Interaction Between Two Anionic Dyes and Cationic Surfactant

Inter fill Between Two Anionic Dyes and cationic SurfactantThe fundamental interaction of the triphenylmethane soil xylenol orangeness with cationic bed wetters cetyltrimethylammonium cliche and cetylpyridinium chloride was analyse by ducking spectrophotometry and principal component analysis of infr atomic number 18d spectra by A. Gojmerac Ivic et al. 24. Upon the addition of wetters the yellow color of the dosageic xylenol orange solution changed to purple-red. Changes in the submergence spectra of the mixture exhibit strong interactions among dye and bedwetters. These interactions were also monitored victimization ATR spectroscopy and the most prominent changes were observe in the vibration of the carbonyl group. The comparison of principal component loadings obtained from unearthly data matrices for xylenol orange and mixtures of xylenol orange with wetters revealed differences in infrared spectra ca utilise only by the interaction of the surfactants with the dye .The interactions of Acid Green 25 (AG), an anionic detergent dye, with two cationic surfactants tetradecyltrimethylammonium bromide (TTAB), and hexadecyltrimethyl ammonium bromide (CTAB) in aqueous solutions far down the stairs the CMC are studied at opposite temperatures using the conductometric method by H. Dezhampanah et. al. 25. Various thermodynamic functions and equilibrium constants for the litigate of dye-surfactant ion equal physical composition were cipher using the conductometric data. There results indicate that the foresighteder aquaphobic chain surfactants had a greater tendency and higher equilibrium constant as compared to shorter hydrophobic chain surfactants and short range, non-electrostatic interactions a massive with long range electrostatic forces redeem a signifi raftt influence on dye surfactant ion span formation.Interaction of a food dye, tartrazine, with around cationic conventional and similitude surfactants, tetradecyltrimethylammonium bromid e (TTAB), N,N-ditetradecyl-N,N,N,N-tetramethyl-N,N-butanediyl-diammonium dibromide (14,4,14), and N,N-didodecyl-N,N,N,N-tetramethyl-N,N- butanediyl-diammonium dibromide (12,4,12), were first investigated comprehensively by A. Asadzadeh Shahir et al. 26, employing conductometry, tensiometry, and UV-visible spectroscopy. Tartrazine was found to behave in the same manner as aromatic counterions. The formation of ion pairs reflected as a considerable increase of the surfactant efficiency in tensiometry plots and their stoichiometry were laid by Jobs method of continuous variations. For the tartrazine/TTAB system, nonionic DS3, ionic DS2-, and/or DS2 ion pairs, their small premicelles, and tartrazine rich micelles were constituted as well as dye-containing TTAB-rich micelles. water-insoluble J-aggregates of DS ion pairs and cylindrical surfactant-rich micelles were also formed in tartrazine/gemini surfactant systems and recognized by transmission electron microscopy. The zeta potential and the coat of the aggregates were determined using dynamic light scattering and confirmed the suggested models for the processes happening in each system. Cyclic voltammetry was applied successfully to track all of these species using tartrazines own reduction peak current for the first time.Reza Hosseinzadeh et al. 27 investigated the solubilization and interaction of azo-dye light yellow (X6G) at/with cationic surfactants cetyltrimethylammonium bromide (CTAB) and cetylpyridinium chloride (CPC) spectrophotometricaly. The effect of cationic micelles on solubilization of anionic azo dye in aqueous micellar solutions of cationic surfactants was studied at pH 7 and 25 -C. The screening of dye to micelles implied a bathochromic shift in dye absorption spectra that indicates dyesurfactant interaction. The results showed that the solubility of dye increased with change magnitude surfactant submersion, as a consequence of the knowledge between the dye and the micelles. The blanket constants, Kb, were obtained from experimental absorption spectra. By using pseudo-phase model, the partition coefficients between the bulk water and surfactant micelles, Kx, were calculated. Gibbs energies of binding and distribution of dye between the bulk water and surfactant micelles were estimated. The results show favorable solubilization of dye in CTAB micelles.The accumulation induced by Alizarin Yellow R (AYR) in the cationic surfactant, cetyltrimethylammonium bromide (CTAB), was investigated by measuring their UVvisible absorption spectra by M. F. Nazar et al. 28. Conductance measurements as a function of surfactant concentration below and above the critical micelle concentration (CMC) were studied. CTAB aggregation takes place at the concentration far below its frequent CMC in the presence of AYR. Both hydrophobic and electrostatic interactions affect the aggregation process in aqueous solution. Different parameters obtained from spectroscopic measurements and conducta nce data indicate an enhanced solubility of AYR dye in the micellar region. Intramolecular hydrogen bond within the dye molecule effectively reduces intermolecular attraction, thereby change magnitude solubility in non-polar solvents (micelles). Medium personal effects on the position of the long wavelength absorption band of the azo dye characterize it as a pH chromic reporter molecule. A partitioning study of the solubilized system provides utilizable insight into the process of solubilization that is applicable to the general problem of membrane solubilization properties and in do drugs delivery to quantify the degree of drug-micelle interaction. The partition coefficient value obtained is essential in micellar electrokinetic capillary chromatography and high pressure liquid chromatography (HPLC) for drug quality control. Thus, interaction with micellar aggregates induces epoch-making pKa shifts of Alizarin Yellow R that can be rationalized in terms of the partitioning of sp ecies and electrostatic contribution. Likewise, knowledge of the effects of organic additives on the CMC of surfactants is used both for abstractive and practical purposes because some additives are likely to be present as impurities or bypperchucts in the manufacturing of surfactants and their presence may cause significant differences in supposedly confusable commercial surfactants.Eosin B and eosin Y have been used to estimate micro- and submicrogram quantities of proteins respectively. A.A. Waheed et al. 29 describe the mechanism of eosin binding to proteins. At pH lower than 3.0 the absorbance of unbound dye is greatly reduced. After the dye binds to protein, the absorption level best of the dye changes from 514 to 530 5 nm. The absorbance and bathochromatic shift in absorption maximum of the proteindye complex are proportional to the concentration of protein. The pH of the check solution does not change due to protein. Arginine, histidine, and lysine (at both acidic and deaf(p) pH) and tryptophan (at acidic pH) residues of a protein bind electrostatically to carboxylic and phenolic resin groups of the dye to produce a stable water-soluble proteindye complex. The binding constants of eosin B with poly-L-arginine, poly-L-histidine, poly-L-lysine, and poly-L-tryptophan at pH 1.96 are 0.37, 0.32, 0.33 and 0.33 nmol/nmol of amino acid, respectively. The binding constants of eosin B and eosin Y with bovine serum ovalbumin (BSA) at pH 1.96 are essentially the same, i.e., 0.82 nmol/nmol of reactive amino acid of BSA. The binding constant varies with solution pH so that a broad range of protein concentrations can be estimated. The reason for the higher absorbance of proteineosin Y complex compared to that of proteineosin B complex is discussed.Javadian et al. 30 studied the interaction of congou Red (CR) with a series of Alkyl trimethyl ammonium bromide (CnTAB), N-hexadecyl pyridinium bromide (CPB) and N-hexadecyl pyridinium chloride (CPC) using conducto metry and UV-Vis spectroscopy technique. Jobs method of continuous variations demo that only DS complexes are formed in the studied mixtures. The formation of DS complexes results in decreasing the systems order so it is an enthalpy-driven reaction under(a) the influence of both hydrophobic and electrostatic interactions. The amount of ion pairs forming through the process is highly dependent on physical conditions and structure of the dyes and the surfactants such as chain length, head group and counterion. By increasing the length in the hydrophobic chain or the charge density of headgroup of a cationic surfactant, the strength of dye-surfactant interaction increases. In addition, the results show that the counter ion has no significant effect on dye-surfactant interaction. The tendency to form DS complexes decreases with increasing temperature in the range of 298.0-313.0 K.K. Fujio et al. 31 examined the effect of added salt on micelle size, shape, and structure the solubilizat ion of Orange OT in aqueous NaBr solutions of decylpyridinium bromide (DePB), dodecylpyridinium bromide (DPB), tetradecylpyridinium bromide (TPB), and hexadecylpyridinium bromide (CPB). The solubilization powers of DePB and DPB micelles increase with increasing NaBr concentration up to 2.86 and 3.07 mol dm3, respectively, but above these concentrations delay unaltered. This suggests that spherical micelles of DePB and DPB can have a maximum and constant size at NaBr concentrations higher than these threshold concentrations. On the other hand, the solubilization powers of TPB and CPB micelles increase in the whole range of NaBr concentration studied. The dependencies of the solubilization powers of their micelles on the counterion concentration change at 0.10 and 0.03 mol dm3 NaBr, respectively, as suggests that TPB and CPB micelles undergo the sphererod transition at those concentrations. Orange OT is a more suitable look into for detecting the presence of the maximum- and constan t-size spherical micelle than Sudan Red B.The interactions between two anionic dyes and a cationic surfactant were studied by conductometric technique by A. A. Rafati et al. 32. The conductance of aqueous solutions of methyl orange (MO) and methyl red (MR) was measured in the presence of a cationic surfactant, cetylpyridinium bromide (CPB) at different temperatures in waterethanol, waterpropanol and waterbutanol mixed solvents, containing different concentration of inebriants. The equilibrium constants and other thermodynamic functions for the process of dyesurfactant ion pair formation were calculated on the basis of a theoretical model. The results showed that the presence of alcohol, as well as increasing the length of the alcohol chain, decreases the tendency for ion pair formation. The results have shown that an increase in temperature lowers the tendency for ion pair formation as the equilibrium constants decrease with increasing temperature. According to the results, long ra nge as well as short range interactions are responsible for the formation of the ion pair. The importance of long range electrical forces is fundamentally to bring the dye anion and the surfactant cation close enough to enable the action of short range interactions whose contribution represents the major part of the ensample discontinue energy change for the formation of the anionic dyecationic surfactant ion pair. By using the association constant (K1) for the first step of the association D+S+(DS), the standard free energy change, standard enthalpy change, and standard entropy change of the association were calculated at low surfactant concentrations.