A diprotic acid, H, A, has acid dissociation constants of K = 2.32 x 10-4 and K2 = 5.84 x 10-12. Calculate the pH and molar concentrations of H, A, HA", and A?- at equilibrium for each of the solutions. A 0.202 M solution of H, A. pH = [H,A] = [HA-] = M [A2-] = ME %3D
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![A diprotic acid, H, A, has acid dissociation constants of K = 2.32 x 10-4 and K2 = 5.84 x 10-12. Calculate the pH and
molar concentrations of H,A, HA", and A2- at equilibrium for each of the solutions.
A 0.202 M solution of H, A.
pH =
(H,A] =
%3D
[HA-] =
[A2-) =
M.
!!
A 0.202 M solution of NaHA.
[H, A] =
pH=](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa58fe29b-8ecd-461b-bc6a-ce3031c7cd18%2F02f3f442-6d24-4993-8479-c6d9bdec9e30%2Fjdp9ocs_processed.jpeg&w=3840&q=75)
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