ChemistryMedium73×since 2002Q1348For a sparingly soluble salt AB2\mathrm{AB}_2AB2, the equilibrium concentrations of A2+\mathrm{A}^{2+}A2+ ions and B−B^{-}B− ions are 1.2×10−4M1.2 \times 10^{-4} \mathrm{M}1.2×10−4M and 0.24×10−3M0.24 \times 10^{-3} \mathrm{M}0.24×10−3M, respectively. The solubility product of AB2\mathrm{AB}_2AB2 is :A0.069×10−120.069 \times 10^{-12}0.069×10−12B0.276×10−120.276 \times 10^{-12}0.276×10−12C6.91×10−126.91 \times 10^{-12}6.91×10−12D27.65×10−1227.65 \times 10^{-12}27.65×10−12Check answerSkip