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Ch.17 - Additional Aspects of Aqueous Equilibria
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 14th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 108
Capitolo 17, Problema 108

The solubility product for Zn1OH22 is 3.0 * 10-16. The formation constant for the hydroxo complex, Zn1OH242 - , is 4.6 * 1017. What concentration of OH- is required to dissolve 0.015 mol of Zn1OH22 in a liter of solution?

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1
Identify the dissolution reaction for Zn(OH)_2: Zn(OH)_2 (s) \(\rightleftharpoons\) Zn^{2+} (aq) + 2OH^- (aq).
Write the expression for the solubility product (K_{sp}): K_{sp} = [Zn^{2+}][OH^-]^2.
Identify the formation reaction for the hydroxo complex: Zn^{2+} (aq) + 4OH^- (aq) \(\rightleftharpoons\) [Zn(OH)_4]^{2-} (aq).
Write the expression for the formation constant (K_f): K_f = \(\frac{[Zn(OH)_4^{2-}\)]}{[Zn^{2+}][OH^-]^4}.
Set up the equilibrium expressions and solve for [OH^-] using the given K_{sp} and K_f values, considering the total concentration of Zn(OH)_2 initially present.

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Solubility Product (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 Zn(OH)2, Ksp = [Zn^2+][OH^-]^2, which helps determine the concentration of ions in a saturated solution.
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01:47
Solubility Product Constant

Formation Constant (Kf)

The formation constant (Kf) quantifies the stability of a complex ion in solution. It is defined as the equilibrium constant for the formation of a complex from its constituent ions. In this case, Kf for Zn(OH)4^2- indicates how readily Zn^2+ ions react with OH- ions to form the hydroxo complex, influencing the solubility of Zn(OH)2 in the presence of hydroxide ions.
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Complex Ions and Formation Constant

Equilibrium and Le Chatelier's Principle

Equilibrium in chemistry refers to the state where the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. Le Chatelier's Principle states that if a system at equilibrium is disturbed, it will shift in a direction that counteracts the disturbance. This principle is crucial for understanding how changes in OH- concentration affect the solubility of Zn(OH)2 and the formation of its hydroxo complex.
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Le Chatelier's Principle
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