The butylammonium ion, C₄H₉NH₃⁺, has a K_a of 2.3 × 10⁻¹¹.

(a) Calculate K_b for the conjugate base, C₄H₉NH₂ (butylamine).
(b) Place the butylammonium ion and its conjugate base in Table 16.2. Name an acid weaker than C₄H₉NH₃⁺ and a base stronger than C₄H₉NH₂.
(c) What is the pH of a 0.015 M solution of butylammonium chloride?

Data given in Table 16.2

Transcribed Image Text:

C4H₂NH3+ (aq) + H₂O(l) → H3O+ (aq) + C4H₂NH₂(aq)