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?

1 Answer
anor277
Oct 22, 2017

We use the relationship....Concentration=Moles of soluteVolume of solution

Explanation:

And of course we need a stoichiometrically balanced equation....

Ba(OH)2(s)+2HCl(aq)→BaCl2(aq)+2H2O(l)

Now barium hydroxide HAS limited solubility in water, certainly not to the extent of 0.163⋅mol⋅L−1; we will work out the MASS of barium hydroxide required for neutralization of the acid....

Moles of HCl=13.8⋅mL×10−3⋅L⋅mL−1×0.170⋅mol⋅L−1=2.35×10−3⋅mol.

And this will neutralize HALF an equiv of Ba(OH)2(s)....

i.e. 2.35×10−3⋅mol×12×171.34⋅g⋅mol−1=0.200⋅g....

Please draw to your teachers attention, the impossibility of the reaction as written. Equations follow chemical reactions; chemical reactions do not follow equations.

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