Calculate the molecular weight of a dibasic acid.0.56gm of which is required 250ml of N/20 sodium hydroxide solution for neutralization.​

Question

Calculate the molecular weight of a dibasic acid.0.56gm of which is required 250ml of N/20 sodium hydroxide solution for neutralization.​

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Ben Gia 6 months 2021-07-13T19:43:48+00:00 1 Answers 5 views 0

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    2021-07-13T19:45:18+00:00

    Answer: The molecular weight of the dibasic acid is 89.6 g/mol

    Explanation:

    Normality is defined as the amount of solute expressed in the number of gram equivalents present per liter of solution. The units of normality are eq/L. The formula used to calculate normality:

    \text{Normality}=\frac{\text{Given mass of solute}\times 1000}{\text{Equivalent mass of solute}\times \text{Volume of solution (mL)}}      ….(1)

    We are given:

    Normality of solution = \frac{1}{20}=0.05N

    Given mass of solute = 0.56 g

    Volume of solution = 250 mL

    Putting values in equation 1, we get:

    0.05=\frac{0.56\times 1000}{\text{Equivalent mass of solute}\times 250}\\\\\text{Equivalent mass of solute}=\frac{0.56\times 1000}{0.05\times 250}=44.8g/eq

    Equivalent weight of an acid is calculated by using the equation:

    \text{Equivalent weight}=\frac{\text{Molar mass}}{\text{Basicity}}   …..(2)

    Equivalent weight of acid = 44.8 g/eq

    Basicity of an acid = 2 eq/mol

    Putting values in equation 2, we get:

    44.8g/eq=\frac{\text{Molar mass}}{2eq/mol}\\\\\text{Molar mass}=(44.8g/eq\times 2eq/mol)=89.6g/mol

    Hence, the molecular weight of the dibasic acid is 89.6 g/mol

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