Question 1

Calculate the pH of a 0.14 M HNO2 solution that is 5.7% ionized.

Accepted Answer

A) 0.85 
B) 1.70 
C) 2.10 
D) 11.90 
E) 13.10 
A) 0.85 
B) 1.70 
C) 2.10 
D) 11.90 
E) 13.10

Question 2

What is the pH of an aqueous solution that contains 5.3 * 1017 OH- ions per liter of solution?

Accepted Answer

A) 5.30 
B) 6.06 
C) 7.94 
D) 8.70 
E) 11.3 
A) 5.30 
B) 6.06 
C) 7.94 
D) 8.70 
E) 11.3

Question 3

Consider the weak bases below and their Kb values: C6H7O Kb = 1.3 * 10-10
 C2H5NH2 Kb = 5.6 * 10-4
 C5H5N Kb = 1.7 * 10-9
 Arrange the conjugate acids of these weak bases in order of increasing acid strength.

Accepted Answer

A) C5H5NH+ 6H7OH 2H5NH 
B) C6H7OH 5H5NH+ 2H5NH 
C) C5H5NH+ 2H5NH3+ 6H7OH 
D) C6H7OH 2H5NH3+5H5NH+ 
E) C2H5NH3+5H5NH+ 6H7OH 
A) C5H5NH+ 6H7OH 2H5NH 
B) C6H7OH 5H5NH+ 2H5NH 
C) C5H5NH+ 2H5NH3+ 6H7OH 
D) C6H7OH 2H5NH3+5H5NH+ 
E) C2H5NH3+5H5NH+ 6H7OH

Question 4

Which one of these net ionic equations represents the reaction of a strong acid with a strong base?

Accepted Answer

A) H+(aq)+ OH-(aq)$\rarr$H2O(aq) 
B) H+(aq)+ CH3NH2(aq)$\rarr$CH3NH3+(aq) 
C) OH-(aq)+ HCN(aq)$\rarr$ H2O(aq)+ CN-(aq) 
D) HCN(aq)+ CH3NH2(aq)$\rarr$CH3NH3+(aq)+ CN-(aq) 
A) H+(aq)+ OH-(aq)$\rarr$H2O(aq) 
B) H+(aq)+ CH3NH2(aq)$\rarr$CH3NH3+(aq) 
C) OH-(aq)+ HCN(aq)$\rarr$ H2O(aq)+ CN-(aq) 
D) HCN(aq)+ CH3NH2(aq)$\rarr$CH3NH3+(aq)+ CN-(aq)

Question 5

Calculate the hydrogen ion concentration in a solution of iced tea with lemon having a pH of 2.87.

Accepted Answer

A) 2.9 * 10-2 M 
B) 5.7 * 10-2 M 
C) 1.3 * 10-3 M 
D) 2.9 * 10-3 M 
E) 5.7 * 10-4 M 
A) 2.9 * 10-2 M 
B) 5.7 * 10-2 M 
C) 1.3 * 10-3 M 
D) 2.9 * 10-3 M 
E) 5.7 * 10-4 M

Question 6

The oxides SO2 and N2O5 will form the following acids in water, respectively.

Accepted Answer

A) H2SO4(aq)and HNO3(aq) 
B) H2SO3(aq)and HNO3(aq) 
C) H2SO4(aq)and HNO2(aq) 
D) H2SO3(aq)and HNO2(aq) 
E) H2S(aq)and HNO3(aq) 
A) H2SO4(aq)and HNO3(aq) 
B) H2SO3(aq)and HNO3(aq) 
C) H2SO4(aq)and HNO2(aq) 
D) H2SO3(aq)and HNO2(aq) 
E) H2S(aq)and HNO3(aq)

Question 7

Predict the direction in which the equilibrium will lie for the reaction H3PO4(aq)+ HSO4-(aq)$\rarr$ H2PO4-(aq) + H2SO4(aq).
Ka1(H3PO4)= 7.5 * 10-3; Ka(H2SO4)= very large

Accepted Answer

A) to the right 
B) to the left 
C) in the middle 
A) to the right 
B) to the left 
C) in the middle

Question 8

A solution containing NH3(aq)and NH4Cl(aq)has a pH of 9.5. What is the [NH3]/[NH4+] ratio in this solution? (For ammonia, Kb = 1.8 *  10-5.)

Accepted Answer

The answer of A solution containing NH3(aq)and NH4Cl(aq)has a pH...

Question 9

Calculate the hydrogen ion concentration in a solution of fruit juice having a pH of 4.25.

Accepted Answer

A) 1.0 * 10-14 M 
B) 5.6 * 10-5 M 
C) 4.0 * 10-25 M 
D) 2.5 * 10-4 M 
E) 5.6 * 10-4 M 
A) 1.0 * 10-14 M 
B) 5.6 * 10-5 M 
C) 4.0 * 10-25 M 
D) 2.5 * 10-4 M 
E) 5.6 * 10-4 M

Question 10

Arrange the acids HOCl, HClO3, and HClO2 in order of increasing acid strength.

Accepted Answer

A) HOCl 3 2 
B) HOCl 2 3 
C) HClO2 3 
D) HClO3 2 
E) HClO3 2 < HOCl 
A) HOCl 3 2 
B) HOCl 2 3 
C) HClO2 3 
D) HClO3 2 
E) HClO3 2 < HOCl

Question 11

Calculate the hydrogen ion concentration in a solution having a pH of 4.60.

Accepted Answer

A) 4.0 * 10-3 M 
B) 4.0 * 10-9 M 
C) 4.0 * 10-10 M 
D) 2.5 * 10-5 M 
E) 2.5 * 10-4 M 
A) 4.0 * 10-3 M 
B) 4.0 * 10-9 M 
C) 4.0 * 10-10 M 
D) 2.5 * 10-5 M 
E) 2.5 * 10-4 M

Question 12

Write the chemical formula for sulfuric acid.

Accepted Answer

The answer of Write the chemical formula for sulfuric acid....

Question 13

Which of these lists of molecules is arranged in order of increasing acid strength?

Accepted Answer

A) H2S 2O 2Se 
B) H2O 2S 2Se 
C) H2Se 2O 2S 
D) H2S 2Se 2O 
E) H2O 2Se 2S 
A) H2S 2O 2Se 
B) H2O 2S 2Se 
C) H2Se 2O 2S 
D) H2S 2Se 2O 
E) H2O 2Se 2S

Question 14

Hydrosulfuric acid is a diprotic acid, for which Ka1 = 5.7 * 10-8 and Ka2 = 1 *10-19. Determine the concentration of sulfide ion in a 0.10 M hydrosulfuric solution.

Accepted Answer

A) 0.10 M 
B) 7.5 * 10-5 M 
C) 5.7 * 10-9 M 
D) 1 * 10-19 M 
E) 1 * 10-20 M 
A) 0.10 M 
B) 7.5 * 10-5 M 
C) 5.7 * 10-9 M 
D) 1 * 10-19 M 
E) 1 * 10-20 M

Question 15

Predict the direction in which the equilibrium will lie for the reaction C6H5COO- + HF  $\rarr$ C6H5COOH + F- . 
 Ka(C6H5COOH)= 6.5 * 10-5; Ka(HF)= 7.1 * 10-4

Accepted Answer

A) to the right 
B) to the left 
C) in the middle 
A) to the right 
B) to the left 
C) in the middle

Question 16

Arrange the acids H2Se, H2Te, and H2S in order of increasing acid strength.

Accepted Answer

A) H2S 2Se 2Te 
B) H2S 2Te 2Se 
C) H2Te 2S 2Se 
D) H2Se 2S 2Te 
E) H2Se 2Te 2S 
A) H2S 2Se 2Te 
B) H2S 2Te 2Se 
C) H2Te 2S 2Se 
D) H2Se 2S 2Te 
E) H2Se 2Te 2S

Question 17

If the pH of stomach acid is 1.0, what is the hydroxide ion concentration in this solution?

Accepted Answer

1 * 10<sup

Question 18

For H3PO4, Ka1 = 7.3 * 10-3, Ka2 = 6.2 * 10-6, and Ka3 = 4.8 * 10-13. An aqueous solution of Na3PO4 therefore would be

Accepted Answer

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

Question 19

Suppose that ammonia, applied to a field as a fertilizer, is washed into a farm pond containing 3.0 * 106 L of water. If the pH of this pond is found to be 9.81, what volume of liquid ammonia found its way into the pond? [Given: Kb(NH3)= 1.8 * 10-5; the density of liquid ammonia is 0.771 g/cm3]

Accepted Answer

A) 15 L 
B) 25 L 
C) 11 L 
D) 19 L 
E) 320 L 
A) 15 L 
B) 25 L 
C) 11 L 
D) 19 L 
E) 320 L

Question 20

The pH of a certain solution is 2.0. How many H+(aq)ions are there in 1.0 L of the solution?

Accepted Answer

A) 0.01 ions 
B) 100 ions 
C) 2 ions 
D) 6. * 1021 ions 
E) 6. * 1023 ions 
A) 0.01 ions 
B) 100 ions 
C) 2 ions 
D) 6. * 1021 ions 
E) 6. * 1023 ions

Exam 16: Acids and Bases

Calculate the pH of a 0.14 M HNO2 solution that is 5.7% ionized.

What is the pH of an aqueous solution that contains 5.3 * 1017 OH- ions per liter of solution?

Consider the weak bases below and their Kb values: C6H7O Kb = 1.3 * 10-10 C2H5NH2 Kb = 5.6 * 10-4 C5H5N Kb = 1.7 * 10-9 Arrange the conjugate acids of these weak bases in order of increasing acid strength.

Which one of these net ionic equations represents the reaction of a strong acid with a strong base?

Calculate the hydrogen ion concentration in a solution of iced tea with lemon having a pH of 2.87.

The oxides SO2 and N2O5 will form the following acids in water, respectively.

Predict the direction in which the equilibrium will lie for the reaction H3PO4(aq)+ HSO4-(aq) →\rarr→ H2PO4-(aq) + H2SO4(aq). Ka1(H3PO4)= 7.5 * 10-3; Ka(H2SO4)= very large

A solution containing NH3(aq)and NH4Cl(aq)has a pH of 9.5. What is the [NH3]/[NH4+] ratio in this solution? (For ammonia, Kb = 1.8 * 10-5.)

Calculate the hydrogen ion concentration in a solution of fruit juice having a pH of 4.25.

Arrange the acids HOCl, HClO3, and HClO2 in order of increasing acid strength.

Calculate the hydrogen ion concentration in a solution having a pH of 4.60.

Write the chemical formula for sulfuric acid.

Which of these lists of molecules is arranged in order of increasing acid strength?

Hydrosulfuric acid is a diprotic acid, for which Ka1 = 5.7 * 10-8 and Ka2 = 1 *10-19. Determine the concentration of sulfide ion in a 0.10 M hydrosulfuric solution.

Predict the direction in which the equilibrium will lie for the reaction C6H5COO- + HF →\rarr→ C6H5COOH + F- . Ka(C6H5COOH)= 6.5 * 10-5; Ka(HF)= 7.1 * 10-4

Arrange the acids H2Se, H2Te, and H2S in order of increasing acid strength.

If the pH of stomach acid is 1.0, what is the hydroxide ion concentration in this solution?

For H3PO4, Ka1 = 7.3 * 10-3, Ka2 = 6.2 * 10-6, and Ka3 = 4.8 * 10-13. An aqueous solution of Na3PO4 therefore would be

Suppose that ammonia, applied to a field as a fertilizer, is washed into a farm pond containing 3.0 * 106 L of water. If the pH of this pond is found to be 9.81, what volume of liquid ammonia found its way into the pond? [Given: Kb(NH3)= 1.8 * 10-5; the density of liquid ammonia is 0.771 g/cm3]

The pH of a certain solution is 2.0. How many H+(aq)ions are there in 1.0 L of the solution?

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

Calculate the pH of a 0.14 M HNO₂ solution that is 5.7% ionized.

What is the pH of an aqueous solution that contains 5.3 * 10¹⁷ OH^- ions per liter of solution?

Consider the weak bases below and their K_b values: C₆H₇O K_b = 1.3 * 10^-10 C₂H₅NH₂ K_b = 5.6 * 10^-4 C₅H₅N K_b = 1.7 * 10^-9 Arrange the conjugate acids of these weak bases in order of increasing acid strength.

The oxides SO₂ and N₂O₅ will form the following acids in water, respectively.

Predict the direction in which the equilibrium will lie for the reaction H₃PO₄(aq)+ HSO₄^-(aq) $\rarr$ H₂PO₄^-(aq)+ H₂SO₄(aq). K_a1(H₃PO₄)= 7.5 * 10^-3; K_a(H₂SO₄)= very large

A solution containing NH₃(aq)and NH₄Cl(aq)has a pH of 9.5. What is the [NH₃]/[NH₄⁺] ratio in this solution? (For ammonia, K_b = 1.8 * 10^-5.)

Arrange the acids HOCl, HClO₃, and HClO₂ in order of increasing acid strength.

Hydrosulfuric acid is a diprotic acid, for which K_a1 = 5.7 * 10^-8 andK_a2 = 1 *10^-19. Determine the concentration of sulfide ion in a 0.10 M hydrosulfuric solution.

Predict the direction in which the equilibrium will lie for the reaction C₆H₅COO^- + HF $\rarr$ C₆H₅COOH + F^-. K_a(C₆H₅COOH)= 6.5 * 10^-5; K_a(HF)= 7.1 * 10^-4

Arrange the acids H₂Se, H₂Te, and H₂S in order of increasing acid strength.

For H₃PO₄, K_a1 = 7.3 * 10^-3, K_a2 = 6.2 * 10^-6, and K_a3 = 4.8 * 10^-13. An aqueous solution of Na₃PO₄ therefore would be

The pH of a certain solution is 2.0. How many H⁺(aq)ions are there in 1.0 L of the solution?