Must Know High School Chemistry by John T. Moore

Author:John T. Moore
Language: eng
Format: epub
Publisher: McGraw-Hill Education
Published: 2019-03-15T00:00:00+00:00

Molarity

In preparing a molar solution, the correct number of moles of solute (commonly converted to grams using the molar mass) is dissolved and diluted to the required volume.

While percentage concentration is common in everyday life, most chemists (and chemistry students) use molarity. Molarity (M) is the number of moles of solute per liter of solution:

M = mol solute/L solution

Refer back to Chapter 4 for problems related to molarity.

Molality

Molality (m) is the moles of solute per kilogram of solvent.

m = mol solute/kg solvent

Notice that it is kilograms of solvent, not solution. In the other concentration units, it has been the mass or volume of the entire solution. In molal solutions, it is the mass of the solvent only.

EXAMPLE

Ethylene glycol (C2H6O2) is in antifreeze. Determine the molality of ethylene glycol in a solution prepared by adding 31.0 g of ethylene glycol to 200.0 g of water.

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