1. Lecture 12

2. Conjugate acid/base pairs HA + B  A - + BH +

3. Salts Ionic solid Product of acid/ base reaction  neutralization

4. Autoprotolysis of water H 2 O + H 2 O  H 3 O + + OH - K w = [OH - ][H 3 O + ]  = 1.01 x 10 -14 @ 25 o C

6. What is pH? pH = -log{H 3 O + } ~ -log[H 3 O + ] pH of pure water? Acidic vs. Bases

8. Strength of Acids/Bases

9. Weak Acid : Doesn’t completely dissociates

10. Strength of Acids/Bases Weak Base: Doesn’t completely dissociates

11. Relationship between K a and K b

12. Polyprotic acids

13. Ionic Strength C = molarity z = charge 1:1 electrolytes (NaCl) - μ = molarity 2:1, etc electrolytes (BaCl 2 ) - μ > molarity

14. What is the ionic strength of 0.1 M LiCl? What is the ionic strength of 0.1M Ca(NO 3 ) 2 ?

15. Electrolyte (salt) effect Effective concentration of ions become less as μ increases Shielding effect Non-ideal behavior

16. Activity [i] o = 1M (makes {i} dimensionless) γ is activity coefficient

18. Extended Debye-Hückel equation α – ion size z - charge γ – activity coefficient μ – ionic strength

20. Interpolate