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A 0.100-L solution is made by dissolving 0.441 g of CaCl2(s) in water. (a) Calculate the osmotic pressure of this solution at27 °C, assuming that it is completely dissociated into its component ions. (b) The measured osmotic pressure of this solution is2.56 atm at 27 °C. Explain why it is less than the value calculated in (a), and calculate the van’t Hoff factor, i, for the solute inthis solution. (c) The enthalpy of solution for CaCl2 is ΔH = -81.3 kJ/mol. If the final temperature of the solution is 27 °C, whatwas 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 thatthe solution loses no heat to its surroundings.)

A 0.100-L solution is made by dissolving 0.441 g of CaCl2(s) in water. (a) Calculate the osmotic pressure of this solution at27 °C, assuming that it is completely dissociated into its component ions. (b) The measured osmotic pressure of this solution is2.56 atm at 27 °C. Explain why it is less than the value calculated in (a), and calculate the van’t Hoff factor, i, for the solute inthis solution. (c) The enthalpy of solution for CaCl2 is ΔH = -81.3 kJ/mol. If the final temperature of the solution is 27 °C, whatwas 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 thatthe solution loses no heat to its surroundings.)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A 0.100-L solution is made by dissolving 0.441 g of CaCl2(s) in water. (a) Calculate the osmotic pressure of this solution at
27 °C, assuming that it is completely dissociated into its component ions. (b) The measured osmotic pressure of this solution is
2.56 atm at 27 °C. 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. (c) The enthalpy of solution for CaCl2 is ΔH = -81.3 kJ/mol. If the final temperature of the solution is 27 °C, 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 surroundings.)

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