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The equivalent (Eq or eq) is a reasonably common measurement unit used in chemistry and the biological sciences. It is a measure of a substance's ability to combine with other substances. It is frequently used in the context of normality.
Additional recommended knowledge
The equivalent is formally defined as the amount of a substance (moles) which will react with 6.022 x 1023 electrons. (This is Avogadro's Number, which is the number of particles in a mole).
Another, slightly less precise, definition describes the equivalent as the number of grams of a substance that will react with a gram of free hydrogen. (This is practically true, since a gram of hydrogen is very close to a mole of hydrogen, and free hydrogen has one spare electron; hence one gram of hydrogen is effectively equivalent to 6.022 x 1023 electrons.)
Hence, the amount of a given substance in equivalents is equal to the amount of the substance in moles divided by the valence of the substance.
Note that the equivalent weight is the mass of one equivalent of a substance.
In practice, the amount of a substance in equivalents often has a very small magnitude, so it is frequently described in terms of milliequivalents (mEq or meq) -- the prefix milli denoting that the measure is divided by 1000. Very often, the measure is used in terms of milliequivalents of solute per litre of solvent (mEq/L). This is especially common for measurement of compounds in biological fluids; for instance, the healthy level of potassium in the blood of a human is defined between 3.5 and 5.0 mEq/L.
Equivalents have advantage over moles in quantitative analysis of reactions. The best feature of using equivalents is that there is no need to study much about the nature of reaction, i.e. no need to analyse and balance chemical equations. Equivalents of reactants react in equal numbers to yield the equal equivalents of products.
Use in biochemistry and medicine
The composition of drug preparations, such as intravenous fluids, is usually stated in mmol/Litre rather than mEq/Litre. This is conceptually easier because the molarity refers to the number of dissolved particles, not the number of available charges. This simplifies understanding the composition of physiological solutions which contain the divalent ions Mg2+ and Ca2+.
|This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Equivalent_(chemistry)". A list of authors is available in Wikipedia.|