1. TOPIC: Intro Solutions and Solubility Do Now: check out test grades

2. Classification of Matter
Pure
Substances
Mixtures
Homogeneous
Heterogeneous
Elements
Compounds
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3. Solution Homogenous Mixture (aka SOLUTION): particles too small to see
Particles evenly distributed
Particles do not settle
-translucent – looks clear

4. Parts of a Solution Solute = dissolved substance
Solvent = dispersing medium (often water)

5. Solubility = the max amount of solute that can be dissolved in a solvent
Many solids and gases dissolve in water
As you increase the temperature, you can dissolve more solid
Does this work the same with gas?
To get gases dissolve, decrease temperature and increase pressure

6. Not everything dissolves in water
Likes dissolve Likes
Water is polar, so only polar things will dissolve in water
Things that dissolve in water
Soluble ionic compounds
Acids (ex HCl)
Bases (ex. NaOH)
Polar covalent molecules

7. Dissolving an Ionic Substance in a Water We say it IONIZES (separates into ions)
Example:
NaCl(s)  Na+(aq) + Cl-(aq)
CaCl2(s)  Ca2+(aq) + 2Cl-(aq)
AlCl3(s)  Al3+(aq) + 3Cl-(aq)
The ions are spread out among the water molecules.

8. Dissolving a Covalent Substance in water stays as molecules
Ex: sucrose
C12H22O11(s)  C12H22O11(aq)
The sugar molecules are spread out among the water molecules.

9. Not everything dissolves in water
Water is often used as a solvent
Not everything dissolves in water
Soluble = dissolves in water = aq
Insoluble = doesn’t dissolve in water
Miscible = 2 liquids that dissolve
Immiscible = 2 liquids that don’t dissolve

10. Summary: Factors Affecting Solubility
Nature of the solvent and the solute:
LIKE DISSOLVES LIKE
Temperature
Pressure (for systems with gases)