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Properties of Water

A 10 ml sampl...

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A 10 ml sample of hydroxylamine (NH2OH) aqueous solution is diluted to 50 ml. This diluted solution was completely reacted with 0.01 moles of Fe3+ ions as per following reaction : 2NH2OH+ 4Fe + →N2O +H2O + 4Fe2+ + 4H+ If molarity of original hydroxylamine solution is x, find the value of 100x.

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Q. Hydroxylamine reduces iron (III) according to the following reaction:

2 N H_{2} O H + F e^{3 +} \to N_{2} O (g) ↑ + H_{2} O + 4 F e^{2 +} + 4 H^{⨁}

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

M n O_{4}^{⊝} + 5 F e^{2 +} + 8 H^{⨁} \to M n^{2 +} + 5 F e^{3 +} + 4 H_{2} O

10

mL sample of hydroxylamine solution was diluted to

1

50

mL of this diluted solution was boiled with an excess of iron (III) solution, the resulting solution required

12

0.02 M

K M n O_{4}

solution for complete oxidation of iron (II). Calculate the weight of hydroxylamine in

1

L of the original solution

(H = 1, N = 14, O = 16, K = 39, M n = 55, F e = 56) :

Q. Hydroxylamine reduces iron (III) according to the equation,

2 N H_{2} O H (a q) + 4 F e^{3 +} (a q) \to N_{2} O (g) ↑ + H_{2} O (l) + 4 F e^{2 +} (a q) + 4 H^{+} (a q)

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

{M n O_{4}}^{-} + 5 F e^{2 +} + 8 H^{+} \to M n^{2 +} + 5 F e^{3 +} + 4 H_{2} O

10 m L

sample of hydroxylamine solution was diluted to one litre.

50 m L

of this diluted solution was boiled with excess of iron (III) solution. The resulting solution required

12 m L

0.02 M K M n O_{4}

solution for complete oxidation of iron (II). Calculate the mass of hydroxylamine in one litre of the original solution.

A sample of hydrazine sulphate

(N_{2} H_{6} S O_{4})

was dissolved in

100

10

mL of this solution was reacted with excess of

F e C l_{3}

solution and warmed to complete the reaction. Ferrous ions formed was estimated and it required

20

\frac{M}{50} K M n O_{4}

solution. Estimate the mass of hydrazine sulphate in one litre of solution.

4 F e^{3 +} + N_{2} H_{4} ⟶ N_{2} + 4 F e^{2 +} + 4 H^{+}

M n O_{4}^{-} + 5 F e^{2 +} + 8 H^{+} ⟶ M n^{2 +} + 5 F e^{3 +} + 4 H_{2} O

Q. A sample of hydrazine sulphate

(N_{2} H_{6} S O_{4})

was dissolved in

100

mL of water and

10

mL of this solution was reacted with excess of ferric chloride solution and warmed to complete the reaction. Ferrous ion formed was estimated and it required

20

\frac{M}{50}

potassium permanganate solution. Estimate the amount of hydrazine sulphate in

1

L of the solution. Reactions are given below:

4 F e^{3 +} + N_{2} H_{4} \to N_{2} + 4 F e^{2 +} + 4 H^{⨁}

M n O_{4}^{⊝} + 5 F e^{2 +} + 8 H^{⨁} \to M n^{2 +} + 5 F e^{3 +} + 4 H_{2} O

Q. In the reaction given below:

M g (s) + N O_{3}^{⊝} + H_{2} O \to M g (O H)_{2} (s) + ⊝ O H (a q) + N H_{3} (g)

20

mL of sample of

N O_{3}^{⊝}

solution is treated with

M g

N H_{3} (g)

was passed into

50

0.1 M

H C l

H C l

30

0.1 M

K O H

for its neutralization. If the molarity of

N O_{3}^{⊝}

ions in the original sample is

x

M, find the value of

10 x

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