Calculating the [H+] and pH of a lactic acid solution

Thread starter biochemstuden
Start date Feb 25, 2009
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Acid Ph

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To calculate the [H+] of a 0.05 M lactic acid solution with a Ka of 1.39 x 10^-4, the dissociation equation for lactic acid must be applied. The Henderson-Hasselbalch equation is not necessary for this calculation, as it is primarily used for buffer solutions. Instead, the equilibrium expression for the dissociation of lactic acid should be used to find [H+]. The discussion also touches on the relevance of the user's academic focus, suggesting a blend of organic and biochemistry. Accurate calculations will yield the pH of the solution based on the derived [H+].

Feb 25, 2009

biochemstuden

How do I calculate the [H+] fo a 0.05 M lactic acid solution. The Ka of the lactic acid is
1.39 X 10-4

is this a henderson - hasselbalch equation?

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Feb 25, 2009

Borek

Mentor

Somehow I feel like I have already answered this question somewhere else...

You have to decide whether you are orgostudent or biochemstudent

Feb 25, 2009

biochemstuden

both :)

thanks!

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