4. Preparation of M/10 Oxalic Acid Solution

4.1. Chemicals Required

• Oxalic acid ( H₂C₂O₄. 2H₂O)
• Distilled water
• Volumetric flask (250 mL)
• Weighing balance

4.2. Procedure

1. Weigh 6.3 g of oxalic acid dihydrate using a balance.
2. Transfer it to a 250 mL volumetric flask.
3. Add about 100 mL of distilled water and swirl to dissolve.
4. Make up the volume to 250 mL with distilled water.
5. Shake well to ensure uniformity.

The prepared solution is 0.1 M oxalic acid.

5. Titration of KMnO₄ with Oxalic Acid

5.1. Reaction Involved

The balanced redox reaction in acidic medium:

5.2. Tabular Observation

(Average volume of KMnO₄ used = XX.XX mL)

5.3. Calculation of KMnO₄ Molarity

Using the reaction: N₁V₁/N₂V₂ = (M₁x5)/(M₂ x 2)

where:

• N₁= M₁= Molarity of oxalic acid = 0.1 M
• V₁ = Volume of oxalic acid used (25 mL)
• N₂ = M₂= Molarity of KMnO₄ (to be determined)
• V₂= Average volume of KMnO₄ used (mL)

Solve for using the experimental value.

5.4. Calculation of g/L of KMnO₄

Molar mass of KMnO₄ = 158 g/mol

Thus, once is determined, multiply by 158 to get g/L of KMnO₄.

6. Conclusion

• Successfully prepared M/10 oxalic acid solution.
• Used it to titrate KMnO₄ solution and determined its molarity and g/L.
• The experiment verified the stoichiometry of the redox reaction.
• Chemical kinetics principles were applied in the reaction monitoring process.

7. Bibliography

1. Atkins, P. & de Paula, J. (2018). Physical Chemistry.
2. Vogel, A. I. (2000). Textbook of Quantitative Chemical Analysis.
3. Online sources on titration and redox reactions.