At ` 25^(@)` C, the solubility product of `Hg_(2)CI_(2)` in water is `3.2xx10^(-17)mol^(3)dm^(-9)` what is the solubility of `Hg_(2)CI_(2)` in water at `25^(@)`C ?

Options

A. `1.2 xx 10^(-12)M `
B. `3.0 xx 10^(-6)` M
C. `2 xx 10^(-6)` M
D. `1.2 xx 10^(-16)` M

Answer

C

Explanation

Here `Hg_(2)Cl_(2) to Hg_(2)^(2+) +2Cl^(-)`
Let the concentration of `Hg_(2)^(2+)` be = x
Now , for each `Hg_(2)^(2+)` ion, two `Cl^(-)` ions are produced
` :. ` concentration of `Cl^(-)` ions = 2x
`K_(sp) = [Hg_(2)^(2+)][Cl^(-)]^(2)`
`x(2x)^(2)=3.2 xx10^(-17) rArr 4x^(3) = 32 xx10^(-18)`
`rArr x^(3) = 32/4 xx10^(-8)rArr x^(3) = 8 xx 10^(-18)`
` :. x = 2 xx 10^(-6) M ` .