The curve below shows the titration of a diprotic acid H₂A with NaOH. Estimate the pKa values for the diprotic acid.

Titration of 75.0 mL of a 1.25 M solution of citric acid with 37.5 mL of 1.25 M NaOH was done. Calculate the pH if the pK_a values for the first, second, and third dissociations are 3.13, 4.76, and 6.40 respectively.

What is the pH for the titration of 55.0 mL of a 0.15 M solution of the protonated form of valine (H₂A⁺: K_a1 = 5.13×10⁻³, K_a2 = 1.82×10⁻¹⁰) with 110.0 mL of 0.15 M KOH?

When a 15.0 mL sample of 5.45 g/L solution of a diprotic acid was titrated against 0.15 M KOH, it required 24.50 mL of the base to reach the endpoint. The pH values at the first and second equivalence points were 5.75 and 10.75, respectively. Calculate the pKa1, pKa2, and the molecular weight of the acid.

One of the following graphs represents the titration of a triprotic acid with a strong base. Which titration curve is it?

What is the molar mass of a 0.738 g of unknown diprotic acid neutralized by titrating with 71.24 mL of 0.167 M calcium hydroxide?