Download PDF

Waste and Biomass Valorization

, Volume 6, Issue 4, pp 547–559 | Cite as

Azolla pinnata: An Efficient Low Cost Material for Removal of Methyl Violet 2B by Using Adsorption Method

  • Muhammad Raziq Rahimi Kooh
  • Linda B. L. Lim
  • Muhammad Khairud Dahri
  • Lee Hoon Lim
  • J. M. R. Sarath Bandara
Original Paper
First Online:
Received:
Accepted:

Abstract

Azolla pinnata (AP), a floating aquatic macrophyte, was studied as a potential adsorbent for the removal of methyl violet (MV) in a batch adsorption system. Surface characterisation, effects of particle size, adsorbent dosage, pH, ionic strength and pre-treatments of adsorbent were carried out. The study of the effects of pH and ionic strength suggested that electronic interaction and hydrophobic–hydrophobic interaction might be the major forces of dye interaction. Pseudo 2nd order kinetic model best-fitted the kinetic data indicating that the adsorption process may be controlled by chemical process. The Weber–Morris and Boyd models were used for describing the diffusion mechanism which showed that intraparticle diffusion was not the rate limiting step, and film diffusion or in combination of other mechanisms might be in control. Isotherm modelling showed that the Langmuir model best-fitted the experimental data with q m of 194.2 mg g−1 at 25 °C and 323.4 mg g−1 at 65 °C. Thermodynamic studies showed that the adsorption process is endothermic, spontaneous and with significant change to the internal structure of adsorbent. The estimated activation energy by Arrhenius equation is 54.8 kJ mol−1, which indicates that the adsorption process may be controlled by chemical process. Adsorbent regenerated using NaOH displayed retention of high adsorption capability almost similar to fresh adsorbent even after five consecutive cycles. Ability to regenerate coupled with good adsorption capability suggests that AP has great potential to be utilised as a low-cost adsorbent for the removal of MV in real life application.

Keywords

Azolla pinnata Low cost adsorbent Methyl violet 2B Adsorption Kinetic studies Regeneration 

Introduction

Synthetic dyes are extensively used in the current era, but they are considered as one of the pollutants that raises concerns due to its impact on the environment as well as its toxic effect on living things. Due to their xenobiotic nature and stability, synthetic dyes are recalcitrant to biodegradation, and are highly visible even in low level contamination. The water bodies, where dyes are discharged, exhibit low biological oxygen demand (BOD) and high chemical oxygen demand (COD) [1]. Furthermore, the dyes can interfere with aquatic ecosystem as they can hinder photosynthetic activity and upset the biological processes [2].

Decolourisation techniques such as the uses of oxidising or reducing agents, biological methods (live plant, fungi or microorganism such as bacteria), electrochemical degradation, ion-exchange, irradiation, precipitation, reverse osmosis and adsorption methods were conventional methods of wastewater treatment. The advantages and disadvantages of these methods are widely discussed in the literatures [3, 4, 5].

Adsorption method is one of the preferred ways of wastewater treatment due to its simplicity in design and usually does not produce harmful side-products [6]. Another attractive feature of this treatment is that the materials used are often abundant in nature such as Causarina equisetifolia needle [7], peat [8], and agricultural residues e.g. rice husk [9], peanut hulls [10], sugarcane bagasse [11, 12], tarap fruit peel [13] and walnut shell [14], and this resulted in lower cost of treatment. The adsorbent can also be physically modified by heat treatment and autoclaved [15], or chemically modified via various methods, such as immobilisation with sodium alginate [16], mineral acid treatment with hydrochloric acid [11, 12] or sulphuric acid [15], and treatment with chelating agents e.g. polyethyleneimine [12, 17], to increase the dye adsorption capacity.

Methyl violet 2B (MV) is a popular purple colour dye used in textile industry, paper printing, and it is also an active ingredient in Gram’s biological stain for bacteria classification [18]. However, MV is known to cause severe irritation to skin, eye, respiratory tract and gastrointestinal tract.

The primary aim of this study is to investigate the potential usage of water fern, Azolla pinnata (AP), as an adsorbent for the removal of MV dye. The AP is an invasive freshwater aquatic fern that contains nitrogen-fixing cyanbacteria, Anabaena azollae, as its symbiont which leads to rapid colonisation of water bodies. Uncontrolled proliferation of AP leads to the formation of dense mat of aquatic fern and the greening of the water (caused by algal bloom of free-living Anabaena azollae) which reduce light penetration into the water. These effects can reduce photosynthetic activity of the submerged aquatic plants and rapid depletion of dissolved oxygen concentration in the water [19]. This can potentially cause harm to the aquatic life. In view of the proliferous growth of AP in association with Anabaena azollae in tropical water bodies with least of attention and input, the main objective of this study was to evaluate the ability of AP as a substrate for remediation of MV in water bodies.

Materials and Methods

Chemicals and Reagents

Biological stain grade methyl violet 2B dye (MV) (C24H28N3Cl; Mr 393.95 g mol−1), with purity of 80 % dye content was purchased from Sigma Aldrich Corporation. pH of solution was adjusted using NaOH and HNO3 which were purchased from Fluka. Spectroscopy grade KBr was used for FTIR analysis and was dried in oven at 110 °C before use. Chemical reagents used for pre-treatment of adsorbent include oxalic acid (99 % purity, Harris Reagent), 85 % phosphoric acid (ACS grade for analysis, Merck) and citric acid (99 % purity, BDH). All chemical were used without further purification.

Adsorbent and Stock Preparation

Azolla pinnata (AP) was obtained from the Agriculture Department, Ministry of Industrial and Primary Resource, Brunei Darussalam. The AP was grown under natural light in plastic containers using water from freshwater fishpond. Multiple harvesting of the AP were carried out over a period of three months and the AP was washed several times with distilled water followed by oven-dried at 75 °C until a constant weight was obtained. Dried samples were ground to fine powder using mortar and pestle and sieved to obtain various particle sizes (>850 μm, 355–850 and <355 μm) and were stored in a desiccator. MV stock solution of 1000 mg L−1 was prepared by dissolving the required amount of MV solid in distilled water. The stock solution was then used to prepare solution of various concentrations. All experiments were carried out in duplicates.

Instrumentation

The absorbance of dye solution was measured at optimum wavelength, λmax, of 584 nm using a single beam UV–vis spectrophotometer (Jenway 6320D spectrophotometer). The elemental CHNS composition of AP was determined using a Thermo Scientific Flash 2000 Organic Elemental Analyzer CHNS/O. Fourier Transform Infrared (FTIR) spectrophotometer (Shimadzu Model IRPrestige-21) was used to characterise the functional groups present in the untreated AP and MV-treated AP. X-ray fluorescene (XRF) spectrophotometer (PANalytical Axiosmax) was used to determine the percentage of elements present in the AP and MV-treated AP. Prior to scanning electron microscope (SEM) imaging, the surface coating of the samples were carried out using an SPI-Module 1143 Sputtering Coater, at plasma current 15 mA for 120 s. SEM images of untreated AP and MV-treated AP were obtained using JEOL JSM-5800LV (Japan), under high vacuum mode and accelerating voltage of 15 kV. Stuart orbital shaker was used for agitation of the solution. Thermo Scientific Orion 2 Star pH Benchtop was used to measure the pH.

Point of Zero Charge

The pHpzc of the adsorbent was determined by the salt addition method using 0.1 M KNO3 solutions [20]. The initial pH (2.5–10.0) of 20 mL KNO3 was adjusted using 0.1 M HNO3 and NaOH, and the pH was measured. 0.04 g adsorbent was added and agitated for 24 h and the final pH was measured. The pHpzc was obtained by plotting the change in pH (final pH—initial pH) versus initial pH.

Batch Experiment Procedures

Batch experiments were carried out by mixing 0.04 g of adsorbent with 20.0 mL of known concentration of MV in a 150 mL Erlenmeyer flask. The mixtures were agitated using orbital shaker at 250 rpm at room temperature. Parameters such as particle size (sieve sizes: >850, 355–850 and <355 μm), adsorbent dosage (0.01–0.10 g), contact time (5–240 min), initial concentration (20–1000 mg L−1), pH (3.0–8.0), temperature (ambient, 35, 45, 55, 65 °C), and ionic strength were investigated. The mixture was filtered and the filtrates were analysed using an UV–vis spectrophotometer. The experiments were carried out under agitation time of 120 min unless otherwise stated.

The amount of MV adsorbed per gram of AP, q e (mg g−1), was calculated by the following equation:
$$ q_{e} = \frac{{\left( {C_{i} - C_{e} } \right)V}}{m} $$
(1)
where C i is the initial dye concentration (mg L−1), C e is the equilibrium dye concentration (mg L−1), V is the volume of MV solution used (L) and m is the mass of AP used (g). The percentage removal of the dye represent by:
$$ {\text{Percentage}}\,\,{\text{removal }} = \frac{{\left( {C_{i} - C_{e} } \right) \times 100 \,\% }}{{C_{i} }} $$
(2)

The adsorption process was described using the Langmuir, Freundlich and Dubinin-Radushkevich isotherm models.

Error Analysis

The kinetic and isotherm models that best fit the equilibrium data were determined by the values of the coefficient of determination (R 2 ). In addition, the predicted q e (q e,cal) were calculated from either the kinetic or isotherm models and error analyses were applied. Best fit of experimental data (q e,exp) was determined by the smallest values of these error analyses functions which indicates the least error [21].

The equations of the four types of error analysis are as follows:
$$ {\text{Sum }}\,{\text{of}}\,{\text{absolute}}\,{\text{error}}\,\left( {\text{EABS}} \right)\,{\hbox{:}} \mathop \sum \limits_{i = 1}^{n} \left| {q_{{e,{ \exp }}} - q_{{e,{\text{cal}}}} } \right| $$
(3)
$$ {\text{Chi-square }}{\text{test}}\, \left({\chi^{2 }} \right){\hbox{:}}\,\mathop \sum \limits_{i = 1}^{n} \frac{{(q_{{e,{ \exp }}} - q_{{e,{\text{cal}}}} )^{2} }}{{q_{{e,{ \exp }}} }} $$
(4)
$$ {\text{Average}}\,{\text{relative }}\,{\text{error}}\,\left( {\text{ARE}} \right)\,{\hbox{:}} \frac{100}{n}\mathop \sum \limits_{i = 1}^{n} \left| {\frac{{q_{e,\exp } - q_{{e,{\text{cal}}}} }}{{q_{e,\exp } }}} \right|_{i} $$
(5)
$$ {\text{Marquardt's}} {\text{percent}}\,{\text{standard}}\,{\text{deviation}}\,\left( {MPSD} \right){\hbox{:}} 100\sqrt {\frac{1}{n - p}\mathop \sum \limits_{i}^{n} \left( {\frac{{q_{e,\exp } - q_{{e,{\text{cal}}}} }}{{q_{e,\exp } }}} \right)^{2} } $$
(6)
where q e,exp is the experimental value while q e,cal is the calculated value, n is the number of data points in the experiment and p is the number of parameters of the isotherm model.

Regeneration Experiment

The regeneration experiments were examined for three different types of solvents: distilled water, 0.1 M HNO3 and 0.1 M NaOH. Three sets of adsorbent were treated with 100 mg L−1 MV to obtained MV-treated AP at the dosage of 0.04 g/20 mL dye. The MV-treated AP was washed with distilled water and shaken in an orbital shaker for 30 min. The washed solution was discarded and the same procedure was repeated until little desorption of dye from the adsorbent into the distilled water. The solid was subsequently dried in oven at 70 °C. Similar procedure was applied to the acid and basic wash, where 20 mL of 0.1 M acid or base added, shaken for 30 min and followed by multiple distilled water washing until pH of the washed solution became near neutral.

Pre-treatment of Adsorbent

AP was subjected to various treatments to assess its adsorption ability and to investigate if such treatment could enhance its adsorption capacity when compared to the untreated adsorbent. The treatment of adsorbent was based on literatures, with some alterations of the procedure.

Briefly, adsorbent was treated with 1.0 M oxalic acid [22] and 0.06 M citric acid [23] at dosage of 10 mL chemical reagent per gram adsorbent and agitated in an orbital shaker for 2 h. Chemical-treated adsorbent was filtered with a Whatman No. 41 filter paper and dried at 60 °C for 24 h. It was heated at 120 °C in an oven for 2 h, followed by 0.05 M NaHCO3 washing, and then repeatedly with distilled water until the pH of effluent was near neutral, and dried at 60 °C.

The chemical treatment with phosphoric acid was carried out at dosage of 10 mL 85 % H3PO4 per gram adsorbent, and was agitated for 2 h and left to stand for 24 h at room temperature [24]. The washing procedure is similar to the oxalic acid and citric acid method as mentioned earlier.

NaOH-treated adsorbent was prepared at the dosage of 10 mL 1 M NaOH per gram adsorbent, agitated for 2 h, washing with distilled water washing until the effluent is near neutral, and dried in an oven at 60 °C [25].

Adsorption capacity of modified adsorbents was investigated at dosage of 0.02 g/20 mL dye at ambient pH.

Results and Discussion

Characterisation of Absorbent

The C, H, N, S compositions of AP on dry weight were 44.18, 6.27, 4.01 and 0.20 % respectively. The XRF elemental analyses of AP before and after dye treatment are as shown in Table 1. After dye treatment, the K and Na contents showed reduction from 14.39 and 4.38 % to 0.19 and 0.14 %, respectively. Such observation could be attributed to the K+ and Na+ ions being displaced by MV, which is a cationic dye. Similar findings were reported for the adsorption of basic dyes using tarap peel and peat soil [13, 26].
Table 1

XRF data of AP before and after treatment of MV

Elements

Normalised percentage (%)

Before

After

Al

0.45

0.39

Mn

0.49

0.35

P

2.48

1.02

Mg

3.66

2.64

Na

4.38

0.14

Cl

8.65

1.03

Ca

12.31

10.71

K

14.39

0.19

O

28.47

29.62

The FTIR spectra of untreated AP and MV-treated AP are shown in Fig. 1. The FTIR spectrum of the untreated AP indicates the presence of various functional groups at wavelengths 3279 cm−1 (O–H stretch), 2918 cm−1 and 2849 cm−1 (C–H stretch), 1651 cm−1 (C=O bending) and 1033 cm−1 (out-of-plane bending of carbonate). FTIR spectrum of MV-treated AP displayed bands at 3319 cm−1 (O–H stretch), 2918 cm−1 and 2849 cm−1 (C–H stretch), 1658 cm−1 (C=O bending) and 1026 cm−1 (out-of-plane bending of carbonate), where the shift of the bands may indicate that these functional groups interact with the MV molecules [9, 27]. The three bands that are present only on MV-treated AP are 1587 cm−1 (–COO− anti-symmetric stretching), 1365 cm−1 (–COO− symmetric stretching) and 1173 cm−1 (C–N stretching of MV) confirmed the loading of MV dye into the adsorbent [9]. This data also suggested that functional groups of –COO− may be responsible for the interaction between the adsorbent and the dye molecules [9].
Fig. 1

FTIR spectra of A untreated AP and B MV-treated AP

The SEM images of untreated and MV-treated AP are as shown in (A) and (B) of Fig. 2, respectively. These images showed that the adsorbent particle surface is rough in nature and no obvious distinction can be found between the adsorbent particles of untreated and MV-treated AP.
Fig. 2

SEM images of a untreated AP, and b MV-treated AP treated, at ×2000 magnification

Effect of Particle Size and Adsorbent Dosage

The three particles sizes, >850 μm, 355–850 and <355 μm, resulted in dye removal of 60.8, 87.2 and 92.4 % respectively. The smaller the particle size, the higher the surface area and hence more functional groups are exposed for the interaction with dye molecules. As particle size of <355 μm gave the highest percentage removal, thus particle of this size was used for the rest of the experiment.

The effect of adsorbent dosage on removal of MV is shown in Fig. 3. The removal of MV increases when the dosage was increased from 0.01 to 0.04 g and no further increase beyond 0.04 g was observed. Therefore, 0.04 g is taken as the optimum dosage and subsequently used for the rest of the experiment.
Fig. 3

Effect of adsorbent dosage on the removal of 100 mg L−1 MV, with total volume of mixture at 20 mL

Effect of Contact Time and Concentration

Determination of the contact time between AP and the MV is essential in adsorption experiment as it ensures that the dye uptake by the AP reaches a saturation point where there will be no significant net transfer of dye between the AP and the solution beyond that point. The effect of contact time on the adsorption of MV by AP at different initial dye concentrations (C i  = 100, 200, 300, 400 mg L−1) is shown in Fig. 4a.
Fig. 4

Effect of contact time at a different initial dye concentrations (100, 200, 300, 400 mg L−1) at ambient temperature of 25 °C, b different temperature (25, 35, 45, 55, 65 °C) at Ci 100 mg L−1 MV, and c effect of concentration of MV adsorption at different temperature

Rapid dye uptake occurred within the first 30 min of contact time and the uptake gradually slowed down until it became constant. The rapid initial MV uptake is due to the availability of large amount of vacant sites at the beginning of the adsorption process, which gradually become less available and more difficult over time due to the build-up of the repulsion forces between the dye molecules in the solid and bulk phases [28]. As seen in Fig. 4a and 4c, higher C i resulted in higher dye uptake because high C i provides the driving force that overcome the resistances and transfer the dye molecules deeper into the micropores of the adsorbent [28].

The time taken to reach equilibrium for C i at 100, 200, 300 and 400 mg L−1 were 60, 60, 90 and 120 min, respectively. Thus, agitation time of 120 min was chosen for all the experiments, to ensure complete equilibrium was attained.

The effect of temperature on dye uptake on 100 mg L−1 MV is shown in Fig. 4b. It can be observed that the dye uptake was more rapid at higher temperature and the equilibrium was attained within the first 30 min. Higher temperature (35–55 °C) also resulted in higher q e at equilibrium point, while adsorption beyond 55 °C did not result in any increase of q e . Further analysis of thermodynamic data using the Arrhenius equation was discussed under the “Thermodynamic Studies” section.

Kinetic Studies

In this study, four widely used kinetics models, namely the Lagergren 1st order [29], pseudo 2nd order [30], Weber-Morris intraparticle diffusion [31] and Boyd [32] models were used in characterising the adsorption mechanism between the dye and the adsorbent.

The Lagergren 1st order is expressed as:
$$ \log (q_{e} - q_{t} ) \, = \log q_{e} - \frac{t}{2.303}K_{1} $$
(7)
where q t is the amount of MV adsorbed per gram of AP (mg g−1) at time t, K 1 is the Lagergren 1st order rate constant (min−1) and t is the time shaken (min).
The pseudo 2nd order is expressed as:
$$ \frac{t}{{q_{t} }} = \frac{1}{{q_{e}^{2} K_{2 } }} + \frac{t}{{q_{e} }} $$
(8)
where K 2 is pseudo second order rate constant (g mg−1 min−1).

The rate constant K 1, K 2 and the q e,cal (predicted adsorbate concentration at equilibrium) were obtained from the linear plot of \( ln\left( {q_{e} - q_{t} } \right) vs t \) and \( \frac{t}{{q_{t} }}vs t \), respectively.

The parameters of Lagergren 1st order and pseudo 2nd order are summarised in Table 2. The values of R 2 of the kinetic models are higher for pseudo 2nd order (R 2 ≥ 0.999) (Fig. 5a) as compared to the Lagergren 1st order for C i of 100, 200, 300 and 400 mg L−1. The calculated adsorption capacity (q e,cal) of the pseudo 2nd order is closer to the experimental adsorption capacity (q e,exp) than that of Lagergren 1st order. For example, using 100 mg L−1 the q e,cal for pseudo 1st and 2nd order are 23.7 and 48.9 mg g−1, respectively, while the q e,exp is 47.2 mg g−1, clearly indicating that the adsorption follows the pseudo 2nd order. This is further supported by the error analyses functions (χ2, ARE, EABS and MSDP) where the pseudo 2nd order showed the lowest values which indicates the least error. Therefore with consideration of the R 2, q e,cal and the values of error analyses function, it is concluded that the pseudo 2nd order best fit the data, and the adsorption process may be governed by chemical process.
Table 2

Parameters of the kinetic models of various concentrations at ambient temperature

Lagergren 1st order model

 C i (mg L−1)

100

200

300

400

 q e,cal (mg g−1)

23.7

34.7

33.9

76.1

 q e,exp (mg g−1)

47.2

100.3

127.3

177.2

 K 1

0.032

0.027

0.021

0.016

 R 2

0.972

0.814

0.714

0.881

 χ 2

135.4

646.5

864.6

907.8

 EABS

209.2

860.7

1060.4

1276.7

 ARE

45.1

74.9

75.8

72.0

 MSDP

74.9

82.1

90.4

79.4

Pseudo 2nd order model

 q e,cal (mg g−1)

48.9

101.5

130.1

183.6

 q e,exp (mg g−1)

47.2

100.3

127.3

177.2

 K 2

0.003

0.002

0.001

0.001

 R 2

0.999

0.999

0.999

0.999

 χ2

1.3

3.4

2.9

5.9

 EABS

13.6

45.8

42.6

61.1

 ARE

3.5

4.3

3.4

4.3

 MSDP

8.3

6.2

5.6

7.8

Weber-Morris Intraparticle diffusion model

Region A

 K 3a (mg g−1 min1/2)

6.585

10.689

10.918

14.977

 C a

7.6

39.7

48.1

48.7

 R 2

0.889

0.901

0.846

0.948

Region B

 K 3b (mg g−1 min1/2)

0.999

0.944

1.238

4.354

 C b

33.9

85.7

110.1

115.9

 R 2

0.841

0.779

0.605

0.774

Boyd Modela

 Slope

0.032

0.032

0.045

0.024

 Intercept

0.191

0.701

0.108

0.064

 R 2

0.972

0.975

0.965

0.995

aParameters calculated from the initial linear region of the plot only

Fig. 5

Plot of a pseudo 2nd order kinetic model, and b Weber-Morris model displayed multi-linearity behavior, for C i of 100, 200, 300 and 400 mg L−1 MV adsorption by AP at dosage of 0.04 g/20 mL dye, at room temperature and ambient pH

Weber-Morris intraparticle diffusion model was used for describing the diffusion mechanism, as this mechanism is not applicable to Lagergren 1st order and pseudo 2nd order models. Typically, the diffusion process of the adsorbate can be classified into three phases. The first phase is a fast external diffusion or the boundary layer diffusion, followed by the gradual surface adsorption owning to the intraparticle diffusion, and lastly, the slow equilibrium phase [33, 34].

The equation of the Weber-Morris intraparticle diffusion model is expressed as:
$$ q_{t} = \, K_{3} t^{1/2} + \, C $$
(9)
where K 3 is the intraparticle diffusion rate constant (mg g−1 min−1/2) and C is the intercept.

The parameters K 3 and C were determined from the linear plot of q t versus t 1/2.

The Weber-Morris plot is as shown in Fig. 5b, where multi-linearity is observed, and the parameters are summarised in Table 2. The fast external diffusion was completed very rapidly within 5 min and thus it is not observed in the Weber-Morris plot. Similar behaviour was observed by Özacar and Şengil in the adsorption of disperse dye onto alunite [34] and the adsorption of phosphate into red mud [33]. The initial region in Fig. 5b represented the gradual surface adsorption owning to intraparticle diffusion phase, while the plateau region represented the slow equilibrium phase. According to the Weber-Morris model, if the linear plot passes through the origin, then the intraparticle diffusion is the rate-limiting step. As shown in Table 2, the values of C (intercept) were non-zero, which indicate that intraparticle diffusion was not the rate-limiting step and other mechanisms may be involved. The C value is associated with the thickness of the boundary layer, and the larger C value may represent thicker boundary layer.

The kinetic data was analysed with the Boyd model to further determine the diffusion mechanism of the adsorption process. The Boyd model can be used to identify whether the adsorption process is governed by film diffusion or particle diffusion. Film diffusion is the transport of adsorbates to the external surface of adsorbent, while particle diffusion is the transport of adsorbates within the pores of the adsorbent [35].

The Boyd model is expressed as:
$$ B_{t} = \, - 0.4977 - \ln \,(1 \, - \, F) $$
(10)
where F is equivalent to q t /q e , and B t is mathematical function of F.

The slopes and intercepts of the linear plot of B t versus t was summarised in Table 2. In our study, multilinearity was also observed for the Boyd plot (plot not shown), only the first linear region (q t 5–30 min) was used for the calculation of the parameters (slope and intercept) [36]. According to the Boyd model, if the linear plot passes through the origin, then the diffusion is controlled by particle diffusion, otherwise it is controlled by film diffusion [35]. As all the values of the Boyd plot intercept are non-zero, this indicates that the diffusion may be controlled by film diffusion or in combination with other mechanisms.

Effects of pH and Ionic Strength

It is well established that adsorption of the dye molecules by adsorbent is mainly by electrostatic interaction, hydrophobic–hydrophobic interaction and hydrogen bonding, and pH affect mainly the electrostatic interaction [37, 38].

Prior to the investigation of the effect of pH on adsorption activity of AP, it is essential to determine the range of pH where the colour intensity of the dye MV will not be affected. As MV is used as pH indicator for low acidic region, the pH region where the colour of MV changes from purple to green and yellow needs to be avoided. The pH range from 2.0 to 12.0 was investigated. The decrease of colour intensity was observed at extreme pH from 11.0 to 12.0, which may be due to alkaline fading [39]. Reduction of colour intensity was also observed at pH <3.0 which may be due to formation of MV-H2+ species, which was observed for another basic dye (malachite green) of same triarylmethane dye category as MV [39]. Therefore the study of the adsorption of MV by AP was limited to range of pH 3.0–10.0.

The effect of pH on dye adsorption by AP is summarised in Fig. 6a. The optimum pH of MV adsorption by the AP is pH 4.0 at 54.1 mg g−1 (94.0 % removal), while ambient pH of 5.4 resulted in q e of 51.5 mg g−1 (93.5 % removal). The differences of dye adsorption between the optimum pH and the ambient pH are insignificant thus all the adsorption experiments were carried out at the ambient pH of 5.4.
Fig. 6

Effect of a pH, and b various concentrations of KNO3, NaCl and MgSO4, on the removal of 100 mg L−1 MV by AP at dosage of 0.04 g AP/20 mL dye

The point of zero charge (pHpzc) of AP was found to be at pH 6.6. Using the concept of pHpzc, the surface of AP will be predominant negatively charged when solution pH > 6.6, while predominant positively charged when pH < 6.6. As MV is a cationic dye, the predominant positively charged surface of AP at pH < 6.6 should be unfavourable for adsorption of MV due to electronic repulsion. However, as observed in Fig. 6a, that pH 3.0–6.0 showed high removal which is not significantly different from adsorption at pH 8.0 and 10.0. This indicates that the adsorption system of AP and MV is not limited to only the electronic interaction. This is further verified by the study on the effect of ionic strength on the adsorption of MV by AP.

Solutions of KNO3, NaCl and MgSO4 were used to study the effect of salt content (concentration 0.01–0.90 M) on the adsorption process of MV by AP. Salt concentration is directly proportionally to the ionic strength and thus a higher salt concentration will result in a higher ionic strength. As seen in Fig. 6b, all the three salts (KNO3, NaCl and MgSO4) resulted in the decrease of MV adsorption as the ionic strength increase. This behaviour is usually observed for adsorption of basic dye in high ionic strength condition [14, 37]. At 0.9 M of KNO3, NaCl and MgSO4, the q e was reduced from approximately 47.0 mg g−1, to 27.0, 39.2 and 36.7 mg g−1, respectively. The reduction in q e is due to the suppression of the electrostatic interaction by the cations (K+, Na+ and Mg2+) which compete with the dye molecules for the negatively charged sites on AP surface [37]. These reduction may give an idea on the amount of dye molecules adsorbed due to electronic attraction. Albeit the supression of electronic interaction between AP and MV, the q e is not zero which indicate that hydrophobic–hydrophobic interaction and hydrogen bonding may be the major force of dye interaction with the adsorbent.

On the positive side, the ability of AP to maintain high removal in high ionic strength condition can be advantageous in treatment of textile wastewater, as the textile wastewater can contain high level of Na, K and Mg salts resulted from chemical salts used for pretreatment of fabrics such as surfactants and electrolytes, and detergent for washing [40].

Isotherm Studies

Three adsorption isotherm models: Langmuir [41], Freundlich [42] and Dubinin-Radushkevich (D-R) [43], were used for describing the sorption of MV onto the adsorbent.

The Langmuir isotherm is the most commonly used isotherm model which assumes that adsorption occurs homogeneously on the surface of the adsorbent resulting in monolayer and no further adsorption can occur once the adsorption site is occupied.

The equation of the Langmuir isotherm is as follows:
$$ \frac{{C_{e} }}{{q_{e} }} = \frac{1}{{K_{L} q_{m} }} + \frac{{C_{e} }}{{q_{m} }} $$
(11)
where q m is the maximum monolayer adsorption capacity of the adsorbent (mg g−1), and K L is the Langmuir adsorption constant (L mg−1) which is related to the free energy of adsorption.
The separation factor (R L ) is a dimensionless constant which is an essential characteristic of the Langmuir model. The equation of R L is expressed as:
$$ R_{L} = \frac{1}{{\left( {1 + K_{L} C_{o} } \right)}} $$
(12)
where C o (mg L−1) is the highest initial dye concentration. R L indicates if the isotherm is unfavourable (R L  > 1), linear (R L  = 1), favourable (0 < R L  < 1), or irreversible (R L  = 0).

The Freundlich isotherm model assumes multilayer coverage of adsorbate onto the adsorbate-saturated adsorbent surface.

The Freundlich isotherm equation is as follows:
$$ \ln \,q_{e} = \frac{1}{{n_{F} }} \ln \, C_{e} + \ln \,K_{F} $$
(13)
where K F (mg1−1/n L1/n g−1) is the adsorption capacity of the adsorbent and \( n_{F} \) (Freundlich constant) indicates the favourability of the adsorption process. The adsorption process is considered favourable if 1 < n F  < 10.
D-R isotherm assumes no homogenous surface of the adsorbent and is temperature-dependent. The equation is as followed:
$$ \ln \, q_{e} = \ln \, q_{m} - K_{DR}^{2} $$
(14)
where q m is the saturation capacity (mg g−1), K DR is a D-R constant (mol2 kJ−2), and ε is the D-R isotherm constant which is also known as the Polanyi potential.
The D-R isotherm constant, ε, is expressed as:
$$ \varepsilon = RT \ln \left[ {1 + \frac{1}{{C_{e} }}} \right] $$
(15)
where R is the gas constant (8.314 × 10−3 kJ mol−1 K−1) and T is temperature (K).
The mean free energy, E (kJ mol−1), of the sorption per molecule of adsorbate is obtained from K DR , and the equation is expressed as:
$$ E = \frac{1}{{\sqrt {2K_{DR} } }} $$
(16)

The linear plots of the Langmuir, Freundlich and D-R isotherm were obtained by plotting:

C e /q e versus C e , ln q e versus ln C e , and ln q e versus ε 2, respectively.

The parameters of the isotherm models and the error analysis are summarised in Table 3. It can be observed that the R 2 value is the highest for Langmuir isotherm when compared with Freundlich and D-R isotherm models for all the temperature. Moreover, the error analysis functions (χ 2, EABS, ARE and MSDP) of the Langmuir isotherm also displayed the smallest values, which indicate that the q e,cal of the Langmuir isotherm is closest to the q e,exp. Therefore with consideration of the R 2 and the error functions, it is concluded that the Langmuir isotherm best fitted the experimental data.
Table 3

Parameters of the Langmuir, Freundlich and Dubinin-Radushkevich isotherm and the error functions analysis

Langmuir isotherm

 T (K)

298.15

308.15

318.15

328.15

338.15

 q m (mg g−1)

194.2

234.3

280.4

291.3

323.4

 K L (L mg−1)

0.066

0.056

0.049

0.048

0.041

 R L

0.014

0.017

0.023

0.022

0.023

 R 2

1.000

0.994

0.997

0.995

0.990

 χ 2

20.2

18.6

27.5

45.0

37.6

 EABS

77.4

98.9

101.9

156.4

141.0

 ARE

14.2

17.9

20.7

20.8

21.7

 MSDP

36.1

36.2

34.4

29.6

38.5

Freundlich isotherm

 K F (mg1−1/n L1/n g−1)

19.3

18.6

17.4

20.0

18.6

 n F

2.515

2.163

2.026

1.944

1.830

 R 2

0.818

0.852

0.853

0.862

0.855

 χ 2

160.6

181.4

166.6

185.8

261.1

 EABS

307.0

399.4

391.0

408.9

476.0

 ARE

31.7

39.6

40.5

37.8

41.1

 MSDP

63.7

62.7

62.9

56.4

64.8

Dubinin-Radushkevich isotherm

 q m (mg g−1)

104.8

165.8

175.7

163.4

197.6

 K DR (mol2 kJ−2)

0.274

0.281

0.274

0.131

0.191

 E (kJ mol−1)

1.350

1.334

1.352

1.952

1.618

 R 2

0.793

0.917

0.948

0.831

0.894

 χ 2

1326.6

2335.0

3058.8

3878.2

4784.9

 EABS

803.7

789.2

822.4

1006.1

1095.5

 ARE

163.3

231.4

270.6

302.1

328.9

 MSDP

263.8

422.3

494.0

562.7

621.3

The R L values of the Langmuir isotherm for all the temperatures are between 0 and 1, which indicated that the adsorption process between MV and AP is favourable.

The low values of K F from the Freundlich isotherm and the low q m and E predicted from the D-R isotherm were probably due to the poor fitting of the experimental data.

The predicted q m from the Langmuir model at ambient temperature is 194.2 mg g−1, while at 65 °C the value increased to 323.4 mg g−1, which could be due to the swelling of the adsorbent particle that lead to an increase in surface area at higher temperature [44]. As summarised in Table 4, AP is a better adsorbent for removal of MV than many of the agricultural residues, but its adsorbent capacity is lower when compared to Pu-erh tea, duckweed (a floating aquatic macrophyte) and synthetic adsorbent (Fe3O4 magnetic nanoparticle) at ambient temperature.
Table 4

Comparison of q m for MV adsorption by various adsorbent

Adsorbent

q m (mg g−1)

T (oC)

Reference

Azolla pinnata (AP)

194.2

Ambient

This work

AP

234.3

35

This work

AP

280.4

45

This work

AP

291.3

55

This work

AP

323.4

65

This work

Rice hull char

48.7

Ambient

[9]

Soybean straw char

70.4

Ambient

[9]

Acid modified activated carbon

83.3

30

[45]

Peanut straw char

101.0

Ambient

[9]

Artocarpus odoratissimus fruit skin

137.3

Ambient

[13]

Casuarina equisetifolia needle

165.0

Ambient

[7]

Water lettuce

267.6

Ambient

[46]

Pu-erh tea

285.7

Ambient

[47]

Duckweed (Lemna minor)

332.5

Ambient

[48]

Fe3O4 magnetic nanoparticle

416.7

Ambient

[49]

Thermodynamic Studies

Thermodynamic parameters such as the Gibbs free energy (∆G o), enthalpy (∆H o) and entropy (∆S o) were investigated by studying the adsorption process at temperature of 25, 35, 45, 55 and 65 °C.

The Van’t Hoff equation was used to calculate the thermodynamic parameters which are expressed as:
$$ \Delta G^{O} = \Delta H^{O} - T\Delta S^{O} $$
(17)
The Gibbs free energy is expressed as:
$$ \Delta G^{O} = - RT\,{\text{ln }}K $$
(18)
$$ K = \frac{{C_{s} }}{{C_{e} }} $$
(19)
where K is the distribution coefficient for adsorption, C S is the adsorbate concentration adsorbed by AP after equilibrium (mg L−1), C e is the adsorbate concentration remaining in solution after equilibrium (mg L−1), R is the gas constant (J mol−1 K−1) and T is the temperature (K).
By integrating Eq. (18) into (17), the following equation is obtained:
$$ \ln K = \frac{{\Delta S^{o} }}{R} - \frac{{\Delta H^{o} }}{RT} $$
(20)

The values of ∆H o and ∆S o can be obtained from the linear plot of ln K versus T −1.

The calculated ∆G° were −7.11, −8.21, −9.16, −9.76 and −10.39 kJ mol−1 for 25, 35, 45, 55, and 65 °C, respectively. Increasing temperature resulted in more negative Gibbs energy which indicate the adsorption process of MV into AP is more spontaneous at higher temperature. The ∆H° was 17.2 kJ mol−1 and the positive value indicate that the adsorption process is endothermic, where heat is gained from the surroundings. The ∆S° value was 0.08 kJ mol−1 K−1 where the positive value indicates an increase in randomness at the solid–liquid interface during the process. Positive ∆S° value also indicates possibility of significant change in the internal structure of the adsorbent [50, 51].

The activation energy (E a ) of the adsorption process is calculated by using the Arrhenius equation, which is expressed as:
$$ \ln K_{2} = \ln A - \frac{{E_{a} }}{RT} $$
(21)
where K 2 is the pseudo 2nd order rate constant (g mg−1 min−1), A is the Arrhenius factor, R is the gas constant, T is temperature (K) and E a is the activation energy (kJ mol−1).

E a was estimated from the linear plot of ln K 2 versus T −1, where value between 5 and 40 kJ mol−1 indicates physical sorption process, while 40–800 kJ mol−1 indicates a chemical sorption process [27]. K 2 values obtained for the removal of 100 mg L−1 MV at temperature of 25, 35, 45, 55 and 65 °C were 0.003, 0.005, 0.013, 0.025 and 0.034 g mg−1 min−1, respectively. The value of E a was found to be 54.8 kJ mol−1, which indicates that the adsorption process may be controlled by chemical process.

Regeneration

To further investigate the capability of AP as adsorbent for MV removal, the regeneration experiment was carried out. The result of the regeneration experiment is summarised in Fig. 7.
Fig. 7

Regeneration experiment of AP washed with three different solvent: Distilled water, 0.1 M HNO3 and 0.1 M NaOH. Cycle 0 represents the MV removed by the AP prior to the washing

Water and acid washing showed gradual reduction in removal of MV with every progressive cycle while only a small variation was observed for washing with NaOH. At the fifth cycle, water and acid washing resulted in MV removal of 47.1 and 51.2 %, respectively, while NaOH-washing resulted in 92.0 % removal when compared to the original removal at 95.9 %. The overall regenerative performance by water and acid washing varied very little and NaOH resulted in the highest regeneration capability of the adsorbent. The reason NaOH successfully regenerated the absorbent may be due to the removal of natural fats, waxes and low molecular weight lignin compounds from the surface of the adsorbent by the base while exposing chemical-reactive functional groups, such as the hydroxyl groups, which may be responsible for removal of dye molecules.

Pre-treatment of Adsorbent

Pre-treatment of adsorbents have been known to enhance their adsorption capacity towards dyes [25]. Here, AP was subjected to various treatment in order to investigate if such chemical treatment could enhance its adsorption capacity towards MV dye. The q e of untreated, oxalic acid, citric acid, phosphoric acid and NaOH-treated adsorbent were 79.8, 47.9, 46.4, 45.6 and 71.3 mg g−1, respectively, where the untreated adsorbent lead to the highest dye removal. Modification with NaOH yielded almost similar q e with untreated AP, which may be due to exposure of favourable chemical-active groups for removal of MV as explained in the regeneration section. Modification with the acids did not improve the removal of MV, and it may be due to the removal of certain soluble organic compounds [52] that favour the removal of MV. It was reported that not all modifications of adsorbent lead to higher adsorption capacities [53].

Conclusions

The capability of AP as a potential adsorbent for the removal of MV was studied in a batch adsorption system. The optimum adsorbent dosage was 0.04 g/20 mL dye and the contact time to reach equilibrium was approximately 120 min. Optimum pH for the removal of MV is 4.0, however, no pH adjustment was made in the rest of the experiments as the removal between pH 4.0 and the ambient pH are comparable. The study of pH and ionic strength indicate that electronic interaction and hydrophobic–hydrophobic interaction may be the major forces of dye interaction. Pseudo 2nd order model best fit the kinetic data which suggested that the adsorption process was governed by chemical process. Weber-Morris model indicated that the rate-limiting step of the diffusion mechanism was not intraparticle diffusion, while the Boyd model suggested film diffusion may be the rate-limiting step or in combination of other mechanisms. The Langmuir isotherm best-fitted the experimental data with q m of 194.2 mg g−1 at 25 °C and 323.4 mg g−1 at 65 °C, thus the increase in temperature leads to significant improvement of dye absorption. Thermodynamic studies showed that the adsorption process is endothermic, spontaneous and has significant changes to the internal structure of adsorbent. The estimated activation energy determined using the Arrhenius equation is 54.8 kJ mol−1, which indicates that the adsorption process may be controlled by chemical process. While regeneration experiment showed that NaOH managed to regenerate the adsorbent with the retention of high adsorption capability almost similar to the unused adsorbent after five cycles. Modifications of adsorbent with various chemical reagents, showed that untreated AP still lead to the highest removal of dye.

Notes

Acknowledgments

The authors would like to thank the Government of Brunei Darussalam and the Universiti Brunei Darussalam for their financial support and Centre for Advanced Material and Energy Sciences (CAMES) of Universiti Brunei Darussalam for the use of XRF. A special thank to Dr H.M Thippeswamy of the Department of Agriculture (Soil and Plant Nutrition unit), Ministry of Industrial and Primary Resource, Brunei Darussalam for the provision of the Azolla pinnata sample.

References

  1. 1.
    Rajeshwarisivaraj, Sivakumar, S., Senthilkumar, P., Subburam, V.: Carbon from Cassava peel, an agricultural waste, as an adsorbent in the removal of dyes and metal ions from aqueous solution. Bioresour. Technol. 80, 233–235 (2001)CrossRefGoogle Scholar
  2. 2.
    Rahchamani, J., Mousavi, H.Z., Behzad, M.: Adsorption of methyl violet from aqueous solution by polyacrylamide as an adsorbent: isotherm and kinetic studies. Desalination 267, 256–260 (2011)CrossRefGoogle Scholar
  3. 3.
    Srinivasan, A., Viraraghavan, T.: Decolorization of dye wastewaters by biosorbents: a review. J. Environ. Manage. 91, 1915–1929 (2010)CrossRefGoogle Scholar
  4. 4.
    Slokar, Y.M., Le Marechal, A.M.: Methods of decoloration of textile wastewaters. Dyes Pigments 37, 335–356 (1998)CrossRefGoogle Scholar
  5. 5.
    Wang, Z., Xue, M., Huang, K., Liu, Z.: Textile dyeing wastewater treatment. In: Hauser, P.J. (ed.) Advances in treating textile effluent, pp. 5–116. InTech, Rijeka (2011)Google Scholar
  6. 6.
    Rafatullah, M., Sulaiman, O., Hashim, R., Ahmad, A.: Adsorption of methylene blue on low-cost adsorbents: a review. J. Hazard. Mater. 177, 70–80 (2010)CrossRefGoogle Scholar
  7. 7.
    Dahri, M.K., Kooh, M.R.R., Lim, L.B.L.: Removal of methyl violet 2B from aqueous solution using casuarina equisetifolia needle. ISRN Environ. Chem. 2013, 8 (2013)CrossRefGoogle Scholar
  8. 8.
    Lim, L.B.L., Priyantha, N., Tennakoon, D.T.B., Zehra, T.: Sorption characteristics of Peat of Brunei Darussalam. II: interaction of aqueous copper(II) species with raw and processed peat. J. Ecotechnol. Res. 17, 45–49 (2013)Google Scholar
  9. 9.
    Xu, R., Xiao, S., Yuan, J., Zhao, A.: Adsorption of methyl violet from aqueous solutions by the biochars derived from crop residues. Bioresour. Technol. 102, 10293–10298 (2011)CrossRefGoogle Scholar
  10. 10.
    Nawaz, S., Bhatti, H.N., Bokhari, T.H., Sadaf, S.: Removal of Novacron Golden Yellow dye from aqueous solutions by low-cost agricultural waste: batch and fixed bed study. Chem. Ecol. 30, 52–65 (2013)CrossRefGoogle Scholar
  11. 11.
    Sadaf, S., Bhatti, H., Nausheen, S., Noreen, S.: Potential use of low-cost lignocellulosic waste for the removal of direct violet 51 from aqueous solution: equilibrium and breakthrough studies. Arch. Environ. Contam. Toxicol. 66, 557–571 (2014)CrossRefGoogle Scholar
  12. 12.
    Sadaf, S., Bhatti, H.N., Nausheen, S., Amin, M.: Application of a novel lignocellulosic biomaterial for the removal of Direct Yellow 50 dye from aqueous solution: batch and column study. J. Taiwan Inst. Chem. Eng. 47, 160–170 (2015)CrossRefGoogle Scholar
  13. 13.
    Lim, L.B.L., Priyantha, N., HeiIng, C., Khairud, D.M., Tennakoon, D.T.B., Zehra, T., Suklueng, M.: Artocarpus odoratissimus skin as a potential low-cost biosorbent for the removal of methylene blue and methyl violet 2B. Desalin. Water Treat (2013). doi: 10.1080/19443994.2013.852136 Google Scholar
  14. 14.
    Dahri, M.K., Kooh, M.R.R., Lim, L.B.L.: Water remediation using low cost adsorbent walnut shell for removal of malachite green: equilibrium, kinetics, thermodynamic and regeneration studies. J. Environ. Chem. Eng. 2, 1434–1444 (2014)CrossRefGoogle Scholar
  15. 15.
    Sadaf, S., Bhatti, H.: Evaluation of peanut husk as a novel, low cost biosorbent for the removal of Indosol Orange RSN dye from aqueous solutions: batch and fixed bed studies. Clean Technol. Environ. 16, 527–544 (2014)CrossRefGoogle Scholar
  16. 16.
    Sadaf, S., Bhatti, H.N.: Batch and fixed bed column studies for the removal of Indosol Yellow BG dye by peanut husk. J. Taiwan Inst. Chem. Eng. 45, 541–553 (2014)CrossRefGoogle Scholar
  17. 17.
    Sadaf, S., Bhatti, H.N.: Equilibrium modeling for adsorptive removal of Indosol Black NF dye by low-cost agro-industrial waste: batch and continuous study. Desalin. Water. Treat. 52, 4492–4507 (2013)CrossRefGoogle Scholar
  18. 18.
    Conn, H.J.: Biological stains: a handbook on the nature and uses of the dyes employed in the biological laboratory, prepared with the collaboration of various members of the Biological Stain Commission. Biotech Publications, Geneva (1953)Google Scholar
  19. 19.
    Mandal, B., Vlek, P., Mandal, L.: Beneficial effects of blue-green algae and Azolla, excluding supplying nitrogen, on wetland rice fields: a review. Biol. Fert. Soils. 28, 329–342 (1999)CrossRefGoogle Scholar
  20. 20.
    Zehra, T., Priyantha, N., Lim, L.B.L., Iqbal, E.: Sorption characteristics of peat of Brunei Darussalam V: removal of Congo red dye from aqueous solution by peat. Desalin. Water. Treat. (2014). doi: 10.1080/19443994.2014.899929 Google Scholar
  21. 21.
    Tsai, S.C., Juang, K.W.: Comparison of linear and nonlinear forms of isotherm models for strontium sorption on a sodium bentonite. J. Radioanal. Nucl. Chem. 243, 741–746 (2000)CrossRefGoogle Scholar
  22. 22.
    Feng, Y., Dionysiou, D.D., Wu, Y., Zhou, H., Xue, L., He, S., Yang, L.: Adsorption of dyestuff from aqueous solutions through oxalic acid-modified swede rape straw: adsorption process and disposal methodology of depleted bioadsorbents. Bioresour. Technol. 138, 191–197 (2013)CrossRefGoogle Scholar
  23. 23.
    Sajab, M.S., Chia, C.H., Zakaria, S., Khiew, P.S.: Cationic and anionic modifications of oil palm empty fruit bunch fibers for the removal of dyes from aqueous solutions. Bioresour. Technol. 128, 571–577 (2013)CrossRefGoogle Scholar
  24. 24.
    Zhao, J.: Effect of surface treatment on the structure and properties of para-aramid fibers by phosphoric acid. Fibers Polym. 14, 59–64 (2013)CrossRefGoogle Scholar
  25. 25.
    Chieng, H.I., Lim, L.B., Priyantha, N.: Enhancing adsorption capacity of toxic malachite green dye through chemically modified breadnut peel: equilibrium, thermodynamics, kinetics and regeneration studies. Environ. Technol. (2014). doi: 10.1080/09593330.2014.938124 Google Scholar
  26. 26.
    Chieng, H.I., Lim, L.B.L., Priyantha, N.: Sorption characteristics of peat from Brunei Darussalam for the removal of rhodamine B dye from aqueous solution: adsorption isotherms, thermodynamics, kinetics and regeneration studies. Desalin. Water Treat. (2014). doi: 10.1080/19443994.2014.919609 Google Scholar
  27. 27.
    Bekçi, Z., Seki, Y., Cavas, L.: Removal of malachite green by using an invasive marine alga Caulerpa racemosa var. cylindracea. J. Hazard. Mater. 161, 1454–1460 (2009)CrossRefGoogle Scholar
  28. 28.
    Mane, V.S., Babu, P.: Studies on the adsorption of Brilliant Green dye from aqueous solution onto low-cost NaOH treated saw dust. Desalination 273, 321–329 (2011)CrossRefGoogle Scholar
  29. 29.
    Lagergren, S.: Zur Theorie der Sogenannten Adsorption gel Ster Stoffe. K. Sven. Vetenskapsakad. Handl. 24, 1–39 (1898)Google Scholar
  30. 30.
    Ho, Y.S., McKay, G.: Pseudo-second order model for sorption processes. Process Biochem. 34, 451–465 (1999)CrossRefGoogle Scholar
  31. 31.
    Weber, W., Morris, J.: Kinetics of adsorption on carbon from solution. J. Sanit. Eng. Div. 89, 31–60 (1963)Google Scholar
  32. 32.
    Boyd, G.E., Adamson, A.W., Myers Jr, L.S.: The exchange adsorption of ions from aqueous solutions by organic zeolites. II. Kinetics. J. Am. Chem. Soc. 69, 2836–2848 (1947)CrossRefGoogle Scholar
  33. 33.
    Zhao, Y., Yue, Q., Li, Q., Xu, X., Yang, Z., Wang, X., Gao, B., Yu, H.: Characterization of red mud granular adsorbent (RMGA) and its performance on phosphate removal from aqueous solution. Chem. Eng. J. 193, 161–168 (2012)CrossRefGoogle Scholar
  34. 34.
    Özacar, M., Şengil, İ.A.: Application of kinetic models to the sorption of disperse dyes onto alunite. Colloids Surf. A 242, 105–113 (2004)CrossRefGoogle Scholar
  35. 35.
    Maiyalagan, T., Karthikeyan, S.: Film-pore diffusion modeling for sorption of azo dye on to exfoliated graphitic nanoplatelets Indian. J. Chem. Technol. 20, 7–14 (2013)Google Scholar
  36. 36.
    Tavlieva, M.P., Genieva, S.D., Georgieva, V.G., Vlaev, L.T.: Kinetic study of brilliant green adsorption from aqueous solution onto white rice husk ash. J. Colloid Interface Sci. 409, 112–122 (2013)CrossRefGoogle Scholar
  37. 37.
    Hu, Y., Guo, T., Ye, X., Li, Q., Guo, M., Liu, H., Wu, Z.: Dye adsorption by resins: effect of ionic strength on hydrophobic and electrostatic interactions. Chem. Eng. J. 228, 392–397 (2013)CrossRefGoogle Scholar
  38. 38.
    Al-Degs, Y.S., El-Barghouthi, M.I., El-Sheikh, A.H., Walker, G.M.: Effect of solution pH, ionic strength, and temperature on adsorption behavior of reactive dyes on activated carbon. Dyes Pigm. 77, 16–23 (2008)CrossRefGoogle Scholar
  39. 39.
    Samiey, B., Toosi, A.R.: Adsorption of malachite green on silica gel: effects of NaCl, pH and 2-propanol. J. Hazard. Mater. 184, 739–745 (2010)CrossRefGoogle Scholar
  40. 40.
    Tomasino, C.: Chemistry & technology of fabric preparation & finishing. North Carolina State University, NC (1992)Google Scholar
  41. 41.
    Langmuir, I.: The constitution and fundamental properties of solids and liquids. J. Am. Chem. Soc. 38, 2221–2295 (1916)CrossRefGoogle Scholar
  42. 42.
    Freundlich, H.M.F.: Over the adsorption in solution. J. Phys. Chem. 57, 385–471 (1906)Google Scholar
  43. 43.
    Dubinin, M.M., Radushkevich, L.V.: Equation of the characteristic curve of activated charcoal. Proc. Acad. Sci. 55, 327 (1947)Google Scholar
  44. 44.
    Forziati, F.H., Brownell, R.M., Hunt, C.M.: Surface areas of cottons and modified cottons before and after swelling as determined by nitrogen sorption. J. Res. Natl. Bur. Stand. 50, 139 (1953)CrossRefGoogle Scholar
  45. 45.
    Din, A.T.M., Hameed, B.H.: Adsorption of methyl violet dye on acid modified activated carbon: isotherms and thermodynamics. J. Appl. Sci. Environ. Sanit. 5, 161–170 (2010)Google Scholar
  46. 46.
    Lim, L.B.L., Priyantha, N., Chan, C.M., Matassan, D., Chieng, H.I., Kooh, M.R.R.: Investigation of the sorption characteristics of water lettuce (WL) as a potential low-cost biosorbent for the removal of methyl violet 2B. Desalin. Water. Treat. in press, (2015) 1–11Google Scholar
  47. 47.
    Li, P., Su, Y.J., Wang, Y., Liu, B., Sun, L.M.: Bioadsorption of methyl violet from aqueous solution onto Pu-erh tea powder. J. Hazard. Mater. 179, 43–48 (2010)CrossRefGoogle Scholar
  48. 48.
    Lim, L.B.L., Priyantha, N., Chan, C.M., Matassan, D., Chieng, H.I., Kooh, M.R.R.: Adsorption behavior of methyl violet 2B using duckweed: equilibrium and kinetics studies. Arab. J. Sci. Eng. 39, 6757–6765 (2014)CrossRefGoogle Scholar
  49. 49.
    Keyhanian, F., Shariati, S., Faraji, M., Hesabi, M.: Magnetite nanoparticles with surface modification for removal of methyl violet from aqueous solutions. Arab. J. Chem. (2011). doi: 10.1016/j.arabjc.2011.04.012 Google Scholar
  50. 50.
    Alkan, M., Demirbas, Ö., Dogan, M.: Adsorption kinetics and thermodynamics of an anionic dye onto sepiolite. Micropor. Mesopor. Mater. 101, 388–396 (2007)CrossRefGoogle Scholar
  51. 51.
    Daneshvar, E., Kousha, M., Sohrabi, M.S., Khataee, A., Converti, A.: Biosorption of three acid dyes by the brown macroalga Stoechospermum marginatum: isotherm, kinetic and thermodynamic studies. Chem. Eng. J. 195–196, 297–306 (2012)CrossRefGoogle Scholar
  52. 52.
    Yuan, T.-Q., Sun, R.-C.: Chapter 7.3—modification of straw for activated carbon preparation and application for the removal of dyes from aqueous solutions. In: Sun, R.-C. (ed.) Cereal straw as a resource for sustainable biomaterials and biofuels, pp. 239–252. Elsevier, Amsterdam (2010)CrossRefGoogle Scholar
  53. 53.
    Ong, S.-T., Keng, P.-S., Lee, C.-K.: Basic and reactive dyes sorption enhancement of rice hull through chemical modification. Am. J. Appl. Sci. 7, 447 (2010)CrossRefGoogle Scholar

Copyright information

© Springer Science+Business Media Dordrecht 2015

Authors and Affiliations

  • Muhammad Raziq Rahimi Kooh
    • 1
  • Linda B. L. Lim
    • 1
  • Muhammad Khairud Dahri
    • 1
  • Lee Hoon Lim
    • 1
  • J. M. R. Sarath Bandara
    • 1
  1. 1.Faculty of ScienceUniversiti Brunei DarussalamBandar Seri BegawanBrunei

Personalised recommendations