Partial molar volume of some monovalent salts and polar molecules in organic solvents

Abstract

The partial molar volumes of a number of monovalent salts and polar species were measured In a series of organic solvents. The solvents Included ethanol, methanol, Af-methylformamlde (NMF), propylene carbonate, sulfolane, acetonitrile, acetone, and 4-methyl-2-pentanone. The polar species were n -propyl bromide, n-propyl iodide, and n-propyl chloride. The monovalent salts that were examined Included LIBr, Lll, LIN03, Nal, KI, Rbl, CsBr, tetrabutylammonlum Iodide, tetrabutylammonlum bromide, and tetrabutylammonlum perchlorate. The major observation was that the solvent effect on the partial molar volumes was most pronounced for monovalent salts. The solvent effect on the partial molar volume of the neutral solute was very small. The largest solvent effects are seen for the small monovalent salts when comparing aprotlc and protlc solvents. The conclusion was that the nonlonlc solutes do not grossly change the structure of the solvent, but the Ionic solutes change the structure of the solvent significantly.

Density and speed of sound of lithium bromide with organic solvents: Measurement and correlation

“…Our V 0 / value for methanol is in agreement with the value reported by Pasztor and Criss [14] and the selected value, 3.1 AE 10 À6 m 3 AE mol À1 , given by Marcus and Hefter [16] in the recent review on the partial molar volume of electrolytes in non-aqueous solvents. Similarly, for LiBr in ethanol solutions, the values of À4.1 AE 10 À6 m 3 AE mol À1 [16], and À6.2 AE 10 À6 m 3 AE mol À1 [15] have been reported. Since for LiBr in ethanol, the V 0 / values have been independently confirmed to a sufficient level of precision, the value of À5.2 AE 10 À6 m 3 AE mol À1 has been recommended by Marcus and Hefter [16].…”

“…The pressure dependence of density values for many solvents, in the form of the Tait equation, has been reported [29][30][31][32][33][34][35][36] which enables us to obtain j T values for the investigated solvents using the relation j T = (o ln d/oP) T . Therefore, using the calculated j T values, along with the equations (6) and (7) [14], and 0.8 AE 10 À6 m 3 AE mol À1 [15], have been obtained by different research groups. Our V 0 / value for methanol is in agreement with the value reported by Pasztor and Criss [14] and the selected value, 3.1 AE 10 À6 m 3 AE mol À1 , given by Marcus and Hefter [16] in the recent review on the partial molar volume of electrolytes in non-aqueous solvents.…”

“…Vapour pressure data are also available for solutions of LiBr in acetone [10], acetonitrile [11] at T = 298.15 K. Also for solutions of LiBr in N,N-dimethylacetamide, vapour pressure data have been reported [12] at T = (323.15 to 423.15) K. However, a little information is available on the volumetric and ultrasonic properties of LiBr in nonaqueous solvents. Volumetric data are available for LiBr in methanol [13][14][15] and ethanol [15,16]. However, the apparent volumes at infinite dilution reported by various authors are different.…”

“…However, the apparent volumes at infinite dilution reported by various authors are different. While there are very few density data for solutions of LiBr in acetone [15], acetonitrile [17][18][19][20], and N,N-dimethylacetamide [21] in the literature, no density data are available for solutions of LiBr in 2-propanol. Ultrasonic data for these non-aqueous systems are scarce.…”

Thermodynamic Properties of Nonaqueous Single Salt Solutions Using the Q-Electrolattice Equation of State

“…(Gmehling, 2012), (C) osmotic coefficient at 298.15 K (○) (Gmehling, 2012), and (D) liquid density at 298.15 K (○) (Pasztor and Criss, 1978). (Takenaka et al, 1994a); b (Glugla et al, 1982); c (Barthel et al, 1998); d (Takenaka et al, 1994b); e (Wawer et al, 2008); f (Takenaka et al, 1994c) (Glugla et al, 1982) …”