Question

34.62 mL of a 0.1510 M barium hydroxide solution was needed to neutralize 50.0 mL of a hydrochloric acidsolution. What is the concentration of the original hydrochloric acid solution?

Answer 1

0.104 M

Step-by-step explanation:

For the titration of an acid and a base , the relation between the molarity and volume is as follows -

M₁V₁ = M₂V₂

where ,

M₁ = concentration of acid ,

V₁ = volume of acid ,

M₂ = concentration of base ,

V₂ = Volume of base ,

from , the question ,

M₁ = ?

V₁ = 50.0 mL

M₂ = 0.1510 M

V₂ = 34.62 mL

Using the above formula , the molarity of the stock solution , can be calculated as ,

M₁V₁ = M₂V₂

M₁ * 50.0 mL = 0.1510 M * 34.62 mL

M₁ = 0.1510 M * 34.62 mL / 50.0 mL

M₁ = 0.104 M