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13 Dec 2019

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?

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Related questions

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.

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

Buffer problems with additional solutions

I know this is different from normal buffer problems in that you have to add additional grams of something at the end, just not sure what to do with all the extra available solutions/solutes listed.

Outline how you would prepare 500 mL of the following solutions:

0.01M Tris, pH 7.5, 100 mM NaCl

0.05 M Tris, pH 7.8, 500 mM NaCl, 20 mM CaCl2

100 mM Tris, pH 8.7, 20 mM EDTA

You have the following available:

Tris base (FW = 121.1 g/n, pKa = 8.21)

NaCl (FW = 58.44 g/n)

100 mM CaCl2

6 M HCl

6 M NaOH

500 mM EDTA

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