# Effect of Methanol on Viscosity of Aqueous Solutions of Cationic Surfactants at 298.15 to 323.15 K

Authors: Sujit Kumar Shah; Sujeet Kumar Chatterjee; Ajaya Bhattarai
Journal: Journal of Chemistry
 (2016)

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## Abstract

Viscosity measurements have been made to the solutions of dodecyltrimethylammonium bromide (DTAB) and cetyltrimethylammonium bromide (CTAB) in 0.10, 0.20, 0.30, and 0.40 volume fractions of methanol in methanol-water mixed solvent media at 298.15, 308.15, 318.15, and 323.25 K. Critical micelle concentration (CMC) values have been determined. From relative viscosity for surfactant solutions, related viscosityB coefficients are calculated and the values are interpreted in terms of solute-solvent interactions.


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## Body

## 1. Introduction

Cationic surfactants find applications on different fields such as antibacterial properties, lubricants, retarding agents, softeners, and antistatic agents [1, 2]. Properties of surfactants are evaluated by the formation of aggregates known as micelle which is affected by different factors such as presence of organic and inorganic additives and temperature. Due to these reasons, micellization of cationic surfactants in binary mixed solvent media has been studied extensively by the researchers [2–8].Study of viscosity is very important to elucidate the behavior of solute-solvent interaction [9] which is important to describe the properties of microemulsion and liquid crystal with respect to micellar solution of surfactant system. In surfactant system, the interaction between surfactant and the solvent is of great interest due to two kinds of interactions: one is interaction of solvent with solvophobic part (tail) and another is solvent with solvophilic part (head) of surfactant molecules. Due to these two interactions there is change in the viscous flow of liquid and thereby change in various physiochemical properties [1].


## 2. Materials and Methods

Two cationic surfactants were used for the investigation: dodecyltrimethylammonium bromide (DTAB) and cetyltrimethylammonium bromide (CTAB). These chemicals were purchased from Loba Chemie Private Limited, Mumbai, India, whereas methanol was purchased from Merck, India.Doubly distilled water was used for all experiments and the solvent mixtures of desired composition were prepared by mixing water and methanol volumetrically in volumetric flask maintained at constant temperature in water bath. The solvent mixture was kept overnight to ensure the proper mixing of the water and alcohol. Accurate weight of surfactant with the help of digital high precision electronic balance (accuracy±0.0001 g) was taken and dissolved in the minimum amount of solvent mixture and was kept overnight for proper dissolution after which the solvent mixture was added to make the desired volume up. The freshly prepared solution was used for the further investigation [8].Viscosities of solutions were calculated by viscous flow time (VFT) method using the Mansingh Survismeter [10]. In this method, the time flow for the given volume of solution and the same volume of solvent is taken with the help of digital watch and the viscosity was calculated with the help of following formula:(1)
η
s
o
l
n
=
t
s
o
l
n
t
s
o
l
v
d
s
o
l
n
d
s
o
l
v
η
s
o
l
v
,where η
s
o
l
n is viscosity coefficient of solution, η
s
o
l
v is viscosity coefficient of solvent, t
s
o
l
v is flow time of solvent, t
s
o
l
n is flow time of solution, d
s
o
l
n is density of solution, and d
s
o
l
v is density of solvent.


## 3. Results and Discussion

When methanol is added in water, it mixes rapidly and the mixing is exothermic due to which there is considerable reduce in volume. The decrease in volume may be due to breaking of “iceberg” structure of water. In spite of this, there is decrease in the dielectric constant and increase in viscosity when methanol is added in water. The physical properties such as density (ρ), viscosity coefficient (η), and dielectric constant (D) of 0.10, 0.20, 0.30, and 0.40 volume fractions of methanol in methanol-water mixed solvent media at 298.15, 308.15, 318.15, and 323.15 K are depicted in Table 1 [11].Table 1
Properties of methanol-water mixtures containing (0.10, 0.20, 0.30, and 0.40) volume fraction of methanol at 298.15 K, 308.15 K, 318.15 K, and 323.15 K.
Volume fraction of methanol
T/K
ρ/(g cm−3)
η/(µPa s)
D
0.10
298.15
0.98297
1084.4
75.09
308.15
0.97973
866.5
71.57
318.15
0.97604
701.7
68.18
323.15
0.97438
637.5
66.45
0.20
298.15
0.96963
1310.6
71.61
308.15
0.96632
1021.7
68.14
318.15
0.96162
807.5
64.80
323.15
0.95875
730.0
63.15
0.30
298.15
0.95620
1471.2
67.65
308.15
0.95160
1141.8
64.25
318.15
0.94626
895.7
60.99
323.15
0.94331
805.2
59.41
0.40
298.15
0.93957
1447.5
63.53
308.15
0.93364
1203.4
60.34
318.15
0.93140
930.9
57.18
323.15
0.92800
828.8
55.62The variation of viscosity with concentration of solutions of DTAB and CTAB is presented in Figures1 and 2, respectively, as representative graphs. It is seen that there is remarkable breakage, called critical micelle concentration (CMC), in the plot in both DTAB and CTAB solutions at particular temperature. The CMC values of DTAB and CTAB in 0.10, 0.20, 0.30, and 0.40 volume fractions of methanol in methanol-water mixed solvent media at 298.15, 308.15, 318.15, and 323.15 K are presented in Table 2. It is obvious from Table 1 that with the increasing volume fraction of methanol, the dielectric constant of medium decreases which causes the increase in electrostatic repulsions between ionic head groups. This makes micellization less favorable and micellization delays. Temperature effect shows that there is increase in CMC with the increase in temperature. This phenomenon is analyzed in terms of two opposing factors. First, with the increase in temperature, the degree of hydration of hydrophilic tails decreases which favors the micellization. And, second, increase in temperature also causes the disruption of the water structure surrounding the hydrophobic group and micellization is delayed [1, 8].Table 2
CMC values of dodecyltrimethylammonium bromide (DTAB) and cetyltrimethylammonium bromide (CTAB) in water and 0.10, 0.20, 0.30, and 0.40 volume fractions of methanol-water at 298.15 K, 308.15 K, 318.15 K, and 323.15 K.
T/K
Volume fraction of methanol
CMC/mM
DTAB
CTAB
298.15
0.0
14.5
0.97
0.1
17.5
1.21
0.2
20.5
1.76
0.3
25.1
3.86
0.4
34.5
6.83
308.15
0.0
15.4
1.12
0.1
18.1
1.38
0.2
21.7
1.80
0.3
26.4
4.56
0.4
35.6
7.23
318.15
0.0
16.3
1.23
0.1
19.5
1.68
0.2
22.8
2.64
0.3
27.3
5.74
0.4
36.7
7.47
323.15
0.0
17.3
1.30
0.1
20.5
1.80
0.2
23.7
2.83
0.3
28.1
5.82
0.4
37.8
7.44Figure 1
Viscosity versus surfactant concentration plot for DTAB in water at 298.15 K.Figure 2
Viscosity versus surfactant concentration plot for CTAB in water at 308.15 K.From Figures1 and 2, at lower concentration, that is, below CMC, the variation of viscosity is almost constant. However, at higher concentration, that is, above CMC, there is considerable variation of viscosity with concentration of surfactant solution. The variation is linear. This shows that the solute-solvent interaction is taking place with the increase in concentration. The increase in viscosity with concentration is attributed to increase in frictional force between solute and solvent. With the addition of methanol viscosity of solution increases (Figures 3 and 4) further at particular temperature. It can be explained by decrease in the average distance between surfactant and water molecules causing stronger frictional force [1, 4]. Viscosity decreases with the increase in temperature because, at higher temperature, kinetic energy of molecules increase which weakens the intermolecular force operating on the viscous flow with the net decrease in the frictional force [10].Figure 3
Viscosity versus concentration of DTAB solution at 298.15 K.Figure 4
Viscosity versus concentration of CTAB solution at 298.15 K.The graphical presentation of CMC with volume fraction of methanol of DTAB and CTAB at different temperatures are given in Figures5 and 6. It is seen from Table 2 and Figures 5 and 6 that CMC strongly depends on the methanol content and also on temperature. With the increase in volume fraction of methanol, CMC increases for both the surfactants at particular temperature. This phenomenon is attributed to physical properties of methanol-water mixed solvent media.Figure 5
Variation of CMC with volume fraction of methanol of DTAB solution at different temperatures.Figure 6
Variation of CMC with volume fraction of methanol of CTAB solution at different temperatures.The interaction between solute and solvent is well described in terms of viscosityB coefficient given by Jones-Dole equation of viscosity as presented in (2) [12]. Consider (2)
η
r
=
1
+
A
c
+
B
c
,where η
r
=
η
/
η
0 is the relative viscosity of a solution and A and B are constants and c represents concentration of solution. Equation (2) can be rearranged as (3)
η
r
-
1
c
=
A
+
B
c
.The A coefficient represents the contribution from interionic electrostatic force. The B coefficient denotes solute-solvent interaction.Plot of(
η
r
-
1
)
/
c versus c for DTAB and CTAB solutions in water and different volume fractions of methanol-water in the range of postmicellar region is presented in Figures 7 and 8 in which the variations are linear. From the slopes of these plots the viscosity B coefficients are determined. The variations of B values of DTAB and CTAB with volume fraction of methanol at different temperatures are presented in Figures 9 and 10, respectively.Figure 7
Plot of(
η
r
-
1
)
/
c versus c for DTAB solution at 298.15 K.Figure 8
Plot of(
η
r
-
1
)
/
c versus c for CTAB solution at 308.15 K.Figure 9
Variation of viscosityB coefficients DTAB solutions with volume fraction of methanol.Figure 10
Variation of viscosityB coefficients of CTAB solutions with volume fraction of methanol.It is seen from Figures9 and 10 that addition of methanol and temperature have considerable influence on the B values. With increased volume fraction, B values increase whereas they decrease with increase in temperature. The former effect can be attributed to the stronger solute and solvent interaction. Addition of methanol makes the solvent more hydrophobic due to which solubilization of micelle takes place and the intermolecular force between more hydrophobic solvent and tail of surfactant molecules increases. The effect of temperature can be attributed to thermal expansion with the increase in temperature. This makes the intermolecular force less effectively competitive and therefore solute-solvent interaction decreases as indicated by lower B values [10, 12].


## 4. Conclusions

The influence of methanol addition on micellization of DTAB and CTAB has been investigated by viscosity measurement. CMC values are determined in 0.10, 0.20, 0.30, and 0.40 volume fractions of methanol-water mixed solvent media at 298.15 K, 308.15 K, 318.15 K, and 323.15 K. These values of CMC reveal that CMC increases with the increase volume fraction of methanol-water due to decrease in dielectric constant of medium as well as due to breaking of water structure. Moreover, calculation of viscosityB coefficient values shows that there is strong solute-solvent interaction that assists the change in micellar structure.



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*Source: 2176769-2016-06-26.xml*