Title: PROTOTYPE COLUMN

Research Question: How does the concentration of salt affect the boiling point of water?

Materials: 3 beakers (100 mL each), thermometer, hot plate, stirring rod

Chemicals: Table salt, distilled water

Procedure:

1. Fill each beaker with 80 mL of distilled water.
2. Label the beakers as A, B, and C.
3. Add 0 grams of salt to beaker A, 5 grams of salt to beaker B, and 10 grams of salt to beaker C.
4. Stir each solution until the salt is completely dissolved.
5. Place beaker A on the hot plate and heat until the water boils. Record the boiling point.
6. Repeat step 5 for beakers B and C.
7. Compare the boiling points of the three solutions.

Q: Conduct the experiment and record your observations.
A: Beaker A (0 grams of salt):
Temperature: 100°C
Observation: The water boils at 100°C as expected, with no salt added.

Beaker B (5 grams of salt):
Temperature: 101°C
Observation: The boiling point is slightly elevated due to the addition of 5 grams of salt.

Beaker C (10 grams of salt):
Temperature: 102°C
Observation: The boiling point increases further with the addition of 10 grams of salt, demonstrating that higher salt concentration raises the boiling point of water.

Q: Conclusion: Explain the experimental result
A: The experimental results show that the boiling point of water increases as the concentration of salt increases. This is due to the phenomenon known as boiling point elevation, which is a colligative property. When salt (a solute) is dissolved in water (a solvent), it disrupts the formation of vapor bubbles that are necessary for boiling. As a result, more heat (higher temperature) is required to reach the boiling point. Therefore, Beaker A with 0 grams of salt has the lowest boiling point, Beaker B with 5 grams of salt has a higher boiling point, and Beaker C with 10 grams of salt has the highest boiling point. This demonstrates how the addition of a solute can affect the physical properties of a solvent.