Question 1

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 2

Calculate K. Cu(OH) 2(aq) ⇌ Cu2+(aq) + 2 OH-(aq) Ksp = 1.6 × 10-19
Cu2+(aq) + 4 NH3(aq) ⇌ Cu(NH3) 42+(aq) Kf = 1.7 × 1013
Cu(OH) 2(aq) + 4 NH3(aq) ⇌ Cu(NH3) 42+(aq) + 2 OH-(aq) K = ?

Accepted Answer

A)   1.06 × 1032
B)   3.7 × 105
C)   9.4 × 10-33
D)   2.7 × 10-6
E)   1.7 × 1013

Question 3

Identify the compound that is base-insoluble.

Accepted Answer

A)   PbCl2
B)   As2S3
C)   ZnS
D)   Ca3(PO4) 2
E)   KCl

Question 4

A 110.0 mL sample of 0.20 M HF is titrated with 0.10 M CsOH.Determine the pH of the solution after the addition of 440.0 mL of CsOH.The Ka of HF is 3.5 × 10-4.

Accepted Answer

A)   13.08
B)   12.60
C)   13.85
D)   12.30
E)   12.78

Question 5

0.10 M potassium chromate is slowly added to a solution containing 0.50 M AgNO3 and 0.50 M Ba(NO3) 2.What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 × 10-12 and 1.2 × 10-10,respectively.

Accepted Answer

A)   6.5 × 10-5 M
B)   1.3 × 10-4 M
C)   3.2 × 10-4 M
D)   6.8 × 10-2 M

Question 6

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF.Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH.Assume no volume change upon the addition of base.The Ka for HF is 3.5 × 10-4.

Accepted Answer

A)   3.46
B)   4.06
C)   2.85
D)   3.63
E)   4.24

Question 7

Calculate the pH of a buffer that is 0.225 M HC2H3O2 and 0.162 M KC2H3O2.The Ka for HC2H3O2 is 1.8 × 10-5.

Accepted Answer

A)   4.89
B)   9.11
C)   4.74
D)   9.26
E)   4.60

Question 8

What is the pH of a solution made by mixing 30.00 mL of 0.10 M HI with 40.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive.

Accepted Answer

A)   0.85
B)   1.85
C)   12.15
D)   13.15

Question 9

A sample contains MgNH4(PO4) 2, Sb2S3,KBr,Cr(OH) 3,and PbCl2.Identify the precipitate after the addition of 6 M HCl.

Accepted Answer

A)   MgNH4(PO4) 2
B)   Sb2S3
C)   KBr
D)   Cr(OH) 3
E)   PbCl2

Question 10

A 1.0 L buffer solution is 0.250 M HC2H3O2 and 0.060 M NaC2H3O2.Which of the following actions will destroy the buffer?

Accepted Answer

A)   adding 0.060 moles of NaC2H3O2
B)   adding 0.060 moles of HC2H3O2
C)   adding 0.060 moles of HCl
D)   adding 0.060 moles of KOH
E)   All of the above will destroy the buffer.

Question 11

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 12

When titrating a weak monoprotic acid with NaOH at 25°C,the

Accepted Answer

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

Question 13

What is the molar solubility of Mg(OH) 2 in a basic solution with a pH of 12.50? Ksp for Mg(OH) 2 is 5.6 × 10-12.

Accepted Answer

A)   1.8 × 10-10 M
B)   5.6 × 10-9 M
C)   2.4 × 10-6 M
D)   1.1 × 10-4 M

Question 14

Determine the molar solubility of BaF2 in a solution containing 0.0750 M LiF. Ksp (BaF2) = 1.7 × 10-6.

Accepted Answer

A)   2.3 × 10-5 M
B)   8.5 × 10-7 M
C)   1.2 × 10-2 M
D)   0.0750 M
E)   3.0 × 10-4 M

Question 15

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 200.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

Accepted Answer

A)   6.44
B)   1.48
C)   2.00
D)   12.52
E)   12.00

Question 16

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3 with 5.00 mL of 0.10 M NH4Cl? Assume that the volume of the solutions are additive and that Kb = 1.8 × 10-5 for NH3.

Accepted Answer

A)   8.25
B)   9.28
C)   10.26
D)   11.13

Question 17

Determine the molar solubility of AgBr in a solution containing 0.150 M NaBr. Ksp (AgBr) = 7.7 × 10-13.

Accepted Answer

A)   8.8 × 10-7 M
B)   3.9 × 10-13 M
C)   5.8 × 10-5 M
D)   5.1 × 10-12 M
E)   0.150 M

Question 18

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 19

A 100.0 mL sample of 0.10 M Ba(OH) 2 is titrated with 0.10 M HCl.Determine the pH of the solution after the addition of 100.0 mL HCl.

Accepted Answer

A)   2.00
B)   12.00
C)   1.30
D)   12.70
E)   7.00

Question 20

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

Accepted Answer

A)   alizarin
B)   thymol blue
C)   crystal violet
D)   phenolphthalein
E)   alizarin yellow R

Exam 17: Aqueous Ionic Equilibrium

What is the molar solubility of Mg(OH) 2 in a basic solution with a pH of 12.50? Ksp for Mg(OH) 2 is 5.6 × 10-12.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

A 110.0 mL sample of 0.20 M HF is titrated with 0.10 M CsOH.Determine the pH of the solution after the addition of 440.0 mL of CsOH.The Ka of HF is 3.5 × 10-4.

Correct AnswerverifiedShow Answer

Calculate the pH of a buffer that is 0.225 M HC2H3O2 and 0.162 M KC2H3O2.The Ka for HC2H3O2 is 1.8 × 10-5.

Correct AnswerverifiedShow Answer

A 1.0 L buffer solution is 0.250 M HC2H3O2 and 0.060 M NaC2H3O2.Which of the following actions will destroy the buffer?

Correct AnswerverifiedShow Answer

A 100.0 mL sample of 0.10 M Ba(OH) 2 is titrated with 0.10 M HCl.Determine the pH of the solution after the addition of 100.0 mL HCl.

Correct AnswerverifiedShow Answer

What is the pH of a solution made by mixing 30.00 mL of 0.10 M HI with 40.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive.

Correct AnswerverifiedShow Answer

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.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Calculate K. Cu(OH) 2(aq) ⇌ Cu2+(aq) + 2 OH-(aq) Ksp = 1.6 × 10-19 Cu2+(aq) + 4 NH3(aq) ⇌ Cu(NH3) 42+(aq) Kf = 1.7 × 1013 Cu(OH) 2(aq) + 4 NH3(aq) ⇌ Cu(NH3) 42+(aq) + 2 OH-(aq) K = ?

Correct AnswerverifiedShow Answer

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF.Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH.Assume no volume change upon the addition of base.The Ka for HF is 3.5 × 10-4.

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

Identify the compound that is base-insoluble.

Correct AnswerverifiedShow Answer

Determine the molar solubility of AgBr in a solution containing 0.150 M NaBr. Ksp (AgBr) = 7.7 × 10-13.

Correct AnswerverifiedShow Answer

Determine the molar solubility of BaF2 in a solution containing 0.0750 M LiF. Ksp (BaF2) = 1.7 × 10-6.

Correct AnswerverifiedShow Answer

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3 with 5.00 mL of 0.10 M NH4Cl? Assume that the volume of the solutions are additive and that Kb = 1.8 × 10-5 for NH3.

Correct AnswerverifiedShow Answer

0.10 M potassium chromate is slowly added to a solution containing 0.50 M AgNO3 and 0.50 M Ba(NO3) 2.What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 × 10-12 and 1.2 × 10-10,respectively.

Correct AnswerverifiedShow Answer

A sample contains MgNH4(PO4) 2, Sb2S3,KBr,Cr(OH) 3,and PbCl2.Identify the precipitate after the addition of 6 M HCl.

Correct AnswerverifiedShow Answer

When titrating a weak monoprotic acid with NaOH at 25°C,the

Correct AnswerverifiedShow Answer

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 200.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

Correct AnswerverifiedShow Answer

What is the molar solubility of Mg(OH) ₂ in a basic solution with a pH of 12.50? K_spfor Mg(OH) ₂ is 5.6 × 10^-¹².

Correct Answer
verified

Correct Answer
verified

A 110.0 mL sample of 0.20 M HF is titrated with 0.10 M CsOH.Determine the pH of the solution after the addition of 440.0 mL of CsOH.The K_a of HF is 3.5 × 10^-4.

Correct Answer
verified

Calculate the pH of a buffer that is 0.225 M HC₂H₃O₂ and 0.162 M KC₂H₃O₂.The K_a for HC₂H₃O₂ is 1.8 × 10^-5.

Correct Answer
verified

A 1.0 L buffer solution is 0.250 M HC₂H₃O₂ and 0.060 M NaC₂H₃O₂.Which of the following actions will destroy the buffer?

Correct Answer
verified

A 100.0 mL sample of 0.10 M Ba(OH) ₂ is titrated with 0.10 M HCl.Determine the pH of the solution after the addition of 100.0 mL HCl.

Correct Answer
verified

Correct Answer
verified

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
verified

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

Correct Answer
verified

Calculate K. Cu(OH) ₂(aq) ⇌ Cu²⁺(aq) + 2 OH^-(aq) K_sp = 1.6 × 10^-19 Cu²⁺(aq) + 4 NH₃(aq) ⇌ Cu(NH₃) ₄²⁺(aq) K_f = 1.7 × 10¹³ Cu(OH) ₂(aq) + 4 NH₃(aq) ⇌ Cu(NH₃) ₄²⁺(aq) + 2 OH^-(aq) K = ?

Correct Answer
verified

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF.Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH.Assume no volume change upon the addition of base.The K_a for HF is 3.5 × 10^-4.

Correct Answer
verified

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.

Correct Answer
verified

Correct Answer
verified

Determine the molar solubility of AgBr in a solution containing 0.150 M NaBr. K_sp (AgBr) = 7.7 × 10^-13.

Correct Answer
verified

Determine the molar solubility of BaF₂ in a solution containing 0.0750 M LiF. K_sp (BaF₂) = 1.7 × 10^-6.

Correct Answer
verified

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH₃ with 5.00 mL of 0.10 M NH₄Cl? Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5for NH₃.

Correct Answer
verified

0.10 M potassium chromate is slowly added to a solution containing 0.50 M AgNO₃ and 0.50 M Ba(NO₃) ₂.What is the Ag⁺ concentration when BaCrO₄ just starts to precipitate? The K_sp for Ag₂CrO₄ and BaCrO₄ are 1.1 × 10^-12 and 1.2 × 10^-1⁰,respectively.

Correct Answer
verified

A sample contains MgNH₄(PO₄) ₂,Sb₂S₃,KBr,Cr(OH) ₃,and PbCl₂.Identify the precipitate after the addition of 6 M HCl.

Correct Answer
verified

Correct Answer
verified

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 200.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Correct Answer
verified