Review of the literature shows that the study of discussion of dye-surfactants and dye-amino acids provide useful important info about physiological systems because of its popular applications and relatively complicated behavior. These investigations are important from perspective of technology of dyeing procedures as well for chemical researches, such as biochemistry, analytical chemistry, and photosensitization. A lot of the work on amino acids and biomolecules have been carried out in genuine and combined aqueous solutions but the research of spectroscopic, tensiometric and thermodynamic properties of amino acids in aqueous dye solution has seldom been done. On the other hand although studies have been made relating dye-surfactant interactions, yet this specific field of research is still very important to improvised dyeing process in conditions of theoretical, technical, environmental as well as financial viewpoint [1]. The dye-surfactant conversation has importance in many areas such as the spectral behaviour of dye in microheterogenous systems, dye-sensitized solar panels, and photocatalysis like photocatalytic drinking water splitting. It is important to understand how surfactants and dyes interact in aqueous answers to clarify the mechanisms of dyeing and other finishing methods. Hence the investigation of interaction between surfactants / amino acid in aqueous dye solution was performed using different useful techniques.
Mata et. al [2] investigated the physicochemical properties of natural cationic surfactants (quaternary salts) in aqueous solution through surface anxiety (at 303. 15 K), conductance (at 293. 15-333. 15 K), dye solubilization and viscosity measurements. From results it appeared that changes in the type of the surfactant (such as changes in chain length, polar mind group or counter ion) have a severe effect on the next self-assembly in water. The upsurge in hydrophobic personality of the surfactant reduces the CMC, induces sphere-to-rod transition at lower attentiveness and increases the solubilizing vitality of surfactant towards orange OT. Viscosity results suggested that how big is the micelles is relatively small at CMC and increases much longer with increasing surfactant concentration. The plots of differential conductivity, (dk/dc)T, P, versus the full total surfactant concentration enables us to look for the CMC prices more precisely.
The critical micelle attention (cmc) and amount of ionization (О) of cationic surfactants, dodecyldimethylethylammonium bromide (DDAB) and dodecyltrimethylammonium chloride (DTAC) in aqueous multimedia were dependant on Mehta et. al [3] from the conductivity measurements at different conditions. The cmc habit of DDAB and DTAC was examined in comparison to the results of DTAB in terms of effect of counter-top ion and increase in alkyl chain. It had been observed that by changing the counter-top ion from chloride (DTAC) to bromide along with the upsurge in alkyl string on polar brain group (DDAB), the cmc shows a decrease. Thermodynamics of the system unveils that at lower heat, the micellization in case there is DDAB was found to be entropy-driven, while at higher heat it was enthalpy driven. In DTAC system only entropic impact dominates over the entire heat range range.
The aggregation properties of a cationic surfactant, DTAB, at different compositions in water-DMSO mixtures was analyzed by Vronique Peyre et. al [4] using combination of techniques such as SANS, conductivity, and density measurements. Different complementary methods were used for the interpretations of data. This multi-technique analysis explains the reason for the reduction in ionization level, role of solvation in micellization and emphasizing the dissymmetric solvation of the string by DMSO and the head by water. The analysis is interesting from the idea of view that micellization process has been identified by using blended research from molecular to macroscopic size.
Apparent and partial molar amounts of decyldimethylbenzylammonium chloride (C10DBACl) at (15, 25, and 35) C have been determined from results of density measurements by A. G. Perez et. al [4]. The specific conductivities of the solutions have been established at the same temps. The results dished up for the estimation of critical micelle amount, cmc, ionization level, (О), and standard free energy of micellization, (Л† G), of the surfactant.
J. J. Galan, J. R. Rodr±guez [5] researched the molality dependence of specific conductivity of pentadecyl bromide, cetylpyridinium bromide and cetylpiridinium chloride in aqueous solutions in the heat range of 30-45 -№C. The critical micelle attentiveness (cmc) and ionization degree of the micelles, О, were decided directly from the experimental data. Looking at our results for C16PBr and C16PCl drinking water solutions, it can be discovered that the substitution of the bromide anion by a lot more hydrophilic chloride causes an increase in cmc by a factor of around 1. 3.
Chanchal Das and Bijan Das [6] have examined the micellization patterns of three cationic surfactants, viz. , hexadecyl-, tetradecyl-, and dodecyltrimethylammonium bromide (CTAB, TTAB, and DTAB, respectively) in ethylene glycol (EG) (1) + normal water (2) merged solvent mass media with differing mass fractions of EG (w1) by means of electro-mechanical conductivity and surface anxiety measurements. Temps dependence of the critical micelle concentrations was also investigated to comprehend the micellar thermodynamics of the systems. From the analysis of the temp dependence of the cmc of the surfactants in the EG (1) + drinking water (2) mix with w1 ) 0. 30, they had demonstrated that the micellization was mainly governed by an enthalpy-entropy compensation impact. Data on the thermodynamics of adsorption demonstrate that the top activity of the surfactant decreases with the addition of EG to normal water at a given temps and that the adsorption of surfactant at the air/combination interface takes place spontaneously.
The micellisation behaviour of cetyltrimethylammonium bromide (CTABr) in several mass small percentage (17-47) of ethylene glycol (EG), dimethylsulfoxide (DMSO), and dimethylformamide (DMF)-water mixed solvents, was researched by Olaseni et. al [7] using electrical power conductivity measurement at different temperature ranges (293. 1-313. 1 K). The results of the thermodynamic evaluation proved that addition of organic solvents, that are principally situated in the bulk phase made the micellisation process less spontaneous. The London-dispersion discussion represented the major attraction drive for micellisation and micellisation proceeded via an exothermic process.
Sar Santosh K and Rathod Nutan [8] assessed cmc, О± value and the thermodynamic parameters of the procedure of micellization for alkyl (C12, C14, and C16) trimethylammonium bromide systems in existence of water-dimethylformamide (5-20 % v/v) binary mixtures more than a temperature selection of 298-318 K. It was observed that both the cmc and О± value were reliant upon the (v/v %) of solvent and heat and the micellization propensity of cationic surfactant lowers in the presence of solvents. It was also noticed that the micellization is favored generally by entropy and enthalpy at higher heat, whereas it is favored mainly by entropy at low conditions.
A. Ali et. al [9] have researched the thermodynamic properties of sodium dodecyl sulphate in micellar solution of L-serine and L-threonine by fluorescence spectroscopy and energetic light scattering techniques. They noticed a decrease in cmc of SDS in Thr alternatives as compared to that in Ser. The motivated beliefs of Л† G become significantly negative in the order: normal water > Ser >Thr, suggesting that the formation of micelles is more beneficial in presence of amino acids than in clear water. The aggregation tendencies of SDS was discussed in terms of structural changes in mixed solutions. Based on vibrant light scattering it was recommended that the size of SDS micelles was influenced by the occurrence of proteins.
F. Jalali and A. Gerandaneh [10] computed the critical micelle focus (cmc) of cetyltrimethylammonium bromide (CTAB) conductometrically in binary mixtures of drinking water + cosolvent at various temperatures and in the presence of potassium bromide (2. 0 - 14 X10-3 M). Dioxane and acetonitrile were used as cosolvents added to drinking water. Addition of organic solvents to drinking water increased the cmc value of CTAB, but the presence of KBr reduced cmc. Thermodynamic parameters of micellization, were evaluated for each and every solution based on the pseudo-phase model, and the changes seen in these parameters were related to the presence of KBr and cosolvents in aqueous solution.
The conductivity of (cosolvent C normal water) in the existence of increasing amount of 1-hexadecylpyridinium bromide was assessed at various temperatures by F. Jalali et al. [11]. Acetonitrile, dimethylformamide, dimethylsulfoxide, dioxane and ethylene glycol were used as cosolvents. In the conductivity data, the critical micelle attention c. m. c. , and the effective degree of counter-top ion dissociation α, were obtained at various conditions. In every the cases studied, a linear relationship between ([c. m. c] / mol. dm-3) and the mass portion of cosolvent in solvent mixtures was discovered. The thermodynamic properties ˆ Hand ˆ Swere examined from the temp dependence of the equilibrium constants for micellization of the surfactant. As the micellization process in pure water is both enthalpy and entropy stabilized, it becomes entropy destabilized in every solvent mixtures used; the prices of ˆ S being more negative with upsurge in the cosolvent content of the solvent mixtures. The producing ˆ H against Tˆ S plot showed a reasonably good linear correlation, indicating the living of an enthalpy-entropy reimbursement in the micellization process.
The aftereffect of the simultaneous presence of the electrolyte (NaBr) and nonelectrolyte kinds (DMSO and AN) in aqueous solution on the micellization of HDPB was researched by F. Jalali and A. Shaeghi Rad [12]. They figured the existence of NaBr favors the micellization of HDPB due mainly to a decrease in repulsions between micelle head organizations. Adding a cosolvent, such as DMSO or AN, to normal water inhibits the formation of micelles due to upsurge in hydrophobic identity of the merged solvent, which increases the attraction of surfactant monomers toward the solvent.
