To calculate the concentration of ions in a solution experiencing the common ion effect:
\[ K_{sp} = [Ion_1] \times [Ion_2] \]
Where:
The common ion effect refers to the decrease in solubility of an ionic compound when a salt containing a common ion is added to the solution. This phenomenon occurs because the addition of a common ion shifts the equilibrium position of the dissolution reaction, reducing the solubility of the compound. The common ion effect is an application of Le Chatelier’s principle, which states that the addition of an ion common to two solutes brings about precipitation or reduced ionization.
Let's assume the following values:
Using the formula:
\[ [Ion_1] = \frac{1.0 \times 10^{-10}}{1.0 \times 10^{-5}} = 1.0 \times 10^{-5} \text{ M} \]
The concentration of Ion_1 is 1.0 x 10-5 M.
Let's assume the following values:
Using the formula:
\[ [Ion_1] = \frac{2.0 \times 10^{-8}}{2.0 \times 10^{-4}} = 1.0 \times 10^{-4} \text{ M} \]
The concentration of Ion_1 is 1.0 x 10-4 M.