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:

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.

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

the right answer is c i just did the question.