Question

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

Answer 1

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.

Answer 2

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