Question
Calculate the ratio of $\mathrm{NaF}$ to $\mathrm{HF}$ required to create a buffer with $\mathrm{pH}=4.00$.
Step 1
In this case, the weak acid is $\mathrm{HF}$ and its conjugate base is $\mathrm{F}^-$. The $\mathrm{pH}$ of a buffer can be calculated using the Henderson-Hasselbalch equation: $$\mathrm{pH} = \mathrm{p}K_a + Show more…
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