Conductometric Probe Analysis of the Effect of Benzyldimethylhexadecylammonium Chloride on the Micellization Behavior of Dodecyltrimethylammonium Bromide in Aqueous/Urea Solution: Investigation of Concentration and Temperature Effect

Abstract

Surfactant mixtures are used in many different industrial formulations. In this study, the mixed micelle formation behavior of 2 different cationic surfactants, namely dodecyltrimethylammonium bromide (DTAB) and benzyldimethylhexadecylammonium chloride (BDHAC), in the absence and presence of urea at various temperatures (298.15–318.15 K) was studied using the conductometric method. The attractive interaction between DTAB and BDHAC was estimated from the values of critical micelle concentration (CMC) and the CMC for ideal mixing (CMCid). Urea increases the CMC value as a result of the enrichment in the surface charge of the micelles/mixed micelles. The values of micellar mole fraction (X1Rub [Rubingh], X1M [Motomura], X1Rod [Rodenas]) and ideal micellar (X1id) of surfactant BDHAC were obtained by different models and are shown to exhibit the high contribution or effective involvement of BDHAC in mixed micelles and increase with increasing BDHAC mole fraction (α1). Activity coefficients (f1 and f2) were also evaluated from the relevant formula given in the literature. The negative values of the interaction parameters (β) show the attractive interaction among the studied components. Excess Gibbs free energy (∆Gex) of micellization revealed that the stability of mixed micelles is higher in aqueous solution than in urea solution. The thermodynamic parameters, namely the Gibbs free energy change, enthalpy change, and entropy change (∆Gom, ΔHom, and ∆Som, respectively), were also calculated from the conventional standard equations.

Aggregation Behavior of Sodium Dodecyl Sulfate and Cetyltrimethylammonium Bromide Mixtures in Aqueous/Chitosan Solution at Various Temperatures: An Experimental and Theoretical Approach

“…The excess free energy of micellization can be utilized to investigate the nonideality of the mixed micelles due to the interaction between the studied surfactants (Azum et al, , , ; Kumar et al, ; Molla et al, ; Picullel and Lindman, ; Rub et al, , , , ) by means of the following equations: …”

“…The excess free energy of micellization can be utilized to investigate the nonideality of the mixed micelles due to the interaction between the studied surfactants (Azum et al, 2016(Azum et al, , 2017c(Azum et al, , 2017dKumar et al, 2018;Molla et al, 2018;Picullel and Lindman, 1992;Rub et al, 2014aRub et al, , 2014bRub et al, , 2017aRub et al, , 2017b by means of the following equations:…”

Effects of temperature and polyols on the ciprofloxacin hydrochloride-mediated micellization of sodium dodecyl sulfate

“…Also, the drug delivery and release rate are functions of the molecular interaction of a drug with surfactants; thus, these molecular interactions can be explained in terms of thermodynamic parameters, and the values of different thermodynamic parameters can be utilized in drug formulation to achieve better drug delivery and drug release rates. The spontaneity or non-spontaneity of micellization can be measured from the DG m values of micellization, which can be executed based on the pseudo-phase partition model [60][61][62][63] through the following relation:…”

Influence of Additives and Temperature on the Interaction of Acid Red 151 Dye with Cetyltrimethylammonium Bromide: A Conductometric Study

“…The values of free energy of micellization (ΔG 0 m ) for ionic surfactants possessing one monovalent head group and a monovalent counterion were calculated using the following equation (Khan et al, 2015;Medoš and Rogač, 2015;Molla et al, 2018):…”

“…where R and X cmc refer to the ideal gas law constant and mole fraction of CTAB at the CMC, respectively. The standard enthalpy changes of micellization ΔH 0 m À Á were estimated through a modified van't Hoff's equation (Khan et al, 2015;Medoš and Rogač, 2015;Molla et al, 2018):…”