Respuesta :

MathPhys

Answer:

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.

The volume of 1.25M HCl acid required to react completely with 45.0ml of 0.500M [tex]Ba(OH)_{2}[/tex] is 36.0ml.

What are the steps for calculating the volume of HCl?

  • At first, we will write the balanced equation.

         [tex]2HCl +Ba(OH)_{2}- > BaCl_{2} +2H_{2} O[/tex]

  • Now, we will calculate the moles of [tex]Ba(OH)_{2}.[/tex].

        [tex]0.500mol/L*0.0450L=0.0225 mol[/tex]

  • So, the number of moles in [tex]Ba(OH)_{2}[/tex] is 0.0225 mol.
  • Now, we will use stoichiometry to find the moles of HCl

               [tex]0.0225mol Ba(OH)_{2}*(2 mol HCl /mol Ba(OH)_{2})=0.0450mol HCl[/tex]

  • We will now calculate the volume needed at the given concentration

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

                                                       [tex]=36.0ml HCl[/tex]

Hence, the volume of 1.25M HCl is 36.0ml.

To learn more about stoichiometry, refer to:

https://brainly.com/question/1309057

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