Answer to Question #192784 in General Chemistry for Moba Limata

Question

A 25 cm3 sample of an aqueous solution of barium hydroxide, of concentration 0.146 mol dm3 was exactly neutralized by 28.7cm3 of aqueous nitric acid, according to the unbalanced equation:

Ba (OH)2 (aq) + HNO3(aq) ˗˗˗˗˗˗˗˗˃ Ba(NO3)2 (aq) + H2O (l)

i. Calculate the amount of nitric acid in terms molarity and in terms of number of moles

Answer 1

Ba(OH)₂ : 1M=2N

0.146mol dm^-3= 0.146M=0.292N

25cm³ of 25ml of 0.292N means 25×0.292= 7.3

HNO₃ :1M= 1N

Conc of HNO₃ = x(N)

28.7 mol of x(N) means 28.7×x mili equFor exact neutralization 28.7×x= 7.3

X= 0.25

Concentration of nitric acid is 0.254M= 0.254 mol dm^-3