Question 1

The pH of a solution is 9.12 at 25 °C. Calculate the pOH of this solution at 25 °C.

Accepted Answer

A)  2.40 
B)  8.33 
C)  4.88 
D)  11.4 
E)  12.7 
A)  2.40 
B)  8.33 
C)  4.88 
D)  11.4 
E)  12.7

Question 2

What is the hydronium ion concentration of an acid rain sample that has a pH of 3. 45?

Accepted Answer

A)  2.82 × 10-11 mol L-1 
B)  3.55 × 10-4 mol L-1 
C)  3. 45 mol L-1 
D)  10. 55 mol L-1 
A)  2.82 × 10-11 mol L-1 
B)  3.55 × 10-4 mol L-1 
C)  3. 45 mol L-1 
D)  10. 55 mol L-1

Question 3

Calculate the pH of a 0.200 mol L-1 solution of formic acid, Ka = 1.8 × 10-4.

Accepted Answer

A)  3.84 
B)  2.22 
C)  4.62 
D)  1.97 
E)  3.07 
A)  3.84 
B)  2.22 
C)  4.62 
D)  1.97 
E)  3.07

Question 4

Calculate the pOH of an aqueous solution with a pH of 9.85 at 25 °C.

Accepted Answer

A)  2.15 
B)  3.15 
C)  4.15 
D)  5.15 
E)  4.00 
A)  2.15 
B)  3.15 
C)  4.15 
D)  5.15 
E)  4.00

Question 5

In a triprotic acid, which Ka has the highest value?

Accepted Answer

A)  Ka1 
B)  Ka2 
C)  Ka3 
D)  Kb1 
E)  Kb2 
A)  Ka1 
B)  Ka2 
C)  Ka3 
D)  Kb1 
E)  Kb2

Question 6

Which of the following is a weak acid?

Accepted Answer

A)  HClO4 
B)  H2SO4 
C)  HCl 
D)  HCO2H 
E)  HNO3 
A)  HClO4 
B)  H2SO4 
C)  HCl 
D)  HCO2H 
E)  HNO3

Question 7

Which of the following is an acid-base neutral ion?

Accepted Answer

A)  Al3+ 
B)  CN- 
C)  CO32- 
D)  Cl- 
E)  NH4+ 
A)  Al3+ 
B)  CN- 
C)  CO32- 
D)  Cl- 
E)  NH4+

Question 8

Which of the following is a triprotic acid?

Accepted Answer

A)  HF 
B)  H2SO4 
C)  H3PO4 
D)  H2SO3 
E)  HC2H3O2 
A)  HF 
B)  H2SO4 
C)  H3PO4 
D)  H2SO3 
E)  HC2H3O2

Question 9

What is the autoionization of water?

Accepted Answer

Autoionization of water is the equilibri

Question 10

Determine the pH of a 0.227 mol L-1 C5H5N solution at 25 °C. The Kb of C5H5N is 1.7 × 10-9.

Accepted Answer

A)  4.59 
B)  9.41 
C)  4.71 
D)  10.14 
E)  9.29 
A)  4.59 
B)  9.41 
C)  4.71 
D)  10.14 
E)  9.29

Question 11

On which equilibrium does the strength of an acid HA depend on?

Accepted Answer

A)  HA(aq) + H2O(l) ⇌ H2A+(aq) + OH-(aq) 
B)  HA(aq) + H2O(l) ⇌ A-(aq) + H3O+(aq) 
C)  HA(aq) + H2O(l) ⇌ H(HO)A-(aq) + H+(aq) 
D)  HA(aq) + OH-(aq) ⇌ A-(aq) + H2O(l) 
E)  HA(aq) + HA(aq) ⇌ H2A+(aq) + A-(aq) 
A)  HA(aq) + H2O(l) ⇌ H2A+(aq) + OH-(aq) 
B)  HA(aq) + H2O(l) ⇌ A-(aq) + H3O+(aq) 
C)  HA(aq) + H2O(l) ⇌ H(HO)A-(aq) + H+(aq) 
D)  HA(aq) + OH-(aq) ⇌ A-(aq) + H2O(l) 
E)  HA(aq) + HA(aq) ⇌ H2A+(aq) + A-(aq)

Question 12

Which of the following species is amphoteric?

Accepted Answer

A)  CO32- 
B)  HCl 
C)  NH4⁺ 
D)  HPO42- 
E)  NaOH 
A)  CO32- 
B)  HCl 
C)  NH4⁺ 
D)  HPO42- 
E)  NaOH

Question 13

Determine the [OH-] concentration of a 0.741 mol L-1 KOH solution at 25 °C.

Accepted Answer

A)  1.34 × 10-13 mol L-1 
B)  1.34 × 10-14 mol L-1 
C)  0.741 mol L-1 
D)  7.41 mol L-1 
E)  7.41 × 10-13 mol L-1 
A)  1.34 × 10-13 mol L-1 
B)  1.34 × 10-14 mol L-1 
C)  0.741 mol L-1 
D)  7.41 mol L-1 
E)  7.41 × 10-13 mol L-1

Question 14

Match the following.
-Bronsted-Lowry acid

Accepted Answer

A) electron pair donor 
B) produces protons in aqueous solution 
C) electron pair acceptor 
D) proton acceptor 
E) produces hydroxide ions in aqueous solution
F)proton donor 
A) electron pair donor 
B) produces protons in aqueous solution 
C) electron pair acceptor 
D) proton acceptor 
E) produces hydroxide ions in aqueous solution
F)proton donor

Question 15

Identify the diprotic acid.

Accepted Answer

A)  HNO3 
B)  HCl 
C)  CH3COOH 
D)  H2SO4 
E)  HClO4 
A)  HNO3 
B)  HCl 
C)  CH3COOH 
D)  H2SO4 
E)  HClO4

Question 16

Determine the [OH-] concentration of a 0.116 mol L-1 Ba(OH)2 solution at 25 °C.

Accepted Answer

A)  4.310 × 10-14 mol L-1 
B)  0.116 mol L-1 
C)  0.232 mol L-1 
D)  8.62 × 10-14 mol L-1 
E)  0.058 mol L-1 
A)  4.310 × 10-14 mol L-1 
B)  0.116 mol L-1 
C)  0.232 mol L-1 
D)  8.62 × 10-14 mol L-1 
E)  0.058 mol L-1

Question 17

Which one of the following salts, when dissolved in water, produces the solution with the lowest pH?

Accepted Answer

A)  NaCl 
B)  KCl 
C)  MgCl2 
D)  AlCl3 
A)  NaCl 
B)  KCl 
C)  MgCl2 
D)  AlCl3

Question 18

What is the hydronium ion concentration of a 0. 500 mol L-1 acetic acid solution with Ka = 1.8 × 10-5? The equation for the dissociation of acetic acid is below: CH3CO2H(aq)+H2O(l) ⇌ H3O+(aq)+CH3CO2-(aq)

Accepted Answer

A)  3.0 × 10-2 mol L-1 
B)  4.2 × 10-2 mol L-1 
C)  3.0 × 10-3 mol L-1 
D)  4.2 × 10-3 mol L-1 
A)  3.0 × 10-2 mol L-1 
B)  4.2 × 10-2 mol L-1 
C)  3.0 × 10-3 mol L-1 
D)  4.2 × 10-3 mol L-1

Question 19

Determine the pH of a 0.00598 mol L-1 HClO4 solution.

Accepted Answer

A)  1.777 
B)  6.434 
C)  7.566 
D)  2.223 
E)  3.558 
A)  1.777 
B)  6.434 
C)  7.566 
D)  2.223 
E)  3.558

Question 20

Describe a molecule that can be a Lewis acid.

Accepted Answer

A molecule with an i

Exam 15: Acids and Bases

The pH of a solution is 9.12 at 25 °C. Calculate the pOH of this solution at 25 °C.

What is the hydronium ion concentration of an acid rain sample that has a pH of 3. 45?

Calculate the pH of a 0.200 mol L-1 solution of formic acid, Ka = 1.8 × 10-4.

Calculate the pOH of an aqueous solution with a pH of 9.85 at 25 °C.

In a triprotic acid, which Ka has the highest value?

Which of the following is a weak acid?

Which of the following is an acid-base neutral ion?

Which of the following is a triprotic acid?

What is the autoionization of water?

Determine the pH of a 0.227 mol L-1 C5H5N solution at 25 °C. The Kb of C5H5N is 1.7 × 10-9.

On which equilibrium does the strength of an acid HA depend on?

Which of the following species is amphoteric?

Determine the [OH-] concentration of a 0.741 mol L-1 KOH solution at 25 °C.

Match the following. -Bronsted-Lowry acid

Identify the diprotic acid.

Determine the [OH-] concentration of a 0.116 mol L-1 Ba(OH)2 solution at 25 °C.

Which one of the following salts, when dissolved in water, produces the solution with the lowest pH?

What is the hydronium ion concentration of a 0. 500 mol L-1 acetic acid solution with Ka = 1.8 × 10-5? The equation for the dissociation of acetic acid is below: CH3CO2H(aq)+H2O(l) ⇌ H3O+(aq)+CH3CO2-(aq)

Determine the pH of a 0.00598 mol L-1 HClO4 solution.

Describe a molecule that can be a Lewis acid.

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry Ii: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

Calculate the pH of a 0.200 mol L^-1 solution of formic acid, K_a = 1.8 × 10^-4.

In a triprotic acid, which K_a has the highest value?

Determine the pH of a 0.227 mol L^-1 C₅H₅N solution at 25 °C. The K_b of C₅H₅N is 1.7 × 10^-9.

Determine the [OH^-] concentration of a 0.741 mol L^-1 KOH solution at 25 °C.

Determine the [OH^-] concentration of a 0.116 mol L^-1 Ba(OH)₂ solution at 25 °C.

What is the hydronium ion concentration of a 0. 500 mol L^-1 acetic acid solution with K_a = 1.8 × 10^-5? The equation for the dissociation of acetic acid is below: CH₃CO₂H(aq)+H₂O(l) ⇌ H₃O+(aq)+CH₃CO₂^-(aq)

Determine the pH of a 0.00598 mol L^-1 HClO₄ solution.