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13 Dec 2019

We want to prepare a buffer by adding 3.00 M HCl to 0.0500 moles of Tris (tris(hydroxymethyl)aminomethane or (HOCH2)3NH2) in 1.00 L (total solution volume) to make a pH = 7.800 solution. Determine the volume of 3.00 M HCl (in mL) that must be added. The pKa for the conjugate acid of Tris is 8.072. Ignore activity for this problem.

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Keith Leannon
Keith LeannonLv2
17 Dec 2019

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Related questions

Consider a 1.00 L buffer prepared by mixing 610 mg of Tris [tris(hydroxymethyl

aminomethane] (pKa = 8.07) in the free-base form (FW = 121.1 g/mol) and 4 mM HCl.

a) What is the pH of the buffer?

b) What would the pH be if we had added 2.8 mM of HCl instead of the amount of HCl in (a)?

c) What would the pH be if we had added 1.00 mL of 0.010 M NaOH to the original amounts in

(a)?

d) Could you use a Tris buffer system to prepare a buffer at pH 7.00? Why or why not?

Tris buffer [a shortened form of Trizma, tris(hydroxymethyl)aminomethane] is very common buffer for biochemical applications. One buys Trizma*HCl, (C4H11NO3*HCl, the acid) and the Trizma base (C4H11NO3, the base) and mixes them in appropriate amounts to make a buffer of the desired pH. If you desire 500 mL of a pH 7.2 solution, how many grams of Trizma*HCl and Trizma base should be dissolved in 500 mL of water? Make the buffer 0.050 M total Tris concentration. The pKa of Triz is 8.1 at 25 degrees Celsius

How would you prepare 1.000 L of a 1.000 mole L-1, pH 7.50Tris—aka, tris(hydroxymethyl)aminomethane—buffer? You have pureTris·HCl, {(HOCH2)3NH+,Cl-}, a pH meter, 1.00 M HCl and 1.00 MNaOH, and all of the pure water and glassware you need. Carefullygo through all mathematical steps, and then describe in detail howyou would make the buffer in the laboratory.

I don't know how to solve this without information on volume. Do Ieven need it?

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