First slide

Solubility product(KSP)

Question

The K_sp of a salt, having the general formula MX₂, in water is 4 × 10^–12. The concentration of M²⁺ ions in the aqueous solution of the salt is

Moderate

A

$\large 2\, \times \,{10^{ - 6}}M$
B

$1\, \times \,{10^{ - 4}}M$
C

$1.6\, \times \,{10^{ - 4}}M$
D

$4\, \times \,{10^{ - 10}}M$

Solution

$\large M{X_2}\left( s \right) \rightleftharpoons \mathop {M{X_2}}\limits_S \left( {aq} \right)\xrightarrow{{}}\mathop {{M^{ + 2}}}\limits_S \left( {aq} \right) + \mathop {2{X^ - }}\limits_{2S} \left( {aq} \right)$
$\large {K_{sp}} = S \times {\left( {2S} \right)^2} = 4{S^3}$
$\large \Rightarrow 4 \times {10^{ - 12}} = 4 \times {S^3}$
$\large \Rightarrow S = {10^{ - 4}}$
$\large \Rightarrow \left[ {{M^{ + 2}}} \right] = {10^{ - 4}}$

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