The concentration of `Ca^(2+)` ions in a saturated `CaF_2` solution is 8.4`mg*L^(-1)` at `25^(@)`C. Calculate the solubility product of `CaF_2` at that temperature.

Explanation

`[Ca^(2+)]=(8.4xx10^(-3))/(40)mol*L^(-1)`
`[F^-]=2xx(8.4xx10^(-3))/(40)mol*L^(-1)`
`CaF_2(s) `K_(sp)=[Ca^(2+)][F^-]^2=(8.4xx10^(-3))/(40)xx((2xx8.4xx10^(-3))/(40))^2`
`=3.7xx10^(-11)`