Calculate the molar solubility of Ni(OH)₂ when buffered at pH (b) 10.0.

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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: Use the relation pOH = 14 - pH to find pOH, then calculate [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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주요 개념

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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 (mol/L). It is a crucial concept in understanding how substances interact in solution, particularly for sparingly soluble compounds like Ni(OH)2. The molar solubility can be influenced by factors such as pH, temperature, and the presence of other ions in solution.

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 nickel(II) hydroxide, Ni(OH)2, an increase in pH (making the solution more basic) can enhance its solubility due to the formation of soluble nickel complexes. Understanding how pH influences the dissociation of hydroxides is essential for calculating molar solubility in buffered solutions.

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. By knowing the Ksp value and the pH of the solution, one can derive the molar solubility by setting up an equilibrium expression that accounts for the concentration of hydroxide ions, which are influenced by the pH.

Calculate the molar solubility of Ni(OH)2 when buffered at pH (b) 10.0.