Respuesta :
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:
[tex]NH_3(aq)+H^+(aq)+NO_3^-(aq)\rightarrow NH_4^+(aq)+NO_3^-(aq)[/tex]
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.
[tex]HNO_3(aq)\rightarrow H^+(aq)+NO_3^-(aq)[/tex]
The net ionic equation for the reaction that occurs when a few drops of nitric acid are added to the buffer is:
[tex]NH_3(aq)+H^+(aq)+NO_3^-(aq)\rightarrow NH_4^+(aq)+NO_3^-(aq)[/tex]
