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?
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To determine the solution's molality, we need to use the formula for boiling point elevation:
ΔTb = Kb * m
Where:
ΔTb is the boiling point elevation
Kb is the molal boiling point elevation constant
m is the molality of the solution
We can rearrange the formula to solve for m:
m = ΔTb / Kb
In this case, we are given the boiling point elevation (ΔTb) as 1.95°C, but we need to find the molal boiling point elevation constant (Kb) for water.
The molal boiling point elevation constant for water is approximately 0.512°C/m.
Substituting the given values into the formula, we have:
m = 1.95°C / 0.512°C/m
Simplifying the equation gives:
m ≈ 3.80 m
Therefore, the solution's molality is approximately 3.80 m.