Removal of Orange G Dye from Aqueous Solution by Adsorption: A Short Review

Journal of Environmental Treatment Techniques

2021, Volume 9, Issue 1, Pages: 318-327

J. Environ. Treat. Tech.

ISSN: 2309-1185

Journal web link: http://www.jett.dormaj.com

https://doi.org/10.47277/JETT/9(1)327

Removal of Orange G Dye from Aqueous Solution

by Adsorption: A Short Review

Saifullahi Shehu Imam , Atika Ibrahim Muhammad , Halimah Funmilayo Babamale ,

Zakariyya Uba Zango³

Department of Pure and Industrial Chemistry, Bayero University, P.M.B 3011, Kano State, Nigeria

Department of Industrial Chemistry, University of Ilorin, P.M.B 1515, Kwara State, Nigeria

Department of Chemistry, Al-Qalam University, P.M.B 2137, Katsina State, Nigeria

Received: 29/08/2020

Accepted: 28/11/2020

Published: 20/03/2021

Abstract

Adsorption is a widely used technique for wastewater remediation. The process is effective and economical for the removal of

various pollutants from wastewater, including dyes. Moreover, Besides commercial activated carbon, different low-cost materials such

as agricultural and industrial wastes are now used as adsorbents. The present review focused on the removal of a teratogenic and

carcinogenic dye, orange G (OG) via adsorption using several adsorbents, together with the experimental conditions and their adsorption

capacities. Based on the information compiled, various adsorbents have shown promising potential for OG removal.

Keywords: Adsorption, Orange G dye, Adsorbents, Wastewater treatment

.1 Toxicity of OG

OG dye has been found to exert hazardous and inevitable

Introduction

Human and animal protection has been disrupted due to

harmful effects on aquatic species and the entire water

environment (4, 11). It has been reported as one of the highly

poisonous anionic dye, which shows so me chromosomal

damage and clastogenic activity (12, 13). Its toxic,

carcinogenic and teratogenic effects to the living organisms

has been attributed to the azo group in its chemical structure

water contamination as a result of numerous pollutants

discharged from various industries (1). Among the most

common contaminants found in the water, those from organic

origins have been found to exert hazardous effects due to their

accumulative and persistent nature in water. Dyes have been

recognized as the most frequent organic pollutants found in the

water due to their wide applications in various industries such

as textile, cosmetics, leather and petrochemical (2). They are

recognized as emerging contaminants due to their resistant

nature of undergoing natural degradations. In fact, United

States Environmental Protection Agency (USEPA) has listed

organic dyes and pigments as hazardous substances (3). Orange

G (OG) belongs to the class of azo dyes of synthetic origin. It

is a form of mono azo and anionic dye, which is soluble in water

and stable at any pH (4). It is usually present as a sodium salt

in two tautomeric forms in aqueous solution, while organic

solvents favour the azo form (5). It has been used for a long

time in United States of America for various applications such

as medication and as a colorant for cosmetics before it was

subsequently abandoned (6). Currently, it is used in textile and

printing industries for dyeing of materials (such as silk and

wool), paper and leather productions etc. (7). Furthermore, OG

is also used in histology in many staining formulations and is

likewise essential to pathologists (8). The colour of OG is due

(

14-16). Not only OG, but the intermediates formed during its

degradation are also toxic too (17). OG is likewise harmful to

plants, flora and fauna (18). Furthermore, for humans, exposure

to OG may result in irritation of the gastrointestinal and

respiratory tract (7). It has also shown genotoxic effects on

experimental animals such as Sw iss albino mice and anaerobic

biomass in aqueous solution (8, 19).

2 Environmental remediations of OG

Owing to the various adverse effects of OG on humans,

aquatic organisms as well as plants, researchers have embarked

on exploring different wastewater remediation techniques for

the removal of this toxic pollutant in the environmental waters.

Various technologies such as coagulation (20), flocculation

(21), bioremediations (22), photocatalytic degradations (23) as

well as physical adsorptions (24) have been reported in

wastewater treatment. The use of physical adsorption has been

highly recognized as an effective wastewater remediation

method due to its promising properties ranging from the

availability of various adsorbent materials, cost-saving,

simplicity of design, flexibility as well as the non-destructive

environmental nature of the method. Moreover, adsorption has

been identified by USEPA as one of the best control methods

(25). As such, this short review is aimed at exploring various

adsorbent materials used for the removal of OG.

to the azo group, while the auxochromes (−푆푂 ,−푂퐻, etc.)

enhances the affinity of the dye (9). The azo bonds are being

adsorbed onto the surface of an adsorbent through a covalent

bond, which makes it more resistant to harsh conditions (10).

The physicochemical properties and molecular structure of OG

are highlighted in Table 1.

Corresponding author: Saifullahi Shehu Imam, Department of Pure and Industrial Chemistry, Bayero University, P.M.B 3011, Kano

State, Nigeria. E-mail: ssimam.chm@buk.edu.ng

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2021, Volume 9, Issue 1, Pages: 318-327

Table 1: Physicochemical properties and molecular structure of OG

Orange G (OG)

7-hydroxy-8-(phenylazo)-1,3-naphthalenedisulfonic acid disodium salt

Acid Orange 10

AO10

Property

Reference

(26)

Chemical formula

Chemical name

Generic name

Abbreviation

C.I.

CAS number

Classification

Colour

C H

2 7

O S

16230

1936-15-8

Azo dye

Orange

475 nm

̶ 4.56

max

Log P (octanol-water)

pKa

Molecular size (Å )

Molecular weight (gmol )

Henry’s law constant

Atmospheric OH rate

constant

11.5

13.08 × 7.53 × 4.98

452.37

-1

5.86E-0.23 atm-m /mole

.49E-0.12 cm /molecule-sec

(29)

Dye content (%)

Melting point

Water solubility

141 °C

5 g/100 mL (20 °C)

(26)

(32)

Chemical structure

(26)

strength, but diminished slightly with increase in temeperature

and initial OG concentration. Maximum adsorption capacity

was found to be 31.25 mg/g and the experimental data fitted

well with the Freundlich adsorption isotherm and pseudo-

second-order Kinetic model. Thermodynamic study revealed

that the adsorption process is spontaneous and exothermic. In a

different study, Kumar, Ahluwalia and Charaya (38) made use

of powdered biomass of Chlorela vulgaris as adsorbent for the

removal of OG dye from aqueous solution. Maximum

performance was recorded using 50 mg/mL biomass dosage.

Optimum pH, temperature and time were found to be 5, 10 ºC

and 10 min. The experimental data fitted the Freundlich

isotherm model (38). Tobacco leaves (TL) were also used by

Mohammed and Al-Mammar (39) as adsorbents for the

removal of OG from aqueous solution. The maximum removal

of OG using TL was recorded at pH of 9 and 10, and adsorption

reaches saturation in 140 min.

Adsorbents used for OG removal

.1 Biomass-based adsorbents

The use of biomass as adsorbents for wastewater

remediation has been widely explored. Biomass is renewable

energy derived from plant and animal organic matter (33). They

offered numerous advantages as an alternative to other

adsorbents used due to their natural occurrence, relative

abundance and existence in various forms, as well as the low-

cost. Various studies have reported the use of several

biosorbents for the biosorption of OG dye. For instance, Ari

and Celik (34) investigated the biosorption potential of both

pristine and hegzadecylethyldimethylammonium bromide

(

HDEDMABr) modified Pyracantha coccinea (P. coccinea)

towards the removal of OG dye from aqueous solution.

Initially, pristine P. coccinea had a biosorption capacity of 4.55

mg/g. However, its capacity increased to 90.16 mg/g after

modification with HDEDMABr. Furthermore, Hsini, Essekri

(

35) prepared a biocomposite (PANI@AS) by coating almond

.2 Activated carbon-based adsorbents

Several studies have reported the use of activated carbon

shell (AS) using polyaniline (PANI) and used as adsorbent for

the removal of OG dye from aqueous solution. The adsorption

of OG dye using PANi@AS reaches equilibrium within 90

min, and the process was spontaneous and endothermic.

The use of modified rice husk char (RHC) using KOH

(

AC) for the removal of OG dye from aqueous solution. In

general, AC is the most widely used sorbent for both

environmental and industrial applications (40). This is due to

its large surface area and ability to adsorb a wide range of

organic compounds (41). Furthermore, any carbonaceous

material of plant or animal origin with high carbon

concentration can be used for the production of AC (42). For

instance, Arulkumar, Sathishkumar (43) studied the

performance of AC prepared via chemical activation of

Thespesia populnea pods using sulphuric acid for the removal

of OG dye from aqueous solution. The maximum adsorption

capacity was found to be 9.129 mg/g and the experimental data

fitted well with the Freundlich isotherm and pseudo-second-

(

KMRHC) as an adsorbent for the removal of OG dye has been

reported by Malik, Khan (36). KMRHC could almost

completely removed OG dye from aqueous solution, as the

removal efficiency reached 96%, in a process that was

spontaneous and exothermic. Also, acid modified wheat husk

was used by Banerjee et al. (37) as an adsorbent for the removal

of OG dye. Low pH was found to enhance the adsorption of

OG dye onto acid-modified wheat husk and equilibrium was

attained within 30 min. The percentage of dye removal was

found to increase with adsorbent dosage, contact time and ionic

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2021, Volume 9, Issue 1, Pages: 318-327

order reaction kinetics model. In the case of Laksaci, Khelifi

combustion method using urea, oxalic acid and citric acid as

fuels. Maximum removal was recorded at pH 4, and the MgO

synthesized using oxalic acid as fuel had the highest adsorption

capacity. The adsorption process was spontaneous and

exothermic.

(

44), raw coffee ground was used as a precursor to prepare AC

for subsequent use as adsorbent for the removal of OG dye. The

AC produced was found to be microporous with a specific

surface area of 1455 m /g, and the adsorption process was

spontaneous and endothermic. Furthermore, Goswami and

Phukan (45) also prepared AC using matured tea leaf

3.5 Layered double hydroxides-based adsorbents

(

MTLAC). Subsequently, the surface of MTLAC was modified

Layered double hydroxides (LDHs) are clay minerals

containing layers of positively charged metal hydroxides and

multivalent anions for neutrality (53). They have a unique

structure, high chemical and thermal stability and could be

synthesized easily (54). Furthermore, due to their low cost, high

surface area, non-toxicity, highly tunable interior architecture

and exchangeable anionic features, studies have reported the

use of LDHs as adsorbents in wastewater remediation (55). For

instance, Abdelkader, Bentouami (6) have reported the use of

by incorporating sulfonic acid to form MTLAC-SA. This

resulted in the decrease of pHpzc value from 5.18 in the case

of MTLAC to 2.48 in the case of MTLAC-SA. Despite such

modification, the adsorption capacity of MTLAC towards OG

dye was still higher than that of MTLAC-SA. Apart from

pristine AC, composites consisting of AC and other adsorbents

have also been used for the removal of OG from aqueous

solution. For instance, Saini, Garg (26) deposited ZnO on AC

to form ZnO-AC nanoparticles for subsequent use as

adsorbents for the removal of OG in bath mode. The

nanoparticles were found to have a maximum adsorption

capacity of 153.8 mg/g for OG, and the adsorption process was

exothermic. Another composite was prepared by Jalali, Rahimi

calcined and uncalcined Mg-Fe-CO

removal of OG dye. The amount adsorbed using calcined Mg-

Fe-CO was much higher than the amount adsorbed using

uncalcined Mg-Fe-CO . Such effect was due to the difference

in adsorption process which might have occurred via ion

exchange mechanism in the case of uncalcined Mg-Fe-CO and

via both surface and ion exchange phenomena in the case of

calcined Mg-Fe-CO

as adsorbent for the

(

2 4

46) via loading SnO /(NH )

-SnCl

-NCs onto AC and used for

the removal of OG. The composite had a pHpzc of 6.0 and was

able to remove up to 97.0% of OG.

.3 Clay-based adsorbents

Several clays have been used as adsorbents for the removal

3.6 Polymer-based adsorbents

Polymers are materials consisting of many repeating units

and have also been used as adsorbents for the removal of

various pollutants including OG dye. For instance, Zhang,

Wang (56) employed the use of pristine and copper modified

poly(m-phenylenediamine) (PmPD) as adsorbents for the

removal of OG dye. Compared to pristine PmPD, the PmPD

of various pollutants, including OG. For instance, Dawood (47)

made use of bentonite as adsorbent for the removal of OG. The

equilibrium time for the adsorption of OG using bentonite was

found to be dependent on the adsorbate concentration. Still, the

percentage removal of OG using bentonite increased with a

decrease in temperature, an indication that the process was

exothermic. Apart from pristine clay, studies have reported the

use of modified clays as adsorbents for the removal of OG. For

instance, Jović-Jovičić, Milutinović-Nikolić (48) modified a

local bentonite using hexadecyl trimethylammoniumbromide

synthesized with Cu was found to have a high surface area.

Such a high surface area resulted in increased performance by

the modified PmPD during adsorption. The equilibrium time

for the adsorption was 180 min, and the isotherm data fitted

well with the Langmuir model, an indication of monolayer

adsorption. The use of surfactants, octadecyl trimethyl

ammonium chloride (OTAC), dioctadecyl dimethyl

ammonium chloride (DDAC), dodecyl trimethyl ammonium

chloride (DTAC) and benzyl hexadecyl dimethyl ammonium

chloride (BHDAC) to enhance the adsorption capacity of

chitosan towards OG dye has been reported by Zhang, Cheng

(57). The adsorption efficiency for OG using the

chitosan/surfactant followed the order: DTAC > DDAC >

OTAC > BHDAC. The maximum removal of OG using

chitosan/DTAC was recorded at pH 3.0, and the removal was

found to decrease with an increase in pH from 3.0 – 10.0.

However, equilibrium was achieved within 240 min, and the

adsorption process was exothermic. In a different study,

magnetic chitosan nanoparticles (MCN) were modified using

ethylenediamine to form EMCN. The adsorption capacity of

EMCN towards OG was higher than that of MCN due to the

higher concentration of active sites in EMCN. Moreover, the

EMCN could be separated easily using a magnet, and the

adsorption process towards OG dye was spontaneous and

exothermic. Another form of modification involves grafting

chitosan onto monomers. For instance, grafted crosslinked

chitosan using N-vinyl-2-pyrrolidone as a monomer. Although

the adsorption capacity of grafted (cts(x)-g-PNVP) towards OG

dye was higher than that of chitosan, however, the adsorption

capacities of both adsorbents were high at low pH due to a

decrease in the number of protonated amines on the adsorbents

with an increase in pH. The low efficiency recorded using the

ungrafted chitosan was due to its high swelling ability, which

makes it very brittle. Furthermore, Konaganti, Kota (58) also

synthesized chitosan-based copolymers by grafting chitosan

(

HDTMA-bromide) to produce HDTMA-bentonite. Compared

to Na-bentonite, the adsorption capacity of HDTMA-bentonite

towards OG was higher. Such performance by HDTMA-

bentonite resulted from the increased affinity of OG due to the

increased hydrophobicity of the bentonite particles. In a

different study, Salam, Kosa (49) modified montmorillonite

nanoclay using octadecylamine. The octadecylamine modified

montmorillonite nanoclay (ODA) had a BET specific surface

area of 16.38 m /g. Adsorption study revealed that the ODA

could remove OG within few minutes with an adsorption

capacity of 39.4 mg/g.

.4 Metal oxides

Various oxides with metal ions have also been used as

adsorbents for the removal of various pollutants, including OG.

For instance, Mondal, Singh (50) made use of hematite (α-

Fe O ) as adsorbent for the removal of OG. The adsorption of

2 3

OG using hematite was found to decrease with increase in pH,

temperature and initial concentration. The adsorption process

was spontaneous and exothermic. In a different study, Gusain,

Dubey (51) made use of nano zirconia (ZrO ) as adsorbent for

the removal of OG. Higher percentage removal was recorded

at pH 2, and the adsorption process was exothermic. Nassar,

Mohamed (16) reported the use of α-Fe O , CoFe O and

2 3 2 4

Co as adsorbents for the removal of OG. Due to electrostatic

attraction at low pH, maximum adsorption using α-Fe

CoFe and Co was recorded at pH 3, 2 and 2. The

adsorption process was endothermic and spontaneous.

Magnesium oxide (MgO) nanostructures have been

synthesized by Nassar, Mohamed (52) via hybrid sol-gel

3 4

O ,

2 3

2 4

3 4

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Journal of Environmental Treatment Techniques

2021, Volume 9, Issue 1, Pages: 318-327

onto a series of poly(alkyl methacrylate)s to produce

ChgPMMA (chitosan grafted poly(methyl methacrylate)),

ChgPEMA (chitosan grafted poly(ethyl methacrylate)),

ChgPBMA (chitosan grafted poly(butyl methacrylate)),

ChgPHMA (chitosan grafted polyhexyl methacrylate)). Both

ungrafted chitosan and the grafted copolymers were

subsequently used as adsorbents for the removal of OG dye.

The grafted polymers were found to exhibit higher adsorption

capacity compared to that of ungrafted chitosan, and adsorption

capacity follows the order ChgPMMA > ChgPEMA >

ChgPBMA > ChgPHMA > ungrafted chitosan. Wu, Wang (59)

also synthesized chitosan/diatomite (CS/DM) membranes by

phase inversion technique. The diatomite was introduced to

improve the mechanical and adsorption properties of CS. The

adsorption capacity of the CS/DM membrane was found to be

dependent on initial OG concentration, pH value, adsorbent

dosage and contact time. The efficiency for the removal of OG

using CS/DM membrane reached 94.0%.

Dulman, Cucu-Man (7) made use of crosslinked acrylic

copolymer functionalized with triethylenetetramine as

adsorbent for the removal of OG. The electrostatic attraction

between the dye anions and the protonated amine groups of the

adsorbent plays a vital role for the system, and the adsorption

process was spontaneous and endothermic. In a different study,

Sandić, Nastasović (60) made use of macroporous

poly(glycidyl methacrylate-coethylene glycol dimethacrylate)

(18) modified sawdust using perchloric acid for use as

adsorbent for the removal of OG dye. The adsorption reaches

equilibrium in 90 min, and the removal percentage decreases

from 78.3 to 36.3% with increase in temperature from 30 to 50

°C, an indication that the process is exothermic. Arzani,

Ashtiani (14) synthesized a carbon mesoporous material

(CMK-3) using SBA-15 silica mesoporous as hard template.

The CMK-3 was considered as a potential candidate for the

removal of OG dye due to its well-ordered mesoporous

structure, high surface area, large pore volume and narrow pore

size distribution. The CMK-3 was found to have a surface area

of 918 m /g and average pore diameter of 3.64 nm. Due to the

protonation of CMK-3 at lower solution pH, its adsorption

capacity towards OG was much higher at low pH. The use of

magnetic biochar derived from the empty fruit bunch (EFB) as

adsorbent for the removal of OG dye has been reported by

Mubarak, Fo (63). The material was reported to possess an

excellent adsorption capacity for the removal of OG dye, and

optimized performance was recorded at pH 2 and contact time

of 120 min. Mesoporous molecular sieves (SBA-3) have also

been used by Anbia, Hariri (64) for the removal of OG. In their

study, SBA-3 was calcined at 550 °C to remove the surfactant

template and produce C-SBA-3. However, it was observed that

the adsorption capability of SBA-3 towards OG dye was higher

than that of C-SBA-3. Such effect was attributed to the polar

groups present on the surface of SBA-3 created by the

surfactant template, which imparted significant adsorption

capacity towards anions to SBA-3.

The use of monoamine modified magnetic silica

(MAMMS) and monoamine modified magnetite-free silica

(MAMPS) as adsorbents for the removal of OG dye from

aqueous solution has been reported by Atia, Donia (65). The

maximum performance using both silica samples was recorded

at pH 3. However, MAMMS showed higher adsorption

capacity towards OG compared to MAMPS. Such performance

by MAMMS was attributed to the thin film of silica that was

formed on the magnetite particles, which increased the number

of exposed active sites available for interaction with OG. In a

different study, Zheng, Zheng (66) made use of quaternary

ammonium group-rich magnetic nanoparticles (MNPs),

Fe3O4@SiO2-MPS-g-DAC (FSMD) synthesized via graft

polymerization, as adsorbent for the removal of OG. FMSD had

a shorter adsorption equilibrium time (20 min) and the main

adsorption mechanism was electrostatic interaction. The

adsorption capacity of FSMD MNPs remained high at pH 2.0

to 7.0, an indication that FMSD MNPs had good affinity to OG

at a wide pH range. The adsorption process was spontaneous

and endothermic. A study aimed at investigating the adsorption

potential of anion exchangers with different functional groups

(Amberlite IRA-900, Amberlite IRA-910, Amberlyst A-21)

towards removing OG dye has been conducted by Greluk and

Hubicki (67). The adsorption capacities of the anion

exchangers towards OG was related to their basicity, as

strongly basic anion exchanger of type 1 (Amberlite IRA-900)

> strongly basic anion exchanger of type 2 (Amberlite IRA-

910) > weakly basic anion exchanger (Amberlyst A-21). The

kinetic measurement showed that the adsorption process was

uniform and rapid.

(

PGME) functionalized with diethylene triamine (PGME-deta)

for the adsorption of OG. Adsorption of OG using PGME-deta

reached 96% at pH 2 but decreased to 5% at pH 11. The dye

sorption was due to the electrostatic attraction between

positively charged amine groups on the PGME-deta surface

and the negatively charged sulfonate groups on OG. Also,

coordination supramolecular polymer [퐶푢(푏푖푝푦)(푆푂 )] , has

푛

been used as adsorbent by Xiao, Xiong (61) for the removal of

a high concentration of OG. The adsorption of OG using

[

퐶푢(푏푖푝푦)(푆푂 )] occurred via ion exchange, and the material

4 푛

displayed high adsorption capacity for the removal of OG.

.7 Other materials

Several other materials have also been used as adsorbents

for the removal of OG dye. For instance, Bhatnagar, Minocha

29) made use of paper mill sludge (a waste material generated

(

from paper industries) as adsorbent for the removal of OG dye.

Maximum percentage removal (75 – 80%) was recorded at pHs

– 4, and the efficiency decreases as the pH increases. Such an

effect was attributed to the electrostatic attraction at low pH and

electrostatic repulsion at high pH. Another waste material from

the sugar industry, bagasse fly ash (BFA) has been used by

Mall, Srivastava (62) as adsorbent for the removal of OG dye

from aqueous solution. BFA was found to have a high surface

area, pore size and pore volume. The removal of OG using BFA

was maximum at acidic pH (pH 3 – 4), and the kinetic study

revealed that the adsorption of OG onto BFA is a gradual

process.

Singh, Banerjee (27) reported the use of raw and modified

(

using sulphuric acid and sodium bicarbonate) sawdust as

adsorbents for the removal of OG dye from aqueous solution.

However, both adsorbents had an appreciable adsorption

capacity towards OG dye, in a process that was spontaneous

and exothermic. In a different study, Banerjee, Chattopadhyaya

Table 2: List of adsorbents used for adsorption studies of OG

Capability

mg/g)

Isotherm

model

Kinetic

model

Adsorbent

Experimental conditions

Ref.

(

Dosage: 0.1 g, volume: 50 mL,

concentration: 10 mg/L, shaking

speed: 150 rpm, temperature: 30 °C

Bagasse fly ash (BFA)

13.79

PSO

(62)

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Journal of Environmental Treatment Techniques

2021, Volume 9, Issue 1, Pages: 318-327

Capability

mg/g)

Isotherm

model

Kinetic

model

Adsorbent

Experimental conditions

Ref.

(29)

(39)

(

Dosage: 0.10 g, volume: 10 mL,

temperature: 25 °C, concentration:

Paper mill sludge

Tobacco leaves (TL)

62.3

PSO

-4

.5 × 10 M

Dosage: 0.25 g, volume: 25 mL,

pH: 10, shaking speed: 110 rpm

Dosage: 0.1 g, volume 100 cm ,

41.66

Monoamine modified magnetic

silica (MAMMS)

temperature: 298 K, concentration:

1.33

8.98

PSO

(65)

-3

48 mg dm , shaking speed: 400

rpm

Dosage: 0.1 g, volume 100 cm ,

Monoamine modified magnetite-

free silica (MAMPS)

temperature: 298 K, concentration:

-3

48 mg dm , shaking speed: 400

rpm

Dosage: 150 mg, volume: 50 mL,

concentration: 300 ppm, pH: 7

Dosage: 150 mg, volume: 50 mL,

concentration: 300 ppm, pH: 7

Dosage: 150 mg, volume: 50 mL,

concentration: 300 ppm, pH: 7

Dosage: 150 mg, volume: 50 mL,

concentration: 300 ppm, pH: 7

Dosage: 150 mg, volume: 50 mL,

concentration: 300 ppm, pH: 7

Dosage: 50 mg, volume: 250 mL,

pH: 7, temperature: 24 °C, initial

concentration: 30 mg/L

Ungrafted chitosan

PSO

(58)

Chitosan grafted poly(methyl

methacrylate)

Chitosan grafted poly(ethyl

methacrylate)

Chitosan grafted poly(butyl

methacrylate)

Chitosan grafted poly(hexyl

methacrylate)

7.2

6.7

0.6

Mesoporous molecular sieves

135.1

0.84

PSO

(64)

(48)

(50)

(

SBA-3)

Dosage: 0.01 g, volume: 0.050

dm3, conc: 50 mg dm-3,

temperature: 25 °C

Na-bentonite

Hexadecyl

trimethylammoniumbromide

Dosage: 0.01 g, volume: 0.050

-3

dm , conc: 50 mg dm ,

temperature: 25 °C

101.42

0.63

(

HDTMA-bromide)

Dosage: 1 g, volume: 50 mL,

concentration: 25 mg/L,

temperature: 303 K

Hematite (α-Fe

2 3

O )

Macroporous poly(glycidyl

methacrylate-coethylene glycol

dimethacrylate) (PGME)

functionalized with diethylene

triamine (PGME-deta)

Dosage: 25 mg, volume: 50 cm³,

temperature: 25 °C

123.9

9.129

PSO

(60)

(43)

Dosage: 0.2 g/25 mL, agitation:

200 rpm, contact time: 300 min,

dye concentration: 10 mg/L.

Dosage: 1 g/L, concentration: 200

mg/L.

Thespesia populnea pods

Uncalcined Mg-Fe-CO

76.4

PSO

(6)

Dosage: 1 g/L, concentration: 200

mg/L.

Calcined Mg-Fe-CO

378.8

Ethylenediamine-modified

magnetic chitosan particles

Dosage: 1 g/L, concentration: 5 ×

10 mmol/L, shaking rate: 200

rpm, temperature: 298 K.

Dosage: 1 g/L, volume: 50 mL, pH:

2, concentration: 2.5 mg/L,

temperature: 308 K

Dosage: 1 g/L, volume: 50 mL, pH:

2, concentration: 2.5 mg/L,

temperature: 308 K

-3

1017

0.24

0.40

(68)

(27)

(

EMCN)

Raw saw dust

Modified saw dust

Dosage: 25 mg, concentration: 240

mg/L, volume: 50 mL, reaction

temperature: 30 °C, reaction time:

poly(m-phenylenediamine)

163.9

387.6

PSO

(56)

180 min.

Dosage: 25 mg, concentration: 240

mg/L, volume: 50 mL, reaction

temperature: 30 °C, reaction time:

Cu - poly(m-phenylenediamine)

180 min.

322

Journal of Environmental Treatment Techniques

2021, Volume 9, Issue 1, Pages: 318-327

Capability

mg/g)

Isotherm

model

Kinetic

model

Adsorbent

Experimental conditions

Ref.

(

Carbon mesoporous material

Dosage: 50 mg, concentration:

1000 mg/L, volume: 25 mL

Dosage: 0.2 g, volume 20 mL,

189

PSO

(14)

(

CMK-3)

Amberlite IRA-900

Amberlite IRA-910

Amberlyst A-21

temperature: 298 K, shaking speed: 1012.62

80 rpm

Dosage: 0.2 g, volume 20 mL,

PSO

(67)

temperature: 298 K, shaking speed: 923.48

PSO

180 rpm

Dosage: 0.2 g, volume 20 mL,

temperature: 298 K, shaking speed: 139.12

PSO

(67)

(69)

(34)

180 rpm

Magnetic graphene oxide

nanocomposite

Pyracantha coccinea modified with

hegzadecylethyldimethylammonium

bromide (HDEDMABr)

Dosage: 1 g/L, pH: 6, temperature:

25 °C, concentration: 60 mg/L

20.85

Dosage: 2.4 g/L, volume: 25 mL,

pH: 4 concentration: 100 mg/L

90.16

Dosage: 20 mg, volume: 100 mL,

concentration: 400 mg/L, pH: 3,

temperature: 293.15 K, shaking

speed: 200 rpm

Dosage: 20 mg, volume: 100 mL,

concentration: 400 mg/L, pH: 3,

temperature: 293.15 K, shaking

speed: 200 rpm

Dosage: 20 mg, volume: 100 mL,

concentration: 400 mg/L, pH: 3,

temperature: 293.15 K, shaking

speed: 200 rpm

Dosage: 20 mg, volume: 100 mL,

concentration: 400 mg/L, pH: 3,

temperature: 293.15 K, shaking

speed: 200 rpm

Activated carbon

Bentonite

555.34

(57)

210.06

128.61

344.76

1270.71

1452.07

Activated clay

Spirulina powder

Chitosan

Dosage: 20 mg, volume: 100 mL,

concentration: 400 mg/L, pH: 3,

temperature: 293.15 K, shaking

speed: 200 rpm

Dosage: 20 mg, volume: 100 mL,

DTAC: 34.10 µM, concentration:

Chitosan/DTAC

PSO

00 mg/L, pH: 3, temperature:

93.15 K, shaking speed: 200 rpm

Dosage: 2 g/L, pH: 2,

concentration: 15 mg/L

Dosage: 20 mg/40 mL,

concentration: 500 mg/L

Dosage: 1.00 g, pH: 2, agitation

speed: 125 rpm, contact time: 120

min

Cerium dioxide nanoparticles

33.33

1333

(70)

(61)

[

퐶푢(푏푖푝푦)(푆푂 )]

PSO

푛

Magnetic biochar

32.36

PSO

(63)

Dosage: 20 g/L, volume: 50 mL,

pH: 2, concentration: 50 mg/L,

shaking speed: 100 rpm

Dosage: 5 g/L, volume: 100 mL,

pH: 2, agitation speed: 200 rpm

Sawdust modified with perchloric

acid

5.48

PFO

PSO

(18)

(37)

(7)

Modified wheat husk

31.25

1218

Crosslinked acrylic copolymer

functionalized with

triethylenetetramine

Chitosan/diatomite (CS/DM)

membrane

Dosage: 0.25 g, volume: 100 mL,

pH: 2, temperature: 323 K.

NLL

Dosage: 8 mg, concentration: 200

mg/L, pH: 3

Dosage: 30 mg/50 mL, pH: 3,

concentration: 50 mg/L,

588

(59)

(71)

3 4

O /MIL-101(Cr)

200

temperature: 298 K.

Dosage: 2 g/L, concentration: 50

ppm, volume: 50 mL, steering

speed: 90 rpm, temperature: 30 °C

Nano zirconia (ZrO

)

(51)

323

Journal of Environmental Treatment Techniques

2021, Volume 9, Issue 1, Pages: 318-327

Capability

mg/g)

Isotherm

model

Kinetic

model

Adsorbent

Experimental conditions

Ref.

(

Dosage: 0.02 g/50 mL, pH: 2,

concentration: 50 mg/L,

ZnO-AC

153.8

PSO

(26)

temperature: 343 K.

Dosage: 0.05 g, volume: 50 mL,

concentration: 50 mg/L, pH: 3,

steering speed: 400 rpm,

α-Fe

62.0

PSO

(16)

temperature: 25 °C

Dosage: 0.05 g, volume: 50 mL,

concentration: 50 mg/L, pH: 2,

steering speed: 400 rpm,

CoFe

52.3

33.3

PSO

temperature: 25 °C

Dosage: 0.05 g, volume: 50 mL,

concentration: 50 mg/L, pH: 2,

steering speed: 400 rpm,

3 4

Co O

temperature: 25 °C

Matured tea leaf activated carbon

MTLAC)

Sulfonic acid functionalized

MTLAC (MTLAC-SA)

Dosage: 1 g/L, concentration: 200

mg/L, temperature: 303 K.

Dosage: 1 g/L, concentration: 200

mg/L, temperature: 303 K

Dosage: 20 mg, volume: 20 mL,

pH: 8, concentration: 50 mg/L,

temperature: 296 K

18.5

05.7

PSO

(45)

(

Octadecylamine modified

montmorillonite nanoclay (ODA)

39.4

19.3

11.8

21.5

18.1

PSO

(49)

(52)

Magnesium oxide (MgO)

synthesized using urea as fuel and

calcined at 550 °C

Magnesium oxide (MgO)

synthesized using urea as fuel and

calcined at 800 °C

Magnesium oxide (MgO)

synthesized using oxalic acid as fuel

and calcined at 550 °C

Magnesium oxide (MgO)

synthesized using oxalic acid as fuel

and calcined at 800 °C

Dosage: 0.05 mg, volume: 25 mL,

pH: 4, temperature: 25 °C

Dosage: 0.05 mg, volume: 25 mL,

pH: 4, temperature: 25 °C

Dosage: 0.05 mg, volume: 25 mL,

pH: 4, temperature: 25 °C

Dosage: 0.05 mg, volume: 25 mL,

pH: 4, temperature: 25 °C

Magnesium oxide (MgO)

synthesized using citric acid as fuel

and calcined at 800 °C

Dosage: 0.05 mg, volume: 25 mL,

pH: 4, temperature: 25 °C

16.5

PSO

(52)

(46)

Dosage: 0.015 g, volume: 50 mL,

pH: 6, concentration: 10 mg/L

Dosage: 2 g/L, pH: 4,

2 4

SnO /(NH )

-SnCl

-NCs-AC

83.34

Rice husk char (RHC) modified

using KOH (KMRHC)

concentration: 80 mg/L,

temperature: 303 K, agitation

speed: 250 rpm

38.8

PSO

(36)

Dosage: 1 g/L, pH: 2.5,

concentration: 50 mg/L,

temperature: 303 K

Dosage: 50 mg, volume: 50 mL,

concentration: 25 mg/L,

temperature: 318 K

γ-alumina

50.1

100

PSO

(72)

(44)

Activated carbon prepared using

raw coffee ground

Dosage: 0.1 g, concentration: 50

mg/L, pH 5

Dosage: 0.1 g, concentration: 50

mg/L, pH 3

Ungrafted chitosan

1.7

PSO

(73)

Grafted chitosan (cts(x)-g-PNVP)

63.7

Dosage: 10 mg, volume: 10 mL,

concentration: 200 mg/L, pH: 3,

shaking speed: 200 rpm,

temperature: 318 K

Quaternary ammonium group-rich

magnetic nanoparticles (MNPs),

Fe O @SiO -MPS-g-DAC (FSMD)

3 4 2

109.1

PSO

(66)

Dosage: 2 mg, volume: 10 mL,

temperature: 298 K, pH: 3

Dosage: 0.5 g/L, concentration: 50

mg/L, pH: 5

Crossed-linked porous polyimide

Polyaniline coated almond shell

833.33

PSO

(74)

(35)

190.98

(

PANI@AS)

Key: L = Langmuir, F = Freundlich, T = Temkin, RP = Redlich-Peterson, NLL = Non-linear Langmuir, PFO = Pseudo first order, PSO = Pseudo second

order

324

Journal of Environmental Treatment Techniques

2021, Volume 9, Issue 1, Pages: 318-327

Garba ZN, Zango ZU, Babando A, Galadima A. Competitive

adsorption of dyes onto granular activated carbon. J Chem Pharm

Res. 2015;7:710-7.

Ghosh JP, Achari G, Langford CH. Design and evaluation of a UV

LED photocatalytic reactor using anodized TiO2 nanotubes. Water

Environment Research. 2016;88(8):785-91.

Limitations

The use of physical adsorption has been highly recognized

as an effective wastewater remediation method due to its

promising properties. Notwithstanding, certain issues still need

to be addressed. For instance, adsorbent capacity progressively

deteriorates as the number of cycles increases, and the spent

adsorbent may be considered as hazardous waste. Furthermore,

the risk of explosion between contaminants and adsorbents also

exists (75).

4. Gan G, Liu J, Zhu Z, Yang Z, Zhang C, Hou X. A novel magnetic

nanoscaled Fe3O4/CeO2 composite prepared by oxidation-

precipitation process and its application for degradation of orange

G in aqueous solution as Fenton-like heterogeneous catalyst.

Chemosphere. 2017;168:254-63.

Kyriakopoulos J, Kordouli E, Bourikas K, Kordulis C,

Lycourghiotis A. Decolorization of Orange-G aqueous solutions

Conclusions and future perspectives

The present study showed various adsorbents that have

over

C60/MCM-41

photocatalysts.

Applied

Sciences.

been used by numerous researchers in the treatment of

wastewater contaminated by OG dye. Based on the literature

survey, it is clear that adsorption of OG dye can be achieved

using different materials such as activated carbons, biomass,

layered double hydroxides, polymers, clays, metal oxides and

many others. Although pristine adsorbents were found to

effective, however, various researchers have modified pristine

adsorbents using different approaches for better removal

efficiency. Most studies have reported high removal efficiency

at low pH values and low removal efficiency at high pH values.

The OG dye removal process in most cases was found to follow

the Langmuir isotherm. Moreover, the kinetics data for the

adsorption of OG dye onto various adsorbents, usually follows

the pseudo-second-order kinetics model, and the adsorption

capacity ranged from 0.24 – 1452.07 mg/g. Finally, based on

the information compiled, adsorption is an effective technique

for the removal of OG dye from aqueous solutions, and various

low-cost and abundantly available materials including biomass,

clays and industrial wastes have shown good capability for the

removal of OG dye. Notwithstanding, to promote the industrial

application of adsorption technique, future researches are

encouraged to focus on the use of immobilized adsorbents due

to their convenient recovery. Also, mixed pollutant effluents

should be used in assessing the capacity of adsorbents. In

addition, most researches are usually conducted in a laboratory-

scale using synthetic wastewater. Thus, much attention should

be given to treating real wastewater samples via adsorption

techniques. Moreover, it is essential to assess the ecotoxicity of

various adsorbents before their widespread application.

2019;9(9):1958.

Abdelkader NB-H, Bentouami A, Derriche Z, Bettahar N, De

Menorval L-C. Synthesis and characterization of Mg–Fe layer

double hydroxides and its application on adsorption of Orange G

from aqueous solution. Chemical Engineering Journal.

011;169(1-3):231-8.

Dulman V, Cucu-Man S-M, Bunia I, Dumitras M. Batch and fixed

bed column studies on removal of Orange G acid dye by a weak

base functionalized polymer. Desalination and Water Treatment.

2016;57(31):14708-27.

Dulman V, Cucu-Man SM, Olariu RI, Buhaceanu R, Dumitraş M,

Bunia I. A new heterogeneous catalytic system for decolorization

and mineralization of Orange G acid dye based on hydrogen

peroxide and

a macroporous chelating polymer. Dyes and

Pigments. 2012;95(1):79-88.

Wang Y, Priambodo R, Zhang H, Huang Y-H. Degradation of the

azo dye Orange G in a fluidized bed reactor using iron oxide as a

heterogeneous photo-Fenton catalyst. RSC

2015;5(56):45276-83.

Advances.

0. Singh J, Uma SB, Sharma YC. A Very Fast Removal of Orange G

from its Aqueous Solutions by Adsorption on Activated Saw Dust:

Kinetic Modeling and Effect of Various Parameters. Rem.

012;5(10):15.

1. Pereira GF, El-Ghenymy A, Thiam A, Carlesi C, Eguiluz KI,

Salazar-Banda GR, et al. Effective removal of Orange-G azo dye

from water by electro-Fenton and photoelectro-Fenton processes

using a boron-doped diamond anode. Separation and Purification

Technology. 2016;160:145-51.

2. Li Y, Yang Z, Zhang H, Tong X, Feng J. Fabrication of sewage

sludge-derived magnetic nanocomposites as heterogeneous

catalyst for persulfate activation of Orange G degradation.

Colloids and Surfaces A: Physicochemical and Engineering

Aspects. 2017;529:856-63.

3. Tarkwa J-B, Oturan N, Acayanka E, Laminsi S, Oturan MA.

Photo-Fenton oxidation of Orange G azo dye: process optimization

and mineralization mechanism. Environmental Chemistry Letters.

Ethical issue

Authors are aware of, and comply with, best practice in

publication ethics specifically with regard to authorship

019;17(1):473-9.

4. Arzani K, Ashtiani BG, Kashi AHA. Equilibrium and kinetic

adsorption study of the removal of Orange-G dye using carbon

(

avoidance of guest authorship), dual submission, manipulation

of figures, competing interests and compliance with policies on

research ethics. Authors adhere to publication requirements

that submitted work is original and has not been published

elsewhere in any language.

mesoporous material. 无机材料学报. 2012;27(6).

5. Nassar MY, Ali AA, Amin AS. A facile Pechini sol–gel synthesis

of TiO2/Zn2TiO2/ZnO/C nanocomposite: an efficient catalyst for

the photocatalytic degradation of Orange G textile dye. RSC

Advances. 2017;7(48):30411-21.

Competing interests

16. Nassar MY, Mohamed TY, Ahmed IS, Mohamed NM, Khatab M.

The authors declare that there is no conflict of interest that

would prejudice the impartiality of this scientific work.

Hydrothermally synthesized Co 3 O 4, α-Fe 2 O 3, and CoFe 2 O

nanostructures: efficient nano-adsorbents for the removal of

Orange G textile dye from aqueous media. Journal of Inorganic

and Organometallic Polymers and Materials. 2017;27(5):1526-37.

7. Jeon P, Park S-M, Baek K. Controlled release of iron for activation

of persulfate to oxidize orange G using iron anode. Korean Journal

of Chemical Engineering. 2017;34(5):1305-9.

8. Banerjee S, Chattopadhyaya MC, Chandra Sharma Y. Removal of

an azo dye (Orange G) from aqueous solution using modified

sawdust. Journal of Water, Sanitation and Hygiene for

Development. 2015;5(2):235-43.

Authors’ contribution

All authors of this study have a complete contribution for

data collection, data analyses and manuscript writing.

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