A diprotic acid, H, A, has acid dissociation constants of Kaj = 1.45 × 104 and K2 = 5.12 x 10-1". Calculate the pH and molar concentrations of H,A, HA", and A- at equilibrium for each of the solutions. A 0.184 M solution of H,A. pH = 2.2865 [H,A] = 0.1788 M [HA"] = 5.17 x10-3 [A] = M 5.12 x10-11 M %3D
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![A diprotic acid, H, A, has acid dissociation constants of K,j = 1.45 x 10-4 and K2 = 5.12 x 10-". Calculate the pH and
molar concentrations of H,A, HA, and A²- at equilibrium for each of the solutions.
A 0.184 M solution of H,A.
pH = 2.2865
[H,A] =
0.1788
[HA"] = 5.17 xI10-3
[A?-] =
M
5.12 x10-11
M
A 0.184 M solution of NaHA.
pH=
[H,A] =
M.
[HA-] =
[A2-] =
M
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff9a76c22-d475-4c5d-b886-213c31f9c22e%2Fabf42acd-9452-4ec8-8754-df376869051a%2Fl3rnzml_processed.png&w=3840&q=75)
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