Silver sulfate: Difference between revisions
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{{chembox |
{{chembox |
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| Watchedfields = changed |
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| verifiedrevid = 464391509 |
| verifiedrevid = 464391509 |
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| Name = Silver sulfate |
| Name = Silver sulfate |
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| ImageFile = silver sulfate.png |
| ImageFile = silver sulfate.png |
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| ImageSize = 160px |
| ImageSize = 160px |
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| ImageName = Skeletal formula of silver sulfate |
| ImageName = Skeletal formula of silver sulfate |
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| ImageFile1 = |
| ImageFile1 = Silver(I)-sulfate-xtal-2x2x2-3D-sf-v2.png |
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| ImageSize1 = 150px |
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| ImageName1 = Sample of silver sulfate |
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| ImageFile2 = Zilversulfaat.JPG |
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| ImageName2 = Sample of silver sulfate |
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| OtherNames = Disilver sulfate <br/> Argentous sulfate |
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| SystematicName = |
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⚫ | |||
| CASNo = 10294-26-5 |
| CASNo = 10294-26-5 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
| CASNo_Ref = {{cascite|correct|CAS}} |
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| InChIKey = YPNVIBVEFVRZPJ-NUQVWONBAA |
| InChIKey = YPNVIBVEFVRZPJ-NUQVWONBAA |
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}} |
}} |
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|Section2={{Chembox Properties |
| Section2 = {{Chembox Properties |
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| Formula = Ag<sub>2</sub>SO<sub>4</sub> |
| Formula = Ag<sub>2</sub>SO<sub>4</sub> |
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| Ag=2 | S=1 | O=4 |
| Ag=2 | S=1 | O=4 |
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| Appearance = Colorless |
| Appearance = Colorless solid |
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| Odor = Odorless |
| Odor = Odorless |
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| Density = 5.45 g/cm<sup>3</sup> (25 °C)<br> 4.84 g/cm<sup>3</sup> (660 °C)<ref name=crc /> |
| Density = 5.45 g/cm<sup>3</sup> (25 °C)<br> 4.84 g/cm<sup>3</sup> (660 °C)<ref name=crc /> |
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| Solubility = 0.57 g/100 mL (0 °C)<br> 0.69 g/100 mL (10 °C)<br> 0.83 g/100 mL (25 °C)<br> 0.96 g/100 mL (40 °C)<br> 1.33 g/100 mL (100 °C)<ref name=sioc>{{cite book| |
| Solubility = 0.57 g/100 mL (0 °C)<br> 0.69 g/100 mL (10 °C)<br> 0.83 g/100 mL (25 °C)<br> 0.96 g/100 mL (40 °C)<br> 1.33 g/100 mL (100 °C)<ref name=sioc>{{cite book|last1 = Seidell|first1 = Atherton|last2 = Linke|first2 = William F.|year = 1919|title = Solubilities of Inorganic and Organic Compounds|url = https://archive.org/details/solubilitiesino01seidgoog|publisher = D. Van Nostrand Company|place = New York|edition = 2nd|pages = [https://archive.org/details/solubilitiesino01seidgoog/page/n647 622]–623}}</ref> |
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| SolubleOther = Dissolves in aq. [[acid]]s, [[alcohol]]s, [[acetone]], [[diethyl ether|ether]], [[acetate]]s, [[amide]]s<ref name=sioc /><br> Insoluble in [[ |
| SolubleOther = Dissolves in aq. [[acid]]s, [[Alcohol (chemistry)|alcohol]]s, [[acetone]], [[diethyl ether|ether]], [[acetate]]s, [[amide]]s<ref name=sioc /><br> Insoluble in [[ethanol]]<ref name=chemister /> |
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| Solubility1 = 8.4498 g/L (0.1 mol<sub>H<sub>2</sub>SO<sub>4</sub></sub>/L<sub>H<sub>2</sub>O</sub>)<ref name=sioc /><br> 25.44 g/100 g (13 °C)<br> 31.56 g/100 g (24.5 °C)<br> 127.01 g/100 g (96 °C)<ref name=chemister>{{cite web|last = Anatolievich|first = Kiper Ruslan |
| Solubility1 = 8.4498 g/L (0.1 mol<sub>H<sub>2</sub>SO<sub>4</sub></sub>/L<sub>H<sub>2</sub>O</sub>)<ref name=sioc /><br> 25.44 g/100 g (13 °C)<br> 31.56 g/100 g (24.5 °C)<br> 127.01 g/100 g (96 °C)<ref name=chemister>{{cite web|last = Anatolievich|first = Kiper Ruslan|url = http://chemister.ru/Database/properties-en.php?dbid=1&id=1253|title = silver sulfate|access-date = 2014-07-19}}</ref> |
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| Solvent1 = sulfuric acid |
| Solvent1 = sulfuric acid |
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| Solubility2 = 7.109 g/L (0.5 n<sub>EtOH/H<sub>2</sub>O</sub>)<ref name=sioc /> |
| Solubility2 = 7.109 g/L (0.5 n<sub>EtOH/H<sub>2</sub>O</sub>)<ref name=sioc /> |
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| BoilingPtC = 1085 |
| BoilingPtC = 1085 |
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| BoilingPt_ref = <ref name=chemister /><ref name=fca /> |
| BoilingPt_ref = <ref name=chemister /><ref name=fca /> |
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| BoilingPt_notes = decomposition |
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| SolubilityProduct = 1.2·10<sup>−5</sup><ref name=crc>{{CRC90}}</ref> |
| SolubilityProduct = 1.2·10<sup>−5</sup><ref name=crc>{{CRC90}}</ref> |
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| MagSus = −9.29·10<sup>−5</sup> cm<sup>3</sup>/mol<ref name=crc /> |
| MagSus = −9.29·10<sup>−5</sup> cm<sup>3</sup>/mol<ref name=crc /> |
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| RefractIndex = ''n''<sub>α</sub> = 1.756<br> ''n''<sub>β</sub> = 1.775<br> ''n''<sub>γ</sub> = 1.782<ref name=nbs25-13 /> |
| RefractIndex = ''n''<sub>α</sub> = 1.756<br> ''n''<sub>β</sub> = 1.775<br> ''n''<sub>γ</sub> = 1.782<ref name=nbs25-13 /> |
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}} |
}} |
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|Section3={{Chembox Structure |
| Section3 = {{Chembox Structure |
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| CrystalStruct = Orthorhombic, [[pearson symbol|oF56]]<ref name=nbs25-13>{{cite book|title = Standard X-ray Diffraction Powder Patterns|section = 13|first1 = Marlene C.|last1 = Morris|first2 = Howard F.|last2 = McMurdie|first3 = Eloise H.|last3 = Evans|first4 = Boris|last4 = Paretzkin|first5 = Johan H. de|last5 = Groot|first6 = Camden R.|last6 = Hubbard|first7 = Simon J.|last7 = Carmel|publisher = Institute for Materials Research National Bureau of Standards|place = Washington|date=June 1976|volume = 25}}</ref> |
| CrystalStruct = Orthorhombic, [[pearson symbol|oF56]]<ref name=nbs25-13>{{cite book|title = Standard X-ray Diffraction Powder Patterns|section = 13|first1 = Marlene C.|last1 = Morris|first2 = Howard F.|last2 = McMurdie|first3 = Eloise H.|last3 = Evans|first4 = Boris|last4 = Paretzkin|first5 = Johan H. de|last5 = Groot|first6 = Camden R.|last6 = Hubbard|first7 = Simon J.|last7 = Carmel|publisher = Institute for Materials Research National Bureau of Standards|place = Washington|date=June 1976|volume = 25}}</ref> |
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| SpaceGroup = Fddd, No. 70<ref name=nbs25-13 /> |
| SpaceGroup = Fddd, No. 70<ref name=nbs25-13 /> |
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| LattConst_alpha = 90 |
| LattConst_alpha = 90 |
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}} |
}} |
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|Section4={{Chembox Thermochemistry |
| Section4 = {{Chembox Thermochemistry |
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| DeltaHf = −715.9 kJ/mol<ref name=crc /> |
| DeltaHf = −715.9 kJ/mol<ref name=crc /> |
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| DeltaGf = −618.4 kJ/mol <ref name=crc /> |
| DeltaGf = −618.4 kJ/mol <ref name=crc /> |
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| Entropy = 200.4 |
| Entropy = 200.4 J/mol·K <ref name=crc /> |
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| HeatCapacity = 131.4 J/mol·K<ref name=crc /> |
| HeatCapacity = 131.4 J/mol·K<ref name=crc /> |
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}} |
}} |
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| Section5 = |
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| Section6 = |
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| GHSPictograms = {{GHS05}}{{GHS09}}<ref name="sigma">{{Sigma-Aldrich|id = 204412|name = Silver sulfate|accessdate = 2014-07-19}}</ref> |
| GHSPictograms = {{GHS05}}{{GHS09}}<ref name="sigma">{{Sigma-Aldrich|id = 204412|name = Silver sulfate|accessdate = 2014-07-19}}</ref> |
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| GHSSignalWord = Danger |
| GHSSignalWord = Danger |
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| NFPA-F = 0 |
| NFPA-F = 0 |
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| NFPA-R = 1 |
| NFPA-R = 1 |
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| NFPA_ref = <ref name=fca>{{cite web|title = MSDS of Silver sulfate|url = https://www.fishersci.ca/viewmsds.do?catNo=S19025 |
| NFPA_ref = <ref name=fca>{{cite web|title = MSDS of Silver sulfate|url = https://www.fishersci.ca/viewmsds.do?catNo=S19025|publisher = Fisher Scientific, Inc|access-date = 2014-07-19}}</ref> |
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'''Silver sulfate''' is the [[inorganic compound]] with the formula Ag<sub>2</sub>SO<sub>4</sub>. It is a white solid with low solubility in water. |
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'''Silver sulfate''' (Ag<sub>2</sub>SO<sub>4</sub>) is an [[ion]]ic compound of [[silver]] used in [[silver plating]] and as a non-staining substitute to [[silver nitrate]]. This [[sulfate]] is stable under ordinary conditions of use and storage, though it darkens upon exposure to air or light. It is minimally soluble in water. |
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==Preparation== |
==Preparation and structure== |
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Silver sulfate |
Silver sulfate precipitates as a solid when an aqueous solution of [[silver nitrate]] is treated with [[sulfuric acid]]: |
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:{{chem2 | 2 AgNO3 + H2SO4 -> Ag2SO4 + 2 HNO3 }} |
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It is purified by recrystallization from concentrated sulfuric acid, a step that expels traces of nitrate.<ref>{{cite book |author1=O. Glemser |title=Handbook of Preparative Inorganic Chemistry, 2nd Ed. |author2=R. Sauer |publisher=Academic Press |year=1963 |editor=G. Brauer |volume=2pages=1042 |place=NY, NY |chapter=Silver Sulfate}}</ref> |
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Silver sulfate and anhydrous [[sodium sulfate]] adopt the same structure.<ref>{{cite journal |doi=10.1524/zkri.1932.82.1.161 |title=Note on the Crystal Structure of Silver Sulphate, Ag<sub>2</sub>SO<sub>4</sub> |year=1932 |last1=Zachariasen |first1=W. H. |journal=Zeitschrift für Kristallographie - Crystalline Materials |volume=82 |issue=1–6 |pages=161–162 |s2cid=101362527 }}</ref> |
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AgNO<sub>3</sub>(aq) + H<sub>2</sub>SO<sub>4</sub>(aq) = AgHSO<sub>4</sub>(aq) + HNO<sub>3</sub>(aq) |
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⚫ | The synthesis of '''silver(II) sulfate''' (AgSO<sub>4</sub>) with a divalent silver ion instead of a monovalent silver ion was first reported in 2010<ref>{{Cite journal| doi = 10.1002/anie.200906863| pmid = 20084660| year = 2010| last1 = Malinowski | first1 = P.| last2 = Derzsi | first2 = M.| last3 = Mazej | first3 = Z.| last4 = Jagličić | first4 = Z.| last5 = Gaweł | first5 = B.| last6 = Lasocha | first6 = W.| last7 = Grochala | first7 = W.| title = Ag(II)SO(4): A Genuine Sulfate of Divalent Silver with Anomalously Strong One-Dimensional Antiferromagnetic Interactions.| volume = 49| issue = 9| pages = 1683–1686| journal = Angewandte Chemie International Edition in English | doi-access = free}}</ref> by adding [[sulfuric acid]] to [[silver(II) fluoride]] ([[Hydrogen fluoride|HF]] escapes). It is a black solid that decomposes exothermically at 120 °C with evolution of oxygen and the formation of the [[pyrosulfate]]. |
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:{{chem2 | AgF2 + H2SO4 -> AgSO4 + 2 HF }} |
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2 AgHSO<sub>4</sub>(aq) <=> Ag<sub>2</sub>SO<sub>4</sub>(s) + H<sub>2</sub>SO<sub>4</sub>(aq) reversible reaction |
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:{{chem2 | 4 AgSO4 -> 2 Ag2S2O7 + O2 }} |
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The precipitate is then washed with hot water and preparation is under ruby red illumination. |
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⚫ | The synthesis of '''silver(II) sulfate''' (AgSO<sub>4</sub>) with a divalent silver ion instead of a monovalent silver ion was first reported in 2010<ref>{{Cite journal| doi = 10.1002/anie.200906863| pmid = 20084660| year = 2010| last1 = Malinowski | first1 = P.| last2 = Derzsi | first2 = M.| last3 = Mazej | first3 = Z.| last4 = Jagličić | first4 = Z.| last5 = Gaweł | first5 = B.| last6 = Lasocha | first6 = W.| last7 = Grochala | first7 = W.| title = Ag(II)SO(4): A Genuine Sulfate of Divalent Silver with Anomalously Strong One-Dimensional Antiferromagnetic Interactions.| volume = 49| issue = 9| pages = 1683–1686| journal = Angewandte Chemie International Edition in English }}</ref> by adding [[sulfuric acid]] to [[silver(II) fluoride]] ([[Hydrogen fluoride|HF]] escapes). It is a black solid that decomposes |
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==References== |
==References== |
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[[Category:Silver compounds]] |
[[Category:Silver compounds]] |
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[[Category:Sulfates]] |
[[Category:Sulfates]] |
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{{inorganic-compound-stub}} |
Latest revision as of 18:48, 10 April 2024
Names | |
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IUPAC name
Silver(I) sulfate
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Other names
Disilver sulfate
Argentous sulfate | |
Identifiers | |
3D model (JSmol)
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ChemSpider | |
ECHA InfoCard | 100.030.581 |
EC Number |
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PubChem CID
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UNII | |
UN number | 3077 |
CompTox Dashboard (EPA)
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Properties | |
Ag2SO4 | |
Molar mass | 311.79 g·mol−1 |
Appearance | Colorless solid |
Odor | Odorless |
Density | 5.45 g/cm3 (25 °C) 4.84 g/cm3 (660 °C)[1] |
Melting point | 652.2–660 °C (1,206.0–1,220.0 °F; 925.4–933.1 K)[1][5] |
Boiling point | 1,085 °C (1,985 °F; 1,358 K)[3][5] decomposition |
0.57 g/100 mL (0 °C) 0.69 g/100 mL (10 °C) 0.83 g/100 mL (25 °C) 0.96 g/100 mL (40 °C) 1.33 g/100 mL (100 °C)[2] | |
Solubility product (Ksp)
|
1.2·10−5[1] |
Solubility | Dissolves in aq. acids, alcohols, acetone, ether, acetates, amides[2] Insoluble in ethanol[3] |
Solubility in sulfuric acid | 8.4498 g/L (0.1 molH2SO4/LH2O)[2] 25.44 g/100 g (13 °C) 31.56 g/100 g (24.5 °C) 127.01 g/100 g (96 °C)[3] |
Solubility in ethanol | 7.109 g/L (0.5 nEtOH/H2O)[2] |
Solubility in acetic acid | 7.857 g/L (0.5 nAcOH/H2O)[2] |
−9.29·10−5 cm3/mol[1] | |
Refractive index (nD)
|
nα = 1.756 nβ = 1.775 nγ = 1.782[4] |
Structure | |
Orthorhombic, oF56[4] | |
Fddd, No. 70[4] | |
2/m 2/m 2/m[4] | |
a = 10.2699(5) Å, b = 12.7069(7) Å, c = 5.8181(3) Å[4] α = 90°, β = 90°, γ = 90°
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Thermochemistry | |
Heat capacity (C)
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131.4 J/mol·K[1] |
Std molar
entropy (S⦵298) |
200.4 J/mol·K [1] |
Std enthalpy of
formation (ΔfH⦵298) |
−715.9 kJ/mol[1] |
Gibbs free energy (ΔfG⦵)
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−618.4 kJ/mol [1] |
Hazards | |
GHS labelling: | |
[6] | |
Danger | |
H318, H410[6] | |
P273, P280, P305+P351+P338, P501[6] | |
NFPA 704 (fire diamond) | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Silver sulfate is the inorganic compound with the formula Ag2SO4. It is a white solid with low solubility in water.
Preparation and structure
[edit]Silver sulfate precipitates as a solid when an aqueous solution of silver nitrate is treated with sulfuric acid:
- 2 AgNO3 + H2SO4 → Ag2SO4 + 2 HNO3
It is purified by recrystallization from concentrated sulfuric acid, a step that expels traces of nitrate.[7] Silver sulfate and anhydrous sodium sulfate adopt the same structure.[8]
Silver(II) sulfate
[edit]The synthesis of silver(II) sulfate (AgSO4) with a divalent silver ion instead of a monovalent silver ion was first reported in 2010[9] by adding sulfuric acid to silver(II) fluoride (HF escapes). It is a black solid that decomposes exothermically at 120 °C with evolution of oxygen and the formation of the pyrosulfate.
- AgF2 + H2SO4 → AgSO4 + 2 HF
- 4 AgSO4 → 2 Ag2S2O7 + O2
References
[edit]- ^ a b c d e f g h Lide, David R., ed. (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN 978-1-4200-9084-0.
- ^ a b c d e Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). New York: D. Van Nostrand Company. pp. 622–623.
- ^ a b c Anatolievich, Kiper Ruslan. "silver sulfate". Retrieved 2014-07-19.
- ^ a b c d e Morris, Marlene C.; McMurdie, Howard F.; Evans, Eloise H.; Paretzkin, Boris; Groot, Johan H. de; Hubbard, Camden R.; Carmel, Simon J. (June 1976). "13". Standard X-ray Diffraction Powder Patterns. Vol. 25. Washington: Institute for Materials Research National Bureau of Standards.
- ^ a b c "MSDS of Silver sulfate". Fisher Scientific, Inc. Retrieved 2014-07-19.
- ^ a b c Sigma-Aldrich Co., Silver sulfate. Retrieved on 2014-07-19.
- ^ O. Glemser; R. Sauer (1963). "Silver Sulfate". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2pages=1042. NY, NY: Academic Press.
- ^ Zachariasen, W. H. (1932). "Note on the Crystal Structure of Silver Sulphate, Ag2SO4". Zeitschrift für Kristallographie - Crystalline Materials. 82 (1–6): 161–162. doi:10.1524/zkri.1932.82.1.161. S2CID 101362527.
- ^ Malinowski, P.; Derzsi, M.; Mazej, Z.; Jagličić, Z.; Gaweł, B.; Lasocha, W.; Grochala, W. (2010). "Ag(II)SO(4): A Genuine Sulfate of Divalent Silver with Anomalously Strong One-Dimensional Antiferromagnetic Interactions". Angewandte Chemie International Edition in English. 49 (9): 1683–1686. doi:10.1002/anie.200906863. PMID 20084660.