Xanthan gum–gelatin complexes
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Transcript of Xanthan gum–gelatin complexes
Xanthan gum–gelatin complexes
C.-y. Lii a,*, S.C. Liaw a, V.M.-F. Lai b, P. Tomasik a,c
a Institute of Chemistry, Academia Sinica, Nankang, 11529 Taipei, Taiwan, ROCb Department of Food and Nutrition, Providence University, Shalu, Taichung, Taiwan, ROC
c Department of Chemistry, University of Agriculture, Mickiewicz Avenue, 21, 31120 Cracow, Poland
Received 30 May 2001; received in revised form 25 October 2001; accepted 15 November 2001
Abstract
Gelatin (G) and xanthan gum (X) formed complexes either on bringing their blends to pH 2.3 or carrying out the
electrode process in aqueous blends of X and G at pHs from 9 to 11. X carboxylic groups and G peptide moieties were
involved in the interactions between the partners. Also non-coulombic interactions with involvement of NH and OH
groups, as well as hydrophobic interactions were involved, as proved by FTIR and thermal analyses, respectively. The
reaction yield declined with increase of concentration of G in the blends. Simultaneously, the thermal stability of the
complexes slightly increased with increase in G content in the blend. The latter increased with its concentration in
the reaction mixture. Slow formation by electrosynthesis provided more an organised matrix. � 2002 Elsevier Science
Ltd. All rights reserved.
Keywords: Coacervation; Electrosynthesis; Polysaccharide–protein complexes; Plant gums
1. Introduction
For over two decades polysaccharide–protein com-
plexes have received considerable attention for both
theoretical and practical reasons [1–5]. Gelatin (G) is
often used as protein component for complexes. It
can complex to carboxymethyl cellulose (CMC) with
involvement of electrostatic interactions [6]. Non-
coulombic interactions were essential in the formation
of complexes of G with pectins and alginates [7]. The
character of the interactions was dependent on the re-
action conditions, mainly on pH and ionic strength of
the reaction mixture, as proved in complexes of G with
CMC [8] and with gum Arabic [9].
Complexation of G with CMC was utilised in puri-
fication of these molecules [6] and complex formation
with acacia gum was patented as a fat replacer in
foodstuffs [10]. Complexes of G with acacia gum [11–16],
pectin [17], gellan gum [18], alginate [19], and CMC [19]
were considered as prospective sources for microcap-
sules.
Xanthan gum (X) as a polysaccharide component of
complexes with proteins was also subjected to numerous
studies. In a complex with milk protein prepared in the
pH range between 3.7 and 6.3, the components bound
via hydrophobic interactions [20]. Complexes of X with
milk proteins appeared to be interesting as potential
shortening agents for bakery, a fat replacer [21], and an
emulsifier for food industry [22,23]. Complexes of X
with soy protein [24,25], casein [24], ovalbumin [20,24],
and whey protein [26] may be used as meat and fat re-
placers. Purification of whey proteins by complexation
to X could be achieved [27].
In this paper, the synthesis and properties of the
complexes formed from G and X are described. Simul-
taneously, the electrode process formerly applied for the
synthesis of polysaccharide–protein complexes [28–32]
with covalent bonds between the partners is shown to be
useful for slow coacervation, providing a more organ-
ised matrix of the resulting complexes.
Although research on protein–polysaccharide com-
plexes has been addressed mainly in food science and
European Polymer Journal 38 (2002) 1377–1381
www.elsevier.com/locate/europolj
* Corresponding author. Tel./fax: +886-2-2783-1237.
E-mail address: [email protected] (C.-y. Lii).
0014-3057/02/$ - see front matter � 2002 Elsevier Science Ltd. All rights reserved.
PII: S0014-3057 (02 )00008-3
technology, the results of such studies might be poten-
tially utilised for non-nutritional purposes. Such mate-
rials could serve as sizes for textiles, fillers and thickeners
for pulp and paper, coatings, microcapsules, and bio-
degradable constructing materials.
2. Results and discussion
Electrosynthesis provided materials, which were 15–
7% richer in G than the blends from which they were
prepared. However, blends richer in G gave products
with a lower excess of G. Generally, the yield of the
products decreased with an increase in pH. High ratios
of G in initial blends resulted in a decreased yield. The
highest yield of the products separating on the anode
was achieved from X:G ¼ 1:2 blends (Table 1).
The current applied (Table 1) was automatically in-
creased with pH. In the blends of 1:1 and 1:2 X:G ratios,
the current rose with time. This might be an effect of a
decrease in solution viscosity caused by the separation of
the product. In the blends containing high ratio G, the
current either remained unchanged, or decreased with
time. The latter could result from the clathration of ions
and/or water in these G-rich products.
The solubility tests for X, G, and the products pre-
pared either by simple coacervation or electrosynthesis
(Table 2), particularly solubility in 7 M aq. urea, re-
vealed that coulombic interactions and formation of
hydrogen bonds between X and G were involved. Thus,
electrosynthesis did not promote formation of covalent
bonds between those partners and the process taking
place at the anode and in its vicinity was also a coac-
ervation process.
Coacervation of X with G took place at a pH of 2.3.
Differential FTIR spectra of 1:1 X–G complex (Figs. 1
and 2) and with the subtracted spectrum of X taken at
pH 2.3 (Fig. 2) showed that although the spectral pat-
terns resembled a simple combination of the spectra of
G and X, the essential band shifts could be observed.
Contrary to X CMC formed complexes with G in
which both partners were covalently bound [33]. X is a
polysaccharide, the anionic property of which results
from the presence of uronic acid moieties. The carb-
oxylic groups in X are directly bound to the pyranose
ring, and anionic properties of CMC result from the
presence of the carboxylic groups bound to the glucose
units through the 6CH2–O–CH2 linkage. The differences
in the bonding of the carboxylic groups in X and CMC
should not be reflected by any essential differences in
their ionisation. Therefore, availability of the carboxylic
Table 1
Composition and yields of X–G complexes
X:G ratio Intended G, % pH Formed Yielda, % Current change, A
Nitrogen content, % Gb, %
1:1 50 9 10.1 58.2 75 0:01! 0:03
10 10.0 57.8 73 0:01! 0:03
11 9.9 57.5 68 0:04! 0:051:2 67 9 12.6 72.6 77 0:01! 0:02
10 13.1 75.5 76 0:01! 0:02
11 12.8 73.9 73 0:04! 0:03
1:3 75 9 14.2 82.1 67 0:01! 0:0110 13.9 80.1 65 0:02! 0:02
11 13.1 75.9 55 0:05! 0:03
1:4 80 9 15.1 87.2 62 0:01! 0:0110 14.6 84.3 58 0:02! 0:01
11 14.7 85.0 54 0:05! 0:02
a The yields were calculated on the basis of the total parent polymer weight with standard deviations of 0.3–3.2%.bThe data were calculated from the nitrogen content in complexes and original G sample (17.29%).
Table 2
Solubility tests of G, X, and X–G complexes
Sample Solvent
H2O 5% Na2CO3 1% NaOH 7 M Urea DMSO 5% HCl
G–X complexesa – – þ þ – –
G – – þ þ þ þX þ – þ þ – þaAll complexes regardless the preparation method, initial composition of the blend and its pH.
1378 C.-y. Lii et al. / European Polymer Journal 38 (2002) 1377–1381
group for the complexing partner, which in X was much
more obstructed by steric hindrances seemed to be cru-
cial for the mode in which partners interact with one
another.
Electrosynthesis of G–X complexes proceeded in the
reaction mixtures of pH 9, 10 or 11 but the local pH
around anode could be different. Indeed, the FTIR
spectra of the 1:1 G–X complexes from both processes
were identical. Table 3 lists the wavelengths of the
spectral bands and their assignments.
The band shifts confirmed the involvement of the
carboxylic groups of X and peptide bond moieties of G
in the G–X interactions. Simultaneously, the shifts of the
vibration bands of the OH and NH groups showed that
non-electrostatic interactions might participate in coac-
ervate formation. The pH at which the syntheses were
carried out had no effect on the FTIR spectra, and
varying proportions of X and G in the initial blends
were reflected exclusively by relative peak intensities.
X was less thermally stable than G as shown by
thermogravimetric (TG) and differential thermogravi-
metric (DTG) analyses (Table 4).
Thermal stability of the products from electrosyn-
thesis slightly increased with an increase of G in prod-
uct. The effect of pH upon the thermal stability of
resulting products could be interpreted in terms of the
effect of pH upon the content of G in the product. At
higher pH, G content in the products decreased (Table
1) and, therefore, the latter slightly less thermally stable.
The processes of thermal decomposition for 1:1
products prepared by coacervation alone and by elec-
trosynthesis were practically identical (Fig. 3).
Slightly higher water content in the electrosynthes-
ised product might be a result of the slower and, per-
haps, more ordered building up of the matrix. The result
of the DTG analysis (Table 4) indicated that both
preparation methods produced products of different
macrostructure. Water in the product formed by coac-
ervation was held more strongly than in the product
prepared by electrosynthesis. It is suggested that the
latter procedure provided a more compact and, possibly,
a better organised matrix.
TG and DTG analyses showed that the X–G com-
plexes decomposed in three steps. The third step took
Fig. 1. FTIR differential spectrum of the 1:1 G–X product from
simple coacervation (below). The spectrum of X taken at pH
2.3 was subtracted from the spectrum of coacervate and spec-
trum of G taken at pH 2.3 was added for comparison (above).
Fig. 2. FTIR differential spectrum of the 1:1 G–X product from
simple coacervation (below). The spectrum of G taken at pH
2.3 was subtracted from the spectrum of complex and spectrum
of X taken at pH 2.3 was added for comparison (above).
Table 3
FTIR spectral patterns of G (at pH 2.3), X (at pH 2.3) and 1:1
G–X complex and the band assignments
m ðcm�1Þ Band assignment
1:1 G–X
complex
G X
3416 s 3416 s mOH intramolecularhydrogen bond
3368 s mNH intramolecularhydrogen bond
3081 sh 3081 w mOH polymeric association2928 w 2947 w 2918 w mC–H1719 m 1733 m mCOOH1652 s 1652 s 1642 m mC@O, dOH
1538 w mCOO�
1447 w 1447 w dCH1404 w 1404 w dCH
1380 m mCOO�
1333 w 1333 w dNH1252 m dCH
1242 m 1238 w dNH,mC�N1152 w 1152 m mC@O glucose units
1080 w dCOH1066 s 1061 s mC–O, mC–C, dCOH, C1–H1033 s 1028 s mC–O, mC–C, dOH, C4–O
C.-y. Lii et al. / European Polymer Journal 38 (2002) 1377–1381 1379
place at temperature above the decomposition point of
X and G and this thermal stabilisation might be ac-
counted for as a result of hydrophobic interactions.
Coacervation of X with G from solutions of X and G
suggested that such a process might be useful in recovery
of X from aqueous solution. Moreover, the increased
stability of the complexes under acidic conditions could
be of practical significance in formation of microcap-
sules, and in application as sizes and biodegradable
materials.
3. Experimental procedures
3.1. Materials
X (G1253) and G (type A from porcine skin, G2500)
were purchased from Sigma Chemical Co., St. Louis,
MO, USA.
3.2. Electrosynthesis
A 400-cm3 beaker equipped with two Pt electrodes
situated at a distance of 2.5 cm from one another was
used as an electrolytic cell. It was connected to a power
supply (model P-3003D, Taiwan). The beaker was filled
with 250 ml of aqueous solution containing 0.125 g of X
and 0.125, 0.250, 0.375 g of G. These concentrations
corresponded to X:G ratios of 1:1, 1:2, 1:3, 1:4 (w/w),
respectively. The polymer solution was completely dis-
solved in distilled water under conditions of mild heating
(�40 �C) and stirring, then cooled to room temperature.
The pH was adjusted to 9, 10 and 11 with 0.01 M
NaOH.
The electrosynthesis was conducted at a constant
potential difference of 12 V for 1.5 h. A layer of white,
gummy product was collected from the surface of anode,
centrifuged to remove liquid, and dried in vacuum at
room temperature.
3.3. Sample coacervation
Aqueous blends of X and G as described in Section
3.2 were adjusted to a pH 2.3 with 0.1 M hydrochloric
acid whilst being agitated. The resulting precipitates
were centrifuged to remove liquid, and dried in vacuum
at room temperature.
3.4. Combustion analysis
Combustion analysis was carried out with a Perkin
Elmer 2400 CHN elemental analyzer (Norwalk, CT,
USA). Analyses were duplicated. They varied by up to
0.25% of recorded values.
3.5. Solubility tests
The solubility of starting materials and the products
in water, 5% hydrochloric acid, 5% Na2CO3, 0.1–1 M
NaOH, DMSO, and 7 M aq. urea were examined at
25 �C.
Fig. 3. The TG curve of the 1:1 G–X product obtained by
simple coacervation (––) and by electrosynthesis (– – –).
Table 4
TG and DTG analysis of G, X as well as 1:1 X–G product
obtained by simple coacervation and by electrosynthesis
Sample Analysis TG DTGa
(�C)Temperature
of the effect
(�C)
Associated
weight lossb
(%)
G 156.4 10.2 75.7
227.3 11.4 307.7c
227.4 52.8
X 144.2 18.0 56.5
206.7 19.3 278.9c
324.5 56.7
1:1 G–X from
simple coacerva-
tion
124.3 9.2 66.7
180.0 10.2
240.0 17.5 234.9
270.0 27.5 293.8c
370.0 60.0 337.1
1:1 G–X from
electrosynthesis
124.6 10.1 60.9
180.0 11.2
240.0 18.0 237.5
270.0 28.0 296.4c
370.0 60.0 333.7
aAll effects were endothermic.b The weight loss from the origin.c The dominating effect.
1380 C.-y. Lii et al. / European Polymer Journal 38 (2002) 1377–1381
3.6. FTIR analysis
The infrared spectra of X, G, and their complexes
were run in KBr discs using a Perkin Elmer FTIR
spectrometer Paragon 1000 (Norwalk, CT, USA), in the
frequency range of 4000–500 cm�1. Differential spectra
of X–G complexes and pure X or G were also recorded.
3.7. Thermal analysis
The thermal characteristics of pure X, G, and X–G
complexes were determined under a nitrogen stream
using a Du Pont TGA 951 system (Wilmington, DE,
USA) scanned from 25 to 500 �C at 10 �C/min.
4. Conclusions
Regardless of preparation methods, X and G formed
complexes with the involvement of weak electrostatic
and non-electrostatic interactions between X and G. The
matrix of the product formed from electrosynthesis
could be more regularly in structure. The role of the
electrode process carried the formation around the an-
ode of a concentration of protons suitable for coacer-
vation of G and X.
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