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A buffer solution is a solution where the pH does not change significantly on dilution or if an acid or base is added at constant temperature. [1] Its pH changes very little when a small amount of strong acid or base is added to it. Buffer solutions are used as a means of keeping pH at a nearly constant value in a wide variety of chemical ...
Pages in category "Buffer solutions" The following 39 pages are in this category, out of 39 total. This list may not reflect recent changes. ...
A simple buffer solution consists of a solution of an acid and a salt of the conjugate base of the acid. For example, the acid may be acetic acid and the salt may be sodium acetate . The Henderson–Hasselbalch equation relates the pH of a solution containing a mixture of the two components to the acid dissociation constant , K a of the acid ...
TAE buffer is commonly prepared as a 50× stock solution for laboratory use. A 50× stock solution can be prepared by dissolving 242 g Tris base in water, adding 57.1 ml glacial acetic acid, and 100 ml of 500 mM EDTA (pH 8.0) solution, and bringing the final volume up to 1 litre.
The useful buffer range for tris (pH 7–9) coincides with the physiological pH typical of most living organisms. This, and its low cost, make tris one of the most common buffers in the biology/biochemistry laboratory. Tris is also used as a primary standard to standardize acid solutions for chemical analysis.
All buffering agents achieve their function because they contain an acidic group (acetate, phosphate, sulphonate ..) or a basic group (amino, pyridyl ..). A consequence of this is that they can form complexes with the biologically important ions Na + , K + , Mg 2+ and Ca 2+ and can compete for the metal ion contained in a metalloprotein .
McIlvaine buffer is a buffer solution composed of citric acid and disodium hydrogen phosphate, also known as citrate-phosphate buffer.It was introduced in 1921 by the United States agronomist Theodore Clinton McIlvaine (1875–1959) from West Virginia University, and it can be prepared in pH 2.2 to 8 by mixing two stock solutions.
They are formulated to give a ready to use borate buffered saline solution upon dissolution in 500 ml of deionized water. Concentration of borate and NaCl as well as the pH can vary, and the resulting solution would still be referred to as "borate buffered saline". Borate concentration (giving buffering capacity) can vary from 10 mM to 100 mM.