The pH of aqueous solution of magnesium hydroxide is 9.0. If K s p of magnesium hydroxide is 1.0 × 10 − 11 M 3 , then the concentration of magnesium ions in the solution is

p H = 9 So [ H + ] = 1 0 - 9 m o l L - 1 or [ O H - ] = 1 0 - 5 m o l L - 1 K s p [ M g ( O H ) 2 ] = [ M g 2 + ] [ O H - ] 2 So Mg 2 + = 1 × 10 − 11 ( 10 − 5 ) 2 = 10 − 1 = 0.1 M

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ChemistryIonic EquilibriumSolubility ProductEasy2 minPYQ_2020

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The pH of aqueous solution of magnesium hydroxide is 9.0. If $K_{s p}$ of magnesium hydroxide is $1.0 \times 10^{- 11} M^{3}$ , then the concentration of magnesium ions in the solution is

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Solution:

$p H = 9$
So $[H^{+}] = 1 0^{- 9} m o l L^{- 1}$
or $[O H^{-}] = 1 0^{- 5} m o l L^{- 1}$
$K_{s p} [M g (O H)_{2}] = [M g^{2 +}] [O H^{-}]^{2}$
So $[{Mg}^{2 +}] = \frac{1 \times 10^{- 11}}{{(10^{- 5})}^{2}} = 10^{- 1} = 0.1 M$

Stream:NTA_ABHYAS_NEETSubject:ChemistryTopic:Ionic EquilibriumSubtopic:Solubility Product

⏱ 2mℹ️ Source: PYQ_2020

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