Silver sulfate: Difference between revisions

Silver sulfate
Names
	IUPAC name Silver(I) sulfate
	Other names Disilver sulfate ; Argentous sulfate
Identifiers
CAS Number	10294-26-5 ;
3D model (JSmol)	Interactive image;
ChemSpider	140554 ;
ECHA InfoCard	100.030.581
EC Number	233-653-7;
PubChem CID	159865;
UNII	8QG6HV4ZPO ;
UN number	3077
CompTox Dashboard (EPA)	DTXSID70172884 ;
	InChI InChI=1S/2Ag.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2+1;/p-2 Key: YPNVIBVEFVRZPJ-UHFFFAOYSA-L ; InChI=1/2Ag.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2+1;/p-2 Key: YPNVIBVEFVRZPJ-NUQVWONBAA;
	SMILES [Ag+].[Ag+].[O-]S([O-])(=O)=O;
Properties
Chemical formula	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)
Melting point	652.2–660 °C (1,206.0–1,220.0 °F; 925.4–933.1 K)
Boiling point	1,085 °C (1,985 °F; 1,358 K) decomposition
Solubility in water	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)
Solubility product (Ksp)	1.2·10−5
Solubility	Dissolves in aq. acids, alcohols, acetone, ether, acetates, amides; Insoluble in ethanol
Solubility in sulfuric acid	8.4498 g/L (0.1 molH2SO4/LH2O); 25.44 g/100 g (13 °C); 31.56 g/100 g (24.5 °C); 127.01 g/100 g (96 °C)
Solubility in ethanol	7.109 g/L (0.5 nEtOH/H2O)
Solubility in acetic acid	7.857 g/L (0.5 nAcOH/H2O)
Magnetic susceptibility (χ)	−9.29·10−5 cm3/mol
Refractive index (nD)	nα = 1.756; nβ = 1.775; nγ = 1.782
Structure
Crystal structure	Orthorhombic, oF56
Space group	Fddd, No. 70
Point group	2/m 2/m 2/m
Lattice constant	a = 10.2699(5) Å, b = 12.7069(7) Å, c = 5.8181(3) Å α = 90°, β = 90°, γ = 90°
Thermochemistry
Heat capacity (C)	131.4 J/mol·K
Std molar; entropy (S⦵298)	200.4 J/mol·K
Std enthalpy of; formation (ΔfH⦵298)	−715.9 kJ/mol
Gibbs free energy (ΔfG⦵)	−618.4 kJ/mol
Hazards
	GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H318, H410
Precautionary statements	P273, P280, P305+P351+P338, P501
NFPA 704 (fire diamond)	2 0 1
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

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Latest revision as of 18:48, 10 April 2024

Silver sulfate is the inorganic compound with the formula Ag₂SO₄. It is a white solid with low solubility in water.

Preparation and structure

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

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

^ ^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.

[crc-1] ^ ^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.

[sioc-2] Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). New York: D. Van Nostrand Company. pp. 622–623.

[chemister-3] Anatolievich, Kiper Ruslan. "silver sulfate". Retrieved 2014-07-19.

[nbs25-13-4] 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.

[fca-5] "MSDS of Silver sulfate". Fisher Scientific, Inc. Retrieved 2014-07-19.

[sigma-6] Sigma-Aldrich Co., Silver sulfate. Retrieved on 2014-07-19.

[7] 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.

[8] 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.

[9] 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.

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@@ Line 87: / Line 87: @@
 ==Preparation and structure==
 Silver sulfate precipitates as a solid when an aqueous solution of [[silver nitrate]] is treated with [[sulfuric acid]]:
+:{{chem2 | 2 AgNO3 + H2SO4 -> Ag2SO4 + 2 HNO3 }}
-:2{{nbsp}}AgNO<sub>3</sub>  + H<sub>2</sub>SO<sub>4</sub> →  Ag<sub>2</sub>SO<sub>4</sub> + 2{{nbsp}}HNO<sub>3</sub>
-It is purified by recrystallization from concentrated sulfuric acid, a step that expels traces of nitrate.<ref>{{cite book|author1=O. Glemser|author2=R. Sauer|chapter=Copper (I) Sulfate|title=Handbook of Preparative Inorganic Chemistry, 2nd Ed. |editor=G. Brauer|publisher=Academic Press|year=1963|place=NY, NY|volume=2pages=1042}}</ref>
+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>
 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>
@@ Line 94: / Line 94: @@
 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&nbsp;°C with evolution of oxygen and the formation of the [[pyrosulfate]].
+:{{chem2 | AgF2 + H2SO4 -> AgSO4 + 2 HF }}
-AgF<sub>2</sub>+H<sub>2</sub>SO<sub>4</sub> →AgSO<sub>4</sub> +2HF
+:{{chem2 | 4 AgSO4 -> 2 Ag2S2O7 + O2 }}
 ==References==
@@ Line 104: / Line 105: @@
 [[Category:Silver compounds]]
 [[Category:Sulfates]]
-{{inorganic-compound-stub}}