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On adding 0.1 M solution each of Ag^(+),...

On adding 0.1 M solution each of `Ag^(+),Ba^(2+), Ca^(2+)` ions in a `Na_(2)SO_(4)` solution, species first precipitated is `(K_(sp)BaSO_(4)=10^(-11),K_(sp)CaSO_(4)=10^(-6),K_(sp) Ag_(2)SO_(4)=10^(-5))`

A

`Ag_(2)SO_(4)`

B

`BaSO_(4)`

C

`CaSO_(4)`

D

All of these

Text Solution

Verified by Experts

The correct Answer is:
B
Solubility of `BaSO_(4) (x) = sqrt(K_(sp)) = sqrt(10^(-11))`
= `3.16 xx10^(-6) ` mol/L
Solubility of `CaSO_(4) (x) = sqrt(K_(sp)) = sqrt(10^(-6))`
`= 1.0 xx 10^(-3) ` mol/L
Solubility of `Ag_(2)SO_(4) = root3 ((K_(sp))/4)`
`( :. " for " Ag_(2)SO_(4),4x^(3)K_(sp)) =root 3(10^(-5)/4) = 1 xx 10^(-2) `
Least solubility is of `BaSO_(4)` , hence it will precipitate first .
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