Normality of (COONa)2 - KMNO4 titration (redox reaction)

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The discussion centers on calculating the Normality of a (COONa)2 solution using a KMnO4 solution of 0.01 Normality. The equation N1V1=N2V2 is proposed for this calculation, where 14ml of KMnO4 is used to titrate 10ml of the (COONa)2 solution. There is consideration of the stoichiometry of the redox reaction, questioning whether to adjust the equation with a coefficient of 5/2 due to the equivalents involved. It is noted that 0.01N permanganate equates to 0.002M, and that the Normality of oxalate is twice its concentration in redox reactions. However, the ambiguity of Normality is acknowledged, with a caution that its use has been discouraged by IUPAC and other organizations for over 40 years.
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We used 14ml of a KMNO4 solution of 0.01 Normality, to find the Normality of a (COONa)2 solution.
If we took 10ml of the (COONa)2 solution, what should its Normality be?

I thought about using the following equation: N1V1=N2V2

Does the stoichiometry of the redox reaction affect the equation above? Should we multiply N2V2 with 5/2 because of it?
 
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Most likely 0.01N permanganate is actually 0.002M (five equivalents per mole), and normality of oxalate is twice its concentration (two equivalents per mole in redox reactions). If so equation as written should work with no additional stoichiometric coefficients.

But you are right that normality can be ambiguous and sometimes depends on the context, so treat above just as a guess.
 
Borek said:
normality can be ambiguous
AAmmmeeeennnnn.
 
Borek said:
But you are right that normality can be ambiguous and sometimes depends on the context, so treat above just as a guess.
And I think therefore its use is discouraged for at least 40 years by IUPAC and other organizations...
 
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