Ch 03 Study Guide

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Ch. #3 Study Guide

Multiple Choice

Identify the choice that best completes the statement or answers the question.

____ 1. Nitroglycerin decomposes violently according to the balanced chemical equation below.2 C3H5(NO3)3( )→ 3 N2(g) + 1/2 O2(g) + 6 CO2(g) + 5 H2O(g)

Which of the following statements concerning this reaction is/are CORRECT?

1. Two moles of nitroglycerine will produce three moles of nitrogen and five moles of

water.

2. Four molecules of nitroglycerine will produced one molecule of oxygen and twelve

molecules of carbon dioxide.3. Six grams of nitroglycerine will produce nine grams of nitrogen and fifteen grams of

water.

a. 1 only b. 2 only c. 3 only d. 1 and 2 e. 1, 2, and 3

____ 2. When propane undergoes complete combustion, the products are carbon dioxide and water.__ C3H8(g) + __ O2(g)→ __ CO2(g) + __ H2O(g)

What are the respective coefficients when the equation is balanced with the smallest whole numbers?

a. 1, 1, 1, 1 b. 1, 3, 1, 3 c. 1, 3, 3, 1 d. 1, 5, 3, 4 e. 2, 5, 3, 4

____ 3. The reaction of elemental chlorine with potassium iodide yields elemental iodine and potassium chloride.

Write a balanced chemical equation for this reaction.

a. Cl2(g) + KI(s) → I(s) + KCl2(s) b. Cl2(g) + 2 KI(s) → I2(s) + 2 KCl(s) c. Cl2(g) + KI2(s) → I2(s) +

KCl2(s) d. Cl(g) + KI(s)→ I(s) + KCl(s) e. Cl2(g) + 2 K2I(s)→ I2(s) + 2 K2Cl(s)

____ 4. Metals react with oxygen gas to produce oxides with the general formula MxOy. Write a balanced chemical

equation for the reaction of titanium with oxygen to yield titanium(IV) oxide.

a. 4 Ti(s) + O2(g)→ 2 Ti2O(s) b. Ti(s) + O2(g)→ TiO2(s) c. 2 Ti(s) + O2(g)→ 2 TiO(s) d. Ti(s) + O(g)

→ TiO(s) e. 8 Ti(s) + O2(g)→ 2 Ti4O(s)

____ 5. The products of the complete combustion of octane, C8H18, are carbon dioxide and water. Write a balanced

chemical equation for this reaction.

a. C8H18( ) → 8 C(s) + 9 H2(g) b. C8H18( ) + 25 O2(g)→ 8 CO2 (g) + 9 H2O(g) c. 2 C8H18( ) + 25 O2(g)

→ 16 CO2(g) + 18 H2O(g) d. C8H18( ) + 16 O2(g)→ 8 CO2(g) + 9 H2(g) e. 2 C8H18( ) + 17 O2(g)→ 16

CO(g) + 18 H2O(g)

____ 6. What is the balanced chemical equation for the complete combustion of benzoic acid, C6H5CO2H, to form

carbon dioxide and water?

a. C6H5CO2H(s) → 6 C(s) + CO2(g) + 3 H2(g) b. C6H5CO2H(s)→ 7 CO2(g) + 3 H2O(g) c. C6H5CO2H(s)+ O2(g)→ CO2(g) + H2O(g) d. C6H5CO2H(s) + 8 O2(g)→ 7 CO2(g) + 3 H2O(g) e. 2 C6H5CO2H(s) + 15

O2(g)→ 14 CO2(g) + 6 H2O(g)



____ 7. Which of the following statements is/are CORRECT?1. A solution is a homogeneous mixture of two or more substances.

2. A solute is a mixture of a solvent and a soluble compound.

3. Aqueous solutions are solutions in which water is a solvent.

a. 1 only b. 2 only c. 3 only d. 1 and 2 e. 1 and 3

____ 8. Which of the following statements is/are CORRECT?

1. All ionic compounds that are soluble in water are electrolytes.

2. All ionic compounds dissolve in water.

3. Molecular compounds are never soluble in water.

a. 1 only b. 2 only c. 3 only d. 1 and 2 e. 2 and 3

____ 9. Which one of the following compounds is a nonelectrolyte when dissolved in water?a. HCl b. CaCl2 c. CCl4 d. Cu(NO3)2 e. NaCH3CO2


1. Most ionic compounds containing nitrate ion are soluble in water.2. Most ionic compounds containing sulfate ion are insoluble in water.

3. Most ionic compounds containing carbonate ion are soluble in water.



1. Most ionic compounds containing phosphate ion are insoluble in water.

2. Most ionic compounds containing potassium ion are insoluble in water.

3. Most ionic compounds containing hydroxide ion are soluble in water.


____ 12. Which of the following compounds are soluble in water: K2CO3, CaCO3, NiCO3, and Fe2(CO3)3?

a. K2CO3 only b. K2CO3 and CaCO3 c. CaCO3 and NiCO3 d. NiCO3 and Fe2(CO3)3 e. CaCO3, NiCO3,

and Fe2(CO3)3

____ 13. All of the following compounds are insoluble in water except ____.

a. BaCO3 b. PbF2 c. Fe(OH)3 d. Ni(ClO4)2 e. PbCrO4

____ 14. A precipitate will form when aqueous Pb(NO3)2 is added to an aqueous solution of ____.

a. Cu(NO3)2 b. NaI c. NaCH3CO2 d. Pb(ClO4)2 e. KNO3

____ 15. A precipitate will form when aqueous nickel(II) chloride is added to an aqueous solution of ____.a. SrI2 b. Cu(NO3)2 c. KOH d. Na2SO4 e. NaBr

____ 16. If an aqueous solution of ____ is added to a mixture of Pb2+ and Ba2+, the lead ion will precipitate, but the

barium ion will remain in solution.

a. NaOH b. Na2SO4 c. K3PO4 d. KCO3 e. Ca(CH3CO2)2



____ 17. If an aqueous solution of ____ is added to a mixture of F– and SO4

2–, the fluoride ion will precipitate, but the

sulfate ion will remain in solution.

a. LiBr b. HNO3 c. Pb(ClO4)2 d. MgNO3 e. AlCl3

____ 18. Write a balanced chemical equation for the reaction of aqueous solutions of sodium sulfide and zinc(II)

chloride.

a. Na2S(aq) + ZnCl2(aq)→ ZnS(s) + 2 NaCl(aq) b. Na2S(aq) + ZnCl2(aq)→ ZnS(s) + 2 NaCl(s)

c. Na2S(aq) + ZnCl2(aq)→ Na2Zn(s) + SCl2(aq) d. Na2S(aq) + ZnCl2(aq)→ Na2Zn(aq) + SCl2(g) e. No

reaction occurs.

____ 19. Write a balanced chemical equation for the reaction of aqueous solutions of magnesium chloride and

potassium phosphate.

a. MgCl2(aq) + K3PO4(aq)→ K3Mg(s) + PO4Cl2(aq) b. 3 MgCl2(aq) + 2 K3PO4(aq)→ 3 K2Mg(s) + 2

PO4Cl3(aq) c. MgCl(aq) + KPO4(aq)→ MgPO4(s) + KCl(aq) d. MgCl2(aq) + 2 KPO4(aq)→ Mg(PO4)2(s)

+ 2 KCl(aq) e. 3 MgCl2(aq) + 2 K3PO4(aq)→ Mg3(PO4)2(s) + 6 KCl(aq)

____ 20. What is the net ionic equation for the reaction of aqueous nickel(II) acetate and aqueous sodium carbonate?

a. Ni

2+

(aq) + 2 CH3CO2

–

(aq)→

Ni(CH3CO2)2(s) b. Na

+

(aq) + CH3CO2

–

(aq)→

NaCH3CO2(aq) c. Na

+

(aq)+ CH3CO2

–(aq) → NaCH3CO2(s) d. Ni2+(aq) + CO32–(aq)→ NiCO3(s) e. Ni2+(aq) + 2 Na+(aq)→

NiNa2(s)

____ 21. What is the net ionic equation for the reaction of aqueous sodium hydroxide and aqueous iron(II) chloride?

a. Na+(aq) + OH–(aq)→ NaOH(s) b. Na+(aq) + Cl–(aq)→ NaCl(s) c. Fe2+(aq) + 2 OH–(aq)→

Fe(OH)2(s) d. Fe2+(aq) + OH–(aq) → FeOH+(s) e. Fe2+(aq) + 2 Cl–(aq)→ FeCl2(s)

____ 22. Which of the following compounds is a weak acid?

a. HCl b. H3PO4 c. HNO3 d. HClO4 e. H2SO4

____ 23. Which of the following compounds is a weak base?

a. NaOH b. H2CO3 c. LiCl d. NH3 e. CH3CO2H

____ 24. Sulfuric acid is the product of the reaction of ____ and H2O.a. SO3 b. SO2 c. S8 d. H2S e. SO4

2–

____ 25. Write a balanced equation for the reaction that occurs when hydrogen sulfate ion behaves as a

Brønsted-Lowry acid in water.

a. HSO4–(aq) + H2O( ) H2SO4(aq) + H3O

+(aq) b. SO4

2–(aq) + H2O( ) HSO4

–(aq) + OH

–(aq)

c. HSO4–(aq) + H2O( ) SO4

2–(aq) + H3O+(aq) d. HSO4

–(aq) + H2O( ) H2SO4(aq) + OH–(aq)

e. H2SO4(aq) + H2O( ) HSO4–(aq) + H3O

+(aq)

____ 26. What is the balanced equation for carbonate ion (CO3

2–) acting as a Brønsted base in a reaction with water?

a. CO32–(aq) + 3 H2O( ) CO4

4–(aq) + 2 H3O+(aq) b. CO32–(aq) + H2O( ) HCO3

–(aq) + OH–(aq)c. CO3

2–(aq) + H2O( ) CO2(g) + 2 OH–(aq) d. CO32–(aq) + 2 H2O( ) HCO3

–(aq) + H3O+(aq)

e. CO32–(aq) + H2O( ) H2CO4

2–(aq)

____ 27. What is the net ionic equation for the reaction of aqueous hydrochloric acid and aqueous potassium

hydroxide?

a. HCl(aq) + OH–(aq)→ H2O( ) + Cl–(aq) b. Cl–(aq) + K+(aq)→ KCl(s) c. HCl(aq) + KOH(aq)→

KCl(aq) + H2O( ) d. Cl–(aq) + K+(aq)→ KCl(aq) e. H+(aq) + OH–(aq)→ H2O( )



____ 28. What are the spectator ions in the reaction between aqueous hydrobromic acid and aqueous sodium

hydroxide?

a. Na+ only b. H

+ and OH

–c. Na

+ and Br

–d. Br

– only e. H

+, Br

–, Na

+, and OH

–

____ 29. What are the spectator ions in the reaction between aqueous nitric acid and ammonia?

a. H+ only b. NO3– only c. H+ and NH4

+ d. NO3– and NH4

+ e. H+, NO3–, and NH4

+

____ 30. Which of the following compounds will produce a basic solution when dissolved in water?a. CaO b. NaHSO4 c. CO2 d. SO2 e. KCl

____ 31. Metal oxides react with water to produce ____.

a. bases b. hydrogen gas c. oxygen gas d. acids e. hydronium ions

____ 32. Write a balanced net ionic equation for the reaction of calcium sulfide and aqueous nitric acid.

a. CaS(s) + 2 H+(aq)→ Ca2+(aq) + S2–(aq) + H2(g) b. CaS(s) + 2 H+(aq)→ Ca2+(aq) + H2S(g) c. CaS(s) +

2 HNO3(aq) → Ca(NO3)2(aq) + H2S(g) d. CaS(s) + 2 HNO3(aq) → Ca(NO3)2(s) + H2S(s) e. S2−(aq) + 2

H

+

(aq)→

H2S(g) ____ 33. Write a balanced chemical equation for the reaction of aqueous solutions of ammonium sulfate and sodium

hydroxide.

a. (NH4)2SO4(aq) + 2 NaOH(aq) → 2 NH4OH(aq) + SO3(g) + Na2O(aq) b. (NH3)2SO4(aq) + NaOH(aq) → 2

NH3(g) + NaOHSO4(aq) c. (NH3)2SO4(aq) + 2 NaOH(aq) → 2 NH3(g) + Na2SO4(aq) + 2 OH−

(aq)

d. (NH4)2SO4(aq) + 2 NaOH(aq) → 2 NH4+(g) + Na2SO4(aq) + 2 OH

−

(aq) e. (NH4)2SO4(aq) + 2 NaOH(aq)

→ 2 NH3(g) + 2 H2O( ) + Na2SO4(aq)

____ 34. Which molecule in the reaction below is the oxidizing agent?

2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(g)

a. C2H6 b. O2 c. H2O d. CO2 e. None

____ 35. Which species in the reaction below undergoes reduction?

H2O(g) + CO(g) → H2(g) + CO2(g)

a. H2O b. CO c. H2 d. CO2 e. None

____ 36. Which species is reduced in the reaction below?

I–(aq) + ClO

–(aq)→ IO

–(aq) + Cl

–(aq)

a. I–

b. H2O c. Cl–

d. IO–

e. ClO–

____ 37. What is the oxidation number of iodine in potassium iodate, KIO3?

a. –1 b. 0 c. +3 d. +5 e. +7

____ 38. What is the oxidation number of sulfur in sulfur in H2S?

a. –2 b. 0 c. +2 d. +4 e. +6

____ 39. What is the oxidation number of each atom in sulfurous acid, H2SO3?

a. H = +1, S = –2, O = –2 b. H = 0, S = +6, O = –2 c. H = 0, S = 0, O = 0 d. H = +1, S = +4, O = –2

e. H = –1, S = +8, O = –2



____ 40. What is the oxidation number of each atom in sodium hydrogen carbonate, NaHCO3?a. Na = +1, H = –1, C = +6, O = –2 b. Na = +1, H = +1, C = +4, O = –2 c. Na = +1, H = –1, C = +2, O =

–2 d. Na = –1, H = +1, C = 0, O = –2 e. Na = 0, H = 0, C = 0, O = 0

____ 41. Which of the following elements generally acts as an oxidizing agent?

a. Br2 b. H2 c. Fe d. C e. Li

____ 42. Which of the following chemical equations show oxidation-reduction reactions?

1. Mg(s) + I2(aq)→ MgI2(s)

2. Pb(ClO4)2(aq) + 2 KI(aq) → PbI2(s) + 2 KClO4(aq)

3. Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g)

a. 1 only b. 2 only c. 1 and 2 d. 1 and 3 e. 2 and 3

____ 43. Which of the following chemical equations is an acid-base reaction?

a. Ba(OH)2(aq) + K2SO4(aq)→ BaSO4(s) + 2 KOH(aq) b. 3 NaOH(aq) + AlCl3(aq) → Al(OH)3(s) + 3

NaCl(aq) c. 2 H+(aq) + Zn(s) → H2(g) + Zn2+(aq) d. 2 HCl(aq) + Pb(NO3)2(aq)→ PbCl2(s) + 2 HNO3(aq)

e. H3PO4(aq) + NH3(aq)→

NH4

+

(aq) + H2PO4

−

(aq)

____ 44. All of the following are oxidation-reduction reactions EXCEPT

a. CaCO3(s)→ CaO(s) + CO2(g) b. 2 Na(s) + Br2(g)→ 2 NaBr(g) c. Fe(s) + 2 HCl(aq)→ FeCl2(aq) +

H2(g) d. 2 C(s) + O2(g)→ 2 CO(g) e. 2 H2O( ) → 2 H2(g) + O2(g)

Short Answer

45. A(n) ________ agent loses electrons in an oxidation-reduction reaction.

46. ________ acid is produced in a larger quantity than any other chemical in the United States. This chemical is

used in the production of fertilizers, pigments, alcohol, paper and detergents. 47. The net ionic equation for the reaction of barium chloride and sodium sulfate is shown below.

Ba2+

(aq) + SO42–

(aq)→ BaSO4(s)

Chloride and sodium ions are referred to as ________ ions because they are not involved in the reaction.

48. A solution is a homogeneous mixture composed of one or more ____________ dissolved in a solvent.

49. Give the name of an acidic oxide and write a balanced chemical equation for the reaction of the oxide with

water.

50. If an aqueous sodium hydroxide solution is left in contact with air, the concentration of hydroxide ion

gradually decreases. The process can be hastened if a person exhales over a sodium hydroxide solution. Writea balanced chemical equation that describes the process by which the hydroxide ion concentration decreases.



Ch. #3 Study Guide

Answer Section

MULTIPLE CHOICE

1. D

2. D

3. B

4. B

5. C

6. E

7. E

8. A

9. C

10. A

11. A 12. A

13. D

14. B

15. C

16. A

17. D

18. A

19. E

20. D

21. C

22. B 23. D

24. A

25. C

26. B

27. E

28. C

29. B

30. A

31. A

32. B

33. E 34. B

35. A

36. E

37. D

38. A

39. D

40. B



41. A

42. D

43. E

44. A

SHORT ANSWER

45. reducing

46. Sulfuric

47. spectator

48. solutes

49. Sulfur dioxide. SO2(g) + H2O( )→ H2SO3(aq). Other examples include carbon dioxide forming carbonic

acid, sulfur trioxide forming sulfuric acid, and nitrogen dioxide forming a mixture of nitrous acid and nitric

acid.

50. OH–(aq) + CO2(aq)→ HCO3

–(aq)

Ch 03 Study Guide

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