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 of the solutions are buffer solutions?

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

The following pictures represent solutions of AgCl,which may also contain ions other than AgS1U1P1+S1S1P0 and ClS1U1P1-S1S1P0 which are not shown.Gray spheres represent AgS1U1P1+S1S1P0 ions and dotted spheres represent ClS1U1P1-S1S1P0 ions. -If solution (1)is a saturated solution of AgCl,which of solutions (1)-(4)represents the solution after a small amount of NH3 is added and equilibrium is restored?

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

Calculate the Ksp for silver sulfite if the solubility of Ag2SO3 in pure water is 4.6 × 10-3 g/L.

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

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 greatest buffer capacity?

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

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 halfway between the first and second equivalence points?

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

A solution may contain the following ions Ag+,Cu2+,Cd2+,Mn2+,Ni2+ and Na+.A white precipitate formed when 0.10 M NaCl was added and after this was removed the solution was treated with H2S gas under acidic conditions and no precipitate formed.When the solution was made basic and again treated with H2S gas a dark colored precipitate formed.If no further tests were made then what conclusions can you draw?

A) possible ions present Ag+,Mn2+,Ni2+ B) possible ions present Ag+,Mn2+,Ni2+,Na+ C) possible ions present Ag+,Cu2+,Cd2+ D) possible ions present Ag+,Cu2+,Cd2+,Na+ A) possible ions present Ag+,Mn2+,Ni2+ B) possible ions present Ag+,Mn2+,Ni2+,Na+ C) possible ions present Ag+,Cu2+,Cd2+ D) possible ions present Ag+,Cu2+,Cd2+,Na+

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 highest pH?

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

Exam 15: Applications of Aqueous Equilibria

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 of the solutions are buffer solutions?

(Multiple Choice)

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Question 81

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

(Multiple Choice)

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Question 82

What is the pH of the solution formed when 50 mL of 0.250 M NaOH is added to 50 mL of 0.120 M HCl?

(Short Answer)

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Question 83

The following pictures represent solutions of AgCl,which may also contain ions other than Ag⁺ and Cl^- which are not shown.Gray spheres represent Ag⁺ ions and dotted spheres represent Cl^- ions. -If solution (1)is a saturated solution of AgCl,which of solutions (1)-(4)represents the solution after a small amount of NH₃ is added and equilibrium is restored?

(Multiple Choice)

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Question 84

TRIS {(HOCH₂)₃CNH₂} is one of the most common buffers used in biochemistry.A solution is prepared by adding enough TRIS and 12 M HCl(aq)to give 1.00 L of solution with [TRIS] = 0.30 M and [TRISH⁺] = 0.60 M.What is the pH of this buffered system if the pK_b is 5.92?

(Multiple Choice)

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Question 85

What is the K_a of the amino acid glycine if it is 75.0% dissociated at pH = 10.08?

(Short Answer)

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Question 86

What is the [CH₃CO₂^-]/[CH₃CO₂H] ratio necessary to make a buffer solution with a pH of 4.44? K_a = 1.8 × 10^-5 for CH₃CO₂H.

(Multiple Choice)

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Question 87

When 50 mL of 0.10 M NaF is added to 50 mL of 0.10 M HF,relative to the pH of the 0.10 M HF solution the pH of the resulting solution will

(Multiple Choice)

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Question 88

Calculate the K_sp for silver sulfite if the solubility of Ag₂SO₃ in pure water is 4.6 × 10^-3g/L.

(Multiple Choice)

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Question 89

Calculate the molar solubility of thallium(I)chloride in 0.40 M NaCl at 25°C.K_sp for TlCl is 1)7 × 10^-4.

(Multiple Choice)

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Question 90

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 greatest buffer capacity?

(Multiple Choice)

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Question 91

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 halfway between the first and second equivalence points?

(Multiple Choice)

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Question 92

Which is a net ionic equation for the neutralization reaction of a weak acid with a weak base?

(Multiple Choice)

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Question 93

Which of these neutralization reactions has a pH < 7 when equal molar amounts of acid and base are mixed?

(Multiple Choice)

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Question 94

A solution may contain the following ions Ag⁺,Cu²⁺,Cd²⁺,Mn²⁺,Ni²⁺ and Na⁺.A white precipitate formed when 0.10 M NaCl was added and after this was removed the solution was treated with H₂S gas under acidic conditions and no precipitate formed.When the solution was made basic and again treated with H₂S gas a dark colored precipitate formed.If no further tests were made then what conclusions can you draw?

(Multiple Choice)

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Question 95

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 M HCl? K_a = 3.0 × 10^-8 for HOCl.

(Multiple Choice)

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Question 96

What is the pH of a buffer solution made by mixing 50.0 mL of 0.100 M potassium hydrogen phthalate with 13.6 mL of 0.100 M NaOH and diluting the mixture to 100.0 mL with water? The K_a2 for hydrogen phthalate is 3.1 × 10^-6.

(Multiple Choice)

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Question 97

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^-5 for CH₃CO₂H.

(Multiple Choice)

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Question 98

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 highest pH?

(Multiple Choice)

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Question 99

The following plot shows two titration curves,each representing the titration of 50.00 mL of 0.100 M acid with 0.100 M NaOH. -Which points a-d represent the half-equivalence point and the equivalence point,respectively,for the titration of a weak acid?

(Multiple Choice)

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Question 100

Showing 81 - 100 of 190

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 of the solutions are buffer solutions?

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

What is the pH of the solution formed when 50 mL of 0.250 M NaOH is added to 50 mL of 0.120 M HCl?

TRIS {(HOCH₂)₃CNH₂} is one of the most common buffers used in biochemistry.A solution is prepared by adding enough TRIS and 12 M HCl(aq)to give 1.00 L of solution with [TRIS] = 0.30 M and [TRISH⁺] = 0.60 M.What is the pH of this buffered system if the pK_b is 5.92?

What is the K_a of the amino acid glycine if it is 75.0% dissociated at pH = 10.08?

What is the [CH₃CO₂^-]/[CH₃CO₂H] ratio necessary to make a buffer solution with a pH of 4.44? K_a = 1.8 × 10^-5 for CH₃CO₂H.

When 50 mL of 0.10 M NaF is added to 50 mL of 0.10 M HF,relative to the pH of the 0.10 M HF solution the pH of the resulting solution will

Calculate the K_sp for silver sulfite if the solubility of Ag₂SO₃ in pure water is 4.6 × 10^-3g/L.

Calculate the molar solubility of thallium(I)chloride in 0.40 M NaCl at 25°C.K_sp for TlCl is 1)7 × 10^-4.

Which is a net ionic equation for the neutralization reaction of a weak acid with a weak base?

Which of these neutralization reactions has a pH < 7 when equal molar amounts of acid and base are mixed?

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 M HCl? K_a = 3.0 × 10^-8 for HOCl.

What is the pH of a buffer solution made by mixing 50.0 mL of 0.100 M potassium hydrogen phthalate with 13.6 mL of 0.100 M NaOH and diluting the mixture to 100.0 mL with water? The K_a2 for hydrogen phthalate is 3.1 × 10^-6.

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^-5 for CH₃CO₂H.

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 highest pH?

The following plot shows two titration curves,each representing the titration of 50.00 mL of 0.100 M acid with 0.100 M NaOH. -Which points a-d represent the half-equivalence point and the equivalence point,respectively,for the titration of a weak acid?

Chemistry: Matter and Measurement

Atoms, molecules, and Ions

Formulas, equations, and Moles

Reactions in Aqueous Solutions

Periodicity and the Atomic Structure of Atoms

Ionic Bonds and Some Main-Group Chemistry

Covalent Bonds and Molecular Structure

Thermochemistry: Chemical Energy

Gases: Their Properties and Behavior

Liquids,solids,and Phase Changes

Solutions and Their Properties

Chemical Kinetics

Chemical Equilibrium

Aqueous Equilibria: Acids and Bases

Thermodynamics: Entropy, free Energy, and Equilibrium

Electrochemistry

Hydrogen, oxygen, and Water

The Main-Group Elements

Transition Elements and Coordination Chemistry

Metals and Solid-State Materials

Nuclear Chemistry

Organic and Biological Chemistry

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Exam 15: Applications of Aqueous Equilibria

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 of the solutions are buffer solutions?

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

What is the pH of the solution formed when 50 mL of 0.250 M NaOH is added to 50 mL of 0.120 M HCl?

TRIS {(HOCH2)3CNH2} is one of the most common buffers used in biochemistry.A solution is prepared by adding enough TRIS and 12 M HCl(aq)to give 1.00 L of solution with [TRIS] = 0.30 M and [TRISH+] = 0.60 M.What is the pH of this buffered system if the pKb is 5.92?

What is the Ka of the amino acid glycine if it is 75.0% dissociated at pH = 10.08?

What is the [CH3CO2-]/[CH3CO2H] ratio necessary to make a buffer solution with a pH of 4.44? Ka = 1.8 × 10-5 for CH3CO2H.

When 50 mL of 0.10 M NaF is added to 50 mL of 0.10 M HF,relative to the pH of the 0.10 M HF solution the pH of the resulting solution will

Calculate the Ksp for silver sulfite if the solubility of Ag2SO3 in pure water is 4.6 × 10-3 g/L.

Calculate the molar solubility of thallium(I)chloride in 0.40 M NaCl at 25°C.Ksp for TlCl is 1)7 × 10-4.

Which is a net ionic equation for the neutralization reaction of a weak acid with a weak base?

Which of these neutralization reactions has a pH < 7 when equal molar amounts of acid and base are mixed?

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 M HCl? Ka = 3.0 × 10-8 for HOCl.

What is the pH of a buffer solution made by mixing 50.0 mL of 0.100 M potassium hydrogen phthalate with 13.6 mL of 0.100 M NaOH and diluting the mixture to 100.0 mL with water? The Ka2 for hydrogen phthalate is 3.1 × 10-6.

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.

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 highest pH?

The following plot shows two titration curves,each representing the titration of 50.00 mL of 0.100 M acid with 0.100 M NaOH. -Which points a-d represent the half-equivalence point and the equivalence point,respectively,for the titration of a weak acid?

Chemistry: Matter and Measurement

Atoms, molecules, and Ions

Formulas, equations, and Moles

Reactions in Aqueous Solutions

Periodicity and the Atomic Structure of Atoms

Ionic Bonds and Some Main-Group Chemistry

Covalent Bonds and Molecular Structure

Thermochemistry: Chemical Energy

Gases: Their Properties and Behavior

Liquids,solids,and Phase Changes

Solutions and Their Properties

Chemical Kinetics

Chemical Equilibrium

Aqueous Equilibria: Acids and Bases

Thermodynamics: Entropy, free Energy, and Equilibrium

Electrochemistry

Hydrogen, oxygen, and Water

The Main-Group Elements

Transition Elements and Coordination Chemistry

Metals and Solid-State Materials

Nuclear Chemistry

Organic and Biological Chemistry

Filters

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 of the solutions are buffer solutions?

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

TRIS {(HOCH₂)₃CNH₂} is one of the most common buffers used in biochemistry.A solution is prepared by adding enough TRIS and 12 M HCl(aq)to give 1.00 L of solution with [TRIS] = 0.30 M and [TRISH⁺] = 0.60 M.What is the pH of this buffered system if the pK_b is 5.92?

What is the K_a of the amino acid glycine if it is 75.0% dissociated at pH = 10.08?

What is the [CH₃CO₂^-]/[CH₃CO₂H] ratio necessary to make a buffer solution with a pH of 4.44? K_a = 1.8 × 10^-5 for CH₃CO₂H.

Calculate the K_sp for silver sulfite if the solubility of Ag₂SO₃ in pure water is 4.6 × 10^-3g/L.

Calculate the molar solubility of thallium(I)chloride in 0.40 M NaCl at 25°C.K_sp for TlCl is 1)7 × 10^-4.

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 M HCl? K_a = 3.0 × 10^-8 for HOCl.

What is the pH of a buffer solution made by mixing 50.0 mL of 0.100 M potassium hydrogen phthalate with 13.6 mL of 0.100 M NaOH and diluting the mixture to 100.0 mL with water? The K_a2 for hydrogen phthalate is 3.1 × 10^-6.

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^-5 for CH₃CO₂H.

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 highest pH?