Question

I messed up on my titration: filled part of the burette with a supersaturated solution of KHTar(2.073g...MM=188.18amu) dissolved in 150mL diH2O, instead of the 0.051M NaOH solution.
I know it wasn't more than a few mL, but I noticed a huge difference in the volume of NaOH needed for the second aliquot.
Is there anyway to determine mathematically the volume of NaOH I should have used? (I need the correct volume to determine the [HTar-] in solution).
Dissociation:

KHTar(aq)--> K+(aq)+HTar-(aq)
HTar-(aq)+OH-(aq)-->Tar^2-(aq)+H2O(l)

Ksp=[K+][HTar-]--> [K+]=[HTar-]

[HTar-]=[NaOH]x Volume(NaOH)added x (1/Volume KHTar solution)

Volume diH20= 150mL
Amount KHTar= 2.073g
Volume of saturated KHTar sol=25.0mL
[NaOH]=0.051M
Need:
Volume NaOH at neutralization and
[HTar-]

Answer 1

You apparently know the concn of the KHTar but as I read the problem you don't know EXACTLY how much of the tartrate you used in the titration. No, there is no way you can reconstruct the data.