Silver Sulfate
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Silver Sulfate
Silver sulfate
Skeletal formula of silver sulfate
Sample of silver sulfate
Names
IUPAC name
Silver sulfate
Other names
disilver sulfate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.030.581
EC Number
  • 233-653-7
UNII
UN number 3077
Properties
Ag2SO4
Molar mass  g·mol-1
Appearance Colorless crystals
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]
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]
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]
n? = 1.756
n? = 1.775
n? = 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]
? = 90°, ? = 90°, ? = 90°
Thermochemistry
131.4 J/mol·K[1]
200.4 kJ/mol[1]
-715.9 kJ/mol[1]
-618.4 J/mol·K[1]
Hazards
GHS pictograms GHS05: CorrosiveGHS09: Environmental hazard[6]
GHS Signal word Danger
H318, H410[6]
P273, P280, P305+351+338, 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).
?Y verify (what is ?Y?N ?)
Infobox references

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.

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[7] 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.

References

  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". http://chemister.ru. Retrieved . External link in |website= (help)
  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. 25. Washington: Institute for Materials Research National Bureau of Standards.
  5. ^ a b c "MSDS of Silver sulfate". https://www.fishersci.ca. Fisher Scientific, Inc. Retrieved . External link in |website= (help)
  6. ^ a b c Sigma-Aldrich Co., Silver sulfate. Retrieved on 2014-07-19.
  7. ^ Malinowski, P.; Derzsi, M.; Mazej, Z.; Jagli?i?, Z.; Gawe?, 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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