# Can solutions of polar covalent compounds conduct electricity?

I learned in class that solutions of polar covalent compounds are weakly conductive, while ionic solutions are strongly conductive.

But I'm getting different answers online. According to this lecture, "They do not conduct electricity in the liquid state, or when soluble in water, do not conduct electricity in aqueous solution."

I saw in lab, however, that a dextrose (D-glucose) solution weakly conducted electricity, and so did that of levulose (D-fructose).

So can solutions of polar covalent compounds conduct electricity? If so, how? Since it's covalent, it's not like anything can dissociate to form ions, right?

• Could someone answer the question or leave a comment instead of just downvoting? Thanks. I'm just a high school chem student wanting to learn – user3932000 Dec 30 '16 at 18:07
• Did you check the conductivity of the pure solvent? – user7951 Dec 30 '16 at 18:34
• @Loong In my data, I checked the conductivity of a tin "solution" (just a piece of tin metal in distilled water) and it was zero as expected. – user3932000 Dec 30 '16 at 20:25
• @Loong Speaking of data, I recall that the pH was unusually low for all the solutions—5.0. I dismissed this as the pH strips being old and inaccurate, but it could be that CO2 dissolved in the water and made it weakly conductive. – user3932000 Dec 30 '16 at 20:50
• The conductivity of highly purified water at a temperature of $T=25\ \mathrm{^\circ C}$ is $\kappa=5.50\times10^{-6}\ \mathrm{S\ m^{-1}}$. The conductivity of water that is saturated with atmospheric $\ce{CO2}$ is increased to $\kappa=1.10\times10^{-4}\ \mathrm{S\ m^{-1}}$. Pure water in contact with air can reach a pH of about 5.8 due to dissolved atmospheric $\ce{CO2}$. – user7951 Dec 30 '16 at 21:13