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?
dT = Kb*m
1.62 = 0.51*m
Solve for m.
To find the solution's molality, we can use the formula:
ΔTb = Kb * m
Where:
- ΔTb is the boiling point elevation (1.62°C in this case),
- Kb is the molal boiling point constant for the solvent (water in this case),
- m is the molality of the solution (what we're looking for).
To solve the equation, we need to know the molal boiling point constant (Kb) for water. The Kb for water is 0.512°C/m.
Now we can plug in the values and solve for m:
1.62°C = 0.512°C/m * m
Divide both sides of the equation by 0.512°C:
1.62°C / 0.512°C = m
m ≈ 3.164 mol/kg
So, the solution's molality is approximately 3.164 mol/kg.