What is the predominant intermolecular force in the liquid state of each of these compounds: methanol (CH3OH), carbon tetrafluoride (CF4), and hydrogen chloride (HCl)?

Throughout the liquid state, certain forces are encountered by the aforementioned molecules:  

Explanation:

CH₃OH: Combining with hydrogen. That's also since O is a very electronegative atom here between O as well as H including its molecule. These powers, with H, propagate between O, F as well as N. That's the main power, then.CF₄: F will establish hydrogen bonds, but it is not bound to H in this situation, so this may not be the primary power. Throughout this situation, owing to its tetrahedral structure, it does not have a net dipole. It then just has dispersion powers, which are sometimes referred to as van der Waals either London forces. HCl: powers of dipole-dipole as well as London dispersion.

It shows that the experiment is designed properly.