Determine the boiling point of a solution formed by dissolving 0.593 moles of ethanol in 100.0 grams of water.(For water, K_b = 0.512°C/m)

Question

Quizplus · Accepted Answer

The boiling point elevation equation is ΔTb = Kbm, where ΔTb is the change in boiling point, Kb is the ebullioscopic constant of the solvent, and m is the molality of the solution.

First, we need to calculate the molality of the solution:

molality (m) = moles of solute / mass of solvent (kg)

We have 0.593 moles of ethanol and 0.100 kg (100.0 g) of water:

m = 0.593 mol / 0.100 kg = 5.93 mol/kg

Next, we can plug in the values into the boiling point elevation equation:

ΔTb = 0.512°C/m * 5.93 mol/kg = 3.04°C

This is the change in boiling point. To find the boiling point of the solution, we need to add this to the boiling point of pure water (which is 100°C at standard pressure):

Boiling point of solution = 100°C + 3.04°C = 103.04°C

Therefore, the answer is choice C.

Determine the Boiling Point of a Solution Formed by Dissolving