When H2SO4 is added to a large beaker of water, how does the resulting solution differ from pure water?

• A. The solution turns into a solid precipitate.
• B. The solution remains neutral with no change in pH.
• C. The solution becomes acidic due to the formation of H+ ions.
• D. The solution becomes basic due to the formation of OH- ions.

Answer: (C)

Verified step by step guidance

1. Recognize that H2SO4 (sulfuric acid) is a strong acid that dissociates completely in water.
2. Write the dissociation reaction of H2SO4 in water: \(\mathrm{H_2SO_4 \rightarrow 2H^+ + SO_4^{2-}}\).
3. Understand that the release of \(\mathrm{H^+}\) ions increases the concentration of hydrogen ions in the solution.
4. Recall that an increase in \(\mathrm{H^+}\) ion concentration lowers the pH, making the solution acidic.
5. Conclude that the solution becomes acidic due to the formation of \(\mathrm{H^+}\) ions, unlike pure water which is neutral.