Question 1

What is the pH of 3.9×10 - 4 M HNO3?

Accepted Answer

A)  - 3.40 
B)  0.03 
C)  3.41 
D)  3.51 
E)  none of these 
A)  - 3.40 
B)  0.03 
C)  3.41 
D)  3.51 
E)  none of these

Question 2

Which of the following salts is(are) considered basic when dissolved in water?
I. NaNO3
II. K3PO4
III. NH4Cl

Accepted Answer

A)  I only 
B)  II only 
C)  I and II 
D)  I and III 
E)  II and III 
A)  I only 
B)  II only 
C)  I and II 
D)  I and III 
E)  II and III

Question 3

A famous brand of sweet and sour barbecue sauce (consisting of tomato paste, water, vinegar, sugar, and secret spices) has a measured pH of 2.6. What is the hydrogen ion concentration in the sauce?

Accepted Answer

A)  0.42 M 
B)  2.4×10 - 2 M 
C)  2.5×10 - 3 M 
D)  3.4×10 - 4 M 
E)  5×10 - 5 M 
A)  0.42 M 
B)  2.4×10 - 2 M 
C)  2.5×10 - 3 M 
D)  3.4×10 - 4 M 
E)  5×10 - 5 M

Question 4

Rank the following three acids in terms of acid strength given the following information:
Acid K a p K a HF 6.9×10 - 4 -- CH3COOH -- 4.74 HNO2 4.5×10 - 4

Accepted Answer

A)  (weakest acid) HF 3COOH 2 (strongest acid) 
B)  (weakest acid) CH3COOH 2 2 3COOH (strongest acid) 
D)  (weakest acid) HF 2 3COOH (strongest acid) 
E)  (weakest acid) HNO2 3COOH < HF (strongest acid) 
A)  (weakest acid) HF 3COOH 2 (strongest acid) 
B)  (weakest acid) CH3COOH 2 2 3COOH (strongest acid) 
D)  (weakest acid) HF 2 3COOH (strongest acid) 
E)  (weakest acid) HNO2 3COOH < HF (strongest acid)

Question 5

Exhibit 15-4 Consider dissolving NaF in water as shown in the equation below to answer the following question(s):
NaF (s) + H₂ O (   )   HF (aq) + NaOH (aq)
-Refer to Exhibit 15-4. What is the pH of this 0.100 M NaF solution?

Accepted Answer

A)  pH = 2.08 
B)  pH = 5.91 
C)  pH = 8.08 
D)  pH = 11.83 
E)  pH = 11.92 
A)  pH = 2.08 
B)  pH = 5.91 
C)  pH = 8.08 
D)  pH = 11.83 
E)  pH = 11.92

Question 6

What is the pH of an aqueous 0.50 M KCN solution?
K a(HCN) = 6.2×10 - 10

Accepted Answer

A)  pH = 2.55 
B)  pH = 3.81 
C)  pH = 4.75 
D)  pH = 9.25 
E)  pH = 11.45 
A)  pH = 2.55 
B)  pH = 3.81 
C)  pH = 4.75 
D)  pH = 9.25 
E)  pH = 11.45

Question 7

The pH of a 1.00 liter solution of the weak base nicotine ( K b = 1.05×10 - 6) is 10.20.
How many moles of nicotine were dissolved to form this solution?

Accepted Answer

A)  0.10 
B)  3.8×10 - 15 
C)  2.4×10 - 2 
D)  1.05×10 - 3 
E)  2.4×10 - 4 
A)  0.10 
B)  3.8×10 - 15 
C)  2.4×10 - 2 
D)  1.05×10 - 3 
E)  2.4×10 - 4

Question 8

The pH of a vinegar solution is 2.32. What is the hydronium ion concentration, [H3O+], for this solution?

Accepted Answer

A)  [H3O+] = 2.1×10 - 12 M 
B)  [H3O+] = 4.8×10 - 3 M 
C)  [H3O+] = 0.36 M 
D)  [H3O+] = 2.3 M 
E)  [H3O+] = 2.1×102 M 
A)  [H3O+] = 2.1×10 - 12 M 
B)  [H3O+] = 4.8×10 - 3 M 
C)  [H3O+] = 0.36 M 
D)  [H3O+] = 2.3 M 
E)  [H3O+] = 2.1×102 M

Question 9

Regarding acid strength, which of the following is not correctly assigned?

Accepted Answer

A)  (weaker acid) NH3 3 (stronger acid) 
B)  (weaker acid) H2PO41 -  3PO4 (stronger acid) 
C)  (weaker acid) HOBr 2 (stronger acid) 
D)  (weaker acid) H2S 3 (stronger acid) 
E)  (weaker acid) H2SeO4 2SO4 (stronger acid) 
A)  (weaker acid) NH3 3 (stronger acid) 
B)  (weaker acid) H2PO41 -  3PO4 (stronger acid) 
C)  (weaker acid) HOBr 2 (stronger acid) 
D)  (weaker acid) H2S 3 (stronger acid) 
E)  (weaker acid) H2SeO4 2SO4 (stronger acid)

Question 10

Consider the salt pyridinium acetate, [(C5H5NH+)(C2H3O21 - )],
That is derived from a combination of a weak acid , HC2H3O2, and a weak base , C5H5N,
As shown below.
C5H5N + HC2H3O2→[(C5H5NH+)(C2H3O21 - )] K b(C5H5N) = 1.7×10 - 9 and K a(HC2H3O2) = 1.8×10 - 5 Which statement listed below is true?

Accepted Answer

A)  This salt is neutral when dissolved in water. 
B)  This salt is acidic when dissolved in water. 
C)  This salt is basic when dissolved in water. 
D)  This salt can be either acidic or neutral depending upon its concentration in water. 
E)  This salt can be either basic or neutral depending upon its concentration in water. 
A)  This salt is neutral when dissolved in water. 
B)  This salt is acidic when dissolved in water. 
C)  This salt is basic when dissolved in water. 
D)  This salt can be either acidic or neutral depending upon its concentration in water. 
E)  This salt can be either basic or neutral depending upon its concentration in water.

Question 11

Which of the following substances would behave as a Lewis acid when combined with a substance such as H2O?
I. BeF2
II. Al3+
III. H+

Accepted Answer

A)  I only 
B)  II only 
C)  III only 
D)  I and II 
E)  All of these 
A)  I only 
B)  II only 
C)  III only 
D)  I and II 
E)  All of these

Question 12

What species are formed in the hydrolysis of KF with water ?
KF + H₂ O   ??

Accepted Answer

A)  KH + H2O + F -  
B)  H2 + K2O + F -  
C)  H3O+ + F -  
D)  H3O+ + KH + F -  
E)  HF + KOH 
A)  KH + H2O + F -  
B)  H2 + K2O + F -  
C)  H3O+ + F -  
D)  H3O+ + KH + F -  
E)  HF + KOH

Question 13

For the reaction CN - (aq) + H₂ O (   )   HCN (aq) + OH - (aq), one of the acid-base conjugate pairs is:

Accepted Answer

A)  HCN, H2O 
B)  HCN, CN -  
C)  H2O, CN -  
D)  HCN, OH -  
E)  CN - , OH -  
A)  HCN, H2O 
B)  HCN, CN -  
C)  H2O, CN -  
D)  HCN, OH -  
E)  CN - , OH -

Question 14

What is the pH of a 0.10 M HCN solution?
K a(HCN) = 4.9×10 - 10

Accepted Answer

A)  1.0 
B)  4.65 
C)  5.15 
D)  9.31 
E)  10.31 
A)  1.0 
B)  4.65 
C)  5.15 
D)  9.31 
E)  10.31

Question 15

After completing the following unfinished table, what is the order of increasing acid strength ?
Acid K a p K a Propanoic acid 1.3×10 - 5 Chlorous acid 1.96 Benzoic acid 6.3×10 - 5

Accepted Answer

A)  (weakest) Propanoic acid < Chlorous acid < Benzoic acid (strongest) 
B)  (weakest) Propanoic acid < Benzoic acid < Chlorous acid (strongest) 
C)  (weakest) Chlorous acid < Propanoic acid < Benzoic acid (strongest) 
D)  (weakest) Benzoic acid < Chlorous acid < Propanoic acid (strongest) 
E)  (weakest) Benzoic acid < Propanoic acid < Chlorous acid (strongest) 
A)  (weakest) Propanoic acid < Chlorous acid < Benzoic acid (strongest) 
B)  (weakest) Propanoic acid < Benzoic acid < Chlorous acid (strongest) 
C)  (weakest) Chlorous acid < Propanoic acid < Benzoic acid (strongest) 
D)  (weakest) Benzoic acid < Chlorous acid < Propanoic acid (strongest) 
E)  (weakest) Benzoic acid < Propanoic acid < Chlorous acid (strongest)

Question 16

What is the pH of aqueous 0.10 M HNO2?
K a(HNO2) = 4.5×10 - 4

Accepted Answer

A)  pH = 1.0 
B)  pH = 1.67 
C)  pH = 2.17 
D)  pH = 3.35 
E)  pH = 4.35 
A)  pH = 1.0 
B)  pH = 1.67 
C)  pH = 2.17 
D)  pH = 3.35 
E)  pH = 4.35

Question 17

What is the Calcium hydroxide concentration, [Ca(OH)2], of an aqueous Ca(OH)2 solution with a pH = 9.60?

Accepted Answer

A)  1.3×10 - 10 M 
B)  2.5×10 - 10 M 
C)  2.0×10 - 5 M 
D)  4.0×10 - 5 M 
E)  8.0×10 - 5 M 
A)  1.3×10 - 10 M 
B)  2.5×10 - 10 M 
C)  2.0×10 - 5 M 
D)  4.0×10 - 5 M 
E)  8.0×10 - 5 M

Question 18

A weak monoprotic acid is dissolved in water. A solution that is 0.10 M is found to be 1.2% ionized. Calculate K a for the acid.

Accepted Answer

A)  1.4×10 - 5 
B)  1.2×10 - 3 
C)  1.1×10 - 2 
D)  0.12 
E)  12 
A)  1.4×10 - 5 
B)  1.2×10 - 3 
C)  1.1×10 - 2 
D)  0.12 
E)  12

Question 19

A solution of KOH is found to have [OH - ] = 0.010 M. What is the pH of this solution?

Accepted Answer

A)  14.0 
B)  12.0 
C)  2.0 
D)  13.0 
E)  1.0 
A)  14.0 
B)  12.0 
C)  2.0 
D)  13.0 
E)  1.0

Question 20

Which of the following is considered a weak acid when dissolved in water?
I. HNO2
II. HF
III. H2SO3

Accepted Answer

A)  I only 
B)  II only 
C)  III only 
D)  All of these 
E)  None of these 
A)  I only 
B)  II only 
C)  III only 
D)  All of these 
E)  None of these

Exam 15: Solutions of Acids and Bases

What is the pH of 3.9×10 - 4 M HNO3?

Which of the following salts is(are) considered basic when dissolved in water? I. NaNO3 II. K3PO4 III. NH4Cl

A famous brand of sweet and sour barbecue sauce (consisting of tomato paste, water, vinegar, sugar, and secret spices) has a measured pH of 2.6. What is the hydrogen ion concentration in the sauce?

Rank the following three acids in terms of acid strength given the following information: Acid K a p K a HF 6.9×10 - 4 -- CH3COOH -- 4.74 HNO2 4.5×10 - 4

Exhibit 15-4 Consider dissolving NaF in water as shown in the equation below to answer the following question(s): NaF (s) + H₂ O ( ) HF (aq) + NaOH (aq) -Refer to Exhibit 15-4. What is the pH of this 0.100 M NaF solution?

What is the pH of an aqueous 0.50 M KCN solution? K a(HCN) = 6.2×10 - 10

The pH of a 1.00 liter solution of the weak base nicotine ( K b = 1.05×10 - 6) is 10.20. How many moles of nicotine were dissolved to form this solution?

The pH of a vinegar solution is 2.32. What is the hydronium ion concentration, [H3O+], for this solution?

Regarding acid strength, which of the following is not correctly assigned?

Which of the following substances would behave as a Lewis acid when combined with a substance such as H2O? I. BeF2 II. Al3+ III. H+

What species are formed in the hydrolysis of KF with water ? KF + H₂ O ??

For the reaction CN - (aq) + H₂ O ( ) HCN (aq) + OH - (aq), one of the acid-base conjugate pairs is:

What is the pH of a 0.10 M HCN solution? K a(HCN) = 4.9×10 - 10

After completing the following unfinished table, what is the order of increasing acid strength ? Acid K a p K a Propanoic acid 1.3×10 - 5 Chlorous acid 1.96 Benzoic acid 6.3×10 - 5

What is the pH of aqueous 0.10 M HNO2? K a(HNO2) = 4.5×10 - 4

What is the Calcium hydroxide concentration, [Ca(OH)2], of an aqueous Ca(OH)2 solution with a pH = 9.60?

A weak monoprotic acid is dissolved in water. A solution that is 0.10 M is found to be 1.2% ionized. Calculate K a for the acid.

A solution of KOH is found to have [OH - ] = 0.010 M. What is the pH of this solution?

Which of the following is considered a weak acid when dissolved in water? I. HNO2 II. HF III. H2SO3

Introduction to Chemistry

Atoms, Molecules, and Ions

Equations, the Mole, and Chemical Formulas

Chemical Reactions in Solution

Thermochemistry

The Gaseous State

Electronic Structure

The Periodic Table: Structure and Trends

Chemical Bonds

Molecular Structure and Bonding Theories

Liquids and Solids

Solutions

Chemical Kinetics

Chemical Equilibrium

Reactions Between Acids and Bases

Chemical Thermodynamics

Electrochemistry

Transition Metals, Coordination Chemistry and Metallurgy

The Chemistry of Hydrogen, Elements in Groups 3A Through 6A, and the Noble Gases

Nuclear Chemistry

Organic Chemistry and Biochemistry

Filters

What is the pH of 3.9×10^{- 4} M HNO₃?

Which of the following salts is(are) considered basic when dissolved in water? I. NaNO₃ II. K₃PO₄ III. NH₄Cl

Rank the following three acids in terms of acid strength given the following information: Acid K _a p K _a HF 6.9×10^{- 4} -- CH₃COOH -- 4.74 HNO₂ 4.5×10^{- 4}

What is the pH of an aqueous 0.50 M KCN solution? K _a(HCN) = 6.2×10^{- 10}

The pH of a 1.00 liter solution of the weak base nicotine ( K _b = 1.05×10^{- 6}) is 10.20. How many moles of nicotine were dissolved to form this solution?

The pH of a vinegar solution is 2.32. What is the hydronium ion concentration, [H₃O⁺], for this solution?

Which of the following substances would behave as a Lewis acid when combined with a substance such as H₂O? I. BeF₂ II. Al³⁺ III. H⁺

What is the pH of a 0.10 M HCN solution? K _a(HCN) = 4.9×10^{- 10}

After completing the following unfinished table, what is the order of increasing acid strength ? Acid K _a p K _a Propanoic acid 1.3×10^{- 5} Chlorous acid 1.96 Benzoic acid 6.3×10^{- 5}

What is the pH of aqueous 0.10 M HNO₂? K _a(HNO₂) = 4.5×10^{- 4}

What is the Calcium hydroxide concentration, [Ca(OH)₂], of an aqueous Ca(OH)₂ solution with a pH = 9.60?

A weak monoprotic acid is dissolved in water. A solution that is 0.10 M is found to be 1.2% ionized. Calculate K _a for the acid.

A solution of KOH is found to have [OH^-] = 0.010 M. What is the pH of this solution?

Which of the following is considered a weak acid when dissolved in water? I. HNO₂ II. HF III. H₂SO₃