If you mean "measuring pH to directly determine concentration of the substance" the answer is "no". Even assuming ideal behavior of the solution and no errors in measurements pH of 2.00 means anything between 1.995 and 2.00499, check how that translates to accuracy of the concentration and compare that to the accuracy you can get from the titration.
pH meter can be great in helping determining the equivalence point of the titration.
Thank you for the feedback.
It seems I have 3 options:
1. Buy a 99.99% pure, analytical grade, oxalic acid and titrate the NaOH solution to standardize it. This is the most expansive option.
2. Buy a 99.6% pure oxalic acid crystals and try to recrystallize it to improve the purity; then weigh in some concentration of it and and titrate NaOH.
3. Recrystallize and fully hydrate the NaOH and weigh in the concentration i want directly, accounting for weight of the water of hydrate.
I am kind of leaning towards option #2. what do you think?
Goal of all this is to get a 0.1M NaOH to measure total acid and free acid of home made parkerizing solution. While also learning the "legit", lab grade, ways of doing it.