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A volume of 32.2 mL of a 1.16 M KMnO4 solution is mixed with 17.7 mL of .692 M KMnO4 Solution. Caclulate the concentration of the final solution.

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Elin Hessel
Elin HesselLv2
28 Sep 2019

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Related questions

A 35.2 mL, 1.66 M KMnO4 solution is mixed with 16.7 mL of 0.892M KMnO4 solution. Calculate the concentration of the final solution (assume the volumes are additive).

a 35.2ml, 1.66M KMnO4 solution is mixed with 16.7ml of .892M KMnO4 solution. Calculate the concentration of the final solution (assume the volumes are additive)

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.

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