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{{Distinguish|Sodium bisulfite}} |
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{{chembox |
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| Watchedfields = changed |
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| verifiedrevid = 432969756 |
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| verifiedrevid = 472263265 |
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| Name = Sodium bisulfate |
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| ImageFileL1 = Sodium bisulfate.svg |
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| Name = Sodium bisulfate |
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| ImageFileL1 = Sodium bisulfate.svg |
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| ImageNameL1 = One sodium cation and one hydrogensulfate anion |
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| ImageSizeL1 = 120px |
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| ImageFileR1 = Sodium-bisulfate-3D-balls-ionic.png |
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| ImageNameL1 = One sodium cation and one hydrogensulfate anion |
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| ImageNameR1 = Ball-and-stick model of the component ions |
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| ImageFileR1 = Sodium-bisulfate-3D-balls-ionic.png |
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| ImageFile2 = Sodium_Bisulfate.jpg |
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| ImageSizeR1 = 120px |
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| ImageSize2 = 150px |
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| ImageNameR1 = Ball-and-stick model of the component ions |
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| ImageName2 = Sodium bisulfate, as a white powder, turns indicator paper red. |
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| ImageFile2 = Sodium_Bisulfate.jpg |
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| IUPACName = Sodium hydrogen sulfate |
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| ImageSize2 = 150px |
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| OtherNames = Sodium acid sulfate<br/>Bisulfate of soda<br/>(sodiooxy)sulfonic acid |
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| ImageName2 = Sodium bisulfate, as a white powder, turns indicator paper red. |
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|Section1={{Chembox Identifiers |
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| IUPACName = Sodium hydrogen sulfate |
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| CASNo = 7681-38-1 |
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| OtherNames = Sodium acid sulfate<br/>Bisulfate of soda |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| Section1 = {{Chembox Identifiers |
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| CASNo1_Ref = {{cascite|correct|??}} |
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| CASNo = 7681-38-1 |
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| CASNo1 = 10034-88-5 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| CASNo1_Comment = (monohydrate) |
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| CASNo1 = 10034-88-5 |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| CASNo1_Comment = (monohydrate) |
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| ChemSpiderID = 56397 |
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| RTECS = VZ1860000 |
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| EINECS = 231-665-7 |
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| RTECS = VZ1860000 |
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| PubChem = 516919 |
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| ChEMBL = 1200488 |
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| EINECS = 231-665-7 |
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| ChemSpiderID = 56397 |
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| PubChem = 516919 |
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| SMILES = .S(=O)(=O)O |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| InChI = 1/Na.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+1;/p-1 |
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| UNII = BU8V88OWIQ |
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| InChIKey = WBHQBSYUUJJSRZ-REWHXWOFAO |
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| UNII1_Ref = {{fdacite|correct|FDA}} |
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| StdInChI = 1S/Na.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+1;/p-1 |
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| UNII1 = 3KLS9Y77YJ |
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| StdInChIKey = WBHQBSYUUJJSRZ-UHFFFAOYSA-M |
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| UNII1_Comment = (monohydrate) |
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| UNNumber = 2837 |
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| SMILES = .S(=O)(=O)O |
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| InChI = 1/Na.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+1;/p-1 |
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| InChIKey = WBHQBSYUUJJSRZ-REWHXWOFAO |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChI = 1S/Na.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+1;/p-1 |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey = WBHQBSYUUJJSRZ-UHFFFAOYSA-M |
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}} |
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}} |
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| Section2 = {{Chembox Properties |
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|Section2={{Chembox Properties |
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| Formula = NaHSO<sub>4</sub> |
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| Formula = NaHSO<sub>4</sub> |
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| MolarMass = 120.06 g/mol (anhydrous)<br/>138.07 g/mol (monohydrate) |
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| MolarMass = 120.06 g/mol (anhydrous)<br/>138.07 g/mol (monohydrate) |
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| Appearance = white solid |
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| Appearance = white solid |
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| Density = 2.742 g/cm<sup>3</sup> (anhydrous) <br> 1.8 g/cm<sup>3</sup> (monohydrate) |
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| Density = 2.742 g/cm<sup>3</sup> (anhydrous) <br> 1.8 g/cm<sup>3</sup> (monohydrate) |
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| Solubility = 50 g/100 mL (0°C) <br> 100 g/100 mL (100°C) |
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| Solubility = 28.5 g/100 mL (25 °C) <br> 100 g/100 mL (100 °C) |
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| SolubleOther = insoluble in ]; decomposed by ] |
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| SolubleOther = Insoluble in ] |
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| pKa = 1.99 |
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| pKa = 1.99 |
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| MeltingPtC = 58.5 |
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| MeltingPt = 58.5°C (monohydrate) <br> 315°C (anhydrous) |
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| MeltingPt_notes = (monohydrate) <br> 315 °C (anhydrous) |
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| BoilingPt = decomposes to ] (+ H<sub>2</sub>O) at 315°C |
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| BoilingPtC = 315 |
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| BoilingPt= decomposes to ] (+ H<sub>2</sub>O) at |
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}} |
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}} |
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| Section3 = {{Chembox Structure |
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|Section3={{Chembox Structure |
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| CrystalStruct = triclinic (anhydrous) <br> monoclinic (monohydrate) |
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| CrystalStruct = triclinic (anhydrous) <br> monoclinic (monohydrate) |
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}} |
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}} |
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| Section7 = {{Chembox Hazards |
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|Section7={{Chembox Hazards |
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| ExternalMSDS = |
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| ExternalSDS = |
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| MainHazards = |
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| EUIndex = Corrosive ('''C''') |
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| MainHazards = |
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| NFPA-H = 2 |
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| NFPA-H = 1 |
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| NFPA-F = 0 |
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| NFPA-F = 0 |
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| NFPA-R = 1 |
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| FlashPt = Non-flammable |
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| NFPA-R = 1 |
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| GHSPictograms = {{GHS05}} |
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| FlashPt = Non-flammable |
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| GHSSignalWord = Danger |
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| RPhrases = {{R34}} {{R37}} {{R41}} |
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| HPhrases = {{H-phrases|318}} |
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| SPhrases = {{S26}} {{S36}} {{S37}} {{S39}} {{S45}} |
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| PPhrases = {{P-phrases|280|305+351+338|310}} |
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}} |
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}} |
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| Section8 = {{Chembox Related |
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|Section8={{Chembox Related |
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| OtherAnions = ] |
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| OtherAnions = ] |
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| OtherCations = ] |
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| OtherCations = ] |
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'''Sodium bisulfate''', also known as '''sodium hydrogen sulfate''' (NaHSO<sub>4</sub>), is an ]. It is a dry granular product that can be safely shipped and stored. The ] form is ]. Solutions of sodium bisulfate are acidic, with a 1M solution having a pH of < 1. |
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'''Sodium bisulfate''', also known as '''sodium hydrogen sulfate''',{{Efn|The prefix "bi" in "bisulfate" comes from an outdated naming system and is based on the observation that there is two times as much ] (SO<sub>4</sub>) in sodium bisulfate (NaHSO<sub>4</sub>) and other bisulfates as in ] (Na<sub>2</sub>SO<sub>4</sub>) and other sulfates.|name=|group=lower-alpha}} is the ] salt of the ] ], with the molecular formula NaHSO<sub>4</sub>. Sodium bisulfate is an ] formed by partial neutralization of ] by an equivalent of sodium base, typically in the form of either ] (lye) or ] (table salt). It is a dry granular product that can be safely shipped and stored. The ] form is ]. Solutions of sodium bisulfate are acidic, with a 1M solution having a pH of slightly below 1. |
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==Production== |
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One production method involves mixing ] quantities of ] and ] which react to form sodium bisulfate and ]. |
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Sodium bisulfate is produced as an intermediate in the ], an industrial process involving the reaction of ] and ]:<ref name=Ull>{{cite journal|author=Helmold Plessen|title=Sodium Sulfates|journal=Ullmann's Encyclopedia of Industrial Chemistry|publisher=Wiley-VCH|year=2000|location=Weinheim|doi=10.1002/14356007.a24_355|isbn=978-3527306732}}</ref> |
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:{{chem2 | NaCl + H2SO4 -> HCl + NaHSO4 }} |
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The process for the formation of sodium bisulfate is highly exothermic. The liquid sodium bisulfate is sprayed and cooled so that it forms a solid bead. The hydrogen chloride gas is dissolved in water to produce ] as a useful coproduct of the reaction. |
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Sodium bisulfate can be generated as a byproduct of the production of many other mineral acids via the reaction of their sodium salts with an excess of ]: |
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:NaOH + H<sub>2</sub>SO<sub>4</sub> → NaHSO<sub>4</sub> + H<sub>2</sub>O |
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:NaX + H<sub>2</sub>SO<sub>4</sub> → NaHSO<sub>4</sub> + HX ( X<sup>−</sup> = CN<sup>−</sup>, NO<sub>3</sub><sup>−</sup>, ClO<sub>4</sub><sup>−</sup>) |
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The acids HX produced have a lower boiling point than the reactants and are separated from the reaction mixture by distillation. |
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===Chemical reactions=== |
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A second production method involves reacting ] (salt) and sulfuric acid at elevated temperatures to produce sodium bisulfate and ] gas. |
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Hydrated sodium bisulfate dehydrates at {{convert|58|C|F}} at which point it separates from the water molecule attached to it. Once cooled again, it is freshly hygroscopic. Heating sodium bisulfate to {{convert|280|C|F}} produces ], another colorless salt:<ref name=Ull/> |
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:{{chem2 | 2 NaHSO4 -> Na2S2O7 + H2O }} |
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==Uses== |
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:NaCl + H<sub>2</sub>SO<sub>4</sub> → NaHSO<sub>4</sub> + HCl |
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Sodium bisulfate is used primarily to lower pH. It is also used in metal finishing, ]s,<ref>John Toedt, Darrell Koza, Kathleen Van Cleef-Toedt ''Chemical Composition of Everyday Products'' </ref> and to lower the pH of water for effective chlorination in swimming pools and hot tubs.<ref>{{cite web|url=https://www.jones-hamilton.com/sodium-bisulfate-pool/|title=Sodium Bisulfate in Pools}}</ref> Sodium bisulfate is also AAFCO approved as a general-use feed additive, including use in ]<ref>{{cite web |title=Sodium bisulfate in Animal Feed, Agriculture|url=https://www.jones-hamilton.com/jhproducts/afg/ |publisher=Jones-Hamilton}}</ref> and companion animal food.<ref>{{cite web |title=Sodium bisulfate Pet Food|url=https://www.petsbs.com|publisher=Jones-Hamilton}}</ref> It is used as a urine acidifier to reduce urinary stones in cats.<ref>{{cite journal |last1=Spears |first1=Julie K. |last2=Grieshop |first2=Christine M. |last3=Fahey |first3=G. C. |date=October 2003 |title=Evaluation of sodium bisulphate and phosphoric acid as urine acidifiers for cats |url=http://www.tandfonline.com/doi/abs/10.1080/00039420310001607743 |journal=Archives of Animal Nutrition |language=en |volume=57 |issue=5 |pages=389–398 |doi=10.1080/00039420310001607743 |pmid=14620912 |s2cid=43171090 |issn=1745-039X}}</ref> |
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It is highly toxic to certain ]s, but fairly harmless to most other life forms; so it is used in controlling outbreaks of ]. |
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The liquid sodium bisulfate is sprayed and cooled so that it forms a solid bead. The hydrogen chloride gas is dissolved in water to produce ] as a useful coproduct of the reaction. |
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Sodium bisulfate was the primary active ingredient in the toilet bowl cleaners ] and ], both now discontinued.<ref>, Reckitt Benckiser.</ref> |
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There are only two producers in the USA: Jones-Hamilton Co. uses the sulfuric acid/sodium chloride process, which produces the anhydrous form. Jost Chemical uses the sodium hydroxide/sulfuric acid method, which produces the monohydrate. |
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In the textiles industry, it is sometimes applied to ] cloth made with a silk backing and a pile of cellulose-based fiber (rayon, cotton, hemp, etc.) to create "burnout velvet": the sodium bisulfate, when applied to such a fabric and heated, causes the cellulose-based fibers to become brittle and flake away, leaving burned-out areas in the finished material, usually in attractive patterns.<ref name="Singer2007">{{cite book|author=Margo Singer|title=Textile Surface Decoration: Silk and Velvet|url=https://books.google.com/books?id=cTC8oKysf_0C&pg=PA35|date=11 July 2007|publisher=University of Pennsylvania|isbn=978-0-8122-2000-1|page=35}}</ref> |
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==Uses== |
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Sodium bisulfate is the active ingredient in some granular ] treatments used to control ammonia.<ref name=":0">{{cite journal |last1=Talghari |first1=Mariam |last2=Behnamifar |first2=Alireza |last3=Rahimi |first3=Shaban |last4=Karimi Torshizi |first4=Mohammad Amir |last5=Beckstead |first5=Robert |last6=Grimes |first6=Jesse L. |date=2020-10-01 |title=The effect of sodium bisulfate and coccidiostat on intestinal lesions and growth performance of Eimeria spp.–challenged broilers |journal=Poultry Science |volume=99 |issue=10 |pages=4769–4775 |doi=10.1016/j.psj.2020.06.060 |issn=0032-5791 |pmc=7598339 |pmid=32988511}}</ref> Sodium bisulfate has also been shown to significantly reduce the concentration of ''Campylobacter'' and ''Salmonella'' in chicken houses.<ref>{{cite web|url=https://naldc.nal.usda.gov/download/12419/PDF|title=Campylobacter and Salmonella Populations Associated with Chickens Raised on Acidified Litter}}</ref> |
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Sodium bisulfate is used primarily to lower pH. For technical grade applications it is used in metal finishing, cleaning products, and to lower the pH of water for effective chlorination, including swimming pools. Sodium bisulfate is also AAFCO approved as a general use feed additive, including companion animal food. It is used as a urine acidifier to reduce urinary stones in cats. Sodium bisulfate is considered GRAS (Generally Recognized As Safe) by FDA<ref></ref> and meets their definition of a natural product. The food grade product meets the requirements set out in the Food Chemicals Codex (FCC). It is denoted by E number E514ii in the EU. Food Grade sodium bisulfate is used in a variety of food products, including beverages, dressings, sauces, and fillings. It is also widely used in meat and poultry processing and most recently in browning prevention of fresh cut produce. |
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Sodium bisulfate is sometimes used as the active ingredient in ] tablets, a step in soil and water quality test kits.<ref>{{cite web|url=https://www.mosserlee.com/wp-content/uploads/2021/08/5504A-Floc-Ex-Tablets-06-01-2015.pdf|title=Floc Ex Tablet MSDS|publisher=LaMotte|date=1 June 2015}}</ref> |
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In ], sodium bisulfate is the primary ingredient used in many ] solutions to remove the oxidation layer from surfaces, which occurs after heating.<ref>{{Citation | last = Fisch | first = Arline M. | title = Textile Techniques in Metal: For Jewelers, Textile Artists & Sculptors | page = 32 | publisher = Lark Books | year = 2003 | url = http://books.google.com/books?id=4eFNLNSDNZgC&pg=PA32 | isbn = 9781579905149 | postscript =.}}</ref> |
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===In food=== |
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Highly toxic to at least some ]s but fairly harmless to most other lifeforms, sodium bisulfate is used in controlling outbreaks of ]. |
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Sodium bisulfate is used as a ] to leaven cake mixes (make them rise)<ref>{{cite web |title=GRAS Notice 000003: Sodium bisulfate - FDA|url=https://www.fda.gov/downloads/Food/IngredientsPackagingLabeling/GRAS/NoticeInventory/ucm264384.pdf |publisher=FDA}}</ref> as well as being used in meat and poultry processing and most recently in browning prevention of fresh-cut produce.<ref>{{cite web |title=Sodium Bisulfate - USDA |publisher=USDA |url=https://www.ams.usda.gov/sites/default/files/media/Sodium%20Bi%20report%202015.pdf}}</ref> Sodium bisulfate is considered ] (GRAS) by the FDA and has been named to the ]<ref>{{cite web |title=EPA Safer Choice Chemical List|date=11 December 2013 |url=https://www.epa.gov/saferchoice/safer-ingredients |publisher=EPA}}</ref> Safer Chemicals Ingredients List. The food-grade product also meets the requirements set out in the ]. It is denoted by ] E514ii in the EU and is also approved for use in Australia, New Zealand, Canada, and Mexico.<ref>{{cite web|url=http://www.legislation.gov.au/Details/F2012C00863/Html/Text|title=Australia New Zealand Food Standards Code - Standard 1.2.4 - Labelling of Ingredients|website=www.legislation.gov.au}}</ref> where it is listed as additive 514<!-- Listed as additive 514 in which one of the aforementioned countries? -->. Food grade sodium bisulfate is used in a variety of food products, including beverages, dressings, sauces, and fillings. It has many synonyms including<ref>{{cite web|url=http://noshly.com/|title=Wise Eating, Made Easy|website=Noshly}}</ref> bisulfate of soda, sodium acid sulfate, mono sodium hydrogen sulfate, sodium hydrogen sulfate, sodium hydrosulfate, and sulfuric acid sodium salt (1:1). |
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Sodium bisulfate lowers the pH without creating a sour taste, and has been used in the place of citric, malic, or phosphoric acids that are commercially available,<ref name=":0" /> and it can also be used as an anti-browning agent.<ref>{{cite journal|last1=Ali|first1=Hussein M.|last2=El-Gizawy|first2=Ahmed M.|last3=El-Bassiouny|first3=Rawia E. I.|last4=Saleh|first4=Mahmoud A.|date=2017-05-04|title=Browning inhibition mechanisms by cysteine, ascorbic acid and citric acid, and identifying PPO-catechol-cysteine reaction products|journal=Journal of Food Science and Technology|volume=52|issue=6|pages=3651–3659|doi=10.1007/s13197-014-1437-0|issn=0022-1155|pmc=4444905|pmid=26028748}}</ref> |
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== Notes == |
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{{Notelist}} |
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The "bi" refers to the presence of the hydrogen. |
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==References== |
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==References== |
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{{reflist}} |
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{{reflist}} |
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== Further reading == |
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== External links == |
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{{Sodium compounds}} |
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{{Sodium compounds}} |
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{{Sulfates}} |
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