Question 1

How would you calculate Kb for the formate ion, given that the Ka for formic acid is 1.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104?

Accepted Answer

A) Kb F1F1F1S1F1F1F10 Ka F1F1F1S1F1F1F10 Kw 
B) Kb F1F1F1S1F1F1F10 Kw / Ka 
C) Kb F1F1F1S1F1F1F10 Ka / Kw 
D) Kb F1F1F1S1F1F1F10 Kw F1F1F1S1F1F1F10 Ka 
E) Kb F1F1F1S1F1F1F10 Kw F1F1F1S1F1F1F10 Ka 
A) Kb F1F1F1S1F1F1F10 Ka F1F1F1S1F1F1F10 Kw 
B) Kb F1F1F1S1F1F1F10 Kw / Ka 
C) Kb F1F1F1S1F1F1F10 Ka / Kw 
D) Kb F1F1F1S1F1F1F10 Kw F1F1F1S1F1F1F10 Ka 
E) Kb F1F1F1S1F1F1F10 Kw F1F1F1S1F1F1F10 Ka

Question 2

The pH of a popular soft drink is 3.4; what is its hydronium ion concentration?

Accepted Answer

A) 5.0 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 M 
B) 4.0 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 M 
C) 2.5 F1F1F1S1F1F1F10 103 M 
D) 1.0 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F107 M 
E) 5.0 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105 M 
A) 5.0 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 M 
B) 4.0 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 M 
C) 2.5 F1F1F1S1F1F1F10 103 M 
D) 1.0 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F107 M 
E) 5.0 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105 M

Question 3

Which one of the following statements is not correct?

Accepted Answer

A) HIO is a stronger acid than HClO. 
B) HClO is a stronger acid than HBrO. 
C) HClO3 is a stronger acid than HClO2. 
D) HPO42F1F1F1S1F1F1F10 is a weaker acid than H2PO4F1F1F1S1F1F1F10. 
E) H2SO4 is a stronger acid than H2SO3. 
A) HIO is a stronger acid than HClO. 
B) HClO is a stronger acid than HBrO. 
C) HClO3 is a stronger acid than HClO2. 
D) HPO42F1F1F1S1F1F1F10 is a weaker acid than H2PO4F1F1F1S1F1F1F10. 
E) H2SO4 is a stronger acid than H2SO3.

Question 4

A solution with a pOH of 4.3 has a [HF1F1F1S1F1F1F10] of ________

Accepted Answer

A) 6.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F109 M. 
B) 3.2 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 M. 
C) 4.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105 M. 
D) 2.0 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1010 M. 
E) 4.3 M. 
A) 6.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F109 M. 
B) 3.2 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 M. 
C) 4.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105 M. 
D) 2.0 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1010 M. 
E) 4.3 M.

Question 5

What is the pH of a 0.030 M solution of oxalic acid? Ka for oxalic acid is 5.9 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F102.

Accepted Answer

A) 1.66 
B) 1.37 
C) 2.78 
D) 12.67 
E) 12.34 
A) 1.66 
B) 1.37 
C) 2.78 
D) 12.67 
E) 12.34

Question 6

A solution with a pH of 2.50 has an [OHF1F1F1S1F1F1F10] of ________

Accepted Answer

A) 3.16 F1F1F1S1F1F1F10 102. 
B) 3.16 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1012. 
C) 3.16 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103. 
D) 3.16 F1F1F1S1F1F1F10 1016. 
E) 3.16 F1F1F1S1F1F1F10 1011. 
A) 3.16 F1F1F1S1F1F1F10 102. 
B) 3.16 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1012. 
C) 3.16 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103. 
D) 3.16 F1F1F1S1F1F1F10 1016. 
E) 3.16 F1F1F1S1F1F1F10 1011.

Question 7

What is the actual concentration of molecular NH3 in a 0.200 M solution of ammonia? The Kb value for ammonia is 1.80 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105.

Accepted Answer

A) 0.200 M 
B) 0.198 M 
C) 1.80 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105 M 
D) 1.90 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103 M 
E) 3.6 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F106 M 
A) 0.200 M 
B) 0.198 M 
C) 1.80 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105 M 
D) 1.90 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103 M 
E) 3.6 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F106 M

Question 8

Aqueous solutions of ________ are basic.

Accepted Answer

A) NaF 
B) NaCl 
C) NaBr 
D) NH4I 
E) KI 
A) NaF 
B) NaCl 
C) NaBr 
D) NH4I 
E) KI

Question 9

Which of the following is a strong acid?

Accepted Answer

A) HNO3 
B) H2S 
C) HNO2 
D) HCO3F1F1F1S1F1F1F10 
E) HOCl 
A) HNO3 
B) H2S 
C) HNO2 
D) HCO3F1F1F1S1F1F1F10 
E) HOCl

Question 10

Solutions of each of the hypothetical bases in the following table are prepared with an initial concentration of 0.100 M. Which of the four solutions will have the lowest pH and be least basic?

Accepted Answer

A) A 
B) B 
C) C 
D) D 
E) All will have the same pH because the concentrations are the same. 
A) A 
B) B 
C) C 
D) D 
E) All will have the same pH because the concentrations are the same.

Question 11

Which one of the following is a strong acid?

Accepted Answer

A) nitrous acid, HNO2 
B) sulfurous acid, H2SO3 
C) carbonic acid, H2CO3 
D) hydrofluoric acid, HF 
E) perchloric acid, HClO4 
A) nitrous acid, HNO2 
B) sulfurous acid, H2SO3 
C) carbonic acid, H2CO3 
D) hydrofluoric acid, HF 
E) perchloric acid, HClO4

Question 12

What is the pH of a 0.35 M solution of sodium azide? The Ka value for hydrazoic acid is 1.9 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105.

Accepted Answer

A) 11.41 
B) 4.87 
C) 9.13 
D) 2.59 
E) 12.47 
A) 11.41 
B) 4.87 
C) 9.13 
D) 2.59 
E) 12.47

Question 13

The acid ionization equilibrium constant, Ka, describes the reaction (where HA is a generic weak acid) ________

Accepted Answer

A) HA F1F1F1S1F1F1F10 OHF1F1F1S1F1F1F10   H2O F1F1F1S1F1F1F10 AF1F1F1S1F1F1F10. 
B) HA F1F1F1S1F1F1F10 H2O   H3OF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 AF1F1F1S1F1F1F10. 
C) HA F1F1F1S1F1F1F10 H3OF1F1F1S1F1F1F10   H2AF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 H2O. 
D) HA F1F1F1S1F1F1F10 H2AF1F1F1S1F1F1F10   H2AF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 HA. 
E) H3OF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 AF1F1F1S1F1F1F10   HA F1F1F1S1F1F1F10 H2O. 
A) HA F1F1F1S1F1F1F10 OHF1F1F1S1F1F1F10   H2O F1F1F1S1F1F1F10 AF1F1F1S1F1F1F10. 
B) HA F1F1F1S1F1F1F10 H2O   H3OF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 AF1F1F1S1F1F1F10. 
C) HA F1F1F1S1F1F1F10 H3OF1F1F1S1F1F1F10   H2AF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 H2O. 
D) HA F1F1F1S1F1F1F10 H2AF1F1F1S1F1F1F10   H2AF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 HA. 
E) H3OF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 AF1F1F1S1F1F1F10   HA F1F1F1S1F1F1F10 H2O.

Question 14

What is the Ka for nitrous acid, given that the pKb for the nitrite ion is 10.61?

Accepted Answer

A) 1.38 F1F1F1S1F1F1F10 104 
B) 4.07 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
C) 1.90 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105 
D) 5.60 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F106 
E) 4.30 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F107 
A) 1.38 F1F1F1S1F1F1F10 104 
B) 4.07 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
C) 1.90 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105 
D) 5.60 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F106 
E) 4.30 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F107

Question 15

A solution of the weak acid HF and a solution of the strong acid HCl have the same pH. Which solution will require the most sodium hydroxide, NaOH, to neutralize?

Accepted Answer

A) HCl, because it is a strong acid and dissociates completely. 
B) HF, because its concentration is larger. 
C) Both will require the same amount because the concentrations are equal. 
D) Both will require the same amount because the H3OF1F1F1S1F1F1F10 concentrations are the same. 
E) HCl, because the stronger acid has the higher concentration. 
A) HCl, because it is a strong acid and dissociates completely. 
B) HF, because its concentration is larger. 
C) Both will require the same amount because the concentrations are equal. 
D) Both will require the same amount because the H3OF1F1F1S1F1F1F10 concentrations are the same. 
E) HCl, because the stronger acid has the higher concentration.

Question 16

Identify the weakest and strongest acids in the group below. The weakest acid is listed first in the responses. HCl, HBr, HI

Accepted Answer

A) HCl F1F1F1S1F1F1F10 HI 
B) HCl F1F1F1S1F1F1F10 HBr 
C) HBr F1F1F1S1F1F1F10 HCl 
D) HBr F1F1F1S1F1F1F10 HI 
E) HI F1F1F1S1F1F1F10 HCl 
A) HCl F1F1F1S1F1F1F10 HI 
B) HCl F1F1F1S1F1F1F10 HBr 
C) HBr F1F1F1S1F1F1F10 HCl 
D) HBr F1F1F1S1F1F1F10 HI 
E) HI F1F1F1S1F1F1F10 HCl

Question 17

Diethylamine ((CH3CH2) NH2) is a weakly basic compound. Calculate the Kb for diethylamine if a 0.127 M solution is 9.61% ionized.

Accepted Answer

A) 1.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105 
B) 4.4 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
C) 5.6 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
D) 1.3 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103 
E) 3.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1010 
A) 1.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105 
B) 4.4 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
C) 5.6 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
D) 1.3 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103 
E) 3.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1010

Question 18

Lactic acid is a major component of Ringer's solution, which is used as an intravenous fluid to maintain fluid balance in trauma patients. The pH of a 0.100 M lactic acid solution is around 2.44. Based on this information, determine the value of the acid ionization constant, Ka, for lactic acid.

Accepted Answer

A) 1.2 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F102 
B) 1.4 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
C) 4.7 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103 
D) 1.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
E) 7.4 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103 
A) 1.2 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F102 
B) 1.4 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
C) 4.7 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103 
D) 1.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
E) 7.4 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103

Question 19

Which one of the following salts does not produce a basic solution when dissolved in water?

Accepted Answer

A) Na2S 
B) NaBr 
C) NaClO2 
D) NaNO2 
E) Na2CO3 
A) Na2S 
B) NaBr 
C) NaClO2 
D) NaNO2 
E) Na2CO3

Question 20

The hydronium ion concentration of a dilute solution of vinegar is 1.45 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105. What is the pH of this solution?

Accepted Answer

A) 5.7 
B) (F1F1F1S1F1F1F104.8) 
C) 4.8 
D) (F1F1F1S1F1F1F105.7) 
E) 7.0 
A) 5.7 
B) (F1F1F1S1F1F1F104.8) 
C) 4.8 
D) (F1F1F1S1F1F1F105.7) 
E) 7.0

Exam 15: Acidbase Equilibria: Proton Transfer in Biological Systems

How would you calculate Kb for the formate ion, given that the Ka for formic acid is 1.8  104?

The pH of a popular soft drink is 3.4; what is its hydronium ion concentration?

Which one of the following statements is not correct?

A solution with a pOH of 4.3 has a [H] of ________

What is the pH of a 0.030 M solution of oxalic acid? Ka for oxalic acid is 5.9  102.

A solution with a pH of 2.50 has an [OH] of ________

What is the actual concentration of molecular NH3 in a 0.200 M solution of ammonia? The Kb value for ammonia is 1.80  105.

Aqueous solutions of ________ are basic.

Which of the following is a strong acid?

Solutions of each of the hypothetical bases in the following table are prepared with an initial concentration of 0.100 M. Which of the four solutions will have the lowest pH and be least basic?

Which one of the following is a strong acid?

What is the pH of a 0.35 M solution of sodium azide? The Ka value for hydrazoic acid is 1.9  105.

The acid ionization equilibrium constant, Ka, describes the reaction (where HA is a generic weak acid) ________

What is the Ka for nitrous acid, given that the pKb for the nitrite ion is 10.61?

A solution of the weak acid HF and a solution of the strong acid HCl have the same pH. Which solution will require the most sodium hydroxide, NaOH, to neutralize?

Identify the weakest and strongest acids in the group below. The weakest acid is listed first in the responses. HCl, HBr, HI

Diethylamine ((CH3CH2) NH2) is a weakly basic compound. Calculate the Kb for diethylamine if a 0.127 M solution is 9.61% ionized.

Lactic acid is a major component of Ringer's solution, which is used as an intravenous fluid to maintain fluid balance in trauma patients. The pH of a 0.100 M lactic acid solution is around 2.44. Based on this information, determine the value of the acid ionization constant, Ka, for lactic acid.

Which one of the following salts does not produce a basic solution when dissolved in water?

The hydronium ion concentration of a dilute solution of vinegar is 1.45  105. What is the pH of this solution?

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

How would you calculate K_b for the formate ion, given that the K_a for formic acid is 1.8  10^⁴?

A solution with a pOH of 4.3 has a [H^] of ________

What is the pH of a 0.030 M solution of oxalic acid? K_a for oxalic acid is 5.9  10^².

A solution with a pH of 2.50 has an [OH^] of ________

What is the actual concentration of molecular NH₃ in a 0.200 M solution of ammonia? The K_b value for ammonia is 1.80  10^⁵.

What is the pH of a 0.35 M solution of sodium azide? The K_a value for hydrazoic acid is 1.9  10^⁵.

The acid ionization equilibrium constant, K_a, describes the reaction (where HA is a generic weak acid) ________

What is the K_a for nitrous acid, given that the pK_b for the nitrite ion is 10.61?

Diethylamine ((CH₃CH₂)NH₂) is a weakly basic compound. Calculate the K_b for diethylamine if a 0.127 M solution is 9.61% ionized.

Lactic acid is a major component of Ringer's solution, which is used as an intravenous fluid to maintain fluid balance in trauma patients. The pH of a 0.100 M lactic acid solution is around 2.44. Based on this information, determine the value of the acid ionization constant, K_a, for lactic acid.

The hydronium ion concentration of a dilute solution of vinegar is 1.45  10^⁵. What is the pH of this solution?