On adding 0.1 , M solution each of [Ag^+], [Ba^ 2+ ], [Ca^ 2+ ] i…

MCQ

On adding $0.1\, M$ solution each of $[Ag^+], [Ba^{2+}], [Ca^{2+}]$ in a $Na_2SO_4$ solution, species first precipitated is $[K_{sp}\, BaSO_4 = 10^{-11}, K_{sp}\, CaSO_4 = 10^{-6}, K_{sp}\,Ag_2SO_4 = 10^{-5}]$

A
$Ag_2SO_4$
✓
$BaSO_4$
C
$CaSO_4$
D
All of these

✓

Answer

Correct option: B.

$BaSO_4$

b
The species having minimum value of $K_{sp}$ will get precipitated first of all because ionic product will exceed the solubility product of such a species. The $K_{sp}$ value is minimum for $BaSO_4(10^{-11})$, so, $BaSO_4$ will get precipitated first of all.

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