Ionic EquilibriumHard
Question
How many times the solubility of CaF2 is decreased in 4 × 10−3 M-KF(aq) solution as compared to pure water at 25o C. Given: Ksp (CaF2) = 3.2 × 10−11
Options
A.50
B.100
C.500
D.1000
Solution
$CaF_{2}(s) \rightleftharpoons \underset{S_{1}M}{Ca^{2 +}} + \underset{2S_{1}\text{ M}}{2F^{-}}$
Now, $K_{sp} = S_{1}.\left( 2S_{1} \right)^{2} \Rightarrow S_{1} = \left( \frac{K_{sp}}{4} \right)^{1/3} = \left( \frac{3.2 \times 10^{- 11}}{4} \right)^{1/3} = 2 \times 10^{- 4}\text{ M}$
Now, in KF solution,
$S_{2} = \frac{K_{sp}}{\left\lbrack F^{-} \right\rbrack^{2}} = \frac{3.2 \times 10^{- 11}}{\left( 4 \times 10^{- 3} \right)^{2}} = 2 \times 10^{- 6}M$
Now, $\frac{S_{2}}{S_{1}} = \frac{2 \times 10^{- 6}}{2 \times 10^{- 4}} = \frac{1}{100}$
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