Salt (chemistry)

This article is about the general chemical term salt. For the everyday meaning, see edible salt or its main ingredient, sodium chloride. For other meanings of the word salt, see salt (disambiguation).

A magnified crystal of a salt (halite/sodium chloride)

A salt, in chemistry, is any ionic compound composed of cations (positively charged ions) and anions (negative ions) so that the product is neutral (without a net charge). These component ions can be inorganic (Cl⁻) as well as organic (CH₃COO⁻) and monoatomic ions(F⁻) as well as polyatomic ions (SO₄²⁻); they are formed when acids and bases react.

There are several varieties of salts: Normal salts are those that do not contain a hydroxide ion (OH⁻) or a hydrogen ion (H⁺). Salts that contain a hydroxide ion are basic salts and salts that contain a hydrogen ion are acid salts. Impure salts is a name for salts which have lost their saltiness, and can also refer to natrons. Zwitterions are salts that contain an anionic center and a cationic center in the same molecule; examples include amino acids, many metabolites, peptides and proteins.

When salts are dissolved in water, they are called electrolytes, and are able to conduct electricity, a property that is shared with molten salts. Mixtures of many different ions in solution—like in the cytoplasm of cells, in blood, urine, plant saps and mineral waters— usually do not form defined salts after evaporation of the water. Therefore, their salt content is given for the respective ions.

Salts can be dehydrating to the human body if consumed in excess.

History

Main article: History of salt

The first registers of salt use were produced around 4000 B.C. in Egypt, and later in Greece and Rome. Salt was very valuable and used to preserve and flavor foods. In Ancient Rome, salt started to be used as money originating the current Latin-derivative term salary. Unfortunately for those paid with salt, it was easily ruined by rain and other factors. Payments to Roman workers were made in salt. Salt was also given to the parents of the groom in marriage until the 8th century.

From the Phoenicians dates the evidence of harvesting solid salt from the sea. They also exported it to other civilizations. As a result of the increased salt supply from the sea, the value of salt depreciated. The harvest method used was flooding plains of land with seawater, then leaving the plains to dry. After the water dried, the salt which was left was collected and sold.

Appearance

Table salt and peppercorns.

Salts are usually solid crystals with a relatively high melting point. However, there exist salts that are liquid at room temperature, so-called ionic liquids. Inorganic salts usually have a low hardness and a low compressibility, similar to edible salt.

Color

Salts can be clear and transparent (sodium chloride), opaque (titanium dioxide), and even metallic and lustrous (iron disulfide).

Salts exist in all different colors, e.g. yellow (sodium chromate), orange (potassium dichromate), red (mercury sulfide), mauve (cobalt chloride hexahydrate), blue (copper sulfate pentahydrate, ferric hexacyanoferrate), green (nickel oxide), colorless (magnesium sulfate), white (titanium dioxide), and black (manganese dioxide). Most minerals and inorganic pigments as well as many synthetic organic dyes are salts.

Taste

Different salts can elicit all five basic tastes, e.g. salty (sodium chloride), sweet (lead diacetate ), sour (potassium bitartrate), bitter (magnesium sulfate), and umami or savory (monosodium glutamate).

Odor

Pure salts are non-volatile and odorless, while impure salts may smell after the conjugate acid (e.g. acetates like acetic acid (vinegar) and cyanides like hydrogen cyanide (almonds) or the conjugate base (e.g. ammonium salts like ammonia) of the component ions.

Nomenclature

Various salt minerals

Chemical composition of sea salt

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 or acetate).

Common salt-forming cations include:

• ammonium NH₄⁺
• calcium Ca²⁺
• iron Fe²⁺ and Fe ³⁺
• magnesium Mg²⁺
• potassium K⁺
• pyridinium C₅H₅NH⁺
• quaternary ammonium NR₄⁺
• sodium Na⁺

Common salt-forming anions (and the name of the parent acids in parentheses) include:

• acetate CH₃COO⁻ (acetic acid)
• carbonate CO₃²⁻ (carbonic acid)
• chloride Cl⁻ (hydrochloric acid)
• citrate HOC(COO⁻)(CH₂COO⁻)₂ (citric acid)
• cyanide C≡N⁻ (hydrogen cyanide)
• hydroxide OH⁻ (water)
• nitrate NO₃⁻ (nitric acid)
• nitrite NO₂⁻ (nitrous acid)
• oxide O²⁻ (water)
• phosphate PO₄³⁻ (phosphoric acid)
• sulfate SO₄²⁻ (sulfuric acid)

Formation

Salts are formed by a chemical reaction between:

• A base and an acid, e.g. NH₃ + HCl → NH_4Cl.

• A metal and an acid, e.g. Mg + H₂SO₄ → MgSO₄ + H₂.

• A base and an acid anhydride, e.g. 2 NaOH + Cl_2O → 2 NaClO + H_2O

• An acid and an basic anhydride, e.g. 2 HNO₃ + Na_2O → 2 NaNO₃ + H_2O

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).

References

• Mark Kurlansky (2002). Salt: A World History. Walker Publishing Company. ISBN 0-14-200161-9.

See also

• Acid salt
• Electrolyte
• Halide
• Ionic bonds
• Kosher salt
• Natron
• Old Salt Route
• Salting the earth is the deliberate massive use of salt to render a soil unsuitable for cultivation and thus discourage habitation.
• Sodium
• Table salt
• Zwitterion
• Salinity
• hypertension

Salt is loved by many people, but it may cause diabeties. Someone died because of too much salt. RIP Sis. Lily.