JEE Main · 2022easyCORD-062

White precipitate of AgCl dissolves in aqueous ammonia solution due to formation of:

Coordination Compounds · Class 12 · JEE Main Previous Year Question

Question

White precipitate of AgCl dissolves in aqueous ammonia solution due to formation of:

Options
  1. a

    [Ag(NH3)4]Cl2[\mathrm{Ag(NH_3)_4}]\mathrm{Cl_2}

  2. b

    [Ag(Cl)2(NH3)2][\mathrm{Ag(Cl)_2(NH_3)_2}]

  3. c

    [Ag(NH3)2]Cl[\mathrm{Ag(NH_3)_2}]\mathrm{Cl}

    ✓
  4. d

    [Ag(NH3)Cl]Cl[\mathrm{Ag(NH_3)Cl}]\mathrm{Cl}

Correct Answerc

[Ag(NH3)2]Cl[\mathrm{Ag(NH_3)_2}]\mathrm{Cl}

Detailed Solution

🧠 The Tollens / AgCl Recipe

Insoluble AgCl\mathrm{AgCl} dissolves in aqueous NH3\mathrm{NH_3} because Ag+\mathrm{Ag^+} is greedy for nitrogen donors. With ammonia present, Ag+\mathrm{Ag^+} forms the diammine-silver(I) cation, [Ag(NH3)2]+[\mathrm{Ag(NH_3)_2}]^+ — linear, two-coordinate, very stable.

The released Cl−\mathrm{Cl^-} stays in solution as the counter-ion. Net product: [Ag(NH3)2]Cl[\mathrm{Ag(NH_3)_2}]\mathrm{Cl}.

🗺️ Eliminate the Wrong Salts

  • (1) [Ag(NH3)4]Cl2[\mathrm{Ag(NH_3)_4}]\mathrm{Cl_2} — would need Ag2+\mathrm{Ag^{2+}} (silver(I) is the only common Ag oxidation state in aqueous chemistry). ✗
  • (2) [Ag(Cl)2(NH3)2][\mathrm{Ag(Cl)_2(NH_3)_2}] — invokes a 4-coordinate neutral Ag(I) species; not the ammonia-dissolution product. ✗
  • (3) [Ag(NH3)2]Cl[\mathrm{Ag(NH_3)_2}]\mathrm{Cl} — the textbook diammine complex. ✓
  • (4) [Ag(NH3)Cl]Cl[\mathrm{Ag(NH_3)Cl}]\mathrm{Cl} — would need Ag2+\mathrm{Ag^{2+}}. ✗

⚡ The "Ag(I) = 2-Coordinate Linear" Anchor

Ag+\mathrm{Ag^+} is d10\mathrm{d^{10}} and almost always forms 2-coordinate linear complexes: [Ag(NH3)2]+[\mathrm{Ag(NH_3)_2}]^+, [Ag(CN)2]−[\mathrm{Ag(CN)_2}]^-, [Ag(S2O3)2]3−[\mathrm{Ag(S_2O_3)_2}]^{3-}. If you see Ag+\mathrm{Ag^+} + ligand → expect two ligands, linear.

⚠️ Don't Promote Ag

Aqueous Ag(I) does not become Ag(II) just to fit 4 ligands. The only common oxidation state in solution is +1+1. Reject any option that demands Ag(+2) or higher.

Answer: (3) [Ag(NH3)2]Cl\boxed{\text{Answer: (3) } [\mathrm{Ag(NH_3)_2}]\mathrm{Cl}}

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