Challenge Your Exam Readiness With Our Free ACS General Chemistry Practice Questions

ACS solution chemistry emphasizes identifying strong electrolytes, spectator ions, and writing net ionic equations. AgNO₃ and NaCl are strong electrolytes that dissociate completely into Ag⁺, NO₃⁻, Na⁺, and Cl⁻. Solubility rules state that most chlorides are soluble except AgCl, PbCl₂ (cold), and Hg₂Cl₂; thus AgCl is insoluble and precipitates. Sodium and nitrate ions remain in solution as spectators. The balanced molecular equation is AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq). Canceling spectators (Na⁺ and NO₃⁻) yields the net ionic equation: Ag⁺(aq) + Cl⁻(aq) → AgCl(s). Distractors include forming impossible compounds (AgNa) or precipitating strong electrolytes that remain soluble (NaCl at these conditions). Recognizing solubility patterns and separating strong electrolyte species into ions are essential skills for precipitations, acid–base reactions, and some redox processes. Writing net ionic equations clarifies which species actually undergo chemical change and is a recurring ACS skill assessment.