vera_ewing
  • vera_ewing
Given that the pKa of acetic acid is 4.8, what would be the likely result of adding 1 mL of 0.1 M HCl to a 0.1 M acetate buffer at a pH of 5.0? A. The pH would drop slightly. B. The pH would increase significantly. C. The pH would drop significantly. D. The pH would increase slightly.
Chemistry
  • Stacey Warren - Expert brainly.com
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SOLVED
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chestercat
  • chestercat
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Cuanchi
  • Cuanchi
any idea?
vera_ewing
  • vera_ewing
Well I feel like it might D maybe?
Cuanchi
  • Cuanchi
why did you choose that?

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More answers

vera_ewing
  • vera_ewing
Since the pKa is 4.8
vera_ewing
  • vera_ewing
Actually, I think it's A
Cuanchi
  • Cuanchi
OK now a little bit closer, If you add an acid to a buffer always the pH is going to drop. If you add a base the pH will increase. How do you know if the pH is dropping slightly or significantly?
vera_ewing
  • vera_ewing
It would drop significantly, since the pKa is 4.8?
Cuanchi
  • Cuanchi
The pKa is not going to tell you if the pH is going to drop slightly or significantly. The buffer capacity and the concentration of the buffer and the amount of acid that you add is going to tell you if the pH change slightly or significantly
vera_ewing
  • vera_ewing
Ohh okay! So the answer is C?
Rushwr
  • Rushwr
Shouldnt it be A? @Cuanchi Can u explain it a little more?
Cuanchi
  • Cuanchi
the problem is giving you two very similar options A and C, how can you figure out which one is the correct answer?
vera_ewing
  • vera_ewing
The pH?
Cuanchi
  • Cuanchi
you have the Henderson-Hasselbalch Equation pH = pKa + log ([base]/[acid]) when the problem said that the concentration of the buffer is 0.1M that means that the concentration of the base/acid = 1 (both are 0.1M) an then the log 1 = 0 then the pH of the buffer is equal to the pKa. when you add HCl to the buffer, the HCl is reacting with the sodium acetate , and produce more acetic acid and decrease the concentration of sodium acetate in the buffer. At this point the relationship [base]/[acid] is <1 then the log of a number <1 is negative and in the equation the pH is going to be lower than the pKa
Rushwr
  • Rushwr
I thought it in this way: since its an acid there should be a slight drop in pH as its concentration is small
vera_ewing
  • vera_ewing
@Cuanchi Is it C then?
Cuanchi
  • Cuanchi
Your idea @Rushwr is correct the only thing you have to be sure that the amount of strong acid (moles) is lower than the amount of salt that you have in your buffer. If the amount of strong acid is bigger than the amount of salt you don't have buffer anymore and you have just acid and NaCl
Cuanchi
  • Cuanchi
I will go for A because the problem doesn't mention the volume of the buffer that you have
Rushwr
  • Rushwr
yey my answer is correct ! @Cuanchi Thank you

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