Question 1

Consider titrating a triprotic acid with standard NaOH as shown in the titration curve below.  What is the relationship between the first equivalence point and the third equivalence point in this titration curve?

Accepted Answer

A)   The pH of the first equivalence point is three times larger than the pH found at the third equivalence point.
B)   The pH of the first equivalence point is three times smaller than the pH found at the third equivalence point.
C)   The volume of titrant required to reach the third equivalence point is three times as large as the volume of titrant required to reach the first equivalence point.
D)   The volume of titrant required to reach the first equivalence point is three times as large as the volume of titrant required to reach the third equivalence point.
E)   There are no relationships between the first and third equivalence points. C

Question 2

Which of the following salts, each having very limited solubility in water, would dissolve to a greater extent upon acidifying the solution?
I. Fe(OH)3
II. AgCN
III. PbI2

Accepted Answer

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

Question 3

What is the pH of a solution that consists of 0.25 M HC2H3O2 and 0.35 M NaC2H3O2?
K a(HC2H3O2) = 1.8×10 - 5

Accepted Answer

A)   0.60
B)   4.60
C)   4.89
D)   5.50
E)   6.07 C

Question 4

What is the pH of a solution that is 0.100 M methylamine (CH3NH2) and 0.200 M methyl ammonium chloride (CH3NH3Cl)?
The K b of methylamine is 3.70×10 - 4.

Accepted Answer

A)   1.00
B)   3.73
C)   10.73
D)   3.43
E)   10.27

Question 5

Calculate the volume of 0.100 M HCl required to neutralize 1.00 g of Ba(OH)2 (molar mass = 171.3 g/mol).

Accepted Answer

A)   58.4 mL
B)   117 mL
C)   29.2 mL
D)   585 mL
E)   no reaction occurs

Question 6

Consider the buffer pair, HF/F - . What can be stated about the relative proportions of this buffer pair if the pH of an aqueous solution of this pair is adjusted tO4.00 and the p K a for HF equals 3.17?

Accepted Answer

A)   This buffer solution contains relatively more HF than F - .
B)   This buffer solution contains relatively more F - than HF.
C)   This buffer solution contains equal concentrations of HF and F - .
D)   More information is needed to determine the relative proportion of each member.

Question 7

A 20.0 mL sample of lactic acid (monoprotic with K a = 1.37×10 - 4) requires 30.0 mL of 0.200 M NaOH for titration to the equivalence point. What is the concentration of the lactic acid solution?

Accepted Answer

A)   0.120 M
B)   0.200 M
C)   0.300 M
D)   6.00×10 - 3 M
E)   cannot be found without the molar mass of lactic acid.

Question 8

A buffer solution maintains a constant pH level to a certain extent when a strong acid such as HCl is added. Which of the following buffer solutions has the greatest buffering capacity to consume added HCl?

Accepted Answer

A)   0.5 M HC2H3O2/0.5 M NaC2H3O2
B)   1.0 M HC2H3O2/0.5 M NaC2H3O2
C)   1.0 M HC2H3O2/1.5 M NaC2H3O2
D)   1.5 M HC2H3O2/1.0 M NaC2H3O2
E)   1.5 M HC2H3O2/0.5 M NaC2H3O2

Question 9

In the titration of 50.0 mL of a 0.100 M HCl solution with 0.100 M NaOH, what is the pH of the solution after the addition of 20.0 mL of the NaOH solution?

Accepted Answer

A)   1.00
B)   1.22
C)   1.15
D)   1.37
E)   12.63

Question 10

Which of the following titration curves listed below best represents a curve for the complete titration of oxalic acid, H2C2O4 (a diprotic acid), with a strong base such as NaOH?

Accepted Answer

A)   2C2O4 (a diprotic acid) , with a strong base such as NaOH? 
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Question 11

Exhibit 16-2 Consider titrating CHS1U1B13S1U1B0COOH with standard NaOH (delivered from the burette) to answer the following question(s).
-Refer to Exhibit 16-2. What compound(s) is(are) present in the region after the titration has begun but before the equivalence point?
I. CH3COOH
II. NaOH
III. CH3COO - Na+

Accepted Answer

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

Question 12

A 350 mL volume of 0.150 M Ba(OH)2 was completely neutralized by 35.0 mL of HCl. What is the molarity of the HCl solution?

Accepted Answer

A)   1.50 M
B)   3.00 M
C)   0.750 M
D)   1.00 M
E)   0.500 M

Question 13

A buffer is made by dissolving 0.10 mol of NaF in 1.00 L of 0.20 M HF. What is the pH of this buffer?
K a(HF) = 6.3×10 - 4

Accepted Answer

A)   1.05
B)   1.58
C)   3.16
D)   3.46
E)   3.70

Question 14

In the titration of 0.100 M HCl with the titrant 0.100 M NaOH, what species are present at any point after NaOH has been added but before the equivalence point?

Accepted Answer

A)   HCl only
B)   NaOH only
C)   NaCl only
D)   HCl and NaOH
E)   HCl and NaCl

Question 15

Which of the following titration curves listed below best represents a curve for the complete titration of the weakly basic dianion, sulfide, S2 - , with a strong acid such as HCl as shown below in the net ionic equation?
S2 -  (aq) + 2 HCl (aq)→H2S (g) + 2 Cl -

Accepted Answer

A)   2 - , with a strong acid such as HCl as shown below in the net ionic equation? S2 -  (aq)  + 2 HCl (aq) →H2S (g)  + 2 Cl -  
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Question 16

Calculate the number of moles of sodium acetate (CH3COONa) that must be added to 1.00 L of 0.100 M CH3COOH ( K a = 1.8×10 - 5) to give a buffer with pH5.00.

Accepted Answer

A)   1.0×10 - 5
B)   0.18
C)   0.057
D)   0.10
E)   0.20

Question 17

Calculate the pH of a solution after 10.0 mL of 0.100 M NaOH is added tO40.0 mL of 0.250 M HBr.

Accepted Answer

A)   0.65
B)   1.00
C)   - 1.0
D)   13.01
E)   0.74

Question 18

What is the pH of a buffer solution that consists of 0.25 M HClO2 and 0.75 M KClO2?
K a(HClO2) = 1.1×10 - 2

Accepted Answer

A)   pH = 1.48
B)   pH = 1.96
C)   pH = 2.44
D)   pH = 3.41
E)   pH = 5.61

Question 19

Which pair(s) of substances would make a suitable buffer pair ?
I. HCl and NaCl
II. HF and NaF
III. NH4Cl and NH3

Accepted Answer

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

Question 20

What is the pH of a solution prepared by mixing 0.250 mol of hydrazoic acid, HN3, and 0.500 mol of sodium azide, NaN3, to make 1.00 liter of solution?
( K a = 1.9×10 - 5)

Accepted Answer

A)   4.42
B)   5.02
C)   9.58
D)   4.72
E)   8.98

Exam 16: Reactions Between Acids and Bases

Consider titrating a triprotic acid with standard NaOH as shown in the titration curve below. What is the relationship between the first equivalence point and the third equivalence point in this titration curve?

Which of the following salts, each having very limited solubility in water, would dissolve to a greater extent upon acidifying the solution? I. Fe(OH) ₃ II. AgCN III. PbI₂

What is the pH of a solution that consists of 0.25 M HC₂H₃O₂ and 0.35 M NaC₂H₃O₂? K _a(HC₂H₃O₂) = 1.8×10^{- 5}

What is the pH of a solution that is 0.100 M methylamine (CH₃NH₂) and 0.200 M methyl ammonium chloride (CH₃NH₃Cl) ? The K _b of methylamine is 3.70×10^{- 4}.

Calculate the volume of 0.100 M HCl required to neutralize 1.00 g of Ba(OH) ₂ (molar mass = 171.3 g/mol) .

Consider the buffer pair, HF/F^-. What can be stated about the relative proportions of this buffer pair if the pH of an aqueous solution of this pair is adjusted tO₄.00 and the p K _a for HF equals 3.17?

A 20.0 mL sample of lactic acid (monoprotic with K _a = 1.37×10^{- 4}) requires 30.0 mL of 0.200 M NaOH for titration to the equivalence point. What is the concentration of the lactic acid solution?

A buffer solution maintains a constant pH level to a certain extent when a strong acid such as HCl is added. Which of the following buffer solutions has the greatest buffering capacity to consume added HCl?

In the titration of 50.0 mL of a 0.100 M HCl solution with 0.100 M NaOH, what is the pH of the solution after the addition of 20.0 mL of the NaOH solution?

Which of the following titration curves listed below best represents a curve for the complete titration of oxalic acid, H₂C₂O₄ (a diprotic acid) , with a strong base such as NaOH?

A 350 mL volume of 0.150 M Ba(OH) ₂ was completely neutralized by 35.0 mL of HCl. What is the molarity of the HCl solution?

A buffer is made by dissolving 0.10 mol of NaF in 1.00 L of 0.20 M HF. What is the pH of this buffer? K _a(HF) = 6.3×10^{- 4}

In the titration of 0.100 M HCl with the titrant 0.100 M NaOH, what species are present at any point after NaOH has been added but before the equivalence point?

Which of the following titration curves listed below best represents a curve for the complete titration of the weakly basic dianion, sulfide, S^{2 -}, with a strong acid such as HCl as shown below in the net ionic equation? S^{2 -} (aq) + 2 HCl (aq) →H₂S (g) + 2 Cl^-

Calculate the number of moles of sodium acetate (CH₃COONa) that must be added to 1.00 L of 0.100 M CH₃COOH ( K _a = 1.8×10^{- 5}) to give a buffer with pH₅.00.

Calculate the pH of a solution after 10.0 mL of 0.100 M NaOH is added tO₄0.0 mL of 0.250 M HBr.

What is the pH of a buffer solution that consists of 0.25 M HClO₂ and 0.75 M KClO₂? K _a(HClO₂) = 1.1×10^{- 2}

Which pair(s) of substances would make a suitable buffer pair ? I. HCl and NaCl II. HF and NaF III. NH₄Cl and NH₃

What is the pH of a solution prepared by mixing 0.250 mol of hydrazoic acid, HN₃, and 0.500 mol of sodium azide, NaN₃, to make 1.00 liter of solution? ( K _a = 1.9×10^{- 5})

Exam 16: Reactions Between Acids and Bases

Consider titrating a triprotic acid with standard NaOH as shown in the titration curve below. What is the relationship between the first equivalence point and the third equivalence point in this titration curve?

Which of the following salts, each having very limited solubility in water, would dissolve to a greater extent upon acidifying the solution? I. Fe(OH) 3 II. AgCN III. PbI2

What is the pH of a solution that consists of 0.25 M HC2H3O2 and 0.35 M NaC2H3O2? K a(HC2H3O2) = 1.8×10 - 5

What is the pH of a solution that is 0.100 M methylamine (CH3NH2) and 0.200 M methyl ammonium chloride (CH3NH3Cl) ? The K b of methylamine is 3.70×10 - 4.

Calculate the volume of 0.100 M HCl required to neutralize 1.00 g of Ba(OH) 2 (molar mass = 171.3 g/mol) .

Consider the buffer pair, HF/F - . What can be stated about the relative proportions of this buffer pair if the pH of an aqueous solution of this pair is adjusted tO4.00 and the p K a for HF equals 3.17?

A 20.0 mL sample of lactic acid (monoprotic with K a = 1.37×10 - 4) requires 30.0 mL of 0.200 M NaOH for titration to the equivalence point. What is the concentration of the lactic acid solution?

A buffer solution maintains a constant pH level to a certain extent when a strong acid such as HCl is added. Which of the following buffer solutions has the greatest buffering capacity to consume added HCl?

In the titration of 50.0 mL of a 0.100 M HCl solution with 0.100 M NaOH, what is the pH of the solution after the addition of 20.0 mL of the NaOH solution?

Which of the following titration curves listed below best represents a curve for the complete titration of oxalic acid, H2C2O4 (a diprotic acid) , with a strong base such as NaOH?

Exhibit 16-2 Consider titrating CH3COOH with standard NaOH (delivered from the burette) to answer the following question(s) . -Refer to Exhibit 16-2. What compound(s) is(are) present in the region after the titration has begun but before the equivalence point? I. CH3COOH II. NaOH III. CH3COO - Na+

A 350 mL volume of 0.150 M Ba(OH) 2 was completely neutralized by 35.0 mL of HCl. What is the molarity of the HCl solution?

A buffer is made by dissolving 0.10 mol of NaF in 1.00 L of 0.20 M HF. What is the pH of this buffer? K a(HF) = 6.3×10 - 4

In the titration of 0.100 M HCl with the titrant 0.100 M NaOH, what species are present at any point after NaOH has been added but before the equivalence point?

Which of the following titration curves listed below best represents a curve for the complete titration of the weakly basic dianion, sulfide, S2 - , with a strong acid such as HCl as shown below in the net ionic equation? S2 - (aq) + 2 HCl (aq) →H2S (g) + 2 Cl -

Calculate the number of moles of sodium acetate (CH3COONa) that must be added to 1.00 L of 0.100 M CH3COOH ( K a = 1.8×10 - 5) to give a buffer with pH5.00.

Calculate the pH of a solution after 10.0 mL of 0.100 M NaOH is added tO40.0 mL of 0.250 M HBr.

What is the pH of a buffer solution that consists of 0.25 M HClO2 and 0.75 M KClO2? K a(HClO2) = 1.1×10 - 2

Which pair(s) of substances would make a suitable buffer pair ? I. HCl and NaCl II. HF and NaF III. NH4Cl and NH3

What is the pH of a solution prepared by mixing 0.250 mol of hydrazoic acid, HN3, and 0.500 mol of sodium azide, NaN3, to make 1.00 liter of solution? ( K a = 1.9×10 - 5)

Which of the following salts, each having very limited solubility in water, would dissolve to a greater extent upon acidifying the solution? I. Fe(OH) ₃ II. AgCN III. PbI₂

What is the pH of a solution that consists of 0.25 M HC₂H₃O₂ and 0.35 M NaC₂H₃O₂? K _a(HC₂H₃O₂) = 1.8×10^{- 5}

What is the pH of a solution that is 0.100 M methylamine (CH₃NH₂) and 0.200 M methyl ammonium chloride (CH₃NH₃Cl) ? The K _b of methylamine is 3.70×10^{- 4}.

Calculate the volume of 0.100 M HCl required to neutralize 1.00 g of Ba(OH) ₂ (molar mass = 171.3 g/mol) .

Consider the buffer pair, HF/F^-. What can be stated about the relative proportions of this buffer pair if the pH of an aqueous solution of this pair is adjusted tO₄.00 and the p K _a for HF equals 3.17?

A 20.0 mL sample of lactic acid (monoprotic with K _a = 1.37×10^{- 4}) requires 30.0 mL of 0.200 M NaOH for titration to the equivalence point. What is the concentration of the lactic acid solution?

Which of the following titration curves listed below best represents a curve for the complete titration of oxalic acid, H₂C₂O₄ (a diprotic acid) , with a strong base such as NaOH?

A 350 mL volume of 0.150 M Ba(OH) ₂ was completely neutralized by 35.0 mL of HCl. What is the molarity of the HCl solution?

A buffer is made by dissolving 0.10 mol of NaF in 1.00 L of 0.20 M HF. What is the pH of this buffer? K _a(HF) = 6.3×10^{- 4}

Which of the following titration curves listed below best represents a curve for the complete titration of the weakly basic dianion, sulfide, S^{2 -}, with a strong acid such as HCl as shown below in the net ionic equation? S^{2 -} (aq) + 2 HCl (aq) →H₂S (g) + 2 Cl^-

Calculate the number of moles of sodium acetate (CH₃COONa) that must be added to 1.00 L of 0.100 M CH₃COOH ( K _a = 1.8×10^{- 5}) to give a buffer with pH₅.00.

Calculate the pH of a solution after 10.0 mL of 0.100 M NaOH is added tO₄0.0 mL of 0.250 M HBr.

What is the pH of a buffer solution that consists of 0.25 M HClO₂ and 0.75 M KClO₂? K _a(HClO₂) = 1.1×10^{- 2}

Which pair(s) of substances would make a suitable buffer pair ? I. HCl and NaCl II. HF and NaF III. NH₄Cl and NH₃

What is the pH of a solution prepared by mixing 0.250 mol of hydrazoic acid, HN₃, and 0.500 mol of sodium azide, NaN₃, to make 1.00 liter of solution? ( K _a = 1.9×10^{- 5})