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Is the response below correct, I would belive that   pOH = – log (12.7) = 1.103 would be -1.103   Please let me know, as that would change the pH of the final solution

Is the response below correct, I would belive that   pOH = – log (12.7) = 1.103 would be -1.103   Please let me know, as that would change the pH of the final solution

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter16: Reactions Between Acids And Bases
Section: Chapter Questions
Problem 16.49QE: Estimate the pH that results when the following two solutions are mixed. a) 50 mL of 0.3 M CH3COOH...
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Is the response below correct, I would belive that
 
pOH = – log (12.7) = 1.103 would be -1.103
 
Please let me know, as that would change the pH of the final solution
 
 
 
 
Step 1

NaOH ---> Na+ + OH– 

[NaOH] = 12.7 M = [OH–] 

So,

pOH  = – log [OH–]

pOH = – log (12.7) = 1.103

 

 

Step 2

Since, we know that ;

pH  + pOH  = 14 

On substituting the values into it, we get ;

pH = 14 – pOH

= 14 – 1.103 = 12.897 ≈ 12.9

Hence,

The pH will be 12.9.

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