Given that #[Ba(OH)_2]=0.163*mol*L^-1#, what volume of this solution is required to neutralize a #13.8*mL# volume of #HCl# whose concentration is #0.170*mol*L^-1#?
We use the relationship....
And of course we need a stoichiometrically balanced equation....
Now barium hydroxide HAS limited solubility in water, certainly not to the extent of
And this will neutralize HALF an equiv of
Please draw to your teachers attention, the impossibility of the reaction as written. Equations follow chemical reactions; chemical reactions do not follow equations.