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Calculate the freezing point of a solution containing 0.402 moles of KCl and 3.300 kg of water. The molal-freezing-point-depression constant (Kf) for water is 1.86 ºC/m. (Note, KCl is an electrolyte, so assume comlete ion dissociation when dissolved).
A. -0.45 ºC
B. -10 ºC
C. 1.23 ºC
I keep getting .2266, please help!!
A solution is made by dissolving 21.5 grams of glucose (C6H12O6) in 255 grams of water. What is the freezing-point depression of the solvent if the freezing point constant is -1.86 °C/m? Show all of the work needed to solve this problem.