Answer :
To find the boiling point of an aqueous solution of AlCl3 that has the same molality as the MgBr2 solution, we use the boiling point elevation formula and the given Kb for water, assuming the same molality as the MgBr2 solution. We should remember to add the resulting value to the boiling point of pure water.
The question relates to the concept of colligative properties in chemistry, which are properties of solutions that depend on the quantity, not the identity, of the solute particles.
Two such colligative properties are freezing point depression and boiling point elevation.
Freezing point depression occurs when a solute is added to a solvent, lowering its freezing point.
Boiling point elevation is the raising of a solvent's boiling point due to the addition of a solute.
In this case, an aqueous solution of MgBr2 was found to have a freezing point of -5.7°C, and you are being asked to calculate the boiling point of an aqueous solution of AlCl3 that has the same molality as the MgBr2 solution.
To find the boiling point of the solution, we need to apply the formula for boiling point elevation: ΔTb = m*Kb*i,
where
ΔTb is the change in boiling point,
m is the molality,
Kb is the elevation constant for water, and
i is the van't Hoff factor, which represents the number of particles a solute formula unit makes in solution.
In the case of AlCl3, i = 4.
Then substituting the given value of Kb for water (0.512 °C/m), and assuming the molality of AlCl3 is the same as the MgBr2 solution, we can compute the boiling point.
However, we also need to add the result to the boiling point of pure water (100°C) to get the boiling point of the solution.
Learn more about the topic of Boiling Point Elevation here:
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