Textbook 6C.21

[Makenna Damhorst 3L]

Suggest an explanation between acetic acid and formic acid

The textbook explanation said that the CH3 group on acetic acid would have electron donating properties, and would be less electron withdrawing than the H on the carboxyl group on formic acid, making formic acid slightly stronger. I don't understand why one Hydrogen would withdraw more electrons than a carbon and three hydrogens, although the H+ donating properties aspect makes sense. Does anyone have more insight on this explanation?

[206171377]

So, the idea is in formic acid, the methyl group is releasing the electron while in acetic acid the H is. Thus, the methyl group will be more stable after releasing the electron, making the acid form of acetic acid more stable. Also, the conjugate base of acetic acid, is less stable than that of formic acid, which also means its is a weaker acid.