Identify the acids in the following reaction: $HCl_{(aq)} + H_2O_{(aq)} \rightleftharpoons H_3O^{+}_{(aq)} + Cl^{-}_{(aq)}$. Which of these acids is stronger?

(A) In the given reaction,$HCl$ acts as a Bronsted-Lowry acid by donating a proton to $H_2O$. The resulting $H_3O^{+}$ ion acts as the conjugate acid of $H_2O$. Between $HCl$ and $H_3O^{+}$,$HCl$ is a strong acid because it undergoes complete dissociation in aqueous solution.