Question 1

Identify the oxidizing and reducing agents in the following oxidation-reduction reaction.
CH4(g) + 2O2(g)   CO(g)+2H2(g)

Accepted Answer

Oxidizing agent: O₂ Reducing agent: CH₄
An oxidizing agent is a chemical species that removes electrons from another species. A reducing agent is a chemical species that gives electrons to another species.

Question 2

Write the balanced molecular equation and the net ionic equation for the reaction of solid magnesium hydroxide with a solution of sulfuric acid.

Accepted Answer

Mg(OH)₂(s) H₂SO₄(aq) MgSO₄(aq) H₂O(l ) Mg(OH)₂(s) 2H₃O⁺(aq) Mg²⁺(aq) 4H₂O(l ) or Mg(OH)₂(s) 2H⁺(aq) Mg²⁺(aq) 2H₂O(l )

Question 3

Molarity, M, is defined as ________

Accepted Answer

A) moles of solute dissolved in 1 mol of solvent. 
B) moles of solute dissolved in 1 kg of solvent. 
C) moles of solute dissolved in 1 L of solvent. 
D) moles of solute dissolved in 1 L of solution. 
E) moles of solute dissolved in the solution. 
A) moles of solute dissolved in 1 mol of solvent. 
B) moles of solute dissolved in 1 kg of solvent. 
C) moles of solute dissolved in 1 L of solvent. 
D) moles of solute dissolved in 1 L of solution. 
E) moles of solute dissolved in the solution. D

Question 4

If 50.0 mL of a 0.10 M solution of sodium chloride is mixed with 50.0 mL of 0.10 M magnesium chloride, what is the molar concentration of chloride in the resulting solution?

Accepted Answer

A) 0.10 M 
B) 0.20 M 
C) 0.05 M 
D) 0.15 M 
E) 0.25 M 
A) 0.10 M 
B) 0.20 M 
C) 0.05 M 
D) 0.15 M 
E) 0.25 M

Question 5

Hartmann's solution is used in intravenous therapy to replace lost body fluid and mineral salts. The total ion concentration in Hartmann's solution is 276 mM. It often is prepared from a more concentrated stock solution. How much stock solution is needed to prepare 500 mL of Hartmann's solution? The total ion concentration in the stock solution is 1.38 M.

Accepted Answer

A) 50 mL 
B) 10 mL 
C) 100 mL 
D) 500 mL 
E) 200 mL 
A) 50 mL 
B) 10 mL 
C) 100 mL 
D) 500 mL 
E) 200 mL

Question 6

Most alkaline earth salts are soluble. Identify an exception to this generalization.

Accepted Answer

A) MgSO4 
B) CaS 
C) Sr(OH)2 
D) BaSO4 
E) Ca(NO3)2 
A) MgSO4 
B) CaS 
C) Sr(OH)2 
D) BaSO4 
E) Ca(NO3)2

Question 7

In a demonstration of strong electrolytes, weak electrolytes, and nonelectrolytes, Professor Popsnorkle used a lightbulb apparatus that showed how much a solution conducted electricity by the brightness of the lightbulb. When pure water was tested, the bulb did not light. Then Professor Popsnorkle tested the following aqueous solutions. Which one caused the bulb to burn the brightest?

Accepted Answer

A) table salt, NaCl 
B) ethanol, CH3CH2OH 
C) table sugar, C12H22O11 
D) acetic acid, CH3COOH 
E) methanol, CH3OH 
A) table salt, NaCl 
B) ethanol, CH3CH2OH 
C) table sugar, C12H22O11 
D) acetic acid, CH3COOH 
E) methanol, CH3OH

Question 8

Which contains more solute particles: a 0.10 M aqueous solution of methanol (CH3OH) or a 0.10 M aqueous solution of salt (NaCl)?

Accepted Answer

A) They contain the same number of solute particles. 
B) The salt solution contains twice as many particles as the methanol solution. 
C) The methanol solution contains three times as many particles as the salt solution. 
D) Neither solution contains solute particles. 
E) The methanol solution contains twice as many particles as the salt solution. 
A) They contain the same number of solute particles. 
B) The salt solution contains twice as many particles as the methanol solution. 
C) The methanol solution contains three times as many particles as the salt solution. 
D) Neither solution contains solute particles. 
E) The methanol solution contains twice as many particles as the salt solution.

Question 9

Draw pictures that represent: (a) a strong electrolyte, (b) a weak electrolyte, and (c) a nonelectrolyte solution. Omit solvent molecules for clarity and use the following formula unit in each diagram as a starting point.   Strong electrolyte Weak electrolyte Nonelectrolyte

Accepted Answer

@#IMG-DLM& Strong electrolyte

Question 10

Sodium fluoride is added to drinking water in some municipalities to protect teeth against cavities. The idea is to convert hydroxyapatite, Ca10(PO4)6(OH)2, into more stable fluorapatite, Ca10(PO4)6F2. What is the molarity of a 5.0 mg/L sodium fluoride solution?

Accepted Answer

The answer of Sodium fluoride is added to drinking water...

Question 11

In which one of the following compounds is the oxidation number of silicon not equal to +4?

Accepted Answer

A) SiO2 
B) SiC 
C) SiO32- 
D) Mg2Si 
E) SiCl4 
A) SiO2 
B) SiC 
C) SiO32- 
D) Mg2Si 
E) SiCl4

Question 12

Why is an aqueous solution of table salt (NaCl) a good conductor of electricity but a solution containing an equal molar concentration of table sugar (C12H22O11) is not?

Accepted Answer

Table salt is an ionic compound. It is a

Question 13

Identify the reducing agent in the following reaction. Fe2+(aq)   Ce4+(aq)   Fe3+(aq)   Ce3+(aq)

Accepted Answer

A) Fe2+(aq) 
B) Fe3+(aq) 
C) Ce3+(aq) 
D) Ce4+(aq) 
E) This is not an example of an oxidation-reduction reaction. 
A) Fe2+(aq) 
B) Fe3+(aq) 
C) Ce3+(aq) 
D) Ce4+(aq) 
E) This is not an example of an oxidation-reduction reaction.

Question 14

If one regular antacid tablet contains 500 mg of solid CaCO3 (100 g/mol), how many mL of 1.0 M stomach acid (HCl) could it neutralize?

Accepted Answer

A) 5 mL 
B) 10 mL 
C) 50 mL 
D) 100 mL 
E) 15 mL 
A) 5 mL 
B) 10 mL 
C) 50 mL 
D) 100 mL 
E) 15 mL

Question 15

Identify which of the following compounds are soluble in water.

Accepted Answer

A)  AgNO3 
B)  Mg(OH)2 
C)  (NH4)2S 
D)  KOH 
E)  CaCO3 
A)  AgNO3 
B)  Mg(OH)2 
C)  (NH4)2S 
D)  KOH 
E)  CaCO3

Question 16

Write the net ionic equation for the precipitation reaction that occurs between potassium bromide and lead(II) nitrate.

Accepted Answer

Pb²⁺(aq)

Question 17

Which one of the following statements is not correct?

Accepted Answer

A) Oxidation refers to a chemical reaction in which a substance loses electrons. 
B) Reduction refers to a chemical reaction in which a substance gains electrons. 
C) The oxidation number represents the charge an atom would have if all its bonds to other atoms were ionic. 
D) An oxidizing agent is a substance that is oxidized in a chemical reaction. 
E) Statements A-D are all correct. 
A) Oxidation refers to a chemical reaction in which a substance loses electrons. 
B) Reduction refers to a chemical reaction in which a substance gains electrons. 
C) The oxidation number represents the charge an atom would have if all its bonds to other atoms were ionic. 
D) An oxidizing agent is a substance that is oxidized in a chemical reaction. 
E) Statements A-D are all correct.

Question 18

In the dilution of 10.0 mL of a 0.10 M solution of HCl to a volume of 20.0 mL, what remains unchanged?

Accepted Answer

A) the moles of HCl in the solution 
B) the concentration of the HCl solution 
C) the volume of the HCl solution 
D) the mass of the HCl solution 
E) All of the above change. 
A) the moles of HCl in the solution 
B) the concentration of the HCl solution 
C) the volume of the HCl solution 
D) the mass of the HCl solution 
E) All of the above change.

Question 19

A typical adult body contains about 6.0 L of blood. The hemoglobin content is about 16 g per 100.0 mL of blood. The molar mass of hemoglobin is approximately 64,000 g/mol. (a) What is the molar concentration of hemoglobin in blood, and (b) how many moles of hemoglobin are present in a typical adult?

Accepted Answer

(a) 2.5 @#IMG-DLM& M

Question 20

Mercury is one of the most toxic metal ions to fish, as they can only tolerate a concentration slightly above 1.5     mM. What is the mercury concentration in $\mu$g/L?

Accepted Answer

A) 6.0     $\mu$g/L 
B) 12 $\mu$g/L 
C) 30 $\mu$g/L 
D) 75 $\mu$g/L 
E) 1.5     $\mu$g/L 
A) 6.0     $\mu$g/L 
B) 12 $\mu$g/L 
C) 30 $\mu$g/L 
D) 75 $\mu$g/L 
E) 1.5     $\mu$g/L

Identify the oxidizing and reducing agents in the following oxidation-reduction reaction. CH₄(g) + 2O₂(g) CO(g)+2H₂(g)

Write the balanced molecular equation and the net ionic equation for the reaction of solid magnesium hydroxide with a solution of sulfuric acid.

Molarity, M, is defined as ________

If 50.0 mL of a 0.10 M solution of sodium chloride is mixed with 50.0 mL of 0.10 M magnesium chloride, what is the molar concentration of chloride in the resulting solution?

Most alkaline earth salts are soluble. Identify an exception to this generalization.

Which contains more solute particles: a 0.10 M aqueous solution of methanol (CH₃OH) or a 0.10 M aqueous solution of salt (NaCl)?

Draw pictures that represent: (a) a strong electrolyte, (b) a weak electrolyte, and (c) a nonelectrolyte solution. Omit solvent molecules for clarity and use the following formula unit in each diagram as a starting point. Strong electrolyte Weak electrolyte Nonelectrolyte

Sodium fluoride is added to drinking water in some municipalities to protect teeth against cavities. The idea is to convert hydroxyapatite, Ca₁₀(PO₄)₆(OH)₂, into more stable fluorapatite, Ca₁₀(PO₄)₆F₂. What is the molarity of a 5.0 mg/L sodium fluoride solution?

In which one of the following compounds is the oxidation number of silicon not equal to +4?

Why is an aqueous solution of table salt (NaCl) a good conductor of electricity but a solution containing an equal molar concentration of table sugar (C₁₂H₂₂O₁₁) is not?

Identify the reducing agent in the following reaction. Fe²⁺(aq) Ce⁴⁺(aq) Fe³⁺(aq) Ce³⁺(aq)

If one regular antacid tablet contains 500 mg of solid CaCO₃ (100 g/mol), how many mL of 1.0 M stomach acid (HCl) could it neutralize?

Identify which of the following compounds are soluble in water.

Write the net ionic equation for the precipitation reaction that occurs between potassium bromide and lead(II) nitrate.

Which one of the following statements is not correct?

In the dilution of 10.0 mL of a 0.10 M solution of HCl to a volume of 20.0 mL, what remains unchanged?

A typical adult body contains about 6.0 L of blood. The hemoglobin content is about 16 g per 100.0 mL of blood. The molar mass of hemoglobin is approximately 64,000 g/mol. (a) What is the molar concentration of hemoglobin in blood, and (b) how many moles of hemoglobin are present in a typical adult?

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

Exam 4: Solution Chemistry: The Hydrosphere

Identify the oxidizing and reducing agents in the following oxidation-reduction reaction. CH4(g) + 2O2(g) CO(g)+2H2(g)

Write the balanced molecular equation and the net ionic equation for the reaction of solid magnesium hydroxide with a solution of sulfuric acid.

Molarity, M, is defined as ________

If 50.0 mL of a 0.10 M solution of sodium chloride is mixed with 50.0 mL of 0.10 M magnesium chloride, what is the molar concentration of chloride in the resulting solution?

Most alkaline earth salts are soluble. Identify an exception to this generalization.

Which contains more solute particles: a 0.10 M aqueous solution of methanol (CH3OH) or a 0.10 M aqueous solution of salt (NaCl)?

Draw pictures that represent: (a) a strong electrolyte, (b) a weak electrolyte, and (c) a nonelectrolyte solution. Omit solvent molecules for clarity and use the following formula unit in each diagram as a starting point. Strong electrolyte Weak electrolyte Nonelectrolyte

Sodium fluoride is added to drinking water in some municipalities to protect teeth against cavities. The idea is to convert hydroxyapatite, Ca10(PO4)6(OH)2, into more stable fluorapatite, Ca10(PO4)6F2. What is the molarity of a 5.0 mg/L sodium fluoride solution?

In which one of the following compounds is the oxidation number of silicon not equal to +4?

Why is an aqueous solution of table salt (NaCl) a good conductor of electricity but a solution containing an equal molar concentration of table sugar (C12H22O11) is not?

Identify the reducing agent in the following reaction. Fe2+(aq) Ce4+(aq) Fe3+(aq) Ce3+(aq)

If one regular antacid tablet contains 500 mg of solid CaCO3 (100 g/mol), how many mL of 1.0 M stomach acid (HCl) could it neutralize?

Identify which of the following compounds are soluble in water.

Write the net ionic equation for the precipitation reaction that occurs between potassium bromide and lead(II) nitrate.

Which one of the following statements is not correct?

In the dilution of 10.0 mL of a 0.10 M solution of HCl to a volume of 20.0 mL, what remains unchanged?

Mercury is one of the most toxic metal ions to fish, as they can only tolerate a concentration slightly above 1.5 mM. What is the mercury concentration in μ\muμ g/L?

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

Identify the oxidizing and reducing agents in the following oxidation-reduction reaction. CH₄(g) + 2O₂(g) CO(g)+2H₂(g)

Which contains more solute particles: a 0.10 M aqueous solution of methanol (CH₃OH) or a 0.10 M aqueous solution of salt (NaCl)?

Sodium fluoride is added to drinking water in some municipalities to protect teeth against cavities. The idea is to convert hydroxyapatite, Ca₁₀(PO₄)₆(OH)₂, into more stable fluorapatite, Ca₁₀(PO₄)₆F₂. What is the molarity of a 5.0 mg/L sodium fluoride solution?

Why is an aqueous solution of table salt (NaCl) a good conductor of electricity but a solution containing an equal molar concentration of table sugar (C₁₂H₂₂O₁₁) is not?

Identify the reducing agent in the following reaction. Fe²⁺(aq) Ce⁴⁺(aq) Fe³⁺(aq) Ce³⁺(aq)

If one regular antacid tablet contains 500 mg of solid CaCO₃ (100 g/mol), how many mL of 1.0 M stomach acid (HCl) could it neutralize?