Question

In qualitative analysis, the metals of group I can be separted 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 be the concentration of Ag⁺ and Pb²⁺ be at equilibrium? (K_sp for AgCl = 1.8 x 10^-¹⁰, Ksp for PbCl₂ = 1.7 x 10^-5)

[Ag⁺] = 1.8 x 10^-7 M; [Pb²⁺] = 1.7 x 10^-6 M

[Ag⁺] = 1.8 x 10^-11 M; [Pb²⁺] = 8.5 x 10^-5 M

[Ag⁺] = 1.8 x 10^-9 M; [Pb²⁺] = 1.7 x 10^-3 M

[Ag⁺] = 1.8 x 10^-11 M; [Pb²⁺] = 8.5 x 10^-4 M

Solution

[Ag⁺] = 1.8 x 10^-9 M; [Pb²⁺] = 1.7 x 10^-3 M

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