2 AgBr (s) + 2 NH4OH (aq) --> Ag2O (s) + H2O (l) +2 NH4Br (aq)
The reaction does not proceed rapidly as in the case of AgCl as AgBr is only slightly soluble in ammonium hydroxide. With more NH4OH, the brown/black Ag2O dissolves forming the soluble salt Silver Di-amine hydroxide:
Ag2O (s) + 4 NH4OH --> 2 [Ag(NH3)2]OH + 3 H2O
I suspect that this reaction is reversible and the loss of NH3 would push the reaction to the left, which may occur naturally with time. This is a major problem as the precipitated Ag2O can further react with NH4OH to form Silver nitride, Ag3N:
2 NH4OH (aq) + 3 Ag2O (s) --> 2 Ag3N (s) + 5 H2O
Silver nitride can be a highly sensitive and powerful contact explosive, even when in solution. This has been ascribed to be the cause of many injuries, and as such, solutions of [Ag(NH3)2]OH should not be stored for safety concerns.
AgBr precipitates and in light decomposes to bromine and silver metal.
2AgNO3 + MgBr2 ----> 2AgBr + Mg(NO3 ) 2
ethyl nitrite
Silver Bromide is AgBr. It is the salt produced from silver and bromine.
The elements present in silver bromide are silver and bromine.
2AgI+2NH3 give you 2AgNH3 + I2.Reaction only occurs when ammonia (NH3) is added in excess.
This equation is:AgNO3 + KBr = AgBr(s) + KNO3Silver bromide is a white precipitate.
AgBr precipitates and in light decomposes to bromine and silver metal.
pudding
2AgNO3 + MgBr2 ----> 2AgBr + Mg(NO3 ) 2
The reaction is:AgNO3 + KBr = AgBr = KNO3Silver bromide is a precipitate.
Examples: silver chloride, silver fluoride, silver iodide, silver bromide, silver astatide, silver sulfide, silver nitrate etc. For silver halogenides a method of preparation is the reaction between silver nitrate and a salt containing the halogen.
Nothing
ethyl nitrite
think so..... decomposition
Silver Bromide is AgBr. It is the salt produced from silver and bromine.
The elements present in silver bromide are silver and bromine.