Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Chapter 15, Problem 63E

Consider the titration of 40.0 mL of 0.200 M HClO4 by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added.

a. 0.0 mL

b. 10.0 mL

c. 40.0 mL

d. 80.0 mL

e. 100.0 mL

(a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The titration concentration of KOH , volume and concentration of HClO4 is given. The pH of resulting solution after the addition of KOH is to be calculated for the given volumes of KOH .

Concept introduction:

Titration is a process to determine the concentration of an unknown solution with the help of a solution of a known concentration value.

The pH is calculated using the formula,

pH=log10[H+]

The relation between pH and pOH is,

pH+pOH=14

To determine the pH of the resulting solution, after the addition of 0.0mL of KOH .

Answer to Problem 63E

The pH of the resulting solution, after the addition of 0.0mL of KOH is 0.699_ .

Explanation of Solution

Explanation

Given

Concentration of HClO4 is 0.200M .

HClO4 is a strong acid; hence, it completely dissociates into ions. The major species present in the solution are H+,ClO4 and H2O .

The pH is determined by [H+] present in the solution.

Since HClO4 completely dissociates into ions, 0.200M HClO4 contains 0.200M H+ .

Formula

The pH is calculated using the formula,

pH=log10[H+]

Where,

  • [H+] is concentration of H+ ions.

Substitute the value of [H+] in the above equation.

pH=log10[H+]=log10(0.200)=0.699_

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The titration concentration of KOH , volume and concentration of HClO4 is given. The pH of resulting solution after the addition of KOH is to be calculated for the given volumes of KOH .

Concept introduction:

Titration is a process to determine the concentration of an unknown solution with the help of a solution of a known concentration value.

The pH is calculated using the formula,

pH=log10[H+]

The relation between pH and pOH is,

pH+pOH=14

To determine the concentration of H+

Answer to Problem 63E

The pH of the resulting solution, after the addition of 10.0mL of KOH is 0.853_ .

Explanation of Solution

Explanation

Given

Concentration of HClO4 is 0.200M .

Concentration of KOH is 0.100M .

Volume of HClO4 original solution is 40mL .

Volume of KOH added is 10mL .

Large quantities of the H+ ions and the OH ions are present. The 1.0mmol (10.0mL×0.100M) of the OH added will react with 1.0mmol H+ to form water:

H++OHH2OBeforereaction40.0mL×0.200M=8.0mmol10.0mL×0.100M=1.00mmolAfterreaction8.01.00=7.0mmol1.001.00=0

After the reaction, the solution contains H+,ClO4,K+ and H2O (the OH ions get consumed).

Formula

The H+ ion concentration, remaining in a given solution, is calculated by the formula,

[H+]=mmolH+leftVolumeoforiginalsolution(mL)×Volumeofcompoundadded(mL)

Substitute the values of mmoles of H+ left, volume of the original solution and the volume of the compound added in the above equation.

[H+]=mmolH+leftVolumeoforiginalsolution(mL)×Volumeofcompoundadded(mL)=7.0mmol(40.0+10.0)mL=0.14M_

To find the pH of the resulting solution, after the addition of 10.0mL of KOH

Formula

The pH is calculated using the formula,

pH=log10[H+]

Where,

  • [H+] is concentration of H+ ions.

Substitute the value of is concentration of [H+] in the above equation.

pH=log10[H+]=log10(0.14)=0.853_

(c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The titration concentration of KOH , volume and concentration of HClO4 is given. The pH of resulting solution after the addition of KOH is to be calculated for the given volumes of KOH .

Concept introduction:

Titration is a process to determine the concentration of an unknown solution with the help of a solution of a known concentration value.

The pH is calculated using the formula,

pH=log10[H+]

The relation between pH and pOH is,

pH+pOH=14

Answer to Problem 63E

The pH of the resulting solution, after the addition of 40.0mL of KOH is 1.30_ .

Explanation of Solution

Explanation

To determine the concentration of H+

Given

Concentration of HClO4 is 0.200M .

Concentration of KOH is 0.100M .

Volume of HClO4 original solution is 40mL .

Volume of KOH added is 40.0mL .

Large quantities of the H+ ions and the OH ions are present. The 4.0mmol (40.0mL×0.100M) of the OH added will react with 1.0mmol H+ to form water:

H++OHH2OBeforereaction40.0mL×0.200M=8.0mmol40.0mL×0.100M=4.00mmolAfterreaction8.04.00=4.0mmol4.004.00=0

After the reaction, the solution contains H+,ClO4,K+ and H2O (the OH ions get consumed).

Formula

The H+ ion concentration, remaining in a given solution, is calculated by the formula,

[H+]=mmolH+leftVolumeoforiginalsolution(mL)×Volumeofcompoundadded(mL)

Substitute the values of mmoles of H+ left, volume of original solution and volume of compound added in the above equation.

[H+]=mmolH+leftVolumeoforiginalsolution(mL)×Volumeofcompoundadded(mL)=4.0mmol(40.0+40.0)mL=0.05M_

To find the pH of the resulting solution, after the addition of 40.0mL of KOH

The concentration of H+ is 0.05M .

Formula

The pH is calculated using the formula,

pH=log10[H+]

Where,

  • [H+] is concentration of H+ ions.

Substitute the value of is concentration of [H+] in the above equation.

pH=log10[H+]=log10(0.05)=1.30_

(d)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The titration concentration of KOH , volume and concentration of HClO4 is given. The pH of resulting solution after the addition of KOH is to be calculated for the given volumes of KOH .

Concept introduction:

Titration is a process to determine the concentration of an unknown solution with the help of a solution of a known concentration value.

The pH is calculated using the formula,

pH=log10[H+]

The relation between pH and pOH is,

pH+pOH=14

Answer to Problem 63E

The pH of the resulting solution, after the addition of 80.0mL of KOH is 7_ .

Explanation of Solution

Explanation

To determine the pH of the resulting solution, after the addition of 80.0mL of KOH .

Given

Concentration of HClO4 is 0.200M .

Concentration of KOH is 0.100M .

Volume of HClO4 original solution is 40mL .

Volume of KOH added is 80.0mL .

Large quantities of the H+ ions and the OH ions are present. The 8.0mmol (80.0mL×0.100M) of the OH added will react with 1.0mmol H+ to form water:

H++OHH2OBeforereaction40.0mL×0.200M=8mmol80.0mL×0.100M=8.00mmolAfterreaction8.008.00=08.008.00=0

After the reaction, the solution contains ClO4,K+ and H2O (the OH ions and H+ get consumed). It means that solution is completely neutralized. Therefore, the pH value of the solution is 7_ .

(e)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The titration concentration of KOH , volume and concentration of HClO4 is given. The pH of resulting solution after the addition of KOH is to be calculated for the given volumes of KOH .

Concept introduction:

Titration is a process to determine the concentration of an unknown solution with the help of a solution of a known concentration value.

The pH is calculated using the formula,

pH=log10[H+]

The relation between pH and pOH is,

pH+pOH=14

Answer to Problem 63E

The pH of the resulting solution, after the addition of 100.0mL of KOH is 12.15_ .

Explanation of Solution

Explanation

To determine the concentration of OH

Given

Concentration of HClO4 is 0.200M .

Concentration of KOH is 0.100M .

Volume of HClO4 original solution is 40mL .

Volume of KOH added is 100.0mL .

Large quantities of the H+ ions and the OH ions are present. The 10.0mmol (100.0mL×0.100M) of the OH added will react with 1.0mmol H+ to form water:

H++OHH2OBeforereaction40.0mL×0.200M=8.0mmol100.0mL×0.100M=10.0mmolAfterreaction8.08.00=010.008.00=2

After the reaction, the solution contains OH,ClO4,K+ and H2O (the H+ ions get consumed).

Formula

The OH ion concentration, remaining in a given solution, is calculated by the formula,

[OH]=mmolOHleftVolumeoforiginalsolution(mL)×Volumeofcompoundadded(mL)

Substitute the values of the mmoles of OH left, volume of original solution and volume of compound added in the above equation.

[OH]=mmolOHleftVolumeoforiginalsolution(mL)×Volumeofcompoundadded(mL)=2.0mmol(40.0+100.0)mL=0.0142M_

To determine the concentration of pOH

Formula

The pOH is calculated using the formula,

pOH=log10[OH]

Where,

  • [OH] is concentration of OH ions.

Substitute the value of is concentration of [OH] in the above equation.

pOH=log10[OH]=log10(0.0142)=1.85_

To determine the pH of the resulting solution, after the addition of 100.0mL of KOH

Formula

The relation between pH and pOH is,

pH+pOH=14

Where,

  • pH is a measure of concentration of H+ .
  • pOH is a measure of concentration of OH .

Substitute the value of pOH in above equation.

pH+pOH=14pH+1.85=14pH=12.15_

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