Ion−Solvent Interactions of Some Halides of Common Cations with Organic Solvent Mixtures by Conductometric, Volumetric, Viscometric, and Refractometric Techniques

Abstract

Electrolytic conductivities, densities, viscosities, and refractive indices of some lithium halides (LiCl, LiBr, and LiI) have been studied in mass fraction (0.10, 0.20, and 0.30) of ethylene glycol monomethyl ether + methyl alcohol mixtures at 303.15 K. The limiting molar conductivities (Λ 0 ), association constants (K A ), and the distance of closest approach of the ion (R) have been evaluated using the Fuoss conductance equation (1978). The Walden product is obtained and discussed. The limiting apparent molar volumes (φ V °), experimental slopes (S V * ) derived from the Masson equation, and viscosity A and B coefficients using the Jones-Dole equation have been interpreted in terms of ion-ion and ion-solvent interactions, respectively.

Conductance, a Contrivance To Explore Ion Association and Solvation Behavior of an Ionic Liquid (Tetrabutylphosphonium Tetrafluoroborate) in Acetonitrile, Tetrahydrofuran, 1,3-Dioxolane, and Their Binaries

“…All the binary solvent mixtures were prepared by mixing the required volume of ACN, THF, and 1,3-DO using the appropriate conversion of the required mass of each solvent into volume at 298.15 K using experimental densities. 28 For the preparation of the solvent mixtures, the required weighed amount of solvent was transferred to a volumetric flask and the flask was filled up to the mark. The stock solutions of the salt in binary solvent mixtures were prepared by mass (Mettler Toledo AG-285 with uncertainty ±0.0003 g).…”

“…The uncertainty in density was estimated to be ±0.000 01 g cm −3 , and the viscosity was measured by means of a suspended Ubbelohde type viscometer, calibrated at 298.15 ± 0.01 K with doubly distilled water and purified methanol using density and viscosity values from the literature, and the efflux time of flow was recorded with a digital stopwatch correct to ±0.01 s. The uncertainty of the viscosity measurements was ±0.003 mPa s. The details of the methods and experimental techniques have been described elsewhere. 28,30 The conductance measurements were carried out in a Systronics-308 conductivity bridge of accuracy ±0.01%, using a dip-type immersion conductivity cell, CD-10, having a cell constant of approximately 0.1 ± 0.001 cm −1 . Measurements were made in a thermostate water bath maintained at T = 298.15 ± 0.01 K. The cell was calibrated by the method proposed by Lind et al, 31 and the cell constant was measured based on 0.01 M aqueous KCl solution.…”

“…The densities of the solvents and solutions were measured with vibrating-tube density meter (Anton Paar, DMA 4500M), maintained at ±0.01 K of the desired temperature and calibrated at the experimental temperature with doubly distilled water and dry air. The uncertainty in density was estimated to be ±0.000 01 g cm –3 , and the viscosity was measured by means of a suspended Ubbelohde type viscometer, calibrated at 298.15 ± 0.01 K with doubly distilled water and purified methanol using density and viscosity values from the literature, and the efflux time of flow was recorded with a digital stopwatch correct to ±0.01 s. The uncertainty of the viscosity measurements was ±0.003 mPa s. The details of the methods and experimental techniques have been described elsewhere. , …”