1. Chapter 12 Section 2

2. Solution Equilibrium- the physical state in which the opposing processes of dissolution and crystallization of a solute occur at equal rates.
A saturated solution in a closed system is at equilibrium. The solute is recrystallizing at the same rate that it is dissolving, even though it appears to have no activity in the system.

3. Saturated Solution- a solution that contains the maximum amount of dissolved solute.
Unsaturated solution- A solution that contains less solute than a saturated solution under the existing conditions.
Supersaturated solution- a solution that contains more dissolved solute than a saturated solution contains under the same conditions.

4. The Solubility of a substance is the amount of that substance required to form a saturated solution with a specific amount of solvent at a specified temperature.
See Figure 2.4

5. The attraction between water molecules and the ions is strong enough to draw the ions away from the crystal surface and into solution, this is called the process referred to as hydration.

6. Immiscible- Liquids that are not soluble in each other.
Miscible- Liquids that dissolve freely in one another in any proportion.

7. Henry’s law- named after the English chemist William Henry, this law states: The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid.
Henry’s law applies to gas- liquid solutions at constant temperature.

8. Effervescence- The rapid escape of a gas from a liquid in which it is dissolved.
Solvated- A solute particle that is surrounded by solvent molecules.
Enthalpy of solution- the net amount of energy absorbed as heat by the solution when a specific amount of solute dissolves in solvent.