Construct a balanced chemical equation for the following reaction:

Lead(II) nitrate $+$ sodium sulfate $\to$ lead(II) sulfate + sodium nitrate

Calcium bromide $+$ sodium carbonate $\to$ calcium carbonate $+$ sodium bromide

Barium chloride + silver nitrate barium nitrate + silver chloride

Potassium bromide + silver nitrate potassium nitrate + silver bromide

The balanced chemical equation for a reaction is:

$\mathrm{Pb}{\left({\mathrm{NO}}_3\right)}_2 \left(\mathrm{aq}\right) + 2\mathrm{KI} \left(\mathrm{aq}\right) \to 2{\mathrm{KNO}}_3 \left(\mathrm{aq}\right) + {\mathrm{PbI}}_2 \left(\mathrm{s}\right)$

What observations did you make? Were they what you expected?

The balanced chemical equation for a reaction is:

$\mathrm{Pb}{\left({\mathrm{NO}}_3\right)}_2 \left(\mathrm{aq}\right) + 2\mathrm{KI} \left(\mathrm{aq}\right) \to 2{\mathrm{KNO}}_3 \left(\mathrm{aq}\right) + {\mathrm{PbI}}_2 \left(\mathrm{s}\right)$

What term do we use to describe this type of reaction?

The balanced chemical equation for a reaction is:

$\mathrm{Pb}{\left({\mathrm{NO}}_3\right)}_2 \left(\mathrm{aq}\right) + 2\mathrm{KI} \left(\mathrm{aq}\right) \to 2{\mathrm{KNO}}_3 \left(\mathrm{aq}\right) + {\mathrm{PbI}}_2 \left(\mathrm{s}\right)$

After $10$ minutes, what did you observe? What was the color of the precipitate that formed?

The balanced chemical equation for a reaction is:

$\mathrm{Pb}{\left({\mathrm{NO}}_3\right)}_2 \left(\mathrm{aq}\right) + 2\mathrm{KI} \left(\mathrm{aq}\right) \to 2{\mathrm{KNO}}_3 \left(\mathrm{aq}\right) + {\mathrm{PbI}}_2 \left(\mathrm{s}\right)$

In this type of reaction, we often refer to the presence of spectator ions. These are ions that do not play a direct part in the reaction. Focusing on the formation of the precipitate lead(II) iodide, what are the spectator ions in this reaction?