[Arathor]

I need to make a chemical using K2[PtCl4] KNO₂ and NH₃. I want my product to be K[PtCl₂(NO₂)(NH3)]
This is what I think for the start
(1)
K₂[PtCl₄] + NH₃  KCl + K[Pt(NH₃)]Cl₃

-but I think that instead of having one NH₃ ligand there will be 2; therefore kicking out the potassium I still want there. Any ideas?

-Edit- just realized chlorines aren't balanced so I'm assuming this isn't right

-Edit-I'm thinking this is right now

K₂[PtCl₄] + 2NH₃  2KCl + [Pt(NH₃)₂]Cl₂

and now have to add KNO₂ so I might get my potassium back

[Arathor]

Okay I believe I solved it
(1)
K₂[PtCl₄] + NH₃  KCl + K[PtCl₃(NH₃)]
(2)
K[PtCl₃(NH₃)] + KNO₂  KCl + K[PtCl₂(NO₂)(NH₃)]

I am hesitant on the fact that this can be square planer with 4 ligands and 2K+ and then still be square planer with 4 ligand and only one K+. Maybe its because the chlorines are being substituted and that they are more electronegative; I have looked into the formal charges of this.
Any objections I think this is solved.

[Borek]

Just because the reaction balances on paper, doesn't mean it goes in the solution.

[Arathor]

Yes true. The main thing I wanted to know is how the substitution worked with KNO3 and NH3 in relation to Cl and asked the question to see if my first reaction made sense (it didn't). Whether the actual reaction worked didn't matter to me just the substitution.