AIPMT MAINS 2011 Chemistry Solubility Product MCQ 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 is 0.10 M. Aqueous HCl is added to this solution until the Cl⁻ concentration is 0.10 M. What will the concentration of Ag⁺ and Pb²⁺ be at equilibrium?
(Ksp for AgCl = 1.8 × 10⁻¹⁰, Ksp for PbCl₂ = 1.7 × 10⁻⁵)
[Ag⁺] = 1.8 × 10⁻⁹ M, [Pb²⁺] = 1.7 × 10⁻³ M
[Ag⁺] = 1.8 × 10⁻¹¹ M, [Pb²⁺] = 1.7 × 10⁻⁴ M
[Ag⁺] = 1.8 × 10⁻⁷ M, [Pb²⁺] = 1.7 × 10⁻⁶ M
[Ag⁺] = 1.8 × 10⁻¹¹ M, [Pb²⁺] = 8.5 × 10⁻⁵ M
Correct Answer
Detailed Explanation
Using the solubility product constants (Ksp), the concentrations of Ag⁺ and Pb²⁺ at equilibrium can be calculated. Ag⁺ is less soluble, so it precipitates first.
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