Problem: A 0.552-g sample of ascorbic acid (vitamin C) was dissolved in water to a total volume of 20.0 mL and titrated with 0.1103 M KOH, and the equivalence point occurred at 28.42 mL. The pH of the solution at 10.0 mL of added base was 3.72.From this data, determine the molar mass for vitamin C.

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We’re being asked to calculate the Molar mass of Ascorbic acid if a 0.552-g sample of ascorbic acid (vitamin C) was dissolved in water to a total volume of 20.0 mL and titrated with 0.1103 M KOH, and the equivalence point occurred at 28.42 mL

Recall that at the equivalence point of a titration:


moles acid = moles base


Since Ascorbic acid is a monoprotic acid, there will be just one equivalence point for the titration. 


This means:

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Problem Details

A 0.552-g sample of ascorbic acid (vitamin C) was dissolved in water to a total volume of 20.0 mL and titrated with 0.1103 M KOH, and the equivalence point occurred at 28.42 mL. The pH of the solution at 10.0 mL of added base was 3.72.

From this data, determine the molar mass for vitamin C.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Equivalence Point concept. If you need more Equivalence Point practice, you can also practice Equivalence Point practice problems.

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Based on our data, we think this problem is relevant for Professor Voznyy's class at TORONTO.