c) What volume of 1M HCl needs to be added to 1L of 0.10 M Tris to obtain a final pH of 7.4? Ignore dilution effects. 3. Blood pH must stay within ±0.4 from normal (pH 7.4). To do this a buffer system involving carbon dioxide (product of respiration) is used. The following two equilibria are involved: and a) What is the approximate range of molar concentrations of hydrogen ions for which life can be sustained? b) At pH 7.4 what are the concentrations of the two forms of carbonic acid if the total concentration is 1 mM? The Ka for the H2CO3/HCO3- buffer pair is 4.3x10-7. c) How can the body use this as a buffer system? (hint: think about La Chatelier’s principle) Worksheet #16ProtonCHEM 300transfer equilibria1. One of the big differences between “P-chem" standard state and "Biochem" standardstate is the pH. The other (somewhat smaller) differences are temperature and pressure.P-chemBiochempHO ([H+] = 1)7%3DTemperature25°C37°CPressure1 bar1 atmCalculate the difference in the equilibrium constant and Gibb's energy for the hydrolysisof 1,3-biphosphoglycerate (1,3-BPG) assuming (a) "P-chem" standard state and (b)"Biochem" standard state. The typical cellular concentrations of the phosphatecomponents of the reaction are given below.1,3- ВРG (аq)+ Н,0(1) — 3- PG(аg)+ НРО" (аq)+ н" (ад)0.001MM0.12 mM1mM 2. “Tris" base is a common biochemical buffer. It's pK, = 8.3.a) At what pH would you expect Tris to act as a buffer in a solution that has equal molarconcentrations of Tris and its conjugate base?b) Calculate the pH of a 0.10 M Tris solution.

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c) What volume of 1M HCl needs to be added to 1L of 0.10 M Tris to obtain a final pH of
7.4? Ignore dilution effects.
3. Blood pH must stay within ±0.4 from normal (pH 7.4). To do this a buffer system
involving carbon dioxide (product of respiration) is used. The following two equilibria are
involved:
and
a) What is the approximate range of molar concentrations of hydrogen ions for which
life can be sustained?
b) At pH 7.4 what are the concentrations of the two forms of carbonic acid if the total
concentration is 1 mM? The Ka for the H2CO3/HCO3- buffer pair is 4.3x10-7.
c) How can the body use this as a buffer system? (hint: think about La Chatelier’s
principle)

Worksheet #16
Proton
CHEM 300
transfer equilibria
1. One of the big differences between “P-chem" standard state and "Biochem" standard
state is the pH. The other (somewhat smaller) differences are temperature and pressure.
P-chem
Biochem
pH
O ([H+] = 1)
7
%3D
Temperature
25°C
37°C
Pressure
1 bar
1 atm
Calculate the difference in the equilibrium constant and Gibb's energy for the hydrolysis
of 1,3-biphosphoglycerate (1,3-BPG) assuming (a) "P-chem" standard state and (b)
"Biochem" standard state. The typical cellular concentrations of the phosphate
components of the reaction are given below.
1,3- ВРG (аq)+ Н,0(1) — 3- PG(аg)+ НРО" (аq)+ н" (ад)
0.001MM
0.12 mM
1mM

2. “Tris" base is a common biochemical buffer. It's pK, = 8.3.
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 base?
b) Calculate the pH of a 0.10 M Tris solution.

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