For this problem, we’re being asked to calculate the **molar s****olubility (in mol/L) of AgCl _{(s)}** in

• Since the AgCl ionic, it will form ions when dissociating in a solution. The dissociation of AgCl in a solution is as follows:

**AgCl _{(s)}**

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

*Note that each concentration is raised by the stoichiometric coefficient: **both [Ag ^{+}] and [Cl^{-}] are raised to 1*

Calculate the molar solubility of AgCl (K _{sp} = 1.8 x 10 ^{-10} at 25 degrees C) in 3.0 M NH_{3}

Ag^{+}(aq) + 2NH_{3}(aq) ⇌ Ag(NH_{3})_{2}^{+}(aq)

K_{f} = 1.6 x 10^{7}

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 Formation Constant concept. If you need more Formation Constant practice, you can also practice Formation Constant practice problems.

What professor is this problem relevant for?

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