Potassium chromate is slowly added to a solution containing 0.20 M AgNO3 and 0.20 M Ba(NO3)2.Describe what happens if the Ksp for Ag2CrO4 is 1.1 × 10-12 and the Ksp of BaCrO4 is 1.2 × 10-10.

A) The BaCrO4 precipitates first out of solution. B) The Ag2CrO4 precipitates first out of solution and then BaCrO4 precipitates. C) Both BaCrO4 and Ag2CrO4 precipitate simultaneously out of solution. D) Neither BaCrO4 nor Ag2CrO4 precipitates out of solution. A) The BaCrO4 precipitates first out of solution. B) The Ag2CrO4 precipitates first out of solution and then BaCrO4 precipitates. C) Both BaCrO4 and Ag2CrO4 precipitate simultaneously out of solution. D) Neither BaCrO4 nor Ag2CrO4 precipitates out of solution.

Consider a buffered solution consisting of H2CO3 and HCO3- where the pKa = 6.4.At pH = 6.4,which of the following is true?

A) [H2CO3] > [HCO3-] B) [H2CO3]3-] C) [H2CO3] = [HCO3-] D) [H2CO3] 3-2] A) [H2CO3] > [HCO3-] B) [H2CO3]3-] C) [H2CO3] = [HCO3-] D) [H2CO3] 3-2]

What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.00? Ksp for Mg(OH)2 is

A) 5.6 × 10-10 M B) 5.6 × 10-8 M C) 2.4 × 10-6 M D) 1.1 × 10-4 M A) 5.6 × 10-10 M B) 5.6 × 10-8 M C) 2.4 × 10-6 M D) 1.1 × 10-4 M

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid HS1U1B12S1U1B0A with NaOH. -Which point a-d represents the HX-/X2- buffer region?

A) point a B) point b C) point c D) point d A) point a B) point b C) point c D) point d

When 70 mL of 0.18 M NH4Cl is added to 70 mL of 0.18 M NH3,relative to the pH of the 0.10 M NH3 solution the pH of the resulting solution will

A) become 7. B) decrease. C) increase. D) remain the same. A) become 7. B) decrease. C) increase. D) remain the same.

The following pictures represent solutions at various stages in the titration of a weak diprotic acid HS1U1B12S1U1B0A with aqueous KOH.Unshaded spheres represent H atoms,black spheres represent oxygen atoms,and shaded spheres represent AS1U1P12-S1S1P0 ions.(KS1U1P1+S1S1P0,HS1U1B13S1U1B0OS1U1P1+S1S1P0 initially present,OHS1U1P1-S1S1P0 initially present and solvent water molecules have been omitted for clarity). -Which picture represents the system with the lowest pH?

A) (1) B) (2) C) (3) D) (4) A) (1) B) (2) C) (3) D) (4)

The following pictures represent solutions that contain a weak acid HA (pKS1U1B1aS1U1B0 = 5.0)and its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent AS1U1P1-S1S1P0 ions.(KS1U1P1+S1S1P0,HS1U1B13S1U1B0OS1U1P1+S1S1P0,OHS1U1P1-S1S1P0,and solvent HS1U1B12S1U1B0O molecules have been omitted for clarity. ) -Which of these solutions are buffers?

A) (1)and (2) B) (1)and (3) C) (1), (2)and (3) D) All are buffer solutions. A) (1)and (2) B) (1)and (3) C) (1), (2)and (3) D) All are buffer solutions.

The following pictures represent solutions that contain a weak acid HA (pKS1U1B1aS1U1B0 = 5.0)and its potassium salt KA.Unshaded spheres represent H atoms,black spheres represent oxygen atoms,and shaded spheres represent AS1U1P1-S1S1P0 ions.(KS1U1P1+S1S1P0,HS1U1B13S1U1B0OS1U1P1+ S1S1P0initially present,OHS1U1P1- S1S1P0initially present and solvent water molecules have been omitted for clarity. ) -Which picture represents the equilibrium state of the solution after addition of one H3O+ ion to the solution shown in picture (1)?

A) (2) B) (3) C) (4) D) (5) A) (2) B) (3) C) (4) D) (5)

The following pictures represent solutions that contain a weak acid HA (pKS1U1B1aS1U1B0 = 5.0)and its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent AS1U1P1-S1S1P0 ions.(KS1U1P1+S1S1P0,HS1U1B13S1U1B0OS1U1P1+S1S1P0,OHS1U1P1-S1S1P0,and solvent HS1U1B12S1U1B0O molecules have been omitted for clarity. ) -Which solution has the lowest pH?

A) (1) B) (2) C) (3) D) (4) A) (1) B) (2) C) (3) D) (4)

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M methylamine,CH3NH2,with 15.00 mL of 0.10 M methylammonium chloride,CH3NH3Cl? Assume that the volume of the solutions are additive and that Kb = 3.70 × 10-4 for methylamine.

A) 10.04 B) 10.57 C) 11.09 D) 11.78 A) 10.04 B) 10.57 C) 11.09 D) 11.78

Exam 16: Applications of Aqueous Equilibria

Selenous acid,H₂SeO₃ has acid dissociation constants K_a1 = 3.5 × 10^-2 and K_a2 = 5 × 10^-8.When 25.00 mL of 0.100 M selenous acid is titrated with 0.200 M NaOH the first equivalence point occurs at pH = ________.

(Short Answer)

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Question 61

What is the pH of the resulting solution if 40.00 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.

(Multiple Choice)

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Question 62

Potassium chromate is slowly added to a solution containing 0.20 M AgNO₃ and 0.20 M Ba(NO₃)₂.Describe what happens if the K_sp for Ag₂CrO₄ is 1.1 × 10^-12 and the K_sp of BaCrO₄ is 1.2 × 10^-10.

(Multiple Choice)

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Question 63

What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 40.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive.K_a = 1.8 × 10^-5for CH₃CO₂H.

(Multiple Choice)

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Question 64

What is the equilibrium constant expression for the K_sp of Sr₃(PO₄)₂?

(Multiple Choice)

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Question 65

Use the graphs below to answer the following questions. -What is the characteristic pH-titrant curve for the titration of a strong base by a strong acid?

(Multiple Choice)

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Question 66

Consider a buffered solution consisting of H₂CO₃ and HCO₃^- where the pKa = 6.4.At pH = 6.4,which of the following is true?

(Multiple Choice)

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Question 67

What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.00? K_sp for Mg(OH)₂ is

(Multiple Choice)

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Question 68

Oxalic acid,H₂C₂O₄ has acid dissociation constants K_a1 = 5.9 × 10^-2 and K_a2 = 6.4 × 10^-5.What is the pH after 20.00 mL of 0.0500 M NaOH is added to 5.00 mL of 0.2000 M H₂C₂O₄?

(Multiple Choice)

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Question 69

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H₂A with NaOH. -Which point a-d represents the HX^-/X2^- buffer region?

(Multiple Choice)

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Question 70

CaF₂ has K_sp = 3.5 × 10^-11.If 25 mL of 8.0 × 10^-4 M Ca(NO₃)₂ is mixed with 75 mL of 4.0 × 10^-4 M KF,a precipitate of CaF₂ ________ (will,will not)form.

(Short Answer)

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Question 71

When 70 mL of 0.18 M NH₄Cl is added to 70 mL of 0.18 M NH₃,relative to the pH of the 0.10 M NH₃solution the pH of the resulting solution will

(Multiple Choice)

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Question 72

The following pictures represent solutions at various stages in the titration of a weak diprotic acid H₂A with aqueous KOH.Unshaded spheres represent H atoms,black spheres represent oxygen atoms,and shaded spheres represent A^2- ions.(K⁺,H₃O⁺ initially present,OH^- initially present and solvent water molecules have been omitted for clarity). -Which picture represents the system with the lowest pH?

(Multiple Choice)

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Question 73

What is the most soluble salt of the following set?

(Multiple Choice)

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Question 74

The following pictures represent solutions that contain a weak acid HA (pK_a = 5.0)and its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent A^- ions.(K⁺,H₃O⁺,OH^-,and solvent H₂O molecules have been omitted for clarity. ) -Which of these solutions are buffers?

(Multiple Choice)

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Question 75

The following pictures represent solutions that contain a weak acid HA (pK_a = 5.0)and its potassium salt KA.Unshaded spheres represent H atoms,black spheres represent oxygen atoms,and shaded spheres represent A^- ions.(K⁺,H₃O⁺initially present,OH^-initially present and solvent water molecules have been omitted for clarity. ) -Which picture represents the equilibrium state of the solution after addition of one H₃O⁺ ion to the solution shown in picture (1)?

(Multiple Choice)

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Question 76

The following pictures represent solutions that contain a weak acid HA (pK_a = 5.0)and its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent A^- ions.(K⁺,H₃O⁺,OH^-,and solvent H₂O molecules have been omitted for clarity. ) -Which solution has the lowest pH?

(Multiple Choice)

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Question 77

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M methylamine,CH₃NH₂,with 15.00 mL of 0.10 M methylammonium chloride,CH₃NH₃Cl? Assume that the volume of the solutions are additive and that K_b = 3.70 × 10^-4 for methylamine.

(Multiple Choice)

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Question 78

Which statement about buffers is true?

(Multiple Choice)

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Question 79

Which set of ions precipitate as sulfides?

(Multiple Choice)

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Question 80

Showing 61 - 80 of 201

Selenous acid,H₂SeO₃ has acid dissociation constants K_a1 = 3.5 × 10^-2 and K_a2 = 5 × 10^-8.When 25.00 mL of 0.100 M selenous acid is titrated with 0.200 M NaOH the first equivalence point occurs at pH = ________.

What is the pH of the resulting solution if 40.00 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.

Potassium chromate is slowly added to a solution containing 0.20 M AgNO₃ and 0.20 M Ba(NO₃)₂.Describe what happens if the K_sp for Ag₂CrO₄ is 1.1 × 10^-12 and the K_sp of BaCrO₄ is 1.2 × 10^-10.

What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 40.00 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 equilibrium constant expression for the K_sp of Sr₃(PO₄)₂?

Use the graphs below to answer the following questions. -What is the characteristic pH-titrant curve for the titration of a strong base by a strong acid?

Consider a buffered solution consisting of H₂CO₃ and HCO₃^- where the pKa = 6.4.At pH = 6.4,which of the following is true?

What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.00? K_sp for Mg(OH)₂ is

Oxalic acid,H₂C₂O₄ has acid dissociation constants K_a1 = 5.9 × 10^-2 and K_a2 = 6.4 × 10^-5.What is the pH after 20.00 mL of 0.0500 M NaOH is added to 5.00 mL of 0.2000 M H₂C₂O₄?

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H₂A with NaOH. -Which point a-d represents the HX^-/X2^- buffer region?

CaF₂ has K_sp = 3.5 × 10^-11.If 25 mL of 8.0 × 10^-4 M Ca(NO₃)₂ is mixed with 75 mL of 4.0 × 10^-4 M KF,a precipitate of CaF₂ ________ (will,will not)form.

When 70 mL of 0.18 M NH₄Cl is added to 70 mL of 0.18 M NH₃,relative to the pH of the 0.10 M NH₃solution the pH of the resulting solution will

What is the most soluble salt of the following set?

The following pictures represent solutions that contain a weak acid HA (pK_a = 5.0)and its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent A^- ions.(K⁺,H₃O⁺,OH^-,and solvent H₂O molecules have been omitted for clarity. ) -Which solution has the lowest pH?

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M methylamine,CH₃NH₂,with 15.00 mL of 0.10 M methylammonium chloride,CH₃NH₃Cl? Assume that the volume of the solutions are additive and that K_b = 3.70 × 10^-4 for methylamine.

Which statement about buffers is true?

Which set of ions precipitate as sulfides?

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Exam 16: Applications of Aqueous Equilibria

Selenous acid,H2SeO3 has acid dissociation constants Ka1 = 3.5 × 10-2 and Ka2 = 5 × 10-8.When 25.00 mL of 0.100 M selenous acid is titrated with 0.200 M NaOH the first equivalence point occurs at pH = ________.

What is the pH of the resulting solution if 40.00 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.

Potassium chromate is slowly added to a solution containing 0.20 M AgNO3 and 0.20 M Ba(NO3)2.Describe what happens if the Ksp for Ag2CrO4 is 1.1 × 10-12 and the Ksp of BaCrO4 is 1.2 × 10-10.

What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 40.00 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 equilibrium constant expression for the Ksp of Sr3(PO4)2?

Use the graphs below to answer the following questions. -What is the characteristic pH-titrant curve for the titration of a strong base by a strong acid?

Consider a buffered solution consisting of H2CO3 and HCO3- where the pKa = 6.4.At pH = 6.4,which of the following is true?

What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.00? Ksp for Mg(OH)2 is

Oxalic acid,H2C2O4 has acid dissociation constants Ka1 = 5.9 × 10-2 and Ka2 = 6.4 × 10-5.What is the pH after 20.00 mL of 0.0500 M NaOH is added to 5.00 mL of 0.2000 M H2C2O4?

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H2A with NaOH. -Which point a-d represents the HX-/X2- buffer region?

CaF2 has Ksp = 3.5 × 10-11.If 25 mL of 8.0 × 10-4 M Ca(NO3)2 is mixed with 75 mL of 4.0 × 10-4 M KF,a precipitate of CaF2 ________ (will,will not)form.

When 70 mL of 0.18 M NH4Cl is added to 70 mL of 0.18 M NH3,relative to the pH of the 0.10 M NH3 solution the pH of the resulting solution will

What is the most soluble salt of the following set?

The following pictures represent solutions that contain a weak acid HA (pKa = 5.0)and its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent A- ions.(K+,H3O+,OH-,and solvent H2O molecules have been omitted for clarity. ) -Which of these solutions are buffers?

The following pictures represent solutions that contain a weak acid HA (pKa = 5.0)and its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent A- ions.(K+,H3O+,OH-,and solvent H2O molecules have been omitted for clarity. ) -Which solution has the lowest pH?

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M methylamine,CH3NH2,with 15.00 mL of 0.10 M methylammonium chloride,CH3NH3Cl? Assume that the volume of the solutions are additive and that Kb = 3.70 × 10-4 for methylamine.

Which statement about buffers is true?

Which set of ions precipitate as sulfides?

Chemical Tools: Experimentation and Measurement

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Selenous acid,H₂SeO₃ has acid dissociation constants K_a1 = 3.5 × 10^-2 and K_a2 = 5 × 10^-8.When 25.00 mL of 0.100 M selenous acid is titrated with 0.200 M NaOH the first equivalence point occurs at pH = ________.

What is the pH of the resulting solution if 40.00 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.

Potassium chromate is slowly added to a solution containing 0.20 M AgNO₃ and 0.20 M Ba(NO₃)₂.Describe what happens if the K_sp for Ag₂CrO₄ is 1.1 × 10^-12 and the K_sp of BaCrO₄ is 1.2 × 10^-10.

What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 40.00 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 equilibrium constant expression for the K_sp of Sr₃(PO₄)₂?

Consider a buffered solution consisting of H₂CO₃ and HCO₃^- where the pKa = 6.4.At pH = 6.4,which of the following is true?

What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.00? K_sp for Mg(OH)₂ is

Oxalic acid,H₂C₂O₄ has acid dissociation constants K_a1 = 5.9 × 10^-2 and K_a2 = 6.4 × 10^-5.What is the pH after 20.00 mL of 0.0500 M NaOH is added to 5.00 mL of 0.2000 M H₂C₂O₄?

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H₂A with NaOH. -Which point a-d represents the HX^-/X2^- buffer region?

CaF₂ has K_sp = 3.5 × 10^-11.If 25 mL of 8.0 × 10^-4 M Ca(NO₃)₂ is mixed with 75 mL of 4.0 × 10^-4 M KF,a precipitate of CaF₂ ________ (will,will not)form.

When 70 mL of 0.18 M NH₄Cl is added to 70 mL of 0.18 M NH₃,relative to the pH of the 0.10 M NH₃solution the pH of the resulting solution will

The following pictures represent solutions that contain a weak acid HA (pK_a = 5.0)and its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent A^- ions.(K⁺,H₃O⁺,OH^-,and solvent H₂O molecules have been omitted for clarity. ) -Which solution has the lowest pH?

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M methylamine,CH₃NH₂,with 15.00 mL of 0.10 M methylammonium chloride,CH₃NH₃Cl? Assume that the volume of the solutions are additive and that K_b = 3.70 × 10^-4 for methylamine.