${K_c}$ for the reaction : ${\left[ {{\rm{Ag}}{{\left( {{\rm{CN}}} \right)}_2}} \right]^ - }\leftrightharpoons{\rm{A}}{{\rm{g}}^ + } + 2{\rm{C}}{{\rm{N}}^ - },$ the equilibrium constant at $25^\circ C{\rm{ }}\;is{\rm{ }}\;4.0{\rm{ }} \times {\rm{ }}{10^{ - 19}},$ then the silver ion concentration in a solution which was originally ${\rm{0}}{\rm{.1}}\;{\rm{molar}}\;{\rm{in}}\;{\rm{KCN}}$ and ${\rm{0}}{\rm{.03}}\;{\rm{molar}}\;{\rm{in}}\;{\rm{AgN}}{{\rm{O}}_3}$ is :

NEET UG CHEMISTRY MCQ: Equilibrium

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Application +4 | -1

{K_c}

for the reaction :

{\left[ {\mathrm{Ag}{{\left( {\mathrm{CN}} \right)}_2}} \right]^ - }\leftrightharpoons\mathrm{A}{\mathrm{g}^ + } + 2\mathrm{C}{\mathrm{N}^ - },

the equilibrium constant at

25^\circ C\mathrm{ }\;is\mathrm{ }\;4.0\mathrm{ } \times \mathrm{ }{10^{ - 19}},

then the silver ion concentration in a solution which was originally

\mathrm{0}\mathrm{.1}\;\mathrm{molar}\;\mathrm{in}\;\mathrm{KCN}

and

\mathrm{0}\mathrm{.03}\;\mathrm{molar}\;\mathrm{in}\;\mathrm{AgN}{\mathrm{O}_3}

is :

View answer and explanation

Correct option: B

7.5 \times {10^{ - 18}}

Option B (

7.5 \times {10^{ - 18}}

) is correct because it calculates the silver ion concentration by considering the formation of the complex ion and using the equilibrium constant.