Question 1

Which compound is manufactured in larger quantities in the U.S.than any other industrial chemical?

Accepted Answer

A) HCl 
B) HNO3 
C) H3PO4 
D) H2SO4 
E) NaOH 
A) HCl 
B) HNO3 
C) H3PO4 
D) H2SO4 
E) NaOH

Question 2

Which statement is correct for pure water?

Accepted Answer

A) Pure water contains equal amounts of hydroxide,[OH-],and hydronium,[H3O+],ions. 
B) Pure water contains larger amounts of hydroxide,[OH-],ions than hydronium,[H3O+],ions. 
C) Pure water contains larger amounts of hydronium,[H3O+],ions than hydroxide,
[OH-],ions. 
D) Pure water is an electrolyte. 
E) Pure water contains no ions. 
A) Pure water contains equal amounts of hydroxide,[OH-],and hydronium,[H3O+],ions. 
B) Pure water contains larger amounts of hydroxide,[OH-],ions than hydronium,[H3O+],ions. 
C) Pure water contains larger amounts of hydronium,[H3O+],ions than hydroxide,
[OH-],ions. 
D) Pure water is an electrolyte. 
E) Pure water contains no ions.

Question 3

The normality of a solution prepared by dissolving 50.0 g of Ca(OH)2 in water to make 250.mL solution is ________ N.

Accepted Answer

A) 1.35 
B) 2.70 
C) 3.51 
D) 5.40 
E) 7.02 
A) 1.35 
B) 2.70 
C) 3.51 
D) 5.40 
E) 7.02

Question 4

A Brønsted-Lowry acid is a substance which

Accepted Answer

A) produces hydrogen ions in aqueous solution. 
B) produces hydroxide ions in aqueous solution. 
C) donates protons to other substances. 
D) accepts protons from other substances. 
E) accepts hydronium ions from other substances. 
A) produces hydrogen ions in aqueous solution. 
B) produces hydroxide ions in aqueous solution. 
C) donates protons to other substances. 
D) accepts protons from other substances. 
E) accepts hydronium ions from other substances.

Question 5

Consider the following reaction: NO2- + HCO3-   
CO3-2  + HNO2
Identify the acid,base,conjugate acid and conjugate base.

Accepted Answer

Acid: HCO₃^- ; Conjugat

Question 6

All of the following species are involved in the blood buffer system except ________.

Accepted Answer

A) CO2 
B) H2CO3 
C) HCO3- 
D) CO32- 
E) none of the above 
A) CO2 
B) H2CO3 
C) HCO3- 
D) CO32- 
E) none of the above

Question 7

Which of the following pH's corresponds to a weakly acidic solution?

Accepted Answer

A) 5.3 
B) 1.4 
C) 7.8 
D) 9.2 
E) 11.5 
A) 5.3 
B) 1.4 
C) 7.8 
D) 9.2 
E) 11.5

Question 8

What is the value of [H3O+] in a solution with pH = 10.82?

Accepted Answer

A) 6.6 × 10-4 M 
B) 1.5 × 10-11 M 
C) 1.03 M 
D) 10.82 M 
E) 3.18 M 
A) 6.6 × 10-4 M 
B) 1.5 × 10-11 M 
C) 1.03 M 
D) 10.82 M 
E) 3.18 M

Question 9

Which of the following is a strong acid?

Accepted Answer

A) HNO3 
B) H3PO4 
C) NH4+ 
D) HCO3- 
E) H2O 
A) HNO3 
B) H3PO4 
C) NH4+ 
D) HCO3- 
E) H2O

Question 10

What is the normality of a solution containing 49 g of H2SO4 in enough water to make 400 mL of solution?

Accepted Answer

A) 2.5 N 
B) 5.0 N 
C) 1.0 N 
D) 10 N 
E) 0.20 N 
A) 2.5 N 
B) 5.0 N 
C) 1.0 N 
D) 10 N 
E) 0.20 N

Question 11

Which compound has a very large value of Ka in aqueous solution?

Accepted Answer

A) NaCl 
B) HNO3 
C) H3PO4 
D) KOH 
E) NH3 
A) NaCl 
B) HNO3 
C) H3PO4 
D) KOH 
E) NH3

Question 12

Which compound produces an acidic solution when dissolved in water?

Accepted Answer

A) NH4Cl 
B) NaF 
C) K2SO4 
D) KCl 
E) Ca(NO3)2 
A) NH4Cl 
B) NaF 
C) K2SO4 
D) KCl 
E) Ca(NO3)2

Question 13

Which net ionic equation correctly represents the neutralization of a solution of barium hydroxide by a solution of nitric acid?

Accepted Answer

A) Ba2+ + 2 NO3- → Ba(NO3)2 
B) H+ + NO3- → HNO3 
C) Ba2+ + 2 OH- → Ba(OH)2 
D) H+ + OH- → H2O 
E) Ba(NO3)2 + H2O → Ba2+ + 2 NO3- 
A) Ba2+ + 2 NO3- → Ba(NO3)2 
B) H+ + NO3- → HNO3 
C) Ba2+ + 2 OH- → Ba(OH)2 
D) H+ + OH- → H2O 
E) Ba(NO3)2 + H2O → Ba2+ + 2 NO3-

Question 14

Which compound has a value of Ka that is close to 10-5?

Accepted Answer

A) NaCl 
B) HNO3 
C) CH3CH2CO2H 
D) KOH 
E) NH3 
A) NaCl 
B) HNO3 
C) CH3CH2CO2H 
D) KOH 
E) NH3

Question 15

Which of the following cannot act as a Brønsted base?

Accepted Answer

A) HCO3- 
B) CO32- 
C) NH3 
D) NH2- 
E) NH4+ 
A) HCO3- 
B) CO32- 
C) NH3 
D) NH2- 
E) NH4+

Question 16

How many mL of 0.150 M NaOH are needed to neutralize 50.00 mL of a 0.120 M solution of H2SO4?

Accepted Answer

A) 40.0 mL 
B) 50.0 mL 
C) 80.0 mL 
D) 120.0 mL 
E) 160.0 mL 
A) 40.0 mL 
B) 50.0 mL 
C) 80.0 mL 
D) 120.0 mL 
E) 160.0 mL

Question 17

To prepare a buffer using sodium phosphate,which of the following would also be needed?

Accepted Answer

A) hydrochloric acid 
B) ammonium hydroxide 
C) ammonium phosphate 
D) phosphoric acid 
E) sodium hydroxide 
A) hydrochloric acid 
B) ammonium hydroxide 
C) ammonium phosphate 
D) phosphoric acid 
E) sodium hydroxide

Question 18

What is the pH of a solution in which the hydrogen ion concentration is 5.1 × 10-8 M?

Accepted Answer

A) 6.71 
B) 1.96 × 10-7 
C) 8.90 
D) 5.10 
E) 7.29 
A) 6.71 
B) 1.96 × 10-7 
C) 8.90 
D) 5.10 
E) 7.29

Question 19

What is the concentration of a nitric acid solution if a 10.00 mL sample of the acid requires 31.25 mL of 0.135 M KOH for neutralization?

Accepted Answer

A) 0.422 M 
B) 0.0432 M 
C) 0.844 M 
D) 0.135 M 
E) 0.211 M 
A) 0.422 M 
B) 0.0432 M 
C) 0.844 M 
D) 0.135 M 
E) 0.211 M

Question 20

Which of the following pH's corresponds to a neutral solution?

Accepted Answer

A) 7.0 
B) 1.8 
C) 6.2 
D) 8.5 
E) 14.0 
A) 7.0 
B) 1.8 
C) 6.2 
D) 8.5 
E) 14.0

Exam 10: Acids and Bases

Which compound is manufactured in larger quantities in the U.S.than any other industrial chemical?

Which statement is correct for pure water?

The normality of a solution prepared by dissolving 50.0 g of Ca(OH)2 in water to make 250.mL solution is ________ N.

A Brønsted-Lowry acid is a substance which

Consider the following reaction: NO2- + HCO3- CO3-2 + HNO2 Identify the acid,base,conjugate acid and conjugate base.

All of the following species are involved in the blood buffer system except ________.

Which of the following pH's corresponds to a weakly acidic solution?

What is the value of [H3O+] in a solution with pH = 10.82?

Which of the following is a strong acid?

What is the normality of a solution containing 49 g of H2SO4 in enough water to make 400 mL of solution?

Which compound has a very large value of Ka in aqueous solution?

Which compound produces an acidic solution when dissolved in water?

Which net ionic equation correctly represents the neutralization of a solution of barium hydroxide by a solution of nitric acid?

Which compound has a value of Ka that is close to 10-5?

Which of the following cannot act as a Brønsted base?

How many mL of 0.150 M NaOH are needed to neutralize 50.00 mL of a 0.120 M solution of H2SO4?

To prepare a buffer using sodium phosphate,which of the following would also be needed?

What is the pH of a solution in which the hydrogen ion concentration is 5.1 × 10-8 M?

What is the concentration of a nitric acid solution if a 10.00 mL sample of the acid requires 31.25 mL of 0.135 M KOH for neutralization?

Which of the following pH's corresponds to a neutral solution?

Matter and Measurements

Atoms and the Periodic Table

Ionic Compounds

Molecular Compounds

Classification and Balancing of Chemical Reactions

Chemical Reactions: Mole and Mass Relationships

Chemical Reactions: Energy, rates, and Equilibrium

Gases, liquids, and Solids

Solutions

Nuclear Chemistry

Introduction to Organic Chemistry: Alkanes

Alkenes, alkynes, and Aromatic Compounds

Some Compounds With Oxygen, sulfur, or a Halogen

Amines

Aldehydes and Ketones

Carboxylic Acids and Their Derivatives

Amino Acids and Proteins

Enzymes and Vitamins

The Generation of Biochemical Energy

Carbohydrates

Carbohydrate Metabolism

Lipids

Lipid Metabolism

Nucleic Acids and Protein Synthesis

Genomics

Protein and Amino Acid Metabolism

Chemical Messengers: Hormones, neurotransmitters, and Drugs

Body Fluids

Filters

The normality of a solution prepared by dissolving 50.0 g of Ca(OH)₂ in water to make 250.mL solution is ________ N.

Consider the following reaction: NO₂^-+ HCO₃^- CO₃^-2 + HNO₂ Identify the acid,base,conjugate acid and conjugate base.

What is the value of [H₃O⁺] in a solution with pH = 10.82?

What is the normality of a solution containing 49 g of H₂SO₄ in enough water to make 400 mL of solution?

Which compound has a very large value of K_a in aqueous solution?

Which compound has a value of K_a that is close to 10^-5?

How many mL of 0.150 M NaOH are needed to neutralize 50.00 mL of a 0.120 M solution of H₂SO₄?

What is the pH of a solution in which the hydrogen ion concentration is 5.1 × 10^-8 M?