Question

IA group elements tend to be reactive due to their electronic configuration ($n{s}^1$) in their valence shell. Depending on their size, they form different type of basic oxide.

10 ml of 0.1 N 'X' solution reacts stoichiometrically with 2.29 ml of $KI{O}_4$ solution. The normality of $KI{O}_4$ solution and volume of $O_2$ released at STP are ___ and ___ respectively.

• A. 0.443 N, 11.2 ml
• B. 0.044 N, 44.8 ml
• C. 0.043 N, 44.8 ml
• D. 0.044 N, 22.4 ml

Answer 1

The correct option is A 0.443 N, 11.2 ml

$KI{O}_4+H_2{\stackrel{2-}{O}}_2⟶KI{O}_3+{\stackrel{0}{O}}_2+H_{2}O$
Here $KI{O}_4$ is getting reduced to $KI{O}_3$ and $H_2{O}_2$ is undergoing disproportionation.
$\text{meq of}{H}_2{O}_2=10ml\times 0.1N=1=\text{meq of}{O}_2$
$\text{no. of mmoles of}O=\frac{\text{meq of}{O}_2}{n-factor}=\frac{1}{2}$
$\text{Volume produced at STP}=\frac{22.4}{2}=11.2ml$

$\text{Normality of}KI{O}_4=\frac{\text{no. of meq}}{\text{sol. in ml}}=\frac{1}{2.29}\approx 0.44N$