Question 1

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges.0.1 M methylamine (pKb = 3.36)

Accepted Answer

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

Question 2

Calculate the pH of a solution made by mixing equal volumes of a solution of HCl with a pH of 1.52 and a solution of HNO3 with a pH of 2.44. (Assume the volumes are additive.)

Accepted Answer

A)  3.97 
B)  1.98 
C)  2.44 
D)  1.77 
E)  1.47 
A)  3.97 
B)  1.98 
C)  2.44 
D)  1.77 
E)  1.47 D

Question 3

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

Accepted Answer

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

Question 4

As water is heated, its pH decreases. This means that

Accepted Answer

A)  [OH-] > [H+]. 
B)  [H+] > [OH-]. 
C)  the water is no longer neutral. 
D)  Two of these are correct. 
E)  None of these is correct. 
A)  [OH-] > [H+]. 
B)  [H+] > [OH-]. 
C)  the water is no longer neutral. 
D)  Two of these are correct. 
E)  None of these is correct.

Question 5

A 0.10-mol sample of a diprotic acid, H2A, is dissolved in 250 mL of water. Ka1 for this acid is 1.0 × 10-5 and Ka2 is 1.0 × 10-10. Calculate the concentration of A2- in this solution.

Accepted Answer

A)  2.0 × 10-3 M 
B)  4.0 × 10-6 M 
C)  0.40 M 
D)  1.0 × 10-10 M 
E)  1.0 × 10-5 M 
A)  2.0 × 10-3 M 
B)  4.0 × 10-6 M 
C)  0.40 M 
D)  1.0 × 10-10 M 
E)  1.0 × 10-5 M

Question 6

The salt BX, when dissolved in water, produces an acidic solution. Which of the following could be true?

Accepted Answer

A)  HX is a weak acid. 
B)  The cation B+ is a weak acid. 
C)  HX is a strong acid. 
D)  All of these could be true. 
E)  Both HX and the cation B+ are weak acids. 
A)  HX is a weak acid. 
B)  The cation B+ is a weak acid. 
C)  HX is a strong acid. 
D)  All of these could be true. 
E)  Both HX and the cation B+ are weak acids.

Question 7

For the equilibrium that exists in an aqueous solution of nitrous acid (HNO2, a weak acid), the equilibrium constant expression is

Accepted Answer

A)    
B)    
C)    
D)  K = [H+][NO2-] 
E)  none of these 
A)    
B)    
C)    
D)  K = [H+][NO2-] 
E)  none of these

Question 8

HCl gas is in a 1.21-L cylinder at 0.870 atm and 28.0° C. This gas is dissolved in 750.0 mL of water. Calculate the pH of this solution (assume no volume change).

Accepted Answer

A)  0.950 
B)  2.52 
C)  1.25 
D)  1.37 
E)  none of these 
A)  0.950 
B)  2.52 
C)  1.25 
D)  1.37 
E)  none of these

Question 9

The pH of a 0.14 M solution of a weak monoprotic acid, HA, is 2.89. Calculate Ka for this acid.​

Accepted Answer

A)  ​1.7 × 10-6 
B)  1.2​​ × 10-5 
C)  ​7.7-10 
D)  ​1.4-4 
E)  ​1.3-3 
A)  ​1.7 × 10-6 
B)  1.2​​ × 10-5 
C)  ​7.7-10 
D)  ​1.4-4 
E)  ​1.3-3

Question 10

The equilibrium constant for the reaction, Is called 
A- + H+  HA

Accepted Answer

A)  Kb 
B)    
C)  KwKa 
D)    
E)  Ka 
A)  Kb 
B)    
C)  KwKa 
D)    
E)  Ka

Question 11

Identify the Brønsted acids and bases in the following equation (A = Brønsted acid, B = Brønsted base).HPO42- + HSO4-   H2PO4- + SO42-

Accepted Answer

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

Question 12

Calculate [H+] in a 1.0 M solution of Na2CO3 (for H2CO3, Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11).

Accepted Answer

A)  6.6 × 10-4 M 
B)  7.5 × 10-13 M 
C)  7.5 × 10-6 M 
D)  1.3 × 10-2 M 
E)  none of these 
A)  6.6 × 10-4 M 
B)  7.5 × 10-13 M 
C)  7.5 × 10-6 M 
D)  1.3 × 10-2 M 
E)  none of these

Question 13

The following three equations represent equilibria that lie far to the right.
HNOS1U1B13S1U1B0(aq) + CNS1U1P1-S1S1P0(aq)   HCN(aq) + NOS1U1B13S1U1B0S1U1P1-S1S1P0(aq)
HCN(aq) + OHS1U1P1-S1S1P0(aq)   HS1U1B12S1U1B0O(l) + CNS1U1P1-S1S1P0(aq)
HS1U1B12S1U1B0O(l) + CHS1U1B13S1U1B0OS1U1P1-S1S1P0(aq)   CHS1U1B13S1U1B0OH(aq) + OHS1U1P1-S1S1P0(aq)
-Identify the strongest base.

Accepted Answer

A)  CH3OH 
B)  CH3O- 
C)  H2O 
D)  NO3- 
E)  CN- 
A)  CH3OH 
B)  CH3O- 
C)  H2O 
D)  NO3- 
E)  CN-

Question 14

Explain why the pH of an aqueous solution of NaHCO3 is independent of concentration.

Accepted Answer

See Sectio

Question 15

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges.
-0.5 M NaHCO3 (pKa1 = 6.37; pKa2 = 10.25)

Accepted Answer

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

Question 16

What is [OH-] in a 0.50 M pyridine (C5H5N; Kb = 1.7 × 10-9) solution?

Accepted Answer

A)  1.8 × 10-9 M 
B)  2.9 × 10-5 M 
C)  0.50 M 
D)  3.3 × 10-10 M 
E)  none of these 
A)  1.8 × 10-9 M 
B)  2.9 × 10-5 M 
C)  0.50 M 
D)  3.3 × 10-10 M 
E)  none of these

Question 17

How many moles of benzoic acid, a monoprotic acid with Ka = 6.4 × 10-5, must be dissolved in 500. mL of H2O to produce a solution with pH = 2.50?

Accepted Answer

A)  1.6 × 10-1 
B)  2.0 × 10-2 
C)  7.8 × 10-2 
D)  0.50 
E)  none of these 
A)  1.6 × 10-1 
B)  2.0 × 10-2 
C)  7.8 × 10-2 
D)  0.50 
E)  none of these

Question 18

Arrange the following 0.10 M solutions from lowest to highest pH: NaF, NaC2H3O2, C5H5NHCl, KOH, HCN. (Ka for HCN is 6.2 × 10-10; Ka for HF is 7.2 × 10-4; Ka for HC2H3O2 is 1.8 × 10-5; and Kb for C5H5N is 1.7 × 10-9)

Accepted Answer

A)  C5H5NHCl, HCN, NaF, NaC2H3O2, KOH 
B)  NaF, NaC2H3O2, HCN, C5H5NHCl, KOH 
C)  KOH, NaC2H3O2, NaF, HCN, C5H5NHCl 
D)  HCN, C5H5NHCl, NaF, NaC2H3O2, KOH 
E)  none of these 
A)  C5H5NHCl, HCN, NaF, NaC2H3O2, KOH 
B)  NaF, NaC2H3O2, HCN, C5H5NHCl, KOH 
C)  KOH, NaC2H3O2, NaF, HCN, C5H5NHCl 
D)  HCN, C5H5NHCl, NaF, NaC2H3O2, KOH 
E)  none of these

Question 19

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges.
-1.0 × 10-12 M HCl

Accepted Answer

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

Question 20

Calculate the pH of a solution made by mixing equal volumes of a solution of NaOH with a pH of 11.40 and a solution of KOH with a pH of 10.30. (Assume the volumes are additive.)

Accepted Answer

A)  11.13 
B)  1.10 
C)  10.85 
D)  21.70 
E)  none of these 
A)  11.13 
B)  1.10 
C)  10.85 
D)  21.70 
E)  none of these

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges.0.1 M methylamine (pK_b = 3.36)

Calculate the pH of a solution made by mixing equal volumes of a solution of HCl with a pH of 1.52 and a solution of HNO₃ with a pH of 2.44. (Assume the volumes are additive.)

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

As water is heated, its pH decreases. This means that

A 0.10-mol sample of a diprotic acid, H₂A, is dissolved in 250 mL of water. K_a1 for this acid is 1.0 × 10^-5 and K_a2 is 1.0 × 10^-10. Calculate the concentration of A^2- in this solution.

The salt BX, when dissolved in water, produces an acidic solution. Which of the following could be true?

For the equilibrium that exists in an aqueous solution of nitrous acid (HNO₂, a weak acid), the equilibrium constant expression is

HCl gas is in a 1.21-L cylinder at 0.870 atm and 28.0° C. This gas is dissolved in 750.0 mL of water. Calculate the pH of this solution (assume no volume change).

The pH of a 0.14 M solution of a weak monoprotic acid, HA, is 2.89. Calculate K_a for this acid.

The equilibrium constant for the reaction, Is called A^- + H⁺ HA

Identify the Brønsted acids and bases in the following equation (A = Brønsted acid, B = Brønsted base).HPO₄^2- + HSO₄^- H₂PO₄^- + SO₄^2-

Calculate [H⁺] in a 1.0 M solution of Na₂CO₃ (for H₂CO₃, K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11).

The following three equations represent equilibria that lie far to the right. HNO₃(aq) + CN^-(aq) HCN(aq) + NO₃^-(aq) HCN(aq) + OH^-(aq) H₂O(l) + CN^-(aq) H₂O(l) + CH₃O^-(aq) CH₃OH(aq) + OH^-(aq) -Identify the strongest base.

Explain why the pH of an aqueous solution of NaHCO₃ is independent of concentration.

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges. -0.5 M NaHCO₃ (pK_a1 = 6.37; pK_a2 = 10.25)

What is [OH^-] in a 0.50 M pyridine (C₅H₅N; K_b = 1.7 × 10^-9) solution?

How many moles of benzoic acid, a monoprotic acid with K_a = 6.4 × 10^-5, must be dissolved in 500. mL of H₂O to produce a solution with pH = 2.50?

Arrange the following 0.10 M solutions from lowest to highest pH: NaF, NaC₂H₃O₂, C₅H₅NHCl, KOH, HCN. (K_a for HCN is 6.2 × 10^-10; K_a for HF is 7.2 × 10^-4; K_a for HC₂H₃O₂ is 1.8 × 10^-5; and K_b for C₅H₅N is 1.7 × 10^-9)

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges. -1.0 × 10^-12 M HCl

Calculate the pH of a solution made by mixing equal volumes of a solution of NaOH with a pH of 11.40 and a solution of KOH with a pH of 10.30. (Assume the volumes are additive.)

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

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Exam 7: Acids and Bases

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges.0.1 M methylamine (pKb = 3.36)

Calculate the pH of a solution made by mixing equal volumes of a solution of HCl with a pH of 1.52 and a solution of HNO3 with a pH of 2.44. (Assume the volumes are additive.)

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

As water is heated, its pH decreases. This means that

A 0.10-mol sample of a diprotic acid, H2A, is dissolved in 250 mL of water. Ka1 for this acid is 1.0 × 10-5 and Ka2 is 1.0 × 10-10. Calculate the concentration of A2- in this solution.

The salt BX, when dissolved in water, produces an acidic solution. Which of the following could be true?

For the equilibrium that exists in an aqueous solution of nitrous acid (HNO2, a weak acid), the equilibrium constant expression is

HCl gas is in a 1.21-L cylinder at 0.870 atm and 28.0° C. This gas is dissolved in 750.0 mL of water. Calculate the pH of this solution (assume no volume change).

The pH of a 0.14 M solution of a weak monoprotic acid, HA, is 2.89. Calculate Ka for this acid.​

The equilibrium constant for the reaction, Is called A- + H+ HA

Identify the Brønsted acids and bases in the following equation (A = Brønsted acid, B = Brønsted base).HPO42- + HSO4- H2PO4- + SO42-

Calculate [H+] in a 1.0 M solution of Na2CO3 (for H2CO3, Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11).

The following three equations represent equilibria that lie far to the right. HNO3(aq) + CN-(aq) HCN(aq) + NO3-(aq) HCN(aq) + OH-(aq) H2O(l) + CN-(aq) H2O(l) + CH3O-(aq) CH3OH(aq) + OH-(aq) -Identify the strongest base.

Explain why the pH of an aqueous solution of NaHCO3 is independent of concentration.

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges. -0.5 M NaHCO3 (pKa1 = 6.37; pKa2 = 10.25)

What is [OH-] in a 0.50 M pyridine (C5H5N; Kb = 1.7 × 10-9) solution?

How many moles of benzoic acid, a monoprotic acid with Ka = 6.4 × 10-5, must be dissolved in 500. mL of H2O to produce a solution with pH = 2.50?

Arrange the following 0.10 M solutions from lowest to highest pH: NaF, NaC2H3O2, C5H5NHCl, KOH, HCN. (Ka for HCN is 6.2 × 10-10; Ka for HF is 7.2 × 10-4; Ka for HC2H3O2 is 1.8 × 10-5; and Kb for C5H5N is 1.7 × 10-9)

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges. -1.0 × 10-12 M HCl

Calculate the pH of a solution made by mixing equal volumes of a solution of NaOH with a pH of 11.40 and a solution of KOH with a pH of 10.30. (Assume the volumes are additive.)

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

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges.0.1 M methylamine (pK_b = 3.36)

Calculate the pH of a solution made by mixing equal volumes of a solution of HCl with a pH of 1.52 and a solution of HNO₃ with a pH of 2.44. (Assume the volumes are additive.)

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

A 0.10-mol sample of a diprotic acid, H₂A, is dissolved in 250 mL of water. K_a1 for this acid is 1.0 × 10^-5 and K_a2 is 1.0 × 10^-10. Calculate the concentration of A^2- in this solution.

For the equilibrium that exists in an aqueous solution of nitrous acid (HNO₂, a weak acid), the equilibrium constant expression is

The pH of a 0.14 M solution of a weak monoprotic acid, HA, is 2.89. Calculate K_a for this acid.

The equilibrium constant for the reaction, Is called A^- + H⁺ HA

Identify the Brønsted acids and bases in the following equation (A = Brønsted acid, B = Brønsted base).HPO₄^2- + HSO₄^- H₂PO₄^- + SO₄^2-

Calculate [H⁺] in a 1.0 M solution of Na₂CO₃ (for H₂CO₃, K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11).

The following three equations represent equilibria that lie far to the right. HNO₃(aq) + CN^-(aq) HCN(aq) + NO₃^-(aq) HCN(aq) + OH^-(aq) H₂O(l) + CN^-(aq) H₂O(l) + CH₃O^-(aq) CH₃OH(aq) + OH^-(aq) -Identify the strongest base.

Explain why the pH of an aqueous solution of NaHCO₃ is independent of concentration.

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges. -0.5 M NaHCO₃ (pK_a1 = 6.37; pK_a2 = 10.25)

What is [OH^-] in a 0.50 M pyridine (C₅H₅N; K_b = 1.7 × 10^-9) solution?

How many moles of benzoic acid, a monoprotic acid with K_a = 6.4 × 10^-5, must be dissolved in 500. mL of H₂O to produce a solution with pH = 2.50?

Arrange the following 0.10 M solutions from lowest to highest pH: NaF, NaC₂H₃O₂, C₅H₅NHCl, KOH, HCN. (K_a for HCN is 6.2 × 10^-10; K_a for HF is 7.2 × 10^-4; K_a for HC₂H₃O₂ is 1.8 × 10^-5; and K_b for C₅H₅N is 1.7 × 10^-9)

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges. -1.0 × 10^-12 M HCl