In the liquid state, pure acids are terrible conductors of electricity. The presence of ions in aqueous solutions of acids is demonstrated by the fact that they conduct electricity. In aqueous solution, acids dissociate to create H+ ions.

H+ ions reach the cathode when electricity is transmitted through an aqueous solution of an acid, and each H+ ion picks up one electron from the cathode to generate H2 gas. An acid aqueous solution conducts electricity as a result of this reaction.

H+(aq) + Cl– HCl(aq) (aq)

In an aqueous solution with water as the solvent, the solute to be dissolved by the solvent contains fewer particles, causing the particles to move randomly. Simply said, the aqueous solution of acid conducts electricity due to the presence of ions.