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| − | [[File:Smw1.png|thumb]] | + | #REDIRECT[[Sulfuric acid]] |
| − | '''Sulfuric acid''' (alternative spelling '''sulphuric acid'''), represented by the molecular formula H<sub>2</sub>SO<sub>4</sub>, is one of the most important [[acid]]s in chemistry and the most important chemical to industries in the world. It is the strongest easily available acid, with a [[Measures of acidity|pK<sub>a</sub>]] of -3.
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| − | ==Properties==
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| − | ===Chemical properties===
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| − | Sulfuric acid is a diprotic acid, it is able to give away two protons (H<sup>+</sup>). It first dissociates to form [[hydronium]] and [[hydrogen sulfate]], with a pKa of -3, indicative of a strong acid:
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| − | :H<sub>2</sub>SO<sub>4</sub> + H<sub>2</sub>O → H<sub>3</sub>O + HSO<sub>4</sub><sup>−</sup>
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| − | The second dissociation forms sulfate and another hydronium ion from a hydrogen sulfate ion. It has a pKa of 1.99, indicative of a weak acid, and occurs like this:
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| − | :HSO<sub>4</sub><sup>−</sup> + H<sub>2</sub>O ⇌ H<sub>3</sub>O<sup>+</sup> + SO<sub>4</sub><sup>2-</sup>
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| − | Concentrated sulfuric acid also has a strong oxidizing effect, converting nonmetals such as [[carbon]] and [[sulfur]] to [[carbon dioxide]] and [[sulfur dioxide]], respectively, reducing sulfuric acid into sulfur dioxide and water in the process. This property is useful for producing large amounts of sulfur dioxide for use as a reducing agent if water is continually removed.
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| − | Sulfuric acid is sufficiently strong enough to protonate [[nitric acid]], forming the nitronium ion, which can be used in a nitration mixture to make [[Alkyl nitrates|alkyl nitrates]].
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| − | In organic chemistry, sulfuric acid is the most practical acid in most cases where a source of H<sub>3</sub>O<sup>+</sup> ions are needed as it introduces the least amount of water. Organic compounds are often easily attacked by the nucleophiles left behind by the dissociation of acids such as HCl which leaves Cl<sup>-</sup> ions behind which can easily attack many organic compounds. However, the [[sulfate]] ions left behind by the dissociation of sulfuric acid are far less reactive than the ions left behind by most acids, it allows to protonate the reaction mixture without causing undesired side reactions in most cases.
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| − | When concentrated, it is strongly [[hygroscopy|hygroscopic]] and has strong dehydrating properties. It can break down most organic molecules containing OH<sup>-</sup> groups to use them to form water, leaving only the carbon behind. This property is exploited in the famous [http://youtu.be/w6lfq7BOCik "black snake" demonstration], where sulfuric acid dehydrates [[sucrose]] (table sugar), forming water with the hydrogen and oxygen atoms and leaving amorphous carbon behind.
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| − | ===Physical properties===
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| − | [[File:H2so4boil.jpg|thumb|342px|Boiling point of H2SO4 VS concentration]]
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| − | Sulfuric acid is a oily liquid at room temperature. It is colorless, but often has a very light yellow color when slightly contaminated with iron ions. Even very small amounts of dissolved organic matter can change the color of concentrated sulfuric acid to pale yellow or pink, red, brown, and even black. It is commonly sold diluted at around 35% w/w with water as car battery acid and concentrated between 95% and 98% w/w as drain cleaner.
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| − | Sulfuric acid's boiling point raises with the concentration as described in this figure to the right. An [[azeotrope]] forms at 98% w/w.
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| − | ==Sources, production, and concentration==
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| − | Sulfuric acid is a commonly used chemical for lead-acid batteries and drain cleaning. Battery acid can often be found at an auto store or a department store, and is approximately 35% sulfuric acid by weight. This is sufficient for most amateur chemists. If more concentrated sulfuric acid is desired, one can look in hardware stores for drain cleaner, which can be over 90% sulfuric acid by weight. For safety purposes, this concentration of sulfuric acid may have a dye in it. Other forms of sulfuric acid may be contaminated and will appear ye
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| − | For some amateurs, it can be hard to find concentrated sulfuric acid, with acid drain cleaners being banned(as a result of [[wikipedia:Acid_throwing|acid throwing]] or illicit drug manufacture) or very contaminated in some countries. Some brand of battery acids however are quite pure and easy to find almost anywhere. To concentrate it from 35 to 98%, one can boil it down to evaporate the water. It is advised to use glassware with anti-splash adapters, as sulfuric acid tends to bump a lot while it boils. The sulfuric acid will be quite concentrated when the temperature reaches around 300°C. The maximum reachable is 98.3% w/w, a point at which the boiling point will be 327°C. Extreme care must be taken when boiling sulfuric acid. The hazards and safety tips section must be read. Near the end, the acid will decompose into various [[sulfur oxides]].
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| − | It is possible to further concentrate sulfuric acid by adding [[sulfur trioxide]], which reacts with the remaining water to form pure sulfuric acid. Sulfur trioxide can continue to be added to the solution to form [[oleum]], which fumes in air to form sulfuric acid droplets. When an equimolar concentration of sulfuric acid and sulfur trioxide are added, it forms [[pyrosulfuric acid]], which is a solid at room temperature.
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| − | ==Projects==
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| − | * Producing metal sulfates
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| − | * Producing nitro compounds through [[nitration]]
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| − | * The dehydration of [[sucrose]] to produce elemental [[carbon]]
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| − | * E[[Esterification|sterifications]] that require a dehydrating agent, such as that of [[methyl salicylate]]
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| − | * Making simple [[rayon]] fibers with [[schweizer's reagent|Schweizer's reagent]] and [[cellulose]]
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| − | * Producing other concentrated acids by reaction of sulfuric acid with an anhydrous salt, such as in the production of fuming [[nitric acid]] and glacial [[acetic acid]]
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| − | ==Handling==
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| − | ===Safety===
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| − | [[File:Corrosive.png|thumb|left|Corrosive]] While low concentration sulfuric acid is relatively safe to work with (under 40% w/w)), concentrated sulfuric acid (over 90% w/w) is extremely corrosive and dangerous. It does not only causes chemical burns, it also causes burns by dehydration of organic materials (like skin), destroying the molecules to form water with the -OH groups in them. Safety measures should be taken and all skin should be covered when working with concentrated sulfuric acid.
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| − | When heating sulfuric acid, it is important to DO NOT OVERFILL THE FLASK. Concentrated sulfuric acid's volume increases by nearly 16% between 0 and 330°C, an overfilled flask will spill its content. Also, sulfuric acid, even diluted, tends to bump when it boils, accumulating heat to release a violent burst of steam from time to time. The use of boiling chips reduces this phenomena, but there is no way to stop it completely. It is advised to take measures to prevent spills, an anti-splash adapter with ground glass joint being a very convenient option.
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| − | Hot concentrated sulfuric acid may decompose to form sulfur dioxide and sulfur trioxide, which are toxic and corrosive, respectively.
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| − | ===Storage===
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| − | Sulfuric acid should be stored in closed bottles.
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| − | ==References==
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| − | ===Relevant Sciencemadness threads===
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| − | [[Category:Chemical compounds]]
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| − | [[Category:Inorganic compounds]]
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| − | [[Category:Acids]]
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| − | [[Category:Strong acids]]
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| − | [[Category:Mineral acids]]
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| − | [[Category:Oxoacids]]
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| − | [[Category:Oxidizing agents]]
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| − | [[Category:Desiccants]]
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| − | [[Category:Corrosive chemicals]]
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| − | [[Category:Materials unstable in basic solution]]
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| − | [[Category:Readily available chemicals]]
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| − | [[Category:DEA List II chemicals]]
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