Salt (chemistry)

In chemistry, a salt is a chemical compound consisting of an ionic assembly of positively charged cations and negatively charged anions, which results in a compound with no net electric charge.[1] A common example is table salt, with positively charged sodium ions and negatively charged chloride ions.

The component ions in a salt compound can be either inorganic, such as chloride (Cl⁻), or organic, such as acetate (CH
₃CO⁻
₂). Each ion can be either monatomic, such as fluoride (F⁻), or polyatomic, such as sulfate (SO²⁻
₄).

Types of salt

Salts can be classified in a variety of ways. Salts that produce hydroxide ions when dissolved in water are called alkali salts and salts that produce hydrogen ions when dissolved in water are called acid salts. Neutral salts are those salts that are neither acidic nor basic. Zwitterions contain an anionic and a cationic centre in the same molecule, but are not considered salts. Examples of zwitterions are amino acids, many metabolites, peptides, and proteins.[2]

Properties

BMIM⁺PF₆⁻, an ionic liquid

Color

Solid salts tend to be transparent, as illustrated by sodium chloride. In many cases, the apparent opacity or transparency are only related to the difference in size of the individual monocrystals. Since light reflects from the grain boundaries (boundaries between crystallites), larger crystals tend to be transparent, while the polycrystalline aggregates look like opaque powders or masses.

Salts exist in many different colors, which arise either from their constituent anions, cations or solvates. For example:

sodium chromate is made yellow by the chromate ion
potassium dichromate is made orange by the dichromate ion
cobalt nitrate is made red by the chromophore of hydrated cobalt(II) ([Co(H₂O)₆]²⁺).
copper sulfate is made blue by the copper(II) chromophore
potassium permanganate is made violet by the permanganate anion.
nickel chloride is typically made green by the hydrated nickel(II) chloride [NiCl₂(H₂O)₄]
sodium chloride, magnesium sulfate heptahydrate appear colorless or white because the constituent cations and anions do not absorb light in the part of the spectrum that is visible to humans.

Few minerals are salts, because they would be solubilized by water. Similarly, inorganic pigments tend not to be salts, because insolubility is required for fastness. Some organic dyes are salts, but they are virtually insoluble in water.

Taste

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

Odor

Salts of strong acids and strong bases ("strong salts") are non-volatile and often odorless, whereas salts of either weak acids or weak bases ("weak salts") may smell like 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. 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

Many ionic compounds exhibit significant solubility in water or other polar solvents. Unlike molecular compounds, salts dissociate in solution into anionic and cationic components. The lattice energy, the cohesive forces between these ions within a solid, determines the solubility. The solubility is dependent on how well each ion interacts with the solvent, so certain patterns become apparent. For example, salts of sodium, potassium and ammonium are usually soluble in water. Notable exceptions include ammonium hexachloroplatinate and potassium cobaltinitrite. Most nitrates and many sulfates are water-soluble. Exceptions include barium sulfate, calcium sulfate (sparingly soluble), and lead(II) sulfate, where the 2+/2− pairing leads to high lattice energies. For similar reasons, most metal carbonates are not soluble in water. Some soluble carbonate salts are: sodium carbonate, potassium carbonate and ammonium carbonate.

Conductivity

Edge-on view of portion of crystal structure of hexamethyleneTTF/TCNQ charge transfer salt.[3]

Salts are characteristically insulators. Molten salts or solutions of salts conduct electricity. For this reason, liquified (molten) salts and solutions containing dissolved salts (e.g., sodium chloride in water) can be used as electrolytes.

Melting point

Salts characteristically have high melting points. For example, sodium chloride melts at 801 °C. Some salts with low lattice energies are liquid at or near room temperature. These include molten salts, which are usually mixtures of salts, and ionic liquids, which usually contain organic cations. These liquids exhibit unusual properties as solvents.

Nomenclature

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⁺
₄
Calcium Ca²⁺
Iron Fe²⁺
and Fe³⁺
Magnesium Mg²⁺
Potassium K⁺
Pyridinium C
₅H
₅NH⁺
Quaternary ammonium NR⁺
₄, R being an alkyl group or an aryl group
Sodium Na⁺
Copper Cu²⁺

Common salt-forming anions (parent acids in parentheses where available) include:

Acetate CH
₃COO⁻
(acetic acid)
Carbonate CO²⁻
₃ (carbonic acid)
Chloride Cl⁻
(hydrochloric acid)
Citrate HOC(COO⁻
)(CH
₂COO⁻
)
₂ (citric acid)
Cyanide C≡N⁻
(hydrocyanic acid)
Fluoride F⁻
(hydrofluoric acid)
Nitrate NO⁻
₃ (nitric acid)
Nitrite NO⁻
₂ (nitrous acid)
Oxide O²⁻
(water)
Phosphate PO³⁻
₄ (phosphoric acid)
Sulfate SO²⁻
₄ (sulfuric acid)

Salts with varying number of hydrogen atoms replaced by cations as compared to their parent acid can be referred to as monobasic, dibasic, or tribasic, identifying that one, two, or three hydrogen atoms have been replaced; polybasic salts refer to those with more than one hydrogen atom replaced. Examples include:

Sodium phosphate monobasic (NaH₂PO₄)
Sodium phosphate dibasic (Na₂HPO₄)
Sodium phosphate tribasic (Na₃PO₄)

Formation

Solid lead(II) sulfate (PbSO₄)

Salts are formed by a chemical reaction between:

A base and an acid, e.g., NH₃ + HCl → NH₄Cl
A metal and an acid, e.g., Mg + H₂SO₄ → MgSO₄ + H₂
A metal and a non-metal, e.g., Ca + Cl₂ → CaCl₂
A base and an acid anhydride, e.g., 2 NaOH + Cl₂O → 2 NaClO + H₂O
An acid and a base anhydride, e.g., 2 HNO₃ + Na₂O → 2 NaNO₃ + H₂O
In the salt metathesis reaction where two different salts are mixed in water, their ions recombine, and the new salt is insoluble and precipitates. For example:
Pb(NO₃)₂ + Na₂SO₄ → PbSO₄↓ + 2 NaNO₃

Strong salt

Strong salts or strong electrolyte salts are chemical salts composed of strong electrolytes. These ionic compounds dissociate completely in water. They are generally odorless and nonvolatile.

Strong salts start with Na__, K__, NH₄__, or they end with __NO₃, __ClO₄, or __CH₃COO. Most group 1 and 2 metals form strong salts. Strong salts are especially useful when creating conductive compounds as their constituent ions allow for greater conductivity.[4]

Weak salt

Weak salts or "weak electrolyte salts" are, as the name suggests, composed of weak electrolytes. They are generally more volatile than strong salts. They may be similar in odor to the acid or base they are derived from. For example, sodium acetate, CH₃COONa, smells similar to acetic acid CH₃COOH.

References

IUPAC, Compendium of Chemical Terminology, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "salt". doi:10.1351/goldbook.S05447
Voet, D. & Voet, J. G. (2005). Biochemistry (3rd ed.). Hoboken, NJ: John Wiley & Sons Inc. p. 68. ISBN 9780471193500. Archived from the original on 2007-09-11.
D. Chasseau; G. Comberton; J. Gaultier; C. Hauw (1978). "Réexamen de la structure du complexe hexaméthylène-tétrathiafulvalène-tétracyanoquinodiméthane". Acta Crystallographica Section B. 34 (2): 689. doi:10.1107/S0567740878003830.
"Acid and Base Strength". Home Bookshelves Physical & Theoretical Chemistry Supplemental Modules (Physical and Theoretical Chemistry) Acids and Bases Ionization Constants. MindTouch and Department of Education Open Textbook Pilot Project. 5 June 2019. Archived from the original on 2016-12-13. Retrieved 6 November 2019.

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

This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.

[1] IUPAC, Compendium of Chemical Terminology, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "salt". doi:10.1351/goldbook.S05447

[2] Voet, D. & Voet, J. G. (2005). Biochemistry (3rd ed.). Hoboken, NJ: John Wiley & Sons Inc. p. 68. ISBN 9780471193500. Archived from the original on 2007-09-11.

[3] D. Chasseau; G. Comberton; J. Gaultier; C. Hauw (1978). "Réexamen de la structure du complexe hexaméthylène-tétrathiafulvalène-tétracyanoquinodiméthane". Acta Crystallographica Section B. 34 (2): 689. doi:10.1107/S0567740878003830.

[4] "Acid and Base Strength". Home Bookshelves Physical & Theoretical Chemistry Supplemental Modules (Physical and Theoretical Chemistry) Acids and Bases Ionization Constants. MindTouch and Department of Education Open Textbook Pilot Project. 5 June 2019. Archived from the original on 2016-12-13. Retrieved 6 November 2019.