If 25.0 mL of 0.100 M #HCl# is titrated with 0.150 M #Ba(OH)_2#. what volume of barium hydroxide is required to neutralize the acid?
A little less than half the volume of the starting hydrochloric acid.
We need (i) a stoichiometric equation:
Which shows us that 2 equiv acid react with the 1 equiv of barium hydroxide.
And (ii) we need the equivalent quantities of acid and base, observing the stoichiometry.
Given the stoichiometry, this molar quantity represents HALF of the molar quantity of barium hydroxide, which of course had an initial concentration of
I have not checked the solubility of the barium salt. Barium hydroxide has limited aqueous solubility. Presumably this question is consistent with experiment.