Question 1

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 0.010 M solution of HClO is ________.

Accepted Answer

A)  1.7 × 10-5 
B)  0.010 
C)  5.8 × 10-10 
D)  4.76 
E)  2.00 
A)  1.7 × 10-5 
B)  0.010 
C)  5.8 × 10-10 
D)  4.76 
E)  2.00

Question 2

What is the selenide ion concentration [Se2-] for a 0.100 M H2Se solution that has the stepwise dissociation constants of Ka1 = 1.3 × 10-4 and Ka2 = 1.0 × 10-11?

Accepted Answer

A)  3.6 × 10-3 M 
B)  1.3 × 10-4 M 
C)  1.3 × 10-5 M 
D)  1.0 × 10-11 M 
A)  3.6 × 10-3 M 
B)  1.3 × 10-4 M 
C)  1.3 × 10-5 M 
D)  1.0 × 10-11 M

Question 3

Identify the base that is in baking soda.

Accepted Answer

A)  CsOH 
B)  NaOH 
C)  NaHCO3 
D)  K2CO3 
E)  LiHCO3 
A)  CsOH 
B)  NaOH 
C)  NaHCO3 
D)  K2CO3 
E)  LiHCO3

Question 4

Determine the pH of a solution that is 0.15 M HClO2 (Ka = 1.1 × 10-2)and 0.15 M HClO (Ka = 2.9 × 10-8).

Accepted Answer

A)  4.18 
B)  9.82 
C)  12.55 
D)  1.39 
E)  3.55 
A)  4.18 
B)  9.82 
C)  12.55 
D)  1.39 
E)  3.55

Question 5

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 6

Which one of the following will form a basic solution in water?

Accepted Answer

A)  KC2H3O2 
B)  KCN 
C)  NaClO2 
D)  LiBrO 
E)  All of the above will form basic solutions. 
A)  KC2H3O2 
B)  KCN 
C)  NaClO2 
D)  LiBrO 
E)  All of the above will form basic solutions.

Question 7

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 8

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

Accepted Answer

A)  1.34 × 10-13 M 
B)  1.34 × 10-14 M 
C)  0.741 M 
D)  7.41 M 
E)  none of the above 
A)  1.34 × 10-13 M 
B)  1.34 × 10-14 M 
C)  0.741 M 
D)  7.41 M 
E)  none of the above

Question 9

Identify the weakest acid.

Accepted Answer

A)  HF 
B)  HCl 
C)  HBr 
D)  HI 
E)  Not enough information is available. 
A)  HF 
B)  HCl 
C)  HBr 
D)  HI 
E)  Not enough information is available.

Question 10

Which of the following is TRUE?

Accepted Answer

A)  A neutral solution contains [H2O] = [H3O⁺]. 
B)  An neutral solution does not contain any H3O+ or OH-. 
C)  An acidic solution has [H3O⁺] > [OH⁻]. 
D)  A basic solution does not contain H3O+. 
E)  None of the above is true. 
A)  A neutral solution contains [H2O] = [H3O⁺]. 
B)  An neutral solution does not contain any H3O+ or OH-. 
C)  An acidic solution has [H3O⁺] > [OH⁻]. 
D)  A basic solution does not contain H3O+. 
E)  None of the above is true.

Question 11

Identify the triprotic acid.

Accepted Answer

A)  HClO3 
B)  H3PO4 
C)  H2SO4 
D)  HFO 
E)  HBr 
A)  HClO3 
B)  H3PO4 
C)  H2SO4 
D)  HFO 
E)  HBr

Question 12

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)  0.118 M 
E)  0.235 M 
A)  4.25 × 10-14 M 
B)  0.470 M 
C)  2.13 × 10-14 M 
D)  0.118 M 
E)  0.235 M

Question 13

Which of the following acids is the weakest? 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)  H COOH, 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)  H COOH, 1.8 × 10-4 
E)  HClO2, 1.1 × 10-2

Question 14

An aqueous solution at 25.0°C contains [   ] = 0.099 M.What is the pH of the solution?

Accepted Answer

A)  1.00 
B)  -1.00 
C)  13.0 
D)  0.0990 
E)  1.00 ×   
A)  1.00 
B)  -1.00 
C)  13.0 
D)  0.0990 
E)  1.00 ×

Question 15

Determine the pH of a 0.188 M NH3 solution at 25°C.The Kb of NH3 is 1.76 × 10-5.

Accepted Answer

A)  5.480 
B)  2.740 
C)  8.520 
D)  11.260 
E)  12.656 
A)  5.480 
B)  2.740 
C)  8.520 
D)  11.260 
E)  12.656

Question 16

Identify the strong diprotic acid.

Accepted Answer

A)  H2SO3 
B)  H2CO3 
C)  HNO3 
D)  H2SO4 
E)  HOOCCH2COOH 
A)  H2SO3 
B)  H2CO3 
C)  HNO3 
D)  H2SO4 
E)  HOOCCH2COOH

Question 17

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 18

Which of the following is a Lewis base?

Accepted Answer

A)  AlCl3 
B)  H2O 
C)  SiBr4 
D)  C4H10 
E)  None of the above is a Lewis base. 
A)  AlCl3 
B)  H2O 
C)  SiBr4 
D)  C4H10 
E)  None of the above is a Lewis base.

Question 19

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)  There is not enough information to calculate the Kw. 
A)  2.34 × 10-7 
B)  5.50 × 10-14 
C)  2.13 × 10-14 
D)  1.00 × 10-14 
E)  There is not enough information to calculate the Kw.

Question 20

The base-dissociation constant of ethylamine (C2H5NH2)is 6.4 × 10-4 at 25.0°C.The [   ] 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

Exam 16: Acids and Bases

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 0.010 M solution of HClO is ________.

What is the selenide ion concentration [Se2-] for a 0.100 M H2Se solution that has the stepwise dissociation constants of Ka1 = 1.3 × 10-4 and Ka2 = 1.0 × 10-11?

Identify the base that is in baking soda.

Determine the pH of a solution that is 0.15 M HClO2 (Ka = 1.1 × 10-2)and 0.15 M HClO (Ka = 2.9 × 10-8).

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

Which one of the following will form a basic solution in water?

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 [OH-] concentration of a 0.741 M KOH solution at 25°C.

Identify the weakest acid.

Which of the following is TRUE?

Identify the triprotic acid.

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

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

An aqueous solution at 25.0°C contains [ ] = 0.099 M.What is the pH of the solution?

Determine the pH of a 0.188 M NH3 solution at 25°C.The Kb of NH3 is 1.76 × 10-5.

Identify the strong diprotic acid.

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

Which of the following is a Lewis base?

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

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

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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 0.010 M solution of HClO is ________.

What is the selenide ion concentration [Se^2-] for a 0.100 M H₂Se solution that has the stepwise dissociation constants of K_a1 = 1.3 × 10^-4 and K_a2 = 1.0 × 10^-11?

Determine the pH of a solution that is 0.15 M HClO₂ (K_a = 1.1 × 10^-2)and 0.15 M HClO (K_a = 2.9 × 10^-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.

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

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

Determine the pH of a 0.188 M NH₃ solution at 25°C.The K_bof NH₃ is 1.76 × 10^-5.

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

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

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