1. Which is the stronger acid? 1.HNO 2 2.HNO 3

2. Which is the stronger base? 1.NO 2 - 2.NO 3 -

3. Acid-Base Reactions strong acid + strong base strong acid + weak base weak acid + strong base weak acid + weak base

4. Extent of Weak Acid-Weak Base Reactions

5. pK a and Acid Strength pK a = -log K a K a pK a Trends:

6. Buffers

7. How Buffers Minimize pH Changes NH 4 + /NH 3 buffer If an acid is added: If a base is added:

8. What controls pH of a buffer?

12. Buffer pH Two cases: 1.When the acid and base of interest are in bulk and control the pH 2.When other acids and bases are in bulk and the acid/base state of the species of interest is controlled by the pH (ex: indicators)

13. 1a. Buffer pH What is the pH of a solution with [H 2 CO 3 ] = 0.25 M and [HCO 3 - ] = 0.25 M?

14. 1b. Buffer pH What is the pH of a solution with [H 2 CO 3 ] = 0.25 M and [HCO 3 - ] = 0.11 M?

18. pH Titration Curves Strong Acid – Strong Base Strong Base – Strong Acid

19. pH Titration Curves Weak Acid – Strong Base: Finding K a

20. pH Titration Curves Strong Acid – Weak Base: Finding K b

21. Polyprotic Acids H 2 CO 3 HCO 3 - CO 3 2- K a1 = 4.2 x 10 -7 K a2 = 4.8 x 10 -11 What is the pH of a 0.10 M solution of H 2 CO 3 ? What is [CO 3 2- ] in this solution?

22. Polyprotic Acids H 2 CO 3 HCO 3 - CO 3 2- K a1 = 4.2 x 10 -7 K a2 = 4.8 x 10 -11

23. Polyprotic pH Titration Curves

25. When pH Controls Acid-Base State: Amino Acids Situations where an acid-base species is a minor component in a solution where other things control the pH. Henderson-Hasselbalch and Alpha plots.

26. When pH Controls Acid-Base State: Amino Acids Situations where an acid-base species is a minor component in a solution where other things control the pH. pH = 0.00 pH = 2.34

27. pH = 0.00pH = 2.34 pH = 7.00 pH = 9.60 pH = 13.00

28. Alpha Plots