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13 Dec 2019

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!!

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Related questions

Calculate the freezing point of a solution containing 5.0 grams of KCl and 550.0 grams of water. The molal-freezing-point-depression constant (Kf) for water is 1.86 °C/m. (Assume 100 % dissociation)

Answers:

A. -0.45 °C

B. -0.23 °C

C. -1.23 °C

D. +0.23 °C

E. +0.45 °C

Calculate the freezing point of 0.15 m calcium chloride aqueous solution. Assume that the molal freezing point depression constant of water is 1.86 Kg/mol and that the freezing point of water is 0.00C

PLEASE SHOW YOUR WORK..

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1.) A protein solution containing 70.0 mg of the protein (dissolved in water) displays an osmotic pressure of 319.88 Pa at 310.15 K. If the volume of the protein solution is 20.0 mL, what is the molar mass of the protein?

2.) Calculate the osmotic pressure at 15°C of a solution of naphthalene (C10H8) in benzene containing 0.228 mol naphthalene per liter of solution.

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