Normality: Difference between revisions
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imported>David E. Volk (New page: {{subpages}} In chemistry, '''normality''' (N) is a term used to indicate chemical concentrations that is typically only used for acid-base reactions. A 1 normal (1 N) solution...) |
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In [[chemistry]], '''normality''' (N) is a term used to indicate chemical concentrations that is typically only used for [[acid]]-[[base]] reactions. A 1 normal (1 N) solution of any acid can neutralize an equal volume of any 1 N base soltuion. | In [[chemistry]], '''normality''' (N) is a term used to indicate chemical concentrations that is typically only used for [[acid]]-[[base]] reactions. A 1 normal (1 N) solution of any acid can neutralize an equal volume of any 1 N base soltuion. A one liter volume of a 1 N acid solution will neutral 1 [[mole (unit)|mole]], or 6.23 * 10^23, hydroxide ions. Normality is always greater than or equal to the related concentration unit [[molarity]], such that | ||
:<math> \mathbf{N} = \mathbf{n} \times \mathbf{M} </math> | |||
where ''n'' is an integer greater than or equal to 1. | |||
For a monoprotic acid, 1M = 1N, while for diprotic and triprotic acids 1M = 2N and 1M = 3N, respectively. | |||
Revision as of 13:57, 20 June 2009
In chemistry, normality (N) is a term used to indicate chemical concentrations that is typically only used for acid-base reactions. A 1 normal (1 N) solution of any acid can neutralize an equal volume of any 1 N base soltuion. A one liter volume of a 1 N acid solution will neutral 1 mole, or 6.23 * 10^23, hydroxide ions. Normality is always greater than or equal to the related concentration unit molarity, such that
where n is an integer greater than or equal to 1.
For a monoprotic acid, 1M = 1N, while for diprotic and triprotic acids 1M = 2N and 1M = 3N, respectively.