For an aqueous solution of HF, determine the van't Hoff factor assuming 0% ionization. i = For the same solution, determine the van't Hoff factor assuming 100% ionization. i = A solution is made by dissolving 0.0400 mol HF in 1.00 kg of water. The solution was found to freeze at -0.0844 °C. Calculate the value of i and estimate the percent ionization of HF in this solution.

For an aqueous solution of HF, determine the van't Hoff factor assuming 0% ionization. i = For the same solution, determine the van't Hoff factor assuming 100% ionization. i = A solution is made by dissolving 0.0400 mol HF in 1.00 kg of water. The solution was found to freeze at -0.0844 °C. Calculate the value of i and estimate the percent ionization of HF in this solution.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter13: The Chemistry Of Solutes And Solutions

Section: Chapter Questions

Problem 64QRT

See similar textbooks

Similar questions

The freezing point of 0.109 m aqueous formic acid is 0.210C. Formic acid, HCHO2, is partially dissociated according to the equation HCHO2(aq)H+(aq)+CHO2(aq) Calculate the percentage of HCHO2 molecules that are dissociated, assuming the equation for the freezing-point depression holds for the total concentration of molecules and ions in the solution.
The freezing point of a 0.031-m solution of copper(II) sulfate in water is 0.075 C. (a) Calculate the vant Hoff factor, i, for this solution. (b) Would the vant Hoff factor be larger, smaller, or the same for a 0.050-m solution of this compound?
A 0.109 mol/kg aqueous solution of formic acid, HCOOH, freezes at −0.210 °C. Calculate the percent dissociation of formic acid.
The vapor pressures of several solutions of water-propanol (CH3CH2CH2OH) were determined at various compositions, with the following data collected at 45C: H2O Vapor pressure(torr) 0 74.0 0.15 77.3 0.37 80.2 0.54 81.6 0.69 80.6 0.83 78.2 1.00 71.9 a. Are solutions of water and propanol ideal? Explain. b. Predict the sign of Hsoln for water-propanol solutions. c. Are the interactive forces between propanol and water molecules weaker than, stronger than, or equal to the interactive forces between the pure substances? Explain. d. Which of the solutions in the data would have the lowest normal boiling point?
Water at 25 C has a density of 0.997 g/cm3. Calculate the molality and molarity of pure water at this temperature.