Question 1

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

Accepted Answer

A) True 
 B)False

Question 2

In the following acid-base equation,the reactant ________ is behaving as the Brønsted-Lowry Acid:
HCN + H2O   CN- + H3O+

Accepted Answer

Question 3

Which solution has the highest pH?

Accepted Answer

A) 4.3 × 10-8 M -OH 
B) 1.0 × 10-7 M -OH 
C) 5.1 × 10-2 M H3O+ 
D) 1.9 × 10-8 M -OH 
E) 1.0 × 10-2 M H3O+ 
A) 4.3 × 10-8 M -OH 
B) 1.0 × 10-7 M -OH 
C) 5.1 × 10-2 M H3O+ 
D) 1.9 × 10-8 M -OH 
E) 1.0 × 10-2 M H3O+

Question 4

Which acid is the strongest?

Accepted Answer

A) Hydrogen sulfate ion HSO4- (Ka = 1.2 × 10-2) 
B) Hydrocyanic acid HCN (Ka = 4.9 × 10-10) 
C) Hydrofluoric acid HF (Ka = 7.2 × 10-4) 
D) Ammonium ion NH4+ (Ka = 5.6 × 10-10) 
A) Hydrogen sulfate ion HSO4- (Ka = 1.2 × 10-2) 
B) Hydrocyanic acid HCN (Ka = 4.9 × 10-10) 
C) Hydrofluoric acid HF (Ka = 7.2 × 10-4) 
D) Ammonium ion NH4+ (Ka = 5.6 × 10-10)

Question 5

The pH of a lime is 1.90. What is the [H3O+]?

Accepted Answer

A) 1.3 × 10-2 M H3O+ 
B) 1.3 × 1012 M H3O+ 
C) 7.9 × 101 M H3O+ 
D) 7.9 × 10-13 M H3O+ 
E) 1.9 M H3O+ 
A) 1.3 × 10-2 M H3O+ 
B) 1.3 × 1012 M H3O+ 
C) 7.9 × 101 M H3O+ 
D) 7.9 × 10-13 M H3O+ 
E) 1.9 M H3O+

Question 6

A sample of urine has a pH of 8.2. Which statement describing the urine sample is NOT true?

Accepted Answer

A) The urine sample is basic. 
B) The urine sample has a hydronium ion concentration greater than that of a neutral solution. 
C) The urine sample has a hydroxide ion concentration greater than its hydronium ion concentration. 
D) The urine sample has a hydroxide ion concentration greater than 1.0 × 10-7. 
A) The urine sample is basic. 
B) The urine sample has a hydronium ion concentration greater than that of a neutral solution. 
C) The urine sample has a hydroxide ion concentration greater than its hydronium ion concentration. 
D) The urine sample has a hydroxide ion concentration greater than 1.0 × 10-7.

Question 7

What is the balanced equation for the acid-base reaction of nitrous acid with lithium hydroxide?

Accepted Answer

A) LiOH(aq)+ HNO3(aq)   H2O(l)+ LiNO3(aq) 
B) Li(OH)2(aq)+ 2 HNO3(aq)   2 H2O(l)+ Li(NO3)2(aq) 
C) LiOH(aq)+ HNO2(aq)   H2O(l)+ LiNO2(aq) 
D) 2 LiOH(aq)+ H2NO2(aq)   2 H2O(l)+ Li2NO2(aq) 
A) LiOH(aq)+ HNO3(aq)   H2O(l)+ LiNO3(aq) 
B) Li(OH)2(aq)+ 2 HNO3(aq)   2 H2O(l)+ Li(NO3)2(aq) 
C) LiOH(aq)+ HNO2(aq)   H2O(l)+ LiNO2(aq) 
D) 2 LiOH(aq)+ H2NO2(aq)   2 H2O(l)+ Li2NO2(aq)

Question 8

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 9

When phosphoric acid (H3PO4)dissolves in water,the following equilibrium is established: H3PO4 + H2O   H3O+ + H2PO4- If Ka = 7.5 × 10-3 for H3PO4,which statement concerning an aqueous solution of phosphoric acid is correct?

Accepted Answer

A) An aqueous solution of phosphoric acid contains mainly H3PO4 molecules. 
B) An aqueous solution of phosphoric acid contains predominantly H3O+ and H2PO4- ions. 
C) An aqueous solution of phosphoric acid contains equal amounts of H3O+ and H3PO4. 
D) An aqueous solution of phosphoric acid contains a greater concentration of dissolved ions than it does neutral phosphoric acid molecules. 
A) An aqueous solution of phosphoric acid contains mainly H3PO4 molecules. 
B) An aqueous solution of phosphoric acid contains predominantly H3O+ and H2PO4- ions. 
C) An aqueous solution of phosphoric acid contains equal amounts of H3O+ and H3PO4. 
D) An aqueous solution of phosphoric acid contains a greater concentration of dissolved ions than it does neutral phosphoric acid molecules.

Question 10

Which species is the conjugate acid of HCO3-?

Accepted Answer

A) CO32- 
B) H2CO3 
C) CO2 
D) H2O 
A) CO32- 
B) H2CO3 
C) CO2 
D) H2O

Question 11

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

Accepted Answer

A) True 
 B)False

Question 12

Which pH value indicates the higher concentration of OH-?

Accepted Answer

A) pH = 3.7 
B) pH = 10.2 
C) pH = 8.8 
D) pH = 6.9 
E) pH = 11.4 
A) pH = 3.7 
B) pH = 10.2 
C) pH = 8.8 
D) pH = 6.9 
E) pH = 11.4

Question 13

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

Accepted Answer

A) True 
 B)False

Question 14

OH- and NH4+ are both examples of Brønsted-Lowry bases.

Accepted Answer

A) True 
 B)False

Question 15

What is the pH of a buffer that contains 0.15 M CH3COOH and 0.10 M NaCH3COO (Ka = 1.8 × 10-5)?

Accepted Answer

A) 4.74 
B) 7.00 
C) 4.57 
D) 4.92 
A) 4.74 
B) 7.00 
C) 4.57 
D) 4.92

Question 16

The pH of a 1.0 × 10-5 M H3O+ solution is 5.00.

Accepted Answer

A) True 
 B)False

Question 17

Which species can act as a Brønsted-Lowry acid?

Accepted Answer

A) CO32- 
B) HCl 
C) Br2 
D) LiOH 
A) CO32- 
B) HCl 
C) Br2 
D) LiOH

Question 18

The addition of a base to water decreases the pH of the solution.

Accepted Answer

A) True 
 B)False

Question 19

Which species is the conjugate base of NH3?

Accepted Answer

A) NH4+ 
B) NH2 
C) NH2- 
D) H2O 
E) NH4OH 
A) NH4+ 
B) NH2 
C) NH2- 
D) H2O 
E) NH4OH

Question 20

An Arrhenius base is ________.

Accepted Answer

A) a compound that contains hydroxide and dissolves in water to form OH- 
B) a compound that is a proton donor 
C) a compound that is a proton acceptor 
D) a compound that contains a hydrogen atom and dissolves in water to form a hydrogen ion,H+ 
A) a compound that contains hydroxide and dissolves in water to form OH- 
B) a compound that is a proton donor 
C) a compound that is a proton acceptor 
D) a compound that contains a hydrogen atom and dissolves in water to form a hydrogen ion,H+

Exam 9: Acids and Bases

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

In the following acid-base equation,the reactant ________ is behaving as the Brønsted-Lowry Acid: HCN + H2O CN- + H3O+

Which solution has the highest pH?

Which acid is the strongest?

The pH of a lime is 1.90. What is the [H3O+]?

A sample of urine has a pH of 8.2. Which statement describing the urine sample is NOT true?

What is the balanced equation for the acid-base reaction of nitrous acid with lithium hydroxide?

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

When phosphoric acid (H3PO4)dissolves in water,the following equilibrium is established: H3PO4 + H2O H3O+ + H2PO4- If Ka = 7.5 × 10-3 for H3PO4,which statement concerning an aqueous solution of phosphoric acid is correct?

Which species is the conjugate acid of HCO3-?

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

Which pH value indicates the higher concentration of OH-?

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

OH- and NH4+ are both examples of Brønsted-Lowry bases.

What is the pH of a buffer that contains 0.15 M CH3COOH and 0.10 M NaCH3COO (Ka = 1.8 × 10-5)?

The pH of a 1.0 × 10-5 M H3O+ solution is 5.00.

Which species can act as a Brønsted-Lowry acid?

The addition of a base to water decreases the pH of the solution.

Which species is the conjugate base of NH3?

An Arrhenius base is ________.

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

Metabolism and Energy Production

Carbohydrate,lipid,and Protein Metabolism

Filters

In the following acid-base equation,the reactant ________ is behaving as the Brønsted-Lowry Acid: HCN + H₂O CN^- + H₃O⁺

The pH of a lime is 1.90. What is the [H₃O⁺]?

When phosphoric acid (H₃PO₄)dissolves in water,the following equilibrium is established: H₃PO₄ + H₂O H₃O⁺ + H₂PO₄^- If K_a = 7.5 × 10^-3 for H₃PO₄,which statement concerning an aqueous solution of phosphoric acid is correct?

Which species is the conjugate acid of HCO₃^-?

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

Which pH value indicates the higher concentration of OH^-?

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

OH^- and NH₄⁺ are both examples of Brønsted-Lowry bases.

What is the pH of a buffer that contains 0.15 M CH₃COOH and 0.10 M NaCH₃COO (K_a = 1.8 × 10^-5)?

The pH of a 1.0 × 10^-5 M H₃O⁺ solution is 5.00.

Which species is the conjugate base of NH₃?