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Journal of Hazardous Materials 171 (2009) 153–159
Contents lists available at ScienceDirect
Journal of Hazardous Materials
journal homepage: www.elsevier.com/locate/jhazmat
Kinetics of hexavalent chromium sorption on amino-functionalized macroporous
glycidyl methacrylate copolymer
A. Nastasović a,∗ , Z. Sandić b , Lj. Suručić c , D. Maksin d , D. Jakovljević a , A. Onjia d
a
Institute of Chemistry, Technology and Metallurgy, University of Belgrade, Polymer Department, Studentski trg 12-16, Belgrade 11001, Serbia
Faculty of Science, Mladena Stojanovića 2, Banja Luka, Republic of Srpska (BIH), Bosnia and Herzegovina
c
Faculty of Forestry, Kneza Višeslava 1, Belgrade, Serbia
d
Vinča Institute of Nuclear Sciences, P.O. Box 522, Belgrade, Serbia
b
a r t i c l e
i n f o
Article history:
Received 9 February 2009
Received in revised form 10 May 2009
Accepted 26 May 2009
Available online 6 June 2009
Keywords:
Glycidyl methacrylate
Amino-functionalized
Chromium sorption
Pseudo-second kinetic model
a b s t r a c t
Two samples of macroporous crosslinked poly(glycidyl methacrylate-co-ethylene glycol dimethacrylate),
poly(GMA-co-EGDMA), with different porosity parameters were synthesized by suspension copolymerization and functionalized with ethylene diamine and diethylene triamine. The kinetics of Cr(VI) sorption
by amino-functionalized poly(GMA-co-EGDMA) was investigated under non-competitive conditions.
Competitive kinetics was studied from following multicomponent solutions: Cu(II) and Cr(VI); Cu(II),
Co(II), Cd(II) and Ni(II); Cr(VI), Cu(II), Co(II) and Cd(II) solutions. Two kinetic models (the pseudo-first
and pseudo-second-order) were used to determine the best-fit equation for the metals sorption by
poly(GMA-co-EGDMA)-en and poly(GMA-co-EGDMA)-deta.
© 2009 Elsevier B.V. All rights reserved.
1. Introduction
Due to their extreme toxicity, the effective removal of Cr(VI)
from industrial waste waters is an issue of major environmental
concern. Since Cr(VI) cannot be destroyed in the natural environment, development of technologies that can remove and/or
recover this metal from the waste waters is in constant focus of
the researchers throughout the world. Conventional methods, like
precipitation, electro winning, membrane separation, evaporation
and solvent extraction suffer from some drawback; since they are
ineffective, expensive, generate secondary pollution, etc. [1,2]. On
the other hand, chelating polymers are preferred due to their high
efficiency, easy handling, reusability and cost effectiveness [3].
They consist of crosslinked copolymer as a solid support and functional group (ligand) containing N, O, S and P donor atoms capable
for coordinating of different metal ions. In the relatively simple
process, chelating copolymer is contacted with the contaminated
solution, loaded with metal ions, and stripped with appropriate
eluent.
Macroporous copolymers based on glycidyl methacrylate are
very suitable for preparation of chelating sorbents, as they can
be prepared by suspension copolymerization in form of spherical beads with desired size and porous structure which can be
∗ Corresponding author. Fax: +38 111 2635 636.
E-mail address: anastaso@chem.bg.ac.rs (A. Nastasović).
0304-3894/$ – see front matter © 2009 Elsevier B.V. All rights reserved.
doi:10.1016/j.jhazmat.2009.05.116
adjusted by the variation of the type and the amount of inert
component and the type and the amount of crosslinking polymer
in the reaction mixture [3–6]. Additionally, the attractiveness of
these copolymers originates from the fact that the epoxy group in
GMA molecule can easily be transformed into a variety of groups,
like iminodiacetate [7,8], thiol [9,10], dithiocarbamate [11], etc.
Amino-functionalized glycidyl methacrylate copolymers have been
obtained by reaction of epoxy groups of the copolymer with ammonia [12], ethylene diamine [9,12–17], diethyl amine [18], diethylene
triamine [19,20], triethylene tetramine [21], etc. These copolymers
posses high capacity and good selectivity for the precious and
heavy metal ions, combined with chemical and mechanical stability
[22].
In this study, two samples of poly(glycidyl methacrylateco-ethylene glycol dimethacrylate) [abbreviated poly(GMA-coEGDMA)], SGE-10/12 and SGE-10/16, with different porosity were
synthesized by suspension copolymerization in the presence of
inert component and additionally functionalized via ring-opening
reaction of the pendant epoxy groups with ethylene diamine and
diethylene triamine.
The sorption kinetics of Cr(VI) and four heavy metals: Cu(II),
Co(II) Cd(II) and Ni(II), was studied under non-competitive (from
single-component metal salt solutions) and competitive conditions
(from mixed metal salt solutions). Kinetic data were analyzed using
two sorption kinetic models (pseudo-first and pseudo-secondorder) to determine the best-fit equation for heavy metal sorption
onto amino-functionalized poly(GMA-co-EGDMA).
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2. Experimental
2.5. Metal sorption batch experiments
2.1. Materials and methods
Sorption of metal ions from aqueous solutions (initial metal concentration 0.05 M, pH 1.8) was investigated in batch experiments
under non-competitive and competitive conditions, at room temperature. The reproducibility of the sorption experiments results
was verified in triplicate.
The amount of metal ions sorbed onto unit mass of macroporous
copolymer beads (sorption capacity, mmol g−1 ) was calculated
from:
All the chemicals were used as received: glycidyl methacrylate (GMA) (Merck), ethylene glycol dimethacrylate (EGDMA)
(Fluka), ethylene diamine (EDA) (Fluka), diethylene triamine (DETA)
(Merck), 2,2′ -azobisiso-butyronitrile (AIBN) (Merck), poly(N-vinyl
pyrrolidone) (Kollidone 90, BASF), cyclohexanol (Merck), dodecanol
and hexadecanol (Merck), copper chloride (Kemika), cobalt chloride (Carlo Erba), nickel chloride (Carlo Erba), cadmium sulphate
(Kemika) and potassium dichromate (Sigma Aldrich). All solutions
were prepared using deionized water.
The copolymer samples were analyzed for their carbon, hydrogen and nitrogen content using the Vario EL III device (GmbH Hanau
Instruments, German) [23]. Elemental analysis was calculated from
multiple determinations within ±0.2% agreement.
The pore size distributions of samples were previously determined by mercury porosimetry (Carlo Erba 2000, software
Milestone 200) [7,23]. The metals concentration was determined
by atomic absorption spectrometry (AAS, SpektrAA Varian Instruments).
Standard statistical methods were used to determine the mean
values and standard deviations for each set of data.
2.2. Preparation of poly(GMA-co-EGDMA)
Macroporous poly(GMA-co-EGDMA) samples were prepared by
a radical suspension copolymerization [7]. The monomer phase
(79.7 g) containing monomer mixture (20.7 g of GMA and 13.8 g of
EGDMA), 2,2-azobis-isobutyronitrile (AIBN) as an initiator (0.8 g),
and 45.2 g of inert component (40.7 g of cyclohexanol and 4.5 g of
dodecanol for SGE-10/12 and hexadecanol for SGE-10/16) was suspended in the aqueous phase consisting of 240.0 g of water and
2.4 g of poly(N-vinyl pyrrolidone). In the labels letter S designates
suspension copolymerization, G and E stand for monomers (GMA
and EGDMA). The first number in a sample labels stands for the
share of aliphatic alcohol in the inert component (w/w) and the
second one for the number of C-atoms in the aliphatic alcohol. The
copolymerization was carried out at 70◦ C for 2 h and at 80◦ C for
6 h with a stirring rate of 200 rpm. After completion of the reaction,
the copolymer particles were washed with water and ethanol, kept
in ethanol for 12 h, dried in vacuum at 40◦ C and purified by Soxhlet
extraction with ethanol. The fraction with average particle diameter
in the range 0.15–0.50 mm was used in subsequent reactions.
2.3. Functionalization of poly(GMA-co-EGDMA) with ethylene
diamine
Four grams of poly(GMA-co-EGDMA) (sample SGE-10/12), 10.0 g
of ethylene diamine and 100 cm3 of toluene were left at room temperature for 24 h [23]. The reaction mixture was heated at 80◦ C
for 6 h. Modified sample was filtered, washed with ethanol, dried
and labeled as SGE-10/12-en (-en designate sample modified with
ethylene diamine).
2.4. Functionalization of poly(GMA-co-EGDMA) with diethylene
triamine
A mixture of 3.6 g of poly(GMA-co-EGDMA) (sample SGE-10/16),
15.7 g of diethylene triamine and 100 cm3 of toluene was left at
room temperature for 24 h, then heated at 80◦ C for 6 h [23]. Modified sample was filtered, washed with ethanol, dried and labeled as
SGE-10/16-deta (-deta designate sample modified with diethylene
triamine).
Q =
(C0 − C) · V
m
(1)
where C0 and C are the concentrations of the metal ions in the initial
solution and in the aqueous phase after treatment for certain period
of time, respectively (in mmol dm−3 ), V is the volume of the aqueous
phase (in dm3 ) and m is the amount of the poly(GMA-co-EGDMA)
amino-functionalized beads used for the experiment (in g).
For determination of Cr(VI) sorption rate from singlecomponent salt solution, 0.25 g of copolymer was contacted with
25 cm3 of metal salt solution. Cu(II) and Cr(VI) sorption rates from
binary salt solutions were determined by contacting 0.5 g of copolymer with 50 cm3 of mixed metal salt solution (25 cm3 of each metal
solution), while Cu(II), Cr(VI), Co(II) and Cd(II) sorption rates were
determined by contacting 20 cm3 of metal salt solution (5 cm3 of
each metal solution).
In each experiment, at appropriate times, 0.5 cm3 of aliquots
were removed and diluted to 50 cm3 . The concentrations of the
metal ions in the aqueous phases were measured by atomic absorption spectrometry (AAS).
3. Results and discussion
The immobilization of low molecular compounds to homopolymers and copolymers can be achieved in two commonly used
ways: copolymerization of suitable monomer that already carries the required functional group and chemical modification
of synthesized polymer in order to introduce chelating groups.
In this study, chemical modification was chosen as a method
to introduce amino ligands into macroporous poly(GMA-coEGDMA). On the basis of our previous results, samples SGE-10/12
(SHg = 50 m2 g−1 , VS = 0.610 cm3 g−1 , DV/2 = 53 nm) [7] and SGE10/16 (SHg = 33 m2 g−1 , VS = 0.755 cm3 g−1 , DV/2 = 87 nm) [7] were
chosen for amino-functionalization and metal sorption experiments. Porosity parameters (specific pore volume, VS , specific pore
area, SHg , and pore diameter that corresponds to the half of the pore
volume, DV/2 ) of amino-functionalized samples are given in Table 1
[23].
The elemental analysis data of amino-functionalized samples, as
well as degree of conversion of epoxy groups, ligand concentration,
CLIG , and amino group concentration, CAG , were given in Table 2. The
lower degree of conversion was obtained for sample functionalized
with diethylene triamine, probably due to a steric effect, which is
one of the main problems in polymer functionalization with larger
groups [24].
3.1. Kinetics
The important physicochemical aspects for the evaluation of
applicability of chelating copolymers are specific and fast complexTable 1
Porosity parameters of amino-functionalized samples [23].
Sample
SHg , m2 /g
VS , cm3 /g
DV/2 , nm
SGE-10/12-en
SGE-10/16-deta
70 ± 0.4
50 ± 0.3
1.18 ± 0.01
0.66 ± 0.005
42 ± 0.6
60 ± 0.4
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155
Table 2
Elemental analysis of amino-functionalized poly(GMA-co-EGDMA) samples, as well as the degree of conversion of epoxy groups, ligand concentration, CLIG , and amino group
concentration, CAG [23].
Elemental analysisa
Sample
SGE-10/12-en
SGE-10/16-deta
a
Found
Calculated
%C
%H
%N
%C
%H
%N
52.6
50.2
8.5
10.1
6.1
6.8
56.3
56.3
8.2
8.2
8.4
8.4
CLIG , mmol g−1
Conv., %
CAG , mmol g−1
2.2 ± 0.004
1.6 ± 0.003
52 ± 0.08
38 ± 0.08
4.4 ± 0.009
4.9 ± 0.008
Elemental analysis was calculated from multiple determinations within ± 0.2% agreement.
Table 3
The sorption half time, t1/2 , sorption capacities after 5 min (Q5 ) and 30 min (Q30 ), maximum sorption capacities (Qmax ) and maximum ligand occupation (Lmax ) for metal
sorption on amino-functionalized poly(GMA-co-EGDMA) samples.
Copolymer sample
pH
Non-competitive conditions
Cr(VI) single-component solution
SGE-10/12-en
1.8
SGE-10/16-deta
1.8
Competitive conditions
Cr(VI) and Cu(II) binary solution
SGE-10/16-deta
Cr(VI)
1.8
Cu(II)
1.8
t1/2 , min
1.0
0.4
11
45
Cr(VI), Cu(II), Co(II) and Cd(II) multi-component solution
SGE-10/16-deta
Cr(VI)
1.0
1.6
Cu(II)
1.0
2.5
Co(II)
1.0
1.2
Cd(II)
1.0
1.2
a
Q5 , mmol g−1 (%)a
Q30 , mmol g−1 (%)a
Qmax , mmol g−1
Qmax , g g−1
Lmax , %
1.84 (90)
1.15 (78)
2.11 (100)
1.37 (93)
2.11
1.48
0.110
0.094
96.8
67.9
0.26 (26)
0.072 (13)
0.76 (76)
0.22 (40)
1.00
0.55
0.052
0.035
61.7
33.9
0.27 (63)
0.22 (63)
0.11 (79)
0.11 (73)
0.22 (63)
0.26 (74)
0.14 (100)
0.11 (100)
0.43
0.35
0.14
0.15
0.024
0.022
0.008
0.017
26.5
21.6
8.6
9.3
Calculated in relation to Qmax .
ation of the metal ions, as well as their regeneration and reusability
[25]. Consequently, the rapid sorption of metal ions by functionalized poly(GMA-co-EGDMA) would be beneficial for practical use,
providing a short solution–sorbent contact time in the actual process.
3.2. Non-competitive conditions
The sorption rates for Cr(VI) ions by SGE-10/12-en and SGE10/16-deta are presented in Fig. 1. Since those samples have
different ligand concentrations, in order to provide a more
appropriate comparison, maximum ligand occupation, Lmax , was
Fig. 1. Sorption of Cr(VI) ions vs. time under non-competitive conditions, on SGE10/12-en and SGE-10/16-deta.
calculated [26]:
Lmax =
Qmax
· 100
CLIG
(2)
From the experimental data, sorption half time, t1/2 (time
required to reach 50% of the total sorption capacity) and maximum
ligand occupation (Lmax ) were calculated and given in Table 3, with
the values of the maximum sorption capacities (Qmax ), sorption
capacities after 5 min (Q5 ) and 30 min (Q30 ), taken from Fig. 1.
The uptake of Cr(VI) ions was very rapid, with t1/2 value of
≤1 min. Somewhat faster sorption was observed for SGE-10/12-en
for which after 30 min maximum sorption capacity was attained.
Also, ligand occupation was lower for SGE-10/16-deta (68%) then for
SGE-10/12-en (97%), i.e. for the sample with 1.4 times higher surface
area (the values of specific surface area for SGE-10/12-en and SGE10/16-deta as given in Table 1 were 70 and 50 m2 g−1 , respectively).
It is in accordance with literature data, which suggest that when the
initial sorption rate is high, the sorption process occurs predominantly at the surface of the highly crosslinked amino-functionalized
beads [27]. After that, the sorption rate becomes slower and saturation was gradually reached. The mechanism of intrapore diffusion
is represented by the slower sorption rate, which was noticed after
30 min of the initial sorption.
Here must be mentioned that poly(GMA-co-EGDMA) was functionalized with two different amines, i.e. ethylene diamine (sample
SGE-10/12-en) and diethylene triamine (sample SGE-10/16-deta),
so the assumption was that we cannot exclude the influence of the
ligand, especially if we bear in mind previous results [23]. Indeed,
sorption capacity seems to be influenced by the ligand type and this
is clear when the values of specific surface area and pore diameters
are the same, like in case of samples SGE-10/16-en, SGE-10/16-deta
and the sample functionalized with triethylene tetramine, SGE10/16-teta (SHg around 50 m2 g−1 , DV/2 30 nm). According to the
previously obtained results, maximum capacities for Cu(II) ions on
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SGE-10/16-deta and SGE-10/16-teta were 1.75 times higher than
for SGE-10/16-en [23]. On the other hand, sorption rates were similar, with t1/2 value for SGE-10/16-en around 4 min, and slightly
lower t1/2 for SGE-10/16-deta and SGE-10/16-teta, of around 3 min.
However, in the case of samples with different surface area used
in this study, like SGE-10/12-en (70 m2 g−1 ) and SGE-10/16-deta
(50 m2 g−1 ) it seems that influence of surface area on the sorption
rate and capacity becomes dominant.
The reported literature data on Cr(VI) removal with commercial and synthetic polymer sorbents are in a wide range, but
they were obtained under different experimental conditions. However, just for the sake of comparison we will mention some of
those results. For example, Saha et al. obtained t1/2 ≈ 3 min for
Cr(VI) sorption on highly crosslinked acrylic resin Amberlite XAD7 impregnated with Aliquat 336 [28]. Hydrophilic methacrylic
based polymer HP-2MG impregnated with Aliquat 336 sorbed
more than 50% of Cr(VI) within the first 10 min [29]. Baran
et al. reported that sorption of Cr(VI) attained an optimum at
30 and 40 min for macroporous strongly acidic poly(styrene-codivinylbenzene) based ion-exchangers Purolite CT-275 and Purolite
MN-500; and 30 min for Amberlite XAD-7 [30]. The high sorption rates of hexavalent chromium at the onset, and then plateau
values gradually reached within 15 min were observed for macroporous basic anion exchange resins containing tertiary amine
groups, Lewatit MP 62 and Lewatit M 610 [31]. Bayramoglu et al.
also observed high initial Cr(VI) sorption rate at pH 2, with time
required to attain the equilibrium of 120 min both for crosslinked
poly(glycidyl methacrylate-co-methyl methacrylate) with attached
ethylene diamine [17] and magnetic poly(GMA-co-EGDMA) with
immobilized poly(ethyleneimine) [32].
3.3. Competitive conditions
The metal ion uptake capacities and selectivity under competitive conditions, besides agitation (static experiments) or flow
rate (column experiments), structural properties of the chelating
copolymers (particle size, porosity parameters), sorption conditions (pH, initial concentration of metal ions), ligand type, kinetic
and thermodynamic stability of the formed metal complexes with
the chemically bonded amine ligands; strongly depend on the presence of the other metal ions which they compete for the active sites
in the copolymer [25]. For that reason, it is almost impossible to
generalize the order of metal sorption (selectivity) or to predetermine the amount of the adsorbed metal ions on the basis of the
results obtained under non-competitive conditions. The decisive
role in determination whether polymer could be used for selective
sorption or not, has the experiments under comparative conditions.
3.4. Metal sorption from binary solutions
The sorption rates for Cr(VI) and Cu(II) ions under competitive conditions from binary metal solutions were determined
for poly(GMA-co-EGDMA)-deta (sample SGE-10/16-deta) and the
results are presented in Fig. 2 and Table 3.
It can be seen that Cr(VI) is preferably taken up by SGE-10/16deta. The main reason could lie in the fact that the experiment
was performed at pH 1.8, which is favorable for maximum Cr(VI)
sorption. The Cr(VI) exists in anionic forms (Cr2 O7 2− , HCrO4 − ,
CrO4 2− and HCr2 O7 − ) in aqueous solution, and the fraction of
any particular species is dependent on chromium concentration
and pH [17]. At low pH, protonated amino groups attached to the
crosslinked copolymer attract the negatively chromium species,
leading to higher sorption. On the other hand, the protonation of
amine group leads to a strong electrostatic repulsion to the copper ions and lower sorption capacities for Cu(II) at low pH [17,19].
The curve for Cr(VI) sorption has higher slope comparing with
Fig. 2. Sorption of Cr(VI) and Cu(II) ions, vs. time under competitive conditions, on
SGE-10/16-deta.
curve for Cu(II), especially within 30 min from the start of the
experiment.
It is very important to emphasize that Cr(VI) and Cu(II) sorption
for SGE-10/16-deta was much slower from their binary solutions
(t1/2 values for the uptake of Cr(VI) and Cu(II) ions of 11 and 45 min),
than from single-component solutions (t1/2 values for Cr(VI) and
Cu(II) ions were 0.5 and 3 min [23]). It seems that two highly sorbed
metals, Cr(VI) and Cu(II), compete for the active sites (ligands) on
the beads and at the same time hinder the metal coordination of
concurrent ion from their binary solution. Even though the sorption
of both metals was very slow, total ligand occupation for SGE-10/16deta was 96%.
3.5. Metal sorption from multicomponent solutions
In our previous study, kinetics of competitive sorption of Cu(II),
Cd(II), Ni(II) and Co(II) on poly(GMA-co-EGDMA)-deta (sample
SGE-10/16-deta) was studied at pH 4, which was favorable for maximum sorption of these metals [33]. Poly(GMA-co-EGDMA)-deta
was selective for Cu(II) over other ions present in the mixed salt
solution. Namely, maximum capacity for Cu(II) from Cu(II), Cd(II),
Ni(II) and Co(II) mixed solution (at pH 4) on poly(GMA-co-EGDMA)deta was 1.15 mmol g−1 , i.e. 1.7; 4.8 and 5.7 times higher than that
of Cd(II), Co(II) and Ni(II), respectively.
Due to the fact that non-competitive experiments on poly(GMAco-EGDMA)-deta showed fast kinetics and high sorption capacity
for Cr(VI) ions, Ni(II) ions were replaced with Cr(VI), and metal
uptake was investigated from the multicomponent solution of
Cr(VI), Cu(II), Cd(II) and Co(II) (Fig. 3, Table 3).
It should be noted that this experiment was performed at pH
1.80, which is not favorable for Cu(II), Co(II) and Cd(II) sorption,
as already mentioned. On the contrary, the maximum sorption
capacities of amino-functionalized poly(GMA-co-EGDMA) for these
metals were observed for pH 5.5 [15,33]. Namely, with the pH
increase more amino groups exist in the neutral form, reducing the
electrostatic repulsion to the copper, cobalt and cadmium ions [19].
As a result, at higher pH values there is an increase in Cu(II), Co(II)
and Cd(II) sorption. The main reason for choosing pH 1.80 was our
intention to study Cr(VI) sorption by amino-functionalized macroporous poly(GMA-co-EGDMA) as well as to investigate the influence
of Cr(VI) on the sorption of other metal ions, and to compare the
results of Cr(VI) sorption form single and Cr(VI)/Cu(II) binary solution, so we have chosen pH at which the maximum Cr(VI) sorption
capacity was observed [23].
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157
Table 4
Kinetic data for heavy metals sorption on poly(GMA-co-EGDMA)-en and poly(GMA-co-EGDMA)-deta.
Sample
Pseudo-first-order kinetics
Pseudo-second-order kinetics
R
k2 , gmmol−1 min−1
Qeq , mmol g−1
R2
5.69
0.57
0.632
0.916
1.508
0.362
2.11
1.49
0.999
0.999
0.037
0.023
0.84
0.57
0.979
0.961
8.23·104
0.034
1.07
0.68
0.999
0.931
Cr(VI), Cu(II), Co(II) and Cd(II) multi-component solution
SGE-10/16-deta
Cr(VI)
0.43
0.048
Cu(II)
0.35
0.020
Co(II)
0.14
0.085
Cd(II)
0.15
0.047
0.23
0.18
0.07
0.05
0.963
0.813
0.853
0.779
0.761
0.409
5.25
4.90
0.44
0.35
0.14
0.15
0.999
0.993
0.999
0.999
Qe,exp , mmol g
−1
−1
k1 , min
Qeq , mmol g
Non-competitive conditions
Cr(VI) single-component solution
SGE-10/12-en
2.11
SGE-10/16-deta
1.48
0.325
0.004
Competitive conditions
Cr(VI) and Cu(II) binary solution
SGE-10/16-deta
Cr(VI)
1.00
Cu(II)
0.55
−1
2
enhances Cr(VI) and Cu(II) sorption compared with the sorption
from their binary solution. Inversely, the presence of Cr(VI) promotes the sorption of cobalt and cadmium which are not so fast
bound from the mixed Cu(II), Co(II), Cd(II) and Ni(II) solution.
Although metals were sorbed slower from mixed Cu(II), Co(II),
Cd(II) and Ni(II) solution, the total amount of bonded metals was
twice higher (2.22 mmol g−1 ) than from Cr(VI), Cu(II), Cd(II) and
Co(II) solution (1.07 mmol g−1 ). It seems that in the case of competitive sorption, pH and the presence of other metals have the
most pronounced influence on the values of sorption rate and
capacities.
3.6. Kinetic models
Fig. 3. Sorption of Cr(VI), Cu(II), Co(II) and Cd(II) vs. time under competitive conditions on SGE-10/16-deta.
Sorption of all metals was very fast, with t1/2 ≤ 2 min for Cr(VI),
Co(II) and Co(II) and 2.5 min for Cu(II). It can be seen that t1/2
values and maximum capacities were quite different comparing
with the results obtained with Cu(II), Cd(II), Ni(II) and Co(II) mixed
solution. In that case, the t1/2 values for the uptake of Cu(II) and
Cd(II) on poly(GMA-co-EGDMA)-deta were approximately 8 and
3.5 min, while t1/2 values for Ni(II) and Co(II) were similar, i.e.
around 5 min [33]. Also, Cu(II) and Cr(VI) sorption was considerably faster from multicomponent Cr(VI), Cu(II), Cd(II) and Co(II),
than from binary Cr(VI) and Cu(II) solution. The presence of Co(II)
and Cd(II) that are not preferentially taken by SGE-10/16-deta
Two kinetic models were used to determine the best-fit equation for the metals sorption by poly(GMA-co-EGDMA)-en and
poly(GMA-co-EGDMA)-deta.
The most commonly used is Lagergren’s equation for pseudofirst-order rate [34]:
log(Qeq − Qt ) = log Qeq −
(k1 t)
2.303
(3)
where k1 is the rate constant of pseudo-first-order sorption (min−1 ),
Qeq and Qt denote the amounts of sorbed metal ions at equilibrium
and at time t (mmol g−1 ), respectively. A plot of log(Qeq − Qt ) versus
t should give a straight line to confirm the applicability of the kinetic
model. In a true first-order process, log(Qeq ) should be equal to the
intercept of a plot log(Qeq ) − Qt against t.
Fig. 4. Pseudo-first (a) and pseudo-second-order kinetics (b) of the Cr(VI), Cu(II), Cd(II) and Co(II) solution ions uptake by SGE-10/16-deta.
Author's personal copy
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A. Nastasović et al. / Journal of Hazardous Materials 171 (2009) 153–159
A pseudo-second-order equation is given as [34]:
1
t
1
=
t
+
Qt
Qeq
k2 Qeq 2
(4)
where k2 (g−1 mmol−1 min−1 ) is the rate constant of pseudosecond-order sorption. A plot of t/Qt versus t should give a linear
relationship for the second-order kinetics.
The rate constants k1 and k2 , equilibrium sorption capacity, Qeq ,
and the correlation coefficient, R2 , calculated from the values of
intercepts and slopes of corresponding plots for pseudo-first and
second-order equations are given in Table 4. As an illustration, plots
log(Qeq − Qt ) − t (pseudo-first-order) and t/Qt − t (pseudo-secondorder) for competitive sorption of Cr(VI), Cu(II), Cd(II) and Co(II)
ions by SGE-10/16-deta were shown in Fig. 4.
The theoretical Qeq values estimated from the first-order kinetic
model gave significantly different values compared to experimental ones, and correlation coefficients are found to be rather low.
The only exception is competitive Cu(II) sorption from binary
Cr(VI)/Cu(II) solution on SGE-10/16-deta, for which the correlation
coefficient is slightly lower and Qeq value higher then experimental one for pseudo-second-order. This indicates that the first-order
kinetic model is not applicable to the sorption of tested metals on
amino-functionalized samples.
On the other hand, theoretical Qeq values for metal ions show
good agreement with the experimental data for second-order
kinetics, with correlation coefficients higher that 0.99 (with one
exception, already mentioned). This suggests that heavy metals
sorption under competitive conditions on poly(GMA-co-EGDMA)deta obeys pseudo-second-order kinetics, meaning that sorption
depends both on the properties of the metal and chelating copolymer.
4. Conclusions
Macroporous crosslinked samples of poly(GMA-co-EGDMA with
different porosity were synthesized by suspension copolymerization and functionalized with ethylene diamine and diethylene
triamine. The uptake of Cr(VI) ions under non-competitive conditions was very rapid (t1/2 ≤ 1 min), presumably because the
sorption process occurs predominantly at the surface of aminofunctionalized beads. In such a case, the influence of surface area
on the sorption rate and capacity becomes dominant. The Cr(VI)
and Cu(II) sorption was much slower from their binary solutions (t1/2 for Cr(VI) and Cu(II) were 11 and 45 min) than from
single-component solutions (t1/2 for Cr(VI) and Cu(II) were 0.5 and
3 min) probably due to their mutual competition for the active
sites on the copolymer beads. In the case of competitive sorption,
pH and the presence of other metals have the most pronounced
influence on the values of sorption rate and capacities. From the
analysis of two kinetic models it was concluded that sorption
of investigated heavy metals by amino-functionalized poly(GMAco-EGDMA) obeys pseudo-second-order kinetics, meaning that
sorption depends both on the properties of the metal and chelating
copolymer.
Acknowledgement
This work was supported by the Serbian Ministry of Science and
Environmental Protection, Project ON 142039.
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