Calculate the volume of 0.05 M `KMnO_(4)` solution required to oxidise completely 2.70 grams of oxalic acid `(H_(2)C_(2)O_(4))` in acidic medium

Answer

240 mL

Explanation

Balanced equation for the redox reaction is
`2KMnO_(4)+5(COOH)_(2)+3H_(2)SO_(4)rarrK_(2)SO_(4)+2MnSO_(4)+10CO_(2)+8H_(2)O`
No of moles of oxalic acid `=2.70//90 =0.03` mole
From the balanced equation 5 moles of `(COOH)_(2)=2 "moles of" KmnO_(4)`
`therefore 0.03 "mole of" (COOH)_(2)=2//5xx0.03=0.012 "mole of" KMnO_(4)`
Now 0.05 mole of `KmnO_(4)` is present in solution =`(1000xx0.012)/(0.05)=240` mL