Final answer:
The concentration of nitric acid (HNO₃) in the titration is calculated to be 0.126 M after determining the moles of barium hydroxide (Ba(OH)₂) used and using the stoichiometry of the balanced chemical equation.
Step-by-step explanation:
To calculate the concentration of nitric acid (HNO₃) in the given titration problem, we need to first determine the amount in moles of barium hydroxide (Ba(OH)₂) used. Since mass is given, we can use the molar mass of Ba(OH)₂ (171.34 g/mol) to find the moles.
Moles of Ba(OH)₂ = 0.108 g / 171.34 g/mol = 0.000630 moles.
The balanced chemical equation provides the mole ratio between Ba(OH)₂ and HNO₃:
Ba(OH)₂ + 2HNO₃→ Ba(NO3)2 + 2H₂O
This indicates that 1 mole of Ba(OH)₂ neutralizes 2 moles of HNO₃. Therefore:
Moles of HNO₃= 2 × moles of Ba(OH)₂ = 2 × 0.000630 moles = 0.00126 moles.
To find the molarity of HNO3, we divide the moles of HNO₃ by the volume of the acid in liters (10.00 mL = 0.01000 L):
Molarity of HNO₃ = 0.00126 moles / 0.01000 L = 0.126 M.