Unit 3 Solubility Lesson 1 Introduction to Solubility

Unit 3: Solubility Lesson 1: Introduction to Solubility

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: CH 3 OH(l) → Cl. O 2(l) →

Types of Solutions • Ionic solutions contain ions. They are usually made up of ionic compounds (metal + nonmetal). • Examples of the formation of ionic solutions: (NH 4)2 HPO 4(s) → Na. H 3 P 2 O 7(s)→

Check Your Understanding • Pg. 74 #1 and 2

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.

Equations for Saturated Solutions When a solution is saturated. . . • The forward reaction is the dissolving reaction. E. g. Ag. Br. O 3(s) → Ag+(aq) + Br. O 3 -(aq) • The reverse reaction is the crystallization reaction. E. g. Ag+(aq) + Br. O 3 -(aq) → Ag. Br. O 3(s) • The overall equilibrium reaction is written as a net ionic equation. E. g. Ag. Br. O 3(s) Ag+(aq) + Br. O 3 -(aq)

Brain Break – Spot 3 Differences!

Demo – Cup Race!

Apply Your Knowledge • Pg. 76 #3 -7