The question asks whether 1) boric acid and 2) 1-hexanol would be more soluble in diethyl ether or aqueous solvent (which just means water right?).
For boric acid, I thought it'd be more soluble in water - since boric acid is polar, and it can hydrogen bond with water but not diethyl ether.
For 1-hexanol, I know the OH group would make it slightly polar, but wouldn't the hydrocarbon chain decrease its solubility in water? So I thought maybe diethyl ether would be the better choice since it's a nonpolar solvent. But is the opportunity for hydrogen bonding in water more important? Not sure if I'm just overthinking this part.
Thanks in advance for any help.