In 1 L saturated solution of AgCl [Ksp (AgCl) = 1.6 × 10–10], 0.1 mol of CuCl [Ksp (CuCl) = 1.0 × 10–6] is added. The resultant concentration of Ag+ in the solution is 1.6 × 10

Engineering

Chemistry

Solubility Equilibria

Question

In 1 L saturated solution of AgCl [K_sp (AgCl) = 1.6 × 10^–10], 0.1 mol of CuCl

[K_sp (CuCl) = 1.0 × 10^–6] is added. The resultant concentration of Ag⁺ in the solution is 1.6 × 10^–x. The value of “x” is :

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$[{Ag}^{+}] = \frac{K_{1}}{\sqrt{K_{1} + K_{2}}} ∵ K_{1} < < K_{2} ∴ K_{1} + K_{2} ≅ K_{2}$

$∴ [{Ag}^{+}] = \frac{1 .6 \times 10^{- 10}}{\sqrt{1 .0 + 10^{- 6}}} = 1 .6 \times 10^{- 7}$

x = 7