We have to calculate the pH of a buffer that is 0.6 M HF and 0.2 M NaF.
HF is a weak acid which dissociates partially in an aqueous solution to produce H3O+ and F- ions.
HF(aq) + H2O(l)⇌ F−(aq) + H3O+(aq)
The fluoride ion (F-) produced as a result of HF dissociation is the conjugate base of HF.
We will use the Henderson-Hasselbalch equation to solve this problem.
What is the pH of a buffer that is 0.6 M HF and 0.2 M NaF? The Ka of HF is 6.8 × 10−4.
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