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18. Aqueous Equilibrium

Titrations: Diprotic & Polyprotic Buffers

18. Aqueous Equilibrium

Titrations: Diprotic & Polyprotic Buffers

Multiple Choice
The titration of 18.0 mL of an unknown diprotic acid requires 15.3 mL of 0.120 M KOH solution to reach the equivalence point. What is the concentration of the unknown acid sample?
Multiple Choice
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.
Multiple Choice
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.
Multiple Choice
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?
Open Question
A 25.0 ml sample of 0.125 moll−1 pyridine (kb=1.7×10−9) is titrated with 0.100 moll−1hcl.
Open Question
What is observed when equal volumes of 0.1 M aqueous HCl and 0.01 M aqueous Na₂SO₃ are mixed?
Open Question
What is the identity of the acid (H₃X) identified via titration of Na₃X with HCl?
Multiple Choice
30.00 mL of a strong, diprotic acid are titrated with 0.1432 M NaOH. If it takes 24.15 mL to reach the endpoint of the titration, what is the concentration of the acid?