Chemistry - Ionic Equilibrium Question with Solution | TestHub

ChemistryIonic EquilibriumSolubility ProductMedium2 minQB

ChemistryMediumsingle choice

Passage / Comprehension

To precipitate ions selectively from a mixture, solid AgNO₃ is added slowly without changing the volume to 1 L of solution containing 0.1 mol Cl⁻ and 0.1 mol PO₄³⁻. Take Ksp(AgCl) = 1.2 × 10⁻¹⁰ and Ksp(Ag₃PO₄) = 2.7 × 10⁻¹⁸.

Find the minimum free $A g^{+}$ concentration for $A g_{3} P O_{4}$ to start precipitating.

Options:

Answer:

Solution:

At the onset, $K_{s p} = [A g^{+}]^{3} [P O_{4}^{3 -}]$ . Taking $[P O_{4}^{3 -}] = 0.1 M$ gives

$[A g^{+}] = 3 \frac{2.7 \times 1 0 ^{- 18}}{0.1} = 3 \times 1 0^{- 6} M .$

Stream:JEESubject:ChemistryTopic:Ionic EquilibriumSubtopic:Solubility Product

⏱ 2mℹ️ Source: QB

Doubts & Discussion

Loading discussions...