   # Calculate the molar solubility of Mg(OH) 2 , K sp = 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 31E
Textbook Problem
1 views

## Calculate the molar solubility of Mg(OH)2, Ksp = 8.9 × 10−12.

Interpretation Introduction

Interpretation: The solubility product of Mg(OH)2 is given. The molar solubility of Mg(OH)2 is to be calculated.

Concept introduction: Solubility is defined as the maximum amount of solute that can dissolve at a certain amount of solvent at certain temperature. The solubility product, Ksp is the equilibrium constant that is applied when salt partially dissolve in a solvent. The solubility product of dissociation of AxBy is calculated as,

Ksp=[A]x[B]y

### Explanation of Solution

Explanation

To determine: The solubility of Mg(OH)2 from the given Ksp value.

The solubility of Mg(OH)2 is 1.3×104mol/L_ .

Given

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

Since, solid Mg(OH)2 is placed in contact with water. Therefore, compound present before the reaction is Mg(OH)2 and H2O . The dissociation reaction of Mg(OH)2 is,

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

Since, Mg2+ does not dissolved initially, hence,

[Mg2+]initial=0

It is assumed that initial concentration of OH is 1×107 .

The solubility of Mg(OH)2 can be calculated from the concentration of ions at equilibrium.

It is assumed that smol/L of solid is dissolved to reach the equilibrium. The meaning of 1:2 stoichiometry of salt is,

smol/LMg(OH)2smol/LMg2++2smol/LOH

Make the ICE table for the dissociation reaction of Mg(OH)2

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