A series of chemicals were added to some AgNO3(aq). NaCl(aq) was added first to the silver nitrate solution to produce a precipitate. NH3(aq) was then added to produce a clear solution. HNO3(aq) was added last to result in a precipitate. Write a balanced net ionic equation for each of the three steps.

First, precipitate of AgCl is formed. Second, a soluble complex of silver and ammonia is formed. Third, AgCl is reproduced due to disappearance of ammonia complex in presence of [tex]HNO_{3}[/tex].

Explanation:

In presence of NaCl, [tex]AgNO_{3}[/tex] forms an insoluble precipitate of AgCl.

Reaction: [tex]Ag^{+}(aq.)+Cl^{-}(aq.)\rightarrow AgCl(s)[/tex]

In presence of [tex]NH_{3}[/tex], AgCl gets dissolved into solution due to formation of soluble [tex][Ag(NH_{3})_{2}]^{+}[/tex] complex.

Reaction: [tex]AgCl(s)+2NH_{3}(aq.)\rightarrow [Ag(NH_{3})_{2}]^{+}(aq.)+ Cl^{-}(aq.)[/tex]

In presence of [tex]HNO_{3}[/tex], [tex][Ag(NH_{3})_{2}]^{+}[/tex] complex gets destroyed and free [tex]Cl^{-}[/tex] again reacts with free [tex]Ag^{+}[/tex] to produce insoluble AgCl

Reaction: [tex][Ag(NH_{3})_{2}]^{+}(aq.)+2H^{+}(aq.)+Cl^{-}(aq.)\rightarrow AgCl(s)+2NH_{4}^{+}(aq.)[/tex]