Question

If it requires 23.4 milliliters of 0.65 molar barium hydroxide to neutralize 42.5 milliliters of nitric acid, solve for the molarity of the nitric acid solution. Show all of the work used to solve this problem. Unbalanced equation: Ba(OH)2 + HNO3 Ba(NO3)2 + H2O

Answer 1

we know that it takes 2 moles of HNO3 to neutralize and each mole of Ba(OH)2 and the total number of moles of Ba(OH)2 to be neutralized is
23.4*10^(-3) litres * 0.65 mol/litre
= 15.21*10^(-3) moles
[ 2*15.21*10^(-3)
= 30.42*10^(-3) moles] of HNO3 in a volume of 42.5 ml
The molarity is 30.42*10^(-3) moles / 42.5*10^(-3) litres
= 0.72 C
hope it helps