Chemical reaction of PO₄³⁻ ion in water: PO₄³⁻(aq) + H₂O(l) → HPO₄²⁻(aq) +OH⁻(aq). Kb = [HPO₄²⁻] · [OH⁻] / [PO₄³⁻]; <span>base ionization constant. </span>Base ionization constant <span>is the equilibrium </span>constant<span> for the </span>ionization<span> of a </span>base<span>. </span>According
to Bronsted-Lowry theory acid are donor of protons and bases are
acceptors of protons (the hydrogen cation or H⁺<span>). </span>PO₄³⁻ is Bronsted base and it can accept proton and
become conjugate acid HPO₄²⁻.
