   # Calculate the concentration of Pb 2+ in each of the following. a. a saturated solution of Pb(OH) 2 , K sp = 1.2 × 10 −15 b. a saturated solution of Pb(OH) 2 buffered at pH = 13.00 c. Ethylenediaminetetraacetate (EDTA 4− ) is used as a complexing agent in chemical analysis and has the following structure: Solutions of EDTA 4− are used to treat heavy metal poisoning by removing the heavy metal in the form of a soluble complex ion. The reaction of EDTA 4− with Pb 2+ is Pb 2 + ( a q ) + E D T A 4 − ( a q ) ⇌ P b E D T A 2 − ( a q ) K = 1.1 × 10 18 Consider a solution with 0.010 mole of Pb(NO 3 ) 2 added to 1.0 L of an aqueous solution buffered at pH = 13.00 and containing 0.050 M Na 4 .EDTA. Does Pb(OH) 2 precipitate from this solution? ### 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 87AE
Textbook Problem
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## Calculate the concentration of Pb2+ in each of the following.a. a saturated solution of Pb(OH)2, Ksp = 1.2 × 10−15b. a saturated solution of Pb(OH)2 buffered at pH = 13.00c. Ethylenediaminetetraacetate (EDTA4−) is used as a complexing agent in chemical analysis and has the following structure: Solutions of EDTA4− are used to treat heavy metal poisoning by removing the heavy metal in the form of a soluble complex ion. The reaction of EDTA4− with Pb2+ is Pb 2 + ( a q )   +   E D T A 4 −   ( a q )   ⇌   P b E D T A 2 − ( a q )   K   =   1.1   ×   10 18 Consider a solution with 0.010 mole of Pb(NO3)2 added to 1.0 L of an aqueous solution buffered at pH = 13.00 and containing 0.050 M Na4.EDTA. Does Pb(OH)2 precipitate from this solution?

(a)

Interpretation Introduction

Interpretation: The concentration of Pb2+ is to be calculated in each of the given cases.

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 by the formula,

Ksp=[A]x[B]y

### Explanation of Solution

Explanation

To determine: The concentration of Pb2+ is to be calculated in a saturated solution of Pb(OH)2 .

The solubility of Pb2+ is 6.7×10-6mol/L_ .

The reaction at equilibrium is,

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

The solubility product of dissociation of Pb(OH)2 is calculated by the formula,

Ksp=[Pb2+][OH]

The solubility of Pb(OH)2 can be calculated from the concentration of its 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/LPb(OH)2smol/LPb2++2smol/OH

Formula

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

Ksp=[Pb2+][OH]2

Where,

• Ksp is solubility product

(b)

Interpretation Introduction

Interpretation: The concentration of Pb2+ is to be calculated in each of the given cases.

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 by the formula,

Ksp=[A]x[B]y

(c)

Interpretation Introduction

Interpretation: The concentration of Pb2+ is to be calculated in each of the given cases.

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 by the formula,

Ksp=[A]x[B]y

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