KMnO4 reacts with ferrous sulphate according to the following equation- Mn O 4- - 5Fe2- - 8H- Mn2- - 5Fe3- - 4H2Ohere- 10 mL of 0-1 M KMnO4 is equivalent to -CPMT 1999-

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Equivalent Mass

KMnO4 reacts ...

Question

$K M n O_{4}$ reacts with ferrous sulphate according to the following equation:
$M n O_{4}^{-} + 5 F e^{2 +} + 8 H^{+} \to M n^{2 +} + 5 F e^{3 +} + 4 H_{2} O$
here, $10 m L$ of $0.1 M K M n O_{4}$ is equivalent to $[C P M T 1999]$

50 m L

0.1 M F e S O_{4}

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20 m L

0.1 M F e S O_{4}

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40 m L

0.1 M F e S O_{4}

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30 m L

0.1 M F e S O_{4}

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Solution

The correct option is B $50 m L$ of $0.1 M F e S O_{4}$
$K M n O_{4}$ reacts with ferrous sulphate according to the following equation,

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

$2 K M n O_{4} + 10 F e S O_{4} + 8 H_{2} S O_{4} ⟶ K_{2} S O_{4} + 2 M n S O_{4} + 5 F e_{2} (S O_{4})_{3} + 8 H_{2} O$

2 moles of $K M n O_{4}$ reacts with 10 moles of $F e S O_{4}$ .

The number of moles of $K M n O_{4}$ in 10 ml of 0.1 M $= 0.1 \times 0.01 = 10^{- 3} m o l e s$

Therefore, $10^{- 3}$ moles $K M n O_{4}$ reacts with $(5 \times 10^{- 3})$ moles of $F e S O_{4}$ .

Hence, option $A (50 m l o f 0.1 M F e S O_{4} = 5 \times 10^{- 3} m o l e s$ of $F e S O_{4})$ is correct.

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Similar questions

$K M n O_{4}$ reacts with ferrous ammonium sulphate according to the equation $M n O_{4}^{-} + 5 F e^{2 +} + 8 H^{+} \to M n^{2 +} + 5 F e^{3 +} + 4 H_{2} O$ , here 10 ml of 0.1 M $K M n O_{4}$ is equivalent to

Q. 50 mL aqueous solution of

F e S O_{4}

required 12 mL of 0.2 M

K M n O_{4}

in acidic medium for complete oxidation. Calculate the molarity of ferrous sulphate 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

K M n O_{4}

reacts with oxalic acid according to the equation

2 M n O_{4}^{-} + 5 C_{2} O_{4}^{2 -} + 16 H^{+} \to 2 M n^{2 +} + 10 C O_{2} + 8 H_{2} O

Here ,

20 m L

of 0.1 M

K M n O_{4}

is equivalent to:

Q. A sample of hydrazine sulphate

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

was dissolved in

100 m L

of water.

10 m L

of this solution was reacted with an excess of

F e C l_{3}

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

20 m L

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

. Estimate the amount of hydrazine sulphate in one litre of solution.
Reactions:

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

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KMnO4 reacts with ferrous sulphate according to the following equation:MnO−4+5Fe2++8H+→Mn2++5Fe3++4H2Ohere, 10 mL of 0.1 M KMnO4 is equivalent to [CPMT1999]

$K M n O_{4}$ reacts with ferrous sulphate according to the following equation:
$M n O_{4}^{-} + 5 F e^{2 +} + 8 H^{+} \to M n^{2 +} + 5 F e^{3 +} + 4 H_{2} O$
here, $10 m L$ of $0.1 M K M n O_{4}$ is equivalent to $[C P M T 1999]$