Ferrous sulphate can be determined by titration using a standard solution of potassium permanganate. The reaction between ferrous sulphate and potassium permanganate produces manganese dioxide, which can be quantified using a redox titration. Here is a step-by-step procedure for ferrous sulphate titration:
- Preparation of Standard Potassium Permanganate Solution:A standard solution of potassium permanganate can be prepared by accurately weighing about 0.1 g of potassium permanganate and dissolving it in a volumetric flask containing a known volume of distilled water. The resulting solution should be approximately 0.01 M.
- Preparation of Ferrous Sulphate Solution:A solution of ferrous sulphate can be prepared by accurately weighing about 0.1 g of ferrous sulphate and dissolving it in a known volume of distilled water. This solution will be used as the analyte in the titration.
- Preparation of Acid Solution:An acid solution, such as sulfuric acid, can be prepared by adding a few drops of sulfuric acid to a small volume of distilled water.
- Titration:
- Fill a burette with the standard potassium permanganate solution.
- Add 5-10 mL of the ferrous sulphate solution to a conical flask.
- Add a few drops of the acid solution to the flask to adjust the pH.
- Add a few drops of a suitable indicator, such as phenolphthalein, to the flask. The indicator should be pink in an acidic solution and colourless in an alkaline solution.
- Titrate the ferrous sulphate solution with the potassium permanganate solution from the burette until a permanent colour change to pink is observed. This indicates the end-point of the reaction.
- Record the volume of potassium permanganate solution required to reach the end-point.
- Calculation:The amount of ferrous sulphate in the analyte solution can be calculated using the following equation:
Moles of ferrous sulphate = Moles of potassium permanganate
The moles of potassium permanganate can be calculated using the concentration of the standard solution and the volume used in the titration.
Example Calculation:
Suppose a 0.1 g sample of ferrous sulphate was titrated with 0.01 M potassium permanganate solution, and it took 0.05 L of the standard solution to reach the end-point. The moles of potassium permanganate used in the titration can be calculated as follows:
Moles of potassium permanganate = (0.01 M) x (0.05 L) = 0.0005 moles
Therefore, the moles of ferrous sulphate in the sample are equal to 0.0005 moles.
In conclusion, the ferrous sulphate titration procedure is a simple and effective way to determine the amount of ferrous sulphate in a sample. By carefully following the steps outlined above and using accurate measurements, accurate results can be obtained.
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