Freezing point depression can be used to experimentally determine the molar mass of a solute in solution. Given the data in the table, please answer the questions below and determine the identi of an unknown alkali metal chloride compound. Mass of solvent (water) Mass of solution Boiling point of water Boiling point elevation constant (K) of water Boiling point of solution (a) What is the boiling point elevation, AT, of the solution? 4.0 °C (d) What is the unknown salt? OLICI (42.39 g/mol) O NaCl (58.44 g/mol) OKCI (74.55 g/mol) O RbCl (120.92 g/mol) (c) How many moles of the chloride salt are in the solution? 4.0✔✓ mol Experimental Results (b) What is the molality, m, of the solution? (Please check the alkali metal salt choices in part d to determine the van't Hoff factor.) 4.0✔✓ m 11.680 g 12.998 g 100.00°C 0.512°C/m 101.55°C

Freezing point depression can be used to experimentally determine the molar mass of a solute in solution. Given the data in the table, please answer the questions below and determine the identi of an unknown alkali metal chloride compound. Mass of solvent (water) Mass of solution Boiling point of water Boiling point elevation constant (K) of water Boiling point of solution (a) What is the boiling point elevation, AT, of the solution? 4.0 °C (d) What is the unknown salt? OLICI (42.39 g/mol) O NaCl (58.44 g/mol) OKCI (74.55 g/mol) O RbCl (120.92 g/mol) (c) How many moles of the chloride salt are in the solution? 4.0✔✓ mol Experimental Results (b) What is the molality, m, of the solution? (Please check the alkali metal salt choices in part d to determine the van't Hoff factor.) 4.0✔✓ m 11.680 g 12.998 g 100.00°C 0.512°C/m 101.55°C

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter10: Properties Of Solutions

Section: Chapter Questions

Problem 7RQ

See similar textbooks

Similar questions

An unknown compound contains only carbon, hydrogen, and oxygen. Combustion analysis of the compound gives mass percents of 31.57% C and 5.30% H. The molar mass is determined by measuring the freezing-point depression of an aqueous solution. A freezing point of 5.20C is recorded for a solution made by dissolving 10.56 g of the compound in 25.0 g water. Determine the empirical formula, molar mass, and molecular formula of the compound. Assume that the compound is a nonelectrolyte.
A gaseous solute dissolves in water. The solution process has H=15 kJ. Its solubility at 22C and 6.00 atm is 0.0300 M. Would you expect the solubility to be greater or less at (a) 22C and 1 atm? (a) 18C and 6 atm? (a) 15C and 10 atm? (a) 35C and 3 atm?
Distinguish between dispersion methods and condensation methods for preparing colloidal systems.
Vodka is advertised to be 80 proof. That means that the ethanol (C2H5OH) concentration is 40% (two significant figures) by volume. Assuming the density of the solution to be 1.0 g/mL, what is the freezing point of vodka? The density of ethanol is 0.789 g/mL.
The vapor pressure of an aqueous solution of urea. CH4N2O, is 291.2 mmHg at a measured temperature. The vapor pressure of pure water at that temperature is 355.1 mmHg. Calculate the mole fraction of each component.
A 12.0-g sample of a nonelectrolyte is dissolved in 80.0 g of water. The solution freezes at -1.94 C. Calculate the molar mass of the substance.