Question 1

What is the pH of pure water at 40.0°C if the Kw at this temperature is 2.92 × 10-14?

Accepted Answer

A) 6.767 
B) 0.465 
C) 7.000 
D) 7.233 
E) 8.446 
A) 6.767 
B) 0.465 
C) 7.000 
D) 7.233 
E) 8.446

Question 2

Identify the strongest acid.

Accepted Answer

A) HClO4 
B) HClO3 
C) HClO2 
D) HClO 
E) Not enough information is given. 
A) HClO4 
B) HClO3 
C) HClO2 
D) HClO 
E) Not enough information is given.

Question 3

Identify the weak diprotic acid.

Accepted Answer

A) HNO3 
B) H3PO4 
C) H2SO3 
D) HClO4 
E) H2SO4 
A) HNO3 
B) H3PO4 
C) H2SO3 
D) HClO4 
E) H2SO4

Question 4

What is the hydronium ion concentration of an acid rain sample that has a pH of 3.45?

Accepted Answer

A) 2.82 × 10-11 M 
B) 3.55 × 10-4 M 
C) 3.45 M 
D) 10.55 M 
A) 2.82 × 10-11 M 
B) 3.55 × 10-4 M 
C) 3.45 M 
D) 10.55 M

Question 5

How many of the following are weak acids?
HCN HClO2 HNO3 H2PO4⁻

Accepted Answer

A) 0 
B) 1 
C) 3 
D) 4 
E) 2 
A) 0 
B) 1 
C) 3 
D) 4 
E) 2

Question 6

What is the hydronium ion concentration and the pH for an aqueous solution of NH3 that has a hydroxide ion concentration of 2.25 × 10-2 M?

Accepted Answer

A) 4.44 × 10-12 M and 2.65 
B) 4.44 × 10-12 M and 11.35 
C) 4.44 × 10-13 M and 1.65 
D) 4.44 × 10-13 M and 12.35 
A) 4.44 × 10-12 M and 2.65 
B) 4.44 × 10-12 M and 11.35 
C) 4.44 × 10-13 M and 1.65 
D) 4.44 × 10-13 M and 12.35

Question 7

Find the percent ionization of a 0.337 M HF solution.The Ka for HF is 3.5 × 10-4.

Accepted Answer

A) 1.1% 
B) 1.2 × 10-2% 
C) 3.2% 
D) 3.5 × 10-2% 
E) 4.7% 
A) 1.1% 
B) 1.2 × 10-2% 
C) 3.2% 
D) 3.5 × 10-2% 
E) 4.7%

Question 8

Calculate the pH of a solution that contains 2.4 × 10-5 M H3O⁺ at 25°C.

Accepted Answer

A) 2.40 
B) 9.38 
C) 4.62 
D) 11.60 
E) 4.17 
A) 2.40 
B) 9.38 
C) 4.62 
D) 11.60 
E) 4.17

Question 9

Describe the relationship between molecular structure and acid strength.

Accepted Answer

1)The stronger the bond between a hydrog

Question 10

Determine the Ka for CH3NH3⁺ at 25°C.The Kb for CH3NH2 is 4.4 × 10-4.

Accepted Answer

A) 3.1 × 10-10 
B) 6.8 × 10-11 
C) 5.6 × 10-10 
D) 2.3 × 10-3 
E) 2.3 × 10-11 
A) 3.1 × 10-10 
B) 6.8 × 10-11 
C) 5.6 × 10-10 
D) 2.3 × 10-3 
E) 2.3 × 10-11

Question 11

Match the following.
-Lewis acid

Accepted Answer

A) electron pair donor 
B) proton donor 
C) produces protons in aqueous solution 
D) produces hydroxide ions in aqueous solution 
E) electron pair acceptor
F)proton acceptor 
A) electron pair donor 
B) proton donor 
C) produces protons in aqueous solution 
D) produces hydroxide ions in aqueous solution 
E) electron pair acceptor
F)proton acceptor

Question 12

Place the following in order of increasing acid strength.
HBrO2 HBrO3 HBrO HBrO4

Accepted Answer

A) HBrO2 4 3 
B) HBrO 2 3 4 
C) HBrO2 3 4 4 2 3 4 3 2 
A) HBrO2 4 3 
B) HBrO 2 3 4 
C) HBrO2 3 4 4 2 3 4 3 2

Question 13

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

Accepted Answer

A) NH4+ 
B) CCl4 
C) NH2- 
D) NH3 
E) Br2 
A) NH4+ 
B) CCl4 
C) NH2- 
D) NH3 
E) Br2

Question 14

The stronger the acid,then which of the following is true?

Accepted Answer

A) The stronger the conjugate acid. 
B) The stronger the conjugate base. 
C) The weaker the conjugate base. 
D) The weaker the conjugate acid. 
E) None of the above. 
A) The stronger the conjugate acid. 
B) The stronger the conjugate base. 
C) The weaker the conjugate base. 
D) The weaker the conjugate acid. 
E) None of the above.

Question 15

Calculate the concentration of H3O⁺ in a solution that contains 5.5 × 10-5 M OH⁻ at 25°C.Identify the solution as acidic,basic or neutral.

Accepted Answer

A) 1.8 × 10-10 M,basic 
B) 1.8 × 10-10 M,acidic 
C) 5.5 × 10-10 M,neutral 
D) 9.2 × 10-1 M,acidic 
E) 9.2 × 10-1 M,basic 
A) 1.8 × 10-10 M,basic 
B) 1.8 × 10-10 M,acidic 
C) 5.5 × 10-10 M,neutral 
D) 9.2 × 10-1 M,acidic 
E) 9.2 × 10-1 M,basic

Question 16

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

Accepted Answer

A) KHCO3 
B) CsClO4 
C) RaO 
D) CH3CH3NH3Cl 
A) KHCO3 
B) CsClO4 
C) RaO 
D) CH3CH3NH3Cl

Question 17

A solution with a hydrogen ion concentration of 3.25 × 10-6 M is ________ and has a hydroxide ion concentration of ________.

Accepted Answer

A) acidic,3.08 × 10-8 M 
B) acidic,3.08 × 10-9 M 
C) basic,3.08 × 10-8 M 
D) basic,3.08 × 10-9 M 
A) acidic,3.08 × 10-8 M 
B) acidic,3.08 × 10-9 M 
C) basic,3.08 × 10-8 M 
D) basic,3.08 × 10-9 M

Question 18

Calculate the pH for an aqueous solution of acetic acid that contains 2.15 × 10-3 M hydronium ion.

Accepted Answer

A) 4.65 × 10-12 M 
B) 2.15 × 10-3 M 
C) 2.67 
D) 11.33 
A) 4.65 × 10-12 M 
B) 2.15 × 10-3 M 
C) 2.67 
D) 11.33

Question 19

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

Accepted Answer

A) HF,3.5 × 10-4 
B) HCN,4.9 × 10-10 
C) HNO2,4.6 × 10-4 
D) HCHO2,1.8 × 10-4 
E) HClO2,1.1 × 10-2 
A) HF,3.5 × 10-4 
B) HCN,4.9 × 10-10 
C) HNO2,4.6 × 10-4 
D) HCHO2,1.8 × 10-4 
E) HClO2,1.1 × 10-2

Question 20

Which one of the following will form an acidic solution in water?

Accepted Answer

A) NH4Cl 
B) NaF 
C) LiI 
D) KNO3 
E) None of the above solutions will be acidic. 
A) NH4Cl 
B) NaF 
C) LiI 
D) KNO3 
E) None of the above solutions will be acidic.

What is the pH of pure water at 40.0°C if the K_w at this temperature is 2.92 × 10^-14?

Identify the strongest acid.

Identify the weak diprotic acid.

What is the hydronium ion concentration of an acid rain sample that has a pH of 3.45?

How many of the following are weak acids? HCN HClO₂HNO₃ H₂PO₄^⁻

What is the hydronium ion concentration and the pH for an aqueous solution of NH₃ that has a hydroxide ion concentration of 2.25 × 10^-² M?

Find the percent ionization of a 0.337 M HF solution.The K_a for HF is 3.5 × 10^-4.

Calculate the pH of a solution that contains 2.4 × 10^-5 M H₃O^⁺ at 25°C.

Describe the relationship between molecular structure and acid strength.

Determine the K_a for CH₃NH₃^⁺at 25°C.The K_b for CH₃NH₂ is 4.4 × 10^-4.

Match the following. -Lewis acid

Place the following in order of increasing acid strength. HBrO₂ HBrO₃ HBrO HBrO₄

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

The stronger the acid,then which of the following is true?

Calculate the concentration of H₃O^⁺ in a solution that contains 5.5 × 10^-5 M OH^⁻ at 25°C.Identify the solution as acidic,basic or neutral.

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

A solution with a hydrogen ion concentration of 3.25 × 10^-6 M is and has a hydroxide ion concentration of .

Calculate the pH for an aqueous solution of acetic acid that contains 2.15 × 10^-³ M hydronium ion.

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

Which one of the following will form an acidic solution in water?

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

What is the pH of pure water at 40.0°C if the Kw at this temperature is 2.92 × 10-14?

Identify the strongest acid.

Identify the weak diprotic acid.

What is the hydronium ion concentration of an acid rain sample that has a pH of 3.45?

How many of the following are weak acids? HCN HClO2 HNO3 H2PO4⁻

What is the hydronium ion concentration and the pH for an aqueous solution of NH3 that has a hydroxide ion concentration of 2.25 × 10-2 M?

Find the percent ionization of a 0.337 M HF solution.The Ka for HF is 3.5 × 10-4.

Calculate the pH of a solution that contains 2.4 × 10-5 M H3O⁺ at 25°C.

Describe the relationship between molecular structure and acid strength.

Determine the Ka for CH3NH3⁺ at 25°C.The Kb for CH3NH2 is 4.4 × 10-4.

Match the following. -Lewis acid

Place the following in order of increasing acid strength. HBrO2 HBrO3 HBrO HBrO4

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

The stronger the acid,then which of the following is true?

Calculate the concentration of H3O⁺ in a solution that contains 5.5 × 10-5 M OH⁻ at 25°C.Identify the solution as acidic,basic or neutral.

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

A solution with a hydrogen ion concentration of 3.25 × 10-6 M is ________ and has a hydroxide ion concentration of ________.

Calculate the pH for an aqueous solution of acetic acid that contains 2.15 × 10-3 M hydronium ion.

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

Which one of the following will form an acidic solution in water?

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

What is the pH of pure water at 40.0°C if the K_w at this temperature is 2.92 × 10^-14?

How many of the following are weak acids? HCN HClO₂HNO₃ H₂PO₄^⁻

What is the hydronium ion concentration and the pH for an aqueous solution of NH₃ that has a hydroxide ion concentration of 2.25 × 10^-² M?

Find the percent ionization of a 0.337 M HF solution.The K_a for HF is 3.5 × 10^-4.

Calculate the pH of a solution that contains 2.4 × 10^-5 M H₃O^⁺ at 25°C.

Determine the K_a for CH₃NH₃^⁺at 25°C.The K_b for CH₃NH₂ is 4.4 × 10^-4.

Place the following in order of increasing acid strength. HBrO₂ HBrO₃ HBrO HBrO₄

Calculate the concentration of H₃O^⁺ in a solution that contains 5.5 × 10^-5 M OH^⁻ at 25°C.Identify the solution as acidic,basic or neutral.

A solution with a hydrogen ion concentration of 3.25 × 10^-6 M is and has a hydroxide ion concentration of .

Calculate the pH for an aqueous solution of acetic acid that contains 2.15 × 10^-³ M hydronium ion.

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