Which among the following anions represents the strongest Bronsted base in aqueous solution? — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

According to the Bronsted-Lowry concept, the stronger an acid, the weaker its conjugate base. The acidic strength of oxyacids of chlorine increases with the oxidation state of Cl: $HClO < HClO_2 < HClO_3 < HClO_4$. Therefore, $HClO$ is the weakest acid, making its conjugate base, $ClO^-$, the strongest base.