Calculate the molar solubility of MX (K_sp = 1.27⨉10^-36) in each liquid or solution. b. 0.25 M MCl₂

검증된 단계별 안내

Step 1: Understand the dissolution process of MX in water. The dissolution of MX can be represented as: \[ \text{MX} \rightleftharpoons \text{M}^{2+} + \text{X}^{-} \]

Step 2: Write the expression for the solubility product constant (K_sp) for MX. The expression is: \[ K_{sp} = [\text{M}^{2+}][\text{X}^{-}] \]

Step 3: Consider the common ion effect due to the presence of 0.25 M MCl₂. Since MCl₂ dissociates completely, it contributes 0.25 M of \( \text{M}^{2+} \) ions to the solution.

Step 4: Let the molar solubility of MX be \( s \). The concentration of \( \text{M}^{2+} \) ions from MX will be \( s \), but due to the common ion effect, the total concentration of \( \text{M}^{2+} \) ions will be \( 0.25 + s \). The concentration of \( \text{X}^{-} \) ions will be \( s \).

Step 5: Substitute these concentrations into the K_sp expression: \[ K_{sp} = (0.25 + s)(s) \]. Since \( K_{sp} \) is very small, assume \( s \) is much smaller than 0.25, simplifying the expression to \[ K_{sp} \approx 0.25s \]. Solve for \( s \) to find the molar solubility.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

도움이 되었나요?

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 equilibrium, expressed in moles per liter (M). It is a crucial concept in understanding how substances dissolve and is often determined using the solubility product constant (Ksp) for sparingly soluble salts.

Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is an equilibrium constant that quantifies the solubility of a sparingly soluble ionic compound. It is defined as the product of the molar concentrations of the ions, each raised to the power of their coefficients in the balanced dissolution equation. A lower Ksp value indicates lower solubility.

Common Ion Effect

The common ion effect describes the decrease in solubility of a salt when a common ion is added to the solution. In this case, the presence of MCl2 introduces the ion M+, which shifts the equilibrium of the dissolution reaction of MX, reducing its molar solubility due to Le Chatelier's principle.

Calculate the molar solubility of MX (Ksp = 1.27⨉10-36) in each liquid or solution. b. 0.25 M MCl2