A 0.881 g sample of a diprotic acid is dissolved in water and titrated with 0.160 M NaOH . What is the molar mass of the acid if 35.8 mL of the NaOH solution is required to neutralize the sample

The molar mass of the acid if 35.8 mL of the NaOH solution is required to neutralize the sample is 308 g/mol

Explanation:

To calculate the number of moles for given molarity, we use the equation:

    .....(1)

Molarity of NaOH solution = 0.160 M

Volume of solution = 35.8 mL

Putting values in equation 1, we get:

As 2 moles of NaOH reacts with = 1 mole of diprotic acid

Thus 0.00573 moles of NaOH reacts with = moles of diprotic acid

mass of acid =

0.881 g =

Thus the molar mass of the acid if 35.8 mL of the NaOH solution is required to neutralize the sample is 308 g/mol

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