This is the property of freezing point depression and boiling point elevation. This is because of the solute absorbing the energy added to the system to heat its own molecules and so it would require more energy to boil the solvent. Likewise for freezing point depression, the molecules retain more energy.
It is called depression of the freezing point (it lowers the F.P. of the solvent).
The boiling point is elevated when solute is added to solvent.
it will raise the boiling point of the solvent
Lower
raise it
It increases the boiling point of the solution and it increases the temperature range over which the solution remains a liquid.
This depends on: molality of the solute, dissociation of the solute, cryoscopic constant of the solvent.
raise its freezing point
When adding a solute to a solvent, the freezing point decreases and is also known as freezing-point depression. Hence when naphthalene is added to camphor the freezing point decreases.
Conductivity
RAISE
When any solute is dissolved into a solvent, the freezing point will always go down.
Boiling point elevation
The freezing point is lowered.
The freezing point is lowered.
The freezing point is lowered.
freezing point depression ..
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.
It increases the boiling point of the solution and it increases the temperature range over which the solution remains a liquid.
A non-volatile solute affects increases osmotic pressure. This is a colligative property. There will be a higher osmotic pressure required to prevent the solvent from flowing into the solution because the solvent has a higher chemical potential without solute in it.
The depression of the freezing point is dependent on the nature of solvent and concentration of solute.
A solute depresses the freezing point of a solution because the solute can not fit perfectly into the crystal lattice of the solid solvent. The normal crystal lattice is the lowest energy arrangement of the molecules or ions of the solid solvent. Therefore, the disordered lattice of a solvent freezing in the presence of a solute has at least slightly higher energy than the lattice of a solid pure solvent and requires at least a slightly lower temperature to solidify.