Cadmium‐based metal–organic framework for removal of dye from aqueous solution

Abstract

Metal–organic framework ([Cd2(oba)2(4‐bpdb)2] n·3.5(DMF)) (TMU‐8) was successfully synthesized via mechanosynthesis by using nonlinear dicarboxylate and linear N‐donor. The TMU‐8 exhibited accessible cages and tunnels, specific adsorption making it excellent adsorbent for dye removal. The obtained TMU‐8 exhibited accessible cages and tunnels, specific adsorption making them excellent adsorbent for dye removal. The adsorption isotherms, kinetics, thermodynamics, and spectroscopic analyses of the removal of the reactive black 5 onto TMU‐8 were studied. Several variables affecting the removal of the reactive black 5, such as sample pH, amount of sorbent, contact time, and salt concentration, were investigated and optimized. The thermodynamic parameters and kinetics characteristics were also analyzed. The thermodynamic parameters and kinetics characteristics were analyzed. The experimental isotherms data were fitted into Freundlich, Temkin, and Langmuir isotherm equations, and the results indicated that the Langmuir isotherm described the data appropriable than others for reactive black 5 adsorptions. The qmax (mg g⁻¹) was calculated from the Langmuir as 79.36 mg g⁻¹. The fitness of equilibrium data to kinetic models such as, pseudo‐first‐order and pseudo‐second‐order were studied. The adsorption followed pseudo‐second‐order kinetics. Thermodynamic parameters like the enthalpy, entropy, and Gibbs free energy were determined by the Gibbs free energy function, confirming that the adsorption process was spontaneous, exothermic, and feasible.

Full text

REMEDIATION TREATMENT
Cadmium-based metal–organic framework for removal
of dye from aqueous solution
Mahnaz Hazrati
1
| Meysam Safari
2
1
Nano Drug Delivery Research Center, Faculty
of Pharmacy, Kermanshah University of
Medical Sciences, Kermanshah, Iran
2
Department of Chemical Engineering,
Kermanshah University of Technology,
Kermanshah, Iran
Correspondence
Meysam Safari, Department of Chemical
Engineering, Kermanshah University of
Technology, Kermanshah, Iran.
Email: m.safary85@gmail.com
Abstract
Metal–organic framework ([Cd
2
(oba)
2
(4-bpdb)
2
]
n
3.5(DMF)) (TMU-8) was successfully
synthesized via mechanosynthesis by using nonlinear dicarboxylate and linear N-donor.
The TMU-8 exhibited accessible cages and tunnels, specific adsorption making it excel-
lent adsorbent for dye removal. The obtained TMU-8 exhibited accessible cages and
tunnels, specific adsorption making them excellent adsorbent for dye removal. The
adsorption isotherms, kinetics, thermodynamics, and spectroscopic analyses of the
removal of the reactive black 5 onto TMU-8 were studied. Several variables affecting
the removal of the reactive black 5, such as sample pH, amount of sorbent, contact
time, and salt concentration, were investigated and optimized. The thermodynamic
parameters and kinetics characteristics were also analyzed. The thermodynamic param-
eters and kinetics characteristics were analyzed. The experimental isotherms data were
fitted into Freundlich, Temkin, and Langmuir isotherm equations, and the results
indicated that the Langmuir isotherm described the data appropriable than others
for reactive black 5 adsorptions. The q
max
(mg g
−1
) was calculated from the Lang-
muir as 79.36 mg g
−1
. The fitness of equilibrium data to kinetic models such as,
pseudo-first-order and pseudo-second-order were studied. The adsorption
followed pseudo-second-order kinetics. Thermodynamic parameters like the
enthalpy, entropy, and Gibbs free energy were determined by the Gibbs free
energy function, confirming that the adsorption process was spontaneous, exo-
thermic, and feasible.
KEYWORDS
adsorbent, metal–organic framework, reactive black 5, removal, TMU-8
1|INTRODUCTION
Dyestuff wastewater from various industries, such as pharmaceuti-
cals,paper,textile,cosmetics,plastic,printinganddyeing,and
leather industries, has received considerable attention due to its
deep chromaticity, high toxicity, and teratogenicity, and so on.
1-6
Nowadays, more than 10,000 various types of dye are commer-
cially produced. It has been estimated that 1.6 million tons of dyes
are annually produced, from which 10–15% is disposed of waste-
water. It has been revealed that the produced wastewater of tex-
tile industries is about 4–8 million cubic meters per year. A
principal characteristic of textile wastewater is its color. Reactive
dyes are the most important dyes used in industries, but its efflu-
ent causes serious environmental problems.
7-11
Therefore, remov-
ingitisessential.
In recent years, researchers have studied different methods for
dye removal, including precipitation, ozonation, chemical oxidation,
reverse osmosis, membrane filtration, ion-exchange, coagulation, floc-
culation, and adsorption.
12-20
However, most of the mentioned
methods have shown various restrictions, including the generation of
huge amounts of sludge by means of chemical and electrochemical
coagulation processes.
21
Received: 19 August 2019 Revised: 15 January 2020 Accepted: 26 January 2020
DOI: 10.1002/ep.13411
Environ Prog Sustainable Energy. 2020;e13411. wileyonlinelibrary.com/journal/ep © 2020 American Institute of Chemical Engineers 1of9
https://doi.org/10.1002/ep.13411

Adsorption process, in comparison with other methods, is a
better procedure in terms of cost, simplicity in design, and operation,
availability, effectiveness, and lack of sensitivity to toxic sub-
stances.
22-28
Many types of adsorbents have been developed to
remove all kinds of dyestuffs from the wastewater.
29-31
In compar-
ison with conventional adsorbents such as silica, zeolites, and acti-
vated carbon, the metal–organic frameworks (MOFs) have
attracted enormous interest.
32-34
MOFs are organic–inorganic
hybrid crystalline porous materials constructed from metal ions or
clusters bridged by organic linkers to form one-, two-, or three-
dimensional (3D) structures.
35
Compared with common conven-
tional adsorbents such as silica, zeolites, activated carbon, MOFs
as new adsorbent has many advantages, including high specific
surface area, specific adsorption affinities, uniformly structured
nanoscale cavities, accessible cages and tunnels, controllable parti-
cle dimensions and morphology, high pore volume, and pore topol-
ogies.ThesepropertiesmadeMOFsasasuperiorcandidatefor
removal.
36-38
Great progresses have been achieved in the preparation and
application of MOFs. However, most MOFs are not stable in water
due to the hydrolysis of the complex of metal and the linker, which
restricts their application in water purification. Water stability is a key
property for MOFs in many applications, especially in sample prepara-
tion techniques of most the biological and environmental samples
containing water.
In this study, we use a facile mechanosynthesis process to pre-
pare TMU-8 (TMU stands for Tarbiat Modares University) as MOF
with a flower-like structure. Also, its adsorption properties, such as
adsorption equilibrium, adsorption mechanism, thermodynamics, and
kinetics were studied. The TMU-8 were demonstrated to exhibit sig-
nificantly fast adsorption kinetics for reactive black 5 (RB 5) dye
removal.
2|EXPERIMENTAL
2.1 |Chemicals and reagents
The Cd(NO
3
)
2
4H
2
O, 4,40-bipyridine, and 4,40-oxybisbenzoic acid
(H
2
oba), sodium chloride, and methanol were purchased from Merck.
RB 5 was used to study the adsorption characteristics of TMU-8
adsorbent in the system. The chemical structure and some properties
of RB 5 are listed (Table 1). A stock solution of RB 5 was prepared by
dissolving the required amount of RB 5 in solution water.
2.2 |Apparatus
UV-vis absorption spectra were measured by an Agilent model 8453
spectrophotometer. The functional groups were characterized by a
Nicolet spectrometer (Thermo Scientific Nicolet IR100, Madison,
WI). The pellets for the measurement were prepared by mixing the
sample with spectroscopic grade KBr powder. The spectra were ana-
lyzed in the range of 4,000–400 cm
−1
. Scanning electron microscopy
(SEM) measurements were carried out on a model EM3200 from
KYKY Zhongguancun (Beijing, China). X-ray diffraction (XRD) pat-
terns were conducted with a Philips-PW 12Cdiffractometer (Philips
PW, Amsterdam, The Netherlands) using Cu Ka radiation. Ther-
mogravimetric analysis (TGA) was performed on a Bahr STA-503
(Germany) instrument.
2.3 |Preparation of TMU-8
TMU-8 ([Cd
2
(oba)
2
(4-bpdb)
2
]
n
3.5(DMF)) was synthesized according
to a previously reported article.
39
Briefly, TMU-8 was isolated after
grinding Cd (OAc)
2
2H
2
O (1 mmol), 4-bpdb (1 mmol), and H
2
oba
(1 mmol) by hand for 30 min. The resulting powder was washed with
small amounts of DMF to remove any unreacted starting material and
then dried at 80C for 18 hr.
2.4 |Adsorption experiments
The removal procedure was described as follows: 8 mg of prepared
TMU-8 adsorbent was added to an aqueous solution of the dye
(40 ml) at various concentrations adjusted at pH = 2. The mixture was
stirred for 6 min at 900 rpm to reach adsorption equilibrium. Finally,
the solution was centrifuged for 3.0 min, and UV-Vis spectrophotom-
eter was used to determine the residual concentrations of RB 5 in the
supernatant (Figure 1). The removal efficiency and adsorption capaci-
ties at equilibrium (mg g
−1
) were calculated using the following Equa-
tions (1) and (2).
qe=C0−Ce
ðÞ×V
Mð1Þ
Dye removal efficiency %ðÞ=C0−Ce
ðÞ
C0
×100 ð2Þ
In which, C
0
is the initial concentration of RB 5 (mg L
−1
), C
e
is the
final concentration of RB 5 (mg L
−1
), Vis the volume of the initial solu-
tion (L), and Mis the mass of adsorbent (g).
40,41
TABLE 1 Chemical structure and some properties of RB 5
Chemical formula
Molecular formula C
26
H
21
N
5
Na
4
O
19
Molecular weight 991.82
λ
max
610 nm
Electrical property Anionic
2of9 HAZRATI AND SAFARI

3|RESULTS AND DISCUSSION
3.1 |Characterization of TMU-8
TMU-8 contains two channels running along the a-axis (aperture size:
9.3 ×3.9 Å and 6.7 ×3.0 Å; 44.3% void space per unit cell), and the
pore walls contain azine groups of 4-bpdb linear pillar ligands.
FT-IR spectra were acquired for TMU-8 between 4,000 and
400 cm
−1
, and are depicted in Figure 2a. The main functional groups
of the predicted structure could be observed with corresponding
infrared absorption bands. The band at 1646 cm
−1
is caused by the
stretching vibration absorption peak of the C O bonds. The bands at
1376 cm
−1
and 1,423 cm
−1
are assigned to the stretching vibration
absorption peak of the C C bonds of the benzene ring while the band
at 2,742 and 2,846 cm
−1
is due to the stretching vibration of the C–H
bond in the benzene ring.
TGA curve TMU-8 is shown in Figure 2b. The TGA result of the
as-synthesized TMU-8 showed that the first mass loss was between
25 and 200C, while the second mass loss was between 270 and
430C. The first mass loss was due to the desorption of water mole-
cules and physically-bound organic solvent and the second mass loss
due to the decomposition of the MOFs. The synthesized material
phase purity and crystal structure were characterized by powder XRD
pattern (Figure 3a). The typical morphology of TMU-8 was character-
ized using SEM. As shown in Figure 3b, micro flower-like morphology
crystals of synthesized TMU-8 were obtained.
3.2 |Adsorption studies
The removal of RB 5 dye using TMU-8 was investigated. The adsorp-
tion of RB 5 may depend on their respective chemical structures and
polarities. Also, its hydrophilic nature, π–πthe interaction between
chelating ligands of MOF and the aromatic ring of RB 5, and the ability
to form the interaction between their aromatic rings and the TMU-8
adsorption is deemed possible. Furthermore, the presence, N, and
COOH could provide a good interaction through hydrogen bonding
with the NH
2
and OH groups from RB 5. To examine the potential of
TMU-8 as an absorbent for removal, several parameters that could
FIGURE 1 Schematic illustration of removal procedure [Color figure can be viewed at wileyonlinelibrary.com]
FIGURE 2 (a) FT-IR spectra of TMU-8. (b) TGA thermograms of
TMU-8 [Color figure can be viewed at wileyonlinelibrary.com]
HAZRATI AND SAFARI 3of9

influence the removal, which includes sample pH, reaction time, amount
of MOF, and salt concentration were then studied and optimized.
3.2.1 |Effect of pH
The solution pH plays a critical role in the removal process because it
affects the form of RB 5. The adsorptions of RB 5 (40 mg L
−1
; 40 mL;
6 min) onto adsorbent (4 mg) studies were conducted at different pH
(sample matrix from pH 2 to 8) by using 0.1 M HCl/NaOH appropri-
ately. The removal efficiency decreased dramatically as the pH was
increased from 2 to 8. Based on the above experimental result, the
optimum pH selected was pH = 2 in the next experiments.
3.2.2 |Effect of adsorbent
Compared to conventional sorbents, MOFs have a higher surface
area. The amount of MOFs adsorbent is known to be related to the
amount of analytes adsorbed. Therefore, the effect of the amount of
TMU-8 was investigated. The effect of TMU-8 on the adsorption
of RB 5 was investigated from 2 to 12 mg at a concentration of
40 mg L
−1
RB 5 for a period of 6 min (Figure 4a). The result shows
that the removal efficiency could reach the maximum plateau when
6 mg of the TMU-8 was used. As the amount of TMU-8 further
increased after 6 mg, the removal began to level off. The adsorption
capacity increased after the dosage of the adsorbent is increased due
to the greater accessibility of surface binding sites with an increased
FIGURE 3 (a) XRD patterns of TMU-
8. (b) SEM images of TMU-8
FIGURE 4 (a)EffectofsorbentamountontheRB5dye.
(40 mg L
−1
; 40 mL; 6 min, pH = 2.0). (b) The reusability of TMU-8
for RB 5 adsorption [Color figure can be viewed at
wileyonlinelibrary.com]
4of9 HAZRATI AND SAFARI

dosage of adsorbent.
42
However, adsorption capacity decreased
with the further increasing amount of MOF due to adsorption sites
remain unsaturated during the adsorption reaction, whereas the
number of sites available for adsorption site increases by increas-
ing the adsorbent dose. The higher amount of MOF may cause
aggregationofadsorptionsites,whichcandecreasethetotalavail-
able adsorbent surface for adsorbate interaction. To ensure suffi-
cient removal, 8 mg of TMU-8 was selected in the following
experiments.
3.2.3 |Effect of adsorption time
One important factor for adsorption is the equilibrium time.
43
So, the
effect of equilibrium time was studied by varying it from 1 to 10 min.
The result showed that the removal of the analytes was increased
from 1 to 6 min and then remained almost constant. The obtained
high adsorption is attributed to the more efficient time allows maxi-
mum contact period for the adsorbent to interact with the RB 5. So,
6 min of removal time was chosen.
3.2.4 |Effect of salt addition
The effect of ionic strength was studied by adding different
amountsofNaCl(i.e.,0,1.0,2.0,3.0,4.0,and5%[w/v])tothe
sample solution. Salt addition has a negative effect on the removal
efficiency. Thus, salt was not added to the samples in future
experiments.
3.2.5 |Effect of sample volume
Theeffectofsamplevolumeonthe adsorption was studied by
removal of the RB 5 in the range of 20–80 ml that was spiked with
0.5 mg of the RB 5 in the presence 8 mg of MOF. The adsorption
efficiencyremainedstablewhenthesamplevolumewasinthe
range of 20.0–40.0 ml. The adsorption efficiency decreased when
thesamplevolumewasgreaterthan40.0mlsincethedispersityof
adsorbent would be reduced in the sample solution.
3.3 |Desorption and regeneration studies
From the view of practical application, the reusable ability of adsor-
bents was very important. To evaluate the reusability of TMU-8, the
used TMU-8 was soaked with 1 ml deionized water for six times by
vortexing for 3 min in a conical flask. The studies showed that TMU-8
could be reused for at least six successive removal processes with
removal efficiency higher than 95% (Figure 4b). Under higher removal
cycles, removal efficiency decreases may be due to oxidation, losing,
and, or dissolving some amounts of the TMU-8 during the successive
steps.
3.4 |Adsorption kinetic study
The kinetics of adsorption of RB 5 on the TMU-8 was investigated.
Two types of kinetic models, pseudo-first-order and pseudo-second-
order model, were employed to fit experimental data.
The equations of the two kinetic models are represented in Equa-
tions (3) and (4), respectively.
ln qe−qt
ðÞ=lnqe−k1tð3Þ
t
qt
=1
k2q2
e
+t
qeð4Þ
In which, q
e
(mg g
−1
) is the adsorption capacity at equilibrium and
q
t
(mg g
−1
) is the amount of dye adsorbed at time t;k
1
and k
2
are the
adsorption rate constant of the pseudo-first-order and pseudo-sec-
ond-order model, respectively. The slopes and the intercepts of each
linear plot are used to calculate the kinetic parameters for RB
5 adsorption.
The linearity fitting results were shown in Figure 5 and Table 2.
Compared with the pseudo-first-order, the determination coefficient
of the pseudo-second-order kinetic model was higher (R
2
> .99),
which indicated that the pseudo-second-order kinetic model could
better describe the adsorption of TMU-8 toward RB 5. Moreover, the
adsorption capability of TMU-8 for RB 5 calculated by the pseudo-
second-order kinetic model was similar to that obtained by the experi-
ment. The good agreement between the experimental data and
pseudo-second-order can further be supported by the similar values
of the experimental Q
e,exp
and the calculated Q
e,cal
from the kinetics
equation.
FIGURE 5 (a) Pseudo first order kinetic plot (b) pseudo second
order kinetic plot [Color figure can be viewed at wileyonlinelibrary.com]
HAZRATI AND SAFARI 5of9

3.5 |Adsorption isotherms
The adsorption isotherm is an equation that shows the transmission
of adsorbate molecules from the liquid phase to the solid phase at
equilibrium condition. Therefore, these isotherms must be measured
to determine and optimize the adsorbent capacity.
The Langmuir (Equation 5), Freundlich (Equation 7), and Temkin
(Equation 6) were the adsorption isotherms models which were
employed here to describe RB 5 adsorption equilibrium:
log qe= logkf+1
nlogCeð5Þ
Ce
qe
=1
KLqmax
+Ce
qmax ð6Þ
q=BTlnCe+BTlnKT ð7Þ
Where q
max
is maximum adsorption capacity, q
e
represents the
adsorption amount at equilibrium, C
e
is the RB5 concentration in sam-
ple solution at equilibrium, K
L
,1/n, and K
F
, are the Langmuir and
Freundlich constant, respectively. Also, ‘BT’(kJ/mol) and “KT”are
Temkin isotherm constants.
The isotherm parameters estimated were present in Table 3
(Figure 6). According to the results, the Langmuir isotherm provided much
higher R
2
values than did the Freundlich isotherm for the adsorption of
RB 5 onto TMU-8, indicating its better fit with the experimental data.
Based on the assumption of Langmuir isotherm, it is clear that
high-affinity adsorption sites were evenly distributed on the surface of
the sorbents, and a monolayer of RB 5 was formed on the surface of
TMU-8. The q
max
(mg g
−1
) and K
L
(L mg
−1
) were calculated from the
Langmuir as 79.36 mg g
−1
and 0.285 L mg
−1
,respectively(Table3).
3.6 |Adsorption thermodynamics
The thermodynamic parameters reveal the spontaneous nature and
feasibility of the adsorption process. To study the effects of tempera-
ture on adsorption of RB 5 onto TMU-8, the adsorption experiments
were carried out. The adsorption isotherm data obtained at 298, 303,
313, and 318 K were used to estimate thermodynamic parameters
such as enthalpy (ΔH), entropy (ΔS), and standards Gibbs free
energy (ΔG) Thermodynamic parameters were calculated according
to the following Equations (8) and (9):
ΔG=ΔH−TΔSð8Þ
ln Kc=ΔS
R
−
ΔH
RT ð9Þ
Where T,R, and K
c
are the absolute temperature (K), the gas con-
stant (8.314 J/mol K
−1
), and the equilibrium constant, the amount of
TABLE 2 Kinetic parameters for dye
solution
Kinetic models
Pseudo-first-order Pseudo-second-order
q
e
(mg g
_1
)k
1
(min
−1
)r
2
q
e
(mg g
_1
)k
2
(g mg
_1
min
_1
)r
2
29.53 0.3444 .9863 43.66 0.013 .9988
TABLE 3 Langmuir and Freundlich isotherm constants and
correlation coefficients
Langmuir model Freundlich model
q
max
(mg g
−1
)K
L
(L mg
−1
)r
2
K
F
(mg g
−1
)nr
2
79.36 0.285 .9901 25 5.017 .9784
FIGURE 6 (a) Freundlich plot (b) Langmuir plot (c) Temkin plot for
dye adsorption by TMU-8 [Color figure can be viewed at
wileyonlinelibrary.com]
TABLE 4 Thermodynamic Parameters for the Adsorption of dye
onto TMU-8
ΔG
0
(kJ/mol) at
ΔH(kJ/mol) ΔS(kJ/mol K)298 K 303 K 318 K
- 5.472 −5.091 −3.949 −28.159 −0.07613
6of9 HAZRATI AND SAFARI

dye adsorbed on the adsorbent of the solution at equilibrium
(mol L
−1
), the equilibrium concentration of dye in the solution
(mol L
−1
), respectively.
44
The values (change in the enthalpy in J/mol)
and (change in the entropy in J/mol K) were calculated from the
slopes and intercepts of the plot log K
c
versus 1/T. The values of the
thermodynamic parameters for the adsorption of RB 5 on TMU-8 are
listed in Table 4. The negative values of standards Gibbs free energy
at 298, 303, 313, and 318 K indicate the feasibility of the process and
spontaneous nature of the adsorption. The negative value of enthalpy
shows the exothermic nature of the reaction during the adsorption
process. The change in entropy shows a negative value indicating a
decreased randomness between the solid/ liquid interfaces.
3.7 |Adsorption mechanism
In the present work, RB 5 was selected as the model analytes to
investigate the applicability of the TMU-8 as an adsorbent for
removal of the compound target from water samples. The sorbent
type is a crucial variable affecting the removal efficiency. Major
interactions expected to be the driving forces for the extractions
included.
(a) hydrophobic interactions, (b) π–πthe interaction between che-
lating ligands of MOF and the aromatic ring of RB, and ability to form
interaction between their aromatic rings and the TMU-8 an adsorp-
tion is deemed possible, (c) The presence of Lewis basic features of
azine groups which are existent in the middle of pillar ligand and
COOH could provide a good interaction through hydrogen bonding
with the NH
2
and OH groups from RB 5.
By consideration of sorption capacity, adsorption time, and
sorbent dosage, the developed method was compared with the
published methods for removal of RB 5 (Table 5). It is clear from
the comparative study that the adsorption capacity of synthe-
sized TMU-8 (79.36 mg g
−1
) is quite comparable or even better
with the other available adsorbent materials.
45-50
It was found
that sorbent is an excellent adsorbent for RB 5. The advantages
of this technique are its simplicity, safety, and fast operation in
comparison with the reported methods. Also, the amount of
absorbent used in this method is less than those in most of the
previous methods.
4|REAL SAMPLE ANALYSIS
The performance of the proposed method was tested by analyzing
river water samples spiked at concentration levels of 30, 60, and
90 mg L
−1
of RB 5. The results are outlined in Table 6, with the recov-
eries between 91.0 and 98.83%.
TABLE 5 Comparison of removal of various adsorbents for RB 5 from water solutions
Method q
e
(mg g
−1
) Adsorption time (min) Amount of sorbent (mg) Ref.
Iron oxide C NPs 18 - 5,000 mg L
−1
45
Sono-sorption (Iranian limestone) 39 10 200 46
a
BPP 49.2 180 30 47
Activated red mud 35.58 60 6,000 mg L
−1
48
b
AC-CS 77.52 5 20 mg/20 ml 49
CuO/Al
2
O
3
91.2 240 200 50
TMU-8 79.36 6 6 Proposed method
a
Banana peel powder.
b
Carbon sorbent-immobilized-cationic surfactant.
TABLE 6 Results of removal
efficiency of dye in water samples RSD (%; n=3)
Sample Added (mg/L) Found (mg/L) Removal (%) Intraday Interday
River water I - n.d - - -
30.0 28.1 93.66 4.3 4.1
60.0 55.4 92.33 4.6 4.8
90.0 85.7 95.22 4.1 3.3
River water II - n.d - - -
30.0 27.3 91.00 5.5 4.2
60.0 59.3 98.83 3.7 4.9
90.0 88.2 98.00 2.1 3.6
Abbreviation: n.d, not detect.
HAZRATI AND SAFARI 7of9

5|CONCLUSIONS
The proposed method demonstrated great potentials of TMU-8 as an
appropriate adsorbent for removal of the RB5 by the adsorption pro-
cess from river water. Due to very high surface, areas, and short diffu-
sion route of the TMU-8 high adsorption capacities can be obtained
in a very short time. Experimental investigations suggested that the
adsorption of RB 5 dye using TMU-8 turns to be cost-effective, effi-
cient, and reusable.
CONFLICT OF INTEREST
All authors declare that they have no conflict of interest.
ORCID
Meysam Safari https://orcid.org/0000-0001-9356-1859
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How to cite this article: Hazrati M, Safari M. Cadmium-based
metal–organic framework for removal of dye from aqueous
solution. Environ Prog Sustainable Energy. 2020;e13411.
https://doi.org/10.1002/ep.13411
HAZRATI AND SAFARI 9of9