A liquid in the lab has a density of 1.17 g/cm^3. Which of the following statements is true if you pour this liquid into a container of water (density = 1.00 g/cm^3)?

• A. The liquid will evaporate immediately upon contact with water.
• B. The liquid will float on top of the water.
• C. The liquid will sink below the water.
• D. The liquid will mix evenly with the water regardless of density.

Answer: (C)

Verified step by step guidance

1. Understand that density is defined as mass per unit volume, given by the formula \(\text{density} = \frac{\text{mass}}{\text{volume}}\).
2. Compare the density of the liquid (1.17 g/cm\(^3\)) with the density of water (1.00 g/cm\(^3\)) to determine relative behavior when mixed.
3. Recall that a substance with a higher density than water will sink below it, while a substance with a lower density will float on top.
4. Evaluate the given options based on the density comparison: since 1.17 g/cm\(^3\) is greater than 1.00 g/cm\(^3\), the liquid will sink below the water.
5. Note that evaporation and mixing behavior depend on other factors such as volatility and miscibility, but density alone determines whether the liquid floats or sinks.