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) rarr 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 xx 10^(-17) rArr 4x^(3) = 32 xx 10^(-18)`
`rArr x^(3) = (32)/(4) xx 10^(-18) :. x = 2 xx 10^(-6) M`