Sodium chloride is commonly known as table salt that we use in our daily lives. In its molten state it has a high boiling point because of the strong force of attraction between the positive and negative ions. In an aqueous solution, the boiling point is much lower because the ions are held in place by strong forces of attraction between water molecules and not by the force of electrostatic attraction. The question asks about raising the boiling point of a solution by adding a non volatile solute.

To raise the boiling point of a solution, its vapor pressure must increase above the surrounding atmospheric pressure. The vapor pressure of the solvent must also increase. This is accomplished by increasing the temperature of the solution.

A solution that contains a non-volatile solute has a lower vapor pressure than its pure solvent because the molecule of the solute is smaller and less dense. This causes the solution to require a higher temperature in order to reach its vapor pressure above the surrounding atmospheric pressure, which is the boiling point.

The concentration of the solute in the solution will determine how much its boiling point will change, which is measured by comparing the normal boiling point of the solvent to the boiling point at different concentrations of the solute. This is a property of a solution that can be derived from a graph. The following graph shows the normal boiling points of water (solvent) as a function of its molality in several solutions of sucrose and urea (non-volatile solutes). Notice that as the molality increases, the boiling point rises.

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.