The following pictures represent solutions of AgCl, which also may contain ions other than Ag+ and Cl- that are not shown. If solution 1 is a saturated solution of AgCl, classify solutions 2–4 as unsaturated, saturated, or supersaturated. (1) (2) (3) (4)

Key Concepts

Saturation and Solubility

Saturation refers to the point at which a solution can no longer dissolve additional solute at a given temperature and pressure. A saturated solution contains the maximum concentration of solute that can be dissolved, while unsaturated solutions can still dissolve more solute. Supersaturated solutions contain more solute than the saturation point, achieved through specific conditions such as temperature changes.

AgCl Solubility Product (Ksp)

The solubility product constant (Ksp) is an equilibrium constant that applies to the solubility of sparingly soluble ionic compounds like AgCl. It is defined as the product of the molar concentrations of the ions in a saturated solution, raised to the power of their coefficients in the balanced equation. For AgCl, Ksp = [Ag+][Cl-], and comparing the ion concentrations in solutions helps classify them as saturated, unsaturated, or supersaturated.

Ionic Concentration and Classification

To classify solutions as saturated, unsaturated, or supersaturated, one must analyze the concentrations of the ions present. If the concentrations of Ag+ and Cl- ions in a solution are less than those in a saturated solution, it is unsaturated. If they are equal, it is saturated, and if they exceed the saturation concentration, the solution is supersaturated. This classification is crucial for understanding the behavior of the solutions in the context of solubility.