Chemistry - Ionic Equilibrium Question with Solution | TestHub

ChemistryIonic EquilibriumPrecipitationMedium2 minQB

ChemistryMediuminteger

At $2 5^{\circ} C$ , the solubility product of $Mg (OH)_{2}$ is $1.0 \times 1 0^{- 11}$ . At which pH , will $Mg^{2 +}$ ions start precipitating in the form of $Mg (OH)_{2}$ from a solution of $0.001 M Mg^{2 +}$ ions?

Answer:

Solution:

$K_{sp} = [Mg^{+ 2}] [OH]^{2}$

$1 \times 1 0^{- 11} (O H^{-})^{2} O H^{-} pO H p H = 1 0^{- 3} \times (O H^{-})^{2} = 1 0^{- 8} = 1 0^{- 4} = 4 = 10$

Stream:JEESubject:ChemistryTopic:Ionic EquilibriumSubtopic:Precipitation

⏱ 2mℹ️ Source: QB

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