18. Aqueous Equilibrium

Calculate the pH of 75.0 mL of a 0.10 M of phosphorous acid, H₃PO₃, when 80.0 mL of 0.15 M NaOH are added. K_a1 = 5.0 × 10⁻², K_a2 = 2.0 × 10⁻⁷.

Find the pH when 100.0 mL of a 0.1 M dibasic compound B (pK_b1 = 4.00; pK_b2 = 8.00) was titrated with 11 mL of a 1.00 M HCl.

Suppose you have 50.1 mL of a H₃PO₄ solution that you titrate with 15.4 mL of 0.10 M KOH solution to reach the endpoint. What is the concentration of H₃PO₄ of the original H₃PO₄ solution?

What is observed when equal volumes of 0.1 M aqueous HCl and 0.01 M aqueous Na₂SO₃ are mixed?

What is the identity of the acid (H₃X) identified via titration of Na₃X with HCl?