The correct equation for the laboratory preparation of nitric acid from potassium nitrate and concentrated sulphuric acid is

K N O_{3} + H_{2} S O_{4} < 200^{\circ} C \to K S O_{4} + H N O_{3}

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K N O_{3} + H_{2} S O_{4} < 200^{\circ} C \to K H S O_{4} + H N O_{3}

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2 K N O_{3} + H_{2} S O_{4} > 200^{\circ} C \to K_{2} S O_{4} + 2 H N O_{3}

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K N O_{3} + H_{2} S O_{4} > 200^{\circ} C \to K S O_{4} + H N O_{3}

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Solution

The correct option is B $K N O_{3} + H_{2} S O_{4} < 200^{\circ} C \to K H S O_{4} + H N O_{3}$

Potassium nitrate or sodium nitrate when made to react with sulphuric acid gives nitric acid leaving behind their bisulphites.

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Similar questions

What is the role of concentrated $H_{2} S O_{4}$ in the laboratory preparation of nitric acid?

(H_{2} S O_{4})

H_{2} S O_{4}

H_{2} S O_{4}

Why is :

(a) concentrated sulphuric acid kept in air tight bottles ?

(b) $H_{2} S O_{4}$ is not used as a drying agent for $H_{2} S$ ?

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