1. Ions in Aqueous Solutions
Dissociation
Ionization
Strong and Weak Electrolytes
Colligative Properties
Vapor-Pressure Lowering
Freezing Point Depression
Boiling Point Elevation
Osmotic Pressure
Electrolytes and Colligative Properties

2. Ions in Aqueous Solutions
Dissociation: the separation of ions that occurs when an ionic compound dissolves
Ionization
Strong and Weak Electrolytes

3. Ions in Aqueous Solutions
Dissociation: the separation of ions that occurs when an ionic compound dissolves
AX → A+ + X-
Precipitation Reactions:
Net Ionic Equations

4. Ions in Aqueous Solutions
Precipitation Reactions: Soluble
Most Sodium, Potassium, and Ammonium compounds are soluble
Most Nitrates, Acetates, and Chlorates are soluble
Most Chlorides are soluble
Except Silver, Mercury(I), and Lead
Lead(II)Chloride is Soluble in Hot H2O
Most Sulfates are soluble
Except those with Barium, Strontium, and Lead

5. Ions in Aqueous Solutions
Precipitation Reactions: Insoluble
Insoluble: most Carbonates, Phosphates, and Silicates
Except with Sodium, Potassium, Ammonium
Insoluble most Sulfides
Except with Calcium, Strontium, Sodium, Potassium, and Ammonium
Net Ionic Equations
Net Ionic Equations: Include only the compounds and ions that change in the reaction
Spectator Ion: Ions that remain unchanged from the beginning to end of the reaction

6. Ions in Aqueous Solutions
Ionization
Ionization: when ions are formed from solute molecules by the action of the solvent
Hydronium Ion: H3O+ or H+

7. Ions in Aqueous Solutions
Strong and Weak Electrolytes
Strong Electrolytes: A compound that conducts electricity well in an aqueous solution
Good Conductivity is usually due to high dissociation of the compound into ions
Weak Electrolytes: A compound that conducts electricity poorly in an aqueous solution
Poor Conductivity is usually due to low dissociation of the compound into ions

8. Colligative Properties
Colligative Properties: properties that depend on solute particle concentration not their identity
Vapor-Pressure Lowering
Freezing Point Depression
Boiling Point Elevation
Osmotic Pressure
Electrolytes and Colligative Properties
Actual Values for Electrolyte Solutions: approximations

9. Colligative Properties
Vapor-Pressure Lowering
Nonvolatile: a substance with little tendency to become a gas under existing conditions

10. Colligative Properties
Freezing Point Depression
Molal Freezing Point Constant (Kf): the freezing point depression of the solvent in a 1 molal solution of a nonvolatile non-electrolytic solute.
Freezing Point Depression (Δtf ) the difference between the freezing point of a pure solvent and a solvent of a non-electrolytic solvent
Freezing Point Depression = molal freezing point depression x molality, Δtf = (Kf)m

11. Colligative Properties
Boiling Point Elevation
Molal Boiling Point Constant (Kb): the boiling point elevation of the solvent in a 1 molal solution of a nonvolatile no electrolytic solute.
Boiling Point Elevation (Δtb ) the difference between the freezing point of a pure solvent and a solvent of a non-electrolytic solvent
Boiling Point Elevation = molal boiling point elevation x molality, Δtb = (Kb)m

12. Colligative Properties
Osmotic Pressure
Semipermeable Membranes: allows the movement of some particles while block others
Osmosis: the movement of the solvent through a semipermeable membrane from the side of lower solute concentration to the side with greater solute concentration
Osmotic Pressure: the external pressure necessary to stop the process of Osmosis.

13. Colligative Properties
Electrolytes and Colligative Properties
Calculated Values for Electrolytic Solutions: is proportional to the moles of ions produced
Actual Values for Electrolyte Solutions: approximations