1. Chapter 111 Chapter 11: Solutions 1. Solutions defined: read (no lecture) 2. Solvation process: energetics, temperature (read, no lecture), pressure 3. Units of concentration; an example 4. Colligative properties; overview solubility vapor pressure lowering boiling point elevation freezing point depression osmosis examples

2. Chapter 112 CHEM101 review topics Lewis structures, molecular geometry entropy, free energy go to slide 5

3. Chapter 113 1. Introduction A solution is a homogenous mixture at the macroscopic and microscopic level

4. Chapter 114

5. 5 2. SolvationWill it dissolve? Look at the energetics of solvation a.  G must be negative b.  H summarizes intermolecular forces among solvent molecules, solute molecules, and between solvent & solute molecules;  H can be positive or negative c.  S is (almost) always positive for mixing; in other words,  S favors mixing

6. Chapter 116 OH 1- causes water molecules to become more ordered

7. Chapter 117 aside: ion-dipole forces act between a dissolved ion and molecules with a permanent dipole moment -- ++ ++

8. Chapter 118 Examples: solute/solventsoluble?explanation NaCl/wateryes strong ion-dipole forces between NaCl and water vs. strong ion-ion forces in NaCl, medium-strong H-bond forces in water entropy! toluene/octane C 7 H 8 /C 8 H 18 yes strong (similar) dispersion forces in toluene, in octane, and between toluene and octane entropy!

9. Chapter 119 solute/solventsoluble?explanation ethanol/water CH 3 CH 2 OH yesstrong (similar) H- bonding forces in ethanol, in water, and between ethanol & water entropy! CCl 4 /H 2 Onostrong dispersion forces in CCl 4, strong H-bonding in H 2 O, and very weak forces between CCl 4 and H 2 O entropy is not enough

10. Chapter 1110 solute/solventsoluble?explanation AgCl/waternostrong ion-dipole forces between AgCl and water vs. very strong ion-ion forces in AgCl, medium- strong H-bond forces in water entropy is not enough Br 2 /H 2 O I 2 /CCl 4