Question 1

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 
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 2

Calculate the pH of a 0.800 M NaCH3CO2 solution.Ka for acetic acid,CH3CO2H,is 1.8 × 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 3

Which of the following is a Lewis acid?

Accepted Answer

A)  AlI3 
B)  CF4 
C)  NH3 
D)  CHI3 
E)  None of the above is a Lewis acid. 
A)  AlI3 
B)  CF4 
C)  NH3 
D)  CHI3 
E)  None of the above is a Lewis acid.

Question 4

Identify the acid in citrus fruits.

Accepted Answer

A)  citric acid 
B)  hydrochloric acid 
C)  carbonic acid 
D)  hydrofluoric acid 
E)  phosphoric acid 
A)  citric acid 
B)  hydrochloric acid 
C)  carbonic acid 
D)  hydrofluoric acid 
E)  phosphoric acid

Question 5

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 
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 6

Identify the acid that is in vinegar.

Accepted Answer

A)  H2SO4 
B)  NaHCO3 
C)  Rb2CO3 
D)  CH3COOH 
E)  HI 
A)  H2SO4 
B)  NaHCO3 
C)  Rb2CO3 
D)  CH3COOH 
E)  HI

Question 7

Determine the pH of 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)  11.00 
B)  10.44 
C)  5.50 
D)  4.31 
E)  3.56 
A)  11.00 
B)  10.44 
C)  5.50 
D)  4.31 
E)  3.56

Question 8

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 0.080 M sodium cyanide (NaCN)?

Accepted Answer

A)  11.11 
B)  2.89 
C)  1.3 × 10-3 
D)  7.8 × 10-12 
E)  3.9 × 10-11 
A)  11.11 
B)  2.89 
C)  1.3 × 10-3 
D)  7.8 × 10-12 
E)  3.9 × 10-11

Question 9

Which of the following is a triprotic acid?

Accepted Answer

A)  HBr 
B)  H2SO4 
C)  H3PO4 
D)  CI4 
E)  HC2H3O2 
A)  HBr 
B)  H2SO4 
C)  H3PO4 
D)  CI4 
E)  HC2H3O2

Question 10

Calculate the hydroxide ion concentration in an aqueous potassium hydroxide solution that contains 3.50 × 10-6 M in hydronium ion.

Accepted Answer

A)  2.86 × 10-1 M 
B)  2.86 × 10-8 M 
C)  2.86 × 10-9 M 
D)  3.50 × 10-9 M 
E)  3.50 × 10-6 M 
A)  2.86 × 10-1 M 
B)  2.86 × 10-8 M 
C)  2.86 × 10-9 M 
D)  3.50 × 10-9 M 
E)  3.50 × 10-6 M

Question 11

Which of the following is a polyprotic acid?

Accepted Answer

A)  HBr 
B)  H2SO4 
C)  KCN 
D)  CF4 
E)  HC2H3O2 
A)  HBr 
B)  H2SO4 
C)  KCN 
D)  CF4 
E)  HC2H3O2

Question 12

Identify the diprotic acid.

Accepted Answer

A)  HNO3 
B)  HBr 
C)  CH3COOH 
D)  H2SO3 
E)  HClO3 
A)  HNO3 
B)  HBr 
C)  CH3COOH 
D)  H2SO3 
E)  HClO3

Question 13

Identify the strongest acid.

Accepted Answer

A)  1.00 M HCOOH 
B)  1.00 M CH3COOH 
C)  1.00 M HCl 
D)  1.00 M HClO 
E)  1.00 M HF 
A)  1.00 M HCOOH 
B)  1.00 M CH3COOH 
C)  1.00 M HCl 
D)  1.00 M HClO 
E)  1.00 M HF

Question 14

The Lewis model describes the transfer of

Accepted Answer

A)  one neutron. 
B)  protons. 
C)  electron pairs. 
D)  neutrons. 
E)  one electron. 
A)  one neutron. 
B)  protons. 
C)  electron pairs. 
D)  neutrons. 
E)  one electron.

Question 15

Calculate the pH for an aqueous solution of pyridine that contains 2.15 × 10-4 M 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 16

What is the conjugate acid of HCO3⁻ ?

Accepted Answer

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

Question 17

Which of the following bases is the weakest? The base is followed by its Kb value.

Accepted Answer

A)  HOCH2CH2NH2, 3.2 × 10-5 
B)  NH3, 1.76 × 10-5 
C)  C5H5N, 1.7 × 10-9 
D)  (CH3CH2)3N, 5.2 × 10-4 
E)  Since these are all weak bases, they have the same strength. 
A)  HOCH2CH2NH2, 3.2 × 10-5 
B)  NH3, 1.76 × 10-5 
C)  C5H5N, 1.7 × 10-9 
D)  (CH3CH2)3N, 5.2 × 10-4 
E)  Since these are all weak bases, they have the same strength.

Question 18

If an equal number of moles of the weak acid HF and the strong base NaOH are added to water,is the resulting solution acidic,basic,or neutral?

Accepted Answer

A)  acidic 
B)  basic 
C)  neutral 
D)  There is insufficient information provided to answer this question. 
A)  acidic 
B)  basic 
C)  neutral 
D)  There is insufficient information provided to answer this question.

Question 19

Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

Accepted Answer

A)  RbI 
B)  RbBr 
C)  RbCl 
D)  RbF 
A)  RbI 
B)  RbBr 
C)  RbCl 
D)  RbF

Question 20

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

Exam 16: Acids and Bases

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

Calculate the pH of a 0.800 M NaCH3CO2 solution.Ka for acetic acid,CH3CO2H,is 1.8 × 10-5.

Which of the following is a Lewis acid?

Identify the acid in citrus fruits.

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.

Identify the acid that is in vinegar.

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

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 0.080 M sodium cyanide (NaCN)?

Which of the following is a triprotic acid?

Calculate the hydroxide ion concentration in an aqueous potassium hydroxide solution that contains 3.50 × 10-6 M in hydronium ion.

Which of the following is a polyprotic acid?

Identify the diprotic acid.

Identify the strongest acid.

The Lewis model describes the transfer of

Calculate the pH for an aqueous solution of pyridine that contains 2.15 × 10-4 M hydroxide ion.

What is the conjugate acid of HCO3⁻ ?

Which of the following bases is the weakest? The base is followed by its Kb value.

If an equal number of moles of the weak acid HF and the strong base NaOH are added to water,is the resulting solution acidic,basic,or neutral?

Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

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

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Chemical Quantities and Aqueous Reactions

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Filters

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?

Calculate the pH of a 0.800 M NaCH₃CO₂ solution.K_a for acetic acid,CH₃CO₂H,is 1.8 × 10^-⁵.

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.

Determine the pH of 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.

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 0.080 M sodium cyanide (NaCN)?

Calculate the hydroxide ion concentration in an aqueous potassium hydroxide solution that contains 3.50 × 10^-6 M in hydronium ion.

Calculate the pH for an aqueous solution of pyridine that contains 2.15 × 10^-⁴M hydroxide ion.

What is the conjugate acid of HCO₃⁻ ?

Which of the following bases is the weakest? The base is followed by its K_b value.

If an equal number of moles of the weak acid HFand the strong base NaOH are added to water,is the resulting solution acidic,basic,or neutral?