Final answer:
The pH of a 2.0 M H2SO3 aqueous solution cannot be accurately calculated without additional information, such as the dissociation constant (Ka) for H2SO3. For a strong acid of the same concentration, a simple calculation using the negative logarithm of the concentration would suffice, but this is a weak acid and behaves differently.
Step-by-step explanation:
To calculate the pH of a 2.0 M H2SO3 aqueous solution, you would first recognize that H2SO3, sulfurous acid, is a weak acid that partially dissociates in water to produce hydronium ions, H3O+, and hydrogen sulfite ions, HSO3-.
To find the pH, we need the concentration of the hydronium ions. Since H2SO3 does not ionize completely, we cannot simply take the negative logarithm of the concentration of the acid. The situation would be more complex, requiring us to know the dissociation constant (Ka) of H2SO3 to find the actual concentration of H3O+. However, without this information provided, an exact calculation isn't possible within the scope of this question.
For a strong acid, a 2.0 M solution would have a pH equal to -log(2.0), but because H2SO3 is a weak acid, the pH would be higher than the corresponding calculated value for a strong acid. The precise value, however, would require more data than is provided in the question, therefore, this question cannot be answered accurately with the given information.