Question 1

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 
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 2

What is the pH of the resulting solution if 45 mL of 0.432 M methylamine,CH3NH2,is added to 15 mL of 0.234 M HCl? Assume that the volumes of the solutions are additive.Ka = 2.70 × 10-11 for CH3NH3+.

Accepted Answer

A) 2.77 
B) 4.09 
C) 9.91 
D) 11.23 
A) 2.77 
B) 4.09 
C) 9.91 
D) 11.23

Question 3

Calculate the pH of a buffer that is 0.060 M HF and 0.030 M KF.The Ka for HF is 3.5 × 10-4.

Accepted Answer

A) 2.06 
B) 4.86 
C) 3.16 
D) 3.56 
E) 3.76 
A) 2.06 
B) 4.86 
C) 3.16 
D) 3.56 
E) 3.76

Question 4

Describe the information necessary (and why)to choose a good indicator for a weak acid/strong base titration.

Accepted Answer

To choose an appropriate indic

Question 5

A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is
3.5 × 10-4 M in calcium ion and 2.33 × 10-4 M in oxalate ion.What will happen once these solutions are mixed? Ksp (CaC2O4)= 2.3 × 10-9.

Accepted Answer

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

Question 6

A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M HBr.Determine the pH of the solution after the addition of 300.0 mL HBr.

Accepted Answer

A) 1.60 
B) 1.30 
C) 1.00 
D) 12.40 
E) 1.12 
A) 1.60 
B) 1.30 
C) 1.00 
D) 12.40 
E) 1.12

Question 7

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) 10.06 
C) 10.25 
D) 11.13 
A) 8.25 
B) 10.06 
C) 10.25 
D) 11.13

Question 8

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.Determine the pH of the solution after the addition of 400.0 mL of KOH.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 
A) 13.08 
B) 12.60 
C) 13.85 
D) 12.30 
E) 12.78

Question 9

Determine the molar solubility of CuCl in a solution containing 0.050 M KCl.Ksp (CuCl)= 1.0 × 10-6.

Accepted Answer

A) 1.0 × 10-12 M 
B) 5.0 × 10-7 M 
C) 2.0 × 10-5 M 
D) 1.0 × 10-3 M 
E) 0.050 M 
A) 1.0 × 10-12 M 
B) 5.0 × 10-7 M 
C) 2.0 × 10-5 M 
D) 1.0 × 10-3 M 
E) 0.050 M

Question 10

Which of the following acids (listed with Ka values)and their conjugate base would form a buffer with a pH of 2.34?

Accepted Answer

A) HC7H5O2,Ka = 6.5 × 10-5 
B) HF,Ka = 3.5 × 10-4 
C) HClO,Ka = 2.9 × 10-8 
D) HCN,Ka = 4.9 × 10-10 
E) HClO2,Ka = 1.1 × 10-2 
A) HC7H5O2,Ka = 6.5 × 10-5 
B) HF,Ka = 3.5 × 10-4 
C) HClO,Ka = 2.9 × 10-8 
D) HCN,Ka = 4.9 × 10-10 
E) HClO2,Ka = 1.1 × 10-2

Question 11

You wish to prepare an HC2H3O2 buffer with a pH of 4.24.If the pKa of is 4.74,what ratio of
C2H3O2-/HC2H3O2 must you use?

Accepted Answer

A) 0.10 
B) 0.50 
C) 0.32 
D) 2.0 
E) 2.8 
A) 0.10 
B) 0.50 
C) 0.32 
D) 2.0 
E) 2.8

Question 12

Determine the molar solubility of MgCO3 in pure water.Ksp (MgCO3)= 6.82 × 10-6.

Accepted Answer

A) 6.82 × 10-6 M 
B) 3.41 × 10-6 M 
C) 4.65 × 10-3 M 
D) 2.61 × 10-3 M 
E) 3.25 × 10-4 M 
A) 6.82 × 10-6 M 
B) 3.41 × 10-6 M 
C) 4.65 × 10-3 M 
D) 2.61 × 10-3 M 
E) 3.25 × 10-4 M

Question 13

A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO3 and 0.075 M in NaCl.What will happen once these solutions are mixed?
Ksp (AgCl)= 1.77 × 10-10.

Accepted Answer

A) Nothing will happen since the molar solubility of AgCl is higher than the solution concentrations. 
B) Silver chloride will precipitate out of solution,leaving an unsaturated solution of AgCl. 
C) Silver chloride will precipitate out of solution,leaving a saturated AgCl solution. 
D) Nothing will happen since NaCl and AgNO3 are both soluble compounds. 
E) There is not enough information to say anything about this solution. 
A) Nothing will happen since the molar solubility of AgCl is higher than the solution concentrations. 
B) Silver chloride will precipitate out of solution,leaving an unsaturated solution of AgCl. 
C) Silver chloride will precipitate out of solution,leaving a saturated AgCl solution. 
D) Nothing will happen since NaCl and AgNO3 are both soluble compounds. 
E) There is not enough information to say anything about this solution.

Question 14

How many milliliters of 0.0850 M NaOH are required to titrate 25.0 mL of 0.0720 M HBr to the equivalence point?

Accepted Answer

A) 21.2 
B) 0.245 
C) 3.92 
D) 0.153 
E) 29.5 
A) 21.2 
B) 0.245 
C) 3.92 
D) 0.153 
E) 29.5

Question 15

A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M HBr.Determine the pH of the solution after the addition of 200.0 mL HBr.

Accepted Answer

A) 2.62 
B) 2.00 
C) 1.48 
D) 12.52 
E) 7.00 
A) 2.62 
B) 2.00 
C) 1.48 
D) 12.52 
E) 7.00

Question 16

Determine the molar solubility of CaSO4 in a solution containing 0.100 M Na2SO4.
Ksp (CaSO4)= 2.4 × 10-5.

Accepted Answer

A) 4.9 × 10-3 M 
B) 2.4 × 10-4 M 
C) 5.8 × 10-10 M 
D) 1.2 × 10-5 M 
E) 0.10 M 
A) 4.9 × 10-3 M 
B) 2.4 × 10-4 M 
C) 5.8 × 10-10 M 
D) 1.2 × 10-5 M 
E) 0.10 M

Question 17

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4Cl with 200.0 mL of
0.12 M NH3.The Kb for NH3 is 1.8 × 10-5.

Accepted Answer

A) 9.06 
B) 9.45 
C) 4.55 
D) 4.74 
E) 9.26 
A) 9.06 
B) 9.45 
C) 4.55 
D) 4.74 
E) 9.26

Question 18

Which of the following compounds will be more soluble in acidic solution than in pure water?

Accepted Answer

A) PbCl2 
B) FeS 
C) Ca(ClO4)2 
D) CuI 
E) None of the above will be more soluble in acidic solution. 
A) PbCl2 
B) FeS 
C) Ca(ClO4)2 
D) CuI 
E) None of the above will be more soluble in acidic solution.

Question 19

Calculate the solubility (in g/L)of calcium fluoride in water at 25°C if the Ksp for CaF2 is 1.5 × 10-10.

Accepted Answer

A) 9.6 × 10-4 g/L 
B) 2.6 × 10-2 g/L 
C) 3.3 × 10-2 g/L 
D) 4.1 × 10-2 g/L 
A) 9.6 × 10-4 g/L 
B) 2.6 × 10-2 g/L 
C) 3.3 × 10-2 g/L 
D) 4.1 × 10-2 g/L

Question 20

Calculate the Ksp for silver sulfite if the solubility in pure water is 4.6 × 10-3 g/L.

Accepted Answer

A) 3.8 × 10-15 
B) 1.5 × 10-14 
C) 2.4 × 10-10 
D) 4.8 × 10-10 
A) 3.8 × 10-15 
B) 1.5 × 10-14 
C) 2.4 × 10-10 
D) 4.8 × 10-10

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

What is the pH of the resulting solution if 45 mL of 0.432 M methylamine,CH₃NH₂,is added to 15 mL of 0.234 M HCl? Assume that the volumes of the solutions are additive.K_a = 2.70 × 10^-11for CH₃NH₃⁺.

Calculate the pH of a buffer that is 0.060 M HF and 0.030 M KF.The K_a for HF is 3.5 × 10^-4.

Describe the information necessary (and why)to choose a good indicator for a weak acid/strong base titration.

A solution containing CaCl₂ is mixed with a solution of Li₂C₂O₄ to form a solution that is 3.5 × 10^-4 M in calcium ion and 2.33 × 10^-4M in oxalate ion.What will happen once these solutions are mixed? K_sp (CaC₂O₄)= 2.3 × 10^-9.

A 100.0 mL sample of 0.10 M Ca(OH)₂ is titrated with 0.10 M HBr.Determine the pH of the solution after the addition of 300.0 mL HBr.

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.

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.Determine the pH of the solution after the addition of 400.0 mL of KOH.The K_a of HF is 3.5 × 10^-4.

Determine the molar solubility of CuCl in a solution containing 0.050 M KCl.K_sp (CuCl)= 1.0 × 10^-6.

Which of the following acids (listed with K_a values)and their conjugate base would form a buffer with a pH of 2.34?

You wish to prepare an HC₂H₃O₂ buffer with a pH of 4.24.If the pK_a of is 4.74,what ratio of C₂H₃O₂^-/HC₂H₃O₂ must you use?

Determine the molar solubility of MgCO₃in pure water.K_sp (MgCO₃)= 6.82 × 10^-6.

A solution containing AgNO₃ is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO₃ and 0.075 M in NaCl.What will happen once these solutions are mixed? K_sp (AgCl)= 1.77 × 10^-¹⁰.

How many milliliters of 0.0850 M NaOH are required to titrate 25.0 mL of 0.0720 M HBr to the equivalence point?

A 100.0 mL sample of 0.10 M Ca(OH)₂ is titrated with 0.10 M HBr.Determine the pH of the solution after the addition of 200.0 mL HBr.

Determine the molar solubility of CaSO₄ in a solution containing 0.100 M Na₂SO₄. K_sp (CaSO₄)= 2.4 × 10^-5.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH₄Cl with 200.0 mL of 0.12 M NH₃.The K_b for NH₃ is 1.8 × 10^-5.

Which of the following compounds will be more soluble in acidic solution than in pure water?

Calculate the solubility (in g/L)of calcium fluoride in water at 25°C if the K_sp for CaF₂ is 1.5 × 10^-10.

Calculate the K_sp for silver sulfite if the solubility in pure water is 4.6 × 10^-3g/L.

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Exam 16: Aqueous Ionic Equilibrium

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

What is the pH of the resulting solution if 45 mL of 0.432 M methylamine,CH3NH2,is added to 15 mL of 0.234 M HCl? Assume that the volumes of the solutions are additive.Ka = 2.70 × 10-11 for CH3NH3+.

Calculate the pH of a buffer that is 0.060 M HF and 0.030 M KF.The Ka for HF is 3.5 × 10-4.

Describe the information necessary (and why)to choose a good indicator for a weak acid/strong base titration.

A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is 3.5 × 10-4 M in calcium ion and 2.33 × 10-4 M in oxalate ion.What will happen once these solutions are mixed? Ksp (CaC2O4)= 2.3 × 10-9.

A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M HBr.Determine the pH of the solution after the addition of 300.0 mL HBr.

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.

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.Determine the pH of the solution after the addition of 400.0 mL of KOH.The Ka of HF is 3.5 × 10-4.

Determine the molar solubility of CuCl in a solution containing 0.050 M KCl.Ksp (CuCl)= 1.0 × 10-6.

Which of the following acids (listed with Ka values)and their conjugate base would form a buffer with a pH of 2.34?

You wish to prepare an HC2H3O2 buffer with a pH of 4.24.If the pKa of is 4.74,what ratio of C2H3O2-/HC2H3O2 must you use?

Determine the molar solubility of MgCO3 in pure water.Ksp (MgCO3)= 6.82 × 10-6.

A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO3 and 0.075 M in NaCl.What will happen once these solutions are mixed? Ksp (AgCl)= 1.77 × 10-10.

How many milliliters of 0.0850 M NaOH are required to titrate 25.0 mL of 0.0720 M HBr to the equivalence point?

A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M HBr.Determine the pH of the solution after the addition of 200.0 mL HBr.

Determine the molar solubility of CaSO4 in a solution containing 0.100 M Na2SO4. Ksp (CaSO4)= 2.4 × 10-5.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4Cl with 200.0 mL of 0.12 M NH3.The Kb for NH3 is 1.8 × 10-5.

Which of the following compounds will be more soluble in acidic solution than in pure water?

Calculate the solubility (in g/L)of calcium fluoride in water at 25°C if the Ksp for CaF2 is 1.5 × 10-10.

Calculate the Ksp for silver sulfite if the solubility in pure water is 4.6 × 10-3 g/L.

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

What is the pH of the resulting solution if 45 mL of 0.432 M methylamine,CH₃NH₂,is added to 15 mL of 0.234 M HCl? Assume that the volumes of the solutions are additive.K_a = 2.70 × 10^-11for CH₃NH₃⁺.

Calculate the pH of a buffer that is 0.060 M HF and 0.030 M KF.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 3.5 × 10^-4 M in calcium ion and 2.33 × 10^-4M in oxalate ion.What will happen once these solutions are mixed? K_sp (CaC₂O₄)= 2.3 × 10^-9.

A 100.0 mL sample of 0.10 M Ca(OH)₂ is titrated with 0.10 M HBr.Determine the pH of the solution after the addition of 300.0 mL HBr.

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.

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.Determine the pH of the solution after the addition of 400.0 mL of KOH.The K_a of HF is 3.5 × 10^-4.

Determine the molar solubility of CuCl in a solution containing 0.050 M KCl.K_sp (CuCl)= 1.0 × 10^-6.

Which of the following acids (listed with K_a values)and their conjugate base would form a buffer with a pH of 2.34?

You wish to prepare an HC₂H₃O₂ buffer with a pH of 4.24.If the pK_a of is 4.74,what ratio of C₂H₃O₂^-/HC₂H₃O₂ must you use?

Determine the molar solubility of MgCO₃in pure water.K_sp (MgCO₃)= 6.82 × 10^-6.

A solution containing AgNO₃ is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO₃ and 0.075 M in NaCl.What will happen once these solutions are mixed? K_sp (AgCl)= 1.77 × 10^-¹⁰.

A 100.0 mL sample of 0.10 M Ca(OH)₂ is titrated with 0.10 M HBr.Determine the pH of the solution after the addition of 200.0 mL HBr.

Determine the molar solubility of CaSO₄ in a solution containing 0.100 M Na₂SO₄. K_sp (CaSO₄)= 2.4 × 10^-5.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH₄Cl with 200.0 mL of 0.12 M NH₃.The K_b for NH₃ is 1.8 × 10^-5.

Calculate the solubility (in g/L)of calcium fluoride in water at 25°C if the K_sp for CaF₂ is 1.5 × 10^-10.

Calculate the K_sp for silver sulfite if the solubility in pure water is 4.6 × 10^-3g/L.