A diprotic acid, H, A, has acid dissociation constants of K₁1 = 4.76 x 10-4 and K₁2 = 3.59 x 10-12. Calculate the pH and molar concentrations of H₂A, HA, and A2- at equilibrium for each of the solutions. A 0.205 M solution of H₂A. pH = [HA-] = A 0.205 M solution of NaHA. pH= [HA] = M M [H₂A] = [A²-] = [H₂A] = [A²-] = M M M M
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![A diprotic acid, H, A, has acid dissociation constants of K₁1 = 4.76 x 10-4 and K₁2 = 3.59 x 10-12. Calculate the pH and
molar concentrations of H₂A, HA, and A2- at equilibrium for each of the solutions.
A 0.205 M solution of H₂A.
pH =
[HA] =
A 0.205 M solution of NaHA.
pH=
[HA] =
M
M
[H₂A] =
[A²-] =
[H₂A] =
[A²-] =
M
M
M
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