Although \(\mathrm{HCl}\) and \(\mathrm{H}_{2} \mathrm{SO}_{4}\) have very different properties as pure substances, their aqueous solutions possess many common properties. List some general properties of these solutions, and explain their common behavior in terms of the species present.

Some general properties of aqueous solutions of \(\mathrm{HCl}\) and \(\mathrm{H}_{2}\mathrm{SO}_{4}\) are: 1. Both are strong acids. 2. Both solutions are highly conductive. 3. They both react with bases to form salts and water. 4. Both solutions have a sour taste. 5. Both acids are corrosive to varying degrees. Now let's analyze the species present in these solutions and understand their common behavior.

When \(\mathrm{HCl}\) and \(\mathrm{H}_{2}\mathrm{SO}_{4}\) are dissolved in water, they form the following species: 1. \(\mathrm{HCl}\) dissociates into ions: \(\mathrm{HCl}\) \(\rightarrow\) \(\mathrm{H}^{+}\) + \(\mathrm{Cl}^{-}\) 2. \(\mathrm{H}_{2}\mathrm{SO}_{4}\) dissociates into ions: \(\mathrm{H}_{2}\mathrm{SO}_{4}\) \(\rightarrow\) \(2\mathrm{H}^{+}\) + \(\mathrm{SO}_{4}^{2-}\)

The common behavior of the aqueous solutions of \(\mathrm{HCl}\) and \(\mathrm{H}_{2}\mathrm{SO}_{4}\) can mainly be attributed to the presence of the \(\mathrm{H}^{+}\) ions (protons) in both solutions. The general properties mentioned in Step 1 can be explained as follows: 1. Strong acids: Both \(\mathrm{HCl}\) and \(\mathrm{H}_{2}\mathrm{SO}_{4}\) dissociate completely into their ions, releasing a high concentration of \(\mathrm{H}^{+}\) ions, which characterizes them as strong acids. 2. High conductivity: The presence of ions such as \(\mathrm{H}^{+}\), \(\mathrm{Cl}^{-}\), and \(\mathrm{SO}_{4}^{2-}\) in their aqueous solutions allows them to conduct electricity, making the solutions highly conductive. 3. Reaction with bases: Both solutions can react with bases to form water and a salt, due to the presence of \(\mathrm{H}^{+}\) ions, which can combine with hydroxide ions (\(\mathrm{OH}^{-}\)) from the base, forming water. The remaining ions form the salt. 4. Sour taste: The sour taste of both solutions can be attributed to the \(\mathrm{H}^{+}\) ions, which can be sensed by our taste buds as sourness. 5. Corrosive nature: The corrosive nature of both solutions is a result of the high concentration of \(\mathrm{H}^{+}\) ions, which can react with various materials, causing them to corrode. In conclusion, the common behavior of aqueous solutions of \(\mathrm{HCl}\) and \(\mathrm{H}_{2}\mathrm{SO}_{4}\) can be attributed to the presence of \(\mathrm{H}^{+}\) ions in both solutions. This is responsible for their general properties and reactivities.