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 25.00 mL of 0.10 M methylamine,CH3NH2,with 25.00 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) 10.27 B) 10.57 C) 10.87 D) 11.78 A) 10.27 B) 10.57 C) 10.87 D) 11.78

The balanced equation for the solubility equilibrium of Fe(OH)2 is shown below.What is the equilibrium constant expression for the Ksp of Fe(OH)2? Fe(OH)2(s)⇌ Fe2+(aq)+ 2 OH-(aq)

A) Ksp = {[Fe2+][OH-]2}/{[Fe(OH)2][H2O]} B) Ksp = {[Fe2+][OH-]2}/[Fe(OH)2] C) Ksp = [Fe2+][OH-]2 D) Ksp = 1/{[Fe2+][OH-]2} A) Ksp = {[Fe2+][OH-]2}/{[Fe(OH)2][H2O]} B) Ksp = {[Fe2+][OH-]2}/[Fe(OH)2] C) Ksp = [Fe2+][OH-]2 D) Ksp = 1/{[Fe2+][OH-]2}

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. ) -For which solution(s)is pH = pKa?

A) only solution (1) B) only solution (2) C) only solution (3) D) solutions (1)and (3) A) only solution (1) B) only solution (2) C) only solution (3) D) solutions (1)and (3)

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 highest pH?

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

In which of the following solutions would solid PbBr2 be expected to be the least soluble at 25°C?

A) 0)1 M H Br B) 0)1 M NaBr C) 0)1 M CaBr2 D) 0)1 M K NO3 A) 0)1 M H Br B) 0)1 M NaBr C) 0)1 M CaBr2 D) 0)1 M K NO3

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 beyond the second equivalence point?

A) (1) B) (2) C) (3) D) (4) A) (1) B) (2) C) (3) D) (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 AgNO3 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 sulfate if the solubility of Ag2SO4 in pure water is 4.5 g/L.

A) 3)0 × 10-6 B) 1)2 × 10-5 C) 2)1 × 10-4 D) 4)2 × 10-4 A) 3)0 × 10-6 B) 1)2 × 10-5 C) 2)1 × 10-4 D) 4)2 × 10-4

Exam 15: Applications of Aqueous Equilibria

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 21

What is not a correct expression for the weak acid HA?

(Multiple Choice)

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Question 22

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine,CH₃NH₂,with 25.00 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 23

The balanced equation for the solubility equilibrium of Fe(OH)₂ is shown below.What is the equilibrium constant expression for the K_sp of Fe(OH)₂? Fe(OH)₂(s)⇌ Fe²⁺(aq)+ 2 OH^-(aq)

(Multiple Choice)

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Question 24

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. ) -For which solution(s)is pH = pK_a?

(Multiple Choice)

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Question 25

The half equivalence point in the titration of 0.100 M HCO₂H (K_a = 1.8 × 10^-4)with 0.250 M NaOH occurs at pH = ________.

(Short Answer)

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Question 26

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 27

The addition of mL of 0.1500 M NaOH is required to titrate 25.00 mL of 0.2250 M HCl to the equivalence point,which occurs at a pH of .

(Short Answer)

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Question 28

Calculate the solubility (in g/L)of silver carbonate in water at 25°C if the K_sp for Ag₂CO₃ is 8)4 × 10^-12.

(Multiple Choice)

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Question 29

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 highest pH?

(Multiple Choice)

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Question 30

In which of the following solutions would solid PbBr₂ be expected to be the least soluble at 25°C?

(Multiple Choice)

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Question 31

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 32

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 beyond the second equivalence point?

(Multiple Choice)

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Question 33

The solution formed upon adding 50.00 mL of 0.10 M NH₄Cl to 50.00 mL of 0.10 M NH₃ will have a pH that is ________ the pH of the original NH₃ solution.

(Short Answer)

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Question 34

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 AgNO₃ is added and equilibrium is restored?

(Multiple Choice)

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Question 35

What is the percent dissociation of ascorbic acid if the solution has a pH = 5.50 and a pK_a = 4.10?

(Multiple Choice)

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Question 36

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 37

The balanced net ionic equation for the neutralization reaction involving equal molar amounts of HCl and CH₃CH₂NH₂ is ________.

(Short Answer)

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Question 38

Calculate the K_sp for silver sulfate if the solubility of Ag₂SO₄ in pure water is 4.5 g/L.

(Multiple Choice)

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Question 39

Sodium hypochlorite,NaOCl,is the active ingredient in household bleach.What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 32.00 mL of 0.500 M HCl to reach the equivalence point?

(Multiple Choice)

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Question 40

Showing 21 - 40 of 190

Exam 15: Applications of Aqueous Equilibria

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 not a correct expression for the weak acid HA?

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine,CH3NH2,with 25.00 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.

The balanced equation for the solubility equilibrium of Fe(OH)2 is shown below.What is the equilibrium constant expression for the Ksp of Fe(OH)2? Fe(OH)2(s)⇌ Fe2+(aq)+ 2 OH-(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. ) -For which solution(s)is pH = pKa?

The half equivalence point in the titration of 0.100 M HCO2H (Ka = 1.8 × 10-4)with 0.250 M NaOH occurs at pH = ________.

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.

The addition of ________ mL of 0.1500 M NaOH is required to titrate 25.00 mL of 0.2250 M HCl to the equivalence point,which occurs at a pH of ________.

Calculate the solubility (in g/L)of silver carbonate in water at 25°C if the Ksp for Ag2CO3 is 8)4 × 10-12.

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 highest pH?

In which of the following solutions would solid PbBr2 be expected to be the least soluble at 25°C?

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.

The solution formed upon adding 50.00 mL of 0.10 M NH4Cl to 50.00 mL of 0.10 M NH3 will have a pH that is ________ the pH of the original NH3 solution.

What is the percent dissociation of ascorbic acid if the solution has a pH = 5.50 and a pKa = 4.10?

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.

The balanced net ionic equation for the neutralization reaction involving equal molar amounts of HCl and CH3CH2NH2 is ________.

Calculate the Ksp for silver sulfate if the solubility of Ag2SO4 in pure water is 4.5 g/L.

Sodium hypochlorite,NaOCl,is the active ingredient in household bleach.What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 32.00 mL of 0.500 M HCl to reach the equivalence point?

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Gases: Their Properties and Behavior

Liquids,solids,and Phase Changes

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Chemical Kinetics

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Aqueous Equilibria: Acids and Bases

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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 25.00 mL of 0.10 M methylamine,CH₃NH₂,with 25.00 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.

The balanced equation for the solubility equilibrium of Fe(OH)₂ is shown below.What is the equilibrium constant expression for the K_sp of Fe(OH)₂? Fe(OH)₂(s)⇌ Fe²⁺(aq)+ 2 OH^-(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. ) -For which solution(s)is pH = pK_a?

The half equivalence point in the titration of 0.100 M HCO₂H (K_a = 1.8 × 10^-4)with 0.250 M NaOH occurs at pH = ________.

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.

The addition of mL of 0.1500 M NaOH is required to titrate 25.00 mL of 0.2250 M HCl to the equivalence point,which occurs at a pH of .

Calculate the solubility (in g/L)of silver carbonate in water at 25°C if the K_sp for Ag₂CO₃ is 8)4 × 10^-12.

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 highest pH?

In which of the following solutions would solid PbBr₂ be expected to be the least soluble at 25°C?

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.

The solution formed upon adding 50.00 mL of 0.10 M NH₄Cl to 50.00 mL of 0.10 M NH₃ will have a pH that is ________ the pH of the original NH₃ solution.

What is the percent dissociation of ascorbic acid if the solution has a pH = 5.50 and a pK_a = 4.10?

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.

The balanced net ionic equation for the neutralization reaction involving equal molar amounts of HCl and CH₃CH₂NH₂ is ________.

Calculate the K_sp for silver sulfate if the solubility of Ag₂SO₄ in pure water is 4.5 g/L.