How does the "normality" of an "oxalic acid" solution relate to its "molarity"?

2 Answers
anor277
Jul 22, 2016

This is formally twice the molar quantity.

Explanation:

Oxalic acid is a diacid, i.e. HO(O=)C-C(=O)OH. Formally each equiv of acid requires 2 equiv of base to achieve neutrality. Of course pK_(a2) will be substantially greater than pK_(a1). You should look these values up.

P dilip_k
Jul 22, 2016

The oxalic acid is available in crystalline form having formula HOOC-COOH.2H_2O

"Its molar mass"=2*12+6*16+6*1=126g/"mol"

The basicity of this acid is 2 as its molecule produces 2 H^+ ions in its aqueous solution.

The equivalent mass of this acid is
="molar mass"/"basicity"=126/2=63g/"equivalent"

Normality of a solution

="No. of gm-equivalent"/L="strength in g/L "/"equivalent mass"

="strength in g/L "/(63g/"equivalent"

So knowing the strength in g/L and deviding it by 63g/"equivalent" we can easily get the Normality of oxalic acid solution

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