Answer:
0.312 °C
Explanation:
When a solvent dissolves a nonvolatile solute, its boiling point increases, because of the interactions between solvent and solute (or solutes) difficulties the vaporization. This phenomenon is a colligative property and is called ebullioscopy. The variation in the temperature (the boiling point elevation) is determined by:
ΔT = Kb*W*i
Where Kb is the ebullioscopic constant (0.52°C/m for water), W is the molality (number of moles of solute/mass of solvent in kg), and i is the van't Hoff factor, which is a measure of the dissociation of the solutes. If the dissociation is complete, i = 1.
Because there are 3 solutes, the molality will be the sum of the number of moles of them divided by the mass of water:
W = (0.010 + 0.020 + 0.030)/0.100
W = 0.600 m
ΔT = 0.52*0.600*1
ΔT = 0.312 °C
