Sodium chloride is added to water (at 25^∘ C ) until it is...

Sodium chloride is added to water (at $25^{\circ} \mathrm{C}$ ) until it is saturated. Calculate the $\mathrm{Cl}^{-}$ concentration in such a solution. \begin{tabular}{lc} Species & $\Delta G^{0}(\mathrm{~kJ} / \mathrm{mol})$ \\ \hline $\mathrm{NaCl}(s)$ & $-384$ \\ $\mathrm{Na}^{+}(a q)$ & $-262$ \\ $\mathrm{Cl}^{-}(a q)$ & $-131$ \end{tabular}

Sodium chloride is added to water (at $25^{\circ} \mathrm{C}$ ) until it is saturated. Calculate the $\mathrm{Cl}^{-}$ concentration in such a solution.
\begin{tabular}{lc}
Species & $\Delta G^{0}(\mathrm{~kJ} / \mathrm{mol})$ \\
\hline $\mathrm{NaCl}(s)$ & $-384$ \\
$\mathrm{Na}^{+}(a q)$ & $-262$ \\
$\mathrm{Cl}^{-}(a q)$ & $-131$
\end{tabular}

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Key Concepts

Solubility Equilibrium

In a saturated solution, the dissolution of a substance reaches equilibrium, meaning the rate of dissolution equals the rate of precipitation. The concentration of dissolved ions is determined by the solubility product, which is an expression of the equilibrium constant for the dissolution reaction. This concept is central when calculating the maximum concentration of ions in solution.

Dissolution Reaction and Stoichiometry

The dissolution process of an ionic compound involves breaking the compound into its constituent ions. Understanding the stoichiometry of this reaction is crucial because it provides the molar relationships between the solid and its dissolved ions, allowing for precise calculation of individual ion concentrations in the saturated solution.

Gibbs Free Energy and Equilibrium Constants

This concept involves the relationship ?G° = -RT ln K, which links the standard Gibbs free energy change of a reaction to its equilibrium constant. This relationship is used to determine the extent to which a reaction will proceed under standard conditions, and is key in calculating solubility when the free energies of the reactants and products are known.

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