Redox Titrations:
a. write 2-3 sentences describing and identifying the type of chemical reaction that occurs when Fe2+ reacts with potassium permanganate (KMnO4) and specifying the type of solution for the reaction to occur.
b. using a standard reduction potential table, identify the oxidation and reduction half-reactions for the reaction.
c. write the balanced net ionic equation for the reaction, and identify which substance is oxidized and which is reduced.
d. Suppose at the endpoint of the reaction 0.030 moles of KMnO4 were added to the analyte. How many moles of Fe2+ were contained in the beaker?
This is urgent! I really need help with this. I have no idea where to even begin. Thank you!!
Would it just be a redox reaction for part a?
Redox Titrations:
a. write 2-3 sentences describing and identifying the type of chemical reaction that occurs when Fe2+ reacts with potassium permanganate (KMnO4) and specifying the type of solution for the reaction to occur.
I don't know why you need more than one word to describe a redox reaction. These titrations with ferrous and permangante usually are carried out in an acidic solution
b. using a standard reduction potential table, identify the oxidation and reduction half-reactions for the reaction.
The obvious place to start here is to look up the standard reduction potentials. The oxidation half is the more negative of the two.
c. write the balanced net ionic equation for the reaction, and identify which substance is oxidized and which is reduced.
5Fe^2+ MnO4^- + 8H^+ ==> 5Fe^3+ + 4H2O + Mn^2+
You add the phases if that is required.
d. Suppose at the endpoint of the reaction 0.030 moles of KMnO4 were added to the analyte. How many moles of Fe2+ were contained in the beaker?
Do you mean it took 0.030 mols KMnO4 to reach the end point. If so then 0.030 mols KMnO4 x (5 mols Fe^2+/1 mol KMnO4) = ?
Post your work if you have other questions about this.