9.1: Mixtures and Solutions Solutions form because a solute and a solvent experience similar intermolecular interactions. 9.2: The Solution Process When a solute dissolves, its individual particles are surrounded by solvent molecules and are separated from each other. 9.3: Solubility The ability of a solute to dissolve in a solvent, its solubility, is dependent on the strength of attraction between the different molecules. A saturated solution will have the maximum amount of solute dissolved. 9.4: The Effect of Temperature on Solubility Temperature can increase or decrease the solubility of a solute. 9.5: The Effect of Pressure on Solubility - Henry’s Law Changes in the partial pressure are directly proportional to the solubility of dissolved gas according to Henry's Law. 9.6: Units of Concentration Various concentration units are used to express the amounts of solute in a solution. Concentration units can be used as conversion factors in stoichiometry problems. New concentrations can be easily calculated if a solution is diluted. 9.7: Dilution A solution can be diluted by adding additional solvent to a fixed amount of solute, decreasing the concentration. 9.8: Ions in Solution - Electrolytes Solutions containing ions can conduct electricity, therefore they are called electrolytes. 9.9: Properties of Solutions Properties of a solution that depend only on the concentration of solute particles are called colligative properties. They include changes in the vapor pressure, boiling point, and freezing point of the solvent in the solution. The magnitudes of these properties depend only on the total concentration of solute particles in solution, not on the type of particles. 9.10: Osmosis and Osmotic Pressure The total concentration of solute particles in a solution determines its osmotic pressure. 9.11: Dialysis Dialysis is similar to osmosis but can allow both solute and solvent particles to pass through a semipermeable membrane.