Practice: Calculate mole fraction of a 2.4 m aqueous solution of citric acid (C6H8O7).
Subjects
| Sections | |||
|---|---|---|---|
| Solutions: Solubility and Intermolecular Forces | 18 mins | 0 completed | Learn |
| Molality | 15 mins | 0 completed | Learn |
| Parts per Million (ppm) | 13 mins | 0 completed | Learn Summary |
| Mole Fraction | 7 mins | 0 completed | Learn |
| Solutions: Mass Percent | 11 mins | 0 completed | Learn |
| Types of Aqueous Solutions | 5 mins | 0 completed | Learn |
| Intro to Henry's Law | 4 mins | 0 completed | Learn Summary |
| Henry's Law Calculations | 13 mins | 0 completed | Learn |
| The Colligative Properties | 15 mins | 0 completed | Learn |
| Boiling Point Elevation | 16 mins | 0 completed | Learn Summary |
| Freezing Point Depression | 11 mins | 0 completed | Learn Summary |
| Osmosis | 15 mins | 0 completed | Learn |
| Osmotic Pressure | 9 mins | 0 completed | Learn |
| Vapor Pressure Lowering (Raoult's Law) | 17 mins | 0 completed | Learn |
| Additional Guides |
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| The Freezing Point Depression (IGNORE) |
Mole Fraction (X) relates the moles of solute and solvent within a solution.
Concept #1: Mole Fraction (X)
Example #1: A solution contains 85.2 g of ascorbic acid (C6H8O6), a water soluble vitamin, in 270.0 g of water. Calculate the mole fraction of ascorbic acid in this solution.
Practice: Calculate mole fraction of a 2.4 m aqueous solution of citric acid (C6H8O7).
Practice: If mole fraction of urea is 4.55 × 10–1, what is the mass of urea needed to prepare 38.0 g of solution in water?
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