10. Given the pH of 1.5 M chloroacetic acid, CH2CICOOH solution is 1.96. a. Write an equation to show the dissociation of CH2CICOOH in water. b. Calculate the Ka of the acid. c. Calculate the pKb of its conjugate base. d. Which is a stronger base, acetate ion or the conjugate base of CH2CICOOH? (Ka of acetic acid, CH3COOH = 1.8 x 10-5) %3D

10. Given the pH of 1.5 M chloroacetic acid, CH2CICOOH solution is 1.96. a. Write an equation to show the dissociation of CH2CICOOH in water. b. Calculate the Ka of the acid. c. Calculate the pKb of its conjugate base. d. Which is a stronger base, acetate ion or the conjugate base of CH2CICOOH? (Ka of acetic acid, CH3COOH = 1.8 x 10-5) %3D

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 38QRT

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