1.065 g of stainless steel was dissolved in hydrochloric acid (chromium as Cr 3+ ) and diluted to 500.0 ml. A 50.00 ml sample was passed through a Walden reducer, where only iron is reduced (Fe3+ + e- Fe2+), and titrated with 0.01920 M KMnO4 solution, which consumed 13.72 ml. A 100.0 ml sample was passed through a Jones reducer (Cr3+ + e- Cr2+ and Fe3+ + e- Fe2+) into 50.00 ml of a 0.1000 M Fe3+ solution. The resulting solution was titrated with 0.01920 M KMnO4 solution and 36.43 ml was consumed. Calculate the Fe and Cr concentrations of the sample in weight percent.
1.065 g of stainless steel was dissolved in hydrochloric acid (chromium as Cr 3+ ) and diluted to 500.0 ml. A 50.00 ml sample was passed through a Walden reducer, where only iron is reduced (Fe3+ + e- Fe2+), and titrated with 0.01920 M KMnO4 solution, which consumed 13.72 ml. A 100.0 ml sample was passed through a Jones reducer (Cr3+ + e- Cr2+ and Fe3+ + e- Fe2+) into 50.00 ml of a 0.1000 M Fe3+ solution. The resulting solution was titrated with 0.01920 M KMnO4 solution and 36.43 ml was consumed. Calculate the Fe and Cr concentrations of the sample in weight percent.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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1.065 g of stainless steel was dissolved in hydrochloric acid (chromium as Cr 3+ ) and diluted to 500.0 ml. A 50.00 ml sample was passed through a Walden reducer, where only iron is reduced (Fe3+ + e- Fe2+), and titrated with 0.01920 M KMnO4 solution, which consumed 13.72 ml. A 100.0 ml sample was passed through a Jones reducer (Cr3+ + e- Cr2+ and Fe3+ + e- Fe2+) into 50.00 ml of a 0.1000 M Fe3+ solution. The resulting solution was titrated with 0.01920 M KMnO4 solution and 36.43 ml was consumed. Calculate the Fe and Cr concentrations of the sample in weight percent.
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