Silver sulfate: Difference between revisions

Silver sulfate
Names
	IUPAC name Silver sulfate
	Other names disilver 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 crystals
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)
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 kJ/mol
Std enthalpy of; formation (ΔfH⦵298)	−715.9 kJ/mol
Gibbs free energy (ΔfG⦵)	−618.4 J/mol·K
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

Browse history interactively

← Previous edit Next edit →

Content deleted Content added

VisualWikitext

Inline

Revision as of 15:05, 7 July 2019

Silver sulfate (Ag₂SO₄) is an ionic 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.

Preparation

Silver sulfate is prepared by adding sulfuric acid to a solution of silver nitrate:

AgNO₃(aq) + H₂SO₄(aq) = AgHSO₄(aq) + HNO₃(aq)

2 AgHSO₄(aq) <=> Ag₂SO₄(s) + H₂SO₄(aq) reversible reaction

The precipitate is then washed with hot water and preparation is under ruby red illumination.

==teddy bean teddy bean is a evil person who will show up in the next avengers movie as the next villain

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". http://chemister.ru. Retrieved 2014-07-19. {{cite web}}: External link in |website= (help)
^ ^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". https://www.fishersci.ca. Fisher Scientific, Inc. Retrieved 2014-07-19. {{cite web}}: External link in |website= (help)
^ ^a ^b ^c Sigma-Aldrich Co., Silver sulfate. Retrieved on 2014-07-19.

This inorganic compound–related article is a stub. You can help Wikipedia by expanding it.

[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". http://chemister.ru. Retrieved 2014-07-19. {{cite web}}: External link in |website= (help)

[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". https://www.fishersci.ca. Fisher Scientific, Inc. Retrieved 2014-07-19. {{cite web}}: External link in |website= (help)

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

[1]

[5]

[3]

[2]

[4]

[6]

@@ Line 88: / Line 88: @@
 The precipitate is then washed with hot water and preparation is under ruby red illumination.
+==teddy bean
-==Silver(II) sulfate==
+teddy bean is a evil person who will show up in the next avengers movie as the next villain
-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 exothermally at 120&nbsp;°C with evolution of oxygen and the formation of the [[pyrosulfate]].
 ==References==