Question 1

Which of the following reactions is associated with the definition of Kb?

Accepted Answer

A)  CN- + H+   HCN 
B)  Cr3+ + 6H2O   Cr(OH2)63+ 
C)  Zn(OH2)62+   [Zn(OH2)5OH]+ + H+ 
D)  F- + H2O   HF + OH- 
E)  none of these 
A)  CN- + H+   HCN 
B)  Cr3+ + 6H2O   Cr(OH2)63+ 
C)  Zn(OH2)62+   [Zn(OH2)5OH]+ + H+ 
D)  F- + H2O   HF + OH- 
E)  none of these

Question 2

A 0.240 M solution of the salt NaA has pH = 8.40. Calculate Ka for the acid HA.

Accepted Answer

A)  2.63 × 10-11 
B)  3.80 × 10-4 
C)  1.05 × 10-5 
D)  6.60 × 10-17 
E)  none of these 
A)  2.63 × 10-11 
B)  3.80 × 10-4 
C)  1.05 × 10-5 
D)  6.60 × 10-17 
E)  none of these

Question 3

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges.0.1 M NaCN (pKa for HCN = 9.31)

Accepted Answer

A)  pH 11.00-14.00 
B)  pH 3.00-5.99 
C)  pH 0.00-2.99 
D)  pH 6.00-8.99 
E)  pH 9.00-10.99 
A)  pH 11.00-14.00 
B)  pH 3.00-5.99 
C)  pH 0.00-2.99 
D)  pH 6.00-8.99 
E)  pH 9.00-10.99

Question 4

In a solution prepared by dissolving 0.100 mol of propionic acid in enough water to make 1.00 L of solution, the pH is observed to be 1.35. What is Ka for propionic acid (HC3H5O2)?

Accepted Answer

A)  4.5 × 10-2 
B)  2.0 × 10-2 
C)  5.0 × 10-12 
D)  3.6 × 10-2 
E)  none of these 
A)  4.5 × 10-2 
B)  2.0 × 10-2 
C)  5.0 × 10-12 
D)  3.6 × 10-2 
E)  none of these

Question 5

Provide an example of a salt that is acidic, a salt that is basic, and a salt that is neutral when dissolved in water. Provide chemical equations for each of these to support your answer.

Accepted Answer

See Sectio

Question 6

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid ammonium fluoride (NH4F)
For NH3, Kb = 1.8 × 10-5; for HF, Ka = 7.2 × 10-4.

Accepted Answer

A)  neutral 
B)  basic 
C)  acidic 
A)  neutral 
B)  basic 
C)  acidic

Question 7

You have at your disposal 100.00 mL of 0.650 M HCl and 500.00 mL of 0.300 M NaOH. How many mL of the base have to be added to the full volume of the acid to reach a pH of 1.90?

Accepted Answer

A)  20.4 mL 
B)  43.3 mL 
C)  10.2 mL 
D)  433 mL 
E)  204 mL 
A)  20.4 mL 
B)  43.3 mL 
C)  10.2 mL 
D)  433 mL 
E)  204 mL

Question 8

Calculate the pH of a 0.30 M solution of NH4Cl. (Kb for NH3 = 1.8 × 10-5)

Accepted Answer

A)  3.33 
B)  11.67 
C)  4.89 
D)  9.11 
E)  7.00 
A)  3.33 
B)  11.67 
C)  4.89 
D)  9.11 
E)  7.00

Question 9

Calculate the pH of a 0.040 M perchloric acid (HClO4) solution.

Accepted Answer

A)  1.40 
B)  2.10 
C)  12.60 
D)  11.90 
E)  none of these 
A)  1.40 
B)  2.10 
C)  12.60 
D)  11.90 
E)  none of these

Question 10

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium cyanide (NaCN)

Accepted Answer

A)  neutral 
B)  basic 
C)  acidic 
A)  neutral 
B)  basic 
C)  acidic

Question 11

In pure liquid ammonia, the equilibrium concentrations of both NH4+ and NH2- are 3 × 10-14 M. Which of the following equations always holds for liquid ammonia solutions?

Accepted Answer

A)  pNH4+ = log [pNH4+] 
B)  pNH4+ = 27.0 
C)  pNH4+ - pNH2- = 13.5 
D)  pNH4+ = 27.0 - pNH2- 
E)  pNH4+ + pNH2- = 13.5 
A)  pNH4+ = log [pNH4+] 
B)  pNH4+ = 27.0 
C)  pNH4+ - pNH2- = 13.5 
D)  pNH4+ = 27.0 - pNH2- 
E)  pNH4+ + pNH2- = 13.5

Question 12

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium bicarbonate (NaHCO}3

Accepted Answer

A)  basic 
B)  neutral 
C)  acidic 
A)  basic 
B)  neutral 
C)  acidic

Question 13

A _____ can furnish more than one proton per molecule and it always dissociates in a stepwise manner, one proton at a time.

Accepted Answer

A)  ​polyprotic acid 
B)  lysergic acid 
C)  lysergic base 
D)  monoprotic acid 
E)  polyprotic base 
A)  ​polyprotic acid 
B)  lysergic acid 
C)  lysergic base 
D)  monoprotic acid 
E)  polyprotic base

Question 14

Calculate the pOH of a 0.74 M solution of acetic acid (Ka = 1.8 × 10-5) at 25°C.

Accepted Answer

A)  2.77 
B)  9.26 
C)  4.88 
D)  11.56 
E)  2.44 
A)  2.77 
B)  9.26 
C)  4.88 
D)  11.56 
E)  2.44

Question 15

What is the equilibrium constant for the following reaction?
NH4+ + OH-  NH3 + H2O

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 16

The hydrogen sulfate or bisulfate ion HSO4- can act as either an acid or a base in water solution. In which of the following equations does HSO4- act as an acid?

Accepted Answer

A)  HSO4- + H2O → SO42- + H3O+ 
B)  HSO4- + H2O → H2SO4 + OH- 
C)  HSO4- + H3O+ → SO3 + 2H2O 
D)  HSO4- + OH- → H2SO4 + O2- 
E)  none of these 
A)  HSO4- + H2O → SO42- + H3O+ 
B)  HSO4- + H2O → H2SO4 + OH- 
C)  HSO4- + H3O+ → SO3 + 2H2O 
D)  HSO4- + OH- → H2SO4 + O2- 
E)  none of these

Question 17

Which of the following reactions is associated with the definition of Kb?

Accepted Answer

A)  [Al(OH2)6]3+   Al(OH)(OH2)52+ + H+ 
B)  OCl- + H2O   HOCl + OH- 
C)  Al3+ + 6H2O   Al(OH2)63+ 
D)  CN- + H+   HCN 
A)  [Al(OH2)6]3+   Al(OH)(OH2)52+ + H+ 
B)  OCl- + H2O   HOCl + OH- 
C)  Al3+ + 6H2O   Al(OH2)63+ 
D)  CN- + H+   HCN

Question 18

Calculate the pH of a solution made by a mixture of the following acids: 0.40 M HC2H3O2 (Ka = 1.8 × 10-5), 0.10 M HOCl (Ka = 3.5 × 10-8), and 0.20 M HCN (Ka = 6.2 × 10-10).

Accepted Answer

A)  2.57 
B)  3.92 
C)  4.95 
D)  4.23 
E)  3.49 
A)  2.57 
B)  3.92 
C)  4.95 
D)  4.23 
E)  3.49

Question 19

Calculate the pH of a 0.02 M solution of KOH.

Accepted Answer

A)  1.7 
B)  We cannot calculate the answer unless a volume is given. 
C)  12.3 
D)  2.0 
E)  12.0 
A)  1.7 
B)  We cannot calculate the answer unless a volume is given. 
C)  12.3 
D)  2.0 
E)  12.0

Question 20

The pH of a 0.100 M solution of an aqueous weak acid (HA) is 3.20. What is Ka for the
Weak acid?

Accepted Answer

A)  4.0 × 10-6 
B)  6.3 × 10-4 
C)  7.2 × 10-5 
D)  3.2 
E)  none of these 
A)  4.0 × 10-6 
B)  6.3 × 10-4 
C)  7.2 × 10-5 
D)  3.2 
E)  none of these

Which of the following reactions is associated with the definition of K_b?

A 0.240 M solution of the salt NaA has pH = 8.40. Calculate K_a for the acid HA.

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges.0.1 M NaCN (pK_a for HCN = 9.31)

In a solution prepared by dissolving 0.100 mol of propionic acid in enough water to make 1.00 L of solution, the pH is observed to be 1.35. What is K_a for propionic acid (HC₃H₅O₂)?

Provide an example of a salt that is acidic, a salt that is basic, and a salt that is neutral when dissolved in water. Provide chemical equations for each of these to support your answer.

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid ammonium fluoride (NH₄F) For NH₃, K_b = 1.8 × 10^-5; for HF, K_a = 7.2 × 10^-4.

You have at your disposal 100.00 mL of 0.650 M HCl and 500.00 mL of 0.300 M NaOH. How many mL of the base have to be added to the full volume of the acid to reach a pH of 1.90?

Calculate the pH of a 0.30 M solution of NH₄Cl. (K_b for NH₃ = 1.8 × 10^-5)

Calculate the pH of a 0.040 M perchloric acid (HClO₄) solution.

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium cyanide (NaCN)

In pure liquid ammonia, the equilibrium concentrations of both NH₄⁺ and NH₂^- are 3 × 10^-14 M. Which of the following equations always holds for liquid ammonia solutions?

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium bicarbonate (NaHCO}₃

A _____ can furnish more than one proton per molecule and it always dissociates in a stepwise manner, one proton at a time.

Calculate the pOH of a 0.74 M solution of acetic acid (K_a = 1.8 × 10^-5) at 25°C.

What is the equilibrium constant for the following reaction? NH₄⁺ + OH^- NH₃ + H₂O

The hydrogen sulfate or bisulfate ion HSO₄^- can act as either an acid or a base in water solution. In which of the following equations does HSO₄^- act as an acid?

Which of the following reactions is associated with the definition of K_b?

Calculate the pH of a solution made by a mixture of the following acids: 0.40 M HC₂H₃O₂ (K_a = 1.8 × 10^-5), 0.10 M HOCl (K_a = 3.5 × 10^-8), and 0.20 M HCN (K_a = 6.2 × 10^-10).

Calculate the pH of a 0.02 M solution of KOH.

The pH of a 0.100 M solution of an aqueous weak acid (HA) is 3.20. What is K_a for the Weak acid?

Atoms, Molecules, and Ions

Stoichiometry

Types of Chemical Reactions and Solution Stoichiometry

Gases

Chemical Equilibrium

Applications of Aqueous Equilibria

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Liquids and Solids

Properties of Solutions

The Representative Elements

Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

Organic and Biochemical Molecules

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Exam 7: Acids and Bases

Which of the following reactions is associated with the definition of Kb?

A 0.240 M solution of the salt NaA has pH = 8.40. Calculate Ka for the acid HA.

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges.0.1 M NaCN (pKa for HCN = 9.31)

In a solution prepared by dissolving 0.100 mol of propionic acid in enough water to make 1.00 L of solution, the pH is observed to be 1.35. What is Ka for propionic acid (HC3H5O2)?

Provide an example of a salt that is acidic, a salt that is basic, and a salt that is neutral when dissolved in water. Provide chemical equations for each of these to support your answer.

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid ammonium fluoride (NH4F) For NH3, Kb = 1.8 × 10-5; for HF, Ka = 7.2 × 10-4.

You have at your disposal 100.00 mL of 0.650 M HCl and 500.00 mL of 0.300 M NaOH. How many mL of the base have to be added to the full volume of the acid to reach a pH of 1.90?

Calculate the pH of a 0.30 M solution of NH4Cl. (Kb for NH3 = 1.8 × 10-5)

Calculate the pH of a 0.040 M perchloric acid (HClO4) solution.

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium cyanide (NaCN)

In pure liquid ammonia, the equilibrium concentrations of both NH4+ and NH2- are 3 × 10-14 M. Which of the following equations always holds for liquid ammonia solutions?

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium bicarbonate (NaHCO}3

A _____ can furnish more than one proton per molecule and it always dissociates in a stepwise manner, one proton at a time.

Calculate the pOH of a 0.74 M solution of acetic acid (Ka = 1.8 × 10-5) at 25°C.

What is the equilibrium constant for the following reaction? NH4+ + OH- NH3 + H2O

The hydrogen sulfate or bisulfate ion HSO4- can act as either an acid or a base in water solution. In which of the following equations does HSO4- act as an acid?

Which of the following reactions is associated with the definition of Kb?

Calculate the pH of a solution made by a mixture of the following acids: 0.40 M HC2H3O2 (Ka = 1.8 × 10-5), 0.10 M HOCl (Ka = 3.5 × 10-8), and 0.20 M HCN (Ka = 6.2 × 10-10).

Calculate the pH of a 0.02 M solution of KOH.

The pH of a 0.100 M solution of an aqueous weak acid (HA) is 3.20. What is Ka for the Weak acid?

Atoms, Molecules, and Ions

Stoichiometry

Types of Chemical Reactions and Solution Stoichiometry

Gases

Chemical Equilibrium

Applications of Aqueous Equilibria

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Liquids and Solids

Properties of Solutions

The Representative Elements

Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

Organic and Biochemical Molecules

Filters

Which of the following reactions is associated with the definition of K_b?

A 0.240 M solution of the salt NaA has pH = 8.40. Calculate K_a for the acid HA.

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges.0.1 M NaCN (pK_a for HCN = 9.31)

In a solution prepared by dissolving 0.100 mol of propionic acid in enough water to make 1.00 L of solution, the pH is observed to be 1.35. What is K_a for propionic acid (HC₃H₅O₂)?

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid ammonium fluoride (NH₄F) For NH₃, K_b = 1.8 × 10^-5; for HF, K_a = 7.2 × 10^-4.

Calculate the pH of a 0.30 M solution of NH₄Cl. (K_b for NH₃ = 1.8 × 10^-5)

Calculate the pH of a 0.040 M perchloric acid (HClO₄) solution.

In pure liquid ammonia, the equilibrium concentrations of both NH₄⁺ and NH₂^- are 3 × 10^-14 M. Which of the following equations always holds for liquid ammonia solutions?

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid sodium bicarbonate (NaHCO}₃

Calculate the pOH of a 0.74 M solution of acetic acid (K_a = 1.8 × 10^-5) at 25°C.

What is the equilibrium constant for the following reaction? NH₄⁺ + OH^- NH₃ + H₂O

The hydrogen sulfate or bisulfate ion HSO₄^- can act as either an acid or a base in water solution. In which of the following equations does HSO₄^- act as an acid?

Which of the following reactions is associated with the definition of K_b?

Calculate the pH of a solution made by a mixture of the following acids: 0.40 M HC₂H₃O₂ (K_a = 1.8 × 10^-5), 0.10 M HOCl (K_a = 3.5 × 10^-8), and 0.20 M HCN (K_a = 6.2 × 10^-10).

The pH of a 0.100 M solution of an aqueous weak acid (HA) is 3.20. What is K_a for the Weak acid?