Chemistry: A titration of ethylamine with HCl.

AI Thread Summary
The discussion focuses on calculating the pH during the titration of 50 mL of 0.150 M ethylamine with 0.100 M HCl. For part a, the challenge lies in determining the pH after adding 10 mL more HCl than needed, which involves understanding limiting reagents. Part b requires applying the Henderson-Hasselbalch equation to find the pH when 75% of the required acid has been added. The given Ka value for ethylamine is 2.34 x 10^-4, which is essential for these calculations. Overall, the thread highlights the complexities of titration calculations and the application of relevant equations.
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Homework Statement


For the titration of 50 mL of 0.150 M ethylamine (C2H5NH2), with 0.100 M HCl, find the pH :
a) when 10 mL more of HCl has been added than is required
b) when 75% of the required acid has been added

Homework Equations


Maybe Henderson Hasselbalch?: pH = pKa + log (base/acid)
Ka = 2.34*10^-4

The Attempt at a Solution


I honestly do not know where to go with this.
 
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I managed to solve most of the problem by now, just can't get the two parts still in the question.
 
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