A student found that the titration had taken 10.00 ml of 0.1002 m naoh to titration 0.132 g of aspirin, a monoprotic acid. calculate the percent purity of aspirin (c9h8o4, molar mass = 180.2 g/mol) sample.

Question

Chemistry

Hamlet

10 June, 08:22

A student found that the titration had taken 10.00 ml of 0.1002 m naoh to titration 0.132 g of aspirin, a monoprotic acid. calculate the percent purity of aspirin (c9h8o4, molar mass = 180.2 g/mol) sample.

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Answers (1)

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Jared Mays · Answer 1

The balanced equation for the reaction between NaOH and aspirin is as follows;

NaOH + C₉H₈O₄ - - > C₉H₇O₄Na + H₂O

stoichiometry of NaOH to C₉H₈O₄ is 1:1

The number of NaOH moles reacted - 0.1002 M / 1000 mL/L x 10.00 mL

Number of NaOH moles - 0.001002 mol

Therefore number of moles of aspirin - 0.001002 mol

Mass of aspirin reacted - 0.001002 mol x 180.2 g/mol = 0.18 g

However the mass of the aspirin sample is 0.132 g but 0.18 g of aspirin has reacted, therefore this question is not correct.