In \[H-F\] there is H-bonding. Hence, the boiling point is
high. There is no H-bonding in \[HCl\]. So the boiling point is less. On moving
further to \[HBr\] and \[HI\], the size of the molecule increases and so the van
der Waals forces increase and so does the boiling point. Hence, \[HCl\] has the
lowest boiling point.
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