A lab technician determines the boiling point elevation of an aqueous solution of a nonvolatile, nonelectrolyte to be 1.62°C. What is the solution's molality?
delta T = Kb*molality
Solve for molality.
To determine the solution's molality, we can use the boiling point elevation equation:
ΔTb = Kb * m
Where:
ΔTb is the boiling point elevation
Kb is the molal boiling point elevation constant (a property dependent on the solvent)
m is the molality of the solute (moles of solute per kilograms of solvent)
In this case, we are given the boiling point elevation (ΔTb = 1.62°C) and need to find the molality (m).
First, we need to find the molal boiling point elevation constant (Kb) for the solvent. The Kb value depends on the solvent, so you need to consult a reference source or a data table to find the value for water.
Let's assume that the molal boiling point elevation constant (Kb) for water is 0.512 °C/m.
Now, we can rearrange the equation to solve for m:
m = ΔTb / Kb
Substituting the known values:
m = 1.62°C / 0.512 °C/m
m ≈ 3.17 mol/kg
Therefore, the solution's molality is approximately 3.17 mol/kg.