When Ca(OH)_2 is added to a large beaker of water, how does the resulting solution differ from pure water?

• A. The solution remains neutral with no change in pH.
• B. The solution becomes basic due to the presence of OH^- ions.
• C. The solution forms a precipitate of Ca^2+ ions.
• D. The solution becomes acidic due to the release of H^+ ions.

Answer: (B)

Verified step by step guidance

1. Identify the compound Ca(OH)\_2 as calcium hydroxide, which is a strong base that dissociates in water.
2. Write the dissociation equation for Ca(OH)\_2 in water: \(\mathrm{Ca(OH)_2 \rightarrow Ca^{2+} + 2OH^-}\).
3. Recognize that the dissociation releases hydroxide ions (OH\^-) into the solution, increasing the concentration of OH\^- ions.
4. Understand that an increase in OH\^- ions causes the solution to become basic, which means the pH will be greater than 7.
5. Conclude that the solution differs from pure water by becoming basic due to the presence of OH\^- ions, not neutral or acidic, and no precipitate forms because Ca(OH)\_2 is soluble.