Question 1

The pH of a solution prepared by mixing 45.0 mL of 0.183 M KOH and 25.0 mL of 0.145 M HCl is __________.

Accepted Answer

A) 1.314 
B) 1.181 
C) 0.00824 
D) 12.819 
E) 12.923 
A) 1.314 
B) 1.181 
C) 0.00824 
D) 12.819 
E) 12.923

Question 2

A 25.0 mL sample of an acetic acid solution is titrated with a 0.175 M NaOH solution. The equivalence point is reached when 26.6 mL of the base is added. The concentration of acetic acid in the sample was __________ M.

Accepted Answer

A) 0.365 
B) 0.175 
C) 0.119 
D) 0.186 
E) none of the above 
A) 0.365 
B) 0.175 
C) 0.119 
D) 0.186 
E) none of the above

Question 3

In which of the following aqueous solutions would you expect PbCl2to have the lowest solubility?

Accepted Answer

A) 0.020 M KCl 
B) 0.020 M BaCl2 
C) 0.015 M PbNO3 
D) pure water 
E) 0.015 M NaCl 
A) 0.020 M KCl 
B) 0.020 M BaCl2 
C) 0.015 M PbNO3 
D) pure water 
E) 0.015 M NaCl

Question 4

The pH of a solution prepared by mixing 50.0 mL of 0.125 M NaOH and 40.0 mL of 0.125 M HNO3 is __________.

Accepted Answer

A) 13.29 
B) 7.00 
C) 8.11 
D) 11.00 
E) none of the above 
A) 13.29 
B) 7.00 
C) 8.11 
D) 11.00 
E) none of the above

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 25.3 mL of base. The concentration of HCl is __________ M.

Accepted Answer

A) 11.7 
B) 0.00352 
C) 0.141 
D) 0.0352 
E) 0.139 
A) 11.7 
B) 0.00352 
C) 0.141 
D) 0.0352 
E) 0.139

Question 6

Calculate the pH of a solution that is 0.295 M in sodium formate (NaHCO2)and 0.205 M in formic acid (HCO2H). The Ka of formic acid is 1.77 × 10-4.

Accepted Answer

A) 3.910 
B) 3.587 
C) 13.84 
D) 10.10 
E) 4.963 
A) 3.910 
B) 3.587 
C) 13.84 
D) 10.10 
E) 4.963

Question 7

The Ksp for Zn(OH)2 is 5.0 × 10-17. Determine the molar solubility of Zn(OH)2 in a buffer solution with a pH of 11.5.

Accepted Answer

A) 5.0 × 106 
B) 1.2 × 10-12 
C) 1.6 × 10-14 
D) 5.0 × 10-12 
E) 5.0 × 10-17 
A) 5.0 × 106 
B) 1.2 × 10-12 
C) 1.6 × 10-14 
D) 5.0 × 10-12 
E) 5.0 × 10-17

Question 8

__________ analysis determines only the presence or absence of a particular metal ion, whereas __________ analysis determines how much of a given substance is present.

Accepted Answer

Qualitativ

Question 9

The solubility of slightly soluble salts containing basic anions is proportional to the pH of the solution.

Accepted Answer

A) True 
 B)False

Question 10

The Ka of acetic acid is 1.76 × 10-5. The pH of a buffer prepared by combining 45.0 mL of 1.00 M potassium acetate and 50.0 mL of 1.00 M acetic acid is __________.

Accepted Answer

A) 1.705 
B) 0.851 
C) 3.406 
D) 4.709 
E) 2.383 
A) 1.705 
B) 0.851 
C) 3.406 
D) 4.709 
E) 2.383

Question 11

The addition of sodium hydroxide and __________ to water produces a buffer solution.

Accepted Answer

A) HCl 
B) NaC2H3O2 
C) NaF 
D) NH3 
E) none of the above 
A) HCl 
B) NaC2H3O2 
C) NaF 
D) NH3 
E) none of the above

Question 12

The Ka of benzoic acid is 6.30 × 10-5. The pH of a buffer prepared by combining 50.0 mL of 1.00 M potassium benzoate and 50.0 mL of 1.00 M benzoic acid is __________.

Accepted Answer

A) 1.705 
B) 0.851 
C) 3.406 
D) 4.201 
E) 2.383 
A) 1.705 
B) 0.851 
C) 3.406 
D) 4.201 
E) 2.383

Question 13

The concentration of iodide ions in a saturated solution of lead (II)iodide is __________ M. The solubility product constant of PbI2 is 1.4 × 10-8.

Accepted Answer

A) 3.8 × 10-4 
B) 3.0 × 10-3 
C) 1.5 × 10-3 
D) 3.5 × 10-9 
E) 1.4 × 10-8 
A) 3.8 × 10-4 
B) 3.0 × 10-3 
C) 1.5 × 10-3 
D) 3.5 × 10-9 
E) 1.4 × 10-8

Question 14

What is the pH of a buffer solution that is 0.255 M in hypochlorous acid (HClO)and 0.333 M in sodium hypochlorite? The Ka of hypochlorous acid is 3.8 × 10-8.

Accepted Answer

A) 13.88 
B) 6.46 
C) 8.49 
D) 7.30 
E) 7.54 
A) 13.88 
B) 6.46 
C) 8.49 
D) 7.30 
E) 7.54

Question 15

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

Accepted Answer

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

Question 16

A solution is prepared by dissolving 0.23 mol of hydrofluoric acid and 0.27 mol of sodium fluoride in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of HCl to this buffer solution causes the pH to drop slightly. The pH does not decrease drastically because the HCl reacts with the __________ present in the buffer solution. The Ka of hydrofluoric acid is 1.36 × 10-3.

Accepted Answer

A) H2O 
B) H3O+ 
C) fluoride ion 
D) hydrofluoric acid 
E) This is a buffer solution: the pH does not change upon addition of acid or base. 
A) H2O 
B) H3O+ 
C) fluoride ion 
D) hydrofluoric acid 
E) This is a buffer solution: the pH does not change upon addition of acid or base.

Question 17

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

Accepted Answer

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

Question 18

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.77 × 10-5.

Accepted Answer

Question 19

The primary buffer system that controls the pH of the blood is the __________ buffer system.

Accepted Answer

A) carbon dioxide, carbonate 
B) carbonate, bicarbonate 
C) carbonic acid, carbon dioxide 
D) carbonate, carbonic acid 
E) carbonic acid, bicarbonate 
A) carbon dioxide, carbonate 
B) carbonate, bicarbonate 
C) carbonic acid, carbon dioxide 
D) carbonate, carbonic acid 
E) carbonic acid, bicarbonate

Question 20

A 25.0 mL sample of a solution of an unknown compound is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The unknown compound is __________.

Accepted Answer

A) a strong acid 
B) a strong base 
C) a weak acid 
D) a weak base 
E) neither an acid nor a base 
A) a strong acid 
B) a strong base 
C) a weak acid 
D) a weak base 
E) neither an acid nor a base

Exam 17: Additional Aspects of Aqueous Equilibria

The pH of a solution prepared by mixing 45.0 mL of 0.183 M KOH and 25.0 mL of 0.145 M HCl is __________.

A 25.0 mL sample of an acetic acid solution is titrated with a 0.175 M NaOH solution. The equivalence point is reached when 26.6 mL of the base is added. The concentration of acetic acid in the sample was __________ M.

In which of the following aqueous solutions would you expect PbCl2to have the lowest solubility?

The pH of a solution prepared by mixing 50.0 mL of 0.125 M NaOH and 40.0 mL of 0.125 M HNO3 is __________.

A 25.0 mL sample of an HCl solution is titrated with a 0.139 M NaOH solution. The equivalence point is reached with 25.3 mL of base. The concentration of HCl is __________ M.

Calculate the pH of a solution that is 0.295 M in sodium formate (NaHCO2)and 0.205 M in formic acid (HCO2H). The Ka of formic acid is 1.77 × 10-4.

The Ksp for Zn(OH)2 is 5.0 × 10-17. Determine the molar solubility of Zn(OH)2 in a buffer solution with a pH of 11.5.

__________ analysis determines only the presence or absence of a particular metal ion, whereas __________ analysis determines how much of a given substance is present.

The solubility of slightly soluble salts containing basic anions is proportional to the pH of the solution.

The Ka of acetic acid is 1.76 × 10-5. The pH of a buffer prepared by combining 45.0 mL of 1.00 M potassium acetate and 50.0 mL of 1.00 M acetic acid is __________.

The addition of sodium hydroxide and __________ to water produces a buffer solution.

The Ka of benzoic acid is 6.30 × 10-5. The pH of a buffer prepared by combining 50.0 mL of 1.00 M potassium benzoate and 50.0 mL of 1.00 M benzoic acid is __________.

The concentration of iodide ions in a saturated solution of lead (II)iodide is __________ M. The solubility product constant of PbI2 is 1.4 × 10-8.

What is the pH of a buffer solution that is 0.255 M in hypochlorous acid (HClO)and 0.333 M in sodium hypochlorite? The Ka of hypochlorous acid is 3.8 × 10-8.

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

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

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.77 × 10-5.

The primary buffer system that controls the pH of the blood is the __________ buffer system.

A 25.0 mL sample of a solution of an unknown compound is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The unknown compound is __________.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

In which of the following aqueous solutions would you expect PbCl₂to have the lowest solubility?

The pH of a solution prepared by mixing 50.0 mL of 0.125 M NaOH and 40.0 mL of 0.125 M HNO₃ is __________.

Calculate the pH of a solution that is 0.295 M in sodium formate (NaHCO₂)and 0.205 M in formic acid (HCO₂H). The K_a of formic acid is 1.77 × 10^-4.

The K_sp for Zn(OH)₂ is 5.0 × 10^-17. Determine the molar solubility of Zn(OH)₂ in a buffer solution with a pH of 11.5.

analysis determines only the presence or absence of a particular metal ion, whereas analysis determines how much of a given substance is present.

The K_a of acetic acid is 1.76 × 10^-5. The pH of a buffer prepared by combining 45.0 mL of 1.00 M potassium acetate and 50.0 mL of 1.00 M acetic acid is __________.

The K_a of benzoic acid is 6.30 × 10^-5. The pH of a buffer prepared by combining 50.0 mL of 1.00 M potassium benzoate and 50.0 mL of 1.00 M benzoic acid is __________.

The concentration of iodide ions in a saturated solution of lead (II)iodide is __________ M. The solubility product constant of PbI₂ is 1.4 × 10^-8.

What is the pH of a buffer solution that is 0.255 M in hypochlorous acid (HClO)and 0.333 M in sodium hypochlorite? The K_a of hypochlorous acid is 3.8 × 10^-8.

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.