How is a saturated solution in water prepared from a given solute?

You can dissolve at 20.0 °C.

30.0 °C is the melting point.

At 30.0 °C, 23.8 g more solute can dissolve.

Saturation characterizes a state of equilibrium.

We might anticipate that as the solvent's temperature rises, the amount of solute it can dissolve should also rise, but we don't have any data to support this theory. This indicates that the solution contains the SAME amount of solute as would be in equilibrium with undissolved solute.

In A-level and first-year chemistry, the definition of saturation presents a challenge because it does not indicate that the solvent can contain all of the solute.

A saturated solution in water is prepared by adding the solute to water until no more solute can dissolve at a given temperature. This can be achieved by gradually adding the solute to the water while stirring continuously until the solution becomes saturated, meaning that any additional solute added will not dissolve and will instead settle at the bottom of the container.

To prepare a saturated solution in water from a given solute, you need to add the maximum amount of solute that can dissolve in the solvent at a specific temperature. This is typically done by adding the solute gradually to the solvent while stirring continuously until no more solute can dissolve and some remains undissolved at the bottom. This indicates that the solution is saturated.