Explanation Here according to the given question, Morphine is a base. We can say that Morphine dissociates in water according to the following reaction. C 17 H 19 N O 3 ( a q ) + H 2 O ( l ) ↔ C 17 H 20 N O 3 + ( a q ) + O H − ( a q ) Now, since pH for Morphine is given, so we can calculate the pOH using the relation between pH and pOH . Now after calculating the pOH , we can calculate the [ OH − ] using the relation between [ OH − ] and pOH . Now, in order to calculate the dissociation constant K b we will construct the ICE table. Given: Initial Concentration of Morphine is 0.150 M pH = 10.5 xs Formula used: pOH can be calculated using the relation pH + pOH = 14 [ OH − ]can be calculated using the relation pOH = -log[ OH − ] [ OH − ] = 10 −pOH The relation between dissociation constant K b and equilibrium concentration is K b = [ P r o d u c t ] [ R e a c t a n t ] Calculation: Here pH = 10.5 pH + pOH = 14 pOH = 14 - pH pOH = 14 - 10.5 pOH = 3.5 Now, pOH = -log[ OH − ] [ OH − ] = 10 −pOH [ OH − ] = 10 −3.5 [ OH − ] = 0...

Chemistry: Structure and Properties Plus Mastering Chemistry with Pearson eText -- Access Card Package (2nd Edition) (New Chemistry Titles from Niva Tro)

2nd Edition

ISBN: 9780134436524

Author: Nivaldo J. Tro

Publisher: PEARSON

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Chapter 16, Problem 95E

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The K_b for Morphine

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Chapter 16, Problem 94E

Chapter 16, Problem 96E

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Chemistry: Structure and Properties Plus Mastering Chemistry with Pearson eText -- Access Card Package (2nd Edition) (New Chemistry Titles from Niva Tro)

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