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6-2.Equilibrium-II (Ionic Equilibrium)
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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 :
A
$0.069 \times 10^{-12}$
B
$6.91 \times 10^{-12}$
C
$0.276 \times 10^{-12}$
D
$27.65 \times 10^{-12}$
(JEE MAIN-2024)
Solution
$ \mathrm{AB}_{2(\mathrm{~s})} \rightleftharpoons \mathrm{A}_{(\mathrm{aq})}^{+2}+2 \mathrm{~B}_{(\mathrm{aq})}^{-} $
$ \mathrm{K}_{\mathrm{sp}}=\left[\mathrm{A}^{+2}\right]\left[\mathrm{B}^{-}\right]^2 $
$=1.2 \times 10^{-4} \times\left(2.4 \times 10^{-4}\right)^2 $
$=6.91 \times 10^{-12} \mathrm{M}^3$
Standard 11
Chemistry
