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| verifiedrevid = 414433768 |
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| verifiedrevid = 429617177 |
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| Name = Mercury(I) sulfate |
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| Name = Mercury(I) sulfate |
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| ImageFile1 = Mercury(I)sulfate.svg |
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| ImageSize1 = 130 |
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| ImageName = |
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| ImageFile2 = EntryWithCollCode248726.png |
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| ImageSize2 = 276 |
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| IUPACName = Mercury(I) sulfate |
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| IUPACName = Mercury(I) sulfate |
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| OtherNames = Mercurous sulfate |
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| OtherNames = Mercurous sulfate |
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| Section1 = {{Chembox Identifiers |
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|Section1={{Chembox Identifiers |
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| CASNo_Ref = {{cascite|correct|??}} |
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| CASNo = 7783-36-0 |
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| CASNo = 7783-36-0 |
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| CASNoOther = |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| CASOther = |
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| UNII = PI950N9DYS |
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| RTECS = |
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| EINECS = |
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| EINECS = 231-993-0 |
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| PubChem = 24545 |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 22951 |
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| SMILES = S(=O)(=O). |
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| StdInChI_Ref = {{stdinchicite|changed|chemspider}} |
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| StdInChI = 1S/2Hg.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2*+1;/p-2 |
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| StdInChIKey_Ref = {{stdinchicite|changed|chemspider}} |
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| StdInChIKey = MINVSWONZWKMDC-UHFFFAOYSA-L |
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| Section2 = {{Chembox Properties |
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|Section2={{Chembox Properties |
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| Formula = Hg<sub>2</sub>SO<sub>4</sub> |
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| Formula = Hg<sub>2</sub>SO<sub>4</sub> |
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| MolarMass = 497.24 g/mol |
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| MolarMass = 497.24 g/mol |
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| Appearance = whitish-yellow crystals |
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| Appearance = whitish-yellow crystals |
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| Density = 7.56 g/cm<sup>3</sup> |
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| Density = 7.56 g/cm<sup>3</sup> |
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| Solubility = 0.051 g/100 mL |
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| Solubility = 0.051 g/100 mL (25 °C) <br /> 0.09 g/100 mL (100 °C) |
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| SolubleOther = soluble in dilute ]<ref name="hand"> |
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| SolubleOther = soluble in dilute ], Insoluble in ], Soluble in hot ]. |
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| SolubilityProduct = 6.5{{e|−7}}<ref name="crc">{{cite book |author1=John Rumble |title=CRC Handbook of Chemistry and Physics |date=June 18, 2018 |publisher=CRC Press |isbn=978-1-138-56163-2 |pages=5–189|edition=99 |language=English}}</ref> |
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{{Citation |
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| first = David R. |
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| year = 1998 |
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| title = Handbook of Chemistry and Physics |
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| edition = 87 |
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| publication-place = Boca Raton, FL |
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| publisher = CRC Press |
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| isbn = 0-8493-0594-2 |
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| pages = 4–69 |
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}}</ref> |
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| MeltingPt = |
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| MeltingPt = |
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| BoilingPt = |
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| BoilingPt = |
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| MagSus = −123.0·10<sup>−6</sup> cm<sup>3</sup>/mol |
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| Section3 = {{Chembox Structure |
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| Coordination = |
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| Coordination = monoclinic |
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| Section4 = {{Chembox Thermochemistry |
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|Section4={{Chembox Thermochemistry |
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| DeltaHf = -743.1 ] |
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| DeltaHf = -743.1 ] |
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| DeltaHc = |
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| DeltaHc = |
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| Entropy = 200.7 J·mol<sup>-1</sup>·K<sup>-1</sup> |
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| Entropy = 200.7 J·mol<sup>−1</sup>·K<sup>−1</sup> |
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| HeatCapacity = 132 J·mol<sup>-1</sup>·K<sup>-1</sup><ref name="hand2"> |
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| HeatCapacity = 132 J·mol<sup>−1</sup>·K<sup>−1</sup><ref name="hand2"> |
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{{Citation |
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{{Citation |
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| last = Lide |
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| last = Lide |
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| first = David R. |
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| first = David R. |
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| author-link = |
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| year = 1998 |
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| title = Handbook of Chemistry and Physics |
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| last2 = |
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| edition = 87 |
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| location = Boca Raton, FL |
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| publisher = CRC Press |
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| publication-date = |
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| isbn = 0-8493-0594-2 |
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| date = |
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| year = 1998 |
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| pages = 5–19 |
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| title = Handbook of Chemistry and Physics |
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| edition = 87 |
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| publication-place = Boca Raton, FL |
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| publisher = CRC Press |
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| isbn = 0-8493-0594-2 |
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| pages = 5–19 |
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}}</ref> |
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| Section7 = {{Chembox Hazards |
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'''Mercury(I) sulfate''', commonly called mercurous sulfate (]) or mercurous sulphate (]) is the ] Hg<sub>2</sub>SO<sub>4</sub>.<ref>''Intermediate Inorganic Chemistry'' by J. W. Mellor, published by Longmans, Green and Company, London, 1941, page 388</ref> It can be produced by a reaction of ] with a source of ] ]s<ref name="google">, accessed 11 December 2010</ref>: |
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'''Mercury(I) sulfate''', commonly called ] (]) or mercurous sulfate (]) is the ] Hg<sub>2</sub>SO<sub>4</sub>.<ref>''Intermediate Inorganic Chemistry'' by J. W. Mellor, published by Longmans, Green and Company, London, 1941, page 388</ref> Mercury(I) sulfate is a metallic compound that is a white, pale yellow or beige powder.<ref>{{Cite web|url=http://www.chemicalbook.com/ChemicalProductProperty_EN_CB0259783.htm|title = Mercurous Sulfate | 7783-36-0}}</ref> It is a metallic salt of sulfuric acid formed by replacing both hydrogen atoms with mercury(I). It is highly toxic; it could be fatal if inhaled, ingested, or absorbed by skin. |
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==Structure== |
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:Hg<sub>2</sub>(NO<sub>3</sub>)<sub>2</sub> + SO<sub>4</sub><sup>2-</sup> → Hg<sub>2</sub>SO<sub>4</sub> + 2 NO<sub>3</sub><sup>-</sup> |
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In the crystal, mercurous sulfate is made up of Hg<sub>2</sub><sup>2+</sup> center with an Hg-Hg distance of about 2.50 Å. The SO<sub>4</sub><sup>2−</sup> anions form both long and short Hg-O bonds ranging from 2.23 to 2.93 Å.<ref>{{cite journal|title=Preparation and Characterization of Dimercury(I)Monofluorophosphate(V), Hg<sub>2</sub>PO<sub>3</sub>F: Crystal Structure, Thermal Behavior, Vibrational Spectra, and Solid-State <sup>31</sup>P and <sup>19</sup>F NMR Spectra|author=Matthias Weil |author2=Michael Puchberger |author3=Enrique J. Baran |journal= Inorg. Chem.|year=2004|volume=43|issue=26|pages=8330–8335|doi=10.1021/ic048741e|pmid=15606179}}</ref> |
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Focusing on the shorter Hg-O bonds, the Hg – Hg – O bond angle is 165°±1°.<ref>{{cite journal|author=Dorm, E.|year=1969|title=Structural Studies on Mercury(I) Compounds. VI. Crystal Structure of Mercury(I) Sulfate and Selenate|journal=Acta Chemica Scandinavica|volume=23|pages=1607–15|doi=10.3891/acta.chem.scand.23-1607|doi-access=free}}</ref><ref>{{cite journal |doi=10.1107/S1600536814011155|title=Crystal structure of Hg2SO4– a redetermination|year=2014|last1=Weil|first1=Matthias|journal=Acta Crystallographica Section E|volume=70|issue=9|pages=i44|pmid=25309168|pmc=4186147}}</ref> |
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It can also be prepared by reacting an excess of ] with concentrated ]<ref name="google"/>: |
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==Preparation== |
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:2 Hg + 2 H<sub>2</sub>SO<sub>4</sub> → Hg<sub>2</sub>SO<sub>4</sub> + 2 H<sub>2</sub>O + SO<sub>2</sub> <!--typical reaction of sulfuric acid as oxidizing agent--> |
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One way to prepare mercury(I) sulfate is to mix the acidic solution of ] with 1 to 6 ] solution:,<ref name="google">, accessed 11 December 2010</ref><ref>''Mercurous Sulphate, cadmium sulphate, and the cadmium cell.'' by Hulett G. A. The physical review.1907. p.19. |
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</ref> |
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:{{chem2 | Hg2(NO3)2 + H2SO4 -> Hg2SO4 + 2 HNO3 }} |
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It can also be prepared by reacting an excess of ] with concentrated ]:<ref name="google"/> |
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:{{chem2 | 2 Hg + 2 H2SO4 -> Hg2SO4 + 2 H2O + SO2}}<!--typical reaction of sulfuric acid as oxidizing agent--> |
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== Use in electrochemical cells== |
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Mercury(I) sulfate is often used in ]s.<ref>"Influence of Microstucture on the Charge Storage Properties of Chemically Synthesized Manganese Dioxide" by Mathieu Toupin, Thiery Brousse, and Daniel Belanger. ''Chem. Mater.'' 2002, 14, 3945–3952</ref><ref>"Electromotive Force Studies of Cell, Cd<sub>x</sub>Hg<sub>y</sub> | CdSO<sub>4</sub>,(m) I Hg<sub>2</sub>SO<sub>4</sub>, Hg, in Dioxane-Water Media" by Somesh Chakrabarti and Sukumar Aditya. ''Journal of Chemical and Engineering Data'', Vol.17, No. 1, 1972</ref><ref>"Characterization of Lithium Sulfate as an Unsymmetrical-Valence Salt Bridge for the Minimization of Liquid Junction Potentials in Aqueous – Organic Solvent Mixtures" by Cristiana L. Faverio, Patrizia R. Mussini, and Torquato Mussini. ''Anal. Chem.'' 1998, 70, 2589–2595</ref> It was first introduced in electrochemical cells by Latimer Clark in 1872,<ref name="GEORGE AUGUSTUS HULETT 2000, p.91-98">"George Augustus Hulett: from Liquid Crystals to Standard Cell" by John T. Stock. ''Bull. Hist. Chem.'' Volume 25, Number 2, 2000, p.91-98</ref> It was then alternatively{{clarify|date=December 2019}} used in ]s made by George Augustus Hulett in 1911.<ref name="GEORGE AUGUSTUS HULETT 2000, p.91-98"/> It has been found to be a good electrode at high temperatures above 100 °C along with silver sulfate.<ref>{{cite journal |last1=Lietzke |first1=M. H. |last2=Stoughton |first2=R. W. |title=The Behavior of the Silver—Silver Sulfate and the Mercury—Mercurous Sulfate Electrodes at High Temperatures 1 |journal=Journal of the American Chemical Society |date=November 1953 |volume=75 |issue=21 |pages=5226–5227 |doi=10.1021/ja01117a024}}{{subscription required}}</ref> |
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Mercury(I) sulfate has been found to decompose at high temperatures. The decomposition process is ], and it occurs between 335 °C and 500 °C. |
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Mercury(I) sulfate has unique properties that make the standard cells possible. It has a rather low solubility (about one gram per liter); diffusion from the cathode system is not excessive; and it is sufficient to give a large potential at a mercury electrode.<ref>"Sulphates of Mercury and Standard Cells." by Elliott, R. B. and Hulett, G. A. ''The Journal of Physical Chemistry'' 36.7 (1932): 2083–2086. |
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</ref> |
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==References== |
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==References== |
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