1 mole of equimolar mixture of ferric oxalate and ferrous oxalate requires x mole of `KMnO_4` in acidic medium for complete oxidation. x is :

1 mole of equimolar mixture of ferric oxalate and ferrous oxalate requres x mole of KMnO_(4) in acidic medium for complete oxidation. X is:

1 mole of equimolar mixture of Fe_(2)(C_(2)O_(4))_(3) and FeC_(2)O_(4) required X moles of KMnO_(4) in acid medium for complete reaction. The value of X is:

Five moles of ferric oxalate are oxidise by how much mole of KMnO_(4) in acidic medium.

2 mole, equimolar mixture of Na_2C_2O_4 and H_2C_2O_4 required V_1L of 0.1MKMnO_4 in acidic medium for complete oxidation. The same amount of the mixture required V_2L of 0.2M NaOH for neutralization. The ratio of V_1 to V_2 is :

2 mole , equimolar mixture of Na_(2)C_(2)O_(4) and H_(2)C_(2)O_(4) "required" V_(1) L of 0.1 M KMnO_(4) in acidic medium for complete oxidation. The same amount of the mixture required V_(2) L of 0.2 M NaOH for neutralisaation. The raation of V_(1) and V_(2) is:

1 mole of ferric oxalate is oxidised by x mole of MnO_(4)^(-) in acidic medium, Hence value of x is:

1 mole of ferric oxalate is oxidised by x mole of MnO_(4)^(-) in acidic medium, Hence value of x 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 :

How many moles of FeC_2O_4 are required to reduce 2 " mol of " KMnO_4 in acidic medium?

How many mole of FeSO_(4) reacted with one mole of KMnO_(4) in acidic medium?