Next Article in Journal
Organic Cotton Clothing Purchase Behavior: A Comparative Study of Consumers in the United States and Bangladesh
Previous Article in Journal
An Overview on Methods for Producing Side-Emitting Polymer Optical Fibers

Adsorption Characteristics of Banana Peel in the Removal of Dyes from Textile Effluent

Department of Environmental Management, Independent University-Bangladesh, Dhaka 1229, Bangladesh
Department of Chemical Engineering, University of South Carolina, Columbia, SC 29208, USA
Wilson College of Textiles, North Carolina State University, Raleigh, NC 27695, USA
Department of Textile Engineering, National Institute of Textile Engineering and Research, Savar, Dhaka 1350, Bangladesh
Authors to whom correspondence should be addressed.
These authors have contributed equally.
Academic Editor: Marta Gmurek
Textiles 2021, 1(2), 361-375;
Received: 29 May 2021 / Revised: 6 September 2021 / Accepted: 7 September 2021 / Published: 10 September 2021
(This article belongs to the Special Issue Advances in Textile Dyeing and Finishing)


Disposal of reactive dye contaminants in surface waters causes serious health risks to the aquatic living bodies and populations adjacent to the polluted water sources. This study investigated the applicability of banana peels to remediate water contamination with reactive dyes used in the textile industry. A set of batch experiments was conducted using a standard dye solution to determine optimum adsorption parameters, and these parameters were used for the removal of dyes from actual wastewater. Fitting experimental data into the isotherm and kinetic models suggested monolayer dye adsorption with chemisorption rate-limiting step. The maximum adsorption found from modeling results was 28.8 mg/g. Fourier transformed infrared (FTIR) spectra revealed the existence of hydroxyl, amine and carboxylic groups, contributing to high adsorption of dye molecules onto the adsorbent surface. About 93% of the dyes from the standard solution were removed at optimum conditions (pH—7.0, initial dye concentration—100 mg/L, contact time—60 min, and adsorbent dose—0.5 g) while this value was 84.2% for industrial textile wastewater. This difference was mainly attributed to the composition difference between the solutions. However, the removal efficiency for actual wastewater is still significant, indicating the high potentiality of banana peel removing dyes from textile effluent. Furthermore, desorption studies showed about 95% of banana peel can be recovered with simple acid-base treatment.
Keywords: adsorption kinetics; banana peel; dye removal; isotherms; textile wastewater adsorption kinetics; banana peel; dye removal; isotherms; textile wastewater

1. Introduction

In the current scenario of rising populations and increasing industrial activities, water pollution causes significant destruction in the ecosystem and creates a potential threat to water security as only about 0.03% of global water resources are currently used for human activities. Direct disposal of untreated or inadequately treated industrial effluent into different water sources has been identified as the primary cause of present water pollution [1,2,3]. Textile dyeing, for instance, is pinpointed as one of the most polluting sectors that releases about 5000~10,000 tons of different reactive dyes each year, contributing about 17–20% of industrial water pollution [3,4,5]. Most of these dyes limit the access of sunlight into the water, causing serious health risks to the aquatic living bodies and populations adjacent to the polluted water sources, thus highlighting the need for proper treatment of textile effluents that protects both the ecosystem and the environment [3,6].
Adsorption is the most common and well-developed technique compared to conventional methods employed for dye removal from textile wastewater due to its ease in process design and operation, low-cost, and high efficiency, even for highly concentrated dye solutions [7,8]. Moreover, the easy availability and biodegradability of adsorbent materials are an extra feature of the adsorption method in removing dyes from the wastewater [9]. Activated carbons and numerous organic resins have achieved amazing success as adsorbents in dye removal, however, the excessive cost of these materials impedes the widespread implementation of adsorption processes, driving researchers to seek alternative adsorbents that can provide the desired level of performance [10]. Recent studies have shown significant improvements in the cost-effectiveness of the adsorption process through the effective substitution of the standard materials by relatively low-cost and environmentally-friendly biowaste-derived adsorbents [10,11,12,13]. Previous studies have also reported that these bio-adsorbents display excellent performance in the removal of dyes [14] and heavy metals [15] from textile manufacturing effluents. These findings have inspired the development of cost-effective, environmentally sound, and efficient adsorbents to remove hazardous dyes from textile wastewater.
Banana peel has attracted attention among all other adsorbents because of its year-round availability throughout the world. The existence of different functional groups in banana peel allows the high sorption of different anionic and cationic compounds onto the surface-active sites [16]. However, most of the available banana peel is underutilized and trashed as bio-waste despite its high potential to remove heavy metals [17], pharmaceutical compounds [18], radioactive elements [19], phenolic compounds [20], etc. as disclosed in many recent research works. Although the adsorption of the dyes onto banana peel was previously studied [21,22,23,24,25,26,27], the potential of banana peel in treating actual textile wastewater has yet to be reported. Most of the current research has highlighted the applicability of banana peel for removal of a specific dye from a standard solution, but no effort is found in literature to the best of the authors’ knowledge that was extended for the removal of different dyes from industrial wastewater. The optimum adsorption parameters determined using a mixture of dye solutions has been applied to remove dyes from textile effluent containing the same dyes. In addition to that, numerous adsorbents derived from banana peel also showed improved dye removal efficiency but have not still been employed in commercial applications due to economic reasons [28]. Therefore, the proper investigation of the use of natural banana peel for efficient water decontamination in the industrial scale is in demand.
Reactive dyes are some of the most utilized dyes for cotton coloration, and the industrial discharge of reactive dyes is increasing enormously. This work utilized natural banana peel as bio-adsorbent to remove reactive dyes from textile effluent through a set of batch adsorption processes. The adsorption performances of banana peel were tested for variable solution pH, adsorbent dose, initial dye concentration, and contact time, followed by FTIR characterization of the banana peel. The initial investigations were done for a standard solution to determine the optimum adsorption parameters, which were later employed in actual wastewater treatment. The experimental adsorption data were precisely fitted with isotherm and kinetic models to demonstrate the adsorption behavior of banana peel for the removal of the dyes from textile wastewater.

2. Materials and Methods

2.1. Chemicals and Materials

The banana peel was collected from a local fruit market. The wastewater and the powder of three reactive dyes, which are commercially known as Deazol Black B EAN, Deafiz Red ME 6BL, and Firstfix Yellow 3RS were collected from a well-known textile dyeing unit located in Gazipur, Bangladesh. As the company only disclosed the commercial names of these dyes, the exact chemical structures were unknown in this study. However, the chemical structure of some of other commercially available dyes with similar generic groups are shown in Figure 1. Hydrochloric acid (HCl) and sodium hydroxide (NaOH), both supplied by Merck (Darmstadt, Germany), were used without further purification to adjust the pH of the solutions.

2.2. Adsorbent Preparation

The banana peels were subsequently sliced into small fragments, washed, dried, crushed, and sieved before using for the adsorption treatment. The peels were washed with deionized water (DI-water) to eliminate adhering dirt particles and dried in ambient conditions for 48 h followed by drying at 80 °C for 8 h in a 3606-1CE vacuum oven. The dried peels were grounded in HR2118 blender (Phillips, Toa Payoh, Singapore) sieved using 100 mesh size (149 µm) and stored in an airtight polythene container.

2.3. Chemical Analysis

A DR/4000U UV-vis spectrophotometer (HACH, Loveland, CO, USA) was used to estimate the dye concentration in the solutions. The pH of the solutions was measured using a Hach-Sension-MM156 instrument, a portable multiparameter meter equipped with a calibrated pH glass electrode. A LMS-1003 magnetic stirrer (LabTech, Hopkinton, MA, USA) was used to maintain the homogeneity of dyes in the solutions. The coexisting functional groups in banana peel were identified by a IR Tracer-100 FTIR system (Shimadzu, Tokyo, Japan) equipped with a high sensitivity mercury-cadmium-telluride (MCT) detector. The equipment was integrated with the LabSolutions IR software for peak analysis. Before recording FTIR spectra, the samples were uniformly mixed with potassium bromide (KBr) with a weight ratio of 1:100 (adsorbent: KBr). The spectra were recorded for the wavenumbers ranged from 4000 to 400 cm−1.

2.4. Standard Solution and Calibration Curve

A standard solution, in which the concentrations of its constituent elements are precisely known, was used to determine the optimum adsorption parameters (pH, adsorption time, initial dye concentration, banana peel dosages, etc.) for textile wastewater treatment. The solution was prepared by dissolving an equal amount of three dyes (mentioned above) in DI-water. It was hypothesized that an equal amount of these three dyes remained in actual textile effluent. The stock solution (standard solution) was yielded by adding 1 g of each dye in a volumetric flask containing 2 L of DI-water. Afterward, the stock solution was stirred in a magnetic stirrer for 60 min with a rotational speed (S) of 180 rpm to obtain homogeneous dye composition.
The absorbance of the standard solution was calibrated against solution concentrations using a wavelength at which maximum adsorption occurred (λmax). The absorbance of the collected wastewater was plotted as a function of wavelengths, which provided the λmax value at 601 nm (Figure 2a). All further spectrophotometric measurements in this study used this λmax value. To perform the calibration study, the stock solution was further diluted to a set of concentrations ranging from 25 to 225 mg/L with pH ~ 7. The absorbance of each solution was measured at room temperature (T ~ 25 °C) and plotted against the concentrations (Figure 2b). The experimental data were precisely fit in a straight line with a linear regression coefficient (R2) of 0.9996, thus allowing to assume a constant molar absorbability throughout the concentration range.

2.5. Adsorption Study

The batch experiments were conducted to investigate the adsorption behavior of banana peel in the removal of dyes from textile effluent. Before employing banana peel to remove dyes from actual wastewater, all adsorption parameters were optimized using the standard solution (for details of the preparation of standard solution see Section 2.4). To find the optimum pH at which maximum adsorption occurred, three different amounts of adsorbent (0.5, 0.75, and 1.0 g) were added in amber bottles containing 250 mL of a dye solution (50 mg/L) at pH between 2.0 and 10.0. Then, the mixtures were agitated using a magnetic stirrer for an hour with a speed of 180 rpm at 25 °C followed by filtration using Whatman No. 1 filter paper. The filtrated solutions were immediately analyzed by the UV-Vis spectrophotometer to estimate the final concentration of the investigated solutions using the calibration curve. In determining the effects of adsorbent dose, different amounts of banana peel (Mads) ranging from 0.1 to 0.8 g were mixed in amber bottles having 250 mL of a dye solution (50 mg/L) at pH ~ 7. The same experimental procedure was followed for pH study.
To obtain equilibrium conditions, the adsorption experiments were performed using four levels of concentration (Ci = 25, 50, 100, and 150 mg/L) at optimum pH. An amount of 0.5 g banana peel was added into each 250 mL dye solution at 25 °C and stirred in the magnetic stirrer for two hours. The samples were taken for spectrophotometric analysis in specific time intervals (t = 0, 10, 20, 30, 45, 60, 90, and 120 min). Equilibrium attained when the concentration of the final solution remained the same with increasing adsorption time. The adsorption efficiency (% removal of dyes) and the adsorption capacity (amount adsorbed, q) were calculated using Equations (1) and (2), respectively [10]:
Removal   efficiency   ( % ) = C i   -   C f C i   ×   100
Adsorption   capacity ,   q   ( mg / g ) = ( C i   -   C f M a d s ) × V
where Ci and Cf denote the initial and final concentration (mg/L) of the dye solution respectively, V is the solution volume (L), and Mads is the weight of adsorbent used (g).

2.5.1. Adsorption Isotherms

The adsorption isotherm analysis provides an equilibrium relationship between adsorbate and adsorbent. The experimental adsorption data were fitted to Langmuir and Freundlich isotherms to obtain a suitable model to design a process for industrial wastewater treatment. The Langmuir isotherm model assumes monolayer adsorption of dyes at homogeneous adsorbent sites (identical and energetically indistinguishable) and that no transmigrations occur between adsorbed molecules on the neighboring sites. The linearized Langmuir isotherm model is expressed by Equation (3) [10]:
C e   q e = C e   q m + 1 K L q m
where qm, qe and KL denoted the maximum adsorption capacity (mg/g), adsorption capacity at equilibrium (mg/g) and Langmuir isotherm constant (L/mg), respectively. The values of qm and KL were estimated by plotting Ce/qe against Ce where qm is the reciprocal of the slope and KL calculated from the intercept. The favorability of dye adsorption onto the banana peel was studied by a dimensionless separation factor RL obtained from the Langmuir isotherm model, which can be expressed as follows [29]:
R L = 1 1 + K L C i
The isotherm model is favorable only when the value of RL remains in between 0 and 1, it is unfavorable, linear, or irreversible if RL > 1, RL = 1, and RL = 0, respectively.
On the other hand, the Freundlich isotherm model postulates multilayer adsorption on heterogeneous adsorbent sites, where adsorbed molecules actively interact with each other. Equation (5) represents the linearized Freundlich isotherm model [10]:
ln ( q e ) = ln ( K F ) + 1 n F l n ( C e )
where 1/nF and KF represent the heterogeneity factor associated with adsorption capacity, and the Freundlich isotherm constant (mg/g), respectively. Similar to the Langmuir isotherm, a linear line of ln(qe) as a function of ln(Ce) was plotted to estimate the value of KF (from the intercept) and nF (from the slope). The value of 1/nF typically ranges from 0 to 1, illustrating the non-linearity of the relationship between dye solution concentration and adsorption. If nF = 1, the adsorption is linear otherwise it implies chemical (1/nF < 1) or physical (1/nF > 1) adsorption [10]. 1/nF < 1 also suggests the favorability of dye adsorption onto the adsorption surface [29].

2.5.2. Adsorption Kinetics

The adsorption kinetics study was done to understand the equilibrium relationships between adsorption and contact time. The experimental adsorption data were precisely fitted into the pseudo-first-order (PFO) and pseudo-second-order (PSO) kinetic models. The linearized equations for PFO and PSO are represented by Equations (6) and (7), respectively. In general, the rate of adoption in PFO is directly proportional to the first power of solution concentration, while the rate is related to the square of solution concentration for PSO [3]:
ln ( q e q t ) = ln ( q e ) k 1 2.303 t
t q t = 1 k 2 q e 2 + 1 q e t
where t is time (min) and qt is adsorption capacity at instant time (mg/g). The rate constant for PFO and PSO adsorption was denoted by k1 and k2, respectively.

2.5.3. Desorption Study

The banana peel (0.5 mg/L) used for the adsorption of dye solution was separated using vacuum filtration. The exhausted adsorbent was treated individually or mutually under acidic and basic medium. Solutions 0.1 M HCl and 0.1 M NaOH were used to make acidic and basic environments, respectively. Prior to drying sample at 80 °C for 12 h, the adsorbent was washed with distilled water three times to remove residual acid or base solution from the adsorbent surface.

3. Results and Discussion

3.1. FTIR Characterization

The presence of important functional groups on the surface of banana peel was identified by the FTIR spectrum shown in Figure 3. The most intense and broadest peak at 3393.8 cm−1 indicates coinciding vibrations of O–H (hydroxyl) stretching of alcohols and phenols and N–H (amine) stretching of amino acid. Other strong peaks were also found in the range of 2850 to 3000 cm−1 that represent C–H stretching of alkanes [30]. Peaks appearing at 1736.9, 1620.2, and 1399.4 cm−1 are designated to C=O stretching of aldehydes or carboxylic acids, –COO symmetric stretching, and O–H bending, respectively. The bands at 1000–1350 cm−1 and 650–1000 cm−1 are attributed to C–O stretching of esters or ethers and N–H deformation of amines, and C–H stretching of alkenes and aromatics, respectively [24,30]. The FTIR spectra revealed that banana peel contained a high amount of hydroxyl and carboxylic groups, potentially from cellulose and amines from hemicellulose. These functional groups on adsorbent surface (–COOH, –NH2, –OH, etc.) participate on hydrogen bonding via an electrostatic attractive force between H-atoms in the functional groups of banana peel surface and more negatively charged atoms (e.g., N, O, etc.) on dye surface [23,31].

3.2. Effects of Solution pH

The pH is one of the most critical parameters primarily used to evaluate the adsorption capacity of banana peel to remove different reactive dyes from solution. The solution pH controls the adsorption capability as it has tremendous effects on the surface properties of the adsorbent and the forms (ionic or neutral) of dyes present in solution. A set of adsorption studies were performed in the pH range of 2–10 for 60 min at three different adsorption doses (0.5, 1.0, and 2.0 g/L) while the initial dye concentration was held at 50 mg/L. The uptake of dyes on the banana peel is exhibited against solution pH in Figure 4. The percent removal of dyes increases with increasing pH and it suddenly goes to the highest (93.4%, 97.1%, and 99.6% for the adsorbent dose of 0.5, 0.75, and 1.0 g, respectively) at pH ~ 7.0. However, the adsorption falls when the pH is further increased. Analogous results were also attained in adsorption of dyes onto the banana peel [32], orange peel [32,33,34], shrimp shell [35], and biological waste slurry [36].
The maximum adsorption at pH = 7.0 implies the presence of equal amounts of anions and cations in the dye solution which were simultaneously neutralized and adsorbed on the banana peel adsorption sites. Strong electrostatic interactions between charged molecules (e.g., Na+, Cl, SO3Na+, –COO, –O, etc.) in dye solution and different functional groups such as –COOH, –OH, –NH2, –SO4, etc in banana peel surface plays one of the major roles in the adsorption of dyes from the waste solution. The neutralization of dyes by H+ ions in acidic medium and OH ions in basic medium might limit the removal of dyes with opposite ions from the solution. Therefore, the rest of the studies in this work was performed for a solution of pH ~ 7.0.

3.3. Effects of Adsorbent Dose

The effects of adsorbent dosage on the removal of dyes are shown in Figure 5. About 20% of dyes were removed when 0.1 g banana peel was used, and almost complete removal (~94%) was observed for 0.5 g adsorbent. Little effect on the removal percentage is noticed for a further increase in the adsorbent dose (~96% removal for 0.8 g dosage). Such a trend is understandable as the number of active sites is increased for the high dosage of banana peel while the amount of adsorbate molecules in the solution remains constant. Conversely, a drop of adsorption capacity from 28.4 mg/g (at 0.2 g dosage) to 14.9 mg/g (at 0.8 g dosage) was observed after an initial increase. At dosages < 0.2 g, the active sites of banana peel may saturate quickly and this left a significant amount of dyes in the solution, leading to an increase in adsorption capacity with increased dosage (up to 0.2 g) [6]. Besides, the decrease in adsorption capacity at higher dosages may be attributed to two reasons. Firstly, the unsaturation of active adsorption sites of banana peel occurred at higher dosages, due to the presence of excess adsorbent than necessary while the adsorption capacity is inversely related to the amount of adsorbent dosage. Secondly, the aggregation of adsorbent particles due to the high addition of adsorbent dosage caused a significant drop in surface area and an increase in diffusional path length [37], leading to limiting the adsorption process.

3.4. Effects of Initial Concentration and Contact Time

The effects of initial dye concentration and contact time were simultaneously studied in this work. The dye removal efficiency and adsorption capacity are demonstrated as a function of time with four levels of dye concentration (Ci = 25, 50, 100, and 150 mg/L) in Figure 6a,b respectively. The analogous trends of percent dye removal in Figure 6a show that the first 10 min of adsorption was very quick which then proceeded slow down until a plateau state was reached. For all initial concentrations, the equilibrium was attained within 60 min of the adsorption process, except for 150 mg/L solution, which plateaued in about 90 min. The abundant availability of active adsorption sites at the initial stage causes high interactions between adsorbent and dyes, resulting in rapid adsorption. Decreasing active sites over time because of the adoption process leads to a gradual decrease in the rate of adsorption, which continues until the dynamic equilibrium between the adsorption and desorption of dyes is achieved. The slower adsorption at high concentration solutions was attributed to the presence of relatively lower number of active sites to remove the same amount of dyes as the solution volume and adsorbent quantity in the system remained constant. In addition to that, the existence of such inadequacy of active sites at higher concentration solutions also offered considerably lower dye removal efficiency. Only 43.4% of dyes were removed at Ci = 150 mg/L while the removal efficiencies were 56%, 96.2%, and 100% for 100, 50, and 25 mg/L solution, respectively. Similar results were also obtained by Arami et al. [9].
Conversely, the adsorption capacity of banana peel was higher for the dye-rich solutions (i.e., 33.5 mg/g at 150 mg/L and 12.5 mg/g at 25 mg/L) as the number of dye molecules in the constant volume and adsorbent mass is increased at high dye concentration solution, resulting in high quantity dye adsorption. However, the trend of adsorption capacities of banana peel in Figure 6b always corresponded to the trend of dye removal efficiency shown in Figure 6a.

3.5. Adsorption Isotherms

Adsorption isotherm studies were conducted in the concentration range 25–200 mg/L under the following conditions: 0.5 g banana peel, pH ~ 7, and 25 °C. The adsorbate-adsorbent mixing was done in the magnetic stirrer for 1 h with a rotational speed of 180 rpm. The same procedure as the adsorption study (Section 2.5) was used to obtain equilibrium concentrations, percent dye removal, and the amount of dye adsorbed. Fitting experimental data to isotherm equations (Equations (3) and (5)) suggest that the Langmuir isotherm model (Figure 7a) shows a relatively better fit to the adsorption data, which revealed by higher R2 value compared to the Freundlich model (Figure 7b). The adsorption parameters with corresponding R2 value for both isotherm model are summarized in Table 1.
The better fitting of experimental data to the Langmuir isotherm model indicates the occurrence of monolayer adsorption at specific homogeneous adsorption sites of the banana peel. The lower R2 value in the Freundlich model was obtained owing to the non-linear adsorption behavior (1/nF ~ 0.114 < 1), especially at high concentrations, which is caused by saturation of adsorbent actives sites on the surface.
To describe the favorability of dye adsorption onto the banana peel by the Langmuir isotherm model, RL was plotted as a function of Ci, which is shown in Figure 8. The highest value of RL (0.133) was obtained at 25 mg/L that decreased to 0.02 at 200 mg/L. However, the values of RL were always found in the range of 0.02–0.14 (<<1), indicating the favorable dye adsorption on a banana peel. Like the Langmuir isotherm model, the Freundlich isotherm model also shows the favorable dye adsorption, which was confirmed by obtaining the value of 1/nF less than unity (Table 1).

3.6. Adsorption Kinetics

In kinetic studies, the adsorption capacity of banana peel at equilibrium was examined for times ranging from 0 to 120 min using three dye concentration levels (25, 50, and 100 mg/L) under the following conditions: 0.5 g banana peel, pH ~ 7, and 25 °C and maintained identical procedure as adsorption study (Section 2.5) to attain equilibrium concentration and adsorption capacity. The adsorption kinetic at different dye concentrations were evaluated by fitting experimental adsorption data into the linearized PFO and PSO model equations, which are shown in Figure 9. The higher R2 value in Figure 9 reveals a better fit of experimental data to the PSO compared to PFO, suggesting a chemisorption-controlled adsorption process [3,38], which is also validated by isotherm studies (reported in Section 3.5) since 1/nF is less than unity. The rate constant (k1 and k2) and theoretical adsorption capacity at equilibrium (qe,calc) along with the R2 values for both kinetic models are listed in Table 2.

3.7. Adsorption Study on Textile Wastewater

The optimized parameters, including solution pH, adsorbent dose, and contact time, found for the standard solution were implemented to treat actual collected textile wastewater. Since the concentration was unknown, the wastewater was diluted until an initial absorbance of about 0.612, which corresponds to 56 mg/L (obtained using calibration curve). A mixture of 0.5 g banana peel and 250 mL wastewater (56 mg/L) was stirred on a magnetic stirrer at pH ~ 7 for an hour with S = 180 rpm. The final concentration found after the adsorption was 8.2 mg/L (absorbance = 0.088), indicating 84.2% of dye removal that is about 9% lower from the value obtained for the standard solution of 50 mg/L. This slightly lower adsorption capacity in dye removal from wastewater may occur due to (1) a small increase in initial dye concentration as the percent dye removal decreases with initial dye concentration (2) the difference of dye composition in wastewater and the standard solution, which can affect the calibration curve, and (3) the presence of dyeing auxiliaries (salts, alkalies, surfactants and softeners) in industrial wastewater (that was not accounted for in the experiments with standard dye solution) might have a negative impact on the adsorption capacity. The adsorption capacities of different forms of banana peel along with other bio-adsorbents to remove dyes have been summarized in Table 3.

3.8. Adsorbent Regeneration Study

Regeneration of adsorbent helps explain the mechanism and recovery of the adsorbate and adsorbent. Figure 10 illustrates the %desorption of dyes in different solvent media. Initially, 0.1 M HCl (A) and 0.1 M NaOH (B) solutions were used to desorb dyes from the adsorbent surface. In both cases, % recoveries were similar (51.2 ± 3.2% with HCl and 47.9 ± 4.6% with NaOH solution). However, when the adsorbent was treated subsequently with 0.1 M HCl and 0.1 M NaOH (C), the regeneration of adsorbent surface was about 94.5 ± 5.1% which was approximately double than seen with the individual acid or base treatments. As mentioned in the adsorption study, the dye solution contained the same amount of positive and negative functional groups and the maximum adsorption was obtained at pH = 7.0, which indicates that both basic and acidic media are required to create extreme conditions and eventually desorb dyes from the adsorbent surface. In acidic medium, the solution consists of a higher amount of H+ that subsequently attach with the dye molecules with negative functional groups and are desorbed from the adsorbent surface. Similarly, in basic medium, the dye molecules containing positive functional groups were removed. Therefore, when treated with acid and base one after another, a very high %recovery is achieved. Here, %recovery of this acid-base treatment is 4.6% less than the combination (99.1%) of individual acid and base treatments because of the neutralization reaction between residual HCl and NaOH solutions.

4. Conclusions

In summary, banana peel has shown tremendous adsorption capacity for the removal of dyes from textile effluents. Prior to treating actual wastewater, a set of parameters were optimized using the standard solution containing a mixture of three major dyes present in the wastewater. The FTIR study revealed that banana peel contained a high amount of hydroxyl, amine and carboxylic groups on the surface that cause high interactions between adsorbate and adsorbent, resulting in high dye removal efficiency and adsorption capacity. The optimum adsorption at pH ~ 7 indicates the presence of equal amounts of anions and cations in the wastewater solution. Although the adsorption capacity was further increased with adsorbent dose, it was minimal for adsorbent doses above 0.5 g. The equilibrium was reached within 60 min of adsorption; however, it was a little longer for solution concentration above 100 mg/L due to insufficient adsorption sites. A Langmuir isotherm model and a pseudo-second-order kinetic model fitted the experimental adsorption data well, which suggested that the dye removal using banana peel is a favorable chemisorption process. This study shows that low-cost and renewable biowaste-derived banana peel has high adsorption performance towards textile dyes. Additionally, about 95% of the banana peel is recoverable with subsequent acid and base treatments and can can be re-used for further dye adsorption.

Author Contributions

Conceptualization, M.Z.A., F.B.A.R. and M.A.; methodology, M.A.; software, F.B.A.R. and S.M.F.K.; validation, M.A., S.M.F.K. and M.Z.A.; formal analysis, F.B.A.R.; investigation, M.A. and F.B.A.R.; resources, M.A.; data curation, S.M.F.K. and F.B.A.R.; writing—original draft preparation, M.A. and F.B.A.R.; writing—review and editing, F.B.A.R., M.A. and S.M.F.K.; visualization, F.B.A.R.; supervision, M.Z.A.; project administration, M.Z.A.; funding acquisition, M.Z.A. All authors have read and agreed to the published version of the manuscript.


This research received no external funding.

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

The data presented in this study are available within the manuscript.

Conflicts of Interest

The authors declare no conflict of interest.


  1. Leal, T.W.; Lourenco, L.A.; Scheibe, A.S.; de Souza, S.M.G.U.; de Souza, A.A.U. Textile wastewater treatment using low-cost adsorbent aiming the water reuse in dyeing process. J. Environ. Chem. Eng. 2018, 6, 2705–2712. [Google Scholar] [CrossRef]
  2. Nuithitikul, K.; Srikhun, S.; Hirunpraditkoon, S. Kinetics and equilibrium adsorption of Basic Green 4 dye on activated carbon derived from durian peel: Effects of pyrolysis and post-treatment conditions. J. Taiwan Inst. Chem. Eng. 2010, 41, 591–598. [Google Scholar] [CrossRef]
  3. Wong, S.; Abd Ghafar, N.; Ngadi, N.; Razmi, F.A.; Inuwa, I.M.; Mat, R.; Amin, N.A.S. Effective removal of anionic textile dyes using adsorbent synthesized from coffee waste. Sci. Rep. 2020, 10, 1–13. [Google Scholar] [CrossRef][Green Version]
  4. Pirkarami, A.; Olya, M.E. Removal of dye from industrial wastewater with an emphasis on improving economic efficiency and degradation mechanism. J. Saudi Chem. Soc. 2017, 21, S179–S186. [Google Scholar] [CrossRef][Green Version]
  5. Yagub, M.T.; Sen, T.K.; Afroze, S.; Ang, H.M. Dye and its removal from aqueous solution by adsorption: A review. Adv. Colloid Interface Sci. 2014, 209, 172–184. [Google Scholar] [CrossRef]
  6. Kabir, S.; Cueto, R.; Balamurugan, S.; Romeo, L.D.; Kuttruff, J.T.; Marx, B.D.; Negulescu, I.I. Removal of acid dyes from textile wastewaters using fish scales by absorption process. Clean Technol. 2019, 1, 311–324. [Google Scholar] [CrossRef][Green Version]
  7. Kabir, S. Waste Management by Waste: Removal of Acid Dyes from Wastewaters of Textile Coloration Using Fish Scales. Master’s Thesis, Louisiana State University, Baton Rouge, LA, USA, 2018. [Google Scholar]
  8. Naushad, M.; Ahamad, T.; Alothman, Z.A.; Ala’a, H. Green and eco-friendly nanocomposite for the removal of toxic Hg(II) metal ion from aqueous environment: Adsorption kinetics & isotherm modelling. J. Mol. Liq. 2019, 279, 1–8. [Google Scholar]
  9. Arami, M.; Limaee, N.Y.; Mahmoodi, N.M.; Tabrizi, N.S. Removal of dyes from colored textile wastewater by orange peel adsorbent: Equilibrium and kinetic studies. J. Colloid Interface Sci. 2005, 288, 371–376. [Google Scholar] [CrossRef]
  10. Gimbert, F.; Morin-Crini, N.; Renault, F.; Badot, P.-M.; Crini, G. Adsorption isotherm models for dye removal by cationized starch-based material in a single component system: Error analysis. J. Hazard. Mater. 2008, 157, 34–46. [Google Scholar] [CrossRef] [PubMed]
  11. Wong, S.; Lim, Y.; Ngadi, N.; Mat, R.; Hassan, O.; Inuwa, I.M.; Mohamed, N.B.; Low, J.H. Removal of acetaminophen by activated carbon synthesized from spent tea leaves: Equilibrium, kinetics and thermodynamics studies. Powder Technol. 2018, 338, 878–886. [Google Scholar] [CrossRef]
  12. Li, W.; Mu, B.; Yang, Y. Feasibility of industrial-scale treatment of dye wastewater via bio-adsorption technology. Bioresour. Technol. 2019, 277, 157–170. [Google Scholar] [CrossRef]
  13. Biswas, S.; Rashid, T.U.; Debnath, T.; Haque, P.; Rahman, M.M. Application of chitosan-clay biocomposite beads for removal of heavy metal and dye from industrial effluent. J. Compos. Sci. 2020, 4, 16. [Google Scholar] [CrossRef][Green Version]
  14. Kabir, S.; Rashid, T.U.; Negulescu, I.I. Gelation of textile dye solution treated with fish scales. Gels 2019, 5, 37. [Google Scholar] [CrossRef] [PubMed][Green Version]
  15. Naushad, M.; Mittal, A.; Rathore, M.; Gupta, V. Ion-exchange kinetic studies for Cd(II), Co(II), Cu(II), and Pb(II) metal ions over a composite cation exchanger. Desalination Water Treat. 2015, 54, 2883–2890. [Google Scholar] [CrossRef]
  16. Munagapati, V.S.; Wen, J.-C.; Pan, C.-L.; Gutha, Y.; Wen, J.-H.; Reddy, G.M. Adsorptive removal of anionic dye (Reactive Black 5) from aqueous solution using chemically modified banana peel powder: Kinetic, isotherm, thermodynamic, and reusability studies. Int. J. Phytoremediation 2020, 22, 267–278. [Google Scholar] [CrossRef]
  17. Vilardi, G.; Di Palma, L.; Verdone, N. Heavy metals adsorption by banana peels micro-powder: Equilibrium modeling by non-linear models. Chin. J. Chem. Eng. 2018, 26, 455–464. [Google Scholar] [CrossRef]
  18. Silva, C.R.; Gomes, T.F.; Andrade, G.C.; Monteiro, S.H.; Dias, A.C.; Zagatto, E.A.; Tornisielo, V.L. Banana peel as an adsorbent for removing atrazine and ametryne from waters. J. Agric. Food Chem. 2013, 61, 2358–2363. [Google Scholar] [CrossRef] [PubMed]
  19. Oyewo, O.A.; Onyango, M.S.; Wolkersdorfer, C. Application of banana peels nanosorbent for the removal of radioactive minerals from real mine water. J. Environ. Radioact. 2016, 164, 369–376. [Google Scholar] [CrossRef]
  20. Achak, M.; Hafidi, A.; Ouazzani, N.; Sayadi, S.; Mandi, L. Low cost biosorbent “banana peel” for the removal of phenolic compounds from olive mill wastewater: Kinetic and equilibrium studies. J. Hazard. Mater. 2009, 166, 117–125. [Google Scholar] [CrossRef] [PubMed]
  21. Kamar, F.H.; Niamat, F.E.; Faisal, A.A.; Mohammed, A.A.; Nechifor, A.C.; Nechifor, G. Use of artificial neural network for modeling and prediction of reactive red dye removal from wastewater using banana peels bio-sorbent. Rev. De Chim. 2018, 69, 1919–1926. [Google Scholar] [CrossRef]
  22. Mondal, N.K.; Kar, S. Potentiality of banana peel for removal of Congo red dye from aqueous solution: Isotherm, kinetics and thermodynamics studies. Appl. Water Sci. 2018, 8, 157. [Google Scholar] [CrossRef][Green Version]
  23. Oyekanmi, A.A.; Ahmad, A.; Hossain, K.; Rafatullah, M. Adsorption of Rhodamine B dye from aqueous solution onto acid treated banana peel: Response surface methodology, kinetics and isotherm studies. PLoS ONE 2019, 14, e0216878. [Google Scholar] [CrossRef]
  24. Memon, J.R.; Memon, S.Q.; Bhanger, M.; Memon, G.Z.; El-Turki, A.; Allen, G.C. Characterization of banana peel by scanning electron microscopy and FT-IR spectroscopy and its use for cadmium removal. Colloids Surf. B Biointerfaces 2008, 66, 260–265. [Google Scholar] [CrossRef]
  25. Munagapati, V.S.; Yarramuthi, V.; Kim, Y.; Lee, K.M.; Kim, D.-S. Removal of anionic dyes (Reactive Black 5 and Congo Red) from aqueous solutions using Banana Peel Powder as an adsorbent. Ecotoxicol. Environ. Saf. 2018, 148, 601–607. [Google Scholar] [CrossRef]
  26. Palma, C.; Contreras, E.; Urra, J.; Martínez, M.J. Eco-friendly technologies based on banana peel use for the decolourization of the dyeing process wastewater. Waste Biomass Valorization 2011, 2, 77–86. [Google Scholar] [CrossRef]
  27. Hashem, A.H.; Saied, E.; Hasanin, M.S. Green and ecofriendly bio-removal of methylene blue dye from aqueous solution using biologically activated banana peel waste. Sustain. Chem. Pharm. 2020, 18, 100333. [Google Scholar] [CrossRef]
  28. Ma, J.; Huang, D.; Zou, J.; Li, L.; Kong, Y.; Komarneni, S. Adsorption of methylene blue and Orange II pollutants on activated carbon prepared from banana peel. J. Porous Mater. 2015, 22, 301–311. [Google Scholar] [CrossRef]
  29. Unuabonah, E.I.; Adie, G.U.; Onah, L.O.; Adeyemi, O.G. Multistage optimization of the adsorption of methylene blue dye onto defatted Carica papaya seeds. Chem. Eng. J. 2009, 155, 567–579. [Google Scholar] [CrossRef]
  30. Pavia, D.L.; Lampman, G.M.; Kriz, G.S.; Vyvyan, J.A. Introduction to Spectroscopy; Cengage learning: Boston, MA, USA, 2014. [Google Scholar]
  31. Laskar, N.; Kumar, U. SEM, FTIR and EDAX studies for the removal of safranin dye from water bodies using modified biomaterial-Bambusa tulda. In Proceedings of the IOP Conference Series: Materials Science and Engineering, Busan, Korea, 25–27 August 2017; p. 012105. [Google Scholar]
  32. Annadurai, G.; Juang, R.-S.; Lee, D.-J. Use of cellulose-based wastes for adsorption of dyes from aqueous solutions. J. Hazard. Mater. 2002, 92, 263–274. [Google Scholar] [CrossRef]
  33. AbdurRahman, F.B.; Akter, M.; Abedin, M.Z. Dyes removal from textile wastewater using orange peels. Int. J. Sci. Technol. Res. 2013, 2, 47–50. [Google Scholar]
  34. Namasivayam, C.; Muniasamy, N.; Gayatri, K.; Rani, M.; Ranganathan, K. Removal of dyes from aqueous solutions by cellulosic waste orange peel. Bioresour. Technol. 1996, 57, 37–43. [Google Scholar] [CrossRef]
  35. Rahman, F.; Akter, M. Removal of dyes form textile wastewater by adsorption using shrimp shell. Int. J. Waste Resour 2016, 6, 2. [Google Scholar]
  36. Yamuna, R.; Namasivayam, C. Color removal from aqueous solution by biogas residual slurry. Toxicol. Environ. Chem. 1993, 38, 131–143. [Google Scholar] [CrossRef]
  37. El Qada, E.N.; Allen, S.J.; Walker, G.M. Adsorption of basic dyes onto activated carbon using microcolumns. Ind. Eng. Chem. Res. 2006, 45, 6044–6049. [Google Scholar] [CrossRef]
  38. Li, H.; Cao, X.; Zhang, C.; Yu, Q.; Zhao, Z.; Niu, X.; Sun, X.; Liu, Y.; Ma, L.; Li, Z. Enhanced adsorptive removal of anionic and cationic dyes from single or mixed dye solutions using MOF PCN-222. RSC Adv. 2017, 7, 16273–16281. [Google Scholar] [CrossRef][Green Version]
  39. Amela, K.; Hassen, M.A.; Kerroum, D. Isotherm and kinetics study of biosorption of cationic dye onto banana peel. Energy Procedia 2012, 19, 286–295. [Google Scholar] [CrossRef][Green Version]
  40. de Sousa, A.É.A.; Gomes, E.C.C.; de Quadros Melo, D.; Diógenes, I.C.N.; Becker, H.; Longhinotti, E. Adsorption of safranin on pseudostem banana fibers. Sep. Sci. Technol. 2014, 49, 2681–2688. [Google Scholar] [CrossRef]
  41. El-Maghraby, A.; Taha, N.A. Equilibrium and kinetic studies for the removal of cationic dye using banana pith. Adv. Environ. Res. Int. J. 2014, 3, 217–230. [Google Scholar] [CrossRef]
  42. Hashem, F.; Amin, M. Adsorption of methylene blue by activated carbon derived from various fruit peels. Desalination Water Treat. 2016, 57, 22573–22584. [Google Scholar] [CrossRef]
  43. Ahmed, A.E.; Majewska-Nowak, K. Removal of Reactive Dye from Aqueous Solutions Using Banana Peel and Sugarcane Bagasse as Biosorbents. Environ. Prot. Eng. 2020, 46, 121–135. [Google Scholar] [CrossRef]
  44. Djilani, C.; Zaghdoudi, R.; Magri, P.; Djazi, F.; Lallam, A.; Bouchekima, B. Elaboration and characterization of chitosan/banana peel biocomposite for the removal of dyes from wastewater. Desalination Water Treat. 2019, 151, 189–198. [Google Scholar] [CrossRef]
Figure 1. Chemical structure of different reactive dyes: (a) Sudan Black B, (b) Direct Red 6BL, and (c) Reactive Yellow 3RS with similar generic name as Deazol Black B EAN, Deafiz Red ME 6BL, and Firstfix Yellow 3RS, respectively.
Figure 1. Chemical structure of different reactive dyes: (a) Sudan Black B, (b) Direct Red 6BL, and (c) Reactive Yellow 3RS with similar generic name as Deazol Black B EAN, Deafiz Red ME 6BL, and Firstfix Yellow 3RS, respectively.
Textiles 01 00018 g001
Figure 2. (a) Determination of wavelength for maximum absorption; (b) calibration curve of standard dye solution at λmax = 601 nm, pH ~ 7, and T = 25 °C.
Figure 2. (a) Determination of wavelength for maximum absorption; (b) calibration curve of standard dye solution at λmax = 601 nm, pH ~ 7, and T = 25 °C.
Textiles 01 00018 g002
Figure 3. FTIR spectra of banana peel; Conditions: 25 °C, banana peel: KBr = 1:100, number of scans: 30, resolution: 2 cm−1.
Figure 3. FTIR spectra of banana peel; Conditions: 25 °C, banana peel: KBr = 1:100, number of scans: 30, resolution: 2 cm−1.
Textiles 01 00018 g003
Figure 4. The adsorption of dyes on the banana peel at variable pH’s (Ci = 50 mg/L, Mads = 0.5, 0.75, and 1.0 g, t = 1 h, T = 25 °C, S = 180 rpm, V = 250 mL).
Figure 4. The adsorption of dyes on the banana peel at variable pH’s (Ci = 50 mg/L, Mads = 0.5, 0.75, and 1.0 g, t = 1 h, T = 25 °C, S = 180 rpm, V = 250 mL).
Textiles 01 00018 g004
Figure 5. Effects of adsorbent dosage on the dye adsorption onto the banana peel (pH = 7, Ci: 50 mg/L, Mads: 0.1 to 0.8 g, t: 1 h, T: 25 °C, S: 180 rpm, solution volume: 250 mL).
Figure 5. Effects of adsorbent dosage on the dye adsorption onto the banana peel (pH = 7, Ci: 50 mg/L, Mads: 0.1 to 0.8 g, t: 1 h, T: 25 °C, S: 180 rpm, solution volume: 250 mL).
Textiles 01 00018 g005
Figure 6. (a) The percent removal of dyes and (b) amount of dyes adsorbed for variable contact time and initial concentration (pH: 7, Ci: 25, 50, 100, and 150 mg/L, Mads: 0.5 g, t: 0 to 120 min, T: 25 °C, S: 180 rpm, solution volume: 250 mL).
Figure 6. (a) The percent removal of dyes and (b) amount of dyes adsorbed for variable contact time and initial concentration (pH: 7, Ci: 25, 50, 100, and 150 mg/L, Mads: 0.5 g, t: 0 to 120 min, T: 25 °C, S: 180 rpm, solution volume: 250 mL).
Textiles 01 00018 g006
Figure 7. (a) Langmuir and (b) Freundlich isotherm model plots for adsorption of dyes onto the banana peel (pH: 7, Ci: 25, 50, 75, 100, 150 and 200 mg/L, Mads: 0.5 g, t: 60 min, T: 25 °C, S: 180 rpm, solution volume: 250 mL).
Figure 7. (a) Langmuir and (b) Freundlich isotherm model plots for adsorption of dyes onto the banana peel (pH: 7, Ci: 25, 50, 75, 100, 150 and 200 mg/L, Mads: 0.5 g, t: 60 min, T: 25 °C, S: 180 rpm, solution volume: 250 mL).
Textiles 01 00018 g007
Figure 8. Graphical presentation of the separation factor (RL) against initial dye concentration (pH: 7, Ci: 25, 50, 75, 100, 150 and 200 mg/L, Mads: 0.5 g, t: 60 min, T: 25 °C, S: 180 rpm, solution volume: 250 mL).
Figure 8. Graphical presentation of the separation factor (RL) against initial dye concentration (pH: 7, Ci: 25, 50, 75, 100, 150 and 200 mg/L, Mads: 0.5 g, t: 60 min, T: 25 °C, S: 180 rpm, solution volume: 250 mL).
Textiles 01 00018 g008
Figure 9. (a) Pseudo-first-order and (b) pseudo-second-order kinetics for the adsorption of dyes onto the banana peel.
Figure 9. (a) Pseudo-first-order and (b) pseudo-second-order kinetics for the adsorption of dyes onto the banana peel.
Textiles 01 00018 g009
Figure 10. Regeneration of banana peel using different solvents: (A) 0.1 M HCl, (B) 0.1 M NaOH, and (C) subsequent addition of 0.1 M HCl and 0.1 M NaOH.
Figure 10. Regeneration of banana peel using different solvents: (A) 0.1 M HCl, (B) 0.1 M NaOH, and (C) subsequent addition of 0.1 M HCl and 0.1 M NaOH.
Textiles 01 00018 g010
Table 1. Adsorption isotherm parameters for dye adsorption onto the banana peel.
Table 1. Adsorption isotherm parameters for dye adsorption onto the banana peel.
qm (mg/g)KL (L/mg)R2RL1/nFKF (mg/g)R2–0.140.11416.50.8266
Table 2. Adsorption kinetic parameters for dye adsorption onto the banana peel.
Table 2. Adsorption kinetic parameters for dye adsorption onto the banana peel.
Kinetic ModelParameterInitial Dye Concentration (mg/L)
k1 (min−1)0.0590.0490.047
qe,calc (mg/g)5.420.821.0
k2 (g mg−1 min−1)0.0320.0360.033
qe,calc (mg/g)12.827.830.7
qe,exp (mg/g)12.524.028.4
Table 3. Adsorption Capacities of banana waste-based adsorbent for the removal of dyes.
Table 3. Adsorption Capacities of banana waste-based adsorbent for the removal of dyes.
AdsorbentAdsorbateqm (mg/g)Conc. (mg/L)Contact TimepH% RemovalRef.
Banana peelMethylene blue18.6475–1003 h4–896–98[39]
Activated banana peelMethylene blue19.6715–1003 h4–890–94
Pseudo stream banana fiberSafanin21.745–4090 min7.5-[40]
Banana pith Methylene blue11.3255–253 h 89[41]
Banana peel ACMethylene blue620100024 h8.0 [42]
Banana peel powderEurozol Navy blue24.095060 min7.068–72[43]
Chitosan/Banana peelMethylene blue- 100 min7.096[44]
Publisher’s Note: MDPI stays neutral with regard to jurisdictional claims in published maps and institutional affiliations.
Back to TopTop