Question

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.

Answer 1

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
`HNO_(3)`.

Step-by-step explanation:

In presence of NaCl,
`AgNO_(3)` forms an insoluble precipitate of AgCl.

Reaction:
`Ag^(+)(aq.)+Cl^(-)(aq.)\rightarrow AgCl(s)`

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

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

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

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