   # Calculate the molar solubility of Cd(OH) 2 , K sp = 5.9 × 10 −11 . ### 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 32E
Textbook Problem
3 views

## Calculate the molar solubility of Cd(OH)2, Ksp = 5.9 × 10−11.

Interpretation Introduction

Interpretation: The solubility product of Cd(OH)2 is given. The molar solubility of Cd(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 Cd(OH)2 from the given Ksp value.

The solubility of Cd(OH)2 is 2.4×104mol/L_ .

Given

Solubility product of Cd(OH)2 is 5.9×1011 .

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

Cd(OH)2(s)Cd2+(aq)+2OH(aq)

Since, Cd2+ does not dissolved initially, hence,

[Cd2+]initial=0

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

The solubility of Cd(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/LCd(OH)2smol/LCd2++2smol/LOH

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

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