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In [[chemistry]], the '''equivalent concentration''' or '''normality''' of a solution is defined as the [[molar concentration]] <math>c_i</math> divided by an equivalence factor <math>f_\mathrm{eq}</math>: | |||
:Normality <math> = \frac {c_i}{f_\mathrm{eq}}</math> | |||
== Units == | |||
The unit symbol "N" is used to denote "Eq/L" (Equivalent per liter) which is normality. Although losing favor, medical reporting of serum concentrations in "mEq/L" (=0.001 N) still occurs. | |||
== Usage == | |||
There are three common areas where normality is used as a measure of reactive species in solution: | |||
*In acid-base chemistry, normality is used to express the concentration of protons (H<sup>+</sup>) or hydroxide ions (OH<sup>−</sup>) in a solution. Here, <math>1/f_\mathrm{eq}</math> is an [[integer]] value. Each solute can produce one or more equivalents of reactive species when dissolved. | |||
*In [[redox]] reactions, the equivalence factor describes the number of [[electron]]s that an oxidizing or reducing agent can accept or donate. Here, <math>1/f_\mathrm{eq}</math> can have a fractional (non-integer) value. | |||
*In [[Precipitation (chemistry)|precipitation]] reactions, the equivalence factor measures the number of ions which will precipitate in a given reaction. Here, <math>1/f_\mathrm{eq}</math> is an integer value. | |||
Normal concentration of an ionic solution is intrinsically connected to the [[conductivity (electrolytic)]] through the equivalent conductivity. | |||
== Examples == | |||
Normality can be used for acid-base titrations. For example, [[sulfuric acid]] (H<sub>2</sub>SO<sub>4</sub>) is a [[diprotic acid]]. Since only 0.5 mol of H<sub>2</sub>SO<sub>4</sub> are needed to neutralize 1 mol of OH<sup>-</sup>, the equivalence factor is: | |||
:<math>f_\mathrm{eq}</math>(H<sub>2</sub>SO<sub>4</sub>) = 0.5 | |||
If the concentration of a sulfuric acid solution is ''c''(H<sub>2</sub>SO<sub>4</sub>) = 1 mol/L, then its normality is 2 N. It can also be called a "2 normal" solution. | |||
Similarly, for a solution with c(H<sub>3</sub>PO<sub>4</sub>) = 1 mol/L, the normality is 3 N because [[phosphoric acid]] contains 3 acidic H atoms. | |||
== Criticism == | |||
Normality is an ambiguous measure of the [[concentration]] of a solution. It needs a definition of the equivalence factor, which depends on the definition of [[Equivalent (chemistry)|equivalents]]. The same solution can possess ''different'' normalities for ''different'' reactions. The definition of the equivalence factor varies depending on the type of chemical reaction that is discussed: It may refer to equations, bases, redox species, precipitating ions, or isotopes. For example, a solution of MgCl<sub>2</sup> that is 2 N with respect to a Cl<sup>−</sup> ion, is only 1 N with respect to an Mg<sup>2+</sup> ion. Since <math>f_\mathrm{eq}</math> may not be unequivocal, [[IUPAC]] and [[NIST]] discourage the use of normality.<ref>http://old.iupac.org/publications/analytical_compendium/Cha06sec3.pdf</ref> | |||
== References == | |||
{{reflist}} | |||
{{Chemical solutions}} | |||
{{DEFAULTSORT:Normality (Chemistry)}} | |||
[[Category:Analytical chemistry]] | |||
[[Category:Chemical properties]] | |||
Revision as of 05:42, 17 October 2013
In chemistry, the equivalent concentration or normality of a solution is defined as the molar concentration divided by an equivalence factor :
Units
The unit symbol "N" is used to denote "Eq/L" (Equivalent per liter) which is normality. Although losing favor, medical reporting of serum concentrations in "mEq/L" (=0.001 N) still occurs.
Usage
There are three common areas where normality is used as a measure of reactive species in solution:
- In acid-base chemistry, normality is used to express the concentration of protons (H+) or hydroxide ions (OH−) in a solution. Here, is an integer value. Each solute can produce one or more equivalents of reactive species when dissolved.
- In redox reactions, the equivalence factor describes the number of electrons that an oxidizing or reducing agent can accept or donate. Here, can have a fractional (non-integer) value.
- In precipitation reactions, the equivalence factor measures the number of ions which will precipitate in a given reaction. Here, is an integer value.
Normal concentration of an ionic solution is intrinsically connected to the conductivity (electrolytic) through the equivalent conductivity.
Examples
Normality can be used for acid-base titrations. For example, sulfuric acid (H2SO4) is a diprotic acid. Since only 0.5 mol of H2SO4 are needed to neutralize 1 mol of OH-, the equivalence factor is:
If the concentration of a sulfuric acid solution is c(H2SO4) = 1 mol/L, then its normality is 2 N. It can also be called a "2 normal" solution.
Similarly, for a solution with c(H3PO4) = 1 mol/L, the normality is 3 N because phosphoric acid contains 3 acidic H atoms.
Criticism
Normality is an ambiguous measure of the concentration of a solution. It needs a definition of the equivalence factor, which depends on the definition of equivalents. The same solution can possess different normalities for different reactions. The definition of the equivalence factor varies depending on the type of chemical reaction that is discussed: It may refer to equations, bases, redox species, precipitating ions, or isotopes. For example, a solution of MgCl2 that is 2 N with respect to a Cl− ion, is only 1 N with respect to an Mg2+ ion. Since may not be unequivocal, IUPAC and NIST discourage the use of normality.[1]
References
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