How do i find the volume needed to titrate a .1135g acid sample if i'm given a 0.04547 M of Ba(OH)2?

Answer 1

We need to know the acid you are titrating against the barium hydroxide. Yes, it does make a difference!

Answer 2

Yu can't even start without saying which acid.

Then divide by molar mass of the acid to go from g acid to moles acid.

Multiply by the number of hydrogen ions you get from each acid molecule (e.g. 1 for HCl, 2 for H2SO4).

That's the number of moles OH- you need.

But you only need half that number moles Ba(OH)2 (work out why)

Then amount (moles) Ba(OH)2 (which you just worked out)
= volume (your unknown; L) x 0.04547 mol Ba(OH)2/L

Principle: when balancing one substance against another (in this case acid against barium hydroxide) use moles,and get the ratio of moles from the ratio in the reaction.