A 0.1 mole of AgNO3 is dissolved in 1 L of 1 M-NH3 . If 0.01 mole of NaCl is added to this solu

step 1 So there is only one mole of here in this problem there is only one mole of CL minus ions presen

A 0.1 mole of AgNO3 is dissolved in 1 L of 1 M-NH3 . If...

A $0.1$ mole of $\mathrm{AgNO}_{3}$ is dissolved in $1 \mathrm{~L}$ of $1 \mathrm{M}-\mathrm{NH}_{3} .$ If $0.01$ mole of $\mathrm{NaCl}$ is added to this solution, will $\mathrm{AgCl}(\mathrm{s})$ precipitate? $K_{\mathrm{sp}}$ for $\mathrm{AgCl}=1.8 \times 10^{-10}$ and $K_{\text {stab }}$ for $\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}=1.6 \times 10^{7} .$ (a) Yes (b) No (c) Addition of $\mathrm{NaCl}$ in any amount can never result precipitation. (d) Addition of even smaller amount of $\mathrm{NaCl}$ may result precipitation.

A $0.1$ mole of $\mathrm{AgNO}_{3}$ is dissolved in $1 \mathrm{~L}$ of $1 \mathrm{M}-\mathrm{NH}_{3} .$ If $0.01$ mole of $\mathrm{NaCl}$ is added to this solution, will $\mathrm{AgCl}(\mathrm{s})$ precipitate? $K_{\mathrm{sp}}$ for $\mathrm{AgCl}=1.8 \times 10^{-10}$ and $K_{\text {stab }}$ for $\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}=1.6 \times 10^{7} .$
(a) Yes
(b) No
(c) Addition of $\mathrm{NaCl}$ in any amount can never result precipitation.
(d) Addition of even smaller amount of $\mathrm{NaCl}$ may result precipitation.

Key Concepts

Complex Ion Formation

This concept refers to the process where a central metal ion binds with one or more ligands to form a complex ion. This formation alters the concentration of free metal ions in solution, which in turn can affect various equilibria such as precipitation reactions. It is vital in understanding how the presence of additional ligands can prevent or promote the formation of insoluble salts.

Solubility Product (Ksp)

The solubility product is the equilibrium constant for the dissolution of a sparingly soluble salt into its constituent ions in solution. It is a measure of the product of the ion concentrations at saturation and is used to predict whether a precipitate will form under a given set of conditions.

Stability Constant (Kstab)

The stability constant quantifies the formation of a complex ion from a metal ion and its ligands. A higher stability constant indicates that the complex ion is strongly favored in solution, thereby decreasing the concentration of free metal ions available to form precipitates.

Common Ion Effect

The common ion effect describes how the addition of an ion that is a part of an equilibrium system can shift the balance, reducing the solubility of a salt or the concentration of free ions. This concept is important when considering how the addition of a salt can influence precipitation equilibria in solutions.

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