Silver carbonate

Structural formula
${\displaystyle \mathrm {\ \!\ {\Biggl [}} }$ ${\displaystyle \mathrm {\ \!\ {\Biggr ]}} }$
General
Surname	Silver carbonate
other names	Silver (I) carbonate SILVER BICARBONATE ( INCI )
Molecular formula	Ag 2 CO 3
Brief description	light yellow powder
External identifiers / databases
CAS number 534-16-7 EC number 208-590-3 ECHA InfoCard 100.007.811 PubChem 92796 ChemSpider 83768 Wikidata Q417067
properties
Molar mass	275.75 g mol −1
Physical state	firmly
density	6.08 g cm −3 (20 ° C)
Melting point	218 ° C (decomposition)
solubility	poor in water (32 mg l −1 at 20 ° C)
safety instructions
GHS labeling of hazardous substances danger H and P phrases H: 318-410 P: 261-273-280-305 + 351 + 338
MAK	0.01 mg m −3
Toxicological data	2168 mg kg −1 ( LD 50 ,  mouse ,  oral ) 3731 mg kg −1 ( LD 50 ,  rat ,  oral )
Thermodynamic properties
ΔH f 0	-505.8 kJ / mol
As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Silver carbonate is a chemical compound of silver from the group of carbonates .

Extraction and presentation

Silver carbonate can be obtained by precipitation from silver-containing solutions, for example silver nitrate , with alkali metal carbonates such as sodium carbonate .

${\displaystyle \mathrm {2\ AgNO_{3}+Na_{2}CO_{3}\longrightarrow Ag_{2}CO_{3}\downarrow +\ 2\ NaNO_{3}} }$

properties

Freshly made silver carbonate is white and quickly turns yellow. Like many silver compounds, it is sensitive to light and should therefore be kept in the dark. It crystallizes in the monoclinic crystal system . When heated above 218 ° C, it decomposes, releasing carbon dioxide .

${\displaystyle \mathrm {Ag_{2}CO_{3}{\xrightarrow {\triangle }}Ag_{2}O+CO_{2}\uparrow } }$

While the compound is only sparingly soluble in water, it dissolves well in acids such as nitric acid or sulfuric acid , potassium cyanide solution and potassium carbonate solutions , with double salts being formed.

use

Silver carbonate is used in synthetic organic chemistry. When applied to kieselguhr , it acts as an oxidizing agent . The connection plays an important role in the Koenigs-Knorr method . Here, 1,2-trans glycosides are selectively obtained from halogen-substituted monosaccharide derivatives . The halogen is precipitated by the silver, and a glycoside can be formed with alcohols.

It is also used for the production of silver powder and for the separation of chloride , bromide and iodide in the ion chromatographic determination of anions in salt water .

Individual evidence

1. ↑ Entry on SILVER BICARBONATE in the CosIng database of the EU Commission, accessed on May 4, 2020.
2. ↑ ^{a b c} Data sheet silver carbonate (PDF) from Merck , accessed on April 23, 2011.
3. ↑ David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 90th edition. (Internet version: 2010), CRC Press / Taylor and Francis, Boca Raton, FL, Properties of the Elements and Inorganic Compounds, pp. 4-88.
4. ↑ ^{a b c} Andreas Brumby et al .: Silver, Silver Compounds, and Silver Alloys. In: Ullmann's Encyclopedia of Industrial Chemistry. 6th edition, Wiley-VCH, Weinheim 2008, doi : 10.1002 / 14356007.a24_107.pub2 .
5. ↑ ^{a b} Entry on silver carbonate in the GESTIS substance database of the IFA , accessed on January 8, 2018(JavaScript required) .
6. ↑ ^{a b} Gigiena Truda i Professional'nye Zabolevaniya. ( Labor Hygiene and Occupational Diseases ). Vol. 27 (12), Pg. 33, 1983.
7. ↑ ^{a b} Entry on silver carbonate in the ChemIDplus database of the United States National Library of Medicine (NLM) .
8. ↑ David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 90th edition. (Internet version: 2010), CRC Press / Taylor and Francis, Boca Raton, FL, Standard Thermodynamic Properties of Chemical Substances, pp. 5-18.
9. ↑ ^{a b c} Entry on silver carbonate. In: Römpp Online . Georg Thieme Verlag, accessed on July 15, 2014.