Question 1

Which pair is not a conjugate acid-base pair?

Accepted Answer

A) (CH3)3N;(CH3)3NH+ 
B) H2SO4;H2SO3 
C) HNO2;NO2- 
D) H3O+;H2O 
A) (CH3)3N;(CH3)3NH+ 
B) H2SO4;H2SO3 
C) HNO2;NO2- 
D) H3O+;H2O

Question 2

Determine the pOH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 × 10-5.

Accepted Answer

A) 2.26 
B) 4.52 
C) 11.74 
D) 9.48 
E) 5.48 
A) 2.26 
B) 4.52 
C) 11.74 
D) 9.48 
E) 5.48

Question 3

In a triprotic acid,which Ka has the highest value?

Accepted Answer

A) Ka1 
B) Ka2 
C) Ka3 
D) Kb1 
E) Kb2 
A) Ka1 
B) Ka2 
C) Ka3 
D) Kb1 
E) Kb2

Question 4

Which solution is least acidic? (HCl is a strong acid and Ka for HF = 3.5 × 10-4)

Accepted Answer

A) 0.1 M HCl 
B) 0.01 M HCl 
C) 0.1 M HF 
D) 0.01 M HF 
A) 0.1 M HCl 
B) 0.01 M HCl 
C) 0.1 M HF 
D) 0.01 M HF

Question 5

Calculate the hydronium ion concentration in an aqueous solution with a pH of 9.85 at 25°C.

Accepted Answer

A) 7.1 × 10-5 M 
B) 4.2 × 10-10 M 
C) 8.7 × 10-10 M 
D) 6.5 × 10-5 M 
E) 1.4 × 10-10 M 
A) 7.1 × 10-5 M 
B) 4.2 × 10-10 M 
C) 8.7 × 10-10 M 
D) 6.5 × 10-5 M 
E) 1.4 × 10-10 M

Question 6

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

Accepted Answer

A) RbI 
B) RbBr 
C) RbCl 
D) RbF 
A) RbI 
B) RbBr 
C) RbCl 
D) RbF

Question 7

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

Accepted Answer

A) NaCl 
B) KCl 
C) MgCl2 
D) AlCl3 
A) NaCl 
B) KCl 
C) MgCl2 
D) AlCl3

Question 8

Determine the Kb for CN⁻ at 25°C.The Ka for HCN is 4.9 × 10-10.

Accepted Answer

A) 4.9 × 10-14 
B) 2.3 × 10-9 
C) 1.4 × 10-5 
D) 2.0 × 10-5 
E) 3.7 × 10-7 
A) 4.9 × 10-14 
B) 2.3 × 10-9 
C) 1.4 × 10-5 
D) 2.0 × 10-5 
E) 3.7 × 10-7

Question 9

Which of the following is a strong base?

Accepted Answer

A) Cl- 
B) NH3 
C) CH3OH 
D) NO3⁻ 
E) KOH 
A) Cl- 
B) NH3 
C) CH3OH 
D) NO3⁻ 
E) KOH

Question 10

Which of the following is a Lewis base?

Accepted Answer

A) AlF3 
B) H2O 
C) SiF4 
D) C5H12 
E) None of the above are Lewis bases. 
A) AlF3 
B) H2O 
C) SiF4 
D) C5H12 
E) None of the above are Lewis bases.

Question 11

What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of 1.50 × 10-2 M?

Accepted Answer

A) 6.67 × 10-12 M,2.82 
B) 6.67 × 10-12 M,11.18 
C) 6.67 × 10-13 M,1.82 
D) 6.67 × 10-13 M,12.17 
A) 6.67 × 10-12 M,2.82 
B) 6.67 × 10-12 M,11.18 
C) 6.67 × 10-13 M,1.82 
D) 6.67 × 10-13 M,12.17

Question 12

What is the difference between a strong and weak acid?

Accepted Answer

A strong acid ionizes/dissocia

Question 13

Determine the pH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 × 10-5.

Accepted Answer

A) 2.26 
B) 4.52 
C) 11.74 
D) 9.48 
E) 5.48 
A) 2.26 
B) 4.52 
C) 11.74 
D) 9.48 
E) 5.48

Question 14

Which of the following is an Arrhenius base?

Accepted Answer

A) CH3CO2H 
B) NaOH 
C) CH3OH 
D) LiCl 
E) More than one of these compounds is an Arrhenius base. 
A) CH3CO2H 
B) NaOH 
C) CH3OH 
D) LiCl 
E) More than one of these compounds is an Arrhenius base.

Question 15

Which is the definition of Lewis base? A Lewis acid is ________.

Accepted Answer

A) an electron pair donor 
B) an electron pair acceptor 
C) a proton donor 
D) proton acceptor 
A) an electron pair donor 
B) an electron pair acceptor 
C) a proton donor 
D) proton acceptor

Question 16

What is the concentration of hydroxide ions in pure water at 30.0∘C,if Kw at this temperature is
1.47 × 10-14?

Accepted Answer

A) 1.00 × 10-7 M 
B) 1.30 × 10-7 M 
C) 1.47 × 10-7 M 
D) 8.93 × 10-8 M 
E) 1.21 × 10-7 M 
A) 1.00 × 10-7 M 
B) 1.30 × 10-7 M 
C) 1.47 × 10-7 M 
D) 8.93 × 10-8 M 
E) 1.21 × 10-7 M

Question 17

Which of the following is a weak acid?

Accepted Answer

A) HClO4 
B) H2SO4 
C) HCl 
D) HCO2H 
E) HNO3 
A) HClO4 
B) H2SO4 
C) HCl 
D) HCO2H 
E) HNO3

Question 18

Calculate the pH of a 0.800 M NaCH3CO2 solution.Ka for acetic acid,CH3CO2H,is 1.8 × 10-5.

Accepted Answer

A) 2.42 
B) 4.68 
C) 9.32 
D) 11.58 
A) 2.42 
B) 4.68 
C) 9.32 
D) 11.58

Question 19

Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 5.00.

Accepted Answer

A) 1.0 × 10-5 
B) 9.00 
C) 1.0 × 10-9 
D) 5.0 × 10-14 
E) 9.0 × 10-14 
A) 1.0 × 10-5 
B) 9.00 
C) 1.0 × 10-9 
D) 5.0 × 10-14 
E) 9.0 × 10-14

Question 20

The base-dissociation constant of ethylamine (C2H5NH2)is 6.4 × 10-4 at 25.0°C.The [H+] in a
1.6 × 10-2 M solution of ethylamine is ________ M.

Accepted Answer

A) 3.5 × 10-12 
B) 2.9 × 10-3 
C) 3.1 × 10-12 
D) 3.2 × 10-3 
E) 11.46 
A) 3.5 × 10-12 
B) 2.9 × 10-3 
C) 3.1 × 10-12 
D) 3.2 × 10-3 
E) 11.46

Which pair is not a conjugate acid-base pair?

Determine the pOH of a 0.461 M C₆H₅CO₂H M solution if the K_a of C₆H₅CO₂H is 6.5 × 10^-5.

In a triprotic acid,which K_a has the highest value?

Which solution is least acidic? (HCl is a strong acid and K_a for HF = 3.5 × 10^-4)

Calculate the hydronium ion concentration in an aqueous solution with a pH of 9.85 at 25°C.

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

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

Determine the K_b for CN⁻ at 25°C.The K_a for HCN is 4.9 × 10^-10.

Which of the following is a strong base?

Which of the following is a Lewis base?

What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of 1.50 × 10^-² M?

What is the difference between a strong and weak acid?

Determine the pH of a 0.461 M C₆H₅CO₂H M solution if the K_a of C₆H₅CO₂H is 6.5 × 10^-5.

Which of the following is an Arrhenius base?

Which is the definition of Lewis base? A Lewis acid is ________.

What is the concentration of hydroxide ions in pure water at 30.0^∘C,if K_w at this temperature is 1.47 × 10^-14?

Which of the following is a weak acid?

Calculate the pH of a 0.800 M NaCH₃CO₂ solution.K_a for acetic acid,CH₃CO₂H,is 1.8 × 10^-5.

Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 5.00.

The base-dissociation constant of ethylamine (C₂H₅NH₂)is 6.4 × 10^-⁴ at 25.0°C.The [H⁺] in a 1.6 × 10^-² M solution of ethylamine is ________ M.

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Filters

Exam 15: Acids and Bases

Which pair is not a conjugate acid-base pair?

Determine the pOH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 × 10-5.

In a triprotic acid,which Ka has the highest value?

Which solution is least acidic? (HCl is a strong acid and Ka for HF = 3.5 × 10-4)

Calculate the hydronium ion concentration in an aqueous solution with a pH of 9.85 at 25°C.

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

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

Determine the Kb for CN⁻ at 25°C.The Ka for HCN is 4.9 × 10-10.

Which of the following is a strong base?

Which of the following is a Lewis base?

What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of 1.50 × 10-2 M?

What is the difference between a strong and weak acid?

Determine the pH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 × 10-5.

Which of the following is an Arrhenius base?

Which is the definition of Lewis base? A Lewis acid is ________.

What is the concentration of hydroxide ions in pure water at 30.0∘C,if Kw at this temperature is 1.47 × 10-14?

Which of the following is a weak acid?

Calculate the pH of a 0.800 M NaCH3CO2 solution.Ka for acetic acid,CH3CO2H,is 1.8 × 10-5.

Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 5.00.

The base-dissociation constant of ethylamine (C2H5NH2)is 6.4 × 10-4 at 25.0°C.The [H+] in a 1.6 × 10-2 M solution of ethylamine is ________ M.

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Filters

Determine the pOH of a 0.461 M C₆H₅CO₂H M solution if the K_a of C₆H₅CO₂H is 6.5 × 10^-5.

In a triprotic acid,which K_a has the highest value?

Which solution is least acidic? (HCl is a strong acid and K_a for HF = 3.5 × 10^-4)

Determine the K_b for CN⁻ at 25°C.The K_a for HCN is 4.9 × 10^-10.

What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of 1.50 × 10^-² M?

Determine the pH of a 0.461 M C₆H₅CO₂H M solution if the K_a of C₆H₅CO₂H is 6.5 × 10^-5.

What is the concentration of hydroxide ions in pure water at 30.0^∘C,if K_w at this temperature is 1.47 × 10^-14?

Calculate the pH of a 0.800 M NaCH₃CO₂ solution.K_a for acetic acid,CH₃CO₂H,is 1.8 × 10^-5.

The base-dissociation constant of ethylamine (C₂H₅NH₂)is 6.4 × 10^-⁴ at 25.0°C.The [H⁺] in a 1.6 × 10^-² M solution of ethylamine is ________ M.