EDTA is used as a complexing agent in chemical analysis. Solutions of EDTA, usually containing the disodium salt Na 2 H 2 EDTA, are also used to treat heavy metal poisoning. The equilibrium constant for the following reaction is 6.7 × 10 21 : Calculate [Pb 2+ ] at equilibrium in a solution originally 0.0050 M in Pb 2+ , 0.075 M in H 2 EDTA 2− , and buffered at pH = 7.00.

Q: Expert Answer

Interpretation Introduction Interpretation: The equilibrium constant of a reaction, pH value of buffer solution, concentration of solution in Pb 2 + and concentration of solution in H 2 EDTA 2 − is given. The concentration of Pb 2 + at equilibrium is to be calculated. Concept introduction: At equilibrium, the equilibrium constant expression is expressed by the formula, K = Concentration of products Concentration of reactants To determine: The concentration of Pb 2 + at equilibrium for the given reaction. Explanation Explanation The [ H + ] is 1 × 10 − 7 M _ . Given The pH value is 6.00 . Formula The concentration of H + is calculated using the formula, pH = − log 10 [ H + ] Substitute the value of pH in the above equation. pH = − log 10 [ H + ] 7 .00 = − log 10 [ H + ] [ H + ] = 1 × 10 − 7 M _ The concentration of Pb 2 + at equilibrium for the given reaction is 8 . 6 × 1 0 5 M _ . Given The value of K is 6.7 × 10 21 . Concentration of solution in Pb 2 + is 0.0050 M . Concentration of solution in H 2 EDTA 2 − is 0.075 M . The given reaction is, Pb 2 + ( s ) + H 2 EDTA 2 − ( a q ) ⇌ PbEDTA 2 − ( a q ) + 2 H + ( a q ) The ICE table for the stated reaction is formed. Pb 2+ ( a q ) + H 2 EDTA 2 − ( a q ) ⇌ PbEDTA − ( a q ) + 2 H + ( a q ) Initial ( M ) : 0.0050 0.070 0 0 Change ( M ) − x − x + x + 2 x Equilibrium ( M ) : 0

Question

Still sussing out bartleby?

Answer 1

BuyFind

Chemistry: An Atoms First Approach

2nd Edition

Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

Solutions

Chapter

Section

Answer 2

BuyFind

Chemistry: An Atoms First Approach

2nd Edition

Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

Solutions

Chapter

Section

Answer 3

Solutions

Chapter

Section

Answer 4

Chapter

Section

Answer 5

Interpretation Introduction

Interpretation: The equilibrium constant of a reaction, pH value of buffer solution, concentration of solution in Pb2+ and concentration of solution in H2EDTA2− is given. The concentration of Pb2+ at equilibrium is to be calculated.

Concept introduction: At equilibrium, the equilibrium constant expression is expressed by the formula,

K=Concentration of productsConcentration of reactants

To determine: The concentration of Pb2+ at equilibrium for the given reaction.

Explanation of Solution

Explanation

The [H+] is 1×10−7 M_ .

Given

The pH value is 6.00 .

Formula

The concentration of H+ is calculated using the formula,

pH=−log10[H+]

Substitute the value of pH in the above equation.

pH=−log10[H+]7.00=−log10[H+][H+]=1×10−7 M_

The concentration of Pb2+ at equilibrium for the given reaction is 8.6×105 M_ .

Given

The value of K is 6.7×1021 .

Concentration of solution in Pb2+ is 0.0050 M .

Concentration of solution in H2EDTA2− is 0.075 M .

The given reaction is,

Pb2+(s)+H2EDTA2−(aq)⇌PbEDTA2−(aq)+2H+(aq)

The ICE table for the stated reaction is formed.

Pb2+(aq)+H2EDTA2−(aq)⇌PbEDTA−(aq)+2H+(aq)Initial(M): 0.00500.07000Change(M) −x−x+x+2xEquilibrium(M):0

Chemistry: An Atoms First Approach

Solutions

Chemistry: An Atoms First Approach

Explanation of Solution

Still sussing out bartleby?

The Solution to Your Study Problems

Chapter 19 Solutions

Additional Science Textbook Solutions