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Ch.17 - Additional Aspects of Aqueous Equilibria
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 15th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 58c
Capitolo 17, Problema 58c

Calculate the solubility of LaF3 in grams per liter in (c) 0.050 M LaCl3 solution.

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Identify the dissolution reaction of LaF_3: LaF_3(s) \(\rightleftharpoons\) La^{3+}(aq) + 3F^{-}(aq).
Write the expression for the solubility product constant (K_{sp}) for LaF_3: K_{sp} = [La^{3+}][F^{-}]^3.
Recognize that in a 0.050 M LaCl_3 solution, the concentration of La^{3+} ions is already 0.050 M due to the complete dissociation of LaCl_3.
Assume the solubility of LaF_3 is 's' mol/L. The concentration of F^{-} ions will be 3s, and the concentration of La^{3+} ions will be 0.050 + s.
Substitute these concentrations into the K_{sp} expression and solve for 's', considering that 's' is small compared to 0.050 M, so 0.050 + s \(\approx\) 0.050.

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Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is a numerical value that represents the equilibrium between a solid and its ions in a saturated solution. For a salt like LaF3, Ksp is determined by the concentrations of the ions produced when the salt dissolves. Understanding Ksp is essential for calculating solubility, especially in the presence of common ions, as it helps predict how much of the salt can dissolve in a given solution.
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Solubility Product Constant

Common Ion Effect

The common ion effect refers to the decrease in solubility of a salt when a common ion is added to the solution. In this case, the presence of LaCl3 introduces La³⁺ ions, which shifts the dissolution equilibrium of LaF3 to the left, reducing its solubility. This concept is crucial for understanding how the solubility of LaF3 is affected in a solution already containing La³⁺ ions.
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Common Ion Effect

Stoichiometry of Dissolution

Stoichiometry of dissolution involves understanding the ratio of ions produced when a compound dissolves. For LaF3, the dissolution can be represented as LaF3(s) ⇌ La³⁺(aq) + 3F⁻(aq). This stoichiometric relationship is important for calculating the concentrations of La³⁺ and F⁻ ions in solution, which are necessary for determining the solubility of LaF3 in the presence of LaCl3.
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Stoichiometry Concept
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