Considering the following precip reaction
Pb(NO3)2(aq)+2KI(aq)----->PbI2(s)+2KNO3(aq)
What is the correct net ionic equation?
I think it is 2NO3+^-+2K^+---->2KNO3
The net ionic equation represents only the species that are directly involved in the reaction. To determine the correct net ionic equation, let's first write the balanced molecular equation using the given reactants and products:
Pb(NO3)2(aq) + 2KI(aq) -----> PbI2(s) + 2KNO3(aq)
In this reaction, the Pb(NO3)2 and KI dissolve in water to form ions, while PbI2 and KNO3 remain as solid or dissolved compounds. To write the net ionic equation, we need to eliminate the spectator ions, which are the ions that do not participate in the reaction.
Step 1: Write the complete ionic equation by separating all the strong electrolytes into their respective ions:
Pb^2+(aq) + 2NO3^-(aq) + 2K^+(aq) + 2I^-(aq) -----> PbI2(s) + 2K^+(aq) + 2NO3^-(aq)
Step 2: Identify the spectator ions, which are the ions that appear unchanged on both sides of the equation. In this reaction, the spectator ions are K^+ and NO3^-.
Step 3: Remove the spectator ions from the equation, as they do not participate in the reaction:
Pb^2+(aq) + 2I^-(aq) -----> PbI2(s)
The resulting equation is the correct net ionic equation:
Pb^2+(aq) + 2I^-(aq) -----> PbI2(s)
Therefore, the net ionic equation for the given precipitation reaction is Pb^2+(aq) + 2I^-(aq) -----> PbI2(s).