Question 1

Carbon dioxide combines with rainwater to form

Accepted Answer

A)  phosphoric acid. 
B)  carbonic acid. 
C)  nitric acid. 
D)  sulfuric acid. 
E)  nitrous acid. 
A)  phosphoric acid. 
B)  carbonic acid. 
C)  nitric acid. 
D)  sulfuric acid. 
E)  nitrous acid. B

Question 2

Identify the acid that is in car batteries.

Accepted Answer

A)  H2SO4 
B)  HNO3 
C)  Na2CO3 
D)  CH3COOH 
E)  HCl 
A)  H2SO4 
B)  HNO3 
C)  Na2CO3 
D)  CH3COOH 
E)  HCl A

Question 3

Which of the following is an Arrhenius base?

Accepted Answer

A)  CH3CO2H 
B)  RbOH 
C)  CH3OH 
D)  KBr 
E)  More than one of these compounds is an Arrhenius base. 
A)  CH3CO2H 
B)  RbOH 
C)  CH3OH 
D)  KBr 
E)  More than one of these compounds is an Arrhenius base. B

Question 4

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

Accepted Answer

A)  7.1 × 10-5 M 
B)  4.2 × 10-10 M 
C)  8.7 × 10-10 M 
D)  6.5 × 10-5 M 
E)  1.4 × 10-10 M 
A)  7.1 × 10-5 M 
B)  4.2 × 10-10 M 
C)  8.7 × 10-10 M 
D)  6.5 × 10-5 M 
E)  1.4 × 10-10 M

Question 5

Which of the following solutions would have the highest pH? Assume that they are all 0.10 M 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 6

Identify the acid that is used to preserve soft drinks.

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 7

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

Accepted Answer

A)  acidic, 3.08 × 10-8 M 
B)  acidic, 3.08 × 10-9 M 
C)  basic, 3.08 × 10-8 M 
D)  basic, 3.08 × 10-9 M 
A)  acidic, 3.08 × 10-8 M 
B)  acidic, 3.08 × 10-9 M 
C)  basic, 3.08 × 10-8 M 
D)  basic, 3.08 × 10-9 M

Question 8

Find the percent ionization of a 0.337 M HF solution.The Ka for HF is 3.5 × 10-4.

Accepted Answer

A)  1.1% 
B)  1.2 × 10-2% 
C)  3.2% 
D)  3.5 × 10-2% 
E)  4.7% 
A)  1.1% 
B)  1.2 × 10-2% 
C)  3.2% 
D)  3.5 × 10-2% 
E)  4.7%

Question 9

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 10

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 
A)  6.767 
B)  0.465 
C)  7.000 
D)  7.233 
E)  8.446

Question 11

Calculate the concentration of bicarbonate ion,HCO3-,in a 0.010 M H2CO3 solution that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Accepted Answer

A)  6.6 × 10-5 M 
B)  4.3 × 10-7 M 
C)  4.3 × 10-9 M 
D)  5.6 × 10-11 M 
A)  6.6 × 10-5 M 
B)  4.3 × 10-7 M 
C)  4.3 × 10-9 M 
D)  5.6 × 10-11 M

Question 12

Which Br∅nsted-Lowry acid is NOT considered to be a strong acid in water?

Accepted Answer

A)  HBr 
B)  HBr  
C)  HNO2 
D)  HNO3 
A)  HBr 
B)  HBr  
C)  HNO2 
D)  HNO3

Question 13

Determine the [H3O⁺] in a 0.265 M HClO solution.The Ka of HClO is 2.9 × 10-8.

Accepted Answer

A)  1.1 × 10-10 M 
B)  7.7 × 10-9 M 
C)  1.3 × 10-6 M 
D)  4.9 × 10-4 M 
E)  8.8 × 10-5 M 
A)  1.1 × 10-10 M 
B)  7.7 × 10-9 M 
C)  1.3 × 10-6 M 
D)  4.9 × 10-4 M 
E)  8.8 × 10-5 M

Question 14

Which one of the following will form an acidic solution in water?

Accepted Answer

A)  NH4Cl 
B)  LiF 
C)  NaI 
D)  LiNO3 
E)  None of the above solutions will be acidic. 
A)  NH4Cl 
B)  LiF 
C)  NaI 
D)  LiNO3 
E)  None of the above solutions will be acidic.

Question 15

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

Accepted Answer

A)  (CH3CH2)2NH, 8.6 × 10-4 
B)  CH3NH2, 4.4 × 10-4 
C)  C6H5NH2, 4.0 × 10-10 
D)  NH3, 1.76 × 10-5 
E)  C5H5N, 1.7 × 10-9 
A)  (CH3CH2)2NH, 8.6 × 10-4 
B)  CH3NH2, 4.4 × 10-4 
C)  C6H5NH2, 4.0 × 10-10 
D)  NH3, 1.76 × 10-5 
E)  C5H5N, 1.7 × 10-9

Question 16

Determine the pH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 × 10-5.

Accepted Answer

A)  2.26 
B)  4.52 
C)  11.74 
D)  9.48 
E)  5.48 
A)  2.26 
B)  4.52 
C)  11.74 
D)  9.48 
E)  5.48

Question 17

What is the pH of a 0.30 M pyridine solution that has Kb = 1.9 × 10-9? The equation for the dissociation of pyridine is: C5H5N(aq)+ H2O(l)⇌ C5H5NH+(aq)+ OH-(aq)

Accepted Answer

A)  4.62 
B)  8.72 
C)  9.38 
D)  10.38 
A)  4.62 
B)  8.72 
C)  9.38 
D)  10.38

Question 18

Calculate the pH of a 1.60 M KBrO solution.Ka for hypobromous acid,HBrO,is

Accepted Answer

A)  2.55 
B)  4.25 
C)  9.75 
D)  11.45 
A)  2.55 
B)  4.25 
C)  9.75 
D)  11.45

Question 19

Identify the substance that is NOT acidic.

Accepted Answer

A)  soft drink 
B)  apple 
C)  household ammonia 
D)  lemon 
E)  plum 
A)  soft drink 
B)  apple 
C)  household ammonia 
D)  lemon 
E)  plum

Question 20

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 
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

Exam 16: Acids and Bases

Carbon dioxide combines with rainwater to form

Identify the acid that is in car batteries.

Which of the following is an Arrhenius base?

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

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

Identify the acid that is used to preserve soft drinks.

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

Find the percent ionization of a 0.337 M HF solution.The Ka for HF is 3.5 × 10-4.

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

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

Calculate the concentration of bicarbonate ion,HCO3-,in a 0.010 M H2CO3 solution that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Which Br∅nsted-Lowry acid is NOT considered to be a strong acid in water?

Determine the [H3O⁺] in a 0.265 M HClO solution.The Ka of HClO is 2.9 × 10-8.

Which one of the following will form an acidic solution in water?

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

Determine the pH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 × 10-5.

What is the pH of a 0.30 M pyridine solution that has Kb = 1.9 × 10-9? The equation for the dissociation of pyridine is: C5H5N(aq)+ H2O(l)⇌ C5H5NH+(aq)+ OH-(aq)

Calculate the pH of a 1.60 M KBrO solution.Ka for hypobromous acid,HBrO,is

Identify the substance that is NOT acidic.

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.

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Chemical Quantities and Aqueous Reactions

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Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

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Filters

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

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

Find the percent ionization of a 0.337 M HF solution.The K_a for HF is 3.5 × 10^-4.

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

Calculate the concentration of bicarbonate ion,HCO₃^-,in a 0.010 M H₂CO₃ solution that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

Determine the [H₃O⁺] in a 0.265 M HClO solution.The K_a of HClO is 2.9 × 10^-8.

Which of the following bases is the strongest? The base is followed by its K_bvalue.

Determine the pH of a 0.461 M C₆H₅CO₂H M solution if the K_a of C₆H₅CO₂H is 6.5 × 10^-5.

What is the pH of a 0.30 M pyridine solution that has K_b = 1.9 × 10^-9? The equation for the dissociation of pyridine is: C₅H₅N(aq)+ H₂O(l)⇌ C₅H₅NH⁺(aq)+ OH^-(aq)

Calculate the pH of a 1.60 M KBrO solution.K_a for hypobromous acid,HBrO,is

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.