(d$\mathrm{H}_2 \mathrm{O}$, HF and $\mathrm{NH}_3$ have hydrogen bonding as the intermolecular forces while $\mathrm{HCl}$ has weaker dipoledipole interaction.
Thus, $\mathrm{HCl}$ has the lowest boiling point.
Among $\mathrm{H}_2 \mathrm{O}$, HF, and $\mathrm{NH}_3 \mathrm{H}_2 \mathrm{O}$ has the highest boiling point due to extensive network of hydrogen bonds.
Among $\mathrm{NH}_3$ and $\mathrm{HF}$, $\mathrm{HF}$ forms stronger hydrogen bonds due to very high electronegativity of fluorine. Thus, the order of boiling point will be :-
$
\mathrm{HCl} < \mathrm{NH}_3 < \mathrm{HF} < \mathrm{H}_2 \mathrm{O}
$