The pH at which begins to precipitate from a solution containing 0.10 M ions is

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Solution

Q.
The pH at which $Mg {(OH)}_{2}$ $[K_{sp} = 1 \times 10^{- 11}]$ begins to precipitate from a solution containing 0.10 M ${Mg}^{2 +}$ ions is __________ . [2024]

Ans.
(9)

$Mg {(OH)}_{2} (s) \overset{H_{2} O}{⇌} {Mg}^{2 +} (aq) + 2 {OH}^{-} (aq)$

lonic product ( $K_{ip}$ ) is given by:

$K_{ip} = [{Mg}^{2 +}] {[{OH}^{-}]}^{2} = 0.1 {[{OH}^{-}]}^{2}$

For precipitation to occur:

$K_{ip} > K_{sp}$

$0.1 {[{OH}^{-}]}^{2} > 1 \times 10^{- 11}$

$[{OH}^{-}] > 10^{- 5} M$

$pOH < 5$

$(14 - pH) < 5$

$pH > 9$

At pH = 9, precipitation just starts to occur.

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