Solubility product of a salt of AB is `1 xx 10^(-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 keptA. between `10^(-8)M` to `10^(-7)M`B. between `10^(-7) M` to `10^(-6)M`C. `gt 10^(-5) M`D. `lt 10^(-8) M`

Solubility product of a salt of AB is `1 xx 10^(-8) M ^(2)` in a solut

1.	Solubility product of a salt of AB is `1 xx 10^(-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 keptA. between `10^(-8)M` to `10^(-7)M`B. between `10^(-7) M` to `10^(-6)M`C. `gt 10^(-5) M`D. `lt 10^(-8) M`
Answer» Correct Answer - C `K_(sp)[AB]=[A^(+)][B^(-)] =10^(-8)` Putting `[A^(+)]=10^(-3)M` we get `[B^(-)]10^(-5)M` AB will precipitate out if ionic produt is more than solubility product. Hence, for the precipitate `[B^(-)]gt 10^(-5)M`

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