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Question

Which of the following statements are correct for a solution of H2O2 having a strength of 17g/litre ?


A

The volume strength H2O2 solution is 5.6 at 1 atmosphere pressure and 273 K temperature

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B

The molarity of given H2O2 solution is 0.5 M

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C

1 ml of the given H2O2 solution will give out 2.8 ml of O2 at 2 atmosphere pressure and 273 K temperature

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D

The normality of given H2O2 solution is 2N.

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Solution

The correct option is C

1 ml of the given H2O2 solution will give out 2.8 ml of O2 at 2 atmosphere pressure and 273 K temperature


Volumes strength of an H2O2 solution is the volume of O2 in litres at NTP produced by 11, of the solution.
2H2O22H2O+O2
68g 22.4 L at NTP
Volume produced by 17g H_2O_2 (present in 1L solutoin) =22.468×17=5.6 L at NTP
So the volume strength is 5.6.
The volume of O2 given out at NTP by 1L of solution = 5.6L
Volume of O2 given out at NTP by 1 ml of solution = 5.6 mL
Converting this volume to volume at 2 atmosphere pressure and 273K temperature, we get P1V1T1=P2V2T2 or volume =5.62=2.8 ml
Moles of H2O2 present in 1L solution =1734
= 0.5 moles
[Mol wt = 34]
Molarity of given solutoin = 0.5 M


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