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
To calculate the mass of FeSO4.7H2O dissolved in one liter of solution, we need to use the stoichiometry of the reaction between KMnO4 and FeSO4.7H2O.
The balanced chemical equation for the reaction is:
2MnO4- + 5Fe2+ + 8H+ → 2Mn2+ + 5Fe3+ + 4H2O
From the equation, we can see that the ratio between KMnO4 and FeSO4.7H2O is 2:5. Therefore, we need to determine how much KMnO4 is decolorized in order to determine the amount of FeSO4.7H2O.
Given that the potassium permanganate solution contains 1.58g of KMnO4 per liter, we need to calculate the moles of KMnO4 added.
The molar mass of KMnO4 is:
Molar mass of K = 39.10 g/mol
Molar mass of Mn = 54.94 g/mol
Molar mass of O = 16.00 g/mol (4 atoms)
Total molar mass of KMnO4 = 39.10 + 54.94 + (16.00 × 4) = 158.04 g/mol
To find the moles of KMnO4:
Moles of KMnO4 = mass of KMnO4 / molar mass of KMnO4
Moles of KMnO4 = 1.58 g / 158.04 g/mol
Now, we can determine the moles of FeSO4.7H2O using the ratio from the balanced chemical equation.
From the equation, the ratio of KMnO4 to FeSO4.7H2O is 2:5. This means that for every 2 moles of KMnO4, there are 5 moles of FeSO4.7H2O.
Moles of FeSO4.7H2O = (moles of KMnO4 × 5) / 2
Finally, we can calculate the mass of FeSO4.7H2O in one liter of solution.
Mass of FeSO4.7H2O = Moles of FeSO4.7H2O × Molar mass of FeSO4.7H2O
The molar mass of FeSO4.7H2O can be calculated as follows:
Molar mass of Fe = 55.85 g/mol
Molar mass of S = 32.06 g/mol
Molar mass of O = 16.00 g/mol (4 atoms)
Total molar mass of FeSO4.7H2O = (55.85 + 32.06 + (16.00 × 4) + (16.00 × 7)) g/mol
Substituting the values into the formula, you can calculate the mass of FeSO4.7H2O dissolved in one liter of solution.