In: Chemistry
(show calculations) make a 40mL, 1 M pH 8 Tris buffer from the following reagent:
a) What is the pKa of Tris? b)The amount of powder you will need to weigh out. c)The amount of water you will use. d) the volume of 1 N HCl or NaOH needed to make the result pH 8. e) Plot the pH as a function of the number of moles of HCl of NaOH.
a) Tris, C4H11NO3 forms an acid/base buffer with the conjugate acid, Tis-H+. The pKa of Tris-H+ is 8.07 and the acid ionization reaction is given as
Tris-H+ (aq) --------> Tris (aq) + H+ (aq); pKa = 8.07
b) Tris is available as a white crystalline powder. The pH of the buffer is given by the Henderson-Hasslebach equation as
pH = pKa + log [Tris]/[Tris-H+]
=====> 8.00 = 8.07 + log [Tris]/[Tris-H+]
=====> log [Tris]/[Tris-H+] = -0.7
=====> [Tris]/[Tris-H+] = antilog (-0.7) = 0.1995 ≈ 0.2000
=====> [Tris] = 0.2000*[Tris-H+] ……..(1)
The total concentration of Tris is given as 1 M; therefore,
[Tris] + [TriS-H+] = 1 M
=====> [Tris] + 0.2000*[Tris] = 1 M
=====> 1.2000*[Tris] = 1 M
=====> [Tris] = (1 M)/(1.2000) = 0.8333 M
[Tris-H+] = 0.2000*[Tris] = 0.2000*(0.8333 M) = 0.1667 M.
Mole(s) of Tris-H+ in 40 mL buffer solution = (40 mL)*(1 L/1000 mL)*(0.1667 M)*(1 mol/L/1 M) = 0.006668 mole.
Tris-H+ is produced by the action of HCl on Tris as below.
Tris (aq) + HCl (aq) ------> Tris-H+ (aq) + Cl- (aq)
As per the stoichiometry of the reaction,
1 mole Tris = 1 mole HCl = 1 mole Tris-H+.
Therefore, 0.006668 mole Tris-H+ = 0.006668 mole Tris.
Moles of Tris required to prepare the buffer = (40 mL)*(1 L/1000 mL)*(0.8333 M)*(1 mol/L/1 M) + 0.006668 mole = 0.0400 mole.
Molar mass of Tris = (4*12.01 + 11*1.008 + 1*14.0067 + 3*15.9994) g/mol = 121.1329 g/mol.
Mass of solid Tris powder required = (0.0400 mole)*(121.1329 g/mol) = 4.845316 g ≈ 4.8453 g (ans).
c) Mole(s) of HCl required = 0.006668 mole (as per the stoichiometry of the reaction).
Volume of 1 N HCl required = (0.006668 mole)/(1 mol/L) = 0.006668 L = (0.006668 L)*(1000 mL/1 L) = 6.668 mL ≈ 6.67 mL.
Weigh out 4.8453 g solid Tris powder, add 6.67 mL of 1 N HCl and (40.00 – 6.67) mL = 33.33 mL water.
d) The volume of 1 N HCl required = 6.67 mL (ans).