4. A diprotic acid has the following pK values: pKa1 = 5.50, pKa2 = 9.50
A. At what pH does [H2A] = [HA- ]?
B. At what pH doe [HA- ] = [A2- ]?
C. Which is the principal species at pH = 3.50, H2A, HA- , or A2- ? Justify your answer using the Henderson-Hasselbach equation.
D. Which is the principal species at pH = 7.5, H2A, HA- , or A2- ? Justify your answer (don’t use Henderson-Hasselbach equation, this is a half-neutralized diprotic acid).
E. Which is the principal species at pH = 9.8, H2A, HA- , or A2-? Justify your answer using the Henderson-Hasselbach equation
a)
for
pH = pKa + log(HA-/H2A)
pH = pKa1 + log(1)
pH = 5.5
b)
same case,
pH = pKa2 = 9.50
c)
at pH 3.5
expect H2A, HA- the most ... especially H2A
since pH range is in pKa1
d)
pH = 7.5 ; expect similar amounts of Ha- and A2- .. the most material is HA-. Still H2A is the most
e)
wehn pH = 9.5
the most species are HA- and A-2
4. A diprotic acid has the following pK values: pKa1 = 5.50, pKa2 = 9.50 A....
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A diprotic acid, H2A, has acid dissociation constants of Kai = 3.52 x 10-4 and Ka2 = 2.03 × 10-11 . Calculate the pH and molar concentrations of H2A, HA, and A2- at equilibrium for each of the solutions. A 0.206 M solution of H,A. pH = H2A] HA1 A 0.206 M solution of NaHA pH- [H2A] = [HA-] = A 0.206 M solution of Na,A. pH- [H2A] EA T [A21