Adsorption in Jar-Test system: a study of the physico-chemical interactions of the chitosan biopolymer with the textile dye DO 2GL

ABSTRACT

The incorrect disposal of contaminated effluents from textile industries is a major contribution to their environmental impact. We aimed to use the chitosan biopolymer from industrial sources as a potential adsorbent agent. The experiments were performed in Jar-Test simulating an industrial scale treatment. Both pH and mass variations were analyzed. Our UV spectra results showed that all datasets fitted to the Langmuir model, indicating the formation of monolayers. Kinetics studies confirmed that adsorption follows a pseudo-second order model, in addition to a chemisorption pattern during adsorption. Kinetics studies also demonstrated intraparticle diffusion, which confirmed a strong adsorbate/adsorbent interaction with the dye. The Jar-Test proved to be an efficient system to simulate treatment of effluents on an industrial scale, thus ranking chitosan powder as a good adsorbent and eligible to future large-scale applications.

Keywords
chitosan; intraparticle diffusions; chemisorption; isotherms; kinetics

1. INTRODUCTION

Water pollution is a major worldwide problems that has been constantly aggravated by increasing anthropogenic activities. The residues of industrial processes and wastewater from domestic sewage are among the pollution sources that are often incorporated into rivers, especially when adequate and effective treatment methods are lacking. In this context, the textile industry is responsible for generating bulk effluents containing mainly synthetic dyes and toxic organic compounds, such as benzene, toluene, ethylbenzene, naphthalene, anthracene and xylene [¹]. Circa 10% of all dyestuffs produced or processed by the textile industries are directly disposed as effluents [²], as the textile industry consumes approximately 10,000 tons per year of synthetic dyes [³]. Once in the environment, dyes and their derivatives may present high toxicity levels with mutagenic and carcinogenic effects on exposed organisms [⁴]. Moreover, the high organic load released into effluents changes local ecosystems due to the increase in water turbidity. The modified environment hinders the penetration of the solar radiation, which can further disturb the photosynthetic activity, decrease gas solubility and reduce the oxygen uptake rates [⁵]. Furthermore, the disposal of textile wastewaters lead to bioaccumulation and ecotoxicological processes [⁶].

There are currently several classes of synthetic dyes available in the textile market: acid, azoic, reactive, direct, dispersed, metallized, bleach and sulfonic. Approximately 60% of the dyes are azoic, being one of the groups of higher environmental impacts. This class often present more than one complex aromatic chain. In general, the functional chromophore groups are a result of the interaction between azo functions (–N=N–) and aromatic species in the dye molecules [⁷]. However, the reductive cleavage of azo bonds in azoic dyes generate toxic and carcinogenic amines [³].

The removal of these dyes from effluents has been studied by physicochemical methods such as ozonization [⁸], photo-electrochemical degradation [⁹], subcritical flow [¹⁰]; and biological methods, such as microbiological degradation [¹¹]. However, the physicochemical methods application costs are much higher, whereas biological methods require a large treatment area and longer effluent retention time. Therefore, dye waste management ends up being unfeasible by the lack of optimal applicability on an industrial scale.

Adsorption is presented as an alternative towards the treatment of textile industry waste. Its viability is due to the availably of many low-cost adsorbent materials. Most adsorbent substrates are biodegradable, easily obtainable in nature and, more importantly, obtained from pre-existing waste. Adsorption is considered a very efficient technique compared to other treatment methods, due to its simplicity of design and operation, associated with its efficacy and minimum to none toxic output [¹²]. Different types of materials have been proposed as good adsorbents, however, activated carbon remains as the most used adsorptive material in processes due to their low cost, suitable physical properties, and regional availability on an industrial scale [¹³].

A highly adsorbent biopolymer be obtained in fishing activities with shrimp and other arthropods as a replacement to activated carbon. Chitosan is a biopolymer obtained by deacetylation of chitin from the exoskeleton of arthropods or fungal cell walls [¹⁵], often synthesized using the fishing residues such as crustacean shells. The world chitosan market share includes 60% nutraceuticals and food use, 17% flocculants, 5% cosmetics, 5% agriculture, 6.5% in the textile and paper industries and 6.5% in the pharmaceutical and medical industries [¹⁶]. Chitosan choice as an adsorbent material is aided by the fact that the fishing market waste itself has become an environmental problem, in which tons of shell residues are disposed daily. It may also represent an abundant source of biopolymers, as the annual global production of shrimp, crayfish, lobsters, and crabs is estimated at 1,44 million tons of dried biomass [¹⁴].

Chitosan is already reported in the literature as a good adsorbent material for dyes [¹⁵], but, to the best of our knowledge, no tests have yet been performed proposing commercial chitosan biopolymer as adsorbent material in textile industry. Thus, the aim of this work was to analyze the potential of industrial chitosan powder as a dye adsorbent. To evaluate the applicability of the material on an larger scale, the Jar-Test system was used to simulate the application in a textile effluent treatment in a real contamination scenario. The Jar-Test is a prospective small-scale simulator of an industrial effluent treatment. We selected the azo reactive dye Direct Orange 2GL as our contaminant to represent the synthetic dyes found in textile dyeing processes. Mathematical models of kinetics and isotherm were applied in the results to specify the main mechanisms of adsorbate/adsorbent interaction that occurred throughout the sorption process.

2. MATERIALS AND METHODS

2.1 Chitosan

The chitosan powder used in this study was obtained from Purifarma Chemistry & Pharmaceutical Brazil-SP, being derived only from shrimp shells with physicochemical characteristics of 90% degree of deacetylation corresponding to 5.60 x 10^-3 mole of amino group per grams of biopolymer, particle size of 80 mesh and density of 0.38 g mL^-1. Its chemical structure is shown in Figure 1.

Figure 1
Chemical structure of chitosan.

2.2 Direct Orange 2GL

Direct Orange 2GL (DO 2GL) dye, Chemical Abstract Service (CAS) number: 1325-54-8 and molar mass of 299 moles was obtained from the company Dimacolor Industry Group Co. It is a stable dye on pH variation with its maximum absorbance at 415 λ. The dye has reactive sulfonic groups, which confers solubility in aqueous medium, besides an azo functional group in its structure (Figure 2).

Figure 2
Chemical structure of the reactive dye Direct Orange 2GL.

2.3 Adsorption test using Jar-Test

Adsorption assays with DO 2GL dye solution were performed through various mass concentrations of the chitosan powder: 0.2; 0.4; 0.6; 0.8 and 1.0 g. The Jar-Test equipment (Policontrol model FlocControl II), was adjusted for constant blade rotation at 60 rpm, with a maximum contact time of 3 hours, at room temperature of 25 ± 2 ºC (Figure 3).

Figure 3
Chemical structure of the reactive dye Direct Orange 2GL.

A dye solution with a concentration of 8.36 x 10^-2 mmol L^-1 (50 mg L^-1) was added to 500 mL in each vat where adsorption took place. The adsorption studies with mass variations were also conducted at different pH values (5.50 and 6.50), as this is the regulated range for the disposal of any treated effluent according to Brazilian environmental laws [¹⁷].

Aliquots of each sample were taken after the final test period, and thereafter they were centrifuged at 3000 rpm for 10 minutes, thus separating the adsorbent from the solution. The aqueous phase was then measured in a UV-Vis spectrophotometer (Thermo Scientific model BioMate 3S) from 300 to 800 nm, using quartz cuvettes with a 10 mm optical path. The dye concentration adsorbed per mass of adsorbent was calculated using Equation 1.

$$qe=\frac{\left(Co-Ce\right).V}{W}$$ (1)

where W is mass (g), V is the volume of the solution (L), Co is the initial concentration and Ce is the concentration of the dye in the solution (mg L^-1) after adsorptions, and qe is the adsorption capacity at equilibrium per mass of chitosan powder (mg g^-1).

The data obtained in this study were analyzed using the mathematical models of the isotherms of Langmuir (1918) [¹⁸] and Freundlich (1906) [¹⁹], which can determine the singular characteristics of the adsorption, besides being able to determine whether the sorption process is physical or chemical.

The Langmuir model (Equation 2) fits to adsorption datasets whose adsorbent is homogeneous. According to Langmuir isotherms, a specific chemical site of the adsorbent surface will interact with the adsorbate having a finite number of binding sites, thus forming a monolayer [²⁰].

$$qe=\frac{qm.l.Ce}{1+Ce. l}$$ (2)

where qm is the maximum amount of dye adsorbed per mass of adsorbent at equilibrium (mg g^-1) and l is the Langmuir constant related to the affinity of the adsorbent and adsorbate (L g^-1).

When linearizing the Langmuir model, we obtained the Equation 3. Through the linear regression of the graph of Ce/qe vs. Ce we found the values of the constants qm and l.

$$\frac{Ce}{qe}=\frac{1}{l.qm}+\frac{Ce}{qm}$$ (3)

The Langmuir separation factor (Rl) was also calculated, using the Equation 4 proposed by McKay et al. (1982) [²¹].

$$Rl=\frac{1}{1+l. Co}$$ (4)

This model helped to determine if the adsorption was favorable or unfavorable. Depending on the Rl results, we considered Rl = 0 the adsorption to be irreversible, Rl = 1 linear, Rl > 1 unfavorable, and 0 < Rl < 1 favorable [²¹].

The Freundlich model (Equation 5), on the other hand, proposes that the surface of the adsorbent is heterogeneous. In other words, the surface has different sites of interaction with the adsorbate, and the occupation of these sites follows a descending order according to their interaction and energy. The decreasing and exponential occupation of the interaction sites lead to the formation of a multiple layer adsorption on the adsorbent [²²].

$$qe=Kf.C{e}^{1/nf}$$ (5)

where Kf is the Freundlich constant related with solid adsorption capacity (L g^-1), and nf is the adsorption constant.

The linearized Freundlich model (Equation 6) and the linear regression plot of lnqe vs. lnCe allowed th calculation of Kf and nf values.

$$\mathrm{In} qe=\mathrm{In} Kf+\frac{1}{nf}. \mathrm{In} Ce$$ (6)

2.4 Kinetics studies in Jar-Test

The kinetic studies were performed separately, using Jar-Test equipment. We added 500 mL of dye solution with an initial concentration of 50 mg L^-1, at pH 6.50 and 5.50, to each vat. Powdered chitosan (1.0 g) was added simultaneously to each vat. The equipment was adjusted for constant blade movement at 60 rpm, at room temperature (25 ± 2 ºC). The dye concentration was monitored at a sequential interval of 10 minutes at a maximum observation time of 90 minutes. The solution aliquots were all centrifuged at 3000 rpm for 10 minutes before each analysis in UV-Vis spectrophotometer.

For a better interpretation of the kinetic data, we used the mathematical models of pseudo-first order (Equation 7) proposed by Lagergren (1898) [²³], and pseudo-second order (Equation 8) proposed by Ho and McKay (1998) [²⁴].

$$\mathrm{In} \left(qe-qt\right)=\mathrm{In} qe\mathit{-}kl.\mathit{ }t$$ (7)

$$\frac{t}{qt}=\frac{1}{ks. q{e}^2}+\frac{t}{qe}$$ (8)

where t is time in minutes, qt is the amount of dye adsorbed at time t (mg g^-1), kl is the adsorption rate constant of the pseudo-first order model (min^-1), and ks is the pseudo-second order rate constant (g mg^-1 min^-1).

Adsorbate is often not restricted to adsorbing only to surface layers, as its penetration into the adsorbent molecule may also occur. In order to evaluate this occurrence, we applied the mathematical model of the intraparticle diffusion proposed by Weber and Morris (1963) [²⁵] (Equation 9).

$$qt=Kdi. t^{0,5}+C$$ (9)

in which Kdi is the constant of intraparticle diffusion rate (g mg^-1 (min^0.5)^-1) and C is a constant related to the thickness of the diffusion layers (mg g^-1).

Still, intraparticle diffusion can occur simultaneously with surface adsorption and may not be the driving factor of the reaction [²²]. We applied the Equation 10 to identify simultaneous intraparticle diffusion, according to the Boyd et al. (1947) model [²⁶].

$$Bt=-0.4977-\mathrm{In} \left(1-\frac{qt}{qe}\right)$$ (10)

In this case, if the Bt vs. t plot passes through the graph coordinate plane origin, intraparticle diffusion is the dominant process in sorption [²⁷].

The second Boyd model (Equation 11) was also used to calculate the effective diffusion coefficient.

$$Di=\frac{r^2. Bb}{{\pi }^2}$$ (11)

in which Di is the effective diffusion coefficient (cm² s^-1) of DO 2GL dye in the chitosan powder, r is the average radius of the chitosan powder particle (0.00885 cm), and Bb is calculated from the graph of Bt as a function of t.

All the kinetic and adsorptive studies conducted in Jar-Tests were done in triplicates. Proper standard deviation (SD) analysis was applied to our data output and to the mathematical models fits using Equation 12.

$$SD=\sqrt{\frac{1}{N-1}\underset{i=1}{\overset{N}{\Sigma }}{\left(\frac{Qie-Qic}{Qie}\right)}^2}$$ (12)

in which Qie and Qic (mg g^-1) are experimental and calculated mass of dye adsorbed by adsorbents materials, and N is the number of measurements made.

The graphs and chemical structures used in this work were designed using proprietary software Origin 6.10 and ACD/ChemSketch.

RESULTS AND DISCUSSION

Our adsorption study with Jar-Test showed that chitosan is a very dense powder. It decanted at the bottom of the vats after 3 hours. Although dense, the blades of the Jar-Test system had no difficulty in keeping constant stirring, thus proving that chitosan powder would be a viable material to upscaled industrial applications.

The sorption rate of the dye compared to the mass of the adsorbent material (Figure 4) showed that adsorption was more efficient at pH 5.50.

Figure 4
Amount of dye adsorbed per mass of chitosan powder.

Chitosan had an adsorption capacity of 24.615 mg g^-1 at pH 6.50. In comparison, Safa [²⁸] reported in a previous studies using rice husk that Direct Orange dye adsorption was 36.14 mg g^-1 at pH 3.0. The maximum adsorption achieved by both materials were similar. However, the use of chitosan in our study is more advantageous because the applied pH is much closer to neutral. Thus, no further adjustments to the pH of the treatment tank output is required before releasing the treated industrial wastewater. Changes in pH would increase the use of chemicals and the overall treatment costs.

The isotherms (Table 1) confirmed that for both pH the adsorption fitted best to the Langmuir model (Figure 5), indicating that a specific site of the adsorbent is interacting with the DO 2GL dye, forming a monolayer.

Figure 5
Adsorption isotherm models: I – Langmuir model in the solution at pH 6.50; II – Freundlich model in the solution at pH 6.50; III – Langmuir model in the solution at pH 5.50 and IV – Freundlich model in the solution at pH 5.50.

Table 1
Adsorption isotherm parameters

Chitosan powder	Langmuir isotherm				Freundlich isotherm
pH	qm (L g-1)	l (L g-1)	Rl	R	SD	Kf (L g-1)	nf	R	SD
5.50	111.482	1.292	0.0152	0.924	1.010	52.527	7.157	0.861	2.835
6.50	111.607	0.310	0.0606	0.983	1.450	27.085	1.830	0.981	3.797

No major variation was found when comparing qm in both pH values, similarly to the values of qe (Figure 5). The maximum sorption rates are likely equivalent in an ideal equilibrium. However, the values of l indicated that the chitosan powder had a much higher adsorbate/adsorbent affinity when in more acidic medium. This result is corroborated when the values of Rl obtained are compared, as it almost approaches 0 in pH 5.50, thus indicating that adsorption is close to irreversible. This result indicates chemical interactions that involve a shared and/or exchanged electron flow between the chitosan powder and the DO 2GL dye molecule. Even so, adsorption was also favorable when pH 6.50, despite not showing high sorption affinity.

Although not following the Freundlich model (Figure 5), the Kf values indicated that solid/liquid adsorption capacity were higher at pH 5.50, confirming a high interaction between adsorbent with adsorbate. In this case, even if adsorption does not fit the Freundlich model, both isotherm and values of nf are greater than 1. The surface interaction promoted by chitosan is homogeneous, reinforcing the best fit to the Langmuir isotherm for both pH values.

The kinetic studies showed that both materials reach the equilibrium of sorption almost at the same time (Figure 6), even in solutions with different pH. The adsorption reaches the equilibrium 10 minutes earlier at pH 5.50 than at pH 6.50, which is not a relevant difference in industrial scale treatments.

Figure 6
Kinetics studies plot: I – Experimental adsorption kinetics at pH 6.50 and II – Experimental adsorption kinetics at pH 5.50.

Both pH and adsorption patterns correlate to the kinetic models of pseudo-second order (Table 2) according to the coefficients obtained in the kinetic studies. This result is corroborated by qe_(exp) and qe_(cal) that were much closer to the pseudo-second order model. An adsorption that follows the pseudo-second order model means that adsorption occurs by a chemical process [²⁹], such as the data obtained in our isotherm studies.

Table 2
Kinetics studies parameters

Chitosan powder		Pseudo-first order				Pseudo-second order
pH	qe(exp) (mg g-1)	kl (min-1)	qe(cal) (mg g-1)	R	SD	ks (g mg-1 min-1)	qe(cal) (mg g-1)	R	SD
5.50	24.955	0.0353	2.940	0.877	0.565	0.0218	25.335	0.995	0.389
6.50	24.615	0.0564	4.207	0.819	1.044	0.0254	25.259	0.996	0.374

Besides, the results of intraparticle diffusion (Figure 7) showed that the diffusion of dye molecules into the chitosan powder occurred at both pH values. We also observed a second linear region, that is possibly related to diffusion occurring at a second layer, also known as macropore layer [²⁴]. The equilibrium is probably achieved in this region, without further penetration of the dye into a third and inner layer.

Figure 7
Intraparticle diffusion: I – Dye solution at pH 6.50 (■ macropore layer; ■ mesopore layer) and II – Dye solution at pH 5.50 (▲ macropore layer; ▲ mesopore layer).

The intraparticle diffusion constants on Table 3 show that the Kdi values of the macropore layer were lower than the first boundary layer. In other words, the diffusion primarily occurred in the second layer (mesopore) by filling all the possible sites in that region before filling the first layer. The constant of diffusion layer thickness was higher in the macropore layer, which indicates its major resistance to dye penetration compared to the first boundary layer. This corroborates our aforementioned results of intraparticle diffusion.

Table 3
Constants values of intraparticle diffusion

pH	First boundary layer				Macropore layer
	Kdi (mg g-1 (min0.5)-1)	C (mg g-1)	R	SD	Kdi (mg g-1 (min0.5)-1)	C (mg g-1)	R	SD
6.5	0.573	19.882	0.997	1.192	0.032	24.317	0.948	2.178
5.5	0.668	19.648	0.983	0.603	0.147	23.508	0.941	0.983

The Boyd plot (Bt vs. t) further confirmed that diffusion is not controlling the sorption process at both pH values since the regression function did not pass through the origin of the coordinate plane (Figure 8). We propose that the main sorption site is on the surface, as the actual adsorption controller.

Figure 8
Boyd function: I – Dye solution at pH 6.50 and II – Dye solution at pH 5.50.

The Bb values for pH 6.50 and 5.50 were 0.0737 and 0.0521 respectively, whereby it was possible to determine the Di values for both pH, being 5.851 x 10^-7 cm² s^-1 at pH 6.50, and 4.137 x 10^-7 cm² s^-1 at pH 5.50. The values of Di on the order of 10^-7 cm² s^-1 confirms that the adsorption took place on both the external and internal surfaces, being much more intense on the surface.

Based on the isotherms and kinetics, we observed that a specific sorption site promoted chemical interaction. Therefore, it was necessary to understand the main sites of possible chemisorption to propose a mechanism that could explain the interaction between the dye and the biopolymer. The DO 2GL dye has sulfonic functional groups (SO₃^-) and the chitosan amino functional groups (NH₂), which gives it ionic interactions capabilities. As a result, any pH changes in the solution is supposed to interfere with the charges and electrostatic interactions between the adsorbate and the adsorbent. The protonated chitosan (NH₃⁺) allows a more efficient interaction with charged dye molecules (Figure 9), being one of the main reasons for the adsorption to be more efficient in a more acidic pH, as observed in this work.

Figure 9
Possible chemical interaction between the chitosan powder and DO 2GL dye.

Thus, a solution set to an acid medium induces the electrostatic interactions that result in the protonation of the amino groups. Therefore, in the presence of acidified aqueous solutions, the functional groups of the chitosan molecule are positively charged and promote strong interactions between the free valences of the amino groups (NH₃⁺) and the anions of the sulfonic radical groups (SO₃^-) belonging to the dye. This type of interaction with chitosan can be extended to other sulfonic dyes.

Based on the maximum effluent disposal regulations in Brazil [¹⁷], along with the tolerable spectrophotometric pattern of dye traces in water for disposal in the environment [³⁰], we can stipulate the monthly costs of treating effluents using the chitosan powder as an adsorbent in a treatment system similar to Jar-Test. Not taking into account electricity, maintenance and equipment costs, and assuming that the adsorbent price is from a Brazilian supplier with fixed capital without inflation effects, it would be necessary to spend approximately US$ 7,075.27 per month to treat a 100 m³ effluent with a concentration of 0.05 g L^-1 of textile dye. A specific amount of adsorbent material may be required to remove the dye according to their respective adsorbate/adsorbent interactions when we consider that the dye to be treated would be DO 2GL. The average price of chitosan powder is US$ 10.61 per kg, while the activated carbon quoted in this work has an average cost of US$ 9.65 per kg, however, due to its high interaction with reactive sulfonic dyes, chitosan becomes more cost-effective. Therefore, chitosan powder can be considered a very feasible adsorbent agent of dyes in industrial scale effluent treatment.

4. CONCLUSIONS

Chitosan powder was a good adsorbent material according to our experimental approach. We propose that it is reasonable replacement for activated carbon, which is currently used in most adsorptive treatments. Besides, chitosan is a low-cost material that is also widely available, at a similar cost range.

Adsorption is more efficient at acidic pH, due to the interactions of the ionic bonds between the amine groups (NH₃⁺) of the adsorbent with the sulfonic groups (SO₃^-) of the adsorbate. Isotherm analysis confirmed that the adsorption occurs due to chemisorption. The kinetic studies showed that chitosan powder reached sorption equilibrium in 60 minutes, which is an ideal time frame for industrial scale treatment.

More studies with industrial chitosan powder are encouraged to evaluate its adsorption capabilities towards other different types of textile dyes or even in dye mixtures. Nevertheless, the use of chitosan powder as adsorbent is recommended for a large-scale treatment of effluents textiles.

ACKNOWLEDGEMENTS

Support from the Brazilian fostering agencie: Coordenação de Aperfeiçoamento de Pessoal Nível Superior (CAPES) – Brazil.

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Publication Dates

• Publication in this collection
  11 Dec 2020
• Date of issue
  2020

History

• Received
  26 Oct 2018
• Accepted
  23 Mar 2020