Experimentally Determining the Freezing Point of Water

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SUMMARY

The discussion focuses on determining the freezing point of a solution made from 50 g of water and 50 g of ethylene glycol (HO-CH2-CH2-OH). The freezing point depression formula, ΔT = Kf × molality, is essential for calculating the new freezing point, where Kf is the cryoscopic constant for water. The freezing point of pure water is confirmed to be experimentally determined rather than assumed to be 0 degrees Celsius due to variations in purity and atmospheric pressure affecting the measurement.

PREREQUISITES
  • Understanding of freezing point depression and colligative properties
  • Familiarity with the formula ΔT = Kf × molality
  • Knowledge of the Van't Hoff factor in solution chemistry
  • Basic concepts of molality and solution preparation
NEXT STEPS
  • Research the cryoscopic constant (Kf) for various solvents
  • Learn about the Van't Hoff factor and its application in colligative properties
  • Explore experimental methods for determining freezing points of solutions
  • Investigate the effects of solute purity on freezing point measurements
USEFUL FOR

Chemistry students, laboratory technicians, and anyone involved in experimental physical chemistry or solution chemistry.

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Homework Statement



1.Antifreeze used in your car is ethylene glycol, HO-CH2-CH2-OH. It is usually diluted 1:1. Assume that you made a solution of 50 g of water (solvent) and 50 g of ethylene glycol (solute). What temperature in Celsius would your car be protected to in cold weather? Assume the freezing point of pure water is 0 degrees Celsius.

2.Why is the freezing point of pure water determined experimentally instead of just assuming tha it is 0 degrees Celsius?


Homework Equations


Do i use the formula, delta T = (Kf)(molality)?
 
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Yes for question number one , were you asked to incorporate the Van't Hoff factor?
 
it doesn't say.
 

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