Question 1

Which one of the following solutions will have the greatest concentration of hydroxide ions?

Accepted Answer

A) 1.10 M rubidium hydroxide 
B) 0.368 M calcium hydroxide 
C) 0.368 M ammonium hydroxide 
D) 0.368 M potassium hydroxide 
E) 0.368 M sulfuric acid 
A) 1.10 M rubidium hydroxide 
B) 0.368 M calcium hydroxide 
C) 0.368 M ammonium hydroxide 
D) 0.368 M potassium hydroxide 
E) 0.368 M sulfuric acid

Question 2

What volume (L)of 0.250 M HNO3 is required to neutralize a solution prepared by dissolving 17.5 g of NaOH in 350 mL of water?

Accepted Answer

A) 1.25 
B) 0.11 
C) 1.75 
D) 0.070 
E) 1.75 ×   
A) 1.25 
B) 0.11 
C) 1.75 
D) 0.070 
E) 1.75 ×

Question 3

Which one of the following compounds is insoluble in water?

Accepted Answer

A) K2SO4 
B) Ca(C2H3O2)2 
C) MgC2O4 
D) ZnCl2 
E) Mn(NO3)2 
A) K2SO4 
B) Ca(C2H3O2)2 
C) MgC2O4 
D) ZnCl2 
E) Mn(NO3)2

Question 4

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

Question 5

Which one of the following is a triprotic acid?

Accepted Answer

A) nitric acid 
B) chloric acid 
C) phosphoric acid 
D) hydrofluoric acid 
E) sulfuric acid 
A) nitric acid 
B) chloric acid 
C) phosphoric acid 
D) hydrofluoric acid 
E) sulfuric acid

Question 6

The net ionic equation for the reaction between aqueous solutions of HF and KOH is ________.

Accepted Answer

A) HF + KOH → H2O + K+ + F- 
B) HF + OH- → H2O + F- 
C) HF + K+ + OH- → H2O + KF 
D) H+ + OH- → H2O 
E) H+ + F- + K+ + OH- → H2O + K+ + F- 
A) HF + KOH → H2O + K+ + F- 
B) HF + OH- → H2O + F- 
C) HF + K+ + OH- → H2O + KF 
D) H+ + OH- → H2O 
E) H+ + F- + K+ + OH- → H2O + K+ + F-

Question 7

In which reaction does the oxidation number of oxygen increase?

Accepted Answer

A) Ba(NO3)2 (aq)+ K2SO4 (aq)→ BaSO4 (s)+ 2KNO3 (aq) 
B) HCl (aq)+ NaOH (aq)→ NaCl (aq)+ H2O (l) 
C) MgO (s)+ H2O (l)→ Mg(OH)2 (s) 
D) 2SO2 (g)+ O2 (g)→ 2SO3 (g) 
E) 2H2O (l)→ 2H2 (g)+ O2 (g) 
A) Ba(NO3)2 (aq)+ K2SO4 (aq)→ BaSO4 (s)+ 2KNO3 (aq) 
B) HCl (aq)+ NaOH (aq)→ NaCl (aq)+ H2O (l) 
C) MgO (s)+ H2O (l)→ Mg(OH)2 (s) 
D) 2SO2 (g)+ O2 (g)→ 2SO3 (g) 
E) 2H2O (l)→ 2H2 (g)+ O2 (g)

Question 8

Calculate the concentration (M)of sodium ions in a solution made by diluting 50.0 mL of a 0.874 M solution of sodium sulfide to a total volume of 250.0 mL.

Accepted Answer

A) 0.175 
B) 4.37 
C) 0.525 
D) 0.350 
E) 0.874 
A) 0.175 
B) 4.37 
C) 0.525 
D) 0.350 
E) 0.874

Question 9

The molarity (M)of an aqueous solution containing 129 g of glucose (C6H12O6)in 200 mL of solution is ________.

Accepted Answer

A) 0.716 
B) 0.0036 
C) 3.58 
D) 0.645 
E) 645 
A) 0.716 
B) 0.0036 
C) 3.58 
D) 0.645 
E) 645

Question 10

What mass (g)of AgBr is formed when   of   AgNO3 is treated with an excess of aqueous hydrobromic acid?

Accepted Answer

A) 4.59 
B) 2.30 
C) 25.7 
D) 0.130 
E) 25,700 
A) 4.59 
B) 2.30 
C) 25.7 
D) 0.130 
E) 25,700

Question 11

Which of the following are strong acids?
HI
HNO3
HF
HBr

Accepted Answer

A) HF, HBr 
B) HI, HNO3, HF, HBr 
C) HI, HF, HBr 
D) HNO3, HF, HBr 
E) HI, HNO3, HBr 
A) HF, HBr 
B) HI, HNO3, HF, HBr 
C) HI, HF, HBr 
D) HNO3, HF, HBr 
E) HI, HNO3, HBr

Question 12

A 25.5 mL aliquot of HCl (aq)of unknown concentration was titrated with 0.113 M NaOH (aq).It took 51.2 mL of the base to reach the endpoint of the titration.The concentration (M)of the acid was ________.

Accepted Answer

A) 1.02 
B) 0.114 
C) 0.454 
D) 0.113 
E) 0.227 
A) 1.02 
B) 0.114 
C) 0.454 
D) 0.113 
E) 0.227

Question 13

When aqueous solutions of AgNO3 and KI are mixed,silver iodide precipitates.The balanced net ionic equation is ________.

Accepted Answer

A) Ag+ (aq)+   (aq)→ AgI (s) 
B) Ag+ (aq)+ NO3- (aq)→ AgNO3 (s) 
C) Ag+ (aq)+ NO3- (aq)→ AgNO3 (aq) 
D) AgNO3 (aq)+ KI (aq)→ AgI (s)+ KNO3 (aq) 
E) AgNO3 (aq)+ KI (aq)→ AgI (aq)+ KNO3 (s) 
A) Ag+ (aq)+   (aq)→ AgI (s) 
B) Ag+ (aq)+ NO3- (aq)→ AgNO3 (s) 
C) Ag+ (aq)+ NO3- (aq)→ AgNO3 (aq) 
D) AgNO3 (aq)+ KI (aq)→ AgI (s)+ KNO3 (aq) 
E) AgNO3 (aq)+ KI (aq)→ AgI (aq)+ KNO3 (s)

Question 14

What volume (mL)of 0.102 M NaOH is required to neutralize   of   HCl?

Accepted Answer

A) 74.3 
B) 3.94 
C) 0.773 
D) 0.0135 
E) 0.000773 
A) 74.3 
B) 3.94 
C) 0.773 
D) 0.0135 
E) 0.000773

Question 15

A 31.5 mL aliquot of H2SO4 (aq)of unknown concentration was titrated with 0.0134 M NaOH (aq).It took 23.9 mL of the base to reach the endpoint of the titration.The concentration (M)of the acid was ________.

Accepted Answer

A) 0.0102 
B) 0.00508 
C) 0.0204 
D) 0.102 
E) 0.227 
A) 0.0102 
B) 0.00508 
C) 0.0204 
D) 0.102 
E) 0.227

Question 16

If an unknown sample contains 39.04% sulfuric acid by mass,then a 0.9368 g of that sample would require ________ mL of 0.2389 M NaOH for neutralization.

Accepted Answer

A) 31.22 
B) 39.98 
C) 7.80 
D) 79.96 
E) 15.61 
A) 31.22 
B) 39.98 
C) 7.80 
D) 79.96 
E) 15.61

Question 17

What is the concentration (M)of potassium ions in 153 mL of a 1.25 M K3PO4 solution?

Accepted Answer

Question 18

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

Accepted Answer

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

Question 19

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

Question 20

Of the choices below,which would be the best for the lining of a tank intended for use in storage of hydrochloric acid?

Accepted Answer

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

Exam 4: Reactions in Aqueous Solution

Which one of the following solutions will have the greatest concentration of hydroxide ions?

What volume (L)of 0.250 M HNO3 is required to neutralize a solution prepared by dissolving 17.5 g of NaOH in 350 mL of water?

Which one of the following compounds is insoluble in water?

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

Which one of the following is a triprotic acid?

The net ionic equation for the reaction between aqueous solutions of HF and KOH is ________.

In which reaction does the oxidation number of oxygen increase?

Calculate the concentration (M)of sodium ions in a solution made by diluting 50.0 mL of a 0.874 M solution of sodium sulfide to a total volume of 250.0 mL.

The molarity (M)of an aqueous solution containing 129 g of glucose (C6H12O6)in 200 mL of solution is ________.

What mass (g)of AgBr is formed when of AgNO3 is treated with an excess of aqueous hydrobromic acid?

Which of the following are strong acids? HI HNO3 HF HBr

A 25.5 mL aliquot of HCl (aq)of unknown concentration was titrated with 0.113 M NaOH (aq).It took 51.2 mL of the base to reach the endpoint of the titration.The concentration (M)of the acid was ________.

When aqueous solutions of AgNO3 and KI are mixed,silver iodide precipitates.The balanced net ionic equation is ________.

What volume (mL)of 0.102 M NaOH is required to neutralize of HCl?

A 31.5 mL aliquot of H2SO4 (aq)of unknown concentration was titrated with 0.0134 M NaOH (aq).It took 23.9 mL of the base to reach the endpoint of the titration.The concentration (M)of the acid was ________.

If an unknown sample contains 39.04% sulfuric acid by mass,then a 0.9368 g of that sample would require ________ mL of 0.2389 M NaOH for neutralization.

What is the concentration (M)of potassium ions in 153 mL of a 1.25 M K3PO4 solution?

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

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.

Of the choices below,which would be the best for the lining of a tank intended for use in storage of hydrochloric acid?

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

What volume (L)of 0.250 M HNO₃is required to neutralize a solution prepared by dissolving 17.5 g of NaOH in 350 mL of water?

The molarity (M)of an aqueous solution containing 129 g of glucose (C₆H₁₂O₆)in 200 mL of solution is ________.

What mass (g)of AgBr is formed when of AgNO₃ is treated with an excess of aqueous hydrobromic acid?

Which of the following are strong acids? HI HNO₃ HF HBr

When aqueous solutions of AgNO₃ and KI are mixed,silver iodide precipitates.The balanced net ionic equation is ________.

A 31.5 mL aliquot of H₂SO₄ (aq)of unknown concentration was titrated with 0.0134 M NaOH (aq).It took 23.9 mL of the base to reach the endpoint of the titration.The concentration (M)of the acid was ________.

What is the concentration (M)of potassium ions in 153 mL of a 1.25 M K₃PO₄ solution?

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