The ammonium salts of nitrate and especially perchlorate are highly explosive, in these cases, ammonium is the reducing agent. An exception is ammonium hexachloroplatinate, the formation of which was once used as a test for ammonium. Most simple ammonium salts are very soluble in water. Salts and characteristic reactions Formation of ammoniumĪmmonium cation is found in a variety of salts such as ammonium carbonate, ammonium chloride, and ammonium nitrate. If the pH is high (the concentration of hydrogen ions is low and hydroxide ions is high), the equilibrium shifts to the left: the hydroxide ion abstracts a proton from the ammonium ion, generating ammonia.įormation of ammonium compounds can also occur in the vapor phase for example, when ammonia vapor comes in contact with hydrogen chloride vapor, a white cloud of ammonium chloride forms, which eventually settles out as a solid in a thin white layer on surfaces. If the pH is low, the equilibrium shifts to the right: more ammonia molecules are converted into ammonium ions. The degree to which ammonia forms the ammonium ion depends on the pH of the solution. When ammonia is dissolved in water, a tiny amount of it converts to ammonium ions: Thus, the treatment of concentrated solutions of ammonium salts with a strong base gives ammonia. The ammonium ion is mildly acidic, reacting with Brønsted bases to return to the uncharged ammonia molecule: The ammonium ion is generated when ammonia, a weak base, reacts with Brønsted acids ( proton donors): Ammonium is also a general name for positively charged (protonated) substituted amines and quaternary ammonium cations ( +), where one or more hydrogen atoms are replaced by organic or other groups (indicated by R).Īcid–base properties Fumes from hydrochloric acid and ammonia forming a white cloud of ammonium chloride It is formed by the protonation of ammonia ( NH 3). The ammonium cation is a positively charged polyatomic ion with the chemical formula NH + 4 or +.
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