The weak base ethanolamine, HOCH₂CH₂NH₂,can be titrated with HCl.

Assume you have 25.0 mL of a 0.010 M solution of ethanolamine and titrate it with 0.0095 M HCl. (Kb for ethanolamine is 3.2 × 10⁻⁵.)
(a) What is the pH of the ethanolamine solution before the titration begins?
(b) What is the pH at the equivalence point?
(c) What is the pH at the halfway point of the titration?
(d) Which indicator in Figure 17.11 would be thebest choice to detect the equivalence point?
(e) Calculate the pH of the solution after adding 5.00, 10.0, 20.0, and 30.0 mL of the acid.
(f) Combine the information in parts (a), (b),(c), and (e), and plot an approximate titration curve.

Data given in figure 17.11

Transcribed Image Text:

HOCH₂CH₂NH₂(aq) + H3O+ (aq) → HOCH₂CH₂NH3+ (aq) + H₂O(l)