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Mole Concept

If 10 ml of...

Question

If $10$ ml of an aqueous solution of $H_{2} O_{2}$ liberates $112$ ml of $O_{2}$ gas at STP upon decomposition, then:

normality of the above sample of

H_{2} O_{2}

0.5 N

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molarity of above sample of

H_{2} O_{2}

1 M

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milliequivalents of hypo required for the titration of liberated

I_{2}

when

10

ml of the same sample of

H_{2} O_{2}

is treated with excess of acidified solution of

K I

20

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% (w / v)

of given sample of

H_{2} O_{2}

3.4 %

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Solution

The correct options are
B $% (w / v)$ of given sample of $H_{2} O_{2}$ is $3.4 %$
C molarity of above sample of $H_{2} O_{2}$ is $1 M$
D milliequivalents of hypo required for the titration of liberated $I_{2}$ when $10$ ml of the same sample of $H_{2} O_{2}$ is treated with excess of acidified solution of $K I$ is $20$
The reaction is as follows:
$H_{2} O_{2} \to H_{2} O + \frac{1}{2} O_{2}$
Volume of $1$ mmol gas at $S T P = 22.4$ ml.
No. of moles in $112$ ml of $O_{2} = \frac{112}{22.4} = 5$ mmol.
Hence, according to reaction,
Number of moles of $H_{2} O_{2}$ $= 2 \times 5$ mmol $= 10$ mmol.
Hence, $molarity = \frac{Number of Moles}{Volume of solution}$ $= \frac{10 m m o l}{10 m l} = 1 M$

Milli equivalent of $H_{2} O_{2}$ reacted with $K I = N \times V = 2 \times 10 = 20$
$∴$ Milli equivalent of hypo required $= 20$
%(w/v) calculation
Molar weight of $H_{2} O_{2} = 34$ g
Weight of $10$ mmol of $H_{2} O_{2} = 10 \times 10^{- 3} \times 34 = 0.34$ g
$% (w / v)$ $= \frac{0.34 g m}{10 m l} \times 100 = 3.4 %$

Suggest Corrections

Similar questions

Q. 10

m L

of a sample of

H_{2} O_{2}

solution liberates 112

m L

O_{2}

gas at STP upon decomposition. Identify the correct statement(s):

25

ml of

H_{2} O_{2}

solution were added to excess of acidified

K I

solution. The iodine so liberated required

20

ml of

0.1 N

N a_{2} S_{2} O_{3}

for titration. Calculate strength of

H_{2} O_{2}

in terms of normality and percentage?

Q. An excess of acidified solution of

K I

is added to a

25

H_{2} O_{2}

solution. The iodine liberated requires

20

mL of

0.3 N N a_{2} S_{2} O_{3}

solution. Calculate the volume strength of

H_{2} O_{2}

Q. The purity of

H_{2} O_{2}

in a given sample is

85 %

. Calculate the weight of impure sample of

H_{2} O_{2}

which requires

10

mL of

\frac{M}{5} K M n O_{4}

solution in a titration in acidic medium.

50

ml of an aqueous solution of

H_{2} O_{2}

were treated with an excess of

K I

solution and dilute

H_{2} S O_{4}

. The liberated iodine required

20

mL of

0.1

N N a_{2} S_{2} O_{3}

solution for complete interaction. The concentration of

H_{2} O_{2}

in g/L is:

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If 10 ml of an aqueous solution of H2O2 liberates 112 ml of O2 gas at STP upon decomposition, then:

If $10$ ml of an aqueous solution of $H_{2} O_{2}$ liberates $112$ ml of $O_{2}$ gas at STP upon decomposition, then: