Answer:
The answer to the question is
The molarity of the nitric acid solution is 6.77 × 10⁻² M
Step-by-step explanation:
The chemical equation for the reaction is Search Results
Ba(OH)₂ + HNO₃ = Ba(NO₃)₂ + H₂O
One mole of Ba(OH)₂ reacts with one mole of nitric acid to form one mole of barium nitrate and one mole of water
We are required to find the molarity of a solution of nitric acid, to do tis, we require to know the number of moles of barium hydrxide present thus
The molar mass of barium hydroxide is 171.34 g/mol
Therefore 0.232 g of barium hydroxide contains (0.232 g)/(171.34 g/mol) = 0.00135 moles or 1.35 × 10⁻³ moles of barium hydroxide
However since in the eaction the number of noles of Ba(OH)₂ and HNO₃ are equal, we have
the quantity in moles of nitric acid present in 20.00 mL solution is = 1.35 × 10⁻³ moles
Therefore, the number of moles in one liter of the nitric acid solution, which is the molarity is given by
(1.35 × 10⁻³ moles)/(20.00 L/1000) = 0.068 = 6.77 × 10⁻² M/L
The molarity of the nitric acid solution is 6.77 × 10⁻² M