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The flow chart is indicative of a compound with a silver cation, because $\ce{Ag+}$ reacts with $\ce{I-}$ to form yellow $\ce{AgI}$. Since $\ce{Ag+}$ does not form a hydroxide complex, it forms the brown $\ce{Ag2O}$ precipitate with excess $\ce{NaOH}$ solution. With $\ce{BaCl2}$, $\ce{AgCl}$ white precipitate forms. When excess $\ce{NH3}$ solution is added to that mixture, the soluble complex ion $\ce{Ag(NH3)2+}$ forms.

So, I can choose between answer choices A and B. However, I am not sure which cation is correct. The answer key says the answer is A, but I am not sure why, because both form white precipitate with $\ce{BaCl2}$.

user8081591
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  • @NilayGhosh Yes, the edits are correct. However, what is the correct anion? – user8081591 Aug 19 '18 at 04:19
  • Both the salts satisfy all the conditions. It's the cation($\ce{Ag+}$) that matters not the anion. – Nilay Ghosh Aug 19 '18 at 04:53
  • @NilayGhosh so there are two answers? – user8081591 Aug 19 '18 at 13:36
  • Seems like 2 answers. – Nilay Ghosh Aug 19 '18 at 15:15