To determine the amount of iron present in steel.
Standard oxalic acid solution (0.1N), potassium permanganate solution (0.1N) and dilute sulphuric acid (2N).
The steel sample is dissolved in dilute sulphuric acid, which converts the iron present in it to ferrous sulphate with the liberation of hydrogen gas.
The amount of Fe2+ present in a solution can be determined by titrating against a standard potassium permanganate solution.
Clean a burette initially with tap water and then rinse it with distilled water as well as potassium permanganate solution. Then, fill it with the potassium permanganate solution and note down the initial reading. Pipette out 10 ml of the standard oxalic acid solution into a 250 ml conical flask. Add 10 ml of dilute sulphuric and heat the solution to about 70°C. Then, titrate this solution slowly against the potassium permanganate solution from the burette until a faint but permanent pink colour persists in the solution. Repeat the titration until consecutive concordant values are obtained. Note down the values in a tabular column and calculate the normality of the potassium permanganate solution.
Dissolve 1 g of steel completely in 100 ml of dilute sulphuric acid and transfer the solution quantitatively into a 250 ml standard flask. Make up the volume to 250 ml by adding distilled water and shake the solution thoroughly. Pipette out 25 ml of the solution into a clean conical flask. Add 10 ml of dilute sulphuric acid and titrate against the potassium permanganate solution taken in the burette. The appearance of a permanent pink colour is the end point of titration. Repeat the titration until concurrent readings are obtained.
1 ml of 0.1N potassium permanganate = 5.585 mg of iron.
Amount of iron present in 250 ml of the solution prepared from 1 g of steel = _____ g.
52.15.80.101