Tris(hydroxymethyl)aminomethane (also known as “tris”) is a weak base commonly used in biochemical research in the preparation of buffers. Tris has low toxicity and a pKb of 5.92 that is appropriate for biological applications. a. In order to make tris buffer, a researcher weighed out 2.00 g of tris (molar mass of 121.14 g/mol) and reacted it with 15.00 mL of 0.800 M HCl. What is the pH of the resulting buffer? You may assume a total final volume of 15.00 mL.
Tris(hydroxymethyl)aminomethane (also known as “tris”) is a weak base commonly used in biochemical research in the...
4.48 The weak base colloquially known as Tris, and more precisely as tris(hydroxymethyl)aminomethane, has pK, = 8.3 at 20°C and is commonly used to produce a buffer for biochemical applications. (a) At what pH would you expect Tris to act as a buffer in a solution that has equal molar concentrations of Tris and its conjugate acid? (b) What is the pH after the addition of 3.3 mmol NaOH to 100 cm3 of a buffer solution with equal molar concentrations...
5. Tris i.e. [tris(hydroxymethyl)aminomethane) is commonly used as a buffer in bioanalytical studies. The pk of Tris is 8.1 at 20°C. (a) Calculate the pH of the Tris buffer after mixing 12.0 mL of 0.15 M of a HCl solution with 20.0 mL of a 0.20 M solution of Tris. (5 points) (b) An amount of 0.00017 mol of H+ was consumed during an enzymatic reaction. What is the pH of the buffer at the end of the reaction? (5...
21.) Tris, (HOCH2)3CNH2 (pKb = 5.91), a very common buffer for studying biochemical processes, is prepared by a biological chemist using 10.0M NaOH to a pH of 7.79 using 31.52 g of (HOCH2)3CNH3Cl, or TrisH+, (MW=157.597g/mol, pKa 8.075). >>>> Need help with second part of question pls>>>>...Now you dilute the solution from problem 21 to 1.0 L and take half of the buffer (500.0 mL) and add 0.0100 moles solid HCl. What is the new pH?
Phosphate buffered saline (PBS) is a buffer solution commonly used in biological research. The buffer helps to maintain a constant pH. The osmolality and ion concentrations of the solution usually match those of the human body. A) You need to prepare a stock solution at pH 7.00 with KH2PO4 and Na2HPO4 (pKa =7.21). What would be the respective concentration of these substances if you wish to obtain the final phosphate concentration [HPO4 −2 ] + [H2PO4 − ] = 0.3...