Homework Answers
pH of buffer solution to be prepared = 10.6
pKa = 9.8
a) Calculation of ratio of [A-]/[HA]
According to Henderson Hasselbalch equation
pH = pKa + log10[A-]/[HA]
10.6 = 9.8 + log10[A-]/[HA]
0.8 = log10[A-]/[HA]
[A-]/[HA] = 6.31
b) As this is acidic buffer we have to have mixture of weak acid (HA) and its conjugate base (A- ) which is strong base hence we have to add strong base.
c) we know that [A-]/[HA] = 6.31/1 hence for 1 equivalent of HA we require 6.31 equivalent of A- hence it is clear that we need to add 6.31 equivalents of strong base.
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