[XGen]

Let me see if I understand it correctly.

Taking the 0.000164492 mol of H+ and dividing it by 0.05 L gives 0.00328984 M of [H+] and 0.00328984 M for [HSO4-].
At pH 2, Ka2 = [10^-2][SO4 2-]/[HSO4-], and the sulfate and hydrogen sulfate concentrations are the same, leaving Ka2 = 10^-2.
Then, letting x = the amount of hydrogen sulfate dissociated, 10^-2 = [0.00328984 + x][ x]/[0.00328984 - x]. Solving, x = 0.00213308 M. Then, 0.00328984 + 0.00213308 = 0.00542292 M, or 2.266, which rounds to 2.27.

It seems that I had made a computation error before. :3

[Borek]

Taking the 0.000164492 mol of H+ and dividing it by 0.05 L gives 0.00328984 M of [H+] and 0.00328984 M for [HSO4-].

Not exactly. You don't know these concentrations. All you can say at this moment is that analytical concentration of sulfuric acid is 0.000164492/2/0.05L. It doesn't say anything about equilibrium concentrations of H⁺ and HSO₄^-.

At pH 2, Ka2 = [10^-2][SO4 2-]/[HSO4-], and the sulfate and hydrogen sulfate concentrations are the same, leaving Ka2 = 10^-2.

Right.

Then, letting x = the amount of hydrogen sulfate dissociated, 10^-2 = [0.00328984 + x][ x]/[0.00328984 - x]. Solving, x = 0.00213308 M. Then, 0.00328984 + 0.00213308 = 0.00542292 M, or 2.266, which rounds to 2.27.

Right.