The freezing point of pure benzene (C6H6) is 5.49 C. The freezing point of a solution made using toluene (C7H8) in benzene is determined to be -13.0 C. What is the molality of the toluene? (Kf benzene = 5.12 C/m)
Added by Abby
Step 1
ΔTf = Tf (pure benzene) - Tf (solution) = 5.49 C - (-13.0 C) = 18.49 C Show more…
Show all steps
Your feedback will help us improve your experience
David Collins and 85 other Chemistry 102 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
The freezing point of benzene (C6H6) is 5.50°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in benzene is DDT. How many grams of DDT, C14H9Cl5 (354.5 g/mol), must be dissolved in 207.0 grams of benzene to reduce the freezing point by 0.500°C? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Kb (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 ____g DDT.
Dinesh S.
Pure benzene has a boiling point of 80.1 °C and a freezing point of 5.5 °C. When a non-electrolyte solvent is dissolved in benzene, the freezing point of the solution is 3.6 °C. What is the boiling point of this solution? For benzene, Kf = 5.12 °C/molal and Kb = 2.53 °C/molal. Answer in °C.
Mahendra R.
Pure benzene, $\mathrm{C}_{6} \mathrm{H}_{6},$ freezes at $5.45^{\circ} \mathrm{C} .$ A solution containing 7.24 $\mathrm{g} \mathrm{C}_{2} \mathrm{Cl}_{4} \mathrm{H}_{2}$ in 115 g of benzene (specific gravity $=0.879$ ) freezes at $3.55^{\circ} \mathrm{C}$ . Based on these data, what is the molal freezing-point constant for benzene?
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD