Final answer:
To calculate the concentration of species in a solution of H₂C₆H₆O6, one would use ICE tables along with the acid dissociation constants. Due to missing specific values, the exact concentrations cannot be provided without additional data.
Step-by-step explanation:
To calculate the concentration (in m) of each species present in a 0.240 m solution of H₂C₆H₆O6, we need to consider the acid dissociation constants (Ka values) for its ionization steps. The first ionization step would provide the concentration of H+ and C₆H₇O6⁻ ions, and the second step would provide the concentration of H+ and C₆H₈O6²⁻ ions. Assuming the ionization of water is negligible, we use an ICE table and the provided acid dissociation constants to solve for each species' concentration at equilibrium.
However, the exact calculations would require the specific acid dissociation constants for each step of ionization of H₂C₆H₆O6, which has not been provided in the information above. Normally, you would set up an ICE table with the initial concentration of H₂C₆H₆O6 and the change in concentration (x) as the acid ionizes. Then you would use the Ka value and the assumption that x is much smaller than the initial concentration to solve for x.