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1.639 g of an unknown diprotic acid are used to make a 100.00 mL solution. Then 25.00 mL of this solution is transferred...

1.639 g of an unknown diprotic acid are used to make a 100.00 mL solution. Then 25.00 mL of this solution is transferred to an Erlenmeyer flask and is titrated with 0.1032 M NaOH. The titration endpoint is reached after 0.00414 mol of NaOH is added using the burette. What is the molar mass of the diprotic acid? Provide your answer to the correct number of significant figures.

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Answer #1

Moles of NaOH added ². Moles of cliprotic = 0.00 414 mol. auid in 25 mL a Moles of Naoh = 0.00414 mo I 2 = 2.07x10-3mol Asto:

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