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A 1.012-g sample of a salt containing Fe2+ is titrated
Chapter 16, Problem 102P(choose chapter or problem)
Problem 102P
A 1.012-g sample of a salt containing Fe2+ is titrated with 0.1201 M KMnO4. The end point of the titration is reached at 22.45 mL. Find the mass percent of Fe2+ in the sample. The unbalanced redox reaction that occurs in acidic solution during the titration is:
Fe2+(aq) + MnO4− (aq) → Fe3+(aq) + Mn2+ (aq)
Questions & Answers
QUESTION:
Problem 102P
A 1.012-g sample of a salt containing Fe2+ is titrated with 0.1201 M KMnO4. The end point of the titration is reached at 22.45 mL. Find the mass percent of Fe2+ in the sample. The unbalanced redox reaction that occurs in acidic solution during the titration is:
Fe2+(aq) + MnO4− (aq) → Fe3+(aq) + Mn2+ (aq)
ANSWER:
Solution 102 P:
Here, we are going to calculate the mass percent of Fe2+ in the sample.
Step 1:
The balanced equation for the redox reaction is
5Fe2+(aq) + MnO4− (aq) +8H+(aq) → 5Fe3+(aq) + Mn2+ (aq) + 4H2O(l)