K sp for Cr ( OH ) 3 is 1.6 × 1 0 − 30 . What is the molar solubility of this salt in water?

Cr ( OH ) 3 ⇌ s Cr 3 + ( aq ) + 3 s 3 OH − ( aq ) K sp = s ( 3 s ) 3 1.6 × 1 0 − 30 = 27 s 4 4 27 1.6 × 1 0 − 30 = s

Chemistry - Ionic Equilibrium Question with Solution | TestHub

ChemistryIonic EquilibriumGeneral (Ostwald's Dilution Law, Degree of Ionisation)Medium2 minPYQ_2025

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$K_{sp}$ for $Cr (OH)_{3}$ is $1.6 \times 1 0^{- 30}$ . What is the molar solubility of this salt in water?

Answer:

Solution:

$Cr (OH)_{3} ⇌ s Cr^{3 +} (aq) + 3 s 3 OH^{-} (aq) K_{sp} = s (3 s)^{3} 1.6 \times 1 0^{- 30} = 27 s^{4} 4 \frac{1.6 \times 1 0 ^{- 30}}{27} = s$

Stream:JEESubject:ChemistryTopic:Ionic EquilibriumSubtopic:General (Ostwald's Dilution Law, Degree of Ionisation)

⏱ 2mℹ️ Source: PYQ_2025

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