Enter the net ionic equation, including phases, for the reaction of AgNO
(aq) and KCl(aq). Refer to the solubility rules as needed. net ionic equation:
The Correct Answer and Explanation is:
Net Ionic Equation: Ag⁺(aq) + Cl⁻(aq) → AgCl(s)
Explanation: To arrive at the net ionic equation for the reaction between silver nitrate (AgNO₃) and potassium chloride (KCl), we begin by writing the molecular equation:
AgNO₃(aq) + KCl(aq) → AgCl(s) + KNO₃(aq)
Silver nitrate and potassium chloride are both soluble in water. This means they dissociate into ions when dissolved. The dissociation is as follows:
AgNO₃(aq) → Ag⁺(aq) + NO₃⁻(aq) KCl(aq) → K⁺(aq) + Cl⁻(aq)
So, the complete ionic equation becomes:
Ag⁺(aq) + NO₃⁻(aq) + K⁺(aq) + Cl⁻(aq) → AgCl(s) + K⁺(aq) + NO₃⁻(aq)
At this stage, we identify the spectator ions. Spectator ions are ions that appear on both sides of the equation unchanged. In this case, K⁺ and NO₃⁻ are spectators. Removing them yields the net ionic equation:
Ag⁺(aq) + Cl⁻(aq) → AgCl(s)
This reaction demonstrates the formation of an insoluble salt, silver chloride, which precipitates from solution. According to solubility rules, most chloride salts are soluble, but silver chloride is an exception. This makes AgCl a solid product, or precipitate, in aqueous solution.
The importance of net ionic equations lies in their ability to highlight the actual chemical change taking place in solution. Rather than accounting for all ions, net ionic equations isolate the ions involved in the formation of new substances. In this case, they show the direct interaction between silver and chloride ions to form an insoluble compound. This type of analysis is crucial in analytical chemistry and in predicting whether certain ionic reactions will result in precipitates.
