A diprotic acid solution h2a has a molarity of 065 mthe

Question

A diprotic acid solution H₂A has a molarity of 0.65 M.The concentrations of the species present at equilibrium are asfollows:

[H⁺]=0.25 M

[HA^-]=0.25

[A^2-]=4.6 x 10^-4 M

The second ionization constant (K_a2) for this acid is4.6 x 10^-4

What is the concentration of H₂A remaining in solution? (It's a weak diprotic acid)