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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 62a
Capitolo 17, Problema 62a

Calculate the molar solubility of Ni(OH)2 when buffered at pH (a) 8.0.

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1
Identify the dissolution equation for Ni(OH)_2: Ni(OH)_2(s) \(\rightleftharpoons\) Ni^{2+}(aq) + 2OH^{-}(aq).
Write the expression for the solubility product constant (K_{sp}) for Ni(OH)_2: K_{sp} = [Ni^{2+}][OH^{-}]^2.
Determine the concentration of OH^{-} ions from the given pH. Since pH + pOH = 14, calculate pOH = 14 - 8.0 = 6.0, then find [OH^{-}] = 10^{-pOH}.
Substitute the [OH^{-}] value into the K_{sp} expression and solve for [Ni^{2+}], which represents the molar solubility of Ni(OH)_2.
Use the known K_{sp} value for Ni(OH)_2 to calculate the molar solubility by substituting the [OH^{-}] concentration and solving for [Ni^{2+}].

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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 substances interact in solution and is influenced by factors such as temperature, pressure, and the presence of other ions.
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Molar Solubility Example

pH and its Effect on Solubility

pH is a measure of the acidity or basicity of a solution, which can significantly affect the solubility of certain compounds. For metal hydroxides like Ni(OH)2, an increase in pH (making the solution more basic) typically increases solubility due to the formation of soluble complexes or the reduction of the concentration of hydroxide ions that would otherwise precipitate the metal hydroxide.
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Solubility at Buffered pH Example

Equilibrium and Ksp

The solubility product constant (Ksp) is an equilibrium constant that applies to the dissolution of sparingly soluble ionic compounds. For Ni(OH)2, the Ksp expression relates the concentrations of the ions in solution at equilibrium. Understanding Ksp is essential for calculating molar solubility, especially when pH influences the concentration of hydroxide ions in the solution.
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Ksp Calculations
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