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Ch.17 - Applications of Aqueous Equilibria
McMurry - Chemistry 8th Edition
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Capitolo 17, Problema 110b

Use Le Châtelier's principle to predict whether the solubility of BaF2 will increase, decrease, or remain the same on addition of each of the following substances. (b) KF

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Identify the dissolution reaction of BaF2 in water: BaF2(s) ⇌ Ba^{2+}(aq) + 2F^{-}(aq).
Recognize that KF dissociates completely in water to form K^{+}(aq) and F^{-}(aq). Adding KF to the solution increases the concentration of F^{-}(aq).
Apply Le Châtelier's principle, which states that if a system at equilibrium is disturbed, it will shift in a direction that helps counteract the disturbance.
Understand that increasing the concentration of F^{-}(aq) by adding KF will shift the equilibrium to the left, according to Le Châtelier's principle, to reduce the excess fluoride ions.
Conclude that the shift of the equilibrium to the left will result in the formation of more solid BaF2, thus decreasing the solubility of BaF2 in the solution.

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Le Châtelier's Principle

Le Châtelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. This principle is crucial for predicting how changes in concentration, pressure, or temperature will affect the position of equilibrium in a chemical reaction.
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Le Chatelier's Principle

Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is an equilibrium constant that applies to the solubility of sparingly soluble ionic compounds. It quantifies the extent to which a compound can dissolve in water, and changes in the concentration of ions can shift the equilibrium, affecting solubility. For BaF2, the Ksp expression involves the concentrations of Ba²⁺ and F⁻ ions.
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Solubility Product Constant

Common Ion Effect

The common ion effect refers to the decrease in solubility of an ionic compound when a common ion is added to the solution. In the case of BaF2, adding KF introduces K⁺ and F⁻ ions, which can shift the equilibrium position according to Le Châtelier's Principle, leading to a decrease in the solubility of BaF2 due to the increased concentration of the common ion F⁻.
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Common Ion Effect
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