We can construct an ** ICE table** for the dissociation of AgI.

Remember that solids are ignored in the ICE table and K_{sp} expression.

The **K _{sp} expression** for AgI is:

$\overline{){{\mathbf{K}}}_{{\mathbf{sp}}}{\mathbf{=}}\frac{\mathbf{products}}{\overline{)\mathbf{reactants}}}{\mathbf{=}}\mathbf{\left[}{\mathbf{Ag}}^{\mathbf{+}}\mathbf{\right]}\mathbf{\left[}{\mathbf{I}}^{\mathbf{-}}\mathbf{\right]}}$

Note that each concentration is raised by the stoichiometric coefficient: [Ag^{+}] and [I^{–}] are raised to 1

We can now plug in the equilibrium concentrations and solve for **x**, which is the **molar solubility of AgI**.

Calculate the molar solubility of AgI in pure water. K _{sp} for AgI is 1.5 X 10 ^{-16}.

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