Question 1

How many grams of NaOH (MW = 40.0)are there in 200.0 mL of a 0.175 M NaOH solution?

Accepted Answer

A) .00219 
B) 114 
C) 1.40 
D) 0.0350 
E) 14.0 
A) .00219 
B) 114 
C) 1.40 
D) 0.0350 
E) 14.0

Question 2

Based on the equations below,which metal is the most active?
Pb(NO3)2 (aq)+ Ni (s)→ Ni(NO3)2 (aq)+ Pb (s)
Pb(NO3)2 (aq)+ Ag (s)→ No reaction
Cu(NO3)2 (aq)+ Ni (s)→ Ni(NO3)2 (aq)+ Cu (s)

Accepted Answer

A) Ni 
B) Ag 
C) Cu 
D) Pb 
E) N 
A) Ni 
B) Ag 
C) Cu 
D) Pb 
E) N

Question 3

How many milliliters of 1.500 M aqueous KI solution must be added to an aqueous solution containing 0.100 mol of Pb(NO3)2 to completely precipitate the lead?

Accepted Answer

A) 7.50 × 10-3 
B) 66.7 
C) 0.0667 
D) 0.133 
E) 133 
A) 7.50 × 10-3 
B) 66.7 
C) 0.0667 
D) 0.133 
E) 133

Question 4

The net ionic equation for the dissolution of zinc metal in aqueous hydrobromic acid is ________.

Accepted Answer

A) Zn (s)+ 2Br- (aq)→ ZnBr2 (aq) 
B) Zn (s)+ 2HBr (aq)→ ZnBr2 (aq)+ 2H+ (aq) 
C) Zn (s)+ 2HBr (aq)→ ZnBr2 (s)+ 2H+ (aq) 
D) Zn (s)+ 2H+ (aq)→ Zn2+ (aq)+ H2 (g) 
E) 2Zn (s)+ H+ (aq)→ 2Zn2+ (aq)+ H2 (g) 
A) Zn (s)+ 2Br- (aq)→ ZnBr2 (aq) 
B) Zn (s)+ 2HBr (aq)→ ZnBr2 (aq)+ 2H+ (aq) 
C) Zn (s)+ 2HBr (aq)→ ZnBr2 (s)+ 2H+ (aq) 
D) Zn (s)+ 2H+ (aq)→ Zn2+ (aq)+ H2 (g) 
E) 2Zn (s)+ H+ (aq)→ 2Zn2+ (aq)+ H2 (g)

Question 5

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

Accepted Answer

A) H+ (aq)+ HNO3 (aq)+ 2OH- (aq)→ 2H2O (l)+ NO3- (aq) 
B) HNO3 (aq)+ NaOH (aq)→ NaNO3 (aq)+ H2O (l) 
C) H+ (aq)+ OH- (aq)→ H2O (l) 
D) HNO3 (aq)+ OH- (aq)→ NO3- (aq)+ H2O (l) 
E) H+ (aq)+ Na+ (aq)+ OH- (aq)→ H2O (l)+ Na+ (aq) 
A) H+ (aq)+ HNO3 (aq)+ 2OH- (aq)→ 2H2O (l)+ NO3- (aq) 
B) HNO3 (aq)+ NaOH (aq)→ NaNO3 (aq)+ H2O (l) 
C) H+ (aq)+ OH- (aq)→ H2O (l) 
D) HNO3 (aq)+ OH- (aq)→ NO3- (aq)+ H2O (l) 
E) H+ (aq)+ Na+ (aq)+ OH- (aq)→ H2O (l)+ Na+ (aq)

Question 6

A 650 mL sodium bromide solution has a bromide ion concentration of 0.245 M.What is the mass (g)of sodium bromide in solution?

Accepted Answer

A) 103 
B) 0.00155 
C) 16400 
D) 16.4 
E) 0.159 
A) 103 
B) 0.00155 
C) 16400 
D) 16.4 
E) 0.159

Question 7

How many milliliters of a 14.2 M HCl solution is needed to prepare 0.715 L solution of HCl with a concentration of 0.350 M?

Accepted Answer

A) 0.0568 
B) 3.55 
C) 56.8 
D) 17.6 
E) 0.0176 
A) 0.0568 
B) 3.55 
C) 56.8 
D) 17.6 
E) 0.0176

Question 8

The molarity of a solution prepared by diluting 43.72 mL of 5.005 M aqueous K2Cr2O7 to 500.mL is ________.

Accepted Answer

A) 0.129 
B) 0.109 
C) 0.438 
D) 0.0175 
E) 0.870 
A) 0.129 
B) 0.109 
C) 0.438 
D) 0.0175 
E) 0.870

Question 9

Which of the following would require the largest volume of 0.100 M sodium hydroxide solution for neutralization?

Accepted Answer

A) 10.0 mL of 0.0500 M phosphoric acid 
B) 20.0 mL of 0.0500 M nitric acid 
C) 5.0 mL of 0.0100 M sulfuric acid 
D) 15.0 mL of 0.0500 M hydrobromic acid 
E) 10.0 mL of 0.0500 M perchloric acid 
A) 10.0 mL of 0.0500 M phosphoric acid 
B) 20.0 mL of 0.0500 M nitric acid 
C) 5.0 mL of 0.0100 M sulfuric acid 
D) 15.0 mL of 0.0500 M hydrobromic acid 
E) 10.0 mL of 0.0500 M perchloric acid

Question 10

What volume (mL)of a concentrated solution of sodium hydroxide (6.00 M)must be diluted to   to make a   solution of sodium hydroxide?

Accepted Answer

A) 99.9 
B) 3600 
C) 287 
D) 0.104 
E) 0.0100 
A) 99.9 
B) 3600 
C) 287 
D) 0.104 
E) 0.0100

Question 11

The point in a titration at which the indicator changes is called the ________.

Accepted Answer

A) equivalence point 
B) indicator point 
C) standard point 
D) end point 
E) volumetric point 
A) equivalence point 
B) indicator point 
C) standard point 
D) end point 
E) volumetric point

Question 12

The process by which metal in the presence of air and water is converted into rust is known as ________.

Accepted Answer

A) activity 
B) reduction 
C) corrosion 
D) metathesis 
E) decomposition 
A) activity 
B) reduction 
C) corrosion 
D) metathesis 
E) decomposition

Question 13

Sodium does not occur in nature as Na (s)because ________.

Accepted Answer

A) it is easily reduced to Na- 
B) it is easily oxidized to Na+ 
C) it reacts with water with great difficulty 
D) it is easily replaced by silver in its ores 
E) it undergoes a disproportionation reaction to Na- and Na+ 
A) it is easily reduced to Na- 
B) it is easily oxidized to Na+ 
C) it reacts with water with great difficulty 
D) it is easily replaced by silver in its ores 
E) it undergoes a disproportionation reaction to Na- and Na+

Question 14

The spectator ions in the reaction between aqueous hydrobromic acid and aqueous ammonia are ________.

Accepted Answer

A) H+ and NH3 
B) H+, Br-, NH3, and NH4+ 
C) Br- only 
D) Br- and NH4+ 
E) H+, Br-, and NH4+ 
A) H+ and NH3 
B) H+, Br-, NH3, and NH4+ 
C) Br- only 
D) Br- and NH4+ 
E) H+, Br-, and NH4+

Question 15

When 0.344 mol of HCl is combined with enough water to make a 450.0 mL solution,the concentration of HCl is ________ M.

Accepted Answer

A) 7.64 × 10-4 
B) 0.155 
C) 1.31 
D) 0.764 
E) 0.344 
A) 7.64 × 10-4 
B) 0.155 
C) 1.31 
D) 0.764 
E) 0.344

Question 16

What is the concentration (M)of CH3OH in a solution prepared by dissolving 34.4 g of CH3OH in sufficient water to give exactly 230 mL of solution?

Accepted Answer

A) 11.9 
B) 0.00159 
C) 1.59 
D) 4.67 
E) 5.31 
A) 11.9 
B) 0.00159 
C) 1.59 
D) 4.67 
E) 5.31

Question 17

Which combination will produce a precipitate?

Accepted Answer

A) NH4OH (aq)and HCl (aq) 
B) AgNO3 (aq)and Ca(C2H3O2)2 (aq) 
C) NaOH (aq)and HCl (aq) 
D) NaCl (aq)and HC2H3O2 (aq) 
E) NaOH (aq)and Fe(NO3)2 (aq) 
A) NH4OH (aq)and HCl (aq) 
B) AgNO3 (aq)and Ca(C2H3O2)2 (aq) 
C) NaOH (aq)and HCl (aq) 
D) NaCl (aq)and HC2H3O2 (aq) 
E) NaOH (aq)and Fe(NO3)2 (aq)

Question 18

With which of the following will the Potassium ion form an insoluble salt?

Accepted Answer

A) Phosphate 
B) Sulfate 
C) Sulfide 
D) Iodide 
E) Potassium will form soluble salts with all choices. 
A) Phosphate 
B) Sulfate 
C) Sulfide 
D) Iodide 
E) Potassium will form soluble salts with all choices.

Question 19

Which of the following reactions is not spontaneous?

Accepted Answer

A) Cu (s)+ 2HCl (aq)→ CuCl2 (aq)+ H2 (g) 
B) Mg (s)+ 2HCl (aq)→ MgCl2 (aq)+ H2(g) 
C) 2Ni (s)+ H2SO4 (aq)→ Ni2SO4 (aq)+ H2 (g) 
D) 2Al (s)+ 6HBr (aq)→ 2AlBr3 (aq)+ 3H2 (g) 
E) Zn (s)+ 2HI (aq)→ ZnI2(aq)+ H2 (g) 
A) Cu (s)+ 2HCl (aq)→ CuCl2 (aq)+ H2 (g) 
B) Mg (s)+ 2HCl (aq)→ MgCl2 (aq)+ H2(g) 
C) 2Ni (s)+ H2SO4 (aq)→ Ni2SO4 (aq)+ H2 (g) 
D) 2Al (s)+ 6HBr (aq)→ 2AlBr3 (aq)+ 3H2 (g) 
E) Zn (s)+ 2HI (aq)→ ZnI2(aq)+ H2 (g)

Question 20

With which of the following will the ammonium ion form an insoluble salt?

Accepted Answer

A) chloride 
B) sulfate 
C) carbonate 
D) sulfate and carbonate 
E) none of the above 
A) chloride 
B) sulfate 
C) carbonate 
D) sulfate and carbonate 
E) none of the above

Exam 4: Reactions in Aqueous Solution

How many grams of NaOH (MW = 40.0)are there in 200.0 mL of a 0.175 M NaOH solution?

Based on the equations below,which metal is the most active? Pb(NO3)2 (aq)+ Ni (s)→ Ni(NO3)2 (aq)+ Pb (s) Pb(NO3)2 (aq)+ Ag (s)→ No reaction Cu(NO3)2 (aq)+ Ni (s)→ Ni(NO3)2 (aq)+ Cu (s)

How many milliliters of 1.500 M aqueous KI solution must be added to an aqueous solution containing 0.100 mol of Pb(NO3)2 to completely precipitate the lead?

The net ionic equation for the dissolution of zinc metal in aqueous hydrobromic acid is ________.

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

A 650 mL sodium bromide solution has a bromide ion concentration of 0.245 M.What is the mass (g)of sodium bromide in solution?

How many milliliters of a 14.2 M HCl solution is needed to prepare 0.715 L solution of HCl with a concentration of 0.350 M?

The molarity of a solution prepared by diluting 43.72 mL of 5.005 M aqueous K2Cr2O7 to 500.mL is ________.

Which of the following would require the largest volume of 0.100 M sodium hydroxide solution for neutralization?

What volume (mL)of a concentrated solution of sodium hydroxide (6.00 M)must be diluted to to make a solution of sodium hydroxide?

The point in a titration at which the indicator changes is called the ________.

The process by which metal in the presence of air and water is converted into rust is known as ________.

Sodium does not occur in nature as Na (s)because ________.

The spectator ions in the reaction between aqueous hydrobromic acid and aqueous ammonia are ________.

When 0.344 mol of HCl is combined with enough water to make a 450.0 mL solution,the concentration of HCl is ________ M.

What is the concentration (M)of CH3OH in a solution prepared by dissolving 34.4 g of CH3OH in sufficient water to give exactly 230 mL of solution?

Which combination will produce a precipitate?

With which of the following will the Potassium ion form an insoluble salt?

Which of the following reactions is not spontaneous?

With which of the following will the ammonium ion form an insoluble salt?

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

Based on the equations below,which metal is the most active? Pb(NO₃)₂ (aq)+ Ni (s)→ Ni(NO₃)₂ (aq)+ Pb (s) Pb(NO₃)₂ (aq)+ Ag (s)→ No reaction Cu(NO₃)₂ (aq)+ Ni (s)→ Ni(NO₃)₂ (aq)+ Cu (s)

How many milliliters of 1.500 M aqueous KI solution must be added to an aqueous solution containing 0.100 mol of Pb(NO₃)₂ to completely precipitate the lead?

The molarity of a solution prepared by diluting 43.72 mL of 5.005 M aqueous K₂Cr₂O₇to 500.mL is ________.

When 0.344 mol of HCl is combined with enough water to make a 450.0 mL solution,the concentration of HClis ________ M.

What is the concentration (M)of CH₃OH in a solution prepared by dissolving 34.4 g of CH₃OH in sufficient water to give exactly 230 mL of solution?