A 110.0-mL sample of spring water was treated to convert any iron present to Fe²⁺. Addition of 25.00 mL of 0.002525 M K₂Cr₂O₇ resulted in the reaction:\[ 6\text{Fe}^{2+} + \text{Cr}_2\text{O}_7^{2−} + 14\text{H}^+ \rightarrow 6\text{Fe}^{3+} + 2\text{Cr}^{3+} + 7\text{H}_2\text{O} \]The excess K₂Cr₂O₇ was back-titrated with 8.05 mL of 0.00951 M Fe²⁺ solution. Calculate the concentration of iron in the sample in parts per million.**Concentration of iron = [blank] ppm**

A 110.0-mL sample of spring water was treated to convert any iron present to Fe2+. Addition of 25.00-mL of 0.002525 M K2 Cr2 O, resulted in the reaction 6Fe?+ + Cr2O,²- + 14H+ → 6Fe³+ + 2Cr³+ + 7H2O The excess K2Cr2O7 was back-titrated with 8.05 mL of 0.00951 M Fe²+ solution. Calculate the concentration of iron in the sample in parts per million. Concentration of iron= ppm

A 110.0-mL sample of spring water was treated to convert any iron present to Fe2+. Addition of 25.00-mL of 0.002525 M K2 Cr2 O, resulted in the reaction 6Fe?+ + Cr2O,²- + 14H+ → 6Fe³+ + 2Cr³+ + 7H2O The excess K2Cr2O7 was back-titrated with 8.05 mL of 0.00951 M Fe²+ solution. Calculate the concentration of iron in the sample in parts per million. Concentration of iron= ppm

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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