initial concentration 40 mg/L. The Freundlich equation's (n f ) parameter was used to subjectively test the adsorption intensity, revealing the adsorbent's affinity for the dye removal, and suggesting good adsorption when it had values greater than 1.
The Langmuir isotherm believes that sorption occurs within the adsorbent at different homogeneous sites. It has been successfully applied to several processes of sorption. The isotherm's physical simplicity is based on some assumptions: Adsorption cannot occur beyond the monolayer coverage. Each site can hold only one adsorbate molecule. All sites are energetically equivalent. The surface is uniform. The linear form of the Langmuir isotherm is given by the following equation, Equation (4): (C e /q e ) = (1/Q 0 b) + (C e /Q 0 ) where C e is the equilibrium concentration (mg/L), q e is the mass adsorbed at equilibrium (mg/g), Q 0 is the adsorbent loading (mg/g), and b is the adsorption energy (Langmuir fixed value of L/mg). The values of Q 0 and b were determined from the slope and intercept of the linear plots' C e/ q e versus C e , respectively, which resulted in a straight line of slope 1/Q 0 corresponding to the total coverage of the monolayer (mg/g), and the intercept is 1/Q 0 b [36]. The Langmuir isotherm believes that sorption occurs within the adsorbent at different homogeneous sites. It has been successfully applied to several processes of sorption. The isotherm's physical simplicity is based on some assumptions: Adsorption cannot occur beyond the monolayer coverage. Each site can hold only one adsorbate molecule. All sites are energetically equivalent. The surface is uniform. The linear form of the Langmuir isotherm is given by the following equation, Equation (4): (Ce/qe) = (1/Q0 b) + (Ce/Q0) (4) where Ce is the equilibrium concentration (mg/L), qe is the mass adsorbed at equilibrium (mg/g), Q0 is the adsorbent loading (mg/g), and b is the adsorption energy (Langmuir fixed value of L/mg). The values of Q0 and b were determined from the slope and intercept of the linear plots' Ce/qe versus Ce, respectively, which resulted in a straight line of slope 1/Q0 corresponding to the total coverage of the monolayer (mg/g), and the intercept is 1/Q0b [36]. Figure 17 shows the application of equilibrium data according to the Langmuir isotherm. For AC400°C MB-0.3:1, the adsorbent loading value (Q0) was 33.5 mg/g. The Langmuir fixed value (b) was 1.47 L/mg for an initial concentration of 40 mg/L. For AC1000 °C MB-0.3:1, the adsorbent loading value (Q0) was 32.8 mg/g, and the Langmuir fixed value (b) was 1.68 L/mg. It is observed from the listed adsorption isothermal models in Table 2 that the adsorption of the DB78 dye using both AC400°C MB-0.3:1 and AC1000°C MB-0.3:1 followed the Langmuir isotherm.  Figure 17 shows the application of equilibrium data according to the Langmuir isotherm. For AC 400 • C MB-0.3:1, the adsorbent loading value (Q 0 ) was 33.5 mg/g. The Langmuir fixed value (b) was 1.47 L/mg for an initial concentration of 40 mg/L. For AC 1000 • C MB-0.3:1, the adsorbent loading value (Q 0 ) was 32.8 mg/g, and the Langmuir fixed value (b) was 1.68 L/mg. It is observed from the listed adsorption isothermal models in Table 2 that the adsorption of the DB78 dye using both AC 400 • C MB-0.3:1 and AC 1000 • C MB-0.3:1 followed the Langmuir isotherm.

Adsorption Kinetics
In order to understand the mechanism of the adsorption process, kinetic studies were conducted by analyzing the samples at time intervals of 10 min until the consecutive residue dye concentrations became closer. The kinetic data for the adsorption process of the DB78 dyes AC 400 • C MB-0.3:1 and AC 1000 • C MB-0.3:1, with initial dye concentrations of 40 mg/L, were examined with the well-known kinetic models: the pseudo first-order model (PFO) and pseudo second-order model (PSO). The plotting of these kinetic models is shown in Figure 18. ln (q e − q t ) = ln q e − k 1 t (5) where q e (mg/g) and qt (mg/g) are the amounts of adsorbed adsorbate at equilibrium and at time (t), respectively, and K 1 (min −1 ) is the rate constant of the pseudo first-order model. The pseudo second-order equation.
The adsorption kinetics can also be described by the pseudo second-order model. The linear form of the pseudo second-order equation is expressed as: (t/q t ) = (1/k 2 q e 2 ) + (1/q e ) t (6) where k 2 (g/mg min) is the equilibrium rare constant of the pseudo second-order adsorption, where q e (mg/g) and qt (mg/g) are the amounts of adsorbed adsorbate at equilibrium and at time (t), respectively. Figure 18 shows the linear plots of the PFO and PSO models of AC 400 • C MB-0.3:1 and AC 1000 • C MB-0.3:1. The kinetic parameters are listed in Table 3. On the basis of the low correlation coefficient for the PSO and the high value for the PFO, the adsorption abilities of AC 400 • C MB-0.3:1 and AC 1000 • C MB-0.3:1 follow the PFO rather than the PSO. These results suggest that, for AC 400 • C MB-0.3:1, the PFO can best predict the kinetic process. The value of q e = 29.5 mg/g calculated by the PFO was more similar to the practical q e = 9.76 mg/g than the PSO. For AC 1000 • C MB-0.3:1, the PFO can best predict the kinetic process. The value of q e = 32.4 mg/g calculated by the PFO was more similar to the practical q e = 9.96 mg/g than the PSO, as listed in Table 3. For AC 400 • C MB-0.3:1 and AC 1000 • C MB-0.3:1, the applicability of the PFO model indicates the interaction between the dye molecules and the microbead surface. Hence, the adsorption system is physical adsorption [37].

Conclusions
The removal of anionic dye (DB78) from synthetic wastewater by adsorption onto novel activated carbon/chitosan microbeads (AC 400 • C MB and AC 400 • C MB) was experimentally studied. Several microbeads with different activated carbon/chitosan ratios (0.1:1, 0.2:1, 0.3:1, 0.4:1, and 0.5:1) were synthetized in order to study the effect of the activated carbon quantity on the removal efficiency. It was observed that the removal efficiency increases with the increasing activated carbon quantity in synthetic microbeads up to a ratio of 0.3:1. The adsorption process is highly dependent on the solution pH, and the ACMB reaches its maximum equilibrium loading under acidic conditions (pH = 4:5). Based on the experimental results, it was observed that the removal efficiencies of 97.8% and 98.4% were obtained by using the adsorbents AC 400 • C MB-0.3:1 and AC 1000 • C MB-0.3:1, respectively, with initial concentrations of 40 mg/L. The equilibrium studies show that the initial shape of the equilibrium curve is an L shape, which means that the adsorption process resulted from the electrostatic interaction between the dye molecules and the adsorbent particles (physical forces). The adsorption studies were studied by using the Langmuir and Freundlich isothermal models, and the results were best fit to the Langmuir