Consider the Ka values for the following acids: Cyanic acid,HOCN,3.5 × 10-4 Formic acid,HCHO2,1.7 × 10-4 Lactic acid,HC3H5O3,1.3 × 10-4 Propionic acid,HC3H5O2,1.3 × 10-5 Benzoic acid,HC7H5O2,6.3 × 10-5 Which has the strongest conjugate base?

A) propionic acid B) benzoic acid C) lactic acid D) formic acid E) cyanic A) propionic acid B) benzoic acid C) lactic acid D) formic acid E) cyanic

If 20 mL of 0.10 M NaOH is added to 30 mL of 0.20 M HC2H3O2,what is the pH of the resulting solution at 25°C? Ka for HC2H3O2 is 1.8 × 10-5 at 25°C.

A) 10.2 B) 4.3 C) 5.0 D) 2.7 E) 4.4 A) 10.2 B) 4.3 C) 5.0 D) 2.7 E) 4.4

A solution contains 0.08 M acetic acid,HC2H3O2 (Ka = 1.7 × 10−5 at 25°C),and 0.15 M sodium acetate,NaC2H3O2.What is the pH of the solution at 25°C?

A) 5.04 B) 6.02 C) 4.28 D) 3.86 E) 7.05 A) 5.04 B) 6.02 C) 4.28 D) 3.86 E) 7.05

Which of the following will give a buffer with a pH near 9.24 when the acid and conjugate base are mixed in equimolar proportions? Acid Ka NH4+ (from ammonia) 5)69 × 10-10 HC2H3O2 (acetic acid) 1)75 × 10-5 HF (hydrofluoric acid) 6)8 × 10-4 CH3CH2NH3+ (from ethylamine) 2)12 × 10-11

A) ammonia B) acetic acid C) hydrofluoric acid D) ethylamine E) none A) ammonia B) acetic acid C) hydrofluoric acid D) ethylamine E) none

15.0 mL of 0.50 M HCl is added to a 100.0-mL sample of 0.484 M HNO2 (Ka for HNO2 = 4.0 × 10-4).What is the equilibrium concentration of NO2- ions?

A) 4.2 × 10-1 M B) 1.7 × 10-4 M C) 5.1 × 10-2 M D) 2.6 × 10-3 M E) none of these A) 4.2 × 10-1 M B) 1.7 × 10-4 M C) 5.1 × 10-2 M D) 2.6 × 10-3 M E) none of these

Exam 16: Acid-Base Equilibria

What is the percent ionization of a solution prepared by dissolving 0.0175 mol of chloroacetic acid,(HC₂H₂O₂Cl)in 1.30 L of water? For chloroacetic acid,K_a = 1.4 × 10^-3.

(Multiple Choice)

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Question 61

What is the equilibrium hydronium ion concentration of an initially 4.5 M solution of hypoiodous acid,HOI,at 25°C (K_a = )?

(Multiple Choice)

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Question 62

Consider the K_a values for the following acids: Cyanic acid,HOCN,3.5 × 10^-4Formic acid,HCHO₂,1.7 × 10^-4Lactic acid,HC₃H₅O₃,1.3 × 10^-4Propionic acid,HC₃H₅O₂,1.3 × 10^-5 Benzoic acid,HC₇H₅O₂,6.3 × 10^-5 Which has the strongest conjugate base?

(Multiple Choice)

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Question 63

The _____ is the shift in an ionic equilibrium caused by the addition of a solute that provides an ion that takes part in the equilibrium.

(Multiple Choice)

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Question 64

If 20 mL of 0.10 M NaOH is added to 30 mL of 0.20 M HC₂H₃O₂,what is the pH of the resulting solution at 25°C? K_a for HC₂H₃O₂ is 1.8 × 10^-5 at 25°C.

(Multiple Choice)

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Question 65

For which of the following equilibria does K_c correspond to the base-ionization constant,K_b,of HCO₃^-?

(Multiple Choice)

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Question 66

A solution contains 10.mmol of H₃PO₄ and 5.0 mmol of NaH₂PO₄.How many milliliters of 0.10 M NaOH must be added to reach the second equivalence point of the titration of the H₃PO₄ with NaOH?

(Multiple Choice)

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Question 67

For which of the following equilibria does K_c correspond to the acid-ionization constant,K_a,of HCO₃^-?

(Multiple Choice)

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Question 68

The K_a for hydrofluoric acid is 6.8 × 10^-4.What is K_b for the fluoride ion?

(Multiple Choice)

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Question 69

Which of the following salts forms an acidic aqueous solution?

(Multiple Choice)

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Question 70

A solution contains 0.08 M acetic acid,HC₂H₃O₂ (K_a = 1.7 × 10⁻⁵ at 25°C),and 0.15 M sodium acetate,NaC₂H₃O₂.What is the pH of the solution at 25°C?

(Multiple Choice)

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Question 71

A 25.00-mL sample of propionic acid,HC₃H₅O₂,of unknown concentration was titrated with 0.141 M KOH.The equivalence point was reached when 43.76 mL of base had been added.What is the hydroxide-ion concentration at the equivalence point? K_a for propionic acid is 1.3 × 10^-5 at 25°C.

(Multiple Choice)

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Question 72

Which of the following will give a buffer with a pH near 9.24 when the acid and conjugate base are mixed in equimolar proportions? Acid K_a NH₄⁺ (from ammonia) 5)69 × 10^-10 HC₂H₃O₂ (acetic acid) 1)75 × 10^-5 HF (hydrofluoric acid) 6)8 × 10^-4 CH₃CH₂NH₃⁺ (from ethylamine) 2)12 × 10^-11

(Multiple Choice)

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Question 73

15.0 mL of 0.50 M HCl is added to a 100.0-mL sample of 0.484 M HNO₂ (K_a for HNO₂ = 4.0 × 10^-4).What is the equilibrium concentration of NO₂^- ions?

(Multiple Choice)

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Question 74

Titration of 0.2834 g of an unknown monoprotic acid dissolved in 25.00 mL of water requires 29.83 mL of 0.1582 M NaOH to reach the endpoint.What is the molar mass of the acid?

(Multiple Choice)

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Question 75

A 25.00-mL sample of propionic acid,HC₃H₅O₂,of unknown concentration was titrated with 0.103 M KOH.The equivalence point was reached when 43.88 mL of base had been added.What was the original concentration of the propionic acid?

(Multiple Choice)

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Question 76

Which of the following mixtures will be a buffer when dissolved in 1 L of water?

(Multiple Choice)

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Question 77

A(n)_____ is a solution characterized by the ability to resist changes in pH when limited amounts of acid or base are added to it.

(Multiple Choice)

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Question 78

Which of the following represents the usual relationship of acid-ionization constants for a triprotic acid?

(Multiple Choice)

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Question 79

What is the hydronium-ion concentration of a solution that is formed by combining 600.mL of 0.30 M NaOH with 400.mL of 0.90 M HNO₃ at 25°C?

(Multiple Choice)

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Question 80

Showing 61 - 80 of 148

Exam 16: Acid-Base Equilibria

What is the percent ionization of a solution prepared by dissolving 0.0175 mol of chloroacetic acid,(HC2H2O2Cl)in 1.30 L of water? For chloroacetic acid,Ka = 1.4 × 10-3.

What is the equilibrium hydronium ion concentration of an initially 4.5 M solution of hypoiodous acid,HOI,at 25°C (Ka = )?

Consider the Ka values for the following acids: Cyanic acid,HOCN,3.5 × 10-4 Formic acid,HCHO2,1.7 × 10-4 Lactic acid,HC3H5O3,1.3 × 10-4 Propionic acid,HC3H5O2,1.3 × 10-5 Benzoic acid,HC7H5O2,6.3 × 10-5 Which has the strongest conjugate base?

The _____ is the shift in an ionic equilibrium caused by the addition of a solute that provides an ion that takes part in the equilibrium.

If 20 mL of 0.10 M NaOH is added to 30 mL of 0.20 M HC2H3O2,what is the pH of the resulting solution at 25°C? Ka for HC2H3O2 is 1.8 × 10-5 at 25°C.

For which of the following equilibria does Kc correspond to the base-ionization constant,Kb,of HCO3-?

A solution contains 10.mmol of H3PO4 and 5.0 mmol of NaH2PO4.How many milliliters of 0.10 M NaOH must be added to reach the second equivalence point of the titration of the H3PO4 with NaOH?

For which of the following equilibria does Kc correspond to the acid-ionization constant,Ka,of HCO3-?

The Ka for hydrofluoric acid is 6.8 × 10-4.What is Kb for the fluoride ion?

Which of the following salts forms an acidic aqueous solution?

A solution contains 0.08 M acetic acid,HC2H3O2 (Ka = 1.7 × 10−5 at 25°C),and 0.15 M sodium acetate,NaC2H3O2.What is the pH of the solution at 25°C?

A 25.00-mL sample of propionic acid,HC3H5O2,of unknown concentration was titrated with 0.141 M KOH.The equivalence point was reached when 43.76 mL of base had been added.What is the hydroxide-ion concentration at the equivalence point? Ka for propionic acid is 1.3 × 10-5 at 25°C.

Which of the following will give a buffer with a pH near 9.24 when the acid and conjugate base are mixed in equimolar proportions? Acid Ka NH4+ (from ammonia) 5)69 × 10-10 HC2H3O2 (acetic acid) 1)75 × 10-5 HF (hydrofluoric acid) 6)8 × 10-4 CH3CH2NH3+ (from ethylamine) 2)12 × 10-11

15.0 mL of 0.50 M HCl is added to a 100.0-mL sample of 0.484 M HNO2 (Ka for HNO2 = 4.0 × 10-4).What is the equilibrium concentration of NO2- ions?

Titration of 0.2834 g of an unknown monoprotic acid dissolved in 25.00 mL of water requires 29.83 mL of 0.1582 M NaOH to reach the endpoint.What is the molar mass of the acid?

A 25.00-mL sample of propionic acid,HC3H5O2,of unknown concentration was titrated with 0.103 M KOH.The equivalence point was reached when 43.88 mL of base had been added.What was the original concentration of the propionic acid?

Which of the following mixtures will be a buffer when dissolved in 1 L of water?

A(n)_____ is a solution characterized by the ability to resist changes in pH when limited amounts of acid or base are added to it.

Which of the following represents the usual relationship of acid-ionization constants for a triprotic acid?

What is the hydronium-ion concentration of a solution that is formed by combining 600.mL of 0.30 M NaOH with 400.mL of 0.90 M HNO3 at 25°C?

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What is the percent ionization of a solution prepared by dissolving 0.0175 mol of chloroacetic acid,(HC₂H₂O₂Cl)in 1.30 L of water? For chloroacetic acid,K_a = 1.4 × 10^-3.

What is the equilibrium hydronium ion concentration of an initially 4.5 M solution of hypoiodous acid,HOI,at 25°C (K_a = )?

Consider the K_a values for the following acids: Cyanic acid,HOCN,3.5 × 10^-4Formic acid,HCHO₂,1.7 × 10^-4Lactic acid,HC₃H₅O₃,1.3 × 10^-4Propionic acid,HC₃H₅O₂,1.3 × 10^-5 Benzoic acid,HC₇H₅O₂,6.3 × 10^-5 Which has the strongest conjugate base?

If 20 mL of 0.10 M NaOH is added to 30 mL of 0.20 M HC₂H₃O₂,what is the pH of the resulting solution at 25°C? K_a for HC₂H₃O₂ is 1.8 × 10^-5 at 25°C.

For which of the following equilibria does K_c correspond to the base-ionization constant,K_b,of HCO₃^-?

A solution contains 10.mmol of H₃PO₄ and 5.0 mmol of NaH₂PO₄.How many milliliters of 0.10 M NaOH must be added to reach the second equivalence point of the titration of the H₃PO₄ with NaOH?

For which of the following equilibria does K_c correspond to the acid-ionization constant,K_a,of HCO₃^-?

The K_a for hydrofluoric acid is 6.8 × 10^-4.What is K_b for the fluoride ion?

A solution contains 0.08 M acetic acid,HC₂H₃O₂ (K_a = 1.7 × 10⁻⁵ at 25°C),and 0.15 M sodium acetate,NaC₂H₃O₂.What is the pH of the solution at 25°C?

A 25.00-mL sample of propionic acid,HC₃H₅O₂,of unknown concentration was titrated with 0.141 M KOH.The equivalence point was reached when 43.76 mL of base had been added.What is the hydroxide-ion concentration at the equivalence point? K_a for propionic acid is 1.3 × 10^-5 at 25°C.

15.0 mL of 0.50 M HCl is added to a 100.0-mL sample of 0.484 M HNO₂ (K_a for HNO₂ = 4.0 × 10^-4).What is the equilibrium concentration of NO₂^- ions?

A 25.00-mL sample of propionic acid,HC₃H₅O₂,of unknown concentration was titrated with 0.103 M KOH.The equivalence point was reached when 43.88 mL of base had been added.What was the original concentration of the propionic acid?

What is the hydronium-ion concentration of a solution that is formed by combining 600.mL of 0.30 M NaOH with 400.mL of 0.90 M HNO₃ at 25°C?