Homework Help: Chemistry

Posted by Jaden on Wednesday, January 30, 2013 at 9:34pm.

If the freezing point of pure toluene is -95.15 oC and its freezing point depression constant is -8.38 oC/molal, what is the freezing point of a solution made by dissolving 39.338g of anthracene (C14H10) in 150.0mL of toluene? (Density of toluene = 0.8669g/mL)

Chemistry - DrBob222, Wednesday, January 30, 2013 at 10:38pm
mol anthracene = grams/molar mass
grams toluene = volume x density
molality = mol anthracene/kg toluene.
delta T = Kf*m. Solve for delta T.
Subtract from zero to find new freezing point.

Answer this Question

Related Questions

chemistry - Calculate the freezing point of 0.15 m calcium chloride aqueous ...
chemistry - A 0.750 g sample of an unknown substance is dissolved in 20.0 g of ...
chemistry - A 0.750 g sample of an unknown substance is dissolved in 20.0 g of ...
molal - the freezing point of ethanol (C2H5OH) is -114.6C. the molal freezing ...
molal - the freezing point of ethanol (C2H5OH) is -114.6C. the molal freezing ...
molal - the freezing point of ethanol (C2H5OH) is -114.6C. the molal freezing ...
chemistry - you are conducting a freezing-point determination in the laboratory ...
chem - freezing point - When 18 g of ethylene glycol C2H6O2 is dissolved in 150 ...
Chemistry - When 0.855 g of this solid was dissolved in 7.50 g of napthalene, ...
chemistry - The procedure described in this experiment was used to determine the...

For Further Reading

First Name:
School Subject:
Answer: