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Ch.18 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 5th Edition
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 5th EditionCh.18 - Aqueous Ionic EquilibriumProblema 95c
Capitolo 18, Problema 95c

Calculate the molar solubility of barium fluoride in each liquid or solution. c. 0.15 M NaF

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Identify the dissolution reaction of barium fluoride: \( \text{BaF}_2 (s) \rightleftharpoons \text{Ba}^{2+} (aq) + 2\text{F}^- (aq) \).
Write the expression for the solubility product constant \( K_{sp} \) for barium fluoride: \( K_{sp} = [\text{Ba}^{2+}][\text{F}^-]^2 \).
Recognize that the presence of 0.15 M NaF provides a common ion, \( \text{F}^- \), which affects the solubility of \( \text{BaF}_2 \).
Let the molar solubility of \( \text{BaF}_2 \) be \( s \). Then, \([\text{Ba}^{2+}] = s\) and \([\text{F}^-] = 0.15 + 2s\).
Substitute these concentrations into the \( K_{sp} \) expression and solve for \( s \), considering that \( s \) is small compared to 0.15 M.

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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.
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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, adding NaF introduces fluoride ions (F-) into the solution, which shifts the equilibrium of barium fluoride dissolution, reducing its molar solubility due to Le Chatelier's principle.
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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 conditions.
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Equilibrium Constant K
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