Can someone please explain to me why compound B is more acidic than compound D?
I know that both substituents on compound B and D are electron donating, which would stabilize the negative charge on the conjugate base. I also know that compound D has a stronger donator.
BUT, I also know that B's substituent can create another very very minor resonance structure if I de-prononate the hydroxyl H (2 neg charges on two carbons and a positive charge on oxygen). Is this why even though compound D is a stronger donator, compound B is more acidic? Thank you.