Question 1

Calculate the [H+] in a solution that has a pH of 9.88.

Accepted Answer

A) 4.1 M 
B) 9.9 M 
C) 7.6 $\times$ 10-5 M 
D) 1.3 $\times$ 10-10 M 
E) none of these 
A) 4.1 M 
B) 9.9 M 
C) 7.6 $\times$ 10-5 M 
D) 1.3 $\times$ 10-10 M 
E) none of these

Question 2

Consider the following reaction: AgBr(s)+ 2CN-(aq) \(\to\0 Ag(CN)2-(aq)+ Br-(aq)
The species that are acting as a Lewis acid and Lewis base,respectively,are

Accepted Answer

A) AgBr and Ag(CN)2- 
B) Ag(CN)2- and Ag+ 
C) Ag+ and Br- 
D) Br- and CN- 
E) Ag+ and CN- 
A) AgBr and Ag(CN)2- 
B) Ag(CN)2- and Ag+ 
C) Ag+ and Br- 
D) Br- and CN- 
E) Ag+ and CN-

Question 3

Which of the following aqueous solutions will have the highest pH? For NH3,Kb = 1.8 $\times$ 10-5;for C2H3O2-,Kb = 5.6 $\times$10-10.

Accepted Answer

A) 2.0 M NaOH 
B) 2.0 M NH3 
C) 2.0 M HC2H3O2 
D) 2.0 M HCl 
E) all the same 
A) 2.0 M NaOH 
B) 2.0 M NH3 
C) 2.0 M HC2H3O2 
D) 2.0 M HCl 
E) all the same

Question 4

If you know Kb for ammonia,NH3,you can calculate the equilibrium constant,Ka,for the following reaction: NH4+   NH3 + H+ by the equation:

Accepted Answer

A) Ka = Kw $\times$ Kb 
B) Ka = Kw / Kb 
C) Ka = 1 / Kb 
D) Ka = Kb / Kw 
E) none of these 
A) Ka = Kw $\times$ Kb 
B) Ka = Kw / Kb 
C) Ka = 1 / Kb 
D) Ka = Kb / Kw 
E) none of these

Question 5

Which of the following is a conjugate acid/base pair?

Accepted Answer

A) HCl/OCl- 
B) H2SO4/SO42- 
C) NH4+/NH3 
D) H3O+/OH- 
E) more than one of these 
A) HCl/OCl- 
B) H2SO4/SO42- 
C) NH4+/NH3 
D) H3O+/OH- 
E) more than one of these

Question 6

Calculate the Ka for an unknown monoprotic acid HX,given that a solution of 0.28 M LiX has a pH of 8.90.

Accepted Answer

A) 2.3 $\times$10-10 
B) 3.5 $\times$ 10-10 
C) 1.8 $\times$ 103 
D) 8.9 $\times$ 10-5 
E) 4.4 $\times$ 10-5 
A) 2.3 $\times$10-10 
B) 3.5 $\times$ 10-10 
C) 1.8 $\times$ 103 
D) 8.9 $\times$ 10-5 
E) 4.4 $\times$ 10-5

Question 7

Calculate the pH of the following aqueous solution: 0.52 M aniline (pKb = 9.42)

Accepted Answer

A) 4.85 
B) 4.30 
C) 9.70 
D) 9.15 
E) none of these 
A) 4.85 
B) 4.30 
C) 9.70 
D) 9.15 
E) none of these

Question 8

Which of the following would produce a basic aqueous solution?

Accepted Answer

A) P4O10 
B) KCl 
C) CO2 
D) NH4Cl 
E) none of these 
A) P4O10 
B) KCl 
C) CO2 
D) NH4Cl 
E) none of these

Question 9

In deciding which of two acids is the stronger,one must know:

Accepted Answer

A) the concentration of each acid solution 
B) the pH of each acid solution 
C) the equilibrium constant of each acid 
D) all of the above 
E) both A and C must be known 
A) the concentration of each acid solution 
B) the pH of each acid solution 
C) the equilibrium constant of each acid 
D) all of the above 
E) both A and C must be known

Calculate the [H⁺] in a solution that has a pH of 9.88.

Consider the following reaction: AgBr(s)+ 2CN^-(aq) \(\to\0 Ag(CN)₂^-(aq)+ Br^-(aq) The species that are acting as a Lewis acid and Lewis base,respectively,are

Which of the following aqueous solutions will have the highest pH? For NH₃,K_b = 1.8 $\times$ 10^-⁵;for C₂H₃O₂^-,K_b = 5.6 $\times$ 10^-¹⁰.

If you know K_b for ammonia,NH₃,you can calculate the equilibrium constant,K_a,for the following reaction: NH₄⁺ NH₃ + H⁺by the equation:

Which of the following is a conjugate acid/base pair?

Calculate the K_a for an unknown monoprotic acid HX,given that a solution of 0.28 M LiX has a pH of 8.90.

Calculate the pH of the following aqueous solution: 0.52 M aniline (pK_b = 9.42)

Which of the following would produce a basic aqueous solution?

In deciding which of two acids is the stronger,one must know:

Chemical Foundations

Atoms, molecules, and Ions

Stoichiometry

Chemical Reactions and Solutions Stoichiometry

Gases

Thermochemistry

Atomic Structure and Periodicity

Bonding: General Concepts

Covalent Bonding: Orbitals

Liquids and Solids

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Solubility and Complex Ion Equilibria

Spontaneity, entropy, and Free Energy

Electrochemistry

The Nucleus: a Chemists View

The Representative Elements

Transition Metals and Coordination Chemistry

Organic and Biological Molecules

Filters

Exam 14: Acids and Bases

Calculate the [H+] in a solution that has a pH of 9.88.

Consider the following reaction: AgBr(s)+ 2CN-(aq) \(\to\0 Ag(CN)2-(aq)+ Br-(aq) The species that are acting as a Lewis acid and Lewis base,respectively,are

Which of the following aqueous solutions will have the highest pH? For NH3,Kb = 1.8 ×\times× 10-5;for C2H3O2-,Kb = 5.6 ×\times× 10-10.

If you know Kb for ammonia,NH3,you can calculate the equilibrium constant,Ka,for the following reaction: NH4+ NH3 + H+ by the equation:

Which of the following is a conjugate acid/base pair?

Calculate the Ka for an unknown monoprotic acid HX,given that a solution of 0.28 M LiX has a pH of 8.90.

Calculate the pH of the following aqueous solution: 0.52 M aniline (pKb = 9.42)

Which of the following would produce a basic aqueous solution?

In deciding which of two acids is the stronger,one must know:

Chemical Foundations

Atoms, molecules, and Ions

Stoichiometry

Chemical Reactions and Solutions Stoichiometry

Gases

Thermochemistry

Atomic Structure and Periodicity

Bonding: General Concepts

Covalent Bonding: Orbitals

Liquids and Solids

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Solubility and Complex Ion Equilibria

Spontaneity, entropy, and Free Energy

Electrochemistry

The Nucleus: a Chemists View

The Representative Elements

Transition Metals and Coordination Chemistry

Organic and Biological Molecules

Filters

Calculate the [H⁺] in a solution that has a pH of 9.88.

Consider the following reaction: AgBr(s)+ 2CN^-(aq) \(\to\0 Ag(CN)₂^-(aq)+ Br^-(aq) The species that are acting as a Lewis acid and Lewis base,respectively,are

Which of the following aqueous solutions will have the highest pH? For NH₃,K_b = 1.8 $\times$ 10^-⁵;for C₂H₃O₂^-,K_b = 5.6 $\times$ 10^-¹⁰.

If you know K_b for ammonia,NH₃,you can calculate the equilibrium constant,K_a,for the following reaction: NH₄⁺ NH₃ + H⁺by the equation:

Calculate the K_a for an unknown monoprotic acid HX,given that a solution of 0.28 M LiX has a pH of 8.90.

Calculate the pH of the following aqueous solution: 0.52 M aniline (pK_b = 9.42)