Question 1

What is the hydronium ion concentration of an acid rain sample that has a pH of 3.35?

Accepted Answer

A) 2.2 × 10-11 mol L-1 
B) 4.5 × 10-4 mol L-1 
C) 3.35 mol L-1 
D) 10.65 mol L-1 
A) 2.2 × 10-11 mol L-1 
B) 4.5 × 10-4 mol L-1 
C) 3.35 mol L-1 
D) 10.65 mol L-1

Question 2

The pH of an aqueous solution at 25.0 °C is 10.55.What is the molarity of  
In this solution?

Accepted Answer

A) 2.8 × 10-11 
B) 3.5 × 10-4 
C) 3.3 
D) 1.1 × 10-13 
E) 3.5 × 1010 
A) 2.8 × 10-11 
B) 3.5 × 10-4 
C) 3.3 
D) 1.1 × 10-13 
E) 3.5 × 1010

Question 3

Choose the INCORRECT statement.The term pH:

Accepted Answer

A) refers to the "potential" of hydrogen ion 
B) = -ln [H+] 
C) = 14 - pOH 
D) is more convenient than exponential notation 
E) = -log [H3O+] 
A) refers to the "potential" of hydrogen ion 
B) = -ln [H+] 
C) = 14 - pOH 
D) is more convenient than exponential notation 
E) = -log [H3O+]

Question 4

Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10-6 mol L-1 in hydroxide ion.

Accepted Answer

A) 4.00 × 10-7 mol L-1 
B) 4.00 × 10-8 mol L-1 
C) 4.00 × 10-9 mol L-1 
D) 5.00 × 10-9 mol L-1 
A) 4.00 × 10-7 mol L-1 
B) 4.00 × 10-8 mol L-1 
C) 4.00 × 10-9 mol L-1 
D) 5.00 × 10-9 mol L-1

Question 5

An aqueous solution at 25.0 °C contains [  ] = 0.085 mol L-1.What is the pH of the solution?

Accepted Answer

A) 1.07 
B) -1.07 
C) 13.0 
D) 0.0850 
E) 1.20 ×   
A) 1.07 
B) -1.07 
C) 13.0 
D) 0.0850 
E) 1.20 ×

Question 6

A 250.0 ml sample of gaseous hydrogen bromide,measured at 22.9 °C and 0.930 atm,was dissolved in sufficient pure water to form 250.0 ml of solution.What was the pH of that solution?

Accepted Answer

A) 1.42 
B) 2.58 
C) 3.83 
D) 4.18 
E) 5.68 
A) 1.42 
B) 2.58 
C) 3.83 
D) 4.18 
E) 5.68

Question 7

What is the [AsO43-] for a solution labeled "0.10 M arsenic acid (H3AsO4)"?
[Ka1 = 6 × 10-3,Ka2 = 1 × 10-7,Ka3 = 3 × 10-12]

Accepted Answer

A) 1 × 10-7 M 
B) 1 × 10-17 M 
C) 3 × 10-12 M 
D) 3 × 10-19 M 
E) 6 × 10-10 M 
A) 1 × 10-7 M 
B) 1 × 10-17 M 
C) 3 × 10-12 M 
D) 3 × 10-19 M 
E) 6 × 10-10 M

Question 8

Determine the ammonia concentration of an aqueous solution that has a pH of 11.00.The equation for the dissociation of NH3 (Kb = 1.8 × 10-5)is below:

Accepted Answer

A) 3.0 mol L-1 
B) 0.056 mol L-1 
C) 1.8 × 10-2 mol L-1 
D) 1.0 × 10-3 mol L-1 
A) 3.0 mol L-1 
B) 0.056 mol L-1 
C) 1.8 × 10-2 mol L-1 
D) 1.0 × 10-3 mol L-1

Question 9

What is the pH of a 0.235 M aqueous solution of potassium fluoride? Ka (HF)= 6.6 × 10-4

Accepted Answer

A) 8.28 
B) 11.45 
C) 8.59 
D) 5.41 
E) 5.72 
A) 8.28 
B) 11.45 
C) 8.59 
D) 5.41 
E) 5.72

Question 10

For NH3,predict whether a 1 M aqueous solution is acidic,basic or neutral and why.

Accepted Answer

A) acidic because NH3 is a strong acid 
B) basic because NH3 is a weak base 
C) neutral because there is no hydrolysis 
D) basic because NH3 is the salt of a weak acid 
E) acidic because NH3 is the salt of a weak base 
A) acidic because NH3 is a strong acid 
B) basic because NH3 is a weak base 
C) neutral because there is no hydrolysis 
D) basic because NH3 is the salt of a weak acid 
E) acidic because NH3 is the salt of a weak base

Question 11

In which of the following cases is water acting as a base under the Lewis definitions,but not under the Bronsted-Lowry definitions?

Accepted Answer

A) H2O(l)+ HF(g)⇌ H3O+(aq)+ F-(aq) 
B) H2O(l)+ CN-(aq)⇌ OH-(aq)+ HCN(aq) 
C) 2 H2O(l)+ Cu2+(aq)⇌ Cu(H2O)22+(aq) 
D) 2 H2O(l)+ PO43-(aq)⇌ 2 OH-(aq)+ H2PO4-(aq) 
E) 2 H2O(l)[electrolysis] ⇌ 2 H2(g)+ O2(g) 
A) H2O(l)+ HF(g)⇌ H3O+(aq)+ F-(aq) 
B) H2O(l)+ CN-(aq)⇌ OH-(aq)+ HCN(aq) 
C) 2 H2O(l)+ Cu2+(aq)⇌ Cu(H2O)22+(aq) 
D) 2 H2O(l)+ PO43-(aq)⇌ 2 OH-(aq)+ H2PO4-(aq) 
E) 2 H2O(l)[electrolysis] ⇌ 2 H2(g)+ O2(g)

Question 12

The definition of a neutralization reaction as a reaction in which an acid reacts with a base to produce water and a salt is inherent in:

Accepted Answer

A) only the Arrhenius theory 
B) both the Arrhenius and the Br∅nsted-Lowry theories 
C) only the Br∅nsted-Lowry theory 
D) both the Br∅nsted-Lowry and the Lewis theories 
E) only the Lewis theory 
A) only the Arrhenius theory 
B) both the Arrhenius and the Br∅nsted-Lowry theories 
C) only the Br∅nsted-Lowry theory 
D) both the Br∅nsted-Lowry and the Lewis theories 
E) only the Lewis theory

Question 13

A saturated aqueous solution of calcium hydroxide is approximately 0.13% calcium hydroxide,by mass,and has a density of 1.02 g ml-1.What is the pH of such a solution?

Accepted Answer

A) 11.95 
B) 12.25 
C) 12.55 
D) 12.75 
E) 13.00 
A) 11.95 
B) 12.25 
C) 12.55 
D) 12.75 
E) 13.00

Question 14

What is the pH of a 0.470 M aqueous solution of pyridine? 
Kb = 1.5 × 10-9

Accepted Answer

A) 9.0 
B) 11.2 
C) 2.8 
D) 9.4 
E) 4.6 
A) 9.0 
B) 11.2 
C) 2.8 
D) 9.4 
E) 4.6

Question 15

A 7.0 × 10-3 mol L-1 aqueous solution of   At 25.0 °C has a pH of:

Accepted Answer

A) 12.15 
B) 1.85 
C) 1.4 × 10-2 
D) 7.1 × 10-13 
E) 11.85 
A) 12.15 
B) 1.85 
C) 1.4 × 10-2 
D) 7.1 × 10-13 
E) 11.85

Question 16

In the following reversible reaction the Br∅nsted acids are ________.
HCO3-(aq)+ OH-(aq)⇌ CO32-(aq)+ H2O

Accepted Answer

A) HCO3- and H2O 
B) HCO3- and CO32-  
C) OH- and CO32-  
D) OH- and H2O 
E) H2O and CO32- 
A) HCO3- and H2O 
B) HCO3- and CO32-  
C) OH- and CO32-  
D) OH- and H2O 
E) H2O and CO32-

Question 17

For which of the following polyprotic acids is the first ionization step approximately 100%?

Accepted Answer

A) H2S 
B) H2SO3  
C) H2CO3  
D) H2SO4  
E) H3PO4  
A) H2S 
B) H2SO3  
C) H2CO3  
D) H2SO4  
E) H3PO4

Question 18

Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

Accepted Answer

A) NaHCO3 
B) KClO4 
C) Na2CO3 
D) CH3NH3Cl  
A) NaHCO3 
B) KClO4 
C) Na2CO3 
D) CH3NH3Cl

Question 19

Which of the following are Lewis bases?
I.BCl3 
II.H- 
III.H2O
IV.NH3 
V.AlCl3

Accepted Answer

A) II,IIIand IV 
B) I,II,and III 
C) III,IVand V 
D) I,II,and V 
E) I,II,and IV 
A) II,IIIand IV 
B) I,II,and III 
C) III,IVand V 
D) I,II,and V 
E) I,II,and IV

Question 20

For NaCl,predict whether the aqueous solution is acidic,basic or neutral and why.

Accepted Answer

A) acidic because NaCl is a strong acid 
B) basic because NaCl is a weak base 
C) neutral because there is no hydrolysis 
D) basic because NaCl is the salt of a weak acid 
E) acidic because NaCl is the salt of a weak base 
A) acidic because NaCl is a strong acid 
B) basic because NaCl is a weak base 
C) neutral because there is no hydrolysis 
D) basic because NaCl is the salt of a weak acid 
E) acidic because NaCl is the salt of a weak base

Exam 16: Acids and Bases

What is the hydronium ion concentration of an acid rain sample that has a pH of 3.35?

The pH of an aqueous solution at 25.0 °C is 10.55.What is the molarity of In this solution?

Choose the INCORRECT statement.The term pH:

Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10-6 mol L-1 in hydroxide ion.

An aqueous solution at 25.0 °C contains [ ] = 0.085 mol L-1.What is the pH of the solution?

A 250.0 ml sample of gaseous hydrogen bromide,measured at 22.9 °C and 0.930 atm,was dissolved in sufficient pure water to form 250.0 ml of solution.What was the pH of that solution?

What is the [AsO43-] for a solution labeled "0.10 M arsenic acid (H3AsO4)"? [Ka1 = 6 × 10-3,Ka2 = 1 × 10-7,Ka3 = 3 × 10-12]

Determine the ammonia concentration of an aqueous solution that has a pH of 11.00.The equation for the dissociation of NH3 (Kb = 1.8 × 10-5)is below:

What is the pH of a 0.235 M aqueous solution of potassium fluoride? Ka (HF)= 6.6 × 10-4

For NH3,predict whether a 1 M aqueous solution is acidic,basic or neutral and why.

In which of the following cases is water acting as a base under the Lewis definitions,but not under the Bronsted-Lowry definitions?

The definition of a neutralization reaction as a reaction in which an acid reacts with a base to produce water and a salt is inherent in:

A saturated aqueous solution of calcium hydroxide is approximately 0.13% calcium hydroxide,by mass,and has a density of 1.02 g ml-1.What is the pH of such a solution?

What is the pH of a 0.470 M aqueous solution of pyridine? Kb = 1.5 × 10-9

A 7.0 × 10-3 mol L-1 aqueous solution of At 25.0 °C has a pH of:

In the following reversible reaction the Br∅nsted acids are ________. HCO3-(aq)+ OH-(aq)⇌ CO32-(aq)+ H2O

For which of the following polyprotic acids is the first ionization step approximately 100%?

Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

Which of the following are Lewis bases? I.BCl3 II.H- III.H2O IV.NH3 V.AlCl3

For NaCl,predict whether the aqueous solution is acidic,basic or neutral and why.

Matter: Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Valence Bond and Molecular Orbital Theories

Intermolecular Forces: Liquids and Solids

Spontaneous Change: Entropy and Gibbs Energy

Solutions and Their Physical Properties

Principles of Chemical Equilibrium

Additional Aspects of Acidbase Equilibria

Solubility and Complex-Ion Equilibria

Electrochemistry

Chemical Kinetics

Chemistry of the Main-Group Elements I: Groups 1,2,13,and 14

Chemistry of the Main-Group Elements Ii: Groups 18,17,16,15,and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10^-⁶ mol L^-1in hydroxide ion.

An aqueous solution at 25.0 °C contains [ ] = 0.085 mol L^-1.What is the pH of the solution?

What is the [AsO₄^3-] for a solution labeled "0.10 M arsenic acid (H₃AsO₄)"? [K_a1 = 6 × 10^-3,K_a2 = 1 × 10^-7,K_a3 = 3 × 10^-12]

Determine the ammonia concentration of an aqueous solution that has a pH of 11.00.The equation for the dissociation of NH₃ (K_b= 1.8 × 10^-5)is below:

What is the pH of a 0.235 M aqueous solution of potassium fluoride? Ka (HF)= 6.6 × 10^-4

For NH₃,predict whether a 1 M aqueous solution is acidic,basic or neutral and why.

A saturated aqueous solution of calcium hydroxide is approximately 0.13% calcium hydroxide,by mass,and has a density of 1.02 g ml^-1.What is the pH of such a solution?

What is the pH of a 0.470 M aqueous solution of pyridine? K_b = 1.5 × 10^-9

A 7.0 × 10^-3 mol L^-1 aqueous solution of At 25.0 °C has a pH of:

In the following reversible reaction the Br∅nsted acids are ________. HCO₃^-(aq)+ OH^-(aq)⇌ CO₃^2-(aq)+ H₂O

Which of the following are Lewis bases? I.BCl₃ II.H^- III.H₂O IV.NH₃ V.AlCl₃