In qualitative analysis, the metals of group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains Ag+ and pb2+ at a concentration of 0.10 M. Aqueous HCl is added to this solution until the Cl$-$ concentration is 0.10 M. What will the concentrations of Ag+ and Pb2+ be at equilibrium ? (Ksp for AgCl = 1.8 $ \times $ 10$-$10, Ksp for PbCl2 = 1.7 $ \times $ 10$-$5)

Question

In qualitative analysis, the metals of group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains Ag⁺ and pb²⁺ at a concentration of 0.10 M. Aqueous HCl is added to this solution until the Cl^$-$ concentration is 0.10 M. What will the concentrations of Ag⁺ and Pb²⁺ be at equilibrium ?

(K_sp for AgCl = 1.8 $ \times $ 10^$-$10, K_sp for PbCl₂ = 1.7 $ \times $ 10^$-$5)

[Ag⁺] = 1.8 $ \times $ 10^$-$7 M, [Pb²⁺] = 1.7 $ \times $ 10^$-$6 M

[Ag⁺] = 1.8 $ \times $ 10^$-$11 M, [Pb²⁺] = 8.5 $ \times $ 10^$-$5 M

[Ag⁺] = 1.8 $ \times $ 10^$-$9 M, [Pb²⁺] = 1.7 $ \times $ 10^$-$3 M

[Ag⁺] = 1.8 $ \times $ 10^$-$11 M, [Pb²⁺] = 1.7 $ \times $ 10^$-$4 M

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