Chapter 2.10, Problem 39P

For each of the following compounds (here shown in their acidic forms), write the form that predominates in a solution with a pH = 5.5:

1. a. CH₃COOH (pK_a = 4.76)
2. b. CH₃CH₂ $\stackrel{\text{+}}{\text{N}}$H₃ (pK_a = 11.0)
3. c. H₃O+ (pK_a = –1.7)
4. d. HBr (pK_a = –9)
5. e. ⁺NH₄ (pK_a = 9.4)

1. f. HNO₂ (pK_a = 3.4)
2. g. HNO₃ (pK_a = –1.3)
3. h. HO $\stackrel{\text{+}}{\text{N}}$H₃ (pK_a = 6.0)