Ammonia reacts with a monobasic acid (A) to form a salt (B). B decomposes at about 250°C to give two products (C) and (D), leaving no residue. The oxide (D) is a liquid at room temperature and neutral to moist litmus, while the gas (C) is a neutral oxide. Identify A, B, C, D. Write the balanced equations involved in the above process.

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Solution

A monobasic acid has one hydrogen atom.
The reaction is:

$N H_{3} + H N O_{3} \to N H_{4} N O_{3} N H_{4} N O_{3} \overset{△}{\to} N_{2} O + H_{2} O$

Thus, we have:
A = HNO₃; B = NH₄NO₃; C = N₂O and D = H₂O

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A monobasic acid has one hydrogen atom. The reaction is: NH3+HNO3→NH4NO3NH4NO3→△ N2O+H2O Thus, we have: A = HNO​3; B = NH4NO3; C = N2O and D = H2O

A monobasic acid has one hydrogen atom.
The reaction is:

$N H_{3} + H N O_{3} \to N H_{4} N O_{3} N H_{4} N O_{3} \overset{△}{\to} N_{2} O + H_{2} O$

Thus, we have:
A = HNO₃; B = NH₄NO₃; C = N₂O and D = H₂O