16.24 mL of 0.325 M Ba(OH)₂ solution is required to completely neutralize 26.58 mL of HNO₃ solution. What is the molarity of the nitric acid solution? Ba(OH)₂(aq) + 2 HNO₃(aq) $\rightarrow$ Ba(NO₃)₂(aq) + 2 H₂O (l)

Question

Quizplus · Accepted Answer

The balanced equation shows that 1 mole of Ba(OH)₂ reacts with 2 moles of HNO₃. Calculate moles of Ba(OH)₂: 0.01624 L * 0.325 M = 0.005278 moles. Since the ratio is 1:2, moles of HNO₃ = 2 * 0.005278 = 0.010556 moles. Molarity of HNO₃ = 0.010556 moles / 0.02658 L = 0.397 M.

1624 ML of 0 →\rightarrow→ Ba(NO3)2 (aq) + 2 H2O (L) A) 0

1624 ML of 0 $\rightarrow$ Ba(NO₃)₂(aq) + 2 H₂O (L)
A) 0