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Sodium carbonate (also known as washing soda, soda ash and soda crystals) is the inorganic compound with the formula Na 2 CO 3 and its various hydrates.All forms are white, odourless, water-soluble salts that yield alkaline solutions in water.
Instead of treating the remaining solution with lime, carbon dioxide and ammonia are pumped into the solution, then sodium chloride is added until the solution saturates at 40 °C. Next, the solution is cooled to 10 °C. Ammonium chloride precipitates and is removed by filtration, and the solution is recycled to produce more sodium carbonate.
When a sodium and carbonate ion-containing compound is used as the reactant, the carbonate anion from sodium bicarbonate or carbonate, reacts with the hydrogen from the carboxyl group (-COOH) in acetic acid, forming carbonic acid. Carbonic acid readily decomposes under normal conditions into gaseous carbon dioxide and water.
This reaction usually produces a salt. One example, hydrochloric acid reacts with disodium iron tetracarbonyl to produce the iron dihydride: 2 HCl + Na 2 Fe(CO) 4 → 2 NaCl + H 2 Fe(CO) 4. Reaction between an acid and a carbonate or bicarbonate salt yields carbonic acid, which spontaneously decomposes into carbon dioxide and water. The release ...
A salt containing reactive cations undergo hydrolysis by which they react with water molecules, causing deprotonation of the conjugate acids. For example, the acid salt ammonium chloride is the main species formed upon the half neutralization of ammonia in aqueous solution of hydrogen chloride: [2] NH 3 + HCl(aq) → [NH 4] + Cl − (aq)
The chloride from the hydrochloric acid in sodium chloride does not hydrolyze, though, so sodium chloride is not basic. The difference between a basic salt and an alkali is that an alkali is the soluble hydroxide compound of an alkali metal or an alkaline earth metal. A basic salt is any salt that hydrolyzes to form a basic solution.
If the two solutions have hydrogen ions and hydroxide ions as the counterions, they will react with one another in what is called an acid–base reaction or a neutralization reaction to form water. [12] Alternately the counterions can be chosen to ensure that even when combined into a single solution they will remain soluble as spectator ions. [11]
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.