Question 1

What is the oxidation number of P in PO43-?

Accepted Answer

A)  +5 
B)  +3 
C)  -2 
D)  -3 
E)  -5 
A)  +5 
B)  +3 
C)  -2 
D)  -3 
E)  -5

Question 2

Which of the following represents reduction?

Accepted Answer

A)  Al Al3+ + 3 e- 
B)  O2 + 4 e- 2 O2- 
C)  Fe Fe2+ + 2 e- 
D)  Na Na+ + e- 
E)  H2 2 H+ + 2 e- 
A)  Al Al3+ + 3 e- 
B)  O2 + 4 e- 2 O2- 
C)  Fe Fe2+ + 2 e- 
D)  Na Na+ + e- 
E)  H2 2 H+ + 2 e-

Question 3

Ammonia and sulfuric acid react according to the equation given below. How many milliliters of 0.110 M sulfuric acid are required to exactly neutralize 25.0 mL of 0.0840 M NH3 solution?

Accepted Answer

A)  1.46 mL 
B)  1.82 mL 
C)  3.64 mL 
D)  5.85 mL 
E)  9.55 mL 
A)  1.46 mL 
B)  1.82 mL 
C)  3.64 mL 
D)  5.85 mL 
E)  9.55 mL

Question 4

If a 45.0 mL sample of 2.20 M Na2SO4 is diluted to yield a final solution that is 0.110 M in sodium ions, what is the volume of the final solution?

Accepted Answer

A)  110 mL 
B)  450 mL 
C)  900 mL 
D)  1800 mL 
E)  4500 mL 
A)  110 mL 
B)  450 mL 
C)  900 mL 
D)  1800 mL 
E)  4500 mL

Question 5

A chemical reaction for which spectator ions are deleted is called a(n) _____________ ionic equation.

Accepted Answer

The answer of A chemical reaction for which spectator ions...

Question 6

Which compound will not dissolve in water in large amounts?

Accepted Answer

A)  KNO3 
B)  NH4Cl 
C)  Ca(OH)2 
D)  AgCl 
E)  Ag2SO4 
A)  KNO3 
B)  NH4Cl 
C)  Ca(OH)2 
D)  AgCl 
E)  Ag2SO4

Question 7

A solution is made by dissolving 60.0 g of AlCl3 in enough water to make 250.0 mL of solution. How many moles of ions are in 5.00 mL of solution?

Accepted Answer

A)  3.60 × 10-2 mol 
B)  1.01 × 10-3 mol 
C)  1.25 × 10-3 mol 
D)  5.00 × 10-3 mol 
E)  9.00 × 10-3 mol 
A)  3.60 × 10-2 mol 
B)  1.01 × 10-3 mol 
C)  1.25 × 10-3 mol 
D)  5.00 × 10-3 mol 
E)  9.00 × 10-3 mol

Question 8

A 25.00 mL sample of HCl solution is neutralized by exactly 41.63 mL of 0.1363 M NaOH. What is the molarity of the HCl solution?

Accepted Answer

A)  0.2270 M 
B)  0.2726 M 
C)  0.06815 M 
D)  0.1135 M 
E)  0.05675 M 
A)  0.2270 M 
B)  0.2726 M 
C)  0.06815 M 
D)  0.1135 M 
E)  0.05675 M

Question 9

Which statement about the reaction below is true, given large amounts of reactants?

Accepted Answer

A)  SrSO4 is soluble in water and will not precipitate. 
B)  NaCl is a spectator ion and will not precipitate. 
C)  SO42- is a spectator ion and will not precipitate. 
D)  Na+ is a spectator ion and will not precipitate. 
E)  All compounds in the reaction are soluble in water and no reaction occurs. 
A)  SrSO4 is soluble in water and will not precipitate. 
B)  NaCl is a spectator ion and will not precipitate. 
C)  SO42- is a spectator ion and will not precipitate. 
D)  Na+ is a spectator ion and will not precipitate. 
E)  All compounds in the reaction are soluble in water and no reaction occurs.

Question 10

How many grams of PbI2 will precipitate from the reaction of 14.0 mL of 0.190 M Pb(NO3)2 with excess KI solution? Assume that all of the PbI2 is insoluble.

Accepted Answer

A)  1.23 g 
B)  1.33 g 
C)  2.66 g 
D)  3.69 g 
E)  6260 g 
A)  1.23 g 
B)  1.33 g 
C)  2.66 g 
D)  3.69 g 
E)  6260 g

Question 11

Which of the following best describes an acid?

Accepted Answer

A)  Acids react with many metals to produce a flammable gas. 
B)  Acids react with many metals to produce precipitates. 
C)  Acids increase the hydrogen ion concentration of water when dissolved in it. 
D)  Both a and c. 
E)  All of these. 
A)  Acids react with many metals to produce a flammable gas. 
B)  Acids react with many metals to produce precipitates. 
C)  Acids increase the hydrogen ion concentration of water when dissolved in it. 
D)  Both a and c. 
E)  All of these.

Question 12

What is the net ionic equation for the reaction of AlCl3 and NaOH?

Accepted Answer

A)  Na+ + Cl- NaCl 
B)  Al+ + OH- AlOH 
C)  Al3+ + 3OH- Al(OH)3 
D)  Al3+ + OH3- AlOH 
E)  Na3+ + 3Cl- NaCl3 
A)  Na+ + Cl- NaCl 
B)  Al+ + OH- AlOH 
C)  Al3+ + 3OH- Al(OH)3 
D)  Al3+ + OH3- AlOH 
E)  Na3+ + 3Cl- NaCl3

Question 13

Which substance is oxidized in the reaction below?

Accepted Answer

A)  Na+ 
B)  PbO 
C)  NaNO3 
D)  NaNO2 
E)  none of these 
A)  Na+ 
B)  PbO 
C)  NaNO3 
D)  NaNO2 
E)  none of these

Question 14

What is the net ionic equation for the reaction of Ca(NO3)2 and Na2SO4?

Accepted Answer

A)  2Ca+ + SO42- Ca2SO4 
B)  Na+ + NO3- NaNO3 
C)  Ca2+ + SO42- CaSO4 
D)  Na2+ + 2NO3- Na(NO3)2 
E)  Ca+ + SO4- CaSO4 
A)  2Ca+ + SO42- Ca2SO4 
B)  Na+ + NO3- NaNO3 
C)  Ca2+ + SO42- CaSO4 
D)  Na2+ + 2NO3- Na(NO3)2 
E)  Ca+ + SO4- CaSO4

Question 15

What is the oxidation number of N in NO?

Accepted Answer

A)  -2 
B)  -1 
C)  0 
D)  +1 
E)  +2 
A)  -2 
B)  -1 
C)  0 
D)  +1 
E)  +2

Question 16

Which element is most reactive?

Accepted Answer

A)  Cu 
B)  Fe 
C)  K 
D)  Mg 
E)  Pb 
A)  Cu 
B)  Fe 
C)  K 
D)  Mg 
E)  Pb

Question 17

How many grams of KCl are in 125.0 mL of 0.375 M KCl?

Accepted Answer

A)  3.49 g 
B)  0.0469 g 
C)  3.49 × 10-3 g 
D)  46.9 g 
E)  0.938 g 
A)  3.49 g 
B)  0.0469 g 
C)  3.49 × 10-3 g 
D)  46.9 g 
E)  0.938 g

Question 18

Which statement about neutralization reactions is true?

Accepted Answer

A)  A weak acid cannot neutralize a strong base. 
B)  The net ionic equation for a neutralization reaction shows the formation of hydrogen gas 
C)  The net ionic equation for a neutralization reaction shows the formation of soluble salts. 
D)  The net ionic equation for a neutralization reaction shows the formation of water. 
E)  Organic acids neutralize bases by forming hydrogen gas. 
A)  A weak acid cannot neutralize a strong base. 
B)  The net ionic equation for a neutralization reaction shows the formation of hydrogen gas 
C)  The net ionic equation for a neutralization reaction shows the formation of soluble salts. 
D)  The net ionic equation for a neutralization reaction shows the formation of water. 
E)  Organic acids neutralize bases by forming hydrogen gas.

Question 19

All of the following are strong electrolytes except:

Accepted Answer

A)  CH3COOH. 
B)  H2SO4. 
C)  HNO3. 
D)  HBr. 
E)  NaOH. 
A)  CH3COOH. 
B)  H2SO4. 
C)  HNO3. 
D)  HBr. 
E)  NaOH.

Question 20

Give an example of a strong base.

Accepted Answer

LiOH, NaOH

What is the oxidation number of P in PO₄^3-?

Which of the following represents reduction?

Ammonia and sulfuric acid react according to the equation given below. How many milliliters of 0.110 M sulfuric acid are required to exactly neutralize 25.0 mL of 0.0840 M NH₃ solution?

If a 45.0 mL sample of 2.20 M Na₂SO₄ is diluted to yield a final solution that is 0.110 M in sodium ions, what is the volume of the final solution?

A chemical reaction for which spectator ions are deleted is called a(n) _____________ ionic equation.

Which compound will not dissolve in water in large amounts?

A solution is made by dissolving 60.0 g of AlCl₃ in enough water to make 250.0 mL of solution. How many moles of ions are in 5.00 mL of solution?

A 25.00 mL sample of HCl solution is neutralized by exactly 41.63 mL of 0.1363 M NaOH. What is the molarity of the HCl solution?

Which statement about the reaction below is true, given large amounts of reactants?

How many grams of PbI₂ will precipitate from the reaction of 14.0 mL of 0.190 M Pb(NO₃)₂ with excess KI solution? Assume that all of the PbI₂ is insoluble.

Which of the following best describes an acid?

What is the net ionic equation for the reaction of AlCl₃ and NaOH?

Which substance is oxidized in the reaction below?

What is the net ionic equation for the reaction of Ca(NO₃)₂ and Na₂SO₄?

What is the oxidation number of N in NO?

Which element is most reactive?

How many grams of KCl are in 125.0 mL of 0.375 M KCl?

Which statement about neutralization reactions is true?

All of the following are strong electrolytes except:

Give an example of a strong base.

The Nature of Chemistry

Atoms and Elements

Chemical Compounds

Quantities of Reactants and Products

Energy and Chemical Reactions

Electron Configurations and the Periodic Table

Covalent Bonding

Molecular Structure

Gases and the Atmosphere

Liquids, Solids, and Materials

Chemical Kinetics: Rates of Reactions

Chemical Equilibrium

The Chemistry of Solutes and Solutions

Acids and Bases

Additional Aqueous Equilibria

Thermodynamics: Directionality of Chemical Reactions

Electrochemistry and Its Applications

Nuclear Chemistry

Filters

Exam 5: Chemical Reactions

What is the oxidation number of P in PO43-?

Which of the following represents reduction?

Ammonia and sulfuric acid react according to the equation given below. How many milliliters of 0.110 M sulfuric acid are required to exactly neutralize 25.0 mL of 0.0840 M NH3 solution?

If a 45.0 mL sample of 2.20 M Na2SO4 is diluted to yield a final solution that is 0.110 M in sodium ions, what is the volume of the final solution?

A chemical reaction for which spectator ions are deleted is called a(n) _____________ ionic equation.

Which compound will not dissolve in water in large amounts?

A solution is made by dissolving 60.0 g of AlCl3 in enough water to make 250.0 mL of solution. How many moles of ions are in 5.00 mL of solution?

A 25.00 mL sample of HCl solution is neutralized by exactly 41.63 mL of 0.1363 M NaOH. What is the molarity of the HCl solution?

Which statement about the reaction below is true, given large amounts of reactants?

How many grams of PbI2 will precipitate from the reaction of 14.0 mL of 0.190 M Pb(NO3)2 with excess KI solution? Assume that all of the PbI2 is insoluble.

Which of the following best describes an acid?

What is the net ionic equation for the reaction of AlCl3 and NaOH?

Which substance is oxidized in the reaction below?

What is the net ionic equation for the reaction of Ca(NO3)2 and Na2SO4?

What is the oxidation number of N in NO?

Which element is most reactive?

How many grams of KCl are in 125.0 mL of 0.375 M KCl?

Which statement about neutralization reactions is true?

All of the following are strong electrolytes except:

Give an example of a strong base.

The Nature of Chemistry

Atoms and Elements

Chemical Compounds

Quantities of Reactants and Products

Energy and Chemical Reactions

Electron Configurations and the Periodic Table

Covalent Bonding

Molecular Structure

Gases and the Atmosphere

Liquids, Solids, and Materials

Chemical Kinetics: Rates of Reactions

Chemical Equilibrium

The Chemistry of Solutes and Solutions

Acids and Bases

Additional Aqueous Equilibria

Thermodynamics: Directionality of Chemical Reactions

Electrochemistry and Its Applications

Nuclear Chemistry

Filters

What is the oxidation number of P in PO₄^3-?

Ammonia and sulfuric acid react according to the equation given below. How many milliliters of 0.110 M sulfuric acid are required to exactly neutralize 25.0 mL of 0.0840 M NH₃ solution?

If a 45.0 mL sample of 2.20 M Na₂SO₄ is diluted to yield a final solution that is 0.110 M in sodium ions, what is the volume of the final solution?

A solution is made by dissolving 60.0 g of AlCl₃ in enough water to make 250.0 mL of solution. How many moles of ions are in 5.00 mL of solution?

How many grams of PbI₂ will precipitate from the reaction of 14.0 mL of 0.190 M Pb(NO₃)₂ with excess KI solution? Assume that all of the PbI₂ is insoluble.

What is the net ionic equation for the reaction of AlCl₃ and NaOH?

What is the net ionic equation for the reaction of Ca(NO₃)₂ and Na₂SO₄?