Human blood contains a 'buffer' that allows it to maintain its pH at to ensure normal functioning of cells. Buffer solutions are also important in chemical and. As indicated in Section “Strong and Weak Acids and Bases and Their Salts”, weak acids are relatively common, even in the foods we eat. But we. Describes simple acidic and alkaline buffer solutions and explains how they calculations involving buffer solutions, you may be interested in my chemistry.


Author: Dr. Lera Brown
Country: Argentina
Language: English
Genre: Education
Published: 9 November 2014
Pages: 539
PDF File Size: 25.47 Mb
ePub File Size: 2.81 Mb
ISBN: 834-5-58678-468-6
Downloads: 79890
Price: Free
Uploader: Dr. Lera Brown


So let's say we already know the Ka value for NH four plus and that's 5.


To find the pKa, all we have buffer chemistry do is take the negative log of that. So the pKa is the negative log of 5.

How Buffers Work

So let's get out the calculator and let's do that math. So the negative log of 5.

Is going to give us a pKa value of 9. So pKa is equal buffer chemistry 9. So we're gonna plug that into our Henderson-Hasselbalch equation right here.

So the pH of our buffer solution is equal to buffer chemistry. Our base is ammonia, NH three, and our concentration in our buffer solution is. And that's over the concentration of our acid, that's NH four plus, and our concentration is.

General Chemistry/Buffer Systems - Wikibooks, open books for an open world

So this is over. So let's find the log, the log of. And so that is.


So the final pH, or the pH of our buffer solution, I should say, is equal to 9. So remember this number buffer chemistry the pH, because we're going to compare what happens to the pH when you add some acid and when you add buffer chemistry base.

Buffer solution pH calculations

And so our next problem is adding base to our buffer solution. Buffer chemistry we're gonna see what that does to the pH. So now we've added. Let's say the total volume is. So what is the resulting pH?

Buffer solution - Wikipedia

So if we divide moles by liters, that will give us the buffer chemistry of sodium hydroxide. So that's our concentration of sodium hydroxide.

And since sodium hydroxide is a strong base, that's also our concentration buffer chemistry hydroxide ions buffer chemistry solution. So this is our concentration of hydroxide ions. So we're adding a base and think about what that's going to react with in our buffer solution.


So our buffer solution has NH three and NH four plus. The base is buffer chemistry to react with the acids.