# Question #739af

All nitrates are soluble; $P b {X}_{2}$ is insoluble.
$P b {\left(N {O}_{3}\right)}_{2} \left(a q\right) + 2 K I \left(a q\right) \rightarrow P b {I}_{2} \left(s\right) \downarrow + 2 K I \left(a q\right)$
Of course I could make this a net ionic equation. However, this question illustrates aqueous solubility rules. All nitrates are soluble; this allows us to get $P {b}^{2 +}$ or $A {g}^{+}$ into aqueous solution. Most halides are soluble. The exceptions are silver halides, mercurous halides, and LEAD HALIDES. $P b {I}_{2}$ wil precipitate from solution as a yellow solid. You should have done experiments to illustrate the reaction.