Find the freezing point depression of pure lauric acid-unknown solution. Find the molality of the unknown....
Find the freezing point depression of pure lauric acid-unknown solution. Find the molality of the unknown.
Info: Kf= 4.40*C/moles solute
Freezing point of pure lauric acid- 43.2*C and freezing point of solution- 42 *C
Mass of unknown solid (nonelectrolyte)- 0.0612g, mass of lauric acid- 3.9321g
Homework Answers
Δ Tf = -42 oC - (- 43.2 oC)
= 1.2 oC
use:
Δ Tf = Kf*mb
1.2 = 4.40 *mb
mb= 0.2727 molal
Answer: 0.273 molal
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Here is some background for the questions:
Thank you in advance.
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Here is some background for the questions:
Thank you in advance.
You add 0.0336 moles of benzoic acid solute to 16.00 g of an unknown solvent, which lowers the freezing point of the solvent by 8.6 °C. Calculate the freezing point depression constant (Kf) of the unknown solvent. You dissolve 1.00 g sample of an unknown solute is in 8.00 g of lauric acid, which lowers the freezing point by 5.0...
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bath and recorded temp drop which stopped at 39.44c
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