First slide

Solubility product(KSP)

Question

To 100ml of 0.1 M AgNO₃ solution, solid K₂SO₄ is added. The concentration of K₂SO₄ that shows the precipitation is (K_sp for Ag₂SO₄ = 6.4 × 10^–5m³/l³)

Easy

A

0.1 M
B

$\large 6.4\, \times {10^{ - 3}}M$
C

$6.4\, \times {10^{ - 7}}M$
D

$6.4\, \times {10^{ - 5}}M$

Solution

For precipitation to occur, K_IP $\geq$ K_sp
OR [Ag⁺]² [SO₄^-2] = 6.4 $\times$ 10^-5
[S $O_{4}^{- 2}$ ] = $\frac{6.4 \times 10^{- 5}}{{[0.1]}^{2}} = 6.4 \times 10^{- 3}$

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