Difference between revisions of "Silver nitrate"
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| OtherNames = Argenti nitras<br>Lunar caustic<br>Nitric acid silver(I) salt<br>Silver(I) nitrate | | OtherNames = Argenti nitras<br>Lunar caustic<br>Nitric acid silver(I) salt<br>Silver(I) nitrate | ||
<!-- Images --> | <!-- Images --> | ||
| − | | ImageFile = | + | | ImageFile = Silver nitrate by NileRed.jpg |
| − | | ImageSize = | + | | ImageSize = 300 |
| ImageAlt = | | ImageAlt = | ||
| ImageName = | | ImageName = | ||
| + | | ImageCaption = Dry silver nitrate crystals | ||
| ImageFile1 = | | ImageFile1 = | ||
| ImageSize1 = | | ImageSize1 = | ||
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| BoilingPt_ref = | | BoilingPt_ref = | ||
| BoilingPt_notes = (decomposes) | | BoilingPt_notes = (decomposes) | ||
| − | | Density = | + | | Density = 4.35 g/cm<sup>3</sup> (24 °C)<br>3.97 g/cm<sup>3</sup> (210 °C) |
| Formula = AgNO<sub>3</sub> | | Formula = AgNO<sub>3</sub> | ||
| HenryConstant = | | HenryConstant = | ||
| Line 64: | Line 65: | ||
| pKa = | | pKa = | ||
| pKb = | | pKb = | ||
| − | | Solubility = 122 g/100 | + | | Solubility = 122 g/100 ml (0 °C)<br>170 g/100 ml (10 °C)<br>256 g/100 ml (25 °C)<br>373 g/100 ml (40 °C)<br>912 g/100 ml (100 °C) |
| − | | SolubleOther = Soluble in [[ammonia]], [[diethyl ether]], [[glycerol]] | + | | SolubleOther = Reacts with alkalis<br>Soluble in [[ammonia]], [[diethyl ether]], [[glycerol]] |
| Solubility1 = 0.0776 g/100 g (30 °C)<br>0.1244 g/100 g (40 °C)<br>0.5503 g/100 g (93 °C) | | Solubility1 = 0.0776 g/100 g (30 °C)<br>0.1244 g/100 g (40 °C)<br>0.5503 g/100 g (93 °C) | ||
| Solvent1 = acetic acid | | Solvent1 = acetic acid | ||
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| Solvent5 = ethyl acetate | | Solvent5 = ethyl acetate | ||
| Taste = Bitter, metallic | | Taste = Bitter, metallic | ||
| − | | VaporPressure = | + | | VaporPressure = ~0 mmHg |
| Viscosity = 3.77 cP (244 °C)<br>3.04 cP (275 °C) | | Viscosity = 3.77 cP (244 °C)<br>3.04 cP (275 °C) | ||
}} | }} | ||
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| OtherFunction = | | OtherFunction = | ||
| OtherFunction_label = | | OtherFunction_label = | ||
| − | | OtherCompounds = [[Silver sulfate]] | + | | OtherCompounds = [[Silver sulfate]]<br>[[Silver perchlorate]] |
}} | }} | ||
}} | }} | ||
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:2 AgNO<sub>3</sub> → 2 Ag + O<sub>2</sub> + 2 NO<sub>2</sub>(g) | :2 AgNO<sub>3</sub> → 2 Ag + O<sub>2</sub> + 2 NO<sub>2</sub>(g) | ||
| + | |||
| + | Molten silver nitrate will ignite many combustible materials, like [[paper]], on direct contact, though a slight delay may occur.<ref>[https://www.youtube.com/watch?v=W_j9UKYyoHs Chlorosulfonic acid. Powerful lachrymator ⚠]</ref> | ||
===Physical=== | ===Physical=== | ||
| − | Silver nitrate is an odorless white salt. Unlike [[silver perchlorate]], it is not hygroscopic. It is soluble in water, acetone, ether. | + | 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. |
==Availability== | ==Availability== | ||
| − | 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. It can also be purchased in solid form, from chemical suppliers. | + | 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. | ||
==Preparation== | ==Preparation== | ||
| − | Silver nitrate can be prepared by reacting [[nitric acid]] with silver metal. Heating the acid accelerates the reaction. | + | Silver nitrate can be prepared by reacting [[nitric acid]] with [[silver]] metal. |
| + | |||
| + | : 3 Ag + 4 HNO<sub>3</sub> (cold and diluted) → 3 AgNO<sub>3</sub> + 2 H<sub>2</sub>O + [[nitric oxide|NO]] | ||
| + | : Ag + 2 HNO<sub>3</sub> (hot and concentrated) → AgNO<sub>3</sub> + H<sub>2</sub>O + NO<sub>2</sub> | ||
| + | |||
| + | Heating the acid accelerates the reaction. The reaction produces lots of [[nitrogen dioxide]]. | ||
==Projects== | ==Projects== | ||
*Make [[silver acetate]] | *Make [[silver acetate]] | ||
*[[Silver carbonate]] synthesis | *[[Silver carbonate]] synthesis | ||
| − | * | + | *Make silver mirror |
*[[Ethyl nitrate]] synthesis | *[[Ethyl nitrate]] synthesis | ||
==Handling== | ==Handling== | ||
===Safety=== | ===Safety=== | ||
| − | Silver nitrate can stain the skin as well as most objects and is toxic if swallowed. | + | 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 | + | Contact with [[ethanol]] may cause explosion. |
===Storage=== | ===Storage=== | ||
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[[Category:Light-sensitive chemicals]] | [[Category:Light-sensitive chemicals]] | ||
[[Category:Solids]] | [[Category:Solids]] | ||
| + | [[Category:Essential reagents]] | ||
| + | [[Category:Irritants]] | ||
Latest revision as of 22:44, 23 April 2024
 Dry silver nitrate crystals
| |
| Names | |
|---|---|
| IUPAC name
Silver nitrate
| |
| Preferred IUPAC name
Silver nitrate | |
| Systematic IUPAC name
Silver nitrate | |
| Other names
Argenti nitras
Lunar caustic Nitric acid silver(I) salt Silver(I) nitrate | |
| Properties | |
| AgNO3 | |
| Molar mass | 169.87 g/mol |
| Appearance | White 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 | Reacts with alkalis 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) |
| Thermochemistry | |
| Std molar
entropy (S |
140.9 J·mol-1·K-1 |
| Std enthalpy of
formation (ΔfH |
−124.4 kJ/mol |
| Hazards | |
| Safety data sheet | FisherScientific |
| Flash point | Non-flammable |
| Related compounds | |
| Related compounds
|
Silver sulfate Silver perchlorate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Silver nitrate is a chemical compound, salt of nitric acid and silver metal. It has the chemical formula AgNO3.
Contents
Properties
Chemical
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)
Molten silver nitrate will ignite many combustible materials, like paper, on direct contact, though a slight delay may occur.[1]
Physical
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.
Availability
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.
Preparation
Silver nitrate can be prepared by reacting nitric acid with silver metal.
- 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.
Projects
- Make silver acetate
- Silver carbonate synthesis
- Make silver mirror
- Ethyl nitrate synthesis
Handling
Safety
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.
Storage
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.
Disposal
Silver nitrate should be reduced to elemental silver, which can be recycled.
