The following pairs of liquids are miscible. Identify the predominant type of intermolecular attraction between each pair.
a) 2-propanone and ethyl ethanoate (ethyl acetate)
b) pentane and octane
c) dichloromethane and 2-butanone
e) methanol and ethanoic acid
A) Esters are polar compounds, including aldehydes and ketones, with dipole-dipole interactions and van der Waals dispersion forces. Since they don't form ester-ester hydrogen bonds, their boiling points are much lower than an acid with the same number of carbon atoms.
B) Only London dispersion forces exist in octane and pentane; ethanol and acetic acid have hydrogen bonding. Since octane is larger than pentane, it has more London dispersion forces, resulting in pentane having the weakest intermolecular forces.
C) dipole-dipole forces as well as London dispersion forces.
E) Hydrogen bonds