A 1.60-g sample of a mixture of naphthalene () and anthracene () is dissolved in 20.0 g of benzene (). The freezing point of the solution is 2.81 ^oC. What is the composition, as mass percent, of the sample mixture? The freezing point of pure benzene is 5.51 ^oC and its cryoscopic constant (K_f) is 5.12 ^oC kg mol-1.

answer

watching

191

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Brian HingpitLv10

11 Dec 2020

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

What is the freezing point and boiling point of an aqueous solution with 0.050 m of ? The cryoscopic constant () of water is 1.853 ^oC kg mol^-1, while the ebullioscopic constant () of water is 0.512 ^oC kg mol^-1. The van't Hoff factor of is 2.7.

amethystcaribou176

) A solution is made from 87.3 of naphthalene (Molar mass 128.17 g/mol) and 3 liters of benzene (density 0.879 g/mL). For this problem you can conceder the naphthalene to be non-volatile. The temperature of the solution is 25 C.

a. What is the molality of this solution?

b. The Freezing point constant for benzene is Kf=5.12 C/m and its normal freezing point is 5.5 C, Whatâs the freezing point of the solution?

c. What/s the osmotic pressure of this solution, assuming that there is no change I volume of the benzene when the naphthalene is added?