a mixture of oxalic nd sulphuric acid gave following titrimetric results..1.)25ml of solution=16.25ml of NaOH solution

2.)25ml of solution warmed =17.50ml of 0.1N KMnO4 solution in presece of acid

To analyze the titrimetric results from your mixture of oxalic and sulfuric acids, we need to break down the data you've provided. The results indicate two different titrations: one with sodium hydroxide (NaOH) and the other with potassium permanganate (KMnO4). Each of these titrations gives us valuable information about the concentrations of the acids in your mixture.

Understanding the Titration Results

The first result shows that 25 mL of your acid solution reacts with 16.25 mL of NaOH. This titration is likely measuring the amount of oxalic acid present, as it is a diprotic acid that reacts with NaOH in a 1:2 molar ratio. The balanced equation for this reaction is:

• Oxalic Acid (H2C2O4) + 2 NaOH → Na2C2O4 + 2 H2O

From this reaction, we can determine the moles of oxalic acid in the solution. If we assume the NaOH solution is 0.1 N (normality), we can calculate the moles of NaOH used:

• Moles of NaOH = Volume (L) × Normality = 0.01625 L × 0.1 N = 0.001625 moles

Since it takes 2 moles of NaOH to neutralize 1 mole of oxalic acid, the moles of oxalic acid in 25 mL of the solution would be:

• Moles of H2C2O4 = 0.001625 moles NaOH / 2 = 0.0008125 moles

Analyzing the Second Titration

The second result indicates that 25 mL of the acid solution reacts with 17.50 mL of 0.1 N KMnO4. In acidic conditions, KMnO4 acts as a strong oxidizing agent and can oxidize oxalic acid to carbon dioxide. The balanced equation for this reaction is:

• 5 H2C2O4 + 2 KMnO4 + 6 H2SO4 → 10 CO2 + 2 MnSO4 + 8 H2O + K2SO4

From this equation, we see that 5 moles of oxalic acid react with 2 moles of KMnO4. First, we calculate the moles of KMnO4 used:

• Moles of KMnO4 = Volume (L) × Normality = 0.01750 L × 0.1 N = 0.00175 moles

Using the stoichiometry from the balanced equation, we can find the moles of oxalic acid that reacted:

• Moles of H2C2O4 = (5 moles H2C2O4 / 2 moles KMnO4) × 0.00175 moles KMnO4 = 0.004375 moles

Calculating Concentrations

Now, we can calculate the concentration of oxalic acid in the original 25 mL solution. Since we have two different calculations for the moles of oxalic acid, we can average them or use them to confirm consistency. The first titration gave us 0.0008125 moles, while the second gave us 0.004375 moles. This discrepancy suggests that the first titration may not have accounted for all the oxalic acid present, or there may be an error in the measurements.

To find the concentration of oxalic acid in the solution, we can use the formula:

• Concentration (M) = Moles / Volume (L)

Assuming the average moles of oxalic acid is around 0.0026 moles (the average of the two results), the concentration would be:

• Concentration = 0.0026 moles / 0.025 L = 0.104 M

Final Thoughts

This analysis provides a comprehensive view of the titrimetric results from your mixture of oxalic and sulfuric acids. By understanding the stoichiometry of the reactions involved, we can derive meaningful insights into the concentrations of the acids in your solution. If you have any further questions or need clarification on any specific point, feel free to ask!