🤓 Based on our data, we think this question is relevant for Professor Hoeltge's class at VERMONT.
The buffer solution is composed of HF and NaF. These two components will break up in the solution:
HF(aq)→ H+(aq) + F-(aq)
NaF(aq)→ Na+(aq) + F-(aq)
HF is a weak acid and based on the Bronsted-Lowry definition, an acid is a proton (H+). Once HF loses its proton, its conjugate base is formed:
HF(aq) + H2O(l) → F-(aq) + H3O+(aq)
(weak acid) (base) (conjugate base) (conjugate acid)
Whenever we have a conjugate base and a weak acid, we have a buffer.
A 1.50 L buffer solution is 0.250 M HF and 0.250 M NaF. What is the pH of the solution after the addition of 0.0500 moles of solid NaOH? Assume no volume change. Ka for HF is 3.5 x 10-4.