Buffer Solution Question

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In summary, the conversation discusses whether preparing a 0.1M buffer solution of acid X by adding a combination of deprotanated and protanted forms to water would work. It is noted that this method may work for acids with a pKa higher than 3.5, but for stronger acids, it would not work due to the immediate change in concentration of the acid's forms. The acid dissociativity constant plays a role in this.
  • #1
PhiPhenomenon
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Hey guys,

This question seems pretty easy and straight forward but there's a nagging part of me that isn't sure. I want to say 'no' because I think that the solution goes back to it's acid constant dissociativity levels but I'm not sure.

So the skinny is that someone needs to prepare a 0.1M buffer solution of acid X. One person decides to do so through by adding the proper combination of 0.08 moles of the deprotanated form and 0.02 moles protanted to 1 liter of water form such that it satisfies the Henderson–Hasselbalch equation. That wouldn't work because the acid dissociativity constant dictates that the concentration of protanated an deprotanated forms of acid would change immediately and ultimately satisfy the ka right?
 
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  • #2
Depends on the acid strength. If pKa is higher than about 3.5 this approach will work, for stronger acids it won't for the reasons you are thinking about.
 

1. What is a buffer solution?

A buffer solution is a solution that resists changes in pH when small amounts of acid or base are added. It is made up of a weak acid and its conjugate base, or a weak base and its conjugate acid.

2. How does a buffer solution work?

A buffer solution works by maintaining a relatively constant pH when small amounts of acid or base are added. This is due to the presence of a weak acid and its conjugate base, or a weak base and its conjugate acid, which can react with the added acid or base to prevent a significant change in pH.

3. Why are buffer solutions important in chemistry?

Buffer solutions are important in chemistry because they help to maintain a stable pH in a system. This is crucial for many chemical reactions and biological processes, as even small changes in pH can significantly affect the outcome.

4. How do you prepare a buffer solution?

To prepare a buffer solution, you will need to mix a weak acid and its conjugate base, or a weak base and its conjugate acid, in specific proportions. The exact proportions will depend on the desired pH of the buffer solution and the pKa of the weak acid or base.

5. What is the difference between a buffer solution and a regular solution?

The main difference between a buffer solution and a regular solution is that a buffer solution contains a weak acid and its conjugate base, or a weak base and its conjugate acid, while a regular solution does not. This allows a buffer solution to resist changes in pH, whereas a regular solution may experience a significant change in pH when acid or base is added.

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