Question 1

Which of the following is not a conjugate acid-base pair?

Accepted Answer

A)  NH4+/NH3 
B)  H3O⁺/OH⁻ 
C)  H2SO3/HSO3⁻ 
D)  C2H3O2⁻/HC2H3O2 
E)  All of the above are conjugate acid-base pairs. 
A)  NH4+/NH3 
B)  H3O⁺/OH⁻ 
C)  H2SO3/HSO3⁻ 
D)  C2H3O2⁻/HC2H3O2 
E)  All of the above are conjugate acid-base pairs.

Question 2

The acid-dissociation constant at 25.0°C for hypochlorous acid (HClO)is 3.0 × 10-8.At equilibrium,the molarity of H3O+ in a 0.044 M solution of HClO is

Accepted Answer

A)  3.6 × 10-5 
B)  0.044 
C)  2.8 × 10-10 
D)  4.44 
E)  1.36 
A)  3.6 × 10-5 
B)  0.044 
C)  2.8 × 10-10 
D)  4.44 
E)  1.36

Question 3

Determine the pH of a 0.62 M 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 4

What is the hydronium ion concentration of an acid solution that has a pH of 5.5?

Accepted Answer

A)  2.8 × 10-9 M 
B)  3.6 × 10-6 M 
C)  1.5 x10-11 M 
D)  3.6 x10-3 M 
A)  2.8 × 10-9 M 
B)  3.6 × 10-6 M 
C)  1.5 x10-11 M 
D)  3.6 x10-3 M

Question 5

Identify the strongest acid.

Accepted Answer

A)  HIO4 
B)  HIO3 
C)  HIO2 
D)  HIO 
E)  Not enough information is given. 
A)  HIO4 
B)  HIO3 
C)  HIO2 
D)  HIO 
E)  Not enough information is given.

Question 6

What is the conjugate base of H2PO4⁻ ?

Accepted Answer

A)  HPO42- 
B)  PO43- 
C)  H3PO4 
D)  H3O+ 
E)  OH⁻ 
A)  HPO42- 
B)  PO43- 
C)  H3PO4 
D)  H3O+ 
E)  OH⁻

Question 7

Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10-2 M in hydronium ion.

Accepted Answer

A)  2.86 × 10-5 M 
B)  2.86 × 10-10 M 
C)  2.86 × 10-13 M 
D)  3.50 × 10-13 M 
A)  2.86 × 10-5 M 
B)  2.86 × 10-10 M 
C)  2.86 × 10-13 M 
D)  3.50 × 10-13 M

Question 8

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

Question 9

Which of these is an example of a polyprotic oxyacid?

Accepted Answer

A)  HClO3 
B)  CH3COOH 
C)  H2SO3 
D)  H2S 
E)  None of the above 
A)  HClO3 
B)  CH3COOH 
C)  H2SO3 
D)  H2S 
E)  None of the above

Question 10

Determine the pH of a 0.22 M NaF solution at 25°C.The Ka of HF is 3.5 × 10-5.

Accepted Answer

A)  10.20 
B)  5.10 
C)  8.90 
D)  11.44 
E)  2.56 
A)  10.20 
B)  5.10 
C)  8.90 
D)  11.44 
E)  2.56

Question 11

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)  HBrO, 2.9 × 10-9 
C)  HNO2, 4.6 × 10-4 
D)  H COOH, 1.8 × 10-4 
E)  HClO2, 1.1 × 10-2 
A)  HF, 3.5 × 10-4 
B)  HBrO, 2.9 × 10-9 
C)  HNO2, 4.6 × 10-4 
D)  H COOH, 1.8 × 10-4 
E)  HClO2, 1.1 × 10-2

Question 12

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 13

What is the pH of a 0.040 M 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 14

Identify the triprotic acid.

Accepted Answer

A)  HNO3 
B)  H3PO4 
C)  H2CO3 
D)  HClO4 
E)  H2SO4 
A)  HNO3 
B)  H3PO4 
C)  H2CO3 
D)  HClO4 
E)  H2SO4

Question 15

Calculate the concentration of bicarbonate ion,HCO3-,in a 0.030 M H2CO3 solution that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Accepted Answer

A)  1.1 × 10-4 M 
B)  4.3 × 10-7 M 
C)  1.3 × 10-8 M 
D)  5.6 × 10-11 M 
A)  1.1 × 10-4 M 
B)  4.3 × 10-7 M 
C)  1.3 × 10-8 M 
D)  5.6 × 10-11 M

Question 16

Calculate the hydronium ion concentration in an aqueous solution with a pH of 4.33 at 25°C.

Accepted Answer

A)  2.1 × 10-10 M 
B)  9.7 × 10-10 M 
C)  4.7 × 10-5 M 
D)  3.8 × 10-5 M 
E)  6.3 × 10-6 M 
A)  2.1 × 10-10 M 
B)  9.7 × 10-10 M 
C)  4.7 × 10-5 M 
D)  3.8 × 10-5 M 
E)  6.3 × 10-6 M

Question 17

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 18

Determine the pOH of a 0.348 M Ca(OH)2 solution at 25°C.

Accepted Answer

A)  13.08 
B)  13.54 
C)  13.84 
D)  0.157 
E)  0.458 
A)  13.08 
B)  13.54 
C)  13.84 
D)  0.157 
E)  0.458

Question 19

How many of the following are weak acids?
HNO2 HClO HNO3 H2PO4⁻

Accepted Answer

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

Exam 17: Acids and Bases

Which of the following is not a conjugate acid-base pair?

The acid-dissociation constant at 25.0°C for hypochlorous acid (HClO)is 3.0 × 10-8.At equilibrium,the molarity of H3O+ in a 0.044 M solution of HClO is

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

What is the hydronium ion concentration of an acid solution that has a pH of 5.5?

Identify the strongest acid.

What is the conjugate base of H2PO4⁻ ?

Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10-2 M in hydronium ion.

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.

Which of these is an example of a polyprotic oxyacid?

Determine the pH of a 0.22 M NaF solution at 25°C.The Ka of HF is 3.5 × 10-5.

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

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

What is the pH of a 0.040 M Ba(OH)2 solution?

Identify the triprotic acid.

Calculate the concentration of bicarbonate ion,HCO3-,in a 0.030 M H2CO3 solution that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Calculate the hydronium ion concentration in an aqueous solution with a pH of 4.33 at 25°C.

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).

Determine the pOH of a 0.348 M Ca(OH)2 solution at 25°C.

How many of the following are weak acids? HNO2 HClO HNO3 H2PO4⁻

Essentials: Units, Measurements, and Problem Solving

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The Quantum Mechanical Model of the Atom

Periodic Properties of the Elements

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Introduction to Solutions and Aqueous Reactions

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Crystalline Solids and Modern Materials

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The acid-dissociation constant at 25.0°C for hypochlorous acid (HClO)is 3.0 × 10^-8.At equilibrium,the molarity of H₃O⁺ in a 0.044 M solution of HClO is

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

What is the conjugate base of H₂PO₄⁻ ?

Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10^-² M in hydronium ion.

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.

Determine the pH of a 0.22 M NaF solution at 25°C.The K_a of HF is 3.5 × 10^-5.

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

What is the pH of a 0.040 M Ba(OH)₂ solution?

Calculate the concentration of bicarbonate ion,HCO₃^-,in a 0.030 M H₂CO₃ solution that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

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).

Determine the pOH of a 0.348 M Ca(OH)₂ solution at 25°C.

How many of the following are weak acids? HNO₂ HClOHNO₃ H₂PO₄⁻