Salt ( chemistry ) - wikipedia Salt ( chemistry ) This article is about the term as used in chemistry. For the chemistry of table salt, see Sodium chloride. For more information about table salt, see Salt. `` Salts '' redirects here. For other uses, see salt ( disambiguation ). The salt potassium dichromate has the bright orange color characteristic of the dichromate anion. In chemistry, a salt is an ionic compound that can be formed by the neutralization reaction of an acid and a base. Salts are composed of related numbers of cations ( positively charged ions ) and anions ( negative ions ) so that the product is electrically neutral ( without a net charge ). These component ions can be inorganic, such as chloride ( Cl ), or organic, such as acetate ( CH CO ) ; and can be monatomic, such as fluoride ( F ), or polyatomic, such as sulfate ( SO ). Contents 1 Kinds of salts 2 Properties 2.1 Color 2.2 Taste 2.3 Odor 2.4 Solubility 2.5 Conductivity 2.6 Melting point 3 Nomenclature 4 Formation 5 Strong salt 6 Weak salts 7 See also 8 References Kinds of salts Salts can be classified in a variety of ways. Salts that produce hydroxide ions when dissolved in water are called alkali salts. Salts that produce acidic solutions are acidic salts. Neutral salts are those salts that are neither acidic nor basic. Zwitterions contain an anionic and a cationic centres in the same molecule, but are not considered to be salts. Examples of zwitterions include amino acids, many metabolites, peptides, and proteins. Properties BMIM PF, an ionic liquid that is liquid at room temperature. 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 white powders. Salts exist in many different colors, which arise either from the anions or cations. For example : sodium chromate is yellow by virtue of the chromate ion potassium dichromate is orange by virtue of the dichromate ion cobalt nitrate is red owing to the chromophore of hydrated cobalt ( II ) ( ( Co ( H O ) ) ). copper sulfate is blue because of the copper ( II ) chromophore potassium permanganate has the violet color of permanganate anion. nickel chloride is typically green of ( NiCl ( H O ) ) sodium chloride, magnesium sulfate heptahydrate are colorless or white because the constituent cations and anions do not absorb in the visible part of the spectrum 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 See also : Solubility § Solubility of ionic compounds in water 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 alkali metal carbonates are not soluble in water. Some soluble carbonate salts are : sodium carbonate, potassium carbonate and ammonium carbonate. Conductivity Salts characteristically are electrical insulator. 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 ) are called electrolytes. Edge - on view of portion of crystal structure of hexamethylene TTF / TCNQ charge transfer salt. 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 Calcium Ca Iron Fe and Fe Magnesium Mg Potassium K Pyridinium C NH Quaternary ammonium NR, R being an alkyl group or an aryl group Sodium Na Copper Cu Common salt - forming anions ( parent acids in parentheses where available ) include : Acetate CH COO ( acetic acid ) Carbonate CO ( carbonic acid ) Chloride Cl ( hydrochloric acid ) Citrate HOC ( COO ) ( CH COO ) ( citric acid ) Cyanide C ≡ N ( hydrocyanic acid ) Fluoride F ( hydrofluoric acid ) Nitrate NO ( nitric acid ) Nitrite NO ( nitrous acid ) Oxide O Phosphate PO ( phosphoric acid ) Sulfate SO ( sulfuric acid ) Formation Solid lead ( II ) sulfate ( PbSO ) Salts are formed by a chemical reaction between : A base and an acid, e.g., NH + HCl → NH Cl A metal and an acid, e.g., Mg + H SO → MgSO + H A metal and a non-metal, e.g., Ca + Cl → CaCl A base and an acid anhydride, e.g., 2 NaOH + Cl O → 2 NaClO + H O An acid and a base anhydride, e.g., 2 HNO + Na O → 2 NaNO + H 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 3 ) 2 + Na 2 SO 4 ⟶ PbSO 4 ↓ + 2 NaNO 3 ( displaystyle ( ce ( ( Pb ( NO3 ) 2 ) + Na2SO4 - > PbSO4 ( v ) + 2NaNO3 ) ) ) 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 odourless 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. Weak salts 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, NaCH COO, smells similar to acetic acid CH COOH. See also Classical elements Stoicheion ( στοιχεῖον ) Greek Air Water Aether Fire Earth Tattva / Panchikarana -- Mahābhūta Hinduism / Jainism -- Buddhism Vayu Ap Akasha Agni Prithvi Wŭ Xíng ( 五行 ) Chinese Wood ( 木 ) Water ( 水 ) Fire ( 火 ) Metal ( 金 ) Earth ( 土 ) Godai ( 五大 ) Japanese Air ( 風 ) Water ( 水 ) Void ( 空 ) Fire ( 火 ) Earth ( 地 ) Bön Tibetan Air Water Aether Fire Earth Alchemy Medieval Air Water Aether Fire Earth Sulphur Mercury Salt 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 / Pyrotechnics ( Salts are what give color to fireworks ) Halide Hypertension Ionic bonds 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 Brønsted -- Lowry acid -- base theory Ionic compound References Jump up ^ Skoog, D.A ; West, D.M. ; Holler, J.F. ; Crouch, S.R. ( 2004 ). Fundamentals of Analytical Chemistry ; Chapters 14, 15 and 16 ( 8th ed. ). Thomson Brooks / Cole. ISBN 0 - 03 - 035523 - 0. Jump up ^ 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. CS1 maint : Multiple names : authors list ( link ) Jump up ^ D. Chasseau ; G. Comberton ; J. Gaultier ; C. Hauw ( 1978 ). `` Réexamen de la structure du complexe hexaméthylène - tétrathiafulvalène - tétracyanoquinodiméthane ''. Acta Crystallogr., Sect. B : Struct. Crystallogr. Cryst. Chem. 34 : 689. doi : 10.1107 / S0567740878003830. Jump up ^ `` Archived copy ''. Archived from the original on 2016 - 12 - 13. Retrieved 2017 - 04 - 16. Mark Kurlansky ( 2002 ). Salt : A World History. Walker Publishing Company. ISBN 0 - 14 - 200161 - 9. 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Question: where does salt come from in the neutralization reaction
Answer: by the neutralization reaction of an acid and a base