Question 1

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

Question 2

Calculate the pH of a 0.020 M carbonic acid solution,H2CO3(aq),that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Accepted Answer

A)  1.70 
B)  4.03 
C)  6.37 
D)  10.25

Question 3

What is the pH of a 0.84 M solution of a base that has a Kb = 7.3 × 10-10?

Accepted Answer

A)  4.11 
B)  7.29 
C)  9.39 
D)  10.98

Question 4

A 8.0 × 10-3 M aqueous solution of  at 25.0°C has a pH of

Accepted Answer

A)  12.20 
B)  1.80 
C)  1.6 × 10-2 
D)  6.3 × 10-13 
E)  11.90

Question 5

Calculate the pH of a 1.60 M NaCH3CO2 solution.Ka for acetic acid,CH3CO2H,is 1.8 × 10-5.

Accepted Answer

A)  2.27 
B)  4.53 
C)  9.47 
D)  11.73

Question 6

Which of the following is a Brønsted-Lowry base?

Accepted Answer

A)  CH4 
B)  HCN 
C)  NH3 
D)  I2 
E)  None of the above are Brønsted-Lowry bases.

Question 7

What is the concentration of hydroxide ions in pure water at 30.0∘C,if Kw at this temperature is 1.47 × 10-14?

Accepted Answer

A)  1.00 × 10-7 M 
B)  1.30 × 10-7 M 
C)  1.47 × 10-7 M 
D)  8.93 × 10-8 M 
E)  1.21 × 10-7 M

Question 8

Do both protons ionize instantaneously from a diprotic acid such as H₂CO₃? Explain your answer.

Accepted Answer

The answer of Do both protons ionize instantaneously from a...

Question 9

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

Question 10

What is the hydronium ion concentration and the pH for an aqueous solution of NH3 that has a hydroxide ion concentration of

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

Question 11

Determine the [OH-] concentration of a 0.153 M Ba(OH)2 solution at 25°C.

Accepted Answer

A)  3.27 × 10-14 M 
B)  0.153 M 
C)  0.306 M 
D)  6.53 × 10-14 M 
E)  0.0765 M

Question 12

Determine the pH in a 0.235 M NaOH solution.

Accepted Answer

A)  13.76 
B)  0.24 
C)  13.37 
D)  0.63 
E)  12

Question 13

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

Question 14

What is the conjugate acid of HCO3⁻ ?

Accepted Answer

A)  H3O+ 
B)  H2O 
C)  CO32- 
D)  OH⁻ 
E)  H2CO3

Question 15

Identify the diprotic acid.

Accepted Answer

A)  HNO3 
B)  HBr 
C)  CH3COOH 
D)  H2SO4 
E)  HClO4

Question 16

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

Question 17

Which of the following species is amphoteric?

Accepted Answer

A)  HPO4- 
B)  H3O+ 
C)  PO43- 
D)  Cl- 
E)  None of the above are amphoteric.

Question 18

Determine the pH of a 0.227 M C5H5N solution at 25°C.The Kb of C5H5N is 1.7 × 10-9.

Accepted Answer

A)  4.59 
B)  9.41 
C)  4.71 
D)  10.14 
E)  9.29

Question 19

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

Accepted Answer

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

Question 20

Calculate the hydronium ion concentration in an aqueous solution with a pH of 11.7 at 25°C.

Accepted Answer

A)  5.7 × 10-11 M 
B)  1.9× 10-12 M 
C)  5.4 × 10-2 M 
D)  6.4 × 10-7 M 
E)  9.5× 10-3 M

Exam 17: Acids and Bases

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

Calculate the pH of a 0.020 M carbonic acid solution,H₂CO₃₍_aq_{) ,}that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

What is the pH of a 0.84 M solution of a base that has a K_b = 7.3 × 10^-10?

A 8.0 × 10^-3 M aqueous solution of at 25.0°C has a pH of

Calculate the pH of a 1.60 M NaCH₃CO₂ solution.K_a for acetic acid,CH₃CO₂H,is 1.8 × 10^-5.

Which of the following is a Brønsted-Lowry base?

What is the concentration of hydroxide ions in pure water at 30.0^∘C,if K_w at this temperature is 1.47 × 10^-14?

Do both protons ionize instantaneously from a diprotic acid such as H₂CO₃? Explain your answer.

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.

What is the hydronium ion concentration and the pH for an aqueous solution of NH₃ that has a hydroxide ion concentration of

Determine the [OH^-] concentration of a 0.153 M Ba(OH) ₂ solution at 25°C.

Determine the pH in a 0.235 M NaOH solution.

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

What is the conjugate acid of HCO₃⁻ ?

Identify the diprotic acid.

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

Which of the following species is amphoteric?

Determine the pH of a 0.227 M C₅H₅N solution at 25°C.The K_b of C₅H₅N is 1.7 × 10^-9.

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

Calculate the hydronium ion concentration in an aqueous solution with a pH of 11.7 at 25°C.

Exam 17: Acids and Bases

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

Calculate the pH of a 0.020 M carbonic acid solution,H2CO3(aq) ,that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

What is the pH of a 0.84 M solution of a base that has a Kb = 7.3 × 10-10?

A 8.0 × 10-3 M aqueous solution of at 25.0°C has a pH of

Calculate the pH of a 1.60 M NaCH3CO2 solution.Ka for acetic acid,CH3CO2H,is 1.8 × 10-5.

Which of the following is a Brønsted-Lowry base?

What is the concentration of hydroxide ions in pure water at 30.0∘C,if Kw at this temperature is 1.47 × 10-14?

Do both protons ionize instantaneously from a diprotic acid such as H2CO3? Explain your answer.

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.

What is the hydronium ion concentration and the pH for an aqueous solution of NH3 that has a hydroxide ion concentration of

Determine the [OH-] concentration of a 0.153 M Ba(OH) 2 solution at 25°C.

Determine the pH in a 0.235 M NaOH solution.

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

What is the conjugate acid of HCO3⁻ ?

Identify the diprotic acid.

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

Which of the following species is amphoteric?

Determine the pH of a 0.227 M C5H5N solution at 25°C.The Kb of C5H5N is 1.7 × 10-9.

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

Calculate the hydronium ion concentration in an aqueous solution with a pH of 11.7 at 25°C.

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

Calculate the pH of a 0.020 M carbonic acid solution,H₂CO₃₍_aq_{) ,}that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

What is the pH of a 0.84 M solution of a base that has a K_b = 7.3 × 10^-10?

A 8.0 × 10^-3 M aqueous solution of at 25.0°C has a pH of

Calculate the pH of a 1.60 M NaCH₃CO₂ solution.K_a for acetic acid,CH₃CO₂H,is 1.8 × 10^-5.

What is the concentration of hydroxide ions in pure water at 30.0^∘C,if K_w at this temperature is 1.47 × 10^-14?

Do both protons ionize instantaneously from a diprotic acid such as H₂CO₃? Explain your answer.

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.

What is the hydronium ion concentration and the pH for an aqueous solution of NH₃ that has a hydroxide ion concentration of

Determine the [OH^-] concentration of a 0.153 M Ba(OH) ₂ solution at 25°C.

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

What is the conjugate acid of HCO₃⁻ ?

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

Determine the pH of a 0.227 M C₅H₅N solution at 25°C.The K_b of C₅H₅N is 1.7 × 10^-9.

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