The titration of acetic acid (CH 3 COOH) with sodium hydroxide (NaOH), both 0.100 M. The titration curve has to be drawn and four regions of importance have to be labeled.

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Answer 1

Question

Chapter 16, Problem 16.8QE

Interpretation Introduction

Interpretation:

The titration of acetic acid (CH₃COOH) with sodium hydroxide (NaOH), both 0.100 M. The titration curve has to be drawn and four regions of importance have to be labeled.

Expert Solution & Answer

Explanation of Solution

Addition of 0 mL of 0.1 M NaOH to25.00 mL of 0.100 M acetic acid:

Acetic acid is a weak acid. The initial point in the titration when the base is not added to the system, the system is a weak acid system.

The iCe table can be set up to calculate the pH of the solution.

HA+H2O⇌H3O++A−i(M)0.10000C(M)−y+y+ye(M)0.100−yyy

Where, HA represents acetic acid and A− represents the conjugate base of acetic acid.

The Ka value for acetic acid is 1.8×10−5. The expression for Ka can be written as given below,

Ka=[H3O+][A−][HA]=1.8×10−5y2(0.100−y)=1.8×10−5

This can be solved by approximation. If y≪0.100, then

y2≈1.8×10−5×0.100=1.8×10−6y=1.8×10−6=1.34×10−3=[H3O+]

The pH of the solution can be calculated as given below.

pH=-log[H3O+]=-log(1.34×10-3)=2.87.

Addition of 10 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

The neutralization reaction can be written as given,

HA(aq)+OH−(aq)→A−(aq)+H2O(l)

Calculation of milimole of acid and base:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=10.00 mL×(0.100 milimol OH−mL)=1 milimol

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1. So the limiting reactant is OH− ion.

HA+OH−→A−+H2Os(mmol)2.510ExcessR(mmol)−1−1+1+1f(mmol)1.501Excess

All the strong base is consumed. There are weak acid (HA) and its conjugate base (A−) in the solution. So this solution is an acidic buffer. By using Henderson-Hasselbalch equation, it’s pH can be calculated.

pH=pKa+lognbna=pKa+log1.51=pKa+0.176=pKa=−log(Ka)=−log(1.8×10−5)+0.176=4.92.

Addition of 25.00 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

Calculation of milimole of acid and base:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=25.00 mL×(0.100 milimol OH−mL)=2.5 milimolTotal volume=25.00+25.00=50.00 mL

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1.

HA+OH−→A−+H2Os(mmol)2.52.50ExcessR(mmol)−2.5−2.5+2.5+2.5f(mmol)002.5Excessc(M)000.05

Both H3O+ and OH− ions have been completely consumed, the titration is at the equivalence point. There is only the conjugate base and water in the solution.

The iCe table can be set up to calculate the pH of the solution.

A−+H2O⇌HA+OH−i(M)0.0500C(M)−y+y+ye(M)0.05−yyy

The expression for Kb can be written as given below,

Kb=[HA][OH−][A−]=y2(0.05−y)

The value of Kb can be calculated as given below.

Kb=KwKa=1.0×10−141.8×10−5=0.56×10−9

This can be solved by approximation. If y≪0.05, then

y2≈0.56×10−9×0.05=2.8×10−11y=2.8×10−11=5.29×10−6=[OH−]

The pH of the solution can be calculated as given below.

pOH=−log[OH−]=−log(5.29×10−6)=5.28pH+pOH=14pH=14−pOH=14−5.28=8.72.

Addition of 30 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

Calculation of milimole of acid and base and total volume:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=30.00 mL×(0.100 milimol OH−mL)=3 milimolTotal volume=25.00+30.00=55.00 mL

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1. So the limiting reactant is H3O+ ion.

HA+OH−→A−+H2Os(mmol)2.530ExcessR(mmol)−2.5−2.5+2.5+2.5f(mmol)00.52.5Excessc(M)09.09×10−30.045

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

pOH=−log[OH−]=−log(9.09×10−3)=2.04pH+pOH=14pH=14−pOH=14−2.04=11.95.

Titration curve:

The titration curve is plotted between volume of base added and the corresponding pH values.

Volume of NaOH(mL)pH02.8710.004.9225.008.7230.0011.95

The titration curve with four important regions is given below.

Chemistry: Principles and Practice, Chapter 16, Problem 16.8QE

Figure 1

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Answer 2

Question

Chapter 16, Problem 16.8QE

Interpretation Introduction

Interpretation:

The titration of acetic acid (CH₃COOH) with sodium hydroxide (NaOH), both 0.100 M. The titration curve has to be drawn and four regions of importance have to be labeled.

Expert Solution & Answer

Explanation of Solution

Addition of 0 mL of 0.1 M NaOH to25.00 mL of 0.100 M acetic acid:

Acetic acid is a weak acid. The initial point in the titration when the base is not added to the system, the system is a weak acid system.

The iCe table can be set up to calculate the pH of the solution.

HA+H2O⇌H3O++A−i(M)0.10000C(M)−y+y+ye(M)0.100−yyy

Where, HA represents acetic acid and A− represents the conjugate base of acetic acid.

The Ka value for acetic acid is 1.8×10−5. The expression for Ka can be written as given below,

Ka=[H3O+][A−][HA]=1.8×10−5y2(0.100−y)=1.8×10−5

This can be solved by approximation. If y≪0.100, then

y2≈1.8×10−5×0.100=1.8×10−6y=1.8×10−6=1.34×10−3=[H3O+]

The pH of the solution can be calculated as given below.

pH=-log[H3O+]=-log(1.34×10-3)=2.87.

Addition of 10 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

The neutralization reaction can be written as given,

HA(aq)+OH−(aq)→A−(aq)+H2O(l)

Calculation of milimole of acid and base:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=10.00 mL×(0.100 milimol OH−mL)=1 milimol

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1. So the limiting reactant is OH− ion.

HA+OH−→A−+H2Os(mmol)2.510ExcessR(mmol)−1−1+1+1f(mmol)1.501Excess

All the strong base is consumed. There are weak acid (HA) and its conjugate base (A−) in the solution. So this solution is an acidic buffer. By using Henderson-Hasselbalch equation, it’s pH can be calculated.

pH=pKa+lognbna=pKa+log1.51=pKa+0.176=pKa=−log(Ka)=−log(1.8×10−5)+0.176=4.92.

Addition of 25.00 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

Calculation of milimole of acid and base:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=25.00 mL×(0.100 milimol OH−mL)=2.5 milimolTotal volume=25.00+25.00=50.00 mL

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1.

HA+OH−→A−+H2Os(mmol)2.52.50ExcessR(mmol)−2.5−2.5+2.5+2.5f(mmol)002.5Excessc(M)000.05

Both H3O+ and OH− ions have been completely consumed, the titration is at the equivalence point. There is only the conjugate base and water in the solution.

The iCe table can be set up to calculate the pH of the solution.

A−+H2O⇌HA+OH−i(M)0.0500C(M)−y+y+ye(M)0.05−yyy

The expression for Kb can be written as given below,

Kb=[HA][OH−][A−]=y2(0.05−y)

The value of Kb can be calculated as given below.

Kb=KwKa=1.0×10−141.8×10−5=0.56×10−9

This can be solved by approximation. If y≪0.05, then

y2≈0.56×10−9×0.05=2.8×10−11y=2.8×10−11=5.29×10−6=[OH−]

The pH of the solution can be calculated as given below.

pOH=−log[OH−]=−log(5.29×10−6)=5.28pH+pOH=14pH=14−pOH=14−5.28=8.72.

Addition of 30 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

Calculation of milimole of acid and base and total volume:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=30.00 mL×(0.100 milimol OH−mL)=3 milimolTotal volume=25.00+30.00=55.00 mL

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1. So the limiting reactant is H3O+ ion.

HA+OH−→A−+H2Os(mmol)2.530ExcessR(mmol)−2.5−2.5+2.5+2.5f(mmol)00.52.5Excessc(M)09.09×10−30.045

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

pOH=−log[OH−]=−log(9.09×10−3)=2.04pH+pOH=14pH=14−pOH=14−2.04=11.95.

Titration curve:

The titration curve is plotted between volume of base added and the corresponding pH values.

Volume of NaOH(mL)pH02.8710.004.9225.008.7230.0011.95

The titration curve with four important regions is given below.

Chemistry: Principles and Practice, Chapter 16, Problem 16.8QE

Figure 1

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Answer 3

Question

Chapter 16, Problem 16.8QE

Interpretation Introduction

Interpretation:

The titration of acetic acid (CH₃COOH) with sodium hydroxide (NaOH), both 0.100 M. The titration curve has to be drawn and four regions of importance have to be labeled.

Expert Solution & Answer

Explanation of Solution

Addition of 0 mL of 0.1 M NaOH to25.00 mL of 0.100 M acetic acid:

Acetic acid is a weak acid. The initial point in the titration when the base is not added to the system, the system is a weak acid system.

The iCe table can be set up to calculate the pH of the solution.

HA+H2O⇌H3O++A−i(M)0.10000C(M)−y+y+ye(M)0.100−yyy

Where, HA represents acetic acid and A− represents the conjugate base of acetic acid.

The Ka value for acetic acid is 1.8×10−5. The expression for Ka can be written as given below,

Ka=[H3O+][A−][HA]=1.8×10−5y2(0.100−y)=1.8×10−5

This can be solved by approximation. If y≪0.100, then

y2≈1.8×10−5×0.100=1.8×10−6y=1.8×10−6=1.34×10−3=[H3O+]

The pH of the solution can be calculated as given below.

pH=-log[H3O+]=-log(1.34×10-3)=2.87.

Addition of 10 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

The neutralization reaction can be written as given,

HA(aq)+OH−(aq)→A−(aq)+H2O(l)

Calculation of milimole of acid and base:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=10.00 mL×(0.100 milimol OH−mL)=1 milimol

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1. So the limiting reactant is OH− ion.

HA+OH−→A−+H2Os(mmol)2.510ExcessR(mmol)−1−1+1+1f(mmol)1.501Excess

All the strong base is consumed. There are weak acid (HA) and its conjugate base (A−) in the solution. So this solution is an acidic buffer. By using Henderson-Hasselbalch equation, it’s pH can be calculated.

pH=pKa+lognbna=pKa+log1.51=pKa+0.176=pKa=−log(Ka)=−log(1.8×10−5)+0.176=4.92.

Addition of 25.00 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

Calculation of milimole of acid and base:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=25.00 mL×(0.100 milimol OH−mL)=2.5 milimolTotal volume=25.00+25.00=50.00 mL

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1.

HA+OH−→A−+H2Os(mmol)2.52.50ExcessR(mmol)−2.5−2.5+2.5+2.5f(mmol)002.5Excessc(M)000.05

Both H3O+ and OH− ions have been completely consumed, the titration is at the equivalence point. There is only the conjugate base and water in the solution.

The iCe table can be set up to calculate the pH of the solution.

A−+H2O⇌HA+OH−i(M)0.0500C(M)−y+y+ye(M)0.05−yyy

The expression for Kb can be written as given below,

Kb=[HA][OH−][A−]=y2(0.05−y)

The value of Kb can be calculated as given below.

Kb=KwKa=1.0×10−141.8×10−5=0.56×10−9

This can be solved by approximation. If y≪0.05, then

y2≈0.56×10−9×0.05=2.8×10−11y=2.8×10−11=5.29×10−6=[OH−]

The pH of the solution can be calculated as given below.

pOH=−log[OH−]=−log(5.29×10−6)=5.28pH+pOH=14pH=14−pOH=14−5.28=8.72.

Addition of 30 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

Calculation of milimole of acid and base and total volume:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=30.00 mL×(0.100 milimol OH−mL)=3 milimolTotal volume=25.00+30.00=55.00 mL

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1. So the limiting reactant is H3O+ ion.

HA+OH−→A−+H2Os(mmol)2.530ExcessR(mmol)−2.5−2.5+2.5+2.5f(mmol)00.52.5Excessc(M)09.09×10−30.045

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

pOH=−log[OH−]=−log(9.09×10−3)=2.04pH+pOH=14pH=14−pOH=14−2.04=11.95.

Titration curve:

The titration curve is plotted between volume of base added and the corresponding pH values.

Volume of NaOH(mL)pH02.8710.004.9225.008.7230.0011.95

The titration curve with four important regions is given below.

Chemistry: Principles and Practice, Chapter 16, Problem 16.8QE

Figure 1

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Answer 4

Question

Chapter 16, Problem 16.8QE

Interpretation Introduction

Interpretation:

The titration of acetic acid (CH₃COOH) with sodium hydroxide (NaOH), both 0.100 M. The titration curve has to be drawn and four regions of importance have to be labeled.

Expert Solution & Answer

Explanation of Solution

Addition of 0 mL of 0.1 M NaOH to25.00 mL of 0.100 M acetic acid:

Acetic acid is a weak acid. The initial point in the titration when the base is not added to the system, the system is a weak acid system.

The iCe table can be set up to calculate the pH of the solution.

HA+H2O⇌H3O++A−i(M)0.10000C(M)−y+y+ye(M)0.100−yyy

Where, HA represents acetic acid and A− represents the conjugate base of acetic acid.

The Ka value for acetic acid is 1.8×10−5. The expression for Ka can be written as given below,

Ka=[H3O+][A−][HA]=1.8×10−5y2(0.100−y)=1.8×10−5

This can be solved by approximation. If y≪0.100, then

y2≈1.8×10−5×0.100=1.8×10−6y=1.8×10−6=1.34×10−3=[H3O+]

The pH of the solution can be calculated as given below.

pH=-log[H3O+]=-log(1.34×10-3)=2.87.

Addition of 10 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

The neutralization reaction can be written as given,

HA(aq)+OH−(aq)→A−(aq)+H2O(l)

Calculation of milimole of acid and base:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=10.00 mL×(0.100 milimol OH−mL)=1 milimol

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1. So the limiting reactant is OH− ion.

HA+OH−→A−+H2Os(mmol)2.510ExcessR(mmol)−1−1+1+1f(mmol)1.501Excess

All the strong base is consumed. There are weak acid (HA) and its conjugate base (A−) in the solution. So this solution is an acidic buffer. By using Henderson-Hasselbalch equation, it’s pH can be calculated.

pH=pKa+lognbna=pKa+log1.51=pKa+0.176=pKa=−log(Ka)=−log(1.8×10−5)+0.176=4.92.

Addition of 25.00 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

Calculation of milimole of acid and base:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=25.00 mL×(0.100 milimol OH−mL)=2.5 milimolTotal volume=25.00+25.00=50.00 mL

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1.

HA+OH−→A−+H2Os(mmol)2.52.50ExcessR(mmol)−2.5−2.5+2.5+2.5f(mmol)002.5Excessc(M)000.05

Both H3O+ and OH− ions have been completely consumed, the titration is at the equivalence point. There is only the conjugate base and water in the solution.

The iCe table can be set up to calculate the pH of the solution.

A−+H2O⇌HA+OH−i(M)0.0500C(M)−y+y+ye(M)0.05−yyy

The expression for Kb can be written as given below,

Kb=[HA][OH−][A−]=y2(0.05−y)

The value of Kb can be calculated as given below.

Kb=KwKa=1.0×10−141.8×10−5=0.56×10−9

This can be solved by approximation. If y≪0.05, then

y2≈0.56×10−9×0.05=2.8×10−11y=2.8×10−11=5.29×10−6=[OH−]

The pH of the solution can be calculated as given below.

pOH=−log[OH−]=−log(5.29×10−6)=5.28pH+pOH=14pH=14−pOH=14−5.28=8.72.

Addition of 30 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

Calculation of milimole of acid and base and total volume:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=30.00 mL×(0.100 milimol OH−mL)=3 milimolTotal volume=25.00+30.00=55.00 mL

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1. So the limiting reactant is H3O+ ion.

HA+OH−→A−+H2Os(mmol)2.530ExcessR(mmol)−2.5−2.5+2.5+2.5f(mmol)00.52.5Excessc(M)09.09×10−30.045

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

pOH=−log[OH−]=−log(9.09×10−3)=2.04pH+pOH=14pH=14−pOH=14−2.04=11.95.

Titration curve:

The titration curve is plotted between volume of base added and the corresponding pH values.

Volume of NaOH(mL)pH02.8710.004.9225.008.7230.0011.95

The titration curve with four important regions is given below.

Chemistry: Principles and Practice, Chapter 16, Problem 16.8QE

Figure 1

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Answer 5

Chapter 16, Problem 16.8QE

Interpretation Introduction

Interpretation:

The titration of acetic acid (CH₃COOH) with sodium hydroxide (NaOH), both 0.100 M. The titration curve has to be drawn and four regions of importance have to be labeled.

Expert Solution & Answer

Explanation of Solution

Addition of 0 mL of 0.1 M NaOH to25.00 mL of 0.100 M acetic acid:

Acetic acid is a weak acid. The initial point in the titration when the base is not added to the system, the system is a weak acid system.

The iCe table can be set up to calculate the pH of the solution.

HA+H2O⇌H3O++A−i(M)0.10000C(M)−y+y+ye(M)0.100−yyy

Where, HA represents acetic acid and A− represents the conjugate base of acetic acid.

The Ka value for acetic acid is 1.8×10−5. The expression for Ka can be written as given below,

Ka=[H3O+][A−][HA]=1.8×10−5y2(0.100−y)=1.8×10−5

This can be solved by approximation. If y≪0.100, then

y2≈1.8×10−5×0.100=1.8×10−6y=1.8×10−6=1.34×10−3=[H3O+]

The pH of the solution can be calculated as given below.

pH=-log[H3O+]=-log(1.34×10-3)=2.87.

Addition of 10 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

The neutralization reaction can be written as given,

HA(aq)+OH−(aq)→A−(aq)+H2O(l)

Calculation of milimole of acid and base:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=10.00 mL×(0.100 milimol OH−mL)=1 milimol

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1. So the limiting reactant is OH− ion.

HA+OH−→A−+H2Os(mmol)2.510ExcessR(mmol)−1−1+1+1f(mmol)1.501Excess

All the strong base is consumed. There are weak acid (HA) and its conjugate base (A−) in the solution. So this solution is an acidic buffer. By using Henderson-Hasselbalch equation, it’s pH can be calculated.

pH=pKa+lognbna=pKa+log1.51=pKa+0.176=pKa=−log(Ka)=−log(1.8×10−5)+0.176=4.92.

Addition of 25.00 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

Calculation of milimole of acid and base:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=25.00 mL×(0.100 milimol OH−mL)=2.5 milimolTotal volume=25.00+25.00=50.00 mL

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1.

HA+OH−→A−+H2Os(mmol)2.52.50ExcessR(mmol)−2.5−2.5+2.5+2.5f(mmol)002.5Excessc(M)000.05

Both H3O+ and OH− ions have been completely consumed, the titration is at the equivalence point. There is only the conjugate base and water in the solution.

The iCe table can be set up to calculate the pH of the solution.

A−+H2O⇌HA+OH−i(M)0.0500C(M)−y+y+ye(M)0.05−yyy

The expression for Kb can be written as given below,

Kb=[HA][OH−][A−]=y2(0.05−y)

The value of Kb can be calculated as given below.

Kb=KwKa=1.0×10−141.8×10−5=0.56×10−9

This can be solved by approximation. If y≪0.05, then

y2≈0.56×10−9×0.05=2.8×10−11y=2.8×10−11=5.29×10−6=[OH−]

The pH of the solution can be calculated as given below.

pOH=−log[OH−]=−log(5.29×10−6)=5.28pH+pOH=14pH=14−pOH=14−5.28=8.72.

Addition of 30 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

Calculation of milimole of acid and base and total volume:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=30.00 mL×(0.100 milimol OH−mL)=3 milimolTotal volume=25.00+30.00=55.00 mL

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1. So the limiting reactant is H3O+ ion.

HA+OH−→A−+H2Os(mmol)2.530ExcessR(mmol)−2.5−2.5+2.5+2.5f(mmol)00.52.5Excessc(M)09.09×10−30.045

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

pOH=−log[OH−]=−log(9.09×10−3)=2.04pH+pOH=14pH=14−pOH=14−2.04=11.95.

Titration curve:

The titration curve is plotted between volume of base added and the corresponding pH values.

Volume of NaOH(mL)pH02.8710.004.9225.008.7230.0011.95

The titration curve with four important regions is given below.

Chemistry: Principles and Practice, Chapter 16, Problem 16.8QE

Figure 1

Answer 6

Chapter 16, Problem 16.8QE

Interpretation Introduction

Interpretation:

The titration of acetic acid (CH₃COOH) with sodium hydroxide (NaOH), both 0.100 M. The titration curve has to be drawn and four regions of importance have to be labeled.

Expert Solution & Answer

Explanation of Solution

Addition of 0 mL of 0.1 M NaOH to25.00 mL of 0.100 M acetic acid:

Acetic acid is a weak acid. The initial point in the titration when the base is not added to the system, the system is a weak acid system.

The iCe table can be set up to calculate the pH of the solution.

HA+H2O⇌H3O++A−i(M)0.10000C(M)−y+y+ye(M)0.100−yyy

Where, HA represents acetic acid and A− represents the conjugate base of acetic acid.

The Ka value for acetic acid is 1.8×10−5. The expression for Ka can be written as given below,

Ka=[H3O+][A−][HA]=1.8×10−5y2(0.100−y)=1.8×10−5

This can be solved by approximation. If y≪0.100, then

y2≈1.8×10−5×0.100=1.8×10−6y=1.8×10−6=1.34×10−3=[H3O+]

The pH of the solution can be calculated as given below.

pH=-log[H3O+]=-log(1.34×10-3)=2.87.

Addition of 10 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

The neutralization reaction can be written as given,

HA(aq)+OH−(aq)→A−(aq)+H2O(l)

Calculation of milimole of acid and base:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=10.00 mL×(0.100 milimol OH−mL)=1 milimol

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1. So the limiting reactant is OH− ion.

HA+OH−→A−+H2Os(mmol)2.510ExcessR(mmol)−1−1+1+1f(mmol)1.501Excess

All the strong base is consumed. There are weak acid (HA) and its conjugate base (A−) in the solution. So this solution is an acidic buffer. By using Henderson-Hasselbalch equation, it’s pH can be calculated.

pH=pKa+lognbna=pKa+log1.51=pKa+0.176=pKa=−log(Ka)=−log(1.8×10−5)+0.176=4.92.

Addition of 25.00 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

Calculation of milimole of acid and base:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=25.00 mL×(0.100 milimol OH−mL)=2.5 milimolTotal volume=25.00+25.00=50.00 mL

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1.

HA+OH−→A−+H2Os(mmol)2.52.50ExcessR(mmol)−2.5−2.5+2.5+2.5f(mmol)002.5Excessc(M)000.05

Both H3O+ and OH− ions have been completely consumed, the titration is at the equivalence point. There is only the conjugate base and water in the solution.

The iCe table can be set up to calculate the pH of the solution.

A−+H2O⇌HA+OH−i(M)0.0500C(M)−y+y+ye(M)0.05−yyy

The expression for Kb can be written as given below,

Kb=[HA][OH−][A−]=y2(0.05−y)

The value of Kb can be calculated as given below.

Kb=KwKa=1.0×10−141.8×10−5=0.56×10−9

This can be solved by approximation. If y≪0.05, then

y2≈0.56×10−9×0.05=2.8×10−11y=2.8×10−11=5.29×10−6=[OH−]

The pH of the solution can be calculated as given below.

pOH=−log[OH−]=−log(5.29×10−6)=5.28pH+pOH=14pH=14−pOH=14−5.28=8.72.

Addition of 30 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

Calculation of milimole of acid and base and total volume:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=30.00 mL×(0.100 milimol OH−mL)=3 milimolTotal volume=25.00+30.00=55.00 mL

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1. So the limiting reactant is H3O+ ion.

HA+OH−→A−+H2Os(mmol)2.530ExcessR(mmol)−2.5−2.5+2.5+2.5f(mmol)00.52.5Excessc(M)09.09×10−30.045

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

pOH=−log[OH−]=−log(9.09×10−3)=2.04pH+pOH=14pH=14−pOH=14−2.04=11.95.

Titration curve:

The titration curve is plotted between volume of base added and the corresponding pH values.

Volume of NaOH(mL)pH02.8710.004.9225.008.7230.0011.95

The titration curve with four important regions is given below.

Chemistry: Principles and Practice, Chapter 16, Problem 16.8QE

Figure 1

Answer 7

Chapter 16, Problem 16.8QE

Interpretation Introduction

Interpretation:

The titration of acetic acid (CH₃COOH) with sodium hydroxide (NaOH), both 0.100 M. The titration curve has to be drawn and four regions of importance have to be labeled.

Answer 8

Expert Solution & Answer

Explanation of Solution

Addition of 0 mL of 0.1 M NaOH to25.00 mL of 0.100 M acetic acid:

Acetic acid is a weak acid. The initial point in the titration when the base is not added to the system, the system is a weak acid system.

The iCe table can be set up to calculate the pH of the solution.

HA+H2O⇌H3O++A−i(M)0.10000C(M)−y+y+ye(M)0.100−yyy

Where, HA represents acetic acid and A− represents the conjugate base of acetic acid.

The Ka value for acetic acid is 1.8×10−5. The expression for Ka can be written as given below,

Ka=[H3O+][A−][HA]=1.8×10−5y2(0.100−y)=1.8×10−5

This can be solved by approximation. If y≪0.100, then

y2≈1.8×10−5×0.100=1.8×10−6y=1.8×10−6=1.34×10−3=[H3O+]

The pH of the solution can be calculated as given below.

pH=-log[H3O+]=-log(1.34×10-3)=2.87.

Addition of 10 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

The neutralization reaction can be written as given,

HA(aq)+OH−(aq)→A−(aq)+H2O(l)

Calculation of milimole of acid and base:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=10.00 mL×(0.100 milimol OH−mL)=1 milimol

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1. So the limiting reactant is OH− ion.

HA+OH−→A−+H2Os(mmol)2.510ExcessR(mmol)−1−1+1+1f(mmol)1.501Excess

All the strong base is consumed. There are weak acid (HA) and its conjugate base (A−) in the solution. So this solution is an acidic buffer. By using Henderson-Hasselbalch equation, it’s pH can be calculated.

pH=pKa+lognbna=pKa+log1.51=pKa+0.176=pKa=−log(Ka)=−log(1.8×10−5)+0.176=4.92.

Addition of 25.00 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

Calculation of milimole of acid and base:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=25.00 mL×(0.100 milimol OH−mL)=2.5 milimolTotal volume=25.00+25.00=50.00 mL

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1.

HA+OH−→A−+H2Os(mmol)2.52.50ExcessR(mmol)−2.5−2.5+2.5+2.5f(mmol)002.5Excessc(M)000.05

Both H3O+ and OH− ions have been completely consumed, the titration is at the equivalence point. There is only the conjugate base and water in the solution.

The iCe table can be set up to calculate the pH of the solution.

A−+H2O⇌HA+OH−i(M)0.0500C(M)−y+y+ye(M)0.05−yyy

The expression for Kb can be written as given below,

Kb=[HA][OH−][A−]=y2(0.05−y)

The value of Kb can be calculated as given below.

Kb=KwKa=1.0×10−141.8×10−5=0.56×10−9

This can be solved by approximation. If y≪0.05, then

y2≈0.56×10−9×0.05=2.8×10−11y=2.8×10−11=5.29×10−6=[OH−]

The pH of the solution can be calculated as given below.

pOH=−log[OH−]=−log(5.29×10−6)=5.28pH+pOH=14pH=14−pOH=14−5.28=8.72.

Addition of 30 mL of 0.100 M NaOH to 25.00 mL of 0.100 M acetic acid:

Calculation of milimole of acid and base and total volume:

Amount of HA=25.00 mL×(0.100 milimol H3O+mL)=2.5 milimolAmount of OH−=30.00 mL×(0.100 milimol OH−mL)=3 milimolTotal volume=25.00+30.00=55.00 mL

Making of sRfc table:

The table can be formed as shown below.

The molar ratio of acid and base is 1:1. So the limiting reactant is H3O+ ion.

HA+OH−→A−+H2Os(mmol)2.530ExcessR(mmol)−2.5−2.5+2.5+2.5f(mmol)00.52.5Excessc(M)09.09×10−30.045

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

pOH=−log[OH−]=−log(9.09×10−3)=2.04pH+pOH=14pH=14−pOH=14−2.04=11.95.

Titration curve:

The titration curve is plotted between volume of base added and the corresponding pH values.

Volume of NaOH(mL)pH02.8710.004.9225.008.7230.0011.95

The titration curve with four important regions is given below.

Chemistry: Principles and Practice, Chapter 16, Problem 16.8QE

Figure 1

Answer 9

Expert Solution & Answer

Answer 10

Expert Solution & Answer

Answer 11

Ch. 16 - Prob. 16.1QE Ch. 16 - Sketch a titration curve for the titration of...Ch. 16 - Prob. 16.4QE Ch. 16 - Prob. 16.5QE Ch. 16 - Explain why the HendersonHasselbalch equation...Ch. 16 - Prob. 16.7QE Ch. 16 - Prob. 16.8QE Ch. 16 - Prob. 16.9QE Ch. 16 - Prob. 16.11QE Ch. 16 - Prob. 16.13QE

The titration of acetic acid (CH 3 COOH) with sodium hydroxide (NaOH), both 0.100 M. The titration curve has to be drawn and four regions of importance have to be labeled.

Concept explainers

Videos

Interpretation:

The titration of acetic acid (CH₃COOH) with sodium hydroxide (NaOH), both 0.100 M. The titration curve has to be drawn and four regions of importance have to be labeled.

Explanation of Solution

Want to see more full solutions like this?

Chapter 16 Solutions

The titration of acetic acid (CH 3 COOH) with sodium hydroxide (NaOH), both 0.100 M. The titration curve has to be drawn and four regions of importance have to be labeled.

Concept explainers

Videos

Interpretation: The titration of acetic acid (CH3COOH) with sodium hydroxide (NaOH), both 0.100 M. The titration curve has to be drawn and four regions of importance have to be labeled.

Explanation of Solution

Want to see more full solutions like this?

Chapter 16 Solutions

Interpretation:

The titration of acetic acid (CH₃COOH) with sodium hydroxide (NaOH), both 0.100 M. The titration curve has to be drawn and four regions of importance have to be labeled.