Given: Ag(NH3)2^+ ⇌Ag^++2 NH3 Kc=7.2 ×10^-8 and Ksp of AgCl=1.8 ×10 at 298 K. If ammonia is add

step 1 Here we have one overall chemical reaction, which we can break down into separate reactions, whi

Given: Ag(NH3)2^+ ⇌Ag^++2 NH3 Kc=7.2 ×10^-8 and Ksp of...

Given: $\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+} \rightleftharpoons \mathrm{Ag}^{+}+2 \mathrm{NH}_{3}$ $K_{\mathrm{c}}=7.2 \times 10^{-8}$ and $K_{\mathrm{sp}}$ of $\mathrm{AgCl}=1.8 \times 10$ at $298 \mathrm{~K}$. If ammonia is added to a water solution containing excess of $\mathrm{AgCl}(\mathrm{s})$ only, calculate the concentration of the complex in $1.0 \mathrm{M}$ aqueous ammonia. (a) $1.0 \mathrm{M}$ (b) $0.091 \mathrm{M}$ (c) $0.0455 \mathrm{M}$ (d) $0.023 \mathrm{M}$

Given: $\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+} \rightleftharpoons \mathrm{Ag}^{+}+2 \mathrm{NH}_{3}$
$K_{\mathrm{c}}=7.2 \times 10^{-8}$ and $K_{\mathrm{sp}}$ of $\mathrm{AgCl}=1.8 \times 10$
at $298 \mathrm{~K}$. If ammonia is added to a water solution containing excess of $\mathrm{AgCl}(\mathrm{s})$ only, calculate the concentration of the complex in $1.0 \mathrm{M}$ aqueous ammonia.
(a) $1.0 \mathrm{M}$
(b) $0.091 \mathrm{M}$
(c) $0.0455 \mathrm{M}$
(d) $0.023 \mathrm{M}$

Key Concepts

Chemical Equilibrium

Chemical equilibrium refers to the state of a reversible reaction where the rate of the forward reaction equals the rate of the reverse reaction, leading to constant concentrations of all species involved. The concept is quantified by equilibrium constants, which help predict the position of the equilibrium and the concentrations of reactants and products at balance.

Complex Ion Formation

Complex ion formation involves the bonding of central metal ions with surrounding molecules or anions called ligands, forming species with unique properties. The process is characterized by a formation (or stability) constant, which indicates the extent to which the complex ion is formed and is critical for understanding how metal ions react in solutions containing ligands.

Solubility Product (Ksp)

The solubility product constant, Ksp, is used to describe the extent to which a sparingly soluble ionic compound dissolves in water. It represents the product of the ion concentrations at equilibrium and is a key parameter in predicting the formation of precipitates and understanding solubility equilibria.

Coupled Equilibria

Coupled equilibria occur when multiple equilibrium reactions take place simultaneously in the same system, such that the shift in one equilibrium affects another. This concept is important when systems involve both solubility equilibria and complex ion formation, as the presence of ligands can alter metal ion concentrations and influence the solubility of a compound.

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