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. (c) NaNO3

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Identify the reaction involved: The dissolution of barium fluoride (BaF2) in water can be represented by the equation: BaF2(s) ⇌ Ba^{2+}(aq) + 2F^{-}(aq).

Recognize the nature of the added substance: Sodium nitrate (NaNO3) dissociates in water to form Na+ and NO3- ions.

Analyze the effect of the added ions on the existing equilibrium: Since neither Na+ nor NO3- ions appear in the dissolution equation of BaF2, they do not directly interact with the Ba^{2+} or F^{-} ions.

Apply Le Châtelier's Principle: Adding NaNO3 does not introduce any ions that would shift the equilibrium of the BaF2 dissolution reaction. Therefore, the position of the equilibrium remains unchanged.

Predict the effect on solubility: Since the equilibrium is not shifted by the addition of NaNO3, the solubility of BaF2 in water will remain the same.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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 solubility of a compound in a solution.

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 in solution can shift the equilibrium, affecting solubility.

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 NaNO3 introduces Na+ ions but does not directly affect the equilibrium of BaF2. However, if the added ions affect the concentration of F- ions, it can influence the solubility of BaF2 through the common ion effect.

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