The initial pH of the solution containing barium hydroxide is to be determined. Concept introduction: A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

Question

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Answer 1

Question

Chapter 8, Problem 64E

(a)

Interpretation Introduction

Interpretation:

The initial pH of the solution containing barium hydroxide is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

(a)

Expert Solution

Answer to Problem 64E

The pH of the initial barium hydroxide solution is 13.30 .

Explanation of Solution

Initial pH of the analyte solution; Ba(OH)2 is a strong base. Therefore, the reaction of this base with water is Ba(OH)2+H2O→Ba+2+2OH−+H2O . Then the initial pOH of the solution can be calculated using the concentration of the base directly. There, the stoichiometry of the above reaction should be considered (one mole of barium hydroxide gives two moles of hydroxide ion).

CBa (OH)2=0.100MCOH−=0.100M×2=2.0×10−1MpOH=−log[OH−]=−log[2.0×10−1]=(1−0.30)=0.70

Using the relationship between pH and pOH, we can determine the initial pH of the analyte solution.

14=pH+pOH14=pH+0.70pH=13.30

(b)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 20.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

(b)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 12.91 .

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×20.0×10−3L=8×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, only 4×10−3mol of the base is reacted with the added acid. Then 4×10−3mol of base remains in the solution. One mole of barium hydroxide produces two moles of hydroxide ions.

moles of Ba(OH)2=4×10−3molmoles of OH−=4×10−3mol×2=8×10−3molConcentation of OH−=8× 10 −3mol(80.0+20.0)× 10 −3L=0.08mol/L

Using this value, the pH of the solution can be determined.

pOH=−log[OH−]=−log[0.08]=1.0914=pH+pOHpH=14−1.09=12.91

(c)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 30.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

(c)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 12.56 .

Explanation of Solution

When 30.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×30.0×10−3L=12×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, only 12×10−3mol2=6×10−3mol of the base is reacted with the added acid. Then (8−6)×10−3mol=2×10−3mol of base remains in the solution. One mole of barium hydroxide produces two moles of hydroxide ions.

moles of Ba(OH)2=2×10−3molmoles of OH−=2×10−3mol×2=4×10−3molConcentation of OH−=4× 10 −3mol(80.0+30.0)× 10 −3L=0.036mol/L

Using this value, the pH of the solution can be determined.

pOH=−log[OH−]=−log[0.036]=1.4414=pH+pOHpH=14−1.44=12.56

(d)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 40.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species are reacted with each other, they form their ionic forms and a neutral solution.

(d)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 7.00 .

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×40.0×10−3L=16×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, 16×10−3mol2=8×10−3mol of the base is reacted with the added acid. Then there is no base remains in the solution. At this pH, the solution becomes neutral and the pH is 7.00 .

(e)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 80.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species are reacted with each other, they form their ionic forms and a neutral solution.

(e)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 1.30 .

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×80.0×10−3L=32×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, 32×10−3mol2=16×10−3mol of the base is reacted with the added acid. Then there is no base remains in the solution and there is excess of acid in the solution.

The amount of acid in the solution =16×10−3mol−8×10−3mol=8×10−3mol

Concentration of the acid =8×10−3mol(80.0+80.0)×10−3L=0.05mol/L

One mole of acid produces one mole of hydrogen ion. Therefore,

pH=−log[H+]=−log[0.05]=1.30

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Answer 2

Question

Chapter 8, Problem 64E

(a)

Interpretation Introduction

Interpretation:

The initial pH of the solution containing barium hydroxide is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

(a)

Expert Solution

Answer to Problem 64E

The pH of the initial barium hydroxide solution is 13.30 .

Explanation of Solution

Initial pH of the analyte solution; Ba(OH)2 is a strong base. Therefore, the reaction of this base with water is Ba(OH)2+H2O→Ba+2+2OH−+H2O . Then the initial pOH of the solution can be calculated using the concentration of the base directly. There, the stoichiometry of the above reaction should be considered (one mole of barium hydroxide gives two moles of hydroxide ion).

CBa (OH)2=0.100MCOH−=0.100M×2=2.0×10−1MpOH=−log[OH−]=−log[2.0×10−1]=(1−0.30)=0.70

Using the relationship between pH and pOH, we can determine the initial pH of the analyte solution.

14=pH+pOH14=pH+0.70pH=13.30

(b)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 20.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

(b)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 12.91 .

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×20.0×10−3L=8×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, only 4×10−3mol of the base is reacted with the added acid. Then 4×10−3mol of base remains in the solution. One mole of barium hydroxide produces two moles of hydroxide ions.

moles of Ba(OH)2=4×10−3molmoles of OH−=4×10−3mol×2=8×10−3molConcentation of OH−=8× 10 −3mol(80.0+20.0)× 10 −3L=0.08mol/L

Using this value, the pH of the solution can be determined.

pOH=−log[OH−]=−log[0.08]=1.0914=pH+pOHpH=14−1.09=12.91

(c)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 30.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

(c)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 12.56 .

Explanation of Solution

When 30.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×30.0×10−3L=12×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, only 12×10−3mol2=6×10−3mol of the base is reacted with the added acid. Then (8−6)×10−3mol=2×10−3mol of base remains in the solution. One mole of barium hydroxide produces two moles of hydroxide ions.

moles of Ba(OH)2=2×10−3molmoles of OH−=2×10−3mol×2=4×10−3molConcentation of OH−=4× 10 −3mol(80.0+30.0)× 10 −3L=0.036mol/L

Using this value, the pH of the solution can be determined.

pOH=−log[OH−]=−log[0.036]=1.4414=pH+pOHpH=14−1.44=12.56

(d)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 40.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species are reacted with each other, they form their ionic forms and a neutral solution.

(d)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 7.00 .

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×40.0×10−3L=16×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, 16×10−3mol2=8×10−3mol of the base is reacted with the added acid. Then there is no base remains in the solution. At this pH, the solution becomes neutral and the pH is 7.00 .

(e)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 80.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species are reacted with each other, they form their ionic forms and a neutral solution.

(e)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 1.30 .

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×80.0×10−3L=32×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, 32×10−3mol2=16×10−3mol of the base is reacted with the added acid. Then there is no base remains in the solution and there is excess of acid in the solution.

The amount of acid in the solution =16×10−3mol−8×10−3mol=8×10−3mol

Concentration of the acid =8×10−3mol(80.0+80.0)×10−3L=0.05mol/L

One mole of acid produces one mole of hydrogen ion. Therefore,

pH=−log[H+]=−log[0.05]=1.30

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Answer 3

Question

Chapter 8, Problem 64E

(a)

Interpretation Introduction

Interpretation:

The initial pH of the solution containing barium hydroxide is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

(a)

Expert Solution

Answer to Problem 64E

The pH of the initial barium hydroxide solution is 13.30 .

Explanation of Solution

Initial pH of the analyte solution; Ba(OH)2 is a strong base. Therefore, the reaction of this base with water is Ba(OH)2+H2O→Ba+2+2OH−+H2O . Then the initial pOH of the solution can be calculated using the concentration of the base directly. There, the stoichiometry of the above reaction should be considered (one mole of barium hydroxide gives two moles of hydroxide ion).

CBa (OH)2=0.100MCOH−=0.100M×2=2.0×10−1MpOH=−log[OH−]=−log[2.0×10−1]=(1−0.30)=0.70

Using the relationship between pH and pOH, we can determine the initial pH of the analyte solution.

14=pH+pOH14=pH+0.70pH=13.30

(b)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 20.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

(b)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 12.91 .

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×20.0×10−3L=8×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, only 4×10−3mol of the base is reacted with the added acid. Then 4×10−3mol of base remains in the solution. One mole of barium hydroxide produces two moles of hydroxide ions.

moles of Ba(OH)2=4×10−3molmoles of OH−=4×10−3mol×2=8×10−3molConcentation of OH−=8× 10 −3mol(80.0+20.0)× 10 −3L=0.08mol/L

Using this value, the pH of the solution can be determined.

pOH=−log[OH−]=−log[0.08]=1.0914=pH+pOHpH=14−1.09=12.91

(c)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 30.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

(c)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 12.56 .

Explanation of Solution

When 30.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×30.0×10−3L=12×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, only 12×10−3mol2=6×10−3mol of the base is reacted with the added acid. Then (8−6)×10−3mol=2×10−3mol of base remains in the solution. One mole of barium hydroxide produces two moles of hydroxide ions.

moles of Ba(OH)2=2×10−3molmoles of OH−=2×10−3mol×2=4×10−3molConcentation of OH−=4× 10 −3mol(80.0+30.0)× 10 −3L=0.036mol/L

Using this value, the pH of the solution can be determined.

pOH=−log[OH−]=−log[0.036]=1.4414=pH+pOHpH=14−1.44=12.56

(d)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 40.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species are reacted with each other, they form their ionic forms and a neutral solution.

(d)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 7.00 .

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×40.0×10−3L=16×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, 16×10−3mol2=8×10−3mol of the base is reacted with the added acid. Then there is no base remains in the solution. At this pH, the solution becomes neutral and the pH is 7.00 .

(e)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 80.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species are reacted with each other, they form their ionic forms and a neutral solution.

(e)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 1.30 .

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×80.0×10−3L=32×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, 32×10−3mol2=16×10−3mol of the base is reacted with the added acid. Then there is no base remains in the solution and there is excess of acid in the solution.

The amount of acid in the solution =16×10−3mol−8×10−3mol=8×10−3mol

Concentration of the acid =8×10−3mol(80.0+80.0)×10−3L=0.05mol/L

One mole of acid produces one mole of hydrogen ion. Therefore,

pH=−log[H+]=−log[0.05]=1.30

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Answer 4

Question

Chapter 8, Problem 64E

(a)

Interpretation Introduction

Interpretation:

The initial pH of the solution containing barium hydroxide is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

(a)

Expert Solution

Answer to Problem 64E

The pH of the initial barium hydroxide solution is 13.30 .

Explanation of Solution

Initial pH of the analyte solution; Ba(OH)2 is a strong base. Therefore, the reaction of this base with water is Ba(OH)2+H2O→Ba+2+2OH−+H2O . Then the initial pOH of the solution can be calculated using the concentration of the base directly. There, the stoichiometry of the above reaction should be considered (one mole of barium hydroxide gives two moles of hydroxide ion).

CBa (OH)2=0.100MCOH−=0.100M×2=2.0×10−1MpOH=−log[OH−]=−log[2.0×10−1]=(1−0.30)=0.70

Using the relationship between pH and pOH, we can determine the initial pH of the analyte solution.

14=pH+pOH14=pH+0.70pH=13.30

(b)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 20.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

(b)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 12.91 .

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×20.0×10−3L=8×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, only 4×10−3mol of the base is reacted with the added acid. Then 4×10−3mol of base remains in the solution. One mole of barium hydroxide produces two moles of hydroxide ions.

moles of Ba(OH)2=4×10−3molmoles of OH−=4×10−3mol×2=8×10−3molConcentation of OH−=8× 10 −3mol(80.0+20.0)× 10 −3L=0.08mol/L

Using this value, the pH of the solution can be determined.

pOH=−log[OH−]=−log[0.08]=1.0914=pH+pOHpH=14−1.09=12.91

(c)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 30.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

(c)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 12.56 .

Explanation of Solution

When 30.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×30.0×10−3L=12×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, only 12×10−3mol2=6×10−3mol of the base is reacted with the added acid. Then (8−6)×10−3mol=2×10−3mol of base remains in the solution. One mole of barium hydroxide produces two moles of hydroxide ions.

moles of Ba(OH)2=2×10−3molmoles of OH−=2×10−3mol×2=4×10−3molConcentation of OH−=4× 10 −3mol(80.0+30.0)× 10 −3L=0.036mol/L

Using this value, the pH of the solution can be determined.

pOH=−log[OH−]=−log[0.036]=1.4414=pH+pOHpH=14−1.44=12.56

(d)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 40.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species are reacted with each other, they form their ionic forms and a neutral solution.

(d)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 7.00 .

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×40.0×10−3L=16×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, 16×10−3mol2=8×10−3mol of the base is reacted with the added acid. Then there is no base remains in the solution. At this pH, the solution becomes neutral and the pH is 7.00 .

(e)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 80.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species are reacted with each other, they form their ionic forms and a neutral solution.

(e)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 1.30 .

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×80.0×10−3L=32×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, 32×10−3mol2=16×10−3mol of the base is reacted with the added acid. Then there is no base remains in the solution and there is excess of acid in the solution.

The amount of acid in the solution =16×10−3mol−8×10−3mol=8×10−3mol

Concentration of the acid =8×10−3mol(80.0+80.0)×10−3L=0.05mol/L

One mole of acid produces one mole of hydrogen ion. Therefore,

pH=−log[H+]=−log[0.05]=1.30

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Answer 5

Chapter 8, Problem 64E

(a)

Interpretation Introduction

Interpretation:

The initial pH of the solution containing barium hydroxide is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

(a)

Expert Solution

Answer to Problem 64E

The pH of the initial barium hydroxide solution is 13.30 .

Explanation of Solution

Initial pH of the analyte solution; Ba(OH)2 is a strong base. Therefore, the reaction of this base with water is Ba(OH)2+H2O→Ba+2+2OH−+H2O . Then the initial pOH of the solution can be calculated using the concentration of the base directly. There, the stoichiometry of the above reaction should be considered (one mole of barium hydroxide gives two moles of hydroxide ion).

CBa (OH)2=0.100MCOH−=0.100M×2=2.0×10−1MpOH=−log[OH−]=−log[2.0×10−1]=(1−0.30)=0.70

Using the relationship between pH and pOH, we can determine the initial pH of the analyte solution.

14=pH+pOH14=pH+0.70pH=13.30

(b)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 20.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

(b)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 12.91 .

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×20.0×10−3L=8×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, only 4×10−3mol of the base is reacted with the added acid. Then 4×10−3mol of base remains in the solution. One mole of barium hydroxide produces two moles of hydroxide ions.

moles of Ba(OH)2=4×10−3molmoles of OH−=4×10−3mol×2=8×10−3molConcentation of OH−=8× 10 −3mol(80.0+20.0)× 10 −3L=0.08mol/L

Using this value, the pH of the solution can be determined.

pOH=−log[OH−]=−log[0.08]=1.0914=pH+pOHpH=14−1.09=12.91

(c)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 30.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

(c)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 12.56 .

Explanation of Solution

When 30.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×30.0×10−3L=12×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, only 12×10−3mol2=6×10−3mol of the base is reacted with the added acid. Then (8−6)×10−3mol=2×10−3mol of base remains in the solution. One mole of barium hydroxide produces two moles of hydroxide ions.

moles of Ba(OH)2=2×10−3molmoles of OH−=2×10−3mol×2=4×10−3molConcentation of OH−=4× 10 −3mol(80.0+30.0)× 10 −3L=0.036mol/L

Using this value, the pH of the solution can be determined.

pOH=−log[OH−]=−log[0.036]=1.4414=pH+pOHpH=14−1.44=12.56

(d)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 40.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species are reacted with each other, they form their ionic forms and a neutral solution.

(d)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 7.00 .

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×40.0×10−3L=16×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, 16×10−3mol2=8×10−3mol of the base is reacted with the added acid. Then there is no base remains in the solution. At this pH, the solution becomes neutral and the pH is 7.00 .

(e)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 80.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species are reacted with each other, they form their ionic forms and a neutral solution.

(e)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 1.30 .

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×80.0×10−3L=32×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, 32×10−3mol2=16×10−3mol of the base is reacted with the added acid. Then there is no base remains in the solution and there is excess of acid in the solution.

The amount of acid in the solution =16×10−3mol−8×10−3mol=8×10−3mol

Concentration of the acid =8×10−3mol(80.0+80.0)×10−3L=0.05mol/L

One mole of acid produces one mole of hydrogen ion. Therefore,

pH=−log[H+]=−log[0.05]=1.30

Answer 6

Chapter 8, Problem 64E

(a)

Interpretation Introduction

Interpretation:

The initial pH of the solution containing barium hydroxide is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

(a)

Expert Solution

Answer to Problem 64E

The pH of the initial barium hydroxide solution is 13.30 .

Explanation of Solution

Initial pH of the analyte solution; Ba(OH)2 is a strong base. Therefore, the reaction of this base with water is Ba(OH)2+H2O→Ba+2+2OH−+H2O . Then the initial pOH of the solution can be calculated using the concentration of the base directly. There, the stoichiometry of the above reaction should be considered (one mole of barium hydroxide gives two moles of hydroxide ion).

CBa (OH)2=0.100MCOH−=0.100M×2=2.0×10−1MpOH=−log[OH−]=−log[2.0×10−1]=(1−0.30)=0.70

Using the relationship between pH and pOH, we can determine the initial pH of the analyte solution.

14=pH+pOH14=pH+0.70pH=13.30

Answer 7

Chapter 8, Problem 64E

(a)

Interpretation Introduction

Interpretation:

The initial pH of the solution containing barium hydroxide is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

Answer 8

(a)

Expert Solution

Answer to Problem 64E

The pH of the initial barium hydroxide solution is 13.30 .

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

Initial pH of the analyte solution; Ba(OH)2 is a strong base. Therefore, the reaction of this base with water is Ba(OH)2+H2O→Ba+2+2OH−+H2O . Then the initial pOH of the solution can be calculated using the concentration of the base directly. There, the stoichiometry of the above reaction should be considered (one mole of barium hydroxide gives two moles of hydroxide ion).

CBa (OH)2=0.100MCOH−=0.100M×2=2.0×10−1MpOH=−log[OH−]=−log[2.0×10−1]=(1−0.30)=0.70

Using the relationship between pH and pOH, we can determine the initial pH of the analyte solution.

14=pH+pOH14=pH+0.70pH=13.30

Answer 13

(b)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 20.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

(b)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 12.91 .

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×20.0×10−3L=8×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, only 4×10−3mol of the base is reacted with the added acid. Then 4×10−3mol of base remains in the solution. One mole of barium hydroxide produces two moles of hydroxide ions.

moles of Ba(OH)2=4×10−3molmoles of OH−=4×10−3mol×2=8×10−3molConcentation of OH−=8× 10 −3mol(80.0+20.0)× 10 −3L=0.08mol/L

Using this value, the pH of the solution can be determined.

pOH=−log[OH−]=−log[0.08]=1.0914=pH+pOHpH=14−1.09=12.91

Answer 14

(b)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 20.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

Answer 15

(b)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 12.91 .

Answer 16

(b)

Expert Solution

Answer 17

(b)

Expert Solution

Answer 18

Expert Solution

Answer 19

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×20.0×10−3L=8×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, only 4×10−3mol of the base is reacted with the added acid. Then 4×10−3mol of base remains in the solution. One mole of barium hydroxide produces two moles of hydroxide ions.

moles of Ba(OH)2=4×10−3molmoles of OH−=4×10−3mol×2=8×10−3molConcentation of OH−=8× 10 −3mol(80.0+20.0)× 10 −3L=0.08mol/L

Using this value, the pH of the solution can be determined.

pOH=−log[OH−]=−log[0.08]=1.0914=pH+pOHpH=14−1.09=12.91

Answer 20

(c)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 30.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

(c)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 12.56 .

Explanation of Solution

When 30.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×30.0×10−3L=12×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, only 12×10−3mol2=6×10−3mol of the base is reacted with the added acid. Then (8−6)×10−3mol=2×10−3mol of base remains in the solution. One mole of barium hydroxide produces two moles of hydroxide ions.

moles of Ba(OH)2=2×10−3molmoles of OH−=2×10−3mol×2=4×10−3molConcentation of OH−=4× 10 −3mol(80.0+30.0)× 10 −3L=0.036mol/L

Using this value, the pH of the solution can be determined.

pOH=−log[OH−]=−log[0.036]=1.4414=pH+pOHpH=14−1.44=12.56

Answer 21

(c)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 30.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species react with each other, they form their ionic forms and a neutral solution.

Answer 22

(c)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 12.56 .

Answer 23

(c)

Expert Solution

Answer 24

(c)

Expert Solution

Answer 25

Expert Solution

Answer 26

Explanation of Solution

When 30.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×30.0×10−3L=12×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, only 12×10−3mol2=6×10−3mol of the base is reacted with the added acid. Then (8−6)×10−3mol=2×10−3mol of base remains in the solution. One mole of barium hydroxide produces two moles of hydroxide ions.

moles of Ba(OH)2=2×10−3molmoles of OH−=2×10−3mol×2=4×10−3molConcentation of OH−=4× 10 −3mol(80.0+30.0)× 10 −3L=0.036mol/L

Using this value, the pH of the solution can be determined.

pOH=−log[OH−]=−log[0.036]=1.4414=pH+pOHpH=14−1.44=12.56

Answer 27

(d)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 40.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species are reacted with each other, they form their ionic forms and a neutral solution.

(d)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 7.00 .

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×40.0×10−3L=16×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, 16×10−3mol2=8×10−3mol of the base is reacted with the added acid. Then there is no base remains in the solution. At this pH, the solution becomes neutral and the pH is 7.00 .

Answer 28

(d)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 40.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species are reacted with each other, they form their ionic forms and a neutral solution.

Answer 29

(d)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 7.00 .

Answer 30

(d)

Expert Solution

Answer 31

(d)

Expert Solution

Answer 32

Expert Solution

Answer 33

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×40.0×10−3L=16×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, 16×10−3mol2=8×10−3mol of the base is reacted with the added acid. Then there is no base remains in the solution. At this pH, the solution becomes neutral and the pH is 7.00 .

Answer 34

(e)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 80.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species are reacted with each other, they form their ionic forms and a neutral solution.

(e)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 1.30 .

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×80.0×10−3L=32×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, 32×10−3mol2=16×10−3mol of the base is reacted with the added acid. Then there is no base remains in the solution and there is excess of acid in the solution.

The amount of acid in the solution =16×10−3mol−8×10−3mol=8×10−3mol

Concentration of the acid =8×10−3mol(80.0+80.0)×10−3L=0.05mol/L

One mole of acid produces one mole of hydrogen ion. Therefore,

pH=−log[H+]=−log[0.05]=1.30

Answer 35

(e)

Interpretation Introduction

Interpretation:

The pH of the barium hydroxide solution when 80.0mL of acid is added to it is to be determined.

Concept introduction:

A strong acid or a strong base can completely dissociate into its ions when they are in an aqueous solution. Barium hydroxide is a strong base while hydrochloric acid is a strong acid. When these two chemical species are reacted with each other, they form their ionic forms and a neutral solution.

Answer 36

(e)

Expert Solution

Answer to Problem 64E

The pH of the resulting solution is 1.30 .

Answer 37

(e)

Expert Solution

Answer 38

(e)

Expert Solution

Answer 39

Expert Solution

Answer 40

Explanation of Solution

When 20.0mL of the acid is added to the base, some amount of the base reacts with the acid. Therefore, we can determine the pH of the resulting solution by calculating the remaining amount of base in the solution.

Total amount of base =0.100mol/L×80.0×10−3L=8×10−3mol

Amount of the acid added to the base =0.400mol/L×80.0×10−3L=32×10−3mol

The reaction between barium hydroxide and hydrochloric acid is as follows:

Ba(OH)2+2HCl→BaCl2+2H2O

This means two moles of the acid react with one mole of the base. Therefore, 32×10−3mol2=16×10−3mol of the base is reacted with the added acid. Then there is no base remains in the solution and there is excess of acid in the solution.