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Question

Calculate the solubility of a sparingly soluble salt, BaSO4 in 0.01 M Na2SO4 solution ?
(Ksp for BaSO4=1.1×1010)

A
3.5×107mol L1
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B
2.9×105mol L1
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C
1.6×107mol L1
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D
1.1×108mol L1
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Solution

The correct option is D 1.1×108mol L1
BaSO4 is a sparingly soluble salt , whereas Na2SO4 is a highly soluble salt.
Let the solubility of BaSO4 be s. Then

BaSO4Ba2++SO24
t=teq cs s s

Sodium sulphate (Na2SO4) is a strong electrolyte and is completely ionised. It shall provide SO24 ion concentration= 0.01 M.

[Ba2+]=s
[SO24]=(s+0.01) M

Ksp=[Ba2+][SO24]=s×(s+0.01)

Since BaSO4 is a highly soluble .So s+0.010.01, because of the sparingly soluble salt (BaSO4) where Ksp<<103
Given Ksp=1.1×1010
1.1×1010=0.01×s
or
s=1.1×10100.01=1.1×108 mol L1

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