[confusedstud]

Usually the interactions between the solvent and solute has to be as strong as the interactions between the solvent and solute individually. So in that case, if I have a diol and a ketone a diol has 2 H bond donor and 4 H bond acceptors. So generally each diol will have 4 hydrogen bonds. When I mix the two together, the total number of hydrogen bonds will still remain the same. So will that mean that they are very soluble in each other? If they are not what is the reason for it because by the "solution equally strong as solvent/solute" explanation they should dissolve extremely well.

I learned about finding the net dipole moment of smaller molecules such as ammonia. But what about molecules with more than 1 important dipole bonds like the diols? Because the carbon chain might be able to move how will we tell how the net dipole moment be like for those molecules (at some point they might cancel out and other variants are possible). So how do I tell their net dipole moment? And thus apply them to solubility.

Thanks