Question

Writing the net ionic equation

2AgNO3(aq)+(NH4)2S(aq)=>Ag2S(s)+2NH4NO3(aq)
please explain how you got the answer!

Answer 1

First write the molecular equation with states:

(NH4)2S (aq) + 2AgNO3(aq) → Ag2S (s) + 2NH4NO3

Now write a full ionic equation by separating into ions all substances that dissociate: anything (s) (g) or (l) does not dissociate

2NH4 + (aq) + S 2-(aq) + 2Ag+ (aq) + 2NO3- (aq) → Ag2S(s) + 2NH4 + (aq) + 2NO3- (aq)

To write the NET IONIC equation, inspect the full ionic equation above and delete anything that appears on both sides of the → sign:

Net ionic equation:

S 2-(aq) + 2Ag + (aq) → Ag2S(s)

Answer 2

Answer: The net ionic equation is written below.

Step-by-step explanation:

Net ionic equation of any reaction does not include any spectator ions.

Spectator ions are defined as the ions which does not get involved in a chemical equation. They are found on both the sides of the chemical reaction when it is present in ionic form.

The chemical equation for the reaction of silver nitrate and ammonium sulfide is given as:

`2AgNO_3(aq.)+(NH_4)_2S(aq.)\rightarrow Ag_2S(s)+2NH_4NO_3(aq.)`

Ionic form of the above equation follows:

`2Ag^+(aq.)+2NO_3^-(aq.)+2NH_4^+(aq.)+S^(2-)(aq.)\rightarrow Ag_2S(s)+2NH_4^+(aq.)+2NO_3^-(aq.)`

As, ammonium and nitrate ions are present on both the sides of the reaction. Thus, it will not be present in the net ionic equation and are spectator ions.

The net ionic equation for the above reaction follows:

`2Ag^+(aq.)+S^(2-)(aq.)\rightarrow Ag_2S(s)`

Hence, the net ionic equation is written above.