So, to solve for a specific buffer's pH, one must know the pKa of the buffer's species, which can usually be found in tables. The next part, {eq}log\frac{ [Base] }{ [Acid] } {/eq}, corrects the pKa in relation to how much acid and base are in the solution. If there is...
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Use theHenderson-Hasselbachequation to calculate how much acid and base you need. You can simplify the calculation if you make 1 liter of buffer. Select the pKa value that is closest to the pH of your buffer. For example, if you want the pH of your buffer to be 7, then use the pKa...
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Write down the equation for the the Ka, the Kb, and the Kw, which is Kw = (Ka)(Kb). Solve the equation for Kb by dividing the Kw by the Ka. You then obtain the equation Kb = Kw / Ka. Step 3 Put the values from the problem into the equation. For example, for the chloride...
The equation is pH = pKa + log [OH-]/[H]So, I start with 7.2 = pKa + log [OH-]/[H]How do I find the value for pKa and [OH-]/[H]?Thank you! Logged Solutions0125 New Member Posts: 3 Mole Snacks: +0/-0 Re: How to prepare 10 mM sodium phosphate buffer, pH 7.2?
Look, I can appreciate that this is a very difficult problem to solve and a lot of effort was put into solving it. This feels like one of those cases where someone spent weeks getting really deep into something and when they finally came up for air they sort of forgot how to talk to...
it won't beexactlythe same for each person. You could come up with more than one way to make the final buffer solution for any given pH, so the lab is flexible depending on how you think about the problem.This type of lab encourages you to use knowledge of chemistry to solve a probl...
Plugging this into the Henderson-Hasselbalch equation, we get pKa = pH + log(100), or pKa = pH + 2. Therefore, the ratio of the different colored forms of the indicator would have originally been 100, and after the addition of the acid, it would be 102. 2. To solve this problem,...