5.5 g of a mixutre of `FeSO_4.7H_2O` and `Fe_2(SO_4)_3.9H_2O` requires 5.4 " mL of " `0.1 N KMnO_4` solution for complete oxidation. Calculate the number of gram moles of hydrated ferric sulphate in the mixture.

3 " mol of "a mixture of FeSO_(4) and Fe_(2)(SO_(4))_(3) requried 100 " mL of " 2 M KMnO_(4) solution in acidic medium. Hence, mole fraction of FeSO_(4) in the mixture is

A mole of a mixture of Mohr's salt and Fe_2(SO_4)_3 requires 500mL of MK_2Cr_2O_7 for complete oxidation in acidic medium. The mole % of the Mohr's salt in the mixture 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:

4 mole of a mixture of Mohr's salt and Fe_(2)(SO_(4))_(3) requires 500mL of 1 M K_(2)Cr_(2)O_(7) for complete oxidation in acidic medium. The mole % of the Mohr's salt in the mixture is:

32g of a sample of FeSO_(4) .7H_(2)O were dissolved in dilute sulphuric aid and water and its volue was made up to 1litre. 25mL of this solution required 20mL of 0.02 M KMnO_(4) solution for complete oxidation. Calculate the mass% of FeSO_(4) .7 H_(2)O in the sample.

32g of a sample of FeSO_(4) .7H_(2)O were dissolved in dilute sulphuric aid and water and its volue was made up to 1litre. 25mL of this solution required 20mL of 0.02 M KMnO_(4) solution for complete oxidation. Calculate the mass% of FeSO_(4) .7 H_(2)O in the sample.

A 3.4g sample of H_2 O_2 solution containing x% h_2O_2 by mass requires x mL of a KMnO_4 solution for complete oxidation under acidic condition. The molarity of KMnO_4 solution is :

Hydroxylamine reduce iron (III) according to the equation : 2NH_(2)OH + 4 Fe^(3+) rarr N_(2)O(g)uarr + H_(2)O + 4Fe^(2+) + 4H^(+) Iron (II) thus produced is estimated by titration with a standard permanganate solution. The reaction is MnO_(4)^(-) + 5 Fe^(2+) + 8H^(+) rarr Mn^(2+) + 5Fe^(3+) + 4H_(2)O A 10 mL sample of hydroxylamine solution was diluted to 1 litre. 50 mL of this diluted solution was boiled with an excess of iron (III) solution. The resulting solution required 12 mL of 0.02 M KMnO_(4) solution for complete oxidation of iron (II). Calculate the weight of hydroxylamine in one litre of the original solution

0.4 g of a mixutre containing sodium oxalate (Na_2C_2O_4) and potassium oxalate requires 50 " mL of " (M)/(60)K_2Cr_2O_7 solution in acidic medium for complete reaction. Calculate the percentage composition of the mixture.

0.108 g of finely divided copper was treated with an excess of ferric sulphate solution untill Cu was completely dissolved. The solution after the addition of excess dil H_2SO_4 , required 33.7mL of 0.1 N KMnO_4 for complete oxidation. Find the equation which represents the reaction between metallic copper and ferric sulphate solution. (Cu=63.7,Fe=56)