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Ch.17 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 4th EditionCh.17 - Aqueous Ionic EquilibriumProblema 87b,c
Capitolo 17, Problema 87b,c

Refer to the Ksp values in Table 17.2 to calculate the molar solubility of each compound in pure water. b. Mg(OH)2 c. CaF2

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Identify the dissolution reaction for each compound. For Mg(OH)_2, the reaction is: Mg(OH)_2 (s) \(\rightleftharpoons\) Mg^{2+} (aq) + 2OH^- (aq). For CaF_2, the reaction is: CaF_2 (s) \(\rightleftharpoons\) Ca^{2+} (aq) + 2F^- (aq).
Write the expression for the solubility product constant (K_{sp}) for each compound. For Mg(OH)_2, K_{sp} = [Mg^{2+}][OH^-]^2. For CaF_2, K_{sp} = [Ca^{2+}][F^-]^2.
Let the molar solubility of Mg(OH)_2 be 's'. Then, [Mg^{2+}] = s and [OH^-] = 2s. Substitute these into the K_{sp} expression for Mg(OH)_2: K_{sp} = s(2s)^2.
Let the molar solubility of CaF_2 be 's'. Then, [Ca^{2+}] = s and [F^-] = 2s. Substitute these into the K_{sp} expression for CaF_2: K_{sp} = s(2s)^2.
Solve the equations for 's' using the given K_{sp} values from Table 17.2 to find the molar solubility of each compound.

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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 that can exist in a saturated solution at a given temperature. For a compound like Mg(OH)2, Ksp is calculated from the concentrations of its dissociated ions, allowing for the determination of its molar solubility in water.
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Solubility Product Constant

Dissociation of Ionic Compounds

Ionic compounds dissociate into their constituent ions when dissolved in water. For example, CaF2 dissociates into one calcium ion (Ca²⁺) and two fluoride ions (F⁻). Understanding the stoichiometry of this dissociation is crucial for calculating molar solubility, as it directly influences the concentrations of the ions involved in the Ksp expression.
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Ionic Compounds Naming

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 derived from the Ksp expression and reflects how much of a compound can dissolve in water. By setting up the Ksp expression based on the dissociation of the compound, one can solve for the molar solubility, which is essential for understanding the compound's behavior in aqueous solutions.
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Molar Solubility Example
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