Question 1

Identify the weak diprotic acid.

Accepted Answer

A)  CH3COOH 
B)  HCOOH 
C)  H3PO4 
D)  H2SO4 
E)  H2CO3 
A)  CH3COOH 
B)  HCOOH 
C)  H3PO4 
D)  H2SO4 
E)  H2CO3

Question 2

Which one of the following will form an acidic solution in water?

Accepted Answer

A)  NH4Cl 
B)  KF 
C)  KI 
D)  KNO3 
E)  None of the above solutions will be acidic. 
A)  NH4Cl 
B)  KF 
C)  KI 
D)  KNO3 
E)  None of the above solutions will be acidic.

Question 3

Which of the following statements is TRUE?

Accepted Answer

A)  A strong acid is composed of a proton and an anion that have a very strong attraction for one another. 
B)  A weak base is composed of a cation and an anion with a very weak attraction between them. 
C)  A strong acid has a strong conjugate base. 
D)  The conjugate base of a very weak acid is stronger than the conjugate base of a strong acid. 
E)  None of the above statements are true. 
A)  A strong acid is composed of a proton and an anion that have a very strong attraction for one another. 
B)  A weak base is composed of a cation and an anion with a very weak attraction between them. 
C)  A strong acid has a strong conjugate base. 
D)  The conjugate base of a very weak acid is stronger than the conjugate base of a strong acid. 
E)  None of the above statements are true.

Question 4

Identify the base that is in baking soda.

Accepted Answer

A)  RbOH 
B)  NaOH 
C)  NaHCO3 
D)  K2CO3 
E)  NH3 
A)  RbOH 
B)  NaOH 
C)  NaHCO3 
D)  K2CO3 
E)  NH3

Question 5

Find the percent ionization of a 0.337 M HF solution.The Ka for HF is 3.5 × 10-4.

Accepted Answer

A)  1.1 % 
B)  1.2 × 10-2 % 
C)  3.2 % 
D)  3.5 × 10-2 % 
E)  4.7 % 
A)  1.1 % 
B)  1.2 × 10-2 % 
C)  3.2 % 
D)  3.5 × 10-2 % 
E)  4.7 %

Question 6

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

Accepted Answer

A)  1.34 × 10-13 M 
B)  1.34 × 10-14 M 
C)  0.741 M 
D)  7.41 M 
E)  none of the above 
A)  1.34 × 10-13 M 
B)  1.34 × 10-14 M 
C)  0.741 M 
D)  7.41 M 
E)  none of the above

Question 7

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 4.33 at 25°C.

Accepted Answer

A)  2.1 × 10-10 M 
B)  9.7 × 10-10 M 
C)  4.7 × 10-5 M 
D)  3.8 × 10-5 M 
E)  6.3 × 10-6 M 
A)  2.1 × 10-10 M 
B)  9.7 × 10-10 M 
C)  4.7 × 10-5 M 
D)  3.8 × 10-5 M 
E)  6.3 × 10-6 M

Question 8

Describe the relationship between molecular structure and acid strength.

Accepted Answer

1)The stronger the bond between a hydrog

Question 9

An aqueous solution of ammonia is found to be basic.This observation can be explained by the net ionic equation

Accepted Answer

A)  NO3-(aq) + H2O(l) → HNO3(aq) + OH-(aq). 
B)  NH3(aq) + H2O(l) → NH4+(aq) + OH-(aq). 
C)  HNO3(aq) + H2O(l) → NO3-(aq) + H3O+(aq). 
D)  NH4+(aq) + H2O(l) → NH3(aq) + H3O+(aq). 
A)  NO3-(aq) + H2O(l) → HNO3(aq) + OH-(aq). 
B)  NH3(aq) + H2O(l) → NH4+(aq) + OH-(aq). 
C)  HNO3(aq) + H2O(l) → NO3-(aq) + H3O+(aq). 
D)  NH4+(aq) + H2O(l) → NH3(aq) + H3O+(aq).

Question 10

What is the hydronium ion concentration of an acid rain sample that has a pH of 3.25?

Accepted Answer

A)  1.78 × 10-11 M 
B)  5.62 × 10-4 M 
C)  3.25 M 
D)  10.75 M 
A)  1.78 × 10-11 M 
B)  5.62 × 10-4 M 
C)  3.25 M 
D)  10.75 M

Question 11

What is the hydronium ion concentration of a 0.400 M acetic acid solution with Ka = 1.8 × 10-5? The equation for the dissociation of acetic acid is:

Accepted Answer

A)  2.7 × 10-2 M 
B)  4.2 × 10-2 M 
C)  2.7 × 10-3 M 
D)  4.2 × 10-3 M 
A)  2.7 × 10-2 M 
B)  4.2 × 10-2 M 
C)  2.7 × 10-3 M 
D)  4.2 × 10-3 M

Question 12

What is the Kw of pure water at 50.0°C,if the pH is 6.630?

Accepted Answer

A)  2.34 × 10-7 
B)  5.50 × 10-14 
C)  2.13 × 10-14 
D)  1.00 × 10-14 
E)  There is not enough information to calculate the Kw. 
A)  2.34 × 10-7 
B)  5.50 × 10-14 
C)  2.13 × 10-14 
D)  1.00 × 10-14 
E)  There is not enough information to calculate the Kw.

Question 13

Which of the following is a strong base?

Accepted Answer

A)  I- 
B)  NH3 
C)  CH3OH 
D)  NO3⁻ 
E)  KOH 
A)  I- 
B)  NH3 
C)  CH3OH 
D)  NO3⁻ 
E)  KOH

Question 14

Which of the following is a Brønsted-Lowry acid?

Accepted Answer

A)  NH4+ 
B)  CI4 
C)  NH2- 
D)  BF3 
E)  I2 
A)  NH4+ 
B)  CI4 
C)  NH2- 
D)  BF3 
E)  I2

Question 15

Calculate the pH for an aqueous solution of acetic acid that contains   hydronium ion.

Accepted Answer

A)  4.65 × 10-12 M 
B)  2.15 × 10-3 M 
C)  2.67 
D)  11.33 
A)  4.65 × 10-12 M 
B)  2.15 × 10-3 M 
C)  2.67 
D)  11.33

Question 16

What is the pH of a 0.100 M NH3 solution that has Kb = 1.8 × 10-5? The equation for the dissociation of NH3 is
NH3(aq)+ H2O(l)⇌ NH4+(aq)+ OH-(aq).

Accepted Answer

A)  1.87 
B)  2.87 
C)  11.13 
D)  10.13 
A)  1.87 
B)  2.87 
C)  11.13 
D)  10.13

Question 17

Calculate the pH of a 0.800 M CH3NH3Cl solution.Kb for methylamine,CH3NH2,is 3.7 × 10-4.

Accepted Answer

A)  1.76 
B)  5.33 
C)  8.67 
D)  12.23 
A)  1.76 
B)  5.33 
C)  8.67 
D)  12.23

Question 18

Which Brønsted-Lowry acid is not considered to be a strong acid in water?

Accepted Answer

A)  HI 
B)  HBr  
C)  H2S O3 
D)  H NO3 
A)  HI 
B)  HBr  
C)  H2S O3 
D)  H NO3

Question 19

Calculate the pH of a solution that contains 3.9 × 10-5 M H3O⁺ at 25°C.

Accepted Answer

A)  5.41 
B)  4.41 
C)  9.59 
D)  8.59 
E)  0.59 
A)  5.41 
B)  4.41 
C)  9.59 
D)  8.59 
E)  0.59

Question 20

Which of the following is a polyprotic acid?

Accepted Answer

A)  HBr 
B)  H2SO4 
C)  HCN 
D)  CH4 
E)  HC2H3O2 
A)  HBr 
B)  H2SO4 
C)  HCN 
D)  CH4 
E)  HC2H3O2

Exam 17: Acids and Bases

Identify the weak diprotic acid.

Which one of the following will form an acidic solution in water?

Which of the following statements is TRUE?

Identify the base that is in baking soda.

Find the percent ionization of a 0.337 M HF solution.The Ka for HF is 3.5 × 10-4.

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

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 4.33 at 25°C.

Describe the relationship between molecular structure and acid strength.

An aqueous solution of ammonia is found to be basic.This observation can be explained by the net ionic equation

What is the hydronium ion concentration of an acid rain sample that has a pH of 3.25?

What is the hydronium ion concentration of a 0.400 M acetic acid solution with Ka = 1.8 × 10-5? The equation for the dissociation of acetic acid is:

What is the Kw of pure water at 50.0°C,if the pH is 6.630?

Which of the following is a strong base?

Which of the following is a Brønsted-Lowry acid?

Calculate the pH for an aqueous solution of acetic acid that contains hydronium ion.

What is the pH of a 0.100 M NH3 solution that has Kb = 1.8 × 10-5? The equation for the dissociation of NH3 is NH3(aq)+ H2O(l)⇌ NH4+(aq)+ OH-(aq).

Calculate the pH of a 0.800 M CH3NH3Cl solution.Kb for methylamine,CH3NH2,is 3.7 × 10-4.

Which Brønsted-Lowry acid is not considered to be a strong acid in water?

Calculate the pH of a solution that contains 3.9 × 10-5 M H3O⁺ at 25°C.

Which of the following is a polyprotic acid?

Essentials: Units, Measurements, and Problem Solving

Atoms

The Quantum Mechanical Model of the Atom

Periodic Properties of the Elements

Molecules and Compounds

Chemical Bonding I

Chemical Bonding Ii

Chemical Reactions and Chemical Quantities

Introduction to Solutions and Aqueous Reactions

Thermochemistry

Gases

Liquids, Solids, and Intermolecular Forces

Crystalline Solids and Modern Materials

Solutions

Chemical Kinetics

Chemical Equilibrium

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry

Transition Metals and Coordination Compounds

Filters

Find the percent ionization of a 0.337 M HF solution.The K_a for HF is 3.5 × 10^-4.

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

What is the hydronium ion concentration of a 0.400 M acetic acid solution with K_a = 1.8 × 10^-5? The equation for the dissociation of acetic acid is:

What is the K_w of pure water at 50.0°C,if the pH is 6.630?

What is the pH of a 0.100 M NH₃ solution that has K_b = 1.8 × 10^-5? The equation for the dissociation of NH₃ is NH₃(aq)+ H₂O(l)⇌ NH₄⁺(aq)+ OH^-(aq).

Calculate the pH of a 0.800 M CH₃NH₃Cl solution.K_b for methylamine,CH₃NH₂,is 3.7 × 10^-4.

Calculate the pH of a solution that contains 3.9 × 10^-⁵ M H₃O⁺ at 25°C.