Chapter 15, Problem 21RQ

Interpretation Introduction

Interpretation:

The reason behind insolubility of $\text{HCl}$ in hexane but solubility in water 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.

Three subcategories exist for electrolyte namely strong electrolyte, weak electrolyte and non-electrolyte. The strong electrolytes on dissolution exhibit $100\text{ \%}$ dissociation; The acids such as $\text{HCl}$ , ${\text{CH}}_{\text{3}}\text{COOH}$, ${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}$, ${\text{HNO}}_3$ that has ability to furnish hydronium ions and bases such as $\text{NaOH}$, $\text{KOH}$ ionize fully to yield hydroxide ions are strong electrolytes.

 In contrast, the weak electrolytes are not $100\text{ \%}$ dissociated, theses may include weak acids and bases such as carbonic acid, nitrous acid, boric acid, $\text{HClO}$, ${\text{NH}}_3$.

The principle of “like dissolves like” holds true and suggests that ionic or polar substances are more soluble in similar polar solvent such as water.