Question 1

Which of the following ionic compounds does not produce a basic aqueous solution at 25 °C?

Accepted Answer

A)  LiCN 
B)  Na3PO4 
C)  LiNO2 
D)  KHSO3 
E)  LiCH3CO2 
A)  LiCN 
B)  Na3PO4 
C)  LiNO2 
D)  KHSO3 
E)  LiCH3CO2

Question 2

Aqueous solutions of ammonia (NH3)and hydrogen cyanide (HCN)react to produce ammonium cyanide,(NH4CN)according to the following equilibrium reaction. NH3(aq)+ HCN(aq)D NH4+(aq)+ CN−(aq)
Given the following equilibrium constants,which statement best describes the reaction once equilibrium is established? (Kw = 1.01 × 10-14)
NH4+
Ka = 5.6 × 10-10
HCN
Ka = 4.0 × 10-10

Accepted Answer

A)  The reaction is product favored. 
B)  The reaction is reactant favored. 
C)  The reaction is neither product nor reactant favored. 
A)  The reaction is product favored. 
B)  The reaction is reactant favored. 
C)  The reaction is neither product nor reactant favored.

Question 3

At 50°C the autoionization constant for pure water,Kw,is   .What is the H3O+ concentration in pure water at 50°C?

Accepted Answer

A)    M 
B)  1.01 × 10-7 M 
C)    M 
D)    M 
E)  1.01 × 10-14 M 
A)    M 
B)  1.01 × 10-7 M 
C)    M 
D)    M 
E)  1.01 × 10-14 M

Question 4

What is the H3O+ concentration in 0.0072 M NaOH(aq)at 25 °C? (Kw = 1.01 × 10-14)

Accepted Answer

A)  1.4 × 10-12 M 
B)  7.2 × 10-3 M 
C)  1.0 × 10-14 M 
D)  1.0 × 10-7 M 
E)  7.2 × 10-17 M 
A)  1.4 × 10-12 M 
B)  7.2 × 10-3 M 
C)  1.0 × 10-14 M 
D)  1.0 × 10-7 M 
E)  7.2 × 10-17 M

Question 5

Which of the following expressions is not equivalent to the formula of pH?

Accepted Answer

A)  -log [H+(aq)] 
B)    
C)  14.0 - pOH 
D)    
E)  -log Kw 
A)  -log [H+(aq)] 
B)    
C)  14.0 - pOH 
D)    
E)  -log Kw

Question 6

Carbonic acid is a diprotic acid,H2CO3,with Ka1 = 4.2 × 10-7 and Ka2 = 4.8 × 10-11 at 25°C.The ion product for water is Kw = 1.0 × 10-14 at 25°C.What is the OH- concentration of a solution that is 0.39 M in Na2CO3?

Accepted Answer

A)  9.0 × 10-3 M 
B)  2.1 × 10-4 M 
C)  9.6 × 10-5 M 
D)  4.3 × 10-6 M 
E)  4.0 × 10-4 M 
A)  9.0 × 10-3 M 
B)  2.1 × 10-4 M 
C)  9.6 × 10-5 M 
D)  4.3 × 10-6 M 
E)  4.0 × 10-4 M

Question 7

The equilibrium constant,Ka,for a monoprotic acid (benzoic acid)is 6.3 × 10-5.Which of the following is the correct value of Kb for the benzoate ion,the conjugate base of benzoic acid?

Accepted Answer

A)  1.6 × 10-10 
B)  6.3 × 10-5 
C)  1.6 × 104 
D)  6.3 × 109 
E)  6.3 × 10-19 
A)  1.6 × 10-10 
B)  6.3 × 10-5 
C)  1.6 × 104 
D)  6.3 × 109 
E)  6.3 × 10-19

Question 8

In the reaction CaO(s)+ CO2(g)→ CaCO3(s),

Accepted Answer

A)  O2- acts as a Lewis base and CO2 acts as a Lewis acid. 
B)  O2- acts as a Lewis base and Ca2+ acts as a Lewis acid. 
C)  CaO is the Lewis acid and CaCO3 is its conjugate base. 
D)  CO2 is the Lewis acid and CaCO3 is its conjugate base. 
E)  Ca2+ acts as a Lewis acid and CO32- acts as a Lewis base. 
A)  O2- acts as a Lewis base and CO2 acts as a Lewis acid. 
B)  O2- acts as a Lewis base and Ca2+ acts as a Lewis acid. 
C)  CaO is the Lewis acid and CaCO3 is its conjugate base. 
D)  CO2 is the Lewis acid and CaCO3 is its conjugate base. 
E)  Ca2+ acts as a Lewis acid and CO32- acts as a Lewis base.

Question 9

Molecules or ions that can alternately behave as either a Brønsted-Lowry acid or base are called

Accepted Answer

A)  polyanions. 
B)  hydronium ions. 
C)  polyprotic acids or bases. 
D)  conjugate acids or bases. 
E)  amphiprotic. 
A)  polyanions. 
B)  hydronium ions. 
C)  polyprotic acids or bases. 
D)  conjugate acids or bases. 
E)  amphiprotic.

Question 10

What is the equilibrium hydronium ion concentration of an initially 4.5 M solution of hypoiodous acid,HOI,at 25°C (Ka =   )?

Accepted Answer

A)    M 
B)    M 
C)    M 
D)    M 
E)    M 
A)    M 
B)    M 
C)    M 
D)    M 
E)    M

Question 11

Calculate the pH of a 1.7 M solution of H2A (Ka1 = 1.0 × 10-6 and Ka2 is 1.0 × 10-10).

Accepted Answer

A)  10.00 
B)  2.88 
C)  11.12 
D)  5.77 
E)  7.00 
A)  10.00 
B)  2.88 
C)  11.12 
D)  5.77 
E)  7.00

Question 12

Which of the following is the correct hydroxide ion concentration in 0.48 M CH3CO2-(aq)? (Kb of CH3CO2- = 5.6 × 10-10)

Accepted Answer

A)  2.7 × 10-10 M 
B)  6.2 × 10-10 M 
C)  1.1 × 10-5 M 
D)  1.6 × 10-5 M 
E)  2.4 × 10-5 M 
A)  2.7 × 10-10 M 
B)  6.2 × 10-10 M 
C)  1.1 × 10-5 M 
D)  1.6 × 10-5 M 
E)  2.4 × 10-5 M

Question 13

At 25 °C,all of the following ions produce an acidic solution,except ____.

Accepted Answer

A)  NH4+ 
B)  HSO3- 
C)  HPO42- 
D)  [Fe(H2O)6]3+ 
E)  [Al(H2O)6]3+ 
A)  NH4+ 
B)  HSO3- 
C)  HPO42- 
D)  [Fe(H2O)6]3+ 
E)  [Al(H2O)6]3+

Question 14

Which one of the following aqueous solutions will have a pH of 2.00 at 25 °C? (Kw = 1.01 × 10-14)

Accepted Answer

A)  0.020 M HNO3 
B)  2.0 M NaOH 
C)  10.0 M HBr 
D)  10.0 M KCl 
E)  0.010 M HCl 
A)  0.020 M HNO3 
B)  2.0 M NaOH 
C)  10.0 M HBr 
D)  10.0 M KCl 
E)  0.010 M HCl

Question 15

Which of the following is true of the equilibrium constants (K,Ka,Kb)?

Accepted Answer

A)  The smaller the value of Ka,the larger the value of Kb. 
B)  A small value of K indicates that ionization products are strongly favored. 
C)  A large value of K indicates that reactants are favored. 
D)  The strongest acids have the smallest Ka values. 
E)  The strongest bases have the smallest Kb values. 
A)  The smaller the value of Ka,the larger the value of Kb. 
B)  A small value of K indicates that ionization products are strongly favored. 
C)  A large value of K indicates that reactants are favored. 
D)  The strongest acids have the smallest Ka values. 
E)  The strongest bases have the smallest Kb values.

Question 16

The complete reaction of an acid and base is as follows. HNO3(aq)+ LiOH(aq)→ H2O(   )+ LiNO3(aq)
What is the equilibrium constant for the net ionic reaction at 25 °C?

Accepted Answer

A)  1.01 × 10-14 
B)  1.01 × 10-7 
C)  1.01 × 107 
D)  1.01 × 1014 
E)  more information required 
A)  1.01 × 10-14 
B)  1.01 × 10-7 
C)  1.01 × 107 
D)  1.01 × 1014 
E)  more information required

Question 17

Given the following equilibrium constants, Ka (HSO4-)= 1.2 × 10-2
Kb (CH3CO2-)= 5.6 × 10-10
Kw = 1.00 × 10-14
determine the equilibrium constant for the reaction below at 25 °C.
HSO4-(aq)+ CH3CO2-(aq)   SO42-(aq)+ CH3CO2H(aq)

Accepted Answer

A)  6.7 × 10-12 
B)  2.1 × 10-7 
C)  1.5 × 10-3 
D)  6.7 × 102 
E)  2.1 × 107 
A)  6.7 × 10-12 
B)  2.1 × 10-7 
C)  1.5 × 10-3 
D)  6.7 × 102 
E)  2.1 × 107

Question 18

All of the following compounds are acids containing chlorine.Which compound is the weakest acid?

Accepted Answer

A)  HCl 
B)  HClO 
C)  HClO2 
D)  HClO3 
E)  HClO4 
A)  HCl 
B)  HClO 
C)  HClO2 
D)  HClO3 
E)  HClO4

Question 19

What is the pH of a 0.33 M solution of methylamine (CH3NH2,Kb = 4.4 × 10-4)at 25oC? (Kw = 1.01 × 10-14)

Accepted Answer

A)  5.56 
B)  0.48 
C)  12.07 
D)  13.52 
E)  1.93 
A)  5.56 
B)  0.48 
C)  12.07 
D)  13.52 
E)  1.93

Question 20

When a Lewis acid and a Lewis base combine,the product may be referred to as an acid-base ________.

Accepted Answer

The answer of When a Lewis acid and a Lewis...

Exam 17: Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Which of the following ionic compounds does not produce a basic aqueous solution at 25 °C?

At 50°C the autoionization constant for pure water,Kw,is .What is the H3O+ concentration in pure water at 50°C?

What is the H3O+ concentration in 0.0072 M NaOH(aq)at 25 °C? (Kw = 1.01 × 10-14)

Which of the following expressions is not equivalent to the formula of pH?

Carbonic acid is a diprotic acid,H2CO3,with Ka1 = 4.2 × 10-7 and Ka2 = 4.8 × 10-11 at 25°C.The ion product for water is Kw = 1.0 × 10-14 at 25°C.What is the OH- concentration of a solution that is 0.39 M in Na2CO3?

The equilibrium constant,Ka,for a monoprotic acid (benzoic acid)is 6.3 × 10-5.Which of the following is the correct value of Kb for the benzoate ion,the conjugate base of benzoic acid?

In the reaction CaO(s)+ CO2(g)→ CaCO3(s),

Molecules or ions that can alternately behave as either a Brønsted-Lowry acid or base are called

What is the equilibrium hydronium ion concentration of an initially 4.5 M solution of hypoiodous acid,HOI,at 25°C (Ka = )?

Calculate the pH of a 1.7 M solution of H2A (Ka1 = 1.0 × 10-6 and Ka2 is 1.0 × 10-10).

Which of the following is the correct hydroxide ion concentration in 0.48 M CH3CO2-(aq)? (Kb of CH3CO2- = 5.6 × 10-10)

At 25 °C,all of the following ions produce an acidic solution,except ____.

Which one of the following aqueous solutions will have a pH of 2.00 at 25 °C? (Kw = 1.01 × 10-14)

Which of the following is true of the equilibrium constants (K,Ka,Kb)?

The complete reaction of an acid and base is as follows. HNO3(aq)+ LiOH(aq)→ H2O( )+ LiNO3(aq) What is the equilibrium constant for the net ionic reaction at 25 °C?

Given the following equilibrium constants, Ka (HSO4-)= 1.2 × 10-2 Kb (CH3CO2-)= 5.6 × 10-10 Kw = 1.00 × 10-14 determine the equilibrium constant for the reaction below at 25 °C. HSO4-(aq)+ CH3CO2-(aq) SO42-(aq)+ CH3CO2H(aq)

All of the following compounds are acids containing chlorine.Which compound is the weakest acid?

What is the pH of a 0.33 M solution of methylamine (CH3NH2,Kb = 4.4 × 10-4)at 25oC? (Kw = 1.01 × 10-14)

When a Lewis acid and a Lewis base combine,the product may be referred to as an acid-base ________.

Basic Concepts of Chemistry

Lets Review: The Tools of Quantitative Chemistry

Atoms, molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

Filters

At 50°C the autoionization constant for pure water,K_w,is .What is the H₃O⁺ concentration in pure water at 50°C?

What is the H₃O⁺ concentration in 0.0072 M NaOH(aq)at 25 °C? (K_w = 1.01 × 10^-14)

Carbonic acid is a diprotic acid,H₂CO₃,with K_a1 = 4.2 × 10^-7 and K_a2 = 4.8 × 10^-11 at 25°C.The ion product for water is K_w = 1.0 × 10^-14 at 25°C.What is the OH^- concentration of a solution that is 0.39 M in Na₂CO₃?

The equilibrium constant,K_a,for a monoprotic acid (benzoic acid)is 6.3 × 10^-5.Which of the following is the correct value of K_b for the benzoate ion,the conjugate base of benzoic acid?

In the reaction CaO(s)+ CO₂(g)→ CaCO₃(s),

What is the equilibrium hydronium ion concentration of an initially 4.5 M solution of hypoiodous acid,HOI,at 25°C (K_a = )?

Calculate the pH of a 1.7 M solution of H₂A (K_a1= 1.0 × 10^-6 and K_a2 is 1.0 × 10^-10).

Which of the following is the correct hydroxide ion concentration in 0.48 M CH₃CO₂^-(aq)? (K_b of CH₃CO₂^- = 5.6 × 10^-10)

Which one of the following aqueous solutions will have a pH of 2.00 at 25 °C? (K_w = 1.01 × 10^-14)

The complete reaction of an acid and base is as follows. HNO₃(aq)+ LiOH(aq)→ H₂O( )+ LiNO₃(aq) What is the equilibrium constant for the net ionic reaction at 25 °C?

Given the following equilibrium constants, K_a (HSO₄^-)= 1.2 × 10^-2K_b (CH₃CO₂^-)= 5.6 × 10^-10 K_w = 1.00 × 10^-14determine the equilibrium constant for the reaction below at 25 °C. HSO₄^-(aq)+ CH₃CO₂^-(aq) SO₄^2-(aq)+ CH₃CO₂H(aq)

What is the pH of a 0.33 M solution of methylamine (CH₃NH₂,K_b = 4.4 × 10^-4)at 25^oC? (K_w = 1.01 × 10^-14)