Determination of the boiling point of 0.01m solution of aluminum chloride and barium chloride and sodium chloride?
To determine the boiling point of a 0.01M solution of aluminum chloride, barium chloride, and sodium chloride, you need to know the molal boiling point elevation constant (Kb) for each individual salt.
The boiling point elevation is a colligative property, meaning it depends on the number of solute particles in a solution, rather than the particular identity of the solute. In this case, the salts will dissociate into ions in solution, which will affect the boiling point.
The equation to calculate boiling point elevation is:
ΔTb = Kb * m
Where:
ΔTb = boiling point elevation
Kb = molal boiling point elevation constant
m = molality of the solution (moles of solute per kilogram of solvent)
The Kb values for aluminum chloride, barium chloride, and sodium chloride can be found in reference books or online databases.
Once you have the Kb values, you can calculate the boiling point elevation (ΔTb) for each salt using the given concentration of 0.01M (0.01 mol/L) and assuming the density of water as 1 g/mL.
Finally, add the calculated boiling point elevation to the normal boiling point of water (100°C or 212°F) to obtain the boiling point of each solution.