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.
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