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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: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.98QE
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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- + 14H+ 6Fe³+ + 2Cr³+ + 7H₂O ( a. 113 b. 138 C 166 d. 183 e 160 1
Transcribed Image Text: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- + 14H+ 6Fe³+ + 2Cr³+ + 7H₂O ( a. 113 b. 138 C 166 d. 183 e 160 1
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