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?Which of the following aqueous solutions has (a) the higher boiling point, (b) the
Chapter 12, Problem 69P(choose chapter or problem)
Which of the following aqueous solutions has (a) the higher boiling point, (b) the higher freezing point, and (c) the lower vapor pressure: 0.35 m \(\mathrm{CaCl}_{2}\) or 0.90 m urea? Explain. Assume \(\mathrm{CaCl}_{2}\) to undergo complete dissociation.
Questions & Answers
QUESTION:
Which of the following aqueous solutions has (a) the higher boiling point, (b) the higher freezing point, and (c) the lower vapor pressure: 0.35 m \(\mathrm{CaCl}_{2}\) or 0.90 m urea? Explain. Assume \(\mathrm{CaCl}_{2}\) to undergo complete dissociation.
ANSWER:Step 1 of 2
We consider as a strong electrolyte and dissociates completely. This means that there is no ion pair and the van't Hoff factor is equal to 3. Thus, the total concentration of ion will be molal that is larger than the concentration of urea which is molal.