The primary intermolecular force between ethanol molecules is hydrogen bonding. Hydrogen bonding is a strong type of dipole-dipole attraction. Other intermolecular forces present in ethanol is the London dispersion forces or Van der waal's force. 

Van der Waals forces of attraction are present in ethanol molecules, alongside stronger hydrogen bonding interactions; essentially, all molecules experience some degree of van der Waals forces, making them present in ethanol as well.