Unlike hydrogen fluoride, anhydrous liquid hydrogen chloride is difficult to work with as a solvent, because its boiling point is low, it has a small liquid range, its dielectric constant is low and it does not dissociate appreciably into H 2Cl + and HCl − a b Vinten-Johansen, Peter, Howard Brody, Nigel Paneth, Stephen Rachman and Michael Rip. (2003). Cholera, Chloroform, and the Science of Medicine. New York:Oxford University.

Chlorine forms four oxoacids: hypochlorous acid (HOCl), chlorous acid (HOClO), chloric acid (HOClO 2), and perchloric acid (HOClO 3). As can be seen from the redox potentials given in the adjacent table, chlorine is much more stable towards disproportionation in acidic solutions than in alkaline solutions: [41] Cl 2 + H 2O Once you’ve determined that chlorine needs to be added, with your pool pump running, pour the chlorine slowly into the deep end of the pool.

What Type of Chlorine Does an Automatic Chlorinator Use?

During the Paris cholera outbreak of 1832, large quantities of so-called chloride of lime were used to disinfect the capital. This was not simply modern calcium chloride, but chlorine gas dissolved in lime-water (dilute calcium hydroxide) to form calcium hypochlorite (chlorinated lime). Labarraque's discovery helped to remove the terrible stench of decay from hospitals and dissecting rooms, and by doing so, effectively deodorised the Latin Quarter of Paris. [77] These "putrid miasmas" were thought by many to cause the spread of "contagion" and "infection" – both words used before the germ theory of infection. Chloride of lime was used for destroying odors and "putrid matter". One source claims chloride of lime was used by Dr. John Snow to disinfect water from the cholera-contaminated well that was feeding the Broad Street pump in 1854 London, [78] though three other reputable sources that describe that famous cholera epidemic do not mention the incident. [79] [80] [81] One reference makes it clear that chloride of lime was used to disinfect the offal and filth in the streets surrounding the Broad Street pump – a common practice in mid-nineteenth century England. [79] :296 Semmelweis and experiments with antisepsis Ignaz Semmelweis

Facts About Chlorine". www.bt.cdc.gov. Archived from the original on 2016-04-23 . Retrieved 2016-04-12. {{ cite web}}: CS1 maint: bot: original URL status unknown ( link) R = Me, Et, Bu n) may still be isolated. Anhydrous hydrogen chloride is a poor solvent, only able to dissolve small molecular compounds such as nitrosyl chloride and phenol, or salts with very low lattice energies such as tetraalkylammonium halides. It readily protonates electrophiles containing lone-pairs or π bonds. Solvolysis, ligand replacement reactions, and oxidations are well-characterised in hydrogen chloride solution: [44] Ph 3SnCl + HCl ⟶ Ph 2SnCl 2 + PhH (solvolysis) Ph 3COH + 3 HCl ⟶ Ph Chloramines & Pool Operation". Centres for Disease Control and Prevention . Retrieved 13 March 2022. Most of the chlorine oxoacids may be produced by exploiting these disproportionation reactions. Hypochlorous acid (HOCl) is highly reactive and quite unstable; its salts are mostly used for their bleaching and sterilising abilities. They are very strong oxidising agents, transferring an oxygen atom to most inorganic species. Chlorous acid (HOClO) is even more unstable and cannot be isolated or concentrated without decomposition: it is known from the decomposition of aqueous chlorine dioxide. However, sodium chlorite is a stable salt and is useful for bleaching and stripping textiles, as an oxidising agent, and as a source of chlorine dioxide. Chloric acid (HOClO 2) is a strong acid that is quite stable in cold water up to 30% concentration, but on warming gives chlorine and chlorine dioxide. Evaporation under reduced pressure allows it to be concentrated further to about 40%, but then it decomposes to perchloric acid, chlorine, oxygen, water, and chlorine dioxide. Its most important salt is sodium chlorate, mostly used to make chlorine dioxide to bleach paper pulp. The decomposition of chlorate to chloride and oxygen is a common way to produce oxygen in the laboratory on a small scale. Chloride and chlorate may comproportionate to form chlorine as follows: [55] ClO −Lefebure, Victor; Wilson, Henry (2004). The Riddle of the Rhine: Chemical Strategy in Peace and War. Kessinger Publishing. ISBN 978-1-4179-3546-8. Chlorination of metals with Cl 2 usually leads to a higher oxidation state than bromination with Br 2 when multiple oxidation states are available, such as in MoCl 5 and MoBr 3. Chlorides can be made by reaction of an element or its oxide, hydroxide, or carbonate with hydrochloric acid, and then dehydrated by mildly high temperatures combined with either low pressure or anhydrous hydrogen chloride gas. These methods work best when the chloride product is stable to hydrolysis; otherwise, the possibilities include high-temperature oxidative chlorination of the element with chlorine or hydrogen chloride, high-temperature chlorination of a metal oxide or other halide by chlorine, a volatile metal chloride, carbon tetrachloride, or an organic chloride. For instance, zirconium dioxide reacts with chlorine at standard conditions to produce zirconium tetrachloride, and uranium trioxide reacts with hexachloropropene when heated under reflux to give uranium tetrachloride. The second example also involves a reduction in oxidation state, which can also be achieved by reducing a higher chloride using hydrogen or a metal as a reducing agent. This may also be achieved by thermal decomposition or disproportionation as follows: [45] EuCl 3 + 1 / 2 H 2 ⟶ EuCl 2 + HCl ReCl 5 at "bp" ⟶ ReCl 3 + Cl 2 AuCl 3 160°C ⟶ AuCl + Cl 2

Given that E°( 1 / 2O 2/H 2O) = +1.229V, which is less than +1.395V, it would be expected that chlorine should be able to oxidise water to oxygen and hydrochloric acid. However, the kinetics of this reaction are unfavorable, and there is also a bubble overpotential effect to consider, so that electrolysis of aqueous chloride solutions evolves chlorine gas and not oxygen gas, a fact that is very useful for the industrial production of chlorine. [41] Hydrogen chloride Structure of solid deuterium chloride, with D···Cl hydrogen bonds a b Hoefer, Jean Chrétien Ferdinand (ed.). "Labarraque, Antoine-Germain". Nouvelle biographie universelle. Vol.28. pp.323–24. OL 24229911M. Koski T. A.; Stuart L. S.; Ortenzio L. F. (1966). "Comparison of chlorine, bromine, iodine as disinfectants for swimming pool water". Applied Microbiology. 14 (2): 276–79. doi: 10.1128/AEM.14.2.276-279.1966. PMC 546668. PMID 4959984. NOAA Office of Response and Restoration, US GOV. "Chlorine". noaa.gov. Archived from the original on 15 October 2015 . Retrieved 25 August 2015. O'Connor J. J.; Robertson E. F. "Michael Faraday". School of Mathematics and Statistics, University of St Andrews, Scotland. Archived from the original on 2010-02-20 . Retrieved 2010-05-08.Kondev, F. G.; Wang, M.; Huang, W. J.; Naimi, S.; Audi, G. (2021). "The NUBASE2020 evaluation of nuclear properties" (PDF). Chinese Physics C. 45 (3): 030001. doi: 10.1088/1674-1137/abddae. Syrian forces 'drop chlorine' on Aleppo". BBC News. 2016-09-07. Archived from the original on 2017-05-13 . Retrieved 2017-05-10.

van Helmont, Joannis Baptistae (1682). Opera omnia [All Works] (in Latin). Frankfurt-am-Main, (Germany): Johann Just Erythropel. From "Complexionum atque mistionum elementalium figmentum." (Formation of combinations and of mixtures of elements), §37, p. 105: "Accipe salis petrae, vitrioli, & alumnis partes aequas: exsiccato singula, & connexis simul, distilla aquam. Quae nil aliud est, quam merum sal volatile. Hujus accipe uncias quatuor, salis armeniaci unciam junge, in forti vitro, alembico, per caementum (ex cera, colophonia, & vitri pulverre) calidissime affusum, firmato; mox, etiam in frigore, Gas excitatur, & vas, utut forte, dissilit cum fragore." (Take equal parts of saltpeter [i.e., sodium nitrate], vitriol [i.e., concentrated sulfuric acid], and alum: dry each and combine simultaneously; distill off the water [i.e., liquid]. That [distillate] is nothing else than pure volatile salt [i.e., spirit of nitre, nitric acid]. Take four ounces of this [viz, nitric acid], add one ounce of Armenian salt [i.e., ammonium chloride], [place it] in a strong glass alembic sealed by cement ([made] from wax, rosin, and powdered glass) [that has been] poured very hot; soon, even in the cold, gas is stimulated, and the vessel, however strong, bursts into fragments.) From "De Flatibus" (On gases), p. 408: "Sal armeniacus enim, & aqua chrysulca, quae singula per se distillari, possunt, & pati calorem: sin autem jungantur, & intepescant, non possunt non, quin statim in Gas sylvestre, sive incoercibilem flatum transmutentur." (Truly Armenian salt [i.e., ammonium chloride] and nitric acid, each of which can be distilled by itself, and submitted to heat; but if, on the other hand, they be combined and become warm, they cannot but be changed immediately into carbon dioxide [note: van Helmont's identification of the gas is mistaken] or an incondensable gas.) In addition to providing a residual, adding chlorine to water will also: oxidize iron, manganese, taste and odour compounds, remove colour in the water, destroy hydrogen sulphide, and aid other water treatment processes, such as sedimentation and filtration. Oxidizing soluble reduced iron and manganese will result in particle formation as oxidized iron and manganese are not soluble in water. Is Chlorine All the Same? Rezayat, C.; Widmann, W. D.; Hardy, M. A. (2006). "Henry Drysdale Dakin: More Than His Solution". Current Surgery. 63 (3): 194–96. doi: 10.1016/j.cursur.2006.04.009. PMID 16757372.Most products you buy will be for about 10,000 gallons of pool water, so if your pool is larger than that, you will need more product. The chlorine oxides are well-studied in spite of their instability (all of them are endothermic compounds). They are important because they are produced when chlorofluorocarbons undergo photolysis in the upper atmosphere and cause the destruction of the ozone layer. None of them can be made from directly reacting the elements. [53] UV rays will eat up your chlorine like yesterday’s lunch if you don’t have anything in the pool to protect it—this means you’re constantly having to add more chlorine, costing time and money.