Question 1

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid ammonium nitrate  (NH4NO3)

Accepted Answer

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

Question 2

For nitrous acid, HNO2, Ka = 4.0 F1F1F1S1F1F1F10 10-4. Calculate the pH of 0.27 M HNO2.

Accepted Answer

A)  2.83 
B)  1.98 
C)  3.40 
D)  0.57 
E)  4.54 
A)  2.83 
B)  1.98 
C)  3.40 
D)  0.57 
E)  4.54

Question 3

Calculate [H+] in a 0.40 M solution of NaH2PO4. (For H3PO4, Ka1 = 7.5 F1F1F1S1F1F1F10 10-3, Ka2 = 6.2 F1F1F1S1F1F1F10 10-8, Ka3 = 4.8 F1F1F1S1F1F1F10 10-13)

Accepted Answer

A)  1.6 F1F1F1S1F1F1F10 10-4 M 
B)  2.5 F1F1F1S1F1F1F10 10-4 M 
C)  0.40 M 
D)  3.9 F1F1F1S1F1F1F10 10-11 M 
E)  2.2 F1F1F1S1F1F1F10 10-5 M 
A)  1.6 F1F1F1S1F1F1F10 10-4 M 
B)  2.5 F1F1F1S1F1F1F10 10-4 M 
C)  0.40 M 
D)  3.9 F1F1F1S1F1F1F10 10-11 M 
E)  2.2 F1F1F1S1F1F1F10 10-5 M

Question 4

Calculate [H+] in a solution that has a pH of 9.7.

Accepted Answer

A)  1 F1F1F1S1F1F1F10F1F1F1S1F1F1F1010-1 M 
B)  5 F1F1F1S1F1F1F10F1F1F1S1F1F1F1010-5 M 
C)  10 M 
D)  4 M 
E)  2 F1F1F1S1F1F1F10 10-10 M 
A)  1 F1F1F1S1F1F1F10F1F1F1S1F1F1F1010-1 M 
B)  5 F1F1F1S1F1F1F10F1F1F1S1F1F1F1010-5 M 
C)  10 M 
D)  4 M 
E)  2 F1F1F1S1F1F1F10 10-10 M

Question 5

A solution is made by mixing equal volumes of 0.20 M HCN (Ka = 6.2 * 10-10) and 0.20 M NH3 (Kb = 1.8 * 10-5). Determine the pH of the solution.

Accepted Answer

The answer of A solution is made by mixing equal...

Question 6

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 7

What is [OH-] in a 0.50 M pyridine (C5H5N; Kb = 1.7 F1F1F1S1F1F1F10 10-9) solution?

Accepted Answer

A)  1.8 F1F1F1S1F1F1F10 10-9 M 
B)  2.9 F1F1F1S1F1F1F10 10-5 M 
C)  0.50 M 
D)  3.3 F1F1F1S1F1F1F10 10-10 M 
E)  none of these 
A)  1.8 F1F1F1S1F1F1F10 10-9 M 
B)  2.9 F1F1F1S1F1F1F10 10-5 M 
C)  0.50 M 
D)  3.3 F1F1F1S1F1F1F10 10-10 M 
E)  none of these

Question 8

A 2.5 M solution of a weak acid is 0.52% ionized. What is Ka for this acid?

Accepted Answer

A)  1.3 F1F1F1S1F1F1F10 10-2 
B)  6.8 F1F1F1S1F1F1F10 10-5 
C)  0.11 
D)  1.1 F1F1F1S1F1F1F10 10-5 
E)  none of these 
A)  1.3 F1F1F1S1F1F1F10 10-2 
B)  6.8 F1F1F1S1F1F1F10 10-5 
C)  0.11 
D)  1.1 F1F1F1S1F1F1F10 10-5 
E)  none of these

Question 9

What is the pH of a 0.2 M solution of NH4Cl? Kb for NH3 is 1.8 F1F1F1S1F1F1F10 10-5.

Accepted Answer

A)  5.0 
B)  11.3 
C)  2.7 
D)  7.0 
E)  9.0 
A)  5.0 
B)  11.3 
C)  2.7 
D)  7.0 
E)  9.0

Question 10

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

Accepted Answer

A)  2.63 F1F1F1S1F1F1F10 10-11 
B)  3.80 F1F1F1S1F1F1F10 10-4 
C)  1.05 F1F1F1S1F1F1F10 10-5 
D)  6.60 F1F1F1S1F1F1F10 10-17 
E)  none of these 
A)  2.63 F1F1F1S1F1F1F10 10-11 
B)  3.80 F1F1F1S1F1F1F10 10-4 
C)  1.05 F1F1F1S1F1F1F10 10-5 
D)  6.60 F1F1F1S1F1F1F10 10-17 
E)  none of these

Question 11

In deciding which of two acids is the stronger, one must know

Accepted Answer

A)  the pH of each acid solution only. 
B)  the concentration of each acid solution only. 
C)  the equilibrium constant of each acid only. 
D)  all of the these. 
E)  both the concentration and the equilibrium constant of each acid. 
A)  the pH of each acid solution only. 
B)  the concentration of each acid solution only. 
C)  the equilibrium constant of each acid only. 
D)  all of the these. 
E)  both the concentration and the equilibrium constant of each acid.

Question 12

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

Question 13

Calculate the pH of a 1.9 M solution of HNO3.

Accepted Answer

A)  -0.64 
B)  -0.28 
C)  14.28 
D)  13.72 
E)  0.28 
A)  -0.64 
B)  -0.28 
C)  14.28 
D)  13.72 
E)  0.28

Question 14

Calculate the pH of a solution made by a mixture of the following acids: 0.40 M HC2H3O2 (Ka = 1.8 F1F1F1S1F1F1F10 10-5), 0.10 M HOCl (Ka = 3.5 F1F1F1S1F1F1F10 10-8), and 0.20 M HCN (Ka = 6.2 F1F1F1S1F1F1F10 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 15

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 F1F1F1S1F1F1F10 10-6 
B)  6.3 F1F1F1S1F1F1F10 10-4 
C)  7.2 F1F1F1S1F1F1F10 10-5 
D)  3.2 
E)  none of these 
A)  4.0 F1F1F1S1F1F1F10 10-6 
B)  6.3 F1F1F1S1F1F1F10 10-4 
C)  7.2 F1F1F1S1F1F1F10 10-5 
D)  3.2 
E)  none of these

Question 16

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

Accepted Answer

See Sectio

Question 17

A 2.58-g sample of NaOH(s) is added to enough water to make 600.0 mL of solution at 25°C. What is the pH of this solution?

Accepted Answer

A)  10.03 
B)  0.97 
C)  13.03 
D)  14.63 
E)  12.59 
A)  10.03 
B)  0.97 
C)  13.03 
D)  14.63 
E)  12.59

Question 18

Which of the following aqueous solutions will have the highest pH? For NH3, Kb = 1.8 F1F1F1S1F1F1F10 10-5; for C2H3O2-, Kb = 5.6 F1F1F1S1F1F1F10 10-10.

Accepted Answer

A)  2.0 M NH3 
B)  2.0 M HCl 
C)  2.0 M NaOH 
D)  2.0 M HC2H3O2 
E)  All these solutions will have the same pH. 
A)  2.0 M NH3 
B)  2.0 M HCl 
C)  2.0 M NaOH 
D)  2.0 M HC2H3O2 
E)  All these solutions will have the same pH.

Question 19

According to the Brønsted-Lowry definition, an acid is

Accepted Answer

A)  a substance that can donate a proton to another species. 
B)  a substance that increases the hydroxide ion concentration in a solution. 
C)  a substance that can accept a proton from another species in solution. 
D)  an electron pair acceptor. 
E)  a substance that increases the hydrogen ion concentration in a solution. 
A)  a substance that can donate a proton to another species. 
B)  a substance that increases the hydroxide ion concentration in a solution. 
C)  a substance that can accept a proton from another species in solution. 
D)  an electron pair acceptor. 
E)  a substance that increases the hydrogen ion concentration in a solution.

Question 20

Which of the species below, when dissolved in H2O, will not produce a basic solution?

Accepted Answer

A)  Ba(OH)2 
B)  NH3 
C)  SO2 
D)  BaO 
E)  none of these; that is, they all will produce a basic solution 
A)  Ba(OH)2 
B)  NH3 
C)  SO2 
D)  BaO 
E)  none of these; that is, they all will produce a basic solution

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid ammonium nitrate (NH₄NO₃)

For nitrous acid, HNO₂, K_a = 4.0  10^-⁴. Calculate the pH of 0.27 M HNO₂.

Calculate [H⁺] in a 0.40 M solution of NaH₂PO₄. (For H₃PO₄, K_a1 = 7.5  10^-³, K_a2 = 6.2  10^-⁸, K_a3 = 4.8  10^-¹³)

Calculate [H⁺] in a solution that has a pH of 9.7.

A solution is made by mixing equal volumes of 0.20 M HCN (K_a = 6.2 * 10^-¹⁰) and 0.20 M NH₃ (K_b = 1.8 * 10^-⁵). Determine the pH of the solution.

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

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

A 2.5 M solution of a weak acid is 0.52% ionized. What is K_a for this acid?

What is the pH of a 0.2 M solution of NH₄Cl? K_b for NH₃ is 1.8  10^-⁵.

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

In deciding which of two acids is the stronger, one must know

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 1.9 M solution of HNO₃.

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?

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

A 2.58-g sample of NaOH(s) is added to enough water to make 600.0 mL of solution at 25°C. What is the pH of this solution?

Which of the following aqueous solutions will have the highest pH? For NH₃, K_b = 1.8  10^-⁵; for C₂H₃O₂^-, K_b = 5.6  10^-¹⁰.

According to the Brønsted-Lowry definition, an acid is

Which of the species below, when dissolved in H₂O, will not produce a basic solution?

Atoms, Molecules, and Ions

Stoichiometry

Chemical Reactions and Solutions 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

Exam 7: Acids and Bases

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid ammonium nitrate (NH4NO3)

For nitrous acid, HNO2, Ka = 4.0  10-4. Calculate the pH of 0.27 M HNO2.

Calculate [H+] in a 0.40 M solution of NaH2PO4. (For H3PO4, Ka1 = 7.5  10-3, Ka2 = 6.2  10-8, Ka3 = 4.8  10-13)

Calculate [H+] in a solution that has a pH of 9.7.

A solution is made by mixing equal volumes of 0.20 M HCN (Ka = 6.2 * 10-10) and 0.20 M NH3 (Kb = 1.8 * 10-5). Determine the pH of the solution.

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

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

A 2.5 M solution of a weak acid is 0.52% ionized. What is Ka for this acid?

What is the pH of a 0.2 M solution of NH4Cl? Kb for NH3 is 1.8  10-5.

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

In deciding which of two acids is the stronger, one must know

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 1.9 M solution of HNO3.

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).

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

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

A 2.58-g sample of NaOH(s) is added to enough water to make 600.0 mL of solution at 25°C. What is the pH of this solution?

Which of the following aqueous solutions will have the highest pH? For NH3, Kb = 1.8  10-5; for C2H3O2-, Kb = 5.6  10-10.

According to the Brønsted-Lowry definition, an acid is

Which of the species below, when dissolved in H2O, will not produce a basic solution?

Atoms, Molecules, and Ions

Stoichiometry

Chemical Reactions and Solutions 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

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid ammonium nitrate (NH₄NO₃)

For nitrous acid, HNO₂, K_a = 4.0  10^-⁴. Calculate the pH of 0.27 M HNO₂.

Calculate [H⁺] in a 0.40 M solution of NaH₂PO₄. (For H₃PO₄, K_a1 = 7.5  10^-³, K_a2 = 6.2  10^-⁸, K_a3 = 4.8  10^-¹³)

Calculate [H⁺] in a solution that has a pH of 9.7.

A solution is made by mixing equal volumes of 0.20 M HCN (K_a = 6.2 * 10^-¹⁰) and 0.20 M NH₃ (K_b = 1.8 * 10^-⁵). Determine the pH of the solution.

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

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

A 2.5 M solution of a weak acid is 0.52% ionized. What is K_a for this acid?

What is the pH of a 0.2 M solution of NH₄Cl? K_b for NH₃ is 1.8  10^-⁵.

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 methylamine (pK_b = 3.36)

Calculate the pH of a 1.9 M solution of HNO₃.

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?

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

Which of the following aqueous solutions will have the highest pH? For NH₃, K_b = 1.8  10^-⁵; for C₂H₃O₂^-, K_b = 5.6  10^-¹⁰.

Which of the species below, when dissolved in H₂O, will not produce a basic solution?