Why is 4-hydroxypyridine more acidic than benzoic acid?

4-hydroxypyridine (or 4-pyridone) has a $mathrm{p}K_mathrm{a}$ in the ballpark of $3$ to $3.33:^1$ (in the pdf linked below, the $mathrm{p}K_mathrm{a}$ of 1-methyl-4-pyridone has been given to be $3.33$, however I suppose removing a methyl would only cause a slight decrease in the $mathrm{p}K_mathrm{a}$ value). This seems an unexpectedly low value to me. 4-pyridone seems more acidic than I expected it to be, since the $mathrm{p}K_mathrm{a}$ of other common acids are:$:^2$

begin{array}{lr}
hline
mathrm{Acid} & mathrm{p}K_mathrm{a} \
hline
text{Benzoic acid} & 4.20 \
text{Formic acid} & 3.75 \
text{Acetic acid} & 4.75\
text{Phenol} & 10.0 \
text{Carbonic acid} & 6.37rlap{:^1} \ hline
end{array}

Now I had expected 4-hydroxypyridine to be more acidic than phenol, because of the negative charge in the former’s conjugate base being delocalised onto the electronegative nitrogen, yielding a more stable resonating structure than the latter’s corresponding resonating structure. I thought that 4-pyridone’s $mathrm{p}K_mathrm{a}$ might be somewhere around $ce{H2CO3}$‘s $mathrm{p}K_mathrm{a}$, but I was wrong. Also, I wasn’t quite sure that it would be acidic enough to have a $mathrm{p}K_mathrm{a}$ value any close to other carboxylic acids. But it seems to me that it is more acidic than benzoic acid, formic acid and acetic acid.

Why is this so? I can’t see any excetional characteristic in its structure which might impart it such a low $mathrm{p}K_mathrm{a}$. This does seem more of an exception to me, as of now, but it would be very helpful if someone clarified and explained such a trend.

References:

$[1]:$ http://gissmo.nmrfam.wisc.edu/static/pKa_compilation_R_Williams.pdf

$[2]:$ https://www2.chemistry.msu.edu/faculty/reusch/VirtTxtJml/acidity2.htm