Ch.4

Question 1

Based on the solubility rules, which one of the following compounds should be insoluble in water?
A. NaCl
B. MgBr2
C. FeCl2
D. AgBr
E. ZnCl2

Answer 1

D

Question 2

Based on the solubility rules, which of the following compounds should be insoluble in water?
A. Na2SO4
B. BaSO4
C. CuSO4
D. MgSO4
E. Rb2SO4

Answer 2

B

Question 3

Based on the solubility rules, which of the following compounds should be insoluble in water?
A. CaCO3
B. (NH4)2CO3
C. Na2CO3
D. K2CO3
E. KNO3

Answer 3

A

Question 4

Based on the solubility rules, which of the following should be soluble in water?
A. Hg2Cl2
B. Na2S
C. Ag2CO3
D. Ag2S
E. BaSO4

Answer 4

B

Question 5

Based on the solubility rules, which of the following should be soluble in water?
A. AgBr
B. AgCl
C. Ag2CO3
D. AgNO3
E. Ag2S

Answer 5

D

Question 6

Based on the solubility rules, which of the following should be soluble in water?
A. (NH4)3PO4
B. Ca3(PO4)2
C. AlPO4
D. Ag3PO4
E. Mg3(PO4)2

Answer 6

A

Question 7

Based on the solubility rules, which of the following should be soluble in water?
A. CaSO4
B. BaSO4
C. PbSO4
D. K2SO4
E. AgCl

Answer 7

D

Question 8

Which of the following will occur when a solution of Pb(NO3)2(aq) is mixed with a solution of KI(aq)?
A. A precipitate of KNO3 will form; Pb2+ and I– are spectator ions.
B. No precipitate will form.
C. A precipitate of Pb(NO3)2 will form; K+ and I– are spectator ions.
D. A precipitate of PbI2 will form; K+ and NO3– are spectator ions.
E. A precipitate of PbI2 will form; Pb2+ and I– are spectator ions.

Answer 8

D

Question 9

Which of the following will occur when solutions of CuSO4(aq) and BaCl2(aq) are mixed?
A. A precipitate of CuCl2 will form; Ba2+ and SO42– are spectator ions.
B. A precipitate of CuSO4 will form; Ba2+ and Cl– are spectator ions.
C. A precipitate of BaSO4 will form; Cu2+ and Cl– are spectator ions.
D. A precipitate of BaCl2 will form; Cu2+ and SO42– are spectator ions.
E. No precipitate will form.

Answer 9

C

Question 10

Which of the following will occur when solutions of ZnSO4(aq) and MgCl2(aq) are mixed?
A. A precipitate of ZnCl2 will form; Mg2+ and SO42– will be spectator ions.
B. A precipitate of ZnSO4 will form ; Mg2+ and Cl– will be spectator ions.
C. A precipitate of MgSO4 will form ; Zn2+ and Cl– will be spectator ions.
D. A precipitate of MgCl2 will form ; Zn2+ and SO42– will be spectator ions.
E. No precipitate will form.

Answer 10

E

Question 11

Identify the precipitate(s) formed when solutions of Na2SO4(aq), Ba(NO3)2(aq), and NH4ClO4(aq) are mixed.
A. Ba(ClO4)2
B. BaSO4 and (NH4)2SO4
C. NH4NO3 and NaClO4
D. BaSO4
E. NaClO4

Answer 11

D

Question 12

Identify the precipitate(s) formed when solutions of NH4Cl(aq), AgClO3(aq), and NaCl(aq) are mixed.
A. AgCl
B. AgCl and NH4ClO3
C. NH4Cl and NaClO3
D. NH4ClO3
E. AgNH4

Answer 12

A

Question 13

Identify the precipitate(s) formed when solutions of Ca(ClO4)2(aq), K2CO3(aq), and NaNO3(aq) are mixed.
A. CaCO3
B. Na2CO3
C. Ca(NO3)2 and NaClO4
D. CaCO3 and Na2CO3
E. KClO4 and Ca(NO3)2

Answer 13

A

Question 14

Identify the precipitate(s) formed when solutions of Pb(NO3)2(aq), Mg(ClO4)2(aq), and (NH4)2SO4(aq) are mixed.
A. PbSO4
B. MgSO4
C. NH4ClO4
D. NH4NO3 and NH4ClO4
E. PbSO4 and MgSO4

Answer 14

A

Question 15

Identify the correct net ionic equation for the reaction that occurs when solutions of Pb(NO3)2 and NH4Cl are mixed.
A. Pb(NO3)2(aq) + 2NH4Cl(aq)  NH4NO3(aq) + PbCl2(s)
B. Pb2+(aq) + 2Cl–(aq)  PbCl2(s)
C. Pb2+(aq) + 2NO3– (aq) + 2NH (aq) + 2Cl–(aq)  2NH (aq) + 2NO3– (aq) + PbCl2(s)
D. NH4+(aq)+ NO3– (aq)  2NH4NO3(s)
E. No reaction occurs when the solutions are mixed.

Answer 15

B

Question 16

Identify the correct net ionic equation for the reaction that occurs when solutions of AgNO3 and NH4Cl are mixed.
A. AgNO3(aq) + NH4Cl(aq)  AgCl(s) + NH4Cl(aq)
B. NH4+(aq) + NO3-(aq)  NH4NO3(s)
C. AgNO3(aq) + NH4Cl(aq)  AgCl(s) + NH4Cl(s)
D. Ag+(aq) + Cl-(aq)  AgCl(s)
E. AgNO3(aq) + NH4+(aq)  NH4AgNO3(s)

Answer 16

D

Question 17

Identify the correct net ionic equation for the reaction that occurs when solutions of Ba(ClO4)2 and K2SO4 are mixed.
A. Ba2+(aq) + SO42-(aq)  BaSO4(s)
B. 2K+(aq) + 2ClO4-(aq)  K2(ClO4)2(s)
C. K+(aq) + ClO4-(aq)  KClO4(s)
D. Ba(ClO4)2(aq) + K2SO4(aq)  BaSO4(s) + 2KClO4(s)
E. Ba2+(aq) + K+(aq) + SO42-(aq)  KBaSO4(s)

Answer 17

A

Question 18

Identify the correct net ionic equation for the reaction that occurs when solutions of Na3PO4 and Ca(NO3)2 are mixed.
A. Ca2+ + PO42-(aq)  CaPO4(s)
B. 3Ca2+(aq) + 2PO43-(aq)  Ca3(PO4)2(s)
C. Na+(aq) + NO3-  NaNO3(s)
D. Na+(aq) + Ca2+(aq) + PO43-(aq)  NaCaPO4(s)
E. 2 Na3PO4(aq) + 3Ca(NO3)2(aq)  6NaNO3(s) + Ca3(PO4)2(s)

Answer 18

B

Question 19

The common constituent in all acid solutions is
A. H2
B. H+
C. OH–
D. H2SO4
E. Cl–

Answer 19

B

Question 20

Which of the following compounds is a weak acid?
A. HF
B. HCl
C. HBr
D. HI
E. HClO4

Answer 20

A

Question 21

Which of the following compounds is a strong acid?
A. HF
B. HI
C. HClO2
D. H2SO3
E. HNO2

Answer 21

B

Question 22

Which of the following compounds is a weak base?
A. KOH
B. Sc(OH)3
C. NH3
D. NH4+
E. CO2

Answer 22

C

Question 23

Which of the following ions is a weak acid?
A. SO42-
B. H2SO4
C. HSO4-
D. HNO3
E. NO3-

Answer 23

C

Question 24

Identify the correct net ionic equation for the reaction that occurs when solutions of HNO3 and KOH are mixed?
A. HNO3(aq) + KOH(aq)  H2O(l) + KNO3(aq)
B. K+(aq) + NO3-(aq)  KNO3(aq)
C. HNO3(aq) + KOH(aq)  H2O(l) + KNO3(s)
D. H+(aq) + OH-(aq)  H2O(l)
E. HNO3(aq) + OH-(aq)  H2O(l) + NO3-(aq)

Answer 24

D

Question 25

Identify the correct net ionic equation for the reaction that occurs when solutions of HClO4 and Ba(OH)2 are mixed. A. H+(aq) + 2OH-(aq)  H2O(l) B. H+(aq) + OH-(aq)  H2O(l) C. 2HClO4(aq) + Ba(OH)2(s)  2H2O(l) + Ba(ClO4)2(aq) D. 2HClO4(aq) + Ba(OH)2(s)  2H2O(l) + Ba(ClO4)2(s) E. 2H+(aq) + Ba(OH)2(s)  2H2O(l) + Ba2+(aq)

Answer 25

B

Question 26

Identify the correct net ionic equation for the reaction that occurs when solutions of HF and KOH are mixed. A. H+(aq) + OH-(aq)  H2O(l) B. HF(aq) + OH-(aq)  H2O(l) + F-(aq) C. H+(aq) + KOH(aq)  H2O(l) + K+(aq) D. HF(aq) + KOH(aq)  H2O(l) + KF(s) E. HF(aq) + KOH(s)  H2O(l) + KF(aq)

Answer 26

B

Question 27

The oxidation number of N in NaNO3 is A. +6. B. +5. C. +3. D. –3. E. None of the above.

Answer 27

B

Question 28

The oxidation number of S in K2SO4 is A. +6. B. +4. C. +2. D. –1. E. None of the above.

Answer 28

A

Question 29

The oxidation number of Mn in KMnO4 is A. +8. B. +7. C. +5. D. –7. E. –8.

Answer 29

B

Question 30

The oxidation number of Fe in K3Fe(CN)6 is A. +3. B. +2. C. +1. D. –3. E. –4.

Answer 30

A

Question 31

The oxidation number of Cr in Cr2O72– is A. –12. B. –7. C. –2. D. +6. E. +7.

Answer 31

D

Question 32

For the chlorate ion, ClO3- , what are the oxidation states of the Cl and O, respectively? A. – 1, – 2 B. +5, – 2 C. +6, – 2 D. +7, – 2 E. +2, – 1

Answer 32

B

Question 33

For the perchlorate ion ClO4- , what are the oxidation states of the Cl and O, respectively? A. – 1, – 2 B. +8, – 2 C. +7, – 2 D. +6, – 2 E. +2, – 1

Answer 33

C

Question 34

The highest possible oxidation number of nitrogen is A. +8. B. +5. C. +3. D. +1. E. –3.

Answer 34

B

Question 35

For which one of the following acids is chlorine in the +5 oxidation state? A. HCl B. HClO C. HClO2 D. HClO3 E. HClO4

Answer 35

D

Question 36

The highest possible oxidation number of carbon is A. +8. B. +6. C. +4. D. +2. E. –4.

Answer 36

C

Question 37

Select the compound in which sulfur has its highest possible oxidation number. A. H2S B. SO2 C. SCl2 D. H2SO3 E. Na2SO4

Answer 37

E

Question 38

The oxidation number of N in N2H4 is A. +4. B. –4. C. +2. D. –2. E. 0.

Answer 38

D

Question 39

Determine the correct oxidation numbers for all three elements in Rb2SO3 in the order that the elements are shown in the formula. A. –2, +6, –2 B. –1, +4, –3 C. +2, +4, –2 D. +1, +4, –2 E. +1, +6, –6

Answer 39

D

Question 40

Determine the correct oxidation numbers for all three elements in Ca(ClO)2 in the order that the elements are shown in the formula? A. +2, +1, –2 B. +2, –2, +1 C. +2, –3, +2 D. –2, +2, –1 E. –2, +3, –2

Answer 40

A

Question 41

Using the redox reaction below determine which element is oxidized and which is reduced. 4NH3 + 3Ca(ClO)2  2N2 + 6H2O + 3CaCl2 A. H is oxidized and N is reduced B. Cl is oxidized and O is reduced C. N is oxidized and Cl is reduced D. Cl is oxidized and N is reduced E. N is oxidized and O is reduced

Answer 41

C

Question 42

How many total electrons are transferred in the following reaction? B2H6(g) + 3O2(g)  B2O3(s) + 3H2O(l) A. 2 B. 3 C. 4 D. 6 E. 12

Answer 42

E

Question 43

How many total electrons are transferred in the following reaction? 4 P(s) + 5O2(g)  2P2O5(s) A. 5 B. 10 C. 15 D. 20 E. 25

Answer 43

D

Question 44

How many total electrons are transferred in the following reaction? 2Na(s) + Cl2(g)  2NaCl(s) A. 1 B. 2 C. 3 D. 4 E. 5

Answer 44

B

Question 45

Which one of the following is a redox reaction? A. 2Al(s) + 3H2SO4(aq)  Al2(SO4)3(aq) + 3H2(g) B. 2KBr(aq) + Pb(NO3)2(aq)  2KNO3(aq) + PbBr2(s) C. CaBr2(aq) + H2SO4(aq)  CaSO4(s) + 2HBr(g) D. H+(aq) + OH– (aq)  H2O(l) E. CO32– (aq) + HSO4–(aq)  HCO3– (aq) + SO42– (aq)

Answer 45

A

Question 46

Which of the following equations does not represent an oxidation-reduction reaction? A. 3Al + 6HCl  3H2 + AlCl3 B. 2H2O  2H2 + O2 C. 2NaCl + Pb(NO3)2  PbCl2 + 3NaNO3 D. 2NaI + Br2  2NaBr + I2 E. Cu(NO3)2 + Zn  Zn(NO3)2 + Cu

Answer 46

C

Question 47

In the following chemical reaction the oxidizing agent is 5H2O2 + 2MnO4– + 6H+  2Mn2+ + 8H2O + 5O2 A. H2O2. B. MnO4–. C. H+. D. Mn2+. E. O2.

Answer 47

B

Question 48

In the following chemical reaction the oxidizing agent is 5S + 6KNO3 + 2CaCO3  3K2SO4 + 2CaSO4 + CO2 + 3N2 A. S B. N2 C. KNO3 D. CaSO4 E. CaCO3

Answer 48

C

Question 49

Identify the oxidizing agent in the following chemical reaction. 2MnO4– + 5H2SO3  2Mn2+ + 5SO42– + 4H+ + 3H2O A. MnO4– B. H2SO3 C. Mn2+ D. SO42– E. H+

Answer 49

A

Question 50

Identify the reducing agent in the following chemical reaction. 5Fe2+(aq) + MnO4–(aq)+ 8H+(aq)  5Fe3+(aq) + Mn2+(aq) + 4H2O(l) A. Fe2+ B. MnO4– C. H+ D. Mn2+ E. Fe3+

Answer 50

A

Question 51

Identify the reducing agent in the following chemical reaction. Cd + NiO2 + 2H2O  Cd(OH)2 + Ni(OH)2 A. Cd B. NiO2 C. H2O D. Cd(OH)2 E. Ni(OH)2

Answer 51

A

Question 52

What element is oxidized in the following chemical reaction? 3Cu + 8HNO3  3Cu(NO3)2 + 2NO + 4H2O A. Cu B. H C. N D. O E. H2O

Answer 52

A

Question 53

What element is oxidized in the following chemical reaction? NiO2 + Cd + 2H2O  Ni(OH)2 + Cd(OH)2 A. Ni B. Cd C. O D. H E. This is not a redox reaction.

Answer 53

B

Question 54

What element is oxidized in the following chemical reaction? H2SO4 + Cd(OH)2  2H2O + CdSO4 A. H B. S C. O D. Cd E. this is not a redox reaction

Answer 54

E

Question 55

What element is reduced in the following chemical reaction? Cu + 2H2SO4  CuSO4 + SO2 + 2H2O A. Cu B. H C. S D. O E. H2O

Answer 55

C

Question 56

Identify the elements that are oxidized and reduced in the following reaction. KClO3(aq) + 6HBr(aq)  KCl(aq) + 3Br2(l) + 3H2O(l) A. Br is oxidized and Cl is reduced B. Cl is oxidized and H is reduced C. H is oxidized and O is reduced D. O is oxidized and Cl is reduced E. Cl is oxidized and Br is reduced

Answer 56

A

Question 57

Predict the products of the following single replacement reaction. Fe(s) + CuSO4(aq)  A. Cu(s) + FeSO4(aq) B. Fe(s) + Cu(s) + SO4(aq) C. CuS(s) + Fe2SO4(aq) D. FeCuSO4(aq) E. FeO(s) + CuSO3(aq)

Answer 57

A

Question 58

Predict the products of the following single replacement reaction. Zn(s) + CoCl2(aq)  A. No reaction occurs B. Co(s) + ZnCl2(aq) C. CoCl(aq) + ZnCl(aq) D. ZnCo(aq) + Cl2(g) E. ZnCoCl2(aq)

Answer 58

B

Question 59

Predict the products of the following single replacement reaction. Ni(s) + Cu(NO3)2(aq)  A. No reaction occurs B. NiNO3(aq) + CuNO3(aq) C. NiCu(aq) 2 NO3-(aq) D. Ni(NO3)2(aq) + Cu(s) E. Ni(NO3)2(aq) + Cu2+(aq)

Answer 59

D

Question 60

Which of the following is an example of a disproportionation reaction? A. 2C2H6(g) + 7O2(g)  4CO2(g) + 6H2O(l) B. 2KBr(aq) + Cl2(g)  2KCl(aq) + Br2(l) C. 2H2O2(aq)  2H2O(l) + O2(g) D. CaBr2(aq) + H2SO4(aq)  CaSO4(s) + 2HBr(g) E. 2Al(s) + 3H2SO4(aq)  Al2(SO4)3(aq) + 3H2(g)

Answer 60

C

Question 61

Which of the following is NOT a redox reaction? A. 2NaN3(s)  2Na(s) + 3N2(g) B. Fe2O3(s) + 2Al(s)  2Fe(s) + Al2O3(s) C. 3NO2(g) + H2O(l)  2HNO3(aq) + NO(g) D. NH4Cl(aq) + AgNO3  NH4NO3(aq) + AgCl(s) E. 2ZnS(s) + 3O2(g)  2ZnO(s) + 2SO2(g)

Answer 61

D

Question 62

Which of the following is NOT a redox reaction? A. 2KBr(aq) + Cl2(g)  2KCl(aq) + Br2(l) B. 2Na(s) + 2H2O(l)  2NaOH(aq) + H2(g) C. V2O5(s) + 5 Ca(l)  2 V(l) + 5 CaO(s) D. 2KNO3(s)  2KNO2(s) + O2(g) E. 2LiOH(aq) + H2SO4(aq)  Li2SO4(aq) + 2H2O(l)

Answer 62

E

Question 63

Which of the following represents a precipitation reaction? A. 2H2(g) + O2(g)  2H2O(l) B. CaBr2(aq) + H2SO4(aq)  CaSO4(s) + 2HBr(g) C. 2KNO3(s)  2KNO2(s) + O2(g) D. 2KBr(aq) + Cl2(g)  2KCl(aq) + Br2(l) E. 2Al(s) + 3H2SO4(aq)  Al2(SO4)3(aq) + 3H2(g)

Answer 63

B

Question 64

Which of the following represents a precipitation reaction? A. 2H2(g) + O2(g)  2H2O(l) B. CaBr2(aq) + H2SO4(aq)  CaSO4(s) + 2HBr(g) C. 2KNO3(s)  2KNO2(s) + O2(g) D. 2KBr(aq) + Cl2(g)  2KCl(aq) + Br2(l) E. 2Al(s) + 3H2SO4(aq)  Al2(SO4)3(aq) + 3H2(g)

Answer 64

B

Question 65

Which of the following represents an acid-base neutralization reaction? A. 2Al(s) + 3H2SO4(aq)  Al2(SO4)3(aq) + 3H2(g) B. SO2(g) + H2O(l)  H2SO3(g) C. LiOH(aq) + HNO3(aq)  LiNO3(aq) + H2O(l) D. 2KBr(aq) + Cl2(g)  2KCl(aq) + Br2(l) E. CaBr2(aq) + H2SO4(aq)  CaSO4(s) + 2HBr(g)

Answer 65

C

Question 66

Which of the following represents a hydrogen displacement reaction? A. 2C2H6(g) + 7O2(g)  4CO2(g) + 6H2O(l) B. 2KBr(aq) + Cl2(g)  2KCl(aq) + Br2(l) C. N2(g) + 3H2(g)  2NH3(g) D. CaBr2(aq) + H2SO4(aq)  CaSO4(s) + 2HBr(g) E. 2Al(s) + 3H2SO4(aq)  Al2(SO4)3(aq) + 3H2(g)

Answer 66

E

Question 67

Which of the following represents a combustion reaction? A. 2C2H6(g) + 7O2(g)  4CO2(g) + 6H2O(l) B. LiOH(aq) + HNO3(aq)  LiNO3(aq) + H2O(l) C. N2(g) + 3H2(g)  2NH3(g) D. 2Na(s) + 2H2O(l)  2NaOH(aq) + H2(g) E. 2Al(s) + 3H2SO4(aq)  Al2(SO4)3(aq) + 3H2(g)

Answer 67

A

Question 68

What type of reaction is the following? Ca(OH)2(s) + 2 HNO3(aq)  Ca(NO3)2(aq) + 2 H2O(l) A. Combination reaction B. Acid-base neutralization reaction C. Hydrogen displacement reaction D. Disproportionation reaction E. Combustion reaction

Answer 68

B

Question 69

What type of reaction is the following? C2H4(g) + 3 O2(g)  2 CO2(g) + 2 H2O(g) A. Combination reaction B. Acid-base neutralization reaction C. Hydrogen displacement reaction D. Disproportionation reaction E. Combustion reaction

Answer 69

E

Question 70

The reaction below can be classified as which type of reaction ? 2 NO2(g) + H2O(l)  HNO2(aq) + HNO3(aq) A. Combination reaction B. Acid-base neutralization reaction C. Hydrogen displacement reaction D. Disproportionation reaction E. Combustion reaction

Answer 70

D

Question 71

Select True or False: Al(NO3)3 is a strong electrolyte.

Answer 71

TRUE

Question 72

Select True or False: NH4NO3 is a weak electrolyte.

Answer 72

FALSE

Question 73

Select True or False: H3PO4 is a weak electrolyte.

Answer 73

TRUE

Question 74

Select True or false: H2CO3is a weak electrolyte.

Answer 74

TRUE

Question 75

Select True or False: CH3OH (methanol) is a weak electrolyte.

Answer 75

FALSE

Question 76

Select True or False: CH3COOH is a weak electrolyte.

Answer 76

TRUE

Question 77

Select True or False: NH3 is a weak electrolyte.

Answer 77

TRUE

Question 78

Select True or False: NH4Cl is a nonelectrolyte.

Answer 78

FALSE

Question 79

What compound is formed, as a precipitate, when solutions of Na3PO4(aq), Ca(NO3)2(aq), and NH4ClO3(aq) are mixed? A. Ca2(PO4)2 B. Ca3(PO4)2 C. Ca3PO4 D. CaPO4 E. None of the above

Answer 79

B

Question 80

What compound is formed, as a precipitate, when solutions of Hg2(ClO4)2(aq), (NH4)2SO4(aq), and Rb2SO4(aq) are mixed? A. RbClO4 B. Rb2(ClO4)3 C. Hg2SO4 D. HgSO4 E. None of the above

Answer 80

C

Question 81

What compound is formed, as a precipitate, when solutions of NaOH(aq), Ca(ClO3)2(aq), and Ba(OH)2(aq) are mixed? A. CaClO3 B. Ba(OH)2 C. NaClO3 D. Ca(OH)2 E. None of the above

Answer 81

D

Question 82

Select True or False: HNO3 is an example of a monoproticacid.

Answer 82

TRUE

Question 83

Select True or False: H2CO3 is an example of a diproticacid.

Answer 83

TRUE

Question 84

Of the following, which is NOT an example of a strong acid? A. hydrochloric acid, HCl B. hydroiodic acid, HI C. carbonic acid, H2CO3 D. perchloric acid, HClO4 E. nitric acid, HNO3

Answer 84

C

Question 85

Select True or False: Na3PO4 is an example of a triproticacid.

Answer 85

FALSE

Question 86

Which of the following, if any, is the correctly balanced net ionic equation for reaction that occurs when aqueous iron(III) sulfate is added to aqueous sodium sulfide to produce solid iron(III) sulfide and aqueous sodium sulfate. A. Fe3+(aq) + 3S2– (aq)  FeS3(s) B. 2Fe3+(aq) + S2– (aq)  Fe2S (s) C. 2Fe3+(aq) + 3S2– (s)  Fe2S3(aq) D. 2Fe3+(aq) + 3S2– (aq)  Fe2S3(s) E. None of the above

Answer 86

D

Question 87

In this compound what is the correct representation for the oxidation number of each of the elements in Cs2Cr2O7? A. +1; +6; -2 B. +2; +4; -2 C. +1; +4; -2 D. +3; +6; -2 E. -1; +6; -2

Answer 87

A

Question 88

Select True or False: Al is being oxidized in the following reaction. 4Al + 3O2  2Al2O3

Answer 88

TRUE

Question 89

Select True or False: Oxygen is the element being reduced in the following reaction. 4Al + 3O2  2Al2O3

Answer 89

TRUE

Question 90

Select True or False: Al is the oxidizing agent in the following reaction. 4Al + 3O2  2Al2O3

Answer 90

FALSE

Question 91

Select True or False: Al is the reducing agent in the following reaction. 4Al + 3O2  2Al2O3

Answer 91

TRUE

Question 92

Select True or False: K is element being oxidized in the following reaction. 2KBr + F2  Br2 + 2KF

Answer 92

FALSE

Question 93

Select True or False: Fluorine is the element being reduced in the following reaction. 2KBr + F2  Br2 + 2KF

Answer 93

TRUE

Question 94

Select True or False: Fluorine is the oxidizing agent in the following reaction. 2KBr + F2  Br2 + 2KF

Answer 94

TRUE

Question 95

Select True or False: Fluorine is the reducing agent in the following reaction. 2KBr + F2  Br2 + 2KF

Answer 95

FALSE

Question 96

Which represents the oxidation number of each of the elements in BaNaPO4? A. +2; +1; +4; -2 B. +1; +1; -5; -2 C. +2; +4; +5; +2 D. +2; +1; +5; -2 E. +1; +2; +5; -2

Answer 96

D

Question 97

Determine the oxidation number of each of the elements in NaAl(OH)4? A. +1; +3; -2; +1 B. +1; +1; -2; +1 C. +2; +3; -1; +1 D. +1; +3; -2; -1 E. None of the above

Answer 97

A

Question 98

Select True or False: Thorium +4 is reduced in this process. (Thorium metal is prepared by reacting thorium oxide with calcium as shown below.) ThO2 + 2Ca  Th + 2CaO

Answer 98

TRUE

Question 99

Select True or False: Th+4 is the reducing agent in this process. (Thorium metal is prepared by reacting thorium oxide with calcium as depicted below.) ThO2 + 2Ca  Th + 2CaO

Answer 99

FALSE

Question 100

Select True or False: Ca is oxidized in this process. (Thorium metal is prepared by reacting thorium oxide with calcium as shown below.) ThO2 + 2Ca  Th + 2CaO

Answer 100

TRUE

Question 101

Select True or False: Ca is the oxidizing agent in this process. (Thorium metal is prepared by reacting thorium oxide with calcium as shown below.) ThO2 + 2Ca  Th + 2CaO

Answer 101

FALSE

Question 102

Select True or False: H2SO4 is reduced in this process. (Batteries in our cars generate electricity by the following chemical reaction.) Pb + PbO2 + 2H2SO4  2PbSO4 + 2H2O

Answer 102

FALSE

Question 103

Select True or False: Pb is the reducing agent in this process. (Batteries in our cars generate electricity by the following chemical reaction.) Pb + PbO2 + 2H2SO4  2PbSO4 + 2H2O

Answer 103

TRUE

Question 104

Select True or False: PbO2 is oxidized in this process. (Batteries in our cars generate electricity by the following chemical reaction.) Pb + PbO2 + 2H2SO4  2PbSO4 + 2H2O

Answer 104

FALSE

Question 105

Select True or False: Pb is the oxidizing agent in this process. (Batteries in our cars generate electricity by the following chemical reaction.) Pb + PbO2 + 2H2SO4  2PbSO4 + 2H2O

Answer 105

FALSE

Question 106

Decide which category to place the following reaction: acid-base neutralization, precipitation, combination, decomposition, combustion, displacement, or disproportionation reaction. CH4(g) + 2 O2(g)  CO2(g) + 2 H2O(g) A. Acid-Base Neutralization B. Precipitation C. Decomposition D. Combustion E. Displacement

Answer 106

D

Question 107

Categorize the following reaction as an acid-base neutralization, precipitation, combination, decomposition, combustion, displacement, or disproportionation reaction. Ba(C2H3O2)2(aq) + Na2CO3(aq)  BaCO3(s) + 2 NaC2H3O2(aq) A. Acid-Base Neutralization B. Precipitation C. Decomposition D. Combustion E. Disproportionation

Answer 107

B

Question 108

Categorize the following reaction as an acid-base neutralization, precipitation, combination, decomposition, combustion, displacement, or disproportionation reaction. 2KClO3(s)  2KCl(s) + 3O2(g) A. Acid-Base Neutralization B. Combination C. Decomposition D. Combustion E. Displacement

Answer 108

C

Question 109

Categorize the following reaction as an acid-base neutralization, precipitation, combination, decomposition, combustion, displacement, or disproportionation reaction. H2SO4(aq) + 2 KOH(aq)  2 H2O(l) + K2SO4(aq) A. Acid-Base Neutralization B. Precipitation C. Decomposition D. Combustion E. Displacement

Answer 109

A

Question 110

Which substance is acting as a Brønsted acid in the following reaction? HSO4– + NH4+  H2SO4 + NH3 A. HSO4– B. NH4+ C. H2SO4 D. NH3 E. Both HSO4– and NH4+

Answer 110

B

Question 111

Select True or False: H2O is acting as a Brønsted acid in the following reaction. NH3 +H2ONH4+ +OH–

Answer 111

TRUE

Question 112

Shown here is the balanced molecular equation that would occur between CaCl2(aq) and Na2CO3(aq). Which of the following is the balanced net ionic equation? Molecular equation: CaCl2(aq) + Na2CO3(aq)  CaCO3(s) + 2NaCl(aq) A. Net ionic equation: Ca2+(aq) + 2 Cl–(aq)  CaCO3(s) B. Net ionic equation: Ca2+(aq) + CO32–(aq)  Ca2+(aq) + CO3(aq) C. Net ionic equation: Ca2+(aq) + CO32–(aq)  CaCO3(s) D. Net ionic equation: 2Na+(aq) + CO32–(aq)  Na2CO3(s) E. None of the above

Answer 112

C

Question 113

True or False: The two reactions shown here represent balanced molecular and net ionic reactions for the acid-base neutralization reaction between H3PO4(aq) and Ba(OH)2(aq). Molecular equation: 2H3PO4(aq) + 3Ba(OH)2(aq)  Ba3(PO4)2(s) + 6H2O(l) Net ionic equation: 2H3PO4(aq) + 3Ba2+(aq) + 6OH–(aq)  Ba3(PO4)2(s) + 6H2O(l)

Answer 113

TRUE

Question 114

Select True or False: The following two equations show both the correct balanced molecular and net ionic equations for the reaction that would occur between Al(s) and Co(NO3)2(aq). Molecular equation: 2Al(s) + 3Co(NO3)2(aq)  2Al(NO3)3(aq) + 3Co(s) Net ionic equation: 2Al(s) + Co2+(aq)  2Al3+(aq) + Co(s)

Answer 114

FALSE

Question 115

Shown here is the balanced molecular equation for the reaction that would occur between CuCl2(aq) and Pb(s). Which of the following, if any, shows the correctly balanced net ionic equation? Molecular equation: CuCl2(aq) + Pb(s)  Cu(s) + PbCl2(s) A. Net ionic equation: Cu2+(aq) + 2Cl–(aq) + Pb(s)  Cu(s) + Pb2+ (aq) + 2 Cl-(aq) B. Net ionic equation: 2Cu2+(aq) + 2Cl–(aq) + Pb(s)  2Cu(s) + PbCl2(s) C. Net ionic equation: Cu2+(aq) + Pb(s)  Cu(s) + Pb2+(aq) D. Net ionic equation: Cu2+(aq) + 2Cl–(aq) + Pb(s)  Cu(s) + PbCl2(s) E. None of the above

Answer 115

D

Question 116

A piece of copper metal was added to an aqueous solution of silver nitrate, and within a few minutes it was observed that a grey crystalline solid formed on surface of the copper. The solution turned a blue color characteristic of copper(II) ions. Select the correct balanced chemical equation for this reaction. A. Cu(s) + AgNO3(aq)  Ag(s) + Cu(NO3)2(aq) B. Cu(s) + AgNO3(aq)  Ag(s) + Cu(NO3)2(aq) C. Cu(s) + 2AgNO3(aq)  2Ag(s) + Cu(NO3)2(aq) D. 2Cu(s) + 2AgNO3(aq) 2Ag(s) + 2Cu(NO3)2(aq) E. None of the above

Answer 116

C

Question 117

A piece of copper metal was added to an aqueous solution of silver nitrate, and within a few minutes it was observed that a grey crystalline solid formed on surface of the copper. The solution turned a blue color characteristic of copper(II) ions. Select the correct net ionic equation for this reaction. A. Cu(s) + Ag+(aq)  Cu2+(aq) + Ag(s) B. Cu(s) + 2Ag+(aq)  Cu2+(aq) + 2Ag(s) C. Cu(aq) + 2Ag+(aq) Cu2+(aq) + 2Ag(aq) D. 2Cu(s) + Ag+(aq)  2Cu2+(aq) + Ag(s) E. None of the above

Answer 117

B

Question 118

A piece of lead metal was added to an aqueous solution of copper(II) nitrate, and within a few minutes it was observed that the lead turned black and crumbled. The characteristic blue solution of copper (II) ions had faded. (NOTE: Lead forms a 2+ ion when it reacts.) Select the balanced chemical equation for this reaction. A. Pb(s) + CuNO3(aq)  Cu(s) + Pb(NO3)2(aq) B. 2Pb(s) + Cu(NO3)2(aq) Cu(s) + 2Pb(NO3)2(aq) C. Pb(s) + Cu(NO3)2(aq) 2 Cu(s) + Pb(NO3)2(aq) D. Pb(s) + Cu(NO3)2(aq)  Cu(s) + Pb(NO3)2(aq) E. None of the above

Answer 118

D

Question 119

Select True or False: The following net ionic equation correctly shows the result of this experiment: A piece of lead metal was added to an aqueous solution of copper(II) nitrate, and within a few minutes it was observed that the lead turned black and crumbled. The characteristic blue solution of copper(II) ions had faded. (NOTE: Lead forms a 2+ ion when it reacts.) Pb(s) + Cu2+(aq)  Pb2+(aq) + Cu(s)

Answer 119

TRUE

Question 120

A piece of zinc metal was added to an aqueous solution of lead(II) nitrate. After some time it was observed that the zinc metal appeared to fall apart and a solid had accumulated at the bottom of the reaction vessel. Select the balanced chemical equation for this reaction. A. Zn(s) + Pb(NO3)2(aq)  Pb(s) + Zn(NO3)2(aq) B. 2Zn(s) + Pb(NO3)2(aq) Pb(s) + 2Zn(NO3)2(aq) C. Zn(s) + 2Pb(NO3)2(aq) Pb(s) + 2Zn(NO3)2(aq) D. Zn(s) + 3Pb(NO3)2(aq) 3Pb(s) + 3Zn(NO3)2(aq) E. None of the above

Answer 120

A

Question 121

Select True or False: The following net ionic equation correctly shows the result when a piece of zinc metal is added to an aqueous solution of lead(II) nitrate. After some time it was observed that the zinc metal appeared to fall apart and a solid had accumulated at the bottom of the reaction vessel. Zn(s) + Pb2+(aq) Zn2+(aq) + Pb(s)

Answer 121

TRUE

Question 122

The following experiments were carried out and observations recorded. Expt. #1: copper metal was added to an aqueous solution of silver nitrate Observation: The copper become coated with a substance. Expt. #2: lead metal was added to an aqueous solution of copper(II) nitrate Observation: The lead turned black and crumbled. Expt. #3: zinc metal was added to an aqueous solution of lead(II) nitrate Observation: The zinc appeared to fall apart. Which, if any, of the following properly ranks the metals from most active to least active. A. Most active Pb, next most active Zn, next most active Cu, least active Ag B. Most active Zn, next most active Ag, next most active Cu, least active Pb C. Most active Zn, next most active Cu, next most active Pb, least active Ag D. Most active Zn, next most active Pb, next most active Cu, least active Ag E. None of the above

Answer 122

D

Question 123

Which, if any of the following correctly shows the balanced molecular equation for the reaction that occurs when aqueous solutions of potassium iodide and lead(II) nitrate are combined. A. 2KI(aq) + Pb(NO3)2(aq)  PbI2(s) + KNO3(aq) B. KI(aq) + Pb(NO3)2(aq)  PbI2(s) + 2KNO3(aq) C. 2KI(aq) + Pb(NO3)2(aq)  PbI2(s) + 2KNO3(aq) D. 2KI(aq) + 2Pb(NO3)2(aq)  PbI2(s) + 2KNO3(aq) E. None of the above

Answer 123

C