Boiling out a solvent is when you heat up a solution to a high enough temperature that the solvent (liquid) evaporates, leaving behind whatever you have dissolved.
The solute increases the boiling point of the solvent
The concentration of solute in the solvent is most responsible for changing the boiling and freezing points. When a solute is added to a solvent, it disrupts the normal intermolecular forces between solvent molecules, which results in a change in the boiling and freezing points of the solvent.
Higher then the boiling point of the solvent.
When a solute is added to a solvent, the vapor pressure of the solution decreases compared to the pure solvent. This means the solution needs less energy to overcome atmospheric pressure and boil. As a result, the boiling point of the solution is lower than that of the pure solvent.
The similarities between the solute and solvent can lead to stronger interactions between them, increasing the boiling point of the solution due to enhanced solute-solvent cohesion. Conversely, dissimilarities may reduce these interactions, lowering the boiling point by weakening the solute-solvent bonds. Overall, the impact on boiling point depends on the specific chemical characteristics of the solute and solvent involved.
The boiling point rises and the freezing point lowers.The reason being, when a solute dissolves in a solvent, the solute molecules wedge themselves between the solvent molecules. In order for the solvent to freeze, its molecules have to get close enough together to form a solid. However, the solute molecules are in the way. As a result, it requires much colder temperatures for the solvent molecules to form a solid, despite the hindrance of the solute's molecules. The same sort of thing happens when trying to boil the solvent, only instead of holding the solvent molecules apart, the solute molecules end up holding them together, preventing them from boiling. Therefore, a more energy is needed to break the bond between solvent and solute, which allows the solvent to boil.
Boiling point elevation
The boiling point of beryllium is 2742 °C at sea level. If you can't move the solvent's boling point, you can always choose a different solvent.
It increases the boiling point of the solution and it increases the temperature range over which the solution remains a liquid.
Boiling-point elevation describes the phenomenon that the boiling point of a liquid (a solvent) will be higher when another compound is added, meaning that a solution has a higher boiling point than a pure solvent. This happens whenever a non-volatile solute, such as a salt, is added to a pure solvent, such as water. The boiling point can be measured accurately using an ebullioscope.
No: the boiling point is increased; see the link below.
The effect of a solute on the freezing point and boiling point of a solvent is related to what is known as the colligative property. Upon addition of the solute, the freezing point will be lowered, and the boiling point will be increased. The magnitude of the change will depend on the solute and how many particles it forms upon dissolving, and on the nature of the solvent and the freezing/boiling point constant for that solvent.