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UNITS OF CONCENTRATION

UNITS OF CONCENTRATION There are a number of different ways of expressing solute CONCENTRATION that are commonly used. Some of these are listed below. Molarity, M = moles solute/liter of solution normality , N = equivalents of solute/liter of solution Weight %, Wt % = (mass of solute/mass of solution) x 100% Parts per million, ppm = (mass of solute/mass of solution) x 106 Mass per volume, mg/L = mass of solute/liter of solution molality, m = moles of solute/mass of solvent mole fraction, = moles of solute/total moles Concentrations expressed as ppm and N are less familiar to most students at this stage. Parts per million: The number of milligrams of solute per kg of solution = one ppm, since 1 mg = 10-3 g and 1 kg = 103 g. Assuming the density of water is g/mL, 1 liter of solution = 1 kg and hence, 1 mg/L = 1 ppm.

Normality is a somewhat dated concentration unit that is still encountered in may texts and lab manuals. It has advantages when carrying out titration calculations, however it can be confusing for the uninitiated. Normality is defined as the number of equivalents of solute per liter, and as such, is similar to Molarity.

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Concentrations expressed as ppm and N are less familiar to most students at this stage. Parts per million: The number of milligrams of solute per kg of solution = one ppm, since 1 mg = 10-3 g and 1 kg = 103 g. Assuming the density of water is 1.00 g/mL, 1 liter of solution = 1 kg and hence, 1 mg/L = 1 ppm.

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