Partial molar volumes and compressibilities of 1-1 type chlorides, bromides, tetraphenylphosphonium chloride, and sodium tetraphenylborate in water-acetone mixtures

Abstract

The densities and adiabatic compressibilities have been measured at 288.15 K for solutions of NaCI, KCI, CsCI, NaBr, KBr, [Ph4P]CI, and Na[Ph4B] dissolved In water-acetone mixtures up to acetone content 50 wt %. The partial molar volume V 2 and partial molar adiabatic compressibilities Kt°h ave been calculated. Variation with composition of the solvent system was more remarkable for K°than for V2. in solvents containing more than 10 wt % of acetone, K,°o f [Ph4P]CI and Na[Ph4B] were positive, while all the other 1-1 type salts always had negative K°values. Ionic division of K,°o f an electrolyte based on the assumption /fs°([Ph4P]+) = fta0([Ph4B]~) seems unacceptable In this mixed solvent.

Apparent molar volumes, expansibilities, and isentropic compressibilities of selected electrolytes in methanol

“…The opposite trend may be found in water [23,25] and dimethylsulfoxide [26]. With increasing ionic radius the compressibility for alkali halides increases due to a decrease of the electrostriction and an increase of the size of the intermediate shell.…”

Hydration and Micellization Processes of n-Octyl β-d-Glucopyranoside in Aqueous Solution. A Thermodynamic and Fluorimetric Study in the Absence and Presence of Salts

“…Apparent Molar Properties. Thermodynamic properties are known to be useful parameters for analyzing the solvent−solvent, solute−solute, and solute−solvent interactions. , Particularly, higher order derivatives of Gibbs free energy, such as apparent molar volumes, V φ , and apparent molar isoentropic compressibilities, K s, φ , have been proven to be a powerful tool in ionic and nonionic solutions. − Both V φ and K s, φ can be calculated from density and isoentropic compressibility data, using where M is the molar mass of the solute, m is the molality of the solution, and d and κ s and d 0 and κ s,o are the densities and the isoentropic compressibilities of the solution and the solvent, respectively. From these values, apparent molar volumes and apparent molar isoentropic compressibilities at infinite dilution, and have usually been determined using an approach based on the Redlich−Rosenfeld equation,35b as follows: where S v and S κ s are the Debye−Hückel limiting slopes, available from the literature, for the apparent molar volume and the apparent molar isoentropic compressibility, respectively.…”

Static Relative Permittivities of Water + Acetone and Water + Dimethyl Sulfoxide under Pressures up to 300 MPa at 298.15 K

“…In this work, we report not only the liquid phase static relative permittivities of water + dimethyl sulfoxide over the entire mole-fraction range under pressures up to 300 MPa at 298.15 K but also the newly-determined static relative permittivities for water + acetone under the same conditions. In addition, we correlate r values with pressure P by use of the Tait-type equation and we evaluate (∂ ln r /∂P) T and r -2 (∂ r /∂P) T values at 0.1 MPa, which are important for analyzing the thermodynamic properties of electrolyte solutions; some limiting partial molar volumes of electrolytes in water + acetone mixtures (Kawaizumi et al, 1988) and in water + dimethyl sulfoxide mixtures (Garcia-Paneda et al, 1996) have been reported.…”