When an electrolyte is placed in an aqueous solution, it partially or completely dissociates into its constituent ions, which become free to move throughout the solution. This phenomenon is known as electrolytic dissociation. The dissolved ions can then interact with water molecules, forming hydrated ions. The presence of these mobile ions in the solution enables it to conduct electricity.

Examples of electrolytes include salts (such as sodium chloride, NaCl), acids (such as hydrochloric acid, HCl), and bases (such as sodium hydroxide, NaOH). When these electrolytes are dissolved in water, they break apart into their respective ions:

- Sodium chloride (NaCl) dissociates into sodium (Na+) and chloride (Cl-) ions.

- Hydrochloric acid (HCl) dissociates into hydrogen (H+) and chloride (Cl-) ions.

- Sodium hydroxide (NaOH) dissociates into sodium (Na+) and hydroxide (OH-) ions.

The resulting solutions contain a mixture of free ions and water molecules. The concentration of these ions in the solution determines its conductivity. The higher the concentration of ions, the better the solution's ability to conduct electricity.

Electrolytes play a crucial role in various biological processes, such as muscle contraction, nerve impulse transmission, and fluid balance. They also have practical applications in batteries, electroplating, and various industrial processes involving electrochemical reactions.