Use the given molar solubilities in pure water to calculate Ksp for each compound. a. MX; molar solubility = 3.27⨉10^-11 M

검증된 단계별 안내

Identify the dissolution equation for the compound MX: MX(s) \(\rightleftharpoons\) M^+(aq) + X^-(aq).

Recognize that the molar solubility of MX is given as 3.27 \(\times\) 10^{-11} M, which means [M^+] = [X^-] = 3.27 \(\times\) 10^{-11} M at equilibrium.

Write the expression for the solubility product constant (K_{sp}): K_{sp} = [M^+][X^-].

Substitute the equilibrium concentrations into the K_{sp} expression: K_{sp} = (3.27 \(\times\) 10^{-11})(3.27 \(\times\) 10^{-11}).

Calculate the K_{sp} value by multiplying the concentrations.

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 is the number of moles of a solute that can dissolve in a liter of solvent at a given temperature, expressed in moles per liter (M). It provides a quantitative measure of how much of a compound can dissolve to form a saturated solution. Understanding molar solubility is essential for calculating the solubility product constant (Ksp) of ionic compounds.

Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is an equilibrium constant that reflects the extent to which a sparingly soluble ionic compound dissolves in water. It is calculated from the concentrations of the ions in a saturated solution, raised to the power of their coefficients in the balanced dissolution equation. Ksp values are crucial for predicting the solubility of compounds and understanding precipitation reactions.

Dissociation of Ionic Compounds

When ionic compounds dissolve in water, they dissociate into their constituent ions. For example, a compound MX will dissociate into M⁺ and X⁻ ions. The stoichiometry of this dissociation is important for calculating Ksp, as the concentrations of the ions produced directly influence the Ksp value. Understanding this process is vital for accurately determining the solubility product from molar solubility.

Use the given molar solubilities in pure water to calculate Ksp for each compound. a. MX; molar solubility = 3.27⨉10-11 M