What do we call a solution that contains more solute than the solvent can normally hold?

A solution that contains more solute than the solvent can normally hold is referred to as supersaturated. In a supersaturated solution, the concentration of the solute exceeds its solubility limit at a given temperature and pressure. This typically occurs when a solvent is heated to dissolve more solute than it could at a cooler temperature, and when it cools down without any solute precipitating out, the solution remains in a supersaturated state. This condition is unstable; thus, if disturbed or if a small crystal of the solute is introduced, it can lead to rapid crystallization as the solute begins to precipitate out of the solution.

In contrast, a dilute solution contains a relatively low concentration of solute. A suspended solution typically refers to a mixture where solid particles are dispersed throughout a liquid but not dissolved, and partially miscible solutions involve substances that have limited solubility in each other. These terms do not accurately describe the phenomenon of a supersaturated solution, which is characterized by its excess solute under specific conditions.