What would the boiling point of acetone increase by if 2.0 moles of glycerol were dissolved in 4.0 kg of acetone?

To determine how much the boiling point of acetone would increase when 2.0 moles of glycerol are dissolved in it, we can use the concept of boiling point elevation, which is governed by colligative properties. The formula to calculate the change in boiling point is given by:

ΔT_b = i * K_b * m

Where:

• ΔT_b is the boiling point elevation.

• i is the van 't Hoff factor, which is 1 for glycerol since it does not ionize.

• K_b is the ebullioscopic constant of the solvent (acetone in this case), which is specific to each solvent.

• m is the molality of the solution, defined as moles of solute per kilogram of solvent.

First, we need to calculate the molality (m):

m = moles of solute / kg of solvent = 2.0 moles / 4.0 kg = 0.50 mol/kg.

Next, we need the value of K_b for acetone, which is typically around 1.71 °C kg/mol.

Now, we can plug in these values into the boiling point elevation formula:

ΔT_b = i * K_b *