The p H o f 1.89 × 10 − 5 M a n d 9.64 × 10 − 7 M H C l O ( a q ) has to be calculated.

Question

Want to see more full solutions like this?

Answer 1

Question

Chapter 6, Problem 6F.10E

(a)

Interpretation Introduction

Interpretation:

The pH of 1.89×10−5M and 9.64×10−7MHClO(aq) has to be calculated.

(a)

Expert Solution

Explanation of Solution

Calculation of pH of 1.89×10−5M HClO(aq):

HClO is a weak acid. Its pH can be calculated as shown below.

HClO(aq)+H2O(l)⇌H3O+(aq)+ClO−(aq)Ka=[H3O+][ClO−][HClO]=3.0×10−8

An equilibrium table can be set up as given below.

Composition(M)HClOH3O+ClO−Initial concentration1.89×10−500Change in concentration−x+x+xEquilibrium concentration1.89×10−5−xxx

Now, the above equilibrium expression can be solved for x.

Ka=[H3O+][ClO−][HClO]=3.0×10−83.0×10−8=(x)(x)(1.89×10−5−x)x2=(3.0×10−8)(1.89×10−5) [Assuming x≪1.89×10−5]x=(3.0×10−8)(1.89×10−5)=7.53×10−7[H3O+]=7.53×10-7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(7.53×10−7)=6.12

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.12.

Calculation of pH of 9.64×10−7M HClO(aq):

HClO is a weak acid. Its pH can be calculated as shown below.

HClO(aq)+H2O(l)⇌H3O+(aq)+ClO−(aq)Ka=[H3O+][ClO−][HClO]=3.0×10−8

An equilibrium table can be set up as given below.

Composition(M)HClOH3O+ClO−Initial concentration9.64×10−700Change in concentration−x+x+xEquilibrium concentration9.64×10−7−xxx

Now, the above equilibrium expression can be solved for x.

Ka=[H3O+][ClO−][HClO]=3.0×10−83.0×10−8=(x)(x)(9.64×10−7−x)x2=(3.0×10−8)(9.64×10−7) [Assuming x≪9.64×10−7]x=(3.0×10−8)(9.64×10−7)=1.7×10−7[H3O+]=1.7×10-7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(1.7×10−7)=6.77

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.77.

(b)

Interpretation Introduction

Interpretation:

The pH of 1.89×10−5M and 9.64×10−7MHClO(aq) has to be calculated by taking into account the autoprotolysis of water.

Concept Introduction:

The contribution of autoprotolysis of water to the calculation of pH of very dilute solutions of weak acid must be taken into consideration if the hydronium ion concentration is less than 10−6M.

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

(b)

Expert Solution

Explanation of Solution

Calculation of pH of 1.89×10−5M HClO(aq):

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

By substituting x for [H3O+] in the above equation, the equation can be solved for x.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0x3+(3.0×10−8)x2−[(1.0×10−14)+(3.0×10−8)×(1.89×10−5)]x−(1.0×10−14)×(3.0×10−8)=0x3+(3.0×10−8)x2−(5.77×10−13)x−(3.0×10−22)=0

Write x=X×10−7 and divide the resulting equation by 10−21.

X3+0.03X2−57.7X−0.03=0X=7.6, so x=7.6×10−7[H3O+]=7.6×10−7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(7.6×10−7)=6.12

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.12.

Calculation of pH of 9.64×10−7M HClO(aq):

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

By substituting x for [H3O+] in the above equation, the equation can be solved for x.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0x3+(3.0×10−8)x2−[(1.0×10−14)+(3.0×10−8)×(9.64×10−7)]x−(1.0×10−14)×(3.0×10−8)=0x3+(3.0×10−8)x2−(3.892×10−14)x−(3.0×10−22)=0 Write x=X×10−7 and divide the resulting equation by 10−21.

X3+0.03X2−3.892X−0.03=0X=1.96, so x=1.96×10−7[H3O+]=1.96×10−7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(1.96×10−7)=6.70

Therefore, the pH of 9.64×10−7M HClO(aq) is 6.70.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Students have asked these similar questions

Correctly name this compound using the IUPAC naming system by sorting the components into the correct order. Br IN Ν H

How is the radical intermediate for this structure formed? Can you please draw arrows from the first radical to the resonance form that would result in this product? I'm lost.

Part VI. (a) calculate the λ max of the compound using woodward - Fieser rules. (b) what types of electronic transitions are present in the compound? (c) what are the prominent peaks in the IR spectrum of the compound?

Answer 2

Question

Chapter 6, Problem 6F.10E

(a)

Interpretation Introduction

Interpretation:

The pH of 1.89×10−5M and 9.64×10−7MHClO(aq) has to be calculated.

(a)

Expert Solution

Explanation of Solution

Calculation of pH of 1.89×10−5M HClO(aq):

HClO is a weak acid. Its pH can be calculated as shown below.

HClO(aq)+H2O(l)⇌H3O+(aq)+ClO−(aq)Ka=[H3O+][ClO−][HClO]=3.0×10−8

An equilibrium table can be set up as given below.

Composition(M)HClOH3O+ClO−Initial concentration1.89×10−500Change in concentration−x+x+xEquilibrium concentration1.89×10−5−xxx

Now, the above equilibrium expression can be solved for x.

Ka=[H3O+][ClO−][HClO]=3.0×10−83.0×10−8=(x)(x)(1.89×10−5−x)x2=(3.0×10−8)(1.89×10−5) [Assuming x≪1.89×10−5]x=(3.0×10−8)(1.89×10−5)=7.53×10−7[H3O+]=7.53×10-7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(7.53×10−7)=6.12

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.12.

Calculation of pH of 9.64×10−7M HClO(aq):

HClO is a weak acid. Its pH can be calculated as shown below.

HClO(aq)+H2O(l)⇌H3O+(aq)+ClO−(aq)Ka=[H3O+][ClO−][HClO]=3.0×10−8

An equilibrium table can be set up as given below.

Composition(M)HClOH3O+ClO−Initial concentration9.64×10−700Change in concentration−x+x+xEquilibrium concentration9.64×10−7−xxx

Now, the above equilibrium expression can be solved for x.

Ka=[H3O+][ClO−][HClO]=3.0×10−83.0×10−8=(x)(x)(9.64×10−7−x)x2=(3.0×10−8)(9.64×10−7) [Assuming x≪9.64×10−7]x=(3.0×10−8)(9.64×10−7)=1.7×10−7[H3O+]=1.7×10-7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(1.7×10−7)=6.77

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.77.

(b)

Interpretation Introduction

Interpretation:

The pH of 1.89×10−5M and 9.64×10−7MHClO(aq) has to be calculated by taking into account the autoprotolysis of water.

Concept Introduction:

The contribution of autoprotolysis of water to the calculation of pH of very dilute solutions of weak acid must be taken into consideration if the hydronium ion concentration is less than 10−6M.

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

(b)

Expert Solution

Explanation of Solution

Calculation of pH of 1.89×10−5M HClO(aq):

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

By substituting x for [H3O+] in the above equation, the equation can be solved for x.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0x3+(3.0×10−8)x2−[(1.0×10−14)+(3.0×10−8)×(1.89×10−5)]x−(1.0×10−14)×(3.0×10−8)=0x3+(3.0×10−8)x2−(5.77×10−13)x−(3.0×10−22)=0

Write x=X×10−7 and divide the resulting equation by 10−21.

X3+0.03X2−57.7X−0.03=0X=7.6, so x=7.6×10−7[H3O+]=7.6×10−7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(7.6×10−7)=6.12

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.12.

Calculation of pH of 9.64×10−7M HClO(aq):

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

By substituting x for [H3O+] in the above equation, the equation can be solved for x.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0x3+(3.0×10−8)x2−[(1.0×10−14)+(3.0×10−8)×(9.64×10−7)]x−(1.0×10−14)×(3.0×10−8)=0x3+(3.0×10−8)x2−(3.892×10−14)x−(3.0×10−22)=0 Write x=X×10−7 and divide the resulting equation by 10−21.

X3+0.03X2−3.892X−0.03=0X=1.96, so x=1.96×10−7[H3O+]=1.96×10−7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(1.96×10−7)=6.70

Therefore, the pH of 9.64×10−7M HClO(aq) is 6.70.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 3

Question

Chapter 6, Problem 6F.10E

(a)

Interpretation Introduction

Interpretation:

The pH of 1.89×10−5M and 9.64×10−7MHClO(aq) has to be calculated.

(a)

Expert Solution

Explanation of Solution

Calculation of pH of 1.89×10−5M HClO(aq):

HClO is a weak acid. Its pH can be calculated as shown below.

HClO(aq)+H2O(l)⇌H3O+(aq)+ClO−(aq)Ka=[H3O+][ClO−][HClO]=3.0×10−8

An equilibrium table can be set up as given below.

Composition(M)HClOH3O+ClO−Initial concentration1.89×10−500Change in concentration−x+x+xEquilibrium concentration1.89×10−5−xxx

Now, the above equilibrium expression can be solved for x.

Ka=[H3O+][ClO−][HClO]=3.0×10−83.0×10−8=(x)(x)(1.89×10−5−x)x2=(3.0×10−8)(1.89×10−5) [Assuming x≪1.89×10−5]x=(3.0×10−8)(1.89×10−5)=7.53×10−7[H3O+]=7.53×10-7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(7.53×10−7)=6.12

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.12.

Calculation of pH of 9.64×10−7M HClO(aq):

HClO is a weak acid. Its pH can be calculated as shown below.

HClO(aq)+H2O(l)⇌H3O+(aq)+ClO−(aq)Ka=[H3O+][ClO−][HClO]=3.0×10−8

An equilibrium table can be set up as given below.

Composition(M)HClOH3O+ClO−Initial concentration9.64×10−700Change in concentration−x+x+xEquilibrium concentration9.64×10−7−xxx

Now, the above equilibrium expression can be solved for x.

Ka=[H3O+][ClO−][HClO]=3.0×10−83.0×10−8=(x)(x)(9.64×10−7−x)x2=(3.0×10−8)(9.64×10−7) [Assuming x≪9.64×10−7]x=(3.0×10−8)(9.64×10−7)=1.7×10−7[H3O+]=1.7×10-7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(1.7×10−7)=6.77

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.77.

(b)

Interpretation Introduction

Interpretation:

The pH of 1.89×10−5M and 9.64×10−7MHClO(aq) has to be calculated by taking into account the autoprotolysis of water.

Concept Introduction:

The contribution of autoprotolysis of water to the calculation of pH of very dilute solutions of weak acid must be taken into consideration if the hydronium ion concentration is less than 10−6M.

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

(b)

Expert Solution

Explanation of Solution

Calculation of pH of 1.89×10−5M HClO(aq):

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

By substituting x for [H3O+] in the above equation, the equation can be solved for x.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0x3+(3.0×10−8)x2−[(1.0×10−14)+(3.0×10−8)×(1.89×10−5)]x−(1.0×10−14)×(3.0×10−8)=0x3+(3.0×10−8)x2−(5.77×10−13)x−(3.0×10−22)=0

Write x=X×10−7 and divide the resulting equation by 10−21.

X3+0.03X2−57.7X−0.03=0X=7.6, so x=7.6×10−7[H3O+]=7.6×10−7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(7.6×10−7)=6.12

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.12.

Calculation of pH of 9.64×10−7M HClO(aq):

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

By substituting x for [H3O+] in the above equation, the equation can be solved for x.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0x3+(3.0×10−8)x2−[(1.0×10−14)+(3.0×10−8)×(9.64×10−7)]x−(1.0×10−14)×(3.0×10−8)=0x3+(3.0×10−8)x2−(3.892×10−14)x−(3.0×10−22)=0 Write x=X×10−7 and divide the resulting equation by 10−21.

X3+0.03X2−3.892X−0.03=0X=1.96, so x=1.96×10−7[H3O+]=1.96×10−7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(1.96×10−7)=6.70

Therefore, the pH of 9.64×10−7M HClO(aq) is 6.70.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 4

Question

Chapter 6, Problem 6F.10E

(a)

Interpretation Introduction

Interpretation:

The pH of 1.89×10−5M and 9.64×10−7MHClO(aq) has to be calculated.

(a)

Expert Solution

Explanation of Solution

Calculation of pH of 1.89×10−5M HClO(aq):

HClO is a weak acid. Its pH can be calculated as shown below.

HClO(aq)+H2O(l)⇌H3O+(aq)+ClO−(aq)Ka=[H3O+][ClO−][HClO]=3.0×10−8

An equilibrium table can be set up as given below.

Composition(M)HClOH3O+ClO−Initial concentration1.89×10−500Change in concentration−x+x+xEquilibrium concentration1.89×10−5−xxx

Now, the above equilibrium expression can be solved for x.

Ka=[H3O+][ClO−][HClO]=3.0×10−83.0×10−8=(x)(x)(1.89×10−5−x)x2=(3.0×10−8)(1.89×10−5) [Assuming x≪1.89×10−5]x=(3.0×10−8)(1.89×10−5)=7.53×10−7[H3O+]=7.53×10-7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(7.53×10−7)=6.12

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.12.

Calculation of pH of 9.64×10−7M HClO(aq):

HClO is a weak acid. Its pH can be calculated as shown below.

HClO(aq)+H2O(l)⇌H3O+(aq)+ClO−(aq)Ka=[H3O+][ClO−][HClO]=3.0×10−8

An equilibrium table can be set up as given below.

Composition(M)HClOH3O+ClO−Initial concentration9.64×10−700Change in concentration−x+x+xEquilibrium concentration9.64×10−7−xxx

Now, the above equilibrium expression can be solved for x.

Ka=[H3O+][ClO−][HClO]=3.0×10−83.0×10−8=(x)(x)(9.64×10−7−x)x2=(3.0×10−8)(9.64×10−7) [Assuming x≪9.64×10−7]x=(3.0×10−8)(9.64×10−7)=1.7×10−7[H3O+]=1.7×10-7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(1.7×10−7)=6.77

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.77.

(b)

Interpretation Introduction

Interpretation:

The pH of 1.89×10−5M and 9.64×10−7MHClO(aq) has to be calculated by taking into account the autoprotolysis of water.

Concept Introduction:

The contribution of autoprotolysis of water to the calculation of pH of very dilute solutions of weak acid must be taken into consideration if the hydronium ion concentration is less than 10−6M.

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

(b)

Expert Solution

Explanation of Solution

Calculation of pH of 1.89×10−5M HClO(aq):

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

By substituting x for [H3O+] in the above equation, the equation can be solved for x.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0x3+(3.0×10−8)x2−[(1.0×10−14)+(3.0×10−8)×(1.89×10−5)]x−(1.0×10−14)×(3.0×10−8)=0x3+(3.0×10−8)x2−(5.77×10−13)x−(3.0×10−22)=0

Write x=X×10−7 and divide the resulting equation by 10−21.

X3+0.03X2−57.7X−0.03=0X=7.6, so x=7.6×10−7[H3O+]=7.6×10−7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(7.6×10−7)=6.12

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.12.

Calculation of pH of 9.64×10−7M HClO(aq):

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

By substituting x for [H3O+] in the above equation, the equation can be solved for x.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0x3+(3.0×10−8)x2−[(1.0×10−14)+(3.0×10−8)×(9.64×10−7)]x−(1.0×10−14)×(3.0×10−8)=0x3+(3.0×10−8)x2−(3.892×10−14)x−(3.0×10−22)=0 Write x=X×10−7 and divide the resulting equation by 10−21.

X3+0.03X2−3.892X−0.03=0X=1.96, so x=1.96×10−7[H3O+]=1.96×10−7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(1.96×10−7)=6.70

Therefore, the pH of 9.64×10−7M HClO(aq) is 6.70.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 5

Chapter 6, Problem 6F.10E

(a)

Interpretation Introduction

Interpretation:

The pH of 1.89×10−5M and 9.64×10−7MHClO(aq) has to be calculated.

(a)

Expert Solution

Explanation of Solution

Calculation of pH of 1.89×10−5M HClO(aq):

HClO is a weak acid. Its pH can be calculated as shown below.

HClO(aq)+H2O(l)⇌H3O+(aq)+ClO−(aq)Ka=[H3O+][ClO−][HClO]=3.0×10−8

An equilibrium table can be set up as given below.

Composition(M)HClOH3O+ClO−Initial concentration1.89×10−500Change in concentration−x+x+xEquilibrium concentration1.89×10−5−xxx

Now, the above equilibrium expression can be solved for x.

Ka=[H3O+][ClO−][HClO]=3.0×10−83.0×10−8=(x)(x)(1.89×10−5−x)x2=(3.0×10−8)(1.89×10−5) [Assuming x≪1.89×10−5]x=(3.0×10−8)(1.89×10−5)=7.53×10−7[H3O+]=7.53×10-7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(7.53×10−7)=6.12

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.12.

Calculation of pH of 9.64×10−7M HClO(aq):

HClO is a weak acid. Its pH can be calculated as shown below.

HClO(aq)+H2O(l)⇌H3O+(aq)+ClO−(aq)Ka=[H3O+][ClO−][HClO]=3.0×10−8

An equilibrium table can be set up as given below.

Composition(M)HClOH3O+ClO−Initial concentration9.64×10−700Change in concentration−x+x+xEquilibrium concentration9.64×10−7−xxx

Now, the above equilibrium expression can be solved for x.

Ka=[H3O+][ClO−][HClO]=3.0×10−83.0×10−8=(x)(x)(9.64×10−7−x)x2=(3.0×10−8)(9.64×10−7) [Assuming x≪9.64×10−7]x=(3.0×10−8)(9.64×10−7)=1.7×10−7[H3O+]=1.7×10-7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(1.7×10−7)=6.77

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.77.

(b)

Interpretation Introduction

Interpretation:

The pH of 1.89×10−5M and 9.64×10−7MHClO(aq) has to be calculated by taking into account the autoprotolysis of water.

Concept Introduction:

The contribution of autoprotolysis of water to the calculation of pH of very dilute solutions of weak acid must be taken into consideration if the hydronium ion concentration is less than 10−6M.

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

(b)

Expert Solution

Explanation of Solution

Calculation of pH of 1.89×10−5M HClO(aq):

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

By substituting x for [H3O+] in the above equation, the equation can be solved for x.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0x3+(3.0×10−8)x2−[(1.0×10−14)+(3.0×10−8)×(1.89×10−5)]x−(1.0×10−14)×(3.0×10−8)=0x3+(3.0×10−8)x2−(5.77×10−13)x−(3.0×10−22)=0

Write x=X×10−7 and divide the resulting equation by 10−21.

X3+0.03X2−57.7X−0.03=0X=7.6, so x=7.6×10−7[H3O+]=7.6×10−7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(7.6×10−7)=6.12

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.12.

Calculation of pH of 9.64×10−7M HClO(aq):

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

By substituting x for [H3O+] in the above equation, the equation can be solved for x.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0x3+(3.0×10−8)x2−[(1.0×10−14)+(3.0×10−8)×(9.64×10−7)]x−(1.0×10−14)×(3.0×10−8)=0x3+(3.0×10−8)x2−(3.892×10−14)x−(3.0×10−22)=0 Write x=X×10−7 and divide the resulting equation by 10−21.

X3+0.03X2−3.892X−0.03=0X=1.96, so x=1.96×10−7[H3O+]=1.96×10−7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(1.96×10−7)=6.70

Therefore, the pH of 9.64×10−7M HClO(aq) is 6.70.

Answer 6

Chapter 6, Problem 6F.10E

(a)

Interpretation Introduction

Interpretation:

The pH of 1.89×10−5M and 9.64×10−7MHClO(aq) has to be calculated.

(a)

Expert Solution

Explanation of Solution

Calculation of pH of 1.89×10−5M HClO(aq):

HClO is a weak acid. Its pH can be calculated as shown below.

HClO(aq)+H2O(l)⇌H3O+(aq)+ClO−(aq)Ka=[H3O+][ClO−][HClO]=3.0×10−8

An equilibrium table can be set up as given below.

Composition(M)HClOH3O+ClO−Initial concentration1.89×10−500Change in concentration−x+x+xEquilibrium concentration1.89×10−5−xxx

Now, the above equilibrium expression can be solved for x.

Ka=[H3O+][ClO−][HClO]=3.0×10−83.0×10−8=(x)(x)(1.89×10−5−x)x2=(3.0×10−8)(1.89×10−5) [Assuming x≪1.89×10−5]x=(3.0×10−8)(1.89×10−5)=7.53×10−7[H3O+]=7.53×10-7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(7.53×10−7)=6.12

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.12.

Calculation of pH of 9.64×10−7M HClO(aq):

HClO is a weak acid. Its pH can be calculated as shown below.

HClO(aq)+H2O(l)⇌H3O+(aq)+ClO−(aq)Ka=[H3O+][ClO−][HClO]=3.0×10−8

An equilibrium table can be set up as given below.

Composition(M)HClOH3O+ClO−Initial concentration9.64×10−700Change in concentration−x+x+xEquilibrium concentration9.64×10−7−xxx

Now, the above equilibrium expression can be solved for x.

Ka=[H3O+][ClO−][HClO]=3.0×10−83.0×10−8=(x)(x)(9.64×10−7−x)x2=(3.0×10−8)(9.64×10−7) [Assuming x≪9.64×10−7]x=(3.0×10−8)(9.64×10−7)=1.7×10−7[H3O+]=1.7×10-7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(1.7×10−7)=6.77

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.77.

Answer 7

Chapter 6, Problem 6F.10E

(a)

Interpretation Introduction

Interpretation:

The pH of 1.89×10−5M and 9.64×10−7MHClO(aq) has to be calculated.

Answer 8

(a)

Expert Solution

Explanation of Solution

Calculation of pH of 1.89×10−5M HClO(aq):

HClO is a weak acid. Its pH can be calculated as shown below.

HClO(aq)+H2O(l)⇌H3O+(aq)+ClO−(aq)Ka=[H3O+][ClO−][HClO]=3.0×10−8

An equilibrium table can be set up as given below.

Composition(M)HClOH3O+ClO−Initial concentration1.89×10−500Change in concentration−x+x+xEquilibrium concentration1.89×10−5−xxx

Now, the above equilibrium expression can be solved for x.

Ka=[H3O+][ClO−][HClO]=3.0×10−83.0×10−8=(x)(x)(1.89×10−5−x)x2=(3.0×10−8)(1.89×10−5) [Assuming x≪1.89×10−5]x=(3.0×10−8)(1.89×10−5)=7.53×10−7[H3O+]=7.53×10-7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(7.53×10−7)=6.12

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.12.

Calculation of pH of 9.64×10−7M HClO(aq):

HClO is a weak acid. Its pH can be calculated as shown below.

HClO(aq)+H2O(l)⇌H3O+(aq)+ClO−(aq)Ka=[H3O+][ClO−][HClO]=3.0×10−8

An equilibrium table can be set up as given below.

Composition(M)HClOH3O+ClO−Initial concentration9.64×10−700Change in concentration−x+x+xEquilibrium concentration9.64×10−7−xxx

Now, the above equilibrium expression can be solved for x.

Ka=[H3O+][ClO−][HClO]=3.0×10−83.0×10−8=(x)(x)(9.64×10−7−x)x2=(3.0×10−8)(9.64×10−7) [Assuming x≪9.64×10−7]x=(3.0×10−8)(9.64×10−7)=1.7×10−7[H3O+]=1.7×10-7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(1.7×10−7)=6.77

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.77.

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

(b)

Interpretation Introduction

Interpretation:

The pH of 1.89×10−5M and 9.64×10−7MHClO(aq) has to be calculated by taking into account the autoprotolysis of water.

Concept Introduction:

The contribution of autoprotolysis of water to the calculation of pH of very dilute solutions of weak acid must be taken into consideration if the hydronium ion concentration is less than 10−6M.

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

(b)

Expert Solution

Explanation of Solution

Calculation of pH of 1.89×10−5M HClO(aq):

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

By substituting x for [H3O+] in the above equation, the equation can be solved for x.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0x3+(3.0×10−8)x2−[(1.0×10−14)+(3.0×10−8)×(1.89×10−5)]x−(1.0×10−14)×(3.0×10−8)=0x3+(3.0×10−8)x2−(5.77×10−13)x−(3.0×10−22)=0

Write x=X×10−7 and divide the resulting equation by 10−21.

X3+0.03X2−57.7X−0.03=0X=7.6, so x=7.6×10−7[H3O+]=7.6×10−7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(7.6×10−7)=6.12

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.12.

Calculation of pH of 9.64×10−7M HClO(aq):

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

By substituting x for [H3O+] in the above equation, the equation can be solved for x.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0x3+(3.0×10−8)x2−[(1.0×10−14)+(3.0×10−8)×(9.64×10−7)]x−(1.0×10−14)×(3.0×10−8)=0x3+(3.0×10−8)x2−(3.892×10−14)x−(3.0×10−22)=0 Write x=X×10−7 and divide the resulting equation by 10−21.

X3+0.03X2−3.892X−0.03=0X=1.96, so x=1.96×10−7[H3O+]=1.96×10−7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(1.96×10−7)=6.70

Therefore, the pH of 9.64×10−7M HClO(aq) is 6.70.

Answer 13

(b)

Interpretation Introduction

Interpretation:

The pH of 1.89×10−5M and 9.64×10−7MHClO(aq) has to be calculated by taking into account the autoprotolysis of water.

Concept Introduction:

The contribution of autoprotolysis of water to the calculation of pH of very dilute solutions of weak acid must be taken into consideration if the hydronium ion concentration is less than 10−6M.

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

Answer 14

(b)

Expert Solution

Explanation of Solution

Calculation of pH of 1.89×10−5M HClO(aq):

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

By substituting x for [H3O+] in the above equation, the equation can be solved for x.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0x3+(3.0×10−8)x2−[(1.0×10−14)+(3.0×10−8)×(1.89×10−5)]x−(1.0×10−14)×(3.0×10−8)=0x3+(3.0×10−8)x2−(5.77×10−13)x−(3.0×10−22)=0

Write x=X×10−7 and divide the resulting equation by 10−21.

X3+0.03X2−57.7X−0.03=0X=7.6, so x=7.6×10−7[H3O+]=7.6×10−7M

Now, the pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log(7.6×10−7)=6.12

Therefore, the pH of 1.89×10−5M HClO(aq) is 6.12.

Calculation of pH of 9.64×10−7M HClO(aq):

For very dilute solutions of weak acid, the given below equation should be used.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0

By substituting x for [H3O+] in the above equation, the equation can be solved for x.

[H3O+]3+Ka[H3O+]2−(KW+Ka[HA]Initial)[H3O+]−KaKW=0x3+(3.0×10−8)x2−[(1.0×10−14)+(3.0×10−8)×(9.64×10−7)]x−(1.0×10−14)×(3.0×10−8)=0x3+(3.0×10−8)x2−(3.892×10−14)x−(3.0×10−22)=0 Write x=X×10−7 and divide the resulting equation by 10−21.