The pKa of the weak acid, based on the titration results, is 4.24.
Only the half-equivalence pH is needed to answer this.
At the half-equivalence point of the titration, half of the monoprotic acid HA has been neutralized and converted to the appropriate salt. That means that the concentration of the acid [HA] is equal to the concentration of its anion [A⁻]. Now, we can consult the Henderson-Hasselbalch equation:
[tex]pH = pKa + log\frac{[A^{-} ]}{[HA]}[/tex]
Because [A⁻] = [HA], that means that:
[A⁻]/[HA] = 1
log(1) = 0
pH = pKa
So, at the half-equivalence point in the titration of the weak acid the pH value of the solution is equal to the pKa value of the weak acid, so pKa = 4.24
You can learn more about weak acids here:
brainly.com/question/12811944
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