Redox titration question? Determine the molarity of a solution? PLEASE HELP!!
Q1. Iron is often used to standardize permanganate solutions. A 0.158 g sample of pure iron wire was dissolved in dilute sulfuric acid to form a solution of iron (II) sulfate. This was titrated with 31.23 mL of a potassium permaganate solution. What is the molarity of the KMNO4 solution??
One equation provided to us was 2KMnO4 + 10FeSO4 + 8H2SO4 --> 2MnSO4 + 5Fe2(SO4)3 + K2SO4 + 8H20. I think I might be able to use it for this problem..
The second question is:
Q2. The above standardized KMnO4 solution was used to titrate the oxalic acid (H2C2O4, this is not a hydrate) in rhubarb leaves. A 12.38 g sample of rhubarb leaves was extracted with water and the resulting oxalic acid solution was titrated with 36.56 mL of the KMnO4 solution. What is the percent oxalic acid in the rhubarb.
Another equation provided to us which I think? might be useful is 2KMnO4 + 5H2C2O2 + 3H2SO4 --> 2MnSO4 + K2SO4 + 10CO2 + 8H2O
Can you please help me with this? I know I need a balanced equation and that this is a stoichiometry problem, but I am just stuck with the steps I need to take. In regards to the second question, the "this is not a hydrate" is throwing me off since it says it was extracted with water. Maybe that is insignificant.
I sincerely appreciate your help!!!!!!!!!