Chemistry, 28.02.2021 17:00 leslie1811
An ore is to be analyzed for its iron content by an oxidation-reduction titration with permanganate ion. A 4.230 g sample of the ore is dissolved in hydrochloric acid and passed over a reducing agent so that all the iron is in the form Fe2+. The Fe2+ (aq) is completely oxidized by 31.60 mL of a 0.05120 M solution of KMnO4. The unbalanced equation for the reaction is:
KMnO4(aq) + HCl(aq) + FeCl(aq) ---> MnCl(aq) + FeCl3(aq) + H2O(1)
the balanced equation is:
8H+ + MnO4 + 5Fe2+ â Mn2+ + 5Fe3+ + 4H2O
Required:
Calculate the amount of iron in the sample and its mass percentage in the ore.
Answers: 1
Another question on Chemistry
Chemistry, 21.06.2019 22:30
Check the correct box to describe the periodic trends in electronegativity. electronegativity across a period: decreases. increases. electronegativity down a group: decreases. increases.
Answers: 2
Chemistry, 22.06.2019 00:30
Water (2510 g ) is heated until it just begins to boil. if the water absorbs 5.09×105 j of heat in the process, what was the initial temperature of the water?
Answers: 3
Chemistry, 22.06.2019 21:00
Which property of water causes water drops to bead on a freshly waxed car?
Answers: 2
You know the right answer?
An ore is to be analyzed for its iron content by an oxidation-reduction titration with permanganate...
Questions
