The solubility of CaF2 is 2×10-4 mole/litre. Its solubility product is

CaF2⇌Ca+2s+2F-2sKsp=(s)(2s)2=4s3s=2×10−4Ksp=42×10−43=4×8×10−12

The solubility of CaF2 is 2×10-4 mole/litre. Its solubility product is

CaF2⇌Ca+2s+2F-2sKsp=(s)(2s)2=4s3s=2×10−4Ksp=42×10−43=4×8×10−12

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The solubility of ${CaF}_{2}$ is $2 \times 10^{- 4}$ mole/litre. Its solubility product is

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$2.0 \times 10^{- 4}$

$4.0 \times 10^{- 8}$

$4 \times 8.0 \times 10^{- 12}$

$3.2 \times 10^{- 4}$

answer is C.

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Detailed Solution

${CaF}_{2} ⇌ \underset{s}{{Ca}^{+ 2}} + \underset{2 s}{2 F^{-}}$
$K_{sp} = (s) {(2 s)}^{2} = 4 s^{3}$

$s = 2 \times 10^{- 4}$

$K_{sp} = 4 {[2 \times 10^{- 4}]}^{3}$

$= 4 \times 8 \times 10^{- 12}$

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The solubility of CaF2 is 2×10-4 mole/litre. Its solubility product is

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The solubility of ${CaF}_{2}$ is $2 \times 10^{- 4}$ mole/litre. Its solubility product is