1 M tris pH 6.8 buffer preparation using tris and Tris HCL (No conc HCL)
Posted 27 September 2016 - 10:43 PM
Posted 28 September 2016 - 06:04 AM
Yes, this is possible... you can use the Henderson-Hasselbalch equation. There are also a number of online calculators that will do this for you. Roche Lab FAQs also has tables for this sort of thing.
Posted 28 September 2016 - 07:51 PM
i tried few calculator, but they give it for making tris buffer upto pH 7.00 only. i want to make pH 6.8. if anyone can give me precise amount of tris and tris Hcl to add to make 1M tris buffer pH 6.8, it would be really helpful.
Posted 29 September 2016 - 06:29 AM
OK... henderson-hasselbalch pH=pKa + log10(conc base/ conc acid)
pH =6.8, pKa =8.08.
substitution gives us that the log10(base/acid)=-1.28... antilog gives us ratio between the two as 0.05248. This means that to balance the pH you will need 19x more tris-HCL than tris base to get pH 6.8. Can you work from that?
- biotef likes this
Posted 30 September 2016 - 07:39 AM
Henderson hasselbalch is a great intellectual exercise but rarely works in real practice when attempting to make buffers with precise pH.
The practical way of making a buffer using acid and conjugate base is to make stocks of both at equal concentration, then add one to the other while stirring with a pH meter until desired pH is met.
For example, if you want 1 M Tris pH 6.8, make a 1 M Tris base solution and a 1 M Tris-HCl solution. Add the Tris base solution dropwise with stirring and a pH meter to the Tris HCl solution until pH is raised to 6.8. Because both Tris stocks are 1 M, the final solution is also 1 M Tris. It may be helpful to do a rough HH calculation beforehand so you know about how much of each 1 M stock solution to make so you don't have an excessive amount of one left over as waste at the end (which bob1 did very nicely for you already).
Edited by labtastic, 30 September 2016 - 08:36 AM.