Question

Writing net ionic equation:

A solution of diamminesilver(I) chloride is treated with dilute nitric acid.

So what I did was..

[Ag(NH3)2]Cl(aq) + HNO3(aq) -> __________

The answer is
[Ag(NH3)2]+ + Cl- + 2H+ -> AgCl + 2NH4+

I would guess that the oxidation #s for diamminesilver(I) chloride would be:
Ag +1
NH3 0
Cl -1

Can someone please show me the steps in between?
I don't really know how to break the [Ag(NH3)2]Cl apart and predict/form the products.

Answer 1

well theres not much to it, NH3 stays together, Ag and Cl recombine to form neutral products

Answer 2

NH3 is a base, so it will pick up protons

Answer 3

Could you write the balanced equation, I'm stuck on the first part.

Answer 4

ahh, first and only time lol

2HNO3(aq) + [Ag(NH3)2]^+ + Cl^- -> AgCl(s) + 2NH4+ + 2NO3^-

Answer 5

you can take out NO3- from both sides, as you have in your answer, i guess that would make it more correct

Answer 6

okay so it would break down like this:

2H+ + 2NO3- + [Ag(NH3)2]+ Cl- -> AgCl + 2NH4+ + 2NO3-
v
Remove spectator 2NO3- from both sides.
v
2H+ + [Ag(NH3)2]+ + Cl- -> AgCl + 2NH4+

Answer 7

yeah, exactly

Answer 8

Thanks :D

Answer 9

no probs !