A 'Green' Chitosan Silver Nanoparticle Composite as a Heterogeneous as Well as Micro-heterogeneous...
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IOP PUBLISHING NANOTECHNOLOGY
Nanotechnology19(2008) 015603 (9pp) doi:10.1088/0957-4484/19/01/015603
A green chitosansilver nanoparticlecomposite as a heterogeneous as well asmicro-heterogeneous catalyst
A Murugadoss1 and Arun Chattopadhyay1,2
1 Department of Chemistry, Indian Institute of Technology Guwahati, Guwahati 781 039, India2 Centre for Nanotechnology, Indian Institute of Technology Guwahati, Guwahati 781 039,
India
E-mail:[email protected]
Received 3 July 2007, in final form 8 October 2007
Published 29 November 2007
Online atstacks.iop.org/Nano/19/015603
Abstract
In this paper, we report on the catalytic activity of a new metal nanoparticlepolymer composite
consisting of Ag nanoparticles (NPs) and environmentally friendly (green) chitosan. The
polymer (chitosan) not only acted as the reducing agent for the metal ions, but also stabilized
the product NPs by anchoring them. The majority of the particles produced in this way had
sizes less than 5 nm. The catalytic activity of the composite was investigated photometrically by
monitoring the reduction of 4-nitrophenol (4NP) in the presence of excess NaBH4in water,
under both heterogeneous and micro-heterogeneous conditions. The reaction was first order
with respect to the concentration of 4NP. We also observed that the apparent rate constant, kapp,
for the reaction was linearly dependent on the amount of Ag NPs present in the composite.Moreover, the turn-over frequency (TOF) of the catalyst was found to be
(1.5 0.3) 103 s1, when the reaction was carried out under heterogeneous conditions. The
Ag NPs in the composite retained their catalytic activities even after using them for ten cycles.
Our observations also suggest that the catalytic efficiency under micro-heterogeneous
conditions is much higher than under heterogeneous conditions. Thus the composite we have
represents an ideal case of an environmentally friendly and stable catalyst, which works under
heterogeneous as well as micro-heterogeneous conditions with the advantage of nanoscopic
particles as the catalyst.
S Supplementary data are available from stacks.iop.org/Nano/19/015603
1. Introduction
The future of sustainable nanoscale science and technology not
only depends on overcoming knowledge barriers in developing
newer principles, but also on appropriately addressing the
environmental and societal concerns, especially when large-
scale material production is involved. The primary challenges
in this regard are the maximization of usage of environmentally
friendly materials and integration of the principles of green
chemistry, as far as chemistry is involved, in the generation
of nanoscale-based products. Among the many products that
have been developed, polymermetal nanoparticle composites
seem to receive special attention because of their applicationpotential in sensors [1], actuators [2], electrodes for fuel
cells [3], supported micro-heterogeneous and heterogeneouscatalyses [4], and in optical and optoelectronic devices [5].
Also, advantages of mechanical, optical, thermal and electrical
properties of the polymer and optical, electrical and catalytic
properties of the metal NPs can be suitably integrated to
achieve superior performance. For example, we have for the
first time synthesized Au nanoparticlepolyaniline composite
in a single reaction condition where the composite product had
higher electrical conductivity in comparison to the polymer
alone [6]. We have subsequently developed methods of
synthesis of a polymermetal composite nanoparticle and a
polymerTiO2 nanoparticle thin film composite with superior
photocatalytic properties [7]. In addition, we have alsodemonstrated that an Au NPpolyaniline composite on a resin
0957-4484/08/015603+09$30.00 2008 IOP Publishing Ltd Printed in the UK1
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bead could act as a catalyst for the oxidation of glucose with
simultaneous colorimetric detection of the product [8]. Several
other groups have subsequently developed various synthetic
schemes for the generation of metal NPpolymer composites
for appropriate applications. For example, Ballauff and
co-workers [9] have synthesized several metal NPpolymer
composites for catalysis with incorporation of thermosensitiveactivity as one of the major advantages. On the other hand,
Gronnowet al[10]have used an expanded starch supported Pd
catalyst with high activity for Suzuki, Heck and Sonogashira
reactions. Among the metal NPs, Ag NPs generated under
various conditions are known to be efficient catalysts for the
reduction of organic dyes [11] and also for the reduction of
4-nitrophenol (4NP) to 4-aminophenol (4AP) [12]. However,
incorporation of Ag NPs into polymer, especially biopolymer,
has not received much attention, possibly because of the
experimental difficulty in the syntheses of composites.
Chitosan, a novel biopolymer, is a product of deacetylation
of chitin, which is the second most abundant natural
polymer in the world after cellulose. The biocompatibilityand antibacterial properties of chitosan and its being an
environmentally friendly polyelectrolyte makes it appealing
for several applications such as water treatment [13], novel
fibers for textiles [14], photographic paper[15], biodegradable
films [16], biomedical devices and microcapsule implants for
controlled release in drug delivery [17]. Thus a composite
of Ag NPs and chitosan would ideally be suited for various
commercial applications, especially if generated under benign
conditions. Although there are methods that are available for
the synthesis of Pd NPchitosan composite, currently there
is no simple method of synthesis of an Ag NPchitosan
composite.
Herein we report the development of a mild one-step
method of Ag NPchitosan composite, by using chitosan as the
reducing agent, at 95 C and in the presence of aqueous sodium
hydroxide. The NPs produced in the medium get attached
to the chitosan and are stable for weeks without noticeable
change in properties. The NPs produced were small, with sizes
mostly below 5 nm, and were found to have high catalytic
activity. Also, the amount of Ag NPs produced could be
easily controlled by controlling the amount of starting material
(AgNO3), without significant variation in sizes. We have
studied the catalytic reduction of 4NP to 4AP by the composite
using NaBH4 as the reducing agent, under both heterogeneous
and micro-heterogeneous conditions. When the heterogeneouscatalytic reaction was carried out in the presence of excess
NaBH4, it was observed to follow pseudo first-order kinetics
and the apparent rate constant depended linearly on the
concentration of Ag NPs present in the composite. The turn-
over frequency (TOF) was observed to be (1.5 0.3)
103 s1, when the reaction was carried out in heterogeneous
conditions. Interestingly, we observed that the composite
could be used for catalyzing the same reaction at least for ten
cycles without significant loss of its activity. Transmission
electron microscopy (TEM) evidence indicated that Ag NPs
were present and sizes were retained even after several cycles
of catalytic reductions. Further, when the reaction was carried
out in micro-heterogeneous conditions the rate constant wasmuch higher.
2. Experimental details
2.1. Materials
Silver nitrate (AgNO3, 99.5%; Merck), acetic acid (glacial,
99100%; Merck), chitosan of high molecular weight (75%
deacetylated; Sigma-Aldrich), sodium borohydride (NaBH4,
95%; Merck), sodium hydroxide (NaOH, 98%; Merck) and4-nitrophenol (95%; Merck) were used as received without
further purification. Milli-Q grade water was used in all
experiments.
2.2. Synthesis of the chitosanAg nanoparticle composite
A 100 ml beaker containing 50 ml of Milli-Q water was kept in
an oil bath at a temperature 9395 C with constant magnetic
stirring. This was followed by addition of 0.1 g of chitosan
into the beaker. A freshly prepared 1 ml solution of 20 mM
AgNO3 was then added to this mixture, which was followed
by addition of 100
l of 0.3 M NaOH. The pH of the solutionwas measured to be 10.4. The resultant solution turned yellow
in about a minute, indicating the formation of Ag NPs in the
medium. The reaction was allowed to continue for additional
10 min. Finally, powdered yellow colored solid appeared at the
bottom of the beaker. The beaker was then taken out from the
oil bath and cooled to room temperature. This was followed
by separation and washing of the powder with Milli-Q water
five times. The solid was then air dried and kept for further
use. The filtrate was treated with concentrated HCl to check
for any excess of Ag+ present in the medium; the result was
negative. In other words, all of the Ag+ ions had reacted in the
production of Ag NPs.
In order to prepare chitosanAg NPs composites withvarying amount of Ag, the concentration of AgNO3 was
appropriately varied, keeping all other conditions the same.
2.3. Catalysis study
2.3.1. Heterogeneous conditions. Investigations of the
catalytic activity of chitosanAg NP composites with different
Ag content were pursued in the following way, using the
reduction of 4NP to 4AP by NaBH4 as a model reaction. In
a 3 ml quartz cuvette, a given amount of chitosanAg NP
composite powder was added and this was followed by the
addition of 2.5 ml of 10 mM NaBH4
solution. Subsequently,
25 l of 10.0 mM of 4NP was added to the mixture and the
cuvette was shaken vigorously for mixing. The cuvette was
then placed in a UVvisible spectrophotometer to monitor the
time-dependent absorption at 400 nm at room temperature (23
24 C).
2.3.2. Micro-heterogeneous conditions. 40 mg of Ag NP
chitosan composite was dissolved in 20 ml 0.1% (V/V) acetic
acid in water. The corresponding solution of the pH was found
to be 4.3. The pH of the solution was then adjusted to around
6.3 by the addition of NaOH solution. This stock solution was
used for further catalysis studies under micro-heterogeneous
conditions. The resultant solution was also used for physicalcharacterization studies of the composite. For catalysis studies,
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Figure 2.(a) and (b): transmission electron micrographs of the chitosanAg NP composite; (c) is the particle size distribution histogram asobtained from figure2(a), and (d) is the selected area electron diffraction pattern corresponding to a particle.
with increase in absorption intensity. This implies that when
the concentration of silver ions was increased, the loading ofthe silver content also increased on the chitosan. However,
increasing the number of Ag+ ions led possibly to an increase
in the number of NPs but not their size. It is also possible that
their size decreased with the loading. This could be due to
different nucleation mechanisms operating at lower and higher
Ag+ concentrations attached to chitosan.
It is important to mention here that the excess amine and
hydroxyl groups present in the chitosan polymer support the
nucleation as well as stabilization of the Ag NPs formed in the
process. In other words, the Ag NPs adsorbed on the surface
of the polymer are prevented from further aggregation. In
order to investigate the size distribution of the Ag NPs on the
surface of the chitosan polymer, TEM studies were pursued.
Typical TEM micrographs of drop cast composite are shown
in figures 2(a) and (b), and the corresponding particle size
histogram, corresponding to the micrograph 2(a), is shown
in figure2(c). As is clear from the figures, small NPs were
formed and deposited all over the polymer. The majority
of the particles formed had sizes less than 5 nm. It is also
interesting to note that the particles were rather uniform in
size. The selected area diffraction (SAD) pattern of the NPs
(figures 2(d)) consisted of a hexagonal structure of the (111)
face of single-crystalline Ag NPs. Also, these results correlated
well with the dynamic light scattering study of the composite
particles. The dynamic light scattering (DLS) measurementsof the composite, dissolved in 0.1% (V/V) acetic acid
in water, also indicated the formation of small particles
with nearly uniform particle size distribution. A typicalparticle size histogram from DLS measurements is shown
in the electronic supplementary information (ESI; figure S3
(available at stacks.iop.org/Nano/19/015603). Clearly, more
than 90% of the particles formed were of sizes in the range 2
4 nm, with the majority of particles formed being about 3.0 nm
in diameter. Thus the present method could produce stable,
small sized Ag NPs in the form of chitosanAg NP composite
with uniform and narrow particle size distributions.
Also important to mention here is the observation that
when chitosanAg NP composite was dissolved in 0.1% (V/V)
of acetic acid in water and kept for a couple of months,
no discernible precipitation could be observed and there was
no change in the UVvisible spectrum, indicating that these
particles were also stable in solution form when present with
the polymer as composite. The ease of synthesis of chitosan
Ag NP composite and the stability of the NPs in the composite
provide opportunities for applications, especially with respect
to the catalysis of important chemical reactions. This is
especially advantageous where the NPs act as the catalyst and
the adherence of the NPs to the bulk and insoluble polymer
helps in recovery and thus repeated use. In order to test the
efficacy of the present composite in catalyzing heterogeneous
chemical reactions, we have studied the reduction of 4NP
to 4AP by NaBH4 in the presence of the composite. The
reactions have been monitored spectrophotometrically. Also,important to mention here is the use of excess NaBH4 so that
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Table 1. ChitosanAg NP composites used in the catalysis studies and corresponding Ag NPs present in the reaction mixture. For thesynthesis of the composite, 0.1 g of chitosan and 0.4 mM AgNO 3in 50 ml solution were used. Different amounts of the composite were takenfrom the powder generated from this reaction medium.
Sl. No.
Amount of chitosanAg NPcomposites in unit volume ofcatalysis reaction mixture
(g l1)
Corresponding amount of Agpresent in the composite inthe catalysis reaction mixture
(mg l1)
Concentration of Ag inthe composite in thecatalysis reactionmixture
(103 mol dm3)
1 0.40 21 0.192 1.20 63 0.583 1.60 84 0.774 2.00 105 0.975 2.84 149 1.336 3.24 170 1.577 3.60 189 1.758 4.40 231 2.179 5.20 273 2.53
Figure 3.UVvisible spectra of solution of 4NP measured atdifferent time intervals in the presence of chitosanAg NP compositeparticles. The reaction conditions were as follows: [4NP]
= 0.1 mM dm3, [NaBH4] = 10 mM dm3, amount of chitosanAgNP composite powder = 2.1 mg in 2.5 ml (i.e. the concentration ofAg was 0.4 mM).
the kinetics of the reaction could be followed as a function of
concentrations of Ag NPs. An aqueous solution of 4NP shows
a distinct spectral profile with an absorption maximum at
317 nm, which shifts to 400 nm in the presence of NaBH4due
to the formation of the 4-nitrophenolate ion[20]. The anionic
species remain stable for weeks in the absence of any other
reagent. However, in the presence of the solid chitosanAg NP
composite the peak at 400 nm gradually decreased with time,along with the appearance of a new peak at 290 nm, which is
known to be due to absorption of 4-amino phenol [20b].
A typical time-dependent catalytic reduction of 4NP as
followed spectrophotometrically is shown in figure 3. As
is clear from the figure, under the reaction conditions, the
reduction took place in about 25 min. Also important to note
is the presence of an isosbestic point at 320 nm (figure 3)
indicating the formation of the product 4AP as a result of
reduction from 4NP. We further pursued the investigations with
respect to the rate of the reaction as a function of concentration
of the catalyst (Ag NPs) in the composite.
This was achieved by varying the amount of composite
while keeping the ratio of chitosan to AgNO3 the same, as
indicated in table 1. Since our observations indicated the
Figure 4. Plot of the absorbance atmaxof 4NP versus time fordifferent amounts of chitosanAg NP composite per unit volume.Corresponding concentrations of Ag in heterogeneous condition aregiven in table1.The reaction conditions were as follows: [4NP]= 0.1 mM dm3 and [NaBH4] = 10 mM dm
3.
absence of Ag+ in the medium after the formation of the
composite, it is possibly safe to assume that all the Ag+
ions present in the medium resulted in the formation of NPs
in the composite. Also, since the particle size distribution
studies indicated that the NPs formed were nearly uniform
in size and spherical in nature, we have used the method
adopted by Pikeramenou et al [21] to calculate the number
of particles present in each amount of composite used for
catalysis. Also, the same method was used to calculate the
number of surface atoms present in the NPs, which was further
used for the calculations of turn-over frequency (TOF). The
details of the method and calculations are included in the
ESI. For each concentration of the composite (and thereby
Ag NPs) the conversion of the 4NP to 4AP was studied
by following the time-dependent absorption changes of 4NP
spectrophotometrically, as before. Since the absorbance of
4NP is proportional to its concentration in the medium, the
ratio of absorbance at timet(A)to that att= 0 (t0), i.e. A/A0,
could be used as the ratio of concentrations of 4NP at timet to that at t0 (i.e. A/A0 = c/c0). The concentrations of
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4NP and NaBH4 (used in excess) were kept constant for all
the reactions. The amount of chitosanAg NP composite used
in each of these reactions is indicated in table 1. Since the
concentration of NaBH4used in the reactions was in far excess
of that of 4NP, the reaction can be considered as a pseudo first-
order reaction. The rate of the reaction is then proportional to
the concentration of 4NP alone, and can be written as follows.
dct
dt ct. (1)
Here, ctis the concentration of 4NP at time t. We observed
that the rate of the reaction increased with the increase in the
amount of chitosanAg NP composite used for the reactions.
A plot of the normalized concentration change as a
function of time for the reduction of 4NP for various amounts
of chitosanAg NP composite (and thus Ag NPs) is shown
in figure 4. As is clear from the figure, the longest time
taken for the completion of the reaction was 32 min, when the
concentration of the Ag used was 0.19 mM. On the other hand,
the reaction was over in about 5 min when the concentration
was 2.53 mM. Thus the catalytic reaction was sensitive to
the amount of Ag NPs present in the composite. It is also
interesting to note that when the concentration of the catalyst
was low (0.19 mM) there was significant induction period
(about 13 min) in the reaction, whereas the reaction started
immediately when the concentration was high (2.53 mM). At
the intermediate concentrations the induction period was also
in between the above values, and it decreased with the increase
in the concentration of the catalyst. The induction periods
and their reduction with the concentration of the catalysts have
been observed also by previous researchers working with metal
NPs and have been attributed to the activation of the catalystpresent in the reaction mixture [20b,22]. In view of the above
observations, equation(1) can be rewritten as
dct
dt= kappct, (2)
where ctis the concentration of p-nitrophenol at time t, and
kapp is the apparent rate constant, which is a function of the
concentration of the chitosanAg NPs used. A plot of the
apparent rate constant with the concentration of the catalyst, as
obtained from the ln(c/c0)versus time plot using the data from
figure4,is shown in figure5(a). As is clear from the figure, the
apparent rate constant of the reaction is linearly proportional tothe amount of catalyst used for the reaction. Thus equation (2)
can be written as
dct
dt= kappct= k1cAgNPct= k
1WchiAgct, (3)
where cAgNPs is the concentration of Ag present in the
composite as per table1;WchiAgis the weight of the chitosan
Ag NP composite present in a unit volume of the system, which
we observed to increase linearly with the amount of Ag+ in the
parent salt that was used to generate the composite (figure5).
k1 and k1 are constants. Since the reaction carried out was
heterogeneous and the same volume of reaction mixture was
used for all the reactions, the weight (WchiAg) used hereincan be assumed to be equivalent to the concentration of Ag
Figure 5. The plot of rate constantkappobtained from figure4. Plot(a) represents the rate constantkappas a function of the amount of
chitosanAg NP composite normalized to the unit volume of thesystem and plot (b) shows the rate constant variation withconcentration of Ag.
NPs (cAgNPs). We have calculated the rate constant (k1)
of the reaction in the present system from the slope of the
graph in figure5(b). The rate constant (k1) was found to be
1.06 mol1 dm3 s1.
An important parameter indicating the efficiency of a
catalyst is the turn-over frequency (TOF). Since the surface
atoms of the catalyst are involved in the catalysis, the efficiency
is related to the number of surface atoms present in the catalyst.
And since the number of surface atoms present in NPs is high
compared to the volume the efficiency is expected to be higher
for NPs in comparison to the bulk catalyst, especially when the
surface to volume ratio is the overriding determining factor.
The TOF is defined as
TOF =M
Ns t, (4)
whereMis the number of molecules (4NP here) reacting in the
presence of catalyst in timetto produce the product, and Ns is
the number of surface atoms of the catalyst that is involved in
the reaction. In calculating the TOF we have assumed that the
average particles size of Ag NP was 4 nm, which was obtainedfrom the TEM picture. Since the amount of Ag as well as
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Table 2. Calculation of the number of surface atoms and TOF (turn-over frequency) with induction period and without induction period. Thevalues in the rows, i.e. number of Ag NPs, correspond to the amount of chitosanAg NP composite as in table 1.
Sl. No.
No. of Ag NPs
(NNPs) 1014
No. of surfaceatoms(NS) 10
17
Time (s)includinginduction period
Time (s)excludinginduction period
TOF(s1) 103
includinginduction period
TOF(s1) 103
excludinginduction period
1 0.60 0.37 1920 1110 2.10 3.6
2 1.80 1.12 1404 804 0.95 1.63 2.40 1.49 984 594 1.00 1.74 3.01 1.87 750 432 1.00 1.85 4.27 2.66 576 378 0.98 1.56 4.87 3.03 510 354 0.97 1.47 5.41 3.33 438 348 1.00 1.38 6.61 4.12 396 306 0.92 1.29 7.82 4.85 330 240 0.94 1.3
Figure 6.Reusability of the composite catalyst as demonstrated byseveral cycles of reactions catalyzed by the same catalyst. The plot
indicates changes in the visible absorption spectra of 4NP due to thereduction to 4AP, as a function of time, for several cycles of use ofthe composite catalyst. The numbers in the right box indicate thecycle number in the catalysis.
the number of Ag NPs were known, the number of surface
Ag atoms present for each amount of composite was then
calculated. Also, the number of reactant molecules (4NP) used
for each case was fixed at 1.50 1017. Hence the TOF was
calculated for each of the reactions carried out with different
amount of catalyst. Table2 lists the amount of Ag NPs used,
the total time taken and the TOF for each reaction. The average
value of TOF was found to be (0.970.02)103 s1. Thesecalculations were performed using the total time as observed,
which included the induction periods for lower concentrations
of Ag NPs (and the lowest concentration data were not
considered). However, if we subtract the induction time period
and discount the first data (with very low concentration of
catalyst) then an average value of(1.5 0.3) 103 s1 was
found for the TOF. This value is reasonable for a nanocatalyst
such as small Ag NPs, and is consistent with the literature
value. One may point out that since Ag NPs are supported
on the chitosan the exact number of surface atoms may not be
exactly the same as the calculated value. However, as indicated
in table2,the consistency of the TOF value at different Ag NP
concentrations suggests that the effect of the support if any may
be minimal in terms of error in the calculation.
We were further interested in finding out the reusability
of the catalyst. For this we carried out a set of reactions, in
sequence, where the ratio of the amount of catalyst (chitosan
Ag NP composite) and the reactant (4NP) were kept nearly
the same. For example, 10 mg (the concentration of Ag was1.9 mM) of the composite was taken in a cuvette with the
addition of 2.5 ml of a solution containing 4NP and NaBH4as before (see the caption of figure 3). Once the reactions
were over (as observed by the absorbance decay of 4NP), the
composite was recovered by decantation of the liquid (using
a micropipette). This was followed by washing of the solid
composite with Milli-Q grade water and decantation of the
liquid again. Then 2.5 ml of the same reaction mixture was
added to the cuvette. The absorbance decay of 4NP with time
was followed as before. The completion of the reaction was
taken as the completion of the second cycle. Similarly, the
cycles were pursued eight more times to have ten cycles ofreaction using the same catalyst. The results are shown in
figure6. As is clear from the figure, the catalytic activity was
retained quite well, even up to the tenth time. For example,
whereas the reaction was completed in 516 s in the first cycle,
it took 1716 s to be completed in the fifth cycle, while the
same reaction took 1075 s in the eighth cycle. The apparent
difference between the progressive cycles could be due to the
loss of catalyst during handling in between two cycles. Also,
oxidation of Ag NPs and subsequent reduction by NaBH4,
while in the composite (in the reaction medium), may alter the
average size of the particle, which may also be the reason for
observed differences between cycles. This means that the AgNPs were stable in the composite and retained their activity.
That the catalytic Ag NPs were stable and remained attached to
chitosan polymer was evident from the TEM measurements of
the catalyst after four cycles of catalytic reactions. The typical
TEM pictures shown in the ESI (figure S3(a) available at
stacks.iop.org/Nano/19/015603 ) clearly indicate the presence
of small Ag NPs in the composite after the fourth cycle
of operation. The SAED patterns (figure S3(b) available at
stacks.iop.org/Nano/19/015603 ) corresponding to the NPs also
corroborate the presence of Ag NPs. These results show that
metal NPs on the surface of the chitosan were not getting
leached significantly during the course of the reaction. This
possibly indicates that the strong affinity of chitosan for AgNPs stabilizes the NPs on the surface and that might prevent
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Figure 7.Plot of the absorbance atmaxof 4NP versus time, in thepresence of different amounts of chitosanAg NP composite per unitvolume. The reaction was conducted under micro-heterogeneousconditions. The reaction conditions were as follows: [4NP]= 0.1 mM dm3, [NaBH4] = 10 mM dm
3.
the metal from leaching during the catalytic reaction. Thus we
have an efficient, workable, easily recoverable Ag NP catalyst
with reasonably high TOF. This is important in terms of value
of a catalyst in industrial applications.
Finally, we were further interested in finding the potential
of the composite as a catalyst working under micro-
heterogeneous conditions for increased efficiency. This would
be even more advantageous if the reaction conditions were
such that the composite would be dispersible in the reaction
mixture at a certain pH and the reaction could be carried out
without the catalyst getting precipitated out of the solution.
Fortuitously, the Ag NPchitosan composite was dispersiblein the reaction mixture (aqueous solution) up to a pH of 6.3,
and the reduction of 4NP to 4AP could be carried out under
this condition using NaBH4 as the reducing agent afterwards.
The results of the catalysis of the conversion of 4NP to 4AP
by the composite in the presence of NaBH4 are shown in
figure7. As is evident from the figure, the reduction of 4NP
under micro-heterogeneous conditions was much faster than
that while using the catalyst under heterogeneous conditions
(figure 4). Also important to note is that the concentrations
of catalyst needed to carry out the same reaction (with
similar concentrations of reactants) were much less when
carried out in micro-heterogeneous conditions in comparison
to heterogeneous conditions. For example, while the catalyst
concentrations needed under heterogeneous condition were on
the order of several g l1, the same reaction could be achieved
in similar times using catalyst concentrations of mg l1. This
indicates that the reaction when carried out using the composite
as the catalyst under micro-heterogeneous conditions is much
more efficient than under heterogeneous conditions.
That the reaction is faster in micro-heterogeneous
conditions can be explained using the concentration of metal
NPs present in the medium, where the rate will directly depend
on the available surface area of the NPs in the medium. In that
case the rate of the reaction can be expressed as
dct
dt= kappct= k2 Sct, (5)
Figure 8. Plots of the rate constantkappobtained from figure7(reaction under micro-heterogeneous conditions). Plot (a) represents
the rate constantkappas function of the amount of chitosanAg NPscomposite and plot (b) shows the rate constant variation withconcentration of Ag normalized to the unit volume of the reactionsystem under micro-heterogeneous conditions.
wherec tis the concentration of 4NP at time t, k2 is the rate
constant, and Sis the total available surface area of the NPs
in the medium (normalized to unit volume of the system).
The validity of this approximation can be made from figure 7,
where it can be observed that increase in the concentration
of the chitosanAg NP composite leads to a rapid increase
in the rate of the reaction. Also, the values of rate constants
in figure 8 support that the apparent rate constant kapp isproportional to the total surface area of the NPs as well as
the concentration of chitosanAg NP composite used in the
system. Further, the amount of chitosanAg NP composite
used in the micro-heterogeneous reaction conditions is much
smaller than that in heterogeneous conditions. From the above
observations, it can be concluded that the rate of the reaction in
the micro-heterogeneous conditions, which can be carried out
with less amount of catalyst, is much faster than that under
heterogeneous conditions. Finally, our observations suggest
that the catalytic activity of chitosanAg NP composite that
we have prepared is much higher in comparison to results
available in the literature. For example, Pradhan et al [12]
have used Ag NPs with an average size of about 25 nm tocatalyze 4NP to 4AP using NaBH4 and have obtained a rate
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8/12/2019 A 'Green' Chitosan Silver Nanoparticle Composite as a Heterogeneous as Well as Micro-heterogeneous Catalyst
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Nanotechnology 19(2008) 015603 A Murugadoss and A Chattopadhyay
constant kapp = 2.3 103 s1 with 5.0 106 mol l1
Ag catalysts at 20 C. The rate constant when normalized
with the surface area of the catalyst was calculated to be
k= 3.78 107 s1 m2 l. On the other hand, Lu et al[22]
synthesized Ag NP composite with a thermosensitive polymer,
having average diameter of the Ag NPs between 8 and 10 nm,
to catalyze the above reaction. They obtained a rate constantk= 5.2102 s1 m2 l, higher than that obtained by Pradhan
et al [12]. In our case, with the sizes of the Ag NPs (in the
composite) much smaller, the rate constant was calculated from
figure8(b) to bek2 = 1.5 101 s1 m2 l, which is higher
than the literature reports. However, considering the sizes of
the NPs in the present system and also the catalyst working in
micro-heterogeneous conditions, this increase in rate constant
is not surprising. The present set of results demonstrate
that the conditions of reaction (micro-heterogeneous versus
heterogeneous) and sizes of the particle (catalyst) are crucial
in catalysis involving metal NPs.
4. Conclusion
We have developed a simple synthetic scheme for the
generation of stable chitosanAg NP composite with high
catalytic activity. The NPs generated in the present method
were of uniform and narrow particle size, with typical size
less than 5 nm. The composite was tested for heterogeneous
catalysis, with Ag NPs being the active catalyst and chitosan
as the support. The catalytic efficiency for the reduction of
4NP to 4AP for the composite was high, with a TOF value
of(1.5 0.3) 103 s1. The small particle size and thus
high number of surface atoms makes the composite a rather
appealing material for catalysis and other applications. Further,the additional advantage of being able to use the catalyst under
micro-heterogeneous conditions makes its usefulness rather
appealing. To the best of our knowledge, there exists no
other report of chitosan being used as a reducing agent for
the production of Ag NPs as well as their stabilizer, although
reports exist of functional NPs that were separately attached
to chitosan for catalysis. The synthetic method, which we
have developed in the present study, might be useful for
further development of green NP synthesis in other situations.
Since chitosan is biocompatible, the composite can be useful
for biological applications, which we are currently pursuing.
Since chitosan can be made in the form of beads, fibers, andmembranes, the application potential of the composite could
become even more versatile.
Acknowledgments
We thank the Department of Science and Technology,
Government of India, for financial assistance (DST Nos
SR/S5/NM-01/2005 and 2/2/2005-S.F.).
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