Calculate the depression in freezing point of a 0.2 molal solution if kf for water is 1.86 K kg mol-1.
Added by Margaret F.
Step 1
2 mol/kg - Freezing point depression constant (\(K_f\)) for water = 1.86 K kg mol\(^{-1}\) Show more…
Show all steps
Your feedback will help us improve your experience
Sima Sarker and 92 other Chemistry 101 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
Determine the freezing point depression of a substance with molality of 0.18 mol/kg and kf = 6.8°C kg/mol.
Sima S.
Calculate the Freezing Point Depression (DT) for the following solution. (Assume the density of water is 1.00 g/mL and Kf = 1.86 Deg C/m) 28g of KCl in 1.9 L of water
Adi S.
Molal depression constant for a solvent is $4.0 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$. The depression in the freezing point of the solvent for $0.03 \mathrm{~mol} \mathrm{~kg}^{-1}$ solution $\mathrm{K}_{2} \mathrm{SO}_{4}$ is: (Assume complete dissociation of the electrolyte) (a) $0.18 \mathrm{~K}$ (b) $0.24 \mathrm{~K}$ (c) $0.12 \mathrm{~K}$ (d) $0.36 \mathrm{~K}$
Solutions
Topic 2 : Colligative Properties of Solutions
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD