Question 1

Select the classification for the following reaction. 2Ag+(aq) + Zn(s) F1F1F1S1F1F1F10 2Ag(s) + Zn2+(aq)

Accepted Answer

A)  displacement 
B)  decomposition 
C)  combination 
D)  precipitation 
E)  acid-base 
A)  displacement 
B)  decomposition 
C)  combination 
D)  precipitation 
E)  acid-base

Question 2

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 3

Consider the reaction: 
3Co2+(aq) + 6NO3-(aq) + 6Na+(aq) + 2PO43-(aq) F1F1F1S1F1F1F10 Co3(PO4)2(s) + 6Na+(aq) + 6NO3-(aq)
Identify the net ionic equation for this reaction.

Accepted Answer

A)  Na+(aq) + NO3-(aq) F1F1F1S1F1F1F10 NaNO3(aq) 
B)  3Co2+(aq) + NO3-(aq) + Na+(aq) + 2PO43-(aq) F1F1F1S1F1F1F10 Co3(PO4)2(s) + NaNO3(aq) 
C)  3Co2+(aq) + 6NO3-(aq) + 6Na+(aq) + 2PO43-(aq) F1F1F1S1F1F1F10 Co3(PO4)2(s) + 6NaNO3(aq) 
D)  3Co2+(aq) + 2PO43-(aq) F1F1F1S1F1F1F10 Co3(PO4)2(s) 
E)  None of the above is the correct net ionic equation. 
A)  Na+(aq) + NO3-(aq) F1F1F1S1F1F1F10 NaNO3(aq) 
B)  3Co2+(aq) + NO3-(aq) + Na+(aq) + 2PO43-(aq) F1F1F1S1F1F1F10 Co3(PO4)2(s) + NaNO3(aq) 
C)  3Co2+(aq) + 6NO3-(aq) + 6Na+(aq) + 2PO43-(aq) F1F1F1S1F1F1F10 Co3(PO4)2(s) + 6NaNO3(aq) 
D)  3Co2+(aq) + 2PO43-(aq) F1F1F1S1F1F1F10 Co3(PO4)2(s) 
E)  None of the above is the correct net ionic equation.

Question 4

For each of the following species, write down, next to the formula, the oxidation number of the indicated atom.
a. P in H2PO2-
b. S in Na2S2O3
c. C in CH2O

Accepted Answer

Question 5

Which one of the following substances, when dissolved in water at equal molar concentrations, will give the solution with the lowest electrical conductivity?

Accepted Answer

A)  CaCl2 
B)  HNO3 
C)  NH3 
D)  C6H12O6 (glucose) 
E)  CO2 
A)  CaCl2 
B)  HNO3 
C)  NH3 
D)  C6H12O6 (glucose) 
E)  CO2

Question 6

In a redox reaction, the oxidizing agent undergoes loss of electrons.

Accepted Answer

A) True 
 B)False

Question 7

Which of the following is most soluble in water?

Accepted Answer

A)  benzene, C6H6 
B)  potassium nitrate, KNO3 
C)  carbon tetrachloride, CCl4 
D)  hexane, C6H14 
E)  ethane, C2H4 
A)  benzene, C6H6 
B)  potassium nitrate, KNO3 
C)  carbon tetrachloride, CCl4 
D)  hexane, C6H14 
E)  ethane, C2H4

Question 8

Which one of the following substances is the best electrolyte?

Accepted Answer

A)  CO 
B)  CH3Cl 
C)  CH4 
D)  C2H5OH 
E)  HCl 
A)  CO 
B)  CH3Cl 
C)  CH4 
D)  C2H5OH 
E)  HCl

Question 9

Select the precipitate that forms when aqueous lead(II) nitrate reacts with aqueous sodium sulfate.

Accepted Answer

A)  NaNO3 
B)  Na2NO3 
C)  PbSO4 
D)  Pb2SO4 
E)  PbS 
A)  NaNO3 
B)  Na2NO3 
C)  PbSO4 
D)  Pb2SO4 
E)  PbS

Question 10

Sulfuric acid (H2SO4) reacts with potassium hydroxide (KOH) as follows.
H2SO4(aq) + 2KOH(aq) F1F1F1S1F1F1F10 K2SO4(aq) + 2H2O(l)
Calculate the volume of 0.100 M sulfuric acid required to neutralize 25.0 mL of 0.0821 M KOH. Show all your work.

Accepted Answer

Question 11

How many milliliters of 1.58 M HCl are needed to react completely with 23.2 g of NaHCO3 (   = 84.02 g/mol)? HCl(aq) + NaHCO3(s) F1F1F1S1F1F1F10 NaCl(s) + H2O(l) + CO2(g)

Accepted Answer

A)  638 mL 
B)  572 mL 
C)  536 mL 
D)  276 mL 
E)  175 mL 
A)  638 mL 
B)  572 mL 
C)  536 mL 
D)  276 mL 
E)  175 mL

Question 12

Select the net ionic equation for the reaction between sodium chloride and mercury(I) nitrate. 2NaCl(aq) + Hg2(NO3)2(aq) F1F1F1S1F1F1F10 NaNO3(aq) + Hg2Cl2(s)

Accepted Answer

A)  Na+(aq) + NO3-(aq) F1F1F1S1F1F1F10 NaNO3(aq) 
B)  Hg22+(aq) + 2Cl-(aq) F1F1F1S1F1F1F10 Hg2Cl2(s) 
C)  NaCl(aq) F1F1F1S1F1F1F10 Na+(aq) + Cl-(aq) 
D)  Hg2(NO3)2(aq) F1F1F1S1F1F1F10 Hg22+(aq) + 2NO3-(aq) 
E)  Hg22+(aq) F1F1F1S1F1F1F10 Hg2(s) 
A)  Na+(aq) + NO3-(aq) F1F1F1S1F1F1F10 NaNO3(aq) 
B)  Hg22+(aq) + 2Cl-(aq) F1F1F1S1F1F1F10 Hg2Cl2(s) 
C)  NaCl(aq) F1F1F1S1F1F1F10 Na+(aq) + Cl-(aq) 
D)  Hg2(NO3)2(aq) F1F1F1S1F1F1F10 Hg22+(aq) + 2NO3-(aq) 
E)  Hg22+(aq) F1F1F1S1F1F1F10 Hg2(s)

Question 13

In each of the following cases, write down the oxidation number of the indicated atom.
a. P in P4
b. C in C2H6
c. S in H2SO4
d. Mn in MnO4-
e. S in S4O62-
f. P in Na3PO4

Accepted Answer

a. 0
b. -3

Question 14

Select the precipitate that forms when the following reactants are mixed. Na2CO3(aq) + BaCl2(aq) F1F1F1S1F1F1F10

Accepted Answer

A)  Ba2CO3 
B)  BaCO3 
C)  NaCl 
D)  NaCl2 
E)  BaO 
A)  Ba2CO3 
B)  BaCO3 
C)  NaCl 
D)  NaCl2 
E)  BaO

Question 15

How many moles of ions are released when 0.27 mol of cobalt(II) chloride, CoCl2, is dissolved in water?

Accepted Answer

A)  0.81 mol 
B)  0.54 mol 
C)  0.27 mol 
D)  0.18 mol 
E)  0.090 mol 
A)  0.81 mol 
B)  0.54 mol 
C)  0.27 mol 
D)  0.18 mol 
E)  0.090 mol

Question 16

Which of the following is a weak base?

Accepted Answer

A)  NH3 
B)  Ca(OH)2 
C)  Ba(OH)2 
D)  NaOH 
E)  CH3COOH 
A)  NH3 
B)  Ca(OH)2 
C)  Ba(OH)2 
D)  NaOH 
E)  CH3COOH

Question 17

Select the classification for the following reaction. 2H2O2(aq) F1F1F1S1F1F1F10 2H2O(l) + O2(g)

Accepted Answer

A)  combination 
B)  decomposition 
C)  displacement 
D)  acid-base 
E)  none of the above 
A)  combination 
B)  decomposition 
C)  displacement 
D)  acid-base 
E)  none of the above

Question 18

Select the precipitate that forms when the following reactants are mixed. 
Mg(CH3COO)2(aq) + LiOH(aq) F1F1F1S1F1F1F10

Accepted Answer

A)  LiCH3COO 
B)  Li(CH3COO)2 
C)  MgOH 
D)  Mg(OH)2 
E)  CH3OH 
A)  LiCH3COO 
B)  Li(CH3COO)2 
C)  MgOH 
D)  Mg(OH)2 
E)  CH3OH

Question 19

The correct method for preparing one liter of a 1.0 M solution of X is to dissolve exactly one mole of X in exactly one liter of water.

Accepted Answer

A) True 
 B)False

Question 20

An aqueous solution of lead nitrate, Pb(NO3)2, is mixed with one of sodium chromate, Na2CrO4, resulting in the formation of a precipitate of lead chromate. Write a balanced net ionic equation for this precipitation reaction, showing all phases.

Accepted Answer

Pb²⁺(aq) + C

Exam 4: The Major Classes of Chemical Reactions

Select the classification for the following reaction. 2Ag+(aq) + Zn(s)  2Ag(s) + Zn2+(aq)

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

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.

For each of the following species, write down, next to the formula, the oxidation number of the indicated atom. a. P in H2PO2- b. S in Na2S2O3 c. C in CH2O

Which one of the following substances, when dissolved in water at equal molar concentrations, will give the solution with the lowest electrical conductivity?

In a redox reaction, the oxidizing agent undergoes loss of electrons.

Which of the following is most soluble in water?

Which one of the following substances is the best electrolyte?

Select the precipitate that forms when aqueous lead(II) nitrate reacts with aqueous sodium sulfate.

Sulfuric acid (H2SO4) reacts with potassium hydroxide (KOH) as follows. H2SO4(aq) + 2KOH(aq)  K2SO4(aq) + 2H2O(l) Calculate the volume of 0.100 M sulfuric acid required to neutralize 25.0 mL of 0.0821 M KOH. Show all your work.

How many milliliters of 1.58 M HCl are needed to react completely with 23.2 g of NaHCO3 ( = 84.02 g/mol)? HCl(aq) + NaHCO3(s)  NaCl(s) + H2O(l) + CO2(g)

Select the net ionic equation for the reaction between sodium chloride and mercury(I) nitrate. 2NaCl(aq) + Hg2(NO3)2(aq)  NaNO3(aq) + Hg2Cl2(s)

In each of the following cases, write down the oxidation number of the indicated atom. a. P in P4 b. C in C2H6 c. S in H2SO4 d. Mn in MnO4- e. S in S4O62- f. P in Na3PO4

Select the precipitate that forms when the following reactants are mixed. Na2CO3(aq) + BaCl2(aq) 

How many moles of ions are released when 0.27 mol of cobalt(II) chloride, CoCl2, is dissolved in water?

Which of the following is a weak base?

Select the classification for the following reaction. 2H2O2(aq)  2H2O(l) + O2(g)

Select the precipitate that forms when the following reactants are mixed. Mg(CH3COO)2(aq) + LiOH(aq) 

The correct method for preparing one liter of a 1.0 M solution of X is to dissolve exactly one mole of X in exactly one liter of water.

An aqueous solution of lead nitrate, Pb(NO3)2, is mixed with one of sodium chromate, Na2CrO4, resulting in the formation of a precipitate of lead chromate. Write a balanced net ionic equation for this precipitation reaction, showing all phases.

Keys to the Study of Chemistry

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: Bonding, Structure, and Reactivity

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 the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Select the classification for the following reaction. 2Ag⁺(aq) + Zn(s)  2Ag(s) + Zn²⁺(aq)

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

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

For each of the following species, write down, next to the formula, the oxidation number of the indicated atom. a. P in H₂PO₂^- b. S in Na₂S₂O₃ c. C in CH₂O

Sulfuric acid (H₂SO₄) reacts with potassium hydroxide (KOH) as follows. H₂SO₄(aq) + 2KOH(aq)  K₂SO₄(aq) + 2H₂O(l) Calculate the volume of 0.100 M sulfuric acid required to neutralize 25.0 mL of 0.0821 M KOH. Show all your work.

How many milliliters of 1.58 M HCl are needed to react completely with 23.2 g of NaHCO₃( = 84.02 g/mol)? HCl(aq) + NaHCO₃(s)  NaCl(s) + H₂O(l) + CO₂(g)

Select the net ionic equation for the reaction between sodium chloride and mercury(I) nitrate. 2NaCl(aq) + Hg₂(NO₃)₂(aq)  NaNO₃(aq) + Hg₂Cl₂(s)

In each of the following cases, write down the oxidation number of the indicated atom. a. P in P₄ b. C in C₂H₆ c. S in H₂SO₄ d. Mn in MnO₄^- e. S in S₄O₆^2- f. P in Na₃PO₄

Select the precipitate that forms when the following reactants are mixed. Na₂CO₃(aq) + BaCl₂(aq) 

How many moles of ions are released when 0.27 mol of cobalt(II) chloride, CoCl₂, is dissolved in water?

Select the classification for the following reaction. 2H₂O₂(aq)  2H₂O(l) + O₂(g)

Select the precipitate that forms when the following reactants are mixed. Mg(CH₃COO)₂(aq) + LiOH(aq) 

An aqueous solution of lead nitrate, Pb(NO₃)₂, is mixed with one of sodium chromate, Na₂CrO₄, resulting in the formation of a precipitate of lead chromate. Write a balanced net ionic equation for this precipitation reaction, showing all phases.