Question 1

Which of the following is an Arrhenius base?

Accepted Answer

A)  CH3CO2H 
B)  NaOH 
C)  CH3OH 
D)  LiCl 
E)  H2CO3 
A)  CH3CO2H 
B)  NaOH 
C)  CH3OH 
D)  LiCl 
E)  H2CO3

Question 2

Calculate the hydronium ion concentration in an aqueous solution with a pH of 9.85 at 25 °C.

Accepted Answer

A)  7.1 × 10-5 mol L-1 
B)  4.2 × 10-10 mol L-1 
C)  8.7 × 10-10 mol L-1 
D)  6.5 × 10-5 mol L-1 
E)  1.4 × 10-10 mol L-1 
A)  7.1 × 10-5 mol L-1 
B)  4.2 × 10-10 mol L-1 
C)  8.7 × 10-10 mol L-1 
D)  6.5 × 10-5 mol L-1 
E)  1.4 × 10-10 mol L-1

Question 3

Calculate the pH 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

Determine the [OH⁻] concentration in a 0.169 mol L-1 Ca(OH)2 solution.

Accepted Answer

A)  0.338 mol L-1 
B)  0.169 mol L-1 
C)  5.92 × 10-14 mol L-1 
D)  2.96 × 10-14 mol L-1 
E)  0.298 mol L-1 
A)  0.338 mol L-1 
B)  0.169 mol L-1 
C)  5.92 × 10-14 mol L-1 
D)  2.96 × 10-14 mol L-1 
E)  0.298 mol L-1

Question 5

What is the pH of a 0.0 40 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 6

Identify the strongest acid.

Accepted Answer

A)  HClO4 
B)  HClO3 
C)  HClO2 
D)  HClO 
A)  HClO4 
B)  HClO3 
C)  HClO2 
D)  HClO

Question 7

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 8

Match the following.
-Arrhenius base

Accepted Answer

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

Question 9

The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0 °C is 4.9 × 10-10. What is the pH of an aqueous solution of 0.87 mol L-1 sodium cyanide (NaCN)?

Accepted Answer

A)  0.06 
B)  13.94 
C)  4.2 × 10-3 
D)  2.38 
E)  11.62 
A)  0.06 
B)  13.94 
C)  4.2 × 10-3 
D)  2.38 
E)  11.62

Question 10

Which of the following increases the strength of a binary acid, HY?

Accepted Answer

A)  decreasing the electron affinity of Y and decreasing the H-Y bond strength 
B)  increasing the electron affinity of Y and increasing the H-Y bond strength 
C)  increasing the electron affinity of Y and decreasing the H-Y bond strength 
D)  decreasing the electron affinity of Y and increasing the H-Y bond strength 
E)  none of the above 
A)  decreasing the electron affinity of Y and decreasing the H-Y bond strength 
B)  increasing the electron affinity of Y and increasing the H-Y bond strength 
C)  increasing the electron affinity of Y and decreasing the H-Y bond strength 
D)  decreasing the electron affinity of Y and increasing the H-Y bond strength 
E)  none of the above

Question 11

Determine the concentration of CO32- ions in a 0.18 mol L-1 H2CO3 solution. Carbonic acid is a diprotic acid with Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Accepted Answer

A)  2.8 × 10-4 mol L-1 
B)  3.2 × 10-6 mol L-1 
C)  5.6 × 10-11 mol L-1 
D)  4.3 × 10-7 mol L-1 
E)  6.9 × 10-8 mol L-1 
A)  2.8 × 10-4 mol L-1 
B)  3.2 × 10-6 mol L-1 
C)  5.6 × 10-11 mol L-1 
D)  4.3 × 10-7 mol L-1 
E)  6.9 × 10-8 mol L-1

Question 12

Which of the following is a general property of a base?

Accepted Answer

A)  Bases have sour taste. 
B)  Bases turn blue litmus paper red. 
C)  Bases leave red litmus paper unchanged. 
D)  Bases turn red litmus paper blue. 
E)  Bases easily dissolve many metallic elements. 
A)  Bases have sour taste. 
B)  Bases turn blue litmus paper red. 
C)  Bases leave red litmus paper unchanged. 
D)  Bases turn red litmus paper blue. 
E)  Bases easily dissolve many metallic elements.

Question 13

Identify the triprotic acid.

Accepted Answer

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

Question 14

Which of the following solutions would have the highest pH? Assume that they are all 0.10 mol L-1 in acid at 25 °C? 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 15

What is the hydronium ion concentration and the pH for an aqueous solution of NH3 that has a hydroxide ion concentration of  2.25 x 10-2 mol L-1?

Accepted Answer

A)  4.44 × 10-12 mol L-1 and 2.65 
B)  4.44 × 10-12 mol L-1 and 11.35 
C)  4.44 × 10-13 mol L-1 and 1.65 
D)  4.44 × 10-13 mol L-1 and 12.35 
A)  4.44 × 10-12 mol L-1 and 2.65 
B)  4.44 × 10-12 mol L-1 and 11.35 
C)  4.44 × 10-13 mol L-1 and 1.65 
D)  4.44 × 10-13 mol L-1 and 12.35

Question 16

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 17

Calculate the pH for an aqueous solution of pyridine that contains  2.15 x 10-4 mol L-1 hydroxide ion.

Accepted Answer

A)  4.65 × 10-11 
B)  2.15 × 10-4  
C)  3. 67 
D)  10. 33 
A)  4.65 × 10-11 
B)  2.15 × 10-4  
C)  3. 67 
D)  10. 33

Question 18

What is the pH of a 0. 40 mol L-1 (H2Se) solution that has the stepwise dissociation constants Ka1 = 1.3 × 10-4 and  Ka2=1.0 x10-11 ?

Accepted Answer

A)  2. 14 
B)  3.89 
C)  4. 28 
D)  5. 57 
A)  2. 14 
B)  3.89 
C)  4. 28 
D)  5. 57

Question 19

A solution with a hydrogen ion concentration of 3.25 × 10-6 mol L-1 is ________ and has a hydroxide ion concentration of ________.

Accepted Answer

A)  acidic; 3.08 × 10-8 mol L-1 
B)  acidic; 3.08 × 10-9 mol L-1 
C)  basic; 3.08 × 10-8 mol L-1 
D)  basic; 3.08 × 10-9 mol L-1 
A)  acidic; 3.08 × 10-8 mol L-1 
B)  acidic; 3.08 × 10-9 mol L-1 
C)  basic; 3.08 × 10-8 mol L-1 
D)  basic; 3.08 × 10-9 mol L-1

Question 20

The pH of a solution is 5.67 at 25 °C. Calculate the pOH of this solution at 25 °C.

Accepted Answer

A)  2.40 
B)  8.33 
C)  4.88 
D)  11.4 
E)  12.7 
A)  2.40 
B)  8.33 
C)  4.88 
D)  11.4 
E)  12.7

Exam 15: Acids and Bases

Which of the following is an Arrhenius base?

Calculate the hydronium ion concentration in an aqueous solution with a pH of 9.85 at 25 °C.

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

Determine the [OH⁻] concentration in a 0.169 mol L-1 Ca(OH)2 solution.

What is the pH of a 0.0 40 mol L-1 Ba(OH)2 solution?

Identify the strongest acid.

What is the pH of a 0. 020 mol L-1 HClO4 solution?

Match the following. -Arrhenius base

The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0 °C is 4.9 × 10-10. What is the pH of an aqueous solution of 0.87 mol L-1 sodium cyanide (NaCN)?

Which of the following increases the strength of a binary acid, HY?

Determine the concentration of CO32- ions in a 0.18 mol L-1 H2CO3 solution. Carbonic acid is a diprotic acid with Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Which of the following is a general property of a base?

Identify the triprotic acid.

Which of the following solutions would have the highest pH? Assume that they are all 0.10 mol L-1 in acid at 25 °C? The acid is followed by its Ka value.

What is the hydronium ion concentration and the pH for an aqueous solution of NH3 that has a hydroxide ion concentration of 2.25 x 10-2 mol L-1?

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 pH for an aqueous solution of pyridine that contains 2.15 x 10-4 mol L-1 hydroxide ion.

What is the pH of a 0. 40 mol L-1 (H2Se) solution that has the stepwise dissociation constants Ka1 = 1.3 × 10-4 and Ka2=1.0 x10-11 ?

A solution with a hydrogen ion concentration of 3.25 × 10-6 mol L-1 is ________ and has a hydroxide ion concentration of ________.

The pH of a solution is 5.67 at 25 °C. Calculate the pOH of this solution at 25 °C.

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Filters

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

Determine the [OH⁻] concentration in a 0.169 mol L^-1 Ca(OH)₂ solution.

What is the pH of a 0.0 40 mol L^-1 Ba(OH)₂ solution?

What is the pH of a 0. 020 mol L^-1 HClO₄ solution?

The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0 °C is 4.9 × 10^-10. What is the pH of an aqueous solution of 0.87 mol L^-1 sodium cyanide (NaCN)?

Determine the concentration of CO₃^2- ions in a 0.18 mol L^-1 H₂CO₃ solution. Carbonic acid is a diprotic acid with K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

Which of the following solutions would have the highest pH? Assume that they are all 0.10 mol L^-1in acid at 25 °C? The acid is followed by its K_a value.

What is the hydronium ion concentration and the pH for an aqueous solution of NH₃ that has a hydroxide ion concentration of 2.25 x 10^-2 mol L^-1?

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 pH for an aqueous solution of pyridine that contains 2.15 x 10^-4 mol L^-1 hydroxide ion.

What is the pH of a 0. 40 mol L^-1 (H₂Se) solution that has the stepwise dissociation constants K_a1 = 1.3 × 10^-4 and K_a2=1.0 x10^-11 ?

A solution with a hydrogen ion concentration of 3.25 × 10^-⁶ mol L^-1 is and has a hydroxide ion concentration of .