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A hypothetical weak base has Kb = 5.0 x 10-8. Calculate the equilibrium concentrations of the base, its conjugate acid, and OH in a 0.15 M solution of the base. What is the pH of the solution? [B] = mol/L [HB+] = [OH-] = pH = mol/L mol/L

A hypothetical weak base has Kb = 5.0 x 10-8. Calculate the equilibrium concentrations of the base, its conjugate acid, and OH in a 0.15 M solution of the base. What is the pH of the solution? [B] = mol/L [HB+] = [OH-] = pH = mol/L mol/L

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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A hypothetical weak base has Kb = 5.0 x 10-8. Calculate the equilibrium concentrations of the base, its conjugate acid, and OH in a 0.15 M solution of the base. What is the pH of the solution? [B] = mol/L [HB+] = [OH-] = pH = mol/L mol/L
Transcribed Image Text:A hypothetical weak base has Kb = 5.0 x 10-8. Calculate the equilibrium concentrations of the base, its conjugate acid, and OH in a 0.15 M solution of the base. What is the pH of the solution? [B] = mol/L [HB+] = [OH-] = pH = mol/L mol/L
The ionization constant of a very weak acid, HA, is 7.0x10-9. Calculate the equilibrium concentrations of H3O+, A, and HA in a 0.040 M solution of the acid. Determine the concentrations of all species at equilibrium and the solution pH. [H3O+] = [A] = [HA] = pH = mol/L mol/L mol/L
Transcribed Image Text:The ionization constant of a very weak acid, HA, is 7.0x10-9. Calculate the equilibrium concentrations of H3O+, A, and HA in a 0.040 M solution of the acid. Determine the concentrations of all species at equilibrium and the solution pH. [H3O+] = [A] = [HA] = pH = mol/L mol/L mol/L
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