Question 1

HCl is a strong electrolyte.A bottle of HCl contains the label 0.015 M HCl(aq).Which statement concerning this HCl solution is FALSE?

Accepted Answer

A) The solution is acidic. 
B) The pH of the solution is 1.5. 
C) The hydronium ion concentration in this solution is 0.015 M. 
D) The solution has a higher concentration of hydronium ions than hydroxide ions. 
E) The solution contains dissolved H3O+ and Cl− ions only; no HCl molecules are present. 
A) The solution is acidic. 
B) The pH of the solution is 1.5. 
C) The hydronium ion concentration in this solution is 0.015 M. 
D) The solution has a higher concentration of hydronium ions than hydroxide ions. 
E) The solution contains dissolved H3O+ and Cl− ions only; no HCl molecules are present. B

Question 2

What term is used to describe the amount of strong acid or strong base that can be added to a buffer solution without significantly changing its pH?

Accepted Answer

A) buffer threshold 
B) Henderson-Hasselbalch strength 
C) conjugate acid-base capacity 
D) buffer capacity 
E) acid dissociation constant 
A) buffer threshold 
B) Henderson-Hasselbalch strength 
C) conjugate acid-base capacity 
D) buffer capacity 
E) acid dissociation constant D

Question 3

Which of the following statements concerning a voltaic cell is FALSE?

Accepted Answer

A) The oxidation half reaction occurs at the cathode. 
B) A voltaic cell uses an oxidation-reduction reaction to produce electrical energy. 
C) The cell consists of two half cells. 
D) The anode and the cathode are separated by a salt bridge. 
E) At the anode a substance will lose electrons. 
A) The oxidation half reaction occurs at the cathode. 
B) A voltaic cell uses an oxidation-reduction reaction to produce electrical energy. 
C) The cell consists of two half cells. 
D) The anode and the cathode are separated by a salt bridge. 
E) At the anode a substance will lose electrons. A

Question 4

Which statement correctly describes what is happening in the reaction shown below? 2Mg(s)+ S2(g)→ MgS(s)

Accepted Answer

A) Mg is oxidized. 
B) S2 loses electrons. 
C) MgS is the reducing agent. 
D) Mg is the oxidizing agent. 
E) MgS gains electrons. 
A) Mg is oxidized. 
B) S2 loses electrons. 
C) MgS is the reducing agent. 
D) Mg is the oxidizing agent. 
E) MgS gains electrons.

Question 5

Sodium hydroxide (NaOH)can react with phosphoric acid (H3PO4)in a neutralization reaction.What is the reacting ratio of NaOH to H3PO4?

Accepted Answer

A) 1:1 
B) 1:3 
C) 3:8 
D) 2:7 
E) 3:1 
A) 1:1 
B) 1:3 
C) 3:8 
D) 2:7 
E) 3:1

Question 6

Which one of the following correctly represents a conjugate acid-base pair?

Accepted Answer

A) H2O,O- 
B) H3O+,OH- 
C) H2CO3,CO32- 
D) HCl,Cl2 
E) H2CO3,HCO3- 
A) H2O,O- 
B) H3O+,OH- 
C) H2CO3,CO32- 
D) HCl,Cl2 
E) H2CO3,HCO3-

Question 7

What is the conjugate base of H2SO4?

Accepted Answer

A) SO42− 
B) HSO4− 
C) H2SO3 
D) SO4− 
E) H2PO4+ 
A) SO42− 
B) HSO4− 
C) H2SO3 
D) SO4− 
E) H2PO4+

Question 8

A sample of black coffee was measured to have [H3O+] = 7.94 × 10−6.What is TRUE about this solution?

Accepted Answer

A) The solution is acidic. 
B) The solution contains less hydronium ions than pure water itself. 
C) The solution does not contain any OH−ions. 
D) The solution has [OH−] = 7.94 × 10−6. 
E) The pH of the solution is 7.94. 
A) The solution is acidic. 
B) The solution contains less hydronium ions than pure water itself. 
C) The solution does not contain any OH−ions. 
D) The solution has [OH−] = 7.94 × 10−6. 
E) The pH of the solution is 7.94.

Question 9

Which one of the following is NOT a characteristic property of a base?

Accepted Answer

A) tastes bitter 
B) feels slippery 
C) increases [H+] in water 
D) is corrosive 
E) causes many metal ions to precipitate 
A) tastes bitter 
B) feels slippery 
C) increases [H+] in water 
D) is corrosive 
E) causes many metal ions to precipitate

Question 10

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

Accepted Answer

A) True 
 B)False

Question 11

A solution containing a buffer has an initial pH of 8.78.If a student adds 5 drops of NaCl(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 12

Strong acids are completely dissociated when dissolved in water.

Accepted Answer

A) True 
 B)False

Question 13

The main buffer system found in blood is the HCl/Cl− system.

Accepted Answer

A) True 
 B)False

Question 14

Which of the following statements concerning acids and bases is FALSE?

Accepted Answer

A) A Brønsted-Lowry acid is a proton (H+)donor. 
B) A Brønsted-Lowry base is a proton (H+)acceptor. 
C) Reactions between acids and bases involve the transfer of a proton (H+)from the acid to the base. 
D) Addition of an acid to water decreases the pH of the solution. 
E) Addition of a base to water increases the hydronium ion concentration of the solution. 
A) A Brønsted-Lowry acid is a proton (H+)donor. 
B) A Brønsted-Lowry base is a proton (H+)acceptor. 
C) Reactions between acids and bases involve the transfer of a proton (H+)from the acid to the base. 
D) Addition of an acid to water decreases the pH of the solution. 
E) Addition of a base to water increases the hydronium ion concentration of the solution.

Question 15

The concentration of a weak acid or base affects its degree of dissociation in water.

Accepted Answer

A) True 
 B)False

Question 16

Calculate the molar concentration of a sodium hydroxide solution if 60.00 mL of this solution were required to neutralize 30.00 mL of a 0.150 M hydrochloric acid solution.NaOH(aq)+ HCl(aq)→ NaCl(aq)+ H2O(l)

Accepted Answer

A) 3.00 M 
B) 6.00 M 
C) 0.0750 M 
D) 0.150 M 
E) 2.25 M 
A) 3.00 M 
B) 6.00 M 
C) 0.0750 M 
D) 0.150 M 
E) 2.25 M

Question 17

Nitric acid is a strong acid and dissociates completely when dissolved in water.

Accepted Answer

A) True 
 B)False

Question 18

An aqueous solution with a low pH is necessary for a certain industrial process.Which of the following solutions would have the lowest pH?

Accepted Answer

A) 2.0 M NaOH 
B) 0.5 M HCl 
C) 1.0 M acetic acid 
D) 1.0 M HCl 
E) All solutions would have the same pH. 
A) 2.0 M NaOH 
B) 0.5 M HCl 
C) 1.0 M acetic acid 
D) 1.0 M HCl 
E) All solutions would have the same pH.

Question 19

According to Arrhenius' theory of acids and bases,acids increase the hydrogen ion concentration in water.

Accepted Answer

A) True 
 B)False

Question 20

What is the general term for the process in which a chemical species loses electrons?

Accepted Answer

A) oxidation 
B) reduction 
C) condensation 
D) Lewis base 
E) decomposition 
A) oxidation 
B) reduction 
C) condensation 
D) Lewis base 
E) decomposition

Exam 8: Acids and Bases

HCl is a strong electrolyte.A bottle of HCl contains the label 0.015 M HCl(aq).Which statement concerning this HCl solution is FALSE?

What term is used to describe the amount of strong acid or strong base that can be added to a buffer solution without significantly changing its pH?

Which of the following statements concerning a voltaic cell is FALSE?

Which statement correctly describes what is happening in the reaction shown below? 2Mg(s)+ S2(g)→ MgS(s)

Sodium hydroxide (NaOH)can react with phosphoric acid (H3PO4)in a neutralization reaction.What is the reacting ratio of NaOH to H3PO4?

Which one of the following correctly represents a conjugate acid-base pair?

What is the conjugate base of H2SO4?

A sample of black coffee was measured to have [H3O+] = 7.94 × 10−6.What is TRUE about this solution?

Which one of the following is NOT a characteristic property of a base?

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

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

Strong acids are completely dissociated when dissolved in water.

The main buffer system found in blood is the HCl/Cl− system.

Which of the following statements concerning acids and bases is FALSE?

The concentration of a weak acid or base affects its degree of dissociation in water.

Calculate the molar concentration of a sodium hydroxide solution if 60.00 mL of this solution were required to neutralize 30.00 mL of a 0.150 M hydrochloric acid solution.NaOH(aq)+ HCl(aq)→ NaCl(aq)+ H2O(l)

Nitric acid is a strong acid and dissociates completely when dissolved in water.

An aqueous solution with a low pH is necessary for a certain industrial process.Which of the following solutions would have the lowest pH?

According to Arrhenius' theory of acids and bases,acids increase the hydrogen ion concentration in water.

What is the general term for the process in which a chemical species loses electrons?

Chemistry - Methods and Measurement

The Structure of the Atom and the Periodic Table

Structure and Properties of Ionic and Covalent Compounds

Calculations, chemical Changes, and the Chemical Equation

States of Matter: Gases, liquids, and Solids

Solutions

Energy,rate and Equilibrium

The Nucleus, radioactivity, and Nuclear Medicine

An Introduction to Organic Chemistry

The Unsaturated Hydrocarbons: Alkenes, alkynes, and Aromatics

Alcohols, phenols, thiols, and Ethers

Aldehydes and Ketones

Carboxylic Acids and Carboxylic Acid Derivatives

Amines and Amides

Carbohydrates

Lipids and Their Functions in Biochemical Systems

Protein Structure and Function

Enzymes

Introduction to Molecular Genetics

Carbohydrate Metabolism

Aerobic Respiration and Energy Production

Fatty Acid Metabolism

Filters

Which statement correctly describes what is happening in the reaction shown below? 2Mg(s)+ S₂(g)→ MgS(s)

Sodium hydroxide (NaOH)can react with phosphoric acid (H₃PO₄)in a neutralization reaction.What is the reacting ratio of NaOH to H₃PO₄?

What is the conjugate base of H₂SO₄?

A sample of black coffee was measured to have [H₃O⁺] = 7.94 × 10⁻⁶.What is TRUE about this solution?

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

The main buffer system found in blood is the HCl/Cl⁻ system.

Calculate the molar concentration of a sodium hydroxide solution if 60.00 mL of this solution were required to neutralize 30.00 mL of a 0.150 M hydrochloric acid solution.NaOH(aq)+ HCl(aq)→ NaCl(aq)+ H₂O(l)