Prelab questions

1. Using the net ionic equation given in the introduction of the lab apply the mole ratio of Fe2+ ions to MnO₄- ions.

2. Again using the net ionic equation given in the introduction calculate the grams of Fe in the sample and the percentage of the iron in the sample.

36.44mL x 0.0244 M KMnO₄ = ____mol of KMnO₄

____mol of KMnO₄ x mole ratio of MnO₄^- to Fe²⁺ = _____ mol Fe²⁺

____ mol Fe²⁺ x 55.85 g/mol Fe²⁺ = _____ g Fe²⁺

_____ g Fe²⁺/1.923g x 100% = ____ % Fe in sample

3. To find the percentage of iron in iron II ammonium sulfate hexahydrate you need to add the molar masses fo the iron II ammonium sulfate hexahydrate. Take the molar mass of iron and divide it by the mass of the iron II ammonium sulfate hexahydrate and multiply by a 100%. I will let you figure out the formula from the name. Hint you have 7 waters.