# Problem: Use the Ksp values to calculate the molar solubility of each of the following compounds in pure water. a) MX (Ksp = 6.99 × 10−11) b) PbCl2 (Ksp = 1.17 × 10−5) c) Ca(OH)2 (Ksp = 4.68 × 10−6)

###### FREE Expert Solution

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

MnNm(s)  n Mm+(aq) + m Nn–(aq)

ICE Chart:

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

where x = molar solubility of the compound.

a) MX M+ + X-

###### Problem Details

Use the Ksp values to calculate the molar solubility of each of the following compounds in pure water.

a) MX (Ksp = 6.99 × 10−11

b) PbCl2 (Ksp = 1.17 × 10−5

c) Ca(OH)2 (Ksp = 4.68 × 10−6)