For this problem, we’re being asked to calculate the **solubility of AgCl** in 010 M MgCl_{2}?

Since the compounds are ionic compounds, they form ions when dissociating in water. The dissociation of AgCl and MgCl_{2} in water are as follows:

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

AgCl_{(s) }⇌ **Ag ^{+}_{(aq)}** + Cl

The chloride ion, Cl^{–}, has a charge of –1. Mg then has a charge of +2:

MgCl_{2(s) }⇌ **Mg ^{2+}_{(aq)}** + 2 Cl

Calculate the Cl^{-} concentration in 0.10 MgCl_{2}.

$\frac{\mathbf{0}\mathbf{.}\mathbf{10}\mathbf{}\mathbf{mol}\mathbf{}{\mathbf{MgCl}}_{\mathbf{2}}}{\mathbf{1}\mathbf{}\mathbf{L}}\mathbf{}\mathbf{\times}\frac{\mathbf{2}\mathbf{}\mathbf{mol}\mathbf{}{\mathbf{Cl}}^{\mathbf{-}}}{\mathbf{1}\mathbf{}\mathbf{mol}\mathbf{}{\mathbf{MgCl}}_{\mathbf{2}}}$

**= 0.2 M Cl**^{-}

The K_{sp} of AgCl is 1.6 x 10^{-10}. What is the solubility of AgCl in 0.10 M MgCl_{2}? Give your answer using scientific notation and to 2 significant figures (i.e., one decimal place).

Frequently Asked Questions

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

Our tutors have indicated that to solve this problem you will need to apply the Ksp concept. You can view video lessons to learn Ksp. Or if you need more Ksp practice, you can also practice Ksp practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Fakhreddine's class at TEXAS.