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Chapter 16: Problem 88

Give an example of how the common-ion effect limits the dissolution of a sparingly soluble ionic compound.

Short Answer

Expert verified
Answer: The common-ion effect limits the dissolution of a sparingly soluble ionic compound, such as Calcium fluoride (CaF2), by shifting the equilibrium in response to the presence of a common ion. When an external source of fluoride ions, like sodium fluoride (NaF), is added to the solution, it increases the concentration of fluoride ions. According to Le Chatelier's principle, the equilibrium will shift to counteract this change, leading to the precipitation of more Calcium fluoride and a decrease in its solubility.

Step by step solution

01

Choose an example of a sparingly soluble ionic compound

A suitable example of a sparingly soluble ionic compound is Calcium fluoride (CaF2).
02

Understanding the common-ion effect

The common-ion effect refers to the decrease in the solubility of a sparingly soluble ionic compound when a solution already contains one of its ions. This effect can be explained by Le Chatelier's principle, which states that when a system at equilibrium experiences a change in concentration, temperature, or pressure, the system will shift to counteract the change and reestablish equilibrium.
03

Write the solubility equilibrium reaction for the chosen compound

For Calcium fluoride (CaF2), the solubility equilibrium reaction can be written as: CaF2 (s) <=> Ca^2+ (aq) + 2F^- (aq)
04

Calculating the solubility product constant (Ksp)

The equilibrium constant expression, also known as the solubility product constant (Ksp), relates the solubility of the ionic compound to the concentrations of its constituent ions at equilibrium. For Calcium fluoride, the Ksp expression is: Ksp = [Ca^2+] * [F^-]^2
05

Adding a common ion to the solution

To demonstrate the common-ion effect, let's consider adding sodium fluoride (NaF) to the solution, which also contains fluoride ions (F^-).
06

Applying Le Chatelier's principle considering the common-ion effect

When sodium fluoride is added to the solution, it increases the concentration of fluoride ions in the solution. According to Le Chatelier's principle, the equilibrium will shift to counteract this change and restore the equilibrium. In this case, the equilibrium will shift to the left, causing more Calcium fluoride to precipitate out of the solution, and thus decreasing its solubility.
07

Conclusion

This example illustrates how the common-ion effect limits the dissolution of a sparingly soluble ionic compound, Calcium fluoride, by introducing an external source of fluoride ions, sodium fluoride, into the solution. The presence of the common ion, fluoride, causes the equilibrium to shift to minimize the change in the system, ultimately leading to a decrease in solubility for the sparingly soluble ionic compound.

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