Which of the following reactions shows nitric acid as an oxidizing agent?

$C + 4 H N O_{3} \to C O_{2} + 2 H_{2} O + 4 N O_{2}$

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$K_{2} O + 2 H N O_{3} \to 2 K N O_{3} + H_{2} O$

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$S + 6 H N O_{3} \to H_{2} S O_{4} + 2 H_{2} O + 6 N O_{2}$

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$3 Z n + 8 H N O_{3} \to 3 Z n (N O_{3})_{2} + 4 H_{2} O + 2 N O$

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Solution

The correct options are
A
$C + 4 H N O_{3} \to C O_{2} + 2 H_{2} O + 4 N O_{2}$

C
$S + 6 H N O_{3} \to H_{2} S O_{4} + 2 H_{2} O + 6 N O_{2}$

D
$3 Z n + 8 H N O_{3} \to 3 Z n (N O_{3})_{2} + 4 H_{2} O + 2 N O$

Nitric acid is a strong oxidizing agent whereby it undergoes reduction in a number of ways. Hence, it can get reduced to $N O$ , $N O_{2}$ $N_{2} O$ etc.

$3 Z n + 8 H N O_{3} \to 3 Z n (N O_{3})_{2} + 4 H_{2} O + 2 N O$

In the above reaction, nitric acid gets reduced to $N O$ . From the given options, only the following reaction is where nitric acid behaves as an acid and not as an oxidizing agent.

$K_{2} O + 2 H N O_{3} \to 2 K N O_{3} + H_{2} O$

So it looks like nitric acid behaves as an acid with bases or basic oxides. On the other hand, it tends to behave as an oxidizing agent when $H N O_{3}$ reacts with elements - metal or non-metal!

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