Question 1

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution after the addition of 150.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

Accepted Answer

A)   1.70
B)   6.44
C)   7.56
D)   12.30
E)   2.30

Question 2

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4Cl with 100.0 mL of 0.20 M NH3.The Kb for NH3 is 1.8 × 10-5.

Accepted Answer

A)   9.13
B)   9.25
C)   9.53
D)   4.74
E)   8.98

Question 3

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution after the addition of 50.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

Accepted Answer

A)   4.74
B)   7.78
C)   7.05
D)   9.26
E)   10.34

Question 4

Which of the following would be considered a complex ion?

Accepted Answer

A)   F-
B)   PO33-
C)   AlF6-
D)   Fe2+
E)   NH4+

Question 5

Identify the indicator that can be used at the lowest pH.

Accepted Answer

A)   2,4-dinitrophenol
B)   thymol blue
C)   crystal violet
D)   thymolphthalein
E)   methyl red

Question 6

Give the equation for an unsaturated solution in comparing Q with Ksp.

Accepted Answer

A)   Q > Ksp
B)   Q sp
C)   Q = Ksp
D)   Q ≠ Ksp
E)   none of the above

Question 7

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl.The Ka for HF is 3.5 × 10-4.

Accepted Answer

A)   3.09
B)   4.11
C)   3.82
D)   3.46
E)   2.78

Question 8

What is the pH of a buffer solution that is 0.222 M in lactic acid and 0.132 M in sodium lactate? The Ka of lactic acid is 1.4 × 10-4.

Accepted Answer

A)   14.23
B)   10.38
C)   5.39
D)   3.62
E)   4.08

Question 9

An important buffer in the blood is a mixture of

Accepted Answer

A)   sodium chloride and hydrochloric acid.
B)   hydrochloric acid and sodium hydroxide.
C)   carbonic acid and bicarbonate ion.
D)   acetic acid and bicarbonate ion.
E)   acetic acid and carbonate ion.

Question 10

What is the molar solubility of silver carbonate ( Ag2CO3 ) in water? The solubility-product constant for Ag2CO3 is 8.1 × 10-12 at 25°C.

Accepted Answer

A)   1.4 × 10-6
B)   2.0 × 10-4
C)   4.0 × 10-6
D)   1.3 × 10-4
E)   2.7 × 10-12

Question 11

Determine the molar solubility of AgI in pure water.Ksp (AgI) = 8.51 × 10-17.

Accepted Answer

A)   9.22 × 10-9 M
B)   4.26 × 10-17 M
C)   8.51 × 10-17 M
D)   2.77 × 10-6 M
E)   4.40 × 10-6 M

Question 12

When titrating a strong monoprotic acid with KOH at 25°C,the

Accepted Answer

A)   pH will be less than 7 at the equivalence point.
B)   pH will be greater than 7 at the equivalence point.
C)   titration will require more moles of base than acid to reach the equivalence point.
D)   pH will be equal to 7 at the equivalence point.
E)   titration will require more moles of acid than base to reach the equivalence point.

Question 13

Calculate the percent ionization of nitrous acid in a solution that is 0.169 M in nitrous acid.The acid dissociation constant of nitrous acid is 4.50 × 10-4.

Accepted Answer

A)   7.61 × 10-5
B)   0.0450
C)   5.16
D)   0.743
E)   3.76

Question 14

Calculate the pH of a buffer that is 0.032 M HF and 0.032 M KF.The Ka for HF is 3.5 × 10-4.

Accepted Answer

A)   2.86
B)   9.31
C)   10.54
D)   3.46
E)   4.89

Question 15

Determine the molar solubility of CuCl in a solution containing 0.040 M KCl.Ksp (CuCl) = 1.0 × 10-6.

Accepted Answer

A)   1.0 × 10-12 M
B)   4.0 × 10-8 M
C)   2.5 × 10-5 M
D)   1.0 × 10-3 M
E)   0.050 M

Question 16

Determine the molar solubility for Pb3(PO4) 2 in pure water.Ksp for Pb3(PO4) 2 is 1.0 × 10-54.

Accepted Answer

A)   4.1 × 10-28 M
B)   5.8 × 10-10 M
C)   1.1 × 10-11 M
D)   6.2 × 10-12 M
E)   1.0 × 10-54 M

Question 17

What is the [CH3CO2-]/[CH3CO2H] ratio necessary to make a buffer solution with a pH of 4.44? Ka = 1.8 × 10-5 for CH3CO2H.

Accepted Answer

A)   0.50:1
B)   0.94:1
C)   1.1:1
D)   2.0:1

Question 18

What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M Ca(OH) 2 with 50.00 mL of 0.100 M NaOH? Assume that the volumes are additive.

Accepted Answer

A)   12.67
B)   12.78
C)   12.95
D)   13.25

Question 19

Determine the molar solubility of BiPO4 in a solution containing 0.358 M K3PO4.The Ksp for BiPO4 is 1.3 × 10-23.

Accepted Answer

A)   5.7 × 10-15
B)   3.6 × 10-23
C)   1.3 × 10-13
D)   1.5 × 10-8
E)   8.3 × 10-18

Question 20

Stalactites and stalagmites form as ________ precipitates out of the water evaporating in underground caves.

Accepted Answer

A)   hydrochloric acid
B)   sodium hydroxide
C)   sodium chloride
D)   calcium carbonate
E)   sodium bicarbonate

Exam 18: Aqueous Ionic Equilibrium

Determine the molar solubility of CuCl in a solution containing 0.040 M KCl.Ksp (CuCl) = 1.0 × 10-6.

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A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution after the addition of 150.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

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Calculate the pH of a buffer that is 0.032 M HF and 0.032 M KF.The Ka for HF is 3.5 × 10-4.

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Determine the molar solubility of AgI in pure water.Ksp (AgI) = 8.51 × 10-17.

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What is the molar solubility of silver carbonate ( Ag2CO3 ) in water? The solubility-product constant for Ag2CO3 is 8.1 × 10-12 at 25°C.

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Determine the molar solubility of BiPO4 in a solution containing 0.358 M K3PO4.The Ksp for BiPO4 is 1.3 × 10-23.

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Calculate the percent ionization of nitrous acid in a solution that is 0.169 M in nitrous acid.The acid dissociation constant of nitrous acid is 4.50 × 10-4.

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What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M Ca(OH) 2 with 50.00 mL of 0.100 M NaOH? Assume that the volumes are additive.

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What is the [CH3CO2-]/[CH3CO2H] ratio necessary to make a buffer solution with a pH of 4.44? Ka = 1.8 × 10-5 for CH3CO2H.

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Stalactites and stalagmites form as ________ precipitates out of the water evaporating in underground caves.

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Identify the indicator that can be used at the lowest pH.

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Give the equation for an unsaturated solution in comparing Q with Ksp.

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What is the pH of a buffer solution that is 0.222 M in lactic acid and 0.132 M in sodium lactate? The Ka of lactic acid is 1.4 × 10-4.

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An important buffer in the blood is a mixture of

Correct AnswerverifiedShow Answer

When titrating a strong monoprotic acid with KOH at 25°C,the

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Which of the following would be considered a complex ion?

Correct AnswerverifiedShow Answer

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl.The Ka for HF is 3.5 × 10-4.

Correct AnswerverifiedShow Answer

Determine the molar solubility for Pb3(PO4) 2 in pure water.Ksp for Pb3(PO4) 2 is 1.0 × 10-54.

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Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4Cl with 100.0 mL of 0.20 M NH3.The Kb for NH3 is 1.8 × 10-5.

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A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution after the addition of 50.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

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Determine the molar solubility of CuCl in a solution containing 0.040 M KCl.K_sp (CuCl) = 1.0 × 10^-6.

Correct Answer
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A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 150.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Correct Answer
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Calculate the pH of a buffer that is 0.032 M HF and 0.032 M KF.The K_a for HF is 3.5 × 10^-4.

Correct Answer
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Determine the molar solubility of AgI in pure water.K_sp (AgI) = 8.51 × 10^-17.

Correct Answer
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What is the molar solubility of silver carbonate ( Ag₂CO₃ ) in water? The solubility-product constant for Ag₂CO₃ is 8.1 × 10^-12 at 25°C.

Correct Answer
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Determine the molar solubility of BiPO₄ in a solution containing 0.358 M K₃PO₄.The Ksp for BiPO₄is 1.3 × 10^-23.

Correct Answer
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Calculate the percent ionization of nitrous acid in a solution that is 0.169 M in nitrous acid.The acid dissociation constant of nitrous acid is 4.50 × 10^-4.

Correct Answer
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What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M Ca(OH) ₂ with 50.00 mL of 0.100 M NaOH? Assume that the volumes are additive.

Correct Answer
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What is the [CH₃CO₂-]/[CH₃CO₂H] ratio necessary to make a buffer solution with a pH of 4.44? K_a = 1.8 × 10^-5for CH₃CO₂H.

Correct Answer
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Give the equation for an unsaturated solution in comparing Q with K_sp.

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What is the pH of a buffer solution that is 0.222 M in lactic acid and 0.132 M in sodium lactate? The K_a of lactic acid is 1.4 × 10^-4.

Correct Answer
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Correct Answer
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A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl.The K_a for HF is 3.5 × 10^-4.

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Determine the molar solubility for Pb₃(PO₄) ₂ in pure water.K_sp for Pb₃(PO₄) ₂ is 1.0 × 10^-54.

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Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH₄Cl with 100.0 mL of 0.20 M NH₃.The K_b for NH₃ is 1.8 × 10^-5.

Correct Answer
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A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 50.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Correct Answer
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