Ksp Video Lessons

Concept:

Problem: Use the given molar solubilities in pure water to calculate Ksp for each compound. a. MX; molar solubility = 3.27 x 10-11 M b. PbF2; molar solubility = 5.63 x 10-3 M c. MgF2; molar solubility = 2.65 x 10-4 M

FREE Expert Solution

Recall that Ksp is an equilibrium constant related to slightly soluble ionic compounds

The dissociation of slightly soluble ionic compounds in solution is as follows:

MnNm(s)  n Mm+(aq) + m Nn–(aq)

The Ksp expression then is:

$\overline{){{\mathbf{K}}}_{{\mathbf{sp}}}{\mathbf{=}}\frac{\mathbf{products}}{\overline{)\mathbf{reactants}}}{\mathbf{=}}{\mathbf{\left[}}{\mathbf{nx}}{{\mathbf{\right]}}}^{{\mathbf{n}}}{\mathbf{\left[}}{\mathbf{mx}}{{\mathbf{\right]}}}^{{\mathbf{m}}}}$

where x = molar solubility of the compound.

Solve Ksp for each:

a. MX; molar solubility = 3.27 x 10-11

MX(s)  M+(aq) +X(aq)

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Problem Details

Use the given molar solubilities in pure water to calculate Ksp for each compound.

a. MX; molar solubility = 3.27 x 10-11

b. PbF2; molar solubility = 5.63 x 10-3

c. MgF2; molar solubility = 2.65 x 10-4 M