What mass of ethylene glycol (C2H6O2, molar mass = 62.1 g/mol), the main component of antifreeze, must be added to 10 L of water to produce a solution for use in a car's radiator that freezes at -23.3°C? Assume the density of water is exactly 1 g/mL. {kf = 1.86°C/m} O a. 776 g O b. 7.76 kg O c. 129 g O d. 1.29 kg

A Pb-concentrated water sample contains 0.0011% Pb by mass. How much of the water (in mL) contains 150 mg of Pb? (Assume a density of 1.0 g/mL)

(Q65) Calculate the vapor pressure (in torr) at 30°C of a solution containing 155.1 grams of the nonelectrolyte glucose (C6H1206) dissolved in 821.4 grams of water. The vapor pressure of pure water at this temperature is 31.80 torr. (4 sf)

a.) Calculate the freezing point and boiling point of the solution when you add 1.00 kg of ethylene glycol (C2H6O2) antifreeze to 4450 g of water in your car’s radiator. Kb = 0.512C°/m; Kf = 1.86C°/mb.) Calculate the freezing point of a solution containing 50.0 g of NaCl in 5000 mL of water. Kf for water is 1.86 C˚/m c.) Calculate the molar mass of sucrose in a solution prepared by dissolving 4.27 grams glucose in 50.0 grams water. The solution boils at 100.13 °C which is above the normal boiling point of pure water. Kb = 0.512C°/m

A 83.5 g sample of a nonelectrolyte is dissolved in 250.1 g of water. The solution is determined to have a boiling point of 102.3 °C. What is the molar mass of the compound? (Kb for water is 0.510 °C/m).

The lattice energy for KF is 821 kJ/mol. The enthalpy of hydration for K+ is -336 kJ/mol and the enthalpy of hydration for F- is -431 kJ/mol. What is the enthalpy in kJ when 24.18 g of KF forms an aqueous solution? (Hint: start by finding the enthalpy of solution)

The boiling point of pure ethanol (C₂H₅OH, MM = 46.07 g/mol) is 78.4 °C. A solution is made using 100.0 g of ethanol (the solvent) and 29.1 g of glucose (MM = 180.16 g/mol). What is the boiling point of this solution, in °C? (Kb of ethanol is 1.22 °C/m)