Chemistry - Ionic Equilibrium Question with Solution | TestHub

ChemistryIonic EquilibriumSolubility ProductEasy2 minPYQ_2020

ChemistryEasysingle choice

What minimum concentration of $S O_{4}^{2 -}$ is required to precipitate $B a S O_{4}$ from the solution containing $1.0 \times 1 0^{- 4} m o les of B a^{2 +}$ ? (Given $K_{s p}$ for $B a S O_{4}$ is $4 \times 1 0^{- 10}$ )

Options:

Answer:

Solution:

$B a S O_{4}$ ⇌ $B a^{2 +} + S O_{4}^{2 -}$
$K_{s p} = [B a^{2 +}] \times [S O_{4}^{2 -}]$
$K_{s p} = S^{2} \Rightarrow S = \sqrt{K_{s p}}$ ;
$4 \times 1 0^{- 10} = [1 \times 1 0^{- 4}] \times [S O_{4}^{2 -}]$
$[S O_{4}^{2 -}] = \frac{4 \times 1 0^{- 10}}{1 \times 1 0^{- 4}} = 4 \times 1 0^{- 6}$ .

Stream:NTA_ABHYAS_NEETSubject:ChemistryTopic:Ionic EquilibriumSubtopic:Solubility Product

⏱ 2mℹ️ Source: PYQ_2020

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