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 0.100 M solution of alanine after 100.00 mL of 0.100 M NaOH has been added?

A) 9.70 B) 10.69 C) 11.11 D) 12.70 A) 9.70 B) 10.69 C) 11.11 D) 12.70

The following pictures represent solutions of CaCOS1U1B13S1U1B0,which may also contain ions other than CaS1U1P12+S1S1P0 and COS1U1B13S1U1B0S1U1P12-S1S1P0 which are not shown.Gray spheres represent CaS1U1P12+S1S1P0 ions and unshaded spheres represent COS1U1B13S1U1B0S1U1P12-S1S1P0 ions. -If solution (1)is a saturated solution of CaCO3,which of solutions (1)-(4)represents the solution after a small amount of Ca(NO3)2 is added and equilibrium is restored?

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 NH3 with 25.00 mL of 0.10 M NH4Cl? Assume that the volume of the solutions are additive and that Kb = 1.8 × 10-5 for NH3.

A) 8.95 B) 9.26 C) 9.56 D) 11.13 A) 8.95 B) 9.26 C) 9.56 D) 11.13

The following pictures represent solutions at various points in the titration of a weak acid HA with aqueous KOH.Unshaded spheres represent H atoms,black spheres represent oxygen atoms,and shaded spheres represent AS1U1P1-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 solution after the equivalence point?

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

The balanced equation for the solubility equilibrium of Ba(OH)2 is shown below.What is the equilibrium constant expression for the Ksp of Ba(OH)2? Ba(OH)2(s)⇌ Ba2+(aq)+ 2 OH-(aq)

A) Ksp = {[Ba2+][OH-]2}/{[Ba(OH)2][H2O]} B) Ksp = {[Ba2+][OH-]2}/[Ba(OH)2] C) Ksp = [Ba2+][OH-]2 D) Ksp = 1/{[Ba2+][OH-]2} A) Ksp = {[Ba2+][OH-]2}/{[Ba(OH)2][H2O]} B) Ksp = {[Ba2+][OH-]2}/[Ba(OH)2] C) Ksp = [Ba2+][OH-]2 D) Ksp = 1/{[Ba2+][OH-]2}

Exam 16: Applications of Aqueous Equilibria

What is the magnitude of the change in pH when 0.005 moles of HCl is added to 0.100 L of a buffer solution that is 0.100 M in CH₃CO₂H and 0.100 M NaCH₃CO₂? The K_a for acetic acid is 1.8 × 10^-5.

(Multiple Choice)

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Question 21

Which pair of ions can be separated by the addition of chloride ion?

(Multiple Choice)

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Question 22

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. -At which point a-d is the pK_a of the acid equal to the pH?

(Multiple Choice)

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Question 23

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 0.100 M solution of alanine after 100.00 mL of 0.100 M NaOH has been added?

(Multiple Choice)

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Question 24

Which pair of ions can be separated by the addition of sulfide ion?

(Multiple Choice)

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Question 25

At 25°C calcium fluoride has a solubility product constant K_sp = 3.5 × 10^-11.The solubility of CaF₂ at this temperature is ________ mol/L.

(Short Answer)

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Question 26

Which of the following mixtures would result in a buffered solution when 1.0 L of each of the two solutions are mixed.

(Multiple Choice)

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Question 27

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 28

Sodium hypochlorite,NaOCl,is the active ingredient in household bleach.What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 31.00 mL of 0.500 M HCl to reach the equivalence point?

(Multiple Choice)

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Question 29

Which of these neutralization reactions has a pH > 7 when equal moles of acid and base are mixed?

(Multiple Choice)

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Question 30

The following pictures represent solutions of CaCO₃,which may also contain ions other than Ca²⁺ and CO₃^2- which are not shown.Gray spheres represent Ca²⁺ ions and unshaded spheres represent CO₃^2- ions. -If solution (1)is a saturated solution of CaCO₃,which of solutions (1)-(4)represents the solution after a small amount of Ca(NO₃)₂ is added and equilibrium is restored?

(Multiple Choice)

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Question 31

A buffer solution is prepared by dissolving 27.22 g of KH₂PO₄ and 3.37 g of KOH in enough water to make 0.100 L of solution.What is the pH of the H₂PO₄^-/HPO₄^2- buffer if the K_a2 = 6.2 × 10^-8?

(Multiple Choice)

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Question 32

Which metal ions can be precipitated out of solution as chlorides?

(Multiple Choice)

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Question 33

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH₃ with 25.00 mL of 0.10 M NH₄Cl? Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5 for NH₃.

(Multiple Choice)

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Question 34

The following pictures represent solutions at various points in the titration of a weak acid HA with aqueous KOH.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 solution after the equivalence point?

(Multiple Choice)

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Question 35

The balanced equation for the solubility equilibrium of Ba(OH)₂ is shown below.What is the equilibrium constant expression for the K_sp of Ba(OH)₂? Ba(OH)₂(s)⇌ Ba²⁺(aq)+ 2 OH^-(aq)

(Multiple Choice)

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Question 36

What is the percent dissociation of glycine if the solution has a pH = 8.60 and a pK_a = 9.60?

(Multiple Choice)

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Question 37

The pH of a solution of HIO₃ (K_a = 1.7 × 10^-1)and KIO₃ is 1.00.What is the molarity of KIO₃ if the molarity of HIO₃ is 0.025 M?

(Short Answer)

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Question 38

What is the equation relating the equilibrium constant K_n for the neutralization of a weak acid with a weak base to the K_a of the acid,the K_b of the base and K_w?

(Essay)

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Question 39

When 110 mL of 0.12 M NaF is added to 110 mL of 0.12 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 40

Showing 21 - 40 of 201

Exam 16: Applications of Aqueous Equilibria

What is the magnitude of the change in pH when 0.005 moles of HCl is added to 0.100 L of a buffer solution that is 0.100 M in CH3CO2H and 0.100 M NaCH3CO2? The Ka for acetic acid is 1.8 × 10-5.

Which pair of ions can be separated by the addition of chloride ion?

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. -At which point a-d is the pKa of the acid equal to the pH?

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 0.100 M solution of alanine after 100.00 mL of 0.100 M NaOH has been added?

Which pair of ions can be separated by the addition of sulfide ion?

At 25°C calcium fluoride has a solubility product constant Ksp = 3.5 × 10-11.The solubility of CaF2 at this temperature is ________ mol/L.

Which of the following mixtures would result in a buffered solution when 1.0 L of each of the two solutions are mixed.

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

Sodium hypochlorite,NaOCl,is the active ingredient in household bleach.What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 31.00 mL of 0.500 M HCl to reach the equivalence point?

Which of these neutralization reactions has a pH > 7 when equal moles of acid and base are mixed?

A buffer solution is prepared by dissolving 27.22 g of KH2PO4 and 3.37 g of KOH in enough water to make 0.100 L of solution.What is the pH of the H2PO4-/HPO42- buffer if the Ka2 = 6.2 × 10-8?

Which metal ions can be precipitated out of solution as chlorides?

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3 with 25.00 mL of 0.10 M NH4Cl? Assume that the volume of the solutions are additive and that Kb = 1.8 × 10-5 for NH3.

The balanced equation for the solubility equilibrium of Ba(OH)2 is shown below.What is the equilibrium constant expression for the Ksp of Ba(OH)2? Ba(OH)2(s)⇌ Ba2+(aq)+ 2 OH-(aq)

What is the percent dissociation of glycine if the solution has a pH = 8.60 and a pKa = 9.60?

The pH of a solution of HIO3 (Ka = 1.7 × 10-1)and KIO3 is 1.00.What is the molarity of KIO3 if the molarity of HIO3 is 0.025 M?

What is the equation relating the equilibrium constant Kn for the neutralization of a weak acid with a weak base to the Ka of the acid,the Kb of the base and Kw?

When 110 mL of 0.12 M NaF is added to 110 mL of 0.12 M HF,relative to the pH of the 0.10 M HF solution the pH of the resulting solution will

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What is the magnitude of the change in pH when 0.005 moles of HCl is added to 0.100 L of a buffer solution that is 0.100 M in CH₃CO₂H and 0.100 M NaCH₃CO₂? The K_a for acetic acid is 1.8 × 10^-5.

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. -At which point a-d is the pK_a of the acid equal to the pH?

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 0.100 M solution of alanine after 100.00 mL of 0.100 M NaOH has been added?

At 25°C calcium fluoride has a solubility product constant K_sp = 3.5 × 10^-11.The solubility of CaF₂ at this temperature is ________ mol/L.

A buffer solution is prepared by dissolving 27.22 g of KH₂PO₄ and 3.37 g of KOH in enough water to make 0.100 L of solution.What is the pH of the H₂PO₄^-/HPO₄^2- buffer if the K_a2 = 6.2 × 10^-8?

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH₃ with 25.00 mL of 0.10 M NH₄Cl? Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5 for NH₃.

The balanced equation for the solubility equilibrium of Ba(OH)₂ is shown below.What is the equilibrium constant expression for the K_sp of Ba(OH)₂? Ba(OH)₂(s)⇌ Ba²⁺(aq)+ 2 OH^-(aq)

What is the percent dissociation of glycine if the solution has a pH = 8.60 and a pK_a = 9.60?

The pH of a solution of HIO₃ (K_a = 1.7 × 10^-1)and KIO₃ is 1.00.What is the molarity of KIO₃ if the molarity of HIO₃ is 0.025 M?

What is the equation relating the equilibrium constant K_n for the neutralization of a weak acid with a weak base to the K_a of the acid,the K_b of the base and K_w?