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Ch.17 - Additional Aspects of Aqueous Equilibria
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 14th EditionCh.17 - Additional Aspects of Aqueous Equilibria문제 62a
17장, 문제 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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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 (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.
추천 영상:
가이드 코스
04:13
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.
추천 영상:
가이드 코스
05:30
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.
추천 영상:
가이드 코스
01:51
Ksp Calculations
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