Final answer:
To find the molarity of the FeSO4 solution, we use the molarity and volume of KMnO4, apply the stoichiometry from the chemical equation, and calculate the moles of Fe2+ reacted. Dividing the moles of Fe2+ by the volume of the FeSO4 solution gives us the concentration which should be checked if there's an error due to mismatching answer choices.
Step-by-step explanation:
To determine the concentration of the FeSO4 solution, we need to use the molarity of the KMnO4 solution and the volumes of both solutions along with the stoichiometry of the reaction. We are given a volume of 16.42 mL (0.01642 L) of 0.1327 M KMnO4 and a volume of 20.00 mL (0.02000 L) of FeSO4. The net ionic equation provided is 5Fe2+ + MnO4- + 8H+ → Mn2+ + 5Fe3+ + 4H2O, which indicates a 5:1 stoichiometric ratio between Fe2+ and MnO4-.
First, calculate the moles of KMnO4 using its concentration and volume:
Moles of KMnO4 = Molarity × Volume = 0.1327 M × 0.01642 L = 0.0021791 moles
Since the stoichiometry is 5:1, the moles of Fe2+ that react will be 5 times the moles of KMnO4.
Moles of Fe2+ = 5 × Moles of KMnO4 = 5 × 0.0021791 = 0.0108955 moles
Finally, to find the concentration of the FeSO4 solution, divide the moles of Fe2+ by the volume of the FeSO4 solution in liters:
Concentration of FeSO4 = Moles of Fe2+ / Volume of FeSO4 solution = 0.0108955 moles / 0.02000 L = 0.544775 M
However, none of the answer options match this value. It seems there might be an error in the given answer choices or in the calculations. Re-check the calculations for any mistakes.