Question 1

A solution containing which one of the following pairs of substances will be a buffer solution?

Accepted Answer

A)  KI, HI
B)  AgBr, HBr
C)  CuCl, HCl
D)  CsI, HI
E)  none of the aboveF) A) and D)
G) A) and B)

Question 2

Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of hydrogen fluoride after addition of 9.00 mL of 0.0100 M HCl to 25.0 mL of this solution is ________ M.

Accepted Answer

A)  0.0953
B)  0.0900
C)  0.130
D)  0.122
E)  0.00976F) C) and D)
G) B) and C)

Question 3

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

Accepted Answer

A)  0.040 M SrBr2
B)  pure water
C)  0.040 M NaBr
D)  0.040 M KBr
E)  0.010 M AgNO3F) None of the above
G) A) and C)

Question 4

Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.322 M in formic acid and 0.178 M in sodium formate (NaHCO2) . The Ka of formic acid is 1.77 × 10-4.

Accepted Answer

A)  35.6
B)  0.1011
C)  10.8
D)  1.03 × 10-3
E)  3.488F) None of the above
G) A) and D)

Question 5

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)  11.7
B)  0.00214
C)  0.0856
D)  0.267
E)  0.139F) A) and B)
G) A) and C)

Question 6

The concentration of fluoride ions in a saturated solution of barium fluoride is ________ M. The solubility product constant of BaF2 is 1.7 × 10-6.

Accepted Answer

A)  3.8 × 10-4
B)  3.0 × 10-3
C)  1.5 × 10-2
D)  7.5 × 10-3
E)  1.4 × 10-4F) A) and D)
G) A) and E)

Question 7

Calculate the percent ionization of nitrous acid in a solution that is 0.260 M in nitrous acid. The acid dissociation constant of nitrous acid is 4.50 × 10-4.

Accepted Answer

A)  1.17 × 10-4
B)  0.0450
C)  4.16
D)  0.314
E)  5.78F) None of the above
G) C) and D)

Question 8

Consider the following table of 3 B) Cd(OH) 2 C) CdCO3 D) AgI E) CaF2" class="answers-bank-image d-inline" rel="preload" > values. 3 B) Cd(OH) 2 C) CdCO3 D) AgI E) CaF2" class="answers-bank-image d-inline" rel="preload" >
-Which compound listed below has the smallest molar solubility in water?

Accepted Answer

A)  ZnCO3
B)  Cd(OH) 2
C)  CdCO3
D)  AgI
E)  CaF2F) A) and B)
G) B) and D)

Question 9

The solubility of manganese (II) hydroxide (Mn(OH) 2) is 2.2 × 10-5 M. What is the Ksp of Mn(OH) 2?

Accepted Answer

A)  1.1 × 10-14
B)  4.3 × 10-14
C)  2.1 × 10-14
D)  4.8 × 10-10
E)  2.2 × 10-5F) B) and C)
G) A) and B)

Question 10

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

Accepted Answer

A)  pure water
B)  0.050 M BaI2
C)  0.050 M NaI
D)  0.050 M KI
E)  0.010 M AgNO3F) A) and B)
G) All of the above

Question 11

What are the principal organs that regulate the pH of the carbonic acid-bicarbonate buffer system in the blood?

Accepted Answer

A)  kidneys, liver
B)  lungs, kidneys
C)  spleen, liver
D)  lungs, skin
E)  brain stem, heartF) C) and D)
G) A) and B)

Question 12

The concentration of iodide ions in a saturated solution of silver iodide is ________ M. The solubility product constant of AgI is 8.3 × 10-17.

Accepted Answer

A)  3.8 × 10-11
B)  3.0 × 10-10
C)  9.1 × 10-9
D)  3.5 × 10-9
E)  1.4 × 10-8F) All of the above
G) B) and D)

Question 13

Which of the following could be added to a solution of acetic acid to prepare a buffer?

Accepted Answer

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

Question 14

Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of fluoride ions after the addition of 9.00 mL of 0.0100 M HCl to 25.0 mL of this solution is ________ M.

Accepted Answer

A)  0.0735
B)  0.0762
C)  0.0980
D)  0.0709
E)  0.00253F) A) and E)
G) B) and E)

Question 15

Calculate the maximum concentration (in M) of silver ions (Ag+) in a solution that contains 0.025 M of CO32-. The Ksp of Ag2CO3 is 8.1 × 10-12.

Accepted Answer

A)  1.8 × 10-5
B)  1.4 × 10-6
C)  2.8 × 10-6
D)  3.2 × 10-10
E)  8.1 × 10-12F) B) and E)
G) A) and B)

Question 16

Calculate the pH of a solution prepared by dissolving 0.250 mol of benzoic acid (C7H5O2H) and 0.150 mol of sodium benzoate (NaC7H5O2) in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.50 × 10-5.

Accepted Answer

A)  4.409
B)  3.965
C)  10.035
D)  9.591
E)  5.190F) C) and D)
G) B) and E)

Question 17

The pH of a solution prepared by dissolving 0.350 mol of solid dimethylamine hydrochloride ((CH3) 2NH2Cl) in 1.00 L of 1.10 M dimethylamine ((CH3) 2NH) is ________. The Kb for methylamine is 5.40 × 10-4. (Assume the final volume is 1.00 L.)

Accepted Answer

A)  1.66
B)  2.77
C)  11.23
D)  11.14
E)  none of the aboveF) A) and E)
G) A) and D)

Question 18

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

Accepted Answer

A)  HONH2, HONH3Cl
B)  NaCl, HCl
C)  RbOH, HF
D)  KOH, HNO2
E)  H2SO3, KHSO3F) B) and E)
G) A) and B)

Question 19

What is the solubility (in M) of PbCl2 in a 0.15 M solution of HCl? The Ksp of PbCl2 is 1.6 × 10-5.

Accepted Answer

A)  2.0 × 10-3
B)  1.1 × 10-4
C)  1.8 × 10-4
D)  7.1 × 10-4
E)  1.6 × 10-5F) A) and E)
G) A) and D)

Question 20

Calculate the maximum concentration (in M) of magnesium ions (Mg+2) in a solution that contains 0.025 M of CO32-. The Ksp of MgCO3 is 3.5 × 10-8.

Accepted Answer

A)  1.8 × 10-5
B)  1.4 × 10-6
C)  2.8 × 10-6
D)  3.2 × 10-10
E)  8.1 × 10-12F) None of the above
G) A) and D)

Exam 17: Additional Aspects of Aqueous Equilibria

The pH of a solution prepared by dissolving 0.350 mol of solid dimethylamine hydrochloride ((CH3) 2NH2Cl) in 1.00 L of 1.10 M dimethylamine ((CH3) 2NH) is ________. The Kb for methylamine is 5.40 × 10-4. (Assume the final volume is 1.00 L.)

Correct AnswerverifiedShow Answer

Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of hydrogen fluoride after addition of 9.00 mL of 0.0100 M HCl to 25.0 mL of this solution is ________ M.

Correct AnswerverifiedShow Answer

Consider the following table of values. -Which compound listed below has the smallest molar solubility in water?

Correct AnswerverifiedShow Answer

A solution containing which one of the following pairs of substances will be a buffer solution?

Correct AnswerverifiedShow Answer

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.

Correct AnswerverifiedShow Answer

Calculate the percent ionization of nitrous acid in a solution that is 0.260 M in nitrous acid. The acid dissociation constant of nitrous acid is 4.50 × 10-4.

Correct AnswerverifiedShow Answer

The concentration of iodide ions in a saturated solution of silver iodide is ________ M. The solubility product constant of AgI is 8.3 × 10-17.

Correct AnswerverifiedShow Answer

Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride. The concentration of fluoride ions after the addition of 9.00 mL of 0.0100 M HCl to 25.0 mL of this solution is ________ M.

Correct AnswerverifiedShow Answer

Calculate the maximum concentration (in M) of silver ions (Ag+) in a solution that contains 0.025 M of CO32-. The Ksp of Ag2CO3 is 8.1 × 10-12.

Correct AnswerverifiedShow Answer

Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.322 M in formic acid and 0.178 M in sodium formate (NaHCO2) . The Ka of formic acid is 1.77 × 10-4.

Correct AnswerverifiedShow Answer

The solubility of manganese (II) hydroxide (Mn(OH) 2) is 2.2 × 10-5 M. What is the Ksp of Mn(OH) 2?

Correct AnswerverifiedShow Answer

Calculate the maximum concentration (in M) of magnesium ions (Mg+2) in a solution that contains 0.025 M of CO32-. The Ksp of MgCO3 is 3.5 × 10-8.

Correct AnswerverifiedShow Answer

Calculate the pH of a solution prepared by dissolving 0.250 mol of benzoic acid (C7H5O2H) and 0.150 mol of sodium benzoate (NaC7H5O2) in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.50 × 10-5.

Correct AnswerverifiedShow Answer

Which of the following could be added to a solution of acetic acid to prepare a buffer?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

The concentration of fluoride ions in a saturated solution of barium fluoride is ________ M. The solubility product constant of BaF2 is 1.7 × 10-6.

Correct AnswerverifiedShow Answer

What is the solubility (in M) of PbCl2 in a 0.15 M solution of HCl? The Ksp of PbCl2 is 1.6 × 10-5.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

What are the principal organs that regulate the pH of the carbonic acid-bicarbonate buffer system in the blood?

Correct AnswerverifiedShow Answer

The pH of a solution prepared by dissolving 0.350 mol of solid dimethylamine hydrochloride ((CH₃) ₂NH₂Cl) in 1.00 L of 1.10 M dimethylamine ((CH₃) ₂NH) is ________. The K_b for methylamine is 5.40 × 10^-4. (Assume the final volume is 1.00 L.)

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Calculate the percent ionization of nitrous acid in a solution that is 0.260 M in nitrous acid. The acid dissociation constant of nitrous acid is 4.50 × 10^-4.

Correct Answer
verified

The concentration of iodide ions in a saturated solution of silver iodide is ________ M. The solubility product constant of AgI is 8.3 × 10^-1⁷.

Correct Answer
verified

Correct Answer
verified

Calculate the maximum concentration (in M) of silver ions (Ag⁺) in a solution that contains 0.025 M of CO₃^2-. The K_sp of Ag₂CO₃ is 8.1 × 10^-12.

Correct Answer
verified

Calculate the percent ionization of formic acid (HCO₂H) in a solution that is 0.322 M in formic acid and 0.178 M in sodium formate (NaHCO₂) . The K_a of formic acid is 1.77 × 10^-4.

Correct Answer
verified

The solubility of manganese (II) hydroxide (Mn(OH) ₂) is 2.2 × 10^-5 M. What is the K_sp of Mn(OH) ₂?

Correct Answer
verified

Calculate the maximum concentration (in M) of magnesium ions (Mg⁺²) in a solution that contains 0.025 M of CO₃^2-. The K_sp of MgCO₃ is 3.5 × 10^-8.

Correct Answer
verified

Calculate the pH of a solution prepared by dissolving 0.250 mol of benzoic acid (C₇H₅O₂H) and 0.150 mol of sodium benzoate (NaC₇H₅O₂) in water sufficient to yield 1.00 L of solution. The K_a of benzoic acid is 6.50 × 10^-5.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

The concentration of fluoride ions in a saturated solution of barium fluoride is ________ M. The solubility product constant of BaF₂ is 1.7 × 10^-⁶.

Correct Answer
verified

What is the solubility (in M) of PbCl₂ in a 0.15 M solution of HCl? The K_sp of PbCl₂ is 1.6 × 10^-5.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified