[Bob Sacamano]

Why can't ether's can hydrogen bond with each other when they can with water?

[orgoclear]

For Hydrogen bonding, the Hydrogen must be bonded with some strongly electronegative atom (F,O,N) But in ethers the bonding is R-O-R. All the hydrogens are attached to carbons and no H is attached with the electronegative oxygen. This prevents intermolecular Hydrogen bonding

But in aqueous solutions, provided the ether is not too sterically crowded, the ether molecules can form Hydrogen bonds with the water molecules. This is why light weight (sterically unhindered) ethers are somewhat soluble in water. (it is less because of presence of +I groups i.e. alkyl groups). For example solubility of diethyl ether is 6.9gm/L
But dimethyl ether is quite soluble because it is least hindered and only methyl groups of lesser +I effect are attached

But a thing to note is that the presence of -R (electron releasing groups) decreases the electronegativity of O by +I effect. Hence the H-bonds with water molecules is considerably weaker. This also leads to reduction of boiling point of the solution (i.e. minimum boiling point azeotrope)

[Borek]

Why can't ether's can hydrogen bond with each other when they can with water?

Obvious question to ask yourself is: "what does water have that ether doesn't".