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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

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

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

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?

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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