How will you account for the acidic nature of $H N O_{3}$ ? Justify your answer by giving three different types of reactions with balanced chemical equations. [5 MARKS]

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Solution

Acidic Nature: 2 Marks
Equations: 3 Marks

Nitric acid behaves as a strong monobasic acid. It ionizes in an aqueous solution to a very great extent.
$H N O_{3} (a q) \to H^{+} + N O_{3}^{-}$
The presence of hydrogen ion imparts the acidic property to the aqueous solution of nitric acid.

The following reactions show the acidic nature of nitric acid:
(a) It reacts with basic oxides to form salt and water.
$C a O + 2 H N O_{3} (d i l .) \to C a (N O_{3})_{2} + H_{2} O$

(b) It reacts with metal hydroxide or basic hydroxides to form salt and water.
$N a O H + H N O_{3} (d i l .) \to N a N O_{3} + H_{2} O$

(c) It reacts with carbonates and bicarbonates to release $C O_{2}$ .
$N a_{2} C O_{3} + 2 H N O_{3} (d i l .) \to 2 N a N O_{3} + H_{2} O + C O_{2} ↑$

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How will you account for the acidic nature of HNO3? Justify your answer by giving three different types of reactions with balanced chemical equations. [5 MARKS]

How will you account for the acidic nature of $H N O_{3}$ ? Justify your answer by giving three different types of reactions with balanced chemical equations. [5 MARKS]