1. Lesson 1: Introduction to Solubility
Unit 3: Solubility
Lesson 1: Introduction to Solubility

2. Types of Solutions
Molecular solutions contain only neutral molecules. They are usually made up of covalent compounds (non-metal + non-metal).
Examples of the formation of molecular solutions:
CH3OH(l) →
ClO2(l) →
Have students jot down their answers – 5 min

3. Types of Solutions
Ionic solutions contain ions. They are usually made up of ionic compounds (metal + non-metal).
Examples of the formation of ionic solutions:
(NH4)2HPO4(s) →
NaH3P2O7(s)→
Have students jot down their answers – 5 min

4. Check Your Understanding
Pg. 74 #1 and 2
5 min

5. Solubility and Saturated Solutions
Think-Pair-Share: What were the definitions used for these terms in Chemistry 11?
“Upgraded” definitions:
The solubility of a substance is the equilibrium concentration of the substance in a saturated solution at a given temperature.
A solution is saturated when:
Some undissolved material is present, AND
Equilibrium exists between the dissolved and the undissolved material.
5 min

6. Equations for Saturated Solutions
When a solution is saturated...
The forward reaction is the dissolving reaction.
E.g. AgBrO3(s) → Ag+(aq) + BrO3-(aq)
The reverse reaction is the crystallization reaction.
E.g. Ag+(aq) + BrO3-(aq) → AgBrO3(s)
The overall equilibrium reaction is written as a net ionic equation.
E.g. AgBrO3(s) Ag+(aq) + BrO3-(aq)

7. Brain Break – Spot 3 Differences!

8. Demo – Cup Race!
Place 2 styrofoam cups in 2 beakers. Ask for volunteers to see who can fill up their cup first. Give one a water squirt bottle and one an acetone squirt bottle. – 15 min

9. Apply Your Knowledge
Pg. 76 #3-7
15 min