Question 1

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)  F) A) and C)
G) C) and E)

Question 2

NH4NO3 is a weak electrolyte.

Accepted Answer

A) True 
 B)False

Question 3

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, HNO3F) All of the above
G) D) and E)

Question 4

HNO3 is an example of a monoproticacid.

Accepted Answer

A) True 
 B)False

Question 5

NH4Cl is a nonelectrolyte.

Accepted Answer

A) True 
 B)False

Question 6

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, - 1F) D) and E)
G) A) and D)

Question 7

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 gF) B) and D)
G) A) and C)

Question 8

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)  F) B) and E)
G) A) and E)

Question 9

H2CO3is a weak electrolyte.

Accepted Answer

A) True 
 B)False

Question 10

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 MF) None of the above
G) B) and C)

Question 11

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) 2F) B) and E)
G) B) and D)

Question 12

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 F) A) and C)
G) B) and C)

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)  F) B) and D)
G) A) and B)

Question 14

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.F) D) and E)
G) B) and E)

Question 15

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 gF) A) and C)
G) A) and D)

Question 16

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 17

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)   Ag2SF) B) and E)
G) B) and D)

Question 18

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)   KNO3F) C) and D)
G) A) and E)

Question 19

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 aboveF) B) and E)
G) A) and B)

Question 20

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

Accepted Answer

A) True 
 B)False

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

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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

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

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Which of the following represents a hydrogen displacement reaction

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

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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

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

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

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Which of the following represents a combustion reaction

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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

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

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H2CO3is a weak electrolyte.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

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NH4NO3 is a weak electrolyte.

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

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HNO3 is an example of a monoproticacid.

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

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

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NH4Cl is a nonelectrolyte.

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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

Correct Answer
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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

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

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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

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

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H₂CO₃is a weak electrolyte.

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

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

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NH₄NO₃ is a weak electrolyte.

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

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HNO₃ is an example of a monoproticacid.

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

Correct Answer
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NH₄Cl is a nonelectrolyte.

Correct Answer
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