not sure about it,
for example; take two different types of oil (not water)
consider the first liquid is 'x' and other is 'y'
you want to change the freezing point of 'x'
by adding 'y' slowly
you can imagine the equations and other because i am a poor 'Indian' 'plus two' (standard education) my English also very bad.
freezing point depression ..
When any solute is dissolved into a solvent, the freezing point will always go down.
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.
The freezing point is lowered.
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.
freezing point depression ..
When any solute is dissolved into a solvent, the freezing point will always go down.
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.
No. dilution is the addition of solvent to decrease the concentration of a solute.
The freezing point is lowered.
The freezing point is lowered.
The freezing point is lowered.
Solutes raise and lower the boiling points of solvents. :)
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.
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.
The addition of solute to a solvent concentrates the overall solution. A nice example is the laundry detergent. Some (less) concentrated detergents are less viscous, while highly concentrated detergents are more viscous (greater density). Also, adding more solute to a solvent can lower the freezing point.
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.