Question 1

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

Accepted Answer

A) 6.82 × 10-6 mol L-1 
B) 3.41 × 10-6 mol L-1 
C) 4.65 × 10-3 mol L-1 
D) 2.61 × 10-3 mol L-1 
E) 3.25 × 10-4 mol L-1 
A) 6.82 × 10-6 mol L-1 
B) 3.41 × 10-6 mol L-1 
C) 4.65 × 10-3 mol L-1 
D) 2.61 × 10-3 mol L-1 
E) 3.25 × 10-4 mol L-1

Question 2

A 100.0 mL sample of 0.10 mol L-1 Ca(OH)2 is titrated with 0.10 mol L-1 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 3

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 mol L-1 NH4Cl with 100.0 mL of 0.20 mol L-1 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 
A) 9.13 
B) 9.25 
C) 9.53 
D) 4.74 
E) 8.98

Question 4

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 mol L-1 
B) 3.6 × 10-10 mol L-1 
C) 9.74 mol L-1 
D) 1.9 × 10-5 mol L-1 
E) 1.3 × 10-5 mol L-1 
A) 9.0 × 10-11 mol L-1 
B) 3.6 × 10-10 mol L-1 
C) 9.74 mol L-1 
D) 1.9 × 10-5 mol L-1 
E) 1.3 × 10-5 mol L-1

Question 5

A 100.0 mL sample of 0.10 mol L-1 NH3 is titrated with 0.10 mol L-1 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 
A) 4.74 
B) 7.78 
C) 7.05 
D) 9.26 
E) 10.34

Question 6

You wish to prepare a buffer containing CH3COOH with a pH of 5.44. If the pKa of acetic acid is 4.74, what ratio of CH3COO⁻/CH3COOH must you use?

Accepted Answer

A) 0.70 
B) 0.20 
C) 1.4 
D) 5.0 
E) 1.1 
A) 0.70 
B) 0.20 
C) 1.4 
D) 5.0 
E) 1.1

Question 7

Describe the solubility of Al(OH)3 with respect to pH.

Accepted Answer

A) soluble at low pH, insoluble in pH-neutral solution, and soluble at high pH 
B) soluble at low pH, insoluble in pH-neutral solution, and insoluble at high pH 
C) insoluble at low pH, insoluble in pH-neutral solution, and soluble at high pH 
D) soluble at low pH, in pH-neutral solution, and at high pH 
E) insoluble at low pH, in pH-neutral solution, and at high pH 
A) soluble at low pH, insoluble in pH-neutral solution, and soluble at high pH 
B) soluble at low pH, insoluble in pH-neutral solution, and insoluble at high pH 
C) insoluble at low pH, insoluble in pH-neutral solution, and soluble at high pH 
D) soluble at low pH, in pH-neutral solution, and at high pH 
E) insoluble at low pH, in pH-neutral solution, and at high pH

Question 8

A 100.0 mL sample of 0.18 mol L-1 HClO4 is titrated with 0.27 mol L-1 NaOH. Determine the pH of the solution before the addition of any NaOH.

Accepted Answer

A) 1.74 
B) 1.05 
C) 0.74 
D) 0.57 
E) 1.57 
A) 1.74 
B) 1.05 
C) 0.74 
D) 0.57 
E) 1.57

Question 9

Solid potassium chromate (K2CrO4)is slowly added to a solution containing 0.50 mol L-1 AgNO3 and 0.50 mol L-1 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 mol L-1 
B) 1.3 × 10-4 mol L-1 
C) 3.2 × 10-4 mol L-1 
D) 6.8 × 10-2 mol L-1 
A) 6.5 × 10-5 mol L-1 
B) 1.3 × 10-4 mol L-1 
C) 3.2 × 10-4 mol L-1 
D) 6.8 × 10-2 mol L-1

Question 10

A 100.0 mL sample of 0.10 mol L-1 NH3 is titrated with 0.10 mol L-1 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 
A) 6.58 
B) 10.56 
C) 8.72 
D) 3.44 
E) 5.28

Question 11

Calculate the pH of a buffer that is 0.020 mol L-1 HF and 0.040 mol L-1 LiF. The Ka for HF is 3.5 × 10-4.

Accepted Answer

A) 2.06 
B) 4.86 
C) 3.16 
D) 3.46 
E) 3.76 
A) 2.06 
B) 4.86 
C) 3.16 
D) 3.46 
E) 3.76

Question 12

Calculate the solubility (in g L-1)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-1 
B) 2.6 × 10-2 g L-1 
C) 3.3 × 10-2 g L-1 
D) 4.1 × 10-2 g L-1 
A) 9.6 × 10-4 g L-1 
B) 2.6 × 10-2 g L-1 
C) 3.3 × 10-2 g L-1 
D) 4.1 × 10-2 g L-1

Question 13

What is the pH of a solution made by mixing 30.00 mL of 0.10 mol L-1 acetic acid (CH3COOH)with 50.00 mL of 0.100 mol L-1 KOH? Assume that the volumes of the solutions are additive. Ka = 1.8 × 10-5 for CH3COOH.

Accepted Answer

A) 8.26 
B) 9.26 
C) 11.13 
D) 12.40 
A) 8.26 
B) 9.26 
C) 11.13 
D) 12.40

Question 14

Calculate the molar solubility of thallium chloride (TlCl)in 0.40 mol L-1 NaCl at 25 °C. Ksp for TlCl is 1.7 × 10-4.

Accepted Answer

A) 6.8 × 10-5 mol L-1 
B) 4.2 × 10-4 mol L-1 
C) 8.2 × 10-3 mol L-1 
D) 1.3 × 10-2 mol L-1 
A) 6.8 × 10-5 mol L-1 
B) 4.2 × 10-4 mol L-1 
C) 8.2 × 10-3 mol L-1 
D) 1.3 × 10-2 mol L-1

Question 15

Which of the following compounds' solubility will not be affected by a low pH in solution?

Accepted Answer

A) AgCl 
B) Mg(OH)2 
C) CaF2 
D) CuS 
E) BaCO3 
A) AgCl 
B) Mg(OH)2 
C) CaF2 
D) CuS 
E) BaCO3

Question 16

A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is 3.5 × 10-4 mol L-1 in calcium ion and 2.33 × 10-4 mol L-1 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 because 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) Nothing will happen because Q = Ksp. 
A) Nothing will happen since both calcium chloride and lithium oxalate are soluble compounds. 
B) Nothing will happen because 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) Nothing will happen because Q = Ksp.

Question 17

A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 mol L-1 in AgNO3 and 0.075 mol L-1 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 the solution, leaving an unsaturated solution of AgCl. 
C) Silver chloride will precipitate out of the solution, leaving a saturated AgCl solution. 
D) Nothing will happen since NaCl and AgNO3 are both soluble compounds. 
E) Silver chloride will precipitate, leaving a pure solution of NaNO3. 
A) Nothing will happen since the molar solubility of AgCl is higher than the solution concentrations. 
B) Silver chloride will precipitate out of the solution, leaving an unsaturated solution of AgCl. 
C) Silver chloride will precipitate out of the solution, leaving a saturated AgCl solution. 
D) Nothing will happen since NaCl and AgNO3 are both soluble compounds. 
E) Silver chloride will precipitate, leaving a pure solution of NaNO3.

Question 18

Calculate the pH of a buffer that is 0.040 mol L-1 HF and 0.020 mol L-1 LiF. The Ka for HF is 3.5 × 10-4.

Accepted Answer

A) 2.06 
B) 4.86 
C) 3.15 
D) 3.46 
E) 3.76 
A) 2.06 
B) 4.86 
C) 3.15 
D) 3.46 
E) 3.76

Question 19

What is the pH of a solution made by mixing 25.00 mL of 0.100 mol L-1 HCl with 40.00 mL of 0.100 mol L-1 KOH? Assume that the volumes of the solutions are additive.

Accepted Answer

A) 0.64 
B) 1.64 
C) 12.36 
D) 13.36 
A) 0.64 
B) 1.64 
C) 12.36 
D) 13.36

Question 20

Which of the following is the correct equation relating Q to Ksp for an unsaturated solution?

Accepted Answer

A) Q > Ksp 
B) Q sp 
C) Q = Ksp 
D) Q ≠ Ksp 
E) Q ≥ Ksp 
A) Q > Ksp 
B) Q sp 
C) Q = Ksp 
D) Q ≠ Ksp 
E) Q ≥ Ksp

Exam 16: Aqueous Ionic Equilibrium

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

A 100.0 mL sample of 0.10 mol L-1 Ca(OH)2 is titrated with 0.10 mol L-1 HBr. Determine the pH of the solution after the addition of 200.0 mL HBr.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 mol L-1 NH4Cl with 100.0 mL of 0.20 mol L-1 NH3. The Kb for NH3 is 1.8 × 10-5.

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.

A 100.0 mL sample of 0.10 mol L-1 NH3 is titrated with 0.10 mol L-1 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.

You wish to prepare a buffer containing CH3COOH with a pH of 5.44. If the pKa of acetic acid is 4.74, what ratio of CH3COO⁻/CH3COOH must you use?

Describe the solubility of Al(OH)3 with respect to pH.

A 100.0 mL sample of 0.18 mol L-1 HClO4 is titrated with 0.27 mol L-1 NaOH. Determine the pH of the solution before the addition of any NaOH.

Solid potassium chromate (K2CrO4)is slowly added to a solution containing 0.50 mol L-1 AgNO3 and 0.50 mol L-1 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.

A 100.0 mL sample of 0.10 mol L-1 NH3 is titrated with 0.10 mol L-1 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.

Calculate the pH of a buffer that is 0.020 mol L-1 HF and 0.040 mol L-1 LiF. The Ka for HF is 3.5 × 10-4.

Calculate the solubility (in g L-1)of calcium fluoride in water at 25 °C if the Ksp for CaF2 is 1.5 × 10-10.

What is the pH of a solution made by mixing 30.00 mL of 0.10 mol L-1 acetic acid (CH3COOH)with 50.00 mL of 0.100 mol L-1 KOH? Assume that the volumes of the solutions are additive. Ka = 1.8 × 10-5 for CH3COOH.

Calculate the molar solubility of thallium chloride (TlCl)in 0.40 mol L-1 NaCl at 25 °C. Ksp for TlCl is 1.7 × 10-4.

Which of the following compounds' solubility will not be affected by a low pH in solution?

A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is 3.5 × 10-4 mol L-1 in calcium ion and 2.33 × 10-4 mol L-1 in oxalate ion. What will happen once these solutions are mixed? Ksp (CaC2O4)= 2.3 × 10-9.

A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 mol L-1 in AgNO3 and 0.075 mol L-1 in NaCl. What will happen once these solutions are mixed? Ksp (AgCl)= 1.77 × 10-10.

Calculate the pH of a buffer that is 0.040 mol L-1 HF and 0.020 mol L-1 LiF. The Ka for HF is 3.5 × 10-4.

What is the pH of a solution made by mixing 25.00 mL of 0.100 mol L-1 HCl with 40.00 mL of 0.100 mol L-1 KOH? Assume that the volumes of the solutions are additive.

Which of the following is the correct equation relating Q to Ksp for an unsaturated solution?

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Filters

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

A 100.0 mL sample of 0.10 mol L^-1 Ca(OH)₂ is titrated with 0.10 mol L^-1 HBr. Determine the pH of the solution after the addition of 200.0 mL HBr.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 mol L^-1 NH₄Cl with 100.0 mL of 0.20 mol L^-1 NH₃. The K_b for NH₃ is 1.8 × 10^-5.

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.

A 100.0 mL sample of 0.10 mol L^-1 NH₃ is titrated with 0.10 mol L^-1 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.

You wish to prepare a buffer containing CH₃COOH with a pH of 5.44. If the pK_a of acetic acid is 4.74, what ratio of CH₃COO⁻/CH₃COOH must you use?

Describe the solubility of Al(OH)₃ with respect to pH.

A 100.0 mL sample of 0.18 mol L^-1 HClO₄ is titrated with 0.27 mol L^-1 NaOH. Determine the pH of the solution before the addition of any NaOH.

Solid potassium chromate (K₂CrO₄)is slowly added to a solution containing 0.50 mol L^-1 AgNO₃ and 0.50 mol L^-1 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.

A 100.0 mL sample of 0.10 mol L^-1 NH₃ is titrated with 0.10 mol L^-1 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.

Calculate the pH of a buffer that is 0.020 mol L^-1 HF and 0.040 mol L^-1 LiF. The K_a for HF is 3.5 × 10^-4.

Calculate the solubility (in g L^-1)of calcium fluoride in water at 25 °C if the K_sp for CaF₂ is 1.5 × 10^-10.

What is the pH of a solution made by mixing 30.00 mL of 0.10 mol L^-1 acetic acid (CH₃COOH)with 50.00 mL of 0.100 mol L^-1 KOH? Assume that the volumes of the solutions are additive. K_a = 1.8 × 10^-5for CH₃COOH.

Calculate the molar solubility of thallium chloride (TlCl)in 0.40 mol L^-1 NaCl at 25 °C. K_sp for TlCl is 1.7 × 10^-4.

A solution containing CaCl₂ is mixed with a solution of Li₂C₂O₄ to form a solution that is 3.5 × 10^-4 mol L^-1 in calcium ion and 2.33 × 10^-4mol L^-1 in oxalate ion. What will happen once these solutions are mixed? K_sp (CaC₂O₄)= 2.3 × 10^-9.

A solution containing AgNO₃ is mixed with a solution of NaCl to form a solution that is 0.10 mol L^-1 in AgNO₃ and 0.075 mol L^-1 in NaCl. What will happen once these solutions are mixed? K_sp (AgCl)= 1.77 × 10^-10.

Calculate the pH of a buffer that is 0.040 mol L^-1 HF and 0.020 mol L^-1 LiF. The K_a for HF is 3.5 × 10^-4.

What is the pH of a solution made by mixing 25.00 mL of 0.100 mol L^-1 HCl with 40.00 mL of 0.100 mol L^-1 KOH? Assume that the volumes of the solutions are additive.

Which of the following is the correct equation relating Q to K_sp for an unsaturated solution?