Chemistry - Ionic Equilibrium Question with Solution | TestHub

ChemistryIonic EquilibriumSolubility ProductMedium2 minQB

ChemistryMediumsingle choice

Passage / Comprehension

Solubility is defined as the maximum number of moles of solute that can be dissolved in 1 litre of solvent. It is affected by the presence of common ions and the hydrolysis of ions. In a container, equal volumes of 0.02 M AgNO₃ and 0.02 M HCN solution are mixed.

$K_{s p}$ of AgCN = $4 \times 1 0^{- 16}$ M²

$K_{a}$ ( HCN)= $4 \times 1 0^{- 10}$ M.

Concentration of $Ag^{+}$ ions in the final solution would be

Options:

Answer:

Solution:

$AgNO_{3} + HCN \to AgCN + HNO_{3}$

0.01 0.01 - -

- - - 0.01

AgCN $⇌$ Ag⁺ + CN⁻ : $K_{s p}$

$x x$

H⁺ + CN⁻ $⇌$ HCN

0.01 $x$ -

$0.01 - x$ - -

AgCN(s) + H⁺(aq) $⇌$ HCN(aq) + Ag⁺(aq)

$0.01 - x$ $x$ $x$

$1 0^{- 6} = \frac{x ^{2}}{( 0.01 - x )} = \frac{x ^{2}}{0.01}$

$x = 1 0^{- 4}$

Stream:JEESubject:ChemistryTopic:Ionic EquilibriumSubtopic:Solubility Product

⏱ 2mℹ️ Source: QB

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