Ask Question
Today, 08:35

77.60 ml of. 210 M NaOH are required to neutralize 25.05 ml

ofH2SO4 solution in a titrationexperiment.

Calculate the molarity and normality of

theH2SO4 solution.

+2
Answers (1)
  1. Today, 09:42
    0
    Molarity = 0.650 M

    Normality = 1.30 N

    Explanation:

    In case of titration, the following formula can be used -

    M₁V₁ = M₂V₂

    where,

    M₁ = concentration of acid,

    V₁ = volume of acid,

    M₂ = concentration of base,

    V₂ = volume of base.

    from, the question,

    M₁ = ? M

    V₁ = 25.05mL

    M₂ = 0.210 M

    V₂ = 77.60 mL

    Using the above formula, the molarity of acid, can be calculated as,

    M₁V₁ = M₂V₂

    M₁ * 25.05mL = 0.210 M * 77.60 mL

    M₁ = 0.650 M

    Hence, the molarity of the acid = 0.650 M

    Normality of a diprotic acid can be calculated by multiplying 2 with the value of molarity,

    Hence,

    Normality = M * 2 = 0.650 * 2 = 1.30 N
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “77.60 ml of. 210 M NaOH are required to neutralize 25.05 ml ofH2SO4 solution in a titrationexperiment. Calculate the molarity and normality ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers