Solubility product of a salt AB is `1xx10^(-8)M^(2)` in a solution in which the concentration of `A^(+)` ions is `10^(-3)M`. The salt will precipitate when the concentration of `B^(-)` ions is kept

Options

A. `10^(-4)M`
B. `10^(-7)M`
C. `10^(-6)M`
D. `10^(-5)M`

Answer

D

Explanation

`[A^(+)][B^(-)]=K[AB]=K_(sp)`
`[10^(-3)][B^(-)]=10^(-8)`
Hence, the salt will precipitate when the conc. Of B becomes more than `10^(-5)` M.