For the diprotic weak acid H2A, Ka₁ =3.4×10⁻⁶ and Ka₂=6.1×10⁻⁹.

What is the pH of a 0.0500 M solution of H2A? What are the equilibrium concentrations of H2A and A2− in this solution?

Express Ka₁ in terms of x, and then show the simplified expression (when x is assumed to be negligible compared to to the initial concentration).

Ka₁=/ =/

numerator in complete expression:
denominator in complete expression:
numerator in simplified expression:
denominator in simplified expression:

Also, give the numerical value of x using the appropriate approximation. What is the pH of the solution if you stopped here?

x:
pH: