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Calculate the pH at 25 of a 0.590 M aqueous solution of a weak base with a Kb value of 1.27 x 10-5.

Calculate the pH at 25 of a 0.590 M aqueous solution of a weak base with a Kb value of 1.27 x 10-5.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Calculate the pH at 25 of a 0.590 M aqueous solution of a weak base with a Kb value of 1.27 x 10-5. 

Expert Solution
Step 1

Given : Initial concentration of weak base B = 0.590 M

Kb of base = 1.27 X 10-5 

Since B is a weak base.

Hence it will undergo hydrolysis as per the reaction,

=> B (aq) + H2O (l) --------> BH+ (aq) + OH- (aq)

 

Step 2

Assuming y concentration of B is ionised in the reaction.

Hence the concentration of ions produced in the reaction are,

=> [BH+ ] = y = [OH- ]

And the concentration of B remaining in the solution, [B] = Initial - ionised = 0.590 - y

Since Kb <<< 1. Hence we can assume negligible concentration of B will ionise.

Hence [B] = 0.590 - y = 0.590 M approx.

 

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