Final answer:
To find the mass of FeCl2 in the sample, calculate the moles of KMnO4 using its molarity and volume, use the stoichiometry of the balanced equation to find the moles of FeCl2, and then convert these moles to mass using the molar mass of FeCl2.
Step-by-step explanation:
The student is asking how to find the mass of iron(II) chloride (FeCl2) in a sample given the volume and molarity of a potassium permanganate (KMnO4) solution used to titrate the FeCl2 to the end point. This is a stoichiometry problem involving a redox titration reaction.
We need to use the provided volume and molarity of the KMnO4 solution to find the number of moles of KMnO4, which will then tell us the moles of FeCl2 due to the stoichiometry of the balanc10ed equation. After finding the moles of FeCl2, we can calculate the mass of FeCl2 using its molar mass.
The calculation goes as follows: First, calculate the moles of KMnO4 using its molarity and the volume used (29.16 mL = 0.02916 L):
Moles KMnO4 = 0.02916 L × 0.1124 mol/L = 0.003277 Moles KMnO4
Then, use the stoichiometry of the balanced equation (which typically requires balancing the redox reaction to determine) to find the moles of FeCl2. Assuming the reaction is 1 mole of KMnO4 to 5 moles of FeCl2 (as an example), we multiply the moles of KMnO4 by the mole ratio to get the moles of FeCl2:
Moles FeCl2 = 0.003277 Moles KMnO4 × (5 moles FeCl2 / 1 mole KMnO4)
Lastly, convert these moles to mass:
Mass FeCl2 = Moles FeCl2 × Molar Mass FeCl2
This will give the mass of FeCl2 in the sample. The specific molar mass value of FeCl2 should be used to complete the calculation.