Ag^++NH3 ⇌[Ag(NH3)^+] ; K1=1.6 ×10^3 [Ag(NH3)^+]+NH3 ⇌[Ag(NH3)2^+] ; K2=6.8 ×10^3 . The formatio

step 1 The question deals with formation of a complex ion by reacting silver ion, AG plus, with ammonia

Ag^++NH3 ⇌[Ag(NH3)^+] ; K1=1.6 ×10^3 [Ag(NH3)^+]+NH3...

$\mathrm{Ag}^{+}+\mathrm{NH}_{3} \rightleftharpoons\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)^{+}\right] ; K_{1}=1.6 \times 10^{3}$ $\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)^{+}\right]+\mathrm{NH}_{3} \rightleftharpoons\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}\right] ;$ $K_{2}=6.8 \times 10^{3} .$ The formation constant of $\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}\right]$ is (a) $1.08 \times 10^{7}$ (b) $6.08 \times 10^{6}$ (c) $1.08 \times 10^{3}$ (d) $1.08 \times 10^{5}$

$\mathrm{Ag}^{+}+\mathrm{NH}_{3} \rightleftharpoons\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)^{+}\right] ; K_{1}=1.6 \times 10^{3}$
$\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)^{+}\right]+\mathrm{NH}_{3} \rightleftharpoons\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}\right] ;$
$K_{2}=6.8 \times 10^{3} .$

The formation constant of $\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}\right]$ is
(a) $1.08 \times 10^{7}$
(b) $6.08 \times 10^{6}$
(c) $1.08 \times 10^{3}$
(d) $1.08 \times 10^{5}$

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Key Concepts

Formation Constant

A formation constant, also known as a stability constant, is a specific type of equilibrium constant that describes the formation of a complex ion from a central metal ion and its ligands. It is crucial in coordination chemistry for understanding the stability of complexes in solution.

Stepwise Complex Formation

Stepwise complex formation refers to the process where a complex ion is formed in a sequence of individual ligand addition reactions. Each step is characterized by its own equilibrium constant, and the overall formation constant for the complex is the product of these sequential, stepwise constants.

Equilibrium Constant

An equilibrium constant quantifies the ratio of concentrations of products to reactants at equilibrium for a reversible reaction. It provides a measure of how far a reaction proceeds before reaching equilibrium, and its value is used to predict the extent of the reaction under given conditions.

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