Chemical elements
    Physical Properties
    Chemical Properties
      Silver fluoride
      Silver subfluoride
      Silver chloride
      Silver subchloride
      Silver bromide
      Silver oxybromide
      Silver subbromide
      Silver iodide
      Silver hypochlorite
      Silver chlorite
      Silver chlorate
      Silver perchlorate
      Silver bromate
      Silver perbromate
      Silver iodate
      Silver periodates
      Silver suboxide
      Silver monoxide
      Higher oxides
      Silver subsulphide
      Silver sulphide
      Silver sulphite
      Silver sulphate
      Silver selenide
      Silver telluride
      Silver thiosulphate
      Silver dithionate
      Silver azide
      Silver hyponitrite
      Silver nitrite
      Silver nitrate
      Silver phosphides
      Silver hypophosphate
      Silver orthophosphate
      Silver pyrophosphate
      Silver metaphosphate
      Silver arsenite
      Silver arsenate
      Silver carbide
      Silver carbonate
      Silver cyanide
      Silver thiocyanate
      Silver borate
    PDB 1aoo-3kso

Silver carbonate, Ag2CO3

When the equivalent proportion of potassium carbonate or potassium hydrogen carbonate is added to a solution of Silver nitrate, silver carbonate, Ag2CO3, is precipitated as a yellow powder. Addition of excess of potassium carbonate causes simultaneous precipitation of a proportion of Silver monoxide. Pure silver carbonate is white, but is sensitive to light. At 200° C. it decomposes with evolution of carbon dioxide. Its heat of formation is 120.8 Cal. Silver nitrate precipitates from a hot, concentrated solution of potassium carbonate a double salt of the formula Ag2CO3,K2CO3. A crystalline double compound with ammonia of the formula Ag2CO3,4NH3,H2O is produced by the spontaneous evaporation in air of an ammoniacal solution of silver oxide. Under the influence of sunlight the crystals become black; and on exposure to air they lose water and ammonia, yielding silver carbonate.

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