Can acetic acid reach a pH of 1.30 at all? I didn't grasp it properly I guess.
Pure acetic acid weighs 1049g/L and 60.05g/mol, that is, 1L contains 17.5mol.
At 1M the dissociation is only 0.4% and this decreases at higher concentration. So even with little water (which would introduce other limits), 1L and 17.5mol would contain less than 0.07mol H+. This gives a pH less strong than 1.16. I suppose the lesser dissociation doesn't let reach 1.30.
From measured pH=2.4 at 1M, pH=1.3 would need over 10× more concentrated H+ and then the ionization of the acid would be over 10× less, rather 0.04% than 0.4%, putting pH=1.3 out of reach.