An analytical chemist weighs out 0.244 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1700M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 21.4 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. mol

Chemistry: Principles and Reactions
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ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
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Chapter14: Equilibria In Acid-base Solutions
Section: Chapter Questions
Problem 65QAP: Follow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105)....
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An analytical chemist weighs out 0.244 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then
titrates this solution with 0.1700M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 21.4 mL of NaOH
solution.
Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits.
mol
Transcribed Image Text:An analytical chemist weighs out 0.244 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1700M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 21.4 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. mol
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