1

IIT-JEE 1983

Subjective

+5

-0

The density of a 3 M Sodium thiosulphate solution (Na

_{2}S_{2}O_{3}) is 1.25 g per ml. Calculate**(i)**the percentage by weight of sodium thiosulphate,**(ii)**the mole fraction of sodium thiosulphate and**(iii)**the molalities of Na^{+}and $$S_2O_3^{-2}$$ ions2

IIT-JEE 1983

Subjective

+4

-0

4.08 g of a mixture of BaO and an unknown carbonate MCO

_{3}was heated strongly. The residue weighed 3.64 g. This was dissolved in 100 ml of 1 N HCl. The excess acid required 16 ml of 2.5 N NaOH solution for complete neutralization. Identify the metal M. (At wt. H = 1, C = 12, O = 16, Cl = 35.5, Ba = 138)3

IIT-JEE 1982

Subjective

+4

-0

Hydroxylamine reduces iron (III) according to the equation:

2NH

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

$$MnO_4^-$$ + 5Fe

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

2NH

_{2}OH + 4Fe^{3+}$$\to$$ N_{2}O(g) $$ \uparrow $$ + H_{2}O + 4Fe^{2+}+ 4H^{+}Iron (II) thus produced is estimated by titration with a standard permanganate solution. The reaction is :

$$MnO_4^-$$ + 5Fe

^{2+}+ 8H^{+}$$\to$$ Mn^{2+}+ 5Fe^{3+}+ 4H_{2}OA 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. (H = 1, N = 14, O = 16, K =39, Mn = 55, Fe = 56)4

IIT-JEE 1981

Subjective

+3

-0

A 1.00 gm sample of H

_{2}O_{2}solution containing X percent H_{2}O_{2}by weight requires X ml of a KMnO_{4}solution for complete oxidation under acidic conditions. Calculate the normality of the KMnO_{4}solution.Questions Asked from Some Basic Concepts of Chemistry (Subjective)

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