A 0.110-L sample of an unknown #HNO_3# solution required 52.7 mL of 0.100 M #Ba(OH)_2# for complete neutralization. What was the concentration of the #HNO_3# solution?

1 Answer
anor277
Nov 15, 2016

Approx. #0.1*mol*L^-1#

Explanation:

We need a stoichiometrically balanced equation:

#Ba(OH)_2(aq) + 2HNO_3(aq) rarr Ba(NO_3)_2(aq) + 2H_2O(l)#

Thus 2 equiv of nitric acid were necessary for each equiv barium hydroxide.

#"Concentration of nitric acid"#

#=# #(52.7xx10^-3Lxx0.100*mol*L^-1xx2)/(0.110*L)=??*mol*L^-1#

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