Question 1

Identify the oxidizing agent in the following redox reaction. Hg2+(aq) + Cu(s) → Cu2+(aq) + Hg(l)

Accepted Answer

A) Hg 2+( aq) 
B) Cu( s) 
C) Cu 2+( aq) 
D) Hg( l) 
E) Hg 2+( aq)and Cu 2+( aq) 
A) Hg 2+( aq) 
B) Cu( s) 
C) Cu 2+( aq) 
D) Hg( l) 
E) Hg 2+( aq)and Cu 2+( aq)

Question 2

Calcium chloride is used to melt ice and snow on roads and sidewalks and to remove water from organic liquids. Calculate the molarity of a solution prepared by diluting 165 mL of 0.688 M calcium chloride to 925.0 mL.

Accepted Answer

A) 3.86 M 
B) 0.743 M 
C) 0.222 M 
D) 0.123 M 
E) 0.114 M 
A) 3.86 M 
B) 0.743 M 
C) 0.222 M 
D) 0.123 M 
E) 0.114 M

Question 3

1.0M aqueous solutions of the following substances are prepared. Which one would you expect to have the lowest electrical conductivity?

Accepted Answer

A) NaOH 
B) CH 3CH 2OH (ethanol) 
C) KBr 
D) CH 3COOH (acetic acid) 
E) HClO 4 
A) NaOH 
B) CH 3CH 2OH (ethanol) 
C) KBr 
D) CH 3COOH (acetic acid) 
E) HClO 4

Question 4

Aqueous potassium iodate (KIO3) and potassium iodide (KI) react in the presence of dilute hydrochloric acid (HCl), as shown below. KIO3(aq) + 5KI(aq) + 6HCl(aq) → 3I2(aq) + 6KCl(aq) + 3H2O(l)
What mass of iodine (I2) is formed when 15.0 mL of 0.0050 M KIO3 solution reacts with 30.0 mL of 0.010 M KI solution in the presence of excess HCl?

Accepted Answer

A) 0.023 g I 2 
B) 0.029 g I 2 
C) 0.057 g I 2 
D) 0.046 g I 2 
E) 0.076 g I 2 
A) 0.023 g I 2 
B) 0.029 g I 2 
C) 0.057 g I 2 
D) 0.046 g I 2 
E) 0.076 g I 2

Question 5

During a titration, the following data were collected. A 25 mL portion of an unknown acid solution was titrated with 1.0 M NaOH. It required 65 mL of the base to neutralize the sample. How many moles of acid are present in 3.0 liters of this unknown solution?

Accepted Answer

A) 2.6 moles 
B) 0.9 moles 
C) 8.7 moles 
D) 7.8 moles 
E) 5.6 moles 
A) 2.6 moles 
B) 0.9 moles 
C) 8.7 moles 
D) 7.8 moles 
E) 5.6 moles

Question 6

How many moles of H+(aq) ions are present in 1.25 L of 0.75 M nitric acid?

Accepted Answer

A) 0.60 mol 
B) 0.75 mol 
C) 0.94 mol 
D) 1.7 mol 
E) 1.9 mol 
A) 0.60 mol 
B) 0.75 mol 
C) 0.94 mol 
D) 1.7 mol 
E) 1.9 mol

Question 7

All acid-base reactions produce a salt and water as the only products.

Accepted Answer

A) True 
 B)False

Question 8

Sodium thiosulfate, Na2S2O3, is used as a "fixer" in black and white photography. Identify the reducing agent in the reaction of thiosulfate with iodine. 2S2O32-(aq) + I2(aq) → S4O62-(aq) + 2I-(aq)

Accepted Answer

A) I 2( aq) 
B) I −( aq) 
C) S 2O 3 2−( aq) 
D) S 4O 6 2−( aq) 
E) S 2O 3 2−( aq)and I −( aq) 
A) I 2( aq) 
B) I −( aq) 
C) S 2O 3 2−( aq) 
D) S 4O 6 2−( aq) 
E) S 2O 3 2−( aq)and I −( aq)

Question 9

Consider the reaction: 3Co2+(aq) + 6NO3(aq) + 6Na+(aq) + 2PO43-(aq) → Co3(PO4)2(s) + 6Na+(aq) + 6NO3(aq)
Identify the net ionic equation for this reaction.

Accepted Answer

A) Na +( aq) + NO 3 −( aq)→ NaNO 3( aq) 
B) 3Co 2+( aq)+ NO 3 −( aq)+ Na +( aq)+ 2PO 4 3−( aq)→ Co 3(PO 4)2( s)+ NaNO 3( aq) 
C) 3Co 2+( aq)+ 6NO 3 −( aq)+ 6Na +( aq)+ 2PO 4 3−( aq)→ Co 3(PO 4)2( s)+ 6NaNO 3( aq) 
D) 3Co 2+( aq)+ 2PO 4 3−( aq)→ Co 3(PO 4)2( s) 
E) None of these choices are correct. 
A) Na +( aq) + NO 3 −( aq)→ NaNO 3( aq) 
B) 3Co 2+( aq)+ NO 3 −( aq)+ Na +( aq)+ 2PO 4 3−( aq)→ Co 3(PO 4)2( s)+ NaNO 3( aq) 
C) 3Co 2+( aq)+ 6NO 3 −( aq)+ 6Na +( aq)+ 2PO 4 3−( aq)→ Co 3(PO 4)2( s)+ 6NaNO 3( aq) 
D) 3Co 2+( aq)+ 2PO 4 3−( aq)→ Co 3(PO 4)2( s) 
E) None of these choices are correct.

Question 10

Select the classification for the following reaction. 2NaCl(l)   2Na(l) + Cl2(g)

Accepted Answer

A) Acid-base 
B) Precipitation 
C) Combination 
D) Displacement 
E) Decomposition 
A) Acid-base 
B) Precipitation 
C) Combination 
D) Displacement 
E) Decomposition

Question 11

The oxidation numbers of P, S, and Cl in H2PO2-, H2S, and KClO4 are, respectively

Accepted Answer

A) −1, −1, +3. 
B) −1, −2, +7. 
C) +1, −2, +7. 
D) −1, −2, +3. 
E) +1, +2, +7. 
A) −1, −1, +3. 
B) −1, −2, +7. 
C) +1, −2, +7. 
D) −1, −2, +3. 
E) +1, +2, +7.

Identify the oxidizing agent in the following redox reaction. Hg²⁺(aq) + Cu(s) → Cu²⁺(aq) + Hg(l)

Calcium chloride is used to melt ice and snow on roads and sidewalks and to remove water from organic liquids. Calculate the molarity of a solution prepared by diluting 165 mL of 0.688 M calcium chloride to 925.0 mL.

1.0M aqueous solutions of the following substances are prepared. Which one would you expect to have the lowest electrical conductivity?

During a titration, the following data were collected. A 25 mL portion of an unknown acid solution was titrated with 1.0 M NaOH. It required 65 mL of the base to neutralize the sample. How many moles of acid are present in 3.0 liters of this unknown solution?

How many moles of H⁺(aq) ions are present in 1.25 L of 0.75 M nitric acid?

All acid-base reactions produce a salt and water as the only products.

Sodium thiosulfate, Na₂S₂O₃, is used as a "fixer" in black and white photography. Identify the reducing agent in the reaction of thiosulfate with iodine. 2S₂O₃²^-(aq) + I₂(aq) → S₄O₆²^-(aq) + 2I^-(aq)

Consider the reaction: 3Co²⁺(aq) + 6NO₃(aq) + 6Na⁺(aq) + 2PO₄³^-(aq) → Co₃(PO₄)₂(s) + 6Na⁺(aq) + 6NO₃(aq) Identify the net ionic equation for this reaction.

Select the classification for the following reaction. 2NaCl(l) 2Na(l) + Cl₂(g)

The oxidation numbers of P, S, and Cl in H₂PO₂^-, H₂S, and KClO₄ are, respectively

Keys to the Study of Chemistry: Definitions, Units, and Problem Solving

The Components of Matter

Stoichiometry of Formulas and Equations

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main-Group Elements

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and Reaction Direction

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Exam 4: Three Major Classes of Chemical Reactions

Identify the oxidizing agent in the following redox reaction. Hg2+(aq) + Cu(s) → Cu2+(aq) + Hg(l)

Calcium chloride is used to melt ice and snow on roads and sidewalks and to remove water from organic liquids. Calculate the molarity of a solution prepared by diluting 165 mL of 0.688 M calcium chloride to 925.0 mL.

1.0M aqueous solutions of the following substances are prepared. Which one would you expect to have the lowest electrical conductivity?

During a titration, the following data were collected. A 25 mL portion of an unknown acid solution was titrated with 1.0 M NaOH. It required 65 mL of the base to neutralize the sample. How many moles of acid are present in 3.0 liters of this unknown solution?

How many moles of H+(aq) ions are present in 1.25 L of 0.75 M nitric acid?

All acid-base reactions produce a salt and water as the only products.

Sodium thiosulfate, Na2S2O3, is used as a "fixer" in black and white photography. Identify the reducing agent in the reaction of thiosulfate with iodine. 2S2O32-(aq) + I2(aq) → S4O62-(aq) + 2I-(aq)

Consider the reaction: 3Co2+(aq) + 6NO3(aq) + 6Na+(aq) + 2PO43-(aq) → Co3(PO4)2(s) + 6Na+(aq) + 6NO3(aq) Identify the net ionic equation for this reaction.

Select the classification for the following reaction. 2NaCl(l) 2Na(l) + Cl2(g)

The oxidation numbers of P, S, and Cl in H2PO2-, H2S, and KClO4 are, respectively

Keys to the Study of Chemistry: Definitions, Units, and Problem Solving

The Components of Matter

Stoichiometry of Formulas and Equations

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main-Group Elements

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and Reaction Direction

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Identify the oxidizing agent in the following redox reaction. Hg²⁺(aq) + Cu(s) → Cu²⁺(aq) + Hg(l)

How many moles of H⁺(aq) ions are present in 1.25 L of 0.75 M nitric acid?

Sodium thiosulfate, Na₂S₂O₃, is used as a "fixer" in black and white photography. Identify the reducing agent in the reaction of thiosulfate with iodine. 2S₂O₃²^-(aq) + I₂(aq) → S₄O₆²^-(aq) + 2I^-(aq)

Consider the reaction: 3Co²⁺(aq) + 6NO₃(aq) + 6Na⁺(aq) + 2PO₄³^-(aq) → Co₃(PO₄)₂(s) + 6Na⁺(aq) + 6NO₃(aq) Identify the net ionic equation for this reaction.

Select the classification for the following reaction. 2NaCl(l) 2Na(l) + Cl₂(g)

The oxidation numbers of P, S, and Cl in H₂PO₂^-, H₂S, and KClO₄ are, respectively