Suppose that you add 25.6 g of an unknown molecular compound to 0.250 kg of benzene, which has a Kf of 5.12 oC/m. With the added solute, you find that there is a freezing point depression of 2.64 oC compared to pure benzene. What is the molar mass (in g/mol) of the unknown compound?
(a) Suppose that you add 25.6 g of an unknown molecular compound to 0.250 kg of benzene, which has a
Kf of 5.12 oC/m. With the added solute, you find that there is a freezing point depression of 2.64 oC compared to pure benzene.
What is the molar mass (in g/mol) of the unknown compound?
(b) What is the freezing point (in degrees Celcius) of 3.77 kg of water if it contains 170.1 g of CaBr2 ? The freezing point depression constant for water is 1.86 oC/m and the molar mass of
CaBr2 is 199.89 g/mol.
(c) What mass, in grams, of NaCl needs to be added to 1.6 kg of water in order to create a solution with a freezing point of -6.0 °C? The freezing point depression constant of water is 1.86 ºC/m.
(d) What mass, in grams, of NaCl needs to be added to 1.6 kg of water in order to create a solution with a freezing point of -6.0 °C? The freezing point depression constant of water is 1.86 ºC/m.
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