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Ch.18 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 6th EditionCh.18 - Aqueous Ionic EquilibriumProblema 101b
Capitolo 18, Problema 101b

Calculate the molar solubility of barium fluoride in each liquid or solution. b. 0.10 M Ba(NO3)2

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Write the dissolution equation for barium fluoride (BaF2): BaF2(s) ⇌ Ba2+(aq) + 2F-(aq).
Identify the initial concentrations of the ions in the solution. Since the solution already contains 0.10 M Ba(NO3)2, the initial concentration of Ba2+ is 0.10 M. The initial concentration of F- is 0 M.
Set up the expression for the solubility product constant (Ksp) of BaF2, which is given by Ksp = [Ba2+][F-]2. Let 's' be the molar solubility of BaF2 in the 0.10 M Ba(NO3)2 solution.
Substitute the equilibrium concentrations into the Ksp expression. Since Ba2+ is already present at 0.10 M, the concentration at equilibrium will be 0.10 M + s. The concentration of F- at equilibrium will be 2s.
Solve the equation for 's' to find the molar solubility of BaF2 in the 0.10 M Ba(NO3)2 solution. This involves substituting the expressions for the equilibrium concentrations into the Ksp equation and solving for 's'.

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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, the presence of Ba<sup>2+</sup> ions from Ba(NO<sub>3</sub>)<sub>2</sub> will shift 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 solutions.
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Equilibrium Constant K
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