Multiple Choice
Calculate 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.
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14. Solutions
Freezing Point Depression
Back14. Solutions
Freezing Point Depression
- Multiple ChoiceWhich of the following aqueous solutions has the lowest freezing point?25views
- Multiple ChoiceWhich of the following is a practical application of freezing point depression?50views
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- 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?
1518views7rank1comments - 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.
1251views3rank - 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.
903views - 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.
854views - 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?
1010views - Open Question
Calculate the freezing point of a solution containing 1.25g of benzene in 100g of chloroform
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