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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?
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
The change in the freezing point of a solvent by the addition of a solute is called?
freezing point depression ..
What is the freezing point depression constant for naphthalene?
The freezing point depression constant for Naphthalene is 6.9 degrees Celsius/mhttp://en.wikipedia.org/wiki/Freezing-point_depression
Could freezing point depression be used for substances that are not soluble in water?
Substances which are insoluble in a given solvent do not cause a freezing point depression in that solvent.
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 the molar freezing point constant?
molal
What does the depression of the freezing point dependent on?
The depression of the freezing point is dependent on the nature of solvent and concentration of solute.
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?
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
What is the tendency of a solute to change the melting point of a solid called?
The answer is "Freezing point depression" on Apex
The change in the freezing point of a solvent by the addition of a solute is called?
freezing point depression ..
What is the freezing point depression constant for naphthalene?
The freezing point depression constant for Naphthalene is 6.9 degrees Celsius/mhttp://en.wikipedia.org/wiki/Freezing-point_depression
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
Could freezing point depression be used for substances that are not soluble in water?
Substances which are insoluble in a given solvent do not cause a freezing point depression in that solvent.
What is freezing point depression?
For the definition and description of freezing point lower or freezing point depression[http://www.answers.com/freezing+point+depression?cat=technology&gwp=13Click here for the answer from Answers.com]For how to solve a freezing point depression problem with step-by-step instructions click on this question:[http://wiki.answers.com/Q/How_do_you_solve_freezing_point_depression_problemsHow do you solve freezing point depression problems?]
What are examples of freezing point depression boiling point elevation and vapor point lowering?
The freezing is ag gago weak
What is the freezing point depression of sodium chloride?
The maximal freezing point depression for sodium chloride is -18 0C. For the theoretical calculus see the link below.
Why is the curve for the freezing point of solvent different from the freezing point of solution?
it is increased with the increasing density
