A solution containing Ag⁺ ions is mixed with a small amount of Cl⁻(aq) and a large…

CHEMISTRY · Single correct · AP · Chemistry · Thermodynamics and Electrochemistry · Thermodynamics and Electrochemistry

Problem

A solution containing Ag⁺ ions is mixed with a small amount of Cl⁻(aq) and a large excess of NH₃(aq). The following reactions occur sequentially: Step 1: Ag⁺(aq) + Cl⁻(aq) → AgCl(s) Step 2: AgCl(s) + 2 NH₃(aq) → [Ag(NH₃)₂]⁺(aq) + Cl⁻(aq) Which overall net ionic equation best represents the chemical change that will be observed under these conditions? (a) Ag+(aq)+Cl−(aq)  →  AgCl(s)Ag^{+}(aq)+Cl^{-}(aq)\;\rightarrow\;AgCl(s) (b) Ag+(aq)+2 NH3(aq)  →  [Ag(NH3)2]+(aq)Ag^{+}(aq)+2\,NH_{3}(aq)\;\rightarrow\;[Ag(NH_{3})_{2}]^{+}(aq) (c) Ag+(aq)+2 NH3(aq)+Cl−(aq)  →  [Ag(NH3)2]+(aq)+Cl−(aq)Ag^{+}(aq)+2\,NH_{3}(aq)+Cl^{-}(aq)\;\rightarrow\;[Ag(NH_{3})_{2}]^{+}(aq)+Cl^{-}(aq) (d) Ag+(aq)+2 NH3(aq)+Cl−(aq)  →  [Ag(NH3)2]Cl(s)Ag^{+}(aq)+2\,NH_{3}(aq)+Cl^{-}(aq)\;\rightarrow\;[Ag(NH_{3})_{2}]Cl(s)

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