# How to compare electrical conductivity of ionic liquids and aqueous electrolytes

I am trying to compare the electrical conductivity of selected ionic liquids (ILs) and aqueous electrolytes.

By ionic liquid (IL), I mean a pure IL -- no water. Electrical conductivity of ILs is measured in units of Siemens per length. For example, the following table from Leys et al., J. Chem. Phys., 2008 gives the electrical conductivity of selected ILs in units of S/m:

On the other hand, aqueous electrolytes are obviously salts in water. I think, then, electrical conductivity of aqueous electrolytes are concentration-dependent. The following table in the CRC Handbook gives the electrical conductivity of selected aqueous electrolytes in units of S cm^2 / mol:

How can I compare the electrical conductivities of ionic liquids and aqueous electrolytes?

In other words, is there a way to relate ionic ($$\sigma$$ in S/m) and molar ($$\Lambda$$ in S cm^2 / mol) conductivities?

• No, it is an apple to orange comparison. They are changing the frequencies and in the molar conductivity measurements you do not know what was the current frequency. Dec 23 '20 at 19:48
• What do you want to learn from this comparison?
– Karl
Dec 23 '20 at 21:06
• @Karl I hope to show that electrical conductivities of aqueous electrolytes are higher than those of ionic liquids (or vice versa). Dec 23 '20 at 21:12
• Yes, aqueous electrolytes must be better because acids and bases have the highest molar conductivity known. IL are bulky, viscous, I don't think they are great conductors. Dec 23 '20 at 22:29
• @M.Farooq How do you think I could quantify that, from results available in the literature? Dec 24 '20 at 2:32