Problem: Use information from Appendix D in the textbook to calculate the pH of the following solutions.Calculate the pH of a solution that is 0.080 M in trimethylamine, (CH3)3N, and 0.12 M in trimethylammonium chloride, ((CH3)3NHCl).

FREE Expert Solution

Whenever we have a conjugate acid and a weak base we have a buffer.


When we are dealing with buffers, we can use the Henderson-Hasselbalch equation:

pOH = pKb + log(Conjugate acidweak base)


pK of  (CH3)3N is 4.194


Calculate pOH:


pOH = 4.194 + log(0.120.08)pOH = 4.194 + 0.176

pOH = 4.37


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Problem Details

Use information from Appendix D in the textbook to calculate the pH of the following solutions.

Calculate the pH of a solution that is 0.080 M in trimethylamine, (CH3)3N, and 0.12 M in trimethylammonium chloride, ((CH3)3NHCl).

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