Tris is a white crystal or powder. Soluble in ethanol and water, slightly soluble in ethyl acetate and benzene, insoluble in ether and carbon tetrachloride, corrosive to copper and aluminum, and irritating chemicals.
Tris is widely used in acute metabolic and respiratory acidemia. It is an alkaline buffer and has a good buffering effect on metabolic acidosis and enzymatic activity.
Tris is often used as a biological buffer and is often formulated with pH values of 6.8, 7.4, 8.0, and 8.8. Its structural formula and pH value vary greatly with temperature. Generally speaking, the pH value drops by 0.03 for every degree increase in temperature.
Tris is widely used in the preparation of buffers in biochemical and molecular biology experiments. For example, Tris is required in both TAE and TBE buffers (for solubilization of nucleic acids) commonly used in biochemical experiments. Since it contains an amino group, it can undergo condensation reactions with aldehydes.
Tris is a weak base with a pKa of 8.1 at room temperature (25°C; according to buffer theory, the effective buffering range of Tris buffers is between pH 7.0 and 9.2.
The pH of the aqueous solution of Tris base is about 10.5. Generally, hydrochloric acid is added to adjust the pH value to the desired value, and then the buffer solution with the pH value can be obtained. However, attention should be paid to the effect of temperature on the pKa of Tris.
Since Tris buffer is a weakly basic solution, DNA will be deprotonated in such a solution, thereby increasing its solubility. People often add EDTA to Tris hydrochloric acid buffer to make “TE buffer”, which is used for DNA stabilization and storage. If you change the pH-adjusting acid solution to acetic acid, you get a “TAE buffer” (Tris/Acetate/EDTA), and to boric acid you get a “TBE buffer” (Tris/Borate/EDTA). These two buffers are commonly used in nucleic acid electrophoresis experiments.
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