A 100.0 mL water sample was mixed with 25.00 mL of 0.002517 M K₂Cr₂O7 (294.2 g/mol) to oxidize Fe²* to Fe³+ The excess K₂Cr₂O7 was back-titrated with 5.30 mL of 0.00949 M Fe²+ on Calculate the concentration of Fe (55.8 g/mol) in the sample in parts per million. + Cr₂O7²- + 14H6Fe³+ + 2Cr³+ + 7H₂O a. 113 b. 138 c 166 d. 183 e 160

A 100.0 mL water sample was mixed with 25.00 mL of 0.002517 M K₂Cr₂O7 (294.2 g/mol) to oxidize Fe²* to Fe³+ The excess K₂Cr₂O7 was back-titrated with 5.30 mL of 0.00949 M Fe²+ on Calculate the concentration of Fe (55.8 g/mol) in the sample in parts per million. + Cr₂O7²- + 14H6Fe³+ + 2Cr³+ + 7H₂O a. 113 b. 138 c 166 d. 183 e 160

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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