What is the pH of a 0.10 M solution of H₂SO₃, given that its pKₐ is 1.77 and the change in concentration is small?

Set up an ICE (Initial, Change, Equilibrium) table to determine the concentrations of the species at equilibrium. Initially, the concentration of H₂SO₃ is 0.10 M, and the concentrations of H⁺ and HSO₃⁻ are 0 M.

Assume that the change in concentration of H₂SO₃ is small, so the equilibrium concentration of H₂SO₃ is approximately 0.10 M. Let x be the concentration of H⁺ and HSO₃⁻ at equilibrium. The equilibrium expression is: $Kₐ=\frac{x^2}{0.10}$.