Mohammad, I don't know whether you tried a search for your "problem " in any data base (or eventually "Googling" if you can do so), which might have answered your request very rapidly. In case you are not allowed (or are not authorized ) to use foreign 'imperialistic' companies I have copied and pasted herein what might be of helpful use to you:

Try:

http://microscopy.berkeley.edu/Resources/instruction/buffers.html ,

press CTRL&F (=SEARCH for/FIND, find the rectangle-insert field), enter there: | TRIS HCl buffer | press RETURN and wait some second (or scroll down in the page) and find:

TRIS BUFFERS

Tris buffers are used commonly in microtechnique applications involving molecular biological procedures. Listed here are a number of common Tris formulations (Maniatis, et al., 1982).

Solution: Preparation of Tris, 1 M [NB added: = 1000mM] stock

Dissolve 121.1 g Tris base in 800 ml DI (=deionized water) and adjust pH with the following approximate amount of HCl:

for pH 7.4: 70 ml

for pH 7.6: 60 ml

for pH 8.0: 42 ml

or try: www.merckmillipore.com/Biopharma/Buffers

Dilute 1:10 with distilled water before use and adjust pH if necessary. Note: Tris-HCl Buffer is used for specific cases of immunohistochemical staining. Tris is a chemical with basic properties, having a pKa of 8.1. It can be used to buffer solutions from drastic pH changes, keeping them in the pH range of 7.0 to 9.0.

or buy/purchase standardized, ready to use-solutions

e.g. (Disclaimer: no affiliation to Technova.com or financial interest!): https://www.teknova.com/v/vspfiles/files/Lit/buffer%20chart_5x7.pdf

or any other chemicals supplier (SIGMA, MERCK, ThermoFisherScientific and others)

or search, e. g. in Research Gate archives for | 10mM TRIS Tris-HCl Buffer |

+38,4 ml of HCl for pH 7.6 for 10mM: dilute 1:10, but check pH again!)

- http://dharmacon.horizondiscovery.com/uploadedFiles/Resources/crrna-tracrrna-resuspension-buffer-protocol.pdf (for pH 7.6 compare with the amounts of HCl to be added ==> above....)

http://www.bio-rad.com/webroot/web/pdf/lsr/literature/Bulletin_6199.pdf :

1 M Tris-HCl, pH 7.6 (100 ml)

Tris base: 12.11 g

Deionized H2O (diH2O) 80 ml

Adjust pH to 7.6 with HCl

finally: diH2O to 100 ml

- https://www.thoughtco.com/how-to-make-tris-buffer-solution-603668

- https://www.protocolsonline.com/recipes/buffers/tris-cl-1m/

- http://www.boneandcancer.org/protocolsh1.htm

NB: No warranty for the correctness of theoretical numbers / displayed concentrations/volumes to be added etc.,etc..... it is quite normal that with your first trials you'll / you might face deviations from the predicted values.

Therefore: you have to play around - at least a bit.... and: always measure, measure, measure...(;-)).

PS: as found in in ResGate Q&A--ARCHIVES:

- https://www.researchgate.net/post/Dose_10mM_Tris-HCl_buffer_have_same_pH_with_1M_Tris-HCl_buffer ;

- https://www.researchgate.net/post/How_can_I_prepare_10mM_Tris-HCl_pH_75, there find:

==> http://www.biomol.net/en/tools/buffercalculator.htm

or (more/less the same calculator:)

==>https://www.liverpool.ac.uk/pfg/Tools/BuffferCalc/Buffer.html

INPUT

- Web: http://www.liv.ac.uk/cpr Buffer recipe, generated by Buffer Calculator (c) Rob Beynon 1996-2015 http://www.liv.ac.uk/buffersThis recipe is thermodynamically correct, although you take responsibility for the results that the software produces.

BUFFER: To make 100 ml of 0.01 M Tris (pKa=8.06) Buffer, pH= 7.6, Ionic strength = 0.005 M, (Ionic strength due to the buffer = 0.005M ) Thermodynamic pKa = 8.06, Apparent pKa' = 7.76 Temperature coefficient = -0.028 per oC Prepared at 20oC, used at 37 oC

RECIPE: Dissolve 0.0005 mol of acid component Dissolve 0.0004 mol of basic component (No added neutral salts, I due to buffer alone.) Make up to 100 ml with pure water

ALTERNATIVELY: Dissolve 0.121 g of Tris base (Mr = 121.14) in approx. 90 ml of pure water. (No added neutral salts, I due to buffer alone.) Titrate to pH 8.07 at the lab temperature of 20oC with monovalent strong base or acid as needed. Make up volume to 100 ml with pure water Buffer will, of course, be pH 7.60 at 37oC

- http://www.bioinformatics.org/jambw/5/4/index.html

Useful Conversion (calculator) of :

1 M = 1000 mM; 1 mM = 0.001 M

@ http://www.endmemo.com/sconvert/mmm.php

http://www.protocol-online.org/biology-forums/posts/11549.html

- https://www.sigmaaldrich.com/life-science/core-bioreagents/biological-buffers/learning-center/buffer-calculator.html

Now you are spoilt for choice, I guess (:-))

Since in my previous answer [001] I addressed

‚Searching the Archive / repository‘ of the Research Gate Data Base,

for completeness I want to add the following (also for future searches on other matters)

Search phrase (change as appropriate, without quotation marks): „ 10 mM tris hcl buffer recipe HPLC “, copy and paste into the rectangle „SEARCH“ (in the middle of the upper menue-line ==> found in THIS page too), click RETURN, wait a second and then choose from

e.g.: Authors, or from PUBLICATIONS: creates RESULTS in the following URL:

https://www.researchgate.net/search.Search.html?type=publication&query=10%20mM%20tris%20hcl%20buffer%20recipe%20HPLC, or in

in Q&A (QUESTIONS and ANSWERS):

https://www.researchgate.net/search.Search.html?type=question&query=10%20mM%20tris%20hcl%20buffer%20recipe%20HPLC.

Best wishes and good luck!

Hi,

You may use this web tool to calculate the concentration.

https://www.alfa-chemistry.com/ph-calculator.htm

Please use Henderson-Helensburgh equation of

pH= pka + log ([base]/[acid])...(1) and

[base]+[acid]= [buffer con]....(2)

In ur case pH is 7.6, the pka of tris-HCl is 8.08 and the buffer con is 10mM or 0.01M. This will give u the amount of the tris base in mgs and the mls of HCl to be used, depending on the volume of buffer u want to prepare. Thanks

To: Alaso Jack

Dear Alaso Jack,

honestly, for 'Henderson-Helensburgh' there was only ONE plausible result (found via Google):

Quote:

" We have a record for a Andrew Henderson living at an address in Helensburgh G84. The record includes the full address, along with information about the ... "

End of Quote....

Therefore I guess you wanted to use / write the

(right now incidentally I found out that to be also wrong!)

name of the cited equation as (very often termed also)

'Henderson-Hasselbach'

(e.g. cf.:

"https://www.researchgate.net/search.Search.html?type=question&query=hasselbach“ >Hasselbach