I need help with this problem. They don't give a pH or a (Ka), so I'm not sure how to go about solving it. Here it is:

A 5.00-g quantity of a diprotic acid is dissolved in water and made up to exactly 250 mL. Calculate the molar mass of the acid if 25.0 mL of this solution required 11.1 mL of 1.00 M KOH for neutralization. Assume that both protons of the acid are titrated.

Thanks!

Can you elaborate on the second part? Why did you find the number of moles in 250 mL?

Okay I get it now! Thank you so much!