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.

The molality of a solute is the number of moles of that solute divided by the weight of the solvent in kilograms