Electrolyte: Difference between revisions
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{{Short description|Ionic solids whose dissociation in water frees up ions carrying the electrical current in solution}} |
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An '''electrolyte''' is a substance containing free [[ion]]s that behaves as an [[electrical conductor|electrically conductive]] medium. Because they generally consist of ions in solution, electrolytes are also known as '''ionic solutions''', but molten electrolytes and [[proton conductor|solid electrolytes]] are also possible. They are sometimes referred to in abbreviated [[jargon]] as '''lytes'''. |
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== Explanation == |
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{{For|the R.E.M. song|Electrolite}} |
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{{Use dmy dates|date=April 2017}} |
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An '''electrolyte''' is a substance that conducts [[electricity]] through the movement of [[ion]]s, but not through the movement of [[electron]]s.<ref>{{Cite journal|last1=Enderby|first1=J E|last2=Neilson|first2=G W|date=1981-06-01|title=The structure of electrolyte solutions|url=https://iopscience.iop.org/article/10.1088/0034-4885/44/6/001|journal=Reports on Progress in Physics|volume=44|issue=6|pages=593–653|doi=10.1088/0034-4885/44/6/001|s2cid=250852242|issn=0034-4885|access-date=18 December 2021|archive-date=18 December 2021|archive-url=https://web.archive.org/web/20211218145748/https://iopscience.iop.org/article/10.1088/0034-4885/44/6/001|url-status=live}}</ref><ref name=":0">{{Cite book|last=Petrovic|first=Slobodan|url=http://worldcat.org/oclc/1202758685|title=Battery technology crash course : a concise introduction|date=29 October 2020|publisher=Springer |isbn=978-3-030-57269-3|oclc=1202758685}}</ref><ref>{{Cite book|last1=Winie|first1=Tan|url=https://books.google.com/books?id=l-C7DwAAQBAJ&dq=introduction+electrolytes&pg=PA137|title=Polymer Electrolytes: Characterization Techniques and Energy Applications|last2 =Arof|first2=Abdul K.|last3=Thomas|first3=Sabu|date=2020-02-18|publisher=John Wiley & Sons|isbn=978-3-527-34200-6|language=en}}</ref> This includes most soluble [[Salt (chemistry)|salts]], [[acid]]s, and [[Base (chemistry)|bases]], dissolved in a [[polar solvent]] like water. Upon dissolving, the substance separates into [[cation]]s and [[anion]]s, which disperse uniformly throughout the solvent.<ref>{{cite journal | author=M Andreev | author2 = JJ de Pablo | author3 = A Chremos | author4=J F Douglas | title=Influence of ion solvation on the properties of electrolyte solutions|journal=The Journal of Physical Chemistry B| volume = 122 | pages = 4029–4034 | year=2018 | issue = 14 | doi= 10.1021/acs.jpcb.8b00518| pmid = 29611710 }}</ref> [[Solid-state electrolyte]]s also exist. In medicine and sometimes in chemistry, the term electrolyte refers to the substance that is dissolved.<ref>{{Cite book|last=Wilkins|first=Lippincott Williams &|url=https://books.google.com/books?id=Xs0YqSKqAlcC&dq=basics+electrolyte&pg=PA18|title=Fluids and Electrolytes|date=2007|publisher=Lippincott Williams & Wilkins|isbn=978-1-58255-923-0|language=en}}</ref><ref>{{Cite web|date=2011-02-02|title=electrolyte|url=https://www.cancer.gov/publications/dictionaries/cancer-terms/def/electrolyte|url-status=live|access-date=2021-12-18|website=National Cancer Institute|language=en|archive-url=https://web.archive.org/web/20180423090514/https://www.cancer.gov/publications/dictionaries/cancer-terms/def/electrolyte |archive-date=23 April 2018 }}</ref> |
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look in a dictionary you homosexual |
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Electrically, such a solution is neutral. If an [[electric potential]] is applied to such a solution, the cations of the solution are drawn to the [[electrode]] that has an abundance of [[electron]]s, while the anions are drawn to the electrode that has a deficit of electrons. The movement of anions and cations in opposite directions within the solution amounts to a current. Some gases, such as [[hydrogen chloride]] (HCL), under conditions of high temperature or low pressure can also function as electrolytes.{{Clarify|date=January 2021}} Electrolyte solutions can also result from the dissolution of some biological (e.g., [[DNA]], [[polypeptides]]) or [[synthetic polymer]]s (e.g., [[polystyrene sulfonate]]), termed "[[polyelectrolyte]]s", which contain charged [[functional group]]s. A substance that dissociates into ions in solution or in the melt acquires the capacity to conduct electricity. [[Sodium]], [[potassium]], [[chloride]], [[calcium]], [[magnesium]], and [[phosphate]] in a liquid phase are examples of electrolytes. |
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== Physiological importance == |
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In medicine, [[oral rehydration therapy|electrolyte replacement]] is needed when a person has prolonged [[vomiting]] or [[diarrhea]], and as a response to sweating due to strenuous athletic activity. Commercial electrolyte solutions are available, particularly for sick children (such as [[Oral rehydration therapy|oral rehydration]] solution, [[Suero Oral]], or [[Pedialyte]]) and athletes ([[sports drink]]s). Electrolyte monitoring is important in the treatment of [[anorexia nervosa|anorexia]] and [[bulimia]]. |
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In [[physiology]], the primary ions of electrolytes are [[sodium]](Na<sup>+</sup>), [[potassium]] (K<sup>+</sup>), [[calcium]] (Ca<sup>2+</sup>), [[magnesium]] (Mg<sup>2+</sup>), [[chloride]] (Cl<sup>-</sup>), [[phosphate]] (PO<sub>4</sub><sup>3-</sup>), and [[hydrogen carbonate]] (HCO<sub>3</sub><sup>-</sup>). The electric charge symbols of plus (+) and minus (-) are used to indicate that the substance indicated is ionic in nature and has an imbalanced distribution of electrons. This is the result of chemical dissociation. |
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In science, electrolytes are one of the main components of [[electrochemical cell]]s.<ref name=":0"/> |
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All higher lifeforms require a subtle and complex electrolyte balance between the [[intracellular]] and [[extracellular]] [[natural environment|milieu]]. In particular, the maintenance of precise [[osmotic]] [[ion gradient|gradient]]s of electrolytes is important. Such gradients affect and regulate the [[hydration]] of the body, [[blood]] [[pH]], and are critical for [[nerve]] and [[muscle]] function. |
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In clinical [[medicine]], mentions of electrolytes usually refer [[metonym]]ically to the ions, and (especially) to their [[concentration]]s (in blood, serum, urine, or other fluids). Thus, mentions of electrolyte levels usually refer to the various ion concentrations, not to the fluid volumes. |
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Both muscle tissue and neurons are considered electric tissues of the body. Muscles and neurons are activated by electrolyte activity between the [[extracellular fluid]] or interstitial fluid, and [[intracellular fluid]]. Electrolytes may enter or leave the cell membrane through specialized protein structures embedded in the [[plasma membrane]] called [[ion channels]]. For example, [[muscle contraction]] is dependent upon the presence of calcium (Ca<sup>2+</sup>), sodium (Na<sup>+</sup>), and potassium (K<sup>+</sup>). Without sufficient levels of these key electrolytes, muscle weakness or severe muscle contractions may occur. |
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== Etymology == |
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Electrolyte balance is maintained by oral, or in emergencies, intravenous (IV) intake of electrolyte-containing substances, and is regulated by [[hormone]]s, generally with the [[kidney]]s flushing out excess levels. In humans, electrolyte [[homeostasis]] is regulated by hormones such as [[antidiuretic hormone]], [[aldosterone]] and [[parathyroid hormone]]. Serious [[electrolyte disturbance]]s, such as [[dehydration]] and [[water poisoning|overhydration]], may lead to cardiac and neurological complications and, unless they are rapidly resolved, will result in a [[medical emergency]]. |
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The word ''electrolyte'' derives from [[Ancient Greek]] ήλεκτρο- (''ēlectro''-), prefix originally meaning ''amber'' but in modern contexts related to electricity, and λυτός (''lytos''), meaning "able to be untied or loosened".{{Cn|date=May 2024}} |
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== History == |
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[[File:Arrhenius2.jpg|thumb|[[Svante Arrhenius]], father of the concept of electrolyte dissociation in [[aqueous solution]] for which he received the [[Nobel Prize in Chemistry]] in 1903 ]] |
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In his 1884 dissertation, [[Svante Arrhenius]] put forth his explanation of solid crystalline salts disassociating into paired charged particles when dissolved, for which he won the 1903 [[Nobel Prize]] in Chemistry.<ref>{{cite web|url=https://www.nobelprize.org/nobel_prizes/chemistry/laureates/1903/index.html|title=The Nobel Prize in Chemistry 1903|access-date=5 January 2017|archive-date=8 July 2018|archive-url=https://web.archive.org/web/20180708044958/https://www.nobelprize.org/nobel_prizes/chemistry/laureates/1903/index.html|url-status=live}}</ref><ref name="columbia">{{cite book|editor1-last=Harris|editor1-first=William|editor2-last=Levey|editor2-first=Judith|title=The New Columbia Encyclopedia|date=1975|publisher=Columbia University|location=New York City|isbn=978-0-231035-729|page=[https://archive.org/details/newcolumbiaencyc00harr/page/155 155]|edition=4th|url-access=registration|url=https://archive.org/details/newcolumbiaencyc00harr/page/155}}</ref><ref name="EncBrit">{{cite book|editor1-last=McHenry|editor1-first=Charles|title=The New Encyclopædia Britannica|date=1992|publisher=Encyclopædia Britannica, Inc.|location=Chicago|isbn=978-085-229553-3|page=587|volume=1|edition=15|bibcode=1991neb..book.....G}}</ref><ref name="SciBio">{{cite book|editor1-last=Cillispie|editor1-first=Charles|title=Dictionary of Scientific Biography|date=1970|publisher=Charles Scribner's Sons|location=New York City|isbn=978-0-684101-125|pages=296–302|edition=1}}</ref> Arrhenius's explanation was that in forming a solution, the salt dissociates into charged particles, to which [[Michael Faraday]] (1791-1867) had given the name "[[ion]]s" many years earlier. Faraday's belief had been that ions were produced in the process of [[electrolysis]]. Arrhenius proposed that, even in the absence of an electric current, solutions of salts contained ions. He thus proposed that chemical reactions in solution were reactions between ions.<ref name="columbia"/><ref name="EncBrit"/><ref name="SciBio"/> |
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Shortly after Arrhenius's hypothesis of ions, [[Franz Hofmeister]] and Siegmund Lewith<ref>{{cite journal | author=Franz Hofmeister | title=Zur Lehre Von Der Wirkung Der Salze|journal=Naunyn-Schmiedeberg's Arch. Pharmacol.|year=1888}}</ref><ref>{{cite journal| author=W. Kunz| author2=J. Henle| author3=B. W. Ninham| title='Zur Lehre von der Wirkung der Salze' (about the science of the effect of salts): Franz Hofmeister's historical papers| url=https://linkinghub.elsevier.com/retrieve/pii/S1359029404000317| journal=Current Opinion in Colloid & Interface Science| year=2004| volume=9| issue=1–2| pages=19–37| doi=10.1016/j.cocis.2004.05.005| access-date=8 November 2021| archive-date=20 January 2022| archive-url=https://web.archive.org/web/20220120080518/https://linkinghub.elsevier.com/retrieve/pii/S1359029404000317| url-status=live}}</ref><ref>{{cite journal | doi = 10.1039/D2CP00847E | volume=24 | title=Understanding specific ion effects and the Hofmeister series | year=2022 | journal=Physical Chemistry Chemical Physics | pages=12682–12718 | last1 = Gregory | first1 = Kasimir P. | last2 = Elliott | first2 = Gareth R. | last3 = Robertson | first3 = Hayden | last4 = Kumar | first4 = Anand | last5 = Wanless | first5 = Erica J. | last6 = Webber | first6 = Grant B. | last7 = Craig | first7 = Vincent S. J. | last8 = Andersson | first8 = Gunther G. | last9 = Page | first9 = Alister J. | issue=21 | pmid=35543205 | bibcode=2022PCCP...2412682G | doi-access = free }}</ref> found that different ion types displayed different effects on such things as the solubility of proteins. A consistent ordering of these different ions on the magnitude of their effect arises consistently in many other systems as well. This has since become known as the [[Hofmeister series]]. |
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Measurement of electrolytes is a commonly performed diagnostic procedure, performed via [[blood test]]ing or [[urinalysis]]. The interpretation of these values is somewhat meaningless without analysis of the [[medical history|clinical history]] and is often impossible without parallel measurement of [[renal function]]. Electrolytes measured most often are sodium and potassium. Chloride levels are rarely measured except for [[arterial blood gas]] interpretation since they are inherently linked to sodium levels. One important test conducted on urine is the [[specific gravity]] test to determine the occurrence of [[electrolyte imbalance]]. |
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While the origins of these effects are not abundantly clear and have been debated throughout the past century, it has been suggested that the charge density of these ions is important<ref>{{cite journal | author=Kasimir P. Gregory | author2=Erica J. Wanless | author3=Grant B. Webber| author4=Vince S. J. Craig | author5=Alister J. Page | title=The Electrostatic Origins of Specific Ion Effects: Quantifying the Hofmeister Series for Anions|journal=Chem. Sci.|year=2021| volume=12 | issue=45 | pages=15007–15015 |doi=10.1039/D1SC03568A| pmid=34976339 | pmc=8612401 | s2cid=244578563 }}</ref> and might actually have explanations originating from the work of [[Charles-Augustin de Coulomb]] over 200 years ago. |
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=== Sports drinks === |
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== Formation == |
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Electrolytes are commonly found in [[sports drink]]s. In [[oral rehydration therapy]], electrolyte drinks containing sodium and potassium salts are used to replenish the body's [[water]] and electrolyte levels after [[dehydration]] caused by [[exercise]], [[diaphoresis]], [[diarrhea]], [[vomiting]] or [[starvation]]. Giving pure water to such a person is not the best way to restore fluid levels because it dilutes the salts inside the body's cells and interferes with their chemical functions. This can lead to [[water intoxication]]. |
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Electrolyte solutions are normally formed when salt is placed into a [[solvent]] such as water and the individual components dissociate due to the [[thermodynamic]] interactions between solvent and solute molecules, in a process called "[[solvation]]". For example, when table salt ([[sodium chloride]]), NaCl, is placed in water, the salt (a solid) dissolves into its component ions, according to the dissociation reaction:{{cn|date=November 2021}} |
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: NaCl<sub>(s)</sub> → Na<sup>+</sup><sub>(aq)</sub> + Cl<sup>−</sup><sub>(aq)</sub> |
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Sports drinks such as [[Gatorade]], [[Powerade]], or [[Lucozade]] are electrolyte drinks with large amounts of added [[carbohydrate]]s, such as [[glucose]], to provide energy. The drinks commonly sold to the public are [[isotonic]] (with [[osmolality]] close to that of blood), with [[hypotonic]] (with a lower osmolality) and [[hypertonic]] (with a higher osmolality) varieties available to athletes, depending on their nutritional needs.[http://www.disen.org/nutrition/pages-to-edit/fluids.htm] |
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It is also possible for substances to react with water, producing ions. For example, [[carbon dioxide]] gas dissolves in water to produce a solution that contains [[hydronium]], [[carbonate]], and [[Carbonic Acid|hydrogen carbonate]] ions.{{cn|date=April 2022}} |
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It is really not necessary to replace losses of sodium, potassium and other electrolytes during exercise since it is unlikely that a significant depletion the body's stores of these minerals will occur during normal training. However, in extreme exercising conditions over 5 or 6 hours (an Ironman or ultramarathon, for example) the consumtion of a complex sports drink with electrolytes is recommended. Athletes who do not consume electrolytes under these conditions risk overhydration (or hyponatremia). [http://sportsmedicine.about.com/cs/hydration/a/aa041103a.htm] |
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[[Molten salt]]s can also be electrolytes as, for example, when sodium chloride is molten, the liquid conducts electricity. In particular, ionic liquids, which are molten salts with melting points below 100 °C,<ref>{{cite journal |year=2002 |script-title=zh:离子液体研究进展 |url=http://files.instrument.com.cn/FilesCenter/20100725/201072512514137980.pdf |journal={{lang|zh-hans|化学通报}} |language=zh-hans |issue=4 |page=243 |last1=Shi |first1=Jiahua |last2=Sun |first2=Xun |first3=Yang |last3=Chunhe |last4=Gao |first4=Qingyu |last5=Li |first5=Yongfang |access-date=2017-03-01 |issn=0441-3776 |archive-url=https://web.archive.org/web/20170302031247/http://files.instrument.com.cn/FilesCenter/20100725/201072512514137980.pdf |archive-date=2 March 2017 |url-status=dead }}</ref> are a type of highly conductive non-aqueous electrolytes and thus have found more and more applications in fuel cells and batteries.<ref> |
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Because sports drinks typically contain very high levels of [[sugar]], they are not recommended for regular use by children. Rather, specially-formulated pediatric electrolyte solutions are recommended. Sports drinks are also not appropriate for replacing the fluid lost during diarrhea. The role of sports drinks is to inhibit electrolyte loss but are insufficient to restore imbalance once it occurs.{{Fact|date=February 2007}} Medicinal rehydration sachets and drinks are available to replace the key electrolyte ions lost. Dentists recommend that regular consumers of sports drinks observe precautions against [[tooth decay]]. |
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{{cite journal |
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|author1=Jiangshui Luo |author2=Jin Hu |author3=Wolfgang Saak |author4=Rüdiger Beckhaus |author5=Gunther Wittstock |author6=Ivo F. J. Vankelecom |author7=Carsten Agert |author8=Olaf Conrad |s2cid=94400312 |year=2011 |
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|title=Protic ionic liquid and ionic melts prepared from methanesulfonic acid and 1H-1,2,4-triazole as high temperature PEMFC electrolytes |
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|journal=[[Journal of Materials Chemistry]] |
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|volume=21 |
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|issue=28 |pages=10426–10436 |
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|doi=10.1039/C0JM04306K |
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|url=https://lirias.kuleuven.be/handle/123456789/313759 }}</ref> |
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An electrolyte in a solution may be described as "concentrated" if it has a high concentration of ions, or "dilute" if it has a low concentration. If a high proportion of the solute dissociates to form free ions, the electrolyte is strong; if most of the solute does not dissociate, the electrolyte is weak. The properties of electrolytes may be exploited using electrolysis to extract constituent elements and compounds contained within the solution.{{cn|date=November 2021}} |
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Electrolyte and sports drinks can be home-made by using the correct proportions of sugar, salt and water. [http://www.webmd.com/hw/health_guide_atoz/str2254.asp?navbar=hw86827] |
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Alkaline earth metals form hydroxides that are strong electrolytes with limited solubility in water, due to the strong attraction between their constituent ions. This limits their application to situations where high solubility is required.<ref>Brown, Chemistry: The Central Science, 14th edition, pg. 680.</ref> |
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In 2021, researchers have found that electrolyte can "substantially facilitate electrochemical corrosion studies in less conductive media".<ref>{{Cite journal|last1=Matějovský|first1=Lukáš|last2=Staš|first2=Martin|last3=Dumská|first3=Karolina|last4=Pospíšil|first4=Milan|last5=Macák|first5=Jan|date=2021-01-01|title=Electrochemical corrosion tests in an environment of low-conductive ethanol-gasoline blends: Part 1 – Testing of supporting electrolytes|url=https://www.sciencedirect.com/science/article/pii/S1572665720311085|journal=Journal of Electroanalytical Chemistry|language=en|volume=880|pages=114879|doi=10.1016/j.jelechem.2020.114879|s2cid=229508133|issn=1572-6657}}</ref> |
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== Physiological importance == |
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{{See also|Electrochemical gradient|Acid–base homeostasis|Electrolyte imbalance}} |
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In [[physiology]], the primary ions of electrolytes are [[sodium]] (Na<sup>+</sup>), [[potassium]] (K<sup>+</sup>), [[calcium]] (Ca<sup>2+</sup>), [[magnesium]] (Mg<sup>2+</sup>), [[chloride]] (Cl<sup>−</sup>), [[Monohydrogen phosphate|hydrogen phosphate]] (HPO<sub>4</sub><sup>2−</sup>), and [[hydrogen carbonate]] (HCO<sub>3</sub><sup>−</sup>).<ref name="auto">{{cite journal |last1=Alfarouk |first1=Khalid O. |last2=Ahmed |first2=Samrein B. M. |last3=Ahmed |first3=Ahmed |last4=Elliott |first4=Robert L. |last5=Ibrahim |first5=Muntaser E. |last6=Ali |first6=Heyam S. |last7=Wales |first7=Christian C. |last8=Nourwali |first8=Ibrahim |last9=Aljarbou |first9=Ahmed N. |last10=Bashir |first10=Adil H. H. |last11=Alhoufie |first11=Sari T. S. |last12=Alqahtani |first12=Saad Saeed |last13=Cardone |first13=Rosa A. |last14=Fais |first14=Stefano |last15=Harguindey |first15=Salvador |last16=Reshkin |first16=Stephan J. |title=The Interplay of Dysregulated pH and Electrolyte Imbalance in Cancer |journal=Cancers |date=7 April 2020 |volume=12 |issue=4 |pages=898 |doi=10.3390/cancers12040898|pmid=32272658 |pmc=7226178 |doi-access=free }}</ref>{{Failed verification|date=December 2021}} The electric charge symbols of plus (+) and minus (−) indicate that the substance is ionic in nature and has an imbalanced distribution of electrons, the result of [[Dissociation (chemistry)|chemical dissociation]]. Sodium is the main electrolyte found in extracellular fluid and potassium is the main intracellular electrolyte;<ref>{{Cite journal |year=1986 |script-title=zh:细胞膜钠泵及其临床意义 |url=http://www.cnki.com.cn/Article/CJFDTotal-SHYX198601021.htm |journal={{lang|zh-hans|上海医学}} [Shanghai Medicine] |language=zh-hans |issue=1 |page=1 |last1=Ye |first1=Shenglong (叶胜龙) |last2=Tang |first2=Zhaoyou (汤钊猷) |access-date=3 March 2017 |archive-date=3 March 2017 |archive-url=https://web.archive.org/web/20170303201749/http://www.cnki.com.cn/Article/CJFDTotal-SHYX198601021.htm |url-status=dead }}</ref> both are involved in fluid balance and [[blood pressure]] control.<ref>{{Cite journal|year=2004|others=张定昌|script-title=zh:电解质紊乱对晚期肿瘤的治疗影响 |journal={{lang|zh-hans|中华中西医杂志}} [Chinese Magazine of Chinese and Western Medicine]| language = zh-hans|issue=10|quote={{lang|zh-hans|在正常人体内, 钠离子占细胞外液阳离子总量的92%, 钾离子占细胞内液阳离子总量的98%左右.钠、钾离子的相对平衡, 维持着整个细胞的功能和结构的完整.钠、钾是人体内最主要的电解质成分...}} |last1=Tu |first1=Zhiquan (涂志全)}}</ref> |
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All known multicellular lifeforms require a subtle and complex electrolyte balance between the [[intracellular]] and [[extracellular]] environments.<ref name="auto"/> In particular, the maintenance of precise [[osmotic]] [[ion gradient|gradient]]s of electrolytes is important. Such gradients affect and regulate the [[Fluid replacement|hydration]] of the body as well as [[Acid–base homeostasis|blood pH]], and are critical for [[nerve]] and [[muscle]] function. Various mechanisms exist in living species that keep the concentrations of different electrolytes under tight control.<ref>{{Citation |last=Open Resources for Nursing |title=Chapter 15 Fluids and Electrolytes |date=2021 |work=Nursing Fundamentals [Internet] |url=https://www.ncbi.nlm.nih.gov/books/NBK591820/ |access-date=2024-02-28 |publisher=Chippewa Valley Technical College |language=en |last2=Ernstmeyer |first2=Kimberly |last3=Christman |first3=Elizabeth}}</ref> |
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Both muscle tissue and [[neuron]]s are considered electric tissues of the body. Muscles and neurons are activated by electrolyte activity between the [[extracellular fluid]] or [[interstitial fluid]], and [[intracellular fluid]]. Electrolytes may enter or leave the cell membrane through specialized protein structures embedded in the [[plasma membrane]] called "[[ion channels]]". For example, [[muscle contraction]] is dependent upon the presence of calcium (Ca<sup>2+</sup>), sodium (Na<sup>+</sup>), and potassium (K<sup>+</sup>). Without sufficient levels of these key electrolytes, muscle weakness or severe muscle contractions may occur.{{cn|date=November 2021}}<ref>{{Cite web |title=Reproductive Consequences of Electrolyte Disturbances in Domestic Animals |url=https://www.researchgate.net/figure/The-most-significant-electrolytes-in-animal-organisms_tbl1_361737152}}</ref> |
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Electrolyte balance is maintained by oral, or in emergencies, intravenous (IV) intake of electrolyte-containing substances, and is regulated by [[hormone]]s, in general with the [[kidney]]s flushing out excess levels. In humans, electrolyte [[homeostasis]] is regulated by hormones such as [[antidiuretic hormone]]s, [[aldosterone]] and [[parathyroid hormone]]s. Serious [[electrolyte disturbance]]s, such as [[dehydration]] and [[Water intoxication|overhydration]], may lead to cardiac and neurological complications and, unless they are rapidly resolved, will result in a [[medical emergency]]. |
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=== Measurement === |
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Measurement of electrolytes is a commonly performed diagnostic procedure, performed via [[blood test]]ing with [[ion-selective electrode]]s or [[urinalysis]] by [[medical technologist]]s. The interpretation of these values is somewhat meaningless without analysis of the [[medical history|clinical history]] and is often impossible without parallel measurements of [[renal function]]. The electrolytes measured most often are sodium and potassium. Chloride levels are rarely measured except for [[arterial blood gas]] interpretations since they are inherently linked to sodium levels. One important test conducted on urine is the [[specific gravity]] test to determine the occurrence of an [[electrolyte imbalance]].{{cn|date=November 2021}} |
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=== Rehydration === |
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According to a study paid for by the [[Gatorade|Gatorade Sports Science Institute]], electrolyte drinks containing sodium and potassium salts replenish the body's water and electrolyte concentrations after dehydration caused by [[exercise]], [[Alcohol abuse|excessive alcohol consumption]], [[diaphoresis]] (heavy sweating), diarrhea, vomiting, [[Substance intoxication|intoxication]] or starvation; the study says that athletes exercising in extreme conditions (for three or more hours continuously, e.g. a [[marathon]] or [[triathlon]]) who do not consume electrolytes risk [[dehydration]] (or [[hyponatremia]]).<ref>{{cite journal |author1=J, Estevez E |author2=Baquero E |author3=Mora-Rodriguez R |title=Anaerobic performance when rehydrating with water or commercially available sports drinks during prolonged exercise in the heat |journal=Applied Physiology, Nutrition, and Metabolism |volume=33 |pages=290–298 |year=2008 |doi=10.1139/H07-188 |pmid=18347684 |issue=2}}</ref>{{needs independent confirmation|reason=Study was paid for |
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by a grant from the Gatorade Sports Science Institute|date=June 2024}} |
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A home-made electrolyte drink can be made by using water, sugar and salt [[mixing ratio|in precise proportions]].<ref>{{cite web|url=https://www.webmd.com/hw-popup/rehydration-drinks |archive-url=https://web.archive.org/web/20081023055047/https://www.webmd.com/hw-popup/rehydration-drinks |url-status=dead |archive-date=2008-10-23 |title=Rehydration drinks |publisher=Webmd.com |date=2008-04-28 |access-date=2018-12-25}}</ref> It is important to include [[glucose]] (sugar) to utilise the co-transport mechanism of sodium and glucose. Commercial preparations are also available<ref>{{cite web |url=http://rehydrate.org/resources/suppliers.htm |title=Oral Rehydration Salt Suppliers |publisher=Rehydrate.org |date=2014-10-07 |access-date=2014-12-04 |archive-date=7 December 2014 |archive-url=https://web.archive.org/web/20141207213450/http://rehydrate.org/resources/suppliers.htm |url-status=live }}</ref> for both human and veterinary use. |
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Electrolytes are commonly found in [[fruit juice]]s, sports drinks, milk, nuts, and many fruits and vegetables (whole or in juice form) (e.g., potatoes, [[avocado]]s). |
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== Electrochemistry == |
== Electrochemistry == |
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{{Main| |
{{Main|Electrolysis}} |
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When [[electrode]]s are placed in an electrolyte and a [[voltage]] is applied, the electrolyte will conduct electricity. Lone [[electron]]s normally cannot pass through the electrolyte; instead, a chemical reaction occurs at the [[cathode]], providing electrons to the electrolyte. Another reaction occurs at the [[anode]], consuming electrons from the electrolyte. As a result, a negative charge cloud develops in the electrolyte around the cathode, and a positive charge develops around the anode. The ions in the electrolyte neutralize these charges, enabling the electrons to keep flowing and the reactions to continue.{{cn|date=November 2021}} |
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[[File:Chloralkali membrane.svg|600px|thumb|right|[[Electrolytic cell]] producing [[chlorine]] (Cl<sub>2</sub>) and [[sodium hydroxide]] (NaOH) from a solution of common salt]] |
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For example, in a solution of ordinary table salt (sodium chloride, NaCl) in water, the cathode reaction will be |
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: 2 H<sub>2</sub>O + 2e<sup>−</sup> → 2 OH<sup>−</sup> + H<sub>2</sub> |
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When two [[electrode]]s are placed in an electrolyte and a [[voltage]] is applied, the electrolyte will conduct electricity. Lone [[electron]]s normally cannot pass through the electrolyte; instead, a chemical reaction occurs at the [[cathode]] consuming electrons from the cathode, and another reaction occurs at the [[anode]] producing electrons to be taken up by the anode. As a result, a negative charge cloud develops in the electrolyte around the cathode, and a positive charge develops around the anode. The ions in the electrolyte move to neutralize these charges so that the reactions can continue and the electrons can keep flowing. |
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For example, in a dilute solution of ordinary salt ([[sodium chloride]], NaCl) in water, the cathode reaction will be |
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:2H<sub>2</sub>O + 2e<sup>−</sup> → 2OH<sup>−</sup> + H<sub>2</sub> |
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and [[hydrogen]] gas will bubble up; the anode reaction is |
and [[hydrogen]] gas will bubble up; the anode reaction is |
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:2H<sub>2</sub>O → O<sub>2</sub> + 4H<sup>+</sup> + 4e<sup>−</sup> |
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: 2 NaCl → 2 Na<sup>+</sup> + Cl<sub>2</sub> + 2e<sup>−</sup> |
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and [[oxygen]] gas will be liberated. The positively charged sodium ions Na<sup>+</sup> will move towards the cathode neutralizing the negative charge of OH<sup>−</sup> there, and the negatively charged chlorine ions Cl<sup>−</sup> will move towards the anode neutralizing the positive charge of H<sup>+</sup> there. Without the ions from the electrolyte, the charges around the electrode would slow down continued electron flow; [[diffusion]] of H<sup>+</sup> and OH<sup>−</sup> through water to the other electrode takes longer than movement of the much more prevalent salt ions. |
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and [[chlorine]] gas will be liberated into solution where it reacts with the sodium and hydroxyl ions to produce [[sodium hypochlorite]] - household [[bleach]]. The positively charged sodium ions Na<sup>+</sup> will react toward the cathode, neutralizing the negative charge of OH<sup>−</sup> there, and the negatively charged hydroxide ions OH<sup>−</sup> will react toward the anode, neutralizing the positive charge of Na<sup>+</sup> there. Without the ions from the electrolyte, the charges around the electrode would slow down continued electron flow; [[diffusion]] of H<sup>+</sup> and OH<sup>−</sup> through water to the other electrode takes longer than movement of the much more prevalent salt ions. |
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Electrolytes dissociate in water because water molecules are dipoles and the dipoles orient in an energetically favorable manner to [[Solvation|solvate]] the ions. |
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In other systems, the electrode reactions can involve the metals of the electrodes as well as the ions of the electrolyte. |
In other systems, the electrode reactions can involve the metals of the electrodes as well as the ions of the electrolyte. |
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Electrolytic conductors are used in electronic devices where the chemical reaction at a metal |
Electrolytic conductors are used in electronic devices where the chemical reaction at a metal-electrolyte interface yields useful effects. |
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*In [[battery (electricity)|batteries]], two |
* In [[battery (electricity)|batteries]], two materials with different electron affinities are used as electrodes; electrons flow from one electrode to the other outside of the battery, while inside the battery the circuit is closed by the electrolyte's ions. Here, the electrode reactions convert chemical energy to electrical energy.<ref name="Kamil Perzyna, Regina Borkowska, Jaroslaw Syzdek, Aldona Zalewska, Wladyslaw Wieczorek 2011 58–65">{{cite journal|author1=Kamil Perzyna |author2=Regina Borkowska |author3=Jaroslaw Syzdek |author4=Aldona Zalewska |author5=Wladyslaw Wieczorek |title=The effect of additive of Lewis acid type on lithium–gel electrolyte characteristics|journal=Electrochimica Acta| volume=57|pages=58–65|year=2011|doi=10.1016/j.electacta.2011.06.014}}</ref> |
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*In some [[fuel cell]]s, a solid electrolyte or [[proton conductor]] connects the plates electrically while keeping the hydrogen and oxygen fuel gases separated. |
* In some [[fuel cell]]s, a solid electrolyte or [[proton conductor]] connects the plates electrically while keeping the hydrogen and oxygen fuel gases separated.<ref name="1,2,4-Triazolium perfluorobutanesulfonate as an archetypal pure protic organic ionic plastic crystal electrolyte for all-solid-state fuel cells"/> |
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*In [[electroplating]] tanks, the electrolyte simultaneously deposits metal onto the object to be plated, and electrically connects that object in the circuit. |
* In [[electroplating]] tanks, the electrolyte simultaneously deposits metal onto the object to be plated, and electrically connects that object in the circuit. |
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*In operation-hours gauges, two thin columns of [[mercury (element)|mercury]] are separated by a small electrolyte-filled gap, and, as charge is passed through the device, the metal dissolves on one side and plates out on the other, causing the visible gap to slowly move along. |
* In operation-hours gauges, two thin columns of [[mercury (element)|mercury]] are separated by a small electrolyte-filled gap, and, as charge is passed through the device, the metal dissolves on one side and plates out on the other, causing the visible gap to slowly move along. |
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*In [[electrolytic capacitor]]s the chemical effect is used to produce an extremely thin |
* In [[electrolytic capacitor]]s the chemical effect is used to produce an extremely thin [[dielectric]] or [[Electrical insulation|insulating]] coating, while the electrolyte layer behaves as one capacitor plate. |
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*In some [[hygrometer]]s the humidity of air is sensed by measuring the conductivity of a nearly dry electrolyte. |
* In some [[hygrometer]]s the humidity of air is sensed by measuring the conductivity of a nearly dry electrolyte. |
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*Hot, softened glass is an electrolytic conductor, and some glass manufacturers keep the glass molten by passing a large |
* Hot, softened glass is an electrolytic conductor, and some glass manufacturers keep the glass molten by passing a large current through it. |
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== Solid electrolytes == |
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==See also== |
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{{ |
{{Main|Fast-ion conductor|Solid-state electrolyte}} |
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Solid electrolytes can be mostly divided into four groups described below. |
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*[[Strong electrolyte]] |
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*[[Weak electrolyte]] |
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*[[Ionic atmosphere]] |
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=== Gel electrolytes === |
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==External links== |
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Gel electrolytes – closely resemble liquid electrolytes. In essence, they are liquids in a flexible [[crystal structure|lattice framework]]. Various [[Food additive|additive]]s are often applied to increase the [[Electrical conductivity|conductivity]] of such systems.<ref name="Kamil Perzyna, Regina Borkowska, Jaroslaw Syzdek, Aldona Zalewska, Wladyslaw Wieczorek 2011 58–65" /><ref name="dry">{{cite web |url=http://www.evworld.com/article.cfm?storyid=933 |title=The Roll-to-Roll Battery Revolution |publisher=Ev World |access-date=2010-08-20 |archive-url=https://web.archive.org/web/20110710210351/http://www.evworld.com/article.cfm?storyid=933 |archive-date=10 July 2011 |url-status=dead }}</ref> |
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*[http://www.disen.org/nutrition/pages-to-edit/fluids.htm Fluids and Hydration in Sport] - includes a discussion of the role of [[hypotonic]], [[isotonic]] and [[hypertonic]] drinks. |
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=== Ceramic electrolytes === |
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[[Category:Electrochemistry]] |
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Solid ceramic electrolytes – [[ion]]s migrate through the ceramic phase by means of vacancies or [[interstitial compound|interstitials]] within the [[Crystal lattice|lattice]]. There are also [[Glass-ceramic|glassy-ceramic]] electrolytes. |
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[[Category:Physical chemistry]] |
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[[Category:Physiology]] |
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=== Polymer electrolytes === |
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[[bg:Електролит]] |
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{{Main|Polymer electrolytes}} |
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[[ca:Electròlit]] |
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Dry polymer electrolytes – differ from liquid and gel electrolytes in the sense that salt is dissolved directly into the solid medium. Usually it is a relatively high-[[Relative permittivity|dielectric constant]] [[polymer]] ([[polyethylene oxide|PEO]], [[Poly(methyl methacrylate)|PMMA]], [[Polyacrylonitrile|PAN]], [[polyphosphazene]]s, [[siloxane]]s, etc.) and a salt with low [[lattice energy]]. In order to increase the [[mechanical strength]] and conductivity of such electrolytes, very often [[composite material|composites]] are made, and inert ceramic phase is introduced. There are two major classes of such electrolytes: polymer-in-ceramic, and ceramic-in-polymer.<ref name="SyzdekBorkowska2007">{{cite journal|vauthors=Syzdek J, Borkowska R, Perzyna K, Tarascon JM, Wieczorek W|title=Novel composite polymeric electrolytes with surface-modified inorganic fillers|journal=Journal of Power Sources|volume=173|issue=2|year=2007|pages=712–720|issn=0378-7753|doi=10.1016/j.jpowsour.2007.05.061|bibcode=2007JPS...173..712S}}</ref><ref name="SyzdekArmand2010">{{cite journal|vauthors=Syzdek J, Armand M, Marcinek M, Zalewska A, Żukowska G, Wieczorek W|title=Detailed studies on the fillers modification and their influence on composite, poly(oxyethylene)-based polymeric electrolytes|journal=Electrochimica Acta|volume=55|issue=4|year=2010|pages=1314–1322|issn=0013-4686|doi=10.1016/j.electacta.2009.04.025}}</ref><ref name="SyzdekArmand2009">{{cite journal|vauthors=Syzdek J, Armand M, Gizowska M, Marcinek M, Sasim E, Szafran M, Wieczorek W|title=Ceramic-in-polymer versus polymer-in-ceramic polymeric electrolytes—A novel approach|journal=Journal of Power Sources|volume=194|issue=1|year=2009|pages=66–72|issn=0378-7753|doi=10.1016/j.jpowsour.2009.01.070|bibcode=2009JPS...194...66S}}</ref> |
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[[cs:Elektrolyt]] |
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[[da:Elektrolyt]] |
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=== Organic plastic electrolytes === |
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[[de:Elektrolyt]] |
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Organic ionic plastic crystals – are a type [[salt (chemistry)|organic salts]] exhibiting [[mesophase]]s (i.e. a [[state of matter]] intermediate between liquid and solid), in which mobile ions are orientationally or rotationally disordered while their centers are located at the ordered sites in the crystal structure.<ref name="1,2,4-Triazolium perfluorobutanesulfonate as an archetypal pure protic organic ionic plastic crystal electrolyte for all-solid-state fuel cells" /> They have various forms of disorder due to one or more solid–solid [[phase transition]]s below the [[melting point]] and have therefore [[Plasticity (physics)|plastic]] properties and good mechanical flexibility as well as an improved electrode-electrolyte interfacial contact. In particular, protic organic ionic plastic crystals (POIPCs),<ref name="1,2,4-Triazolium perfluorobutanesulfonate as an archetypal pure protic organic ionic plastic crystal electrolyte for all-solid-state fuel cells"> |
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[[et:Elektrolüüt]] |
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{{cite journal |
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[[es:Electrolito]] |
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|author1=Jiangshui Luo |author2=Annemette H. Jensen |author3=Neil R. Brooks |author4=Jeroen Sniekers |author5=Martin Knipper |author6=David Aili |author7=Qingfeng Li |author8=Bram Vanroy |author9=Michael Wübbenhorst |author10=Feng Yan |author11=Luc Van Meervelt |author12=Zhigang Shao |author13=Jianhua Fang |author14=Zheng-Hong Luo |author15=Dirk E. De Vos |author16=Koen Binnemans |author17=Jan Fransaer |s2cid=84176511 |year=2015 |
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[[eo:Elektrolito]] |
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|title=1,2,4-Triazolium perfluorobutanesulfonate as an archetypal pure protic organic ionic plastic crystal electrolyte for all-solid-state fuel cells |
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[[fr:Électrolyte]] |
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|journal=[[Energy & Environmental Science]] |
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[[ko:전해질]] |
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|volume=8 |
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[[hr:Elektrolit]] |
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|issue=4 |pages=1276–1291 |doi=10.1039/C4EE02280G |
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[[io:Elektrolito]] |
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}}</ref> which are solid [[protic]] organic salts formed by [[proton]] transfer from a [[Brønsted–Lowry acid–base theory|Brønsted acid]] to a Brønsted base and in essence are protic [[ionic liquid]]s in the [[Molten salt|molten state]], have found to be promising solid-state [[proton conductor]]s for [[fuel cell]]s. Examples include [[Triazolium salt#1,4-disubstituted 1,2,4-triazolium salts|1,2,4-triazolium]] [[Nonaflate|perfluorobutanesulfonate]]<ref name="1,2,4-Triazolium perfluorobutanesulfonate as an archetypal pure protic organic ionic plastic crystal electrolyte for all-solid-state fuel cells" /> and [[Imidazole|imidazolium]] [[methanesulfonate]].<ref> |
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[[id:Elektrolit]] |
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{{cite journal |
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[[it:Elettrolita]] |
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|author1=Jiangshui Luo |author2=Olaf Conrad |author3=Ivo F. J. Vankelecom |s2cid=96622511 |year=2013 |
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[[lv:Elektrolīts]] |
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|title=Imidazolium methanesulfonate as a high temperature proton conductor |
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[[hu:Elektrolit]] |
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|journal=[[Journal of Materials Chemistry A]] |
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[[nl:Elektrolyt]] |
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|volume=1 |
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[[no:Elektrolytt]] |
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|issue=6 |pages=2238–2247 |doi=10.1039/C2TA00713D |
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[[ja:電解質]] |
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|url=https://lirias.kuleuven.be/handle/123456789/392330 }}</ref> |
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[[pl:Elektrolit]] |
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[[sk:Elektrolyt]] |
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== See also == |
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[[sl:Elektrolit]] |
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* [[Electrochemical machining]] |
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[[sr:Електролит]] |
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* [[Elektrolytdatenbank Regensburg]] |
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[[fi:Elektrolyytti]] |
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* [[Ion transport number]] |
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[[sv:Elektrolyt]] |
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* [[ITIES]] (interface between two immiscible electrolyte solutions) |
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[[th:อิเล็กโทรไลต์]] |
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[[ |
* [[Salt bridge]] |
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* [[Strong electrolyte]] |
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* [[Supporting electrolyte]] (background electrolyte) |
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* [[VTPR]] |
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== References == |
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{{Reflist}} |
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== External links == |
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* {{Commonscat-inline}} |
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* {{cite journal|doi=10.1063/1.1730863|title=Mayer's Ionic Solution Theory Applied to Electrolyte Mixtures |year=1960 |last1=Friedman |first1=Harold L. |journal=The Journal of Chemical Physics |volume=32 |issue=4 |pages=1134–1149 |bibcode=1960JChPh..32.1134F |doi-access=free }} |
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* {{cite journal|doi=10.1021/j150612a033|title=Multicomponent diffusion of electrolytes with incomplete dissociation. Diffusion in a buffer solution |year=1981 |last1=Leaist |first1=Derek G. |last2=Lyons |first2=Philip A. |journal=The Journal of Physical Chemistry |volume=85 |issue=12 |pages=1756–1762 }} |
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* {{cite journal|doi=10.1039/DF9572400171|title=Ion-solvent interaction and the viscosity of strong-electrolyte solutions |year=1957 |last1=Kaminsky |first1=Manfred |journal=Discussions of the Faraday Society |volume=24 |page=171 }} |
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{{Galvanic cells}} |
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{{Authority control}} |
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[[Category:Electrolytes| ]] |
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[[Category:Blood tests]] |
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[[Category:Urine tests]] |
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[[Category:Physical chemistry]] |
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[[Category:Acid–base physiology]] |
Latest revision as of 00:25, 17 December 2024
An electrolyte is a substance that conducts electricity through the movement of ions, but not through the movement of electrons.[1][2][3] This includes most soluble salts, acids, and bases, dissolved in a polar solvent like water. Upon dissolving, the substance separates into cations and anions, which disperse uniformly throughout the solvent.[4] Solid-state electrolytes also exist. In medicine and sometimes in chemistry, the term electrolyte refers to the substance that is dissolved.[5][6]
Electrically, such a solution is neutral. If an electric potential is applied to such a solution, the cations of the solution are drawn to the electrode that has an abundance of electrons, while the anions are drawn to the electrode that has a deficit of electrons. The movement of anions and cations in opposite directions within the solution amounts to a current. Some gases, such as hydrogen chloride (HCL), under conditions of high temperature or low pressure can also function as electrolytes.[clarification needed] Electrolyte solutions can also result from the dissolution of some biological (e.g., DNA, polypeptides) or synthetic polymers (e.g., polystyrene sulfonate), termed "polyelectrolytes", which contain charged functional groups. A substance that dissociates into ions in solution or in the melt acquires the capacity to conduct electricity. Sodium, potassium, chloride, calcium, magnesium, and phosphate in a liquid phase are examples of electrolytes.
In medicine, electrolyte replacement is needed when a person has prolonged vomiting or diarrhea, and as a response to sweating due to strenuous athletic activity. Commercial electrolyte solutions are available, particularly for sick children (such as oral rehydration solution, Suero Oral, or Pedialyte) and athletes (sports drinks). Electrolyte monitoring is important in the treatment of anorexia and bulimia.
In science, electrolytes are one of the main components of electrochemical cells.[2]
In clinical medicine, mentions of electrolytes usually refer metonymically to the ions, and (especially) to their concentrations (in blood, serum, urine, or other fluids). Thus, mentions of electrolyte levels usually refer to the various ion concentrations, not to the fluid volumes.
Etymology
[edit]The word electrolyte derives from Ancient Greek ήλεκτρο- (ēlectro-), prefix originally meaning amber but in modern contexts related to electricity, and λυτός (lytos), meaning "able to be untied or loosened".[citation needed]
History
[edit]In his 1884 dissertation, Svante Arrhenius put forth his explanation of solid crystalline salts disassociating into paired charged particles when dissolved, for which he won the 1903 Nobel Prize in Chemistry.[7][8][9][10] Arrhenius's explanation was that in forming a solution, the salt dissociates into charged particles, to which Michael Faraday (1791-1867) had given the name "ions" many years earlier. Faraday's belief had been that ions were produced in the process of electrolysis. Arrhenius proposed that, even in the absence of an electric current, solutions of salts contained ions. He thus proposed that chemical reactions in solution were reactions between ions.[8][9][10]
Shortly after Arrhenius's hypothesis of ions, Franz Hofmeister and Siegmund Lewith[11][12][13] found that different ion types displayed different effects on such things as the solubility of proteins. A consistent ordering of these different ions on the magnitude of their effect arises consistently in many other systems as well. This has since become known as the Hofmeister series.
While the origins of these effects are not abundantly clear and have been debated throughout the past century, it has been suggested that the charge density of these ions is important[14] and might actually have explanations originating from the work of Charles-Augustin de Coulomb over 200 years ago.
Formation
[edit]Electrolyte solutions are normally formed when salt is placed into a solvent such as water and the individual components dissociate due to the thermodynamic interactions between solvent and solute molecules, in a process called "solvation". For example, when table salt (sodium chloride), NaCl, is placed in water, the salt (a solid) dissolves into its component ions, according to the dissociation reaction:[citation needed]
- NaCl(s) → Na+(aq) + Cl−(aq)
It is also possible for substances to react with water, producing ions. For example, carbon dioxide gas dissolves in water to produce a solution that contains hydronium, carbonate, and hydrogen carbonate ions.[citation needed]
Molten salts can also be electrolytes as, for example, when sodium chloride is molten, the liquid conducts electricity. In particular, ionic liquids, which are molten salts with melting points below 100 °C,[15] are a type of highly conductive non-aqueous electrolytes and thus have found more and more applications in fuel cells and batteries.[16]
An electrolyte in a solution may be described as "concentrated" if it has a high concentration of ions, or "dilute" if it has a low concentration. If a high proportion of the solute dissociates to form free ions, the electrolyte is strong; if most of the solute does not dissociate, the electrolyte is weak. The properties of electrolytes may be exploited using electrolysis to extract constituent elements and compounds contained within the solution.[citation needed]
Alkaline earth metals form hydroxides that are strong electrolytes with limited solubility in water, due to the strong attraction between their constituent ions. This limits their application to situations where high solubility is required.[17]
In 2021, researchers have found that electrolyte can "substantially facilitate electrochemical corrosion studies in less conductive media".[18]
Physiological importance
[edit]In physiology, the primary ions of electrolytes are sodium (Na+), potassium (K+), calcium (Ca2+), magnesium (Mg2+), chloride (Cl−), hydrogen phosphate (HPO42−), and hydrogen carbonate (HCO3−).[19][failed verification] The electric charge symbols of plus (+) and minus (−) indicate that the substance is ionic in nature and has an imbalanced distribution of electrons, the result of chemical dissociation. Sodium is the main electrolyte found in extracellular fluid and potassium is the main intracellular electrolyte;[20] both are involved in fluid balance and blood pressure control.[21]
All known multicellular lifeforms require a subtle and complex electrolyte balance between the intracellular and extracellular environments.[19] In particular, the maintenance of precise osmotic gradients of electrolytes is important. Such gradients affect and regulate the hydration of the body as well as blood pH, and are critical for nerve and muscle function. Various mechanisms exist in living species that keep the concentrations of different electrolytes under tight control.[22]
Both muscle tissue and neurons are considered electric tissues of the body. Muscles and neurons are activated by electrolyte activity between the extracellular fluid or interstitial fluid, and intracellular fluid. Electrolytes may enter or leave the cell membrane through specialized protein structures embedded in the plasma membrane called "ion channels". For example, muscle contraction is dependent upon the presence of calcium (Ca2+), sodium (Na+), and potassium (K+). Without sufficient levels of these key electrolytes, muscle weakness or severe muscle contractions may occur.[citation needed][23]
Electrolyte balance is maintained by oral, or in emergencies, intravenous (IV) intake of electrolyte-containing substances, and is regulated by hormones, in general with the kidneys flushing out excess levels. In humans, electrolyte homeostasis is regulated by hormones such as antidiuretic hormones, aldosterone and parathyroid hormones. Serious electrolyte disturbances, such as dehydration and overhydration, may lead to cardiac and neurological complications and, unless they are rapidly resolved, will result in a medical emergency.
Measurement
[edit]Measurement of electrolytes is a commonly performed diagnostic procedure, performed via blood testing with ion-selective electrodes or urinalysis by medical technologists. The interpretation of these values is somewhat meaningless without analysis of the clinical history and is often impossible without parallel measurements of renal function. The electrolytes measured most often are sodium and potassium. Chloride levels are rarely measured except for arterial blood gas interpretations since they are inherently linked to sodium levels. One important test conducted on urine is the specific gravity test to determine the occurrence of an electrolyte imbalance.[citation needed]
Rehydration
[edit]According to a study paid for by the Gatorade Sports Science Institute, electrolyte drinks containing sodium and potassium salts replenish the body's water and electrolyte concentrations after dehydration caused by exercise, excessive alcohol consumption, diaphoresis (heavy sweating), diarrhea, vomiting, intoxication or starvation; the study says that athletes exercising in extreme conditions (for three or more hours continuously, e.g. a marathon or triathlon) who do not consume electrolytes risk dehydration (or hyponatremia).[24][needs independent confirmation]
A home-made electrolyte drink can be made by using water, sugar and salt in precise proportions.[25] It is important to include glucose (sugar) to utilise the co-transport mechanism of sodium and glucose. Commercial preparations are also available[26] for both human and veterinary use.
Electrolytes are commonly found in fruit juices, sports drinks, milk, nuts, and many fruits and vegetables (whole or in juice form) (e.g., potatoes, avocados).
Electrochemistry
[edit]When electrodes are placed in an electrolyte and a voltage is applied, the electrolyte will conduct electricity. Lone electrons normally cannot pass through the electrolyte; instead, a chemical reaction occurs at the cathode, providing electrons to the electrolyte. Another reaction occurs at the anode, consuming electrons from the electrolyte. As a result, a negative charge cloud develops in the electrolyte around the cathode, and a positive charge develops around the anode. The ions in the electrolyte neutralize these charges, enabling the electrons to keep flowing and the reactions to continue.[citation needed]
For example, in a solution of ordinary table salt (sodium chloride, NaCl) in water, the cathode reaction will be
- 2 H2O + 2e− → 2 OH− + H2
and hydrogen gas will bubble up; the anode reaction is
- 2 NaCl → 2 Na+ + Cl2 + 2e−
and chlorine gas will be liberated into solution where it reacts with the sodium and hydroxyl ions to produce sodium hypochlorite - household bleach. The positively charged sodium ions Na+ will react toward the cathode, neutralizing the negative charge of OH− there, and the negatively charged hydroxide ions OH− will react toward the anode, neutralizing the positive charge of Na+ there. Without the ions from the electrolyte, the charges around the electrode would slow down continued electron flow; diffusion of H+ and OH− through water to the other electrode takes longer than movement of the much more prevalent salt ions. Electrolytes dissociate in water because water molecules are dipoles and the dipoles orient in an energetically favorable manner to solvate the ions.
In other systems, the electrode reactions can involve the metals of the electrodes as well as the ions of the electrolyte.
Electrolytic conductors are used in electronic devices where the chemical reaction at a metal-electrolyte interface yields useful effects.
- In batteries, two materials with different electron affinities are used as electrodes; electrons flow from one electrode to the other outside of the battery, while inside the battery the circuit is closed by the electrolyte's ions. Here, the electrode reactions convert chemical energy to electrical energy.[27]
- In some fuel cells, a solid electrolyte or proton conductor connects the plates electrically while keeping the hydrogen and oxygen fuel gases separated.[28]
- In electroplating tanks, the electrolyte simultaneously deposits metal onto the object to be plated, and electrically connects that object in the circuit.
- In operation-hours gauges, two thin columns of mercury are separated by a small electrolyte-filled gap, and, as charge is passed through the device, the metal dissolves on one side and plates out on the other, causing the visible gap to slowly move along.
- In electrolytic capacitors the chemical effect is used to produce an extremely thin dielectric or insulating coating, while the electrolyte layer behaves as one capacitor plate.
- In some hygrometers the humidity of air is sensed by measuring the conductivity of a nearly dry electrolyte.
- Hot, softened glass is an electrolytic conductor, and some glass manufacturers keep the glass molten by passing a large current through it.
Solid electrolytes
[edit]Solid electrolytes can be mostly divided into four groups described below.
Gel electrolytes
[edit]Gel electrolytes – closely resemble liquid electrolytes. In essence, they are liquids in a flexible lattice framework. Various additives are often applied to increase the conductivity of such systems.[27][29]
Ceramic electrolytes
[edit]Solid ceramic electrolytes – ions migrate through the ceramic phase by means of vacancies or interstitials within the lattice. There are also glassy-ceramic electrolytes.
Polymer electrolytes
[edit]Dry polymer electrolytes – differ from liquid and gel electrolytes in the sense that salt is dissolved directly into the solid medium. Usually it is a relatively high-dielectric constant polymer (PEO, PMMA, PAN, polyphosphazenes, siloxanes, etc.) and a salt with low lattice energy. In order to increase the mechanical strength and conductivity of such electrolytes, very often composites are made, and inert ceramic phase is introduced. There are two major classes of such electrolytes: polymer-in-ceramic, and ceramic-in-polymer.[30][31][32]
Organic plastic electrolytes
[edit]Organic ionic plastic crystals – are a type organic salts exhibiting mesophases (i.e. a state of matter intermediate between liquid and solid), in which mobile ions are orientationally or rotationally disordered while their centers are located at the ordered sites in the crystal structure.[28] They have various forms of disorder due to one or more solid–solid phase transitions below the melting point and have therefore plastic properties and good mechanical flexibility as well as an improved electrode-electrolyte interfacial contact. In particular, protic organic ionic plastic crystals (POIPCs),[28] which are solid protic organic salts formed by proton transfer from a Brønsted acid to a Brønsted base and in essence are protic ionic liquids in the molten state, have found to be promising solid-state proton conductors for fuel cells. Examples include 1,2,4-triazolium perfluorobutanesulfonate[28] and imidazolium methanesulfonate.[33]
See also
[edit]- Electrochemical machining
- Elektrolytdatenbank Regensburg
- Ion transport number
- ITIES (interface between two immiscible electrolyte solutions)
- Salt bridge
- Strong electrolyte
- Supporting electrolyte (background electrolyte)
- VTPR
References
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External links
[edit]- Media related to Electrolytes at Wikimedia Commons
- Friedman HL (1960). "Mayer's Ionic Solution Theory Applied to Electrolyte Mixtures". The Journal of Chemical Physics. 32 (4): 1134–1149. Bibcode:1960JChPh..32.1134F. doi:10.1063/1.1730863.
- Leaist DG, Lyons PA (1981). "Multicomponent diffusion of electrolytes with incomplete dissociation. Diffusion in a buffer solution". The Journal of Physical Chemistry. 85 (12): 1756–1762. doi:10.1021/j150612a033.
- Kaminsky M (1957). "Ion-solvent interaction and the viscosity of strong-electrolyte solutions". Discussions of the Faraday Society. 24: 171. doi:10.1039/DF9572400171.