Explanation Let BOH be a weak base. When it dissociates in water we can see the following reaction. B O H ( a q ) + H 2 O ( l ) ↔ B + ( a q ) + O H − ( a q ) Now, since pH for the base 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 base is 0.135 pH = 11.23 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 =11.23 pH + pOH = 14 pOH = 14 - pH pOH = 14 - 11.23 pOH = 2.77 Now, pOH = -log[ OH − ] [ OH − ]= 10 −pOH [ OH − ]= 10 −2.77 [ OH − ]= 0...

Selected Solutions Manual for Chemistry: Structure and Properties

2nd Edition

ISBN: 9780134460673

Author: Nivaldo J. Tro, Kathy Thrush-Shaginaw, Mary Beth Kramer

Publisher: PEARSON

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Chapter 16, Problem 96E

Interpretation Introduction

To determine:

The K_b for base

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Chapter 16, Problem 95E

Chapter 16, Problem 97E

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Chapter 16 Solutions

Selected Solutions Manual for Chemistry: Structure and Properties

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