A diprotic acid, H, A. has acid dissociation constants of K₁1 = 4.63 x 10 and K₂ = 5.82 x 10-12. Calculate the pH and molar concentrations of H₂A, HA, and A2 at equilibrium for each of the solutions. A 0.126 M solution of H.A. Macmillan Learning pH= [HA] = A 0.126 M solution of NaHA. pH [HA] = A 0.126 M solution of Na, A. pH= M M [H₂A] = |A³] = [H₂A) = |A³|= [H₂A = M M M M M
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![A diprotic acid, H, A. acid dissociation constants of K₁1 = 4.63 x 10 and K = 5.82 x 10-¹2. Calculate the pH and
molar concentrations of H₂A. HA, and A2 at equilibrium for each of the solutions.
A 0.126 M solution of H, A.
Macmillan Learning
2
pH=
[HA] =
A 0.126 M solution of NaHA.
pH
[HA] =
A 0.126 M solution of Na, A.
pH=
[HA] =
M
[H₂A] =
M
|A²] =
(H₂A) =
M |A²-|-
[H₂A] =
|A³-1-
M
M
M
M
M
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