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A saturated solution is defined as one that contains the maximum concentration of solute that can dissolve in a solvent at a specific temperature and pressure. In a saturated solution, the solute is in a state of equilibrium with the undissolved solute; any additional solute added will not dissolve but will remain in its solid form. This equilibrium occurs because the rate of dissolution of the solid solute into the solution equals the rate of precipitation of solute out of the solution.

This concept is fundamental in understanding the solubility of substances, as different solutes have varying levels of solubility depending on the solvent and the conditions, such as temperature. As the temperature increases, for many solids, solubility also increases, allowing the solution to hold more solute before it reaches saturation.

Options suggesting that a saturated solution contains no solute, can dissolve more solute, or only contains solid solutes do not accurately describe the conditions that characterize a saturated solution. A saturated solution must necessarily contain both dissolved and undissolved solute to maintain that equilibrium state.