Polarity of alcohols and their miscibility in water I am an AP Chemistry student and there is a small detail concerning polarity of molecules that I am confused about. 

My review book (Princeton review) says that ethanol has stronger intermolecular forces than methanol because it has a large molecular mass and is therefore more polarizable and more soluble in water than methanol.

Yet, my chemistry textbook says that both ethanol and methanol are miscible in water, but the more the carbon chain increases, the less miscible it becomes. Further supporting this statement is the fact that methanol is less soluble in hexane, a nonpolar substance, than ethanol. Therefore ethanol is less polar. Plus, heptanol is hardly soluble in water, but according to the Princeton Review's logic, it should be even more soluble in water than methanol because it has a larger molecular mass. 

So, which is it? Does the addition of CH3s make a molecule more or less polar, and more or less miscible in water?
If your book says exactly that, then it says nonsense. Sure enough, the addition of CH2's makes a molecule less polar. As for the solubility in water, methanol is miscible - i.e., infinitely well soluble in it. So is ethanol. How would you compare the two infinities?

That being said, the bigger molecule of ethanol is indeed more polarizable (not more polar, mind you!), and has more intermolecular interactions per molecule than methanol, which accounts for the higher boiling point.