Question

How can the value of Ksp be related to the molar solubility of a compound? View Available Hint(s) How can the value of Ksp be related to the molar solubility of a compound? When a common ion is present, the solubility of the compound decreases, and this is reflected in a lower value of Ksp. The square of a compound's molar solubility equals the value of Ksp for the compound. The value of Ksp equals the concentration of the compound in a saturated solution, which can be converted to the molar solubility using the molar mass. The molar solubility can be used to calculate the concentrations of ions in solution, which in turn are used to calculate Ksp.

Answer 1

The molar solubility can be used to calculate the concentrations of ions in solution, which in turn are used to calculate Ksp.

Step-by-step explanation:

Consider a slightly soluble solid with formula M₃X₂. Its solubility product expression is

`\begin{array}{rcccc}M_(3)X_(2)(s) & \rightleftharpoons&3M^(2+)(aq) & + & 2X^(3-)(aq)\\& & 3s & &2s\\\\K_\text{sp}& = & [3s]^(3)[2s]^(2)&= & 108s^(5)\\\\\end{array}`

Thus, the molar solubility can be used to calculate the concentrations of ions in solution, which in turn are used to calculate Ksp.

A is wrong. The solubility product constant is a constant. It does not change in the presence of a common ion.

B is wrong. It is correct only for compounds with formula MX.

C is wrong. Ksp does not equal the concentration of the compound in solution.