Question 1

What is the Kw of pure water at 50.0 °C,if the pH is 6.630?

Accepted Answer

A) 2.34 × 10-7 
B) 5.50 × 10-14 
C) 2.13 × 10-14 
D) 1.00 × 10-14 
E) 2.34 × 10-14 
A) 2.34 × 10-7 
B) 5.50 × 10-14 
C) 2.13 × 10-14 
D) 1.00 × 10-14 
E) 2.34 × 10-14

Question 2

Determine the pH of a 0.62 mol L-1 NH4NO3 solution at 25 °C.The Kb for NH3 is 1.76 × 10-5.

Accepted Answer

A) 2.48 
B) 9.27 
C) 11.52 
D) 4.73 
E) 9.45 
A) 2.48 
B) 9.27 
C) 11.52 
D) 4.73 
E) 9.45

Question 3

Calculate the pOH of a solution that contains 2.4 × 10-5 mol L-1 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 4

Identify acid,base,conjugate acid,and conjugate base in the following reaction: 
H2CO3(aq)+ H2O(l)⇌ HCO3-(aq)+ H3O+(aq)

Accepted Answer

A) H2CO3 is an acid,H2O is a base,HCO3- is a conjugate base,and H3O+ is a conjugate acid. 
B) H2CO3 is a conjugate acid,H2O is a conjugate base,HCO3- is a base,and H3O+ is an acid. 
C) H2CO3 is an acid,H2O is a conjugate base,HCO3- is a base,and H3O+ is a conjugate acid. 
D) H2CO3 is a conjugate acid,H2O is a base,HCO3- is a conjugate base,and H3O+ is an acid. 
E) H2CO3 is an acid,H2O is a conjugate acid,HCO3- is a base,and H3O+ is a conjugate base. 
A) H2CO3 is an acid,H2O is a base,HCO3- is a conjugate base,and H3O+ is a conjugate acid. 
B) H2CO3 is a conjugate acid,H2O is a conjugate base,HCO3- is a base,and H3O+ is an acid. 
C) H2CO3 is an acid,H2O is a conjugate base,HCO3- is a base,and H3O+ is a conjugate acid. 
D) H2CO3 is a conjugate acid,H2O is a base,HCO3- is a conjugate base,and H3O+ is an acid. 
E) H2CO3 is an acid,H2O is a conjugate acid,HCO3- is a base,and H3O+ is a conjugate base.

Question 5

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

Accepted Answer

A) CH3COOH,1.8 × 10-5 
B) HIO,2.3 × 10-11 
C) HBrO,2.3 × 10-9 
D) HClO,2.9 × 10-8 
E) C6H5COOH,6.3 × 10-5 
A) CH3COOH,1.8 × 10-5 
B) HIO,2.3 × 10-11 
C) HBrO,2.3 × 10-9 
D) HClO,2.9 × 10-8 
E) C6H5COOH,6.3 × 10-5

Question 6

Calculate the pH of a 0.800 mol L-1 NaCH3CO2 solution.Ka for acetic acid,CH3CO2H,is $1.8 \times 10 ^- 5$

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 7

Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10-4 mol L-1 in hydronium ion.

Accepted Answer

A) 2.86 × 10-3 mol L-1 
B) 2.86 × 10-10 mol L-1 
C) 2.86 × 10-11 mol L-1 
D) 3.50 × 10-11 mol L-1 
A) 2.86 × 10-3 mol L-1 
B) 2.86 × 10-10 mol L-1 
C) 2.86 × 10-11 mol L-1 
D) 3.50 × 10-11 mol L-1

Question 8

What is the pH of a 0.040 mol L-1 Ba(OH)2 solution?

Accepted Answer

A) 1.10 
B) 1.40 
C) 12.60 
D) 12.90 
A) 1.10 
B) 1.40 
C) 12.60 
D) 12.90

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

Determine the pOH of a 0.116 mol L-1 Ba(OH)2 solution at 25 °C.

Accepted Answer

A) 8.62 
B) 13.06 
C) 13.37 
D) 0.63 
E) 12.56 
A) 8.62 
B) 13.06 
C) 13.37 
D) 0.63 
E) 12.56

Question 11

Which of the following is correct?

Accepted Answer

A) According to the Bronsted-Lowry theory,an acid is a proton donor while a base is a proton acceptor. 
B) According to the Bronsted-Lowry theory,an acid is a proton acceptor while a base is a proton donor. 
C) According to the Bronsted-Lowry theory,an acid is a proton donor while a base is a hydroxide ion acceptor. 
D) According to the Bronsted-Lowry theory,an acid is a hydroxide donor while a base is a proton acceptor. 
E) According to the Bronsted-Lowry theory,an acid is a hydroxide donor while a base is a hydroxide acceptor. 
A) According to the Bronsted-Lowry theory,an acid is a proton donor while a base is a proton acceptor. 
B) According to the Bronsted-Lowry theory,an acid is a proton acceptor while a base is a proton donor. 
C) According to the Bronsted-Lowry theory,an acid is a proton donor while a base is a hydroxide ion acceptor. 
D) According to the Bronsted-Lowry theory,an acid is a hydroxide donor while a base is a proton acceptor. 
E) According to the Bronsted-Lowry theory,an acid is a hydroxide donor while a base is a hydroxide acceptor.

Question 12

Determine the [OH-] concentration of a 0.741 mol L-1 KOH solution at 25 °C.

Accepted Answer

A) 1.34 × 10-13 mol L-1 
B) 1.34 × 10-14 mol L-1 
C) 0.741 mol L-1 
D) 7.41 mol L-1 
E) 7.41 × 10-13 mol L-1 
A) 1.34 × 10-13 mol L-1 
B) 1.34 × 10-14 mol L-1 
C) 0.741 mol L-1 
D) 7.41 mol L-1 
E) 7.41 × 10-13 mol L-1

Question 13

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

Accepted Answer

A) NH4+/NH3 
B) H3O+/OH- 
C) H2SO3/SO32- 
D) SO42-/SO32- 
E) NaOH/Na+ 
A) NH4+/NH3 
B) H3O+/OH- 
C) H2SO3/SO32- 
D) SO42-/SO32- 
E) NaOH/Na+

Question 14

Which of the following groups is found in carboxylic acids (like acetic acid)?

Accepted Answer

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

Question 15

Calculate the pH of a 0.60 mol L-1 H2SO3 solution that has the stepwise dissociation constants Ka1 = 1.5 × 10-2 and $K _ { \mathrm { a } 2 } = 6.3 \times 10 ^{- 8}$

Accepted Answer

A) 1.02 
B) 1.06 
C) 1.82 
D) 2.04 
A) 1.02 
B) 1.06 
C) 1.82 
D) 2.04

Question 16

Find the percent ionization of a 0.337 mol L-1 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 17

Determine the pOH of a 0.741 mol L-1 KOH solution at 25 °C.

Accepted Answer

A) 0.13 
B) 13.87 
C) 0.17 
D) 12.65 
E) 11.88 
A) 0.13 
B) 13.87 
C) 0.17 
D) 12.65 
E) 11.88

Question 18

Calculate the pOH of an aqueous solution with a pH of 9.85 at 25 °C.

Accepted Answer

A) 2.15 
B) 3.15 
C) 4.15 
D) 5.15 
E) 4.00 
A) 2.15 
B) 3.15 
C) 4.15 
D) 5.15 
E) 4.00

Question 19

What is the pH of a 0.020 mol L-1 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

Question 20

Determine the [OH-] concentration in a 0.235 mol L-1 NaOH solution.

Accepted Answer

A) 4.25 × 10-14 mol L-1 
B) 0.470 mol L-1 
C) 2.13 × 10-14 mol L-1 
D) 0.198 mol L-1 
E) 0.235 mol L-1 
A) 4.25 × 10-14 mol L-1 
B) 0.470 mol L-1 
C) 2.13 × 10-14 mol L-1 
D) 0.198 mol L-1 
E) 0.235 mol L-1

Exam 15: Acids and Bases

What is the Kw of pure water at 50.0 °C,if the pH is 6.630?

Determine the pH of a 0.62 mol L-1 NH4NO3 solution at 25 °C.The Kb for NH3 is 1.76 × 10-5.

Calculate the pOH of a solution that contains 2.4 × 10-5 mol L-1 H3O+ at 25 °C.

Identify acid,base,conjugate acid,and conjugate base in the following reaction: H2CO3(aq)+ H2O(l)⇌ HCO3-(aq)+ H3O+(aq)

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

Calculate the pH of a 0.800 mol L-1 NaCH3CO2 solution.Ka for acetic acid,CH3CO2H,is 1.8×10−51.8 \times 10 ^- 51.8×10−5

Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10-4 mol L-1 in hydronium ion.

What is the pH of a 0.040 mol L-1 Ba(OH)2 solution?

Which of the following is a strong base?

Determine the pOH of a 0.116 mol L-1 Ba(OH)2 solution at 25 °C.

Which of the following is correct?

Determine the [OH-] concentration of a 0.741 mol L-1 KOH solution at 25 °C.

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

Which of the following groups is found in carboxylic acids (like acetic acid)?

Calculate the pH of a 0.60 mol L-1 H2SO3 solution that has the stepwise dissociation constants Ka1 = 1.5 × 10-2 and Ka2=6.3×10−8K _ { \mathrm { a } 2 } = 6.3 \times 10 ^{- 8}Ka2​=6.3×10−8

Find the percent ionization of a 0.337 mol L-1 HF solution.The Ka for HF is 3.5 × 10-4.

Determine the pOH of a 0.741 mol L-1 KOH solution at 25 °C.

Calculate the pOH of an aqueous solution with a pH of 9.85 at 25 °C.

What is the pH of a 0.020 mol L-1 HClO4 solution?

Determine the [OH-] concentration in a 0.235 mol L-1 NaOH solution.

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules,compounds,and Nomenclature

Chemical Reactions and Stoichiometry

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 Molecular Orbital Theory

Liquids, solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry II: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

What is the K_w of pure water at 50.0 °C,if the pH is 6.630?

Determine the pH of a 0.62 mol L^-1 NH₄NO₃ solution at 25 °C.The K_b for NH₃ is 1.76 × 10^-5.

Calculate the pOH of a solution that contains 2.4 × 10^-5 mol L^-1 H₃O⁺ at 25 °C.

Identify acid,base,conjugate acid,and conjugate base in the following reaction: H₂CO₃(aq)+ H₂O(l)⇌ HCO₃^-(aq)+ H₃O⁺(aq)

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

Calculate the pH of a 0.800 mol L^-1 NaCH₃CO₂ solution.K_a for acetic acid,CH₃CO₂H,is $1.8 \times 10 ^- 5$

Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10^-⁴ mol L^-1 in hydronium ion.

What is the pH of a 0.040 mol L^-1 Ba(OH)₂ solution?

Determine the pOH of a 0.116 mol L^-1 Ba(OH)₂ solution at 25 °C.

Determine the [OH^-] concentration of a 0.741 mol L^-1 KOH solution at 25 °C.

Calculate the pH of a 0.60 mol L^-1 H₂SO₃ solution that has the stepwise dissociation constants K_a1 = 1.5 × 10^-2 and $K _ { \mathrm { a } 2 } = 6.3 \times 10 ^{- 8}$

Find the percent ionization of a 0.337 mol L^-1 HF solution.The K_a for HF is 3.5 × 10^-4.

Determine the pOH of a 0.741 mol L^-1 KOH solution at 25 °C.

What is the pH of a 0.020 mol L^-1 HClO₄ solution?

Determine the [OH^-] concentration in a 0.235 mol L^-1 NaOH solution.