Chapter 15, Problem 15RQ

Interpretation Introduction

Interpretation:

The reason behind non-conductance of electric current when aqueous ${\text{CH}}_3\text{OH}$ solution is taken but conductance when solution of sodium hydroxide is taken has to be explained.

Concept Introduction:

An electrolyte refers to an ionic compound that on solvation in polar protic solvents ionizes to yield cationic and anionic species. The free movement of such ionic species results in the conduction of electricity. For example, when $\text{HCl}$ is taken in hexane, the $\text{HCl}$ cannot into ${\text{H}}^{+}$ and ${\text{Cl}}^{-}$. This is since hence is non-polar solvent and therefore no inter ionic attraction exists between $\text{HCl}$ and hexane. Thus in absence of ${\text{H}}^{+}$ and ${\text{Cl}}^{-}$ current does not flow.

On the other hand, $\text{HCl}$ easily dissolves in water because of polar nature of water. Thus on dissolution in water $\text{HCl}$ dissociates into ${\text{H}}^{+}$ and ${\text{Cl}}^{-}$ that can move freely in aqueous form and hence conducts electricity.