Question 1

A necessary requirement for a Brønsted base is

Accepted Answer

A) the presence of water as a reaction medium. 
B) the presence of hydroxide in its formula. 
C) a lone pair of electrons in its Lewis dot structure. 
D) the production of hydronium ion upon reaction with water. 
E) the presence of a metal ion in its formula. 
A) the presence of water as a reaction medium. 
B) the presence of hydroxide in its formula. 
C) a lone pair of electrons in its Lewis dot structure. 
D) the production of hydronium ion upon reaction with water. 
E) the presence of a metal ion in its formula.

Question 2

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 3

Which of these,if dissolved in 1.0 L of pure water,would produce a buffer solution?

Accepted Answer

A) 0.1 mol NaCl + 0.1 mol KCl 
B) 0.1 mol H3O+ + 0.1 OH- 
C) 0.1 mol NaH2PO4 + 0.1 mol Na2HPO4 
D) 0.1 mol HCl + 0.1 mol NaOH 
E) 0.1 mol H3O+ + 0.1 mol Cl- 
A) 0.1 mol NaCl + 0.1 mol KCl 
B) 0.1 mol H3O+ + 0.1 OH- 
C) 0.1 mol NaH2PO4 + 0.1 mol Na2HPO4 
D) 0.1 mol HCl + 0.1 mol NaOH 
E) 0.1 mol H3O+ + 0.1 mol Cl-

Question 4

The net ionic equation for the reaction of formic acid,a weak acid,with potassium hydroxide,a strong base,is

Accepted Answer

A) HCO2H(aq)+ KOH(aq)→ KHCO2(aq)+ H2O(l). 
B) HCO2H(aq)+ K+(aq)+ OH-(aq)→ K+(aq)+ HCO2-(aq)+ H2O(l). 
C) HCO2H(aq)+ OH-(aq)→ HCO2-(aq)+ H2O(l). 
D) HCO2-(aq)+ KOH(aq)→ KHCO2(aq)+ OH-(aq). 
E) H+(aq)+ HCO2-(aq)+ K+(aq)+ OH-(aq)→ K+(aq)+ HCO2-(aq)+ H2O(l). 
A) HCO2H(aq)+ KOH(aq)→ KHCO2(aq)+ H2O(l). 
B) HCO2H(aq)+ K+(aq)+ OH-(aq)→ K+(aq)+ HCO2-(aq)+ H2O(l). 
C) HCO2H(aq)+ OH-(aq)→ HCO2-(aq)+ H2O(l). 
D) HCO2-(aq)+ KOH(aq)→ KHCO2(aq)+ OH-(aq). 
E) H+(aq)+ HCO2-(aq)+ K+(aq)+ OH-(aq)→ K+(aq)+ HCO2-(aq)+ H2O(l).

Question 5

Of the following four substances,which would form a basic solution when dissolved in water:
NH4Cl Cu(NO3)2 K2CO3 NaF

Accepted Answer

A) NH4Cl,Cu(NO3)2 
B) K2CO3,NH4Cl 
C) NaF,K2CO3 
D) NaF only 
E) none of them 
A) NH4Cl,Cu(NO3)2 
B) K2CO3,NH4Cl 
C) NaF,K2CO3 
D) NaF only 
E) none of them

Question 6

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 7

Acetic acid is a weak acid in water because it is

Accepted Answer

A) dilute. 
B) only slightly soluble. 
C) unable to hold onto its hydrogen ion. 
D) only slightly dissociated into ions. 
E) completely dissociated into hydronium ions and acetate ions. 
A) dilute. 
B) only slightly soluble. 
C) unable to hold onto its hydrogen ion. 
D) only slightly dissociated into ions. 
E) completely dissociated into hydronium ions and acetate ions.

Question 8

Write the balanced chemical reaction between methyl amine (CH3NH2)and hydrobromic acid (HBr).

Accepted Answer

CH₃NH₂ + HBr

Question 9

What is the pH of a solution in which [H3O+] = 4.1 × 10-2 M?

Accepted Answer

A) 12.61 
B) 1.39 
C) 1.10 
D) 12.90 
E) 4.10 
A) 12.61 
B) 1.39 
C) 1.10 
D) 12.90 
E) 4.10

Question 10

A Brønsted-Lowry base 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 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

In an aqueous solution that is basic,[H3O+] is ________ than 1.0 × 10-7 and ________ than [OH-].

Accepted Answer

A) greater;less 
B) less;greater 
C) greater;greater 
D) less;less 
E) none of the above 
A) greater;less 
B) less;greater 
C) greater;greater 
D) less;less 
E) none of the above

Question 13

Which statement concerning Arrhenius acid-base theory is not correct?

Accepted Answer

A) An Arrhenius acid produces hydrogen ions in water solution. 
B) An Arrhenius base produces hydroxide ions in water solution. 
C) A neutralization reaction produces water plus a salt. 
D) Acid-base reactions must take place in aqueous solution. 
E) none of the above 
A) An Arrhenius acid produces hydrogen ions in water solution. 
B) An Arrhenius base produces hydroxide ions in water solution. 
C) A neutralization reaction produces water plus a salt. 
D) Acid-base reactions must take place in aqueous solution. 
E) none of the above

Question 14

Match the following.
-conjugate base

Accepted Answer

A) the species that results when a base accepts a proton 
B) an acid-base theory that bases reactions on hydrogen and hydroxide ions 
C) a theory that treats acid-base reactions as proton-transfer reactions 
D) a substance which can behave as either an acid or a base 
E) the species that results when an acid donates a proton 
A) the species that results when a base accepts a proton 
B) an acid-base theory that bases reactions on hydrogen and hydroxide ions 
C) a theory that treats acid-base reactions as proton-transfer reactions 
D) a substance which can behave as either an acid or a base 
E) the species that results when an acid donates a proton

Question 15

How many mL of 0.241 M H2SO4 will be needed to neutralize a 50.0 mL sample of 0.191 M KOH?

Accepted Answer

A) 19.8 mL 
B) 31.5 mL 
C) 39.6 mL 
D) 79.3 mL 
E) 126 mL 
A) 19.8 mL 
B) 31.5 mL 
C) 39.6 mL 
D) 79.3 mL 
E) 126 mL

Question 16

Calculate the hydrogen ion concentration in a solution with pH = 6.35.

Accepted Answer

A) 7.65 M 
B) 6.35 M 
C) 4.5 × 10-7 M 
D) 0.80 M 
E) 2.2 × 10-8 M 
A) 7.65 M 
B) 6.35 M 
C) 4.5 × 10-7 M 
D) 0.80 M 
E) 2.2 × 10-8 M

Question 17

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 18

At 25°C,the value of Kw is

Accepted Answer

A) 1.00. 
B) 1.00 × 10-7. 
C) 1.00 × 10-14. 
D) 1.00 × 107. 
E) 1.00 × 1014. 
A) 1.00. 
B) 1.00 × 10-7. 
C) 1.00 × 10-14. 
D) 1.00 × 107. 
E) 1.00 × 1014.

Question 19

According to Brønsted-Lowry theory,acid-base reactions can be described as ________ reactions.

Accepted Answer

A) electrolytic 
B) electron transfer 
C) gas phase 
D) nuclear transfer 
E) proton transfer 
A) electrolytic 
B) electron transfer 
C) gas phase 
D) nuclear transfer 
E) proton transfer

Question 20

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

Exam 10: Acids and Bases

A necessary requirement for a Brønsted base is

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

Which of these,if dissolved in 1.0 L of pure water,would produce a buffer solution?

The net ionic equation for the reaction of formic acid,a weak acid,with potassium hydroxide,a strong base,is

Of the following four substances,which would form a basic solution when dissolved in water: NH4Cl Cu(NO3)2 K2CO3 NaF

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

Acetic acid is a weak acid in water because it is

Write the balanced chemical reaction between methyl amine (CH3NH2)and hydrobromic acid (HBr).

What is the pH of a solution in which [H3O+] = 4.1 × 10-2 M?

A Brønsted-Lowry base is a substance which

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

In an aqueous solution that is basic,[H3O+] is ________ than 1.0 × 10-7 and ________ than [OH-].

Which statement concerning Arrhenius acid-base theory is not correct?

Match the following. -conjugate base

How many mL of 0.241 M H2SO4 will be needed to neutralize a 50.0 mL sample of 0.191 M KOH?

Calculate the hydrogen ion concentration in a solution with pH = 6.35.

Which statement is correct for pure water?

At 25°C,the value of Kw is

According to Brønsted-Lowry theory,acid-base reactions can be described as ________ reactions.

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

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

Aldehydes and Ketones

Amines

Carboxylic Acids and Their Derivatives

Amino Acids and Proteins

Enzymes and Vitamins

Carbohydrates

The Generation of Biochemical Energy

Carbohydrate Metabolism

Lipids

Lipid Metabolism

Protein and Amino Acid Metabolism

Nucleic Acids and Protein Synthesis

Genomics

Chemical Messengers: Hormones, neurotransmitters, and Drugs

Body Fluids

Filters

Of the following four substances,which would form a basic solution when dissolved in water: NH₄Cl Cu(NO₃)₂ K₂CO₃ NaF

Write the balanced chemical reaction between methyl amine (CH₃NH₂)and hydrobromic acid (HBr).

What is the pH of a solution in which [H₃O⁺] = 4.1 × 10^-2 M?

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

In an aqueous solution that is basic,[H₃O⁺] is than 1.0 × 10^-7 and than [OH^-].

How many mL of 0.241 M H₂SO₄ will be needed to neutralize a 50.0 mL sample of 0.191 M KOH?

At 25°C,the value of K_w is

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