Multiple Choice
If 29.5g of sodium phosphate (Na3PO4) is dissolved in 500.0g of water, what is the boiling point of this solution? Assume the boiling point elevation constant (Kb) for water is 0.512 °C/m and the molar mass of Na3PO4 is 163.94 g/mol.
14. Solutions
Boiling Point Elevation
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What is the boiling point of a solution that contains 50.0 g of FeBr3 in 200.0 g of water, given that the boiling point elevation constant (Kb) for water is 0.512 °C/m?
A
103.0 °C
B
101.5 °C
C
100.0 °C
D
102.0 °C
Verified step by step guidance1
Calculate the molar mass of FeBr3 by adding the atomic masses of one iron (Fe) atom and three bromine (Br) atoms.
Determine the number of moles of FeBr3 by dividing the mass of FeBr3 (50.0 g) by its molar mass.
Calculate the molality of the solution by dividing the moles of FeBr3 by the mass of water in kilograms (200.0 g of water is 0.200 kg).
Use the boiling point elevation formula: ΔT = i * Kb * m, where ΔT is the boiling point elevation, i is the van't Hoff factor (which is 4 for FeBr3 as it dissociates into 4 ions: 1 Fe^3+ and 3 Br^-), Kb is the boiling point elevation constant, and m is the molality.
Add the boiling point elevation (ΔT) to the normal boiling point of water (100.0 °C) to find the boiling point of the solution.
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