Asked by mohd
A 1.362 g sample of an iron ore that contained Fe_3O_4 was dissolved in acid and all the iron was reduced to Fe^2+. the solution was then acidified with H_2SO_4 and titrated with 39.42 mL of 0.0281 M KMnO_4 , which oxidized the iron to Fe^3+.
Net ionic equation
5Fe^(2+)+MnO_4^-+8H^+→5Fe^(3+)+Mn^(2+)+4H_2O
a) what was the percentage by mass of iron in the ore?
b) what was the percentage by mass of Fe_3O_5 in the or
Net ionic equation
5Fe^(2+)+MnO_4^-+8H^+→5Fe^(3+)+Mn^(2+)+4H_2O
a) what was the percentage by mass of iron in the ore?
b) what was the percentage by mass of Fe_3O_5 in the or
Answers
Answered by
Damon
There is a chemist around but how would he know to read this?
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.