Is this question correctly formulated? If so, could you provide it as is; if not, modify it as needed and return it in JSON format: Calculate the concentration of all species in a 0.500 M solution of H2SO3.

Verified step by step guidance

1. <insert step 1: Understand that H2SO3 is a diprotic acid, meaning it can donate two protons (H+ ions) in solution.>
2. <insert step 2: Write the dissociation equations for H2SO3. The first dissociation is H2SO3 ⇌ H+ + HSO3^-. The second dissociation is HSO3^- ⇌ H+ + SO3^2-.>
3. <insert step 3: Use the given initial concentration of H2SO3 (0.500 M) and set up an ICE (Initial, Change, Equilibrium) table for each dissociation step to track the changes in concentration.>
4. <insert step 4: Apply the equilibrium constant expressions for each dissociation step. For the first dissociation, use Ka1 = [H+][HSO3^-]/[H2SO3]. For the second dissociation, use Ka2 = [H+][SO3^2-]/[HSO3^-].>
5. <insert step 5: Solve the equilibrium expressions simultaneously to find the concentrations of all species: [H2SO3], [HSO3^-], [SO3^2-], and [H+].>