Question 1

A neutralization reaction between an acid and a metal hydroxide produces ________.

Accepted Answer

A) water and a salt 
B) hydrogen gas 
C) oxygen gas 
D) sodium hydroxide 
E) ammonia 
A) water and a salt 
B) hydrogen gas 
C) oxygen gas 
D) sodium hydroxide 
E) ammonia

Question 2

When aqueous solutions of Pb(NO3)2 and NaCl are mixed,lead(II)chloride precipitates.The balanced net ionic equation is ________.

Accepted Answer

A) Pb2+ (aq)+ 2Cl- (aq)→ PbCl2 (s) 
B) Pb2+ (aq)+ 2NO3- (aq)→ Pb(NO3)2 (s) 
C) Pb2+ (aq)+ 2NO3- (aq)→ Pb(NO3)2 (aq) 
D) Pb(NO3)2 (aq)+ 2NaCl (aq)→ PbCl2 (s)+ 2NaNO3 (aq) 
E) Pb(NO3)2 (aq)+ 2NaCl (aq)→ PbCl2 (aq)+ 2NaNO3 (s) 
A) Pb2+ (aq)+ 2Cl- (aq)→ PbCl2 (s) 
B) Pb2+ (aq)+ 2NO3- (aq)→ Pb(NO3)2 (s) 
C) Pb2+ (aq)+ 2NO3- (aq)→ Pb(NO3)2 (aq) 
D) Pb(NO3)2 (aq)+ 2NaCl (aq)→ PbCl2 (s)+ 2NaNO3 (aq) 
E) Pb(NO3)2 (aq)+ 2NaCl (aq)→ PbCl2 (aq)+ 2NaNO3 (s)

Question 3

What are the spectator ions in the reaction between KCl (aq)and AgNO3 (aq)?

Accepted Answer

A) K+ and Ag+ 
B) Ag+ and Cl- 
C) K+ and NO3- 
D) Ag+ and NO3- 
E) K+ only 
A) K+ and Ag+ 
B) Ag+ and Cl- 
C) K+ and NO3- 
D) Ag+ and NO3- 
E) K+ only

Question 4

What are the respective concentrations (M)of Mg2+ and Cl- afforded by dissolving 0.325 mol MgCl2 in water and diluting to 250 mL?

Accepted Answer

A) 0.0013 and 0.0013 
B) 0.0013 and 0.0026 
C) 1.30 and.1.30 
D) 1.30 and 2.60 
E) 2.60 and 2.60 
A) 0.0013 and 0.0013 
B) 0.0013 and 0.0026 
C) 1.30 and.1.30 
D) 1.30 and 2.60 
E) 2.60 and 2.60

Question 5

One method for removal of metal ions from a solution is to convert the metal to its elemental form so it can be filtered out as a solid. Which metal can be used to remove aluminum ions from solution?

Accepted Answer

A) zinc 
B) cobalt 
C) lead 
D) copper 
E) none of these 
A) zinc 
B) cobalt 
C) lead 
D) copper 
E) none of these

Question 6

The net ionic equation for the reaction between aqueous sulfuric acid and aqueous sodium hydroxide is ________.

Accepted Answer

A) H+ (aq)+ HSO4- (aq)+ 2OH- (aq)→ 2H2O (l)+ SO42- (aq) 
B) H+ (aq)+ HSO4- (aq)+ 2Na+ (aq)+ 2OH- (aq)→ 2H2O (l)+ 2Na+ (aq)+ SO42-(aq) 
C) SO42- (aq)+ 2Na+ (aq)→ 2Na+ (aq)+ SO42-(aq) 
D) H+ (aq)+ OH- (aq)→ H2O( l) 
E) 2H+ (aq)+ SO42- (aq)+ 2Na+ (aq)+ 2OH- (aq)→ 2H2O (l)+ 2Na+ (aq)+ SO42- (aq) 
A) H+ (aq)+ HSO4- (aq)+ 2OH- (aq)→ 2H2O (l)+ SO42- (aq) 
B) H+ (aq)+ HSO4- (aq)+ 2Na+ (aq)+ 2OH- (aq)→ 2H2O (l)+ 2Na+ (aq)+ SO42-(aq) 
C) SO42- (aq)+ 2Na+ (aq)→ 2Na+ (aq)+ SO42-(aq) 
D) H+ (aq)+ OH- (aq)→ H2O( l) 
E) 2H+ (aq)+ SO42- (aq)+ 2Na+ (aq)+ 2OH- (aq)→ 2H2O (l)+ 2Na+ (aq)+ SO42- (aq)

Question 7

What is the molarity of a NaOH solution if 15.5 mL of a 0.220 M H2SO4 solution is required to neutralize a 25.0-mL sample of the NaOH solution?

Accepted Answer

A) 0.273 
B) 0.355 
C) 0.710 
D) 42.6 
E) 0.136 
A) 0.273 
B) 0.355 
C) 0.710 
D) 42.6 
E) 0.136

Question 8

Oxidation cannot occur without ________.

Accepted Answer

A) acid 
B) oxygen 
C) water 
D) air 
E) reduction 
A) acid 
B) oxygen 
C) water 
D) air 
E) reduction

Question 9

Ca(OH)2 is a strong base.

Accepted Answer

A) True 
 B)False

Question 10

A stock solution of HNO3 is prepared and found to contain 12.7 M of HNO3.If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L,the concentration of the diluted solution is ________ M.

Accepted Answer

A) 0.254 
B) 1.57 
C) 0.635 
D) 635 
E) 254 
A) 0.254 
B) 1.57 
C) 0.635 
D) 635 
E) 254

Question 11

Which of these metals will be oxidized by the ions of cobalt?

Accepted Answer

A) nickel 
B) tin 
C) iron 
D) copper 
E) silver 
A) nickel 
B) tin 
C) iron 
D) copper 
E) silver

Question 12

How many moles of K+ are present in 343 mL of a 1.27 M solution of K3PO4?

Accepted Answer

A) 0.436 
B) 1.31 
C) 0.145 
D) 3.70 
E) 11.1 
A) 0.436 
B) 1.31 
C) 0.145 
D) 3.70 
E) 11.1

Question 13

Calculate the mass percent of sulfuric acid in a solid sample given that a 0.8390 g sample of that solid required 32.22 mL of 0.2012 M NaOH for neutralization.

Accepted Answer

A) 62.11 
B) 2.64 
C) 37.89 
D) 75.78 
E) 1.27 
A) 62.11 
B) 2.64 
C) 37.89 
D) 75.78 
E) 1.27

Question 14

The balanced reaction between aqueous potassium hydroxide and aqueous acetic acid is ________.

Accepted Answer

A) KOH (aq)+ HC2H3O2 (aq)→ OH- (l)+ HC2H3O2+ (aq)+ K (s) 
B) KOH (aq)+ HC2H3O2 (aq)→ H2O (l)+ KC2H3O2 (aq) 
C) KOH (aq)+ HC2H3O2 (aq)→ H2C2H3O3 (aq)+ K (s) 
D) KOH (aq)+ HC2H3O2 (aq)→ KC2H3O3 (aq)+ H2 (g) 
E) KOH (aq)+ HC2H3O2 (aq)→ H2KC2H3O (aq)+ O2 (g) 
A) KOH (aq)+ HC2H3O2 (aq)→ OH- (l)+ HC2H3O2+ (aq)+ K (s) 
B) KOH (aq)+ HC2H3O2 (aq)→ H2O (l)+ KC2H3O2 (aq) 
C) KOH (aq)+ HC2H3O2 (aq)→ H2C2H3O3 (aq)+ K (s) 
D) KOH (aq)+ HC2H3O2 (aq)→ KC2H3O3 (aq)+ H2 (g) 
E) KOH (aq)+ HC2H3O2 (aq)→ H2KC2H3O (aq)+ O2 (g)

Question 15

Of the following elements,________ is the least easily oxidized. sodium
Calcium
Hydrogen
Gold
Platinum

Accepted Answer

A) sodium 
B) gold 
C) calcium 
D) hydrogen 
E) platinum 
A) sodium 
B) gold 
C) calcium 
D) hydrogen 
E) platinum

Question 16

The molarity of an aqueous solution containing 75.3 g of glucose (C6H12O6)in 35.5 mL of solution is ________.

Accepted Answer

A) 14.8 
B) 2.12 
C) 481 
D) 0.0118 
E) 11.8 
A) 14.8 
B) 2.12 
C) 481 
D) 0.0118 
E) 11.8

Question 17

An aliquot (28.7 mL)of a KOH solution required 31.3 mL of 0.118 M HCl for neutralization.What mass (g)of KOH was in the original sample?

Accepted Answer

A) 0.129 
B) 0.190 
C) 0.173 
D) 0.207 
E) 0.215 
A) 0.129 
B) 0.190 
C) 0.173 
D) 0.207 
E) 0.215

Question 18

Which of these metals is the least easily oxidized?
Na
Au
Fe
Ca
Ag

Accepted Answer

A) Na 
B) Au 
C) Fe 
D) Ca 
E) Ag 
A) Na 
B) Au 
C) Fe 
D) Ca 
E) Ag

Question 19

The balanced net ionic equation for the precipitation of calcium carbonate when aqueous solutions of Na2CO3 and CaCl2 are mixed is ________.

Accepted Answer

A) 2Na+ (aq)+ CO32- (aq)→ Na2CO3 (aq) 
B) 2Na+ (aq)+ 2Cl- (aq)→ 2NaCl (aq) 
C) Na+ (aq)+ Cl- (aq)→ NaCl (aq) 
D) Ca+(aq)+ CO32- (aq)→ CaCO3 (s) 
E) Na2CO3 (aq)+ Ca   (aq)→ 2NaCl (aq)+ CaCO3 (s) 
A) 2Na+ (aq)+ CO32- (aq)→ Na2CO3 (aq) 
B) 2Na+ (aq)+ 2Cl- (aq)→ 2NaCl (aq) 
C) Na+ (aq)+ Cl- (aq)→ NaCl (aq) 
D) Ca+(aq)+ CO32- (aq)→ CaCO3 (s) 
E) Na2CO3 (aq)+ Ca   (aq)→ 2NaCl (aq)+ CaCO3 (s)

Question 20

Which of the following is an oxidation-reduction reaction?

Accepted Answer

A) Cu (s)+ 2AgNO3 (aq)→ 2Ag (s)+ Cu(NO3)2 (aq) 
B) HCl (aq)+ NaOH (aq)→ H2O (l)+ NaCl (aq) 
C) AgNO3 (aq)+ HCl (aq)→ AgCl (s)+ HNO3 (aq) 
D) Ba(C2H3O2)2 (aq)+ Na2SO4 (aq)→ BaSO4 (s)+ 2NaC2H3O2(aq) 
E) H2CO3 (aq)+ Ca(NO3)2 (aq)→ 2HNO3 (aq)+ CaCO3 (s) 
A) Cu (s)+ 2AgNO3 (aq)→ 2Ag (s)+ Cu(NO3)2 (aq) 
B) HCl (aq)+ NaOH (aq)→ H2O (l)+ NaCl (aq) 
C) AgNO3 (aq)+ HCl (aq)→ AgCl (s)+ HNO3 (aq) 
D) Ba(C2H3O2)2 (aq)+ Na2SO4 (aq)→ BaSO4 (s)+ 2NaC2H3O2(aq) 
E) H2CO3 (aq)+ Ca(NO3)2 (aq)→ 2HNO3 (aq)+ CaCO3 (s)

Exam 4: Reactions in Aqueous Solution

A neutralization reaction between an acid and a metal hydroxide produces ________.

When aqueous solutions of Pb(NO3)2 and NaCl are mixed,lead(II)chloride precipitates.The balanced net ionic equation is ________.

What are the spectator ions in the reaction between KCl (aq)and AgNO3 (aq)?

What are the respective concentrations (M)of Mg2+ and Cl- afforded by dissolving 0.325 mol MgCl2 in water and diluting to 250 mL?

One method for removal of metal ions from a solution is to convert the metal to its elemental form so it can be filtered out as a solid. Which metal can be used to remove aluminum ions from solution?

The net ionic equation for the reaction between aqueous sulfuric acid and aqueous sodium hydroxide is ________.

What is the molarity of a NaOH solution if 15.5 mL of a 0.220 M H2SO4 solution is required to neutralize a 25.0-mL sample of the NaOH solution?

Oxidation cannot occur without ________.

Ca(OH)2 is a strong base.

A stock solution of HNO3 is prepared and found to contain 12.7 M of HNO3.If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L,the concentration of the diluted solution is ________ M.

Which of these metals will be oxidized by the ions of cobalt?

How many moles of K+ are present in 343 mL of a 1.27 M solution of K3PO4?

Calculate the mass percent of sulfuric acid in a solid sample given that a 0.8390 g sample of that solid required 32.22 mL of 0.2012 M NaOH for neutralization.

The balanced reaction between aqueous potassium hydroxide and aqueous acetic acid is ________.

Of the following elements,________ is the least easily oxidized. sodium Calcium Hydrogen Gold Platinum

The molarity of an aqueous solution containing 75.3 g of glucose (C6H12O6)in 35.5 mL of solution is ________.

An aliquot (28.7 mL)of a KOH solution required 31.3 mL of 0.118 M HCl for neutralization.What mass (g)of KOH was in the original sample?

Which of these metals is the least easily oxidized? Na Au Fe Ca Ag

The balanced net ionic equation for the precipitation of calcium carbonate when aqueous solutions of Na2CO3 and CaCl2 are mixed is ________.

Which of the following is an oxidation-reduction reaction?

Introduction: Matter, energy, and Measurement

Atoms, molecules, and Ions

Chemical Reactions and Reaction Stoichiometry

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

When aqueous solutions of Pb(NO₃)₂ and NaCl are mixed,lead(II)chloride precipitates.The balanced net ionic equation is ________.

What are the spectator ions in the reaction between KCl (aq)and AgNO₃(aq)?

What are the respective concentrations (M)of Mg²⁺ and Cl^- afforded by dissolving 0.325 mol MgCl₂in water and diluting to 250 mL?

What is the molarity of a NaOH solution if 15.5 mL of a 0.220 M H₂SO₄solution is required to neutralize a 25.0-mL sample of the NaOH solution?

Ca(OH)₂ is a strong base.

A stock solution of HNO₃ is prepared and found to contain 12.7 M of HNO₃.If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L,the concentration of the diluted solution is ________ M.

How many moles of K⁺ are present in 343 mL of a 1.27 M solution of K₃PO₄?

The molarity of an aqueous solution containing 75.3 g of glucose (C₆H₁₂O₆)in 35.5 mL of solution is ________.

The balanced net ionic equation for the precipitation of calcium carbonate when aqueous solutions of Na₂CO₃ and CaCl₂ are mixed is ________.