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A 1.60-g sample of a mixture of naphthalene (C10H8) and anthracene (C14H10) is dissolved in 20.0g benzene (C6H6). the freezing point of the solution is 2.81°C. What is the composition as a mass percent of the sample mixture? the freezing point of benzene is 5.51°C and KF is 5.12°C Kg/mol.

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Christian Tuso
Christian TusoLv10
18 Nov 2020

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Related questions

7.85 g of a compound with an unknown formula is dissolved in 300 g of benzene. The freezing point of the solution is 2.10 degrees celsius below that of pure benzene. What is the molar mass of the compound? (FP of pure benzene=5.51 degrees celsius; Kf(benzene)=5.12 degrees C/molal)

Please explain how you got your answer.

1. How many grams of ethylene glycol, C2H4(OH)2, are needed per kilogram of water to protect radiator fluid against freezing down to -10°C?

2. For benzene, C6H6, the freezing point constant, Kf, is 5.12 K oC/m and its normal freezing point is 5.5°C. What is the freezing point of a solution containing 100.0 g of benzene and 20.0 g of naphthalene (C10H8)?

3. When 5.0 g of an unknown substance is dissolved in 100.0 g of water, the freezing point of the solution decreases by 1.5°C. What is the molar mass of the unknown substance if the compound does not dissociate to form ions in solution?

4. If 2.00 moles of a substance is dissolved in 1.00 kg of water, the freezing point of the solution decreases by 7.44°C. Does this substance dissociate to form ions in solution? Explain why.

5. Calculate the freezing point of a 0.2 m CaCl2 aqueous solution, assuming it dissociates completely to form ions in solution.

Calculate the freezing point and boiling point of a solution containing 15.8 g of naphthalene (C10H8) in 115.0 mL of benzene. Benzene has a density of 0.877 g/cm3.

a. Calculate the freezing point of a solution. (Kf(benzene)=5.12∘C/m.)

b. Calculate the boiling point of a solution. (Kb(benzene)=2.53∘C/m.)

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