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A 240.0-mL sample of spring water was treated to convert any iron present to Fe2+. Addition...

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Chemistry

A 240.0-mL sample of spring water was treated to convert anyiron present to Fe2+. Addition of 27.00-mL of 0.002520 MK2Cr2O7 resulted in thereaction

6Fe2+ + Cr2O72- +14H+ ----> 6Fe3+ + 2Cr3+ +7H2O

The excess K2Cr2O7 wasback-titrated with 8.80 mL of 0.00936 M Fe2+ solution.Calculate the concentration of iron in the sample in parts permillion.

Concentration of iron = _______ ppm?

Answer & Explanation Solved by verified expert
3.9 Ratings (551 Votes)
The balanced Redox reaction between Fe2 and dichromate in acidic medium is 6 Fe2 Cr2O72 14 H 6 Fe3 2 Cr3 7 H2O Number of moles of Cr2O72 initially added MV 0002520 M    See Answer
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