Write the balanced NET ionic equation for the reaction when AgNO3 and KCI are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction. AgNO3(aq) + KCl(aq)
The Correct Answer and Explanation is :
Balanced Net Ionic Equation:
When silver nitrate (AgNO₃) and potassium chloride (KCl) are mixed in aqueous solution, a precipitation reaction occurs. The reaction forms silver chloride (AgCl), an insoluble solid, and potassium nitrate (KNO₃), which remains dissolved in solution.
The net ionic equation for this reaction is:
[
\text{Ag}^+ (aq) + \text{Cl}^- (aq) \rightarrow \text{AgCl} (s)
]
Explanation:
- Reaction Type:
This is a double displacement (precipitation) reaction. In such reactions, two aqueous ionic compounds exchange ions, leading to the formation of one insoluble product (precipitate). - Dissociation of Reactants:
- Silver nitrate (AgNO₃) dissociates into silver ions ((\text{Ag}^+)) and nitrate ions ((\text{NO}_3^-)) in water:
[
\text{AgNO}_3 (aq) \rightarrow \text{Ag}^+ (aq) + \text{NO}_3^- (aq)
] - Potassium chloride (KCl) dissociates into potassium ions ((\text{K}^+)) and chloride ions ((\text{Cl}^-)) in water:
[
\text{KCl} (aq) \rightarrow \text{K}^+ (aq) + \text{Cl}^- (aq)
]
- Formation of Precipitate:
When the ions mix, silver ions ((\text{Ag}^+)) combine with chloride ions ((\text{Cl}^-)) to form silver chloride ((\text{AgCl})), which is insoluble in water:
[
\text{Ag}^+ (aq) + \text{Cl}^- (aq) \rightarrow \text{AgCl} (s)
]
Silver chloride precipitates out as a solid. - Spectator Ions:
The potassium ((\text{K}^+)) and nitrate ((\text{NO}_3^-)) ions remain unchanged in the reaction and are considered spectator ions. They do not appear in the net ionic equation. - Net Ionic Equation:
The net ionic equation only includes the species directly involved in the reaction, which are the silver ions and chloride ions. - Verification of Charge and Mass Balance:
- Total charge on both sides: (+1) (from (\text{Ag}^+)) and (-1) (from (\text{Cl}^-)) balance to zero.
- Atoms: One silver and one chlorine atom are balanced.
This reaction demonstrates the principles of solubility rules and ionic equations, specifically how some combinations of ions result in insoluble products.