What mass of $H N O_{3}$ is required to make 1 litre of $2 N$ solution to be used as an oxidizing agent in the reaction?
$3 C u + 8 H N O_{3} ⟶ 3 C u (N O_{3})_{2} + 2 N O + 4 H_{2} O$

63 g

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21 g

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42 g

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84 g

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Solution

The correct option is B $42 g$
$3 C u + 8 H N O_{3} ⟶ 3 C u (N O_{3})_{2} + 2 N O + 4 H_{2} O$
+5 +5 +2
So, change in oxidation state is $3$ .
and equivalent weight of $H N O_{3} = 63 / 3 = 21$
So, to make $1$ N solution, mass of $H N O_{3}$ required is $21$ ,
So, for $2$ N solution, mass required is $42$ g.

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