Question 1

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

Accepted Answer

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

Question 2

The concentration of iodide ions in a 0.193 M solution of barium iodide is .

Accepted Answer

A)  0.0965 M 
B)  0.0643 M 
C)  0.386 M 
D)  0.579 M 
E)  0.193 M 
A)  0.0965 M 
B)  0.0643 M 
C)  0.386 M 
D)  0.579 M 
E)  0.193 M

Question 3

What is the concentration (M) of a NaCl solution prepared by dissolving 9.3 g of NaCl in sufficient water to give 350 mL of solution?

Accepted Answer

A)  27 
B)  2.7 × 10- 2  
C)  18 
D)  0.16 
E)  0.45 
A)  27 
B)  2.7 × 10- 2  
C)  18 
D)  0.16 
E)  0.45

Question 4

How many grams of NaOH (MW = 40.0) are there in 500.0 mL of a 0.175 M NaOH solution?

Accepted Answer

A)  3.50 × 103 
B)  14.0 
C)  2.19 × 10- 3 
D)  114 
E)  3.50 
A)  3.50 × 103 
B)  14.0 
C)  2.19 × 10- 3 
D)  114 
E)  3.50

Question 5

A 13.8 mL aliquot of 0.176 M H3PO4 (aq) is to be titrated with 0.110 M NaOH (aq). What volume (mL) of base will it take to reach the equivalence point?

Accepted Answer

A)  20.9 
B)  7.29 
C)  199 
D)  66.2 
E)  22.1 
A)  20.9 
B)  7.29 
C)  199 
D)  66.2 
E)  22.1

Question 6

How many grams of sodium chloride are there in 550 mL of a 1.90 M aqueous solution of sodium chloride?

Accepted Answer

A)  6.11 × 104  
B)  1.05 
C)  61.1 
D)  122 
E)  30.5 
A)  6.11 × 104  
B)  1.05 
C)  61.1 
D)  122 
E)  30.5

Question 7

What volume (mL) of 7.48 × 10- 2 M phosphoric acid can be neutralized with 115 mL of 0.244 M sodium hydroxide?

Accepted Answer

A)  375 
B)  750 
C)  75.0 
D)  125 
E)  188 
A)  375 
B)  750 
C)  75.0 
D)  125 
E)  188

Question 8

The molarity of a solution prepared by diluting 43.72 mL of 1.005 M aqueous K2Cr2O7 to 500 mL is

Accepted Answer

A)  87.9 
B)  0.0218 
C)  0.0115 
D)  0.0879 
E)  0.870 
A)  87.9 
B)  0.0218 
C)  0.0115 
D)  0.0879 
E)  0.870

Question 9

What volume (mL) of 0.135 M NaOH is required to neutralize 13.7 mL of 0.129 M HCl?

Accepted Answer

A)  14.3 
B)  0.24 
C)  0.076 
D)  6.55 
E)  13.1 
A)  14.3 
B)  0.24 
C)  0.076 
D)  6.55 
E)  13.1

Question 10

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

Accepted Answer

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

Question 11

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

Accepted Answer

A)  0.0044 
B)  57.2 
C)  0.438 
D)  0.870 
E)  0.0879 
A)  0.0044 
B)  57.2 
C)  0.438 
D)  0.870 
E)  0.0879

Question 12

A weak electrolyte exists predominantly as _ in solution.

Accepted Answer

A)  atoms 
B)  molecules 
C)  ions 
D)  an isotope 
E)  electrons 
A)  atoms 
B)  molecules 
C)  ions 
D)  an isotope 
E)  electrons

Question 13

The compound NH4Cl is a weak acid.

Accepted Answer

A) True 
 B)False

Question 14

The spectator ions in the reaction between aqueous hydrochloric acid and aqueous ammonia are

Accepted Answer

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

Question 15

An aqueous ethanol solution (400 mL) was diluted to 4.00 L, giving a concentration of 0.0400 M. The concentration of the original solution was M.

Accepted Answer

A)  0.400 
B)  2.00 
C)  0.200 
D)  4.00 
E)  1.60 
A)  0.400 
B)  2.00 
C)  0.200 
D)  4.00 
E)  1.60

Question 16

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

Question 17

The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is

Accepted Answer

A)  HNO3 (aq) + Sr(OH)2 (aq) - Sr(NO3)2 (aq) + H2 (g) 
B)  2HNO3 (aq) + Sr(OH)2 (aq) - 2H2O (l) + Sr(NO3)2 (aq) 
C)  HNO3 (aq) + SrOH (aq) -H2O (l) + SrNO3 (aq) 
D)  2HNO3 (aq) + Sr(OH)2 (aq) - Sr(NO3)2 (aq) + 2H2 (g) 
E)  HNO3 (aq) + Sr(OH)2 (aq) -H2O (l) + Sr(NO3)2 (aq) 
A)  HNO3 (aq) + Sr(OH)2 (aq) - Sr(NO3)2 (aq) + H2 (g) 
B)  2HNO3 (aq) + Sr(OH)2 (aq) - 2H2O (l) + Sr(NO3)2 (aq) 
C)  HNO3 (aq) + SrOH (aq) -H2O (l) + SrNO3 (aq) 
D)  2HNO3 (aq) + Sr(OH)2 (aq) - Sr(NO3)2 (aq) + 2H2 (g) 
E)  HNO3 (aq) + Sr(OH)2 (aq) -H2O (l) + Sr(NO3)2 (aq)

Question 18

Which solution contains the largest number of moles of chloride ions?

Accepted Answer

A)  4.00 mL of 1.000M NaCl 
B)  25.00 mL of 0.400M KCl 
C)  10.0 mL of 0.500M BaCl2 
D)  30.00 mL of 0.100M CaCl2 
E)  7.50 mL of 0.500M FeCl3 
A)  4.00 mL of 1.000M NaCl 
B)  25.00 mL of 0.400M KCl 
C)  10.0 mL of 0.500M BaCl2 
D)  30.00 mL of 0.100M CaCl2 
E)  7.50 mL of 0.500M FeCl3

Question 19

What mass (g) of barium iodide is contained in 250 mL of a barium iodide solution that has an iodide ion concentration of 0.193 M?

Accepted Answer

A)  9.44 
B)  18.9 
C)  0.024 
D)  37.7 
E)  0.048 
A)  9.44 
B)  18.9 
C)  0.024 
D)  37.7 
E)  0.048

Question 20

What is the molarity of a NaOH solution if 28.2 mL of a 0.355 M H2SO4 solution is required to neutralize a 25.0- mL sample of the NaOH solution?

Accepted Answer

A)  0.400 
B)  0.315 
C)  125 
D)  0.629 
E)  0.801 
A)  0.400 
B)  0.315 
C)  125 
D)  0.629 
E)  0.801

Exam 4: Aqueous Reactions and Solution Stoichiometry

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

The concentration of iodide ions in a 0.193 M solution of barium iodide is .

What is the concentration (M) of a NaCl solution prepared by dissolving 9.3 g of NaCl in sufficient water to give 350 mL of solution?

How many grams of NaOH (MW = 40.0) are there in 500.0 mL of a 0.175 M NaOH solution?

A 13.8 mL aliquot of 0.176 M H3PO4 (aq) is to be titrated with 0.110 M NaOH (aq). What volume (mL) of base will it take to reach the equivalence point?

How many grams of sodium chloride are there in 550 mL of a 1.90 M aqueous solution of sodium chloride?

What volume (mL) of 7.48 × 10- 2 M phosphoric acid can be neutralized with 115 mL of 0.244 M sodium hydroxide?

The molarity of a solution prepared by diluting 43.72 mL of 1.005 M aqueous K2Cr2O7 to 500 mL is

What volume (mL) of 0.135 M NaOH is required to neutralize 13.7 mL of 0.129 M HCl?

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

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

A weak electrolyte exists predominantly as _ in solution.

The compound NH4Cl is a weak acid.

The spectator ions in the reaction between aqueous hydrochloric acid and aqueous ammonia are

An aqueous ethanol solution (400 mL) was diluted to 4.00 L, giving a concentration of 0.0400 M. The concentration of the original solution was M.

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 balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is

Which solution contains the largest number of moles of chloride ions?

What mass (g) of barium iodide is contained in 250 mL of a barium iodide solution that has an iodide ion concentration of 0.193 M?

What is the molarity of a NaOH solution if 28.2 mL of a 0.355 M H2SO4 solution is required to neutralize a 25.0- mL sample of the NaOH solution?

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Gases

Intermolecular Forces, Liquids, and Solids

Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Chemistry of Coordination Compounds

The Chemistry of Life: Organic and Biological Chemistry

Filters

A 13.8 mL aliquot of 0.176 M H₃PO₄(aq) is to be titrated with 0.110 M NaOH (aq). What volume (mL) of base will it take to reach the equivalence point?

What volume (mL) of 7.48 × 10^-²M phosphoric acid can be neutralized with 115 mL of 0.244 M sodium hydroxide?

The molarity of a solution prepared by diluting 43.72 mL of 1.005 M aqueous K₂Cr₂O₇to 500 mL is

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

The compound NH₄Cl is a weak acid.

What is the molarity of a NaOH solution if 28.2 mL of a 0.355 M H₂SO₄solution is required to neutralize a 25.0- mL sample of the NaOH solution?