Question 1

A 25.0 mL sample of an HCl solution is titrated with a 0.139 M NaOH solution. The equivalence point is reached with 15.4 mL of base. The concentration of HCl is M.

Accepted Answer

A)   0.267
B)   0.0856
C)   0.00214
D)   0.139
E)   11.7 B

Question 2

Calculate the pH of a solution prepared by dissolving 0.750 mol of NH3 and 0.250 mol of NH4Cl in water sufficient to yield 1.00 L of solution. The Kb of ammonia is 1.77 × 10- 4.

Accepted Answer

A)   8.78
B)   0.89
C)   9.73
D)   4.27
E)   5.22 C

Question 3

Which below best describe(s) the behavior of an amphoteric hydroxide in water?

Accepted Answer

A)   With conc. aq. NaOH, its suspension dissolves.
B)   With conc. aq. HCl, its clear solution forms a precipitate.
C)   With conc. aq. HCl, its suspension dissolves.
D)   With both conc. aq. NaOH and conc. aq. HCl, its suspension dissolves.
E)   With conc. aq. NaOH, its clear solution forms a precipitate. D

Question 4

A 50.0 mL sample of an aqueous H2SO4 solution is titrated with a 0.375 M NaOH solution. The equivalence point is reached with 62.5 mL of the base. The concentration of H2SO4 is _ _ M.

Accepted Answer

A)   0.469
B)   0.234
C)   0.150
D)   0.300
E)   0.938

Question 5

In which of the following aqueous solutions would you expect AgBr to have the highest solubility?

Accepted Answer

A)   0.10 M AgNO3
B)   0.20 M NaBr
C)   0.10 M LiBr
D)   0.15 M KBr
E)   pure water

Question 6

For any buffer system, the buffer capacity depends on the amount of acid and base from which the buffer is made.

Accepted Answer

A) True 
 B)False

Question 7

A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba2+. When the concentration of F- exceeds M, BaF2 will precipitate. Neglect volume changes. For BaF2,
Ksp = 1.7 × 10- 6.

Accepted Answer

A)   1.1 × 10- 2 
B)   1.2 × 10- 4 
C)   2.4 × 10- 8 
D)   2.7 × 10- 3 
E)   5.9 × 10- 5

Question 8

Human blood is .

Accepted Answer

A)   slightly acidic
B)   slightly basic
C)   very basic
D)   very acidic
E)   neutral

Question 9

Calculate the pH of a solution prepared by dissolving 0.150 mol of benzoic acid (HBz) and
0)300 mol of sodium benzoate in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.50 × 10- 5.

Accepted Answer

A)   2.51
B)   4.19
C)   4.49
D)   3.89
E)   10.1

Question 10

Calculate the pH of a buffer that contains 0.270 M hydrofluoric acid (HF) and 0.180 M cesium fluoride (CsF). The Ka of hydrofluoric acid is 6.80 × 10^-⁴.

Accepted Answer

The answer of Calculate the pH of a buffer that...

Question 11

Which one of the following pairs cannot be mixed together to form a buffer solution?

Accepted Answer

A)   RbOH, HBr
B)   KOH, HF
C)   H3PO4, KH2PO4
D)   NaC2H3O2, HCl (C2H3O2- = acetate) 
E)   NH3, NH4Cl

Question 12

A 25.0 mL sample of 0.150 M nitrous acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The Ka of nitrous acid is 4.50 × 10- 4.

Accepted Answer

A)   3.35
B)   7.00
C)   8.11
D)   10.35
E)   10.65

Question 13

Of the following solutions, which has the greatest buffering capacity?

Accepted Answer

A)   0.100 M HF and 0.217 M NaF
B)   0.821 M HF and 0.909 M NaF
C)   0.821 M HF and 0.217 M NaF
D)   They are all buffer solutions and would all have the same capacity.
E)   0.121 M HF and 0.667 M NaF

Question 14

A 25.0- mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution. What is the pH before any base is added? The Ka of butanoic acid is 1.5 × 10- 5.

Accepted Answer

A)   1.0 × 104 
B)   1.5 × 10- 3 
C)   4.00
D)   2.83
E)   4.82

Question 15

The pH of a solution prepared by mixing 45 mL of 0.183 M KOH and 65 mL of 0.145 M HCl is
)

Accepted Answer

A)   70.145
B)   2.92
C)   0.74
D)   1.31
E)   1.97

Question 16

A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The concentration of the monoprotic acid is about mol/L.

Accepted Answer

A)   0.100
B)   0.120
C)   25.0
D)   0.0600
E)   0.240

Question 17

In which of the following aqueous solutions would you expect AgBr to have the lowest solubility?

Accepted Answer

A)   0.20 M NaBr
B)   0.10 M LiBr
C)   0.15 M KBr
D)   pure water
E)   0.10 M AgNO3

Question 18

The molar solubility of _ is not affected by the pH of the solution.

Accepted Answer

A)   Na3PO4 
B)   AlCl3 
C)   NaF
D)   KNO3 
E)   MnS

Question 19

Which of the following could be added to a solution of potassium fluoride to prepare a buffer?

Accepted Answer

A)   ammonia
B)   hydrochloric acid
C)   sodium hydroxide
D)   sodium fluoride
E)   potassium acetate

Question 20

Which of the following could be added to a solution of acetic acid to prepare a buffer? sodium acetate sodium hydroxide nitric acid hydrofluoric acid

Accepted Answer

A)   nitric acid only
B)   sodium acetate only
C)   sodium hydroxide only
D)   sodium acetate or sodium hydroxide
E)   hydrofluoric acid or nitric acid

Exam 17: Additional Aspects of Equilibria

A 25.0 mL sample of an HCl solution is titrated with a 0.139 M NaOH solution. The equivalence point is reached with 15.4 mL of base. The concentration of HCl is M.

Calculate the pH of a solution prepared by dissolving 0.750 mol of NH₃and 0.250 mol of NH₄Cl in water sufficient to yield 1.00 L of solution. The K_bof ammonia is 1.77 × 10^-⁴.

Which below best describe(s) the behavior of an amphoteric hydroxide in water?

A 50.0 mL sample of an aqueous H₂SO₄solution is titrated with a 0.375 M NaOH solution. The equivalence point is reached with 62.5 mL of the base. The concentration of H₂SO₄is _ _ M.

In which of the following aqueous solutions would you expect AgBr to have the highest solubility?

For any buffer system, the buffer capacity depends on the amount of acid and base from which the buffer is made.

A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba²⁺. When the concentration of F^-exceeds M, BaF₂will precipitate. Neglect volume changes. For BaF₂, K_sp= 1.7 × 10^-⁶.

Human blood is .

Calculate the pH of a solution prepared by dissolving 0.150 mol of benzoic acid (HBz) and 0) 300 mol of sodium benzoate in water sufficient to yield 1.00 L of solution. The K_aof benzoic acid is 6.50 × 10^-⁵.

Calculate the pH of a buffer that contains 0.270 M hydrofluoric acid (HF) and 0.180 M cesium fluoride (CsF). The Ka of hydrofluoric acid is 6.80 × 10^-⁴.

Which one of the following pairs cannot be mixed together to form a buffer solution?

A 25.0 mL sample of 0.150 M nitrous acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The K_aof nitrous acid is 4.50 × 10^-⁴.

Of the following solutions, which has the greatest buffering capacity?

A 25.0- mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution. What is the pH before any base is added? The K_aof butanoic acid is 1.5 × 10^-⁵.

The pH of a solution prepared by mixing 45 mL of 0.183 M KOH and 65 mL of 0.145 M HCl is )

A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The concentration of the monoprotic acid is about mol/L.

In which of the following aqueous solutions would you expect AgBr to have the lowest solubility?

The molar solubility of _ is not affected by the pH of the solution.

Which of the following could be added to a solution of potassium fluoride to prepare a buffer?

Which of the following could be added to a solution of acetic acid to prepare a buffer? sodium acetate sodium hydroxide nitric acid hydrofluoric acid

Exam 17: Additional Aspects of Equilibria

A 25.0 mL sample of an HCl solution is titrated with a 0.139 M NaOH solution. The equivalence point is reached with 15.4 mL of base. The concentration of HCl is M.

Calculate the pH of a solution prepared by dissolving 0.750 mol of NH3 and 0.250 mol of NH4Cl in water sufficient to yield 1.00 L of solution. The Kb of ammonia is 1.77 × 10- 4.

Which below best describe(s) the behavior of an amphoteric hydroxide in water?

A 50.0 mL sample of an aqueous H2SO4 solution is titrated with a 0.375 M NaOH solution. The equivalence point is reached with 62.5 mL of the base. The concentration of H2SO4 is _ _ M.

In which of the following aqueous solutions would you expect AgBr to have the highest solubility?

For any buffer system, the buffer capacity depends on the amount of acid and base from which the buffer is made.

A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba2+. When the concentration of F- exceeds M, BaF2 will precipitate. Neglect volume changes. For BaF2, Ksp = 1.7 × 10- 6.

Human blood is .

Calculate the pH of a solution prepared by dissolving 0.150 mol of benzoic acid (HBz) and 0) 300 mol of sodium benzoate in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.50 × 10- 5.

Calculate the pH of a buffer that contains 0.270 M hydrofluoric acid (HF) and 0.180 M cesium fluoride (CsF). The Ka of hydrofluoric acid is 6.80 × 10- 4.

Which one of the following pairs cannot be mixed together to form a buffer solution?

A 25.0 mL sample of 0.150 M nitrous acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The Ka of nitrous acid is 4.50 × 10- 4.

Of the following solutions, which has the greatest buffering capacity?

A 25.0- mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution. What is the pH before any base is added? The Ka of butanoic acid is 1.5 × 10- 5.

The pH of a solution prepared by mixing 45 mL of 0.183 M KOH and 65 mL of 0.145 M HCl is )

A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The concentration of the monoprotic acid is about mol/L.

In which of the following aqueous solutions would you expect AgBr to have the lowest solubility?

The molar solubility of _ is not affected by the pH of the solution.

Which of the following could be added to a solution of potassium fluoride to prepare a buffer?

Which of the following could be added to a solution of acetic acid to prepare a buffer? sodium acetate sodium hydroxide nitric acid hydrofluoric acid

Calculate the pH of a solution prepared by dissolving 0.750 mol of NH₃and 0.250 mol of NH₄Cl in water sufficient to yield 1.00 L of solution. The K_bof ammonia is 1.77 × 10^-⁴.

A 50.0 mL sample of an aqueous H₂SO₄solution is titrated with a 0.375 M NaOH solution. The equivalence point is reached with 62.5 mL of the base. The concentration of H₂SO₄is _ _ M.

A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba²⁺. When the concentration of F^-exceeds M, BaF₂will precipitate. Neglect volume changes. For BaF₂, K_sp= 1.7 × 10^-⁶.

Calculate the pH of a solution prepared by dissolving 0.150 mol of benzoic acid (HBz) and 0) 300 mol of sodium benzoate in water sufficient to yield 1.00 L of solution. The K_aof benzoic acid is 6.50 × 10^-⁵.

Calculate the pH of a buffer that contains 0.270 M hydrofluoric acid (HF) and 0.180 M cesium fluoride (CsF). The Ka of hydrofluoric acid is 6.80 × 10^-⁴.

A 25.0 mL sample of 0.150 M nitrous acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The K_aof nitrous acid is 4.50 × 10^-⁴.

A 25.0- mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution. What is the pH before any base is added? The K_aof butanoic acid is 1.5 × 10^-⁵.