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Ch.18 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 5th Edition
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Tro 5th EditionCh.18 - Aqueous Ionic Equilibrium문제 95b
18장, 문제 95b

Calculate the molar solubility of barium fluoride in each liquid or solution. b. 0.10 M Ba(NO3)2

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1
Write the dissolution equation for barium fluoride (BaF2): BaF2(s) ⇌ Ba2+(aq) + 2F-(aq).
Identify the initial concentrations of the ions in the solution. Since the solution already contains 0.10 M Ba(NO3)2, the initial concentration of Ba2+ is 0.10 M. The initial concentration of F- is 0 M.
Set up the expression for the solubility product constant (Ksp) of BaF2, which is given by Ksp = [Ba2+][F-]2. Let 's' be the molar solubility of BaF2 in the 0.10 M Ba(NO3)2 solution.
Substitute the equilibrium concentrations into the Ksp expression. Since Ba2+ is already present at 0.10 M, the concentration at equilibrium will be 0.10 M + s. The concentration of F- at equilibrium will be 2s.
Solve the equation for 's' to find the molar solubility of BaF2 in the 0.10 M Ba(NO3)2 solution. This involves substituting the expressions for the equilibrium concentrations into the Ksp equation and solving for 's'.

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주요 개념

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

Molar Solubility

Molar solubility refers to the maximum amount of a solute that can dissolve in a given volume of solvent at a specific temperature, expressed in moles per liter (M). It is a crucial concept in understanding how ionic compounds dissociate in solution and is often determined through equilibrium expressions.
추천 영상:
가이드 코스
04:13
Molar Solubility Example

Common Ion Effect

The common ion effect describes the decrease in solubility of an ionic compound when a common ion is added to the solution. In this case, the presence of Ba<sup>2+</sup> ions from Ba(NO<sub>3</sub>)<sub>2</sub> will shift the equilibrium of barium fluoride dissolution, reducing its molar solubility due to Le Chatelier's principle.
추천 영상:
가이드 코스
02:53
Common Ion Effect

Equilibrium Constant (Ksp)

The solubility product constant (Ksp) is an equilibrium constant that applies to the dissolution of sparingly soluble ionic compounds. It quantifies the product of the molar concentrations of the ions in a saturated solution, raised to the power of their coefficients in the balanced dissolution equation, and is essential for calculating molar solubility in different solutions.
추천 영상:
가이드 코스
01:14
Equilibrium Constant K
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