Question 1

What is the pH of a solution that has [H3O+] = 6.0 × 10−3 M?

Accepted Answer

A) 1.7 × 10−12 
B) 2.22 
C) 3.60 
D) 5.12 
E) 11.78 
A) 1.7 × 10−12 
B) 2.22 
C) 3.60 
D) 5.12 
E) 11.78

Question 2

What is the pH of a 0.035 M HCl solution?

Accepted Answer

A) 3.50 
B) 1.46 
C) 2.27 
D) 5.59 
E) 12.54 
A) 3.50 
B) 1.46 
C) 2.27 
D) 5.59 
E) 12.54

Question 3

A particular buffer solution consists of a weak acid and its conjugate base.How could this buffer solution be modified so as to increase its buffer capacity against added base?

Accepted Answer

A) Increase the concentration of the weak acid. 
B) Increase the concentration of its conjugate base. 
C) Use a strong base and its conjugate acid instead. 
D) Use a strong acid and its conjugate base instead. 
E) Make the concentrations of the weak acid and its conjugate base equal. 
A) Increase the concentration of the weak acid. 
B) Increase the concentration of its conjugate base. 
C) Use a strong base and its conjugate acid instead. 
D) Use a strong acid and its conjugate base instead. 
E) Make the concentrations of the weak acid and its conjugate base equal.

Question 4

Morphine is used medicinally as a pain reliever.If an aqueous solution of morphine has [H3O+] = 1.1 × 10−10 M,what is the pH of this solution?

Accepted Answer

A) 1.00 
B) 3.69 
C) 8.96 
D) 9.96 
E) 11 
A) 1.00 
B) 3.69 
C) 8.96 
D) 9.96 
E) 11

Question 5

All Brønsted-Lowry bases contain hydroxide.

Accepted Answer

A) True 
 B)False

Question 6

A pH of 0 is considered neutral.

Accepted Answer

A) True 
 B)False

Question 7

During an oxidation-reduction reaction,the oxidizing agent loses electrons.

Accepted Answer

A) True 
 B)False

Question 8

Which of the following is an example of a diprotic acid?

Accepted Answer

A) NH2− 
B) H2SO4 
C) HCl 
D) CH4 
E) NH2− and H2SO4 are correct. 
A) NH2− 
B) H2SO4 
C) HCl 
D) CH4 
E) NH2− and H2SO4 are correct.

Question 9

A solution containing a buffer has an initial pH of 8.78.If a student adds 5 drops of HCl(aq)to this solution,what would be a reasonable pH for the resulting solution?

Accepted Answer

A) 5.22 
B) 7.00 
C) 8.64 
D) 8.78 
E) 8.89 
A) 5.22 
B) 7.00 
C) 8.64 
D) 8.78 
E) 8.89

Question 10

What is the conjugate acid of NH2−?

Accepted Answer

A) NH2− 
B) NH3 
C) NH4+ 
D) NH2+ 
E) NH4− 
A) NH2− 
B) NH3 
C) NH4+ 
D) NH2+ 
E) NH4−

Question 11

A buffer solution contains carbonic acid (H2CO3)and sodium bicarbonate (NaHCO3),each at a concentration of 0.100 M.The relevant equilibrium is shown below.What is the pH of this buffer solution? H2CO3(aq)+ H2O(l) ?  H3O+(aq)+ HCO3?(aq) Ka = 4.5 × 10?7

Accepted Answer

A) 4.50 
B) 7.00 
C) 6.35 
D) 7.65 
E) 2.16 
A) 4.50 
B) 7.00 
C) 6.35 
D) 7.65 
E) 2.16

Question 12

The ion-product of water is affected by a change in temperature.

Accepted Answer

A) True 
 B)False

Question 13

Which statement correctly describes conjugate acids and bases according to the Brønsted-Lowry theory?

Accepted Answer

A) A conjugate base is the species formed when an acid donates a proton; a conjugate acid is the species formed when a base accepts a proton. 
B) A conjugate base is the species formed when an acid accepts a proton; a conjugate acid is the species formed when a base donates a proton. 
C) A conjugate acid is the species formed when an acid donates a proton; a conjugate base is the species formed when a base accepts a proton. 
D) A conjugate acid is an acid that does not completely transfer a proton to water; a conjugate base is a base that does not completely accept a proton from water. 
E) A conjugate acid is the solution formed when an acid is added to water; a conjugate base is the solution formed when a base is added to water. 
A) A conjugate base is the species formed when an acid donates a proton; a conjugate acid is the species formed when a base accepts a proton. 
B) A conjugate base is the species formed when an acid accepts a proton; a conjugate acid is the species formed when a base donates a proton. 
C) A conjugate acid is the species formed when an acid donates a proton; a conjugate base is the species formed when a base accepts a proton. 
D) A conjugate acid is an acid that does not completely transfer a proton to water; a conjugate base is a base that does not completely accept a proton from water. 
E) A conjugate acid is the solution formed when an acid is added to water; a conjugate base is the solution formed when a base is added to water.

Question 14

Butyric acid is a weak acid.Which reaction equation properly represents the dissociation of butyric acid in water?

Accepted Answer

A) CH3CH2CH2COOH(aq)+ H2O(l)? CH3CH2CH2COO- (aq)+ H3O+(aq) 
B) CH3CH2CH2COOH(aq)+ H2O(l) ?  CH3CH2CH2COO-(aq)+ H3O+(aq) 
C) CH3CH2CH2COOH(aq)+ H2O(l)? CH3CH2CH2COOH2+(aq)+ OH-(aq) 
D) CH3CH2CH2COOH(aq)+ H2O(l) ?  CH2CH2CH2COOH(aq)+ H3O+(aq) 
E) CH3CH2CH2COOH(aq)+ H2O(l)? CH3CH2CH2COO- (aq)+ H3O+(aq)and CH3CH2CH2COOH(aq)+ H2O(l) ?  CH3CH2CH2COO-(aq)+ H3O+(aq)are correct. 
A) CH3CH2CH2COOH(aq)+ H2O(l)? CH3CH2CH2COO- (aq)+ H3O+(aq) 
B) CH3CH2CH2COOH(aq)+ H2O(l) ?  CH3CH2CH2COO-(aq)+ H3O+(aq) 
C) CH3CH2CH2COOH(aq)+ H2O(l)? CH3CH2CH2COOH2+(aq)+ OH-(aq) 
D) CH3CH2CH2COOH(aq)+ H2O(l) ?  CH2CH2CH2COOH(aq)+ H3O+(aq) 
E) CH3CH2CH2COOH(aq)+ H2O(l)? CH3CH2CH2COO- (aq)+ H3O+(aq)and CH3CH2CH2COOH(aq)+ H2O(l) ?  CH3CH2CH2COO-(aq)+ H3O+(aq)are correct.

Question 15

In electrolysis,electrical energy is used to drive a non-spontaneous oxidation-reduction reaction to occur.

Accepted Answer

A) True 
 B)False

Question 16

All metal hydroxides are strong bases.

Accepted Answer

A) True 
 B)False

Question 17

What is the pH of a 1.0 × 10−4 M solution of KOH?

Accepted Answer

A) 4.00 
B) 6.00 
C) 7.00 
D) 10.00 
E) 14.00 
A) 4.00 
B) 6.00 
C) 7.00 
D) 10.00 
E) 14.00

Question 18

For the reaction shown below,which of the following correctly represents a conjugate acid-base pair? HCO2H(aq)+ H2O(l) ?  H3O+(aq)+ HCO2?(aq)

Accepted Answer

A) HCO2H/H3O+ 
B) HCO2H/H2O 
C) H2O/HCO2- 
D) H3O+/HCO2- 
E) HCO2H/HCO2? 
A) HCO2H/H3O+ 
B) HCO2H/H2O 
C) H2O/HCO2- 
D) H3O+/HCO2- 
E) HCO2H/HCO2?

Question 19

Which of the following compounds is NOT considered a polyprotic acid?

Accepted Answer

A) H2SO4 
B) H3PO4 
C) H2CO3 
D) H2SO3 
E) CH3COOH 
A) H2SO4 
B) H3PO4 
C) H2CO3 
D) H2SO3 
E) CH3COOH

Question 20

The species that remains after an acid donates a proton is called its conjugate base.What is the conjugate base of the hydronium ion,H3O+?

Accepted Answer

A) OH- 
B) H2O- 
C) H2O 
D) H2O+ 
E) H3O+ has no conjugate base. 
A) OH- 
B) H2O- 
C) H2O 
D) H2O+ 
E) H3O+ has no conjugate base.

Exam 8: Acids and Bases

What is the pH of a solution that has [H3O+] = 6.0 × 10−3 M?

What is the pH of a 0.035 M HCl solution?

A particular buffer solution consists of a weak acid and its conjugate base.How could this buffer solution be modified so as to increase its buffer capacity against added base?

Morphine is used medicinally as a pain reliever.If an aqueous solution of morphine has [H3O+] = 1.1 × 10−10 M,what is the pH of this solution?

All Brønsted-Lowry bases contain hydroxide.

A pH of 0 is considered neutral.

During an oxidation-reduction reaction,the oxidizing agent loses electrons.

Which of the following is an example of a diprotic acid?

A solution containing a buffer has an initial pH of 8.78.If a student adds 5 drops of HCl(aq)to this solution,what would be a reasonable pH for the resulting solution?

What is the conjugate acid of NH2−?

A buffer solution contains carbonic acid (H2CO3)and sodium bicarbonate (NaHCO3),each at a concentration of 0.100 M.The relevant equilibrium is shown below.What is the pH of this buffer solution? H2CO3(aq)+ H2O(l) ? H3O+(aq)+ HCO3?(aq) Ka = 4.5 × 10?7

The ion-product of water is affected by a change in temperature.

Which statement correctly describes conjugate acids and bases according to the Brønsted-Lowry theory?

Butyric acid is a weak acid.Which reaction equation properly represents the dissociation of butyric acid in water?

In electrolysis,electrical energy is used to drive a non-spontaneous oxidation-reduction reaction to occur.

All metal hydroxides are strong bases.

What is the pH of a 1.0 × 10−4 M solution of KOH?

For the reaction shown below,which of the following correctly represents a conjugate acid-base pair? HCO2H(aq)+ H2O(l) ? H3O+(aq)+ HCO2?(aq)

Which of the following compounds is NOT considered a polyprotic acid?

The species that remains after an acid donates a proton is called its conjugate base.What is the conjugate base of the hydronium ion,H3O+?

Chemistry - Methods and Measurement

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States of Matter: Gases, liquids, and Solids

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An Introduction to Organic Chemistry

The Unsaturated Hydrocarbons: Alkenes, alkynes, and Aromatics

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Carboxylic Acids and Carboxylic Acid Derivatives

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Introduction to Molecular Genetics

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Filters

What is the pH of a solution that has [H₃O⁺] = 6.0 × 10⁻³ M?

Morphine is used medicinally as a pain reliever.If an aqueous solution of morphine has [H₃O⁺] = 1.1 × 10⁻¹⁰ M,what is the pH of this solution?

What is the conjugate acid of NH₂⁻_?

A buffer solution contains carbonic acid (H₂CO₃)and sodium bicarbonate (NaHCO₃),each at a concentration of 0.100 M.The relevant equilibrium is shown below.What is the pH of this buffer solution? H₂CO₃(aq)+ H₂O(l) ? H₃O⁺(aq)+ HCO₃^?(aq)K_a = 4.5 × 10^?7

What is the pH of a 1.0 × 10⁻⁴ M solution of KOH?

For the reaction shown below,which of the following correctly represents a conjugate acid-base pair? HCO₂H(aq)+ H₂O(l) ? H₃O⁺(aq)+ HCO₂^?(aq)

The species that remains after an acid donates a proton is called its conjugate base.What is the conjugate base of the hydronium ion,H₃O⁺?