Question 1

35.0 mL of 0.255 M nitric acid is added to 45.0 mL of 0.328 M Mg(NO3)2. What is the concentration of nitrate ion in the final solution

Accepted Answer

A)  0.481 M 
B)  0.296 M 
C)  0.854 M 
D)  1.10 M 
E)  0.0295 M 
A)  0.481 M 
B)  0.296 M 
C)  0.854 M 
D)  1.10 M 
E)  0.0295 M

Question 2

Based on the solubility rules, which of the following should be soluble in water

Accepted Answer

A)  AgBr 
B)  AgCl 
C)  Ag2CO3 
D)  AgNO3 
E)  Ag2S 
A)  AgBr 
B)  AgCl 
C)  Ag2CO3 
D)  AgNO3 
E)  Ag2S

Question 3

During a titration the following data were collected. A 10. mL portion of an unknown monoprotic acid solution was titrated with 1.0 M NaOH; 40. mL of the base were required to neutralize the sample. What is the molarity of the acid solution

Accepted Answer

A)  1.0 M 
B)  2.0 M 
C)  3.0 M 
D)  4.0 M 
E)  None of the above 
A)  1.0 M 
B)  2.0 M 
C)  3.0 M 
D)  4.0 M 
E)  None of the above

Question 4

Identify the precipitate(s) formed when solutions of Ca(ClO4)2(aq), K2CO3(aq), and NaNO3(aq) are mixed.

Accepted Answer

A)  CaCO3 
B)  Na2CO3 
C)  Ca(NO3)2 and NaClO4 
D)  CaCO3 and Na2CO3 
E)  KClO4 and Ca(NO3)2 
A)  CaCO3 
B)  Na2CO3 
C)  Ca(NO3)2 and NaClO4 
D)  CaCO3 and Na2CO3 
E)  KClO4 and Ca(NO3)2

Question 5

Thorium +4 is reduced in this process. (Thorium metal is prepared by reacting thorium oxide with calcium as shown below.)
ThO2 + 2Ca $\rarr$ Th + 2CaO

Accepted Answer

A) True 
 B)False

Question 6

If 73.5 mL of 0.200 M KI(aq) was required to precipitate all of the lead(II) ion from an aqueous solution of lead(II) nitrate, how many moles of Pb2+ were originally in the solution

Accepted Answer

A)  7.25 $\rarr$ 10-3 moles of Pb2+ 
B)  7.35 $\rarr$ 10-3 moles of Pb2+ 
C)  7.45 $\rarr$ 10-3 moles of Pb2+ 
D)  7.55 $\rarr$ 10-3 moles of Pb2+ 
E)  None of the above 
A)  7.25 $\rarr$ 10-3 moles of Pb2+ 
B)  7.35 $\rarr$ 10-3 moles of Pb2+ 
C)  7.45 $\rarr$ 10-3 moles of Pb2+ 
D)  7.55 $\rarr$ 10-3 moles of Pb2+ 
E)  None of the above

Question 7

HNO3 is an example of a monoproticacid.

Accepted Answer

A) True 
 B)False

Question 8

For the chlorate ion, ClO3- , what are the oxidation states of the Cl and O, respectively

Accepted Answer

A)  - 1, - 2 
B)  +5, - 2 
C)  +6, - 2 
D)  +7, - 2 
E)  +2, - 1 
A)  - 1, - 2 
B)  +5, - 2 
C)  +6, - 2 
D)  +7, - 2 
E)  +2, - 1

Question 9

Which of the following represents a combustion reaction

Accepted Answer

A)  2C2H6(g) + 7O2(g) $\rarr$ 4CO2(g) + 6H2O(l) 
B)  LiOH(aq) + HNO3(aq) $\rarr$  LiNO3(aq) + H2O(l) 
C)  N2(g) + 3H2(g) $\rarr$  2NH3(g) 
D) 2Na(s) + 2H2O(l) $\rarr$  2NaOH(aq) + H2(g) 
E)  2Al(s) + 3H2SO4(aq) $\rarr$ Al2(SO4)3(aq) + 3H2(g) 
A)  2C2H6(g) + 7O2(g) $\rarr$ 4CO2(g) + 6H2O(l) 
B)  LiOH(aq) + HNO3(aq) $\rarr$  LiNO3(aq) + H2O(l) 
C)  N2(g) + 3H2(g) $\rarr$  2NH3(g) 
D) 2Na(s) + 2H2O(l) $\rarr$  2NaOH(aq) + H2(g) 
E)  2Al(s) + 3H2SO4(aq) $\rarr$ Al2(SO4)3(aq) + 3H2(g)

Question 10

NH4NO3 is a weak electrolyte.

Accepted Answer

A) True 
 B)False

Question 11

A solution is a homogeneous mixture of two or more substances.

Accepted Answer

A) True 
 B)False

Question 12

NH4Cl is a nonelectrolyte.

Accepted Answer

A) True 
 B)False

Question 13

Which of the following represents a hydrogen displacement reaction

Accepted Answer

A)  2C2H6(g) + 7O2(g) $\rarr$ 4CO2(g) + 6H2O(l) 
B) 2KBr(aq) + Cl2(g) $\rarr$ 2KCl(aq) + Br2(l) 
C)  N2(g) + 3H2(g) $\rarr$ 2NH3(g) 
D) CaBr2(aq) + H2SO4(aq) $\rarr$ CaSO4(s) + 2HBr(g) 
E)  2Al(s) + 3H2SO4(aq) $\rarr$ Al2(SO4)3(aq) + 3H2(g) 
A)  2C2H6(g) + 7O2(g) $\rarr$ 4CO2(g) + 6H2O(l) 
B) 2KBr(aq) + Cl2(g) $\rarr$ 2KCl(aq) + Br2(l) 
C)  N2(g) + 3H2(g) $\rarr$ 2NH3(g) 
D) CaBr2(aq) + H2SO4(aq) $\rarr$ CaSO4(s) + 2HBr(g) 
E)  2Al(s) + 3H2SO4(aq) $\rarr$ Al2(SO4)3(aq) + 3H2(g)

Question 14

What mass of Na2SO4 is needed to prepare 350. mL of a solution having a sodium ion concentration of 0.125 M

Accepted Answer

A)  3.11 g 
B)  24.9 g 
C)  12.4 g 
D)  6.21 g 
E)  8.88 g 
A)  3.11 g 
B)  24.9 g 
C)  12.4 g 
D)  6.21 g 
E)  8.88 g

Question 15

What mass of K2CO3 is needed to prepare 200. mL of a solution having a potassium ion concentration of 0.150 M

Accepted Answer

A)  4.15 g 
B)  10.4 g 
C)  13.8 g 
D)  2.07 g 
E)  1.49 g 
A)  4.15 g 
B)  10.4 g 
C)  13.8 g 
D)  2.07 g 
E)  1.49 g

Question 16

Predict the products of the following single replacement reaction.
Ni(s) + Cu(NO3)2(aq) $\rarr$

Accepted Answer

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) 
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)

Question 17

Of the following, which is NOT an example of a strong acid

Accepted Answer

A)  hydrochloric acid, HCl 
B)  hydroiodic acid, HI 
C)  carbonic acid, H2CO3 
D)  perchloric acid, HClO4 
E)  nitric acid, HNO3 
A)  hydrochloric acid, HCl 
B)  hydroiodic acid, HI 
C)  carbonic acid, H2CO3 
D)  perchloric acid, HClO4 
E)  nitric acid, HNO3

Question 18

H2CO3is a weak electrolyte.

Accepted Answer

A) True 
 B)False

Question 19

Which of the following will occur when a solution of Pb(NO3)2(aq) is mixed with a solution of KI(aq)

Accepted Answer

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. 
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.

Question 20

Based on the solubility rules, which of the following compounds should be insoluble in water

Accepted Answer

A)  CaCO3 
B)  (NH4)2CO3 
C)  Na2CO3 
D)  K2CO3 
E)  KNO3 
A)  CaCO3 
B)  (NH4)2CO3 
C)  Na2CO3 
D)  K2CO3 
E)  KNO3

Exam 4: Reactions in Aqueous Solutions

35.0 mL of 0.255 M nitric acid is added to 45.0 mL of 0.328 M Mg(NO3)2. What is the concentration of nitrate ion in the final solution

Based on the solubility rules, which of the following should be soluble in water

During a titration the following data were collected. A 10. mL portion of an unknown monoprotic acid solution was titrated with 1.0 M NaOH; 40. mL of the base were required to neutralize the sample. What is the molarity of the acid solution

Identify the precipitate(s) formed when solutions of Ca(ClO4)2(aq), K2CO3(aq), and NaNO3(aq) are mixed.

Thorium +4 is reduced in this process. (Thorium metal is prepared by reacting thorium oxide with calcium as shown below.) ThO2 + 2Ca →\rarr→ Th + 2CaO

If 73.5 mL of 0.200 M KI(aq) was required to precipitate all of the lead(II) ion from an aqueous solution of lead(II) nitrate, how many moles of Pb2+ were originally in the solution

HNO3 is an example of a monoproticacid.

For the chlorate ion, ClO3- , what are the oxidation states of the Cl and O, respectively

Which of the following represents a combustion reaction

NH4NO3 is a weak electrolyte.

A solution is a homogeneous mixture of two or more substances.

NH4Cl is a nonelectrolyte.

Which of the following represents a hydrogen displacement reaction

What mass of Na2SO4 is needed to prepare 350. mL of a solution having a sodium ion concentration of 0.125 M

What mass of K2CO3 is needed to prepare 200. mL of a solution having a potassium ion concentration of 0.150 M

Predict the products of the following single replacement reaction. Ni(s) + Cu(NO3)2(aq) →\rarr→

Of the following, which is NOT an example of a strong acid

H2CO3is a weak electrolyte.

Which of the following will occur when a solution of Pb(NO3)2(aq) is mixed with a solution of KI(aq)

Based on the solubility rules, which of the following compounds should be insoluble in water

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35.0 mL of 0.255 M nitric acid is added to 45.0 mL of 0.328 M Mg(NO₃)₂. What is the concentration of nitrate ion in the final solution

Identify the precipitate(s) formed when solutions of Ca(ClO₄)₂(aq), K₂CO₃(aq), and NaNO₃(aq) are mixed.

Thorium +4 is reduced in this process. (Thorium metal is prepared by reacting thorium oxide with calcium as shown below.) ThO₂ + 2Ca $\rarr$ Th + 2CaO

If 73.5 mL of 0.200 M KI(aq) was required to precipitate all of the lead(II) ion from an aqueous solution of lead(II) nitrate, how many moles of Pb²⁺ were originally in the solution

HNO₃ is an example of a monoproticacid.

For the chlorate ion, ClO₃^- , what are the oxidation states of the Cl and O, respectively

NH₄NO₃ is a weak electrolyte.

NH₄Cl is a nonelectrolyte.

What mass of Na₂SO₄ is needed to prepare 350. mL of a solution having a sodium ion concentration of 0.125 M

What mass of K₂CO₃ is needed to prepare 200. mL of a solution having a potassium ion concentration of 0.150 M

Predict the products of the following single replacement reaction. Ni(s) + Cu(NO₃)₂(aq) $\rarr$

H₂CO₃is a weak electrolyte.

Which of the following will occur when a solution of Pb(NO₃)₂(aq) is mixed with a solution of KI(aq)