A volumetric and viscosity study for the mixtures of 1-n-butyl-3-methylimidazolium tetrafluoroborate ionic liquid with acetonitrile, dichloromethane, 2-butanone and N, N ? dimethylformamide

Abstract

The densities and viscosities for mixtures of 1-n-butyl-3-methylimidazolium tetrafluoroborate ionic liquid with acetonitrile, dichloromethane, 2-butanone and N,N-dimethylformamide have been determined at 298.15 K. From these measurements, it was found that viscosities of the mixtures can generally be described by an exponential equation. Their densities are linear functions of the mass fraction of the ionic liquid in the mixtures. These physical properties can be predicted as a function of the concentration of ionic liquid provided that the properties for pure components are known. The excess molar volume V E m and the excess logarithm viscosities (ln h) E were calculated and fitted to the Redlich-Kister polynomials. It is shown that the values of V E m are negative but those of (ln h) E are positive. Surprisingly, the minimum in V E m and the maximum in (ln h) E are observed at about the same mole fraction of the ionic liquid, x ≈ 0.3. The results are discussed in terms of the ion-dipole interactions between the cations of the ionic liquid and the organic solutes.

Viscosities of the Mixtures of 1-Ethyl-3-Methylimidazolium Chloride with Water, Acetonitrile and Glucose: A Molecular Dynamics Simulation and Experimental Study

“…Nevertheless, an exponential dependence of the viscosity of a solution of an IL with a low viscosity cosolvent has been observed previously. 54,55 For example, Wang et al 55 have reported measurements of the viscosity of mixtures of 1-n-butyl-3-methylimidazolium tetrafluoroborate ([bmim][BF4]) with four small organic molecules including acetonitrile. It was found that all four cosolvents lowered the viscosity of the IL-co-solvent solution and followed a seemingly universal exponential relationship, η mix ) η 1 exp(-x 2 /a), in which a ) 0.216.…”

Transport properties of protic ionic liquids, pure and in aqueous solutions: Effects of the anion and cation structure

“…8 and 9 that for given (PIL + water) solutions, the molar conductivity of the PIL increases with x w . This observation is easy to understand by considering that the viscosity of the water is much lower than that of the PILs (see Table 2), the addition of water into a PIL can reduce, then, its viscosity significantly [35,36]. Therefore, the mobility of ions or charge carriers is enhanced when the concentration is increased due to the viscosity reduction and finally, the solution becomes more conductive.…”

Excess molar volumes and viscosity behaviour of binary mixtures of aniline/or N,N-dimethylaniline with imidazolium ionic liquids having triflate or bistriflamide anion

“…On the other hand, ionic liquids reveal very interesting fundamental features: i) they have specific structure represented by polar (ionic) and non-polar (aliphatic) domains [4], which is crucial for the aforementioned diverse solvent power and ii) they allow a variety of interactions in their mixtures: dispersion forces between aliphatic chains present in the mixtures of imidazolium ionic liquids with alcohols [15]; strong interactions such as ionic (Coulomb forces [16] and ion-dipole interactions [17]), hydrogen bonds [15,[18][19][20], and specific interactions with the aromatic compounds [21][22][23].…”