Both ionicity and diffusivity determine the ionic conductivity of solutions. Viscosity is known to affect the diffusivity and hence mobility of ions. Previous research on RTIL and solvent system used low-viscosity solvents to mix ILs, making it challenging to analyze the hydrogen bonding on the transport behavior due to the high viscosity of the IL. However, recent studies have examined IL mixtures with slightly more viscous molecular solvents (e.g., ethylene glycol (EG) with a viscosity of 16.8 cP) to understand hydrogen bonding effects better. Studies are available for a mixture of ILs and EG report viscosity and density. The study of viscosity and density of 1-butyl-3-methylimidazolium tetrafluoroborate [BMIM][BF4] and 1-ethyl-3-methylimidazolium tetrafluoroborate [EMIM][BF4] in EG was performed, and negative deviation in viscosity measurement was observed in both the studies. Pal et al. studied the behavior of mixing of aprotic and protic ILs in EG with the help of Fourier transform infrared spectroscopy (FT-IR). They observed that the interaction of hydrogen bonding was not imitated at the molecular level in the macroscopic behavior of the mixing. The hydrogen bonding and ion dissociation in a mixture of [BMIM][BF4] and EG was studied with the estimation of the viscosity of the solution, and it was observed that dilute ionic liquid solutions show isolated ion pairs surrounded by solvent. Cation-anion pair size increases nonlinearly with concentration, leaving isolated solvent monomers in concentrated IL solutions. However, studies for the conductivity analysis of the mixture of ILs and EG are very scarce. Recently, Nordness et al. The conductivities of all three mixtures attained a maximum at a particular composition and then decreased. They reported that this phenomenon was responsible due to the competition between free-ion concentration and viscous forces hindering ion diffusion. The available studies only qualitatively highlight the ion dissociation phenomena for the limited number of IL/solvent systems. There is still a need for a comprehensive theory that enables a better understanding of how ion dissociation varies with the size/type of anions and cations, as well as their concentrations in a range of solvents.