A saturated solution of potassium chloride at #60# #""^@C#, is cooled to #20# #""^@C#. What happens, and how do we describe the solutions?
Saturation defines an equilibrium condition. The solution at
Now you have saturated
Of course, the solute might not precipitate out. In this case the solvent contains a greater amount of solute than would be in equilibrium with undissolved solute. This describes a SUPERSATURATED SOLUTION.
The CONCLUSION: a saturated solution holds an amount of solute equal to that amount that would be in equilibrium with undissolved solute. Normally a temperature is specified because a hot solution can hold more solute than a cold one. As temperature decreases, if solute precipitates (i.e. becomes undissolved), the solution maintains saturation as per the definition.
The one fatal error you can make is to say that