A balanced net ionic equation for the reaction of AgNO3(aq) with KCl(aq). a. AgNO3(aq) + KCl(aq) → AgCl(aq) + KNO3(aq) b. Ag+(aq) + Cl-(aq) → AgCl(s) c. Ag+(aq) + NO3-(aq) + K+(aq) + Cl-(aq) → AgCl(s) + K+(aq) + NO3-(aq) d. Ag+(aq) + NO3-(aq) + K+(aq) + Cl-(aq) → Ag+(aq) + Cl-(aq) + KNO3(aq) e. K+(aq) + Cl-(aq) → KCl(s)
The Correct Answer and Explanation is:
The correct balanced net ionic equation for the reaction of AgNO₃(aq) with KCl(aq) is:
b. Ag⁺(aq) + Cl⁻(aq) → AgCl(s)
Explanation:
When silver nitrate (AgNO₃) and potassium chloride (KCl) are mixed in aqueous solution, they undergo a double replacement reaction, which is a type of precipitation reaction. In solution, both compounds dissociate into their respective ions:
- AgNO₃ dissociates into Ag⁺ and NO₃⁻
- KCl dissociates into K⁺ and Cl⁻
So, the full ionic equation is:
Ag⁺(aq) + NO₃⁻(aq) + K⁺(aq) + Cl⁻(aq) → AgCl(s) + K⁺(aq) + NO₃⁻(aq)
In this equation, we can see that K⁺ and NO₃⁻ ions appear on both sides of the equation without changing. These are called spectator ions because they do not participate directly in the chemical reaction. To focus on the actual chemical change occurring, we eliminate the spectator ions, which gives us the net ionic equation:
Ag⁺(aq) + Cl⁻(aq) → AgCl(s)
This shows that silver ions (Ag⁺) and chloride ions (Cl⁻) combine to form solid silver chloride (AgCl), which precipitates out of the solution. The formation of a solid product (precipitate) is evidence of a chemical reaction taking place in solution.
Other choices are incorrect for the following reasons:
- a shows the molecular form, not the net ionic equation.
- c includes spectator ions and is not a net ionic equation.
- d incorrectly suggests no reaction, as it shows ions on both sides unchanged.
- e is a reaction that does not occur under normal aqueous conditions, as KCl is highly soluble and does not form a solid.
Thus, option b is the correct net ionic equation.
