Questions: Select the net ionic equation for the reaction that occurs when potassium iodide and lead(II) mixed. No reaction occurs K^+(aq)+I^-(aq) → KI(s) Pb^2+(aq)+I^-(aq) → PbI(s) 2 K^+(aq)+2 I^-(aq)+Pb^2+(aq)+2 NO3^-(aq) → 2 K^+(aq)+2 NO3^-(aq)+PbI2(s) 2 K^+(aq)+2 I^-(aq) → K2I2(s) Pb^2+(aq)+2 I^-(aq) → PbI2(s)

Select the net ionic equation for the reaction that occurs when potassium iodide and lead(II) mixed.
No reaction occurs
K^+(aq)+I^-(aq) → KI(s)
Pb^2+(aq)+I^-(aq) → PbI(s)
2 K^+(aq)+2 I^-(aq)+Pb^2+(aq)+2 NO3^-(aq) → 2 K^+(aq)+2 NO3^-(aq)+PbI2(s)
2 K^+(aq)+2 I^-(aq) → K2I2(s)
Pb^2+(aq)+2 I^-(aq) → PbI2(s)

Transcript text: Select the net ionic equation for the reaction that occurs when potassium iodide and lead(II) mixed. No reaction occurs $\mathrm{K}^{+}(a q)+\mathrm{I}^{-}(a q) \rightarrow \mathrm{KI}(s)$ $\mathrm{Pb}^{2+}(a q)+\mathrm{I}^{-}(a q) \rightarrow \mathrm{PbI}(s)$ $2 \mathrm{~K}^{+}(a q)+2 \mathrm{I}^{-}(a q)+\mathrm{Pb}^{2+}(a q)+2 \mathrm{NO}_{3}{ }^{-}(a q) \rightarrow 2 \mathrm{~K}^{+}(a q)+2 \mathrm{NO}_{3}{ }^{-}(a q)+\mathrm{PbI}_{2}(s)$ $2 \mathrm{~K}^{+}(a q)+2 \mathrm{I}^{-}(a q) \rightarrow \mathrm{K}_{2} \mathrm{I}_{2}(s)$ $\mathrm{Pb}^{2+}(a q)+2 \mathrm{I}^{-}(a q) \rightarrow \mathrm{PbI}_{2}(s)$

Solution

Solution Steps

Step 1: Identify the Reactants and Products

When potassium iodide (KI) and lead(II) nitrate (Pb(NO$_3$)$_2$) are mixed, the potential reaction involves the formation of lead(II) iodide (PbI$_2$), which is an insoluble compound that precipitates out of solution.

Step 2: Write the Balanced Molecular Equation

The balanced molecular equation for the reaction is: \[ 2 \text{KI}(aq) + \text{Pb(NO}_3\text{)}_2(aq) \rightarrow 2 \text{KNO}_3(aq) + \text{PbI}_2(s) \]

Step 3: Write the Complete Ionic Equation

The complete ionic equation shows all the ions present in the reaction: \[ 2 \text{K}^+(aq) + 2 \text{I}^-(aq) + \text{Pb}^{2+}(aq) + 2 \text{NO}_3^-(aq) \rightarrow 2 \text{K}^+(aq) + 2 \text{NO}_3^-(aq) + \text{PbI}_2(s) \]

Step 4: Identify and Remove Spectator Ions

Spectator ions are ions that do not participate in the actual chemical reaction. In this case, the potassium ions ($\text{K}^+$) and nitrate ions ($\text{NO}_3^-$) are spectator ions.

Step 5: Write the Net Ionic Equation

After removing the spectator ions, the net ionic equation is: \[ \text{Pb}^{2+}(aq) + 2 \text{I}^-(aq) \rightarrow \text{PbI}_2(s) \]