J. Biomedical Science and Engineering, 2010, 3, 735-741 JBiSE
doi:10.4236/jbise.2010.37098 Published Online July 2010 (http://www.SciRP.org/journal/jbise/).
Published Online July 2010 in SciRes. http://www.scirp.org/journal/jbise
Removal of hexavalent chromium by an aromatic alcohol
Ankita Basu, Rumpa Saha, Jayashree Mandal, Sumanta Ghosh, Bidyut Saha*
Bioremediation Lab, Department of Chemistry, the University of Burdwan, Golapbag, India;
Email: b_saha31@rediffmail.com
Received 17 May 2010; revised 21 May 2010; accepted 28 May 2010.
ABSTRACT
Cr(VI) is a widespread environmental contaminant
and a known human carcinogen. Biosorption is a
very common method to remove toxic Cr(VI) from
industrial waste water. In biosorption Cr(VI) is re-
duced to less toxic Cr(III) and adsorbed in biosor-
bent as Cr(III). Effective biosorbents contain hydro-
xy groups; it may be aliphatic or aromatic. Kinetics
of reduction of Cr(VI) by an aromatic alcohol, benzyl
alcohol, (which is an important volatile component of
flowers of some night blooming plants) in micellar
media have been studied spectrophotometrically.
Micellar media is a probe to establish the mechanistic
paths of reduction of Cr(VI) to Cr(III). Effects of
electrolytes are studied to support the proposed reac-
tion mechanism. Suitable surfactant & suitable con-
centration of electrolyte enhance the biosorption pro-
perty.
Keywords: Biosorption; Carcinogen; Kinetics; Chro-
mium (VI); Benzyl Alcohol; Non Functional Surfactants;
Salt Effect
1. INTRODUCTION
Chromate [Cr(VI)] compounds are widely used in in-
dustry. Large amounts of toxic Cr(VI) are annually re-
introduced into the environment through the discharge
of chromium-containing industrial waste [1-4]. In the
last few decades, the amount of chromium in aquatic
and terrestrial eco-systems has increased a consequence
of different human activities. Chromium is the new en-
try, after lead, cadmium and mercury in the major toxic
metal series. In the Hinkley (a small desert town in San
Bernardino Country, USA) case hexavalent chromium
was used by Pacific Gas and Electric Company (PG &
E) in cooling systems to prevent pipes from rusting. The
runoff of hexavalent chromium contaminated water on
the PG & E property, seeped into the ground and con-
taminated local water supplies. PG & E was required to
compensate the plaintiffs $ 333 million, clean up the
hexavalent chromium contamination, and stop using he-
xavalent chromium in their operation this is the highest
amount of compensation in metal toxicity history. Vari-
ous methods used for removal of Cr (VI) ions include
chemical reduction and precipitation, reverse osmosis,
ion exchange and adsorption on activated carbon or
similar material [5]. But all these methods suffer from
severe constraints, such as incomplete metal removal,
high reagent or energy requirements, generation of toxic
sludge or other waste products that require safe disposal.
Some of the treatment methods involve high operating
and maintenance cost. The high cost of the chemical
reagents and the problems of secondary pollution also
make the above physico-chemical methods rather lim-
ited in application. There is, therefore, a need for some
alternative technique, which is efficient and cost-effec-
tive. The process of heavy metal removal by biological
mate- rials is known as biosorption and the biological
materials used are called biosorbents. Various biosor-
bents like bacteria, fungi, yeasts, agricultural by prod-
ucts, industrial wastes, etc have been used for biosorp-
tion. In this regard, considerable attention has been fo-
cused in recent years upon the field of biosorption for
the removal of heavy metal ions from aqueous solutions
[6]. Recently it is established that for chromium (VI)
biosorption, chromium (VI) is first reduced to chro-
mium (III) and then it is adsorbed as chromium (III) in
the biosorbent [7]. Understanding of mechanism of
chromium (VI) reduction to chromium (III) by some
alcohol is important in this context. In this respect ben-
zyl alcohol is ideal one. Benzyl alcohol is a volatile
component of flower of a night blooming plant Gaura
drummondii [8] and strawberry leaves [9]. The present
investigations have been carried out in micro-hetero-
geneous systems to substantiate the proposed reaction
mechanism as we carried out for other systems [10-17].
Effects of electrolytes are studied to support the pro-
posed reaction mechanism.
2. THEORETICAL
It is expected that the reduction of Cr(VI) by benzyl al-
A. Basu et al. / J. Biomedical Science and Engineering 3 (2010) 735-741
Copyright © 2010 SciRes. JBiSE
736
cohol in aqueous surfactant media is proceed through
normal oxidation mechanism by chromate ester. Benzyl
alcohol is oxidized to benzaldehyde and Cr(VI) is re-
duced to Cr(IV). The over-all reaction can be written
as:
3 PhCH2OH + 2HCrO4- + 8H+ 3 PhCHO + 2Cr(III) +
8 H2O.
3. EXPERIMENTAL
3.1. Table for Materials and Reagents
The materials and reagents are shown in Table 1.
3.2. Procedure and Kinetic Measurements
Under the kinetic conditions, solutions of the oxidant
and mixtures containing the known quantities of the sub-
strate(s) (i.e, benzyl alcohol) (under the conditions [S]T
>> [Cr(VI)]T), acid and the other necessary chemi- cals
were separately thermostated (±0.1). The reaction was
initiated by mixing the requisite amounts of the oxidant
with the reaction mixture. It is assumed that zero time
was taken when half of the required volume of the oxi-
dant solution had been added. The progress of the reac-
tion was followed by monitoring the decay of oxidant
[Cr(VI)] at 415 nm at different time intervals (2 minutes)
with a UV-VIS spectrophotometer [UV-2450 (SHIMA-
DZU)]. Quartz cuvettes of path length 1cm were used.
The observed pseudo-first-order rate con- stants [kobs(s-1)]
were determined from the linear part of the plots of
ln(A415) versus time(t). Reproducible results giving
first-order plots (co-relation co-efficient, R2 0.998)
were obtained for each reaction run. A large ex- cess (
15-fold) of reductant was used in all kinetic runs. No
interference due to other species at 415 nm was veri-
fied. Under the experimental conditions, the possibility
of decomposition of the surfactants by Cr(VI) was inves-
Table 1. Materials and reagents.
Materials Brand
1. Benzyl alcohol AR, Merck, India
2. K2Cr2O7 AR, BDH, India
3. N-cetylpyridinium chloride (CPC)AR, SRL, India
4. Sodium dodecylsulphate (SDS) AR, SRL, India
5. TX-100 AR, SRL, India
6. NaCl AR, Merck, India
7. NH4Cl AR, Ranbaxy, India
tigated and the rate of decomposition in this path was
found to be kinetically negligible.
3.3. Product Analysis and Stoichiometry
Under the kinetic condition benzyl alcohol is oxidized to
benzaldehyde and estimation of the reaction products
was carried by gravimetrically as 2, 4-dinitrophenyl hy-
drazone [18]. In a typical experimental set, 10ml of 0.06
mol dm-3 Cr(VI) in 1.0 mol dm-3 H2SO4 was added to 40
ml of 0.2 mol dm-3 benzyl alcohol and the reaction was
allowed to proceed to completion. Then the reaction
mixture was added slowly with stirring to 60 ml of a
saturated solution of 2,4-dinitrophenyl hydrazine in 2.0
mol dm-3 HCl. After storing for about 1hr in an ice-bath,
the precipitate was collected weighed sintered glass cru-
cible, washed with 2.0mol dm-3 HCl followed by water
and dried to a constant weight at 100-105. The found
ratio, [Cr(VI)]T/[Carbonyl compound]T 2/3 (from 3
independent determinations) supports the fol- lowing
Stoichiometry.
3PhCH2OH + 2HCrO4- + 8H+ 3 PhCHO + 2Cr(III) + 8
H2O. (1)
4. RESULTS AND DISCUSSION
4.1. Dependence on [Substrate]T i.e, [Benzyl
Alcohol]T
From the plot of kobs vs [benzyl alcohol]T, it is estab-
lished that the path shows a first order dependency on
[substrate]T i.e, [benzyl alcohol]T i.e., with increasing
substrate concentration the rate of the reaction increases
in a straight line manner. (Figure 1).
So, kobs = ks[S]T
The above first order dependence on [S]T also main-
tained in the presence of surfactant like CPC, SDS,
TX-100.
4.2. Dependence on [H+]
The acid dependence was followed in aqueous HClO4
media at fixed Cr(VI) and [S]T. From the experimental
fit (Figure 2), the observation is
kobs = kH[H+]2
The above second order dependency is also main-
tained in the presence of surfactant (e.g, SDS).
5. EFFECT OF SURFACTANTS
5.1. Effect of SDS
Sodium dodecyl sulphate(SDS, a representative anionic
surfactant) accelerate the reaction path. The plot of kobs
vs [SDS]T [Figure 3] shows a continuous increase up to
the concentration of SDS.
A. Basu et al. / J. Biomedical Science and Engineering 3 (2010) 735-741
Copyright © 2010 SciRes. JBiSE
737
Fig
1
0
10
20
30
40
50
00.05 0.1 0.15
[Benzyl alcohol] (mol dm
-3
)
10
4
k
obs
(s
-1
)
A
C
D
B
Figure 1. Dependence of kobs on [benzyl alcohol] for the chro-
mium (VI) oxidation of benzyl alcohol at 30. [Cr(VI)]T = 5 ×
10-4 mol dm-3, [H2SO4] = 0.25 mol dm-3. A([SDS]T = 2 × 10-2
mol dm-3, [CPC]T = 0 mol dm-3, [TX-100]T = 0 mol dm-3),
B([SDS]T = 0 mol dm-3, [CPC]T = 0 mol dm-3, [TX-100]T = 2 ×
10-2 mol dm-3), C ([SDS]T = 0 mol dm-3, [CPC]T = 0 mol dm-3,
[TX-100]T = 0 mol dm-3), D([SDS]T = 0 mol dm-3, [CPC] = 2 ×
10-3 mol dm-3, [TX-100]T = 0 mol dm-3).
0
5
10
15
20
25
30
35
40
45
00.511.522.53
[HClO4 ]
2
(mol
2
dm
-6
)
10
4
k
obs
(s
-1
)
A
B
Figure 2. Dependence of kobs on [H+] for the chromium(VI)
oxidation of benzyl alcohol at 30 in aqueous medium.
[Cr(VI)]T = 5 × 10-4 mol dm-3, [benzyl alcohol]T = 150 × 10-4
mol dm-3, [H2SO4] = 0.25 mol dm-3. A([SDS]T = 2 × 10-2),
B([SDS] T = 0).
5.2. Effect of CPC
Cetyl Pyridinium Chloride (CPC, a representative cati-
onic surfactant is found to retard the reaction path. Plot
of kobs vs [CPC]T [Figure 4] shows a continuous de-
crease and finally it tends to level off at higher concen-
tration of CPC. The observation is identical to that ob-
served by Bunton and Cerichelli [19] in the oxidation of
ferrocene by ferric salt salts in the presence of cationic
surfactant cetyl trimethyl ammonium bromide (CTAB).
Fig
3
0
3
6
9
12
15
0 0.020.040.060.08
[SDS] (mol dm
-3
)
10
4
k
obs
(s
-1
)
Figure 3. Dependence of kobs on [SDS]T for the chromium (VI)
oxidation of benzyl alcohol at 30. [Cr(VI)]T = 5 × 10-4mol
dm-3, [benzyl alcohol]T = 150 × 10-4 mol dm-3, [H2SO4] = 0.25
mol dm-3.
1
1.5
2
2.5
3
00.003 0.006 0.009 0.012
[CPC] (mol dm
-3
)
10
4
k
obs
(s
-1
)
Figure 4. Dependence of kobs on [CPC]T for the chromium(VI)
oxidation of benzyl alcohol at 30. [Cr(VI)]T = 5 × 10-4 mol
dm-3, [benzyl alcohol]T = 150 × 10-4 mol dm-3, [H2SO4] = 0.25
mol dm-3.
5.3. Effect of TX-100
Triton X-100(TX-100, a representative neutral surfactant)
accelerates the reaction path. But the acceleration rate in
TX-100 is less than that of SDS. The plot of kobs vs
[TX-100]T [Figure 5], shows a continuous increase up to
the concentration of TX-100.
5.4. Test for Acrylonitrile Polymerization
Under the experimental conditions, the existence of free
radical was indicated by polymerization of acrylonitrile
under a nitrogen atmosphere.
5.5. Mechanism and Interpretation
Scheme 1 leads to the flowing rate law:
A. Basu et al. / J. Biomedical Science and Engineering 3 (2010) 735-741
Copyright © 2010 SciRes. JBiSE
738
CH2OH
+HCrO4+H
+K1
CH2O
O
Cr O
OH
CH2OO
Cr
O
OH +H
+K2
CH2O
O
Cr O
OH2
CH
O
Cr
O
O
OH2
Hk
CH O
+Cr
IV
+H
+
H2O
+
+
+
Scheme 1. Cr(Vl) reduction of Benzyl alcohol.
0
1.5
3
4.5
6
00.02 0.040.06 0.08
[TX-100] (mol dm-3)
104kobs (s-1)
Figure 5. Dependence of kobs on [TX-100]T for the chro- mium
(VI) oxidation of benzyl alcohol at 30. [Cr(VI)]T = 5 ×
10-4mol dm-3, [benzyl alcohol]T = 150 × 10-4mol dm-3, [H2SO4]
= 0.25 mol dm-3.
kobs = (2/3) kK1K2[S]T[H+]2 (2)
The pseudo-first-order rate constants (kobs) in the pre-
sence of various concentrations of different types of sur-
factants, SDS (Sodium dodecyl sulfate, a representative
anionic surfactant), CPC (N-cetyl pyridinium chloride, a
representative anionic surfactant) and TX-100 (Trian
X-100, a neutral surfactant) are presented in Figures 4-6.
The pseudo phase ion-exchange (PIE) [20] model is ap-
plied most widely in micellar catalysis. The basic assum-
ption of the PIE is as follows:
1) Micelles act as a separate phase from water, all re-
actants are distributed quickly between water and micel-
lar phase, and the reaction rate can be considered as the
sum of that in two phases.
2) The reaction in the micellar pseudo phase occurs
mainly at micelle surface.
3) The reactant ions and the inert ions compete at the
charged micellar surface.
The data reveal that SDS and TX-100 accelerate the
rate where as CPC decreases the rate. The rate accelera-
tion is higher in the case of SDS than TX-100. This can
be explained by Schemes 2 and 3.
kWProduct
kMProduct
[Neutral ester]+ [H+]
[Neutral ester]+ [H+]
K
KS
ww
M
M
Scheme 2. Partitioning of the reactive species between
the aqueous and micellar phases.
OSO
3
O
3
SO
OSO
OSO
3
O
3
SO
O
3
SO
O
3
SO OSO
3
OSO
3
OSO
3
OSO
3
H
+
H
+
Na
+
Na
+
Na
+
H
+
Stern Laye
r
Gou
y
-Chapman
Layer
H
+
O
3
SONa
+
H
+
Core
Na
+
Na
+
H
+
OSO
3
=
CH
3
(CH
2
)
11
OSO
3
Na
+
(SDS)
py
+
Cl
Cl
Cl
Cl
py
+
py
+
py
+
+
yp
py
+
py
+
+
yp
+
yp
py
+
+
yp
+
yp Cl
Cl
X
Cl
Cl
X
N
+
CH
2
(CH
2
)
14
CH
3
py
+
=
Cl
(CPC, i.e. hexadecylpyridinium chloride)
Scheme 3. Structural representation of anionic & cationic sur-
factants.
A. Basu et al. / J. Biomedical Science and Engineering 3 (2010) 735-741
Copyright © 2010 SciRes. JBiSE
739
The formation of micelles by ionic surfactants is as-
cribed to a balance between hydrocarbon chain attraction
and ionic repulsion. The net charge of micelles is less
than the degree of micellar aggregates, indicating that a
large fraction of counter ions remains associated with the
micelle; these counter ions form the Stern layer at the
micellar surface. For nonionic surfactants, however, the
hydrocarbon chain attraction is opposed by the require-
ments of hydrophilic groups for hydration and space.
Therefore, the micellar structure is determined by equi-
librium between the repulsive forces among hydrophilic
groups and the short-range attractive forces among hy-
drophobic groups. For bimolecular reactions inhibition
arises from incorporation of one reactant into the micel-
lar pseudo phase and exclusion of the other from it. Ca-
talysis is apparently caused, for the most part, by con-
centration of the two reactants into a small volume in the
micellar Stern layer [21].
The substrate is partitioned in the Stern layer of the
micellar phase. SDS being an anionic surfactant, owing
to the electrostatic attraction between the positively
charged [H+] species and negatively charged micellar
head groups. [H+] easily attaches to the Stern layer of the
micelle. The reaction takes place in both the micellar and
aqueous media. The observed rate acceleration is due to
the favored reaction in the micellar phase, where both H+
and the neutral ester are preferably accumulated. In the
case of TX-100, H+ also attaches to the Stern layer of the
micelle, but the amount is less compared to SDS because
TX-100 is a neutral surfactant, so no electrostatic attrac-
tion takes place. CPC is a cationic surfactant and con-
sequently due to the electrostatic repulsion between the
positively charged [H+] species and positively charged
micellar head group, [H+] does not attaches to the Stern
layer of micelle through the substrate. The reaction takes
place only in aqueous media, which is depleted in the
substrate concentration.
5.6. Effect of Added Electrolyte
Experimental evidence has shown that electrolyte inhibi-
tion of micellar catalysis is a general phenomenon [22-
24] with one apparent exception [25]. The proposed
study has taken into consideration for better under stan-
ding of reduction mechanism. Electrolyte inhibition is
rationalized by assuming that a counter ion competes
with an ionic reagent (e.g., OH-, H3O+, and X-) for a site
on the ionic micelle [26]. When NH4Cl is added the in-
hibition phenomena comes into play (Figure 7). But for
the case of NaCl inhibition followed by enhancement
takes place which is interesting (Figure 6). Enhance-
ment of micellar catalysis by added salt is caused by
their changing the shape or reducing the charge density
0.3 0.4 0.5 0.6 0.7 0.8
0.0
0.2
0.4
0.6
0.8
1.0
1.2
1.4
1.6
1.8
2.0
Fig 6
10 4kobs (s-1)
[NaCl] (mol dm-3)
Figure 6. Dependence of kobs on [NaCl] for the chromium(VI)
oxidation of benzyl alcohol at 300C in SDS medium. [Cr(VI)]T
= 5 × 10-4mol dm-3, [benzyl alcohol]T = 150 × 10-4mol dm-3,
[H2SO4] = 0.25 mol dm-3.
0.3 0.4 0.5 0.6 0.7 0.8
1.0
1.2
1.4
1.6
1.8
2.0
2.2 Fig 7
104kobs(s-1)
[NH4Cl](mol dm-3)
Figure 7. Dependence of kobs on [NH4Cl] for the chromium(VI)
oxidation of benzyl alcohol at 300C in SDS medium. [Cr(VI)]T
= 5 × 10-4 mol dm-3, [benzyl alcohol]T = 150 × 10-4 mol dm-3,
[H2SO4] = 0.25 mol dm-3.
of the micelle. Salts decrease the cmc (critical micelle
concentration) and increase the aggregation no of ionic
micelles [27-28] probably because increased screening
by the counter ions decreases the effective charge den-
sity of the micelle.
6. CONCLUSIONS
Kinetics and mechanism of Cr(VI) reduction by benzyl
alcohol in aqueous acid media have been studied under
the conditions [benzyl alcohol]T>>[Cr(V I)]T. under the
kinetic conditions, the monomeric species of Cr(VI) has
been found kinetically active. Cr(VI)-substrate ester ex-
periences a redox decomposition through 2e- transfer at
A. Basu et al. / J. Biomedical Science and Engineering 3 (2010) 735-741
Copyright © 2010 SciRes. JBiSE
740
Table 2. Presentation of rate constants values (kobs) of benzyl alcohol oxidation in different surfactant medium.
[benzyl alcohol]T
(mol dm-3)
[SDS]T
(mol dm-3) 104kobs(s-1) [CPC]T
(mol dm-3) 104kobs(s-1) [TX-100]T
(mol dm-3) 104kobs (s-1)
1500 10-4 0.02 5.68 0.002 0.002(M) 2.668 0.001 0.02 1.95 0.003
1500 10-4 0.03 7.54 0.002 0.004(M) 2.46 0.002 0.03 2.36 0.002
1500 10-4 0.04 9.14 0.002 0.006(M) 2.395 0.001 0.04 2.95 0.001
1500 10-4 0.05 10.04 0.003 0.008(M) 2.25 0.001 0.05 3.98 0.003
1500 10-4 0.06 11.39 0.002 0.01(M) 2.013 0.002 0.06 4.85 0.003
the rate determining step. The reaction shows both 1st
order dependency on [benzyl alcohol]T and [Cr(VI)]T
and 2nd order dependency on [H+] ion. In the presence of
some non-functional surfactants, the orders remain un-
changed. CPC has been found to retard the rate while
SDS and TX-100 shows the rate acceleration effect (Ta-
ble 2). The effect of added electrolye gives different ob-
servations. Inhibition followed by enhancement is the
effect of NaCl but for NH4Cl inhibition is the only fate.
So for waste water treatment with biosorbent, SDS or
TX-100 and suitable concentration of NaCl may be used
for quick result.
7. ACKNOWLEDGEMENTS
Financial support from UGC, New Delhi is thankfully acknowledged.
REFERENCES
[1] Nriagu, J.O. and Nieboer, E., Eds. (1988) Chromium in
the natural and human environments. Advances in Envir-
onmental Science and Technology. John Willey and Sons,
New York, 20, 1-501.
[2] Sorahan, T., Burges, D.C., Hamilton, L. and Harrington,
J.M. (1998) Lung cancer mortality in nickel/chromium
plates. Occupational and Environmental Medicine, 55(4),
236-242.
[3] Mancuso, T.F. (1997) Chromium as an industrial carcin-
ogen. American Journal of Industrial Medicine, 31(2),
129-139.
[4] Langardt, S. (1990) One hundred years of chromium and
cancer: A review of epidemiological evidence and se-
lected case reports. American Journal of Industrial Me-
dicine, 17(2), 189-214.
[5] Ahluwalia, S.S. and Goyal, D. (2007) Microbial and
plant derived biomass for removal of heavy metals from
wastewater. Bioresource Technology, 98(12), 2243-2257.
[6] Volesky, B. and Holan, Z.R. (1995) Biosorption of heavy
metals. Biotechnology Progress, 11(3), 235-250.
[7] Park, D., Yun, Y.S., Kim, J.Y. and Park, J.M. (2008) How
to study Cr (VI) biosorption: Use of fermentation waste
for detoxifying Cr (VI) in aqueous solution. Chemical
Engineering Journal, 136, 173-179.
[8] Shaver, T.N., Lingren, P.D. and Marshall, H.F. (1997)
Nighttime variation in volatile content of flowers of the
night blooming plant, Gaum drummondii. Journal of
Chemical Ecology, 23(12), 2673-2682.
[9] Nkpwatt, D.A., Krimm, U., Coiner, H.A., Schreiber, L.
and Schwab, W. (2006) Plant volatiles can minimize the
growth suppression of epiphytic bacteria by the phytopa-
thogenic fungus Botrytis cinerea in co-culture experi-
ments. Environmental and Experimental Botany, 56(1),
108-119.
[10] Das, A.K., Roy, A., Saha, B., Mohanty, R.K. and Das, M.
(2001) Micellar effect on the reaction of Chromium (VI)
oxidation of D-fructose in the presence and absence of
picolinic acid in aqeous media: A kinetic study. Journal
of Physical Organic Chemistry, 14(3), 333-342.
[11] Bayen, R., Islam, M., Saha, B. and Das, A.K. (2005)
Oxidation of D-glucose in the presence of 2,2’-bipyridine
by CrVI in aqueous micellar media: a kinetic study. Car-
bohydrate Research, 340(13), 2163-2170.
[12] Islam, M., Saha, B. and Das, A.K. (2005) Kinetics and
mechanism of 2,2’-bipyridyl and 1,10-phenanthroline-
catalysed chromium(VI) oxidation of d-fructose in aqu-
eous micellar media. Journal of Molecular Catalysis A:
Chemical, 236(1-2), 260-266.
[13] Islam, M., Saha, B. and Das, A.K. (2006) Chromic acid
oxidation of hexitols in the presence of 2,2’-bipyridyl
catalyst in aqueos micellar media: a kinetic study. Inter-
national Journal of Chemical Kinetics, 38(9), 531-539.
[14] Islam, M., Saha, B. and Das, A.K. (2007) Kinetics and
mechanism of picolinic acid promoted chromic acid oxi-
dation of maleic acid in aqueous micellar media. Journal
of Molecular Catalysis A: Chemical, 266(1-2), 21-30.
[15] Saha, B., Sarkar, S. and Choudhury, K.M. (2008) Micel-
lar effect of quinquivalent vanadium ion oxidation of
D-glucose in aqueous acid media: a kinetic study. Inter-
national Journal of Chemical Kinetics, 40(5), 282-286.
[16] Choudhury, K.M., Mandal, J. and Saha, B. (2009) Mi-
cellar catalysis of Chromium (VI) oxidation of ethane-1,
2-diol in presence and absence of 2,2’-bipyridine in
aqueos acid media. Journal of Coordination Chemistry,
62(11), 1871-1878.
[17] Ghosh, S.K., Basu, A., Paul, K.K. and Saha, B. (2009)
Micelle catalyzed oxidation of propan-2-ol to acetone by
penta-valent vanadium in aqueous acid media. Molecular
Physics, 107(7), 615-619.
[18] Vogel, A.I. (1958) Elementary practical organic chemis-
try, Part-III, quantitative organic analysis, ELBS and
Longman Group Ltd., London, p. 739.
[19] Bunton, C.A. and Cerichelli, G. (1980) Micellar effects
A. Basu et al. / J. Biomedical Science and Engineering 3 (2010) 735-741
Copyright © 2010 SciRes. JBiSE
741
upon electron transfer from ferrocenes. International
Journal of Chemical Kinetics, 12(8), 519-533.
[20] Menger, F.M. and Portnoy, C.E. (1967) Chemistry of rea-
ctions proceeding inside molecular aggregates. Journal
of the American Chemical Society, 89(18), 4698- 4703.
[21] Bunton, C.A. (1979) Reaction kinetics in aqueous surfac-
tant solutions. Catalysis Reviews - Science and Engineer-
ing, 20(1), 1-56.
[22] Morawetz, H. (1969) Catalysis and inhibition in solu-
tions of synthetic polymers and in micellar solutions.
Advances in Catalysis & Related Subjects, 20, 341-371.
[23] Cordes, E.M. and Dunlop, R.B. (1969) Kinetics of or-
ganic reactions in micellar systems. Accounts of Chemi-
cal Research, 2(11), 329-337.
[24] Fendler, E.J. and Fendler, J.H. (1971) Micellar catalysis
in organic reactions: Kinetic and mechanistic implica-
tions. Advances in Physical Organic chemistry, 76, 271-
406.
[25] Bunton, C.A., Minch, M. and Sepulveda, L. (1971) En-
hancement of micellar catalysis by added electrolyte.
Journal of Physical Chemistry, 76(2), 2707-2709.
[26] Das, A.K. (2004) Micellar effect on the kinetics and
mechanism of chromium (VI) oxidation of organic sub-
strates. Coordination Chemistry Review, 248(1-2), 81-99.
[27] Mysels, K.J. and Princen, L.H. (1957) Light scattering by
ideal colloidal electrolyte. Journal of Colloid Science,
12(6), 594-605.
[28] Shinoda, K. (1955) The critical micellar concentrations
in aqueous solutions of potassium alkyl malonates. Jour-
nal of Physical Chemistry, 59(5), 432-435.