Question 1

Which ions are spectator ions in the formation of a precipitate of AgCl via combining aqueous solutions of CoCl2 and AgNO3?

Accepted Answer

A)  Co2+ and NO3-
B)  NO3- and Cl-
C)  Co2+ and Ag+
D)  Cl-
E)  NO3-F) B) and C)
G) A) and B)

Question 2

When aqueous solutions of ________ are mixed, a precipitate forms.

Accepted Answer

A)  NiBr2 and AgNO3
B)  NaI and KBr
C)  K2SO4 and CrCl3
D)  KOH and Ba(NO3) 2
E)  Li2CO3 and CsIF) A) and B)
G) A) and C)

Question 3

Of the species below, only ________ is not an electrolyte.

Accepted Answer

A)  HBr
B)  LiCl
C)  Ne
D)  KOH
E)  NaNO3F) C) and D)
G) A) and B)

Question 4

What is the molarity of a NaOH solution if 15.5 mL of a 0.220 M H2SO4 solution is required to neutralize a 25.0-mL sample of the NaOH solution?

Accepted Answer

A)  0.273
B)  0.355
C)  0.710
D)  42.6
E)  0.136F) A) and E)
G) C) and D)

Question 5

What mass (g) of barium iodide is contained in 188 mL of a barium iodide solution that has an iodide ion concentration of 0.532 M?

Accepted Answer

A)  19.6
B)  39.1
C)  19,600
D)  39,100
E)  276F) C) and D)
G) C) and E)

Question 6

A 31.5 mL aliquot of HNO3 (aq) of unknown concentration was titrated with 0.0134 M NaOH (aq) . It took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was ________.

Accepted Answer

A)  0.0102
B)  0.0051
C)  0.0204
D)  0.227
E)  1.02F) A) and D)
G) A) and C)

Question 7

How many moles of Co2+ are present in 0.200 L of a 0.400 M solution of CoI2?

Accepted Answer

A)  2.00
B)  0.500
C)  0.160
D)  0.0800
E)  0.0400F) D) and E)
G) B) and D)

Question 8

How many milliliters of a stock solution of 11.7 M HNO3 would be needed to prepare 0.500 L of 0.500 M HNO3?

Accepted Answer

A)  0.0468
B)  21.4
C)  2.93
D)  46.8
E)  0.0214F) C) and E)
G) B) and D)

Question 9

The molarity of a solution prepared by diluting 43.72 mL of 1.005 M aqueous K2Cr2O7 to 500. mL is ________.

Accepted Answer

A)  0.0879
B)  87.9
C)  0.0218
D)  0.0115
E)  0.870F) A) and D)
G) A) and B)

Question 10

Calculate the number of grams of solute in 500.0 mL of 0.159 M KOH.

Accepted Answer

A)  176
B)  1.42
C)  4.46 × 103
D)  4.46
E)  1.42 × 10-3F) B) and D)
G) A) and D)

Question 11

What is the concentration (M)of CH3OH in a solution prepared by dissolving 10.2 g of CH3OH in sufficient water to give exactly 230 mL of solution?

Accepted Answer

Question 12

Which of the following are strong acids? HI
HNO3
HF
HBr

Accepted Answer

A)  HF, HBr
B)  HI, HNO3, HF, HBr
C)  HI, HF, HBr
D)  HNO3, HF, HBr
E)  HI, HNO3, HBrF) C) and D)
G) None of the above

Question 13

One method for removal of metal ions from a solution is to convert the metal to its elemental form so it can be filtered out as a solid. Which metal can be used to remove aluminum ions from solution?

Accepted Answer

A)  zinc
B)  cobalt
C)  lead
D)  copper
E)  none of theseF) A) and D)
G) C) and E)

Question 14

Which of the following would require the largest volume of 0.100 M sodium hydroxide solution for neutralization?

Accepted Answer

A)  10.0 mL of 0.0500 M phosphoric acid
B)  20.0 mL of 0.0500 M nitric acid
C)  5.0 mL of 0.0100 M sulfuric acid
D)  15.0 mL of 0.0500 M hydrobromic acid
E)  10.0 mL of 0.0500 M perchloric acidF) A) and B)
G) A) and C)

Question 15

Which solution has the same number of moles of KCl as 75.00 mL of 0.250 M solution of KCl?

Accepted Answer

A)  20.0 mL of 0.200 M solution of KCl
B)  25.0 mL of 0.175 M solution of KCl
C)  129 mL of 0.145 M solution of KCl
D)  50.0 mL of 0.125 M solution of KCl
E)  100 mL of 0.0500 M solution of KClF) D) and E)
G) All of the above

Question 16

A solution is prepared by mixing 15.0 mL of 0.100 M HCl and 5.00 mL of 0.200 M NaCl. What is the molarity of chloride ion in this solution?

Accepted Answer

A)  0.175
B)  8.00
C)  1.25
D)  0.0250
E)  0.125F) A) and B)
G) None of the above

Question 17

Which one of the following is a diprotic acid?

Accepted Answer

A)  nitric acid
B)  chloric acid
C)  phosphoric acid
D)  hydrofluoric acid
E)  sulfuric acidF) A) and C)
G) B) and D)

Question 18

In the following reaction, which species is reduced? Au(s)  + 3NO3-(aq)  + 6H+(aq)  → Au3+(aq)  + NO(g)  + 3H2O (l) 
H+
N+5
O2-
H2O
Au

Accepted Answer

A)  H+
B)  N+5
C)  O2-
D)  H2O
E)  AuF) None of the above
G) B) and D)

Question 19

In which reaction does the oxidation number of oxygen increase?

Accepted Answer

A)  Ba(NO3) 2 (aq)  + K2SO4 (aq)  → BaSO4 (s)  + 2KNO3 (aq) 
B)  HCl (aq)  + NaOH (aq)  → NaCl (aq)  + H2O (l) 
C)  MgO (s)  + H2O (l)  → Mg(OH) 2 (s) 
D)  2SO2 (g)  + O2 (g)  → 2SO3 (g) 
E)  2H2O (l)  → 2H2 (g)  + O2 (g) F) B) and E)
G) A) and B)

Question 20

Which of the following are weak electrolytes? HNO3
HF
NH3
LiBr

Accepted Answer

A)  HNO3, LiBr
B)  HNO3, HF, NH3, LiBr
C)  HF, LiBr
D)  HF, NH3
E)  HNO3, NH3, LiBrF) C) and E)
G) A) and E)

Exam 4: Aqueous Reactions and Solution Stoichiometry

In the following reaction, which species is reduced? Au(s) + 3NO3-(aq) + 6H+(aq) → Au3+(aq) + NO(g) + 3H2O (l) H+ N+5 O2- H2O Au

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Which solution has the same number of moles of KCl as 75.00 mL of 0.250 M solution of KCl?

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Which ions are spectator ions in the formation of a precipitate of AgCl via combining aqueous solutions of CoCl2 and AgNO3?

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Which one of the following is a diprotic acid?

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What is the molarity of a NaOH solution if 15.5 mL of a 0.220 M H2SO4 solution is required to neutralize a 25.0-mL sample of the NaOH solution?

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A 31.5 mL aliquot of HNO3 (aq) of unknown concentration was titrated with 0.0134 M NaOH (aq) . It took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was ________.

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Which of the following are strong acids? HI HNO3 HF HBr

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Of the species below, only ________ is not an electrolyte.

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What is the concentration (M)of CH3OH in a solution prepared by dissolving 10.2 g of CH3OH in sufficient water to give exactly 230 mL of solution?

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Which of the following would require the largest volume of 0.100 M sodium hydroxide solution for neutralization?

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The molarity of a solution prepared by diluting 43.72 mL of 1.005 M aqueous K2Cr2O7 to 500. mL is ________.

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What mass (g) of barium iodide is contained in 188 mL of a barium iodide solution that has an iodide ion concentration of 0.532 M?

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How many milliliters of a stock solution of 11.7 M HNO3 would be needed to prepare 0.500 L of 0.500 M HNO3?

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A solution is prepared by mixing 15.0 mL of 0.100 M HCl and 5.00 mL of 0.200 M NaCl. What is the molarity of chloride ion in this solution?

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One method for removal of metal ions from a solution is to convert the metal to its elemental form so it can be filtered out as a solid. Which metal can be used to remove aluminum ions from solution?

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How many moles of Co2+ are present in 0.200 L of a 0.400 M solution of CoI2?

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When aqueous solutions of ________ are mixed, a precipitate forms.

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Calculate the number of grams of solute in 500.0 mL of 0.159 M KOH.

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Which of the following are weak electrolytes? HNO3 HF NH3 LiBr

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In which reaction does the oxidation number of oxygen increase?

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In the following reaction, which species is reduced? Au(s) + 3NO₃^-(aq) + 6H⁺(aq) → Au³⁺(aq) + NO(g) + 3H₂O (l) H⁺ N⁺⁵ O^2- H₂O Au

Correct Answer
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Which ions are spectator ions in the formation of a precipitate of AgCl via combining aqueous solutions of CoCl₂ and AgNO₃?

Correct Answer
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Correct Answer
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What is the molarity of a NaOH solution if 15.5 mL of a 0.220 M H₂SO₄solution is required to neutralize a 25.0-mL sample of the NaOH solution?

Correct Answer
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A 31.5 mL aliquot of HNO₃ (aq) of unknown concentration was titrated with 0.0134 M NaOH (aq) . It took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was ________.

Correct Answer
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Which of the following are strong acids? HI HNO₃ HF HBr

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Correct Answer
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What is the concentration (M)of CH₃OH in a solution prepared by dissolving 10.2 g of CH₃OH in sufficient water to give exactly 230 mL of solution?

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Correct Answer
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The molarity of a solution prepared by diluting 43.72 mL of 1.005 M aqueous K₂Cr₂O₇ to 500. mL is ________.

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Correct Answer
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How many milliliters of a stock solution of 11.7 M HNO₃ would be needed to prepare 0.500 L of 0.500 M HNO₃?

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How many moles of Co²⁺ are present in 0.200 L of a 0.400 M solution of CoI₂?

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Which of the following are weak electrolytes? HNO₃ HF NH₃ LiBr

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Correct Answer
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