# α and γ Alumina Spheres for Azo Dye (Allura Red) Removal from Aqueous Media

Authors: Jonatan Torres-Pérez; Nahum Medellín-Castillo; Simón Yobanny Reyes-López
Journal: Adsorption Science & Technology
 (2022)

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## Abstract

Allura red or Red 40 (R40) is a dye widely used in the food, textile, and pharmaceutical industries; it is considered dangerous because it is soluble in water, and it has high toxicity and resistance to natural degradation. Several advanced wastewater treatments have been shown to be effective for R40 removal but some of them present disadvantages such as by-products obtention, high energy consumption, and high cost of the reactants used in the removal process. In the present work,α-Alumina (Alu) and γ-Alu spheres were synthesized by the encapsulation method. The prepared spheres were characterized by FT-IR, XRD, SEM/EDS, and SBET, and it was determined the presence of only inorganic bonds from ceramic material, and the amorphous alumina was observed in spheres with a smooth and uniform surface and with pores. R40 adsorption kinetics and isotherms were performed, as well as material regeneration for consequent sorption cycles. Sorption tests for R40 removal were carried out under different conditions of initial concentration, pH value, and the presence of interfering ions. The maximal sorption capacity of the synthetized α- and γ-Alu spheres were situated between 0.1765 and 18.9865 mg/g. Different kinetic and isothermal equations were applied and finally, the experimental data was described by Elovich and Freundlich models. The γ-Alu spheres after five heat treatment regeneration cycles showed stable behavior and potential re-use in new sorption processes with R40 removal >97.7% at pH 3 and >85.6% at C0 =10 mg/L. The obtained results showed that the γ-Alu spheres are novel, alternative, and sustainable synthesized materials for the advanced treatment of wastewater by adsorption process for the removal of Allura red azo dye in aqueous media.


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## Body

## 1. Introduction

Azo dyes are the largest group of synthetic organic dyes, and most of the colored molecules are used in the textile and food industry. Large amounts of dyes are disposed into the sewer system, so the elimination from wastewater presents a greater challenge than the treatment of other organic and inorganic compounds that are degraded by conventional treatments. Azo dyes are the most used synthetic organic compounds to give color to a great variety of commercial products and these kinds of dyes have the particularity to contain one or more azo groups (N=N). One of the most popular azo dyes used around the world is Allura Red (R40) and it has been proved in previous studies that it is carcinogenic and mutagenic [1]. Therefore, there is an urgency to develop effective methods for the advanced treatment of wastewater contaminated with organic azo dyes. Several treatment methods have been developed; however, most of the applied technologies are ineffective since they generate by-products that are sometimes molecules with greater toxicity than the original compound [2, 3].An advanced water treatment technique is adsorption, which has been proved to be one of the most effective and economical treatments; its application is easy as well as its operation and profitability, in addition to the fact that, unlike other technologies, it does not generate secondary by-products, which transforms this technology into a highly sustainable alternative for polluted water treatment. The materials that have been used throughout history in sorption processes have natural or synthetic origin. One of the most used materials for the elimination of dyes from wastewater is activated carbon; however, due to its high cost and manufacturing complexity, several investigations have focused on alternative adsorbents that have a high adsorption capacity, paying increased attention to synthetic materials [4]. Among the diversity of existing synthetic materials, there are the polymeric and ceramic spheres prepared by encapsulation techniques. Also, alumina spheres have been tested for adsorption of various contaminants from an aqueous solution and their high efficiency has been proven, because they have excellent physical and textural properties. The most abundant metal on Earth is aluminum, which is found in combination with other elements such as oxygen and silicon. Alumina is an oxide composed of this metallic element, and it can be found in bauxite deposits such as gibbsite and boehmite. It is a material that has very good physicochemical properties; however, these depend on the way in which it is synthesized [5]. Other researchers found that the most important polymorphs of alumina are γ-AlOOH, η-Al2O3, and α-Al2O3, and commonly γ-Al2O3 and α-Al2O3 are used as adsorbents, catalysts, and catalytic supports [6, 7].The use of gamma-alumina (γ-Alu) as an adsorbent and catalyst support stands out because it has a large surface area, high stability, and several acid/base sites. Previous research has been elaborated γ-Alu nanoparticles for the removal of yellow eosin dye; the kinetic test was carried out at pH 4 where it was obtained a 99.36% dye removal [8]. Several adsorption models were used, and the Langmuir isotherm was the one that best described the sorption process because it obtained a high correlation coefficient.A previous study prepared porousγ-Alu microspheres using the modified spray drying method [9]; the material was employed to eliminate the Congo Red dye and it had great retention capacity. In another study, Congo Red has been removed from an aqueous medium with manufactured porous microspheres of ZnO-Al2O3; the material had good adsorption performance compared to ZnO and pure Al2O3, since the composite has more specific surface area [10]. However, there are no reports of studies about the removal of R40 azo dye onto α- and γ-Alumina spheres converting these materials into novel alternatives for the advanced treatment of water contaminated with organic pollutants.


## 2. Materials and Methods

### 2.1. Preparation of Sodium Alginate, Polyvinyl Alcohol (PVA), and Barium Chloride Solutions

A 10% sodium alginate solution was prepared by dissolving 1 g of sodium alginate in 10 mL of deionized water. The mixture was heated to 60°C with constant stirring until the alginate was completely dissolved. The PVA solution was prepared at 7%, and 1.75 g of PVA was dissolved in 25 mL of deionized water. The mixture was heated to 60°C with constant stirring until completely dissolved. The barium chloride solution was prepared at 0.6 M using deionized water.


### 2.2. Suspension of Alumina

A mixture of 1 g of alumina powder, 0.31 g of the 10% sodium alginate solution, 0.15 g of PVA solution, and 0.91 mL of deionized water was made, and finally, the mixture was stirred at 25°C and it obtained a white paste. The alumina suspension was dropped into the barium chloride solution. Since the spheres were formed, they were subjected to different heat treatments; the first at 100°C for 24 h (ThermoScientific® oven), the second one at 800°C in a muffle (ThermoScientific®) for 2 h, and the last one was exposed to the highest temperature at 1000°C for 4 h forγ-Alu and 1600°C for 2 h α-Alu spheres (Nabertherm® oven) [7].


### 2.3. Characterization of Alumina Spheres

The alumina spheres were characterized by Fourier-transform infrared (FT-IR) spectroscopy, X-ray diffraction (XRD), scanning electron microscope (SEM) with energy-dispersive X-ray spectroscopy (EDS), and specific surface area (SBET).


#### 2.3.1. FT-IR

The FT-IR analysis was employed to determine the chemical groups on the sphere’s surface. The alumina spheres were grounded prior to analysis. A Bruker FT-IR instrument was employed with Platinum-ATR; the analysis was conducted by 32 times scanning (4 cm-1) and measures were done in the 400 and 4000 cm-1 intervals [11].


#### 2.3.2. XRD

XRD was used to make an identification of the crystalline phases in alumina spheres. For this analysis, a X’Pert PRO PANalytical instrument (Cu kα =1.54056, 20 kV, 10-80°) was used, and scanning speed of 2°/min.


#### 2.3.3. SEM/EDS

The samples were sputtered with gold employing a Denton Vacuum DeskV instrument. After this procedure, the samples were chemically and morphologically characterized using a Field Emission Scanning Electron microscope SU5000 Hitachi, and JEOL JSM-6010 PLUS/LA Analytical SEM.


#### 2.3.4. SBET

The specific surface area, pore volume, and pore diameter of spheres were measured using N2 and the BET equation, using a physisorption equipment (ASAP2010, Micromeritics). Before analysis, the samples were preheated at 150°C for 2 h to eliminate adsorbed water.


### 2.4. Sorption Tests

The maximal sorption capacity and the equilibrium time of the alumina spheres were determined by adsorption tests performed with the variation of concentration and pH of the solution. Prior to the sorption tests, the materials were dried for 12 h at 105°C. The specific surface area and pore volume of alumina fibers were measured using N2 and the BET equation, using a physisorption equipment (ASAP2010, Micromeritics). Before analysis, the samples were preheated at 150°C for 2 h to eliminate adsorbed water.


### 2.5. Sorption Kinetics

For the sorption kinetics, 500 mL was prepared with R40 at 10 ppm for theα-Alu and γ-Alu spheres. This solution was placed in two plastic reactors and then 0.25 g of α-Alu and γ-Alu spheres was added to them. Subsequently, the solutions with the spheres were placed on a Barnstead/Lab-line® A-class plate shaker and were measured every hour for 8 hours and then every 24 hours for 5 days. The concentration of each obtained aliquot was measured at 505 nm wavelength in a Jenway® spectrophotometer (model 7315).


#### 2.5.1. Effect of Initial Concentration

For the initial concentration, three 500 mL solutions were prepared at 10, 50, and 100 ppm. They were divided into six reactors and the concentration was measured at a wavelength of 505 nm; 0.25 g ofα-Alu and γ-Alu spheres was weighed and deposited in each of the used reactors. Finally, the solutions with the spheres were shaked and the solutions were sampled every hour for 8 hours and then every 24 hours for 5 days.


#### 2.5.2. Effect of pH

Two batches of 500 mL solution were made with R40 at 10 ppm concentration; subsequently, the pH of the solutions was modified with HCl (0.1 N) or NaOH (0.1 N) to reach pH 3 and 10, respectively, and the value was measured with a Hanna Instruments® potentiometer (Model HI8915). The solutions were placed in two plastic reactors and then 0.25 g of spheres of each material was added. Subsequently, the solutions with the spheres were placed on a Barnstead/Lab-line® A-class plate shaker and these solutions were sampled every hour for 8 hours and then every 24 hours for 5 days. The concentration of each aliquot obtained was measured at a wavelength of 505 nm.


### 2.6. Sorption Isotherms

Sorption isotherms were made from different solutions of R40 at 1, 2, 3, 4, 5, 6, 7, 8, 9, and 10 ppm as initial concentration. 0.05 g ofα-Alu and γ-Alu spheres was placed in 50 mL of the solutions and was left under constant agitation on a Fisher Scientific® brand orbital shaker for 5 days. After this time, an aliquot was taken from each solution and the concentration was measured at 505 nm.


#### 2.6.1. Effect of Ionic Strength

The ionic strength effect over R40 sorption process ontoγ-Alu spheres was evaluated. The experimentation was conducted in the same way than it was described previously in the effect of initial concentration section. It was employed a commercial bottled water with specific ion concentrations in it (Ca2+ (80 mg/L), HCO-3 (360 mg/L), Mg+2 (26 mg/L), Na+ (6.5 mg/L), Si+2 (15 mg/L), SO-24 (14 mg/L), Cl- (10 mg/L), NO-23 (3.8 mg/L), and CaCO3 (300 mg/L).


## 2.1. Preparation of Sodium Alginate, Polyvinyl Alcohol (PVA), and Barium Chloride Solutions

A 10% sodium alginate solution was prepared by dissolving 1 g of sodium alginate in 10 mL of deionized water. The mixture was heated to 60°C with constant stirring until the alginate was completely dissolved. The PVA solution was prepared at 7%, and 1.75 g of PVA was dissolved in 25 mL of deionized water. The mixture was heated to 60°C with constant stirring until completely dissolved. The barium chloride solution was prepared at 0.6 M using deionized water.


## 2.2. Suspension of Alumina

A mixture of 1 g of alumina powder, 0.31 g of the 10% sodium alginate solution, 0.15 g of PVA solution, and 0.91 mL of deionized water was made, and finally, the mixture was stirred at 25°C and it obtained a white paste. The alumina suspension was dropped into the barium chloride solution. Since the spheres were formed, they were subjected to different heat treatments; the first at 100°C for 24 h (ThermoScientific® oven), the second one at 800°C in a muffle (ThermoScientific®) for 2 h, and the last one was exposed to the highest temperature at 1000°C for 4 h forγ-Alu and 1600°C for 2 h α-Alu spheres (Nabertherm® oven) [7].


## 2.3. Characterization of Alumina Spheres

The alumina spheres were characterized by Fourier-transform infrared (FT-IR) spectroscopy, X-ray diffraction (XRD), scanning electron microscope (SEM) with energy-dispersive X-ray spectroscopy (EDS), and specific surface area (SBET).


### 2.3.1. FT-IR

The FT-IR analysis was employed to determine the chemical groups on the sphere’s surface. The alumina spheres were grounded prior to analysis. A Bruker FT-IR instrument was employed with Platinum-ATR; the analysis was conducted by 32 times scanning (4 cm-1) and measures were done in the 400 and 4000 cm-1 intervals [11].


### 2.3.2. XRD

XRD was used to make an identification of the crystalline phases in alumina spheres. For this analysis, a X’Pert PRO PANalytical instrument (Cu kα =1.54056, 20 kV, 10-80°) was used, and scanning speed of 2°/min.


### 2.3.3. SEM/EDS

The samples were sputtered with gold employing a Denton Vacuum DeskV instrument. After this procedure, the samples were chemically and morphologically characterized using a Field Emission Scanning Electron microscope SU5000 Hitachi, and JEOL JSM-6010 PLUS/LA Analytical SEM.


### 2.3.4. SBET

The specific surface area, pore volume, and pore diameter of spheres were measured using N2 and the BET equation, using a physisorption equipment (ASAP2010, Micromeritics). Before analysis, the samples were preheated at 150°C for 2 h to eliminate adsorbed water.


## 2.3.1. FT-IR

The FT-IR analysis was employed to determine the chemical groups on the sphere’s surface. The alumina spheres were grounded prior to analysis. A Bruker FT-IR instrument was employed with Platinum-ATR; the analysis was conducted by 32 times scanning (4 cm-1) and measures were done in the 400 and 4000 cm-1 intervals [11].


## 2.3.2. XRD

XRD was used to make an identification of the crystalline phases in alumina spheres. For this analysis, a X’Pert PRO PANalytical instrument (Cu kα =1.54056, 20 kV, 10-80°) was used, and scanning speed of 2°/min.


## 2.3.3. SEM/EDS

The samples were sputtered with gold employing a Denton Vacuum DeskV instrument. After this procedure, the samples were chemically and morphologically characterized using a Field Emission Scanning Electron microscope SU5000 Hitachi, and JEOL JSM-6010 PLUS/LA Analytical SEM.


## 2.3.4. SBET

The specific surface area, pore volume, and pore diameter of spheres were measured using N2 and the BET equation, using a physisorption equipment (ASAP2010, Micromeritics). Before analysis, the samples were preheated at 150°C for 2 h to eliminate adsorbed water.


## 2.4. Sorption Tests

The maximal sorption capacity and the equilibrium time of the alumina spheres were determined by adsorption tests performed with the variation of concentration and pH of the solution. Prior to the sorption tests, the materials were dried for 12 h at 105°C. The specific surface area and pore volume of alumina fibers were measured using N2 and the BET equation, using a physisorption equipment (ASAP2010, Micromeritics). Before analysis, the samples were preheated at 150°C for 2 h to eliminate adsorbed water.


## 2.5. Sorption Kinetics

For the sorption kinetics, 500 mL was prepared with R40 at 10 ppm for theα-Alu and γ-Alu spheres. This solution was placed in two plastic reactors and then 0.25 g of α-Alu and γ-Alu spheres was added to them. Subsequently, the solutions with the spheres were placed on a Barnstead/Lab-line® A-class plate shaker and were measured every hour for 8 hours and then every 24 hours for 5 days. The concentration of each obtained aliquot was measured at 505 nm wavelength in a Jenway® spectrophotometer (model 7315).


### 2.5.1. Effect of Initial Concentration

For the initial concentration, three 500 mL solutions were prepared at 10, 50, and 100 ppm. They were divided into six reactors and the concentration was measured at a wavelength of 505 nm; 0.25 g ofα-Alu and γ-Alu spheres was weighed and deposited in each of the used reactors. Finally, the solutions with the spheres were shaked and the solutions were sampled every hour for 8 hours and then every 24 hours for 5 days.


### 2.5.2. Effect of pH

Two batches of 500 mL solution were made with R40 at 10 ppm concentration; subsequently, the pH of the solutions was modified with HCl (0.1 N) or NaOH (0.1 N) to reach pH 3 and 10, respectively, and the value was measured with a Hanna Instruments® potentiometer (Model HI8915). The solutions were placed in two plastic reactors and then 0.25 g of spheres of each material was added. Subsequently, the solutions with the spheres were placed on a Barnstead/Lab-line® A-class plate shaker and these solutions were sampled every hour for 8 hours and then every 24 hours for 5 days. The concentration of each aliquot obtained was measured at a wavelength of 505 nm.


## 2.5.1. Effect of Initial Concentration

For the initial concentration, three 500 mL solutions were prepared at 10, 50, and 100 ppm. They were divided into six reactors and the concentration was measured at a wavelength of 505 nm; 0.25 g ofα-Alu and γ-Alu spheres was weighed and deposited in each of the used reactors. Finally, the solutions with the spheres were shaked and the solutions were sampled every hour for 8 hours and then every 24 hours for 5 days.


## 2.5.2. Effect of pH

Two batches of 500 mL solution were made with R40 at 10 ppm concentration; subsequently, the pH of the solutions was modified with HCl (0.1 N) or NaOH (0.1 N) to reach pH 3 and 10, respectively, and the value was measured with a Hanna Instruments® potentiometer (Model HI8915). The solutions were placed in two plastic reactors and then 0.25 g of spheres of each material was added. Subsequently, the solutions with the spheres were placed on a Barnstead/Lab-line® A-class plate shaker and these solutions were sampled every hour for 8 hours and then every 24 hours for 5 days. The concentration of each aliquot obtained was measured at a wavelength of 505 nm.


## 2.6. Sorption Isotherms

Sorption isotherms were made from different solutions of R40 at 1, 2, 3, 4, 5, 6, 7, 8, 9, and 10 ppm as initial concentration. 0.05 g ofα-Alu and γ-Alu spheres was placed in 50 mL of the solutions and was left under constant agitation on a Fisher Scientific® brand orbital shaker for 5 days. After this time, an aliquot was taken from each solution and the concentration was measured at 505 nm.


### 2.6.1. Effect of Ionic Strength

The ionic strength effect over R40 sorption process ontoγ-Alu spheres was evaluated. The experimentation was conducted in the same way than it was described previously in the effect of initial concentration section. It was employed a commercial bottled water with specific ion concentrations in it (Ca2+ (80 mg/L), HCO-3 (360 mg/L), Mg+2 (26 mg/L), Na+ (6.5 mg/L), Si+2 (15 mg/L), SO-24 (14 mg/L), Cl- (10 mg/L), NO-23 (3.8 mg/L), and CaCO3 (300 mg/L).


## 2.6.1. Effect of Ionic Strength

The ionic strength effect over R40 sorption process ontoγ-Alu spheres was evaluated. The experimentation was conducted in the same way than it was described previously in the effect of initial concentration section. It was employed a commercial bottled water with specific ion concentrations in it (Ca2+ (80 mg/L), HCO-3 (360 mg/L), Mg+2 (26 mg/L), Na+ (6.5 mg/L), Si+2 (15 mg/L), SO-24 (14 mg/L), Cl- (10 mg/L), NO-23 (3.8 mg/L), and CaCO3 (300 mg/L).


## 3. Results and Discussion

In the last years, the research about the synthesis of new and alternative adsorbent materials for water treatment has been increased. Such synthetic materials asα-Alu and γ-Alu spheres have remarkable importance because they have the viability to substitute conventional and non-environmentally friendly materials. The preparation and application of such alternative materials require creative and expert approach of researchers on the basic factors affecting the sorption process of different organic molecules. The characterization of the obtained materials was performed to know their general surface properties. Moreover, their environmental applications were done by comparing the synthetized α-Alu and γ-Alu spheres with their effectiveness to remove R40 azo dye from water, the sorption capacity and removal efficiency determined by sorption experiments.


### 3.1. Characterization of the Materials

#### 3.1.1. Ft-IR

Figure1 shows the infrared spectra obtained from α-Alu and γ-Alu spheres. It was not observed typical vibrational bands as evidence of functional groups and bonds present in PVP and alginate. This fact was promoted by decomposition of organic molecules after spheres thermal treatment. Only the inorganic bonds from ceramic material were observed. At 968-400 cm-1, it was observed a wide band that represents the stretching vibration of Al-O bonds in different alumina polymorphs. At 830 and 507-530 cm-1 appear bands corresponding to γ-Al2O3, and at 800 cm-1 and 500-750 cm-1 were detected bands from aluminum in tetrahedral (AlO4) and octahedral (AlO6) coordination, respectively. The octahedral aluminum of α-alumina generates bands placed at 438-456, 491-499, 550, 576-601, 635-644, and 755-763 cm-1 [6]. The materials after dye sorption were analyzed; therefore, no changes were observed in the FT-IR spectra because the presence of the R40 on the surface was not in amounts to be detected by the instrument (figure does not show).Figure 1
Infrared spectra forα-Alu and γ-Alu spheres.


#### 3.1.2. XRD

Figure2 shows diffraction patterns of α-Alu and γ-Alu spheres; small non-defined crystallographic peaks in the diffractogram are evidence of the presence of amorphous alumina in spheres. γ-Alu crystalline planes (222), (400), and (400) are located at 39°, 46°, and 67°, respectively; the γ-Alu characteristic peaks disappear at 1600°C to give a phase transition to α-alumina phase. The turnover is represented by the peak’s appearance at 25, 35, 37.5, 43, 52, 57, 61.5, 66, and 68°, corresponding to (012), (104), (110), (113), (024), (116), (018), (214), and (300) crystalline planes, respectively, when it was compared with JCPDS 83-2081 pattern.Figure 2
Diffraction patterns forα-Alu and γ-Alu spheres.


#### 3.1.3. SEM/EDS

Figures3 and 4 show the micrographs of the α-Alu and γ-Alu spheres; in these micrographs, it is observed that the surface of the alumina sphere is smooth, uniform, and with pores (Figure 3(a)), and the porosity is greater in the γ-Alu sphere according to SEM micrograph magnifications of the studied area (Figures 4(b)–4(d)). Also, it was observed a higher degree of sintering in the α-Alu sphere where there are well-defined grains in the form of hexagonal plates and some small fibers (Figures 3(b)–3(d)); it is reported in the literature that the formation of structures is obtained in sintered α-Alu composites. The materials after dye sorption were analyzed by SEM; therefore, no changes were observed in the images or elemental composition because the presence of the R40 on the surface was not detected by the instrument (figure does not show). EDS analysis was performed on the periphery and on the core of the γ-Alu and α-Alu spheres; the analysis only shows aluminum and oxygen as the main components and traces of barium due to the encapsulation process of the alumina spheres with barium chloride.Figure 3
SEM images forα-Alu at (a) 30x, (b) 5000x, (c) 7000x, and (d) 15000x.
(a)(b)(c)(d)Figure 4
SEM images forγ -Alu at (a) 35x, (b) 500x, (c) 1000x, and (d) 5000x.
(a)(b)(c)(d)


#### 3.1.4. Specific Surface Area (SBET)

The result of SBET shows a specific surface area of 190 m2/g, pore volume of 0.52 cm3/g, and pore diameter 11 nm for γ-Alu and specific surface area of 0.66 m2/g, pore volume of 0.0016 cm3/g, and pore diameter 10.19 nm for α-Alu. These results confirm the fact that sintering process forms a more solid mass of ceramic material with low surface areas.


### 3.2. Azo Dye (R40) Removal

#### 3.2.1. Sorption Kinetics

The removal of R40 was carried out by adsorption withα-Alu and γ-Alu spheres synthesized by the encapsulation method; the results showed that only γ-Alu spheres were capable to remove the R40 dye from aqueous media (82% R40 removal); on the other hand, α-Alu spheres did not show any important sorption capacity (1.8% R40 removal) (Figure 5). Because of these results, the consequent experiments were performed only by using the material that presented sorption capacity (γ-Alu spheres). By increasing the contact time and the initial concentration of R40, the capacity of the sphere to remove the dye continually increased until equilibrium establishment.Figure 5
Sorption kinetic test for R40 removal byα-Alu and γ-Alu spheres.(1) Effect of Initial Concentration on Sorption Process. The effect of the R40 initial concentration onto sorption process was conducted at 10, 50, and 100 mg/L. Figure 6 shows the sorption kinetics of γ-Alu spheres and the R40 dye decrease as function of the time. The γ-Alu spheres reached 82, 27, and 19% OTC removal at C0 =10, 50, and 100 mg/L, respectively.Figure 6
Effect of initial concentration on the sorption of R40 ontoγ-Alu spheres.The effect of contact time on dye sorption such as orange G (OG) by alumina particles was reported previously at 28°C and the results showed that the sorption capacity was higher when the contact time rises to 30 min until the equilibrium was reached [12]. This work assumes that the required time to accomplish OG-alumina nanoparticle interactions into equilibrium state was 30 min under the different dye concentrations. In this case, the interaction is independent from initial dye concentrations. In the present study, only γ-Alu spheres showed sorption capacity, but it does not coincide with that result; the time required to attain steady state was higher (more than 24 h). For R40 sorption evaluation on the γ-Alu spheres, the experimental results from sorption tests were adjusted to the pseudo-first order (PFO), pseudo-second order (PSO), intraparticle diffusion (ID), and Elovich (ELOV) models. The PFO equation permitted to discover the sorption capacity of the adsorbent: 8.1, 13.6, and 19.0 mg/g at C0 =10, 50, and 100 mg/L, respectively, also the sorption rate constants and the correlation coefficients for γ-Alu spheres. The fitting of the experimental results to the equations is described in Table 1. The PFO kinetic model has acceptable R values for 10 and 50 mg/L, showing that the sorption process takes place on a homogeneous surface considered the available sorption sites [13]. When equilibrium was reached approximately between 24 and 48 h, the sorption capacity remains without important changes. The sorption rate becomes a constant value because no more binding sites are available.Table 1
Kinetic parameters from the PFO, PSO, ID, and ELOV models applied to the adsorption process of R40 on theγ-Alu spheres at C0 =10, 50, and 100 mg/L.
Kinetic modelC0 =10 mg/LR40 removal =81.9793 ± 0.4782%ParametersPFOqe (mg/g)8.1979kL(h-1)0.0177R0.9818PSOk (g/mgh)21.2427R0.9699IDkid (mg/g/min)0.6146R0.9966ELOVa0.6268b0.1662R0.9952Kinetic modelC0 = 50 mg/LR40 removal =27.1959 ± 0.5776%ParametersPFOqe (mg/g)13.5980kL(h-1)0.0166R0.9830PSOk (g/mgh)76.5649R0.9409IDkid (mg/g/min)1.0129R0.9913ELOVa0.9393b0.0943R0.9944Kinetic modelC0 =100 mg/LR40 removal =18.9865 ± 4.9235%ParametersPFOqe (mg/g)18.9865kL(h-1)0.0223R0.9045PSOk (g/mgh)433.017R0.9357IDkid (mg/g/min)1.5623R0.9483ELOVa2.6635b0.0879R0.9396The dye removal at the initial contact time could be due to the sorption sites on the spheres because they were empty and able to retain dye anions from the aqueous phase [14]. As the sorption proceeds on the materials, the rate is getting slow and sorption gets the equilibrium, meaning the active sites saturation. On the other hand, the adjustment to the PSO kinetic model was lower at low concentrations (10 and 50 mg/L), giving the assumption that chemical sorption is the speed limiting step, involving valence forces when sharing or exchanging electrons between spheres and azo dye [15]. When the results were fitted to ELOV, the R value was important (>0.9), then a chemical sorption between the functional groups of the spheres and the dye was done [16].(2) Effect of pH on Sorption Process. The effect of pH variations (at 3, 5, and 10) of the aqueous solution over the R40 sorption was evaluated through adsorption kinetics (C0 =10 mg/L). In sorption processes, the pH value is a very important parameter that can affect the sorption capacity of the γ-Alu spheres [17]. The R40 removal improves at low pH values of the media, being 95 and 85% for pH 3 and 5, respectively, and 54% R40 removal for higher pH value (pH =10) (Figure 7). The pH of the system can show higher effect on the uptake of azo dye on γ-Alu spheres’ surface. This effect is promoted by the H+ concentration that establish the total charge of the spheres and the level of ionization/dissociation of the R40 azo dye; this can determine the electrostatic interaction linking the R40 and the γ-Alu spheres. The assessment of the pH effect on the sorption can supply data about the electrostatic interactions [18].Figure 7
Effect of pH on the sorción of R40 ontoγ-Alu spheres.At pH 10, the negative surface charge on theγ-Alu spheres rises, escalating the repulsion by electrostatic interactions between the material and the R40 (54% at pH =10), and because of that, the R40 removal at high pH is lower than at acid pH of the aqueous media. Table 2 shows the kinetic parameters from the fitting of experimental data to PFO, PSO, ID, and Elovich models, and it was observed that the pH modification does not affect the fitting to previous kinetic models. In all cases, the PFO was the equation that describes in better way the sorption process compared to PSO. Moreover, ELOV model fitted to the experimental data, elucidating a chemical sorption of R40 onto the γ-Alu spheres.Table 2
Kinetic parameters from the adjustment of PFO, PSO, ID, and ELOV models applied to the adsorption process of R40 on theγ-Alu spheres at pH =3.0, 5.0, and 10.0 (C0 =10 mg/L).
Kinetic modelpH 3.0R40 removal =94.9610 ± 0.1978%ParametersPFOqe (mg/g)9.4961kL(h-1)0.0147R0.9921PSOk (g/mgh)20.5581R0.9768IDk (mg/g/min)0.5235R0.9683ELOVa0.6806b0.1740R0.9942Kinetic modelpH 5.0R40 removal =84.5150 ± 0.4782%ParametersPFOqe (mg/g)8.4515kL(h-1)0.0177R0.9818PSOk (g/mgh)21.2427R0.9699IDk (mg/g/min)0.6146R0.9966ELOVa0.6268b0.1662R0.9952Kinetic modelpH 10.0R40 removal =53.7524 ± 0.6108%ParametersPFOqe (mg/g)5.3752kL(h-1)0.0051R0.9862PSOk (g/mgh)1.7872R0.9394IDk (mg/g/min)0.2320R0.9917ELOVa0.0807b0.1719R0.9905The sorption mechanism can be elucidated based on the surface chemistry of theγ-Alu spheres where the presence of a metal oxide in the aqueous phase leads to the hydroxylation of the metal oxide surface [19]. Under these conditions, the metal oxide surface is amphoteric, and it can lead toward acid-base reactions by the pH modification [12].A possible mechanism of this phenomenon is the pH dependence of theγ-Alu spheres’ surface. At high pH values, the net surface charge gets negative due to deprotonation, leading to low sorption of organic molecules because of columbic repulsion. In acidic pH condition (pH =3 and 5), the surface is positively charged, and is electrostatically attracted to the R40 anionic species leading to a higher adsorption of R40 anions (Figure 8). Other studies have reported the adsorption of anionic dyes with similar behavior [19–21].Figure 8
Possible mechanism for R40 sorption ontoγ-Alu spheres.The actual mechanistic step that commands the sorption process rate has been reported by other researchers [12] by employing the experimental results from all kinetic tests in the ID model [22]. By plotting a linear relationship and the intercept in zero, it is suitable to determine if the ID model can describe the sorption process and it is indicative of pore diffusion, being in this case the rate controlling step (Figure 9).Figure 9
Intraparticle diffusion plots obtained for various sorption processes at (a) different initial concentrations (C0 =10, 50, and 100 mg/L) and (b) pH values (3, 5, and 10).
(a)(b)The plots ofqe vs t0.5 are almost straight over the entire time range, and they are only in one linear section (single segmented plots) in the test at different initial concentrations (Figure 9(a)). In other studies, it was established that the presence of several segments in the plots validates the participation of a phenomenon in multiple stages for the sorption of dyes by alumina nanoparticles [12]. In the case of R40 sorption onto γ-Alu spheres at C0 =10, 50, and 100 mg/L (Figure 9(a)), the first linear plot demonstrates external mass transfer, in which the adsorbate migrated through solution to the external surface of the adsorbent resulting in high uptake rate. The results advise that the rate limiting step is intraparticle diffusion and the R40 sorption process is controlled by this mechanism. In the case of pH value variation (pH =3, 5, and 10), the plot showed only one segment for pH =10, but at pH =3 and 5, it was clear that the sorption follows multisegmented plots (Figure 9(b)), indicating that the R40 molecules move into the interior of the γ-Alu spheres by intraparticle diffusion (second linear segment in the plot). Moreover, the rate constant (kid) values (Table 1) have the same trend as that reported for PFO and PSO kinetic models.


#### 3.2.2. Sorption Isotherms

The isotherm tests were applied to obtain data about the interaction between the R40 concentration in water and the amount of R40 removed by theγ-Alu spheres at constant temperature. The experiment was performed by contact test using distilled water and another one with ion strength; the Langmuir, Freundlich, Temkin, and Dubinin-Radushkevich isotherm models were used. The γ-Alu spheres showed qe =7.6 mg/g in distilled media and 7.5 mg/g in water with ionic strength.Equilibrium data obtained by nonlinear fitting of the experimental results provided information of sorption capacity and enabled practical design, and possible use of the materials in advanced water treatment [23]. In a previous study, the sorption capacity of a magnetic nanocomposite (Fe3O4@CuS@Ni2P-CNTs) for R40 removal was tested; the experimental results confirmed the formation of a R40 monolayer onto the adsorbent (Langmuir fitting) at the tested concentration intervals [24]. The Langmuir model is based on the monolayer adsorption of R40 onto homogenous surface of γ-Alu spheres; it assumes that all adsorptive sites are the same and only one molecule is present as thickness. This leads to a surface with specific number of sorption sites, so R40 was retained onto monolayer of synthetized spheres, while Freundlich equation is employed to suppose the multilayer sorption of R40 onto heterogeneous surface [25]. In the present study, the Freundlich model showed the best fitting to the kinetic tests (R >0.98). The Kf is related to the sorption force and 1/n gives an estimation of the R40 sorption intensity [12] being this intensity higher for sorption process in distilled media than ionic water (Table 3). The adsorption capacity of the γ-Alu spheres increased until a maximum of 7.5 mg/g with the R40 concentration increase in water. The uptake capacity of the adsorbent is a result of high driving force for mass transfer [26].Table 3
Parameters obtained from the adjustment of Langmuir, Freundlich, Temkin, and Dubinin-Radushkevich isotherm models applied to the adsorption process of OTC on theγ-Alu spheres in distilled and ionic water.
Isotherm modelDistilled waterParametersLangmuirb1.7701Kt (mg/g)7.6189R0.9406Freundlichn0.6360Kf4.5980R0.9895TemkinB1.4810BT1672.9R0.8205Dubinin-Radushkevichqs (mg/g)7.6189KD (mol2/kJ2)-3 × 10-9R0.9421Isotherm modelIonic waterParametersLangmuirb1.4089Kt (mg/g)7.5434R0.9391Freundlichn0.7202Kf3.8771R0.9948TemkinB0.4693BT5279.2R0.8987Dubinin-Radushkevichqs (mg/g)7.5434KD (mol2/kJ2)-4 × 10-9R0.9741The application of the Temkin model was useful to obtain theB constant associated to adsorption heat. If B values are placed in the interval of 8 to 16 kJ/mol, the removal of R40 occurs by chemical interactions, but if the value is situated under 8 kJ/mol, the sorption process occurs by physical interactions [27]. This last case occurs for the R40 sorption process of R40 onto γ-Alu spheres in both media (B =0.5 to 1.5 for ions presence and distilled media, respectively). The Dubinin-Radushkevich (D-R) isotherm equations establish a relationship between the size of micropores and the equilibrium sorption ratio; this relation can be indicated by the sorption potential (ε). In a general way, the D-R model is used to describe the sorption mechanisms with a Gaussian energy distribution onto the heterogeneous surface of the adsorbent [28].In a recent study, the organic dye methylene blue (MB) adsorption onto Al2O3 nanofibers was described using the Langmuir and Freundlich isotherm models, and the fitting was better for the Langmuir equation [29]. This indicates that MB adsorption onto porous alumina is carried out by monolayer adsorption process on the adsorbent homogeneous surface, without considering the interaction between adsorbate molecules. In the present study, the behavior was opposite (best fitting to Freundlich), inferring that the adsorption process was done onto a heterogeneous surface.(1) Effect of Competing Ions over R40 Sorption. To study the behavior of the γ-Alu spheres under more realistic conditions, the sorption process was featured under ion strength promoting the contact between adsorbent and adsorbate in aqueous media with presence of calcium, bicarbonates, magnesium, sodium, silicon, sulfates, chlorides, nitrates, and carbonates. The ionic strength in the medium did not significantly affect the performance of the sorption process. The results showed that γ-Alu spheres presented affinity for R40 dye, and the maximum adsorption capacity did not change when it was compared to the sorption tests that take place in distilled media. The interfering ions occupy the sorption sites of the γ-Alu spheres, probably due to a competition between these ions and the R40 molecules. Therefore, in the sorption tests with ionic strength, usually the capacity of the adsorbents to remove molecules is affected [30, 31]. The γ-Alu spheres showed a good fitting to the Langmuir equation (R =0.94) (Table 3), but the fit for Freundlich was better (R =0.99). The n parameter of the Freundlich model was lower than 1, so the spheres showed an important retention of R40 dye. For the Temkin equation, γ-Alu spheres had a better fit with the presence of ions than in distilled media; this suggests that part of the energy of the medium go down while take place interactions between the γ-Alu spheres and the R40 dye [31].The ionic strength slightly affects the sorption capacity of theγ-Alu spheres. The dependence for R40 sorption decreased when some electrolytes are present in the aqueous media, so a cation exchange could occur as sorption mechanism [32]. In general, other researchers found that ionic strength (SO42−) slightly inhibits the organic molecule’s elimination by some adsorbents, due to the sorption determined by cation sorption and by H-bonding competition [33].


### 3.3. Regeneration Cycles

The re-use of the saturated adsorbent materials is a very important topic to ensure the sustainability of the process; this re-use can be achieved by regeneration of theγ-Alu spheres. The regeneration of the adsorbent materials is vital at industrial scales and the option to have access to the use of the adsorbent several cycles without reducing their performance is very important. In the present work, the re-use of γ-Alu spheres was promoted by thermic method (450°C/60 min). After thermal treatment, the sorption process was performed by 5 cycles under the same conditions than the original process (initial concentration of 10, 50, and 100 mg/L and pH values of 3, 5, and 10). The results showed that in almost all the cases, the performance of the γ-Alu spheres was not affected after thermal treatment and in the sorption capacity, it was acceptable along all the 5 sorption cycles for R40 removal (Figure 10).Figure 10
Sorption cycles of R40 ontoγ-Alu spheres after regeneration.
(a)(b)Other research findings (Table4) showed that the sorption capacity of different adsorbent materials goes from 0.46 mg/g for a commercial 4A zeolite (4AZ) [39] and higher as 29.4 mg/g for a modified organoclay - C3H1[38]. The qe values for the synthetized α- and γ-Alu spheres are in the interval of 0.1765 to 18.9865 mg/g; these novel adsorbent materials have interesting sorption capacities compared to those existing already. Moreover, the γ-Alu spheres have important regeneration properties that allow to use them in consequent sorption cycles.Table 4
Comparison of R40 removal by different adsorbent materials.
Adsorbent materialSorption capacityqe (mg/g)ReferenceZirconia fibers0.8950Ávila-Martínez et al. [34]Activated charcoal (walnut shells)9.9865Herrera-García, Aguirre-Ramírez, and Torres-Pérez [35]Basic anion-exchanger (Lewatit MonoPlus M-600)3.4120Wawrzkiewicz and Hubicki [36, 37]Amberlite IRA-9009.9950Wawrzkiewicz and Hubicki [36, 37]Amberlite IRA-91010.095Wawrzkiewicz and Hubicki [36, 37]Modified organoclay - C3H129.400Ullah et al. [38]Modified organoclay - C2CB125.300Ullah et al. [38]Modified organoclay - C2S120.300Ullah et al. [38]Commercial 4A zeolite (4AZ)0.4627Erdoğan [39]α-Alu spheres (C0 =10 mg/L)0.1765This workγ-Alu spheres (C0 =10 mg/L)8.1979This workγ-Alu spheres (C0 = 50 mg/L)13.5980This workγ-Alu spheres (C0 =100 mg/L)18.9865This workγ-Alu spheres (pH =3.0)9.4961This workγ-Alu spheres (pH =5.0)8.4515This workγ-Alu spheres (pH =10.0)5.3752This work


## 3.1. Characterization of the Materials

### 3.1.1. Ft-IR

Figure1 shows the infrared spectra obtained from α-Alu and γ-Alu spheres. It was not observed typical vibrational bands as evidence of functional groups and bonds present in PVP and alginate. This fact was promoted by decomposition of organic molecules after spheres thermal treatment. Only the inorganic bonds from ceramic material were observed. At 968-400 cm-1, it was observed a wide band that represents the stretching vibration of Al-O bonds in different alumina polymorphs. At 830 and 507-530 cm-1 appear bands corresponding to γ-Al2O3, and at 800 cm-1 and 500-750 cm-1 were detected bands from aluminum in tetrahedral (AlO4) and octahedral (AlO6) coordination, respectively. The octahedral aluminum of α-alumina generates bands placed at 438-456, 491-499, 550, 576-601, 635-644, and 755-763 cm-1 [6]. The materials after dye sorption were analyzed; therefore, no changes were observed in the FT-IR spectra because the presence of the R40 on the surface was not in amounts to be detected by the instrument (figure does not show).Figure 1
Infrared spectra forα-Alu and γ-Alu spheres.


### 3.1.2. XRD

Figure2 shows diffraction patterns of α-Alu and γ-Alu spheres; small non-defined crystallographic peaks in the diffractogram are evidence of the presence of amorphous alumina in spheres. γ-Alu crystalline planes (222), (400), and (400) are located at 39°, 46°, and 67°, respectively; the γ-Alu characteristic peaks disappear at 1600°C to give a phase transition to α-alumina phase. The turnover is represented by the peak’s appearance at 25, 35, 37.5, 43, 52, 57, 61.5, 66, and 68°, corresponding to (012), (104), (110), (113), (024), (116), (018), (214), and (300) crystalline planes, respectively, when it was compared with JCPDS 83-2081 pattern.Figure 2
Diffraction patterns forα-Alu and γ-Alu spheres.


### 3.1.3. SEM/EDS

Figures3 and 4 show the micrographs of the α-Alu and γ-Alu spheres; in these micrographs, it is observed that the surface of the alumina sphere is smooth, uniform, and with pores (Figure 3(a)), and the porosity is greater in the γ-Alu sphere according to SEM micrograph magnifications of the studied area (Figures 4(b)–4(d)). Also, it was observed a higher degree of sintering in the α-Alu sphere where there are well-defined grains in the form of hexagonal plates and some small fibers (Figures 3(b)–3(d)); it is reported in the literature that the formation of structures is obtained in sintered α-Alu composites. The materials after dye sorption were analyzed by SEM; therefore, no changes were observed in the images or elemental composition because the presence of the R40 on the surface was not detected by the instrument (figure does not show). EDS analysis was performed on the periphery and on the core of the γ-Alu and α-Alu spheres; the analysis only shows aluminum and oxygen as the main components and traces of barium due to the encapsulation process of the alumina spheres with barium chloride.Figure 3
SEM images forα-Alu at (a) 30x, (b) 5000x, (c) 7000x, and (d) 15000x.
(a)(b)(c)(d)Figure 4
SEM images forγ -Alu at (a) 35x, (b) 500x, (c) 1000x, and (d) 5000x.
(a)(b)(c)(d)


### 3.1.4. Specific Surface Area (SBET)

The result of SBET shows a specific surface area of 190 m2/g, pore volume of 0.52 cm3/g, and pore diameter 11 nm for γ-Alu and specific surface area of 0.66 m2/g, pore volume of 0.0016 cm3/g, and pore diameter 10.19 nm for α-Alu. These results confirm the fact that sintering process forms a more solid mass of ceramic material with low surface areas.


## 3.1.1. Ft-IR

Figure1 shows the infrared spectra obtained from α-Alu and γ-Alu spheres. It was not observed typical vibrational bands as evidence of functional groups and bonds present in PVP and alginate. This fact was promoted by decomposition of organic molecules after spheres thermal treatment. Only the inorganic bonds from ceramic material were observed. At 968-400 cm-1, it was observed a wide band that represents the stretching vibration of Al-O bonds in different alumina polymorphs. At 830 and 507-530 cm-1 appear bands corresponding to γ-Al2O3, and at 800 cm-1 and 500-750 cm-1 were detected bands from aluminum in tetrahedral (AlO4) and octahedral (AlO6) coordination, respectively. The octahedral aluminum of α-alumina generates bands placed at 438-456, 491-499, 550, 576-601, 635-644, and 755-763 cm-1 [6]. The materials after dye sorption were analyzed; therefore, no changes were observed in the FT-IR spectra because the presence of the R40 on the surface was not in amounts to be detected by the instrument (figure does not show).Figure 1
Infrared spectra forα-Alu and γ-Alu spheres.


## 3.1.2. XRD

Figure2 shows diffraction patterns of α-Alu and γ-Alu spheres; small non-defined crystallographic peaks in the diffractogram are evidence of the presence of amorphous alumina in spheres. γ-Alu crystalline planes (222), (400), and (400) are located at 39°, 46°, and 67°, respectively; the γ-Alu characteristic peaks disappear at 1600°C to give a phase transition to α-alumina phase. The turnover is represented by the peak’s appearance at 25, 35, 37.5, 43, 52, 57, 61.5, 66, and 68°, corresponding to (012), (104), (110), (113), (024), (116), (018), (214), and (300) crystalline planes, respectively, when it was compared with JCPDS 83-2081 pattern.Figure 2
Diffraction patterns forα-Alu and γ-Alu spheres.


## 3.1.3. SEM/EDS

Figures3 and 4 show the micrographs of the α-Alu and γ-Alu spheres; in these micrographs, it is observed that the surface of the alumina sphere is smooth, uniform, and with pores (Figure 3(a)), and the porosity is greater in the γ-Alu sphere according to SEM micrograph magnifications of the studied area (Figures 4(b)–4(d)). Also, it was observed a higher degree of sintering in the α-Alu sphere where there are well-defined grains in the form of hexagonal plates and some small fibers (Figures 3(b)–3(d)); it is reported in the literature that the formation of structures is obtained in sintered α-Alu composites. The materials after dye sorption were analyzed by SEM; therefore, no changes were observed in the images or elemental composition because the presence of the R40 on the surface was not detected by the instrument (figure does not show). EDS analysis was performed on the periphery and on the core of the γ-Alu and α-Alu spheres; the analysis only shows aluminum and oxygen as the main components and traces of barium due to the encapsulation process of the alumina spheres with barium chloride.Figure 3
SEM images forα-Alu at (a) 30x, (b) 5000x, (c) 7000x, and (d) 15000x.
(a)(b)(c)(d)Figure 4
SEM images forγ -Alu at (a) 35x, (b) 500x, (c) 1000x, and (d) 5000x.
(a)(b)(c)(d)


## 3.1.4. Specific Surface Area (SBET)

The result of SBET shows a specific surface area of 190 m2/g, pore volume of 0.52 cm3/g, and pore diameter 11 nm for γ-Alu and specific surface area of 0.66 m2/g, pore volume of 0.0016 cm3/g, and pore diameter 10.19 nm for α-Alu. These results confirm the fact that sintering process forms a more solid mass of ceramic material with low surface areas.


## 3.2. Azo Dye (R40) Removal

### 3.2.1. Sorption Kinetics

The removal of R40 was carried out by adsorption withα-Alu and γ-Alu spheres synthesized by the encapsulation method; the results showed that only γ-Alu spheres were capable to remove the R40 dye from aqueous media (82% R40 removal); on the other hand, α-Alu spheres did not show any important sorption capacity (1.8% R40 removal) (Figure 5). Because of these results, the consequent experiments were performed only by using the material that presented sorption capacity (γ-Alu spheres). By increasing the contact time and the initial concentration of R40, the capacity of the sphere to remove the dye continually increased until equilibrium establishment.Figure 5
Sorption kinetic test for R40 removal byα-Alu and γ-Alu spheres.(1) Effect of Initial Concentration on Sorption Process. The effect of the R40 initial concentration onto sorption process was conducted at 10, 50, and 100 mg/L. Figure 6 shows the sorption kinetics of γ-Alu spheres and the R40 dye decrease as function of the time. The γ-Alu spheres reached 82, 27, and 19% OTC removal at C0 =10, 50, and 100 mg/L, respectively.Figure 6
Effect of initial concentration on the sorption of R40 ontoγ-Alu spheres.The effect of contact time on dye sorption such as orange G (OG) by alumina particles was reported previously at 28°C and the results showed that the sorption capacity was higher when the contact time rises to 30 min until the equilibrium was reached [12]. This work assumes that the required time to accomplish OG-alumina nanoparticle interactions into equilibrium state was 30 min under the different dye concentrations. In this case, the interaction is independent from initial dye concentrations. In the present study, only γ-Alu spheres showed sorption capacity, but it does not coincide with that result; the time required to attain steady state was higher (more than 24 h). For R40 sorption evaluation on the γ-Alu spheres, the experimental results from sorption tests were adjusted to the pseudo-first order (PFO), pseudo-second order (PSO), intraparticle diffusion (ID), and Elovich (ELOV) models. The PFO equation permitted to discover the sorption capacity of the adsorbent: 8.1, 13.6, and 19.0 mg/g at C0 =10, 50, and 100 mg/L, respectively, also the sorption rate constants and the correlation coefficients for γ-Alu spheres. The fitting of the experimental results to the equations is described in Table 1. The PFO kinetic model has acceptable R values for 10 and 50 mg/L, showing that the sorption process takes place on a homogeneous surface considered the available sorption sites [13]. When equilibrium was reached approximately between 24 and 48 h, the sorption capacity remains without important changes. The sorption rate becomes a constant value because no more binding sites are available.Table 1
Kinetic parameters from the PFO, PSO, ID, and ELOV models applied to the adsorption process of R40 on theγ-Alu spheres at C0 =10, 50, and 100 mg/L.
Kinetic modelC0 =10 mg/LR40 removal =81.9793 ± 0.4782%ParametersPFOqe (mg/g)8.1979kL(h-1)0.0177R0.9818PSOk (g/mgh)21.2427R0.9699IDkid (mg/g/min)0.6146R0.9966ELOVa0.6268b0.1662R0.9952Kinetic modelC0 = 50 mg/LR40 removal =27.1959 ± 0.5776%ParametersPFOqe (mg/g)13.5980kL(h-1)0.0166R0.9830PSOk (g/mgh)76.5649R0.9409IDkid (mg/g/min)1.0129R0.9913ELOVa0.9393b0.0943R0.9944Kinetic modelC0 =100 mg/LR40 removal =18.9865 ± 4.9235%ParametersPFOqe (mg/g)18.9865kL(h-1)0.0223R0.9045PSOk (g/mgh)433.017R0.9357IDkid (mg/g/min)1.5623R0.9483ELOVa2.6635b0.0879R0.9396The dye removal at the initial contact time could be due to the sorption sites on the spheres because they were empty and able to retain dye anions from the aqueous phase [14]. As the sorption proceeds on the materials, the rate is getting slow and sorption gets the equilibrium, meaning the active sites saturation. On the other hand, the adjustment to the PSO kinetic model was lower at low concentrations (10 and 50 mg/L), giving the assumption that chemical sorption is the speed limiting step, involving valence forces when sharing or exchanging electrons between spheres and azo dye [15]. When the results were fitted to ELOV, the R value was important (>0.9), then a chemical sorption between the functional groups of the spheres and the dye was done [16].(2) Effect of pH on Sorption Process. The effect of pH variations (at 3, 5, and 10) of the aqueous solution over the R40 sorption was evaluated through adsorption kinetics (C0 =10 mg/L). In sorption processes, the pH value is a very important parameter that can affect the sorption capacity of the γ-Alu spheres [17]. The R40 removal improves at low pH values of the media, being 95 and 85% for pH 3 and 5, respectively, and 54% R40 removal for higher pH value (pH =10) (Figure 7). The pH of the system can show higher effect on the uptake of azo dye on γ-Alu spheres’ surface. This effect is promoted by the H+ concentration that establish the total charge of the spheres and the level of ionization/dissociation of the R40 azo dye; this can determine the electrostatic interaction linking the R40 and the γ-Alu spheres. The assessment of the pH effect on the sorption can supply data about the electrostatic interactions [18].Figure 7
Effect of pH on the sorción of R40 ontoγ-Alu spheres.At pH 10, the negative surface charge on theγ-Alu spheres rises, escalating the repulsion by electrostatic interactions between the material and the R40 (54% at pH =10), and because of that, the R40 removal at high pH is lower than at acid pH of the aqueous media. Table 2 shows the kinetic parameters from the fitting of experimental data to PFO, PSO, ID, and Elovich models, and it was observed that the pH modification does not affect the fitting to previous kinetic models. In all cases, the PFO was the equation that describes in better way the sorption process compared to PSO. Moreover, ELOV model fitted to the experimental data, elucidating a chemical sorption of R40 onto the γ-Alu spheres.Table 2
Kinetic parameters from the adjustment of PFO, PSO, ID, and ELOV models applied to the adsorption process of R40 on theγ-Alu spheres at pH =3.0, 5.0, and 10.0 (C0 =10 mg/L).
Kinetic modelpH 3.0R40 removal =94.9610 ± 0.1978%ParametersPFOqe (mg/g)9.4961kL(h-1)0.0147R0.9921PSOk (g/mgh)20.5581R0.9768IDk (mg/g/min)0.5235R0.9683ELOVa0.6806b0.1740R0.9942Kinetic modelpH 5.0R40 removal =84.5150 ± 0.4782%ParametersPFOqe (mg/g)8.4515kL(h-1)0.0177R0.9818PSOk (g/mgh)21.2427R0.9699IDk (mg/g/min)0.6146R0.9966ELOVa0.6268b0.1662R0.9952Kinetic modelpH 10.0R40 removal =53.7524 ± 0.6108%ParametersPFOqe (mg/g)5.3752kL(h-1)0.0051R0.9862PSOk (g/mgh)1.7872R0.9394IDk (mg/g/min)0.2320R0.9917ELOVa0.0807b0.1719R0.9905The sorption mechanism can be elucidated based on the surface chemistry of theγ-Alu spheres where the presence of a metal oxide in the aqueous phase leads to the hydroxylation of the metal oxide surface [19]. Under these conditions, the metal oxide surface is amphoteric, and it can lead toward acid-base reactions by the pH modification [12].A possible mechanism of this phenomenon is the pH dependence of theγ-Alu spheres’ surface. At high pH values, the net surface charge gets negative due to deprotonation, leading to low sorption of organic molecules because of columbic repulsion. In acidic pH condition (pH =3 and 5), the surface is positively charged, and is electrostatically attracted to the R40 anionic species leading to a higher adsorption of R40 anions (Figure 8). Other studies have reported the adsorption of anionic dyes with similar behavior [19–21].Figure 8
Possible mechanism for R40 sorption ontoγ-Alu spheres.The actual mechanistic step that commands the sorption process rate has been reported by other researchers [12] by employing the experimental results from all kinetic tests in the ID model [22]. By plotting a linear relationship and the intercept in zero, it is suitable to determine if the ID model can describe the sorption process and it is indicative of pore diffusion, being in this case the rate controlling step (Figure 9).Figure 9
Intraparticle diffusion plots obtained for various sorption processes at (a) different initial concentrations (C0 =10, 50, and 100 mg/L) and (b) pH values (3, 5, and 10).
(a)(b)The plots ofqe vs t0.5 are almost straight over the entire time range, and they are only in one linear section (single segmented plots) in the test at different initial concentrations (Figure 9(a)). In other studies, it was established that the presence of several segments in the plots validates the participation of a phenomenon in multiple stages for the sorption of dyes by alumina nanoparticles [12]. In the case of R40 sorption onto γ-Alu spheres at C0 =10, 50, and 100 mg/L (Figure 9(a)), the first linear plot demonstrates external mass transfer, in which the adsorbate migrated through solution to the external surface of the adsorbent resulting in high uptake rate. The results advise that the rate limiting step is intraparticle diffusion and the R40 sorption process is controlled by this mechanism. In the case of pH value variation (pH =3, 5, and 10), the plot showed only one segment for pH =10, but at pH =3 and 5, it was clear that the sorption follows multisegmented plots (Figure 9(b)), indicating that the R40 molecules move into the interior of the γ-Alu spheres by intraparticle diffusion (second linear segment in the plot). Moreover, the rate constant (kid) values (Table 1) have the same trend as that reported for PFO and PSO kinetic models.


### 3.2.2. Sorption Isotherms

The isotherm tests were applied to obtain data about the interaction between the R40 concentration in water and the amount of R40 removed by theγ-Alu spheres at constant temperature. The experiment was performed by contact test using distilled water and another one with ion strength; the Langmuir, Freundlich, Temkin, and Dubinin-Radushkevich isotherm models were used. The γ-Alu spheres showed qe =7.6 mg/g in distilled media and 7.5 mg/g in water with ionic strength.Equilibrium data obtained by nonlinear fitting of the experimental results provided information of sorption capacity and enabled practical design, and possible use of the materials in advanced water treatment [23]. In a previous study, the sorption capacity of a magnetic nanocomposite (Fe3O4@CuS@Ni2P-CNTs) for R40 removal was tested; the experimental results confirmed the formation of a R40 monolayer onto the adsorbent (Langmuir fitting) at the tested concentration intervals [24]. The Langmuir model is based on the monolayer adsorption of R40 onto homogenous surface of γ-Alu spheres; it assumes that all adsorptive sites are the same and only one molecule is present as thickness. This leads to a surface with specific number of sorption sites, so R40 was retained onto monolayer of synthetized spheres, while Freundlich equation is employed to suppose the multilayer sorption of R40 onto heterogeneous surface [25]. In the present study, the Freundlich model showed the best fitting to the kinetic tests (R >0.98). The Kf is related to the sorption force and 1/n gives an estimation of the R40 sorption intensity [12] being this intensity higher for sorption process in distilled media than ionic water (Table 3). The adsorption capacity of the γ-Alu spheres increased until a maximum of 7.5 mg/g with the R40 concentration increase in water. The uptake capacity of the adsorbent is a result of high driving force for mass transfer [26].Table 3
Parameters obtained from the adjustment of Langmuir, Freundlich, Temkin, and Dubinin-Radushkevich isotherm models applied to the adsorption process of OTC on theγ-Alu spheres in distilled and ionic water.
Isotherm modelDistilled waterParametersLangmuirb1.7701Kt (mg/g)7.6189R0.9406Freundlichn0.6360Kf4.5980R0.9895TemkinB1.4810BT1672.9R0.8205Dubinin-Radushkevichqs (mg/g)7.6189KD (mol2/kJ2)-3 × 10-9R0.9421Isotherm modelIonic waterParametersLangmuirb1.4089Kt (mg/g)7.5434R0.9391Freundlichn0.7202Kf3.8771R0.9948TemkinB0.4693BT5279.2R0.8987Dubinin-Radushkevichqs (mg/g)7.5434KD (mol2/kJ2)-4 × 10-9R0.9741The application of the Temkin model was useful to obtain theB constant associated to adsorption heat. If B values are placed in the interval of 8 to 16 kJ/mol, the removal of R40 occurs by chemical interactions, but if the value is situated under 8 kJ/mol, the sorption process occurs by physical interactions [27]. This last case occurs for the R40 sorption process of R40 onto γ-Alu spheres in both media (B =0.5 to 1.5 for ions presence and distilled media, respectively). The Dubinin-Radushkevich (D-R) isotherm equations establish a relationship between the size of micropores and the equilibrium sorption ratio; this relation can be indicated by the sorption potential (ε). In a general way, the D-R model is used to describe the sorption mechanisms with a Gaussian energy distribution onto the heterogeneous surface of the adsorbent [28].In a recent study, the organic dye methylene blue (MB) adsorption onto Al2O3 nanofibers was described using the Langmuir and Freundlich isotherm models, and the fitting was better for the Langmuir equation [29]. This indicates that MB adsorption onto porous alumina is carried out by monolayer adsorption process on the adsorbent homogeneous surface, without considering the interaction between adsorbate molecules. In the present study, the behavior was opposite (best fitting to Freundlich), inferring that the adsorption process was done onto a heterogeneous surface.(1) Effect of Competing Ions over R40 Sorption. To study the behavior of the γ-Alu spheres under more realistic conditions, the sorption process was featured under ion strength promoting the contact between adsorbent and adsorbate in aqueous media with presence of calcium, bicarbonates, magnesium, sodium, silicon, sulfates, chlorides, nitrates, and carbonates. The ionic strength in the medium did not significantly affect the performance of the sorption process. The results showed that γ-Alu spheres presented affinity for R40 dye, and the maximum adsorption capacity did not change when it was compared to the sorption tests that take place in distilled media. The interfering ions occupy the sorption sites of the γ-Alu spheres, probably due to a competition between these ions and the R40 molecules. Therefore, in the sorption tests with ionic strength, usually the capacity of the adsorbents to remove molecules is affected [30, 31]. The γ-Alu spheres showed a good fitting to the Langmuir equation (R =0.94) (Table 3), but the fit for Freundlich was better (R =0.99). The n parameter of the Freundlich model was lower than 1, so the spheres showed an important retention of R40 dye. For the Temkin equation, γ-Alu spheres had a better fit with the presence of ions than in distilled media; this suggests that part of the energy of the medium go down while take place interactions between the γ-Alu spheres and the R40 dye [31].The ionic strength slightly affects the sorption capacity of theγ-Alu spheres. The dependence for R40 sorption decreased when some electrolytes are present in the aqueous media, so a cation exchange could occur as sorption mechanism [32]. In general, other researchers found that ionic strength (SO42−) slightly inhibits the organic molecule’s elimination by some adsorbents, due to the sorption determined by cation sorption and by H-bonding competition [33].


## 3.2.1. Sorption Kinetics

The removal of R40 was carried out by adsorption withα-Alu and γ-Alu spheres synthesized by the encapsulation method; the results showed that only γ-Alu spheres were capable to remove the R40 dye from aqueous media (82% R40 removal); on the other hand, α-Alu spheres did not show any important sorption capacity (1.8% R40 removal) (Figure 5). Because of these results, the consequent experiments were performed only by using the material that presented sorption capacity (γ-Alu spheres). By increasing the contact time and the initial concentration of R40, the capacity of the sphere to remove the dye continually increased until equilibrium establishment.Figure 5
Sorption kinetic test for R40 removal byα-Alu and γ-Alu spheres.(1) Effect of Initial Concentration on Sorption Process. The effect of the R40 initial concentration onto sorption process was conducted at 10, 50, and 100 mg/L. Figure 6 shows the sorption kinetics of γ-Alu spheres and the R40 dye decrease as function of the time. The γ-Alu spheres reached 82, 27, and 19% OTC removal at C0 =10, 50, and 100 mg/L, respectively.Figure 6
Effect of initial concentration on the sorption of R40 ontoγ-Alu spheres.The effect of contact time on dye sorption such as orange G (OG) by alumina particles was reported previously at 28°C and the results showed that the sorption capacity was higher when the contact time rises to 30 min until the equilibrium was reached [12]. This work assumes that the required time to accomplish OG-alumina nanoparticle interactions into equilibrium state was 30 min under the different dye concentrations. In this case, the interaction is independent from initial dye concentrations. In the present study, only γ-Alu spheres showed sorption capacity, but it does not coincide with that result; the time required to attain steady state was higher (more than 24 h). For R40 sorption evaluation on the γ-Alu spheres, the experimental results from sorption tests were adjusted to the pseudo-first order (PFO), pseudo-second order (PSO), intraparticle diffusion (ID), and Elovich (ELOV) models. The PFO equation permitted to discover the sorption capacity of the adsorbent: 8.1, 13.6, and 19.0 mg/g at C0 =10, 50, and 100 mg/L, respectively, also the sorption rate constants and the correlation coefficients for γ-Alu spheres. The fitting of the experimental results to the equations is described in Table 1. The PFO kinetic model has acceptable R values for 10 and 50 mg/L, showing that the sorption process takes place on a homogeneous surface considered the available sorption sites [13]. When equilibrium was reached approximately between 24 and 48 h, the sorption capacity remains without important changes. The sorption rate becomes a constant value because no more binding sites are available.Table 1
Kinetic parameters from the PFO, PSO, ID, and ELOV models applied to the adsorption process of R40 on theγ-Alu spheres at C0 =10, 50, and 100 mg/L.
Kinetic modelC0 =10 mg/LR40 removal =81.9793 ± 0.4782%ParametersPFOqe (mg/g)8.1979kL(h-1)0.0177R0.9818PSOk (g/mgh)21.2427R0.9699IDkid (mg/g/min)0.6146R0.9966ELOVa0.6268b0.1662R0.9952Kinetic modelC0 = 50 mg/LR40 removal =27.1959 ± 0.5776%ParametersPFOqe (mg/g)13.5980kL(h-1)0.0166R0.9830PSOk (g/mgh)76.5649R0.9409IDkid (mg/g/min)1.0129R0.9913ELOVa0.9393b0.0943R0.9944Kinetic modelC0 =100 mg/LR40 removal =18.9865 ± 4.9235%ParametersPFOqe (mg/g)18.9865kL(h-1)0.0223R0.9045PSOk (g/mgh)433.017R0.9357IDkid (mg/g/min)1.5623R0.9483ELOVa2.6635b0.0879R0.9396The dye removal at the initial contact time could be due to the sorption sites on the spheres because they were empty and able to retain dye anions from the aqueous phase [14]. As the sorption proceeds on the materials, the rate is getting slow and sorption gets the equilibrium, meaning the active sites saturation. On the other hand, the adjustment to the PSO kinetic model was lower at low concentrations (10 and 50 mg/L), giving the assumption that chemical sorption is the speed limiting step, involving valence forces when sharing or exchanging electrons between spheres and azo dye [15]. When the results were fitted to ELOV, the R value was important (>0.9), then a chemical sorption between the functional groups of the spheres and the dye was done [16].(2) Effect of pH on Sorption Process. The effect of pH variations (at 3, 5, and 10) of the aqueous solution over the R40 sorption was evaluated through adsorption kinetics (C0 =10 mg/L). In sorption processes, the pH value is a very important parameter that can affect the sorption capacity of the γ-Alu spheres [17]. The R40 removal improves at low pH values of the media, being 95 and 85% for pH 3 and 5, respectively, and 54% R40 removal for higher pH value (pH =10) (Figure 7). The pH of the system can show higher effect on the uptake of azo dye on γ-Alu spheres’ surface. This effect is promoted by the H+ concentration that establish the total charge of the spheres and the level of ionization/dissociation of the R40 azo dye; this can determine the electrostatic interaction linking the R40 and the γ-Alu spheres. The assessment of the pH effect on the sorption can supply data about the electrostatic interactions [18].Figure 7
Effect of pH on the sorción of R40 ontoγ-Alu spheres.At pH 10, the negative surface charge on theγ-Alu spheres rises, escalating the repulsion by electrostatic interactions between the material and the R40 (54% at pH =10), and because of that, the R40 removal at high pH is lower than at acid pH of the aqueous media. Table 2 shows the kinetic parameters from the fitting of experimental data to PFO, PSO, ID, and Elovich models, and it was observed that the pH modification does not affect the fitting to previous kinetic models. In all cases, the PFO was the equation that describes in better way the sorption process compared to PSO. Moreover, ELOV model fitted to the experimental data, elucidating a chemical sorption of R40 onto the γ-Alu spheres.Table 2
Kinetic parameters from the adjustment of PFO, PSO, ID, and ELOV models applied to the adsorption process of R40 on theγ-Alu spheres at pH =3.0, 5.0, and 10.0 (C0 =10 mg/L).
Kinetic modelpH 3.0R40 removal =94.9610 ± 0.1978%ParametersPFOqe (mg/g)9.4961kL(h-1)0.0147R0.9921PSOk (g/mgh)20.5581R0.9768IDk (mg/g/min)0.5235R0.9683ELOVa0.6806b0.1740R0.9942Kinetic modelpH 5.0R40 removal =84.5150 ± 0.4782%ParametersPFOqe (mg/g)8.4515kL(h-1)0.0177R0.9818PSOk (g/mgh)21.2427R0.9699IDk (mg/g/min)0.6146R0.9966ELOVa0.6268b0.1662R0.9952Kinetic modelpH 10.0R40 removal =53.7524 ± 0.6108%ParametersPFOqe (mg/g)5.3752kL(h-1)0.0051R0.9862PSOk (g/mgh)1.7872R0.9394IDk (mg/g/min)0.2320R0.9917ELOVa0.0807b0.1719R0.9905The sorption mechanism can be elucidated based on the surface chemistry of theγ-Alu spheres where the presence of a metal oxide in the aqueous phase leads to the hydroxylation of the metal oxide surface [19]. Under these conditions, the metal oxide surface is amphoteric, and it can lead toward acid-base reactions by the pH modification [12].A possible mechanism of this phenomenon is the pH dependence of theγ-Alu spheres’ surface. At high pH values, the net surface charge gets negative due to deprotonation, leading to low sorption of organic molecules because of columbic repulsion. In acidic pH condition (pH =3 and 5), the surface is positively charged, and is electrostatically attracted to the R40 anionic species leading to a higher adsorption of R40 anions (Figure 8). Other studies have reported the adsorption of anionic dyes with similar behavior [19–21].Figure 8
Possible mechanism for R40 sorption ontoγ-Alu spheres.The actual mechanistic step that commands the sorption process rate has been reported by other researchers [12] by employing the experimental results from all kinetic tests in the ID model [22]. By plotting a linear relationship and the intercept in zero, it is suitable to determine if the ID model can describe the sorption process and it is indicative of pore diffusion, being in this case the rate controlling step (Figure 9).Figure 9
Intraparticle diffusion plots obtained for various sorption processes at (a) different initial concentrations (C0 =10, 50, and 100 mg/L) and (b) pH values (3, 5, and 10).
(a)(b)The plots ofqe vs t0.5 are almost straight over the entire time range, and they are only in one linear section (single segmented plots) in the test at different initial concentrations (Figure 9(a)). In other studies, it was established that the presence of several segments in the plots validates the participation of a phenomenon in multiple stages for the sorption of dyes by alumina nanoparticles [12]. In the case of R40 sorption onto γ-Alu spheres at C0 =10, 50, and 100 mg/L (Figure 9(a)), the first linear plot demonstrates external mass transfer, in which the adsorbate migrated through solution to the external surface of the adsorbent resulting in high uptake rate. The results advise that the rate limiting step is intraparticle diffusion and the R40 sorption process is controlled by this mechanism. In the case of pH value variation (pH =3, 5, and 10), the plot showed only one segment for pH =10, but at pH =3 and 5, it was clear that the sorption follows multisegmented plots (Figure 9(b)), indicating that the R40 molecules move into the interior of the γ-Alu spheres by intraparticle diffusion (second linear segment in the plot). Moreover, the rate constant (kid) values (Table 1) have the same trend as that reported for PFO and PSO kinetic models.


## 3.2.2. Sorption Isotherms

The isotherm tests were applied to obtain data about the interaction between the R40 concentration in water and the amount of R40 removed by theγ-Alu spheres at constant temperature. The experiment was performed by contact test using distilled water and another one with ion strength; the Langmuir, Freundlich, Temkin, and Dubinin-Radushkevich isotherm models were used. The γ-Alu spheres showed qe =7.6 mg/g in distilled media and 7.5 mg/g in water with ionic strength.Equilibrium data obtained by nonlinear fitting of the experimental results provided information of sorption capacity and enabled practical design, and possible use of the materials in advanced water treatment [23]. In a previous study, the sorption capacity of a magnetic nanocomposite (Fe3O4@CuS@Ni2P-CNTs) for R40 removal was tested; the experimental results confirmed the formation of a R40 monolayer onto the adsorbent (Langmuir fitting) at the tested concentration intervals [24]. The Langmuir model is based on the monolayer adsorption of R40 onto homogenous surface of γ-Alu spheres; it assumes that all adsorptive sites are the same and only one molecule is present as thickness. This leads to a surface with specific number of sorption sites, so R40 was retained onto monolayer of synthetized spheres, while Freundlich equation is employed to suppose the multilayer sorption of R40 onto heterogeneous surface [25]. In the present study, the Freundlich model showed the best fitting to the kinetic tests (R >0.98). The Kf is related to the sorption force and 1/n gives an estimation of the R40 sorption intensity [12] being this intensity higher for sorption process in distilled media than ionic water (Table 3). The adsorption capacity of the γ-Alu spheres increased until a maximum of 7.5 mg/g with the R40 concentration increase in water. The uptake capacity of the adsorbent is a result of high driving force for mass transfer [26].Table 3
Parameters obtained from the adjustment of Langmuir, Freundlich, Temkin, and Dubinin-Radushkevich isotherm models applied to the adsorption process of OTC on theγ-Alu spheres in distilled and ionic water.
Isotherm modelDistilled waterParametersLangmuirb1.7701Kt (mg/g)7.6189R0.9406Freundlichn0.6360Kf4.5980R0.9895TemkinB1.4810BT1672.9R0.8205Dubinin-Radushkevichqs (mg/g)7.6189KD (mol2/kJ2)-3 × 10-9R0.9421Isotherm modelIonic waterParametersLangmuirb1.4089Kt (mg/g)7.5434R0.9391Freundlichn0.7202Kf3.8771R0.9948TemkinB0.4693BT5279.2R0.8987Dubinin-Radushkevichqs (mg/g)7.5434KD (mol2/kJ2)-4 × 10-9R0.9741The application of the Temkin model was useful to obtain theB constant associated to adsorption heat. If B values are placed in the interval of 8 to 16 kJ/mol, the removal of R40 occurs by chemical interactions, but if the value is situated under 8 kJ/mol, the sorption process occurs by physical interactions [27]. This last case occurs for the R40 sorption process of R40 onto γ-Alu spheres in both media (B =0.5 to 1.5 for ions presence and distilled media, respectively). The Dubinin-Radushkevich (D-R) isotherm equations establish a relationship between the size of micropores and the equilibrium sorption ratio; this relation can be indicated by the sorption potential (ε). In a general way, the D-R model is used to describe the sorption mechanisms with a Gaussian energy distribution onto the heterogeneous surface of the adsorbent [28].In a recent study, the organic dye methylene blue (MB) adsorption onto Al2O3 nanofibers was described using the Langmuir and Freundlich isotherm models, and the fitting was better for the Langmuir equation [29]. This indicates that MB adsorption onto porous alumina is carried out by monolayer adsorption process on the adsorbent homogeneous surface, without considering the interaction between adsorbate molecules. In the present study, the behavior was opposite (best fitting to Freundlich), inferring that the adsorption process was done onto a heterogeneous surface.(1) Effect of Competing Ions over R40 Sorption. To study the behavior of the γ-Alu spheres under more realistic conditions, the sorption process was featured under ion strength promoting the contact between adsorbent and adsorbate in aqueous media with presence of calcium, bicarbonates, magnesium, sodium, silicon, sulfates, chlorides, nitrates, and carbonates. The ionic strength in the medium did not significantly affect the performance of the sorption process. The results showed that γ-Alu spheres presented affinity for R40 dye, and the maximum adsorption capacity did not change when it was compared to the sorption tests that take place in distilled media. The interfering ions occupy the sorption sites of the γ-Alu spheres, probably due to a competition between these ions and the R40 molecules. Therefore, in the sorption tests with ionic strength, usually the capacity of the adsorbents to remove molecules is affected [30, 31]. The γ-Alu spheres showed a good fitting to the Langmuir equation (R =0.94) (Table 3), but the fit for Freundlich was better (R =0.99). The n parameter of the Freundlich model was lower than 1, so the spheres showed an important retention of R40 dye. For the Temkin equation, γ-Alu spheres had a better fit with the presence of ions than in distilled media; this suggests that part of the energy of the medium go down while take place interactions between the γ-Alu spheres and the R40 dye [31].The ionic strength slightly affects the sorption capacity of theγ-Alu spheres. The dependence for R40 sorption decreased when some electrolytes are present in the aqueous media, so a cation exchange could occur as sorption mechanism [32]. In general, other researchers found that ionic strength (SO42−) slightly inhibits the organic molecule’s elimination by some adsorbents, due to the sorption determined by cation sorption and by H-bonding competition [33].


## 3.3. Regeneration Cycles

The re-use of the saturated adsorbent materials is a very important topic to ensure the sustainability of the process; this re-use can be achieved by regeneration of theγ-Alu spheres. The regeneration of the adsorbent materials is vital at industrial scales and the option to have access to the use of the adsorbent several cycles without reducing their performance is very important. In the present work, the re-use of γ-Alu spheres was promoted by thermic method (450°C/60 min). After thermal treatment, the sorption process was performed by 5 cycles under the same conditions than the original process (initial concentration of 10, 50, and 100 mg/L and pH values of 3, 5, and 10). The results showed that in almost all the cases, the performance of the γ-Alu spheres was not affected after thermal treatment and in the sorption capacity, it was acceptable along all the 5 sorption cycles for R40 removal (Figure 10).Figure 10
Sorption cycles of R40 ontoγ-Alu spheres after regeneration.
(a)(b)Other research findings (Table4) showed that the sorption capacity of different adsorbent materials goes from 0.46 mg/g for a commercial 4A zeolite (4AZ) [39] and higher as 29.4 mg/g for a modified organoclay - C3H1[38]. The qe values for the synthetized α- and γ-Alu spheres are in the interval of 0.1765 to 18.9865 mg/g; these novel adsorbent materials have interesting sorption capacities compared to those existing already. Moreover, the γ-Alu spheres have important regeneration properties that allow to use them in consequent sorption cycles.Table 4
Comparison of R40 removal by different adsorbent materials.
Adsorbent materialSorption capacityqe (mg/g)ReferenceZirconia fibers0.8950Ávila-Martínez et al. [34]Activated charcoal (walnut shells)9.9865Herrera-García, Aguirre-Ramírez, and Torres-Pérez [35]Basic anion-exchanger (Lewatit MonoPlus M-600)3.4120Wawrzkiewicz and Hubicki [36, 37]Amberlite IRA-9009.9950Wawrzkiewicz and Hubicki [36, 37]Amberlite IRA-91010.095Wawrzkiewicz and Hubicki [36, 37]Modified organoclay - C3H129.400Ullah et al. [38]Modified organoclay - C2CB125.300Ullah et al. [38]Modified organoclay - C2S120.300Ullah et al. [38]Commercial 4A zeolite (4AZ)0.4627Erdoğan [39]α-Alu spheres (C0 =10 mg/L)0.1765This workγ-Alu spheres (C0 =10 mg/L)8.1979This workγ-Alu spheres (C0 = 50 mg/L)13.5980This workγ-Alu spheres (C0 =100 mg/L)18.9865This workγ-Alu spheres (pH =3.0)9.4961This workγ-Alu spheres (pH =5.0)8.4515This workγ-Alu spheres (pH =10.0)5.3752This work


## 4. Conclusions

The synthesis of adsorbent material by chemical precipitation method was successful for the obtention ofα- and γ-Alu spheres as adsorbent materials. From characterization techniques, it was found that the spheres presented a slight irregular surface and a structure with high mechanical strength. The alumina polymorph is very important because of its hardness and stability. Only the synthesized γ-Alu spheres presented an important percentage of R40 removal at C0 =10, 50, and 100 mg/L, reaching 81, 14, and 19% removal, respectively, and showed the best fitting to the Elovich equation, advising that the γ-Alu spheres remove R40 azo dye by chemisorption. Acidic pH values were appropriate for the removal of R40.γ-Alu spheres have a slightly higher sorption capacity for R40 removal in distilled media than in aqueous media with ionic strength. The R40 sorption mechanism can be achieved by cation exchange capacity and electrostatic forces. The results denote the importance to find alternative and sustainable synthesized materials for the advanced treatment of wastewater by adsorption process for the removal of organic dyes (R40) as an emerging pollutant.



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*Source: 3786561-2022-05-04.xml*