Kesharsingh J. Patil

Self-aggregation of Methylene Blue in aqueous medium and aqueous solutions of Bu4NBr and urea

The self-aggregation of Methylene Blue [MB] (1×10−6–4×10−4 M) in water and in aqueous solutions of Bu4NBr (0.1–0.3 M) and urea (0.1–4 M) has been investigated by recording electronic spectra in the wavelength range 550 to 700 nm. Analysis of the spectral data yielded the dimer dissociation constant, and individual characteristic monomer and dimer spectra. By applying the exciton model for the first time, the interaction energy between the MB molecules in the dimer species has been evaluated. Further, information about the dimer geometry and the twist angle between the dipoles of the MB molecules in the dimer species has been obtained. Similar data have also been obtained for solutions of MB in aqueous urea and Bu4NBr solutions. The significant observation is the change in the dimer geometry from sandwich type to end-on-end type in the presence of urea and Bu4NBr. It is observed that the contribution to the interaction energy is mainly from van der Waals type and dispersion forces, in addition to short-range forces involving multipoles. However, the contribution from hydrogen-bonding interactions between MB and water molecules is found to be significantly low. It is proposed that water structural effects and hydrophobic interactions are the major factors in the phenomenon of aggregation.

Thermodynamic studies of ionic interactions in aqueous solutions of imidazolium-based ionic liquids [Emim][Br] and [Bmim][Cl].

Experimental measurements of density at different temperatures ranging from 293.15 to 313.15 K, the speed of sound and osmotic coefficients at 298.15 K for aqueous solution of 1-ethyl-3-methylimidazolium bromide ([Emim][Br]), and osmotic coefficients at 298.15 K for aqueous solutions of 1-butyl-3-methylimidazolium chloride ([Bmim][Cl]) in the dilute concentration region are taken. The data are used to obtain compressibilities, expansivity, apparent and limiting molar properties, internal pressure, activity, and activity coefficients for [Emim][Br] in aqueous solutions. Experimental activity coefficient data are compared with that obtained from Debye-Hückel and Pitzer models. The activity data are further used to obtain the hydration number and the osmotic second virial coefficients of ionic liquids. Partial molar entropies of [Bmim][Cl] are also obtained using the free-energy and enthalpy data. The distance of the closest approach of ions is estimated using the activity data for ILs in aqueous solutions and is compared with that of X-ray data analysis in the solid phase. The measured data show that the concentration dependence for aqueous solutions of [Emim][Br] can be accounted for in terms of the hydrophobic hydration of ions and that this IL exhibits Coulombic interactions as well as hydrophobic hydration for both the cations and anions. The small hydration numbers for the studied ILs indicate that the low charge density of cations and their hydrophobic nature is responsible for the formation of the water-structure-enforced ion pairs.

Studies of partial molar volumes of 18-crown-6 in water at 25 C

Abstract Measurements are reported for the density of aqueous solutions of 18-crown-6 in the concentration range of 0.1 m to 4.5 m at 25 C. The data is used to obtain apparent and partial molar volumes of 18-crown-6. It is observed that the partial molar volume goes through a minimum at about 2.5 m concentration. The limiting partial molar volume obtained, indicate a large negative limiting excess volume. These results are compared with the similar data reported earlier in D2O. It is sugessted that the hydrophobic hydration of the 18-crown-6 is important in dilute concentration range due to which a structure making effect similar to that of apolar solutes is observed.

Studies of Activity Coefficients for Ternary Systems: Water + 18-Crown-6 + Alkali Chlorides at 298.15 K

Osmotic vapor pressure measurements have been carried out for three ternary systems, H2O + 0.2 m 18-crown-6 + LiCl, H2O + 0.2 m 18-crown-6 + NaCl and H2O + 0.2 m 18-crown-6 + KCl at 298.15 K using vapor pressure osmometry. Water activities for each ternary system were measured and used to calculate the activity coefficients of 18-crown-6 (18C6) and its salts following the methodology developed by Robinson and Stokes for isopiestic measurements. In the concentration range studied, it was found that (in NaCl and KCl solutions) there is considerable lowering of activity coefficients of one component in the presence of other solutes that has been attributed to the formation of the complexed 18C6:Na+ (or 18C6:K+) species in solution. The Gibbs energies of transfer of alkali chlorides from water to aqueous 18C6 solutions and that of 18C6 from water to aqueous electrolyte solutions have been calculated. These were further used to evaluate the pair and triplet interaction parameters. The calculation of thermodynamic equilibrium constants using the pair interaction parameter, gNE (i.e., the nonelectrolyte–electrolyte pair interaction) for the studied complexation of cations yields values which are in good agreement with those reported in literature obtained by using ion-selective potentiometry and calorimetry. The results are discussed in terms of water structural effects, complex formation, and hydrophobic interactions.

Thermodynamic studies of aqueous solutions of 2,2,2-cryptand at 298.15 K: enthalpy-entropy compensation, partial entropies, and complexation with K+ ions.

The osmotic coefficient measurements for binary aqueous solutions of 2,2,2-cryptand (4,7,13,16,21,24-hexaoxa-1,10-diazabicyclo[8.8.8] hexacosane) in the concentration range of ~0.009 to ~0.24 mol·kg(-1) and in ternary aqueous solutions containing a fixed concentration of 2,2,2-cryptand of ~0.1 mol·kg(-1) with varying concentration of KBr (~0.06 to ~0.16 mol·kg(-1)) have been reported at 298.15 K. The diamine gets hydrolyzed in aqueous solutions and needs proper approach to obtain meaningful thermodynamic properties. The measured osmotic coefficient values are corrected for hydrolysis and are used to determine the solvent activity and mean ionic activity coefficients of solute as a function of concentration. Strong ion-pair formation is observed, and the ion-pair dissociation constant for the species [CrptH](+)[OH(-)] is reported. The excess and mixing thermodynamic properties (Gibbs free energy, enthalpy, and entropy changes) have been obtained using the activity data from this study and the heat data reported in the literature. Further, the data are utilized to compute the partial molal entropies of solvent and solute at finite as well as infinite dilution of 2,2,2-cryptand in water. The concentration dependent non-linear enthalpy-entropy compensation effect has been observed for the studied system, and the compensation temperature along with entropic parameter are reported. Using solute activity coefficient data in ternary solutions, the transfer Gibbs free energies for transfer of the cryptand from water to aqueous KBr as well as transfer of KBr from water to aqueous cryptand were obtained and utilized to obtain the salting constant (ks) and thermodynamic equilibrium constant (log K) values for the complex (2,2,2-cryptand:K(+)) at 298.15 K. The value of log K = 5.8 ± 0.1 obtained in this work is found to be in good agreement with that reported by Lehn and Sauvage. The standard molar entropy for complexation is also estimated for the 2,2,2-cryptand-KBr complex in aqueous medium.

The studies of viscosity behaviour in aqueous 18-crown-6 solutions at 25°C

Abstract The viscosities of aqueous solutions of 18-crown-6 (0.04 – 0.24 M) have been measured at 25°C. The relative viscosities, in the studied concentration range, can be fitted well with the relation η = 1 + Bc + Dc2. The viscosity B-coefficient and D-coefficient are found to be high when compared with those reported for other simple non-electrolyte solutes. These results are interpreted in terms of hydrophobic hydration and occupation of crown ether cavities by water molecules, leading to the formation of a spherical entity (brownon), slipping through the hydrophobic hydration sheath. The analysis of the data shows that ⋍ 5 water molecules are embedded in the crown ether cavity. The structural interactions may involve stacking type equilibria stabilized by co-operative interactions amongst the water molecules in the cavity of one crown ether molecule with those of the other crown ether molecule. Preliminary results of the viscosity measurements of the 0.24 M aqueous 18C6 solutions involving varied amounts of the salt, KBr are also reported. The viscosity B-coefficient for KBr in aqueous crown ether solutions is found to be almost similar to that found in the aqueous solutions. However, the A-coefficient (a measure of ion-ion interactions) cannot be interpreted unambiguously.

Near infrared spectral investigations of hydration of 18-crown-6 in HDO-D2O solutions at different temperatures

Near infrared spectra of solution of 6.4 M HDO in D(2)O have been obtained at 15, 25, 30, and 35 degrees C. It was observed that the bands of HDO in D(2)O occur at 1416, 1525, 1556, and 1666 nm, which are in good agreement with the similar data reported earlier by Worley and Klotz. The calculations of enthalpy change for hydrogen bond formation (DeltaH degrees ) yielded the value of -2.5+/-0.4 kcal mol(-1), which is in excellent agreement with the value reported by Walrafen. Similar spectra were recorded for 1 and 2 m 18-crown-6 (18C6) dissolved in the solution of HDO in D(2)O at different temperatures. The band positions remain unchanged, however, the variation of intensity as a function of concentration of 18C6 and temperature clearly indicate that 18C6 acts as a structure making solute. The structural temperature and DeltaH degrees values have been obtained for the 18C6 solutions. These results are explained on the basis of the stabilization of 18C6 in the D(3d) conformation through hydrogen bonding of HDO molecules [doubly hydrogen bonded, i.e. bridging, and singly hydrogen bonded] to the oxygen atoms of 18C6 molecules. Slightly different DeltaH degrees values obtained can be attributed to clathrate like structure at 1 m 18C6 concentration while at 2 m 18C6 concentration it is postulated that the hydrophobic interactions are contributing additionally.