Redox titration-potassium permanganate as oxidant, Chemistry tutorial


If we remind in chapter 7, one of the acid - base titrations we executed, was the determination of the percentage purity of a substance. In the demonstration of a alike applicability to redox reactions, we shall in this practical laboratory class attempt to find out the percentage purity of a reductant, FeSO4.7H7O. This we will do via titrating against the standardized solution of potassium permanganate.


Determination of the concentrations of a solution of FeSO4.7H2O using a standard solution of potassium permanganate.



Apparatus                                   Quantity

KMnO4 solution

2M H2SO4

FeSO4 .7H2O

Distilled water

Burette (50cm3)

Pipette (25cm3)

Bunsen burner

Wire Gauze

Tripod stand


Conical flask (25cm3)









1. Rinse the burette (50.0cm3) twice with a few cm3 of KMnO4 solution. Fill the burette with the KMnO4 solution above the Zero mark and drain to this mark, making sure the burette tip is full and any air is ejected within the body of the KMnO4 solution.

2. Pipette out 25.0cm3 of the solution of FeSO4.7H20 into a 250cm3conical flask and add to it 20cm3 of 2moldm-3 sulphuric acid. Heat to between 60 and 80°c.

3. Titrate the hot mixture through KMnO4 from the burette until the solution in the conical flask attains a permanent faint pink colour.

4. Recur the titration using fresh samples each time until at least 2 titrations are within 0.2cm3   accuracy.

5 Record your titre values using the format in earlier experiments and discover the average titre value.

6 From us consequences, determine

a The number of moles of potassium permanganate utilized in the solution.

b The number of moles of the iron compound.

c The concentration in moldm-3 of the iron compound

d The percentage purity of the crystals.

(Mn = 55, K = 39, 0 =16, C=12, H = 1, N =14, 5

S = 32, Fe =56)


Burette Reading

lst   titration

2nd   titration

3rd  titration

Final reading




Initial Readings




Volume of KMnO4





Treatment of Results

Step 1: The equation of the reaction

MNO-4(aq) + Fe2+ (aq) + 8H (aq)          Mn 2+ (aq ) + 4H2O

Step 2. We shall assume the followings:

1. The permanganate solution used is the standardized solution from the earlier experiment.

2. The amount in moldm-3 of the KMnO4 is 0.002  moldm-3.  

3. The average titre value for KMnO4 is Wcm3 .

4. The FeSO4.7H2O solution was prepared in dissolving about 7.6g of the crystals in 250cm3 of solution.

Step3. The number of moles MnO = Molarity x (volume).W/ 1000

=W x 0.02 /1000

= M moles

Step4. Find the number of moles of the iron II crystals from the stoichimetric equation of the reaction

1 mole MnO4.5 moles Fe2+(aq )

M mole MnO4   = 5 x M mole Fe2+ (aq)

                         = 5 M mole in 25cm3

Step 5.The number in moles dm-3 of the Fe2+    

= No of mole x 1000 / Volume

= 5M x 1000 / 25

= 200M molesdm-3  

Step6. The mass Concentration of the FeSO4.7H2O

 Mass concentration    = moldin-3 x molar Mass

                                    = 20M x 278gdm-3  

                                    = 5560Mgdm-3  

                                    = Ngdm-3  

Step7. Estimate the percentage purity of the iron salt

Percent purity = mass determined during experiment / Actual mass of iron in 100cm3  

= Ngdm-3 x 100 / 4 x 7.6

= q%.

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