Refer to the Ksp values in Table 17.2 to calculate the molar solubility of each compound in pure water. a. MX (Ksp = 1.27⨉10^-36) b. Ag₂CrO₄ c. Ca(OH)₂

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Identify the dissolution equation for each compound. For example, for MX, the dissolution is MX(s) \(\rightleftharpoons\) M^+(aq) + X^-(aq).

Write the expression for the solubility product constant (K_{sp}) for each compound. For MX, K_{sp} = [M^+][X^-].

Express the concentrations of the ions in terms of the molar solubility (s). For MX, [M^+] = s and [X^-] = s, so K_{sp} = s^2.

Solve for the molar solubility (s) by substituting the given K_{sp} value into the expression and solving for s. For MX, s = \(\sqrt{K_{sp}\)}.

Repeat the process for Ag_2CrO_4 and Ca(OH)_2, considering their respective dissolution equations and stoichiometry. For Ag_2CrO_4, K_{sp} = [Ag^+]^2[CrO_4^{2-}], and for Ca(OH)_2, K_{sp} = [Ca^{2+}][OH^-]^2.

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주요 개념

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Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is an equilibrium constant that applies to the solubility of sparingly soluble ionic compounds. It represents the maximum concentration of ions in a saturated solution at a given temperature. For a salt MX that dissociates into M⁺ and X⁻, Ksp is expressed as Ksp = [M⁺][X⁻]. Understanding Ksp is crucial for calculating the molar solubility of compounds in water.

Molar Solubility

Molar solubility is defined as the number of moles of a solute that can dissolve in one liter of solution at equilibrium. It is directly related to the Ksp value of the compound; a higher Ksp indicates greater molar solubility. To find the molar solubility, one must set up an expression based on the dissociation of the compound and solve for the concentration of the ions in solution.

Dissociation of Ionic Compounds

Ionic compounds dissociate into their constituent ions when they dissolve in water. For example, when Ca(OH)₂ dissolves, it separates into Ca²⁺ and 2OH⁻ ions. The stoichiometry of this dissociation is essential for calculating molar solubility, as it determines the relationship between the concentrations of the ions and the Ksp value. Understanding this process is key to solving solubility problems.

Refer to the Ksp values in Table 17.2 to calculate the molar solubility of each compound in pure water. a. MX (Ksp = 1.27⨉10-36) b. Ag2CrO4 c. Ca(OH)2