Why does an Aqueous Solution of Acid conduct electricity?

Answer. 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 an 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 aqueous acid solution conducts electricity as a result of this reaction.

HCl(aq) → H⁺(aq) + Cl⁻(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.

As is well known, the acid in its pure state will not carry electricity. 

When an acid and water are mixed, the hydrogen ion joins with a water molecule to generate the hydronium ion. 

This hydronium ion is responsible for electrical conduction in an acidic aqueous solution. 

As a result, acid conducts electricity.

The presence of hydrogen ions in an aqueous acid solution causes it to conduct electricity. 

Only in the presence of ions can electricity be conducted. Their heated nature is the cause behind this. 

Anions and cations are released as the acid dissociates into the aqueous solution. In acids, cations are hydrogen ions. As a result, these ions migrate in order to transmit charge and conduct electricity. 

Acids are chemicals that can contribute to or receive protons and electrons.