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A solution was prepared by dissolving 1.664 g of a salt into 25.000 g of water. It was observed that the
solution temperature decreases when the salt dissolved. The solution was then put into an ice bath and the
freezing point of the solution was found to be 1.8 °C lower than the freezing point of pure solvent (water).
1. Assuming the salt has a molar mass of 118 g/mol, what is the molality of the solution formed?
m
2. Using the answer to question 1, and the magnitude of the decrease in the freezing point, what is the
value of the van't Hoff factor, i, for this solution? For water: K₁ =1.86 °C kg mol-1
3. When the solution was initially made by adding the salt to the water, the temperature of the solution
was observed to decrease. This allows us to conclude that ΔH for the solution process is
Ogreater than zero
O equal to zero
Oless than zero
4. Since the solid actually did dissolve in the water, we can conclude that the solution process for this
reaction is
O not spontaneous
O spontaneous
5. Using the answers to questions 3 and 4, what can we conclude about ΔS for the solution process?
It is equal to zero
It could be either positive or negative
It is positive
It is negative
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