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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 $CN^{-}$ in the final solution would be

Options:

Answer:

Solution:

$[CN^{-}] = \frac{K _{sp}}{[ Ag ^{+} ]} = \frac{4 \times 1 0 ^{- 16}}{1 0 ^{- 4}} = 4 \times 1 0^{- 12}$

Stream:JEESubject:ChemistryTopic:Ionic EquilibriumSubtopic:Solubility Product

⏱ 2mℹ️ Source: QB

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