Question

If 25.0 mL of 0.100 M Ca(OH)2 is titrated with 0.200 M HNO3, what volume of nitric acid is required to neutralize the base?

Answer 1

25 mL

Step-by-step explanation:

The reaction that takes place is:

• Ca(OH)₂ + 2HNO₃ → Ca(NO₃)₂ + 2H₂O

First we calculate how many Ca(OH)₂ moles were spent in the titration:

• 25.0 mL * 0.100 M = 2.5 mmol Ca(OH)₂

Then we convert Ca(OH)₂ moles into HNO₃ moles, using the stoichiometric ratio:

• 2.5 mmol Ca(OH)₂ *
  `(2mmolHNO_3)/(1mmolCa(OH)_2)` = 5.0 mmol HNO₃

Finally we calculate the volume of required nitric acid solution, using the concentration:

• 5.0 mmol ÷ 0.200 mmol/mL = 25 mL