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Question about getting the pH

  • Thread starter em-kay
  • Start date
  • #1
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Homework Statement


What will be the final pH of the solution if a drop (approximately equal to 1/20 mL) of 1.0M HCl is added to a 10mL 0.1 M CH3COOH sol'n?


Homework Equations


pH = -log [H+]


The Attempt at a Solution


I first determined the number of moles of H+ from the partial ionization of CH3COOH (CH3COOH <--> CH3COO- + H+) using the ICE table. The number of moles H+ from my computation is 4.024922359 x 10^-5.

Then I also determined the number of moles of H+ from HCl--> H+ + Cl-. What I got is 5 x 10^-5 moles.

I added the two values to get the total number of moles H+.

The pH I got is 2.52.


Is my answer correct?
I'm not quite sure about how I solved it.
Need help. Thanks. :smile:
 

Answers and Replies

  • #2
3
0
How do I apply the common-ion effect for this problem?
 
  • #3
Borek
Mentor
28,326
2,713
Do an ICE table for acetic acid treating H+ from HCl as initial concentration.
 
  • #4
3
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Thanks much. I'll do that.
 

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