What does it mean for a solution to be supersaturated?

A supersaturated solution is characterized by containing more dissolved solute than what would typically be found in a stable equilibrium state at a given temperature. In a saturated solution, the amount of solute present is at its maximum capacity, meaning no more solute can be dissolved at that specific temperature. However, when a solution becomes supersaturated, it has been prepared under conditions (like increased temperature or pressure) that allow for more solute to dissolve than what is normally possible. Once these conditions change, such as through cooling or seeding, the extra solute may precipitate out of the solution, as the system seeks to return to an equilibrium state.

This is distinct from a saturated solution, which has reached the equilibrium concentration of solute and cannot dissolve any more at that specific temperature, and from an undersaturated solution, where the concentration of solute is lower than that of the equilibrium concentration. The concept of supersaturation is important in various applications, including crystallization processes and understanding solution behaviors in chemistry.