Question

Which one of the following equations represents the net ionic equation for the reaction between aqueous potassium chloride and aqueous silver nitrate? A. Cl- (aq) + Ag+ (aq) AgCl (s) B. K+ (aq) + Cl- (aq) + Ag+ (aq) + NO3- (aq) AgCl (s) + K+ (aq) + NO3- (aq) C. KCl (aq) + AgNO3 (aq) AgCl (s) + KNO3 (aq) D. K+ (aq) + NO3- (aq) KNO3 (aq)

Answer 1

Ag⁺(aq) +Cl⁻(aq) → AgCl(s)

Step-by-step explanation:

The questions requires we write the net ionic equation for the reaction between aqueous potassium chloride and aqueous silver nitrate.

Step 1: Writing a balanced equation for the reaction.

• The balanced equation for the reaction between aqueous potassium chloride and aqueous silver nitrate will be given by;

KCl(aq) + AgNO₃(aq) → KNO₃(aq) +AgCl(s)

• AgCl is the precipitate formed by the reaction.

Step 2: Write the complete ionic equation.

• The complete ionic equation for the reaction is given by showing all the ions involved in the reaction.

K⁺(aq)Cl⁻(aq) + Ag⁺(aq)NO₃⁻(aq) → K⁺(aq)NO₃⁻(aq) +AgCl(s)

• Only ionic compounds are split into ions.

Step 3: Write the net ionic equation for the reaction.

• The net ionic equation for a reactions only the ions that fully participated in the reaction and omits the ions that did not participate in the reaction.
• The ions that are not involved directly in the reaction are known as spectator ions and are not included while writing net ionic equation.

Ag⁺(aq) +Cl⁻(aq) → AgCl(s)