Question

In: Chemistry

Discuss why the freezing point of a solution is typically lower than the freezing point of...

Discuss why the freezing point of a solution is typically lower than the freezing point of pure solvent?

why molality is used as the unit of concentration in colligative property calculation?

Solutions

Expert Solution

Solution :-

The freezing point is the state where the liquid phase and solid phase are in equilibrium with each other

When we add solute to the liuid then the potential of the liquid phase decreases therefore it becomes more stable than solid phase

The concentration of the solute is directly proportional to the freezing point decrease of the solution. Therefore the freezing point of the solution is lower than the freezing point of the pure solvent.

In the calculation of the concetration of the colligative property calculations the molaity is the unit used for the concentration because. Molaity is moles per kg solvent the mass of the solvent does not change so the concentration also does not chages for the solution if the molarity is used then as the temperature changes the volume of the liquid can change because volume is affected by the temperature so the concetration also chages which would lead to the incorrect calculations therefore in the colligative property calculations concentration is used in molality.


Related Solutions

Discuss why the freesing point of a solution is typically lower than the freezing poiunt of...
Discuss why the freesing point of a solution is typically lower than the freezing poiunt of pure solvent
. The freezing point of benzene is 5.5oC What is the freezing point of a solution...
. The freezing point of benzene is 5.5oC What is the freezing point of a solution of 5.00 g C10H8 in 444 g   of benzene. You will need to look up the freezing point depression constant for benzene in a reference book.                 Calculated FP: Benzene Kf = ___________ *remember you will need “m”, which is in Kg     Name of reference used: __________________       Calculated FP:     i factor used and explain i factor:
The freezing point of benzene is 5.5°C. What is the freezing point of a solution of...
The freezing point of benzene is 5.5°C. What is the freezing point of a solution of 2.80 g of naphthalene (C10H8) in 355 g of benzene (Kf of benzene = 4.90°C/m)? Please answer in how many degrees of Celcius
The boiling point of an aqueous solution is 102.34 °C. What is the freezing point?
The boiling point of an aqueous solution is 102.34 °C. What is the freezing point?
What are the boiling point and freezing point of a 1.47 m solution of naphthalene in...
What are the boiling point and freezing point of a 1.47 m solution of naphthalene in benzene? (The boiling point and freezing point of benzene are 80.1°C and 5.5°C respectively. The boiling point elevation constant for benzene is 2.53°C/m, and the freezing point depression constant for benzene is 5.12°C/m.) Boiling point = °C Freezing point = °C
What are the freezing point and boiling point of a solution prepared by dissolving 18.6g of...
What are the freezing point and boiling point of a solution prepared by dissolving 18.6g of CaCl2 in 200.0g of water? (kf = -1.86�/m and kb= 0.512�/m)?
What is the molality of a solution of naphthalene in benzene if the freezing point of...
What is the molality of a solution of naphthalene in benzene if the freezing point of pure benzene is 5.5°C and the freezing point of the solution is 4.0°C. The freezing point depression constant for benzene is 5.12°C m-1.
How is a solution freezing point and boiling point affected by addition of a dissolved solute?
How is a solution freezing point and boiling point affected by addition of a dissolved solute?
The boiling point of an aqueous solution is 102.32 °C. What is the freezing point? Constants...
The boiling point of an aqueous solution is 102.32 °C. What is the freezing point? Constants can be found here.
1) The boiling point of an aqueous solution is 101.98 ∘C. What is the freezing point?...
1) The boiling point of an aqueous solution is 101.98 ∘C. What is the freezing point? Consult the table of colligative constants. freezing point:   °C 2) Quinine is a natural product extracted from the bark of the cinchona tree, which is native to South America. Quinine is used as an antimalarial agent. When 0.829 g of quinine is dissolved in 25.0 g of cyclohexane, the freezing point of the solution is lowered by 2.13 ∘C. Look up the freezing point...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT