A solution of 10.41 g of anhydrous aluminum chloride (AICI3) in 53.70 g of water freezes at -10.82°C. Calculate the molar mass of AICI, from the formula. Calculate the molar mass from the freezing point depression, assuming AICI, does not dissociate in ions. g/mol Comparing the two values, how many ions will AICI, form?.. 1 g/mol 2 3 4

A solution of 10.41 g of anhydrous aluminum chloride (AICI3) in 53.70 g of water freezes at -10.82°C. Calculate the molar mass of AICI, from the formula. Calculate the molar mass from the freezing point depression, assuming AICI, does not dissociate in ions. g/mol Comparing the two values, how many ions will AICI, form?.. 1 g/mol 2 3 4

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...

See similar textbooks

Similar questions

At a particular temperature, the solubility of NO₂ in water is 0.0350 M when the partial pressure is 0.0800 atm. What will the solubility (in M) be when the partial pressure of NO₂ is 2.05 atm?
Calculate the vapor pressure of a solution at 20oC formed by dissolving 25 moles of glucose (C6H12O6) in 75 moles of water (Vapor Pressure of pure water at 20oC is 17.5 torr) 10.5 torr b. 13.1 torr 15.5 torr d. none of these
At a particular temperature, the solubility of O₂ in water is 0.0500 M when the partial pressure is 0.120 atm. What will the solubility (in M) be when the partial pressure of O₂ is 0.530 atm?
147.5 g of an unknown molecular compound is added to 500.0 mL of water. The freezing point of the solution is found to be -3.24 °C. What is the molar mass of the unknown compound? (K. of water is 1.86 °C/m.) g/mol
Alcohols are organic compounds which are soluble in water, but are nonelec- trolytes. If a 6.247 g sample of an alcohol is dissolved in 57.493 g of water, and a freezing point of -6.3°C is measured for the resulting solution, what is the molar mass of the alcohol? The freezing point depression constant of water is 1.86°C kg mol. mol-1
Vitamin K is involved in normal blood clotting. When 0.641 g of vitamin K is dissolved in 25.0 g of camphor, the freezing point of the solution is lowered by 2.15 °C. Look up the freezing point and K, constant for camphor in the Colligative Constants table. Calculate the molar mass of vitamin K. molar mass: g/mol
Calculate the freezing point of a solution of 1.82 g of NaCl in 152.2 g of water. Kf for water is 1.86°C/m and the freezing point of pure water is 0.0 °C. Assume that NaCl completely dissociates into its ions and its molar mass is 58.44 g/mol.
Please help
How much does the vapor pressure of water lower (dP) by dissolving 41.0 g NaOH in 60 moles of pure water. The vapor pressure of pure water at 25°C is 23.8 torr. Molar Mass NaOH is 40g/mol.
At a particular temperature, the solubility of O₂ in water is 0.0500 M when the partial pressure is 0.120 atm. What will the solubility (in M) be when the partial pressure of O₂ is 0.632 atm?
Using butanol (C4H9OH) rather than ethanol (C₂H5OH) as a gasoline additive has an advantage in providing a higher fuel value when mixed with octane. V At 20°C, the vapor pressure of butanol is 5.00 torr and the vapor pressure of octane is 10.0 torr. What is the vapor pressure at 20°C of a solution prepared by mixing 16.2 g of butanol and 127 g of octane? torr
Calculate the freezing point for a 2.50 M CaCl2 aqueous solution assuming ideal behavior. (Kf for water is 1.86ºC/m and the density of the solution is 1.21 g/mL. MWCaCl2 110.98 amu)