Question 1

A 0.0925 g sample of a monoprotic base (mm = 17.03 g/mol)was dissolved in water to produce 100 mL of solution with a pH = 11.00.What is the ionization constant of this base?

Accepted Answer

A) 1.8 × 10-6 
B) 1.8 × 10-11 
C) 1.8 × 10-21 
D) 1.8 × 10-5 
E) 1.1 × 10-6 
A) 1.8 × 10-6 
B) 1.8 × 10-11 
C) 1.8 × 10-21 
D) 1.8 × 10-5 
E) 1.1 × 10-6

Question 2

If one mole of Ba(OH)2 is added to enough water to make 10 liters of solution,the pH of the resulting solution is ________.

Accepted Answer

A) 13.3 
B) 1.0 
C) 0.7 
D) 13.0 
E) 12.5 
A) 13.3 
B) 1.0 
C) 0.7 
D) 13.0 
E) 12.5

Question 3

Amine bases are known as strong bases.

Accepted Answer

A) True 
 B)False

Question 4

Calculate the pH for an aqueous solution of pyridine that contains 4.15 × 10-4 mol L-1 hydroxide ion.

Accepted Answer

A) 2.41 × 10-11 
B) 4.15 × 10-4  
C) 3.382 
D) 10.618 
A) 2.41 × 10-11 
B) 4.15 × 10-4  
C) 3.382 
D) 10.618

Question 5

Choose the Br∅nsted-Lowry acids and bases in the following equation:
NH4+ + OH- ⇌ H2O + NH3

Accepted Answer

A) acids NH4+,OH- bases H2O,NH3  
B) acids OH-,H2O bases NH3,NH4+  
C) acids NH4+,OH- bases NH4+,H2O 
D) acids NH4+,H2O bases OH-,NH3  
E) acids NH4+,NH3 bases OH-,H2O 
A) acids NH4+,OH- bases H2O,NH3  
B) acids OH-,H2O bases NH3,NH4+  
C) acids NH4+,OH- bases NH4+,H2O 
D) acids NH4+,H2O bases OH-,NH3  
E) acids NH4+,NH3 bases OH-,H2O

Question 6

The acid-dissociation constant at 25.0 °C for hypochlorous acid (HClO)is 3.0 ×   .At equilibrium,the molarity of   In a 0.010 mol L-1 aqueous solution of HClO is:

Accepted Answer

A) 1.7 ×   
B) 0.010 
C) 5.8 ×   
D) 4.76 
E) 2.00 
A) 1.7 ×   
B) 0.010 
C) 5.8 ×   
D) 4.76 
E) 2.00

Question 7

What is the indication of the relative acid strengths of the following acids?
CH3CH2CHClCOOH CH3CHClCH2COOH CH2ClCH2CH2COOH

Accepted Answer

A) CH3CHClCH2COOH > CH2ClCH2CH2COOH > CH3CH2CHClCOOH 
B) CH2ClCH2CH2COOH > CH3CH2CHClCOOH > CH3CHClCH2COOH 
C) CH2ClCH2CH2COOH > CH3CHClCH2COOH > CH3CH2CHClCOOH 
D) CH3CH2CHClCOOH > CH3CHClCH2COOH > CH2ClCH2CH2COOH 
E) CH3CH2CHClCOOH > CH2ClCH2CH2COOH > CH3CHClCH2COOH 
A) CH3CHClCH2COOH > CH2ClCH2CH2COOH > CH3CH2CHClCOOH 
B) CH2ClCH2CH2COOH > CH3CH2CHClCOOH > CH3CHClCH2COOH 
C) CH2ClCH2CH2COOH > CH3CHClCH2COOH > CH3CH2CHClCOOH 
D) CH3CH2CHClCOOH > CH3CHClCH2COOH > CH2ClCH2CH2COOH 
E) CH3CH2CHClCOOH > CH2ClCH2CH2COOH > CH3CHClCH2COOH

Question 8

What is the pH of a 0.30 mol L-1 pyridine solution that has Kb = 1.9 × 10-9? The equation for the dissociation of pyridine is below:

Accepted Answer

A) 4.62 
B) 8.72 
C) 9.38 
D) 10.38 
A) 4.62 
B) 8.72 
C) 9.38 
D) 10.38

Question 9

Which of the following statements concerning aqueous solutions of salts is FALSE?

Accepted Answer

A) For any salt of a strong acid and a strong base,the pH will be about 7. 
B) For any salt of a strong acid and a weak base,the pH will be 7. 
D) For any salt of a weak acid and a weak base,the pH will be about 7. 
E) Salt solutions can have a pH of 7. 
A) For any salt of a strong acid and a strong base,the pH will be about 7. 
B) For any salt of a strong acid and a weak base,the pH will be 7. 
D) For any salt of a weak acid and a weak base,the pH will be about 7. 
E) Salt solutions can have a pH of 7.

Question 10

List the following acids in order of increasing strength:
HBrO HIO HClO

Accepted Answer

A) HIO < HClO < HBrO 
B) HClO < HIO < HBrO 
C) HBrO < HIO < HClO 
D) HIO < HBrO < HClO 
E) HClO< HBrO < HIO 
A) HIO < HClO < HBrO 
B) HClO < HIO < HBrO 
C) HBrO < HIO < HClO 
D) HIO < HBrO < HClO 
E) HClO< HBrO < HIO

Question 11

What would be the pH of a solution prepared by dissolving 14.4 g NaOH (MW = 40.0 g/mol)in enough water to make 1.05 L of solution?

Accepted Answer

A) 13.54 
B) 0.46 
C) 13.58 
D) 13.66 
E) 7.00 
A) 13.54 
B) 0.46 
C) 13.58 
D) 13.66 
E) 7.00

Question 12

What is the pH of a 0.240 M aqueous solution of potassium cyanide? 
Ka (HCN)= 6.2 × 10-10

Accepted Answer

A) 11.3 
B) 2.7 
C) 4.9 
D) 9.1 
E) 9.4 
A) 11.3 
B) 2.7 
C) 4.9 
D) 9.1 
E) 9.4

Question 13

The first ionization step is approximately 100% for H2SO3.

Accepted Answer

A) True 
 B)False

Question 14

What is the [HPO4-2] of a solution labeled "0.10 M phosphoric acid"?
[Ka1 = 7.1 × 10-3;Ka2 = 6.3 × 10-8;Ka3 = 4.2 × 10-13]

Accepted Answer

A) 4.2 × 10-13 M 
B) 6.3 × 10-8 M 
C) 7.1 × 10-3 M 
D) 1.6 × 10-9 M 
E) 1.6 × 10-16 M 
A) 4.2 × 10-13 M 
B) 6.3 × 10-8 M 
C) 7.1 × 10-3 M 
D) 1.6 × 10-9 M 
E) 1.6 × 10-16 M

Question 15

Calculate the pH of a 0.60 mol L-1 aqueous H2SO3 solution that has the stepwise dissociation constants Ka1 = 1.5 × 10-2 and

Accepted Answer

A) 1.02 
B) 1.06 
C) 1.82 
D) 2.04 
A) 1.02 
B) 1.06 
C) 1.82 
D) 2.04

Question 16

0.653 g of a monoprotic acid (MW= 157 g/mol)is dissolved in water to produce 50.0 mL of a solution with pH = 2.13.Determine the ionization constant of the acid.

Accepted Answer

A) 7.9 × 10-3  
B) 8.9 × 10-2  
C) 6.6 × 10-4  
D) 3.9 × 10-2  
E) 3.6 × 10-6  
A) 7.9 × 10-3  
B) 8.9 × 10-2  
C) 6.6 × 10-4  
D) 3.9 × 10-2  
E) 3.6 × 10-6

Question 17

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

Accepted Answer

A) HBr 
B) HI  
C) HIO4 
D) HNO3 
A) HBr 
B) HI  
C) HIO4 
D) HNO3

Question 18

The base-dissociation constant of ethylamine (       )is 6.4 ×  
At 25.0 °C.The [   ] in a  
Aqueous solution of ethylamine is ________ mol L-1.

Accepted Answer

A) 3.5 ×   
B) 2.9 ×   
C) 3.1 ×   
D) 3.2 ×   
E) 11.46 
A) 3.5 ×   
B) 2.9 ×   
C) 3.1 ×   
D) 3.2 ×   
E) 11.46

Question 19

What is the pH of an aqueous solution labeled "0.10 M phosphoric acid"?
[Ka1 = 7.1 × 10-3;Ka2 = 6.3 × 10-8;Ka3 = 4.2 × 10-13]

Accepted Answer

A) 5.7 
B) 4.3 
C) 3.1 
D) 2.3 
E) 1.6 
A) 5.7 
B) 4.3 
C) 3.1 
D) 2.3 
E) 1.6

Question 20

Choose the Br∅nsted-Lowry acids and bases in the following equation:
HCN + OH- ⇌ H2O + CN-

Accepted Answer

A) acids HCN,CN- bases OH-,H2O 
B) acids CN-,OH- bases HCN,H2O 
C) acids HCN,H2O bases OH-,CN-  
D) acids OH-,H2O bases CN-,HCN 
E) acids HCN,OH- bases H2O,CN-  
A) acids HCN,CN- bases OH-,H2O 
B) acids CN-,OH- bases HCN,H2O 
C) acids HCN,H2O bases OH-,CN-  
D) acids OH-,H2O bases CN-,HCN 
E) acids HCN,OH- bases H2O,CN-

Exam 16: Acids and Bases

A 0.0925 g sample of a monoprotic base (mm = 17.03 g/mol)was dissolved in water to produce 100 mL of solution with a pH = 11.00.What is the ionization constant of this base?

If one mole of Ba(OH)2 is added to enough water to make 10 liters of solution,the pH of the resulting solution is ________.

Amine bases are known as strong bases.

Calculate the pH for an aqueous solution of pyridine that contains 4.15 × 10-4 mol L-1 hydroxide ion.

Choose the Br∅nsted-Lowry acids and bases in the following equation: NH4+ + OH- ⇌ H2O + NH3

The acid-dissociation constant at 25.0 °C for hypochlorous acid (HClO)is 3.0 × .At equilibrium,the molarity of In a 0.010 mol L-1 aqueous solution of HClO is:

What is the indication of the relative acid strengths of the following acids? CH3CH2CHClCOOH CH3CHClCH2COOH CH2ClCH2CH2COOH

What is the pH of a 0.30 mol L-1 pyridine solution that has Kb = 1.9 × 10-9? The equation for the dissociation of pyridine is below:

Which of the following statements concerning aqueous solutions of salts is FALSE?

List the following acids in order of increasing strength: HBrO HIO HClO

What would be the pH of a solution prepared by dissolving 14.4 g NaOH (MW = 40.0 g/mol)in enough water to make 1.05 L of solution?

What is the pH of a 0.240 M aqueous solution of potassium cyanide? Ka (HCN)= 6.2 × 10-10

The first ionization step is approximately 100% for H2SO3.

What is the [HPO4-2] of a solution labeled "0.10 M phosphoric acid"? [Ka1 = 7.1 × 10-3;Ka2 = 6.3 × 10-8;Ka3 = 4.2 × 10-13]

Calculate the pH of a 0.60 mol L-1 aqueous H2SO3 solution that has the stepwise dissociation constants Ka1 = 1.5 × 10-2 and

0.653 g of a monoprotic acid (MW= 157 g/mol)is dissolved in water to produce 50.0 mL of a solution with pH = 2.13.Determine the ionization constant of the acid.

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

The base-dissociation constant of ethylamine ( )is 6.4 × At 25.0 °C.The [ ] in a Aqueous solution of ethylamine is ________ mol L-1.

What is the pH of an aqueous solution labeled "0.10 M phosphoric acid"? [Ka1 = 7.1 × 10-3;Ka2 = 6.3 × 10-8;Ka3 = 4.2 × 10-13]

Choose the Br∅nsted-Lowry acids and bases in the following equation: HCN + OH- ⇌ H2O + CN-

Matter: Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Valence Bond and Molecular Orbital Theories

Intermolecular Forces: Liquids and Solids

Spontaneous Change: Entropy and Gibbs Energy

Solutions and Their Physical Properties

Principles of Chemical Equilibrium

Additional Aspects of Acidbase Equilibria

Solubility and Complex-Ion Equilibria

Electrochemistry

Chemical Kinetics

Chemistry of the Main-Group Elements I: Groups 1,2,13,and 14

Chemistry of the Main-Group Elements Ii: Groups 18,17,16,15,and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

If one mole of Ba(OH)₂ is added to enough water to make 10 liters of solution,the pH of the resulting solution is ________.

Calculate the pH for an aqueous solution of pyridine that contains 4.15 × 10^-4 mol L^-1 hydroxide ion.

Choose the Br∅nsted-Lowry acids and bases in the following equation: NH₄⁺ + OH^- ⇌ H₂O + NH₃

The acid-dissociation constant at 25.0 °C for hypochlorous acid (HClO)is 3.0 × .At equilibrium,the molarity of In a 0.010 mol L^-1 aqueous solution of HClO is:

What is the indication of the relative acid strengths of the following acids? CH₃CH₂CHClCOOH CH₃CHClCH₂COOH CH₂ClCH₂CH₂COOH

What is the pH of a 0.30 mol L^-1 pyridine solution that has K_b = 1.9 × 10^-9? The equation for the dissociation of pyridine is below:

What is the pH of a 0.240 M aqueous solution of potassium cyanide? K_a (HCN)= 6.2 × 10^-10

The first ionization step is approximately 100% for H₂SO₃.

What is the [HPO₄^-2] of a solution labeled "0.10 M phosphoric acid"? [K_a1 = 7.1 × 10^-3;K_a2 = 6.3 × 10^-8;K_a3 = 4.2 × 10^-13]

Calculate the pH of a 0.60 mol L^-1 aqueous H₂SO₃ solution that has the stepwise dissociation constants K_a1 = 1.5 × 10^-2 and

The base-dissociation constant of ethylamine ( )is 6.4 × At 25.0 °C.The [ ] in a Aqueous solution of ethylamine is ________ mol L^-1.

What is the pH of an aqueous solution labeled "0.10 M phosphoric acid"? [K_a1 = 7.1 × 10^-3;K_a2 = 6.3 × 10^-8;K_a3 = 4.2 × 10^-13]

Choose the Br∅nsted-Lowry acids and bases in the following equation: HCN + OH^- ⇌ H₂O + CN^-