The solubility of Ca-F-2- is 2 times -10- - 4- mole-litre- Its solubility product is-2-0 times -10- - 4-4-0 times -10- - 8-8-0 times 8-0 times -10- - 12-3-2 times -10- - 11-

Question

Toppr Admin · Accepted Answer

We haveCaF2-x2192-Ca2-2F-x2212-Kw - 4S3Kw-4-x2217-2-x2217-10-x2212-4-3Kw- 4-xD7-8-xD7-10-x2212-12

The solubility of $C a F_{2}$ is $2 \times 10^{- 4}$ mole/litre. Its solubility product is:

$2.0 \times 10^{- 4}$
$4.0 \times 10^{- 8}$
$8.0 \times 8.0 \times 10^{- 12}$
$3.2 \times 10^{- 11}$

We have
$C a F_{2} \to C a^{2 +} + 2 F^{-}$
$K_{w}$ = $4 S^{3}$
$K_{w} = 4 * (2 * 10^{- 4})^{3}$
$K_{w}$ = $4 \times 8 \times 10^{- 12}$

The solubility of CaF2 is 2×10−4 mole/litre. Its solubility product is:2.0×10−44.0×10−88.0×8.0×10−123.2×10−11

We haveCaF2→Ca2++2F−Kw = 4S3Kw=4∗(2∗10−4)3Kw= 4×8×10−12

The solubility of $C a F_{2}$ is $2 \times 10^{- 4}$ mole/litre. Its solubility product is:

$2.0 \times 10^{- 4}$
$4.0 \times 10^{- 8}$
$8.0 \times 8.0 \times 10^{- 12}$
$3.2 \times 10^{- 11}$

We have
$C a F_{2} \to C a^{2 +} + 2 F^{-}$
$K_{w}$ = $4 S^{3}$
$K_{w} = 4 * (2 * 10^{- 4})^{3}$
$K_{w}$ = $4 \times 8 \times 10^{- 12}$