Question 1

How many grams of sodium chloride are there in 55.0 mL of a 1.90 M aqueous solution of sodium chloride?

Accepted Answer

A) 0.105 
B) 6.11 
C) 3.21 
D) 6.11 × 103 
E) 12.2 
A) 0.105 
B) 6.11 
C) 3.21 
D) 6.11 × 103 
E) 12.2

Question 2

A weak electrolyte exists predominantly as __________ in solution.

Accepted Answer

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

Question 3

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 4

When aqueous solutions of AgNO3 and NaCl are mixed, AgCl precipitates. The balanced net ionic equation is __________.

Accepted Answer

A) Ag+ (aq)+ Cl- (aq)→ AgCl (s) 
B) Ag+ (aq)+ NO3- (aq)→ AgNO3 (s) 
C) Ag+ (aq)+ NO3- (aq)→ AgNO (aq) 
D) AgNO3 (aq)+ NaCl (aq)→ AgCl (s)+ NaNO3 (aq) 
E) AgNO3 (aq)+ NaCl (aq)→ AgCl (aq)+ NaNO3 (s) 
A) Ag+ (aq)+ Cl- (aq)→ AgCl (s) 
B) Ag+ (aq)+ NO3- (aq)→ AgNO3 (s) 
C) Ag+ (aq)+ NO3- (aq)→ AgNO (aq) 
D) AgNO3 (aq)+ NaCl (aq)→ AgCl (s)+ NaNO3 (aq) 
E) AgNO3 (aq)+ NaCl (aq)→ AgCl (aq)+ NaNO3 (s)

Question 5

The concentration of chloride ions in a 0.193 M solution of potassium chloride is __________.

Accepted Answer

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

Question 6

Ammonia is a strong base.

Accepted Answer

A) True 
 B)False

Question 7

How many grams of sodium chloride are there in 550.0 mL of a 1.90 M aqueous solution of sodium chloride?

Accepted Answer

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

Question 8

What is the concentration (M)of KCl in a solution made by mixing 30.0 mL of 0.100 M KCl with 50.0 mL of 0.100 M KCl?

Accepted Answer

A) 0.100 
B) 0.0500 
C) 0.0333 
D) 0.0250 
E) 125 
A) 0.100 
B) 0.0500 
C) 0.0333 
D) 0.0250 
E) 125

Question 9

When gold dissolves in aqua regia, into what form is the gold converted?

Accepted Answer

The answer of When gold dissolves in aqua regia, into...

Question 10

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 11

What are the spectator ions in the reaction between Mg(OH)2 (aq)and HCl (aq)?

Accepted Answer

A) Mg+2 and H+ 
B) H+ and OH- 
C) Mg+2 and Cl- 
D) H+ and Cl- 
E) OH- only 
A) Mg+2 and H+ 
B) H+ and OH- 
C) Mg+2 and Cl- 
D) H+ and Cl- 
E) OH- only

Question 12

Which of the following would require the largest volume of 0.100 M sodium hydroxide solution for neutralization?

Accepted Answer

A) 10.0 mL of 0.0500 M phosphoric acid 
B) 20.0 mL of 0.0500 M nitric acid 
C) 5.0 mL of 0.0100 M sulfuric acid 
D) 15.0 mL of 0.0500 M hydrobromic acid 
E) 10.0 mL of 0.0500 M perchloric acid 
A) 10.0 mL of 0.0500 M phosphoric acid 
B) 20.0 mL of 0.0500 M nitric acid 
C) 5.0 mL of 0.0100 M sulfuric acid 
D) 15.0 mL of 0.0500 M hydrobromic acid 
E) 10.0 mL of 0.0500 M perchloric acid

Question 13

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

Question 14

In which species does sulfur have the highest oxidation number?

Accepted Answer

A) S8 (elemental form of sulfur) 
B) H2S 
C) SO2 
D) H2SO3 
E) K2SO4 
A) S8 (elemental form of sulfur) 
B) H2S 
C) SO2 
D) H2SO3 
E) K2SO4

Question 15

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

Question 16

How many milliliters of 0.132 M HClO4 solution are needed to neutralize 50.00 mL of 0.0789 M NaOH?

Accepted Answer

A) 0.521 
B) 0.0120 
C) 83.7 
D) 0.0335 
E) 29.9 
A) 0.521 
B) 0.0120 
C) 83.7 
D) 0.0335 
E) 29.9

Question 17

Oxalic acid is a diprotic acid. Calculate the percent of oxalic acid (H2C2O4)in a solid given that a 0.7984-g sample of that solid required 37.98 mL of 0.2283 M NaOH for neutralization.

Accepted Answer

A) 48.89 
B) 97.78 
C) 28.59 
D) 1.086 
E) 22.83 
A) 48.89 
B) 97.78 
C) 28.59 
D) 1.086 
E) 22.83

Question 18

A 36.3 mL aliquot of 0.0529 M H2SO4 (aq)is to be titrated with 0.0411 M NaOH (aq). What volume (mL)of base will it take to reach the equivalence point?

Accepted Answer

A) 93.4 
B) 46.7 
C) 187 
D) 1.92 
E) 3.84 
A) 93.4 
B) 46.7 
C) 187 
D) 1.92 
E) 3.84

Question 19

The net ionic equation for formation of an aqueous solution of Al(NO3)3 via mixing solid Al(OH)3 and aqueous nitric acid is __________.

Accepted Answer

A) Al(OH)3 (s)+ 3HNO3 (aq)→ 3 H2O (l)+ Al(NO3)3 (aq) 
B) Al(OH)3 (s)+ 3NO3- (aq)→ 3OH- (aq)+ Al(NO3)3 (aq) 
C) Al(OH)3 (s)+ 3NO3- (aq)→ 3OH- (aq)+ Al(NO3)3 (s) 
D) Al(OH)3 (s)+ 3H+ (aq)→ 3 H2O (l)+ Al3+ (aq) 
E) Al(OH)3 (s)+ 3HNO3 (aq)→ 3 H2O (l)+ Al3+ (aq)+ NO3- (aq) 
A) Al(OH)3 (s)+ 3HNO3 (aq)→ 3 H2O (l)+ Al(NO3)3 (aq) 
B) Al(OH)3 (s)+ 3NO3- (aq)→ 3OH- (aq)+ Al(NO3)3 (aq) 
C) Al(OH)3 (s)+ 3NO3- (aq)→ 3OH- (aq)+ Al(NO3)3 (s) 
D) Al(OH)3 (s)+ 3H+ (aq)→ 3 H2O (l)+ Al3+ (aq) 
E) Al(OH)3 (s)+ 3HNO3 (aq)→ 3 H2O (l)+ Al3+ (aq)+ NO3- (aq)

Question 20

The net ionic equation for formation of an aqueous solution of NiI2 accompanied by evolution of CO2 gas via mixing solid NiCO3 and aqueous hydriodic acid is __________.

Accepted Answer

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

Exam 4: Aqueous Reactions and Solution Stoichiometry

How many grams of sodium chloride are there in 55.0 mL of a 1.90 M aqueous solution of sodium chloride?

A weak electrolyte exists predominantly as __________ in solution.

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

When aqueous solutions of AgNO3 and NaCl are mixed, AgCl precipitates. The balanced net ionic equation is __________.

The concentration of chloride ions in a 0.193 M solution of potassium chloride is __________.

Ammonia is a strong base.

How many grams of sodium chloride are there in 550.0 mL of a 1.90 M aqueous solution of sodium chloride?

What is the concentration (M)of KCl in a solution made by mixing 30.0 mL of 0.100 M KCl with 50.0 mL of 0.100 M KCl?

When gold dissolves in aqua regia, into what form is the gold converted?

Which one of the following is a triprotic acid?

What are the spectator ions in the reaction between Mg(OH)2 (aq)and HCl (aq)?

Which of the following would require the largest volume of 0.100 M sodium hydroxide solution for neutralization?

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?

In which species does sulfur have the highest oxidation number?

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?

How many milliliters of 0.132 M HClO4 solution are needed to neutralize 50.00 mL of 0.0789 M NaOH?

Oxalic acid is a diprotic acid. Calculate the percent of oxalic acid (H2C2O4)in a solid given that a 0.7984-g sample of that solid required 37.98 mL of 0.2283 M NaOH for neutralization.

A 36.3 mL aliquot of 0.0529 M H2SO4 (aq)is to be titrated with 0.0411 M NaOH (aq). What volume (mL)of base will it take to reach the equivalence point?

The net ionic equation for formation of an aqueous solution of Al(NO3)3 via mixing solid Al(OH)3 and aqueous nitric acid is __________.

The net ionic equation for formation of an aqueous solution of NiI2 accompanied by evolution of CO2 gas via mixing solid NiCO3 and aqueous hydriodic acid is __________.

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

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When aqueous solutions of AgNO₃ and NaCl are mixed, AgCl precipitates. The balanced net ionic equation is __________.

What are the spectator ions in the reaction between Mg(OH)₂ (aq)and HCl (aq)?

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 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?

How many milliliters of 0.132 M HClO₄ solution are needed to neutralize 50.00 mL of 0.0789 M NaOH?

Oxalic acid is a diprotic acid. Calculate the percent of oxalic acid (H₂C₂O₄)in a solid given that a 0.7984-g sample of that solid required 37.98 mL of 0.2283 M NaOH for neutralization.

A 36.3 mL aliquot of 0.0529 M H₂SO₄ (aq)is to be titrated with 0.0411 M NaOH (aq). What volume (mL)of base will it take to reach the equivalence point?

The net ionic equation for formation of an aqueous solution of Al(NO₃)₃via mixing solid Al(OH)₃ and aqueous nitric acid is __________.

The net ionic equation for formation of an aqueous solution of NiI₂ accompanied by evolution of CO₂gas via mixing solid NiCO₃ and aqueous hydriodic acid is __________.