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Silver nitrate

Silver nitrate
Skeletal formula of silver nitrate
Sample of silver nitrate
Names
IUPAC name
Silver(I) nitrate, Silver nitrate
Other names
Nitric acid silver(1+) salt
Identifiers
7761-88-8 YesY
3D model (Jmol) Interactive image
ChEBI CHEBI:32130 YesY
ChEMBL ChEMBL177367 YesY
ChemSpider 22878 YesY
ECHA InfoCard 100.028.958
EC Number 231-853-9
PubChem 24470
RTECS number VW4725000
UNII 95IT3W8JZE YesY
UN number 1493
Properties
AgNO3
Molar mass 169.87 g·mol−1
Appearance colorless solid
Odor Odorless
Density 4.35 g/cm3 (24 °C)
3.97 g/cm3 (210 °C)
Melting point 209.7 °C (409.5 °F; 482.8 K)
Boiling point 440 °C (824 °F; 713 K)
decomposes
122 g/100 mL (0 °C)
170 g/100 mL (10 °C)
256 g/100 mL (25 °C)
373 g/100 mL (40 °C)
912 g/100 mL (100 °C)
Solubility Soluble in acetone,ammonia, ether, glycerol
Solubility in acetic acid 0.776 g/kg (30 °C)
1.244 g/kg (40 °C)
5.503 g/kg (93 °C)
Solubility in acetone 0.35 g/100 g (14 °C)
0.44 g/100 g (18 °C)
Solubility in benzene 0.22 g/kg (35 °C)
0.44 g/kg (40.5 °C)
Solubility in ethanol 3.1 g/100 g (19 °C)
Solubility in ethyl acetate 2.7 g/100 g (20 °C)
log P 0.19
−45.7·10−6 cm3/mol
1.744
Viscosity 3.77 cP (244 °C)
3.04 cP (275 °C)
Structure
Orthorhombic, oP56
P212121, No. 19
222
a = 6.992(2) Å, b = 7.335(2) Å, c = 10.125(2) Å
α = 90°, β = 90°, γ = 90°
Thermochemistry
93.1 J/mol·K
140.9 J/mol·K
−124.4 kJ/mol
−33.4 kJ/mol
Pharmacology
D08AL01 (WHO)
Hazards
Main hazards Explosively reacts with ethanol. Corrosive.
GHS pictograms The flame-over-circle pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS)The corrosion pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS)The environment pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS)
GHS signal word Danger
H272, H314, H410
P220, P273, P280, P305+351+338, P310, P501
Oxidizing Agent O Corrosive C Dangerous for the Environment (Nature) N
R-phrases R8, R34, R50/53
S-phrases S26, S36/37/39, S45, S60, S61
NFPA 704
Flammability code 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g., canola oil Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas Reactivity code 3: Capable of detonation or explosive decomposition but requires a strong initiating source, must be heated under confinement before initiation, reacts explosively with water, or will detonate if severely shocked. E.g., fluorine Special hazard OX: Oxidizer. E.g., potassium perchlorateNFPA 704 four-colored diamond
Lethal dose or concentration (LD, LC):
800 mg/kg (rabbit, oral)
20 mg/kg (dog, oral)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
YesY  (what is YesYN ?)
Infobox references

Silver nitrate is an inorganic compound with chemical formula AgNO
3. This compound is a versatile precursor to many other silver compounds, such as those used in photography. It is far less sensitive to light than the halides. It was once called lunar caustic because silver was called luna by the ancient alchemists, who believed that silver was associated with the moon.

In solid silver nitrate, the silver ions are three-coordinated in a trigonal planar arrangement.

Albertus Magnus, in the 13th century, documented the ability of nitric acid to separate gold and silver by dissolving the silver. Magnus noted that the resulting solution of silver nitrate could blacken skin.

Silver nitrate can be prepared by reacting silver, such as a silver bullion or silver foil, with nitric acid, resulting in silver nitrate, water, and oxides of nitrogen. Reaction byproducts depend upon the concentration of nitric acid used.

This is performed under a fume hood because of toxic nitrogen oxide(s) evolved during the reaction.

A typical reaction with silver nitrate is to suspend a rod of copper in a solution of silver nitrate and leave it for a few hours. The silver nitrate reacts with copper to form hairlike crystals of silver metal and a blue solution of copper nitrate:

Silver nitrate decomposes when heated:

Qualitatively, decomposition is negligible below the melting point, but becomes appreciable around 250 °C and totally decompose at 440 °C.

Most metal nitrates thermally decompose to the respective oxides, but silver oxide decomposes at a lower temperature than silver nitrate, so the decomposition of silver nitrate yields elemental silver instead.

Silver nitrate is the least expensive salt of silver; it offers several other advantages as well. It is non-hygroscopic, in contrast to silver fluoroborate and silver perchlorate. It is relatively stable to light. Finally, it dissolves in numerous solvents, including water. The nitrate can be easily replaced by other ligands, rendering AgNO3 versatile. Treatment with solutions of halide ions gives a precipitate of AgX (X = Cl, Br, I). When making photographic film, silver nitrate is treated with halide salts of sodium or potassium to form insoluble silver halide in situ in photographic gelatin, which is then applied to strips of tri-acetate or polyester. Similarly, silver nitrate is used to prepare some silver-based explosives, such as the fulminate, azide, or acetylide, through a precipitation reaction.


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