What is the volume of 1.25 M hydrochloric acid required to react completely with 45.0 mL of 0.500 M Ba (OH) 2?

36.0 mL

Explanation:

The volume of 1.25 M hydrochloric acid required to react completely with 45.0 mL of 0.500 M Ba (OH) 2 is 36.0 mL.

You would use the following equation to solve this:

2HCl + Ba (OH) ₂ → BaCl₂ + 2H₂O

36.0 mL

Explanation:

First, write the balanced reaction.

2HCl + Ba (OH) ₂ → BaCl₂ + 2H₂O

Calculate the moles of Ba (OH) ₂:

0.500 mol/L * 0.0450 L = 0.0225 mol Ba (OH) ₂

Use stoichiometry to find moles of HCl:

0.0225 mol Ba (OH) ₂ * (2 mol HCl / mol Ba (OH) ₂) = 0.0450 mol HCl

Now calculate the volume needed at the given concentration.

0.0450 mol HCl * (1 L / 1.25 mol) = 0.0360 L HCl

You need 36.0 mL of 1.25 M HCl.