Question 1

Most chloride salts are soluble. Identify an exception to this generalization.

Accepted Answer

A) AgCl 
B) CaCl2 
C) MgCl2 
D) BaCl2 
E) NaCl 
A) AgCl 
B) CaCl2 
C) MgCl2 
D) BaCl2 
E) NaCl

Question 2

In the following reaction, which element or ion is reduced? Cl2(g)   NaBr(aq)   NaCl(aq)   Br2(g)

Accepted Answer

A) Br2 
B) Na+ 
C) Cl2 
D) Br - 
E) C- 
A) Br2 
B) Na+ 
C) Cl2 
D) Br - 
E) C-

Question 3

In which one of the following compounds is the oxidation number of S equal to +4?

Accepted Answer

A) H2S 
B) S2Cl2 
C) MgSO4 
D) S8 
E) Na2SO3 
A) H2S 
B) S2Cl2 
C) MgSO4 
D) S8 
E) Na2SO3

Question 4

In the following reaction, which element is oxidized? Cu   FeSO4   Fe  CuSO4

Accepted Answer

A) Cu 
B) Fe 
C) S 
D) O 
E) None, this is not a redox reaction. 
A) Cu 
B) Fe 
C) S 
D) O 
E) None, this is not a redox reaction.

Question 5

A chemistry student attempted to make a 0.2000 M solution of NaCl using a 100.0 mL volumetric flask. She added exactly 100.0 mL of water to the flask, then added 0.02000 mol of NaCl, and found that the total volume in the flask was above the 100.0 mL mark. What was the concentration of the solution?

Accepted Answer

A) exactly 0.2000 M 
B) a bit less than 0.2000 M 
C) a bit more than 0.2000 M 
D) exactly 0.2002 M 
E) There is insufficient information to select one of the above responses. 
A) exactly 0.2000 M 
B) a bit less than 0.2000 M 
C) a bit more than 0.2000 M 
D) exactly 0.2002 M 
E) There is insufficient information to select one of the above responses.

Question 6

Identify the base in the following acid-base reaction. NaNO2(aq)   HI(aq)   NaI(aq)   HNO2(aq)

Accepted Answer

A) Na+ 
B) NO2- 
C) I- 
D) HI 
E) HNO2 
A) Na+ 
B) NO2- 
C) I- 
D) HI 
E) HNO2

Question 7

If 100 mL of 3.0 M solution were diluted to 250 mL, what would the concentration be?

Accepted Answer

A) 0.012 M 
B) 0.12 M 
C) 1.2 M 
D) 12 M 
E) 120 M 
A) 0.012 M 
B) 0.12 M 
C) 1.2 M 
D) 12 M 
E) 120 M

Question 8

The National Primary Drinking Water Regulations limit the concentration of lead in drinking water to 0.015 mg/L, which is ________

Accepted Answer

A) 0.015 ppb. 
B) 15 ppm. 
C) 1.5 ppb. 
D) 15 ppb. 
E) 150 ppb. 
A) 0.015 ppb. 
B) 15 ppm. 
C) 1.5 ppb. 
D) 15 ppb. 
E) 150 ppb.

Question 9

Which one of the following statements regarding a strong acid is not correct?

Accepted Answer

A) A strong acid ionizes completely in water. 
B) A strong acid ionizes in water to produce hydronium ions. 
C) A strong acid neutralizes bases. 
D) HCl is an example of a strong acid. 
E) Acids are only strong at a high concentration. 
A) A strong acid ionizes completely in water. 
B) A strong acid ionizes in water to produce hydronium ions. 
C) A strong acid neutralizes bases. 
D) HCl is an example of a strong acid. 
E) Acids are only strong at a high concentration.

Question 10

Commercial hydrochloric acid is 12.1 M. What volume of commercial HCl solution should be used to prepare 250.0 mL of 3.00 M HCl?

Accepted Answer

A) 139 mL 
B) 126 mL 
C) 252 mL 
D) 62 mL 
E) 83 mL 
A) 139 mL 
B) 126 mL 
C) 252 mL 
D) 62 mL 
E) 83 mL

Question 11

What mass of barium sulfate (molar mass = 233 g/mol) is produced when 125 mL of a 0.150 M solution of barium chloride is mixed with 125 mL of a 0.150 M solution of iron(III) sulfate?

Accepted Answer

A) 7.59 g 
B) 3.65 g 
C) 13.1 g 
D) 18.8 g 
E) 4.37 g 
A) 7.59 g 
B) 3.65 g 
C) 13.1 g 
D) 18.8 g 
E) 4.37 g

Question 12

How many grams of magnesium chloride, MgCl2, are needed to make up 500.0 mL of a solution that is 0.300 M ?

Accepted Answer

A) 14.3 g 
B) 57.1 g 
C) 158 g 
D) 1.58      g 
E) 1.75     g 
A) 14.3 g 
B) 57.1 g 
C) 158 g 
D) 1.58      g 
E) 1.75     g

Question 13

If 1.0 L of 1.0 M HCl spilled and needed to be neutralized, how many grams of the solid sodium carbonate (Na2CO3, 106 g/mol) would be required?

Accepted Answer

A) 53 g 
B) 106 g 
C) 1,060 g 
D) 530 g 
E) 212 g 
A) 53 g 
B) 106 g 
C) 1,060 g 
D) 530 g 
E) 212 g

Question 14

What is meant by the terms solution, solvent, and solute?

Accepted Answer

A solution is a homogeneous mixture of t

Question 15

Which of the following compounds is a nonelectrolyte?

Accepted Answer

A) sulfuric acid, H2SO4 
B) acetic acid, CH3COOH 
C) hexane, C6H14 
D) nitrous acid, HNO2 
E) potassium hydroxide, KOH 
A) sulfuric acid, H2SO4 
B) acetic acid, CH3COOH 
C) hexane, C6H14 
D) nitrous acid, HNO2 
E) potassium hydroxide, KOH

Question 16

What volume of 0.25 M hydrochloric acid (HCl) solution contains 0.15 mol HCl?

Accepted Answer

A) 6.0 mL 
B) 60 mL 
C) 600 mL 
D) 1.7 L 
E) 170 mL 
A) 6.0 mL 
B) 60 mL 
C) 600 mL 
D) 1.7 L 
E) 170 mL

Question 17

Arsenic, which is toxic, can be removed from drinking water by precipitation as the sulfide. Write the net ionic equation for the precipitation of As3+ using sodium sulfide, Na2S.

Accepted Answer

2As³⁺(aq)

Question 18

Identify the acid in the following acid-base reaction. PbCO3(s)   H2SO4(aq)   PbSO4(s)   CO2(g)   H2O(l)

Accepted Answer

A) PbCO3(s) 
B) CO2(g) 
C) PbSO4(s) 
D) H2O(l) 
E) H2SO4(aq) 
A) PbCO3(s) 
B) CO2(g) 
C) PbSO4(s) 
D) H2O(l) 
E) H2SO4(aq)

Question 19

In a spontaneous oxidation reduction reaction between aluminum and silver ion, the aluminum(III) ion and solid silver are formed. If 0.1 mol of aluminum is consumed in this reaction, how much silver will be produced?

Accepted Answer

A) 0.3 mol 
B) 0.1 mol 
C) 1.0 mol 
D) 3 mol 
E) 0.2 mol 
A) 0.3 mol 
B) 0.1 mol 
C) 1.0 mol 
D) 3 mol 
E) 0.2 mol

Question 20

A 125 mL sample of orange juice was titrated using a redox reaction to the equivalence point with the addition of 7.6 mL of a 0.0025M iodine (I2) solution. What is the concentration of vitamin C (C6H8O6) in this sample? C6H8O6(aq)   I2(aq)   C6H6O6(aq)   2I-(aq)   2H+(aq)

Accepted Answer

A) 30 mM 
B) 15 mM 
C) 19 mM 
D) 0.30 mM 
E) 0.15 mM 
A) 30 mM 
B) 15 mM 
C) 19 mM 
D) 0.30 mM 
E) 0.15 mM

Exam 4: Solution Chemistry: The Hydrosphere

Most chloride salts are soluble. Identify an exception to this generalization.

In the following reaction, which element or ion is reduced? Cl2(g) NaBr(aq) NaCl(aq) Br2(g)

In which one of the following compounds is the oxidation number of S equal to +4?

In the following reaction, which element is oxidized? Cu FeSO4 Fe CuSO4

Identify the base in the following acid-base reaction. NaNO2(aq) HI(aq) NaI(aq) HNO2(aq)

If 100 mL of 3.0 M solution were diluted to 250 mL, what would the concentration be?

The National Primary Drinking Water Regulations limit the concentration of lead in drinking water to 0.015 mg/L, which is ________

Which one of the following statements regarding a strong acid is not correct?

Commercial hydrochloric acid is 12.1 M. What volume of commercial HCl solution should be used to prepare 250.0 mL of 3.00 M HCl?

What mass of barium sulfate (molar mass = 233 g/mol) is produced when 125 mL of a 0.150 M solution of barium chloride is mixed with 125 mL of a 0.150 M solution of iron(III) sulfate?

How many grams of magnesium chloride, MgCl2, are needed to make up 500.0 mL of a solution that is 0.300 M ?

If 1.0 L of 1.0 M HCl spilled and needed to be neutralized, how many grams of the solid sodium carbonate (Na2CO3, 106 g/mol) would be required?

What is meant by the terms solution, solvent, and solute?

Which of the following compounds is a nonelectrolyte?

What volume of 0.25 M hydrochloric acid (HCl) solution contains 0.15 mol HCl?

Arsenic, which is toxic, can be removed from drinking water by precipitation as the sulfide. Write the net ionic equation for the precipitation of As3+ using sodium sulfide, Na2S.

Identify the acid in the following acid-base reaction. PbCO3(s) H2SO4(aq) PbSO4(s) CO2(g) H2O(l)

In a spontaneous oxidation reduction reaction between aluminum and silver ion, the aluminum(III) ion and solid silver are formed. If 0.1 mol of aluminum is consumed in this reaction, how much silver will be produced?

A 125 mL sample of orange juice was titrated using a redox reaction to the equivalence point with the addition of 7.6 mL of a 0.0025M iodine (I2) solution. What is the concentration of vitamin C (C6H8O6) in this sample? C6H8O6(aq) I2(aq) C6H6O6(aq) 2I-(aq) 2H+(aq)

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

In the following reaction, which element or ion is reduced? Cl₂(g) NaBr(aq) NaCl(aq) Br₂(g)

In the following reaction, which element is oxidized? Cu FeSO₄ Fe CuSO₄

Identify the base in the following acid-base reaction. NaNO₂(aq) HI(aq) NaI(aq) HNO₂(aq)

How many grams of magnesium chloride, MgCl₂, are needed to make up 500.0 mL of a solution that is 0.300 M ?

If 1.0 L of 1.0 M HCl spilled and needed to be neutralized, how many grams of the solid sodium carbonate (Na₂CO₃, 106 g/mol) would be required?

Arsenic, which is toxic, can be removed from drinking water by precipitation as the sulfide. Write the net ionic equation for the precipitation of As³⁺ using sodium sulfide, Na₂S.

Identify the acid in the following acid-base reaction. PbCO₃(s) H₂SO₄(aq) PbSO₄(s) CO₂(g) H₂O(l)

A 125 mL sample of orange juice was titrated using a redox reaction to the equivalence point with the addition of 7.6 mL of a 0.0025M iodine (I₂) solution. What is the concentration of vitamin C (C₆H₈O₆) in this sample? C₆H₈O₆(aq) I₂(aq) C₆H₆O₆(aq) 2I^-(aq) 2H⁺(aq)