Question 1

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M butanoic acid to the equivalence point? 
The Ka of butanoic acid is 1.5 × 10-5.

Accepted Answer

A) 4.90 
B) 50.0 
C) 41.6 
D) 60.1 
E) 4.65

Question 2

Determine the molar solubility of BaF2 in pure water.Ksp (BaF2)= 2.45 × 10-5.

Accepted Answer

A) 1.83 × 10-2 M 
B) 1.23 × 10-5 M 
C) 2.90 × 10-2 M 
D) 4.95 × 10-3 M 
E) 6.13 × 10-6 M

Question 3

What is the pH of the resulting solution if 25.00 mL of 0.10 M acetic acid is added to 10.00 mL of 0.10 M NaOH? 
Assume that the volumes of the solutions are additive.Ka = 1.8 × 10-5 for CH3CO2H.

Accepted Answer

A) 9.43 
B) 9.08 
C) 4.92 
D) 4.57

Question 4

Identify the most common indicator.

Accepted Answer

A) Alizarin 
B) Thymol blue 
C) Crystal violet 
D) Phenolphthalein 
E) Alizarin yellow R

Question 5

A 1.00 L buffer solution is 0.150 M in HC7H5O2 and 0.250 M in LiC7H5O2.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl.The Ka for HC7H5O2 is 6.5 × 10-5.

Accepted Answer

A) 4.19 
B) 5.03 
C) 4.41 
D) 3.34 
E) 3.97

Question 6

A 25.0 mL sample of 0.150 M hypochlorous acid is titrated with a 0.150 M NaOH solution.What is the pH after 26.0 mL of base is added? 
The Ka of hypochlorous acid is 3.0 × 10-8.

Accepted Answer

A) 2.54 
B) 11.47 
C) 7.00 
D) 7.51 
E) 7.54

Question 7

The molar solubility of Ag2S is 1.26 × 10-16 M in pure water.Calculate the Ksp for Ag2S.

Accepted Answer

A) 1.59 × 10-32 
B) 1.12 × 10-8 
C) 6.81 × 10-63 
D) 3.78 × 10-12 
E) 8.00 × 10-48

Question 8

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous formic acid requires 29.80 mL of 0.3567 M NaOH? 
Ka = 1.8 × 10-4 for formic acid.

Accepted Answer

A) 2.06 
B) 5.48 
C) 8.52 
D) 11.94

Question 9

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 10

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

Accepted Answer

A) 6.58 
B) 10.56 
C) 8.72 
D) 3.44 
E) 5.28

Question 11

A 25.0 mL sample of 0.150 M acetic acid is titrated with a 0.150 M NaOH solution.What is the pH at the equivalence point? The Ka of acetic acid is 4.50 × 10-4.

Accepted Answer

A) 11.74 
B) 9.26 
C) 4.74 
D) 7.00 
E) 8.81

Question 12

What is the molar solubility of AgCl in 0.10 M NaCN if the colorless complex ion Ag(CN)2- forms? 
Ksp for AgCl is 1.8 × 10-10 and Kf for Ag(CN)2- is 1.0 × 1021.

Accepted Answer

A) 0.050 M 
B) 0.10 M 
C) 0.20 M 
D) 0.40 M

Question 13

A 1.50 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 0.0500 moles of solid NaOH.Assume no volume change upon the addition of base.The Ka for HF is 3.5 × 10-4.

Accepted Answer

A) 3.34 
B) 3.46 
C) 3.57 
D) 3.63 
E) 2.89

Question 14

A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is
2.1 × 10-5 M in calcium ion and 4.75 × 10-5 M in oxalate ion.What will happen once these solutions are mixed? Ksp (CaC2O4)= 2.3 × 10-9.

Accepted Answer

A) A precipitate will form since Q > Ksp for calcium oxalate. 
B) Nothing will happen since both calcium chloride and lithium oxalate are soluble compounds. 
C) Nothing will happen since calcium oxalate is extremely soluble. 
D) Nothing will happen since Ksp > Q for all possible precipitants. 
E) There is not enough information to determine.

Question 15

Give the expression for the solubility product constant for PbCl2.

Accepted Answer

A)   
B)   
C) [Pb2+][Cl⁻]2 
D)   
E) [Pb2+]2[Cl⁻]

Question 16

Fluffy,your prized Himalayan cat,was outside when your dad was changing the antifreeze in the car.Fluffy licked up a large amount of the antifreeze off the driveway.You live many miles from the veterinarian.What could you give Fluffy to drink to counteract the effects of antifreeze?

Accepted Answer

A) mineral oil 
B) rubbing alcohol 
C) a strong alcoholic drink 
D) gasoline 
E) vegetable oil

Question 17

A solution contains 2.2 × 10-3 M in Cu2+ and 0.33 M in LiCN.If the Kf for Cu(CN)42- is 1.0 × 1025,how much copper ion remains at equilibrium?

Accepted Answer

A) 3.8 × 10-24 M 
B) 1.9 × 10-26 M 
C) 6.7 × 10-28 M 
D) 2.9 × 10-27 M 
E) 4.6 × 10-25 M

Question 18

What is the pH of a solution made by mixing 10.00 mL of 0.10 M acetic acid with 10.00 mL of 0.10 M KOH? 
Assume that the volumes of the solutions are additive.Ka = 1.8 × 10-5 for CH3CO2H.

Accepted Answer

A) 5.28 
B) 7.00 
C) 8.72 
D) 10.02

Question 19

What is the molar solubility of silver chloride (AgCl)in water? The solubility-product constant for AgCl is 1.8 × 10-10 at 25°C.

Accepted Answer

A) 9.0 × 10-11 
B) 3.6 × 10-10 
C) 9.74 
D) 1.9 × 10-5 
E) 1.3 × 10-5

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 16: Aqueous Ionic Equilibrium

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M butanoic acid to the equivalence point? The K_a of butanoic acid is 1.5 × 10^-5.

Determine the molar solubility of BaF₂in pure water.K_sp (BaF₂) = 2.45 × 10^-5.

What is the pH of the resulting solution if 25.00 mL of 0.10 M acetic acid is added to 10.00 mL of 0.10 M NaOH? Assume that the volumes of the solutions are additive.K_a = 1.8 × 10^-5for CH₃CO₂H.

Identify the most common indicator.

A 1.00 L buffer solution is 0.150 M in HC₇H₅O₂ and 0.250 M in LiC₇H₅O₂.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl.The K_a for HC₇H₅O₂ is 6.5 × 10^-5.

A 25.0 mL sample of 0.150 M hypochlorous acid is titrated with a 0.150 M NaOH solution.What is the pH after 26.0 mL of base is added? The K_a of hypochlorous acid is 3.0 × 10^-8.

The molar solubility of Ag₂S is 1.26 × 10^-16 M in pure water.Calculate the K_sp for Ag₂S.

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous formic acid requires 29.80 mL of 0.3567 M NaOH? K_a = 1.8 × 10^-4 for formic acid.

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.

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

A 25.0 mL sample of 0.150 M acetic acid is titrated with a 0.150 M NaOH solution.What is the pH at the equivalence point? The K_a of acetic acid is 4.50 × 10^-4.

What is the molar solubility of AgCl in 0.10 M NaCN if the colorless complex ion Ag(CN) ₂^- forms? K_sp for AgCl is 1.8 × 10^-10 and K_f for Ag(CN) ₂^- is 1.0 × 10²¹.

A 1.50 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 0.0500 moles of solid NaOH.Assume no volume change upon the addition of base.The K_a for HF is 3.5 × 10^-4.

A solution containing CaCl₂ is mixed with a solution of Li₂C₂O₄ to form a solution that is 2.1 × 10^-5 M in calcium ion and 4.75 × 10^-5 M in oxalate ion.What will happen once these solutions are mixed? K_sp (CaC₂O₄) = 2.3 × 10^-9.

Give the expression for the solubility product constant for PbCl₂.

Fluffy,your prized Himalayan cat,was outside when your dad was changing the antifreeze in the car.Fluffy licked up a large amount of the antifreeze off the driveway.You live many miles from the veterinarian.What could you give Fluffy to drink to counteract the effects of antifreeze?

A solution contains 2.2 × 10^-3M in Cu²⁺ and 0.33 M in LiCN.If the K_f for Cu(CN) ₄^2- is 1.0 × 10²⁵,how much copper ion remains at equilibrium?

What is the pH of a solution made by mixing 10.00 mL of 0.10 M acetic acid with 10.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive.K_a = 1.8 × 10^-5for CH₃CO₂H.

What is the molar solubility of silver chloride (AgCl) in water? The solubility-product constant for AgCl is 1.8 × 10^-10 at 25°C.

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

Exam 16: Aqueous Ionic Equilibrium

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M butanoic acid to the equivalence point? The Ka of butanoic acid is 1.5 × 10-5.

Determine the molar solubility of BaF2 in pure water.Ksp (BaF2) = 2.45 × 10-5.

What is the pH of the resulting solution if 25.00 mL of 0.10 M acetic acid is added to 10.00 mL of 0.10 M NaOH? Assume that the volumes of the solutions are additive.Ka = 1.8 × 10-5 for CH3CO2H.

Identify the most common indicator.

A 1.00 L buffer solution is 0.150 M in HC7H5O2 and 0.250 M in LiC7H5O2.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl.The Ka for HC7H5O2 is 6.5 × 10-5.

A 25.0 mL sample of 0.150 M hypochlorous acid is titrated with a 0.150 M NaOH solution.What is the pH after 26.0 mL of base is added? The Ka of hypochlorous acid is 3.0 × 10-8.

The molar solubility of Ag2S is 1.26 × 10-16 M in pure water.Calculate the Ksp for Ag2S.

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous formic acid requires 29.80 mL of 0.3567 M NaOH? Ka = 1.8 × 10-4 for formic acid.

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.

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

A 25.0 mL sample of 0.150 M acetic acid is titrated with a 0.150 M NaOH solution.What is the pH at the equivalence point? The Ka of acetic acid is 4.50 × 10-4.

What is the molar solubility of AgCl in 0.10 M NaCN if the colorless complex ion Ag(CN) 2- forms? Ksp for AgCl is 1.8 × 10-10 and Kf for Ag(CN) 2- is 1.0 × 1021.

A 1.50 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 0.0500 moles of solid NaOH.Assume no volume change upon the addition of base.The Ka for HF is 3.5 × 10-4.

A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is 2.1 × 10-5 M in calcium ion and 4.75 × 10-5 M in oxalate ion.What will happen once these solutions are mixed? Ksp (CaC2O4) = 2.3 × 10-9.

Give the expression for the solubility product constant for PbCl2.

Fluffy,your prized Himalayan cat,was outside when your dad was changing the antifreeze in the car.Fluffy licked up a large amount of the antifreeze off the driveway.You live many miles from the veterinarian.What could you give Fluffy to drink to counteract the effects of antifreeze?

A solution contains 2.2 × 10-3 M in Cu2+ and 0.33 M in LiCN.If the Kf for Cu(CN) 42- is 1.0 × 1025,how much copper ion remains at equilibrium?

What is the pH of a solution made by mixing 10.00 mL of 0.10 M acetic acid with 10.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive.Ka = 1.8 × 10-5 for CH3CO2H.

What is the molar solubility of silver chloride (AgCl) in water? The solubility-product constant for AgCl is 1.8 × 10-10 at 25°C.

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

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M butanoic acid to the equivalence point? The K_a of butanoic acid is 1.5 × 10^-5.

Determine the molar solubility of BaF₂in pure water.K_sp (BaF₂) = 2.45 × 10^-5.

What is the pH of the resulting solution if 25.00 mL of 0.10 M acetic acid is added to 10.00 mL of 0.10 M NaOH? Assume that the volumes of the solutions are additive.K_a = 1.8 × 10^-5for CH₃CO₂H.

A 1.00 L buffer solution is 0.150 M in HC₇H₅O₂ and 0.250 M in LiC₇H₅O₂.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl.The K_a for HC₇H₅O₂ is 6.5 × 10^-5.

A 25.0 mL sample of 0.150 M hypochlorous acid is titrated with a 0.150 M NaOH solution.What is the pH after 26.0 mL of base is added? The K_a of hypochlorous acid is 3.0 × 10^-8.

The molar solubility of Ag₂S is 1.26 × 10^-16 M in pure water.Calculate the K_sp for Ag₂S.

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous formic acid requires 29.80 mL of 0.3567 M NaOH? K_a = 1.8 × 10^-4 for formic acid.

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.

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

A 25.0 mL sample of 0.150 M acetic acid is titrated with a 0.150 M NaOH solution.What is the pH at the equivalence point? The K_a of acetic acid is 4.50 × 10^-4.

What is the molar solubility of AgCl in 0.10 M NaCN if the colorless complex ion Ag(CN) ₂^- forms? K_sp for AgCl is 1.8 × 10^-10 and K_f for Ag(CN) ₂^- is 1.0 × 10²¹.

A 1.50 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 0.0500 moles of solid NaOH.Assume no volume change upon the addition of base.The K_a for HF is 3.5 × 10^-4.

A solution containing CaCl₂ is mixed with a solution of Li₂C₂O₄ to form a solution that is 2.1 × 10^-5 M in calcium ion and 4.75 × 10^-5 M in oxalate ion.What will happen once these solutions are mixed? K_sp (CaC₂O₄) = 2.3 × 10^-9.

Give the expression for the solubility product constant for PbCl₂.

A solution contains 2.2 × 10^-3M in Cu²⁺ and 0.33 M in LiCN.If the K_f for Cu(CN) ₄^2- is 1.0 × 10²⁵,how much copper ion remains at equilibrium?

What is the pH of a solution made by mixing 10.00 mL of 0.10 M acetic acid with 10.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive.K_a = 1.8 × 10^-5for CH₃CO₂H.

What is the molar solubility of silver chloride (AgCl) in water? The solubility-product constant for AgCl is 1.8 × 10^-10 at 25°C.