A potassium permanganate solution containing 1.58g of KMnO4 per liter is added into 5 ml of an acidified iron (||) sulfate solution. Decolorizing of KMnO4 solution has been added .Calculate the mass of FeSo4.7H2O which has been dissolved in one liter of solution.
mols KMnO4 = grams/molar mass
M = mols/L.
5Fe^2+ + MnO4^- ==> 5Fe^3+ + Mn^2+
mols KMnO4 used = M x L. You don't show L KMnO4. Without that you can't finish the problem.
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To calculate the mass of FeSO4·7H2O dissolved in one liter of the solution, we need to use a balanced chemical equation and information about the reaction that occurred between the potassium permanganate (KMnO4) and iron (||) sulfate (FeSO4) in the solution. The balanced equation for this reaction is:
5 FeSO4 + 2 KMnO4 + 8 H2SO4 -> 5 Fe2(SO4)3 + 2 MnSO4 + K2SO4 + 8 H2O
From the equation, we can see that the stoichiometric ratio of FeSO4 to KMnO4 is 5:2. Therefore, we can set up a proportion to calculate the mass of FeSO4·7H2O that has been dissolved in one liter of solution.
Let x be the mass of FeSO4·7H2O dissolved in one liter of solution.
1.58 g KMnO4 x g FeSO4·7H2O
-------------- = -------------------
1 L solution 5 g FeSO4
Solving the proportion:
1.58 g KMnO4 * 5 g FeSO4 = x g FeSO4·7H2O * 1 L solution
---------------------------------
1 L solution
(1.58 * 5) / 5 = x
x = 1.58 g
Therefore, the mass of FeSO4·7H2O dissolved in one liter of solution is 1.58 grams.