Many biological processes occurring on the lab bench require a stable pH to ensure results accuracy. A buffer is one of the best methods of achieving pH stability without interfering with the underlying process. Buffer solutions do in fact occur naturally; an example can be found in our own bodies, as our blood needs to maintain a pH of 7.35 to function properly. This basic premise is harnessed by reference material manufacturers to create stabilizing reagents for biochemical research. Sodium carbonate bicarbonate is one such example.
Why Is A Buffer Important?
pH buffers are comprised of a conjugate base and a weak acid, which allows them to maintain stable pH levels in the main solution, even if a strong acid or base is added. Using a pH buffer in an experiment or process can be extremely useful for