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Ch.18 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 5th Edition
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Tutti i libri di testoTro 5th EditionCh.18 - Aqueous Ionic EquilibriumProblema 129
Capitolo 18, Problema 129

Calculate the solubility of CuX in a solution that is 0.150 M in NaCN. Ksp for CuX is 1.27⨉10-36.

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Identify the relevant chemical equilibrium: CuX(s) ⇌ Cu⁺(aq) + X⁻(aq).
Write the expression for the solubility product constant (Ksp): Ksp = [Cu⁺][X⁻].
Recognize that NaCN provides CN⁻ ions, which can complex with Cu⁺ to form Cu(CN)₂⁻, affecting the solubility of CuX.
Write the equilibrium expression for the complexation reaction: Cu⁺ + 2CN⁻ ⇌ Cu(CN)₂⁻, and note that this will reduce the concentration of free Cu⁺ ions.
Use the Ksp expression and the complexation equilibrium to set up equations that relate the solubility of CuX to the concentration of CN⁻, and solve for the solubility of CuX.

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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 is defined as the product of the molar concentrations of the ions, each raised to the power of their coefficients in the balanced equation. For a compound like CuX, Ksp helps determine how much of the compound can dissolve in a solution before reaching saturation.
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Solubility Product Constant

Common Ion Effect

The common ion effect refers to the decrease in solubility of an ionic compound when a common ion is added to the solution. In this case, the presence of NaCN introduces CN⁻ ions, which shifts the equilibrium of the dissolution of CuX, reducing its solubility. Understanding this effect is crucial for calculating the new solubility in the presence of a common ion.
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Common Ion Effect

ICE Table (Initial, Change, Equilibrium)

An ICE table is a tool used to track the concentrations of reactants and products during a chemical reaction at different stages: Initial, Change, and Equilibrium. For solubility calculations, it helps organize the initial concentrations of ions, the changes that occur as the system reaches equilibrium, and the final concentrations. This systematic approach is essential for accurately determining the solubility of CuX in the given solution.
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ICE Charts and Equilibrium Amount
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