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If each molecule of unknown had dissociated into two ions in the lauric acid solution what effect would there have been on the freezing point depression of the solution?
Wiki User
∙ 15y ago
Freezing point depression is more significant if a molecule dissociates. It is the molality of the solution of osmotically active particles and freezing/melting point constant (k) of the solvent that determine the magnitude of freezing point depression.
In these experiments, we are usually measuring freezing point depression to determine molar mass of the unknown solute. The calculated molar mass would be would be lower than the actual mass of the intact molecule. If you have half as many intact particles, the intact molecular weight must be double to obtain the same formula ratio:
MW = g / mol ... since mol actually less of the intact particle, MW must be more
Wiki User
∙ 15y ago
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What colligative property is responsible for antifreeze?
Freezing point depression. When a solution is formed the molecules of the solute prevent the solution from freezing at its normal freezing point, it must be colder.
The solution has a freezing point of -2.79 . The freezing point depression constant for water is 1.86 K m-1. What is the nitrate concentration in the solution?
The solution has a freezing point of 2.79 and this is the frezzing point of mercury
What compounds break up into ions in solution?
Ionic compounds are dissociated in water solution.
What is the approximate freezing point depression of a 0.050 m aqueous solution?
-0.37 C
Calculate the freezing point depression of an aqueous solution of 0.22 m FeCl3 Assume complete dissociation?
look at Calculate_the_boiling_point_elevation_of_an_aqueous_solution_of_0.0500_m_CaCl2_Assume_complete_dissociationvery similar questionanswer is 1.64 lower than the originial freezing pointif the freezing point is 0 for example the freezing point depression is -1.64
The freezing point of a solution containing 4.12 g of unknown solute in 100 grams of camphor is 166.2 degrees C what is the freezing point depression?
f.p depression = (freezing point of pure solvent)-(freezing point of solution) -------> 178.4-166.2=12.2
What colligative property is responsible for antifreeze?
Freezing point depression. When a solution is formed the molecules of the solute prevent the solution from freezing at its normal freezing point, it must be colder.
The solution has a freezing point of -2.79 . The freezing point depression constant for water is 1.86 K m-1. What is the nitrate concentration in the solution?
The solution has a freezing point of 2.79 and this is the frezzing point of mercury
What compounds break up into ions in solution?
Ionic compounds are dissociated in water solution.
What is the approximate freezing point depression of a 0.050 m aqueous solution?
-0.37 C
Calculate the freezing point depression of an aqueous solution of 0.22 m FeCl3 Assume complete dissociation?
look at Calculate_the_boiling_point_elevation_of_an_aqueous_solution_of_0.0500_m_CaCl2_Assume_complete_dissociationvery similar questionanswer is 1.64 lower than the originial freezing pointif the freezing point is 0 for example the freezing point depression is -1.64
How does changing the concentration of a solution affect the kf?
Increasing the concentration of a solute the freezing point depression is increased.
How is the dissolving process of sugar and salt different?
Salt is dissociated in ions in the solution; sugar is not dissociated.
How is salt and sugar dissolving process is different?
Salt is dissociated in ions in the solution; sugar is not dissociated.
How do you solve freezing depression?
You need to know the solute and the solvent and whether the solute is molecular or ionic and how many ions it contains. The formula is the change in freezing point equals the number of ions times the freezing point depression constant times the molality of the solution.
Why is the curve for the freezing point of solvent different from the freezing point of solution?
it is increased with the increasing density
What is an electrolyte when placed in an aqueous solution?
A salt, acid or base which can be dissociated in ions in an aqueous solution.
