For this problem, we’re being asked to calculate the **solubility (in g/L) of AgCl(s)** in **0.010 M FeCl_{3}(aq)**. Since the compounds are ionic compounds, they form ions when dissociating in water. The dissociation of

The chloride ion, Cl^{–}, has a charge of –1. Ag has a charge is +1:

AgCl(s) ⇌ Ag^{+}(aq) + **Cl ^{–}(aq)**

The chloride ion, Cl^{–}, has a charge of –1. Fe has a charge is +3:

AlCl_{3}(s) ⇌ Al^{3+}(aq) + 3 **Cl ^{–}(aq)**

Calculate the molarity of Cl^{-}:

$\frac{\mathbf{0}\mathbf{.}\mathbf{010}\overline{)\mathbf{}{\mathbf{AlCl}}_{\mathbf{3}}\mathbf{}\mathbf{mol}}}{\mathbf{1}\mathbf{}\mathbf{L}}\mathbf{}\mathbf{\times}\mathbf{}\frac{\mathbf{3}\mathbf{}\mathbf{mol}\mathbf{}{\mathbf{Cl}}^{\mathbf{-}}}{\mathbf{1}\mathbf{}\overline{)\mathbf{}{\mathbf{AlCl}}_{\mathbf{3}}\mathbf{}\mathbf{}\mathbf{mol}}}$

**= 0.030 M Cl**^{-}

Notice that there is a common ion present, **Cl ^{–}**. The

The K_{sp} of AgCl is 1.6 x 10^{-10}. What is the solubility of AgCl in 0.010 M AlCl_{3}? Give your answer using scientific notation (1.23E-4) and to 2 significant figures (i.e., one decimal place).

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What scientific concept do you need to know in order to solve this problem?

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