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. (d) Ba1NO322

검증된 단계별 안내

Identify the equilibrium reaction for the dissolution of BaF_2: \[ \text{BaF}_2 (s) \rightleftharpoons \text{Ba}^{2+} (aq) + 2\text{F}^- (aq) \]

Recognize that adding Ba(NO_3)_2 will increase the concentration of \( \text{Ba}^{2+} \) ions in the solution.

Apply Le Châtelier's principle, which states that if a system at equilibrium is disturbed, the system will shift in a direction that counteracts the disturbance.

Determine the direction of the shift: the increase in \( \text{Ba}^{2+} \) concentration will cause the equilibrium to shift to the left, favoring the formation of solid BaF_2.

Conclude that the solubility of BaF_2 will decrease as a result of adding Ba(NO_3)_2, due to the common ion effect.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

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 the solubility of a compound, like BaF2, will respond to the addition of other substances.

Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is an equilibrium constant that applies to the solubility of sparingly soluble ionic compounds. For BaF2, the Ksp expression involves the concentrations of Ba²⁺ and F⁻ ions in solution. Changes in these ion concentrations, due to the addition of other substances, can shift the equilibrium and affect 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 Ba(NO3)2 introduces Ba²⁺ ions, which can shift the equilibrium to the left, reducing the solubility of BaF2 due to the common ion effect.