Problem: What is the boiling point of a 0.10 M solution of NaHSO4 if the solution has a density of 1.002 g/mL?

FREE Expert Solution

We’re being asked to determine the boiling point of a solution. The solution is composed of 0.10 M NaHSO4


Recall that the boiling point of a solution is higher than that of the pure solvent and the change in boiling point (ΔTb) is given by:


Tb=Tb, solution-Tb, pure solvent


The change in boiling point is also related to the molality of the solution:


Tb=iKbm

where: 

i = van’t Hoff factor

m = molality of the solution (in m or mol/kg)

Kb = boiling point elevation constant (in ˚C/m)


Recall that the molality of a solution is given by:


Molality(m)=moles of solutekg of solvent


And the molarity of a solution is given by:

Molarity (M)=moles of soluteLiter of solution


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Problem Details

What is the boiling point of a 0.10 M solution of NaHSO4 if the solution has a density of 1.002 g/mL?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Boiling Point Elevation concept. If you need more Boiling Point Elevation practice, you can also practice Boiling Point Elevation practice problems.