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
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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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![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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F00dfa9a6-2135-456b-a954-559b7173c7cf%2F43722370-7993-4c1d-82d0-9e6ed04f57e2%2Fftwzvpq_processed.jpeg&w=3840&q=75)
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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