Complete and balance the following equations:

Cl₂ + OH^- $$\to$$ Cl^- + ClO^-

Hydroxylamine reduces iron (III) according to the equation:

2NH₂OH + 4Fe³⁺ $$\to$$ N₂O(g) $$ \uparrow $$ + H₂O + 4Fe²⁺ + 4H⁺

Iron (II) thus produced is estimated by titration with a standard permanganate solution. The reaction is :

$$MnO_4^-$$ + 5Fe²⁺ + 8H⁺ $$\to$$ Mn²⁺ + 5Fe³⁺ + 4H₂O

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 KMnO₄ solution for complete oxidation of iron (II). Calculate the weight of hydroxylamine in one litre of the original solution. (H = 1, N = 14, O = 16, K =39, Mn = 55, Fe = 56)

Balance the following Equations:

(i) Cu₂O + H⁺ + $$NO_3^ - \to $$ Cu²⁺ + NO + H₂O

(ii) K₄[Fe(CN)₆] + H₂SO₄ + H₂O $$\to$$ K₂SO₄ + FeSO₄ + (NH₄)₂SO₄ + CO

(iii) C2H5OH + I₂ + OH^- $$\to$$ CHI₃ + $$HCO_3^-$$ + I^- + 4H₂O

A 1.00 gm sample of H₂O₂ solution containing X percent H₂O₂ by weight requires X ml of a KMnO₄ solution for complete oxidation under acidic conditions. Calculate the normality of the KMnO₄ solution.