A solution of 1.50 g of solute dissolved in 25.0 mL of H2O at 258C has a boiling point
Chapter 13, Problem 13.133(choose chapter or problem)
A solution of 1.50 g of solute dissolved in 25.0 mL of H2O at 258C has a boiling point of 100.458C. (a) What is the molar mass of the solute if it is a nonvolatile nonelectrolyte and the solution behaves ideally (d of H2O at 258C 5 0.997 g/mL)? (b) Conductivity measurements show that the solute is ionic with general formula AB2 or A2B. What is the molar mass if the solution behaves ideally? (c) Analysis indicates an empirical formula of CaN2O6. Explain the difference between the actual formula mass and that calculated from the boiling point elevation. (d) Find the vant Hoff factor (i) for this solution.
Unfortunately, we don't have that question answered yet. But you can get it answered in just 5 hours by Logging in or Becoming a subscriber.
Becoming a subscriber
Or look for another answer