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A sample consisting of chocolate-brown powder of $P b O_{2}$ is allowed to react with excess of $K l$ and iodine liberated is reacted with $N_{2} H_{4}$ in another container. The volume of $N_{2}$ gas liberated from this second container at STP was measured out to be $1.135$ htre. Find the volume (in L) of decimolar $N a O H$ solution required to dissolve $P b O_{2}$ completely and convert it to $N a_{2} P b O_{y}$ (Assume all reactions are $100 %$ complete).

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answer is 2.

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Detailed Solution

$n_{N_{2}} = \frac{1.135}{22.7} = 0.05 = n_{N_{2} H_{4}}$

$(n . f = 4)$

eq. of $N_{2} H_{4} =$ eq. of $I_{2} = eq$ . of ${PbO}_{2}$

$0.05 \times 4 = n \times 2$

$\Rightarrow n = 0.1 =$ moles of ${PbO}_{2}$

${PbO}_{2} + 2 NaOH ⟶ {Na}_{2} {PbO}_{3} + H_{2} O$

$0.1 0.2 = \frac{1}{10} x V \Rightarrow V = 2 L$

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