For a sparingly soluble salt \( \mathrm{AB_2} \), the equilibrium concentrations of \( \mathrm{A^{2+}} \) ions and \( \mathrm{B^-} \) ions are \( 1.2 \times 10^{-4} \, \mathrm{M} \) and \( 0.24 \times 10^{-3} \, \mathrm{M} \), respectively. The solubility product of \( \mathrm{AB_2} \) is:
