The present paper investigations made on the ion-solvation interaction of new class of salts ionic liquids (IL) such as 1-Ethyle-3-methylimidazolium Tetrafluoroborate and 1-Butyl-3-methylimidazolium Tetrafluoroborate in N,N-Dimethylformamide and Acetonitrile at temperature range of 283.15 to 318.15K with the aid of using electrical conductivity precept. The electrical conductance data were analyzed with the aid of Fuoss – Justice equation of conductivity. The molar conductance (Λ), the limiting molar conductance (Λ0), the association constants (KA), the Walden product (Λ0 η0), The Eyring activation energy of charge transport (ΔH‡λ) and the standard thermodynamic parameters of association (〖∆G〗_A^o, 〖∆H〗_A^oand 〖∆S〗_A^o) were calculated and mentioned. The results show that, the molar conductance and the limiting molar conductance values have been diminished as the relative permittivity of the solvent lowered at the same time, the association constant increased. Additionally, the outcome exhibit that the values of the molar conductance, and the limiting molar conductance were increased as the temperature increased at the same time, the association constant increased indicating that the association process is an endothermic one as indicated from 〖∆H〗_A^o value. The effect of the alkyl chain length of IL is clear on the thermodynamic parameters and association properties.