Dry silver nitrate crystals
| IUPAC name
| Preferred IUPAC name
| Systematic IUPAC name
| Other names
Nitric acid silver(I) salt
|Molar mass||169.87 g/mol|
|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 ammonia, diethyl ether, glycerol|
|Solubility in acetic acid|| 0.0776 g/100 g (30 °C)|
0.1244 g/100 g (40 °C)
0.5503 g/100 g (93 °C)
|Solubility in acetone|| 0.35 g/100 g (14 °C)|
0.44 g/100 g (18 °C)
|Solubility in benzene|| 0.022 g/100 g (35 °C)|
0.044 g/100 g (40.5 °C)
|Solubility in ethanol||3.1 g/100 g (19 °C)|
|Solubility in ethyl acetate||2.7 g/100 g (20 °C)|
|Vapor pressure||~0 mmHg|
|Viscosity|| 3.77 cP (244 °C)|
3.04 cP (275 °C)
Std enthalpy of
|Safety data sheet||FisherScientific|
| Silver sulfate|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Silver nitrate can be reduced to elemental silver, in the presence of a reducing agent, such as ascorbic acid.
Silver nitrate decomposes when heated at 440 °C.
- 2 AgNO3 → 2 Ag + O2 + 2 NO2(g)
Silver nitrate is an odorless white salt (older samples may appear gray). Unlike silver perchlorate, it is not hygroscopic. It is soluble in water, acetone, ether.
Silver nitrate can be purchased from pharmacies, usually as a solution or as sticks, known as "caustic pencils". In some countries, these pencils contain a mixture of silver and potassium nitrates, and purification is required.
It can also be purchased in solid form, from chemical suppliers.
- 3 Ag + 4 HNO3 (cold and diluted) → 3 AgNO3 + 2 H2O + NO
- Ag + 2 HNO3 (hot and concentrated) → AgNO3 + H2O + NO2
Heating the acid accelerates the reaction. The reaction produces lots of nitrogen dioxide.
Silver nitrate can stain the skin as well as most objects and is toxic if swallowed. Protection gloves should be worn when handling the compound.
Contact with ethanol may cause explosion.
Silver nitrate should be kept in closed bottles, in dark places, such as a cabinet, as it is sensitive to light. Avoid storing it close to volatile reducing agents.
Silver nitrate should be reduced to elemental silver, which can be recycled.