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Open Access Original Research

Adsorption of Rhodamine-B (RhB) and Regeneration of MCM-41 Mesoporous Silica

Thiago Rodrigo Barbosa Barros , Thianne Silva Batista Barbosa , Tellys Lins Almeida Barbosa , Meiry Gláucia Freire Rodrigues †,*

  1. Federal University of Campina Grande, Academic Unit of Chemical Engineering, Av. Aprígio Veloso, 882-Bodocongó, Zip code 58109-970, Campina Grande-PB, Brazil

  2. † These authors contributed equally to this work.

Correspondence: Meiry Gláucia Freire Rodrigues

Academic Editor: Prem Kumar Seelam

Special Issue: Advances in Porous Catalytic Materials

Received: November 01, 2022 | Accepted: February 20, 2023 | Published: March 01, 2023

Catalysis Research 2023, Volume 3, Issue 1, doi:10.21926/cr.2301010

Recommended citation: Barbosa Barros TR, Silva Batista Barbosa T, Lins Almeida Barbosa T, Freire Rodrigues MG. Adsorption of Rhodamine-B (RhB) and Regeneration of MCM-41 Mesoporous Silica. Catalysis Research 2023; 3(1): 010; doi:10.21926/cr.2301010.

© 2023 by the authors. This is an open access article distributed under the conditions of the Creative Commons by Attribution License, which permits unrestricted use, distribution, and reproduction in any medium or format, provided the original work is correctly cited.


Rhodamine (RhB) adsorption was carried out on MCM-41 and MCM-41 calcined. The effect of parameters such as pH was investigated. The reusability potential of MCM-41 was also established and the mechanism of RhB adsorption was discussed. MCM-41 was synthesized and calcined, with all samples characterized by X-Ray Diffractometry, X-ray Fluorescence by Dispersive Energy, Infrared Spectroscopy, Scanning Electron Microscopy, and Thermogravimetric analysis. The results of the characterization techniques performed confirmed the formation of the MCM-41 structure. During the adsorption of the RhB dye, high removal percentages and rapid kinetics occur in an acid medium. The adsorption kinetics was evaluated by two models: pseudo-first order and pseudo-second order. The pseudo-first-order kinetic model represented the interaction mechanism well during RhB adsorption by MCM-41. However, the pseudo-second-order model better represented the interaction mechanism during RhB adsorption by MCM-41 calcined. The regeneration study found that the MCM-41 and MCM-41 calcined were maintained at 80 and 90% of their original condition after three successive regeneration cycles. The overall results show that the process could be used as a strategy for environmentally sustainable wastewater treatment.

Graphical abstract

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MCM-41; RhB dye; adsorption; kinetics; regeneration

1. Introduction

Pollution from dye effluents has become a serious environmental problem during the last decade, due to the increasing use of dyes in various applications [1]. The worldwide textile industry is the main source of these effluents [2,3]. Dyes are organic compounds used to color different substrates and are raw materials used in many manufacturing processes, such as: textiles, paper, plastic, leather, food, and pharmaceuticals [4,5].

RhB is a basic, reddish dye in the Xanthene class, and is highly soluble in water [6]. Xanthene is an organic compound based on a class of dyes; such as fluorescein, eosins, and rhodamines derived from this structure. Xanthene dyes are among the oldest and most used synthetic dyes. Xanthene dyes tend to be fluorescent, giving bright colors, from pinkish yellows to bluish reds [7]. These dyes are similar in color and exist in wastewater effluents; therefore, their removal and determination are important [8]. RhB is widely used as a dye in textiles, food [1,9], medicine (for animals), and in coloring biological samples [8]. It is also a fluorescent marker for water [6]. The improper disposal of this dye prevents sunlight from penetrating water, leading to serious environmental problems and being toxic and carcinogenic to living beings [10]. Therefore, its removal from aquatic wastewater is essential [11].

The adsorption method has been used in several ways and with different adsorbents to remove the RhB dye from an aqueous solution [1,12,13]. Adsorption is one of the superior processes due to its cheapness, ease of operation, high efficiency, and rapidity. The adsorption technique removes organic dyes from aqueous solution by employing efficient materials such as SBA-15, MOFs, MCM-41, etc. [14]. The MCM-41 molecular sieve is a crystalline solid with a highly-defined hexagonal structure, a surface area greater than 700 m²/g, excellent thermal stability, and a structure that can be modified in several ways [15,16]. These materials have many applications as adsorbents [17,18,19,20], especially about the adsorption of dyes [21,22,23,24,25].

The use of the adsorption process as a dye removal technology stands out especially due to the wide variety of adsorbent materials that can be applied. The effective separation of several contaminants by the adsorption process generally requires the porous structure of the adsorbents, which contributes to the improvement of their surface area and adsorption capacity [26].

This study is part of a line of research developed at the New Materials Development Laboratory (LABNOV) at the UFCG. This line of research covered a series of studies on the synthesis and characterization of molecular sieves, which could be used in various processes [27,28,29,30,31,32,33,34,35,36,37,38,39,40]. This work was carried out in two stages, the first stage presented the obtained results on the characterization of both MCM-41 and MCM-41 calcined. The second part investigated the effect of parameters such as pH. The adsorption kinetics for RhB using MCM-41 and MCM-41 calcined were also studied. Furthermore, a regeneration study was carried out to investigate the reusability of the adsorbent. To our knowledge, there is no study about the adsorption of the RhB on MCM41.

2. Materials and Methods

2.1 Materials

Cetyltrimethylammonium Bromide (CTAB, 98%), ammonium hydroxide (NH4OH, 29%) and tetraethylorthosilicate (TEOS, 98%) were purchased from Sigma-Aldrich (MERCK). The main properties of dye RhB are summarized in Table 1.

Table 1 Overview of physicochemical properties of the RhB.

2.2 Synthesis of Silica MCM-41

MCM-41 was prepared using the hydrothermal crystallization method. The proposed method was based on changes made to the procedure reported by the authors [41]. The method was as follows: (A) CTAB was dissolved in deionized water at 50°C under agitation for 30 min. The solution was cooled to approximately 25°C; (B) NH4OH was added into the solution with stirring for 15 min; (C) Then, the TEOS was introduced; (D) After 2 h, the reaction mixture was submitted to hydrothermal treatment at 30°C for 24 h; (E) The resulting product was filtered, washed with deionized water and then the material was dried at 60°C for 24 h; (F) Material was calcined in a muffle furnace from room temperature up to 550°C, using a 5°C/min heating ramp remaining at the final temperature (550°C) for 7 h.

2.3 Characterization

X-ray diffraction patterns were carried out on a Shimadzu XRD 6000 using Cu Kα radiation at 40 kV/30 mA, with a goniometer velocity of 2°/min and step of 0.02° in the 2θ range from 3.0° to 10.0°.

To obtain the infrared, IR VERTEX 70 equipment from BRUKER was used. The samples in the form of tablets were dried in an oven in advance and placed in the sample holder. The IR spectra were obtained at wavelengths in the 400-4000 cm-1 range with a resolution of 4 cm-1. To identify and quantify the chemical composition of the synthesized samples, an S2 Ranger Bruker dispersive energy X-ray spectrophotometer was used. A VEGA TESCAN scanning electron microscope was used to perform microscopy on the samples. The powder samples were covered with a thin layer of gold by a metallizer and fixed to support with carbon adhesive tape. Thermogravimetric analysis was performed in a Shimadzu DTG-60H Thermal Analyzer in a nitrogen atmosphere with a 50 mL/min gas flow. The sample was heated from room temperature up to 1000°C, at a heating rate of 10°C/min.

2.4 Batch Adsorption Experiments

2.4.1 Influence of pH

The influence of the pH of the RhB dye solution on the adsorption capacity of each sample was tested with a concentration of 15 mg/L of dye, adjusted to different pH levels. For each sample, 30 mL of dye was used with the mass of each sample being 0.3 g. Samples were prepared with a pH ranging from 1 to 14 in intervals of one unit, totaling 14 samples. The samples were acidified and made alkaline using 3 M hydrochloric acid and 1 M sodium hydroxide solutions. The pH of the dye solution is a parameter of significant influence in determining the adsorption capacity [42].

2.4.2 Adsorption Kinetics

RhB adsorption kinetics were acquired in batch experiments. These experiments were performed at 25°C using a solution of 15 mg/L of RhB, which was put in contact with 0.3 g of samples. Adsorption experiments were conducted in conical flasks at controlled pH (1.0) and under a shaking table at 200 rpm. Aliquots from the solution were collected at time intervals (20 min) between 0 and 180 min. Afterward, the solutions were centrifuged and analyzed for residual dye concentration with a UV-vis spectrophotometer.

The concentration of RhB dye was determined using a UV-VIS 1600 spectrometer with a wavelength of 554 nm [43]. The removal percentage (R%) and the quantity of adsorbed RhB (q) were obtained using Equations 1 and 2, respectively.

\[ R\%=\left(\dfrac{C_i-C}{C_i}\right)*100 \tag{1} \]

\[ q=\dfrac{V}{m}\left(C_i-C\right) \tag{2} \]

where: R% = removal percentage; q = quantity of adsorbed RhB (mg of RhB/g of adsorbent); V = volume of dye solution (L); m = mass of adsorbent (g); Ci = initial concentration of dye solution (mg/L); and C = final concentration remaining after the batch process (mg/L).

2.5 Evaluation of Regenerated MCM-41

The capacity of an adsorbent material to be regenerated and reused is key to its ability to be used in wastewater treatment. To check the ability to reuse MCM-41, repeated runs were performed at the optimum conditions found and adapted by other authors [44]. Each cycle consisted of a 1.0 g sample with 100 mL of dye at pH 1, stirred for 30 min. Regeneration was performed by washing each sample with 100 mL of deionized water and 50 mL of methyl alcohol (MeOH). After washing, the samples were filtered and dried at 60°C for 24 h.

3. Results

3.1 Characterization

Figure 1 shows the diffractogram of MCM-41 obtained from X-ray diffraction. Figure 2 presents the FTIR spectra of MCM-41 and MCM-41 calcined in the range 4000-500 cm-1 evaluated at room temperature.

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Figure 1 X-ray diffraction patterns of the MCM41.

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Figure 2 FTIR spectra of the MCM-41 and MCM-41 calcined.

The XRD of the synthesized MCM-41 molecular sieve exhibits an intense peak at 2θ = 2.2° corresponding to the plane (1 0 0) and two to three small peaks between 3.5° and 6.0° due to the planes (1 1 0), (2 0 0) and (2 1 0) that show the presence of ordered mesoporous hexagonal MCM-41 [41,45,46,47,48].

In Figure 2 (MCM-41 and MCM-41 calcined), the spectra show bands in 940 and 950 cm-1 corresponding to angular vibrations of the Si-OH bond of the silanol groups existing in the MCM-41 structure. The spectra of the synthesized and calcined samples show bands in the 500-4000 cm-1 region characteristic of the fundamental vibrations of the functional groups present in the structures of the molecular sieves MCM-41 [46]. It is possible to observe the presence of a main band at 1050 and 1066 cm-1 composed of another secondary band, less developed at 1025 and 1190 cm-1, which corresponds to asymmetric stretches of the Si-O-Si connection [47,48]. The spectra also show vibrational bands at 1465 and 2920 cm-1 attributed to the stretches between CH of the CH2 and CH3 groups, which correspond to the presence of the surfactant, cetyltrimethylammonium bromide (CTAB) which is occluded in the pores of MCM-41 [49]. MCM-41 calcined shows a broadband without definition corresponding to the template's removal.

Chemical composition percentage concentrations determined by Dispersive Energy X-Ray Fluorescence (ED-XRF) for MCM-41 showed a high silicon dioxide (SiO2) content, 99.85% and some impurities.

Three mass loss events can be observed from the thermogravimetric curve of the synthesized MCM-41 shown in Figure 3. The first event below 150°C related to the desorption of physisorbed water in the pores of the material that corresponds to 4% of mass loss, the second in the range of 150-320°C attributed to the decomposition of the driving ions (CTAB) where the greater mass loss of 31% and the third between 400-550°C due to the residual removal of CTAB, resulting from the secondary condensation process of the silanol groups corresponding to 13% of the total loss [48,49,50,51,52].

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Figure 3 TG/DTG curves of the MCM-41.

The Morphology of MCM-41 (Figure 4) is similar to those of authors [53] who synthesized the MCM-41 using NH4OH at different temperatures. The particles have spongy, irregular, and non-uniform spherical clusters.

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Figure 4 Micrograph of the MCM-41.

Figure 5 (a) shows the adsorption and desorption curves of N2 for MCM-41 calcined, and (b) shows the pore size distribution obtained through the BJH method.

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Figure 5 N2 adsorption and desorption of the MCM-41 calcined isotherm and pore size distributions.

According to the IUPAC classification, the samples exhibited type IV isotherms and different hysteresis loops [54]. According to IUPAC isotherms of this type are typical of mesoporous materials with multilayer adsorption cycles. Nitrogen adsorption occurs on the material surface at a relative pressure (P/P0) below 0.2. Then the monolayer is formed, and multi-layers develop over it. From (P/P0) 0.4 there is an increase in the capacity of adsorbed nitrogen, called hysteresis, associated with capillary nitrogen condensation in the mesopores [48]. This behavior is observed for both materials. In the final part of the isotherm, the pore is saturated after capillary condensation. A small amount of N2 was adsorbed on the outer walls, resulting in a maximum volume of adsorbed gas of approximately 450 cm³/g for MCM-41.

The behavior of the MCM-41 isotherm exhibited H4-type hysteresis that corresponds to porous materials made up of narrow, slit-shaped pores. The pore diameter distribution showed a peak at around 2.70 nm attributed to the micropore region and a peak at 36 nm attributed to the mesoporous region of the MCM-41.

Table 2 shows the values obtained for the network parameter a0 (nm) which can be calculated in a simplified way using the formula a0 = 2d100.(31/2)-1, where d100 corresponds to the interplanar distance in the (1 0 0) diffraction plane. The surface area, SBET (m²/g), was obtained using the BET method and the average pore diameter, Dp (nm), was obtained using the BJH method. Vp (cm³/g) corresponds to the pore volume of the samples and Wt corresponds to the nanometer thickness of the structural wall, calculated as the difference between the network parameter a0 and the pore diameter, Dp [55,56].

Table 2 Synthesis parameters and characterization of the MCM-41 calcined.

According to Table 2, the BET surface area of MCM-41 calcined is 726 m²/g, a value relative as shown in the literature [57,58]. The wall thickness of the MCM-41 calcined is by the authors exhibiting a value between 1 and 1.5 nm [16]. This thin wall takes the material to low chemical and hydrothermal stability.

3.2 Batch Adsorption Experiments

3.2.1 Influence of pH

The pH of the aqueous medium is an important factor that can modify RhB adsorption. The chemical characteristics of both adsorbent and adsorbate can vary depending on the pH. The pH of the solution affects the degree of ionization and speciation of various dyes, which subsequently changes the reaction kinetics and equilibrium characteristics of the adsorption process [20,59]. Experiments were performed to study the influence of the pH on the adsorption capacity of materials, varying the pH from 1 to 13. The experimental results for the RhB adsorption on both samples (MCM-41 and MCM-41 calcined) are shown in Figure 6.

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Figure 6 Effect of pH on the adsorption of RhB by MCM-41 and MCM-41 calcined.

For the MCM-41 (Figure 6), the internal pore region is obstructed by the template, meaning that the adsorption of the dye can be effective only on the structure's external surface. MCM-41 showed a low adsorption removal, mainly at pH 7, 9, and 11. It was noted that the most favorable adsorption of RhB dye occurs at acidic pH levels, according to the literature [23,59,60].

Results for the MCM-41 calcined (Figure 6) indicate that the effect of pH was not so prominent. As can be seen, the MCM-41 calcined adsorbs and removes high percentages of RhB dye at almost all pH levels, from acidic to basic. This can be attributed to the fact that the adsorption occurred both on the surface of the MCM-41 calcined and in the internal pore region, due to the greater number of active sites on the MCM-41 calcined.

Figure 6 clearly shows that the adsorption of RhB onto the MCM-41 is quite different from the adsorption of the dye onto the MCM-41 calcined.

3.2.2 Dye Adsorption

It must be noted that the surface of the adsorbent changes its polarization according to the pH value of the solution and the isoelectric point (IEP) of the solid [61]. The pH chosen for the tests was lower than the isoelectric point pHiep of MCM-41, which was 1. When the pH of the solution is lower than pHiep, a material surface is positively charged, and the sorption of anionic species to a positively charged sorbent occurs through the Coulomb force of attraction. The opposite occurs at higher pH values [25], when decreasing dye adsorption levels may be attributed to the competition of OH- with the dye ions for the adsorption sites on the material. The increased number of hydroxyl groups decreases the number of positively charged sites and reduces the attraction between the dye and the adsorbent surface [24]. As described in the literature [20], the complex structure of some dyes causes multiple possible interactions among dye molecules and adsorbents.

3.2.3 Adsorption Kinetics

Adsorption kinetics of the RhB dye was determined from batch experiments with constant agitation. Kinetic studies for the adsorption of RhB dye were performed at a 15 mg/L concentration. The pH was adjusted to 1 and 0.3 g of MCM-41 was used in each batch. Figure 7 and Figure 8 show the kinetic curves obtained from the RhB dye adsorption tests for samples (MCM-41 and MCM-41 calcined), that fit the pseudo-first-order and pseudo-second-order models.

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Figure 7 Adsorption kinetics of RhB dye onto MCM-41 and non-linear fits: pseudo-first order and pseudo-second order.

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Figure 8 Adsorption kinetics of RhB dye onto MCM-41 calcined and non-linear fits: pseudo-first order and pseudo-second order.

Rapid adsorption was observed in the first 20 minutes of contact time between the RhB dye solution and the material, after which the adsorption equilibrium was established, with few variations in the adsorption capacity until the final contact time of 180 minutes (Figure 7). MCM-41 showed a maximum adsorption capacity of 1.50 (mg/g) in 20 min. The pseudo-first-order was the kinetic adsorption model that best fit the MCM-41 behavior, presenting a good coefficient of determination values. In contrast, the second-order model showed a lower determination coefficient (R2) due to the low interaction between the chemical species adsorbed on the surface of the adsorbent and the amount adsorbed at steady state [62,63].

According to the data presented in Figure 8, excellent adsorption was observed for the calcined samples. It is possible to state that, in the first 15 minutes of contact time between the RhB dye solution and the material, the adsorption equilibrium was established, as few variations were seen in the adsorption capacity until the final contact time of 180 minutes. MCM-41 calcined had a maximum adsorption capacity of 1.59 (mg/g) in 80 minutes of contact. kinetic model that best fit, and obtained the best value for the coefficient of determination for the MCM-41 calcined, was the pseudo-second-order model, due to the greater adsorbate-adsorbent interaction characteristic of the chemisorption that occurs in this model [64].

Table 3 shows the kinetic parameters of the pseudo-first order and pseudo-second order models obtained from the non-linear model generated by the Origin 8.0® software.

Table 3 Kinetic model parameters for RhB dye adsorption onto MCM-41 and MCM-41 calcined.

3.2.4 Evaluation of Regenerated MCM-41 and MCM-41 Calcined

Reusing the adsorbents (MCM-41 and MCM-41 calcined) was investigated under optimized conditions. Figure 9 shows the data on the removal percentage in each adsorption cycle.

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Figure 9 Recyclability tests adsorbed with RhB.

Results in Figure 9, for the reuse of each sample in three consecutive cycles of adsorption of the RhB dye at a pH of 1, showed that the adsorption capacity decreased considerably from the first to the second cycle and from the second to the third cycle, for both samples. MCM-41 calcined had a higher adsorption capacity than the as-synthesized MCM-41, for the three reuse cycles. The molecular structure of RhB (dimension ~ 1.20 nm) [65] compared to the pore diameter (3.5 nm) of the MCM-41 calcined, provides a favorable condition for the entry of this dye molecule into the pores of the adsorbent. Therefore, washing MCM-41 calcined with methanol does not compromise the structure of the mesoporous silica, making this material suitable for reuse up to 3 times after regeneration.

The data obtained in this study on the adsorption capacity of the materials from the adsorption of the RhB dye are shown in Table 4 along with other data from the literature.

Table 4 Various types of adsorbents for the removal of RhB and their maximum adsorption capacity.

Reusability experiments were carried out to investigate the performance of the MCM-41. At the end of the adsorption process, the saturated sorbent was separated by filtration, and then regenerated using methanol, followed by drying at 60°C for 24 h. The regenerated adsorbent was reused in a subsequent run under the same conditions.

Based on the adsorption RhB, MCM-41 and MCM-41 calcined were efficient, removing up to 80% of the RhB. The results of adsorption capacity for RhB were 1.35 and 1.52 mg/g for MCM-41 and MCM-41 calcined, respectively.

Lower results were found in the literature [66,67]. However, it was noted that the MCM-41 and MCM-41 calcined (present study) removed more than the zeolites. Two factors can explain this fact: i) different structures; and ii) different experimental conditions. Compared with the results found in the literature, the MCM-41 and MCM-41 calcined results produced in this study were satisfactory [66,67].

3.3 Possible Adsorption Mechanisms

The adsorption of RhB dye onto the MCM-41 and MCM-41 calcined was studied to understand the influence of surfactant CTAB on the adsorption behavior. It was observed that several factors significantly influence the adsorption of dyes on mesoporous structures, such as the dye structure itself, the textural and chemical properties of the adsorbent surface, and the specific interaction between the adsorbent surface and the adsorbate [68]. The structure of the MCM-41 consists of SiO2 tetrahedra ending in siloxane (Si–O–Si) or silanol (Si–OH) groups on the surface [18].

Therefore, it is understood that the adsorption of RhB dye on MCM-41 calcined was higher than that obtained on MCM-41 due to the CTAB chain affecting the adsorption behavior. It was shown that mesoporous materials containing surfactant could limit and restrict the diffusion of molecules within the phase of the materials [69]. Another way to interpret the above results may be with the difference existing in the interactions between basic dyes and surface hydroxyl groups of MCM-41. RhB possesses polar atoms (N), so the interaction between RhB and MCM-41 may be stronger. This may induce a collapse in the pore structure of MCM-41, and then create a sharp decrease in the adsorption capacity. On the other hand, the free silanol groups, after calcination, found on the surface of mesoporous silica, can interact with the nitrogen and hydrogen groups of the dye through hydrogen bonding [70].

After drying, the regenerated samples from the third RhB adsorption cycle were analyzed through FTIR. Figures 10 (a) and (b) show the FTIR spectra in the range 4000-500 cm-1 evaluated at room temperature.

Figure 10 (a) shows the well-known vibration mode of the -CH2 and -CH3 groups of the CTAB surfactant of MCM-41 (2935 cm-1). In Figure 10 (a) and (b), the spectra in the range between 3409-1635 cm-1, corresponding to the axial deformation of the C-H bond and the aromatic bonds of RhB [68]. In other bands, at 1190-1205 and 940-950 cm-1, the RhB functional groups are located in the same regions as those that characterize the groups of MCM-41, indicating a possible interaction of the dye with the silanol groups [71,72].

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Figure 10 FTIR spectra of the MCM-41 (a) calcined (b) after adsorption of RhB.

4. Conclusions

According to the XRD, ED-XRF, FTIR, and nitrogen adsorption isotherm results, MCM-41 and MCM-41 calcined were effectively synthesized and produced a mesoporous material. This study showed that the MCM-41 and MCM-41 calcined are effective adsorbents for removing RhB dye from an aqueous solution. The results indicate that the template played an important role in adsorption due to its strong hydrophobic properties. The effect of parameters such as pH was studied, finding that acidic conditions favored the RhB dye removal process. MCM-41 showed a greater adsorption capacity at acidic pH levels in all tests performed. Pseudo-first-order and pseudo-second-order kinetic models were fitted to the experimental data. For the MCM-41 system (RhB), The pseudo-first-order model was a bit better for the MCM-41 system (RhB), but for the MCM-41 calcined system (RhB), the pseudo-second-order model fit better. The regeneration of MCM-41 and MCM-41 calcined performed well with RhB after three successive processes. Therefore, MCM-41 and MCM-41 calcined can be used as effective adsorbents for RhB, and also demonstrated favorable regeneration capacity, which is relevant when considering their potential use for industrial sector applications, as well as being an important strategy for environmental sustainability.


The authors gratefully acknowledge to the CNPq (Conselho Nacional de Desenvolvimento Científico e Tecnológico) and CAPES (Coordenação de Aperfeiçoamento de Pessoal de Nível Superior) for their financial support.

Author Contributions

Thiago Rodrigo Barbosa Barros: Investigation, Formal analysis, Thianne Silva Batista Barbosa: Investigation, Formal analysis, Writing – Original Draft; Tellys Lins Almeida Barbosa: conceptualization, Formal analysis, Methodology; Meiry Gláucia Freire Rodrigues: Conceptualization, Formal analysis, Funding acquisition, Writing – Review & Editing.


Coordenação de Aperfeiçoamento de Pessoal de Nível Superior (CAPES).

Competing Interests

The authors have declared that no competing interests exist.


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