A 0.010 M solution of the weak acid HA has an osmotic pressure (see chapter on solutions and colloids) of 0.293 atm at 25 °C. A 0.010 M solution of the weak acid HB has an osmotic pressure of 0.345 atm under the sameconditions.(a) Which acid has the larger equilibrium constant for ionizationHA [HA(aq) ⇌ A−(aq) + H+(aq)] or HB [HB(aq) ⇌ H+(aq) + B−(aq)] ?(b) What are the equilibrium constants for the ionization of these acids?
A 0.010 M solution of the weak acid HA has an osmotic pressure (see chapter on solutions and colloids) of 0.293 atm at 25 °C. A 0.010 M solution of the weak acid HB has an osmotic pressure of 0.345 atm under the sameconditions.(a) Which acid has the larger equilibrium constant for ionizationHA [HA(aq) ⇌ A−(aq) + H+(aq)] or HB [HB(aq) ⇌ H+(aq) + B−(aq)] ?(b) What are the equilibrium constants for the ionization of these acids?
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A 0.010 M solution of the weak acid HA has an osmotic pressure (see chapter on solutions and colloids) of 0.293 atm at 25 °C. A 0.010 M solution of the weak acid HB has an osmotic pressure of 0.345 atm under the same
conditions.
(a) Which acid has the larger equilibrium constant for ionization
HA [HA(aq) ⇌ A−(aq) + H+(aq)] or HB [HB(aq) ⇌ H+(aq) + B−(aq)] ?
(b) What are the equilibrium constants for the ionization of these acids?
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