Why does an aqueous solution of an acid conduct electricity?

An aqueous solution of an acid conducts electricity because the acid dissociates into ions when it is dissolved in water. This dissociation produces positively charged hydrogen ions (H+) and negatively charged ions, such as chloride ions (Cl-) in the case of hydrochloric acid (HCl) or nitrate ions (NO3-) in the case of nitric acid (HNO3).

These ions are free to move in the solution and are capable of carrying an electric charge, making the solution electrically conductive. The more ions that are present in the solution, the greater the conductivity. Strong acids, such as hydrochloric acid and sulfuric acid, dissociate almost completely into ions when dissolved in water, making their solutions highly conductive.

The ability of an acid solution to conduct electricity is directly related to the concentration of hydrogen ions in the solution. Acids with higher concentrations of hydrogen ions produce solutions that are more conductive. Conversely, weak acids, which dissociate only partially into ions, produce solutions with lower concentrations of ions and lower conductivity.