General Chemistry Challenge Problem: Properties of Solution.
A 0.100 L solution is made by dissolving 0.441g of CaCl2 in water
A) Calculate the osmotic pressure of this solution at 27 degrees Celsius assuming that it is completely dissociated into its component ions.
B) The measured osmotic pressure of this solution is 2.56 atm at 27 degrees Celsius. Explain why it is less than the value calculated in A) and calculate the van't Hoff factor,i, for the solute in this solution.

Question

General Chemistry Challenge Problem: Properties of Solution.
A 0.100 L solution is made by dissolving 0.441g of CaCl2 in water
A) Calculate the osmotic pressure of this solution at 27 degrees Celsius assuming that it is completely dissociated into its component ions.
B) The measured osmotic pressure of this solution is 2.56 atm at 27 degrees Celsius. Explain why it is less than the value calculated in A) and calculate the van't Hoff factor,i, for the solute in this solution.

anonymous · Answer

C) The enthalpy of solution for CaCl2 is (Heat change=-81.3 kJ/mol. If the final temperature of the solution is 27 degrees Celsius, what was its initial temperature? (Assume that the density of the solution is 1.00 g/mL, that its specific heat is 4.18 J/g*K and that the solution loses no heat to its surrondings.

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