Silver sulfate


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

Silver sulfate
Skeletal formula of silver sulfate
Sample of silver sulfate
IUPAC name
Silver(I) sulfate
Other names
Disilver sulfate
Argentous sulfate
  • 10294-26-5 checkY
3D model (JSmol)
  • Interactive image
  • 140554 checkY
ECHA InfoCard 100.030.581 Edit this at Wikidata
EC Number
  • 233-653-7
  • 159865
  • 8QG6HV4ZPO checkY
UN number 3077
  • DTXSID70172884 Edit this at Wikidata
  • InChI=1S/2Ag.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2*+1;/p-2 checkY
  • InChI=1/2Ag.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2*+1;/p-2
  • [Ag+].[Ag+].[O-]S([O-])(=O)=O
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 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]
nα = 1.756
nβ = 1.775
nγ = 1.782[4]
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°
131.4 J/mol·K[1]
200.4 J/mol·K [1]
−715.9 kJ/mol[1]
−618.4 kJ/mol [1]
GHS labelling:
GHS05: CorrosiveGHS09: Environmental hazard[6]
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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Infobox references

Preparation and structureEdit

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) sulfateEdit

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 exothermally at 120 °C with evolution of oxygen and the formation of the pyrosulfate.


  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.
  2. ^ 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.
  3. ^ a b c Anatolievich, Kiper Ruslan. "silver sulfate". Retrieved 2014-07-19.
  4. ^ 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.
  5. ^ a b c "MSDS of Silver sulfate". Fisher Scientific, Inc. Retrieved 2014-07-19.
  6. ^ a b c Sigma-Aldrich Co., Silver sulfate. Retrieved on 2014-07-19.
  7. ^ O. Glemser; R. Sauer (1963). "Copper (I) 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.