[LackOfNames34]

Hello! I'm working on a chemistry assignment and have struggled with a question about describing a given titration curve graph (link to picture below, I also attempted to attach the image).

https://drive.google.com/file/d/1ymNKFzBV8hhGjrbjRJeFqi8ZIhXI3cEB/view?usp=sharing

The question I'm having issues with is:

 "Identify if the analyte and titrants are strong or weak acids/bases"

 I'm pretty much lost on where to start. But if I had to guess, I would say it's a weak acid strong base because the starting PH is higher than 0. But I'm by no means confident in this answer. Did I approach this question correctly? And if not, what should I do?

[Borek]

I would say it's a weak acid strong base because the starting PH is higher than 0.

It all depends on the concentration: what is pH of 0.01 M HCl? Is HCl a strong acid?

I am not sure there is enough information to answer the question. Separation of endpoints tells a lot about second and third dissociation constants, but not so much about the first.

[LackOfNames34]

Would knowing the pKa1 and pKa2 values help? Because I have those two values as well.

[Borek]

If you refer to the values read at half-points - beware, as pKa1 is incorrect (think again about 0.01 M HCl  titration, at half point its pH is about 2.5, does it mean pKa of HCl is 2.5?).