14. Solutions

How many moles of ethylene glycol, C₂H₆O₂, must be added to 1,000 g of water to form a solution that has a freezing point of –10ºC?

An ethylene glycol solution contains 28.3 g of ethylene glycol, C₂H₆O₂ in 97.2 mL of water. Calculate the freezing point of the solution. The density of water 1.00 g/mL.

When 825 g of an unknown is dissolved in 3.45 L of water, the freezing point of the solution is decreased by 2.89°C. Assuming that the unknown compound is a non-electrolyte, calculate its molar mass.

Determine the freezing point depression of a solution that contains 30.7 g glycerin (C₃H₈O₃, molar mass = 92.09 g/mol) in 376 ml of water. Some possibly useful constants for water are k_f = 1.86°C/m and k_b = 0.512°C/m.

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C₁₀H₈, molar mass = 128.16 g/mol) dissolved in 722 ml of benzene (d = 0.877 g/ml). pure benzene has a melting point of 5.50 °C and a freezing point depression constant of 4.90 °C/m.

What mass of glucose (C₆H₁₂O₆) should be dissolved in 12.0 kg of water to obtain a solution with a freezing point of -5.8^∘C?

Calculate the freezing point of a solution containing 1.25g of benzene in 100g of chloroform