What is the KF value of camphor?
The freezing point of camphor is 178.4 C and its molar freezing point depression constant (Kf) is 37.7 C kg/mol.
How do you calculate freezing point depression?
The freezing point depression ∆T = KF·m where KF is the molal freezing point depression constant and m is the molality of the solute. Rearrangement gives: mol solute = (m) x (kg solvent) where kg of solvent is the mass of the solvent (lauric acid) in the mixture. This gives the moles of the solute.
What is the freezing point depression constant?
The freezing point depression is the difference in temperature between the freezing point of the pure solvent and that of the solution. The molal freezing-point depression constant is equal to the change in the freezing point for a 1-molal solution of a nonvolatile molecular solute.
Why is camphor preferred in the determination of depression in freezing point?
Why is camphor preferred solvent in the determination of molecular mass of non-volatile solute by cryoscopic method (Rast method)? Answer: Camphor has a large value of (39.7 °C). Therefore there is large value of depression in freezing point of solution which can be measured by ordinary thermometer.
What is KF formula?
To calculate the freezing point depression constant, or Kf, you’ll need the equation: delta Tf = Kfcm where cm is the molal concentration of the solution.
Which solvent has highest KF value?
– Hence, camphor has the highest value of Kf among the following.
Is freezing point depression positive or negative?
The change in the freezing point is proportional to the amount of solute added. This phenomenon is called freezing point depression. The change in the freezing point is defined as: ∆Tf = Tf,solution − Tf,solvent. ∆Tf is negative because the temperature of the solution is lower than that of the pure solvent.
Why is there a depression in freezing point?
Freezing point depression is the phenomena that describes why adding a solute to a solvent results in the lowering of the freezing point of the solvent. When a substance starts to freeze, the molecules slow down due to the decreases in temperature, and the intermolecular forces start to take over.
Is freezing point depression a Colligative property?
Freezing point depression is a colligative property observed in solutions that results from the introduction of solute molecules to a solvent. The freezing points of solutions are all lower than that of the pure solvent and is directly proportional to the molality of the solute.
Why there is depression in freezing point?
Is KF acid or base?
KF is a salt that comes from a strong base, KOH, and a weak acid, HF. Because HCl is listed in Table 12.2 “Strong Acids and Bases”, it is a strong acid.
What is a KF value?
Kf is a constant for a given solvent. Kf is called the molal freezing point depression constant and represents how many degrees the freezing point of the solvent will change when 1.00 mole of a nonvolatile nonionizing (nondissociating) solute dissolves in one kilogram of solvent.
What is the freezing point of camphor and molar mass?
When 0.186 g of an organic substance of unknown molar mass is dissolved in 22.01 g of liquid camphor, the freezing point of the mixture is found to be 176.7 °C. What is the molar mass of the solute?
What is the van’t Hoff factor for freezing point depression?
In a more generic way, it is called the “molal freezing point depression constant.” The constant called the van ‘t Hoff factor is symbolized with the letter ‘i’ and is discussed below the example problems. These are some sample cryoscopic constants: 40. 30. The units on the constant are degrees Celsius per molal (°C m¯ 1 ).
Which is an example of a freezing point depression?
Example #5: Camphor (C 6H 16O) melts at 179.8 °C, and it has a particularly large freezing point depression constant, K f = 40.0 °C/m. When 0.186 g of an organic substance of unknown molar mass is dissolved in 22.01 g of liquid camphor, the freezing point of the mixture is found to be 176.7 °C.
How to calculate the freezing point depression of benzene?
Step 1: Calculate the freezing point depression of benzene. Tf = (Freezing point of pure solvent) – (Freezing point of solution) (5.5 oC) – (2.8 oC) = 2.7 oC. Step 2 : Calculate the molal concentration of the solution. molality = moles of solute / kg of solvent. moles of naphthalene = (1.60 g) (1 mol / 128 g) = 0.0125 mol naphthalene.