Question 1

What volume (mL)of 0.102 M NaOH is required to neutralize 17.1 mL of 0.443 M 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 2

Which combination will produce a precipitate?

Accepted Answer

A) Pb(NO3)2 (aq)and HCl (aq) 
B) Cu(NO3)2 (aq)and KC2H3O2 (aq) 
C) KOH (aq)and HNO3 (aq) 
D) AgC2H3O2 (aq)and HC2H3O2 (aq) 
E) NaOH (aq)and Sr(NO3)2 (aq) 
A) Pb(NO3)2 (aq)and HCl (aq) 
B) Cu(NO3)2 (aq)and KC2H3O2 (aq) 
C) KOH (aq)and HNO3 (aq) 
D) AgC2H3O2 (aq)and HC2H3O2 (aq) 
E) NaOH (aq)and Sr(NO3)2 (aq)

Question 3

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 4

Pure acetic acid (HC2H3O2)is a liquid and is known as glacial acetic acid. Calculate the molarity of a solution prepared by dissolving 20.00 mL of glacial acetic acid at 25 °C in sufficient water to give 500.0 mL of solution. The density of glacial acetic acid at 25 °C is 1.05 g/mL.

Accepted Answer

A) 2.52 × 103 
B) 42.0 
C) 0.0420 
D) 0.699 
E) 6.99 × 10-4 
A) 2.52 × 103 
B) 42.0 
C) 0.0420 
D) 0.699 
E) 6.99 × 10-4

Question 5

There are ________ mol of bromide ions in 0.700 L of a 0.400 M solution of AlBr3.

Accepted Answer

Question 6

Of the following elements, ________ is the least easily oxidized. zinc
Iron
Hydrogen
Aluminum
Lead

Accepted Answer

A) zinc 
B) iron 
C) hydrogen 
D) aluminum 
E) lead 
A) zinc 
B) iron 
C) hydrogen 
D) aluminum 
E) lead

Question 7

When 0.500 mol of HC2H3O2 is combined with enough water to make a 300.0 mL solution, the concentration of HC2H3O2 is ________ M.

Accepted Answer

A) 3.33 
B) 1.67 
C) 0.835 
D) 0.00167 
E) 0.150 
A) 3.33 
B) 1.67 
C) 0.835 
D) 0.00167 
E) 0.150

Question 8

What mass (g)of potassium chloride is contained in 430.0 mL of a potassium chloride solution that has a chloride ion concentration of 0.193 M?

Accepted Answer

A) 0.0643 
B) 0.0830 
C) 12.37 
D) 0.386 
E) 6.19 
A) 0.0643 
B) 0.0830 
C) 12.37 
D) 0.386 
E) 6.19

Question 9

What mass (g)of CaF2 is formed when 30.4 mL of 0.438 M NaF is treated with an excess of aqueous calcium nitrate?

Accepted Answer

A) 0.520 
B) 1.04 
C) 1040 
D) 0.171 
E) 5420 
A) 0.520 
B) 1.04 
C) 1040 
D) 0.171 
E) 5420

Question 10

Which one of the following is a correct expression for molarity?

Accepted Answer

A) mol solute/L solvent 
B) mol solute/mL solvent 
C) mmol solute/mL solution 
D) mol solute/kg solvent 
E) μmol solute/L solution 
A) mol solute/L solvent 
B) mol solute/mL solvent 
C) mmol solute/mL solution 
D) mol solute/kg solvent 
E) μmol solute/L solution

Question 11

Oxalic acid is a diprotic acid. If a solid material contains 53.66 percent of oxalic acid (H2C2O4), by mass, then a 0.6543-g sample of that solid will require ________ mL of 0.3483 M NaOH for neutralization.

Accepted Answer

A) 11.19 
B) 97.78 
C) 28.59 
D) 1.119 
E) 22.39 
A) 11.19 
B) 97.78 
C) 28.59 
D) 1.119 
E) 22.39

Question 12

The concentration of sulfate ions in a 0.233 M solution of sulfuric acid is ________.

Accepted Answer

A) 0.699 M 
B) 0.233 M 
C) 0.466 M 
D) 0.0777 M 
E) 0.155 M 
A) 0.699 M 
B) 0.233 M 
C) 0.466 M 
D) 0.0777 M 
E) 0.155 M

Question 13

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 14

Which combination will produce a precipitate?

Accepted Answer

A) NaC2H3O2 (aq)and HCl (aq) 
B) NaOH (aq)and HCl (aq) 
C) AgNO3(aq)and Ca(C2H3O2)2 (aq) 
D) KOH (aq)and Mg(NO3)2 (aq) 
E) NaF (aq)and HCl (aq) 
A) NaC2H3O2 (aq)and HCl (aq) 
B) NaOH (aq)and HCl (aq) 
C) AgNO3(aq)and Ca(C2H3O2)2 (aq) 
D) KOH (aq)and Mg(NO3)2 (aq) 
E) NaF (aq)and HCl (aq)

Question 15

What are the respective concentrations (M)of Cu+2 and Cl- afforded by dissolving 0.871 mol CuCl2 in water and diluting to 259 mL?

Accepted Answer

A) 3.36 and 6.73 
B) 0.00336 and 3.36 
C) 0.00336 and 0.00336 
D) 3.36 and 3.36 
E) 0.297 and 0.113 
A) 3.36 and 6.73 
B) 0.00336 and 3.36 
C) 0.00336 and 0.00336 
D) 3.36 and 3.36 
E) 0.297 and 0.113

Question 16

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

Accepted Answer

A) Mg3(PO4)2 
B) Na2S 
C) (NH4)2CO3 
D) Ca(OH)2 
E) Ba(C2H3O2)2 
A) Mg3(PO4)2 
B) Na2S 
C) (NH4)2CO3 
D) Ca(OH)2 
E) Ba(C2H3O2)2

Question 17

Which of the following reactions will not occur as written?

Accepted Answer

A) Zn (s) + Pb(NO3)2 (aq) → Pb (s) + Zn(NO3)2 (aq) 
B) Mg (s) + Ca(OH)2 (aq) → Ca (s) + Mg(OH)2 (aq) 
C) Sn (s) + 2AgNO3 (aq) → 2Ag (s) + Sn(NO3)2 (aq) 
D) Co (s) + 2AgCl (aq) → 2Ag (s) + CoCl2 (aq) 
E) Co (s) + 2HI (aq) → H2 (g) + CoI2 (aq) 
A) Zn (s) + Pb(NO3)2 (aq) → Pb (s) + Zn(NO3)2 (aq) 
B) Mg (s) + Ca(OH)2 (aq) → Ca (s) + Mg(OH)2 (aq) 
C) Sn (s) + 2AgNO3 (aq) → 2Ag (s) + Sn(NO3)2 (aq) 
D) Co (s) + 2AgCl (aq) → 2Ag (s) + CoCl2 (aq) 
E) Co (s) + 2HI (aq) → H2 (g) + CoI2 (aq)

Question 18

How many grams of CH3OH must be added to water to prepare 150 mL of a solution that is 2.0 M CH3OH?

Accepted Answer

A) 0.0096 
B) 430 
C) 2.4 
D) 9.6 
E) 4.3 
A) 0.0096 
B) 430 
C) 2.4 
D) 9.6 
E) 4.3

Question 19

What is the concentration (M)of a NaCl solution prepared by dissolving 3.8 g of NaCl in sufficient water to give 245 mL of solution?

Accepted Answer

The answer of What is the concentration (M)of a NaCl...

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: Aqueous Reactions and Solution Stoichiometry

What volume (mL)of 0.102 M NaOH is required to neutralize 17.1 mL of 0.443 M HCl?

Which combination will produce a precipitate?

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

Pure acetic acid (HC2H3O2)is a liquid and is known as glacial acetic acid. Calculate the molarity of a solution prepared by dissolving 20.00 mL of glacial acetic acid at 25 °C in sufficient water to give 500.0 mL of solution. The density of glacial acetic acid at 25 °C is 1.05 g/mL.

There are ________ mol of bromide ions in 0.700 L of a 0.400 M solution of AlBr3.

Of the following elements, ________ is the least easily oxidized. zinc Iron Hydrogen Aluminum Lead

When 0.500 mol of HC2H3O2 is combined with enough water to make a 300.0 mL solution, the concentration of HC2H3O2 is ________ M.

What mass (g)of potassium chloride is contained in 430.0 mL of a potassium chloride solution that has a chloride ion concentration of 0.193 M?

What mass (g)of CaF2 is formed when 30.4 mL of 0.438 M NaF is treated with an excess of aqueous calcium nitrate?

Which one of the following is a correct expression for molarity?

Oxalic acid is a diprotic acid. If a solid material contains 53.66 percent of oxalic acid (H2C2O4), by mass, then a 0.6543-g sample of that solid will require ________ mL of 0.3483 M NaOH for neutralization.

The concentration of sulfate ions in a 0.233 M solution of sulfuric acid is ________.

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

Which combination will produce a precipitate?

What are the respective concentrations (M)of Cu+2 and Cl- afforded by dissolving 0.871 mol CuCl2 in water and diluting to 259 mL?

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

Which of the following reactions will not occur as written?

How many grams of CH3OH must be added to water to prepare 150 mL of a solution that is 2.0 M CH3OH?

What is the concentration (M)of a NaCl solution prepared by dissolving 3.8 g of NaCl in sufficient water to give 245 mL of solution?

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 and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

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

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Pure acetic acid (HC₂H₃O₂)is a liquid and is known as glacial acetic acid. Calculate the molarity of a solution prepared by dissolving 20.00 mL of glacial acetic acid at 25 °C in sufficient water to give 500.0 mL of solution. The density of glacial acetic acid at 25 °C is 1.05 g/mL.

There are ________ mol of bromide ions in 0.700 L of a 0.400 M solution of AlBr₃.

When 0.500 mol of HC₂H₃O₂ is combined with enough water to make a 300.0 mL solution, the concentration of HC₂H₃O₂is ________ M.

What mass (g)of CaF₂ is formed when 30.4 mL of 0.438 M NaF is treated with an excess of aqueous calcium nitrate?

Oxalic acid is a diprotic acid. If a solid material contains 53.66 percent of oxalic acid (H₂C₂O₄), by mass, then a 0.6543-g sample of that solid will require ________ mL of 0.3483 M NaOH for neutralization.

What are the respective concentrations (M)of Cu⁺² and Cl^- afforded by dissolving 0.871 mol CuCl₂ in water and diluting to 259 mL?

How many grams of CH₃OH must be added to water to prepare 150 mL of a solution that is 2.0 M CH₃OH?