Calculate the percent ionization of nitrous acid in a solution that is 0.222 M in nitrous acid (HNO2)and 0.278 M in potassium nitrite (KNO2).The acid dissociation constant of nitrous acid is 4.50 × 10-4.

A) 55.6 B) 0.162 C) 15.5 D) 2.78 × 10-3 E) 3.448 A) 55.6 B) 0.162 C) 15.5 D) 2.78 × 10-3 E) 3.448

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M HCHO2 with 100.0 mL of 0.20 M LiCHO2.The Ka for HCHO2 is 1.8 × 10-4.

A) 3.87 B) 3.74 C) 10.53 D) 3.47 E) 10.13 A) 3.87 B) 3.74 C) 10.53 D) 3.47 E) 10.13

What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.50? Ksp for Mg(OH)2 is 5.6 × 10-12.

A) 1.8 × 10-10 M B) 5.6 × 10-9 M C) 2.4 × 10-6 M D) 1.1 × 10-4 M A) 1.8 × 10-10 M B) 5.6 × 10-9 M C) 2.4 × 10-6 M D) 1.1 × 10-4 M

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution after the addition of 150.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

A) 1.70 B) 6.44 C) 7.56 D) 12.30 E) 2.30 A) 1.70 B) 6.44 C) 7.56 D) 12.30 E) 2.30

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M methylamine,CH3NH2,with 20.00 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) 10.17 B) 10.57 C) 10.97 D) 11.78 A) 10.17 B) 10.57 C) 10.97 D) 11.78

What volume of 5.00 × 10-3 M HNO3 is needed to titrate 80.00 mL of 5.00 × 10-3 M Ca(OH)2 to the equivalence point?

A) 10.0 mL B) 40.0 mL C) 80.0 mL D) 160.mL A) 10.0 mL B) 40.0 mL C) 80.0 mL D) 160.mL

Exam 16: Aqueous Ionic Equilibrium

A solution is prepared by dissolving 0.23 mol of hydrazoic acid and 0.27 mol of sodium azide in water sufficient to yield 1.00 L of solution.The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly.The pH does not increase drastically because the NaOH reacts with the ________ present in the buffer solution.The K_a of hydrazoic acid is 1.9 × 10^-5.

(Multiple Choice)

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Question 121

Calculate the percent ionization of nitrous acid in a solution that is 0.222 M in nitrous acid (HNO₂)and 0.278 M in potassium nitrite (KNO₂).The acid dissociation constant of nitrous acid is 4.50 × 10^-4.

(Multiple Choice)

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Question 122

Which metal hydroxide is most soluble in water?

(Multiple Choice)

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Question 123

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl.The K_a for HF is 3.5 × 10^-4.

(Multiple Choice)

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Question 124

Which of the following solutions is a good buffer system?

(Multiple Choice)

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Question 125

Which one of the following statements is true?

(Multiple Choice)

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Question 126

What is the hydronium ion concentration in a solution prepared by mixing 50.00 mL of 0.10 M HCN with 50.00 mL of 0.030 M NaCN? Assume that the volumes of the solutions are additive and that K_a = 4.9 × 10^-10 for HCN.

(Multiple Choice)

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Question 127

Which of the following compounds will have the highest molar solubility in pure water?

(Multiple Choice)

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Question 128

Determine the molar solubility of AgI in pure water.K_sp (AgI)= 8.51 × 10^-17.

(Multiple Choice)

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Question 129

A buffer solution is 0.100 M in both HC₇H₅O₂ and LiC₇H₅O₂ and has a pH of 4.19.Which of the following pH values would you be most likely to see from the addition of a small amount of a dilute solution of a strong base?

(Multiple Choice)

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Question 130

The molar solubility of CuI is 2.26 × 10^-6 M in pure water.Calculate the K_sp for CuI.

(Multiple Choice)

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Question 131

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M HCHO₂ with 100.0 mL of 0.20 M LiCHO₂.The K_a for HCHO₂ is 1.8 × 10^-4.

(Multiple Choice)

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Question 132

What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.50? K_spfor Mg(OH)₂ is 5.6 × 10^-1².

(Multiple Choice)

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Question 133

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 150.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

(Multiple Choice)

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Question 134

Match the following. -pH = pK_a

(Multiple Choice)

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Question 135

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M methylamine,CH₃NH₂,with 20.00 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 136

Explain the common ion effect with respect to molar solubility.

(Essay)

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Question 137

Which buffer controls the pH of blood?

(Multiple Choice)

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Question 138

What volume of 5.00 × 10^-3 M HNO₃ is needed to titrate 80.00 mL of 5.00 × 10^-3 M Ca(OH)₂ to the equivalence point?

(Multiple Choice)

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Question 139

A 100.0 mL sample of 0.18 M HClO₄ is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 100.0 mL of LiOH.

(Multiple Choice)

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Question 140

Showing 121 - 140 of 148

Calculate the percent ionization of nitrous acid in a solution that is 0.222 M in nitrous acid (HNO₂)and 0.278 M in potassium nitrite (KNO₂).The acid dissociation constant of nitrous acid is 4.50 × 10^-4.

Which metal hydroxide is most soluble in water?

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl.The K_a for HF is 3.5 × 10^-4.

Which of the following solutions is a good buffer system?

Which one of the following statements is true?

What is the hydronium ion concentration in a solution prepared by mixing 50.00 mL of 0.10 M HCN with 50.00 mL of 0.030 M NaCN? Assume that the volumes of the solutions are additive and that K_a = 4.9 × 10^-10 for HCN.

Which of the following compounds will have the highest molar solubility in pure water?

Determine the molar solubility of AgI in pure water.K_sp (AgI)= 8.51 × 10^-17.

A buffer solution is 0.100 M in both HC₇H₅O₂ and LiC₇H₅O₂ and has a pH of 4.19.Which of the following pH values would you be most likely to see from the addition of a small amount of a dilute solution of a strong base?

The molar solubility of CuI is 2.26 × 10^-6 M in pure water.Calculate the K_sp for CuI.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M HCHO₂ with 100.0 mL of 0.20 M LiCHO₂.The K_a for HCHO₂ is 1.8 × 10^-4.

What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.50? K_spfor Mg(OH)₂ is 5.6 × 10^-1².

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 150.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Match the following. -pH = pK_a

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M methylamine,CH₃NH₂,with 20.00 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.

Explain the common ion effect with respect to molar solubility.

Which buffer controls the pH of blood?

What volume of 5.00 × 10^-3 M HNO₃ is needed to titrate 80.00 mL of 5.00 × 10^-3 M Ca(OH)₂ to the equivalence point?

A 100.0 mL sample of 0.18 M HClO₄ is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 100.0 mL of LiOH.

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Exam 16: Aqueous Ionic Equilibrium

Calculate the percent ionization of nitrous acid in a solution that is 0.222 M in nitrous acid (HNO2)and 0.278 M in potassium nitrite (KNO2).The acid dissociation constant of nitrous acid is 4.50 × 10-4.

Which metal hydroxide is most soluble in water?

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl.The Ka for HF is 3.5 × 10-4.

Which of the following solutions is a good buffer system?

Which one of the following statements is true?

What is the hydronium ion concentration in a solution prepared by mixing 50.00 mL of 0.10 M HCN with 50.00 mL of 0.030 M NaCN? Assume that the volumes of the solutions are additive and that Ka = 4.9 × 10-10 for HCN.

Which of the following compounds will have the highest molar solubility in pure water?

Determine the molar solubility of AgI in pure water.Ksp (AgI)= 8.51 × 10-17.

A buffer solution is 0.100 M in both HC7H5O2 and LiC7H5O2 and has a pH of 4.19.Which of the following pH values would you be most likely to see from the addition of a small amount of a dilute solution of a strong base?

The molar solubility of CuI is 2.26 × 10-6 M in pure water.Calculate the Ksp for CuI.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M HCHO2 with 100.0 mL of 0.20 M LiCHO2.The Ka for HCHO2 is 1.8 × 10-4.

What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.50? Ksp for Mg(OH)2 is 5.6 × 10-12.

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution after the addition of 150.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

Match the following. -pH = pKa

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M methylamine,CH3NH2,with 20.00 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.

Explain the common ion effect with respect to molar solubility.

Which buffer controls the pH of blood?

What volume of 5.00 × 10-3 M HNO3 is needed to titrate 80.00 mL of 5.00 × 10-3 M Ca(OH)2 to the equivalence point?

A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 100.0 mL of LiOH.

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Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

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Liquids, Solids, and Intermolecular Forces

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Chemical Kinetics

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Calculate the percent ionization of nitrous acid in a solution that is 0.222 M in nitrous acid (HNO₂)and 0.278 M in potassium nitrite (KNO₂).The acid dissociation constant of nitrous acid is 4.50 × 10^-4.

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl.The K_a for HF is 3.5 × 10^-4.

What is the hydronium ion concentration in a solution prepared by mixing 50.00 mL of 0.10 M HCN with 50.00 mL of 0.030 M NaCN? Assume that the volumes of the solutions are additive and that K_a = 4.9 × 10^-10 for HCN.

Determine the molar solubility of AgI in pure water.K_sp (AgI)= 8.51 × 10^-17.

A buffer solution is 0.100 M in both HC₇H₅O₂ and LiC₇H₅O₂ and has a pH of 4.19.Which of the following pH values would you be most likely to see from the addition of a small amount of a dilute solution of a strong base?

The molar solubility of CuI is 2.26 × 10^-6 M in pure water.Calculate the K_sp for CuI.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M HCHO₂ with 100.0 mL of 0.20 M LiCHO₂.The K_a for HCHO₂ is 1.8 × 10^-4.

What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.50? K_spfor Mg(OH)₂ is 5.6 × 10^-1².

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 150.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Match the following. -pH = pK_a

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M methylamine,CH₃NH₂,with 20.00 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.

What volume of 5.00 × 10^-3 M HNO₃ is needed to titrate 80.00 mL of 5.00 × 10^-3 M Ca(OH)₂ to the equivalence point?

A 100.0 mL sample of 0.18 M HClO₄ is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 100.0 mL of LiOH.