The solubility product of a salt having general formula `MX_(2)` in water is `4xx10^(-12)`. The concentration of `M^(2+) ions` in the aqueous solution of the salt is:

Options

A. `4.0x10^(-10)M`
B. `1.6xx10^(-4)M`
C. `1.0xx10^(-4)M`
D. `2.0xx10^(-6)M`

Answer

C

Explanation

`MX_(2)hArr M^(2+)+underset(2s)(2X)`
`K_(sp)=[M^(2-)][X^(-)]^(2)`
If solubility be s then
`K_(sp)=(s)(2s)^(2)=4s^(3)`
`4s^(3)=4xx10^(-12)`
`therefores=1xx10^(-4)M`
`thereforeM^(2-)=s=1xx10^(-4)M`