   # Calculate the solubility of Co(OH) 2 ( s ) ( K sp = 2.5 × 10 −16 ) in a buffered solution with a pH of 11.00. ### 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 38E
Textbook Problem
25 views

## Calculate the solubility of Co(OH)2(s) (Ksp = 2.5 × 10−16) in a buffered solution with a pH of 11.00.

Interpretation Introduction

Interpretation: The solubility product of Co(OH)2 is given. The solubility of Co(OH)2 is to be calculated for the given pH value.

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

Where,

• x is coefficient of concentration of A .
• y is coefficient of concentration of B .

The ion product of water is calculated using the formula,

Kw=[H+][OH]

Where,

• Kw is ion product of water (1×1014) .

### Explanation of Solution

Explanation

To determine: The solubility of Co(OH)2 in a buffered solution at pH=11.0 .

The concentration of H+ is 1.0×1011M_ .

Given

Solubility product of Co(OH)2 is 2.5×1016 .

The pH value of buffered solution is 11.0 .

Formula

The pH is calculated using the formula,

pH=log10[H+]

Substitute the value of pH in the above equation.

pH=log10[H+]11.0=log10[H+][H+]=1.0×1011M_

The concentration of OH is 1.0×103M_ .

The concentration of H+ is 1.0×1011M .

Formula

The ion product of water is calculated using the formula,

Kw=[H+][OH]

Where,

• Kw is ion product of water (1×1014) .

Substitute the values of [H+] and Kw in the above equation.

Kw=[H+][OH](1×1014)=(1.0×1011M)[OH][OH]=1.0×103M_

The solubility of Co(OH)2 in a buffered solution at pH=11.0 is 2.5×1010mol/L_ .

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

The dissociation reaction of Co(OH)2 is,

Co(OH)2(s)Co2+(aq)+2OH(aq)

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

smol/LCo(OH)2smol/LCo2++2smol/LOH

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

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