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.
sondawg
Messages
2
Reaction score
0

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.
 
Last edited:
Physics news on Phys.org
I managed to solve most of the problem by now, just can't get the two parts still in the question.
 
I don't get how to argue it. i can prove: evolution is the ability to adapt, whether it's progression or regression from some point of view, so if evolution is not constant then animal generations couldn`t stay alive for a big amount of time because when climate is changing this generations die. but they dont. so evolution is constant. but its not an argument, right? how to fing arguments when i only prove it.. analytically, i guess it called that (this is indirectly related to biology, im...
Thread 'How to find the pH of a galvanic cell (MIT OCW problem set)'
This is the final problem in this problem set from MIT OCW. Here is what I did to try to solve it The table cited in the problem is below We can easily spot the two redox couples that are in the electrochemical cell we are given. The hydrogen-based electrode has standard potential zero, and the silver-based electrode has standard potential 0.22. Thus, the hydrogen electrode, with the lower potential, is the reducing agent (ie, it is where oxidation happens) and is the anode. Electrons...
Back
Top