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(D) The Henderson-Hasselbalch equation is given by $pH = pK_a + \log \frac{[Salt]}{[Acid]}$.For a buffer to be most efficient,the $pH$ of the solution

Vedclass · Accepted Answer

Acetoacetic acid $(pK_a = 3.58)$

Vedclass · Answer

(D) The Henderson-Hasselbalch equation is given by $pH = pK_a + \log \frac{[Salt]}{[Acid]}$.For a buffer to be most efficient,the $pH$ of the solution should be as close as possible to the $pK_a$ of the weak acid used,i.e.,$pH \approx pK_a$.Given the target $pH = 3.58$,we look for an acid with a $pK_a$ value closest to $3.58$.Comparing the given options:$(A)$ $pK_a = 3.98$$(B)$ $pK_a = 4.41$$(C)$ $pK_a = 2.97$$(D)$ $pK_a = 3.58$Since Acetoacetic acid has a $pK_a$ of $3.58$,which is exactly equal to the desired $pH$,it provides the maximum buffer capacity at this $pH$.

$A$ physician wishes to prepare a buffer solution at $pH = 3.58$ that efficiently resists changes in $pH$ yet contains only small concentration of the buffering agents. Which of the following weak acids together with its sodium salt would be best to use?

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