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5. 2.6477 g of the reducing agent FeSO4 was titrated to the equivalence point with 17.25 mL of a KMNO4 solution. a. Calculate the molarity of the KMNO4 solution. 2.L477 FESO4 x L mol 151-915 Imol Khga 5 molFe = 0.2021 M RMOg 0.01725 L * b. What volume (in mL) of the KMNO4 solution would be needed to react with 12.50 grams of 30.0 % H2O2 solution?

5. 2.6477 g of the reducing agent FeSO4 was titrated to the equivalence point with 17.25 mL of a KMNO4 solution. a. Calculate the molarity of the KMNO4 solution. 2.L477 FESO4 x L mol 151-915 Imol Khga 5 molFe = 0.2021 M RMOg 0.01725 L * b. What volume (in mL) of the KMNO4 solution would be needed to react with 12.50 grams of 30.0 % H2O2 solution?

Chemistry
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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I need help with number 5, a and b.
5. 2.6477 g of the reducing agent FeSO4 was titrated to the equivalence point with 17.25 mL of a KMNO4 solution. a. Calculate the molarity of the KMNO4 solution. ImolMhg 5 molFe = 0.20지 M Kn04 2.L477 FeS04 x L mol x 0.01725 L * b. What volume (in mL) of the KMNO4 solution would be needed to react with 12.50 grams of 30.0 % H2O2 solution? *6. In a redox titration, 12.52 mL of a 0.3264 M KMNO4 solution were required to titrate 1.7832 g of a reducing agent (“X"). If the reducing agent undergoes a 3-electron change per formula unit: Write the two ionic half reactions and the balanced net ionic equation. a. Mn Ouiaq) t 3e > 5MnO4 Ionic MnO4 : eid Ionic Reducing Agent: X X+ 3c= noutotoslq Net ionic: b. Calculate the molar mass of the reducing agent. hola 94
Transcribed Image Text:5. 2.6477 g of the reducing agent FeSO4 was titrated to the equivalence point with 17.25 mL of a KMNO4 solution. a. Calculate the molarity of the KMNO4 solution. ImolMhg 5 molFe = 0.20지 M Kn04 2.L477 FeS04 x L mol x 0.01725 L * b. What volume (in mL) of the KMNO4 solution would be needed to react with 12.50 grams of 30.0 % H2O2 solution? *6. In a redox titration, 12.52 mL of a 0.3264 M KMNO4 solution were required to titrate 1.7832 g of a reducing agent (“X"). If the reducing agent undergoes a 3-electron change per formula unit: Write the two ionic half reactions and the balanced net ionic equation. a. Mn Ouiaq) t 3e > 5MnO4 Ionic MnO4 : eid Ionic Reducing Agent: X X+ 3c= noutotoslq Net ionic: b. Calculate the molar mass of the reducing agent. hola 94
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