Question 1

Which of the following bases can accepted only one proton?

Accepted Answer

A)  NH3 
B)  CH3NH2 
C)  (CH3)2NH 
D)  all of them 
A)  NH3 
B)  CH3NH2 
C)  (CH3)2NH 
D)  all of them

Question 2

Which of the following solutions will require the most NaOH in a titration experiment? Assume complete neutralization.

Accepted Answer

A)  25 mL of 0.500 M HC2H3O2 
B)  25 mL of 0.250 M H2SO4 
C)  25 mL of 0.167 M H3PO4 
D)  They all require the same amount. 
A)  25 mL of 0.500 M HC2H3O2 
B)  25 mL of 0.250 M H2SO4 
C)  25 mL of 0.167 M H3PO4 
D)  They all require the same amount.

Question 3

Examine the activity series given below.  
-In the activity series shown, where are the strongest reducing agents located?

Accepted Answer

A)  near the top 
B)  near the middle 
C)  near the bottom 
D)  It depends on the oxidizing agent involved. 
A)  near the top 
B)  near the middle 
C)  near the bottom 
D)  It depends on the oxidizing agent involved.

Question 4

What is the name of the acid which dissociates to give the cyanide ion, CN-?

Accepted Answer

A)  cyanic acid 
B)  cyanidic acid 
C)  cyanous 
D)  hydrocyanic acid 
A)  cyanic acid 
B)  cyanidic acid 
C)  cyanous 
D)  hydrocyanic acid

Question 5

An HCl solution has a pH of 3.10, what is the [OH-] in this solution?

Accepted Answer

A)  7.9 × 10-18 M 
B)  1.3 × 10-11 M 
C)  7.9 × 10 4 M 
D)  1.3 × 103 M 
A)  7.9 × 10-18 M 
B)  1.3 × 10-11 M 
C)  7.9 × 10 4 M 
D)  1.3 × 103 M

Question 6

The pKa of acetic acid, HC2H3O2, is 4.75. What is the pH of a buffer in which [HC2H3O2] = 0.20 M and [NaC2H3O2] = 2.0 M?

Accepted Answer

A)  3.75 
B)  4.75 
C)  5.75 
D)  7.00 
A)  3.75 
B)  4.75 
C)  5.75 
D)  7.00

Question 7

Which of the following is true about buffers such as HEPES, TRIS, MOPS, etc.?

Accepted Answer

A)  The Henderson-Hasselbalch equation applies to them. 
B)  They consist of simple weak acids and bases. 
C)  They are less resistant to changes in temperature than are other buffers. 
D)  We can use them interchangeably because they all have the same pKa. 
A)  The Henderson-Hasselbalch equation applies to them. 
B)  They consist of simple weak acids and bases. 
C)  They are less resistant to changes in temperature than are other buffers. 
D)  We can use them interchangeably because they all have the same pKa.

Question 8

When solid sodium hydroxide is dissolved in water which of the following species is not present in the solution?

Accepted Answer

A)  NaOH(aq) 
B)  H2O(l) 
C)  OH-(aq) 
D)  None, they are all present. 
A)  NaOH(aq) 
B)  H2O(l) 
C)  OH-(aq) 
D)  None, they are all present.

Question 9

Which of the following is the conjugate base of acetic acid, CH3COOH?

Accepted Answer

A)  H3O+ 
B)  CH3COOH2+ 
C)  CH3COO- 
D)  OH- 
A)  H3O+ 
B)  CH3COOH2+ 
C)  CH3COO- 
D)  OH-

Question 10

Which of the following occurs when an acid reacts with an active metal?

Accepted Answer

A)  The metal is oxidized. 
B)  H+ is reduced. 
C)  both a and b 
D)  neither a nor b 
A)  The metal is oxidized. 
B)  H+ is reduced. 
C)  both a and b 
D)  neither a nor b

Question 11

When hydrogen chloride gas is dissolved in water which of the following species is not present in the solution?

Accepted Answer

A)  HCl(aq) 
B)  H2O(l) 
C)  Cl-(aq) 
D)  None, they are all present. 
A)  HCl(aq) 
B)  H2O(l) 
C)  Cl-(aq) 
D)  None, they are all present.

Question 12

Why does the label ammonium hydroxide on a bottle give a false impression about the bottle=s contents?

Accepted Answer

A)  There is a large amount of NH4+(aq) but only a small amount of OH-(aq). 
B)  There is a small amount of NH4+(aq) but only a large amount of OH-(aq). 
C)  There is a large amount of NH3(aq) but only small amount of OH-(aq). 
D)  None of the above, the label accurately describes the contents. 
A)  There is a large amount of NH4+(aq) but only a small amount of OH-(aq). 
B)  There is a small amount of NH4+(aq) but only a large amount of OH-(aq). 
C)  There is a large amount of NH3(aq) but only small amount of OH-(aq). 
D)  None of the above, the label accurately describes the contents.

Question 13

Which of the following solutions will require the most NaOH in a titration experiment?

Accepted Answer

A)  25 mL of 0.5 M HCl 
B)  25 mL of 0.5 M HCOOH 
C)  25 mL of 0.5 M HC2H3O2 
D)  They all require the same amount. 
A)  25 mL of 0.5 M HCl 
B)  25 mL of 0.5 M HCOOH 
C)  25 mL of 0.5 M HC2H3O2 
D)  They all require the same amount.

Question 14

The term "litmus test" is commonly used to mean a totally definitive test. In chemistry litmus is used as an acid-base indicator. Which of the following properly relates the chemical and common usages of the term "litmus test"?

Accepted Answer

A)  Common usage is correct because the litmus test definitively defines a substance as an acid or a base. 
B)  Common usage is correct because litmus dye changes color at pH = 7. 
C)  Common usage is incorrect because litmus dye changes color over a range, most of which is above pH = 7. 
D)  Common usage is incorrect because litmus dye changes color over a range, most of which is below pH = 7. 
A)  Common usage is correct because the litmus test definitively defines a substance as an acid or a base. 
B)  Common usage is correct because litmus dye changes color at pH = 7. 
C)  Common usage is incorrect because litmus dye changes color over a range, most of which is above pH = 7. 
D)  Common usage is incorrect because litmus dye changes color over a range, most of which is below pH = 7.

Question 15

When acetic acid is dissolved in water which of the following is true of the equilibrium which is established as represented below?

Accepted Answer

A)  It lies very far to the left. 
B)  It lies slightly to the left. 
C)  It lies very far to the right. 
D)  It lies slightly to the right. 
A)  It lies very far to the left. 
B)  It lies slightly to the left. 
C)  It lies very far to the right. 
D)  It lies slightly to the right.

Question 16

Examine the activity series given below.  
-Examine the following image. Assume the solution in the beaker is a buffer solution.   What is the pOH of the solution in the beaker?

Accepted Answer

A)  9.67 
B)  14.00 
C)  2.13 × 10-10 
D)  4.68 × 10-5 
A)  9.67 
B)  14.00 
C)  2.13 × 10-10 
D)  4.68 × 10-5

Question 17

Which of the following occurs when the weak base ammonia, NH3, is dissolved in water?

Accepted Answer

A)  A very small number of ammonia molecules break up. 
B)  A very small number of ammonia molecules take an H+ from the water. 
C)  A very small number of molecules of NH4OH are formed. 
D)  A very small number of water molecules take an H+ from ammonia. 
A)  A very small number of ammonia molecules break up. 
B)  A very small number of ammonia molecules take an H+ from the water. 
C)  A very small number of molecules of NH4OH are formed. 
D)  A very small number of water molecules take an H+ from ammonia.

Question 18

Which of the following gases is produced when an acid reacts with an active metal?

Accepted Answer

A)  CO2(g) 
B)  H(g) 
C)  H2(g) 
D)  H2O(g) 
A)  CO2(g) 
B)  H(g) 
C)  H2(g) 
D)  H2O(g)

Question 19

Which of the following is true of a buffer prepared with equal concentrations of an acid and its conjugate base?

Accepted Answer

A)  pH = 7 
B)  pH = pKa 
C)  The pH depends on the concentration of the buffer. 
D)  none of the above 
A)  pH = 7 
B)  pH = pKa 
C)  The pH depends on the concentration of the buffer. 
D)  none of the above

Question 20

A sodium hydroxide solution has a pH of 11.40, what is the [H3O+] in this solution?

Accepted Answer

A)  4.0 × 10-26 M 
B)  4.0 × 10-12 M 
C)  2.5 × 10-3 M 
D)  2.5 × 1011 M 
A)  4.0 × 10-26 M 
B)  4.0 × 10-12 M 
C)  2.5 × 10-3 M 
D)  2.5 × 1011 M

Exam 8: Acids and Bases

Which of the following bases can accepted only one proton?

Which of the following solutions will require the most NaOH in a titration experiment? Assume complete neutralization.

Examine the activity series given below. -In the activity series shown, where are the strongest reducing agents located?

What is the name of the acid which dissociates to give the cyanide ion, CN-?

An HCl solution has a pH of 3.10, what is the [OH-] in this solution?

The pKa of acetic acid, HC2H3O2, is 4.75. What is the pH of a buffer in which [HC2H3O2] = 0.20 M and [NaC2H3O2] = 2.0 M?

Which of the following is true about buffers such as HEPES, TRIS, MOPS, etc.?

When solid sodium hydroxide is dissolved in water which of the following species is not present in the solution?

Which of the following is the conjugate base of acetic acid, CH3COOH?

Which of the following occurs when an acid reacts with an active metal?

When hydrogen chloride gas is dissolved in water which of the following species is not present in the solution?

Why does the label ammonium hydroxide on a bottle give a false impression about the bottle=s contents?

Which of the following solutions will require the most NaOH in a titration experiment?

The term "litmus test" is commonly used to mean a totally definitive test. In chemistry litmus is used as an acid-base indicator. Which of the following properly relates the chemical and common usages of the term "litmus test"?

When acetic acid is dissolved in water which of the following is true of the equilibrium which is established as represented below?

Examine the activity series given below. -Examine the following image. Assume the solution in the beaker is a buffer solution. What is the pOH of the solution in the beaker?

Which of the following occurs when the weak base ammonia, NH3, is dissolved in water?

Which of the following gases is produced when an acid reacts with an active metal?

Which of the following is true of a buffer prepared with equal concentrations of an acid and its conjugate base?

A sodium hydroxide solution has a pH of 11.40, what is the [H3O+] in this solution?

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What is the name of the acid which dissociates to give the cyanide ion, CN^-?

An HCl solution has a pH of 3.10, what is the [OH^-] in this solution?

The pK_a of acetic acid, HC₂H₃O₂, is 4.75. What is the pH of a buffer in which [HC₂H₃O₂] = 0.20 M and [NaC₂H₃O₂] = 2.0 M?

Which of the following is the conjugate base of acetic acid, CH₃COOH?

Which of the following occurs when the weak base ammonia, NH₃, is dissolved in water?

A sodium hydroxide solution has a pH of 11.40, what is the [H₃O⁺] in this solution?