Research Article  Open Access
Siti Kartina Abdul Karim, Soh Fong Lim, S. N. David Chua, Shanti Faridah Salleh, Puong Ling Law, "Banana Fibers as Sorbent for Removal of Acid Green Dye from Water", Journal of Chemistry, vol. 2016, Article ID 9648312, 11 pages, 2016. https://doi.org/10.1155/2016/9648312
Banana Fibers as Sorbent for Removal of Acid Green Dye from Water
Abstract
In this study, banana fibers extracted from banana leaves, stem, and stalk were used to remove acid green dye from aqueous solution. Three initial concentrations (750, 1000, and 1500 ppm) were chosen to determine the kinetic characteristics of the banana fiber sorbents at 25°C, agitation speed of 200 rpm, and total contact time of 3 hours. The pseudofirstorder, pseudosecondorder, and DunwaldWagner kinetic models were applied to the experimental kinetic data. For isotherm study, the batch experiments were performed at 25°C, initial pH 2, agitation speed of 200 rpm, and initial concentrations between 100 and 2000 ppm. The experimental data was fitted to the Langmuir, Freundlich, DubininRadushkevich, and Temkin isotherms. The equilibrium was achieved in less than 90 minutes. The removal of the acid green dye was found to be following closely the pseudosecondorder kinetic model. For equilibrium study, the Freundlich isotherm was found to fit well with adsorption of acid green dye on the banana leaves, stem, and stalk sorbents. The calculated mean free energy of 4–11 J/mol indicated that the sorption process was mostly physical in nature. Experimental results also showed the adsorption performance is greatly affected by the initial solution pH.
1. Introduction
There are various industries that use dyes as colouring agents, such as textile, paint, pharmaceuticals, beauty products, and food. The release of dyes to water is harmful to the aquatic lives as most dyes are complex in nature and of synthetic origin [1]. Moreover, dyes hinder sunlight from entering water and slowing photosynthesis for plants in water [2]. Some of the techniques used to treat dyecontaining wastewater are Fenton oxidation, membrane filtration, photodegradation, coagulationflocculation, biosorption, and adsorption [3–10]. Ease of use, low energy application, and simple operation are some of the advantages of using membrane and coagulationflocculation [6, 7]. The drawbacks include searching for the right coagulants to maximize the process and membrane fouling. Chemical processes such as oxidation have high efficiency, though the high cost and disposal pose concern on the treatment process [11]. Adsorption is a physical process and has the advantages of simplicity, easy usage, and low energy consumption, similar to membrane and coagulationflocculation [12]. The use of natural fibers as sorbents is an attractive option, as it is biodegradable and low cost.
The use of natural fibers has been studied over a wide range of water pollutants. The sorbents are used in natural or unmodified form, as activated carbon, as biochar, or modified with other chemicals. Modification of natural fibers as activated carbon has been demonstrated using pineapple waste [2], where the surface area of activated carbon was higher than 500 m^{2}/g and the maximum adsorption capacity was found to be 288 mg/g for adsorption of methylene blue. Biochar activated with microwave treatment was performed on P. juliflora species [13], where the surface area of adsorbents used was between 220 and 330 m^{2}/g, and the maximum adsorption capacity increased compared to the nonmicrowavetreated biochar. The use of unmodified and modifiedbycalcination rice bran revealed that calcination at high temperature had an adverse effect on the adsorption capacity of the adsorbents [1]. Using methylene blue and crystal violet dyes as model compounds, the adsorption capacity for uncalcined and calcined rice bran decreased from 325.9 to 172.5 mg/g and from 783.8 to 401.3 mg/g, respectively. The use of modification for natural fibers has to take into account the cost and environmental effects, as opposed to the increase (or decrease) in adsorption capacity.
Therefore, in this study, the natural form of banana is chosen as adsorbent. The banana plant used is taken from three parts of banana, which are the leaves, stem, and stalk. The three parts are used to remove acid green (AG) dye in aqueous solution.
2. Materials and Methods
2.1. Materials
The AG dye was purchased from Acros Organics. Analytical grade sodium hydroxide from Systerm (Malaysia) and 70.0% nitric acid from J.T. Baker (USA) were used to adjust the pH of solution. The acid and base were prepared at a concentration of 0.1 M. The sorbents were prepared by using banana plants collected from Samarahan, Sarawak, Malaysia. The dye stock solution of 10000 ppm was prepared by adding 10 g of the AG dye powder in 1000 mL of deionised water. The stock solution was diluted to the desired AG dye concentrations for experimental usage.
2.2. Preparation of Banana Fiber Sorbents
Three different parts of banana plant were used to prepare the sorbents, which were the leaves, stem, and stalk. The plants were scraped and the fibers extracted from the different parts. Next, the extracted fibers were cut to about 2 cm before they were washed several times with deionised water. The drying took place next, with room temperature drying for three days and oven drying at 60°C for 24 hours. After drying, the banana parts were ground and sieved using 500micron mesh size. The prepared sorbents were then stored in dry, airtight containers before use.
2.3. Batch Adsorption Experiments
In kinetic study, the experimental conditions were temperature at 25°C, agitation speed of 200 rpm, adsorbent dosage of 60 g/L, and initial pH 2. The AG dye concentrations were varied at 750, 1000, and 1500 ppm. The experiments were carried out at predetermined experimental contact time, varying from 1 minute to 3 hours. After the predetermined contact time, the samples were filtered and the residual solutions were analysed using UVVis spectrophotometer (Thermo Scientific, model Evolution 201) at 624 nm of .
Adsorption isotherm study for the batch adsorption experiments was conducted at 25°C with agitation speed of 200 rpm, adsorbent dosage of 60 g/L, contact time of 3 hours, and initial solution pH of approximately 2. The initial AG dye concentrations were varied from 100 ppm to 2000 ppm. After 3 hours of experimental contact time, the samples were filtered and the residual solutions were analysed using the UVVis spectrophotometer at 624 nm of .
The solution pH effect study was performed for initial AG dye concentration of 1000 ppm at operating temperature of 25°C with agitation speed of 200 rpm, adsorbent dosage of 60 g/L, and total experimental contact time of 3 hours. The initial solution pH was varied between 2 and 12. After 3 hours of experimental contact time, the samples were filtered and the residual solutions were analysed using UVVis spectrophotometer (Thermo Scientific, model Evolution 201) at 624 nm of .
Each batch experiment was carried out in duplicate and the average value was tabulated in graph form. The percentage removal was calculated using the following formula:where is the initial concentration and is the concentration at time interval.
The adsorption capacity, , was calculated using where is the initial concentration, is the concentration at time interval, is the volume of solution used, and is the mass of sorbent.
2.4. Characterisation of the Sorbents
The sorbents were characterised using scanning electron microscopy (SEM) (JEOL Analytical Scanning Microscope, model JSM6390LA) to visualise the surface morphologies of the sorbents and Fourier Transform Infrared (FTIR) to analyse the surface functional groups of the sorbents. The FTIR spectra were recorded using Shimadzu ASC 7000 Autosampler in the range of 400–4000 cm^{−1} with a resolution of 4 cm^{−1}.
3. Results and Discussion
3.1. Kinetic Batch Experiments
The interaction between sorbent and sorbate is generally seen in the contact time needed to remove the sorbate from water. The adsorption capacities of the three banana sorbents at different contact time were illustrated in Figure 1. In general, the adsorption capacity increases rapidly in the first 15 minutes and then increases gradually when nearing the equilibrium stage before becoming near constant at equilibrium. The rapid increase in adsorption at the initial stage is due to the availability of sorption sites. As the sorption sites are filled, the sorption becomes slower and causes the smaller increase in adsorption capacity. At equilibrium, the sorption sites are fully occupied with sorbate or there is nearly no sorbate to interact with. At different initial concentrations, the adsorption capacity is seen to increase with the increase in initial concentration. This can be attributed to the higher concentration difference, which can provide stronger driving force. For banana leaves sorbent, the adsorption capacities at 750, 1000, and 1500 ppm are 9.48, 11.01, and 18.40 mg/g, respectively. Lower adsorption capacities are found for banana stem sorbent (8.03, 10.54, and 17.02 mg/g) and banana stalk sorbent (7.28, 10.39, and 15.33 mg/g). Furthermore, at higher initial concentrations, longer contact time is needed to achieve equilibrium as there are higher amount of sorbates. At 1500 ppm for banana leaves, the equilibrium is achieved after 90 minutes, whereas the equilibrium is achieved after 25 minutes at 1000 ppm. Similar trend is exhibited with banana stem and banana stalk sorbents. At higher initial concentrations, there are more sorbate molecules to be sorbed. Therefore, longer time is needed to achieve the equilibrium state. Nevertheless, the sorption will be constant after equilibrium, indicating the saturation of sorption sites even with higher amount of sorbates. The equilibrium time for acid green dye was also found to be under 90 minutes using the Fenton method [5] and photodegradation with cobalt impregnated ZSM5 catalyst [14].
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3.2. The Effect of pH
Figure 2 shows the AG dye adsorption is greatly influenced by the acidic nature of solution. At highly acidic condition, with initial solution pH at approximately 2, the banana leaves, stem, and stalk sorbents produce the highest adsorption capacity of 28.7 mg/g, 18.5 mg/g, and 18.3 mg/g, respectively. For banana leaves and stalk sorbents, the adsorption capacity decreases to a constant value over a large range of initial solution pH (3 to 11). It can be seen in Figure 3 that, for these two sorbents, the final solution pH is equilibrated at around 6 for initial pH between 3 and 11, which explains why the adsorption capacity values became constant. For banana stem sorbent, the adsorption capacity is steadily decreasing as the solution pH increased. This could be due to the higher buffering value for this sorbent, which is at solution pH of 8 and 10. As this solution pH is basic, it gives a negative effect to the AG dye adsorption using the banana stem sorbent. The solution pH influences the interaction between the surface of the sorbent and the adsorbate [15, 16]. The AG dye is an anionic dye, and highly positive surface charge at initial solution pH 2 attracts the negative functional group in the AG dye.
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3.3. Adsorption Kinetics
The data from the kinetic experiments was further analysed and fitted to kinetic model equations. The best fit model was selected based on correlation of coefficients, where higher correlation gives the best fit model to the kinetic data. Several kinetic models were used to model the rate of adsorption of AG dye on banana leaves, stem, and stalk sorbents.
The pseudofirstorder kinetic equation describes adsorption rate based on adsorption capacities, where it assumes that one adsorbate molecule is adsorbed onto one active site [16]. The linear pseudofirstorder equation is given as where and are the adsorption capacity of sorbent (mg/g) at equilibrium and time , respectively. The pseudofirstorder rate constants (min^{−1}) are determined from the slope of this equation.
Meanwhile, the pseudosecondorder equation is also used to describe adsorption rate based on adsorption capacities [17]. In this equation, one adsorbate molecule is assumed to be held onto two active sites. The linear form of this equation is given bywhere and are the adsorption capacity of sorbent (mg/g) at equilibrium and time , respectively. The pseudosecondorder rate constants, (g/mg·min), are determined based on the slope of the equation.
The intraparticle diffusion model is used to explain the kinetics when pore diffusion is controlling the adsorption process. A common equation used to describe intraparticle diffusion is the DunwaldWagner equation:
The intraparticle diffusion equation will be crossing the origin if it is the only step that control the rate of adsorption [18, 19]. The parameters involved in the kinetic equations and the regression coefficients () are given in Table 1.

The kinetics data fitted very well into the pseudosecondorder model, with the correlation coefficient, , of more than 0.94 for all three sorbents. This indicates that sorption of AG dye on banana stem, stalk, and leaves sorbents may be controlled by chemisorption, through sharing of valence forces or ion exchange. The pseudofirstorder kinetic equation has lower values than pseudosecondorder one, although the correlation is still considered good with . The pseudofirstorder plots in Figure 4 show the nonlinearity of sorption using the three sorbents at 750 and 1000 ppm. Moreover, calculated adsorption capacities using pseudofirstorder equation are not satisfactory in representing the experimental data compared to pseudosecondorder equation. Based on the pseudosecondorder plots in Figure 5, the experimental data conforms to the linear form of the equation well. The pseudosecondorder kinetics fits well with most systems of dye adsorption using natural fibers, such as adsorption of methylene blue and direct red using garlic straw [20, 21], adsorption of crystal violet dye using sugarcane bagasse [11], removal of tartrazine using Lantana camara [22], crystal violet dye removal using papaya seed [23], and adsorption of navy blue using powdered orange [24]. Comprehensive review on pseudosecondorder model has demonstrated that this model is clearly advantageous in predicting adsorption of pollutants in aqueous solution, as there is no need to know the equilibrium capacity from the experiment, as it can be calculated from the model [25]. The intraparticle diffusion model has similar correlation coefficient values with pseudofirstorder model, with . Based on Figure 6, the linear line for the equation does not cross the origin, indicating that the intraparticle diffusion is not the primary ratecontrolling step.
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3.4. Adsorption Isotherm
Four isotherm equations were chosen to represent the adsorption of AG dye onto banana stem, stalk, and leaves sorbents. The isotherm experiments data were fitted with four isotherm equations, namely, Langmuir, Freundlich, DubininRadushkevich, and Temkin.
The assumptions of Langmuir isotherm were homogeneous adsorption sites, where a single layer of adsorption occurs [26, 27]. Since the adsorption occurs in a monolayer, there are no further adsorption once the active site is occupied. The linear form of this model is written aswhere is the equilibrium concentration (mg/L), is the equilibrium adsorption capacity (mg/g), is the maximum adsorption capacity (mg/g), and is the Langmuir isotherm constant (L/mg). An important dimensionless constant that can be extracted from Langmuir isotherm is called the separation factor, . is a dimensionless constant that indicates whether the adsorption is favourable (), unfavourable (), linear (), or irreversible (). can be expressed as
On the other hand, the Freundlich isotherm model was more commonly applied to explain adsorption that occurs in multiple layers, and there is interaction between adsorbed molecules [2, 27]. Unlike the Langmuir model, the adsorption sites in Freundlich model were heterogeneous, with the adsorption energy that declines exponentially as it nears the adsorption centers. The values indicate the degree of linearity of adsorption. When value is between 0 and 1, there exists some nonlinearity in the relationship between the solution concentration and adsorption. When value is 1, the adsorption is linear. The linear form of Freundlich isotherm is given aswhere is the equilibrium concentration (mg/L), is the equilibrium adsorption capacity (mg/g), is the Freundlich isotherm constant ( L^{1/n} g^{−1}), and is the adsorption intensity.
In order to calculate the apparent free energy of adsorption, the DubininRadushkevich model can be used [27, 28]. The DubininRadushkevich model is given by this linear equation:where is the equilibrium adsorption capacity (mg/g), is the saturation adsorption capacity (mg/g), is DubininRadushkevich isotherm constant related to adsorption energy (mol^{2}/kJ^{2}), and is the Polanyi potential, which is defined aswhere is the universal gas constant (8.314 J/mol·K) and is the temperature in Kelvin.
Where the Freundlich isotherm assumes that the adsorption energy declines exponentially, the Temkin isotherm assumes that the heat of sorption declines linearly with temperature [27, 28] on the basis that the binding energies are uniformly distributed. The linear form of Temkin model is given aswhere is the equilibrium concentration (mg/L), is the equilibrium adsorption capacity (mg/g), is the universal gas constant (8.314 J/mol·K), is the temperature in Kelvin, is the Temkin isotherm equilibrium binding constant (L/mg), and is defined aswhere is the Temkin isotherm constant.
The parameters associated with adsorption isotherm models above are given in Table 2. For all three sorbents, the Freundlich isotherm model is the best fitting isotherm, with of 0.8934 for banana leaves sorbent, 0.9792 for banana stem sorbent, and 0.9079 for banana stalk sorbent. This points to multilayer adsorption with interaction between adsorbed AG dye molecules. The isotherm is in line with kinetics, where the tendency for pseudosecondorder model indicates the interaction of one dye molecule to two adsorption sites. The three sorbents performed the worst for Langmuir isotherm model, with of less than 0.68. Nonetheless, the separation factor calculated using this model is between 0 and 1 for all three sorbents, showing that the adsorption is favourable under the conditions used. The maximum adsorption capacities calculated using Langmuir model are 79.36 mg/g for banana leaves sorbent, 157.73 mg/g for banana stem sorbent, and 48.08 mg/g using banana stalk sorbent. The DubininRadushkevich isotherm fits satisfactorily for banana leaves and banana stem sorbent, with of 0.8688 and 0.8692, respectively. Using this model, the apparent free adsorption energy for each sorbent is calculated. The banana leaves sorbent has the highest free energy of 11.71 J/mol, the banana stalk sorbent is the next with 10.56 J/mol, and the banana stem sorbent has the lowest energy at 4.58 J/mol. All these energy values are very low, indicating physisorption nature of adsorption, as it is lower than 8.0 kJ/mol [29]. The experimental and calculated adsorption capacities were presented in Figure 7. The calculated adsorption capacities were close to the experimental ones at lower than 100 mg/L. At higher equilibrium concentrations, the calculated adsorption capacities were closely represented by using Langmuir and Temkin isotherms for banana leaves and stalk sorbents and by using Freundlich for banana stem sorbents.

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3.5. Characterisation
The micrographs of SEM in Figure 8 show the surface morphologies of the sorbent after adsorption of the AG dye. The fibrillar structure in banana can be seen in the banana leaves, stem, and stalk sorbents, as has been reported in literature [30–32]. The stem and stalk sorbents are more homogeneous in structure, with smooth surface, compared to banana leaves sorbent. After the adsorption process, the AG dye molecules seem to cover part of the surface of the sorbents, as can be seen in Figures 8(a)–8(c) for the adsorption using 750 ppm of the AG dye and Figures 8(d)–8(f) for the adsorption using 1000 ppm of the AG dye. Similar morphologies were also found for the adsorption using 1500 ppm of the AG dye (not shown). The AG dye molecules were seen on the surface and inside the cavities of the sorbents.
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FTIR spectra after adsorption of the AG dye for the banana leaves, stem, and stalk sorbents are given in Figure 9. The surface functional groups found in the banana leaves, stem, and stalk sorbents are hydroxyl group at around 3400 cm^{−1}, CH_{2} symmetric stretching at around 2900 cm^{−1}, overlapping peaks between 1600 and 1250 cm^{−1} for CC, C=C, OH, CO, , and COC commonly found in polysaccharides, peak at around 1050 cm^{−1} for CO in alcohol group, and peaks between 550 and 430 cm^{−1} for deformations of CH groups in aromatic linkages, as described in our previous work [33]. The functional groups detected in AG dye (inset of Figure 9) are very similar to the ones in the sorbents used; thus, the FTIR of the banana leaves, stem, and stalk sorbents remain the same after the adsorption. As can be seen, the peaks for functional groups at 3400 cm^{−1}, 2900 cm^{−1}, 1600–1250 cm^{−1}, 1050 cm^{−1}, and 550 to 430 cm^{−1} are unshifted for all sorbents after the adsorption. Only the intensity of the hydroxyl group becomes less at concentration of 1500 ppm, though the peaks remain unshifted. This could indicate that the adsorption of these sorbents is more physical than chemical, as the functional groups are not strongly affected after adsorption took place.
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4. Conclusions
The batch kinetics study for AG dye using banana leaves, stem, and stalk sorbents showed that the adsorption capacity for removal of AG dye is between 8 and 18 mg/g across all three concentrations used. The adsorption capacity increases with the increase in initial concentration in the range of concentrations tested. Sorption capacities of AG dye on banana leaves, stem, and stalk sorbents are higher at very low pH (initial pH = 2), whereas at higher pH the sorption capacities do not vary much, due to the buffering effect.
The sorption of all three sorbents follows closely pseudosecondorder kinetics, suggesting chemisorption involved as ratecontrolling step. However, calculated mean free energy (using DubininRadushkevich model) showed that the adsorption produces energy of less than 12 J/mol, which is much lower than chemisorption energy of 8 kJ/mol. The intraparticle diffusion model shows good conformity to the data, but all linear lines do not pass through origin, indicating that this is not the sole ratelimiting step. The adsorption of AG dye using banana stalk, stem, and leaves sorbents was found to fit into the Freundlich isotherm, suggesting multilayer adsorption.
Competing Interests
The authors declare that there is no conflict of interests regarding the publication of this paper.
Acknowledgments
The authors would like to thank Universiti Malaysia Sarawak for the use of laboratory facilities and equipment.
References
 F. Ogata, D. Imai, and N. Kawasaki, “Cationic dye removal from aqueous solution by waste biomass produced from calcination treatment of rice bran,” Journal of Environmental Chemical Engineering, vol. 3, no. 3, pp. 1476–1485, 2015. View at: Publisher Site  Google Scholar
 M. N. Mahamad, M. A. A. Zaini, and Z. A. Zakaria, “Preparation and characterization of activated carbon from pineapple waste biomass for dye removal,” International Biodeterioration & Biodegradation, vol. 102, pp. 274–280, 2015. View at: Publisher Site  Google Scholar
 S. Wang, Y. Guan, L. Wang et al., “Fabrication of a novel bifunctional material of BiOI/Ag_{3}VO_{4} with high adsorption–photocatalysis for efficient treatment of dye wastewater,” Applied Catalysis B: Environmental, vol. 168169, pp. 448–457, 2015. View at: Publisher Site  Google Scholar
 A. Siddiqa, D. Masih, D. Anjum, and M. Siddiq, “Cobalt and sulfur codoped nanosize TiO_{2} for photodegradation of various dyes and phenol,” Journal of Environmental Sciences, vol. 37, pp. 100–109, 2015. View at: Publisher Site  Google Scholar
 R. J. Ramírez, C. A. P. Arellano, A. A. Á. Gallegos, A. E. J. González, and S. S. Martínez, “H_{2}O_{2}assisted TiO_{2} generation during the photoelectrocatalytic process to decompose the acid green textile dye by Fenton reaction,” Journal of Photochemistry and Photobiology A: Chemistry, vol. 305, pp. 51–59, 2015. View at: Publisher Site  Google Scholar
 N. A. Oladoja, “Headway on natural polymeric coagulants in water and wastewater treatment operations,” Journal of Water Process Engineering, vol. 6, pp. 174–192, 2015. View at: Publisher Site  Google Scholar
 M. R. S. Kebria, M. Jahanshahi, and A. Rahimpour, “SiO2 modified polyethyleneiminebased nanofiltration membranes for dye removal from aqueous and organic solutions,” Desalination, vol. 367, pp. 255–264, 2015. View at: Publisher Site  Google Scholar
 P. Sun, C. Hui, S. Wang, L. Wan, X. Zhang, and Y. Zhao, “Bacillus amyloliquefaciens biofilm as a novel biosorbent for the removal of crystal violet from solution,” Colloids and Surfaces B: Biointerfaces, vol. 139, pp. 164–170, 2016. View at: Publisher Site  Google Scholar
 A. Masoumi, K. Hemmati, and M. Ghaemy, “Lowcost nanoparticles sorbent from modified rice husk and a copolymer for efficient removal of Pb(II) and crystal violet from water,” Chemosphere, vol. 146, pp. 253–262, 2016. View at: Publisher Site  Google Scholar
 T. Sarat Chandra, S. N. Mudliar, S. Vidyashankar et al., “Defatted algal biomass as a nonconventional lowcost adsorbent: surface characterization and methylene blue adsorption characteristics,” Bioresource Technology, vol. 184, pp. 395–404, 2015. View at: Publisher Site  Google Scholar
 B. C. S. Ferreira, F. S. Teodoro, A. B. Mageste, L. F. Gil, R. P. de Freitas, and L. V. A. Gurgel, “Application of a new carboxylatefunctionalized sugarcane bagasse for adsorptive removal of crystal violet from aqueous solution: kinetic, equilibrium and thermodynamic studies,” Industrial Crops and Products, vol. 65, no. 1, pp. 521–534, 2015. View at: Publisher Site  Google Scholar
 A. Bhatnagar, M. Sillanpää, and A. WitekKrowiak, “Agricultural waste peels as versatile biomass for water purification—a review,” Chemical Engineering Journal, vol. 270, pp. 244–271, 2015. View at: Publisher Site  Google Scholar
 V. Nair and R. Vinu, “Peroxideassisted microwave activation of pyrolysis char for adsorption of dyes from wastewater,” Bioresource Technology, vol. 216, pp. 511–519, 2016. View at: Publisher Site  Google Scholar
 Z. M. ElBahy, M. M. Mohamed, F. I. Zidan, and M. S. Thabet, “Photodegradation of acid green dye over CoZSM5 catalysts prepared by incipient wetness impregnation technique,” Journal of Hazardous Materials, vol. 153, no. 12, pp. 364–371, 2008. View at: Publisher Site  Google Scholar
 J. Zolgharnein, M. Bagtash, and T. Shariatmanesh, “Simultaneous removal of binary mixture of Brilliant Green and Crystal Violet using derivative spectrophotometric determination, multivariate optimization and adsorption characterization of dyes on surfactant modified nanoγalumina,” Spectrochimica Acta Part A: Molecular and Biomolecular Spectroscopy, vol. 137, pp. 1016–1028, 2015. View at: Publisher Site  Google Scholar
 T. A. Khan, E. A. Khan, and Shahjahan, “Removal of basic dyes from aqueous solution by adsorption onto binary ironmanganese oxide coated kaolinite: nonlinear isotherm and kinetics modeling,” Applied Clay Science, vol. 107, pp. 70–77, 2015. View at: Publisher Site  Google Scholar
 Y. S. Ho and G. McKay, “Pseudosecond order model for sorption processes,” Process Biochemistry, vol. 34, no. 5, pp. 451–465, 1999. View at: Publisher Site  Google Scholar
 H. Qiu, L. Lv, B.C. Pan, Q.J. Zhang, W.M. Zhang, and Q.X. Zhang, “Critical review in adsorption kinetic models,” Journal of Zhejiang University: Science A, vol. 10, no. 5, pp. 716–724, 2009. View at: Publisher Site  Google Scholar
 S.F. Lim and A. Y. W. Lee, “Kinetic study on removal of heavy metal ions from aqueous solution by using soil,” Environmental Science and Pollution Research, vol. 22, no. 13, pp. 10144–10158, 2015. View at: Publisher Site  Google Scholar
 F. Kallel, F. Chaari, F. Bouaziz, F. Bettaieb, R. Ghorbel, and S. E. Chaabouni, “Sorption and desorption characteristics for the removal of a toxic dye, methylene blue from aqueous solution by a low cost agricultural byproduct,” Journal of Molecular Liquids, vol. 219, pp. 279–288, 2016. View at: Google Scholar
 F. Kallel, F. Bouaziz, F. Chaari, L. Belghith, R. Ghorbel, and S. E. Chaabouni, “Interactive effect of garlic straw on the sorption and desorption of Direct Red 80 from aqueous solution,” Process Safety and Environmental Protection, vol. 102, pp. 30–43, 2016. View at: Google Scholar
 R. K. Gautam, P. K. Gautam, S. Banerjee et al., “Removal of tartrazine by activated carbon biosorbents of Lantana camara: kinetics, equilibrium modeling and spectroscopic analysis,” Journal of Environmental Chemical Engineering, vol. 3, no. 1, pp. 79–88, 2015. View at: Publisher Site  Google Scholar
 F. A. Pavan, E. S. Camacho, E. C. Lima, G. L. Dotto, V. T. A. Branco, and S. L. P. Dias, “Formosa papaya seed powder (FPSP): preparation, characterization and application as an alternative adsorbent for the removal of crystal violet from aqueous phase,” Journal of Environmental Chemical Engineering, vol. 2, no. 1, pp. 230–238, 2014. View at: Publisher Site  Google Scholar
 S. Irem, Q. Mahmood Khan, E. Islam et al., “Enhanced removal of reactive navy blue dye using powdered orange waste,” Ecological Engineering, vol. 58, pp. 399–405, 2013. View at: Publisher Site  Google Scholar
 Y.S. Ho, “Review of secondorder models for adsorption systems,” Journal of Hazardous Materials, vol. 136, no. 3, pp. 681–689, 2006. View at: Publisher Site  Google Scholar
 T. S. Anirudhan and M. Ramachandran, “Adsorptive removal of basic dyes from aqueous solutions by surfactant modified bentonite clay (organoclay): kinetic and competitive adsorption isotherm,” Process Safety and Environmental Protection, vol. 95, pp. 215–225, 2015. View at: Publisher Site  Google Scholar
 S. Rangabhashiyam, N. Anu, M. S. Giri Nandagopal, and N. Selvaraju, “Relevance of isotherm models in biosorption of pollutants by agricultural byproducts,” Journal of Environmental Chemical Engineering, vol. 2, no. 1, pp. 398–414, 2014. View at: Publisher Site  Google Scholar
 A. O. Dada, A. P. Olalekan, A. M. Olatunya, and O. Dada, “Langmuir, freundlich, temkin and dubinin–radushkevich isotherms studies of equilibrium sorption of Zn^{2+} unto phosphoric acid modified rice husk,” IOSR Journal of Applied Chemistry, vol. 3, no. 1, pp. 38–45, 2012. View at: Publisher Site  Google Scholar
 P. C. N. Ejikeme, E. M. Ejikeme, and G. N. Okonkwo, “Equilibrium, kinetic and thermodynamic studies on basic dye adsorption using composite activated carbon,” International Journal of Technical Research and Applications, vol. 2, pp. 96–103, 2014. View at: Google Scholar
 H. Becker, R. F. Matos, J. A. D. Souza, D. D. A. Lima, F. T. C. D. Souza, and E. Longhinotti, “Pseudostem banana fibers: characterization and chromium removal,” Orbital, vol. 5, no. 3, 2013. View at: Google Scholar
 S. S. Pillai, B. Deepa, E. Abraham et al., “Biosorption of Cd(II) from aqueous solution using xanthated nano banana cellulose: equilibrium and kinetic studies,” Ecotoxicology and Environmental Safety, vol. 98, pp. 352–360, 2013. View at: Publisher Site  Google Scholar
 R. R. Mohammed and M. F. Chong, “Treatment and decolorization of biologically treated Palm Oil Mill Effluent (POME) using banana peel as novel biosorbent,” Journal of Environmental Management, vol. 132, pp. 237–249, 2014. View at: Publisher Site  Google Scholar
 S. K. A. Karim and S.F. Lim, “Removal of lead(II) ions in water using banana fiber,” Australian Journal of Basic and Applied Sciences, vol. 9, pp. 62–66, 2015. View at: Google Scholar
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Copyright © 2016 Siti Kartina Abdul Karim et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.