In general, a dibasic acid is not more acidic than a monobasic acid. The acidity of an acid is determined by its ability to donate a proton (H+ ion). The more easily an acid can donate a proton, the stronger the acid.

The strength of an acid is also influenced by the charge of the conjugate base. The conjugate base of a dibasic acid has a -2 charge, while the conjugate base of a monobasic acid has a -1 charge. The more negative the charge of the conjugate base, the weaker the acid.

Therefore, a dibasic acid is not necessarily more acidic than a monobasic acid. The acidity of an acid depends on several factors, including the strength of the O-H bond, the charge of the conjugate base, and the solvation of the ions.