pH-Triggered Interfacial Interaction of Kaolinite / Chitosan Nanocomposites with Anionic Azo Dye

Advanced engineering of naturally occurring materials opens new doors in nanoscience and nanotechnology for the separation and/or removal of environmental hazards. Here, a series of nanocomposites containing kaolinite and chitosan varying in the range of 20 to 80% (w/w) kaolinite were used for the adsorptive removal of a reactive textile dye, Remazol Red, from an aqueous solution. Batch experiments were carried out to investigate the effects of pH, contact time, and initial dye concentration on the adsorption capacity. Nanocomposites containing 80% kaolinite (w/w) and 20% chitosan (w/w), i.e., NK80C20, showed an equilibrium adsorption capacity of 371.8 mg/g at pH 2.5, which was 5.2 times higher than that of commercial activated charcoal. Moreover, NK80C20 was regenerated instantly up to 99.9% at pH 10. Therefore, NK80C20 can be effectively utilized as a potential adsorbent for the separation of Remazol Red and homologous azo dyes from industrial effluents. We expect that the findings from this study will play a vital role in environmental research leading to advanced applications in water purification.


Introduction
Nanocomposites (NCPs) offer several advantages and better performances over traditional composites since the interface and morphology of NCPs are totally different from those of traditional composite materials [1].A large fraction of the polymer matrix is converted into an interface of different properties due to the smaller particle size and larger surface area of the dispersed phase, and also due to smaller inter-particle distances [2].As a result, there is a substantial improvement in properties such as strength, flame retardancy, modulus, decrease in gas permeability, thermal stability, etc. [3].These improved properties help NCPs find potential applications in various fields such as adsorbents, automotive industries, exterior step assists, tennis rackets, tennis balls, soccer balls, hockey sticks, tires, electrostatic dissipation, beverage containers, films, latex gloves, auto fuel systems, etc. [4].Due to their environment-friendly and cost-effective nature, NCPs from waste and naturally occurring materials are gaining rapid interest for the remediation of hazardous pollutants [5][6][7].
Azo dyes, extensively used in textile industries, pose a great threat to both aquatic organisms and animals as they are toxic, carcinogenic, and mutagenic [8].Due to their higher solubility in water, high molecular weight, and stability under the effects of light, heat, and oxidizing agents, it is very difficult to either degrade or remove these dyes from effluents with conventional wastewater treatment methods [9].Adsorptive removal is considered to be a highly efficient technique for the separation of these stubborn dyes from wastewater [10].In this regard, biopolymer chitosan is an excellent choice because of its higher adsorption capacity for dyes.The enhanced adsorption capacity of chitosan has been attributed to the presence of hydroxyl (-OH) and amino (-NH 2 ) functional groups, which serve as reaction and coordination sites [11].Since chitosan displays polycationic nature in acidic media due to the protonation of amino functional groups, it can strongly adsorb anionic azo dyes by the electrostatic force of attraction [12].Remazol Red (RR) is an anionic reactive azo dye that contains a sulfonic acid group.Therefore, for the removal of RR from textile effluents, chitosan can be applied as a potential adsorbent, but it does have some limitations.Chitosan becomes soft in aqueous media due to its hydrophilicity and has a tendency to form a gel; it swells and floats in water.Furthermore, it has a low specific gravity and smaller surface area, weak mechanical properties, higher solubility in acidic media, etc. [13][14][15].The formation of composites with chitosan has been considered an efficient pathway for overcoming these drawbacks [10].
To date, a few kaolinite/chitosan composite adsorbents have been reported in the literature [5][6][7].Kanchana et al. reported a binary composite of nanochitosan/kaolin clay for the adsorption of Pb (II) [5].Zhu et al. developed a ternary composite of chitosan/kaolin/nanosized γ-Fe 2 O 3 for the adsorption of methyl orange [6].Chen et al. prepared chitosan/coated kaolinite beads for the adsorption of Cu (II) [7].In our previous study, we demonstrated a simple dropping technique for the fabrication of NCPs from kaolinite and chitosan [41].However, to the best of our knowledge, there is no literature report on kaolinite/chitosan NCP adsorbents for the removal of RR.In this study, we report the adsorption performance of kaolinite/chitosan NCPs at various operating conditions of pH, contact time, and dye concentration.In addition, we clearly demonstrate the pH-controlled reversible interaction of RR with the adsorbent surface.Moreover, we investigated the probable mechanism for the variation of the adsorption performance of the NCPs with increasing kaolinite content.Because it offers several technological advantages in terms of facile fabrication, adsorption capacity, reusability, cost, and environment-friendly nature, the fabricated NCP is expected to find outstanding applications in the separation of azo dyes and similar hazardous pollutants from effluents of textile, food, leather, pharmaceutical, and other industries.

Materials
Kaolinite and waste prawn shells were collected from a local source in Bangladesh.Purified sodium hydroxide pellets and 35% hydrochloric acid (w/w) were supplied by Active Fine Chemicals Limited (Dhaka, Bangladesh).Acetic acid and ethanol were purchased from Merck KGaA (64271 Darmstadt, Germany).The selected azo dye (RR) was collected from a local textile industry in Bangladesh.All of the chemicals were used without further purification.

Preparation of NCPs
The NCPs were successfully prepared and characterized as reported in our recently published article [41].The process we followed is briefly described here.Chitosan flakes were dissolved in 100 mL acetic acid (1 M) and kaolinite (acid activated) was then added to the chitosan solution.The resulting mixture was agitated by a sonicator for 30 min.The mixture was then sprayed dropwise into a neutralization solution of 15% NaOH (w/v) and 95% ethanol (v/v) in a volume ratio of 4:1.The formed composite beads were washed several times and dried in an oven at 60 • C for 10 h.The beads after drying were ground to reduce their size for the enhancement of adsorption capacity.Five different NCPs were prepared with different ratios of chitosan and kaolinite as shown in Table 1.Thermal stability of the NCPs was examined by a thermogravimetric analyzer (TGA-50, Shimadzu Corporation, Kyoto, Japan) with an alumina cell under a nitrogen atmosphere at the flow rate of 10 mL/min (for both balance and sample) and at the heating rate of 10 • C/min.The samples were heated from 25 • C to 1000 • C. From TGA data, the loading of chitosan in mmol per mol of kaolinite was calculated.

Adsorption of RR
Twenty (20) milliliters of RR solution with different concentrations (from 60 to 100 ppm) were added to Erlenmeyer flasks with air-tight stoppers.Five (5) milligrams of each type of NCP was used throughout the adsorption study.For adjusting the pH of the solutions, 0.1 M NaOH and 0.1 M HCl were employed.The flasks were shaken at room temperature (25 • C) by a shaker at 150 rpm until the equilibrium point was reached.An ultraviolet (UV)-Vis spectrophotometer (UV-2100PC HumanLab Instrument Co., Suwon-city, Korea) was used to determine the concentration of RR in the solution by measuring the absorbance at 518 nm (Figure S1).The equilibrium adsorption capacity (q e ) was calculated according to the following formula: where C o is the initial concentration of RR (ppm), C e is the equilibrium concentration of RR (ppm), m is the weight of the adsorbent used for the adsorption studies (g), and V is the volume of RR solution taken (L).

Desorption of RR
The regeneration of an adsorbent is very important for its practical application.After adsorption, the dye-loaded adsorbents were subjected to alkaline media of pH 8.0, 9.0, and 10.0 in order to investigate their regeneration efficiency.

Effect of Operating Conditions
Various parameters, e.g., surface charge of an adsorbent, degree of ionization, structural changes of dye molecules, dissociation of functional groups on its active sites, etc., are strongly affected by the pH of the solution [42].We closely monitored the effects of pH, contact time, and initial RR concentration on the adsorption capacity of NCPs.

Effect of pH
In our previous study, we demonstrated the influence of pH on the adsorption of RR by chitosan (Figure 1a) [43].Chitosan showed an adsorption capacity of 313.4 mg/g at pH 3.0.In acidic media, there was a strong electrostatic force of attraction between the anionic RR molecules and chitosan due to the protonation of the amino functional groups on the surface of chitosan.The highest adsorption capacity of chitosan at pH 3.0 might be attributed to the maximum protonation of the amino functional groups at pH 3.0.The decrease in adsorption capacity at a pH below 3 might occur due to the dissolution of chitosan.When the pH of the solution was increased above 3, the adsorption capacity also decreased because of the lower degree of protonation of amino functional groups.Chitosan exhibited a very low adsorption capacity at a pH above 7 because the amino functional groups of chitosan no longer remained protonated in alkaline media.

Effect of Contact Time
The fundamental basis of adsorption kinetics is the effect of contact time on the adsorption capacity [46].
Figures 2a,b depict the effect of contact time on the adsorption capacity of chitosan and NK80C20 for RR.
In the case of chitosan, as illustrated in Figure 2a, the rate of adsorption was very rapid up to the first 20 min and then the rate was very slow.The equilibrium was reached after 30 min.In the case of NK80C20, as shown in Figure 2b, the rate of adsorption increased rapidly during the first 10 min, then All of the NCPs showed a higher adsorption capacity than chitosan and kaolinite as presented in Figure 1b.However, the adsorption behavior was similar to chitosan.There was only one exception which was that the maximum adsorption occurred at pH 2.5 for the NCPs, not at pH 3.0.Ngah et al. also reported the maximum adsorption capacity of a crosslinked chitosan-coated bentonite bead for anionic tartrazine at pH 2.5 [44].The similarity between the two studies at a particular pH strongly supports that 2.5 could be the most suitable pH for the adsorption of anionic dye molecules by chitosan/clay composites.The pH stability of chitosan was improved due to the attachment of chitosan on the surface of kaolinite in the formation of the composite, which resisted the dissolution of chitosan up to pH 2.5.The adsorption behavior of NK 80 C 20 below pH 2.5 was totally different from others, as explained later.
In the case of kaolinite, as depicted in Figure 1c, there was a progressive increase in the adsorption capacity as the pH of solution decreased below 6.The maximum adsorption capacity of 9 mg/g was observed at pH 1.0.In acidic media, protons were available which were responsible for the electrostatic attraction between the negatively charged RR molecules and the kaolinite surface.With the gradual decrease in the pH of the solution, there was a progressive increase in the availability of protons resulting in the enhanced adsorption of RR molecules.With an increase in the pH of the solution, there was a relative decrease in the positive charge on the surface and an increase in the negative charge.Adsorption of anionic dyes was not favored on the negatively charged kaolinite surface due to electrostatic repulsion.Also, in alkaline media, there was competition between the hydroxyl ions and the dye anions for the adsorbent [45].
The formation of NCPs not only eliminated the crystallinity of chitosan but also caused an increase in specific gravity.Chitosan is a semi-crystalline polymer and, as a result, the penetration of dye molecules through the crystalline region is very difficult.Prior to composite formation, chitosan was dissolved in acetic acid, which caused the loss of crystallinity.Moreover, NCPs possessed higher surface area than the flaky chitosan due to the smaller particle size.All of these factors contributed to the higher adsorption capacity of NCPs as compared to chitosan.
The adsorption performance of the NCPs was compared with the commercial activated charcoal.Activated charcoal showed an adsorption capacity of only 71 mg/g for RR at pH 1.0, as illustrated in Figure 1d.This capacity was very low compared to chitosan and NK 80 C 20 .The comparison strongly supports the notion that kaolinite/chitosan NCPs have huge potential to be industrially used as adsorbents for anionic azo dyes.

Effect of Contact Time
The fundamental basis of adsorption kinetics is the effect of contact time on the adsorption capacity [46].Figure 2a,b depict the effect of contact time on the adsorption capacity of chitosan and NK 80 C 20 for RR.In the case of chitosan, as illustrated in Figure 2a, the rate of adsorption was very rapid up to the first 20 min and then the rate was very slow.The equilibrium was reached after 30 min.In the case of NK 80 C 20 , as shown in Figure 2b, the rate of adsorption increased rapidly during the first 10 min, then increased slowly and after 15 min reached equilibrium.The higher initial rate of adsorption is attributed to the higher number of vacant active sites on the surface of the adsorbent.Dye molecules gradually cover these active sites, but near the equilibrium it is difficult for the dye molecules to occupy the remaining active sites, probably due to the slow pore diffusion [47].Contact times of 30 min and 15 min were selected for chitosan and NK 80 C 20 , respectively, for further study.

Mechanistic View of Adsorption Performance
As shown in Figure 3a, the NCPs showed a progressive increase in adsorption capacity with the increase in kaolinite content.Among the NCPs, the lowest adsorption capacity of 325 mg/g found was for NK20C80 and the highest adsorption capacity of 371.8 mg/g found was for NK80C20.Here, we propose a mechanism for the progressive increase in adsorption capacity with the gradual increase in kaolinite content, which is illustrated in Figure 3b.
Due to low specific gravity, soft and flexible chitosan swelled and floated in water.The polymer could not move uniformly throughout the dye solution and its effective contact with the dye molecules was low.Therefore, it showed low adsorption capacity.With the incorporation of kaolinite, the macromolecule electrostatically attached itself to the heavier kaolinite nanoparticles.The specific gravity of the macromolecules was increased due to their self-assembly on the negatively charged kaolinite surface.The movement of NCPs was more uniform throughout the dye solution as compared to the movement of chitosan alone.In these NCP systems, the surface-attached chitosan found more scope for effective contact with the dye molecules.The number of surface-attached chitosan increased gradually with increasing the kaolinite content.In this study, the porous structure of the chitosan-immobilized NCPs played a vital role in adsorption.In the case of NK20C80, chitosan might form densely packed multilayers on the kaolinite surface.This hard shell showed an adsorption behavior similar to that of chitosan.In the case of NK80C20, kaolinite might be partially covered, i.e., chitosan might form less densely packed thin layers on the kaolinite surface.This soft shell showed the highest adsorption behavior.The charge distribution on the surface at this condition might create a suitable environment for the NCP, facilitating the interaction tendency towards dye uniformly.Because it exhibited the most effective surface attachment, NK80C20 showed the highest

Effect of Initial RR Concentration
The adsorption capacity of both chitosan and NK 80 C 20 was influenced by the initial RR concentration.As shown in Figure 2c,d, it was observed that the adsorption capacity of both chitosan and NK 80 C 20 increased with increasing the initial concentration of RR.During the adsorption process, dye molecules are diffused from the bulk of the solution to the adsorbent surface.The driving force for this mass transfer process is the concentration gradient between the bulk of the solution and the adsorbent surface [48].With an increase in the initial RR concentration, the concentration gradient increased, resulting in the enhanced diffusion of RR molecules.As a result, the rate of adsorption of RR on both chitosan and NK 80 C 20 increased with increasing the initial concentration of RR.

Mechanistic View of Adsorption Performance
As shown in Figure 3a, the NCPs showed a progressive increase in adsorption capacity with the increase in kaolinite content.Among the NCPs, the lowest adsorption capacity of 325 mg/g found was for NK 20 C 80 and the highest adsorption capacity of 371.8 mg/g found was for NK 80 C 20 .
Here, we propose a mechanism for the progressive increase in adsorption capacity with the gradual increase in kaolinite content, which is illustrated in Figure 3b.adsorption capacity at pH 2.5 and the highest resistance to dissolution below pH 2.5 as compared to the other NCPs.

Thermogravimetric Analysis (TGA)
Some useful information was derived from the TGA thermograms as illustrated in Figure 3c.From the thermograms, it was observed that chitosan decomposed at 600 °C, whereas no decomposition of kaolinite occurred at this temperature.The content of thermally stable kaolinite controlled the decomposition pattern of the NCPs.Based on the weight loss of the NCPs at 600 °C, we calculated the loading of chitosan in mmol per mol of kaolinite using their respective molecular weights.As demonstrated in Figure 3d, the highest amount of chitosan in mmol was loaded per mol of kaolinite in the case of NK20C80, whereas the least amount of chitosan loading was calculated for NK80C20.

Surface Charge Calculation
The surface charge of an adsorbent plays the determining role in the adsorption process.Therefore, it is very important to quantify the charge distribution on the surface of an adsorbent.Since NK80C20 showed the highest adsorption capacity, we calculated the surface charge per gram of NK80C20.The value for NK80C20 was calculated to be 109 C. The protonation of amino functional groups at pH 2.5 was responsible for the presence of a positive charge on the surface of the NK80C20.This quantity of positive charge on the surface must be balanced by an equivalent quantity of negative charge on the adsorbed dye molecules.The adsorption capacity for NK80C20 was 371.8 mg/g, i.e., 371.8 mg dye must carry an equivalent quantity of negative charge to balance the 109 C positive charge.The estimated charge on 371.8 mg of RR was 147 C. RR is an anionic azo dye and the highest Due to low specific gravity, soft and flexible chitosan swelled and floated in water.The polymer could not move uniformly throughout the dye solution and its effective contact with the dye molecules was low.Therefore, it showed low adsorption capacity.With the incorporation of kaolinite, the macromolecule electrostatically attached itself to the heavier kaolinite nanoparticles.The specific gravity of the macromolecules was increased due to their self-assembly on the negatively charged kaolinite surface.The movement of NCPs was more uniform throughout the dye solution as compared to the movement of chitosan alone.In these NCP systems, the surface-attached chitosan found more scope for effective contact with the dye molecules.The number of surface-attached chitosan increased gradually with increasing the kaolinite content.In this study, the porous structure of the chitosan-immobilized NCPs played a vital role in adsorption.In the case of NK 20 C 80 , chitosan might form densely packed multilayers on the kaolinite surface.This hard shell showed an adsorption behavior similar to that of chitosan.In the case of NK 80 C 20 , kaolinite might be partially covered, i.e., chitosan might form less densely packed thin layers on the kaolinite surface.This soft shell showed the highest adsorption behavior.The charge distribution on the surface at this condition might create a suitable environment for the NCP, facilitating the interaction tendency towards dye uniformly.Because it exhibited the most effective surface attachment, NK 80 C 20 showed the highest adsorption capacity at pH 2.5 and the highest resistance to dissolution below pH 2.5 as compared to the other NCPs.

Thermogravimetric Analysis (TGA)
Some useful information was derived from the TGA thermograms as illustrated in Figure 3c.From the thermograms, it was observed that chitosan decomposed at 600 • C, whereas no decomposition of kaolinite occurred at this temperature.The content of thermally stable kaolinite controlled the decomposition pattern of the NCPs.Based on the weight loss of the NCPs at 600 • C, we calculated the loading of chitosan in mmol per mol of kaolinite using their respective molecular weights.As demonstrated in Figure 3d, the highest amount of chitosan in mmol was loaded per mol of kaolinite in the case of NK 20 C 80 , whereas the least amount of chitosan loading was calculated for NK 80 C 20 .

Surface Charge Calculation
The surface charge of an adsorbent plays the determining role in the adsorption process.Therefore, it is very important to quantify the charge distribution on the surface of an adsorbent.Since NK 80 C 20 showed the highest adsorption capacity, we calculated the surface charge per gram of NK 80 C 20 .The value for NK 80 C 20 was calculated to be 109 C. The protonation of amino functional groups at pH 2.5 was responsible for the presence of a positive charge on the surface of the NK 80 C 20 .This quantity of positive charge on the surface must be balanced by an equivalent quantity of negative charge on the adsorbed dye molecules.The adsorption capacity for NK 80 C 20 was 371.8 mg/g, i.e., 371.8 mg dye must carry an equivalent quantity of negative charge to balance the 109 C positive charge.The estimated charge on 371.8 mg of RR was 147 C. RR is an anionic azo dye and the highest adsorption capacity was found at pH 2.5.Therefore, at this strong acidic condition the additional 38 C negative charge on RR might be balanced by the protonated azo functional groups [49].

Demonstration of a Reversible Interaction
Since acidic media were preferable for the adsorption of RR by both chitosan and NK 80 C 20 , we employed alkaline media for their regeneration.Alkaline pH played a vital role in the regeneration of these two adsorbents because there was an immediate desorption of dye molecules from both chitosan and NK 80 C 20 (Figure 4a).The pH-controlled reversible interaction between NCPs and RR in the aqueous phase is schematically illustrated in Figure 4b.
adsorption capacity was found at pH 2.5.Therefore, at this strong acidic condition the additional 38 C negative charge on RR might be balanced by the protonated azo functional groups [49].

Demonstration of a Reversible Interaction
Since acidic media were preferable for the adsorption of RR by both chitosan and NK80C20, we employed alkaline media for their regeneration.Alkaline pH played a vital role in the regeneration of these two adsorbents because there was an immediate desorption of dye molecules from both chitosan and NK80C20 (Figure 4a).The pH-controlled reversible interaction between NCPs and RR in the aqueous phase is schematically illustrated in Figure 4b.With the gradual increase in pH of the media, there was a progressive increase in the desorption of RR from both chitosan and NK80C20.As depicted in Figure 4b, the dye molecules were trapped on the NCP surface at pH 2.5 but at pH 10, the captured dye molecules were liberated from the surface.Therefore, the adsorbent was regenerated and was ready to be used again.From this schematic representation, it can be concluded that the interfacial interaction of NK80C20 with RR was reversible, and was completely controlled by the pH of the medium.This interfacial interaction was further confirmed by recording the FTIR spectrum of dye-loaded NK80C20 (Figure S2).Chitosan and NK80C20 showed the highest desorption ratios of 0.967 and 0.999, respectively, at pH 10.0.The dye molecules might be trapped inside the spiral polymeric chains of chitosan.However, in the case of NK80C20, the spiral chains could be more disentangled.This factor might contribute to the higher desorption of RR from NK80C20 than from chitosan.With the gradual increase in pH of the media, there was a progressive increase in the desorption of RR from both chitosan and NK 80 C 20 .As depicted in Figure 4b, the dye molecules were trapped on the NCP surface at pH 2.5 but at pH 10, the captured dye molecules were liberated from the surface.Therefore, the adsorbent was regenerated and was ready to be used again.From this schematic representation, it can be concluded that the interfacial interaction of NK 80 C 20 with RR was reversible, and was completely controlled by the pH of the medium.This interfacial interaction was further confirmed by recording the FTIR spectrum of dye-loaded NK 80 C 20 (Figure S2).Chitosan and NK 80 C 20 showed the highest desorption ratios of 0.967 and 0.999, respectively, at pH 10.0.The dye molecules might be trapped inside the spiral polymeric chains of chitosan.However, in the case of NK 80 C 20 , the spiral chains could be more disentangled.This factor might contribute to the higher desorption of RR from NK 80 C 20 than from chitosan.

Comparison of Adsorption Performance
According to previously reported literature, treated sawdust showed an adsorption capacity of only 8.0 mg/g for RR at pH 2.0 after a very long time of 12 h [50].In our previous study, chitosan showed an adsorption capacity of 313.4 mg/g for RR at pH 3.0 after 30 min [43].However, in this present study, we found that the fabrication of kaolinite/chitosan NCPs enhanced the adsorption capacity of chitosan for RR.Moreover, there was a successive increase in the adsorption capacity of the NCPs with the gradual increase in kaolinite content, due to the progressive formation of self-assembly.Out of the five NCPs, NK 80 C 20 contained only 20% (w/w) chitosan and 80% (w/w) kaolinite.Kaolinite is a naturally occurring and cheap raw material, whereas chitosan needs to be prepared from waste prawn shells through some expensive chemical steps.Therefore, the NCP prepared with the least amount of chitosan and the highest amount of kaolinite should be the cheapest one.Out of the five NCPs utilized in this study, NK 80 C 20 was the most cost-effective composite.NK 80 C 20 also showed the highest adsorption capacity of 371.8 mg/g within only 15 min and had 99.9% instant regeneration.We also employed the widely used adsorbent, i.e., activated charcoal for the adsorption of RR.However, it showed an adsorption capacity of only 71 mg/g for RR at pH 1.0.Therefore, from the discussion above, it can be said that NK 80 C 20 is a much more effective adsorbent for RR as compared to other adsorbents reported in literature.
The potential differences between chitosan and NK 80 C 20 , as found in this study, are summarized in Table 2 and Figure S3 clearly distinguishes their adsorption performance.

Conclusions
Hazardous pollutants have severe negative environmental impacts.In order to defend nature against such detrimental impacts, nanoscience and nanotechnology can play a pivotal role.In this study, we report kaolinite/chitosan NCPs as a potential remedy for water pollution by RR.We closely observed that the fabrication of NCPs improved the pH stability and adsorption capacity of chitosan.All of the NCPs exhibited a higher adsorption capacity than kaolinite, chitosan, and activated charcoal.The NCPs showed a successive increase in the adsorption capacity with a gradual increase in kaolinite content, due to the progressive formation of self-assembly.The pH-controlled interaction of NCPs with RR has been clearly demonstrated in this report.Self-assembly of the majority of the polymeric chains on the kaolinite's surface contributed to the maximum capture of dye molecules on NK 80 C 20 .The higher adsorption capacity, quick and higher regeneration efficiency, and cost-effective nature of NK 80 C 20 indicate that for the removal of RR and similar pollutants from industrial effluents, NK 80 C 20 can be effectively utilized as a potential adsorbent.

Figure 2 .
Figure 2. Effect of contact time on the adsorption capacity of (a) chitosan and (b) NK80C20; effect of the initial concentration of Remazol Red (RR) on the adsorption capacity of (c) chitosan and (d) NK80C20.

Figure 2 .
Figure 2. Effect of contact time on the adsorption capacity of (a) chitosan and (b) NK 80 C 20 ; effect of the initial concentration of Remazol Red (RR) on the adsorption capacity of (c) chitosan and (d) NK 80 C 20 .

Figure 4 .
Figure 4. (a) Bar diagram of desorption ratio vs. pH and (b) schematic illustration for the adsorptiondesorption mechanism of RR.

Figure 4 .
Figure 4. (a) Bar diagram of desorption ratio vs. pH and (b) schematic illustration for the adsorption-desorption mechanism of RR.
: Visible spectra for aqueous solutions of RR; Figure S2: FTIR spectrum of (a) RR, (b) NK 80 C 20 , and (c) RR-loaded NK 80 C 20 ; Figure S3: Image of (a) RR solution before adsorption, (b) RR solution after adsorption by chitosan, and (c) RR solution after adsorption by NK 80 C 20 .

Table 1 .
Nanocomposites (NCPs) prepared from different proportions of chitosan and kaolinite.

Table 2 .
Comparison of adsorption performance between chitosan and NK 80 C 20 .