The boiling points of alcohols are in general much higher than comparably sized ethers. That can be explained by the extra intermolecular forces between the alcohol molecules due to the hydrogen bonding. There is no such hydrogen bonding between the ether molecules because all the hydrogen atoms are not bonded to an Oxygen or a Nitrogen. Since there is not any possibility of Hydrogen bonding the forces between the ether molecules are much weaker and can be much more easily vaporized. Since the size of the molecules of the two compounds are approximately the same, this dramatic difference can only be explained by the presence of hydrogen bonding with the alcohol.
Polyhydric alcohols have higher boiling points when compared to similar sized monohydric alcohols.
This is easily explained since we have more than one Hydroxyl group in the molecule there would be extensively higher hydrogen bonding between the alcohol molecules. The water solubility of alcohols and ethers are much more similar. Low moolecular weight alcohols and ethers are water solubility such as Methanol, Ethanol, and Dimethyl ether. But four carbon alcohols and higher and three carbon ethers or higher have a much lower water solubility. This can be explained by considering the way that water molecules can disperse solute molecules into a solution.