Improved Adsorption Capacity of Nannochloropsis sp. through Modification with Cetyltrimethylammonium Bromide on the Removal of Methyl Orange in Solution

Abstract

In this research, biomass modification of Nannochloropsis sp. with surfactant cetyltrimethylammonium bromide (CTAB) through a cation exchange reaction to produce adsorbent Nannochloropsis sp.-cetyltrimethylammonium bromide (AlgN-CTAB) has been carried out. Biomass modification of Nannochloropsis sp. by CTAB has been successfully carried out through confirmation from the analysis data produced by Fourier-transform infrared spectroscopy (FTIR) and scanning electron microscopy and energy-dispersive X-ray spectroscopy (SEM-EDX). AlgN-CTAB adsorbent has been tested for its adsorption ability against anionic dye of methyl orange (MO) in solution by way of a sequence of experiments by the batch method. The optimum conditions for MO removal from the solution occurred at an adsorbent quantity of 0.1 g, pH of 5, and an interaction time of 60 min. MO adsorption kinetic data by AlgN and AlgN-CTAB tended to take the kinetic model of pseudo-second-order (PSO) with PSO rate constant ( $k_{2}$ ) values of 0.56 and 2.17 g mg^-1 min^-1, serially. The MO adsorption isotherm pattern by AlgN tends to take the Freundlich adsorption isotherm, whereas in AlgN-CTAB it follows the Langmuir and Dubinin-Radushkevich adsorption isotherms. The results of the adsorption-desorption of MO by AlgN-CTAB with 4 repetition cycles resulted in % removal of $MO > 80 %$ . The AlgN-CTAB adsorbent can be used repeatedly and is very effective in absorbing MO in water.

1. Introduction

One of the major problems at this time is water contaminants which are caused by various activities of human life. Increasing technological and industrial advances so far have increased the release of unwanted contaminants like dyes, toxic metals, and pesticides into the surroundings [1, 2]. This waste is generated from the by-products of processing industrial materials such as textiles, tannery, rubber, plastics, food, and cosmetics which can have an impact on the health of living things and their ecosystems [3, 4]. One industry that is often found to produce dangerous contaminants like dyes resulting in toxic chemicals is the industry of textile. Dyestuff waste from the textile industry is a source of contaminants that are often found in the environment. Methyl orange (MO) is a coloring agent which is broadly utilized as a coloring agent in several industrial fields like fabric, leather, paper, and pharmaceutical manufacturing. The majority of the artificial dyes and their derivation products own a high environmental effect, particularly in waters because of their wide application but with poor levels of sewage treatment [5]. Since the dye goes in the wastewater, the blend is more stabilized and complicated to break down because of its complex chemical composition [6]. Dyes are able to lead to a rise in biological oxygen demand (BOD) and can transmit water-borne diseases although they just produce a little share to the amount of organic charge in wastewater [7].

Methyl orange (C₁₄H₁₄N₃NaO₃S) is an anionic coloring agent usually produced by azo compounds and their descendant from the group of benzene. The benzene groups are very difficult to degrade because of their stable structure. Azo compounds are compounds that have the –N=N group called the azo structure and are mostly present in waste. The compounds of azo in case overly lengthy in the surroundings are able to be a resource of illness due to their carcinogenic and mutagenic properties [8–11]. Therefore, it is necessary to reduce this dye in industrial waste, particularly in waste handling prior to its spread to the environment.

Treatment of dye waste such as MO was performed by way of various treatments consisting of coagulation, oxidation, flocculation, ion exchange, and adsorption [12–15]. The method that is quite effective and does not result in by-products which can damage the surroundings in treatment of waste containing dyes from various existing methods is the adsorption process [16, 17]. However, the effectiveness in the adsorption process is strongly influenced by the selection of characteristic and the type of adsorbent to be implemented.

Currently, many adsorbents based on natural materials have been developed, such as algal biomass. Algal biomass is a very effective adsorbent for absorbing organic compound pollutants derived from dyes [18–20]. This is because algal biomass has functional groups that can act as active adsorption sites. From several studies that have been reported, algal biomass and the results of its modification with various supporting matrices are very effective in absorbing positively charged chemical compounds such as metal cations and cationic dyes [21–23], but it is less effective for absorbing anionic compounds. This happens because algal biomass contains active groups such as hydroxyl, amino, sulphate ions, and carboxyl [23, 24] which tend to be negatively charged.

In previous studies, the researchers had increased the biomass adsorption ability of Nannochloropsis sp. to absorb anionic dyes such as MO by modifying the algal biomass using cationic surfactants. Surface modification utilizing cationic surfactants has been shown to be an effective technology for increasing adsorbent adsorption capability. Cationic surfactants can make adsorbents rich in positive charges. Cationic surfactants that have been utilized effectively for an adsorbent surface modified by researchers were polyethylenimine (PEI), dodecylbenzyldimethylammonium chloride, and [3-(2-amino ethyl amino) propyl] trimethoxysilane (APTS) [25–27]. Algae biomass adsorbent is negatively charged by having an active group of alkaline or alkaline earth cation exchangers such as Na⁺, K⁺, or Ca²⁺ ions. The cations that are bound to the negative charge of algae biomass functional groups act like a counterweight to their charge which can be exchanged with other cations such as cationic surfactants [3, 28, 29].

In this research, the adsorption characteristics of the adsorbent from the modified algal biomass of Nannochloropsis sp. with surfactant cetyltrimethylammonium bromide (CTAB) (AlgN-CTAB) were investigated which is cationic to adsorb MO dyes in solution. The increase in the adsorption ability of AlgN-CTAB on MO dyes can be determined by determining the kinetics and adsorption isotherm parameters. Thus, it can be obtained that modified algal biomass adsorbent is effective for application to absorb anionic dyes. Biomass modification increases the ability of algal biomass as a functional material that plays a role in absorbing toxic chemical compounds in chemical waste treatment.

2. Materials and Methods

2.1. Materials

Methyl orange and other chemicals required for the process of algal biomass modification and adsorption such as NaCl, CTAB, HCl, NaOH, citrate, and phosphate buffer are of analytical reagent (AR) grade and purchased based on the European Pharmacopoeia. Algae Nannochloropsis sp. was obtained from cultivation at the Center for Marine Cultivation in Lampung, Indonesia, and prepared into algal biomass in the Inorganic Chemistry Laboratory of FMIPA University of Lampung.

2.2. AlgN and AlgN-CTAB Preparation

Algae Nannochloropsis sp. was prepared to be biomass of Nannochloropsis sp. (AlgN) by drying it to air up to 72 h and in an oven at 40°C for 3 h [2]. Furthermore, 30 g of AlgN was reacted with 400 mL of 1 M NaCl solution in a 500 mL Erlenmeyer flask. After that, the solution was stirred with a shaker for 1 hour. The solution was then kept for 1 day and filtered. The solid produced was cleaned using H₂O to neutral pH and dried at 25°C to give AlgN-Na. Then, 5 g of AlgN-Na was reacted with 500 mL CTAB and stirred for 4 h using a magnetite stirrer at 50°C. The solid produced was neutralized by deionized water, dried at room temperature, and ground by a grinder to be fine with a 100-mesh size to produce AlgN-CTAB.

2.3. Characterization of AlgN and AlgN-CTAB

Characterization of AlgN and AlgN-CTAB was undertaken to analyze the appearance of functional groups by Fourier-transform infrared spectroscopy (FTIR) (Shimadzu Prestige-21 IR, Japan), while identification of surface morphology and elemental constituents was done by scanning electron microscopy with energy-dispersive X-ray spectroscopy (SEM-EDX) (FEI Inspect-S50, USA).

2.4. Analysis of the Point of Zero Charge (pH_pzc) Adsorbent

A total of 0.05 g of adsorbent was put into each beaker glass continued by adding 10 mL of 0.1 M NaNO₃. Furthermore, each solution pH was arranged with a range between 3 and 12. The pH adjustment was done by the addition of 0.1 M hydrochloric acid for acidic conditions and 0.1 M sodium hydroxide for alkaline conditions. The solution was stirred up to 24 h, and the last pH for each solution was observed [21].

2.5. Batch Adsorption Experiment

The ability of the AlgN and AlgN-CTAB adsorbents to absorb MO anionic dyes was investigated by studying the impact of AlgN-CTAB dose, contact time, pH, concentration variations, and the ability to reuse adsorbent. A total of 1 g L^-1 of stock solution of MO was made and further applied to result in the standard solution and initial concentration ([MO]_o) by diluting the stock solution accordingly. All experiments were undertaken at temperatures of 27°C. In the adsorbent dose determination experiment, 25 mL of ${[MO]}_{o} = 10 mg L^{- 1}$ was reacted to the adsorbent with a weight varying between 0.05 and 0.25 g. Furthermore, the optimum adsorbent dose was used in the next adsorption experiment. In the pH effect experiment, [MO]_o was prepared at a pH varying from 3 to 12. The optimum pH obtained was used in the experiment of contact time with time variations between 15 and 120 min. For the concentration effect experiment, the experiments were carried out at optimum pH and time conditions with ${[MO]}_{o} = 0 - 300 mg L^{- 1}$ . The [MO] obtained after the adsorption process was explored by a UV-Vis spectrophotometer with a maximal wavelength of 465 nm (UV-Vis spectrophotometer (Agilent Cary 100, U.S.A)). All experiments in this research were carried out in 3 repetitions. Furthermore, the [MO] dye adsorbed was identified by calculating the MO dye bound per unit mass of adsorbent and the percentage of MO removal was determined using $\begin{matrix} (1) & q_{e} = \frac{(C_{o} - C_{e})}{m} x V, \\ q_{t} = \frac{(C_{o} - C_{t})}{m} x V, \\ R (%) = \frac{(C_{o} - C_{t})}{C_{o}} \times 100, \end{matrix}$

where $C_{o}$ is the concentration in the initial state, $C_{e}$ is the concentration at equilibrium, $C_{t}$ is the concentration at a certain time $t$ of [MO] (mg L^-1), $m$ is the adsorbent mass (g), $V$ is the solution volume (L), $q$ is the amount of MO bound per unit mass (mg g^-1), and $R$ is the percentage of MO removal.

The adsorption data of MO adsorbed by AlgN and AlgN-CTAB were analyzed by determining the correlation between the amount of MO in the adsorbed solution experimentally and the estimation results with the adsorption isotherm of Langmuir (AIML), Freundlich (AIMF), Dubinin-Radushkevich (AIMDR), and Temkin (AIMT). The evaluation was carried out by determining the root mean squared error (RMSE) and chi-square test ( $χ^{2}$ ) [30, 31].

2.6. Regeneration

Reuse of the AlgN-CTAB adsorbent was observed by performing adsorption experiments at optimum conditions. The MO dye that had been adsorbed by AlgN-CTAB was removed again using an eluent in the form of 0.1 M hydrochloric acid (50 mL). The adsorption-desorption processes were undertaken several times, until the % MO adsorption was <80%.

3. Results and Discussion

3.1. Preparation and Characterization of Adsorbents

AlgN-CTAB is an adsorbent based on the algal biomass of Nannochloropsis sp. modified by cation exchange reaction using CTAB surfactant. The procedure for making AlgN-CTAB is shown in Figure 1.

Figure 1

Adsorbent AlgN-CTAB preparation scheme.

AlgN-CTAB was made by uniforming the charge with excess Na⁺ cations using NaCl solution which is aimed at increasing the cation exchange capacity [5]. Ions of Na⁺ contained in the algal biomass of Nannochloropsis sp. were replaced with CTAB surfactant via a cation exchange reaction which produces AlgN-CTAB. Then, the AlgN-CTAB adsorbent was characterized by FTIR for functional group determination and SEM-EDX for surface morphology and elemental investigation.

Figure 2 illustrates that the IR spectrum of AlgN indicates an absorption band at wave number 1613.07 cm^-1 identifying a typical C=O absorption of a carboxylic acid. In addition, the absorption appears at the wave numbers around 2854.85 and 2924.09 cm^-1, respectively, obtained from the –CH₂ symmetrical stretching and asymmetry vibration of a carbon chain (aliphatic) [32, 33]. The absorption at wave number 3695.61 cm^-1 comes from the overlap of the -O-H and -N-H groups. In AlgN-CTAB, all characteristic IR spectra of the algal biomass of Nannochloropsis sp. appeared with the addition of a new absorption at a wavelength of 1465.90 cm^-1 indicating the existence of the CH group which is the methyl group from CTAB [34–36].

Figure 2

IR spectra of AlgN and AlgN-CTAB.

The surface morphology of AlgN-CTAB was explored with SEM coupled with the determination of constituent elements using EDX. SEM characterization provides main information on the surface morphology of adsorbent. In Figure 3(b), it could be investigated that, in AlgN-CTAB, the surface morphology area is wider than that in AlgN (Figure 3(a)) and there are sticky grains which indicate the existence of molecules of CTAB on the surface layer of the algal biomass of Nannochloropsis sp. Cetyltrimethylammonium bromide molecules do not enter the algae but only cover the algal cell walls after surfactant modification [5]. The presence of CTAB on the AlgN surface is also supported by the EDX data in Figure 3(d) which shows the appearance of the Br element derived from CTAB in AlgN-CTAB that did not previously appear in the EDX data from AlgN (Figure 3(c)).

Figure 3

SEM-EDX of (a, c) AlgN and (b, d) AlgN-CTAB.

(b)

(c)

(d)

3.2. Impact of Adsorbent Dosage on Adsorption

Dosage of adsorbent is one of the main parameters in deciding the effective adsorption conditions so that it is economically feasible to use adsorbents for certain purposes. In this research, the impact of the adsorbent dosage was studied using AlgN-CTAB in the range 0.1-0.5 g in 10 mg L^-1 [MO] (25 mL) as displayed in Figure 4.

Figure 4

Impact of adsorbent mass on sorption of MO dye on AlgN-CTAB ( ${[MO]}_{o} = 10 mg L^{- 1}$ , $interaction time = 60 \min$ , and $T = 27^{°} C$ ).

Figure 4 illustrates the impact of the adsorbent dose on the absorption percentage of MO dye which increases by the rise in the adsorbent dosage and the optimum at the particular adsorbent dosage used. This shows that raising the dose of adsorbent applied increases the amount of adsorption sites to absorb MO dye, but the increase in the amount of MO adsorbed is also limited by the amount of adsorbate concentration used. It may be seen in Figure 4 that the optimal AlgN dose is 0.1 g. This dose is used for further trials.

3.3. Impact of Solution Acidity on Adsorption

In this experiment, the impact of pH of MO dye solution on AlgN-CTAB adsorbent was studied in the pH range between 3 and 12. Figure 5 explains that the change in the pH value of the MO dye solution has no impact on the percentage of MO adsorbed by AlgN-CTAB. From these data, it appears that the removal efficiency of MO solution in the pH range 3-12 is more than 96%. This can occur because the interaction between MO dye and AlgN-CTAB occurs through an electrostatic interaction mechanism among the positive charges of AlgN-CTAB and MO dye [37, 38]. The existence of biomass modification with CTAB has increased its ability to absorb anionic dyes. This is supported by % MO which is adsorbed at very low AlgN in all pH ranges. This happens because AlgN is dominated by active groups that are negatively charged, so there is repulsion with MO dye which is negatively charged; as a result, the adsorption process is not optimal.

Figure 5

Impact of pH on the removal of MO dye using AlgN and AlgN-CTAB ( $adsorbent mass = 0.1 g$ , ${[MO]}_{o} = 10 mg L^{- 1}$ , $interaction time = 60 \min$ , and $T = 27^{°} C$ ).

Increasing the $pH value > 6$ indicates a few reductions in adsorption; this is because at higher pH, the increased OH^- ion level will compete with MO dye which is anionic to occupy the active site of the positively charged AlgN-CTAB (Figure 5) [37]. This is also supported by the pH_pzc value of AlgN-CTAB which is 8.0 (Figure 6). The surface charge of the adsorbent is positive as $pH < p H_{pzc}$ , whereas the surface charge is negative as $pH > p H_{pzc}$ [39]. Thus, at $pH < 8$ , the AlgN-CTAB surface is positively charged, making it very effective at absorbing MO dyes that are negatively charged. Based on these considerations, the next experiment was carried out with a pH of 5. At that pH, the AlgN-CTAB adsorbent surface charge is positive while the MO dye adsorbent charge is negative. Thus, under these conditions, the interaction between AlgN-CTAB and MO dye that occurs electrostatically is more optimal.

Figure 6

Investigation of pH_pzc of the AlgN and AlgN-CTAB.

3.4. Impact of Contact Time on Adsorption

In order to observe the impact of contact time, adsorption experiments were done by the MO dye solution at varying contact times between 0 and 120 minutes. The resulting adsorption data is illustrated in Figure 7, and it shows that more than 94% of MO dye was absorbed by AlgN-CTAB in the initial 15 minutes and the adsorption stability period was reached at 60 min. Increasing the contact time of more than 60 minutes apparently did not increase the percentage of MO adsorbed by AlgN and AlgN-CTAB, by about 24.56 and 98.69%, respectively. Therefore, the equilibrium time was used for further experiments.

Figure 7

Impact of interaction time on the removal of MO dye using AlgN and AlgN-CTAB ( $adsorbent mass = 0.1 g$ , ${[MO]}_{o} = 10 mg L^{- 1}$ , $pH = 5$ , and $T = 27^{°} C$ ).

3.5. Adsorption Kinetics

Adsorption kinetic models are applied to identify the dominant mechanisms determining process of adsorption like chemical reactions and mass transfer. In this study, the pseudo-first-order (PFO), pseudo-second-order (PSO), and intraparticle diffusion (IPD) models have been used to explore the adsorption facts shown in Figure 7.

The PFO kinetic model presumes that the adsorption rate of the filled sites is combined by the amount of unfilled sites described by the next linear equation [40]. $\begin{matrix} (2) & \log (q_{e} - q_{t}) = \log q_{e} - \frac{k_{1}}{2.303} t . \end{matrix}$

The PSO kinetic model supposes that the capacity of adsorption is comparable to the amount of active sites that existed on the adsorbent using a linear equation. $\begin{matrix} (3) & \frac{t}{q_{t}} = \frac{1}{k_{2} q_{e}^{2}} + \frac{t}{q_{e}}, \end{matrix}$ where $q_{t}$ and $q_{e}$ (mg g^-1) represent the total MO dye adsorption capacity at period $t$ and at stability, serially, and $k_{1}$ and $k_{2}$ describe the rate constants of the PFO and PSO, serially. The facts of data analysis from the two adsorption kinetic patterns are described in Figure 8 and listed in Table 1.

Figure 8

Linearized (a) PFO and (b) PSO kinetic models on adsorption of MO dye.

(b)

Table 1

Kinetic parameters for the adsorption of MO dye on AlgN and AlgN-CTAB.

Adsorbents	PFO				PSO
Adsorbents	$q_{e (\exp)}$ (mg g^-1)	$q_{e (cal)}$ (mg g^-1)	$k_{1}$ (min^-1)	$R^{2}$	$q_{e (cal)}$ (mg g^-1)	$k_{2}$ (g mg^-1 min^-1)	$R^{2}$
AlgN	0.609	0.504	0.001	0.324	0.632	0.557	0.983
AlgN-CTAB	2.474	2.960	0.642	0.473	2.477	2.173	0.990

The use of the Morris-Weber kinetic model [41, 42] assumes that the diffusion process of adsorbates such as MO dye to the adsorbent is controlled by a physical mechanism that leads to a main part in the process of adsorption as described in $\begin{matrix} (4) & q_{t} = k_{id} t^{0.5} + C, \end{matrix}$

where $k_{id}$ (mg g⁻¹ min^−0.5) expresses the rate constant of IPD and the value of $C$ (mg g⁻¹) describes a constant representing resistance to mass transfer in limit layer. $k_{id}$ and $C$ were computed by the slope and intercept of stripes that resulted from the graph of $q_{t}$ against $t^{0.5}$ .

Data in Figure 7 were also analyzed with an IPD model that can describe the process of diffusion from the objects absorbed by the adsorbent which could be applied to simulate data of kinetics [43]. The results of the analysis are described in Figure 9 and listed in Table 2. It may be observed in Figure 8(c) that the entire plots contain two linear sections. These patterns show that there is over one adsorption model linked. The initial linear part covers time of adsorption of 0–60 minutes representing the external transfer of mass. The next linear part covers time of adsorption of 60–120 minutes, indicating a pattern depicting intraparticle diffusion. The second linear part does not pass through the origin ( $C \neq 0$ ); this indicates that intraparticle diffusion is not only stage of rate control and external mass transfer but it also occurs in unison [41, 42].

Figure 9

Linearized kinetic model of IPD on adsorption of MO dye.

Table 2

Intraparticle diffusion model for MO dye adsorption onto AlgN and AlgN-CTAB.

Adsorbent	Initial linear portion			Second linear portion
Adsorbent	$k_{i 1}$ (mg g^-1 min^0.5)	$C_{1}$ (mg g^-1)	$R_{1}^{2}$	$k_{i 2}$ (mg g^-1 min^0.5)	$C_{2}$ (mg g^-1)	$R_{2}^{2}$
AlgN	0.054	0.274	0.906	0.022	0.267	0.959
AlgN-CTAB	0.057	2.203	0.935	0.029	2.450	0.923

The results of the analysis of the MO adsorption data by AlgN and AlgN-CTAB using the PFO, PSO, and IPD models are linearly shown in Figures 8 and 9 as well as in Tables 1 and 2. If the value of linear correlation coefficient ( $R^{2}$ ) of the PFO and PSO kinetic models is compared, the $R^{2}$ value in the PSO is greater than that in the PFO kinetic model (Table 1). This indicates that the MO adsorption by AlgN and AlgN-CTAB tends to follow the PSO kinetic model. In addition, the kinetic rate constant of PSO ( $k_{2}$ ) MO by AlgN-CTAB is greater than that by AlgN (Table 1). This can be explained by the modification of the algal biomass of Nannochloropsis sp. with cationic surfactants such as CTAB which can make the adsorbent rich in positive charges [44]. Thus, the MO molecule which is anionic is very suitable for the positively charged AlgN-CTAB conditions for the occurrence of electrostatic interactions. In AlgN, the adsorbent surface is dominated by active sites with negative charges originating from the algal biomass functional group so that there will tend to be a repulsive force with MO molecules which results in a low amount of MO adsorbed.

According to the investigation in Figure 9, there are two stages that describe the transfer of MO from the solution to the adsorbent outer surface and further directional diffusion of the MO to active sites of the adsorbent through pore cavities and active groups, respectively. The mechanism of adsorption is able to be described in two dissimilar manners, namely, diffusion through adsorbent pores and electrostatic interactions in the existence of positive charges of functional groups from the modification of AlgN to AlgN-CTAB [45]. This is in line with the data analysis of the PSO kinetics discussed earlier.

3.6. Impact of MO Concentration on Adsorption

To determine the impact of [MO] on the adsorption capacity of AlgN and AlgN-CTAB and to learn the equilibrium of the adsorption process, adsorption tests at various ${[MO]}_{o} = 0 - 300 mg L^{- 1}$ were carried out. This experimentation was performed in 25 mL of [MO], and other experimental situations like adsorbent mass, initial pH, and contact time were at optimum conditions. Algal biomass modification by Nannochloropsis sp. with CTAB has increased the amount of MO dye adsorbed (Figure 10(b)).

Figure 10

The impact of [MO]_o on the amount of MO adsorbed in (a) AlgN and (b) AlgN-CTAB based on experimental results ( $q_{\exp}$ ) and estimation using the AIML, AIMF, AIMDR, and AIMT equations.

(b)

The increase in $q_{\exp}$ occurred in line with the increase in [MO]_o used. It may be explained that raising the initial concentration of the adsorbate will increase the driving force which decreases the mass transfer resistance between the adsorbent and the adsorption medium. In addition, the increase in $q_{\exp}$ is also related to the competition between active adsorption sites available on the adsorbent [46, 47]. The amount of MO absorbed per gram ( $q_{\exp}$ ) of AlgN and AlgN-CTAB vs. [MO]_o is displayed in Figure 10.

3.7. Adsorption Isotherm

Adsorption isotherm data is the main indicator to know in explaining the adsorption process. The isotherm shows the relationship between the amounts of MO bound by the adsorbent at fixed temperature. The adsorption isotherm patterns that are often utilized in deciding the adsorption parameters are the Langmuir and Freundlich adsorption isotherm models (AIML and AIMF). In addition, the Dubinin-Radushkevich and Temkin models (AIMDR and AIMT) can also be used because they may present extra information consisting of energy and mechanism of adsorption. The products of the MO adsorption information analysis by AlgN and AlgN-CTAB are shown in Table 3. The relationship between [MO]_o and the amount of MO dye bound in AlgN and AlgN-CTAB is according to experimental results ( $q_{\exp}$ ), and estimates using adsorption equations of AIML, AIMF, AIMDR, and AIMT can be seen in Figure 10.

Table 3

Adsorption isotherm parameters of MO dye on AlgN and AlgN-CTAB.

	Adsorbent	AlgN	AlgN-CTAB
	Parameters
Experiment	$q_{\exp}$ (mg g^-1)	25.776	66.422
AIML	$q_{m}$ (mg g^-1)	5.044	76.479
	$K_{L}$ (L mg^-1)	1.479	5.986
	$R^{2}$	0.702	0.999
	RMSE	6.863	10.47
	$χ^{2}$	24.284	26.145
AIMF	$K_{F}$ ((mg g^-1) (L mg^-1)^1/n)	2.037	16.376
	$n$	0.831	1.585
	$R^{2}$	0.988	0.955
	RMSE	5.743	6.282
	$χ^{2}$	17.218	7.525
AIMDR	$q_{DR}$ (mg g^-1)	20.186	106.933
	$B_{DR} \times 10^{- 6}$	2.524	7.333
	$R^{2}$	0.662	0.999
	RMSE	3.639	3.043
	$χ^{2}$	7.094	1.539
AIMT	$b_{Te} \times 10^{- 2}$ (J mol⁻¹)	2.435	5.223
	$a_{Te} \times 10^{- 2}$ (L g⁻¹)	1.023	1.215
	$R^{2}$	0.832	0.967
	RMSE	3.543	4.961
	$χ^{2}$	2.128	4.133

The AIML presumes that, on the adsorbent surface, there is an amount of active sites which is proportionate toward the uniform surface area of the adsorbent accompanied by a monolayer adsorption process [48, 49]. The linear equation of AIML is displayed in Equation (5), while the AIMF is an empirical equation applied to multilayer adsorption and heterogeneous system [50]. The linear equation of AIMF is shown in Equation (6). $\begin{matrix} (5) & \frac{1}{q_{e}} = \frac{1}{q_{m} K_{L} C_{e}} + \frac{1}{q_{m}}, \\ (6) & \log q_{e} = \log K_{F} + \frac{1}{n} \log C_{e} . \end{matrix}$

The AIMDR has more universal assumptions than the AIML. The AIMDR presumes that the adsorption surface is not homogeneous [51]. The adsorption isotherm equation of this model in linear form is expressed in Equation (7). Meanwhile, the AIMT calculates the complete interaction between adsorbent and adsorbate. The main significant presumption of the AIMT is that the adsorption heat will reduce linearly by the increase in the adsorbent surface coverage [20]. The AIMT linear equation is observed in Equation (8). $\begin{matrix} (7) & \ln q_{e} = q_{DR} - 2 B_{DR} R T \ln (\frac{1 + 1}{C_{e}}), \\ (8) & q_{e} = \frac{R T}{b_{Te}} \ln (K_{Te} C_{e}), \end{matrix}$

where $q_{e}$ (mg g^-1) presents the total of MO bound at condition of equilibrium, $q_{m}$ (mg g^-1) represents the maximal adsorption capacity of MO which indicates the monolayer adsorbent ability to absorb MO, $C_{e}$ (mg L^-1) belongs to the equilibrium [MO], and $K_{L}$ describes the equilibrium constant containing the binding site affinity (L mg^-1). $K_{L}$ and $q_{m}$ may be evaluated from the linear equation graph of $\log 1 / q_{e}$ versus $C_{e}$ which is going to result in a linear line with $1 / q_{m} K_{L}$ as the slope and $1 / q_{m}$ as the intercept. $K_{F}$ presents the factor of the adsorption capacity and $n$ represents the value of the adsorption intensity factor (1-10) [52]. The graph of $\log q_{e}$ against $\log C_{e}$ will yield $K_{F}$ and the exponent $n$ . Furthermore, a constant linked to the adsorption energy is presented by $ε_{DR}$ (the Polanyi potential), the isotherm constants of D-R are displayed by $q_{DR}$ (mg g^-1) and $B_{DR}$ (mol² kJ^-2), serially, the Temkin constant linked to the heat adsorption is presented by $b_{Te}$ (J mol^-1), $R$ belongs to the gas constant (8.314 kJ mol^-1), the equilibrium binding constant is written by $K_{Te}$ (L g^-1), and the absolute temperature is expressed by $T$ (K).

Table 3 explains that in accord with the regression coefficient data ( $R^{2}$ ) of each MO adsorption isotherm model by AlgN and AlgN-CTAB, the MO adsorption process tends to follow the AIML and AIMDR pattern compared to AIMF and AIMT. In both adsorption isotherm models, the value of $R^{2}$ is close to 1. However, when viewed from the RMSE and $χ^{2}$ values, the AIMDR has a smaller value than the AIMF. In addition, in Figure 10, it may be concluded that the plot of the relationship between adsorbed MO to [MO]_o estimated by the AIMDR equation ( $q_{cal ‐ DR}$ ) is relative to the experimental results ( $q_{\exp}$ ).

Relatively, it could be deduced that among the dissimilar isotherm patterns, the AIML and AIMDR can satisfy the experimental data more precisely than AIMF and AIMT. Therefore, it can be stated that the MO adsorption by AlgN-CTAB does not fully occur through chemical or physical interactions, but it is a combination of both [53].

3.8. Regeneration of Adsorbent AlgN-CTAB

The ability to reuse adsorbent needs to be known so that the adsorbent can be of practical use without drastic reduction after reuse. For this reason, the ability to reuse AlgN-CTAB adsorption against MO was performed through a series of repeated adsorption-desorption experiments with MO as seen in Figure 11. The MO adsorption and desorption results using eluent of 0.1 M hydrochloric acid continually for 4 times did not decrease the % removal of MO from 80%. The AlgN-CTAB adsorbent reuse data can be used as a reference that the adsorbent can be used repeatedly and efficiently in absorbing anionic dyes such as MO in aqueous solutions.

Figure 11

Reusability number efficiency of the adsorption of MO on AlgN-CTAB.

3.9. Comparing the AlgN-CTAB Adsorption Capacity to Other Materials

AlgN-CTAB is an adsorbent which is very effective in absorbing MO dyes. This may be observed from the value of $q_{\max}$ which is relatively large in absorbing MO dye contrasted to other adsorbents as seen in Table 4. In addition, the process of making AlgN-CTAB is very simple at a relatively low cost. This is one of the considerations for applying this adsorbent in the treatment of waste containing anionic dyes.

Table 4

Comparing the adsorption capacity of MO on AlgN-CTAB with other adsorbents.

Adsorbent	$q_{\max}$	References
Multiwalled carbon nanotubes	52.86	[54]
Maghemite/chitosan of nanocomposite film	29.41	[55]
Cross-linked chitosan	89.29	[37]
Chitosan/alumina composite	33.00	[56]
Fe-La oxide-coloaded MgO (Fe-La/MgO) nanosheets	30.38	[57]
Modified wheat straw 3.0	50.40	[58]
m-CS/Y-Fe₂O₃/MWCNTs	66.09	[59]
AlgN-CTAB	76.48	This research

4. Conclusions

Biomass modification of Nannochloropsis sp. with CTAB surfactant through cation exchange reaction to produce adsorbent Nannochloropsis sp.-cetyltrimethylammonium bromide (AlgN-CTAB) has been successfully carried out. The ability of the AlgN-CTAB adsorbent to absorb methyl orange (MO) anionic dye is optimum at an $adsorbent mass = 0.1 g$ , $pH = 5$ , $interaction time = 60 \min$ , and ${[MO]}_{o} = 300 mg L^{- 1}$ producing the number of MO bound $(q_{m}) = 76.48 mg g^{- 1}$ . The MO adsorption kinetic data by AlgN-CTAB tend to take the PSO kinetic model, AIML and AIMDR. The results of the adsorption-desorption of MO by AlgN-CTAB with 0.1 M HCl eluent with 4 repetitions of the cycle resulted in % removal of $MO > 80 %$ . Adsorbent modified by Nannochloropsis sp. with CTAB owns a generally great adsorption rate and adsorption capacity confronted to the unmodified biomass. The adsorbent can be used repeatedly to absorb MO anionic dyes in solution.

Footnotes

Data Availability

The data used to support the findings of this study are available from the corresponding author upon request.

Conflicts of Interest

The authors declare that they have no conflicts of interest.

Acknowledgments

This work was funded by Ministry of Education, Culture, Research and Technology (Kemdikbudristek) of the Republic of Indonesia with contract number 120/E4.1/AK.04.PT/2021. The authors thank the Center for Marine Cultivation Development-Lampung (Balai Besar Pengembangan Budi Daya Laut (BBPBDL) Lampung) for participating in this research.

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Improved Adsorption Capacity of Nannochloropsis sp. through Modification with Cetyltrimethylammonium Bromide on the Removal of Methyl Orange in Solution

Abstract

1. Introduction

2. Materials and Methods

2.1. Materials

2.2. AlgN and AlgN-CTAB Preparation

2.3. Characterization of AlgN and AlgN-CTAB

2.4. Analysis of the Point of Zero Charge (pHpzc) Adsorbent

2.5. Batch Adsorption Experiment

2.6. Regeneration

3. Results and Discussion

3.1. Preparation and Characterization of Adsorbents

3.2. Impact of Adsorbent Dosage on Adsorption

3.3. Impact of Solution Acidity on Adsorption

3.4. Impact of Contact Time on Adsorption

3.5. Adsorption Kinetics

3.6. Impact of MO Concentration on Adsorption

3.7. Adsorption Isotherm

3.8. Regeneration of Adsorbent AlgN-CTAB

3.9. Comparing the AlgN-CTAB Adsorption Capacity to Other Materials

4. Conclusions

Footnotes

Data Availability

Conflicts of Interest

Acknowledgments

References

2.4. Analysis of the Point of Zero Charge (pH_pzc) Adsorbent