AgNO3 + NH3?

  • Thread starter Kitty808
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  • #1
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Ok, lab work...
I have to figure out a way to separate out the individual cations from a solution containing Fe(NO3)2, Cr(NO3)2, Ag(NO3), and Ni(NO3)2 and get each one into a particular form and perform a confirmatory test on it.
I've think I know how to get started on it. First adding some NH3 to the solution I should have Ni(NH3)6(2+) (aq), Fe(OH)3(s), Cr(OH)3(s), and Ag(NH3)2(s). Centrifuging out the solid should leave the Ni(NH3)6(2+) which I can run the confirmatory test on.

This is where I get a little stuck. I think by adding NaOH to the solids I should get Fe(OH)3(s), Cr(OH)4(-1)(aq), and Ag(OH)(aq)? I'm not sure about the Ag(OH) if that is correct and whether it is aq or s.

If I did my reaction right its:
Ag(NH3)2(+) + NaOH --> Ag(OH) + Na(NH3)?

If I could get some input as to whether I'm on the right track or not it would be appreciated very much.
 

Answers and Replies

  • #2
Borek
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I would separate Ag+ as chloride. Ag(NH3)2+ is not a solid.

But it seems like you are contradicting yourself in your post.
 
  • #3
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Ok, lab work...
I have to figure out a way to separate out the individual cations from a solution containing Fe(NO3)2, Cr(NO3)2
Maybe you intended [tex]Fe(NO_3)_3,\ Cr(NO_3)_3? [/tex] Otherwise they can't then give [tex]Fe(OH)_3,\ Cr(OH)_3[/tex] as you write after
, Ag(NO3), and Ni(NO3)2 and get each one into a particular form and perform a confirmatory test on it.
I've think I know how to get started on it. First adding some NH3 to the solution I should have Ni(NH3)6(2+) (aq), Fe(OH)3(s), Cr(OH)3(s), and Ag(NH3)2(s). Centrifuging out the solid should leave the Ni(NH3)6(2+) which I can run the confirmatory test on.
And [tex]Ag(NH_3)_2^+[/tex], as Borek wrote.
This is where I get a little stuck. I think by adding NaOH to the solids I should get Fe(OH)3(s), Cr(OH)4(-1)(aq), and Ag(OH)(aq)? I'm not sure about the Ag(OH) if that is correct and whether it is aq or s.

If I did my reaction right its:
Ag(NH3)2(+) + NaOH --> Ag(OH) + Na(NH3)?
No.

[tex]2Ag(NH_3)_2^+\ +\ 2NaOH\ \rightarrow\ Ag_2O\ +\ 2Na^+\ +\ 4NH_3\ +\ H_2O[/tex]

(Initially it forms AgOH, which quickly decomposes into the oxide).

Anyway, adding OH- to an ammonia solution of silver can produce dangerous compounds, so it's not advisable.
 
Last edited:
  • #4
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Borek,

First off I am into learning on my own, but I am stuck here and could use a little help.

I am working on equation writing, I have NH3(aq) + AgNO3. I have hit the Raymond Chang, Ninth edition for explanation on solving this, but I might be in the wrong section for comprehension. Could you guide me in the direction of information that could help me solve this, Thanks.
 
  • #5
Borek
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Go net ionic. Ag+ is getting complexed by two ammonia molecules.

Please don't necropost, rather start a new thread.
 
  • #6
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Will do, thanks.
 

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