Here is an abbreviated phosphate buffer table taken from Clark's Determination of Hydrogen Ions:
pH | mL NaOH | pH | mL NaOH |
5.8 | 3.72 | 7.0 | 29.63 |
6.0 | 5.70 | 7.2 | 35.00 |
6.2 | 8.60 | 7.4 | 39.50 |
6.4 | 12.60 | 7.6 | 42.80 |
6.6 | 17.80 | 7.8 | 45.20 |
6.8 | 23.65 | 8.0 | 46.80 |
Be sure you're using the correct phosphate. There are several potassium phosphates which can NOT be used interchangeably in buffer solutions! You want KH2PO4.
Formula | Systematic name | Other names |
KH2PO4 | potassium dihydrogen phosphate | acid potassium phosphate monobasic potassium phosphate monopotassium phosphate potassium biphosphate |
K2HPO4 | potassium hydrogen phosphate | dipotassium phosphate dibasic potassium phosphate |
K3PO4 | potassium phosphate | tripotassium phosphate tribasic potassium phosphate |
If you can't find such a recipe, follow this procedure:
pH = pKa + log | ( | CA- CHA | ) |
![]() | This quintessential handbook contains data for about 2500 inorganic compounds and 12000 organic compounds. Relevant physical properties listed include crystal structure, color, solubility, melting points, boiling points, heats of formation, heats of vaporization, heats of fusion, entropies, heat capacities, critical pressure and temperature, vapor pressure, and optical properties. (Book/CDROM; no Web access). http://www.crcpress.com/catalog/9720.htm (12/12/98) |
Copyright © 1997-2010 by Fred Senese
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Last Revised 02/23/18.URL: http://antoine.frostburg.edu/chem/senese/101/acidbase/faq/print-preparing-buffers.shtml