Question 1

Calculate the concentration of OH⁻ in a solution that contains 3.9 × 10-4 M H3O⁺ at 25°C.Identify the solution as acidic,basic or neutral.

Accepted Answer

A) 2.6 × 10-11 M,acidic 
B) 2.6 × 10-11 M,basic 
C) 3.9 × 10-4 M,neutral 
D) 2.7 × 10-2 M,basic 
E) 2.7 × 10-2 M,acidic 
A) 2.6 × 10-11 M,acidic 
B) 2.6 × 10-11 M,basic 
C) 3.9 × 10-4 M,neutral 
D) 2.7 × 10-2 M,basic 
E) 2.7 × 10-2 M,acidic A

Question 2

Calculate the pH of a 1.60 M CH3NH3Cl solution.Kb for methylamine,CH3NH2,is 3.7 × 10-4.

Accepted Answer

A) 1.61 
B) 5.18 
C) 8.82 
D) 12.39 
A) 1.61 
B) 5.18 
C) 8.82 
D) 12.39 B

Question 3

What is the pH of a 0.020 M HClO4 solution?

Accepted Answer

A) 0.020 
B) 0.040 
C) 1.70 
D) 12.30 
A) 0.020 
B) 0.040 
C) 1.70 
D) 12.30 C

Question 4

Which of the following acids is the weakest? The acid is followed by its Ka value.

Accepted Answer

A) HC2H3O2,1.8 × 10-5 
B) HIO,2.3 × 10-11 
C) HBrO,2.3 × 10-9 
D) HClO,2.9 × 10-8 
E) C6H5CO2H,6.3 × 10-5 
A) HC2H3O2,1.8 × 10-5 
B) HIO,2.3 × 10-11 
C) HBrO,2.3 × 10-9 
D) HClO,2.9 × 10-8 
E) C6H5CO2H,6.3 × 10-5

Question 5

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:
NH3(aq)+ H2O(l)⇌ NH4+(aq)+ OH-(aq)

Accepted Answer

A) 3.0 M 
B) 0.056 M 
C) 1.8 × 10-2 M 
D) 1.0 × 10-3 M 
A) 3.0 M 
B) 0.056 M 
C) 1.8 × 10-2 M 
D) 1.0 × 10-3 M

Question 6

Which will be the most predominant species in a 0.1 CH3COOH solution in water? (Ka = 1.8 × 10-5)

Accepted Answer

A) H3O+ ions 
B) CH3COO- ions 
C) CH3COOH molecules 
D) all of the above 
A) H3O+ ions 
B) CH3COO- ions 
C) CH3COOH molecules 
D) all of the above

Question 7

Calculate the pH of a 1.60 M KBrO solution.Ka for hypobromous acid,HBrO,is 2.0 × 10-9.

Accepted Answer

A) 2.55 
B) 4.25 
C) 9.75 
D) 11.45 
A) 2.55 
B) 4.25 
C) 9.75 
D) 11.45

Question 8

Determine the [OH⁻] concentration in a 0.235 M NaOH solution.

Accepted Answer

A) 4.25 × 10-14 M 
B) 0.470 M 
C) 2.13 × 10-14 M 
D) 0.198 M 
E) 0.235 M 
A) 4.25 × 10-14 M 
B) 0.470 M 
C) 2.13 × 10-14 M 
D) 0.198 M 
E) 0.235 M

Question 9

Which of the following is a Br∅nsted-Lowry acid?

Accepted Answer

A) NH4+ 
B) CH4 
C) NH2- 
D) NH3 
E) Br2 
A) NH4+ 
B) CH4 
C) NH2- 
D) NH3 
E) Br2

Question 10

What does the term amphoteric mean?

Accepted Answer

A substance is ampho

Question 11

Define a Lewis acid.

Accepted Answer

A Lewis ac

Question 12

Calculate the pOH of a solution that contains 3.9 × 10-5 M H3O⁺ at 25°C.

Accepted Answer

A) 5.41 
B) 4.41 
C) 9.59 
D) 8.59 
E) 0.59 
A) 5.41 
B) 4.41 
C) 9.59 
D) 8.59 
E) 0.59

Question 13

Which of the following bases is the strongest? The base is followed by its Kb.

Accepted Answer

A) (CH3CH2)2NH,8.6 × 10-4 
B) CH3NH2,4.4 × 10-4 
C) C6H5NH2,4.0 × 10-10 
D) NH3,1.76 × 10-5 
E) C5H5N,1.7 × 10-9 
A) (CH3CH2)2NH,8.6 × 10-4 
B) CH3NH2,4.4 × 10-4 
C) C6H5NH2,4.0 × 10-10 
D) NH3,1.76 × 10-5 
E) C5H5N,1.7 × 10-9

Question 14

What is the conjugate acid of HCO3⁻?

Accepted Answer

A) H3O+ 
B) H2O 
C) CO32- 
D) OH⁻ 
E) H2CO3 
A) H3O+ 
B) H2O 
C) CO32- 
D) OH⁻ 
E) H2CO3

Question 15

Which of the following is a Br∅nsted-Lowry base?

Accepted Answer

A) CH4 
B) HCN 
C) NH3 
D) Cl2 
E) None of the above are Br∅nsted-Lowry bases. 
A) CH4 
B) HCN 
C) NH3 
D) Cl2 
E) None of the above are Br∅nsted-Lowry bases.

Question 16

The pOH of pure water at 40oC is 6.8.What is the hydronium ion concentration in pure water [H3O+] at this temperature?

Accepted Answer

A) 6.3 × 10-8 
B) 1 × 10-14 
C) 1.0 × 10-7 
D) 1.6 × 10-7 
A) 6.3 × 10-8 
B) 1 × 10-14 
C) 1.0 × 10-7 
D) 1.6 × 10-7

Question 17

Which of the following species is amphoteric?

Accepted Answer

A) CO32- 
B) HF 
C) NH4⁺ 
D) HPO42- 
E) None of the above are amphoteric. 
A) CO32- 
B) HF 
C) NH4⁺ 
D) HPO42- 
E) None of the above are amphoteric.

Question 18

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

Accepted Answer

A) 4.00 × 10-7 M 
B) 4.00 × 10-8 M 
C) 4.00 × 10-9 M 
D) 5.00 × 10-9 M 
A) 4.00 × 10-7 M 
B) 4.00 × 10-8 M 
C) 4.00 × 10-9 M 
D) 5.00 × 10-9 M

Question 19

Which Br∅nsted-Lowry acid is not considered to be a strong acid in water?

Accepted Answer

A) HI 
B) HBr  
C) H2SO3 
D) H NO3 
A) HI 
B) HBr  
C) H2SO3 
D) H NO3

Question 20

What is the hydronium ion concentration of a 0.150 M hypochlorous acid solution with
Ka = 3.5 × 10-8? The equation for the dissociation of hypochlorous acid is:
HOCl(aq)+ H2O(l)⇌ H3O+(aq)+ OCl-(aq)

Accepted Answer

A) 1.9 × 10-4 M 
B) 7.2 × 10-4 M 
C) 2.8 × 10-5 M 
D) 7.2 × 10-5 M 
A) 1.9 × 10-4 M 
B) 7.2 × 10-4 M 
C) 2.8 × 10-5 M 
D) 7.2 × 10-5 M

Calculate the concentration of OH^⁻ in a solution that contains 3.9 × 10^-4 M H₃O⁺ at 25°C.Identify the solution as acidic,basic or neutral.

Calculate the pH of a 1.60 M CH₃NH₃Cl solution.K_b for methylamine,CH₃NH₂,is 3.7 × 10^-4.

What is the pH of a 0.020 M HClO₄ solution?

Which of the following acids is the weakest? The acid is followed by its K_a value.

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: NH₃(aq)+ H₂O(l)⇌ NH₄⁺(aq)+ OH^-(aq)

Which will be the most predominant species in a 0.1 CH₃COOH solution in water? (K_a = 1.8 × 10^-5)

Calculate the pH of a 1.60 M KBrO solution.K_a for hypobromous acid,HBrO,is 2.0 × 10^-⁹.

Determine the [OH⁻] concentration in a 0.235 M NaOH solution.

Which of the following is a Br∅nsted-Lowry acid?

What does the term amphoteric mean?

Define a Lewis acid.

Calculate the pOH of a solution that contains 3.9 × 10^-5 M H₃O⁺ at 25°C.

Which of the following bases is the strongest? The base is followed by its K_b.

What is the conjugate acid of HCO₃^⁻?

Which of the following is a Br∅nsted-Lowry base?

The pOH of pure water at 40^oC is 6.8.What is the hydronium ion concentration in pure water [H₃O⁺] at this temperature?

Which of the following species is amphoteric?

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

Which Br∅nsted-Lowry acid is not considered to be a strong acid in water?

What is the hydronium ion concentration of a 0.150 M hypochlorous acid solution with K_a = 3.5 × 10^-8? The equation for the dissociation of hypochlorous acid is: HOCl(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ OCl^-(aq)

Matter, Measurement, and Problem Solving

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Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

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Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

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

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Filters

Exam 15: Acids and Bases

Calculate the concentration of OH⁻ in a solution that contains 3.9 × 10-4 M H3O⁺ at 25°C.Identify the solution as acidic,basic or neutral.

Calculate the pH of a 1.60 M CH3NH3Cl solution.Kb for methylamine,CH3NH2,is 3.7 × 10-4.

What is the pH of a 0.020 M HClO4 solution?

Which of the following acids is the weakest? The acid is followed by its Ka value.

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: NH3(aq)+ H2O(l)⇌ NH4+(aq)+ OH-(aq)

Which will be the most predominant species in a 0.1 CH3COOH solution in water? (Ka = 1.8 × 10-5)

Calculate the pH of a 1.60 M KBrO solution.Ka for hypobromous acid,HBrO,is 2.0 × 10-9.

Determine the [OH⁻] concentration in a 0.235 M NaOH solution.

Which of the following is a Br∅nsted-Lowry acid?

What does the term amphoteric mean?

Define a Lewis acid.

Calculate the pOH of a solution that contains 3.9 × 10-5 M H3O⁺ at 25°C.

Which of the following bases is the strongest? The base is followed by its Kb.

What is the conjugate acid of HCO3⁻?

Which of the following is a Br∅nsted-Lowry base?

The pOH of pure water at 40oC is 6.8.What is the hydronium ion concentration in pure water [H3O+] at this temperature?

Which of the following species is amphoteric?

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

Which Br∅nsted-Lowry acid is not considered to be a strong acid in water?

What is the hydronium ion concentration of a 0.150 M hypochlorous acid solution with Ka = 3.5 × 10-8? The equation for the dissociation of hypochlorous acid is: HOCl(aq)+ H2O(l)⇌ H3O+(aq)+ OCl-(aq)

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

Calculate the concentration of OH^⁻ in a solution that contains 3.9 × 10^-4 M H₃O⁺ at 25°C.Identify the solution as acidic,basic or neutral.

Calculate the pH of a 1.60 M CH₃NH₃Cl solution.K_b for methylamine,CH₃NH₂,is 3.7 × 10^-4.

What is the pH of a 0.020 M HClO₄ solution?

Which of the following acids is the weakest? The acid is followed by its K_a value.

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: NH₃(aq)+ H₂O(l)⇌ NH₄⁺(aq)+ OH^-(aq)

Which will be the most predominant species in a 0.1 CH₃COOH solution in water? (K_a = 1.8 × 10^-5)

Calculate the pH of a 1.60 M KBrO solution.K_a for hypobromous acid,HBrO,is 2.0 × 10^-⁹.

Calculate the pOH of a solution that contains 3.9 × 10^-5 M H₃O⁺ at 25°C.

Which of the following bases is the strongest? The base is followed by its K_b.

What is the conjugate acid of HCO₃^⁻?

The pOH of pure water at 40^oC is 6.8.What is the hydronium ion concentration in pure water [H₃O⁺] at this temperature?

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

What is the hydronium ion concentration of a 0.150 M hypochlorous acid solution with K_a = 3.5 × 10^-8? The equation for the dissociation of hypochlorous acid is: HOCl(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ OCl^-(aq)