Sage Journals: Discover world-class research

Abstract

This study deals with the application of Iranian zeolite as a low cost adsorbent for the removal of the Direct blue 71 (DB 71) from colored solution. Important parameters including equilibrium and contact time, initial dye concentration, effect of pH, and zeolite dosage were evaluated. Maximum dye removal was obtained at about 99.8% for 25 mg/L at 120 min of equilibrium. Higher adsorption efficiency of direct dye was obtained at higher dose and acidic pH. To analyze the adsorption equilibrium and kinetic, Langmuir, Freundlich, and Temkin isotherms as well as four kinetic models encompassing pseudo first-order, pseudo second-order, intraparticle diffusion, and Elovich were evaluated. The Langmuir isotherm (R²= 0.995) and pseudo second-order models, gave the best fit to equilibrium experimental data. In Langmuir analysis, the maximum adsorption capacity (q_m) by 13.66 mg/g was determined. Finally, the characteristics of zeolite including both natural and modified, such as compositions, surface morphology by X-ray diffraction technique (XRD), X-ray fluorescence (XRF), and scanning electron microscopy (SEM) were obtained. According to XRF analysis, it was demonstrated that Al₂O₃ and SiO₂ are the most part of natural and modified zeolite. Furthermore, the clinoptilolite was determined as the significant crystalloid phase by XRD pattern.

Keywords

Direct dye adsorption equilibrium and kinetics Direct blue 71 N-cetyl pyridinium bromide (CPB)zeolite

Introduction

Nowadays, the textile industry plays a key role in the economy of countries around the world (Amin, 2009). Among the textile operation, dyeing is a fundamental process which produces large volume of colored wastewater that can affect environmental ecosystems, especially aqueous ambient. Direct blue 71 is an azo dye group with three azo bonds. The potential toxicity and carcinogenicity of azo dyes has been reported (El-Bahy et al., 2009). In addition to aesthetically displeasing, some dyes (as azo group dye) are toxic to some microorganisms and may cause direct destruction or inhibition of their catalytic activities (Armagan et al., 2004). According to reports, Direct dyes constitute about 17% of all dyes employed for dyeing textiles and about 30% of dyes used for dyeing cellulose fiber (Sax, 1981). Therefore, this products need to be treated before delivery. The conventional methods for the decolorization of dyes from aqueous solutions are oxidation, precipitation, ion exchange, bio-sorption, electrochemical treatment, and adsorption (Bulut et al., 2007; Shirmardi et al., 2013). The use of each method depends on the economical, technical requirements, and wastewater characteristics. As a result of the adsorption advantage, (i) it is considered to be relatively superior to other techniques due to its low cost, (ii) simplicity of design, (iii) viability, and (iv) ability to treat dyes in more concentrated form (Arami et al., 2006; Hossini et al., 2015; Malakootian et al., 2011). On the contrary, adsorption has been found to be superior to other techniques for water re-use in terms of initial cost and insensitivity to toxic substances (Meshko et al., 2001). Zeolites material including synthetic and natural forms have become increasingly important due to the wide range of their chemical and physical characteristics, and have been applied as adsorbents, ion exchangers, membranes, molecular sieves, and catalysts in the past decades (Wang et al., 2006). In this study, the potential of Iranian zeolite was tested as a low cost adsorbent. The aim of this study is to estimate the ability of modified Iranian zeolite for the removal of Direct dyes. The optimum parameters were determined to be used in column design and other applications. Furthermore, the equilibrium and kinetic studies were carried out for this adsorbent.

Materials and methods

All chemical reagent and material were prepared in laboratory grade.

Adsorbent

The natural zeolite was prepared from Semnan mines, Iran. After derivation, the natural zeolite was rinsed for 24 h and was dried at 200℃ to remove the impurity, contaminant, and moisture. Subsequently, zeolite was grinded and sorted by sieving in 50–70 meshes. Thereafter, in order to produce a higher quality zeolite, it was placed in contact with 1 M sodium chloride for 48 h and was shook at about 170 r/min. Saturation with sodium chloride provides more uniformity of zeolite surface, and enhances the cation exchange capacity. The saturated zeolite was washed with deionized water and was dried at 50℃. Finally, it was treated with 2 mmol/L of N-cetylpyridinium bromide (CPB) for 24 h and 170 r/min. Thereafter, samples were rinsed and placed at 50℃.

Adsorbate

Direct blue 71 has three azo bonds, and it is in the group of azo dyes with a large molecular weight (Molar mass 1029.87 g/mol). The molecular structure of Direct blue 71 is shown in Figure 1. Molecular formula is C₄₀H₂₃N₇Na₄O₁₃S₄. The stock solution of Dye was prepared by dissolving 200 mg of Direct blue 71 in 1000 mL deionized water. The other concentrations were diluted with stock solution. To evaluate the effect of initial dye concentrations, four values of 25, 50, 75, and 100 mg/L were selected. Due to typical concentration in textile wastewaters (about 50 mg/L) (Saien and Soleymani, 2007), the range of 25–100 mg/L was considered. The pH was adjusted to the desired value with 1 M NaOH and 1 M HCl.

Figure 1.

Direct blue 71 structure.

Analysis

Before the samples were analyzed, the filtration was employed to remove the solid material. pH was measured with a pH meter (Metrohm). The decolorization rate of the Direct blue 71 in the solution samples was analyzed by spectrophotometer (Perkin Elmer Lambda 25—uv/vis spectrometer), at a wavelength of maximum absorbance of 585 nm, respectively. The XRD, XRF, and SEM images were taken from both zeolite (natural and modified) by X’ Pert MPD Philips Holland, PW 2404 Philips Holland and XL30 Philips Holland, respectively. The experiments were carried out at room temperature of about 23℃ ± 1℃.

Kinetic and isotherm study

To analyze the adsorption equilibrium and kinetic, the most three common isotherms (Langmuir, Freundlich, and Temkin) and four kinetic models (pseudo first, pseudo second-order, intraparticle diffusion, and Elovich) were evaluated. The linearized form of equations was employed for determining the equilibrium, kinetic constants, and coefficients.

Results and discussion

Effect of contact time and initial concentrations

An investigation was conducted in order to study the effect of contact time at various initial dye concentrations (25, 50, 75, and 100 mg/L) on the rate of dye removal from solution. It can be clearly seen from Figure 2 that the adsorption increases rapidly in the first 0 to 30 min, and then gradually increases until it reaches the equilibrium in all dye concentrations at 120 min. The adsorption efficiency of modified zeolite were about 99.8, 85.6, 62.33, and 49% at 12 min of equilibrium for 25, 50, 75, and 100 mg/L dye concentrations, respectively. Maximum dye adsorption was obtained for 25 mg/L, and efficiency was reduced with increase in initial dye concentrations. Thereafter, 50 mg/L was chosen for other experiments.

Figure 2.

Effect of contact time and initial concentrations on Direct 71 adsorption.

Effect of initial pH and dosage

The pH is an important parameter in adsorption processes due to the following: it is a controlling factor that strongly affects the sorption mechanism of surface complexation and on the other hand, the pH of the system controls the adsorption capacity because of its influence on the surface properties of the adsorbent (Ajouyed et al., 2010), and provides the optimum condition for conversion of pollutant materials.

To determine the optimum pH, batch experiments were performed by taking in contact 100 mg/L of Direct 71 solution with 5 g of modified zeolite (CPB) for 120 min shaking time. For this object, several values of pH were considered such as 3, 5, 7, and 9. The adsorbed Direct 71 efficiency was calculated from the difference between initial C₁ and final C₂ concentrations of initial Direct 71 concentration in colored solution, before and after shaking (equation (1)).

Adsorbed Dye % = \frac{C_{1} - C_{2}}{C_{1}} \times 100

(1)

As shown in Figure 3, the percentage of adsorption decreased, when the initial pH of colored solution increased. This fact can occur due to characteristic changes of zeolite surface. In lower pH, the zeolite surface is charged positively as a result of higher proton ions and it can provide higher adsorption rates. On the other hand, due to negative charges, the dye molecule in aqueous solution and the positive sites of the adsorbent, are favorable for sorption of the dye (Xiong et al., 2010). Similarly, higher adsorption efficiency of direct dye in acidic pH was reported by (Nemr et al., 2009) and (Xiong et al., 2010).

Figure 3.

Effect of initial pH on Direct 71 adsorption.

The effect of initial Zeolite dosage is shown in Figure 4. In order to find the proper dose, five doses (2.5, 5, 7.5, 10, and 12.5 g) were tested. According to results, it can be seen that the higher dye molecule was removed at higher dosage of modified zeolite. Nevertheless, with regards to 5% Error bar, no significant efficiency percentage was observed for 5 g with upper doses.

Figure 4.

Effect of modified zeolite (CPB) dosage on Direct 71 adsorption.

Isotherm studies

In general, isotherms have been applied to describe the equilibrium between liquid and solid phases (Meshko et al., 2001). In other words, isotherm is the relationship between the equilibrium amount of adsorbed (Direct Blue 71) on sorbent surface (modified zeolite (CPB)) and residual concentration of adsorbed in solution. To analyze the adsorption isotherm, three models were employed including the Langmuir, Freundlich, and Temkin isotherms. The comprehensive detail of isotherm model has been reported by Foo and Hameed (2010). The following relations can represent the linear forms of the isotherm models (Hossini et al., 2014; Niri et al., 2015; Wang et al., 2010)

Langmuir equation \frac{C_{e}}{q_{e}} = \frac{1}{K_{c} q_{m}} + \frac{C_{e}}{q_{m}}

(2)

Freundlich equation \log q_{e} = \log (K_{F}) + 1 / n \log (C_{e})

(3)

Temkin equation q_{e} = B_{1} \ln k_{t} + B_{1} \ln C_{e}

(4)

As shown in Figure 5, the adsorption isotherm models comprising Langmuir (Figure 5(a)), Freundlich (Figure 5(b)), and Temkin (Figure 5(c)) are shown for experimental data. Regarding R² value of models, better correlation between isotherms and experimental data can be found. Nevertheless, the Langmuir with R² 0.995 indicates the best fit with the adsorption experimental data. Furthermore, in Langmuir analysis, the maximum adsorption capacity (q_m) by 13.66 mg/g was determined. As shown in Table 1, there are more details of isotherms including the constants and adsorption values for Direct blue 71 onto modified zeolite. A comparison of equilibrium constants of various dyes for zeolite is shown in Table 2. With regard, the adsorption of DB71 by zeolite is best correlated with the Langmuir and Freundlich isotherms. In addition, the maximum adsorption capacity was observed for all of them. It is obvious that the maximum adsorption capacity is between 0.5 and over 85 mg/g. However, a maximum adsorption capacity of 13.66 mg/g for Direct Blue 71 onto modified zeolite can be appropriate in the present work.

Figure 5.

Langmuir (a), Freundlich (b), and Temkin (c) isotherms.

Table 1.

Isotherm constants and correlation coefficients.

Isotherm	k_L	k_f	k_t	q _m(mg/g)	B	n	r ²
Langmuier	0.873			13.66	1.8459		0.995
Freundlich		5.221				3.547	0.879
Temkin			6.7061		3.91		0.947

Table 2.

Comparative evaluation of equilibrium constants for various adsorbates.

Adsorbent	Adsorbate	Equilibrium values and constants	Ref.
Surfactant-modified zeolites (SMZs)	Anionic dye Congo red	Langmuir, pseudo-second-order kinetic qm ∼ 69.94 mg/g at pH 6 and 20℃	Liu et al. (2014)
Australian natural zeolite	Basic dye	Langmuir and Freundlich models Cation-exchange capacity of 120 meq/100 g	Wang and Zhu (2006)
Mexican natural zeolites	basic blue 9 and basic violet 3	Langmuir and Sips isotherms qm ∼ 86.27 and 83.79 mg/g for basic blue 9 and basic violet 3 respectively	Hernández-Montoya et al. (2013)
Modified clinoptilolite	Congo red	qm ∼ 36.7 mg/g	Akgül (2014)
Turkish zeolite	Toluidine Blue O	Langmuir and Freundlich models Second-order adsorption model qm ∼ 2.1×10⁻⁴ mol g⁻¹ at solution pH of 11	Alpat et al. (2008)
Modified zeolite (clinoptilolite)	Three reactive dyes (Everzol Black, Everzol Red, Everzol Yellow)	qm ∼ 2.9 to 7.6 mg/g	Armağan and Turan (2004)
Zeolite MCM-22	Basic dyes including methylene blue, crystal violet, and rhodamine B	Langmuir and the Freundlich models Pseudo-second-order model qm ∼ 1.1 × 10⁻⁴ to 7 × 10⁻⁴ mol/g	Wang et al. (2006)
Surfactant-modified zeolite	Reactive Black 5 and Reactive Red 239	Freundlich Pseudo second-order kinetics 12.17–12.92 mg/g	Karadag et al. (2007)
Agricultureal by-product (wheat shells)	Direct blue 71	Freundlich Pseudo second-order kinetics qm ∼ 40.82, 45.66, and 46.30 mg/g at different temperatures 293, 303, and 313 K, respectively	Bulut et al. (2007)
Modified zeolites	Rhodamine B	Langmuir and Freundlich isothermal Pseudo-second-order kinetic qm ∼ 4.41 mg/g at 303 K	Cheng et al. (2016)
Zeolite synthesized from cycloneash Modified form (using hexadecyltrimethylammonium bromide)	Reactive Orange 16	Langmuir isotherm qm ∼ 0.58 mg/g qm ∼ 12.6 mg/g	Fungaro et al. (2013)
Surfactant-modified zeolites	Congo Red	Langmuir and Freundlich isothermal Pseudo-second-order kinetic	Sun et al. (2013)
Present study	Direct blue 71	The Langmuir isotherm (R² 0.995) Pseudo second-order models qm ∼ 13.66 mg/g	—

Kinetics studies

To investigate the capacity of mass transfer of dye molecules to zeolite sites, the kinetic relations were employed. Other beneficial aspects of kinetic studies are as follows: (i) to know more details about adsorption performance, facilities and apparatus, and mechanisms, (ii) to be effective for the pilot application, (iii) to determine the solution uptake rate (Qiu et al., 2009).

The four most popular kinetic models including pseudo first, pseudo second-order, intraparticle diffusion, and Elovich were evaluated, to determine the better mass transfer model. Hence, the linearized form of kinetic relations was employed. The linearized equations can represent the following (Equation (5)–(8)) (Arab Markadeh et al., 2016; Hossini et al., 2016; Moussavi et al., 2013)

Pseudo first-order equation log (q_{e} - q_{t}) = \log (q_{e}) - \frac{k_{1}}{2.303} t

(5)

Pseudo second - order equation \frac{t}{q_{t}} = \frac{1}{h} + \frac{1}{q_{e}} t

(6)

Elovich equation q_{t} = \frac{1}{β} 1 n (α . β) + \frac{1}{β} 1 n (t)

(7)

Intraparticle diffusion {\log q}_{t} = {\log k}_{id} + a \log (t)

(8)

Figure 6 illustrates the complete pattern of pseudo first-order (Figure 6(a)), pseudo second-order (Figure 6(b)) and Elovich (Figure 6(c)) as well as Intraparticle diffusion (Figure 6(d)) kinetics for each dye concentration. The results of kinetic study with its details are shown in Table 3. According to correlation coefficient values (R²), it can be concluded that the pseudo-second-order model is more fitted with the experimental data. Furthermore, as can be seen from Table 2, they are best correlated with the second-order kinetic.

Figure 6.

Pseudo first-order (a), pseudo second-order (b), Elovich (c), and intraparticle diffusion (d) kinetics.

Table 3.

Kinetic constants and correlation coefficients.

Kinetic	Direct blue 71 (mg/L)	K ₁	q_e (mg/g)	K ₂	K _id	β	α	r ²
P-first order	25	0.054581	1.2462					0.8303
	50	0.019806	2.0941					0.7275
	75	0.025563	4.7076					0.91
	100	0.044218	59.5388					0.8938
P-second order	25		4.9554	0.4906				1
	50		9.6993	0.1663				0.9999
	75		11.6144	0.0384				0.9996
	100		14.3885	0.025				0.9994
Intraparticle diffusion	25				0. 0604			0.7862
	50				0.1465			0.6993
	75				0.301			0.8186
	100				0.3686			0.8837
Elovich	25					3.8153	2.8973	0.915
	50					0.7739	1.1765	0.8494
	75					1.5384	1.2734	9312
	100					0.6491	1.1141	0.9527

XRD, XRF, and SEM analyses

In order to review the modified zeolite, the X-ray diffraction technique (XRD), X-ray fluorescence (XRF), and scanning electron microscope (SEM) analysis were taken. As shown in Figure 7, data points of experimental X-ray diffraction patterns were observed for the natural and modified zeolite sample. According to XRD pattern (Figure 7(a)), it can be seen that the zeolite used in this study, was mainly composed of clinoptilolite (10–60°θ) and cristalloite. The lower part belongs to Quartz (20–22°θ). Surfactant modification of this natural zeolite is seen in 50–60°θ on the structure (Figure 7(b)). In addition, more crystalline peak (24–26, 30–32, and 34–36°θ) were created during surface modification. Figure 8 shows the structure and morphological characteristics of the zeolite, before and after modification by SEM image. Proper structure of surface zeolite is represented. To identify the constituents of zeolite, the XRF analysis was considered. As shown in Table 4, details of XRF analysis are presented. According to zeolite constituents, Al₂O₃ and SiO₂ are the integral part of natural (raw) and modified zeolite. However, several elements such as P₂O₅, SO₃, Sr, and Zr were added when modification was carried out. The LOI is loss on ignition which shows the volatile portion after the heating of zeolite, and is a common method for determining the organic and carbonate content of samples (Heiri et al., 2001). The loss of ignition percentage of about ∼11.3% was determined for both types.

Figure 7.

XRD image of zeolite (a) natural zeolite and (b) modified zeolite with PCB.

Figure 8.

SEM image of zeolite (a) natural zeolite and (b) modified zeolite with PCB.

Table 4.

XRF test for both natural and modified zeolite.

Composition	Raw-zeolite (%)	M-zeolite (%)
Al₂O₃	10.49	10.475
SiO₂	69.33	69.32
Fe₂O₃	0.68	0.0662
TiO₂	0.2	0.191
CaO	1.3	1.289
K₂O	4.05	4.028
Mg O	0.42	0.41
P₂O₅	—	0.02
SO₃	—	0.045
Sr	—	0.028
Zr	—	0.017
Na₂O	2.25	2.244
LOI	11.28	11.27

Conclusion

This work identified modified zeolite as a suitable adsorbent for decolorization of Direct dye with large molecule weight from aqueous solution. Based on results, the following conclusion can be suggested. The adsorptions were rapid during the first 30 min, and reached equilibrium in 120 min. The adsorption efficiency of modified zeolite was about 99.8, 85.6, 62.33 and 49% at 12 min of equilibrium for 25, 50, 75, and 100 mg/L dye concentrations, respectively. Higher adsorption efficiency of direct dye was obtained at higher dose and acidic pH. The Langmuir isotherm (R² 0.995) and pseudo second-order models gave the best fit to equilibrium experimental data. In addition, according to XRD pattern, it can be inferred that the clinoptilolite is the most important ingredient of crystalloid phase.

Footnotes

Acknowledgements

The authors acknowledge all non-financial support provided by Kashan and Tehran University of Medical Sciences.

Declaration of Conflicting Interests

The author(s) declared no potential conflicts of interest with respect to the research, authorship, and/or publication of this article.

Funding

The author(s) received no financial support for the research, authorship, and/or publication of this article.

Appendix

References

Ajouyed

Hurel

Ammari

et al. (2010) Sorption of Cr(VI) onto natural iron and aluminum (oxy)hydroxides: Effects of pH, ionic strength and initial concentration. Journal of Hazardous Materials 174(1–3): 616–622.

Akgül

(2014) Enhancement of the anionic dye adsorption capacity of clinoptilolite by Fe 3+-grafting. Journal of Hazardous Materials 267: 1–8.

Alpat

Özbayrak

Alpat

et al. (2008) The adsorption kinetics and removal of cationic dye, Toluidine Blue O, from aqueous solution with Turkish zeolite. Journal of Hazardous Materials 151(1): 213–220.

Amin

(2009) Removal of direct blue-106 dye from aqueous solution using new activated carbons developed from pomegranate peel: Adsorption equilibrium and kinetics. Journal of Hazardous Materials 165(1–3): 52–62.

Arab Markadeh

Rezaee

Rastegar

et al. (2016) Optimization of Remazol Brilliant Blue adsorption process from aqueous solutions using multi-walled carbon nanotube. Desalination and Water Treatment 57(28): 13357–13365.

Arami

Limaee

Mahmoodi

et al. (2006) Equilibrium and kinetics studies for the adsorption of direct and acid dyes from aqueous solution by soy meal hull. Journal of Hazardous Materials 135(1–3): 171–179.

Armağan

Turan

(2004) Equilibrium studies on the adsorption of reactive azo dyes into zeolite. Desalination 170(1): 33–39.

Armagan

Turan

Elik

(2004) Equilibrium studies on the adsorption of reactive azo dyes into zeolite. Desalination 170(1): 33–39.

Bulut

Gözübenli

Aydın

(2007) Equilibrium and kinetics studies for adsorption of direct blue 71 from aqueous solution by wheat shells. Journal of Hazardous Materials 144(1–2): 300–306.

10.

Cheng

Pan

(2016) The adsorption of Rhodamine B in water by modified zeolites. Modern Applied Science 10(5): 67.

11.

El-Bahy

Ismail

Mohamed

(2009) Enhancement of titania by doping rare earth for photodegradation of organic dye (Direct Blue). Journal of Hazardous Materials 166(1): 138–143.

12.

Foo

Hameed

(2010) Insights into the modeling of adsorption isotherm systems. Chemical Engineering Journal 156(1): 2–10.

13.

Fungaro

Borrely

Carvalho

TEM.

(2013) Surfactant modified zeolite from cyclone ash as adsorbent for removal of Reactive Orange 16 from aqueous solution. American Journal of Environmental Protection 1(1): 1–9.

14.

Heiri

Lotter

Lemcke

(2001) Loss on ignition as a method for estimating organic and carbonate content in sediments: Reproducibility and comparability of results. Paleolimnology 25: 101–110.

15.

Hernández-Montoya

Pérez-Cruz

Mendoza-Castillo

et al. (2013) Competitive adsorption of dyes and heavy metals on zeolitic structures. Journal of Environmental Management 116: 213–221.

16.

Hossini

Esmaeili Taheri

Arab Markadeh

et al. (2016) Optimization of effective parameters in the biosorption of Cr(VI) using acid treated date palm fiber from aqueous solution. Desalination and Water Treatment 57(11): 4994–5003.

17.

Hossini

Rezaee

Mohamadiyan

(2015) Hexavalent chromium removal from aqueous solution using functionalized multi-walled carbon nanotube: Optimization of parameters by response surface methodology. Health Scope 4(1): e19892.

18.

Hossini

Rezaee

Rastegar

et al. (2014) Equilibrium and kinetic studies of chromium adsorption from wastewater by functionalized multi-wall carbon nanotubes. Reaction Kinetics, Mechanisms and Catalysis 112(2): 371–382.

19.

Karadag

Turan

Akgul

et al. (2007) Adsorption equilibrium and kinetics of Reactive Black 5 and Reactive Red 239 in aqueous solution onto surfactant-modified zeolite. Journal of Chemical & Engineering Data 52(5): 1615–1620.

20.

Liu

Ding

et al. (2014) Adsorption of the anionic dye Congo red from aqueous solution onto natural zeolites modified with N, N-dimethyl dehydroabietylamine oxide. Chemical Engineering Journal 248: 135–144.

21.

Malakootian

Jaafarzadeh

Hossaini

(2011) Efficiency of perlite as a low cost adsorbent applied to removal of Pb and Cd from paint industry effluent. Desalination and Water Treatment 26(1–3): 243–249.

22.

Meshko

Markovska

Mincheva

et al. (2001) Adsorption of basic dyes on granular acivated carbon and natural zeolite. Water Research 35(14): 3357–3366.

23.

Moussavi

Hosseini

Alahabadi

(2013) The investigation of diazinon pesticide removal from contaminated water by adsorption onto NH 4 Cl-induced activated carbon. Chemical Engineering Journal 214: 172–179.

24.

Nemr

Abdelwahab

El-Sikaily

et al. (2009) Removal of direct blue-86 from aqueous solution by new activated carbon developed from orange peel. Journal of Hazardous Materials 161(1): 102–110.

25.

Niri

Mahvi

Alimohammadi

et al. (2015) Removal of natural organic matter (NOM) from an aqueous solution by NaCl and surfactant-modified clinoptilolite. Journal of Water and Health 13(2): 394–405.

26.

Qiu H, Lu Lv, Pan B, et al (2009) Critical review in adsorption kinetic models. Journal of Zhejiang University Science A 10: 716–724.

27.

Saien

Soleymani

(2007) Degradation and mineralization of Direct Blue 71 in a circulating upflow reactor by UV/TiO2 process and employing a new method in kinetic study. Journal of Hazardous Materials 144(1–2): 506–512.

28.

Sax NI (1981) Cancer Causing Chemicals: Van Nostrand Reinhold. New York.

29.

Shirmardi

Mahvi

Hashemzadeh

et al. (2013) The adsorption of malachite green (MG) as a cationic dye onto functionalized multi walled carbon nanotubes. Korean Journal of Chemical Engineering 30(8): 1603–1608.

30.

Sun

Lin

Zhan

(2013) Adsorption of Congo red from aqueous solution on surfactant-modified zeolites with different coverage types: Behavior and mechanism. Separation Science and Technology 48(13): 2036–2046.

31.

Wang

Zhang

Zhao

et al. (2010) Adsorption of basic dyes on activated carbon prepared from Polygonum orientale Linn: Equilibrium, kinetic and thermodynamic studies. Desalination 254(1–3): 68–74.

32.

Wang

(2006) Application of zeolite MCM-22 for basic dye removal from wastewater. Journal of Colloid and Interface Science 295(1): 71–78.

33.

Wang

Zhu

(2006) Characterisation and environmental application of an Australian natural zeolite for basic dye removal from aqueous solution. Journal of Hazardous Materials 136(3): 946–952.

34.

Xiong

Meng

Zheng

TL.

(2010) Biosorption of C.I. Direct Blue 199 from aqueous solution by nonviable Aspergillus niger. Journal of Hazardous Materials 175(1–3): 241–246.

Equilibrium and kinetics studies of Direct blue 71 adsorption from aqueous solutions using modified zeolite

Abstract

Keywords

Introduction

Materials and methods

Adsorbent

Adsorbate

Analysis

Kinetic and isotherm study

Results and discussion

Effect of contact time and initial concentrations

Effect of initial pH and dosage

Isotherm studies

Kinetics studies

XRD, XRF, and SEM analyses

Conclusion

Footnotes

Acknowledgements

Declaration of Conflicting Interests

Funding

Appendix

References