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Applied Water Science

, Volume 1, Issue 3–4, pp 135–145 | Cite as

Sugarcane bagasse for the removal of erythrosin B and methylene blue from aqueous waste

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Abstract

Present study explores the potentiality of locally available cellulose, hemicellulose and lignin-rich agricultural by-product sugarcane bagasse (SB) for the removal of erythrosin B (EB) and methylene blue (MB) from aqueous waste. The SB has been characterized by Fourier transform infrared and scanning electron microscopy analytical techniques. Batch experiments have been carried out to determine the influence of parameters like initial dye concentration, pH of the medium, contact time between the adsorbate and adsorbent, weight of adsorbent and system temperature on the removal of EB and MB. Optimum conditions for adsorption are found to be pH 9, temperature 308 K and an equilibration time of 1 h. Under these conditions equilibrium isotherms have been analysed by Langmuir and Freundlich isotherm equations. Based on the Langmuir adsorption isotherm model, the predicted maximum monolayer adsorption capacities of SB for EB and MB are found to be 500 mg g–1 (at 328 K) and 1,000 mg g–1 (at 308 K), respectively. The separation factor reveals the favourable nature of the isotherm for the studied dyes—SB system. The thermodynamic study indicates that the adsorptions of dyes are spontaneous and endothermic process. High temperatures favour EB adsorption whereas optimum temperature for MB adsorption is 318 K.

Keywords

Erythrosin B Methylene blue Sugarcane bagasse Adsorption Isotherms 

Introduction

Expansion of business activities and explosion of population coupled with industrial revolution results in pollution of water, air and soil. The discharge of pollutants from various industries poses threat to Earth’s biodiversity. Among various types of environmental pollutions water pollution is of major concern and for its occurrence dye-based industries are the main cause and foremost. Dyes are released into the environment, entering into aquatic ecosystem, deteriorating the water quality and thereby affecting the flora and fauna. Globally, it is estimated that 10% of the total dyestuffs used or about 7 × 105 tons per annum are released into the environment. These dyestuffs cause aesthetic and real hazards to environment. The real hazards caused by these coloured and solid wastes in aqueous solution is considered as often toxic, carcinogenic, mutagenic or even explosive that might affect aquatic biota and also humans (Zahrim et al. 2011; Saha 2010; Han et al. 2008). These dyes get accumulated in living tissues throughout the food chain which has human at its top. Due to increasing use of dyes for various purposes, this danger seems to multiply. Thus, there is a need to control an emission of dyes into the environment.

In order to keep the ecosystem green, recently an increasing interest has been focused on the adsorption techniques (El-Sayed 2011; Aksu 2005). This technique is quite popular due to its simplicity as well as the availability of a wide range of adsorbents and it proved to be an effective and attractive process for the removal of non-biodegradable pollutants (including dyes) from wastewater (Ali and Gupta 2007; Saad et al. 2010; da Silva et al. 2011). In the past decade, Gupta et al. (2000, 2004a, b, 2005, 2006a, b, 2007a, b, 2008a, b, 2009a, b, c, 2011) made some great efforts to give collective information through review articles and research papers/reports about the current available techniques and adsorbents, for the dye removal and decolourization of aqueous waste. Most commercial systems use activated carbon as adsorbent to remove dyes from water because of its significant adsorption capacity. Although activated carbon is a preferred adsorbent yet its widespread use is restricted due to its cost. In order to decrease the cost of treatment, some attempts have been made to find low-cost alternative adsorbents. Recently, numerous studies have been conducted to develop cheaper and effective adsorbents from a variety of starting materials. By selecting proper adsorbent, it is possible to make the adsorption process promising and economically viable for the removal of contaminants (Annadurai et al. 2002; Sivaraj et al. 2001). Therefore, it is preferable to use low-cost adsorbents such as an industrial waste, natural ores and agricultural by-products (Jain et al. 2003; Kumar and Sivanesan 2006; Han et al. 2006; Low et al. 2011; Sharma et al. 2010; Bhattacharya and Sharma 2004; Mall et al. 2005; Lakshmi et al. 2009; Mohanty et al. 2006). In our recently published review article (Sharma et al. 2011), we have compiled an extensive list of adsorbents obtained from different sources, and this review also reports the optimum processing parameters to get maximum dye removal from effluent water. In the same review article, a comparison between the adsorbent capacities of chemically modified, pre-treated, and untreated adsorbents has also been made.

The prime objective of the proposed work is to study the adsorption efficiency of SB for the removal of EB and MB from aqueous waste by adsorption treatment. Moreover, dynamical behaviour of adsorption has been measured by the effect of concentration, pH, contact time, adsorbent dosage and system temperature. Equilibrium adsorption isotherms play an important role in the predictive modelling that is used for the analysis and design of adsorption systems. Therefore, adsorption equilibrium has also been modelled using the Langmuir and Freundlich adsorption isotherms. The dynamic steps involved in the adsorption have been evaluated at different concentrations and thermodynamic parameters such as Gibbs free energy change (∆Go), enthalpy change (∆Ho) and entropy change (∆So) have also been calculated.

Materials and methods

Pre-treatment of SB

Sugarcane bagasse is collected from nearby sugar mill of Phagwara, Punjab, India and it is primarily washed with tap water at least four to five times. After that it is soaked into distilled water for 48 h and then dried for 24 h at 373 K. The dried material is pulverized to convert it into fine powder and then used as adsorbent for the removal of EB and MB. Studies about surface functional groups and surface morphology of SB have been made by the most widely used diagnostic techniques, i.e. FT-IR and SEM, respectively (Ferrero 2007; Garg et al. 2004; Hameed 2009). FT-IR spectroscopy study has been performed on Shimadzu FT-IR 8400S spectrometer. The sample is prepared with KBr and pressed into pellets. A spectrum is collected in the mid-IR range from 400–4,000 cm−1 with a resolution of 1 cm−1. The morphology and particle size of SB specimen has been examined by SEM. For SEM, the sample is dispersed onto carbon tape and coated with gold using a sputter coater system to prevent charge accumulation on the sample. The SB particles are then observed on a JEOL JSM-5800 microscope operating in SEM mode at 20 kV.

Dye solution

For the present study, EB and MB have been supplied by CDH and Merck Specialities Pvt. Ltd., respectively. The dye stock solution of 1,000 ppm is prepared by dissolving 1 g of each dye in 1,000 mL of distilled water. The experimental solutions of desired concentrations are prepared by diluting the stock solution with distilled water. The characteristics and some properties of EB and MB are listed in Table 1.
Table 1

Physico-chemical properties of dyes erythrosin B and methylene blue

Dye

Erythrosin B

Methylene blue

Molecular structure

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Molecular formula

C20H6I4Na2O5

C16H18N3SCl

IUPAC name

2-(6-hydroxy-2,4,5,7-tetraiodo-3-oxo-xanthen-9-yl) benzoic acid

3,7-bis(dimethylamino)- phenothiazin-5-ium chloride

Synonyms

Erythrosine B; Acid red 51; 2′,4′,5′,7′-Tetraiodo-3′,6′-dihydroxy-spiro[3H-isobenzofuran-1,9′-xanthen]-3-one disodium salt, Acid red 51 sodium salt, etc.

3,7-Bis(dimethylamino)5-phenothiazinium chloride, Aizen methylene blue BH, Basic blue 9, Tetramethylthionine chloride, etc.

Molecular weight

879.86 g

319.85 g

Solubility in water

Soluble (11%)

Soluble (3.5%)

Absorption maxima

524 nm

668 nm

Colour index

45,430

52,015

Appearance

Dark red powder

Dark green powder

Sorption experiments

The adsorption of EB and MB on SB in liquid–solid system has been studied using a standard batch technique. The adsorption experiments have been carried out in 250 mL conical flasks by mixing a pre-weighed amount of desired adsorbent and 25 mL of aqueous dye solution of fixed concentration. The flasks are then clamped in a horizontal shaker with an intensity of agitation 4 rps to mix the reaction mixture for predetermined time interval at constant temperature. The agitation rate is same for all experiments. The parameters such as initial dye concentration, pH of the medium, time of contact, adsorbent dosage and system temperature are varied during different sets of batch experiments. After adsorption, the samples are filtered out using the Whatmann filter paper number-42 and care has been taken to repeatedly centrifuge the solution at high speed to avoid any solid particles in the solution phase. The left out concentration in the supernatant solution after adsorption process has been analysed using a Systronics 2201 double beam UV–VIS spectrophotometer by recording the absorbance changes at a wavelength of maximum absorbance (524 nm for EB and 668 nm for MB). The amount of dye adsorbed on the adsorbent surface has been calculated from the difference in the concentration of the solution phase before and after adsorption. All the experiments have been carried out in duplicate. The adsorption data is reported in terms of distribution coefficient (Kd) and adsorption percentage using the following equation:
$$ K_{\text{d}} = \left[ {\frac{{C_{\text{o}} - C_{\text{e}} }}{{C_{\text{e}} }}} \right] \times \left[ \frac{V}{W} \right] $$
(1)
$$ \% {\text{Adsorption}} = \left[ {\left( {C_{\text{o}} - C_{\text{e}} } \right)/C_{\text{o}} } \right] \times 100 $$
(2)
where Co and Ce are initial and equilibrium dye concentrations (mg L–1), respectively, V is the volume of solution in mL and W is the weight of adsorbent in g.

Thermodynamic parameters studies

The ∆Go of the adsorption process is related to the equilibrium constant by the classic Van’t Hoff equation:
$$ \Delta G^{\text{o}} = - RT\ln K_{\text{d}} $$
(3)
According to thermodynamics, ∆Go is also related to the ∆So and ∆Ho at constant temperature by the following equation:
$$ \Delta G^{\text{o}} = \Delta H^{\text{o}} - T\Delta S^{\text{o}} $$
(4)
On combining Eqs. (3) and (4), we get
$$ \ln K_{\text{d}} = - \Delta G^{\text{o}} /RT = \left( {\Delta S^{\text{o}} /R} \right) - \left( {\Delta H^{\text{o}} /RT} \right) $$
(5)
where the symbols have their respective meanings. ∆So and ∆Ho can be recorded from the intercept and the slope, respectively, of linear Van’t Hoff plot, i.e. lnKd versus 1/T.

Adsorption isotherm

Using a method of linear regression, the adsorption data have been fitted to Langmuir (Langmuir 1918) adsorption model to describe the adsorption processes between solid–liquid interface.

Langmuir isotherm;
$$ C_{\text{e}} /q_{\text{e}} = 1/\left( {K_{\text{L}} q_{\text{m}} } \right) + C_{\text{e}} /q_{\text{m}} $$
(6)
(Linear form)
$$ q_{\text{e}} = \left( {C_{\text{o}} - C_{\text{e}} } \right) \times V/W $$
(7)
where qe is the amount of dye adsorbed per unit weight of adsorbent (mg g–1). KL and qm are the Langmuir coefficients representing the equilibrium constant for the adsorbate—adsorbent equilibrium and the monolayer capacity, respectively. A plot of Ce/qe versus Ce indicates a straight line of slope 1/qm and an intercept of 1/KLqm. The value of qm represents the practical limiting adsorption capacity or maximum value of monolayer adsorption.
Furthermore, the feasibility of the adsorption process is evaluated by the method suggested by Weber and Chakravorti (1974). One of the essential characteristics of Langmuir equation could be expressed by a dimensionless constant called equilibrium parameter or separation factor, RL which can be calculated by the following equation (Hall et al. 1966):
$$ R_{\text{L}} = 1/\left( {1 + K_{\text{L}} C_{\text{o}} } \right) $$
(8)
where Co is the highest initial dye concentration (mg L–1).
The Freundlich isotherm is a special case for heterogeneous surface energy in which energy in the Langmuir equation varies as a function of surface coverage strictly due to variation of adsorption (Freundlich 1906). The linear form of Freundlich isotherm is given as:
$$ { \log } q_{\text{e}} = \log K_{\text{F}} + \frac{1}{n}{ \log } C_{\text{e}} $$
(9)
where KF and n are Freundlich constants. The value of KF can be taken as a relative indicator of adsorption capacity while n shows the energy or intensity of adsorption.

Results and discussion

Fourier transform infrared spectroscopy analysis

The FT-IR spectrum of SB, presenting the plot of percentage transmission versus wave number, is given in Fig. 1. The FT-IR spectrum shows that sugarcane bagasse has functional groups of standard polymer α-cellulose and coir pith-lignin. The FT-IR spectroscopic analysis indicates broad band observed at 3,424 cm–1 representing bonded –OH groups. The band observed at about 2,927 cm–1 could be assigned to the aliphatic C–H group. The peaks described in the region of 1,600–1,590 cm–1 represent skeletal vibrations of benzene ring. The peaks observed at 1,420–1,300 cm–1 are attributed to C = C–H in plane bending indicating several bands in cellulose and xylose. Vibrational bands around wave number 1,356 cm–1 may be due to –CH2 wagging and twisting indicates several bonds in deoxysugars complex. The peak observed at 1,121 cm–1 represents C–O–C stretching as appears in polysaccharides.
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Fig. 1

FTIR spectra of SB

Scanning electron microscopic study

The SEM images of typical SB sample at different magnifications have been taken to analyse the morphology of the material more clearly. Micrographs (Fig. 2) show that SB particles have fibrous character. These images also reveal that SB samples have compacted layer character in which thin layers of cellulosic material are laying one on one. These fibres are of generally ~1.0 mm in length and of ~0.35 mm diameter. The second micrograph depicts that some very small particles of nearly 0.5–2.0 μm in size adhere to the surface of large size fibres. These small grains may also take part in the adsorption process.
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Fig. 2

SEM images of SB at two different magnifications

Effect of initial concentration of dye on adsorption

The effects of EB and MB dye concentrations on adsorption process have been studied at neutral pH and equilibration time of 1 h. To study the effects of initial dye concentration, EB solution of concentration 10, 100, 200, 400 and 600 mg L−1 are used in conjunction with SB sample of 50, 200 and 400 mg. On the other hand, MB solution of concentration 100, 500 and 1000 mg L−1 are used in conjunction with SB doses of 100, 200 and 400 mg. From Fig. 3 it has been found that the adsorption percentage decreases with increase in concentration of the adsorbate while the amount of dye removed at equilibrium increases with increase in dye concentration in both the cases. This is so because the initial dye concentration provides the driving force to overcome the resistance to mass transfer of dye (EB and MB) between the aqueous and solid phase (Azhar et al. 2005).
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Fig. 3

Variation in percentage adsorption with dyes concentration: a EB on three different SB doses, b MB on 200 mg of SB

Effect of pH

The pH value of the solution is an important factor that must be considered during adsorption studies. The range of pH has been adjusted between pH 1–9. Digital pH meter (Model LT-10) has been used for the pH measurements. The initial pH of the working solutions has adjusted by addition of dilute HCl and NaOH solution (Analytical grade, CDH and S.D.fine Pvt. Ltd). The effect of pH on the adsorption of EB and MB by SB is shown in Fig. 4. It has been found that adsorption increases with increase in pH. This may be due to the fact that at higher pH values the surface of adsorbent becomes negative which enhances the adsorption of positively charged MB cations through electrostatic force of attraction. Although EB is an anionic dye, it still shows maximum adsorption at high pH (7–9) which indicates that there is not much effect of hydroxide ion at these pH values. If we compare the %adsorption of EB corresponding to pH 7 and 9, then we find that amount of dye adsorbed on the adsorbent is nearly same (Zhang et al. 2011). This reveals that at neutral pH, EB shows maximum adsorption.
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Fig. 4

Effect of initial pH of the medium on the adsorption of EB and MB on SB

Effect of contact time

Batch adsorption studies have also been conducted at different contact times (10, 30, 60, 90, 120, 150, and 180 min) by taking initial concentration of dye 100 mg L–1 with 200 mg adsorbent dose of SB in 25 mL dye solution of EB as well as MB, at neutral pH and 308 K temperature. Effects of contact time on adsorption of EB and MB dyes onto SB are illustrated in Fig. 5. This data reveals that as the contact time increases, rate of adsorption first increases and then becomes almost constant. This is due to the aggregation of dye molecules with the increase in contact time, which makes it almost impossible to diffuse deeper into the adsorbent structure at higher energy sites. This aggregation negates the influence of contact time as the pores get filled up and start offering resistance to diffusion of aggregated dye molecules in the adsorbents (Mall et al. 2005). It has been seen that the equilibration time of 1 h is sufficient since maximum adsorption is attained during this period.
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Fig. 5

Effect of contact time between the adsorbent and adsorbate on the percentage adsorption of EB and MB on SB

Effect of adsorbent dosage

The adsorbent dose is also one of the important parameters to optimize an adsorption system. The effect of adsorbent dose on the adsorption of dyes has been investigated by employing different doses of SB varying from 50 to 1,500 mg. These adsorption experiments are performed at neutral pH, 308 K, equilibration time 1 h and at different dye concentrations. Figure 6 demonstrates that the removal of dye increases with increase in adsorbent dosage. An increase in the adsorption with increase in adsorbent dosage can attribute to greater surface area and the availability of more adsorption surface sites (Sharma et al. 2010; Gupta et al. 2004b). It can be seen that for 10 mg L–1 EB solution, 50 mg of SB in 25 mL is sufficient for the adsorption studies as it shows 100% adsorption but for higher concentration dye solutions, higher dosage of SB is required (Fig. 6a). While in case of MB removal, a high dosage of SB (Fig. 6b) is required even for low-concentrated dye solution.
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Fig. 6

Variation in percentage adsorption of: a EB on SB and b MB on SB at three concentrations with change in adsorbent doses

Effect of temperature

In order to optimize the system temperature for the maximum removal efficiency, experiments have been conducted at three different temperatures 308, 318 and 328 ± 0.1 K by varying dye concentration and keeping other parameters constant such as neutral pH, equilibration time 1 h, adsorbent dose of 200 mg. Experimental results concerning the effect of temperature on the adsorption of dyes at different initial dye concentration are demonstrated in Fig. 7. In case of EB adsorption on SB, the adsorption percentage increases when the temperature of solution is increased from 308 to 328 K which indicates that the process is endothermic in nature. Better adsorption at higher temperature may be either due to the acceleration of some originally slow adsorption steps or due to the retardation of the processes such as association of ions, aggregation of molecules, ion pairing and complex formation in the system because of thermal agitation. This can also be due to creation of new active sites on the adsorbent surface. Thus, an increase in temperature will reduce the electrostatic repulsion between the surface and the adsorbing species and this allow adsorption to occur more readily. This could also be due to enhanced mobility of dye molecules from solution to the sorbent surface (Sharma and Tomar 2011). Furthermore, increasing temperature may produce a swelling effect within the internal structure of SB enabling large dye to penetrate further. In case of MB, the adsorption percentage first increases when temperature rises from 308 to 318 K and then start decreasing with further increase in temperature indicating that the process is exothermic in nature. This decrease indicates that there are very weak binding forces between the dye molecule and adsorbent surface which may break at high temperature. This is because with increasing temperature the attractive forces between adsorbent surface and dye molecule are weakened and the adsorption decreases (>318 K). Increase in temperature may also cause the more pore expansion which may leads to leaching of MB molecules adsorbed on the SB (Khattri and Singh 2011).
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Fig. 7

Effect of temperature on percentage adsorption of: a EB on SB and b MB on SB at different dye concentrations

Thermodynamic parameters

Thermodynamic parameters, i.e. free energy change (ΔG°), enthalpy change (ΔH°) and entropy change (ΔS°), vary with the thermodynamic equilibrium constant (Kd) (Fig. 8) and have been calculated using standard equations (Eqs. 3 and 5) mentioned above. The values of thermodynamic parameters for EB on SB are reported in Table 2. The negative values of ΔG° obtained in both the cases reveal that the adsorption of dye is thermodynamically feasible and spontaneous. Positive value of ∆Ho confirms the endothermic nature the adsorption process. Hence, on increasing temperature, degree of adsorption will increase. The numerical value of ∆Ho also predicts the physisorption behaviour of these adsorption processes. The positive values of ΔS° reflect the affinity of SB towards EB and also indicate that the randomness is increased at the solid/solution interface during the adsorption process (Acemioglu 2005; Yuan 2008; Ahmad et al. 2007; Bestani et al. 2008; Azhar et al. 2005).
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Fig. 8

Variation of ln Kd with temperature (1/T) for the adsorption of EB onto SB (Van’t Hoff plot)

Table 2

Thermodynamic parameters for the adsorption of EB on SB at five different concentrations

Initial dye concentration (mg L−1)

∆Ho (J mol−1)

∆So (J mol−1K−1)

∆Go (J mol−1)

308 K

318 K

328 K

10

91.09

1.52

−376.43

−391.61

−406.79

100

44.90

1.33

−365.20

−378.51

−391.83

200

46.25

1.32

−360.89

−374.11

−387.32

400

50.00

1.32

−355.28

−368.44

−381.60

600

47.81

1.29

−349.69

−362.60

−375.50

Adsorption isotherms parameters

The adsorption isotherm studies provide information about the capacity of adsorbent to remove dyes under given set of conditions. Experimental results obtained for the adsorption of EB and MB dyes on agricultural waste SB at three different temperatures (308, 318 and 328 K) have been fitted to Langmuir isotherm model. The plot between Ce/qe and Ce yield straight lines (Fig. 9). The obtained R2 values confirm that the adsorption equilibrium data fitted well to the Langmuir model under the studied conditions. These isotherms are found to be linear over the entire studied concentration range with extremely high R2 values (Table 3). The R2 values suggest that the Langmuir isotherm provides a good model for the present adsorption systems. This indicates uniform adsorption and strong dye–adsorbent interactions over the surfaces of the adsorbent. Figs. 9a, b show the Langmuirian plots for EB and MB adsorption on SB, respectively. The values of the Langmuir constant (KL), the monolayer capacity of adsorbent (qm), and R2 values are listed in Table 3. The qm values reveal that adsorption capacity of SB for MB adsorption (1,000.0 mg g–1) is double in comparison to EB adsorption (500.0 mg g–1). High KL values also indicate the high affinity of SB for the adsorption of EB and MB.
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Fig. 9

Langmuir adsorption isotherms for; a EB adsorption on SB and b MB adsorption on SB at three different temperatures

Table 3

Adsorption isotherms constants for EB and MB adsorption on SB at three different temperatures

Isotherm

Parameters

EB adsorption on SB

MB adsorption on SB

308 K

318 K

328 K

308 K

318 K

328 K

Langmuir

qm (mg g−1)

333.3

333.3

500.0

1,000.0

1,000.0

1,000.0

K L (L mg−1)

0.070

0.081

0.053

0.005

0.006

0.005

R 2

0.99

0.99

0.99

0.95

0.98

0.99

R L

0.023

0.020

0.031

0.159

0.140

0.158

Freundlich

K F

2.16

2.80

3.33

0.11

1.17

1.05

1/n

0.42

0.39

0.38

0.68

0.68

0.67

R 2

0.99

0.99

0.99

0.99

0.99

0.98

The RL parameter is considered as a more reliable indicator of adsorption. There are four possibilities for RL values: (1) for favourable adsorption, 0 < RL < 1; (2) for unfavourable adsorption, RL > 1; (3) for linear adsorption, RL = 1; and (iv) for irreversible adsorption, RL = 0 (Senturk et al. 2009). In both the cases, the values of RL (Table 3) are found to be positive and less than unity indicating thereby a highly favourable adsorption in all cases.

Freundlich adsorption isotherm gives an expression encompassing the surface heterogeneity and the exponential distribution of active sites and their energies. For a favourable adsorption process, the value of 1/n should be less than 1 and higher than 0.1 (Senturk et al. 2009). The Freundlich constants KF and 1/n are determined from the slope and intercept of ln qe versus ln Ce plots (Fig. 10) and are tabulated in Table 3 along with the correlation coefficient values (R2). The high correlation coefficients (R2 = 0.98 − 0.99) reflect that the experimental data agree well with the Freundlich adsorption isotherm model. The values of 1/n are higher than 0.1 and smaller than 1, indicating a favourable adsorption of dyes on SB. According to the statistical theory of adsorption when the value of 1/n is less than unity, it also implies heterogeneous surface with minimum interactions between the adsorbed molecules. The KF values (Table 3) indicate that SB has good adsorption capacity for MB removal from aqueous system in comparison to EB. This isotherm does not predict any saturation of the adsorbent by the adsorbate thus infinite surface coverage is predicted mathematically indicating the multilayer sorption of the surface.
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Fig. 10

Freundlich adsorption isotherms for; a EB adsorption on SB and b MB adsorption on SB at three different temperatures

Conclusions

The removal of EB and MB from wastewater using SB has been investigated under different experimental conditions in batch mode. The adsorption of EB and MB has found to be dependent on the adsorbent dose and initial dye concentration. Thus, the efficient removal of these dyes from an effluent using SB may require pH adjustment 7–9. It has been found that optimum dose of 200 mg of SB adsorbs 93.3% EB and 83.6% MB of initial dye concentration (100 mg L–1). Equilibration time of 1 h is sufficient between adsorbent and adsorbate to carry out the adsorption experiments for these adsorption systems and 308–318 K is the optimum temperature to perform the adsorption experiments and to achieve the maximum removal of dyes from aqueous waste. This work also presents the experimental results concerning monolayer and multilayer adsorption isotherms of dyes on SB. Both the adsorption isotherm models (Langmuir and Freundlich) give good agreement with experimental results for the adsorption of EB as well as MB on SB. A maximum monolayer adsorption capacity of SB is 500 mg g–1 for EB and 1,000 mg g–1 for MB. It is much higher than that of the other reported adsorbents (Sharma et al. 2010; Crini 2006; Gupta and Suhas 2009). The thermodynamics of EB–SB system indicates spontaneous and endothermic nature of the process. The obtained results reveal that the low-cost adsorbent (sugarcane bagasse) can be used for the removal of EB and MB from aqueous waste.

References

  1. Acemioglu B (2005) Batch kinetic study of sorption of methylene blue by perlite. Chem Eng J 106:73–81CrossRefGoogle Scholar
  2. Ahmad AL, Loh MM, Aziz JA (2007) Preparation and characterization of activated carbon from oil palm wood and its evaluation on methylene blue adsorption. Dye Pigment 75:263–272CrossRefGoogle Scholar
  3. Aksu Z (2005) Application of biosorption for the removal of organic pollutants: a review. Process Biochem 40:997–1026CrossRefGoogle Scholar
  4. Ali I, Gupta VK (2007) Advances in water treatment by adsorption technology. Nat Protoc 1:2661–2667CrossRefGoogle Scholar
  5. Annadurai G, Juang RS, Lee DJ (2002) Use of cellulose-based wastes for adsorption of dyes from aqueous solutions. J Hazard Mater 92:263–274CrossRefGoogle Scholar
  6. Azhar SS, Liew AG, Suhardy D, Hafiz KF, Hatim MD (2005) Dye removal from aqueous solution by using adsorption on treated sugarcane baggase. Am J App Sci 2:1499–1503CrossRefGoogle Scholar
  7. Bestani B, Benderdouche N, Benstaali B, Belhakem M, Addou A (2008) Methylene blue and iodine adsorption onto an activated desert plant. Bioresour Technol 99:8441–8444CrossRefGoogle Scholar
  8. Bhattacharya KG, Sharma A (2004) Azadirachta indica leaf powder as an effective biosorbent for dyes: a case study with aqueous congo red solutions. J Environ Manag 71:217–229CrossRefGoogle Scholar
  9. Crini G (2006) Non-conventional low-cost adsorbents for dye removal: a review. Bioresour Technol 97:1061–1085CrossRefGoogle Scholar
  10. da Silva LG, Ruggiero R, Gontijo PDM, Pinto RB, Royer B, Lima EC, Fernandes THM, Calvete T (2011) Adsorption of Brilliant Red 2BE dye from water solutions by a chemically modified sugarcane bagasse lignin. Chem Eng J 168:620–628CrossRefGoogle Scholar
  11. El-Sayed GO (2011) Removal of methylene blue and crystal violet from aqueous solutions by palm kernel fiber. Desalination 272:225–232CrossRefGoogle Scholar
  12. Ferrero F (2007) Dye removal by low cost adsorbent: hazelnut shells in comparison with wood sawdust. J Hazard Mater 142:144–152CrossRefGoogle Scholar
  13. Freundlich HMF (1906) Uber die adsorption in Losungen. Z Phys Chem 57:385–470Google Scholar
  14. Garg VK, Amita M, Kumar R, Gupta R (2004) Basic dye (methylene blue) removal from simulated wastewater by adsorption using Indian Rosewood sawdust: a timber industry waste. Dye Pigment 63:243–250CrossRefGoogle Scholar
  15. Gupta VK, Ali I (2008) Removal of endosulfan and methoxychlor from water on carbon slurry. Environ Sci Technol 42:766–770CrossRefGoogle Scholar
  16. Gupta VK, Suhas (2009) Application of low-cost adsorbents for dye removal—a review. J Environ Manag 90:2313–2342Google Scholar
  17. Gupta VK, Mohan D, Sharma S, Sharma M (2000) Removal of basic dyes (rhodamine B and methylene blue) from aqueous solutions using bagasse fly ash. Sep Sci Technol 35:2097–2113CrossRefGoogle Scholar
  18. Gupta VK, Mittal A, Krishna L, Gajbe V (2004a) Adsorption kinetics and column operations for the removal and recovery of malachite green from wastewater using bottom ash. Sep Purif Technol 40:87–96CrossRefGoogle Scholar
  19. Gupta VK, Suhas AliI, Saini VK (2004b) Removal of rhodamine B, fast green, and methylene blue from wastewater using red mud, an aluminum industry waste. Ind Eng Chem Res 43:1740–1747CrossRefGoogle Scholar
  20. Gupta VK, Ali I, Saini VK, Van Gerven T, Van Bruggen BD, Vandecasteele C (2005) Removal of dyes from wastewater using bottom ash. Ind Eng Chem Res 44:3655–3664CrossRefGoogle Scholar
  21. Gupta VK, Mittal A, Gajbe V, Mittal J (2006a) Removal and recovery of the hazardous azo dye acid orange 7 through adsorption over waste materials: bottom ash and de-oiled soya. Ind Eng Chem Res 45:1446–1453CrossRefGoogle Scholar
  22. Gupta VK, Mittal A, Jain R, Mathur M, Sikarwar S (2006b) Adsorption of Safranin-T from wastewater using waste material-activated carbon and activated rice husks. J Colloid Inter Sci 303:80–86CrossRefGoogle Scholar
  23. Gupta VK, Ali I, Saini VK (2007a) Adsorption studies on the removal of Vertigo Blue 49 and Orange DNA13 from aqueous solutions using carbon slurry developed from a waste material. J Colloid Inter Sci 315:87–93CrossRefGoogle Scholar
  24. Gupta VK, Jain R, Varshney S (2007b) Removal of Reactofix golden yellow 3 RFN from aqueous solution using wheat husk—an agricultural waste. J Hazard Mater 142:443–448CrossRefGoogle Scholar
  25. Gupta VK, Mittal A, Gajbe V, Mittal J (2008) Adsorption of basic fuchsin using waste materials—bottom ash and deoiled soya—as adsorbents. J Colloid Inter Sci 319:30–39CrossRefGoogle Scholar
  26. Gupta VK, Carrott PJM, Ribeiro Carrott MML, Suhas (2009a) Low-cost adsorbents: growing approach to wastewater treatment—a review. Crit Rev Environ Sci Technol 39:783–842Google Scholar
  27. Gupta VK, Mittal A, Malviya A, Mittal J (2009b) Adsorption of carmoisine A from wastewater using waste materials—bottom ash and deoiled soya. J Colloid Inter Sci 335:24–33CrossRefGoogle Scholar
  28. Gupta VK, Gupta B, Rastogi A, Agarwal S, Nayak A (2011) A comparative investigation on adsorption performances of mesoporous activated carbon prepared from waste rubber tire and activated carbon for a hazardous azo dye—Acid Blue 113. J Hazard Mater 186:891–901CrossRefGoogle Scholar
  29. Hall KR, Eagleton LC, Acrivos A, Vermeulen T (1966) Pore and solid diffusion kinetics in fixed adsorption constant pattern conditions. Ind Eng Chem Res 5:212–223Google Scholar
  30. Hameed BH (2009) Removal of cationic dye from aqueous solution using jackfruit peel as a non-conventional and low-cost adsorbent. J Hazard Mater 162:344–350CrossRefGoogle Scholar
  31. Han RP, Wang YF, Han P, Shi J, Yang J, Lu YS (2006) Removal of methylene blue from aqueous solution by chaff in batch mode. J Hazard Mater 137:550–557CrossRefGoogle Scholar
  32. Han R, Dandan D, Xu Y, Zou W, Wang Y, Li Y, Zou L (2008) Use of rice husk for the adsorption of Congo red from aqueous solution in column mode. Bioresour Technol 99:2938–2946CrossRefGoogle Scholar
  33. Jain AK, Gupta VK, Bhatnagar A, Suhas (2003) A comparative study of adsorbents prepared from industrial waste for the removal of dyes. Sep Sci Technol 38:463–481Google Scholar
  34. Khattri SD, Singh MK (2011) Use of Sagaun sawdust as an adsorbent for the removal of crystal violet dye from simulated wastewater. Environ Prog Sustainable Energy. doi: 10.1002/ep.10567
  35. Kumar KV, Sivanesan S (2006) Equillibrium data isotherm parameters and process design for partial and complete isotherm of methylene blue onto activated carbon. J Hazard Mater 131:217–228CrossRefGoogle Scholar
  36. Lakshmi UR, Srivastva CV, Mall DI, Lataye DH (2009) Rice husk ash as an effective adsorbent: evaluation of adsorptive characteristics for indigo carmine dye. J Environ Manag 90:710–720CrossRefGoogle Scholar
  37. Langmuir I (1918) The adsorption of gases on plane surfaces of glass, mica and platinum. J Am Chem Soc 40:1361–1403CrossRefGoogle Scholar
  38. Low LW, Teng TT, Ahmad A, Morad N, Wong YS (2011) A novel pretreatment method of lignocellulosic material as adsorbent and kinetic study of dye waste adsorption. Water Air Soil Poll 218:293–306CrossRefGoogle Scholar
  39. Mall ID, Srivastva VC, Agarwal NK, Mishra IM (2005) Removal of Congo red from aqueous solution by baggase fly ash and activated carbon: kinetic study and equilibrium isotherm analyses. Chemosphere 61:492–501CrossRefGoogle Scholar
  40. Mohanty K, Naidu JT, Meikap BC, Biswas MN (2006) Removal of crystal violet from wastewater by activated carbons prepared from rice husk. Ind Eng Chem Res 45:5165–5171CrossRefGoogle Scholar
  41. Saad SA, Isa KM, Bahari R (2010) Chemically modified sugarcane bagasse as a potentially low-cost biosorbent for dye removal. Desalination 264:123–128CrossRefGoogle Scholar
  42. Saha P (2010) Assessment on the removal of methylene blue dye using tamarind fruit shell as biosorbent. Water Air Soil Poll 217:287–299CrossRefGoogle Scholar
  43. Senturk HB, Ozdes D, Gundogdu A, Duran C, Soylak M (2009) Removal of phenol from aqueous solutions by adsorption onto organomodified Tirebolu bentonite: equilibrium, kinetic and thermodynamic study. J Hazard Mater 172:353–362CrossRefGoogle Scholar
  44. Sharma P, Tomar R (2011) Sorption behaviour of nanocrystalline MOR type zeolite for Th(IV) and Eu(III) removal from aqueous waste by batch treatment. J Colloid Inter Sci 362:144–156CrossRefGoogle Scholar
  45. Sharma P, Kaur R, Baskar C, Chung WJ (2010) Removal of methylene blue from aqueous waste using rice husk and rice husk ash. Desalination 259:249–257CrossRefGoogle Scholar
  46. Sharma P, Kaur H, Sharma M, Sahore V (2011) A review on applicability of naturally available adsorbents for the removal of hazardous dyes from aqueous waste. Environ Monit Assess. doi: 10.1007/s10661-011-1914-0
  47. Sivaraj R, Namasivayam C, Kadirvelu K (2001) Orange peel as an adsorbent in the removal of Acid violet 17 from aqueous solutions. Waste Manag 21:105–110CrossRefGoogle Scholar
  48. Weber TW, Chakravorti RK (1974) Pore, solid diffusion models for fixed bed adsorbers. AIChE J 20:228–238CrossRefGoogle Scholar
  49. Yuan Z (2008) Kinetics and Mechanism of the adsorption of methylene blue onto ACFs. J China Univ Min Technol 18:0437–0440CrossRefGoogle Scholar
  50. Zahrim AY, Tizaoui C, Hilal N (2011) Coagulation with polymers for nanofiltration pre-treatment of highly concentrated dyes: a review. Desalination 266:1–16CrossRefGoogle Scholar
  51. Zhang G, Li X, Li Y, Wu T, Sun D, Lu F (2011) Removal of anionic dyes from aqueous solution by leaching solutions of white mud. Desalination 274:255–261CrossRefGoogle Scholar

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Authors and Affiliations

  1. 1.Department of ChemistryLovely School of Sciences, Lovely Professional UniversityPhagwaraIndia
  2. 2.Energy Materials Center, Korea Institute of Energy ResearchDaejeonRepublic of Korea

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