Deciphering aggregation behavior and thermodynamic properties of anionic surfactant sodium hexadecyl sulfate in aqueous solutions of ionic liquids [C5mim][Br] and [C6mim][Br]

Article abstract of DOI:10.1016/j.molliq.2019.111949

The present work aims to study the interactions of cationic imidazolium based ionic liquids i.e. 1-alkyl-3-methylimidazolium bromide ([C_nmim][Br], where n = 5 &6) with anionic surfactant sodium hexadecyl sulfate (SHS) in aqueous media employing the various techniques such as conductivity measurement, fluorescence spectroscopy, UV–visible spectroscopy and FT-IR spectroscopy. The temperature dependence of critical micelle concentration (CMC) determined using conductivity measurements at temperatures (298.15, 303.15 and 308.15) K at different concentrations (0.02, 0.05 and 0.1) wt. %, of ionic liquids (ILs) in aqueous medium was used to calculate the various thermodynamic parameters of micellization such as, standard free energy of micellization (ΔG_m ⁰), standard enthalpy of micellization (ΔH_m ⁰), and standard entropy of micellization (ΔS_m ⁰). Further, fluorescence and UV–Visible spectroscopy have been utilized to confirm the CMC values obtained from conductivity measurements, which were found to be in good agreement. A continuous increment in CMC value was observed with the increase in concentration of ILs as well as in temperature. Further FT-IR Spectroscopic studies have been done to demonstrate the structural alterations occurring in the respective mixtures.

Full text of DOI:10.1016/j.molliq.2019.111949

Journal Pre-proof
Deciphering aggregation behavior and thermodynamic properties of anionic
surfactant sodium hexadecyl sulfate in aqueous solutions of ionic liquids [C mim][Br]
5
and [C mim][Br]
6
Harsh Kumar, Gagandeep Kaur
PII:
S0167-7322(19)34941-4
DOI:
https://doi.org/10.1016/j.molliq.2019.111949
MOLLIQ 111949
Reference:
To appear in: Journal of Molecular Liquids
Received Date: 4 September 2019
Revised Date: 27 September 2019
Accepted Date: 16 October 2019
Please cite this article as: H. Kumar, G. Kaur, Deciphering aggregation behavior and thermodynamic
properties of anionic surfactant sodium hexadecyl sulfate in aqueous solutions of ionic liquids
[
C mim][Br] and [C mim][Br], Journal of Molecular Liquids (2019), doi: https://doi.org/10.1016/
5 6
j.molliq.2019.111949.
This is a PDF file of an article that has undergone enhancements after acceptance, such as the addition
of a cover page and metadata, and formatting for readability, but it is not yet the definitive version of
record. This version will undergo additional copyediting, typesetting and review before it is published
in its final form, but we are providing this version to give early visibility of the article. Please note that,
during the production process, errors may be discovered which could affect the content, and all legal
disclaimers that apply to the journal pertain.
©
2019 Published by Elsevier B.V.

GRAPHICAL ABSTRACT
Deciphering aggregation behavior and thermodynamic properties of anionic
surfactant sodium hexadecyl sulfate in aqueous solutions of ionic liquids
[
C mim][Br] and [C mim][Br]
5
6
Harsh Kumar*, Gagandeep Kaur
Department of Chemistry, Dr B R Ambedkar National Institute of Technology,
Jalandhar – 144011, Punjab, India

Deciphering aggregation behavior and thermodynamic properties of anionic
surfactant sodium hexadecyl sulfate in aqueous solutions of ionic liquids
[
C mim][Br] and [C mim][Br]
5
6
Harsh Kumar*, Gagandeep Kaur
Department of Chemistry, Dr B R Ambedkar National Institute of Technology,
Jalandhar – 144011, Punjab, India
ABSTRACT
The present work aims to study the interactions of cationic imidazolium based ionic liquids i.e.
1
n
-alkyl-3-methylimidazolium bromide ([C mim][Br], where n=5 &6) with anionic surfactant
sodium hexadecyl sulfate (SHS) in aqueous media employing the various techniques such as
conductivity measurement, fluorescence spectroscopy, UV-visible spectroscopy and FT-IR
spectroscopy. The temperature dependence of critical micelle concentration (CMC) determined
using conductivity measurements at temperatures (298.15, 303.15 and 308.15) K at different
concentrations (0.02, 0.05 and 0.1) wt. %, of ionic liquids (ILs) in aqueous medium was used to
calculate the various thermodynamic parameters of micellization such as, standard free energy of
0
m
0
m
micellization (∆G ), standard enthalpy of micellization ( ∆H ), and standard entropy of
0
m
micellization (∆S ). Further, fluorescence and UV-Visible spectroscopy have been utilized to
confirm the CMC values obtained from conductivity measurements, which were found to be in
good agreement. A continuous increment in CMC value was observed with the increase in
concentration of ILs as well as in temperature. Further FT-IR Spectroscopic studies have been
done to demonstrate the structural alterations occurring in the respective mixtures.
Keywords: 1-alkyl-3-methylimidazolium bromide [C mim][Br]; sodium hexadecyl sulfate
n
(SHS); Fluorescence; UV-visible; Micellization; FT-IR
*
Corresponding author e-mail: h.786.man@gmail.com; manchandah@nitj.ac.in
1

INTRODUCTION
The use of surfactants have been the focus of significant research interest due to their
applications in numerous fields such as biotechnology [1], solubilizing and emulsifying agents
[2], personal care and laundry products [3], pharmaceuticals [4], nano-reactors for enzymatic
reactions [5] This is due to their capability to form spontaneous self-assembled structures in
different solvents [6]. On the other hand, ionic liquids are of significant interest due to their
useful properties such as non-flammability, negligible volatility, high ion conductivity, thermal
and chemical stability. Also they are known to be safe and sustainable substitutes to various
organic solvents for their use in many applications [7, 8]. They can alter the surface and
thermodynamic properties of various surfactants [9–18], which help to understand various types
of interactions between ionic surfactants and ionic liquids [19]. The magnitude of change in
properties of surfactant on using IL as an additive depends upon the composition of IL as well as
various interactions of IL with the surfactant [20, 21].
Micelle is an aggregate of surfactant molecules formed above a particular concentration. Critical
micelle concentration (CMC) is the concentration above which the monomers of surfactant
aggregate and micelle formation takes place [22-24]. The formation of micelle occur when there
is balance between hydrophobic and hydrophilic forces. This governs the aggregation properties
of surfactant solutions in the presence of different additives. The aggregation properties show
variations by the change in temperature and concentration of surfactant solutions. The
hydrophobic interactions between the hydrophobic chains is the driving force for micelle
formation. This corresponds to favorable contribution towards free energy of micellization. But
electrostatic repulsions between surfactant head groups at the surface of micelle contribute to
positive free energy, which is unfavorable for micelle formation. This type of micelle
destabilizing interactions can be reduced by the adsorption of counterions at the surface of
micelle. Thus the degree of counterion binding (α) governs the stability of micelles [25]. The
inclusion of additive into an associates of an amphiphiles will affect their physicochemical
characteristics for instance the degree of ionization, reaction rates and clouding or phase
separation [26-29].
Armstrong's group [30] was first to explore the aggregation behavior of different surfactants in
ILs 1-butyl-3-methylimidazolium chloride [C mim][Cl] and 1-butyl-3-methylimidazolium
4
2

4 6
hexafluorophosphate [C mim][PF ]. The observed CMCs were found to be higher than the
CMCs of same surfactants in aqueous solution [30]. Reddy's group investigated the aggregation
properties of aqueous sodium dodecyl sulfate (SDS) with the variation in alkyl chains of ILs
[
31]. Javadian et al. studied the micellization behavior of cetyltrimethyl ammonium bromide
CTAB) in various ILs in aqueous media [21]. Bermudez and Chen uses 1-ethyl-3-
(
2 2 3
methylimidazolium ethyl sulfate [C mim][C OSO ] as the solvent to study the aggregation and
interfacial behavior of anionic and cationic surfactants [18]. Pandey et al. observed the
aggregation behavior of SDS in the presence of hydrophobic IL 1-butyl-3-methylimidazolium
6
hexafluorophosphate, [bmim][PF ] and a hydrophilic IL 1-butyl-3-methylimidazolium
tetrafluoroborate, [bmim][BF ] [32-35].
4
In this paper, we report the aggregation behavior of anionic surfactant sodium hexadecyl sulfate
(
SHS) in the presence of imidazolium based ILs such as 1-pentyl-3-methylimidazolium bromide
mim][Br] and 1-hexyl-3-methylimidazolium bromide [C mim][Br]. Conductivity
[C
5
6
measurements have been performed to evaluate the CMC as well as various thermodynamic
parameters of micellization for the aggregation of sodium hexadecyl sulfate (SHS) in the
presence both the ILs at different concentrations i.e. (0.02, 0.05 and 0.10) wt. % and at different
temperatures i.e. (298.15, 303.15 and 308.15) K. Further fluorescence spectroscopy and UV-
visible spectroscopic techniques have been employed to validate the CMC values obtained using
conductivity measurement at 298.15 K. These investigations provide the better insight for the
types of interactions existing in hydrophobic and hydrophilic parts of surfactant and ILs.
2
2
1
. EXPERIMENTAL
.1 Chemicals
-methylimidazole (purity >99.0%) purchased from HIMEDIA Laboratories Pvt. Ltd. is used to
synthesize the ionic liquid [C
5 6
mim][Br] and [C mim][Br]. The alkyl halides i.e. 1-bromopentane
(purity >98.0%) and 1-bromohexane (purity 99.0%) used for this purpose are obtained from TCI
Pvt. Ltd. and HIMEDIA Laboratories Pvt. Ltd. respectively. Acetonitrile (purity >99.5%), which
was used as a solvent was procured from LOBA Chemie Pvt. Ltd. The anionic surfactant Sodium
hexadecyl sulfate (SHS) used in this study was procured from TCI Pvt. Ltd. Before the use of
2 5
SHS, it was dried under vacuum and then stored over P O in vacuum desiccators for at least
3

4
8h. All the chemicals used during the experimental work along with their details have been
enlisted in Table 1.
2
.2 Synthesis of ionic liquids
1
-Bromopentane was added drop wise into a vigorously stirred solution of 1-methylimidazole
and acetonitrile in the ratio 1:1.2 in 500ml round bottom flask. The solution was refluxed at
◦
around 80 C for 48 h. To monitor the progress of reaction thin layer chromatography is used.
Then the reaction mixture was cooled to room temperature. Rota evaporator was used to remove
the excess of acetonitrile present in the reaction mixture. The obtained ionic liquid, 1-pentyl-3-
methylimidazolium bromide [C mim][Br], was then washed several times using hexane. To
5
6
synthesize 1-hexyl-3-methylimidazolium bromide [C mim][Br], the same procedure is repeated
with 1-bromohexane instead of 1-bromopentane. The synthesized ionic liquid is dried under
1
vacuum for few days before its use. The structure of both the ILs is confirmed by using H NMR
1
(
Bruker 400 MHz) and FT-IR (Agilent Carry 630) spectroscopic studies. The H NMR and FT-
IR spectroscopic studies of [C mim][Br] have been reported as Figure S1 and that for
5
[C
6
mim][Br] have been shown as Figure S2 in supporting information. The results obtained for
both the ionic liquids are found to be in good agreement with the literature data [36].
2
.3 Instruments and methods
Doubly distilled deionized water from Millipore, Milli-Q Academic water purification system
-1
having conductance < 5 ꢀS cm had been used for sample preparation. To prepare the stock
solutions, the required amount of ILs was accurately weighed using Sartorius CPA 225 D with
a precision of ±0.00001g. Microsoft Excel and OriginPro 8 software were used to analyze the
data as per the model/equations given in the different sections and used in the present study.
2
.3.1 Conductivity measurements
The measurements of electrical conductivities for all mixtures had been performed at different
temperatures (298.15, 303.15, 308.15) K using a digital conductivity meter (Systronics 308) in a
water jacketed flow dilution cell. The solution was maintained at specific temperatures using
refrigerated circulated water thermostat provided by Macro Scientific Works Pvt. Ltd. Delhi
which controlled temperature with accuracy of ±0.1 K as already mentioned our previous study
[37]. The calibration of conductivity meter had been done before the measurements using the
4

−
1
aqueous KCl solutions in the concentration range of 0.01-1.0 mol kg . The value of conductivity
is noted after adding the required amount of homogeneous solution of surfactant followed by the
proper stirring of solution.
2
.3.2 Fluorescence measurements
The fluorescence measurements had been done on a RF 5301 PC spectrophotometer purchased
from Shimadzu in the range 350–600 nm at an excitation wavelength of 320 nm. TCC 240A
thermoelectrically temperature controlled cell holder was used to maintain a constant
temperature within ±1 °C. Pyrene was utilized as fluorescence probe, whose stock solution had
been prepared in methanol at a very low concentration i.e. 1 ꢀM, to prevent excimer formation.
Doubly distilled de-ionized degassed water had been used to prepare the solutions of
[
C mim][Br] + SHS and [C mim][Br] + SHS at different concentrations. The ratio ‘I / I ’ of the
5 6 I III
fluorescence intensities of the first and third vibronic peaks was then calculated, as it gives a
measure of the polarity of the microenvironment of pyrene in the micelles.
2
.3.3 UV-visible spectroscopy
Agilent Technologies Cary series UV-Vis spectrophotometer using a quartz cuvette having path
length of 1 cm was employed to record the UV spectra. The stock solution of SHS was added
using micro syringe to the aqueous solutions of IL taken in the cuvette. A number of spectra
were recorded after addition of particular amount of SHS in the cuvette. The absorbance
behavior of IL was monitored in the UV-visible range (200-800 nm) by varying the
concentration of SHS in the aqueous solutions of both the ILs.
2
.3.4 FT-IR spectroscopic study
Agilent technologies Carry 630 FT-IR Spectrophotometer was utilized to carry out FT-IR
-1
-1
spectral studies in the wave number region from 4000 cm to 400 cm . The FT-IR spectra were
recorded for different concentrations (0.02, 0.05and 0.10 wt. %) of both the ILs as well as
SHS/IL mixtures when the concentration of SHS in respective IL correspond to concentration at
CMC, below CMC and above CMC.
3
. RESULT AND DISCUSSIONS
5

Aggregation behavior of sodium hexadecyl sulfate (SHS) has been investigated in the absence
and presence of ionic liquids in aqueous media using conductivity measurement, fluorescence
spectroscopy, UV-Visible spectroscopy and FT-IR spectroscopy.
3
3
.1 Conductivity measurements
.1.1 Critical micelle concentration (CMC) and degree of counterion dissociation (α)
Specific conductivity is the important property to study the aggregation behavior of surfactants.
Electrical conductivity measurements are made to study the aggregation behavior of anionic
surfactant sodium hexadecyl sulfate (SHS) in the absence and presence of ionic liquids
[
C mim][Br] and [C mim][Br] in aqueous medium. The measurements were taken for different
5 6
IL/SHS mixtures at different concentrations of both the ionic liquids i.e. (0.02, 0.05 and 0.1) wt.
of ionic liquids and at various temperatures (298.15, 303.15 and 308.15) K. The measured
%
values of specific conductivity have been shown in Table 2 and Table 3. The variation of specific
conductivity, κ with the change in concentration of sodium hexadecyl sulfate (SHS) is plotted at
different concentrations of both the ionic liquids at various temperatures. The respective plots
have been shown in Figure 1 and Figure 2. The specific conductivity varies linearly with the
change in concentration of anionic surfactant but the slope in the premicellar region is always
greater than the postmicellar region [38, 39].The point of intersection of the two line segments
corresponding to premicellar and postmicellar region was termed as critical micelle
concentration (CMC). The ratio of slope in the postmicellar to the premicellar region give rise to
the degree of counterion dissociation (α). The value of CMC obtained for aqueous SHS in the
absence of IL is in good agreement with literature [40]. The value of CMC as well as α have
5
been reported in Table 4 for IL/SHS mixtures at various concentrations of [C mim][Br] at
various temperatures. Similarly these values at various concentrations of [C mim][Br] and at
6
various temperatures have been reported in Table 5.
The value of critical micelle concentration (CMC) as well as degree of counterion dissociation
(α) increases with the increase in concentration of both the ionic liquids. The process of
micellization is mainly dependent upon two types of interactions i.e. electrostatic interactions
occurring between the charged head groups as well as hydrophobic interactions occurring in the
hydrophobic tails of different components. These two types of interactions have opposite effects.
This is because electrostatic interactions can lower the CMC of mixture thereby favoring the
6

micellization by reducing the repulsions among the charged head groups. On the other hand
hydrophobic interactions can lead to increase in CMC of mixture by stabilizing the surfactant
monomers thereby delaying the micellization [41]. The hydrophobic interactions dominates over
the electrostatic interactions due to the insertion of ionic liquid into inter-cluster space of water
+
+
which in turn lead to increase in CMC of mixture. Here [C mim] and [C mim] of ionic liquid
5
6
interacts with the anion of SHS through hydrophobic interactions which leads to increase in
CMC upon addition of both the ionic liquids.
At a particular concentration of ionic liquid, the value of CMC increases with the increase in
temperature. On increasing temperature, the degree of hydration of hydrophilic parts decreases,
thereby reducing the CMC. But increasing temperature can also lead to disruption of water
structure, which can delay the tendency of micellization. Thus these two opposite effects prevail
in the mixture on increasing the temperature. As the CMC increases with increase in
temperature, hence latter effect dominates.
But the micellization of SHS takes place rapidly in case of [C mim][Br] in comparison to
6
[C
5
mim][Br] as the value of CMC in case of [C
6
mim][Br] is always less than that of
[
C mim][Br] at all the concentrations of IL as well as at all the studied temperatures. This is
5
because the hexyl chain in [C mim][Br] is more flexible as compared to the pentyl chain in
6
[C
5
mim][Br], which leads to increase in the value of change in entropy of system, thereby
increasing the tendency of micellization in case of [C mim][Br] as compared to[C mim][Br].
6
5
3
.1.2 Thermodynamics of micellization
The conductivity measurement of the studied IL/SHS mixtures at various temperatures can also
lead to evaluation of various thermodynamic parameters of micellization such as the standard
0
m
Gibbs’ free energy change of micellization, ∆G , the standard enthalpy change of micellization,
0
m
0
m
∆
H
and the standard entropy change of micellization, ∆S by using the equations (1)-(3).
0
m
(1)
(2)
(3)
∆
G
= (2-α) RT (lnXCMC)
0
m
2
∆
H
= -RT (2-α) [d(ln XCMC)/dT]
0
m
0
0
m
∆
S
= ( ∆Hm
-
∆G ) / T
7

,
where R is gas constant, T is temperature and α is degree of counter ion dissociation, XCMC is the
0
0
value of CMC in the mole fraction unit [42]. After evaluating ∆G and ∆H , from equation (1)
m
m
0
m
and (2), the value of ∆S can be calculated by equation (3). The values of all these
thermodynamic parameters of micellization have been enlisted in Table 4 for SHS in presence of
different wt. % of [C mim][Br] in aqueous medium. Similarly these values for SHS in presence
5
of different wt. % of [C mim][Br] in aqueous medium have been shown in Table 5. The values
6
of these thermodynamic parameters helps in understanding the driving force of micellization.
0
0
0
The variation of ∆Gm , ∆H and ∆S with the change in temperature and concentration of both
m m
0
m
the ionic liquids has been shown in Figure 3 and 4. It can be observed that the value of ∆G and
0
m
∆
H
is negative for all the studied mixtures which indicates the process of micellization is
0
m
spontaneous and exothermic in nature. The value of ∆G becomes less negative with the
addition of different wt. % of ionic liquids at a particular temperature indicating the decrease in
0
m
tendency of micellization upon addition of both the ionic liquids. The value of ∆G is dependent
0
m
0
m
0
m
upon two terms, entropic (-T ∆S ) and enthalpic ( ∆H ) contribution. From the values of ∆S
0
m
and ∆H , it can be seen that the process of micellization is entropy driven for both the studied
mixtures.
3
.2 Fluorescence probe behavior
Pyrene is used as a fluorescent probe showing the significant vibrational bands in their
fluorescence spectra. The ratio of first to third vibrational peaks of pyrene is widely used for the
I
determination of the CMC of micellar systems [43-51]. Pyrene I / IIII versus the concentration of
SHS in the presence of different wt. % of both the ILs has been given as Table S1 and S2. These
values have also been shown graphically in Figures 5 and 6. The curves obtained in all the plots
shows a sigmoidal decrease, which fit well to Boltzmann type equation [49]. The I / I remains
I
III
constant up to a particular concentration and then decreases rapidly on the onset of micellization.
This is because this ratio is very sensitive to solvent polarity. Initially before the micellization,
this ratio is high in polar medium, but as the concentration of SHS increases, the micellization of
SHS takes place. This decreases the polarity of medium, which in turn is responsible for the
abrupt decrease in value of I / I upon micellization as the non-polar pyrene goes into
I
III
8

hydrophobic micellar phase. The midpoint of the curves obtained corresponds to CMC of
IL/SHS mixtures. The values of CMC obtained using fluorescence spectroscopy for SHS in
presence of different concentrations of both the ionic liquids at 298.15 K have been reported in
Table 6. The values of CMC obtained using Fluorescence spectroscopy are quite close to that
obtained using conductivity measurements.
3
.3 UV-visible spectroscopy
In the present study, the absorbance behavior of ionic liquid is monitored in UV–visible range
200–800 nm) on the addition of SHS. This method of analyzing absorbance versus
(
concentration of SHS can be regarded as simplest and quickest method for the determination of
CMC. In case of imidazolium based ionic liquids, there is inherent structural feature that makes
them to absorb in the entire UV-region [52-54]. The presence of imidazolium ring in these type
of ionic liquids negate the requirement of any probe for the determination of CMC [55]. The
absorbance versus concentration of SHS is plotted to determine the CMC of SHS in presence of
imidazolium based ionic liquid. But this method cannot help to evaluate CMC in the absence of
imidazolium based ionic liquid in aqueous media, because water itself does not absorb in UV-
region. The absorbance varies linearly with concentration of SHS up to a certain concentration of
SHS, but after the micellization of SHS begins, the rate of the increase is different from the rate
before. Then the point of intersection of two lines in the plot corresponds to the point of CMC
[
56]. The plots of absorbance versus concentration of SHS in the presence of different wt. % of
mim][Br] and [C mim][Br] in aqueous medium have been shown in Figures 7 and 8,
[C
5
6
respectively. The absorbance values for the same are reported in Tables S3 and S4. The CMC of
SHS in presence of different wt. % of both the ionic liquids at 298.15 K is compared with that
obtained through conductivity and fluorescence spectroscopy. The same is listed in Table 6. It
can be observed from the table that the value of CMC of obtained using these three methods are
very close to each other.
3
.4 FT-IR spectroscopic study
The variation of local polarity and conformation of alkyl chains with temperature is indicator of
micellization, which can be ascertained using FT-IR spectroscopic technique [57-59]. The
various molecular scale interactions occurring in the mixtures can be monitored using FT-IR
spectroscopic technique, which is remarkable tool for obtaining such information. The mixture
9

constituting surfactant and ionic liquid show various structural alterations upon micellization. In
this study, FT-IR spectra of SHS in presence of different concentrations of both the ionic liquids
have been recorded for concentration of SHS below CMC, at CMC and above CMC. The
spectrum is unique for different IL/SHS mixture. The obtained spectra are shown in as Figures
S3 and S4 of supplementary data. FT-IR spectra of SHS in (0.02, 0.05, and 0.10) wt. % of
-1
[C
5
mim][Br] and [C
6
mim][Br] in the wavenumber range 3000-3600 cm at different
concentrations of SHS have been shown in Figures 9 and 10. The spectra shows two major
-1
peaks. The one peak, which is appearing in the wavenumber 3200-3300cm may be due to N-H
-1
stretching whereas the other that appearing in the 1600-1690cm wavenumber range may be due to
N-H bending and C=C stretching. There is a shift in the wavenumber which is contained in Table
7
that indicate interactions prevailing in the mixture of SHS in presence of ionic liquid [60]. This
specifies that, the SHS interacts with both the imidazolium based ionic liquids giving rise to
various structural alterations within the mixture.
4
. CONCLUSION
Aggregation behavior of conventional anionic surfactant SHS have been examined in the
presence of imidazolium based ionic liquids in aqueous media at different temperatures by
utilizing various techniques. An increase in CMC is obtained for SHS in presence of different wt.
%
of both the ionic liquids, which may be due to hydrophobic interactions that stabilize the
surfactant monomers, which in turn is responsible for delay in tendency of micellization. On the
other hand, the value of CMC of SHS in presence of both the ionic liquids increases with the
increase in temperature, indicating the delay in micellization on increasing temperature from
2
98.15 K to 308.15 K. The value of CMC in presence of [C mim][Br] is always less than that in
6
presence of [C mim][Br] at a particular temperature and concentration of ionic liquid. This
5
shows the tendency of micellization of SHS is more in presence of [C mim][Br] as compared to
6
0
m
[
C mim][Br]. Further, the large negative value of ∆G for both the studied mixtures indicates the
5
0
m
process of micellization is spontaneous in nature. The negative ∆H values indicate the
0
m
exothermic nature of micellization. The large positive values of ∆S reveals that the process of
micellization is entropy driven, where the hydrophobic interactions between the alkyl chains
plays prominent role. The CMC values determined for both the mixtures from all methods are
found to be in good agreement with each other. Also, the FT-IR spectra shows the various shifts
1
0

in the wavenumber in for the mixtures constituting SHS in presence of different wt. % of both
the ionic liquids.
Acknowledgements
Authors (H.K) are thankful to Science and Engineering Research Board (SERB), New Delhi for
providing financial assistance to carry out research work vide sanction order number
EMR/2015/002059. Gagandeep Kaur is thankful to Department of Science and Technology
(DST), New Delhi for providing DST INSPIRE Fellowship (IF170753) with application
reference number [DST/INSPIRE/03/2017/001654]. The authors are also thankful to DST, New
Delhi for DST-FIST [CSI-228/2011] Program and The Director and Head, Department of
Chemistry for providing necessary facilities.
1
1

References
[
1] J.H. Fendler, Membrane Mimetic Chemistry: Characterizations and Applications of
Micelles, Microemulsions, Monolayers, Bilayers, Vesicles and Host-Guest Systems,
Wiley, New York, NY, 1983.
[2] Y. Moroi, Micelles: Theoretical and Applied Aspects, Springer, New York, NY, 1992.
[3] R. Savic, L. Luo, A. Eisenberg, D. Maysinger, Science, 300 (2003) 615-618.
[4] C. Allen, D. Maysinger, A. Eisenberg, Colloids Surf. B., 16 (1999) 3-27.
[5] F.M. Menger, J.U. Rhee, H.K. Rhee, J. Org. Chem., 40 (1975) 3803-3805.
[6] R.M. Hill, K. Ogino, M. Abe, Mixed surfactant systems, Surfactant Science Series, 46,
Marcel Dekker, New York, 1993.
[7] T. Welton, Chem. Rev., 99 (1999) 2071-2084.
[8] S. Keskin, D. Kayrak-Talay, U. Akman, O. Hortacsu, J. Supercrit. Fluids, 43 (2007) 150-
1
80.
[9] A. Pal, S. Chaudhary, Colloids Surf. A., 430 (2013) 58-64.
[
10] L. Shi, X. Jing, H. Gao, Y. Gu, L. Zheng, Colloid Polym. Sci., 291 (2013) 1601-1612.
11] M.T. Lam, W.D Adamson, S. Miao, R. Atkin, G.G. Warr, J. Colloid Interface Sci., 552
[
(2019) 597-603.
[
[
[
[
[
[
[
[
[
[
12] A. Pal, S. Chaudhary, Fluid Ph. Equilibria, 352 (2013) 42-46.
13] K.A. Fletcher, S. Pandey, Langmuir, 20 (2004) 33-36.
14] S. Chaudhary, A. Pal, J. Mol. Liquids, 190 (2014) 10-15.
15] A. Pal, A. Pillania, J. Surfactants Deterg., 22 (2019) 327-338.
16] S. Das, S. Ghosh, B. Das, J. Chem. Eng. Data, 63 (2018) 3784-3800.
17] A. Pal, A. Pillania, Colloids Surf. A., 452 (2014) 18-24.
18] L.G. Chen, H. Bermudez, Langmuir, 28 (2012) 1157-1162.
19] V. Srinivasan, D. Blankschtein, Langmuir, 19 (2003) 9946-9961.
20] L. Shi, X. Jing, H. Gao, Y. Gu, L. Zheng, Colloid Polym. Sci., 291 (2013) 1601-1612.
21] S. Javadian, V. Ruhi, A. Heydari, A.A. Shahir, A. Yousefi, J. Akbari, Ind. Eng. Chem.
Res., 52 (2013) 4517-4526.
[22] N. Azum, M.A. Rub, A.M. Asiri, H.A. Kashmery, J. Mol. Liquids, 260 (2018) 159-165.
[23] D. Kumar, N. Azum, M.A. Rub, A.M. Asiri, J. Mol. Liquids, 262 (2018) 86-96.
[24] D. Kumar, M.A. Rub, J. Mol. Liquids, 274 (2019) 639-645.
1
2

[
25] M.S. Bakshi, N. Kaur, R.K. Mahajan, J. Singh, N. Singh, Colloid Polym. Sci., 284 (2006)
79-885.
26] N. Azum, A. Ahmed, M.A. Rub, A.M. Asiri, S.F. Alamery, J. Mol. Liquids, 290 (2019)
11187.
8
[
1
[
[
[
27] D. Kumar, M.A. Rub, J. Mol. Liquids, 240 (2017) 253-257.
28] A.Z. Naqvi, M.A. Rub, Kabir-ud-Din, Colloid J., 77 (2015) 525-531.
29] M.A. Rub, N. Azum, S.B. Khan, H.M. Marwani, A.M. Asiri, J. Mol. Liquids, 212 (2015)
5
32-543.
30] J.L. Anderson, V. Pino, E.C. Hagberg, V.V. Sheares, D.W. Armstrong, Chem. Commun.,
9 (2003) 2444-2445.
[
1
[
[
[
[
[
[
[
[
31] A. Beyaz, W.S. Oh, V.P. Reddy, Colloids Surf. B., 35 (2004) 119-124.
32] K. Behera, P. Dahiya, S. Pandey, J. Colloid Interface Sci., 307 (2007) 235-245.
33] K. Behera, S. Pandey, Langmuir, 24 (2008) 6462-6469.
34] K. Behera, S. Pandey, J. Phys. Chem. B, 111 (2007) 13307-13315.
35] K. Behera, S. Pandey, J. Colloid Interface Sci., 316 (2007) 803-814.
36] J. Vitz, T. Erdmenger, C. Haensch, U.S. Schubert, Green Chemistry, 11 (2009) 417-424.
37] H. Kumar, A. Katal, J. Mol. Liquids, 266 (2018) 252-258.
38] J.L. Del Castillo, M.J. Suarez-Filloy, A. Castedo, T. Svitova, J.R. Rodriguez, J. Phys.
Chem. B, 101 (1997) 2782-2785.
[39] A. Dominoques, A. Fermandez, N. Gonzalez, E. Inglesias, L. Montonegro, J. Chem.
Educ., 74 (1997) 1227-1231.
[40] V. Kumar, T.W. Gilbert, J. Electroanal. Chem., 40 (1972) 419-429.
[41] R.K. Mahajan, R. Sharma, J. Colloid Interface Sci., 363 (2011) 275-283.
[42] M.J. Rosen, Surfactants and interfacial phenomena, 3rd ed., John Wiley and Sons, New
York, 2004.
[43] K. Kalyanasundaram, J.K. Thomas, J. Am. Chem. Soc., 99 (1977) 2039-2044.
[44] A.I. Mitsionis, T.C. Vaimakis. Chem. Phys. Lett., 547 (2012) 110-113.
[45] O. Topel, B.A. Cakir, L. Budama, N. Hoda, J. Mol. Liquids, 177 (2013) 40-43.
[46] K.P. Ananthapadmanabhan, E.D. Goddard, N.J. Turro, P.L. Kuo, Langmuir, 1 (1985) 352-
3
55.
1
3

[47] K. Kalyanasundaram, Photochemistry in microheterogeneous systems, Academic Press,
New York, 1987.
[
48] O. Regev, R. Zana, J. Colloid Interface Sci., 210 (1999) 8-17.
49] J. Aguiar, P. Carpena, J.A. Molina-Bolivar, C.C. Ruiz, J. Colloid Interface Sci., 258
[
(2003) 116-122.
[
[
[
[
[
[
[
[
[
[
[
50] W. Caetano, M. Tabak, J. Colloid Interface Sci., 225 (2000) 69-81.
51] O. Anthony, R. Zana, Macromolecules, 27 (1994) 3885-3891.
52] A. Paul, P.K. Mandal, A. Samanta, J. Phys. Chem. B, 109 (2005) 9148-9153.
53] A. Paul, P.K. Mandal, A. Samanta, Chem. Phys. Lett., 402 (2005) 375-379.
54] M.A. Bhat, C.K. Dutta, G.M. Rather, J. Mol. Liquids, 181 (2013) 142-151.
55] F. Ysambertt, F. Vejar, J. Paredes, J.L. Salager, Colloids Surf. A., 137 (1998) 189-196.
56] M.A. Rather, G.M. Rather, S.A. Pandit, S.A. Bhat, M.A. Bhat, Talanta, 131 (2015) 55-58.
57] C. Guo, J. Wang, H.Z. Liu, J.Y. Chen, Langmuir, 15 (1999) 2703-2708.
58] C. Guo, H.Z. Liu, J.Y. Chen, Colloid Polym. Sci., 277 (1999) 376-381.
59] Y.L. Su, H.Z. Liu, J. Wang, J.Y. Chen, Langmuir, 18 (2002) 865-871.
60] S.K. Mehta, S. Chaudhary, K.K. Bhasin, R. Kumar, M. Aratono, Colloids Surf. A., 304
(2007) 88-95.
1
4

Table 1: Specification of chemicals
Chemicals
Source
CAS No
Purification
Method
Mass Fraction
#
Purity
1
-methylimadazole
616-47-7
No further
purification
>99.0%
HIMEDIA
Laboratories Pvt.
Ltd
1
1
-bromopentane
-bromohexane
TCI Pvt. Ltd
110-53-2
111-25-1
No further
purification
No further
purification
>98.0%
99.0%
HIMEDIA
Laboratories Pvt.
Ltd
Acetonitrile
LOBA Chemie
Pvt. Ltd Mumbai
75-05-8
1120-01-0
129-00-0
No further
purification
Vacuum drying
>99.5%
>95.0%
98.0%
Sodium Hexadecyl
Sulfate
Pyrene
TCI Pvt. Ltd
No further
purification
SIGMA
ALDRICH Pvt.
Ltd.
#
As declared by supplier
1
5

Table 2: Conductance κ (µS) of SHS in (0.02, 0.05, 0.10) wt. % of [C
5
mim] [Br] at different
temperatures (298.15, 303.15 and 308.15) K
0
.02 wt.% [C mim] [Br]
0.05 wt.% [C mim] [Br]
5
0.10 wt.% [C mim] [Br]
5
5
Conc.
mM)
298.15K 303.15K 308.15K 298.15K 303.15K 308.15K 298.15K 303.15K 308.15K
(
κ (µS)
201.1
201.6
202.2
202.7
202.9
203.0
203.9
204.4
205.1
206.3
207.7
208.9
210.5
212.7
214.3
215.4
216.9
218.8
220.9
223.5
225.6
227.5
κ (µS)
309.3
309.6
309.9
310.1
310.5
310.9
311.5
311.7
312.7
313.7
315.6
317.5
319.4
322.1
323.9
325.8
327.3
329.7
332.0
334.6
336.9
339.6
κ (µS)
540.1
540.2
540.4
540.7
540.9
541.0
541.1
541.4
541.8
542.4
543.4
544.5
545.6
546.8
548.1
549.1
549.9
551.1
552.3
553.6
555.1
556.5
0
0
0
0
0
0
0
0
0
0
0
0
0
0
0
0
0
0
0
0
0
0
.00746
.01141
.01632
.02217
.02893
.03659
.04510
.05445
.07279
.09944
.13346
.17374
.21904
.26814
.31983
.37303
.42678
.49844
.58032
.66559
.74912
.83755
180.3
180.8
181.3
181.8
182.3
182.9
183.5
184.1
185.1
186.3
188.4
190.3
191.9
194.0
195.6
197.4
199.2
201.9
204.8
207.3
210.2
212.9
207.8
208.4
208.7
209.2
210.1
210.5
211.0
212.0
212.8
214.1
216.8
218.8
221.6
224.9
228.1
229.8
231.9
234.7
238.5
241.4
244.9
248.6
283.8
284.1
284.4
285.5
285.9
286.6
287.1
287.3
288.4
289.8
291.5
293.7
296.3
299.1
301.6
303.6
305.8
308.3
311.1
314.0
316.7
319.9
338.6
338.9
339.1
339.6
339.9
340.4
340.9
341.3
341.8
343.1
344.9
346.7
348.7
350.9
353.1
354.5
356.1
357.9
360.7
363.0
365.2
368.1
494.8
495.3
495.5
495.8
496.1
496.4
496.8
497.1
497.7
498.7
500.5
502.2
504.1
506.3
508.4
509.9
511.3
513.2
515.3
517.6
519.9
522.3
577.6
578.1
578.0
578.5
578.7
578.9
579.2
579.4
579.8
580.2
581.6
582.6
583.8
585.1
586.3
587.8
588.7
590.1
591.4
592.8
594.4
595.8
Standard uncertainties s are s (T) = ±0.1 K, s (κ) = ±0.1 µS
1
6

6
Table 3: Conductance κ (µS) of SHS in (0.02, 0.05, 0.10) wt. % of [C mim] [Br] at different
temperatures (298.15, 303.15 and 308.15) K
0
.02 wt.% [C
6
mim] [Br]
0.05 wt.% [C
6
mim] [Br]
6
0.10 wt.% [C mim] [Br]
Conc.
mM)
298.15K 303.15K 308.15K 298.15K 303.15K 308.15K 298.15K 303.15K 308.15K
(
κ (µS)
170.7
170.9
171.2
172.3
172.8
173.3
174.1
174.7
175.9
177.7
179.9
183.1
185.9
189.6
191.5
194.2
196.8
199.8
203.8
207.6
211.5
215.1
κ (µS)
295.6
295.9
296.4
296.9
297.2
297.9
298.3
298.5
299.4
300.5
302.6
304.8
306.9
309.4
311.8
313.7
315.6
317.8
320.9
323.3
326.1
329.0
κ (µS)
476.6
476.9
477.1
477.4
477.7
478.1
478.4
478.7
479.3
480.2
481.5
482.8
484.4
486.1
487.8
489.2
490.4
492.1
493.9
495.8
497.7
499.8
0
0
0
0
0
0
0
0
0
0
0
0
0
0
0
0
0
0
0
0
0
0
.00746 157
183.9
184.1
185.1
186.2
187.1
187.4
188.6
189.3
190.1
192.1
194.9
199.1
202.2
206.3
210.2
212.2
215.5
219.8
223.4
228.9
232.6
237.6
270.4
270.8
271.1
271.5
272.1
272.3
272.8
273.3
273.9
275.3
276.9
279.2
281.3
283.9
285.8
287.4
289.1
291.3
293.9
296.5
299.2
302.1
324.6
324.9
325.3
325.8
326.4
327.1
327.7
328.1
329.2
330.5
332.4
334.9
337.8
340.4
343.3
345.5
347.8
350.4
353.7
356.9
360.1
363.2
438.6
438.8
439
518
.01141 158.2
.01632 158.4
.02217 158.7
.02893 159.3
.03659 160.3
.04510 161.2
.05445 162.1
.07279 163.5
.09944 165.3
.13346 167
.17374 170.2
.21904 173.1
.26814 176.5
.31983 178.7
.37303 180.5
.42678 183.8
.49844 187.1
.58032 190.6
.66559 195.1
.74912 198.2
.83755 202.5
518.5
518.8
519.1
519.7
520.1
520.5
521.1
522.1
523.7
525.6
527.8
530.6
533.5
536.6
538.7
540.7
543.5
546.6
549.6
552.7
556.4
439.5
439.9
440.1
440.8
441.1
441.9
443.1
444.9
446.7
448.4
450.7
452.9
454.4
456.1
458.1
460.5
463.1
465.3
468.1
Standard uncertainties s are s (T) = ±0.1 K, s (κ) = ±0.1 µS
1
7

0
Table 4: Critical micelle concentration (CMC), degree of counter ion binding (α), free energy of micellization (ꢁG
m
), enthalpy of
0
0
micellization (ꢁH ), and entropy of micellization (ꢁS ) of SHS in (0.02, 0.05, 0.10) wt.% of [C mim] [Br] at different temperatures
m
m
5
(298.15, 303.15 and 308.15) K.
0
-1
0
-1
0
-1
-1
[C
5
mim] [Br]
CMC (mM)
α
ꢀG (kJ⋅mol )
ꢀH (kJ⋅mol )
ꢀS (J⋅mol ⋅K )
m
m
m
(wt.%)
T = 298.15 K
0
0
0
0
.00
.02
.05
.10
0.2173
0.2568
0.2849
0.3247
0.612
0.614
0.618
0.624
-42.84
-42.22
-41.72
-41.11
-20.28
-17.83
-14.42
-10.92
75.67
81.81
91.57
101.25
T = 303.15 K
0
0
0
0
.00
.02
.05
.10
0.2435
0.2879
0.3098
0.3499
0.620
0.621
0.624
0.627
-42.91
-42.29
-41.94
-41.43
-20.84
-18.33
-14.84
-11.26
72.79
79.05
89.40
99.52
T = 308.15 K
0
0
0
0
.00
.02
.05
.10
0.2648
0.3056
0.3281
0.3615
0.628
0.630
0.632
0.636
-43.08
-42.52
-42.21
-21.42
-18.82
-15.25
-11.56
70.31
76.90
87.48
97.94
-41.75
0
-1
0
-1
0
Standard uncertainties s are s (T) = ±0.1 K, s (CMC) = ± 0.0001 mM, s (ꢁG ) = ±0.03 kJ⋅mol , s (ꢁH ) = ±0.02 kJ⋅mol , s (ꢁS ) =
±
m
m
m
-1
-1
0.02 J⋅mol ⋅K
1
8

0
Table 5: : Critical micelle concentration (CMC), degree of counter ion binding (α), free energy of micellization (ꢁG
m
), enthalpy of
0
0
micellization (ꢁH ), and entropy of micellization (ꢁS ) of SHS in (0.02, 0.05, 0.10) wt.% of [C mim] [Br] at different temperatures
m
m
6
(298.15, 303.15 and 308.15) K.
0
-1
0
-1
0
-1
-1
[
C mim] [Br]
CMC (mM)
α
ꢀG (kJ⋅mol )
ꢀH (kJ⋅mol )
ꢀS (J⋅mol ⋅K )
6
m
m
m
(wt.%)
T = 298.15 K
0
0
0
0
.00
.02
.05
.10
0
0
0
0
.2173
.2378
.2669
.3069
0.612
0.625
0.629
0.632
-42.84
-42.14
-41.62
-41.06
-20.28
-17.54
-13.75
-10.62
75.67
82.50
93.46
102.08
T = 303.15 K
0
0
0
0
.00
.02
.05
.10
0
0
0
0
.2435
.2619
.2871
.3219
0.620
0.635
0.638
0.643
-42.91
-42.19
-41.78
-41.23
-20.84
-18.00
-14.12
-10.89
72.79
79.79
91.23
100.09
T = 308.15 K
0
0
0
0
0
.2648
.2826
.3057
.3409
0.628
0.641
0.644
0.646
-43.08
-42.45
-42.08
-21.42
-18.52
-14.53
-11.23
70.31
77.65
89.40
98.67
0
0
0
.02
.05
.10
-41.64
0
-1
0
-1
0
Standard uncertainties s are s (T) = ±0.1 K, s (CMC) = ± 0.0001 mM, s (ꢁG
±
m
) = ±0.03 kJ⋅mol , s (ꢁH
m
) = ±0.02 kJ⋅mol , s (ꢁS
m
) =
-1
-1
0.02 J⋅mol ⋅K
1
9

5
Table 6: Critical micelle concentration (mM) of SHS in (0.02, 0.05, 0.10) wt.% of [C mim] [Br]
CMC (mM)
Conductivity
measurement
Fluorescence
spectroscopy
UV-visible
spectroscopy
[
C mim] [Br] (wt.%)
5
0
0
0
.00
.02
.05
0.2173
0.2568
0.2849
0.3247
0.2154
0.2521
0.2789
0.3146
-
0.2575
0.2844
0.3112
0
.1
6
[C mim] [Br] (wt.%)
0
0
0
0
.00
.02
.05
.10
0.2173
0.2378
0.2669
0.3069
0.2154
0.2292
0.2661
0.3095
-
0.2388
0.2671
0.3131
and [C mim] [Br] using different techniques at 298.15K
6
Standard uncertainties s in s (CMC) = ± 0.0001 mM
2
0

Table 7: Wavenumber obtained from FT-IR spectra recorded for (0.02, 0.05, 0.10) wt. % of ILs
[
C mim][Br] and [C mim][Br] in the absence and presence of sodium hexadecyl sulfate (SHS)
5 6
-
1
wt.% of IL
SHS / (mM)
Wavenumber (cm )
5
[C mim] [Br]
0.02
0.05
0.10
0
3257
3272
3275
3269
3269
3256
3268
3272
3254
3273
3278
3269
0
0
0
0
0
0
0
0
0
0
0
.12832
.25663
.38495
.14197
.28393
.42590
.15987
.31973
.47960
[
C mim][Br]
6
0.02
0.05
0.10
0
0
0
0
0
0
0
0
0
0
0
0
3272
3277
3262
3278
3271
3269
3270
3272
3285
3272
3271
3278
.11823
.23647
.35470
.13357
.26713
.40070
.15402
.30803
.46205
2
1

Figure 1 Specific conductance (κ) versus concentrations of SHS in (0.02, 0.05 and 0.10) wt. %
of aqueous [C mim][Br] solutions at temperatures (298.15, 303.15 and 308.15) K
5
2
2

Figure 2 Specific conductance (κ) versus concentrations of SHS in (0.02, 0.05 and 0.10) wt. %
of aqueous [C mim][Br] solutions at temperatures (298.15, 303.15 and 308.15) K
6
2
3

0
Figure 3 Plot of standard free energy of micellization ꢁG , standard enthalpy of micellization
m
0
0
ꢁH
and standard entropy of micellization ꢁS of SHS solutions in water and in the presence
m
m
of (0.02, 0.05 and 0.10) wt. % of aqueous [C
and 308.15) K in the aqueous media
5
mim][Br] solutions at temperatures (298.15, 303.15
2
4

0
Figure 4 Plot of standard free energy of micellization ꢁG , standard enthalpy of micellization
m
0
0
ꢁH
and standard entropy of micellization ꢁS of SHS solutions in water and in the presence
m
m
of (0.02, 0.05 and 0.10) wt. % of aqueous [C
and 308.15) K in the aqueous media
6
mim][Br] solutions at temperatures (298.15, 303.15
2
5

Figure 5 Pyrene I / I versus [SHS] in presence of (a) 0.02 wt. % (b) 0.05 wt. % (c) 0.10 wt. %
I
III
of [C mim][Br] in the aqueous media, λ =320 nm.
5
ex
2
6

Figure 6 Pyrene I
I
/ IIII versus [SHS] in presence of (a) 0.02 wt. % (b) 0.05 wt. % (c) 0.10 wt. %
of [C mim][Br] ] in the aqueous media, λ =320 nm.
6
ex
2
7

Figure 7 Variation of absorbance with concentration of SHS in presence of (a) 0.02 wt. % (b)
.05 wt. % (c) 0.10 wt. % of [C mim][Br] in the aqueous media.
0
5
2
8