1. Properties of Solutions
Chapter 11

2. The Energies of Solution Section 11.2
A solution is formed when the solute becomes completely dispersed throughout the solvent
Solubility depends on two major factors:
Intermolecular forces
Natural tendency for objects to spread out as much as possible

3. Solvation of NaCl
The solvation process occurs when the intermolecular forces between solvent-solute are greater than that of solute-solute:

4. NaCl vs. Hexane
Why doesn’t NaCl dissolve in nonpolar solvents such as hexane, C6H14?

5. Energy Changes and Solution Formation
Hsoln = H1 + H2 + H3

6. Factors Affecting Solubility Section 11.3
The stronger the intermolecular forces between solute and solvent (as opposed to solute-solute), the greater the solubility
Ex: NaCl/H2O vs. C6H12O6/H2O
I2/H2O vs. I2/Benzene
What intermolecular forces exist and which have the greatest magnitude?

7. Solutions of Liquids (Miscibility)
Essentially follows the rule that "like dissolves like"
Dipole-dipole interactions between solvent and solute determine the miscibility of liquids
butanol/H2O  soluble
diethyl ether/H2O  only slightly soluble

9. Thin Layer Chromatography (TLC)