query: propan 2 ol on reaction with iodine and sodium hydroxide gives

pos: Haloform reaction methyl ketone. When iodine and sodium hydroxide are used as the reagents a positive reaction gives iodoform, which is a solid at room temperature and tends to precipitate out of solution causing a distinctive cloudiness. In organic chemistry, this reaction may be used to convert a terminal methyl ketone into the analogous carboxylic acid. It was formerly used to produce iodoform, bromoform, and even chloroform industrially. Water chlorination can result in the formation of haloforms if the water contains suitable reactive impurities (e.g. humic acid). There is a concern that such reactions may lead to the presence of carcinogenic compounds

pos: Iodoform by reaction of potassium with ethanolic iodine in the presence of water; and at much the same time independently by John Thomas Cooper. It is synthesized in the haloform reaction by the reaction of iodine and sodium hydroxide with any one of these four kinds of organic compounds: a methyl ketone (CHCOR), acetaldehyde (CHCHO), ethanol (CHCHOH), and certain secondary alcohols (CHCHROH, where R is an alkyl or aryl group). The reaction of iodine and base with methyl ketones is so reliable that the "iodoform test" (the appearance of a yellow precipitate) is used to probe the presence of a methyl

neg: Favorskii reaction are inexpensive relative to generating an alkoxide or acetylide with reagents such as elemental lithium, sodium, or potassium. Additionally, the stringent reaction conditions used by most alternatives, such as excluding moisture and atmospheric oxygen, are less important, making the reaction easier to perform. This reaction is used to protect alkynes: the alkyne is either converted with acetone to a 2-hydroxyprop-2-yl-alkyne or a protected alkyne can be directly synthesized using the commercially available 2-methyl-3-butyn-2-ol as an the alkyne source. The protective group can be removed by heating the compound in a solution of potassium hydroxide in propan-2-ol (a retro-Favorskii reaction). Favorskii

neg: Allylic rearrangement process referred to as S2' substitution. This is likely in cases when the allyl compound is unhindered, and a strong nucleophile is used. The products will be similar to those seen with S1' substitution. Thus reaction of 1-chloro-2-butene with sodium hydroxide gives a mixture of 2-buten-1-ol and 3-buten-2-ol: Nevertheless, the product in which the OH group is on the primary atom is minor. In the substitution of 1-chloro-3-methyl-2-butene, the tertiary 2-methyl-3-buten-2-ol is produced in a yield of 85%, while that for the primary 3-methyl-2-buten-1-ol is 15%. In one reaction mechanism the nucleophile attacks not directly at the electrophilic site but

neg: Iodine-123 proton to form xenon-123, or else loses two neutrons to form caesium-123, which decays to xenon-123. The xenon-123 formed by either route then decays to iodine-123, and is collected on the side of the capsule under refrigeration, then eluted with dilute sodium hydroxide in a halogen disproportionation reaction, similar to collection of iodine-125 after it is formed from xenon by neutron irradiation (see that article for more). Iodine-123 is usually supplied as []-sodium iodide in dilute sodium hydroxide solution (0.1 N), at 99.8% isotopic purity. I-123 for medical applications has also been produced at Oak Ridge National Laboratories by proton

neg: Sodium peroxide is produced by treating sodium hydroxide with hydrogen peroxide. Sodium peroxide can be prepared on a large scale by the reaction of metallic sodium with oxygen at 130–200 °C, a process that generates sodium oxide, which in a separate stage absorbs oxygen: It may also be produced by passing ozone gas over solid sodium iodide inside a platinum or palladium tube. The ozone oxidizes the sodium to form sodium peroxide. The iodine can be sublimed by mild heating. The platinum or palladium catalyzes the reaction and is not attacked by the sodium peroxide. Sodium peroxide hydrolyzes to give sodium hydroxide

neg: Carvone of reduction; the product of reduction depends on the reagents and conditions used. Catalytic hydrogenation of carvone (1) can give either carvomenthol (2) or carvomenthone (3). Zinc and acetic acid reduce carvone to give dihydrocarvone (4). MPV reduction using propan-2-ol and aluminium isopropoxide effects reduction of the carbonyl group only to provide carveol (5); a combination of sodium borohydride and CeCl (Luche reduction) is also effective. Hydrazine and potassium hydroxide give limonene (6) via a Wolff-Kishner reduction. Oxidation of carvone can also lead to a variety of products. In the presence of an alkali such as Ba(OH), carvone is oxidised

neg: 1-Propanol 1-Propanol 1-Propanol is a primary alcohol with the formula CHCHCHOH (sometimes represented as PrOH or n"-PrOH). This colorless liquid is also known as propan-1-ol, 1-propyl alcohol, n"-propyl alcohol, and "n"-propanol. It is an isomer of 2-propanol (propan-2-ol, isopropyl alcohol, isopropanol). It is formed naturally in small amounts during many fermentation processes and used as a solvent in the pharmaceutical industry mainly for resins and cellulose esters. 1-Propanol shows the normal reactions of a primary alcohol. Thus it can be converted to alkyl halides; for example red phosphorus and iodine produce n-propyl iodide in 80% yield, while PCl with catalytic ZnCl

neg: 1-Propanol of propanol is 118 and anti-knock index (AKI) is 108. 1-Propanol 1-Propanol is a primary alcohol with the formula CHCHCHOH (sometimes represented as PrOH or n"-PrOH). This colorless liquid is also known as propan-1-ol, 1-propyl alcohol, n"-propyl alcohol, and "n"-propanol. It is an isomer of 2-propanol (propan-2-ol, isopropyl alcohol, isopropanol). It is formed naturally in small amounts during many fermentation processes and used as a solvent in the pharmaceutical industry mainly for resins and cellulose esters. 1-Propanol shows the normal reactions of a primary alcohol. Thus it can be converted to alkyl halides; for example red phosphorus and iodine produce

neg: Universal indicator Universal indicator A universal indicator is a pH indicator made of a solution of several compounds that exhibits several smooth colour changes over a wide range pH values to indicate the acidity or alkalinity of solutions. Although there are several commercially available universal pH indicators, most are a variation of a formula patented by Yamada in 1933. Details of this patent can be found in "Chemical Abstracts". Experiments with Yamada's universal indicator are also described in the "Journal of Chemical Education". A universal indicator is typically composed of water, propan-1-ol, phenolphthalein sodium salt, sodium hydroxide, methyl red, bromothymol blue monosodium

neg: Nucleophilic substitution at the γ unsaturated carbon in place of the carbon bearing the leaving group. This may be seen in the reaction of 1-chloro-2-butene with sodium hydroxide to give a mixture of 2-buten-1-ol and 1-buten-3-ol: The Sn1CB mechanism appears in inorganic chemistry. Competing mechanisms exist. In organometallic chemistry the nucleophilic abstraction reaction occurs with a nucleophilic substitution mechanism. Nucleophilic substitution via the S1 or S2 mechanism does not generally occur with vinyl or aryl halides or related compounds. Under certain conditions nucleophilic substitutions may occur, via other mechanisms such as those described in the nucleophilic aromatic substitution article. When the substitution

neg: Sodium iodide even bromide: Sodium iodide Sodium iodide (chemical formula NaI) is an ionic compound formed from the chemical reaction of sodium metal and iodine. Under standard conditions, it is a white, water-soluble solid comprising a 1:1 mix of sodium cations (Na) and iodide anions (I) in a crystal lattice. It is used mainly as a nutritional supplement and in organic chemistry. It is produced industrially as the salt formed when acidic iodides react with sodium hydroxide. Sodium iodide, as well as potassium iodide, is commonly used to treat and prevent iodine deficiency. Iodized table salt contains 10 ppm iodide. Sodium iodide

neg: Sodium iodide Sodium iodide Sodium iodide (chemical formula NaI) is an ionic compound formed from the chemical reaction of sodium metal and iodine. Under standard conditions, it is a white, water-soluble solid comprising a 1:1 mix of sodium cations (Na) and iodide anions (I) in a crystal lattice. It is used mainly as a nutritional supplement and in organic chemistry. It is produced industrially as the salt formed when acidic iodides react with sodium hydroxide. Sodium iodide, as well as potassium iodide, is commonly used to treat and prevent iodine deficiency. Iodized table salt contains 10 ppm iodide. Sodium iodide is used

neg: Sodium bifluoride reacts with acids to give HF. Illustrative is its reaction with bisulfate to form sodium sulfate and hydrogen fluoride. Strong bases deprotonate bilfluoride. For example, calcium hydroxide gives calcium fluoride. Sodium bifluoride is produced by neutralizing waste hydrogen fluoride, which results from the production of superphosphate fertilizers. Typical bases are sodium carbonate and sodium hydroxide. The process occurs in two steps, illustrated with the hydroxide: Sodium bifluoride reacts with water or moist skin to produce hydrofluoric acid. It also gives off hydrofluoric acid and hydrogen gas when it is heated to a gaseous state. The chemical can decompose upon contact

neg: Sodium tungstate carbide with a mixture of sodium nitrate and sodium hydroxide in a fusion process which overcomes the high exothermicity of the reaction involved. Several polymorphs of sodium tungstate are known, three at only one atmosphere pressure. They feature tetrahedral orthotungstate dianions but differ in the packing motif. The WO anion adopts a structure like sulfate (SO). Treatment of sodium tungstate with hydrochloric acid gives the trioxide: This reaction can be reversed using aqueous solution of sodium hydroxide In organic chemistry, sodium tungstate is used as catalyst for epoxidation of alkenes and oxidation of alcohols into aldehydes or ketones. It is

neg: Xanthate salts are produced by the reaction of an alkoxide salt with carbon disulfide. The reaction involves the attack of the alkoxide nucleophile on the electrophile CS. Often the alkoxide is generated in situ by treating the alcohol with sodium or potassium hydroxide: For example, sodium ethoxide gives sodium ethyl xanthate. Many alcohols can be used in this reaction. Technical grade xanthate salts are usually of 90–95% purity. Impurities include alkali-metal sulfides, sulfates, trithiocarbonates, thiosulfates, sulfites, or carbonates as well as residual raw material such as alcohol and alkali hydroxide. These salts are available commercially as powder, granules, flakes, sticks, and

neg: Sodium nitrate natural sources. Chile still has the largest reserves of caliche,with active mines in such locations as Pedro de Valdivia, María Elena and Pampa Blanca, and there it used to be called "white gold". Sodium nitrate, potassium nitrate, sodium sulfate and iodine are all obtained by the processing of caliche. The former Chilean saltpeter mining communities of Humberstone and Santa Laura were declared Unesco World Heritage sites in 2005. Sodium nitrate is also synthesized industrially by neutralizing nitric acid with sodium carbonate or sodium bicarbonate: or also by neutralizing it with sodium hydroxide (however, this reaction is very exothermic): or by

neg: Aromatic hydrocarbon in the formation of new carbon–carbon bonds e.g., alkylarenes, vinyl arenes, biraryls, new carbon–nitrogen bonds (anilines) or new carbon–oxygen bonds (aryloxy compounds). An example is the direct arylation of perfluorobenzenes Hydrogenation of arenes create saturated rings. The compound 1-naphthol is completely reduced to a mixture of decalin-ol isomers. The compound resorcinol, hydrogenated with Raney nickel in presence of aqueous sodium hydroxide forms an enolate which is alkylated with methyl iodide to 2-methyl-1,3-cyclohexandione: Cycloaddition reaction are not common. Unusual thermal Diels–Alder reactivity of arenes can be found in the Wagner-Jauregg reaction. Other photochemical cycloaddition reactions with alkenes occur through excimers. In

neg: Alkali soil irrigation and/or flood water. Sodium carbonate in water can produce carbon dioxide (CO), escaping as a gas or absorbed by Algae, and sodium hydroxide (NaOH), which is alkaline (or rather basic) and gives high pH values (pH>8.5). The reaction between NaCO and HO can be represented as follows: Carbonic acid HCO is unstable and produces HO (water) and CO (carbon dioxide gas, escaping into the atmosphere). This explains the remaining alkalinity (or rather basicity) in the form of soluble sodium hydroxide and the high pH or low pOH. Not all the dissolved sodium carbonate undergoes the above chemical reaction. The

neg: Sodium tetrathionate Sodium tetrathionate Sodium tetrathionate is a salt of sodium and tetrathionate with the formula NaSOHO. The salt normally is obtained as the dihydrate ( = 2). It is a colorless, water-soluble solid. It is one member of the polythionates, which have the formula [S(SO)]. Other members include trithionite ( = 1), pentathionate ( = 3), hexathionate ( = 4). Sodium tetrathionate is formed by the oxidation of sodium thiosulfate (NaSO), e.g. by the action of iodine:. The reaction is signaled by the decoloration of iodine. This reaction is the basis of iodometric titrations. Other methods include the couping of sodium

neg: Triiodide Lugol's iodine contains potassium iodide and a stoichiometric amount of elemental iodine, so that significant amounts of triiodide ion exist in this solution. Tincture of iodine, although nominally a solution of elemental iodine in ethanol, also contains significant amounts of triiodide, due to its content of both iodide and water. The following exergonic equilibrium gives rise to the triiodide ion: In this reaction, iodide is viewed as a Lewis base, and the iodine is a Lewis acid. The process is analogous to the reaction of S with sodium sulfide, except that the higher polyiodides have branched structures. Triiodide In chemistry,

neg: Sodium hydroxide converted to soap. Despite solubility in propylene glycol it is unlikely to replace water in saponificaction due to propylene glycol primary reaction with fat before reaction between sodium hydroxide and fat. Sodium hydroxide is industrially produced as a 50% solution by variations of the electrolytic chloralkali process. Chlorine gas is also produced in this process. Solid sodium hydroxide is obtained from this solution by the evaporation of water. Solid sodium hydroxide is most commonly sold as flakes, prills, and cast blocks. In 2004, world production was estimated at 60 million dry metric tonnes of sodium hydroxide, and demand was estimated

neg: Sodium hydroxide burns may result if the area is not washed thoroughly and for several minutes with running water. Splashes in the eye can be more serious and can lead to blindness. Strong bases attack aluminium. Sodium hydroxide reacts with aluminium and water to release hydrogen gas. The aluminium takes the oxygen atom from sodium hydroxide, which in turn takes the oxygen atom from the water, and releases the two hydrogen atoms, The reaction thus produces hydrogen gas and sodium aluminate. In this reaction, sodium hydroxide acts as an agent to make the solution alkaline, which aluminium can dissolve in. This reaction

neg: Sodium hydroxide frosts the glass. Sodium hydroxide does not attack iron at room temperatures, since iron does not have amphoteric properties (i.e., it only dissolves in acid, not base). Nevertheless at high temperatures (e.g. above 500°C), iron can react endothermically with sodium hydroxide to form iron(III) oxide, sodium metal, and hydrogen gas. This is due to the lower enthalpy of formation of iron(III) oxide (-824.2kJ/mol) compared to sodium hydroxide (-427kJ/mol), thus the reaction is thermodynamically favorable, although its endothermic nature indicates non-spontaneity. Consider the following reaction between molten sodium hydroxide and finely divided iron filings: A few transition metals, however, may react

neg: Total base number relative changes that occur in an oil sample during its use under oxidising conditions. A sample is dissolved in a solvent mixture of Toluene/ Propan-2-ol with 0.5% deionised water. A methyl orange indicator is added and the solution is titrated using alcoholic potassium hydroxide. The end point is indicated by a colour change from orange to green. In thermometric titrations, a constant addition rate of titrant equates to a constant amount of heat being given out or consumed, and hence a more or less constant temperature change up to the endpoint. In a titration, the titrant reacts with the analyte

neg: Sodium sulfite Sodium sulfite can be prepared in lab by reacting sodium hydroxide solution with sulfur dioxide gas: Evolution of SO by adding few drops of concentrated hydrochloric acid will indicate if sodium hydroxide is nearly gone, turned to aqueous sodium sulfite: Sodium sulfite is made industrially by reacting sulfur dioxide with a solution of sodium carbonate. The initial combination generates sodium bisulfite (NaHSO), which is converted to the sulfite by reaction with sodium hydroxide or sodium carbonate. The overall reaction is: Sodium sulfite is primarily used in the pulp and paper industry. It is used in water treatment as an oxygen

neg: Zinc hydroxide hydroxide ions causes a similar reaction as sodium hydroxide and creates a +2 charged complex with a co-ordination number of 4 with the ammonia ligands - this makes the complex soluble so that it dissolves. One major use is as an absorbent in surgical dressings. It is also used to find zinc salts by mixing sodium hydroxide with the suspect salt. Zinc hydroxide Zinc hydroxide Zn(OH) is an inorganic chemical compound. It also occurs naturally as 3 rare minerals: wülfingite (orthorhombic), ashoverite and sweetite (both tetragonal). Like the hydroxides of other metals, such as lead, aluminium, beryllium, tin and chromium,

neg: Sodium iodate organic compounds, carbon, hydrogen peroxide, sulfides. Sodium iodate Sodium iodate (NaIO) is the sodium salt of iodic acid. Sodium iodate is an oxidizing agent, and as such it can cause fires upon contact with combustible materials or reducing agents. It can be prepared by reacting a sodium-containing base such as sodium hydroxide with iodic acid, for example: It can also be prepared by adding iodine to a hot, concentrated solution of sodium hydroxide or its carbonate: Sodium iodate can be oxidized to sodium periodate in water solutions by hypochlorites or other strong oxidizing agents: Conditions/substances to avoid are: heat, shock,

neg: Sodium iodate Sodium iodate Sodium iodate (NaIO) is the sodium salt of iodic acid. Sodium iodate is an oxidizing agent, and as such it can cause fires upon contact with combustible materials or reducing agents. It can be prepared by reacting a sodium-containing base such as sodium hydroxide with iodic acid, for example: It can also be prepared by adding iodine to a hot, concentrated solution of sodium hydroxide or its carbonate: Sodium iodate can be oxidized to sodium periodate in water solutions by hypochlorites or other strong oxidizing agents: Conditions/substances to avoid are: heat, shock, friction, combustible materials, reducing materials, aluminium,

neg: Alcohol and where precise identification of the substance is important, especially in cases where the relative complexity of the molecule does not make such a systematic name unwieldy. In naming simple alcohols, the name of the alkane chain loses the terminal "e" and adds the suffix "-ol", "e.g.", as in "ethanol" from the alkane chain name "ethane". When necessary, the position of the hydroxyl group is indicated by a number between the alkane name and the "-ol": propan-1-ol for , propan-2-ol for . If a higher priority group is present (such as an aldehyde, ketone, or carboxylic acid), then the prefix

neg: Dicopper chloride trihydroxide It can easily be converted to copper hydroxide by reacting with sodium hydroxide (eq. 2). Its pH in water is 6.9 measured by EPA method SW846-9045. Most of the published scientific literature on the properties of the compound has focused on specimens found as natural minerals or corrosion products on copper alloys, or prepared under laboratory conditions. Cu(OH)Cl can be prepared by hydrolysis of a CuCl solution at pH 4 ~7. A variety of bases such as sodium carbonate, ammonium, calcium, or sodium hydroxide may be used (eq. 3). Cu(OH)Cl can also be prepared by the reaction of a hot

neg: Potassium hydroxide KOH was made by adding potassium carbonate to a strong solution of calcium hydroxide (slaked lime) The salt metathesis reaction results in precipitation of solid calcium carbonate, leaving potassium hydroxide in solution: Filtering off the precipitated calcium carbonate and boiling down the solution gives potassium hydroxide ("calcinated or caustic potash"). This method of producing potassium hydroxide remained dominnt until the late 19th century, when it was largely replaced by the current method of electrolysis of potassium chloride solutions. The method is analogous to the manufacture of sodium hydroxide (see chloralkali process): Hydrogen gas forms as a byproduct on the cathode;

neg: Oxime related reaction is the Japp–Klingemann reaction. The hydrolysis of oximes proceeds easily by heating in the presence of various inorganic acids, and the oximes decompose into the corresponding ketones or aldehydes, and hydroxylamines. The reduction of oximes by sodium metal, sodium amalgam, hydrogenation, or reaction with hydride reagents produces amines. Typically the reduction of aldoximes gives both primary amines and secondary amines; however, reaction conditions can be altered (such as the addition of potassium hydroxide in a 1/30 molar ratio) to yield solely primary amines. In general, oximes can be changed to the corresponding amide derivatives by treatment with various

neg: Iodine clock reaction by the bisulfite) to form the dark blue complex with starch. This clock reaction uses sodium, potassium or ammonium persulfate to oxidize iodide ions to iodine. Sodium thiosulfate is used to reduce iodine back to iodide before the iodine can complex with the starch to form the characteristic blue-black color. Iodine is generated: And is then removed: Once all the thiosulfate is consumed the iodine may form a complex with the starch. Potassium persulfate is less soluble (cfr. Salters website) while ammonium persulfate has a higher solubility and is used instead in the reaction described in examples from Oxford University.

neg: Sodium hydroxide vigorously with sodium hydroxide. In 1986, an aluminium road tanker in the UK was mistakenly used to transport 25% sodium hydroxide solution, causing pressurization of the contents and damage to the tanker. The pressurization was due to the hydrogen gas which is produced in the reaction between sodium hydroxide and aluminium: Unlike sodium hydroxide, the hydroxides of most transition metals are insoluble, and therefore sodium hydroxide can be used to precipitate transition metal hydroxides. The following colours are observed: blue-copper, green-iron(II), yellow/brown-iron(III). Zinc and lead salts dissolve in excess sodium hydroxide to give a clear solution of NaZnO or NaPbO.

neg: Carbonyl oxidation with hypervalent iodine reagents silyl enol ethers as substrates and peracids as oxidants. Oxidative rearrangements are generally easier to accomplish using hypervalent iodine reagents than other oxidizing agents. The Willgerodt-Kindler reaction of alkyl aryl ketones, for instance, requires forcing conditions and often gives low yields of amide products. Hydroxy(mesyloxy)iodobenzene (3.16 g, 10 mmol) was added to a solution of the methyl trimethylsilyl phenylketene acetal derived from methyl phenylacetate (3.33 g, 15 mmol) in dry dichloromethane (50 mL). The mixture was stirred at room temperature for 2 hours and then washed with aqueous sodium bicarbonate solution (3 × 50 mL). The organic phase was dried

neg: Sodium formate reaction of formaldehyde with the aldol reaction product trimethylol acetaldehyde [3-hydroxy-2,2-bis(hydroxymethyl)propanal]. In the laboratory, sodium formate can be prepared by neutralizing formic acid with sodium carbonate. It can also be obtained by reacting chloroform with an alcoholic solution of sodium hydroxide. or by reacting sodium hydroxide with chloral hydrate. The latter method is, in general, preferred to the former because the low aqueous solubility of CHCl makes it easier to separate out from the sodium formate solution, by fractional crystallization, than the soluble NaCl would be. Sodium formate may also be created via the haloform reaction between ethanol and sodium

neg: Castner–Kellner process the mercury to transport the dissolved sodium metal from the outside cells to the center cell. The anode reaction in the center cell takes place at the interface between the mercury and the sodium hydroxide solution. Finally at the iron cathode (D) of the center cell the reaction is The net effect is that the concentration of sodium chloride in the outside cells decreases and the concentration of sodium hydroxide in the center cell increases. As the process continues some sodium hydroxide solution is withdrawn from center cell as output product and is replaced with water. Sodium chloride is added

neg: Thermometric titration oxalate is undesirable due to the toxicity of the reagent. A thermometric titration was devised by diluting the aliquot with propan-2-ol and titration with standard KOH in propan-2-ol. Most of the metal content precipitated prior to the commencement of the titration, and a clear, sharp endpoint for the sulfuric acid content was obtained. The determination of trace acids in organic matrices is a common analytical task assigned to titrimetry. Examples are Total Acid Number (TAN) in mineral and lubricating oils and Free Fatty Acids (FFA) in edible fats and oils. Automated potentiometric titration procedures have been granted standard method status,

neg: Sodium selenite Sodium selenite Sodium selenite is the inorganic compound with the formula NaSeO. This salt is a colourless solid. The pentahydrate NaSeO(HO) is the most common water-soluble selenium compound. Sodium selenite usually is prepared by the reaction of selenium dioxide with sodium hydroxide: The hydrate converts to the anhydrous salt upon heating to 40 °C. Akin to the related salt sodium sulfite, NaSeO features a pyramidal dianion SeO. Oxidation of this anion gives sodium selenate, NaSeO. Together with the related barium and zinc selenites, sodium selenite is mainly used in the manufacture of colorless glass. The pink color imparted by these

neg: Iodine clock reaction cycle from colorless to blue and back to colorless, until the reagents are depleted. This reaction starts from a solution of hydrogen peroxide with sulfuric acid. To this is added a solution containing potassium iodide, sodium thiosulfate, and starch. There are two reactions occurring in the solution. In the first, slow reaction, iodine is produced: HO + 2I + 2H → I + 2HO In the second, fast reaction, iodine is reconverted to 2 iodide ions by the thiosulfate: 2SO + I → SO + 2I After some time the solution always changes color to a very dark blue, almost

neg: Wenker synthesis of the intermediate. The Wenker synthesis protocol using "trans"-2-aminocyclooctanol, available from reaction of ammonia with the epoxide of cyclooctene, gives a mixture of cyclooctenimine (the Wenker aziridine product) and cyclooctanone (a competing Hofmann elimination product). Wenker synthesis The Wenker synthesis is an organic reaction converting a beta amino alcohol to an aziridine with the aid of sulfuric acid. The original Wenker synthesis of aziridine itself takes place in two steps. In the first step ethanolamine is reacted with sulfuric acid at high temperatures (250 °C) to form the sulfate mono-ester. This salt is then reacted with sodium hydroxide in the

neg: Sodium thiosulfate aquariums, swimming pools, and spas (e.g., following superchlorination) and within water treatment plants to treat settled backwash water prior to release into rivers. The reduction reaction is analogous to the iodine reduction reaction. In pH testing of bleach substances, sodium thiosulfate neutralizes the color-removing effects of bleach and allows one to test the pH of bleach solutions with liquid indicators. The relevant reaction is akin to the iodine reaction: thiosulfate reduces the hypochlorite (active ingredient in bleach) and in so doing becomes oxidized to sulfate. The complete reaction is: Similarly, sodium thiosulfate reacts with bromine, removing the free bromine from

neg: Sodium monothiophosphate Sodium monothiophosphate Sodium monothiophosphate, or sodium phosphorothioate, is a inorganic compound with the molecular formula NaPOS(HO). All are white solids. The anhydrous material (x = 0) decomposes without melting at 120-125 °C. More common is the dodecahydrate. A nonahydrate is also known. Related salts are the "di"thiophosphate NaPSO11HO, "tri"thiophosphate NaPSO11HO, and "tetra"thiophosphate NaPS8HO. Sodium monothiophosphate is prepared by the base hydrolysis of thiophosphoryl chloride using aqueous sodium hydroxide: This reaction affords the dodecahydrate, which is easily dehydrated. Partial dehydration over 6.5 M HSO gives the nonahydrate. Under flowing N2, the anhydrous salt is formed. Sodium phosphorothiolate decomposes at neutral pH.

neg: Neutralization (chemistry) strong acid. A strong base is one that is fully dissociated in aqueous solution. For example, sodium hydroxide, NaOH, is a strong base. Therefore, when a strong acid reacts with a strong base the neutralization reaction can be written as For example, in the reaction between hydrochloric acid and sodium hydroxide the sodium and chloride ions, Na and Cl take no part in the reaction. The reaction is consistent with the Brønsted–Lowry definition because in reality the hydrogen ion exists as the hydronium ion, so that the neutralization reaction may be written as When a strong acid is neutralized by

neg: Prévost reaction Prévost reaction The Prévost reaction is chemical reaction in which an alkene is converted by iodine and the silver salt of benzoic acid to a vicinal diol with anti stereochemistry. The reaction was discovered by the French chemist Charles Prévost (1899–1983). The reaction between silver benzoate (1) and iodine is very fast and produces a very reactive iodinium benzoate intermediate (2). The reaction of the iodinium salt (2) with an alkene gives another short-lived iodinium salt (3). Nucleophilic substitution (S2) by the benzoate salt gives the ester (4). Another silver ion causes the neighboring group substitution of the benzoate ester

neg: Sodium hydroxide water molecules. The hydrogen atoms of the hydroxyls form strong bonds with oxygen atoms within each O layer. Adjacent O layers are held together by hydrogen bonds between water molecules. Sodium hydroxide reacts with protic acids to produce water and the corresponding salts. For example, when sodium hydroxide reacts with hydrochloric acid, sodium chloride is formed: In general, such neutralization reactions are represented by one simple net ionic equation: This type of reaction with a strong acid releases heat, and hence is exothermic. Such acid-base reactions can also be used for titrations. However, sodium hydroxide is not used as a

neg: Aldol reaction the product. This reaction is an important approach to the formation of carbon-carbon bond in organic molecules containing ring systems. For example, under strong basic conditions (e.g. sodium hydroxide), hexane-2,5-dione (compound A in Figure 1) can cyclize via intramolecular aldol reaction to form the 3-methylcyclopent-2-en-1-one (compound B). Mechanism of the intramolecular aldol reaction involves formation of a key enolate intermediate and an intramolecular nucleophilic addition process. First, hydroxide abstracts the α-hydrogen on carbon 6 to form the enolate. Next, nucleophilic attack of the ketone carbon 2 by the enolate forms the carbon-carbon bond between carbons 2 and 6. At last,

neg: Peroxide value where 2 is valence). Note also that the unit of milliequivalent has been commonly abbreviated as mequiv or even as meq. The peroxide value is determined by measuring the amount of iodine which is formed by the reaction of peroxides (formed in fat or oil) with iodide ion. 2 I + HO + HOOH -> HOH + 2OH + I Note that the base produced in this reaction is taken up by the excess of acetic acid present. The iodine liberated is titrated with sodium thiosulphate. 2SO + I -> SO + 2 I The acidic conditions (excess acetic acid)

neg: Sodium bisulfite place in presence of a base such as sodium bicarbonate or sodium hydroxide and the bisulfite is liberated as sulfur dioxide. Examples of such procedures are described for benzaldehyde, 2-tetralone, citral, the ethyl ester of pyruvic acid and glyoxal. In the ring-expansion reaction of cyclohexanone with diazald, the bisulfite reaction is reported to be able to differentiate between the primary reaction product cycloheptanone and the main contaminant cyclooctanone. The other main use of sodium bisulfite is as a mild reducing agent in organic synthesis in particular in purification procedures. It can efficiently remove traces or excess amounts of chlorine, bromine,

neg: Sodium hydroxide hydroxide in a metathesis reaction. (Sodium hydroxide is soluble while calcium carbonate is not.) This process was called causticizing. This process was superseded by the Solvay process in the late 19th century, which was in turn supplanted by the chloralkali process which we use today. Sodium hydroxide is also produced by combining pure sodium metal with water. The byproducts are hydrogen gas and heat, often resulting in a flame, making this a common demonstration of the reactivity of alkali metals in academic environments; however, it is not commercially viable, as the isolation of sodium metal is typically performed by reduction

neg: Sodium oxide the reaction of sodium with sodium hydroxide, sodium peroxide, or sodium nitrite: Most of these reactions rely on the reduction of something by sodium, whether it is hydroxide, peroxide, or nitrite. Burning sodium in air will produce NaO and about 20% sodium peroxide NaO. Alternatively, sodium carbonate can be heated to 851 °C, producing carbon dioxide and sodium oxide. Sodium oxide is a significant component of glasses and windows although it is added in the form of "soda" (sodium carbonate). Sodium oxide does not explicitly exist in glasses, since glasses are complex cross-linked polymers. Typically, manufactured glass contains around 15%

neg: Solid state ionics situ" chemical reaction between the Li anode and iodine-poly(2-vinylpyridine) cathode, and therefore was self-healed from erosion and cracks during the operation. Sodium-sulfur cells, based on ceramic β-AlO electrolyte sandwiched between molten-sodium anode and molten-sulfur cathode showed high energy densities and were considered for car batteries in the 1990s, but disregarded due to the brittleness of alumina, which resulted in cracks and critical failure due to reaction between molten sodium and sulfur. Replacement of β-AlO with NASICON did not save this application because it did not solve the cracking problem, and because NASICON reacted with the molten sodium. Yttria-stabilized zirconia is

neg: Kraft process (lime). Calcium oxide (lime) is reacted with water to regenerate the calcium hydroxide used in Reaction 2: The combination of reactions 1 through 4 form a closed cycle with respect to sodium, sulfur and calcium and is the main concept of the so-called recausticizing process where sodium carbonate is reacted to regenerate sodium hydroxide. The recovery boiler also generates high pressure steam which is fed to turbogenerators, reducing the steam pressure for the mill use and generating electricity. A modern kraft pulp mill is more than self-sufficient in its electrical generation and normally will provide a net flow of energy

neg: 2-Undecanone that it may be useful as a mosquito repellent, as effective as, or even more effective than, DEET. 2-Undecanone is a ketone that is soluble in ethanol, benzene, chloroform, and acetone, but its large carbon chain renders it insoluble in water. Like most methyl ketones, 2-undecanone undergoes a haloform reaction when in the presence of a basic solution of hypochlorite. For example, the reaction between 2-undecanone and sodium hypochlorite yields sodium decanoate, chloroform, and sodium hydroxide. 2-Undecanone 2-Undecanone, also known as methyl nonyl ketone and IBI-246, is an oily organic liquid manufactured synthetically, but which can also be extracted from

neg: Raney nickel third metal is called a "promoter". The promoter changes the mixture from a binary alloy to a ternary alloy, which can lead to different quenching and leaching properties during activation. In the activation process, the alloy, usually as a fine powder, is treated with a concentrated solution of sodium hydroxide. The simplified leaching reaction is given by the following chemical equation: The formation of sodium aluminate (Na[Al(OH)]) requires that solutions of high concentration of sodium hydroxide be used to avoid the formation of aluminium hydroxide, which otherwise would precipitate as bayerite. Hence sodium hydroxide solutions with concentrations of up to

neg: Organochloride less expensive and more readily available. Alkyl chlorides readily undergo attack by nucleophiles. Heating alkyl halides with sodium hydroxide or water gives alcohols. Reaction with alkoxides or aroxides give ethers in the Williamson ether synthesis; reaction with thiols give thioethers. Alkyl chlorides readily react with amines to give substituted amines. Alkyl chlorides are substituted by softer halides such as the iodide in the Finkelstein reaction. Reaction with other pseudohalides such as azide, cyanide, and thiocyanate are possible as well. In the presence of a strong base, alkyl chlorides undergo dehydrohalogenation to give alkenes or alkynes. Alkyl chlorides react with magnesium

neg: Diazonium compound salts. For example, treatment of benzenediazonium chloride with benzene (an aromatic compound) in the presence of sodium hydroxide gives diphenyl: This reaction is known as the Gomberg–Bachmann reaction. A similar conversion is also achieved by treating benzenediazonium chloride with ethanol and copper powder. Diazonium fluoroborates react with an aliphatic carboxylic acid yield the corresponding benzoic acid. This reaction provides a method to prepare aromatic carboxylic acids from aliphatic carboxylic acids: Benzenediazonium chloride reacts with compounds containing activated double bonds to produces phenylated products. The reaction is called the Meerwein arylation: In their reactions with metal complexes, diazonium cations behave similarly

neg: Salt metathesis reaction forms when boiling a slurry of copper(I) thiocyanate and barium hydroxide in water: Metal complexes are alkylated via salt metathesis reactions. Illustrative is the methylation of titanocene dichloride to give the Petasis reagent: The salt product typically precipitates from the reaction solvent. A neutralization reaction is a type of double replacement reaction. A neutralization reaction occurs when an acid reacts with an equal amount of a base. This usually creates a solution of a salt and water. For example, hydrochloric acid reacts with sodium hydroxide to produce sodium chloride and water: Reaction between an acid and a carbonate or bicarbonate

neg: Copper and halides. Both cuprous and cupric oxides are known. Among the numerous copper sulfides, important examples include copper(I) sulfide and copper(II) sulfide. Cuprous halides (with chlorine, bromine, and iodine) are known, as are cupric halides with fluorine, chlorine, and bromine. Attempts to prepare copper(II) iodide yield only cuprous iodide and iodine. Copper forms coordination complexes with ligands. In aqueous solution, copper(II) exists as [Cu(HO)]. This complex exhibits the fastest water exchange rate (speed of water ligands attaching and detaching) for any transition metal aquo complex. Adding aqueous sodium hydroxide causes the precipitation of light blue solid copper(II) hydroxide. A simplified

neg: Functional group to label isomers, for example, isopropanol (IUPAC name: propan-2-ol) is an isomer of n-propanol (propan-1-ol). The following is a list of common functional groups. In the formulas, the symbols R and R' usually denote an attached hydrogen, or a hydrocarbon side chain of any length, but may sometimes refer to any group of atoms. Functional groups, called hydrocarbyl, that contain only carbon and hydrogen, but vary in the number and order of double bonds. Each one differs in type (and scope) of reactivity. There are also a large number of branched or ring alkanes that have specific names, e.g., tert-butyl,

neg: Cicutoxin of acetylene accompanied by addition of iodine in the presence of platinum (IV) catalyst and sodium iodide. The last keyfragment, THP-protected 4,6-heptadiyn-1-ol (6) is a known compound. The first step is the Sonogashira coupling of compound 8 and 9. This step gave dienynol (10) with 63 percent yield. The second step is a palladium -catalyzed coupling reaction. The coupling of compound 6 and 10 leads to the 17-carbon frame (11) with 74 percent yield. Compound 11 already has the stereo center in place and only needs a few structural changes: the third and fourth step. The third step is the

neg: Alkynylation an alternative set of reaction conditions, which involves prereaction of the acetylene with an alkali metal hydroxide such as KOH. The reaction proceeds through equilibria, making the reaction reversible: To overcome this reversibility, the reaction often uses an excess of base to trap the water as hydrates. Chemist Walter Reppe pioneered catalytic, industrial-scale ethynylations using acetylene with alkali metal and copper(I) acetylides: These reactions are used to manufacture propargyl alcohol and butynediol. Alkali metal acetylides, which are often more effective for ketone additions, are used to produce 2-methyl-3-butyn-2-ol from acetylene and acetone. Alkynylation Alkynylation is an addition reaction in organic

neg: Mercury battery a salt bridge. Two half-reactions occur at the anode. The first consists of an electrochemical reaction step: followed by the chemical reaction step: yielding an overall anode half-reaction of: The overall reaction for the battery is: In other words, during discharge, zinc is oxidized (loses electrons) to become zinc oxide (ZnO) while the mercuric oxide gets reduced (gains electrons) to form elemental mercury. A little extra mercuric oxide is put into the cell to prevent evolution of hydrogen gas at the end of life. Sodium hydroxide or potassium hydroxide are used as an electrolyte. Sodium hydroxide cells have nearly constant

neg: Azanide Azanide Azanide is the negatively-charged compound NH. It is isoelectric with water and fluoronium. Because it is the conjugate base of ammonia, it is formed by the self-ionization of ammonia. The amide anion can form salts like lithium amide, sodium amide, and potassium amide. These salts are difficult to create using neutralization reactions (Instead of ammonia serving as a base to neutralize sodium hydroxide and yield water and sodium amide, the reverse reaction actually takes place.) and are therefore typically created by reacting ammonia with the metal that is to be the cation, resulting in a redox reaction like 2

neg: Desomorphine to the skin, blood vessels, bone and muscles, sometimes requiring limb amputation in long-term users. Causes of this damage are from iodine and phosphorus (and other toxic substances) that are present after synthesis. Addicts often use readily available but relatively toxic and impure solvents such as battery acid, gasoline or paint thinner during the reaction scheme, without adequately removing them afterwards before injection. Strong acids and bases such as hydrochloric acid and sodium hydroxide are also employed without measuring pH of the final solution and analysis of leftover solutions of "krokodil" in used syringes showed the pH was typically less

neg: Sodium nitrate mixing stoichiometric amounts of ammonium nitrate and sodium hydroxide, sodium bicarbonate or sodium carbonate: Sodium nitrate can be combined with sulfuric acid and nitric acid distilled off. At lower pressure the lower temperature needed results in less decomposition. The theoretical 2 moles of nitric acid per 1 mole of sulfuric acid results in a very high end temperature, much decomposition and a solid neutral sulfate that is difficult to remove. When this reaction was important industrially, it was common practice to operate with sulfuric acid in excess to end on a mostly bisulfate product poured molten out of the retort.

neg: Potassium nitrate after being cut off from its supplies of mineral sodium nitrates from Chile (see nitratite). Potassium nitrate can be made by combining ammonium nitrate and potassium hydroxide. An alternative way of producing potassium nitrate without a by-product of ammonia is to combine ammonium nitrate, found in instant ice packs, and potassium chloride, easily obtained as a sodium-free salt substitute. Potassium nitrate can also be produced by neutralizing nitric acid with potassium hydroxide. This reaction is highly exothermic. On industrial scale it is prepared by the double displacement reaction between sodium nitrate and potassium chloride. Potassium nitrate has a wide variety

neg: Sodium polysulfide a photochemical solution, and in the tanning industry to remove hair from hides. As exploited in the sodium-sulfur battery, the polysulfides absorb and release reducing equivalents by breaking and making S-S bonds, respectively. An idealized reaction for sodium tetrasulfide is shown: Alkylation gives organic polysulfides according to the following idealized equation: Alkylation with an organic dihalide gives polymers called thiokols. Protonation of these salts gives hydrogen sulfide and elemental sulfur, as illustrated by the reaction of sodium pentasulfide: Sodium polysulfide Sodium polysulfide is a general term for salts with the formula NaS, where "x" = 2 to 5. The species

neg: Iodine value with sodium thiosulfate. Introduced the iodine value was Hübl which titrated fats in the presence of mercuric chloride with iodine, but with the actual reagent (probably iodine chloride) is formed in situ from mercuric chloride and iodine. Addition of iodine chloride and back-titration with sodium thiosulphate by DIN 53241-1:1995-05. The fat is mixed with an excess of bromine. This bromine is added to the double bonds in the unsaturated fats. This reaction must be carried out in the dark, since the formation of bromine radicals is suppressed by light. This would lead to undesirable side reactions, and thus falsifying a

neg: Sodium acetate reacting acetic acid with sodium hydroxide using water as the solvent. Sodium acetate can be used to form an ester with an alkyl halide such as bromoethane: Sodium acetate undergoes decarboxylation to form methane (CH) under forcing conditions (pyrolysis in the presence of sodium hydroxide): Caesium salts catalyze this reaction. Sodium acetate Sodium acetate, CHCOONa, also abbreviated NaOAc, is the sodium salt of acetic acid. This colorless deliquescent salt has a wide range of uses. Sodium acetate is used in the textile industry to neutralize sulfuric acid waste streams and also as a photoresist while using aniline dyes. It is

neg: Chloramine-T electrophilic chlorine in organic synthesis. The anionic sulfonamide is stabilized by delocalization of the nitrogen lone pair across the SO group, facilitating deprotonation of the parent amine by bases such as hydroxide. It is readily biodegradable by use of ultraviolet (UV) light. Chloramine-T is prepared from "p"-toluenesulfonamide and sodium hypochlorite, with the latter being produced "in situ" from sodium hydroxide and chlorine (Cl). Hypochlorite released from chloramine-T acts as an effective oxidizing agent for iodide to form iodine monochloride (ICl). ICl rapidly undergoes electrophilic substitution predominantly with activated aromatic rings, such as those of the amino acid tyrosine. Thus, chloramine-T

neg: Alkaline hydrolysis Alkaline hydrolysis Alkaline hydrolysis, in organic chemistry, usually refers to types of nucleophilic substitution reactions in which the attacking nucleophile is a hydroxide ion. In the alkaline hydrolysis of esters and amides the hydroxide ion nucleophile attacks the carbonyl carbon in a nucleophilic acyl substitution reaction. This mechanism is supported by isotope labeling experiments. For example, when ethyl propionate with an oxygen-18 labeled ethoxy group is treated with sodium hydroxide (NaOH), the oxygen-18 is completely absent from the sodium propionate product and is found exclusively in the ethanol formed. The reaction is often used to turn solid organic matter into

neg: Sodium bicarbonate washing with about 6 ounces (170 g) of baking soda in 2 gallons (7.5 l) of water will help to wash it out. Sodium bicarbonate is an amphoteric compound. Aqueous solutions are very mildly alkaline due to the formation of carbonic acid and hydroxide ion: Sodium bicarbonate can be used as a wash to remove any acidic impurities from a "crude" liquid, producing a purer sample. Reaction of sodium bicarbonate and an acid produces a salt and carbonic acid, which readily decomposes to carbon dioxide and water: Sodium bicarbonate reacts with acetic acid (found in vinegar), producing sodium acetate, water,

neg: Barium chloride Ba is 8 in the fluorite structure and 9 in the cotunnite structure. When cotunnite-structure BaCl is subjected to pressures of 7–10 GPa, it transforms to a third structure, a monoclinic post-cotunnite phase. The coordination number of Ba increases from 9 to 10. In aqueous solution BaCl behaves as a simple salt; in water it is a 1:2 electrolyte and the solution exhibits a neutral pH. Its solutions react with sulfate ion to produce a thick white precipitate of barium sulfate. Oxalate effects a similar reaction: When it is mixed with sodium hydroxide, it gives the dihydroxide, which is moderately

neg: Nonafluoro-tert-butyl alcohol Nonafluoro-tert-butyl alcohol Nonafluoro-"tert"-butyl alcohol ("IUPAC name": 1,1,1,3,3,3-hexafluoro-2-(trifluoromethyl)propan-2-ol) is a fluorinated alcohol. It is the perfluorinated analog of "tert"-butyl alcohol. Notably, as a consequence of its electron withdrawing fluorine substituents, it is very acidic for an alcohol, with a p"K" value of 5.4, similar to that of a carboxylic acid. As another consequence of being a perfluorinated compound, it is also one of the lowest boiling alcohols, with a boiling point lower than that of methanol. It is prepared by addition of trichloromethyllithium to hexafluoroacetone, followed by halogen exchange with antimony pentafluoride. The aluminate derived from its alkoxide anion, tetrakis[1,1,1,3,3,3-hexafluoro-2-(trifluoromethyl)propan-2-oxy]aluminate(1–), {Al[(CF)CO]}

neg: Permethrin m-phenoxybenzyl alcohol, through a transesterification reaction with base. Tetraisopropyl titanate or sodium ethylate may be used as the base. The alcohol precursor may be prepared in three steps. First, m-cresol, chlorobenzene, sodium hydroxide, potassium hydroxide, and copper chloride react to yield m-phenoxytoluene. Second, oxidation of m-phenoxytoluene over selenium dioxide provides m-phenoxybenzaldehyde. Third, a Cannizzaro reaction of the benzaldehyde in formaldehyde and potassium hydroxide affords the m-phenoxybenzyl alcohol. In Nordic countries and North America, a permethrin formulation for lice treatment is marketed under trade name Nix, available over the counter. Johnson & Johnson's UK brand Lyclear covers an assortment of different

neg: Sodium hydroxide soluble in water, with a lower solubility in polar solvents such as ethanol and methanol. NaOH is insoluble in ether and other non-polar solvents. Similar to the hydration of sulfuric acid, dissolution of solid sodium hydroxide in water is a highly exothermic reaction where a large amount of heat is liberated, posing a threat to safety through the possibility of splashing. The resulting solution is usually colorless and odorless. As with other alkaline solutions, it feels slippery with skin contact due to the process of saponification that occurs between NaOH and natural skin oils. Sodium hydroxide, NaOH, as a fluid

neg: Khristo Ivanov reaction of 2-benzylbenzazoles with aromatic aldehydes in detail under phase-transfer catalysis or in aprotic solvents in the presence of a water solution of sodium hydroxide leading to 2-styrylbenzazols or alcohols having a benzazole ring. Detailed studies have been done under the conditions of the Michael reaction on the addition of metallic derivatives of CH-acidic compounds to substrates containing carbonyl or azomethine group or to substrates with an activated double bond. Ivanov was the initiator of studies on the reaction of nucleophilic reagents with coumarins. A new interesting rearrangement of 3-substituted coumarins to 2-oxochromans-4-acetic acid derivatives was found for the first

neg: Ethanethiol underground mine shall, consist of the introduction into all workplaces of sufficient quantities of ethyl mercaptan gas or similar gas to be readily detectable by all workers". Ethanethiol is a reagent in organic synthesis. In the presence of sodium hydroxide, it gives the powerful nucleophile SEt. The salt can be generated quantitatively by reaction with sodium hydride. Ethanethiol can be oxidized to ethyl sulfonic acid, using strong oxidizing agents. Weaker oxidants, such as ferric oxide or hydrogen peroxide give the disulfide, diethyl disulfide: Like other thiols, it behaves comparably to hydrogen sulfide. For example, it binds, concomitant with deprotonation to

neg: Pyrithione "N"-oxide. A substitution reaction using either sodium dithionite () or sodium sulfide with sodium hydroxide will allow the replacement of the bromo substituent with a thiol functional group. The alternative strategy is to form the mercaptan before introducing the "N"-oxide moiety. 2-Mercaptopyridine was originally synthesized in 1931 by heating 2-chloropyridine with calcium bisulfide, an approach similar that first used to prepare pyrithione. The analogous thiourea approach via a uronium salt was reported in 1958 and provides a more convenient route to 2-mercaptopyridine. Oxidation to the "N"-oxide can then be undertaken. Pyrithione is found as a natural product in the "Allium

neg: Tetrazole Tetrazole Tetrazoles are a class of synthetic organic heterocyclic compound, consisting of a 5-member ring of four nitrogen atoms and one carbon atom. The simplest is tetrazole itself, CHN. They are unknown in nature. Tetrazole was first prepared by the reaction of anhydrous hydrazoic acid and hydrogen cyanide under pressure. Treatment of organic nitriles with sodium azide in the presence of iodine or silica-supported sodium bisulfate as a heterogeneous catalyst enables an advantageous synthesis of 5-substituted 1"H"-tetrazoles. 2-Aryl-"2H"-tetrazoles are synthesized by a [3+2] cycloaddition reaction between an aryl diazonium and trimethylsilyldiazomethane. There are several pharmaceutical agents which are tetrazoles. Tetrazoles

neg: Sodium 2-hydroxyethyl sulfonate the reaction must be performed under careful control of mass ratios and process conditions. Excess sulfite (SO) or bisulfite (HSO) lead to an unpleasant odor of the downstream product, higher levels of ethylene glycol or glycol ethers (formed by the hydrolysis and ethoxylation of ethylene oxide) give hygroscopic and greasy surfactants. Concentrated ethylene glycol-containing sodium 2-hydroxyethyl sulfonate solutions can subsequently mostly be freed from ethylene glycol by continuous extraction with e.g. isopropanol (<0.5%). Therefore, in the continuous industrial process an aqueous sodium hydrogen sulfite solution is prepared in a first reactor by mixing a sodium hydroxide solution and sulfur dioxide.

neg: Sodium polysulfide these salts are dense solids with strong association of the sodium cations with the anionic termini of the chains. Sodium polysulfide can produced by dissolving sulfur in a solution of sodium sulfide. Alternatively they are produced by the redox reaction of aqueous sodium hydroxide with sulfur at elevated temperatures. Finally they arise by the reduction of elemental sulfur with sodium, a reaction often conducted in anhydrous ammonia. These salts are used in the production of polysulfide polymers, as a chemical fungicide, as a blackening agent on copper jewellery, as a component in a polysulfide bromide battery, as a toner in

neg: Sodium tellurite a weak reducing agent. Telluric acid loses a proton at this pKa. Hydrogen tellurite loses a proton at this pKa to become the tellurite ion. This would happen in the reaction of tellurous acid with sodium hydroxide to make sodium tellurite. This is the reaction of tellurium dioxide with a base to make a tellurite salt. Sodium tellurite improves the corrosion resistance of electroplated nickel layers. Solutions of sodium tellurite are used for black or blue-black coatings on iron, steel, aluminum, and copper. In microbiology, sodium tellurite can be added to the growth medium to isolate bacteria with an inherent

neg: Stearin from the liquid, which is typically enriched in fats derived from oleic acid. It can be obtained by interesterification, again exploiting its higher melting point which allows the higher melting tristearin to be removed from the equilibrated mixture. Stearin is a side product obtained during the extraction of cod liver oil removed during the chilling process at temperatures below . It is used as a hardening agent in the manufacture of candles and soap. In the manufacture of soap, stearin is mixed with a sodium hydroxide solution in water. The following reaction gives glycerin and sodium stearate, the main ingredient

neg: Quinine total synthesis is hydrogenated to the amine 11 with platinum in acetic acid and alkylation with iodomethane gives the quaternary ammonium salt 12 and subsequently the betaine 13 after reaction with silver oxide. Quinine's vinyl group is then constructed by Hofmann elimination with sodium hydroxide in water at 140 °C. This process is accompanied by hydrolysis of both the ester and the amide group but it is not the free amine that is isolated but the urea 14 by reaction with potassium cyanate. In the next step the carboxylic acid group is esterified with ethanol and the urea group replaced with a

neg: Drain cleaner Oxide: AlO + 2NaOH + 3HO → 2Na [Al(OH)] 2. Oxidation of Aluminum metal: 2Al + 2NaOH + 6HO → 2Na[Al(OH)] + 3H The actual breakdown of a clog occurs by reaction with the basic sodium hydroxide (lye). Clogs are often composed of natural substances such as hair, fats, oils, etc. and breakdown occurs via a saponification reaction of a base and triglycerol. Essentially, the hydroxide ions from the basic lye attack the carbonyl carbons of the fat, which eventually kicks off the hydrophobic tails of the triglyceride (tristearin/fat) to isolate glycerol. Alkaline drain openers can dissolve hair (containing proteins)

neg: Calcium hydroxide where it is an intermediate in the reaction in the production of sodium hydroxide. This conversion is part of the "causticizing" step in the Kraft process for making pulp. In the causticizing operation burned lime is added to "green liquor" which is a solution primarily of sodium carbonate and sodium sulfate produced by dissolving "smelt", which is the molten form of these chemicals from the recovery furnace. Because of its low toxicity and the mildness of its basic properties, slaked lime is widely used in the food industry to: In Spanish, calcium hydroxide is called "cal". Maize cooked with "cal"

neg: Sodium selenide Sodium selenide Sodium selenide is an inorganic compound of sodium and selenium with the chemical formula NaSe. This colourless solid is prepared by the reaction of selenium with a solution of sodium in liquid ammonia at -40 °C. Alternatively, sodium selenide can be prepared by the reaction of gaseous hydrogen selenide with metallic sodium at 100 °C. Like other alkali metal chalcogenides, this material is highly sensitive to water, easily undergoing hydrolysis to give mixtures of sodium biselenide (NaSeH) and hydroxide. This hydrolysis occurs because of the extreme basicity of the Se ion. Similarly, sodium selenide is readily oxidized to

neg: Soda lime why soda lime is faster in chemical reactivity than calcium hydroxide alone. It reacts much more quickly and so contributes to a faster elimination of the CO from the rebreathing circuit. The formation of water and the moisture from the respiration also act as a solvent for the reaction. Reactions in aqueous phase are generally faster than between a dry gas and a dry solid. A quite didactic parallelism can be drawn between the catalytic role of sodium hydroxide in the process of carbonation of soda lime and the role of sodium hydroxide played in the alkali-silica reaction, a slow

neg: Castner process neck (B) and liquid in the body of the vessel. Sodium metal forms at the cathode but is less dense than the fused sodium hydroxide electrolyte. Wire gauze (G) confines the sodium metal to accumulating at the top of the collection device (P). The cathode reaction is The anode reaction is Despite the elevated temperature, some of the water produced remains dissolved in the electrolyte. This water diffuses throughout the electrolyte and results in the reverse reaction taking place on the electrolized sodium metal: with the hydrogen gas also accumulating at (P). This, of course, reduces the efficiency of the

neg: Iodine clock reaction An experimental iodine clock sequence has also been established for a system consisting of iodine potassium-iodide, sodium chlorate and perchloric acid that takes place through the following reactions. Triiodide is present in equilibrium with iodide anion and molecular iodine: Chlorate ion oxidizes iodide ion to hypoiodous acid and chlorous acid in the slow and rate-determining step: Chlorate consumption is accelerated by reaction of hypoiodous acid to iodous acid and more chlorous acid: More autocatalysis when newly generated iodous acid also converts chlorate in the fastest reaction step: In this clock the induction period is the time it takes for autocatalytic

neg: Zinc hydroxide Zn is known to form hexa-aqua ions at high water concentrations and tetra-aqua ions at low concentrations of water and, thus, this reaction may be better written as the reaction of the aquated ion with hydroxide through donation of a proton, as follows. Subsequent reactions discussed below can also, therefore, be considered as reactions with the aquated zinc ion and one can adjust them accordingly. However, for simplicity, the water molecules are omitted from here-on. If excess sodium hydroxide is added, the precipitate of zinc hydroxide will dissolve, forming a colorless solution of zincate ion: This property can be used

neg: Iodine the Finkelstein reaction is slightly complicated by the fact that iodide is a better leaving group than chloride or bromide. The difference is nevertheless small enough that the reaction can be driven to completion by exploiting the differential solubility of halide salts, or by using a large excess of the halide salt. In the classic Finkelstein reaction, an alkyl chloride or an alkyl bromide is converted to an alkyl iodide by treatment with a solution of sodium iodide in acetone. Sodium iodide is soluble in acetone and sodium chloride and sodium bromide are not. The reaction is driven toward products

neg: Cannizzaro reaction Cannizzaro reaction The Cannizzaro reaction, named after its discoverer Stanislao Cannizzaro, is a chemical reaction that involves the base-induced disproportionation of a non-enolizable aldehyde. Cannizzaro first accomplished this transformation in 1853, when he obtained benzyl alcohol and potassium benzoate from the treatment of benzaldehyde with potash (potassium hydroxide). More typically, the reaction would be conducted with sodium or potassium hydroxide: The oxidation product is a salt of a carboxylic acid and the reduction product is an alcohol. The reaction involves a nucleophilic acyl substitution on an aldehyde, with the leaving group concurrently attacking another aldehyde in the second step. First,

neg: Trinitroanisole Trinitroanisole Trinitroanisole is a chemical compound that exists as pale yellow crystals with a melting point of 68 °C. It is an explosive with a detonation velocity of 7200 meters per second. Trinitroanisole can be prepared by the reaction of 2,4-dinitrochlorobenzene with methanol in the presence of sodium hydroxide followed by the nitration of the resulting product. Alternatively, it can be prepared directly by the reaction of picryl chloride with methanol in the presence of sodium hydroxide. Historically, trinitroanisole was used as a military explosive (e.g., Japanese ""), however, due to its tendency to form picric acid and dangerous picrate

neg: Trinitroanisole salts, its use has largely been abandoned. Trinitroanisole Trinitroanisole is a chemical compound that exists as pale yellow crystals with a melting point of 68 °C. It is an explosive with a detonation velocity of 7200 meters per second. Trinitroanisole can be prepared by the reaction of 2,4-dinitrochlorobenzene with methanol in the presence of sodium hydroxide followed by the nitration of the resulting product. Alternatively, it can be prepared directly by the reaction of picryl chloride with methanol in the presence of sodium hydroxide. Historically, trinitroanisole was used as a military explosive (e.g., Japanese ""), however, due to its tendency

neg: Ethyl acetate Fischer equilibrium mentioned above. In the laboratory, and usually for illustrative purposes only, ethyl esters are typically hydrolyzed in a two-step process starting with a stoichiometric amount of a strong base, such as sodium hydroxide. This reaction gives ethanol and sodium acetate, which is unreactive toward ethanol: The rate constant is 0.111 L/mol·s at 25 °C. The for rats is 5620 mg/kg, indicating low toxicity. Given that the chemical is naturally present in many organisms, there is little risk of toxicity. Overexposure to ethyl acetate may cause irritation of the eyes, nose, and throat. Severe overexposure may cause weakness, drowsiness,

neg: Cannizzaro reaction product. Certain ketones can undergo a Cannizzaro-type reaction, transferring one of their two carbon groups rather than the hydride that would be present on an aldehyde. Cannizzaro reaction The Cannizzaro reaction, named after its discoverer Stanislao Cannizzaro, is a chemical reaction that involves the base-induced disproportionation of a non-enolizable aldehyde. Cannizzaro first accomplished this transformation in 1853, when he obtained benzyl alcohol and potassium benzoate from the treatment of benzaldehyde with potash (potassium hydroxide). More typically, the reaction would be conducted with sodium or potassium hydroxide: The oxidation product is a salt of a carboxylic acid and the reduction product