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Ammonium chloride is an inorganic chemical compound with the chemical formula N H 4 Cl, also ... the production of ammonium chloride from organic substances (such as ...
Ammonium bromide – NH 4 Br [37] Ammonium chromate – [NH 4] 2 CrO 4 [38] Ammonium cerium(IV) nitrate – [NH 4] 2 [Ce(NO 3) 6] Ammonium cerium(IV) sulfate – [NH 4] 4 [Ce(SO 4) 4] Ammonium chloride – [NH 4]Cl [39] Ammonium chlorate – [NH 4]ClO 3 [40] Ammonium cyanide – [NH 4]CN [41] Ammonium dichromate – [NH 4] 2 Cr 2 O 7 [42 ...
Sal alembroth – salt composed of chlorides of ammonium and mercury. Sal ammoniac – ammonium chloride. Sal petrae (Med. Latin: "stone salt")/salt of petra/saltpetre/nitrate of potash – potassium nitrate, KNO 3, typically mined from covered dungheaps. Salt/common salt – a mineral, sodium chloride, NaCl, formed by evaporating seawater ...
The component ions in a salt can be either inorganic, such as chloride (Cl −), or organic, such as acetate (CH 3 COO −). Each ion can be either monatomic (termed simple ion), such as sodium (Na +) and chloride (Cl −) in sodium chloride, or polyatomic, such as ammonium (NH + 4) and carbonate (CO 2− 3) ions in ammonium carbonate.
For example, in ammonium chloride solution, NH + 4 is the main influence for acidic solution. It has greater K a value compared to that of water molecules; K a of NH + 4 is 5.6 × 10 −10, and K w of H 2 O is 1.0 × 10 −14. This ensures its deprotonation when reacting with water, and is responsible for the pH below 7 at room temperature.
The tables below provides information on the variation of solubility of different substances (mostly inorganic compounds) in water with temperature, at one atmosphere pressure. Units of solubility are given in grams of substance per 100 millilitres of water (g/(100 mL)), unless shown otherwise. The substances are listed in alphabetical order.
The ammonium salts of nitrate and especially perchlorate are highly explosive, in these cases, ammonium is the reducing agent. In an unusual process, ammonium ions form an amalgam. Such species are prepared by the addition of sodium amalgam to a solution of ammonium chloride. [3] This amalgam eventually decomposes to release ammonia and ...
In aqueous solution, chloramine slowly decomposes to dinitrogen and ammonium chloride in a neutral or mildly alkaline (pH ≤ 11) medium: 3 NH 2 Cl → N 2 + NH 4 Cl + 2 HCl However, only a few percent of a 0.1 M chloramine solution in water decomposes according to the formula in several weeks.