(Solved): Salculate the solublity of \( \mathrm{Pbl}_{2} \) at a certain temperature in which \( K_{5 p}=1.2 ...

Salculate the solublity of \( \mathrm{Pbl}_{2} \) at a certain temperature in which \( K_{5 p}=1.2 \times 10^{-8} \). HOW DO WE GET THERE? To find the solubility of \( \mathrm{Pbl}_{2} \), we must find the equilibrium concentrations of the \( \mathrm{Pb}^{2+} \) and \( \mathrm{I}^{-} \)lons. We do this in the usual way by specilying the initial. concentrations and then defining the change required to reach equilibrium. Since, in this case, we do not know the solubility, we will assume that \( x \) mol/ of the solid dissolves to reach equilibrium, The \( 1: 2 \) stoichiometry of the sait means that: \( x \) mol/L \( \mathrm{Pbl}_{2}(\mathrm{~s})+x \mathrm{~mol}^{2} \mathrm{~Pb}^{2+}(\mathrm{aq})+2 \times \mathrm{mol}^{2} / \mathrm{L}^{2}(\mathrm{sq})- \) The concentrations are as follows: Intial cone Equilibrium conc. \( \left.\left[P b^{2}\right]_{0}=0 \quad\left[P b^{2}\right]\right\}=x \) \( \left.[1]_{0}=0 \quad[1]\right\}=2 x \) Substitute the equilibrium concentrations into the expression for \( K_{s 0} \) to solve for the solubility. moil Ticill \( (3 \) of 3\( ) \)