Calculate the boiling point elevation of 0.100 kg of water containing 0.010 mol of NaCl, 0.020 mol of Na2SO4, and 0.030 mol of MgCl2, assuming complete dissociation of these electrolytes.

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