Question 1

Of the following elements, is the only one that cannot be found in nature in its elemental form.

Accepted Answer

A)  Ag 
B)  Cu 
C)  Na 
D)  Hg 
E)  Au 
A)  Ag 
B)  Cu 
C)  Na 
D)  Hg 
E)  Au

Question 2

Which one of the following is not true concerning 2.00 L of 0.100 M solution of Ca3(PO4)2?

Accepted Answer

A)  This solution contains 0.800 mol of oxygen atoms. 
B)  This solution contains 6.67 × 10- 2 mol of Ca2+. 
C)  There are 6.02 × 1022 phosphorus atoms in 500.0 mL of this solution. 
D)  This solution contains 0.200 mol of Ca3(PO4)2. 
E)  1.00 L of this solution is required to furnish 0.300 mol of Ca2+ ions. 
A)  This solution contains 0.800 mol of oxygen atoms. 
B)  This solution contains 6.67 × 10- 2 mol of Ca2+. 
C)  There are 6.02 × 1022 phosphorus atoms in 500.0 mL of this solution. 
D)  This solution contains 0.200 mol of Ca3(PO4)2. 
E)  1.00 L of this solution is required to furnish 0.300 mol of Ca2+ ions.

Question 3

Which combination will produce a precipitate?

Accepted Answer

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

Question 4

What mass (g) of CaF2 is formed when 47.8 mL of 0.334 M NaF is treated with an excess of aqueous calcium nitrate?

Accepted Answer

A)  2.49 
B)  0.472 
C)  1.25 
D)  0.623 
E)  0.943 
A)  2.49 
B)  0.472 
C)  1.25 
D)  0.623 
E)  0.943

Question 5

How many moles of Co2+ are present in 0.200 L of a 0.400 M solution of CoI2?

Accepted Answer

A)  2.00 
B)  0.500 
C)  0.160 
D)  0.0400 
E)  0.0800 
A)  2.00 
B)  0.500 
C)  0.160 
D)  0.0400 
E)  0.0800

Question 6

A solution is prepared by mixing 50.0 mL of 0.100 M HCl and 10.0 mL of 0.200 M NaCl. What is the molarity of chloride ion in this solution?

Accepted Answer

A)  8.57 
B)  0.183 
C)  3.50 
D)  0.0500 
E)  0.117 
A)  8.57 
B)  0.183 
C)  3.50 
D)  0.0500 
E)  0.117

Question 7

Combining aqueous solutions of BaI2 and Na2SO4 affords a precipitate of BaSO4. Which ion(s) is/are spectator ions in the reaction?

Accepted Answer

A)  SO42- and I- 
B)  Ba2+ only 
C)  Na+ and I- 
D)  Na+ only 
E)  Ba2+ and SO42- 
A)  SO42- and I- 
B)  Ba2+ only 
C)  Na+ and I- 
D)  Na+ only 
E)  Ba2+ and SO42-

Question 8

Which compound has the atom with the highest oxidation number?

Accepted Answer

A)  Al(NO2)3  
B)  MgSO3  
C)  CaS 
D)  Na3N 
E)  NH4Cl 
A)  Al(NO2)3  
B)  MgSO3  
C)  CaS 
D)  Na3N 
E)  NH4Cl

Question 9

Oxidation is the _ and reduction is the .

Accepted Answer

A)  gain of electrons, loss of electrons 
B)  gain of oxygen, loss of electrons 
C)  loss of oxygen, gain of electrons 
D)  gain of oxygen, loss of mass 
E)  loss of electrons, gain of electrons 
A)  gain of electrons, loss of electrons 
B)  gain of oxygen, loss of electrons 
C)  loss of oxygen, gain of electrons 
D)  gain of oxygen, loss of mass 
E)  loss of electrons, gain of electrons

Question 10

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)  0.227 
C)  0.0204 
D)  0.0051 
E)  0.102 
A)  0.0102 
B)  0.227 
C)  0.0204 
D)  0.0051 
E)  0.102

Question 11

The net ionic equation for formation of an aqueous solution of NiI2 accompanied by evolution of C O2 gas via mixing solid NiCO3 and aqueous hydriodic acid is .

Accepted Answer

A)  NiCO3 (s) + 2HI (aq) -H2O (l) + CO2 (g) + Ni2+ (aq) + 2I-  (aq) 
B)  NiCO3 (s) + 2HI (aq) - 2H2O (l) + CO2 (g) + NiI2 (aq) 
C)  NiCO3 (s) + 2H+ (aq) -H2O (l) + CO2 (g) + Ni2+ (aq) 
D)  NiCO3 (s) + I- (aq) - 2H2O (l) + CO2 (g) + Ni2+ (aq) + HI (aq) 
E)  2NiCO3 (s) + HI (aq) - 2H2O (l) + CO2 (g) + 2Ni2+ (aq) 
A)  NiCO3 (s) + 2HI (aq) -H2O (l) + CO2 (g) + Ni2+ (aq) + 2I-  (aq) 
B)  NiCO3 (s) + 2HI (aq) - 2H2O (l) + CO2 (g) + NiI2 (aq) 
C)  NiCO3 (s) + 2H+ (aq) -H2O (l) + CO2 (g) + Ni2+ (aq) 
D)  NiCO3 (s) + I- (aq) - 2H2O (l) + CO2 (g) + Ni2+ (aq) + HI (aq) 
E)  2NiCO3 (s) + HI (aq) - 2H2O (l) + CO2 (g) + 2Ni2+ (aq)

Question 12

In which reaction does the oxidation number of hydrogen change?

Accepted Answer

A)  CaO (s) + H2O (l) -Ca(OH)2 (s) 
B)  HCl (aq) + NaOH (aq) -NaCl (aq) + H2O (l) 
C)  2 Na (s) + 2 H2O (l) -2 NaOH (aq) + H2 (g) 
D)  2 HClO4 (aq) + CaCO3 (s) -Ca(ClO4)2 (aq) + H2O (l) + CO2 (g) 
E)  SO2(g) + H2O (l) -H2SO3 (aq) 
A)  CaO (s) + H2O (l) -Ca(OH)2 (s) 
B)  HCl (aq) + NaOH (aq) -NaCl (aq) + H2O (l) 
C)  2 Na (s) + 2 H2O (l) -2 NaOH (aq) + H2 (g) 
D)  2 HClO4 (aq) + CaCO3 (s) -Ca(ClO4)2 (aq) + H2O (l) + CO2 (g) 
E)  SO2(g) + H2O (l) -H2SO3 (aq)

Question 13

A 0.200 M K2SO4 solution is produced by .

Accepted Answer

A)  dissolving 20.2 g of K2SO4 in water and diluting to 250.0 mL, then diluting 25.0 mL of this solution to a total volume of 500.0 mL 
B)  diluting 20.0 mL of 5.00 M K2SO4 solution to 500.0 mL 
C)  dissolving 43.6 g of K2SO4 in water and diluting to a total volume of 250.0 mL 
D)  dilution of 1.00 mL of 250 M K2SO3 to 1.00 L 
E)  dilution of 250.0 mL of 1.00 M K2SO4 to 1.00 L 
A)  dissolving 20.2 g of K2SO4 in water and diluting to 250.0 mL, then diluting 25.0 mL of this solution to a total volume of 500.0 mL 
B)  diluting 20.0 mL of 5.00 M K2SO4 solution to 500.0 mL 
C)  dissolving 43.6 g of K2SO4 in water and diluting to a total volume of 250.0 mL 
D)  dilution of 1.00 mL of 250 M K2SO3 to 1.00 L 
E)  dilution of 250.0 mL of 1.00 M K2SO4 to 1.00 L

Question 14

You are given two clear solutions of the same unknown monoprotic acid, but with different concentrations. Which statement is true?

Accepted Answer

A)  A smaller volume of the less concentrated solution contains the same number of moles of the acid compared to the more concentrated solution. 
B)  The product of concentration and volume of the less concentrated solution equals the product of concentration and volume of the more concentrated solution. 
C)  It would take more base solution (per milliliter of the unknown solution) to neutralize the more concentrated solution. 
D)  There is no chemical method designed to tell the two solutions apart. 
E)  If the same volume of each sample was taken, then more base solution would be required to neutralize the one with lower concentration. 
A)  A smaller volume of the less concentrated solution contains the same number of moles of the acid compared to the more concentrated solution. 
B)  The product of concentration and volume of the less concentrated solution equals the product of concentration and volume of the more concentrated solution. 
C)  It would take more base solution (per milliliter of the unknown solution) to neutralize the more concentrated solution. 
D)  There is no chemical method designed to tell the two solutions apart. 
E)  If the same volume of each sample was taken, then more base solution would be required to neutralize the one with lower concentration.

Question 15

What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 200. mL to make a 1.50 M solution of sodium hydroxide?

Accepted Answer

A)  0.800 
B)  800 
C)  45 
D)  50.0 
E)  0.05 
A)  0.800 
B)  800 
C)  45 
D)  50.0 
E)  0.05

Question 16

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

Accepted Answer

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

Question 17

A stock solution of HNO3 is prepared and found to contain 13.5 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)  1.48 
B)  0.270 
C)  675 
D)  0.675 
E)  270 
A)  1.48 
B)  0.270 
C)  675 
D)  0.675 
E)  270

Question 18

Which of the following is soluble in water at 25°C?

Accepted Answer

A)  Fe(NO3)2  
B)  FeS 
C)  Fe(OH)2  
D)  Fe3(PO4)2  
E)  FeCO3 
A)  Fe(NO3)2  
B)  FeS 
C)  Fe(OH)2  
D)  Fe3(PO4)2  
E)  FeCO3

Question 19

Zinc is more active than cobalt and iron but less active than aluminum. Cobalt is more active than nickel but less active than iron. Which of the following correctly lists the elements in order of increasing activity?

Accepted Answer

A)  Ni < Co < Fe < Zn < Al 
B)  Zn < Al < Co < Ni < Fe 
C)  Ni < Fe < Co < Zn < Al 
D)  Fe < Ni < Co < Al < Zn 
E)  Co < Ni < Fe < Zn < Al 
A)  Ni < Co < Fe < Zn < Al 
B)  Zn < Al < Co < Ni < Fe 
C)  Ni < Fe < Co < Zn < Al 
D)  Fe < Ni < Co < Al < Zn 
E)  Co < Ni < Fe < Zn < Al

Question 20

In which reaction does the oxidation number of oxygen increase?

Accepted Answer

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

Exam 4: Aqueous Reactions and Solution Stoichiometry

Of the following elements, is the only one that cannot be found in nature in its elemental form.

Which one of the following is not true concerning 2.00 L of 0.100 M solution of Ca3(PO4)2?

Which combination will produce a precipitate?

What mass (g) of CaF2 is formed when 47.8 mL of 0.334 M NaF is treated with an excess of aqueous calcium nitrate?

How many moles of Co2+ are present in 0.200 L of a 0.400 M solution of CoI2?

A solution is prepared by mixing 50.0 mL of 0.100 M HCl and 10.0 mL of 0.200 M NaCl. What is the molarity of chloride ion in this solution?

Combining aqueous solutions of BaI2 and Na2SO4 affords a precipitate of BaSO4. Which ion(s) is/are spectator ions in the reaction?

Which compound has the atom with the highest oxidation number?

Oxidation is the _ and reduction is the .

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 .

The net ionic equation for formation of an aqueous solution of NiI2 accompanied by evolution of C O2 gas via mixing solid NiCO3 and aqueous hydriodic acid is .

In which reaction does the oxidation number of hydrogen change?

A 0.200 M K2SO4 solution is produced by .

You are given two clear solutions of the same unknown monoprotic acid, but with different concentrations. Which statement is true?

What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 200. mL to make a 1.50 M solution of sodium hydroxide?

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

A stock solution of HNO3 is prepared and found to contain 13.5 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 the following is soluble in water at 25°C?

Zinc is more active than cobalt and iron but less active than aluminum. Cobalt is more active than nickel but less active than iron. Which of the following correctly lists the elements in order of increasing activity?

In which reaction does the oxidation number of oxygen increase?

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

Which one of the following is not true concerning 2.00 L of 0.100 M solution of Ca₃(PO₄)₂?

What mass (g) of CaF₂is formed when 47.8 mL of 0.334 M NaF is treated with an excess of aqueous calcium nitrate?

How many moles of Co²⁺are present in 0.200 L of a 0.400 M solution of CoI₂?

Combining aqueous solutions of BaI₂and Na₂SO₄affords a precipitate of BaSO₄. Which ion(s) is/are spectator ions in the reaction?

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 .

The net ionic equation for formation of an aqueous solution of NiI₂accompanied by evolution of C O₂gas via mixing solid NiCO₃and aqueous hydriodic acid is .

A 0.200 M K₂SO₄solution is produced by .

A stock solution of HNO₃is prepared and found to contain 13.5 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.