   # The solubility of Pb(IO 3 ) 2 ( s ) in a 7.2 × 10 −2 - M KIO 3 solution is 6.0 × 10 −9 mol/L. Calculate the K sp value for Pb(IO 3 ) 2 ( s ). ### 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 96CWP
Textbook Problem
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## The solubility of Pb(IO3)2(s) in a 7.2 × 10−2-M KIO3 solution is 6.0 × 10−9 mol/L. Calculate the Ksp value for Pb(IO3)2(s).

Interpretation Introduction

Interpretation: The solubility of Pb(IO3)2 in a 7.2×102 M KIO3 solution is given. The value of Ksp for Pb(IO3)2 is to be calculated.

Concept introduction: The constant Ksp is known as solubility product or solubility product constant. It is equilibrium constant and for a given solid, it has a particular value at a given temperature. However, the solubility is equilibrium position. The solubility product expression comprises of product of the ion concentrations.

### Explanation of Solution

Explanation

To determine: The Ksp value for Pb(IO3)2 .

Given

The solubility of Pb(IO3)2 in a 7.2×102 M KIO3 solution is 6.0×109 mol/L .

The salt Pb(IO3)2 dissolves according to the equilibrium given below.

Pb(IO3)2(s)Pb2+(aq)+2IO3(aq)

Since one mole of Pb(IO3)2 gives one mole of Pb2+ and two mole of IO3 .

Therefore, the concentration of Pb2+ =6.0×109 mol/L .

The concentration of IO3=2×6.0×109 mol/L=12×109 mol/L

The salt KIO3 dissolves according to the equilibrium given below.

KIO3(s)K+(aq)+IO3(aq)

The concentration of KIO3 is 7.2×102 mol/L .

Therefore, the concentration of IO3=7.2×102 mol/L .

The solubility product expression of Pb(IO3)2 is,

Ksp=[Pb2+][IO3-]total2

Where,

• Ksp is the solubility product of Pb(IO3)2 .
• [IO3-]total is the total concentration of IO3 from Pb(IO3)2 and KIO3

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