Because of time constraints, the following data has been collected for you. In a
ID: 910166 • Letter: B
Question
Because of time constraints, the following data has been collected for you. In a previous experiment, 0.800 g of the green complex iron salt was placed in an Erlenmeyer flask and heated with concentrated sulfuric acid until all oxalate ion was destroyed (CO2, SO2 and H2O are formed). Ferric ion (Fe3+) remained in solution and was reduced to Fe2+ by reaction with Al wire. The ferrous ion (Fe2+) was then titrated with KMnO4 solution according to equation (2) and 32.60 mL of 0.0100 M permanganate solution was required to reach the endpoint. The blank required 0.03 mL of the permanganate solution. Find the mass % of iron in the complex salt.
Explanation / Answer
what is equation 2
according to data the balance redox equation is
MnO4- + 8H+ + 5Fe2+ ---> 5Fe3+ + Mn2+ + 4H2O
and calculate mass % of iron in the complex salt
is 11.4%