Stoichiometry of a RedOx Reaction. (I)
Iron(II) ion, reacts with permanganate ion, in acidic solution to produce iron(III) ion and manganese(II) ion.
If exactly 60.0 mL of an Fe2+ solution is required to react completely with 75.0 mL of a 0.0950 M permanganate solution, what is the molarity of the Fe2+ solution?
2007-09-28 08:46:44 · 2 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
The balanced equation is
5 Fe2+ + MnO4- + 8H+ --> 5 Fe3+ + Mn2+ + 4H2O
Moles permanganate = 75.0 x 0.0950 / 1000 = 0.00713
The ratio between Fe2+ and MnO4- is 5 : 1
5 : 1 = x : 0.00713
x = moles Fe2+ = 0.0356
M = moles / L
V = 60.0 mL = 0.0600 L
M = 0.0356 / 0.0600 = 0.594 M
2007-09-28 08:56:08 · answer #1 · answered by Dr.A 7 · 1⤊ 0⤋
Mole ratio is 1:5 (you need to write the balanced equation).
So the moles of Fe2+ are 5 x 75/1000 x 0.950 moles.
Now multiply this by 1000/60 for your final answer.
2007-09-28 15:52:54 · answer #2 · answered by Gervald F 7 · 1⤊ 0⤋