Question

1. balance the double replacement reaction by dragging the correct coefficients. ? pb(no₃)₂(aq) + ? ki(aq) → ? pbi₂(s) + ? kno₃(aq) submit answer 0 / ∞ submissions used score: 0/1 6. build the net ionic equation for the reaction that produces the lead(ii) iodide precipitate. a net ionic equation shows only the ions that participate in the reaction. these are the ions that react to form the precipitate. ions that remain aqueous in a reaction are called spectators. the spectator ions are not included in the net ionic equation. what is a net ionic equation? ? cation + ? anion → ? precipitate

Explanation:

Step1: Balance the double - replacement reaction

We need to balance the atoms on both sides of the equation. For the reaction $Pb(NO_3)_2(aq)+KI(aq)\to PbI_2(s)+KNO_3(aq)$, we balance the nitrate, potassium and iodine atoms.
$Pb(NO_3)_2(aq)+2KI(aq)\to PbI_2(s)+2KNO_3(aq)$

Step2: Write the complete ionic equation

The complete ionic equation is $Pb^{2 + }(aq)+2NO_3^{-}(aq)+2K^{+}(aq)+2I^{-}(aq)\to PbI_2(s)+2K^{+}(aq)+2NO_3^{-}(aq)$

Step3: Identify spectator ions

The spectator ions are $K^{+}$ and $NO_3^{-}$ as they remain in the aqueous state on both sides of the equation.

Step4: Write the net - ionic equation

Removing the spectator ions, the net - ionic equation is $Pb^{2+}(aq)+2I^{-}(aq)\to PbI_2(s)$

Answer:

1. Coefficients: 1, 2, 1, 2
2. $Pb^{2+}(aq)+2I^{-}(aq)\to PbI_2(s)$