${\rm{A}}{{\rm{g}}^ + } + {\rm{N}}{{\rm{H}}_3}\;\leftrightharpoons{\left[ {{\rm{Ag}}\left( {{\rm{N}}{{\rm{H}}_3}} \right)} \right]^ + };\;\;{K_1} = 3.5 \times {10^{ - 3}}$ ${\left[ {{\rm{Ag}}\left( {{\rm{N}}{{\rm{H}}_3}} \right)} \right]^ + } + {\rm{N}}{{\rm{H}}_3}\;\leftrightharpoons{\left[ {{\rm{Ag}}{{\left( {{\rm{N}}{{\rm{H}}_3}} \right)}_2}} \right]^ + };$ ${K_2} = 1.7 \times {10^{ - 3}}$ Then the formation constant of${\left[ {{\rm{Ag}}{{\left( {{\rm{N}}{{\rm{H}}_3}} \right)}_2}} \right]^ + }$ is

NEET UG CHEMISTRY MCQ: Equilibrium

1 Hard

1 of 1

Application +4 | -1

\mathrm{A}{\mathrm{g}^ + } + \mathrm{N}{\mathrm{H}_3}\;\leftrightharpoons{\left[ {\mathrm{Ag}\left( {\mathrm{N}{\mathrm{H}_3}} \right)} \right]^ + };\;\;{K_1} = 3.5 \times {10^{ - 3}}

{\left[ {\mathrm{Ag}\left( {\mathrm{N}{\mathrm{H}_3}} \right)} \right]^ + } + \mathrm{N}{\mathrm{H}_3}\;\leftrightharpoons{\left[ {\mathrm{Ag}{{\left( {\mathrm{N}{\mathrm{H}_3}} \right)}_2}} \right]^ + };

{K_2} = 1.7 \times {10^{ - 3}}

Then the formation constant of

{\left[ {\mathrm{Ag}{{\left( {\mathrm{N}{\mathrm{H}_3}} \right)}_2}} \right]^ + }

View answer and explanation

Correct option: A

6.08 \times {10^{ - 6}}

Option A (

6.08 \times {10^{ - 6}}

) is correct because the overall formation constant is the product of the individual stepwise formation constants.