Question 1

Normal gastric juice has a pH of about 2. Assuming that normal gastric juice is primarily aqueous HCl, what is the concentration of HCl in the stomach?

Accepted Answer

A) 2 M HCl 
B) 1.0 × 102 M HCl 
C) 0.01 M HCl 
D) 0.14 M HCl 
A) 2 M HCl 
B) 1.0 × 102 M HCl 
C) 0.01 M HCl 
D) 0.14 M HCl

Question 2

All compounds can be classified as either an acid or a base.

Accepted Answer

A) True 
 B)False

Question 3

Which diagram properly depicts the dissolved species present in an aqueous solution of KOH? (water molecules are not shown)

Accepted Answer

A)    
B)    
C)    
D)    
A)    
B)    
C)    
D)

Question 4

HPO42- is amphoteric. The conjugate acid of HPO42- is _____ and its conjugate base is _____.

Accepted Answer

Question 5

Which term correctly describes the medical condition in which the pH of blood is greater than 7.45, and therefore the blood is more basic than normal?

Accepted Answer

A) respiratory alkalosis 
B) alkalosis 
C) respiratory acidosis 
D) acidosis 
A) respiratory alkalosis 
B) alkalosis 
C) respiratory acidosis 
D) acidosis

Question 6

For a solution labeled 0.15 M CH3COOH, the [H3O+] is 0.15 M.

Accepted Answer

A) True 
 B)False

Question 7

Which salt forms a basic solution when dissolved in water?

Accepted Answer

A) KCl 
B) NH4Br 
C) LiNO3 
D) Na3PO4 
A) KCl 
B) NH4Br 
C) LiNO3 
D) Na3PO4

Question 8

Which buffer solution has the lowest pH (HF has Ka = 7.2 × 10-4)?

Accepted Answer

A) 0.10 M HF and 0.10 M NaF 
B) 0.20 M HF and 0.20 M NaF 
C) 0.20 M HF and 0.10 M NaF 
D) 0.10 M HF and 0.20 M NaF 
E) All of the buffer solutions described above have the same pH. 
A) 0.10 M HF and 0.10 M NaF 
B) 0.20 M HF and 0.20 M NaF 
C) 0.20 M HF and 0.10 M NaF 
D) 0.10 M HF and 0.20 M NaF 
E) All of the buffer solutions described above have the same pH.

Question 9

The addition of an acid to water increases the [H3O+] of the solution and increases the solution pH.

Accepted Answer

A) True 
 B)False

Question 10

In the reaction: SO32-(aq)+ H2O(l)   HSO3-(aq)+ -OH(aq), H2O acts as a Brønsted-Lowry acid.

Accepted Answer

A) True 
 B)False

Question 11

Ammonia, NH3, is an example of a

Accepted Answer

A) strong acid 
B) strong base 
C) weak acid 
D) weak base 
A) strong acid 
B) strong base 
C) weak acid 
D) weak base

Question 12

The products are favored in the acid-base reaction: HI(aq)+ NH3(aq)   NH4+(aq)+ I-(aq).

Accepted Answer

A) True 
 B)False

Question 13

An aqueous solution whose pH is greater than 7 has a higher [H3O+] than pure water itself.

Accepted Answer

A) True 
 B)False

Question 14

An aqueous solution containing an equal number of moles of NaF and HF is an example of a buffer solution.

Accepted Answer

A) True 
 B)False

Question 15

Water is amphoteric; it can act as an acid or a base.

Accepted Answer

A) True 
 B)False

Question 16

Which solution containing an equal number of moles of each of the substances is a buffer?

Accepted Answer

A) HCl and NaCl 
B) HNO2 and HNO3 
C) CH3COOH and NaCH3COO 
D) H2CO3 and CO32- 
E) More than one of the solutions above is a buffer. 
A) HCl and NaCl 
B) HNO2 and HNO3 
C) CH3COOH and NaCH3COO 
D) H2CO3 and CO32- 
E) More than one of the solutions above is a buffer.

Question 17

The principal buffer in the blood is carbonic acid/bicarbonate (H2CO3/HCO3-), keeping the normal blood pH of a healthy individual in the range of 7.35 to 7.45.

Accepted Answer

A) True 
 B)False

Question 18

In an acidic solution, [H3O+] > [-OH].

Accepted Answer

A) True 
 B)False

Question 19

An aqueous solution containing an equal number of moles of Na2HPO4 and H3PO4 is an example of a buffer solution.

Accepted Answer

A) True 
 B)False

Question 20

If two solutions differ in their [H3O+] by a factor of 2.0, the difference in their pH will be 2.0.

Accepted Answer

A) True 
 B)False

Exam 9: Acids and Bases

Normal gastric juice has a pH of about 2. Assuming that normal gastric juice is primarily aqueous HCl, what is the concentration of HCl in the stomach?

All compounds can be classified as either an acid or a base.

Which diagram properly depicts the dissolved species present in an aqueous solution of KOH? (water molecules are not shown)

HPO42- is amphoteric. The conjugate acid of HPO42- is _____ and its conjugate base is _____.

Which term correctly describes the medical condition in which the pH of blood is greater than 7.45, and therefore the blood is more basic than normal?

For a solution labeled 0.15 M CH3COOH, the [H3O+] is 0.15 M.

Which salt forms a basic solution when dissolved in water?

Which buffer solution has the lowest pH (HF has Ka = 7.2 × 10-4)?

The addition of an acid to water increases the [H3O+] of the solution and increases the solution pH.

In the reaction: SO32-(aq)+ H2O(l) HSO3-(aq)+ -OH(aq), H2O acts as a Brønsted-Lowry acid.

Ammonia, NH3, is an example of a

The products are favored in the acid-base reaction: HI(aq)+ NH3(aq) NH4+(aq)+ I-(aq).

An aqueous solution whose pH is greater than 7 has a higher [H3O+] than pure water itself.

An aqueous solution containing an equal number of moles of NaF and HF is an example of a buffer solution.

Water is amphoteric; it can act as an acid or a base.

Which solution containing an equal number of moles of each of the substances is a buffer?

The principal buffer in the blood is carbonic acid/bicarbonate (H2CO3/HCO3-), keeping the normal blood pH of a healthy individual in the range of 7.35 to 7.45.

In an acidic solution, [H3O+] > [-OH].

An aqueous solution containing an equal number of moles of Na2HPO4 and H3PO4 is an example of a buffer solution.

If two solutions differ in their [H3O+] by a factor of 2.0, the difference in their pH will be 2.0.

Matter and Measurement

Atoms and the Periodic Table

Ionic Compounds

Covalent Compounds

Chemical Reactions

Energy Changes, Reaction Rates, and Equilibrium

Gases, Liquids, and Solids

Solutions

Nuclear Chemistry

Introduction to Organic Molecules and Functional Groups

Alkanes

Unsaturated Hydrocarbons

Organic Compounds That Contain Oxygen, Halogen, or Sulfur

The Three-Dimensional Shape of Molecules

Aldehydes and Ketones

Carboxylic Acids, Esters, and Amides

Amines and Neurotransmitters

Lipids

Carbohydrates

Amino Acids, Proteins, and Enzymes

Nucleic Acids and Protein Synthesis

Digestion and the Conversion of Food Into Energy

Carbohydrate, Lipid, and Protein Metabolism

Filters

HPO₄^2- is amphoteric. The conjugate acid of HPO₄^2- is _ and its conjugate base is _.

For a solution labeled 0.15 M CH₃COOH, the [H₃O⁺] is 0.15 M.

Which buffer solution has the lowest pH (HF has K_a = 7.2 × 10^-4)?

The addition of an acid to water increases the [H₃O⁺] of the solution and increases the solution pH.

In the reaction: SO₃^2-(aq)+ H₂O(l) HSO₃^-(aq)+ ^-OH(aq), H₂O acts as a Brønsted-Lowry acid.

Ammonia, NH₃, is an example of a

The products are favored in the acid-base reaction: HI(aq)+ NH₃(aq) NH₄⁺(aq)+ I^-(aq).

An aqueous solution whose pH is greater than 7 has a higher [H₃O⁺] than pure water itself.

The principal buffer in the blood is carbonic acid/bicarbonate (H₂CO₃/HCO₃^-), keeping the normal blood pH of a healthy individual in the range of 7.35 to 7.45.

In an acidic solution, [H₃O⁺] > [^-OH].

An aqueous solution containing an equal number of moles of Na₂HPO₄ and H₃PO₄ is an example of a buffer solution.

If two solutions differ in their [H₃O⁺] by a factor of 2.0, the difference in their pH will be 2.0.