Question 1

What is the concentration of OH- ion in pure water?

Accepted Answer

A)  1 F1F1F1S1F1F1F10 10-14 M 
B)  2 F1F1F1S1F1F1F10 10-14 M 
C)  1 F1F1F1S1F1F1F10 107 M 
D)  1 F1F1F1S1F1F1F10 10-7 M 
A)  1 F1F1F1S1F1F1F10 10-14 M 
B)  2 F1F1F1S1F1F1F10 10-14 M 
C)  1 F1F1F1S1F1F1F10 107 M 
D)  1 F1F1F1S1F1F1F10 10-7 M

Question 2

Which of the following is a true statement about an aqueous solution of a base when describing it as strong?

Accepted Answer

A)  It is a good conductor of electricity. 
B)  Much of the unionized base exists in the solution. 
C)  It is a poor conductor of electricity. 
D)  none of the above 
A)  It is a good conductor of electricity. 
B)  Much of the unionized base exists in the solution. 
C)  It is a poor conductor of electricity. 
D)  none of the above

Question 3

A buffer could be prepared by mixing lactic acid with

Accepted Answer

A)  HCl. 
B)  sodium acetate. 
C)  sodium lactate. 
D)  ammonium chloride. 
A)  HCl. 
B)  sodium acetate. 
C)  sodium lactate. 
D)  ammonium chloride.

Question 4

Describe the purpose of buffers in the blood stream.

Accepted Answer

The pH of blood is about 7.4. If the pH

Question 5

Individuals who experience frequent acid reflux have a condition called ____________________.

Accepted Answer

GERD (gast

Question 6

How would you prepare a buffer?

Accepted Answer

Mix a weak acid with its conju

Question 7

When the relative amounts of reactant and product are in balance, the reaction has reached ____________________.

Accepted Answer

chemical e

Question 8

The mixture of a weak acid and its conjugate base produces

Accepted Answer

A)  a salt. 
B)  a strong acid and strong base. 
C)  water. 
D)  a buffer. 
A)  a salt. 
B)  a strong acid and strong base. 
C)  water. 
D)  a buffer.

Question 9

In a dilute solution of acid at 25°C, the concentration of H3O+ is 1 F1F1F1S1F1F1F10 10-3 M. What is the concentration of OH- ions?

Accepted Answer

A)  1 F1F1F1S1F1F1F10 1011 M 
B)  1 F1F1F1S1F1F1F10 10-4 M 
C)  1 F1F1F1S1F1F1F10 10-7 M 
D)  1 F1F1F1S1F1F1F10 10-11 M 
A)  1 F1F1F1S1F1F1F10 1011 M 
B)  1 F1F1F1S1F1F1F10 10-4 M 
C)  1 F1F1F1S1F1F1F10 10-7 M 
D)  1 F1F1F1S1F1F1F10 10-11 M

Question 10

A solution of an acid exhibits very good electrical conductivity. It is a

Accepted Answer

A)  weak acid. 
B)  strong acid. 
C)  covalent molecule. 
D)  all of the above 
A)  weak acid. 
B)  strong acid. 
C)  covalent molecule. 
D)  all of the above

Question 11

Which of the following solutions is acidic?

Accepted Answer

A)  [OH-] = 1 F1F1F1S1F1F1F10 10-8 M 
B)  [OH-] = 1 F1F1F1S1F1F1F10 10-7 M 
C)  [OH-] = 1 F1F1F1S1F1F1F10 10-5 M 
D)  [OH-] = 1 F1F1F1S1F1F1F10 10-2 M 
A)  [OH-] = 1 F1F1F1S1F1F1F10 10-8 M 
B)  [OH-] = 1 F1F1F1S1F1F1F10 10-7 M 
C)  [OH-] = 1 F1F1F1S1F1F1F10 10-5 M 
D)  [OH-] = 1 F1F1F1S1F1F1F10 10-2 M

Question 12

Show the reaction that demonstrates trimethylamine, (CH3)3NH2 as a Brønsted-Lowry base.

Accepted Answer

(CH₃)₃NH₂(aq) + H₂O(l) F

Question 13

Why is a weak acid, such as acetic acid, a weak conductor of electricity?

Accepted Answer

Acetic acid dissociates in water to form

Question 14

Balance the equation for the neutralization of calcium hydroxide, Ca(OH)2, and sulfuric acid, H2SO4.

Accepted Answer

A)  Ca(OH)2(aq) + H2SO4(aq) F1S1S1W1F1F1F10 2H2O(l) + CaSO4(s) 
B)  Ca(OH)2(aq) + 2H2SO4(aq) F1S1S1W1F1F1F10 2H2O(l) + CaSO4(s) 
C)  2Ca(OH)2(aq) + H2SO4(aq) F1S1S1W1F1F1F10 2H2O(l) + CaSO4(s) 
D)  3Ca(OH)2(aq) + 2H2SO4(aq) F1S1S1W1F1F1F10 H2O(l) + CaSO4(s) 
A)  Ca(OH)2(aq) + H2SO4(aq) F1S1S1W1F1F1F10 2H2O(l) + CaSO4(s) 
B)  Ca(OH)2(aq) + 2H2SO4(aq) F1S1S1W1F1F1F10 2H2O(l) + CaSO4(s) 
C)  2Ca(OH)2(aq) + H2SO4(aq) F1S1S1W1F1F1F10 2H2O(l) + CaSO4(s) 
D)  3Ca(OH)2(aq) + 2H2SO4(aq) F1S1S1W1F1F1F10 H2O(l) + CaSO4(s)

Question 15

Describe the action of a carbonic acid (H2CO3) and bicarbonate (HCO3-) buffer when a base is introduced.

Accepted Answer

The hydroxide generated with t

Question 16

At 25°C the concentration of OH- in a solution is 1 F1F1F1S1F1F1F10 10-8 M. What is the pH of the solution?

Accepted Answer

A)  8 
B)  6 
C)  -8 
D)  -6 
A)  8 
B)  6 
C)  -8 
D)  -6

Question 17

Nitric acid is a strong acid and dissociates in water. What species are present in the aqueous solution of 0.1 M HNO3?

Accepted Answer

A)  HNO3 only 
B)  primarily HNO3 but some H3O+ and NO3- 
C)  primarily H3O+ and NO3- but some HNO3 
D)  H3O+ and NO3- only 
A)  HNO3 only 
B)  primarily HNO3 but some H3O+ and NO3- 
C)  primarily H3O+ and NO3- but some HNO3 
D)  H3O+ and NO3- only

Question 18

Lactic acid, CH3CH(OH)CO2H, is a weak acid that dissociates in water according to the equation CH3CH(OH)CO2H(aq) + H2O(l) F1S1S1W1F1F1F10 CH3CH(OH)CO2-(aq) + H3O+(aq). What species are in the aqueous solution of 0.1 M lactic acid?

Accepted Answer

A)  CH3CH(OH)CO2H only 
B)  CH3CH(OH)CO2H primarily but some H3O+ and CH3CH(OH)CO2- 
C)  H3O+ and CH3CH(OH)CO2- only 
D)  H3O+ and CH3CH(OH)CO2- primarily but some CH3CH(OH)CO2H 
A)  CH3CH(OH)CO2H only 
B)  CH3CH(OH)CO2H primarily but some H3O+ and CH3CH(OH)CO2- 
C)  H3O+ and CH3CH(OH)CO2- only 
D)  H3O+ and CH3CH(OH)CO2- primarily but some CH3CH(OH)CO2H

Question 19

What is the conjugate acid of OH-? Describe and explain the relative strength of each.

Accepted Answer

The conjugate acid o

Question 20

What is the conjugate base of ammonium, NH4+?

Accepted Answer

A)  OH 
B)  H2O 
C)  NH3 
D)  NH52+ 
A)  OH 
B)  H2O 
C)  NH3 
D)  NH52+

What is the concentration of OH^- ion in pure water?

Which of the following is a true statement about an aqueous solution of a base when describing it as strong?

A buffer could be prepared by mixing lactic acid with

Describe the purpose of buffers in the blood stream.

Individuals who experience frequent acid reflux have a condition called ____________________.

How would you prepare a buffer?

When the relative amounts of reactant and product are in balance, the reaction has reached ____________________.

The mixture of a weak acid and its conjugate base produces

In a dilute solution of acid at 25°C, the concentration of H₃O⁺ is 1  10^-3 M. What is the concentration of OH^- ions?

A solution of an acid exhibits very good electrical conductivity. It is a

Which of the following solutions is acidic?

Show the reaction that demonstrates trimethylamine, (CH₃)₃NH₂ as a Brønsted-Lowry base.

Why is a weak acid, such as acetic acid, a weak conductor of electricity?

Balance the equation for the neutralization of calcium hydroxide, Ca(OH)₂, and sulfuric acid, H₂SO₄.

Describe the action of a carbonic acid (H₂CO₃) and bicarbonate (HCO₃^-) buffer when a base is introduced.

At 25°C the concentration of OH^- in a solution is 1  10^-8 M. What is the pH of the solution?

Nitric acid is a strong acid and dissociates in water. What species are present in the aqueous solution of 0.1 M HNO₃?

Lactic acid, CH₃CH(OH)CO₂H, is a weak acid that dissociates in water according to the equation CH₃CH(OH)CO₂H(aq) + H₂O(l)  CH₃CH(OH)CO₂^-(aq) + H₃O⁺(aq). What species are in the aqueous solution of 0.1 M lactic acid?

What is the conjugate acid of OH^-? Describe and explain the relative strength of each.

What is the conjugate base of ammonium, NH₄⁺?

Antibiotics and Resistance: an Introduction to the Molecules of Life

Elements of Life and Death: The Chemistry of Elements and Atoms

Chemical Bonding

Carbon: The Element of Life

Molecular Diversity

Chemical Reactions

Monomers and Polymers

The Unusual Nature of Water

Molecules and Ions in Solution

Measuring Concentration

DNA: The Molecule of Heredity

From DNA to Proteins

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Exam 11: Acids and Bases

What is the concentration of OH- ion in pure water?

Which of the following is a true statement about an aqueous solution of a base when describing it as strong?

A buffer could be prepared by mixing lactic acid with

Describe the purpose of buffers in the blood stream.

Individuals who experience frequent acid reflux have a condition called ____________________.

How would you prepare a buffer?

When the relative amounts of reactant and product are in balance, the reaction has reached ____________________.

The mixture of a weak acid and its conjugate base produces

In a dilute solution of acid at 25°C, the concentration of H3O+ is 1  10-3 M. What is the concentration of OH- ions?

A solution of an acid exhibits very good electrical conductivity. It is a

Which of the following solutions is acidic?

Show the reaction that demonstrates trimethylamine, (CH3)3NH2 as a Brønsted-Lowry base.

Why is a weak acid, such as acetic acid, a weak conductor of electricity?

Balance the equation for the neutralization of calcium hydroxide, Ca(OH)2, and sulfuric acid, H2SO4.

Describe the action of a carbonic acid (H2CO3) and bicarbonate (HCO3-) buffer when a base is introduced.

At 25°C the concentration of OH- in a solution is 1  10-8 M. What is the pH of the solution?

Nitric acid is a strong acid and dissociates in water. What species are present in the aqueous solution of 0.1 M HNO3?

Lactic acid, CH3CH(OH)CO2H, is a weak acid that dissociates in water according to the equation CH3CH(OH)CO2H(aq) + H2O(l)  CH3CH(OH)CO2-(aq) + H3O+(aq). What species are in the aqueous solution of 0.1 M lactic acid?

What is the conjugate acid of OH-? Describe and explain the relative strength of each.

What is the conjugate base of ammonium, NH4+?

Antibiotics and Resistance: an Introduction to the Molecules of Life

Elements of Life and Death: The Chemistry of Elements and Atoms

Chemical Bonding

Carbon: The Element of Life

Molecular Diversity

Chemical Reactions

Monomers and Polymers

The Unusual Nature of Water

Molecules and Ions in Solution

Measuring Concentration

DNA: The Molecule of Heredity

From DNA to Proteins

Enzymes As Biological Catalysts

Drug Development

Filters

What is the concentration of OH^- ion in pure water?

In a dilute solution of acid at 25°C, the concentration of H₃O⁺ is 1  10^-3 M. What is the concentration of OH^- ions?

Show the reaction that demonstrates trimethylamine, (CH₃)₃NH₂ as a Brønsted-Lowry base.

Balance the equation for the neutralization of calcium hydroxide, Ca(OH)₂, and sulfuric acid, H₂SO₄.

Describe the action of a carbonic acid (H₂CO₃) and bicarbonate (HCO₃^-) buffer when a base is introduced.

At 25°C the concentration of OH^- in a solution is 1  10^-8 M. What is the pH of the solution?

Nitric acid is a strong acid and dissociates in water. What species are present in the aqueous solution of 0.1 M HNO₃?

Lactic acid, CH₃CH(OH)CO₂H, is a weak acid that dissociates in water according to the equation CH₃CH(OH)CO₂H(aq) + H₂O(l)  CH₃CH(OH)CO₂^-(aq) + H₃O⁺(aq). What species are in the aqueous solution of 0.1 M lactic acid?

What is the conjugate acid of OH^-? Describe and explain the relative strength of each.

What is the conjugate base of ammonium, NH₄⁺?