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Science Chemistry Chemistry: An Atoms-Focused Approach

The degree of ionization and K a of the unknown acid. Solution: The degree of ionization of the unknown acid is 1.63 % , and its K a is 6.74 × 10 - 5 . Explanation: Concept: Degree of ionization of a weak acid (or base) is the fraction of the acid that has ionized into ions in a solution. The part of the originally present acid that ionizes can be calculated on the basis of a RICE table and the given equilibrium value of H + ions in the solution. The acid dissociation constant is the equilibrium constant for the ionization reaction. Formula: P e r c e n t i o n i z a t i o n = H + e q u i l i b r i u m H A i n i t i a l × 100 K a = H 3 O + A - [ H A ] Given: H 3 O + e q u i l i b r i u m = 4.07 × 10 - 3 M H A i n i t i a l = 0.250 M Calculations: The equilibrium concentration of H 3 O + is given as 4.07 × 10 - 3 M . Inserting the values of initial given concentration of the acid and equilibrium concentration of the conjugate base, we get P e r c e n t i o n i z a t i o n = H + e q u i l i b r i u m H A i n i t i a l × 100 P e r c e n t i o n i z a t i o n = 4.07 × 10 - 3 M 0.250 M × 100 P e r c e n t i o n i z a t i o n = 1.628 % Thus, the percent dissociation of the acid is 1.63 % . At equilibrium, H 3 O + = A - = 4.07 × 10 - 3 M . The equilibrium concentration for the acid is H A e q u i l i b r i u m = H A i n i t i a l - H 3 O + e q u i l i b r i u m H A e q u i l i b r i u m = 0.250 M - 4.07 × 10 - 3 M = 0.24593 M H A e q u i l i b r i u m = 0.24593 M Inserting the equilibrium values for all the species in the K a expression, we get K a = ( 4.07 × 10 - 3 ) ( 4.07 × 10 - 3 ) 0.24593 K a = 6.7356 × 10 - 5 Thus, the acid dissociation constant value for the unknown acid is 6.74 × 10 - 5 . Conclusion: From the initial concentration of a weak acid and equilibrium concentration of its conjugate base, we can find the percent ionization of the acid.

The degree of ionization and K a of the unknown acid. Solution: The degree of ionization of the unknown acid is 1.63 % , and its K a is 6.74 × 10 - 5 . Explanation: Concept: Degree of ionization of a weak acid (or base) is the fraction of the acid that has ionized into ions in a solution. The part of the originally present acid that ionizes can be calculated on the basis of a RICE table and the given equilibrium value of H + ions in the solution. The acid dissociation constant is the equilibrium constant for the ionization reaction. Formula: P e r c e n t i o n i z a t i o n = H + e q u i l i b r i u m H A i n i t i a l × 100 K a = H 3 O + A - [ H A ] Given: H 3 O + e q u i l i b r i u m = 4.07 × 10 - 3 M H A i n i t i a l = 0.250 M Calculations: The equilibrium concentration of H 3 O + is given as 4.07 × 10 - 3 M . Inserting the values of initial given concentration of the acid and equilibrium concentration of the conjugate base, we get P e r c e n t i o n i z a t i o n = H + e q u i l i b r i u m H A i n i t i a l × 100 P e r c e n t i o n i z a t i o n = 4.07 × 10 - 3 M 0.250 M × 100 P e r c e n t i o n i z a t i o n = 1.628 % Thus, the percent dissociation of the acid is 1.63 % . At equilibrium, H 3 O + = A - = 4.07 × 10 - 3 M . The equilibrium concentration for the acid is H A e q u i l i b r i u m = H A i n i t i a l - H 3 O + e q u i l i b r i u m H A e q u i l i b r i u m = 0.250 M - 4.07 × 10 - 3 M = 0.24593 M H A e q u i l i b r i u m = 0.24593 M Inserting the equilibrium values for all the species in the K a expression, we get K a = ( 4.07 × 10 - 3 ) ( 4.07 × 10 - 3 ) 0.24593 K a = 6.7356 × 10 - 5 Thus, the acid dissociation constant value for the unknown acid is 6.74 × 10 - 5 . Conclusion: From the initial concentration of a weak acid and equilibrium concentration of its conjugate base, we can find the percent ionization of the acid.

Solution Summary: The author explains how to determine the K_a value of an unknown acid and its degree of ionization in a solution of known equilibrium concentration.

Chemistry: An Atoms-Focused Approach

Chemistry: An Atoms-Focused Approach

1st Edition

ISBN: 9780393124200

Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster

Publisher: W. W. Norton & Company

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