The "Temperature and Solubility" experiment aims to investigate how the solubility of a substance is influenced by the temperature of the solvent. This experiment is based on the hypothesis that the solubility of a solute increases with the temperature of the solvent, a concept fundamental to understanding solutions in chemistry.
Materials You Need
- Sodium chloride (table salt) or sugar (sucrose)
- Distilled water
- Three beakers or glass jars
- Stirring rods
- Heating source (like a hot plate or Bunsen burner)
- Balance scale
- Graduated cylinders
- Label the beakers as 'Cold', 'Room Temperature', and 'Hot'. Measure and pour equal volumes of distilled water into each.
- Adjust the temperature of the water in each beaker: add ice for 'Cold' to reach about 5°C, leave 'Room Temperature' as is, and heat 'Hot' to approximately 60°C.
- Weigh out an equal amount of the solute and add it to each beaker.
- Stir each solution continuously and observe the solute's dissolving rate until saturation.
Observations and Results
Record the time each solute takes to dissolve in the different temperature conditions. Note the amount of undissolved solute at the saturation point for each temperature. Compare the solubility in cold, room temperature, and hot water.
Analyze the data to determine if the hypothesis holds true. The conclusion should discuss whether the solubility of the solute was greater in hot water compared to cold, and what this implies about the relationship between temperature and solubility in solutions.