1. A sample of iron ore weighing 0.6428 g is dissolved in acid The iron is reduced to Fe*2 and titratedwith 36.30 mL of a 0.1052 N solution of K2Cr207. (a) Calculate the percentage of iron (Fe) in thesample. (b) Express the percentage as Fe,03 rather than Fe.Hint: The reaction of Fe2+ with Cr,0,2 involves one electron to oxidize it to Fe*.

1. A sample of iron ore weighing 0.6428 g is dissolved in acid The iron is reduced to Fe* and titrated with 36.30 mL of a 0.1052 N solution of K,Cr207. (a) Calculate the percentage of iron (Fe) in the sample. (b) Express the percentage as Fe203 rather than Fe. Hint: The reaction of Fe2+ with Cr20,2 involves one electron to oxidize it to Fe*.

1. A sample of iron ore weighing 0.6428 g is dissolved in acid The iron is reduced to Fe* and titrated with 36.30 mL of a 0.1052 N solution of K,Cr207. (a) Calculate the percentage of iron (Fe) in the sample. (b) Express the percentage as Fe203 rather than Fe. Hint: The reaction of Fe2+ with Cr20,2 involves one electron to oxidize it to Fe*.

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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