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5 August, 23:35

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?

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  1. 6 August, 00:00
    0
    0.104 M

    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
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