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We make an approximately 0.04 M solution of KMnO4 . We dissolve 500 mg of primary standard of sodium oxalate in 250 ml of water and use this to standardize. A volume of 39.07 ml is required to titrate the standard solution. What is the actual concentration of MnO4- ?

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Related questions

You standardize a solution of KMnO4 by titration with a solutionof oxalic acid. You weight out 1.378g H2C2O4ร‚ยท2H2O and dissolve itwith deionized water in a 25.00 mL volumetric flask.

1. What is the molarity of this oxalic acid solution?
2. What is the balanced overall net-ionic equation for the reactionbetween oxalic acid and the permanganate ion, MnO4-?
3. What is the molarity of the KMnO4 solution if it requires 15.42mL of KMnO4 solution to reach the endpoint in a titration with10.00 mL of the oxalic acid solution?

I. Standardization of KMNO4 solution

Procedure:

Add 0.010 g samples of sodium oxalate (Na2C2O4) to separate Erlenmeyer flasks. In each flask put 30 mL DI H2O, 1.0 mL 9 M sulfuric acid (H2SO4), and 2 drops of 0.1 M manganese (II) sulfate (MnSO4). Use a graduated pipet with 0.02 M KMnO4 to titrate each solution.

Mass Na2C2O4- Sample 1: 0.010 g , Sample 2: 0.010 g , Sample 3: 0.010 g

Volume KMnO4- Sample 1: 1.35 mL , Sample 2: 1.42 mL , Sample 3: 1.39 mL --- this is the amount of KMnO4 that was used to turn solution a faint pink color

From this data:

*What is the molarity of KMnO4 for sample 1?

*What is the molarity of KMnO4 for sample 2?

*What is the molarity of KMnO4 for sample 3?

*What is the average molarity of the KMnO4 solution?

*Calculate the standard deviation of the molarity of the KMnO4 solution.


A solution of sodium oxalate (Na2C2O4) in acidic solution is titrated with a solution of potassium permanganate (KMnO4) according to the following balanced chemical equation:

2KMnO4(aq) + 8H2SO4(aq) + 5Na2C2O4(aq) รขย†ย’ 2MnSO4(aq) + 8H2O(l) + 10CO2(g) + 5Na2SO4(aq) + K2SO4(aq)

What volume of 0.0203 M KMnO4 is required to titrate 0.119 g of Na2C2O4 dissolved in 20.0 mL of solution?

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