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 0.0500 M solution of alanine after 25.00 mL of 0.100 M NaOH has been added?

A) 2)34 B) 4)85 C) 5)59 D) 6)72 A) 2)34 B) 4)85 C) 5)59 D) 6)72

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid HS1U1B12S1U1B0A with NaOH. -Which point a-d represents the second equivalence point?

A) point a B) point b C) point c D) point d A) point a B) point b C) point c D) point d

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid HS1U1B12S1U1B0A with NaOH. -What is the pH at the first equivalence point?

A) pH = pKa1 B) pH = 14 - pKa1 C) pH = (pKa1 + pKa2)/2 D) pH = pKa1 + pKa2 A) pH = pKa1 B) pH = 14 - pKa1 C) pH = (pKa1 + pKa2)/2 D) pH = pKa1 + pKa2

What volume of 5.00 × 10-3 M HNO3 is needed to titrate 100.00 mL of 5.00 × 10-3 M Ca(OH)2 to the equivalence point?

A) 12.5 mL B) 50.0 mL C) 100.mL D) 200.mL A) 12.5 mL B) 50.0 mL C) 100.mL D) 200.mL

What is the common ion in a solution prepared by mixing 0.10 M NaCH3CO2 with 0.10 M CH3CO2H?

A) H3O+ B) Na+ C) CH3CO2- D) OH- A) H3O+ B) Na+ C) CH3CO2- D) OH-

What is the pH of a buffer system made by dissolving 10.70 grams of NH4Cl and 20.00 mL of 12.0 M NH3 in enough water to make 1.000 L of solution? Kb = 1.8 × 10-5 for NH3.

A) 9)18 B) 9)26 C) 9)34 D) 11.03 A) 9)18 B) 9)26 C) 9)34 D) 11.03

What is the molar solubility of CaF2 in 0.10 M NaF solution at 25°C? The Ksp for CaF2 is

A) 8)5 × 10-10 M B) 3)4 × 10-10 M C) 3)4 × 10-9 M D) 2)0 × 10-4 M A) 8)5 × 10-10 M B) 3)4 × 10-10 M C) 3)4 × 10-9 M D) 2)0 × 10-4 M

When 50 mL of 0.10 M NH4Cl is added to 50 mL of 0.10 M NH3,relative to the pH of the 0.10 M NH3 solution the pH of the resulting solution will

A) become 7. B) decrease. C) increase. D) remain the same. A) become 7. B) decrease. C) increase. D) remain the same.

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H2A+ with NaOH.Which point a-d represents the isoelectric point?

A) point a B) point b C) point c D) point d A) point a B) point b C) point c D) point d

What is the chromium ion concentration for a saturated solution of Cr(OH)3 if the Ksp for Cr(OH)3 is 6.7 × 10-31?

A) 8)19 × 10-16 M B) 1)26 × 10-8 M C) 2)17 × 10-8 M D) 3)76 × 10-8 M A) 8)19 × 10-16 M B) 1)26 × 10-8 M C) 2)17 × 10-8 M D) 3)76 × 10-8 M

Exam 15: Applications of Aqueous Equilibria

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 0.0500 M solution of alanine after 25.00 mL of 0.100 M NaOH has been added?

(Multiple Choice)

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Question 121

What is the resulting pH when 0.005 moles of KOH is added to 0.100 L of a buffer solution that is 0.100 M in H₂PO₄^- and 0.100 M HPO₄^2- and the K_a2 = 6.2 × 10^-8?

(Multiple Choice)

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Question 122

What is the approximate value of the equilibrium constant,K_n,for the neutralization of nitrous acid with ammonia,shown in the equation below? The K_a for HNO₂ is 4.5 × 10^-4 and the K_b for NH₃ is 1)8 × 10^-5. HNO₂(aq)+ NH₃(aq)⇌ NH₄NO₂(aq)

(Multiple Choice)

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Question 123

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H₂A with NaOH. -Which point a-d represents the second equivalence point?

(Multiple Choice)

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Question 124

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H₂A with NaOH. -What is the pH at the first equivalence point?

(Multiple Choice)

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Question 125

What volume of 5.00 × 10^-3 M HNO₃ is needed to titrate 100.00 mL of 5.00 × 10^-3 M Ca(OH)₂ to the equivalence point?

(Multiple Choice)

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Question 126

What is the common ion in a solution prepared by mixing 0.10 M NaCH₃CO₂ with 0.10 M CH₃CO₂H?

(Multiple Choice)

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Question 127

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous formic acid requires 29.80 mL of 0.0567 M NaOH? K_a = 1.8 × 10^-4for formic acid.

(Multiple Choice)

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Question 128

What is the pH of a buffer system made by dissolving 10.70 grams of NH₄Cl and 20.00 mL of 12.0 M NH₃ in enough water to make 1.000 L of solution? K_b = 1.8 × 10^-5 for NH₃.

(Multiple Choice)

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Question 129

What is the molar solubility of CaF₂ in 0.10 M NaF solution at 25°C? The K_sp for CaF₂ is

(Multiple Choice)

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Question 130

What is the approximate value of the equilibrium constant,K_n,for the neutralization of acetic acid with sodium hydroxide,shown in the equation below? The K_a for acetic acid is 1.8 × 10^-5. CH₃CO₂H(aq)+ NaOH(aq)⇌ H₂O(l)+ NaCH₃CO₂(aq)

(Multiple Choice)

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Question 131

When 50 mL of 0.10 M NH₄Cl is added to 50 mL of 0.10 M NH₃,relative to the pH of the 0.10 M NH₃solution the pH of the resulting solution will

(Multiple Choice)

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Question 132

What is the equilibrium constant expression for the K_sp of Ca₃(PO₄)₂?

(Multiple Choice)

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Question 133

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H₂A⁺ with NaOH.Which point a-d represents the isoelectric point?

(Multiple Choice)

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Question 134

What is the chromium ion concentration for a saturated solution of Cr(OH)₃ if the K_sp for Cr(OH)₃ is 6.7 × 10^-31?

(Multiple Choice)

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Question 135

When equal molar amounts of the following sets of compounds are mixed in water,which will not form a buffer solution?

(Multiple Choice)

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Question 136

What is the [CH₃CO₂-]/[CH₃CO₂H] ratio necessary to make a buffer solution with a pH of 4.34? K_a = 1.8 × 10^-5for CH₃CO₂H.

(Multiple Choice)

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Question 137

Which of the following reactions are not consistent with the concept of acid base amphoterism?

(Multiple Choice)

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Question 138

What is the most soluble salt of the following set?

(Multiple Choice)

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Question 139

Formic acid (HCO₂H,K_a = 1.8 × 10^-4)is the principal component in the venom of stinging ants.What is the molarity of a formic acid solution if 25.00 mL of the formic acid solution requires 29.80 mL of 0.0567 M NaOH to reach the equivalence point?

(Multiple Choice)

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Question 140

Showing 121 - 140 of 190

Exam 15: Applications of Aqueous Equilibria

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 0.0500 M solution of alanine after 25.00 mL of 0.100 M NaOH has been added?

What is the resulting pH when 0.005 moles of KOH is added to 0.100 L of a buffer solution that is 0.100 M in H2PO4- and 0.100 M HPO42- and the Ka2 = 6.2 × 10-8?

What is the approximate value of the equilibrium constant,Kn,for the neutralization of nitrous acid with ammonia,shown in the equation below? The Ka for HNO2 is 4.5 × 10-4 and the Kb for NH3 is 1)8 × 10-5. HNO2(aq)+ NH3(aq)⇌ NH4NO2(aq)

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H2A with NaOH. -Which point a-d represents the second equivalence point?

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H2A with NaOH. -What is the pH at the first equivalence point?

What volume of 5.00 × 10-3 M HNO3 is needed to titrate 100.00 mL of 5.00 × 10-3 M Ca(OH)2 to the equivalence point?

What is the common ion in a solution prepared by mixing 0.10 M NaCH3CO2 with 0.10 M CH3CO2H?

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous formic acid requires 29.80 mL of 0.0567 M NaOH? Ka = 1.8 × 10-4 for formic acid.

What is the pH of a buffer system made by dissolving 10.70 grams of NH4Cl and 20.00 mL of 12.0 M NH3 in enough water to make 1.000 L of solution? Kb = 1.8 × 10-5 for NH3.

What is the molar solubility of CaF2 in 0.10 M NaF solution at 25°C? The Ksp for CaF2 is

What is the approximate value of the equilibrium constant,Kn,for the neutralization of acetic acid with sodium hydroxide,shown in the equation below? The Ka for acetic acid is 1.8 × 10-5. CH3CO2H(aq)+ NaOH(aq)⇌ H2O(l)+ NaCH3CO2(aq)

When 50 mL of 0.10 M NH4Cl is added to 50 mL of 0.10 M NH3,relative to the pH of the 0.10 M NH3 solution the pH of the resulting solution will

What is the equilibrium constant expression for the Ksp of Ca3(PO4)2?

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H2A+ with NaOH.Which point a-d represents the isoelectric point?

What is the chromium ion concentration for a saturated solution of Cr(OH)3 if the Ksp for Cr(OH)3 is 6.7 × 10-31?

When equal molar amounts of the following sets of compounds are mixed in water,which will not form a buffer solution?

What is the [CH3CO2-]/[CH3CO2H] ratio necessary to make a buffer solution with a pH of 4.34? Ka = 1.8 × 10-5 for CH3CO2H.

Which of the following reactions are not consistent with the concept of acid base amphoterism?

What is the most soluble salt of the following set?

Formic acid (HCO2H,Ka = 1.8 × 10-4)is the principal component in the venom of stinging ants.What is the molarity of a formic acid solution if 25.00 mL of the formic acid solution requires 29.80 mL of 0.0567 M NaOH to reach the equivalence point?

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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 0.0500 M solution of alanine after 25.00 mL of 0.100 M NaOH has been added?

What is the resulting pH when 0.005 moles of KOH is added to 0.100 L of a buffer solution that is 0.100 M in H₂PO₄^- and 0.100 M HPO₄^2- and the K_a2 = 6.2 × 10^-8?

What is the approximate value of the equilibrium constant,K_n,for the neutralization of nitrous acid with ammonia,shown in the equation below? The K_a for HNO₂ is 4.5 × 10^-4 and the K_b for NH₃ is 1)8 × 10^-5. HNO₂(aq)+ NH₃(aq)⇌ NH₄NO₂(aq)

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H₂A with NaOH. -Which point a-d represents the second equivalence point?

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H₂A with NaOH. -What is the pH at the first equivalence point?

What volume of 5.00 × 10^-3 M HNO₃ is needed to titrate 100.00 mL of 5.00 × 10^-3 M Ca(OH)₂ to the equivalence point?

What is the common ion in a solution prepared by mixing 0.10 M NaCH₃CO₂ with 0.10 M CH₃CO₂H?

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous formic acid requires 29.80 mL of 0.0567 M NaOH? K_a = 1.8 × 10^-4for formic acid.

What is the pH of a buffer system made by dissolving 10.70 grams of NH₄Cl and 20.00 mL of 12.0 M NH₃ in enough water to make 1.000 L of solution? K_b = 1.8 × 10^-5 for NH₃.

What is the molar solubility of CaF₂ in 0.10 M NaF solution at 25°C? The K_sp for CaF₂ is

What is the approximate value of the equilibrium constant,K_n,for the neutralization of acetic acid with sodium hydroxide,shown in the equation below? The K_a for acetic acid is 1.8 × 10^-5. CH₃CO₂H(aq)+ NaOH(aq)⇌ H₂O(l)+ NaCH₃CO₂(aq)

When 50 mL of 0.10 M NH₄Cl is added to 50 mL of 0.10 M NH₃,relative to the pH of the 0.10 M NH₃solution the pH of the resulting solution will

What is the equilibrium constant expression for the K_sp of Ca₃(PO₄)₂?

The following plot shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H₂A⁺ with NaOH.Which point a-d represents the isoelectric point?

What is the chromium ion concentration for a saturated solution of Cr(OH)₃ if the K_sp for Cr(OH)₃ is 6.7 × 10^-31?

What is the [CH₃CO₂-]/[CH₃CO₂H] ratio necessary to make a buffer solution with a pH of 4.34? K_a = 1.8 × 10^-5for CH₃CO₂H.

Formic acid (HCO₂H,K_a = 1.8 × 10^-4)is the principal component in the venom of stinging ants.What is the molarity of a formic acid solution if 25.00 mL of the formic acid solution requires 29.80 mL of 0.0567 M NaOH to reach the equivalence point?