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Calculate the solubility of Mg(OH) 2 (K sp = 8.9 × 10 −12 ) in an aqueous solution buffered at pH = 9.42.
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Chemistry: An Atoms First Approach
2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
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Chapter
Section
BuyFindarrow_forward
Chemistry: An Atoms First Approach
2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 19, Problem 89CWP
Textbook Problem
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Calculate the solubility of Mg(OH)2 (Ksp = 8.9 × 10−12) in an aqueous solution buffered at pH = 9.42.
Interpretation Introduction
Interpretation: The solubility of
Concept introduction: The concentration of hydroxide ion is calculated as,
The solubility product constant is calculated by the formula,
To determine: The solubility of
Explanation of Solution
Given
The
The solubility product constant,
The concentration of hydroxide ion is calculated as,
Substitute the value of
The dissolution equilibrium of
The solubility of
The concentration of the ions formed in the above reaction is shown in the table below,
Chapter 19 Solutions
Chemistry: An Atoms First Approach
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