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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