Introduction and Solvent Properties

Ion-pair and triple-ion formation of some tetraalkylammonium iodides in n-hexanol and its binary mixtures with o-toluidine

“…Finally, the corresponding K 0 and K A values are obtained which are reported in table 3 along with R and d for the binary mixtures of the salts. DG is given by the relationship [25] and given in table I (supplementary material), This fact is in line with the decrease of the viscosity for the solvent mixtures with increasing content of o-toluidine suggests concomitant increase in limiting molar conductance for the electrolytes [14,26] which is opposite to the results obtained in our recently published paper where the limiting molar conductance of the tetraalkyammonium salts decreases with the decrease in the viscosity of the solvent mixture [27].…”

“…Thus, extensive studies on electrical conductances in various mixed organic solvents have been performed in recent years [9][10][11][12][13] to examine the nature and magnitude of ion-ion and ion-solvent interactions. Tetraalkylammonium salts are frequently selected as desired electrolytes in conductance studies, even though they show little or no solvation in solution due to their low surface charge density [14,15]. In continuation of our investigation on electrical conductance [8,10,11], the present work deals with the conductance measurements of some tetraalkylammonium iodides, R 4 NI (R = butyl to heptyl), in binary mixtures of o-toluidine in n-hexanol at T = 298.15 K.…”

Viscous synergy and antagonism and isentropic compressibility of ternary mixtures containing 1,3-dioxolane, water and monoalkanols at 303.15K

“…The solvents finally obtained after purification was 99.9% pure. The purity of the liquids was checked by measuring their densities and viscosities at 303.15 K which was quite in agreement with the literature values [39][40][41][42].…”

Characteristics of the electroosmotic flow of electrolyte systems for nonaqueous capillary electrophoresis

“…In dipolar-aprotic solvents, dipoledipole forces exist that are weaker than hydrogen bonding. Amphiprotic solvents can be distinguished from dipolar-aprotic solvents by the value of their pK auto , which for amphiprotic solvents must be less than 20 [16,17].…”