Assuming 100% dissociation, calculate the freezing point and boiling point of 2.96 m Na2SO4(aq).
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Solutions, Molarity and Intermolecular Forces | 7 mins | 0 completed | Learn |
Henry's Law | 20 mins | 0 completed | Learn Summary |
Calculate Molarity | 27 mins | 0 completed | Learn Summary |
Mass Percent | 10 mins | 0 completed | Learn |
Molality | 15 mins | 0 completed | Learn |
Mole Fraction | 14 mins | 0 completed | Learn |
The Colligative Properties | 45 mins | 0 completed | Learn |
Additional Practice |
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Making Solutions |
Freezing Point Depression |
Colloid |
Additional Guides |
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ppm |
The Freezing Point Depression |
Boiling Point Elevation |
Assuming 100% dissociation, calculate the freezing point and boiling point of 2.96 m Na2SO4(aq).
We’re being asked to determine the freezing point and boiling point of an aqueous Na2SO4 solution. Aqueous means that Na2SO4 was dissolved in water.
When calculating the freezing point of a solution, we’re going to use the Freezing Point Depression equation. On the other hand, when calculating for the boiling point of a solution we’re going to use the Boiling Point Elevation equation.
Freezing Point Depression:
∆Tf = change in freezing point = Tf pure solvent –Tf solution
Kf = freezing point depression constant
i = van' t Hoff factor of the solute = no. of ions
m = molality
Boiling Point Elevation:
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