Acid Base Titrations...

Titration is define as the interaction of any two given chemical substances. Usually we take acid and base for studying titrations. Titrations of KMnO4  along with Oxalic Acid is one of the important titration reaction.
We could get volume of the substance used as well as the molarity , molality and normality.
 

Potassium permanganate, KMnO4, is a strong oxidizing agent. Permanganate, MnO4-, is an intense dark purple color. Reduction of purple permanganate ion to the colorless Mn+2 ion, the solution will turn from dark purple to a faint pink color at the equivalence point. No additional indicator is needed for this titration. The reduction of permanganate requires strong acidic conditions.

In this experiment, permanganate will be reduced by oxalate, C2O42- in acidic conditions. Oxalate reacts very slowly at room temperature so the solutions are titrated hot to make the procedure practical. The unbalance redox reaction is shown below.

MnO4- + C2O42- → Mn2+ + CO2 (acidic solution)

In part I of this experiment, a potassium permanganate solution will be standardized against a sample of potassium oxalate. Once the exact normality (eq/L) of the permanganate solution is determined, it can be used as a standard oxidizing solution. In part II of this experiment, the standard permanganate solution will be used to find the concentration of iron(II) in a ferrous solution (g/L). The unbalanced redox reaction is shown below.

MnO4- + Fe2+ → Mn2+ + Fe3+ (acidicsolution)
Phosphoric acid will be used to ensure that the ferric product, Fe3+ remains in its colorless form. 

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