On Air

Investment

Buy this Domain?
Do you interesting about this domain and the running project?
Feel free to send your offer to webmaster.
pay with Paypal

Advertising

Salt (chemistry)

In chemistry, a salt is an ionic compound that can be formed by the neutralization reaction of an acid and a base.{{cite book |last=Skoog |first=D.A |author2=West, D.M.|author3= Holler, J.F.|author4= Crouch, S.R. |title=Fundamentals of Analytical Chemistry; Chapters 14, 15 and 16 |publisher=Thomson Brooks/Cole |year=2004 |edition=8th |isbn=0-03-035523-0 }} 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 (); and can be monatomic, such as fluoride (F−), or polyatomic, such as sulfate (). There are several varieties of salts. Salts that hydrolyze to produce hydroxide ions when dissolved in water are alkali salts; those that hydrolyze to produce hydronium ions in water are acidic salts. Neutral salts are those salts that are neither acidic nor basic. Zwitterions contain an anionic centre and a cationic centre in the same molecule, but are not considered to be salts. Examples of zwitterions include amino acids, many metabolites, peptides, and proteins. Usually, non-dissolved salts at standard conditions for temperature and pressure are solid, but there are exceptions (see molten salts and ionic liquids). Molten salts and solutions containing dissolved salts (e.g., sodium chloride in water) are called electrolytes, as they are able to conduct electricity. As observed in the cytoplasm of cells, in blood, urine, plant saps and mineral waters, 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

Salts can appear to be clear and transparent ( sodium chloride), opaque, and even metallic and lustrous ( iron disulfide). 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, for example: Most minerals and inorganic pigments, as well as many synthetic organic dyes, are salts. The color of the specific salt is due to the electronic structure in the d-orbitals of transition elements or in the conjugated organic dye framework.

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 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 can be 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 on 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 sulfates – barium sulfate, calcium sulfate (sparingly soluble) and lead(II) sulfate are examples of exceptions. However, ions that bind tightly to each other and form highly stable lattices are less soluble, because it is 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. Some soluble carbonate salts are: sodium carbonate, potassium carbonate and ammonium carbonate.

Conductivity

Solid salts do not conduct electricity. However, liquid salts do. Moreover, solutions of salts also conduct electricity.

Chemical compound

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

Formation

Salts are formed by a chemical reaction between:

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. And most group 1 and 2 metals are salts. Strong salts are especially useful when creating conductive compounds as their constituent ions allow for greater conductivity.http://chem.libretexts.org/Core/Physical_and_Theoretical_Chemistry/Acids_and_Bases/Ionization_Constants/Acid_and_Base_Strength

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, NaCH3COO, smells similar to acetic acid CH3COOH.

See also

References

  • Mark Kurlansky (2002). Salt: A World History. Walker Publishing Company. .
"green air" © 2007 - Ingo Malchow, Webdesign Neustrelitz
This article based upon the http://en.wikipedia.org/wiki/Salt_(chemistry), the free encyclopaedia Wikipedia and is licensed under the GNU Free Documentation License.
Further informations available on the list of authors and history: http://en.wikipedia.org/w/index.php?title=Salt_(chemistry)&action=history
presented by: Ingo Malchow, Mirower Bogen 22, 17235 Neustrelitz, Germany