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When something is dissolved in water, the temperature that it takes for the solution to boil is higher than that of pure water. This is because the molecules of the solvent have to overcome the vapor pressure of the air to turn from liquid to gas phase, and it requires more energy (heat) to do this. This phenomenon is called boiling point elevation. It happens whenever a non-volatile solute, such as salt, is added to a pure solvent, such as water.
In order to observe the effect of adding a solute on the boiling point, you can set up an experiment using three test tubes filled with the same volume of water. Label one of the test-tubes with the concentration of the solute, such as “5% NaCl”. Place all of the test-tubes in a Bunsen burner and heat them equally until bubbles begin to form at the top of the water test-tube. After the bubbling stops, measure the temperature of the water by placing a thermometer into the test-tube. Take note of the temperature that the bubbles first began to form at.
The test-tube that contains 5% NaCl will have a higher boiling point than the other two tests, because the bonds in the NaCl ionic compound are stronger, and therefore require more heat to break them. However, it is important to remember that the difference in boiling points between a solution and the original solvent can also be caused by other factors, such as temperature and vapor pressure.