A lab technician determines the boiling point elevation of an aqueous solution of a nonvolatile, nonelectrolyte to be 1.95°C. What is the solution's molality?
delta T = Kb*m
delta T os 1.95
Kb for water is 0.512
solve for m.
for which of the following liquids the molecular weight can be determined by the method dumas :glycerin - benzen -dichloromethane
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?
To find the solution's molality, we need to use the equation for boiling point elevation (ΔTb):
ΔTb = Kbm
Where:
ΔTb is the boiling point elevation
Kb is the molal boiling point elevation constant for the solvent
m is the molality of the solute
Given that the boiling point elevation is 1.95°C and assuming water as the solvent, we need to find the molal boiling point elevation constant (Kb) for water.
The molal boiling point elevation constant (Kb) for water is 0.512 °C/m.
Now we can rearrange the equation and solve for the molality (m):
m = ΔTb / (Kb)
Plugging in the values:
m = 1.95°C / 0.512 °C/m
m ≈ 3.80 mol/kg
Therefore, the solution's molality is approximately 3.80 mol/kg.