Molarity Of Potassium Permanganate

Redox Reaction Lab Practical
Luis Suarez and Lukyon Mendrin
CHEM 1A Lab, Department of Chemistry, California State University, Fresno, CA 93740
[e-mail]
April 13, 2016
In This experiment we used potassium permanganate (KMnO4) as our titrant and our titrand was oxalic acid (H2C2O4● 2H2O). The objective of the experiment was to titrate the solutions to determine the molarity of potassium permanganate. We had to dilute the stock solutions to a specific molarity for the experiment. Using the same method, an unknown solution called “120x” was titrated to find its percentage of oxalic acid.
Introduction
The purpose of the experiment was to use volumetric analysis, a chemical analysis involving measuring a liquids volume to
The calculations ask for the unknown trails are similar to the calculation above, with a small difference. The calculations ask for the percent of oxalic acid dehydrate in the sample. To calculate the percent of oxalic acid, first convert the volume changes from ml to liters, and then multiply by the molarity of KMnO4 to identify the mole of KMnO4. then you multiply it by the Molar Ratio to determine The moles of H2C2O4● 2H2O Then multiply it by the molar mass of H2C2O4● 2H2O to get the grams of H2C2O4● 2H2O in the solution. Then divide it by the mass of the unknown and multiply it by 100% to identify the percent of H2C2O4● 2H2O. The calculations for the other trails for the unknown are the same except for the volume change because each trial required a different amount of solution to reach the end-point and mass of the
The average percent was 10.90%. the precision of the experiment was 1.1419 error.
Acknowledgment. I thank California state university for supplying all the materials that were needed, instructor Manee Patanapongpibul and my lab partner, Lukyon Mendrin.
References
Chemistry 1A Laboratory Manual, Fall 2015 Edition, 163-172
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