Suppose 1.624g of salt FeSO4 is placed in a 250mL flask to which 50mL of water and 10 mL of 3M H2SO4 are added. How many mL of .1062 M KMnO4 solution are required to reach the endpoint?

first step is to convert all measurements to moles.

Then consult your equation to figure amounts of moles per reagent.

What about the mL of water and H2SO4

water is 0M H2SO4

10mL of 3M contains 0.03 moles H2SO4

To determine the amount of .1062 M KMnO4 solution required to reach the endpoint, we need to perform a titration calculation. Let me guide you through the steps:

Step 1: Write the balanced chemical equation for the reaction between FeSO4 and KMnO4. The reaction occurs in an acidic medium, as indicated by the presence of H2SO4:

5FeSO4 + 2KMnO4 + 8H2SO4 → 5Fe2(SO4)3 + K2SO4 + 2MnSO4 + 8H2O

Step 2: Calculate the moles of FeSO4 used. We are given the mass of FeSO4 (1.624 g), so we need to convert it to moles using the molar mass of FeSO4. The molar mass of FeSO4 is:
(1x 55.85 g/mol [Fe]) + (1 x 32.07 g/mol [S]) + (4 x 16.00 g/mol [O]) = 151.91 g/mol

1.624 g FeSO4 x (1 mol FeSO4 / 151.91 g FeSO4) = 0.0107 moles FeSO4

Step 3: Calculate the moles of KMnO4 needed. From the balanced equation, the stoichiometry between KMnO4 and FeSO4 is 2:5. Therefore, the moles of KMnO4 required is:

(0.0107 moles FeSO4) x (2 moles KMnO4 / 5 moles FeSO4) = 0.00428 moles KMnO4

Step 4: Calculate the volume of the .1062 M KMnO4 solution required. We can use the formula:

Moles = Concentration x Volume

(0.00428 moles KMnO4) = (0.1062 M KMnO4) x Volume (in liters)

Volume (in liters) = (0.00428 moles KMnO4) / (0.1062 M KMnO4)
Volume (in liters) = 0.04028 L

Step 5: Convert the volume to milliliters:

Volume (in mL) = 0.04028 L x (1000 mL / 1 L)
Volume (in mL) = 40.28 mL

Therefore, approximately 40.28 mL of the 0.1062 M KMnO4 solution is required to reach the endpoint.