0.10 M potassium chromate is slowly added to a solution containing 0.10 M AgNO3 and 0.10 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.

A) 6.5 × 10-5 M B) 1.3 × 10-4 M C) 3.2 × 10-4 M D) 3.0 × 10-2 M A) 6.5 × 10-5 M B) 1.3 × 10-4 M C) 3.2 × 10-4 M D) 3.0 × 10-2 M

The following pictures represent solutions that contain a weak acid HA and/or 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 greatest buffer capacity?

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

What is the molar solubility of lead(II)chromate in 0.10 M HNO3 if the Ksp for PbCrO4 is 2.8 × 10-13 and the Ka2 for H2CrO4 is 3.0 × 10-7? Note that H2CrO4 is considered to be a strong acid.

A) 9.2 × 10-11 M B) 2.9 × 10-10 M C) 9.3 × 10-7 M D) 3.1 × 10-4 M A) 9.2 × 10-11 M B) 2.9 × 10-10 M C) 9.3 × 10-7 M D) 3.1 × 10-4 M

Which metal sulfides can be precipitated from a solution that is 0.01 M in Mn2+,Zn2+,Pb2+ and Cu2+ and 0.10 M in H2S at a pH of 1.0?

A) MnS B) CuS C) PbS,CuS D) ZnS,PbS,CuS A) MnS B) CuS C) PbS,CuS D) ZnS,PbS,CuS

What is the pH of the resulting solution if 40.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+.

A) 2.84 B) 4.02 C) 9.97 D) 11.16 A) 2.84 B) 4.02 C) 9.97 D) 11.16

The neutralization constant Kn for the neutralization of acetylsalicylic acid (C9H8O4)and codeine (C18H21NO3)is 4.8 × 104.The acid dissociation constant Ka for acetylsalicylic acid is 3.0 × 10-4.What is the base dissociation constant Kb for codeine?

A) 4.8 × 10-24 B) 6.3 × 10-23 C) 1.6 × 10-6 D) 1.4 × 1015 A) 4.8 × 10-24 B) 6.3 × 10-23 C) 1.6 × 10-6 D) 1.4 × 1015

The dissociation equilibrium constants for the protonated form of alanine (a diprotic amino acid,H2X+)are Ka1 = 4.6 × 10-3 and Ka2 = 2.0 × 10-10.What is the pH of 50.00 mL of a 0.050 M solution of alanine after 37.50 mL of 0.100 M NaOH has been added?

A) 4.85 B) 6.02 C) 7.39 D) 9.70 A) 4.85 B) 6.02 C) 7.39 D) 9.70

Exam 16: Applications of Aqueous Equilibria

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0.100 M NaOH? K_a = 6.76 × 10^-4 for HF.

(Multiple Choice)

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Question 81

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0.400 M NaOH? K_a = 6.76 × 10^-4 for HF.

(Multiple Choice)

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Question 82

Calculate the solubility (in g/L)of calcium fluoride in water at 25°C if the K_sp for CaF₂ is 3.5 × .

(Multiple Choice)

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Question 83

0.10 M potassium chromate is slowly added to a solution containing 0.10 M AgNO₃ and 0.10 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.

(Multiple Choice)

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Question 84

What is the pH of a buffered system made by dissolving 17.42 g of KH₂PO₄ and 20.41 g of K₂HPO₄ in water to give a volume of 200.0 mL? The K_a2 for dihydrogen phosphate is 6.2 × 10^-8 and the equilibrium reaction of interest is H₂PO₄^-(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ HPO₄^-(aq).

(Multiple Choice)

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Question 85

The following pictures represent solutions that contain a weak acid HA and/or 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 greatest buffer capacity?

(Multiple Choice)

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Question 86

What is the least soluble salt of the following set?

(Multiple Choice)

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Question 87

What is the molar solubility of lead(II)chromate in 0.10 M HNO₃ if the K_sp for PbCrO₄ is 2.8 × 10^-13 and the K_a2 for H₂CrO₄ is 3.0 × 10^-7? Note that H₂CrO₄ is considered to be a strong acid.

(Multiple Choice)

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Question 88

The solution formed upon adding 80.00 mL of 0.50 M NH₄Cl to 80.00 mL of 0.50 M NH₃ will have a pH that is ________ the pH of the original NH₃ solution.

(Short Answer)

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Question 89

What is the pH of the resulting solution if 30.00 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 90

What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 45.00 mL of 0.100 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 91

Which metal sulfides can be precipitated from a solution that is 0.01 M in Mn²⁺,Zn²⁺,Pb²⁺ and Cu²⁺ and 0.10 M in H₂S at a pH of 1.0?

(Multiple Choice)

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Question 92

What volume of 0.100 M NaOH is needed to make 100.0 mL of a buffer solution with a pH of 6.00 if one starts with 50.0 mL of 0.100 M potassium hydrogen phthalate? The K_a2 for potassium hydrogen phthalate is 3.1 × 10^-6.

(Multiple Choice)

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Question 93

What is the pH of the resulting solution if 40.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⁺.

(Multiple Choice)

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Question 94

What is the Henderson-Hasselbalch equation for the acidic buffer HA/A^-?

(Multiple Choice)

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Question 95

The neutralization constant K_n for the neutralization of acetylsalicylic acid (C₉H₈O₄)and codeine (C₁₈H₂₁NO₃)is 4.8 × 10⁴.The acid dissociation constant K_a for acetylsalicylic acid is 3.0 × 10^-4.What is the base dissociation constant K_b for codeine?

(Multiple Choice)

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Question 96

The dissociation equilibrium constants for the protonated form of alanine (a diprotic amino acid,H₂X⁺)are K_a1 = 4.6 × 10^-3 and K_a2 = 2.0 × 10^-10.What is the pH of 50.00 mL of a 0.050 M solution of alanine after 37.50 mL of 0.100 M NaOH has been added?

(Multiple Choice)

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Question 97

Addition of 0.0125 mol KOH to 150 mL of a 0.150 M formic acid/0.100 M sodium formate buffer results in a pH = ________.The K_a of formic acid is 1.8 × 10^-4.

(Short Answer)

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Question 98

The equivalence point pH of the titration of four weak acids is given.Which is the strongest acid?

(Multiple Choice)

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Question 99

Which is the best acid to use in the preparation of a buffer with pH = 9.3?

(Multiple Choice)

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Question 100

Showing 81 - 100 of 201

Exam 16: Applications of Aqueous Equilibria

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0.100 M NaOH? Ka = 6.76 × 10-4 for HF.

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0.400 M NaOH? Ka = 6.76 × 10-4 for HF.

Calculate the solubility (in g/L)of calcium fluoride in water at 25°C if the Ksp for Ca F2 is 3.5 × .

0.10 M potassium chromate is slowly added to a solution containing 0.10 M AgNO3 and 0.10 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.

What is the pH of a buffered system made by dissolving 17.42 g of KH2PO4 and 20.41 g of K2HPO4 in water to give a volume of 200.0 mL? The Ka2 for dihydrogen phosphate is 6.2 × 10-8 and the equilibrium reaction of interest is H2PO4-(aq)+ H2O(l)⇌ H3O+(aq)+ HPO4-(aq).

The following pictures represent solutions that contain a weak acid HA and/or 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 greatest buffer capacity?

What is the least soluble salt of the following set?

What is the molar solubility of lead(II)chromate in 0.10 M HNO3 if the Ksp for PbCrO4 is 2.8 × 10-13 and the Ka2 for H2CrO4 is 3.0 × 10-7? Note that H2CrO4 is considered to be a strong acid.

The solution formed upon adding 80.00 mL of 0.50 M NH4Cl to 80.00 mL of 0.50 M NH3 will have a pH that is ________ the pH of the original NH3 solution.

What is the pH of the resulting solution if 30.00 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.

What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 45.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.Ka = 1.8 × 10-5 for CH3CO2H.

Which metal sulfides can be precipitated from a solution that is 0.01 M in Mn2+,Zn2+,Pb2+ and Cu2+ and 0.10 M in H2S at a pH of 1.0?

What volume of 0.100 M NaOH is needed to make 100.0 mL of a buffer solution with a pH of 6.00 if one starts with 50.0 mL of 0.100 M potassium hydrogen phthalate? The Ka2 for potassium hydrogen phthalate is 3.1 × 10-6.

What is the pH of the resulting solution if 40.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+.

What is the Henderson-Hasselbalch equation for the acidic buffer HA/A-?

The neutralization constant Kn for the neutralization of acetylsalicylic acid (C9H8O4)and codeine (C18H21NO3)is 4.8 × 104.The acid dissociation constant Ka for acetylsalicylic acid is 3.0 × 10-4.What is the base dissociation constant Kb for codeine?

The dissociation equilibrium constants for the protonated form of alanine (a diprotic amino acid,H2X+)are Ka1 = 4.6 × 10-3 and Ka2 = 2.0 × 10-10.What is the pH of 50.00 mL of a 0.050 M solution of alanine after 37.50 mL of 0.100 M NaOH has been added?

Addition of 0.0125 mol KOH to 150 mL of a 0.150 M formic acid/0.100 M sodium formate buffer results in a pH = ________.The Ka of formic acid is 1.8 × 10-4.

The equivalence point pH of the titration of four weak acids is given.Which is the strongest acid?

Which is the best acid to use in the preparation of a buffer with pH = 9.3?

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What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0.100 M NaOH? K_a = 6.76 × 10^-4 for HF.

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0.400 M NaOH? K_a = 6.76 × 10^-4 for HF.

Calculate the solubility (in g/L)of calcium fluoride in water at 25°C if the K_sp for CaF₂ is 3.5 × .

0.10 M potassium chromate is slowly added to a solution containing 0.10 M AgNO₃ and 0.10 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.

What is the pH of a buffered system made by dissolving 17.42 g of KH₂PO₄ and 20.41 g of K₂HPO₄ in water to give a volume of 200.0 mL? The K_a2 for dihydrogen phosphate is 6.2 × 10^-8 and the equilibrium reaction of interest is H₂PO₄^-(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ HPO₄^-(aq).

What is the molar solubility of lead(II)chromate in 0.10 M HNO₃ if the K_sp for PbCrO₄ is 2.8 × 10^-13 and the K_a2 for H₂CrO₄ is 3.0 × 10^-7? Note that H₂CrO₄ is considered to be a strong acid.

The solution formed upon adding 80.00 mL of 0.50 M NH₄Cl to 80.00 mL of 0.50 M NH₃ will have a pH that is ________ the pH of the original NH₃ solution.

What is the pH of the resulting solution if 30.00 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.

What is the pH of a solution made by mixing 30.00 mL of 0.10 M acetic acid with 45.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.K_a = 1.8 × 10^-5for CH₃CO₂H.

Which metal sulfides can be precipitated from a solution that is 0.01 M in Mn²⁺,Zn²⁺,Pb²⁺ and Cu²⁺ and 0.10 M in H₂S at a pH of 1.0?

What volume of 0.100 M NaOH is needed to make 100.0 mL of a buffer solution with a pH of 6.00 if one starts with 50.0 mL of 0.100 M potassium hydrogen phthalate? The K_a2 for potassium hydrogen phthalate is 3.1 × 10^-6.

What is the pH of the resulting solution if 40.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⁺.

What is the Henderson-Hasselbalch equation for the acidic buffer HA/A^-?

The neutralization constant K_n for the neutralization of acetylsalicylic acid (C₉H₈O₄)and codeine (C₁₈H₂₁NO₃)is 4.8 × 10⁴.The acid dissociation constant K_a for acetylsalicylic acid is 3.0 × 10^-4.What is the base dissociation constant K_b for codeine?

The dissociation equilibrium constants for the protonated form of alanine (a diprotic amino acid,H₂X⁺)are K_a1 = 4.6 × 10^-3 and K_a2 = 2.0 × 10^-10.What is the pH of 50.00 mL of a 0.050 M solution of alanine after 37.50 mL of 0.100 M NaOH has been added?

Addition of 0.0125 mol KOH to 150 mL of a 0.150 M formic acid/0.100 M sodium formate buffer results in a pH = ________.The K_a of formic acid is 1.8 × 10^-4.