Write the net ionic equation for the reaction that occurs when a few drops of nitric acid are added to the buffer. Express your answer as a chemical equation. Identify all of the phases in your answer.

This i an incomplete question, here is a complete question.

A buffer is prepared by adding 10.0 g of ammonium chloride (NH₄Cl) to 250 mL of 1.00 M NH₃ solution.

Write the net ionic equation for the reaction that occurs when a few drops of nitric acid are added to the buffer. Express your answer as a chemical equation. Identify all of the phases in your answer.

Answer : The net ionic equation for the reaction that occurs when a few drops of nitric acid are added to the buffer is:

Explanation :

Net ionic equation : In the net ionic equations, we are not include the spectator ions in the equations.

Spectator ions : The ions present on reactant and product side which do not participate in a reactions. The same ions present on both the sides.

As we know that nitric acid a strong acid it is completely dissociates into hydrogen ion and nitrate ion.

The net ionic equation for the reaction that occurs when a few drops of nitric acid are added to the buffer is:

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explanation:

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