Question 1

What is the OH- concentration of an aqueous solution with a pH of 9.83? (Kw = 1.01 × 10-14)

Accepted Answer

A)  1.3 × 10-10 M 
B)  6.8 × 10-5 M 
C)  6.8 × 10-1 M 
D)  1.5 × 10-2 M 
E)  7.4 × 109 M 
A)  1.3 × 10-10 M 
B)  6.8 × 10-5 M 
C)  6.8 × 10-1 M 
D)  1.5 × 10-2 M 
E)  7.4 × 109 M

Question 2

Which of the following molecules or ions is the strongest acid?

Accepted Answer

A)  CH3CO2- 
B)  CH3CO2H 
C)  CFH2CO2H 
D)  CF2HCO2H 
E)  CF3CO2H 
A)  CH3CO2- 
B)  CH3CO2H 
C)  CFH2CO2H 
D)  CF2HCO2H 
E)  CF3CO2H

Question 3

What is the pH of the solution which results from mixing 50.0 mL of 0.30 M HF(aq)and 50.0 mL of 0.30 M NaOH(aq)at 25 °C? (Ka of HF = 7.2 × 10-4)

Accepted Answer

A)  1.98 
B)  5.84 
C)  8.16 
D)  10.85 
E)  12.02 
A)  1.98 
B)  5.84 
C)  8.16 
D)  10.85 
E)  12.02

Question 4

An aqueous solution with a pH of 10.60 is diluted from 1.0 L to 2.0 L.What is the pH of the diluted solution?

Accepted Answer

A)  5.30 
B)  9.60 
C)  10.30 
D)  10.60 
E)  10.90 
A)  5.30 
B)  9.60 
C)  10.30 
D)  10.60 
E)  10.90

Question 5

What is the equilibrium pH of an initially 0.83 M solution of the monoprotic acid 3-chloropropanoic acid at 25°C (Ka =   )?

Accepted Answer

A)  2.10 
B)  7.00 
C)  1.79 
D)  12.21 
E)  5.21 
A)  2.10 
B)  7.00 
C)  1.79 
D)  12.21 
E)  5.21

Question 6

A molecule that can behave as either a Brønsted-Lowry acid or base is termed ________.

Accepted Answer

amphiproti

Question 7

Given the equilibrium constants for the equilibria, H2O(l)   H3O+(aq); K =   2CH3COOH(aq)+ 2H2O(l)   2CH3COO−(aq)+ 2H3O+(aq); K =   determine Kc for the following equilibrium.
CH3COOH(aq)+ NH3(aq)   CH3COO−(aq)+ NH4+(aq)

Accepted Answer

A)  3.08 × 104 
B)  3.25 × 10-5 
C)  9.96 × 10-15 
D)  1.00 × 1014 
E)  1.75 × 10-5 
A)  3.08 × 104 
B)  3.25 × 10-5 
C)  9.96 × 10-15 
D)  1.00 × 1014 
E)  1.75 × 10-5

Question 8

Which of the following statements about the reaction below is correct? HCO3-(aq)+ H2O(   )   CO32-(aq)+ H3O+(aq)

Accepted Answer

A)  H3O+ is an acid and HCO3- is its conjugate base. 
B)  HCO3- is an acid and CO32- is its conjugate base. 
C)  HCO3- is an acid and H2O is its conjugate base. 
D)  H2O is an acid and CO32- is its conjugate base. 
E)  H3O+ is an acid and CO32- is its conjugate base. 
A)  H3O+ is an acid and HCO3- is its conjugate base. 
B)  HCO3- is an acid and CO32- is its conjugate base. 
C)  HCO3- is an acid and H2O is its conjugate base. 
D)  H2O is an acid and CO32- is its conjugate base. 
E)  H3O+ is an acid and CO32- is its conjugate base.

Question 9

What is the pH of a 0.046 M HClO4(aq)at 25 °C? (Kw = 1.01 × 10-14)

Accepted Answer

A)  15.34 
B)  3.08 
C)  12.66 
D)  1.34 
E)  10.92 
A)  15.34 
B)  3.08 
C)  12.66 
D)  1.34 
E)  10.92

Question 10

Which of the following species is the strongest acid in an aqueous solution?

Accepted Answer

A)  CH3CH2CO2H 
B)  CH2ClCO2H 
C)  CH3CO2H 
D)  CCl3CO2H 
E)  CHCl2CO2H 
A)  CH3CH2CO2H 
B)  CH2ClCO2H 
C)  CH3CO2H 
D)  CCl3CO2H 
E)  CHCl2CO2H

Question 11

What is the pH of a solution prepared by dissolving 0.523 g of NaOH(s)in 5.50 L of water? (Kw = 1.01 × 10-14)

Accepted Answer

A)  1.884 
B)  12.116 
C)  7.000 
D)  11.376 
E)  2.624 
A)  1.884 
B)  12.116 
C)  7.000 
D)  11.376 
E)  2.624

Question 12

Write a net ionic equation for the neutralization reaction of hydrochloric acid and potassium hydroxide.Identify the spectator ion(s).

Accepted Answer

Net ionic equation:

Question 13

Which of the following does not behave as an amphiprotic species in water?

Accepted Answer

A)  HClO3 
B)  HSO3- 
C)  H3O+ 
D)  HS- 
E)  HCO3- 
A)  HClO3 
B)  HSO3- 
C)  H3O+ 
D)  HS- 
E)  HCO3-

Question 14

Consider the reaction CO32-(aq)+ H2O(l)   HCO3-(aq)+ OH-(aq).Kb for CO32- is 2.1 × 10-4 at 25°C.What is Ka for the HCO3- ion at 25°C?

Accepted Answer

A)  4.8 × 103 
B)  4.8 × 10-11 
C)  2.1 × 10-4 
D)  7.2 × 10-12 
E)  9.2 × 10-8 
A)  4.8 × 103 
B)  4.8 × 10-11 
C)  2.1 × 10-4 
D)  7.2 × 10-12 
E)  9.2 × 10-8

Question 15

Which of the following statements is true of the acid-base properties of common cations and anions in aqueous solutions?

Accepted Answer

A)  The anions that are conjugate bases of strong acids are strong bases. 
B)  The acid-base behavior of anions of polyprotic acids is independent of the extent of deprotonation. 
C)  Alkali metal and alkali earth cations have no measurable effect on solution pH. 
D)  Basic anions are conjugate bases of acidic cations. 
E)  Basic cations are conjugate bases of weak acids. 
A)  The anions that are conjugate bases of strong acids are strong bases. 
B)  The acid-base behavior of anions of polyprotic acids is independent of the extent of deprotonation. 
C)  Alkali metal and alkali earth cations have no measurable effect on solution pH. 
D)  Basic anions are conjugate bases of acidic cations. 
E)  Basic cations are conjugate bases of weak acids.

Question 16

What is the hydroxide-ion concentration in a solution formed by combining 200.mL of 0.15 M HCl with 300.mL of 0.090 M NaOH at 25°C? HCl(aq)+ NaOH(aq)→ NaCl(aq)+ H2O(l)

Accepted Answer

A)  1.7 × 10-13 M 
B)  0.090 M 
C)  1.7 × 10-12 M 
D)  0.054 M 
E)  1.0 × 10-7 M 
A)  1.7 × 10-13 M 
B)  0.090 M 
C)  1.7 × 10-12 M 
D)  0.054 M 
E)  1.0 × 10-7 M

Question 17

Which of the following is the correct equation for the reaction of ammonia in water?

Accepted Answer

A)  NH3(aq)+ H2O(l)   NH4+(aq)+ OH−(aq) 
B)  NH3(aq)+ H2O(l)   NH2−(aq)+ H3O+(aq) 
C)  NH3(aq)+ H3O+(aq)   NH4+(aq)+ H2O(l) 
D)  NH3(aq)+ OH−(aq)   NH2−(aq)+ H2O(l) 
E)  NH3(aq)+ H2O(l)   NH2−(aq)+ H3O+(aq) 
A)  NH3(aq)+ H2O(l)   NH4+(aq)+ OH−(aq) 
B)  NH3(aq)+ H2O(l)   NH2−(aq)+ H3O+(aq) 
C)  NH3(aq)+ H3O+(aq)   NH4+(aq)+ H2O(l) 
D)  NH3(aq)+ OH−(aq)   NH2−(aq)+ H2O(l) 
E)  NH3(aq)+ H2O(l)   NH2−(aq)+ H3O+(aq)

Question 18

A 0.10 M solution of a weak monoprotic acid has a hydronium-ion concentration of 8.0 × 10-4 M.What is the acid-ionization constant,Ka,for this acid?

Accepted Answer

A)  2.8 × 10-2 
B)  7.5 × 10-3 
C)  8.0 × 10-4 
D)  6.4 × 10-6 
E)  9.6 × 10-5 
A)  2.8 × 10-2 
B)  7.5 × 10-3 
C)  8.0 × 10-4 
D)  6.4 × 10-6 
E)  9.6 × 10-5

Question 19

What is the pH of the final solution when 25 mL of 0.021 M HCl has been added to 35 mL of 0.035 M HCl at 25°C?

Accepted Answer

A)  3.4 
B)  1.9 
C)  1.5 
D)  2.8 
E)  3.5 
A)  3.4 
B)  1.9 
C)  1.5 
D)  2.8 
E)  3.5

Question 20

What is the H3O+ concentration in 0.0055 M Ba(OH)2(aq)at 25 °C? (Kw = 1.01 × 10-14)?

Accepted Answer

A)  1.1 × 10-2 M 
B)  5.5 × 10-3 M 
C)  9.1 × 10-13 M 
D)  1.8 × 10-12 M 
E)  1.0 × 10-7 M 
A)  1.1 × 10-2 M 
B)  5.5 × 10-3 M 
C)  9.1 × 10-13 M 
D)  1.8 × 10-12 M 
E)  1.0 × 10-7 M

Exam 17: Principles of Chemical Reactivity: the Chemistry of Acids and Bases

What is the OH- concentration of an aqueous solution with a pH of 9.83? (Kw = 1.01 × 10-14)

Which of the following molecules or ions is the strongest acid?

What is the pH of the solution which results from mixing 50.0 mL of 0.30 M HF(aq)and 50.0 mL of 0.30 M NaOH(aq)at 25 °C? (Ka of HF = 7.2 × 10-4)

An aqueous solution with a pH of 10.60 is diluted from 1.0 L to 2.0 L.What is the pH of the diluted solution?

What is the equilibrium pH of an initially 0.83 M solution of the monoprotic acid 3-chloropropanoic acid at 25°C (Ka = )?

A molecule that can behave as either a Brønsted-Lowry acid or base is termed ________.

Given the equilibrium constants for the equilibria, H2O(l) H3O+(aq); K = 2CH3COOH(aq)+ 2H2O(l) 2CH3COO−(aq)+ 2H3O+(aq); K = determine Kc for the following equilibrium. CH3COOH(aq)+ NH3(aq) CH3COO−(aq)+ NH4+(aq)

Which of the following statements about the reaction below is correct? HCO3-(aq)+ H2O( ) CO32-(aq)+ H3O+(aq)

What is the pH of a 0.046 M HClO4(aq)at 25 °C? (Kw = 1.01 × 10-14)

Which of the following species is the strongest acid in an aqueous solution?

What is the pH of a solution prepared by dissolving 0.523 g of NaOH(s)in 5.50 L of water? (Kw = 1.01 × 10-14)

Write a net ionic equation for the neutralization reaction of hydrochloric acid and potassium hydroxide.Identify the spectator ion(s).

Which of the following does not behave as an amphiprotic species in water?

Consider the reaction CO32-(aq)+ H2O(l) HCO3-(aq)+ OH-(aq).Kb for CO32- is 2.1 × 10-4 at 25°C.What is Ka for the HCO3- ion at 25°C?

Which of the following statements is true of the acid-base properties of common cations and anions in aqueous solutions?

What is the hydroxide-ion concentration in a solution formed by combining 200.mL of 0.15 M HCl with 300.mL of 0.090 M NaOH at 25°C? HCl(aq)+ NaOH(aq)→ NaCl(aq)+ H2O(l)

Which of the following is the correct equation for the reaction of ammonia in water?

A 0.10 M solution of a weak monoprotic acid has a hydronium-ion concentration of 8.0 × 10-4 M.What is the acid-ionization constant,Ka,for this acid?

What is the pH of the final solution when 25 mL of 0.021 M HCl has been added to 35 mL of 0.035 M HCl at 25°C?

What is the H3O+ concentration in 0.0055 M Ba(OH)2(aq)at 25 °C? (Kw = 1.01 × 10-14)?

Basic Concepts of Chemistry

Lets Review: The Tools of Quantitative Chemistry

Atoms, molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

Filters

What is the OH^- concentration of an aqueous solution with a pH of 9.83? (K_w = 1.01 × 10^-14)

What is the pH of the solution which results from mixing 50.0 mL of 0.30 M HF(aq)and 50.0 mL of 0.30 M NaOH(aq)at 25 °C? (K_a of HF = 7.2 × 10^-4)

What is the equilibrium pH of an initially 0.83 M solution of the monoprotic acid 3-chloropropanoic acid at 25°C (K_a = )?

Given the equilibrium constants for the equilibria, H₂O(l) H₃O⁺(aq); K = 2CH₃COOH(aq)+ 2H₂O(l) 2CH₃COO−(aq)+ 2H₃O⁺(aq); K = determine K_c for the following equilibrium. CH₃COOH(aq)+ NH₃(aq) CH₃COO−(aq)+ NH₄⁺(aq)

Which of the following statements about the reaction below is correct? HCO₃^-(aq)+ H₂O( ) CO₃^2-(aq)+ H₃O⁺(aq)

What is the pH of a 0.046 M HClO₄(aq)at 25 °C? (K_w = 1.01 × 10^-14)

What is the pH of a solution prepared by dissolving 0.523 g of NaOH(s)in 5.50 L of water? (K_w = 1.01 × 10^-14)

Consider the reaction CO₃^2-(aq)+ H₂O(l) HCO₃^-(aq)+ OH^-(aq).K_b for CO₃^2- is 2.1 × 10^-4 at 25°C.What is K_a for the HCO₃^- ion at 25°C?

What is the hydroxide-ion concentration in a solution formed by combining 200.mL of 0.15 M HCl with 300.mL of 0.090 M NaOH at 25°C? HCl(aq)+ NaOH(aq)→ NaCl(aq)+ H₂O(l)

A 0.10 M solution of a weak monoprotic acid has a hydronium-ion concentration of 8.0 × 10^-4 M.What is the acid-ionization constant,K_a,for this acid?

What is the H₃O⁺ concentration in 0.0055 M Ba(OH)₂(aq)at 25 °C? (K_w = 1.01 × 10^-14)?