Multiple Choice
Which of the following occurs during the process of freezing in terms of freezing point depression?
14. Solutions
Freezing Point Depression
Back14. Solutions
Freezing Point Depression
- Multiple Choice
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.
- Multiple ChoiceWhat is the effect of adding a solute to water on its freezing point?
- Multiple ChoiceCalculate the mass of KCl used to prepare a solution in 3.00 L of water with a freezing point of –1.20 °C. Assume that the density of water = 1.00 g/mL.
- Multiple ChoiceWhat happens to the volume of liquid water when it freezes?
- Multiple ChoiceHow can the freezing of water lead to the cracking of boulders?
- Multiple Choice
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?
- Multiple Choice
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.
- Open Question
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 kf = 1.86°C/m and kb = 0.512°C/m.
- Open Question
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.
- Open Question
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?
- Open Question
Calculate the freezing point of a solution containing 1.25g of benzene in 100g of chloroform
- Multiple ChoiceA glucose solution contains 55.8 g of glucose (C6H12O6) in 455 g of water. Determine the freezing point of the solution. The freezing point depression constant (Kf) for water is 1.86°C/m. What is the freezing point of the solution?
- Multiple ChoiceA solution containing 20.0 g of an unknown liquid and 110.0 g of water has a freezing point of -1.32 °C. Given Kf = 1.86 °C/m for water, the molar mass of the unknown liquid is ________ g/mol.
- Multiple ChoiceA solvent has a freezing point of 10.1°C and a freezing point depression constant of 6.16°C/m. If a solution, made by dissolving 1.218 g of an unknown solute into 25.0 g of the solvent, has a freezing point of 8.8°C, what is the molar mass of the solute?