Question 1

Which of the following is the conjugate base of H2PO4−?

Accepted Answer

A)  H3PO4 
B)  HPO42− 
C)  PO43− 
D)  OH− 
A)  H3PO4 
B)  HPO42− 
C)  PO43− 
D)  OH−

Question 2

Examine the activity series given below.   Which of the following elements would be the least likely to release hydrogen gas (H2) upon reaction with water or acid?

Accepted Answer

A)  Ag 
B)  Ni 
C)  Al 
D)  Mg 
A)  Ag 
B)  Ni 
C)  Al 
D)  Mg

Question 3

Which of the following must be increased in order to increase the pH of a buffer made using acetic acid and sodium acetate?

Accepted Answer

A)  the amount of water present 
B)  [C2H3O2−] 
C)  [HC2H3O2] 
D)  both [C2H3O2−] and [HC2H3O2] 
A)  the amount of water present 
B)  [C2H3O2−] 
C)  [HC2H3O2] 
D)  both [C2H3O2−] and [HC2H3O2]

Question 4

Which of the following appears in the numerator of the fractional term of the Henderson-Hasselbalch equation?

Accepted Answer

A)  the weight of the conjugate base 
B)  the weight of the weak acid 
C)  the concentration of the conjugate base 
D)  the concentration of the weak acid 
A)  the weight of the conjugate base 
B)  the weight of the weak acid 
C)  the concentration of the conjugate base 
D)  the concentration of the weak acid

Question 5

Which of the following will determine the pH of a buffer made using acetic acid and sodium acetate?

Accepted Answer

A)  the amount of water present 
B)  the amount of C2H3O2− present 
C)  the amount of HC2H3O2 produced 
D)  the ratio of [C2H3O2−]/[HC2H3O2] 
A)  the amount of water present 
B)  the amount of C2H3O2− present 
C)  the amount of HC2H3O2 produced 
D)  the ratio of [C2H3O2−]/[HC2H3O2]

Question 6

In a particular titration experiment, a 25.0-mL sample of an unknown monoprotic acid required 30.0 mL of 0.200 M NaOH for the end point to be reached. Which of the following can be determined from the information given here?

Accepted Answer

A)  the identity of the acid sample 
B)  the pH of the acid sample 
C)  the strength of the acid sample 
D)  none of these 
A)  the identity of the acid sample 
B)  the pH of the acid sample 
C)  the strength of the acid sample 
D)  none of these

Question 7

An ammonia solution has a pH of 8.30. What is its [OH−]?

Accepted Answer

A)  5.0 × 10−23 M 
B)  2.0 × 10− 6 M 
C)  5.0 × 10−9 M 
D)  2.0 × 108 M 
A)  5.0 × 10−23 M 
B)  2.0 × 10− 6 M 
C)  5.0 × 10−9 M 
D)  2.0 × 108 M

Question 8

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

Accepted Answer

A)  The metal is reduced. 
B)  The water is oxidized. 
C)  The metal is reduced and the water is oxidized. 
D)  None of these. 
A)  The metal is reduced. 
B)  The water is oxidized. 
C)  The metal is reduced and the water is oxidized. 
D)  None of these.

Question 9

Which of the following is the relationship between pH and pOH?

Accepted Answer

A)  pH × pOH = 14 
B)  pH/pOH = 14 
C)  pH + pOH = 14 
D)  pH - pOH = 14 
A)  pH × pOH = 14 
B)  pH/pOH = 14 
C)  pH + pOH = 14 
D)  pH - pOH = 14

Question 10

Which of the following is the numerical value of the Kw of pure water at room temperature?

Accepted Answer

A)  1.0 × 10−14 
B)  1.0 × 10−7 
C)  1.0 × 107 
D)  1.0 × 1014 
A)  1.0 × 10−14 
B)  1.0 × 10−7 
C)  1.0 × 107 
D)  1.0 × 1014

Question 11

Which of the following is the conjugate acid of ammonia, NH3?

Accepted Answer

A)  H+ 
B)  H3O+ 
C)  NH2− 
D)  NH4+ 
A)  H+ 
B)  H3O+ 
C)  NH2− 
D)  NH4+

Question 12

What is the concentration of hydroxide ions in pure water at room temperature?

Accepted Answer

A)  1.0 × 10−14 M 
B)  1.0 × 10−7 M 
C)  1.0 × 107 M 
D)  1.0 × 1014 M 
A)  1.0 × 10−14 M 
B)  1.0 × 10−7 M 
C)  1.0 × 107 M 
D)  1.0 × 1014 M

Question 13

Which of the following appears in the denominator of the fractional term of the Henderson-Hasselbalch equation?

Accepted Answer

A)  the weight of the conjugate base 
B)  the weight of the weak acid 
C)  the concentration of the conjugate base 
D)  the concentration of the weak acid 
A)  the weight of the conjugate base 
B)  the weight of the weak acid 
C)  the concentration of the conjugate base 
D)  the concentration of the weak acid

Question 14

Which of the following can be characterized as a strong acid?

Accepted Answer

A)  0.001 M HCl 
B)  3.0 M HCl 
C)  both 0.001 M HCI and 3.0 HCI 
D)  neither 0.001 M HCI or 3.0 HCI 
A)  0.001 M HCl 
B)  3.0 M HCl 
C)  both 0.001 M HCI and 3.0 HCI 
D)  neither 0.001 M HCI or 3.0 HCI

Question 15

Given the following information, which of these acids is the weakest? Ka of boric acid is 7.3 × 10−10.
PKa of acetic acid is 4.75.
Ka of lactic acid is 8.4 × 10−4.
PKa of phenol is 9.89.

Accepted Answer

A)  acetic acid 
B)  formic acid 
C)  lactic acid 
D)  phenol 
A)  acetic acid 
B)  formic acid 
C)  lactic acid 
D)  phenol

Question 16

Which of the following is not true of pH indicators?

Accepted Answer

A)  They all change color at pH = 7. 
B)  Their colors are different in acidic solutions and in basic solutions. 
C)  They can be papers that have been soaked in specific compounds. 
D)  None of these, all the statements are true. 
A)  They all change color at pH = 7. 
B)  Their colors are different in acidic solutions and in basic solutions. 
C)  They can be papers that have been soaked in specific compounds. 
D)  None of these, all the statements are true.

Question 17

Which of the following is true of the equivalence point of an acid-base titration? It is the point where a pH indicator changes color.

Accepted Answer

A)  It is the point where equal volumes of the reactants have been used. 
B)  It is the point where the acid and base have been added in proper stoichiometric amounts. 
C)  It is the point where a pH indicator changes color. 
D)  None of these is true. 
A)  It is the point where equal volumes of the reactants have been used. 
B)  It is the point where the acid and base have been added in proper stoichiometric amounts. 
C)  It is the point where a pH indicator changes color. 
D)  None of these is true.

Question 18

Which of the following is found in baking powder but not in baking soda?

Accepted Answer

A)  NaHCO3(s) 
B)  KH2PO4(s) 
C)  both NaHCO3(s) and KH2PO4(s) 
D)  none of these 
A)  NaHCO3(s) 
B)  KH2PO4(s) 
C)  both NaHCO3(s) and KH2PO4(s) 
D)  none of these

Question 19

Which of the following is true of the indicator methyl orange?

Accepted Answer

A)  It is orange in acidic solutions. 
B)  It is orange in neutral solutions 
C)  It is orange in neutral solutions. 
D)  It changes color from red to yellow. 
A)  It is orange in acidic solutions. 
B)  It is orange in neutral solutions 
C)  It is orange in neutral solutions. 
D)  It changes color from red to yellow.

Question 20

In an aqueous solution, [OH−] is 1.0 × 10−6 M. What is [H+]?

Accepted Answer

A)  1.0 × 10−9 M 
B)  1.0 × 10−8 M 
C)  1.0 × 10− 6 M 
D)  1.0 × 108 M 
A)  1.0 × 10−9 M 
B)  1.0 × 10−8 M 
C)  1.0 × 10− 6 M 
D)  1.0 × 108 M

Exam 8: Acids and Bases

Which of the following is the conjugate base of H2PO4−?

Examine the activity series given below. Which of the following elements would be the least likely to release hydrogen gas (H2) upon reaction with water or acid?

Which of the following must be increased in order to increase the pH of a buffer made using acetic acid and sodium acetate?

Which of the following appears in the numerator of the fractional term of the Henderson-Hasselbalch equation?

Which of the following will determine the pH of a buffer made using acetic acid and sodium acetate?

In a particular titration experiment, a 25.0-mL sample of an unknown monoprotic acid required 30.0 mL of 0.200 M NaOH for the end point to be reached. Which of the following can be determined from the information given here?

An ammonia solution has a pH of 8.30. What is its [OH−]?

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

Which of the following is the relationship between pH and pOH?

Which of the following is the numerical value of the Kw of pure water at room temperature?

Which of the following is the conjugate acid of ammonia, NH3?

What is the concentration of hydroxide ions in pure water at room temperature?

Which of the following appears in the denominator of the fractional term of the Henderson-Hasselbalch equation?

Which of the following can be characterized as a strong acid?

Given the following information, which of these acids is the weakest? Ka of boric acid is 7.3 × 10−10. PKa of acetic acid is 4.75. Ka of lactic acid is 8.4 × 10−4. PKa of phenol is 9.89.

Which of the following is not true of pH indicators?

Which of the following is true of the equivalence point of an acid-base titration? It is the point where a pH indicator changes color.

Which of the following is found in baking powder but not in baking soda?

Which of the following is true of the indicator methyl orange?

In an aqueous solution, [OH−] is 1.0 × 10−6 M. What is [H+]?

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Which of the following is the conjugate base of H₂PO₄⁻?

Examine the activity series given below. Which of the following elements would be the least likely to release hydrogen gas (H₂) upon reaction with water or acid?

An ammonia solution has a pH of 8.30. What is its [OH⁻]?

Which of the following is the numerical value of the K_w of pure water at room temperature?

Which of the following is the conjugate acid of ammonia, NH₃?

Given the following information, which of these acids is the weakest? K_a of boric acid is 7.3 × 10⁻¹⁰. PK_a of acetic acid is 4.75. K_a of lactic acid is 8.4 × 10⁻⁴. PK_a of phenol is 9.89.

In an aqueous solution, [OH⁻] is 1.0 × 10⁻⁶ M. What is [H⁺]?