Question 1

The molarity (M)of an aqueous solution containing 52.5 g of sucrose (C12H22O11)in 35.5 mL of solution is __________.

Accepted Answer

A) 5.46 
B) 1.48 
C) 0.104 
D) 4.32 
E) 1.85 
A) 5.46 
B) 1.48 
C) 0.104 
D) 4.32 
E) 1.85

Question 2

The balanced net ionic equation for precipitation of CaCO3 when aqueous solutions of Na2CO3 and CaCl2 are mixed is __________.

Accepted Answer

A) 2Na+ (aq)+ CO32-  (aq)→ Na2CO3 (aq) 
B) 2Na+ (aq)+ 2Cl- (aq)→ 2NaCl (aq) 
C) Na+ (aq)+ Cl- (aq)→ NaCl (aq) 
D) Ca2+ (aq)+ CO32- (aq)→ CaCO3 (s) 
E) Na2CO3 (aq)+ CaCl2 (aq)→ 2NaCl (aq)+ CaCO3 (s) 
A) 2Na+ (aq)+ CO32-  (aq)→ Na2CO3 (aq) 
B) 2Na+ (aq)+ 2Cl- (aq)→ 2NaCl (aq) 
C) Na+ (aq)+ Cl- (aq)→ NaCl (aq) 
D) Ca2+ (aq)+ CO32- (aq)→ CaCO3 (s) 
E) Na2CO3 (aq)+ CaCl2 (aq)→ 2NaCl (aq)+ CaCO3 (s)

Question 3

The concentration of species in 500 mL of a 2.104 M solution of sodium sulfate is __________ M sodium ion and __________ M sulfate ion.

Accepted Answer

A) 2.104, 1.052 
B) 2.104, 2.104 
C) 2.104, 4.208 
D) 1.052, 1.052 
E) 4.208, 2.104 
A) 2.104, 1.052 
B) 2.104, 2.104 
C) 2.104, 4.208 
D) 1.052, 1.052 
E) 4.208, 2.104

Question 4

When H2SO4 is neutralized by NaOH in aqueous solution, the net ionic equation is __________.

Accepted Answer

A) SO42- (aq)+ 2Na+ (aq)→ Na2SO4 (aq) 
B) SO42- (aq)+ 2Na+ (aq)→ Na2SO4 (s) 
C) H+ (aq)+ OH- (aq)→ H2O (l) 
D) H2SO4 (aq)+ 2OH- (aq)→ 2 H2O (l)+ SO42- (aq) 
E) 2H+ (aq)+ 2NaOH (aq)→ 2 H2O (l)+ 2Na+ (aq) 
A) SO42- (aq)+ 2Na+ (aq)→ Na2SO4 (aq) 
B) SO42- (aq)+ 2Na+ (aq)→ Na2SO4 (s) 
C) H+ (aq)+ OH- (aq)→ H2O (l) 
D) H2SO4 (aq)+ 2OH- (aq)→ 2 H2O (l)+ SO42- (aq) 
E) 2H+ (aq)+ 2NaOH (aq)→ 2 H2O (l)+ 2Na+ (aq)

Question 5

The molarity of an aqueous solution containing 75.3 g of glucose (C6H12O6)in 35.5 mL of solution is __________.

Accepted Answer

A) 1.85 
B) 2.12 
C) 0.197 
D) 3.52 
E) 11.8 
A) 1.85 
B) 2.12 
C) 0.197 
D) 3.52 
E) 11.8

Question 6

When aqueous solutions of AgN O3 and KI are mixed, AgI precipitates. The balanced net ionic equation is __________.

Accepted Answer

A) Ag+ (aq)+ I- (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)+ I- (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 7

An aliquot (28.7 mL)of a KOH solution required 31.3 mL of 0.118 M HCl for neutralization. What mass (g)of KOH was in the original sample?

Accepted Answer

A) 1.64 
B) 7.28 
C) 0.173 
D) 0.207 
E) 0.414 
A) 1.64 
B) 7.28 
C) 0.173 
D) 0.207 
E) 0.414

Question 8

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

Accepted Answer

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

Question 9

What volume (mL)of a concentrated solution of sodium hydroxide (6.00 M)must be diluted to 200.0 mL to make a 0.880 M solution of sodium hydroxide?

Accepted Answer

A) 2.64 
B) 176 
C) 26.4 
D) 29.3 
E) 50.0 
A) 2.64 
B) 176 
C) 26.4 
D) 29.3 
E) 50.0

Question 10

Which of the following are weak acids?

Accepted Answer

A) HF, HBr 
B) HI, HNO3, HBr 
C) HI, HF 
D) HF 
E) none of the above 
A) HF, HBr 
B) HI, HNO3, HBr 
C) HI, HF 
D) HF 
E) none of the above

Question 11

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

Question 12

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 13

Of the reactions below, only __________ is not spontaneous.

Accepted Answer

A) Mg (s)+ 2HCl (aq)→ MgCl2 (aq)+ H2 (g) 
B) 2Ag (s)+ 2HNO3 (aq)→ 2AgNO3 (aq)+ H2 (g) 
C) 2Ni (s)+ H2SO4 (aq)→ Ni2SO4 (aq)+ H2 (g) 
D) 2Al (s)+ 6HBr (aq)→ 2AlBr3 (aq)+ 3 H2 (g) 
E) Zn (s)+ 2HI (aq)→ ZnI2 (aq)+ H2 (g) 
A) Mg (s)+ 2HCl (aq)→ MgCl2 (aq)+ H2 (g) 
B) 2Ag (s)+ 2HNO3 (aq)→ 2AgNO3 (aq)+ H2 (g) 
C) 2Ni (s)+ H2SO4 (aq)→ Ni2SO4 (aq)+ H2 (g) 
D) 2Al (s)+ 6HBr (aq)→ 2AlBr3 (aq)+ 3 H2 (g) 
E) Zn (s)+ 2HI (aq)→ ZnI2 (aq)+ H2 (g)

Question 14

Which of these metals will be oxidized by the ions of cobalt?

Accepted Answer

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

Question 15

What is the concentration (M)of CH3OH in a solution prepared by dissolving 11.7 g of CH3OH in sufficient water to give exactly 230. mL of solution?

Accepted Answer

A) 11.9 
B) 1.59 
C) 0.00159 
D) 3.17 
E) 0.0841 
A) 11.9 
B) 1.59 
C) 0.00159 
D) 3.17 
E) 0.0841

Question 16

What are the respective concentrations (M)of Fe3+ and I- afforded by dissolving 0.200 mol FeI3 in water and diluting to 725 mL?

Accepted Answer

A) 0.276 and 0.828 
B) 0.828 and 0.276 
C) 0.276 and 0.276 
D) 0.145 and 0.435 
E) 0.145 and 0.0483 
A) 0.276 and 0.828 
B) 0.828 and 0.276 
C) 0.276 and 0.276 
D) 0.145 and 0.435 
E) 0.145 and 0.0483

Question 17

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

Accepted Answer

A) 0.300 M rubidium hydroxide 
B) 0.100 M magnesium hydroxide 
C) 0.100 M ammonia 
D) 0.100 M beryllium hydroxide 
E) 0.100 M hydrochloric acid 
A) 0.300 M rubidium hydroxide 
B) 0.100 M magnesium hydroxide 
C) 0.100 M ammonia 
D) 0.100 M beryllium hydroxide 
E) 0.100 M hydrochloric acid

Question 18

Of the metals below, only __________ will not dissolve in an aqueous solution containing nickel ions. aluminum
Chromium
Barium
Tin
Potassium

Accepted Answer

A) aluminum 
B) chromium 
C) barium 
D) tin 
E) potassium 
A) aluminum 
B) chromium 
C) barium 
D) tin 
E) potassium

Question 19

In which reaction does the oxidation number of hydrogen change?

Accepted Answer

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

Question 20

The spectator ions in the reaction between aqueous perchloric acid and aqueous barium hydroxide are __________.

Accepted Answer

A) OH- and ClO4- 
B) H+, OH-, ClO4-, and Ba2+ 
C) H+ and OH- 
D) H+ and Ba2+ 
E) ClO4- and Ba2+ 
A) OH- and ClO4- 
B) H+, OH-, ClO4-, and Ba2+ 
C) H+ and OH- 
D) H+ and Ba2+ 
E) ClO4- and Ba2+

Exam 4: Aqueous Reactions and Solution Stoichiometry

The molarity (M)of an aqueous solution containing 52.5 g of sucrose (C12H22O11)in 35.5 mL of solution is __________.

The balanced net ionic equation for precipitation of CaCO3 when aqueous solutions of Na2CO3 and CaCl2 are mixed is __________.

The concentration of species in 500 mL of a 2.104 M solution of sodium sulfate is __________ M sodium ion and __________ M sulfate ion.

When H2SO4 is neutralized by NaOH in aqueous solution, the net ionic equation is __________.

The molarity of an aqueous solution containing 75.3 g of glucose (C6H12O6)in 35.5 mL of solution is __________.

When aqueous solutions of AgN O3 and KI are mixed, AgI precipitates. The balanced net ionic equation is __________.

An aliquot (28.7 mL)of a KOH solution required 31.3 mL of 0.118 M HCl for neutralization. What mass (g)of KOH was in the original sample?

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

What volume (mL)of a concentrated solution of sodium hydroxide (6.00 M)must be diluted to 200.0 mL to make a 0.880 M solution of sodium hydroxide?

Which of the following are weak acids?

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

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

Of the reactions below, only __________ is not spontaneous.

Which of these metals will be oxidized by the ions of cobalt?

What is the concentration (M)of CH3OH in a solution prepared by dissolving 11.7 g of CH3OH in sufficient water to give exactly 230. mL of solution?

What are the respective concentrations (M)of Fe3+ and I- afforded by dissolving 0.200 mol FeI3 in water and diluting to 725 mL?

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

Of the metals below, only __________ will not dissolve in an aqueous solution containing nickel ions. aluminum Chromium Barium Tin Potassium

In which reaction does the oxidation number of hydrogen change?

The spectator ions in the reaction between aqueous perchloric acid and aqueous barium hydroxide are __________.

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

The Chemistry of Life: Organic and Biological Chemistry

Filters

The molarity (M)of an aqueous solution containing 52.5 g of sucrose (C₁₂H₂₂O₁₁)in 35.5 mL of solution is __________.

The balanced net ionic equation for precipitation of CaCO₃ when aqueous solutions of Na₂CO₃ and CaCl₂ are mixed is __________.

The concentration of species in 500 mL of a 2.104 M solution of sodium sulfate is M sodium ion and M sulfate ion.

When H₂SO₄ is neutralized by NaOH in aqueous solution, the net ionic equation is __________.

The molarity of an aqueous solution containing 75.3 g of glucose (C₆H₁₂O₆)in 35.5 mL of solution is __________.

When aqueous solutions of AgN O₃ and KI are mixed, AgI precipitates. The balanced net ionic equation is __________.

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

What is the concentration (M)of CH₃OH in a solution prepared by dissolving 11.7 g of CH₃OH in sufficient water to give exactly 230. mL of solution?

What are the respective concentrations (M)of Fe³⁺ and I^- afforded by dissolving 0.200 mol FeI₃ in water and diluting to 725 mL?