A 25.0 mL volume of a 0.200 M N₂H₄ solution ( K _b = 1.70×10^{- 6}) is titrated to the equivalence point with 0.100 M HCl. What is the pH of this solution at the equivalence point?
The titration is:
N₂H₄ + HCl→N₂H₅⁺ + Cl^-

Question

Quizplus · Accepted Answer

At the equivalence point, N₂H₅⁺ is formed, which is a weak acid. Calculate the concentration of N₂H₅⁺ and use its K_a (derived from K_w/K_b) to find [H⁺], then pH.

A 250 ML Volume of a 0