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selena selena
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A year ago
A 0.214 M aqueous solution of a monoprotic base has a pH of 11.48.  What is the ionization constant of this base?

▸ 1.4 × 10-2

▸ 4.3 × 10-5

▸ 1.5 × 10-11

▸ 5.1 × 10-23

▸ 2.0 × 10-6
Textbook 

General Chemistry: Principles and Modern Applications


Edition: 11th
Authors:
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jbarnett14jbarnett14
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A year ago Edited: 2 months ago, bio_man
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Pick (B)

================

pH = 11.48

pOH = 14 - 11.48 = 2.52

[OH-] = 10-pOH = 10-2.52 = 0.003 M

[BH+] = [OH-] = 0.003 M

= 0.214 - 0.003 = 0.211 M

Kb = [OH-] [BH+] /

Kb = [0.003][0.003] / [0.211]

Kb = 4.26 x 10-5
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