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{{about|the term as used in chemistry|the chemistry of table salt|Sodium chloride}}
[[Image:Chalcanthite-cured.JPG|thumb|upright=1.5|The blue salt [[copper(II) sulfate]] in the form of the [[mineral]] [[chalcanthite]] ]]
In [[chemistry]], '''salts''' are [[ionic compound]]s that result from the [[neutralization (chemistry)|neutralization]] reaction of an [[acid]] and a [[Base (chemistry)|base]]. They are composed of an equal number of [[cation]]s (positively [[electric charge|charged]] ions) and [[anion]]s (negative ions) so that the product is electrically [[electric charge|neutral]] (without a net charge). These component ions can be [[inorganic compound|inorganic]] such as chloride (Cl<sup>−</sup>), as well as [[organic chemistry|organic]] such as [[acetate]] (CH<sub>3</sub>COO<sup>−</sup>) and [[monatomic ion]]s such as fluoride (F<sup>−</sup>), as well as [[polyatomic ion]]s such as [[sulfate]] (SO<sub>4</sub><sup>2−</sup>).
There are several varieties of salts. Salts that [[hydrolyze]] to produce [[hydroxide]] ions when dissolved in [[water]] are ''[[basic salts]]'' and salts that hydrolyze to produce [[hydronium]] ions in water are ''[[acid salt]]s''. ''Neutral salts'' are those that are neither acid nor basic salts. [[Zwitterion]]s contain an anionic center and a cationic center in the same [[molecule]] but are not considered to be salts. Examples include [[amino acid]]s, many [[metabolite]]s, [[peptide]]s, and [[proteins]].
[[Molten salt]]s and solutions containing dissolved salts (e.g., sodium chloride in water) are called [[electrolyte]]s, as they are able to [[Electrical conductor|conduct electricity]]. As observed in the [[cytoplasm]] of [[cell (biology)|cell]]s, in [[blood]], [[urine]], [[plant saps]] and [[mineral water]]s, mixtures of many different ions in solution usually do not form defined salts after evaporation of the water. Therefore, their salt content is given for the respective ions.
== Properties ==
=== Color ===
[[Image:Potassium-dichromate-sample.jpg|thumb|Potassium dichromate, a bright orange salt used as a pigment]]
Salts can appear to be clear and [[Transparency (optics)|transparent]] ([[sodium chloride]]), [[Opacity (optics)|opaque]], and even metallic and lustrous ([[pyrite|iron disulfide]]). In many cases the apparent [[Opacity (optics)|opacity]] or [[Transparency (optics)|transparency]] are only related to the difference in size of the individual [[monocrystal]]s. Since light reflects from the [[Crystallite|grain boundaries]] (boundaries between crystallites), larger [[crystal]]s tend to be transparent, while [[polycrystalline]] aggregates look like white powders.
Salts exist in many different [[color]]s, for example:
*yellow ([[sodium chromate]])
*orange ([[potassium dichromate]])
*red ([[potassium ferricyanide]])
*[[mauve]] ([[cobalt(II) chloride|cobalt chloride hexahydrate]])
*blue ([[copper(II) sulfate|copper sulfate]] pentahydrate, [[Prussian blue|ferric hexacyanoferrate]])
*purple ([[potassium permanganate]])
*green ([[nickel(II) chloride|nickel chloride]] hexahydrate)
*colorless ([[sodium chloride]], [[Magnesium sulfate|magnesium sulfate heptahydrate]])—may appear white when powdered or in small pieces
Most [[minerals]] and inorganic [[pigment]]s as well as many synthetic organic [[dye]]s are salts. The color of the specific salt is due to the presence of unpaired electrons in the d-orbital of transition elements.
=== Taste ===
Different salts can elicit all five [[basic taste]]s, e.g., salty ([[sodium chloride]]), sweet ([[lead diacetate]], which will cause [[lead poisoning]] if ingested), sour ([[potassium bitartrate]]), [[Bitter (taste)|bitter]] ([[magnesium sulfate]]), and [[umami]] or savory ([[monosodium glutamate]]).
=== Odor ===
Salts of strong acids and strong bases ("[[strong salts]]") are non-[[Volatility (chemistry)|volatile]] and odorless, whereas salts of either weak acids or weak bases ("[[weak salts]]") may smell after the [[conjugate acid]] (e.g., acetates like acetic acid ([[vinegar]]) and cyanides like [[hydrogen cyanide]] ([[almond]]s)) or the conjugate base (e.g., ammonium salts like [[ammonia]]) of the component ions. That slow, partial decomposition is usually accelerated by the presence of water, since [[hydrolysis]] is the other half of the [[reversible reaction]] equation of formation of [[weak salts]].
=== Solubility ===
{{see also|Solubility#Solubility of ionic compounds in water}}
Many ionic compounds can be [[Dissolution (chemistry)|dissolved]] in water or other similar solvents. The exact combination of ions involved makes each compound have a unique solubility in any solvent. The solubility is dependent upon how well each ion interacts with the solvent, so there are certain patterns. For example, all salts of [[sodium]], [[potassium]] and ammonium are soluble in water, as are all [[nitrates]] and many [[sulfate]] salts except barium sulfate, calcium sulfate (sparingly soluble) and Lead(2)sulfate However, ions that bind tightly to each other and form highly stable lattices would be less soluble, because it would be harder for these structures to break apart for the compounds to dissolve. For example, most [[carbonate]] salts are not soluble in water, such as [[lead carbonate]] and [[Barium carbonate]]
Soluble carbonate salts are:
[[Sodium carbonate]],
[[Potassium carbonate]] and
[[Ammonium carbonate]]
== Degenerationism ==
The name of a salt starts with the name of the cation (e.g., ''sodium'' or ''ammonium'') followed by the name of the anion (e.g., ''chloride'' or ''acetate''). Salts are often referred to only by the name of the cation (e.g., ''sodium salt'' or ''ammonium salt'') or by the name of the anion (e.g., ''chloride salt'' or ''acetate salt'').
Common salt-forming cations include:
* [[Ammonium]] NH<sub>4</sub><sup>+</sup>
* [[Calcium]] Ca<sup>2+</sup>
* [[Iron]] Fe<sup>2+</sup> and Fe<sup>3+</sup>
* [[Magnesium]] Mg<sup>2+</sup>
* [[Potassium]] K<sup>+</sup>
* [[Pyridinium]] C<sub>5</sub>H<sub>5</sub>NH<sup>+</sup>
* [[Quaternary ammonium cation|Quaternary ammonium]] NR<sub>4</sub><sup>+</sup>
* [[Sodium]] Na<sup>+</sup>
Common salt-forming anions (parent acids in parentheses where available) include:
* [[Acetate]] CH<sub>3</sub>COO<sup>−</sup> ([[acetic acid]])
* [[Carbonate]] CO<sub>3</sub><sup>2−</sup> ([[carbonic acid]])
* [[Chloride]] Cl<sup>−</sup> ([[hydrochloric acid]])
* [[Citrate]] HOC(COO<sup>−</sup>)(CH<sub>2</sub>COO<sup>−</sup>)<sub>2</sub> ([[citric acid]])
* [[Cyanide]] C≡N<sup>−</sup> ([[hydrocyanic acid]])
* [[Nitrate]] NO<sub>3</sub><sup>−</sup> ([[nitric acid]])
* [[Nitrite]] NO<sub>2</sub><sup>−</sup> ([[nitrous acid]])
* [[Phosphate]] PO<sub>4</sub><sup>3−</sup> ([[phosphoric acid]])
* [[Sulfate]] SO<sub>4</sub><sup>2−</sup> ([[sulfuric acid]])
== Formation ==
[[Image:Lead(II) sulfate.jpg|thumb|Solid lead(II) sulfate (PbSO<sub>4</sub>)]]
Salts are formed by a [[chemical reaction]] between:
* A [[base (chemistry)|base]] and an [[acid]], e.g., [[ammonia|NH<sub>3</sub>]] + [[hydrochloric acid|HCl]] → [[ammonium chloride|NH<sub>4</sub>Cl]]
* A [[metal]] and an [[acid]], e.g., [[magnesium|Mg]] + [[sulfuric acid|H<sub>2</sub>SO<sub>4</sub>]] → [[magnesium sulfate|MgSO<sub>4</sub>]] + [[hydrogen|H<sub>2</sub>]]
* A metal and a non-metal, e.g., [[calcium|Ca]] + [[chlorine|Cl<sub>2</sub>]] → [[calcium chloride|CaCl<sub>2</sub>]]
* A [[base (chemistry)|base]] and an [[Oxide|acid anhydride]], e.g., 2 [[Sodium Hydroxide|NaOH]] + [[Dichlorine monoxide|Cl<sub>2</sub>O]] → 2 [[Sodium hypochlorite|NaClO]] + [[Water|H<sub>2</sub>O]]
* An [[acid]] and a [[Oxide|basic anhydride]], e.g., 2 [[nitric acid|HNO<sub>3</sub>]] + [[Sodium oxide|Na<sub>2</sub>O]] → 2 [[Sodium nitrate|NaNO<sub>3</sub>]] + [[Water|H<sub>2</sub>O]]
* Salts can also form if solutions of different salts are mixed, their ions recombine, and the new salt is insoluble and precipitates (see: [[solubility equilibrium]]), for example:
*: Pb(NO<sub>3</sub>)<sub>2</sub>(aq) + Na<sub>2</sub>SO<sub>4</sub>(aq) → PbSO<sub>4</sub>(s) + 2 NaNO<sub>3</sub>(aq)
== See also ==
{{classic element}}
* [[Acid salt]] ''also known as'' Hydrogen salt
* [[Alkali salts]] ''also known as'' Basic salt
* [[Bresle method]]'' (The method used to test for salt presence during coating applications.)''
* [[Edible salt]]
* [[Electrolyte]]
* [[Fireworks#Pyrotechnic_compounds|Fireworks / Pyrotechnics]] '' (Salts are what give color to fireworks)''
* [[Halide]]
* [[Hypertension]]
* [[Ionic bond]]s
* [[Kosher salt]]
* [[Natron]]
* [[Old Salt Route]]
* [[Road salt]]
* [[Salinity]]
* [[Salting the earth]] ''(the deliberate massive use of salt to render a soil unsuitable for cultivation and thus discourage habitation)''
* [[Sea salt]]
* [[Sodium]]
* [[Table salt]]
* [[Zwitterion]]
== References ==
{{reflist}}
* [[Mark Kurlansky]] (2002). ''Salt: A World History''. Walker Publishing Company. ISBN 0-14-200161-9.
{{clear}}
[[Category:Chemical compounds]]
[[Category:Salts| ]]
[[Category:Alchemical substances]]
[[ar:ملح (كيمياء)]]
[[an:Sal (quimica)]]
[[az:Duzlar]]
[[zh-min-nan:Iâm (hoà-ha̍k)]]
[[be:Солі]]
[[be-x-old:Солі]]
[[bg:Сол]]
[[bs:Soli]]
[[ca:Sal (química)]]
[[cv:Тăвар]]
[[cs:Soli]]
[[cy:Halwyn]]
[[da:Salt]]
[[de:Salze]]
[[et:Soolad]]
[[el:Άλας]]
[[es:Sal (química)]]
[[eo:Salo]]
[[fa:املاح]]
[[hif:Nimak]]
[[fr:Sel (chimie)]]
[[gl:Sal (química)]]
[[ko:염]]
[[hy:Աղեր]]
[[hi:लवण]]
[[hr:Soli]]
[[id:Garam (kimia)]]
[[ia:Sal]]
[[is:Salt (efnafræði)]]
[[it:Sale]]
[[he:מלח (כימיה)]]
[[ka:მარილები]]
[[kk:Тұздар]]
[[sw:Chumvi]]
[[la:Sal]]
[[lv:Sāļi]]
[[lt:Druska]]
[[ln:Móngwa]]
[[jbo:silna]]
[[lmo:Saa]]
[[hu:Só]]
[[mk:Соли]]
[[ml:ലവണം]]
[[nl:Zouten]]
[[ja:塩 (化学)]]
[[no:Salt]]
[[nn:Salt]]
[[oc:Sal (quimia)]]
[[pnb:لون]]
[[nds:Solt]]
[[pl:Sole]]
[[pnt:Άλας]]
[[pt:Sal]]
[[ro:Sare (chimie)]]
[[qu:Kachi]]
[[rue:Солї]]
[[ru:Соли]]
[[sq:Kripërat]]
[[simple:Salt]]
[[sl:Sol (kemija)]]
[[sr:Со]]
[[sh:Sol]]
[[su:Uyah (kimia)]]
[[fi:Suola]]
[[sv:Salter]]
[[tl:Asin (kimika)]]
[[ta:உப்பு (வேதியியல்)]]
[[th:เกลือ (เคมี)]]
[[tr:Tuz (kimya)]]
[[uk:Солі (хімія)]]
[[ur:نمک (کیمیاء)]]
[[vi:Muối (hóa học)]]
[[fiu-vro:Soolaq]]
[[war:Asin (kimika)]]
[[yi:זאלץ]]
[[zh-yue:鹽]]
[[diq:Sole]]
[[zh:盐]]
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