molarity of kmno4 and strength of kmno4 in M/25 solution experiment of oxalic acid.......
You need to provide adequate information if you want answers.
To find the molarity and strength of KMnO4 in a M/25 solution experiment of oxalic acid, follow these steps:
Step 1: Determine the balanced chemical equation for the reaction between oxalic acid and KMnO4. In this case, it is:
5H2C2O4 + 2KMnO4 + 3H2SO4 -> 2MnSO4 + 10CO2 + 8H2O + K2SO4
Step 2: Calculate the stoichiometry of the reaction. From the balanced equation, you can see that 2 moles of KMnO4 react with 5 moles of H2C2O4.
Step 3: Determine the volume of oxalic acid used in the experiment. Suppose you used V ml of oxalic acid solution.
Step 4: Convert the volume of oxalic acid to moles using its molarity. Let the molarity of oxalic acid be Mox.
Number of moles of oxalic acid = Mox * V / 1000 (convert ml to liters)
Step 5: Since the reaction is 2:5 for KMnO4 and H2C2O4, the number of moles of KMnO4 will be (2/5) times the moles of oxalic acid.
Number of moles of KMnO4 = (2/5) * (Mox * V / 1000)
Step 6: Divide the number of moles of KMnO4 by the volume used in the experiment to get the molarity of KMnO4.
Molarity of KMnO4 = (2/5) * (Mox * V / 1000) / (V / 1000)
Simplifying, you get:
Molarity of KMnO4 = 2 * Mox / 5
Step 7: The strength of the KMnO4 solution is the molarity multiplied by its equivalent weight. The equivalent weight of KMnO4 is 158 g/equivalent.
Strength of KMnO4 = Molarity of KMnO4 * Equivalent weight of KMnO4
So, the strength of the KMnO4 solution in M/25 experiment of oxalic acid can be calculated using the above formula.
To determine the molarity and strength of a KMnO4 solution in an experiment involving oxalic acid, you can follow the steps below:
1. Obtain the balanced chemical equation for the reaction between KMnO4 and oxalic acid. This will help you understand the stoichiometry of the reaction.
2. Prepare a standard solution of oxalic acid. This solution should have a known concentration, for example, 0.1 M.
3. Take a known volume, V1, of the oxalic acid solution. Measure this volume accurately using a graduated cylinder or a pipette.
4. Add an indicator to the oxalic acid solution. In this case, you can use a suitable indicator that changes color when the reaction is complete, such as phenolphthalein.
5. Begin adding the KMnO4 solution to the oxalic acid solution slowly, while stirring continuously. The KMnO4 solution should also have a known concentration, for example, M/25 (meaning one-twenty-fifth of 1 M).
6. Observe the color change of the reaction mixture as you add the KMnO4 solution. Initially, the oxalic acid will react with the KMnO4, causing the color to change. Once the reaction is complete, the color will remain constant. This is known as the "end point" of the titration.
7. Record the volume, V2, of the KMnO4 solution required to reach the end point of the reaction.
8. Calculate the molarity (C2) of the KMnO4 solution using the formula: C2 = (C1 * V1) / V2, where C1 is the molarity of the oxalic acid solution, V1 is the volume of oxalic acid used, and V2 is the volume of KMnO4 solution required.
9. The "strength" of the KMnO4 solution refers to the amount of KMnO4 present in a given volume. Since the molarity (C2) of the KMnO4 solution is now known, you can calculate its strength by multiplying the molarity by the molecular weight of KMnO4.
For example, if the molarity is found to be 0.025 M (M/25) and the molecular weight of KMnO4 is 158.04 g/mol, then the strength would be 0.025 M * 158.04 g/mol = 3.951 g/L.
Remember, accuracy in measurements and proper technique is crucial in obtaining accurate results.