A diprotic acid, H2A, has acid dissociation constants of 𝐾a1=3.89×10−4 and 𝐾a2=2.94×10−11. Calculate the
Posted: Mon Nov 15, 2021 4:52 pm
A diprotic acid, H2A, has acid dissociation constants of
𝐾a1=3.89×10−4 and 𝐾a2=2.94×10−11. Calculate the pH and molar
concentrations of H2A, HA−, and A2− at equilibrium for each of the
solutions.
A diprotic acid, H, A, has acid dissociation constants of K21 = 3.89 x 10-* and K22 = 2.94 x 10-". Calculate the pH and molar concentrations of H,A, HA , and A?- at equilibrium for each of the solutions. A 0.183 M solution of H.A. pH = [ HA] = M [HA-] = M [A2-) = M A 0.183 M solution of NaHA. pH= [ HA] = M [HA] = M [A2-) = M
A 0.183 M solution of Na, A. pH= [HA] = M [HA ) = M [A2-) = M
𝐾a1=3.89×10−4 and 𝐾a2=2.94×10−11. Calculate the pH and molar
concentrations of H2A, HA−, and A2− at equilibrium for each of the
solutions.
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A 0.183 M solution of Na, A. pH= [HA] = M [HA ) = M [A2-) = M