Multiple Choice
What is the net ionic equation for the reaction that occurs when aqueous solutions of sodium hypochlorite (NaOCl) and ammonia (NH3) are mixed?
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6. Chemical Quantities & Aqueous Reactions
Complete Ionic Equations
Multiple Choice
Which of the following is the correct net ionic equation for the precipitation reaction that occurs when aqueous solutions of AgNO_3 and NaCl are mixed?
A
AgCl (aq) → Ag^+ (aq) + Cl^- (aq)
B
Ag^+ (aq) + Cl^- (aq) → AgCl (s)
C
AgNO_3 (aq) + NaCl (aq) → AgCl (s) + NaNO_3 (aq)
D
Ag^+ (aq) + NO_3^- (aq) + Na^+ (aq) + Cl^- (aq) → Ag^+ (aq) + NO_3^- (aq) + Na^+ (aq) + Cl^- (aq)
Verified step by step guidance1
Identify the reactants and products in the given reaction: aqueous solutions of AgNO_3 and NaCl are mixed, resulting in the formation of AgCl as a precipitate and NaNO_3 remaining in solution.
Write the full molecular equation for the reaction: \(\mathrm{AgNO_3 (aq) + NaCl (aq) \rightarrow AgCl (s) + NaNO_3 (aq)}\).
Dissociate all strong electrolytes (soluble ionic compounds) into their ions to write the complete ionic equation: \(\mathrm{Ag^+ (aq) + NO_3^- (aq) + Na^+ (aq) + Cl^- (aq) \rightarrow AgCl (s) + Na^+ (aq) + NO_3^- (aq)}\).
Identify the spectator ions, which are ions that appear unchanged on both sides of the equation. In this case, \(\mathrm{Na^+}\) and \(\mathrm{NO_3^-}\) are spectator ions.
Remove the spectator ions to write the net ionic equation, which shows only the species involved in the formation of the precipitate: \(\mathrm{Ag^+ (aq) + Cl^- (aq) \rightarrow AgCl (s)}\).
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