   # The concentration of Mg 2+ in seawater is 0.052 M . At what pH will 99% of the Mg 2+ be precipitated as the hydroxide salt? [ K sp for Mg(OH) 2 = 8.9 × 10 −12 . ] ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 15, Problem 48E
Textbook Problem
447 views

## The concentration of Mg2+ in seawater is 0.052 M. At what pH will 99% of the Mg2+ be precipitated as the hydroxide salt? [Ksp for Mg(OH)2 = 8.9 × 10−12.]

Interpretation Introduction

Interpretation: The solubility product of Mg(OH)2 and concentration of Mg2+ is given. The pH value at which the given percentage of Mg2+ is precipitated as the hydroxide salt is to be calculated.

Concept introduction: The formation of solid in a solution is known as precipitation.

The solubility product, Ksp is the equilibrium constant that is applied when a salt partially dissolves in a solvent. The solubility product of dissociation of AxBy is calculated by the formula,

Ksp=[A]x[B]y

The relation between pH and pOH is,

pH+pOH=14

### Explanation of Solution

Explanation

To determine: The pH value at which the given percentage of Mg2+ is precipitated as the hydroxide salt.

The total concentration of Mg2+ is 0.051M_ .

Given

Solubility product of Mg(OH)2 is 8.9×1012 .

Concentration of Mg2+ in sea water is 0.052M .

It is given that 99% of Mg2+ is precipitated as the hydroxide salt, but the concentration of Mg2+ in sea water is 0.052M . Therefore, the total concentration of Mg2+ is,

99100×0.052M=0.051M_

The concentration of OH is 1.3×105M_ .

The dissociation reaction of Mg(OH)2 is,

Mg(OH)2(s)Mg2+(aq)+2OH(aq)

The ratio of moles between ions is 1:2 .

Formula

The solubility product of Mg(OH)2 is calculated as,

Ksp=[Mg2+][OH]2

Where,

• Ksp is the solubility product.
• [Mg2+] is the concentration of Mg2+ .
• [OH] is the concentration of OH

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