First slide

Solubility product(KSP)

Question

At 25⁰C, in the saturated solution of Ag₂CrO₄. If concentration of CrO₄^–2 ion is 1 × 10^–4mol/l, then the solubility product of Ag₂CrO₄ at 25⁰C is

Easy

A

$\large 5\, \times \,{10^{ - 16}}{m^3}/{l^3}$
B

$4\, \times \,{10^{ - 12}}{m^3}/{l^3}$
C

$1\, \times \,{10^{ - 18}}{m^3}/{l^3}$
D

$4\, \times \,{10^{ - 8}}{m^3}/{l^3}$

Solution

In the saturated solution, following equilibrium exists
$\large A{g_2}Cr{O_4}\left( s \right) \rightleftharpoons \mathop {A{g_2}Cr{O_4}}\limits_S \left( {aq} \right) \to \mathop {2A{g^ + }}\limits_{2S} \left( {aq} \right) + \mathop {CrO_4^{ - 2}}\limits_S \left( {aq} \right)$
$\large {K_{sp}} = {\left( {2S} \right)^2} \times S = 4{S^3} = 4 \times {\left( {{{10}^{ - 4}}} \right)^3}$
$\large {K_{sp}} = 4 \times {10^{ - 12}}mo{l^3}/{\ell ^3}$

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