1. Lecture 122/12/07

2. pH What is it? How do you measure it?

3. Fig. 162-, p.775

4. Autoionization of Water What is it? What is the definition of: Neutral solutions? Acidic solutions? Basic solutions?

5. T (°C)KwKw 100.29 x 10 -14 150.45 x 10 -14 200.68 x 10 -14 251.01 x 10 -14 301.47 x 10 -14 505.48 x 10 -14

6. pH vs. pOH

7. Degree of ionization

8. pH of strong acid? What is the pH of a 0.001 M HNO 3 solution?

9. Strong Bases: What is the pH of 0.01 M solution of each of the strong bases? NaOH CaO

10. Weak acids and bases HA + H 2 O ↔ H 3 O + + A - HF + H 2 O ↔ H 3 O + + F - K a = A - + H 2 O ↔ HA + OH - F - + H 2 O ↔ HF + OH - NH 3 + H 2 O ↔ NH 4 + + OH - K b =

11. Fig. 16-1, p.770

13. CH 3 COOH (aq) + H 2 O (l) ⇆ CH 3 COO - (aq) + H 3 O + (aq) K a = 1.8 x 10 -5 CH 3 COO - (aq) + H 2 O (l) ⇆ CH 3 COOH (aq) + OH - (aq) K b = 5.6 x 10 -10 2 H 2 O (l) ⇆ OH - (aq) + H 3 O + (aq) K w = K a K b

14. What is the pH of a 0.05 M solution of benzoic acid ( C 6 H 5 COOH)? K a = 6.3 x 10 -5 at 25°C