When 99% of the glycine is in its
-NH3+ form (see question 9), what is the
numerical relation between the pH of the solution and the pKa of
the amino group?
Group of answer choices
pH = pKa - 2
pH = pKa - 1
pH = pKa +1
None of the answers is correct
question 9:
The amino acid glycine is often used as the main ingredients of
a buffer in biochemical experiments. The amino group of glycine,
which has a pKa of 9.6, can exist either in the protonated
(-NH3+) or as the free base
(-NH2), because of the reversible equilibrium:
R-NH3+ ⟺ R-NH2 +
H+
In what pH range can glycine be used as an effective buffer due
to its amino group?
Group of answer choices
8.6-10.6
8.6-9.6
9.6-10.6
7.6-8.6