Difference between revisions of "Silver carbonate"
| Line 56: | Line 56: | ||
| HenryConstant = | | HenryConstant = | ||
| LogP = | | LogP = | ||
| − | | MolarMass = | + | | MolarMass = 275.75 g/mol |
| MeltingPt = | | MeltingPt = | ||
| MeltingPtC = 218 | | MeltingPtC = 218 | ||
| Line 64: | Line 64: | ||
| pKa = | | pKa = | ||
| pKb = | | pKb = | ||
| − | | Solubility = 0. | + | | Solubility = 0.0031 g/100 ml (15 °C)<br>0.0032 g/100 ml (25 °C)<br>0.05 g/100 ml (100 °C) |
| SolubleOther = Reacts with acids<br>Insoluble in [[acetone]], liq. [[ammonia]], [[chloroform]], [[ethanol]], [[ethyl acetate]], [[methanol]], [[toluene]], [[xylene]] | | SolubleOther = Reacts with acids<br>Insoluble in [[acetone]], liq. [[ammonia]], [[chloroform]], [[ethanol]], [[ethyl acetate]], [[methanol]], [[toluene]], [[xylene]] | ||
| Solvent = | | Solvent = | ||
| − | | VaporPressure = | + | | VaporPressure = ~0 mmHg |
}} | }} | ||
| Section3 = {{Chembox Structure | | Section3 = {{Chembox Structure | ||
| Line 129: | Line 129: | ||
==Preparation== | ==Preparation== | ||
| − | Silver carbonate can be prepared by reacting a mixture of [[silver nitrate]] with another of [[sodium carbonate]]. Since silver carbonate is | + | Silver carbonate can be prepared by reacting a mixture of [[silver nitrate]] with another of [[sodium carbonate]]. Since silver carbonate is practically insoluble in water, it will precipitate out of the solution, while [[sodium nitrate]] will remain in solution. |
: 2 AgNO<sub>3</sub> + Na<sub>2</sub>CO<sub>3</sub> → Ag<sub>2</sub>CO<sub>3</sub> + 2 NaNO<sub>3</sub> | : 2 AgNO<sub>3</sub> + Na<sub>2</sub>CO<sub>3</sub> → Ag<sub>2</sub>CO<sub>3</sub> + 2 NaNO<sub>3</sub> | ||
Latest revision as of 17:07, 6 July 2019
| Names | |
|---|---|
| IUPAC name
Silver carbonate
| |
| Other names
Disilver carbonate
Silver(I) carbonate | |
| Properties | |
| Ag2CO3 | |
| Molar mass | 275.75 g/mol |
| Appearance | Pale yellow solid |
| Odor | Odorless |
| Density | 6.077 g/cm3 |
| Melting point | 218 °C (424 °F; 491 K) (decomposition begins around 120 °C) |
| Boiling point | Decomposes |
| 0.0031 g/100 ml (15 °C) 0.0032 g/100 ml (25 °C) 0.05 g/100 ml (100 °C) | |
| Solubility | Reacts with acids Insoluble in acetone, liq. ammonia, chloroform, ethanol, ethyl acetate, methanol, toluene, xylene |
| Vapor pressure | ~0 mmHg |
| Thermochemistry | |
| Std molar
entropy (S |
167.4 J·mol-1·K-1 |
| Std enthalpy of
formation (ΔfH |
−505.8 kJ/mol |
| Hazards | |
| Safety data sheet | Sigma-Aldrich |
| Lethal dose or concentration (LD, LC): | |
| LD50 (Median dose)
|
3,730 mg/kg (mice, oral) |
| Related compounds | |
| Related compounds
|
Silver nitrate Silver perchlorate Silver sulfate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Silver carbonate is a silver chemical compound with the formula Ag2CO3.
Contents
Properties
Chemical
Like all other carbonates, silver carbonate will react with acids to give their respective silver salts and give off carbon dioxide.
- Ag2CO3 + 2 HNO3 → 2 AgNO3 + H2O + CO2
Silver carbonate reacts with ammonia to give the explosive silver fulminate.
- 4 Ag2CO3 + 4 NH3 → 4 AgCNO + 6 H2O + 4 Ag + O2
No conditions are given for this reaction.
Physical
Silver carbonate is colorless solid which quickly turns yellow upon exposure to light and finally brown if kept too much in light. It is poorly soluble in water and organic solvents. Silver carbonate will decompose if heated above the boiling point of water.
Availability
Silver carbonate is sold by various suppliers, but it's not cheap.
Preparation
Silver carbonate can be prepared by reacting a mixture of silver nitrate with another of sodium carbonate. Since silver carbonate is practically insoluble in water, it will precipitate out of the solution, while sodium nitrate will remain in solution.
- 2 AgNO3 + Na2CO3 → Ag2CO3 + 2 NaNO3
Projects
- Make silver fulminate
- Make silver mirror
- Catalyst in Koenigs–Knorr reaction
- Oxidizer in Fétizon oxidation
Handling
Safety
Silver carbonate is light-sensitive, decomposition begins in seconds after synthesis under light and tends to stain. Wear proper protection when handling the compound. Ingestion of the compound may lead to argyria.
Storage
In closed opaque plastic or dark amber glass bottles, in a dark place, away from light.
Disposal
Adding a reducing agent, such as formaldehyde or ascorbic acid will cause it to decompose to metallic silver which can be recycled.
