An impure sample of oxalic acid (H2C2O4) was oxidized by potassium permanganate. A 0.261-g sample of oxalic acid was dissolved, and the solution was diluted to 100.0 mL. A 25.0-mL portion of the oxalic acid solution was titrated with 26.2 mL of o.0107 M potassium permanganate. 2. a) Write a balanced equation for the titration reaction. b) How many moles of potassium permanganate were used? (ans: 2.80 x 10-4 mol) c) How many moles of oxalic acid were titrated?

An impure sample of oxalic acid (H2C2O4) was oxidized by potassium permanganate. A 0.261-g sample of oxalic acid was dissolved, and the solution was diluted to 100.0 mL. A 25.0-mL portion of the oxalic acid solution was titrated with 26.2 mL of o.0107 M potassium permanganate. 2. a) Write a balanced equation for the titration reaction. b) How many moles of potassium permanganate were used? (ans: 2.80 x 10-4 mol) c) How many moles of oxalic acid were titrated?

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.112PAE: 4.112 A metallurgical firm wishes to dispose of 1300 gallons of waste sulfuric acid whose molarity...

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Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for

Question

An impure sample of oxalic acid (H;C:04) was oxidized by potassium permanganate. A 0.261-g sample of
oxalic acid was dissolved, and the solution was diluted to 100.0 mL. A 25.0-mL portion of the oxalic acid
solution was titrated with 26.2 mL of o.0107 M potassium permanganate.
2.
a) Write a balanced equation for the titration reaction.
b) How many moles of potassium permanganate were used?
(ans: 2.80 x 10-4 mol)
c) How many moles of oxalic acid were titrated?
(ans: 7.01 x 10-4 mol)
d) Calculate the percent purity of the oxalic acid sample.
(ans: 96.7%)

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