removal of aliphatic amino acids by hybrid organic–inorganic layered compounds
TRANSCRIPT
www.elsevier.com/locate/apsusc
Applied Surface Science 253 (2007) 5756–5761
Removal of aliphatic amino acids by hybrid organic–inorganic
layered compounds
Fabiano Silverio *, Marcio Jose dos Reis, Jairo Tronto, Joao Barros Valim
Departamento de Quımica, Faculdade de Filosofia Ciencias e Letras de Ribeirao Preto, Universidade de Sao Paulo,
Av. Bandeirantes, 3900, 14040-901 Ribeirao Preto, CEP, Brazil
Available online 27 December 2006
Abstract
Amino acids have been extensively used in several processes of the pharmaceutical and food industries. Treatments for the recovery and reuse of
the wastewaters generated from these processes are few and little known. This work aims at studying the influence of variables like temperature, pH
and ionic strength on the adsorption of the amino acids Asp and Glu, contained in aqueous solutions, on layered double hydroxides of the Mg–Al–
CO3–LDH system. The adsorption experiments were performed at two different temperatures (298 and 310 K), two different pH values (7.0 and
10.0), and two ionic strength conditions (with or without the addition of NaCl). The adsorption isotherms exhibited similar profiles under the
various conditions studied: an increase in temperature as well as an increase in the pH value decreased the amount of adsorbed amino acid while an
increase in the ionic strength increased Asp and Glu adsorption. The PXRD analysis showed that the diffractograms obtained before and after the
adsorption of amino acids have a similar pattern. The FT-IR spectra of the adsorbed material presented specific bands, which are related to the
amino acids. The concentration range varied up to the anion solubility product and the extraction rate lay between 2.7 and 23.4% at higher
equilibrium concentrations, showing that Mg–Al–CO3–LDH is efficient at removing the amino acids from the aqueous medium.
# 2007 Elsevier B.V. All rights reserved.
Keywords: Hydrotalcite; Layered double hydroxides; Aspartic acid; Glutamic acid; Adsorption
1. Introduction
Layered double hydroxides (LDHs) have received con-
siderable attention during last years owing to their properties
and applications [1–7]. These materials can be structurally
described starting from the structure of Brucite, Mg(OH)2. This
mineral consists of octahedra sharing their edges, being the
magnesium cations located in the centers of such octahedra and
the hydroxyl anions placed on their vertices, which results in
plane and neutral layers (see Fig. 1a) stacked together by
hydrogen-bonds. If some of the bivalent cations are iso-
morphically substituted by trivalent ones in this structure, the
resulting layers display a residual positive charge that needs to
be neutralized. Neutralization is possible due to anions and
water molecules localized between the layers, which stacks the
double hydroxide layers and leads to the hydrotalcite-like
structure (Fig. 1b). These compounds are represented by the
* Corresponding author. Tel.: +55 16 3602 3881; fax: +55 16 3602 4838.
E-mail address: [email protected] (J.B. Valim).
0169-4332/$ – see front matter # 2007 Elsevier B.V. All rights reserved.
doi:10.1016/j.apsusc.2006.12.040
general formula: ½M1�x2þMx
3þðOHÞ2�Ax=mm� � nH2O, where
M2+ is a bivalent cation, M3+ is a trivalent cation, Am� is the
interlayer anion with m� charge. Several organic or inorganic
anions can occupy the interlayer domain of LDHs. Due to their
high porosity and high specific surface area, LDHs are
extensively used as catalysts and adsorbents [8,9]. Hydro-
talcite-like compounds can remove anions from aqueous
solution by three different processes: (i) adsorption, (ii) anion
exchange, and (iii) regeneration of a calcined precursor [10–
16].
Because they have high specific surface area, hydrotalcite-
like compounds have been used in the removal of different
anionic species from aqueous solutions and for gas adsorption.
Adsorption from aqueous solution can occur when the
interlayer anion presents low exchange tendency, as in the
case of carbonate [17]. Our research group has demonstrated
the efficacy of LDHs of the [Mg–Al–CO3] system, calcined or
not, in the sorption and adsorption of surfactants and organic
compounds from aqueous solutions [13,15,16,18,19].
Amino acids like aspartic acid (Asp) and glutamic acid (Glu)
are used in several sections of chemical, pharmaceutical, and
Fig. 1. Schematic structural representation: (a) brucite; (b) hydrotalcite.
F. Silverio et al. / Applied Surface Science 253 (2007) 5756–5761 5757
food industries, where the treatment of industrial wastewaters is
little practised [20–24]. Both amino acids have two carboxylic
groups in their structure, and they differ just by the presence of
an extra –(CH2)– group in the Glu aliphatic chain, which
enhances its hydrophobic character. The aim of this work is to
study the effects of temperature, pH, and ionic strength on the
adsorption of the amino acids Asp and Glu, contained in
aqueous solutions, on layered double hydroxides.
2. Experimental methods
2.1. Preparation of Mg–Al–CO3–LDH—the adsorbent
The LDH was prepared by the pH variable coprecipitation
method proposed by Reichle [25]. The reactants were all
purchased from Merck (>99% assay). All the solids were
characterized by powder X-ray diffraction (PXRD), Fourier-
transform infrared spectroscopy (FT-IR), and specific surface
area (SBET).
2.2. Aspartic acid and glutamic acid—the adsorbates
The amino acids Asp and Glu were obtained from Merck
(>99.5% assay) and used without further purification. All the
amino acid solutions and their dilutions were prepared with
deionized water, and the pH was adjusted to 7 (with HCl) and/or
10 (with NaOH), with good control of the involved variables.
2.3. Adsorption experiments
The adsorption isotherms were obtained by the batch
method, which consisted in adding 50 cm3 aliquots of the
amino acid solution at different initial concentrations (in the
range 1.0 � 10�4 to 6.0 � 10�2 mol dm�3) to a constant mass
(500 mg) of the adsorbent LDH previously dried under vacuum
at room temperature, contained in erlenmeyers with stoppers.
The amino acid solutions were prepared at pH 7 or 10, with or
without the addition of 0.1 mol dm�3 NaCl. The obtained
suspensions were submitted to ultrasonication for 10 min, in
order to homogenize particle size. The isotherms were obtained
at 298 and 310 K.
The samples were kept in a thermostatic bath with orbital
shaking at a constant temperature (T, �0.5 K) for 70 h, to
ensure that the adsorption equilibrium was reached. After this
time, each sample was divided into two parts: one was
centrifuged at 10,000 � g for 20 min, separating the super-
natant (in which the amount of the amino acid was quantified by
UV–vis spectrophotometry) from the solid (which was dried
and characterized); the other part of the sample was kept in
aqueous suspension, for determination of the electrokinetic
potential. After a decanting time of 10 min, the electrokinetic
potential of the suspensions was measured at the same
temperature of the adsorption experiments.
3. Results and discussion
On the basis of the data of elemental and TG analyses, the
adsorbent LDH prepared herein was assigned the empirical
formula ½Mg0:7Al0:3ðOHÞ2�0:3þðCO3Þ0:15
2� � 0:7H2O, which
corresponds to a 2.5:1 Mg/Al ratio. This data is extremely
important because the adsorption capacity depends on the
charge density and is directly related to this ratio.
The adsorption isotherms for Asp and Glu are shown in
Fig. 2. The experiments were carried at two temperatures (298
and 310 K), two different pH values (7 or 10), and two ionic
strength conditions (with or without addition of 0.1 mol dm�3
NaCl) at 298 K.
According to the Giles classification for adsorption
isotherms [26], the adsorption of Asp (Fig. 2a) leads to L-
type 1 isotherms for the following conditions: 298 K, pH 7,
with or without addition of 0.1 mol dm�3 NaCl; and 310 K,
pH 10, with addition of 0.1 mol dm�3 NaCl and where no
Fig. 2. Adsorption isotherms under different conditions: (a) Asp; (b) Glu.
F. Silverio et al. / Applied Surface Science 253 (2007) 5756–57615758
adsorption plateau is observed. This is because the concentra-
tion of the amino acid solutions is limited by the amino acid
solubility products (Ksp) under these conditions. The other
isotherms are L-type 2. Adsorption isotherms obtained for Glu
(Fig. 2b) without the addition of NaCl are L-type 2, while the
others are S-type 1. The S-type isotherms give evidence of
cooperative adsorption, which takes place because of the van
der Waals interactions between the hydrophobic part of the
amino acid (–CH2 groups of Glu molecule).
All isotherms indicate that an increase in temperature seems
to have limited influence on adsorption below certain
equilibrium concentrations, after which the increase in
temperature causes a decrease in the amount adsorbed. This
behavior can be explained considering that the adsorption
process reduces the entropy of the system (DS < 0). Therefore,
the higher the temperature of the system, the higher the positive
entropic contribution to the Gibb’s free energy (DG =
DH � T DS) of the process. This decreases the contribution
of the exothermic enthalpy to the negative free energy. Thus,
the organization of compact aggregates with a larger number of
amino acid molecules in/on the LDH should become more
difficult at higher temperatures. This behavior has been
reported for several systems involving the adsorption of
surfactants on mineral oxides [12,13,27–29].
Although a decrease in adsorption with the increasing pH
can be seen for both amino acids, this effect can be more clearly
observed by comparing the isotherms of Glu at 298 K obtained
at pH 7 and pH 10, both without the addition of NaCl. This
decreased adsorption upon the increasing pH can be explained
by considering two factors: (i) the increase in the negative
charge of Asp and Glu (�1 at pH 7 and �2 at pH 10), and (ii)
the decrease in the surface charge of the adsorbent with the
increase of pH. The isotherm at pH 10 displays a plateau
beginning at an equilibrium concentration that is almost half of
that of the corresponding isotherm at pH 7. Moreover, at pH 10,
the amino acid has two charged extremities and can be adsorbed
in two different orientations: perpendicular to the layers of the
LDH (which is more probable at pH 7), and parallel to them,
occupying two sites per molecule of amino acid (which is more
probable at pH 10). So, considering that adsorption occurs
predominantly by electrostatic interactions, i.e., it depends on
the LDH surface charge, the amount of amino acid removed at
pH 10 should be lower than that removed at pH 7 [28,30–34].
The adsorption of Asp generally increases with the addition
of NaCl, except for low concentrations at pH 10, when the
adsorbed amounts are similar for the experiments carried out
with and without the addition of NaCl. The isotherms for Glu
adsorption at pH 10 show that the adsorption increases a lot
with the ionic strength for equilibrium concentrations higher
than 0.02 mol dm�3; below this concentration, a small variation
can be noticed. At pH 7, a similar behavior is observed, but the
adsorption starts to increase with the ionic strength at
equilibrium concentrations higher than 0.04 mol dm�3, which
is almost twice that observed at pH 10. This fact shows that the
effect of the ionic strength is more pronounced at concentra-
tions near the saturation of the adsorption. So the increased
adsorption at higher ionic strength should be explained in terms
of a decrease in the repulsion between the polar groups of the
amino acid molecule.
The electrokinetic potential curves are very similar for both
amino acids, with high and positive values at low equilibrium
concentrations (see Fig. 3). These values decrease quickly as
the amino acid concentration increases, reaching negative
values for the isotherms at pH 10. Isotherms obtained at pH 7
present positive electrokinetic potential values only, which
means that the saturation of the positive charge of the particles
does not take place in this condition. These results are in
agreement with the isotherm profiles. The rate of extraction of
Asp and Glu by the LDH is shown in Table 1. The material is
highly capable of removing these amino acids, especially when
one considers that the LDH had not been pre-calcined and that
the plateau had not been completely achieved under all the
conditions used here. At low Asp and Glu initial concentrations,
approximately 22 and 29% of the amino acid is removed,
respectively, whereas the extraction rate is as high as 16% in the
last points of the isotherms, where the initial amino acid
concentration is in the limit of its respective solubility. Bearing
in mind that the amino acids limit concentration is almost
0.06 mol dm�3, the material is potentially applicable to the
treatment of wastewater containing these species [35,36].
Fig. 3. Electrokinetic potential related to the adsorption: (a) Asp; (b) Glu.
Table 1
Extraction rate (ER, %) of Asp and Glu by Mg–Al–CO3–LDH under different conditions
Aspartic acid Glutamic acid
pH 7 pH 10 pH 7 pH 10 pH 7 pH 10 pH 7 pH 10
298 K,
I � 0 M
310 K,
I � 0 M
298 K,
I � 0 M
310 K,
I � 0 M
298 K,
I = 0.1 M
298 K,
I = 0.1 M
298 K,
I � 0 M
310 K 298 K,
I � 0 M
310 K,
I � 0 M
298 K,
I = 0.1 M
298 K,
I = 0.1 M
0.0 0.0 0.0 0.0 0.0 0.0 0.0 0.0 0.0 0.0 0.0 0.0
22.0 8.4 12.0 9.6 18.2 15.4 23.7 24.1 28.8 14.0 25.6 15.0
7.7 4.6 26.3 14.1 12.3 16.4 18.1 21.2 20.4 17.6 22.4 7.1
6.0 4.5 23.8 14.1 12.7 14.7 16.6 20.1 22.3 15.1 20.6 22.5
4.5 3.1 16.6 5.7 12.1 16.0 13.7 17.0 11.9 12.5 16.8 16.3
8.2 3.8 22.4 10.9 13.0 13.7 11.9 12.4 7.6 9.8 10.9 10.1
3.7 2.2 18.4 6.2 27.1 20.0 8.8 12.8 7.0 8.9 7.8 8.3
5.5 4.9 15.3 5.7 28.1 15.5 9.6 10.5 7.8 9.2 4.8 6.3
9.2 5.5 13.9 5.0 22.4 15.6 8.6 9.4 7.9 7.8 5.3 3.8
10.2 7.2 12.6 3.7 23.8 16.2 10.2 10.4 7.4 7.1 5.2 5.4
11.9 6.4 10.5 4.0 23.0 15.3 10.2 10.5 7.6 6.1 4.2 4.5
12.3 5.9 8.3 3.9 18.0 15.0 9.6 10.3 7.9 5.9 5.4 11.0
12.1 6.3 6.8 3.6 23.2 15.4 10.2 10.4 7.1 5.3 5.7 15.9
13.7 6.6 5.9 3.1 20.3 14.4 10.5 10.8 6.8 4.6 6.2 18.7
14.4 6.8 5.6 2.8 18.4 12.6 11.3 9.7 6.1 4.4 6.3 18.9
12.8 5.6 5.0 3.0 17.1 12.4 10.7 9.3 6.1 4.2 7.2 17.6
14.0 6.3 4.8 2.7 16.7 12.0 9.1 7.8 4.8 3.5 10.1 15.4
Table 2
General parameters observed for the pure LDH and LDH after adsorption of Asp and Glu under different conditions
Sample Medium particle
size (A)
SBET (m2 g�1) Pores’ total
volume (cm�3 g�1)
Pores’ medium
diameter (A)
Pure LDH 507.9 34.5 0.127 147.4
Asp 298 K; pH 7; I � 0 M 597.5 38.1 0.117 122.6
Asp 310 K; pH 7; I � 0 M 690.8 40.9 0.170 166.3
Asp 298 K; pH 7; I � 0.1 M 655.6 41.0 0.163 159.6
Asp 298 K; pH 10; I � 0 M 690.8 40.8 0.246 241.1
Asp 310 K; pH 10; I � 0 M 690.8 41.6 0.222 213.2
Asp 298 K; pH 10; I = 0.1 M 655.6 43.1 0.108 100.4
Glu 298 K; pH 7; I � 0 M 655.6 41.6 0.110 105.4
Glu 310 K; pH 7; I � 0 M 896.4 40.0 0.170 170.0
Glu 298 K; pH 7; I = 0.1 M 655.6 45.1 0.134 118.9
Glu 298 K; pH 10; I � 0 M 690.7 1.6 0.006 151.1
Glu 310 K; pH 10; I � 0 M 690.7 2.3 0.009 163.1
Glu 298 K; pH 10; I = 0.1 M 690.6 42.7 0.220 205.9
F. Silverio et al. / Applied Surface Science 253 (2007) 5756–5761 5759
Fig. 4. Left: PXRD; right: FT-IR (a) clean LDH; and LDH adsorbed with (b) Asp at 298 K, pH 7, I � 0.0 M; (c) Asp at 298 K, pH 10, I = 0.1M; (d) Glu at 298 K, pH
7, I � 0.0 M; (e) Glu at 298 K, pH 10, I = 0.1 M.
F. Silverio et al. / Applied Surface Science 253 (2007) 5756–57615760
The solids were characterized by PXRD and FT-IR analyses
before and after the adsorption experiments (Fig. 4). The PXRD
analysis shows there is no difference in the basal spacing of
7.6 A, which corresponds to intercalation of carbonate anions.
The fact that the basal spacing does not change gives evidence
that the there is no anionic exchange with the amino acid
anions. The FT-IR analysis shows the presence of organic
species in the LDH (Asp and Glu), as seen by the increase in the
two bands related to the asymmetric and symmetric stretches of
the carboxylate group at 1590 and 1400 cm�1, respectively.
The average particle size of the materials was calculated
from the PXRD data by means of the Debye–Scherer method
[37], and the results are shown in Table 2. The average particle
sizes of the adsorbed solids are close, and they are larger than
that of the pure LDH, which suggests an improvement in the
stacking of the LDH after adsorption. This is probably because
the adsorption process can organize and aggregate small
particles, thus producing larger particles.
The specific surface area (SBET) of the solids adsorbed with
Asp under different conditions is larger than that of the clean
LDH. The solids adsorbed with Glu also present larger SBET
than the clean adsorbent, except for the samples adsorbed at pH
10 and lower ionic strength, where the plateau is reached at a
much lower equilibrium concentration than the others,
producing solid aggregates with very small pores. The same
can be observed for the total volume of the pores.
4. Conclusions
This work presents a new alternative for the removal of
amino acids from aqueous solution with potential application in
the treatment of wastewater from industrial processes. Our
results have shown that adsorption occurs at a very efficient
extraction rate, even at high amino acid concentrations. The
removal of Asp and Glu by adsorption is greatly dependent on
the studied variables. Our results suggest that an increase in
temperature reduces the amount of removed amino acid, mainly
at higher concentrations. An increase in the pH value, from 7 to
10, results in an increase in the negative charge of the amino
acid and a reduction in the positive charge of the adsorbent,
consequently leading to a decrease in the amount of adsorbed
Asp and Glu. On the other hand, an increase in the ionic
strength, by addition of NaCl, results in a large increase in the
amount of removed Asp and Glu, except in the case of Glu at pH
10. This effect is probably due to the higher hydrophobic
character of Glu, which makes its adsorption less influenced by
the ionic strength, thus reducing the electrostatic character of
the adsorption, if compared with the electrostatic character of
Asp under the same condition.
Acknowledgements
The authors thank Coordenacao de Aperfeicoamento de
Pessoal de Nıvel Superior, CAPES, Conselho Nacional de
Desenvolvimento Cientıfico e Tecnologico, CNPq, and
Fundacao de Amparo a Pesquisa do Estado de Sao Paulo,
FAPESP for the financial support.
References
[1] R. Tanner, D. Enache, R.P.K. Wells, G. Kelly, J. Casci, G.J. Hutchings,
Catal. Lett. 100 (2005) 259.
[2] S. Velu, K. Suzuki, M. Vijayaraj, S. Barman, C.S. Gopinath, Appl. Catal.
B—Environ. 55 (2005) 287.
F. Silverio et al. / Applied Surface Science 253 (2007) 5756–5761 5761
[3] R. Anbarasan, W.D. Lee, S.S. Im, Bull. Mater. Sci. 28 (2005) 145.
[4] M.X. Zhu, Y.P. Li, M. Xie, H.Z. Xin, J. Hazard, Materials 120 (2005) 163.
[5] E. Klumpp, C. Contreras-Ortega, P. Klahre, F.J. Tino, S. Yapar, C. Portillo,
S. Stegen, F. Queirolo, M.J. Schwuger, Colloid Surf. A—Physicochem.
230 (2003) 111.
[6] F. Leroux, P. Aranda, J.P. Besse, E. Ruiz-Hitzky, Eur. J. Inorg. Chem. 6
(2003) 1242.
[7] J. Tronto, M.J. dos Reis, F. Silverio, V.R. Balbo, J.M. Marchetti, J.B.
Valim, J. Phys. Chem. Solids 65 (2004) 475.
[8] A. Vaccari, Catal. Today 41 (1998) 53.
[9] J. Roch, M. del Arco, V. Rives, M.A. Ulibarri, J. Mater. Chem. 9 (1999)
2499.
[10] K. Takehira, T. Kawabata, S. Shishido, K. Murakami, T. Ohi, D. Shoro, M.
Honda, K. Takaki, J. Catal. 231 (2005) 92.
[11] S. Aisawa, H. Kudo, T. Hoshi, S. Takahashi, H. Hirahara, Y. Umetsu, E.
Narita, J. Solid Stat. Chem. 177 (2004) 3987.
[12] P.C. Pavan, E.L. Crepaldi, G.D. Gomes, J.B. Valim, Colloids Surf. A—
Physicochem. 154 (1999) 399.
[13] M.J. dos Reis, F. Silverio, J. Tronto, J.B. Valim, J. Phys. Chem. Solids 65
(2004) 487.
[14] P.C. Pavan, G.D. Gomes, J.B. Valim, Microporous. Mesoporous. Mater. 21
(1998) 659.
[15] P.C. Pavan, E.L. Crepaldi, J.B. Valim, J. Colloid. Interf. Sci. 229 (2000)
346.
[16] P.C. Pavan, L.P. Cardoso, E.L. Crepaldi, J.B. Valim, Stud. Surf. Sci. Catal.
129 (2000) 443.
[17] G.N. Manju, M.C. Gigi, T.S. Anirudhan, Indian J. Chem. Technol. 6
(1999) 134.
[18] L.P. Cardoso, J. Tronto, E.L. Crepaldi, J.B. Valim, Mol. Cryst. Liq. Cryst.
390 (2003) 49.
[19] L.P. Cardoso, J.B. Valim, J. Phys. Chem. Solids 65 (2004) 481.
[20] K. Ohtsubo, K. Suzuki, Y. Yasui, T. Kasumi, J. Food Compos. Anal. 18
(2005) 303.
[21] I.L. Shih, Y.T. Van, Biores. Tech. 79 (2001) 207.
[22] C.H. Lee, S.W. Oh, I.H. Kim, Y.E. Kim, J.H. Hwang, K.W. Yu, Food Sci.
Biotech. 13 (2004) 167.
[23] R. Wattanapat, T. Nakayama, L.R. Beuchat, J. Food Sci. 60 (1995) 443.
[24] M.R. Cloninge, R.E. Baldwin, J. Food Sci. 39 (1974) 347.
[25] W.T. Reichle, S.Y. Kang, D.S. Everhardt, J. Catal. 101 (1986) 352.
[26] C.H. Giles, D. Smith, A. Huitson, J. Colloid Interf. Sci. 47 (1974)
755.
[27] D. Bitting, J.H. Harwell, Langmuir 3 (1987) 500.
[28] P. Somasundaran, D.W. Fuerstenau, Society of mining engineers, AIME
252 (1972) 275.
[29] D.A. Fridriksberg, K.P. Tikihomolova, M.P. Sidorova, Croatica Chem.
Acta 52 (1979) 125.
[30] P. Roy, D.W. Fuersten, Surf. Sci. 30 (1972) 487.
[31] P. Somasundaran, Croatica Chem. Acta 52 (1979) 67.
[32] M.J. Rosen, J. Am. Oil Chem. Soc. 52 (1975) 431.
[33] R. Denoyel, F. Rouquerol, J. Rouquerol, J. Colloids Surf. 37 (1989) 295.
[34] N.V. Sastry, J.M. Sequaris, M.J. Schwuger, J. Colloid Interf. Sci. 171
(1995) 224.
[35] C.C. Chan, S.S. Wang, J. Membr. Sci. 76 (1993) 219.
[36] D.N. Muravev, A.D. Saurin, Zhurnal Fizicheskoi Khimii 54 (1980)
1271.
[37] A.R. West, Solide State Chemistry and Its Applications, Chichester, 1987.