Question

Which of the following statements are correct for a solution of $H_2{O}_2$ having a strength of 17g/litre ?

• A. The volume strength $H_2{O}_2$ solution is 5.6 at 1 atmosphere pressure and 273 K temperature
• B. The molarity of given $H_2{O}_2$ solution is 0.5 M
• C. 1 ml of the given $H_2{O}_2$ solution will give out 2.8 ml of $O_2$ at 2 atmosphere pressure and 273 K temperature
• D. The normality of given $H_2{O}_2$ solution is 2N.

Answer 1

Answer: (A), (B), (C)

1 ml of the given $H_2{O}_2$ solution will give out 2.8 ml of $O_2$ at 2 atmosphere pressure and 273 K temperature

Volumes strength of an $H_2{O}_2$ solution is the volume of $O_2$ in litres at NTP produced by 11, of the solution.
$2H_2{O}_2\to 2H_{2}O+O_2$
68g 22.4 L at NTP
$\therefore$ Volume produced by 17g H_2O_2 (present in 1L solutoin) $=\frac{22.4}{68}\times 17=5.6LatNTP$
So the volume strength is 5.6.
The volume of $O_2$ given out at NTP by 1L of solution = 5.6L
$\therefore$ Volume of $O_2$ 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 $\frac{P_1{V}_1}{T_1}=\frac{P_2{V}_2}{T_2}$ or volume $=\frac{5.6}{2}=2.8ml$
Moles of $H_2{O}_2$ present in 1L solution $=\frac{17}{34}$
= 0.5 moles
[Mol wt = 34]
$\therefore$ Molarity of given solutoin = 0.5 M