Practice: What is the mass percent of NH3 of a 1.25 m aqueous solution of NH3?
Subjects
Sections | |||
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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 (IGNORE) |
Boiling Point Elevation |
Molality (m) represents the amount of solute dissolved per kilogram of solvent.
Example #1:
Molality is depicted as moles of solute per kilograms of solvent.
Concept #1: Ionic molality or osmolality represents the molality of dissolved ions in a solution.
Example #2:
A solution is prepared by dissolving 43.0 g potassium chlorate, KClO3, in enough water to make 100.0 mL of solution. If the density of the solution is 1.760 g/mL, what is the molality of KClO3 in the solution? MW of KClO3 is 122.55 g/mol.
Example #3:
If the molality of glucose, C6H12O6, in an aqueous solution is 2.56 what is the molarity? Density of the solution is 1.530 g/mL.
Example #4:
What is the ionic molality of nitrate ions in 0.305 m lead (IV) nitrate, Pb(NO3)4?.
Practice: What is the mass percent of NH3 of a 1.25 m aqueous solution of NH3?
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