A solution of ethylene glycol in water at 20.0°C has a mass percent of 8.25% of...
A solution of ethylene glycol in water at 20 degrees celsius has a mass percent of 9.78% of ethylene glycol with a density of 1.0108 g/mL. The freezing point depression constant for water (solvent for all solutions) is Kf=-1.86 percent celsius kg/mol and the boiling point elevation constant is Kb=0.512 degrees celsius kg/mol. The density of neat water at 20.0 degrees celsius is 0.9982 g/mL. Answer the following: 1. What is the molarity of the solution? 2. What is the...
In an ethylene glycol-water solution, there are 20.0 g ethylene glycol for every 80.0 g water. This solution is used for filling a 450.0 gallon reservoir. Suppose the density of this mixture solution is ρ= 1.0529 g/ml. (a) What is the molarity of this solution? (b) If you need to fill the 450.0 gallon tank in 170.0 s, what is the volumetric flow rate of the solution into the tank? (c) How many moles of ethylene glycol are in the...
8. Ethylene glycol, HO-CH2-CH2-OH, a nonelectrolyte, is added to the water in a radiator to give a solution containing 515 g of ethylene glycol in 565 g of water. a. What is the molality of this solution? b. What is the boiling point of this solution? (Kb = 0.512 °C kg/mol for water)
What volume of ethylene glycol (HOCH2CH2OH, density = 1.12 g mL-1) must be added to 20.0 L of 112 of water (Kf = 1.86 °C kg mol-1) to produce a solution that freezes at -10 °C?
An aqueous antifreeze solution is 31.0 % ethylene glycol (C2 H4 O2) by mass. The density of the solution is 1.05 g/cm3. Calculate the molality, molarity and mole fraction of the ethylene glycol Molality mol/kg Molarity mol/L Mole fraction
[References] What volume of ethylene glycol (C2HO2), a nonelectrolyte, must be added to 12.0 L water to produce an antifreeze solution with a freezing point of-19.0°C? (The density of ethylene glycol is 1.11 g/cm°, and the density of water is 1.00 g/cm³. K, for water is 0.51°C•kg/mol and Kf is 1.86°C kg/mol.) Volume %3D What is the boiling point of this solution? Boiling point °C %3D 5 item attempts remaining Submit Answer Try Another Version [References] Consider an aqueous solution...
An ethylene glycol solution contains 27.6 g of ethylene glycol (C2H6O2) in 92.0 mL of water. (Assume a density of 1.00 g/mL for water.) Determine the freezing point of the solution. Determine the boiling point of the solution.
Antifreeze is an 50% by mass aqueous solution of the non-electrolyte ethylene glycol (C2H6O2). What is the freezing point of this solution? The Kf for water is 1.86oC∙kg∙mol−1 and assume a density of 1.00g/mL.
An ethylene glycol solution contains 24.4 g of ethylene glycol (C2H6O2) in 85.4 mL of water. (Assume a density of 1.00 g/mL for water.) 1.Determine the freezing point of the solution. 2.Determine the boiling point of the solution.
The liquid in automobile cooling systems is prepared by dissolving ethylene glycol (HOCH_2CH_2OH) in water. Ethylene glycol has a molar mass of 62. 07 g/mol and a density 1. 115 g/ml at 50. 0 degree C. Calculate the vapor pressure at 50 degree C of a coolant solution that is 51. 0: 49. 0 ethylene glycol to water by volume At 50. 0degree C the density of water is 0. 9880 g/ml, and its vapor pressure is 92 torr. The...