`0.3 g` of an oxalate salts was dissolved in `100 mL` solution. The solution required `90 mL` of `N//20 KMnO_(4)` for complete oxidation. The `%` of oxalate ion in salt is:

0.3 g of an oxalate salt was dissolved in 100 ml solution. The solution required 90 m! of N/20KMnO_4 for complete oxidation. The % of oxalate ion in salt is

10 g of oxalate was dissolved in 300 mL of solution. This solution required 250 mL of (M/10)KMnO_(4) in acidic medium for complete oxidation. The percentage purity of oxalate ion in the salt is :

10 g of oxalate was dissolved in 300 mL of solution. This solution required 250 mL of (M/10)KMnO_(4) in acidic medium for complete oxidation. The percentage purity of oxalate ion in the salt is :

Calculate the percentage of oxalate ion in a given sample of oxalate salt of which 0.6 g dissolved 100 " mL of " water required 90 " mL of " (M)/(100)KMnO_(4) for complete oxidation.

Calculate the percentage of oxalate ion in a given sample of oxalate salt of which 0.6 g dissolved 100 " mL of " water required 90 " mL of " (M)/(100)KMnO_(4) for complete oxidation.

Find out the % of oxalate ion in given sample of oxalate salt of which 0.3 g is present in 100 mL of solution required 90 mL. N//20KMnO_(4) for complete oxidation.

Find out the % of oxalate ion in given sample of oxalate salt of which 0.3 g is present in 100 mL of solution required 90 mL. N//20KMnO_(4) for complete oxidation.

3.92 g of ferrous ammonium sulphate crystals are dissolved in 100 ml of water, 20 ml of this solution requires 18 ml of KMnO_(4) during titration for complete oxidation. The weight of KMnO_(4) present in one litre of the solution is