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# Molality

See all sections
Sections
Solutions
Solubility and Intermolecular Forces
Solutions: Mass Percent
Percent Concentrations
Molarity
Osmolarity
Parts per Million (ppm)
Solubility: Temperature Effect
Intro to Henry's Law
Henry's Law Calculations
Dilutions
Solution Stoichiometry
Electrolytes (Simplified)
Equivalents
Molality
The Colligative Properties
Boiling Point Elevation
Freezing Point Depression
Osmosis
Osmotic Pressure

Molality (m) represents the amount of solute dissolved per kilogram of solvent.

###### Understanding Molality

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.

###### Molality Calculations

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?